MANUAL OP PHARMACY AND Pharmaceutical Chemistry. DESIGNED ESPECIALLY FOR THE USE OF THE PHARMACEUTICAL STUDENT AND FOR PHARMACISTS IN GENERAL. CHAS. F. HEEBNER, Ph. G., Phm. B„ »•• DEAN, PROFESSOR OF PHARMACY AND DIRECTOR OF THE PHARMACAL LABORATORY AT THE ONTARIO COLLEGE OF PHARMACY, TORONTO, ONT.; LECTURER IN MATERIA MEDICA AND ELEMENTARY THERAPEUTICS, MEDICAL FACULTY, UNIVERSITY OF TORONTO ; GRADUATE IN PHARMACY OF THE COLLEGE OF PHARMACY OF THE CITY OF NEW YORK, CLASS OF ’81 ; FORMERLY INSTRUCTOR IN THEORY AND PRACTICE OF PHARMACY AT THE COLLEGE OF • PHARMACY OF THE CITY OF NEW YORK. FOURTH EDITION. NEW YORK: PUBLISHED BY THE AUTHOR. 1894. Entered according to Act of Congress in the year 1887, By CHAS. F. HEEBNER, in the Office of the Librarian of Congress, at Washington. PBEFACE TO THE TIIIED EDITION. The appearance of this edition is in a sense premature, owing to the fact that several cnanges and additions were contemplated and are even now in preparation, with a view to increasing the already inestimable value of the Manual, and extending its present popularity m the attainment of the object of its mission to those for whom it was prepared. This new matter the author intended to incorporate in the present edition, but the somewhat startling information reaches him that die second edition is entirely exhausted and lienee the necessity of an immediate reprint. In passing, attention is directed to the treatment of the principle of Alligation in its application to Pharmacy (page 31), the study and use of which will save much needless calculation and consequent inexactness of work. The method is exceedingly comprehensible and practical, and though its application to the uses of the pharmacist originated with the author, and its utility was demonstrated and taught to his classes at the College of Pharmacy of the City of New York during several years prior to the advent of the Manual, *it was, however, first submitted to the pharmaceutical-public on the debut of this work, and is now treated of in many of the latest editions of the pharmaceutical works of the day. January, 1892. PREFACE TO THE SECOND EDITION. The collation of material for a useful treatise on pharmacy is by no means an easy task, nor can it be accomplished in a short time, while the arrangement of such material and its condensation into small space without injury to the clearness of the text, or the sacrifice of essential points and explanations, is, indeed, a stupendous task. Hence the marked favor with which the Manual has been re- ceived by the pharmaceutical profession, is a source of gratification to the author, emphatically testifying, as it has, that his labors have been appreciated, and that this little volume has succeeded in the attainment of the object of its mission, on the score of convenience and practical utility to those for whom it was prepared. The inception of the Manual was in the notes prepared by the author for use in his classes at the College of Pharmacy, and were compiled soon after the last decennial revision of the U. S. Pharma- copoeia was handed to the public. As his experience in the capacity of a teacher grew upon him, showing him the needs of the pharma- ceutical student, these notes were subjected to critical revisions annually, thereby embodying in them a variety of information and explanations deduced by further research and daily experience in the pharmaceutical laboratory, or gathered from scientific works not readily accessible to the student. Thus the notes elaborated into their present form, and every year’s added experience will doubtless find something in them to change and improve. The features of the book that are considered of especial impor- tance, and which have no doubt led to its adoption as a text-book or book of reference by colleges of pharmacy, are, its scope and great amount of material presented, its simple method of arrangement, its compactness and conciseness, and the clearness of its explanations. The experienced teacher will at once appreciate the importance of these characteristics.. The speedy exhaustion of the first edition has called for the early appearance of a second. The changes and additions of the second edition have increased the size of the volume by thirty-eight pages. The work has been revised and practically freed from typographical PREFACE TO THE SECOND EDITION. errors. The new matter consists of a chapter treating on complete Urinalysis, illustrated by twelve cuts of microscopical slides of urine sediments, and an index, complete excepting that but few com- pounds are mentioned under the Latin names. The generally acknowledged importance of the study of Urinaly- sis, and the increasing recognition of its practical application to the diagnosis and stage of disease, accompanied by the fact that the pharmacist is frequently called upon to apply the same for the physician, will no doubt furnish a sufficient vindication for the in- troduction of the author’s methods on this subject. Revised and enlarged in the manner indicated above, the author trusts that the second edition will be found as acceptable and useful as its predecessor, and that it may merit a reception equally as favorable. January, 1889. PKEFACE. The special aim of this work is to aiford a short but instructive course in the Department of Pharmacy. It is the outgrowth of a want long felt by students at the various Colleges of Pharmacy, for a book especially adapted to their use as a class-book, or note-book. All the unnecessary matter of many text- books has been here eliminated. The amount of material presented, as well as the arrangement of the various topics and the manner of their treatment have been sim- plified as far as can consistently be done, thereby producing a work of such a nature, that the student will find it most advantageous as a book for study in reviewing the subjects for the class, and pre- liminary to examinations. For a similar reason, it commends itself as a book of reference to Pharmacists ; also to Pharmaceutical students or drug clerks, especially in preparing for the examinations of the various Boards of Pharmacy. It cannot take the place of lectures in Pharmacy, nor replace many of the exhaustive works on this subject, some of which should be read in connection with this work. Many of the facts within the following pages represent compila- tions from authorized sources, with many original explanations and practical hints. It was the author’s intention to have placed this treatise in the hands of the Pharmaceutical public, two years since, but illness re- tarded the completion of the necessary work. It is hoped that the Manual of Pharmacy and Pharmaceuti- cal Chemistry may prove of material service to those for whom it has been prepared. Oct 26,1887. Chas. F. Heebner. TABLE OF CONTENTS. INTRODUCTION. Pharmacy. Pharmacopeias. Dispensatories 13 PART I. Metrology. Gravitation. Weight. Weighing. The Balance. Systems of Weights. Troy. Avoirdupois. Apothecaries. Liquid Measures. Metric System. Specific Gravity, and Methods for Determination. Specific Volume. Rules for Proportionate Mixing 14-33 Collection, Preparation, and Preservation of Botanical Drugs. Des- sication. Garbling 34-35 Mechanical Subdivision. Comminution. Contusion. Trituration. De- gree of Subdivision. Levigation. Elutriation 36-37 Heat. Its Determination. Sensible Heat. Latent Heat. The Thermom- eter. Comparison of Different Thermometric Scales. Bunsen Burner. Blowpipe. Crucible 37-39 Processes Requiring Heat. Sublimation. Ignition. Incineration. Calci- nation. Fusion. Torrefaction. Reduction. Deflagration. Oxidation. Carbonization. Methods for controlling Heat. Boiling Point 39-41 Solution. Simple. Chemical. Saturated and Super-saturated Solutions. Circulatory Displacement. Solvents. Complex Solution. Dialysis—41-43 Maceration. Digestion. Infusion. Decoction 43-44 Percolation. Methods. Relation to Fluid Extracts. Requisites for their reliable preparation. Determination of Menstruum. Quantity of Per- colate. Test for Exhaustion. Theory of Percolation and Exhaustion. Re-percolation (Illustration) 45-51 Processes. Lixiviation. Expression. Filtration. Colation. Clarifica- tion. (Various methods). Decolorization and Deodorization. Sedi ment. Decantation. Syphon 53-53 VI CONTENTS. Vaporization. Evaporation—Spontaneous and In Vacuo. Distillation. Simple. Apparatus Required. Fractional and Destructive Distillation. Sublimation 54-55 Separation op Solids from Solution. Crystallization. Methods. Amor- phous. Dimorphous. Isomorphous. Mother Liquor. Water of Crystallization. Efflorescence. Deliquescence. Size of Crystals. Granulation. Crystallography. Precipitation. Washing the Precipi- tate. Character of Precipitate. Examples 55-58 Generation, Absorption, and Collection of Gases 58-59 CLASSIFICATION OF PHARMACOFCEIAL PREPARATIONS. Liquids. Aceta. Aqu®. Collodia. Decocta. Elixiria. Extracta. Flui- da. Glycerita. Infusa. Linimenta. Liquores. Mellita. Misturae. Mucilagines. Oleata. Oleo - resinge. Spiritus. Syrupi. Tinctur®. Vina 59-61 Solids. Abstracts. Cerata. Chart®. Confectiones. Emplastra. Extracta. Mass®. Pilul®. Pulveres. Resin®. Suppositoria. Triturationes. Troehisci. Unguenta • 61-63 PART II. Inorganic Pharmacy. —Preparations. Aqua. Aqua Destillata 64 Acids. Definition. Basylous Radical. Acidulous Radical. Salts. Acidum Sulphuricum. Acidum Sulphuricum Aromaticum. Acidum Sulphur- icum Dilutum. Acidum Sulphurosum. Acidum Hydrochloricum. Aci- dum Hydrochloricum Dilutum. Acidum Nitro-Hydrochloricum. Aci- dum Nitro-Hydrochloricum Dilutum. Acidum Nitricum. Acidum Acet- icum. Acidum Aceticum Dilutum. Acidum Aceticum Glacial 64-70 Potassium Salts. Source. Reactions. General Impurities. Potassii Car- bonas. Potassii Bicarbonas. Potassii Nitras. Potassii Bitartras. Po- tassii Tartras. Potassii et Sodii Tartras. Potassii Acetas. Potassa. Potassa cum Calce. Liquor Potass*. Potassa Sulphurata. Potassii Chloras. Potassii Citras. Potassii Sulphas. Potassii Sulphis: (Other salts of Potassium found elsewhere) 70-77 ALKALIES AND THEIR COMPOUNDS. CONTENTS. Sodium Salts. Source. Reaction. General Impurities. Tests. Sodii Chloridum. Sodii Carbonas. Sodii Carbonas Exsiccatus. Sodii Bicar- bonas. Soda. Liquor Sodse Sodii Acetas. Sodii Benzoas. Sodii Boras. Acidum Boricum. Sodii Chloras. Sodii Nitras. Sodii Salicylas. Sodii Sulphas. Sodii Sulphis. Sodii Sulpho-Carbolas. Liquor Sodii Silicatis. (Other Sodium Salts found elsewhere) 77-85 Ammonium Salts. Sources. Ammonia. Reactions. General Impurities. Tests. Ammonii Chloridum. Ammonii Sulphas. Ammonii Carbonas. Liquor Ammonii Acetatis. Ammonii Nitras. Aqua Ammoniae. Lini- mentum Ammoniae. Spiritus Ammoniae Aromaticus. Aqua Ammoniae Fortior. Spiritus Ammoniae. Ammonii Benzoas. Ammonii Bromi- dum. Ammonii Iodidum. Ammonii Phosphas. Ammonium Oxalate. Ammonium Citrate. Ammonium Tartrate 85-90 ALKALINE EARTHS AND THEIR COMPOUNDS. Calcium Salts. Sources. Tests. Calx. Liquor Calcis. Syrupus Calcis. Calcii Bromidum. Calcii Carbonas Praecipitatis. Creta Preeparata. Pulvis Cretee Compositus. Mistura Cretae. Trochisi Cretae. Calcii Phosphas Praecipitatis. Calx Sulphurata 91-94 Magnesium Salts. Sources. Tests. General Impurities. Magnesii Sul- phas. Magnesii Carbonas. Magnesia. Magnesia Ponderosa. Trochisci Magnesia}. Magnesii Citratis Granulatus. Liquor Magnesii Citratis 94-97 Barium Salts. (None officinal). Tests. Barium Sulphate Barium Chlo- ride. Barium Carbonate. Barium Peroxide. Barium Hydroxide 97 Strontium Salts. (None officinal). Tests. Strontium Nitrate 98 Lithium Salts. Source. Tests. General Impurities. Lithii Carbonas. Lithii Benzoas. Lithii Bromidum. Lithii Citras. Lithii Salicylas 98-99 Cerium Salts. Cerii Oxalas. Cerium Nitrate 99 Aluminium Salts. Source. Tests. General Impurities. Alums.—Compo- sition. Alumen. Alumen Exsiccatum. Aluminii Hydras. Aluminii Sulphas 100-101 THE HALOGENS AND THEIR SALTS. Chlorine. Properties. Tests. Aqua Chlori. Calx Chlorates. Liquor So- dii Chloratee. Javelle Water. Iodum. Source. Preparation. Purifi- cation. Tests. Syrupus Acidi Hydriodici. Potassii Iodidum. Sodii Iodidum. Iodoformum. Bromum. Source. Preparation. Tests. Po- tassii Bromidum. Sodii Bromidum. Acidum Hydrobromieum Dilutum. Cyanogen Salts. Cyanogen. Potassii Ferro.cyanidum. Potassium Ferricyanide. Ferrocyanide of Iron. Potassii Cyanidum. Acidum Hydrocyanicum Dilutum. Ammonium Sulphocyanide 101-111 CONTENTS. PREPARATIONS OF THE METALLIC AND NON-METALLIC ELEMENTS. Sulphur. Occurrence. Sulphur Sublimatum. Sulphur Lotum. Sulphur Prascipitatum. Sulphuris Iodidum. Lac Sulphuris. Hydrosulphuric Acid. Carbonei Bisulphidum 111-113 •Phosphorus. Preparation. Oxides.' Amorphous Phosphorus. Acidum Phosphoricum. Acidum Phosphoricum Dilutum. Oleum Phosphora- tum. Pilulse Phosphori. Sodii Phosphas. Sodii Pyrophosphas. Cal- eb Hypophosphis. • Sodii Hypophosphis. Potassii Hypophosphis. Hy- pophosphorous Acid. 114-118 Ferrum. Tests. Ferri Chloridum. Liquor Ferri Chloridi. Tinctura Ferri Chloridi. Ferri Iodidum Saccharatum. Syrupus Ferri Iodidi. Syrupus Ferri Bromidi. Ferri Lactas. Ferri Sulphas. Ferri Sulphas Exsiccatus. Pilulae Aloes et Ferri. Ferri Sulphas Praecipitatus. Mis- tura Ferri Composita. Ferri Carbonas Saccharatus. Massa Ferri Car- bonatis. Pilulse Ferri Composite Ferri Oxalas. Liquor Ferri Subsul- phatis. Liquor Ferri Tersulphatis. Ferri Oxidum Hydratum. Trochis- ci Ferri. Emplastrum Ferri. Ferrum Reductum. Pilulse Ferri Iodidi. Ferri Oxidum Hydratum cum Magnesia. Ferri et Ammonii Sulphas. Ferri Hypophosphis. Liquor Ferri Acetatis. Tinctura Ferri Acetatis. Ferri Valerianas. Liquor Ferri Citratis. The Scale Salts. Charac- teristics, etc. Ferri et Ammonii Tartras. Ferri et Potassi Tartras. Ferri et Ammonii Citras. (Vinum Ferri Citratis.) (Liquor Ferri et Qui- ninee Citratis.) Ferri et Strychninse Citras. (Vinum Ferri Amarum.) Ferri Citras. Ferri et Quininse Citras. Citrate of Iron, Quinine, and Strychnine. Ferri Phosphas. Ferri Pyrophosphas. (Dialysed Iron.)..118-130 Manganum. Occurrence. Tests. Mangani Oxidum Rubrum. Mangani Sulphas. Potassii Permanganas 130-132 Argentum. Occurrence. Tests. Argenti Nitras. Argenti Nitras Dilutus. Argenti Nitras Fusus. Argenti Oxidum. Argenti Cyanidum 132-133 Cuprum. Occurrence. Tests. Cupri Acetas. Cupri Sulphas. Ammoni- ated Copper 134 Plumbum. Occurrence. Tests. Plumbi Oxidum. Liquor Plumbi Subace- tatis. Emplastrum Plumbi. Plumbi Acetas. Plumbi Carbonas. Plum- bi Iodidum. Plumbi Nitras 135-137 Chromium. Occurrence. Tests. Potassii Bichromas. Acidum Chromi- cum 137-138 Cadmium. Occurrence. (No Officinal Preparations.) Cadmium Iodide. Cadmium Sulphate 138-139 Zinoum. Occurrence. Tests. General Impurities. Liquor Zinci Chloridi. Zinci Chloridum. Zinci Oxidum. Zinci Sulphas. Zinci Corbonas Prse- cipitatus. Zinci Bromidum. Zinci Iodidum. Zinci Valerianas 139-142 Arsenium. Occurrence. Tests. Antidotes. Acidum Arseniosum. Liquor Acidi Arseniosi. Liquor Potassii Arsenitis. Arsenii Iodidum. Liquor Arsenii et Hydrargyri Iodidi. Sodii Arsenias. Liquor Sodii Arseniatis. Scheele’s Green. Paris Green 142-145- Stibium. Occurrence. Tests. Antimonii Sulphidum. Antimonii Sulphi- CONTENTS. IX dum Purificatum. Antimonii Sulphuratum. Pil. Antimonii Comp. An- timonii Oxidum. Pulvis Antimonialis. Antimonii et Potassii Tartras. Syr. Scill® Comp. Vinum Antimonii. Mist. Glycyrrhiz® Comp 145-147 Bismuthum. Occurrence. Tests. Bismuthi Subcarbonas. Bismuthi Sub- nitras. Bismuthi Citras. Bismuthi et Ammonii Citras 147-149 Hydrargyrum. Occurrence. Preparation. Tests, etc. Emplastrum Am- moniaci cum Hydrargyro. Emplastrum Hydrargyri. Massa Hydrar- gyri. Unguentum Hydrargyri. Hydrargyri Chloridum Corrosivum. Hy- drargyri Chloridum Mite. Pil. Cathartic® Comp. Hydrargyri Iodidum Rubrum. Liq. Arsenii et Hydrargyri Iodidi. Hydrargyri Oxidum Ru- brum. Hydrargyri Oxidum Flavum. Oleatum Hydrargyri. Hydrar- gyri Cyanidum. Hydrargyri Subsulphas Flavus. Hydrargyrum Am- moniatum. Liq. Hydrargyri Nitratis, Ung. Hydrargyri Nitratis. Hy- drargyri Sulphidum Rubrum 149-154 PART III. Organic Pharmacy. Relations of Pharmacy to Organic Chemistry. Composition of Plants. Cassiflcation of Proximate Principles 155 THE CELLULIN GROUP. CELLULOSE. Gossypium. Cotton and Linen Fibre. Tests. Pyroxylinum. Collodium. Collodium Flexile. Collodium Stypticum. Collodium cum Cantharide. Paper. Preparation. Chart®. Parchment Paper. Ox- alic Acid 156-158 Destructive Distillation of Cellulin. Acidum Aceticum. Methylic Al- cohol. Pix Liquida. Syrupus Picis Liquid®. Oleum Picis Liquid®. Pitch. Carbo Animalis. Carbo Animalis Purificatus. Creasotum. Aqua Creasoti. Acidum Carbolicum Crudum. Acidum Carbolicum. Acidum Salicylicum. Oleum Succini. Coal. Coal Tar 159-162 Amylum. Amylum Iodatum. Glyceritum Amyli. Dextrin. Glucose. Feh- ling’s Test. Saccharum. Syrupus. Saccharum Lactis. Caramel. Mel. Mel Despumatum. Confectio Ros®. Mel Ros® 162-165 Wax. Cera Flava. Cera Alba. Ceratum 165-166 AMYLACEOUS BODIES AND THEIR DERIVATIVES. X CONTENTS. EXUDATIONS OP PLANTS. Gums. Definition. Classification. Acacia. Mucilago Acaciae. Syrupus Aca- cise. Tragacantha. Mucilago Tragacantha. Mucilagines 167-168 Gum Resins. Definition. Ammoniaeum. Asafcetida. Cambogia. Myrrha. Misturse 168-169 Resins. Definition. Natural Resins. Mastiche. Pix Burgundica. Pix Canadensis. Guaiaci Resina. Gutta Perclia. Scammonium. Arti- ficial Resins. Resina. Resina Jalapse. Resina Podophylli. Resina Scammonii. Extractum Colocynthidis Comp 170-172 Oleo-Resins. Definition. Natural Oleo-Resins. Terebinthina. Oleum Terebinthinee. Terebinthina Canadensis. Copaiba. Massa Copaibse. Derived Oleo-Resins. Preparation. Oleoresinse 172-174 Balsams. Definition. Balsamum Peruvianum. Balsamum Tolutanum. Styrax. Benzoinum. Adeps Benzoinatus. Acidum Benzoicum 174-175 Maltum. Extractum Malti 175-176 Fermentation. Various Kinds. Products. Whiskey. Brandy. Gin. Rum. Alcohol. Dilute Alcohol. Fusel Oil. Vinum Album. Vinum Album Fortior. Vinum Rubrum. Acidum Tartaricum. (Acidum Citricum.) Spiritus Vini Gallici. Spiritus Frumenti 176-180 Alcohol Decomposition Products. .Ether. Spiritus ACtheris. ASther For- tior. Spiritus AStheris Comp. Oleum ASthereum. AEther Aceticus. Spiritus AStheris Nitrosi. Amyl Nitris. Chloral. Butyl Chloral Hy- drate. Chloroformum Venale. Linimentum Chloroformi. Chioroform- um Purificatium. Mistura Chloroformi 180-185 Volatile Oils. Definition. Description. Source. Reactions. Composi- tion. Methods of Preparation. En-fleurage. Preservation. Restora- tion. Adulterations. Tests. Oils derived by the Action of Ferment. Table of Officinal Volatile Oils 185-189 Stearoptens from Volatile Oils. Camphora. (Camphor Monobromata.) Menthol. Thymol. Test 189-190 Fixed Oils and Fats. Definition. Description. Chemical Composition. SteaTin; Palmitin. Olein. Purification. Decomposition. Protection. Restoration. Preparation. Adulterations. Tests. Table of Officinal Fixed Oils and Fats 191-193 Emulsion. Definition. Theory. Emulsifying Agents. Emulsion of Cod Liver Oil 192 Saponification Derivatives. Soaps. Preparation. Soluble Soaps. In- soluble Soaps. Description. Chemical Composition. Sapo. Sapo Vi- ridis. Tinctura Sapo Viridis. Linimentum Calcis. Emplastrum Plum- bi. Glycerinum. Nitroglycerin. Acidum Oleicum. Oleates. Precipi- tated Oleates 192-196 Alkaloids. Occurrence. Composition. Solvents. Nomenclature. For- mation of Salts. General Methods of Extraction. Theory of Isolation. Opium. Opium Denarcotissatum. Assay. Extraction of Morphine. Cinchona. Assay. General tests for Alkaloids. Table of Officinal Al- kaloids 107-204 CONTENTS. XI Glucosides. Definition. Characteristics. Chrysarobinum. Elaterium. Picrotoxinum. Salicinum. Santoninum. Sodii Santoninas. Unoffici- nal Glucosides 205-206 Organic Acids. Acidum Gallicum. Acidum Tannicum. Valerianic Acid. 207 Drugs Contributed by the Animal Kingdom. Acidum Lacticum. Aci- dum Oleicum. Adeps. Oleum Adipis. Cantharis. Carbo Animalis. Cera Flava. Cera Alba. Cetaceum. Coccus. Fel Bovis. Ichthyocol- la. Moschus, Oleum Morrhuae. Pepsinum Saccharatum. Tests. Sac- charum Lactis. Sevum. Vitellus. Unofficinals. Castoreum. Gelatin. Colla. Koumiss. Pancreatin, etc 207-211 Toxicology. Poisons. Definition. Antidote. Definition. General Reme- dies. General Antidote. Classification of Poisons. Symptoms. Spec- ial Antidotes 211-213 PART IV. Urinalysis. URINE. Secretion. Collection, Retention and Excretion. Normal Urine. Description. Varieties. Urina Potus. Urina Cibi. Urina Sanguinis. Pathological Urine. Average Composition of Healthy Urine. Classifica- tion of the Study of Urine 214-217 QUALITATIVE ANALYSIS. Physical Properties. Quantity. Color. Abnormal Colors. Transparency. Odor. Specific Gravity. Reaction. Acid Fermentation. Alkaline Fermentation. Sediments 217-220 Normal Constituents. Chlorides. Sulphates. Phosphates. Urea. In- dican 220-221 Abnormal Constituents. Albumin. Heller's Test. Paraglobin or Serum Globulin. Peptone. Mucin. Glucose (Grape Sugar). Fehling’s Test. Moore's Test. Boettger’s Test. Indigo-Carmine Test. Bile (Pigment and Salts). Gmelin’s Test. Ultzmann's Test. Pettenkofer’s Test. Blood. Alemen’s Test. Heller’s Test 221-224 QUANTITATIVE ANALYSIS. Total Solids. Reaction. Acidimetry. Al- kalimetry. Sulphates. Chlorides. Phosphates. Glucose (Grape-Sugar). Urea. Fowler’s Method. Uric Acid. Albumin. Eschbach's Method. Scherer’s Method 224-230 Microscopical Examination of Urinary Deposits. Unorganized Deposits. Uric Acid. Acid Urates. Calcium Oxalate. Phosphates. Leucin and Tyrosin. Cystin 230-232 Organized Deposits. Blood Corpuscles. Epithelial Cells. Tube Casts (Blood. Hyaline. Wax. Epithelial. Granular. Oil. Mucous) 232-234 Urinary Calculi. Composition. Qualitative Analysis 234-235 Method of Recording Urinalysis 236 Special Reagents Magnesian Mixture. Solution Sodium Phosphotung- state. Solution Uranic Acetate. Solution Di-sodic Phosphate. Solution Sodium Acetate 237 Illustrations. Microscopical Urine Sediments 238-239 MANUAL OF PHARMACY AND PHARMACEUTICAL CHEMISTRY. INTRODUCTION. Pharmacy. The art or science of preparing, preserving, and compounding substances for the purposes of medicine; the profes- sion of a pharmacist. The name is also applicable to the place where medicines are compounded and dispensed. Pharmacopceia. An authorized treatise on the several kinds of medicine, and formulas for preparing them. There are in use at the present day about twenty-three different Pharmacopoeias, authorized by as many nations. The U. S. Pharmacopceia was pub- lished in 1820, and the several decennial revisions in 1830, 1842, 1851, 1868, 1873, and 1882 respectively. These revisions are con- ducted by a convention of men appointed for that purpose, by cer- tain pharmaceutical and medical bodies; other Pharmacopoeias are produced through the respective governments. Dispensatory. A commentary on one or more Pharmacopoeias, giving the history, properties, doses, etc., of officinal and unoffic- inal drugs. There are three Dispensatories published in the United States, viz.: The National Dispensatory, U. S. Dispensatory, and King’s Dispensatory (Eclectic). PART I. METROLOGY. Metrology is the determination of the bulk or extension of sub- stances (measure)-, their excess of gravitating force (weight)-, and the relation of these to each other (specific gravity and specific volume). Gravitation. The attraction existing between all masses. Weight, in any terrestrial substance, is the excess of attraction which the earth and the substance have for each other, over and above the attraction of each in opposite directions, by the various heavenly bodies. By the law of gravitation, an attraction is exerted by the sun, moon, and other planets for a body near the earth, as well as for the earth itself, and vice versa,—but on account of the rapid diminution of the force, by the increase of distance (inversely as the square of the distance), the earth’s attraction overcomes that of the heavenly bodies, and draws the body toward itself. Weighing, is the determination of the excessive attraction by the earth by comparison with a substance of known gravitating force. Accomplished by means of various instruments known as steelyards, scales, etc., all dependent upon the principle of the balance. The instruments employed by most pharmacists for weighing are called Balances. The Balance. The Knife-edges of a balance are the sharp points (made either of steel or agate) which act as bearings for the beam. They are three in number, two of which are known as Points of Suspension,—the points at each end of the beam, from which the pans are suspended; and one, the Point of Support,—the point at the middle of the beam which supports it upon the upright. The Centre of Gh'avity is in a perpendicular line extending through the point of balance. METROLOGY. 15 Conditions upon which the stability, sensibility, and accuracy of the balance depend. 1. The Centre of Gravity must be situated below the Point of Support (the central knife-edge). 2. The Centre of Gravity should be as near to the Point of Sup- port as possible. 3. The three knife-edges should be in the same plane, and their edges parallel to each other. 4. The construction of the beam should be as light as possible ; light but strong and inflexible. 5. Within limits, sensibility increases with the length of the arms. 6. Also affected by the friction between the knife-edges and planes (which in fine balances should be made of agate). 7. The Points of Suspension should be equi-distant from the Point of Support. There are four, viz.: Troy, Apothecaries’, Avoirdupois, and Metric. Troy Weight, used by jewellers. The grain and ounce were adopted by the U. S. Pharmacopoeia, 1870. Systems of Weights used in Pharmacy. 3! grains = 1 carat. 24 grains = 1 pennyweight. 20 pennyweights = 1 oz. = 480 grs. 12 ounces = 1 lb. = 5760 grs. Apothecaries’ Weight, used in the compounding of medicines. 20 grains — 1 scruple— 3. 3 scruples = 1 drachm— 3 = 60 grs. 8 drachms = 1 ounce— % = 480 grs. 12 ounces = 1 pound = 5760 grs. (Of the above denominations, all are employed in pharmacy ex- cepting the pound.) Avoirdupois Weight, used in the purchase of drugs, and for general commercial transactions; also recognized by the Br. P. 27| grains = 1 drachm. 16 drachms = 1 ounce—oz. = 437.5 grs. 16 ounces = 1 pound—lb. = 7000 grs. etc. (The oz. and lb. are the denominations usually employed.) 16 MANUAL OF PHARMACY. The only denomination common to the above three systems is the grain. Derivation of the Grain. According to a law enacted in 1266, in England, “An English penny weighed thirty-two wheat corns, taken from the midst of the ear and well-dried; twenty such pence make an ounce, and twelve ounces one pound.” Another law, enacted in 1304, reads “ that every pound of money or of med- icines is of twenty shillings’ weight, but the pound of all other things is twenty-five shillings’ weight. The ounce of medicine con- sists of twenty pence, and the pound contains twelve ounces,” etc. Liquid Measure. Medicines are measured by means of graduated conical or cylin- der glass vessels, known as graduates. Systems of measures used in pharmacy. There are three, viz.,—Liquid or Wine, Imperial or British, and Metric. Liquid or Wine Measure ; used in the U. S. 60 minims—ni = 1 fluidrachm—-f 3 . 8 fluidrachms = 1 fluidounce—-f 3 = 480 Tip 16 fluidounces = 1 pint — O = 7680 up 8 pints = 1 gallon —Cong. = 61440 up Imperial or British Measure; recognized by the British Phar- macopoeia. 60 minims—ni = 1 fluidrachm—-fl. 8 fluidrachms = 1 fluidounce—-fl = 480 up 20 fluidounces = 1 pint —O = 9600 up 8 pints = 1 gallon —Cong. — 76800 up Comparisons op Weights and Measures. Sixteen troy ozs. = 7680 grs.; sixteen Av. ozs. = 7000 grs. (680 grs. less): 16 troy ozs. = about 1TV Av. lbs. Distilled water at 60° F. (80 inches barometer). One cubic inch weighs 252.45 grs. Liquid or Wine Measure. One fluidounce weighs 455.7 grs.; one pint, 7291.2 grs.; one minim, .95 gr.; one gallon, about 8\ av. lbs.; one gallon contains 281 cu. in. Imperial Measure. One fluidounce water (under above con- ditions) weighs 437.5 grs.; one pint, 8750 grs.; one gallon, ten Av. lbs.: one minim, .91 gr. 17 METRIC SYSTEM. Terms used in referring to Domestic Measures, and their equiva- lents; viz. -. Teaspoonful = one fluidrachm ; dessertspoonful = two fl. drs. ; tablespoonful = four fl. drs. ; wineglassful = two fl. ozs. ; teacup- ful = five fl. ozs. ; tumblerful = 12 fl. ozs. The TJ. S. Pharmacopoeia recognizes no general system of weights or measures. In most cases the term parts is used, referring to weight, and applicable to any system. In a few instances (formulas for Fluid Extracts) cubic centimeters are employed to denote the amount of finished product. The gram and grain are also used in certain for- mulas (pills and troches). Problems.—1. If one pint elix. potass, bromid. contains troy ozs. of the chemical, how much in each fluidrachm ? 2. One pint elixir bromide of sodium contains 1280 grs.; how much in one fluidrachm ? 3. How much powd. coca leaves must I employ to make one pint of elixir, each fluidrachm to represent 20 grs. ? 4. One gallon of the elixir represents 11.7028 Av. ozs.; how much calisaya bark to each fluidrachm ? Testing of Graduates. With the graduate standing on a level surface, pour into it 455.7 grs. distilled water at 15.6° C. (60°F.): the liquid should measure one fluidounce. Or pour into the graduate 30 cm3 of water, which is the equivalent to a fluid- ounce. METRIC SYSTEM. The Metric System of Weights and Measures is based upon the decimal system, the various denominations increasing and decreas- ing by tenths. Its use is legalized in America and England, and made obligatory by all other governments of the civilized world. The unit or standard is the Meter (/.terpor, a measure), which is the unit of linear measure, and represents nnnunnnj of a quadrant of the earth’s polar circumference, equivalent to 39.37 English inches. The Oram is the unit of weight; the Liter of capacity (although the cubic centimeter is oftener and more desirably used); the Are, of surface measure. The denominations representing the subdivisions of any unit are expressed by prefixing the Latin numer- als deci, centi, and milli to the unit, meaning respectively one tenth, one hundredth, and one thousandth; the multiples are expressed by 18 MANUAL OF PHARMACY. prefixing the Greek numerals, deka, hecto, kilo, and myria, meaning ten, hundred, thousand, and ten thousand. 10,000.000—Myra—(M.) 1000.000—Kilo—(K.) 100.000—Hecto-(H.) 10.000—Deka—(D.) 1.000—Unit (Meter, Gram, Liter, Are). .1—Deci—(d.) .01—Centi—(c.) .001—Milli—(m.) Comparison of the Value of the Several Denominations. Derivation of the Are. The square of ten meters (one Deka- meter), representing one square Hecto-meter=100 m2. Derivation of the Gh'am. The meter is divided into one hundred equal parts, called centi-meters; upon one centi-metre as a base, a cube is erected having for its three dimensions, one c. m. each; the contents of this cube will be one cubic-centimeter (cm3), meas- uring one milli-liter. This quantity of distilled water at its maxi- mum density (4° C. = 39.2° F.) and 30 inches barometric pressure, weighs one gram = 15.432 grains. # Derivation of the Liter. The meter is divided into tenths, called deci-meters. If a cube is erected, having a deci-meter for each of its three dimensions, its contents will be (1 X 1 X 1 = 1 dm3) one cubic deci-meter (dm3); the capacity of which is one Liter. One Liter = 1000 cm3 = 33.81/§ = 2.113 pints. One liter of distilled water at 4° C. (30 in. barometer) weighs 1000 grams = 1 kilo-gram = 15432 grains = 2.2 lbs av. Abbreviations. The term Kilo, refers to kilogram; while cm3, or c.c. are used to express cubic centimeters. To convert metric weights into other systems: Reduce to grains by multiplying the number of grams by 15.432 and divide by the number of grains in the denomination of the system required. To convert metric measures into other systems : Find the number of cm3, multiply by 15.432, and divide by the number of grains of water in the denomination of the system required. To convert weights of other systems into metric weights: Reduce to grains and divide by 15.432 ; the quotient will represent the num- ber of grams. METRIC SYSTEM. 19 To convert measures of other systems into metric measures : Re- duce to grains (as though water were referred to), and divide by 15.432 ; the quotient will represent the number of cm3. In writing the various metric denominations, it is advised to sub- stitute the decimal point by a perpendicular line, and thereby avoid possible errors in placing the point. For example. « Pulv. Aloes 9 74 Polv. Myrrhce 6 50 Pulv. Bhei 18 00 01. Mentbee pip 0 65 Misce fiant pilules No. 100. R Chloralis 8 00 Potass. Bromidi 12 00 Syr. Zingiberis 32 00 Syrupi 96 00 Misce fiat mistura, etc. In the above there can be no mistaking of the quantities desired, as all solids are weighed, and all liquids measured; gram being the unit of weight, and the cubic-centimeter of measure. Examples to test the knowledge of the student, on writing and convert- ing the metric system into other systems: How many c. m. in 1 D. m. ? D. m. in 1 K. m. ? c. g.in 1 d. g. ? c. g. in 1 H. g. ? D. g. in 1 Kilo ? m. 1. in 1 D. 1. ? H. 1. in 1 M.l. ? g. in 1 H. g. ? c. g. in 1 D. g. ? etc. 1. What is the cost of 18425 grams tartaric acid at $1.00 per Kilo. ? Ans. $18,425. 2. Cost of 425 grams zinc sulphate at 33£ cents per Kilo. ? Ans. $0.14+. 3. Cost of 7500 grams potassium chlorate at 50 cents per Kilo. ? 4. Cost of 6218 grams potassium bromide at $1.40 per Kilo. ? 5. Cost of lbs. alum at 22 cents per Kilo. ? 6. Cost of 150 Kilos, iodine at $2.75 per lb? Ans. $907.50. 7. Cost of 60 Kilos, citric acid at 3£ cents per oz. ? 8. Cost of 25 grams quinine at $1.10 per oz. ? 9. How many grams in 42 troy ozs. ? 10. How many inches in 25 meters? 11. How many f § in 1 liter? 12. How many grams in 1 Av. oz. ? 13. How many Av. lbs. in 2000 grams? 14. Cost of 1 liter at $1.25 per d. 1. ? Ans. $12.50. 15. Two casks hold respectively 136 and 125 liters of water; what is the weight of water that both will hold ? Ans. 261 Kilos. 16. From 735 c. m. subtract 3 m. 86 c. m. ? Ans. 3 m. 49 c. m. 17. From 9 m. 8 m. m. subtract 57 c. m. ? Ans. 8 m. 51 c. m. 20 MANUAL OF PHARMACY. 18. a. Wishing to find the capacity of a bottle, I weigh it (having no measure); its weight is 520 grams ; filled with water it weighs 1 K. 810 grams; what is its capacity? Ans. 1 K. 290 grams. b. How many fi. ozs. ? Am. 43 f 5 312.18 grs.—or 43 f § . 5.28 f 3 . 19. Add 43 H. g., 25 K. g., 27 c. g., 3204 m. g., 68 D. g., 27| g., and 52| D. g. Am. 30538.474. Work. 43 Hecto grams, 4300 25 Kilos., 25000 27 Centi grams, 27 3204 Milli-grams, 3 204 68 Deka-grams, 680 27i Grams, 27 5 52f Deka grams, 527 5 "30538 474 Ans. 30 Kilos 538 grams 474 milligrams, or 30,538 grams 474 milligrams. Note.—In reading of denominations of weight, always give the number of grams; then follow with the fraction, reading it as so many of the loivest denom- ination; or mention the number of Kilos., then the remaining grams, and the number of the lowest denomination. 20. Add 225 c. g., 83 d. g., 10002 m. g., 250 grams, 2| D. g., 183 K. g., 19 H. g., 205 m. g. Ans. 185195.757. 21. Add 27£ grams, 438 c. g., 2786 D. g., 3487| c. g., 42£ K. g., 235 d. g., 324 M. g., 8f K. g., 16 m. g., 84 d. g., 23i H. g., and give answer in av. lbs., ozs., and grs., using three decimal places throughout (1 gram = 15.4 grs.). Ans. 894 lbs., 5 ozs., 374 grs. 22. Add 425 D. g., 8£ K. g., 3f M. g., 825 d. g., 460 m. g., 18 grams. Ans. 50350.960. 23. Add 54 d. g., 10 D. g., 4 c. g., 14 K. g., 7 M. g., 2638 d. g., 5 m. g., 18f grams, 42£ D. g., 10 M. g., 26 m. g. Ans. 184813.021. 24. Add 5 K. g., |H. g., 5 M. g., 500 grams, 50 d. g., c. g., 5 m. g., 5 c. g. Am. 25. Add )M. g., 50 H. g., 5 K. g., 500 D. g., 5000 grams, 50 c. g., i d. g., 5 m. g. Ans. 25000.555. 26. Add 210 d. g., 42 D. g., 6 m. g., 456 c. g., 4368 m. g., 22 H. g., 3i M. g., 6J grams, 248 d. g., 86 m. g., 43 grams, and reduce to Troy ozs. and grs. 27. I have ten vessels filled with water, which hold respectively 265 d. g., 44 m. g., 235 c. g., 45 D. g., 266K, g., 18| grams, 525d. g.. 21 SPECIFIC GRAVITY. 3002 grams, 46 d. g., 25638 m. g.; how many pints are represented by the whole? Ans. 570.57 pts. SPECIFIC GRAVITY. Specific Gravity is the relation of weight to volume; or, the weight of a substance, as compared to the weight of an equal volume of another substance, taken as a unit. Unit. The unit for the specific gravity of all solids and liquids is distilled water at 60° F. and BO inches barometric pressure ; for gases, either hydrogen or air is taken as the unit. The specific gravity of U. S. P. officinals is taken at 59° F. (with a few exceptions) in order to avoid fractions in the Centigrade equiv- alent; 59° F.=r 15° C., while 60".F. = 15.6° C. The principle for determining specific gravity was discovered by Archimedes, the philosopher. King Hiero, of Syracuse, having or- dered a golden crown made, suspected its purity when completed, and demanded that Archimedes should test it. The latter, after many unsuccessful attempts, wTas about to give up in despair, when one day, while taking his bath, he observed that, the deeper his body became immersed, the greater the quantity of water that overflowed the sides of the tub, showing that he displaced an equal volume of water. He rushed through the streets, naked, shouting “Eureka! Eureka!” and procuring a piece of pure gold of the same weight as the crown, compared the specific gravities of the two, when the latter was found deficient. Laws on which Specific Gravity is Based. 1. Fluids buoy up all solids with a force equal to the weight of liquid displaced. 2. Floating bodies displace their weight of liquid; immersed bodies their bulk. Methods for the Determination of Specific Gravity. 1. Hydrostatic Balance (for solids only). 2. Specific Gravity Bottle {solids and liquids). 3. Loaded Cylinder (for liquids only). 4. Hydro- meter (for liquids only). Hydrostatic Balance. The Hydrostatic Balance is merely an accurate prescription balance, so arranged that one of the pans is suspended by shorter cords, and has a hook attached from the bottom, from which a sub- stance may be attached by means of horse-hair or a piece of thread, for the purpose of weighing the substance in water. 22 MANUAL OF PHARMACY. Methods of use. I. For solids insoluble in, and heavier than, water. Determine the weight of the substance in air; immerse it in water and again note its weight; the difference between these two weights (i.e., its loss of weight in water) represents the weight of liquid displaced, or the weight of an equal volume of water. Hav- ing the weight of the substance, and the weight of an equal volume of water, a comparison represents the sp. gr.—; water being the unit, we divide the weight in air by the weight of an equal hulk of water, the quotient representing the sp. gr. II. For solids soluble in, and heavier than, water. Weigh the sub- stance in air, and again in some liquid of known sp. gr., in which it is insoluble; the difference represents the weight of an equal volume of the liquid used. On dividing this into the weight in air, the quotient multiplied by the specific gravity of the liquid used gives the sp. gr. of the substance. Example 28. A piece of lead weighs in air 228 grs., in water 208 grs.; what is its sp. gr.? 228 — 208 = 20 ; 228 -e 20 = 11.4, Ans. The above losec in weight in water 228 — 208 = 20 grs.; hence, 20 grs. is the weight of an equal bulk of water; 228 grs. representing the weight of the lead—then 228 -e 20 = the sp. gr. or 11.4. {Note: The Rule of Three facilitates calculations in Specific Gravity, but is recommended by the author only to be used for rapid calculat- ing, after the student has become thoroughly conversant with the prin- ciples of sp. gr. In all cases the weight of liquid displaced is the first term, the weight in air the second term, and the specific gravity of the liquid used the third term; thus 20 : 228:: 1.000 : x = 11.4. Ex. 29. A nail weighs in air 50 grs., in water 43 grs.; what is its sp. gr.? Ans. 7.14. 30. A piece of gold weighs 700 grs., in water 664 grs.; what is its sp. gr;? Ans. 19.4. 31. A piece of copper weighs 360 grs. in air, in water 320 grs.; what is its sp. gr.? Ans. 9. 32. A silver chain weighs 848 grs., in water it weighs 768 grs.; what is its sp. gr.? Ans. 10.6. 33. A platinum crucible weighs 749 grs., in water it weighs 714 grs.; what is its sp. gr.? Ans. 21.4. 34. A piece of phosphorus weighs 45f grs., in air, in water 20£ grs.; whatisitssp.gr.? Ans. 1.83. 35. A solid, soluble in water, weighs in air 680 grs., in ether (s. g. .750) 540 grs.; what is itssp. gr.? 680 — 540 = 140 ; 680-el40 — SPECIFIC GRAVITY. 23 4.85 X .750 = 3.63, Ans. (The loss of weight in ether is 680 — 540 = 140 grs., which represents the weight of an equal bulk of ether. 680-h140 = 4.85 = sp. gr. as compared to ether for a unit, but as ether is only .750 as heavy as water, we will have to multiply by .750 in order to make the answer compare to water as the unit. 4.85 X .750 = 3.63, Ans. 36. Weight of a solid in air is 845 grs., in benzine (s. g. 0.835) 795 grs.; what is sp. gr.? Ans. 14.11. 37. Weight of apiece of alum 124 grs., in oil of turpentine (sp. gr. 0.872) 62 grs.; what is sp. gr.? Ans. 1.74. 38. Weight in air 1250 grs., in ether fortior (sp. gr. .725) 1200 grs.; what is sp. gr.? 1250 — 1200 = 50; 50 : 1250 :: 0.725 : x = 18.125, Ans. 39. A lump of sugar weighing 100 grs. was found to weigh when immersed in oil of turpentine (sp. gr. 0.87) 45.62 grs. What is its sp. gr.? 40. A piece of sodium chloride weighs 450 grs.; in alcohol (sp. gr. 0.820) 375 grs. What is its sp. gr.? Ans. 4.92. III. For solids lighter than, and insoluble in water. As a floating body displaces its own weight of water, it is necessary to attach a heavy body to immerse it, before we can arrive at the weight of an equal volume of water. Consequently it becomes necessary to attach a heavy body sufficiently large to sink the lighter, to one arm of the balance, and counterpoise it; to the cord from which it is suspended, the light body is attached, which, on account of the buoyant power of the water, raises the heavy weight; now the weight required to restore the equilibrium of the balance must be added to the weight in air, the sum representing the weight of an equal bulk of water ; on dividing the weight in air by this weight, the sp. gr. is attained. Ex. 41. A piece of wax weighs in air 240 grs. For a sinker I use a nail weighing in water 86 grs.; the wax and nail weigh in water 76 grs.; what is the sp. gr. of the wax ? 86 — 76 = 10; 240 —f- 10 = 250; 240 250 = 0.96. If the wax had been placed in water without the nail attached, it would have displaced 240 grs. of water; but by attaching to the nail it is wholly immersed, and displaces 86 — 76 = 10 grs. more water ; then 240 + 10 = 250 grs., is the weight of an equal volume of water ; or, 250 : 240 :: 1.000 x = 0.96. 42. A piece of cork weighs 154 grs. ; I use a sinker weighing 921 grs. in water ; the cork and sinker weigh together in water 425 grs. What is the sp. gr.? 921 — 425 = 496 4- 154 = 650 grs., weight of an equal volume of water; 154 -4-650 = 0.236, sp. gr. 24 MANUAL OF PHARMACY. 43. Weight of wax in air 2334 grs. A sinker is counterpoised in water and the wax attached, when it requires an addition of 75 grs. to overcome the buoyant power of the wax. What is its sp. gr.? Ans. 0.969. 44. A light substance weighs 120 grs. in air ; being attached to a piece of lead and weighed in water, the united weight is 40 grs., while the lead alone in water shows 50 grs. What is its sp. gr.? 45. A sample of wax weighs 300 grs.; on attaching to a piece of copper counterpoised in water, the two combined lose 7 grs. in weight. What is the sp. gr. of wax ? 46. One cubic inch of cork weighs 60.6 grs. What is its sp, gr.? IV. For solids lighter than, and soluble in water. Proceed as in the previous method, using a liquid that is not a solvent for the sub- stance, and multiply the result by the sp. gr. of the liquid. Ex. 47. A piece of potassium weighs in air 200 grs.; a lead sinker weighs in petroleum (sp. gr. 0.75), 350 grs. ; with the potassium attached their combined weight in water is 347.6 grs. What is the sp. gr. of the potassium? 350 — 347.6 = 2.4 + 200 = 202.4 ; 200 202.4 = .988 X .75 = .741, Ans.-, or 202.4 : 200 :: .75 : x = .741. Specific Gravity Bottle. I. For Liquids. Perhaps the simplest and best method of taking the sp, gr. of liquids is the Specific Gravity Bottle. It generally consists of a flat bottom globular flask with slender neck, on which a mark is placed to indicate the level of a liquid; in some cases the neck is accurately fitted with a perforated glass stopper. A coun- terpoise of the exact weight of the flask accompanies it. The flask may hold exactly 100 or 1000 grs. of distilled water at 15.6° C. Determination of the Specific Gravity of a Liquid. Fill the flask to the mark on its neck with the liquid, and weigh the contents, using the counterpoise to represent the tare of the bottle. This weight divided by 100 or 1000 will give the sp. gr. of the liquid, since the same volume of water weighs 100 or 1000 grs. according to the flask used : i.e., divide the weight of the contents by the weight of an equal bulk of water. Ex. A 1000-gr. flask will hold 1420 grs. of ni- tric acid, which at once shows the specific gravity, viz.: 1420 -j- 1000 = 1.420. Care of Specific Gravity Bottles. Should be wiped dry to remove adhering moisture ; and handled as little as possible while contain- ing the liquid under operation, to prevent change of temperature. SPECIFIC GRAVITY. 25 An ordinary prescription bottle may be used for the same pur- pose as a specific gravity flask, by first weighing and making a counterpoise ; it is then filled with distilled water at 15.6°C. (60° F.), the level of the liquid marked, and the weight of its contents noted. The sp. gr. of any liquid may be readily determined by fill- ing the bottle with it, and weighing. This latter weight divided by the weight of water will show the sp. gr. Ex. A bottle holds 525 grs. water; the same bottle holds 609 grs. of hydrochloric acid ; then 609 -4- 525 = the sp. gr. 1.160. Ex. 48. A bottle holds 1250 grs. of water; the same bottle holds 1332.85 grs. dilute sulphuric acid. What is its sp. gr.? 1332.85 -r- 1250 = 1.066, Am.-, or 1250 : 1332.85 :: 1.000 : x = 1.066. 49. A bottle holding one fl. oz., holds 569.6 grains of glycerin or 373.67 grs. alcohol; or 330.38 grs. stronger ether; or 838.49 grs. sulphuric acid; or 1353.43 grs. bromine. What is sp. gr. of each? 50. A bottle holding one cubic inch, when filled with aqua ammo- nia contains 242.10 grs. What is its sp. gr.? 51. A bottle that will hold 500 grs. of water, when filled with mercury weighs 6750 grs. What is its sp. gr.? 52. A one-liter flask holds 1840 grams of sulphuric acid ; what is the sp. gr.? II. For Solids (in the form of a powder). Weigh the powder, and place in a counterpoised flask of known capacity; add a small quan- tity of distilled water, and shake to remove air-bubbles; then fill the flask with water to the established mark on the neck, and weigh again. From the combined weight of water and substance, subtract the amount due to the substance; the difference represents the weight of water in the flask. Subtract this weight from the weight of water the bottle originally held, and the difference represents the weight of water that the bulk of the powder now occupies, or the weight of an equal bulk of water. Having the weight in air, and the weight of an equal bulk of water, dividing the former by the latter gives the sp. gr. If the powder is soluble in water, use a liquid of known sp. gr. in which it is not soluble, and proceed as above, and multiply the re- sult by the sp. gr. of the liquid. Ex. 53. A powder weighing 360 grs. is placed in a flask (which holds 1000 grs. of water), and the latter is filled with water ; the combined weight of powder and water is 1260 grs. What is the sp. gr. of the powder ? 1260 grs. (weight of powder and water) less 360 26 MANUAL OF PHARMACY. grs. (weight of powder) = 900 grs. (weight of water in flask); 1000 grs. (quantity of water the flask will hold) less 900 grs. = 100 grs. (weight of an equal bulk of water); 360 -+- 100 = 3.6, Am.; or 100 : 360 :: 1000 : x = 3.6 54. 200 grs. of calomel is placed in a fiask (1050 grs. water capac- ity) and the latter filled with water; the combined weight is 1223 grs. What is the sp. gr.? 1223 — 200 = 1023 grs. (water in flask); 1050 - 1023 = 27 grs.; 200 -s- 27 = 7.4, Ans. 55. Powd. silver weighs 105 grs.; bottle holds 300 grs. water ; sil- ver and water, when bottle is filled, weigh 395 grs. What is sp. gr.? 56. A powder weighs 300 grs.; placed in a 5000 gr. flask, and filled with water, the combined weight of powder and water is 5250 grs. What is the sp. gr.? 57. One troy oz. powder, placed in a 1250 gr. flask and filled with water; the combined weight of powder and water is 1575 grs. What is the sp. gr.? 58. Calomel 100 grams is placed in a one-liter flask, and the latter filled with water; contents of flask weighs 1086 grams. What is the sp. gr.? The Loaded Cylinder. The Loaded Cylinder is used for determining the specific gravity of dense viscid liquids—such as balsams, oils, etc.—that are not easily removed from hydrometers or sp. gr. bottles, which are constructed of thin glass, and easily fractured. Construction. Merely a rod of glass, or some metal that will sink in the liquid. It displaces its own bulk of the liquid. Use. 1. Weigh the cylinder in air, then in water, and note the loss, which is the weight of an equal volume of water. 2. Weigh in the liquid under consideration and again note the loss, which rep- resents the weight of an equal volume of the liquid. 3. Having the weights of equal volumes of water and the liquid under considera- tion, divide the latter weight by the former. Ex. 59. A glass rod weighs in air 57 grs.; in water 35.5 grs.; in oil 39 grs. Sp. gr. of latter? 57 less 35.5 =21.5 (weight of equal vol- ume of water); 57 less 39 = 18 (weight of equal volume of oil); 18 21.5= 0.837, Am.; or, 21.5 : 18 :: 1.000 : * = 0.837. 60. Cylinder weighs 80 grs.; in water 61 grs.; in solution chloride calcium 52 grs. Sp. gr. of solution ? 61. Glass rod weighs 100 grs.; in water 91 grs.; in sulphuric acid 84.44 grs. Sp. gr. of acid? SPECIFIC GRAVITY. 27 62. Glass rod weighs 200 grs.; in water 180 grs.; in glycerin 175 grs. Sp. gr. of glycerin ? 63. Glass stopper loses by immersion in water J71 grs.; in another liquid 143 grs. Sp. gr. of latter ? 64. Loaded cylinder weighs 200 grs.; in water 140 grs.; in SDlution chlor. zinc 106.7 grs. Sp. gr.of latter? Construction. A glass tube with a graduated stem, having a bulb at the lower end, loaded with mercury or small shot, to keep the instrument in an upright position. Principle. Floating bodies displace their own weight of a liquid; therefore, the volume of liquid displaced weighs as much as the whole instrument; consequently, the lower the sp. gr. of the liquid, the deeper will the hydrometer sink. Graduation. The point to which the instrument sinks in water at 60° F. is called 1.000 or 1000. It is then placed in a heavy or light liquid of known sp. gr., the corresponding point of immersion marked on the stem, and the interspace equally subdivided. The point to which the instrument sinks in the liquid indicates the sp. gr. It is seldom that a hydrometer is graduated for liquids both lighter and heavier than water, as the instrument would be on the one hand either long and cumbersome, or on the other hand the grad- uations would be close and indistinct. For this reason, we have in general two kinds of instruments: 1. For liquids lighter than water, with the water-mark low down on the stem. 2. For liquids heavier than water, with the water-mark near the top of the stem. For special uses, hydrometers are made, having only a portion of the graduated scale on either of the above; or having arbitrary scales of graduations,—such as the Alcohometer, Lactometer, Urinometer, Saccharometer, Acidometer, Barkometer, and Elaeometer., etc. Arbitrary Graduations. Baume’s, Trade’s, Cartier’s, Twadell’s, all of which should be avoided, and are being rapidly replaced by the Specific Gravity scale. Baume’s hydrometers, which were the first of these peculiarly graduated instruments, may answer as a type. 1. Pese-Esprit, for liquids lighter than water. The point to which the instrument was immersed in a 10$ salt solution was marked 0°, Hydrometer (for liquids only). 28 MANUAL OF PHARMACY. and the point at which it rested in water was called 10°, and the intervening space equally subdivided. 2. Pese Sirop or Pese Acide, for liquids heavier than water. The points at which the instrument rested in water and a 15% salt solu- tion, were respectively marked 0° and 15°—and uniformly graduated between these points. Rules for converting Beaume Degrees to Sp. Or. Scale, and vice versa. 1 For heavy liquids. B° to S. G. = i45~Z~B°: S- G- t0 B° = 145 ~ 2. For light liquids. B°t0 s-G- = sftW s- g- t0 B° = on - 130- Reading' of Hydrometers. These instruments are constructed to be read from above the surface (i.e., the top of the meniscus), be- cause they are often used with colored and opaque liquids which prevent reading from below. [Meniscus: the tendency of all liquids (excepting mercury) to adhere to the sides of a vessel, due to capillary attraction, produces a semi-circular surface in narrow ves- sels, called a meniscus.] Ex. 65. A hydrometer weighing 300 grs. sinks to a certain point in water; how much must it weigh to sink to the same point in glycerin (sp. gr. 1.250)? 300 X 1.250 = 375 grs.; or, 1.000 : 1.250 :: 300 : x = 375. Explanation: Since the hydrometer displaces its own weight of any liquid, the above instrument displaces 300 grs. of water; in order to displace the same volume, or 375 grs., of glycerin (this liquid being as heavy as water, and X 300 = 375) it must weigh 375 grs. From .the above facts we deduce the following principle : The weights of equal volumes are to each other as the sp. gr. of the liquids. Rule. Multiply the weight of the hydrometer by the sp. gr. of the liquids. 66. How much should a hydrometer (weighing 100 grs.) weigh, to sink to same point in sulphuric acid (1.840) as it does in water? 67. A hydrometer weighs 500 grs. It sinks in water to a certain point, how much should it weigh to sink to the same point in stronger water of ammonia (0.900)? 68. Hydrometer weighs 250 grs. It rests at a certain point in SPECIFIC GRAVITY. 29 water ; how much weight must be added to cause it to rest at the same point in nitric acid (1.420)? 69. A hydrometer displaces 375 grs. of water ; how much stronger ether (0.725) will it displace? and how much sulphuric acid? Determination of Specific Gravity, Weight or Volume, when two of the factors are given. - I. Weight and Measure given, to find Specific Gravity. Divide the weight given, expressed in grains, by the weight of an equal bulk of W water-, or S. G. = -y-. Ex. 70. 44 troy ozs. of a liquid measure 32 fl. ozs.; what is its sp. gr.? Ans. 1.448. 44 troy ozs. =21120 grs.; 32 fl. ozs. water weighs (32 X 455.7) 14582.4 grs. If the same quantity of the liquid weighs 21120 grs. then its sp. gr. is (21120 -h 14582.4) 1.448. 71. 16 troy ozs. measure 14 fl. ozs.; what is the sp. gr.? 72. One Imperial fluid oz. of a liquid weighs 366| grs.; what is its sp. gr.? 73. 1 liter sulphuric acid weighs 28394.88 grs.; what is its sp. gr.? 74. Equal volumes of benzol (sp. gr. 0.850) and glycerin weigh 34 and 49 parts respectively ; what is the sp. gr. of glycerin ? Ans. 1.225. II. Measure and Specific Gravity given, to find Weight. Multiply the weight of an equal volume of water by the sp. gr. and the result rep- resents the number of grains ; or, W = V X S.G. Ex. 75. How many Av. ozs. will one pint glycerin (1.250) weigh ? 1 pint of water weighs 7291.2 grs. X 1.250 = 9114 grs.; 9114-t- 437.5 = 20.83 ozs., Ans. 76. What will 2 pints ether (0.750) weigh, in troy ozs.? 77. What will 20 fl. ozs. of a liq. (0.835) weigh in grams ? 78. How many Av. lbs. and ozs. will 1 gal. Monsel’s solution (1.555) weigh ? 79. What will 500 cm3 of nitric acid (1.420) weigh? 710 grams. 80. What will 10 L. ether (0.725) weigh in Kilos.? 81. How many grains will 250 cm3 of nitric acid weigh? III. Weight and Specific Gravity given, to find Measure : Divide the weight (in grains) by the sp. gr.;- the quotient represents the weight W in grains of an equal volume of water, or V = 5-= . D. U. Ex. 82. Measure of 20 troy ozs. of sulphuric acid (1.840) in fl. ozs.? Ans. 11.448 fl. ozs. 30 MANUAL OF PHARMACY. 20 troy ozs. = 9600 grs. 1.840 — 5217. 3 grs. = weight of an equal volume of water. 5217.3 -s- 455.7 = 11.448 11 ozs. 83. Measure (fl. ozs.) of 18 Av. ozs. glycerin (1.250)? 84. Measure (fl. drachms) 20 troy ozs. nitric acid (1.420)? 85. Measure (cm3 and liters) 12 Kilos of a liquid (1.200)? 86. Measure (fl. ozs. and grs.) of 7291.2grs. of hydrochloric acid? Specific Volume, or Comparative Volume, is the relation of volume to weight; that is, the volume of a liquid as compared with another liquid of equal weight used as standard. Unit or Standard. Distilled water at 15.6° C. (60° F.), 30 inches barometer. Theorem. The volumes of equal weights of two liquids are to each other inversely as the specific gravity of the liquids. Explanation. To arrive at this explanation, we will return to a theorem in specific gravity for our introduction. Suppose we have before us two vessels, of one quart capacity each, and place a pint of water in the one, and the same quantity of glycerin in the other; we have now equal volumes of the two liquids ; and if we represent the weight of the water as 1, the relative weight of the glycerin is 1£ the sp. gr., showing the latter to be 1.250 times as heavy as water, —hence the weights of equal volumes are to each other as the sp. gr. of the liquids. But now, to reverse the above, let us again return to the two vessels containing one pint each of water and glycerin. Their volumes, being equal, are represented by the ratio 1 : 1, or 1000 : 1000; but we have unequal weights, as glycerin is 1.250 or 1£ times as heavy as water, and in order to have equal weights of both liquids, we must add 1 pint of water to the pint already in the vessel, mak- ing the bulk of water 1£ times that of the glycerin ; now if we rep- resent the volume of glycerin as 1000; the comparative volume of water will be represented by 1250, or their ratio as 1000 : 1250 ; there- fore the volume of glycerin will be as great as that of the water, and hence the axiom: The volumes of equal weights are to each other inversely as the sp.gr. of the liquids. Ex. 87. What is the specific volume of ether (.750)? Ans. 1.33 0.750 : 1.000 :: 1 : x = 1.33, or = 1.33 88. A hydrometer displaces a definite quantity of water; what will be the comparative volume displaced by sulphuric acid (1.840)? Ans. .54 1840 : 1000 :: 1 : x, or = .54 SPECIFIC VOLUME. CALCULATIONS. 31 89. The portion of a glass tube immersed in water is represented by one half its length; what portion of its length will be immersed in nitric acid (1.420)? of .5 — .35 or 1.420: 1.000 :: .5: x = .35 90. Three fourths of a tube is immersed in alcohol (.820); what portion will be immersed in glycerin (1.250)? 91. A hydrometer weighing 650 grs. has six tenths of its length immersed in chloroform (1.490); what portion will be immersed in hydrochloric acid? What is the weight of hydrochloric acid dis- placed ? Formula for Determining the Quantities to be employed, in Mixing Drugs of unlike Percentage Strength, or dif- ferent Specific Gravities, when a mixture of Definite Strength or Specific Gravity is desired. Example. A pharmacist having on hand water of ammonia of 4% and 24$ strength, wishes to mix them, to make a mixture that shall contain 16$ of ammonia; what proportions of each shall he employ? Ans. 8 parts of 4$, and 12 parts of 24$. Method. 16 | jjjj Proof.jJ 20 lbs. mixture 320 lbs. at 1% = 16)320 20 lbs. at 16$. Explanation. The gain and loss of the percentage strength of the two solutions, as compared with the mean percentage, must bal- ance. Hence we compare a percentage less than the mean, with one greater—4$ with 24$. On every part of 4% water of ammonia employed to make the 16% mixture, there is a gain of 12% ; and on every part of 24% used in the 16% mixture, there is a loss of 8$ of ammonia. Therefore, as the gain and loss on equal parts of each are to each other as 12 to 8, we must take parts that are to each other as 8 to 12. Rule. 1. Write the values in a column, and the mean value on the left. Link the ingredients in pairs, one less than the mean with one greater; and take the difference between the mean and the numbers representing the percentage strength of each ingredient, and write it opposite the value with which it is linked. These differences are the relative quantities of the ingredients taken in the order in which their values stand. 32 MANUAL OF PHARMACY. 2. If the quantity of one ingredient is given; to find the cor responding quantities of the others, multiply their differences by the ratio of the given quantity to the difference of the ingredient it rep- resents. 3. If the quantity of the mixture is given ; to find the quan- tity of the ingredients, multiply their differences by the ratio of the given quantity to the sum of the differences. Example. In what proportions must powd. opium, of 8, 10, 15, and 16% morphine strength he taken, to make a mixture of 14% strength? Ans. 2, 1, 4, and 6 parts respectively; or 1, 2, 6, 4. (No. 1.) (No. 2.) f 8 2 r 8—1 1 14 101 14 ) 15J 1 4 i4 J10—n2 141 15 1 6 ll6 6 116 4 Proof No. 1. Proof No. 2. 2 X 8 = 16 1X8= 8 1 X 10 = 10 2 X 10 = 20 4 X 15 = 60 6 X 15 = 90 6 X 16 = 96 4 X 16 = 64 13 13)182 13 13)182 14 14 Example. Having powd. opium containing 7, 8, 9, 12, 16, and 20% morphine ; how shall I mix them to produce a 14% product ? 7 6 8 2 14 9 j 2 14121 2 16UL 6 + 5 + 2 = 13 20 7 6 X 7 = 42 2 X 8 = 16 2 X 9 = 18 2 X 12 = 24 13 X 16 = 208 7 X 20 = 140 32 32)448 14 Example. A pharmacist desires some powd. opium containing 12% morphine; how much shall he use each of 6, 8, 10, 13, 14, and 18% powder? Ans. 6, 2, 1, 2, 4, and 6 respectively. Example. It is desired to dilute stronger water of ammonia (28%) to make a 10% water of ammonia; what proportions shall I use 7 Ans. 10 parts of 28% sol.; 18 parts of water. 10 | Water is represented by 0. Example. How shall I mix powd. opium (14$ morphine) with milk sugar, to make a uniform mixture containing 12% morphine? Ans. 12 parts of powd. opium, and 2 parts milk sugar. Example. A drug-broker wishes to mix 500 lbs. of powd. jalap CALCULATIONS. 33 containing 14# resin, with lots containing 9# and 11# to make a mix- ture containing 12.5#. How many pounds must he use of each lot? 14T" 1.5 -f- 8.5 = 5 500 12.5 9J 1.5 cnn . r _ inn 1.5X100 = 150 11_ 1.5 500 5 _ 100 15 x 1Q0 _ igQ Example. How many ounces of resins of scammony containing respectively 85, 90, and 92# of resin, must be mixed with 54 ozs. as- saying 75# resin, to form a mixture that will test 80# ? Ans. 10 ozs. of each. Example. How many grams each of powdered opium, assaying respectively 9, 10, 12, 16, and 18# morphine, must be used to make a mixture of 100 grams that will contain 14# morphine? Ans. 21.052 grams, 9#; 10.526 grams, 10#; 10.526 grams, 12#; 31.578 grams, 16# ; and 26.315 grams, 18#. 9 4 4 X 5.263 = 21.052 grams. 10— 2 2 X “ = 10.526 “ 1412-1 2 2 X “ = 10.526 “ 16i_ 4 + 2= 6 X “ = 31.578 “ 18 5 5 X “ = 26.315 “ 19)100 99.997 grams. 5.263 Example. I desire to produce 240 gallons of bay-rum containing 60# alcohol, by mixing several lots containing respectively 70, 62, 58, and 50# alcohol; how much of each shall I use? Ans. '100 gals, of 70#, 20 gals, of 62#, 20 gals, of 58#, and 100 gals, of 50#. Example. 100 ozs. of a lot of tincture nux vomica assays 2£# of extract, how much alcohol shall 1 mix with it to produce the of- ficinal tincture (2# extract)? Ans. 25 ozs. Example. Wishing to make 5 lbs. solution of soda sp. gr. 1.120, and having on hand a solution, sp. gr. 1.400—how much water must I use to produce the quantity of the sp. gr. desired ? Ans. 1 lb. 1.400-1.12 X 12.5 = 1.5 lbs. 1.120 1.000J.28 X 12.5 = 3.5 lbs. ■ 40) 5 0 uTo lbs. 12.5 Example. How much glycerin shall I mix with water to make 25 lbs. of a solution, sp. gr. 1.160? Ans. 16 lbs. 34 MANUAL OF PHARMACY. Collection, Preparation and Preservation of Botanical Drugs. Division of the plant into parts for the use of the pharmacist. Root, stem, pith, bark, buds, leaves, flowers, fruit and seed. Each part requires the observance of special rules, regarding its collec- tion, desiccation and preservation for medicinal uses. Time for General Collection. At that period of the plant’s growth, when the peculiar juices are most abundant in the portion desired. Collection of Special Parts. Roots. Of annual plants, should be collected just before the flower forms. Of biennials, late in the autumn of the first year or very early in the spring of the second year. Of perennials, immedi- ately after the first appearance of the plant above ground. Stem. Of herbaceous plants, should be collected after foliation, but before floration. Bark. Of trees, should be collected in the spring-, of shrubs, in the autumn, at which seasons they can be most readily detached from the wood, on account of the ascent and descent of the sap. The outer portion or epidermis should always be discarded. Leaves. Gather when fully developed and before they begin to wither and fall. Of biennials, during the second season. (Ex., Hyo- scyamus, Digitalis, etc.) After the appearance of the flowers, the leaves begin to lose their activity, the juices going to develop the fruit. The slowly devel- oped leaves of a dry season are considered to be most active. Herb or.Flowering Tops. By this term we refer to the whole plant (though often the root is rejected), which should be collected while the plant is in flower. Flowers. May be gathered just before they are perfectly de- veloped; the scent is less lively, and the color paler in fully ex- panded flowers in consequence of the ovary growing at the expense of the accessory organs. The French or red rose is always gathered in bud, the astringent principle and red color being then most de- veloped. Flowers should be collected at about midday, or as soon as the sun has dried oif the dew. Fruit. Berries. Collect when perfectly ripe, but not dead ripe; the vegetable acids have not then been so completely converted into sugar, and the aroma is fresher and stronger. Seeds. When perfectly ripe. BOTANICAL. DRUGS. 35 The process of removing water from a solid substance at a low temperature. Botanical drugs are generally bulky, and are liable to become mouldy, hence desiccation is resorted to with a view to reducing their bulk, aiding their preservation, and.facilitating subdivision. In order to facilitate dessication by the exposure of a large sur- face to the air, substances of vegetable origin (with a few exceptions, the roots of burdock, belladonna, etc.) should be cut in thin slices transversely to the direction of the vascular and fibrous tissue, thereby opening the cells and ducts of the part used. The knife used should be sharp, to prevent tearing of the cellular structure and loss of juice. (Ex., fleshy or succulent roots, etc.—squill bulb, jalap tuber, colchicum corm, columbo root, etc.). Seeds require very little drying, if any. Flowers are dessicated in the shade without artificial heat to avoid the loss of essential oils. Hoots, herbs, barks, and leaves that contain no volatile principles may be dessicated at a temperature not exceeding 150° F.; it is well to employ this temperature in order to destroy the eggs deposited by insects. Worm-eaten jalap (if the resin is sought) is most profitable, as the parasite eats only the starchy matter. The natural moisture in botanical drugs varies from 30-80$ of their weight. (Elecampane root, 88$; Stramonium leaves, 90$.) Garbling. This process, to which the drug should be subjected after desiccation, consists in the separation of impurities and adul- terations, as well as decayed or deteriorated portions. Gums, gum-resins, and resins often contain pieces of bark, stone, gravel, etc., which should be removed. Tests. The tests for botanical drugs, except those containing important alkaloids (for which there are prescribed methods of assay), are few; the most readily applied being taste, odor, fracture, color of powder, medicinal activity, and a microscopical examination. Preservation. Botanical drugs, whether in powder form or not, are best preserved from deterioration by keeping in a dry place en- closed in vessels which will admit air but exclude light. Unless they contain volatile oils, they will keep well in paper boxes. A vial of ether or chloroform placed in the container, prevents the destruc- tion of the drug by insects. Odorous and inodorous drugs should always be kept separated. Desiccation. 36 MANUAL OF PHARMACY. Mechanical, Subdivision of Drugs. Comminution. The process of reducing a vegetable substance to finer particles. Drugs must be subdivided before use in the various manipulations of pharmacy, for the purpose of increasing their surface, thereby allowing a freer action of solvents, and facili- tating the extraction of tty? medicinal principles. The various forms of subdivision are obtained by—slicing {Ex., squills), chopping, cutting {Ex., columbo), crushing, filing, rasping {Ex., guaiac), sawing {Ex., rhubarb, camphor), bruising, grinding, grating {Ex., nutmeg), sifting, levigating {Ex.,prepared chalk), elutri- ating {Ex., purif. sulphide antimony), triturating, granulating {Ex., acacia), subliming {Ex., sulphur, camphor), and precipitating {Ex., calcium phosphate). Processes usually conducted by the use of the mortar: Contusion or Bruising, and Trituration. For contusion or bruising, the mortar should be made of metal (iron or brass), deep, and with flaring edges; the pestle should be heavy, and the con- vexity of its base should coincide with the concave surface of the mortar; the motion is a succession of blows. The process is hastened by working small portions of drug at a time, and sifting frequently. For trituration, shallow mortars of Wedgewood ware or porcelain, without flaring edges, are best adapted. The motion is a circular one, with downward pressure. Grinding, or Pulverization. Usually accomplished on a large scale by means of drug mills of various construction, and sieves; or on a smaller scale by the use of mortar and sieve. Sifting. The process of separating the coarser from the finer particles of pulverized substances; and is generally performed by pressing them through the meshes of fine wire, horsehair, or muslin sieves. Fineness of Powders.—Graded by terms expressing the number of meshes to the linear inch of the sieve, through which the powder will pass. Not more than a small portion should be able to pass through a sieve having ten meshes more to the linear inch. Gradation of Powder. Coarse, or No. 20 20 mesh sieve. Moderately coarse, “ 40 40 “ “ fine, “ 50 50 “ Fine, “ 60 60 “ Very fine, “ 80 or more 80 “ ‘‘ or more. DETERMINATION OF HEAT. 37 Dusted Powders. Powders carried to a certain height by draughts of air caused by the revolution of mill-stones, and de- posited on shelves within the inclosure. Granular Powder. A powder obtained in the form of small granules made uniform by rejecting that which passes through a No. 30 mesh, and that which fails to pass through a No. 20 mesh. Levigation. The process of reducing to tine particles by rub- bing with a small quantity of water. {Ex., powd. salep, nux vomica, ignatia). Performed on a slab with a muller, or in a mortar with a pestle. Elutriation. The process of removing the coarser from the finer, or heavier from lighter particles by mixing them with water, so that the finer, light, powdery portion may be poured off after the coarser particles have subsided. {Ex., prepared chalk.) Heat or temperature is measured by the thermometer, which in- dicates the degree of heat, but not the amount. Sensible Heat is that which can be shown by the thermometer. Latent Heat. The heat that a body gives out or takes up, in passing from one state to another, not shown by the thermometer. The latent heat of water is 142.56° F.; that is, ice at 32° F., in changing to water at 32° F., absorbs 142.56° of heat. Illustration. Take 1 lb. water at 174.56° F. and mix with it 1 lb. water at 32°. When the temperature has become uniform, we have 2 lbs. water at 103.28° F., the mean proportional between the two temperatures. Again, take 1 lb. water at 174.56° F., and mix with 1 lb. chopped ice at 32° F.; on taking the temperature of the mix- ture, when the ice has become entirely converted into the liquid state, we have 2 lbs. water at 32° F., while 142.56° of temperature have been lost or absorbed by the ice. Determination and Application of Heat. The Thermometer. An instrument consisting of a glass tube of small bore termi- nating in a bulb, and containing mercury or alcohol, which, by its expansion or contraction, according to the temperature to which it is exposed, indicates the degree of heat by the position of the top of the liquid column on a graduated scale. Method of Construction. A glass tube with bore of uniform diameter, and a bulb blown at one end, is heated over a lamp, causing the air in it to expand, forming a partial vacfuum. The heated tube is inverted, and the open end plunged into a vessel of mercury. 38 MANUAL OF PHARMACY. On cooling, the air in the tube contracts, thereby drawing the mercury into the bulb. The latter is then heated till the mercury overflows at the top, when the tube is quickly sealed by a blowpipe. Method of Graduating. The fixed points are the boiling and freezing points of water; these are determined by placing the instru- ment into melting ice for a time, and the point to which the mercury rises, represents the freezing-point; on immersing it in steam from boiling water for a time, the height of the mercurial column is noted, which represents the boiling-point. Scales in Use. Fahrenheit, Centigrade or Celsius, and Reamur. F. C. R. Boiling Point.. 212° 100° 80° Freezing Point. 32 0 0 Comparison. The intervening spaces are equally subdivided (making 180 degrees on F. scale, 100 in C., and 80 in R.) as well as the extension above the boiling-point and below the freezing-point. Water is not adapted for use in the thermometer, on account of the fact that it does not expand and contract regularly; it becomes a solid at 32° F. (0° C.) and a gas at 212° F. (100° C.). At 89.2° F. (4° C.) it is at its greatest density, and expands by either an increasing or diminishing temperature from that point. Alcohol is often used in thermometers to indicate low tempera- tures because of its low freezing-point (its boiling-point is 170° F., (76.6° C.), but on account of its lightness and great expansive power, a long column of the liquid must be employed, making an unwieldy instrument. Mercury is best adapted for use in thermometers. On account of its weight, only a short column is required; it does not adhere to the sides of the tube; has a low freezing-point, — 40° F. (— 40° C.) and high boiling point 662° F. (350° C.); expands and contracts regularly. Relation of Fahrenheit and Centigrade Seales. 180° F. = 100° C.; 9° F. =5° C.; or, 1° F. = |° C. and vice versa 1° C. = f ° F. Conversion from One System to the Other. 1. Above 32° Fahrenheit to Centigrade.—Rule. Subtract 32°; x 5, and -4- 9 = C°. APPLICATION OP HEAT. 39 2. Between 0° and 32° F. to C.—Rule. 32° — F.°; X 5 -5- 9 = C.°. 3. Below 0° F. to C.—Rule. Minus F.° -{- 32; x5t9 = C.°. Centigrade Degrees to Fahrenheit. 4. Above 0° C. to F.—Rule. C.° X 9 -s- 5; add 32° = F.°. 5. Between 0° and —17.7° C. to F.—Rule. C° X 9 -5- 5 = x; 32° — x = F.°. 6. Below —17.7°.—Rule. Minus C° X 9 -f- 5 - 32° = F.°. In each of the above instances the calculations with 32° are nec- essary in order to learn the number of degrees the given temperature represents, above or below the freezing-point. General Rules. The two following rules will answer for all cases, providing the algebraic signs are properly observed: To reduce F.° to C.°.—Rule. Add — 32° x5-i-9 = C.°. To reduce C.° to F.°.—Rule. Multiply by 9 -s- 5, add -f- 32° = F.°- Example. Reduce 10° C. to F. Ans. 50° F. Reduce 65.5° C. to F. Ans. 150° F. 21.1° C. = 70° F.; 93.3° C. = 200° F.; - 20° C. = - 4° F. - 40° C. = - 40° F.; - 9° F. = — 22.7° C.; 20° F. = - 6.6° C.; 190° F. = 87.7° C.; 100° F. = 37.7" C.; 60° F. =15.6° C. Direct Application op Heat. Sources of Heat. The combustion of coal, illuminating gases, alcohol, kerosene, charcoal, sperm oil, etc. Media of Application. Stoves, furnaces, lamps, Bunsen burners, blowpipes, etc. Apparatus for Applying a High Heat. Bunsen burner, blowpipe, crucible, sand bath, etc. Bunsen Burner. The combustion of gas in the presence of a good supply of oxygen from the air, drawn from the bottom of and through the centre of the burner. Burns with a light-blue flame. Blowpipe and its Use. A metallic or glass instrument by which a current or blast of air is forced from the mouth through a flame, for the purpose of reducing or oxidizing chemical subtances. Crucible and its Use. A cup-shaped vessel or melting-pot, so tempered and baked as to endure extreme heat without melting. Made of the following materials, viz.—platinum, plumbago, clay, Wedgewood ware, iron, silver, porcelain, etc. Processes Requiring a High Heat. Sublimation. The process by which a solid is changed into vapor, by the application of heat, and recovered in a solid form by 40 MANUAL OF PHARMACY. passing into a cooled receiver. Examples—Benzoic acid from benzoin. Corrosive sublimate. Calomel. Chloride ammonium. Sulphur. Camphor. Iodine, etc. Powder sublimates are obtained when there is a great difference in temperature between the condenser and retort, and cake sublimates when the temperature of the condenser is but little below that at which the volatile body sublimes. Ignition. A process of strongly heating either an organic or in- organic substance, with access of air, the residue left being sought. Examples. Quantitative tests for various salts, including manganese sulphate, sol. chloride iron, chloride of gold and sodium, etc. Incineration. A process similar to ignition, except that it is ap- plied to oi'ganic substances, with a view to burning up the carbona- ceous principles, converting them into C02, which usually remains in the ash, combined with an alkali present. Calcination, or Dehydration. A process of strongly heating inorganic crystalline substances, with a view to the removal of water, C02, or other volatile constituent. Examples. Dried alum, sodium pyrophosphate, magnesia, lime, etc. Fusion. A process of heating an organic or inorganic substance until it liquefies or melts. Examples. Melting of wax, spermaceti, the preparation of fused nitrate of silver, arsenic iodide, zinc chlor- ide, diluted nitrate of silver, etc. By fusion, chemicals are made to dissolve in their own water of crystallization. Torrefaction or Roasting. A process of heating organic sub- stances to change their qualities, by the modification of certain con- stituents, without altering others or charring. Examples. Torrefied rhubarb; representing a loss of the cathartic power of rhubarb without imparing its astringency. Coffee; some empyreumatic principles are generated, without the destruction of its important alkaloidal princi- ple, caffeine. Reduction. A process of reducing inorganic substances to ob- tain a lower degree of combination, or the element itself, by the aid of some reducing agent. Example. Reduced iron from the ox- ide, As. from As203. Deflagration. A process of heating one inorganic substance with another capable of yielding oxygen (permanganates, chlorates, nitrates, etc.), producing sudden combustion, without explosion. Example. Sodium arseniate. Oxidation. 1. A process of heating with access of air, inor SOLUTION. 41 ganic substances having a strong affinity for oxygen, which element they absorb from the air. 2. Also accomplished by the action of nitrates, chromates, manganates, sulphates, chlorine, etc., with the application of heat. {Ex.—1. ZnO, PbO, Asa Os, etc. 2. Phosphoric acid, valerianic acid, solutions of ferric salts, etc.) Carbonization. A process of heating organic substances with- out access of air, until the volatile products are driven off, and a charred residue remains, having a black color like charcoal. Ex- amples. Charcoal, kelp, etc. Methods for Equalizing and Controlling Heat; and the Tem peratures attainable. Water bath; below 212° F. Saline baths; saturated solutions chloride sodium, 227° F.; chlor- ide calcium, 354° F.; nitrate potassium, 240° F., etc. Steam bath ; above 212° F. Super-heated steam bath; i.e., steam under pressure. Pressure 5 lbs. = 226° F.; 10 lbs. = 240° F., etc. Oil bath ; below 500° F. Glycerin bath ; below 482° F. Paraffin bath ; below 680° F. Hot air bath; Sand-bath; and Card-teeth bath; for extreme tem- peratures. Boiling Point. The boiling point of a substance is modified by the pressure of the air, or the vapor formed, and by the nature of the containing vessel. A liquid boils, when the tension of its vapor equals or exceeds the pressure of the superincumbent atmosphere. On the summits of some high mountains, water boils at a tempera- ture as low as 185° F. (85° C.) SOLUTION. The process of placing a substance in contact with a liquid, there- by causing it to take the fluid state and become intimately mixed with the liquid. The liquid used to produce this change is called the solvent or menstruum, and the product a solution. Simple Solution. When the dissolved body may be recovered without having undergone any chemical change, on the evaporation of the solvent, or its removal in some other way. Examples. Chlor- ine in water, carbonic-acid gas in water, glycerin in alcohol, chlor- ide of sodium in water, etc. Phenomenon exhibited during the Process. Reduction of tempera- ture ; but with dehydrated salts, increased temperature. 42 MANUAL OF PHARMACY. Chemical Solution. A solution in which the dissolved body undergoes some chemical alteration, either in composition or decom- position. Examples. Copper in sulphuric acid, zinc in hydrochloric acid, syrup iodide of iron, solution chloride of iron, etc. Phenomena accompanying Chemical Solution. Generation of heat; effervescence; light (sometimes); changes of color, odor and taste; and always a new product. Methods for Facilitating Solution. Mechanical subdivision ; heat (except with gases, and some calcium salts,—viz., tartrate and cit- rate); agitation. Saturated Solution. A solution that contains as much of the dissolved body as it can take up at the normal temperature. The degree of concentration of a saturated solution depends on the temperature of the atmosphere, and in order to establish a standard for comparison, the U. S. P. indicates the solubility of of- ficinals at 15° C. (59° F.) in water, and in alcohol—thus, potassium iodide is soluble in water 0.8 parts, in alcohol 18 parts ; potassium bromide is soluble in water 1.6, in alcohol 200 parts. A solution that is saturated with one solid may also dissolve another, and on this principle many salts are purified. Super-saturated Solution. A solution made by heating the solvent, and dissolving to saturation at the temperature employed. Usually effected at the boiling-point of the solvent. The U. S. P. states the solubility of chemicals in boiling water, and in boiling alcohol—thus, quinine is soluble in boiling water 700 parts, boiling alcohol 2 parts; silver nitrate in boiling water 0.1, in boiling alcohol 5 parts. By a reduction of the temperature of an over-saturated solution, the excess of dissolved body is thrown out of solution, in the form of crystalline or amorphous masses; consequently a means of purification. Circulatory Displacement. The process of effecting the solu- tion of a solid, by placing it on a perforated diaphragm (or in a bag) that is immersed just below the surface of the liquid. That portion of the liquid having the greatest solvent power is always in contact with the solid, thereby keeping up a continual circulation in the fluid ; hence the term circulatory displacement. Solvents. The simple solvents used in pharmacy are as follows, arranged in order of importance; Water, Alcohol, Ether, Glycerin, SOLUTION. 43 Benzine, Chloroform, Carbon Bisulphide, and Oils. Acids, Amylic Alcohol, Wine, and Vinegar are less frequently employed. Principles dissolved by: Water. Gums, albumen, sugars, pectin, etc. Alcohol. Volatile oils, resins, alkaloids, etc. Ether. Fats, oils, resins, oleo-resins, alkaloids, etc. Glycerin. General solvent and preservative agent. Chloroform. Oils, resins, alkaloids, gutta-percha, etc. Benzine. Oils, resins, alkaloids, etc. Oils. Solvents for both fixed and volatile oils, resins, coloring matter, etc. Complex Solution. The liquid obtained by treating bodies (such as barks, roots, herbs, etc.) composed of both soluble and in- soluble principles, with a solvent suited to the principle desired, leaving behind the insoluble portions. Apparatus employed for making Complex Solutions. Mortar and pestle, percolators, infusion and decoction mugs, macerating jars, still and condenser. Processes for effecting Complex Solution. Maceration, Digestion, Infusion, Decoction, Dialysis, Distillation, and Percolation. Dialysis. The separation of crystalloids from colloids, by diffusing through a septum or diaphragm. Crystalloids. Substances capable of assuming a crystalline form. (Examples, salt, sugar, chemical salts, etc.) Colloids. Amorphous bodies; usually forming gelatinous masses with water, as glue, gelatin, starch, gums, dextrin, etc. The Septum or Diaphragm may be most advantageously made of parchment paper, which is now used to replace bladder, parch- ment, skins, etc. Construction of Dialyser. A short cylinder of glass (having one aperture covered with a septum), into which the substances are placed in liquid form. This vessel is floated in distilled water and by the force of osmosis, the crystalloids pass through the sep- tum into the water, while the colloids remain in the dialyser. There are two kinds of osmosis exhibited during the above process, viz.: Exosmosis, the passage of the denser liquid into the lighter , and Endosmosis, the passage from the lighter to the heavier. The application of the process of Dialysis has been resorted to, in 44 MANUAL OF PHARMACY. the preparation of Dialysed Tinctures* (which were originated, and their preparation practically demonstrated, by the author), in which the active crystalline principles have been separated from gummy, resinous, extractive, and coloring matter. Preparations made by Dialysis. Dialysed Iron; many of the costly chemical salts are purified by dialysis. Maceration. The process of treating a complex substance to the action of a fluid, at a temperature between 60°-90° F., until the soluble portion has all been dissolved. This process is very little used at present, as it leaves a finished tincture in the residue. Apparatus for Conducting Maceration. Wide-mouthed bot- tles or jars, into which the drug is placed, and the proper menstru- um poured on it; it is then set aside, and agitated occasionally, for 2-16 days, when the liquid is poured off, and the residue ex- pressed to recover the remainder of the liquid. Digestion. The process of subjecting a complex substance to the action of a fluid, above the normal temperature, yet below the boiling point of the liquid. The process of treating a coarsely comminuted complex sub- stance to the action of either hot or cold water for a specified time, and straining. The solution obtained is called an Infusion. Two officinal infusions are made by percolation, the remainder by the general process as above. Strength. An ordinary infusion, the strength of which is not directed by the physician nor specified by the U. S. P., should rep- resent 10# of the drug. Infusion. The process of treating a coarsely comminuted complex sub- stance with water, and boiling for a greater or less period of time, finally cooling and straining. Strength; when not designated by the physician nor directed by the U. S. P., should be 10$. Decoction. * See thesis by the author, on Dialysed Tinctures, N. Y. College of Phar- macy, 1881; New Remedies, May, 1881, p. 132; Pharmaceutical Journal and Transactions, III. Series, No. 570. Proceedings, A. P. A., 1881, p. 101. PERCOLATION. 45 PERCOLATION. Percolation {per, colo, to strain, or trickle through), also known as Displacement. A process, whereby a solution of vegetable principles is obtained, by passing a liquid solvent through a pow- dered drug. Apparatus. The apparatus used to hold the powder is a Perco- lator; it is a cylindrical or conical vessel of glass or stoneware, with a funnel-shaped termination at the smaller end, the aperture of which is fitted with a cork bearing a glass tube, provided with a closely fitting rubber tube, at least one fourth longer than the percolator itself, and ending in another glass tube, whereby the rubber tube-may be so suspended that its orifice shall be above the surface of the liquid in the percolator. Forms of Percolators. 1. Conical (funnel-shaped); 2. Cylindri- cal (length four or five times its diameter); 3. Well-tube (Dr. Squibb’s) percolator. The 1st., is used for tinctures mostly; the 2d., for fluid extracts; 3d., for general use. The Well- Tube Percolator is probably the most complete form for use with either small or large quantities of drug. A glass well- tube is placed in the centre of a slightly tapering jar or pot, and held in place by the drug packed about it. The menstruum, after percolating through the drug, accumulates in the well-tube, from which it is removed by a syphon, so arranged that the rate of re- moval may be regulated. Menstruum; the solvent employed. Percolate; the liquid passing from the percolator, containing the soluble constituents in solution. Residue or Marc; the inert, insoluble portion remaining after the completion of the process. Classes of Preparations requiring Percolation in their Process of Manufacture. Eleven, viz.: Aceta, Aquce (several by percolation through cotton, impregnated with a volatile oil), Elixi- ria, Extracta, Extracta Fluida, Infusa (two), Mellita (one), Oleo-resi- nce, Tinctures, Syrupi, and Vina Medicata. The Fluid Extracts depend entirely for their strength and re- liability on the skill with which percolation is conducted; conse- quently, the application of this process to their manufacture is selected as a means to outline the several steps of percolation. 46 MANUAL OF PHARMACY. Requisites for the Preparation of a Reliable Fluid Extract. 1. Reliable Drug. 2. Uniform Powder. 3. Proper Menstruum. 4. Uniform Moistening. 5. Uniform Packing. 6. Proper Appli- cation of Menstruum. 7. Maceration. 8. Percolating at a Proper and Uniform Rate. 9. Quantity of Percolate obtained. 1. Reliable Drugs. Obtained by careful garbling, and sub- jecting to microscopical and other examinations. 2. Uniform Powder. Obtained by the use of two sieves, one having ten meshes more to the linear inch than the size of mesh desired; reject the portion passing through the finer, and reserve all passing through the coarser. The degree of comminution de- pends upon the structure of the drug, the solubility of its active principles, and the rapidity with which it absorbs the menstruum. Drugs possessing a loose texture can be used in a coarse condition {Examples, Dandelion, Rhubarb, Sarsaparilla), while those having a tough, horny structure must be in a fine powder. {Examples, Nux Vomica, Ignatia Bean, etc.) 3. Proper Menstruum. The menstruum can be determined only by experiment. It is necessary to use such an one as is best adapted as a solvent for the active principles desired, and leaving undissolved in the residue the inert and objectionable principles; it should also be chosen with a view to the permanence of the finished fluid extract under the influence of changes in temperature, etc. If the active constituents exist in a saccharine, albuminous, or other water soluble principle, the character of the menstruum would be chiefly water, while on the other hand if an oil, resin, or certain alkaloidal principles are desired, alcohol should predominate. A drug containing one or more of each of these two classes of con- stituents would be percolated with dilate alcohol. The menstrua for officinal Fluid Extracts comprise the following solvents,—either singly or combined. Alcohol, water, boiling water, glycerin, ether, aqua ammonia, hydrochloric and acetic acids. When one or more of the solvents are to be used in combi- nation, they should invariable be mixed before applying to the drug. 4. Uniform Moistening. Most vegetable drugs, in their natural condition, are in a moist state, but after desiccation and comminu- tion the cellular tissue becomes dry, hard and tough, and like a dry sponge will not readily absorb moisture, but when dampened absorption follows immediately. If the powdered drug were 47 PERCOLATION. packed in its dry state, the subsequent application of the menstruum would produce a swelling of the particles to such an extent as to prevent the passage of the liquid through the drug. Previous moistening is then necessary, in order to produce a quick absorption of menstruum, and to facilitate its uniform descent through the packed drug. Method. The drug is placed in a suitable vessel, and the neces- sary quantity of menstruum poured on, and it is thoroughly stirred with a spatula, or suitable instrument (when operating with a large amount of drug, the hand is used) until it appears uniform. The moist powder is then passed through a coarser sieve, in order tc break up any lump?, that although externally moist (owing to the adhesive nature of certain drugs), may be dry internally,—as is true with licorice, cascara sagrada, buckthorn berries, etc. Quantity of Menstruum for Moistening: Dependent on the nature of the drug, and character of the menstruum. In all cases the moistened particles should cohere to form a mass when pressed in the hand, but should readily fall apart when subjected to a slight rolling pressure by the fingers and thumb. When moistened to excess, the drug invariably packs itself too hard. 5. Uniform Packing. When working with the amount of drug specified in the Pharmacopoeia, the entire quantity may be poured into the percolator at once (haying previously arranged the porous diaphragm of felt or cotton over the orifice), but a larger amount must be packed in fractions. The first portion is simply shaken down, the next subjected to a slight uniform pressure with the closed hand, and each subsequent layer packed with an increased pressure, using however, a uniform degree of pressure throughout each separate layer. Ligneous drugs should be very firmly packed, while drugs of a more loose cellular structure are subjected to a moderate pressure. Again, the alcoholic strength of the menstruum regulates the pressure to be applied. It must be correspondingly firmer, as the menstruum is stronger in alcohol. Nux vomica, aconite, ginger, orris, etc., requiring a strong alcoholic menstruum, may be packed “firmly,” while gentian, wild cherry, dandelion, rhubarb, etc., having menstrua of diluted alcohol, are packed “moderately.” Unless properly packed, the menstruum does not descend uniformly and slowly. 6. Application of the Menstruum. When well packed, a disk of paper or muslin is spread upon the surface, and held down 48 MANUAL OF PHARMACY. by a layer of pebbles or some suitable weight, to prevent the pour- ing on of the menstruum from disturbing the packing of the sur- face of the drug. The menstruum may now be added in portions, until it ceases to be absorbed, care being taken that the drug is kept continually covered with a stratum of the liquid, to prevent the formation of fissures through the mass, through which the menstruum would rapidly pass. The percolator is then covered to prevent evaporation. 7. Maceration. Since the soluble and active principles of vege- table matter are in a dry condition, and contained in cells which are more or less broken up by the process of comminution, the powder is submitted to maceration for a specified period of time, before percolation proper begins, thus securing contact with the solvent for a longer time, while the cells are completely softened and expanded, without the unnecessary use of a large quantity of menstruum. The period of maceration specified is two days, but a corre spondingly longer time is adopted when working large quantities, from 4-10 days. 8 Percolating at a Proper and Uniform Rate. Unless the quantity of material in operation is largely in excess of the Pharma- macopceial quantities, the rate of percolation should not exceed the limit of 10 to 30 drops per minute. The rate is about 60 drops per minute with large manufacturers. To begin percolation, the rub- ber tube is lowered and its glass end introduced into the neck of a bottle previously marked for the quantity of liquid required for the product. The rapidity may be increased or lessened by raising or lowering the receptacle, or in the Well-tube Percolator by raising or lower- ing the glass syphon. When the process is properly conducted, the first percolate will be nearly saturated with the soluble constituents of the drug; the successive portions having a paler color, until finally devoid of taste, color and odor, except those due to the menstruum itself. 9. (Quantity of Percolate Obtained. 100 cm3 for each 100 grams of drug by the following process: Percolate 70-90# of the required amount and reserve; continue percolation till the drug is exhausted; evaporate this second percolate to a soft extractive con- sistence, and dissolve in the reserved percolate; filter, and add through the filter sufficient menstruum to complete the required measure. 49 PERCOLATION. 1000 cm3 (15432 grs. of water) represent 1000 grams (15432 grs.) of powder; 15432 grs. water = 16128 minims. If 16128 minims (2.1 pts.) represent 15432 grs. (2.2 lbs. Av.) then one minim represents 95- 100 grains of drug. Exhaustion of the Drug. Can only be determined by a previous knowledge as to the constituents that the menstruum will extract. Usually, freedom from color, odor, and taste is the test—but there are exceptions; with some drugs the absence of color in the percolate would be the test, as is the case with red saunders, cochineal, saf- fron, etc., where the color alone is desired. The absence of a pre- cipitate, or a cloudiness when mixed with water (due to an oily or resinous body), is the test for exhaustion in some drugs, -such as guaiac, lupulin, cannabis indica, etc. The absence of bitterness in others, due to bitter alkaloids—colchicum, cinchona, opium, nux vomica, etc. The absence of astringency in drugs having tannin as their valuable principle,—as catechu, white oak bark, galls, kino, etc. Recovery of Alcohol or Ether from the Residue: By distillation and subsequent rectification, or by percolation with water, after having previously mixed with sawdust, excelsior, sand, or some other inert substance. Expression is also often employed. Theory of the Principles of Percolation and Exhaustion. Having carefully followed all the details for conducting percolation perfectly, all of the drug particles are necessarily under the same pressure of surrounding menstruum, as in maceration ; and on ac- count of the gravitation of the liquid in the mass, it passes through the porous particles rather than around them. A small proportion of the menstruum is at first gradually absorbed into each particle (by endosmosis) till filled. Other portions of the menstruum which is continually added, are deflected by the upper surface of the drug particles, and directed into a circuitous course towards the orifice of the percolator; but every particle of menstruum has had a strong tendency to pass in a straight line, from the surface of the drug to the outlet, consequently, it penetrates the porous surface of each drug particle in the direction of this straight line, to a distance controlled by its falling force, and the resistance and solubility of the surface. This force is then divided, one portion being retained by the deflected particle in its retarded course, and the remainder distributed to the interior of each drug particle. This force from without, destroys the counterbalance between co- hesion and gravitation, by giving the balance of power to gravita- 50 MANUAL OF PHARMACY. don, and a downward current is established within the drug parti- cles. This current is, by density of the moving matter, by friction, *nd by the length and area of channels, rendered indefinitely slow, and can only be hurried within the extremely limited compass in- volved in the keeping of a line of particles behind. Any further supply of menstruum is in excess, and after the surface of the drug particles are washed free from soluble matter, and are saturated with particles of menstruum in slow motion; this excess serves only to dilute the solution and wash it away as it is slowly pushed through. Thus a copious supply of menstruum would, in time, wash the drug particles free from soluble matter, and the latter would be in a very dilute solution. If, however, the soluble constituents are required in concentrated solution, the excess of menstruum which simply flows between the drug particles must be avoided. The outlet of the percolator must be closed, and only enough menstruum added to keep the upper surface constantly covered. The soluble matter will then all be in dense solution, the menstruum between the drug-particles sharing with the particles themselves, the portion of soluble matter which was on or near the surface, and if the outlet of the percolator be opened, so as to allow the liquid to flow out only at the rate of one drop each minute for example, the laws of hydrostatics require that this rate shall be supplied from every atom of the total contents of the percolator. Hence the current established in all parts of the percolator must be very slow, and by this diminished velocity, must be proportionately relieved from friction and increased in power; or in other words, the currents between, are retarded approxi- mately to the same rate as the currents tcithin the drug parti- cles, and hence, the superincumbent vertical lines of particles of liquid are not deflected from the surfaces of the drug particles, but pass through them in the straight lines required by gravi- tation, becoming more and more highly charged with the soluble matter until they escape below comparatively undiluted.* Objections to the U. S. P. Method for FI. Exts. The temperature required for evaporation of the second percolate, isnjurious to the activities of some constituents, while any volatile oils or volatile alkaloids are almost entirely lost, and often an extract is obtained that is practically insoluble in the first percolate. By * The above represents essentially the theory advanced by Dr. E. R. Squibb. 51 RE-PERCOLATION. the process of Re-percolation, or Fractional Percolation, the applica- tion of heat is avoided Re-percolation. This process consists in dividing the powdered drug into portions, and percolating each portion separately, in such a manner, that a mixture of the more concentrated p ortions of each percolation, pro- duces a liquid of fluid extract strength. Illustration. Take 44 Av. ozs. of powdered drug, and percolate to obtain 42 fl. ozs. of fluid extract. Divide the drug into three portions, the first representing 22 ozs., the second, 14 ozs., and the third, 8 ozs. Moisten the 22 ozs. with the menstruum, pack, mac- erate, and percolate till 8 fl. ozs. have passed, which reserve. Con- tinue percolation to exhaustion, and use this second percolate to moisten the second portion, which prepare for percolation as before. Reserve 14 fl. ozs. of percolate, and exhaust the drug. Use this second percolate to prepare the third portion for percolation; perco- late till 20 fl. ozs. pass—and mix with the previously reserved por- tions, making 42 fl. oz. in all. Should the percolate have a color or taste after 20 fl. ozs. have been taken from the third portion, then continue percolation to ex- haustion, reserving the percolate to be used as menstruum in sub- sequent operations. Another method (Dr. Squibb’s). Divide 82 parts of powdered drug into four portions of 8 parts each. No. 1 is moistened, packed, macerated and percolated until exhausted. Reserve the first 6 parts, and use the remainder to macerate No. 2, which percolate, and reserve 8 parts ; repeat the process with No. 3, and No. 4, reserv- ing 8 parts of percolate from each. Mix the reserved portions, thereby making 30 parts total. The weaker percolate of the fourth portion is reserved for subsequent operations, when from each 8 parts of drug, 8 parts of percolate are obtained. It has been proven, that the first 12 ozs. of percolate contains from 70-78$ of the total extract obtainable from 16 troy ozs. of drug. Preservation ot’ Fluid Extracts. The bottles containing them should be tightly corked, and not exposed to direct sunlight, or to any great or sudden changes in temperature. Thereby, loss of alco- hol by evaporation is prevented, and the deposition of sediments retarded. 52 MANUAL OP PHARMACY. Lixiviation. A process similar to percolation, by which soluble substances are separated from insoluble porous matter. Ex. The exhaustion of wood ashes with water to obtain pearlash, and nut-galls to obtain gallic acid. Expression. The forcible separation of liquids from solids, effected by various kinds of Presses, viz., hydraulic press, screw press, filter press, roller press, spiral twist press, and lever press. FILTRATION. The process of separating an undissolved substance from a liquid, by passing through the pores of a medium, the latter being imper- vious to the undissolved substance. The medium is called the Filter, the undissolved substance retained on the filter, the Precipi- tate, and the liquid obtained, the Filtrate. Filtering Media; Paper, paper pulp, asbestos (for strong acids), ground glass (for strong alkalies), sand, charcoal, precipitated calcium phosphate, etc. Paper Pulp. The best method for obtaining good paper pulp, is to beat up filter paper with liquor potassa, wash with water and dry. Rapid filtration may be effected by various means,—viz., heat, pressure, aspirators, filter pumps, etc. The support for the filter is called a funnel. Colation, or Straining. A process of filtration, the medium for separation being a cloth or porous substance, such as muslin, flannel, gauze, felt, bolting cloth, etc. The support for a strainer is called a tenaculum. CLARIFICATION. The process of separating from a liquid, undissolved matter which impairs its transparency and which cannot be removed by filtration. Methods. 1.. By the Application of Heat; thereby increasing the fluidity of the liquid, and enabling the heavy particles to either rise or fall, depending on their density. On rising to the surface they may be skimmed off. 2. By the use of Gelatin. Used when the liquid contains tannin (to which its cloudiness is due), forming with it an insoluble compound, which subsides. 53 DECANTATION. 3. By the use of Albumen. On the application of heat, the albu- men coagulates and envelopes the suspended matter which caused opacity, and carries it to the surface. The white of an egg is usually sufficient to clarify one gallon of the liquid. 4. By the use of Milk. This method is adopted with liquids con- taining free acids; the latter coagulates the casein of the milk, which carries the particles producing cloudiness with it to the bottom. Used to clarify sour wines and vinegars. 5. By the use of Paper Pulp. This affords a mechanical separation, the paper acting as a filter, filling the pores of the strainer. 6. By Fermentation. Dependent on the principle that the albumen present in most vegetable juices becomes insoluble in the alcohol generated by fermentation, and deposits. Decolorization and Deodorization. Processes by which substances are deprived of color and odor. Usually accompanies the process of clarification, and is accomplished by the use of animal or vegetable charcoal. Sediment. Insoluble matter separated by gravity, from the liquid in which it has been suspended, and hence differs from a precipitate (see page 57). DECANTATION. The process of removing a liquid from another liquid or insoluble solid, by pouring it off, or by the use of a syphon, or pipette. In decanting, care must be taken not to disturb the deposit, nor to allow the liquid to run down the sides of the vessel. Avoided by greasing the lip of the vessel, and by using a glass rod as a guid- ing rod. Syphon and its Use. A bent tube having one arm shorter than the other. When once filled with water, and the short arm im- mersed below the surface of the liquid, the atmospheric pressure forces the liquid up the shorter arm, while the excess of weight of the liquid in the longer arm causes a continuous flow. The flow takes place only when the discharging orifice is lower than the surface of the liquid, and no part of the tube is higher above it than the point to which the same liquid will rise by atmos- pheric pressure, that is, thirty-three feet for water, thirty inches for mercury, etc. 54 MANUAL OF PHARMACY. VAPORIZATION. The act of vaporizing; or the process of changing a solid or liquid into the form of vapor. Evaporation. The liberation of a liquid below its boiling-point in the form of vapor, directly from the surface exposed to the air, with a view to the involatile portion. Employed in the preparation of Extraction Ergotse, Fel Bovis In- spissatum, the scale salts, the concentration of syrups, fluid ex- tracts, etc. Process conducted by the use of the various baths, etc., described on page 41. Spontaneous Evaporation. Evaporation at the normal tem- perature of the atmosphere, without the employment of artificial heat. Evaporation in Yacuo. Evaporation conducted in a closed vessel, having appliances attached for removing the atmospheric pressure. The liquid boils at a low temperature, evaporation pro- ceeding actively at 120° F. In the manufacture of cane sugar, the syrup is concentrated in a vacuum pan before crystallization, in order to prevent discoloration by high temperatures. Distillation, Simple. The process of converting a liquid into vapor by the aid of heat, and passing the vapor into a cooled chamber called a Condenser, where its latent heat is abstracted, and it is deposited as a liquid called the Distillate. The involatile, or less volatile portion re- maining, is termed the Residue. This process is resorted to with a view to the volatile body, or both the volatile and involatile. U. S. P. preparations employing distillation: Abstracts, extracts, fluid extracts, oleo-resins, distilled water, etc. Apparatus used for conducting this process : Alembic, Retort, Still, Condenser, Receiver, Worm, etc. The Retort is a long-necked flask of glass or other material, hav- ing the neck bent to form an acute angle with the body of the flask. The tubulated and stoppered retorts are arranged with an opening at the top, that they may be readily refilled, and at the same time a continuous flow of the liquid kept up. Receiver. A flask having a heavy glass rim around the top of DISTILLATION. the neck,—the latter tapering so as to fit the exit-tube of the retort. When the receiver has an orifice at the top, it is called tubulated; if an opening at the bottom tapered and drawn out to a point, for the purpose of drawing off and measuring the distillate, it is called quilled. These have been superseded by the Liebig’s condenser. Liebig’s Condenser. A glass tube fitted by means of corks into a glass, copper or tinned iron tube ; into the lower end of this second tube a stream of cold water is passed, which on becoming heated by the condensing vapors passing through the glass tube, is discharged at the upper end. The glass tube is connected at one end Avitli the retort, at the other with the receiver. Safety Tube. A modified funnel tube, bent in the form of an S, for the purpose of regulating sudden disengagement of vapors, thereby avoiding explosions. Stills. The modified forms of the alembic and retort, now extensively used. When the neck of the still is connected with a spiral coil of pipe immersed in water to condense the vapors, this form of condenser is termed a Worm. A process by which constituents of different volatilities are sepa- rated, by collecting and removing the distillates obtained at different temperatures. Examples. Various gases, benzine, benzol, naphtha, gasoline, kerosene, etc., obtained by the fractional distillation of Petroleum. Fractional Distillation. Destructive or Dry Distillation. A process by which organic bodies are subjected to a gradually increased heat out of contact with air, whereby their original com- plex conditions are broken up into simpler forms. Example. Pro- duction of pyroligneous acid, tar, creosote, etc., from wood, or il- luminating gas, carbolic acid, ammonia, etc., from coal. The following four products are always obtained during destruct- ive distillation: From Wood. From, Coal. 1. Gas. Alkaline reaction. (Ammonia, representing animal matter.) 2. Liquid. Acid reaction. (Pyroligneous Acid.) 3. Tar. Creasote. Carbolic Acid. 4. Charcoal. Charcoal. Coke. Sublimation. See page 39. 56 MANUAL OF PHARMACY. CRYSTALLIZATION. The process which chemical substances undergo in passing from a liquid or gaseous state into a solid, to assume definite and regu- lar geometrically formed bodies. These mathematical forms are termed Crystalline, and the bodies possessing them called Crystals. Amorphous (from Greek a popcpe—without form), not suscepti- ble to crystallization ; Dimorphous, crystallizing in two forms; Poly- morphous, in several forms; Isomorphous, a term applied to substances having the same form of crystal, but having unlike properties. Methods for effecting Crystallization. 1. By deposition during the evaporation of a solution. 2. By deposition from a supersaturated solution on cooling, or partial cooling. 3. By fusion. (.Examples. Sulphur, bismuth, antimony, etc.) 4. By sub- limation. (Examples. Benzoic acid, iodine, corrosive sublimate, etc.) 5. By precipitation. {Examples. Mercuric iodide, oxalate of iron, etc.) Mother Liquor. The solution remaining after the first crop of crystals has been separated; it is a saturated solution of the salt, and may contain another salt, as well as coloring matter and other impurities, hence crystallization is a means of purification. By con- centrating the mother liquor and cooling, another crop of crystals can be obtained; this process may be repeated until the liquid is freed from crystalline matter. Water of Crystallization. The water appropriated by most sub- stances and entering into combination when passing into the crystal- line state. Under ordinary circumstances the amount of water in the same crystal is uniform. Efflorescence. The property that certain crystals possess, of part- ing with some of their water of crystallization at the ordinary tem- perature, forming a dry powder. {Ex., Carb. soda, zinc sulphate.) Deliquescence. The act of absorbing moisture from the air. Such crystals are called Hygroscopic. {Ex., Calcium and magnesium chlorides, sodium iodide, etc.) Water of crystallization in certain salts; viz , the sulphates of iron (ferrous), zinc, and magnesium have each seven molecules of water; quinine sulphate has seven; the alums have twenty-four, etc. The Size of Crystals is dependent upon the rapidity of evaporation, and the degree of concentration of the solution. Large PRECIPITATION. 57 crystals are obtained from cold saturated solutions, by slow evapora- tion ; small crystals by rapid cooling of supersaturated solutions. Crystallization is facilitated by suspending some foreign sub- stance in the solution, such as threads, wire, pieces of wood or lead, around which the crystals quickly form. (Milk sugar is crystallized on pieces of wood, rock candy on threads, etc.) The presence of a perfect crystal induces the formation of perf .ct crystals throughout the solution. Granulation. The process of obtaining broken crystals by rapidly stirring an evaporating saturated solution or a supersaturated solution while cooling. Many chemical salts are purified by this process, by avoid- ing the impurities of the water of crystallization taken up by larger crystals. (Ex., potass, chlorate, ammon. chloride, etc.) Creeping of crystals. Certain crystals possess great powers of ab- sorption, thereby carrying mother liquor through themselves, and causing new crystals to form on their upper surface. This process is repeated by the crystals until finally a coating has formed over the top and outside of the vessel. In the preparation of expensive salts and alkaloids this proves a considerable loss, and may be remedied by making a line of melted paraffin around the inner surface of the vessel. Crystallography. The science of the geometrical forms of crystals. All crystalline substances have forms belonging to one of the seven systems of crystallography, viz.:— I. Regular cubic or monometric. II. Quadratic or dimetric. III. Hexagonal or rhombohedra. IV. Rhombic or trimetric. V. Oblique prismatic or monoclinic. VI. Diclinic. VII. Doubly-oblique pris- matic or triclinic. The process of forming an insoluble substance from a solution, by the means of light, heat, or chemical action. The insoluble body formed is the Precipitate; the substance producing the precipitate is called the Precipitant; the liquid remaining above the precipi- tate is the Supernatant Liquid. Objects of Precipitation. Purification, subdivision, and the forma- tion of new compounds. PRECIPITATION. 58 MANUAL OF PHARMACY. Example. If a solution of mercuric chloride is mixed with a solution of potassium iodide, double decomposition results, forming mercuric iodide and potassium chloride, the former depositing while the latter remains in solution in the supernatant liquid. Reaction. HgCl2 -(- 2KI = Hgl2 -f- 2KC1. Washing. In order to recover the mercuric iodide free from potass, chloride, the supernatant liquid must be removed (by decan- tation or syphoning), and the precipitate well washed by introducing it upon a filter and pouring water over it, until the filtrate shows no trace of the dissolved body. When washing precipitates entirely insoluble in water, use hot water ; or cold water when slightly soluble. Character of Precipitates. Their physical characteristics are expressed by the terms: crystalline, amorphous, granular, flocculent, dense, bulky, heavy, light, curdy, gelatinous, etc. A thick, tenacious or gelatinous precipitate left on decanting the supernatant liquid is called a Magma. Heavy precipitates are produced by concentrated hot solutions (Ex., heavy carbonate of magnesia), while dilute solu- tions produce light precipitates. Precipitating Jars, are vessels of glass or stoneware, slightly tapering from the bottom upwards. Examples of U. S. P. preparations made by this process : Lead iodide, mercuric oxide, white precipitate, aluminium hydroxide, alkaloids, etc. Generation, Collection and Absorption of Gases. Various gases are frequently required in the production of cer- tain pharmaceutical preparations, and as tests. (Examples. Chlorine Water, Syr. Hydriodic Acid, Aqua Ammonia, etc.) The most important gases are C02, H2S, Cl, NHS, and HC1. Solution. Effected by conducting the gas a short distance below the surface of the liquid used as a solvent, when, as it bubbles up through the liquid, absorption takes place to a greater or less degree dependent upon whether the gas combines with the water to form a compound or not. (Ex., NH3 and HC1 form compounds with water, and are readily absorbed, but Cl, C02, and H2S not as readily.) Solubility is increased by forcing the gas into the liquid under pres- sure. Washing. They should invariably be passed through water in a wash bottle for purification, before solution. ACETA VINEGARS. Changes of Temperature. Gases are more rapidly absorbed by cold than by hot liquids, consequently, the receivers should be kept cool. By the action of sunlight, chlorine water decomposes and becomes hydrochloric acid. Having described all of the processes resorted to in producing galenical preparations, a classification of these products follows. CLASSIFICATION OF PHARMACOPOEIA PREPARATIONS. I. Liquids. Solutions of medicinal organic constituents obtained by percolat- ing the drug, using dilute acetic acid as a menstruum. The men- struum produces soluble salts with the alkaloidal principles, besides having antiseptic properties. Aceta—Vinegars (medicated). Number 4. Waters which have been impregnated with volatile substances. Made by, 1, Simple Solution, 2, by Absorption, 3, by Percolation, through cotton impregnated with the substance ; and 4, by Distilla- tion. AqiLE—Waters (medicated). Number 14. Collodia—Collodions. Number 4. Solutions of pyroxylin or gun-cotton in a mixture of stronger ether and alcohol, impregnated with a medicinal agent. Used ex- ternally, by application with a brush ; on evaporation of the solvent, a film remains, which acts as a protection or brings the medicament in direct contact with the skin. Made by, 1, Solution, and 2, Percola- tion. Decocta—Decoctions. Number 2. Solutions of the active principles of vegetable drugs obtained by boiling with water. Sweetened and aromatized alcoholic preparations or cordials, con- taining minute quantities of medicinally active ingredients in solu- tion. Elixiria—Elixirs. Number 1. Extracta Fluida—Fluid Extracts. Number 79. Permanent, concentrated solutions of the active constituents of vegetable drugs, of such a strength that 1 cm3 contains the medij- 60 MANUAL OP PHABMACY. inal principles and represents the virtues of 1 Gm. of the drug. Made by, 1, Percolation, 2, Re-percolation. Glycerita—Glycerites. Number 2. Solutions of medicinal substances in glycerin. Made by Tritura- tion, either with or without heat. Infusa—Infusions. Number 5. Aqueous solutions of the soluble principles of vegetable drugs, obtained by Maceration or Digestion in hot or cold water. Liquid or semi-liquid preparations having for a base cotton seed oil, alcohol or turpentine, intended for external use, and are applied to the skin with friction. Made by Solution, and Digestion. Liniment a—Liniments. Number 10. Liquores—Solutions. Number 26. Aqueous solutions without sugar, in which the substances acted upon are wholly soluble in water excepting solutions of volatile substances. Gutta-percha solution alone has a menstruum other than water. Made by, 1, Simple Solution, 2, Chemical Solution. Mellita—Honeys. Number 3. Mixtures of honey with certain medicinal substances. Mtstitre—Mixtures. Number 11. Aqueous liquid preparations which contain insoluble substances in suspension. Made by Trituration. Mucilagines—Mucilages. Number 5. Aqueous solutions of gums or mucilaginous principles of vegetable drugs. Made by Maceration, either with or without heat. Solutions of metallic oleates or alkaloids in oleic acid. Made by Trituration. Oleata—Oleates. Number 2. Liquid preparations consisting of an oil, either fixed or volatile, holding resin and other constituents in solution. Made by percolat- ing the drug with stronger ether till exhausted, and distilling off the ether from the percolate. Oi.eoresine—Oleoresins. Number 6. SPIRITUS SPIRITS. 61 Spiritus—Spirits. Number 22. Alcoholic solutions of volatile substances, either solid, liquid, or gaseous. Made by, 1, Simple solution, 2, Chemical solution, 3, Chemical reaction, 4, Maceration, 5, Absorption. Syrupi—Syrups. Number 34. Concentrated solutions of sugar in watery fluids, with or without medication. Made by, 1, Solution with heat, 2, Agitation without heat, 3, Digestion or Maceration, 4, Percolation, 5, Simple admixture. Tinctur®—Tinctures. Number 73. Alcoholic solutions of non-volatile, medicinal substances, prepared by Percolation, Maceration, or Solution. Solutions in aromatic spirits of ammonia and ether are included under the same name, although specially distinguished by the titles of Ammoniated and Ethereal Tinctures. Vina (Medicata)—Medicated Wines. Number 11. Solutions of medicinal substances, organic or inorganic, in stronger white wine, made by Percolation, Maceration and Simple Solution. II. Solids. Solid powdered preparations representing the soluble constituents of vegetable drugs combined with sugar of milk, so that one part represents two parts of the drug. Made by exhausting the drug by percolation with alcohol, evaporating, diluting with milk sugar to the required weight, and powdering when dry. Abstract a—Abstracts. Number 11. Cerata—Cerates. Number 8. Unctuous preparations which in consistence are midway between plasters and ointments, sufficiently soft to be spread at the ordinary temperature, and yet firm enough to adhere to the skin without melting. Cerates, as the name indicates, contain cera (wax), an ingre- dient. Oil, lard, or petrolatum is used as a basis. Made, 1, by Fu- sion,. 2, Incorporation. Preparations intended for external use, resembling plasters spread upon non-absorbent paper, the process necessarily varying with the nature of the substance. Chart.®—Papers. Number 3. 62 MANUAL OF PHARMACY. Confectiones—Confections. Number 2. Soft solids formerly known as conserves and electuaries, in which one or more medicinal substances are incorporated with a saccharine body, for the purpose of preservation and convenient administra- tion. Emplastra—Plasters. Number 17. Solid tenacious preparations, intended for external use, harder than cerates, yet pliable and adhesive at the temperature of the body, and requiring heat to spread them. They have for a basis, 1, Lead plaster, 2, Resin Plaster, 3, Gum Resins, 4, Burgundy Pitch. Extracta—Extracts. Number 32. Preparations obtained by removing the medicinal principles from crude drugs by solution, and evaporating to a solid or semi-solid consistence. Made by percolation and subsequent evaporation, with introduction of glycerin if necessary. Mass/e—Pill Masses. Number 3. Solid masses kept in bulk, to be used in making pills. Pilule—Pills. Number 15. Medicaments in the form of small globular, ovoid, or lenticular solids, intended to be swallowed without being previously masti- cated. Pill masses are composed of two parts, viz.—active ingre- dients, and excipient. The latter is the substance used to give the mass its proper consistence. Excipients to be used with soft or liquid substances, are inert powders, as licorice root, bread crupib, soap, acacia, starch, etc. With powders syrup, honey, glucose, mucilage, confections, glycerin, glycerite of starch, etc., are used. Coatings for pills. Sugar, gelatin, tolu, gold or silver foil. Compound powders. Pul verbs—Powders. Number 9. Resina—Resins. Number 4. Solid preparations consisting principally of the resinous principles of vegetable drugs insoluble in water. Made by Precipitation, Dis- tillation, or Percolation distillation and precipitation. Suppositorle—Suppositories. Solid preparations intended to be introduced into the rectum, urethra or vagina, to produce medical action, and of such a con- 63 SUPPOSITORIES—SUPPOSITORIES. sistence that they will melt at the temperature of the body. Their form is usually conical with rounded apex, made by pressure, mould- ing or rolling. Base. Cacao butter, on account of its low fusing point, and its property of becoming solid at a temperature just below that point. Method of preparation. Mix the medicinal portion (previously brought to a proper consistence, if necessary) with a small quantity of cacao butter by rubbing together, and add the mixture to the re- mainder of the cacao butter previously melted and cooled at 95° F. Then mix thoroughly and pour into suitable moulds, which are cooled by being placed on ice, or immerced in iced water. In the absence of suitable moulds, the above mixture may be cooled, di- vided into parts of definite weight and made into a conical or other form by the fingers. Unless otherwise specified, Suppositories should be made to weigh about 15 grains or 1 gram. Powders prepared by triturating a medicinal substance with a definite quantity of milk sugar. Strength—10# of the medicinal substance. Triturationes—Triturations. Number 1. Mixtures of medicinal substances with sugar or extract of lico- rice, formed by the aid of mucilage into stiff pasty masses, and divided into flat circular, oblong, rectangular, or stellate pieces usu- ally weighing about 10 or 20 grains. Prepared by incorporating the ingredients into a plastic and adhesive mass, rolling into a thin sheet, and cutting into proper shape with a lozenge cutter. Trochisci—Troches. Number 16. Unguenta.—Ointments. Number 26 Fatty preparations of such a consistence that they may be easily rubbed on the skin, and becoming gradually liquefied while in con- tact. Bases. Lard or benzoinated lard, combined in some cases with a very small quantity of wax. Made by, 1, Fusion, 2, Incorporation, and 3, Chemical Reaction. PART II. PREPARATIONS. Inorganic Pharmacy. Natural water in the purest attainable state. Description. A colorless, limpid liquid, odorless and tasteless at ordinary temperatures, and remaining odorless while being heated to boiling; neutral reaction; containing no more than 0.01# of fixed impurities. (H20—18) Aqua.—Water. (II20—18) Aqua Destillata.—Distilled Water. Prepared by distillation, refusing the first 5#, and the last 15# of the distillate. Description. A colorless, limpid liquid; odorless; tasteless; neutral reaction. Should contain no metals, sulphates, chlorides, calcium, ammonia and ammonium salts, or organic matters: and no fixed residue on evaporating one liter. ACIDS. An Acid is a compound of an electro-negative radical or a halogen with hydrogen, which hydrogen it can part with in exchange for a metal or basylous radical. Basylous Radical. A metal or unsaturated group of elements possessing electro-positive properties, and capable of displacing the replaceable hydrogen of an acid to produce a salt. In inorganic chemistry, bases or basylous radicals are generally metals, their ox- ides or hydroxides. Acidulous Radical. An element or unsaturated group of ele- ments possessing electro-negative properties, and capable of com- bining with hydrogen to form an acid, or with a basylous radical to form a salt. Salt. A body formed by the union or attraction of bases with acids, or basylous on acidulous radicals. ACIDS. 65 (H2S04—98) Acidum Sulphuricum.—Sulphuric Acid (Oil of vitriol.) Preparation. Sulphur or iron pyrites (FeSs), is burned in a fur- nace so arranged that the sulphurous acid gas is mixed with air; in the same furnace by the heat of the burning sulphur, nitric acid is generated from a mixture of nitrate of sodium and sulphuric acid, the fumes of nitric acid being carried with the mixed sulphurous oxide and air into a leaden chamber, where the current of these gases comes in contact with a jet of steam. Reaction. 3S02 + 2HN03 + 2H20 = N202 + 3H2S04. /Sulphurous\ /Nitric\ (Steam.) /Nitrogen\ /Sulphuric\ \ Oxide. / \ Acid./ * \ Dioxide./ \ Acid. ) The N202 takes up O from the air and becomes N204 (nitrogen tetroxide) which immediately decomposes into N202 and 02—the latter being utilized to oxidize more S02. This process is contin- ually repeated, the N202 acting as the O carrier to the S02. The following may serve to illustrate the entire changes that take place. S + 02 = 80,-tSO, -f H20 = H2S04 S + 02 = S02-j-rS03 + H20 = II2S04 s + o2 = so2—so3 + h2o = h2so4 HNOs HN03 H20 n2o2 N202 -f- 02 ~ n2o4 (y -— SO3 -f- H20— H2S04 u3 Dl 2U4 _ JN 2u2 0 + g0a _ S03 _J_ Ha0= H2g04 The dilute acid taken from the leaden chamber, called “ chamber acid” (50° B. sp. gr. 1.53-1.58), is evaporated in shallow leaden pans until its density is 60° B. sp. gr. 1.70-1.75 called “pan acid,” and finally concentrated by distilling in glass or platinum stills to 66° B. sp. gr. 1.840. Description. Colorless liquid, of an oily appearance, inodorous, strongly caustic taste, strong acid reaction. Sp. gr. 1.840—contains 96$ absolute sulphuric acid. Miscible in all proportions with alcohol and water, with evolution of heat. Chars organic matter. Test for Identity. White precipitate with soluble barium or lead salts, insoluble in hydrochloric acid. Impurities and tests. Lead: Acid (1) -f- ale. (4) = white ppt. Nitric Acid— With diluted acids: -|- Sulphate of iron = brown or reddish zone. Hydrochloric Acid: -f- Sol. sulphate of silver = ppt. 66 MANUAL OP PHARMACY. Iron: -f- Water ammonia (excess) = brown ppt. Copper: -f-Water ammonia = blue color. Arsenic : -(- H2S = yellow ppt. Arsenious or Sulphurous Acid: Diluted acid + test zinc; the gas evolved blackens paper wet with solution nitrate of silver. Officinal Preparations. 1. Acidum Sulphuricum Aromaticum. 2. Acid. Sulphuricum Dilutum. Acidum Sulphuricum Aromaticum.—Aromatic Sulphuric Acid. (Elixir of Vitriol). Add sulphuric acid (200) to alcohol (700) and allow to cool. Add tinct. ginger (45), oil of cinnamon (1), and alcohol to make 1000. Contains about 20# of officinal sulphuric acid, partly in the form of ethyl-sulphuric acid (C2H5HS04), Sp. gr. 0.955. Acidum Sulphuricum Dilutum.—Diluted Sulphuric Acid. Acid (1) + water (9). Pour the acid into the water under constant stirring, to avoid sudden evolution of heat. Sp. gr. 1.067—con- tains 10# of officinal sulphuric acid. (H2S03—82) Acidum Sulphurosum.—Sulphurous Acid. Made by heating sulphuric acid and charcoal together; the gas evolved is passed into ice-cold distilled water. Reaction. 4H2S04 + C4 = 2COa -f 4S02 + 4HaO. /Sulphuric \ (Charcoal.) / Carbon \ / SulphurY (Water.) \ Acid. ) VDioxide./ \ Dioxide./ Tests for Identity. 1. White precipitate with barium chloride, soluble in hydrochloric acid. 2. Add to diluted H2S04 and test zinc; H2S is evolved, which blackens paper moistened with solution of silver nitrate. 3. Decolorizes and deoxidizes an acid solution of potassium per- manganate. Description. A colorless liquid; sulphurous odor and taste; strong acid reaction. Sp. gr. 1.022-1.023, contains about 3.5# of S02, and 96.5# of water. Impurities and tests. H2S04 (limit)-, -f- HC1 BaCla = white ppt. (HC1—36.4) Acidum Hydrochloricum.—Hydrochloric Acid. (Muriatic acid.) Preparation. The action of sulphuric acid on sodium chloride; -distilled in glass or iron retorts. Reaction. 2NaCl + H2S04 = Na2S04 + 2HC1. /Sodium \ /Sulphuric \ / Sodium \ / Hydrochloric \ VChloride./ \ Acid. / VSulphate.) \ Acid. / ACIDS. 67 The gaseous HC1 is passed into distilled water, until the liquid has attained the proper degree of concentration. Description. A colorless, fuming liquid, of a pungent suffo- cating odor, and an intensely acid taste, and strong acid reaction. Completely volatilized by heat. Sp. gr. 1.160—contains 31.9$ ab- solute hydrochloric acid, and 68.1$ water. Impurities and tests. Iron: Dilute acid (1-10)-|-NH4OH, or (NH4)2S = Ppt. Copper : Dilute acid (1-10) + NH4OH = Blue color. Lead: Dilute acid + NH4HS = Black color. Chlorine: Dilute acid (1-5) -j- sol. KI = Liberation of iodine. Sulphuric Acid: Dilute acid-|-Ba (N03)2 = White ppt. Sulphurous and Arsenious Acid: Dil. acid-|-test zinc; gas evolved blackens paper wet with nitrate of silver solution. Officinal Preparations. Diluted Hydrochloric Acid. Nitro- Hydrochloric Acid. Diluted Nitro-Hydrochloric Acid. Acidum IIydrochloricum Dilutum. (Diluted Hydrochloric Acid). Acid (6) water (13)—mix. Sp. gr. 1.049—contains about 10$ absolute hydrochloric acid. Acidum Nitrohydrochloricum. (Aqua Regia. Nitro-Muriatic Acid). HN03 (4) -f- HC1 (15). Mix in large glass vessel. When effervescence ceases, pour into g. s. botts. Keep in cool place in bottles not more than half full. Reaction. HN03 + 3HC1 = Cl2 + NOC1 + 2H30. /Nitric\ /HydrochloricX (Chlorine.) / Chloro- \ (Water.) \ Acid./ \ Acid. ) \nitrous Acid./ Description. Golden-yellow, fuming liquid: very corrosive, having strong odor of chlorine. Dissolves gold, platinum, and the higher metals (hence called aqua regia), forming chlorides. Acidum Nitrohydrochloricum Dilutum (Diluted Nitro- Hydrochloric Acid): HN03 (4) -)- HC1 (15). Mix, and when effer- vescence ceases, add distilled water (76). (HN03—63). Acidum Nitricum.—Nitric Acid* (Aqua Fortis). Preparation. Made by the decomposition of NaN03 (Chili nitre), or KN03 (Calcutta nitre) by H2S04, in iron or glass retorts. Reaction. NaN03 + H2S04 = NaHS04 + HNOa / SodiurrA /Sulphuric \ / Sodium \ /Nitric \ \ Nitrate. ) \ Acid. / \ Bisulphate. / V Acid. ) or by using more nitrate, tbe following reaction: 2NaN03 + H2S04 = Na3S04 + 2HN03. 68 MANUAL OF PHARMACY. The sodium bi-sulphate does not froth so readily, and is easily removed from the retort. The gas is passed into water, until it ac- quires the proper density; concentrated by distillation from cone. H2SO4, which abstracts water. Description. A colorless, fuming, very caustic and corrosive liquid; strong acid taste and reaction; suffocating odor. Sp. gr. 1.420—contains 69.4# absolute nitric acid, and 30.6# water. Impurities and tests. Iron : -f- Aq. ammon. (excess) = brown ppt. Copper: -f- Aq. ammon. (excess) = blue color. Lead: -j- Aq. am- mon. -|-NIL,IIS = blk. ppt. H2S04: -{-Barium nitrate = white ppt. HC1: -{- Silver nitrate = white ppt. Iodine: Dil. acid (1-10) + gelatinized starch = blue color. Iodic Acid: After above test, add H2S cautiously = blue zone. Arsenic Acid: Fleitmann’s test (see Arsenic). Officinal Preparations. Diluted Nitric Acid. Nitrohydrochloric Acid. Diluted Nitrohydrochloric Acid. Acidum Nitricum Dilutum (Diluted Nitric Acid). HNOs (1) -{-water (6)—mix. Sp. gr. 1.059—contains 10# absolute HN03. Preparation. Obtained during the destructive distillation of wood, at'a temperature much less than that necessary to produce charcoal. The process is conducted in sheet - iron cylinders: the condensable vapors are condensed in tubes immersed in cold water, while the uncondensable gases are carried into the furnace to be burned as fuel. The condensed portion contains methylic alcohol, acetones, furfurol, acetic and various other acids, and empyreu- matic products, in a watery liquid; and an oily layer of tar, em- pyreumatic oils, resins, cresylic and phenylic compounds, and other hydrocarbons. The watery liquid constitutes Crude Pyroligneous Acid or Wood Vinegar, from which methylic alcohol may be ob- tained. To recover the acetic acid, the pyroligneous acid is treated with milk of lime in excess, for the purpose of forming calcium acetate, as well as to remove various tarry products as insoluble cal- cium compounds. The calcium acetate solution freed from precipi- tate is evaporated to dryness, and heated till it chars, then redis- solved in water, the solution treated with H2S04 and distilled. Owing to the difficulty in regulating the heat to prevent the decom- position of calcium acetate, the solution of this salt is usually de- composed by sodic sulphate. (HC2 H302—60) Acidum Aceticum. Acetic Acid. ACIDS. 69 Reaction. Ca (C2H302)2 -f- Na2S04 = 2NaC2H302 -f- CaS04. ( Calcic \ ( Sodic \ ( Sodic \ ( Calcic \ VAcetate./ VSulphate./ VAcetate./ VSulphate.) The calcic sulphate (gypsum) is filtered out, and the filtrate evaporated to dryness; the dry mass is heated to above 260° C (500° F.) to destroy the empyreumatic compounds, and finally puri- fied by dissolving in water, decanting from the sediment, adding sulphuric acid, separating the liquid from crystals of sodic sulphate and distilling. Reaction. NaC2H302 -f- H2S04 = NaIIS04 -)- HC2H302. Acetic acid is also made by pouring a mixture of alcohol and water upon beech shavings, the alcohol becoming oxidized by the action of the air. Description. A clear, colorless, volatile liquid of distinct vine- gar-like odor, purely acid taste and reaction. Miscible in all pro- portions with water and alcohol. Sp. gr. 1.048—contains 36# abso- lute acid, and 64# of water. Acetic Acid “ No. 8,” of commerce (so-called because it was used in the proportion of one part in eight to make diluted acetic acid or distilled vinegar) has the sp. gr. 1.040—and contains 28.8# absolute acid. The Specific Gravity of acetic acid is not a reliable criterion of its strength, since the acid of maximum strength increases in its re- lative weight on being mixed with water, until the percentage is re- duced to 79#, when the maximum density is reached. An acid of 43# has the same sp. gr. as one of 100# ; and between 72—85# the density shows very little variation. Hence, a better test than sp. gr. is its neutralizing power of volumetric sol. soda. Identification Test. Neutralize with NH4OH, add Fe2Cl6 = deep- red color, + H2S04 becomes colorless. On heating with II2S04 the characteristic odor of vinegar is given off. Impurities and tests. Lead, Copper, Tin: -f- H2S = ppt. Iron: -f- NH4OH = brown ppt. Calcium: -f- Ammon, oxalate (NH4)2C204 = white ppt. Cop- per : -j- NH4OH = blue tint. Empyreumatic substances: Supersat- urate with KOH = smoky odor or taste. Diluted acid (1-5) + test sol. potass, permanganate = colorless solution. Organic substances : II2S04 -j- boil = dark color. Nitric Acid: + FeS04 + H2S04 = red brown zone around the crystal. Sulphuric Acid: -f- BaCl2 = white 70 MANUAL OF PHABMACY. ppt. Hydrochloric Acid: + AgN03 = white ppt. Sulphurous Acid: -{- AgN03 and warming = dark color. Ofitcinal Preparations. Diluted Acetic Acid. Acidum Aceticum Dilutum (Diluted Acetic Acid). Acetic Acid (17)+ distilled water (83)—Sp. gr. 1.0083—contains 6% absolute acid. Preparation. Made by heating pure crystallized sodium acetate until the water of crystallization is expelled, and the salt is fused. The residue is powdered, mixed with cone. H2S04 and distilled. Reaction. NaC2H302 + II2S04 = NaHS04 + HC2H302. Description. At or below 15° C. (59° F.) a crystalline solid ; at higher temperatures a colorless liquid. Sp. gr. 1.056-1.058; nearly or quite absolute acid. Ten parts should dissolve one part oil of lemon. [Note. Other acids are treated of elsewhere under the important elements entering into their composition.] Acidum Aceticum Glaciale.—Glacial Acetic Acid. ALKALIES AND THEIR COMPOUNDS. Ammonium (NH4) is a compound and volatile alkali, while the others are simple and fixed. The elements of the simple alkalies are obtained, by exposing their carbonates mixed with charcoal to a high heat, when the metals vaporize and may be condensed. Potassium, Sodium, Ammonium, and Lithium. Reaction. K2C03 -|- 2C -f- Heat = K2 -f- 3CO. /Potassium \ (Carbon.) (Potassium.) / Carbon \ \Carbonate.J (Monoxide./ Preservation. On account of being readily oxidized in contact with air, these alkali metals must be kept under petroleum naphtha. POTASSIUM SALTS. Source. 1. Ashes of land plants; Plants take their inorganic constituents from the soil, and when incinerated leave them behind as ashes. The ash of most plants contains potassium, sodium, cal- cium and silica among other elements. 2. “ Snint ” (from the water used in washing sheep); 3. Argols (the deposits in wine casks); 4. Calcutta Nitre (KN03—occurring as an efflorescence on the soil); 5. The principal source at present is Kainite or Karnellite, an impure chloride obtained from the Stassfurt mines, Germany. THE POTASSIUM SALTS. 71 Properties and tests. Potassa is a very strong alkali and com- pletely neutralizes the strongest acids. The salts are colorless, un- less the acid itself has a marked color, and have a neutral reaction, except those made from the weak acids, which are alkaline. Readily soluble in water, and in cone, solutions are precipitated white by ammonium perchlorate, tartaric acid, and sodium bitar- trate ; and yellow by sodium picrate and platinic chloride. The flame when viewed through blue glass is of a purplish tinge. General impurities to be tested for : Alkaline earths (a limit): -f- Test sol. Na2C03 = cloudiness. Chloride (a limit): -f- HN03 AgN03 = white ppt. Sulphate (a limit): -f- IIN03 -f Ba(NOs)2 = white ppt. Carbonate : -}- dilute acid = effervescence. ((K2C03)2, 3H20.—330) Potassii Carbonas.—Carbonate of „ Potassium. (Salt of Tartar, so-called because formerly made from crude cream of tartar, or argols.) Made by leaching or lixiviating wood - ashes with water, and evaporating the concentrated solution to obtain a dry mass when cool; this constitutes crude potash of a brownish color, consist ing principally of carbonate with metallic and organic impuri- ties ; on calcining, a white, anhydrous salt is obtained, called pearlash. By treating the latter with cold water, decanting and fil- tering the quite clear solution and granulating, the pure carbonate is obtained. May also be obtained by heating the bicarbonate in a crucible to redness, dissolving and granulating. Reaction. 2KHC03 -f Heat = K2C03 -f- C03 + H20. /Potass.\ /Potass. \ /Carbon \ (Water.) VBicarb./ \ Carb. ) \Dioxicle.j Also the potassium salts from the Stassfurt. mines are converted into a sulphate, and then into carbonate by a process similar to that of Leblanc for soda, by heating with lime and charcoal, forming K2C03 and an insoluble oxysulphide of calcium. Description. White, crystalline or granular powder, very deli- quescent; odorless; strong alkaline taste, and reaction. Solvents. Water (1)—insol. alcohol. Impurities and tests: Silica: Add HN03—evap. solution, and treat residue with water = a residue remains. Alkaline Earths (a limit): Test sol. Na2COs MANUAL OF PHARMACY. = only a cloudiness. Chlorides (a limit): -f- HN03 -f- AgNOs = only slight turbidity. Sulphates (a limit): -f- HNOs -f- Ba(N03)2 = only slight turbidity. Officinal Preparation. Unguentum Sulphuris Alkalinum (Al- kaline Sulphur Ointment). Sulphur (20), K2C03 (10), H20 (5), Benzoinated Lard (65). (KHC03) Potassii Bicarbonas. Bicarbonate of Potassium. Made by passing carbon dioxide (generated from marble, CaC03, by aid of H2S04) into a concentrated solution of potass, carb.— evaporating and crystallizing; the unchanged carbonate remaining in the mother-liquor. Salaeratus is an impure powdered bicarbon- ate of potassium. Reaction. K2C03 -f- H20 -f- C02 = 2KHCOa. / Potassium \ (Water.) / Carbon \ ( Potassium \ \Carbonate.) \Dioxide.) V, Bicarbonate.,/ Description. Colorless, transparent crystals, permanent in dry air ; odorless ; saline and slightly alkaline taste ; feebly alkaline re- action. Sol. water (3.2), aim. insol. alcohol. At a red heat loses 31$ of its weight. Impurities and tests. General impurities and Carbonates (limit): Vol. sol. BaCl3 = ppt. or opalescence. (KN03—101) Potassii Nitras.—Nitrate of Potassium. (Nitre. Saltpetre.) Found native as an efflorescence on the soil near dwellings in India. Now obtained from the impure KC1 of the Stassfurt mines by decomposition with native nitrate of sodium (Chili saltpetre). Equivalent quantities of the two salts are boiled together with water until sodium chloride separates; then, by concentration, all of the latter salt separates, and the solution is allowed to cool, when potassium nitrate crystallizes out. Purified by recrystallization and granulation. Reaction. NaN03 + KC1 = KN03 -f NaCl. /Sodium \ /Potassium\ / Potassium\ / Sodium \ \ Nitrate.) \ Chloride. / \ Nitrate. ) 'Chloride.) In granulating, the impurities of the mother-liquor locked up in the crystals are removed. Description. Colorless, transparent crystals, or a crystalline powder, permanent in the air; odorless; cooling, saline, and pun- gent taste ; neutral reaction. Sol. water (4), aim. ins. in alcohol THE POTASSIUM SALTS. 73 Impurities and tests. General impurities, and Metals: -(- H2S, or + (NH4)2S = ppt. Officinal Preparations. 1. Argenti Nitras Dilutus (See Silver). 2. Charta Potassii Nitratis. (KHC4H4O8—188) Potassii Bitartras.—Bitartrate of Potassium. (Cream of Tartar.) The crude tartar or argots, which is deposited in wine-casks during fermentation, is composed of potassium bitartrate and calcium tar- trate, coloring and extractive matter. On boiling with water, adding clay, and subsequently filtering through animal charcoal (to remove coloring matter), and repeatedly re-crystallizing, a quite pure salt is obtained. Description. Colorless, or slightly opaque crystals, or a white, gritty powder; odorless, pleasant acidulous taste, and acid reaction. Sol. water (210)—very slowly sol. in alcohol. Impurities and tests. General impurities and Calcium Tartrate (more than 6$): Yol. sol. ammonium oxalate. Officinal Preparations. Pulvis Jalaps Compositus. (Com- pound Powder of Jalap. Cathartic Powder.) Powd. Jalap (85), Powd. Cream of Tartar (65). Hydragogue cathartic. Dose, 10-80 grs. ((K2C4H408) H20—470) Potassii Tartras.—Tartrate of Potassium. (Soluble Tartar.) Made by neutralizing potassium bitartrate with potassium bicar- bonate in the presence of water, filtering out the calcium tartrate (impurity in cream of tartar) which subsides, and crystallizing. Reaction. KHC4H406 + KHC03 = K2C4H406 + H20 + C02. /'Potasslum\ / Potassium \ /PotassiumN (Water.) ( Carbon\ \Bitartrate.) \ Bicarbonate./ \ Tartrate. ) \Dioxide.) Description. Small, transparent, or white crystals or a white deliquescent powder. Odorless; saline, slightly bitter taste; neutral reaction. Sol. water (0.7)—aim. ins. alcohol. Impurities and tests. General impurities, and Calcium : + (NH4)2C204 = white ppt. (KNaC4H406, 4H20—282) Potassii et Sodii Tartras.—Tar- trate of Potassium and Sodium. (Rochelle Salt.) Made by adding potassium bitartrate to a solution of sodium car- bonate, filtering out the precipitated calcium tartrate; evaporating and crystallizing. 74 MANUAL OF PHARMACY. 2KHC4H40„ + Na2C03 = 2KNaC4H406 4- H20 + C02. /Potassium\ / Sodium \ / Potassium and \ (Water.) / CarbonV (Bitartrate./ (Carbonate./ (Sodium Tartrate./ (Dioxide./ Description. Colorless, transparent crystals, slightly efflores- cent, or a white powder ; odorless ; cooling, saline and bitter taste ; neutral reaction. Sol. water (2.5)—aim. ins. alcohol. Impurities and tests. General impurities, and Ammonium salts ■ Heat with KOH = ammonia vapors. Officinal Preparations. Pulvis Effervescens Compositus. (Com- pound Effervescing Powder. Seidlitz Powders.) NaHC03, 40grs., and KNaC4H406 120 grs. in blue paper; H2C4H406, 85 grs. in white paper. Each to be dissolved in water separately, and the so- lutions mixed, and drank at once. Made by neutralizing acetic acid with potassium bicarbonate, evaporating, fusing and granulating. (KC2H302—98) Potassii Acetas.—Acetate of Potassium. Reaction. HC2H302 -f KHC03 = KC2H302 -f H20 -f C02. /AceticV / Potassium \ / PotassiumV (Water.) / CarbonV V Acid. / VBicarbonate./ V Acetate. ) (Dioxide./ May also be prepared by the mutual decomposition between lead acetate and potassium carbonate. Reaction. Pb(C2H302)2 + K2C03 = PbC03 + 2KC2H302. / Lead V / Potassium V f Lead V / Potassium V (Acetate./ VCarbonate./ VCarbonate./ V Acetate. / Description. White, satiny crystalline masses, or a white, gran- ular powder; very deliquescent; odorless; pungent and saline taste; neutral or faintly alkaline reaction. Sol. water (0.4), alco- hol (2.5). Impurities and tests. General impurities, and Organic Impurities: -|- H2S04 = discoloration of acid. Made by the action of slaked lime on K2C03 in solution. The solu- tion is decanted from the precipitate and evaporated, fused and cast into moulds. (KOH—56) Potassa.—Caustic Potash. (Potassium Hydrate.) Reaction. K2C03 -{- Ca(OH)2 = 2KOH -f- CaC03. / PotassiumV / Calcium V / Potassium V / Calcium \ (Carbonate./ (Hydroxide./ (Hydroxide./ (Carbonate./ Purification. By treatment with barium hydroxide, to separate sulphate as barium sulphate, and alcohol which dissolves only the caustic potassa. Description. White, hard, dry solid, generally in the form of 75 THE POTASSIUM SALTS. pencils; very deliquescent; odorless, or having a faint lye odor; acrid caustic taste, and alkaline reaction. Contains 90# absolute KOH. Sol. water (0.5), alcohol (2). Impurities and tests. General impurities, and Silica : Sol. -|- al- cohol = ppt. Organic Matter: Solution has color. Carbonate : -f- acid = effervescence. Officinal Preparations. 1. Potassa cum Calce. 2. Liq. Potass*. Potassa cum Calce. Potassa with Lime. (Vienna Caustic.) Made by rubbing together equal weights of potassa and lime, till a uniform powder is obtained. A milder caustic than potassa. Liquor Potass.® .—Solution of Potassa or Potash. Preparation. Made by double decomposition between KHCOa in solution and milk of lime, Ca(OH)2. The solution of the bicar- bonate is heated to drive off the excess of carbonic acid, while potassium carbonate remains in solution. 2KHCO3 + Ca(OH)2 = 2KOH + CaC03 + C02 + II20. /Acid Potassium\ / Calcium \ / Potassium \ / Calcium \ / Carbon \(Water.) \ Carbonate. ) '.Hydroxide.) \Hydroxide.) \Carbonate.) \Dioxide.) Extemporaneous formula. Dissolve KOH (56) in water (944). Description. A clear, colorless liquid, odorless ; very acrid and caustic taste, strong alkaline reaction ; miscible with water and al- cohol. Sp. gr. 1.036—contains 5# KOH. Impurities and tests. General impurities, and Foreign Impurities: Evap. neutralized solution to dryness ; residue -f- water = some in- soluble matter. Test to distinguish from Liq. Sod* : KOH -(- cone, sol. tartaric acid = white ppt. soluble in excess of KOH. Potassa Sulphurata.—Sulphurated Potassa. (Liver of Sulphur.) Made by melting together in a crucible, sublimed sulphur (1) and K2C03 (2), pouring on a marble slab while hot, and allowing to cool. This preparation is not a definite chemical compound. 3K2C03 + 4S2 = SK3S3 + K2S203 + 3C02. /PotassIum\ (Sulphur.) /Potass.TriA /Potass.ThioA / Carbon \ ' Carbonate.) \ Sulphide.) \ Sulphite. ) \Dloxide.) Description. Irregular pieces of a liver-brown color when fresh, but gradually turning yellow; faint, disagreeable odor; bitter, al- kaline taste and reaction. (KCIO3—122.4) Potassii Chloras.— Chlorate of Potassium. Preparation. A solution of caustic potassa is obtained by the decomposition of K2C03 with Ca(OH)2, and Cl generated from 76 MAXUAL OF PHARMACY. manganese dioxide and HC1 is passed into the mixture until ab- sorption ceases, with the following result: Reaction. 6KOH + 6C1 = 3KC1 + 3KC10 + 3H20. / Potassium \ (Chlorine.) /Potassium\ / Potassium \ (Wate .) (Hydroxide.) ( Chloride. ) (Hypochlorite.) On boiling the solution it decomposes, forming a chloride and chlorate. 3KC10 + 3KC1 + Boil = KC103 -f 5KC1. / Potassium \ /Potassium\ /Potassium-, /Potassium\ (Hypochlorite.) ( Chloride. ) ( Chlorate. ) ( Chloride. ) The solution is filtered, evaporated and crystallized ; purified by re-crystallization, most of the chloride remaining in the mother liquor. On account of the cheapness of KC1 obtained from the Stassfurt mines, the chlorate is now most advantageously made from that salt, by the aid of calcium hypochlorite; on boiling a solution of the latter salt, calcium chloride and chlorate are formed. Reaction. 3Ca(C10)2 = 2CaCl2 -f- Ca(C103)2. / Calcium \ /Calcium \ /Calcium \ (Hypochlorite./ (Chloride.) (Chlorate.) When solution of calcium chlorate is heated with potassium chlo- ride, the following mutual decomposition results: Reaction. Ca(C103)2 + 2KC1 = 2KC103 + CaCl2. /Caloium \ /PotassiumN /PotassiumX /Calcium \ (Chlorate./ ( Chloride. ) V Chlorate. ) (Chloride./ Description. Colorless crystals or plates ; pearly lustre; perma- nent in air ; odorless ; cooling saline taste ; neutral reaction. When strongly heated it gives oil all of its oxygen, while potas- sium chloride remains. Sol. water (16.5)—slowly sol. in ale. General Impurities: A trace of chloride is allowed. Potassium chlorate should never be triturated with tannin, sul- phur, sugar, or any oxidizable or combustible substance, except in the presence of water; or, if used in dry mixtures, the ingredients should be powdered separately, and mixed by means of a sieve and without friction, in order to avoid violent explosions. Officinal Preparation. Trochisci Potassii Chloratis—5 grs. in each. (KsC6H507,H20—324) Potassii Citras.—Citrate of Potassium. Made by saturating citric acid with potassium bicarbonate, filtering, evaporating and crystallizing. Reaction. H3C6HsC)7 -f- 3KHC03 = KsCeEUCb + 3C02 + 3H20. /Citric\ /Potass. Bi-\ /Potassium \ / Carbon \ (.Water.) V Acid./ (carbonate.) ( Citrate. ) 'Dioxide./ 77 THE SODIUM SALTS. Description. White, granular deliquescent powder ; odorless ; cooling, faintly alkaline taste; neutral or alkaline reaction. Sol- uble in water (0.6)—very slowly soluble in alcohol. Impurities and tests. General impurities, and tartrate: Cone. sol. -j- HC2H302 = white crystalline ppt. (K2S04—174) Potassii Sulphas.—Sulphate of Potassium. Obtained as a by-product in the manufacture of iodine, nitric and hydrochloric acids, etc. Also made from Kainite, a mixture of sul- phates and chlorides of potassium and magnesium. Description. Colorless crystals ; odorless ; sharp, saline, bitter taste ; “neutral reaction. Sol. in water (9), insol. ale. Impurities and tests. General impurities, and metals: -(- (NH4)2S or H2S = ppt. (K2S03—194) Potassii Sulphis.—Sulphite of Potassium. Prepared by passing S02 into a solution of K2C03 until the C02 has been expelled, and then adding more carbonate to form a neutral salt. Reaction. K2C03 -f- S02 = K2S03 -j- C02. (PotassiumX /Sulphur \ /Potassiurm / Carbon \ (Carbonate.) ' Dioxide./ ( Sulphite. ) (Dioxide.) Description. White, opaque crystals, somewhat deliquescent. Sol. water. Impurities and tests: Sulphate: -(- IICl -)- BaCl2 = white ppt. Note.—The following salts of potassium are treated of elsewhere: Potassium bichromate (under Chromium)-, bromide (under Bromine); cyanide, and ferro- cyanide (under Cyanogen); hypophosphite {under Phosphorus)-, iodide (under Iodine); permanganate (under Manganese). SODIUM SALTS. Sources. 1. Sea water (NaCI); 2. Mineral and brine spring's; 3. “ Barilla ” or “ Salicor ” (ash of plants growing near the sea); 4 Chili Nitre (NaN03); 5. Borax springs and lakes ; 6. Cryolite (6NaF.+A12F6). Properties and Tests. The Salts of Sodium are more frequently used than those of Potassium, on account of their comparative cheap- ness, and greater solubility; they are colorless, unless the acid has a distinctive color, and have a neutral reaction, except those with weak acids. The flame has an intense yellow color, not visible through blue glass. Readily soluble in water, and yield a white crystalline MANUAL OF PHARMACY. ppt. when neutral or alkaline, with metantimoniate of potassium,— but as other metallic salts have a similar reaction, it is not a reliable and practical test. - General Impurities. Sulphate (limit): -(- HC1 -f- BaCl2 = white ppt. Chloride (limit): -f- HN03 -j- AgN03 = white ppt. Carbonate : -f-Acid = effervescence. Metals:H2S, or (NH4)2S = ppt. Alka- line earths: + Na2C03 = cloudiness. (NaCl—58.4) Sodii Ciilokidum.—Chloride of Sodium. (Common Salt.) Found native in salt mines as impure rock salt, which may be purified by solution and re-crystallization. Also obtained from the brine of salt springs, which is evaporated by solar heat and allowed to crystallize, producing rock salt, or when evaporated at a boiling temperature, producing a finer grade, or table salt. Extracted from seawater by evaporation or freezing. When frozen, sea-water yields pure ice and a concentrated saline solution. Description. White, shining, hard, cubical crystals, or a crystal- line powder, permanent in air (the deliquescence often observed being due to the presence of magnesium or calcium chloride as impuri- ties); odorless; purely saline taste; neutral reaction: sol. water (2.8) —aim. insol. in alcohol. Impurities and tests. General impurities and Iodide or Bromide : Evap. ale. sol. to dryness; dissolve residue in water, add gelatinized starch and chlorine water = colored tint. (Na2CO3.10H2O—286) Sodii Carbonas.—Carbonate of Sodium. (Purified Sal Soda.) Made extensively from sodium chloride and from cryolite, in- volving three important processes: 1. Leblanc’s Process. Common salt is first converted into so- dium sulphate by heating with H2S04—the resulting product being called the salt-cake. Reaction. 2NaCl + H2S04 = Na2S04 -f 2HC1. ( Sodium \ /Sulphuric. ( Sodium \ /HydrochloricX (Chloride.) ( Acid. ) (Sulphate./ V Acid. ) The dried sulphate is powdered and mixed with chalk and coal, and heated to fusion, with the following reaction : Na2S04 + 4C + 2CaC03 = Na2C03 + CaS.Ca0 + 4C0 -f C02. ( Sodium \(Coal.) / Calcium V Sodium \( Calcium \/ Carbon \f Carbon \ } VCarbonate. ACarbonate. AOxysulphide./ VMonoxide.) (Dioxide./ THE SODIUM SALTS. The resultant black product (termed black ash or ball soda), is lixiviated with cold water, which dissolves out the sodium carbon- ate (and some hydroxide which is also formed) from the insoluble impurities. The solution is evaporated to dryness, and the residue calcined with charcoal, converting it fully to a carbonate. Solution and evaporation yield soda-ash, containing about 50# of sodium car- bonate. Repeated re-crystallization produces the pure salt. 2. Cryolite Process. Cryolite (6NaF,Al2Fe) a mineral found in Greenland, consists of fluoride of sodium and aluminium, and rep- resents the chief source of the sodium salts in the United States. When a mixture of cryolite and chalk is heated to redness, the fol- lowing reaction results: (6NaF + A12F6) + 6CaC03 = 3Na20,Al20s + 6CaF2 + 6C02. (Cryolite.) ( Calcium \ / Sodium \ ! Calcium \ (Carbon \ (Carbonate.) (Aluminate.) 'Fluoride.) (Dioxide.) The sodium salt, which is soluble, is extracted by lixiviation, and decomposed by passing C02 under pressure through the solution, aluminium hydroxide precipitating, with sodium carbonate in solu- tion. (3Na20 + A1203) + 3COa -f 3H20 = 3Na2C03 + Al2(OH)6. (Sodium Aluminate.) . / Carbon \ (Water.) / Sodium \ /Aluminlum\ (Dioxide.) (Carbonate.) (Hydroxide.) 3. Solvay’s Process. Also known as the ammonia-soda process. Consists in conducting under pressure, into a cold solution of com- mon salt, first ammonia gas, and afterwards C02, with the follow- ing result: NaCl + NH3 + C02 + II20 = NaHC03 + NH«C1. / Sodium \ (Ammonia.) (Carbon \ (Water.) / Sodium \ (AmmotilurrA Vchlorlde.) (Dioxide.) (Bicarbonate.) V Chloride, ) The sodium salt is deposited, while the ammonium chloride re- mains in solution. By heating the bicarbonate to redness, dissolv- ing and crystallizing, the carbonate is obtained. Reaction. 2NaHC03 -f- Heat — Na2C03 -f- HaO C02. ( Sodium \ / Sodium \ (Water.) (Carbon \ (Bicarbonate.) VCarbonate.) VDioxide.) Description. Large, colorless crystals, very efflorescent; odor- less; sharp alkaline taste and reaction. Sol. water (1.6), insol. ale. Should contain at least 98# of pure, crystallized Na2C03. Impurities and tests. General impurities, and Alumina (if made from cryolite); -f- HC1 -}- excess NH4OH -f- boil = gelatinous ppt. (Na2C032H20—142) Sodit Carbonas Exsiccatus. Dried Carbonate of Sodium. Na2C03 (200) is exposed to warm air till 80 MANUAL OF PHARMACY. effloresced, then heated till it becomes a fine powder weighing 100 parts. Sodii Bicarbonas Venalis.—Commercial Bicarbonate of Sodium. Preparation* Sodium carbonate is placed in a chamber, so arranged that water may be drained oil; C02 is then admitted, and sodium bicarbonate is formed, while the water of crystallization is liberated and carried off to prevent its solvent action. Reaction. Na2CO3,10H2O -|- C02 = 2NaHC03-(-9H20. / Sodium \ / Carbon \ ( Sodium \ (Water.) VCarbonate./ VDioxide./ VBiearbonate./ Also prepared by Solvay’s process (see Sodium Carbonate). (NaHC03—84) Sodii Bicarbonas.—Bicarbonate of Sodium. Made by purifying the commercial bicarbonate, by placing it in a glass percolator and washing with cold water, until the washings cease to give a ppt. with magnesium sulphate, thereby removing carbonate, traces of sulphate and chloride, and ammonium salts. Description. A white, opaque, odorfess powder; cooling, mildly saline taste; alkaline reaction. Sol. water (12), ins. alcohol. Should contain at least 99% pure Nall CO 3; and the commercial, at least 95%. Impurities and tests. General impurities, and Ammonia (if made by Solvay’s process): -f- NaOH -f- heat = ammoniacal odor. Carbonate (more than 3%): -(- HgCl2 = red ppt.—only white cloud if less than 3%. Officinal Preparations. 1. Mistura Rhei et Sodae (Mixture of Rhu- barb and Soda) NaHC03 (30), FI. Ext. Rhubarb (30), Spts. Pepper- mint (30), and water ft. 100. 2. Trochisci Sodii Bicarbonatis (three grs. in each). Made by the double decomposition between sodium carbonate in solution, and milk of lime, heated to boiling. (NaOH—40) Soda.—Caustic Soda. (Sodium Hydroxide.) Reaction, Na2C03 -f- Ca(OH)2 = 2NaOH -f- CaC03. / Sodium \ / Calcium \ / Sodium \ / Calcium \ VCarbonate./ VHydroxide./ VHydroxide./ '.Carbonate./ The solution is decanted from the precipitated calcium carbonate, and evaporated to a solid mass. Description. White, hard, opaque, solid, fibrous pieces, or white cylindrical pencils; deliquescent in moist air, but efflorescent in dry air, odorless; acrid and caustic taste; alkaline reaction. THE SODIUM SALTS. 81 Sol. water (1.7)—very sol. ale. Impurities and tests. General impurities, and Organic Matter: Aqueous solution is colorless. Silica: Aq. sol. (1 in 2) -(- ale. = ppt. Officinal Preparation.—Liquor Soda: (Solution of Caustic Soda). Made by double decomposition (see Soda), or by dissolving soda (56) in water (944). Description. A clear, colorless liquid. Sp. gr. 1.059—contain ing 5# of NaOII. (NaC2H302.3H20—136) Sodii Acetas.—Acetate of Sodium. Made by saturating acetic acid with Na2C03, evaporating, and crystallizing. Reaction. Na2C03 + 2HC2H302 = 2NaC2H302 + C02 + II20. ( Sodium \ /Acetic\ / Sodium \ ( Carbon \ (Water ) VCarbonateJ \ Acid. ) VAcetate.y VDioxide./ Description. Colorless, transparent crystals ; efflorescent in dry air ; odorless; saline, bitter taste; neutral or alkaline reaction. Sol. water (3), ale. (30). Impurities and tests. General impurities, and Organic Matter: Salt -j- cone. H2S04 = color to acid. Silica: Sol. HN03 -|- evap. = residue not all soluble in water. Made by saturating benzoic acid in solution with NaHC03, evap- orating and crystallizing. (NaC7H5O2.lI.2O.) Sodii Benzoas.—Benzoate of Sodium. Reaction. HC7H502 -f- NaHC03 = N&.C7H5O2 -(- C02 -j- H30. /BenzoicN / Sodium \ / Sodium \ I Carbon \ (Water.) V Acid. ) \Bicarbonate. / \Benzoate. / \Dioxide. / Description. White amorph. powder; efflorescent; odorless, or having faint odor of benzoin; sweet astringent taste; neutral re- action. Sol. water (1.8), alcohol (45). (NaHS03—104) Sodii Bisulphis.—Bisulphite of Sodium. Made by saturating a solution of Na2C03 with sulphurous acid gas, and crystallizing. Na2C03 + 2S02 -f 2H20 = 2NaHS03 + H20 -f C02. ( Sodium \ /Sulphurous\ (Water.) / Sodium \ (Water.) / Carbon \ (Carbonate.) \ Acid Gas. ) (Bi-sulphite.) (Dioxide.) Description. Opaque crystals, or a crystalline or granular powder; faint, sulphurous odor and taste; alk. reaction. Sol. water (4), ale. (72). Impurities and tests. Sulphate: -f- HC1 -)- BaCl2 = cloudiness. 82 manual of pharmacy, Test to distinguish from hyposulphite: Aq. sol. -|- HC1 = evolution of sulphurous vapors, but no cloudiness. (Na2B4O-,.10H2O—882) Sodii Boras.—Borate of Sodium. (Borax. Biborate of Sodium.) Found native as tincal, an incrustation on the shores of certain lakes, and as a crystalline deposit at the bottom of the borax lake in California. Purification, by solution and re-crystallization, yields the olficinal salt. Description. Colorless, transparent, shining crystals; efflorescent in dry air; odorless; mild, cooling, sweetish taste; alk. reaction. Sol. water (16), insol. alcohol. General Impurities. (ir3B03—62) Acidum Boricum.—Boric Acid. (Boracic Acid.) Found native in the lagoons of the volcanic districts of Sicily and Tuscan}, and converted into borax. The boric acid is prepared foi medicinal use, by adding HC1 or H2S04 to a solution of this salt; on standing the acid crystallizes out. Na2B4O7.10H2O + 2HC1 = 2NaCl + 4H3B03 + 5H20. (Sodium Borate.) /Hydrochloric} / Sodium } , Borie\ (Water.) V Acid. ) VChlorideJ (AcidJ Description. Transparent, colorless plates; slightly unctuous to the touch; odorless; cooling, bitterish taste; feebly acid reaction in solution, and turns turmeric paper brown, which color is unaffected by HC1. Sol. water (25), alcohol (15). The alcoholic solution burns with green flame. Impurities and tests. Sulphate: -f- Bad? = white ppt. Calcium: -(-oxalate of ammonium = ppt. Chloride: -|- HN03 -f- AgNo3 = white ppt. Metals: -(-(NH4)2S = dark ppt. Sodium Salt: yellow flame. (NaClOs—106.4) Sodii Chloras.—Chlorate of Sodium. Made by the mutual decomposition between sodium bitartrate and potassium chlorate, both in solution. Reaction. NaHC4H406 + KC10S = IvHC4H406 + NaC103. ( Sodium \ /Potassium} /Potassium} / Sodium } VBitartrate./ \ Chlorate. ) \Bitartrate./ \Chlorate./ Purified by re-crystallizing from alcoholic solution. Description. Colorless, transparent, crystals; odorless; cooling, saline taste; neutral reaction. Sol. water (1.1), alcohol (40). THE SODIUM SALTS. 83 Impurities and tests. General impurities, and Potassium: -{-sol. bitartrate sodium = white cryst. ppt. Precautions. Same as those given under Potassium Chlorate. (Na2S203.5H20—248) Sodii Hyposulphis.—Hyposulphite of Sodium. (Sodium Thiosulphate.) Made by decomposing Na2C03 with calcium thiosulphate. The latter salt is obtained commercially by oxidizing the gas-lime (mostly CaS5) obtained in the purification of gas by dry lime. Reaction. CaS203 -(- Na2C03 = Na2S203 -f- CaC03. / Calcium \ / Sodium \ / Sodium \ / Calcium \ (Thiosulphate./ (Carbonate./ (Thiosulphate./ (Carbonate.) Description. Large, colorless crystals or plates; efflorescent; odorless; cooling, bitter and sulphurous taste; neutral or faintly alkaline reaction. Sol. water (1.5), insol. alcohol. Test to distinguish from bisulphite and sulphite: -j- H2S04 = odor of burning sulphur, and white ppt. of sulphur. (NaNOs—85) Sodii Nitras.—Nitrate of Sodium. (Cubic Nitre. Chili Saltpetre.) A native salt, found in Chili and Peru, forming beds of vast extent. Purified by crystallization from its aqueous solution. By the aid of mechanical methods employing steam, it may be made to contain only 0.5 % of impurities. Description. Colorless, transparent crystals; slightly deliques- cent; odorless; cooling, saline and slightly bitter taste; neutral re- action. Sol. water (1.3), scarcely sol. in alcohol. Impurities and tests. General impurities, and Potassium: -(- NatIC4H406 = white crys. ppt. Iodide: -f-H2S-j-gelat. starch-f- chlorine water = blue color. (2NaC7H503.H20—338) Sodii Salicylas,—Salicylate of Sodium. Prepared by saturating salicylic acid with sodium bicarbonate, filtering and evaporating. Reaction. NaHC03 -f- H C7H603 = NaC7H603 + H20 -f- C02, ( Sodium \ /Salicylic \ / Sodium \ (Water.) /Carbon \ ■ Bicarbonate./ ( Acid. / (Salicylate./ \Dioxide.y Description. Small, white, crystalline plates, or a crystalline powder; odorless; sweetish, saline and mildly alkaline taste ; feebly acid reaction. Sol. water (1.5)—alcohol (6). Impurities and tests. General impurities, and Organic matter: 84 MANUAL OF PHARMACY. -f II2S04 = coloration of acid. Identification test: -f- ferric salts = intense violet color. (Na2SO4.10H2O) Sodii Sulphas.—Sulphate of Sodium. Found native, and also obtained as a by-product in the manu- facture of many chemicals, including Na2C03 (Leblanc’s process), IIC1, 1IN03, C02 (from NaHC03), etc. Purified by repeated recrystallizations. Description. Large, colorless, transparent crystals ; exceeding- ly efflorescent; odorless ; cooling, saline, bitter taste ; neutral reac- tion. Sol. water (2.8)—ins. alcohol. Impurities and tests. General impurities and Ammonia: -|- HN03 soda -f- heat = alkaline vapors. (Na2S03.7H20—252) Sodii Sulphis.— Sjlpiute of Sodium. Formed bypassing S02 into a solution of Na2C03 till saturated, and bisulphite of sodium is formed; an equal weight of Na2C03 is dis- solved in the liquid, which is evaporated to crystallization. Reaction. Na2C03 -f- S02 = Na2S03 -f- C02. ( Sodium \ /"Sulphur \ /"Sodium \ (Carbon \ VCarbonate.) \Dioxide.y \Sulphite.y VDioxide / Description. Colorless, transparent crystals ; efflorescent in dry air; odorless; cooling, saline and sulphurous taste; neutral or feebly alkaline reaction. Sol. water (4)—sp. sol. alcohol. Test.—(difference from hyposulphite): Aq. sol. -f- HC1 = odor of burning sulphur, but no cloudiness of solution. (NaC6HBS04.2H20—232) Sodii Sulphocarbolas. (Sulphocarbolate (Sulphophenate) of Sodium.) On dissolving crystal carbolic acid in strong H2S04, a new acid results, sulpho-carbolic or orthophenolsulphonic acid. Reaction. C6H6OH + II2S04 = HC6H5S04 -f H20. (Phenol.) j (Water.) The mixture is digested for three days at a temperature of 60° C. (140°F.), and diluted with water. It is now saturated with barium carbonate, barium sulphate (due to free H2S04) precipitating, with barium sulphocarbolate in solution. The latter solution is used to decompose Na2S04, the solution filtered and crystallized. Ba(C6H6S04)2 + Na2S04 = 2NaC6II5S04 + BaS04 / Barium \ ( Sodium \ ( Sodium \ ( Barium \ VSulphocarbolate./ VSulphate./ \Sulphocarbolate./ (Sulphate./ THE AMMONIUM SALTS. 85 Description. Colorless, transparent crystals ; odorless, or nearly so ; cooling, saline, bitter taste ; neutral reaction. Sol. water (5), alcohol (132). Impurity.—Sulphate: -j-HCl-j-BaCL = white ppt. Liquor Sodii Silicatis. Solution op Silicate op Soda. (Liquid Glass. Soluble Glass.) Made by fusing together 1 part of fine sand or powd. flint and 2 parts dried Na2C03, dissolving the mass in boiling water, filtering and evaporating. Description. A semi-transparent, yellowish, or pale-greenish yellow, viscid liquid—Sp.gr. 1.300-1.400—odorless; sharp, saline and alkaline taste; alk. reaction. Sol. in boiling water, insol. ale. Impurity. Excess of Alkali: Caustic effect, when applied to the skin. Used for surgical dressings. [Note. The following sodium salts are treated of elsewhere: Sodium arseni- iate (under Arsenic), bromide (Bromine), hypophosphite, phosphate and pyro- phosphate (Phosphorus), iodide (Iodine), santoninate (Olucosides).] AMMONIUM SALTS. Sources: Coal-gas Liquor, and Bone Spirit. By-products from the manufacture of illuminating gas and bone-black. Ammonia (SH3) is always a product of the putrefaction or de- structive distillation of animal matter. It is a colorless gas, having a penetrating odor and an acrid, alkaline taste ; and its hydroxide, unlike potassa or soda, will not saponify the fats. Properties and tests: The salts of ammonium are all color- less, very soluble in water, and have a neutral or faintly alkaline reaction. They are volatilized at high temperatures, and when heated with the hydroxide of sodium, potassium, or calcium, evolve the odor of ammonia, which changes the color of red litmus to blue; darkens the color of sulphate of copper paper, and forms a white cloud with HC1. Platinic chloride yields a yellow precipitate in the presence of HC1, with ammonium salts. General Impurities and tests : Sulphate: -j- BaCla = white ppt. Chloride (limit): -{- HN03 -f- AgN03 = white ppt. Metals: -f- HaS or -[-(NHOaS = ppt. Derivation of Ammonium Salts. The so-called coal-gas liquor is a watery liquid condensed in the preparation and purification of coal gas, and contains principally carbonate of ammonium, besides 86 MANUAL OF PHARMACY. some cyanide, sulphide and empyreumatic products. It is saturated with H2S04, and on evaporation, brown crystals of ammonium sulphate are obtained, which are mixed with sodium chloride and sublimed from iron pots, the vapors of ammonium chloride con- densing upon the inside of leaden or iron domes. Reaction. . (NH4)2S04 -f 2NaCl = 2NH4C1 -p Na2S04. /Ammoniumx / Sodium \ /'Ammonium'v ( Sodium \ ( Sulphate. / (Chloride./ ( Chloride. / (Sulphate./ The ammonia of the gas-liquor is sometimes converted directly to the chloride, by the addition of HC1 or CaCl2, and on evapora- tion, brown crystals of NH4C1 result, which may be purified by sublimation. (NH4)2C03 + CaCl2 = 2NH4C1 + CaC03. (NH4C1—53.4) Ammonii Chloridum.—Chloride of Ammonium. (Sal Ammoniac.) Made by re-subliming the crude salt obtained from gas liquor, as above, and further purifying by granulation. Iron, a usual im- purity, is removed by the addition of water of ammonia to a solution of the salt. Reaction. Fe2 Cl, + 6 NII4OH = 6 NH4C1 -f Fe2(OH)6. ( Ferric \ /AmmonlumX /Ammonium\ ( Ferric \ (Chloride./ (.Hydroxide./ \ Chloride. / (Hydroxide./ Description. A snow-white, crystalline powder; odorless; cool- ing, saline taste, and slight acid reaction; Sol. water (3), sp. sol. ale. Impurities and tests: General impurities, and Barium: -(- dil. F2S04 = white ppt.; Iron: -(- ferrocyanide potass. = blue color. Officinal Preparation. Trochisci Ammonii Chloridi. (Troches of Ammonium Chloride.). 2 grains in each. ((NH4)2S04—132) Ammonii Sulphas.—Sulphate of Ammonium. Preparation. Ammonical gas-liquor, or fetid bone-spirit, after saturation with H2S04 is sublimed, and repeatedly submitted to solution and crystallization until pure. Also made by passing the gas-liquor through calcium sulphate. Reaction. CaS04 -f- (NH4)2C03 = CaC03 -f- (NH4)2S04. ( Calcium \ /Ammonlum\ / Calcium \ (AmmoniumN (Sulphate./ ( Carbonate. ) (Carbonate./ ( Sulphate. / CaC03 remains undissolved, while (NH4)2S04 is in solution. Description. Colorless, transparent crystals; odorless; saline taste; neutral reaction. Sol. water (1.3) si. sol. alcohol. General impurities. Used only for preparing alum, and sulphate of iron and ammonium. THE AMMONIUM SALTS. 87 (NH4HC03,NH4NH2C02—157) Ammonii Carbonas.—Carbonate of Ammonium. (Sal Volatile. Alkali Volatile.) Made by sublimation of ammonium chloride or sulphate with an excess of calcium carbonate, and purified by re-sublimation. 2(NH4)2S04 + 2CaC03 = (NH4HC03 + NH4NH2C02) + 2CaS04 / Ammonium\ / Calcium \ / Ammonium \ /AmmoniumN / Calcium \ \ Sulphate. ) (Carbonate./ (Bicarbonate./ (Carbamate./ (Sulphate./ 4- nh3 + h2o. (Ammonia.) (Water.) Description. White, translucent masses consisting of acid car- bonate, and carbamate of ammonium. On exposure becoming opaque, and finally converted into the bicarbonate (acid carbonate). Pungent ammoniacal odor, free from empyreuma; sharp, saline taste; alkaline reaction. Sol. water (4)—alcohol dissolves the car- bamate, leaving the bicarbonate. Impurities and tests. General impurities, and Empyrejimatic matter: excess of H2S04, -f H20 -f- sol. potass, permanganate =. bleaching of latter. Officinal Preparation. Aromatic Spirit of Ammonia. Liquor Ammonii Acetatis. (Solution of Acetate of Ammonium. Spirit of Mindererus.) Made by saturating dilute acetic acid with ammonium carbonate, and should be freshly made when required. Also made by preparing separate solutions of the carbonate and acetic acid in water, and mixing equal weights when wanted. (NH4HC03 + NH4NH2C02) + 3HC2H302 = 3NH4C2H302 + 2COa /Ammonium Bicarbonate and\ /Acetic/ /Ammonium\ / Carbon \ ( Carbamate. / ( Acid. / ( Acetate. / (Dioxide./ + h2o. (Water.) This solution contains about 7.6% of ammonium acetate. Officinal Preparation. Mistura Ferri et Ammonii Acetatis. (NH4N03—80) Ammonii Nitras.—Nitrate of Ammonium. Made by neutralizing ammonium carbonate with nitric acid, and crystallizing. (NH4HCO3 + NH4NH2C02) + 3HNOs=3NH4N03 + 2C02 -f II20. /Ammonium Bicarbonate and\ /Nitrlc\ /Ammonium\ / Carbon \ (Water.* V Carbamate. / V Acid./ V Nitrate. / (Dioxide./ Description. Colorless crystals, or fused masses; deliquescent; odorless; sharp bitter taste; neutral reaction. Sol. water (0.5), alcohol (20). When gradually heated, it is decomposed into nitrous oxide gas and water. 88 MANUAL OP PHARMACY. Reaction. NH4N03 -f- Heat = N20 -f- 2H20. /AmmouiunA /Nitrous Oxide, or\ (Water.) ( Nitrate. / ( Laughing Gas. / This salt absorbs ammonia gas at a low temperature, evolving it again at a moderate heat. General impurities. (NH40H + H20) Aqua Ammonia:.—Water of Ammonia. Made by distilling a mixture of NH4C1. milk of lime and water. 2NH4C1 + Ca(OH)2 = 2NH3 + CaCl2 + 2H20. /AmmouiumN / Calcium \ (Ammonia.) / Calcium \ (Water.) V Chloride. / (Hydroxide./ (Chloride./ The ammonia gas, after passing through a wash-bottle, is passed into cold distilled water. Description. Colorless, transparent liquid; pungent odor; acrid, alkaline taste; alkaline reaction. Sp. gr. .959—contains 10# by weight of ammonia. Impurities and tests. General impurities, and Carbonate: -f lime-water = cloudiness. Calcium: -f- ammon. oxalate = white ppt. Empyreumatic matter: -f- excess dilute H2S04 = characteristic odor. Officinal Preparations. Liniment, and Aromatic Spirits. Linimentijm Ammonias. (Ammonia Liniment. Volatile Liniment.) Mix aq. ammonia (80), and cotton-seed oil (70). Spiritus Ammonia; Aromaticus. (Aromatic Spirit of Ammonia.) Containing ammonium carbonate, water of ammonia, oils of laven- der fi’s, lemon and pimento, alcohol and water. Sp. gr. 0.885. Officinal Preparations. Tinctura Guaiaci Ammoniata. Tinctura Valerianae Ammoniata—each containing 20# of the drug. Aqua Ammonia; Fortior.—Stronger Water op Ammonia. An aqueous solution of ammonia (NH3), containing 28% by weight. Sp. gr. 0.900. Officinal Preparations. Spiritus Ammoniae (Spirit of Ammonia.) An alcoholic solution of ammonia (NH3) containing 10# by weight. Sp. gr. about 0.810. Made by distilling aq. ammon. fortior with alcohol, which has been kept in glass vessels. Examples. How much stronger water of ammonia must be mixed with water, to make 100 lbs. of the weaker? Ans. 35.7 lbs. Explanation. One hundred lbs. of 10# water of ammonia is equivalent to 1000 lbs. at 1%; or as many lbs. of the 28#, as 28 is con- tained times in 1000 = 35.7. 28 :100 :: 10 : x = 35.7. Having several lots of water of ammonia of 10#, 14#, 16# and 20# THE AMMONIUM SALTS. 89 strength, and wishing them mixed to make a uniform mixture of 15$, how much of each must be used? Am. 5 lbs. of 10$; 1 lb. 14$; 1 lb. 16$; 5 lbs. 20$. (See page 31, part I.) 5 —10 Proof. 5 lbs. at 10$ = 50 lbs. at 1$ 1 tie 15 1 lb. at 14$ = 14 lbs. at 1$ 1 1 lb. at 16$ = 16 lbs. at 1$ 5 —20 5 lbs. at 20$ = 100 lbs. at 1$ Total, 180 lbs. at 1$, or as many lbs. at 15$ as 15 is contained times in 180 = 12 lbs. (NH4C7II5O2—189) Ammonii Benzoas.—Benzoate op Ammonium. Made by saturating benzoic acid with water of ammonia, evap- orating and crystallizing. Reaction. NH4OH -f HC,H502 = NH4C7H502 + H20. /Ammonium/ /Benzoic/ /Ammonium/ (Water.) \ Hydroxide.) V Acid. ) \ Benzoate. ) Description. Thin, white crystals; slight odor of benzoic- acid ; saline, bitter, acrid taste; neutral reaction. Sol. water (5), alcohol (28). (NH4Br—97.8) Ammonii Bromidum.—Bromide op Ammonium. By several of the processes in use for preparing this salt, an un- stable compound is obtained, but the following gives a more stable salt: viz., subliming a mixture of KBr and (NH4)2S04. Reaction. 2KBr -f- (NH4)2S04 = K2S04 + 2NH4Br. /Potassium/ /Ammonium/ /Potassium/ /Ammonium/ \ Bromide. ) \ Sulphate. ) \ Sulphate.) \ Bromide. ) or, by the reaction between bromine and ammonia in the presence of water, concentrating the solution, and granulating or crystallizing. Reaction. 8NH4OH -f 3Bra = 6NH4Br + N2 + 8H20. /Ammonium/ (Bromine.) /Ammonium/ (Nitrogen.) (Water.) \ Hydroxide. / \ Bromide. ) Description. White granular salt, or colorless, transparent crys- tals, becoming yellow on exposure to air; pungent, saline taste; neutral reaction. Sol. water (1.5), alcohol (150). Impurities and Tests. General Impurities, and Bromate: -{- dil. H2SO4 = yellow color. Iodide: Sol. -j-gelatinized starch -f- Cl = blue zone. (NH4I—144.6) Ammonii Iodidum.—Iodide op Ammonium. Made by adding to boiling water, a mixture of potassium iodide and ammonium sulphate. Reaction. 2KI + = 2NHJ -f K2S04. /Potassium', /Ammonium/ /Ammonium/ /Potassium/ \ Iodide. ) \ Sulphate. ) \ Iodide. ) \ Sulphate.) 90 manual of pharmacy. On the addition of alcohol and the application of cold to the above mixture, potassium sulphate separates as a crystalline powder, and after filtration, the solution is evaporated to dryness. This salt should not be made by the action of iodine on water of ammonia, as nitrogen iodide (a very explosive compound) is thus generated. Reaction. NH4OH -f 61 = 3HI -f NI, 4- H20. /Ammonium) (Iodine.) /Hydriodic) /Nitrogen) (Water.) V. Hydroxide./ V Acid. ) \ Iodide. ) Description. White, granular salt, or in crystals ; very deli- quescent, and fast becoming yellow on exposure to air; odorless ; sharp, alkaline taste; neutral reaction. Sol. water (1), alcohol (9). When deeply colored, it should not be dispensed, but may be de- prived of iodine by washing with stronger ether, and rapidly drying. Impurities and tests. General impurities, and Iron: -f- Potass. Ferrocyanide = blue color. Iodine (free): -f- starch jelly = deep blue color. Bromide and Chloride: Dissolve in NH4OH; -j- AgJ^03 -J- HN03 (excess) = white ppt. ((NH4)2HP04—132) Ammonii Phosphas.—Phosphate of Am- monium. (Dianunonium Orthophosphate.) Made by saturating phosphoric acid with water of ammonia. Reaction. 2NH4OH + H3P04 = (NH4)2HP04 -j- 2H20. /Ammonium) /Phosphoric) /Ammonium \ (Water.) \ Hydroxide./ V Acid. ) \ Phosphate. / Description. Colorless, translucent crystals, losing ammonia on exposure to dry air; odorless; cooling, saline taste; neutral or faintly alkaline reaction. General impurities. Oxalate of Ammonium ((NH4)2C204) is a very poisonous salt; used in pharmacy only as a reagent for calcium salts, producing with them a white precipitate of calcium oxalate, insoluble in acetic acid, Citrate of Ammonium ((NIDsCeHsO,), and Tartrate of Am- monium ((NH4)2C4H406) are used as solvents for the iron salts, etc. The former is also a solvent for bismuth citrate, and its solution sometimes employed in the place of Liq. Ammon. Acetatis. ALKALINE EARTHS AND THEIR COM- POUNDS. Calcium, Magnesium, Barium and Strontium. Points of Distinction from the Alkalies. The carbonates of the alkalies are soluble and have an alkaline reaction, while the alkaline earth carbonates are insoluble, and have a neutral reaction. THE CALCIUM SALTS. 91 CALCIUM SALTS Sources. A very abundant natural production. Found as a carbonate in chalk, marble, calcareous spar, limestone and shells ; as a sulphate in the different kinds of gypsum ; as a phosphate in the bones of animals; and combined with silica in a great variety of minerals. Tests. Ammonium oxalate gives a white ppt, insoluble in acetic acid, but soluble in excess of HC1; the blowpipe flame is colored reddish-yellow. The alkaline carbonates, sulphuric acid, and phos- phates also produce insoluble precipitates. (CaO—56) Calx.—Lime. (Burned Lime. Quicklime. Calx usta.) Made by calcining marble or limestone with a strong heat, until all of the C02 is expelled. Reaction. CaC03 -(- Heat = CaO -j- C02 ( Calcium \ /CalciumN / Carbon \ (Carbonate./ ( Oxide. ) (DioxideJ Description. Hard, white or grayish-white masses ; attracts moisture and C02 on exposure to air, and falls to a white powder; odorless; sharp, caustic taste; alkaline reaction. SI. sol. water (750) insol. alcohol. Slaked Lime. When lime is treated with half its weight of water, it absorbs the latter, becomes heated, and gradually con- verted into a white powder. The addition of sufficient water to this powder to produce fluidity yields Milk op Lime. Impurities and tests. Carbonate (limit): + HN03 = effervescence. Alkalies, and their carbonates: + C02 to saturate = alkaline reaction. Insoluble Matter: Nitric acid solution leaves residue. Officinal Preparations. 1. Liquor Calcis; 2. Potassa cum Calce (See Potass.)-, 3. Syrupus Calcis. Liquor Calcis. (Solution of Lime. Lime Water.) An aqueous solution containing 0.15# calcium hydroxide (Ca(OH)2) — Sp. gr. 1.0015. Made by adding an excess of washed slaked lime to water. Offikinal Preparation. Linimentum Calcis, (Lime Liniment. Carron Oil.) Lime water and cotton-seed oil equal parts, mix. Syrupus Calcis. (Syrup of Lime. Saccharate of Calcium.) Lime (5) and sugar \30) are triturated and dissolved in boiling water, filtered and evaporated (to 100). (CaBr2—199.6) Calcii Bromidum.— Bromide op Calcium. Made by saturating hydrobromic acid with calcium carbonate, and evaporating to dryness. 92 MANUAL OF PHARMACY. Reaction. CaC03 -(- 2HBr = CaBr2 -f- C02 -f- H20. / Calcium \ /Hydrobromtc\ /Calcium \ /Carbon \ (Water.) \CarbonateJ \ Acid. / VBromide.y \Dioxide.) (CaC03—100) Calcii Carbonas Pra/kcipitatus. Precipitated Carbonate of Calcium. (Precipitated Chalk.) Made by the mutual decomposition between sodium carbonate and calcium chloride; washing and drying the ppt. Reaction. CaCl2 -f- Na2C03 = 2NaCl + CaC03. /Calcium \ / Sodium \ / Sodium \ / Calcium \ VChloride./ VCaibonate./ VChloride./ \ Carbonate./ Boiling solutions yield the most minute division of the particles. For ordinary use this salt is not superior to Prepared Chalk. Description. Very fine, white, impalpable powder; odorless; tasteless; insol. water, and alcohol. Impurities and tests. Magnesium: Make neutral solution in acetic acid; -f- NH4C1 -j- (NH4)2C03 -f- NH4OH (excess) -|- heat; fil- trate -|- Na2HP04 = white ppt. Aluminium, iron, or phosphate: -|- HC1 (to dissolve) -{- heat -f- NH4OH (excess) = ppt. Native friable calcium carbonate (CaC03) freed from most of its impurities by elutriation. Made on a large scale from whiting. (Calcium carbonate exists in mineral and spring waters held in solu- tion by C02, forming a bicarbonate. Waters containing CaII2(C03)2 are said to possess temporary hardness, and are rendered soft by boiling, thereby driving off the excess of C02, while CaC03 ppts. IfCaS04 is present, water possesses permanent hardness ; unaffected by boiling, but made soft by the use of a fixed alkali carbonate or hydroxide.) Preparation. Native chalk is pulverized and rubbed with water on a porphyry slab, by means of a muller of the same material. It is then agitated with water, which on standing deposits the coarser particles; on pouring off the liquid, the remainder slowly falls in an impalpable state. (This process combines elutriation and levigation.) This impalpable powder is made to fall on an absorbent surface in small portions, by means of a mechanical contrivance, and on diy- ing assumes a conical shape. Description. White, amorphous powder, or in the form of small cones; odorless, and tasteless; insoluble in water, or alcohol. Impurities and tests. Magnesium (limit): (See Carbonate.) Barium and Strontium: + Test sol. CaS04 = ppt. Iron (a limit): -f- Potass, ferrocyanide = blue color. (CaC03—100) Creta Pileparata.—Prepared Chalk. THE CALCIUM SALTS. 93 Officinal Preparations. 1. Hydrargyrum cum Creta (See Mer- cury.) 2. Pulvis Cretse Compositus. 3. Trochisci Crete. Pulvis Cretse Compositus—Compound Chalk Powder. Prepared chalk (30), powd. acacia (20), powdered sugar (50)---mix. Officinal Preparation. Mistura Cret/e. (Chalk Mixture). Compound chalk powder (20), cinnamon water (40), water (40). Should be freshly made when wanted. Trochisci Crete. (Chalk Troches.) 4 grs. in each. (CaCl2—110.8) Calcii Chloridum. (Chloride of Calcium.) Obtained as a by-product in many chemical processes; or may be made by the action of HC1 on marble or chalk, evaporating the solu- tion to dryness, and fusing the salt at a red heat. CaC03 + 2HC1 = CaCl2 + H20 + C02. / Calcium \ /Hydrochloric\ / Calcium \ (Water.) / Carbon \ (Carbonate./\ Acid. / (Chloride./ (Dioxide./ Description. Colorless, hard masses; very deliquescent, odorless; hot, sharp, saline taste; neutral or faint alkaline reaction. Soluble in water (1.5), ale. (8). Impurities and Tests. Aluminium, iron, etc: -)- NH4OH = ppt. Sulphate:-J-BaCl2 = white ppt. Magnesium (a limit): See Carbonate. (Ca3(P04)2—310) Calcii Phosphas Precipitated Phosphate of Calcium. Made by dissolving calcined bone in HC1, and treating the solu- tion with water of ammonia, producing NH4C1 in solution, while calcium phosphate precipitates. 1. Ca3(P04)2 + 4HC1 = CaH4(P04)2 + 2CaCl2. / Calcium \ /Hydrochloric\ ( Calcium \ / Calcium \ (Phosphate./ ( Acid. ) (Acid Phosphate./ ( Chloride./ 2. CaII4(P04)2 + 2CaCl2 + 4NH4OH = Ca3(P04)2 / Calcium \ (Calcium \ /Ammonium\ / Calcium \ \Acid-phosphateJ VChlorideJ V Hydroxide./ VPhosphate./ + 4NH4C1 + 4HaO. /Ammonium\ (Water.) V Chloride. ) Also made by the mutual decomposition between calcium chloride and sodium phosphate. Description. A light, white, amorphous powder; odorless, and tasteless; insol. water, or ale. Often used as a filtering media. Impurities and tests. Carbonate: + HN03, or HC1 = efferves- cence; Aluminium,: -f- KOH -(- boil = ppt. Officinal Preparation. Syrupus Calcii Lactophosphatis. (Syrup of Lactophosphate of Calcium.) A solution of re-precipi- 94 MANUAL OF PHARMACY. tated calcium phosphate in lactic acid and water, flavored with orange-flower water, and protected by sugar. A mixture (commonly misnamed Sulphide of Calcium) consisting chiefly of calcium sulphide and sulphate (CaS, and CaS04), in vary- ing proportions, but containing not less than 36# of absolute calcium sulphide. Made by heating lime and precipitated sulphur together in a crucible. Calx Sulphurata. (Sulphurated Lime.) Reaction. 4CaO -f- 2S2 = 3CaS -f- CaS04. (Lime.) (Sulphur.) (Calcium \ / Calcium \ '.Sulphide./ (Sulphate./ Description. Grayish-white, or yellowish-white powder; grad- ually changed by exposure; faint H2S odor; offensive, alkaline taste; alkaline reaction; v. si. sol. water, insol. ale. [Note.—For Calx Chlorata, see Chlorine; Calcis Hypophosphis, see Phos- phorus.] Calcium Sulphate is recognized only in the form of a Test Solution. MAGNESIUM SALTS. Sources. Found in the serpentine rocks of Pennsylvania, Ohio, and Hoboken, N. J., ns siliceous hydrate; as carbonate in Magnesite, on the •coast of Greece; as a double carbonate of magnesium and calcium in Dolomite; as impure sulphate in the Kieserite of the Stassfurt mines; also in soapstone, talc, asbestos, chrysolite, bitter spar, magnesian lime-stone, sea-water and mineral springs (chloride and sulphate), and the bittern of salt works. The magnesium minerals are mostly of a green color, and have a soft and unctuous feeling to the touch. Magnesium. The metal is produced by decomposing its chloride with potassium. They are fused together, ignited, and the KC1 washed out with water, MgCl2 -(- Ka = 2KC1 -f- Mg. It has a silvery appearance, is soft and malleable, and burns with an intense white light. Tests. With magnesium salts, solution of sodium phosphate gives a white crystalline precipitate; K*C03 or Na3C03 produce white precipitates; and caustic alkalies yield a gelatinous precipitate. General Impurities. Chloride: -|- AgNOs = white ppt. Sulphate: -|- BaCla = white ppt. (MgS04.7H20—246) Magnesii Sulphas.—Sulphate of Mag- nesium. (Epsom Salts.) Originally obtained by the evaporation of the waters of the Epsom Springs (Eng.),—also made from the Kieserite deposits of Stassfnrt. THE MAGNESIUM SALTS. 95 At present, most extensively made from the siliceous hydrate, on account of the absence of lime. The mineral is powdered, and saturated with H2S04, the mass dried and calcined at a red heat (to convert any ferrous sulphate present into red oxide), dissolved and crystallized. Purified by recrystallization. Description. Small, colorless crystals; efflorescent in dry air; odorless ; cooling, saline, hitter taste ; neutral reaction. Sol. water (8), insol. ale. Impurities and tests: General impurities, and Metals: -|- H2S, or (NH4)2S = ppt. Other alkaline earths: Sol. -J- NH4C1 -f- (NH4)2C03 -}- NH4OH = ppt. Alkali Sulphates (over Sol +NH4C1-f- (NH4)3P04 -f- NH4OH; evap. tilt, to dryness, ignite, -f- H20 -j- HC1 + ale. (or BaCl2) = ppt. Officinal Preparation. Infusum Senn/e Compositum. (Compound Infusion of Senna. Black Draught.) Contains Senna (6), manna (12), MgS04. (12), fennel (2), and water (to make 100). ((MgC03)4Mg(0H)2.5H20—484) Magnesii Carbonas.—Carbonate of Magnesium. Made from dolomite, magnesite, the bittern of salt works, etc. The purest carbonate is made by obtaining a pure sulphate of mag- nesium, decomposing with a solution of pure sodium carbonate, washing and drying the precipitate. Reaction. 5Na2C03 + 5MgS04 + H20 = 4MgC03 ( Sodium \ /Magnesium\ (Water.) /Magnesium\ (Carbonate./ V Sulphate. J \ Carbonate./ + Mg(OH)2 + 5Na2S04 + C02. /"MagneslumN / Sodium \ / Carbon \ (Hydroxide./ (Sulphate./ (Dioxide./ If the Light Carbonate of Magnesium (U. S. P.) is wanted, cold diluted solutions are used, and the mixture boiled for fifteen min- utes, then the precipitate is washed and dried. If the Heavy Car- bonate is desired, more concentrated solutions are employed, and the mixture evaporated to dryness on a sand bath; the residue is di- gested, washed and dried. Description. Light, white, friable masses, or light, white powder; odorless; tasteless; insoluble in alcohol—aim. ins. water, to which it imparts a feebly alkaline reaction. Impurities and tests. General impurities, and Aluminium, or Calcium: IIC1 + (NH4)2C03 (excess) = white ppt. Metals: acetic acid sol. -f- HC1, or (NH4)2C03 and NH4OH, or(NH4)2S = ppt. Officinal Preparation. Mistura Magnesise et Asafoetidae. (Mix- 96 MANUAL OF PHARMACY. ture of Magnesia and Asafetida. Dewees’ Carminative.) Contains MgC03, tinctures of asafetida, and opium, sugar and water. (MgO—40) Magnesia.—Light Magnesia. (Calcined Magnesia. Magnesia Usta.) Made by the calcination of light magnesium carbonate. 4MgC03 + Mg(OH)2 + 5H20 + Heat = 5MgO + 6H20 -f 4C02 /Magnesium carbonate\ (Water.) /Magnesium\ (Water.) / Carbon \ \ officinal. ) \ Oxide. J {Dioxide. J Description. Light, white, odorless powder; having an earthy, but no saline taste; faint alkaline reaction when moistened with water, aim. insol. water, insol. alcohol. Impurities and tests. General impurities, and Carbonate: -f- dil. H2S04 = effervescence. Officinal Preparations. 1. Ferri Oxidum Hydratum cum Magnesia (see Iron). 2. Pulvis Rhei Comp. 3. Trochisci Magnesiae. Pulvis Rhei Compositus. (Compound Powder of Rhubarb.} Contains powd. rhubarb (25), magnesia (65), and powd. ginger (10). Trochisci Magnesle. (Troches of Magnesia.) Each contains magnesia (3 grs.). powd. nutmeg and sugar. (MgO—40) Magnesia Ponderosa.—Heavy Magnesia. Made by calcining heavy magnesium carbonate. Description. White, dense, fine powder; in other respects re- sembling the light salt. Magnesii Citratus Granulatus. (Granulated Citrate of Magnesia.) Mg3(C6H607)2, etc. Magnesium carbonate (11), citric acid (48), sodium bicarbonate (37), powd. sugar (8), alcohol, and water ft. (100). Triturate the magnesium carbonate with part of the citric acid and distilled water q.s. to make a thick paste; dry and powder; mix with the powd. sugar, sodium bicarbonate, and the remainder of the citric acid (powdered). Dampen the mass with alcohol, and rub through a tinned iron sieve to form a coarse granular powder. Description. White, coarse, granular salt; deliquescent on ex- posure; odorless; mildly acidulous refreshing taste; acid reaction. Soluble water (2), with copious effervescence. Impurity (or adulteration) and test, lartaric acid: + solution potass, acetate -f- acetic acid = white cryst. ppt. Liquor Magnesii Citratis. (Solution of Citrate of Magnesium). Made by dissolving magnesium carbonate in citric acid and water, THE BARIUM AND STRONTIUM SALTS. 97 flavoring with syrup of citric acid, and adding potassium bicarbon- ate to generate C02. (MgS03.6H20—212) Magnesii Sulphis.—Sulphite of Magne- sium. Made by passing S02 into a mixture of magnesium carbonate in water, until all of the C02 has been expelled. Mg(OH)a -I- 4MgCOa + 5S02 = 5MgS03 + 4C02. + H20. /.uagnesium carbonateV /Sulphur \ /MattneslumV / Carbon \ (Water.) \ officinal. ) VDloxlde./ \ Sulphite. ) VDloxide./ Description. White, crystalline powder; bitter and sulphurous taste; neutral, or slightly alkaline reaction; sol. water (22), insol. ale. BARIUM AND STRONTIUM SALTS. Barium Salts. Found as Heavy Spar (BaS04), Witherite (BaCOs), Baryta (BaO). Tests. The soluble salts are tests for sulphuric acid and sul- phates, and vice versa, producing insoluble white precipitates; the color of its blowpipe flame is light green; white precipitates are produced by the soluble carbonates. There are no officinal salts of barium, but the following are often used. All are poisonous. Barium Sulphate. (Heavy Spar)—(BaS04). The mineral from which the compounds of barium are prepared. The impure sul- phate is first converted into a sulphide by igniting with charcoal. Reaction. BaS04 + C2 = BaS -(- 2C02. / Barium \ (Carbon.) / Barium \ / Carbon \ VSulphate.J '.Sulphide./ \ Dioxide./ The BaS is dissolved and treated with dil. H2S04, thus forming BaS04. Called permanent white, or hlanc fix, and used for glazing cards ; also as an adulterant of white lead. Barium Chloride (BaCl2). Made by dissolving BaCOs in HC1, or BaS in HC1. Reaction. BaS -f- 2HC1 = BaCl2 -f- H2S. /Barium /HydroehloricV / Barium \ /HydrogenV (Sulphide. \ Acid. ) (Chloride./ (Sulphide./ The Test Solution contains 10# of the salt. Barium Carbonate (BaC03). Found native as Witherite. May be made by the double decomposition between a soluble bari- um salt, and an alkaline carbonate. Barium Peroxide (Ba02). Made by passing oxygen or atmos- pheric air over the oxide or hydroxide, heated to dull redness. By treating with HC1 this salt yields peroxide of hydrogen. Reaction. Ba02 -(- 2HC1 = H202 -{- BaCl2. / Barium \ /HydroehloricV /HydrogenV / Barium \ (.Peroxide./ \ Acid. ) \ Peroxide./ (Chloride./ The barium chloride is removed by the addition of silver sulphate. Barium Hydroxide (Ba(OH)„). Made by calcining the nitrate, or a mixture of the nitrate and sulphate, thereby forming an oxide, to which is added water, causing it to slake like lime, forming Ba(OH)2. Refaction. BaO -f- H20 = Ba(OH)2. /BariumV (Water.) / Barium \ V Oxide.) VHydroxide./ 98 MANUAL OF PHARMACY. Strontium Salts. There are no officinal salts of strontium" some of its compounds are used as tests, or for making colored tires. Strontium nitrate (Sr(N()3)2) is the most common salt. Tests. The blowpipe flame has a bright crimson color; solutions of the salts produce precipitates with carbonates and sulphates. LITHIUM SALTS. Source. Lithium is found in the mineral springs of Carlsbad, Marienbad and Franzensbrun. Met with as phosphate in monte- brasite, as fluoride, or silicate, in lepidolite or spodumene. It is the lightest of all metals. Sp. gr. 0.6, and burns with a carmine flame. Its salts are precipitated white, by sodium phosphate and ammonium carbonate. ■General impurities and tests: Salts of Alkalies: Ignite; residue -j- dil. HC1 + evap. to dryness ; residue (1) -{- abs. ale. (3) = sol. -j- ether = ppt. Salts of alkaline earths: Aqueous sol. of above residue in water -j- (NH4)2 C204 = white ppt. Metals: -f- H2S, or (NH4)2S = ppt. This salt is the origin of the other lithium compounds. Lepidolite is heated with 1I2S04, and the aqueous solution, containing impure Li2S04, treated with lime—to separate metallic oxides and earths— and with BaCl2 to remove H2S04, and (NH4)2C204 to remove cal- cium, leaving impure lithium chloride in solution. Evaporate to dryness, and dissolve the residue in a mixture of alcohol and ether (to remove the chlorides of rubidium, caesium, sodium and potassi- um, which are present in lepidolite). Evaporate again, dissolve resi- due in water, and add (NI14)2C03, when Li2C03 precipitates. Wash with alcohol to remove LiCl. (Li2C03—74) Lithii Carbon as.—Carbonate of Lithium. Reaction. 2LiCl (NH4)2C03 — Li2C03 -f- 2NH4CI. /Lithium' /Ammonium' / Lithium ' /Ammonium' 'Chloride./ ' Carbonate. / 'Carbonate./ ' Chloride. / Description. Light, white powder; odorless; alkaline taste, and reaction. Sol. water (130), insol. ale. General impurities. (LiC7H502—128) Lithii Benzoas.—Benzoate of Lithium. Made by treating a mixture of Li2C03 and boiling water, with benzoic acid, evaporating or crystallizing. Li2C03 + 2HC,H502 = 2LiC,H602 + C02 + H20. ( Lithium \ /Benzoic' (Lithium \ (Carbon \ (Water.) 'Carbonate./ \ Acid. ) 'Benzoate./ 'Dioxide./ Description. A white powder, or small, shining scales; faintly benzoin-like odor; cooling, sweetish taste; faintly acid reaction. Sol. water (4), ale. (12). General impurities. Made by dissolving Li2C03 in IIBr, or by the mutual decomposi- tion between Li2C03 and ferrous bromide; filtration and evaporation. (LiBr—86.8) Lithii Bromidum.—Bromide of Lithium. Reaction. FeBr2 L12CO3 — 2LiBr -)— FeC03. / Ferrous ' / Lithium ' ( Lithium ' / Ferrous ' '.Bromide. 7 'Carbonate./ 'Bromide./ 'Carbonate,/ 99 THE CERIUM SALTS. Description. A white, granular salt; very deliquescent; odor- less; sharp, bitter taste; neutral reaction. General impurities. (Li3C6H507—210.). Lithii Citras.—Citrate of Lithium. Made by saturating a solution of citric acid with Li2C03, and evaporating. 3Li2C03 + 2H3C6H507 = 2Li3C6H507 -f 3COa + 3H20. / Lithium \ /CitricX /Lithium\ / Carbon \ (Water.) VCarbonate./ \ Acid./ V Citrate./ VDioxide./ Description. White powder; deliquescent; odorless; cooling, faintly alkaline taste; neutral reaction. Sol. water (5.5), si. sol. ale. (2LiC7H503.H20—B06) Lithii Salicylas.—Salicylate of Lithium. Made by saturating salicylic acid with Li2C03, and evaporating. Reaction. Li2C03 + 2HC7H503 = (2LiC7H503 + H20) + C02. / Lithium \ /'Salicylic -, (Lithium Salicylate.) / Carbon \ VCarbonate./ \ Acid. / VDioxide./ Description. White powder; deliquescent; odorless; sweetish taste; faintly acid reaction; very soluble in water, alcohol and ether. Impurities and tests. General impurities, and Carbonate: HC1 = effervescence. Foreign organic matters: cone. H2S04 = color. CERIUM SALTS. Source. The metal Cerium is found in the minerals cerite and allanite, as silicates of cerium, lanthanum and didymium. (Ce2(C204)3.9H20) Cerii Oxalas.—Oxalate of Cerium. Preparation. The powdered mineral is heated with cone. H2S04 to decompose the silicates, the dried mass ignited, and dissolved in HN03 and treated with H2S to remove copper, etc. A little HC1 is added to hold in solution the calcium salts present, and the cerite metals are precipitated by oxalic acid. The oxalates are purified by calcining with MgC03, thereby decomposing them; the residue dissolved in HN03, and the solution poured into water containing about of H2S04; ceric sulphate is precipitated yellow, while the lanthanum, didymium, and magnesium salts remain in solution. The ceric sulphate is dissolved in fI2S04, and reduced to cerous sulphate by the aid of sodium hyposulphite; by treating the solution with oxalic acid, cerium oxalate precipitates. Description. White, granular powder; odorless; tasteless; insol. in water, and ale.; sol. in HC1. Dose, grs. i-iv. Impurities. Carbonate, metals and aluminium. Cerium Nitrate. Ce2(N03)6, not officinal. Made by the double decomposition between barium nitrate and cerium sulphate. Reaction. 3Ba(N03)2 -f- Ce2(S04)3 — Ce2(N03)e 3BaS04. /Barium \ / Cerium \ /Cerium \ / Barium \ VNitrateJ VSulphate./ VNitrate./ VSulphate./ Description. Colorless crystals; very deliquescent; freely solu- ble in water or alcohol. Dose, grs. i-iv. 100 MANUAL OF PHARMACY. ALUMINIUM SALTS. Source. Exist as a silicate in the ordinary clays; as a fluoride in cryolite (Al2F«.6NaF); also found in the minerals alum-stone, alunite (of Italy), and alum-slate ; as native hydroxide in gibbsite Al2(OH)6 of North America, and diaxpore (A12(OII)2O2) of Europe; as oxide in the ruby, sapphire, corundum, and emery. Aluminium is a very light (sp. gr. 2.67) silvery white metal. Used as an alloy, and in making aluminium-bronze, which bears the color and appearance of gold, and is much more durable than that metal. The propelling-screw of many of the largest ocean steamers is made of this alloy. Tests. Hydroxide of sodium or potassium produce white precipi- tates (Al2(OH)6) soluble in excess of the alkali. Water of ammonia yields a like precipitate, insoluble in excess. Alkaline carbonates give a similar reaction, with the evolution of C02. Ammonium sulphide also precipitates Al2(OH)6, but with evolution of H2S. General Impurities and tests. Iron (limit): Potass, ferrocyanide = blue color. Zinc, or lead: -f- NaOH -f- (NH4)2S = ppt. Alums. An alum is the double sulphate of a monad and pseudo- triad element, crystallizing in cubes and octahedra, with twenty- four molecules of water. Examples. Alums containing Aluminium: K2S04 + A12(S04)3 + 24H20 = K2A12(S04)4 . 24H20. /Potassium\ /Aluminium \ (Water.) (Potassium Alum.) \ Sulphate. / \ Sulphate. ) (NH4)2A12(S04)4.24H20 (Ammonium alum); Na2Al2(S04)4.24H20 (Sodium alum); Al2Cs2(S04)4.24H20 (Caesium alum), Al2Rb2(S04)4. 24H20 (Rubidium alum),Ag2Al2(S04)4.24H20 (Silver alum), etc. Alums not containing Aluminium: (NH4)2Fe2(S04)4.24H20 (Am- monio-ferric alum), (NH4)2Cr2(S04)4.24H20 (Chromium alum), K2Fe2(S04)4.24H20 (Potassio-ferric alum), etc. (K2A12(S04)4.24H20—948) Alumen.—Potassa Alum. (Sulphate of Aluminium and Potassium.) Preparation. Clays (Pipe clay) are selected as free from iron and CaC03 as possible, and calcined to oxidize the iron, as well as to render them pulverizable. They are then treated with dilute H2SO4 and heated. The resulting solution of aluminium sulphate is mixed with K2S04; and on concentration and cooling, crystals of alum are obtained. Also made from cryolite by the same method. Description. Large, colorless, octahedral crystals; odorless; sweet, astringent taste; acid reaction; sol. water (10.5), insol. ale. Impurities and tests. General impurities, and Ammonia alum: -|- KOH -f Heat = odor of NH3, or the same reaction if powder is dropped on slaking lime. Officinal Preparations. Alumen Exsiccatum. (Dried Alum. Burnt Alum.) (K2A12(S04)4—516.) Made by driving off the water of crystallization from alum (184) at a temperature below 401° F., and heating until the mass becomes porous and weighs (100). THE HALOGEN SALTS. 101 Description. A white, granular powder; attracts moisture from air; v. si. sol. in water (20); other characteristics like the crystal. Alum is often used as a mordant (mordeo—to bite) for fixing colors in fabrics, and other material; also forms lakes (compounds of alumina with coloring matter), by adding alum to the solution con- taining coloring matter, when the lake precipitates. Ammonia-Alum. ((NH4)2A12(S04)4.24H20.) Not officinal; but extensively used. Made by treating a solution of A12(S04)3 with (NH4)2S04 and crystallizing. (Al2(OH)6—156) Aluminii Hydras.—Hydrated Alumina. (Hydroxide of Aluminium.) Made by mixing boiling hot solutions of alum and sodium car- bonate. The precipitate is well washed and dried. Reaction. K2A12(S04)4 -f- 3Na2C03 + 3H20 = Al2(OH)e (Potassa-alum.) / Sodium \ (Water.) /Aluminlum\ VCarbonate./ \ Hydroxide./ + K2S04 + 3Na2S04 + 3C02. / Potasslum\ / Sodium \ / Carbon \ \ Sulphate. ) \Sulphate.) \ Dioxide./ Description. White, light, amorphous powder; odorless; taste- less; insol. water, or alcohol. Impurities and tests. General impurities, and sulphate HC1-)- BaCl2 = white ppt. Alkaline earths (a limit): Boil with H20 -}- evap. = residue. (A12(S04)3.18H20—666) Aluminii Sulphas.—Sulphate op Aluminium. Made by dissolving Al2(OH)6 in dilute H2S04, and evaporating to dryness. Reaction. Al2(OH)s -f 3H2S04 = A12(S04)3 + 6H20. /'Aluminium'. /SulphurieX /'Aluminium'v (Water.) VHydroxide./ \ Acid. / \ Sulphate. / Description. White crystalline powder; odorless; sweet, as- tringent taste; acid reaction; sol. water (1.2), insol. ale. THE HALOGENS AND THEIR SALTS. The above are called halogens (salt producers), and their salts termed haloid salts (ctXj—sea salt, ei'Soi—like, resembling sea-salt). Chlorine, Iodine, Bromine and Fluorine. CHLORINE. Discovered 1774, by Sckeele. Description. A heavy, yellowish-green gas, having an irritating and suffocating odor; Sp. gr. 2.450. A great bleaching agent and disinfectant. Preparation. Made by the action of H2S04 on NaCl and Mn02; the mixture is heated, and the gas evolved. 102 MANUAL OF PHARMACY. Reaction. 4NaCl + Mn02 -j- 2H2S04 = MnCl2 ( Sodium \ /Manganese\ /SulphurlcX / Manganese\ * (Chloride./ ( Dioxide. ) ( Acid. / ( Chloride. ) + Cl2 + 2Na2S04 + 2H20. (Chlorine.) / Sodium \ (Water.) (Sulphate.) Other methods: Mn02 -f- 4HC1 = MnCl2 -(- Cl2 -j- 2H20 or, K2Cr207 + 14HC1 = 3C12 + 2KC1 -f Cr2Cl6 + 7H20. / Potassium \/HydrochloricN (Chlorine.) /Potassium\ /'Chromium'v (Water.) (Bichromate./( Acid. / (Chloride.) (Chloride. / 4KC103 + 12HC1 = C1,90. + 4KC1 + 6H20. (Euchlorine), a very explosive gas. Euchlorine (-f water) = Cl9 -j- 3C102. or, Tests for Chlorides and Hydrochloric Acid: A curdy white precipi- tate is produced with AgN03, soluble in NH4OH, but insol. in HN03. Aqua Chlori.—Chlorine Water. By the action of HC1 on Mn02 (as shown above) Cl. is evolved, and passed into cold distilled water until the latter is saturated. Description. A greenish-yellow liquid ; suffocating odor; dis- agreeable taste. Contains 0.4$ of Cl. Should leave no residue on evaporation; and is- decomposed by exposure to air or sunlight, forming HC1. 2C1 -f H20 = 2HC1 + O. Impurity. Hydrochloric Acid: Shake with mercury in excess, until the odor of Cl. disappears ; the remaining liquid gives an acid reaction. The Assay Process is based upon the amount of volumetric solu- tion of sodium hyposulphite required to decolorize the iodine liber- ated from a solution of potassium iodide, by a definite quantity of Cl. water. Extemporaneous preparation of Chlorine Water. 1. NaCl—60 grs., lead oxide (red)—350 grs., triturate and introduce into a bottle; add water f 1 viij and H2S04 f 3 ij and let stand; PbS04 precipitates, while Cl. and Na2S04 are in solution. 2. KC103—60 grs., is put into an 8-oz. bottle; add HC1 f 3 ij; let stand till reaction ceases, and add water to make one pint. Made by the action of Cl. on milk of lime. Calx Chlorate.—Chlorinated Lime. (Chloride of Lime.) 2Ca(OH)2 + 4C1 = (CaCl2 + Ca(C10)2 + 2H20). ( Calcium \ (Chlorine.) (Calcium \ ( Calcium \ (Water.) (Hydroxide.) (chloride./ (Hypochlorite./ CaCl2Ca(C10)2 = 2(CaO)Cl2; the supposed composition of this salt; hence the name “ Chloride of Lime.” Description. White, or grayish-white powder (slightly damp); —or friable lumps; becoming moist, and gradually decomposing on exposure to air; feeble, chlorine-like odor; disagreeable, saline taste. Partially soluble in water, and in alcohol; completely sol. in HC1. evolving Cl., the solution having an alkaline reaction. 2(CaO)Cl2 -f 4HC1 = 2CaCl2 + 2C12 + 2H20. (Chloride of Lime.) /Hydrochloric\ ( Calcium \ (Chlorine.) (Water.) ( Acid. ) ( Chloride./ THE HALOGEN SALTS. 103 The aqueous solution quickly bleaches the color of litmus or indigo. Chlorinated Lime should contain at least 25% of available chlorine. Assay Process. Mix 0.71 Gm. CaOCl2 with sol. KI (1.25 Gm. in 122 cm3 water) and dilute HC19 Gms.; the red-brown solution should require not less than 50 cm3 of volumetric solution of sodium hyposulphite for complete decoloration. Explanation. The available chlorine is derived from the Ca(C10)2 (one of the portions of this salt), as the CaCl2 cannot give up its Cl. In the first part of the assay process, iodine is liberated from the potassium salt, producing the red-brown solution (or in the case of the presence of gelatinized starch, as in Liq. Sodse Chloratae, a blue color); the hyposulphite causes the formation of tetrathionate and iodide of sodium, the red or blue color disappearing as soon as all of the free iodine has been converted into the iodide. Reaction. 2Na2S203 -f- I2 = 2NaI -f- Na2S4Oe. ( Sodium \ (Iodine.) /SodiumN ( Sodium \ (Hyposulphite./ (Iodide./ (Tetrathionate./ Properties. A great bleaching agent and disinfectant. Liquor Soda; Chlorate.—Solution of Chlorinated Soda. (Labarraque’s Solution.) Made by decomposing a mixture of chlorinated lime and water, with a boiling hot solution of Na2C03; CaC03 precipitates, and the clear solution is decanted. Reaction. Ca(C10)2 -j- CaCl2 -{- 2Na2C03 — / Calcium \ / Calcium \ / Sodium \ (Hypochlorite./ (Chloride./ (Carbonate./ 2CaC03 + 2NaCl + 2NaC10. ( Calcium \ / Sodium \ / Sodium \ (Carbonate./ (Chloride.) (Hypochlorite./ or CaOCl2 + Na2C03 = Na2OCl2 + CaC03. Description. Clear, colorless liquid ; faint odor of Cl; alkaline taste and reaction ; decolorizes indigo. Sp. gr. 1.044. HC1 causes effervescence of Cl and C02. Sol. Chlorinated Soda should contain at least 2 % of available chlorine. Assay Process. 8.88 Gm. of the solution-f-sol. KI (2.6 Gm. in 200 cm3 water) +18 Gm. HC1 and a little gelatinized starch, should require for complete decoloration not less than 50 cm3 of vol. sol. sodium hyposulphite. Javelle Water.—(Solution Chlorinated Potassa.) Not officinal. Made by substituting an equal quantity of K2C03 for Na2C03 in the above formula. IODUM (Iodine). This non-metallic element is obtained from kelp, the ashes of cer- tain sea-weeds, and from the mother liquor left on crystallizing Chili nitre (NaN03); also found in many mineral springs, in sea- water, cod-liver oil, sponge, coal, etc. Preparation. The sea-weeds are charred at as low a temperature as possible to avoid loss of I. The ash is lixiviated with water, and 104 MANUAL OF PHARMACY. the solution concentrated. During evaporation Na2S04 separates out, and on cooling KC1 deposits. The uncrystallizable mother liquor contains I in the form of iodide and iodate of sodium. On mixing with excess of H2S04 and heating with Mn02, the I, dis- tils, leaving sodium and manganous sulphates in the retort. Reaction. 2NaI -|- Mn02 -(- 2H2S04 = I2 /Sod in m\ /ManganeseX /SulphuricX (Iodine) \ Iodide.) \ Dioxide. ) \ Acid. ) + Na2S04 + MnS04 + 2H20. / Sodium X /ManganousX (Water.) VSulphate./ \ Sulphate. ) Purification. In its crude state I is contaminated with water, and sometimes ICN or IC1. Purify by drying, and then subliming; ION and IC1 (the more volatile compounds) sublime first; then the receiver is changed and the heat raised till the iodine has all dis- tilled over. The presence of water may be detected by shaking with chloroform, when a limpid, unclear liquid results. Description. Heavy, bluish-black, dark and friable, rhombic plates, of a metallic lustre, resembling iron ; distinctive odor; sharp, acrid taste, and neutral reaction. Imparts a deep brown, slowly evanescing stain to the skin, and destroys vegetable colors ; sp. sol. water, sol. ale. (1), very sol. ether, CS2, chloroform, and KI solu- tion. Should contain 100$ of absolute iodine, the quantitative test de- pendent upon the amount of a volumetric solution of hyposulphite of sodium required to decolorize a solution of a definite quantity of iodine in solution of potassium iodide. Tests for Iodine and Iodides. Iodine: With gelatinized starch in a cold solution, iodine gives a dark, blue color. Iodides: 1. Add chlorine water to liberate free iodine, and apply the above starch test; or if the colored liquid be agitated with ether, benzin, CS2, or chloroform, the iodine dissolves. 2. With soluble salts of lead, the neutral iodides produce a yellow precipitate. 3. With mercuric chloride, a red precipitate. 4. With silver nitrate, a white precipitate, si. sol. in NII4OH, insol. in HN03. Officinal Preparations. 1. Liquor Iodi Compositus (Lugol’s Solu- tion) contains I (5), KI (10), Water (85); about 3£ grs. I in f3j. 2. Tinctura Iodi—8$ Iodine. 3. Unguentum Iodi. Contains I (4), KI (1), Water (2), Benz. Lard (93). Syrupus Acidi Hydriodici.—Syrup op Hydriodic Acid. Made by passing H2S into an alcoholic solution of I mixed with syrup, until the latter becomes light yellow in color, heating to drive off H2S, flavoring with spirit of orange and dissolving more sugar in the liquid. Reaction. I2 -f H2S = 2HI -f- S. (Iodine.) I'Hydrogenj j (Sulphur.) Description. A transparent, colorless, or pale, straw - colored liquid; odorless; sweet, acidulous taste; acid reaction; sp. gr. 1.300—contains 1% of absolute HI. THE HALOGEN SALTS. 105 (KI—165.6) Potassii Iodidum.—Iodide of Potassium. Made by adding Iodine to a hot solution of KOH, until the liquid remains slightly colored from excess of iodine, when iodide and iodate of potassium are formed. Reaction. 6KOH 4- 61 = 5KI + KIOs + 3H20. /Potassium \ (Iodine) /Potassium\ /Potassium\ (Water.) \Hydroxide.) \ Iodide. ) \ Iodate. ) The solution is evaporated to dryness, powdered charcoal is added, and the mixture heated to redness, in order to deoxidize the iodate, thereby converting it to the iodide. Reaction. KI03 + 3C + Heat = KI -f 3CO. /PotassiumN (Charcoal.) /'PotassiumN ( Carbon \ ( Iodate. ) ( Iodide. ) \Monoxide./ Dissolve, evaporate and crystallize. Description. When pure it occurs in colorless, translucent, cubical crystals, slightly deliquescent, having a peculiar faint odor ; a pungent, saline, bitter taste; neutral reaction ; sol. water (0.8), ale. (18). The commercial salt appears in white, opaque crystals, having a faintly alkaline reaction (due to crystallization from an alkaline solution, thus producing a more stable salt), but single crystals placed on moistened red litmus paper should not at once produce a violet-blue stain (showing the absence of more than 0.1$ of alkali). Impurities and tests. Iodate: -f- gelatinized starch -|- dilute H2S04 (or H2C4H406) = blue color. Chloride, or bromide: Sol. in NH4OH -(- AgN03; lilt, -f- HN03 (excess) = cloudiness. Sulphate (limit): -f- Ba(N03)2 = white ppt. A simple test to distinguish between KI and KBr is their solubility: KI (1) in water (0.8)—KBr (1) in water (1.6). KI (1) in alcohol (18)—KBr (1) in alcohol (200). Officinal Preparations. Unguentum Potassii Iodidi (Ointment of Iodide of Potassium). Contains KI (12), Na2S203 (1), boiling water (6), and benz. lard (81). The hyposulphite of sodium is added to prevent the liberation of free iodine, which would change the color of the ointment from white to yellow or brown. (Nal—149.6) Sodii Iodidum.—Iodide of Sodium. Made by a process analogous to that by which KI is produced— (1) 6NaOH + 61 = 5NaI + NaI03 + 3H20. ( Sodium \ (Iodine.) /Sodium\ /SodiumX (Water.) (Hydroxide.) (iodide.) (iodate.) (2) NaI03 4- 3C = Nal + 3CO. or made by the double decomposition between ferrous iodide and sodium carbonate. Reaction. Fel2 -(- Na2003 == 2NaI FeC03. /Ferrcus\ ( Sodium \ /Sodium\ ( Ferrous \ \ Iodide. / \Carbonate.) \ Iodide. ) (Carbonate.) This salt is little used on account of its great deliquescent nature. Description. Minute, colorless, or white, monodinic crystals, or a crystalline powder; very deliquescent; odorless; having a saline and 106 MANUAL OF PHARMACY. slightly bitter taste; neutral or faintly alkaline reaction; sol. water (0.6), ale. (1.8). Impurities, same as KI. (CHI3—892.8) Iodoformum.—Iodoform. (Methenyl Iodide.) Made by the action of I. on alcohol in the presence of a fixed alkali or alkali carbonate; also true regarding the action of I on certain ethers, aldehyd, acetone, amylene; butyl, capryl, and propyl alcohols, kinic, lactic, meconic acids, and other compounds. Process. Iodine, KHC03, water, and alcohol are mixed in a flask and heated until the color has disappeared, then more iodine is added in portions as long as the liquid remains colorless on heating; set aside to cool and crystallize. Reaction. C2H5OH —|— 81 -f- 6KHCO3 = CHI3 ( Ethyl \ (Iodine.) / Potassium \ (Iodoform.) (Hydroxide./ (Bicarbonate./ + 5KI + KCHOa + 6C02 + 5H20. /PotassiumN /Potassiuim / Carbon \ (Water.) \ Iodide. ) \ Formate. / \Dioxide.) Both iodide and formate of potassium are always produced, but additional crystals of CHI3 may be obtained by passing Cl into the mother liquor, by which the KI becomes decomposed, I being set free, which in turn decomposes the alcohol, producing more CHI3. Description. Small, lemon-yellow, lustrous crystals of the hexa- gonal system; saffron like and almost insuppressible odor; unpleas- ant iodine-like taste; neutral reaction in solution. Insol. water; sol. in alcohol (80), ether (5.2), chloroform, CS2, benzol, benzin, fixed and volatile oils. Impurities and tests. Iodide, or iodate: Shake with water = no change of color to litmus paper; and filtrate + AgNO:) = white ppt. Officinal Preparation. Unguenttjm Iodoformi (Iodoform Oint- ment) contains iodoform (10), incorporated with benzoinated lard (90). Note.—To disguise the unpleasant odor of iodoform, in mixtures and oint- ments, add 3-5 drops of oil of peppermint to the ounce; balsam peru, couma- rin, oils of fennel, anise and thyme are also employed for the same purpose. BROMUM (Bromine). A liquid non metallic element obtained from sea-water, and from saline springs. Occurrence. It is found as magnesium or calcium bromide, and obtained in considerable quantities from the mother liquors of many salt works in the United States and Europe. Preparation. These mother liquors (bittern), which have been freed by crystallization as much as possible from alkaline chlorides and sulphates, contain the bromine usually in combination, as MgBr2 or CaBiv After evaporation, the concentrated solution is heated with HC1 and MnO», and Br. distils. The neck of the retort is plunged into cold water, and the Br. collects in drops at the bottom of the re- ceiver. THE HALOGEN SALTS. 107 Reaction. MgBr2 -f" 4HC1 Mn02 = MgCl2 /Magnesium\ /Hydrochloric'. /Manganese\ /MagnesiumX V Bromide. ) V Acid. / \ Dioxide. / \ Chloride. / + MnCl2 + Br2 + 2H20. /Manganese\ (Bromine.) (Water.) V Chloride. / The MgBr2 is sometimes decomposed by passing Cl. directly into the solution. Reaction. MgBr2 + 2C1 = MgCl2 + Br2. /Magnesium'. (Chlorine.) /Magnesium', (Bromine.) \ Bromide. ) \ Chloride. / Description. Dark, brownish-red mobile liquid, evolving at all temperatures a yellowish-red vapor, very corrosive and suffocating, and highly irritating to the eyes and lungs, and having a peculiar suffocating odor, resembling chlorine. Sp. gr. 2.990—sol. water (33), v. sol. alcohol and ether, gradually decomposing these two liquids, also very soluble in chloroform, CS2; destroys color of litmus and sulphate of indigo. Impurities. Chlorine, and Iodine; a limit of each allowed. Tests for Bromine and Bromides. Bromine: With gelat- inized starch, gives a yellow color. Bromides: 1. Add chlorine to strong solution, bromine is liberated, and apply the above starch test; or if the colored liquid be agitated with ether, chloroform, CS2 or benzine, the bromine dissolves. 2. With silver nitrate a yellow- ish-white precipitate results, insoluble in HNOa, slightly soluble in NH4OH. 3. Concentrated H2S04 added to the salt, yields reddish vapors of bromine. (KBr—118.8) Potassii Bromidum.—Bromide of Potassium. Pkeparation. Made by three processes. 1. The double decom- position between ferrous bromide and K2C03: Reaction. FeBr2 -f- K2C03 = 2KBr -)- FeC03. / Ferrous \ /Potassium \ /Potassium', / Ferrous \ '.Bromide./ '.Carbonate./ \ Bromide. / VCarbonate./ 2. The double decomposition between calcium bromide and potas- sium sulphate: Reaction. CaBr2 -f- K2S04 = CaS04 -f- 2KBr. * (Calcium \ /'Potassium'. /'Calcium'. /Potassium\ 'Bromide./ \Sulphate./ VSuiphate./ \ Bromide. / 3. The action of bromine on a solution of potash, thereby produc- ing bromide and bromate of potassium, calcining with charcoal, solution, filtration and crystallization: (a) 6KOH + 6Br = 5KBr + KBr03 + 3H20. /Potassium \ (Bromine.) /PotassiumN /PotassiumX (Water.) VHydroxide./ V Bromide. ) \ Bromate. ) (b) KBr03 + 3C = KBr + 3CO. /Potassium\ (Charcoal.) /PotassiumN / Carbon \ \ Bromate. / \ Bromide. / VMonoxide./ The latter step may also be accomplished as follows: KBrOs -f- 3H2S = KBr + 3H20 + S3. Description. When pure: colorless, translucent, cubical crys- tals, permanent in dry air, odorless, having a pungent, saline taste, 108 MANUAL OF PHARMACY. and a neutral reaction. Soluble in water (1.6), alcohol (200). The commercial salt appears in white opaque, or semi-transparent crys- tals; faintly alkaline reaction (due to crystallization from an alka- line liquid), but single crystals laid on moistened red litmus paper should not at once produce a violet-blue stain (absence of more than 0.1$ alkali). Impurities and tests. Bromate: Drop dil. H2S04 on crushed crystals = yellow color. Iodide: Sol. + starch jelly -j- Cl. water = blue zone. Sulphate (a limit): -)- Ba(N03)2 = white ppt. Chloride: (more than 3$): Volumetric test for chlorides, using potass, bichrom- ate as an indicator, and AgN03 as the precipitant. Made by processes identical with those for KBr., substituting a sodium salt for the potassium compound. Description. Small, colorless or white, monoclinic crystals, or a crystalline powder; permanent in dry air; odorless; saline, slightly bitter taste; neutral or faintly alkaline reaction. Sol. water (1.2), alcohol (13). Impurities, and tests for their presence, are identical with those found under Potassium Bromide. (NaBr—102.8) Sodii Bromidum.—Bromide of Sodium. (HBr—80.8) Acidum Hydrobromicum Dilutum.—Diluted Hydrobromic Acid. Preparation. Several methods. 1. The action of H2S04 on KBr; the crystals of K2S04 are allowed to crystallize out, the mother liquor distilled, and the distillate diluted to the proper degree : Reaction. 2KBr -|- H2S04 = K2S04 + 2HBr. /Potassium\ /Sulphuric-) /Potassium-) /Hydrobromic-) \ Bromide. ) \ Acid. ) \ Sulphate. / \ Acid. ) 2. The decomposition of KBr by tartaric acid; potassium bitar- trate precipitates, while HBr is left in solution: Reaction. KBr -)- H2C4H4O6 = KHC4H406 + HBr. /Potassium-) /Tartaric-) /Potassium-) /Hydrobromic-) „ V Bromide. / \ Acid. / V Bitartrate./ V Acid. / 3. By the action of Br. on phosphorus, pentabromide of phos- phorus is formed; this taking place in the presence of water, the latter decomposes, as is shown below : Reaction. PBr5 + 4H20 = H3P04 -j- 5HBr. / Phosphorus \ (Water.) /Phosphoric\ /Hydrobromic-) vPentabromide.,/ \ Acid. ) \ Acid. / The HBr is distilled off, and H3P04 remains in the retort. Description. A clear, colorless liquid; odorless; strongly acid taste; acid reaction; contains 10$ absolute HBr and 90$ water. Sp. gr. 1.077. Tent. Same as for bromides. Impurities and tests. Organic matter : discolored by age. Sul- phuric acid: -j- BaCl2 = white ppt. THE CYANOGEN SALTS. 109 CYANOGEN SALTS. Cyanogen. (CN) is a gas obtained by heating mercuric cyanide (Hg(CN )2) or silver cyanide (AgCN). (K4Fe(CN)8.3H20—421.9) Potassii Ferrocyanidum.—Ferro- cyanide of Potassium. (Yellow Prussiate of Potash.) Prepared by heating in suitable iron vessels K2C03 (free from sulphate, to prevent the formation of sulpliocyanide) until melted, and introducing a mixture composed of iron filings and charcoal obtained from refuse animal matter rich in nitrogen. When C02 and inflammable gases cease to be evolved, the liquid mass is ladled out, cooled, lixiviated with water, and the resulting solution crys- tallized. “Purified by re-crystallization. [Note. This process is one of pure synthesis; the nitrogenous bodies produce the N and C, which combine with the Fe and K.] Description. Large, coherent, lemon-yellow, translucent, soft crystals; slightly efflorescent in dry air; odorless; sweet, saline taste; neutral reaction. Sol. water (4), insol. alcohol. Tests. Aqueous solution with ferric salts gives, a dark-blue pre- cipitate (Prussian Blue); with ferrous salts bluish-ichite gradually turning darker; with copper salts, red-brown (chocolate); with lead acetate, white ; with mercuric salts, white. Impurities and tests. Carbonate: —(— dil. H2S04 = effervescence. Sulphate (a limit): HC1 -J- BaCl2 = cloudiness, or white ppt. Chloi'ide (a limit): Fuse with KN03 4- H20; filt. -f- AgN03 = white ppt. This salt is the source of the other compounds of cyanogen. Ferricyanide of Potassium.—Red Prussiate of Potash. (K8Fe2(CN)42).—Officinal as Test-solution. Made by passing Cl into a cold solution of the ferrocyanide; the liquid changes in color from yellow to red, and when it ceases to produce a blue precipitate or blue color with ferric chloride, it is concentrated to crystallization. Reaction. 2K4Fe(CK)« -f- Cl2 = K6Fe2(CN)i2 -f- 2KC1. . / Potassium \ (Chlorine.) ( Potassium \ /PotassiumV VFerrocyanlde./ VFerricyanide./ V Chloride. / On exposure to air, this salt decomposes into the ferrocyanide. The fresh aqueous solution is used as a test; with ferrous salts, it gives a dark-blue precipitate (Turnbull’s Blue); with copper salts. brownish-yellow; mercurous salts, red-brown; silver salts, orange colored ; but no precipitates, with ferric, mercuric, or lead salts. Ferrocyanide of Iron.—Prussian Blue. (Paris Blue. Williamson’s Blue. Fe43Fe(CN)8.) Not officinal. Made by double decomposition between ferrocyanide of potassium and a ferric salt, washing and drying the precipitate. 3K4Fe(CN)8 + 2Fe2(S04)3 = Fe4(FeCN6)8 + 6K2S04. / Potassium \ ( Ferric \ / Ferric \ /PotassiumV VFerrocyanlde./ VSulphate./ VFerrocyanlde.) V Sulphate. ) Also made by precipitating ferrous sulphate with potass, ferro- cyanide, and exposing the bluish-white precipitate to the air, till it ■has acquired the proper color. 110 MANUAL OF PHARMACY. (KCN—65) Potassii Cyanidtjm.— Cyanide of Potassium. Made by fusing exsiccated potassium ferrocyanide with K-2C03; pour the liquid mass from the sediment of iron, and allow the former to cool and solidify. 2K4Fe(CN)« + 2K2C03 = 10KCN -f 2KCNO + Fe2 + 2C02. / Potassium \ /Potassium ! /Potassium \ /Potassium \ (Iron.) / Carbon \ (Ferrocyanide./ (Carbonate./ ( Cyanide. / ( Cyanate. / (Dioxide./ The cyanate is dissolved out with CS2. Another method. HCN is passed into an alcoholic solution of KOH, and the crystalline precipitate washed with alcohol and dried. May also be made by heating the ferrocyanide. The KCN is dissolved out with water, while carbide of iron re- mains undissolved. Description. White, opaque, amorphous pieces, or a white, granular powder; deliquescent in damp air; odorless when perfectly dry, but generally of a peculiar, characteristic odor; sharp, alkaline, and bitter almond taste; strong alkaline reaction; sol. water (2), sp. sol. alcohol. Should contain at least 90$ of pure KCN, determined by the amount of volumetric solution of silver nitrate it will precipitate. Impurity. Carbonate: -|- acid = brisk effervescence. Most poisonous salt known; rarely given internally. Dose, to gr. K4Fe(CN)6 + Heat = 4KCN + N2 + FeC2. (HCN—27) Acidum Hydrocyanicum Diltjtum.—Diluted Hydrocyanic Acid. (Prussic Acid.) Two methods given in the U. 8. Pharmacopoeia. First Method. Made by distilling a mixture of H2S04, ferro- cjanide of potassium, and water; the condensed vapor is dissolved in diluted alcohol, and sufficient water is added to bring the product to the proper degree of strength. The equation for the reaction taking place in the above process may be written as follows: 2K4Fe(CN), + 3H2SO4 = 3K2SO4 4- Fe2K2(CN)6 / Potassium ! /Sulphuric"! /Potassium! / Potassium Ferrous ! (Ferrocyanide./ V Acid. / (Sulphate./ (Ferrocyanide (Everitt’s Salt)./ + 6HCN. The intermediate reactions are as follows: (1) K4Fe(CN)6 + 2H2SO.i = 2K2S04 + H4Fe(CN)6. (Hydroferrocyanic acid.) (2) H4Fe(CN)6+ K4Fe(CN)6+H2S04=6HCN+ K2SO4+ K2Fe2(CN)6 (Everitt’s salt— a white salt rapidly turning green and then blue in the presence of oxygen.) Extemporaneous Method. Mix HC1 (5) with dist. water (55), add AgCN (6) and shake; let the precipitate subside, and pour off the clear liquid. Reaction. AgCN + HC1 = AgCl + HCN. / Silver \ /Hydrochloric! / Silver ! /Hydrocyanic! (Cyanide./ ( Acid. / (Chloride./ V Acid. / SULPHUR. Description. A colorless liquid, having odor and taste of bitter almonds; slightly acid reaction; completely volatilized by heat. Test for identity. Acid -f- KOH (excess) -j- FeS04 -f- Fe2Cl6 + HC1 = blue ppt. Should contain 2% absolute HCN. Assay Process. 6.75 gms. diluted HCN -j- 30 cm3 water, mixed with sufficient aqueous suspension of magnesia to make the mixture quite opaque, and afterwards with a few drops of a dilute solution of potassium chromate, should require 50 cm3 of the volumetric sol. of AgN03, before the red color caused by the latter ceases to disappear on stirring. Explanation. The magnesia is added not only to pre- vent the volatilization of the acid, but also because the double cyanides of silver with alkali-metals are very permanent; and to pro- duce a white background to show the red precipitate. Chromate of potassium is used as an indicator, as all of the cyanide will be pre- cipitated white, before the red silver chromate forms. Diluted hydrocyanic acid becomes discolored on keeping, due to the formation of paracyanogen. It has been suggested that, if kept in cork-stoppered bottles, this change can be prevented or retarded, but such appears not to be the case. Dose. Two to four drops. Extremely poisonous. Antidotes. Mild inhalations of ammonia or chlorine, and the application of cold water to the head and spine, or take the following three solutions, in order, viz.: Ao. 1. K2C03, 20 grs. in water f 1 j. No. 2. FeS04, 10 grs. in water f 1 j. No. 3. Tinct. Fe2CU, f 3 j. The object of the above being to form, first, potassium cyanide; second, potassium ferrocyanide; third, ferrocyanide of iron (insoluble Prussian Blue). Ammonium Sulphocyanide. (NH4CNS.) Made by dissolving CS2 in alcohol and heating in the presence of ammonia. CS2 -f- 2NH;, = nh4cns + h2s. Potassium Sulphocyanide. (KCNS.) Made by heating K2C03, sulphur and K ,Fe(CN)(;, treating the cooled mass with alcohol, and crystallizing. The two salts just treated of are very delicate tests for ferric salts, giving a blood-red precipitate, which is not discharged by HC1 (differ- ence from acetates and formates), but disappears on the addition of mercuric chloride (difference from meconates). SULPHUR. Occurrence. Found native in great abundance in volcanic regions, beds of which have been discovered in the Western United States, Mexico, West Indies, etc. The chief supply however, comes from Italy. Sulphur is also a constituent of the volatile oils of mustard, garlic and horseradish; and of albumen and other proteids; also found in mineral waters as H2S and sulphates; in iron pyrites (FeS2), galena (PbS), blende (ZnS), black antimony (Sb2S3), cinnabar (HgS), gypsum (CaS04), heavy spar (BaS04), etc. 112 MANUAL OP PHARMACY. Recovery. Obtained by melting it from the ore, running into moulds and solidifying, forming the rough-sulphur of commerce. Sulphur is officinal in three forms, viz.: sublimed, washed and pre- cipitated. Sulphur Sublimatum.—Sublimed Sulphur. (Flowers of Sulphur.) Made by subliming the rough sulphur from iron retorts. It con- denses in the form of a fine powder, which is removed from time to time, before the condensing chamber becomes too hot. If however, the operation is not interrupted, the brick walls of the condenser be- come hot enough to melt the sulphur, which is then conducted into moulds, and constitutes brimstone or roll-sulphur. Description. Fine, citron-yellow powder, of a slight character- istic odor; faintly acid taste; acid reaction; insol. water, or alcohol. Officinal Preparations. 1. Sulphur lotum. 2. Sulphur praecipita- tum. 3. Unguentum sulphuris (Sulphur Ointment). Contains sub- limed sulphur (30), benzoinated lard (70). Sulphur Lotum.—Washed Sulphur. Made by washing sublimed S. with a dilute water of ammonia (to remove H2S04 and other impurities) until the washings cease to precipitate BaCl2, then draining and drying and passing through a 30-mesh sieve. The ammonia neutralizes the acid, forming (NH4)2S04, which is washed out. Description. Fine, citron-yellow powder; odorless; almost taste- less; insoluble in water and alcohol; sol. in boiling solution NaOH, or in CS2. Impurities and tests. Free acid: litmus paper = red color. Arsenious sulphide: -(- NH4OH (2); tilt, -f- IICl (excess) = ppt. Arsenious acid: filtrate from above -f- H2S = yellow ppt. Officinal Preparations. 1. Pulv. glycyrrhizse compositus (Com- pound licorice powder). Contains senna (18), glycyrrhiza (16), fennel (8), washed S (8), sugar (50). 2. Ung. sulphuris alkalinum (See K2C03). 3. Sulphuris iodidum. Sulphuris Iodidum.—Iodide op Sulthur. Subiodide of Sulphur. (S2I2.) Made by fusing together, in a flask, washed sulphur (1) and iodine (4). Used in ointments. Sulphur Pr.ecipitatum.—Precipitated Sulphur. (Milk of Sulphur.) Slaked lime is boiled with sublimed S (forming calcium penta sulphide and thiosulphate), then HC1 is added to nearly neutralize the mixture; sulphur precipitates, and is thoroughly washed with water and dried. First reaction. 3Ca(OH)2 -J- 6S2 = 2CaS5 + CaS203 ( Calcium \ (Sulphur.) / Calcium \ /Calcium ThioA (Hydroxide./ \Pentasulphide.y V sulphate. / -f 3H20. (Water.) SULPHUR. 113 Second reaction. 2CaS5 -f- CaS203 -f- 6HC1 = 6S2 / Calcium \ ( Calcium \ /HydrochloricX (Sulphur.) \Pentasulphide.) (.Thiosulphate./ \ Acid. ) + 3CaCl2 + 3H20. / Calcium \ (Water.) (chloride./ Lac sulphuris, made by adding H2S04 to the solution obtained by the first step of the above process; contains a large quantity of CaS04, which is most objectionable, thus : Reaction. 2CaS5 -+- CaS203 -(- 3H2S04 = 3CaS04 / Calcium \ ( Calcium \ /Sulphuric\ (Calcium \ VPentasulphide.) \Thiosulphate.) ( Acid. ) \Sulphate./ + 6S2 + 3H20. (Sulphur.) (Water.) Description. Fine, yellowish-white, amorph. powder; odorless; almost tasteless; insol. water, or alcohol; soluble boiling sol. NaOH, or in CS2. Impurities and tests. Free acid : -|- blue litmus paper = red color. Calcium sulphate: Boil with dil. HC1; tilt, -f- BaCl2 or (NH4)2C03 = ppt. Alkalies, alkaline earths, or sulphide: Digest successively with water, HC1, and NH4OH; evap. flit, from each = residue. Arsenious acid: same test as under Washed Sulphur. Hydrosulfhuric Acid. (H2S.) Made by the action of dil. H2S04 on ferrous sulphide (FeS): the gas H2S (Hydrogen sulphide, or sulphuretted hydrogen) is washed and passed into water and dissolved. FeS H2S04 = H2S -f- FeS04. Used as a test for the metals, yielding with their salts character- istic precipitates. (CS2—76) Carbonei Bisulfhidum.—Bisulphide, or Disulphide of Carbon. Made by heating fragments of charcoal or coke to redness, and dropping through a tube to the bottom of the retort, pieces of sul- phur, which vaporize and unite with the red-hot charcoal. The condensed liquid contains S in solution, and other impurities. Purification. Agitation with Ca(OH)2, litharge, mercury, mer- curic chloride, or copper sulphate, and distilling the decanted liquid with a bland fixed oil or beeswax, and rectifying repeatedly in a water-bath. Used as a solvent for fats, essential oils, rubber, etc. Description. Clear, colorless, highly refractive, very diffusive liquid; strong, characteristic odor; sharp, aromatic taste; neutral reaction; insol. water, sol. in ale., ether, chloroform, fixed and volatile oils. Sp. gr. 1.272. Vaporizes at ordinary temperatures; highly inflammable, burns with blue flame. Impurities and tests. Sulphurous acid: -f- blue litmus paper = red color. Sulphur: -|- evap. spontaneously = residue. Hydrogen sulphide: -f- lead acetate (sol.) = black ppt. 114 MANUAL OF PHARMACY. PHOSPHORUS. Occurrence. This non-metallic element exists as phosphates in all plants and animals. Preparation. Calcined bones containing calcium phosphate are treated with H2S04, thereby converting the salt into acid calcium phosphate, while CaS04 is also formed, thus: Ca3(P04)2 + 2H2S04 = CaH4(P04)a + 2CaS04. / Calcium \ /SulphuricN /Acid Calcium\ / Calcium \ VPhosphate./ V Acid. ) \ Phosphate. J 'Sulphate.; The solution of the acid phosphate is evaporated to dryness, after having added charcoal, and the residue distilled in a stoneware re- tort. The distilled P is condensed under water and run into tubes, and congealed. Reaction. 3CaH4(P04)2 + 16C = Ca3(P04)2 + 2Pa /"Acid Calcium \ (Carbon.) ( Calcium \ (Phosphorus.) \ Phosphate. ) V Phosphate.; + 16C0 + 12H. / Carbon \ (Hydrogen.) .VMonoxide./ Description. Translucent, nearly colorless solid, of a waxy lustre; of about the consistency of beeswax at ordinary temperatures; dis- tinctive and disagreeable taste and odor (tbe latter due to ozone pro- duced by the decomposition of the air by P), melts at 111.2° F.— Sp. gr. 1.830 at 50° F.; insol. water; sol. in abs. ale. (350), abs. ether (80), fatty oils (50), CS2, chloroform. Emits white fumes on expos- ure to air, which are luminous in the dark, with an odor resembling that of garlic. On long exposure to air it takes tire spontaneously. Should be kept under water in a moderately cool, dark place. Impurities. Arsenic (due to the II2S04 used in making it being made from iron pyrites) and sulphur. Dose: to grain. Officinal Preparations. 1. Acidum phosphoricum. 2. Oleum phos- phoratum. 3. Pilulae plxosphori. Amorphous Phosphorus, or red phosphorus. Made by heating ordinary or vitreous phosphorus for a long time to near its boiling point, in an atmosphere of C02. Non-luminous and ron-poisonous. Oxides of Phosphorus. Hypophosphorus oxide (P'20) producing hypophosphorous acid (II3P02) mono-basic; phosphorous oxide (P'"203), yielding phosphorous acid (H3P03) di-basic; and phosphoric oxide (Pv205) the source of orthophosphoric acid (H3P04), tribasic. Meta- phosphoric acid is derived by taking one molecule of H20 from phosphoric acid, thus: 113P04 less H20 = HP03; pyrophosphoric acid by removing from two molecules of phosphoric acid, one of water, thus: 2H3P04 less H20 = H4P207. Phosphorous acid and phosphites are rarely, if ever, employed in pharmacy. (H3PO4) Acidum Phosphoricum.—Phosphoric Acid. Preparation. Phosphorus in small pieces is added to a mixture of equal weights of IIN03 and water, and the mixture gradually heated until reaction commences, the heat being regulated in order PHOSPHORUS. 115 to keep the reaction under control. When the phosphorus is en tirely dissolved, the excess of HN03 is driven off by heating till an odorless, syrupy liquid remains, and on cooling diluted with water to the proper degree of strength. The phosphorus is oxidized by the nitric acid, and with the water forms phosphoric acid. 6P2 + 20HNO3 + 8H20 = 12H3P04 + 10N2O2. (Phosphorus.) /NitricX (Water.) /Phosphoric\ /Nitrogen \ \ Acid. / \ Acid. ) \ Dioxide./ Description.—Colorless, odorless liquid, of a strong acid taste and reaction; sp. gr. 1.347; contains 50$ orthophosphoric acid, and 50$ water. When heated loses water, and at 392°F. gradually be- comes converted into pyro- and meta-phosphoric acids, which may be volatized at a red heat. If the acid is saturated with NH4OH, the addition of test mixture of magnesium gives a white, crystalline precipitate; this precipitate dissolved in dil. acetic acid yields a yellow precipitate with AgNOs. Impurities and tests. Phosphorous acid: Dil. acid -j- AgN03 = blk.; or -f- HgCl2 = whitish ppt. Arsenic acid: Heat to 158°F. -J- H2S, and cool = lemon yellow ppt. Nitric acid: -|- FeS04 and H2S04 = brown or reddish zone. /Sulphuric acid: -)- BaCl2 = white ppt. Hydrochloric acid: AgN03 = white ppt. Meta- or Pyro-phosphoric acid: -f- tincture chloride of iron = ppt. after several hours. The impurities nitric, phosphorous and arsenic acids may be re- moved in the following manner: Nitric Acid: Evaporate till no reaction for nitric acid can be obtained, cool, and replace the loss of water. Phosphorous Acid: Add nitric acid and distilled water and evaporate till no reaction for phosphorous or nitric acids can be obtained; restore original weight with water. 3H3P03 -f- 2HN03 = 3H3P04 4- H20 -f- N202. Arsenic Acid: Dilute, heat to 158°F. and pass H2S into it for one half-hour; remove the heat, and con- tinue passing the gas into the liquid until cold; filter, heat to drive off excess of H2S, filter and evaporate to proper degree of strength. Tests for: Solution Albumen. BaCla CaClj AgNOs Metaphosphoric Acid. White ppt. White ppt. White ppt. Transparent gelatinous ppt. Pyrophosphoric Acid No reaction. No reaction. No reaction. White ppt. Orthophosphoric Acid. No reaction. No reaction. No reaction. Yellow ppt. Sol. in NH4OH. Reagent. Officinal Preparations. Acidum Phosphoricum Dilutum.— Diluted Phosphoric Acid.—Phosphoric acid (20) water (80)—Sp. gr. 1.057—contains 10$ orthophosphoric acid. Should be tested for the impurities common to the stronger acid. Unless free from pyro- phosphoric acid, a gelatinous precipitate results on adding to tinc- ture of chloride of iron. Oleum Phosphoratum.—Phosphorated Oil. Made by dis- 116 MANUAL OF PHARMACY. solving 1% P. in expressed almond oil. The expressed oil of almond is first heated to 482°F., cooled, and filtered, for the purpose of removing air and moisture, also certain organic matters are volatil- ized or destroyed, the oil becoming nearly colorless, separating a little flocculent matter which is removed by filtration. The P. is dissolved by the aid of heat, and on cooling, stronger ether (9) is added to prevent phosphorescence in the dark. Pilulas Phosphori.—Pills of Phosphorus. A solution of P. in chloroform is added to a mixture of powdered althaea and acacia, and the mass completed with glycerin and water; after rolling the pills, they are coated with a solution of tolu in ether, to protect them from moisture and oxidation. Chloroform used as a solvent here, because it is non-inflammable, while its vapor prevents oxida- tion of P. Tgr. P. in each pill. Dose, 1-2 pills. (Na2HP04.12H20—358) Sodii Phosphas.—Phosphate of So- dium. Preparation. Bone-ash (calcined bones) is treated with H2S04 as in the preparation of phosphorus (see page 114), and the heated solution of acid calcium phosphate, freed from the precipitated CaS04, treated with Na2C03; mono-calcic phosphate precipitates, C02 is given off, and sodium phosphate is in solution; the filtered liquid is evaporated to crystallization. Reaction. CaH4(P04)2 + Na2C03 = Na2HP04 /Acid CalciumX / Sodium \ / Di-sodic \ \ Phosphate. ) \Carbonate./ /Phosphate./ + CaIIP04 + C02 + H20. /Mono calcic \ /Carbon \ (Water.) V Phosphate. / VDioxide./ Description.—Large, colorless, transparent crystals; very efflores- cent ; odorless; cooling, saline and feebly alkaline taste, and a slightly alkaline reaction; sol. in water (6), insol. alcohol. Impurities and tests. Carbonate: -|- acid = effervescence. Metals: 4- H2S or (NH4)2S = ppt. Sulphate: -(- HN03 Ba (N03)2 = ppt. Chloride: -|- IIN03 -f- AgNOa = ppt. (Na4P2O7.10H2O—446) Sodii Pyrophosphas.—(Pyrophosphate of Sodium.) Made by heating sodium phosphate to dull redness, until its solu- tion gives a white precipitate, free from yellow tint, with AgN03t dissolve and crystallize. Reaction. 2Na2HP04 + Heat = Na4P207 -j- H20. / Di-sodic \ ( Sodium \ (Water.) VPhosphate./ \Pyrophosphate. / Description.—Colorless, translucent prisms; odorless; sweetish, saline and mildly alkaline taste; feeble acid reaction; sol. in water (12), insol. alcohol. Impurities and tests, same as under Sodii Phosphas. (CaH4(P02)2—170) Calcii Hyfophosphis.—Hypophosphite of Calcium. Made by boiling P. with milk of lime ; phospkoretted hydrogen PHOSPHORUS, 117 is evolved, and the solution containing calcium hypophosphite is evaporated to crystallization. 3Ca(OH)2 -f 4P2 + 6H20 = 3CaH4(P02)2 + 2PH3. ( Calcium \ (Phosphorus.) (Water.) / Calcium \ (PhosphorettedN VHydroxide.) VHypophosphiteJ V Hydrogen. ) Description. Colorless, or white crystals, or in scales of a pearly lustre ; odorless ; nauseous, bitter taste ; neutral reaction ; soluble in water (6.8), insol. alcohol. Test for Hypophosphites. 1. When heated they give off water, then evolve spontaneously inflammable PH3. 2. Mercury is precipi- tated on adding a solution of mercuric chloride. 3. An acid solu- tion of potassium permanganate is decolorized. Impurities and tests. Insoluble calcium salts: Should be entirely soluble in water. Soluble phosphates: -f- Lead acetate = ppt., or -|- BaCl2 = ppt. Magnesium: See test under Calcium Salts. Officinal Preparation. Syrupus IIyfophosfhitum. (Syrup of Hypophosphites). Contains the hypophosphites calcium, sodium and potassium; citric acid, sugar, and water—flavored with spirit of lemon. Dose, | to 1 fluidraelim. Officinal Preparation. Syrupus Hyfophosphitum cum Ferro. (Syrup of Hypophosphites with Iron.) Made by dissolving lactate of iron (1) in syrup of hypophosphites (100) by trituration. Dose i to 1 fluidrachm. (NaH2P02.H20—106) Sodii Hypophosphis.—Hypophosphite op • Sodium. Made by double decomposition of sodium carbonate and calcium hypophosphite: calcium carbonate precipitates, while sodium hy- pophosphite is in solution, and is obtained by evaporation at a low temperature, and crystallization. CaII4(P02)2 -f- Na2C03 = 2NaH2P02 -f- CaC03. ( Calcium \ ( Sodium \ / Sodium \ ( Calcium \ VHypophosphite.) (Carbonate./ VHypophosphite.) (Carbonate./ Description. Small, colorless, or white, rectangular plates, or a white, granular powder; deliquescent; odorless; sweetish, saline taste, and neutral reaction. Sol. in water (1), alcohol (30). On trit- urating or heating with an oxidizing agent, the mixture explodes. Impurities and tests. Carbonate: -f- Acid = effervescence. Cal- cium : -j- (NH4)2C204 = white ppt. Potassium: -f- NaHC4H4Oa = ppt. Sulphate: 4- BaCl2 = ppt. Phosphate (a limit): test s°l- magnesium = white ppt. (KH2P02—104) Potassii Hypophosphis.—Hypophosphite op Potassium. Made similar to sodium hypophosphite, by substituting K2C03 for Na2C03 in the preceding process. Description. White, opaque, confused—crystalline masses, or a white, granular powder ; very deliquescent; odorless ; sharp, sa- line, bitterish taste; neutral reaction; sol. in water.(0.6), ale. (7.3). Impurities ; same as under Sodium Hypophosphite. 118 MANUAL OF PHARMACY. Hypophospiiorous Acid (H3P02). Not officinal. Used as a solvent for liypophosphites. Made by the action of oxalic acid on calcium hypophosphite in solution. Reaction. CaH4(P02)2 -f- H2C204 = CaC204 4- 2H3P02. / Calcium \ /Oxalic \ /CalciunA / Hy pophosphorous\ VHypophosphlte. J V Acid. / \OxalateJ V Acid. / FERRUM.—(FE.—55.9) Ferri Chloridum. Fe2CI? (grs. i-v.) Liquor—S. G. 1 (TTJ,. i-v, in syrup.) I Liq Fe2CI6 33 1 Tincturas Alcohol, 65 Wcg/.s.x-xxx) ( Mix. 100 ’ Mistura Ferri et Ammonii Acet. f \ ss-i.) Ferri Iodidum Sacch. 20% Fe I2(grs. ii-v.) Syr. Ferri Iodidi, 10$ Fel2 (gtts. x-xl.) Syr. Ferri Bromidi, 10$ FeBr2 (gtts. x-xl.) Ferri Lactas, Fe(C3H503'2 (1 gr. up- toards.) Syr Hypophos. cum Ferro (f 3 i-ii.) Ferri Sulphas, FeS04.7H20 (grs. i-ii.) Ferri Sulphas, FeS04.7H20. Ferri Sulphas Exsiccatus, FeS04.H20. Pil. Aloe et Ferri—(grs. v-xv.) Ferri Sulphas Praecipitatus. FeS04 7H20. Mistura Ferri Comp—£ 3 ss-iss.) Liq. Ferri Subsulphatis, Fe40 (S04)6 S. G. I®51 (grs. v-xv.) Ferri Carbonas Sacch. 15$ FeC03. (grs. v. upwards.) Massa Ferri Carbonatis (grs. iii-v.) Pilulae Ferri Comp.—(pH. ii-vi.) Ferri Oxalas, FeC204—(grs. ii-iii.) Liq. Ferri Tersulph. Fe2(S04)3—S. G. 1 122. Liquor Ferri Tersulphatis,‘Fe2(S04)3. Ferri Oxidum Hydratum, Fe2(OH)6. Ferrum Reduct, um—(grs. iii-v.) Pil. Ferri Iodidi—(grs. iii-viii ) Emplastrum Ferri—10$ Fe2fOH)6. Troehisci Ferri—5$ Fe2(OH)6 (i-vi.) Ferri Oxidum Hydratum cum Magne- sia. Ferri et Ammon. Sulph Fe2(NH4)2 (S04)4 24H20 (grs. v-xv.) Ferri et Ammon. Tartras (grs. x-xxx.) Ferri et Potassii Tartras (grs. x-xxx.) Ferri Hypophosphis, Fe2(H2P02')g (grs. iv-xii.) Liq. Ferri Nitratis, Fe2(N03)g S. G. 1 afii contains 6$ salt (gtts. vii-viii.) Liq. Ferri Acetatis, Fe2(C2H302)6— S. G. (TTLii-vi.) Tinctura—(gtts. xx-£ 3 id Ferri Valerianas, Fe2(C6H902)g. (1 gr. upwards.) Liq Ferri Citratis, Fe2(C6H507)2 S. G. J .262 (grs. V-XX.) Ferri et Ammon. Citras (grs. v up- tvards.) Vinum Ferri Citratis—(f 3 i.) Liq. Ferri et j 6$ Quinine. Quin. Cit. i Dose: Vinum Ferri Amarum (f 3 ii-iv.) Ferriet Strych. j 1$ Strychnine. Citras. i Dose: (grs. iii-v.> Ferri Citras, Fe2(C6H507)26H20 (grs. v.) Ferri et Quini- J 12$ Quinine nae Citras f (grs v-vi.) Ferri Phosphas, Fe2(P04)2 (grs. v-x.) Syr. Ferri et Quin, et Strych. Phos. (f 3 i.) Ferri Pyrophosphas, Fe4(P207)3 (grs. ii-v.) Ferrum—Iron. Metallic iron in the form of fine, bright and non elastic wire. Card teeth, represents iron in one of its purest forms, and is ex- tensively employed in the manufacture of its preparations. Tests for Iron Salts. 1. Ferric salts with potassium ferro- cyanide produce a deep blue color (Prussian Blue) at once; ferrous salts yield a bluish white precipitate gradually changing to a pale 119 THE IRON SALTS. blue. 2. Ferrous salts give a deep blue color (Turnbull’s Blue) with potassium ferricyanide; ferric salts strike a greenish or olive color. 3. Water of ammonia with ferrous salts gives a white precipitate of ferrous hydroxide, gradually becoming green, then black and brown; with ferric salts, a brown precipitate of ferric hydroxide re- sults. 4. Ammonium sulphide give a black precipitate with iron salts. 5. Sulphocyanide of potassium strikes a blood-red color with ferric salts. 6. With ferric salts, tannic acid produces a greenish black precipitate (.ink); no reaction with ferrous salts, that have not been oxidized. (Fe2Cl6.12H20—540.2) Ferri Chloridum.—Chloride of Iron. (Ferric Chloride. Sesqui chloride of Iron.) Made by treating iron wire with dilute HC1, allowing the mixture to stand till effervescence ceases, boiling and filtering, thus producing a solution of ferrous chloride (FeCl2), hydrogen being evolved. Reaction. Fe -j- 2HC1 = FeCl2 -t~ 2H. (Iron.) /HydrochloricN / Ferrous \ (Hydrogen.) ( Acid. ) (Chloride.) The ferrous chloride is oxidized to ferric chloride by adding more HC1, and pouring into HN03. 6FeCl2 + 6IIC1 + 2HN03 = 3Fe2Cl, + NaOa + 4H20. I Ferrous \ /Hydrochloric\ /Nitric\ / Ferric \ /NltrogenN (Water.) (.Chloride.) \ Acid. ) ( Acid.) (Chloride.) (Dioxide.) The nitric oxide vapors are driven off by heat, and the solution tested for ferrous salt with ferricyanide of potassium; if a blue color results, HN03 is added and the excess evaporated off as before. An excess of HC1 is added and the solution set aside till a solid crystal- line mass is obtained. Description. Orange yellow crystalline pieces; very deliquescent; odorless, or faint odor of HC1; styptic taste; freely soluble in water, ale. and ether. Impurities and tests. Nitric acid: -)- FeS04 H2S04 = brown zone. Ferrous chloride: -)- potass, ferricyanide = blue color. Oxy- chloride : 1% sol. in water -j- boil = cloudiness. Liquor Ferri Chloridi.—Solution of Ferric Chloride. (Solution Sesqui chloride of Iron.) Made by the process used for Ferri Chloridum, retaining the salt in the form of a solution. Description. Reddish-Drown liquid; faint odor of HC1; acid styptic taste; acid reaction. Sp. gr. 1.405 —contains 87.8$ of anhy- drous Fe2Cl6, and some free HC1. If red brown ppt. forms in this solution, add a few drops of HC1 and heat. If colored black, add few drops of HN03 and heat to the boiling point. Impurities and tests, same as given under Ferri Chloridum. Officinal Preparation. Tinctura Ferri Chloridi. (Tincture of Chloride of Iron.) Contains solution chloride of iron (35), and alcohol (65). Mix, and let stand for three months. During that time several ethereal compounds are produced by the action of the 120 MANUAL OF PHARMACY. chloride and free HC1 on the alcohol. A red brown ppt. in this pre- paration denotes a deficiency of HC1; this ppt. is very slowly dissolved on adding HC1. Officinal Preparation. Mistura Ferri et Ammonii Acetatis. (Mixture of Acetate of Iron and Ammonium. Basham’s Mixture.) Contains tinct. chloride iron (2), dil. acetic acid (3), solution ammo- nium acetate (20), (slightly acid to prevent formation of carbonate of iron) elixir of orange (10), syrup (15),water (50). Ferri Iodidum Saccharatum. (Saccharated Iodide of Iron.) Iodine (17) and iron (6), are combined in the presence of water, forming a green solution of ferrous iodide, which when it has lost its •odor of iodine is filtered into a capsule containing sugar of milk (40); •evaporate the mixture to dryness, add sugar of milk (40) and powder. Description. Yellowish-white, or grayish powder; very hygro- scopic; odorless; sweet ferruginous taste; slightly acid reaction; soluble in water, partially soluble in alcohol. Contains at least 20$ of ferrous iodide (FeI-2), determined by volumetric solution of AgN03. Impurity. Free iodine: -j- starch jelly = blue color. Syrtjptjs Ferri Iodidi. (Syrup of Iodide of Iron.) A solution of ferrous iodide made as above, is filtered upon sugar, which is disolved in it by the aid of heat, and the finished syrup kept in a place accessible to sunlight. The reaction between iodine and iron is feeble at first, but on the formation of a small quantity of Fel2, the latter acts as a solvent for more iodine, which combines with the iron so rapidly as to cause a brisk reaction If violet vapors are given off, the reaction should be somewhat retarded to prevent loss of iodine. Description. Transparent, pale-green syrupy liquid; ferruginous taste; neutral reaction; contains 10# ferrous iodide (Fel2), estimated by volumetric solution AgN03. Syrupus Ferri Bromidi. (Strep of Bromide of Iron.) Made in the same manner as syrup of iodide of iron, substituting Br. for I. Resembles syrup of iodide of iron, and contains 10$ ferrous bromide (FeBr2). (Fe (CsHsOa^.SHaO—287.9) Ferri Lactas. Lactate of Iron. (Ferrous Lactate.) Made by the double decomposition between calcium lactate and ferrous sulphate in solution. Reaction. -f- FeSOi — CaSCK -l- Fe(C3H503)2. / Ferrous \ /Calcium \ /Ferrous \ VLactate./ VSulphate./ \Sulphate./ V Lactate, j Also made by the action of diluted lactic acid on iron, and the subsequent evaporation of the solution to crystallization. Reaction. Fe 2HC3H5O3 — Fe(C3H603)2 -f- Ha. (Iron.) (Lactic Acid.) /Ferrous\ (Hydrogen.) V Lactate./ THE IRON SALTS. 121 Description. Pale, greenish-white crystalline crusts or grains; odorless ; sweet, ferruginous taste ; feeble acid reaction ; soluble in water, and solution of sodium citrate, aim. ins. alcohol. Impurities and tests. Sulphate, tartrate, citrate (a limit of each): -j- lead acetate = white cloudiness. Officinal Preparation. Syr. Hypophosphitum cum Ferro. (FeS04.7H20—277.9) Ferri Sulphas.—Sulphate of Iron. (Ferrous Sulphate.) Made by the action of diluted II2S04 on iron ; evaporating and crystallizing. The commercial copperas, or green vitriol, is obtained by the use of an impure H2S04, obtained during the purification of kerosene and other petroleum hydrocarbons, but for pharmaceuti- cal purposes a pure H2S04 should be employed. Reaction. Fe -|- H2S04 = FeS04 + H2. (Iron.) /Sulphuric ; / Ferrous \ (Hydrogen.) \ Acid. ) (Sulphate./ Description. Large, bluish-green, monoclinic prisms; efflores- cent and absorbing oxygen on exposure to air; odorless; saline, styptic taste ; acid reaction ; sol. in water (1.8), ins. alcohol. Impurities and tests. Copper: -f- II2S04 -{- II2S = colored ppt. Ferric salt: + H2S04 + II2S = white turbidity. Officinal Preparations. 1. Ferri sulphas exsiccatus. 2. Ferri sulphas prsecipitatus. % of anhydrous Fe2(N03)6. Liquor Ferri Acetatis. — Solution of Acetate of Iron. (Solution of Ferric Acetate.) Prepare Fe2(OH)«, and after removing water by powerful expres- sion, dissolve in glacial acetic acid. Beaction. Fe2(OH)B -f- 6HC2H3O2 = Fe2(C2H302)6 + 6H20. ( Ferric \ /AceticV ( Ferric \ (Water.) VHydroxide.) \ Acid. / VAcetate./ Description. Dark, red-brown, transparent liquid; sp. gr. 1.160; contains 33$ anhydrous Fe2(C2H302)8; acetous odor; sweetish, styptic taste; acid reaction. 126 MANUAL OF PHARMACY. Impurities and tests. Zinc: Precip. iron from sol.: flit. -{- H2S = white ppt. Fixed Alkalies: Precip. iron by NH4OH; tilt. —(- evap. -f ignition = residue. Officinal Preparation. Tinctura Ferri Acetatis. (Tinct. Ferric Acetate.) Solution acetate of iron (50), add to a mixture of alcohol (30) and acetic ether (20). Sp. gr. 0.950. Liable to decompose, giving a red-brown ppt. insol. in acetic acid. Fe2(C6H902)6—717.8) Ferri Valertanas.—Valerianate of Iron. (Ferric Valerianate.) Made by double decomposition, employing solutions of ferric sul- phate and sodium valerianate; the iron salt precipitating, with sodium sulphate in solution. 6NaC5H902 + Fe2(S04)3 = 3Na2S04 + Fe2(C5H902)6. / Sodium \ / Ferric \ / Sodium \ l Ferric \ (Valerianate.) ' Sulphate./ (Sulphate./ (Valerianate./ Description. D&ik, tile-red, amorph. powder; faint odor of valerianic acid; mildly, styptic taste; insol. in water, sol. in alcohol; decomposed by boiling water, setting free valerianic acid, leaving Fe2(OH)6. Rarely used in pharmacy. Liquor Ferri Citratis.—Solution of Citrate of Iron. (Solution of Ferric Citrate.) Freshly prepared Fe2(OH)8 is dissolved by the addition of citric acid crystals heating to 140° F.; the liquid is filtered and concen- trated by evaporation. Reaction. Fe2(OH)6 -{- 2H3C6H6O7 = -(- 6H20- ( Ferric \ /Citric, I Ferric \ (Water.) (Hydroxide.) (Acid./ (Citrate./ Description. Dark-brown liquid; odorless; slight ferruginous taste; acid reaction. Sp. gr. 1.260; contains about 35.5$ anhydrous 60)7)3 • Impurity (or adulteration). Tartaric acid: -(- HC1 -f- cone. sol. potass, acetate = cryst. ppt. Officinal Preparations. 1. Ferri et Ammonii Citras. 2. Ferri Citras. The Scale Salts of Iron, and their Officinal Preparations. The interesting and popular compounds comprising the Scale Salts (so-called on account of their appearance), may properly be con- sidered as a class, from the fact that the general processes of manu- facture are somewhat similar. They are eight in number, viz.: 1. Ferri et ammonii tartras; 2. Ferri et potassii tartras; 3. Ferri citras: 4. Ferri et ammonii citras; 5. Ferri et quininse citras; 6. Ferri et strychnin® citras; 7. Ferri phosphas; 8. Ferri pyrophosphas. Characteristics. The two last occur in bright green scales, while the others are garnet-red, or yellow-brown. With but two exceptions, they are all compound salts, having present besides the iron salt, some alkali salt of citric or tartaric acid which has the property of increasing their solubility; the exceptions are Ferri citras, 127 THE IRON SALTS. and Ferri et quininae citras, these are very slowly soluble, while the others are very soluble in water, and are deliquescent. Preparation. Solution of tersulphateof iron is really the starting- point with each salt, the former being the source of the ferric hydroxide, which is employed in its freshly precipitated state for subsequent solu- tion. After obtaining the desired salt in solution, the latter is evap- orated at a temperature below 140° F. {to prevent conversion to ferrous compounds) to a syrupy consistence, and spread on plates of glass so that when dry, the salt may be obtained in scales. Failure in scaling is usually due to the incomplete saturation of the acid with ferric hy- droxide, or to the presence of sulphates in the imperfectly w ashed hydroxide. Ferri et Ammonii Tartras.—Tartrate of Iron and Ammonium. (Ammonio-ferric Tartrate.) After preparing ferric hydroxide, it is dissolved in a solution of acid tartrate of ammonium (made by neutralizing tartaric acid with ammonium carbonate and adding another equivalent of tartaric acid), and scaled by the usual method. The possible composition of the double salt may be shown by the following reaction: Fe2(OH)6 -j- 6]STH4HC4H406 = Fe2(NH4)6(C4H406)6 -t- 6EUO. / Ferric \ /Acid Ammonium\ /Ammonio-ferric \ (Water.) V Hydroxide./ \ Tartrate. / \ Tartrate. / Description. Transparent, garnet-red, or yellow-brown scales; slightly deliquescent; odorless; sweet, ferruginous taste; neutral re- action; very sol. in water, insol. alcohol. When deprived of iron by boiling with an excess of solution of potash,* a white crystalline pre- cipitate of potassium bitartrate will be produced on supersaturating the concentrated and cooled filtrate w7ith acetic acid. Impurities. Fixed alkalies: -f- incineration = residue having alka- line reaction. Ferri et Potassii Tartras. Tartrate of Iron and Potassium. (Potassio-ferric Tartrate.) Made by dissolving potassium bitartrate in a mixture of freshly- prepared ferric hydroxide and water by the aid of heat; a small amount of NH,OH is added to produce a perfectly and readily solu- ble salt, scaled by the usual method. Pe2(OH), + 6KHC4H406 = Fe2K6(C4H406)6 + 6H20. / Ferric \ l Potassium \ /Potassioferric \ (Water.) VHydroxideJ V Bi tartrate./ \ Tartrate. ) Description. Properties, solvents, etc., resemble tartrate of iron and ammonium. Ferri et Ammonii Citras.—Citrate of Iron and Ammonium. (Ammonio-ferric Citrate.) Made by adding NH4OII to a solution of citrate of iron, and scal- ing by usual method. * Note.—'The text of the U. S. P. states solution of soda, which is doubtless an error. 128 MANUAL OF PHARMACY. In composition, it is probably a mixture of ammonio-ferric citrate with ferric oxycitrate. Description. Transparent, garnet-red scales; deliquescent on ex posure to damp air; odorless; saline, mild ferruginous taste; neutral reaction; sol. in water, insol. alcohol. Impurities. Fixed alkalies: -f- incineration = ash with alkaline re- action. Officinal Preparations. 1. Vinum ferri citratis; 2. Liquor ferri et quininae citratis; 3. Ferri et strychnin® citras. Contains ammonio-ferric citrate (4), tincture of sweet orange-peel (12), syrup (12), and stronger white wine (72). Liquor Ferri et Quinine Citratis.—Solution of Citrate of Iron and Quinine. Vinum Ferri Citratis.—Wine of Citrate of Iron. Made by adding to a solution of citrate of iron and ammonium, citric acid and quinine, concentrating and adding alcohol. Description. Dark, greenish-yellow liquid; transparent in thin layers; odorless; bitter, mildly ferruginous taste; slight acid reaction. Contains 6% quinine. Reaction. On supersaturating the diluted solution with a slight excess of NH4OH the color deepens and a white curdy precipitate deposits, soluble in ether and answering to the reaction of quinine. Assay. To 8 grams of solution, add wrater ft. 80 cm3; introduce it into a glass separator, add a solution of 0.5 grams tartaric acid, then NaOH in excess. Extract the alkaloid by agitation with four successive portions of chloroform, each of 15 cm3. Separate the chloroformic layers, mix them, evaporate and dry residue at 212° F.; it should weigh 0.48 grams. Explanation. The tartaric acid combining with the soda produces a tartrate of soda which holds the iron in solution, while the excess of soda solution precipitates the quinine, for which chloroform is a ready solvent, not mixing with the watery liquid. Officinal Preparations. Vintjm Ferri Amarum (Bitter Wine of Iron). Contains solution of citrate of iron and quinine (8); tincture of sweet orange-peel (12), syrup (86), and stronger white wine (44). Each drachm contains nearly one grain of citrate of iron and quin. Ferri et Strychnine Citras. (Citrate of Iron and Strychnine.) Preparation. Strychnine dissolved in water with the aid of citric acid (thus producing citrate of strychnine) is added to a solution of citrate of iron and ammonium, and scaled by the usual method. Description Similar to ammonio-ferric citrate, except that it has a bitter taste and produces a white precipitate with NH4OH. Con tains 1% of strychnine. Assay. Dissolve one gram of the salt in 4 cm3 water in a test tube; add one cm3 of liquor potassa, and shake with chloroform; the residue left on evaporating the cliloroformic layer will answer to the reaction for strychnine, and weigh about 0 01 gram. THE IKON SALTS. 129 (Fe2(C6Hs07)2.6H20—597.8) Ferri Citras.—Citrate of Iron. (Ferric Citrate.) Made by evaporating the officinal solution of citrate of iron, and scaling by the usual method. Description. Transparent, garnet red scales; not deliquescent; odorless; faint ferruginous taste; acid reaction; very slowly sol. in cold water but readily in boiling water, insol. in alcohol. Impurities and tests. Fixed alkalies: -|- incineration = ash with alkaline reaction. Tartaric acid (adulteration): acidulate with HC1; -}- KC2H302 = white ppt. Officinal Preparations.—Ferri et Quininje Citras (Citrate of Iron and Quinine). Made by dissolving citrate of iron in wa- ter below 140° F., and dissolving quinine in the solution; subse- quently evaporating and scaling. No definite compound is formed, the quinine not entering into any chemical combination with the iron salt. Description. Transparent, odorless, thin scales; varying in color from red-brown to yellow-brown; slowly deliquescent; bitter ferruginous taste; acid reaction; slowly but wholly soluble in cold water, more readily so in hot water, insol. in alcohol. Contains 12$ of dry quinine. Assay process, same as for solution of citrate of iron and quinine, except that the same result is derived by the use of one half as much salt as the required amount of solution. Remarks. The above salt on account of its exceedingly slow solubility in cold water, is a very undesirable preparation for the use of pharmacists except when desired in* pill form, and conse- quently but little used. Citrate of Iron and Quinine, containing 10$ of quinine, is a better preparation. It contains a small amount of ammonium citrate, which renders the salt exceedingly soluble and of a greenish, golden- yellow color. A soluble non-oflicinal scale salt, extensively used; containing quinine 10$, strychnine 1$. Color same as the soluble citrate of iron and quinine. Citrate of Iron, Quinine and Strychnine. Ferri Phosphas.—Phosphate of Iron. (Ferric Phosphate.) Preparation. Citrate of iron is dissolved in water by the aid of heat, and sodium phosphate dissolved in the solution, which is evaporated and scaled. Ferric phosphate and acid citrate of sodium are formed, the latter acting as a solvent for the former. Reaction. 2Na2HP04 -j- Fe2(C6H607)2 + 6H20 / Disodic \ V Ferric \ (Water.) VPhosphate.) VCitrate. / = Fe2(P04)2, 2Na2H(C6H507), 6H20. ( Ferric \ /Acid SodiumN (Water.) VPhosphate.) V Citrate. ) The name of this preparation gives no idea as to its composition, ferric phosphate being a white, amorphous, insoluble powder. A 130 MANUAL OF PHARMACY. better name for the officinal salt might be one of the following, viz.: citro-sodic ferric-phosphate, sodio-ferric citro-phosphate, or, soluble ferric phosphate. Description. Thin, bright green, transparent scales, turning dark on exposure to light; odorless; saline taste; slight acid re- action; sol. in water, insol. alcohol. Officinal Preparations. Syrupus Ferri, Quininse et Strychnin* Phospliatum. (Syrup of phosphate of iron, quinine and strychnine. Eaton’s Syrup.) Contains phosphate of iron (1.33) quinine (1.33) strychnine (.04) phosphoric acid (8) sugar (60) and water ft. 100. Ferri Pyrophosphas.—Pyrophosphate of Iron. (Ferric Pyrophosphate.) Made by dissolving sodium pyrophosphate in a solution of citrate of irorf, evaporating and scaling. Reaction. 3Na4P2C>7 -|- 2Fe2(C6Hs07)2 -f- I2H2O / Sodium \ ( Ferric \ (Water.) VPyrophosphate./ VCitrate./ = Fei(P20,)3.4Na3C6H50, . 12H20. r Ferric \ /Sodium \ (Water.) VPyrophosphate./ VCitrate./ This salt like the phosphate is incorrectly named, pyrophosphate of iron being an insoluble white salt, the sodium citrate acting as its solvent. A better name would be soluble pyrophosphate of. iron; or, sodio-ferric citro-pyropliosphate. Description. Reactions, and its behavior to solvents, are identical with phosphate of iron, with the following exception: Test to distinguish from phosphate. Remove the iron from a solution of the salt by boiling with KOH (in excess); ferric hydroxide pre- cipitates; supersaturate the filtrate with acetic acid, and add solu- tion of silver nitrate,—result a white ppt.\ under similar conditions the phosphate gives a yellow ppt. Dialysed Iron. (Unofficinal.) Made by treating solution of ferric chloride with water of am- monia, and dissolving the precipitated magma in solution of ferric chloride; by placing the mixture on a dialysator and subjecting to dialysis, it is freed from ammonium chloride and any free HC1 that may be present, a solution of oxychloride of iron remaining, the latter is diluted with water to the sp. gr. 1.047. Description. A dark-brown liquid, transparent in thin layers; permanent; odorless; tasteless, or slightly acid taste; slightly acid reaction; miscible with water and alcohol in all proportions. MANGANUM. Manganese. (Mn.—54.) Occurrence. Found in Nature as an impure oxide; or, in com- bination' with iron, calcium, silica, baryta, zinc, etc., as pyrolusite, braunnite, franklinite, and manganite. Tests for Manganese salts in solution: 1. Ammonium sulphide solution produces a flesh-colored precipitate (MnS) soluble in acetic THE MANGANESE SALTS. 131 acid. 2. Water of ammonia yields a white precipitate (Mn(OII)2) changing to brown. (Mn02—86) Mangani Oxidum Nigrum.— Black Oxide of Manganese. (Di- or Per-oxide of Manganese.) Native crude binoxide of manganese, containing at least 66# of the pure oxide. Description. Heavy, grayish-black, gritty powder; odorless; tasteless; insol. in water, or ale. Oxygen is evolved at a high heat, and in the presence of HC1 with heat, chlorine is given oft'. Used in the preparation of Aq. chlori. (MnS04.4H20—222) Mangani Sulphas.—Sulphate of Manganese. Preparation. Binoxide of manganese is heated with charcoal, converting it into a monoxide (MnO), then treated with strong H2S04, heated and evaporated to dryness, then heated to redness to decompose iron sulphate; the residue is dissolved in water, the solution filtered and crystallized. Description. Colorless, or pale rose-colored crystals; odorless; slightly bitter and astringent taste; faint acid reaction; sol. in water (0.7), insol. in alcohol. Impurities, to be tested for, are zinc, iron, copper, alkalies and magnesium. (K2Mn208—314) Potassii Permanganas.—Permanganate of Potassium. Made by fusing KOH with Mn02 and KC103. Reaction. 6K0H + 3Mn02 + KC103 = 3K2Mn04 / Potassium X /ManganeseX / PotassiumX f Potassium X V Hydroxide./ V Dioxide. / V Chlorate. / VManganate./ 4- KCl 4 3H20. I PotassiumX (Water.) V Chloride. / The resulting green mass is boiled in water to decompose the potassium manganate formed, yielding a purple solution containing potassium permanganate and KOH, while Mn02 is deposited. 3K2Mn04 + 2H20 = K2Mn208 + Mn02 + 4K0H. / Potassium \ (Water.) / Potassium \ (ManganeseX / Potassium X VManganate./ VPermanganate./ V Dioxide. ) V Hydroxide, j The KOH is neutralized by the addition of H2S04, Mn02 removed by filtration through asbestos, and on crystallizing the K2Mn208 is obtained, while KC1 and K2S04 remain in the mother liquor. Description. Deep, purple-violet, needle shaped rhombic prisms; unchangeable in air; neutral reaction; odorless; sweet, astringent taste; Sol. in water (20); decomposed by alcohol. When heated to redness, oxygen is given oil. The rose color of its solution is destroyed by the addition of organic substances, with the formation of a brown precipitate, soluble in dilute H2S04 forming a colorless liquid. On mixing a solution of the salt with glycerin, syrup, or other solutions 132 MANUAL OF PHARMACY. of organic matter in a closed vessel, a similar decomposition results followed by explosion. Impurities and test. Nitrate: Make colorless solution by addition of oxalic acid, and dil. H2S04 and treat with solution FeS04 in H2S04=brown zone. Chloride: The above colorless solution -f- AgN03 = white ppt. Sulphate (a limit allowed). Properties. Permanganate of potassium is a great disinfectant, deodorizer, and oxidizing agent, and hence should not be triturated nor combined in solution with organic or readily oxidizab/e substances. When desired in pill form the following excipients may be em- ployed with safety; vaseline, cocoa butter, kaolin, kaolin with resin cerate, etc. This salt is often used for purifying water, and rendering it palatable by adding the solution by drops until its color ceases to be destroyed. Other Salts of Manganese, (unofficinal) Iodide of manganese; occasionally employed in the form of a syrup, and the Hypophosphite in certain preparations of Syrup Hypophosphites Co. ARGENTUM. Silver. (Ag —107.7) Occurrence. Found native as silver glance (sulphide); horn-silver (chloride), and combined with lead in galena. Description. A brilliant, white metal; very ductile, and malle- able; Sp. gr. 10.5; soluble in HN03 forming silver nitrate, which is the starting-point of the other salts. Metallic silver is used in the form of silver leaf for coating pills. The salts are so easily decomposed and reduced to the metallic state, that their preservation in dark, amber-colored vials should be observed. Test for Silver salts. With hydrochloric acid a white precipitate of silver chloride results, soluble in NH4OH, and re-precipitated by HNOs. (AgN03—169.7) Argenti Nitras.—Nitrate of Silver. Made by dissolving silver in nitric acid, and crystallizing. Reaction. GAg -f 8HN03 = 6AgNOs -f- N202 -f- 4H20. (Silver.) /NitricN / Silver \ /Nitrogen\ (Water.) VAcid. / \ Nitrate.) \ Dioxide.) Description. Colorless, transparent crystals; becoming grayish- black on exposure to light in the presence of organic matter; sol. in water (0.8), alcohol (26). It has a very caustic action on the skin, and is a highly corrosive poison when taken internally. Dose. One eighth to one fourth grain. Antidote. NaCI, which produces an insoluble chloride. Impurities and tests Copper: -j- NH.OH = blue color. General foreign metallic impurities: Solution -f- HC1; filtrate + evap. = residue. Officinal Reparations. Argent! nitras dilutus. Argenti nitras fusus. THE SILVER SALTS. 133 Argenti Nitras Dilutus.—Mitigated Nitrate of Silver. . (Diluted Nitrate of Silver.) Made by melting together equal parts of AgNOs and KN03, casting into suitable moulds and cooling. Description. White, hard solid, in the form of pencils or cones. Argenti Nitras Fusus.—Moulded Nitrate of Silver. (Lunar Caustic.) Made by melting AgN03 (100) and adding HC1 (4), heating until nitrous vapors cease to be evolved, and casting into suitable moulds. The resulting product contains 5% of silver chloride, which renders it less fragile. Impurities and tests. Copper: 4- NH4OH = blue color. Possible adulterations. KN03 or other alkaline salts: On reducing to a fine powder with twice its weight of sugar and igniting, the ash produced will impart a saline or alkaline taste. (Ag20—231.4) Argenti Oxidum. (Oxide of Silver.) Made by precipitating a solution of silver nitrate with KOH, washing and drying the precipitate. Reaction. 2AgN03 + 2K0H = Ag20 + 2KN03 + H20. / Silver \ / Potassium \ /Silver \ / Potasslum\ (Water.) (Nitrate./ (Hydroxide./ (Oxide./ ( Nitrate. ) Description. Brown, or brownish black powder; feeble alkaline reaction; si. sol. in water, insol. in alcohol; when freshly prepared soluble in NH4OH, leaving a black powder called fulminating silver, which is violently explosive. Caution : Should hot be triturated with readily oxidizable or combustible substances, and should not be brought in contact with ammonia; hence the use of any saccharine substance as an excipient (when the oxide is desired in pill form) is not allowable. (AgCN—133.7) Argenti Cyanidum.—Cyanide of Silver. Made by passing HCN gas into a solution of silver nitrate, or by the double decomposition between KCN and AgNOs in solution; in either case AgCN precipitates, is washed and dried. Reactions. 1. HCN + AgN03 = AgCN + HN03. /Hydrocyanic\ ( Silver \ / Silver \ /Nitr1c\ ( Acid. ) (Nitrate./ (Cyanide./ (Acid./ 2. KCN + AgN03 = AgCN -f KN03. /Potassium \ ( Silver \ / Silver \ /Potassium \ ( Cyanide. / (Nitrate./ (Cyanide./ ( Nitrate. / Description. White powder, gradually becoming brown on exposure; odorless; tasteless; insol. in water and alcohol. Officinal Preparation. Diluted hydrocyanic acid. Made by precipitating a solution of AgN03 with KI. (Agl—234.3) Argenti Iodidum.—Iodide of Silver. Reaction. AgNOs -f- KI = Agl -(- KN03. / Sliver \ / Potassium \ ( Silver \ /Potassium \ \Nltrate.) \ Iodide. / (iodide./ ( Nitrate. / Description. Heavy, amorphous, light-yellow powder; odor- less; tasteless; insol. in water or alcohol. 134 MANUAL OF PHARMACY. CUPRUM.—Copper. (Cu—63.2) Occurrence: Found native on the borders of .uake Superior, also as an oxide, phosphate, arseniate, carbonate (malachite) and sul- phides {copper pyrites—Cu2S,Fe2S3). A brilliant metal of reddish color; sp. gr. 8.92; very ductile and malleable. Tests for Copper Compounds. 1. Water of ammonia produces an intense blue color with dilute solutions of copper salts, or a pale blue precipitate with cone, solutions. 2. Potassium ferrocyanide gives a red-brown precipitate. 3. II2S and (NH4)2S give black pre- cipitates. 4. If a piece of bright steel or zinc is introduced into the solution of a copper salt, it becomes coated wTith metallic copper. 5. Color of blowpipe flame is green. Antidote. Albumen. (Cu(C2II302)2II20—199.2) CuPRr Acetas.—Acetate of Copper. (Crystallized Verdigris.) Made by dissolving verdigris in dilute acetic acid. (Verdigris is the subacetate of copper (Cu20(C2H302)2)—made by allowing the marc obtained from the wine or cider-press, to undergo acetic fer- mentation, and placing it between sheets of copper; after a time the verdigris is scraped off) or, by the mutual decomposition between acetate of lead and copper sulphate, subsequently filtering and evaporating to crystallization. Reaction. Pb(C2H302)3 -f CuS04 = Cu(C2H302)3 -f- PbS04. / Lead \ / Copper \ / Copper \ / Lead \ \Acetate.y \Sulphate.y VAcetate./ VSulphate./ Description. Deep-green, prismatic crystals; efflorescent; odor- less; metallic taste; acid reaction; sol. in water (15), alcohol (135). (CuS04,5H20—249.2) Cupri Sulphas.—Sulphate of Copper. (Blue Vitriol. Blue Stone.) Prepared from copper pyrites; also by evaporating the water that collects in the copper mines; and by oxidation of the artificially prepared sulphide obtained by placing sulphur upon red-hot sheets of copper. Also formed during the purification of silver; or by dissolving the black scales obtained in coppersmithing in weak sul- phuric acid; and by the action of hot sulphuric acid on the metal. Reaction. Cu -j- H2S04 = CuS04 -j- H2 (Copper.) fSulphuric\ ( Copper V (Hydrogen.) V Acid. ) \SulphateJ Description. Large, translucent, deep-blue, triclinic crystals; efflorescent; odorless; nauseous metallic taste; acid reaction; sol. in water (2.6), insol. alcohol. Impurities and tests. Foi'eign metals: alkalies, and alk. earths: 5% solution + HC1 -}- H2S04, precip. with H2S; filt.-f- evap. = residue. Test for iron (ferrous) by oxidizing with chlorine, and adding NH4OH, which precipitates Fe2(OH)6. Properties. Astringent, emetic, and poisonous in large doses. THE LEAD SALTS. 135 Ammoniated Copper, or Ammoniated Sulphate of Copper. Made by dissolving CuS04 in NH4OH; on mixing the solution with alcohol, the blue salt precipitates. Reaction. CuS04 + 4NH4OH = Cu(NH3)4S04 + 4H20. ( Copper \ /Ammonium' / Ammoniated \ (Water.) VSulphate./ V Hydroxide./ VCopper Sulphate./ Occurrence. Found in the United States as oxide, carbonate (white lead ore), and most abundantly as galena, a sulphide (PbS). The metal is obtained from galena by roasting; at first a sulphate is formed through oxidation by the oxygen from air; by the action of more galena on this sulphate, the latter splits up into lead and S02. PLUMBUM.—Lead. (Pb.—206.5) First reaction. PbS -f- Heat -J- 202 = PbS04. / Lead \ /Oxygen, \ / Lead \ 'Sulphide./ \from air. ' vSulphate./ Second reaction. PbS04 + PbS = Pb2 -j- 2S02. [ Lead \ / Lead \ (Lead.) /Sulphur \ VSulphate./ /Sulphide./ VDioxide./ Description. A bluish-gray metal; malleable; ductile; sp. gr. 11.4 Tests for Lead Salts. 1. Solutions of the lead salts yield white precipitates, with HC1, H2S04, or potassium ferrocyanide. 2. Yel- low precipitates result when tested with iodide or chromate of potassium. 3. H2S and (NH4)2S yield black precipitates. 4. The introduction of metallic zinc or tin into the solution of a lead salt, causes a deposition of metallic lead. Antidote. Soluble sulphates, producing an insoluble lead sul- phate. (PbO—222.5) Plumbi Oxidum.—Oxide of Lead. (Litharge.) Made by heating the metal in contact with air to a white heat. Description. Heavy, reddish-yellow powder or scales; odor- less; tasteless; insoluble in water or alcohol. Impurities and tests. Carbonate: -f-HN03 = effervescence. Zinc, alkalies, and alk. earths (a limit): solution in ILN03 -f- H2S; filt. -f- evap. = residue. Officinal Preparations. 1. Liquor plumbi subacetatis. 2. Em- plastrum plumbi. Red Lead. (Pb304.) This is a higher oxide, made by exposing litharge which has not been fused, to a dull red heat. Emplastrum Plumbi.—Lead Plaster. (Diachylon Plaster.) Made by boiling olive oil, litharge, and water -together; saponifi- cation takes place, producing an insoluble lead soap. Officinal Preparation. Unguentum Diachylon. Also used as a base in making the following-named plasters: Ammoniac with mer- cury, asafetida, iron, galbanum, mercurial, opium, resin, and soap. Unguentum Dxachyuon. (Diachylon Ointment. Hebra’s Oint- ment.) Made by dissolving lead plaster (60) in olive oil (39) by the aid of heat, and adding oil of lavender (1). 136 MANUAL OF PHARMACY. (Pb(C2H302)2.3H20—378.5) Plumbi Acetas.—Acetate of Lead (Sugar of Lead.) Made by dissolving litharge in acetic acid, evaporating, crystal- lizing, purifying, and re-crystallizing. Reaction. PbO + 2HC2H302 = Pb(C2H302)2 -4- H20. (Lead Oxide.) (Acetic Acid.) (Lead Acetate.) (Water.) The impure brown acetate of lead is made by suspending sheet-lead in pyroligneous acid. Description. Colorless, transparent crystals or scales; efflor- escent, and attracting C02 on exposure to air; faint acetous odor; sweet astringent, afterward metallic taste; faint acid reaction; sol. in water (1.8), alcohol (8). Solution of this salt should be effected with distilled water only, otherwise a slight turbidity results, due to the formation of car- bonate, by the action of the dissolved C02 in alimentary waters. Impurities and tests. General impurities. Copper: -f- H2S04; lilt, -j- NH4OH (excess) = blue color. Zinc, alkalies, and alk. earths: Sol. -f- H2S; lilt. -|-evap. — residue. Officinal Preparation. Liquor Plumbi Subacetatis. (Solution of Subacetate of Lead. Goulard’s Extract.) Made by boiling litharge with solution of lead acetate. Description. A clear, colorless liquid; sweet, astringent taste; alkaline reaction; precipitates slightly on exposure to air; incom- patible with mucilage of acacia; sp. gr. 1.228; contains about 25# subacetate of lead (Pb20(C2H302)2). Officinal Preparations. 1. Liquor Plumbi Subacetatis Dilutus. 2. Ceratum Plumbi Subacetatis. 3. Linimentum Plumbi Subace- tatis. Liquor Plumbi Subacetatis Dilutus. (Diluted Solution of Subacetate of Lead. Lead Water.) Made by diluting Goulard’s Extract (3) with distilled water (97) previously boiled (to remove) air and C02) and cooled. Ceratum Plumbi Subacetatis. (Cerate of Subacetate of Lead. Goulard’s Cerate.) Made by incorporating Goulard’s Extract (20) with camphor cerate (80). Should be freshly made when needed. Linimentum Plumbi Subacetatis. (Liniment of Subacetate of Lead. Contains Goulard’s Extract (40), and Cotton-seed Oil (60) thoroughly mixed. ((PbC03)2. Pb(OH)2—773.5) Plumbi Carbon as.—Carbonate of Lead. (White Lead.) Made by passing C02 into a solution of lead acetate, or by the mutual decomposition between an alkali carbonate and a neutral lead salt, both in solution. First method. 3Pb(C2H302)2 + 2C02 -f* 4H20 (Lead Acetate.) / Carbon \ (Water.) (Dioxide./ = (PbC03)2. Pb(OH)2 + 6HC2Hs02. (Officinal Lead Carbonate.) (Acetic Acid.) 137 CHROMIUM. Second method. 3Pb(N03)2 -j- 3Na2C03 -(- 2H20 / Lead \ / Sodium \ (Water.) (Nitrate.) (Carbonate.) = (PbC03)2. Pb(OH)a + C02 + H20 + 6NaN03. /Lead Carbonate. \ / Carbon \ (Water.) /Sodium \ ( U. S. P. ) (Dioxide.) VNitrate./ Also made by the action of C02 from decaying vegetable matter, and acetous vapors, on lead. Description. Heavy, white powder; odorless; tasteless; insol. in water, or alcohol. Impurities: Zinc, alkalies, and alk. earths. (See Acetate.) Officinal Preparations. Unguentum Plumbi Carbonatis. (Oint- ment of Carbonate of Lead.) Contains lead carbonate (10) incor- porated with benzoinated lard (90). Made by mutual decomposition between potassium iodide and lead nitrate in solution; the precipitate is collected, washed and dried. (Pbl2—459.7) Plumbi Iodidum.—Iodide of Lead. Reaction. Pb(N03)2 -f- 2KI = Pbl2 -]- 2KN03. / Lead \ /PotassiumV / Lead \ /PotassiumX VNitrate./ ( Iodide. / (iodide.) V Nitrate. / Lead acetate cannot be substituted for the above nitrate, inasmuch as the double iodide of lead and potassium is formed, which dis- solves in the potassium acetate formed in the supernatant liquid. Description. A heavy, bright yellow powder; odorless; taste- less; neutral reaction; aim. insol. in water and alcohol; sol. in acetates of the alkalies, and NH4C1. Impurities: Same as other lead salts. Officinal Preparations. Unguentum Plumbi Iodidi. (Ointment of Iodide of Lead.) Incorporate powd. iodide of lead (10), with benzoinated lard (90). (Slow process.) Dissolve lead in warm diluted HN03. (Quick process.) Dissolve litharge or lead carbonate in dil. HN03, (Pb(N03)2—880.5) Plumbi Nitras.—Nitrate of Lead. First. 8Pb + 8HNOs = 8Pb(N03), + N202 -f 4H20. (Lead.) /NitricX / Lead \ /NitrogenX (Water.) V Acid./ (Nitrate./ V Dioxide./ Second. PbO + 2HN03 = Pb(N03)2 + H20. / Lead \ /NitricX / Lead \ (Water.) VOxide./ V Acid./ (Nitrate.) Description. Colorless, transparent, or white crystals; odor- less; sweet, astringent, afterwards metallic taste; acid reaction; sol. in water (2), aim. ins. alcohol. Impurities: Same as under Acetate. CHROMIUM. (Cr.—52.4) Occurrence. Found in United States and Russia as a mineral, chromate of lead, also as chrome iron ore (Fe0,Cr203). Tests for Chromium Salts. 1. (NH4)3 S, NaOH, and KOH give green precipitates of chromic hydroxide with solution of chromium salts. 2. Soluble lead salts precipitate yellow chromate of lead. 138 MANUAL OF PHARMACY. (K2Cr207—294.8) Potassii Bichromas.—Bichromate of Potassium. Preparation. Chrome iron ore is roasted, powdered and mixed with K2C03 and CaC03, and the mixture strongly heated in a cur- rent of air, thereby oxidizing the iron and chromium oxides to ferric oxide and chromic acid, the latter combining with K2C03 to make neutral potassium chromate, C02 being evolved. Reaction. 2(FeO, Cr203) + 4K2C03 + 70 = 4K2Cr04 (Chrome Iron Ore. \ / PotassiumX (Oxygen) /Potassium\ / (Carbonate./ (Chromate./ + Fe203 + 4C02. 1 Ferric \ / Carbon \ (Oxide./ (Dioxide./ The above mass is lixiviated with water, which dissolves out the potassium salt, and on adding H2S04 to the solution and evapor- ating, potassium bichromate crystallizes out. 2K2Cr04 + II2S04 = K2Cr20, + K2S04 + H20. /Potassium\ /Sulphuric\ / Potassium \ /Potassium\ (Water.) (Chromate./ ( Acid. / (Bichromate./ (Sulphate. / Description. Large, orange-red, transparent crystals; odorless; bitter, disagreeable, metallic taste; acid reaction; sol. in water (10), insol. in alcohol. Impurities. Sulphate : sol. -|- HNOs -f- BaCl2 = ppt. (Cr03—100.4) Acidum Chromicum.—Chromic Acid. (Chromic Anhydride ) Made by the action of H2S04 on potassium bichromate in solution; on standing crystals of chromic acid separate. K2Cr20, + 2H2S04 = 2KHSO4 + 2CrOs -f HaO /Potassium \ /SulphuricN /Acid PotassiumN /Chromic\ (Water.) (Bichromate./ ( Acid. ) ( Sulphate. ) ( Acid. / Description. Small, crimson, needle-shaped crystals, deliques- cent; odorless; having a caustic effect on the skin and other animal tissues; acid reaction; very soluble in water; decomposes with alco- hol. Caution. On contact, triturating or warming with strong alcohol, glycerin, spirit of nitrous ether, or other easily oxidizable substances, it is liable to cause sudden combustion or explosion. At a moder- ately high temperature it rapidly dissolves all animal tissues im- mersed in it, including even hair, bone, and teeth. Impurities: Sulphuric acid: 1% sol. -(- HC1 + BaCla = white ppt. CADMIUM. (Cd.—hi.8) Occurrence. Found as a sulphide (greenochite), hut more fre quently combined with zinc ore. Description. A malleable and ductile metal, having the color of tin; sp. gr. 8.7 There are no officinal preparations of cadmium; the salts are used extensively in photography, and often in medicine. The more im- portant salts follow. THE ZINC SALTS. 139 Cadmium Sulphate. (8CdS04.8H20—767.4) Made by the action of dilute H2S04 on cadmium in the presence of HNOs. Reaction. 3Cd2 + 6H2S04 -f 4HN03 = 6CdS04 (Cadmium.) /SulphuricN / Nitric N /CadmiumN \ Acid. / v Acid./ \Sulphate. / + 8H20 + 2N202. (Water.) /NitrogenX \ Dioxide./ Description. Colorless crystals; efforescent; astringent taste; acid reaction; sol. in water or alcohol. Cadmium Iodide. (Cdl2—865.8) Made by the mutual decomposition between potassium iodide and cadmium sulphate. Reaction. CdS04 -|- 2KI = K2S04 + Cdl2. /CadmiumN /PotassiumN /PotassiumN /CadmiumN \ Sulphate./ \ Iodide. / \ Sulphate. / \ Iodide. ) Description. White, flat crystals of a pearly lustre; sol. in water and alcohol. ZINCUM—Zinc. (Zn.—64.9) Occurrence. Found in combination as a silicate {calamine), car- bonate (Smithsonite), or sulphide {blende). Made by roasting the impure carbonate with charcoal in iron re- torts, when the zinc distils and is condensed. Description. A bluish-white metal; sp. gr. 6.9 Officinal in the form of thin sheets, or irregular, granulated pieces. Impurities and tests: Arsenic: dil. H2S04, the gas evolved blackens paper wet with AgN03. Lead iron, or copper: -f- NH4OH (excess) = ppt. Reactions of the Zinc Salts in Solution: With ammonium sulphide = a white precipitate (sulphide). “ water of ammonia = white precipitate. “ potassium ferrocyanide = white precipitate. “ potassium ferricyanide = orange precipitate. “ alkali carbonates = white precipitate. Antidotes. Na2C03; tannic acid; albumen. General impurities of the zinc salts and tests for their presence: Lead or copper: Sol. -|- HC1 + H2S = dark ppt. Iron, aluminium, alkaline earths: Sol. -f- (NH4)2C03 (excess) = ppt. Salts of alkalies or alk. earths: Sol. + (NH4)2S; tilt, -j- evap. + ignition = fixed residue. Liquor Zinci Chloridi.—Solution op Chloride op Zinc. (Burnett’s Disinfecting Fluid.) Made by dissolving granulated zinc in HC1, straining the liquid., adding HN03 (to oxidize the ferrous chloride formed, due to the iron usually present in zinc) evaporating to dryness and fusing. By re- dissolving in distilled water, and agitating the solution with ZnC03 140 MANUAL OP PHARMACY. the iron is precipitated as an oxide together with the excess of ZnC03 added, both of which are removed by filtration. Reaction. Zn2 -j- 4HC1 — 2ZnCl2 -j- 2H2. (Zinc.) /Hydrochloric/ / Zinc / (Hydrogen.) ( Acid. ) (Chloride.) Reactions representing the removal of iron ; 1. 6FeCl2 + 6HC1 + 2HN03 = 3Fe2Cl6 + N202 /Ferrous \ /Hydrochloric) /Nitric/ / Ferric / /Nitrogen/ (Chloride.) ( Acid. ) (Acid.) (Chloride.) (Dioxide.) + 4H20. (Water.) 2. Fe2Cl6 —3ZnC03 — 3ZnCl2 —(- Fe203 -j— 3C02 ( Ferric \ / Zinc \ / Zinc \ /Ferric \ / Carbon \ (Chloride.) (Carbonate.! (Chloride./ (Oxide.) (Dioxide./ Description. Clear, colorless, odorless liquid; astringent, sweet- ish taste; acid reaction; sp. gr. 1.555, contains about 50$ of ZnCl2. (ZnCl2—135 7) Zinci Chloridu.vi.—Chloride op Zinc. Made by evaporating a solution of zinc chloride, which has been made in accordance with the requirements for the officinal solution. Description. White, crystalline powder, or opaque pieces; very deliquescent; odorless; astringent, caustic, saline and metallic taste; acid reaction; very sol. in water or alcohol. General impurities. Made by driving off the C02 from ZnC03 by heat. Description. Pale-yellowish, nearly white powder; odorless; tasteless; insol in water or alcohol; sol. in acids, without efferves- cence. General impurities. Officinal Preparations. Unguentum Zinci Oxidi (Ointment of Ox- ide of Zinc). Contains ZnO (20), thoroughly incorporated with ben- zoinated lard (90). (ZnO—80.9) Zinci Oxidum.—Oxide op Zinc. (ZnS04.7 H20—286.9) Zinci Sulphas.—Sulphate op Zinc. (White Vitriol.) Made by dissolving zinc in dilute H2S04, oxidizing and precipitat- ing any iron salt that may be present, as an oxide, by the addition of chlorine and ZnC03. Reaction. Zn2 -f- 2H2S04 = 2ZnS04 -f 2H2. (Zinc.) /Sulphuric/ / Zinc \ (Hydrogen. V Acid. ) (Sulphate./ Description. Small, colorless, needle-shaped crystals; slowly efflorescent in dry air; sharp, saline, nauseous, metallic taste; acid re- action; sol. in water (0.6), insol. in alcohol. General impurities, and Chloride: + AgN03 = white ppt. This salt is often confounded with magnesium sulphate, which it somewhat resembles in appearance. ((ZnC03)2.3Zn(0H)2—546.5) Zinci Carbonas Pr^ecipitatus.— Precipitated Carbonate of Zinc. Made by precipitating a boiling solution of ZnS04 with a boiling solution of Na2C03, washing and drying the precipitate. The pre- cipitated ZnC03 is soluble in excess of Na2C03, also in a solution of THE ZINC SALTS. 141 C02, hence boiling solutions are used to drive off the excess of the lat- ter. 5ZnS04 + 5Na2C03 + 3H20 = (ZnC03)2 . 3Zn(OH)2 / Zinc \ / Sodium \ (Water.) (Zinc Carbonate.) (Sulphate.) (Carbonate.) + 5Na2S04 + 3C02. ./ Sodium \ / Carbon \ (Sulphate.) (Dioxide.) Description. White, impalpable powder; odorless; tasteless; insol. in water or alcohol; sol. in acids with copious effervescence. General impurities. Zn(C2H302)2.3H20—236.9) Zinci Acetas.—Acetate of Zinc. Made by digesting the commercial oxide or carbonate of zinc in diluted acetic acid, boiling the solution, and crystallizing. Reaction. ZnO -(- 2HC2H302 = Zn(C2H302)2 4- H20. / Zinc / (Acetic Acid.) (Zinc Acetate.) (Water.) (Oxide.) Description. Soft, white, pearly octahedral tablets or scales; faint acetous odor; sharp, metallic taste; slight acid reaction; sol. in water (3), alcohol (30). General impurities. (ZnBr2—224.5) Zinci Bromidum.—Bromide of Zinc. Made by digesting zinc in HBr, or by the mutual decomposition between ZnS04 and KBr; zinc bromide and potassium sulphate are both formed in solution, and the latter removed by adding alcohol and filtering through asbestos. First method. Zn -j- 2HBr = ZnBr2 -)- H2. (Zinc.) /Hydrobromic/ / Zinc \ (Hydrogen.) ( Acid. ) (Bromide./ Second method. ZnS04 2KBr = ZnBr2 -j K2S04. / Zinc \ /Potassium/ / Zinc \ /Potassium/ \Sulphate.l ( Bromide. ) (Bromide./ ( Sulphate. ) Description. White, granular powder; very deliquescent; odor- less; sharp, alkaline, metallic taste; neutral reaction; very sol. in water, or alcohol. General impurities. Made by dissolving zinc oxide or carbonate, in hydriodic acid, or by digesting zinc with iodine in water, until the liquid becomes col- orless; filter through powdered glass and evaporate. (Znl2—818.1) Zinci Iodidum.—Iodide of Zinc. First reaction. (ZnC03)2 . 3Zn(OH)2 4~ 10HI = 5ZnI2 (Zinc Carbonate.) /Hydriodic\ ( Zinc \ V Acid. ) (Iodide.) + 2C02 + 8H20. / Carbon \ (Water.) (Dioxide.) Second reaction. Zn -)- I2 = Znl2. (Zinc.) (Iodine.) (Zinc Iodide.) Description. White, granular powder; very deliquescent; odor- less; sharp, saline taste; acid reaction; very sol. in water, or alcohol, General impurities. 142 MANUAL OF PHARMACY. (Zn3P2—256.7) Zinci Phosphidum.—Phosphide of Zinc. Made by fusing zinc in a current of hydrogen, and introducing vapors of phosphorus. Description. Small, crystalline, friable fragments of metallic lustre; or a grayish-black powder having faint odor and taste of phos- phorus; insol. in water, or alcohol; sol. in HC1, or H2S04. General impurities. (Zn(C6H902)2.H20—284.9) Zinci Valerianas.—Valerianate of Zinc. Made by the mutual decomposition between sodium valerianate and zinc sulphate, both in hot solutions; on cooling, the zinc salt crystal- lizes out; also by dissolving fresh moist zinc carbonate in valerianic acid. 2NaC6H902 + ZnS04 = Zn(C6H9Oa)2 + Na2S04 / Sodium \ / Zinc \ / Zinc \ ( Sodium \ VValerianate.y VSulphate./ \Valerianate./ • VSulphate./ or, (ZnC03)2 . 3Zn(OH)2 -f 10HC5H9O2 = 5Zn(C6H902)2 (Zinc Carbonate.) (Valerianic Acid.) (Zinc Valerianate.) + 2C02 + 8H20. ( Carbon \ (Water.) /Dioxide./ Description. Soft, white, pearly scales; odor of valerianic acid; sweet, styptic, and metallic taste; acid reaction; sol. in water 100, al- cohol 40. General impurities, and Butyrate: Sol. -f- copper acetate = ppt. ARSENIUM.—Arsenic. (As.—74.9) Occurrence. The metalloid arsenic is found as native arsenic, also as cobaltum or fly-stone, but more frequently as sulphides, red orpiment, or realgar (As2S2), yellow orpiment (As2S3), mispickel (Fe2S2,FeAs2). Preparation. Made by roasting mispickel {arsenical pyrites), or by roasting arsenious oxide with charcoal. Description. Steel-gray, crystalline mass; volatile; sp. gr. 5.73-5.96. When heated in the air it absorbes oxygen and forms arsenious oxide (As2Os). 1. H2S; with acid solutions of arsenic or its salts, gives a bright yel'ow precipitate, soluble in alkalies, but insoluble in HC1. 2. Ammoniacal solution of copper sulphate; produces a grass- green precipitate (Scheele’s Green), soluble in excess of NII4OH. 3. Ammoniacal solution of silver nitrate; yields a lemon-yellow precipitate (silver arsenite), soluble in excess of N1I40H. 4. Berzelius’ test : On beating in a test tube with charcoal, an iron-gray mirror of metallic arsenic, having an alliaceous odor, deposits on the tube. 5. Reinch’s test: If a strip of bright copper foil is boiled with a solution of arsenic acidulated with HG1, a deposition of gray metal- lic arsenic takes place on the copper, accompanied by bluish spots. Reactions of Arsenic and its salts. ABSENTC. 143 6. Marsh’s test: Arseniuretted hydrogen (AsH3) is evolved on treat- ing test-zinc with the arsenic solution (acidulated with H2S04); the gas on ignition deposits a brown-black spot of metallic arsenic upon a piece of porcelain held in the flame, which dissolves on adding moist chlorinated lime or solution of chlorinated soda. Antimony com- pounds yield a similar spot, which remains unaffected by the hypo- chlorites. If the delivery tube through which the gas passes is heated, arseniuretted hydrogen is decomposed and metallic arsenic is de- posited just beyond the point of flame; antimony deposits just at the point of flame. If dry II%S is passed through the tube after the formation of the mirror, and the tube heated, the volatilized metal (arsenic or antimony) again deposits as a sulphide with its characteristic color, yellow or orange-red. 7. Fleitmann’s test: Also depends upon the generation of AsH3, sub- stituting for the dilute acid, a strong solution of potassa or soda (which prevents the formation of antimoniuretted hydrogen); the evolved AsH3 produces a black stain on filter paper moistened with silver nitrate solution. Aluminium wire is often used in the above, in place of zinc. Antidotes for Arsenic poison. After evacuating the stomach by means of emetics or the stomach pump, give freshly precipitated hydrated oxide of iron, hydrated oxide of iron with magnesia, dialysed iron, saccliarated carbonate of iron, or, solution of ferric chloride. The following reaction with ferric hydroxide is possible: 2Fe2(OH)6 + As203 = Fe3(As04)2 + Fe(OH)2 -f 5H20. / Ferric \ /Arsenious\ / Ferrous \ ( Ferrous \ (Water.) \Hydroxide./ \ Oxide. ) VArseniate./ VHydroxide.) The strength of all officinal arsenical solutions is equivalent to about 1$ arsenious acid. Dose, 5-8 minims. (As203 —197.8) Acidum Arseniosum.— Arsenious Acid. (White Arsenic. Arsenious Anhydride. Arsenious Oxide.) Made from the arsenical ores by roasting; purified by sublimation. The action of water on As203 produces the true arsenious acid: [Arsenic Oxide (As205) is made by the oxidation of As203 by HN03. It is but little used.] Description.—A heavy white solid, occurring either as an opaque powder, or in glass-like, transparent pieces (when freshly made); odorless; tasteless; faint acid reaction; sol. in water 30-80, depend- ent on its physical condition; sp. sol. in alcohol. Should contain at least 97$ of As203. Assay, dependent on the quantity of volumetric solution of iodine it decolorizes, after being dissolved in boiling water by the aid of sodium bicarbonate. As203 4- 3H20 = 2II3As03. As203 + 2h + 5H20 = 2H3As04 + 4HI. /"ArseniousN (Iodine.) (Water.) (ArsenicN /Hydriodic\ V Oxide. ) V Acid. ) V Acid. ) Officinal Preparations. 1 Liquor acidi arseniosi. 2. Liquor potassii arsenitis. 144 MANUAL OF PHARMACY. Liquor Acidi Arseniosi.—Solution of Arsenious Acid. Formerly termed Solution of Arsenic Chloride. Made by dis- solving arsenious acid (1), in boiling water containing HC1 (2), filtering and adding water ft. 100. No chemical action takes place, as the HC1 is merely added as solvent for As203. Description. A colorless solution; sp. gr. 1.009; contains \% As203, or 4 grs. to each fluid ounce. [Valangin’s Solution contains 0.38$, or If grs. in the fluid ounce.] Assay, dependent on quantity of volumetric solution of iodine it decolorizes. Liquor Potassii Arsenitis.—Solution of Arsenite of Pot- assium. (Fowler’s Solution. Arsenical Solution.) Made by boiling white arsenic with acid potassium carbonate, and flavoring with compound tincture of lavender. Reaction. As203 + 2KHC03 + H20 = 2KH2As03 -f- 2C02. /Arseniousx /Acid Potassium \ (Water.) / Potassium/ / Carbon \ \ Oxide. ) v Carbonate. / V Arsenite. ) \Dioxide.y Description. A reddish liquid, somewhat opalescent; alkaline reaction; sp. gr. 1.009; contains 1% As203. Assay. The amount of As203 is ascertained with iodine, using starch jelly as an indicator, which does not become permanently blue until the arsenioun is oxidized to arsenic acid. (See reaction for assay under Arsenic.) (AsI3—454.7) Arsenii Iodidum.—Arsenious Iodide. (Iodide of Arsenic.) Made by combining iodine and metallic arsenic by heating gently until liquefied; also made by dissolving As2Os in HI. Reaction. As203 —6HI — 2ASI3 -j— 3H20. /ArsenlousN /HydriodicN /Arsenious\ (Water.) \ Oxide. / \ Acid. / \ Iodide ) Description. Glossy, orange-red crystalline masses, or scales; neutral reaction; odor and taste of iodine; sol. in water (3.5), alco- hol (10), ether, and CS2. Officinal Preparation. Liquor Arsenii et Hydrargyri Iodidi. (Solution of Iodide of Arsenic and Mercury. Donovan’s Solution.) Contains Asl3 (1) and Hgl2 (1), dissolved in water ft. 100. No chemical combination takes place between the two iodides. Description. A light, yellow-colored liquid, becoming darker by age; original color may be restored by agitation with a small quantity each of mercury and arsenic. (Na2HAs04.7H20—311.9) Sodii Arsenias.—Arseniate of So- dium. Made by heating arsenious acid, exsiccated sodium carbonate, and sodium nitrate to fusion; dissolving, filtering, and crystallizing. Reaction. As203 —|— 2NaN03 —|— Na2C03 — Na4As207 /Arsenlous\ /SodiumA / Sodium \ ( Sodium \ \ Oxide. ) \Nitrate.) VCarbonate./ \Pyro-arseniate./ + co2 + n2o3. / Carbon \ /Nitrogen \ \DioxideJ VTrioxide./ 145 ANTIMONY. Reaction. Na4As207 -f- H20 = 2Na2HAs04. ( Sodium \ (Water.) ( Sodium \ \Pyro-arseniate.y (Arseniate.) On dissolving the pyro-arseniate in water,ortho-arseniate is formed. Description. Colorless, transparent crystals; odorless; feeble alkaline taste and reaction; sol* in water (4), alcohol (slightly).—Im- purity, Arsenite: Cold aq. sol. -f- HC1 -f- HaS = yellow color, or ppt. Officinal Preparation. Liquor Sodii Arseniatis.—Solution op Arseniate of Sodium. Made by dissolving anhydrous sodium arseniate (1), in distilled water (99). Pearson’s Solution. Contains crystallized arseniate of sodium 1 gr., dissolved in water 600 grs. or, one tenth the strength of the officinal solution. Clemen’s Solution. A solution of arsenious bromide in dis- tilled water. Dose, 1-4 drops. Sclieele’s Green. 3CuO, As203, 2H20. Paris Green. (Schweinfurth’s Green. Vienna Green.) An aceto-arsenite of copper. Formula of best variety is: 3Cu0,As203 + 2Cu(C2H30j)a + 5H20. STIBIUM—Antimony. (Sb—120) Occurrence. Found native, but more abundantly as sulphide (black antimony or stibnite), oxide, or oxysulphide. Metallic anti- mony is not used in pharmacy, its chief use being for type metal. Description. A brilliant, brittle metal, of crystalline structure, having a silver-white color; sp. gr. 6.7 Reactions of Antimony and its Salts. 1. H2S yields an oi'ange-red precipitate soluble in (NH4)2S, and in boiling HC1. 2. On introducing a piece of bright iron or zinc into the solution, metallic antimony precipitates as a black powder. For other tests, see Arsenic. (Sb2S3—336) Antimonii Sulphidum.—Sulphide of Antimony. (Black Antimony.) Native sulphide of antimony, purified by fusion and as nearly free from arsenic as possible. Description. Steel-gray masses, of a metallic lustre, and crystal- line fracture; forming a dull, blackish powder; odorless; tasteless; insol. in water or alcohol; sol in boiling HC1. Often adulterated with coal dust, and clay. Officinal Preparation. Antimonii Sulphidum Purificatum. Antimonii Sulphidum Purificatum.—Purified Sulphide of Antimony. Preparation. Sulphide of antimony is powdered, and the coarser particles separated by elutriation; after allowing the finely divided sulphide to deposit, the water is removed, and the sulphide macerated for five days with Is II,OH, which dissolves out the arsenious sulphide; the powder is then washed with water and dried. 146 MANUAL OF PH A KM ACT. Description. Dark-gray powder; odorless; tasteless; insol. in water or alcohol; sol. in boiling HC1. Impurities: Other metallic sulphides. Officinal Preparation. Antimonium Sulphuratum. Antimonium Sulphuratum.—Sulphurated Antimony. (Golden Sulphur.) Chiefly antimonious sulphide (Sb2S3) with a very small amount of antimonious oxide. Made by boiling the purified sulphide with dilute solution of soda, then straining and slowly adding H2S04 to the liquid as long as a precipitate is produced, wash, dry and powder. (1) 4Sb2S3 + 8Na01I = 3Na28b284 + 2NaSb02 /AntlmonyX / Sodium \ / Sodium \ / Sodium \ \ Sulphide. / VHydroxide.) vSulphantimonlte.) VAntlmonlte./ + 4HaO. (Water.) (2) 3Na2Sb2S4 + 2NaSb02 + 4H2S04 = 4Sb2S3 / Sodium \ / Sodium \ /Sulphuric) /Antimony) VSulphantimonlte./ VAntimonite./ V Acid. / \ Sulphide. / + 4Na2804 + 4H20. / Sodium ) (Water.) (Sulphate. / Description. A reddish-brown, amorphous powder; odorless; tasteless; insol. in water, or alcohol; sol. in hot HC1. Impurities and tests. Sulphate (a limit): -j-H20 + boil; flit, -f- BaCl3 = white ppt. Officinal Preparation. Pilul/E Antimonii Composite. (Com- pound Pills of Antimony. Plummer’s Pill.) Each pill contains i grain each of sulphurated antimony and calomel, and 1 gr. guaiac. (Sb203—288) Antimonii Oxidum.—Oxide of Antimony. (Antimonious Oxide.) Made by dissolving sulphurated antimony in hot HC1, and pour- ing the antimonious chloride solution thus formed into water; the oxy chloride precipitates, is allowed to subside, and washed with water, then with NH4OH (forming the oxide), again washed with water and dried. Sb2S3 + 6HC1 = 2SbCl3 + 3H2S. /Antimony) /Hydrochloric) / Antimonious) /Hydrogen) V Sulphide. / \ Acid. ) \ Chloride. / \ Sulphide./ 12SbCl3 + 15H20 = 2SbCl3 . 5Sb203 + 30HC1. /Antimonious) (Water.) /Antimony Oxy) /Hydrochloric) \ Chloride. ) V chloride. / \ Acid. / 2SbCl3 . 5Sb203 + 6NH4OH = 6Sb203 4 6NH4C1 + 3H20. /Antimony Oxy-\ /AmmoniumN /Antimony\ /Ammonium) (Water.) \ chloride. ) \ Hjfdroxide.) \ Oxide. / \ Chloride. / Description. Heavy, grayish-white powder; aim. insol. in water; insol. alcohol; sol. in HC1 and warm solution of tartaric acid. Impurities and tests. Chloride: Sol. 4 AgN03 = white ppt. Sulphate: Sol. 4 BaCl2 = white ppt.. Iron and other metals: Sol. 4 potass. ferrocyanide = ppt. Officinal Preparation. Pul vis Antimoniat.is. (Antimonial Powder. .Tames’ Powder. Pulvis Jacobi.) Contains antimonious oxide (83), diluted with precipitated calcium phosphate (67). THE BISMUTH SALTS. 147 (2KSb0C4II406.H20) Antimonii etPotassii Tartras.— Tartrate of Antimony and Potassium. (Tartar Emetic.) Made by boiling potassium bitartrate and antimonious oxide with water, filtering and crystallizing. Reaction. 2KHC4H406 -f- Sb203 = 2KSb0C4H406, H20. /Potassium-, /Antimonlous\ /Antimoniated Potassium\ VBitartrate.) \ Oxide. / \ Tartrate. ) Description. Small, transparent crystals, becoming white on exposure to air; sweet, afterward disagreeable taste; feebly acid reaction; sol. in water 17, boiling water 8, insol. in alcohol. Properties. Very poisonous. Most powerful emetic known. Dose: one grain. Impurities and tests. Besides those given under Antimonii Oxidum, the following, viz.: Calcium: -f- (NH4)2C204 = white ppt. Arsenic: Fleitmann’s test (see Arsenic). Officinal Preparation. 1. Syrupus scillse compositus. 2. Vinum antimonii. Syrupus Scii/l/e Compositus. (Compound Syrup of Squill. Hive Syrup. Croup Syrup.) The active ingredients are squill, seneka, and tartar emetic; three parts of the last mentioned in 2000 parts, or 0.15$. Dose, 10-30 drops. Vinum Antimonii.—Wine of Antimony. Made by dissolving tartar emetic (4), in boiling water (60), and adding to stronger white wine ft. 1000. Contains 0.4$ tartar emetic. Dose. 10 drops. Officinal Preparation Mistura Glycyrriiiz/e Composita. (Compound Licorice Mixture. Brown Mixture.) Contains purified extract licorice, sugar, acacia, paregoric, wine of antimony, spirit of nitrous ether, and water. Contains 6$ wine of antimony. Dose four fluid-drachms. BISMUTHUM.—Bismuth. (Bi.—210) Occurrence. Found in the metallic state associated with cobalt, nickel and silver ores; occasionally found as sulphide. Description. Brilliant, grayish-white metal, of a crystalline texture; sp. gr. 9.88; sol. in UNO3. Usually contaminated with arsenic. Reactions of Bismuth and its salts. 1. H2S: gives black precipitate, soluble in HN03. 2. Water of Ammonia: yields a white precipitate, insoluble in excess. 3. Potassium chromate: produces a yellow precipitate. ((Bi0)2C03.H20—580) Bismuthi Subcarbonas.—Subcarbonate of Bismuth. Preparation. Metallic bismuth is dissolved in dilute nitric acid, forming a solution of bismuthous nitrate, which is diluted with water and filtered, then still further diluted and poured into water of ammonia. The resulting precipitate is drained, washed and dis- solved in nitric acid; the solution, diluted with water, is filtered and added to a cold solution of sodium carbonate, when bismuth sub- carbonate precipitates, which is drained, washed and dried.. Explanation of above process. Most metallic bismuth contains 148 MANUAL OF PHARMACY. some arsenic, which is oxidized by the nitric acid, so that arseniate of bismuth is formed, most of which deposits on diluting. The clear liquid still retaining small quantities of arsenic, is deprived of it by pouring into an excess of NH4OH, producing nitrate and arseniate of ammonium (both soluble) while bismuthous hydroxide precipitates, and is further converted into the subcarbonate by dissolving in nitric acid and pouring into a solution of sodium car- bonate. First step. 2Bi 4 8HN03 = 2Bi(N03)3 4 N202 4 4H20. (Bismuth.) /NitricX /BismuthX /Nitrogen) (Water.) VAcid. / VNitrate./ VDioxide./ Second step. 2Bi(N03)3 4 6NH4OH = 2Bi(OH)3 4 6NH4N03. /BismuthX /AmmoniumX /BismuthousX /Ammonium) VNitrate./ VHydroxide./ VHydroxide./ V Nitrate. / Third step. 2Bi(OH)3 4 6HN03 = 2Bi(N03)3 4 6H20. /BismuthousX /NitricX /BismuthX (Water.) VHydroxide./ V Acid./ V Nitrate./ Fourth step. 2Bi(N03)3 + 3Na2C03 = (Bi0)2C03 /BismuthX / Sodium X / Bismuthous X VNitrate. / VCarbonate./ VSubcarbonate./ 4- 6NaN03 4- 2C02. / Sodium \ / Carbon X VNitrate./ VDioxide./ Description. Pale, yellowish-white powder; odorless; tasteless; insol. in water or alcohol; sol. in nitric acid with effervescence. Impurities and tests. Insoluble foreign matter: 4 HN03 = solu- tion with residue. Lead: Solution 4 H20; tilt. 4 HaS04 = cloud- iness. Copper ! Solution 4 NH4OII = blue color. Chlorides: Solu- tion 4 AgN03 = white ppt. Sulphates: Solution 4Ba(N03)2 = white ppt. Silver : Solution 4 HC1 = white ppt. Alkalies, and Aik. earths : 4 dil. HC2H3Oa 4 boil; hit. 4 H2S; tilt. 4 evaP- = fixed residue. Antimony, arsenic, and tin: 4 solution soda 4 boil 4H20; tilt. 4 HC14 H2S = yellow, or orange ppt. Arsenic: Fleitmann’s test. (See Arsenic.) (Bi0N03.H20—806) Bismuthi Subnitras.—Subnitrate of Bismuth. Preparation. After preparing the washed bismuthous sub- carbonate, as shown above, dissolve in diluted nitric acid, filter and pour into water containing a small amount of NH4OH to partly neutralize the HN03, in order to precipitate the greater part of the bismuth, some of which would still remain held in solution by the nitric acid of the supernatant liquid. The subnitrate deposits, is washed and dried. (Bi0)2C03 4 6HN03 = 2Bi(N03)3 4 C02 4 3H20. / Bismuthous \ /NitricX /BismuthX / Carbon X (Water.) VSubcarbonate./ VAcid./ VNitrate./ VDioxide./ 6Bi(N03)3 4 10H2O = 5Bi0N03,II20 4 Bi(N03)3 4 10HNO3. /BismuthX (Water.) / Bismuth X /BismuthX (Nitric Acid.) V Nitrate./ VSubnitrate./ V Nitrate./ Description. Heavy, white powder; odorless; almost tasteless; slight acid reaction; insol. in'water or alcohol. Impurities and tests. Carbonate: -|- HN03 = effervescence; and those found under the Subcarbonate. THE MERCURY SAUTS. 149 (BiC6H60T—399) Bismuthi Citras.—Citrate of Bismuth. Made by boiling bismuth subnitrate in a solution of citric acid, until a drop of the mixture yields a clear solution with water of ammonia; on adding water, the citrate deposits, is drained, washed and dried. Bi0N03 + HsC.HsOt = BiC6H607 + HN03 + H20. ( Bismuth \ (Citric Acid.) /BismuthN /Nitric\ (Water.) VSubnitrate.), V Citrate. J \ Acid./ Description. White, amorphous powder; odorless; tasteless; insol. in water or alcohol; soluble in NH4OH. Impurity. Nitrate : + NH4OH -|- H2S; tilt. -|- FeS04 = brown zone. Officinal Preparation. Bismuthiet Ammonii Citras.—Citrate of Bismuth and Ammonium. Made by dissolving bismuth citrate in diluted water of ammonia, evaporating to a syrupy consistence and scaling. Description. Small, shining, pearly or translucent scales, be- coming opaque on exposure; odorless; acidulous, metallic taste; neutral or faintly alkaline reaction; very soluble in water; sp. sol. in alcohol. Impurity; same as in the Citrate. HYDRARGYRUM.—Mercury. (Quicksilver.) Hg. Occurrence. Found in nature most abundantly as cinnabar (HgS), in California, Peru; China, and Spain. Preparation. Obtained by roasting the ore. Conducted in such a manner, that the sulphur is burned into S02, while the metal volatilizes and is condensed in a series of chambers called aludels; the incondensable gases escaping. Reaction. 2HgS -j- 202 = IIg2 + 2S02. / Mercury \ / Oxygen. \ (Mercury.) ( Sulphur \ \ Sulphide. J \(from Air)/ \ Dioxide.' Description. Shining, silver-white metal; liquid between — 40° and 662° F. ( — 40° and 850° C.); sp. gr. 13.5; insoluble in ordinary solvents; sol. in nitric acid; odorless; tasteless. Forms two kinds of salts, mercuric and mercurous. Impurities and Tests. The presence of other metals is indica- ted by the shape of the globule; which should be round and not elongated ; it should not adhere to paper, nor leave a dark streak upon it, nor fail to have a bright surface. Purification. Accomplished by re-distillation, or by digesting with diluted nitric acid, washing well, drying, and passing forcibly through chamois; the contaminating metals become oxidized, and only a small portion of the mercury passes into solution. Also purified by agitation with solution of ferric chloride, or cone. II2S04. Subdivision. The subdivision of mercury is termed extinguish- ing or killing, and is accomplished by trituration with foreign sub- stances; the minute globules becoming coated with the substance used, thus preventing them from cohering. The officinal degree of 150 MANUAL OF PHARMACY. extinction is reached, when globules are no longer visible under a magnifying power of ten diameters. With With Reagent. mercurous salts mercuric salts gives; gives; Potassium Iodide Green ppt. Red ppt. Potassium Hydroxide.Black ppt. Yellow ppt. Hydrogen Sulphide.. .Black ppt. Black ppt. Stannous Chloride... .Gray-black ppt. Gray-black ppt. Bright Copper Wire.. .Coatingof Mercury. Coating of Mercury. Hydrochloric Acid White ppt. No reaction. Reactions of Mercury Salts. Antidote. Albumen in the form of egg, flour or milk, fol- lowed by emetics. Officinal Preparations. 1. Emplastrum Ammoniaci cum hydrar- gyro. 2. Emplastrum hydrargyri. 3. Hydrargyrum cum creta. 4. Massa hydrargyri. 5. Unguentum hydrargyri. Emplastrum Ammoniaci cum Hydrargyro.—Ammoniac Plas- ter with Mercury. Made by dissolving sulphur (1) in hot olive oil (8) and triturating mercury (180) with it till extinguished; incorpo- rate with a hot emulsion of ammoniac (720), (made by digestion with diluted acetic acid and evaporation) and lead plaster ft. 1000 parts. Contains 18$ mercury. Emplastrum Hydrargyri.—Mercurial Plaster. Made by extinguishing mercury (30) with a mixture of rosin (10) and olive oil (10), and incorporating with it melted lead plaster (50). Contains 30,® mercury. Hydrargyrum cum Creta.—Mercury with Chalk. Made by the extinction of mercury (38) with milk sugar (12) and chalk (50), using ether and alcohol to moisten the mass. Description. Gray, non-gritty, odorless and tasteless powder. Contains 38,® mercury. Caution. On exposure to light or air, oxidation takes place; the mercurous oxide being identified by dissolving out with diluted acetic acid, and treating with HC1, which produces a cloudiness; mercuric oxide, after dissolving out with the aid of HC1, a black pre- cipitate is produced with 1I2S, or gray with stannous chloride. Dose, 3-10 grs. Massa Hydrargyri.—Blue Mass. (Blue Pill.) Made by ex- tinguishing mercury (33) with honey of roses (34) and glycerin (3), and incorporating with powdered licorice (5) and marshmallow (25). Contains 33$ mercury. Dose, 3-10 grs. Unguentum Hydrargyri.—Mercurial Ointment. (Blue Oint- ment.) Made by extinguishing mercury (450) with tinct. benzoin comp. (40), and mercurial ointment (100), and incorporating with a previously melted mixture of lard and suet. The storax in tincture benzoin comp, aids in readily extinguishing the mercury, while the balsamic matter of tolu and benzoin after evaporation of the alcohol, act as preservative agents. Contains 50$ mercury. THE MERCURY SALTS. 151 (HgCl2—270.5) Hydrargyri Chloridum Corrosivum.—Cor- rosive Chloride of Mercury. (Bi- or Perchloride of Mer- cury. Mercuric Chloride. Corrosive Sublimate.) Made by boiling mercury with H2S04 until a dry mass (mercuric sulphate) remains, which is mixed with sodium chloride and sub- limed; mercuric chloride volatilizes. 1. Hg2 + 4H2S04 = 2HgS04 + 2S02 4 4H20. (Mercury.) /Sulphuric) /Mercuric) /Sulphur) (Water.) ( Acid. / (Sulphate./ (Dioxide./ 2. HgS04 4 2XaCl = Xa2S04 4 HgCl2. /Mercuric) /Sodium) /Sodium) /Mercuric) (Sulphate./ VChloride./ (Sulphate./ (Chloride./ Description. Heavy, colorless rhombic crystals, or crystalline masses; odorless, acrid and persistent metallic taste; acid reaction; sol. in water 16, alcohol 3, ether 4, and very soluble in ammonium chloride solution. Dose, 4 -£ grain. Impurities and tests. Arsenic: Fleitmann’s test, using aluminium wire in the place of zinc. (Hg2Cl2—470.2) Hydrargyri Chloridum Mite.—Mild Chlo- ride of Mercury. (Sub- or Protochloride of Mercury. Mer- curous Chloride. Calomel.) Preparation. Mercuric sulphate (as made by the process given under mercuric chloride) is mixed with the requisite quantity of mercury to form mercurous sulphate. Reaction. Hg2 4- 2HgS04 = 2Hg2S04. (Mercury) /Mercuric ) /Mercurous) (Sulphate./ ( Sulphate. / Sodium chloride is added to the mercurous salt, and the mixture heated, when IIg2Cl2 sublimes. Reaction. Hg2S04 4 2NaCl = Hg2Cl2 -|- Xa2S04. /Mercurous) / Sodium ) /Mercurous) / Sodium ) V Sulphate. / (Chloride./ ( Chloride. ) (Sulphate./ The vaporized Hg2Cl2 passes into a suitable condenser, falling as a powder, while Xa2S04 remains. Some mercuric chloride also forms, but may be removed by washing with water, or by injecting steam into the condenser as sublimation proceeds. Bose, 5-20 grains. Description. White, impalpable powder; odorless; tasteless; insol. in water, alcohol or ether; blackened by NII4OH. Impurities and tests. Mercuric chloride : Treat with water or alcohol; tilt, 4 II2S = black ppt.; or bit. 4 AgN03 = white ppt. Ammoniated mercury: -)- KOH -j- Heat = odor of NH3, besides above reactions. Officinal Preparations. 1. Pilulae antimonii comp. (See Anti- mony.) 2. Pilulze Cathartics Composite.—Compound Cathartic Pills. (Anti-bilious Pills.) Each pill contains comp, extract of colocyntb 1.3 gr.; abstract jalap, 1 grain; calomel, 1 gr.; powd. gamboge, 0.25 grain. Dose, 1-3 pills. 152 MANUAL OF PHARMACY. (Hgl2—452.9) Hydrargyri Iodidum Rubrum. Red Iodide of Mercury. (Biuiodide, or Deutoiodide of Mercury. Mercuric Iodide.) Made by the mutual decomposition between mercuric chloride and potassium iodide, both in solution. Wash and dry the pre- cipitate. Reaction. 2KI HgCL = Hgl2 + 2KC1. /Potassium/ /Mercuric/ /Mercuric/ /Potassium/ \ Iodide. / VChloride./ y Iodide. / \ Chloride. / The precipitated iodide is soluble in excess of either of the chemicals used. Description. Scarlet-red, crystalline powder; odorless; taste- less; almost insol. in water; sol. in alcohol (130), and in solution of KI, or HgCL, also in a hot solution of NaCl, from which it crystal- lizes on cooling. Dose, grain. Impurities and tests. Soluble iodides and chlorides : -(- H20; filt. + AgN03 = white ppt. Officinal Preparation. Liquor arsenii et hydrargyri iodidi. (See Arsenic. (Hg2I2—652.6) Hydrargyri Iodidum Yiride.—Green Iodide of Mercury. Protoiodide of Mercury. Mercurous Iodide.) Made by triturating together mercury (8) and iodine (5) (using alcohol to keep down the temperature) until a greenish yellow color is acquired. Some Hgl2 is also produced which is removed by washing with alcohol till the washings are not affected by II2S. Keep in dark-colored bottles. Description. Dull green, to greenish yellow powder; becoming more yellow by exposure to light; odorless; tasteless; aim. insol. in water; insol. alcohol or ether. On exposure to light, it decom- poses into mercuric iodide. Dose, -1 grain. Impurities and tests. Mercuric Iodide : -f- ale.; hit. 4- II20 = opalescence; or, on evaporating on white porcelain, only a faint red stain remains. (HgO—215.7) Hydrargyri Oxidum Flavum.—Yellow Oxide of Mercury. (Mercuric Oxide.) Made by the mutual decomposition between mercuric chloride in solution, and solution of potash, pouring the former into the latter (to prevent the formation of red oxide). Reaction. HgCL -f- 2KOH = HgO -|- 2KC1 -f- H20. /Mercuric\ / Potassium \ /Mercuric/ /Potassium/ (Water.) /Chloride./ /Hydroxide./ V Oxide. / / Chloride. / Description. Light, orange-yellow, impalpable powder; be coming darker on exposure; odorless; tasteless; insol. in water, or alcohol; sol. in HNO„ or HC1. Difference from, red oxide: When digested with solution of oxalic acid, it forms a white mercuric oxalate. Officinal Preparations. 1. Oleatum bydrargyri. 2. Ung. hydrar- gyri oxidi flavi. THE MERCURY SALTS. 153 Oleatum Hydrargyri.—Mercuric Ole ate. Made by dis- solving yellow oxide of mercury (10) in oleic acid (90), with the aid of heat, below 165° F. Unguentum Hydrargyri Oxidi Flavi. (Ointment of Yellow Oxide of Mercury.) Yellow HgO (10), incorporated with ointment (90). Avoid using metallic utensils. (HgO—215.7) Hydrargyri Oxidum Rubrum.—Red Oxide of Mercury. (Red Precipitate. Peroxide of Mercury. Red Mercuric Oxide.) Made by first forming a mercuric nitrate, by treating the metal with diluted HN03, and evaporating to dryness, when another equivalent of mercury is added, and the mixture heated till nitrous fumes cease to be evolved. (1) 3Hg + 8HN03 = 3Hg (H03)2 + N202 + 4H20. (Mercury.) /NitrleN / MercuricN /NitrogenX (Water.) \ Acid./ \ Nitrate. / V Dioxide./ (2) 2Hg(N03)2 -f- Hg2 Heat = 4HgO -{- 2N204. /Mercuric\ (Mercury.) /Mercuric\ / Nitrogen \ \ Nitrate. / \ Oxide. / VTetroxide./ Description. Heavy, orange-red crystalline scales, or a crystal- line powder, becoming yellow by trituration; odorless; tasteless; insol. in water or alcohol; sol. in HN03, or HC1. Impurities and tests. Nitrate: + Heat = dark color, and reddish fumes. Difference from yellow oxide: Digest with strong solution oxalic acid = no change in color in two hours. Officinal Preparations. Unguentum Hydrargyri Oxidi Rubri. (Ointment of Red Oxide of Mermiry.) Contains red HgO (10), in- corporated with ointment (90). Avoid using metallic utensils. (Hg(CN)2—251.7) Hydrargyri Cyanidum.—Cyanide of Mer- cury. (Mercuric Cyanide.) Made by dissolving HgO in IICN, also by boiling potassium ferrocyanide with solution of mercuric sulphate, and separating the cyanide by crystallization from alcohol. (1) 2HCJNT + HgO = Hg(CN)2 + H20. /HydroeyanicN /Mercuric\ /Mercuric \ (Water.) \ Acid. ) \ Oxide. ) \ Cyanide./ (2) 2K4Fe(CN)6 + 7HgS04 = 6Hg(CN)2 + Hg / Potassium \ / Mercuric \ /Mercuric \ (Mercury.) \Ferrocyanide./ V Sulphate./ V Cyanide./ + 4K2S04 + Fe2(S04)3. /PotassiumN / Ferric \ \ Sulphate. / \Sulphate.y Description. Colorless, or white crystals, becoming dark on ex- posure to light; odorless; bitter, metallic taste; neutral reaction; sol. in water (12.8), ale. (15). Impurities and tests. Mercuric chloride : -f- KI = red ppt. soluble in excess. 154 MANUAL OP PHARMACY. (Hg(Hg0)2S04—727.1) Hydrargyri Subsulphas Flavus.— Yellow Subsulphate op Mercury. Made by dissolving mercury in a mixture of H2S04, HN03 and water, forming a solution of normal mercuric sulphate (Hg2 -f- 2II2S04 + 2HN03 = 2HgS04 -f 3H20 + N203), which on being poured into boiling water, yields a precipitate of mercury subsul- phate, while acid mercuric sulphate remains in solution. Description. Heavy, lemon-yellow powder; odorless; almost tasteless; insol. in water, or alcohol; sol. in HN03, or HC1. (Basic Mercuric Sulphate. Turpeth Mineral.) (NIl2IIgCl—251.1) Hydrargyrum Ammoniatum.—Ammoniated Mercury. (White Precipitate. Mercur-ammonium Chloride.) Made by pouring a solution of HgCl2 into NH4OH, keeping the latter in slight excess; wash and dry the precipitate. HgCl2 + 2NH4OH = NH2HgCl + NH4CI -f 2H20. /Mercuric \ /Ammonium\ /Mercur-Aiumonium\ /Ammonium\ (Water). VChloride./ \ Hydroxide.) \ Chloride. ) V Chloride. / Description. White, pulverulent pieces; or, a white powder; odorless; tasteless; insol. in water or alcohol. Impurities and tests. Mercurous salt: -j- HC1 = not wholly solu- ble. Carbonate : -(- HC1 = effervescence. Lead: -J- acetic acid = Sol. + II2SO4 = white ppt. Officinal Preparation. Unguentum Hydrargyrum Ammonia- tum. (Ointment of Ammoniated Mercury.) Made by incorporating ammoniated mercury (10) with benzoinated lard (90). Liquor Hydrargyri Nitratis—Solution op Nitrate op Mercury. (Solution of Pernitrate of Mercury.) Made by dissolving mercury in diluted IINO3. (See Reaction under Red Oxide). Description. Colorless liquid; strong acid reaction; odor of IIN03; sp. gr. 2.100, contains about 50$ Hg(N03)2. Unguentu.u Hydrargyri Nitratis. (Ointment of Nitrate of Mercury. Citrine Ointment.) Made by treating lard oil at 158° F. with HN03 and heating till effervescence ceases; when cool, it is incorporated with solution of mercuric nitrate, made by the action of nitric acid on mercury. A very complex reaction takes place in this preparation; the fat is oxidized, N202 and N204 are evolved, and the olein of the oil con- verted to solid elaidin. (HgS—281.7) Hydrargyri Sulphidum Rubrum.—Red Sulphide op Mercury. (Cinnabar. Vermilion. Paris Red. Red Mer- curic Sulphide.) Made by melting mercury (40) with sulphur (8), and subliming. It has the same composition as native cinnabar. Description. Brilliant, dark-red, crystalline masses; or fine, bright, scarlet powder; odorless; tasteless; insol. in water, alcohol, HN03 or HC1; sol. in Nitroliydrochloric Acid, 8. ppting. PART III. ORGANIC PHARMACY. Relations of Pharmacy to Organic Chemistry. Organic Chemistry is the science which treats of carbon com- pounds. The term organic chemistry originally referred to the chemistry of compounds formed only in the bodies of animals and plants, but this erroneous idea was overthrown by the result of the experiments of Wohler in 1828, who produced urea by artificial means. Composition of Plants. All plants are composed mainly of woody fibre termed Cellulose or Cellulin, which represents the framework or cells (these cells are lined with a material called Lignin, which tends to harden them), also certain organic proximate principles, which, when further resolved, are found to consist of carbon, hydrogen and oxygen. When hydrogen and oxygen are present in the proportion in which they unite to form water, they are termed Carlo-hydrates. Some proximate principles are distinguished by containing nitro- gen, and some phosphorus or sulphur. Paints of Similarity. The existence of one or more proximate principles in excess, in any group of animal or vegetable products, generally adapts its individual members to certain methods of man- ipulation and uses in medicine, and constitutes strong features of resemblance among them. Substances in which a starchy matter predominates, to whiqb their utility is due, are classified as Farina- ceous; the Gums are associated with each other; the Narcotics, con- taining alkaloidal principles; the Aromatics, containing essential oils; the Resins, etc. The Proximate Principles of Plants may be divided into two classes, viz.; I. Nutritions or Inert. Comprising cellulose; starch; gums; sugars; fixed oils; fats, etc. II. Non-Nntritious and Poisonous. Comprising crystallizable and non-crystallizable neutral principles; vegetable acids; vegetable alkalies; essential oils; resins, etc. 156 MANUAL OP PHARMACY. THE CELLULIN GROUP. Cellulin in a nearly pure condition constitutes cotton, linen, and the best kinds of unsized paper, since the processes to which the woody fibre is subjected in these materials, separate the lignin and bodies which accompany it. Description. An inert, colorless (sometimes translucent), taste- less, odorless, organized substance; insol. in water, dilute acids, or alkalies. Its only solvent is Schweizer’s Solution, an ammoniacal solution of copper oxide, made by dissolving CuS04 (10) in water (100) and adding solution of potash (5-50); wash the precipitate, and dissolve in a 20$ sol. NH4OH. On treating with cone. H2S04, cellulose is converted into soluble cellulose or Dextrin, and on diluting and boiling this solution with water Glucose is obtained; by fusing with KOH it is changed into oxalic acid. Cellulose is officinal in the form of Gossypium. n Cellulose.—Cellulin. (C6Hi0O5) Gossypium.—Cotton. (Purified Cotton. Absorbent Cotton.) The hairs of the seeds of Gossypium herbaceum, and other species of Gossypium, freed from adhering impurities and deprived of fatty matter. Method of Purification. Cotton is boiled with solution potash or soda, and washed to remove the soap formed, expressed and immersed in a 5$ solution of chlorinated soda to bleach it, then washed again and treated with water acidulated with HC1, washed, expressed and dried. Loses 7% of its weight. Properties. When thrown on water, it absorbs moisture readily and sinks; the water should have a neutral reaction; inodorous, tasteless; insoluble except in Schweizer’s Solution. Tests to distinguish between Cotton and Linen fibre. 1. Boil with KOH; linen partakes of a deep yellow color within two min- utes, cotton remains white. 2. Tincture of Madder: With linen = yellowish red color, with cotton = light yellow. 3. Cone. H2S04; chars and destroys cotton in |-2 minutes, linen not as readily. 4. Olive oil; renders cotton transparent, linen is unchanged. 5. Microscopical examination; cotton fibres appear as flat, ribbon-like joints, linen fibres like long, straight, slender tubes. 6. Wool and silk may be distinguished from cotton and linen and all other carbo- hydrates, by treating with percliloride of tin, which bleaches the latter, while wool and silk are unchanged. Ofikinal Preparation. Pyroxylinum. Pyroxylinum.—Soluble Gun Cotton. (Collodion Cotton.) Cotton (1) is macerated with a mixture of HNO3(10) and H2S04 (12) for about ten hours, and washed with cold water to remove acid, then with boiling water, and finally drained and dried. It should be soluble in a mixture of alcohol one volume, and stronger ether three volumes. THE CELLULIN PRODUCTS. 157 The following reactions show the important kinds of pyroxylin that may be formed: (Cellulin.) (Nitric Acid.) (Nitro-Cellulin.) (Water.) (1) C12H20O10 + 2HNO3 = C12H1B(NO2)2O10 4- 2H20. (2) Ci2H2oOio -f- 4HN03 = Ci2Hie(NO2)4Oi0 4 4H20. (3) Ci2H2oOio -j- 6HN03 = Ci2Hi4(N02)sOio 4 6H20. (1) Non-explosive; insoluble in ether-alcohol. (2) Officinal. Slightly explosive; soluble in ether-alcohol. (3) Highly explosive; insoluble in ether-alcohol. Officinal Preparation. Collodium. Collodium.—Collodion. (Contractile Collodion.) Made by dissolving pyroxylin (4) in a mixture of stronger ether (70) and alcohol (26). Description. Colorless, slightly yellow liquid of a syrupy con- sistence, and ethereal odor. Leaves a thin, transparent, closely adhering him on evaporation. Officinal Preparations. 1. Collodium flexile. 2. Collodium stypti- cum. Collodium Flexile.—Flexible Collodion. Canada turpen- tine (5) and castor oil (3) are dissolved in collodion (92). Description. Appearance like collodium; produces a flexible, opaque him on evaporation, afterwards becoming transparent. Collodium Stypticum.—Styptic Collodion. (Xylostyptic Ether.) Made by dissolving tannic acid (20) in a mixture of alcohol (5), ether (20) and collodion (55). Prop. Styptic and htemostatic. COLLODIUM CUM CaNTHARIDE.—CANTHARIDAL COLLODION. (Blistering Fluid.) Made by exhausting powd. cantharides (60) by percolating with chloroform, distilling the percolate to (15), and dissolving in flex- ible collodion ft. (100). Description. A transparent, brownish-green liquid. Properties. Vesicant, and epispastic. Paper, another form of cellulin, is made from wood (spruce or poplar), straw, cotton, linen, hemp, jute, etc. Ledger paper, and the finest grades of writing paper are made en- tirely from linen rags; many of the cheaper grades of printing and wall papers contain clay, added to increase their weight, which however, renders them brittle. This admixture may he detected by ignition, when a heavy ash remains. Preparation. Wood is converted into a pulp as follows: After chipping and heating with steam at 120 lbs. pressure for 12 hours, it is blown upon a strainer by means of live steam, and washed with hot water; it is next boiled with soda, to remove all resinous and fatty matter, then washed and ground with water, drained, and treated as rag pulp. Rags are treated as follows: They are cut into small pieces, put Paper. 158 MANUAL OF PHARMACY. into a revolving iron cylinder and boiled with lime and water, resulting in the removal of all adhering impurities, and loosening of coloring matter; they are next placed in “ beating-engines,” and while mixed with water, are finely cut by revolving knives and at the same time bleached by the addition of chlorinated lime, and the lime fixed with H2S04. After draining the mass, it is passed into a Jordan engine (composed of an iron cylinder in which a conical wheel of knives revolves) where the mass is ground to a smooth pulp with water, forming a milky mixture which is repeatedly washed and drained upon a belt of wire-gauze, and passed between rollers which press the pulp down to the thickness of paper desired; it is then caught upon an endless sheet of felt, and by means of the latter carried over heated, revolving, iron cylinders, till completely dry, when it is cut into sheets of the desired size, [b.h.s.] There are three officinal medicated papers, viz.: Charta canthari- dis, Charta potassii nitratis, and Charta sinapis. These are made by impregnating paper with the medicinal ingredient in the form of mixture or solution. (See Part I. page 61.) Medicated Papers.—Charts. Parchment Paper. Made by immersing unsized paper made from rags, in sulphuric acid (sp. gr. 1.56-1.60) for a short time, and washing with diluted water of ammonia to neutralize any adhering acid, and finally with water. Parchment, parcliment-paper, bladder, skin, etc., have the property of separating crystalloid bodies from colloids by a process called Dialysis. (See Part I. page 43.) (H2C2O4.2H20—126) Oxalic Acid. Occurs combined with ammonium in guano, with calcium in a large number of plants, in rhubarb, curcuma, ginger, squill, orris, valerian, quassia, etc. Preparation. May be made by the action of nitric acid on sugar, molasses, or starch; but usually made from sawdust (cellulin) by heating with potash and soda on iron plates, forming oxalates of potassium and sodium; on treating with Na2C03 the potassium salt is washed out as K2CO3, the less soluble sodium oxalate.remain- ing. Milk of lime is then added, and NaOH and CaCsOi are formed, the latter precipitating, and on treating with H2804, oxalic acid is set free in solution and obtained by crystallization. (1) 2K2C2O4 + Na2C204 + 2Na2C03 = 2K2C03 -f 3Na2C204. /Potassium/ / Sodium / / Sodium / /Potassium / / Sodium / V Oxalate. / VOxalate./ VCarbonate./ VCarbonate./ VOxalate./ (2) Na2C204 + Ca(0H)a = 2NaOH + CaC204. / Sodium / / Calcium / / Sodium / /Calcium/ VOxalate./ VHydroxide./ VHydroxide./ VOxalate./ (3) CaC204 + H2S04 = CaS04 + H2C2O4. / Calcium/ /Sulphuric/ /Calcium/ (Oxalic Acid.) VOxalate./ V Acid. / VSulphate./ Description. Colorless, transparent, odorless crystals; strong, acid taste, and reaction: sol. in water, or alcohol. CELLULIN DECOMPOSITION PRODUCTS. 159 Impurities and tests. Sulphuric add: Ba(N03)2 = white ppt. Organic impurities: -(- II2S04 -(- boil = black color. Officinal as a Volumetric Solution. Antidote. Magnesia, chalk or some other calcium salt. Destructive Distillation of Cellulin. Acidum Aceticum. See Part II, page 68. (CH3OH) Methylic Alcohol.—Wood Alcohol. (Methyl Alcohol. Wood Naphtha. Pyroxylic, or Pyroligneous Spirit.) Found in the aqueous distillate obtained by the destructive distil- lation of wood, to the extent of 1%, together with acetic acid, acetone, etc. Separated by distilling with chalk to fix the acetic acid. Purified by distilling with calcium chloride, and again with water; rectified by carefully distilling with lime. Properties. A good sol- vent for shellac, etc. Methylated Spirit. A mixture of ethyl and methyl alcohol contain- ing 10# of the latter, and called Methylated Spirit is not held for duty in England. Pix Liquida.—Tar. An empyreumatic oleoresin obtained by the destructive distillation of the wood of Pinus Palustris, and other species of Pinus. Preparation. Billets of wood are piled in conical furnaces, and covered with a layer of earth and ignited above, with a draft regulated to keep up a slow combustion without flame; the tarry products collect in a ditch at the bottom of the pile. The pyrolig- neous acid and volatile oils of the wood are allowed to escape, thereby leaving charcoal and tar of a better quality than if the above were recovered. Description. Thick, viscid, semi-fluid; blackish-brown; heavier than water; transparent in thin layers; becoming granular (due to the presence of pyro-catecliin) or opaque by age; acid reaction; un- pleasant, empyreumatic odor and taste. Slightly sol. in water, sol. in alcohol, ether or chloroform, fixed and volatile oils, and solu- tions of soda or potash. Officinal Preparations. 1. Syrupus picis liquid*. 2. Unguentum picis liquid*. Sykupus Picis Liquids .—Syrup of Tar. Tar is washed with cold water by maceration, to remove acetic acid. The soluble con- stituents of tar are then extracted by boiling water, and sugar is dissolved in the filtered liquid. Bose: f § ss—f § ij. Unguentum Picis Liquids. (Ointment of Tar.) Incorporate tar (50) with suet (50), using heat. Oleum Picis Liquid.*®.—Oil op Tar. A volatile oil distilled from tar. Description. An almost colorless liquid when fresh, but soon acquires a dark, reddish-brown color; strong tarry odor and taste, acid reaction; sp. gr., about 0.970; sol. in alcohol. Pitch. Black Pitch. Pix navalis. The residue left after distilling the oil from tar. 160 MANUAL OP PHARMACY Charcoal prepared from soft wood. Made by heating wood to about 572° F., out of contact with air. Used as an ingredient in dentifrices. Prop. A great deoxidizer, absorbent and disinfectant. Carbo Ligni.—Charcoal. Wood Charcoal. Carbo Animalis.—Animal Charcoal. (Bone black. Ivory black.) Animal charcoal prepared from bone. Made by roasting bones de- prived of fat in iron cylinders; an ammoniacal liquid called bone- spirit, and a dark tar called bone-oil distil over, the charcoal and in- organic constituents remaining. Description. Dull black powder, or granular fragments; odor- less; nearly tasteless; insol. in water or alcohol. Officinal Preparation. Carbo Animalis Purificatus.—Puri- fied Animal Charcoal. Made by digesting animal charcoal with diluted HC1, decanting the liquid, and again digesting with water, washing thoroughly, draining, drying, and heating to redness. This process removes calcium phosphate and carbonate, and mag- nesium compounds. Description. Dull black powder: odorless; tasteless; insoluble. Impurities and tests. Phosphates: -f- HC1 (dil.); filtrate -f- NH4OH -f- test sol. magnesium = white ppt. Properties: Removes organic coloring matters from solution, also tannin, alkaloids, and some metallic salts. Creasotum.—Creasote. («peas—flesh; |cu-i save.) (Oil of Smoke). A product of the distillation of wood tar. The distillate sepa- rates into a heavy and light oily layer; the heavy oil is treated with Na2C03.and distilled, that portion of the distillate which is heavier than water is treated with KOH, which dissolves the crea- sote, separating eupion. By repeated fractional distillations of the solution, alternately treating with H2S04 and KOH, a pure product is obtained. Description. An almost colorless, or yellowish, oily, inflamma- ble liquid, becoming reddish yellow or brown on exposure to light; penetrating, smoky odor; burning caustic taste; neutral reaction; sp. gr. 1.035-1.085; sol. in water (80), abs. alcohol, ether, chloroform, benzin. Impurities. Carbolic acid. See page 161. Officinal Preparation. Aqua Creasoti (Creasote Water). A one per cent solution in distilled water. A liquid obtained during the distillation of coal tar between the temperatures of 170°-190° C. (338 -874° F.), containing carbolic and cresylic acids in variable proportions, together with other substances. Obtained directly by distillation of the dead oil derived from coal tar. Description. A nearly colorless or reddish-brown liquid; strong, disagreeable, empyreumatic odor, having a benumbing, blanching, and caustic effect on the skin or mucous membrane; neutral reaction. Acidum Carbolicum Crudum.—Crude Carbolic Acid. CELLULIN DECOMPOSITION PRODUCTS. 161 Impurities. Water: -f- equal vol. chloroform = separation; alka- lies: -f- litmus = blue color. (CeHsOH — 94) Acidum Carbolicum. — Carbolic Acid. (Phenol. Phenic Acid. Phenylic Acid.) A product of the distillation of coal tar between the temperatures of 180°-190° C. (356°-374° F.). Description. Colorless, needle-shaped crystals, acquiring a pink- ish tint, and becoming deliquescent on exposure; action on the skin same as the crude acid; neutral reaction; slightly aromatic odor resem- bling creasote; sweet taste (when diluted) with a slight burning after- taste. Forms 5% and 95% solutions with water, other proportions pro- ducing turbidity. Sol. in alcohol, ether, chloroform, glycerin, benzol, CS2, and oils. Crystals melt at 97°-107° F.; boil at 357°-366° F. Characteristic reactions of Creasote and Carbolic Acid. Creasote: -f- collodion (or albumen solution) = transparent solution. Carbolic acid: -f- collodion (or albumen solution) = gelatinous mass. Creasote: Sol. -f- sol. Fe2Cl6 = blue color changing to green and browrn, with brown ppt. Carbolic acid: Sol. -f sol. Fe2Cl6 = red solution, becoming violet-blue. Creasote: Splinter of fir wood dipped into the solution, and then into HN03 or HC1 = no reaction. Car- bolic acid: Under similar circumstances = first blue, then brown. On mixing equal volumes of 95% carbolic acid and glycerin, a clear mixture results, which remains clear on the addition of three volumes of water. (Creasote and cresylic acid produce turbidity.) Water is detected by the chloroform test. Officinal Preparations. Unguentum Acidi Carbolici.—(Oint- ment of Carbolic Acid.) Made by incorporating carbolic acid (10) with ointment ft. 100. (HCtHbOs—188) Acidum Salicylicum.—Salicylic Acid. Formerly prepared from oil of wintergreen, but at present from carbolic acid, which is converted into sodium carbolate and evapo- rated to dryness at a high heat in an atmosphere of C02, with the fol- lowing reaction: 2NaCeH60 + C02 = Na2C,H403 + C6H6(OH). / Sodium \ (Carbon \ f Sodium \ (Phenol.)1 VCarbolateJ VDioxide./ 'Salicylate./ The residue after solution, is decomposed by HC1, forming impure salicylic acid. Reaction: Na2C7H403 + 2 HC1 = HC,H503 + 2 NaCl. The acid is purified by solution in alcohol, filtration through ani- mal charcoal, and crystallization, or by subliming with steam. Description. Fine, white, light acicular crystals; free from car- bolic acid odor, but having a slight aromatic odor; sweetish and acrid taste; acid reaction; sol. in water (450r, alcohol (2,5), ether (2), chlo- roform (80). Test: With iron salts it produces a violet red color. Impurities and tests Hydrochloric acid: -j- AgNOs = white ppt. Organic matter, and iron: Evaporate solution = colored residue. Foreign organic matter: -(- cone. H2S04 = color. Carbolic acid: Sol. + KClOs + HC1 + NH4OH = red or brown tint. 162 MANUAL OF PHARMACY. Oleum Succini.—Oil of Amber. A volatile oil obtained by the destructive distillation of amber and purified by subsequent rectification. [Amber is a fossil resin ob- tained from a number of extinct coniferous trees found in Europe, Greenland and N. A.]. Description. Colorless, or pale-yellow, thin liquid; becoming dark and thick by age, and on exposure; empyreumatic and bal- samic odor; sp. gr. 0.920; sol. in alcohol; produces with fuming HN03, a brown resinous mass called artificial musk on account of its odor. A fossil formation produced by a peculiar decomposition or fermentation of buried vegetable matter, found below the surface of the earth. Coal. Theory of formation. 2C0Hi0Os = 5CH4 -f- 5C02 + C2. (Cellulin.) (Methane.) / Carbon \ (Carbon.) VDloxide./ The residue obtained as one of the secondary products of coal gas manufacture. By the action of various acids and alkalies on coal tar, the beautiful aniline colors are produced. Coal Tar. AMYLACEOUS PRINCIPLES AND THEIR PRODUCTS. Amylum.—Starch.—Wheat Starch. The fecula of the seed of Triticum vulgare. (N. 0. Graminacesp.) Starch has the same chemical composition as cellulose, CeHi0O5, but differs widely from it in physical properties. It exists in various parts of plants during some period of their growth, in tuberous and bulbous roots., but especially in the seed in minute cells which may be dis- tinguished by the aid of the microscope. Its usefulness in the seed as a storehouse of food for the plant, de- pends upon its conversion into grape-sugar by the action of the moisture and warmth of the soil, wThen it is readily assimilated by the developing plantlet. Occurrence. Starch occurs most abundantly in the following plants: Potato, barley, indian corn, rye, wheat, arrow-root, salep, Iceland-moss, sago and tapioca. Preparation. Made by macerating potatoes, wheat, or other grain in warm water (to which an alkali is sometimes added) until the outer coat softens; it is then ground or grated under water. The resulting soft mass is washed upon a sieve, when the starch granules pass through with the water, from which they separate on standing; finally drained and dried. The alkali water acts as a solvent for the gluten, but the latter is often removed by allowing the grain to un- dergo a slight fermentation. The quality of the starch depends upon the purity and quantity of the water used in washing. The envelope of the starch granule is insoluble in cold water, but is ruptured on the application of heat, so that the contents are ex- THE AMYLUM GROUP. 163 posed and become dissolved, hence starch is said to be insoluble in cold, but soluble in hot icater. Restoration. Musty and mouldy starch may be restored by washing well with water, and re-drying. Description. Irregular, angular, white masses, easily reduced to powder; odorless; tasteless; insol. in ether, alcohol or cold water. On triturating with cold water, the filtrate should have a neutral reaction. Test. On boiling with water, it yields a white jelly, having a bluish tinge, which on cooling acquires a deep blue color on the ad- dition of a solution of iodine (with bromine, a yellow or brown color results). Officinal Preparations. 1. Amylum Iodatum. 2. Glyceritum Amyli. Amylum Iodatum.—Iodized Starch. (Iodide of Starch.) Made by triturating iodine (5) with a small amount of water, gradually adding the starch under trituration till a uniform dark-blue color results, drying below 104° F. and powdering. Better results may be obtained by using ether in the place of water. This preparation decolorizes by the action of sunlight. Often used as a general antidote for poisons. Syrup of Iodide of Starch. (Unofficinal.) Made by dis- solving iodized starch in water, adding sugar, and heating till dissolved. Glyceritum Amyli. — Glycerite of Starch. (Plasma.) Made by rubbing starch (10) to a fine powder, then with glycerin (90) and heating to 284° F. (not above 291°) till the starch granules dissolve and form a translucent jelly. Use. An excellent excipient for most pill masses, and a valuable substitute for lard or ointment in compound ointments. Made by baking starch at about 500° F., or, by boiling starch with water acidulated with sulphuric or oxalic acid. Dextrin.—British Gum. (CeHioOa) Reaction. CisHsoOis + H20 -f- H2S04 = C6Hi206 (Starch.) (Water.) (Sulphuric Acid.) (Glucose.) + 2CflHi„05 + H28O4. (Dextrin.) (Sulphuric Acid.) A small quantity of glucose is also formed, which may be removed by treating with dilute alcohol, while the acid is neutralized by CaC03. Description. Exists in granular form, or an amorphous gummy mass; sol. in water, insol. in alcohol or ether. The solution is often used as a mucilage, and is employed for that purpose on postage stamps by the U. S. P. O. Dept. (Cr.H120G) Glucose.—Grape-Sugar.—Starch-Sugar. Exists naturally in the grape, and other fruit. Preparation. Made by boiling starch (100) with water (400) and sulphuric acid (5), until iodine ceases to produce a blue coloration. The free acid is neutralized with chalk, the filtrate clarified and 164 MANUAL OF PHARMACY. decolorized (by treating with clay and animal charcoal) and con- centrated in a vacuum pan. Solid Grape Sugar occurs in whitish, granular powder, or masses; glucose also occurs as a syrupy liquid. When made directly from corn it is termed Corn Syrup. Test for identity. Test-Solution of Potassio-Cupric Tartrate (simi- lar to Fehling’s Solution), which on boiling with a solution contain- ing glucose, deposits a brick-red precipitate {cuprous oxide). Fehling’s Solution. Dissolve 34.64 grams CuS04 in 200 cm3 distilled water, and mix with a cold solution of 200 grams tartrate of sodium and potassium in 600 cm3 solution of soda (sp. gr. 1.20) and dilute with water to one liter. Ten (10) cm3 of this solution are reduced by 0.05 grams of grape-sugar. SACCHARINE PRINCIPLES. (C12H22O11—342) Saccharum.—Refined Sugar.—Cane Sugar. The refined sugar of Saccharum officinarum. Cane-sugar exists in the sugar-cane, sugar maple, beet root, birch, palm, honey, sorghum, etc. Preparation. Made by crushing the sugar-cane and expressing its juice, then clarifying by boiling—a little lime being added to neutralize free acid,—straining, and concentrating by rapid evapo- ration, then cooling and transferring to perforated casks, to drain off the liquid portion. The solid portion is called raw or muscovado sugar, and the liquid product treacle or molasses. Refining. The raw sugar is dissolved in water, and the solution heated with blood, which acts as a mechanical clarifier. After straining, the liquid is filtered through animal charcoal. The color- less filtrate is concentrated in a vacuum pan (boiling at about 120° F.), and when of the proper density, cooled to crystallize, and placed in centrifugal machines to remove the mother-liquor from the crystals. The product constitutes the or loaf sugar, and the uncrystallizable mother-liquor is known as sugar-house molasses. Slightly discolored (yellow) sugar is made whiter by the addition of Prussian Blue, thereby producing a bluish white. Description. White, dry, hard, crystalline granules; odorless; purely sweet taste; neutral reaction. Soluble in water (0.5), alcohol (175), insol. ether. Impurities and tests. Insoluble salts, foreign matter, ultra- marine, prussian blue, etc.: Aq. or ale. solution deposits sediment on long standing. Grape-sugar, and inverted sugar: Sol. -(- AgN03 + NH4OH + boil = black ppt. Use. As a preservative for liquid preparations, and to mask the taste of unpleasant medicines. Officinal Preparation. Syrupus (and compound syrups). Syrupus.—Syrup. Sugar (65) is dissolved in water (35) using heat, and strained. Sp. gr. 1.310. Officinal Preparation. Syrupus Acacise (see Acacia.) THE SACCHARINE GROUP. 165 Made by heating cane-sugar to 392° F.; also prepared from infe- rior qualities of sugar, molasses or glucose. Used as a coloring agent. Caramel.—Burnt Sugar. (Ci2H1809). (CiaHajOn.HnO—360) Saccharum Lactis.—Milk Sugar. (Lactose.) A peculiar crystalline sugar, obtained from the whey of cow’s milk. Preparation. Made by removing the cream from milk, then on the addition of an acid the caseine is removed in a coagulated con- dition called curds. The liquid portion (or whey) is concentrated and allowed to crystallize on sticks or cords suspended in large tanks. Whiter crystals are derived by re-crystallization from an aqueous solution. Description. White, hard, crystalline masses, yielding a white powder, feeling gritty on the tongue; odorless; faint, sweet taste; neutral reaction; sol. in water (7), insol. alcohol, ether or chloro- form. Impurities and tests. Cane-sugar: -|- HaS04 = brown or black color, within an hour. A saccharine secretion deposited in the honey-comb by Apis mellifica (Honey Bee) (Class, Insecta; Order, Ilyrnenoptera). Ob- tained by draining the comb, thus producing virgin honey the purest article. A darker-colored honey is obtained by the use of pressure or heat. Composition. Contains about 80% sugar, representing about equal quantities of grape-sugar or dextrose (which renders honey granular) and fruit-sugar or levulose, which remains liquid. Description. A syrupy liquid, light-yellow or brown-yellow in color; gradually becoming crystalline by age or reduction of tem- perature; sweet, faintly acrid taste. Impurities and tests. Any admixture of glucose may be detected by testing for calcium sulphate. Starch: Boiled solution + I = blue color. Chlorides: -|- AgN03 = white ppt. Officinal Preparation. Mel Despumatum. — Clarified Honey. Heat honey on water-bath, and add a small quantity of cold water; the scum which arises and floats on the water can be poured off, free from all honey. Officinal Preparations. 1. Confectio rosse. 2. Mel rosae. [j. a.] Conpectio Ros^e.—Confection of Rose. Contains powd. red rose (8), powd. sugar (64), clarified honey (12). and rose-water (16). Mel Ros/e.—Honey of Rose. Powd. red rose is percolated with diluted alcohol, and mixed with clarified honey. Mel.—Honey. A peculiar, concrete substance prepared by Apis melliftca—Honey bee (Class, Insecta ; Order, Ilyrnenoptera.) Wax is secreted in thin scales about the abdomen of the honey bee, and is used in the for- Cera Flay a.—Yellow Wax. Beeswax. 166 MANUAL OF PHARMACY. mation of the hexagonal cells of the comb, in which the honey is afterwards deposited. How Obtained. By draining off the honey, and expressing the comb, or separating by means of centrifugal machines, melting in water, and running into moulds. Composition. Myricin, cerotic acid or cerin, cerolein, and aromatic and coloring matter. Description. Yellowish, or brownish yellow solid; agreeable, honey-like odor; faint, balsamic taste; brittle when cold, becoming plastic by the heat of the hand; fusing at 145°-147° F., insol. in water, sol. in boiling alcohol (300), partly sol. in cold alcohol, sol. in ether (35), chloroform (11), turpentine and oils; sp. gr. 0.955- 0.967. Impurities, adulterations and tests. Paraffin: 1. When melted wax congeals, it presents a smooth level surface; while the surface of paraffin, or of wax adulterated with paraffin, is concave. 2. When heated with 1I2S04, wax is completely destroyed, while paraffin (also mineral, or earth wax) is unaffected. Fats, fatty acids, Japan wax, resin: -fsol. NaOH-j-boil: lilt, -j-HC1 = ppt. Soap: boil: filt. -f- IIC1 = ppt. Officinal Preparations. 1. Ceratum Resin* (and compound cerates). 2. Unguentum. Ceratum Resina. — Resin Cerate. (Basilicon ointment.) Contains resin (35), yellow wax (15), lard (50), incorporated by heat. Officinal Preparation. Linimentum (Turpen- tine Liniment.) Melted resin cerate (65), oil of turpentine (35), are thoroughly incorporated. Unguentum.—Ointment. Contains lard (80), yellow wax (20), thoroughly incorporated by heat. Cera Alba.—White Wax. Yellow wax, bleached. Method. Melted wax is run through a trough upon wet revolving cylinders, where it congeals in thin ribbon-like sheets (or it is granulated) and is exposed to light and air, being frequently turned and moistened. The process is repeated until the wax is white. Sometimes bleached by the aid of chlorine, which is objectionable. Description. A yellowish-white solid, generally in the form of circular cakes; translucent in thin layers; slightly rancid odor; insipid taste; melts at 149° F.; sp. gr. 0.965-0.975. Impurities: Same as mentioned under yellow wax. Officinal Preparation. Ceratum (and compound cerates). Ceratum. (Cerate. Simple cerate.) Incorporate white wax (30), and lard (70), with heat. GUMS AND MUCILAGINOUS PRINCIPLES. 167 EXUDATIONS OF PLANTS. The Exudations of Plants represent the moisture derived from the soil and atmosphere, holding in solution some peculiar medicament found in the plant. GUMS. The gums are concrete substances that flow from trees and harden by spontaneous evaporation; nearly or wholly soluble in water, but the insoluble portion is also insoluble in alcohol. Gums are divided into two classes: True Gums. 1. Arabins: wholly soluble in water. 2. Bassorins. insoluble in, but swelling with water. Ceracins (cherry gums; etc.). Insoluble in water. Solutions of gums are called mucilages. A gummy exudation from Acacia Verek, and from other species of Acacia (N. O. Leguminosoz. Mimosa). Hob. Egypt, Smyrna, Turkey. Collection. The gum exudes spontaneously during the hot summer months, but is hastened by incisions. Description. Boundish tears, or angular fragments, having a glass-like fracture; opaque from numerous fissures, but transparent in thin pieces. The best quality is colorless or white, while inferior varieties have more or less of a yellowish or brownish tint; odorless; insipid mucilaginous taste; insol. in alcohol; sol. in water, forming a thick mucilaginous liquid, having an acid reaction. Incoinpatibles. Its solution yields gelatinous precipitates with solution subacetate of lead (but not with acetate of lead), and soluble silicates, ferric salts, and borax. Sp. gr. 1.355-1.525. Composition. A compound of arabic or gummic acid, with calcium, magnesium or potassium. Impurities and adulterations. Flour: Boil with water = gelatinous mass. Starch: + test-sol. iodine = blue color. Dextrin: Fehling’s Solution = red ppt.,due to the presence of glucose, always found in dextrin. The best test for purity and quality may be said to be the absence of color in the mucilage. Acacia is used in the preparation of many of the officinal mixtures and troches. Officinal Preparation. Mucilago Acacle. (Mucilage of Acacia.) Made by washing acacia (34) with cold water, and dissolving in water (66) by agitation. Best made by circulatory displacement. Used as a vehicle and an emulsifying agent. Officinal Preparation. Syrufus Ac acre. (Syrup of Acacia.) Mucilage acacia (25), syrup (75), mix. Should be freshly made when required for use. Acacia.—Gum Arabic. Tragacantha.—Tragacanth. A gummy exudation from Astragalus gummifer, and from other pecies of Astragalus. (N. O. Leguminosce. Papilionacm.) 168 MANUAL OF PHARMACY. Hub. Asia Minor, Persia. Composition. Contains a large amount of soluble gum (not iden- tical with arabin) and an insoluble gum, bassorin, and pectin. Description. Narrow, or broad ribbons; more or less curved or contorted, marked by parallel lines or ridges; color white or faintly yellowish; translucent, hornlike, tough, swelling in water to a gelatinous mass (which is tinged blue by test-solution iodine), the fluid portion of which is precipitated by alcohol. Used as an excipient in pill masses and troches. Officinal Preparation. Mucilago Tragacanthas. (Mucilage of Tragacanth.) Tragacanth is digested in a boiling mixture of glycerin (18) and water (76) and strained forcibly through muslin. The glycerin prevents it from drying out and rendering pills in- soluble, when used as an excipient. Beside the mucilages of acacia and tragacanth already referred to, three others are officinal. Mucilago Cydonii. (Quince-Seed Mucilage. Bandolin.) Made by macerating cydonium (2) with distilled water, and straining. Not precipated by borax. Muctlago Sassafras Medulla. (Mucilage of Sassafras-Pith.) Sassafras-pith (2), water (100), made by maceration. Not precip- itated by alcohol. Mucilago Ulmi. (Mucilage of Slippery Elm Bark.) Digest sliced elm bark (6) with boiling water (100). Precipitated by alcohol, and lead acetate. Flaxseed also produces a mucilage with water, but there is no officinal preparation. The mucilage is precipitated by alcohol, and lead subacetate. Syrupus Altileal—Syrup of Althaea. A mucilage is obtained by macerating cut althaea (4) with cold water. In forty parts of the drained mucilage, sugar (60) is dissolved by agitation. Mucilagines.— Mucilages. GUM RESINS. The gum-resins are exudations partly soluble in water, and partly in alcohol, insoluble in diluted alcohol, and form emulsions when triturated with water. Am mon i acum. —Ammonia c . A gum resin obtained from Dorema ammoniacum (N. 0. TJmbelli- ferce.) Ilab. Persia, Tartary. Composition. Contains about 4# of volatile oil, 70$ resin, 22$ gum, and 4$ bassorin or gluten. When fused with KOH, resorcin, oxalic acid and a fatty acid result. Description. Roundish tears; externally pale yellowish-brown, internally milk-white, of a peculiar odor; bitter, acrid, nauseous taste; yields a milk-white emulsion. Officinal Preparations. 1. Mistura ammoniaci. 2. Emplastrum am* moniaci. 3. Emp. ammoniaci cum liydrargyro. (See Mercury.) GUM RESINS. 169 Misttjra Ammoniaci. (Ammoniac Mixture.) Rub ammoniac (4) with water (100), in portions; when thoroughly mixed, strain. Emplastrum Ammoniaci. (Ammoniac plaster.) Digest am- moniac (100) in dilute acetic acid (140), until entirely emulsionized; strain and evaporate to plaster consistence. Asafcetida.—Asafetida. A gum resin obtained from the roots of Ferula norther and Ferula scorodosma (N. 0. Umbelliferce. Orthospermce.) Hab. Africa. Composition. 9# volatile oil (sulphide of ferulylor lasseryl C6Hn), 65# resin, and 25# gum. Description. Masses of whitish tears, imbedded in a yellowish gray, or brownish-gray sticky mass; internally, the tears are of a milk-white color, which changes to pink, and gradually to brown; persistent, alliaceous odor; bitter, acrid taste. When triturated with water, it yields a milk-white emulsion. Officinal Preparations. 1. Emplastrum asafcetidae. 2. Mistura asa- foetidae. 8. Pilulse aloes et asafcetidae. 4. Pil. asafcetidae. 5. Pil. galbani compositse. 6. Tinctura asafcetidae(20#). Emplastrum Asafcetidae. (Asafetida Plaster.) Asafetida (85), lead plaster (35), galbanum (15), and yellow wax (15), are thoroughly incorporated by the aid of alcohol and heat. Mistura Asafcetidae. (Asafetida mixture. Milk of asafetida.) Rub asafetida (4) with water (100) gradually added. PilulaE Aloes et Asafcetidae. (Pills of aloes and asafetida.) Each pill contains 11- grains, each, purif. aloes, asafetida, and soap. PilulaE Galbari CompositaE. (Compound pills of galbanum.) Each contains galbanum gr., myrrh 1| gr., gr., and syrup. PilulaE Asafcetidae. (Pills of asafetida.) Each pill contains asafetida 3 grs., and soap. A gum resin obtained from Garcinia Hanburii. AST. O. Guttiferce.) Hab. China, Siam. Description. Solid or hollow cylindrical sticks, called pipes (on account of the juice being conveyed into bamboo canes, drying out in the above form). Orange-red, or in powder bright yellow; odorless; acrid taste; the powder, sternutatory; yields bright yellow emulsion with water, and forms an orange-red solution with KOH, from which HC1 precipitates a yellow resin. Composition. Contains gambogic acid, which precipitates yellow with lead acetate, and brown with iron, or copper salts. Officinal Preparation. Pil. cathartic* comp. (See Calomel.) Cambogia.—Gamboge. Myrrha. —Myrrh. A gum resin obtained from Balsamodendron Myrrha. (N. O. Bur- seracce.) Hab. Africa. Contains 60# gum, 36% resin, 2\% vol. oil. Description. Roundish, or irregular tears, or masses ; brownish yellow or reddish brown; balsamic odor; bitter, acrid taste. Yields a brownish-yellow emulsion, with H2Q. 170 MANUAL OF PHARMACY. Officinal Preparations. Mistura ferri composite (see Iron). 2. Pil. aloes et myrrhse. 8. Pil. ferri comp, (see Iron). 4. Pil. galbani comp, (see Asafetida). 5. Tinct. aloes et myrrhse (10$ of each). 6. Tinct. Myrrhse (20$). Pilulse Aloes et Myrrhse (Pills of aloes and myrrh. Rufus’ Pills). Each contains purified aloes 2 grs., myrrh 1 gr., aromatic powder \ gr. Resins are solid or semi-solid exudations, insoluble in water, gen- erally soluble in alcohol, ether, chloroform and light hydrocarbons. RESINS. Natural Resins. M astiche. —Mastic. A concrete resinous exudation from Pistacia Lentiscus. (N. O. Terebinthacece. Anacardiece.) Hab. Grecian Archipelago. Composition. Volatile oil, mastichic acid 90% (a resin soluble in alcohol.) Description. Globular or elongated tears; about the size of a pea; pale-yellow, transparent; brittle, becoming plastic when chewed; resinous odor; turpentine taste. Officinal Preparation. Pilulse Aloes et Mastiches. (Pills of Aloes and Mastic. Lady Webster’s Dinner Pills.) Each contains puri- fied aloes 2 grs., mastic £ gr., and powd. red rose gr. Pix Burgundica.—Burgundy Pitch. The prepared resinous exudation of Abies excelsa. (N. O. Conferee.) Hab. N. Asia, N. Europe. Contains. A vol. oil and resin {abietic acid.) Description. Hard, gradually taking the form of the vessel in which it is kept; brittle, opaque or translucent; reddish-brown color; aromatic, not bitter taste; almost entirely insoluble in glacial acetic acid. Officinal Preparations. 1. Emplastrum Picis Burgundies:. 2. Emp. Picis cum. Cantharide. Emplastrum Picis Burgundicse. (Burgundy Pitch Plaster.) Bur- gundy pitch (90), and yellow wax (10), incorporated with heat. Emplastrum Picis cum Cantharide. (Pitch Plaster with Can- tharides. Warming Plaster.) Burg. Pitch (92), and cerate can- tharides (8); incorporate, using heat. Pix Canadensis.—Canada Pitch. (Hemlock Pitch.) The prepared resinous exudation of Abies Canadensis (N. O. Coni- fers.). Hab. Canada and No. U. S. Contains one or more resins and a small quantity of volatile oil (called oil of spruce, or oil of hemlock, Description. Resembles Burgundy Pitch. Officinal Preparation. Emplastrum Picis Canadensis. (Canada, or Hemlock Pitch Plaster.) Canada pitch (90), yellow wax (10); incor- porate, using heat. RESIN'S. The resin of the wood of Cuaiacum officinale (N. O. Zygophyllacece.) The heart-wood is officinal also, under the name of Guaiaci lig- num, and is used in the form of raspings. Contains 20-25$ resin. Hab. W. Indies, and coast of S. A. and Florida. Composition of Resin. Contains three acids (guaiacic 10$, guaiaretic 10$, and guaiaconic 70$), gum 4$, and impurities. Description. In masses, or sub-globular pieces; greenish, or reddish-brown color, depending on the age of the trees; feebly aromatic and acrid; powder grayish, becoming green on exposure; sol. in solution potash, and in alcohol. The alcoholic solution is colored blue by tincture of ferric chloride. Officinal Preparations. 1. Tinctura Guaiaci (20$). 2. Tinctura Guaiaci Ammoniata (20$). Guaiaci Resina.—Guaiac. Gutta Percha. The concrete exudation of Jsonandra Gutta. (N. O. Sapotaceas.) Hab. Malayan Peninsula, and Archipelago. Contains a white crystalline resin, called Albane, and yellow amorphous fluavil. Description. Grayish, or yellowish, hard, somewhat flexible, but scarcely elastic mass; plastic above 140° F., and very soft at 212° F. Insoluble in water or alcohol; sol. in chloroform, oil of turpentine, CS2, benzin or benzol. Officinal Preparation. Liquor Gutta-Perchse. (Solution of gutta- percha.) Made by dissolving gutta-percha (9) in chloroform (91), and clarifying by means of lead carbonate in fine powder (10), which carries the impurities to the bottom. Scammonium.—Scammony. A resinous exudation from the root of Convolvulus Scammonia (N.O. Convolvulacece.) Hab. Asia Minor. The root yields about 5$ of resin. Scammony should contain 80-90$ of resin; the finest grade is known in commerce as virgin scammony, the pure resin is termed scammonin. Description. Irregular, angular pieces, or circular cakes; greenish-gray, or blackish; peculiar cheese-like odor; slightly acrid taste; yields a greenish emulsion with water. Ether should dissolve at least 75$, and on evaporating the ether, the residue dissolved in hot solution of potash is not precipitated by dil. H2S04. Adulterations. Chalk: -(- dil. HC1 = effervescence. Starch : Cooled decoction -f- test-sol. iodine = blue color. Officinal Preparation. Resina Scammonii. (See Artificial Resins.) Artificial Resins. Artificial resins are extracted from the drug by means of a simple solvent, the resulting solution after concentration being poured into water, when the resin separates, falling to the bottom of the vessel; or, made by distilling the volatile oil from an oleo-resin. 172 MANUAL OF PHARMACY. The residue left after distilling off the volatile oil from Turpentine. Composition. The anhydride of abieiic acid, which is converted into the acid on agitation with warm diluted alcohol. Description. A transparent, amber-colored substance; hard, brittle, with a glossy and shallow conchoidal fracture; turpentine odor and taste: sp. gr. 1.07-1.08; sol. in alcohol, ether, fixed and volatile oils. Officinal Preparations. 1. Ceratum resinae (see Wax). 2. Em- plastrum resinae. (Resin Plaster. Adhesive Plaster.) Resin (14), lead plaster (80), and yellow wax (6); incorporate, using heat. Resina.—Resin. (Colophony.) Resina Copaiba.—Resin of Copaiba. (Copaivic Acid.) The residue left after distilling of the volatile oil from Copaiba. Obtained from Jalapa, the tuberous root of Exegonium Purga, which should assay not less than 12% resin. Powdered Jalap is percolated with alcohol till exhausted, and the percolate reduced to a syrupy consistence and poured into cold water. The resin subsides, while the water holds in solution the sugar and other principles. Description. Partly soluble in ether; insol. in CS2, soluble in NH4OH (50), and on evaporation the residue dissolves in water. The ammoniacal solution should not gelatinize on cooling, and should not be precipitated by an acid. Resina Jalaive.—Resin of Jalap. Process identical with that for resin of jalap, except that the water employed is acidulated with 1% of HC1. Description. Grayish white, with a tinge of yellow. Partly soluble in ether; the residue after solution in KOH is precipitated by HC1. Resina Podophylli.—Resin of Podophyllum. Resina Scammonii.—Resin of Scammony. Powd. scammony is exhausted by digestion, using boiling alco- hol, but otherwise treated like jalap. Soluble in ether. Officinal Preparation. Extractum colocynthidis compositum. (Compound extract of colocynth.) Contains extract of colocynth (16), aloes (50), cardamom (6), resin scammony (14), and powd. soap, thoroughly incorporated, dried and powdered. Officinal Preparation. Pil. catharticse comp. (See Calomel.) OLEO-RESINS. The Oleo-Resins are resins combined with a volatile oil; obtained either as an exudation, or derived from the portion of the plant in which they exist, by means of a solvent. Natural Oleo-resins. Terebinthina.—Turpentine. (Crude Turpentine.) A concrete oleo-resin obtained from Finns Australis, and from other species of Pinus. (N. O. Conifer*.) Hab. Southern United States. OLEO-RESmS. 173 A volatile oil distilled from turpentine. Description. Thin, colorless liquid; characteristic odor and taste; neutral, or faint acid reaction, sp. gr. 0.855-0.870; sol. in alcohol (6); explodes with bromine or iodine, and takes fire if brought in contact with a mixture of HN03 and H2S04. Officinal Preparations. 1. Linimentum Cantharidis. 2. Linimen- tum Terebinthinse. Linimentum Cantharidis. (Cantharides Liniment.) Digest can- tharides (60) with oil turpentine (100) for three hours; strain and add q.s. oil turpentine ft. (100). Linimentum Terebinthinse. (Turpentine Liniment.) Made by mixing resin cerate (65), and oil of turpentine (35). Oleum Terebinthin.e. (Oil of Turpentine.) Terebinthina Canadensis. (Canada Turpentine. Balsam Fir. Canada Balsam.) The liquid oleo-resin obtained from Abies Balsamea. (N.O. Co a if era.) Hob. 1ST. A. Description. Yellowish, or faintly greenish, transparent, viscid liquid of an agreeable terebinthinate odor; bitterish, slightly acrid taste; soluble in ether, chloroform, or benzol. Copaiba.—Copaiba Balsam. (Copaiva.) The oleo-resin of Copaifera Langsdorfii, and other species of Copaifera. (N. O. Legummosce.) Hub. So. America. Description. A transparent or translucent, viscid liquid; pale yellow to brownish yellow; peculiar, aromatic odor; bitter and acrid taste; sp. gr. 0.940-0.993. Soluble in abs. alcohol. Impurities and tests. Turpentine: -f- heat = turpentine odor. Fixed oils: After distillation, a resin not hard or friable remains. Ourjun balsam: Solution in CS2 + mixture of H2S04 and HN03 = purple, or violet color. Officinal Preparation. Massa Copaiba.—Mass of Copaiba. (Pill Copaiba.) Copaiba (94), magnesia (6); mix intimately and set aside to form a pilular mass. If a pilular consistence does not re- sult in 8 or 10 hours, a deficiency of water in the copaiba may be in- ferred. This difficulty may be avoided by shaking the oleo-resin with 5$ of water, and after standing for a time, decant from the uncombined water. The Derived Oleo-resins are made by percolating the powdered drug with stronger ether till exhausted; the residue left on evapor- ation of the solvent is the oleo-resin. The following six are officinal: Oleoresina Aspidii (yield Capsici (yield about 4$); Cubebte (yields 18-25$); Lupulin (yield 50$); Piperis (yield 5$); Zingiberis (yield 5-7$). Emplastrum Capsici. (Capsicum Plaster.) Melted resin plaster is thinly spread on muslin, and when cooled, a thin coating of oleo- resin capsicum is applied by means of a brush. Each sq. inch should contain one-fourth grain oleo-resin. Derived Oleo-resins. 174 MANUAL OF PHARMACY. Trochisci Cubeile. (Troches of Cubeb.) Each contains | grain oleo-resin cubeb, combined with oil of sassafras, extract of glycyr- rhiza, powdered acacia and syrup tolu. BALSAMS. Balsams are oleo-resins or gum-resins, containing either benzoic or cinnamic acid, or both. A balsam obtained from Myroxylon Pereirce. (N. O. Leguminosce.) Hab. Cent. America. Constituents. Cinnamic and benzoic acids, resin 32$, benzylic benzoate and cinnamate 60 %, and stilbene. Description. A thick, brownish-black liquid ; syrupy consis- tence; smoky, but agreeable balsamic odor; warm, bitter and acrid taste; sp. gr. 1.135-1.150; sol. in alcohol (5); miscible with absolute alcohol, chloroform, and glacial acetic acid. Impurities and tests. Fixed oils, and alcohol: -f- equal vol. benzin or water=diminished volume. Other adulterations: copaiba, gurjun balsam, rosin, turpentines, storax and alcohol. Balsamum Peruvianum.—Balsam Peru. Balsamum Tolutanum.—Balsam of Tolu. A balsam obtained from Myroxylon Toluifera (N.O. Leguminosce.) Hab. So. America. Constituents. Cinnamic and benzoic acids, amorphous resin, ben- zylic ether of cinnamic and benzoic acids, toluene 1$, and toluol. Description. Yellowish or brownish-yellow semi-fluid or nearly solid mass; brittle when cold; agreeable balsamic odor; mild arom- atic taste. Its alcoholic solution has an acid reaction; almost insol. in water and benzine. Adulterations. Turpentines (sol. in CS2), copaiba and castor oil. Officinal Preparations. 1. Syrupus Tolutana. 2. Tinctura Tolutana (10$). Syrupus Tolutana (Syrup of Tolu). Digest Tolu (4) with sugar and water at 180° F. for two hours; cool and strain ft. 100. [An objectional method, yielding an unsightly preparation.] Styrax.—Storax. (Liquid Storax). A balsam prepared from the inner bark of Liquidambar orientalis. (N. O. Hnmamelacece.) Hab. Asia Minor. Constituents. Styrole (or cinnamin), styracin, cinnamic acid, ben- zoic acid, storesin, and two resins. Description. Semi-liquid, gray, sticky, opaque; agreeable odor; balsamic taste; sol. in warm alcohol. Officinal Preparation. Tinct. benzoinii composita. Benzoinum.—Gum Benzoin. (Gum Benjamin.) A balsamic resin obtained from Styrax Benzoin. (N. O. Styracem.) Hab. E. Indies and China. Constituents. Benzoic acid (12-20$), but no cinnamic acid; vola- tile oil, and several resins. BALSAMS. 175 Description. Masses of yellowish-brown tears (internally milk white) or reddish-brown mass mottled from the presence of whitish tears (the number of whitish tears diminishing as the trees become old). Almost wholly soluble in warm alcohol (5), and solution of potassa. When heated, fumes of benzoic acid are given off; slight aromatic taste, agreeable balsamic odor. To detect Cinnamic Acid: Boil with milk of lime; the hot filtrate should not evolve the odor of HCN on adding test solution of potass, permanganate. Officinal Preparations. 1. Adeps benzoinatus. 2. Tinct. benzoinii (20%). 3. Tinct. benzoinii compositse. Adeps Benzoinatus.—Benzoinated Lakd. (Ointment of Ben- zoin.) Made by suspending powdered benzoin (2) in melted lard (100), for two hours at 140° F., straining and stirring while cooling. Used in preparing many of the compound ointments. (HC7H502—122) Acidum Benzoicum.—Benzoic Acid. (Flowers of Benzoin.) Occurrence. Found in benzoin, balsams tolu and peru, storax and other resinous exudations. Preparation. Made by subliming benzoin, and allowing the vapors to pass through a cone of filter paper into a condenser, or by decomposing a solution of benzoate of sodium or calcium with HC1, and purifying the resulting crystals. Most of the benzoic acid of commerce is, however, derived from urine or tar products. The urine of cattle or horses is treated with lime in excess and evaporated; the resulting calcium hippurate is decomposed with HC1, forming impure hippuric acid, which after purification and subsequent boiling with HC1, produces the following result. Reaction. C9H9N03 + H20 = C,H602 + C2H5N02. /'Hippurlc\ (Water.) /'Kenzoicx (Glycocoll.) \ Acid. ) \ Acid. ) When made from Naphthalene Ci0He (a derivative of coal tar), this substance is treated with HN03, producing phthalic acid, C8II604, which is converted into a calcium salt, and on mixing with excess of Ca(OH)2 is decomposed into calcium carbonate and benzoate; from the latter, benzoic acid is liberated by treating with HC1. Description. White, lustrous scales or friable needles, perma- nent in air; slight aromatic odor of benzoin; warm, acid taste and reaction ; sol. in water (500), alcohol (3), ether (3), chloroform (7) and CS2. Test. The neutral salts produce flesh-colored precipitates with dilute solutions of ferric sulphate. Impurities and tests. Chlorobenzoic add: On igniting in a loop of platinum wire with cupric oxide = greenish color. Cinnamic Acid: See Benzoin for test. > The seed of Hordeum distichum, caused to enter the incipient stage of germination by artificial means, and dried. Maltum.—Malt. (Barley Malt.) 176 MANUAL op phaemacy. Made by soaking barley in water and placing in heaps, when heat is spontaneously generated and germination takes place; the germ, (or sprout) having acquired the desired length, the grain is quickly dried, and becomes malt. During the germination of all seeds, either by natural or artificial means, a peculiar substance is developed, known as diastase, a body which, like piyalin, possesses the properties of converting starch into dextrin and glucose. Officinal Preparation. Extractum Malti. . (Extract of Malt.) Made by macerating malt with water and digesting with more water below 130° F., expressing, and evaporating the liquid to a thick honey consistence. FERMENTATION. The term fermentation refers to several processes of decomposition dependent on the presence of a certain substance or a compound called a ferment, which does not enter into any chemical composi- tion with the fermenting body, and is capable of producing an un- limited quantity of products. Kinds. There are various kinds of fermentation; the conversion of starch into dextrin or sugar by diastase is called saccharine fermen- tation; the transformation of milk sugar into lactic acid by casein is termed lactic fermentation; the changing of cane-sugar into mucus and mannit by proteids is known as muck fermentation; the produc- tion of butyric acid from milk sugar and lactic acid is designated bu- tyric fermentation; the production of alcohol from grape- or fruit- sugar by the action of yeast signifies alcoholic or vinous fermentation; the oxidation of alcohol into acetic acid is acetic fermentation. Other kinds of fermentation may be represented by the action of pepsin on albumen, piyalin on starch, pancreatin on fats, emulsin on glucosides, etc. Alcohol is produced by the fermentation of grape sugar. Cane- sugar is unfermentable until it has been inverted by the action of di- luted acids or a ferment. Preparation. Nearly all alcohol is derived from amylaceous substances, such as corn, rye. potatoes, etc., which are mashed with water, and on the addition of malt, by the influence of its diastase, the starch of the grain is converted into maltose. ALCOHOL. Then by the action of maltose upon more starch, glucose is ob- tained. Reaction. SCeHioOs -|— H2O — C12H22O11 —(— CeHmOs. (Starch.) (Water.) (Maltose.) (Starch.) Reaction. C12H22O11 -j- CeHioOs —)— 2HaO — 3C6H12O6. (Maltose.) (Starch.) (Water.) (Glucose.) On the addition of yeast to the mixture, which must be kept at a temperature of 64°-820 F., the yeast-plant (saccharomyces cereviske) converts the grape-sugar into alcohol and carbonic anhydride. FERMENTATION DERIVATIVES. 177 Reaction. C6H1206 = 2C2H5OH -(- 2C02. (Glucose.) (Alcohol.) (Carbon Dioxide.) There is also produced at the same time glycerin, fusel oil, succinic acid, etc. On distilling the fermented liquid, a weak spirit called crude whiskey is obtained. Preparation of Liquors.—If the mash is made of potatoes or grain, the distilled spirit is termed whiskey, and contains amylic alco- hol, oenanthic and other ethers, to which the odor is due; if distilled from wine, brandy is obtained—odor due to oenanthic, propylic and other ethers; when distilled from fermented molasses, rum is obtained —odor due to butyric acid; on distilling spirits with juniper berries, gin is obtained. Purification of Alcohol. To obtain pure alcohol, the crude whiskey is leached through charcoal which absorbs most of its fusel oil, and sometimes distilled with certain chemicals (AgN03, K2Mn208, etc.) with a view to further destroying the remaining fusel oil. The spirit is concentrated by distillation in a column-still, thereby remov- ing the last traces of fusel oil. and most of the water. Absolute Alcohol. To obtain absolute alcohol, the strong alcohol is treated for some time with lime, chloride of calcium, or some other deliquescent salt for the purpose of removing water, and afterwards carefully distilled. Absolute alcohol must be kept in well-corked bot- tles, on account of its great affinity for moisture of the atmosphere. (C2H5OH—46) Alcohol.—Ethyl Alcohol. A liquid composed of 91$, by weight, (94$ by volume) of ethyl al- cohol, and 9$ weight, (6$ by volume) of water. Sp. gr. 0.820 at 60° F„ or 0.812 at 77° F. Description. A transparent, colorless, volatile liquid, with a char- acteristic, pungent and agreeable odor, and burning taste; neutral re- action; boils at 78° C. (172.4° F.), burns with blue flame, without smoke. Impurities and tests. Fusel oil: -|- equal volume water -f- \ vol. glycerin; on wetting a piece of blotting paper with the mixture, and allowing the alcohol vapor to disappear, an irritating or foreign odor remains. Amyl alcohol: Evap. to -1 its vol.: add equal vol. H2S04 = reddish color. Methyl alcohol, aldehyd and oak-tannin: -f- equal vol. liq. potassa = dark color. Methyl alcohol: Digest with lead carbon- ate and filter; distil filtrate on water-bath; first distillate -(- K2Mn20s — no color. Foreign organic matter, fusel oil, etc.: -j- test solution AglSTOa and exposure to direct sunlight for one day = opalescence. Officinal Preparations. Alcohol Dilutum.—Dilute Alcohol. Mix alcohol (50) with water (50).—Sp. gr. 0.928 at 60° F., or 0.920 at 77° F. Contains ethyl alcohol 45 5$ by weight, or 53$ by volume. To prepare diluted alcohol from alcohol of any higher per cent, di- vide the percentage by weight of the stronger by 45.5 and subtract one from the quotient. The remainder represents the number of parts of water to be added to one part alcohol. Proof Spirits. Dilute alcohol differs from the United States 178 MANUAL OF PHARMACY. Proof Spirits, the latter containing only 50# alcohol by volume. Sp. gr. 0.936 at 60° F. A peculiar alcohol derived from fermented grain or potatoes, by continuing the process of distillation after the ethyl alcohol has ceased to distil. Use. Used in the manufacture of certain alkaloids, on account of its great solvent power, also as a source of valerianic acid and various flavoring ethers. (C5H11OH—88) Fusel Oil.—Amylic Alcohol. A pale-amber, or straw-colored alcoholic liquid, made by ferment- ing the unmodified juice of the grape, free from seeds, stems and skins. During the fermentation of grape-juice, if the latter contains only a limited amount of sugar, sufficient to produce by its decomposition 16# or less of alcohol, a dry wine is obtained; but if fermentation ceases before the sugar is entirely decomposed, a sweet wine results, and if the wine is bottled before fermentation is completed a sparkling wine will be obtained, effervescence being due to the presence of C02. During grape juice fermentation, as the alcohol increases, the tar- trates of potassium and calcium becomes less soluble and are depos- ited in crusts, called argots (see Tartaric Acid). Description. A full, fruity, agreeable taste, without excess of sweetness or acidity ; pleasant odor. Should contain 10-12# of absolute alcohol by weight Impurities and tests. Tannin: Dilute and add Sol. Fe2Cl« = dark brown color. On evaporating and drying, it should leave not less than 1.5# nor more than 3# residue. Officinal Preparation. Vinum Album Fortior.—Stronger White Wine. Mix white wine (7), alcohol (1). Contains 20-25# absolute alcohol (weight). Used in preparing the eleven officinal medicated wines. Vinum Album.—White Wine. Vinum Rubrum.—Red Wine. A deep-red, alcoholic liquid, made by fermenting the juice of colored grapes in the presence of their skins. Description. A full, fruity, moderately astringent taste, with- out decided sweetness, or excessive acidity; pleasant odor. Con- tains 10-12# alcohol (weight). Should yield 1.6-3.5# dried residue. Impurities: aniline colors. (H2C4H406—150) Acidum Tartaricum.—Tartaric Acid. Occurrence. Found either free or in combination with bases, in grapes, tamarinds, sumach berries, pineapples, and other acidu- lous fruits. Preparation. Acid tartrate of potassium is deposited in wine casks during the fermentation of grape juice in crystalline crusts called crude tartar or argols, composed of neutral calcium tartrate, acid potassium tartrate, coloring and extractive matter, yeast and other vegetable fragments. This crude tartar is dissolved in water, FRUIT ACIDS. 179 chalk is added, forming calcium tartrate which precipitates, leaving neutral potassium tartrate in solution. Reaction. 2KHC4H408 + CaCOs = K2C4H406 /Acid PotassiumX / Calcium \ /Neutral PotassiumN ( Tartrate. / (Carbonate.) ( Tartrate. ) + CaC4H406 -f H20 + C02. /Calcium \ (Water.) / Carbon \ (Tartrate.) (Dioxide.) The calcium tartrate is decomposed with H2S04. Reaction. CaC4H406 + H2S04 = CaS04 -j- H2C4H406. /Calcium \ /Sulphuric\ / Calcium \ (Tartaric Acid.) \Tartrate.) \ Acid. ) (Sulphate./ Calcium sulphate subsides, tartaric acid remaining in solution. The neutral potassium tartrate remaining in solution in the early stage of the process, is converted to CaC4H406 by the addition of CaCl2. Reaction. K2C4H406 + CaCl2 = CaC4H406 + 2KC1. /Potassium : / Calcium \ /Calcium \ /PotassiumX V Tartrate. ) ( Chloride.) (Tartrate.) ( Chloride. ) The precipitated calcium tartrate is decomposed by H2S04 as above, tartaric acid remaining in solution, and obtained by crystal- lization. Purified by re-crystallization, yielding colorless crystals. Description. Nearly or entirely colorless, transparent crystals; odorless; purely acid taste; acid reaction; sol. in water (0.7), alco- hol (2.5), ether (23). Ted for identity. Aqueous solution -(- sol. potassium acetate -f- alcohol = white crystalline ppt. Impurities and tests. Lead or copper: -j- II2S = black colora- tion. Copper: Ash -(- NH4OH = blue color. Lead, copper, iron: -j- (NH4)2S = black coloration. Sulphuric acid: -j- HC1 -j- BaCl2 — ppt. within five mins. Source. Lemon, lime and other fruits of the Citrus family. Preparation. The expressed juice of the fruit is clarified by ebullition, but if decayed fruit is used, it is allowed to undergo vinous fermentation. After decantation and straining, chalk is added in excess, also some milk of lime. Calcium citrate is formed, and being less soluble in hot than in cold water, the mixture is heated to boiling, and while hot the clear liquid is drawn off from the precipitated salt, which is washed with boiling water to remove extractive matter. The calcium citrate is then decomposed by diluted H2S04 in slight excess; calcium sulphate precipitates, citric acid remaining in solution. The solution is decanted, concentrated by evaporation, and allowed to crystallize in lead-lined tanks. (H3C6H507.H20—210) Acidum Citricum.—Citric Acid. (1) 2H3C6H607 -(- 3CaC03 — Ca3(CeH507)2 -(- 3H20 -|- 3C02. (Citric Acid.) / Calcium \ /CalciumX (Water.) / Carbon \ (Carbonate.) ( Citrate./ (Dioxide.) (2) Ca3(C6H607)2 + 3H2S04 = 3CaS04 + 2H3C6H607. (Calcium Citrate.) /Sulphuric: /Calcium \ (Citric Acid.) ( Acid. ) (Sulphate.) 180 MANUAL OF PHARMACY. The crystals are purified by re-dissolving, filtering through animal charcoal and re-crystallizing. Description. Colorless crystals, deliquescent in moist air; ef- florescent in warm air; odorless; agreeable, purely acid taste; acid reaction; sol. in water (0.75), alcohol (1), ether 48. Test. On adding an aqueous solution to lime-water, a clear mix- ture results until boiled, when a white precipitate separates which is nearly all re-dissolved on cooling. Impurities and tests. Tartaric and oxalic acids: Sol. acid -}- sol. potass, acetate -f- equal volume alcohol = cloudy mixture. Tartaric acid (1$ or more): Sol. acid -f- sol. potass, bichromate = dark color within 5 mins.; also, potass, permanganate gives dark ppt. of per- oxide of manganese. Lead and copper: —|- 1I2S = dark ppt. Cop- per: ash NH401I = blue color. Lead, copper, iron: 4~ (N1I4)2S = black color. Sulphuric acid: BaCl2 = white ppt. Officinal Preparation. Syrupus Acidi Citrici. (Syrup of Citric Acid.) Contains spirit of lemon (4), syrup (980), citric acid (8), water (8). Spiritus Vint Gallici.—Brandy. An alcoholic liquid obtained by the distillation of fermented grapes, and at least four years old. During the ageing process, the fusel oil becomes converted into several fragrant ethers, principally cenanthic, acetic and propylic. Description. Pale-amber color; distinctive taste and odor. Contains 89-47$ (weight) alcohol, 46-55$ (volume). Impurities and tests. Fusel oil: By evaporating on a water bath, the last portions have a harsh disagreeable odor. Excess of solid matter: Yields more than 0.25$ dry residue. Sugars, glycerine, svices: Taste. Spiritus Frumenti.—Whiskey. An alcoholic liquid obtained by the distillation of fermented grain, usually corn, wheat, or rye, and at least two years old. Process. Raw whiskey (see alcohol) is kept in barrels for two years, when it acquires mellowness and improves in flavor, due to the formation of certain compound ethers, by the oxidation of the fusel oil. Description. Amber color; distinctive taste, and odor. Contains 44-50$ (weight) alcohol, 50-58$ (volume). Impurities: same as under brandy. ALCOHOL DECOMPOSITION PRODUCTS Preparation. On mixing alcohol 'with H2S04 in a still, and heating between 266“-280° F., the following decomposition takes place: ((C2H5)20) —Ether. Sulphuric Ether. Reaction. C2H6OH -f H2S04 = C2H6HS04 + H20. (Alcohol) /Sulphurlc\ /Ethyl-sulphuric or\ (Water.) \ Acid. ) \ Sulphovinic Acid./ More alcohol is then added and heat applied, when ether forms, and H2S04 is reproduced. ALCOHOL DECOMPOSITION PRODUCTS. 181 Reaction. C2H5HSO4 -f- • C2H5OH = (C2H5)20 + H2S04. / Ethyl sulphuric\ (Alcohol.) (Ether.) /SulphuricX V Acid. ) \ Acid. ) The distillate is carried through a solution of potash to neutralize any acidulous vapors, and finally through a series of fractional con- densers where alcohol vapors are condensed and returned by a tube into the still, while the ether vapors pass into a final condenser. Description. Sp. gr. 0.750; contains about 74$ ethyl oxide ((C2H5)20) and about 26$ alcohol, containing a little water; sol. in water (5 vols.) See yEther fortior. Officinal Preparation.—Spikitus (Spirit of Ether.) Contains ether (30), and alcohol (70). Represents the Compound Spirit of Ether of the German Pharmacopoeia. ASther Fortior.—Stronger Ether. (Washed Ether.) Made by washing ether with water to remove alcohol, decanting and distilling the ethereal layer with lime and calcium chloride, thereby removing the remaining water and most of the alcohol. Description. A thin, very diffusive, clear, colorless liquid; characteristic odor; burning, sweetish taste; neutral reaction; sol. in water (8), alcohol, chloroform, and the light hydrocarbons; boils at 98.6" F.; highly inflammable; contains 94$ of ethyl oxide and 6$ alcohol; sp. gr. 0.725. Impurities and tests. Adds: -j- litmus = red color: Foreign mat- ter: Leaves fixed residue with odor. Alcohol: 10 cm3 ether fort. -)-10 cm3 glycerine; the ethereal layer = less than 8.6 cm3. Stronger ether should boil actively in a test tube, when held in the hand, on addition of pieces of broken glass. Officinal Preparation. Spiritus AItheris Compositus.—Com- pound Spirit of Ether (Hoffmann’s Anodyne). Contains, stronger ether (80), alcohol (67), and ethereal oil (3). Often adulterated with light oil of wine, or castor oil. Oleum ASthereum.—Ethereal Oil. (Heavy Oil of Wine.) (C2H6)2S04, (C2II4)2S03 = c\nlt,s2o7. Made by distilling a mixture of alcohol and H2S04 between 150°-157° C., (302°-314.6° F.), until the yellow liquid ceases to come over, and a black froth forms in the retort. The ethereal layer of the distillate is separated and exposed to air for 24 hours in a cap- sule, drained on a wet filter and washed with water, again drained and mixed with an equal volume of stronger ether. Reactions. On heating alcohol with sulphuric acid, svlphomnic acid is produced (as shown under Ether), and on distilling at the temperature designated in the presence of uncombined H2S04 and alcohol, ether and water are volatilized, followed by S02, ethylene or olefiant gas (C2H4), and heavy oil of wine. The distillate finally contains an aqueous solution of S02, and a yellowish ethereal layer of heavy oil of wine. By exposing the ethereal portion of the distillate to the air, ether evaporates, while the oil with some acid watery liquid remains. After properly washing the oil, it is dissolved in an equal volume of 182 MANUAL OF PHARMACY. stronger ether, to avoid spontaneous, decomposition, and a separ- ation into two liquids. Description. Transparent, nearly colorless, volatile liquid; pe- culiar, aromatic, ethereal odor; pungent, refreshing, bitterish taste; neutral reaction. Sp. gr. 0.910 Officinal Preparation. Spiritus aetheris comp, (see JPAhir fortior.) (C2H5C2H302) .Ether Aceticus.—Acetic Ether. (Acetate of Ethyl.) Made by distilling a mixture of alcohol and H2S04 with dehydrated sodium acetate. "The distillate contains acetic ether, alcohol, water and acetic acid; the latter is removed by treatment with chalk, forming calcium acetate in solution. Dried calcium chloride is added, and the mixture distilled; acetic ether separates from the distillate, is decanted and rectifled by re-distillation. Reaction. Sulphovinic acid is first formed, and on rectifying with sodium acetate, the following results: C2H5HS04 + NaC2H302 = NaHS04 -f C2H5C2H302. /Sulphovinie \ /Sodium \ /Acid Sodium\ (Ethyl Acetate.) \ Acid. ) VAcetate./ V Sulphate. ) Description. Transparent and colorless liquid; strong, fragrant, ethereal, acetous odor; refreshing taste; neutral reaction; sol. in water (17), ether, chloroform, and alcohol; sp. gr. 0.889-0.897. Officinal Preparations. 1. Tinctura Ferri Acetatis (see Iron). 2. SpiritusOdoratus. (Perfumed Spirit. Cologne Water.) A solu- tion of oils of bergamot, lemon, rosemary, lavender and orange flowers, and acetic ether in alcohol and water. Spiritus tEtheris Nitrosi —Spirit of Nitrous Ether. (Sweet.Spirit of Nitre.) An alcoholic solution of ethyl nitrite (C2H6N02) containing 5% of the crude ether. Made by mixing H2S04 with alcohol, and when cool adding HN03 and distilling through well-cooled condensers into a receiver surrounded by broken ice, which is connected by means of a glass tube with a small vial containing water to absorb the incondensable vapors. The distillate obtained between 176°-180° F., is shaken with ice-cold water (to remove various acid products that, may be present), the ethereal layer separated and mixed with 19 times its weight of alcohol. Explanation. In the above process H2S04 acts merely to dehydrate the nitric acid as well as to absorb the water formed during the process; by the action of nitric acid on alcohol, aldehyd is formed as well as ethyl nitrite. 2C2H5OH + HN03 = C2H40 + C2H5N02 -f 2H20. (Alcohol.) /Nitric\ (Aldehyd.) / Ethyl \ (Water.) \ Acid. / 'Nitrite./ Preservation. By age, or on exposure to direct sunlight, the aldehyd formed in the above process oxidizes into acetic acid. Reaction. C2H40 -f- O = HC2H302. (Aldehyd.) / Oxygen \ (Acetic Acid.) Vfrorn Air./ ALCOHOL DECOMPOSITION PRODUCTS. 183 The free acid may he neutralized by keeping a small quantity of magnesia or potassium bicarbonate in contact with the spirit. The German Pharmacopoeia suggests that crystals of potassium tar- trate be kept in the bottle, thereby neutralizing any free acid and forming a proportionate amount of potassium bitartrate which ppts. Description. A transparent, mobile, volatile, inflammable liquid; greenish-yellow tint; agreeable fruit-like odor; sharp and burning taste; sp. gr. 0.823-0.825 ; slightly reddens litmus, but should not effervesce when a crystal of IyHC03 is placed into it; mixes with water in all proportions. Assay. (Showing at least 4% of ethyl nitrite.) Macerate 10 grams with 1.5 gram KOH for 12 hours with agitation, add an equal vol. of water, and set aside till the alcohol odor has disappeared, then acidulate with dil. II2S04, add 0.335 grams test-sol. potass, perman- ganate, when the color of the latter disappears. Officinal Preparation. Mistura Glycyrrhizae Composita. (C5H14N02—117) Amyl Nitris.—Nitrite of Amyl. (Amylo-Nitrous Ether.) Made by the action of HN03 on purified amylic alcohol and dis- tilling; purified by washing with water and an alkali and care- fully re-distilling. 2C6Hi,OH -(- FINOs = C5H„N02 + C6H10O -f 2IUO. (Amylic Alcohol.) /Nitric\ /AmylicX /ValerianicN (Water.) \ Acid./ VNitrite./ \ Aldehyd./ Description. Pale-yellowish liquid; ethereal, fruity odor; aro- matic taste; neutral or slightly acid reaction; sp. gr. 0.872-0.874; insol. in water, sol. in alcohol, ether, chloroform, etc. Usually put up in glass “tears” containing five drops; the glass to be crushed in the handkerchief, and its contents inhaled. Dose, 3-5 drops. (C2HC130,H20—165.2) Chloral.—Hydrate of Chloral. Made by the long continued action of dry chlorine (dried by pass- ing through H2S04 or CaCl2) on absolute alcohol; the crude chloral obtained is purified by treating with H2S04 and distilling over a mixture of lime and chalk. To the distillate the necessary quantity of water is added, forming a solid mass, chloral hydrate. When dry chlorine gas is passed into alcohol, aldehyd and HC1 are formed. Reaction. C2H5OH -f Cl2 = C2H40 + 2HC1 (Alcohol.) (Chlorine.) (Aldehyd.) and by the continued action of dry chlorine, chloral is produced: C2H40 + 3C12 = C2HCI3O + 3HC1. (Aldehyd.) (Chlorine.) (Chloral.) If water is present in either chlorine or alcohol, chloral is not formed, but the following reactions result: C2H40 + H20 + Cl2 = C2H402 -f- 2HC1. (Aldehyd.) (Water.) (Chlorine.) 184 MANUAL OF PHARMACY. and, C2II402 + C2H6OH = C2H6C2H302 + H20. (Acetic Acid.) (Alcohol.) (Acetic Ether.) (Water.) The acetic ether thus formed cannot be further converted into chloral. Description. Separate, rliomboidal, colorless, transparent crys- tals; evaporating when exposed to air; aromatic, penetrating, slightly acrid odor; bitterish caustic taste; neutral reaction; sol. in water, alcohol, ether, chloroform (4), glycerin, and the light hydro- carbons. Liquefies when mixed with carbolic acid or camphor. When a hot aqueous solution is treated with solution of potash, soda or ammonia, a vaporous milky mixture of chloroform is ob- tained with a formate in solution. Impurities and tests. Acids: -f- litmus paper = red color. Hydro- chloric acid: -f-11 NO., -f- AgN03 = white ppt. Chloral alcoliolate : Dissolves in less than 4 p. chloroform. Boiling-point higher than 206° P. Aq. solution warmed with KOH; tilt, -f-test solution of iodine = yellow ppt. (iodoform). Camphorated Chloral. The liquid mixture of camphor and chlo- ral is said to be a true chemical compound called camphorated chloral, but is decomposed by water, chloral dissolving while camphor precipitates. Dose of Chloral, ten to twenty grains. Butyl Chloral Hydrate. (Croton Chloral Hydrate.) Made by passing chlorine into acetic aldehyd, and subjecting the mass to repeated fractional distillations; the distillate on dis- solving in water is converted into the hydrate. Dose. Three to ten grains. Made by distilling a mixture of alcohol, chlorinated lime and water. The distillate is washed with water, and the aqueous layer poured off, crude chloroform remaining. By the action of the chlo- rine present in the lime compound on the alcohol, aldehyd is formed, which by the further action of chlorine is converted into chloral and finally into chloroform. Ckloroformum Yenale.—Commercial Chloroform. (1) C2H6OH + CaOCls = C2IT40 -f CaCl2 + H20. (Alcohol.) /ChlorinatedX (Aldehyd.) (Calcium \ (Water.) \ Lime. ) VChloride.) (2) 2C2H40 + 6CaOCl2 = 2C2HC130 -f 3CaCl2 + 3Ca(OH)2. (Aldehyd.) /Chlorinated\ (Chloral.) / Calcium \ ( Calcium \ \ Lime. / VChlorlde./ VHydroxlde./ (3) 2C2HC130 + Ca(OH)2 = 2CHCL -f Ca(CH02)2 (Chloral.) ( Calcium \ (Chloroform.) /Calcium \ VHydroxide./ \ Formate. / Description. (See Ckloroformum Purif.) Sp. gr. 1.470; con- taining at least 98$ chloroform; when shaken with an equal vol. H2SO4, the acid layer should not become quite black within 24 hours. Officinal Preparations. 1. Linimentum Ckloroformi. 2. Chloro* formum Purificatum. Linimentum Chloroformi. (Chloroform Liniment.) Contains commercial chloroform (40), and soap liniment (60). VOLATILE OILS. 185 (CHC13—119.2) Chloroformum Purificatum. (Purified Chloroform.) Made by agitating crude chloroform with H2S04 which destroys the impurities in the former, the lighter chloroformic layer is separated, and further agitated with solution of sodium carbonate for the purpose of removing any adherent acid, the chloroform is then separated from the supernatant liquid, mixed with 1% of alco- hol, and distilled over lime to remove water, at a temperature be- low 152° F., thereby leaving behind all impurities which have escaped the action of the acid and that have a higher boiling-point than chloroform; the alcohol is added to prevent decomposition and the formation of dangerous chlorine compounds. Description. A heavy, clear, colorless, diffusive liquid; charac- teristic, pleasant ethereal odor; burning, sweet taste; neutral re- action; sol. in water (200), alcohol, ether, etc. Sp. gr. 1.485-1.490; contains 0.75 to 1% alcohol. On agitating with cone. H2S04 and allowing to stand for 24 hours, both liquids should remain colorless. Impurities and tests. Acids: Agitate with water; washings-f- litmuspaper = red color. Chlorides: Above washingsAgN03 = white ppt. Chlorine: Above washings-f-KI = coloration. Alde- hyd: Digest with KOH = dark color. Officinal Preparations: 1. Mistura Chloroformi. 2. Spiritus Chloroformi. Mistura Chloroformi. (Chloroform Mixture. Chloroform Emulsion.) Contains purif. chloroform (8), camphor (2), fresh yolk of egg (10), water (80), made into a uniform mixture, by the use of a mortar. Spiritus Chloroformi. (Spirit of Chloroform. Chloric Ether.) Contains purif. Chloroform (10), and alcohol (90). VOLATILE OILS.—ESSENTIAL OILS. Yolatile oils are the proximate principles to which the odor of most plants is due. They are odorous, volatile, inflammable liquids, freely soluble in alcohol, ether, chloroform, CS2, benzol, and the fixed oils, slightly soluble in water. When dropped on paper they leave a fatty stain which disappears on the application of heat. Source. Found in the majority of plants, existing in every part from root to seed; in some instances produced by the action of a ferment. Color. Colorless when pure, but acquiring certain colors on ex- posure to air and light, the color developed being due to the pres- ence of distinct compounds. Specific Gravity. Their Specific Gravities range between 0.850 to 0.990, while a few are even heavier than water. The lightest are oils of lemon and erigeron (0.850), the heaviest, oil of wintergreen (1.180). Reactions. Rapidly decomposed by strong HN03; certain oils 186 MANUAL OF PHARMACY. produce explosive fulminates with iodine; H2S04 yields characteristic color reactions. Composition. Hydrocarbons (mostly terpenes) and hydrocarbons with oxygen represent the elements found in the majority, but some contain sulphur (Ex. Oils or mustard, asafetida, horse-radish, etc.), and are characterized by a disagreeable, penetrating odor, while a few others contain nitrogen in the form of hydrocyanic acid. (Ex. Oils of bitter almond, cherry laurel, etc.) All oxygenated volatile oils contain at least two proximate principles having different boiling and congealing points; elaeopten (mostly Ci0H16 or C10H14) has the lowest boiling-point, stearopten or “cam- phor” as it is termed (an oxide or hydroxide of the terpene) is that portion which volatilizes last and congeals in crystals near the ordi- nary temperatures, and is usually isomeric with common camphor. Methods of Preparation. I. Simple Distillation. This process is employed in obtaining oils of turpentine, copaiba, tar, amber (by destructive distillation), etc. II. Distillation with Water. The substance either in fresh or dried state, is cut up and macerated with water, then the mass is placed in a suitable still and mixed with more water, which prevents the burning and decomposition of the vegetable matter and facilitates the vaporizing of the oil, which readily distils with the steam produced on applying heat. Salt is sometimes added to raise the temperature of the boiling-point in making some of the heavier oils. The milky distillate on cooling separates into two layers, one being a solution of oil in water, the other the pure oil, which may be separated by means of a separating funnel, or other convenient contrivance. Examples. Oils of orange flotcers, cinnamon, cloves, and wintergreen. III. Expression. This process avoids the use of heat (which in- jures the odor of certain delicate oils) and produces the most fragrant odors; such oils are however, cloudy in appearance, due to the presence of albuminous matter. Examples. Oils of almond, lemon, orange, bergamot, etc. IV. Solution. Comprising several processes; Percolation, using purified CS2 or petroleum benzin for a menstruum, and the subsequent distillation of the solvent from the oil. Maceration, or digestion with some inodorous fixed oil. Enfleurage. Several trays are covered with a layer of purified tallow, or some inodorous fat, and then with a layer of fkwers, the latter being replaced by fresh flowers from time to time. The re- sulting product after separating the flowers, represents the pom- mades employed by perfumers, the commercial strengths of which are denoted by the numbers, 6, 12, 18, 24, 30 and 36. To obtain the volatile oil, the pommade is melted and macerated with cologne spirits, the latter dissolving the odorous principles, the solution obtained constituting the extracts of perfumers, the small portion of dissolved fat being removed by chilling and filtering. VOLATILE OILS. 187 Preservation. When the volatile oils are exposed to air and light, ozone is developed, causing them to become viscid, or-occa- sionally forming a solid resin; hence, they should be kept in a cool place, in well-stoppered, amber-colored vials, to prevent rancidity and oxidation. Many of the oils are preserved by the addition of 5# of alcohol. Restoration, Some old and resinified oils may be restored by rectification with water to which an alkali has been added or, by agitation with borax solution and animal charcoal ; the oil separates free from resin, having its original odor. Also purified by agitation with potassium permanganate and decanting. Adulterations. Fixed oils, alcohol, cheaper volatile oils, water, chloroform or camphene. Specific gravity is no test for purity. Tests for Impurities. Fixed oils: 1. Leaves a permanent greasy stain on paper. 2. The residue left on distilling with water is saponifiable. 3. Strong alcohol dissolves out the volatile oil, leaving the fixed oil undissolved (true of all except castor oil). Alcohol. 1. A separation with fixed oils (except castor oil), the alcoholic solution of volatile oil being above, and the fixed oil be- neath. 2. A diminution of the volume of volatile oil, when agitated with an equal bulk of water or glycerin in a graduated tube. 3. Fused potassium acetate or calcium chloride are insoluble in the volatile oils, but become soft or liquid in the presence of alcohol. 4. Red aniline is insoluble in the oil, but becomes soluble if alco- hol is present, producing a red color. 5. On heating potassium acetate and H2S04 with the oil, if alcohol is present, acetic ether is produced. Cheap volatile oils: Difficult to detect in many instances, but such adulterations are often indicated by the odor remaining after partial evaporation from bibulous paper. Oleum Amygdalae Amaile.—Oil of Bitter Almond. Oils Derived by the Action of a Ferment. A volatile oil obtained from bitter almond by maceration with water and subsequent distillation. The oil does not pre-exist in the almond, but is produced by the decomposition of amygdalin by emulsin. Preparation. After extracting the fixed oil, the residue is treated with water, and emulsin or synnptase is set free, which decomposes the amygdalin, producing the oil which is separated by distillation. C20H2,NO„ + 2H20 = C,HsO + 2C6HI2Oe + HCN. (Amygdalin.) (Water.) ( Oil of Almond. \ (Glucose.) /Hydrocyanic\ • \Benzyl Aldehyd./ \ Acid. / Oleum Sin apis Volatile. (Volatile Oil of Mustard.) A volatile oil obtained from black mustard by maceration with water and subsequent distillation. 188 MANUAL OF PHARMACY. A peculiar ferment myrosin, becomes active in the presence of water, converting the potassium myronate into sulphocyanide of allyl (C3H6CNS). Officinal Volatile Oils. Name. Source. Natural Order. Method of Extraction. Sp. Gr. Oleum Amygdalae 1 Seeds (Amygdal-) Maceration Amarce (Oil of Bit- •< us comunis var. > Rosacea. and Dis- ter Almonds) ( amara) \ dilation. 1.043-1.049 Oleum Anisi (Oil of Anise) f Fruit (Pimpinel-1 -{ la anisum or j- P. illicium) j Umbellif- erce, Magnolia- Distillation 0.976-0.990 Oleum Aurantii Cor- ticis (Oil of Orange Peel) i Fresh peel ((Jit- ) •< rus vulgaris or V ( C. aurantium) ) Auranti- acece. Mechanical Means. 0.860 Oleum Aurantii Flor- um (Oil of Orange Flowers) j Fresh Flowers j (Citrus v ulgaris) C Auranti- acece. Distillation 0.850-0.890 Oleum Berqamii (Oil ( Fresh peel (Cit-1 -< rus Bergamia, V ( var. vulgaris) \ Auranti- Mechanical of Bergamot) cicece. Means. 0.860-0.890 Oleum Cajuputi (Oil of Cajuput) J Leaves (Melaleu-1 I ca Cajuputi) 1 Myrtacece. Distillation 0.920 Oleum Cari (Oil of J Fruit (Carum I Umbellif- Caraway) I carui) \ eroe. Distillation 0.920 Oleum Caryophylli (Oil of Cloves) Flower Buds (Eu-1 < genia Cary- V Myrtacece. Distillation 1.050 Oleum Chenopodii i Fruit (Chenopod- i Chenopodi- acece. (Oil of American Wormseed) ■< ium anthelmin- > ( ticum) | Distillation 0.920 Oleum Cinnamomi (Oil of Cinnamon (Ceylon); Oil of Cin- namon (Chinese) f Bark of Shoots j i (Cinnamomum, -{ Zelanycum and ) ! Chinese Cinna- | [ mon) j Oleo Resin (Co- ( Lauracece. Distillation f Ceylon, ! 1.040 | Chinese, 1 1.160 Oleum Copaibce (Oil Legumin- of Copaiba) 1 paiba) ( osce. Distillation 0.890 Oleum Coriandri (Oil ‘ Fruit (Coriand- i Umbellif- of Coriander) I rum sativum) ( ercB. Distillation 0.870 Oleum Cubebce (Oil of Cubeb) i Unripe Fruit (Cm- i ( beba officinalis') ( Piper acece. Distillation 0.920 Oleum Erigerontis (Oil of Fleabane) i Fresh FI. Herb -! (Erigeron Can- V 1 adensis) 1 Composite. Distillation 0.850 Oleum Eucalypti (Oil of Eucalyptus) j Fresh Leaves j < (Eucalyptus ( globulus, etc.) ) Myrtacece. Distillation 0.900 Oleum Fceniculi (Oil J Fruit (Foenicu-1 Umbellif- of Fennel) ) turn vulgare) ( even. Distillation 0.960 Oleum Gaultherice (Oil of Wintergreen) i Leaves (Gaulthe- j \ riaprocum.be ns) ( Ericaceae. Distillation 1.180 Oleum Hedeomce (Oil of Pennyroyal) i Fresh Herb < (Hedeoma pul- > ( egioides) ) Labiatoe. Distillation 0.940 Oleum Juniperi (Oil of Juniper Berries) J Fruit (Juniperus ( I communis) | Coniferce. Distillation 0.870 Oleum Lavendulce (Oil of Lavender) | FI. Top or whole 1 -' Herb (Laven- > ( dula vera) ) Labiatoe. Distillation 0.890 OFFICINAL VOLATILE OILS. 189 Officinal Volatile Oils—Continued. Name. Source. Natural Order. Method of Extraction. Sp. Gr. Oleum Lavendulce 1Fresh Flowers Florum (Oil of Lav- K (Lavendula Labiatce. Distillation 0.890 encler Flowers) ( vera) Oleum Limonis (Oil j Fresh peel (Cit- Auranti- Mechanical of Lemon) | rus limonum) acece. Means. 0.850 Oleum Menthce Pi- i Leaves and Tops peritoe (Oil of Pep- -< (Mentha pi- Labiatce. Distillation 0.900 permint) Oleum Menthce Viri- ( perita) i Leaves and Tops dis (Oil of Spear- -< (Mentha viri- V Labiatce. Distillation 0.900 mint) l dis) Oleum Myrcice (Oil of Bay) j Leaves (Myrcia | acris) Myrtacece. Distillation 1.040 Oleum Myristicce (Oil j Seed (Myristica Myristica- of Nutmeg) I fragrans) cece. Distillation 0.900 Oleum Picis Liquidce (Oil of Tar) ) Oleo Resin (Pix 1 liquida) Coniferce Distillation 0.970 Oleum Pimentce (Oil of Pimento) j Fruit (Eugenia } pimenta) Myracece. Distillation 1.040 Oleum Rosas, (Oil of Rose) j Fresh FIs. (Rosa l damascena) Rosacece. Distillation 0.860 Oleum Rutce (Oil of Rue) j Herb (Ruta gra- } veolens) Rutacece. Distillation 0.880 Oleum Rosmarini (Oil of Rosemary) Oleum Sabince (Oil of Savin) j Herb (Rosmari-1 1 nus officinalis) 1 j Tops (Juniperus \ 1 Sabina) 1 Labiatce. Coniferce. Distillation Distillation 0.950 0.910 Oleum Santali (Oil of Sandal-wood) j Wood (Santalum i } album) ( Santala- ceoe. Distillation 0.945 Oleum Sassafras (Oil of Sassafras) l Barit or Boot 1 -< (Sassafras off - > Lauracece. Distillation 1.090 Oleum Sinapis Vola- (Seed (Sinapis Cruciferce. Maceration tile (Oil of Mustard) j nigra) & Distill. 1.017-1 021 Oleum Succini (Oil of Amber) | Fossil (Amber) Coniferce. Destructive Distillat'n 0.920 Oleum Terebinthinas (Oil of Turpentine) ( Oleo Resin (Pin- -< us australis, / etc.) Coniferce. Distillation 0.855-0.870 Oleum Thymi (Oil of j Herb (Thymus 1 ) vulgaris) j j Root (Valeriana 1 Labiatce. Distillation 0.880 Oleum Valerianae (Oil Valerian- of Valerian) ) officinalis) f acece. Distillation 0.950 STEAROPTENS. A stearopten (or concrete volatile oil) derived from Ginnamomum Camphom, and purified by sublimation. (N. O. Lauracece.) Hab. Asia, China and Japan. Preparation. Obtained from the root, trunk and branches of the Camphor Laurel. The wood is cut into chips and boiled with water in a still, the camphor sublimes and the oil is drained from it. Camphor may be obtained as an impalpable powder by careful sublimation and a skilful arrangement of the temperature of the condensing chamber. (C i o H16 O—152) C amphora .—Camphor. 190 MANUAL OF PHARMACY. Description. White, translucent masses of a tough consistence and crystalline structure. Readily powdered by the aid of a little alcohol, ether or chloroform. Penetrating odor; pungent taste; sol. in alcohol, ether, chloroform, CS2, etc., sp. sol. in water. Officinal Preparations. 1. Aqua camphor* (0.8$). 2. Linimentum camphor*. 3. Linimentum saponis. 4. Bpiritus camphor* (10$). 5. Tinctura opii camphorata. Linimentum Camphors. (Camphor Liniment.) Contains cam- phor (20), dissolved in cotton-seed oil (80). Linimentum Saponis. (Liquid Opodeldoc. Soap Liniment.) Contains soap (10), camphor (5), and oil of rosemary (1), dissolved in alcohol (70) and water ft. 100. (CioHisBrO—230.8) Camphora Monobromata. (Bromated, or Mono-bromated Camphor.) Made by uniting camphor and bromine with the aid of heat, and purifying by re-crystallizing from a solution in benzine. Description. Colorless, prismatic needles or scales; mild cam- phoraceous odor and taste; neutral reaction; almost insol. in water; sol. in alcohol, ether, chloroform and fixed oils. (CioHisOH—150) Thymol.—Thymic Acid. Obtained from oil of thyme by distillation; the portion distilling above 392“ F. is agitated with NaOH and the thymol-sodium solu- tion formed is treated with HC1 to liberate the thymol, NaCl remaining in solution. Purified by crystallization from an alcoholic solution. Description. Large, colorless crystals; aromatic, thyme-like odor; pungent, aromatic taste; neutral reaction; aim. insol. in water; sol. in alcohol (1), ether, chloroform and oils. Impurities. Carbolic acid: Aq. solution -j- sol. Fe2Cl6 = blue color. Menthol. Found in most plants of the mint family, and extracted from oil of peppermint, by rectifying by fractional distillation and sub- jecting the heavier distillate to a temperature of —10“ C., or less, when the crystals of menthol separate. Occurs in snow-white acicu- lar crystals. Uses. As a local anaesthetic, and to relieve the pain of burns. Oil of peppermint is often met with in commerce, from which the menthol has been extracted. Tests to detect the removal of pip-menthol from oil of peppermint. A test-tube partially filled with the oil under examination, is placed in a freezing mixture of snow and salt for 10 to 15 minutes. If the oil has not been tampered with, it will become cloudy, thick and of a jelly-like consistence, and if four or five small crystals of menthol are added and the tube replaced in the freezing mixture, the oil will soon form a solid mass of crystals. If limpid or partially so, it indicates adulteration or removal of menthol. 191 FIXED OILS AND FATS. FIXED OILS AND FATS. The Fixed Oils or Fats, are solid or liquid bodies, derived from both animal and vegetable kingdoms, greasy to the touch, leaving a permanent fatty stain on paper, which is unaffected by heat. Consistence. If liquid at ordinary temperatures they constitute the true ox fibred oils, and if solid they are called/ate. Color, etc. Colorless, odorless and tasteless when pure, but as often seen, many are not darker than light yellow, and have a dis- tinctive odor and taste, often due to impurities. Specific Gravities. All lighter than water, ranging between 0.860 and 0.970. Solvents. Insoluble in water, sp. soluble in cold alcohol, soluble in ether, chloroform, CS2, benzol, benzine, turpentine and volatile oils. Chemical Composition. Mixtures of two or more fats, having different fusing points, and which may be separated by fractional refrigeration. These fats are the compound ethers of the higher members of the fatty acids, the triatomic alcohol being glycerin, and the radical propenyl. In most cases they consist of two or three proximate principles, viz.: Olein, Palmitin, and Stearin, which may be called respectively, the oleate, palmiiate and stearate of propenyl. The acids belong to two series of the fatty acid group, of the gen- eral formula CnII2n02, and the oleic acid group CnH2n.202. Stearic acid, Ci8H3a02; palmitic acid, Ci8H3202; oleic acid, Ci8H3402. Olein (from eXaiov—oil) C3H5"' (C18H3302)3' is a liquid, while palmitin, C3HB(C,(iHsi02)3, and stearin (from cr reap — suet) C3H5(Ci8H3502)3 are both solids. Purification. Purified by treatment with H2S04, which car- bonizes the impurities (or oxidized by permanganic or chromic acids, or the hypochlorites), agitating with water, decanting and filtering through charcoal to absorb coloring matter. Another method is by washing with a cold solution of an alkali carbonate. Results of Heating. If solid they melt, or if liquid become thinner. When heated to about 572° F., they decompose, and evolve offensive and irritating vapors (causing a copious flow of tears) containing acrolein, C3H40. They burn with a sooty flame, generating much heat. Result of Exposure to Air. They acquire an acrid, disagreeable odor and taste and an acid reaction and are then said to be rancid. This change is due to the presence of impurities in the form of protein and mucilaginous compounds, or animal or vegetable tissue. This decomposition liberates the fatty acids, producing odorous and volatile acids (butyric, valerianic, etc.), acrolein and coloring matter. Protection. Keep in a cool, dry place, away from light and air. Restoration. By washing the rancid fat wfith wTarm water, or a weak alkali solution, and again washing with strong alcohol. Some times treated with powdered borax and dried sodium carbonate. 192 manual of pharmacy. 1. Fusion, by itself. Example: Cod Liver Oil. 2. Fusion in the presence of water. Example: Lard. [In either case subsequent straining or skimming is resorted to, to remove the tissue.] From Vegetable Tissues. 1. Expression. Either cold (oil of linseed), or between iron plates heated above the fusing point of the fat (olive and castor oils). 2. Solution. Accomplished by maceration or percolation, using CS2 or benzin, and finally distilling off the solvent (oils of lobelia and pumpkin seed). 3. Decoction. The oil separates and rises to the surface of the water, during this process. Adulterations. The high-priced fats are adulterated with cheaper grades, but on account of their similarity of composition, such admixtures are difficult to recognize. A change in the fusing or congealing points is sometimes pro- duced by such additions. Sp. gr., color, odor and taste, often lead to their detection. Nitric acid and cone, sulphuric acid produce with different oils mixtures varying in color. [Table of Officinal Oils and Fats, on page 193.] Preparation.—From Animal Tissues. The suspension of oily or resinous bodies in a watery menstruum by the aid of a mucilaginous body. Them'y of emulsification. The oil globules are separated and each covered with a mucilage to prevent them from cohering. Milk and the yolk of egg (vitellum) are types of perfect emulsion. Emulsifying agents. Gums, glyconin (Glyceritum Vitelli), Irish moss, Iceland moss, pancreatin, etc. Method for preparing Emulsio Morrhme (containing 50% of oil). Put eight ounces of cod liver oil into a dry mortar and add 2 ozs. powd. acacia, rubbing with the pestle; when a uniform mix- ture results, add 6 ozs. of water all at once, and stir the mix- ture till a perfect emulsion results. Emulsions. Soaps are metallic salts of the fatty acids; the process by which they are formed is termed saponification. Preparation. 1. Soluble Soaps (detergent, and soluble in water or alcohol). Made by boiling fats with a solution of soda or potash; the fatty acids unite with the alkali forming the soap, which remains dissolved in the waier together with glycerin which has also been liberated from the fat. The lye is employed in a diluted state, and gradually added until in excess, thereby facilitating saponifica- tion. Boiling is continued until the mixture is transparent and tenacious. The excess of alkali is removed by adding NaCl, as soap is insoluble in solutions of most potassium or sodium salts. Potash soaps are soft, soda soaps hard. SOAPS. SAPONIFICATION PRODUCTS. 193 Name and Synonym. Source. Order. Kingdom. Method of Extraction. Specific Gravity. Lard. (Adefis.) 1 Seeds (A mygdalus com ) •< munis var. amara or V ( dulcis.) ) j Seed (Gossypium herba- I | ceum, etc.) j Seed (Linum usitatissi- ) | mum.) 1 Pachydermata. Animal. Cold expression. O.9OO—0.920 Oleum Amygdala Expressum. Rosacea. Vegetable. Hot expression. O.9I4 0.920 Oleum Gossypii Seminis. (Cot- Malvacece. Vegetable. Cold expression. O.92O — O.93O Oleum Lini. (Oil of Flaxseed. Linacece, Vegetable. Cold expression. ( Fusion; expres-1 •< sion; decoc- V ( tion. ) j Expression; so- / j lution. f All four methods. Expression. Expression. 0.936 Oleum Morrhua. (Cod-liver j Fresh Cod Livers (Gadus ) 1 Morrhua, etc.) j Ripe Fruit {Olea Europen.) Seed (Ricinus Communis.) Seed (Sesamum Indicum.) Seed (Croton Tiglium.) Teleostia. Animal. 0.920 O.925 Oleacece. Vegetable. 0.915—0.918 Oleum Ricini. (Castor oil) Oleum Sesami. (Benne oil) Oleum Tiglii. (Croton oil)... Euphorbiacece. Pedaliacece. E uphorbiaceai. Vegetable. Vegetable. Vegetable. O.95O O.97O O.9I4—O.923 O.94O—O.955 Fats. i Abdomen (Sus. Scro/a— ) 1 Hog.) j ( Head (Physeter Macro-) •< cephalus — Sperm V ( Whale.) ) Seed {Theobroma Cacao.) (Abdomen {Ovis Aries—1 1 Sheep.) f Pachydermata. Animal. (Fusion withwat’r) ( and straining.) Fusion with water. o.cn8 (about). Animal. 0.94s Oleum Theobromce. (Butter of ) Cacao) ( Sterculiacece. Ruminantia. Vegetable. Animal. Hot expresssion. j Fusion and ( j straining. ) ' Suet should be kept in well closed vessels im- pervious to fat, and should not be used af- ter it has be- .com erancid OFFICINAL FIXED OILS AND FATS. 194 MANUAL OF PHARMACY. 2. Insoluble Soaps; Made by combining a metallic oxide or an alkaline earth (as a base) with the fatty acids. Soaps of the alkaline earths are employed for waterproofing fabrics, by impreg- nating the fabric with alum or some calcium or barium salt, and digesting in a soap solution. The soluble soaps decompose when used with hard waters, form- ing insoluble calcium soaps. / Description. Pure soaps (soluble) are mostly white, the color and marbled appearance being due to impurities or the presence of salts intentionally added to make them attractive. Chemical Composition. One or more of the following salts of sodium or potassium. Examples of soluble soaps: €3H5"'(C18H3502)'3 + 8K0H = 3KC18H3502 / Stearin. \ ( Potassium \ (Potassium Stearate.) VPropenyl tri-stearate./ \ Hydroxide./ + C,H."'(OH)',. / Glycerin. \ \Propeiij i Hydrate./ C3H5(C18H3302)'3 + 3KOH = 3KCi8H3302 / Olein. \ /'Potassium \ (Potassium Oleate.) \Propenyl tri-oleate./ VHydroxide./ + C3H5(OH)3. (Glycerin.) C3H6(C18H3104)s + 3KOH = 3KCi8H8i02 / Palmltln. \ / Potassium \ (Potassium Palmitate.) VPropenyl tripalmitate./ VHydroxide./ + C3H5(OH)3. (Glycerin.) Sapo.—Soap. (Hard Soap. Castile Soap.) Soap prepared from soda and olive oil. Description. White or nearly white solid; alkaline taste and reaction; sol. in water, or alcohol. Should contain not more than 34$ water, no metals,, animal fats, or excess of alkali. Officinal Preparations. 1. Linimentum Saponis (see Camphor). 2. Emplastrum Saponis. (Soap Plaster). Contains powd. soap (10) incorporated with lead plaster (90). Soap prepared from potassa and fixed oils. oil is often employed for this purpose. Although termed green soap, it is scarcely ever of that color unless artificially colored. Its usual color is brownish yellow. Officinal Preparation. Tinctura Saponis Viridis (Tincture of Green Soap). Contains green soap (65) and oil of lavender (2), dissolved in alcohol (ft. 100) by maceration. Officinal Insoluble Soaps. Linimentum Calcis (see Calcium). Emplastrum Plumbi (see Lead). Sapo Yikidis.—Green Soap. (Soft Soap.) Reaction. 8PbO -|- 2C3H6(Ci8H3302)3 + 3H20 = (Litharge.) (Olein.) (Water.) 3Pb(C,8H3302)2 + 2C3H5(OH)3. (Lead Oleate.) (Glycerin.) FIXED OILS AND FATS. 195 Water is required in the above reaction (as well as in the process of preparation) to furnish the elements to produce glycerin. Glycerinum.—Glycerin (yAvecvi—sweet.) A liquid obtained by the decomposition of fats or fixed oils, and containing not less than 95$ absolute glycerin—(C3H6(OH)3—92). Source and Preparation. Always a product of saponification. Discovered by Scheele in 1779, and called “the sweet principle of fats.” First made during the process for making lead plaster (see reaction above), the soft plaster being well washed with water to dissolve out the glycerin. The modern method for its production depends on the decompo- sition of fats or fixed oils by super-heated steam at high pressure, when the fatty acid rises to the surface of the glycerin solution. C3H5(C1hH3302)3 + 3H20 = C3H5(OH)3 + 3HC18HS302; (Olein.) (Water.) (Glycerin.) (Oleic Acid.) or, C3H6(C18H3502)3 + 3H20 = C3He(OH)3 + 8HC18H 3602. (Stearin.) (Water.) (Glycerin.) (Stearic Acid.) Purification. Purified by treatment with animal charcoal and fractional distillation. Composition. A triatomic alcohol, often termed glyceryl, pro- penyl hydrate or propenyl alcohol. [Nitroglycerin.—Glonoin. (C3H5(N02)303). Obtained by the action of a mixture of concentrated I1N03 and H2S04 on glycerin, at a freezing temperature. A very explosive compound, soluble in alcohol, or ether, insol. in water; the basis of dynamite.] Description. Glycerin is a clear, colorless liquid; syrupy con- sistence; hygroscopic; sweet taste, and neutral reaction; sol. in water or alcohol; insol. in ether, chloroform, benzol and the fixed oils; sp. gr. 1.250. Properties. A great antiseptic and solvent. Impurities and tests. Butyric, and other volatile acids: —|- dil. H2S04 -|- Heat = odor. Cane-sugar: Warm with 112S04 = dark color. Sugars, and dextrin: Heat and ignite = a porous coal remains. Glucose: -f- test-sol. potassio-cupric tartrate = yellowish- brown ppt. Acrylic, or Hydrochloric acids: -f- AgNOs = white ppt. Sulphuric, and oxalic acids ; calcium, iron, and metals: Usual tests. Officinal Preparations. 1. Glyceritum amyli (see Amylum). 2. Mucilago tragacanthse (see Gums). 3. Glyceritum Yitelli (Glycerite of Yolk of Egg. Glyconin). Contains yolk of egg (45) thoroughly mixed with glycerin (55). (HCi8H3s02—282) Acidum Oleictjm.—Oleic Acid. (Elaic Acid.) May be made by forming lead soap (using almond or olive oil), decomposing with HC1 and dissolving out the acid with ether or benzin, evaporating off the solvent and washing with water. 3Pb(C18H 33 0 2)2 + 6HC1 = 3PbCl2 + 6HC18H 33 0 2. (Lead Oleate.) /Hydrochloric'v ( Lead \ (Oleic Acid.) V Acid. ) '.Chloride./ Also made by chilling fats to 40° F. and expressing, the solid portion being rejected. 196 MANUAL OF PHARMACY. Description. A yellowish, oily liquid, becoming brown, rancid and acid on exposure to air; odorless; tasteless; neutral reaction; sp. gr. 0.900-0.910; insol. in water, sol. in alcohol, chloroform, benzine, etc. A solvent for fats and fatty acids. Unites with basylous radicals to form salts called oleates. OLEATUM.—OLEATES. Oleatum Hydrargyri. (Oleate op Mercury.) Contains 10$ yellow oxide. See Hydrargyrum. Oleatum Veratrina. (Oleate op Veratrine.) A 2$ solution of veratrine in oleic acid. Many unofficinal oleates are now being extensively employed. They are made by decomposing sodium or potassium oleate by a salt of the base required (both in solution), and subsequently melt- ing, washing and drying the precipitate. Aluminium Oleate—Al2(Ci8H3302)6. Made by the double decom- position between aluminium sulphate and sodium oleate. Precipitated Oleates. A12(S04)s + 6NaC18H3302 = A12(C18H33 02)6 + 3Na2S04. Arsenic Oleate. As(Ci8H3303)3. Reaction. AsC13 + 3NaCi8H3302 = 3NaCl -+- As(Ci8H3302)3. Bismuth Oleate. Bi(C18H 33 0 2)s. Reaction. Bi(N03)3 + 3NaCi8H3302 = Bi(Ci8H3302)3 + 3NaN03. Copper Oleate. Cu(Ci8H3302)2. Reaction. CuS04 -f 2NaCi8H 33 02 = Cu(Ci8H3302)2 + Na2S04. Ferric Oleate. Fe2(Ci8H3302)6. Ferrous sulphate and sodium oleate; boil the mixture to oxidize the ferrous to a ferric salt. Manganese Oleate. Mn(Ci8H3302)2. Manganese sulphate and sodium oleate. Nickel Oleate. Ni(Ci8H3302)2. Nickel sulphate and sodium oleate. Lead Oleate. Pb(CieH3302)2. Lead nitrate and sodium oleate. Silver Oleate. AgCi8H 33 02. Silver nitrate and sodium oleate. Sodium Oleate. NaCieH3302. Made by dissolving castile soap (1) in water (8); on standing, sodium palmitate deposits, and the solu- tion containing the oleate may be decanted. Tin Oleate. Sn(Ci8H3302)4. Tin chloride and sodium oleate. Zinc sulphate and sodium oleate. Can be obtained as an impal- pable white powder. Zinc Oleate. Zn(Ci8H3302)2. Oleates op the Alkaloids. To prepare these salts, the alkaloidal salt must be placed in solu- tion, and an alkali added to combine with the acidulous radical, causing the alkaloid to be precipitated; after washing, draining and drying, it is then ready for solution in oleic acid. ALKALOIDS. 197 ALKALOIDS. Discovery really dates back to 1816, when Serttlrner, a German apothecary, announced the existence of true morphine, and learned its characteristics. Occurrence. In both animal and vegetable kingdoms. Existing in all parts of plants excepting perhaps the wood or stem. Definition. Alkaloids are mostly crystallizable bodies of animal or vegetable origin, generally representing the active principles of the plants producing them. They have an alkaline reaction, com- bine with acids to form salts, but are distinguished from alkalies and alkaline earths by the fact that they do not saponify the fats, and are destructible by heat. When heated with an alkali, they evolve an ammoniacal odor. Composition. They contain the elements C, H, O, and N, and are either compound amines or amides (the latter contain oxygen, while the former do not), or ammonia in which one or more hydro- gen atoms have been replaced by a hydrocarbon radical. Ex. Conine, C8HiBN = N j g8^14 and may be looked upon as NH3 with two H atoms replaced by the dyad radical C8Hi4. N-J C5H7 Nicotine, Ci0Hi4N2 = XT 57 is a diamine, or represents two molecules of NH3, in each of which all the hydrogen atoms are re- placed by C5H7. Existence. They do not exist naturally in a free state, but as acid or neutral salts, in which the alkaloids are combined with such common acids as tannic, citric, tartaric, malic, acetic, etc., or some acid peculiar to the plant, as kinic, meconic, igasuric, acon- itic, etc. Solvents. Soluble in alcohol, chloroform, benzin, benzol, amylic alcohol, kerosene, etc.; and some are soluble in ether. Insoluble in water. Mbst of the alkaloids are solid bodies, but a few are liquid and volatile. Ex. Conine, sparteine, nicotine, lobeline. These are all amines, containing no oxygen. Nomenclature. For the purpose of ready distinction from other principles, the terminations of all alkaloids are ine (aconitine, atropine), the Latin being ina (quinina, strychnine). Glucosides and neutral principles all end in in. Ex. Glycyrrhizin, gelatin, glycerin, etc. Formation of Alkaloid Salts. When forming salts, the alka- loids do not replace the hydrogen of acids, consequently the terms sulphate, chloride, etc., are incorrect when applied to an alkaloidal salt, but should be respectively, hydrosulphate, hydrochloride, etc. The type of these salts may be said to be ammonium chloride (or ammonia hydrochloride), forming their salts in the same manner that NH3 and HC1 produce the above salt. 198 MANUAL OF PHARMACY, Illustrations: Type. NH3 + HC1 = NH3, HC1. or NH4C1. (Ammonia.) /Hydrochloric) / Ammonia \ /Ammonium) \ Acid. / VHydrochloride./ \ Chloride. / CuH19N03 + HC1 = C17H19N03, HC1. (Morphine.) (Morpliine Hydrochloride.) 2C20H24N2O2 -f- H2SO4 — (C2 oH > H2SO4. (Quinine.) j (Quinine Hydrosulphate.) C21H22N2O2 “I- HC2H302 = C21H22N2O2, HC2H302. (Strychnine.) (A ’etic Acid.) (Strychnine Hydro-acetate.) C17H21N04 + HC1 = C17H2iN04, hcl (Cocaine.) (Cocaine Hydrochloride.) I. Mhen the native alkaloidal salt (the chemical combination of the alkaloid in the plant) is soluble in water, and the alkaloid itself in- soluble; the addition of a strong alkali to an infusion or decoction of the vegetable substance, neutralizes the organic acid with which the alkaloid is associated, precipitating the alkaloid in a more or less pure form. II. When the native salt is insoluble, or not freely soluble in water (as is more frequently the case). A dilute acid is then used for its extraction, so that its salt with an inorganic acid is obtained, and upon decomposition with an alkali, yields the quite pure precipi- tated alkaloid. In many cases, however, the extraction requires a more complex process, but all methods comprise the following six steps, viz.: 1. Solution. 2. Precipitation. 3. Re-solution. 4. De- colorization. 5. Purilication. 6. Crystallization. Decolorization: Effected by treatment with animal charcoal, or lime. Theory of Isolation. The separation of the alkaloids may be thoroughly understood, by writing an equation to represent each step in which an important change occurs. The following method is suggested by the author. First. To illustrate the extraction of morphine from opium, the native salt morphine hydro-meconate, soluble in a simple solvent. The + and — signs used, respectively indicating the basylous and acidulous radicals. General Methods of Extraction. Mo. Mec. + NH4OH = Mo + NH4Mec. -f H20. / Morphine ) /'Ammonium) (Morphine.) ( Ammonia \ (Water.) \Hydro-meconate.) \ Hydroxide .) V Hydro-meconate J Second. When the native salt is insoluble in a simple solvent. Reaction. Qu.Kin -f- HC1 = Qu. HC1 -f~ Kin. ( Quinine \ /Hydrochloric\ ( Quinine \ (Kinic Acid.) VHydro-Kinate./ \ Acid. ) VHydrochloride.) 2Qu.HCl -f- Ca(OH)2 = 2Qu. -f- CaCla -f- 2H2O. / Quinine \ ( Calcium \ (Quinine.) / Calcium \ (Water.) (.Hydrochloride./ VHydroxide./ (Chloride./ Cinchona contains quinine hydro-kinate. ALKALOIDS. 199 2Coc.Tan. + H2S04 = Coc2H2S04 + Tan. / Cocaine \ /Sulphuric") ( Cocaine \ (Tannic Acid.) \ Hydro-tanuate./ \ Acid. / VHydrosulphate./ Coc2.H2S04 + Na2C03 = 2Coc. -f Na2S04 -f H20 + C02. / Cocaine \ / Sodium \ (Cocaine.) ( Sodium \ (Water.) / Carbon \ VHydrosulphate./ VCarbonateJ \SulphateJ (Dioxide./ Erythroxylon contains cocaine hydro-tannate. Then to form cocaine hydrochloride: Coc. + HC1 = Coc.PICl. (Cocaine.) /HydrochloricN / Cocaine \ \ Acid. ) V Hydrochloride./ Opium.—Gum Opium. The concrete milky exudation obtained in Asia Minor, by incising the unripe capsules of Papaver somniferum. (N.O. Papaveraceat.) In its normal moist condition yielding not less than 9# of morphine by the officinal assay process. Opii Pul vis.—Powdered Opium. Should contain mor- phine. Any powdered opium of a higher percentage may be brought within these limits, by admixture with powd. opium of a lower percentage in proper proportions, by the method given in Part I, page 31, for mixing solutions, etc., of different strengths. Example. Having powdered opium, several lots, assaying 9, 11, 15 and 18#; how much of each shall I use to make 80 ozs. equivalent to 14# ? Answer : 9- 4 X 6.153 = 24.6 ozs. 11— -i 1 X 6153 = 6.1 ozs. 14 15--1 3 X 6.153 = 18.4 ozs. 18- 5 X 6.153 = 30.7 ozs. 13)80 79.8 ozs. Proof: 4 x 9 = 36 1 X 11 = 11 3 X 15 = 45 5 X 18 = 90 13)182 of H ujT Opium Denarcotissatum. vDenarcotized Opium.) Made by repeatedly macerating powd. opium (14# morphine) with stronger ether to remove narcotine (vapKrj—torpor), drying the residue, and adding to it powdered milk-sugar to restore the original weight, Assay of Opium. U. 8. P. (Mohr’s modified process.) Opium (7 grams) is triturated with freshly slaked lime (3 grams) and water (20 cm3) to make a uniform mixture. Then water (50 cm3) is added and the mixture macerated with occasional stirring for one-half hour. Filter off 50 cm3 of liquid—representing 5 grams opium—add alcohol (5 cm3) and stronger ether (25 cm3); shake; add NH„C1 (3 grams), shake one-half hour and let stand 12 hours. Counterbalance two small filters, place one within the other and decant the ethereal layer as completely as possible on a filter. Add stronger ether (10 cm3) and rotate, again decant the ethereal layer upon the filter, and afterwards wash the filter with stronger ether (5 cm8). Dry the filter and pour upon it the liquid in the flask; wash the flask and filter, 200 MANUAL OF PHARMACY. with water (10 cm3); drain and dry the precipitate at 181°-140° F. Weigh crystals on inner filter, using the outer as a counterbalance. Multiply weight in grams by 20, and the product represents the per- centage of morphine. Explanation. The above process is dependent upon the solubility of morphine in milk of lime, narcotine being only slightly soluble. NIL,Cl is added, forming CaCl2 and NH4OH, the latter precipitating pure morphine. Ether is used to extract any narcotine that may be present, the alcohol dissolving coloring matter, resins, caoutchouc, etc. It is re- ported, on good authority, that this process yields 10% less morphine than really exists in the opium, this amount being retained in the mother liquor. Synopsis of a Method for the Extraction of Morphine. An infusion of opium is prepared, then the meconate and lactate of morphine in solution are decomposed by the addition of NH4OII, but which also precipitates coloring matter, and the other alkaloids, and in order to avoid this admixture with the precipitated morphine, alcohol is added to the solution to deprive it of its impurities and coloring matter. The crystals are purified by re solution and filtration with animal charcoal. Reaction. 2NH4C1 + Ca(OH)2 = 2NH4OH + CaCl 2. Cinchona. The bark of any species of Cinchona containing at least 3% of its peculiar alkaloids and at least 2% of quinine. (N.O. Ruhiacece.) Contains about 20 alkaloids. Cinchona Flava—Calisaya Bark. Cinchona Rubrum—Red Bark. Summary of Assay for Total Alkaloids. Make a milk of lime and mix with 20 grams cinchona (80 powder, and dried at 212° F.); dry the mixture below 176° F. (Kinate of calcium is formed, and the alkaloids are set free.) Digest with alcohol near the boiling-point for an hour; cool and filter; add q.s. dil. H2S04 ft. acid to test-paper (forming hydrosulphate of the alkaloids in solution). Let the pre- cipitate (CaS04) subside, filter the liquid, and wash the filter with alcohol. Evaporate the alcohol from the filtrate, filter and wash filter with dil. II2S04 until the washings give no turbidity with NaOH; concentrate by evaporation and add solution soda till strongly alkaline, forming Na2S04 in solution, the alkaloids precipitating. Collect the precipitate on a filter, wash, drain and dry. Multiplying the weight of the crystals in grams by 5 gives the percentage of total alkaloids. Assay for Quinine. Dissolve the total alkaloids from 20 grams cinchona in water with the aid of q.s. dil. H2S04 to make the liquid acid to test-paper (thus making acid hydrosulphates of the alkaloids); add solution of soda to neutralize the solution, thus producing neutral hydrosulphates, a small amount of Na2S04 being in solution. Digest and cool to 59° F. If crystals do not appear, the total alkaloids do ALKALOIDS. 201 not contain quinine in quantity over 8$ of their weight, or quinine hydrosulphate 9$—(the other alkaloids remain in solution). If crystals appear, filter the solution, washing the crystals on the filter with sufficient water to make the entire liquid weigh 90 times the weight of total alkaloids taken. Dry the crystals at 140° F. To the weight of the effloresced hydrosulphate of quinine so ob- tained, add 11.5$ of its amount for water of crystallization, and 0.12$ of the weight of the entire liquid for solubility of the crystals at 59° F. Multiplying the sum in grams by 5, equals the percentage of crystallized quinine hydrosulphate, equivalent to quinine in the cin- chona. Preparation op Quinine. Powdered cinchona is boiled with dil. HC1, forming soluble hydro- chlorides of the alkaloids, which are decomposed by lime, precipitating the liberated alkaloids, leaving CaCl2 and most of the impurities in solution. Dissolve out the alkaloids by digesting with alcohol, evaporate and dissolve the amorphous mass in dil. H2S04, forming the hydrosulphate. Dissolve and filter with animal charcoal to purify, and crystallize. Dissolve the crystals in water acidulated with H2S04, and add water of ammonia till no further precipitation i*esults, wash and dry. Kerosene is now employed by many manufacturers in the place of alcohol. General Tests for Alkaloids, yielding Characteristic Precipitates. Marines Solution, (Cdl2 (2); KI. (4); Water (12)) gives a gelatinous ppt. Mayer’s Solution of lodohydrargyrate of Potassium (HgCl2-13.5 grams; KI-49.8 grams; Water ft. 1 liter) produces a ppt. Sonnenschein’s Solution of sodium phospho-molybdate; yields a yellow ppt. Schiebler’s Solution of sodium phospho-tungstate; produces a ppt. Precipitates are also obtained with, Picric acid, mercuric chloride, platinic chloride, auric chloride, stannous chloride, tannic acid, Lugol’s Solution, potassium iodide, lead acetate, and lead subacetate. 202 MANUAL OF PHARMACY. Name, Synonym and Chemical Formula. Source. Natural Order. Description. Solubilities. Properties and Doses. Distinctive Tests. Apomorphince Hydrochloras (Hydrochlorate of Apo- morphine). c17h17no2.hci Morphine. (De- composition Product). Papaver- acece. Colorless, or grayish white crystals. Water, 6.8 Alcohol, 50 Ether, aim. ins. Chloroform,al. ins. Powerful emet- ic. Dose, J4 grain. atropine. On heating the diluted green so- lution obtained by the action ol sulphuric acid and bichromate potass, on atro- pine, the odor of roses and orange flowers is devel- oped. ACONITINE. 1. S u 1 p h u ric acid colors it orange yellow, changing to brown. 2. Characteris- tic tingling sen- sation when a drop of very dil- ute solution is placed on the tongue. Atropina. (Atropine.) C17H23NOs Root and leaves of Atropa Belladonna. Solanacece. Colorless, or white acicu- lar crystals. Water, 600 Alcohol, v. s. Ether, 60 Chloroform, 3 Mydriatic and narcotic Dose, T^-ifogr. Atropines Sulphas (Sulphate of Atropine). (C17H23N03)2H2S04 do. Solanacece. White crystal- line powder. Water, 0.4 Alcohol, 6.5 Mydriatic and narcotic, Dose, .Ij-Agr. Caffeina. (Caffeine.) C8H10N4O2.H2O Lvs. Camellia thea; Seeds Coffea arabi- ca; Paullinia sor- bilis. Temstrce- macece. Rubiaceoe. Sapinda- cece. Colorless crys- tals. Water, 75 Alcohol, 35 Ether, si. sol. Chloroform, 6 Nervous stimu- lant. Dose, 1-3 grs. Chinoidinum. (Chinoidine.) (Quinidin.) Cinchona Bark Mixture of alkaloids (by- products) Rubiaceoe. Brown or black amorphous solid. Water, aim. ins. Alcohol, v. s. Ether, si. sol. Chloroform, v. s. Tonic and anti- periodic. Dose, 5-30 grs. Cinchonidincs Sulphas. (Sul- phate of Cinchonidine.) (C20H24N2O)2H2SO4.3H20 Cinchona Bark Rubiaceoe. White silky needles or prisms. Water, 100 Alcohol, 71 Ether, sp. sol. Chloroform, 1000 Antiperiodic, tonic and an- tipyretic. Dose. 5-20 grs. Cinchonina. (Cinchonine.) C20H24NQO Cinchona Bark Rubiaceoe. White prisms or needles. Water, aim. ins. Alcohol, 110 Ether, 371 Chloroform, 350 Antiperiodic, tonic and an- tipyretic. Dose. 15-40 grs. Arrangement of Officinal Alkaloids. OFFICINAL ALKALOIDS. - Cinchoninoe Sulphas. (Sulphate of Cinchonine.) (CaoHa4NaO)aHaS04. 2Ha0 Cinchona Bark Rubiacece. Hard, white shining prisms Water, 70 Alcohol, 6 Ether, 60 Chloroform, insol. Antiperiodic, tonic and an- tipyretic. Dose, 15-40 grs. MORPHINE. 1. With solution of chloride of iron it gives a pale blue color, destroyed by acids or alcohol. 2. HN03 pro- duces a red color changing to yel- low. 3. Chlorine water & NH4OH gives red color changing to brown. MECONIC ACID. Tincture of chloride of iron gives dark red color. — Codeina. (Codeine.) C18HaiN03.Ha0 Opium. Papaver- acece. White or yel- lowish prisms. Water, 80 Alcohol, v. s. Ether, 10 Chloroform, v. s. Sedative. Dose, M gr. Hyoscya mince Sulphas. (Sul- phate of Hyoseyamine.) (Ci7Ha3N03)aHaS04 Leaves, Hyos- cyamus niger. Solanacece. Golden yellow or yellowish white crystal- line powder. Water, v. s. Alcohol, v. s. Narcotic seda- tive. Dose, sV gr. Morphina. (Morphine.) C17H19N03.Ha0 Opium. Papaver- acece. White crystals or powder. Alcohol, 10 Narcotic and sedative. Dose, i gr. Morphines Acetas. (Acetate of Morphine.) C,7H19N03HCaH3Oa.3HaO Opium. Papaver- aceoe. White or yel- lowish white crystalline powder. Water, 12 Alcohol, 68 Ether, 60 Narcotic and sedative Dose, i gr. Morphines Hydrochloras. (Hydrochiorate of Morph- ine.) C]7H19N03HC1.3Ha0 Opium. Pctpaver- aceoe. White, feath’ry acicular crys- tals. Water, 24 Alcohol, 63 Ether, insol. Narcotic and sedative. Dose, | gr. Morphince Sulphas. (Sulph- ate of Morphine.) (C17H19N03)aHaS04.5Ha0 Opium. Papaver- acece. White, feath’ry acicular crys- tals. Water, 24 Alcohol, 702 Narcotic and sedative. Dose. 1 gr. Magendie’s So- lutioncontains 2 grs. in each fluid-drachm. Physostigmince Salicylas. (Salicylate of Physostig- mine.) C16HalN30aC7He03 Seeds. Physo- stigma vene- nosum (Cala- bar Bean). Legumin- osoe. Colorlessacicu- lar or short columnar crystals. Water, 130 Alcohol, 12 Mydriatic nerve seda- tive. Dose. gV - A gr- Pilocarpince Hydrochloras. (Hydrochiorate of Pilo- carpine.) C„H16NaOaHCl Leaflets. Pilo- carpus pen- natifolius (Jaborandi). Rutacece. Small white crystals. Water, v. s. Alcohol, v. s. Ether, al. ins. Chloroform, al. ins. Diaphoretic and siala- gogue. Dose, gr. 204 MANUAL OF PHARMACY. Name, Synonym and Chemical Formula. Source. Natural Order. Description. Solubilities. Properties and Doses. Distinctive Tests. Quinina. (Quinine.) CaoHa4N202.3HaO Cinchona Bark Rubiacece. White flaky powder. Water, 1600 Alcohol, 6 Ether, 25 Chloroform, 5 Antiperiodic, tonic, antipy- retic Dose, 2-20 grs. quinine. 1. Solution in diluted H2S04 has blue fluor- escence. 2. Treated with chlorine water, followed by an excess of NH4OH gives an emerald green color and coagulum,known as Thalleiochin. 3. HN03 does not redden it. STRYCHNINE. 1. To cold sul- phuric acid add one drop of a so- lution of strych- nine and a small crystal of potas- sium bichromate. A deep blue color results, becom- ing violet, cherry- red, and finally fading. Quinince Hydrobromas (Hy- drobromate of Quinine.) CaoH24N202HBr.2H20 Cinchona Bark Rubiacece. Colorless lus- trous needles. Water, 16 Alcohol, 3 Ether, 6 Chloroform, 12 Antiperiodic, tonic, antipy- retic Dose, 2 -20 grs. Quinince Bisulphas. (Bisulphate of Quinine). CaoHa4Na02H2S04.H20 Cinchona Bark Rubiacece. Colorless or- thorhombic crystals. Water, 10 Alcohol, 32 do. Quinince Hydrochloras (Hy- drochlorate of Quinine.) C20H24N!iO2HC1.2H2O Cinchona Bark Rubiacece. White lustrous needles. Water. 34 Alcohol, 3 do. Quinince Sulphas (Sulphate of Quinine). (C20H24N2O2)2H2SO4. ?h2o Cinchona Bark Rubiacece. White filiform crystals. Water, 740 Alcohol, 65 Ether, slightly Chloroform, 1000 Glycerin, 40 do. Quinince Valerianas. (Val- erianate of Quinine.) • H20 Cinchona Bark Rubiacece. White pearly lustrous crys- tals. Water, 100 Alcohol, 5 Ether, slightly do. (Also nervine) Dose, 2-10 grs. Strychnina. (Strychnine.) C21H22N202 Strychnines Sulphas). Sulph- ate of Strychnine.) (C24H22N202)2H2S04.7H20 Seeds; Strych- nos Nux Vomica and Strychnos Ig- natia. Logani- acece. Colorless octa- hedral crys- tals or pow- der. Water, 6700 Alcohol, 110 Chloroform, 6 Ether, ins. Tonic and spinal nerv- ine. Dose, bV-yS gr. do. Logani- acece. Colorless or white pris- matic crystals Water, 10 Alcohol, 60 Ether. ins. do. Veratrina. (Veratrine.) Mixture of Al- kaloids from Asagrcea of- ficinalis. Melantha- cece. White amorph- ous powder. Water, v. si. sol. Alcohol, 3 Ether, 6 Chloroform, 2 do. Dose, gr. Arrangement of Officinal Alkaloids—Continued. GLUCOSIDES. 205 GLUCOSIDES. Glucosides are proximate principles that yield when boiled with a dilute acid, glucose and a new body. They are usually active principles, yet unlike the alkaloids, they do not combine with acids, but unite with alkalies to produce salts, and are not precipitated by tannic or picric acids. A few are active poisons, others are harm- less bitters, associated with resins, oils and alkaloids. Solvents: Some are soluble in water, some in alcohol, and others in ether. Officinal Glucosides, and Neutral Principles. A mixture of proximate principles (commonly mis-named chryso- phanic acid), extracted from Goa powder, a substance found de- posited in the wood of the trunk of Andira araroba. Description. Pale, orange-yellow crystalline powder; odorless; tasteless; almost insol. in water, si. sol. alcohol, sol. in ether and boiling benzol. Officinal Preparation. Unguentum Chrysarobini. (Ointment of Chrysarobin.) Contains chrysarobin (10), and benzoinated lard (90). Chrysarobinum.—Chrysarobin. (C2oH2S05.) Elaterinum.— Eeaterin. A neutral principle extracted from Elaterium, a substance de- posited by the juice of the fruit of Ecbalium Elaterium. (N. O. Cucurbitacese.) ' Extracted by dissolving out with chloroform, and precipitating with ether. Description. Small, colorless scales or prisms; odorless; bitter, acrid taste; neutral reaction; insol. in water, sol. in alcohol. Prop. Purgative. Dose TV grain. Officinal Preparation. Trituratio Elaterini (Trituration of Ela- terin). Contains elaterin (10), sugar of milk (90). A neutral principle prepared from the seeds of Anamirta paniculata (N. O. Menispermacece). Made by treating the kernel of the Cocculus Indicus seed (fish berries) with magnesia and hot alcohol; the evap- orated solution is treated with animal charcoal and crystallized. Description. Colorless, prismatic crystals; odorless; bitter taste; neutral reaction; sol. in water and alcohol. Prop. Tonic and antispasmodic. Dose -fa grain. PlCROTOXINUM.—PlCROTOXIN. A neutral principle obtained from the bark of Salix Helix, and other species of Salix. (N. O. Salicacece.) Preparation. A decoction of willow bark is deprived of tannin and coloring matter by precipitating with basic lead acetate, and the free acid neutralized with calcium carbonate. The filtrate on concentration yields crystals, which are purified by recrystallization. (CiaHisO,.) Salicintjm.—Salicin. 206 MANUAL OF PHARMACY. Description. Colorless, or white, silky crystals; odorless; bitter taste; neutral reaction; soluble in water and alcohol. On boiling with dilute acids the following decomposition takes place- Reaction. C13H18O7 -f- H20 — C7lls02 -f- CoHmOg. (Saliclu.) (Water.) (Saligenin) (Glucose.) Prop. Antifebrine. Dose. 20 - 80 grains. (C J 5 H1 gOa —246) S ANTONINUM. —S AN TON IN. A neutral principle prepared from Santonica. Made by exhaust- ing a mixture of santonica and lime with diluted alcohol, thereby obtaining a solution of calcium santoninate, from which the alcohol is distilled, and acetic acid added tq, the residue; santonin precipi- tates, and calcium acetate is in solution. Purified by treatment with animal charcoal, and recrystallization. Distinctive reaction: Yields a scarlet red liquid gradually becom- ing colorless with alcoholic solution of potash. Properties. Anthelmintic. Dose. Two grains. (2NaCi5H1904.7H20—698) Sodii Santoninas. (Santoninate of Sodium.) Made by heating solution of soda with santonin till dissolved; filter and crystallize. Description. Colorless, transparent crystals; becoming yellow on exposure to light; odorless; saline and bitter taste; slight alkaline reaction; sol. in water and alcohol. Other glucosides {unofficinai) with sources: TEaculin (horse-chest- nut); amygdalin (bitter almond); arbutin (uva ursi); arnidn (arnica); colocyntliin (colocynth); convallerin (lily of valley); convolvulin {scam- mony); crocin (saffron); daphnin (mezereum); digitalin (foxglove); gentiopicrin (gentian); glycyrrhizin (licorice); jalapin (jalap); populin (willow); quercitnn (oak); saponin (soap bark); thujin (arbor vita). ORGANIC ACIDS {not mentioned before). (HO7H5O6.EUO—188) Acidum Gallicum.—Gallic Acid. Found in nutgalls, sumach, uva ursi, etc. Made by macerating powd. nutgalls with cold water for about a month, then expressing, and rejecting the liquid. Boil the residue with water and filter while hot through animal charcoal, and set aside to crystallize. Purified by re-crystallization. By this process, pure tannin, which is digallic acid, an anhydride of gallic acid, is converted into the latter. Reaction. Ci4H10O9 -j- H20 = ‘hNHoOs. (Tannin.) (Water.) (Gallic Acid.) Description. Nearly, or quite colorless silky needles, or triclinic prisms; odorless; astringent, acid taste; acid reaction; sol. in water (100), alcohol (4.5), ether and glycerin. Impurities and tests: Tannic acid: -f- solution of alkaloids, gelatin, albumen, starch jelly, or tartar emetic with NH4C\,= ppt. Officinal Preparation. Unguentum Acidi Gallici (Ointment of gallic acid). Contains gallic acid (10), incorporated with benzoinated lard (90). Avoid use of iron spatula. ORGANIC ACIDS. 207 Pyrogallic Acid. (C6H603) Made by the sublimation of gallic acid, or powdered nutgalls. Reaction. O7H6O5 — CeHeOa —j— 0O2. (Gallic Acid.) /Pyrogallic\ /Carbon \ \ Acid. ) \Dioxide.) Properties. Readily reduces salts of mercury, silver, gold and platinum. Used with silver nitrate in photography, and for hair dyes and marking inks. {Ci4H10O9—chiefly) Acidum Tannicum.—Tannic Acid. (Tannin.) Made by exposing powdered nutgalls to a damp atmosphere, macerating with ether, expressing, evaporating and drying below 212° F. Description. Light yellow scales; faint, peculiar odor; astrin- gent taste; acid reaction; sol. in water (6), alcohol (0.6) glycerin (6). Test; see Gallic Acid. Officinal Preparation. 1. Collodium stypticum (see Collodium). 2. Trochisci acidi tannici (contain 1 grain each); 3. Unguentum acidi tannici (contains tannic acid (10) incorporated with benzoinated lard (90).) Avoid use of iron spatula. Valerianic Acid. (HC5H902—102) Occurrence. Found in valerian-root, chamomile, wormwood, angelica-root, etc. Preparation. Made from valerian-root by distillation; or arti- ficially by the action of H2S04 and potassium bichromate on fusel oil; the aqueous distillate is treated with NaOH, and the resulting salt of sodium valerianate decomposed by H2S04, liberating valeri- anic acid. Description. Colorless, thin oily liquid; disagreeable odor of valerian, and of old cheese; sour, acrid taste. Substances Contributed by the Animal Kingdom. (Officinals.) Source. Produced during the spontaneous fermentation of milk- sugar, under the influence of casein; this transformation is termed lactic fermentation. A similar change occurs in dextrin, glucose, cane-sugar, etc., by the action of casein and other proteids, conse- quently lactic acid is met with in many vegetable products which have become sour. Preparation. Now made from cane-sugar, which is changed into invert sugar by boiling with dil. H2SG4; solution of soda is added, and the mixture heated until it ceases to react with Fehling’s Solution. H2S04 is added to neutralize; the resulting Na2S04 is partly removed hy re-crystallization, and the remainder precipitated with alcohol. One half of the alcoholic liquid is heated, neutralized with zinc carbonate, mixed with the remainder and cooled. Zinc lactate crystallizes out, and yields the acid in solution when treated with H2S, zinc sulphide precipitating. Description. Nearly colorless, syrupy liquid; odorless; very acid (HC3Ht03—90) Acidum Lacticum.—Lactic Acid. 208 MANUAL OF PHARMACY. taste and reaction; miscible with water, alcohol and ether; sp. gr. 1.212; contains 75$ absolute lactic acid. Impurities: HC],H2S04,sarcolacticacid, lead, iron, sugar or glycerin. Officinal Preparation. Syrupus Calcii Lactophosphatis (see Cal- cium). Acidum Oleicum. (Oleic Acid.) See page 195. Adeps.—Lard. The prepared internal fat of the abdomen of the hog, Sus scrofa (Class, Mammalia. Ord. Pachydermata), purified by washing with water, melting and straining. Description. A soft, white, unctuous solid; melts at 95° F.; faint odor, free from rancidity; bland taste; neutral reaction; sol in ether, benzin and CS2. Used as a base for ointments as benzoinated lard, in which form it is protected from rancidity. Officinal Preparations. 1. Adeps benzoinatus (see page 175). 2. Ceratum (White wax (30), lard (70). 3. Ceratum resinae. Basilicon ointment. (Resin (35), yellow wax (15), lard (50)). 4. Unguentum— Ointment. (Lard (80), yellow wax (20)). Oleum Adipis. (Lard Oil.) See page 193. Cantharis.—Cantharides. (Spanish Flies.) Cantharis vesicatoria (Class, Insecta. Order, Co- leoptera (Beetles)). Collected chiefly in Hungary and Southern Russia. Its blistering properties are due to the presence of cantharidin (C10II12O4) which crystallizes in colorless prisms and scales; sol. in alcohol, ether, chloroform, acetic ether, glacial acetic acid, and oils. Cantharis presents a shining coppery-green color; grayish-brown in powder, containing green, shining particles; odor strong and disa- greeable. Should be kept in well-closed vessels containing a little camphor. Officinal Preparations. 1. Ceratum Cantharidis (Blistering Cerate); contains powd. cantharides (85), incorporated with yellow wax (20), resin (25), and lard (25). 2. Ceratum Extracti Cant! .ridis (Cerate of extract of cantharides); made by percolating powd cantharides (30) with alcohol, evaporating (to 15) and incorporating with resin (15), yellow wax (35), and lard (35), using heat. 3. Chart* Cantharidis (Can- tharides paper). 4. Collodium cum Cantliaride. 5 Linimentum Can- tharidis (Cantharides Liniment); contains cantharmes (15), and oil of turpentine ft. 100 made by digestion. 6. Tiactura Cantharidis (Tincture of cantharides) contains 5# cantharides. Carbo Animalis. See page 160. Cera Flava. See page 165. Cera Alba. See page 166. Cetaceum.—Spermaceti. A peculiar concrete fatty substance obtained from the bead of the sperm whale. The upper jaw of the whale has a large cavity containing an oily liquid, which is removed and congeals into a yellow mass, it is drained, and expressed to remove oil; the pressed cake is purified by THE ANIMAT PRODUCTS, 209 melting in water, skimming, boiling with KOH and washing with water. Constituents. Cetin (cetyl palmitate, Ci«H8s(Ci6HsiOa)), myristic, lauric and stearic acids, combined with alcohol radicals. Description. White, somewhat translucent masses, of a scaly, crystalline fracture; pearly lustre; becoming yellow and rancid on exposure to air; odorless; mild, bland taste; neutral reaction; sp. gr. 0.945; sol. in ether, chloroform, CS2, and boiling alcohol. Officinal Preparations. 1. Ceratum Cetacei. (Spermaceti cerate.) Contains spermaceti (10), white wax (85), and olive oil (55). 2. Ungu- entum Aquse Rosse. (Ointment of Rose Water. Cold Cream.) Melt together expressed oil of almond (50), spermaceti (10), and white wax (10), and mix with rose water (30). The dried female insect, coccus cacti (Class, Insecta. Ord. Hem- iptera.) Constituents. Besides fat, mucilaginous and glutinous com- pounds, cochineal contains carminic acid (CitIIibOio) to which it owes its red color. Carmine is obtained by treating a decoction of cochineal with a little alum, or cream of tartar, and setting aside to deposit. Use. A coloring agent, and enters into the preparation of Tinct. Cardamom Comp. COCCUS.—COCHINE AL. The fresh gall of Bos Taurus (Class, Mammalia; Order, Rumin- antia). A green or brownish-green, viscid liquid, which is separated by the liver in the gall-bladder. It has a peculiar odor; disagreeably bitter taste; slight alkaline reaction; sp. gr. 1.018-1.028; contains bilirubin (a coloring matter); a fat, cholestrin (C26H440), glycocholic and taurocholic acids. Officinal Preparations. 1. Fel Bovis Inspissatum. 2. Fel Bovis Purificatum. Fel Bovis Inspissatum. (Inspissated Ox Gall.) Made by heat- ing ox-gall to 176° F., straining, and evaporating to 15$ of its weight. Fel Bovis Purificatum. (Purified Ox Gall.) Evaporate ox gall to i its weight, treat with an equal vol. of alcohol, filter, distil off the alcohol, and evaporate to pilular consistence. Glycerinum. See page 195. Fel Bovis.—Ox Gall. Ox Bile. Ichthyocolla.—Isinglass. The swimming-bladder of Acipenser Huso, and other species of Acipenser. (Class, Pisces. Ord. Sturiones.) The officinal isinglass is that known in commerce as Russian, which is obtained from stur- geons in the Black Sea. The air-bag, or swimming-bladder, is cut open, washed, and dried by stretching on boards, the dried product being leaf isinglass. Sol. in boiling water, and boiling diluted alco- hol. Officinal Preparation. Emplastrum Ichthyocolla (Isinglass Plas- ter. Court Plaster). Made by coating taffeta on one side with a 210 MANUAL OF PHARMACY. solution of isinglass in water, glycerin and alcohol, and on the other with tinct. benzoin comp. Mel. See page 165. Moschus.—Musk. The dried secretion from the preputial follicles of Moschus mos- chiferous (the musk deer). (Class, Mammalia. Ord. Ruminantia.) Constituents: Cholestrin, various fats and wTaxy substances, gela- tinous and albuminous compounds, and salts. The odorous princi- ple is probably formed by the slow decomposition of one of its constituents. When treated with KOH, ammonia is given off. Officinal Preparation. Tinctura Moschi (Tincture of Musk. 10%). A fixed oil obtained from the fresh livers of Oadus Morrhuce, or other species of Oadus. (Class, Pisces. Ord. Teleostia.) The oil is separated and put into tanks in a cooling-room until it freezes, when it is placed in canvas bags and expressed, the product being an almost colorless liquid. Constituents. Besides the common fats, stearin, myristin, palmitin and olein, small quantities of iodine, bromine, phosphorus and sul- phur, also gadium (Cs5H4609). Description. Colorless, or pale-yellow, thin, oily liquid; slight- ly fishy odor; bland, slightly fishy taste;'faint acid reaction; sp. gr. 0.920-0.925; soi. in acetic ether, and ether, but scarcely in alcohol. Oleum MoRRHUiE. (Cod Liver Oil.) Pepsin, the digestive principle of the gastric juice, obtained from the mucous membrane of the stomach of the hog, and mixed with powdered milk sugar. Preparation. The well-washed fresh stomach of the hog is finely chopped, and macerated in water containing HC1; the pepsin is separated from the solution, by the addition of sodium chloride, which causes it to float on the surface of the liquid, it is then drained and dried. To make saccharaied pepsin, sufficient milk sugar is added to make a powder, 10 grains of which will dissolve 500 of coagulated albumen. Peptones. When fibrin or coagulated albumen are digested with pepsin, peptones are formed which have the property of di- gesting an additional quantity of the same, to a limited degree. Several so-called pepsins of commerce are simply dried peptones, and do not relieve the distress caused by certain digestive disorders in any considerable degree. Description. A white powder; slight, but not disagreeable odor and taste; slightly acid reaction. Not completely sol. in water, leaving floccules of pepsin floating in the solution, which dissolve on the addition of a small quantity of HC1. One part dissolved in water (500) containing HC1(7.5), should dissolve at least 50 of hard-boiled egg albumen in 5 - 6 hours at 100°-104° F. Officinal Preparations. Liquor Pepsini (Solution of Pepsin. Liquid Pepsinum Saccharatum. (Saccliarated- Pepsin.) TOXICOLOGY. 211 Pepsin). A solution of sacch. pepsin (4$) in glycerin and water acidulated with HC1. Use a filtered 3$ solvtion in water. 1. On boiling in a test tube; Peptone produces marked cloudiness and precipitation; Pepsin, a slight cloudiness without precipitation. 2. With strong iIN03, the Pepsin solution gives slight opales- cence, while the Peptone solution becomes yellow. 3. NaOH; precipitates Peptone, but not Pepsin. 4. NaCl; yields a white, gelatinous precipitate with Pepsin on standing; Peptone none. 5. Ba(OH)2: with Peptone, a precipitate; with Pepsin, none. 6. Alcohol: with Pepsin a gelatinous ppt. insol. in water; with Peptone a granular ppt. sol. in water. Saccharum Lactis. See page 165. Sevum. (Prepared Suet. Mutton Suet.) See page 193. Vitellus. (Yolk of Egg.) The yolk of the egg of Callus Bankiva, var. domesticus (Class, Aves. Order Gallince). Composition: 16$ Vitel- lin (a proteid closely related to casein), 30$ fat, 1.5$ organic salts coloring matter and sugar, 0.42$ cholestrin and 55$ water. [Oleum ovi (Oil of eggs). The fat expressed from the coagulated yolk, or obtained by exhaustion with ether.] Vitellus is used as an emulsifier. Officinal Preparation. Glyceritum Vitelli. (Glycerite of Yolk of Egg.) Contains fresh yolk of egg (45), and glycerin (55). Unofficinal Products derived from the Animal Kingdom. Ambergris; a morbid excretion from the intestines of the sperm whale, found floating on the sea. Used in making perfumes. Sanguis (Ox Blood). Castoreum (Castor); the preputial follicles of both male and female animals Castor fiber. Civet (from civet cat); used in perfumery. Blatta orientalis (cockroach). Egg A Ibumen. Extractum Carnis. (Extract of Beef.) Formic Acid. Gelatin. (Artificial isinglass.) Obtained by boiling in water under pressure, bones, cartilage, skins, ligaments, etc.; on cooling, a jelly results which is dried in the form of thin sheets. Colla (Glue). Obtained by subjecting the offal of abattoirs and tanneries to a process identical with that for making gelatin. Koumiss. Hirudo (Leech). Lac (Milk). Pancreatin. Obtained from the pancreas or sweetbread of sheep. An emulsifying agent, digesting the oils and fats. Tests to distinguish between Pepsin and Peptone. (Tofixot'—a poison; Aoyos—a discourse.) TOXICOLOGY. Poison. Any substance which, when introduced into the animal organism, swallowed, absorbed, or applied externally, will produce a morbid, noxious or deadly effect upon it. The poisons are derived from all three kingdoms, viz.: Animal: (Ex. Cantharides, cochineal, etc.) Vegetable: (Ex. Euphorbium, ela- 212 MANUAL OF PHARMACY. terium, savin, etc.) Mineral: (Ex. Mineral acids, copper salts, etc.) Antidotes. Two classes. First. Chemicals that cause a decomposition with the poison, giving rise to an insoluble or harmless body. Second. Alkaloidal Principles that have an antagonistic action to that of the poison, thereby counteracting its effect. General Remedies in Cases of Poisoning. Evacuation of the stomach (except in poisoning by the mineral acids) by means of the stomach pump, or the use of some of the fol- lowing emetics: Warm water in copious draughts, water containing a tablespoonful of mustard, salt water, zinc sulphate, copper sul- phate, ipecac, tartar emetic accompanied with ipecac, and me- chanically by tickling the throat with a feather, etc. Demulcents: Mucilages of acacia, flax-seed, or slippery elm bark; starch; egg albumen; olive oil; soapsuds; albumen, in the form of milk, flour, blood, etc. General Antidotes, in case the nature of the poison is un- known. A mixture of equal parts of magnesia, powd. charcoal and hydrated oxide of iron, given in water. Classification of Poisons. 1. Corrosive. Examples. Mineral acids, oxalic acid, caustic alka- lies, phosphorus, bromine, etc. 2. Irritant. Examples. Aloes, capsicum, colocynth, creasote, croton-oil, elaterium, euphorbium, gamboge, jalap, savin, scammony, etc. 3. Narcotic. Examples. Opium, HCN, hyoscyamus, cannabis indica, etc. 4. Narcotico-Irritant. Examples. Digitalis, veratrum viride, conium, colchicum, lobelia, aconite, belladonna, stramonium, tobacco, nux vomica, etc. Corrosives and Irritants. Their action is local, the Corrosives causing vomiting, acting mostly on the mucous linings of the oesophagus, etc., producing intense inflammation, while the Irritants exert their irritating action lower down, and especially on the bowels, producing hyper-catharsis. Narcotics. Symptoms: sleepiness, dimness of sight, stupor, de- lirium, etc. Alimentary canal not affected, but lower bowels con- stipated. / Narcotico-Irritants. Effects closely allied to the narcotics, but having a more direct action on the spinal marrow and nerves, producing more frequent occurrence of convulsions and paralysis. They differ much from each in their action on the system, and owe their properties to the presence of an alkaloidal principle. Symptoms: Vertigo, coma, delirium, paralysis, or convulsions, with pain and disturbance of the stomach and intestines. TABLE OF ANTIDOTES. 213 The following table gives the most recently approved antidotes for many of the poisons: Poison: Antidotes: Mineral Acids. j (H2S04, HN03. HC1, and \ nitro-hydrochloric acid.) J Oive.no emetic. Magnesia mixed with water, milk, chalk, whiting, potass, bicarb., fixed oils, demulcents. Laudanum (20 drops), it much pain. Vegetable Acids. (Oxalic acid and salts, j- Tartaric acid and salts.) j Chalk, whiting, air-slacked lime with vinegar. (No soda or potash to neutralize acid.) Mustard water, olive oil, demulcents and stimulants. Alkalies. ( (NaOH, KOH, NH4OH, ( and their carbonates.; ( Warm water till emetic; vinegar, lemon juice, or citric acid. Olive oil. demulcents, and lauda- num (20 drops) if much pain. Barium, lead, and their -j salts. ( Epsom 0 oz.) or Glauber’s salt (1 oz ) in water. Emetic (mustard water), milk and demulcents, and laudanum if needed. Arsenic, and all its com- -j pounds. 1 Emetic (mustard water"). Hydrated oxide of iron, or hydrated oxide of iron with magnesia, . olive oil, albumen, demulcents, and laudanum. Antimony salts, cantha- ] rides, colchicum, elateri- \ um, iodine, copper, mer- 1 cury, croton oil, savin, [ tansy, potass, bichromate, | tin and zinc salts. Albumen diffused in water. Emetics (warm water with NaHC03 or mustard), strong- tea or coffee, or tannin, stimulants, laudanum (if needed), and demulcents. Cannabis Indica, opium J and morphine. Emetics (mustard water) or stomach pump, cold affusions, strong tea or coffee; electro-magnetism. Keep patient awake and in motion. Artificial ( respiration. HCN (see page 111) and 1 cyanides, alcohol, chloral, \ chloroform, ether, CS2, | etc. J Emetics (mustard water), fresh air, keep body warm, rouse by ammonia, cold affusions, fric- tion and mustard plaster to limbs, and artificial respiration. Aconite, digitalis, ergot, 'i lobelia, tobacco, veratrum, \ belladonna, conium, hen- \ bane, santonin, stramoni- um, calabar bean. Emetics (mustard water); strong tea or coffee. Hypodermics of morphine; powdered charcoal; f stimulants (whiskey, etc.). Warmth to extremi- ties and artificial respiration. Nux vomica and strych- nine. ( Emetics (mustard water), powdered charcoal, 1 iodized starch, or tannin. To relieve spasms; in- { halations of chloroform, or internally 25 grs. chloral hydrate, or i oz. potassium bromide. ( Lose no time. Silver nitrate. ( Sodium chloride ; emetics (mustard water)— \ demulcents. Phosphorus. 1 Emetics (CuS04 —3 grains every 5 mins.), f 3 i | old spts. turpentine, MgS04 0 oz.). No oils. PART IV. URINALYSIS. Secretion and Excretion of the Urine. A theoky that is entirely satisfactory and explanatory of all facts concerning the secretion and excretion of the urine does not as yet exist. However, we may accept the following statements until a more probable theory is advanced. The Secretion of the Urine is the function of the kidneys, the process taking place in the cortical portion. The urine is filtered through the tubular portion, and after having undergone some elaborating action on the part of the epithelium of the tubules, is percolated through the apices of the tubular papillae into the pelvis of the kidney, and transmitted by it to the ureters. The Collection, Retention, and Excretion of the Urine is the function of the bladder and ureters. The ureters convey the fluid slowly, but continuously, into the bladder, where it remains de- posited until its accumulation excites a desire to void it. The excre- tion of the urine takes place through the urethra, and is caused by the action of the abdominal muscles and diaphragm, and the con- traction of the fibrous coat of the bladder. NORMAL URINE. Description of Normal Urine. This excrementitial fluid is thin and transparent; having a citron-yellow color; a peculiar, aromatic odor; a slight acid reaction, and an acid, saline and slightly bitter taste. In this connection, three distinct varieties may be recognized, viz.: a. Urina Potns. (Urine of drink.) Referring to urine voided some little time after taking fluids. It is generally pale in color, and of low sp. gr., ranging between 1003 and 1009. COMPOSITION OF URINE. 215 b. Urina Cibi. (Urine of digestion.) Urine passed after the digestion of a full meal. Darker in color; heavier odor, and higher sp. gr., 1020 to 1028 or 1030. c. Urina Sanguinis. (Urine of blood.) Secreted independently of the immediate stimulus of food and drink—as after a night’s rest. Usually of average density, and presents the essential characters of urine. Sp. gr. 1015-1025. Composition of Normal Urine. Represents mainly a solution of urea and sodium chloride with small quantities of other organic and inorganic constituents of the blood; also certain substances introduced into the system, which are excreted either in an unaltered condition, or after chemical decomposition. Inorganic Constituents. Sodium and potassium chlorides, phosphates of sodium, potassium, calcium, and magnesium; alkali sulphates, iron salts, gases (C02, N, and O), and coloring matters. Organic Constituents. Urea, uric acid, hippuric acid, xanthin, creatinin, lactic acid, mucus, coloring matters, etc. Substances found in Pathological Urine. Beside the above- mentioned normal substances, the following may be present, viz.: grape sugar, albumin, inosit, bile, ammonium and calcium carbon- ates, calcium oxalate, fats, leucin and tyrosin, pus, blood, casts, H2S, epithelium, tube-casts, spermatozoa, fungi, infusoria, etc. Average Composition of Healthy Urine. Percentage Grains Composition, per dap. Water 96.0 50 fl. ozs. Urea, 2.5 625.00 grs. Uric Acid, 055 13.75 Hippuric Acid, 050 12.50 Creatinin, .075 18.75 Pigment, Mucus, Xanthin, other extractives, etc., . .500 125.00 Phosphates of Mg and Ca, . .080 20.00 Phosphates of K and Xa, . .120 30.00 Chlorides of K and Xa, . .500 125.00 Sulphates of K and Ca, . .120 30.00 Total solids, .... 4.0 100.0 1000.00 grs. Although the above represents an analysis giving the chief con- stituents of the urine excreted by. a healthy male adult during 24 hours, yet even in health special circumstances may cause variations in the quantity of one or more constituents. • 216 MANUAL OF PHARMACY. THE STUDY OF URINE IN HEALTH ANI) DISEASE. As the condition of the urine points us to the changes going on in the economy, an analysis asserts its value in the diagnosis of disease, and in some instances it alone gives insight into the stage, nature and intensity of the disease. Although it is not to be supposed that all diseases can be diagnos- ticated by an examination of urine, yet it would be unjustifiable to neglect examination entirely. The various steps essential to the complete analysis of urine are treated of and classified in the follow- ing order: QUALITATIVE ANALYSIS. Physical Properties. a. Quantity per diem. b. Color. c. Transparency. d. Odor. e. Specific gravity. f. Reaction. g. Presence or absence of sediment. a. Chlorides. b. Sulphates. Normal Constituents. c. Phosphates. d. Urea. e. Indican. a. Albumin. b. Paragloblin, or Serum Globu- lin. c. Peptone. Abnormal Constituents. d. Mucin. e. Glucose. f Hilci Bile Pigment, *'• i5lle \ Rile salts. g. Blood. QUANTITATIVE ANALYSIS. a. Urinary solids. Acidimetry, Alkalimetry. e. Phosphates Alkali phosphates. Earthy phosphates. b. Reaction c. Sulphates. d. Chlorides. /. Glucose. g. Urea. h. Uric acid. i. Albumin. MICROSCOPICAL EXAMINATION. Unorganized Sediments. Urinary Deposits. a. Uric Acid. Amorphous, Crystalline. e. Calcium Oxalate. d. Phosphates. e. Leucin and Tyrosin. /. Cyst in. A. Acid urates ■ QUALITATIVE ANALYSIS OF URINE. 217 a. Blood Corpuscles. Organized Sediments, Blood, Hyaline, Wax, Epithelial, Granular, Oil or fatty, Mucous. Round, Flat, Columnar. b. Epithelial cells d. Tube-casts c. Mucus or pus corpuscles. e. Spermatozoa. Analysis of Calculi. Qualitative Analysis. All examinations of urine should be conducted with a part of the mixed urine voided during twenty-four hours, unless otherwise directed. PHYSICAL PROPERTIES. Quantity. Collect all of the 24 hours urine and measure it in a cylindrical graduate divided into cubic centimeters. The normal amount is 1000 to 1500 c.m.3 (88-50 fl. ozs.) for an adult male, and 900 to 1200 c.m.3 (80-40 fl. ozs.) for an adult female. In order to find the average excretion, the urine for several succes- sive 24-hour periods should be collected and averaged. Remarks. The quantity of urine voided depends: a. On the amount and kinds of food taken—some foods giving up water in the system, and others acting as a diuretic. b. On the perspiration, respiration, temperature and density of the atmosphere, amount of exercise, etc. The greatest quantity is secreted during the afternoon; the smallest during the night; the mean occurring in the morning, at which time the urine represents about an average, being least influenced by meals. Color. Into a beaker of 6-7 c.m (21-2f inch.) diameter, put 100 c.m.3 (3± ti. ozs.) of filtered urine. Look through it at the light from a win- dow (artificial light must be avoided), and note the color. Remarks. Urine colors may be classified as follows: 1. Pale ; colorless to straw yellow. 2. Ordinary; golden yellow to amber. 3. Highly-colored; red-yellow to brown Variation in color is due to excess or deficiency of water or color- 218 MANUAL OF PHARMACY. ing matter; to disease, and to the ingestion of certain foods and drugs. Abnormal Colors. A dirty green or reddish brown is due to the presence of bile pigments; blue color arises from indican, most fre- quently met with in cholera and typhus; a brownish color is some- times due to coffee; greenish-brown or yellow to rhubarb; red or crimson with alkali, to santonin; red to madder; black to logwood; brownish blue to black, to tar, carbolic acid, or creosote. Pathological importance increases directly as the color; high colors denoting acute disease, a pale color indicating chronic disease. (See Leucin and Tyro sin.) Transparency. Generally speaking, normal urine is transparent, although turbid- ity does not necessarily denote any pathological condition, and it by no means follows because a given specimen of urine is transparent that it is therefore normal. Urine containing a faint cloud of mucus soon after voiding, or urine that is partially opaque, owing to the presence of earthy phosphates, and forming a flocculent floating mass within half an hour afterwards, or a cloudy, bulky sediment within an hour, cannot be called abnormal. The mucus may be derived from the genito-urinary tract, while the earthy phosphates in the quantity mentioned may be due to diminished acidity and the substi- tution of alkalinity during digestion. Upon shaking normal urine, foam is formed which disappears in a short time; but if sugar, bile or albumin is present, the foam remains for some time. Put about 60 c.m.s (2 fl. ozs.) urine into a beaker of suitable ca- pacity and gently wave the beaker back and forth under the nose. Note whether the odor is “natural,” “strongly urinous,” “ am- moniacal,” “ like violets,” or otherwise peculiar. Remarks. Concentrated urines possess a strong odor. Old urines exhibit an ammoniacal, putrescent odor, which if observed in a recently voided specimen indicates chronic disease of the urinary tract. Peculiar odors are imparted to healthy urine by certain kinds of food and drugs, viz.: copaiba, cubebs, sandalwood, turpentine, asparagus, sodium salicylate, saffron, etc. Odor. Determined either by the use of the urinometer or sp. gr. bottle. The sp. gr. must be taken at the temperature of 60° F. (15.6° C.); if of a different temperature, it must be warmed or cooled by im- mersion in warm or cold water until the proper temperature is reached. Specific Gravity. QUALITATIVE ANALYSIS OF URINE—REACTION. 219 If the urinometer is used, it should be first tested with distilled water at 60° F., into which it should sink to the mark 0 or 1000. The cylinder used should have a diameter double that of the urin- ometer bulb, and of such length that the instrument may be com- pletely immersed. Use. Fill the cylinder to within one-fourtlx of the top, remove all air-bubbles with filtering-paper, float the urinometer in the urine, and fill to the brim, reading the sp. gr. at the point where the meniscus cuts the graduation of the instrument. If only a limited amount of urine is attainable, and insufficient to fill the cylinder, the sp. gr. may be determined as follows: Add to the urine enough 'distilled water to fill the tube, and take the sp. gr. of the mixture. Suppose it requires the addition of six times as much water as urine, making seven volumes, and the sp. gr. of the mixed fluid is 1003, then that of the urine will be 1000 + (3 X 7)= 1021. The average sp. gr. of normal urine is about 1020, but this figure varies considerably even in healthy urine. (See page 214.) If persistent above 1015, Albuminaria or Diabetes Insipidus may exist; if persistent above 1030, Diabetes Mellitus may be suspected. Reaction. Dip a piece of red and a piece of blue litmus paper into the urine. If the original colors remain, the reaction is neutral; if the red turns blue, the urine is alkaline; if the blue paper turns red, the re- action is acid; if no change, the urine is neutral. In order to determine whether an alkaline urine contains either volatile or fixed alkali, moisten one-half of a piece of red litmus paper with the freshly voided urine and dry it; if on drying the blue color remains, the alkalinity is due to fixed alkali (soda or potassa), while if the blue color becomes red, to volatile alkali (ammonia). If a slight excess of HC1 is added to a portion of the warm urine in a test-tube and effervescence results, the alkalinity is caused by carbonates; if no effervescence results, to phosphates. Remarks. The normal urine of 24 hours is acid, but this acidity is not due to free acids, but to the presence of acid salts—as NaH2P04, and sometimes to uric and hippuric acids. Great acidity is of importance, from the fact that it may favor the development of sediments or calculi, thereby causing irritation of the kidneys and urinary passages. Acid Fermentation. An increased acidity is sometimes de- veloped in urine that has been standing for a short time at a moder- ate temperature, during which time the mucus acting as a ferment decomposes the coloring matters of the urine, setting free lactic and acetic acids which cause a decomposition of urates, precipitating uric and oxalic acids, the acid urates of sodium, potassium, etc. Alkaline Fermentation. On standing for a longer time, espe- cially during hot weather, urine develops an ammoniacal odor and 220 MANUAL OP PHARMACY. acquires an alkaline reaction, due to the action of mucus as a fer- ment, which decomposes urea into ammonium carbonate according to the following reaction: CII4N20 + 2H20 = (NH4)2C03, (Urea.) (Water.) /AmmoniumX \ Carbonate. ) and causes deposits of the crystalline or triple phosphates of ammo- nium and magnesium, of the amorphous phosphate of calcium, of ammonium urate and bacteria. Presence or Absence of a Sediment. A portion of urine (one or two 11. ozs.) should always be set aside in a moderately cool place for a few hours in a conical glass vessel in order to collect any sediment that may appear. The supernatant liquid should receive further examination. NORMAL CONSTITUENTS. Test. Put about 5 c.m.3 (90 nj,) of urine into a test tube, acidulate with a few drops HN03 and add solution AgN03; a curdy white ppt. results. Chlorides. Reaction: NaCl + AgN03 = AgCl -f- NaN03. / Sodium \ / Silver \ / Silver \ /Sodium \ (Chloride.) (Nitrate./ (Chloride.) (Nitrate.) add an excess of NH4OII and agitate,—the ppt. re-dissolves, now add HN03 again till in excess and the white ppt. again forms. Sulphates. Test. To 5 c.m.3 (90 iU) of the urine acidulated with HC1, add a few drops of sol. BaCl2, a white turbidity or ppt. results. Reaction: H2S04 + BaCl2 = BaSQ4 + 2HC1. /SulphurieX / Barium \ / Barium \ /HydrochloA ( Acid. ) (Chloride./ (Sulphate.) ( ric Acid. ) Tests, a. To 5 c.m 3 (90 tti) of urine add a few drops of magne- sian mixture ; a white crystalline ppt. results, soluble in HC1. b. To 5 c.m.3 (90 nt) of the urine add sol. AgN03; a yellow ppt. results which re-dissolves on addition of NH4OH in excess. c. Add sol. AgNOa to a second portion; the ppt. is dissolved on adding HN03 and agitating. Phosphates. Urea. (Carbamide.) (NH2)2CO. Urea is the result of the oxidation of nitrogenous substances. Test. Evaporate the urine to a thin syrupy consistence, and add HN08; urea nitrate crystals will precipitate iu rhombic plates. By ABNORMAL URINE CONSTITUENTS—ALBUMIN. 221 decomposing them with BaC03, and drying, the urea may be dis- solved out with alcohol, crystallizing from the solution in four-sided prisms. Indican. Indican is a pigment always found in normal urine, but present in excess in certain pathological specimens. Test. Put about 3-4 c.m.3 (50-60 H) IIC1 into a beaker, and to this add 10-20 drops of urine, and stir the mixture with a glass rod. Under normal conditions indicau is present in sufficient quantity to give only a light yellowish-red tint; but if the acid, becomes blue or violet, then indican is present in excess. Biliary coloring matters interfere with the above test; therefore these must be removed before applying the test, by precipitation with lead acetate, and filtration. ABNORMAL CONSTITUENTS. Albumin, Normal urine should never contain albumin. It is frequently found in great quantities during disease of the kidneys as serum albumin or paraglobulin. If other fluids are pres- ent in the urine (blood, pus, etc.l, that kind of albumin which is characteristic of these will be found. Urine containing albumin has usually a lighter sp. gr. than normal urine, because the normal quantity of urea is not excreted. In true albuminaria it is important that the amount of albumin excreted in 24 hours be determined in order to note whether im- provement is, or is not, taking place. [If the urine is not perfectly clear, filter.] Tests, a. Ascertain the reaction of the urine. If alkaline, make it faintly acid to blue litmus paper with acetic acid, and fill the test- tube nearly to the top with the acidulated urine. On holding the tube at the bottom and heating the upper portion to near the boiling- point, phosphates and albumin are precipitated, rendering the liquid more or less opaque. Now add slowly HN03 (25 to 30 drops); phosphates are dissolved, and any remaining ppt. indicates albumin. b. A cold solution of picric acid precipitates albumin, alkaloids, oleo-resins, and peptones, and on heating all but albumin re-dissolve. c. Heller’s Test. Put about 2 c.m.3(30 m,) of HN03 into a test- tube. Hold the tube at an angle of about 45°, and allow the urine to trickle slowly from a pipette (the upper end of which has been slightly roughened by a file) down the side of the tube upon the sur- face of the HN03; a sharp white band or milky zone at the point of contact denotes albumin. Caution. Urine containing excess of urates hut no albumin will cause a white zone, which is, however, observed above the point of contact of the liquids, and although its lower border is sharply 222 MANUAL OF PHARMACY. defined, the upper border fades gradually into the layer of urine which may become turbid ; this turbidity may be dissipated by cautiously holding the tube in hot water. If resinous bodies are present, these may precipitate with IIN03; but the yellowish-white ring thus formed is dissolved on adding alcohol. Concentrated urines (those highly charged with urea) sometimes cause crystalline rings of urea nitrate, but these are dissolved by placing the tube in hot water. Urines containing an excess of coloring matter or bile pigments may yield a ring of deep coloration at the point of contact, thereby con- cealing the milky zone obtained with albuminous urine. Paraglobiu or Serum Globulin. Test. Dilute filtered urine (previously made faintly acid with acetic acid if necessary) with water to sp. gr. 1002; a cloudiness on diluting or after passing through it a current of C02 indicates para- globin. Peptone. The urine must first be freed from mucin and albumin, and de- colorized by the following method: Add to 500 c.m.3 (17 fl. ozs.)of urine, neutral lead acetate solu- tion till no further ppt. occurs, and filter. To the filtrate add acetic acid and a few drops of fresh sol. potass, ferrocyanide. Any ppt. indicates albumin; to remove which the ferrocyanide solution is added as long as a ppt. occurs, and the solution is filtered. Tests, a. To a portion of this filtrate add 20$ of its bulk of acetic acid, and then an acid solution of sodium phospho-tuugstate; any immediate cloudiness, or after ten minutes, indicates peptone. 1). To another portion of the above filtrate add one-half its volume of HN03, and completely ppt. with sol. sodium phospho-tungstate. Wash the ppt. as quickly as possible upon a filter with dilute 1I2S04 (1-20) till the washings are colorless. Mix the washed ppt. thoroughly with powd. Ba(OH)2; add a little water, and, after warming for 15-20 minutes on a water bath, filter. Make a portion of the filtrate strongly alkaline with sol. KOII, and add one drop of test-sol. CuS04. A reddish violet color denotes peptone. Mucin. Pour 2 c.m.3 (30 til) of acetic acid into a test-tube, and overlay it with clear urine. A cloudiness forming after standing for a time, and remaining undissolved on heating, just above the point of contact of the two liquids, indicates mucin. Glucose. (Grape-Sugar.) (C8Hi206.) Note. In testing for glucose the urine must Refresh and free from albumin, and, if not already of an acid reaction, must be acidulated with acetic acid. To remove the albumin: beat the urine in a flask TESTS FOR GLUCOSE AND BILE. 223 till it boils, add 2 drops acetic acid, and boil for 20-30 minutes, ol until the albumin separates as a tlocculent ppt., and filter. Tests, a. Eeliling’s Test. Put about 2 c.m.3 (30 ik) of Felil- ing’s solution (see page 164) into a test-tube and boil; the presence of any red coloration or specks indicates the deterioration of the solu- tion, and it should be replaced by some that has been freshly mixed. If it remains clear, add to it 2-3 drops of urine and boil again. In the absence of a red color, add more urine and boil again. Repeat until a red or yellow ppt. appears—showing the presence of grape-sugar—or until a bulk of urine equal to that of the reagent has been used without developing a red ppt., in which case sugar is absent. b. Moore’s Test. To 4 c.m.3 (60 ni) of the urine in a test-tube, add 2 c.m.3 (30 ik) of sol. KOH and boil for about one minute. If glucose is present, a yellow color appears, darkening to brown as boiling is continued. The addition of a few drops of HNOs decolorizes the liquid and develops the odor of burnt sugar. c. Boettger’s Test. Make the urine strongly alkaline with Na2C03 and place a portion in each of two test-tubes. To one add about three grains of bismuth subnitrate, and to the other an equiva- lent amount of litharge, and boil each for 1-2 minutes; in the pres- ence of sugar, black metallic bismuth deposits, while litharge is un- affected. Note. Both the subnitrate and litharge are blackened by urine containing a sulphide or any compound containing sulphur. (1. Indigo-carmine Test. Place 2 c.m.3 (30 ttlj of the urine in a test-tube, add powd. Na2Co3 till strongly alkaline, and sufficient solution indigo-carmine (sodium sulph-indigdtate) to produce a blue color; heat to boiling with as little agitation as possible. If glucose is present, a beautiful violet-color develops in the blue solution, quickly changing to purple, red, orange, and finally becomes of a straw-color. Now shake the tube and the colors return in the in- verse order in which they appeared, the rapidity with which the colors change depending upon the amount of glucose present. Remarks. Diabetic urine usually has a high sp. gr. 1025-1050, is of a pale color, is abundant in quantity (often enormously so), and has a sweetish odor and taste. The breath of some persons suffering with diabetes has an odor of chloroform: the urine, odorless when voided, soon develops a sim- ilar odor. 1. BILE PIGMENT. Always dilute dark-colored urines for these tests, and examine the urine as soon as possible after it has been voided. a. Gmelin’s Test. Pour about 3 c m.3 (48 irt) of fuming HNOs (nitrous acid) into a test-tube, and overlay it with an equal volume of the urine; if biliary coloring-matters are present, a set of colors is formed at the point of contact of the two liquids, with green upper- Bile. (Pigment and Salts.) 224 MANUAL OF PHARMACY. most and gradually rising higher, and is succeeded from below by blue, violet, red, and yellow or yellowish-green. Green is the important color in this test; as the other colors may be absent or may be produced by other coloring-matters, especially indican. Note. Nitrous acid for the above test may be produced by placing a piece of wood into pure HN03; heat until the acid assumes a yellow color; pour into another test-tube, and cool. b. On agitating the urine with ether, decanting the yellow etheral layer which separates on standing, and underlying it with a dilute sol. bromine (.aqueous), the ether assumes a blue color. c. Ultzinanii’s Test. Put 10 c.m.3 (165 tti) of urine into a test- tube, add 3-4 c.m.3 (48-60 ti() sol. potassa (1 in 3), shake, and acidulate with HC1; the mixture turns emerald-green. 2. BILE SALTS. Before applying the test, all albumin, mor- phine, and other occasional constituents of the urine which have the same reaction as the biliary salts should be removed in the following manner; Evaporate about 60 c.m.3 (2 fl. ozs.) of the urine to dry- ness, using a water-bath. Treat the residue with 6 c.m.3 (90 rip) strong alcohol, filter, and mix the filtrate with 60 c.m.3 (2 fl. ozs.) of stronger ether. Drain the ppt. which results on a small filter, wash it with ether, and dissolve in 2 c.m.3 (30 tt[) distilled water. This liquid represents a solution of the biliary salts, to which may be applied the following test: Pettenkof'er’s Test. To the above solution add one drop of sol. cane-sugar (1-3), and float on the mixture a little H.2S04 (the two liquids must not be allowed to mix). If the bile acids are present, the urine becomes and, on standing, a purple-red zone forms at the point of contact of the two liquids, which gradually mix, form- ing after a few hours a homogeneous dark-purple liquid. Blood. Test. a. If alkaline, make the urine faintly acid with acetic acid. Heat to near the boiling-point; and if blood is present, the color be- comes lighter and a dark-colored coagulum is formed. b. Alemen’s Test. Mix equal parts of oil of turpentine and tincture guaiac, agitate well, and add drop by drop an equal volume of urine. Shake gently and allow the emulsion to separate. Blood gives a blue or greenish-blue color c. Heller’s Test. Make the urine distinctly alkaline with KOH and gently heat to near boiling; a blood-red ppt. results if blood- pigment is present. If a ppt. does not form, add 1-2 drops of the magnesian mixture and heat as before. (Quantity of Total Urinary Solids. Quantitative Analysis. The normal quantity of solids excreted in 24 hours is 60-70 grams. The presence of more than 200 grams indicates diabetes; or if only 21 grams (the quantity of urine being normal) hydruria. QUANTITATIVE ANALYSIS OF URINE REACTION. 225 The quantity of solid matter (and with this as a factor, the amount of water) may be approximately estimated in the following manner: Method. Determine the amount of the 24 hours’ urine, and its sp. gr. Multiply the two last figures of the sp. gr. (expressed in four figures) by 2.33, and the product represents the number of grams of solids in 1000 c.m.3 of urine ; this, when multiplied by the number of c.m.3 of urine and divided by 1000, gives the number of grams in the urine of 24 hours. Example. Urine in 24 hours = 1500 c.m.3 — sp. gr. = 1025. 58 25 V 1 500 25 X 2.33=58.25 grams in 1000 c.m.3-—^Q -~ = 87.375 grams. Reaction. The normal amount of acidity of the 24 hours’ urine is equivalent to 2-4 grams oxalic acid. a. Acidimetry. To determine the degree of acidity of urine, prepare a decinormal volumetric solution of caustic soda by diluting the volumet sol. of soda with 9 times its weight of distilled water. Thus prepared each c.m.3 contains 0.004 gram NaOH (absolute), and is the equivalent of 0.0063 gram oxalic acid (H2C2O4 2H20). Put 50 c.m.3 of urine in a beaker, and add gradually from a burette the decinormal solution of soda until the mixture on stirring shows a neutral reaction with litmus or some other suitable indicator. The number of c.m.3 of soda solution used (as shown by the burette) multiplied by 0.0063 shows the acidity of 50 c.m.3 of urine repre- sented in grams of oxalic acid; and the total acidity is determined by multiplying by the quantity of urine in 24 hours and dividing by 50. Example. Urine in 24 hours — 1500 c.m.3 Decinormal solution soda used = 15 c.m.3 15 X 0.0063 = 0.0945 gram of oxalic acid = 50 c.m.3 urine. 0.0945 X 1500 _ CQ .. ... 0.. = 2.83 grams = oxalic acid in 24 hours urine. b. Alkalimetry. To determine the degree of alkalinity of urine, prepare a decinormal volumetric solution of oxalic acid by diluting the volumetric solution of oxalic acid with nine times its weight of distilled water. Thus prepared, each c.m.3 contains 0.0063 gram oxalic acid (H2C2O4.2H2O), and is the equivalent of 0.004 gram NaOH (abs.). Follow out the same scheme as for acidimetry, using decinormal sol. oxalic acid instead of the soda solution. By multiplying the number of c.m.3 of acid solution employed to neutralize the urine by 0.004, the alkalinity of 50 c.m.3 of urine is determined; this result, multiplied by the total quantity and divided by 50, shows the alkalinity of the urine of 24 hours. Example. Urine in 24 hours = 1250 c.m.8 Decinormal acid solution used = 8.6 c.m.3 8.6 X 0.004 = 0.0844 gram = NaOH = alkalinity of 50 c.m.3 urine. 0.0344X 1250 . — = 0.86 gram = soda solution in 24 hours urine. ou 226 MANUAL OF PHARMACY. Sulphates. (Estimated as II2S04.) Normal amount of Hu SO, = 1.5-2.5 grams daily. The sulphates found in urine are the neutral sulphates of sodium and potassium. Method. Acidulate 100 c.m.3 urine with HC1 5 c.m.3; heat slowly to near the boiling-point, and add test-sol. barium chloride until a ppt. ceases to be formed. Drain the ppt. on a filter and dry below 210° F. Burn the filter in a tared platinum crucible until a white ash re- mains. Subtract the weight of the crucible and filter ash from the weight of the crucible, ash and BaS04, and multiply the difference by 0.421 = weight of H2S04 in 100 c.m.3 urine; this weight, multi- plied by the c.m.8 of 24 hours’ urine and divided by 100 = amount of H2S04 for 24 hours. Example. Urine in 24 hours = 1350 c.m.3 Weight of crucible, BaS04 and ash = 36.4921 grams. “ “ “ and ash = 36.1101 “ Weight of BaS04 = 0.3820 “ 0.382 X 0.421 = 0.1608 = grams H2S04 in 100 c.m.3 urine. 0 1608 X 1350 Tt o . t. , . Jqq =2.17 grams = H2q04 in 24 hours urine. Chlorides. (Estimated as NaCl or Cl.) Normal amount as NaCl = 10-12 grams daily or 6-7.2 grams Cl. The kidney excretes only the excess of chlorides; their increased diminution represents an increase of the disease (in connection with acute processes) and vice versa. Absence of chlorides always indi- cates a grave affection. All albumin, mucus, and uric acid should be removed by the fol- lowing method before applying the reagents : Mix 5 c.m.3 of urine with 2 grams pure sodium nitrate, and evapo- rate in a platinum capsule over a water-bath; ignite at a red heat until a colorless fused mass remains; cool, and dissolve the residue with hot distilled water, filter, acidulate with HN03 and neutralize with powdered CaC03. Method. To the solution thus obtained, add 2 drops teet-sol. potassium chromate (as an indicator), and titrate the mixture with volumetric solution of silver nitrate, from a burette, until a red ppt. remains on stirring. Each c.m.3 of the AgN03 so ution used contains 0.01697 gram AgN03, representing 0.00584 gram NaCl in 5 c.m.3 urine, from which the NaCl in 24 hours is estimated. The quantity of NaCl multiplied by 0.6 gives t,lie amount as chlorine. Example. Urine in 24 hours = 1350 c.m.3 Vol. sol. AgN03 used = 12.5 c.m.3 12 5 X 0.00584 = 0.073 grams NaCl in 5 c.m.3 urine. 0 v 1 *-^0 — •- = 19.71 gms. NaCl(X 0.6=11.8gms. Cl)in24hrs- urine. o 227 QUANTITATIVE ANALYSIS OF URINE PHOSPHATES. The normal daily elimination of phosphoric oxide (P205) is about 2.5-3.5 grams, of which 1.7-2.3 grams are in combination as alkali phosphates, and 0.8-1.2 grams as alkaline earth phosphates. The daily variations may be great, the maximum quantity being present after a meal until evening, the minimum during the night until next morning. Their clinical significance depends on their state, but not on their amount. When they are persistently thrown out of solution, the probabilities are that a calculus may be formed. Methods, a. Phosphoric Oxide (P30B). Mix 50 c.m.3 of urine with 5 c.m.3 of sodium acetate sol. and heat on a water-bath. From a burette containing sol. uranium acetate, add 1 c.m.3 at a time until a drop of the mixture, when placed on a piece of white porcelain, produces a brown color on the addition of test sol. potass, ferro- cyanide. Multiplying the number of c.m.3 of uranium solution used, by 0.005 (1 c.m.3 uranium sol = 0.005 grams P206) shows the amount of P205 in 50c.m.3 urine. Find the amount in 24 hours’ urine by a method in accordance with the following example: Phosphates. (Estimated as P205.) Example. Urine in 24 hours = 1400 c.m.3 Uranium solution used = 22.5 c.m.3 22.5 X 0.005 = 0.1125 grams = P205 in 50 c.m.3 urine. 1400 X 0.1125 1R n . 0. . = 3 15 = grams P205 in 24 hours. b. Phosphoric Oxide Combined as Alkaline Earth Phos- phates. Add NH4OH to 100 c.m.3 urine till alkaline, and set aside for 12 hours. Wash the ppt. which forms, on a filter with diluted NH4OH (1:3). Perforate the apex of the filter and wash the ppt, through the hole into a beaker with water acidulated with a very few drops of acetic acid, and add sufficient acetic acid to just dissolve. Add 5 c.m.3 sodium acetic solution and enough water tc make 50 c.m ,3 and titrate as given under a. c. Phosphoric Oxide Combined as Alkali Phosphates. Sub- tract the amount of P205 as obtained in b, from the total P205 shown by a, and the difference shows the amount combined as alkali phosphates. Glucose. Grape-Sugar. (C6H,206.) Into a half-pint flask pour 20 c.m3 of H20 and 10 c.m.3 of Fehl- ing’s solution (see page 164). If the urine is highly saccharine, dilute it with 9 vols. H20; if containing but a small quantity of glucose, dilute with 4 vols. (or less) H20 (the amount of dilution necessary is shown by the degree of reaction in the qualitative reaction (see page 222), and fill the burette with the mixture. Heat the Fehling’s solution to boiling, add a few drops of NH4OH and run in about 5 c.m.3 of the diluted urine from the burette, and boil again, Repeat the alternate addi- tion of urine and boiling until the blue color is very faint, then add 228 MANUAL OF PHAEMACY. only 1 c.m.3 at a time, and boil until the blue color is just dis- charged, which may be determined by filtering a few drops into a white porcelain capsule and noticing the color. Divide the c m.3 of copper solution used, by 5 or 10 (dependent as to whether the urine wTas diluted with 4 or 9vols. H20), and the quotient gives the number of c.m.3 of urine, each representing 0.05 grams glucose, from which calculate the total daily elimination as follows : Example. Urine in 24 hours = 2300 c.m.3 Diluted urine (1:4) used = 20 c.m.3 20 ~s- 5 = 4 = c.m.3 urine containing 0.05 grams of glucose, or 80 c.m.3 urine = 1 gram glucose. 2300 -i- 80 = 28.75 grams glucose in 24 hours. Urea. (NH+CO. Urea is the most constant constituent of the urine and the one that occurs in greatest amount, representing nearly one-half the total urinary solids, or about 30-40 grams daily. Any excess is indicated by a higher, or a deficiency by a lower, sp. gr. than normal. Explanation of Fowler’s Method of estimation. This method is based upon the fact that the difference in sp. gr. of urine, both before and after the decomposition of its urea by the hypochlorites, bears a definite relation to the quantity of urea present. Every degree of sp. gr. (represented by four figures) lost represents about 0.77$ or 3) grs. per fl. oz. Seven parts of sol. chlorinated soda (Squibb’s) will decompose the urea in one part of urine unless the quantity is in great excess, in which case the urine should be diluted with an equal volume of water, and the final result multiplied by 2. The following reaction shows the decomposition of urea: N2H4CO + 3Na2OCl2 = 6NaCl + C02 +177 4- 2HaO. /CTreaA /Chlorinated\ ( Sodium \ / Carbon \ /NltvogenA / Water. \ J V Soda. 1 (Chloride.) (Dioxide.) V ) V ) Fowler’s Method. Ascertain the sp. gr. of the urine, and of some Liq. sod® chlorate (Squibb’s) at the same temperature, and dilute 1 vol. of the urine with 7 vols. of the solution. Brisk effer- vescence results, due to the evolution of N and C02. Let the mixture stand for one hour, agitating at intervals, and take its sp. gr. at the same temperature as employed above. Add once the sp. gr. of the urine to seven times the sp. gr. of the soda solution and divide the sum by 8. From the quotient thus obtained, subtract the sp. gr. of the mix- ture after decomposition; multiply the difference by 0.7791, and the product represents the amount of urea in 100 c.m.3 of urine, from which determine the amount in 24 hours’ urine as follows : Example. Urine in 24 hours = 1300 c.m.3 Sp. gr. of liq. sod® chlorate = 1042 “ “ “ urine =1022 “ “ “ mixture after decomposition = 1035.5. QUANTITATIVE ANALYSIS OF URINE ALBUMIN. 229 (1042 X 7) + 1022 g— = 1039.5 = sp.gr. of mixture before decomposition. .Aoe, ». . . . 0.7791 x 4 x 1300 .. 1039.5 — 1035 5 = 4= loss in sp. gr. = 40.513 grams urea in 24 hours. Uric Acid. (C5H4N4O8.) The normal daily amount of uric acid eliminated = 0.5-1.0 grams. Acidulate 200 c.m.3 of urine with 20 c.m.3 HC1, and let stand in a cool place for 48 hours. Collect the crystals of uric acid that have formed, on a filter, and wash them with water until the filtrate has a neutral reaction to litmus. Dry the filter and uric acid at 212° F., and weigh. From this weight deduct the weight of the filter, and the result represents the uric acid in 200 c.m.3 of urine, except the small portion dissolved in the washings, for which add 0.000038 gram for each c m.3 of wash water used, and determine the amount in 24 hours’ urine in the following manner : Example. Urine in 24 hours = 1540 c.m.3 Weight of dried filter with contents = 1.238 grams Tare of filter = 1.097 “ Approximation of uric acid in 200 c.m.3 = 0.141 “ Wash water 52 c.m.3 X 0.000088 = 0.0019 “ Corrected uric acid in 200 c.m.3 = 0.1429 “ 0.1429X 1540 1 i aaq • = 1.1003 grams uric acid in 24 hours. a. Eschbacli’s Method. This test requires the use of the albu- minometer, which consists of a glass tube 15 c.m. long and 1.5 c.m. in diameter, graduated into grams, and having two marks, one near the middle marked U, the other near the top marked R. The test solution required consists of 10 grams picric acid, 50 c m.3 acetic acid, and 1120 ft. 1 litre. Process. An alkaline urine should be acidulated with acetic acid. If the sp. gr. of the urine is less than 1008, fill the tube to the lower mark, U, with it, and add sufficient of the test-sol. to fill to the upper mark, R. Close the opening of the tube with a rubber stopper and set aside for twelve hours, shaking two or three times during that period to insure the deposition of the albumin. The amount of albumin is read off at the graduation. If the sp. gr. of the urine is above 1008, it must he diluted with wTater. If diluted to double its volume, multiply the result obtained by 2; if to three times its volume, multiply by 3; and so on. b. Scherer’s Gravimetric Method. Put 100 c.m.3 of clear urine in a beaker of 200 c.m.3 capacity, and acidulate with a few drops of acetic acid, unless it be already very acid. Heat in a water- bath, add 1-2 drops acetic acid, and heat to boiling, continuing for a Albumin. 230 MANUAL OF PHARMACY. half-hour or until the ppt. settles. Collect the ppt. upon a small filter which has been dried at 110° F. and weighed. Wash the ppt. with water containing a little NH4OH (to remove uric acid and urates); then with hot water till the filtrate shows no reaction for chlorides, then with alcohol, and lastly with ether. Dry the filter and ppt at 110° F., and weigh; deduct the weight of the filter: the difference represents the amount of albumin in 100 c.m.3 urine. Multiply this amount by the c.m.3 of 24 hours’ urine, and divide by 100: the quotient shows the amount of albumin eliminated in 24 hours. Example. Urine in 24 hours = 1300 c.m.3 Sp. gr. urine = 1007 “ Weight of dried filter and ppt. = 4.182 grams. “ “ filter = 1.082 “ Albumin in 100 c.m.3 urine = 8.1 3.1 X 1300 _ , . = 40.3 grams = albumin in 24 hours urine. Microscopical Examination. Urinary Deposits. Recently voided normal urine of acid reaction contains no sediment excepting a faint cloud of mucus, which gradually de- posits, carrying with it a few mucus corpuscles, and sometimes an occasional epithelial cell. In the course of twelve hours or more, the time required depeud- ing upon the temperature, the so-called acid and alkaline fermenta- tions (see page 219) have developed, causing various deposits; and to prevent a complication of deposits arising from such decompositions of normal urine ingredients, deposits should be examined early, ex- cept when the urine contains albumin, necessitating a search for casts, when a period of about 12 hours should elapse to ensure com- plete deposition. Having set aside the urine as directed under Sediments (see page 220), and the deposit having collected at the point of the conical glass, take up a few drops of the sediment by the careful use of the pipette (thereby excluding an excess of liquid portion), and transfer a drop or two to a glass slide, within a ring of cement which has been previously prepared and thoroughly dried. Put on a clean cover- glass, remove any excess of liquid with bibulous paper, and examine the object with the microscope. Caution. A little care and practice are required to prevent being misled by supposed deposits found in urine. Slides and cover-glasses should be scrupulously clean, and should be examined microscopi- cally for scratches and marks which may confuse the beginner; if these become tilled with coloring matters, they are still more likely to mislead. Fibres of cloth, hair, bread-crumbs, etc , are liable to get into the urine, and the student should therefore familiarize him- MICROSCOPICAL EXAMINATION OF.URINE. 231 self with their microscopical appearance before the examination of urine sediment. UNORGANIZED DEPOSITS. Uric Acid. Deposits of uric acid occur in acid urines; are always crystalline; crystals sometimes large enough to be seen by the'naked eye, and in their aggregation forming masses of comparatively large size, to which the terms sand, gravel, and red-pepper are applied; color, light yellow to dark red; responds to the murexid test; are insol. in hot or cold water; soluble in N1I40H. The more usual forms of uric acid are shown in Fig. 1—a, while b are exceptional forms. The urine of healthy persons depositing uric acid in 12-24 hours after emission is normal, while a deposit.,formed 3-4 hours after micturition is abnormal. Acid Urates. a. Amorphous. These are mostly acid urates of sodium, often accompanied with very small quantities of ammonium, potassium, and calcium urates. The deposit is amorphous, composed of mi- nute. granular particles, usually yellow or red, and often termed a Wick-dust or lateritious sediment. Urates are soluble in hot w’ater; hence any deposit that disappears on heating is composed of amorphous urates. They respond to the murexid test. Fig. 2—a represents amorphous urates. b. Crystalline. Sodium urate usually crystallizes in prisms arranged in stellate bundles or rosettes (Fig. 2—b); while ammonium urate forms only in alkaline urines, and in the form of spheres and globular masses often armed with small spikes (Fig. 2—c). Occurs in minute, flat, octahedral crystals which refract light very much (Fig. 3—a), and frequently in dumb-bell forms or modifica- tions thereof (Fig. 3—b); may occur in urine of any reaction—in acid urine accompanying uric acid crystals, in alkaline or neutral urine with triple phosphate crystals; insoluble in acetic acid (differ- ence from triple phosphate), alcohol, water, and alkalies, but solu- ble in HN03 The dumb-bell variety is liable to form the nuclei of calculi, and when present, efforts should be made to keep them in solution. Calcium Oxalate. Phosphates. a. Ammonio-magnesian (Triple) Phosphates. NH4MgP04 - 6H20. Found in urines that are neutral or alkaline from the pres- ence of ammonia; usually of the forms shown by Fig. 4—a, of which the typical is a triangular prism with bevelled ends, and some- times it forms stellate, feathery crystals, Fig. 4—b. 232 MANUAL OF PHARMACY. b. Calcium Phosphate (amorphous). Ca3(P04)2. Most frequently found amorphous under the same conditions as the triple phosphate. Although held in solution while the urine is acid, they are de- posited by boiling (thereby expelling C02, the cause of acidity), but are distinguished from albumin by redissolving on the addition of a mineral acid. Occasionally the crystalline phosphate (CaIIP042H20) separates from the urine in wedge-shaped or conical crystals arranged in rosettes, their points uniting (see Fig. 5), or sometimes as spherules or as dumb-bells. These crystalline bodies always occur together, and are found only in urines that contain biliary pigments. They result from the de- composition of albumin and its nearest derivatives, and are symptoms of grave destructive diseases of the liver. Their deposition may be hastened by slight evaporation of the urine Leucin (Celli3.NO2) presents itself as yellow-tinged, highly re- fracting spheres of different sizes, which by suitable illumination are found to be marked with radiate and delicate concentric lines, (Fig. 6—a). Tyrosin (C9HnlSr03) occurs in very fine silky needles arranged in sheaf-like bundles or crosses (Fig. 6—b). Test for Tyrosin: On boiling a few drops of solution of mercuric nitrate with the urine! a red ppt. results with a supernatant liquid of red or purple. Leucin and Tyrosin. Cystin. Cystin appears as colorless, regular, hexagonal plates of various sizes, arranged either singly or with one or more smaller crystals lying upon a larger one (Fig. 7). Can be distinguished from uric acid by the following test: Allow a drop of NH4OH to flow under the cover-glass; cystin dissolves while uric acid remains, and on evaporation, cystin crystal- lizes again. Cystin occurs in pale, acid, or alkaline urine. ORGANIZED DEPOSITS. Blood-corpuscles. These are recognized as round bodies, and present interesting optical properties owing to their bi-concave cen- tres. This is due to the reversal of light and shadow which they undergo in focussing; the centres and circumferences alternating in brightness or shadow as the objective is moved toward or away from the slide (Fig 8—a). In dilute urines the blood-discs swell up, be- coming bi-convex (instead of bi-concave), and finally spherical; then the reversal of light and shadow' is no longer visible (Fig. 8—b). MICROSCOPICAL EXAMINATION OE URINE. In concentrated urines or by the action of salts, the concavity be- comes greater, the corpuscle shrinks and becomes crenate, or of horse-chestnut form (Fig. 8—c). Epithelial Cells originate from the urinary tract, from the glands opening into it, and from the vagina. They are present in health and disease, but their appearance and numbers often direct to the nature, location, and severity of morbid processes. If in abundance, they denote catarrhal inflammation. The epithelial cells met with in urine are:— a. Bound Cells, which come from the convoluted tubules and the pelvis of the kidney, the bladder, and the male urethra. They are irregularly round, granular bodies, larger than pus-corpuscles* and have a single large nucleus. (Fig. 9—a.) b. Flat Cells are derived from the vagina and bladder; they are large, irregular, flat, scale-like bodies, faintly granular, containing a single nucleus. (Fig. 9—b.) c. Columnar (or Conical) and Spindle Cells, from the pelvis of the kidney, the ureters and urethra; they are elongated, irregularly conical, granular bodies, containing a single nucleus. (Fig. 9—c.) Mucus or Pus-corpuscles. These corpuscles are similar in appearance under the microscope. They are round, granular cells to inch in diam.) larger than blood-corpuscles and containing one or more nuclei (Fig. 10). Acetic acid causes them to swell and destroys their granular appear- ance, while the nuclei become more distinct, and the cell gradually becomes invisible. Water produces a similar effect, but acts slower. Tube-casts. For a microscopical search for casts, use only the sediment obtained from urine that has been allowed to stand for 12 hours. Casts (or epithelial cylinders) are the moulds of the uriniferous tubules produced by the exudation (due to capillary rupture) of co- agulable material from the blood into these tubules, which solidifies and entangles whatever it may have surrounded while in its fluid state. These casts contract and slip out of the tubules into the pelvis of the kidney; are thence carried into the bladder and voided with the urine. Their appearance indicates disease of the kidney. a. Blood-casts (Fig. 11—a) have granular markings, having blood- corpuscles inclosed in them, and are in reality miniature clots. b. Hyaline (or Transparent) Casts (Fig. 11—b) are perfectly clear, transparent, long and narrow cylinders, usually unmarked, although often having a few particles of granular matter entangled in them. Some are so delicate as to be overlooked unless the light from the mirror be modified or a drop of a solution of anilin violet be added to the deposit before applying the cover-glass. C. Wax Casts (Fig. 11—c). Hyaline casts that are denser and more highly refractive, having an appearance like molten wax, are called wax casts. 234 MANUAL OF PHARMACY. d. Epithelial Casts (Fig. 11—d) are clear, cylindrical bodies, entangling epithelium. e. Granular Casts result from the inclosing of granular matter in the forming cast, the granules resulting from the degeneration of epithelium and of blood-corpuscles. They are termed highly granu- lar (Fig. 11—e), moderately, and faintly granular, depending on the amount of granular matter present. f. Oil (or Fatty) Casts (Fig. 11—/) are loaded with oil globules, either free or contained in epithelial cells. g. Mucous Casts (Fig. 11—/ are smooth, transparent bodies, usually of great length, frequently branching and diminishing in diameter as division proceeds, thereby showing that they come from the kidney. Spermatozoa. These are recognized by the oval head or body, and the delicate,, tail-like appendage projecting from it (Fig. 12). In the urine they are motionless and resist decomposition for days, URINARY CALCULI. Calculi are hard, stony bodies composed of normal or abnormal constituents of the urine. In size they vary from such as can hardly be seen by the aid of the microscope, to some that are as large or larger than the fist. The nucleus is the most important part of a calculus, as it shows the origin of the concretion If the calculus is made up of more than one constituent, the additional constituents may be seen arranged in several concentric layers about the nucleus. Composition. Of the compounds that represent the composition of the nuclei of urinary calculi, the following are the most important, viz.: uric acid and urates, representing the nucleus of 80# of all calculi; calcium oxalate, about 5# ; cystin, about 1.5#; earthy phos- phates, about 8.5# ; foreign bodies, 8.3#. Qualitative Analysis. The calculus should be divided into two equal parts by means of a fine watchmaker’s saw. The saw-dust should be collected for analysis, and a piece of the nucleus powdered for a separate exam- ination. In order to determine the arrangement of the several layers, one half of the calculus is polished upon glass until these layers can be easily observed. A separate portion of the powder should be used for each operation in the following scheme, unless otherwise directed. Scheme of Analysis.* 1 Heat on platinum foil till colorless: a. If entirely volatile—see 2; b. If a residue remains—see 5. * Witrhaus’s scheme of analysis of urinary calculi has been found to be the most thorough and simple, in the hands of the author; hence its adoption. URINARY CALCULI. 235 2. Moisten a portion with HN03; evaporate to dryness at a low heat; add NH4OH : a. If a red color results—see 8; b. If no red color—see 4. 3. Treat a portion with KOH, without heating : a. If an ammoniacal odor results Ammonium urate. b. No ammoniacal odor Uric acid. 4. a. If on evaporating the HN03, solution becomes yellow; the yellow residue becomes reddish yellow on addition of KOH, and, on heating with KOH, violet-red Xanthin. b. If the.HN03 solution becomes dark brown on evaporation, Gystin. 5. Moisten a portion with HN03, evap. to dryness over a water- bath; add NH4OH: a. If a red color results—see 6; b. If no red color—see 9. 6. Heat before the blow-pipe on platinum foil: a. If it fuses—see 7; b. It does not fuse—see 8. 7. Bring into blue flame on clean platinum wire: a. If flame is yellow Sodium urate. b. Violet flame when seen through blue glass. .Potassium urate. 8. The residue from 6: a. Dissolves in dil. HC1 with effervescence; the solution forms a white ppt. with ammonium oxalate Calcium urate. b. Dissolves with slight effervescence in dil. H2S04; the solu- tion neutralized with NH4OH gives a white ppt. with Na2HP04 Magnesium urate. 9. Heat a portion on platinum foil: a. If it fuses Ammonio-magnesian phosphate. b. It does not fuse—see 10. 10. The residue from 9, moistened with II20, and tested with red litmus, is: a. Alkaline—see 11. b. Not alkaline Tricalcic phosphate. 11. If the original substance dissolves in HOI: a. With effervescence Calcium carbonate. b. Without effervescence Calcium oxalate. 236 MANUAL OF PHARMACY. Method of Recording an Examination of Urine. It is important that all results derived by a careful examination of urine should be recorded in a brief and systematical manner. The following represents a good form for tabulating such a record: Urine Analysis.—Made Feb. 26—1S89. Name. .C. M. Jacobs. Age. .22 years. Physical Properties. Quantity (24 hours) .. .600 c.m.3 Color Pale yellow, somewhat cloudy. Sp. gr 1006. Reaction Acid. Sediment Moderate, flocculent. Normal Constituents. HaSO4test.gr. — Cl. m.— Ind. m. -f- Epb. gr.— U I u! gr. .Apli. .Spli. m. Abnormal Constituents in Solution. Albumin , 40 per cent. Sediment. Mucus in normal quantity Microscopically. Several oil casts; free oil globules , Diagnosis.. Fatty degeneration of kidney. Abbreviations for the constituents referred to in the above form “t~ are to be understood as follows: Ind. = Indican; U = Urea; U = Uric Acid; Cl. = Chlorides; Eph. = Earthy phosphates; Aph. = Alkaline phosphates; Spli. = Sulphates. In order to indicate whether a substance is present in the normal, or a greater or smaller quantity, these signs are employed: Increase, ; diminution, “—”; normal, “n.”; great increase, “gr. -j-”; great diminution, “gr. —”; moderate increase or diminution “m-f-” and “ m. — URINALYSIS RE AGENTS. 237 REAGENTS REQUIRED FOR URINALYSIS. The “ test solutions ” and “ volumetric solutions ” referred to under the various tests are those of the U. S. Pharmacopoeia, 1880. The following volumetric solutions are also designated in connec- tion with certain tests for the approximate examination of the con- stituents of urine. In preparing these solutions only distilled water should be used, and the chemical reagents must be chemically pure. 1. Magnesian Mixture. Magnesium sulphate, 1.5 ; ammonium chloride, 1.5; water, 10.0; add aqua ammon., 2,5;—let stand 2 days, and filter. To a boiling solution of sodium phosphotungstate add q. s. H3P04 to give an acid reaction; cool; add acetic acid till strongly acid; let stand 24 hours, and tilter. 2. Solution Sodium Phosphotungstate. 3. Solution Uranic Acetate. Dissolve yellow uranic oxide 33. grams in glacial acetic acid and dilute with q.s. water ft. 900 c.m.3 Place 50 c.m.3 of solution di-sodic phosphate in a beaker and add of the above uranium solution 5 c.m.3; heat on a water-bath, and add more uranium solution from a burette until a drop of the mixture produces a brown color when brought in contact with a drop of solu- tion of potassium ferrocyanide. The number of c.m.3 of uranium solution used corresponds to 0.1 gram P205, which multiplied by 50 gives the number of c.m.3 of uranium sol. representing 5 grams P206, to which enough water must be added to make 1000 c.m.3 Each c.m.3 of the solution thus prepared represents 0.005 gram P 2Os. 4. Solution Di-sodic Phosphate. Dissolve non-effloreseed di-sodic phosphate (Na2HP04.12H20) 10.085 grams in enough water to make 1000 c.m.3 Each c.m.3 represents 0.1 gram P205. 5. Solution Sodium Acetate. Dissolve sodic acetate (NaC2H302.3H20) 100 grams in water 100 c.m.3; add glacial acetic acid 100 c.m.3 and water sufficient to make 1000 c.m.3 FIG .1 FIG. 2 FIG.3 FIG .4- FIG.5 FIG.6 FIG. 7 FIG. 8 FIG.9 FIG.10 FIG.II FIG. 12 INDEX. A Absorption of gases, 58, 61 Abstracta, 61 Abstracts, 54, 61 Acacia 167 mucilage 167 syrup, 167 Aceta, 59 Acid, acetic, 68, 69 flacial, 70 ilute, 70 “No. 8.” 69 arsenious, 143 solution, 113, 144 benzoic, 175 boric (boraeic), 82 carbolic. 55, 161 crude, 160 ointment, 161 carminic, 209 chromic, 138 citric, 179 copaivic, 172 cresylic, 68, 160 definition, 64 elaic, 195 ethyl-sulphuric, 66 gallic, 206 hydriodic, syrup of, 104 hydrochloric, 66, 213 dilute, 67 bydrobromic dilute, 108 hydrocyanic dilute, 110, 123 hypophosphorous, 114, 118 hydrosulphuric, 113 lactic, 207 meconic, test, 203 meta-phosphoric, 114 muriatic, 66 nitric, 68 dilute, 68 nitro-hydrochloric, 67 dilute, 67 nitro-muriatic, 67 oleic, 195 orthophenolsulphonic, 84 oxalic, 158 phenic, 161 phenylic, 161 phosphoric (ortho), 114, 115 dilute, 115 phosphorous, 114 prussic, 110 pyrogailic, 207 pyroligneous, 55, 68 Acid, pyrophosphoric, 114,115 salicylic, 161 sulphocarbolic, 84 sulphovinic, 66, 180, 181 sulphuric, 65 aromatic, 66 dilute, 66 sulphurous, 66 tannic, 207 tartaric, 178 thymic, 190 uric. 229, 230 valerianic, 207 Acidulous radical, 64 Aconitine, tests, 202 Acrolein, 191 Adeps, 208 Agitation, 61 Albumin, 111 in urine, 221 Alcohol, 43, 176 absolute, 177 amylic, 178 dilute, 177 ethyl. 176, 177 methylic, 159 wood, 159 Alembic, 54 Alemen's test (blood), 224 Allanite, 99 Almond, bitter, oil, 187 sweet, oil, 193 Aloes and iron, pills, 118, 121 Alkali volatile, 87 Alkaline earths, compounds, 90 Alkalies and compounds, 70 Alkaloids, 197 composition, 197 definition, 197 discovery, 197 existence, 197 extraction, 198 theory of isolation, 198 nomenclature, 197 occurrence,197 oleates, 196 formation of salts, 197 table of. 202, 203, 204 tests (general), 201 Aludels. 149 Alumen, 100 Alum, ammonio-ferric, 100,118, 124 ammonium, 100, 101 burnt, 100 caesium, 100 chromium, 100 242 INDEX. Alum, definition, 100 dried, 100 potassio-ferric, 100 potassium, 100 rubidium, 100 silver, 100 sodium, 100 Alum-slate, 100 Alum-stone, 100 Alumina, hydrated, 101 Aluminium and potassium sulphate, 100 bronze, 100 hydroxide, 101 salts. 100 sulphate 101 Alums without aluminium, 100 Alunite, 100 Ambar. 162 oil, 162 Ambergris. 211 Amides, 197 Amines, 197 Ammonia, 55, 85 liniment, 88 spirit, 8s aromatic, 87, 88 water 88 stronger, 88 Ammoniac, 168 with mercury, plaster, 150 Ammonium, 70 acetate, solution, 87, 90 benzoate, 89 bi-carbonate, 87 bromide. 89 carbamate, 87 carbonate, 87 chloride, 86 troches, 86 citrate, 90 iodide, 89 nitrate, 87 oxalate, 90 phosphate, 90 salts, 85 sulphate, 86 sulphocyanide, 111 tartrate, 90 Amorphous, 56, 58 Amyl, nitrite. 183 Amyli glycentum, 163 Amylum, 162 iodatum, 163 Anilin, IU2 Animal products, 207 Antidotes, definition, 212 general, 212 classified table of, 213 Antimonial powder, 146 Antimony, 145 and potassium tartrate, 147 compound, pills, 151 black, 111, 145 oxide, 146 sulphide, 145 purified, 145 Antimony, sulphurated, 146 wine, 147 Aqua, 64 destillata, 64 fortis, 67 regia, 67 Aquae, 69 Arabins, 167 Are. 17, 18 Argols. 70. 71, 73, 178 Arsenic, 142 antidotes, 124, 143 chloride, solution, 144 iodide. 144 and mercury, solution, 144 native, 142 oxides. 143 solution. Clemen’s, 145 Donovan’s, 144, 162 Fowler’s, 144 Pearson’s. 145 Valangin’s. 144 tests, 142, 143 white 143 Arsenical pyrites, 142 Arsenious oxide, 143 Asafetida, 169 Asbestos, 94 Atropine, tests, 202 Averaging mixtures, 31, 32, 33 Averaging percentages, 81, 32, 33 B Balance, 14 hydrostatic. 21 Balsam fir, 173 Peru, 174 tolu, 174 Balsams, 174 Barilla, 77 Barium carbonate, 97 chloride, 97 hydroxide, 97 per-oxide, 97 salts, 97 sulphate, 97 Barley malt, 175 Baryta, 97 Basilicon ointment, 166 Bassorin, 167, 168 Basylous radical, 64 Baths, lands, 41 Beef, extract, 211 Beeswax, 165 Benne, oil, 193 Benzine, 43. 55 Benzoin. 174 flowers. 175 Benzol. 55 Berzelius test. 142 Bismuth citrate, 149 sub-carbonate, 147 sub-nitrate, 148 Bittern, 94. 106 INDEX. 243 Black, bone, 160 ivory, 160 draught 95 Blanc fix, 97 Blatta orientalis, 211 Blend, 111, 139 Blistering cerate, 208 fluid, 157 Blood, Alemen’s test, 224 in urine, 224, 232 Blowpipe, 39 Blue mass, 150 ointment, 150 Paris, 109 pill, 150 Prussian, 109, 118 stone 131 Turnbull’s, 109, 119 vitriol 134 Williamson’s, 109 Boettger’s test, 223 Boiling-point, 41 temperatures, 41 Bone ash. 116 black. 160 spirit 85, 86 Borax, 82 springs, 77 Bottle, specific gravity, 24 Brandy, 177, 180 Braunnite, 130 Brimstone 112 British gum. 163 mea-ure, 16 Bruising, 36 Bromides, tests, 107 Bromine, 106 Brown mixture, 147 Bunsen burner, 39 Burgundy pitch, 170 Burnett’s disinfecting fluid, 139 c Cacao butter. 63, 193 Cadmium 138 iodide, 139 sulphate. 139 Caesium, 98 Calamine, 139 Calcareous spar, 91 Calcination, 40 Calcium bi-carbonate, 92 bromide, 9 carbonate. 91 precipitated, 92 chloride, 93 hypophosphite, 116 laco-phosphate, syrup, 93 oxalate (in urine), 231 phosphate (in urine). 232 precipitated, 91, 93 saccharate, 91 salts, 91 sulphate, 91, 94 tartrate, 4.', 73 Calculi, urinary. 234, 235 Calcutta nitre, 70 Calomel, 40,151 Calx (usta), !>l Camphor, 189 bromated (mono-), 190 Canada balsam, 173 pitch. 170 turpentine, 173 Cantharides. 208 Capsicum, plaster, 173 Caramel. 165 Carbamide, 221 Carbo animalis. 160 hydrates, 155 ligni. 160 Carbon bi- (di-) sulphide, 113 Carbonization, 41 Card teeth, 118 Carlsbad springs, 98 Carmine 209 Carron oil. 91 Castor (Castoreum), 211 oil, 193 Casts in urine, 233, 234 Cathartic powder, 73 pills, comp., 151 Cellulin, 155, 156, 157 destructive distillation, 159 Cellulose, 155, 156 Ceracins, 167 Cerates (Cerata), 61,166 Cerite, 99 Cerium nitrate, 99 oxalate, 99 salts, 99 Cerous sulphate, 99 Cetaceum, 193, 208 Cetin, 209 Chalk, 91 mixture, 93 powder compound, 93 precipitated, 92 prepared, 92 troches, 93 Charcoal, :3, 55. 160 animal 55, 160 purified, 160 wood, 55,160 Chartse (Papers), 61, 158 Chemistry, Organic, 155 Chloral 183 butyl hydrate, 184 camphorated, 184 hydrate, 113 Croton, 184 Chlorides in urine, 220, 226 Chlorine, 101 assay, 102, 103 water, 102 Chloroform, 43, 184 purified. 185 spirit, 185 Chrome iron ore, 137. 138 Chromium. 137 Chromic anhydride, 138 244 INDEX. Chrysarobin, 205 Chrysolite, 94 Cinchona, 200 ■ assays. 200 Cinnabar, 111, 149, 154 Circulatory displacement, 42 Citrine ointment, 154 Civet, 211 Clarification, 52 methods and application, 52, 53 Clemen's solution, 145 Coal, 103, 162 destructive distillation, 55 Coal-gas liquor, 85 Cobaltum, 142, 147 Cocaine, 199 Coccus, 209 Cochineal, 209 Cockroach, 211 Cod liver oil, 192,193, 210 emulsion, 192 Coke, 55 Colation, 52 Colla (glue), 211 Collodia, 59, 157 Collodion, cantharidal, 157 contractile, 157 flexible, 157 styptic, 157 Colloids, 43 Colophony, 172 Comminution, 36 Condenser, 54 Liebig’s, 55 Confectiones, 62 Conserves, 62 Contusion, 36 Copaiba, 173 mass (pill), 173 resin, 172 Copper, 131 acetate, 134 ammoniated, 135 pyrites, 134 sub-acetate, 134 sulphate, 134 ammoniated, 135 Copperas, 121 Corpuscles, blood, 232 Corrosive sublimate, 40, 151 Corundum, 100 Cotton. 156 absorbent, 156 collodion-, 156 gun, 156 purified, 156 soluble. 156 Cotton seed oil. 193 Cream of tartar, 71, 73 Creasote, 55, 160, 161 water, 160, 161 Croton, oil 192, 193 Crucible, 39 Cryolite, 77, 100 process (sodium carbonate), 79 Crystalline, 56, 53 Crystallization, 56 facilitated, 57 methods, 56 water of, 56 Crystallography, 57 Crystalloids, 43 Crystals, 56 creeping of, 57 size, 56 Cubeb, troches, 174 Cyanogen, 109 Cylinder, loaded, 26 Cystin in urine, 232 D Decantation, 53 Decocta, 59 Decoction, 43, 44 Decolorization, 53 Deliquescence, 56 Deodorizationj 53 Dewee's carminative, 96 Dextrin, 163 Deflagration, 40 De-hydration, 40 Desiccation, 35 Diachylon, ointment, 135 plaster, 135 Diaspore, 100 Dialysed tinctures, 44 Dialyser, 43 Dialysis, 43 Diaphragm, 43 Didymium, 99 Digestion, 43, 44, 60, 61 Di-morphous, 56 Disinfecting fluid, Burnett’s, 139 Dispensatories, 13 Displacement, circulatory, 42 Distillate, 54 Distillation, 43, 54, 62 destructive, 55 products, 55 fractional, 55 Dolomite 94 Donovan’s solution, 144 Drugs botanical), collection, 34 exhaustion, 49 preservation 35 reliable, 46 tests, 35 E Earths, alkaline, compounds, 90 Ebullition, 41 Efflorescence, 56 Egg albumen, 211 oil, 211 yolk 211 glycerite. 195, 211 Elseopten, 186 Elaidln, 154 Elaterin, 205 Electuaries. 62 INDEX. 245 Elements. 70 Elixirs (Elixiria), 59 Elm (slippery), mucilage, 168 Elutriation, 37 Emery, 100 Emplastra, 62 Emulsification, theory, 192 Emulsifying agents, 192 Emulsin, 187 Emulsion, 192 Endosmosis, 43 Enfieurage, 186 Eschbach’s test (uric acid), 229 Ether, 43, 180 acetic, 182 amylo-nitrous, 183 chloric, 185 nitrous, spirit of, 182 spirit, compound, 181 stronger, 181 sulphuric, 180 washed, 181 xylostyptic, 157 Ethereal oil, 181 Ethyl, acetate, 182 nitrite, 182 oxide, 180, 181 Evaporation, 54 in vacuo, 54 spontaneous, 54 Exhaustion, 49 theory, 49 Exosmosis, 43 Expression, 52 Extracts, 54, 62 fluid. 45, 54, 59 Excipient, 62 Exudations, 167 F Fats. 191, 193 Fehling's test (grape sugar), 164,207,223 Fel bovis, 209 Ferment, 176, 187, 207 Fermentation, 176, 207 acetic, 176 alcoholic. 176 butyric, 176 lactic, 176, 207 mucic, 176 saccharine, 176 vinous, 176 Ferric salts, see Iron Salts Ferrous salts, see Iron Salts Filter, 52 Filtering-media, 52 Filtrate, 52 Filtration, 52 Flaxseed, oil, 173 mucilage, 168 Fleitmann’s test, 68, 143, 151 Flocculent, 58 Fluid, blistering, 157 extracts, 45, 54, 59 methods, 45 preservation, 51 Fly-stone, 142 Fowler’s solution, 144 Fowler’s test (urea), 228 Franklinite, 130 Funnel. 52 Fusel oil, 178 Fusion, 40, 61, 63 G Galena, 111, 132, 135 Gamboge, 169 Garbling, 35 Gas, 55, 58 absorption, 58, 59*61 collection, 58 generation, 58 solution, 58 washing, 58 Gelatin, 53, 211 Gibbsite, 100 Gin, 177 Glass, soluble (liquid), 85 Glonoin, 195 Glucose, 163 Glucosides, 205 unofflcinal, 206 Glue, 211 Glycerin, 43, 177, 191, 195 nitro-, 195 Glycerites, 60 Glyconin, 195 Gmelin’s test (bile), 223 Goulard’s cerate, 136 extract, 136 Golden sulphur, 146 Gossypium, 156 Graduates, testing of, 17 Grain, derivation, 16 Gram, 17,18 Granular powder, 37 Grape-sugar, 163 in urine, 220, 227 Gravitation, 14 Green, Paris, 145 Scheele's, 145 Schweinfurth's, 145 Vienna, 145 Griffith’s mixture, 121 pills, 122 Grinding, 36 Guaiac, 171 Gum arabic, 167 Benjamin, 174 benzoin, 174 British. 163 Gums, 167 Gum-resins, 168 Gutta percha, 171 Gypsum 69, 91, 111 246 INDEX. H Halogens, 101 Haloid salts, 101 Heat, application, 39 determination, 37 equalization, 41 latent, 37 sensible, 37 sources, 39 temperatures attainable, 41 Heller’s test (albumin), 221 Heller’s test (blood), 224 Hirudo, 211 Hoffmann’s anodyne, 181 Honey, 165 clarified, 165 Honeys, 60 Horn-silver, 132 Hydrogen, peroxide, 97 sulphide, 113 Hydrometer, 27, 28 Hydrostatic balance, 21, 22, 23, 24 Hygroscopic, 56 Hypophosphites, syrup, 117 with iron, syrup, 117, 118, 121 tests, 117 I Ichthyocolla, 209 Ignition, 40 Imperial measure, 16 Incineration, 40 Incorporation, 61, 63 Indican. in urine, 221 Infusions (Infusa), 43, 44, 60 Iodides, tests, 104 Iodine, 103 ointment, 104 solution, compound, 104 tincture, 104 Iodoform, 106 ointment, 106 Iron, 118 acetate, solution. 118,125 tincture, 118, 126 andammon. acet. mixture, 87,118,120 ammonium citrate, 118,126, 127 sulphate. H8, 125 tartrate, 118, 126, 127 and potassium tartrate, 118, 126, 127 and quinine citrate, 118, 126, 129 solution, 118, 128 and strychnine citrate, 118, 126, 128 bromide, syrup, 118, 120 carbonate, mass, 118,122 saccharated, 118,122 chloride, 118. 119 solution, 118, 119 tincture, 118. 119 citrate, 118, 126, 129 solution, 118, 126 wine, 118, 128 compound mixture, 118, 121 Iron, compound pills 118, 122 compounds, synopsis, 118 dialysed, solution, 130 hypophosphite, 118, 125 iodide, pills, 118, 124 sacch., 118, 120 syrup, 118, 120 lactate, 118, 120 nitrate, solution, 118, 125 oxalate, 118, 122 oxide, hydrated, 118, 123, 212 with magnesia.96,118,124, 212, 213 phosphate, 118, 126, 129 plaster, 118, 124 pyrites, 6", 111 pyrophosphate, 118, 126, 130 quinine and strychnine citrate, 129 phosphate syrup, 118, 130 reduced, 118, 123 scale salts, 126 sesqui-chloride, 119 subsulphate, solution, 118, 123 sulphate, 118, 121 sulphate, dried, 118, 121 sulphate, precip., 118, 121 tersulphate, solution, 118,123 troches, 118, 124 valerianate, 118,126 wine, bitter, 118,128 Isinglass, 209 artificial, 211 Isomorphous, 56 J Jacobi, pulvis, 146 Jalap, powder, compound, 73 resin, 172 James powder, 146 Javelle water, 103 K Kainite, 70 Karnellite, 70 Kelp, 103 Kerosene, 55 Kieserite, 94 Kilo, 18 Koumiss, 211 Ii Lac, 211 Lactose, 165 Labarraque’s solution, 103 Lake, 101 Lanthanum, 99 Lard, 193, 208 oil. 193, 208 Lead, 135 acetate, 136 carbonate, 136 ointment, 137 INDEX. Lead, chromate, 137 iodide, 137 ointment, 137 nitrate, 137 oxides, 135 plaster, 135, 194 red, 135 subacetate, cerate, 136 liniment, 136 solution, 135, 136 diluted, 136 sugar of, 136 water, 136 white, 136 Leblanc’s process (sodium carb.), 78 Leech. 211 Lepidolite, 98 Leucin in urine, 232 Levigation. 37 Licorice, mixture compound, 147 powder compound, 112 Lignin, 155. 156 Lime, 91 burned, 91 chloride (chlorinated), 102 liniment, 91 milk. 91 quick, 91 slaked, 91 solution, 91 syrup, 91 water, 91 Limestone, 91 magnesian, 94 Linen, tests. 156 Liniment, volatile, 88 Linimenta, 60 Liquid measure, 16 supernatant, 57 Liquores < Solutions), 60 Liquor, mother, 56 Liter, 18 Litharge. 135 Lithium benzoate, 98 bromide, 98 carbonate, 98 citrate, 99 salicylate, 99 salts, 98 Liver of sulphur, 75 Lixiviation, 52 Loaded cylinder, 26 Lugol's solution, 104 M •laceration, 43, 44, 48, 60, 61 Magnesia, 96 and asafetida, mixture, 95 calcined. 96 heavy, 96 troches. 96 usta. 96 Magnesian mixture, 237 .Magnesite, 95 Magnesium, 94 and calcium carbonate, 94 carbonate, 94, 95 chloride, 94 citrate, granulated, 96 solution, 96 salts, 94 sulphate, 94 sulphite, 97 Malachite, 134 Malt, 175 extract, 176 Maltose, 176 Manganese, 130 hypophosphite, 132 iodide, 132 oxide, black, 131 di-, 131 per-, 131 sulphate, 131 Manganite, 130 Marble, 91 Marc, 45 Marme’s solution, 201 Marshmallow, syrup, 168 Marsh’s test, 143 Mass® (Pill Masses), 62 Mastic, 170 Mayer’s solution, 201 Measure, 14 Measures, domestic, 17 liquid. 16, 17 Mel, 165 Mellita (Honeys), 60 Meniscus. 28 Menstruum, 41, 45, 46, 47 Menthol, 190 Mercurial ointment, 151 plaster. 150 Mercur-ammonium chloride, 154 Mercuric (see Mercury salts), 149, 150, 151, 152 Mercurous (see Mercury salts), 149,150, 151, 152 Mercury, 149 ammoniated, 154 ointment, 154 bichloride, 151 chloride, corrosive, 151 mild. 151 cyanide, 109, 153 extinguishing (killing), 149 iodide, bin-, 152 deuto-, 152 green, 152 proto-, 152 red, 152 mass, 150 nitrate, solution, 154 oleate. 153 oxide per-, 153 red, 153 ointment, 153 yellow, 152 ointment, 153 perchloride, 151 248 INDEX. Mercury, pernitrate, solution, 154 proto-chloride, 151 purification, 149 subchloride, 151 subdivision, 149 subsulphate, yellow, 154 sulphate, 151 basic-, 154 sulphide, red, 154 tests, 149, 150 with chalk, 93, 150 Meter, 17 Methenyl iodide, 106 Metric system, 17 Metrology, 14 Milk. 211 sugar, 165 Mindererus, spirit, 87 Mispickel, 142 Misturee (Mixtures), 60 Mixtures, averaging strength of, 31, 32, 33 Molasses, 164 Monsel’s solution, 123 Montebrasite, 98 Moore’s test (albumin), 223 Mordant, 101 Morphine, extraction, 200 tests, 203 Mortar, 36 Mucilages (Mucilagines), 60, 167, 168 Moschus, 210 Mother liquor, 56 Musk, 210 artificial, 162 Mustard, oil (volatile), 187 Myrosin, 188 Myrrh, 169 N Naphtha, 55 wood, 159 Nickel, 147 Nitre, 72 Calcutta, 70 Chili, 77, 83 cubic, 83 sweet spirit of, 182 Nitro-glyeerin, 195 o Oil, carron, 91 cod liver, emulsion, 192 ethereal, 181 fusel, 178 olive, 193 phosphorated, 114, 115 wine, 181 Oils, 43 essential, 185 fixed. 191, 193 adulterations, tests, 192 composition, 191 Oils, fixed, extraction, 192 purification, 191 restoration, 191 table of, 193 volatile, 185, 189 adulterations, tests, 187 enfleurage process, 186 by ferment, 187 preservation, 187 table of, 189 extraction, 186 Ointment, simple, 166 Ointments (Unguenta), 63 Oleates, 60, 196 of alkaloids, 196 precipitated, 196 Olein 191 Oleo-resins. 54, 60, 172 derived, 173 natural, 172 Olive oil. 193 Opium, 199 assay, 199 denarcotized, 199 powdered, 199 Orpiment, red, 142 yellow, 142 Osmosis, 43 Ox bile, 209 blood, 211 gall, 209 inspissated, 209 purified, 209 Oxidation, 40 P Palmatin, 191 Pancreatin, 211' Paper, 157 ledger, 157 medicated, 61, 158 mustard, 158 nitre, 158 parchment, 43, 158 printing, 157 Spanish fly, 158 wall, 157 writing, 157 Paper pulp, 52 Paris blue, 109 Paris green, 145 Paris red, 154 Pearlash, 71 Pearson’s solution, 145 Pepsin, 210 saccharated, 210 Peptones, 210 tests. 211 (in urine), 222 Percentages, averaging of, 31 Percolate, 45 Percolation, 43, 45, 60, 61, 62 fractional, 51 theory, 49 Percolator, 45 INDEX. 249 Percolator, forms of, 45 Pettenkofer’s test (bile), 224 Phosphates in urine. 220, 227, 231 Phosphorus, 114, 155 amorphous. 114 pills. 114, 116 red, 114 Pharmacopoeias, 13 Pharmacy, 13 inorganic. 64 organic, 155 Phenol, 161 Picrotoxin, 205 Pill masses, 62 Pills. 62 Pitch, 159 black, 159 Pix liquida, 159 navalis, 159 Plant, composition, 155 exudations, 167 proximate principles, 155 Plasma, 163 Plasters (Emplastra), 62 Plummer’s pill, 146 Podophyllum, resin, 172 Poisons, 212 classification, 212 corrosives, 212 irritants, 212 narcotics, 212 narcotico-irritants, 212 table with antidotes, 213 treatment, 212 Polymorphous, 56 Pommade, 186 Potash, caustic, 74 crude, 71 prussiate, red, 109 yellow, 109 solution, 75 with lime, 75 Potassa, 74 chlorinated, solution, 103 sulphurated, 75 Potassium acetate, 74 and sodium tartrate, 73 arsenite, solution, 143,144 bicarbonate, 72 bichromate, 138 bitartrate, 73 bromate, 107 bromide, 107 carbonate, 71 chlorate, 75, 76 troches, 76 chloride. 70 citrate, 76 cyanide, 110 ferricyanide, 109 ferrocyanide, 109 hydroxide, 74 hypophosphite, 117 iodate. 105 iodide, 105 ointment, 105 Potassium nitrate, 72 permanganate, 131 salts. 70, 71 sulphate, 77 sulphite, 77 sulphocyanide,lll tartrate, 73 Powder, cathartic, 73 dusted, 37 fineness. 36 gradation, 36 granular, 37 uniform, 46 compound effervescing, 74 Powders (Pulveres), 62 Precipitant, 57 Precipitate, 52, 57 red, 153 • white, 154 treatment of, 58 Precipitation, 57. 62 Preparations (U.S.P.) classified, 59 Problems, 17, 19, 20, 22, 23, 24,25, 26, 27, 28, 29, 30. 31. 32, 33, 38, 39, 88, 89, 199 Proof-spirits, 178 Proteids, ill Prussian blue, 109, 118 Pulverization, 36 Pulvis Jacobi, 146 Pyroligneous spirit, 159 Pyrolusite, 130 Pyroxylic spirit, 159 Pyroxylin, 156 Q Quince seed, mucilage, 168 Quinine, assay, 200 extraction, 201 tests, 204 R Radical, acidulous, 64 basylous, 64 Receiver, 54 Reduction, 40 Re-percolation, 50, 60 Resin, 172 cerate, 166 Resins (Resinae), 62,170 artificial, 171 natural, 170 Residue, 45, 54 Retort, 54 Rhubarb and soda, mixture, 80 powder, compound, 96 Roasting, 40 Rochelle salt, 73 Roses, confection, 165 honey, 165 Rubidium, 98 Rum, 177 Ruby, 100 250 INDEX. S Saccharum, 164 lactis, 165 Safety-cube, 55 Salicin. 205 Sal volatile, 87 Salaeratus, 72 Salicor, 77 Salt, common, 78 definition, 64 Epsom 94 -petre. 72, 83 Rochelle, 73 of tartar, 71 Salts, haloid, 101 Sanguis, 211 Santonin, 206 • Saponification, 192 Sapphire, 100 Sassafras pith, mucilage, 168 Scammony, 171 resin, 172 Scheele’s green, 145 Scheibler’s solution, 201 Scherer’s test (uric acid), 229 Schweinfurth’s green, 145 Schweizer's solution, 156 Sediment, 53 Senna, infusion, compound, 95 Septum, 43 Sevum, 193 Sifting, 36 Silica, 91 Siliceous hydrate, 94, 95 Silver, 132,147 cyanide, 109, 133 fulminating, 133 glance, 132 horn 132 iodide, 133 leaf, 132 nitrate, 132 diluted 73, 132,133 mitigated, 133 moulded, 132, 133 oxide, 133 Siphon, 53 Smithsonite, 139 Smoke, oil, 160 Soap, cast ile, 194 composition, 194 green, 194 ard, 192, 194 insoluble, 194 lead, 135, 194 soft, 192, 194 soluble, 192 Soapstone, 94 Soaps. 192 Soda, caustic, 80 chlorinated, solution, 103 solution, 81 Sodium acetate, 81 solution, 237 arseniate. 144 Sodium arseniate, solution, 145 benzoate. 81 bi-caibonate 80 troches 80 bi-sulphite, 81 borate, 82 bromide 108 carbonate. 78 dried 79 chlorate, 82 chloride, 78 hydroxide, 80 hypophosphite. 117 hyposulphite, 83 iodate, 105 iodide. 105 nitrate, 83 phosphate (di-sodic), 116 solution, 237 phosphotungstate, solution, 201, 237 pyro-arseniate, 145 pyrophosphate, 116 salicylate, 83 salts, 77 santoninate, 206 silicate, solution, 85 sulphate, 84 sulphite. 84 sulpho-carbolate, 84 thiosulphate, 83 Solution, 41. 42 chemical, 42, 60 61 complex. 43 saturated 42 simple. 41. 60, 61 super-saturated, 42 Solutions (Liquores). 60 Solvay’s process (sodium carb.), 79 Solvent. 41 42 43 Sonnenschein’s solution, 201 Spanish flies, 208 Spar, bitter. 94 calcareous, 91 heavy, 97 Spermaceti, 193, 208 Specific gravity, 14, 21, 29 bottle, 24, 25, 26 Specific volume, 1.4, 30 Spirit, methylated, 159 proof: 177 pyroligneous, 159 pyroxylic, 159 Spirits, 61 Spodumene, 98 Sponge, 103 Squill comp, syrup, 147 Starch.162 glycerite. 163 iodide (iodized), 163 syrup. 163 -sugar, 163 Stearin, 191 Stearoptens. 186, 189 Stibnite, 145 Still, 54. 55 Storax, 174 INDEX 251 Storax. liquid. 174 Straining. 52 Strontium nitrate, 98 salts. 98 Strychnine, 204 Sublimation. 39 Suet, prepared, 193 Sugar, burnt, 165 cane, 164 grape, 163 milk, 165 raw (muscavado), 164 refined, 164 starch, 163 Sumt 70 Sulphates in urine, 220, 226 Sulphur. Ill, 155 flowers, 112 golden, 146 iodide, 112 liver, 75 milk, 112 ointments, 72, 112 precipitated, 112 roll, 112 rough, 112 sublimed, 112 washed 112 Sulphuretted hydrogen, 113 Supernatant liquid, 57 Suppositories (Suppositorise), 62 Synaptase, 187 Syrup, 61, 164 Syrups, 61 - T Tartar emetic, 147 salt of, 71 cream of, 72, 73 crude, 73, 178 soluble, 73 Talc, 94 Tar, wood, 159 oil, 159 syrup, 159 ointment, 159 coal, 162 Tannin, 207 Tenaculum, 52 Testing graduates. 17 botanical drugs, 35 for exhaustion, 49 Thermometer. 38 comparative scales, 38 Fahrenheit. 38 Centigrade (Celsius), 38 Reamiir, 38 Thymol, 190 Tincal, 82 Tincturae, 61 Tinctures, 61 dialysed, 44 Tolu, balsam, 174 syrup, 174 Torrefaction, 40 Toxicology, 211 Tragacanth, 167 mucilage, 168 Treacle, J 64 Troches, 63 Trochisci, 63 Trituration, 36, 60 Triturationes, 63 Troy weight, 15 Turpentine, 172 oil, 173 Canada, 173 liniment, 166 Turnbull’s blue, 109,119 Turpeth mineral, 154 Tyrosin in urine, 232 u Ultzmann's test (bile), 224 Unguenta, 63, 166 Uranic acetate, solution, 237 Urates, acid, 231 Urea, 155 220, 228 Urinary calculi, analysis, 234, 235 Urina cibi, 215 p tus, 214 sanguinis, 215 Urinalysis, 214 reagents, 237 recording, 236 Urinary deposits, 216, 230, 231, 232 Urine, acid fermentation, 219 acidimetry, 225 albumin. 221 alkalimetry, 225 alkaline fermentation, 219 bile, 223. 232 blood. 221, 232 chlorides, 220, 226 color, 217 composition. 215 grape sugar, 220, 227 indican, 221 leucin, 232 mucin, 222 microscopical, 216, 230 normal, 214, 215 odor. 218 paragloblin, 222 pathological, 215 phosphates, 220, 227, 231 physical properties, 214, 216, 217 qualitative analysis, 216, 217 quantitative analysis, 216, 224 quantity, 217 reaction. 219, 225 secretion and excretion, 214 sediments, 216, 220, 231, 232 serum-globulin, 222 specific gravity. 218 sulphates, 220. 226 total solids, 224 transparency, 218 252 INDEX. Urine, tyrosin, 232 uric acid, 229, 230 V Valangin’s solution, 144 Yallet’s mass, 122 Vaporization, 54 Verdigris, 134 Vermilion, 154 Vienna green, 145 Vina medicata, 61 Vinegars (medicated), 59 Vitellus, 211 glycerite, 195, 211 Vitriol, blue, 134 elixir, 66 green, 121 oil. 65 white, 140 Volume, 29 specific, 30 w Water, 43, 64 chlorine, 102 distilled, 54, 64 hard, 92 javelle, 103 medicated, 59 soft, 92 Wax, white. 166 yellow, 165 Weighing, 14 Weight, 14, 29 Weight, troy, 15 apothecaries’, 15 avoirdupois, 15 systems, 15 Whisky, 177, 180 White permanent, 97 Whiting, 92 Williamson’s blue, 109 Witherite, 97 Wine, measure, 16 oil of, 181 red, 178 white, 178 medicated, 61 Wood, destruct. distil., 55, 68,159, 160 naphtha, 159 Wool, 156 Worm, 54, 55 Y Yolk of egg, 211 glycerite, 195, 211 Z Zinc, 139 acetate, 141 bromide. 141 carbonate, precip., 140 chloride, 140 solution. 139 iodide, 141 oxide, 140 phosphide, 141 sulphate, 140 valerianate, 141 THIRD EDITION. MANUAL OF PHARMACY AND PHARMACEUTICAL CHEMISTRY. BY CHAS. F. HEEBNER, PH. G., (N. y.) PHM.B., Professor of Pharmacy and Director of the Pharmacal Laboratory at the Ontaru. College of Pharmacy. Formerly Instructor in Theory and Practice of Phar- macy in the College of Pharmacy of the City of New York. The study of Pharmacy simplified by a systematic and practical arrangement of topics, and the elimination of unnecessary matter. The Hook is a Cloth-Bound, 13mo, of 353 pages. The most practical work yet published for the use of pharmaceutical students preparing for College or State Board Examinations It can be read with profit by all pharmacists seek- ing the correct understanding of scientific pharmaceutical literature in general It is also calculated to insure a sound foundation to the beginner contemplating a subsequent course of training in colleges of pharmacy The first edition has been thoroughly revised and freed from typographical errors; in addition thereto the third edition contains a treatise on Urinalysis, chemical and micro- scopical (fully illustrated! and a full index. The book has been well received everywhere, and has been adopted either as a text-book or book for reference by most of the colleges of pharmacy. Head the following opinions on the merits of the book. I am much pleased with the work; it is concise and gives the students the main points. I especially like the work because it does not step in and usurp the place of our national authority, the U. S. P.—Prof. A. B. Stevens, University of Mich gan, Ann Arbor. This book contains not only all that is essential to a knowledge of the branches it relates to, but it also embraces a large amount of information, useful and practical, which is even not found in larger treatises.—The American Druggist, New York City. Mr. Heebner’s experience in teaching has stood him in good stead in the present volume, in pointing out to him not only what students of pharmacy should learn, but also the best method of imparting that information. * * * * The author has endeavored to furnish a man- ual which, while complete, should be concise; while condensed, explicit; and we can con- gratulate both the author and the student-public for whom the work is intended upon his success.—The Druggists' Circular, New York City. The publication of this compact but most desirable pharmaceutical book will prove a great help, not only to students, but cannot fall short of great value to pharmacists as well. It will be found exceedingly reliable in its statements, terse in language, and thoroughly practical. * * * * The reader will not waste time with unnecessary details, but here find all important facts and explanations that will make plain any point not before comprehended as fully as was desired. The book should be in every pharmacy, and the student who does not secure a copy, will miss one of the best aids yet prepared for his advancement.—The Pharmaceutical Record, New York City. To the busy druggist or drug clerk it will prove a handy book to pick up and read at odd times, for each page contains practical information, and it is not necessary to read the entire work through, or even several pages, in order to finish a subject.—The Druggist, St. Louis, Mo. We have critically examined this little work, and look upon it with high favor. With a fair knowledge of the contents of this book, which can easily be acquired by a limited amount of application, as it is readily understood, applicants for registration before our State Boards of Pharmacy need have no apprehension as to the result. It is a great improvement over any of the Quiz Compendiums that we have examined, being much more comprehensive and decidedly more scientific.—The Medical Record. The author by his research and judicious selection of material has made much more than a students’ manual. * * * * The book possesses a character of permanent value as a refer ence book for the practicing pharmacist.—The Scientific American. The general arrangement of the work is convenient, and the notes under each head are intentionally brief, but are sufficient for recalling to mind the important practical and theo- retical points connected with each subject The book is valuable as a note book to pharma- ceutical students, and as an outline of the scope embracing theoretical and practical phar- macy.—The American J urnal of Pharmacy, Philadelphia, Pa. The volume before us is certainly small; to some it will seem perhaps disappointingly so, \ but it is surprisingly complete. The matter has been judiciously selected, and rather with 1 reference to its intrinsic value to the student than to the idea of preparing him to pass ' examinations. * * * It contains no padding, and is the work of one who is at once a practi- I cal pharmacist and an experienced teacher.—Pharmaceutical Era, Detroit, Mich. This work is something on the Quiz book order, but decidedly superior to most of them. I The portions treating of general pharmaceutical practice are well presented, the author : evidently being able to draw from personal experience. — he Western Druggist, Chicago, 111. I Das Studium des Manuals wird durch grot* 3 Uebersichtlichkeit erleichtert, wie uberhaupt der Inhalt, dessen Anordnung und die Ausstattung des Buchs demselben nur zur Empfehl- ung gereichen ktinnen —Deutsch-Amerikanische Apotheker Zeitung, New York City. The work is to be commended for its general accuracy. * * * * Well calculated to fulfil its mission and prove a useful repitorium for the pharmaceutical student.-—Pharmaceutische Rundschau, New York City. The author’s experience as a teacher has qualified him for the preparation of such a guide as is best suited to the pharmacist’s requirements. The feature of his book is its con- ciseness and its freedom from much matter which is incorporated into many treatises on the same subject, for no better apparent reason than to swell their size —The Medical Aye. It is a very valuable vade mecum, especially useful as a book of reference, and to the college student. By using symbols the author has compressed a great deal into a small space.—The Drugman, Nashville, Tenn. * * * * A book to be used by students or pharmacists, who desire, either as a preparation for examination or for other reasons, to review the whole subject in a condensed form.- Science, New York City. The book is neatly and tastefully bound and printed, and will doubtless prove of much service to those for whom it is designed. — The Druggists' Bulletin. Those interested in pharmacy will find their interests advanced by consulting this work. —The American Lancet. This work, though intended for the American pharmacist, contains a good deal of in- formation likely to prove serviceable to the English student of pharmacy. The Chemistry and Pharmacy are of high order.—The Journal of Microscopy and Natural Science, Bath, Eng'and. The author has succeeded in crowding into a small space a vast amount of pharma- c 'utical knowledge. * * * The style is original, showing careful research and a practical knowledge of the subjects discussed. The book is a happy combination of the -l quiz ” and text book.—The American Drug Clerks' Journal, Chicago, 111. The book, although designed especially for pharmacists and pharmaceutical students, contains information that is of great interest to the general practitioner of medicine or den- tistry.—The Ohio Journal of Dental Science. Price $'4.00 and $4.43 (interleaved) net. by mail, postage prepaid.