QP5"i + H31 College of 1$l)v&itiau& anb ££>urgeotu( |DR. WILLIAM J. GIES J? | to enrich the library resources available to holders ofthe G1ES FELLOWSHIP in Biological Chemistry Digitized by the Internet Archive in 2010 with funding from Columbia University Libraries http://www.archive.org/details/practicalphysiolOOhawk PRACTICAL PHYSIOLOGICAL CHEMISTRY HAWK Absorption Spectra. PLATE I. 3 <& Oxyhaemoglobln. Haemoglobin. Carboxy- haemoglobin. Neutral Met- haemoglobin. Alkaline Met- haemoglobin. Alkali Haematin. Absorption Spectra. PLATE H. Reduced Alkali Haematin or Haemochromogen. Acid Haematin in ethereal solution. Acid Haemato- porphyrin. Alkaline Haematopor- phyrin. Urobilin or Hydro- bilirubin in acid solution. Urobilin or Hydro- bilirubin in alkaline solution after the addition of zinc chloride solution. Bilicyanin or Cholecyanin in alkaline solution. 0 PRACTICAL PHYSIOLOGICAL CHEMISTRY A BOOK DESIGNED FOR USE IN COURSES IN PRACTICAL PHYSIOLOGICAL CHEMISTRY IN SCHOOLS OF MEDICINE AND OF SCIENCE BY PHILIP B. HAWK, M.S., Ph.D. PROFESSOR OF PHYSIOLOGICAL CHEMISTRY IN THE UNIVERSITY OF ILLINOIS WITH TWO FULL PAGE PLATES OF ABSORPTION SPECTRA IN COLORS, FOUR ADDITIONAL FULL PAGE COLOR PLATES AND ONE HUN- DRED AND TWENTY-SIX FIGURES OF WHICH TWELVE ARE FN COLORS SECOND EDITION, REVISED AND ENLARGED PHILADELPHIA P. BLAKISTON'S SON & CO. 10I2 WALNUT STREET I9O9 PREFACE TO SECOND EDITION The kind reception accorded this volume by the instructors in physiological chemistry in the United States and Great Britain has made the preparation of a new edition imperative, notwithstanding the fact that less than two years have elapsed since the former edition appeared. The advance and development made in the field of physiological chemistry during this period have been both rapid and important; conditions which would of themselves have neces- sitated the revision of the volume at an early date. The book has been thoroughly revised in all departments and in part rewritten, the system of spelling officially adopted by the American Chemical Society having been followed throughout the volume. Besides introducing many neAv qualitative tests and quan- titative methods, the author has added a chapter on " Enzymes and Their Action " and has rewritten the two chapters on Proteins. The term " protein " has been substituted for " proteid " and the classification of proteins as recently adopted by the American Physi- ological Society and the American Society of Biological Chemists has been introduced and is followed throughout the text ; the classi- fication adopted by the British Medical Association is also included. The original plan of the book has been adhered to with the excep- tion that the chapter on " Enzymes and Their Action " has been made Chapter I and the practical work upon the proteins is pre- ceded by a chapter giving a brief discussion of protein substances from the standpoint of their decomposition and synthesis. We believe that the student will be able to pursue his practical work more intelligently and will derive greater benefit therefrom if the plan of instruction as suggested in Chapters IV and V be followed in the presentation of the subject of " Proteins." The author wishes to express his thanks to all those who so kindly offered suggestions for the betterment of the book. He is particu- larly desirous of expressing his gratitude to Professor Lafayette B. Mendel and Dr. Thomas B. Osborne for the many helpful sugges- tions they have so kindly given him. His thanks are also due Pro- fessor C. A. Herter, Dr. H. D. Dakin, Dr. S. R. Benedict and Mr. S. C. Clark for permission to insert unpublished material, to Mr. Paul E. Howe for valuable assistance rendered in the reading of Vlll PREFACE TO SECOND EDITION. proof and in the verification of tests and methods, and to Dr. M. E. Rehfuss for assistance in proof reading. The author takes this opportunity of making an acknowledg- ment which was inadvertently omitted from the first edition. He wishes to express his obligation to the laboratories of physiological chemistry at Yale University and at Columbia University (College of Physicians and Surgeons) in the latter of which he was Assistant to Professor W. J. Gies for two years. The courses given in these laboratories formed the basis of many of the experiments included in this volume and it is with feelings of deepest gratitude that he records this acknowledgment of the assistance thus rendered by those in charge of these courses. Philip B. Hawk. Urbana, Illinois, Fehruary I, 1909. PREFACE TO FIRST EDITION The plan followed in the presentation of the subject of this volume is rather different, so far as the author is aware, from that set forth in any similar volume. This plan, however, he feels to be a logical one and has followed it with satisfactory results during a period of three years in his own classes at the University of Penn- sylvania. The main point in which the plan of the author differs from those previously proposed is in the treatment of the food stuffs and their digestion. In Chapter IV the " Decomposition Products of Proteids " has been treated although it is impracticable to include the study of this topic in the ordinary course in practical physiological chemistry. For the specimens of the decomposition products, the crystalline forms of which are reproduced by original drawings or by micro- photographs, the author is indebted to Dr. Thomas B. Osborne, of New Haven, Conn. Because of the increasing importance attached to the examina- tion of feces for purposes of diagnosis, the author has devoted a chapter to this subject. He feels that a careful study of this topic deserves to be included in the courses in practical physiological chemistry, of medical schools in particular. The subject of solid tissues (Chapters XIII, XIV and XV) has also been somewhat more fully treated than has generally been customary in books of this character. The author is deeply indebted to Professor Lafayette B. Mendel, of Yale University, for his careful criticism of the manuscript and to Professor John Marshall, of the University of Pennsylvania, for his painstaking revision of the proof. He also wishes to express his gratitude to Dr. David L. Edsall for his criticism of the clinical portion of the volume ; to Dr. Otto Folin for suggestions regarding several of his quantitative methods, and to Mr. John T. Thomson for assistance in proof reading. For the micro-photographs of oxyhemoglobin and haemin repro- duced in Chapter XI the author is indebted to Professor E. T. Reichert, of the University of Pennsylvania, who, in collaboration with Professor A. P. Brown, of the University of Pennsylvania, is making a very extended investigation into the crystalline forms of X PREFACE TO FIRST EDITION. biochemic substances. The micro-photograph of allantoin was kindly furnished by Professor Mendel. The author is also indebted for suggestions and assistance received from the lectures and pub- lished writings of numerous authors and investigators. The original drawings of the volume were made by Mr. Louis Schmidt whose eminently satisfactory efforts are highly appreciated by the author. Philip B. Hawk. Philadelphia. CONTENTS CHAPTER I. Enzymes and Their Action i CHAPTER II. Carbohydrates 21 CHAPTER III. Salivary Digestion 53 CHAPTER IV. Proteins: Their Decomposition and Synthesis 61 CHAPTER V. Proteins : Their Classification and Properties 85 CHAPTER VI. Gastric Digestion 118 CHAPTER VII. Fats 131 CHAPTER VIII. Pancreatic Digestion 140 CHAPTER IX. Bile 150 CHAPTER X. Putrefaction Products 162 CHAPTER XL Feces 172 CHAPTER XII. Blood 182 xi Xll CONTENTS. CHAPTER XIII. Milk 218 CHAPTER XIV. Epithelial and Connective Tissues 227 CHAPTER XV. Muscular Tissue 235 CHAPTER XVI. Nervous Tissue 248 CHAPTER XVII. Urine : General Characteristics of Normal and Path- ological Urine 254 CHAPTER XVIII. Urine : Physiological Constituents 264 CHAPTER XIX. Urine : Pathological Constituents 305 CHAPTER XX. Urine: Organized and Unorganized Sediments . . 343 CHAPTER XXI. Urine : Calculi 362 CHAPTER XXII. Urine : Quantitative Analysis 366 CHAPTER XXIII. Quantitative Analysis of Milk, Gastric Juice and Blood 410 Index 427 LIST OF ILLUSTRATIONS Plate I. Absorption Spectral „ .. L. TT . , . _r \- Frontispiece 11. Absorption Spectra J III. Osazones Opposite page 24 IV. Normal Erythrocytes and Leucocytes Opposite page 184 V. Uric Acid Crystals Opposite page 273 VI. Ammonium Urate Opposite page 348 Figure Page 1. Dialyzing Apparatus for Students' Use 25 2. Einhorn Saccharometer 31 3. One Form of Laurent Polariscope 33 4. Diagrammatic Representation of the course of the Light through the Laurent Polariscope 33 5. Polariscope (Schmidt and Hansen Model) 34 6. Iodoform 42 7. Potato Starch 45 8. Bean Starch 45 9. Arrowroot Starch 45 10. Rye Starch 45 11. Barley Starch 45 12. Oat Starch 45 13. Buckwheat Starch 45 14. Maize Starch 45 15. Rice Starch 45 16. Pea Starch 45 17. Wheat Starch 45 18. Microscopical Constituents of Saliva 56 19. Glycocoll Ester Hydrochloride 68 20. Serine 69 21. Phenylalanine 70 22. Fischer Apparatus 71 23. Tyrosine J2 24. Cystine y^ 25. Histidine Dichloride 74 26. Leucine 76 xiii XIV LIST OF ILLUSTRATIONS. Figure Page 27. Lysine Picrate 78 28. Aspartic Acid 78 29. Glutamic Acid 79 30. Levo-a-Proline 80 31. Copper Salt of Proline . . . . . 81 32. Coagulation Temperature Apparatus 100 33. Edestin 104 34. Excelsin, the Protein of the Brazil Nut 105 35. Beef Fat 131 36. Mutton Fat '. 134 37. Pork Fat 136 38. Palmitic Acid 137 39. Melting-Point Apparatus 138 40. Bile Salts 152 41. Bilirubin (Hematoidin) 153 42. Cholesterol 159 43. Taurine 160 44. Glycocoll 161 45. Ammonium Chloride 166 46. Microscopical Constituents of Feces 172 47. Hematoidin Crystals from Acholic Stools 173 48. Charcot-Leyden Crystals 174 49. Boas' Sieve 177 50. Oxyhemoglobin Crystals from Blood of the Guinea Pig. 186 51. Oxyhemoglobin Crystals from Blood of the Rat 186 52. Oxyhemoglobin Crystals from Blood of the Horse 187 53. Oxyhemoglobin Crystals from Blood of the Squirrel . . . 187 54. Oxyhemoglobin Crystals from Blood of the Dog 188 55. Oxyhemoglobin Crystals from Blood of the Cat 188 56. Oxyhemoglobin Crystals from Blood of the Necturus . . 189 57. Effect of Water on Erythrocytes 195 58. Hemin Crystals from Human Blood 198 59. Hemin Crystals from Sheep Blood , 198 60. Sodium Chloride ' 200 61. Direct -vision Spectroscope 203 62. Angular-vision Spectroscope Arranged for Absorption Analysis 204 63. Diagram of Angular-vision Spectroscope 204 64. Fleischl's TIemometer 208 65. Pipette of Fleischl's Hemometer 208 LIST OF ILLUSTRATIONS. XV Figure Page 66. Colored Glass Wedge of Fleischl's Hiemometer 209 6y. Dare's Hsemoglobinometer 210 68. Horizontal Section of Dare's Hsemoglobinometer 211 69. Method of Filling the Capillary Observation Cell of Dare's Hasmoglobinometer 212 70. Thoma-Zeiss Counting Chamber 213 71. Thoma-Zeiss Capillary .Pipettes 214 72. Ordinary Ruling of Thoma-Zeiss Counting Chamber ... 215 73. Zappert's Modified Ruling of Thoma-Zeiss Counting Chamber 216 74. Normal Milk and Colostrum 219 75. Lactose 220 76. Calcium Phosphate 224 yy. Creatine 238 78. Xanthine 239 79. Hypoxanthine Silver Nitrate 245 80. Xanthine Silver Nitrate 247 81. Deposit in Ammoniacal Fermentation 257 82. Deposit in Acid Fermentation 257 83. Urinometer and Cylinder 258 84. Beckmann-Heidenhain Freezing-Point Apparatus 260 85. Urea 266 86. Urea Nitrate 268 87. Melting-Point Tubes Fastened to Bulb of Thermometer. 269 88. Urea Oxalate . . . 270 89. Pure Uric Acid 274 90. Creatinine 277 91. Creatinine-Zinc Chloride 278 92. Hippuric Acid 282 93. Allantoin from Cat's Urine 286 94. Benzoic Acid 289 95. Calcium Sulphate 298 96. " Triple Phosphate " .' 301 97. The Purdy Electric Centrifuge 343 98. Sediment Tube for the Purdy Electric Centrifuge 343 99. Calcium Oxalate 345 100. Calcium Carbonate 346 101. Various Forms of Uric Acid 347 102. Acid Sodium Urate 348 103. Cystine 349 XVI LIST OF ILLUSTRATIONS. Figure Page 104. Crystals of Impure Leucine 350 105. Epithelium from Different Areas of the Urinary Tract. . 352 106. Pus Corpuscles 353 107. Hyaline Casts 354 108. Granular Casts 355 109. Granular Casts 356 1 10. Epithelial Casts ■ 356 in. Blood, Pus, Hyaline and Epithelial Casts 356 1 12. Fatty Casts 357 113. Fatty and Waxy Casts 357 1 14. Cylindroids ' 358 115. Crenated Erythrocytes 359 116. Human Spermatozoa 360 117. Esbach's Albuminometer 367 118. Marshall's Urea Apparatus 375 1 19. Hiifner's Urea Apparatus 377 120. Doremus-Hinds Ureometer 378 121. Folin's Urea Apparatus 379 122. Folin's Ammonia Apparatus 380 123. Folin Absorption Tube 381 124. Berthelot-Atwater Bomb Calorimeter 388 125. Soxhlet Apparatus 410 126. Feser's Lactoscope 41 1 PHYSIOLOGICAL CHEMISTRY. CHAPTER I. ENZYMES AND THEIR ACTION. According to the old classification ferments were divided into two classes, the organized ferments and the unorganized ferments. As organized ferments or true ferments there were grouped such substances as yeast and certain bacteria which were supposed to act by virtue of vital processes, whereas the unorganized ferments included salivary amylase (ptyalin), gastric protease (pepsin), pancreatic protease (trypsin), etc., which were described as "non- living unorganized substances of a chemical nature." Kuhne des- ignated this latter class of substances as enzymes (iv typy — in yeast). This division into organized ferments (true ferments) and unorganized ferments (enzymes) was generally accepted and was practically unquestioned until Buchner overthrew it in the year 1897 by his epoch-making investigations on zymase. Previous to this time many writers had expressed the opinion that the action of the ferment organisms was similar to that of the unorganized ferments or enzymes and that therefore the activity of the former was possibly due to the production of a substance in the cell, which was in nature similar to an enzyme. Investigation after investiga- tion, however, failed to isolate any such principle from an active cell and the exponents of the " vital " theory became strengthened in their belief that certain fermentative processes brought about by living cells could not occur apart from the biological activity of such cells. However, as early as 1858, Traube had enunciated, in substance, the principles which were destined to be fundamental in our modern theory of fermentation. He expressed the belief that the yeast cell produced a product in its metabolic activities which had the property of reacting with sugar with the production of carbon dioxide and alcohol, and further that this reaction be- tween the product of the metabolism of the yeast cell and the sugar 2 1 2 PHYSIOLOGICAL CHEMISTRY. occurred without aid from the original cell. It was not until 1897, however, that this theory was placed upon a firm experimental basis. This was brought about through the efforts of Buchner who succeeded in isolating from the living yeast cells a substance (zymase) which, when freed from the last trace of organized cel- lular material, was able to bring about the identical fermentative processes, which, up to this time, had been deemed possible only in the presence of the active, living yeast cell. Buchner's manipulation of the yeast cells consisted in first grind- ing them with sand and infusorial earth after which the finely divided material was subjected to great pressure (300 atmospheres) and yielded a liquid which possessed the fermentative activity of the unchanged yeast cell.1 This liquid contained zymase, the prin- cipal enzyme of the yeast cell. Later the lactic-acid- and acetic- acid-producing bacteria were subjected by Buchner to treatment similar to that accorded the yeast cells, and the active intracellular enzymes were obtained. Many other instances are on record in which a soluble, active, agent has been isolated from ferment cells, with the result that it is pretty well established that all the so-called organized ferments elaborate substances of this character. Therefore, basing our definition on the work of Buchner and others we may define an enzyme, as an unorganised, soluble ferment, which is elaborated by an animal or vegetable cell and wihose ac- tivity is entirely independent of any of the life processes of such a cell. According to this definition the enzyme zymase elaborated by the yeast cell is entirely comparable to the enzyme pepsin elabor- ated by the cells of the stomach mucosa. One is derived from a vegetable cell, the other from an animal cell, yet the activity of neither is dependent upon the integrity of the cell. Enzymes act by catalysis and hence may be termed catalyzers or catalysts. A simple rough definition of a catalyzer is " a sub- stance which alters the velocity of a chemical reaction without un- dergoing any apparent physical or chemical change itself and with- out becoming a part of the product formed." It is a well-known fact that the velocity of the greater number of chemical reactions may be changed through the presence of some catalyzer. For example, take the case of hydrogen peroxide. It spontaneously decomposes slowly into water and oxygen. In the presence of colloidal plati- 1 In later investigations the process was improved by freezing the ground cells with liquid air and finely pulverizing them, before applying the pressure. ENZYMES AND THEIR ACTION. 3 num,1 however, the decomposition is much accelerated and ceases only when the destruction of the hydrogen peroxide is complete. Without multiplying instances, suffice it to say that there is an analogy between inorganic catalyzers and enzymes, the main point of difference between the enzymes and most of the inorganic cataly- zers being that the enzymes are colloids.2 Inasmuch as each of the enzymes has an action which is more or less specific in character, and since it is a fairly simple matter, ordinarily, to determine the character of that action, the classifi- cation of the enzymes is not attended with very great difficulties. They are ordinarily classified according to the nature of the sub- strate3 or according to the type of reaction they bring about. Thus we have various classes of enzymes such as amylolytic* proteolytic, lipolytic, glycolytic, mucolytic, autolytic, oxidizing, reducing, in- verting, protein-coagulating, deaniidizing, etc. In every instance the class name indicates the individual type of enzymatic activity which the enzymes included in that class are capable of accomplish- ing. For example, amylolytic enzymes facilitate the hydrolysis of starch (amylum) and related substances, lipolytic enzymes facilitate the hydrolysis of fats (Xi7ro?) whereas through the agency of uri- colytic enzymes, uric acid is broken down. There is a tendency, at the present time, to harmonize the nomenclature of the enzymes by the use of the termination, -ase. According to this system of nomenclature, all starch-transforming enzymes, or so-called amy- lolytic enzymes, are called amylases, all fat-splitting enzymes are called lipases, etc. Thus ptyalin the amylolytic enzyme of the saliva, would be termed salivary amylase in order to distinguish it from pancreatic amylase (amyl opsin) and vegetable amylases (di- astase, etc.). According to the same system, the fat-splitting enzyme of the gastric juice would be termed gastric lipase to dif- ferentiate it from pancreatic lipase (steapsin), the fat splitting enzyme of the pancreatic juice. Our knowledge regarding the distribution of enzymes has been wonderfully broadened in recent years. Up to within a few years, 1 Produced by the passage of electric sparks between two platinum terminals immersed in distilled water, thus liberating ultra-microscopic particles. 2 Bredig has been able to obtain certain inorganic catalyzers in colloidal solution. These he calls "inorganic enzymes." 3 Substance acted upon. 4 Armstrong suggests the use of the termination " clastic " instead of " lytic." He calls attention to the fact that amylolytic} in analogy with electrolytic, means " decomposition by means of starch " and is therefore a misnomer. He sug- gests the use of aniyloclastic, protco clastic, etc. 4 PHYSIOLOGICAL CHEMISTRY. the real scientific information as to the enzymes of the animal organism, for example, was limited, in the main, to a rather crude understanding of the enzymes intimately connected with the main digestive functions of the organism. We now have occasion to believe that enzymes are doubtless present in every animal cell and are actively associated with all vital phenomena. As a preeminent example of such cellular activity may be cited the liver cell with its reputed complement of 15-20 or more enzymes. In text-book discussions of the enzymes it is customary to say that very little is known regarding the chemical characteristics of these substances since no member of the enzyme group has, up to the present time, been prepared in an absolutely pure condition. Apparently, however, from the nature of the facts in the case, it would be much more accurate to say that we absolutely do not knozv whether a specific enzyme lias, or has not, been prepared in a pure state. (Some authors, like Arthus, have assumed that enzymes are not chemical individuals, but properties conferred upon bodies.) The enzymes are very difficult to prepare in anything like a con- dition approximating purity, since they are very prone to change their nature during the process by which the investigator is attempt- ing to isolate them. For this reason we have absolutely no proof that the final product obtained is, or is not, in the same state of purity it possessed in the original cell. Some of the enzymes are more or less closely associated with the proteins from the fact that they are both formed in every cell as the result of the cellular acti- vity, both may be removed from solution by " salting-out," both are for the most part non-diffusible and are probably very similar as regards elementary composition. Hence in the preparation of some enzymes it is extremely difficult to make an absolute separation from the protein.1 Under certain conditions enzymes are readily adsorbed by shredded protein material, such as fibrin, and may successfully resist the most prolonged attempts at washing them free. We may summarize some of the properties of the great body of enzymes as follows : Enzymes are soluble in dilute glycerol, sodium chloride solution, dilute alcohol and water, and precipitable by ammonium sulphate and strong alcohol. Their presence may be proven from the nature of the end-products of their action and not through the agency of any chemical test. They are colloidal and non-diffusible ,and occur closely associated with protein material with which they possess many properties in common. Each enzyme 1 Others seem to be like the substrate on which they act, e. g., carbohydrate. ENZYMES AND THEIR ACTION. 5 shows the greatest activity at a certain temperature called the optimum temperature; there is also a minimum and a maximum temperature for each specific enzyme. Their action is inhibited by sufficiently lowering the temperature, and the enzyme, if in solution, is entirely destroyed by subjecting it to a temperature of ioo° C. The best known enzymes, whether derived from warm-blooded or cold-blooded animals, are most active between 35°-45° C. The nature of the surrounding media alters the velocity of the enzymatic action, some enzymes being more active in acid solution whereas others require an alkaline fluid. Many of the more important enzymes do not occur preformed within the cell, but are present in the form of a zymogen or mother- substance. In order to yield the active enzyme this zymogen must be transformed in a certain specific manner and by a certain specific substance. This transformation of the inactive zymogen into the active enzyme is termed activation. For instance, the zymogen of the enzyme pepsin of the gastric juice, termed pepsinogen, is acti- vated by the hydrochloric acid secreted by the gastric cells ( see p. 119), whereas the activation of the trypsinogen of the pancreatic juice is brought about by a substance termed entcrokinasc1 ( see p. 141). These are examples of many well known activation pro- cesses going on continually within the animal organism. The ag'ency which is instrumental in activating a zymogen is generally termed a zymo-excitcr or a kinase. In the cases cited hydrochloric acid would be termed a zymo-exciter and enterokinase would be termed a kinase. After filtering yeast juice, prepared by the Buchner process (see p. 2), through a Martin gelatin filter. Harden and Young showed that the colloids left behind and the filtrate were both inactive fermentatively. Upon treating the colloid material (enzyme) with some of the filtrate, however, the mixture was shown to be able to bring about pronounced fermentation. It is believed that a co- enzyme present in the filtrate was the efficient agent in the trans- formation of the inactive enzyme. It is necessary to make frequent renewals of the co-enzyme in order to maintain continuous fermen- tation. It was further shown that this co-enzyme, in addition to being diffusible, was not destroyed by boiling and that it disappeared from yeast juice when this latter was fermented or allowed to undergo autolysis. The exact nature of this co-enzyme of zymase 1 According to Delezenne trypsinogen ma}- be rapidly activated by soluble calcium salts. 6 PHYSIOLOGICAL CHEMISTRY. is unknown. The co-enzyme action, in this case, is probably de- pendent upon the presence of two individual agencies, one of which' is phosphates. It has been shown by Loevenhart that the property of acting as a pancreatic lipase co-enzyme is vested in bile salts, and Magnus has further shown that the synthetic salts are as efficient in this regard as the natural ones. A few other instances of co-enzyme demonstrations have been reported. The so-called " specificity " of enzyme action is an interesting and important fact. That enzymes are very specific as to the character of the substrate or substance acted upon, is well known. Emil Fischer investigated this problem of specificity extensively in connection with the fermentation of sugars and reached the conclusion that enzymes, with the possible exception of certain oxi- dases, can act only upon such substances as have a specific stereo- isomeric relationship to themselves. He considers that the enzyme and its substrate must have an interrelation, such as the key has to the lock, or the reaction does not occur. Fischer was able to predict, in certain definite cases, from a knowledge of the consti- tition and stereo-chemical relationships of a substance, whether or not it would be acted upon by a certain enzyme. An applica- tion of this specificity of enzyme action may be seen in the well- known facts that certain enzymes act on carbohydrates, others on fats, and others on protein, and moreover, that the group of those which transform carbohydrates, for example, is further subdivided into specific enzymes each of which has the power of acting alone upon some one sugar.' It has been conclusively shown, in the case of certain enzymes,1 at least, that their action is a reversible one and is, in all its main features, directly analogous to the reversible reactions produced by chemical means. For instance, in the saponification of ethyl-buty- rate by means of pancreatic lipase, it has been shown that upon the formation of the end-products of the reaction, i. e., butyric acid and ethyl alcohol, there is reversion2 and the reaction is stationary. This does not mean that there are no chemical changes going on, but simply indicates that chemical equilibrium has been established, 1 This is probably a general condition. 2 The re-synthesis of ethyl-butyrate from its hydrolysis products. This may be indicated thus : CsHtCOOGH, + H.O <=* C3HrCOOH + C2H5OH. Ethyl butyrate. Butyric acid. Ethyl alcohol. ENZYMES AND THEIR ACTION. / and that the change in one direction is counterbalanced by the change in the opposite direction. Pancreatic lipase was one of the first enzymes to have the reversibility of its reaction clearly demon- strated.1 A knowledge of the fact that lipase possesses this rever- sibility of action is of extreme physiological importance and aids us materially in the explanation of the processes involved in the digestion, absorption and deposition of fats in die animal organ- ism (see p. 133). In respect to many enzymes it has been found that the law gov- erning the action of inorganic catalyzers is directly applicable, i. e., that the intensity is almost directly proportional to the concentra- tion of the enzyme. In the case of enzymes, however, there is a difference in that a maximum intensity is soon reached and that subsequent concentration of the enzyme is productive of no further increase in intensity. The enzymes which have been shown to obey this linear lazv are lipase, invertase, rennin and trypsin. In certain instances, where this law of direct proportionality between the intensity of action and the concentration of enzyme does not hold, it has been found that the law of Schiitz, first experimentally demonstrated by E. Schiitz, was applicable. This is to the effect that the intensity is directly proportional to the square root of the concentration, or conversely, that the relative concentrations of enzymes are directly proportional to the squares of the intensities.2 It has been shown that there are certain substances which possess the property of directly inhibiting or preventing the action of a catalyzer. These are called anti-catalyzers or paralyzers and have been compared to the anti-toxins. Related to this class of anti- catalytic agents stand the anti-enzymes. The first anti-enzyme to be reported was the anti-rennin of Morgenroth. This was pro- duced by injecting into an animal increasing doses of rennet solu- tion, whereupon an " anti " substance was subsequently found both in the serum and in the milk, which prevented the enzyme rennin from exerting its normal activity in the presence of- caseinogen. In other words, anti-rennin had been formed in the serum of the animal,3 through the repeated injections of rennet solution. Since the discovery of this anti-enzyme, anti-bodies have been demon- strated for pepsin, trypsin, lipase, urease, amylase, laccase, tyro- sinase, emulsin, papain, and thrombin. According to Weinland, 1 The principle was first demonstrated in connection with the enzyme maltase (see p. 55). 2 This law of Schiitz is not generally applicable. 3 Serum is normally anti-try ptic. 5 PHYSIOLOGICAL CHEMISTRY. the reason why the stomach does not digest itself is, that during life there is present in the mucous membrane of the stomach an anti-enzyme {anti-pepsin') which has the property of inhibiting the action of pepsin. A similar substance (anti-trypsin) is present in the intestinal mucosa as well as in the tissues of various intestinal worms. Some investigators are not inclined to accept the enzyme nature of these inhibitory agents as proven. EXPERIMENTS ON ENZYMES AND ANTI-ENZYMES A. Experiments on Enzymes.1 I. AMYLASES. i. Demonstration of Salivary Amylase.2 — To 25 c.c. of a one per cent starch paste in a small beaker, add 5 drops of saliva and stir thoroughly. At intervals of a minute remove a drop of the so- lution to one of the depressions of a test-tablet and test by the iodine test.3 If the blue color with iodine still forms after five minutes, add another five drops of saliva. The opalescence of the starch solution should soon disappear, indicating the formation of soluble starch (aniidulin) which gives a blue color with iodine. This body should soon be transformed into erythrodextrin which gives a red color with iodine and this, in turn, should pass into* achroodex- trin which gives no color with iodine. This point is called the achromic point. When this point is reached test by Fehling's test4 to show the production of a reducing substance (maltose). A posi- tive Fehling's test may be obtained while the solution still reacts red with iodine inasmuch as some sugar is formed from the soluble starch coincidently with the formation of the erythrodextrin. For further discussion of the transformation of starch see p. 54. 2. Demonstration of Pancreatic Amylase.5 — Proceed exactly as indicated above in the Demonstration of Salivary Amylase ex- cept that the saliva is replaced by 5 c.c. of pancreatic extract pre- pared as described on p. 144. Pancreatic amylase transforms the starch in a manner entirelv analogous to the transformation result- ing from the action of salivary amylase. 1If it is deemed advisable by the instructor to give all the practical work upon enzymes at this point in the course, additional experiments will be found in Chapters III, VI and VIII. 2 For a discussion of this enzyme see p. 54. 3 See p. 44. * See p. 27. 5 For a discussion of this enzyme see p. 142. ENZYMES AND Till: Ik ACTION. 9 3. Preparation of Vegetable Amylase. — Extracl finely ground malt with water, filter and subject the filtrate to alcoholic fermenta- tion by means of yeast. When fermentation is complete filter off the yeast and precipitate the amylase from the filtrate by the addi- tion of alcohol. The precipitate may he filtered off and obtained in the form of a fine white powder. 4. Demonstration of Vegetable Amylase. — This enzyme may be demonstrated according to the directions given under Demonstra- tion of Salivary Amylase, p. 8, with the exception that the saliva used in that experiment is replaced by an aqueous solution of the vegetable amylase powder prepared as described above.1 II. PROTEASES. i. Preparation of Gastric Protease.2 — Treat the finely com- minuted mucosa of a pig's stomach with 0.4 per cent hydrochloric acid and extract at 380 C. for 24-48 hours. The filtrate from this mixture constitutes a very satisfactory acid extract of gastric protease (see p. 122). 2. Demonstration of Gastric Protease. — Introduce some pro- tein material (fibrin, coagulated egg-white, or washed lean beef) into the acid extract of gastric protease prepared as above described.3 add an equal volume of 0.4 per cent hydrochloric acid and place the mixture at 38 ° C. for 2-3 days. Identify the products of digestion according to directions given on p. 122. 3. Preparation of Pancreatic Protease.4 — A satisfactory ex- tract of this enzyme may be made from the pancreas of a pig or sheep according to the directions given on p. 144. 4. Demonstration of Pancreatic Protease. — Into an alkaline extract of pancreatic protease,5 prepared as directed on p. 144. in- troduce some fibrin, coagulated egg-white or lean beef and place the mixture at 380 C. for 2-5 days.0 At the end of that period 1 If desired the first aqueous extract of the original malt may be used in this demonstration. Commercial taka-diastase may also be employed. 2 Also called pepsin, pepsase, gastric proteinase, and acid protease. For a dis- cussion of this enzyme see p. 120. 3 If so desired a solution of commercial pepsin powder in 0.2 per cent hydro- chloric acid may be substituted. 4 Also called trypsin, trypsasc. pancreatic proteinase and alkali proteinase. For a discussion of this enzyme see p. 141. 5 A 0.25 per cent sodium carbonate solution of commercial trypsin may bo substituted. 6 A few c.c. of toluene or an alcoholic solution of thymol should be added to prevent putrefaction. IO PHYSIOLOGICAL CHEMISTRY. separate and identify the end-products of the action of pancreatic protease according to the directions given on p. 145. 5. Demonstration of a Vegetable Protease. — A commercial preparation of papain (papayotin, carase or papase) , the protease of the fruit of the pawpaw (carica papaya), may be used in this connection. Follow the same procedure as that described under gastric protease (see p. 9). III. LIPASES. i. Preparation of Pancreatic Lipase.1 — An extract of this en- zyme may be prepared from the pancreas of the pig or sheep ac- cording to the directions given on p. 144.2 2. Demonstration of Pancreatic Lipase. — Into each of two test-tubes introduce 10 c.c. of milk and a small amount of litmus powder. To the contents of one tube add 3 c.c. of a neutral ex- tract of pancreatic lipase and to the contents of the other tube add 3 c.c. of a boiled neutral extract of pancreatic lipase. Keep the tubes at 38 ° C. and watch for color changes. The blue color of the litmus powder will gradually give place to a red. This change in the color of the litmus from blue to red has been brought about by the fatty acid which has been produced through the lipolytic ac- tion exercised by the lipase upon the milk fats. 3. Preparation of Vegetable Lipase. — This enzyme may be readily prepared from castor beans, several months old, by the fol- lowing procedure :3 Grind the shelled beans' very fine4 and ex- tract for twenty-four hour periods with alcohol-ether and ether, in turn. Reduce the semi-fat-free material to the finest possible con- sistency by means of mortar and pestle and pass this material through a sieve of very fine mesh. Place this material in a Soxhlet extractor and extract for one week. This fat-free powder may then be used to demonstrate the action of vegetable lipase. Powder prepared as described may be used in quantitative tests. For ordi- nary qualitative tests it is not necessary to remove the last traces of fat and therefore the extraction period in the Soxhlet apparatus may be much shortened. 1 Also called steapsin. For a discussion of this enzyme see p. 143. A very active lipolytic extract may also be prepared from the liver. 2 If preferred a glycerol extract may be prepared according to the directions given by Kanitz ; Zeitschrift fur physiologische Chemie, 1906, XLVI, p. 482. 3 A. E. Taylor: On Fermentation; University of California Publications, 1907. 1 The shells should be removed without the use of water. These beans are poisonous due to their content of ricin. ENZYMES AND THEIR ACTION. I I 4. Demonstration of Vegetable Lipase. — The lipolytic action of the lipase prepared from the castor bean, as just described, may be demonstrated in a manner entirely analogous to that used in the Demonstration of Pancreatic Lipase, see p. 10. Proceed as indi- cated in that experiment and substitute the vegetable lipase powder for the neutral extract of pancreatic lipase. The type of action is entirely analogous in the two instances. An experiment similar to Experiment 2, p. 149, may also be tried if desired. In this experiment 0.2 c.c. of either ethyl batyrate or aniyl acetate may be employed. IV. INVERTASES.1 i. Preparation of an Extract of Sucrase.2 — Treat the finely divided epithelium of the small intestine of a dog, pig, rat, rabbit, or hen, with about three volumes of a two per cent solution of sodium fluoride and permit the mixture to stand at room temperature for twenty-four hours. Strain the extract through cloth or absorbent cotton and use the strained material in the following demonstra- tion. 2. Demonstration of Sucrase. — To about 5 c.c. of a one per cent solution of sucrose, in a test-tube, add about one cubic centi- meter of a two per cent sodium fluoride intestinal extract, prepared as described above. Prepare a control tube in which the intestinal extract is boiled before being added to the sugar solution. Place the two tubes at 380 C. for two hours.3 Heat the mixture to boil- ing to coagulate the protein material, filter, and test the filtrate by Fehling's test (see p. 27). The tube containing the boiled extract should give no response to Fehling's test whereas the tube con- taining the unboiled extract should reduce the Fehling's solution. This reduction is due to the formation of invert sugar (see p. 41 ^ from the sucrose through the action of the enzyme sucrase which is present in the intestinal epithelium. 3. Preparation of Vegetable Sucrase. — Thoroughly grind about 100 grams of brewer's yeast in a mortar with sand. Spread the ground yeast in thin layers on glass or porous plates and dry it rapidly in a current of dry, warm air. Powder this dry yeast, extract it with distilled water and filter. Pour the filtrate into 1 The inverting enzymes of the alimentary tract; Mendel and Mitchell : American Journal of Physiology, 1907-08, XX, p. 81. 2 For a discussion of this enzyme see p. 144. 8 If a positive result is not obtained in this time permit the digestion to proceed for a longer period. 12 PHYSIOLOGICAL CHEMISTRY. acetone, stir and after permitting the acetone mixture to stand for a few minutes filter on a Buchner funnel. The resulting precipi- tate, after drying and pulverizing, may be used to demonstrate vegetable sucrase. 4. Demonstration of Vegetable Sucrase. — To about 5 c.c. of a one per cent solution of sucrose in a test-tube add a small amount of the sucrase powder prepared as directed above. Place the tube at 380 C. for 24-72 hours and at the end of that period test the solution by Fehling's test. Reduction indicates that the active sucrase powder has transformed the non-reducing sucrose into dextrose and lsevulose, and these sugars, in turn, have reduced the Fehling solution. 5. Preparation of an Extract of Lactase.1 — Treat the finely divided epithelium of the small intestine of a kitten, puppy, or pig embryo with about three volumes of a two per cent solution of sodium fluoride and permit the mixture to stand at room tempera- ture for twenty- four hours. Strain the extract through cloth or absorbent cotton and use the strained material in the following demonstration. 6. Demonstration of Lactase.2 — To about 5 c.c. of a one per cent solution of lactose in a test-tube add about one cubic centi- meter of a toluene-water extract or a two per cent sodium fluoride extract of the first part of the small intestine3 of a kitten, puppy, or pig embryo prepared as described above. Prepare a control tube in which the intestinal extract is boiled before being added to the sugar solution. Place the two tubes at 38 ° C. for 24 hours. At the end of this period add one cubic centimeter of the digestion mixture to 5 c.c. of Barfoed's4 reagent and place the tubes in a boiling water-bath.5 Examine the tubes at the end of three min- utes against a black background in a good light. If no cuprous oxide is visible replace the tubes and repeat the examination at the end of the fourth and fifth minutes. If no reduction is then ob- served permit the tubes to stand at room temperature for 5-10 min- utes and examine again.6 1 For a discussion of this enzyme see p. 144. 3 Roaf ; Bio-Chemical Journal, 1908, III, p. 182. 3 Duodenum and first part of jejunum. 4 To 4.5 grams of neutral crystallized cupric acetate in 900 c.c. of water, add 0.6 c.c. of glacial acetic acid and make the total volume of the solution one liter. 5 Care should be taken to see that the water in the bath reaches at least to the upper level of the contents of the tubes. 6 Sometimes the drawing of conclusions is facilitated by pouring the mixture from the tube and examining the bottom of the tube for adherent cuprous oxide. ENZYMES AND THEIR ACTION. 13 It has been determined that disaccharide solutions will not reduce' Barf oed's reagent until after they have been heated for 9-10 minutes on a boiling- water-bath in contact with the reagent.1 Therefore in the above test, if the tube containing the unboiled extract exhibits any reduction after being heated as indicated, for a period of five minutes or less, and the control tube containing boiled extract shows no reduction, it may be concluded that lactase was present in the intestinal extract.2 7. Preparation of an Extract of Maltase.3 — Treat the finely divided epithelium of the small intestine of a cat, kitten, or pig (embryo or adult) with about three volumes of a two per cent solu- tion of sodium fluoride and permit the mixture to stand at room temperature for twenty-four hours. Strain the extract through cloth and use the strained material in the following demonstration. 8. Demonstration of Maltase. — Proceed exactly as indicated in the demonstration of lactase, above, except that a one per cent solu- tion of maltose is substituted for the lactose solution. The extract used may be prepared from the upper part of the intestine of a cat, kitten, or pig (embryo or adult). In the case of lactase, as indi- cated, the intestine used should be that of a kitten, puppy, or pig (embryo). V. EREPSIN.4 1. Preparation of Erepsin. — Grind the mucous membrane of the small intestine of a cat, dog or pig, with sand in a mortar. Treat the mortared membrane with toluene- or chloroform-water and permit the mixture to stand, with occasional shaking, for 24-72 hours.5 Filter the extract thus prepared through cotton and use the filtrate in the following experiment. 2. Demonstration of Erepsin. — To about 5 c.c. of a one per cent solution of Witte's peptone in a test-tube -add about one c.c. of the erepsin extract prepared as described above and make the mixture slightly alkaline (0.1 per cent) with sodium carbonate. Prepare a second tube containing a like amount of peptone solu- tion but boil the erepsin extract before introducing it. Place the xThe heating for 9-10 minutes is sufficient to transform the disaccharide into monosaccharide. 2 The reduction would, of course, be due to the action of the dextrose and galactose which had been formed from the lactose through the action of the enzyme lactase. 3 For a discussion of this enzyme see p. 55. 4 Also called erepsase. For a discussion of this enzyme see p. 143. 5 The enzyme may also be extracted by means of glycerol or alkaline "physi- ological" salt solution if desired. 14 PHYSIOLOGICAL CHEMISTRY. two tubes at 380 C. for 2-3 days. At the end of that period heat the contents of each tube to boiling, filter and try the biuret test on each filtrate. In making these tests care should be taken to use like amounts of filtrate, potassium hydroxide and cupric sulphate in each test in order that the drawing of correct conclusions may be facilitated. The contents of the tube which contained the boiled extract should show a deep pink color with the biuret test, due to the peptone still present. On the other hand the biuret test upon the contents of the tube containing the unboiled extract should be negative or exhibit, at the most, a faint pink or blue color, signify- ing that the peptone, through the influence of the erepsin, has been transformed, in great part at least, into amino acids which do not re- spond to the biuret test.1 VI. URICOLYTIC ENZYME.2 1. Preparation of Uricolytic Enzyme. — Extract pulped liver tissue with toluene- or chloroform-water at 380 C. for 24 hours, with occasional shaking. Filter the extract and use the filtrate in the following experiment. 2. Demonstration of Uricolytic Enzyme. — Add about 0.1 gram of uric acid to 10 c.c. of water and bring the uric acid into solution by the addition of the minimal quantity of potassium hy- droxide. To 5 c.c. of this uric acid solution, in a test-tube, add 5 c.c. of the uricolytic enzyme extract prepared as described above. Prepare a second tube containing a like amount of uric acid solution but boil the extract before it is introduced. Place the two tubes at 38 ° C. for 3-4 days and titrate the two digestive mixtures with a solution of potassium permanganate according to directions given under Folin-Shaffer Method, Chapter XXII. It will be found that the mixture containing the boiled extract requires a much larger volume of the permanganate to complete the titration than the other tube. This indicates that a uricolytic enzyme has destroyed at least a portion of the uric acid which was originally present in the tube containing the unboiled extract. VII. CATALASE. Demonstration of Catalase. — The various animal tissues, such as liver, kidney, blood, lung, muscle and brain contain an enzyme 1 Strictly speaking this erepsin demonstration is not adequate unless a control test is made with native protein (except caseinogen, histones and protamines) to show that the extract is trypsin-free and digests peptone but not native protein. 2 Mendel and Mitchell ; American Journal of Physiology, 1908, XX, p. 97. ENZYMES AND THEIR ACTION. I 5 called caialase which possesses the property of decomposing hydro- gen peroxide. The presence of this enzyme may he demonstrated as follows: Introduce into a low, broad, wide-mouthed bottle some pulped liver tissue and a porcelain crucible containing neutral hydro- gen peroxide.1 Connect the bottle with a eudiometer filled with water, upset the crucible of hydrogen peroxide upon the liver pulp and note the collection of gas in the eudiometer. This gas is oxy- gen which has been liberated from the hydrogen peroxide through the action of the catalase of the liver tissue. B. Experiments on Anti-Enzymes. 1. Preparation of an Extract of Anti-Pepsin.2-— Grind up a number of intestinal worms (ascaris)3 with quartz sand in a mortar. Subject this mass to high pressure, filter the resultant juice and treat it with alcohol until a concentration of sixty per cent is reached. If any precipitate forms it should be filtered off4 and alcohol added to the filtrate until the concentration of alcohol is 85 per cent, or over. The anti-enzyme is precipitated by this concentration. Permit this precipitate to stand for twenty-four hours, then filter it off, wash it with 95 per cent alcohol, absolute alcohol, and ether, in turn, and finally dry the substance over sulphuric acid. The sticky powder which results may be used in this form or may be dissolved in water as desired and the aqueous solution used.5 2. Demonstration of Anti-Pepsin.6 — Introduce into a test-tube a few fibrin shreds and equal volumes of pepsin-hydrochloric acid7 and ascaris extract made as indicated above. Prepare a control tube in which the ascaris extract is replaced by water. Place the two tubes at 380 C. Ordinarily in one hour the fibrin in the control tube will be completely digested. The fibrin in the tube containing the ascaris extract may, however, remain unchanged for days, thus indicating the inhibitory influence exerted by the anti-enzyme pres- ent in this extract. 3. Preparation of an Extract of Anti-Trypsin.s — The extract 1 Mendel and Leavenworth; American' Journal of Physiology, 1908, XXI, p. 85. ~ Anti-gastric-protease or anti-acid-protease. 3 These may be readily obtained from pigs at a slaughter house. 4 This precipitate consists of impurities, the anti-enzyme not being precipitated until a higher concentration of alcohol is reached. 5 The original ascaris extract possesses much greater activity than either the powder or the aqueous solution. 6 Martin H. Fischer; Physiology of Alimentation, 1907, p. 134. 7 Made by bringing 0.015 gram of pepsin into solution in 7 c.c. of water and 0.23 gram of concentrated hydrochloric acid. s Anti-pancreatic-protease or Anti-alkali-protease. 1 6 PHYSIOLOGICAL CHEMISTRY. may be prepared from the intestinal worm, ascaris, according to the directions given on page 15. 4. Demonstration of Anti-Trypsin. — Introduce into a test-tube a few shreds of fibrin and equal volumes of an artificial tryptic solution1 and the ascaris extract made as described on page 15. Prepare a control tube in which the ascaris extract is replaced by water. Place the two tubes at 38 ° C. Ordinarily the fibrin in the control tube will be completely digested in two hours. The fibrin in the tube containing the ascaris extract may, however, remain unchanged for days, thus indicating the inhibitory influence of the anti-enzyme. Blood serum also contains anti-try p sin. This may be demon- strated as follows : Introduce equal volumes of serum and artificial tryptic solution (prepared as described above) into a test-tube and add a few shreds of fibrin. Prepare a control tube containing boiled serum. Place the two tubes at 380 C. It will be observed that the fibrin in the tube containing the boiled serum digests, whereas that in the other tube does not digest. The anti-trypsin present in the unboiled serum has exerted an inhibitory influence upon the action of the trypsin. C. Quantitative Applications. 1. Quantitative Determination of Amy loly tic Activity. — Wohl- gemuth^ Method. — Arrange a series of test-tubes with diminishing quantities of the enzyme solution under examination, introduce into each tube 5 c.c. of a 1 per cent solution of soluble starch2 and place each tube at once in a bath of ice water.3 When all the tubes have been prepared in this way and placed in the ice water-bath they are transferred to a water-bath or incubator and kept at 38 ° C. for from thirty minutes to an hour.4 At the end of this digestion 1 Made by dissolving 0.04 gram of sodium carbonate and 0.015 gram of trypsin in 8 c.c. of water. 2 Kahlbaum's soluble starch is satisfactory. In preparing the 1 per cent solu- tion, the weighed starch powder should be dissolved in the proper volume of cold, distilled water and stirred until a homogeneous suspension is obtained. The mixture should then be heated, with constant stirring, in a porcelain dish, until it is clear. This ordinarily takes about 8-10 minutes. A slightly opaque solution is thus obtained which should be cooled before using. 3 Ordinarily a series of six tubes is satisfactory, the volumes of the enzyme solution used ranging from 1 c.c. to 0.1 c.c. and the measurements being made by means of a 1 c.c. graduated pipette. Each tube should be placed in the ice water bath as soon as the starch solution is introduced. It will be found convenient to use a small wire basket to hold the tubes. 4 Longer digestion periods may be used where it is deemed advisable. If ex- ceedingly weak solutions are being investigated, it may be most satisfactory to permit the digestion to extend over a period of 24 hours. ENZYMES AND THEIR ACTION. 17 period the tubes are again removed to the bath of ice water in order that the action of the enzyme may be stopped. Dilute the contents of each tube, to within about one-half inch of the top, with water, add one drop of a T^ solution of iodine and shake the tube and contents thoroughly. A series of colors rang- ing from dark blue through bluish-violet and reddish-yellow to yellow, will be formed.1 The dark blue color shows the presence of unchanged starch, the bluish-violet indicates a mixture of starch and erythrodextrin, whereas the reddish-yellow signifies that eryth- rodextrin and maltose are present, and the yellow solution denotes the complete transformation of starch into maltose. Examine the tubes carefully before a white background and select the last tube in the series which shows the entire absence of all blue color, thus indicating that the starch has been completely transformed into dextrins and sugar. In case of indecision between two tubes, add an extra drop of the iodine solution, and observe them again, after shaking, Calculation. — The amylolytic activity2 of a given solution is expressed in terms of the activity of i c.c. of such a solution. For example, if it is found that 0.02 c.c. of an amylolytic solution, acting at 380 C. completely transformed the starch in 5 c.c. of a 1 per cent starch solution in 30 minutes, the amylolytic activity of such a solution would be expressed as follows : < = 25o. This indicates that 1 c.c. of the solution under examination pos- sesses the power of completely digesting 250 c.c. of a 1 per cent starch solution in 30 minutes at 38 ° C. 2. Quantitative Determination of Peptic Activity, (a) Mett's Method. — The determination of the actual rate of peptic ac- tivity is a most important procedure under certain conditions. Sev- eral methods of making this determination are in use. The method of Sprigg3 is probably the most accurate method yet devised for this purpose. It is, however, too complicated and time-consuming for clinical purposes. The method of Mett, given below, is very simple although not strictly accurate. The procedure is as follows : To about 5 c.c. of the gastric juice under examination in a test- 1 See p. 44. ' Designated by " D " the first letter of " diastatic." 3 Sprigg: Zeitschrift fur physiologische Chemie, 1902. XXXV, p. 465. 1 8 PHYSIOLOGICAL CHEMISTRY. tube add a section of a Mett tube1 and place the mixture at 380 C. for ten hours. At the end of this period, the tube should be re- moved from the gastric juice and the length of the column of coagulated albumin which has been digested, carefully determined by means of a low power microscope and a millimeter scale. In normal human gastric juice the upper limit is 4 mm. However, control tests should always be made to determine the digestibility of the coagulated albumin in artificial gastric juice inasmuch as this factor will vary with different albumin preparations. In connection with this test Schiitz's law should be borne in mind. This principle is to the effect that the amount of proteolytic enzyme present in a digestion mixture is proportional to the square of the number of millimeters of albumin digested. Therefore a gastric juice which digests 2 mm. of albumin contains four times as much pepsin as a gastric juice which digests only 1 mm. of albu- min. And further, if the quantities of albumin digested are 2 mm. and 3 mm. respectively, the ratio between the pepsin values will be as 4 : 9. It is claimed by Nirenstein and Schiff that the principle of Schutz does not apply to gastric juice unless this fluid be diluted with fifteen volumes of N/20 hydrochloric acid. (b) Fuld and Levison's Method. — This test is founded upon the fact, shown by Osborne, that edestin when brought into solu- tion in dilute acid will change in its solubility, due to the contact with the acid, and that a protean called edestan, which is insoluble in neutral fluid, will be formed. The procedure is as follows : Dilute the gastric juice under examination with 20 volumes of water and introduce gradually decreasing volumes of the diluted juice into a series2 of narrow test-tubes about 1 cm. in diameter. 1 In the preparation of these tubes, egg-white is diluted with an equal volume of water, the precipitated globulin filtered off and the filtrate collected in a tall, narrow beaker or a large test-tube. A bundle of capillary tubes about 10 cm. in length and 2 mm. in diameter are now placed in this vessel in such a manner that they are completely submerged in the albumin solution. After an examination has shown that the tubes are completely filled with the albumin solution and that there are no interfering air-bubbles, the vessel and its con- tained tubes is heated for 5-15 minutes in a boiling water-bath, in order to coagulate the albumin. When this coagulation is complete, the tubes are re- moved, all albumin adhering to them is carefully cleaned off, and the tubes rendered air-tight by the application of sealing wax at either end. When needed for use, these tubes are cut into sections about 2 cm. in length. 2 The longer the series, the more accurate the deductions which may be drawn. ENZYMES AND THEIR ACTION. 19 The measurements of gastric juice may conveniently be made with a one c.c. pipette which is accurately graduated in Moo c.c. Into the first tube in the series may be introduced one c.c. of gastric juice, and the tubes which follow in the series may receive vol- umes which differ, in each instance, from the volume introduced into the preceding tube by Moo, Yso, !•!<>• or Mo of a cubic centi- meter. Now rapidly introduce into each tube the same volume (e. g., 2 c.c.) of a i : iooo solution of edestin'1 and place the tubes at 40 ° C. for one-half hour. At the end of this time stratify ammonium hydroxide upon the contents of each tube,2 place the tubes in position before a black background and examine them carefully. The ammonium hydroxide, by diffusing into the acid fluid, forms a neutral zone and in this zone will be precipitated any undigested edestan which is present. Select the tube in the series which contains the least amount of gastric juice and which ex- hibits no ring, signifying that the edestan has been completely digested, and calculate the peptic activity of the gastric juice under examination on the basis of the volume of gastric juice used in this particular tube. Calculation. — Multiply the number of c.c. of edestin solution used by the dilution to which the gastric juice was originally sub- jected and divide the volume of gastric juice necessary to com- pletely digest the edestan by this product. For example, if 2 c.c. of the edestin solution was completely digested by 0.25 c.c. of a 1 : 20 gastric juice we would have the following expression ; 0.25 -i- 20 X 2 or 1 : 160. This peptic activity may be expressed in several ways, e. g., (a) 1:160 pepsin; (b) 160 pepsin content; (c) 160 parts. 3. Quantitative Determination of Tryptic Activity. — Gross' Method. — This method is based upon the principle that faintly alka- line solutions of casein are precipitated upon the addition of dilute (1 per cent) acetic acid whereas its digestion products are not so precipitated. The method follows : Prepare a series of tubes each 1 This edestin should be prepared in the usual way (see p. 103), and brought into solution in a dilute hydrochloric acid of approximately the same strength as that which occurs normally in the human stomach. This may be conveniently made by adding 30 c.c. of fT) hydrochloric acid to 70 c.c. of water. Ordinarily it should not take longer than one minute to introduce the edestin solution into the entire series of tubes. However, if the edestin is added to the tubes in the same order as the ammonium hydroxide is afterward stratified, no appreciable error is introduced. 2 Making the stratification in the same order as the edestin solution was added. 20 PHYSIOLOGICAL CHEMISTRY. containing 10 c.c. of a o. i per cent solution of pure, fat-free, casein,1 which has been heated to a temperature of 400 C. Add to the contents of the series of tubes increasing amounts of the trypsin solution under examination,2 and place them at 400 C. for fifteen minutes. At the end of this time remove the tubes and acidify the contents of each with a few drops of dilute (1 per cent) acetic acid. The tubes in which the casein is completely digested will remain clear when acidified while those tubes which contain undi- gested casein will become more or less turbid under these condi- tions. Select the first tube in the series which exhibits no turbidity upon acidification, thus indicating complete digestion of the casein, and calculate the tryptic activity of the enzyme solution under ex- amination. Calculation. — The unit of tryptic activity is an expression of the power of 1 c.c. of the fluid under examination exerted for a period of fifteen minutes on 10 c.c. of a 0.1 per cent casein solution. For example, if 0.5 c.c. of a trypsin solution completely digests 10 c.c. of a 0.1 per cent solution of casein iii fifteen minutes the activity of that solution would be expressed as follows : Tryptic activity = 1 -f- 0.5 = 2. Such a trypsin solution would be said to possess an activity of 2. If 0.3 c.c. of the trypsin solution had been required the solution would be said to possess an activity of 3.3 i. e., 1 -^-0.3 = 3.3. 1 Made by dissolving one gram of Griibler's casein in a liter of 0.1 per cent sodium carbonate. A little chloroform may be added to prevent bacterial action. 2 The amount of solution used may vary from 0.1-1 c.c. The measurements may conveniently be made by means of a 1 c.c. graduated pipette. CHAPTER II. CARBOHYDRATES. The name carbohydrates is given to a class of bodies which are an especially prominent constituent of plants and which are found also in the animal body either free or as an integral part of various proteins. They are called carbohydrates because they contain the elements C, H and O; the H and O being present in the proportion to form water. The term is not strictly appropriate inasmuch as there are bodies such as acetic acid, lactic acid and inosite which have H and O present in the proportion to form water, but which are not carbohydrates, and there are also true carbohydrates which do not have H and O present in this proportion, e. g., rhamnose, C6H1205. Chemically considered, the carbohydrates are aldehyde or ketone derivatives of complex alcohols. Treated from this standpoint the aldehyde derivatives are spoken of as aldoses, and the ketone deriva- tives are spoken of as ketoses. The carbohydrates are also fre- quently named according to the number of oxygen atoms present in the molecule, e. g., trioses, pentoses and hexoses. The more common carbohydrates may be classified as follows : I. Monosaccharides. i. Hexoses, CGH12O0. (a) Dextrose. (b) Lsevulose. (c) Galactose. 2. Pentoses, C5H10O5. (a) Arabinose. (b) Xylose. (c) Rhamnose (Methyl-pentose), C6H1205. II. Disaccharides, C12H22On. i. Maltose. 2. Lactose. 3. Iso-Maltose. 4. Sucrose. 22 PHYSIOLOGICAL CHEMISTRY. III. Trisaccharides, C1SH3201G. i. Raffinose. IV. Polysaccharides, (C6H10O5)x. i. Starch Group. (a) Starch. (b) Inulin. (c) Glycogen. (d) Lichenin. 2. Gum and Vegetable Mucilage Group. (a) Dextrin. (b) Vegetable Gums. 3. Cellulose Group. (a) Cellulose. (b) Hemi-Cellulose. Each member of the above carbohydrate classes, except the mem- bers of the pentose group, may be supposed to contain the group C6H10O5 called the saccharide group. The polysaccharides consist of this group alone taken a large number of times, whereas the disaccharides may be supposed to contain two such groups plus a molecule of water, and the monosaccharides to contain one such group plus a molecule of water. Thus, (C6H10O5)x = polysac- charide, (C6H10O5)2 -f- H20 = disaccharide, C6H10O5 -f- H20 = monosaccharide. In a general way the solubility of the carbo- hydrates varies with the number of saccharide groups present, the substances containing the largest number of these groups being the least soluble. This means simply that, as a class, the monosac- charides (hexoses) are the most soluble and the polysaccharides (starches and cellulose) are the least soluble. MONOSACCHARIDES. Hexoses, C6H1206. The hexoses are monosaccharides containing six oxygen atoms in the molecule. They are the most important of the simple sugars, and two of the principal hexoses, dextrose and lsevulose, occur widely distributed in plants and fruits. Of these two hexoses, dextrose results from the hydrolysis of starch whereas both dextrose and lsevulose are formed in the hydrolysis of sucrose. Galactose, which with dextrose results from the hydrolysis of lactose, is also CARBOHYDRATES. 23 an important hexose. These three hexoses are fermentable by yeast, and yield laevulinic acid upon heating with dilute mineral acids. They reduce metallic oxides in alkaline solution, are optically active, and extremely soluble. With phenylhydrazine they form characteristic osazones. CH2OH DEXTROSE, (CHOH)4. CHO Dextrose, also called glucose or grape sugar, is present in the blood in small amount and may also occur in traces in normal urine. After the ingestion of large amounts of sucrose, lactose or dex- trose, causing the assimilation limit to be exceeded, an alimentary glycosuria may arise. In diabetes mellitus very large amounts of dextrose are excreted in the urine. The following structural for- mula has been suggested by Victor Meyer for d-dextrose : COH H - C - OH HO - C - H I H - C - OH H - C - OH CH2OH (For further discussion of dextrose see section on Hexoses, page 22.) Experiments on Dextrose. 1. Solubility. — Test the solubility of dextrose in the "ordinary solvents" and in alcohol. (In the solubility tests throughout the book we shall designate the following- solvents as the " ordinary solvents": H20 ; 10 per cent NaCl; 0.5 per cent Na2COs ; 0.2 per cent HC1; concentrated KOH; concentrated HC1.) 2. Molisch's Reaction. — Place approximately 5 c.c. of concen- trated H2S04 in a test-tube. Incline the tube and slowly pour down the inner side of it approximately 5 c.c. of the sugar solution to which 2 drops of Molisch's reagent (a 15 per cent alcoholic solution 24 PHYSIOLOGICAL CHEMISTRY. of a-naphthol) has been added, so that the sugar solution will not mix with the acid. A reddish-violet zone is produced at the point of contact. The reaction is due to the formation of furfurol, HC^CH HC C-CHO, \/ 0 by the acid. The test is given by all bodies containing a carbohy- drate group and is therefore not specific and, in consequence, of very little practical importance. 3. Phenylhydrazine Reaction. — Test according to one of the following methods: (a) To a small amount of phenylhydrazine mixture, furnished by the instructor,1 add 5 c.c. of the sugar solu- tion, shake well and heat on a boiling water-bath for one-half to three-quarters of an hour. Allow the tube to cool slowly and examine the crystals microscopically (Plate III, opposite). If the solution has become too concentrated in the boiling process it will be light-red in color and no crystals will separate until it is diluted with water. Yellow crystalline bodies called osazones are formed from certain sugars under these conditions, in general each individual sugar giving rise to an osazone of a definite crystalline form which is typical for that sugar. It is important to remember in this connec- tion that of the simple sugars of interest in physiological chemistry, dextrose and kevulose yield the same osazone. Each osazone has a definite melting-point and as a further and more accurate means of identification it may be recrystal'lized and identified by the determi- nation of its melting-point and nitrogen content. The reaction tak- ing place in the formation of phenyldextr osazone is as follows : C6H1206 + 2(H2N-NH-C6H5) = Dextrose. Phenylhydrazine. C6H10O4(NNHC6H5)2 + 2H20 + H2. Phenyldextrosazone. (b) Place 5 c.c. of the sugar solution in a test-tube, add 1 c.c. of 1 This mixture is prepared by combining one part of phenylhydrazine hydro- chloride and two parts of sodium acetate, by weight. These are thoroughly mixed in a mortar. PLATE III. OSAZONES. Upper form, dextrosazone or lxvulosazone ; central form, maltosazone ; lower form. lactosazone. CARBOHYDRATES. 25 the phenylhydrazine-acetate solution furnished by the instructor,1 and heat on a boiling water-bath for one-half to three-quarters of an hour. Allow the liquid to cool slowly and examine the crystals microscopically (Plate III, opposite p. 24). The phenylhydrazine test has been so modified by Cipollina as to be of use as a rapid clinical test. The directions for this test are given in the next experiment. 4. Cipollina's Test. — Thoroughly mix 4 c.c. of dextrose solu- tion, 5 drops of phenylhydrazine (the base) and y2 c.c. of glacial acetic acid in a test-tube. Heat the mixture for about one minute over a low flame, shaking the tube continually to prevent loss of fluid by bumping. Add 4-5 drops of sodium hydroxide (sp. gr. 1. 16), being certain that the fluid in the test-tube remains acid, heat the mixture again for a moment and then cool the contents of the tube. Ordinarily the crystals form at once, especially if the sugar solution possesses a low specific gravity. If they do not appear immediately allow the tube to stand at least 20 minutes before deciding upon the absence of sugar. Examine the crystals under the microscope and compare them with those shown in Plate III, opposite page 24. 5. Precipitation by Alcohol. — To 10 c.c. of 95 per cent alcohol add about 2 c.c. of dextrose solution. Compare the result with that obtained under Dextrin, 7, page 49. Fig. 1. Dialyzixg Apparatus for Students' Use. 6. Iodine Test.— Make the regular iodine test as given under Starch, 5, page 44, and keep this result in mind for comparison with the results obtained later with starch and with dextrin. 7. Diffusibility of Dextrose. — Test the diffusibility of dextrose 1 This solution is prepared by mixing one part by volume, in each case, of glacial acetic acid, one part of water and two parts of phenylhydrazine (the base). 26 PHYSIOLOGICAL CHEMISTRY. solution through animal membrane, or parchment paper, making a dialyzer like one of the models shown in Fig. I, p. 25. 8. Moore's Test. — To 2-3 c.c. of sugar solution in a test-tube add an equal volume of concentrated KOH or NaOH, and boil. The solution darkens and finally assumes a brown color. At this point the odor of caramel may be detected. This is an exceedingly crude test and is of little practical value. The brown color is due to the oxidation of the dextrose and the resulting formation of the potassium or sodium salts of certain organic acids which are formed as oxidation products. 9. Reduction Tests. — To their aldehyde or ketone structure many sugars owe the property of readily reducing alkaline solu- tions of the oxides of metals like copper, bismuth and mercury; they also possess the property of reducing ammoniacal silver solu- tions with the separation of metallic silver. Upon this property of reduction the most widely used tests for sugars are based. When whitish-blue cupric hydroxide in suspension in an alkaline liquid is heated it is converted into insoluble black cupric oxide, but if a reducing agent like certain sugars be present the cupric hydroxide is reduced to insoluble yellow cuprous hydroxide, which in turn, on further heating, may be converted into brownish-red or red cuprous oxide. These changes are indicated as follows : OH / Cu s^Cu = 0 + H20. ^v Cupric oxide ^tt (black). Cupric hydroxide (whitish-blue). OH / Cu \ OH 2Cu-OH + H20 = 0. / Cu \ OH f^TX Cuprous hydroxide (yellow). Cu-OH L- CARBOHYDRATES. 2J Cu X0 + H20. OH / Cu Cuprous hydroxide Cuprous oxide (yellow). (brownish-red). The chemical equations here discussed are exemplified in Trom- mer's and Fehling's tests. (a) Trommer's Test. — To 5 c.c. of sugar solution in a test- tube add one-half its volume of KOH or NaOH. Mix thor- oughly and add, drop by drop, a very dilute solution of cupric sulphate. Continue the addition until there is a slight permanent precipitate of cupric hydroxide and in consequence the solution is slightly turbid. Heat, and the cupric hydroxide is reduced to yellow cuprous hydroxide or to brownish-red cuprous oxide. If the solution of cupric sulphate used is too strong a small brownish- red precipitate produced in a weak sugar solution may be entirely masked. On the other hand, particularly in testing for sugar in the urine, if too little cupric sulphate is used a light-colored pre- cipitate formed by uric acid and purine bases may obscure the brownish-red precipitate of cuprous oxide. The action of KOH or NaOH in the presence of an excess of sugar and insufficient copper will produce a brownish color. Phosphates of the alkaline earths may also be precipitated in the alkaline solution and be mistaken for cuprous hydroxide. Trommer's test is not very satis- factory. (b) Fehling's Test. — To about 1 c.c. of Fehling's solution1 in a test-tube add about 4 c.c. of water, and boil. This is done to determine whether the solution will of itself cause the forma- tion of a precipitate of brownish-red cuprous oxide. If such a precipitate forms, the Fehling's solution must not be used. Add sugar solution to the warm Fehling's solution a few drops at a time and heat the mixture after each addition. The production of yellow cuprous hydroxide or brownish-red cuprous 1 Fehling's solution is composed of two definite solutions— a cupric sulphate solution and an alkaline tartrate solution, which may be prepared as follows : Cupric sulphate solution = 34.65 grams of cupric sulphate dissolved in water and made up to 500 c.c. Alkaline tartrate solution = 125 grams of potassium hydroxide and 173 grams ■of Rochelle salt dissolved in water and made up to 500 c.c. These solutions should be preserved separately in rubber-stoppered bottles and mixed in equal volumes when needed for use. This is done to prevent deterioration. 28 PHYSIOLOGICAL CHEMISTRY. oxide indicates that reduction has taken place. The yellow pre- cipitate is more likely to occur if the sugar solution is added rap- idly and in large amount, whereas with a less rapid addition of smaller amounts of sugar solution the brownish-red precipitate is generally formed. This is a much more satisfactory test than Trommer's, but even this test is not entirely reliable when used to detect sugar in the urine. Such bodies as conjugate glycuronates, uric acid, nucieo- protein and homogentisic acid when present in sufficient amount may produce a result similar to that produced by sugar. Phos- phates of the alkaline earths may be- precipitated by the alkali of the Fehling's solution and in appearance may be mistaken for cuprous hydroxide. Cupric hydroxide may also be reduced to cuprous oxide and this in turn be dissolved by creatinine, a normal urinary constituent. This will give the urine under examination a greenish tinge and may obscure the sugar reaction even when a considerable amount of sugar is present. (c) Benedict's Modifications of Fehling's Test. — First Modifi- cation.— To 2 c.c. of Benedict's solution1 in a test-tube add 6 c.c. of distilled water and 7-9 drops (not more) of the solution under examination. Boil the mixture vigorously for about 15-30 sec- onds and permit it to cool to room temperature spontaneously. (If desired this process may be repeated, although it is ordinarily un- necessary.) If sugar is present in the solution a precipitate will form which is often bluish-green or green at first, especially if the percentage of sugar is low, and which usually becomes yellowish upon standing. If the sugar present exceeds 0.06 per cent this precipitate generally forms at or below the boiling point, whereas if less than 0.06 per cent of sugar is present the precipitate forms more slowly and generally only after the solution has cooled. Benedict claims that, whereas the original Fehling test will not serve to detect sugar when present in a concentration of less than 0.1 per cent that the above modification will serve to detect sugar when present in as small quantity as 0.015-0.02 per cent. 1 Benedict's modified Fehling solution consists of two definite solutions — a cupric sulphate solution and an alkaline tartrate solution, which may be pre- pared as follows : Cupric sulphate solution = 34.65 grams of cupric sulphate dissolved in water and made up to 500 c.c. Alkaline tartrate solution = 100 grams of anhydrous sodium carbonate and 173 grams of Rochelle salt dissolved in water and made up to 500 c.c. These solutions should be preserved separately in rubber-stoppered bottles and mixed in equal volumes when needed for use. This is done to prevent deterioration. CARBOHYDRATES. 29 The modified Fehling solution used in the above test differs from the original Fehling solution in that 100 grams of sodium car- bonate is substituted for the 125 grams of potassium hydroxide ordinarily used, thus forming a Fehling solution which is consid- erably less alkaline than the original. This alteration in the com- position of the Fehling solution is of advantage in the detection of sugar in the urine inasmuch as the strong alkalinity of the ordinary Fehling' solution has a tendency, when the reagent is boiled with a urine containing a small amount of dextrose, to decompose sufficient of the sugar to render the detection of the remaining portion exceedingly difficult by the usual technique. Benedict claims that for this reason the use of his modified solu- tion permits the detection of much smaller amounts of sugar than does the use of the ordinary Fehling solution. He has further modified his solution for use in the quantitative determination of sugar (see Chapter XXII). Second Modification} — Very recently Benedict has further modi- fied his solution and has succeeded in obtaining one which does not deteriorate upon long standing.2 The following is the procedure for the detection of dextrose in solution : To five cubic centimeters of the reagent in a test-tube add eight (not more) drops of the solution under examination. Boil the mixture vigorously for from one to two minutes and then allow the fluid to cool spontaneously. In the presence of dextrose the entire body of the solution zvill be filled with a precipitate, which may be red, yellow or green in color, depending upon the amount of sugar present. If no dextrose is present, the solution will remain perfectly clear. (If urine is being tested, it may show a very faint turbidity, due to precipitated urates.) Even very small quantities of dextrose (o. 1 per cent) 1 Private communication from Dr. S. R. Benedict. 2 Benedict's new solution has the following composition : Cupric sulphate 17.3 grams. Sodium citrate 173.0 grams. Sodium carbonate (anhydrous) 100.0 grams. Distilled water to make 1 liter. With the aid of heat dissolve the sodium citrate and carbonate in about 600 c.c. of water. Pour (through a folded filter paper if necessary) into a glass gradu- ate and make up to 850 c.c. Dissolve the cupric sulphate in about 100 c.c. of water and make up to 150 c.c. Pour the carbonate-citrate solution into a large beaker or casserole and add the cupric sulphate solution slowly, with constant stirring. The mixed solution is ready for use and does not deteriorate upon long standing:. 30 PHYSIOLOGICAL CHEMISTRY. yield precipitates of surprising bulk with this reagent, and the posi- tive reaction for dextrose is the filling of the entire body of the solution with a precipitate, so that the solution becomes opaque. Since amount rather than color of the precipitate is made the basis of this test, it may be applied, even for the detection of small quan- tities of dextrose, as readily in artificial light as in daylight. (d) Boettger's Test. — To 5 c.c. of sugar solution in a test-tube add 1 c.c. of KOH or NaOH and a very small amount of bismuth subnitrate, and boil. The solution will gradually darken and finally assume a black color due to reduced bismuth. If the test is made on urine containing albumin this must be removed, by boiling and filtering, before applying the test, since with albumin a similar change of color is produced (bismuth sulphide). (e) Nylander's Test (Almen's Test). — To 5 c.c. of sugar solu- tion in a test-tube add one-tenth its volume of Nylander's reagent1 and heat for five minutes in a boiling water-bath.2 The solution will darken if reducing sugar is present and upon standing for a few moments a black color will appear. This color is due to the precipitation of bismuth. If the test is made on urine containing albumin this must be removed, by boiling and filtering, before applying the test, since with albumin a similar change of color is produced. Dextrose when present to the extent of 0.08 per cent, may be detected by this reaction. It is claimed by Bechold that Nylander's and Boettger's tests give a negative reaction with solutions containing sugar when mercuric chloride or chloroform is present. Other observers have failed to verify the inhibitory action of mercuric chloride and have shown that the inhibitory in- fluence of chloroform may be overcome by raising the tempera- ture of the urine to the boiling-point for a period of five minutes previous to making the test. Urines rich in indican, uroerythrin or hcemaio porphyrin, as well as urines excreted after the inges- tion of large amounts of certain medicinal substances, may give a darkening of Nylander's reagent similar to that of a true sugar reaction. According to Rustin and Otto the addition of PtCl4 increases the delicacy of Nylander's reaction. They claim that this pro- ' Nylander's reagent is prepared by digesting 2 grams of bismuth subnitrate and a grams of Rochelle salt in 100 c.c. of a 10 per cent potassium hydroxide solution. The reagent is then cooled and filtered. 2 Hammarsten suggests that the mixture should be boiled 2-5 minutes (accord- ing to the sugar content) over a free flame and the tube then permitted to stand K minutes before drawing conclusions. CARBOHYDRATES. 31 cedure causes the sugar to be converted quantitatively. No quan- titative method has yet been devised, however, based upon this principle. A positive Nylander or Boettger test is probably due to the fol- FlG. 2. lowing reactions : (a) Bi(OH)2NO, + KOH = Bi(OH)8 + KN03. (b) 2Bi(OH)3 - 30 = Bi2 + 3H20. 10. Fermentation Test. — " Rub up " in a mortar about 20 c.c. of the sugar solution with a small piece of compressed yeast. Transfer the mixture to a saccharometer ( shown in Fig. 2) and stand it aside in a warm place for about twelve hours. If the sugar is fermentable, alcoholic fermen- tation will occur and carbon dioxide will collect as a gas in the upper portion of the tube. On the completion of fermentation introduce a little potassium hydroxide solu- tion into the graduated portion by means of a bent pipette, place the thumb tightly over the opening in the apparatus and in- vert the saccharometer. Explain the result. 11. Barfoed's Test. — Place .about 5 c.c. of Barfoed's solution1 in a test-tube and heat to boiling. Add dextrose solution slowly, a few drops at a time, heating after each addition. Reduction is indicated by the formation of a red precipitate. If the precipitate does not form upon continued boiling allow the tube to stand a few minutes and examine. Sodium chloride interferes with the reaction (Welker). Barfoed's test is not a specific test for dextrose as is frequently stated, but simply serves to detect monosaccharides. Disac- charides will also respond to the test, according to Hinkel and Sherman, if the sugar solution is boiled sufficiently long, in contact with the reagent, to hydrolyze the disaccharide through the action of the acetic acid present in the Barfoed's solution. 12. Formation of Caramel. — Gently heat a small amount of 1 Barfoed's solution is prepared as follows : Dissolve 4.5 grams of neutral, crystallized cupric acetate in 100 c.c. of water and add 0.12 c.c. of 50 per cent acetic acid. Einhorx Saccharometer. 32 PHYSIOLOGICAL CHEMISTRY. pulverized dextrose in a test-tube. After the sugar has melted and turned brown, allow the tube to cool, add water and warm. The coloring' matter produced is known as caramel. 13. Demonstration of Optical Activity. — A demonstration of the use of the polariscope, by the instructor, each student being, required to take readings and compute the " specific rotation." Use of the Polariscope. For a detailed description of the different forms of polariscopes, the method of manipulation and the principles involved the student is referred to any standard text-book of physics. A brief descrip- tion follows : An ordinary ray of light vibrates in every direction. If such a ray is caused to pass through a " polarizing " Nicol prism it is resolved into two rays, one of which vibrates in every direction as before and a second ray which vibrates in one plane only. This latter ray is said to be polarized. Many organic sub- stances (sugars, proteins, etc.) have the power of twisting or rotat- ing this plane of polarized light, the extent to which the plane is rotated depending upon the number of molecules which the polar- ized light passes. Substances which possess this power are said to be " optically active." The specific rotation of a substance is the rotation expressed in degrees which is afforded by one gram of substance dissolved in 1 c.c. of water in a tube one decimeter in length. The specific rotation, (a)v, may be calculated by means of the following formula, in which d = sodium light. a == observed rotation in degrees. p = grams of substance dissolved in 1 c.c. of liquid. / = length of the tube in decimeters. If the specific rotation has been determined and it is desired to ascertain the per cent of the substance in solution, this may be obtained by the use of the following formula, P = («V The value of p multiplied by 100 will be the percentage of the substance in solution. CARBOHYDKATKS. 33 An instrument by means of which the extent of the rotation may be determined is called a polariscope or polarimeter. Such an in- strument designed especially for the examination of sugar solutions is termed a saccharimeter or polarizing saccharimeter. The form of Fig. 3. One Form of Laurent Polariscope. B, Microscope for reading the scale ; C, a vernier ; E, position of the analyzing Nicol prism ; H, polarizing Nicol prism in the tube below this point. polariscope shown in Fig. 3, above, consists essentially of a long barrel provided with a Nicol prism at either end (Fig. 4, below). The solution under examination is contained in a tube which is placed between these two prisms. At the front end of the instru- ment is an adjusting eye-piece for focusing and a large recording Fig. 4. HO ^> Diagrammatic Representation of the Course of the Light through the Laurent Polariscope. (The direction is reversed from that of Fig. 3, above.) a, Bichromate plate to purify the light ; b, the polarizing Nicol prism ; c, a thin quartz plate covering one-half the field and essential in producing a second polarized plane ; d, tube to contain the liquid under examination ; e, the analyzing Nicol prism ; f and g, ocular lenses. disc which registers in degrees and fractions of a degree. The light is admitted into the far end of the instrument and is polarizad by passing through a Nicol prism. This polarized ray then traverses the column of liquid within the tube mentioned above and if the sub- 4 34 PHYSIOLOGICAL CHEMISTRY. stance is optically active the plane of the polarized ray is rotated to the right or left. Bodies rotating the ray to the right are called dextro-rotatory and those rotating it to the left Icevo-rotatory. Within the apparatus is a disc which is so arranged as to be without lines and uniformly light at zero. Upon placing the opti- Fig. 5. Polariscope (Schmidt and Hansch Model). cally active substance in position, however, the plane of polarized light is rotated or turned and it is necessary to rotate the disc through a certain number of degrees in order to secure the normal conditions, i. e., " without lines and uniformly light." The differ- ence between this reading and the zero is a or the observed rotation in degrees. Polarizing saccharimeters are also constructed by which the per- centage of sugar in solution is determined by making an observa- tion and multiplying the value of each division on a horizontal slid- ing scale by the value of the division expressed in terms of dex- trose. This factor may vary according to the instrument. CARBOHYDRATES. 35 CH2OH LJEVULOSE, (CHOH)3. CO CHoOH As already stated, lsevulose, sometimes called fructose or fruit sugar, occurs widely disseminated throughout the plant kingdom in company with dextrose. Its reducing power is somewhat weaker than that of dextrose. Lsevulose does not ordinarily occur in the urine in diabetes mellitus, but has been found in exceptional cases. With phenylhydrazine it forms the same osazone as dextrose. With methylphenylhydrazine, lsevulose forms a characteristic methyl- phenyllsevulosazone. (For a further discussion of lsevulose see the section on Hexoses, p. 22.) Experiments on L^vulose. I— ii. Repeat these experiments as given under Dextrose, pages 23-3I- 12. Seliwanoff's Reaction. — To 5 c.c. of Seliwanoff's reagent1 in a test-tube add a few drops of a lsevulose solution and heat the mixture to boiling. A positive reaction is indicated by the produc- tion of a red color and the separation of a red precipitate. The latter may be dissolved in alcohol to which it will impart a striking red color. If the boiling be prolonged a similar reaction may be obtained with solutions of dextrose or maltose. 13. Borchardt's Reaction. — To about 5 c.c. of a solution of lsevulose in a test-tube add an equal volume of 25 per cent hydro- chloric acid and a few crystals of resorcin. Heat to boiling and after the production of a red color, cool the tube under running water and transfer to an evaporating dish or beaker. Make the mixture slightly alkaline with solid potassium hydroxide, return it to a test tube, add 2-3 c.c. of acetic ether and shake the tube vig- orously. In the presence of lsevulose, the acetic ether is colored yellow. (For further discussion of the test see Chapter XIX.) 14. Formation of Methylphenyllaevulosazone. — To a solution 1 Seliwanoff's reagent may be prepared by dissolving 0.05 gram of resorcin in 100 c.c. of dilute (1:2) hydrochloric acid. 36 PHYSIOLOGICAL CHEMISTRY. of 1.8 gram of lsevulose in 10 c.c. of water add 4 grams1 of methyl- phenylhydrazine and enough alcohol to clarify the solution. Intro- duce 4 c.c. of 50 per cent acetic acid and heat the mixture for 5-10 minutes on a boiling water-bath.2 On standing 15 minutes at room temperature, crystallization begins and is complete in two hours. By scratching the sides of the flask or by inoculation, the solution quickly congeals to form a thick paste of reddish yellow silky needles. These are the crystals of methylphenyllcevulosazone. They may be recrystallized from hot 95 per cent alcohol and melt at 153° C CH2OH GALACTOSE, (CHOH)4. CHO Galactose occurs with dextrose as one of the products of the hydrolysis of lactose. It is dextro-rotatory, forms an osazone with phenylhydrazine and ferments slowly with yeast. Upon oxida- tion with nitric acid galactose yields mucic acid, thus differentiat- ing this monosaccharide from dextrose and lsevulose. Lactose also yields mucic acid under these conditions. The mucic acid test may be used in urine examination to differentiate lactose and galactose from other reducing sugars. Experiments on Galactose. 1. Tollens' Reaction. — To equal volumes of galactose solu- tion and hydrochloric acid (sp. gr. 1.09) add a little phloroglucin, and heat the mixture on a boiling water-bath. Galactose, pentose and glycuronic acid will be indicated by the appearance of a red color. Galactose may be differentiated from the two latter sub- stances in that its solutions exhibit no absorption bands upon spec- Iroscopical examinations. 2. Mucic Acid Test. — Treat 100 c.c. of the solution containing galactose with 20 c.c. of concentrated nitric acid (sp. gr. 1.4) and evaporate the mixture in a broad, shallow glass vessel on a boiling water-bath until the volume of the mixture has been reduced to about 20 c.c. At this point the fluid should be clear, and a .fine white precipitate of mucic acid should form. If the percentage of galactose present is low it may be necessary to cool the solution 1 3.66 grams if absolutely pure. 2 Longer heating is to be avoided. CARBOHYDRATES. 37 and permit it to stand for some time before the precipitate will form. It is impossible to differentiate between galactose and lactose by this test, but the reaction serves to differentiate these two sugars from all other reducing sugars. Differentiate lactose from galac- tose by means of Barfoed's test (p. 31). 3. Phenylhydrazine Reaction. — Make the test according to directions given under Dextrose, 3 or 4, pages 24 and 25. Pentoses, C5H10O5. In plants and more particularly in certain gums, very complex carbohydrates, called pentosans, occur. These pentosans through hydrolysis by acids may be transformed into pentoses. Pentoses do not ordinarily occur in the animal organism, but have been found in the urine of morphine habitues and others, their occur- rence sometimes being a persistent condition without known cause. They are non- fermentable, have strong reducing power and form osazones with phenylhydrazine. Pentoses are an important constitu- ent of the dietary of herbivorous animals. Glycogen is said to be formed after the ingestion of these sugars containing five oxygen atoms. This, however, has not been conclusively proven. On distillation with strong hydrochloric acid pentoses and pentosans yield furfurol, which can be detected by its characteristic red reac- tion with aniline-acetate paper. CH2OH ARABINOSE, (CHOH)3. CHO Arabinose is one of the most important of the pentoses. The /-arabinose may be obtained from gum arabic, plum or cherry gum by boiling for several hours with 1-2 per cent sulphuric acid. This pentose is dextrorotatory, forms an osazone and has reducing power. The i-arabinose has been isolated from the urine and yields an osazone which melts at 166-1680 C. Experiments on Arabinose. 1. Tollens' Reaction. — To equal volumes of arabinose solu- tion and hydrochloric acid (sp. gr. 1.09) add a little phloroglucin and heat the mixture on a boiling water-bath. Galactose, pentose or glycuronic acid will lie indicated by the appearance of a red 38 PHYSIOLOGICAL CHEMISTRY. color. To differentiate between these bodies make a spectroscopic examination and look for the absorption band between D and E given by pentoses and glycuronic acid. Differentiate between the two latter bodies by the melting-points of their osazones. Compare the reaction with that obtained with galactose (page 36) . 2. Orcin Test. — Repeat 1, using orcin instead of phloroglucin. A succession of colors from red through reddish-blue to green is produced. A green precipitate is formed which is soluble in amyl alcohol and has absorption bands between C and D. 3. Phenylhydrazine Reaction. — Make this test on the arabinose solution according to directions given under Dextrose, 3 or 4, pages 24 and 25. CH2OH xylose, (CHOH)3. I CHO Xylose, or wood sugar, is obtained by boiling wood gums with dilute acids as explained under Arabinose, page 37. It is dextro- rotatory and forms an osazone. Experiments on Xylose. 1-3. Same as for arabinose (see page 37). RHAMNOSE, C6H1205. Rhamnose or methyl-pentose is an example of a true carbohydrate which does not have the H and O atoms present in the proportion to form water. Its formula is C0H12O5. It has been found that rhamnose when ingested by rabbits or hens has a positive influence upon the formation of glycogen in those organisms. DISACCHARIDES, C12H22On. The disaccharides as a class may be divided into two rather dis- tinct groups. The first group would include those disaccharides which are found in nature as such, e. g., sucrose and lactose and the second group would include those disaccharides formed in the hydrolysis of more complex carbohydrates, e. g., maltose, and iso-maltose. CARBOHYDRATES. 39 The disaccharides have the general formula C]2H22On, to which, in the process of hydrolysis, a molecule of water is added causing the single disaccharide molecule to split into two monosaccharide (hexose) molecules. The products of the hydrolysis of the more common disaccharides are as follows : Maltose — dextrose -J- dextrose. Lactose = dextrose -\- galactose. Sucrose = dextrose -\- lsevulose. All of the more common disaccharides except sucrose have the power of reducing certain metallic oxides in alkaline solution, notably those of copper and bismuth. This reducing power is due to the presence of the aldehyde group ( — CHO) in the sugar molecule. MALTOSE, CjaHaaOn. Maltose or malt sugar is formed in the hydrolysis of starch through the action of an enzyme, vegetable amylase (diastase) , con- tained in sprouting barley or malt. Certain enzymes in the saliva and in the pancreatic juice may also cause a similar hydrolysis. Maltose is also an intermediate product of the action of dilute mineral acids upon starch. It is strongly dextro-rotatory, reduces metallic oxides in alkaline solution and is fermentable by yeast after being inverted (see Polysaccharides, page 43) by the enzyme maltase of the yeast. In common with the other disaccharides, maltose may be hydrolyzed with the formation of two molecules of monosac- charide. In this instance the products are two molecules of dex- trose. With phenylhydrazine maltose forms an osazone, maltosa- zone. The following formula represents the probable structure of maltose : CH2OH CHO CHOH CHOH 4q physiological chemistry. Experiments on Maltose. i-ii. Repeat these experiments as given under Dextrose, pages 23-3I- ISO-MALTOSE, C^H^On. Iso-maltose, an isomeric form of maltose, is formed, along with maltose, by the action of diastase upon starch paste, and also by the action of hydrochloric acid upon dextrose. It also occurs with maltose as one of the products of salivary digestion. It is dextro- rotatory and with phenylhydrazine gives an osazone which is char- acteristic. Iso-maltose is very soluble and reduces the oxides of bismuth and copper in alkaline solution. Pure iso-maltose is prob- ably only slightly fermentable. LACTOSE, C^H^On. Lactose or milk sugar occurs ordinarily only in milk, but has often been found in the urine of women during pregnancy and lactation. It may also occur in the urine of normal persons after the ingestion of unusually large amounts of lactose in the food. It has a strong reducing power, is dextro-rotatory and forms an osazone with phenylhydrazine. Upon hydrolysis lactose yields one molecule of dextrose and one molecule of galactose. In the souring of milk the bacterium lactis and certain other micro-organisms bring about lactic acid fermentation by transform- ing the lactose of the milk into lactic acid, H OH H - C - C - COOH, I I H H and alcohol. This same reaction may occur in the alimentary canal as the result of the action of putrefactive bacteria. In the prepara- tion of kephyr and koumyss the lactose of the milk undergoes alco- holic fermentation, through the action of ferments other than yeast, and at the same time lactic acid is produced. Lactose and galactose yield mucic acid on oxidation with nitric acid. This fact is made use of in urine analysis to facilitate the differentiation of these sugars from other reducing sugars. Lactose is not fermentable by pure yeast. carbohydrates. 41 Experiments on Lactose. i— i i. Repeat these experiments as given under Dextrose, pages 23-31. 12. Mucic Acid Test. — Treat 100 c.c. of the solution containing lactose with 20 c.c. of concentrated nitric acid (sp. gr. 1.4) and evaporate the mixture in a broad, shallow, glass vessel on a boiling water-bath, until the volume of the mixture has been reduced to about 20 c.c. At this point the fluid should be clear, and a fine white precipitate of mucic acid should form. If the percentage of lactose present is low it may be necessary to cool the solution and permit it to stand for some time before the precipitate will appear. It is impossible to differentiate between lactose and galactose by this test, but the reaction serves to differentiate these two sugars from all other reducing sugars. Differentiate lactose from galactose by means of Barfoed's test, page 31. SUCROSE, CioHooOn. Sucrose, also called saccharose or cane sugar, is one of the most important of the sugars and occurs very extensively distributed in plants, particularly in the sugar cane, sugar beet, sugar millet and in certain palms and maples. Sucrose is dextro-rotatory and upon hydrolysis, as before men- tioned, the molecule of sucrose takes on a molecule of water and breaks down into two molecules of monosaccharide. The mono- saccharides formed in this instance are dextrose and lsevulose. This is the reaction : G12R22Oxl + H20 = C6H1206 -f- C6H1206. Sucrose. Dextrose. Lsevulose. This process is called inversion and may be produced by bacteria, enzymes and certain weak acids. After this inversion the previously strongly dextro-rotatory solution becomes laevo-rotatory. This is due to the fact that the lsevulose molecule is more strongly lawo- rotatory than the dextrose molecule is dextro-rotatory. The product of this inversion is called invert sugar. Sucrose does not reduce metallic oxides in alkaline solution and forms no osazone with phenylhydrazine. It is not fermentable directly by yeast, but must first be inverted by the enzyme sitcrase (invertase or inverting contained in the yeast. The probable struc- ture of sucrose may be represented by the following formula. 42 PHYSIOLOGICAL CHEMISTRY. Note the absence of any" true sugar group or free ketone or alde- hyde group. CH2OH CHOH CHO -0 CH2OH H Sucrose. Fig. 6. Experiments on Sucrose. i-ii. Repeat these experiments according to the directions given under Dextrose, pages 23-31. 12. Inversion of Sucrose. — To 25 c.c. of sucrose solution in a beaker add 5 drops of concentrated HC1 and boil one minute. Cool the solution, render alkaline with solid KOH and upon the resulting fluid repeat experiments 3 (or 4) and 9 as given under Dextrose, pages 24-26. Explain the results. 13. Production of Alcohol by Fermentation. — Prepare a strong (10-20 per cent) solution of sucrose, add a small amount of egg albumin or commercial peptone and introduce the mixture into a bottle of appropriate size. Add yeast, and b)^ means of a bent tube inserted through a stopper into the neck of the bottle, con- duct the escaping gas into water. As fermentation proceeds readily in a warm place the escaping gas may be collected in a eudiometer tube and examined. When the activity of the yeast has prac- tically ceased, filter the contents of the bottle into a flask and distil the mixture. Catch the first portion of the distillate separately and test for alco- hol by one of the following reactions : (a) Iodoform Test. — Render 2-3 c.c. of the distillate alkaline with potassium hydroxide solution and add a few drops of iodine Iodoform. (Autenrietk.) CARBOHYDRATES. 43 solution. Heat gently and note the formation of iodoform crystals. Examine these crystals under the microscope and compare them with those in Fig. 6, p. 42. (b) Aldehyde Test.— Place 5 c.c. of the distillate in a test-tube, add a few drops of potassium dichromate solution, K2Cr207, and render it acid with dilute sulphuric acid. Boil the acid solution and note the odor of aldehyde. TRISACCHARIDES, C1SH32016. RAFFINOSE. This trisaccharide, also called melitose or melitriose, occurs in cotton seed, Australian manna and in the molasses from the prepara- tion of beet sugar. It is dextro-rotatory, does not reduce Fehling's solution and is only partially fermentable by yeast. Raffinose may be hydrolyzed by weak acids the same as the poly- saccharides are hydrolyzed, the products being lsevulose and meli- biose; further hydrolysis of the melibiose yields dextrose and galactose. POLYSACCHARIDES, (C6H10O5)x. In general the polysaccharides are amorphous bodies, a few, how- ever, are crystallizable. Through the action of certain enzymes or weak acids the polysaccharides may be hydrolyzed with the for- mation of monosaccharides. As a class the polysaccharides are quite insoluble and are non-fermentable until inverted. By inversion is meant the hydrolysis of disaccharide or polysaccharide sugars to form monosaccharides, as indicated in the following equations : (a) C12H22On + H2O = 2(CfiH12O0). (b) CflH10OB + H2O = C6H"12Oe. STARCH, (C6H1005)x. Starch is widely distributed throughout the vegetable kingdom, occurring in grains, fruits and tubers. It occurs in granular form, the microscopical appearance being typical for each individual starch. The granules, which differ in size according to the source, are composed of alternating concentric rings of granulose and cel- lulose. Ordinary starch is insoluble in cold water, but if boiled with water the cell walls are ruptured and starch paste results. In general starch gives a blue color with iodine. 44 PHYSIOLOGICAL CHEMISTRY. Starch is acted upon by amylases, e. g., salivary amylase (ptyalin) and pancreatic amylase (amylopsin) , with the formation of soluble starch, erythro-dextrin, achroo-dextrins , maltose, iso-maltose and dextrose (see Salivary Digestion, page 54). Maltose is the principal end-product of this enzyme action. Upon boiling a starch solution with a dilute mineral acid a series of similar bodies is formed, but under these conditions dextrose is the principal end-product. Experiments on Starch. 1. Preparation of Potato Starch. — Pare a raw potato, com- minute it upon a fine grater, mix with water, and "whip up" the pulped material vigorously before straining it through cheese cloth or gauze to remove the coarse particles. The starch rapidly settles to the bottom and can be washed by repeated decantation. Allow the compact mass of starch to drain thoroughly and spread it out on a watch glass to dry in the air. If so desired this preparation may be used in the experiments which follow. 2. Microscopical Examination. — Examine microscopically the granules of the various starches submitted and compare them with those shown in Figs. 7-17, page 45. The suspension of the granules in a drop of water will facilitate the microscopical examination. 3. Solubility. — Try the solubility of one form of starch in each of the ordinary solvents (see page 23). If uncertain regarding the solubility in any reagent, filter and test the filtrate with iodine solu- tion as given under 5 below. The production of a blue color would indicate that the starch had been dissolved by the solvent. 4. Iodine Test. — Place a few granules of starch in one of the depressions of a porcelain test-tablet and treat with a drop of a dilute solution of iodine in potassium iodide. The granules are colored blue due to the formation of so-called iodide of starch. The cellulose of the granule is not stained as may be seen by examining microscopically. 5. Iodine Test on Starch Paste.1 — Repeat the iodine test using the starch paste. Place 2-3 c.c. of starch paste2 in a test-tube, add 1 Preparation of Starch Paste. — Grind 2 grams of starch powder in a motar with a small amount of cold water. Bring 200 c.c. of water to the boiling-point and add the starch mixture from the mortar with continuous stirring. Bring again to the boiling-point and allow it to cool. This makes an approximate T per cent starch paste which is a very satisfactory strength for general use. 2 For this particular test a starch paste of very satisfactory strength may be made by mixing 1 c.c. of a 1 per cent starch paste with 100 c.c. of water. Fig. 7 CARBOHYDRATES. Fig. 8. 45 Pea. Wheat. Starch Granules from Various Sources. (Leffman and Beam.) 46 PHYSIOLOGICAL CHEMISTRY. a drop of the dilute iodine solution and observe the production of a blue color. Heat the tube and note the disappearance of the color. It reappears on cooling. In similar tests note the influence of alcohol and of alkali upon the so-called iodide of starch. The composition of the iodide of starch is not definitely known. 6. Fehling's Test. — On starch paste (see page 27). 7. Hydrolysis of Starch. — Place about 25 c.c. of starch paste in a small beaker, add 10 drops of concentrated HC1, and boil. By- means of a small pipette, at the end of each minute, remove a drop of the solution to the test-tablet and make the regular iodine test. As the testing proceeds the blue color should gradually fade and finally disappear. At this point, after cooling and neutralizing with solid KOH, Fehling's test (see page 27) should give a positive result due to the formation of a reducing sugar from the starch. Make the phenylhydrazine test upon some of the hydrolyzed starch. What sugar has been formed? 8. Influence of Tannic Acid. — Add an excess of tannic acid solution to a small amount of starch paste in a test-tube. The liquid will become strongly opaque and ordinarily a yellowish-white pre- cipitate is produced. Compare this result with the result of the similar experiment on dextrin (page 49). 9. Diffusibility of Starch Paste. — Test the diffusibility of starch paste through animal membrane or parchment paper, making a dialyzer like one of the models shown in Fig. 1, page 25. INULIN, (C6H10O5)x. Inulin is a polysaccharide which may be obtained as a white, odorless, tasteless powder from the tubers of the artichoke, elecam- pane or dahlia. It has also been prepared from the roots of chicory, dandelion and burdock. It is very slightly soluble in cold water and quite easily soluble in hot water. In cold alcohol of 60 per cent or over it is practically insoluble. Inulin gives a negative reac- tion with iodine solution. The " yellow " color reaction with iodine mentioned in many books is doubtless merely the normal color of the iodine solution. It is very difficult to prepare inulin which does not reduce Fehling's solution slightly. This reducing power may be due to an impurity. Practically all commercial preparations of inulin possess considerable reducing power. Inulin is lsevo-rotatory and upon hydrolysis by acids or by the CARBOHYDRATES. 47 enzyme inulase it yields the monosaccharide l^evulose which readily reduces Fehling's solution. The ordinary amylolytic enzymes occur- ring in the animal body do not digest inulin. Experiments on Inulin. 1. Solubility. — Try the solubility of inulin powder in each of the ordinary solvents. If uncertain regarding the solubility in any reagent, filter and neutralize the nitrate if it is alkaline in reaction. Add a drop of concentrated hydrochloric acid to the filtrate and boil it for one minute. Render the solution neutral or slightly alkaline with solid potassium hydroxide and try Fehling's test. What is the significance of a positive Fehling's test in this connection ? 2. Iodine Test. — (a) Place 2-3 c.c. of the inulin solution in a test-tube and add a drop of dilute iodine solution. What do you observe ? (b) Place a small amount of inulin powder in one of the depres- sions of a test-tablet and add a drop of dilute iodine solution. Is the effect any different from that observed above? 3. Molisch's Reaction. — Repeat this test according to directions given under Dextrose, 2, page 23. 4. Fehling's Test. — Make this test on the inulin solution accord- ing to the instructions given under Dextrose, page 27. Is there any reduction?1 5. Hydrolysis of Inulin. — Place 5 c.c. of inulin solution in a test-tube, add a drop of concentrated hydrochloric acid and boil it for one minute. Now cool the solution, neutralize it with con- centrated KOH and test the reducing action of 1 c.c. of the solution upon 1 c.c. of diluted (1:4) Fehling's solution. Explain the result.2 GLYCOGEN, (C6H10O5)x. (For discussion and experiments see Muscular Tissue, Chapter XV.) 1 See the discussion of the properties of inulin, page 46. 2 If the inulin solution gave a positive Fehling test in the last experiment it will be necessary to check the hydrolysis experiment as follows : To 5 c.c. of the inulin solution in a test-tube add one drop of concentrated hydrochloric acid, neutralize with concentrated KOH solution and test the reducing action of i c.c. of the resulting solution upon I c.c. of diluted (1:4) Fehling's solu- tion. This will show the normal reducing power of the inulin solution. In case the inulin was hydrolyzed, the Fehling's test in the hydrolysis experiment should show a more pronounced reduction than that observed in the check experiment. 48 PHYSIOLOGICAL CHEMISTRY. LICHENIN, (C6H10O5)x. Lichenin may be obtained from Cetraria islandica (Iceland moss). It forms a difficultly soluble jelly in cold water and an opalescent solution in hot water. It is optically inactive and gives no color with iodine. Upon hydrolysis with dilute mineral acids lichenin yields dextrins and dextrose. It is said to be most nearly related chemically to starch. Saliva, pancreatic juice, malt diastase and gas- tric juice have no noticeable action on lichenin. DEXTRIN, (C6H1005)x. The dextrins are the bodies formed midway in the stages of the hydrolysis of starch by weak acids or an enzyme. They are amor- phous bodies which are easily soluble in water, acids and alkalis but are insoluble in alcohol or ether. Dextrins are dextro-rotatory and are not fermentable by yeast. The dextrins may be hydrolyzed by dilute acids to form dextrose. With iodine one form of dextrin (erythro-dextrin) gives a red color. Their power to reduce Fehling's solution is questioned. Experiments on Dextrin. i. Solubility. — Test the solubility of pulverized dextrin in the ordinary solvents (see page 23). 2. Iodine Test. — Place a drop of dextrin solution in one of the depressions of the test-tablet and add a drop of a dilute solution of iodine in potassium iodide. A red color results due to the forma- tion of the red iodide of dextrin. If the reaction is not sufficiently pronounced make a stronger solution from pulverized dextrin and repeat the test. The solution should be slightly acid to secure the best results. Make proper tests to show that the red iodide of dextrin is influenced by heat, alkali and alcohol in a similar manner to the blue iodide of starch (see page 46). 3. Fehling's Test. — See if the dextrin solution will reduce Feh- ling's solution. 4. Hydrolysis of Dextrin. — Take 25 c.c. of dextrin solution in a small beaker, add 5 drops of dilute hydrochloric acid, and boil. By means of a small pipette, at the end of each minute, remove a drop of the solution to one of the depressions of the test-tablet and CARBOHYDRATES. 49 make the iodine test. The power of the solution to produce a color with iodine should rapidly disappear. When a negative reaction is obtained cool the solution and neutralize it with concentrated potas- sium hydroxide. Try Fehling's test (see page 27). This reaction is now strongly positive, due to the formation of a reducing sugar. Determine the nature of the sugar by means of the phenylhydrazine test (see pages 24 and 25). 5. Influence of Tannic Acid. — Add an excess of tannic acid solution to a small amount of dextrin solution in a test-tube. No precipitate forms. This result differs from the result of the similar experiment upon starch (see Starch, 8, page 46). 6. Diffusibility of Dextrin. — (See Starch, 9, page 46.) 7. Precipitation by Alcohol. — To about 50 c.c. of 95 per cent alcohol in a small beaker add about 10 c.c. of a concentrated dextrin solution. Dextrin is thrown out of solution as a gummy white precipitate. Compare the result with that obtained under Dextrose, 5, page 25. CELLULOSE, (C6H10O5)x. This complex polysaccharide forms a large portion of the cell wall of plants. It is extremely insoluble and its molecule is much more complex than the starch molecule. The best quality of filter paper and the ordinary absorbent cotton are good types of cellulose. Experiments on Cellulose. 1. Solubility. — Test the solubility of cellulose in the ordinary solvents (see page 23). 2. Iodine Test. — Add a drop of dilute iodine solution to a few shreds of cotton on a test-tablet. Cellulose differs from starch and dextrin in giving no color with iodine. 3. Formation of Amyloid.1 — Add 10 c.c. of dilute and 5 c.c. of concentrated H2S04 to some absorbent cotton in a test-tube. When entirely dissolved (without heating) pour one-half of the solution into another test-tube, cool it and dilute with water. Amy- loid forms as a gummy precipitate and gives a brown or blue colora- tion with iodine. After allowing the second portion of the acid solution of cotton to stand about 10 minutes, dilute it with water in a small beaker and boil for 15-30 minutes. Now cool, neutralize with solid KOH and 1 This body derives its name from amylum (starch) and is not to be con- founded with amyloid, the glycoprotein (page 106). 5 5o PHYSIOLOGICAL CHEMISTRY. test with Fehling's solution. Dextrose has been formed from the cellulose by the action of the acid. 4. Schweitzer's Solubility Test. — Place a little absorbent cotton in a test-tube, add Schweitzer's reagent,1 and stir the cellulose with' a glass rod. When completely dissolved- acidify the solution with acetic acid. An amorphous precipitate of cellulose is produced. Schweitzer's reagent is the only solvent for cellulose. REVIEW OF CARBOHYDRATES. In order to facilitate the student's review of the carbohydrates, the preparation of a chart similar to the appended model is recom- MODEL CHART FOR REVIEW PURPOSES. Carbohydrate. "o t/2 0> H 01 a -3 0 V H VI "11 u 0 0 s QJ H *u V 6 s 0 H 01 H "bo a o> fa H V V 0 M 01 H V T3 C rt V H -a o> ,o (A 0 0 rt 0 .2 o> J" a J3 0 0 .3 ■3 « C 0> 0) H "G w .3 > '■5 c: ■£ B <-; the ube vdro "for po st b 1 1 <0 »c 0) s 13 ir> rtj c/j — ^ o ^ o F ^1^3, — ° S l* 3 I* < 2 s O W r- *r ■" xo2o CJ ^ t> CD -TT — ■pq a-a- (* c 3 O O g cc 2 »3 B a; ■<-< to u s u> bos rt Cl B 2 <*> £ Gg to ^s r* , Ri .§ o C ^ TO «- cj — 3 ._ 4-. I- O ^ fi -3 Cj ^ S Pi ^ cr. o ~ ^ ^ c- rt u «« o Cj ^n <-m O c^- C cr« B a-> 5 o u ■tt'O o o „ y-° rt^ V4-, 5 O 2 ^ 3 be c .5 o o z I >fl i " I h (! •^ rt^; .-3 -3 « ^ o ^E-5 - c t3 >>£ S"5 2 5 ^ -3 — ' J. js >- ?3 3 3 o •3 . rt o"e gj ^ OJ - 3 ^" ^ f,-2 tS: u iy v Gj f^rt § 3 O u ?"' «»iB cj "3'" 2 •& &« CO ,+i ^ TO <»1 - E .3 bO ii ~ ct C C 3 O ra ? 2 >> i o 5^ *3 -", (J bO P-l (y. 52 physiological chemistry. "Unknown" Solutions of Carbohydrates. At this point the student will be given several " unknown " solu- tions, each solution containing one or more ot the carbohydrates studied. He will be required to detect, by means of the tests on the preceding pages, each carbohydrate constituent of the several "unknown" solutions and hand in, to the instructor, a written report of his findings, on slips furnished by the laboratory. The scheme given on page 51 may be of use in this connection. CHAPTER III. SALIVARY DIGESTION. The saliva is secreted by three pairs of glands, the submaxillary, sublingual and parotid, reinforced by numerous small glands called buccal glands. The saliva secreted by each pair of glands possesses certain definite characteristics peculiar to itself. For instance, in man, the parotid glands ordinarily secrete a thin, watery fluid, the submaxillary glands secrete a somewhat thicker fluid containing mucin, while the product of the sublingual glands has a more muci- laginous character. The saliva as collected from the mouth is the combined product of all the glands mentioned. The saliva may be induced to flow by many forms of stimuli, such as chemical, mechanical, electrical, thermal and psychical, the nature and amount of the secretion depending, to a limited degree, upon the particular class of stimuli employed as well as upon the character of the individual stimulus. For example, in experiments upon dogs it has been found that the mechanical stimulus afforded by dropping several pebbles into the animal's mouth caused the flow of but one or two drops of saliva, whereas the mechanical stimulus afforded by sand thrown into the mouth induced a copious flow of a thin watery fluid. Again, when ice-water or snow was placed in the animal's mouth no saliva was seen, while an acid or anything pos- sessing a bitter taste, which the dog wished to reject, caused a free flow of the thin saliva. On the other hand, when articles of food were placed in the dog's mouth the animal secreted a thicker saliva having a higher mucin content — a fluid which would lubricate the food and assist in the passage of the bolus through the oesophagus. It was further found that by simply drawing the attention of the animal to any of the substances named above, results were obtained similar to those secured when the substances were actually placed in the animal's mouth. For example, when a pretense was made of throwing sand into the dog's mouth, a watery saliva was secreted, whereas food under the same conditions excited a thicker and more slimy secretion. The exhibition of dry food, in which the dog had no particular interest (dry bread) caused the secretion of a large 53 54 PHYSIOLOGICAL CHEMISTRY. amount of watery saliva, while the presentation of moist fooclr which was eagerly desired by the animal, called forth a much smaller secretion, slimy in character. These experiments show it to be rather difficult to differentiate between the influence of physio- logical and psychical stimuli. The amount of saliva secreted by an adult in 24 hours has been variously placed, as the result of experiment and observation, be- tween 1000 and 1500 c.c, the exact amount depending, among other conditions, upon the character of the food. The saliva ordinarily has a weak, alkaline reaction to litmus, but becomes acid, in some instances, 2-3 hours after a meal or during fasting. The alkalinity is due principally to di-sodium hydrogen phosphate (Na2HP04) and its average alkalinity may be said to be equivalent to 0.08-0.1 per cent sodium carbonate. The saliva is the most dilute of all the digestive secretions, having an average specific gravity of 1.005 and containing only 0.5 per cent of solid matter. Among the solids- are found albumin, globulin, mucin, urea, the enzymes, salivary amylase (ptyalin) and maltase, phosphates and other inorganic constituents. Potassium thiocyanate, KSCN, is also generally present in the saliva. It. has been claimed that this substance is present in greatest amount in the saliva of habitual smokers. The significance of thiocyanate in the saliva is not known ; it probably comes from the ingested thiocyanates and from the breaking down of protein material. The so-called tartar formation on the teeth is composed almost entirely of calcium phosphate with some calcium carbonate, mucin, epithelial cells and organic debris derived from the food. The cal- cium salts are held in solution as acid salts, and are probably pre- cipitated by the ammonia of the breath. The various organic sub- stances just mentioned are carried down in the precipitation of the .calcium salts. The principal enzyme of the saliva is known as salivary amylase or ptyalin. This is an amylolytic enzyme (see p. 3), so-called because it possesses the property of transforming complex carbo- hydrates such as starch and dextrin into simpler bodies. The action of salivary amylase is one of hydrolysis and through this action a series of simpler bodies are formed from the complex starch. The first product of the action of the ptyalin of the saliva upon starch paste is soluble starch (amidulin) and its forma- tion is indicated by the disappearance of the opalescence of the starch solution. This body resembles true starch in giving a SALIVARY DIGESTION. 55 blue color with iodine. Next follows the formation, in succession, of a series of dextrins, called erythro-dextrin, a-achroo-dcxlrin , (3-achroo-dextrin and. y-achroo-dextrin, the erythro-dextrin being formed directly from soluble starch and later being itself trans- formed into a-achroo-dextriu from which in turn are produced /?- achroo-dextrin and y-achroo-dextrin. Accompanying each dextrin a small amount of iso-maltose is formed, the quantity of iso-mal- tose growing gradually larger as the process of transformation pro- gresses. (Erythro-dextrin gives a red color with iodine, the other dextrins give no color.) The next stage is the transformation of the y-achroo-dextrin into iso-maltose and subsequently the transfor- mation of the iso-maltose into maltose, the latter being the princi- pal end-product of the salivary digestion of starch. At this point a small amount of dextrose is formed from the maltose, through the action of the enzyme maltase. Salivary amylase acts in alkaline, neutral or combined acid solu- tions. It will act in the presence of relatively strong combined HC1 (see page 119), whereas a trace (0.003 Per cent to 0.006 per cent) of ordinary free hydrochloric acid will not only prevent the action but will destroy the enzyme. By sufficiently increasing the alkalinity of the saliva to litmus, the action of the salivary amylase is inhibited. It has recently been shown by Cannon, that salivary digestion may proceed for a considerable period after the food reaches the stomach, owing to the slowness with which the con- tents are thoroughly mixed with the acid gastric juice and the conse- quent tardy destruction of the enzyme. Food in the pyloric end of the stomach is soon mixed with the gastric secretion but food in the cardiac end is not mixed with the acid gastric juice for a con- siderable period of time and in this region during that time sali- vary digestion may proceed undisturbed. Maltase, sometimes called glucase, is the second enzyme of the saliva. It is an amylolytic enzyme whose principal function is the splitting of maltose into dextrose. Besides occurring in the saliva it is also present in the pancreatic and intestinal juices. For experi- mental purposes the enzyme is ordinarily prepared from corn. The principles of the " reversibility " of enzyme action were first demonstrated in connection with maltase by Croft Hill. Microscopical examination of the saliva reveals salivary corpus- cles, bacteria, food debris, epithelial cells, mucus and fungi. In certain pathological conditions of the mouth, pus cells and blood cor- puscles may be found in the saliva. 56 PHYSIOLOGICAL CHEMISTRY. Experiments on Saliva. A satisfactory method of obtaining the saliva necessary for the experiments which follow is to chew a small piece of pure paraffin wax, thus stimulating the flow of the secretion, which may be col- lected in a small beaker. Filtered saliva is to be used in every ex- periment except for the microscopical examination. i. Microscopical Examination. — Examine a drop of unfiltered saliva microscopically and compare with Fig. 18 below. 2. Reaction. — Test the reaction to litmus. Fig. 18. ^ :%'• Microscopical Constituents of Saliva. a, Epithelial cells ; b, salivary corpuscles ; c, fat drops ; d, leucocytes ; e, f and gx bacteria ; h, i and k, fission-fungi. 3. Specific Gravity. — Partially fill a urinometer cylinder with saliva, introduce the urinometer, and observe the reading. 4. Test for Mucin. — To a small amount of saliva in a test-tube add 1-2 drops of dilute acetic acid. Mucin is precipitated. 5. Biuret Test.1 — Render a little saliva alkaline with an equal volume of KOH and add a few drops of a very dilute (2-5 drops in a test-tube of. water) cupric sulphate solution. The formation of a purplish-violet color is due to mucin. . 6. Millon's Reaction.2 — Add a few drops of Millon's reagent to a little saliva. A light yellow precipitate formed by the mucin gradually turns red upon being gently heated. 7. Preparation of Mucin. — Pour 25 c.c. of saliva into 100 c.c. of 95 per cent alcohol, stirring constantly. Cover the vessel and allow the precipitate to stand at least 12 hours. Pour off the supernatant liquid, collect the precipitate on a filter and wash it, in The significance of this reaction is pointed out on page 92. The significance of this reaction is pointed out on page 90. SALIVARY DIGESTION. 5/ turn, with alcohol and ether. Finally dry the precipitate, remove it from the paper and make the following tests on the mucin: (a) Test its solubility in the ordinary solvents (see page 23), (b) Millon's reaction, (c) dissolve a small amount in KOH, and try the biuret test on the solution, (d) boil the remainder, with 10-25 c.c. of water to which 5 c.c. of dilute HC1 has been added, until the solution becomes brownish. Cool, render alkaline with solid KOH, and test by Fehling's solution. A reduction should take place. Mucin is what is known as a conjugated protein or glyco- protein (see p. 87) and upon boiling with the acid the carbohydrate group in the molecule has been split off from the protein portion and its presence is indicated by the reduction of Fehling's solution. 8. Inorganic Matter. — Test for chlorides, phosphates, sulphates and calcium. For chlorides, acidify with HN03 and add AgN03. For phosphates, acidify with HN03, heat and add molybdic solu- tion.1 For sulphates, acidify with HC1 and add BaCl2 and warm. For calcium, acidify with acetic acid, CH3COOH, and add ammon- ium oxalate, (NH4)2C204. 9. Viscosity Test. — Place filter papers in two funnels, and to each add an equal quantity of starch paste (5 c.c). Add a few drops of saliva to one lot of paste and an equivalent amount of water to the other. Note the progress of filtration in each case. Why does one solution filter more rapidly than the other? 10. Test for Nitrites. — Add 1-2 drops of dilute H2S04 to a little saliva and thoroughly stir. Now add a few drops of a potas- sium iodide solution and some starch paste. Nitrous acid is formed which liberates iodine, causing the formation of the blue iodide of starch. 11. Thiocyanate Tests. — (a) Ferric Chloride Test, — To a little saliva in a small porcelain crucible, or dish, add a few drops of dilute ferric chloride and acidify slightly with HC1. Red ferric thiocyanate forms. To show that the red coloration is not due to iron phosphate add a drop of HgCl2 when colorless mercuric thio- cyanate forms. (b) Solera's Reaction. — This test depends upon the liberation of iodine through the action of thiocyanate upon iodic acid. Moisten 1 Molybdic solution is prepared as follows, the parts being by weight : 1 part, molybdic acid. 4 parts, ammonium hydroxide (Sp. gr. 0.96). 15 parts, nitric acid (Sp. gr. 1.2). 58 PHYSIOLOGICAL CHEMISTRY. a strip of starch paste-iodic acid test paper1 with a little saliva. If thiocyanate be present the test paper will assume a blue color, due to the liberation of iodine and the subsequent formation of the so-called iodide of starch. 12. Digestion of Starch Paste. — To 25 c.c. of starch paste in a small beaker, add 5 drops of saliva and stir thoroughly. At in- tervals of a minute remove a drop of the solution to one of the de- pressions in a test-tablet and test by the iodine test. If the blue color with iodine still forms after 5 minutes, add another 5 drops of saliva. The opalescence of the starch solution should soon dis- appear, indicating the formation of soluble starch which gives a blue color with iodine. This body should soon be transformed into erythro-dextrin which gives a red color with iodine and this in turn should pass into achroo-dextrin which gives no color with iodine. This is called the achromic point. When this point is reached test by Fehling's test to show the production of a reducing body. A positive Fehling's test may be obtained while the solution still reacts red with iodine inasmuch as some iso-maltose is formed from the soluble starch coincidently with the formation of the erythro-dextrin. How long did it take for a complete transforma- tion of the starch? 13. Digestion of Dry Starch. — In a test-tube shake up a small amount of dry starch with a little water. Add a few drops of saliva, mix well and allow to stand. After 10-20 minutes filter and test the filtrate by Fehling's test. What is the result and why ? 14. Digestion of Inulin. — To 5 c.c. of inulin solution in a test- tube add 10 drops of saliva and place the tube in the water-bath at 400 C. After one-half hour test the solution by Fehling's test.2 Is any reducing substance present ? What do you conclude regard- ing the salivary digestion of inulin? 15. Influence of Temperature. — In each of four tubes place about 5 c.c. of starch paste. Immerse one tube in cold water from the faucet, keep a second at room temperature and place a third on the water-bath at 40 ° C. Now add to the contents of each of these three tubes two drops of saliva and shake well; to the 1 This test paper is prepared as follows : Saturate a good quality of filter paper with 0.5 per cent starch paste to which has been added sufficient iodic acid to make a 1 per cent solution of iodic acid and allow the paper to dry in the air. Cut it in strips of suitable size and preserve for use. 2 If the inulin solution gives a reduction before being acted upon by the saliva it will be necessary to determine the extent of the original reduction by means of a "check" test (see page 47). SALIVARY DIGESTION. 59 contents of the fourth tube add two drops of boiled saliva. Test frequently by the iodine test, using the test-tablet, and note in which tube the most rapid digestion occurs. Explain the results. 16. Influence of Dilution. — Take a series of 6 test-tubes each containing 9 c.c. of water. Add 1 c.c. of saliva to tube 1 and shake thoroughly. Remove 1 c.c. of the solution from tube 1 to tube 2 and after mixing' thoroughly remove 1 c.c. from tube 2 to tube 3. Continue in this manner until you have 6 saliva solutions of gradu- ally decreasing strength. Now add starch paste in equal amounts to each tube, mix very thoroughly and place on the water-bath at 400 C. After 10-20 minutes test by both the iodine and Feh- ling's tests. In how great dilution does your saliva act? 17. Influence of Acids and Alkalis. — (a) Influence of Free Acid. — Prepare a series of six tubes in each of which is placed 4 c.c. of one of the following strengths of free HC1 : 0.2 per cent, o. 1 per cent, 0.05 per cent, 0.025 per cent, 0.0125 per cent and 0.006 per cent. Now add 2 c.c. of starch paste to each tube and shake them thoroughly. Complete the solutions by adding 2 c.c. of saliva to each and repeat the shaking. The total acidity of this series would be as follows: 0.1 per cent, 0.05 per cent, 0.025 per cent, 0.0125 per cent, 0.006 per cent and 0.003 Per cent- Place these tubes on the water-bath at 40° C. for 10-20 minutes. Divide the contents of each tube into two parts, testing one part by the iodine test and testing the other, after neutralization, by Fehling's test. What do you find? (b) Influence of Combined Acid. — Repeat the first three experi- ments of the above series using combined hydrochloric acid (see page 119) instead of the free acid. How does the action of the combined acid differ from that of the free acid? (c) Influence of Alkali. — Repeat the first four experiments under (a) replacing the HC1 by 2 per cent, 1 per cent, 0.5 per cent and 0.25 per cent Na2C03. Neutralize the alkalinity before trying the iodine test (see Starch, 5, page 44). (d) Nature of the Action of Acid and Alkali. — Place 2 c.c. of saliva and 2 c.c. of 0.2 per cent HC1 in a test-tube and leave for 15 minutes. Neutralize the solution, add 4 c.c. of starch paste and place the tube on the water-bath at 400 C. In 10 minutes test by the iodine and Fehling's tests and explain the result. Repeat the experiment, replacing the 0.2 per cent HC1 by 2 per cent Na2C03. What do you deduce from these two experiments? 18. Influence of Metallic Salts, etc. — In each of a series of 60 PHYSIOLOGICAL CHEMISTRY. tubes place 4 c.c. of starch paste and x/z c.c. of one of the solutions named below. Shake well, add ^ c.c. of saliva to each tube, thor- oughly mix, and place on the water-bath at 400 C. for 10-20 minutes. Show the progress of digestion by means of the iodine and Fehling tests. Use the following chemicals : Metallic salts, 10 per cent plumbic acetate, 2 per cent cupric sulphate, 5 per cent ferric chloride, 8 per cent mercuric chloride; Neutral salts, 10 per cent sodium chloride, 10 per cent magnesium sulphate, 3 per cent barium chloride, 10 per cent Rochelle salt. Also try the influence of 2 per cent carbolic acid, 95 per cent alcohol, and ether and chlor- oform. What are your conclusions? 19. Excretion of Potassium Iodide. — Ingest a small dose of potassium iodide (0.2 gram) contained in a gelatin capsule, quickly rinse out the mouth with water and then test the saliva at once for iodine. This test should be negative. Make additional tests for iodine at 2 minute intervals. The test for iodine is made as fol- lows : Take 1 c.c. of NaN02 and 1 c.c. of dilute HoSCV in a test- tube, add a little saliva directly from the mouth, and a small amount of starch paste. If convenient, the urine may also be tested. The formation of a blue color signifies that the potassium iodide is being excreted through the salivary glands. Note the length of time elapsing between the ingestion of the potassium iodide and the appearance of the first traces of the substance in the saliva. The chemical reactions taking place in this experiment are indicated in the following equations : ( a) 2NaN02 + H2S04 = 2HN02< + Na2S04. ( b ) 2KI + H2S04 = 2HI + K2S04. (c) 2HN02 + 2HI = I2 + 2H20 + 2NO. 20. Qualitative Analysis of the Products of Salivary Diges- tion.— To 25 c.c. of the products of salivary digestion (saved from Experiment 12 or furnished by the instructor), add 100 c.c. of 95 per cent alcohol. Allow to stand until the white precipitate has settled. Filter, evaporate the filtrate to dryness, dissolve the resi- due in 5-10 c.c. of water and try Fehling's test (page 27) and the phenylhydrazine reaction (see Dextrose, 3, page 24). On the dex- trin precipitate try the iodine test (page 44). Also hydrolyze the dextrin as given under Dextrin, 4, page 48. 1 Instead of this mixture a few drops of HNOs possessing a yellowish or brownish color due to the presence of HNO2 may be employed. CHAPTER IV. PROTEINS.1 THEIR DECOMPOSITION AND SYNTHESIS. The proteins are a class of substances, which in the light of our present knowledge, consist, in the main of combinations of a- amino-acids or their derivatives. These protein substances form the chief constituents of many of the fluids of the body, constitute the organic basis of animal tissue, and at the same time occupy a decidedly preeminent position among our organic food-stuffs. They are absolutely necessary to the uses of the animal organism for the continuance of life and they cannot be satisfactorily replaced in the diet of such an organism by any other dietary constituent either organic or inorganic. Such an organism may exist without pro- tein food for a period of time, the length of the period varying according to the specific organism and the nature of the substitu- tion offered for the protein portion of the diet. Such a period is, however, distinctly one of existence rather than one of normal life and one which is consequently not accompanied by such a full and free exercise of the various functions of the organism as would be possible upon an evenly balanced ration, i. c., one containing the requisite amount of protein food. These protein substances, are. furthermore, essential constituents of all living cells and therefore without them vegetable life as well as animal life is impossible. The proteins, which constitute such an important group of sub- stances, differ from the carbohydrates and fats very decidedly in elementary composition. In addition to containing carbon, hy- drogen, and oxygen, which are present in fats and carbohydrates, the proteins invariably contain nitrogen in their molecule and gen- erally sulphur also. Proteins have also been identified which con- tain phosphorus, iron, copper, iodine, manganese, and sine. The percentage composition of the more important members of the group of protein substances would fall within the following limits : C = 50-55 per cent, H= 6-7.3 Per cent- 0 = 19-24 per cent, N= 15-19 per cent. 5 = 0.3-2.5 per cent, P = 0.4-0.8 per cent 1 The term proteid has been very widely used by English-speaking scientists to signify the class of substances we have called proteins. 61 62 PHYSIOLOGICAL CHEMISTRY. when present. When iron, copper, iodine, manganese, or zinc are present in the protein molecule they are practically without excep- tion present only in traces} Of all the various elements of the protein molecule, nitrogen is by far the most important. The human body needs nitrogen for the continuation of life, but it cannot use the nitrogen of the air or that in various other combinations as we find it in nitrates, nitrites, etc. However, in the protein molecule the nitrogen is pres- ent in a form which is utilizable by the body. The nitrogen in the protein molecule occurs in at least four different forms as follows : I. Monamino acid nitrogen. II. Diamino acid nitrogen or basic nitrogen. III. Amide nitrogen. IV. A guanidine residue. The actual structure of the protein molecule is still unknown, and we have as yet no means by which its molecular weight can be even approximately established. The many attempts which have been made to determine this have led to very different results, some of which are given in the following table: Serum albumin = 4572-5 100-5 135 Egg albumin = 4900-6542 Globin = 1 5000-16086 Oxyhemoglobin = 1 4800-1 5000-1 665 5-1 6730 Of these figures, those given for oxyhemoglobin deserve the most consideration, for these are based on the atomic ratios of the sulphur and iron contained in this substance. The simplest formula that can be calculated from analyses of oxyhemoglobin, namely, C658H1181N207S2FeO210, serves to show the great complexity of this substance. The following formulas which have been proposed for typical protein substances may serve to further impress the fact of the great size of the protein molecule : Egg albumin = C239H386N5SS207S Serum albumin = C450H720N11GS6O140 The decomposition2 of protein substances may be brought about 1 Some investigators regard these elements as contaminations, or constituents of some non-protein substance combined with the protein. 2 The terms " degradation," " dissociation," and " cleavage," are often used in this connection. PROTEINS. 63 by oxidation or hydrolysis, but inasmuch as the hydrolytic proce- dure has been productive of the more satisfactory results, that type of decomposition procedure alone is used at present. This hydrolysis of the protein molecule may be accomplished by acids, alkalis, or superheated steam, and in digestion by the action of the proteolytic enzymes. The character of the decomposition products varies ac- cording to the method utilized in tearing the molecule apart. Bear- ing this in mind, we may say that the decomposition products of proteins include proteoses, peptones, peptides, carbon dioxide, am- monia, hydrogen sulphide, and amino acids. These amino acids constitute a long list of important substances which contain nuclei belonging either to the aliphatic, carbocyclic, or heterocyclic series. The list includes, glycocoll, alanine, serine, phenylalanine, tyrosine, cystine, tryptophane, histidine, valine, arginine, leucine, isoleucine, lysine, aspartic acid, glutamic acid, proline, oxy proline, and diamino- trihydroxydodecanoic acid. Of these amino acids, tyrosine and phenylalanine contain carbocyclic nuclei, histidine, proline and tryp- tophane contain heterocyclic nuclei, and the remaining members of the list, as given, contain aliphatic nuclei. The amino acids are pre- eminently the most important class of protein decomposition prod- ucts. These amino acids are all a-amino acids, and, with the exception of glycocoll, are all optically active. Furthermore they are amphoteric substances and consequently are able to form salts with both bases and acids. These properties are inherent in the NH2 and COOH groups of the amino acids. The decomposition products of protein may be grouped as pri- mary and secondary decomposition products. By primary products are meant those which exist as radicals within the protein molecule and which are liberated, upon cleavage of this molecule, with their carbon chains intact and the position of their nitrogen unaltered. The secondary products are those which result from the disintegra- tion of the primary cleavage products. No matter what method is used to decompose a given protein molecule, the primary products are largely the same under all conditions.1 In the process of hydrolysis the protein molecule is gradually broken dow.n and less complicated aggregates than the original molecule are formed, which are known as proteoses, peptones and peptides and which still possess true protein characteristics. Fur- ther hydrolysis causes the ultimate transformation of these sub- 1 Alkaline hydrolysis yields urea and ornithine which result from arginine, the product of acid hydrolysis. 64 PHYSIOLOGICAL CHEMISTRY. stances, of a protein nature, into the amino acids of known chemi- cal structure. In this decomposition the protein molecule is not broken down in a regular manner into y2, Ya, % portions and the amino acids formed in a group at the termination of the hy- drolysis. On the contrary, certain amino acids are formed very early in the process, in fact while the main hydrolytic action has proceeded no further than the proteose stage. Gradually the com- plexity of the protein portion undergoing decomposition is sim- plified by the splitting off of the amino acids and finally it is so far decomposed through previous cleavages that it yields only amino acids at the succeeding cleavage. In short the general plan of the hydrolysis of the protein molecule is similar to the hydrolysis of starch. In the case of starch there is formed a series of dextrins of gradually decreasing complexity and coincidently with the formation of each dextrin a small amount of sugar is split off and finally nothing but sugar remains. In the case of protein hydrolysis there is a series of proteins of gradually decreasing complexity produced and coincidently with the formation of each new protein substance amino acids are split off and finally the sole products remaining are amino acids. Inasmuch as diversity in the method of decomposing a given protein does not result in an equally diversified line of decomposition products, but, on the other hand, yields products which are quite comparable in character, it may be argued that there are probably well denned lines of cleavage in the individual protein molecule and that no matter what the force brought to bear to tear such a molecule apart, the disintegration, when it comes, will yield in every case, certain definite fragments. These fragments may be called the " building stones " of the protein molecule, a term used by some of the German investigators. Take, for example, the decomposition of protein which may be brought about through the action of the enzyme trypsin of the pancreatic juice. When this enzyme is allowed to act upon a given protein, the latter is disintegrated in a series of definite cleavages, resulting in the for- mation of proteoses, peptones and peptides in regular order, the peptides being the last of the decomposition products which possess protein characteristics. They are all built up from amino acids and are therefore closely related to these acids on the one side and to peptones on the other. We have di-, tri-, tetra-, penta-, deca-, and poly-peptides which are named according to the number of amino acids included in the peptide molecule. Following the peptides PROTEINS. 65 there are a diverse assortment of monamino and diamino acids which constitute the final products of the protein decomposition. These acids are devoid of any protein characteristics and are there- fore decidedly different from the original substance from which they were derived. From a protein of huge molecular weight, a typical colloid, perhaps but slightly soluble, and entirely non-dif- fusible, we have passed by way of proteoses, peptones, and pep- tides to a class of simpler crystalline substances which are, for the most part, readily soluble and diffusible. These amino acids after their production in the process of diges- tion, as just indicated, are synthesized within the organism to form protein material which goes to build up the tissues of the body. It is thus seen that the amino acids are of prime importance in the animal economy. Moreover, it is important to remember that these essential factors in metabolism and nutrition cannot be produced within the animal organism from their elements, but are only yielded upon the hydrolysis of ingested protein of animal or vegetable origin. When we examine the formulas of the principal members of the crystalline end-products of protein decomposition we note that they are invariably acids, as has already been mentioned, and contain an NH2 group in the a position. This relation of the NH2 group to the acid radical is constant, no matter what other groups or radicals are present. We may have straight chains as in alanine and glu- tamic acid, the benzene ring as in phenylalanine or we may have sulphurised bodies as in cystine and still the formula is always of the same type, i. e., NH2 I E - CH - COOH It is seen that this characteristic grouping in the amino acid pro- vides each one of these ultimate fragments of the protein molecule with both a strong acid and a strong basic group. For this reason it is theoretically possible for a large number of these amino acids to combine and the resulting combinations may be very great in number, since there is such a varied assortment of the acids. The protein molecule, which is of such mammoth proportions, is prob- ably constructed on a foundation of this sort. Of late much valu- able data have been collected regarding the synthetic production of protein substances, the leaders in this line of investigation being Fischer and Abderhalden. After having gathered a mass of data 6 66 PHYSIOLOGICAL CHEMISTRY. regarding the final products of the protein decomposition and demonstrating that amino acids were the ultimate results of the various forms of decomposition, these investigators, and notably Fischer, set about in an effort to form, from these amino acids, by- synthetic means, substances which should possess protein character- istics. The simplest of these bodies formed in this way was synthe- sized from two molecules of glycocoll with the liberation of water, thus: CH9 - NEL - CO iOH Hi HN - CEL - COOH. L2 -L-N J.O-2 The body thus formed is a dipeptide, called glycyl-glycine. In an analogous manner may be produced leucyl-leucine , through the synthesis of two molecules of leucine or leucyl-alanyl- glycine through the union of one molecule of leucine, one of alanine, and one of glycocoll. By this procedure Fischer and his pupils have been able to make a large number of peptides containing varied numbers of amino acid radicals, the name polypeptides being given to the whole group of synthetic substances thus formed. The most complex poly- peptide yet produced is one containing fifteen glycocoll and three leucine residues. Notwithstanding the fact that most synthetic polypeptides are produced through a union of amino acids by means of their imide bonds, it must not be imagined that the protein molecule is con- structed from amino acids linked together in straight chains in a manner analogous to the formation of simple peptides, such as glycyl-glycine. The molecular structure of the proteins is much too complex to be explained upon any such simple formation as that. There must be a variety of linkings, since there is a varied assort- ment of decomposition products of totally different structure. Many of these synthetic bodies respond to the biuret test, are precipitated by phosphotungstic acid and behave, in other ways, as to leave no doubt as to their protein characteristics. For instance, a number of amino acids each possessing a sweet taste have been synthesized in such a manner as to yield a polypeptide of bitter taste, a well known characteristic of peptones. From the fact that the polypeptides formed in the manner indicated have free acidic and basic radicals we gather the explanation of the amphoteric character of true proteins. Fischer expresses the encouraging belief that he will soon be able to produce a true protein by the synthesis of its decomposition products. Silk fibroin is the protein substance he expects to synthesize. He no doubt will perform this PROTEINS. 67 joint office for organic and physiological chemistry if it is capable of performance by the present methods of technique. Even Fischer, however, is frank enough to say that the production of the great body of protein substances synthetically, will, under the most en- couraging conditions, be a terrific task, involving the " life-work of a whole army of inventive and diligent chemists." For the benefit of those especially interested in such matters a photograph of the Fischer apparatus (Fig. 22, page 71) used in the fractional distillation, in vacuo, of the esters of the decompo- sition products of the proteins, as well as micro-photographs and drawings of preparations of several of these decomposition products (Figs 19 to 31, pages 68 to 81) are introduced. For the prepara- tions and the photograph of the apparatus the author is indebted to Dr. T. B. Osborne, of New Haven, Conn., who has made many important observations upon the hydrolysis of proteins. The repro- duction of the crystalline form of some of the more recent of the products may be of interest to those viewing the field of physio- logical chemistry from other than the student's aspect. An extended discussion of the various decomposition products being out of place in a book of this character, we will simply make a few general statements in connection with the primary decompo- sition products. DISCUSSION OF THE PRODUCTS. Ammonia, NH3. — Ammonia is an important decomposition product of all proteins and probably arises from an amide group combined with a carboxyl group of some of the amino acids. It is possible that the dibasic acids, aspartic and glutamic, furnish most of these carboxyl groups. This is indicated by the more or less close relationship which exists between the amount of ammonia and that of the dibasic acids which the several proteins yield upon decomposition. The elimination of the ammonia from proteins under the action of acids and alkalis is very similar to that from amides like asparagine. Glycocoll, C2H5N02. — Glycocoll, or amino acetic acid, is the simplest of the amino acids and has the following formula : NH2 H-C-COOH. I H 68 PHYSIOLOGICAL CHEMISTRY. Glycocoll, as the formula shows, contains no asymmetric carbon atom, and is the only amino acid yielded by protein decomposition which is optically inactive. Glycocoll and leucine were the first decom- position products of proteins to be discovered (1820). Upon ad- ministering benzoic acid to animals the output of hippuric acid in the urine is greatly increased, thus showing a synthesis of benzoic acid and glycocoll in the organism (see p. 160, Chapter IX) . Glyco- coll, ingested in small amount, is excreted in the urine as urea, whereas if administered in excess it appears in part unchanged in the urine. It is usually separated from the mixture of protein de- composition products as the hydrochloride of the ester. The crys- talline form of this compound is shown in Fig. 19. Fig. 19. Glycocoll Ester Hydrochloride. Alanine, C3H7N02. — Alanine is a-amino-propionic acid, and as such it may be represented structurally as follows : H NH2 H-C-C-COOH. H H Obtained from protein substances, alanine is dextro-rotatory, is very soluble in water, and possesses a sweet taste. Tyrosine, phenylalanine, cystine and serine are derivatives of alanine. This amino acid has been obtained from nearly all proteins examined. Its absence, from those proteins from which it has not been obtained. PROTEINS. 69 has not been proven. Most proteins yield relatively small amounts of alanine. Serine, C3H7N03. — Serine is a-amino-P-hydroxy-propionic acid and possesses the following structural formula : OH NH2 H _ C - C - COOH I I H H Fig. 20. Serine. Serine obtained from proteins is laevo-rotatory, possesses a sweet taste and is quite soluble in water. Serine is not obtained in quantity from most proteins but is yielded abundantly by silk glue. Owing to the difficulty of separating serine it has not been found in a number of proteins in which it probably occurs. Serine crystals are shown in Fig. 20, above. Phenylalanine, C9HuN02. — This product is phenyl-a-amino- propionic acid, and may be represented graphically as follows : H NHo -C-C-COOH. H H The laevo-rotatory form is obtained from proteins. Phenylalanine has been obtained from all the proteins examined except from the yo PHYSIOLOGICAL CHEMISTRY. protamines and some of the albuminoids. The yield of this body from the decomposition of proteins is frequently greater than the Fin. 21. Phenylalanine. yield of tyrosine. The crystalline form of phenylalanine is shown in Fig. 21. Tyrosine, CgH^NC^. — Tyrosine, one of the first discovered end- products of protein decomposition, is the amino acid, p-oxyphenyl- a-amino-propionic acid. It has the following formula : H NH2 I I _C-C-COOH. H H OH The tyrosine which results from protein decomposition is usually lsevo-rotatory although the dextro-rotatory form sometimes occurs. Tyrosine is one of the end-products of tryptic digestion and usually separates in conspicuous amount early in the process of digestion. It does not occur, however, as an end-product of the decomposition of gelatin. Tyrosine is found in old cheese, and derives its name from this fact. It crystallizes in tufts, sheaves or balls of fine needles, which decom- pose at 295 ° C. and are sparingly soluble in cold (1-2454) water, PROTEINS. 7< but much more so in boiling (1-154) water. Tyrosine forms sol- uble salts with alkalis, ammonia or mineral acids, and is soluble, Fig. 22. Fischer Apparatus. Reproduced from a photograph made by Prof. E. T. Reichert, of the University of Pennsylvania. The negative was furnished by Dr. T. B. Osborne, of New Haven, Conn. A, Tank into which freezing mixture is pumped and from which it flows through the condenser, B ; C, flask from which the esters are distilled, the distillate being collected in D ; E, a Dewar flask containing liquid air serving as a cooler for con- densing tube F ; G and G' , tubes leading to the Geryck pump by which the vacuum is maintained ; /, tube leading to a McLeod gauge (not shown in figure) ; /, a bath con- taining freezing mixture in which the receiver D is immersed ; K, a bath of water during the first part of the distillation and of oil during the last part of the process ; 1-5, stop cocks which permit the cutting out of different parts of the apparatus as the procedure demands. with difficulty, in acetic acid. It responds to Millon's reaction, thus showing the presence of the hydroxyphenyl group, but gives no 72 PHYSIOLOGICAL CHEMISTRY. other protein test. The aromatic groups present in tyrosine, phenyl- alanine and tryptophane cause proteins to yield a positive xantho- proteic reaction. In severe cases of typhoid fever and smallpox, Fig. 23- Tyrosine. in acute yellow atrophy of the liver, and in acute phosphorus poison- ing-, tyrosine has been found in the urine. Tyrosine crystals are shown in Fig. 23, above. Cystine, C6H1204N2S2. — Friedmann has recently shown cystine to be the disulphide of a-amino-fi-thiolactic acid1 and to possess the following structural formula: CH2-S — kvCxl2 CHNH2 CH-NH2 I I COOH COOH. Cystine is the principal sulphur-containing body obtained from the decomposition of protein substances. It is obtained in greatest amount as a decomposition product of such keratin-containing tis- sues as horn, hoof and hair. Cystine occurs in small amount in normal urine and is greatly increased in quantity under certain pathological conditions. It crystallizes in thin, colorless hexagonal plates which are shown in Fig. 24, p. 73. Cystine is very slightly soluble in water but its salts, with both bases and acids, are readily soluble in water. It is lsevo-rotatory. 1 Also called a-diamino-/3-dithio-dilactylic acid. PROTEINS. 73 It has recently been claimed that cystine occurs in two forms, i. e., stone-cystine and protein-cystine and that these two forms are distinct in their properties. This view is incorrect. Fig. 2a. Cystine. For a discussion of cystine sediments in urine see Chapter XX. Tryptophane, CnH12N202. — According to Ellinger, tryptophane is indol-amino-propionic acid. Recently Ellinger and Flamand have shown that it possesses the following formula : /\ C-CH2CH(NH2)-COOH U\Ah NH Tryptophane is the mother-substance of indole, skatole, skatole acetic acid and skatole carboxylic acid, all of which are formed as secondary decomposition products of proteins. Its presence in protein substances may be shown by means of the Adamkiewicz reaction or the Hopkins-Cole reaction (see page 91). It may be detected in a tryptic digestion mixture through its property of giving a violet color-reaction with bromine water. Tryptophane is yielded by nearly all proteins but has been shown to be entirely absent from zein, the prolamin (alcohol-soluble protein) of maize. Solutions of tryptophane in sodium hydroxide are dextro-rotatory. Upon being heated to 266 ° C. tryptophane decomposes with the evo- lution of gas. 74 PHYSIOLOGICAL CHEMISTRY. Histidine, C6H9N302. — Histidine is a-amino-fS-imidazol-pro- pionic acid with the following structural formula : H NH2 HC = C-C-C-COOH. I I H H HN\/N CH The histidine obtained from proteins is laevo-rotatory. It has been obtained from all the proteins thus far examined, the majority of them yielding about 2.5 per cent of the amino acid. How- Fig. 25. Histidine Dichloride. ever, about 1 1 per cent was obtained by Abderhalden from globin, the protein constituent of oxyhemoglobin and about 13 per cent by Kossel and Kutscher from the protamine sturine. Crystals of histidine dichloride are shown in Fig. 25, above. Knoop's Color Reaction for Histidine. — To an aqueous solu- tion of histidine or a histidine salt in a test-tube add a little bromine water. A yellow coloration develops in the cold and upon further addition of bromine water becomes permanent. If the tube be heated,1 the color will disappear and will shortly be replaced by a faint red coloration which gradually passes into a deep wine red. Usually black, amorphous particles separate out and the solution becomes turbid. 1 The same reaction will take place in the cold more slowly. PROTEINS. 75 The reaction cannot be obtained in solutions containing free alkali. It is best to use such an amount of bromine as will produce a permanent yellow color in the cold. The use of a less amount of bromine than this produces a weak coloration whereas an excess of bromine prevents the reaction. The test is not very delicate, but a characteristic reaction may always be obtained in I : iooo solu- tions. The only histidine derivative which yields a similar colora- tion is imidazolethylamine, and the reaction in this case is rather weak as compared with the color obtained with histidine or histi- dine salts. Valine, C5HnN02. — The amino-valerianic acid obtained from proteins is a-amino-isovalerianic acid, and as such bears the follow- ing formula : CH3 NH2 H-C C-COOH. I I CH3 H It closely resembles leucine in many of its properties, but is more soluble in water. It is a difficult matter to identify valine in the presence of leucine and isoleucine inasmuch as these amino acids crystallize together in such a way that the combination persists even after repeated recrystallizations. Valine is dextro-rotatory. Arginine, C6H14N402. — Arginine is guanidine-a-amino-valeri- anic acid and possesses the following structural formula : H H H NH2 NH-C-C-C-C-COOH. I I I I I NH = C H H H H NH2 It has been obtained from every protein so far subjected to decom- position. The arginine obtained from proteins is dextro-rotatory, and has pronounced basic properties, reacts strongly alkaline to litmus, and forms stable carbonates. Because of these facts, some investigators consider arginine to be the nucleus of the protein molecule. It is obtained in widely different amounts from different proteins, over 85 percent of certain protamines having been obtained in the form of this amino acid. It is claimed that in the ordinary 76 PHYSIOLOGICAL CHEMISTRY. metabolic activities of the animal body arginine gives rise to urea. While this claim is probably true, it should, at the same time, be borne in mind that the greater part of the protein nitrogen is eliminated as urea and that, therefore, but a very small part can arise from arginine. Leucine, C6H13N02. — Leucine is an abundant end-product of the decomposition of protein material, and, together with glycocoll, was the first of these products to be discovered (1820). It is a-amino-isobutyl-acetic acid, and therefore has the following for- mula : CIL NIL CH-CH.-C-COOH. CIL H The leucine which results from protein decomposition is /-leucine. Leucine is present normally in the pancreas, thymus, thyroid, spleen, brain, liver, kidneys and salivary glands. It has been found patho- logically in the urine (in acute yellow atrophy of the liver, in acute phosphorus poisoning and in severe cases of typhoid fever and smallpox), and in the liver, blood and pus. Fig. 26. Leucine. Pure leucine crystallizes in thin, white hexagonal plates. Crystals of pure leucine are reproduced in Fig. 26. It is rather easily soluble in water (46 parts), alkalis, ammonia and acids. On rapid heating PROTEINS. 77 to 2950 C, leucine decomposes with the formation of carbon dioxide, ammonia and amylamine. Aqueous solutions of leucine obtained from proteins are lsevo-rotatory, but its acid or alkaline, solutions are dextro-rotatory. So-called impure leucine1 is a slightly refractive substance, which generally crystallizes in balls having a radial structure or in aggregations of spherical bodies, Fig. 104, Chapter XX. Isoleucine, CGH13N02. — Isoleucine is a-amino-methyl-ethyl-pro- pionic acid, and possesses the following structural formula: CH3 NH2 H • C-COOH. A 2H5 H This amino acid was recently discovered by Ehrlich. Its presence has been established among the decomposition products of only a few proteins although it probably occurs among those of many or most of them. Ehrlich has shown that the d-amyl alcohol which is produced by yeast fermentation originates from isoleucine and the isoamylalcohol originates frOm leucine. Isoleucine is dextro- rotatory. Lysine, CGH14N202. — The three bodies, lysine, arginine and his- tidine, are frequently classed together as the hexone bases. Lysine was the first of the bases discovered. It is a-e-diamino-caproic acid and hence possesses the following structure : NH2H H H NH2 1 X 1 I I H-C - C-C-C-C-COOH. H H H H H It is dextro-rotatory and is found in relatively large amount in casein and gelatin. Lysine is obtained from nearly all proteins but is absent from the vegetable proteins which are soluble in strong alcohol. It is the mother-substance of cadaverin and has never been obtained in crystalline form. Lysine is usually obtained as 1 These balls of so-called impure leucine do contain considerable leucine, but inasmuch as they may contain many other things it is a bad practice to allude to them as leucine. 78 PHYSIOLOGICAL CHEMISTRY. the picrate which is sparingly soluble in water and crystallizes readily. These crystals are shown in Fig. 27. Fig. 27. Lysine Picrate. Aspartic Acid, C4H7N04. — Aspartic acid is amino-succinic acid and has the following structural formula : Aspartic Acid. PROTEINS. 79 The amide of aspartic acid, asparaginic, is very widely distributed in the vegetable kingdom. The crystalline form of aspartic acid is exhibited in Fig. 28. Aspartic acid has been found among the decomposition products of all the proteins examined, except the protamines. It has not been obtained, however, in very large proportion from any of them. The aspartic acid obtained from protein is laevo-rotatory. Glutamic Acid, C5H9N04. — This acid is a-amino-normal-glntaric acid and as such bears the following graphic formula: NH2 CHCOOH I CH2 CH2COOH. Glutamic acid is yielded by all the proteins thus far examined, except the protamines, and by most of these in larger amount than any other of their decomposition products. It is yielded in espe- cially large proportion by most of the proteins of seeds, 41.32 per Fig. 29. m e Glutamic Acid. Reproduced from a micro-photograph made by Prof. E. T. Reichert, of the University of Pennsylvania. cent having been obtained very recently by Kleinschmitt from the hydrolysis of hordcin the prolamin of barley. This is the largest 8o PHYSIOLOGICAL CHEMISTRY. amount of any single decomposition product yet obtained from any protein except the protamines.1 Glutamic acid and aspartic acid are the only dibasic acids which have thus far been obtained as decomposition products of proteins. As there is an apparent relation between the proportion of these acids and that of ammonia which the different proteins yield it is possible that one of the carboxyl groups of these acids is united with NH2 as an amide, the other carboxyl group being united in poly- peptide union (see page 66) with some other amino acid. This might be represented by the following formula : R-CHNH-COOH C0-CHNH9-CH9-CH9-C0NH9. It has not been definitely proven, however, that this form of link- ing actually occurs. The glutamic acid, yielded by proteins upon hydrolysis, is dextro- rotatory. Crystals of glutamic acid are reproduced in Fig. 29, page 79. Proline, C5H9N02. — Proline is a-pyrrolidine-carboxylic acid and possesses the following graphic structure : HoC CHo H2C\/CHCOOH. NH Fig. 30. L.ffiVO-a-PROLINE. 1Up to this time the yield of 37.33 per cent obtained by Osborne and Harris from gliadin of wheat was the maximum yield PROTEINS. 8 1 Proline was first obtained as a decomposition product of casein. Proline obtained from proteins is lsevo-rotatory and is the only protein decomposition product which is readily soluble in alcohol. It is also one of the few heterocyclic compounds obtained from pro- teins. Proline was quite recently discovered but has since been found among the decomposition products of all proteins except the protamines. The maximum yield reported is 13.73 Per cent obtained by Osborne and Clapp from the hydrolysis of hordein. The crystal- line form of lav o-a- proline is shown in Fig-. 30, and the copper Fig. 31. Copper Salt of Proline. Reproduced from a micro-photograph made by Prof. E. T. Reichert, of the University of Pennsylvania. salt of proline is represented by a micro-photograph in Fig. 31, above. The crystals of the copper salt have a deep blue color but when they lose their water of crystallization they assume a char- acteristic violet color. Oxyproline, C5H9N03. — Oxyproline was recently discovered by Fischer. It has as yet been obtained from only a few proteins, but this may be due to the fact that only a few have been examined for its presence. Its structure has not yet been established. Diaminotrihydroxydodecanoic Acid, C12PI2gNo05. — This amino acid was discovered by Fischer and Abderhalden as a product of the hydrolysis of casein. It has thus far been obtained from no other source. It is lsevo-rotatory and its constitution has not been determined. 82 physiological chemistry. Experiments. While the ordinary courses in physiological chemistry preclude any extended study of the decomposition products of proteins, the manipulation of a simple decomposition and the subsequent isola- tion and study of a few of the products most easily and quickly obtained will not be without interest.1 To this end the student may use the following decomposition procedure : Treat the protein in a large flask with water containing 3-5 per cent of H2S04 and place it on a water-bath until the protein material has been decomposed and there remains a fine, fluffy, insoluble residue. Filter off this residue and neutralize the filtrate with Ba(OH)2 and BaC03. Filter off the precipitate of BaS04 which forms and when certain that the fluid is neutral or faintly acid,2 concentrate (first on a wire gauze and later on a water-bath) to a syrup. This syrup contains the end-products of the decomposition of the protein, among which are proteoses, peptones, tyrosine, leucine, etc. Add 95 per cent alcohol slowly to the warm syrup until no more precipitate forms, stirring continuously with a glass rod. This precipitate consists of proteoses and peptones. Gather the sticky precipitate on the rod or the sides of the dish and, after warming the solution gently for a few mo- ments, filter it through a filter paper which has not been previously moistened. After dissolving the precipitate of proteoses and pep- tones in water3 the solution may be treated according to the method of separation given on page 114. The leucine and tyrosine, etc., are in solution in the warm alcoholic filtrate. Concentrate this filtrate on the water-bath to a thin syrup, transfer it to a beaker, and allow it to stand over night in a cool place for crystallization. The tyrosine first crystallizes (Fig. 23, page 72), followed later by the formation of characteristic crystals of impure leucine (see Fig. 105, Chapter XX). After examining these crystals under the microscope, strain off the crystalline material through fine muslin, heat it gently in a little water to dissolve the leu- 1The procedure here set forth has nothing in common with the procedure by means of which the long line of decomposition products just enumerated are obtained. This latter process is an exceedingly complicated one which is entirely outside the province of any course in physiological chemistry. 2 If the solution is alkaline in reaction at this point, the amino acids will be broken down and ammonia will be evolved. 3 At this point the aqueous solution of the proteoses and peptones may be filtered to remove any BaS04 which may still remain. Tyrosine crystals will also be found here, since it is less soluble than the leucine and may adhere to the proteose-peptone precipitate. Add the crystals of tyrosine to the warm al- cohol filtrate. PROTEINS. 83 cine (the tyrosine will be practically insoluble) and filter. Concen- trate the filtrate and allow it to stand in a cool place over night for the crude leucine to crystallize. Filter off the crystals and use them in the tests for leucine given on page 84. The crystals of tyrosine remaining on the paper from the first filtration may be used in the tests for tyrosine as given below. If desired, the tyrosine and leucine may be purified by recrystallizing in the usual manner. Habermann has suggested a method of separating leucine and tyrosine by means of glacial acetic acid. Experiments on Tyrosine. Make the following tests with the tyrosine crystals already pre- pared or upon some pure tyrosine furnished by the instructor. 1. Microscopical Examination. — Place a minute crystal of ty- rosine on a slide, add a drop of water, cover with a cover glass, and examine microscopically. Now run more water under the cover glass and warm in a bunsen flame until the tyrosine has dissolved. Allow the solution to cool slowly then examine again microscopically and compare the crystals with those shown in Fig. 23, page 72. 2. Solubility. — Try the solubility of very small amounts of tyro- sine in cold and hot water, cold and hot 95 per cent alcohol, dilute NH4OH, dilute KOH and dilute HC1. 3. Sublimation. — Place a little tyrosine in a dry test-tube, heat gently and notice that the material does not sublime. How does this compare with the result of Experiment 3 under Leucine? 4. Hoffman's Reaction. — This is the name given to Millon's reaction when employed to detect tyrosine. Add about 3 c.c. of water and a few drops of Millon's reagent to a little tyrosine in a test-tube. Upon dissolving the tyrosine by heat the solution gradu- ally darkens and may assume a dark red color. What group does this test show to be present in tyrosine? 5. Piria's Test. — Warm a little tyrosine on a watch glass on a boiling water-bath for 20 minutes with 3-5 drops of cone. H2S04. Tyrosine sulphuric acid is formed in the process. Cool the solution and wash it into a small beaker with water. Now add CaC03 in substance slowly with stirring, until the reaction of the solution is no longer acid. Filter, concentrate the filtrate and add to it a few drops (avoid an excess) of very dilute neutral ferric chloride. A purple or violet color, due to the formation of the ferric salt of tyrosine-sulphuric acid, is produced. This is one of the most satis- factory tests for the identification of tyrosine. 84 PHYSIOLOGICAL CHEMISTRY. 6. Morner's Test. — Add about 3 c.c. of Morner's reagent1 to a little tyrosine in a test-tube, and gently raise the temperature to the boiling-point. A green color results. Experiments on Leucine. Make the following tests upon the leucine crystals already pre- pared or upon some pure leucine furnished by the instructor. 1, 2 and 3. Repeat these experiments according to the directions given under Tyrosine (page 83). 1 Morner's reagent is prepared by thoroughly mixing i volume of formalin. 45 volumes of distilled water and 55 volumes of concentrated sulphuric acid. CHAPTER V. PROTEINS: THEIR CLASSIFICATION AND PROPERTIES. From what has already been said in Chapter IV, regarding the protein substances it will be recognized that the grouping of the diverse forms of this class of substances in a logical manner is not an easy task. The fats and carbohydrates may be classified upon the fundamental principles of their stereo-chemical relationships whereas such a system of classification in the case of the proteins is absolutely impossible since, as we have already stated, the mole- cular structure of these complex substances is unknown. Because of the diversity of standpoint from which the proteins may be viewed, relative to their grouping in the form of a logically classified series, it is obvious that there is an opportunity for the presen- tation of classifications of a widely divergent character. The fact that there were until recently at least a dozen different classifica- tions which were recognized by various groups of English-speaking investigators, emphasizes the difficulties in the way of the individual or individuals who would offer a classification which should merit universal adoption. Realizing the great handicap and disadvantage which the great diversity of the protein classifications was forcing upon the workers in this field the British Medical Association re- cently drafted a classification which appealed to that body of scien- tists as fulfilling all requirements and presented it for the consid- eration of the American Physiological Society and the American Society of Biological Chemists. The outcome of this has been that there are now only two protein classifications which are recognized by English-speaking scientists, one the British Classification the other the American Classification. These classifications are very similar and doubtless will ultimately be merged into a single classification. In our consideration of the proteins we shall conform in all de- tails to the American Classification. In this connection we will say, however, that we feel that the British Medical Association has strong grounds for preferring the use of the term scleroprotcins for albuminoids and chromoproteins for haemoglobins. The two classi- fications are as follows : 85 86 PHYSIOLOGICAL CHEMISTRY. CLASSIFICATION OF PROTEINS ADOPTED BY THE AMERICAN PHYSIOLOGICAL SOCIETY AND THE AMERICAN SOCIETY OF BIOLOGICAL CHEMISTS. I. SIMPLE PROTEINS. Protein substances which yield only a-amino acids or their de- rivatives on hydrolysis. (a) Albumins. — Soluble in pure water and coagulable by heat, e. g., ovalbumin, serum albumin, lactalbumin, vegetable albumins. (b) Globulins. — Insoluble in pure water but soluble in neutral solutions of salts of strong bases with strong acids,1 e. g., serum globulin, ovo globulin, edestin, amandin and other vegetable globu- lins. (c) Glutelins. — Simple proteins insoluble in all neutral solvents but readily soluble in very dilute acids and alkalis,2 e. g., glutenin. (d) Alcohol-soluble proteins (Prolamins).3 — Simple proteins soluble in 70-80 per cent alcohol, insoluble in water, absolute alcohol and other neutral solvents,4 e. g., zein, gliadin, hordein and bynin. (e) Albuminoids. — Simple proteins possessing a similar struc- ture to those already mentioned, but characterized by a pronounced insolubility in all neutral solvents,5 e. g., elastin, collagen, keratin. (/) Histones. — Soluble in water and insoluble in very dilute ammonia, and, in the absence of ammonium salts, insoluble even in excess of ammonia; yield precipitates with solutions of other pro- teins and a coagulum on heating which is easily soluble in very dilute acids. On hydrolysis they yield a large number of amino acids among which the basic ones predominate. In short histones are basic proteins which stand between protamines and true pro- teins, e. g., globin, thymus histone, scombrone. 1 The precipitation limits with ammonium sulphate should not be made a basis for distinguishing the albumins from the globulins. 2 Such substances occur in abundance in the seeds of cereals and doubtless represent a well-defined natural group of simple proteins. 3 The name prolamins has been suggested for these alcohol-soluble proteins by Dr. Thomas B. Osborne (Science, 1908, XXVIII, p. 417). It is a very- fitting term inasmuch as upon hydrolysis they yield particularly large amounts of proline and ammonia. 4 The subclasses defined (a, b, c, d,) are exemplified by proteins obtained from both plants and animals. The use of appropriate prefixes will suffice to indicate the origin of the compounds, e. g., ovoglobulin, lactalbumin, etc. 5 These form the principal organic constituents of the skeletal structure of animals and also their external covering and its appendages. This definition does not provide for gelatin which is, however, an artificial derivative of collagen. PROTEINS. 87 {g) Protamines. — Simpler polypeptides than the proteins in- cluded in the preceding groups. They are soluble in water, uncoag- ulable by heat, have the property of precipitating aqueous solutions of other proteins, possess strong basic properties and form stable salts with strong mineral acids. They yield comparatively few amino acids, among which the basic ones predominate. They are the simplest natural proteins, e. g., sahnine, sturine, clupeine, scorn- brine. II. CONJUGATED PROTEINS. Substances which contain the protein molecule united to some other molecule or molecules otherwise than as a salt. (a) Nucleoproteins. — Compounds of one or more protein mole- cules with nucleic acid, e. g., cytoglobulin, nucle ohist one. (b) Glycoproteins. — Compounds of the protein molecule with a substance or substances containing a carbohydrate group other than a nucleic acid, e. g., mucins and mucoids {osseomucoid, tendomu- coid, ichthulin, helicoprotein) . (c) Phosphoproteins. — Compounds of the protein molecule with some, as yet undefined, phosphorus-containing substances other than a nucleic acid or lecithin,1 e. g., caseinogen, vitellin. {d) Haemoglobins. — Compounds of the protein molecule with hsematin, or some similar substance, e. g., hcemoglobin, hcemocya- nin. {e) Lecithoproteins. — Compounds of the protein molecule with lecithins, e. g., lecithans, phosphatides. III. DERIVED PROTEINS. I. Primary Protein Derivatives. Derivatives of the protein molecule apparently formed through hydrolytic changes which involve only slight alteration of the pro- tein molecule. (a) Proteans. — Insoluble products which apparently result from the incipient action of water, very dilute acids or enzymes, e. g., myosan, edestan. (b) Metaproteins. — Products of the further action of acids and alkalis whereby the molecule is so far altered as to form products soluble in very weak acids and alkalis but insoluble in neutral fluids, e. g., acid metaprotein {acid albuminate) , alkali mctaprotein {alkali albuminate) . 1 The accumulated chemical evidence distinctly points to the propriety of classi- fying the phosphoproteins as conjugated compounds, i. c, they are possibly esters of some phosphoric acid or acids and protein. 55 PHYSIOLOGICAL CHEMISTRY. (c) Coagulated Proteins. — Insoluble products which result from (i) the action of heat on their solutions, or (2) the action of alcohol on the protein. 2. Secondary Protein Derivatives.1 Products of the further hydrolytic cleavage of the protein molecule. (a) Proteoses. — Soluble in water, non-coagulable by heat, and precipitated by saturating their solutions with ammonium — or zinc sulphate,2 e. g., protoproteose, deuteroproteose. (b) Peptones. — Soluble in water, non-coagulable by heat, but not precipitated by saturating their solutions with ammonium sul- phate,3 e. g., antipeptone, ampho peptone. (c) Peptides. — Definitely characterized combinations of two or more amino acids, the carboxyl group of one being united with the amino group of the other with the elimination of a molecule of water,4 e. g., dipeptides, tripeptides, tetrapeptides, pentapeptides. CLASSIFICATION OF PROTEINS ADOPTED BY THE BRITISH MEDICAL ASSOCIATION. I. Simple Proteins. 1. Protamines, e. g., salmine, clupeine. 2. Histones, e. g., globin, scombrone. 3. Albumins, e. g., ovalbumin, serum albumin, vegetable albu- mins. 4. Globulins, e. g., serum globulin, ovoglobulin, vegetable glob- ulins. 5. Glutelins, e. g., glutenin. 6. Alcohol-soluble proteins, e. g., zein, gliadin. 7. Scleroproteins, e. g., elastin, keratin. 8. Phosphoproteins, e. g., caseinogen, vitellin. 1 The term secondary hydrolytic derivatives is used because the formation of the primary derivatives usually precedes the formation of these secondary derivatives. 2 As thus defined, this term does not strictly cover all the protein derivatives commonly called proteoses, e. g., heteroproteose and dysproteose. 8 In this group the kyrines may be included. For the present it is believed that it will be helpful to retain this term as defined, reserving the expression peptide for the simpler compounds of definite structure, such as dipeptides, etc. 4 The peptones are undoubtedly peptides or mixtures of peptides, the latter term being at present used to designate those of definite structure. PROTEINS. 89 II. Conjugated Proteins. 1. Oncoproteins, e. g., mucins, mucoids. 2. Nucleoproteins, e. g., nucleohistone, cytoglobulin. 3. Chromoproteins, e. g., hemoglobin, hccmocyanin. III. Products of Protein Hydrolysis. 1. Infraproteins, e. g., acid infraprotein (acid albuminate) , alkali infraprotein (alkali albuminate). 2. Proteoses, e. g., protoproteose, heteroproteose, deuteroproteose. 3. Peptones, e. g., ainphopeptone, antipeptone. 4. Polypeptides, e. g., dipeptides, tripeptides, tetrapeptides. CONSIDERATIONS OF THE VARIOUS CLASSES OF PROTEINS. SIMPLE PROTEINS. The simple proteins are true protein substances which, upon hy- drolysis, yield only a-amino acids or their derivatives. "Although no means are at present available whereby the chemical individual- ity of any protein can be established, a number of simple proteins have been isolated from animal and vegetable tissues which have been so well characterized by constancy of ultimate composition and uniformity of physical properties that they may be treated as chemical individuals until further knowledge makes it possible to characterize them more definitely." Under simple proteins we may class, albumins, globulins, glutelins, prolamins, albuminoids, his- tones and protamines. ALBUMINS. Albumins constitute the first class of simple proteins and may be defined as simple proteins which are coagulable by heat and soluble in pure (salt-free) water. Those of animal origin are not precipitated upon saturating their neutral solutions at 300 C. with sodium chloride or magnesium sulphate, but if a saturated solution of this character be acidified with acetic acid the albumin precipi- tates. All albumins of animal origin may be precipitated by sat- urating their solutions with ammonium sulphate.1 They may be 1 In this connection, Osborne's observation that there are certain vegetable albumins which are precipitated by saturating their solutions with sodium chlor- ide or magnesium sulphate or by half-saturating with ammonium sulphate, is of interest. 90 PHYSIOLOGICAL CHEMISTRY. thrown out of solution by the addition of a sufficient quantity of a mineral acid, whereas a weak acidity produces a slight precipitate which dissolves upon agitating the solution. Metallic salts also possess the property of precipitating albumins, some of the precipi- tates being soluble in excess of the reagent whereas others are in- soluble in such an excess. Of those proteins which occur native the albumins contain the highest percentage of sulphur, ranging from 1.6 to 2.5 per cent. Some albumins have been obtained in crystalline form, notably egg albumin, serum albumin and lactal- bumin but the fact that they may be obtained in crystalline form does not necessarily prove them to be chemical individuals. GENERAL COLOR REACTIONS OF PROTEINS. These color reactions are due to a reaction between some one or more of the constituent radicals or groups of the complex protein molecule and the chemical reagent or reagents used in any given test. Not all proteins contain the same groups and for this reason the various color tests will yield reactions varying in intensity of color according to the nature of the groups contained in the par- ticular protein under examination. Various substances not pro- teins respond to certain of these color reactions and it is therefore essential to submit the material under examination to several tests before concluding definitely regarding its nature. TECHNIQUE OF THE COLOR REACTIONS. i. Millon's Reaction. — To 5 c.c. of a dilute solution of egg albumin in a test-tube add a few drops of Millon's reagent. A white precipitate forms which turns red when heated. This test is a particularly satisfactory one for use on solid proteins, in which case the reagent is added directly to the solid substance and heat applied, which causes the substance to assume a red color. Such proteins as are not precipitated by mineral acids, for example certain of the proteoses and peptones, yield a red solution instead of a red precipitate. The reaction is due to the presence of the hydroxy-phenyl group, — C6H4OH, in the protein molecule and certain non-proteins such as tyrosine, phenol (carbolic acid) and thymol also respond to the reaction. Inasmuch as the tyrosine grouping is the only hy- droxy-phenyl grouping which has definitely been proven to be PROTEINS. 91 present in the protein molecule it is evident that protein substances respond to Millon's reaction because of the presence of this tyro- sine complex. The test is not a very satisfactory one for use in solutions containing inorganic salts in large amount, since the mer- cury of the Millon's reagent1 is thus precipitated and the reagent rendered inert. This reagent is therefore never used for the detec- tion of protein material in the urine. 2. Xanthoproteic Reaction. — To 2-3 c.c. of egg albumin solu- tion in a test-tube add concentrated nitric acid. A white precipi- tate forms, which upon heating turns yellow and finally dissolves, imparting to the solution a yellow color. Cool the solution and carefully add ammonium hydroxide, potassium hydroxide or sod- ium hydroxide in excess. Note that the yellow color deepens into an orange. This reaction is due to the presence in the protein molecule of the phenyl group, with which the nitric acid forms certain nitro modifications. The particular complexes of the pro- tein molecule which are of especial importance in this connection are those of tyrosine, phenylalanine and tryptophane. The test is not a satisfactory one for use in urinary examination because of the color of the end-reaction. 3. Adamkiewicz Reaction. — Thoroughly mix 1 volume of con- centrated sulphuric acid and 2 volumes of acetic acid in a test-tube, add a few drops of egg albumin solution and heat gently. A reddish-violet color is produced. Gelatin does not respond to this test. This reaction shows the presence of the tryptophane group (see next experiment). The test depends upon the presence of glyoxylic acid, CHO ■ COOH + H20 or CH(OH)2COOH, in the reagents. This is shown by the failure to secure a positive reaction when acetic acid free from glyoxylic acid is used. Rosenheim has recently advanced the view that the reaction may be due to the presence of oxidizing agents such as nitrous acid and ferric salts in the sulphuric acid. 4. Hopkins-Cole Reaction. — Place 1-2 c.c. of egg albumin solu- tion and 3 c.c. of glyoxylic acid, CHO " COOH -j- H20 or CH(OH)2COOH, solution (Hopkins-Cole reagent2) in a test-tube 1 Millon's reagent consists of mercury dissolved in nitric acid containing some nitrous acid. It is prepared by digesting one part (by weight) of mercury with two parts (by weight) of HN03 (sp. gr. 1.42) and diluting the resulting solution with two volumes of water. 2 Hopkins-Cole reagent is prepared as follows: To one liter of a saturated solution of oxalic acid add 60 grams of sodium amalgam and allow the mixture to stand until the evolution of gas ceases. Filter and dilute with 2-3 volumes of water. 92 PHYSIOLOGICAL CHEMISTRY. and mix thoroughly. In a second tube place 5 c.c. of concentrated sulphuric acid. Incline the tube containing the sulphuric acid and by means of a pipette allow the albumin-glyoxylic acid solution to flow carefully down the side. When stratified in this manner a reddish-violet color forms at the zone of contact of the two fluids. This color is due to the presence of the tryptophane group. Gelatin does not respond to this test. For formula for tryptophane see page 73. 5. Biuret Test. — To 2-3 c.c. of egg albumin solution in a test- tube add an equal volume of concentrated potassium hydroxide solu- tion, mix thoroughly, and add slowly a very dilute (2-5 drops in a test-tube of water) cupric sulphate solution until a purplish-violet or pinkish-violet color is produced. The depth of the color depends upon the nature of the protein, proteoses and peptones giving a de- cided pink, while the color produced with gelatin is not far removed from a blue. This reaction is given by those substances which con- tain two amino groups in their molecule, these groups either being joined directly together or through a single atom of nitrogen or carbon. The amino groups mentioned must either be two CONH2 groups or one CONH2 group and one CSNH2, C(NH)NH2 or CH2NH2 group. It follows from this fact that substances which are non-protein in character but which contain the necessary groups will respond to the biuret test. As examples of such substances may be cited oxamide, CONH2 and biuret, CONH2 CONH2 \ NH . / CONH2 The test derives its name from the fact that this latter sub- stance which is formed on heating urea to 1800 C. (see page 269), will respond to the test. Protein material responds positively since there are two CONH2 groups in the protein molecule. According to Schiff the end-reaction of the biuret test is depend- ent upon the formation of a copper-potassium-biuret compound (cupri-potassium biuret or biuret potassium cupric hydroxide). This substance was obtained by Schiff in the form of long red needles. It has the following formula : PROTEINS. 93 OH OH CO • NH2 Cu NH2C0 \ " / NH HN / \ 00 • NH,— K K— NH2 • CO I I OH OH 6. Posner's Modification of the Biuret Test. — This test is par- ticularly satisfactory for use on dilute protein solutions, and is carried out as follows : To some dilute egg albumin in a test- tube add one-half its volume of potassium hydroxide solution. Now hold the tube in an inclined position and allow some very dilute cupric sulphate solution, made as suggested on page 92 (5), to flow down the side, being especially careful to prevent the fluids from mixing. At the juncture of the two solutions the typical end- reaction of the biuret test should appear as a colored zone (see Biuret Test, page 92). 7. Liebermann's Reaction. — Add about 10 drops of concen- trated egg albumin solution (or a little dry egg albumin) to about 5 c.c. of concentrated HC1 in a test-tube. Boil the mixture until a pinkish-violet color results. This color was originally sup- posed to indicate the presence of a carbohydrate group in the pro- tein molecule, the furfurol formed through the action of the acid upon the protein reacting with the hydroxy-phenyl group of the pro- tein producing the pinkish-violet color. It is now considered un- certain whether the carbohydrate group enters into the reaction. Cole has called attention to the fact that a blue color results if pro- tein material which has been boiled with alcohol and subsequently washed with ether be used in making the test. He believes the blue* color to be due to an interaction between the glyoxylic acid, which was present as an impurity in the ether used in washing the protein, and the tryptophane group of the protein molecule which was split off through the action of the acid. 8. Acree-Rosenheim Formaldehyde Reaction. — Add a few drops of a dilute (1 15000) solution of formaldehyde to 2-3 c.c. of egg albumin solution in a test-tube. Mix thoroughly and after 2-3 minutes carefully introduce a little concentrated sulphuric acid into the tube in such a manner that the two solutions do not mix. A violet zone will be observed at the point of juncture of the 94 PHYSIOLOGICAL CHEMISTRY. two solutions especially if the mixture is slightly agitated. This color probably results through the union of the protein and the formaldehyde. If the sulphuric acid is added to the protein before the formaldehyde is added the typical end-reaction is not obtained. So far as is known this is a specific test for pro- teins. The reaction cannot be applied satisfactorily with concen- trated formaldehyde. Rosenheim claims the reaction is due to the presence of oxidizing material in the sulphuric acid and that when pure sulphuric acid is used no reaction is obtained. He advises the use of a slight amount of an oxidizing agent, e. g., ferric chloride or potassium nitrite (0.005 gram per 100 c.c. of sulphuric acid) in order to facilitate the reaction. Rosenheim further states that proteins respond to the formaldehyde reaction because of the presence of the tryptophane group, a statement which Acree does not accept as proven. 9. Bardach's Reaction.1 — This is the most recent test which has been described for the detection of protein material. The test depends upon the property possessed by protein substances of preventing the formation of typical iodoform crystals through the interaction of an alkaline acetone solution with iodopotassium iodide. Instead of the typical hexagonal plates or stellar forma- tions of iodoform there are produced, under the conditions of the test, fine yellow needles which are apparently some iodine compound other than iodoform. The technique of the test is as follows : Place about 5 c.c. of the protein solution2 under examination in a test-tube, add 2-3 drops of a 0.5 per cent solution of acetone and sufficient Lugol's solution3 to supply a moderate excess of iodine and produce a red-brown coloration. (The amount of Lugol's solu- tion necessary will depend upon the content of protein, sugar and other iodine-reacting substances in the solution under examination and may vary from one drop to several cubic centimeters.) Add an excess (ordinarily about 3 c.c.) of concentrated ammonium hydroxide and thoroughly mix the solution. Place the tube in the test-tube rack, examine the contents at intervals of five minutes, and when it is evident that crystals have formed, place a drop of 1 Bardach : Zeitschrift fur Physiologische Chemie, 1908, LIV, p. 355 ; also Seaman and Gies: Proceedings of the Society for Experimental Biology and Medicine, 1908, V, p. 125. 2 The solution should not contain more than 5 per cent of protein material. 8 Dissolve 4 grams of iodine and 6 grams of potassium iodide in 100 c.c. of dis- tilled water. PROTEINS. 95 the mixture upon a microscopic slide, put a cover glass in position and examine the mixture under the microscope. The formation of canary yellow crystals indicates the presence of protein material in the solution examined. The crystals are ordinarily needle-like in appearance and show a tendency to assume rosette or bundle-like formations but under certain conditions they may show knobbed (nail-like) and branching variations. If a moderate excess of iodine is used in making the test a black precipitate of iodonitro compounds is at once formed upon the ad- dition of the ammonium hydroxide and yellow needles are sub- sequently deposited upon it. In case just the proper amount of iodine is used, the solution soon assumes a yellow color and the black precipitate formed upon the addition of the ammonium hy- droxide is gradually transformed more or less completely into the yellow crystals. In either case the needles ordinarily form within an hour, and frequently in a much shorter time. If too great an excess of iodine is employed the heavy black pre- cipitate may obscure or even prevent the reaction. The presence of insufficient iodine or excess protein may likewise prevent the reaction. In tests in which a concentrated protein solution and an excess of iodine are used, the addition of ammonium hydroxide immediately produces a grayish-green precipitate. In such instances, if the proportions are favorable, and the mixture be stirred with a glass rod for a few minutes, the precipitate is grad- ually transformed into the crystals before mentioned. It is probable that all soluble proteins will respond to Bardach's reaction, but the relative delicacy of the reaction as well as the value of the test as compared with other protein tests remain to be deter- mined. The only disturbing factor noted thus far is the presence of earthy phosphates in the solution under examination. PRECIPITATION REACTIONS AND OTHER PROTEIN TESTS. There are three forms in which proteins may be precipitated i. e., unaltered, as an albuminate, and as an insoluble salt. An instance of the precipitation in a native or unaltered condition is seen in the so-called salting-out experiments. Various salts, notably (NH4)2S04, ZnS04, MgS04,Na2S04 and NaCl possess the power when added in solid form to certain definite protein solutions, of g6 PHYSIOLOGICAL CHEMISTRY. rendering the menstruum incapable of holding the protein in solu- tion, thereby causing the protein to be precipitated or salted-out to use the common term. Mineral acids and alcohol also precipitate proteins unaltered. Proteins are precipitated as albuminates when treated with certain metallic salts, and precipitated as insoluble salts when weak organic acids such as certain of the alkaloidal reagents are added to their solutions. It is generally stated that globulins are precipitated from their solutions upon half saturation with ammonium sulphate and that al- bumins are precipitated upon complete saturation by this salt. Com- paratively few exceptions were found to this rule until proteins of vegetable origin came to be more extensively studied. These studies, furthered especially by Osborne, and associates, have dem- onstrated very clearly that the characterization of a globulin as a protein which is precipitated by half saturation with ammonium sulphate, can no longer hold. Certain vegetable globulins have been isolated which are not precipitated by this salt until a concen- tration is reached greater than that secured by ]ialf -saturation. As an example of an albumin which does not conform to the defini- tion of an albumin as regards its precipitation by ammonium sul- phate, may be mentioned the leucosin of the wheat germ which is precipitated from its solution upon /^//-saturation with ammonium sulphate. The limits of precipitation by ammonium sulphate, therefore, do not furnish a sufficiently accurate basis for the differentiation of globulins from albumins. It has further been determined that a given protein which is precipitable by ammonium sulphate cannot be " salted-out " by the same concentration of the salt under all conditions. Experiments. i. Influence of Concentrated Mineral Acids, Alkalis and Or- ganic Acids. — Prepare five test-tubes each containing 5 c.c. of con- centrated egg albumin solution. To the first add concentrated H2S04, drop by drop, until an excess of the acid has been added. Note any changes which may occur in the solution. Allow the tube to stand for 24 hours and at the end of that period observe any alteration which may have taken place. Heat the tube and note any further change which may occur. Repeat the experiment in the four remaining tubes with concentrated hydrochloric acid, concentrated nitric acid, concentrated potassium hydrox- ide and acetic acid. How do strong mineral acids, strong alkalis and PROTEINS. 97 strong organic acids differ in their action toward protein solutions? 2. Precipitation by Metallic Salts. — Prepare four tubes each containing 2-3 c.c. of dilute egg albumin solution. To the first add mercuric chloride, drop by drop, until an excess of the reagent has been added, noting any changes which may occur. Repeat the experiment with plumbic acetate, argentic nitrate, cupric sulphate, ferric chloride and barium chloride. Egg albumin is used as an antidote for lead or mercury poisoning. Why? 3. Precipitation by Alkaloidal Reagents. — Prepare six tubes each containing 2-3 c.c. of dilute egg albumin solution. To the first add picric acid drop by drop until an excess of the reagent has been added, noting any changes which may occur. Repeat the experi- ment with trichloracetic acid, tannic acid, phosphotungstic acid, phospho-molybdic acid and potassio-mercuric iodide. Acidify with hydrochloric acid before testing with the three last reagents. 4. Heller's Ring Test. — Place 5 c.c. of concentrated nitric acid in a test-tube, incline the tube, and by means of a pipette allow the dilute albumin solution to flow slowly down the side. The liquids should stratify with the formation of a white zone of precipitated albumin at the point of juncture. This is a very delicate test and is further discussed on p. 314. An apparatus called the albumoscope or horismacope has been devised for use in the tests of this character and has met with con- siderable favor. The method of using the albumoscope is described below. Use of the Albumoscope. — This instrument is intended to facili- tate the making of " ring " tests such as Heller's and Roberts'. In making a test about 5 c.c. of the solution under examination is first introduced into the apparatus through the larger arm and the re- agent used in the particular test is then introduced through the capillary arm and allowed to flow down underneath the solution under examination. If a reasonable amount of care is taken there is no possibility of mixing the two solutions and a definitely defined white " ring " is easily obtained at the zone of contact. 5. Roberts' Ring Test. — Place 5 c.c. of Roberts' reagent1 in a test-tube, incline the tube, and by means of a pipette allow the al- bumin solution to flow slowly down the side. The liquids should 1 Roberts' reagent is composed of 1 volume of concentrated HNOs and 5 volumes of a saturated solution of MgSOi. 98 PHYSIOLOGICAL CHEMISTRY. stratify with the formation of a white zone of precipitated albumin at the point of juncture. This test is a modification of Heller's ring test and is rather more satisfactory. The albumoscope may also be used in making this test. (See page 97.) 6. Spiegler's Ring Test. — Place 5 c.c. of Spiegler's reagent1 in a test-tube, incline the tube, and by means of a pipette allow 5 c.c. of albumin solution, acidified with acetic acid, to flow slowly down the side. A white zone will form at the point of contact. This is an exceedingly delicate test, in fact, too delicate for ordi- nary clinical purposes, since it serves to detect albumin when present in the merest trace (1 1250,000). This test is further discussed on page 316. 7. Jolles' Reaction. — Shake 5 c.c. of albumin solution with 1 c.c. of 30 per cent acetic acid and 4 c.c. of Jolles' reagent2 in a test-tube. A white precipitate of albumin should form. Care should be taken to use the correct amount of acetic acid. For further discussion of the test see page 316. 8. Tanret's Test. — To 5 c.c. of albumin solution in a test-tube add Tanret's reagent,3 drop by drop, until a turbidity or precipitate forms. This is an exceedingly delicate test. Sometimes the al- bumin solution is stratified upon the reagent as in Heller's or Rob- erts' ring teste. In urine examination it is claimed by Repiton that the presence of urates lowers the delicacy of the test. Tanret has however very recently made a statement to the effect that the re- moval of urates is not necessary inasmuch as the urate precipitate will disappear on warming and the albumin precipitate will not. He says, however, that mucin interferes with the delicacy of his test and should be removed by acidification with acetic acid and filtration before testing for albumin. 1 Spiegler's reagent has the following composition : Tartaric acid 20 grams. Mercuric chloride 40 " Glycerol 100 " Distilled water 1000 " a Jolles'' reagent has the following composition: Succinic acid 40 grams. Mercuric chloride 20 " Sodium chloride 20 " Distilled water 1000 " 'Tanret's reagent is prepared as follows: Dissolve 1.35 gram of mercuric chloride in 25 c.c. of water, add to this solution 3.32 grams of potassium iodide dissolved in 25 c.c. of water, then make the total solution up to 60 c.c. with water and add 20 c.c. of glacial acetic acid to the combined solutions. PROTEINS. 99 9. Sodium Chloride and Acetic Acid Test. — Mix two volumes of albumin solution and 1 volume of a saturated solution of sodium chloride in a test-tube, acidify with acetic acid and heat to b< tiling. The production of a cloudiness or the formation of a precipitate indicates the presence of albumin. 10. Acetic Acid and Potassium Ferrocyanide Test. — To 5 c.c. of dilute egg albumin solution in a test-tube add 5-10 drops of acetic acid. Mix well, and add potassium ferrocyanide, drop by drop, until a precipitate forms. This test is very delicate. Schmiedl claims that a precipitate of Fe(Cn)6K2Zn or Fe(Cn)6- Zn2, is formed when solutions containing zinc are subjected to this test, and that this precipitate resembles the precipitate secured with protein solutions. In the case of human urine a reaction was obtained when 0.000022 gram of zinc per cubic centimeter was pres- ent. Schmiedl further found that the urine collected from rabbits housed in zinc-lined cages possessed a zinc content which was suffi- cient to yield a ready response to the test. Zinc is the only in- terfering substance so far reported. 11. Salting-out Experiments. — (a) To 25 c.c. of egg albumin solution in a small beaker add solid ammonium sulphate to the point of saturation, keeping the temperature of the solution below 400 C. Filter, test the precipitate by Millon's reaction and the filtrate by the biuret test. What are your conclusions? (b) Repeat the above ex- periment making the saturation with solid sodium chloride. How does this result differ from the result of the saturation with am- monium sulphate? Add 2-3 drops of acetic acid. What occurs? All proteins except peptones are precipitated by saturating their so- lutions with ammonium sulphate. Globulins are the only proteins precipitated by saturating with sodium chloride (see Globulins, page 102), unless the saturated solution is subsequently acidified, in which event all proteins except peptones are precipitated. Soaps may be salted-out in a similar manner (see p. 137). 12. Coagulation or Boiling Test. — Heat 25 c.c. of dilute egg albumin solution to the boiling-point in a small evaporating dish. The albumin coagulates. Complete coagulation may be obtained by acidifying the solution with 3-5 drops of acetic acid1 at the boiling- point. Test the coagulum by Millon's reaction. The acid is added to neutralize any possible alkalinity of the solution, and to dissolve any substances which are not albumin (see further discussion on page 316). 1 Nitric acid is often used in place of acetic acid in this test. In case nitric acid is used, ordinarily 1-2 drops is sufficient. IOO PHYSIOLOGICAL CHEMISTRY. Fig. 32. 13. Coagulation Temperature. — Prepare 4 test-tubes each con- taining 5 c.c. of neutral egg albumin solution. To the first add 1 drop of 0.2 per cent hydrochloric acid, to the second add 1 drop of 0.5 per cent sodium carbonate solution, to the third add 1 drop of 10 per. cent sodium chloride solution and leave the fourth neutral in reaction. Partly fill a beaker of medium size with water and place it within a second larger beaker which also contains water, the two vessels being separated by pieces of cork. Fasten the four test-tubes compactly together by means of a rubber band, lower them into the water of the inner beaker and suspend them, by means of a clamp attached to one of the tubes, in such a manner that the albumin solutions shall be midway between the upper and lower surfaces of the water. In one of the tubes place a thermometer with its bulb entirely beneath the surface of the albumin solution (Fig. 32). Gently heat the water in the beakers, noting carefully any changes which may occur in the albumin solutions and record the exact temperature at which these changes occur. The first ap- pearance of an opacity in an albumin solution indicates the commencement of coagulation and the temperature at which this occurs should be recorded as the coagulation temperature for that particular albu- min solution. What is the order in which the four solutions coagulate? Repeat the experiment, adding to the first tube 1 drop of acetic acid, to the second 1 drop of concentrated potassium hydroxide solution, to the third 2 drops of a 10 per cent sodium chloride solu- tion and leave the fourth neutral as before. What is the. order of coagulation here? Why? 14. Precipitation by Alcohol. — Prepare 3 test-tubes each con- taining about 10 c.c. of 95 per cent alcohol. To the first add one Coagulation Temperature Apparatus. PROTEINS. IOI drop of 0.2 per cent hydrochloric acid, to the second one drop of potassium hydroxide solution and leave the third neutral in reac- tion. Add to each tube a few drops of egg albumin solution and note the results. What do you conclude from this experiment? Alcohol precipitates proteins unaltered but if allowed to remain under alcohol the protein is transformed. The "fixing" of tissues for histological examination by means of alcohol is an illustra- tion of the application of this transformation produced by alcohol. It apparently is a process of dehydrolysis. 15. Preparation of Powdered Egg Albumin. — This may be prepared as follows : Ordinary egg-white finely divided by means of scissors or a beater is treated with four volumes of water and filtered. The filtrate is evaporated on a water-bath at about 500 C. and the residue powdered in a mortar. 16. Tests on Powdered Egg Albumin. — With powdered albu- min prepared as described above (by yourself or furnished by the instructor), try the following tests: (a) Solubility. (b) Millon's Reaction. (c) Hopkins-Cole Reaction. — When used to detect the presence of protein in solid form this reaction should be conducted as follows : Place 5 c.c. of concentrated sulphuric acid in a test-tube and add carefully, by means of a pipette, 3-5 c.c. of Hopkins-Cole reagent. Introduce a small amount of the solid substance to be tested, agitate the tube slightly, and note that the suspended pieces assume a reddish-violet color, which is the characteristic end-reaction of the Hopkins-Cole test; later the solution will also assume the reddish-violet color. (d) Composition Test. — Heat some of the powder in a test- tube in which is suspended a strip of moistened red litmus paper and across the mouth of which is placed a piece of filter paper moistened with plumbic acetic solution. As the powder is heated it chars, indicating the presence of carbon; the fumes of ammonia are evolved, turning the red litmus paper blue and indicating the presence of nitrogen and hydrogen; the plumbic acetate paper is blackened, indicating the presence of sulphur, and the deposition of moisture on the side of the tube indicates the presence of hydrogen. (e) Immerse a dry test-tube containing a little powdered egg albumin in boiling water for a few moments. Remove and test the solubility of the albumin according to the directions given under 102 PHYSIOLOGICAL CHEMISTRY. (a) p. ioi. It is still soluble. Why has it not been coagulated? Repeat the above experiments with powdered serum albumin and see how the results compare with those just obtained. SULPHUR IN PROTEIN. Sulphur is believed to be present in two different forms in the protein molecule. The first form, which is present in greatest amount, is that loosely combined with carbon and hydrogen. Sul- phur in this form is variously termed unoxidized, loosely combined, mercaptan and lead-blackening sulphur. The second form is com- bined in a more stable manner with carbon and oxygen and is known as oxidised or acid sulphur. The protamines are the only class of sulphur-free proteins. Tests for Sulphur. i. Test for Loosely Combined Sulphur. — To equal volumes of KOH and egg albumin solutions in a test-tube add 1-2 drops of plumbic acetate solution and boil the mixture. Loosely combined sulphur is indicated by a darkening of the solution, the color deep- ening into a black if sufficient sulphur is present. Add hydrochloric acid and note the characteristic odor evolved from the solution. Write the reactions for this test. 2. Test for Total Sulphur (Loosely Combined and Oxidized). — Place the substance to be examined (powdered egg albumin) in a small porcelain crucible, add a suitable amount of solid fusion mixture (potassium hydroxide and potassium nitrate mixed in the proportion 5:1) and heat carefully until a colorless mixture results. (Sodium peroxide may be used in place of this fusion mixture if desired.) Cool, dissolve the cake in a little warm water and filter. Acidify the filtrate with hydrochloric acid, heat it to the boiling- point and add a small amount of barium chloride solution. A white precipitate forms if sulphur is present. What is this pre- cipitate? GLOBULINS. Globulins are simple proteins especially predominant in the vege- table kingdom. They are closely related to the albumins and in common with them give all the ordinary protein tests. Globulins differ from the albumins in being insoluble in pure (salt-free) water. They are, however, soluble in neutral solutions of salts of strong bases with strong acids. Most globulins are precipitated from their PROTEINS. I03» solutions by saturation with solid sodium chloride or magnesium sulphate. As a class they are much less stable than the albumins, a fact shown by the increasing difficulty with which a globulin dissolves during the course of successive reprecipitations. We have used an albumin of animal origin (egg albumin) for all the protein tests thus far, whereas the globulin to be studied will be prepared from a vegetable source. There being no essential difference between animal and vegetable proteins, the vegetable globulin we shall study may be taken as a true type of all globulins, both animal and vegetable. Experiments on Globulin. Preparation of the Globulin. — Extract 20-30 grams fa hand- ful) of crushed hemp seed with a 5 per cent solution of sodium chlo- ride for one-half hour at 60 ° C. Filter while hot through a paper moistened with 5 per cent sodium chloride solution. Place the nitrate in the water-bath at 60 ° C. and allow it to stand for 24 hours in order that the globulin may crystallize slowly. In case the filtrate is cloudy is should be warmed to 6o° C. in order to produce a clear solution. The globulin is soluble in hot 5 per cent sodium chloride solution and is thus extracted from the hemp seed, but upon cooling this solution much of the globulin separates in crystalline form. This particular globulin is called edestin. It crystallizes in several different forms, chiefly octahedra (see Fig. 33, page 104). (The crystalline form of excelsin, a protein ob- tained from the Brazil nut, is shown in Fig. 34, page 105. This vegetable protein crystallizes in the form of hexagonal plates.) Filter off the edestin and make the following tests on the crystalline body and on the filtrate which still contains some of the extracted globulin. Tests on Crystallized Edestin. — (1) Microscopical examina- tion (see Fig. 33, p. 104). (2) Solubility. — Try the solubility in the ordinary solvents (see page 23). Keep these solubilities in mind for comparison with those of edestan, to be made later (see page 109). (3) Milloris Reaction. (4) Coagulation Test. — Place a small amount of the globulin in a test-tube, add a little water and boil. Now add dilute hydrochloric acid and note that the protein no longer dissolves. It has been coagulated. # IO4 PHYSIOLOGICAL CHEMISTRY. (5) Dissolve the remainder of the edestin in 0.2 per cent hydro- chloric acid and preserve this acid solution for use in the experiments on proteans (see page 109). Fig. 33. Edestin. Tests on Edestin Filtrate. — (1) Influence of Protein Pre- cipitants. — Try a few protein precipitants such as nitric acid, tannic acid, picric acid and mercuric chloride. (2) Biuret Test. (3) Coagulation Test. — Boil some of the filtrate in a test-tube. What happens ? (4) Saturation with Sodium Chloride. — Saturate some of the filtrate with solid sodium chloride. How does this result differ from that obtained upon saturating egg albumin solution with solid sodium chloride? (5) Precipitation by Dilution. — Dilute some of the filtrate with 10-15 volumes of water. Why does the globulin precipitate? Glutelins. It has been repeatedly shown, particularly by Osborne, that after extracting the seeds of cereals with water, neutral salt solution and strong alcohol, there still remains a residue which contains protein material which may be extracted by very dilute acid or alkali. These proteins which are insoluble in all neutral solvents, but readily soluble in very dilute acids and alkalis are called glutelins. The only member of the group which has yet received a name, is the glutenin of wheat, a protein which constitutes nearly fifty per cent PROTEINS. I05 of the gluten. It is not definitely known whether glutelins occur as constituents of all seeds. Prolamins (Alcohol-soluble Proteins). The term prolamin has been proposed by Osborne, for the group of proteins formerly termed "alcohol-soluble proteins." The name is very appropriate inasmuch as these proteins yield, upon hydroly- sis, especially large amounts of proline and ammonia. The pro- lamins are simple proteins which are insoluble in water, absolute alcohol and other neutral solvents, but are soluble in 70 to 80 per cent alcohol and in dilute acids and alkalis. They occur widely dis- tributed, particularly in the vegetable kingdom. The only prolamins yet described are the zein of maize, the hordein of barley, the gliadin of wheat and rye and the bynin of malt. They yield relatively large amounts of glutamic acid on hydrolysis but no lysin. The largest Fig. 34. EXCELSIN, THE PROTEIN OF THE BRAZIL NUT. (Drawn from crystals furnished by Dr. Thomas B. Osborne, New Haven, Conn.) percentage of glutamic acid (41.32 per cent) ever obtained as a decomposition product of a protein substance has very recently been obtained by Kleinschmitt from the hydrolysis of the prolamin hordein.1 This yield of glutamic acid is also the largest amount of any single decomposition product yet obtained from any protein except protamines. 'Up to this time the yield of 37.33 per cent obtained by Osborne and Harris from gliadin, was the maximum yield. 106 PHYSIOLOGICAL CHEMISTRY. Albuminoids. (Scleroproteins.) The albuminoids yield similar hydrolytic products to those ob- tained from the other simple proteins already considered, thus indi- cating that they possess essentially the same chemical structure. They differ from all other proteins, whether simple, conjugated or derived, in that they are insoluble in all neutral solvents. The albuminoids include "the principal organic constituents of the skeletal structure of animals as well as their external covering and its appendages." Some of the principal albuminoids are keratin, elastin, collagen, reticulin, spongin, and fibroin. Gelatin cannot be classed as an albuminoid although it is a transformation product of collagen. The various albuminoids differ from each other in certain fundamental characteristics which will be considered in detail under Epithelial and Connective Tissue (see Chapter XIV, p. 227). CONJUGATED PROTEINS. Conjugated proteins consist of a protein molecule united to some other molecule or molecules otherwise than as a salt. We have glycoproteins, nude 0 proteins, hcemoglobins (chromoproteins), phosphoproteins and lecitho proteins as the five classes of conju- gated proteins. Glycoproteins may be considered as compounds of the protein molecule with a substance or substances containing a carbohydrate group other than a nucleic acid. The glycoproteins yield, upon decomposition, protein and carbohydrate derivatives, notably gly- cosamine, CH2OH- (CHOH)3-CH(NH2) -CHO, and galactosa- mine, OHCH2- (CHOH)3-CH(NH2) -CHO. The principal gly- coproteins are mucoids, mucins and chondro proteins. By the term mucoid we may designate those glycoproteins which occur in tis- sues, such as tendomucoid from tendinous tissue and osseomucoid from bone. The elementary composition of these typical mucoids is as follows : N. S. C. H. O. Tendomucoid 11.75 2.33 48.76 6.53 30.60 (Chittenden and Gies) Osseomucoid 12.22 2.32 47.43 6.63 31.40 The term mucins may be said to include those forms of glyco- proteins which occur in the secretions and fluids of the body. Chondroproteins are so named because chondromucoid, the prin- cipal member of the group, is derived from cartilage (chondrigen). Amyloid, which appears pathologically in the spleen, liver and kidneys, is also a chondroprotein. PROTEINS. I07 The nucleoproteins occur principally in animal and vegetable cells, and following the destruction of these cells they are Eound in the fluids of the body. These proteins are discharged into the tissue fluids by the activity or disintegration of cells. Combined with the simple protein in the nucleoprotein molecule we find nucleic acid, a body which contains phosphorus and which yields purine bases and pyrimidine bases (thymine, cytosine and uracil) upon decomposition. The so-called nucleins are formed in the gas- tric digestion of nucleoproteins. Wheeler-Johnson Reaction for Uracil and Cytosine. — To about 5 c.c. of the solution under examination add bromine water until the color is permanent.1 In case the solution contains only small quantities of cytosine or uracil, it is advisable to remove the excess of bromine by passing a stream of air through the solution. Now add an excess of an aqueous solution of barium hydroxide and note the appearance of a purple color. Very dilute solutions do not give the test. Under these condi- tions the solution should be evaporated to dryness, the residue dis- solved in a little bromine water and the excess of bromine removed. Then upon adding an excess of barium hydroxide a decided bluish- pink or lavender color will appear in the presence of as small an amount as 0.00 1 gram of uracil. In testing solutions for cytosine, it is preferable to warm or boil the solution with bromine water, and after cooling the solution to apply the test as suggested above, being careful to have a slight excess of bromine present before adding barium hydroxide. The phospho proteins are called nude 0 albumins in many classi- fications and are grouped among the simple proteins. They are considered to be " compounds of the protein molecule with some, as yet undefined, phosphorus-containing substances other than a nucleic acid or lecithin." The percentage of phosphorus in phos- phoproteins is very similar to that in nucleoproteins but they differ from this latter class of proteins in that they do not yield any purine bases upon hydrolytic cleavage. Two of the common phos- phoproteins are the caseinogen of milk and the ovovitellin of the egg-yolk. The hemoglobins (chromoproteins) are compounds of the pro- tein molecule with hsematin or some similar substance. The prin- 1 Avoid the addition of a large excess of bromine inasmuch as this will interfere with the test. 108 PHYSIOLOGICAL CHEMISTRY. cipal member of the group is the haemoglobin of the blood. Upon hydrolytic cleavage this haemoglobin yields a protein termed globin and a coloring matter termed hcemochromogen. The latter sub- stance contains iron and upon coming in contact with oxygen is oxidized to form hcematin. Hcemocyanin, another member of the class of haemoglobins, occurs in the blood of certain invertebrates, notably cephalopods, gasteropods, and Crustacea. Haemocyanin generally contains either copper, manganese, or zinc in place of the iron of the haemoglobin molecule. The lecitho proteins include such substances as lecithans and phosphophatides which consist of a protein molecule joined to leci- thin. They have been comparatively little studied until recently, and in much of the older research they were undoubtedly con- sidered as lecithins. For experiments on conjugated proteins see pages 56, 195, 196, 199, 201, 203, 223 and 228. DERIVED PROTEINS. These substances are derivatives which are formed through hy- drolytic changes of the original protein molecule. They may be divided into two groups, the primary protein derivatives and the secondary protein derivatives. The term secondary derivatives is made use of in this connection since the formation of the primary derivatives generally precedes the formation of these secondary derivatives. These derived proteins are obtained from native simple proteins by hydrolyses of various kinds, e. g., through the action of acids, alkalis, heat or enzymes. The particular class of derived protein desired regulates the method of treatment to which the native protein is subjected. Primary Protein Derivatives. The primary protein derivatives are " apparently formed through hydrolytic changes which involve only slight alterations of the protein molecule." This class includes proteans, metaproteins, and coagulated proteins. PROTEANS. Proteans are those insoluble protein substances which are pro- duced from proteins originally soluble through the incipient action of water, enzymes, or very dilute acids. It is well known that PROTEINS. IO9 globulins become insoluble upon repeated reprecipitation and it may possibly be found that the greater number of the proteans are transformed globulins. Osborne, however, believes that nearly all proteins may give rise to proteans. This investigator who has so very thoroughly investigated many of the vegetable proteins claims that the hydrogen ion is the active agent in the transformation. The protein produced from the transformation of edestin is called edestan, that produced from myosin is called myosan, etc. The name protean was first given to this class of proteins by Osborne in 1900 in connection with his studies of edestin. Experiments on Proteans. Preparation and Study of Edestan. — Prepare edestin accord- ing to the directions given on page 103. Bring the edestin into solu- tion in 0.2 per cent hydrochloric acid and permit the acid solution to stand for about one-half hour.1 Neutralize, with a 0.5 per cent solution of sodium carbonate, filter off the precipitate of edestan and make the following tests : 1. Solubility. — Try the solubility in the ordinary solvents (see page 23). Note the altered solubility of the edestan as compared with that of edestin (see page 103). 2. Millon's Reaction. 3. Coagulation Test. — Place a small amount of the protean in a test-tube, add a little water and boil. Now add dilute hydro- chloric acid and note that the protein no longer dissolves. It has been coagulated. 4. Tests on Edestan Solution. — Dissolve the remainder of the edestan precipitate in 0.2 per cent hydrochloric acid and make the following tests : (a) Biuret Test. (b) Influence of Protein Precipitants. — Try a few protein precipitants such as picric acid and mercuric chloride. METAPROTEINS. The metaproteins are formed from the native simple proteins through an action similar to that by which proteans are formed. In the case of the metaproteins, however, the changes in the origi- nal protein molecule are more profound. These derived proteins are characterized by being soluble in very weak acids and alkalis, lThe edestan solution preserved from experiment (5), page 104, may be used. IIO PHYSIOLOGICAL CHEMISTRY. but insoluble in neutral fluids. The metaproteins have generally been termed albuminates, but inasmuch as the termination ate sig- nifies a salt it has always been somewhat of a misnomer. Two of the principal metaproteins are the acid metaprotein or so-called acid albuminate and the alkali metaprotein or so-called alkali albuminate. They differ from the native simple proteins principally in being insoluble in sodium chloride solution and in not being coagulated except when suspended in neutral fluids. Both forms of metaprotein are precipitated upon the approximate neutraliza- tion of their solutions. They are precipitated by saturating their solutions with ammonium sulphate, and by sodium chloride, also, provided they are dissolved in an acid solution. Acid metaprotein contains a higher percentage of nitrogen and sulphur than the alkali metaprotein from the same source, since some of the nitro- gen and sulphur of the original protein is liberated in the forma- tion of the latter. Because of this fact, it is impossible to trans- form an alkali metaprotein into an acid metaprotein, while it is possible to reverse the process and transform the acid metaprotein into the alkali modification. Experiments on Metaproteins. ACID METAPROTEIN (ACID ALBUMINATE). Preparation and Study. — Take 25 grams of hashed lean beef, washed free from the major portion of blood and inorganic matter, and place it in a medium-sized beaker with 100 c.c. of 0.2 per cent HC1. Place it on a boiling water-bath for one-half hour, filter, cool and divide the filtrate into two parts. Neutralize the first part with dilute KOH solution, filter off the precipitate of acid meta- protein and make the following tests : ( 1 ) Solubility. — Solubility in the ordinary solvents (see page 23 ) . (2) Milton's Reaction. (3) Coagulation Test. — Suspend a little of the metaprotein in water (neutral solution) and heat to boiling for a few moments. Now add 1-2 drops of KOH solution to the water and see if the metaprotein is still soluble in dilute alkali. What is the result and why? (4) Test for Loosely Combined Sulphur (see page 102). Subject the second part of the original solution to the following tests : PROTEINS. ' I ' (i) Coagulation Test. — Heat some of the solution to boiling in a test-tube. Does it coagulate ? ( 2 ) Biuret Test. • (3) Influence of Protein Precipitants. — Try a few protein pre- cipitants such as picric acid and mercuric chloride. How do the results obtained compare with those from the experiments on egg albumin? (See page 97.) ALKALI METAPROTEIN (ALKALI ALBUMINATE). Preparation and Study. — Carefully separate the white from the yolk of a hen's egg and place the former in an evaporating dish. Add concentrated potassium hydroxide solution, drop by drop, stir- ring continuously. The mass gradually thickens and finally as- sumes the consistency of jelly. This is solid alkali metaprotein or " Lieberkiihn's jelly." Do not add an excess of potassium hydrox- ide or the jelly will dissolve. Cut it into small pieces, place a cloth or wire gauze over the dish and by means of running water wash the pieces free from adherent alkali. Now add a small amount of water, which forms a weak alkaline solution with the alkali within the pieces, and dissolve the jelly by gentle heat. Cool the solution and divide it into two parts. Proceed as follows with the first part: Neutralize with dilute hydrochloric acid, noting the odor of the liberated hydrogen sulphide as the alkali metaprotein precipitates. Filter off the precipitate and test as for acid metaprotein, page no, noting particularly the sulphur test. How does this test compare with that given by the acid metaprotein? Make tests on the second part of the solution the same as for acid metaprotein, page no. Coagulated Proteins. These derived proteins are produced from unaltered protein materials by heat, by long standing under alcohol, or by the con- tinuous movement of their solutions such as that produced by rapid stirring or shaking. In particular instances, such as the formation of fibrin from fibrinogen (see page 191), the coagula- tion may be produced by enzyme action. Ordinary soluble proteins after having been transformed into the coagulated modification are no longer soluble in the ordinary solvents. Upon being heated in the presence of strong acids or alkalis, coagulated proteins are convened into metaproteins. '-•'-I protems consulate at an approximately fixed temperature 112 PHYSIOLOGICAL CHEMISTRY. under definite conditions (see pp. ioo and 242). This characteristic may be applied to separate different coagulable proteins from the same solution by fractional coagulation. The coagulation temperature frequently may serve in a measure to identify proteins in a manner similar to the melting-point or boiling-point of many other organic substances. The separation of proteins by fractional coagulation is thus analogous to the separation of volatile substances by means of fractional distillation. This method of separating proteins is not a satisfactory one, however, inasmuch as proteins in solution have different effects ,upon one another and also because of the fact that the nature of the solvent causes a variation in the tem- perature at which a given protein coagulates. The nature of the process involved in the coagulation of proteins by heat is not well understood, but it is probable that in addition to the altered arrangement of the component atoms in the molecule, there is a mild hydrolysis which is accompanied by the liberation of minute amounts of hydrogen, nitrogen and sulphur. The presence of a neutral salt or a trace of a mineral acid may facilitate the coagula- tion of a protein solution (see page 100), whereas any appreciable amount of acid or alkali will retard or entirely prevent such coagu- lation. Experiments on Coagulated Protein. Ordinary coagulated egg-white may be used in the following tests : 1. Solubility. — Try the solubility of small pieces of the coagu- lated protein in each of the ordinary solvents (see page 23). 2. Millon's Reaction. 3. Xanthoproteic Reaction. — Partly dissolve a medium-sized piece of the protein in concentrated nitric acid. Cool the solution and add an excess of ammonium hydroxide. Both the protein solution and the undissolved protein will be colored orange. 4. Biuret Test. — Partly dissolve a medium-sized piece of the protein in concentrated potassium hydroxide solution. If the proper dilution of cupric sulphate solution is now added the white coagu- lated protein, as well as the protein solution, will assume the char- acteristic purplish-violet color. 5. Hopkins-Cole Reaction. — Conduct this test according to the modification given on page 10 1. PROTEINS. I I 3 Secondary Protein Derivatives. These derivatives result from a more profound cleavage of the protein molecule than that which occurs in the formation of the primary derivatives. The class includes proteoses, peptones and peptides. PROTEOSES AND PEPTONES. Proteoses are intermediate products in the digestion of proteins by proteolytic enzymes, as well as in the decomposition of proteins by hydrolysis and the putrefaction of proteins through the action of bacteria. Proteoses are also called albumoses by some writers, but it seems more logical to reserve the term albumose for the proteose of albumin. Peptones are formed after the proteoses and it has been cus- tomary to consider them as the last product of the processes before mentioned which still possess true protein characteristics. In other words it has been considered that the protein nature of the end- products of the cleavage of the protein molecule ceased with the peptones, and that the simpler bodies formed from peptones were substances of a different nature (see page 63). However, as the end-products have been more carefully studied, it has been found to be no easy matter to designate the exact character of a peptone or to indicate the exact point at which the peptone characteristic ends and the peptide characteristic begins. The situation regarding the proteoses, peptones and peptides, is at present a most unsatis- factory one because of the unsettled state of our knowledge regard- ing them. The exact differences between certain members of the peptone and peptide groups remain to be more accurately estab- lished. It has been quite well established that the peptones are peptides or mixtures of peptides, but the term peptide is used at present to designate only those possessing a definite structure. There are several proteoses (protoproteose, heteroproteose and deuteroproteose), and at least two peptones (amphopeptone and antipeptone), which result from proteolysis. The differentiation of the various proteoses and peptones at present in use is rather unsatisfactory. These compounds are classified according to their varying solubilities, especially in ammonium sulphate solutions of different strengths. The exact differences in composition between the various members of the group remain to be more accurately established. Because of the difficulty attending the separation of these bodies, pure proteose and peptone are not easy to procure. 9 114 PHYSIOLOGICAL CHEMISTRY. The so-called peptones sold commercially contain a large amount of proteose. As a class the proteoses and peptones are very soluble, diffusible bodies which are non-coagulable by heat. Peptones differ from proteoses in being more diffusible, non-precipitable by (NH4)2S04, and by their failure to give any reaction with potas- sium ferrocyanide and acetic acid, potassio-mer curie iodide and HC1, picric acid, and trichloracetic acid. The so-called primary proteoses are precipitated by HN03 and are the only members of the proteose-peptone group which are so precipitated. Some of the more general characteristics of the proteose-peptone group may be noted by making the following simple tests on a proteose-peptone powder : ( i ) Solubility. — Solubility in the ordinary solvents ( see page 23 ) . (2) Millon's Reaction. Dissolve a little of the powder in water and test the solution as follows : (1) Precipitation by Picric Acid. — To 5 c.c. of proteose-peptone solution in a test-tube add picric acid until a permanent precipi- tate forms. The precipitate disappears on heating and returns on cooling. (2) Precipitation by a Mineral Acid. — Try the precipitation by nitric acid. (3) Coagulation Test. — Heat a little proteose-peptone solution to boiling. Does it coagulate like the other simple proteins studied ? SEPARATION OF PROTEOSES AND PEPTONES.1 Place 50 c.c. of proteose-peptone solution in an evaporating dish or casserole, and half-saturate it with ammonium sulphate solution, which may be accomplished by adding an equal volume of saturated ammonium sulphate solution. At this point note the appearance of a precipitate of the primary proteoses (protoproteose and hetero- proteose). Now heat the half-saturated solution and its suspended precipitate to boiling and saturate the solution with solid ammo- nium sulphate. At full saturation the secondary proteoses (deu- teroproteoses) are precipitated. The peptones remain in solution. Proceed as follows with the precipitate of proteoses : Collect the sticky precipitate on a rubber-tipped stirring rod or remove it by means of a watch glass to a small evaporating dish and dissolve 1 The separation of proteoses and peptones by means of fractional precipitation with ammonium sulphate does not possess the significance it once possessed inasmuch as the boundary between these substances and peptides is not well defined (see p. 113). PROTEINS. I I 5 it in a little water. To remove the ammonium sulphate, which adhered to the precipitate and is now in solution, add barium car- bonate, boil, and filter off the precipitate of barium sulphate. Con- centrate the proteose solution to a small volume1 and make the following tests : (i) Biuret Test. (2) Precipitation by Nitric Acid. — What would a precipitate at this point indicate? (3) Precipitation by Trichloracetic Acid. — This precipitate dis- solves on heating and returns on cooling. (4) Precipitation by Picric Acid. — This precipitate also disap- pears on heating and returns on cooling. (5) Precipitation by Potassio-mercuric Iodide and Hydrochloric Acid. (6) Coagulation Test. — Boil a little in a test-tube. Does it coagulate? (7) Acetic Acid and Potassium Ferrocyanide Test. The solution containing the peptones should be cooled and fil- tered, and the ammonium sulphate in solution removed by boiling with barium carbonate as described above. After filtering off the barium sulphate precipitate, concentrate the peptone filtrate to a small volume1 and repeat the test as given under the proteose solu- tion, above. In the biuret test the solution should be made very strongly alkaline with solid potassium hydroxide. PEPTIDES. The peptides are " definitely characterized combinations of two or more amino acids, the carboxyl (COOH) group of one being united with the amino (NH2) group of the other with the elimina- tion of a molecule of- water." These peptides are more fully dis- cussed on pages 66 and 113. REVIEW OF PROTEINS. In order to facilitate the student's review of the proteins, the preparation of a chart similar to the model on p. 117 is recom- mended. The signs + and — may be conveniently used to indi- cate positive and negative reactions. 1 If the proteoses are desired in powder form, this concentrated proteose solu- tion may now be precipitated by alcohol, and this precipitate, after being washed with absolute alcohol and with ether, may be dried and powdered. n6 PHYSIOLOGICAL CHEMISTRY. W H O c4 (u fa o S3 O H U H P W H H O fa w w u en ■d u u G .2 *> ■Ecu a a J; ~ V u ?\ V en I >-2 Ht/p. Is p. 2cd §-g«" ja 5J-C "c" ■- c " V o 3 CO ■5 j, 6 *■ « « ~ S ij £ *v> .a 3.o o 8.S 8J2 2 g-o E .S § ^ *j ^» bo ia v5 ™ o o ..- .s ^z 3 *» ° ' )"Ci o — '"2 t. l- 8 o p, ^ .a ^-o 2 « 3'i ^ §.2 5 «» « •£ s* ^^ 3 e p 3 S « °-3 : — o&m 9 5^-,: o >. o — <*j rn p ^ , «j-5 c cKjatS: Pi £=. m sffi o;z «Z - — u * » S ^■3£°«t O tj (3 ™ ,«8 — .8 p,> ^_>> i S3 c S(j bio o u 2 ti s;^ -s > S S o u S "si *^ ■« *o ^ p. a S^r= d o, c <« S >,« ^.fs O =1 K| C?o | 8. P.O ■o.S 3 - CS 3 o m "ho c ° s S "^ 4S« x ho « » a; m o ja" S 3 u 3 5 ^ o fcH .*^ o « ■a, s-d « D " J "T S 3 S 2.2 K ja rt ho ^ ^ 4J U S3 S 3 ho Bs U ''3 1-. "3 « .s ^ a ^ •o B c rt 5 d 73 c4 u QJ a .2 3 3-2 a 3 g 0 PROTEINS. 117 MODEL CHART FOR REVIEW PURPOSES. Protein. Solubility. H O "o U g 0 u Oh Precipitation Tests. Salting. out Tests. a 0 1 5 0 EC >< Xt c 0 -. 3 CO a 0 'J u V D 0 u X •*. 0 u z ■*. 10 0 0 a 0 a 0 U O 0 a 0 O 72 " "o .c 0 5 •"3 . >■< 2 .a Potassio- mercuric Iodide + HC1. Picric Acid. Trichloracetic Acid. * O CO X Z 0 n 2 Albumin. Globulin. 1 Protean. j Acid metaprotein. Alkali metaprotein. Proteose. — — Peptone. Coagulated protein. 1 " Unknown " Mixtures and Solutions of Proteins. At this point the student's knowledge of the characteristics of the various proteins studied will be tested by requiring him to examine several "unknown" protein mixtures or solutions and make full report upon the same. The scheme given on page 116 may be used in this examination. CHAPTER VI. GASTRIC DIGESTION. Gastric digestion takes place in the stomach and is promoted by the gastric juice, which is secreted by the glands of the stomach mucosa. These glands are of two kinds, fundus glands and pyloric glands which are situated, as their names imply, in the regions of the fundus and pylorus. The principal foods acted upon in gastric digestion are the proteins which are so changed by its pro- cesses as to become better prepared for further digestion in the intestine and for their final absorption. From reliable experiments made upon lower animals it is evident that the gastric juice is secreted as the result of stimuli of two forms, i. e., psychical stimuli and chemical stimuli. The psychical form of stimuli may be produced by the sight, thought or taste of food, and the chemical stimuli may be produced by certain substances such as water, the extractives of meat, etc., when com- ing in contact with the stomach mucosa. The volume of gastric juice secreted during any given period of digestion, varies with the quantity and kind of the food. These conclusions were deduced principally from a series of so-called delusive feeding experiments. A dog was prepared with two oesophageal openings and a gastric fistula. When thus prepared and fed foods of various kinds such as meat and bread, the material instead of passing to the stomach, would invariably find its way out of the animal's body at the upper oesophageal opening. Through the medium of the gastric fistula the course of the secretion of gastric juice could be carefully followed. It was found that when the dog ate meat, for example, there was a large secretion of gastric juice notwithstanding no por- tion of the food eaten had reached the stomach. Further experi- ments made through the medium of a cul-de-sac formed from the stomach wall have given us many valuable conclusions, among others those regarding the influence of the chemical stimuli. The method followed was to feed the animal certain substances and note the secretion of gastric juice in the miniature stomach while the real process of digestion was taking place in the stomach proper. Normal gastric juice is a thin, light colored fluid which is acid 118 GASTRIC DIGESTION. 119 in reaction and has a specific gravity varying between i.ooi and 1. 010. It contains only 2-3 per cent of solid matter which is made up principally of hydrochloric acid, sodium chloride, potassium chloride, earthy phosphates, mucin and the enzymes pepsin, gastric rennin and gastric lipase; the hydrochloric acid and the enzymes are of the greatest importance. The acidity of the gastric juice is due to free hydrochloric acid which is secreted by the parietal cells of the fundus as well as by the chief cells of both the fundus and pyloric glands, and, in man, is generally present to the extent of 0.2-0.3 per cent. When the amount of hydrochloric acid varies to any considerable degree from these values a condition of hypoacidity or hyperacidity is established. Hydrochloric acid has the power of combining with protein substances taken in the food, thus forming so-called combined hydrochloric acid. This combined acid is a less potent germicide than free hydrochloric acid and has less power to destroy the amylolytic enzyme salivary amylase (ptyalin) of the saliva. This last fact explains to a degree the possibility of the continuance of salivary digestion in the stomach. The hydrochloric acid of the gastric juice forms a medium in which the pepsin can most satisfactorily digest the protein food, and at the same time it acts as an antiseptic or germicide which prevents putrefactive processes in the stomach. It also possesses the power of inverting cane sugar, this property being due to the hydrogen ion. When the hydrochloric acid of the gastric juice is diminished in quan- tity (hypoacidity) or absent, as it may be in many cases of func- tional or organic disease, there is no check to the growth of micro- organisms in the stomach. There are however certain of the more resistant spores which even the normal acidity of the gastric juice will not destroy. A condition of hypoacidity may also give rise to fermentation with the formation of comparatively large amounts of such substances as lactic acid and butyric acid. The question of the origin of the hydrochloric acid of the gastric juice is a problem to whose solution many investigators have given much attention. Many theories have been proposed, among them being Bunge's mass action theory, Koppe's electrolytic dissociation theory, and the more recent theory based upon the interaction of sodium chloride and lactic acid. We cannot go into a discussion of these various theories. Each of them has met with objection and we have, as yet, no generally accepted theory as to the origin of the hydrochloric acid of the gastric juice. That this hydrochloric acid originates from the chlorides of the blood is apparently a well 120 PHYSIOLOGICAL CHEMISTRY. established fact, but farther than this no positive statement can be made. The most important of the enzymes of the gastric juice is the proteolytic enzyme pepsin. The pepsin does not originate as such in the gastric cells but is formed from its precursor the zymo- gen or mother-substance pepsinogen which is produced by the parietal cells of the fundus as well as by the chief cells of the fun- dus and pyloric glands. Upon coming in contact with the hy- drochloric acid of the secretion this pepsinogen is immediately transformed into pepsin. Pepsin is not active in alkaline or neu- tral solutions but requires at least a faint acidity before it can exert its power to dissolve and digest proteins. The percentage of hydrochloric acid facilitating the most rapid peptic action varies with the character of the protein acted upon, e. g., 0.08 per cent to 0.1 per cent for the digestion of fibrin and 0.25 per cent for the di- gestion of coagulated egg-white. While hydrochloric acid is the acid usually employed to promote artificial peptic proteolysis, other acids, organic and inorganic, will serve the same purpose. Acidity of the liquid is necessary to promote the activity of the pepsin, but the acidity need not necessarily be confined to hydrochloric acid. In common with many other enzymes pepsin acts best at about 38°-40° C. and its digestive power decreases as the temperature is lowered, the enzyme being only slightly active at o° C. Its power is only temporarily inhibited by the application of such low temperatures, however, and the enzyme regains its full proteo- lytic power upon raising the temperature to 40 ° C. As the tempera- ture of a digestive mixture is raised above 400 C. the pepsin grad- ually loses its activity until at about 8o°-ioo° C. its proteolytic power is permanently destroyed. Our ideas regarding the nature of the products formed in the course of peptic proteolysis have undergone considerable revision in recent years. The former view that these products included only acid albuminate (acid metaprotein), proteoses and peptones is no longer tenable. From the investigations of numerous ob- servers we have learned that artificial gastric digestion if permitted to proceed for a sufficiently long period will yield, in addition to proteoses and peptones, a long list of protein cleavage products which are crystalline in character, including leucine, tyrosine, alanine, phenylalanine, aspartic acid, glutamic acid, proline, leucinimide, valine and lysine. A similar group of substances may result from GASTRIC DIGESTION. I 2 I the action of the enzyme trypsin (see p. 141). The relative amounts of proteoses, peptones and crystalline substances formed depends to a great extent upon the character of the protein undergoing digestion, e. g., a greater proportion of proteoses results from the digestion of fibrin than from the digestion of coagulated egg-white. We must not be led into the error of thinking that the large num- ber of protein cleavage products just mentioned are formed in the course of normal gastric digestion within the animal organism. They are formed only after comparatively long-continued hydroly- sis. In pancreatic digestion, however, there are formed even under normal conditions, the large number of cleavage products to which reference has been made. Peptic proteolysis therefore, within the animal organism differs from tryptic proteolysis (see page 141) in that the former yields larger amounts of proteoses, smaller amounts of peptones and no considerable quantity of crystalline bodies as end-products in the brief period during which proteins are ordinarily subjected to gastric digestion. Prolonged hydrolysis with gastric juice does, however, yield considerable quantities of the non-pro- tein end-products. Gastric rennin, the second enzyme of the gastric juice, is what is known as a milk curdling or protein coagulating enzyme. Rennin acts upon the caseinogen of the milk, splitting it into a proteose- like body and soluble casein. This soluble body, in the presence of calcium salts, combines with calcium, forming calcium casein or true casein which is insoluble and precipitates. There is some uncertainty regarding the reaction to litmus in which gastric rennin shows the greatest activity. It is, however, said to be active in neutral, alkaline or acid solution. However, it probably pos- sesses its greatest activity in the presence of a slight acid reaction, as would naturally be expected. It is especially abundant in the gastric mucosa of the calf, and is used to curdle the milk used in cheese making. Gastric rennin is always present normally in the gastric juice but in certain pathological conditions such as atrophy of the mucosa, chronic catarrh of the stomach or in carcinoma it may be absent. The theory that the proteolytic activity and the milk curdling property of the gastric juice reside in a single molecule is causing much controversy at the present time. The theory was originally advanced by the Pawlow school. Gastric lipase, the third enzyme of the gastric juice, is a fat- splitting enzyme. It possesses but slight activity when the gastric 122 PHYSIOLOGICAL CHEMISTRY. juice is of normal acidity, but evinces its action principally at such times as a gastric juice of low acidity is secreted either from physiological or pathological cause. The digestion of fat in the stomach is, however, at most, of but slight importance as com- pared with the digestion of fat in the intestine through the action of the lipase of the pancreatic juice (see page 143). PREPARATION OF AN ARTIFICIAL GASTRIC JUICE. Dissect the mucous membrane of a pig's stomach from the mus- cular portion and discard the latter. Divide the mucous membrane into two parts (4/5 and 1/5). Cut up the larger portion, place it in a large-sized beaker with 0.4 per cent hydrochloric acid and keep at 38°-40° C. for at least 24 hours. Filter off the residue, consisting principally of nuclein and anti-albumid, and use the filtrate as an artificial gastric juice. This filtrate contains pepsin, rennin and the products of the digestion of the stomach tissue, i. e., acid metaprotein (acid albuminate), proteoses, peptones, etc. Preparation of a Glycerol Extract of Pig's Stomach. Take the one-fifth portion of the mucous membrane of the pig's stomach not used in the preparation of the artificial gastric juice, cut it up very finely, place it in a small-sized beaker and cover the membrane with glycerol. Stir frequently and allow to stand at room temperature for at least 24 hours. The glycerol will extract the pepsinogen. Separate, with a pipette or by other means, the glycerol from the pieces of mucous membrane and use the glycerol extract as required in the later experiments. Products of Gastric Digestion. Into the artificial gastric juice, prepared as above described, place the protein material (fibrin, coagulated egg-white, or lean beef) provided for you by the instructor, add 0.4 per cent hydro- chloric acid as suggested by the instructor and keep the digestion mixture at 400 C. for 2 to 3 days. Stir frequently and keep free hydrochloric acid present in the solution (for tests for free hydro- chloric acid see p. 123). The original protein has been digested and the solution now con- tains the products of peptic proteolysis, i. e., acid metaprotein (acid albuminate), proteoses, peptones, etc. The insoluble residue may include nuclein and anti-albumid. Filter the digestive mixture and GASTRIC DIGESTION. I 23 after testing for free hydrochloride acid neutralize the filtrate with potassium hydroxide solution. If any of the acid metaprotein (acid albuminate) is still untransformed into proteoses it will precipitate upon neutralization. If any precipitate forms heat the mixture to boiling, and filter. If no precipitate forms proceed without fil- tering. We now have a solution containing a mixture consisting princi- pally of proteoses and peptones. Separate and identify the pro- teoses and peptones according to the directions given on pages 114 and 115. Tests for Free and Combined HC1. These tests are made with a class of reagents known as indicators, so-called because they serve to indicate the nature of the reaction of a solution. These indicators are weak acids or bases and are but slightly dissociable. The dissociation, with the formation of the colored ion, forms the basis for the color reaction. Examine each of the following solutions by means of the tests given below and report the results in a form similar to the chart given on page 125: (1) 0.2 per cent free hydrochloric acid. (2) 0.05 per cent free hydrochloric acid. (3) 0.01 per cent free hy- drochloric acid. (4) 0.05 per cent combined hydrochloric acid. (5) 1 per cent lactic acid. (6) Equal volumes of 0.2 per cent free hydrochloric acid and 1 per cent lactic acid. (7) 1 per cent potas- sium hydroxide. 1. Dimethyl-amino-azobenzene (or Topfer's Reagent),1 N(CH3)2-C6H4-N = N-C6H5. Place 1-2 drops of the reagent in the solution to be tested. Free mineral acid (hydrochloric acid) is indicated by the production of a pinkish-red color. If free acid is absent a yellow color ordinarily results. 2. Giinzberg's Reagent.2 — Place 1-2 drops of the reagent in a small porcelain evaporating dish and carefully evaporate to dryness over a low flame. Insert a glass stirring rod into the mixture to be tested and draw the moist end of the rod through the dried reagent. Warm again gently and note the production of a purplish-red color in the presence of free hydrochloric acid. lTo prepare Topfer's reagent dissolve 0.5 gram of di-methyl-amino-azobenzene in 100 c.c. of 95 per cent alcohol. "Giinzberg's reagent is prepared by dissolving 2 grams of phloroglucin and 1 gram of vanillin in 100 c.c. of 95 per cent alcohol. 124 PHYSIOLOGICAL CHEMISTRY. 3. Boas' Reagent.1 — Perform this test in the same manner as 2, p. 123. Free hydrochloric acid is indicated by the production of a rose-red color, which becomes less pronounced on cooling. 4. Congo Red,2 NH, SO,Na 'x A/' N=N<_><__>N=N 'x S08Na NH2 Conduct this test according to the directions given under 1 or 2, page 123. A blue color indicates free hydrochloric acid, a violet color indicates an organic acid and a brown color indicates com- bined hydrochloric acid. Congo red paper, made by immersing ordinary filter paper in the indicator and subsequently drying, may be used in this test. 5. Tropaeolin OO,3 NH(C6HB) -C6H4-N = N-C6H4-S03Na. Place 2 drops of the solution to be tested and 1 drop of the indicator in an evaporating dish and evaporate to dryness over a low flame. The formation of a reddish-violet color indicates free hydrochloric acid. This test may also be conducted in the same manner as 2, page 123. 6. Phenolphthalein,4 C6H4OH / C-C6H4OH /"\ C6H4 0 \/ C \ 0 Add the indicator directly to the solution, or apply the test ac- 1 Boas' reagent is prepared by dissolving 5 grams of resorcin and 3 grams of sucrose in 100 c.c. of 95 per cent alcohol. - This indicator is prepared by dissolving 0.5 gram of congo red in 90 c.c. of water and adding 10 c.c. of 95 per cent alcohol. 3 Prepared by dissolving 0.05 gram of tropaeolin OO in 100 c.c. of 50 per cent alcohol. * This indicator is prepared by dissolving 1 gram of phenolphthalein in 100 c.c of 95 per cent alcohol. GASTRIC DIGESTION. 125 cording to the directions given under 2 on page 123. This indicator serves to denote the total acidity since it is acted upon by free min- eral acids, combined acids, organic acids and acid salts. A red color indicates the presence of an alkali and the indicator is colorless in the presence of a neutral or acid reaction. This indicator is unsatisfactory in the presence of ammonia. 7. Sodium Alizarin Sulphonate,1 CO (OH), / \ / CGH4 CGH \ / \ CO SOJSTa This indicator may be used directly in the solution to be tested, or the test may be applied as 2, page 123. It serves to indicate all acid reactions except those due to combined acids. A reddish-violet color indicates an alkaline reaction, while a yellow color indicates an acid reaction due to a free mineral acid, an organic acid or an acid salt. Report the results of your tests tabulated in the form given below : Name of Indicator. Solutions Examined. 0.2 $ HC1. 0.05 % HU. O.OI <& HC1. 0.0s $ 1 1 a EciuaJ vols. Combined Lactic 1 o.s*HU x* HO. Acid. T an.d '/< KOH. Lactic Acid. Topfer's Reagent. Giinzberg's Reagent. Boas' Reagent. Congo Red. Tropseolin OO. Phenolphthalein. j Alizarin. 1 GENERAL EXPERIMENTS ON GASTRIC DIGESTION. I. Conditions Essential for the Action of Pepsin. — Prepare four test-tubes as follows : (a) Five c.c. of pepsin solution. 1 Prepare this indicator by dissolving i gram of sodium alizarin sulphonate in ioo c.c. of water. 126 PHYSIOLOGICAL CHEMISTRY. (b) Five c.c. of 0.4 per cent hydrochloric acid. (c) Five c.c. of pepsin-hydrochloric acid solution. (d) Two or three c.c. of pepsin solution and 2-3 c.c. of 0.5 per cent sodium carbonate solution. Introduce into each tube a small piece of fibrin and place them on the water-bath at 400 C. for one-half hour, carefully noting any changes which occur.1 Now combine the contents of tubes (a) and (b) and see if any further change occurs after standing at 400 C. for 15-20 minutes. Explain the results obtained from these five experiments. 2. Influence of Different Temperatures. — In each of four test- tubes place 5 c.c. of pepsin-hydrochloric acid solution. Immerse one tube in cold water from the faucet, keep a second tube at room temperature and place a third on the water-bath at 400 C. Boil the contents of the fourth tube for a few moments, then cool and also keep it at 40 ° C. Into each tube introduce a small piece of fibrin and note the progress of digestion. In which tube does the most rapid digestion occur? Explain this. 3. The Most Favorable Acidity. — Prepare three tubes as follows : (a) Five c.c. of 0.2 per cent pepsin-hydrochloric acid solution. (b) Two or three c.c. of 0.2 per cent hydrochloric acid -f- 1 c.c. of concentrated hydrochloric acid -j- 5 c.c. of pepsin solution. (c) One c.c. of 0.2 per cent pepsin-hydrochloric acid solution -f- 5 c.c. of water. Introduce a small piece of fibrin into each tube, keep them at 400 C, and note the progress of digestion. In which degree of acidity does the fibrin digest the most rapidly? 4. Differentiation Between Pepsin and Pepsinogen. — Prepare five tubes as follows : (a) Few drops of glycerol extract of pepsinogen -f- 2-3 c.c. of water. (b) Few drops of glycerol extract of pepsinogen -f- 5 c.c. of 0.2 per cent hydrochloric acid. 1 Digestion of fibrin in a pepsin-hydrochloric acid solution is indicated first by a swelling of the protein due to the action of the acid, and later by a disintegra- tion and dissolving of the fibrin due to the action of the pepsin-hydrochloric acid. If uncertain at any time whether digestion has taken place, the solution under examination may be filtered and the biuret test applied to the filtrate. A positive reaction will signify the presence of acid metaprotein (acid albuminate), pro- teoses (albumoses) or peptones, the presence of any one of which would indi- cate that digestion has taken place. GASTRIC DIGESTION. I 2J (c) Few drops of glycerol extract of pepsinogen -f- 5 c.c. of 0.5 per cent sodium carbonate. (d) Two or three c.c. of pepsin solution -f- 2-3 c.c. of 1 per cent sodium carbonate. (?$C 0.1' IB Bc^ -• SKKM ^tagBpS,'- %'M '&/ 7m |fe Mutton Fat. (Long.) " carbon moiety " of protein material. The formation of adipocere and the occurrence of fatty degeneration are sometimes given as proofs of the formation of fat from protein. This is questioned by many investigators. Rather more satisfactory and direct proof of the formation of fat from protein material has been obtained by Hofmann in experimentation with fly-maggots. The normal content of fat in a number of maggots was determined and later the fat content of others which had developed in blood (84 per cent of the solid matter of blood plasma is protein material) was determined. The fat content was found to have increased 700 to 1 100 per cent as a result of the diet of blood proteins. The cele- brated experiments of Pettenkofer and Voit, however, have fur- nished what is, perhaps, the most substantial positive evidence of the formation of fat from protein. These investigators fed dogs large amounts of lean meat, daily, and through subsequent urinary and fecal examinations were enabled to account for only part of the ingested carbon, although obtaining a satisfactory nitrogen balance. The discrepancy in the carbon balance was explained upon the theory that the protein of the ingested meat had been split into a nitrogenous and a non-nitrogenous portion in the organ- ism, and that the non-nitrogenous portion, the so-called " carbon FATS. I 3 5 moiety" of the protein, had been subsequently transformed into fat and deposited as such in the tissues of the organism. Some in- vestigators are not inclined to accept these data regarding the for- mation of fat from protein as conclusive. The latest evidence in favor of the formation of fat from pro- tein is furnished by the very recently reported experiments of Weinland. This investigator worked with the larva? of Calliphora,1 these larvae being rubbed up in a mortar" with Witte's peptone and water to form a homogeneous mixture. After placing these mix- tures at 380 C. for 24 hours the fat content was found to have increased, as much as 140 per cent in some instances. The active agency in this transformation of fat is the larval tissue since the tissues of both the dead and living larvae possess the property. Data are given from control tests which show that the action of bacteria in this transformation of protein was excluded. Experiments on Fats. 1. Solubility. — Test the solubility of olive oil in each of the ordinary solvents (see page 23) and in cold alcohol, hot alcohol, chloroform, ether, and carbon tetrachloride. 2. Formation of a Transparent Spot on Paper. — Place a drop of olive oil upon a piece of ordinary writing paper. Note the trans- parent appearance of the paper at the point of contact with the fat. 3. Reaction. — Try the reaction of fresh olive oil to litmus. Repeat the test with rancid olive oil. What is the reaction of a fresh fat and how does this reaction change upon allowing the fat to stand for some time? 4. Formation of Acrolein. — To a little olive oil in a mortar add some dry potassium bisulphate, KHS04, and rub up thor- oughly. Transfer to a dry test-tube and cautiously heat. Note the irritating odor of acrolein. The glycerol of the fat has been dehydrolyzed and acrylic aldehyde or acrolein has been produced. This is the reaction which takes place : CH2OH CHO CH-OH -> CH + 2PLO. CH2-OH CH2 Glycerol. Acrolein. 1 The ordinary " blow-fly." 2 Intact larvse were used in some experiments. 136 PHYSIOLOGICAL CHEMISTRY. 5. Emulsification. — (a) Shake up a drop of neutral1 olive oil with a little water in a test-tube. The fat becomes finely divided, forming an emulsion. This is not a permanent emulsion since the fat separates and rises to the top upon standing. (b) To 5 c.c. of water in a test-tube add 2 or 3 drops of 0.5 per cent Na2C03. Introduce into this faintly alkaline solution a drop of neutral olive oil and shake. The emulsion while not per- manent is not so transitory as in the case of water free from sodium carbonate. (c) Repeat (b) using rancid olive oil. What sort of an emul- sion do you get and why? (d) Shake a drop of neutral olive oil with a dilute albumin solution. What is the nature of this emulsion? Examine it under the microscope. 6. Fat Crystals. — Dissolve a small piece of lard in ether in a test-tube, add an equal volume of alcohol and allow the alcohol- Fig. 37. Pork Fat. ether mixture to evaporate spontaneously. Examine the crystals under the microscope and compare them with those reproduced in Figs. 35, 36 and 37, on pages 131, 134 and 136. 7. Saponification of Bayberry Tallow.2 — Fill a large casserole 1 Neutral olive oil may be prepared by shaking ordinary olive oil with a 10 per cent solution of sodium carbonate. This mixture should then be extracted with ether and the ether removed by evaporation. The residue is neutral olive oil. 2 Bayberry tallow is derived from the fatty covering of the berries of the wax myrtle. It is therefore frequently called " myrtle wax " or " bayberry wax." FATS. 137 two-thirds full of water rendered strongly alkaline with solid potas- sium hydroxide (a stick one inch in length). Add about 10 grams of bayberry tallow and boil, keeping the volume constanl by adding water as needed. When saponification is complete1 remove 25 c.c. of the soap solution for use in Experiment 8 and add concentrated hydrochloric acid slowly to the remainder until no further precipi- tate is produced.2 Cool the solution and the precipitate of free fatty acid will rise to the surface and form a cake. In this instance the fatty acid is principally palmitic acid. Remove the cake, break it into small pieces, wash it with water by clecantation and transfer Fig. -8. Palmitic Acid. to a small beaker by means of 95 per cent alcohol. Heat on a water-bath until the palmitic acid is dissolved, then filter through a dry filter paper and allow the filtrate to cool slowly in order to obtain satisfactory crystals. ^Trite the reactions which have taken place in this experiment. When the palmitic acid has completely crystallized filter off the alcohol, dry the crystals between filter papers and try the tests given in Experiment 9, p. 138. 8. Salting-out Experiment. — To 25 c.c. of soap solution, pre- pared as described above, add solid sodium chloride to the point of saturation, with continual stirring. A menstruum is thus 1 Place 2 or 3 drops in a test-tube full of water. If saponification is complete the products will remain in solution and no oil will separate. 2 Under some conditions a purer product is obtained if the soap solution is cooled before precipitating the fatty acid. 138 PHYSIOLOGICAL CHEMISTRY. Fig. 39. formed in which the soap is insoluble. This salting-out process is entirely analogous to the salting-out of proteins (see page 99). 9. Palmitic Acid. — (a) Examine the crystals under the micro- scope and compare them with those shown in Fig. 38, p. 137. (b) Solubility. — Try the solubility of palmitic acid in the same solvents as used on fats (see page 135). (c) Melting-Point. — Determine the melting-point of palmitic acid by one of the methods given on page 139. (d) Formation of Transparent Spot on Paper. — Melt a little of the fatty acid and allow a drop to fall upon a piece of ordinary writing paper. How does this compare with the action of a fat under similar circumstances ? (e) Acrolein Test. — Apply the test as given under 4, page 135. Explain the result. 10. Saponification of Lard. — To 25 grams of lard in a flask add 75 c.c. of alcoholic-potash solution and warm upon a water-bath until saponi- fication is complete. (This point is indicated by the complete solubility of a drop of the solution when allowed to fall into a little water.) Now trans- fer the solution from the flask to an evaporating' dish containing about 100 c.c. of water and heat on a water-bath until all the alcohol has been driven off. Precipitate the fatty acid with hydrochloric acid and cool the solution. Remove the fatty acid which rises to the surface, neu- tralize the solution with sodium carbonate and evaporate to dryness. Extract the residue with alcohol, remove the alcohol by evaporation upon a water-bath and on the residue of glycerol thus obtained make the tests as given below. 11. Glycerol, (a) Taste. — What is the taste of glycerol? (b) Solubility. — Try the solubility of glycerol in water, alcohol and ether. (c) Acrolein Test. — Repeat the test as given under 4, page 135. Melting-Point Apparatus. FATS. 139 ((/) Borax Fusion Test. — Fuse a little glycerol on a platinum wire with some powdered borax and note the characteristic green flame. This color is due to the glycerol ester of boric acid. (e) Fehling's Test. — How does this result compare with the results on the sugars? (/) Solution of Cu(OH)2. — Form a little cupric hydroxide by mixing cupric sulphate and potassium hydroxide. Add a little glycerol to this suspended precipitate and note what occurs. 12. Melting-Point of Fat. First Method. — Insert one of the melting-point tubes, furnished by the instructor, into the liquid fat and draw up the fat until the bulb of the tube is about one-half full of the material. Then fuse one end of the tube in the flame of a bunsen burner and fasten the tube to a thermometer by means of a rubber band in such a manner that the bottom of the fat column is on a level with the bulb of the thermometer (Fig. 39, page 138). Fill a beaker of medium size about two-thirds full of water and place it within a second larger beaker which also contains water, the two vessels being separated by pieces of cork. Immerse the bulb of the thermometer and the attached tube in such a way that the bulb is about midway between the upper and the lower surfaces of the water of the inner beaker. The upper end of the tube being open it must extend above the surface of the surround- ing water. Apply gentle heat, stir the water, and note the tem- perature at which the fat first begins to melt. This point is indicated by the initial transparency. For ordinary fats, raise the temperature very cautiously from 300 C. To determine the con- gealing-point remove the flame and note the temperature at which the fat begins to solidify. Record the melting- and congealing- points of the various fats submitted by the instructor. Second Method. — Fill a small evaporating dish about one-half full of mercury and place it on a water-bath. Put a small drop of the fat under examination on an ordinary cover glass and place this upon the surface of the mercury. Raise the temperature of the water-bath slowly and by means of a thermometer whose bulb is immersed in the mercury, note the melting-point of the fat. Determine the congealing-point by removing the flame and leaving the fat drop and cover glass in position upon the mercury. How do the melting-points as determined by this method compare with those as determined by the first method? Which method is the more accurate, and why? CHAPTER VIII. PANCREATIC DIGESTION. As soon as the food mixture leaves the stomach it comes into intimate contact with the bile and the pancreatic juice. Since these fluids are alkaline in reaction there can obviously be no further peptic activity after they have become intimately mixed with the chyme and have neutralized the acidity previously imparted to it by the hydrochloric acid of the gastric juice. The pancreatic juice reaches the intestine through the duct of Wirsung which opens into the intestine near the pylorus. Normally the secretion of pancreatic juice is brought about by the stimulation produced by the acid chyme as it enters the duodenum. This secretion is probably not due to a nervous reflex as was believed by Pawlow but rather, as Bayliss and Starling have shown, is de- pendent upon the presence, in the epithelial cells of the duodenum and jejunum of a body known as prosecretin. This body is changed into secretin1 through the hydrolytic action of the acid present in the chyme. The secretin is then absorbed by the blood, passes to the pancreas and stimulates the pancreatic cells, causing a flow of pancreatic juice. The quantity of juice secreted under these con- ditions is proportional to the amount of secretin present. The ac- tivity of secretin solutions is not diminished by boiling, hence the body does not react like an enzyme. Further study of the body may show it to be a definite chemical individual of relatively low molecular weight. It has not been possible thus far to obtain secre- tin from any tissues except the mucous membrane of the duodenum and jejunum. The juice as obtained from a permanent fistula differs greatly in its properties from the juice as obtained from a temporary fistula, and neither form of fluid possesses the properties of the normal fluid. Pancreatic juice collected by Glaessner from a natural fistula has been found to be a colorless, clear, strongly alkaline fluid which foams readily. It is further characterized by containing albumin, 1 Secretin belongs to the class of substances called hormones or chemical messengers. 140 PANCREATIC DIGESTION. 141 globulin, proteose and peptone ; nuclei ipr< >tein isalsi 1 presenl in 1 races. The average daily secretion of pancreatic juice is 650 c.c. and it- specific gravity is 1.00S. The fluid contains 1.3 per cent of solid matter and the freezing-point is — 0.470 C. The normal pancreatic secretion contains at least four distinct enzymes. They are trypsin, a proteolytic enzyme ; pancreatic amylase (amyl< ipsin) , an amyli >lyi ic enzyme; pancreatic lipase (steapsin), a fat-splitting enzyme: and. pancreatic renniu, a milk-coagulating enzyme. Lactase, the lactose- splitting enzyme, is also present at certain times. The most important of the four enzymes of the pancreatic juice is the proteolytic enzyme trypsin. This enzyme resembles pepsin in so far as each has the power of breaking down protein material, but the trypsin has much greater digestive power and is able to cause a more complete decomposition of the complex protein molecule. In the process of normal digestion the protein constituents of the diet are for the most part transformed into proteoses (albumoses) and peptones before coming in contact with the enzyme trypsin. This is not absolutely essential however, since trypsin possesses digestive ac- tivity sufficient to transform unaltered native proteins and to produce from their complex molecules comparatively simple fragments. Among the products of tryptic digestion are proteoses, peptones, peptides, leucine, tyrosine, aspartic acid, glutamic acid, alanine, phen- ylalanine, glycocoll, cystine, serine, valine, proline, oxyproline, iso- leucine, arginine, lysine, histidine and tryptophane. (The crystalline forms of many of these products are reproduced in Chapter IV.) Trypsin does not occur preformed in the gland, but exists there as a zymogen called tripsinogen which bears the same relation to trypsin that pepsinogen does to pepsin. Trypsin has never been obtained in a pure form and therefore very little can be stated definitely as to its nature. The enzyme is the most active in alkaline solution but is also active in neutral or slightly acid solutions. Trypsin is destroyed by mineral acids and may also be destroyed by comparatively weak alkali (2 per cent sodium carbonate) if left in contact for a sufficiently long time. Trypsinogen. on the other hand, is more resistant to the action of alkalis. In pancreatic di- gestion the protein does not swell as is the case in gastric digestion, but becomes more or less " honeycombed " and finally disintegrates. The pancreatic juice which is collected by means of a fistula possesses practically no power to digest protein matter. A body called euterokinase occurs in the intestinal juice and has the power ^laessner: Zeitschrift fiir physiologische Chemie, 1904. 40. p. 476. 142 PHYSIOLOGICAL CHEMISTRY. of converting tripsinogen into trypsin. This process is known as the " activation " of trypsinogen and through it a juice which is incapable of digesting protein may be made active. Enterokinase is not always present in the intestinal juice since it is secreted only after the pancreatic juice reaches the intestine. It resembles the enzymes in that its activity is destroyed by heat, but differs mate- rially from this class of bodies in that a certain quantity is capable of activating only a definite quantity of trypsinogen. It is how- ever generally classified as an enzyme. Enterokinase has been de- tected in the higher animals, and a kinase possessing similar proper- ties has been shown to be present in bacteria, fungi, impure fibrin, lymph glands and snake-venom. The activation of trypsinogen into trypsin may be brought about in the gland as well as in the intestine of the living organism (Mendel and Rettger). The manner of the activation in the gland and the nature of the body causing it are unknown at present. Delezenne claims that trypsinogen may be activated by soluble calcium salts. He reports experiments which indicate that pro- teolytically inactive pancreatic juice, obtained directly from the duct, when treated with salts of this character assumes the property of digesting protein material. This process by which the trypsinogen is activated through the instrumentality of calcium salts is very rapid and is designated by Delezenne as an " explosion." The recent suggestion of Mays that there may possibly be several pre- cursors of trypsin one of which is activated by enterokinase and the others by other agents, is of interest in this connection. Pancreatic amylase (amylopsin) , the second of the pancreatic en- zymes, is an amylolytic enzyme which possesses somewhat greater digestive power than the salivary amylase (ptyalin) of the saliva. As its name implies, its activity is confined to the starches, and the products of its amylolytic action are dextrins and sugars. The sugars are principally iso-maltose and maltose and these by the further action of an inverting enzyme are partly transformed into dextrose. It is possible that the saliva as a digestive fluid is not absolutely essential. The salivary amylase (ptyalin) is destroyed by the hy- drochloric acid of the gastric juice and is therefore inactive when the chyme reaches the intestine. Should undigested starch be pres- ent at this point however, it would be quickly transformed by the active pancreatic amylase. This enzyme is not present in the pancreatic juice of infants during the first few weeks of life, thus PANCREATIC DIGESTION. 143 showing very clearly that a starchy diet is not normal for this period It has been claimed that pancreatic amylase has a slight digestive action upon unboiled starch. The third enzyme of the pancreatic juice is called pancreatic lipase (steapsin) and is a fat-splitting enzyme. It has the power of splitting the neutral fats of the food by hydrolysis, into fatty acid and glycerol. A typical reaction would be as follows : C3H5(a;C15H31CO)3+3H20 = 3(C15H31COOH)+C3H5(OH)3. Tri-palmitin. Palmitic acid. Glycerol. Recent researches make it probable that fats undergo saponifica- tion to a certain extent prior to their absorption. The fatty acids formed, in part unite with the alkalis of the pancreatic juice and intestinal secretion to form soluble soaps ; in part they are doubt- less absorbed dissolved in the bile. Some observers believe that the fats may also be absorbed in emulsion — a condition promoted by the presence of the soluble soaps. After absorption the fatty acids are re-synthesized to form neutral fats with glycerol. Pancreatic lipase is very unstable and is easily rendered inert by the action of acid. For this reason it is not possible to prepare an extract having a satisfactory fat-splitting power from a pancreas which has been removed from the organism for a sufficiently long time to have become acid in reaction. The fourth enzyme of the pancreatic juice is called pancreatic rennin. It is a milk-coagulating enzyme whose action is very similar to that of the enzyme gastric rennin found in the gastric juice. It is supposed to show its greatest activity at a temperature varying from 6o° to 65° C. The. enzymes of the intestinal juice are of great importance to the animal organism. These enzymes include crcpsin (erepsase), sue rase, maltose, lactase, and enterokinasc. Erepsin is a proteolytic enzyme which has the property of acting upon the proteoses and peptones which are formed through the action of trypsin and further splitting them into amino acids. Erepsin has no power of digesting any native proteins except caseinogen, histones and protamines. It possesses its greatest ac- tivity in an alkaline solution although it is slightly active in acid solution. An extract of the intestinal erepsin may be prepared by treating the finely divided intestine of a cat, dog, or pig with toluene- or chloroform-water and permitting the mixture to stand with oc- 144 PHYSIOLOGICAL CHEMISTRY. casional shaking for 24-72 hours.1 Enzymes similar to erepsin occur in various tissues of the organism. The three invertases sucrase, maltase and lactase are also im- portant enzymes of the intestinal mucosa. The sucrase acts upon sucrose and inverts it with the formation of invert sugar (dextrose and kevulose). Some investigators claim that sucrase is also present in saliva and gastric juice. It probably does not exist nor- mally in either of these digestive juices, however, and if found owes its presence to the excretory processes of certain bacteria. Sucrases may also be obtained from several vegetable sources. For investigational purposes it is ordinarily obtained from yeast (see p. 11). In exhibits its greatest activity in the presence of a slight acidity but if the acidity be increased to any extent the reac- tion is inhibited. Lactase is an enzyme which inverts lactose with the consequent formation of dextrose and galactose. Its action is entirely analo- gous, in type, to that of sucrase. It has apparently been proven that lactase occurs in the intestinal mucosa of the young of all animals which suckle their offspring.2 It may also occur in the intestinal mucosa of certain adult animals if such animals be main- tained upon a ration containing more or less lactose. Fischer and Armstrong have demonstrated the reversible action3 of lactase. For discussions of maltase and entcrokinase see pages 55 and 141 respectively. PREPARATION OF AN ARTIFICIAL PANCREATIC JUICE.4 After removing the fat from the pancreas of a pig or sheep, finely divide the organ by means of scissors and grind it in a mortar. If convenient, the use of an ordinary meat chopper is a very satis- factory means of preparing the pancreas. When finely divided as above the pancreas should be placed in a 500 c.c. flask, about 150 c.c. of 30 per cent alcohol added and the flask and contents shaken frequently for twenty-four hours. (What is the reaction of this alcoholic extract at the end of this period, and why?) Strain the alcoholic extract through cheese 1 See p. 13. "Mendel and Mitchell: American Journal of Physiology, 1907, XX, p. 81. sSee p. 6. 4 For other methods of preparation see Karl Mays : Zeitschrift fur phys- iologische Chemie, 1903, XXXVIII, p. 428. PANCREATIC DIGESTION. H5 cloth, filter, nearly neutralize with potassium hydroxide solution and then exactly neutralize it with 0.5 per cent sodium carl innate. Products of Tryptic Digestion. Take about 200 grams of lean beef which has been freed from fat and finely ground and place it in a large-sized beaker. Intro- duce equal volumes of the pancreatic extract prepared as above and 0.5 per cent sodium carbonate, add 5 c.c. of an alcoholic solu- tion of thymol to prevent putrefaction, and place the beaker in an incubator at 40 ° C. Stir the contents of the beaker frequently and add more thymol if it becomes necessary. Allow digestion to proceed for from 2 to 5 days and then separate the products formed as follows : Strain off the undissolved residue through cheese cloth, nearly neutralize the solution with dilute hydrochloric acid and then exactly neutralize it with 0.2 per cent hydrochloric acid. A precipitate at this point would indicate alkali metaprotein (alkali albuminate). Filter off any precipitate and divide the fil- trate into two parts, a one-fourth and a three-fourth portion. Transfer the one-fourth portion to an evaporating dish and make the separation of proteoses and peptones as well as the final tests upon these bodies according to the directions given on page 114. Place about 5 c.c. of the three-fourth portion in a test-tube and add about 1 c.c. of bromine water. A violet coloration indicates the presence of tryptophane (see page 73). Concentrate1 the remain- der of the three-fourth portion to a thin syrup and make the sep- aration of leucine and tyrosine according to the directions given on page 82. GENERAL EXPERIMENTS ON PANCREATIC DIGESTION. Experiments on Trypsin. 1. The Most Favorable Reaction for Tryptic Digestion. — Prepare seven tubes as follows : (a) 2-3 c.c. of neutral pancreatic extract -f- 2-3 c.c. of water. (6) 2-3 c.c. of neutral pancreatic extract -j- 2-3 c.c. of 1 per cent sodium carbonate. (c) 2-3 c.c. of neutral pancreatic extract -J- 2-3 c.c. of 0.5 per cent sodium carbonate. 1 If the solution is alkaline in reaction, while it is being concentrated, the amino acids will be broken down and ammonia will be liberated. I46 PHYSIOLOGICAL CHEMISTRY. (d) 2-3 c.c. of neutral pancreatic extract -f- 2-3 c.c. of 0.2 per cent hydrochloric acid. (e) 2-3 c.c. of neutral pancreatic extract + 2-3 c.c. of 0.2 per cent combined hydrochloric acid. (/) 2-3 c.c. of neutral pancreatic extract -.]- 2-3 c.c. of 0.4 per cent boric acid. (g) 2-3 c.c. of neutral pancreatic extract -f- 2-3 c.c. of 0.4 per cent acetic acid. Add a small piece of fibrin to the contents of each tube and keep them at 400 C. noting the progress of digestion. In which tube do we find the most satisfactory digestion, and why? How do the indications of the digestion of fibrin by trypsin differ from the indications of the digestion of fibrin by pepsin? 2. The Most Favorable Temperature. — (For this and the following series of experiments under tryptic digestion use the neutral extract plus an equal volume of 0.5 per cent sodium car- bonate.) In each of four tubes place 5 c.c. of alkaline pancreatic extract. Immerse one tube in cold water from the faucet, keep a second at room temperature and place a third on the water-bath at 400 C. Boil the contents of the fourth for a few moments, then cool and also keep it at 400 C. Into each tube introduce a small piece of fibrin and note the progress of digestion. In which tube does the most rapid digestion occur? What is the reason? 3. Influence of Metallic Salts, etc. — Prepare a series of tubes and into each tube place 6 volumes of water, 3 volumes of alkaline pancreatic extract and 1 volume of one of the chemicals listed in Experiment 18 under Salivary Digestion, page 59. Introduce a small piece of fibrin into each of the tubes and keep them at 40 ° C. for one-half hour. Shake the tubes frequently. In which tubes do we get the least digestion ? 4. Influence of Bile. — Prepare five tubes as follows : (a) Five c.c. of pancreatic extract -j- J^-i c.c. of bile. (b) Five c.c. of pancreatic extract ~f- 1-2 c.c. of bile. (c) Five c.c. of pancreatic extract -j- 2-3 c.c. of bile. (d.) Five c.c. of pancreatic extract -j- 5 c.c. of bile. (H7COO ■ C2H5, and a small amount of litmus powder. To the contents of one tube add 4 c.c. of neutral pancreatic extract and to the contents of the other tube add 4 c.c. of water or boiled neutral pancreatic extract. Keep the tubes at 400 C. and observe any changes which may occur. What is the result and how do you explain it? Write the equation for the reaction which has taken place. Experiments on Pancreatic Rennin. Prepare four test-tubes as follows : (a) Five c.c. of milk -\- 10 drops of neutral pancreatic extract. (7?) Five c.c. of milk -j- 20 drops of neutral pancreatic extract. (c) Five c.c. of milk -j- 10 drops of alkaline pancreatic extract. (d) Five c.c. of milk -\- 20 drops of alkaline pancreatic extract. Place the tubes at 6o°-65° C. for a half hour without shaking. Note the formation of a clot.1 How does the action of pancreatic rennin compare with the action of the gastric rennin? 1 This reaction will not always succeed, owing to conditions which are not well understood. CHAPTER IX BILE. The bile is secreted continuously by the liver and passes into the intestine through the common bile duct which opens near the pylorus. Bile is not secreted continuously into the intestine. In a fasting animal no bile enters the intestine, but when food is taken the bile begins to flow ; the length of time elapsing between the ingestion of the food and the secretion of the bile as well as the qualitative and quantitative characteristics of the secretion de- pending upon the nature of the food ingested. Fats, the extrac- tives of meat and the protein end-products of gastric digestion, (proteoses and peptones) cause a copious secretion of bile, whereas such substances as water, acids and boiled starch paste fail to do so. In general a rich protein diet is supposed to increase the amount of bile secreted, whereas a carbohydrate diet would cause a much less decided increase and might even tend to decrease the amount. It has been demonstrated by Bayliss and Starling that the secretion of bile is under the control of the same mechanism that regulates the flow of pancreatic juice (see p. 140). In other words, the hydrochloric acid of the chyme, as it enters the duodenum transforms prosecretin into secretin and this in turn enters the circulation, is carried to the liver and stimulates the bile-forming mechanism to increased activity. We may look upon the bile as an excretion as well as a secretion. In the fulfillment of its excretory function it passes such bodies as lecithin, metallic substances, cholesterol and the decomposition products of haemoglobin into the intestine and in this way aids in re- moving them from the organism. The bile assists materially in the absorption of fats from the intestine by its solvent action on the fatty acids formed by the action of the pancreatic juice. The bile is a ropy, viscid substance which is alkaline in reaction to litmus,1 and ordinarily possesses a decidedly bitter taste. It varies in color in the different animals, the principal variations being yellow, brown and green. Fresh human bile from the living organism ordinarily has a green or golden-yellow color. Post- 1 It does not contain any free hydroxyl ions, however. 150 BILE. I 5 [ mortem bile is variable in color. It is very difficult to determine accurately the amount of normal bile secreted during any given period. For an adult man it lias been variously estimated at from 500 c.c. to 1 100 c.c. for twenty-four hours. The specific' gravity of the bile varies between 1.010 and 1.040, and the freezing-point is about — 0.560 C. As secreted by the liver, the bile is a clear, limpid fluid which contains a relatively low content of solid matter. Such bile would have a specific gravity of approximately 1.010. After it reaches the gall-bladder, however, it becomes mixed with mucous material from the walls of the gall-bladder, and this proc- ess coupled with the continuous absorption of water from the bile has a tendency to concentrate the secretion. Therefore the bile as we find it in the gall-bladder, ordinarily possesses a higher specific gravity than that of the freshly secreted fluid. The specific gravity under these conditions may run as high as 1.040. The principal constituents of the bile are the salts of the bile acids, bile pigments, neutral fats, lecithin, pliosphatidcs and cholesterol, besides the salts of iron, copper, calcium and magnesium. Zinc has also frequently been found in traces. The bile acids, which are elaborated exclusively by the hepatic cells, may be divided into two groups, the glycocholic acid group and the taurocholic acid group. In human bile glycocholic acid predominates, while taurocholic acid is the more abundant in the bile of carnivora. The bile acids are conjugate amino-acids, the glycocholic acid yielding glycocoll, CH2NH2 COOH, and cholic acid upon decomposition, whereas taurocholic acid gives rise to taurine, CH2NH2 CH2S02OH, and cholic acid under like conditions. Glycocholic acid contains some nitrogen but no sulphur, whereas taurocholic acid contains both these elements. The sulphur of the taurocholic acid is present in the taurine (amino-ethyl-sulphonic acid), of which it is a characteristic constituent. There are several varieties of cholic acid and there- fore we have several forms of glycocholic and taurocholic acids, 152 PHYSIOLOGICAL CHEMISTRY. the variation in constitution depending upon the nature of the cholic acid which enters into the combination. The bile acids are present in the bile as salts of one of the alkalis, generally sodium. The sodium glycocholate and sodium taurocholate may- be isolated in crystalline form, either as balls or rosettes of fine needles or in the form of prisms having ordinarily four or six sides (Fig. 40, below). The salts of the bile acids are dextro-rotatory. Among other properties these salts have the power of holding the choles- terol and lecithin of the bile in solution. Hammarsten has demonstrated a third group of bile acids in the bile of the shark. This same group very probably occurs in certain other animals also. These acids are very rich in sulphur and resemble ethereal sulphuric acids inasmuch as upon treatment with boiling hydrochloric acid they yield sulphuric acid. Fig. 40. ile Salts. The bile pigments are important and interesting biliary consti- tuents. The following have been isolated : bilirubin, biliverdin, bili- fuscin, biliprasin, bilihumin, bilicyanin, choleprasin and choletelin. Of these, bilirubin and biliverdin are the most important and pre- dominate in normal bile. The colors possessed by the various varieties of normal bile are due almost entirely to these two pig- ments, the. biliverdin being the predominant pigment in greenish bile and the bilirubin being the principal pigment in lighter colored bile. The pigments, other than the two just mentioned, have been found almost exclusively in biliary calculi or in altered bile ob- tained at post-mortem examinations. BILE. I 5 I Bilirubin, which is perhaps the most important of the bile pig- ments, is apparently derived from the blood pigment, the iron freed in the process being held in the liver. Bilirubin lias the same percentage composition as ha?matoporphyrin, which may be pro- duced from ■ haematin. It is a specific product of the liver cells but may also be formed in other parts of the body. The pig- ment may be isolated in the form of a reddish-yellow powder or may be obtained in part, in the form of reddish-yellow rhombic plates (Fig. 41, below) upon the spontaneous evaporation of its Fig. 41. Bilirubin (H^matoidin). (Ogden.) chloroform solution. The crystalline form of bilirubin is prac- tically the same as that of hsematoidin. It is easily soluble in chloroform, somewhat less soluble in alcohol and only slightly soluble in ether and benzene. Bilirubin has the power of combin- ing with certain metals, particularly calcium, to form combinations which are no longer soluble in the solvents of the unaltered pig- ment. Upon long standing in contact with the air, the reddish- yellow bilirubin is oxidized with the formation of the green bili- verdin. Bilirubin occurs in animal fluids as soluble bilirubin-alkali. Solutions of bilirubin exhibit no absorption-bands. If an am- moniacal solution of bilirubin-alkali in water is treated with a solution of zinc chloride, however, it shows bands similar to those of bilicyanin (Absorption Spectra, Plate II), the two bands be- tween C and D being rather well defined. Biliverdin is particularly abundant in the bile of herbivora. It is soluble in alcohol and glacial acetic acid and insoluble in water, chloroform and ether. Biliverdin is formed from bilirubin upon oxidation. It is an amorphous substance, and in this (litters from bilirubin which may be at least partly crystallized under proper 154 PHYSIOLOGICAL CHEMISTRY. conditions. Biliverdin may be obtained in the form of a green powder. In common with bilirubin, it may be converted into hy- drobilirubin by nascent hydrogen. The neutral solution of bilicyanin or cholecyanin is bluish-green or steel-blue and possesses a blue fluorescence, the alkaline solution is green with no appreciable fluorescence and the strongly acid so- lution is violet-blue. The alkaline solution exhibits three absorp- tion-bands, the first a dark, well-defined band between C and D, somewhat nearer C ; the second a less sharply-defined band extend- ing across D and the third a rather faint band between E and F, near E (Absorption Spectra, Plate II). The strongly acid so- lution exhibits two absorption bands, both lying between C and E and separated by a narrow space near D. A third band, exceed- ingly faint, may ordinarily be seen between b and F. Biliary calculi, otherwise designated as biliary concretions or gall stones, are frequently formed in the gall-bladder. These de- posits may be divided into three classes, cholesterol calculi, pigment calculi and calculi made up almost entirely of inorganic material. This last class of calculus is formed principally of the carbonate and phosphate of calcium and is rarely found in man although quite common to cattle. The pigment calculus is also found in cattle, but is more common to man than the inorganic calculus. This pigment calculus ordinarily consists principally of bilirubin in com- bination with calcium; biliverdin is sometimes found in small amount. The cholesterol calculus is the one found most frequently in man. These may be formed almost entirely of cholesterol, in which event the color of the calculus is very light, or they may con- tain more or less pigment and inorganic matter mixed with the cholesterol, which tends to give us calculi of various colors. For discussion of cholesterol see page 250. Experiments on Bile. 1. Reaction. — Test the reaction of fresh ox bile to litmus. 2. Nucleoprotein. — Acidify a small amount of bile with dilute acetic acid. A precipitate of nucleoprotein forms. 3. Inorganic Constituents. — Test for chlorides, sulphates and phosphates (see page 57). 4. Tests for Bile Pigments, (a) Gmelin's Test. — To about 5 c.c. of concentrated nitric acid in a test-tube add 2-3 c.c. of diluted bile carefully so that the two fluids do not mix. At the point of contact note the various colored rings, green, blue, violet, red and BILE. 155 reddish-yellow. Repeat this test with different dilutions of bile and observe its delicacy. (b) Rosenbach's Modification of Gmeliris Test. — loiter 5 c.c. of diluted bile through a small filter paper. Introduce a drop of concentrated nitric acid into the cone of the paper and note the suc- cession of colors as given in Gmelin's test. (c) Nakaxama's Reaction. — To 5 c.c. of diluted bile in a test-tube add an equal volume of a 10 per cent solution of barium chloride, centrifugate the mixture, pour off the supernatant fluid and heat the precipitate with 2 c.c. of Nakayama's reagent.1 In the presence of bile pigments the solution assumes a blue or green color. (d) Huppert's Reaction. — Thoroughly shake equal volumes of undiluted bile and milk of lime in a test-tube. The pigments unite with the calcium and are precipitated. Filter off the precipitate, wash it with water and transfer to a small beaker. Add alcohol acidified slightly with hydrochloric acid and warm upon a water- bath until the solution becomes colored an emerald green. In examining urine for bile pigments, according to Steensma, this procedure may give negative results even in the presence of the pigments, owing to the fact that the acid-alcohol is not a sufficiently strong oxidizing agent. He therefore sug'gests the addition of a drop of a 0.5 per cent solution of sodium nitrite to the acid-alcohol mixture before warming on the water-bath. Try this modifica- tion also. ( wash it with water. Remove the precipitate to a small porcelain dish, add 3 c.c. of an acid-alcohol mixture1 and a few drops of a dilute solution of sodium nitrite and heat. The production of a green color indicates the presence of bile pigments. 5. Tests for Bile Acids, (a) Pettenkofer's Test. — To 5 c.c. of diluted bile in a test-tube add 5 drops of a 5 per cent solution of sucrose. Now run about 2-3 c.c. of concentrated sulphuric acid carefully down the side of the tube and note the red ring at the point of contact. Upon slightly agitating the contents of the tube the whole solution gradually assumes a reddish color. As the tube becomes warm, it should be cooled in running water in order that the temperature of the solution may not rise above 700 C. (b) My Hits' 's Modification of Pettenkofer's Test. To approxi- mately 5 c.c. of diluted bile in a test-tube add 3 drops of a very dilute (1 : 1,000) aqueous solution of furfurol, HC-CH II II HC C-CHO. \/ 0 Now run about 2—3 c.c. of concentrated sulphuric acid carefully down the side of the tube and note the red ring as above. In this case also, upon shaking the tube the whole solution is colored red. Keep the temperature of the solution below yo° C. as before. (c) Neukomm's Modification of Pettenkofer's Test. — To a few drops of diluted bile in an evaporating dish add a trace of a dilute sucrose solution and one or more drops of dilute sulphuric acid. Evaporate on a water-bath and note the development of a violet color at the edge of the evaporating mixture. Discontinue the evaporation as soon as the color is observed. (d) v. Udrdnsky's Test. — To 5 c.c. of diluted bile in a test-tube add 3-4 drops of a very dilute (1 :i,ooo) aqueous solution of fur- furol. Place the thumb over the top of the tube and shake the tube until a thick foam is formed. By means of a small pipette add 2-3 drops of concentrated sulphuric acid to the foam and note the dark pink coloration produced. (e) Guerin's Reaction. — To equal volumes of diluted bile and alcohol in a test-tube add 5-6 drops of a saturated aqueous solution 1 Made by adding 5 c.c. of concentrated hydrochloric acid to 95 c.c. of 96 per cent alcohol. BILK. 157 of furfural and 5 6 drops of concentrated sulphuric acid. A blue color indicates bile acids. (/) Hay's Test. — This test is based upon the principle thai bile- acids have the property of reducing the surface tension of fluids in which they are contained. The test is performed as follows : Cool about 10 c.c. of diluted bile in a test-tube to 17° C. or lower and sprinkle a little finely pulverized sulphur upon the surface of the fluid. The presence of bile acids is indicated if the sulphur sinks to the bottom of the liquid, the rapidity with which the sulphur sinks depending upon the quantity of bile acids present in the mix- ture. The test is said to react with bile acids when they are present in the proportion 1 : 120,000. Some investigators claim that it is impossible to differentiate be- tween bile acids and bile pigments by this test. 6. Crystallization of Bile Salts. — To 25 c.c. of undiluted bile in an evaporating dish add enough animal charcoal to form a paste and evaporate to dryness on a water-bath. Remove the resi- due, grind it in a mortar and transfer it to a small flask. Add about 50 c.c. of 95 per cent alcohol and boil on a water-bath for 20 minutes. Filter, and add ether to the filtrate until there is a slight permanent cloudiness. Cover the vessel and stand it away until crystallization is complete. Examine the crystals under the microscope and compare them with those shown in Fig. 40, page 152. Try one of the tests for bile acids upon some of the crystals. i58 PHYSIOLOGICAL CHEMISTRY. 7. Analysis of Biliary Calculi. — Grind the calculus in a mortar with 10 c.c. of ether. Filter. Filtrate I. Allow to evaporate and examine for cholesterol crystals (Fig. 42, p. 159). (For further tests see ex- periment 8, below.) Residue I. (On paper and in mortar.) I Treat with dilute hydrochloric acid and filter. Filtrate II. Test for calcium, phos- phates and iron. Evapo- rate remainder of filtrate to dryness in porcelain crucible and ignite. Dis- solve residue in dilute hydrochloric acid and make alkaline with am- monium hydroxide. Blue color indicates copper. Residue II. (On paper and in mortar.) Wash with a little water. Dry the filter paper. Treat with 5 c.c. chloroform and filter. Filtrate III. Residue III. Bilirubin. (On paper and in (Apply test for bile mortar.) pigments.) Treat with 5 c.c. of hot alcohol. Biliverdin. S. Tests for Cholesterol. (a) Microscopical Examination. — Examine the crystals under the microscope and compare them with those shown in Fig. 42, page 159- (b) Iodine-Sulphuric Acid Test. — Place a few crystals of choles- terol in one of the depressions of a test-tablet and treat with a drop of concentrated sulphuric acid and a drop of a very dilute solution of iodine. A play of colors consisting of violet, blue, green and red results. (c) The Liebermann-Bur chard Test. — Dissolve a few crystals of cholesterol in 2 c.c. of chloroform in a dry test-tube. Now add 10 drops of acetic anhydride and 1-3 drops of concentrated sulphuric acid. The solution becomes red, then blue, and finally bluish- green in color. (d) Salkou'ski's Test. — Dissolve a few crystals of cholesterol in a little chloroform and add an equal volume of concentrated sul- phuric acid. A play of colors from bluish-red to cherry-red and i:ilk. '59 purple is noted in the chloroform while the acid assumes a marked green fluorescence. (e) Schiff's Reaction.-— To a little cholesterol in an evaporating dish add a few drops of Schiff's reagent.'1 Evaporate to dryness Cholesterol. over a low flame and observe the reddish-violet residue which changes to a bluish-violet. 9. Preparation of Taurine. — To 300 c.c. of bile in a casserole add 100 c.c. of hydrochloric acid and heat until a sticky mass (dyslysin) is formed. This point may be determined by drawing- out a thread-like portion of the mass by means of a glass rod, and if it solidifies immediately and assumes a brittle character we may conclude that all the taurocholic and glycochblic acid has been decomposed. Decant the solution and concentrate it to a small vol- ume on the water-bath. Filter the hot solution to remove sodium chloride and other substances which may have separated, and evaporate the filtrate to dryness. Dissolve the residue in 5 per cent hydrochloric acid and precipitate with ten volumes of 95 per cent alcohol. Filter off the taurine and recrystallize it from hot water. (Save the alcoholic filtrate for the preparation of glycocoll, page 160.) Alake the following tests upon the taurine crystals: (a) Examine them under the microscope and compare with Fig. 43, P- l6°- (b) Heat a crystal upon platinum foil. The taurine at first 1 Schiff's reagent consists of a mixture of three volumes of concentrated sulphuric acid and one volume of 10 per cent ferric chloride. i6o PHYSIOLOGICAL CHEMISTRY. melts, then turns brown and finally carbonizes as the temperature is raised. Note the suffocating odor. What is it? (c) Test the solubility of the crystals in water and in alcohol. (d) Grind up a crystal with four times its volume of dry sodium carbonate and fuse on platinum foil. Cool the residue, transfer it to a test-tube and dissolve it in water. Add a little dilute sul- phuric acid and note the odor of hydrogen sulphide. Hold a piece Fig. 43. Taurine. of filter paper, moistened with a small amount of lead acetate, over the opening of the test-tube and observe the formation of lead sul- phide. 10. Preparation of Glycocoll. — Concentrate the alcoholic filtrate from the last experiment (9) until no more alcohol remains. The glycocoll is present here in the form of an hydrochloride and may be liberated from this combination by the addition of freshly pre- cipitated lead hydroxide or by lead hydroxide solution. Remove the lead by hydrogen sulphide. Filter and decolorize the filtrate by animal charcoal. Filter again, concentrate the nitrate and set it aside for crystallization. Glycocoll separates as colorless crystals (Fig. 44, p. 161), n. Synthesis of Hippuric Acid. — To some of the glycocoll pre- pared in the last experiment or furnished by the instructor, add a little water, about 1 c.c. of benzoyl chloride and render alkaline with potassium hydroxide solution. Stopper the tube and shake it until no more heat is evolved. Now render strongly alkaline with potassium hydroxide and shake the mixture until no odor of MILK. 161 benzoyl chloride can be detected. Cool, acidify with hydrochloric acid, add an equal volume of petroleum ether and shake thoroughly to remove the benzoic acid. (Evaporate this solution and note Fig. 44. Glycocoll. the crystals of benzoic acid. Compare them with those shown in Fig. 94, page 289.) Decant the ethereal solution into a porcelain dish and extract again with ether. The hippuric acid remains in the aqueous solution. Filter it off and wash it with a small amount of cold water while still on the filter. Remove it to a small, shallow vessel, dissolve it in a small amount of hot water and set it aside for crystallization. Examine the crystals microscopically and com- pare them with those in Fig. 92, page 282. The chemistry of the synthesis is represented thus : CH2NH2 COC1 OCNHCH.COOH. + 11=11 + HO. COOH Glycocoll. Benzoyl chloride. Hippuric acid. CHAPTER X. PUTREFACTION PRODUCTS. The putrefactive processes in the intestine are the result of the action of bacteria upon the protein material present. This bac- terial action which is the combined effort of many forms of micro- organisms is confined almost exclusively to the large intestine. Some of the products of the putrefaction of proteins are identical with those formed in tryptic digestion, although the decomposition of the protein material is much more extensive when subjected to putrefaction. Some of the more important of the putrefaction products are the following : Indole, skatole, paracresol, phenol, para- oxyphenylpropionic acid, para-oxyphenylacetic acid, volatile fatty acids, hydrogen sulphide, methane, methyl mercaptan, hydrogen, and carbon dioxide, beside proteoses, peptones, ammonia and amino acids. Of these the indole, skatole, phenol and paracresol appear in part in the urine as ethereal sulphuric acids, whereas the oxyacids mentioned pass unchanged into the urine. The potassium indoxyl sulphate (page 279) content of the urine is a rough indicator of the extent of the putrefaction within the intestine. The portion of the indole which is excreted in the urine is first subjected to a series of changes within the organism and is sub- sequently eliminated as indican. These changes may be represented thus : /\ CH /\ C(OH) I I II +0 = | J || WCH \/\/CH NH NH Indole. Indoxyl. /\ C(OH) /\ C(0-S03H) I I || + H2S04 = I I || +H20 \/\/CH \/\/CH NH NH Indoxyl. Indoxyl sulphuric acid. In the presence of potassium salts the indoxyl sulphuric acid is then transformed into indoxyl potassium sulphate (or indican), 162 PUTREFACTION PRODUCTS. 1 63 /\ C(0-SO,K), \/\/CH NH and eliminated as such in the urine. Indican may be decomposed by treatment with concentrated hy- drochloric acid (see tests on page 280) into sulphuric acid and in- doxyl. The latter body may then be oxidized to form indigo-blue thus : /\ C(OH) /\ CO OC /\ 2 1 I || +20 = 1 II III +2H20 \A/CH \/\/C=C\/\/ NH NH NH Tndoxyl. Indigo-blue. This same reaction may also occur under pathological conditions unthin the organism, thus giving rise to the appearance of crystals of indigo-blue in the urine. Skatole is likewise changed within the organism and eliminated in the form of a chromogenic substance. Skatole is, however, of less importance as a putrefaction product than indole and ordinarily occurs in much smaller amount. The tryptophane group of the protein molecule yields the indole and skatole formed in intestinal putrefaction, but the reasons for the transformation of the major portion of this tryptophane into indole and the minor portion into skatole are not well understood. Indole is more toxic than skatole. Phenol occurs in fairly large amount in certain abnormal con- ditions of the organism, but ordinarily the amount is very small. It is probably derived from the tyrosine group of the protein mole- cule. Phenol is conjugated in the liver to form phenyl potassium sulphate and appears in the urine in this form (Baumann and Herter). Para-cresol occurs in the urine as cresyl potassium sul- phate. Regarding the claim of Nencki that methyl mercaptan is formed as a g'as during intestinal putrefaction it is an important fact that Herter1 has been unable to detect the mercaptan in fresh feces. He is therefore, not inclined to accept the theory that methyl mercap- tan is formed in ordinary intestinal putrefaction but believes that it may be formed in exceptional cases. Hydrogen sulphide is. how- ever, formed in all cases of intestinal putrefaction. 1 Herter : Bacterial Infections of the Digestive Tract, p. 22*. 164 physiological chemistry. Experiments on Putrefaction Products. In many courses in physiological chemistry the instructors are so limited for time that no extended study of the products of putre- faction can very well be attempted. Under such conditions the scheme here submitted may be used profitably in the way of a dem- onstration. Where the number of students is not too great, a single large putrefaction may be started, and, after the initial distillation, both the resulting distillate and residue may be dis- tributed to the members of the class for individual manipulation. Preparation of Putrefaction Mixture. — Place a weighed mix- ture of coagulated egg albumin and ground lean meat in a flask or bottle and add approximately 2 liters of water for every kilogram of protein used. Sterilize the vessel and contents, inoculate with the colon bacillus and keep at 40 ° C. for two or three weeks. If cultures of the colon bacillus are not available, add 60 c.c. of a cold saturated solution of sodium carbonate for every liter of water pre- viously added and inoculate with some putrescent material (pan- creas or feces).1 Mix the putrefaction mixture very thoroughly by shaking and insert a cork furnished with a glass tube to which is attached a wash bottle containing a 3 per cent solution of mer- curic cyanide.2 This device is for the purpose of collecting the methyl mercaptan, a gas formed during the process of putrefac- tion. It also serves to diminish the odor arising from the putre- fying material. Place the putrefaction mixture at 400 C. for two or three weeks and at the end of that time make a separation of the products of putrefaction according to the following directions : Subject the mixture to distillation until the distillate and residue are approximately equal in volume. 1 Putrefying protein may be prepared by treating 10 grams of finely ground lean meat with 100 c.c. of water and 2 c.c. of a saturated solution of sodium carbonate and keeping the mixture at 400 C. for twenty-four hours. - Concentrated sulphuric acid containing a small amount of isatin may be used as a substitute for mercuric cyanide. When this modification is employed it is necessary to use calcium chloride tubes to exclude moisture from the isatin solution. PUTREFACTION PRODUCTS. I65 PART I MANIPULATION OF THE DISTILLATE. Acidify with hydrochloric acid and extract with ether. Ether Extract No. 1. Add an equal volume of water, make alkaline with potassium hy- droxide and shake thoroughly. Residue No. 1. Allow the ether to volatilize. Evaporate and detect ammonium chloride crystals (Fig. 45, p. 166). Ether Extract No. 2. Evaporate spontaneously. Indole and skatole remain. Try proper reactions (see pages 168 and 170). Alkaline Solution No. 1. Acidify with hydrochloric acid, add sodium carbonate and extract with ether. Ether Extract No. 3. Evaporate. Detect phenol and cresol (paracresol). See p. 170. Alkaline Solution No. 2. Acidify with hydrochloric acid, and extract with ether. Ether Extract No. 4. Evaporate. Volatile fatty acids remain. Final Residue. (Discard.) DETAILED DIRECTIONS FOR MAKING THE SEPARATIONS INDICATED IN THE SCHEME. Preliminary Ether Extraction. — This extraction may be conven- iently conducted in a separatory funnel. Mix the fluids for ex- traction in the ratio of lzv,o volumes of ether to three volumes of the distillate. Shake very thoroughly for a few moments then draw off the extracted fluid and add a new portion of the distillate. Re- peat the process until the entire distillate has been extracted. Add a small amount of fresh ether at each extraction to replace that dissolved by the water in the preceding- extraction. Residue No. 1. — Unite the portions of the distillate extracted as above and allow the ether to volatilize spontaneously. Evaporate until crystallization begins. Examine the crystals under the micro- scope. Ammonium chloride predominates. Explain its presence. 1 66 PHYSIOLOGICAL CHEMISTRY. Ether Extract No. I. — Add an equal volume of water, render the mixture alkaline with potassium hydroxide and shake thoroughly by means of a separatory funnel as before. The volatile fatty acids, Fig. 45. Ammonium Chloride. contained among the putrefaction products, would be dissolved by the alkaline solution (No. 1) whereas any indole or skatole would remain in the ethereal solution (No. 2). Alkaline Solution No. 1. — Acidify with hydrochloric acid and add sodium carbonate solution until the fluid is neutral or slightly acid from the presence of carbonic acid. At this point a portion of the solution, after being heated for a few moments, should pos- sess an alkaline reaction on cooling. Extract the whole mixture with ether in the usual way, using care in the manipulation of the stop cock to relieve the pressure due to the evolution of carbon dioxide. The ether (Ether Extract No. 3) removes any phenol or cresol which may be present while the volatile fatty acids will remain in the alkaline solution (No. 2) as alkali salts. Ether Extract No. 2. — Drive off the major portion of the ether at a low temperature on a water-bath and allow the residue to evap- orate spontaneously. Indole and skatole should be present here. Prove the presence of these bodies. For tests for indole and skatole see pp. 168 and 170. Alkaline Solution No. 2. — Make strongly acid with hydrochloric acid and extract with a small amount of ether, using a separatory funnel. As carbon dioxide is liberated here, care must be used in the manipulation of the stop cock of the funnel in relieving the PUTREFACTION PRODUCTS. l6/ pressure within the vessel. The volatile fatty acids are dissolved by the ether (Ether Extract No. 4). Ether Extract No. J. — Evaporate this ethereal solution on a water-bath. The oily residue contains phenol and cresol. The cresol is present for the most part as paracresol. Add some water to the oily residue and heat it in a flask. Cool and prove the pres- ence of phenol and cresol. For tests for these bodies see page 170. Ether Extract No. 4. — Evaporate on a water-bath. The volatile fatty acids remain in the residue. PART II. MANIPULATION OF THE RESIDUE. Evaporate, filter and extract with ether. Ether Extract. Evaporate, extract the residue with warm water and filter. Aqueous Solution. Evaporate until crystals hegin to from. Stand in a cold place until crystallization is complete. Filter. Crystalline Deposit. Consists of a mixture of leucine and tyrosine crystals. (Figs. 23, 26 and 104, pages 72, 76 and 350.) Filtrate No. 1. Contains proteose, pep- tone, aromatic acids and tryptophane. Filtrate No. 2. Contains oxyacids and skatolc-carbonic acid. Residue. Contains non-volatile fatty acids. DETAILED DIRECTIONS FOR MAKING THE SEPARATIONS INDICATED IN THE SCHEME. Preliminary Ether Extraction. — This extraction may be con- ducted in a separatory funnel. In order to make a satisfactory ex- traction the mixture should be shaken very thoroughly. Separate the ethereal solution from the aqueous portion and treat them ac- cording to the directions given on p. 168. 1 68 PHYSIOLOGICAL CHEMISTRY. Ether Extract. — Evaporate this solution on a safety water-bath until the ether has been entirely removed. Extract the residue with warm water and filter. Aqueous Solution. — Evaporate this solution until crystallization begins. Stand the solution in a cold place until no more crystals form. This crystalline mass consists of impure leucine and tyro- sine. Filter off the crystals. Crystalline Deposit. — Examine the crystals under the microscope and compare them with those reproduced in Figs. 23, 26 and 104, pages J2, 76 and 350. Do the forms of the crystals of leucine and tyrosine resemble those previously examined? Make a separation of the leucine and tyrosine and apply typical tests according to directions given on pages 83 and 84. Filtrate No. 1. — Make a test for tryptophane with bromine water (see page 145)., and, also with the Hopkins-Cole reagent (see page 91). Use the remainder of the filtrate for the separation of pro- teoses and peptones. Make the separation according to the direc- tions given on page 114. Filtrate No. 2. — This solution contains para-oxyphenylacetic acid, para-oxyphenylpropionic acid and skatole-carbonic acid. Prove the presence of these bodies by appropriate tests. Tests for oxyacids and skatole-carbonic acid are given on page 171. TESTS FOR VARIOUS PUTREFACTION PRODUCTS. Tests for Indole. 1. Herter's /3-Naphthaquinone Reaction. — (a) To a dilute aqueous solution of indole (1:500,000) add one drop of a 2 per cent solution of /?-naphthaquinone-sodium-monosulphonate. No reaction occurs. Add a drop of a 10 per cent solution of potassium hydroxide and note the gradual development of a blue or blue-green color which fades to green if an excess of the alkali is added. Ren- der the green or blue-green solution acid and note the appearance of a pink color. Heat facilitates the development of the color re- action. One part of indole in one million parts of water may be detected by means of this test if carefully performed. (b) If the alkali be added to a more concentrated indole solu- tion before the introduction of the naphthaquinone the course of the reaction is different, particularly if the indole solution is some- PUTREFACTION PRODUCTS. 169 what more concentrated than that mentioned above and if heal is used. Under these conditions the blue indole compound ultimately forms as fine acicnlar crystals which rise to the surface. If we do not wait for the production of the crystalline body but as soon as the blue color forms, shake the aqueous solution with chlor- oform, the blue color disappears from the solution and the chloro- form assumes a pinkish-red hue. This is a distinguishing feature of the indole reaction and facilitates the differentiation of indole from other bodies which yield a similar blue color. 2. Konto's Reaction. — Distil the solution to be tested until only one-third of the original solution remains. Make the distillate al- kaline with sodium hydroxide and distil again in order to separate the indole from the phenol, the latter remaining in the residue. In- asmuch as this second distillate generally contains a large amount of ammonia it should be acidified with dilute sulphuric acid and again distilled. To i c.c. of this ammonia-free distillate in a test- tube add 3 drops of a 40 per cent solution of formaldehyde and 1 c.c. of concentrated sulphuric acid. Now agitate the mixture and note the appearance of a violet red color if a trace of indole is present. The test is said to serve for the detection of indole when present in a dilution of 1 1700,000. Skatole gives a yellow or brown color under the above conditions. 3. Cholera-red Reaction. — To a little of the residue in a test- tube add one-tenth its volume of a 0.02 per cent solution of potas- sium nitrite and mix thoroughly. Carefully run concentrated sul- phuric acid down the side of the tube so that it forms a layer at the bottom. Note the purple color. Neutralize with potassium hydroxide and observe the production of a bluish-green color. 4. Legal's Reaction. — To a small amount of the residue in a test-tube add a few drops of a freshly prepared solution of sodium nitroprusside, Na2Fe(CN)5NO -j- 2H0O. Render alkaline with potassium hydroxide and note the production of a violet color. If the solution is now acidified with glacial acetic acid the violet is transformed into a blue. 5. Pine Wood Test. — Moisten a pine splinter with concentrated hydrochloric acid and insert it into the residue. The wood as- sumes a cherry-red color. 6. Nitroso-indole Nitrate Test. — Acidify some of the residue with nitric acid, add. a few drops of a potassium nitrite solution and note the production of a red precipitate of nitroso-indole nitrate. If the residue contains but little indole simply a red coloration will 170 PHYSIOLOGICAL CHEMISTRY. result. Compare this result with the result of the similar test on skatole. Tests for Skatole. i. Herter's Para-dimethylaminobenzaldehyde Reaction.1 — To 5 c.c. of the distillate or aqueous solution under examination add i c.c. of an acid solution of para-dimethylaminobenzaldehyde2 and heat the mixture to boiling. A purplish-blue coloration is produced3 which may be intensified through the addition of a few drops of concentrated hydrochloric acid. If the solution be cooled under running water it loses its purplish tinge of color and becomes a definite blue. The solution at this point may be somewhat opal- escent through the separation of uncombined para-dimethylamino- benzaldehyde. Care should be taken not to add an excess of hy- drochloric acid inasmuch as the end-reaction has a tendency to fade under the influence of a high acidity. A rough idea regarding the actual quantity of skatole in a mix- ture may be obtained by extracting this blue solution with chloro- form and subsequently comparing this chloroform solution, by means of a colorimeter (Duboscq), with the maximal reaction, ob- tained with a skatole solution of known strength. 2. Color Reaction with Hydrochloric Acid. — Acidify some of the residue with concentrated hydrochloric acid. Note the pro- duction of a violet color. 3. Acidify some of the residue with nitric acid and add a few drops of a potassium nitrite solution. Note the white turbidity. Compare this result with the result of the similar test on indole. Tests for Phenol and Cresol. 1. Color Test. — Test a little of the solution with Millon's re- agent. A red color results. Compare this test with the similar one under Tyrosine ( see page 83 ) . 2. Ferric Chloride Test. — Add a few drops of neutral ferric chloride solution to a little of the residual fluid. A dirty bluish- gray color is formed. 3. Formation of Bromine Compounds. — Add some bromine water to a little of the fluid under examination. Note the crys- talline precipitate of tribromphenol and tribromcresol. 1Herter: Bacterial Infections of the Digestive Tract, 1907, p. 141. 2 Made by dissolving 5 grams of para-dimethylaminobenzaldehyde in 100 c.c. of 10 per cent sulphuric acid. 3 If the color does not appear add more of the aldehyde solution. PUTREFACTION PRODUCTS. I 7 I Tests for Oxyacids. 1. Color Test. — Test a little of the solution with Millon's re- agent. A red color results. 2. Bromine Water Test. — Add a few drops of bromine water to some of the filtrate. A turbidity or precipitate is observed. Test for Skatole-carbonic Acid. Ferric Chloride Test. — Acidify some of the filtrate with hydro- chloric acid, add a few drops of ferric chloride solution and heat. Compare the end-reaction with that given by phenol. CHAPTER XI FECES. The feces is the residual mass of material remaining in the intes- tine after the full and complete exercise of the digestive and ab- sorptive functions and is ultimately expelled from the body through the rectum. The amount of this fecal discharge varies with the individual and the diet. Upon an ordinary mixed diet the daily ex- cretion by an adult male will aggregate 1 10-170 grams with a solid content ranging between 25 and 45 grams; the fecal discharge of Fig. 46. Microscopical Constituents of Feces, (v. Jaksch.) a, Muscle fibers ; b, connective tissue ; c, epithelium ; d, leucocytes ; e, spiral cells ; f, g, h, h various vegetable cells ; k, " triple phosphate " crystals ; /, woody vegetable cells ; the whole interspersed with innumerable micro-organisms of various kinds. such an individual upon a vegetable diet will be much greater and may even be as great as 350 grams and possess a solid content of 75 grams. The variation in the normal daily output being so great renders this factor of very little value for diagnostic purposes, except where the composition of the diet is accurately known. Lesions of the digestive tract, a defective absorptive function or increased peristalsis as well as an admixture of mucus, pus, blood and pathological products of the intestinal wall may cause the total amount of excrement to be markedly increased. 172 FECES. 1/3 The fecal pigment of the normal adult is hydrobilirubin. This pigment originates from the bilirubin which is secreted into the in- testine in the bile, the transformation from bilirubin to hydrobili- rubin being brought about through the activity of certain bacteria. Hydrobilirubin is sometimes called stercobilin and bears a close re- semblance to urobilin or may even be identical with that pigment. Neither bilirubin nor biliverdin occurs normally in the fecal dis- charge of adults, although the former may be detected in the ex- crement of nursing infants. The most important factor, however, in determining the color of the fecal discharge is the diet. A mixed diet for instance produces stools which vary in color from light to dark brown, an exclusive meat diet gives rise to a brown- ish-black stool, whereas the stool resulting" from a milk diet is in- variably light colored. Certain pigmented foods such as the chlo- rophyllic vegetables, and various varieties of berries, each afford stools having a characteristic color. Certain drugs act in a similar way to color the fecal dis- charge. This is well illustrated by the occurrence of green stools following the use of calomel and of H/EMATOiDix Crystals from Acholic Stools, {v. Jaksch.) Color of crystals same as the color of those in Fig. 41, p. 153. black stools after bismuth ingestion. The green color of the calo- mel stool is generally believed to be due to biliverdin. v. Jaksch. however, claims to have proven this view to be incorrect since he was able to detect hydrobilirubin (or urobilin) but no biliverdin in stools after the administration of calomel. The bismuth stool derives its color from the black sulphide which is formed from the subnitrate of bismuth. In cases of biliary obstruction the grayish-white acholic stool is formed. Under normal conditions the odor of feces is due to skatole and indole, two bodies formed in the course of putrefactive processes occurring within the intestine (see page 162). Such todies as methane, methyl mercaptan and hydrogen sulphide may also add to the disagreeable character of the odor. The intensity of the odor depends to a large degree upon the character of the diet, being very marked in stools from a meat diet, much less marked in stools from a vegetable diet and frequently hardly detectable in 174 PHYSIOLOGICAL CHEMISTRY. stools from a milk diet. Thus the stool of the infant is ordi- narily nearly odorless and any decided odor may generally be read- ily traced to some pathological source. A neutral reaction ordinarily predominates in normal stools al- though slightly alkaline or even acid stools are met with. The acid reaction is encountered much less frequently FlG- 48- than the alkaline and then commonly only fol- lowing a vegetable diet. The form and consistency of the stool is de- pendent, in large measure, upon the nature of the diet and particularly upon the quantity of water ingested. Under normal conditions the consistency may vary from a thin, pasty dis- Charcot-Leyden io,ii-i Crystals. charge to a firmly formed stool, btools which are exceedingly thin and watery ordinarily have a pathological significance. In general the feces of the carnivorous animals is of a firmer consistency than that of the herbivora. It is frequently desirable for clinical or experimental purposes to make an examination of the fecal output which constitutes the residual mass from a certain definite diet. Under such conditions, it is customary to cause the person under observation to ingest some substance, at the beginning and end of the period in ques- tion, which shall sufficiently differ in color and consistency from the surrounding feces as to render comparatively easy the differentiation of the feces of that period from the feces of the immediately pre- ceding and succeeding periods. One of the most satisfactory meth- ods of making this " separation " is by means of the ingestion of a gelatin capsule containing about 0.2 gram of powdered char- coal at the beginning and end of the period under observation. This procedure causes the appearance of tzt'.o black zones of char- coal in the fecal mass and thus renders comparatively simple, the differentiation of the feces of the intermediate period. Some similar method for the " separation of feces " is' universally prac- ticed in connection with the scientifically accurate type of nutri- tion or metabolism experiment which embraces the collection of useful data regarding the income and outgo of nitrogen, and other elements. Among the macroscopical constituents of the feces may be men- tioned the following : Intestinal parasites, undigested food particles, gall stones, pathological products of the intestinal wall, enteroliths, intestinal sand and objects which have been accidentally swallowed. FECES. 175 The fecal constituents which at various times and under different conditions may be detected by the use of the microscope are as fol- lows: Constituents derived from the food, such as muscle fibers, connective tissue shreds, starch granules and fat; formed elements derived from the intestinal tract, such as epithelium, erythrocytes and leucocytes; mucus; pus corpuscles; parasites and bacteria. In addition to the constituents named, the following crystalline deposits may be detected: cholesterol, soaps, fatty acid, fat, bismuth sul- phide, liccmatoidin. " triple phosphate," C hare ot-Ley den crystals and the oxalate, carbonate, phosphate, sulphate and lactate of cal- cium. The detection of minute quantities of blood in the feces (" oc- cult blood") has recently become a recognized aid to a correct diagnosis of certain disorders. In these instances the hemorrhage is ordinarily so slight that the identification by means of macro- scopical characteristics as well as the microscopical identification through the detection of erythrocytes are both unsatisfactory in their results. Of the tests given for the detection of " occult blood" the aloin-turpentinc test (page 178) is probably the most satisfactory. Since " occult blood " occurs with considerable regularity and frequency in gastrointestinal cancer and in gastric and duodenal ulcer, its detection in the feces is of especial value as an aid to a correct diagnosis of these disorders. It has been quite clearly shown that the intestine of the newly born is sterile. However this condition is quickly altered and bac- teria may be present in the feces before or after the first inges- tion of food. There are three possible means of infecting the intestine, i. e., by way of the mouth or anus or through the blood. The infection by means of the blood seldom occurs except under pathological conditions, thus limiting the general infection to the mouth and anus. In infants with pronounced constipation two-thirds of the dry substance of the stools has been found to consist of bacteria. In the stools of normal adults probably about one-third of the dry substance is bacteria.1 The average excretion of dry bacteria in twenty-four hours for an adult is about eight grams. Some of the more important organisms met with in the feces are the following :2 B. coli, B. lactis aerogenes, Bact. JJ'elchii, B. bifidus and coccal forms. Of these the first three types mentioned 1 Schittenhelm and Tollens found bacteria to comprise 42 per cent of the dry matter. This value is, however, probably too high. ' Herter and Kendall: Journal of Biological Chemistry, 1908, V, p. 283. 176 PHYSIOLOGICAL CHEMISTRY. are gas- forming organisms. The production of gas by the fecal flora in dextrose-bouillon is subject to great variations under path- ological conditions : alterations in the diet of normal persons will also cause wide fluctuations. In this connection Herter has ob- served a marked reduction or even complete cessation of gas pro- duction by the mixed fecal bacteria while considerable doses of benzoate were being given. A return to the former plane of gas production followed .the discontinuation of the benzoate.1 Data as to the production of gas are of considerable importance in a diag- nostic way although the exact cause of the variations is not yet es- tablished. It should be borne in mind in this connection that gas volumes are frequently variable with the same individual. For this reason it is necessary in every instance to follow the gas pro- duction for a considerable period of time before drawing conclu- sions.2 For diagnostic purposes the macroscopical and microscopical ex- aminations of the feces ordinarily yield much more satisfactory data than are secured from its chemical examination. Experiments on Feces. 1. Macroscopical Examination. — If the stool is watery pour it into a shallow dish and examine directly. If it is firm or pasty it should be treated with water and carefully stirred before the examination for macroscopical constituents is attempted. The macroscopical constituents may be collected very satisfactor- ily by means of a Boas sieve (Fig. 49, page 177). This sieve is constructed of two easily detachable hemispheres which are held together by means of a bayonet catch. In using the apparatus the feces is spread out upon a very fine sieve contained in the lower hemisphere and a stream of water is allowed to play upon it through the medium of an opening in the upper hemisphere. The apparatus is provided with an orifice in the upper hemisphere through which the feces may be stirred by means of a glass rod during the washing process. After 15-30 minutes washing noth- ing but the coarse fecal constituents remain upon the sieve. 2. Microscopical Examination. — Watery stools should be placed in a shallow dish, thoroughly mixed and a small amount removed to a slide for examination. Stools of a firm or pasty consistency should be rubbed up in a mortar with physiological salt solution 1 Private communication from Professor C. A. Herter. 2 Herter and Kendall : he. cit. FECES. 177 Fig. 49. Boas' Sieve. and a small portion of the resulting- mixture transferred to a slide for examination. In normal feces look for food particles, bacteria and crystalline bodies. In pathological stools, in addition to these substances, look for animal parasites and pathological products of the intes- tinal wall. See Fig. 46, page 172. 3. Reaction. — Thoroughly mix the feces and apply moist red and blue litmus papers to the sur- face. If the stool is hard it should be mixed with water before the reaction is taken. Examine the stool as soon after defecation as is convenient, since the reaction may change very rapidly. The reaction of the normal stools of adult man is ordinarily neutral or faintly alkaline to litmus, but seldom acid. Infants' stools are generally acid in reaction. 4. Starch. — If any imperfectly cooked starch- containing' food has been ingested it will be pos- sible to detect starch granules by a microscopical examination of the feces. If the granules are not detected by a microscopical ex- amination, the feces should be placed in an evaporating dish or casserole and boiled with water for a few minutes. Filter and test the filtrate by the iodine test in the usual way (see page 44). 5. Cholesterol and Fat. — Extract the dry feces with ether in a Soxhlet apparatus (see Fig. 125). If this apparatus is not avail- able transfer the dry feces to a flask, add ether and shake fre- quently for a few hours. Filter and remove the ether by evapora- tion. The residue contains cholesterol and the mixed fats of the feces. For every gram of fat add about i}4 gram of solid potassium hydroxide and 25 c.c. of 95 per cent alcohol and boil in a flask on a water-bath for one-half hour, maintaining the volume of alcohol constant. This alcoholic-potash has saponified the mixed fats and we now have a mixture of soaps and cholesterol. Add sodium chloride, in substance, to the mixture and extract with ether to dissolve out the cholesterol. Remove the ether by evapora- tion and examine the residue microscopically for cholesterol crystals. Try any of the other tests for cholesterol as given on page 158. 6. Blood. — Undecomposed blood may be detected macroscopi- cally. If uncertain, look for erythrocytes under the microscope, and spectroscopically for the spectrum of oxyhemoglobin (see Absorption Spectra, Plate I). 13 178 PHYSIOLOGICAL CHEMISTRY. In case the blood has been altered or is present in minute amount ("occult blood"), and cannot be detected by the means just men- tioned, the following tests may be tried : (a) Aloin-Turp entitle Test. — Mix the stool very thoroughly and take about 5 grams of the mixture for the test. Reduce this sam- ple to a semi-fluid mass by means of distilled water and extract very thoroughly with an equal volume of ether to remove any fat which may be present. Now treat the extracted feces with one- third its volume of glacial acetic acid and 10 c.c. of ether and ex- tract very thoroughly as before. The acid-ether extract will rise to the top and may be removed. Introduce 2-3 c.c. of this acid-ether solution into a test-tube, add an equal volume of a dilute solution of aloin in 70 per cent al- cohol and 2-3 c.c. of ozonized turpentine and shake the tube gently. If blood is present the entire volume of fluid ordinarily becomes pink and finally cherry red. In some instances the color will be limited to the aloin solution which sinks to the bottom. This color reaction should occur within fifteen minutes in order to indicate a positive test for blood, since the aloin will turn red of itself if allowed to stand for a longer period. The color is ordinarily light yellow in a negative test. Hydrogen peroxide is not a satis- factory substitute for turpentine in this test. (b) Weber's Guaiac Test. — Mix a little feces with 30 per cent acetic acid to form a fluid mass. Transfer to a test-tube and ex- tract with ether. If blood is present the ether will assume a brown- ish-red color. Filter off the ether extract and to a portion of the filtrate, add an alcoholic solution of guaiac (strength about 1 : 60), 1 drop by drop, until the fluid becomes turbid. Now add hydrogen peroxide or old turpentine. In the presence of blood a blue color is produced (see page 196). (c) Cozme's Guaiac Test. — To 1 gram of moist feces add 4-5 c.c. of glacial acetic acid and extract the mixture with 30 c.c. of ether. To 1-2 c.c. of the extract add an equal volume of water, agitate the mixture, introduce a few granules of powdered guaiac resin, and after bringing the resin into solution, gradually add 30 drops of old turpentine or hydrogen peroxide. A blue color indicates the presence of blood. Cowie claims that by means of this test an intestinal hemorrhage of 1 gram can easily be detected by an examination of the feces. 1 Buckmaster advises the use of an alcoholic solution of guaiaconic acid instead of an alcoholic solution of guaiac resin. FECES. 179 (d) Acid-Hcematin. — Examine some of the ethereal extract from Experiment ( b ) spectroscopically. Note the typical spectrum of acid-hsematin (see Absorption Spectra, I Mate II). 7. Hydrobilirubin. Schmidt's Test. — Rub up a small amount of feces in a mortar with a concentrated aqueous solution of mercuric chloride. Transfer to a shallow, flat-bottomed dish and allow to stand 6-24 hours. The presence of hydrobilirubin will be indicated by a deep red color being; imparted to the particles of feces con- taining this pigment. 1 "his red color is due to the formation of hydrobilirubin-mercury. If unaltered bilirubin is present in any portion of the feces that portion will be green in color due to the oxidation of bilirubin to biliverdin. Another method for the detection of hydrobilirubin is the fol- lowing: Treat the dry feces with absolute alcohol acidified with sulphuric acid and shake thoroughly. The acidified alcohol extracts the pigment and assumes a reddish color. Examine a little of this fluid spectroscopically and note the typical spectrum of hydro- bilirubin (Absorption Spectra, Plate II). 8. Bilirubin.1 (a) Gmelin's Test. — Place a few drops of con- centrated nitric acid in an evaporating dish or on a porcelain test- tablet and allow a few drops of feces and water to mix with it. The usual play of colors of Gmelin's test is produced, i. e., green, blue, violet, red and yellow. If so desired, this test may be exe- cuted on a slide and observed under the microscope. (b) Happert's Test. — Treat the feces with water to form a semi- fluid mass, add an equal amount of milk of lime, shake thorough- ly and filter. Wash the precipitate with water, then transfer both the paper and the precipitate to a small beaker or flask, add a small amount of 95 per cent alcohol acidified slightly with sulphuric acid and heat to boiling on a water-bath. The presence of bilirubin is indicated by the alcohol assuming a green color. Steensma advises the addition of a drop of a 0.5 per cent solu- tion of sodium nitrite to the acid-alcohol mixture before warming on the water-bath. Try this modification also. 9. Bile Acids. — Extract a small amount of feces with alcohol and filter. Evaporate the filtrate on a water-bath to drive off the alcohol and dissolve the residue in water made slightly alkaline with potassium hydroxide. Upon this aqueous solution try any of the tests for bile acids given on page 156. 1The detection of bilirubin in the feces is comparatively simple provided it is not accompanied by other pigments. When other pigments are present, how- ever, it is difficult to detect the bilirubin and at times, ma}- be found impossible. 1 8o PHYSIOLOGICAL CHEMISTRY. 10. Caseinogen. — Extract the fresh feces first with a dilute so- lution of sodium chloride, and later with water acidified with dilute acetic acid, to remove soluble proteins. Now extract the feces with 0.5 per cent sodium carbonate and filter. Add dilute acetic acid to the filtrate to precipitate the caseinogen, being careful not to add an excess of the reagent as the caseinogen would dissolve. Filter off the caseinogen and test it according to directions given on page 224. Caseinogen is found principally in the feces of children who have been fed a milk diet.- Mucin would also be extracted by the dilute alkali, if present in the feces. What test could you make on the newly precipitated body to differentiate between mucin and caseinogen ? 11. Nucleoprotein. — Mix the stool thoroughly with water, trans- fer to a flask, and add an equal amount of saturated lime water. Shake frequently for a few hours, filter, and precipitate the nucleo- protein with acetic acid. Filter off this precipitate and test it as follows : (a) Phosphorus. — Test for phosphorus by fusion (see page 251). (b) Solubility. — Try the solubility in the ordinary solvents. (c) Protein Color Test. — Try any of the protein color tests. What proof have you that the above body was not mucin? What other test can you use to differentiate between nucleoprotein and mucin ? 12. Albumin and Globulin. — Extract the fresh feces with a dilute solution of sodium chloride. (The preliminary extract from the preparation of caseinogen (10), above, may be utilized here.) Filter, and saturate a portion of the filtrate with sodium chloride in substance. A precipitate signifies globulin. Filter off the pre- cipitate and acidify the filtrate slightly with dilute acetic acid. A precipitate at this point signifies albumin. Make a protein color test on each of these bodies. 13. Proteose and Peptone. — Heat to boiling the portion of the sodium chloride extract not used in the last experiment. Filter off the coagulum, if any forms. Acidify the filtrate slightly with acetic acid and saturate with sodium chloride in substance. A pre- cipitate here indicates proteose. Filter it off and test it according to directions given on page 115. Test the filtrate for peptone by the biuret test. 14. Inorganic Constituents. — Prepare a dilute aqueous solution of dry feces and decolorize it by means of purified animal charcoal. Make the following tests upon the clear solution : FECES. I S I (a) Chlorides. — Acidify with nitric acid and add argentic nitrate. (b) Phosphates. — Acidify with nitric acid, add molybdic solution and warm gently. (c) Sulphates. — Acidify with hydrochloric acid, add barium chloride and warm. 15. Konto's Reaction for Indole. — Rub up the stool with water to form a thin paste. From this point the test is the same as for the detection of indole in putrefaction mixtures (see page 169). 16. Schmidt's Nuclei Test. — This test serves as an aid to the diagnosis of pancreatic insufficiency. The test is founded upon the theory that cell nuclei are digestible only in pancreatic juice, and therefore that the appearance in the feces of such nuclei indi- cates insufficiency of pancreatic secretion. The procedure is as follows : Cubes of fresh beef about one-half centimeter square are enclosed in small gauze bags and ingested with a test meal. Subsequently the fecal mass resulting from this test-meal is exam- ined, the bag opened and the condition of the enclosed residue de- termined. Under normal conditions the nuclei would be digested. Therefore if the nuclei are found to be for the most part undi- gested, and the intervening period has been sufficient to permit of the full activity of the pancreatic function (at least 6 hours), it may be considered a sign of pancreatic insufficiency. It has been claimed by Steele that under certain conditions the non-digestion of the nuclei may indicate a general lowering of the digestive power rather than a true pancreatic insufficiency. CHAPTER XII BLOOD. Blood is composed of four types of form-elements (erythrocytes or red blood corpuscles, leucocytes or white blood corpuscles, blood plates or plaques and blood dust or hsemoconien) held in suspen- sion in a fluid called blood plasma. These form-elements compose about 60 per cent of the blood, by weight. Ordinarily blood is a dark red, opaque fluid due to the presence of the red blood corpus- cles, but through the action of certain substances such as water, ether or chloroform it may be rendered transparent. Blood so altered is said to be laked. The laking process is simply a liberation of the haemoglobin from the stroma of the red blood corpuscle. Normal blood is alkaline in reaction1 to litmus, the alkalinity being due principally to sodium carbonate and phosphate. The specific gravity of the blood of adults ordinarily varies between 1.045 and 1.075. It varies somewhat with the sex, the blood of males hav- ing a rather higher specific gravity than that of females of the same species. Under pathological conditions also the density of the blood may be very greatly altered. The freezing'-point (A) of normal blood is about — 0.560 C. Variations between — 0.5 1° and 0.62 ° C. may be due entirely to dietary conditions, but if any marked variation is noted it can in most cases be traced to a dis- ordered kidney function. The total amount of blood in the body has been variously estimated at from one-twelfth to one-fourteenth of the body weight. Perhaps 1/13.5 is the most satisfactory figure. Among the most important constituents of blood plasma are the four protein bodies, fibrinogen, nucleoprotein, serum globulin (eu- globulin and pseudo-globulin) and scrum albumin. Plasma con- tains about 8.2 per cent of solids of which the protein constituents named above constitute approximately 84 per cent and the inor- ganic constituents (mainly chlorides, phosphates and carbonates) approximately 10 per cent. Among the inorganic 'constituents sodium chloride predominates. To prevent coagulation, blood plasma is ordinarily studied in the form of an oxalated or salted 1 Recently it has been shown by physico-chemical methods that the blood is in reality neutral in reaction. 182 BLOOD. 183 plasma. The former may be obtained by allowing the blood to flow from an opened artery into an equal volume of 0.2 per cent ammonium oxalate solution, whereas in the preparation of a salted plasma 10 per cent sodium chloride solution may be used as the diluting fluid. Fibrinogen is perhaps the most important of the protein con- stituents of the plasma. It is also found in lymph and chyle as well as in certain exudates and transudates. Fibrinogen possesses the general properties of the globulins, but differs from serum globu- lin in being precipitated upon half -saturation with sodium chloride. In the process of coagulation of the blood the fibrinogen is trans- formed into fibrin. This fibrin is one of the principal constituents of the ordinary blood-clot. The nucleoprotein of blood possesses many of the characteristics of serum globulin. In common with this body it is easily soluble in sodium chloride, and is completely precipitated from its solu- tions upon saturation with magnesium sulphate. It is much less soluble in dilute acetic acid than serum globulin and its solutions coagulate at 6$°-6g° C. The body formerly called serum globulin is probably not an in- dividual substance. Recent investigations seem to indicate that it may be resolved into two individual bodies called eu globulin and pseudo globulin. The euglobulin is practically insoluble in water and may be precipitated in the presence of 28-36 per cent of saturated ammonium sulphate solution. The pseudoglobulin, on the contrary, is soluble in water and is only precipitated by ammonium sulphate in the presence of from 36 to 44 per cent of saturated ammonium sulphate solution. In common with serum globulin the body known as serum albu- min seems also to consist of more than a single individual sub- stance. The so-called serum albumin may be separated into at least two distinct bodies, one capable of crystallization, the other an amor- phous body. The solution of either of these bodies in water gives the ordinary albumin reactions. The coagulation temperature of the serum albumin mixture as it occurs in serum or plasma varies from 700 to 85 ° C. according to the reaction of the solution and its content of inorganic material. Serum albumin differs from egg albumin in being more lsevorotatory, in being rendered less insolu- ble by alcohol, and in the fact that when precipitated by hvdro- chloric acid it is more easily soluble in an excess of the reagent. 184 PHYSIOLOGICAL CHEMISTRY. When blood coagulates and the usual clot forms, a light yellow fluid exudes. This is blood serum. It differs from blood plasma in containing a large amount of fibrin ferment, a body of great importance in the coagulation of the blood, and also in possessing a lower protein content. The protein material present in plasma and not found in serum is the fibrinogen which is transformed into fibrin in the process of coagulation and removed. The specific gravity of the serum of human blood varies between 1.026 and 1.032. If blood be drawn into a vessel and allowed to remain with- out stirring or agitation of any sort the major portion of the red corpuscles will sink away from the upper surface, causing this portion of the clot to assume a lighter color due to the predomin- ance of leucocytes. This light-colored portion of the clot is called the "buffy coat." Beside the protein constituents already mentioned, other bodies which are found in both the plasma and serum are the following: Sugar (dextrose), fat, enzymes, lecithin, cholesterol and its esters, gases, coloring-matter (lutein or lipochrome) and mineral sub- stances. In addition to these bodies the following substances have been detected in normal human blood : Creatine, carbamic acid, hip- puric acid, paralactic acid, urea and uric acid {urates). Some of the pathological constituents of blood are proteoses, leucine, tyrosine and other amino acids, biliary constituents and purine bodies. There has recently been considerable controversy regarding the form of the erythrocytes or red blood corpuscles of human blood. It is claimed by some investigators that the cells are bell-shaped or cup-shaped. As the erythrocytes occur normally in the circulation, however, they are probably thin, non-nucleated, biconcave discs. When examined singly under the microscope, they possess a pale greenish-yellow color (see Plate IV, opposite), whereas when grouped in large masses a reddish tint is noted. The blood of most mammals contains erythrocytes similar in form to those of human blood. In the blood of birds, fishes, am- phibians and reptiles the erythrocytes are ordinarily more or less elliptical, biconvex and possess a nucleus. The erythrocytes vary in size with the different animals. The average diameter of the erythrocytes of blood from various species is given in the follow- ing table ■} 1 Wormley's Micro-Chemistry of Poisons, second edition, p. 733. PLATE IV. Normal Erythrocytes and Leucocytes. BLOOD. I CH N-C-N / CH Hypoxanthine, C5H4N40. 6-oxypurine. HN-CO OC C-NH I II \ I II / HN-C-NH Uric Acid, C5H4N4O3. 2-6-8-trioxyp u rin e. CO 'N-C6 ,V C5-N- \c, 3N-G4-N, Purine Nucleus. HN-CO OC C-NH / CH HN-C-N Xanthine, CsH^XiOn 2-6-dioxypurin e. N-CNHo HC C-NH \ / CH N-C-N Adenine, C5H5Nt3. 6-aminopurine. HN-CO H„NC C-NH II II \ N-C-N Guanine, C5H.-,X.-,0. 2-amino-6-oxy purine. Experiments on Muscular Tissue. I. Experiments on " Living " Muscle. i. Preparation of Muscle Plasma (Halliburton). — Wash out the blood vessels of a freshly killed rabbit with 0.9 per cent sodium 17 242 PHYSIOLOGICAL CHEMISTRY. chloride. This can best be done by opening the abdomen and in- serting a cannula into the aorta. Now remove the skin from the lower limbs, cut away the muscles and divide them into very small pieces by means of a meat chopper. Transfer the pieces of muscle to a mortar and grind them with clean sand and a little 5 per cent magnesium sulphate. Filter off the salted muscle plasma and make the following tests : (a) Reaction. — Test the reaction to litmus. What is the reac- tion of this fresh muscle plasma? (b) Fractional Coagulation. — Place a little muscle plasma in a test-tube and arrange the apparatus for fractional coagulation as explained on page 100. Raise the temperature very carefully from 30 ° C. and note any changes which may occur and the exact tem- perature at which such changes take place. When the first protein (para-myosinogen) coagulates filter it off and then heat the clear filtrate as before, being careful to note the exact temperature at which the next coagulation (myosinogen) occurs. There will probably be a preliminary opalescence in each case before the real coagulation occurs. Therefore do not mistake the real coagulation- point and filter at the wrong time. What are the coagulation tem- peratures of these two proteins? Which protein was present in greater amount? (c) Formation of the Myosin Clot. — Dilute a portion of the plasma with 3 or 4 times its volume of water and place it on a water-bath or in an incubator at 35 ° C. for several hours. A typical myosin clot should form. Note the muscle serum surround- ing the clot. Now test the reaction. Has the reaction changed, and if so to what is the change due? Make a test for lactic acid. What do you conclude? 2. Preparation of Muscle Plasma (v. Fiirth). — Remove the blood-free muscles of a rabbit as explained on page 241. Finely divide by means of a meat chopper and grind in a mortar with a little clean sand and some 0.9 per cent sodium chloride. Wrap portions of the muscle in muslin and press thoroughly by means of a tincture press or lemon squeezer. Filter and make the tests according to the directions given in the last experiment. 3. " Fuchsin-Frog " Experiment. — Inject a saturated aqueous solution of Fuchsin " S " into the lymph spaces of a frog three or four times daily for two or three days, in this way thoroughly satu- rating the tissues with the dye. Pith the animal (insert a heavy wire or blunt needle through the occipito atlantoid membrane), re- MUSCULAR TISSUE. 243 move the skin from both hind legs and expose the sciatic nerve in one of them. Insert a small wire hook through the jaws of the frog and suspend the animal Erom an ordinary clamp or iron ring. Pass electrodes under the exposed sciatic nerve, and after tying the other leg to prevent any muscular movement, stimulate the exposed nerve by means of make and break shocks from an induc- tion coil. The stimulated leg responds by pronounced muscular con- tractions, whereas the tied leg remains inactive. Continue the stim- ulation until the muscles are fatigued. The muscular activity has caused the production of lactic acid and this in turn has reacted with the injected fuchsin to cause a pink or red color to develop. The muscles of the inactive leg still remain unchanged in color. The normal color of the Fuchsin " S " when injected was red, but upon being absorbed it became colorless through the action of the alkalinity of the blood. Upon stimulating the muscles, how- ever, as above explained, lactic acid was formed and this acid re- acted with the fuchsin and again produced the original color of the dye. II. Experiments on " Dead " Muscle. i. Preparation of Myosin. — Take 25 grams of finely divided lean beef which has been carefully washed to remove blood and lymph constituents and place it in a beaker with 10 per cent sodium chloride. Stir occasionally for several hours. Strain off the meat pieces by means of cheese cloth, filter the solution and saturate it with sodium chloride in substance. Filter off the precipitate of my- osin and make the tests as given below. This filtration will pro- ceed very slowly. Myosin collects as a film on the sides of the filter paper and may be removed and tested before the entire volume of fluid has been filtered. If this precipitate remains for any length of time on the paper in contact with the air it will become trans- formed into the protean myosan. Test the myosin precipitate as follows : (a) Solubility. — Try its solubility in the ordinary solvents. Is myosin an albumin or a globulin? (b) Xanthoproteic Reaction. — See page 91. (c) Coagulation Test. — Suspend a little of the myosin in water in a test-tube and heat to boiling for a few moments. Now re- move the suspended material and try its solubility in 10 per cent sodium chloride. What property does this experiment show myosin to possess ? Test the filtrate from the original myosin precipitate as follows : (a) Biuret Test. — What does this show ?J 244 PHYSIOLOGICAL CHEMISTRY. (b) Place a little of the solution in a test-tube and heat to boiling. At the boiling-point add a drop of dilute acetic acid and filter. Test this filtrate for proteose with picric acid. Is any proteose present ? Saturate another portion of the filtrate with ammonium sulphate and test for peptone in the usual way (see page 114). Do you find any peptone? From your experiments on "living" and " dead " muscle what are your ideas regarding the proteins of muscle ? 2. Preparation of Glycogen. — Grind a few scallops in a mor- tar with sand. Transfer to an evaporating dish, add water and boil for 20 minutes. At the boiling-point faintly acidify with acetic acid. Why is this acid added ? Filter, and divide the filtrate into two parts. Note the opalescence of the solution. Test one portion of the filtrate as follows : (a) Iodine Test. — To 5 c.c. of the solution in a test-tube add 5-10 drops of iodine solution and 2-3 drops of 10 per cent sodium chloride. What do you observe? Is this similar to the iodine test upon any other body with which we have had to deal ? (&) Reduction Test. — Does the solution reduce Fehling's solu- tion? (c) Hydrolysis of Glycogen. — Add 10 drops of concentrated hydrochloric acid to 10 c.c. of the solution and boil for 10 minutes. Cool the solution, neutralize with solid potassium hydroxide and test with Fehling's solution. Does it still fail to reduce Fehling's solution? If you find a reduction how can you prove the identity of the reducing substance? (d) Influence of Saliva. — Place 5 c.c. of the solution in a test- tube, add 5 drops of saliva and place on the water-bath at 400 C. for 10 minutes. Does this now reduce Fehling's solution? To the second part of the glycogen filtrate add 3-4 volumes of «95 per cent alcohol. Allow the glycogen precipitate to settle, de- cant the supernatant fluid, filter the remainder and upon the glyco- gen make the following tests : (a) Solubility. — Try its solubility in the ordinary solvents. (b) Iodine Test. — Place a small amount of the glycogen in a de- pression of a test-tablet and add 2-3 drops of dilute iodine solution and a trace of a sodium chloride solution. The same wine-red color is observed as in the iodine test upon the glycogen solution. MUSCULAR TISSUE. 245 Separation of Extractives from Muscle. 1. Creatine. — Dissolve about 10 grams of a commercial extract of meat in 200 c.c. of warm water. Precipitate the inorganic constituents by neutral lead acetate, being careful not to add an ex- cess of the reagent. Write the equations for the reactions taking place here. Allow the precipitate to settle, then filter and remove the excess of lead in the zvarm filtrate by hydrogen sulphide. Filter while the solution is yet warm, evaporate the clear filtrate to a syrup and allow it to stand at least 48 hours in a cool place. Crys- tals of creatine should form at this point. Examine under the microscope (Fig. yy, page 238). Treat the syrup with 200 c.c. of 88 per cent alcohol, stir well with a glass rod to bring all soluble material into solution, and then filter. The purine bases have been dissolved and are in the filtrate, whereas the creatine crystals were insoluble in the 88 per cent alcohol and remain on the filter paper. Wash the crystals with 88 per cent alcohol, then remove them and bring them into solution in a little hot water. Decolorize the solu- Fig. 79. Hypoxanthine Silver Nitrate. tion by animal charcoal and concentrate it to a small volume. Allow the solution to cool and note the separation of colorless crys- tals of creatine. Examine these crystals under the microscope and compare them with those reproduced in Fig. yy, page 238. 2. Hypoxanthine. — Evaporate the alcoholic filtrate from the creatine to remove the alcohol. Make the solution ammoniacal and add ammoniacal silver nitrate until precipitation ceases. The 246 PHYSIOLOGICAL CHEMISTRY. precipitate consists principally of hypoxanthine silver and xanthine silver. Collect these silver salts on a filter paper and wash them with water. Place the precipitate and paper in an evaporating dish and boil for one minute with nitric acid having a specific gravity of 1.1. Filter while hot through a double paper, wash with the same strength of nitric acid and allow the solution to cool. By this treatment with nitric acid hypoxanthine silver nitrate and xan- thine silver nitrate have been formed. The former is insoluble in the cold solution and separates on standing. After standing several hours filter off the hypoxanthine silver nitrate and wash with water until the wash-water is only slightly acid in reaction. Ex- amine the crystals of hypoxanthine silver nitrate under the micro- scope and compare them with those in Fig. 79, page 245. Now wash the crystals from the paper into a beaker with a little water and warm the liquid. Remove the silver by hydrogen sulphide and filter. By this means hypoxanthine nitrate has been formed and is present in the filtrate. Concentrate on a water-bath to drive off hydrogen sulphide and render the solution slightly alkaline with ammonia. Warm for a time, to remove the free ammonia, filter, concentrate the filtrate to a small volume and allow it to stand in a cool place. Hypoxanthine should crystallize in small colorless needles. Examine the crystals under the microscope. 3. Xanthine. — To the filtrate from the above experiment con- taining the xanthine silver nitrate add ammonia in excess. (The crystalline form of xanthine silver nitrate is shown in Fig. 80, p. 247.) A brownish-red precipitate of xanthine silver forms. Treat this suspended precipitate with hydrogen sulphide (do not use an excess of hydrogen sulphide), warm the mixture for a few moments and filter while hot. Concentrate the filtrate to a small volume and put away in a cool place for crystallization (Fig. 78, p. 239). To obtain xanthine in crystalline form special precautions are generally necessary. Evaporate the solution to dryness. Make the following tests on the crystals or residue : (a) Xanthine Test. — Place about one-half of the crystalline or amorphous material in a small evaporating dish, add a few drops of concentrated nitric acid and evaporate to dryness very carefully on a water-bath. The yellow residue upon moistening with caustic potash becomes red in color and upon further heating assumes a purplish-red hue. Now add a few drops of water and warm. In this way a yellow solution results which yields a red residue upon evaporation. . How does this differ from the Murexide test upon uric acid? MUSCULAR TISSUE. 247 (b) W ridel's Reaction. — By gently heating bring the remain- der of the xanthine crystals or residue into solution in bromine- water. Evaporate the solution to dryness on a water-bath. Re- move the stopper from an ammonia bottle and by blowing across Fig. 8c Xanthine Silver Nitrate. the mouth of the bottle direct the fumes of ammonia so that they come in contact with the dry residue. Under these conditions the presence of xanthine is shown by the residue assuming a red color. A somewhat brighter color may be obtained by using a trace of nitric acid with the bromine-water. By the use of this modification however we may get a positive reaction with bodies other than xanthine. Hurthle's Experiment. Tease a very small piece of frog's muscle on a microscopical slide. Expose the slide to ammonia vapor for a few moments, then ad- just a cover glass and examine the muscle fibers under the micro- scope. Note the large number of crystals of ammonium magnesium phosphate, NH4-0 \ Mg-O— P = 0 \/ 0 distributed everywhere throughout the muscle fiber, thus demon- strating the abundance of phosphates and magnesium in the muscle (Fig. 96, page 301). CHAPTER XVI. NERVOUS TISSUE. In common with the other solid tissues of the body, nervous tissue contains a large amount of water. The percentage of water present depends upon the particular form of nervous tissue but in all forms it is invariably greater in the gray matter than in the white. Embryonic nervous tissues also contain a larger percentage of water than the tissues of adult life. The gray matter of the brain of the foetus, for instance, contains about 92 per cent of water, whereas the gray matter of the brain of the adult contains but 83-84 per cent of the fluid. Among the solid constituents of nervous tissue are proteins, chol- esterol, cerebrin, lecithin, kephalin, protagon (f), paranucleopro- tagon, nuclein, neurokeratin, collagen, extractives and inorganic salts. The proteins are present in the greatest amount and com- prise about 50 per cent of the total solids. Three distinct proteins, two globulins and a nucleoprotein, have been isolated from nervous tissue. The globulins coagulate at 47 ° C. and 70-75 ° C. respec- tively, while the nucleoprotein coagulates at 56-600 C. This nuc- leoprotein contains about 0.5 per cent of phosphorus (Hallibur- ton, Levene). Nervous tissue is composed of a relatively large quantity of a variety of compounds which collectively may be grouped under the term " lipoid " — substances resembling the fats in some of their physical properties and reactions but distinct in their composition. We will class cerebrin, cholesterol and the phosphorized fats, as " lipoids." The group of phosphorized fats are very important constituents of nervous tissue. The best known members of this group are lecithin, protagon (f) and kephalin. Lecithin occurs in larger amount than the other members of the group, has been more thor- oughly studied than the others and is apparently of greater impor- tance. Upon decomposition lecithin yields fatty acid, glycero-phos- phoric acid and choline. Each lecithin molecule contains two fatty acid radicals which may be those of the same or different fatty acids. Thus we have different lecithins depending upon the particu- 248 NERVOUS TISSUE. 249 lar fatty acid radicals which are present in the molecule. The for- mula of a typical lecithin would be the following: J CH20-C17H35CO JHO -C17H3BCO CH90-P0-0-C,H4 \ (CH3)3-N / OH HO This lecithin would be called distearyl-lecithin or choline-distearyl- glycero-phosphoric acid. Upon decomposition the molecule splits according to the following reaction : C44H90NPO9+3H2O=2(C18H3GO2)+C.,H0PO6+C5H15NO2. Lecithin. Stearic acid. Glycero-phosphoric Choline. acid. The lecithins are not confined to the nervous tissues but are found in nearly all animal and vegetable tissues. Lecithin is a primary constituent of the cell. It is soluble in chloroform, ether, alcohol, benzene and carbon disulphide. The chloroform or alcohol-ether solution may be precipitated by acetone. Lecithin may be caused to crystallize in the form of small plates by cooling the alcoholic solu- tion to a low temperature. It has the power of combining with acids and bases, and the hydrochloric acid combination has the power of forming a double salt with platinic chloride. Choline, as was indicated above, is one of the decomposition products of lecithin. It is trimethyl-oxyethyl-ammonhtm hydroxide and has the following formula : CH2CH2(OH) / N-(CH3)3 \ OH Recent researches have shown that great importance is to be attached to the detection of choline in the cerebro-spinal fluid and the blood in certain cases of degenerative disease of the nervous system. In this connection tests for choline (see p. 252) are of interest and value. Protagon, another nitrogenous phosphorized substance is a body 25O PHYSIOLOGICAL CHEMISTRY. over which there has been much discussion. Upon decomposition it is said by some investigators to yield cerebrin and the decomposi- tion products of lecithin. It has recently been shown by Posner and Gies as well as by Rosenheim and Tebb that protagon is a mixture and has no existence as a chemical individual. Kephalin is the third member of the group of phosphorized fats. It is precipitated from its acetone-ether extract by alcohol. It contains about 4 per cent of phosphorus and has been given the formula C42H79NP013. Kephalin may be a stage in lecithin meta- bolism. Cerebrin, a substance containing nitrogen but no phosphorus, is an important constituent of the white matter of nervous tissue. It has also been found in the spleen, pus and in egg yolk. It may be extracted from the tissue by boiling alcohol and is insoluble in cold alcohol, cold and hot ether and in water and dilute alkalis. Cerebrin is a mixture containing phrenosin (pseudo-cerebrin or cerebron), a body yielding the carbohydrate galactose on decom- position. Cholesterol, one of the primary cell constituents, is present in fairly large amount in nervous tissue. It is a mon-atomic alcohol with the formula C27H45OH. It was formerly called a "non-sap- onifiable fat " but since it is not changed in any way by boiling al- kalis it is not a fat. It is soluble in ether, chloroform, benzene and hot alcohol. It crystallizes in the form of thin, colorless, transparent plates (Fig. 42, p. 159). Cholesterol occurs abundantly in one form of biliary calculus. It has also been found in feces, wool fat, egg yolk, and milk, frequently in the form of its esters of higher fatty acids. Paranucleoprotagon is a phosphorized substance originally iso- lated from brain tissue by Ulpiani and Lelli and recently reinvesti- gated by Steel and Gies. It is said to possess lecithoprotein char- acteristics. Nervous tissue yields about 1 per cent of ash which is made up in great part of alkaline phosphates and chlorides. Experiments on the Lipoids of Nervous Tissue.1 1. Preparation of Lecithin. — Treat the macerated brain of a sheep with ether and allow it to stand in the cold for 48-72 1 Preparation of So-called Protagon. — Macerate the brain of a sheep, treat with 85 per cent alcohol and warm on a water-bath at 450 C. for two hours. Filter hot into a bottle or strong flask and cool to 0° C. for one-half hour by NERVOUS TISSUE. 25 I hours. The cold ether will extract lecithin and cholesterol. Filter and add acetone to the filtrate to precipitate the lecithin. Filter off the lecithin and test it as follows : (a) Microscopical Examination. — Suspend a small portion in a drop of water on a slide and examine under the microscope. (b) Osmic Acid Test. — Treat a small portion with osmic acid. What happens? (c) Acrolein Test. — Make the acrolein test according to direc- tions on page 135. (d) "Fusion" Test for Phosphorus. — Place some of the leci- thin prepared above in a small porcelain crucible, add a suitable amount of a fusion mixture composed of potassium hydroxide and potassium nitrate (5:1) and heat carefully until the resulting mixture is colorless. Cool, dissolve the mass in a little warm water, acidify with nitric acid, heat to boiling and add a few cubic centi- meters of molybdic solution. In the presence of phosphorus a yellow precipitate forms. What is it? 2. Preparation of Cholesterol. — Place a small amount of mac- erated brain tissue under ether and stir occasionally for one hour. Filter, evaporate the filtrate to dryness on a water-bath and test the cholesterol according to directions given below. (If it is de- sired, the ether extract from the so-called protagon, or the ether- acetone filtrate from the lecithin may be used for the isolation of cholesterol. In these cases it is simply necessary to evaporate the solution to dryness on a water-bath.) Upon the cholesterol pre- pared by either of the above methods make the following tests : (a) Microscopical Examination. — Examine the crystals under the microscope and compare them with those in Fig. 42, page 159. (b) Iodine -Sulphuric Acid Test. — Place a few crystals of chol- esterol in one of the depressions of a test-tablet and treat with a drop of concentrated sulphuric acid and a drop of a very dilute solu- tion of iodine. A play of colors, consisting of violet, blue, green and red, results. (c) The Liebcrmann-Bur chard Test. — Dissolve a few crystals of cholesterol in 2 c.c. of chloroform in a dry test-tube. Now add 10 drops of acetic anhydride and 1-3 drops of concentrated sulphuric acid. The solution becomes red, then blue, and finally bluish-green in color. means of a freezing mixture. By this procedure both protagon and choles- terol are caused to precipitate. Filter the cold solution rapidly and treat the precipitate on the paper with ice cold ether to dissolve out the cholesterol. The protagon may now be redissolved in warm 85 per cent alcohol from which solution it will precipitate upon cooling. 252- PHYSIOLOGICAL CHEMISTRY. (d) Salkowski's Test. — Dissolve a few crystals of cholesterol in a little chloroform and add an equal volume of concentrated sul- phuric acid. A play of colors from bluish-red to cherry-red and purple is noted in the chloroform, while the acid assumes a marked green fluorescence. (e) Schiff's Reaction. — To a little cholesterol in an evaporating dish add a few drops of Schiff's reagent.1 Evaporate to dryness over a low flame and observe the reddish-violet residue which changes to a bluish-violet. (/) Phosphorus. — Test for phosphorus according to directions given on page 251. Is phosphorus present ? 3. Preparation of Cerebrin. — Treat the macerated brain tissue, in a flask, with 95 per cent alcohol and boil on a water-bath for one-half hour, keeping the volume constant by adding fresh alcohol as needed. Filter the solution hot and stand the cloudy filtrate away for twenty-four hours. (If the filtrate is not cloudy concentrate it upon the water-bath until it is so.) Filter off the cerebrin and test it as follows : (a) Microscopical Examination. — Suspend a small portion in a drop of water on a slide and examine under the microscope. (b) Solubility. — Try the solubility of cerebrin in the usual sol- vents and in hot and cold alcohol and hot and cold ether. (c) Phosphorus. — Test for phosphorus according to directions on page 251. How does the result compare with that on lecithin? (d) Place a little cerebrin on platinum foil and warm. Note the odor. ( ute febrile diseases. Chyluria. Purulent diseases of the urinary tract. Santonin, chrysophanic acid. Haematoporphyrin. Unchanged haemoglobin. Pigments in food (log- wood, madder, bilberries, fuchsin). Haematin. Methaemoglobin. Melanin. Hydrochinon and catechol. Bile-pigments. A dark-blue scum on sur- face, with a blue deposit, due to an excess of indi- go- forming substances. Haemorrhages, or haemo- globinuria. Small haemorrhages. Methaemoglobinuria. Melanotic sarcoma. Carbolic-acid poisoning. Jaundice. Cholera, typhus ; seen espe- cially when the urine is putrefying. Substances contained in senna, rhubarb, and che- lidonium which are in- troduced into the sys- tem. Transparency. — Normal urine is ordinarily perfectly clear and transparent when voided. On standing for a variable time however, a cloud (nubecula) consisting principally of nucleoprotein or mu- coid (see p. 320) and epithelial cells forms. A turbidity due to the precipitation of phosphates is normally noted in urine passed after a hearty meal. The urine obtained 2-3 hours after a meal or later is xThis dirty green or blue color also occurs after the use of methylene-blue in the organism. 256 PHYSIOLOGICAL CHEMISTRY. ordinarily free from turbidity. Permanently turbid urines ordinar- ily arise from' pathological conditions. Odor. — The odor of normal urine is of a faint, aromatic type. The bodies to which this odor is due are not well known, but it is claimed by some investigators to be due, at least in part, to the presence of minute amounts of certain volatile organic acids. When the urine undergoes decomposition, e. g., in alkaline fermen- tation a very unpleasant ammoniacal odor is evolved. All urines are subject to such decomposition if allowed to stand for a suffi- ciently long time. Under normal conditions the urine very often possesses a peculiar odor due to the ingestion of some certain drug or vegetable. For instance, cubebs, copaiba, myrtol, saffron, tolu and turpentine each imparts a somewhat specific odor to the urine. After the ingestion of asparagus, the urine also possesses a typical odor. Frequency of Urination. — The frequency of urination varies greatly in different individuals but in general is dependent upon the amount of fluid in the bladder. In pathological conditions an inflam- matory affection of the urinary tract or any disturbance of the in- nervation of the bladder will influence the frequency. Affections of the spinal cord which lead to an increased irritability of the blad- der or a weakening of the sphincter will result in increasing the fre- quency of urination. Reaction. — The mixed twenty-four hour urinary excretion of a normal individual ordinarily possesses an acid reaction to litmus. This acidity is now believed to be due to the presence of various acidic radicals and not to the presence of sodium di-hydrogen phos- phate as was formerly held (see Phosphates, p. 299). This con- clusion is reinforced by the observation that urine may be divided into two portions, one part consisting almost entirely of inorganic matter, including practically all of the phosplmtes and having an alkaline reaction, the other containing practically all of the organic substances and no phosphates and having an acid reaction. The acidity imparted to the urine by any particular acid depends entirely upon the extent to which the acid is dissociable, since it is the hy- drogen ion which is responsible for the acid reaction. The composition of the food is perhaps the most important factor in determining the reaction of the urine. The reaction ordinarily varies considerably according to the time of day the urine is passed. For instance for a variable length of time after a meal the urine may be neutral or even alkaline in reaction to litmus, owing to the URINE. 257 claim of the gastric juice upon the acidic radicals to further the formation of hydrochloric acid for use in carrying' out the diges- tive secretory function. This change in reaction is known as the alkaline tide and is common to perfectly healthy individuals. The urine may also become temporarily alkaline in reaction to litmus, as the result of ingesting alkaline carbonates or certain salts of tar- Fig. 81. Deposit in Ammoniacal Fermentation. a, Acid ammonium urate ; b, ammonium magnesium phosphate ; c, bacteria. Fig. 82. ■ *& rmM ._ b Redraw tf^<* 1 $ "h, CK ^ .* J \ ; Deposit in Acid Fermentation. a, Fungus, b, amorphous sodium urate ; c, uric acid ; d, calcium oxalate. taric and citric acids which may be transformed into carbonates within the organism. Normal urine upon standing for some time becomes alkaline in reaction to litmus, owing to the inception of al- kaline or ammoniacal fermentation through the agency of micro- organisms. This fermentation has no especial diagnostic value 258 PHYSIOLOGICAL CHEMISTRY. Fig. 83. /nCI^ except in cases where the urine has undergone this change within the organism and is voided in the decomposed state. Ammonia- cal fermentation is ordinarily due to cystitis or occurs as the result of infection in the process of catheterization. A microscopical ex- amination of such urine (Fig. 81, p. 257) shows the presence of ammonium magnesium phosphate crystals, amorphous phosphates and not infrequently ammonium urate. Occasionally a urine which possesses a normal acidity when voided, upon standing instead of undergoing am- moniacal fermentation as above described will be- come still more strongly acid in reaction. Such a phenomenon is termed acid fermentation. Accom- panying this increased acidity there is ordinarily a deepening of the tint of the urinary color. Such urines may contain acid urates, uric acid, fungi and calcium oxalate (Fig. 82, p. 257). On standing for a sufficiently long time any urine which exhibits acid fermentation will ultimately change in reaction, due to the inception of alkaline fermentation, and will show the microscopical deposits characteristic of such a urine. Specific Gravity. — The specific gravity of the urine of normal individuals varies ordinarily be- tween 1. 01 5 and 1.025. This value is subject to wide fluctuations under various conditions. For in- stance following copious water- or beer-drinking the specific gravity may fall to 1.003. or lower, whereas in cases of excessive perspiration it may rise as high as 1.040 or even higher. Where a very accu- rate determination of the specific gravity is desired use is commonly made of the pyknometer or of the Westphal hydrostatic balance. These instruments, however, are not suited for clinical use. The clinical method of determining the specific gravity is by means of a urinometer (Fig. 83, p. 258). This affords a very rapid method and at the same time is sufficiently accurate for clinical purposes. The urinometer is always calibrated for use at a specific temperature and the observations made at any other temperature must be sub- jected to a certain correction to obtain the true specific gravity. In making this correction one unit of the last order is added to the observed specific gravity for every three degrees above the normal Urinometer and Cylinder. URINE. 259 temperature and subtracted for every three degrees below the nor- mal temperature. For instance, if in using a urinometer calibrated for 15° C. the specific gravity of a urine having a temperature of 21 C. is determined as 1.018 it is necessary to add to the observed specific gravity two units of the third order to obtain the real spe- cific gravity of the urine. Therefore the true specific gravity, at 1 5° C, of a urine having a specific gravity of [.Ol8 at 21 ° C. is 1. 018 -f 0.002 = 1.020. Pathologically, the specific gravity may he subjected to very wide variations. This is especially true in diseases of the kidneys. In acute nephritis ordinarily the urine is concentrated and of a high specific gravity, whereas in chronic nephritis the reverse conditions are more apt to prevail. In fact under most conditions, whether physiological or pathological, the specific gravity of the urine is in- versely proportional to the volume excreted. This is not true of diabetes mellitus, however, where the volume of urine is large and the specific gravity is also high, owing to the sugar contained in the urine. The amount of solids eliminated in the excretion for twenty-four hours may be roughly calculated by means of Long's coefficient, i. e., 2.6. The solid content of 1,000 c.c. of urine is obtained by multiplying the last two figures of the specific gravity observed at 25 ° C. by 2.6. To determine the amount of solids excreted in twenty-four hours if the volume was 1,120 c.c. and the specific grav- ity was 1. 018 the calculation would be as follows: (a) 18X2.6 = 46.8 grams of solid matter in 1,000 c.c. of urine. f, N 46.8 X 1 120 . \o) -— -== ^2.4 grams of solid matter in 1.120 c.c. of 1000 ° & urine. The coefficient of Haser (2.33) which has been in use for years probably gives values that are inaccurate for conditions existing in America. This coefficient was calculated on the basis of the specific gravity determined at a temperature of 150 C. Freezing-Point (Cryoscopy). — The freezing-point of a solu- tion depends upon the total number of molecules of solid matter dissolved in it. The determination of the osmotic pressure by this method has recently come to be of some clinical importance particularly as an aid in the diagnosis of kidney disorders. In this connection it is best to collect the urine from each kidney separately and determine the freezing-point in the individual samples so col- 260 PHYSIOLOGICAL CHEMISTRY. Fig lected. By this means considerable aid in the diagnosis of renal diseases may be secured. The fluids most frequently examined cryoscopically are the blood (seep. 182) and the urine. The freezing-point is denoted by A. The value of A for normal urine varies ordinarily between — 1.30 and — 2.30 C, the freezing-point of pure water being taken as o°. A is subject to very wide fluctuations under unusual conditions. For instance following copious water- or beer- drinking A may have as high a value as — 0.2 ° C. whereas on a diet containing much salt and deficient in fluids the value of A may be lowered to — 30 C. or even lower. The freezing-point of normal blood is gen- erally about — 0.560 C. and is not subject to the wide variations noted in the urine, be- cause of the tendency of the organism to maintain the normal osmotic pressure of the blood under all conditions. Variations be- tween — 0.5 1 ° and — 0.62 ° C. may be due entirely to dietary conditions but if any marked variation is noted it can, in most cases, be traced to a disordered kidney function. Freezing-point determinations may be made by means of the Beckmann-Heiden- hain apparatus (Fig. 84, p. 260) or the Zikel Pektoscope. The Beckmann - Heidenhain apparatus consists of the following parts : A strong battery jar or beaker (C) fur- nished with a metal cover which is provided with a circular hole in its center. This strong glass vessel serves to hold the freez- ing mixture by means of which the tem- perature of the fluid under examination is lowered. A large glass tube (B) designed as an air-jacket, and formed after the man- ner of a test-tube is introduced through the central aperture in the metal cover and into this air-jacket is low- ered a smaller tube (A) containing the fluid to be tested. A very Beckmann-Heidenhain Freezing-point Appa- ratus. (Long.) D, a delicate thermom- eter ; C, the containing jar ; B, the outside or air mantle tube ; A, the tube in which the mixture to be observed is placed. Two stirrers are shown, one for the cooling mix- ture in the jar and one for the experimental mix- ture. URINE. 26l delicate thermometer (D), graduated in hundredths of a degree is introduced into the inner tube and is held in place by means of a cork so that the mercury bulb is immersed in the fluid under ex- amination but does not come in contact with any glass surface. A small platinum wire stirrer serves to keep the fluid under examina- tion well mixed while a larger stirrer is used to manipulate the freez- ing mixture. (Rock salt and ice in the proportion 1 : 3 form a very satisfactory freezing mixture.) In making a determination of the freezing-point of a fluid by means of the Beckmann-Heidenhain apparatus proceed as follows : Place the freezing mixture in the battery jar and add water (if necessary) to secure a temperature not lower than 30 C. In- troduce the fluid to be tested into tube A, place the thermometer and platinum wire stirrer in position and insert the tube into the air jacket which has previously been inserted through the metal cover of the battery jar. Manipulate the two stirrers in order to insure an equalization of temperature and observe the course of the mercury column of the thermometer very carefully. The mer- cury will gradually fall and this gradual lowering of the tempera- ture will be followed by a sudden rise. The point at which the mercury rests after this sudden rise is the freezing-point. This rise is due to the fact that previous to freezing, a fluid is always more or less over cooled and the thermometer temporarily registers a temperature somewhat belozv. the freezing-point. As the fluid freezes however there is a very sudden change in the temperature of the liquid and this change is imparted to the thermometer and causes the rise as indicated. It occasionally occurs that the fluid under examination is very much over cooled and does not freeze. Under such circumstances a small piece of ice is introduced into it by means of the side tube noted in the figure. This so-called " inoculation " causes the fluid to freeze instantaneously. (For details of the method of determining the freezing-point consult standard works on physical or organic chemistry.) Electrical Conductivity. — The electrical conductivity of the urine is dependent upon the number of inorganic molecules or ions present, and in this differs from the freezing-point which is de- pendent upon the total number of molecules both inorganic and organic which are in solution. The conductivitv of the urine has been investigated but slightly, and this very recently, but from the data secured it seems that the value generally falls below * = 0.03. The conductivity of blood serum has been determined as * = 0.012. 262 PHYSIOLOGICAL CHEMISTRY. Up to the present time the determination of the electrical conduc- tivity of any of the fluids of the body has been put to very slight clinical use. Experience may show the conductivity value to be a more important aid to diagnosis than it is now considered, particu- larly if it is taken in connection with the determination of the freezing-point. By a combination of these two methods the por- tion of the osmotic pressure due respectively to electrolytes and non-electrolytes may be determined. For a discussion of electrical conductivity, the method by which it is determined and the princi- ples involved consult standard works on physical or electrochemis- try. Collection of the Urine Sample. — If any dependable data are desired regarding the quantitative composition of the urine the ex- amination of the mixed excretion for twenty-four hours is abso- lutely necessary. In collecting the urine the bladder may be emp- tied at a given hour, say 8 A. M., the urine discarded and all the urine from that hour up to and including that passed the next day at 8 A. M., saved, thoroughly mixed and a sample taken for analysis. Powdered thymol, CH3 \/OH CH3 — CH — CH3, is a very satisfactory preservative since the excess may be re- moved by nitration, if desired, and any small amount which may go into solution will have no appreciable influence upon the de- termination of any of the urinary constituents. It has no reducing power and so may safely be used to preserve diabetic urines. To insure the preservation of the mixed urine of the twenty-four hour period it is advisable to place a small amount of the thymol powder :in the urine receptacle before the first fraction of urine is voided. In order to further insure the preservation of the urine the cleaned and dried urine receptacle may' be rinsed with an alcoholic solution of thymol and subsequently thoroughly dried before introducing the urine. Toluene is also used for the preservation of urine. In certain pathological conditions it is desirable to collect the urine passed during the day separately from that passed during the URINE. 263 night. When this is done the urine voided between 8 A. M. and 8 P. M. may be taken as the day sample and that voided between 8 P. M. and 8 A. M. as the night sample. The qualitative testing of urine voided at random, except in a few specific instances, is of no particular value so far as giving us any accurate knowledge as to the exact urinary characteristics of the individual is concerned. In the great majority of cases the qualitative as well as the quantitative tests should be made upon the mixed excretion for a twenty-four hour period. CHAPTER XVIII URINE: PHYSIOLOGICAL CONSTITUENTS.1 i. Organic Physiological Constituents. Urea. Uric acid. Creatinine. Creatine. Ethereal sulphuric acids Hippuric acid. Oxalic acid. Neutral sulphur compounds. Allantom. Aromatic oxyacids Indoxyl-sulphuric acid. Phenol- and />-cresol-sulphuric acids. Pyrocatechin-sulphuric acid. , Skatoxyl-sulphuric acid. ' Cystine. Chondroitin-sulphuric acid. Thiocyanates. Taurine derivatives. Oxyproteic acid. Alloxyproteic acid. Uro ferric acid. Paraoxyphenyl-acetic acid. Paraoxyphenyl-propionic acid. Homogentisic acid. Uroleucic acid. Oxymandelic acid. ^Kynurenic acid. Benzoic acid. Nucleoprotein. Oxaluric acid. 1 It is impossible to make any absolute classification of the physiological and pathological constituents of the urine. A substance may be present in the urine in small amount physiologically and be sufficiently increased under cer- tain conditions as to be termed a pathological constituent. Therefore it de- pends, in some instances, upon the quantity of a constituent present whether it may be correctly termed a physiological or a pathological constituent. 264 URINE. 265 Enzymes Volatile fatty acids Paralactic acid. Phenaceturic acid. Phosphorized compounds. ' Pepsin. Gastric rennin. Amylase, f Acetic acid. «J Butyric acid. Formic acid. Pigments Ptomaines and leucomaines. Purine bases. j Glycerophosphoric acid. \ Phosphocarnic acid. 'Urochrome. Urobilin. Uroerythrin. Adenine. Guanine. Xanthine. Epiguanine. Episarkine. Hypoxanthine. Paraxanthine. Heteroxanthine. i-Methylxanthine. 2. Inorganic Physiological Constituents. Ammonia. Sulphates. Chlorides. Phosphates. Sodium and potassium. Calcium and magnesium. Carbonates. Iron. Fluorides. Nitrates. Silicates. Hydrogen peroxide. NH2 UREA, C=0. I NHo 266 PHYSIOLOGICAL CHEMISTRY. Urea is the principal end-product of the metabolism of protein substances. It has been generally believed that about 90 per cent of the total nitrogen of the urine was present as urea. Recently, however, Folin has shown that the distribution of the nitrogen of the urine among urea and the other nitrogen-containing bodies present depends entirely upon the absolute amount of the total nitrogen excreted. He found that a decrease in the total nitrogen excretion was always accompanied by a decrease in the percentage of the total nitrogen excreted as urea, and that after so regulating the diet of a normal person as to cause the excretion of total nitro- Fig. 85. Urea. gen to be reduced to 3-4 grams in 24 hours, only about 60 per cent of this nitrogen appeared in the urine as urea. His experiments also seem to show urea to be the only one of the nitrogenous ex- cretions which is relatively as well as absolutely decreased as a result of decreasing the amount of protean metabolized. This same investigator reports a hospital case in which only 14.7 per cent of the total nitrogen was present as urea and about 40 per cent was present as ammonia. Morner had previously reported a case in which but 4.4 per cent of the total nitrogen of the urine was present as urea, and 26.7 per cent was present as ammonia. Urea occurs most abundantly in the urine of man and carnivora and in somewhat smaller amount in the urine of herbivora; the urine of fishes, amphibians and certain birds also contains a small amount of the substance. Urea is also found in nearly all the fluids and in many of the tissues and organs of mammals. The amount URINE. 267 excreted under normal conditions, by an adult man in 24 hours is about 30 grams; women excrete a somewhat smaller amount. The excretion is greatest in amount after a diet of meat, and least in amount after a diet consisting of non-nitrogenous foods; this is due to the fact that the last mentioned diet has a tendency to de- crease the metabolism of the tissue proteins and thus cause the out- put of urea under these conditions to fall below the output of urea observed during starvation. The output of urea is also increased after copious water- or beer-drinking. This increase is probably due primarily to the washing out of the tissues of the urea previ- ously formed, but which had not been removed in the normal proc- esses, and, secondarily to a stimulation of protein catabolism. Urea may be formed in the organism from amino acids such as leucine, glycocoll and aspartic acid : it may also be formed from ammonium carbonate (NH4)2C03 or ammonium carbamate, H4N-OCONH2. There are differences of opinion regarding the transformation of the substances just named into urea but there is rather conclusive evidence that at least a part of the urea is formed in the liver ; it may be formed in other organs or tissues as well. Urea crystallizes in long, colorless, four or six-sided, anhydrous, rhombic prisms (Fig. 85, p. 266), which melt at 1320 C. and are soluble in water or alcohol and insoluble in ether or chloroform. If a crystal of urea is heated in a test-tube, it melts and decomposes with the liberation of ammonia. The residue contains cyanuric COH /\ N N II I HOC COH \// N acid, and biuret, NH2 I C = 0 \ NH / 0 = 0 I NIT., 268 PHYSIOLOGICAL CHEMISTRY. The biuret may be dissolved in water and a reddish-violet color ob- tained by treating the aqueous solution with cupric sulphate and potassium hydroxide (see Biuret Test, p. 92). Certain hypo- chlorites or hypobromites in alkaline solution have the power of decomposing urea into nitrogen, carbon dioxide and water. Sodium hypobromite brings about this decomposition, as follows : CO(NH2)2 + 3NaOBr = 3NaJBr + N2 + C02 + 2H20. This property forms the basis for a clinical quantitative determina- tion of urea (see page 374). Urea has the power of forming crystalline compounds with certain acids : urea nitrate and urea oxalate are the most important of these compounds. Urea nitrate, CO(NH2)2 -HN03, crystal- lizes ill colorless, rhombic or six-sided tiles (Fig. 86, below), which are easily soluble in water. Urea oxalate, 2 •CO(NH2)2-H2C204, crystallizes in the form of rhombic or six-sided prisms or plates (Fig. 88, p. 270) : the oxalate differs from the nitrate in being somewhat less soluble in water. A decrease in the excretion of urea is observed in many diseases in which the diet is much reduced and in some disorders as a result of alterations in metabolism, e. g., myxcedema, and in others as a result of changes in excretion, as in severe and advanced kidney dis- Fig. 86. Urea Nitrate. ease. A pathological increase is found in a large proportion of diseases which are associated with a toxic state. URINE. 269 Fig. 87. Experiments on Urea. 1. Isolation from the Urine. — Place 800 c.c. of urine in a pre- cipitating jar, add 250 c.c. of baryta mixture1 and stir thoroughly. Filter off the precipitate of phosphates, sulphates, urates and hip- purates and evaporate the filtrate on a water-bath to a thick syrup. This syrup contains chlorides, creatinine, organic salts, pigments and urea. Extract the syrup with warm 95 per cent alcohol and filter again. The filtrate contains the urea contaminated with pig- ment. Decolorize the filtrate by boiling with animal charcoal, filter again and stand the filtrate away in a cold place for crystallization. Examine the crystals under the microscope and compare them with those shown in Fig. 85, page 266. 2. Solubility. — Test the solubility of urea, prepared by yourself or furnished by the instructor, in the ordinary solvents (see p. 23) and in alcohol and ether. 3. Melting-Point. — Determine the melting- point of some pure urea furnished by the instructor. Proceed as follows : Into an ordi- nary melting-point tube, sealed at one end, introduce a crystal of urea. Fasten the tube to the bulb of a thermometer as shown in Fig. 87, p. 269, and suspend the bulb and its at- tached tube in a small beaker containing sul- phuric acid. Gently raise the temperature of the acid by means of a low flame, stirring the fluid continually, and note the tempera- ture at which the urea begins to melt. 4. Crystalline Form. — Dissolve a crystal of pure urea in a few drops of 95 per cent alcohol and place 1-2 drops of the alcoholic solution on a microscopic slide. Allow the alcohol to evaporate spontaneously, examine the crystals under the microscope and compare them with those reproduced in Fig. 85, p. 266. Recrystallize a little urea from water in the same way and compare the crystals with those obtained from the alcoholic solution. 5. Formation of Biuret. — Place a small amount of urea in a dry test-tube and heat carefully in a low flame. The urea melts at 1 Baryta mixture consists of a mixture of one volume of a saturated solution of Ba(NOs)2 and two volumes of a saturated solution of Ba(OH):. Melting-point Tubes Fastened to Bulb of Thermometer. 270 PHYSIOLOGICAL CHEMISTRY. 1320 C. and liberates ammonia. Continue heating until the fused mass begins to solidify. Cool the tube, dissolve the residue in dilute potassium hydroxide solution and add very dilute cupric sulphate solution (see p. 92). The purplish- violet color is due to the presence of biuret which has been formed from the urea through the application of heat as indicated. This is the reaction : NIL NH2 0 = 0 | \ 2.0 = 0 = NH + NH3 | / NH2 0 = 0 Urea. 1 NH2 Biuret. 6. Urea Nitrate. — Prepare a concentrated solution of urea by dissolving a little of the substance in a few drops of water. Place a drop of this solution on a microscopic slide, add a drop of con- FlG. Urea Oxalate. centrated nitric acid and examine under the microscope. Compare the crystals with those reproduced in Fig. 86, p. 268. 7. Urea Oxalate. — To a drop of a concentrated solution of urea, prepared as described in the last experiment (6), add a drop of a saturated solution of oxalic acid. Examine under the microscope and compare the crystals with those shown in Fig. 88, above. URINE. 271 8. Decomposition by Sodium-Hypobromite. — Into a mixture of 3 c.c. of concentrated sodium hydroxide solution and 2 c.c. of bromine water in a test-tube introduce a crystal of urea or a -.mall amount of a concentrated solution of urea. Through the influence of the sodium-hypobromitc, NaOBr, the urea is decomposed and carbon dioxide and nitrogen are liberated. The carbon dioxide is absorbed by the excess of sodium hydroxide while the nitrogen is evolved and causes the marked effervescence observed. This property forms the basis for one of the methods in common use for the quantitative determination of urea. Write the equation show- ing the decomposition of urea by sodium-hypobromite. 9. Furfurol Test. — To a few crystals of urea in a small por- celain dish add 1-2 drops of a concentrated aqueous solution of furfurol and 1-2 drops of a concentrated hydrochloric acid. Note the appearance of a yellow color which gradually changes into a purple. Allantoin also responds to this test (see page 287). HN-C uric acid, OC C— NH '^CO. HN-C-NH Uric acid is one of the most important of the constituents of the urine. It is generally stated that normally about 0.7 gram is ex- creted in 24 hours but that this amount is subject to wide variations, particularly under certain dietary and pathological conditions. Very recently it has been shown that the average daily excretion of uric acid for ten men ranging in age from 19 to 29 years and fed a normal mixed diet was 0.597 gram, a value somewhat lower than the generally accepted average of 0.7 gram for such a period. Uric acid is a diureide and consequently upon oxidation yields two molecules of urea. It acts as a weak dibasic acid and forms two classes of salts, neutral and acid. The neutral potassium and lith- ium urates are the most easily soluble of the alkali salts; the am- monium urate is difficultly soluble. The acid-alkali urates are more insoluble and form the major portion of the sediment which sepa- rates upon cooling concentrated urine ; the alkaline earth urates are very insoluble. Ordinarily uric acid occurs in the urine in the form of urates and upon acidifying the liquid the uric acid is liberated and deposits in crystalline form. This property forms the basis 272 PHYSIOLOGICAL CHEMISTRY. of one of the older methods for the quantitative determination of uric acid (Heintz Method, p. 373). Uric acid is very closely related to the purine bases as may be seen from a comparison of its structural formula with those of the purine bases given on page 241. According to the purine nomen- clature it is designated 2-6— 8-trioxypurine. Uric acid forms the principal end-product of the nitrogenous metabolism of birds and scaly amphibians; in the human organism it occupies the fourth position inasmuch as here urea, ammonia and creatinine are the chief end-products of nitrogenous metabolism. It is generally said that the relation existing between uric acid and urea in human urine under normal conditions varies on the average from 1 -.40 to 1 :ioo and is subject to wider variations under pathological conditions; and further that because of the high content of uric acid in the urine of new-born infants the ratio may be reduced to 1 :io or even lower. We now know that this ratio of uric acid to urea is of little significance under any conditions. In man, uric acid probably results principally from the destruc- tion of nuclein material. It may arise from nuclein or other purine material ingested as food ©r from the disintegrating cellular matter of the organism. The uric acid resulting from the first process is said to be of exogenous origin, whereas the product of the second form of activity is said to be of endogenous origin. As a result of experi- mentation, Siven, and Burian and Schur, and Rockwood claim that the amount of endogenous uric acid formed in any given period is fairly constant for each individual under normal conditions, and that it is entirely independent of the total amount of nitrogen elimi- nated. Recently Folin has taken exception to the statements of these investigators and claims that, following a pronounced decrease in the amount of protein metabolized, the absolute quantity of uric acid is decreased but that this decrease is relatively smaller than the decrease in the total nitrogen excretion and that the per cent of the uric acid nitrogen, in terms of the total nitrogen, is therefore de- cidedly increased. In birds and scaly amphibians the formation of uric acid is anal- ogous to the formation of urea in man. In these organisms it is derived principally from the protein material of the tissues and the food and is formed through a process of synthesis which occurs for the most part in the liver; a comparatively small fraction of the total uric acid excretion of birds and scaly amphibians may result from nuclein material. PLATE V. Uric Acid Crystals. Normal Color. (From Purdy, after Peyer.) URINE. 2/3 When pure, uric acid may be obtained as a white, odorless, and tasteless powder which is composed principally of small transparent crystalline rhombic plates. Uric acid as it separates from the urine is invariably pigmented, and crystallizes in a large variety of char- acteristic tonus, e. g.} dumb-bells, wedges, rhombic prisms, irregu- lar rectangular or hexagonal plates, whetstones, prismatic rosettes, etc. Uric acid is insoluble in alcohol and ether, soluble with diffi- cult}' in boiling' water (1:1800) and practically insoluble in cold water (1:39,480, at 18° C). It is soluble in alkalis, alkali car- bonates, boiling glycerol, concentrated sulphuric acid and in cer- tain organic bases such as ethylamine and piperidine. It is claimed that the uric acid is held in solution in the urine by the urea and disodium hydrogen phosphate present. L'ric acid possesses the power of reducing cupric hydroxide in alkaline solution and may thus lead to an erroneous conclusion in testing for sugar in the urine by means of Fehling's or Trommer's tests. A white precipitate of cuprous urate is formed if only a small amount of cupric hydroxide is present, but if enough of the copper salt is present the character- istic red or brownish-red precipitate of cuprous oxide is obtained. Uric acid does not possess the power of reducing bismuth in alka- line solution and therefore does not interfere in testing for sugar in the urine by means of Boettger's or Nylander's tests. In addition to being an important urinary constituent uric acid is normally present in the brain, heart, liver, lungs, pancreas and spleen ; it also occurs in the blood of birds and has been detected in traces in human blood under normal conditions. Pathologically, the excretion of uric acid is subject to wide vari- ations but the experimental findings are rather contradictorv. It may be stated with certainty, however, that in leukaemia the uric acid output is increased absolutely as well as relatively to the urea output; under these conditions the ratio between the uric acid and urea may be as low as 1:9, whereas the normal ratio, as we have seen, is 1:50 or higher. In the study of the influence of X-ray on metabolism Edsall has very recently reached some in- teresting conclusions. He found that the excretion of uric acid is usually increased and that in some conditions, particularly in leukaemia, it may be greatly increased. The excretion of total nitrogen, phosphates and other substances may also be considerably increased. !9 274 PHYSIOLOGICAL CHEMISTRY, Experiments on Uric Acid. i. Isolation from the Urine. — Place about 200 c.c. of filtered urine in a beaker, render it acid with 2-10 c.c. of concentrated hydrochloric acid, stir thoroughly and stand the vessel in a cold place for 24 hours. Examine the pigmented crystals of uric acid under the microscope and compare them with those shown in Fig. 101, p. 347 and PI. V., opposite p. 273. 2. Solubility. — Try the solubility of pure uric acid, furnished by the instructor, in the ordinary solvents (see p. 23) and in alcohol, ether, concentrated sulphuric acid and in boiling glycerol. 3. Crystalline Form of Pure Uric Acid. — Place about 100 c.c. of water in a small beaker, render it distinctly alkaline with potas- sium hydroxide solution and add a small amount of pure uric acid, stirring continuously. Cool the solution, render it distinctly acid with hydrochloric acid and allow it to stand in a cool place for crys- tallization. Examine the crystals under the microscope and com- pare them with those reproduced in Fig. 89, below. 4. Murexide Test. — To a small amount of pure uric acid in a small evaporating dish add 2-3 drops of concentrated nitric acid. Evaporate to dryness carefully on a water-bath or over a very low Fig. 8g. Pure Uric Acid. flame. A red or yellow residue remains which turns purplish-red after cooling the dish and adding a drop of very dilute ammonium hydroxide. The color is due to the formation of murexide. If po- tassium hydroxide is used instead of ammonium hydroxide a pur- URINE. 2/5 plish-violet color clue to the production of the potassium sail is ob- tained. The color disappears upon warming; with certain related bodies (purine bases) the color persists under these conditions. 5. Moreigne's Reaction. — To equal volumes of Moreigne's re- agent' and the solution to be tested add a tew drops of concen- trated potassium hydroxide. A blue color indicates the presence of uric acid. 6. Schiff's Reaction. — Dissolve a small amount of pure uric acid in sodium carbonate solution and transfer a drop of the resulting mixture to a strip of filter paper saturated with argentic nitrate solution. A yellowish-brown or black coloration due to the forma- tion of reduced silver is produced. 7. Influence upon Fehling's Solution. — Dilute 1 c.c. of Feh- ling's solution with 4 c.c. of water and heat to boiling. Now add slozvly, a few drops at a time, 1-2 c.c. of a concentrated solution of uric acid in potassium hydroxide, heating after each addition. From this experiment what do you conclude regarding the possi- bility of arriving' at an erroneous decision when testing for sugar in the urine by means of Fehling's test? 8. Reduction of Nylander's Reagent. — To 5 c.c. of a solution of uric acid in potassium hydroxide add about one-half a cubic centimeter of Nylander's reag"ent and heat to boiling for a few mo- ments. Do you obtain the typical black end-reaction signifying the reduction of the bismuth ? NH CO I CREATININE, C = NH N • CH3 • CH2. Creatinine is the anhydride of creatine and is a constituent of normal human urine. The theory that creatinine is derived from the creatine of ingested muscular tissue as well as from the creatine of the muscular tissue of the organism has recently been proven to be incorrect by Folin, Klercker, and \\o\i and Shaffer. Shaffer believes that creatinine is the result of some special process of normal metabolism which takes place to a large extent, if not entirely, in the muscles and further that the amount of such creatin- 1 Moreigne's reagent is made by combining 20 grams of sodium tungstate, 10 grams of phosphoric acid (sp. gr. 1.13) and 100 c.c. of water. Boil this mixture for twenty minutes, add water to make the volume of the solution equivalent to the original volume and acidify with hydrochloric acid. 276 PHYSIOLOGICAL CHEMISTRY. ine elimination, expressed in milligrams per kilogram body weight, is an index of this special process.1 He further states that the mus- cular efficiency of the individual depends upon the intensity of this process. Under normal conditions about 1 gram of creatinine is ex- creted by an adult man in 24 hours,2 the exact amount depending in great part upon the nature of the food and decreasing markedly in starvation. Very little that is important is known regarding the excretion of creatinine under pathological conditions. The creatinine content of the urine is said to be increased in typhoid fever, typhus, tetanus and pneumonia, and to be decreased in ansemia, chlorosis, paralysis, muscular atrophy, advanced degeneration of the kidneys, and in leucaemia (myelogenous, lymphatic and pseudo). An increase of creatinine was also noted in diabetes, an increase probably due to the creatinine content of the meat eaten. The greater part of the data, however, relating to the variation of the creatinine excretion under pathological conditions are not of much value since in nearly every instance, the diet was not sufficiently controlled to permit the collection of reliable data. And further, until the advent of the Folin method (see p. 392), there was no accurate method for the quantitative determination of cre- atinine. Shaffer has very recently called attention to the fact that a low excretion of creatinine is found in the urine of a remarkably large number of pathological subjects, representing a variety of con- ditions, and that it is therefore evident that the excretion of an ab- normally small-amount of this substance is by no means peculiar to any one disease. Creatinine crystallizes in colorless, glistening monoclinic prisms (Fig. 90, p. 277) which are soluble in about 12 parts of cold water; they are more soluble in warm water and in warm alcohol. One of the most important and interesting of the compounds of creatin- ine is creatinine -zinc chloride, (C4H7N30)2ZnCl2, which is formed from an alcoholic solution of creatinine upon treatment with zinc chloride in acid solution. Creatinine has the power of reducing cupric hydroxide in alkaline solution and in this way may interfere with the determination of sugar in the urine. In the reduction by creatinine the blue liquid is first changed to a yellow and the for- mation of a brownish-red precipitate of cuprous oxide is brought 1 He proposes to designate as the " creatinine coefficient " the excretion of creatinine-nitrogen (mgs.) per kilogram of body weight. ' According to Shaffer the amount excreted by strictly normal individuals is between 7 and 11 milligrams of creatinine-nitrogen per kilogram of body weight. URINE. 277 about only after continuous boiling w ith an excess of the copper salt. Creatinine does not reduce alkaline bismuth solutions and there tore does not interfere with Xvlander's and Boettger's tests. Fig. <)o. Creatinine. It has recently been shown by Folin that the absolute quantity of creatinine eliminated in the urine on a meat-free diet is a constant quantity different for different individuals, but wholly independ- ent of quantitative changes in the total amount of nitrogen elimin- ated. Shaffer has very recently confirmed these findings and has shown that the output of creatinine under these conditions is con- stant from hour to hour as well as from day to day. Experiments on Creatinine. 1. Separation from the Urine. — Place 250 c.c. of urine in a casserole or beaker, render it alkaline with milk of lime and then add CaCl2 solution until the phosphates are completely precipitated. Filter off the precipitate, render the filtrate slightly acid with acetic acid and evaporate it to a syrup. While still warm this syrup is treated with about 50 c.c. of 95- 97 per cent alcohol and the mix- ture allowed to stand 8-12 hours in a cool place. The precipitate is now filtered off and the filtrate treated with a little sodium acetate and about one-half c.c. of acid-free zinc chloride solution having a specific gravity of 1.2. This mixture is stirred thoroughly and allowed to stand in a cold place for 48-72 hours. Creatinine- zinc chloride (Fig. 91, p. 278) will crystallize out under these con- 278 PHYSIOLOGICAL CHEMISTRY. ditions. Collect. the crystals on a filter paper and wash them with alcohol to remove chlorides. Now treat the zinc chloride compound with a little warm water, boil with lead oxide and filter. The fil- trate may now be decolorized by animal charcoal, evaporated to Fig. 91. Creatinine-Zinc Chloride. (Salkowski.) dryness and the residue extracted with strong- alcohol. (Creatine remains undissolved under these conditions. ) The alcoholic extract of creatinine is now evaporated to incipient crystallization and left in a cool place until crystallization is complete. If desired the crys- tals may be purified by recrystallization from water. 2. Weyl's Test. — Take 5 c.c. of urine in a test-tube, add a few drops of sodium nitro-prusside and render the solution alkaline with potassium hydroxide solution. A ruby-red color results which soon turns yellow. See Legal's test for acetone, page 329. 3. Salkowski's Test. — To the yellow solution obtained in Weyl's test above add an excess of acetic acid and apply heat. A green color results and is in turn displaced by a blue color. A precipi- tate of Prussian blue may form. 4. Jaffe's Reaction. — Place 5 c.c. of urine in a test-tube, add an aqueous solution of picric acid and render the mixture alkaline with potassium hydroxide solution. A red color is produced which turns yellow if the solution be acidified. Dextrose gives a similar red color but only upon the application of heat. This color reaction observed when creatinine in alkaline solution is treated with picric acid is the basic principle of Folin's colorimetric method for the quantitative determination of creatinine (see page 392). URINE. 279 ETHEREAL SULPHURIC ACIDS. The most important of the ethereal sulphuric acids found in the urine are phenol-sulphuric acid, p-cresol-^sulphuric acid, indoxyl- sulphuric acid and skatoxyl-sulphuric acid, l'yrocatechin-sulphuric acid also occurs in traces in human urine. The total output of ethereal sulphuric acid varies from 0.09 to 0.62 gram for 24 hours. In health the ratio of ethereal sulphuric acid to inorganic sulphuric acid is about 1 : 10. These ethereal sulphuric acids originate in part from the phenol, cresol, indole and skatole formed in the putrefac- tion of protein material in the intestine. The phenol passes to the liver where it is conjugated to form phenyl potassium sulphate and appears in this form in the urine whereas the indole and skatole undergo a preliminary oxidation to form indoxyl and skatoxyl respectively before their elimination. It has generally been considered that each of the ethereal sul- phuric acids was formed principally in the putrefaction of protein material in the intestine and that therefore a determination of the total ethereal sulphuric acid content of the urine was an index of the extent to which these putrefactive processes were proceeding within the organism. Recently, however, Folin has conducted a series of experiments which seem to show that the ethereal sulphuric acid con- tent of the urine does not afford an index of the extent of intestinal putrefaction, since these bodies arise only in part from putrefactive processes. He claims that the ethereal sulphuric acid excretion represents a form of sulphur metabolism which is more in evidence upon a diet containing a very small amount of protein or upon a diet containing absolutely no protein. The ethereal sulphuric acid content of the urine diminishes as the total sulphur content diminishes but the percentage decrease is much less. There- fore when considered from the standpoint of the total sulphuric acid content the ethereal sulphuric acid content is not diminished but is increased, although the total sulphuric acid content is dimin- ished. Folin's experiments also seem to show that the indoxyl sulphuric acid (indoxyl potassium sulphate or indican ) content of the urine does not originate to any degree from the metabolism of protein material but that it arises in great part from intestinal putrefaction and that the excretion of indoxyl sulphuric acid may alone be taken as a rough index of the extent of putrefactive proc- esses within the intestine. Indoxyl sulphuric acid, 28o PHYSIOLOGICAL CHEMISTRY. CH //\ HC C-C(0-S08H), I II II HC C CH \/\/ CH NH therefore, which occurs in the urine as indoxyl potassium sulphate or indican, CH //\ HC C-C(0-S03K), I II II HC C CH \/\/ CH NH is clinically the most important of the ethereal sulphuric acids. Tests for Indican. i. Jaffe's Test. — Nearly fill a test-tube with a mixture composed of equal volumes of concentrated HC1 and the urine under exam- ination. Add 2-3 c.c. of chloroform and a few drops of a calcium hypochlorite solution, place the thumb over the end of the test- tube and shake the tube and contents thoroughly. The chloroform is colored more or less, according to the amount of indican present. Ordinarily a blue color due to the formation of indigo-blue is produced ; less frequently a red color due to indigo-red may be noted. This is the reaction (see also pages 162 and 163) : CH //\ HC C-C-OH 2 I || II +20 = HC C CH CH NH Indoxyl, C8H7NO. CH CH //\ /\ HC O-C-0 O-C-C CH I I II I II I +2H20 HC C C C C CH V \/ \/ \// CH NH NH CH Indigo-blue, Ci6Hi0N2O2. URINE. 251 2. Obermayer's Test. — Nearly fill a test-tube with a mixture composed of equal volumes of Obermayer's reagent1 and the urine under examination. Add 2-3 c.c. of chloroform, place the thumb over the end of the test-tube and shake thoroughly. How does this compare with Jaffe's test? 3. Giirber's Reaction. — To one volume of the urine under ex- amination and two volumes of concentrated hydrochloric acid in a test-tube add 2-3 drops of a 1 per cent solution of osmic acid and 2-3 c.c. of chloroform and shake the tube and contents thoroughly. Compare the color with those obtained in Jaffe's and Obermayer's tests. An excess of osmic acid does not affect the reaction. Occa- sionally better results are obtained if the solution of osmic acid is added directly to the urine before the addition of the hydro- chloric acid. If the urine under examination be strongly colored or of high specific gravity it should first be treated with basic lead acetate (one-eighth volume). The precipitate is then removed by filtration and the resulting filtrate used in making the test for indican. 4. Rossi's Reaction. — To equal volumes of concentrated hydro- chloric acid and the urine under examination, in a test-tube, add 1 drop of a 10 per cent solution of ammonium persulphate and 2-7, c.c. of chloroform. Agitate the mixture vigorously and note the color of the chloroform. Compare this result with those obtained in the other indican tests. 5. Lavelle's Reaction. — To 10 c.c. of urine in a test-tube add 2-3 c.c. of Obermayer's reagent1 and a similar volume of concen- trated sulphuric acid. (During the addition of the acid the tube should be held under running water in order that the temperature of the mixture may not rise too high.) Add 2-7, c.c. of chloro- form, shake the tube vigorously, and observe the depth of color assumed by the chloroform. The sponsor for this reaction claims it to be the most satisfactory of the indican tests. CO XHCH2COOH. HIPPURIC ACID, \/ 'Obermayer's reagent is prepared by adding J-4 grams ,it" tonic chloride to a liter of concentrated HC1 (sp. gr. 1.10). 282 PHYSIOLOGICAL CHEMISTRY. This acid occurs normally in the urine of both the carnivora and herbivora but is more abundant in the urine of the latter. It is formed by a synthesis of benzoic acid and glycocoll which takes place in the kidneys. The average excretion of an adult man for 24 hours under normal conditions is about 0.7 gram. Hippuric Hippuric Acid. acid crystallizes in needles or rhombic prisms (see Fig. 92, above) the particular form depending upon the rapidity of crystallization. Pure hippuric acid melts at 1870 C. The most satisfactory method for the isolation of hippuric acid from the urine in crystalline form is that proposed by Roaf (see p. 283). It is easily soluble in alcohol or hot water, and only slightly soluble in ether. The output of hippuric acid is increased in diabetes owing probably to the ingestion of much protein and fruit. It is decreased in fevers and in certain kidney disorders where the synthetic activity of the renal cells is diminished. Hippuric acid may be determined quan- titatively by means of Dakin's methods (see p. 383). Experiments on Hippuric Acid. 1. Separation from the Urine, (a) First Method. — Render 500- 1000 c.c. of urine of the horse or cow1 alkaline with milk of lime, 1 If urine of the horse or cow is not available human urine may serve the purpose fully as well provided means are taken to increase it's content of hippuric acid. This may be conveniently accomplished by ingesting 2 grams of ammonium benzoate at night. The fraction of urine passed in the morning will be found to have a high content of hippuric acid. The ammonium benzoate is in no way harmful. URINE. 283 boil for a few moments and filter while hot. Concentrate the fil- trate, over a burner, to a small volume. Cool the solution, acidify it strongly with concentrated hydrochloric acid and stand it in a cool place for 24 hours. Filter off the crystals of hippuric acid which have formed and wash them with a little cold water. Re- move the crystals from the paper, dissolve them in a very small amount of hot water and percolate the hot solution through thor- oughly washed animal charcoal, being careful to wash out the last portion of the hippuric acid solution with hot water. Filter, con- centrate the filtrate to a small volume and stand it aside for crys- tallization. Examine the crystals under the microscope and com- pare them with those in Fig. 92, page 282. This method is not as satisfactory as Roaf's method (see below). (b) Roaf's Method. — Place 500 c.c. of urine of the horse or cow1 in a casserole or precipitating jar and add an equal volume of a saturated solution of ammonium sulphate2 and 7.5 c.c. of con- centrated sulphuric acid. Permit the mixture to stand for twenty- four hours and remove the crystals of hippuric acid by filtration. Purify the crystals by recrystallization according to the directions given above under First Method. Examine the crystals under the microscope and compare them with those given in Fig. 92, p. 282. If sufficient urine is not available to permit the use of 500 c.c. a smaller volume may be used inasmuch as it is possible, by the above technique, to isolate hippuric acid in crystalline form from as small a volume as 25-50 c.c. of herbivorous urine. The greater the amount of ammonium sulphate added the more rapid the crystallization until at the saturation point the crystals of hippuric acid sometimes form in about ten minutes. 2. Melting-Point. — Determine the melting-point of the hip- puric acid prepared in the above experiment (see p. 269). 3. Solubility. — Test the solubility of hippuric acid in the ordi- nary solvents (page 23) and in alcohol, and ether. 4. Dehn's Reaction. — Introduce about 5 c.c. of the urine or the solution under examination into a test-tube and add sufficient hvpo- bromite solution3 to impart to the mixture a permanent yellow color. In the case of urine enough hypobromite should be added to decom- pose the urea. Fleat the mixture to boiling and note the forma- tion of an orange or brown-red precipitate if hippuric acid is pres- 1 See note on p. 282. 2 125 grams of solid ammonium sulphate may be substituted. 3 See note on p. 375. 284 PHYSIOLOGICAL CHEMISTRY. ent. If the solution under examination contains only a trace of hippuric acid the solution will appear smoky and faintly red in color whereas if a larger amount of the acid be present the solution will become opaque and of an orange or brown-red color. In either case after standing for some time the solution should clear up and a light, finely divided precipitate should be deposited. This precip- itate consists of earthy phosphates mixed with an amorphous orange or brown-red substance of unknown composition. 5. Formation of Nitro-Benzene. — To a little hippuric acid in a small porcelain dish add 1-2 c.c. of concentrated HNOs and evaporate to dryness on a water-bath. Transfer the residue to a dry test-tube, apply heat and note the odor of the artificial oil of bitter almonds (nitro-benzene). 6. Sublimation. — Place a few crystals of hippuric acid in a dry test-tube and apply heat. The crystals are reduced to an oily fluid which solidifies in a crystalline mass upon cooling. When stronger heat is applied the liquid assumes a red color and finally yields a sublimate of benzoic acid and the odor of hydrocyanic acid. 7. Formation of Ferric Salt. — Render a small amount of a so- lution of hippuric acid neutral with dilute potassium hydroxide. Now add 1-3 drops of neutral ferric chloride solution and note the formation of the ferric salt of hippuric acid as a cream colored precipitate. COOH OXALIC ACID, J COOH. Oxalic acid is a constituent of normal urine, about 0.02 gram being eliminated in 24 hours. It is present in the urine as cal- cium oxalate, which is kept in solution through the medium of the acid phosphates. The origin of the oxalic acid content of the urine is not well understood. It is eliminated, at least in part, unchanged when ingested, therefore since many of the common articles of diet, e. g., asparagus, apples, cabbage, grapes, lettuce, spinach, tomatoes, etc., contain oxalic acid it seems probable that the in- gested food supplies a portion of the oxalic acid found in the urine. There is also experimental evidence that part of the oxalic acid of the urine is formed within the organism in the course of protein and fat metabolism. It has also been suggested that oxalic acid may arise from an incomplete combustion of carbohydrates, espe- cially under certain abnormal conditions. Pathologically, oxalic URINE. 2.S5 acid is found to be increased in amount in diabetes mellitUS, in or- ganic diseases of the liver and in various other conditions which are accompanied by a derangement of the oxidation mechanism. An abnormal increase of oxalic acid is termed oxaluria. A consid- erable increase in the content ot oxalic acid may be noted unaccom- panied by any other apparent symptom. Calcium oxalate crystal- lizes in at least two distinct forms, dumb-bells and octahedra I Fig. 99.. Pa§"e 345)- Experiments. Preparation of Calcium Oxalate. First Method. — Place 200- 250 c.c. of urine in a beaker, add 5 c.c. of a saturated solution of calcium chloride, make the urine slightly acid with acetic acid and stand the beaker aside in a cool place for 24 hours. Examine the sediment under the microscope and compare the crystalline forms with those shown in Fig. 99, p. 345. Second Method. — Proceed as above, replacing the acetic acid by an excess of ammonium hydroxide and filtering off the precipitate of phosphates. NEUTRAL SULPHUR COMPOUNDS. Under this head may be classed such bodies as cystine (see p. 72), chrondroitin-sulphuric acid, oxyproteic acid, alloxyproteic acid, uroferric acid, thiocyanates and taurine derivatives. The sul- phur content of the bodies just enumerated is generally termed loosely combined or neutral sulphur in order that it may not be con- fused with the acid sulphur which occurs in the inorganic sulphuric acid and ethereal sulphuric acid forms. Ordinarily the neutral sul- phur content of normal human urine is 14-20 per cent of the total sulphur content. NHCHHN ALLANTOIN, 00 00. NH-CO NH2 Allantoi'n has been found in the urine of suckling calves as well as in that of the dog and cat. It has also been detected in the urine of infants within the first eight days after birth, as well as in the urine of adults. It is more abundant in the urine of women during" pregnancy. Underhil] also reports the presence of allantoin in the urine of fasting dog's, an observation which makes it probable 280 PHYSIOLOGICAL CHEMISTRY. that allantoin is a constant constituent of the urine of such animals. Allantoin is formed by the oxidation of uric acid and the output is increased by thymus or pancreas feeding. When pure it crystal- lizes in prisms (Fig. 93, below) and when impure in granules and Fig. 93. Allantoin, from Cat's Urine. a and b, Forms in which it crystallized from the urine ; c, re-crystallized allantoin. (Drawn from micro-photographs furnished by Prof. Lafayette B. Mendel of Yale University.) knobs. Pathologically, it has been found increased in diabetes insipidus and in hysteria with convulsions (Pouchet). Experiments. 1. Separation from the Urine.1 — Meissner's Method. — Precipi- tate the urine with baryta water. Neutralize the nitrate carefully with dilute sulphuric acid, filter immediately and evaporate the fil- trate to incipient crystallization. Completely precipitate this warm fluid with 95 per cent alcohol (reserve the precipitate). Decant or filter and precipitate the solution by ether. Combine the ether and alcohol precipitates and extract with cold water or hot alcohol; allantoin remains undissolved. Bring the allantoin into solution in hot water and recrystallize. Allantoin may be determined quantitatively by the Paduschka- Underhill-Kleiner method (see p. 407) or by Loewi's method.2 2. Preparation from Uric Acid. — Dissolve 4 grams of uric 1 The urine of the dog after thymus, pancreas or uric acid feeding may be employed. 2Archiv fur Experimentelle Pathologie und Pharmakologie, 1900, xliv, p. 20. URINE. 287 acid in too c.c. of water rendered alkaline with potassium hydrox- ide. COol nnd carefully add 3 grams of potassium permanganate. Filter, immediately acidulate the filtrate with acetic acid and allow it to stand in a cool place over night. Filter off the crystal- and wash them with water. Save the wash water and filtrate, unite them and after concentrating to a small volume stand away for crystallization. Now combine all the crystals and recrystallize them from hot water. Use these crystals in the experiments which follow. 3. Microscopical Examination. — Examine the crystals made in the last experiment and compare them with those shown in Fig. 93, page 286. 4. Solubility. — Test the solubility of allantoin in the ordinary solvents (page 23). 5. Reaction. — Dissolve a crystal in water and test the reaction to litmus. 6. Furfurol Test. — Place a few crystals of allantoin on a test- tablet or in a porcelain dish and add 1-2 drops of a concentrated aqueous solution of furfurol and 1-2 drops of concentrated hydro- chloric acid. Observe the formation of a yellow color which turns to a light purple if allowed to stand. This test is given by urea but not by uric acid. 7. Murexide Test. — Try this test according to the directions given on page 274. Note that allantoin fails to respond. 8. Reduction of Fehling's Solution. — Make this test in the usual way (see p. 27) except that the boiling must be prolonged and excessive. Ultimately the allantoin will reduce the solution. Compare with the result on uric acid, page 275. AROMATIC OXYACIDS. Two of the most important of the oxyacids are paraoxy-phenyl- acetic acid, CHoCOOH, 0 OH and paraoxy phenyl-propionic acid, CH2CH2COOH. OH 288 PHYSIOLOGICAL CHEMISTRY. They are products of the putrefaction of protein material and tyrosine is an intermediate stage in their formation. Both these acids for the most part pass unchanged into the urine where they occur normally in very small amount. The content may be in- creased in the same manner as the phenol content, in particular by acute phosphorus poisoning. A fraction of the total aromatic oxy- acid content of the urine is in combination with sulphuric acid, but the greater part is present in the form of salts of sodium and potassium. Homogentisic Acid or di-oxyphenyl-acetic acid, OH j^iCH2-COOH, \y OH is another important oxyacid sometimes present in the urine. Under the name glycosuric acid it was first isolated from the urine by Prof. John Marshall of the University of Pennsylvania; sub- sequently Baumann isolated it and determined its chemical constitu- tion. It occurs in cases of alcaptonuria. A urine containing this oxyacid turns greenish-brown from the surface downward when treated with a little sodium hydroxide or ammonia. If the solution be stirred the color very soon becomes dark brown or even black. Homogentisic acid reduces alkaline copper solutions but not alka- line bismuth -solutions. Uroleucic acid is similar in its reactions to homogentisic acid. Oxyiiiandelic Acid or paraoxyphenyl-glycolic acid, OH CH(OH)COOH, has been detected in the urine in cases of yellow atrophy of the liver. Kynurenic Acid or y-oxy-/?-quinoline carbonic acid, CH COH HC C C-COOH, I II I HC C CH CH N I -RINK. 289 is present in the urine of the dog and has recently been detected by Swain in the urine of the coyote. To isolate it from the urine proceed as follows: Acidify the urine with hydrochloric aeid in the proportion 1 : .25. From this aeid fluid both the uric aeid and the kynurenic aeid separate in the course of 24 48 hours. Filter off the combined crystalline deposit of the two acids, dissolve the kynurenic acid in dilute ammonia (uric acid is insoluble) and re- precipitate it with hydrochloric acid. Kynurenic acid may he quantitatively determined by Capaldi's method.1 COOH. BENZOIC ACID, \, Benzoic acid has been detected in the urine of the rabbit and dog. It is also said to occur in human urine accompanying renal disor- ders. The benzoic acid probably originates' from a fermentative decomposition of the hippuric acid of the urine. Experiments. 1. Solubility. — Test the solubility of benzoic acid in water, alco- hol and ether. Fig. 94. Benzoic Acid. 2. Crystalline Form. — Recrystallize some benzoic acid from hot water, examine the crystals under the microscope and compare them with those reproduced in Fig. 94. above. 1 Zeitschrift fiir physiologische Chemie, 1897, xxiii, p. 92. 20 29O PHYSIOLOGICAL CHEMISTRY. 3. Sublimation. — Place a little benzoic acid in a test-tube and heat over a flame. Note the odor which is evolved and observe that the acid sublimes in the form of needles. 4. Dissolve a little sodium benzoate in water and add a solution of neutral ferric chloride. Note the production of a brownish-yel- low precipitate (salicylic acid gives a reddish-violet color under the same conditions). Add ammonium hydroxide to some of the pre- cipitate. It dissolves and ferric hydroxide is formed. Add a little hydrochloric acid to another portion of the original precipitate and stand the vessel away over night. What do you observe? NUCLEOPROTEIN. The nubecula of normal urine has been shown by one investigator to consist of a mucoid containing 12.7 per cent of nitrogen and 2.3 per cent of sulphur. This body evidently originates in the uri- nary passages. It is probably slightly soluble in the urine. Some investigators believe that the body forming the nubecula of normal urine is nucleoprotein and not a mucin or mucoid as stated above. A discussion of nucleoprotein and related bodies occurring in the urine under pathological conditions will be found on page 320. NH-CO OXALURIC ACID, CO NH2 COOH. Oxaluric acid is not a constant constituent of normal human urine, and when found occurs only in traces as the ammonium salt. Upon boiling oxaluric acid it splits into oxalic acid and urea. ENZYMES. Various types of enzymes produced within the organism are ex- creted in both the feces and the urine. In this connection it is interesting to note that pepsin, gastric rennin and an amylase have been positively identified in the urine. The occurrence of trypsin in the urine, at least under normal conditions, is questioned. VOLATILE FATTY ACIDS. ■ Acetic, butyric and formic acids have been found under normal conditions in the urine of man and of certain carnivora as well as in the urine of herbivora. Normally they arise principally from URINE. 29I the fermentation of carbohydrates and the putrefaction of proteins. The acids containing" the fewest carbon atoms I formic and acetic) are found to be present in larger percentage than those which con tain a larger number of such atoms. The volatile fatty acid- occur in normal urine in traces, the total output tor twenty-four hour-, according to different investigators, varying from 0.008 gram to 0.05 gram. Pathologically, the excretion of volatile fatty acids is increased in diabetes, fevers, and in certain hepatic diseases in which the parenchyma of the liver is seriously affected. Under other patho- logical conditions the output may be diminished. These variations, however, in the excretion of the volatile fatty acids possess very little diagnostic value. CH3 PARALACTIC ACID, OH (OH) I COOH. Paralactic acid is supposed to pass into the urine when the supply of oxygen in the organism is diminished through any cause, c. g., after acute yellow atrophy of the liver, acute phosphorus poisoning or epileptic attacks. This acid has also been found in the urine of healthy persons following the physical exercise incident to pro- longed marching. Paralactic acid has been detected in the urine of birds after the removal of the liver. Underhill reports the oc- currence of this acid in the urine of a case of pernicious vomiting of pregnancy. CH.COXHCHoCOOH. /\ PHENACETURIC ACID, I Phenaceturic acid occurs principally in the urine of herbivorous animals but has frequently been detected in human urine. It is pro- duced in the organism through the synthesis of glycocoll and phenylacetic acid. It may be decomposed into its component parts by boiling with dilute mineral acids. The crystalline form of phenaceturic acid (small rhombic plates with rounded angles) re- sembles one form of uric acid crystal. PHOSPHORIZED COMPOUNDS. Phosphorus in organic combination has been found in the urrne in such bodies as glycerophosphoric acid, which may arise from 292 PHYSIOLOGICAL CHEMISTRY. the decomposition of lecithin, and phosphocarnic acid. It is claimed that on the average about 2.5 per cent of the total phosphorus elimi- nation is in organic combination. PIGMENTS. There are at least three pigments normally present in human urine. These pigments are urochrome, urobilin and uroerythrin. A. UROCHROME. This is the principal pigment of normal urine and imparts the characteristic yellow color to that fluid. It is apparently closely related to its associated pigment urobilin since the latter may be readily converted into urochrome through evaporation of its aque- ous-ether solution. Urochrome may be obtained in the form of a brown, amorphous powder which is readily soluble in water and 95 per cent alcohol. It is less soluble in absolute alcohol, acetone, amyl alcohol and acetic ether and insoluble in benzene, chloroform and ether. Urochrome is said to be a nitrogenous body (4.2 per cent nitrogen), free from iron. B. UROBILIN. Urobilin, which was at one time considered to be the principal pigment of urine, in reality contributes little toward the pigmenta- tion of this fluid. It is claimed that no urobilin is present in freshly voided normal urine but that its precursor, a chromogen called urobilinogen, is present and gives rise to urobilin upon de- composition through the influence of light. It is claimed by some investigators that there are various forms of urobilin, e. g., normal, febrile, physiological and pathological. Urobilin is said to be very similar to, if not absolutely identical with, hydrobilirubin (see page 173). Urobilin may be obtained as an amorphous powder which varies in color from brown to reddish-brown, red and reddish-yellow de- pending upon the way in which it is prepared. It is easily soluble in ethyl alcohol, amyl alcohol and chloroform,, and slightly soluble in ether, acetic ether and in water. Its solutions show characteristic absorption-bands (see Absorption Spectra, Plate II). Under normal conditions urobilin is derived from the bile pigments in the intestine. Urobilin is increased in most acute infectious diseases such as ery- sipelas, malaria, pneumonia and scarlet fever. It is also increased URINE. 293 in appendicitis, carcinoma of the liver, catarrhal icterus, pernicious ainciuia and in cases of poisoning by antifebrin, antipyrin, pyridin, and potassium chlorate. In general if is usually increased when blood destruction is excessive and in many disturbances of the liver. It is markedly decreased in phosphorus poisoning. Experiments. 1. Spectroscopic Examination. — Acidify the urine with hydro- chloric acid and allow it to remain exposed to the air for a few- moments. By this means if any urobilinogen is present it will be transformed into urobilin. The urine may now be examined by means of the spectroscope. If urobilin is present in the fluid the characteristic absorption-band lying" between b and F will be ob- served (see Absorption Spectra, Plate II). It may be found neces- sary to dilute the urine with water before a distinct absorption- band is observed. This test may be modified by acidifying 10 c.c. of urine with hydrochloric acid and shaking- it gently with 5 c.c. of amyl alcohol. The alcoholic extract when examined spectro- scopicallv will show the characteristic urobilin absorption-band. (Note the spectroscopic examination in the next experiment. ) 2. Ammoniacal-Zinc Chloride Test. — Render some of the urine ammoniacal by the addition of ammonium hydroxide, and after allowing" it to stand a short time filter off the precipitate of phos- phates and add a few drops of zinc chloride solution to the filtrate. Observe the production of a greenish fluorescence. Examine the fluid by means of the spectroscope and note the absorption-band which occupies much the same position as the absorption-band of urobilin in acid solution (see Absorption Spectra. Plate II). 3. Gerhardt's Test. — To 20 c.c. of urine add 3-5 c.c. of chloro- form and shake well. Separate the chloroform extract and add to it a few drops of iodine solution (I in KI). Render the mixture alkaline with dilute solution of potassium hydroxide and note the production of a yellow or yellowish-brown color. The solution ordinarily exhibits a greenish fluorescence. 4. Wirsing's Test. — To 20 c.c. of urine add 3 5 c.c. of chloro- form and shake gently. Separate the chloroform extract and add to it a drop of an alcoholic solution of zinc chloride. Note the rose-red color and the greenish fluorescence. If the solution is turbid it may be rendered clear by the addition of a tew c.c. of absolute alcohol. c. Ether-Absolute Alcohol Test. — Mix urine and pure ether 294 PHYSIOLOGICAL CHEMISTRY. in equal volumes and shake gently in a separatory funnel. Sepa- rate the ether extract, evaporate it to dryness and dissolve the resi- due in 2-3 c.c. of absolute alcohol. Note the greenish fluorescence. Examine the solution spectroscopically and observe the characteristic absorption-band (see Absorption Spectra, Plate II). 6. Ring Test. — Acidify 25 c.c. of urine with 2-3 drops of con- centrated hydrochloric acid, add 5 c.c. of chloroform and shake the mixture. Separate the chloroform, place it in a test-tube and add carefully 3-5 c.c. of an alcoholic solution of zinc acetate. Observe the formation of a green ring at the zone of contact of the two fluids. If the tube is shaken a fluorescence may be observed. C. UROERYTHRIN. This pigment is frequently present in small amount in normal urine. The red color of urinary sediments is due in great part to the presence of uroerythrin. It is easily soluble in amyl alcohol, slightly soluble in acetic ether, absolute alcohol or chloroform, and nearly insoluble in water. Dilute solutions of uroerythrin are pink in color while concentrated solutions are orange-red or bright red : none of its solutions fluoresce. Uroerythrin is increased in amount after strenuous physical exercise, digestive disturbances, fevers, cer- tain liver disorders and in various other pathological conditions. PTOMAINES AND LEUCOMAINES. These toxic substances are said to be present in small amount in normal urine. Very little is known, definitely, however, about them. It is claimed that five different poisons may be detected in the urine, and it is further stated that each of these substances pro- duces a specific and definite symptom when injected intravenously into a rabbit. The resulting symptoms are narcosis, salivation, mydriasis, paralysis and convulsions. The day urine is principally narcotic and is 2-4 times as toxic as the night urine which is chiefly productive of convulsions. PURINE BASES. The purine bases found in human urine are adenine, carnine, epiguanine, episarkine, guanine, xanthine, heteroxanthine, hypo- xanthine, paraxanthine and i-methylxanthine. The main bulk of the purine base content of the urine is made up of paraxanthine. heteroxanthine and i-methylxanthine which are derived for the most part from the caffeine, theobromine and theophylline of the URINE. 295 food. The total purine base content is made up of the- products of two distinct forms of metabolism, i. <•., metabolism of ingested nucleins and purines and metabolism of tissue nuclein material. Purine bases resulting from the fust Form of metabolism are said to be of exogenous origin whereas those resulting from the second form of metabolism are said to be of endogenous origin. The daily output of purine bases by the urine is extremely small and varies greatly with the individual (16 60 milligrams). The output is in- creased after the ingestion of nuclein material as well as after the increased destruction of leucocytes. A well marked increase ac- companies leukaemia. Edsall has very recently shown that the out- put of purine bases by the urine is increased as a result of X-ray treatment. Experiment. 1. Formation of the Silver Salts. — Add an excess of magnesia mixture1 to 25 c.c. of urine. Filter off the precipitate and add am- moniacal silver solution2 to the filtrate. A precipitate composed of the silver salts of the various purine bases is produced. The purine bases may be determined quantitatively by means of Kriiger and Schmidt's method (see p. 405). 2. Inorganic Physiological Constituents. Ammonia. Next to urea, ammonia is the most important of the nitrogenous end-products of protein metabolism. Ordinarily about 4.6-5.6 per cent of the total nitrogen of the urine is eliminated as ammonia and on the average this would be about 0.7 gram per day. Under normal conditions the ammonia is present in the urine in the form of the chloride, phosphate or sulphate. This is due to the fact that combinations of this sort are not oxidized in the organism to form urea, but are excreted as such. This explains the increase in the output of ammonia which follows the administration of the am- monium salts of the mineral acids or of the acids themselves. On the other hand when ammonium acetate and many other ammonium salts of certain organic acids are administered no increase in the 1 Magnesia mixture may be prepared as follows: Dissolve 175 grams of MgS< ' and 350 grams of NHiCl in 1400 c.c. of distilled water. Add 700 grams of concentrated NH,OH, mix very thoroughly and preserve the mixture in a glass- stoppered bottle. 2 Ammoniacal silver solution may be prepared according to directions given on page 407. 296 ' PHYSIOLOGICAL CHEMISTRY. output of ammonia occurs since the salt is oxidized and its nitrogen ultimately appears in the urine as urea. ' The acids formed during the process of protein destruction within the body have an influence upon the excretion of ammonia similar to that exerted by acids which have been administered. Therefore a pathological increase in the output of ammonia is ob- served in such diseases as are accompanied by an increased and im- perfect protein metabolism, and especially in diabetes, in which disease diacetic acid and /?-oxybutyric acid are found in the urine in combination with the ammonia. As the result of recent experiments Folin claims that a pro- nounced decrease in the extent of protein metabolism, as measured by the total nitrogen in the urine, is frequently accompanied by a decreased elimination of ammonia. The ammonia elimination is therefore probably determined by other factors than the total protein catabolism as such. Furthermore, he believes that a de- cided decrease in the total nitrogen excretion is always accompanied by a relative increase in the ammonia-nitrogen, provided the food is of a character yielding an alkaline ash. The quantitative determination of ammonia must be made upon the fresh urine since upon standing the normal urine will undergo ammoniacal fermentation (see page 257). Sulphates. Sulphur in combination is excreted in two forms in the urine ; first, as loosely combined, unoxidized or neutral sulphur and second, as oxidized or acid sulphur. The loosely combined sulphur is ex- creted mainly as a constituent of such bodies as cystine, cysteine, taurine, hydrogen sulphide, ethyl sulphide, thiocyanates, sul- phonic acids, oxyproteic acid, alloxpyroteic acid and uroferric acid. The amount of loosely combined sulphur eliminated is in great measure independent of the extent of protein decomposition or of the total sulphur excretion. In this characteristic it is somewhat similar to the excretion of creatinine. The oxidized sulphur is eliminated in the form of sulphuric acid, principally as salts of sodium, potassium, calcium and magnesium; a relatively small amount occurs in the form of ethereal sulphuric acid, i. e., sulphuric acid in combination with such aromatic bodies as phenol, indole, skatole, cresol, pyrocatechin and hydroquinone. Sulphuric acid in combination with Na, K, Ca or Mg is sometimes termed inorganic or preformed sulphuric acid whereas the ethereal sulphuric acid is URINE. 297 sometimes called conjugate sulphuric acid. The greater pan of the sulphur is eliminated in the oxidized form but the absolute per- centage of sulphur excreted as the preformed, ethereal or loosely combined type depends upon the total quantity of sulphur present, i. c, there is no definite ratio between the three forms of sulphur which will apply tinder all conditions. The preformed sulphuric acid may he precipitated directly from acidified urine with BaCL, whereas the ethereal sulphuric acid must undergo a preliminary boiling in the presence of a mineral acid before it can he so precipi- tated. The sulphuric acid excreted by the urine arises principally from the oxidation of protein material within the body; a relatively small amount is due to ingested sulphates. Under normal condition- about 2.5 grams of sulphuric acid is eliminated daily. Since the sulphuric acid content of the urine has, for the most part, a protein origin and since one of the most important constituents of the pro- tein molecule is nitrogen, it would be reasonable to suppose that a fairly definite ratio might exist betwen the excretion of these two elements. However, when we appreciate that the percentage con- tent of X and S present in different proteins is subject to rather wide variations, the fixing of a ratio which will express the exact relation existing between these two substances, as they appear in the urine as end-products of protein metabolism, is practically im- possible. It has been suggested that the ratio 5:1 expresses this relation in a general way. Pathologically, the excretion of sulphuric acid by the urine is in- creased in acute fevers and in all other diseases marked by a stimu- lated metabolism, whereas a decrease in the sulphuric acid excretion is observed in those diseases which are accompanied by a loss of appetite and a diminished metabolic activity. Experiments. 1. Detection of Inorganic Sulphuric Acid. — Place about 10 c.c. of urine in a test-tnbe. acidify with acetic acid and add some barium chloride solution. A white precipitate of barium sulphate forms. 2. Detection of Ethereal Sulphuric Acid. — Filter ^\'( the barium sulphate precipitate formed in the above experiment, add 1 c.c. of hydrochloric acid and a little barium chloride solution to the filtrate and heat the mixture to boiling for [-2 minutes. Note the appearance of a turbidity due to the presence of sulphuric acid 298 PHYSIOLOGICAL CHEMISTRY. Fig. 95. which has been separated from the ethereal sulphates and has com- bined with the barium of the BaCl2 to form BaS04. 3. Detection of Loosely Combined or Neutral Sulphur. — Place about 10 c.c. of urine in a test-tube, introduce a small piece of zinc, add sufficient hydrochloric acid to cause a gentle evolution of hydrogen and over the mouth of the tube place a filter paper satu- rated with plumbic acetate solution. In a short time the portion of the paper in contact with the vapors within the test-tube becomes blackened due to the formation of lead sulphide. The nascent hydrogen has reacted with the loosely combined or neutral sulphur to form hydrogen sulphide and this gas coming in contact with the plum- bic acetate paper has caused the production of the black lead sulphide. Sulphur in the form of inorganic or ethereal sulphuric acid does not respond to this test. 4. Calcium Sulphate Crystals. — Place 10 c.c. of urine in a test- tube, add 10 drops of calcium chlo- ride solution and allow the tube to stand until crystals form. Examine the calcium sulphate crystals, under the microscope and compare them with those shown in Fig. 95, above. Calcium Sulphate. and Weil.) (Hensel Chlorides. Next to urea, the chlorides constitute the chief solid constituent of the urine. The principal chlorides found in the urine are those of sodium, potassium, ammonium and magnesium, with sodium chloride predominating: The excretion of chlorides is dependent, in great part, upon the nature of the diet, but on the average the daily output is about 10-15 grams, expressed as sodium chloride. Copious water-drinking increases the output of chlorides consider- ably. Because of their solubility, chlorides are never found in the urinary sediment. Since the amount of chlorides excreted in the urine is due pri- marily to the chloride content of the food ingested, it follows that a decrease in the amount of ingested chloride will likewise cause a decrease in the chloride' content of the urine. In cases of actual fasting the chloride content of the urine may be decreased to a slight trace which is derived from the body fluids and tissues. URINK. 299 Under these conditions, however, an examination of the- blood of the fasting subject will show the percentage of chlorides in this fluid to be approximately normal. This forms a very striking ex- ample of the care nature takes to maintain the normal composition of the blood. There is a limit to the power of the body to main- tain this equilibrium, however, and if the fasting organism be sub- jected to the influence of diuretics for a time, a point is reached where the composition of the blood can no longer be maintained and a gradual decrease in its chloride content occurs which finally re- sults in death. Death is supposed to result not so much because of a lack of chlorine as from a deficiency of sodium. This is shown from the fact that potassium chloride, for instance, cannot replace the sodium chloride of the blood when the latter is decreased in the manner above stated. When this substitution is attempted the potassium salt is excreted at once in the urine, and death follows as above indicated. Pathologically, the excretion of chlorides may be decreased in some fevers, chronic nephritis, croupous pneumonia, diarrhoea, cer- tain stomach disorders and in acute articular rheumatism. Experiment. Detection of Chlorides in Urine.— Place about 5 c.c. of urine in a test-tube, render it acid with nitric acid and add a few drops of a solution of argentic nitrate. A white precipitate, due to the forma- tion of argentic chloride, is produced. This precipitate is soluble in ammonium hydroxide. Phosphates. Phosphoric acid exists in the urine in two general forms : First, that in combination with the alkali metals, sodium and potassium, and the radical ammonium; second, that in combination with the alkaline .earths, calcium and magnesium. Phosphates formed through a union of phosphoric acid with the alkali metals are termed alkaline phosphates, or phosphates of the alkali metals, whereas phosphates, formed through a union of phosphoric acid with the alkaline earths are termed earthy phosphates, or phosphates of the alkaline earths. Three series of salts are formed by phosphoric acid : Normal , M3P04,] mono-hydrogen, M2HP04, and di-hydrogen, MH2P04. The di-hydrogen salts are acid in reaction and it was generally be- lieved that about 60 per cent of the total phosphate content of the 1 M may be occupied by any of the alkali metals or alkaline earths. 300 PHYSIOLOGICAL CHEMISTRY. urine was in the form of this type of salt, and that the acidity of the urine was due in great part to the presence of sodium di-hydro-' gen phosphate. Recently, however, it has been quite clearly shown that the normal acidity of the urine is not due to the presence of this salt but is due, at least in part, to the presence of various acidic radicals. In this connection Folin believes that the phosphates in clear acid urine are all of the mono-hydrogen type, and that the acidity of the urines of this character is generally greater than the combined acidity of all the phosphates present ; the excess in the acidity above that due to phosphates he believes to be due to free organic acids. The observation has recently been made that urine may be separated into two portions, one part consisting al- most entirely of inorganic matter including practically all of the phosphates and having an alkaline reaction, the other containing practically all of the organic substances and no phosphates and hav- ing an acid reaction. In bones the phosphates occur principally in the form of the nor- mal salts of calcium and magnesium. The mono-hydrogen salts as a class are alkaline in reaction to litmus, and it is to the presence of di-sodium hydrogen phosphate, Na2HP04, that the greater part of the alkalinity of the saliva is due. The excretion of phosphoric acid is extremely variable but on the average the total output for 24 hours is about 2.5 grams, ex- pressed as P205. Ordinarily the total output is distributed be- tween alkaline phosphates and earthy phosphates approximately in the ratio 2:1. The greater part of this phosphoric acid arises from the ingested food, either from the preformed phosphates or more especially from the phosphorus in organic combination such as we find it in phosphoproteins, nude 0 proteins and lecithins; the phos- phorus-containing tissues of the body also contribute to the total output of this element. Alkaline phosphates ingested with the food have a tendency to increase the phosphoric acid content of the urine to a greater extent than the earthy phosphates so ingested. This is due, in a measure, to the fact that a portion of the earthy phosphates, under certain conditions, may be precipitated in the intestine and excreted in the feces ; this is especially to be noted in the case of herbivorous animals. Since the extent to which the phosphates are absorbed in the intestine depends upon the form in which they are present in the food, under ordinary conditions, there can be no absolute relationship between the urinary output of nitrogen and phosphorus. If the diet is constant however, I 'KIN K. 30I from day to day, thus allowing of the preparation of both a nitrogen and a phosphorus balance,3 a definite ratio may be established. In experiments upon dogs, which were fed an exclusive meat diet, the ratio of nitrogen to phosphorus, in the urine and feces, was found to be 8.1 : 1. Pathologically the excretion of phosphoric acid is increased in such diseases of the hones as diffuse periostosis, osteomalacia and rickets; according to some investigators, in the early stages of pul- monary tuberculosis; in acute yellow atrophy of the liver : in diseases which are accompanied by an extensive decomposition of nervous tissue and after sleep induced by potassium bromide or choral hy drate (Mendel). It is also increased after copious water-drinking. A decrease in the excretion of phosphates is at times noted in febrile affections, such as the acute infectious diseases; in pregnancy, in the period during which the fcetal hones are forming, and in diseases of the kidneys, because of non-elimination. Experiments. 1. Formation of "Triple Phosphate." — Place some urine in a beaker, render it alkaline with ammonium hydroxide, add a small Fig. 96. + \ " Tkiple Phosphate." | Ogden. I amount of magnesium sulphate solution and allow the beaker to stand in a cool place over night. Crystals of ammonium magnesium phosphate, "triple phosphate," form under these conditions. Ex- 1 In metabolism experiments, a statement showing the relation existing between the nitrogen content of the food on the one hand and that of the mine and feces on the other, for a definite period, is termed a nitrogen balance or a "balance of the income and outgo of nitrogen." 302 PHYSIOLOGICAL CHEMISTRY. amine the crystalline sediment under the microscope and compare the forms of the crystals with those shown in Fig. 96, page 301. 2. " Triple Phosphate " Crystals in Ammoniacal Fermenta- tion.— Stand some urine aside in a beaker for several days. Am- moniacal fermentation will develop and " triple phosphate " crystals will form. Examine the sediment under the microscope and com- pare the crystals with those shown in Fig. 96, p. 301. 3. Detection of Earthy Phosphates. — Place 10 c.c. of urine in a test-tube and render it alkaline with ammonium hydroxide. Warm the mixture and note the separation of a precipitate of earthy phosphates. 4. Detection of Alkaline Phosphates. — Filter off the earthy phosphates as formed in the last experiment, and add a small amount of magnesia mixture (see page 295) to the filtrate. Now warm the mixture and observe the formation of a white precipitate due to the presence of alkaline phosphates. Note the difference in the size of the precipitates of the two forms of phosphates from this same volume of urine. Which form of phosphates were present in the larger amount, earthy or alkaline ? 5. Influence upon Fehling's Solution. — Place 2 c.c. of Fell- ling's solution in a test-tube, dilute it with 4 volumes of water and heat to boiling. Add a solution of sodium dihydrogen phosphate, NaH2P04, a small amount at a time, and heat after each addition. What do you observe? What does this observation force you to' conclude regarding the interference of phosphates in the testing of diabetic urine by means of Fehling's test? Sodium and Potassium. The elements sodium and potassium are always present in the urine. Usually they are combined with such acidic radicals as CI, C03, S04 and P04. The amount of potassium, expressed as K20, excreted in 24 hours by an adult, subsisting upon a mixed diet, is on the average 2-3 grams, whereas the amount of sodium, expressed as Na20, under the same conditions, is ordinarily 4-6 grams. The ratio of K to Na is generally about 3:5. The ab- solute quantity of these elements excreted, depends, of course, in large measure, upon the nature of the diet. Because of the non- ingestion of NaCl and the accompanying destruction of potassium- containing body tissues, the urine during fasting contains more potassium salts than sodium salts. Pathologically the output of potassium, in its relation to sodium, URINE. 303 may be increased during fever; following the crisis, however, the output of this element may be decreased. It may also he increased in conditions associated with acid intoxication. Calcium and Magnesium. The greater part of the calcium and magnesium excreted in the urine is in the form of phosphates. The daily output, which depends principally upon the nature of the diet, aggregates ori the average about 1 gram and is made up of the phosphate- of cal- cium and magnesium in the proportion 1 : 2. The percentage of calcium salts present in the urine at any one time forms no depend able index as to the absorption of this class of salts, since they arc- again excreted into the intestine after absorption. It is therefore impossible to draw any satisfactory conclusions regarding the ex- cretion of the alkaline earths unless we obtain accurate analytical data from both the feces and the urine. Very little is known positively regarding the actual course of the excretion of the alkaline earths under pathological conditions except that an excess of calcium is found in acid intoxication and some diseases of the bones. Carbonates. Carbonates generally occur in small amount in the urine of man and carnivora under normal conditions, whereas much larger quan- tities are ordinarily present in the urine of herbivora. The alkaline reaction of the urine of herbivora is dependable in great measure upon the presence of carbonates. In general a urine containing carbonates in appreciable amount is turbid when passed or becomes so shortly after. These bodies ordinarily occur as alkali or alkaline earth compounds and the turbid character of urine containing them is usually due principally to the latter class of substances. The carbonates of the alkaline earths are often found in amorphous urinary sediments. Iron. Iron is present in small amount in normal urine. It probably occurs partly in inorganic and partly in organic combination. The iron contained in urinary pigments or chromogens is in organic com- bination. According to different investigators the iron content of normal urine will probably not average more than 0.001 gram per day. 304 physiological chemistry. Experiment. Detection of Iron in Urine. — Evaporate a convenient volume ( 10-15 c.c.) of urine to dryness. Incinerate and dissolve the residue in a few drops of iron-free hydrochloric acid and dilute the acid solution with 5 c.c. of water. Divide the acid solution into two parts and make the following tests: (a) To the first part add a solution 'of ammonium thiocyanate; a red color indicates the pres- ence of iron, (b) To the second part of the solution add a little potassium ferrOcyanide solution ; a precipitate of Prussian blue forms upon standing. Fluorides, Nitrates, Silicates and Hydrogen Peroxide. These substance are all found in traces in human urine under normal conditions. Nitrates are undoubtedly introduced into the organism in the water and ingested food. The average excre- tion of nitrates is about 0.5 gram per day, the output being the larg'est upon a vegetable diet and smallest upon a meat diet. Ni- trites are found only in urine which is undergoing decomposition and are formed from the nitrates in the course of ammoniacal fermentation. Hydrogen peroxide has been detected in the urine, but its presence is believed to possess no pathological importance. CHATTER XIX. URINE: PATHOLOGICAL CONSTITUENTS.' Dextrose. Serum albumin. Serum globulin. Proteins Proteoses Blood Bile Deutero-proteose. Hetero-proteose. " Bence- Jones' protein. Peptone. Nucleoprotein. Fibrin. Oxyhemoglobin. Form elements. Pigment, f Pigments. I Acids. Acetone. Diacetic acid. /3-Oxy butyric acid. Conjugate glycuronates. Pentoses. Fat. Ha?matoporphy rin . Lactose. Galactose. Lasvulose. Inosite. Laiose. Melanin. Urorosein. Unknown substances. DEXTROSE. Traces of this sugar occur in normal urine, but the amount is not sufficient to be readily detected by the ordinary simple qualitative 1 See note at the bottom of page 264. 21 305 306 PHYSIOLOGICAL CHEMISTRY. tests. There are two distinct types of pathological glycosuria, i. e., transitory glycosuria and persistent glycosuria. The transitory type may follow the ingestion of an excess of sugar, causing the assimilation limit to be exceeded, or it may accompany any one of several disorders which cause an impairment of the power of assimilating sugar. In the persistent type large amounts of sugar are excreted daily in the urine for long- periods of time. Under such circumstances a condition known as diabetes mellitus exists. Ordinarily, diabetic urine which contains a high percentage of sugar possesses a faint yellow color, a high specific gravity and a volume which is above normal. Experiments. i . Phenylhydrazine Reaction. — Test the urine according to one of the following methods : (a) To a small amount of phenylhy- drazine mixture, furnished by the instructor,1 add 5 c.c. of the urine, shake well and heat on a boiling water-bath for one-half to three- quarters of an hour. Allow the tube to cool slowly and examine the crystals microscopically (Plate III., opposite page 24). If the solution has become too concentrated in the boiling process it will be light-red in color and no crystals will separate until it is diluted with water. Yellow crystalline bodies called osazones are formed from cer- tain sugars under these conditions, in general each individual sugar giving rise to an osazone of a definite crystalline form which is typical for that sugar. It is important to remember in this con- nection that, of the simple sugars of interest in physiological chem- istry, dextrose and lsevulose yield the same osazone, with phenylhy- drazine. Each osazone has a definite melting-point, and as a fur- thur and more accurate means of identification it may be recrys- tallized and identified by the determination of its melting-point and nitrogen content. The reaction taking place in the formation of phenyldextrosazone is as follows : C6H1206 + 2(H2N-NH-C6H5) = Dextrose. Phenylhydrazine. C6H10O4(NNHC6H5)2 + 2H20 + H2. Phenyldextrosazone. (b) Place 5 c.c. of the urine in a test-tube, add 1 c.c. of phen- 1 This mixture is prepared by combining one part of phenylhydrazine-hydro- chloride and two parts of sodium acetate, by weight. These are thoroughly mixed in a mortar. URINE. 307 ylhydrazine-acetate solution furnished by the instructor,1 and heat on a boiling water-bath for one-half to three-quarters of an hour. Allow the liquid to cool slozvly and examine the crystals microscop- ically (Plate III., opposite p. 24). The phenylhydrazine test has been so modified by Cipollina as to be of use as a rapid clinical test. The directions for this test are given in the next experiment. 2. Cipollina's Test. — Thoroughly mix 4 c.c. of urine, 5 drops of phenylhydrazine (the base) and one-half c.c. of glacial acetic acid in a test-tube. Heat the mixture for about one minute over a low flame, shaking the tube continually to prevent loss of fluid by bumping. Add 4-5 drops of potassium hydroxide or sodium hydroxide (sp. gr. 1.16), being certain that the fluid in the test- tube remains acid ; heat the mixture again for a moment and then cool the contents of the tube. Ordinarily the crystals form at once, especially if the urine possesses a low specific gravity. If they do not appear immediately allow the tube to stand at least 20 min- utes before deciding upon the absence of sugar. Examine the crystals under the microscope and compare them with those shown in Plate III., opposite page 24. 3. Reduction Tests. — To their aldehyde or ketone structure many sugars owe the property of readily reducing the alkaline solutions of the oxides of metals like copper, bismuth and mercury; they also possess the property of reducing ammoniacal silver solu- tions with the separation of metallic silver. Upon this property of reduction the most widely used tests for sugars are based. When whitish-blue cupric hydroxide in suspension in an alkaline liquid is heated it is converted into insoluble black cupric oxide, but if a reducing agent like certain sugars be present the cupric hy- droxide is reduced to insoluble yellow cuprous hydroxide, which in turn on further heating may be converted into brownish-red or red cuprous oxide. These changes are indicated as follows : OH / Cu ^— Cu == 0 + H20. \ Cupric oxide \ (black 1. OH Cupric hydroxide (whitish-blue). 1 This solution is prepared by mixing one part by volume, in each case, of glacial acetic acid, one part of water and two parts of phenylhydrazine (the base). 3o8 PHYSIOLOGICAL CHEMISTRY. OH Cu / i \ Cu \ OH OH OH 2Cu - OH + H20 + 0. Cuprous hydroxide (yellow). Cu Cu-OH Cu-OH Cu \ ( / 0 + H20. Cuprous hydroxide Cuprous oxide (yellow). (brownish-red). The chemical equations here discussed are exemplified in Trom- mer's and Fehling's tests. (a) Trommer's Test. — To 5 c.c. of urine in a test-tube add one-, half its volume of KOH or NaOH. Mix thoroughly and add, drop by drop, agitating after the addition of each drop, a very dilute solution of cupric sulphate. Continue the addition until there is a slight permanent precipitate of cupric hydroxide and in con- sequence the solution is slightly turbid. Heat, and the cupric hy- droxide is reduced to yellow cuprous hydroxide or to brownish-red cuprous oxide. If the solution of cupric sulphate used is too strong, a small brownish-red precipitate produced in the presence of a low percentage of dextrose may be entirely masked. On the other hand, if too little cupric sulphate is used a light-colored precipitate formed by uric acid and purine bases may obscure the brownish- red precipitate of cuprous oxide. The action of KOH or NaOH in the presence of an excess of sugar and insufficient copper will produce a brownish color. Phosphates of the alkaline earths may also be precipitated in the alkaline solution and be mistaken for cuprous hydroxide. Trommer's test is not very satisfactory. (b) Fehling's Test. — To about 1 c.c. of Fehling's solution1 in 1 Fehling's solution is composed of two definite solutions — a cupric sulphate solution and an alkaline tartrate solution, which may be prepared as follows : Cupric sulphate solution = 34.65 grams of cupric sulphate dissolved in water and made up to 500 c.c. Alkaline tartrate solution = 125 grams of potassium hydroxide and 173 grams of Rochelle salt dissolved in water and made up to 500 c.c. URINE. 309 a test-tube add about 4 c.c. of water, and boil. This is done to determine whether the solution will of itself cause the formation of a precipitate of brownish-red cuprous oxide. If such a pre- cipitate forms, the behling's solution must not be used. Add urine to the warm Fehling's solution, a few drops at a tunc, and heat the mixture after each addition. 'The production of yellow cuprous hydroxide or brownish-red cuprous oxide indicates that reduction has taken place. The yellow precipitate is more likely to occur if the urine is added rapidly and in large amount, whereas with a less rapid addition of smaller amounts of urine the brownish- red precipitate is generally formed. This is a much more satisfactory test than Trommer's, but even this test is not entirely reliable when used to detect sugar in the urine. Such bodies as conjugate giycuronates, uric acid, nucleo- protein and homogentisic acid, when present in sufficient amount, may produce a result similar to that produced by sugar. Phosphates of the alkaline earths may be precipitated by the alkali of the Feh- ling's solution and in appearance may be mistaken for the cuprous diydroxide. Cupric hydroxide may also be reduced to cuprous oxide and this in turn be dissolved by creatinine^ a normal urinary constituent. This will give the urine under examination a greenish tinge and may obscure the sugar reaction even when a considerable amount of sugar is present. (c) Benedict's Modifications of Fehling's Test. — First Modifi- cation.— To 2 c.c. of Benedict's solution1 in a test-tube add 6 c.c. of distilled water and 7-9 drops (not more) of the urine under examination. Boil the mixture vigorously for about 15-30 sec- onds and permit it to cool to room temperature spontaneously. ( If desired this process may be repeated, although it is ordinarily un- necessary.) If sugar is present in the solution a precipitate will form which is often bluish-green or green at first, especially if the These solutions should be preserved separately in rubber-stoppered bottles and mixed in equal volumes when needed for use. This is done to prevent de- terioration. 1 Benedict's modified Fehling solution consists of two definite solution? — a cupric sulphate solution and an alkaline tartrate solution, which may be pre- pared as follows : Cupric sulphate solution = 34.65 grams of cupric sulphate dissolved in water and made up to 500 c.c. Alkaline tartrate solution = 100 grams of anhydrous sodium carbonate and 173 grams of Rochelle salt dissolved in water and made up to 500 c.c. These solutions should be preserved separately in rubber-stoppefed bottles and mixed in equal volumes when needed for use. This is done to prevent deterioration. 3IO PHYSIOLOGICAL CHEMISTRY. percentage of sugar is low, and which usually becomes yellozvish upon standing. If the sugar present exceeds 0.06 per cent this precipitate generally forms at or below the boiling-point, whereas if less than 0.06 per cent of sugar is present the precipitate forms more slowly and generally only after the solution has cooled. The greenish precipitate obtained with urines containing small amounts of sugar may be a compound of copper with the sugar or a com- pound of some constituent of the urine with reduced copper oxide instead of being a precipitate of cuprous hydroxide or oxide as is the case when the original Fehfing solution is reduced. Benedict claims that, whereas the original Fehling test will not serve to detect sugar when present in a concentration of less than 0.1 per cent that the above modification will serve to detect sugar when present in as small quantity as 0.015-0.02 per cent. The modified solution used in the above test differs from the original in that 100 grams of sodium carbonate is substituted for the 125 grams of potassium hydroxide ordinarily used, thus forming a Fehling solution which is considerably less alkaline than the orig- inal. This alteration in the composition of the Fehling solution is of advantage in the detection of sugar in the urine inasmuch as the strong alkalinity of the ordinary Fehling solution has a tendency, when the reagent is boiled with a urine containing a small amount of dextrose, to decompose sufficient of the sugar to render the de- tection of the remaining portion exceedingly difficult by the usual technique. Benedict claims that for this reason the use of his mod- ified solution permits the detection of smaller amounts of sugar than Joes the use of the ordinary Fehling solution. Benedict has fur- ther modified his solution for use in the quantitative determination of sugar (see page 368). Second Modification.1 — Very recently Benedict has further modi- fied his solution and has succeeded in obtaining one which does not deteriorate upon long standing.2 The following is the procedure 1 Private communication from Dr. S. R. Benedict. 2 Benedict's new solution has the following composition : Cupric sulphate 17.3 gm. Sodium citrate I73-0 gm. Sodium carbonate (anhydrous) 100.0 gm. Distilled water to 1000.0 c.c. With the aid of heat dissolve the sodium citrate and carbonate in about 600 c.c. of water. Pour (through a folded filter if necessary) into a glass graduate and make up to 850 c.c. Dissolve the cupric sulphate in about 100 c.c. of water and make up to 150 c.c. Pour the carbonate-citrate solution into a large beaker or casserole and add the cupric sulphate solution slowly, with constant stirring. The mixed solution is ready for use, and does not deteriorate upon long standing. URINE. 31 I "for the detection of dextrose in the urine : To five cubic centimeters of the reagent in a test-tube add eight (not more) drops of the urine to be examined. The fluid is then boiled vigorously for from one to two minutes and then allowed to cool spontaneously. In the presence of dextrose the entire body of the solution will be filled with a precipitate, which may be red, yellow or green in color, depending upon the amount of sugar present. [f no dextrose is present, the solution will either remain perfectly clear, or will show a very faint turbidity, due to precipitated urates. Even very small quantities of dextrose in urine (0.1 per cent) yield precipitates of surprising bulk with this reagent, and the positive reaction for dex- trose is the filling of the entire body of the solution with a precipi- tate, so that the solution becomes opaque. Since amount rather than color of the precipitate is made the basis of this test, it may be applied, even for the detection of small quantities of dextrose, as readily in artificial light as in daylight. (d) Allen's Modification of Fehling's Test. — The following pro- cedure is recommended : " From 7 to 8 c.c. of the sample of urine to be tested is heated to boiling in a test-tube, and, without separat- ing any precipitate of albumin which may be produced, 5 c.c. of the solution of cupric sulphate used for preparing Fehling's solution is added. This produces a precipitate containing uric acid, xanthine, hypoxanthine, phosphates, etc. To render the precipitation complete, however, it is desirable to add to the liquid, when partially cooled. from 1 to 2 c.c. of a saturated solution of sodium acetate having a feebly acid reaction to litmus.1 The liquid is filtered and to the filtrate, which will have a bluish-green color, 5 c.c. of the alkaline tartrate mixture used for preparing Fehling's solution is added, and the liquid boiled for 15-20 seconds. In the presence of mure than 0.25 per cent of sugar, separation of cuprous oxide occurs before the boiling-point is reached; but with smaller quantities precipitation takes place during the cooling of the solution, which becomes greenish, opaque, and suddenly deposits cuprous oxide as a fine brownish-red precipitate." (e) Boettger's Test. — To 5 c.c. of urine in a test-tube add 1 c.c 1 Sufficient acetic acid should be added to the sodium acetate solution to render it feebly acid to litmus. A saturated solution of sodium acetate keeps well, but weaker solutions are apt to become mould}-, and then possess the power of reducing Fehling's solution. Hence it is essential in all cases of importance to make a blank test by mixing equal measures of cupric sulphate solution, alkaline tartrate solution and water, adding a little sodium acetate solution, and heating the mixture to boiling. 312 PHYSIOLOGICAL CHEMISTRY. of KOH or NaOH and a very small amount of bismuth subnitrate, and boil. The solution will gradually darken and finally assume a black color due to reduced bismuth. If the test is made with urine containing albumin this must be removed, by boiling and fil- tering, before applying the test, since with albumin a similar change of color is produced (bismuth sulphide). (/) Nylander's Test (Ahnen's Test). — To 5 c.c. of urine in a test-tube add one-tenth its volume of Nylander's reagent1 and heat for five minutes in a boiling water-bath.2 The mixture will darken if reducing sugar is present and upon standing for a few moments a black color will appear. This color is clue to the precipitation of bismuth. If the test is made on urine containing albumin this must be removed, by boiling and filtering, before applying the test since with albumin a similar change of color is produced. Dextrose when present to the extent of 0.08 per cent may be de- tected by this reaction. It is claimed by Bechold that Nylander's and Boettger's tests give a negative reaction with solutions con- taining sugar when mercuric chloride or chloroform is present. Other observers have failed to verify the inhibitory action of the mercuric chloride and have shown that the inhibitory influence of chloroform may be overcome by raising the temperature of the urine ,to the boiling-point for a period of five minutes previous to making the test. Urines rich in indican, uroerythrin or h(E mat 0 porphyrin, as well as urines excreted after the ingestion of large amounts of certain medicinal substances, may give a darkening of Nylander's reagent similar to that of a true sugar reaction. According to Rustin and Otto the addition of PtCl4 increases the delicacy of Nylander's reaction. They claim that this procedure causes the sugar to be converted quantitatively. No quantitative method has yet been devised, however, based upon this principle. A positive Nylander or Boettger test is probably due to the fol- lowing reactions : (a) Bi(OH)2N03 + KOH = Bi(OH)3 + KNO„. (6) 2Bi(OH)3 - 30 = Bi2 + 3H20. 4. Fermentation Test. — Rub up in a mortar about 15 c.c. of 1 Nylander's reagent is prepared by digesting 2 grams of bismuth subnitrate and 4 grams of Rochelle salt in 100 c.c. of a 10 per cent potassium hydroxide solution. The reagent is then cooled and filtered. 3 Hammarsten suggests that the solution be boiled for 2-5 minutes (accord- ing to the sugar content) over a free flame and the tube then permitted to stand five minutes before drawing conclusions. URINE. J ' 3 the urine with a small piece of compressed yeast. Transfer the mixture to a saccharometer ( Fig. -'. p. 3] ) and stand it aside in a warm place for about 12 hours. It dextrose is present, alco- holic fermentation will occur and carbon dioxide will colled as a gas in the upper portion of the tube. On the completion of fer- mentation introduce, by means of a bent pipette, a little ECOH 50 lution into the graduated portion, place the thumb tightly over the opening in the apparatus and invert the saccharometer. Explain the result. 5. Barfoed's Test. — Place about 5 c.c. of Barfoed's solution1 in a test-tube and heat to boiling. Add the urine under examination slowly, a few drops at a time, heating after each addition. Re- duction is indicated by the production of a red precipitate. If the precipitate does not form upon continued boiling allow the tube to stand a few minutes and examine. XaCl interferes with this test (Welker). Barfoed's test is not a specific test for dextrose as is frequently stated, but simply serves to detect monosaccharides. Disaccharides will also respond to the test, according to Hinkel and Sherman, if the solution is boiled sufficiently long in contact with the reagent to hydrolyze the disaccharide through the action of the acetic acid present in the Barfoed's solution. 6. Polariscopic Examination. — For directions as to the use of the polariscope see page 32. PROTEINS. Normal urine contains a trace of protein material but the amount present is so slight as to escape detection by any of the simple tests in general use for the detection of protein urinary constituents. The following are the more important forms of protein material which have been detected in the urine under pathological conditions : ( 1 ) Serum albumin. (2) Serum globulin. I Deutero-proteose. (3) Proteoses -i Hetero-proteose. I " Bence-Jones' protein." (4) Peptone. (5) Nucleoprotein. (6) Fibrin. (7) Oxyhemoglobin. 'Barfoed's solution is prepared as follow-: Dissolve 4.5 grams of neutral, crystallized cupric acetate in too c.c. of water and add 0.12 c.c. of 50 per cent acetic acid. 314 PHYSIOLOGICAL CHEMISTRY. ALBUMIN. Albuminuria is a condition in which serum albumin or serum globulin appears in the urine. There are two distinct forms of albuminuria, i. e., renal albuminuria and accidental albuminuria. Sometimes the terms "true" albuminuria and "false" albuminuria are substituted for those just given. In the renal type the albumin is excreted by the kidneys. This is the more serious form of the malady and at the same time is more frequently encountered than the accidental type. Among the causes of renal albuminuria are altered blood pressure in the kidneys, altered kidney structure, or changes in the composition of the blood entering the kidneys, thus allowing the albumin to diffuse more readily. In the accidental form of albuminuria the albumin is not excreted by the kidneys as is the case in the renal form of the disorder, but arises from the blood, lymph or some albumin-containing exudate coming into con- tact with the urine at some point below the kidneys. Experiments. i. Heller's Ring Test. — Place 5 c.c. of concentrated HN03 in a test-tube, incline the tube, and, by means of a pipette allow the urine to flow slowly down the side. The liquids should stratify with the formation of a white zone of precipitated albumin at the point of juncture. If the albumin is present in very small amount the white zone may not form until the tube has been allowed to stand for several minutes. If the urine is quite concentrated a white zone, due to uric acid or urates, will form upon treatment with nitric acid as indicated. This ring may be easily differentiated from the albumin ring by repeating the test after diluting the urine with 3 or 4 volumes of water, whereupon, the ring, if due to uric acid or urates, will not appear. It is ordinarily possible to differ- tiate between the albumin ring and the uric acid ring without diluting the urine, since the ring, when due to uric acid, has ordi- narily a less sharply defined upper border, is generally broader than the albumin ring and frequently is situated in the urine above the point of contact with the nitric acid. Concentrated urines also oc- casionally exhibit the formation, at the point of contact, of a crys- talline ring with very sharply defined borders. This is urea nitrate and is easily distinguished from the "fluffy" ring of albumin. If there is any difficulty in differentiation a simple dilution of the urine with water, as above described, will remove the difficulty. Various URINE. 315 colored zones, due either to the presence of indican, bile pigments or to the oxidation of other organic urinary constituents, may form in this test under certain conditions. These colored rings should never be confounded with the white ring which alone denotes the presence of albumin. After the administration of certain drugs a white precipitate of resin acids may form at the point of contact of the two fluids and may cause the observer to draw wrong conclusions. This ring, if composed of resin acids, will dissolve in alcohol, whereas the albu- min ring will not dissolve. Weinberger has recently shown that a ring closely resembling the albumin ring is often obtained in urines preserved by thymol when subjected to Heller's test. The ring is due to the formation of nitro- sothymol and possibly nitrothymol. If the thymol is removed from the urine by extraction with petroleum ether1 previous to adding nitric acid, the ring does not form. An instrument called the albunioscope (horismascope) has been devised for use in this test and has met with considerable favor. The method of using the albumoscope is described below. Use of the Albunioscope. — This instrument is intended to facili- tate the making of " ring " tests such as Heller's and Roberts'. In making a test about 5 c.c. of the solution under examination is first introduced into the apparatus through the larger arm and the re- agent used in the particular test is then introduced through the capillary arm and allowed to flow down underneath the solution under examination. If a reasonable amount of care is taken there is no possibility of mixing the two solutions and a definitely defined white " ring " is easily obtained at the zone of contact. 2. Roberts' Ring Test. — Place 5 c.c. of Roberts' reagent- in a test-tube, incline the tube, and, by means of a pipette, allow the urine to flow slowly down the side. The liquids should stratify with the formation of a white zone of precipitated albumin at the point of juncture. This test is a modification of Heller's ring test and is rather more satisfactory than that test, since the colored rings never form and the consequent confusion is avoided. The albu- moscope (see above) may also be used in making this test. Accomplished readily by gently agitating equal volumes of petroleum ether and the urine under examination, for tzvo minutes in a test-tube, before ap- plying the test. " Roberts' reagent is composed of 1 volume of concentrated HXOj and 5 volumes of a saturated solution of MgSO.. 316 PHYSIOLOGICAL CHEMISTRY. 3. Spiegler's Ring Test. — Place 5 c.c. of Spiegler's reagent1 in a test-tube, incline the tube, and, by means of a pipette, allow 5 c.c. of urine, acidified with acetic acid, to flow slowly down the side. A white zone will form at the point of contact. This is an exceedingly- delicate test, in fact, too delicate for ordinary clinical purposes, since it serves to detect albumin when present in the merest trace (1 1250,000) and hence most normal urines will give a positive re- action for albumin when this test is applied. Some investigators claim that the delicacy of this test depends upon the presence of sodium chloride in the urine, the test losing accuracy if the sodium chloride content be low. 4. Jolles' Reaction. — Shake 5 c.c. of urine with 1 c.c. of 30 per cent acetic acid and 4 c.c. of Jolles' reagent2 in a test-tube. A white precipitate indicates the presence of albumin. Care should be taken to use the correct amount of acetic acid, since the use of too small an amount may result in the formation of mercury combinations which may cause confusion. In the presence of iodine, mercuric iodide will form but may readily be differenti- ated from albumin through the fact that it is soluble in alcohol. 5. Coagulation or Boiling Test. — (a) Heat 5 c.c. of urine to boiling in a test-tube. A precipitate forming at this point is due either to albumin or to phosphates. Acidify the urine slightly by the addition of 3-5 drops of very dilute acetic acid, adding the acid drop by drop to the hot solution. If the precipitate is due to phos- phates it will disappear under these conditions, whereas if it is due to albumin it will not only fail to disappear but will become more flocculent in character, since the reaction of a fluid must be acid to secure the complete precipitation of the albumin by this coagulation process. Too much acid should be avoided since it will cause the albumin to go into solution. Certain resin acids may be precipi- tated by the acid, but the precipitate due to this cause may be easily differentiated from the albumin precipitate by reason of its solubility in alcohol. 1 Spiegler's reagent has the following composition : Tartaric acid 20 grams. Mercuric chloride 40 grams. Glycerol 100 grams. Distilled water 1000 grams. 2 Jolles' reagent has the following composition : Succinic acid 40 grams. Mercuric chloride 20 grams. Sodium chloride 20 grams. Distilled water 1000 grams. URINE. 317 (h) A modification of this test in quite general use is as follows: Fill a test-tube two-thirds full of urine and gently heal the upper half of the fluid to boiling, being careful that this fluid does nol mix with the lower half. A turbidity indicates albumin or phosph Acidify the urine slightly by the addition of 3 5 drops of dilute acetic acid, when the turbidity, if due to phosphates, will disap- pear. Nitric acid is often used in place of acetic acid in these t c - 1 > . In case nitric acid is used ordinarily 1—2 drops is sufficient. 6. Acetic Acid and Potassium Ferrocyanide Test. — To 5 c.c. of urine in a test-tube add 5—10 drops of acetic acid. Mix well and add potassium ferrocyanide drop by drop, until a precipitate forms. This is a very delicate test. Schmiedl claims that a precipitate of Fe(Cn)cK2Zn or Fe(Cn)cZn2 is formed when urines contain- ing zinc are subjected to this test and that this precipitate resembles the precipitate secured with protein solutions. In the case of human urine a reaction was obtained when 0.000022 gram of zinc per cubic centimeter was present. Schmiedl further found that the urine collected from rabbits housed in zinc-lined cages possessed a zinc content which was sufficient to yield a ready response to the test. Zinc is the only interfering substance so far reported. 7. Tanret's Test. — To 5 c.c. of urine in a test-tube add Tanret's reagent1 drop by drop until a turbidity or precipitate forms. This is an exceedingly delicate test. Sometimes the urine is stratified upon the reagent as in Heller's or Roberts' ring test. According to Repiton, urates interfere with the delicacy of this test. Tanret. however, claims that urates do not interfere inasmuch as any pre- cipitate due to urates may be brought into solution by heat whereas an albumin precipitate under the same conditions will persist. Tanret further states that mucin interferes with the delicacy of the test and that it should therefore be removed from the urine under examination, by acidification with acetic acid and filtration before testing for albumin. 8. Sodium Chloride and Acetic Acid Test. — Mix two volumes of urine and one volume of a saturated solution of sodium chloride in a test-tube, acidify with acetic acid and heat to boiling. The pro- duction of a cloudiness or the formation of a precipitate indicates tanret's reagent is prepared as follows: Dissolve [.35 gram of mercuric chloride in 25 c.c. of water, add to this solution 3.32 grams of potassium iodide dissolved in 25 c.c. of water, then make the total solution up to 60 c.c. with water and add 20 c.c. of glacial acetic acid to the mixture. 3 l8 PHYSIOLOGICAL CHEMISTRY. the presence of albumin. The resin acids may interfere here as in the ordinary coagulation test (page 316) but they may be easily differentiated from albumin by means of their solubility in alcohol. GLOBULIN. Serum globulin is not a constituent of normal urine but fre- quently occurs in the urine under pathological conditions and is ordinarily associated with serum albumin. In albuminuria globulin in varying amounts often accompanies the albumin, and the clinical significance of the two is very similar. Under certain conditions globulin may occur in the urine unaccompanied by albumin. . Experiments. Globulin will respond to all the tests just outlined under Albumin. If it is desirable to differentiate between albumin and globulin in any urine the following processes may be employed : 1. Saturation With Magnesium Sulphate. — Place 25 c.c. of neutral urine in a small beaker and add pulverized magnesium sul- phate in substance to the point of saturation. If the protein present is globulin it will precipitate at this point. If no precipitate is pro- duced acidify the saturated solution with acetic acid and warm gently. Albumin will be precipitated if present. The above procedure may be used to separate globulin and albu- min if present in the same urine. To do this filter off the globulin after it has been precipitated by the magnesium sulphate, then acidify the clear solution and warm gently as directed. Note the formation of the albumin precipitate. 2. Half-Saturation With Ammonium Sulphate. — Place 25 c.c. of neutral urine in a small beaker and add an equal volume of a saturated solution of ammonium sulphate. Globulin, if present, will be precipitated. If no precipitate forms add ammonium sul- phate in substance to the point of saturation. If albumin is present it will be precipitated upon saturation of the solution as just indi- cated. This method may also be used to separate globulin and albumin when they occur in the same urine. Frequently in urine which contains a large amount of urates a precipitate of ammonium urate may occur when the ammonium sulphate solution is added to the urine. This urate precipitate should not be confounded with the precipitate due to globulin. The two precipitates may be differentiated by means of , the fact that the urate precipitate ordinarily appears only after, the lapse of sev- eral minutes whereas the globulin generally precipitates at once. URINE. 319 PROTEOSE AND PEPTONE. Proteoses, particularly deutero-proteose and hetero proteose, have frequently been found in the urine under various pathological con- ditions such as diphtheria, pneumonia, intestinal ulcer, carcinoma, dermatitis, osteomalacia, atrophy of the kidneys and in sarcomata of the bones of the trunk. " Bence-Jones' protein," a proteose-like substance, is of interest in this connection and its appearance in the urine is believed to be of great diagnostic importance in cases of multiple myeloma or myelogenic osteosarcoma. By some investi- gators this protein is held to be a variety of hetero-proteose whereas others claim that it possesses albumin characteristics. Peptone certainly occurs much less frequently as a constituent of the urine than does proteose, in fact most investigators seriously question its presence under any conditions. There are many in- stances of peptonuria cited in the early literature but because of the uncertainty in the conception of what really constituted a peptone it is probable that in many cases of so-called peptonuria the protein present was really proteose. Experiments. 1. Boiling Test. — Make the ordinary coagulation test according to the directions given under Albumin, page 316. If no coagulable protein is found allow the boiled urine to stand and note the gradual appearance, in the cooled fluid, of a flaky precipitate of proteose. This is a crude test and should never be relied upon. 2. Schulte's Method. — Acidify 50 c.c. of urine with dilute acetic acid and filter off any precipitate of nucleoprotein which may form. Now test a few cubic centimeters of the urine for coagulable pro- tein, by tests 2 and 5 under Albumin, pp. 315 and 316. If coagula- ble protein is present remove it by coagulation and filtration before proceeding. Introduce 25 c.c. of the urine, freed from coagulable protein, into 150 c.c. of absolute alcohol and allow it to stand for 12-24 hours. Decant the supernatant fluid and dissolve the pre- cipitate in a small amount of hot water. Now filter this solution, and after testing again for nucleoprotein with very dilute acetic acid, try the biuret test. If this test is positive the presence of pro- teose is indicated.1 Urobilin does not ordinarily interfere with this test since it is al- most entirely dissolved by the absolute alcohol when the proteose is precipitated. 'If it is considered desirable to test for peptone the proteose may he removed by saturation with (NH.hSCX according' to the directions given on page 115 and the filtrate tested for peptone by the biuret test. 320 PHYSIOLOGICAL CHEMISTRY. 3. v. Aldor's Method. — Acidify 10 c.c. of urine with hydro- chloric acid, add phosphotungstic acid until no more precipitate forms and centifugate1 the solution. Decant the supernatant fluid, add some absolute alcohol to the precipitate and centrifugate again. This washing with alcohol is intended to remove the urobilin and hence should be continued so long as the alcohol exhibits any colora- tion whatever. Now suspend the precipitate in water and add potassium hydroxide to bring it into solution. At this point the solution may be blue in color, in which case decolorization may be secured by gently heating. Apply the biuret test to the cool solu- tion. A positive biuret test indicates the presence of proteoses. 4. Detection of " Bence-Jones' Protein." — Heat the suspected urine very gently, carefully noting the temperature. At as low a temperature as 40 ° C. a turbidity may be observed and as the tem- perature is raised to about 60 ° C. a flocculent precipitate forms and clings to the sides of the test-tube. If the urine is now acidified very slightly with acetic acid and the temperature further raised to ioo° C. the precipitate at least partly disappears; it will return upon cooling the tube. This property of precipitating at so low a temperature and of dissolving at a higher temperature is typical of " Bence-Jones' pro- tein" and may be used to differentiate it from all other forms of protein material occurring in the urine. NUCLEOPROTEIN. There has been considerable controversy as to the proper classi- fication for the protein body which forms the " nubecula " of normal urine. By different investigators it has been called mucin, mucoid, phospho protein, nude 0 albumin and nude o protein. Of course, according to the modern acceptation of the meanings of these terms they cannot be synonymous. Mucin and mucoid are gly- coproteins and hence contain no phosphorus (see p. 106), whereas phosphoproteins and nucleoproteins are phosphorized bodies. It may possibly be that both these forms of protein, i. e., the glycopro- tein and the phosphorized type, occur in the urine under certain con- ditions (see page 290). In this connection we will use the term nucleo protein. The pathological conditions under which the con- tent of nucleoprotein is increased includes all affections of the urinary passages and in particular pyelitis, nephritis and inflamma- tion of the bladder. 1 If not convenient to use a centrifuge the precipitate may be filtered off and washed on the filter paper with alcohol. URINE. 32 1 Experiments. t. Detection of Nucleoprotein. — Place [0 c.c. of urine in a small beaker, dilute it with three volumes of water, to prevenl pre cipit'ation of urates, and make the reaction very strongly acid with acetic acid. If the urine becomes turbid it is an indication that nucleoprotein is present. If the urine under examination contains albumin the greater por- tion of this substance should be removed by boiling the urine before testing it for the presence of nucleoprotein. 2. Ott's Precipitation Test. — Mix 25 c.c. of the urine with an equal volume of a saturated solution of sodium chloride and slowly add Almen's reagent.1 In the presence of nucleoprotein a volumin- ous precipitate forms. BLOOD. The pathological conditions in which blood occurs in the urine may be classified under the two divisions hematuria and hemo- globinuria. In haematuria we are able to detect not only the haemo- globin but the unruptured corpuscles as well, whereas in hemo- globinuria the pigment alone is present. Hematuria is brought about through blood passing into the urine because of some lesion of the kidney or of the urinary tract below the kidney. Hemoglobi- nuria is brought about through hemolysis, i. e., the rupturing of the stroma of the erythrocyte and the liberation of the haemoglobin. This may occur in scurvy, typhus, pyemia, purpura and in other diseases. It may also occur as the result of a burn covering a con- siderable area of the body, or may be brought about through the action of certain poisons or by the injection of various substances having the power of dissolving the erythrocytes. Transfusion of blood may also cause hemoglobinuria. Experiments. 1. Heller's Test. — Render 10 c.c. of urine strongly alkaline with potassium hydroxide solution and heat to boiling. Upon allowing the heated urine to stand a precipitate of phosphates, colored red by the contained hematin, is formed. It is ordinarily well to make a " control " experiment using normal urine, before coming to a final decision. Certain substances such as cascara sagrada, rhubarb, santonin, 1 Dissolve 5 grams of tannin in 240 c.c. of 50 per cent alcohol and add 10 c.c. of- 25 per cent acetic acid. 22 322 PHYSIOLOGICAL CHEMISTRY. and senna cause the urine to give a similar reaction. Reactions due to such substances may be differentiated from the true blood reac- tion by the fact that both the precipitate and the pigment of the former reaction disappear when treated with acetic acid, whereas if the color is due to hsematin the acid will only dissolve the precipitate of phosphates and leave the pigment undissolved. 2. Teichmann's Haemin Test. — Place a small drop of the sus- pected urine or a small amount of the moist sediment on a micro- scopic slide, add a minute grain of sodium chloride and carefully evaporate to dryness over a low flame. Put a cover glass in place, run underneath it a drop of glacial acetic acid and warm gently until the formation of gas bubbles is observed. Cool the prepara- tion, examine under the microscope and compare the form of the crystals with those reproduced in Figs. 58 and 59, page 198. (See Atkinson and Kendall's modification, p. 197.) 3. Heller-Teichmann Reaction. — Produce the pigmented pre- cipitate according to directions given in Heller's test on p. 321. If there is a copious precipitate of phosphates and but little pigment the phosphates may be dissolved by treatment with acetic acid and the residue used in the formation of the haemin crystals according to directions in Experiment 2, above. 4. v. Zeynek and Nencki's Haemin Test. — To 10 c.c. of the urine under examination add acetone until no more precipitate forms. Filter off the precipitate and extract it with 10 c.c. of acetone rendered acid with 2-3 drops of hydrochloric acid. Place a drop of the resulting colored extract on a slide, immediately place a cover glass in position and examine under the microscope. Com- pare the form of the crystals with those shown in Figs. 58 and 59, page 198. Haemin crystals produced by this manipulation are sometimes very minute, thus rendering it difficult to determine the exact form of the crystal. 5. Schalfijew's Haemin Test. — Place 20 c.c. of glacial acetic acid in a small beaker and heat to 8o° C. Add 5 c.c. of the urine under examination, raise the temperature to 8o° C. and stand the mixture aside to cool. Examine the crystals under the microscope and compare them with those shown in Figs. 58 and 59, page 198. 6. Guaiac Test. — Place 5 c.c. of urine in a test-tube and by means of a pipette introduce a freshly prepared alcoholic solution of guaiac (strength about 1 :6o) into the fluid until a turbidity re- sults then add old turpentine or hydrogen peroxide, drop by drop, until a blue color is obtained. This is a very delicate test when URINE. 323 properly performed. Buckmaster has recently suggested the use of guaiaconic acid instead of the solution of guaiac. Sec discussion on page 192 and test on page T96. 7. Schumm's Modification of the Guaiac Test.— To about 5 c.c. of urine1 in a test-tube add about 10 drop- of a freshly prepared alcoholic solution of guaiac. Agitate the tube gently, add about 20 drops of old turpentine, subject the tube to a thorough shaking and permit it to stand for about 2-3 minutes. A blue color indicates the presence of blood in the solution under examination. In case there is insufficient blood to yield a blue color under these con ditions, a few c.c. of alcohol should be added and the tube gently shaken, whereupon a blue coloration will appear in the upper al- cohol-turpentine layer. A control test should always be made using water in place of urine. In the detection of very minute traces of blood only 3-5 drops of the guaiac solution should be employed. 8. Adler's Benzidine Reaction. — This is one of the most deli- cate of the reactions for the detection of blood. Different benzidine preparations vary greatly in their sensitiveness, however. Inas- much as benzidine solutions change readily upon contact with light, it is essential that they be kept in a dark place. The test is per- formed as follows: To a saturated solution of benzidine in alcohol or glacial acetic acid add an equal volume of 3 per cent hydrogen peroxide and one c.c. of the urine under examination. If the mix- ture is not already acid, render it so with acetic acid, and note the appearance of a green or blue color. A control test should be made substituting water for the urine. Often when urines containing a small amount of blood are tested by this reaction, the mixture is rendered so turbid as to make it difficult to decide as to the presence of a faint green color. Such urines should be extracted with an ether-acetic acid solution and the resulting extract washed with water before the test is applied to it. The sensitiveness of the benzidine reaction is greater when applied to aqueous solutions than when applied to the urine. 9. Spectroscopic Examination. — Submit the urine to a spectro- scopic examination according to the directions given on page 203 looking especially for the absorption-bands of oxyhannoglobin and methsemoglobin (see Absorption Spectra, Plate I. I. 1 Alkaline urine should be made slightly acid with acetic acid as the blue end- reaction is very sensitive to alkali. 324 PHYSIOLOGICAL CHEMISTRY. BILE. Both the pigments and the acids of the bile may be detected in the urine under certain pathological conditions. Of the pig- ments, bilirubin is the only one which has been positively identi- fied in fresh urine ; the other pigments, when present, are probably derived from the bilirubin. A urine containing bile may be yel- lowish-green to brown in color and when shaken foams readily. The staining of the various tissues of the body through the ab- sorption of bile due to occlusion of the bile duct causes a condi- tion known as icterus or jaundice. Bile is always present in the urine under such conditions unless the amount of bile reaching the tissues is extremely small. Experiments. Tests for Bile Pigments. 1. Gmelin's Test. — To about 5 c.c. of concentrated nitric acid in a test-tube add an equal volume of urine carefully so that the two fluids do not mix. At the point of contact note the various colored rings, green, blue, violet, red and reddish-yellow. 2. Rosenbach's Modification of Gmelin's Test. — Filter 5 c.c. of urine through a small filter paper. Introduce a drop of con- centrated nitric acid into the cone of the paper and observe the ■ succession of colors as given in Gmelin's test. 3. Nakayama's Reaction. — To 5 c.c. of urine in a test-tube add an equal volume of a 10 per cent solution of barium chloride. Cen- trifugate the mixture, pour off the supernatant fluid and heat the precipitate with 2 c.c. of Nakayama's reagent.1 In the presence of bile pigments the solution assumes a blue or green color. 3. Huppert's Reaction. — Thoroughly shake equal volumes of urine and milk of lime in a test-tube. The pigments unite with the calcium and are precipitated. Filter off the precipitate, wash it with water and transfer to a small beaker. Add alcohol acidified slightly with hydrochloric acid and warm upon a water-bath until the solution becomes colored an emerald green. According to Steensma, this procedure may give negative results even in the presence of the pigments, owing to the fact that the acid-alcohol is not a sufficiently strong oxidizing agent. He there- fore suggests the addition of a drop of a 0.5 per cent solution of 1 Prepared by combining 99 c.c. of alcohol and 1 c.c. of fuming hydrochloric acid containing 4 grams of ferric chloride per liter. urim:. 325 sodium nitrite to the acid-alcohol mixture before warming on the water-bath. Try this modification also. 5. Salkowski's Test.— Render 5 c.c. of urine alkaline with a few drops of a 10 per cent sodium carbonate solution and add a 10 per cent solution of calcium chloride, drop by drop, until the supernatant fluid exhibits the normal urinary color when the con- tents of the test-tube are thoroughly mixed. Filter off the pre- cipitate, and after washing it, place it in a second tube with 95 per cent alcohol. Acidify the alcohol with hydrochloric acid and, if necessary, shake the tube to bring the precipitate into solution. Heat the solution to boiling and observe the appearance of a green color which changes through blue and violet to red; if no bile is present the solution does not undergo any color change. This test will frequently exhibit greater delicacy than Gmelin's test. Steens- ma's suggestions mentioned under Huppert's Reaction, p. 324, ap- ply in connection with this test also. 4. Hammarsten's Reaction. — To about 5 c.c. of Hammarsten- reagent1 in a small evaporating dish add a few drops of urine. A green color is produced. If more of the reagent is now added the play of colors as noted in Gmelin's test may be obtained. 5. Smith's Test. — To 2-3 c.c. of urine in a test-tube add care- fully about 5 c.c. of dilute tincture of iodine (1 : 10) so that the fluids do not mix. A green ring is observed at the point of con- tact. 6. Salkowski-Schippers Reaction. — Neutralize the aciditv of 10 c.c. of the urine under examination with a few drops of a dilute solution of sodium carbonate, and add 5 drops of a 20 per cent solution of sodium carbonate and 10 drops of a 20 per cent solution of calcium chloride. Filter off the resultant precipitate upon a hardened filter-paper and wash it with water. Remove the precipitate to a small porcelain dish, add 3 c.c. of an acid- alcohol mixture2 and a few drops of a dilute solution of sodium nitrite and heat. The production of a green color indicates the presence of bile pigments. Tests for Bile Acids. i. Pettenkofer's Test. — To 5 c.c. of urine in a test-tube add 5 drops of a 5 per cent solution of sucrose. Now incline the tube. 1 Hammarsten's reagent is made by mixing I volume of 25 per cent nitric acid and 19 volumes of 25 per cent hydrochloric acid and then adding 1 volume oi this acid mixture to 4 volumes of 95 per cent alcohol. 2 Made by adding 5 c.c. of concent rated hydrochloric acid to 05 c.c. of 06 per cent alcohol. 326 PHYSIOLOGICAL CHEMISTRY. run about 2-3 c.c. of concentrated sulphuric acid carefully down the side and note the red ring at the point of contact. Upon slightly agitating the contents of the tube the whole solution gradually as- sumes a reddish color. As the tube becomes warm, it should be cooled in running water in order that the temperature may not rise above 70 ° C. 2. Mylius's Modification of Pettenkofer's Test. — To approx- imately 5 c.c. of urine in a test-tube add 3 drops of a very dilute (1:1,000) aqueous solution of furfurol, HC— CH HC C-CHO. \/ 0 Now incline the tube, run about 2-3 c.c. of concentrated sulphuric acid carefully down the side and note the red ring as above. In this case also, upon shaking the tube, the whole solution is colored red. Keep the temperature below 70 ° C. as before. 3. Neukomm's Modification of Pettenkofer's Test. — To a few drops of urine in an evaporating dish add a trace of a dilute sucrose solution and one or more drops of dilute sulphuric acid. Evaporate on a water-bath and observe the development of a violet color at the edge of the evaporating mixture. Discontinue the evaporation as soon as the color is observed. 4. v. Udransky's Test. — To 5 c.c. of urine in a test-tube add 3-4 drops of a very dilute (1 : 1,000) aqueous solution of furfurol. Place the thumb over the top of the tube and shake until a thick foam is formed. By means of a small pipette add 2-3 drops of con- centrated sulphuric acid to the foam and observe the dark pink col- oration produced. 6. Hay's Test. — This test is based upon the principle that bile acids have the property of reducing the surface tension of fluids in which they are contained. The test is performed as follows : Cool about 10 c.c. of urine in a test-tube to 170 C. or lower, and sprinkle a little finely pulverized sulphur upon the surface of the fluid. The presence of bile acids is indicated if the sulphur sinks to the bottom of the liquid, the rapidity with which the sulphur sinks depending upon the amount of bile acids present in the urine. The test is said to react with bile acids when the latter are present in the proportion 1 : 120,000. URINE. 327 Some investigators claim that it is impossible to differentiate between bile acids and bile pigments by this test. (II.. ACETONE, ( ! = 0. I I L it was formerly very generally believed that acetone appeared 111 the urine under pathological conditions because of increased protein decomposition. It is now generally thought that, in man, the nut- put of acetone arises principally from the breaking down of fatty tissues or fatty foods within the organism. The quantity of acetone eliminated has been shown to increase when the subject is fed an abundance of fat-containing food as well as during fasting, where- as a replacement of the fat with carbohydrates is followed by a marked decrease in the acetone excretion. Conditions are different with certain of the lower animals. With the dog, for instance, the output of acetone is not diminished when the animal is fed upon a carbohydrate diet, is decreased during fasting and increased when the animal is fed upon a diet of meat. Acetone and the closely related bodies, /3-oxybutyric acid and dia- cetic acid, are generally classified as the acetone bodies. They are all associated with a deranged metabolic function and may appear in the urine together or separately, depending upon the conditions. Acetone and diacetic acid may occur alone in the urine but |8-oxy- butyric acid is never found except in conjunction with one or the other of these bodies. Acetone and diacetic acid arise chiefly from the oxidation of /8-oxybutyric acid. The relation existing between these three bodies is shown in the following reactions : (a) CH3CH(OH)CH2-COOH + 0 = ^3-oxybutyric acid. CH,COCH2COOH + 11,0. Diacetic acid. (b) CH3CO-CH2-COOH= (CH3)2CO + CO,. Diacetic acid. Acetone. Acetone, chemically considered, is a ketone, di-methyl ketone. When pure it is a liquid which possesses a characteristic aromatic fruit-like odor, boils at 56— 570 C. and is miscible with water, alcohol or ether in all proportions. Acetone is a physiological as well as 328 PHYSIOLOGICAL CHEMISTRY. a pathological constituent of the urine and under normal con- ditions the daily output is about 0.01-0.03 gram. Pathologically, the elimination of acetone is often greatly in- creased and at such times a condition of acetonuria is said to exist. This pathological acetonuria may accompany diabetes mellitus, scarlet fever, typhoid fever, pneumonia, nephritis, phosphorus pois- oning, grave anaemias, fasting and a deranged digestive function; it also frequently accompanies auto-intoxication and chloroform and ether anaesthesia. The types of acetonuria most frequently met with are those noted in febrile conditions and in advanced cases of diabetes mellitus. Experiments. 1. Isolation from the Urine. — In order to facilitate the detection of acetone in the urine, the specimen under examination should be distilled and the tests as given below applied to the resulting dis- tillate. If it is not convenient to distil the urine, the tests may be conducted upon the undistilled fluid. To obtain an acetone dis- tillate proceed as follows : Place 100-250 c.c. of urine in a distilla- tion flask or retort and render it acid with acetic acid. Collect about one-third of the original volume of fluid as a distillate, add 5 drops of 10 per cent hydrochloric acid and redistil about one- half of this volume. With this final distillate conduct the tests as given below. 2. Gunning's Iodoform Test. — To about 5 c.c. of the urine or distillate in a test-tube add a few drops of Lugol's solution1 or ordinary iodine solution (I in KI) and enough NH4OH to form a black precipitate (nitrogen iodide). Allow the tube to stand (the length of time depending upon the content of acetone in the fluid under examination) and note the formation of a yellow- ish sediment consisting of iodoform. Examine the sediment under the microscope and compare the form of the crystals with those shown in Fig. 6, p. 42. If the crystals are not well formed recrys- tallize them from ether and examine again. The crystals of iodo- form should not be confounded with those of stellar phosphate (Fig. 76, p. 224) which may be formed in this test, particularly if made upon the undistilled urine. This test is preferable to Lieben's test (4) since no substance other than acetone will produce iodoform when treated according to the directions for this test ; both alcohol and aldehyde yield iodoform when tested by Lieben's test. 1 Lugol's solution may be prepared by dissolving 4 grams of iodine and 6 grams of potassium iodide in 100 c.c. of distilled water. URINE. Gunning's test is rather the most satisfactory test yet suggested for the detection of acetone, and may he used with good results even upon the undistilled urine. In some instances where the amount of acetone present is very small it is necessary to allow the tube to stand 24 hours he fore making the examination for iodoform crystals. This test serves to detect acetone when present in the ratio 1 : 100,000. 3. Legal's Test. — Introduce about 5 c.c. of the urine or distil- late into a test-tube, add a few drops of a freshly prepared aqueous solution of sodium nitroprusside and render the mixture alkaline with potassium hydroxide. A ruby red color, due to creatinine, a normal urinary constituent, is produced (see WeyTs test, p. 278). Add an excess of acetic acid and if acetone is present the red color will be intensified, whereas in the absence of acetone a yellow color will result. Make a control test upon normal urine to show that this is so. A similar red color may be produced by paracreso] in urines containing no acetone. 4. Lieben's Test. — Introduce 5 c.c. of the urine or distillate into a test-tube, render it alkaline with potassium hydroxide and add t-2 c.c. of iodine solution, drop by drop. If acetone is present a yellowish precipitate of iodoform will be produced. Identify the iodoform by means of its characteristic odor and its typical crystalline form (see Fig. 6, p. 42). While fully as delicate as Gun- ning's test (2) this test is not as accurate since by means of the procedure involved, either alcohol or aldehyde will yield a precipi- tate of iodoform. This test is especially liable to lead to erroneous deductions when urines from the advanced stages of diabetes are under examination, because of the presence of alcohol formed from the sugar through fermentative processes.1 5. Reynolds-Gunning Test. — This test depends upon the solu- bility of mercuric oxide in acetone and is performed as follows: To 5 c.c. of the urine or distillate add a few drops of mercuric chloride, render the solution alkaline with potassium hydroxide and add an equal volume of 95 per cent alcohol. Shake thoroughly in order to bring the major portion of the mercuric oxide into so- lution and filter. Render the clear filtrate faintly acid with hy- drochloric acid and stratify some ammonium sulphide, (Nil - 1 Welker reports the production of a pink or red color during the application of this test to the distillates from pathological urines which had been preserved with powdered thymol. He found the color to be due to an iodothymol com- pound which had been previously prepared synthetically by Messinger and Vortmann. 330 PHYSIOLOGICAL CHEMISTRY. upon this acid solution. At the zone of contact a blackish-gray ring- of precipitated mercuric sulphide, HgS, will form. Alde- hyde also responds to this test. Aldehyde, however, has never been detected in the urine and could only be present in this instance if the acidified urine was distilled too far. 6. Taylor's Test. — To 10 c.c. of the urine or distillate in a test- tube add a few drops of a freshly prepared aqueous solution of sodium nitroprusside and stratify concentrated ammonium hydrox- ide upon the mixture. The production of a magenta color at the point of contact indicates the presence of acetone in the urine or distillate under examination. Normal urine yields an orange-red color when subjected to this technique. CH3 DIACETIC ACID, C = 0 CH2-COOH. Diacetic or acetoacetic acid occurs in the urine only under patho- logical conditions and is rarely found except associated with acetone. It is formed from /?-oxybutyric acid, another of the acetone bodies, and upon decomposition yields acetone and carbon dioxide. Dia- ceturia occurs ordinarily under the same conditions as the patholog- ical acetonuria, i. e., in fevers, diabetes,, etc. (see p. 328). If very little diacetic acid is formed it may all be transformed into acetone, whereas if a larger quantity is produced both acetone and diacetic acid may be present in the urine. Diaceturia is most frequently observed in children, especially accompanying fevers and digestive disorders ; it is perhaps less frequently observed in adults, but when present, particularly in fevers and diabetes, it is frequently followed by fatal coma. Diacetic acid is a colorless liquid which is miscible with water, alcohol, and ether, in all proportions. It differs from acetone in giving a violet-red or Bordeaux-red color with a dilute solution of ferric chloride. Experiments. 1. Gerhardt's Test. — To 5 c.c. of urine in a test-tube add ferric chloride solution, drop by drop, until no more precipitate forms. In the presence of diacetic acid a Bordeaux-red color is produced ; this color may be somewhat masked by the precipitate of ferric phosphate, in which case the fluid should be filtered. UK1NE. 331 A positive result from the above manipulation simply indicates the possible presence of diacetic acid. Before making a final de- cision regarding the presence of this body make the two Following control experiments : (a) Place 5 c.c. of urine in a test-tube and boil it vigorously for 3-5 minutes. Cool the tube and, with the boiled urine, make the tesl as given on p. 330. As has been already stated, diacetic acid yields acetone upon decomposition and acetone duo not give a Bordeaux- red color with ferric chloride. By boiling as indicated above, there- fore, any diacetic acid present would be decomposed into acetone and carbon dioxide and the test upon the resulting fluid would be negative. If positive the color is due to the presence .of bodies other than diacetic acid. (b) Place 5 c.c. of urine in a test-tube, acidify with H2S04, to free diacetic acid from its salts, and carefully extract the mix- ture with ether by shaking. If diacetic acid is present it will be extracted by the ether. Now remove the ethereal solution and add to it an equal volume of dilute ferric chloride ; diacetic acid is indicated by the production of the characteristic Bordeaux-red color. This color disappears spontaneously in 24-48 hours. Such sub- stances as antipyrin, kairin, phenacetin, salicylic acid, salicylates, sodium acetate, thiocyanates and thallin yield a similar red color under these conditions, but when due to the presence of any of these substances the color does not disappear spontaneously but may remain permanent for days. Many of these disturbing sub- stances are soluble in benzene or chloroform and may be removed from the urine by this means before extracting with ether as above. Diacetic acid is insoluble in benzene or chloroform. 2. Arnold-Lipliawsky Reaction. — This reaction is somewhat more delicate than Gerhardt's test ( 1 ) and serves to detect diacetic acid when present in the proportion of 1 : 25,000. It is also negative toward acetone, /3-oxybutyric acid and the interfering drugs men- tioned as causing erroneous deductions in the application of Ger- hardt's test. If the urine under examination is highly pigmented it should be partly decolorized by means of animal charcoal before applying the test as indicated below. Place 5 c.c. of the urine under examination and an equal volume of the Arnold-Lipliawsky reagent1 in a test tube, add a few drops 1 This reagent consists of two definite solutions which are ordinarily preserved separately and mixed just before using. The two solutions are prepared as follows : (a) One per cent aqueous solution of potassium nitrite. 332 PHYSIOLOGICAL CHEMISTRY. of concentrated ammonia and shake the tube vigorously. Note the production of a brick-red color. Take 1-2 c.c. of this colored solution, add 10-20 c.c. of hydrochloric acid (sp. gr. 1.19), 3 c.c. of chloroform and 2-4 drops of ferric chloride solution and care- fully mix the fluids without shaking. Diacetic acid is indicated by the chloroform assuming a violet or blue color ; if diacetic acid is absent the color may be yellow or light red. H OH H /3-OXYBUTYRIC ACID, H — C — C — C — COOH. H H H This acid does not occur as a normal constituent of urine but is found only under pathological conditions and then always in eon- junction with either acetone or diacetic acid. Either of these bodies may be formed from /3-oxybutyric acid under proper conditions. It is present in especially large amount in severe cases of diabetes and has also been detected in digestive disturbances, continued fevers, scurvy, measles and in starvation. It is probable that, in man, /?- oxybutyric acid, in common with acetone and diacetic acid, arises principally from the breaking down of fatty tissues within the or- ganism. The condition in which large amounts of acetone and diacetic acid, and in severe cases /?-oxybutyric acid also, are excreted in the urine is known as " acidosis." In diabetes the deranged metabolic conditions cause the production of great quantities of these substances which lead to an acid intoxication and ultimately to diabetic coma. Ordinarily /3-oxybutyric acid is an odorless, transparent syrup, which is lsevorotatory and easily soluble in water, alcohol and ether ; it may be obtained in crystalline form. Experiments. 1. Black's Reaction. — Inasmuch as the urinary pigments as well as any contained sugar or diacetic acid will interfere with the deli- cacy of this test when applied to the urine directly the following preliminary procedure is necessary : Concentrate 10 c.c. of the (b) One gram of />-amino-acetophenon dissolved in 100 c.c. of distilled water and enough hydrochloric acid (about 2 c.c.) added, drop by drop, to cause the solution, which is at first yellow, to become entirely colorless. An excess of acid must be avoided. Before using, a and b are mixed in the ratio 1 : 2. urine. 333 urine under examination to one-third or one fourth of its original volume in an evaporating dish at a gentle heat. Acidif) the resi due with a few drops of concentrated hydrochloric arid, add suffi- cient plaster of Paris to make a thick paste and allow the mixture to stand until it begins to "set." It should now he stirred and broken up in the dish by means of a stirritlg rod with a blunl end. Extract the porous meal thus produced twice with ether by stirring and decantation. Any /?-oxybutyric acid present will be extracted by the ether. Evaporate the ether extract spontaneously or on a water-bath, dissolve the residue in water and neutralize it with barium carbonate. To five to ten c.c. of this neutral fluid in a tube add two to three drops of ordinary commercial acid hydro-en peroxide. Mix by shaking and add a few drops of Black's reagent.1 Permit the tube to stand and note the gradual development of a rose color which increases to its maximum intensity and then gradually fades.2 In carrying out the test care should be taken to see that the solution is cold and approximately neutral and that a large excess of hydrogen peroxide and Black's reagent are not added. In case but little /?-oxybutyric acid is present the color will fail to appear or will be but transitory if the oxidizing agents are added in too great excess. It is preferable to add a few drops of the reagent and at intervals of a few minutes repeat the process until the color under- goes no further increase in intensity. One part of /8-oxybutyric acid in 10,000 parts of the solution may be detected by this test. 2. Polariscopic Examination. — Subject some of the urine (free from protein) to the ordinary fermentation test (see page 313). This will remove dextrose and laevulose, which would interfere with the polariscopic test. Now examine the fermented fluid in the polariscope and if it is l?evorotatory the presence of /3-oxybutyric acid is indicated. This test is not absolutely reliable, however, since conjugate glycuronates are also l?evorotatory after fermenta- tion. 3. Kiilz's Test. — Evaporate the urine, after fermenting it as indicated in the last test, to a syrup, add an equal volume of con- centrated sulphuric acid and distil the mixture directly without cool- ing. Under these conditions a-crotonic acid is formed and is . present in the distillate. Allow the distillate to cool slowly and 'Made by dissolving five grams of ferric chloride ami 0.4 gram of ferrous chloride in 100 c.c. of water. "This disappearance of color is due to the further oxidation of the diacetic acid. 334 PHYSIOLOGICAL CHEMISTRY. note the formation of crystals of a-crotonic acid which are soluble in ether ancl melt at 72 ° C. In case very slight traces of j8-oxy- butyric acid be present in the urine under examination the amount of a-crotonic acid formed may be too small to yield a crystalline product. In this event the distillate should be extracted with ether, the ethereal extract evaporated and the residue washed with water. Under these conditions the impurities will be removed and the a- crotonic acid will remain behind as a residue. The melting-point of this residue may then be determined. CONJUGATE GLYCURONATES. Glycuronic acid does not occur free in the urine but is found, for the most part, in combination with phenol. Much smaller quan- tities are excreted in combination with indoxyl and skatoxyl. The total content of conjugate glycuronates seldom exceeds 0.004 Per cent under normal conditions. The output may be very greatly in- creased as the result of the administration of antipyrin, borneol, camphor, chloral, menthol, morphine, naphthol, turpentine, etc. The glycuronates as a group are lsevorotatory, whereas glycuronic acid is dextrorotatory. Most of the glycuronates reduce alkaline metallic oxides and so introduce an error in the examination of urine for sugar. Conjugate glycuronates often occur associated with dextrose in glycosuria, diabetes mellitus and in some other disorders. As a class the glycuronates are non-fermentable. Experiments. 1. Fermentation-Reduction Test. — Test the urine by Fehling's test. If there is reduction try Barfoed's test. If negative this indicates the absence of monosaccharides. A negative fermentation test would now indicate the presence of conjugate glycuronates (or lactose in rare cases).1 If dextrose is present in the urine tested for glycuronates the urine must first be subjected to a polariscopic examination, then fermented and a second polariscopic examination made. The sugar being dextrorotatory and fermentable and the glycuronates being lsevorotatory and non-fermentable the second polariscopic test will show a lsevorotation indicative of conjugate glycuronates. 2. Tollens' Reaction. — Make this test according to directions given under Pentoses, page 37. 3 If necessary to differentiate between lactose and glycuronates apply the mucic acid test (see p. 337) or the phenylhydrazine reaction (see p. 306). urine. 335 PENTOSES. We have two distinct types of pentosuria, /'. obtained as a decomposition product Crystals of Impure Leucine. f protejn see pig 2g p> y^ Tyro- sine crystallizes in urinary sediments in the well-known sheaf or tuft formation (Fig. 23, p. 72). For other tests on leucine and tyrosine see pages 83 and 84. Haematoidin and Bilirubin. — There are divergent opinions re- garding the occurrence of these bodies in urinary sediment. Each of them crystallizes in the form of tufts of small needles or in the form of small plates which are ordinarily yellowish-red in color (Fig. 41, p. 153). Because of the fact that the crystalline form of the two substances is identical many investigators claim them to be one and the same body. Other investigators claim, that while the crystalline form is the same in each case, that there are certain chemical differences which may be brought out very strikingly by properly testing. For instance, it has been claimed that haematoidin may be differentiated from bilirubin through the fact that it gives a momentary color reaction (blue) when nitric acid is brought in contact with it, and further, that it is not dissolved on treatment with ether or potassium hydroxide. Pathologically, typical crystals of haematoidin or bilirubin have been found in the urinary sediment in jaundice, acute yellow atrophy of the liver, carcinoma of the liver, cirrhosis of the liver, and in phosphorus poisoning, typhoid fever and scarlatina. Magnesium Phosphate. — Magnesium phosphate crystals occur rather infrequently in the sediment of urine which is neutral, alka- line or feebly acid in reaction. It ordinarily crystallizes in elon- gated, highly refractive, rhombic plates which are soluble in acetic acid. URINE. 3 5 I Indigo. — Indigo crystals are frequently found in urine which has undergone alkaline fermentation. The) result from the breaking down of indoxyl-sulphates or indoxyl-glycuronates. Ordinarily indigo deposits as dark blue stellate needles or occurs as amorphous particles or broken fragments. These crystalline or amorphous forms may occur in the sedimenl or may form a blue film on the sur- face of the urine. Indigo crystals generally occur in urine which is alkaline in reaction, but they have been detected in acid urine. Xanthine. — Xanthine is a constituent of normal urine hut is found in the sediment in crystalline form very infrequently, and then only in pathological urine. When present in the sediment xanthine generally occurs in the form of whetstone-shaped crystals some- what similar in form to the whetstone variety of uric acid crystal. They may be differentiated from uric acid by the great ease with which they may be brought into solution in dilute ammonia and on applying heat. Xanthine may also form urinary calculi. The clinical significance of xanthine in urinary sediment is not well understood. Melanin. — Melanin is an extremely rare constituent of urinary sediments. Ordinarily in melanuria the melanin remains in solu- tion; if it separates it is generally held in suspension as fine amor- phous granules. (b) Organized Sediments. Epithelial cells. Pus cells. ' Hyaline. Granular. Epithelial. Casts. -| Blood. Fatty. Waxy. _ Pus. Cylindroids. Erythrocytes. Spermatozoa. Urethral filaments. Tissue debris. Animal parasites. Micro-organisms. Fibrin. Foreign substances due to contamination. 352 PHYSIOLOGICAL CHEMISTRY. Epithelial Cells.---The detection of a certain number of these cells in urinary sediment is not, of itself, a pathological sign, since they occur in normal urine. However, in certain pathological con- ditions they are greatly increased in number, and since different areas of the urinary tract are lined with different forms of epithelial cells, it becomes necessary, when examining urinary sediments, to note not only the relative number of such cells, but at the same time to carefully observe the shape of the various individuals in order to determine, as far as possible, from what portion of the tract they have been derived. Since the different layers of the epithelial lin- ing are composed of cells different in form from those of the as- sociated layers, it is evident that a careful microscopical examina- tion of these cells may tell us the particular layer which is being desquamated. It is frequently a most difficult undertaking, how- ever, to make a clear differentiation between the various forms of epithelial cells present in a sediment. If skilfully done, such a microscopical differentiation may prove to be of very great diag- nostic aid. The principal forms of epithelial cells met with in urinary sedi- ments are shown in Fig. 105, below. Fig. 105. Epithelium from Different Areas of the Urinary Tract. a, Leucocyte (for comparison) ; b, renal cells ; c, superficial pelvic cells ; d, deep pelvic cells ; e, cells from calices ; /, cells from ureter ; g, g, g, g, gt squamous epi- thelium from the bladder ; h, h, neck-of-bladder cells ; i, epithelium from prostatic urethra ; k, urethral cells ; I, I, scaly epithelium ; m, m' , cells from seminal passages ; n, compound granule cells ; o, fatty renal cell. (Ogden.) URINE. 353 Pus Cells. — Pus corpuscles or leucocytes are presenl in extremely small numbers in normal urine. Any considerable increase in the number, however, ordinarily denotes a pathological condition, -en erally an acute or chronic inflammatory condition of some portion of the urinary tract. The sudden appearance of a large amount of pus in a sediment denotes the opening of an abscess into the urinary tract. Other form elements, such as epithelial cells, cast., etc., ordinarily accompany pus corpuscles in urinary sediment and a careful examination of these associated elements is necessary in order to form a correct diagnosis as to the origin of the pus. Pro- tein is always present in urine which contains pus. Fig. 106. Pus Corpusci.es. (.After Ultsmann.) i, Normal; 2, showing amoeboid movements; 3, nuclei rendered distinct by acetic acid 4, as observed in chronic pyelitis ; 5, swollen by ammonium carbonate. The appearance which pus corpuscles exhibit under the micro- scope depends greatly upon the reaction of the urine containing them. In acid urine they generally present the appearance of round, colorless cells composed of refractive, granular protoplasm, and may frequently exhibit amoeboid movements, especially if the slide containing them be warmed slightly. They are nucleated (one or more nuclei), the nuclei being clearly visible only upon treating the cells with water, acetic acid or some other suitable reagent. In urine which has a decided alkaline reaction, on the other hand, the pus corpuscles are often greatly degenerated. They may be seen as swollen, transparent cells, which exhibit no granular 24 354 PHYSIOLOGICAL CHEMISTRY. structure and as the process of degeneration continues the cell out- line ceases to be visible, the nuclei fade, and finally only a mass of debris containing isolated nuclei and an occasional cell remains. It is frequently rather difficult to make a differentiation between pus corpuscles and certain types of epithelial cells which are similar in form. Such confusion may be avoided by the addition of iodine solution (I in KI), a reagent which stains the pus corpuscles a deep mahogany-brown and transmits to the epithelial cells a light yellow tint. The test proposed by Vitali often gives very satisfactory re- sults. This simply consists in acidifying the urine (if alkaline) with acetic acid, then filtering, and treating the sediment on the filter paper with freshly prepared tincture of guaiac. The presence of pus in the sediment is indicated if a blue color is observed. Large numbers of pus corpuscles are present in the urinary sedi- ment in gonorrhoea, leucorrhcea, chronic pyelitis and in abscess of the kidney. Fig. 107. Hyaline Casts. One cast is impregnated with four renal cells. Casts. — These are cylindrical formations, which originate in the uriniferous tubules and are forced out by the pressure of the urine. They vary greatly in size but in nearly every instance they possess parallel sides and rounded ends. The finding of casts in the urine URINE. 355 is very important because of the fact thai they generally indicate some kidney disorder; if albumin accompanies the casts the indica- tion is much accentuated. Casts have been classified according to their microscopical characteristics as follows: (a) Hyaline. r the examinatii »n for filaments. These filaments may ordinarily be removed by a pipette since they arc generally macroscopic. Tissue Debris. — Masses of cells or fragments of tissue are fre- quently found in the urinary sediment. They may be found in the sediment in tubercular affections of the kidney and urinary tract or in tumors of these organs. Ordinarily it is necessary to make a histological examination of such tissue fragments before coming to a final decision as to their origin. Animal Parasites. — -The cysts, hooklets and membrane shreds of ecJiinococci are sometimes found in the urinary sediments. Other animal organisms which are more rarely met with in the urine are embryos of the Filaria sanguinis and eggs of the Distoma haematobium and Ascarides. Animal parasites in general occur most frequently in the urine in tropical countries. Micro-Organisms. — Bacteria as well as yeasts and moulds are frequently detected in the urine. Both the pathogenic and non- pathogenic forms of bacteria may occur. The non-pathogenic forms most frequently observed are micrococcus urea, bacillus ureas, and staphylococcus urea liquefaciens. Of the pathogenic forms many have been obsrved, e. g., Bacterium Coli, typhoid ba- cillus, tubercle bacillus, gonococcus, bacillus pyocyaneus and pro tens vulgaris. Yeast and moulds are most frequently met with in dia- betic urine. Fibrin. — Following hematuria, fibrin clots are occasionally ob- served in the urinary sediment. They are generally of a semi- gelatinous consistency and of a very light color, and when examined under the microscope they are seen to be composed of bundles of highly refractive fibers which run parallel. Foreign Substances Due to Contamination. — Such foreign substances as fibers of silk, linen or wool; starch granules, hair, fat and sputum, as well as muscle fibers, vegetable cells and food par- ticles are often found in the urine. Care should be taken that these foreign substances are not mistaken for any of the true sedi- mentary constituents already mentioned. CHAPTER XXI. URINE: CALCULI. Urinary calculi, also called concretions, or concrements are solid masses of urinary sediment formed in some part of the urinary tract. They vary in shape and size according- to their location, the smaller calculi termed sand or gravel in general arising from the kidney or the pelvic portion of the kidney, whereas the large calculi are ordinarily formed in the bladder. There are two general classes of calculi as regards composition, i. e., simple and compound. The simple form is made up of but a single constituent whereas the compound type contains two or rfiore individual constituents. The structural plan of most calculi consists of an arrangement of con- centric rings about a central nucleus, the number of rings frequently being dependent upon the number of individual constituents which enter into the structure of the calculus. In case two or more cal- culi unite to form a single calculus the resultant body will obviously contain as many nuclei as there were individual calculi concerned in its construction. Under certain conditions the growth of a cal- culus will be principally in only one direction, thus preventing the nucleus from maintaining a central location. The qualitative com- position of urinary calculi is dependent, in great part, upon the re- action of the urine e. g., if the reaction of the urine is acid the calculi present will be composed, in great part at least, of substances that are capable of depositing in acid urine. According to Ultzmann, out of 545 cases of urinary calculus, uric acid and urates formed the nucleus in about 81 per cent of the cases; earthy phosphates in about 9 per cent; calcium oxalate in about 6 per cent ; cystine in something over 1 per cent, while in about 3 per cent of the cases some foreign body comprised the nucleus. In the chemical examination of urinary calculi the most valuable data are obtained by subjecting each of the concentric layers of the calculus to a separate analysis. Material for examination may be conveniently obtained by sawing the calculus carefully through the nucleus, then separating the various layers or by scraping off from each layer (without separating the layers) enough powder to con- duct the examination as outlined in the scheme (see page 364). 362 URINE. 363 Varieties of Calculus. Uric Acid and Urate Calculi. — Uric acid and urates constitute the nuclei of a large proportion ("8r per cent) of urinary concre tions. Such stones are always colored, the tint varying from a pale yellow to a brownish-red. The surface of such calculi is generally smooth but it may be rough and uneven. Phosphatic Calculi. — Ordinarily these concretions consist prin- cipally of ''triple phosphate" and other phosphates of the alkaline earths, with very frequent admixtures of urates and oxalates. The surface of such calculi is generally rough but may occasionally be rather smooth. The calculi are somewhat variable in color, ex- hibiting gray, white or yellow tints under different conditions. When composed of earthy phosphates the calculi are character- ized by their friability. Calcium Oxalate Calculi. — This is the hardest form of calculus to deal with, and is rather difficult to crush. They ordinarily occur in two general forms, i. c, the small, smooth concretion which is characterized as the hemp-seed calculus and the medium-sized or large stone possessing an extremely uneven surface which is gen- erally classed as a mulberry calculus. This roughened surface of the latter form of calculus is due, in many instances, to protruding calcium oxalate crystals of the octahedral type. Calcium Carbonate Calculi. — Calcium carbonate concretions are quite common in herbivorous animals but of exceedingly rare occurrence in man. They are generally small, white or grayish calculi, spherical in form and possess a hard, smooth surface. Cystine Calculi. — The cystine calculus is a rare variety of cal- culus. Ordinarily they occur as small, smooth, oval or cylindrical concretions which are white or yellow in color and of a rather soft consistency. Xanthine Calculi.- — -This form of calculus is somewhat more rare than the cystine type. The color may vary from white to brownish-yellow. Very often uric acid and urates are associated with xanthine in this type of calculus. Upon rubbing a xanthine calculus it has the property of assuming a wax-like appearance. Urostealith Calculi. — This form of calculus is extremely rare. Such concretions are composed principally of fat and fatty acid. When moist they are soft and elastic but when dried they become brittle. Urostealiths are generally light in color. Fibrin Calculi. — Fibrin calculi are produced in the proce- 364 PHYSIOLOGICAL CHEMISTRY. On Heating the Powder on Platinum Foil, It Does not burn Does burn The powder when treated with HC1 With flame Without flame Does not effervesce ffQ 3' ft n SL p 3 Q. The pow- 3 -o Hcj » a p" 0 *A P- p* 2-q tn p- rt' (3! & 0 der gives the murexide test The gently-heated powder with HC1 •a S rt p- 3 ft °* ft tn ft pins rt P 0 2. CTQ The powder when moistened The pow- With a little KOH 3- O ft s o-rT der whe n 3 8 Ua- rt rt tn - rt < tn rt treated with i> ' p 0 51 I2J *T3 p g-3 ft £;. KOH gives tn =r 0 ° <-t p m 3 U 0 • 3 CL C. ft 3 ft -2 c rt 2 5 3 P 3 n *"* Si c 2. 0 p* In n O 3 3" p 3 »-! tn P £■ p rt tn 0 cr 0 Q' 1: 2 n tn tn ^ R w 5 p 3 5-2- p Ho 51 -*1 w p P O 0 •"d 0 0 d en 3 0 rt g. tn 3 O • P "> fD >T3 2- — 3* ft ft 0 0- O O - 3 " d 5 p 0' S2- us. p 5, 0 ►1 P l-tj 3 ft ^^ 13 ft 3 - O rt 0 O C ti rt « ft ^ 3 a. §2 in 3 •1 a a 2. p S. rt 1° ^3 p 3 rt < ft U) O ft tn W 33 ft < ft en O ft in ft !^ 1-" p q rf 2, w *r ■ 0 3 HH Ofg ^ 2. p 5" •-{ ft cn^ 5" 0 -t 13 So 3 2 0 ■ 5° « — Cl tn' erg ft S-. p n' p 0 SI O i-j ffl n 3 p* 0 • 3 p" HO ,— . O S 3 3 &■ 0 2 3- O-i O tn" C tn 0 _. p 3 0 >— • p Scr Pj O, orcj re &• i-« _ p ft c >-( 3_ 5' OfQ HrJ O P M 3^ 3 ^ O Cb 3 rt Eh tn' tn O^ <" 3 2. p p. §.1 3 5. oq g* c rt rt p 0 5" 3 p >-( rt p 0' 3 m 0 ?■ ~ tn tn ft .3 ^ ft H 0 tn P 3 CT En' 3 ^ O C 3 3 ft en O O ft 0 3 H O O P 0. 5" 3 0 X SL p* ft" 1 rt n> in c"d p 3 cr 2 pr f» r T3 3 3" rt O ffi. w O P > 3 3 0 3. S" 3 c •t p Triple pho e" (mixed wi nown amount liy phosphate' -a c 2 3- 3 B p c added to the final result. Calculate the quantity of uric acid in the twenty-four hour urine specimen. 2. Heintz Method. — This is a very simple method and was the first one in general use for the quantitative determination of uric acid. It is believed to be somewhat less accurate than the method just described. The procedure is as follows: Place [00 c.c. of filtered urine in a beaker, add 5 c.c. of concentrated hydrochloric acid, stir the fluid thoroughly and stand it away in a cool place for 24 hours. Filter off the uric acid crystals upon a washed, dried and weighed filter paper and wash them with cold distilled water, a few- cubic centimeters at a time until the chlorides are removed. Now wash, in turn, with alcohol and with ether and finally dry the paper and crystals to constant weight at no C. In the process of Avashing the uric acid free from chlorides an error is introduced, since every cubic centimeter of water so used dissolves 0.00004 gram of uric acid. For this reason a correction is necessary. Jt has been suggested that the pigment of the crystals is equivalent in weight to the amount of uric acid dissolved by the first 30 c.c. of water, and this factor should be taken into account in the computation of the percentage of uric acid. Calculation. — Since 100 c.c. of urine was used the corrected weight of the uric acid crystals, in grams, will express the percent- age of uric acid present. 3. Kriiger and Schmidt's Method. — This method serves for the detection of both uric acid and the purine bases. The principle involved is the precipitation of both the uric acid and the purine bases in combination with copper oxide and the subsequent decom- position of this precipitate by means of sodium sulphide. The uric acid is then precipitated by means of hydrochloric acid and the purine bases are separated from the filtrate in the form of their copper or silver compounds. The nitrogen content of the pre- cipitates of uric acid and purine bases is then determined by means of the Kjeldahl method (see p. 381) and the corresponding values for uric acid and purine bases calculated. The method i^ as fol- lows: To 400 c.c. of albumin-free urine1 in a liter flask,2 add 24 1 If albumin is present, the urine should be heated 10 boiling, acidified with acetic acid and filtered. 2 The total volume of urine for the twenty-four hours should be sufficiently diluted with water to make the total volume "f the solution 1000 2000 CC. 374 PHYSIOLOGICAL CHEMISTRY. grams of sodium acetate, 40 c.c. of a solution of sodium bisulphite1 and heat the mixture to boiling. Add 40-80 c.c.2 of a 10 per cent solution of cupric sulphate and maintain the temperature of the mixture at the boiling-point for at least three minutes. Filter off the flocculent precipitate, wash it with hot water until the wash water is colorless, and return the washed precipitate to the flask by puncturing the tip of the filter paper and washing the precipi- tate through by means of hot water. Add water until the volume in the flask is approximately 200 c.c, heat the mixture to boil- ing and decompose the precipitate of copper oxide by the addition of 30 c.c. of sodium sulphide solution.3 After decomposition is com- plete, the mixture should be acidified with acetic acid and heated to boiling until the separating sulphur collects in a mass. Filter the hot fluid by means of a filter pump, wash with hot water, add 10 c.c. of 10 per cent hydrochloric acid and evaporate the filtrate in a porcelain dish until the total volume has been reduced to about ten cubic centimeters. Permit this residue to stand about two hours to allow for the separation of the uric acid,, leaving the purine bases in solution. Filter off the precipitate of uric acid, using a small filter paper, and wash the uric acid, with water made acid with sulphuric acid, until the total volume of the original filtrate and the wash water aggregates 75 c.c. Determine the nitrogen content of the precipitate by means of the Kjeldahl method (see p. 381) and calculate the uric acid equivalent. Calculation. — In calculating the uric acid value from the total nitrogen simply multiply the latter by three and add 0.0035 to the product as a correction for the uric acid remaining in solution in the 75 c.c. IV. Urea. 1. Knop-Hiifner Hypobromite Method (using Marshall's Urea Apparatus). — Place the thumb over the side opening of the bulbed-tube of the apparatus (Fig. 118, p. 375) and carefully 1 A solution containing 50 grams of Kahlbaum's commercial sodium bisulphite in 100 c.c. of water. 2 The exact amount depending upon the content of the purine bases. 3 This is made by saturating a one per cent solution of sodium hydroxide with hydrogen sulphide gas and adding an equal volume of one per cent sodium hydroxide. Ordinarily the addition of 30 c.c. of this solution is sufficient, but the presence of an excess of sulphide should be proven by adding a drop of lead acetate to a drop of the solution. Under these conditions a dark brown color will show the presence of an excess of sodium sulphide. urine: quantitative analv-i-. 375 Fig. ■ r8. till i lie tube with sodium hypobromite solution.1 Close the opening in the end of the tube with a rubber stopper, incline the tube to allow air-bubbles to escape and finally invert the tube and fix the stoppered end in the saucer shaped vessel. l'.\ means of the grab" uated pipette rapidly introduce i c.c. of urine- into the hypobromite solution through the side opening of the bulbed- tube. Withdraw the pipette immedi- ately after the urine has been intro- duced. When the decomposition oi the urea is completed (10-20 minutes) gently tap the bulbed-tube with the finger in order to dislodge any gas bubbles which may have collected on the inner surface of the glass. The atmospheric pressure should now be equalized by attaching the funnel-tube to the bulbed-tube at the side opening and introducing hypobromite solution into it until the columns of liquid in the two tubes are uniform in height. The graduated scale of the bulbed- tube should now be read in order to determine the number of cubic centimeters of nitrogen gas evolved. By means of the appended formula the weight of the urea present in the urine under examination may be computed. Calculation/' — By properly substituting in the following formula the weight of urea, in grams, contained in the volume of urine de- composed ( 1 c.c. or more ) may readily be determined : 1 The ingredients of the sodium hypobromite solution should be prepared in the form of tzvo separate solutions. When needed for use mix equal volumes of solution a, solution b and water. (a) Dissolve 125 grams of sodium bromide in water, add 125 grams of bromine and make the total volume of the solution i liter. (b) A solution of sodium hydroxide having a specific gravity of I.250. This is approximately a 22.5 per cenl solution. Preserve both solutions in rubber-stoppered bottles. "Ordinarily 1 c.c. of urine is sufficient; more may be used, however, if it > content of urea is very low. 3 0.003665 = coefficient of expansion of gases for i° C. 354.5 = number of cc of nitrogen gas evolved from 1 gram of urea. '■ Hl'lll'll'l "■ ' ■ ■ ' Marshall's Urea Apparatus. (Tyson.) a, Bulbed measuring tube ; b, saucer-shaped vessel ; c, graduated pipette ; d, funnel-tube. 3^6 PHYSIOLOGICAL CHEMISTRY. 354.5 X 760(1 +0.003665O w = weight of urea, in grams. v = observed volume of nitrogen expressed in cubic centimeters. p — barometric pressure expressed in mm. of mercury. T = tension of aqueous vapor1 for temperature t. t = temperature (centigrade). If we wish to calculate the percentage of urea we may do so by means of the following proportion in which y represents the vol- ume of urine used and w denotes the weight of the urea contained in the volume y : y : w : : 100 : x (percentage of urea) . Sodium hypobromite solution may also be employed for the de- termination of urea in the apparatus devised by Htifner which is pictured in Fig. 119, page 377. 2. Knop-Hiifner Hypobromite Method (using the Doremus- Hinds Ureometer). — In common with the method already de- scribed this method depends upon the measurement of the volume of nitrogen gas liberated when the urea of the urine is decomposed by means of sodium hypobromite solution. The Doremus-Hinds ureometer (Fig. 120, p. 378), is one of the simplest and cheapest forms of apparatus in general use for the determination of urea by the hypobromite process. In using this apparatus proceed as fol- lows : Fill the side tube B and the lumen of the stopcock C with the urine under examination. Carefully wash out tube A with water and introduce into it sodium hypobromite solution2 being careful to fill the bulb sufficiently full to prevent the entrance of air into the 1 The values of T for the temperatures ordinarily met with are given in the following table : Tension in Tension in Temp. Mm. Temp. Mm. 15° C... 12.677 210 C 18.505 160 C 13.519 22° C 19.675 17° C 14.009 23° C 20.909 180 C 15-351 24° C 22.211 19° C 16.345 25° C 23.582 20° C 17.396 2 For directions as to the preparation of this solution see page 375. urine: quantitative analysis. graduated portion. Now allow I ' ";- "9« c.c. of urine1 to flow from tube B into tube A and after the evolution of gas bubbles has ceased (10-20 minutes) take the reading' of the graduated scale on tube A. In common with all other meth- ods which are based upon the de- composition of urea by means of hypobromite solution, this method is not absolutely correct. It is. however, sufficiently accurate for ordinary clinical purposes. Calculation. — Observe the reading on the graduated scale of tube A. This tube is so graduated as to rep- resent the weight of urea, in grams, per cubic centimeter of urine. If we wish to compute the percentage of urea present this may be done very readily by simply moving the deci- mal point two places to the right, e. g., if the reading is 0.02 gram the urine contains 2 per cent of urea. 3. Folin's Method. — This is one of the most accurate methods yet devised for the determination of urea in the urine. The procedure is as follows : Place 5 c.c. of urine in a 200 c.c. Erlenmeyer flask and add to it 5 c.c. of concentrated hydrochloric acid. 20 grams of crystallized magnesium chloride, a piece of paraffin the size of a hazel nut and 2-3 drops of a 1 per cent aqueous solution of "aliz- arin red.'' Insert a Folin safety tube I Fig. 1 _• i . p. 370") into the neck of the flask and boil the mixture until each drop of reflow from the safety tube produces a very perceptible bump: the heat is then reduced somewhat and continued one and one-half hours. The contents of the flask must not remain alkaline and to obviate this, at the first appearance of a reddish tinge in the contents <>\ the 'If the content of urea in the urine under examination is large, the urine may be diluted with water before determining the urea. If this is done it must of course be taken into consideration in computing the content of urea. Hufner's Urea Apparatus. 378 PHYSIOLOGICAL CHEMISTRY. flask a few drops of the acid distillate are shaken back into the flask. At the end of 1^2 hours the contents of the vessel are transferred to a 1 liter flask with about 700 c.c. of distilled water, about 20 c.c. of 10 per cent potassium hydroxide or sodium hydroxide solution is added and the mixture distilled into a known volume of -^L sulphuric acid until the contents of the flask are nearly dry or until the dis- FlG. tillate fails to give an alkaline reaction usmp' to litmus, showing the absence of ammonia. The time devoted to this process is ordinarily about an hour. Boil the distillate a few moments to free it from C02, then cool and titrate the mixture with -j-q sodium hydroxide, " alizarin red " as indicator. A " check " experiment should al- ways be made to determine the orig- inal ammonia content of the urine and of the magnesium chloride, if it is not absolutely pure, which of course should be subtracted from the total amount of ammonia as determined by the above process. The Folin method is extremely accu- rate under all conditions except when the urine contains sugar. When this ^g^ is the case the carbohydrate and the urea unite, upon being heated, and form a very stable combination. For this reason the Folin method is not suitable for use in the examination of such urines. The best method for use under such conditions is the combination Morner-Sjoqvist-Folin method which is given below. 4. Morner-Sjoqvist-Folin Method. — As has already been stated in the last experiment this method excels the Folin method in ac- curacy only in the determination of urea in the presence of carbo- hydrate bodies. Briefly the procedure is as follows ■} Bring the major portion of 1.5 gram of powdered barium hydroxide into solution in 5 c.c. of urine in a small flask, and treat the mixture with 100 c.c. of an alcohol-ether solution, consisting of two volumes 1The original description of the method may be found in an article by Morner: Skandinavisches Archiv fur Physiologic, 1903, xiv, p. 297. DOREMUS-HlNDS UrEOMETER. urine: quantitative analysis. 379 Fig. of 97 per cent alcohol and one volume of ether. Stopper the flask and allow it to stand 12 24 hours. Filter off the precipitate, wash it with the alcohol-ether mixture and remove the alcohol and ether from the filtrate by distillation, being careful to keep the tempera- ture of the mixture below 50° C.1 Treat the remaining fluid 1 aboul 25 c.c.) with 2 c.c. of hydrochloric acid (sp. gr. [.124) transfer it carefully to a 200 c.c. flask and evaporate the mixture to drynes a water-bath. Now add 20 grams of crystallized magnesium chloride and 2 c.c. of concentrated hydrochloric acid to the residue and after fitting the flask with a return cooler boil the mixture on a wire gauze over a small flame for two hours. Cool the solution, dilute to 750 c.c. or to 1000 c.c. with water, render the mixture alkaline with potas- sium hydroxide or sodium hydroxide, distil off the ammonia and collect it in an acid solution of known strength. Boil the distillate to remove carbon dioxide, cool and titrate with an alkali of known strength. In this method, as well as in Folin's method (see p. 377), correction must be made for the ammonia originally present in the urine and in the magnesium chloride. 5. Benedict and Gephart's Method. — Introduce into a rather wide test- tube or a small Erlenmeyer flask 5 c.c. of the urine under examination and an equal volume of dilute (1:4) hydrochloric acid. Cover the mouth of the tube or flask with a cap made by folding a piece of lead-foil over the top and place the vessel in an autoclave maintained at a temperature of 150-155° C. for one and one-half hours.'- After the autoclave has cooled, wash the contents of the tube into an Soo c.c. Kjeldahl distillation flask, dilute the urine mixture to about 400 c.c. with distilled water, add 20 c.c. of a to per cent solution of sodium 1 There is some decomposition of urea at 6o° C. "This corresponds to a pressure of about six kilograms per square centimeter. The cap? may be conveniently labelled with a stylus. Folin's Urea Appaiu 38o PHYSIOLOGICAL CHEMISTRY. hydroxide and distil about 40 minutes into an excess of standard acid. Complete the process as described under the Kjeldahl method (p. 381). Subtract the original ammonia content of the urine from the total ammonia content (ammonia -+- urea) as determined by the Kjeldahl method. V. Ammonia. 1. Folin's Method. — Place 25 c.c. of urine in an aerometer cylin- der, 30-40 cm. in height (Fig. 122, below), add about one gram of dry sodium carbonate and introduce some crude petroleum to pre- vent foaming. Insert into the neck of the cylinder a rubber stopper provided with two perforations into each of which passes a glass tube one of which reaches below the surface of the liquid. The shorter tube (10 cm. in length) is connected with a calcium chloride tube filled with cotton and this tube is in turn joined to a glass tube extending to the bottom of a 500 c.c. wide-mouthed flask which is intended to absorb the ammonia and for this purpose should con- tain 20 c.c. of f-Q sulphuric acid, 200 c.c. of distilled water and a few drops of an indicator ("alizarin red"). To insure the complete absorption of the ammonia the absorption flask is provided with a Fig. 122. Folin's Ammonia Apparatus. Folin improved absorption tube (Fig. 123, p. 381) which is very effective in causing the air passing from the cylinder to come into intimate contact with the acid in the absorption flask. In order to exclude any error due to the presence of ammonia in the air a similar urine: quantitative anal 38! Fig. 1 .- •;. absorption apparatus to the one just described is attached to the other side of the aerometer cylinder, thus insuring the passaj ammonia-free air into the cylinder. With an ordinary filter pump and good water pressure the last trace of ammonia should he removed from the cylinder in about one and one-half hours.1 The number of cubic centimeters of the ,N(I sul- phuric acid neutralized by the ammonia of the urine may be determined by direct titration with f^ sodium hydroxide. This is one of the most satisfactory methods yet devised for the determination of ammonia. Calculation. — Subtract the number of cubic centimeters of j-q sodium hydroxide used in the titration from the number of cubic centimeters of jq sulphuric acid taken. The remainder is the number of cubic centimeters of yo sulphuric acid neutralized by the NH3 of the urine. 1 c.c. of jQ sulphuric acid is equivalent to 0.001/ gram of NH3. Therefore if y represents the volume of urine used in the determination and y' the number of cubic centimeters of j-$ sulphuric acid neutralized b\ the NHZ of the urine, we have the following proportion : y : 100 ::y' X 0.0017 : x (percentage of XH3 in the urine examined). Folix Improved Ab- sorption Tube. Calculate the quantity of NH3 in the twenty-four hour urine specimen. VI. Nitrogen. Kjeldahl Method.2 — The principle of this method is the con- version of the various nitrogenous bodies of the urine into ammon- ium sulphate by boiling with concentrated sulphuric acid, the subse- quent decomposition of the ammonium sulphate by means of a fixed alkali (NaOH) and the collection of the liberated ammonia in an acid of known strength. Finally, this partly neutralized acid solu- 1 With any given filter pump a "check" test should be made with urine or better with a solution of an ammonium salt of known strength to determine how long the air current must be maintained to remove all the ammonia from 25 c.c. of the solution. "There are numerous modifications of the original Kjeldahl method; the one described here, however, has given excellent satisfaction and is recommended for the determination of the nitrogen content of urine. 382 PHYSIOLOGICAL CHEMISTRY. tion is titrated with an alkali of known strength and the nitrogen content of the urine under examination computed. The procedure is as follows : Place 5 c.c. of urine in a 500 c.c. long-necked, Jena glass Kjeldahl flask, add 20 c.c. of concentrated sulphuric acid and about 0.2 gram of cupric sulphate and boil the mixture for some time after it is colorless (about one hour) . Allow the flask to cool and dilute the contents with about 200 c.c. of water. Add a little more of a concentrated solution of NaOH than is nec- essary to neutralize the sulphuric acid1 and introduce into the flask a little coarse pumice stone or a few pieces of granulated zinc,2 to prevent bumping, and a small piece of paraffin to lessen the tendency to froth. By means of a safety-tube connect the flask with a con- denser so arranged that the delivery-tube passes into a vessel con- taining a known volume (the volume used depending upon the nitro- gen content of the urine) of y^- sulphuric acid, using care that the end of the delivery-tube reaches beneath the surface of the fluid.3 Mix the contents of the distillation flask very thoroughly by shak- ing and distil the mixture until its volume has diminished about one-half. Titrate the partly neutralized y^- sulphuric acid solution by means of yy sodium hydi oxide, using congo red as indicator, and calculate the content of nitrogen of the urine examined. Calculation. — Subtract the number of cubic centimeters of yg- sodium hydroxide used in the titration from the number of cubic centimeters of yg- sulphuric acid taken. The remainder is equiva- lent to the number of cubic centimeters of jq sulphuric acid, neu- tralised by the ammonia of the urine. One c.c. of j-$ sulphuric acid is equivalent to 0.0014 gram of nitrogen. Therefore, if 3' repre- sents the volume of urine used in the determination, and y' the number of cubic centimeters of yg- sulphuric acid neutralised by the ammonia of the urine, we have the following proportion : y: 100: :y' X 0.0014 :.r (percentage of nitrogen in the urine ex- amined). Calculate the quantity of nitrogen in the twenty-four hour urine specimen. 1 This concentrated sodium hydroxide solution should be prepared in quantity and "check" tests made to determine the volume of the solution necessary to neutralize the volume (20 c.c.) of concentrated sulphuric acid used. 2 Powdered zinc may be substituted. 3 This delivery-tube should be of large caliber in order to avoid the " sucking back" of the fluid. urine: quantitative analysi 383 VII. Hippuric Acid. Dakin's Methods.1 Preliminary Procedure. Place [50C.C. (or more) of the urine under examination in a porcelain evaporating dish and evaporate almost to dryness upon a water hath. \dd about 1 gram, of sodium dihydrogen phosphate, about 25 grams of gypsum (CaSO,, 2H20) and rub up with a pestle and stir with a spatula until a uniform mixture results. Dry the powder thus pro duced in a water-oven for about two hours, at the end of which period it should he rubbed up a second time, to remove lumps, and transferred to a Schleicher and Schtill "extraction shell" and ex- tracted in a Soxhlet apparatus in the usual way. (see p. 410). The extraction medium is ethyl acetate and the flask containing the acetate should be strongly heated over a sand-bath2 for about two hours. The ethyl acetate extract is now transferred to a separators- funnel, and the original flask rinsed with sufficient fresh ethyl acetate to make the total volume in the separately funnel3 about 100 c.c. Wash the ethyl acetate solution five limes with a saturated solution of sodium chloride, using 8 c.c. of the sodium chloride solution at each extraction, shaking vigorously and removing the sodium chloride extract in each case before adding fresh sodium chloride solution. The sodium chloride removes the urea completely and the hippuric acid is then determined in the urea-free solution by the fol- lowing volumetric or gravimetric procedure : 1. Volumetric Determination. — Transfer the urea-free ethyl acetate solution, prepared as described above, to a Kjeldahl flask. add about 25 c.c. of water, a small piece of pumice stone to prevent bumping, attach a condenser and distil off the ethyl acetate4 over a free flame. After practically all of the ethyl acetate has been dis- tilled off the nitrogen in the remaining solution should be deter- mined by means of the Kjeldahl method (see p. 381). The main source of error in this method is the fact that any nitrogen present in the form of phenaceturic acid or indole aeetie acid is determined as hippuric acid nitrogen. The error from this source is, however, usually trifling. Calculation. — Calculate as usual for nitrogen determinations, re- 1 Private communication to the author from Dr. H. D. Dakin. 2 A water-bath cannot be substituted inasmuch as the resultant extr would be too slow. 3 This ethyl acetate solution contain- hippuric acid, urea and other substances. 4 The ethyl acetate after separation from the watery layer of the distillate may be dried over calcium chloride and used again. 384 PHYSIOLOGICAL CHEMISTRY. membering that 1 c.c. of j-q sulphuric acid is equivalent to 0.0179 gram hippuric acid. 2. Gravimetric Determination. — The urea-fr.ee ethyl acetate so- lution, contained in the separatory funnel, after washing with sodium chloride solution, as described under Preliminary Procedure, p. 383, is washed with 5 c.c. of distilled water to remove the major portion of the sodium chloride. Transfer the solution from the separatory funnel to a round-bottomed flask and subject it to a steam distillation in the usual way. A slow current of steam should be used while the ethyl acetate is being distilled off and later a more rapid current may be employed. The distillation should be con- tinued for twenty minutes. Now add about 0.1 gram of charcoal to the aqueous solution which is heated to boiling and filtered hot. Evaporate the solution in a weighed Jena glass dish on a water-bath until the volume of the solution is reduced to about 3 c.c. Stand the dish in a warm place until evaporation is complete and a crys- talline residue remains. Wash the residue, in turn, with 2 c.c. of dry ether, and 1 c.c. of water, dry it in an air-bath at ioo° C. and weigh. If it is so desired the residue may be recrystallized from a little hot water and the melting-point determined. Pure hippuric acid melts at 1870 C. Contamination with phenaceturic acid may be detected both by the melting-point and the microscopical char- acteristics. VIII. Sulphur. 1. Total Sulphates. — Folin's Method. — Place 25 c.c. of urine in a 200-250 c.c. Erlenmeyer flask, add 20 c.c. of dilute hydrochloric acid1 (1 volume of concentrated HC1 to 4 volumes of water) and gently boil the mixture for 20-30 minutes. To minimize the loss of water by evaporation the mouth of the flask should be covered with a small watch glass during the boiling process. Cool the flask for 2-3 minutes in running water, and dilute the contents to about 150 c.c. by means of cold water. Add 10 c.c. of a 5 per cent solution of barium chloride slowly, drop by drop, to the cold solution.2 The contents of the flask should not be stirred or shaken during the ad- dition of the barium chloride. Allow the mixture to stand at least 1 If it is desired, 50 c.c. of urine and 4 c.c. of concentrated acid may be used instead. 2 A dropper or capillary funnel made from an ordinary calcium chloride tube and so constructed as to deliver 10 c.c. in 2-3 minutes is recommended for use in adding the barium chloride. urine: quantitative analysis. J85 one hour, then shake up (he solution and filter it through a weighed Gooch crucible.1 Wash the precipitate of I'.aSo, with aboul 250 c.c. of cold water, dry it in an air-hath or over a very low flame, then ignite,2 cool and weigh. Calculation. — Subtract the weight of the Gooch crucible from the weight of the crucible and the I in SO, precipitate n, ..htain the weight of the precipitate. The weight of So,:; in the volume of urine taken may be determined by means of the following propor tion. Mol. wt. Wt. of Mo', wt. BaS04:BaS04: :SO:j:.r (wt. of SOa in gram.). ppt. Representing the weight of the BaS04 precipitate by y and substi- tuting the proper molecular weights, we have the following pro- portion : 231.7:3/: -.yg.^-.x (wt. of S03 in grams in the quantity of urine used). Calculate the quantity of S03 in the twenty-four hour specimen of urine. To express the result in percentage of SOs simply divide the value of x, as just determined, by the quantity of urine used. 2. Inorganic Sulphates. — Folin's Method. — Place 25 c.c. of 1If a Gooch crucible is not available the precipitate of BaSO. may be filtered off upon a washed filter paper (Schleicher & Schull's, No. 589, blue ribbon) and after washing the precipitate with about 250 c.c. of cold water the paper and precipitate may be dried in an air-bath, or over a low flame. The ignition may then be carried out in the usual way in the ordinary platinum or porcelain crucible. In this case correction must be made for the weight of the ash of tin- filter paper used. 2 Care must be taken in the ignition of precipitates in Gooch crucibles. The flame should never be applied directly to the perforated bottom or to the sides of the crucible, since such manipulation is invariably attended by mechanical losses. The crucibles should always be provided with lids and tight bottoms during the ignition. In case porcelain Gooch crucibles, whose bottoms are nol provided with a non-perforated cap, are used, the crucible may be placed upon the lid of an ordinary platinum crucible durin.n ignition. The lid should be sup- ported on a triangle, the crucible placed upon the lid and the Same applied to the improvised bottom. Ignition should be complete in to minutes if no organic matter is present. 3 It is considered preferable by many investigators to express all sulphur values in terms of S rather than SO3. 26 386 PHYSIOLOGICAL CHEMISTRY. urine and ioo c.c. of water in a 200-250 c.c. Erlenmeyer flask and acidify the diluted urine with 10 c.c. of dilute hydrochloric acid ( 1 volume of concentrated HC1 to 4 volumes of water). In case the urine is dilute 50 c.c. may be used instead of 25 c.c. and the volume of water reduced proportionately. Add 10 c.c. of 5 per cent barium chloride slowly, drop by drop, to the cold solution and from this point proceed as indicated in the method for the determination of Total Sulphates, page 384. Calculate the quantity of inorganic sulphates, expressed as S03, in the twenty-four hour urine specimen. Calculation. — Calculate according to the directions given under Total Sulphates, page 385. 3. Ethereal Sulphates. — Foliris Method. — Place 125 c.c. of urine in an Erlenmeyer flask of suitable size, dilute it with 75 c.c. of water and acidify the mixture with 30 c.c. of dilute hydrochloric acid (1 volume of concentrated HO to 4 volumes of water). To the cold solution add 20 c.c. of a 5 per cent solution of barium chlor- ide, drop by drop.1 Allow the mixture to stand about one hour, then filter it through a dry filter paper.2 Collect 125 c.c. of the filtrate and boil it gently for at least one-half hour. Cool the solution, filter off the precipitate of BaS04, wash, dry and ignite it according to the directions given on page 385. Calculation. — The weight of the BaS04 precipitate should be multiplied by 2 since only one-half (125 c.c.) of the total volume (250 c.c.) of fluid was precipitated by the barium chloride. The remaining calculation should be made according to directions given under Total Sulphates, page 385. Calculate the quantity of ethereal sulphates, expressed as SOs, in the twenty- four hour urine specimen. 4. Total Sulphur. — Osborne-Folin Method. — Place 25 c.c. of urine3 in a 200-250 c.c. nickel crucible and add about 3 grams of sodium peroxide. Evaporate the mixture to a syrup upon a steam water-bath and heat it carefully over an alcohol flame until it solidi- fies (15 minutes). Now remove the crucible from the flame and 1 See note (2) at the bottom of page 384. 2 This precipitate consists of the inorganic sulphates. If it is desired, this BaSOi precipitate may be collected in a Gooch crucible or on an ordinary quanti- tative filter paper and a determination of inorganic sulphates made, using the same technique as that suggested on p. 385. In this way we are enabled to determine the inorganic and ethereal sulphates in the same sample of urine. 3 If the urine is very dilute 50 c.c. may be used. urine: quantitative analysi allow it to cool. Moisten the residue with i 2 c.c. of water,1 sprinkle about 7-8 grams of sodium peroxide over the contents oi the crucible and fuse the mass over an alcohol flame for about io minutes. Allow the crucible to cool for a few minutes, add about 100 c.c. of water to the contents and heal at leasl one half hour over an alcohol flame, to dissolve the alkali and decompose the sodium peroxide. Next rinse the mixture into a 400 1.50 c.c. Er lenmeyer flask, by means of hot water, and dilute it to about 25OC.C Heat the solution nearly to the boiling point and add concentrated hydrochloric acid slowly until the nickelic oxide, derived from tin- crucible, is just brought into solution.- A few minutes boiling should now yield a clear s< ilutii in. In ease t< i< 1 lilt le pen ixide or too much water was added for the final fusion a clear solution will not be obtained. In this event cool the solution and remove the in- soluble matter by filtration. To the clear solution add 5 c.c. of very dilute alcohol 1 about [8 20 per cent) and continue the boiling for a few minutes. The alc< >- hoi is added to remove the chlorine which was formed when the solution was acidified. Add 10 c.c. of a 10 per cent solution of barium chloride, slowly, drop by drop,3 to the liquid. Allow the precipitated solution to stand in the cold two days and then filter and continue the manipulation according to the directions given under Total Sulphates, page 384. Calculation. — Make the calculation according to directions given under Total Sulphates, p. 384. Calculate the quantity of sulphur, expressed as S03 or S, present in the twenty-four hour urine specimen. 5. Total Sulphur. — Sodium Hydroxide and Potassium Nitrate Fusion Method. — Place 25 c.c. of urine in a silver crucible and evaporate to a thick syrup on a water-bath. Add 10 gram- of sodium hydroxide and 2 grams of potassium nitrate to the residue and fuse the mass, over an alcohol flame, until all organic matter has disappeared and the fused mixture is clear. Cool the mixture. transfer it to a casserole, by means of hot water, acidify slightly with hydrochloric acid and evaporate it to dryness on a water bath. Moisten the residue with a few drops of dilute hydrochloric acid and bring it into solution with hot water. Filter, heat the filtrate to boiling and immediately precipitate it by the addition "i 10 c.c. xThis moistening of the residue with a small amount of water 1- verj essential and should not be neglected. "About 18 c.c. of acid is required for S grams of sodium peroxide. 3 See note (2) at the bottom of page 384. 388 PHYSIOLOGICAL CHEMISTRY. of a 10 per cent solution of barium chloride, adding the solution slowly, drop by drop. Allow the precipitated solution to stand 2 hours and filter while cold. Ignite, weigh and calculate according to directions given under Total Sulphates, p. 384. Compute the quantity of sulphur, expressed as SOs or S, present in the twenty-four hour urine specimen. Ftg. 124. Berthelot-Atwater Bomb Calorimeter. (Cross-section of Apparatus as Ready for Use.) A, Steel cup or bomb proper ; C, collar of steel ; G, opening through which oxygen is forced into the bomb ; H and I', insulated wires which serve to conduct an electric current for igniting the substance which is held in the small capsule ; L, a stirrer which serves to keep the water surrounding the bomb in motion and insures the equalization of temperature ; P, a delicate thermometer which shows the rise in temperature of the water surrounding the bomb. URINE: QUANl N \Tl\ I. ANALYSIS. 6. Total Sulphur. — Sherman's Compressed Oxygen Method.1 — Evaporate as much urine on an absorbenl filter block2 at 55 1 the block will conveniently absorb and burn the block so prepared in a bomb-calorimeter3 using 25 30 atmospheres of oxygen. Connect the bomb with a wash-bottle containing water, and allow the gas to bubble through the liquid until the high pressure within the apparatus has been reduced to atmospheric pressure. Now open the bomb and thoroughly rinse the interior, using water from the wash-bottle for the first rinsing. Dissolve any ash found in the combustion capsule in hydrochloric acid and add this solution to the main solution. Evaporate to 150 c.c, filter and cool the filtrate. Add 10 c.c. of a 5 per cent solution of barium chloride to the cold filtrate, slowly, drop by drop.4 The contents of the flask should not be stirred or shaken during- the addition of the barium chloride. Allow the mixture to stand at least one hour, then shake up the solution and filter it through a weighed Gooch crucible. Manipu- late the precipitate of BaS04 according to direction given under Total Sulphates, page 384. Calculate the quantity of sulphur, expressed as SO:J or S, present in the twenty-four hour urine specimen. IX. Phosphorus. 1. Total Phosphates. — Uranium Acetate Method. — To 50 c.c. of urine in a small beaker or Erlenmeyer flask add 5 c.c. of a special sodium acetate solution5 and heat the mixture to the boiling-point. From a burette, run into the hot mixture, drop by drop, a standard solution of uranium acetate0 until a precipitate ceases to form and 1 See Sherman's Organic Analysis, p. 19. 2 Only a small amount of urine should be added at one time, it being nee to make several evaporations before the block contains sufficient urinary residue to proceed with the combustion. 3 The Berthelot-Atwater apparatus (Fig. 124, page 388) is well adapted to this purpose. 4 See note (2) at the bottom of page 3X4. 5 The sodium acetate solution is prepared by dissolving 100 grams of sodium acetate in 800 c.c. of distilled water, adding 100 c.c. of 30 per cent acetic acid to the solution and making the volume of the mixture up to 1 liter with water. "This uranium acetate solution may he prepared by dissolving 35401 grams of uranium acetate in one liter of water. One c.c. of such a solution should be equivalent to 0.005 gram of P-Oe, phosphoric anhydride. This solution may be standardized as follows: To 51' c.c. of a standard solution of disodium hyd phosphate, of such a strength that the 50 c.c. contains 0.1 gram of PjO§, add 5 c.c. of the sodium acetate solution, mentioned above, and titrate with the uranium solution to the correct end-reaction as indicated in the method proper. 390 PHYSIOLOGICAL CHEMISTRY. a drop of the mixture when removed by means of a glass rod and brought in contact with a drop of a solution of potassium ferrocya- nide on a porcelain test-tablet produces instantaneously a brownish- red coloration.1 Take the burette reading and calculate the P205 content of the urine under examination. Calculation. — Multiply the number of cubic centimeters of uran- ium acetate solution used by 0.005 to determine the number of grams of P205 in the 50 c.c. of urine used. To express the result in percentage of P205 multiply the value just obtained by 2, e. g., if 50 c.c. of urine contained 0.074 gram of P205 it would be equiva- lent to 0.148 per cent. Calculate, in terms of P205, the total phosphate content of the twenty-four hour urine specimen. 2. Earthy Phosphates. — To 100 c.c. of urine in a beaker add an excess of ammonium hydroxide and allow the mixture to stand 12-24 hours. Under these conditions the phosphoric acid in com- bination with the alkaline earths, calcium and magnesium, is pre- cipitated as phosphates of these metals. Collect the precipitate on a filter paper and wash it with very dilute ammonium hydroxide. Pierce the paper, and remove the precipitate by means of hot water. Bring the phosphates into solution by adding a small amount of dilute acetic acid to the warm solution. Make the volume up to 50 c.c. with water, add 5 c.c. of sodium acetate solution and de- termine the P2Os content of the mixture according to the directions given under the previous method. Calculation. — Multiply the number of cubic centimeters of uran- ium acetate solution used by 0.005 to determine the number of grams of P205 in the 100 c.c. of urine used. Since 100 c.c. of urine was taken this value also expresses the percentage of P205 present. Calculate the quantity of earthy phosphates, in terms of P2Os, present in the twenty-four hour urine specimen. The quantity of phosphoric acid present in combination with the alkali metals may be determined by subtracting the content of earthy phosphates from the total phosphates. 3. Total Phosphorus. — Sodium Hydroxide and Potassium Nit- Inasmuch as 1 c.c. of the uranium solution should precipitate 0.005 gram of P2O5, exactly 20 c.c. of the uranium solution should be required to precipitate 50 c.c. of the standard phosphate solution. If the two solutions do not bear this relation to each other they may be brought into proper relation by diluting the uranium solution with distilled water or by increasing its strength. XA ten per cent solution of potassium ferrocyanide is satisfactory. urine: quantitative analysis. rate Fusion Method. — Place 25 i-.r. of urine in a large silver cru- cible and evaporate to a syrup on a water-bath. \<1<1 i<> gram- of NaOIl and 2 grains of KXO:, to the residue and fuse the mass until all organic matter has disappeared and the fused mixture is clear. Cool the mixture, transfer it to a casserole by means of hoi water, acidify the solution slightly with purr nitric acid and evapo- rate to dryness on a water-bath. Moisten the residue with a drops of dilute nitric acid, dissolve it in hoi water and transfer to a beaker. Now add an equal volume <>\ molyhdic solution1 and keep the mixture at 40 C. for twenty-four hours. Filter off the precipitate, wash it with dilute molyhdic solution and dissolve it in dilute ammonia. Add dilute hydrochloric acid to the solution, being careful to leave the solution distinctly ammoniacal. Magnesia mix- ture2 (10-15 c-c-) should now be added and after stirring thorough- ly and making strongly ammoniacal with concentrated ammonia the solution should be allowed to stand in a cool place for twenty- four hours. Filter off the precipitate, wash it free from chlorine by means of dilute ammonia (1:5), dry, incinerate and weigh, as magnesium pyrophosphate, Mg2P207, in the usual manner. In this method the phosphoric acid of the urine is precipitated as ammonium magnesium phosphate and in the process of incinera- tion this body is transformed into magnesium pyrophosphate. Calculation, — The quantity of phosphorus, expressed in terms of P2Os, in the volume of urine taken may be determined by means of the following proportion : Mol. wt. Wt. of Mol. wt. Mg2P207 : Mg2P207 : :P2C>5 : x (wt. of P2Ofi in grams), ppt. If y represents the weight of the Mg2P207 precipitate and we make the proper substitutions we have the following proportion: 221. 1 : y : : 140.9: x (wt. of P205, in grams, in the quantity of urine used.) To express the result in percentage of P20B simply divide the value of x, as just determined, by the quantity of urine used. 1 Directions for the preparation of the solution arc given on p. 57- 2 Directions for the preparation of magnesia mixture may be found on p 392 PHYSIOLOGICAL CHEMISTRY. i X. Creatinine. Folin's Colorimetric Method. — This method is based upon the characteristic property possessed alone by creatinine, of yielding a certain definite color-reaction in the presence of picric acid in alkaline solution. The procedure is as follows: Place 10 c.c. of urine in a 500 c.c. volumetric flask, add 15 c.c. of a saturated solu- tion of picric acid and 5 c.c. of a 10 per cent solution of sodium hydroxide, shake thoroughly and allow the mixture to stand for 5 minutes. During this interval pour a little § potassium bichro- mate solution1 into each of the two cylinders of the color- imeter (Duboscq's) and carefully adjust the depth of the solution in one of the cylinders to the 8 mm. mark. A few pre- liminary colorimetric readings may now be made with the solution in the other cylinder, in order to insure greater accuracy in the sub- sequent examination of the solution of unknown strength. Obvi- ously the two solutions of potassium bichromate are identical in color and in their examination no two readings should differ more than 0.1-0.2 mm. from the true value (8 mm.). Four or more readings should be made in each case and an average taken of all of them exclusive of the first reading, which is apt to be less ac- curate than the succeeding readings. In time as one becomes pro- ficient in the technique it is perfectly safe to take the average of the first huo readings. At the end of the 5-6 minute interval already mentioned, the con- tents of the 500 c.c. flask are diluted to the 500 c.c. mark, the bichro- mate solution is thoroughly rinsed out of one of the cylinders and replaced with the solution thus prepared and a number of colorimet- ric readings are immediately made. Ordinarily 10 c.c. of urine is used in the determination by this method but if the content of creatinine is above 15 mg. or below 5 mg. the determination should be repeated with a volume of urine selected according to the content of creatinine. This variation in the volume of urine according to the content of creatinine is quite essential, since the method loses in accuracy when more than 15 mg. or less than 5 mg. of creatinine is present in the solution of unknown strength. Calculation. — By experiment it has been determined that 10 mg. of pure creatinine, when brought into solution and diluted to 500 c.c. as explained in the above method, yields a mixture 8.1 mm. of which possesses the same colorimetric value as 8 mm. of a 1 This solution contains 24.55 grams of potassium bichromate to the liter. urine: quantitative analysis. 393 f solution of potassium bichromate*. ('.caring this in mind the com putation is readily ma.K- l»y means of the following proportion in which y represents the number of mm. of the solution of unknown strength equivalent to the 8 nun. of the potassium bichromate solu- tion : y.8.1:: io:.v (mgs. of creatinine in the quantity of urine used). This proportion may be used for the calculation no matter what volume of urine (5, 10 or 15 c.c. ) is used in the determination. The 10 represents 10 mg. of creatinine which gives a color equal to 8.1 mm., whether dissolved in 5, to or [5 c.c. of fluid. Calculate the quantity of creatinine in the twenty-four hour urine specimen. XI. Creatine. Folin-Benedict Method. — To about 20 c.c. of urine in a 50 c.c. volumetric flask, add 20 c.c. of normal hydrochloric acid and place the flask in an autoclave at a temperature of 117-1200 C. for one- half hour. Add distilled water until the volume of the acid- urine mixture is exactly 50 c.c, close the flask by means of a stopper, and shake it thoroughly. Approximately neutralize 25 c.c. of this mixture, introduce it into a 500 c.c. volumetric flask and deter- mine its creatinine content according to Folin's Method (see p. 31 12 1 . Calculation. — Calculate as explained on p. 392, and from this value substract the value for the original content of creatinine before hydrolysis. The difference between these two values will be the creatine content of the original urine in terms of creatinine. XII. Indican. Ellinger's Method.— This method for the quantitative determin- ation of indican is based upon the principle underlying Jaffe's test for the detection of indican (see p. 280). The method is as f< 'Hi iws : To 50 c.c. of urine1 in a small beaker or casserole add 5 c.c. of basic lead acetate solution, mix thoroughly and Alter. Transfer 40 c.c. of the filtrate to a separatory funnel, add an equal volume of Obermaver's reagent (see p. 281) and 20 c.c. of chloroform and extract in the usual manner. This extraction with chloroform should be repeated until the chloroform solution remains colorless. Now filter the combined chloroform extracts through a dry filter lIf the urine under examination is neutral or alkaline in reaction it should he made faintly acid with acetic acid before adding the basic lead acetate. 394 PHYSIOLOGICAL CHEMISTRY. paper into a dry Erlenmeyer flask. Distil off the chloroform, heat the residue on a boiling water-bath for 5 minutes in the open flask, and wash the dried residue with hot water.1 Add 10 c.c. of con- centrated sulphuric acid to the washed residue, heat on the water- bath for 5-10 minutes, dilute with 100 c.c. of water and titrate the blue solution with a very dilute solution of potassium permangan- ate.2 The end-point is indicated by the dissipation of all the blue color from the solution and the formation of a pale yellow color. Calculation. — Ellinger claims that one-sixth of the amount deter- mined must be added to the value obtained by titration in order to secure accurate data. This correction should always be made. XIII. Chlorides. 1. Clark's Modification of Dehn's Method.3 — In this method the organic compounds, that hold the chlorine too firmly for its quantitative precipitation with argentic nitrate, are destroyed by oxidation with sodium peroxide. Sodium peroxide in the pres- ence of water gives off nascent oxygen according to the following equation. Na202 + H20 =2NaOH + O The oxygen then attacks the organic matter and the chlorine is left as sodium chloride. The procedure is as follows : To 10 c.c. of urine in a 75-100 c.c. casserole, add 1. 0-1.2 gram of sodium peroxide and evaporate the mixture to dryness on a boiling water- bath. In case the residue is not pure white, thus indicating that in- sufficient sodium peroxide has been added, the residue should be moistened with distilled water, additional sodium peroxide added, and the mixture again evaporated to dryness. When the oxidation is complete, treat the mass with 10-20 c.c. of distilled water and stir until it has practically all been brought into solution. Then intro- duce a bit of litmus paper and add dilute nitric acid (1:1) until the litmus paper turns red and all effervescence ceases. Now place the 1 The washing should be continued until the wash water is no longer colored. Ordinarily two or three washings are sufficient. If a separation of indigo particles takes place during the washing process, the wash water should be filtered, the indigo extracted with chloroform and the usual method applied from this point. 2 A " stock solution " of potassium permanganate containing three grams per liter should be prepared, and when needed for titration purposes a suitable volume of this solution should be diluted with 40 volumes of water. The potassium permanganate solution should be standardized with pure indigo. 3 Private communication to the author from Mr. S. C. Clark. urine: QUANTITATIVE ANALYS] casserole on a hot plate or on a gauze and heal the contents almost to the boiling-point.3 To the hoi solution add a standard solution of argentic nitrate (see page 396) in slight excess.2 Filter off fi- ver chloride while the solution is still hot and wash the precipitate thoroughly with distilled water. To the lilt rate, add 1 <■..-. of a saturated solution of ferric ammonium sulphate and then titrate with a standard solution of ammonium thiocyanate 1 see page ,v;7) until the clear, slightly yellow fluid (or the opalescent, milky thud, in case there is much excess of argentic nitrate) change- to a slight red dish-brown color. The color of the end-point varies with the in- dividual. The exact end-point reached is not so important a- 1- t he- securing of the same end-point in a series of determinations as that obtained in the standardization of the standard solutions used. Calculation. — The standard solution of argentic nitrate should be made up so that I c.c. equals 0.010 gram of sodium chloride and 1 c.c. of the ammonium thiocyanate should he equivalent to 1 c.c. of the argentic nitrate solution (see pp. 396 and 397). Then, if the number of cubic centimeters of ammonium thiocyanate u-c<\ he sub- tracted from the number of cubic centimeters of argentic nitrate, the difference is the number of cubic centimeters of argentic nitrate actually used in the precipitation of chlorine as silver chloride. This number, multiplied by 0.010, gives the weight in grams of the sodium chloride in the 10 c.c. of urine used. If it is desired to express the result in percentage of sodium chloride, move the deci- mal point one place to the right. In a similar manner the weight or percentage of chlorine may be computed, using the factor 0.006 as explained in Mohr's method, page 396. Calculate the quantity of sodium chloride and of chlo- rine in the twenty-four hour urine specimen. 2. Mohr's Method. — To 10 c.c. of urine in a small platinum or porcelain crucible or dish add about 2 grams of chlorine-free potas- sium nitrate and evaporate to dryness at 100 ° C. (The evapora- tion may be conducted over a low flame provided care is taken to prevent loss by spurting.) By means of crucible tongs hold the crucible or dish over a free flame until all carbonaceous matter has disappeared and the fused mass is slightly yellow in color. Cool the residue somewhat and bring it into solution in a small amount 1 1 g xIf there is a slight precipitate, due to silicic acid from the casserole, this is filtered ofif and the filtrate collected in a 200 c.c. beaker. 2 This point is most easily recognized by keeping the solution h"t and in constant agitation while adding the argentic nitrate so that the silver chloride formed coagulates and sinks, leaving a clear, supernatant fluid. 396 PHYSIOLOGICAL CHEMISTRY. 25 c.c.) of distilled water acidified with about 10 drops of nitric acid. Transfer the solution to a small beaker, being sure to rinse out the crucible or dish very carefully. Test the reaction of the fluid, and if not already acid in reaction to litmus, render it slightly acid with nitric acid. Now neutralize the solution by the addition of calcium carbonate in substance,1 add 2-5 drops of neutral potas- sium chromate solution to the mixture and titrate with a standard argentic nitrate solution.2 This standard solution should be run in from a burette, stirring the liquid in the beaker after each addition. The end-reaction is reached when the yellow color of the solution changes to a slight orange-red. At this point take the burette reading and compute the percentage of chlorine and sodium chloride in the urine ex- amined. Calculation. — Since 1 c.c. of the standard argentic nitrate solu- tion is equivalent to 0.010 gram of sodium chloride, to obtain the weight, in grams, of the sodium chloride in the 10 c.c. of urine used multiply the number of cubic centimeters of standard solu- tion used by 0.0 10. If it is desired to express the result in per- centage of sodium chloride move the decimal point one place to the right. To obtain the zveight, in grams, of the chlorine in the 10 c.c. of urine used multiply the number of cubic centimeters of standard solution used by 0.006, and if it is desired to express the result in percentage of chlorine move the decimal point one place to the right. Calculate the quantity of sodium chloride and chlorine in the twenty- four hour urine specimen. 3. Volhard-Arnold Method. — Place 10 c.c. of urine in a 100 c.c. volumetric flask, add 20-30 drops of nitric acid (sp. gr. 1.2) and 2 c.c. of a cold saturated solution of ferric alum. If necessary, at this point a few drops of an 8 per cent solution of potassium permanganate may be added to dissipate the red color. Now slow- ly run in the standard argentic nitrate3 solution (20 c.c. is ordi- narily used) until all the chlorine has been precipitated and an excess 1 The cessation of effervescence and the presence of some undecomposed cal- cium carbonate at the bottom of the vessel are the indications of neutralization. 2 Standard argentic nitrate solution may be prepared by dissolving 29.060 grams of argentic nitrate in 1 liter of distilled water. Each cubic centimeter of this solution is equivalent to 0.010 gram of sodium chloride or to 0.006 gram of chlorine. 3 See note (2) at the bottom of page 384. urine: quantitative ANALYS] of the argentic nitrate solution is present, continually shaking the mixture during the addition of the standard solution. Allow the flask to -.land 10 minutes, thru fill n to the coo c.c. graduation with distilled water and thoroughly mix the contents. Now filter the mixture through a dry filter paper, colled 50 c.c. of the filtrate and titrate it with standardized ammonium thiocyanate solution.1 The first permanent tinge of brown indicates the end-point. Take the burette reading and compute the weight of sodium chloride in the 10 c.c. of urine used. Calculation. — The number of cubic centimeters of ammonium thiocyanate solution used indicates the excess of standard argentic nitrate solution in the 50 c.c. of filtrate titrated. Multiply this reading by 2, inasmuch as only one-half of the filtrate was employed, and subtract this product from the number of cubic centimeter- of argentic nitrate (20 c.c.) originally used, in order to obtain the actual number of cubic centimeters of argentic nitrate utilized in the precipitation of the chlorides in the 10 c.c. of urine employed. To obtain the weight in grams, of the sodium chloride in the 10 c.c. of urine used multiply the number of cubic centimeter- of the standard argentic nitrate solution, actually utilized in the pre- cipitation, by 0.010. If it is desired to express the result in per- centage of sodium chloride move the decimal point one place to the right. In a similar manner the weight, or percentage of chlorine may be computed using the factor 0.006 as explained in Mohr's method. page 396. Calculate the quantity of sodium chloride and chlorine in the twenty-four hour urine specimen. XIV. Acetone and Diacetic Acid. 1. Folin-Hart Method. — This method serves the same purpose as the Messinger-Huppert Method, /*. c, the determination of both 'This solution is made of such a strength that I c.c. of it is equal to i c.c. of the standard argentic nitrate solution used. To prepare the solution di« 12.9 grams of ammonium thiocyanate, NHiSCN, in a little less than a liter of water. In a small flask place 20 c.c. of the standard argentic nitrate solution. 5 c.c. of the ferric alum solution and 4 c.c. of nitric acid (sp. gr. r.2), add water to make the total volume 100 c.c. and thoroughly mix the contents of the flask. Now run in the ammonium thiocyanate solution from a burette until a permanent brown tinge is produced. This is the end-reaction and indicates that the last trace of argentic nitrate has been precipitated. Take the burette reading and calculate the amount of water necessary to use in diluting the ammonium thiocyanate in order that 10 c.c. of this solution may be exactly equal to 10 c.c. of the argentic nitrate solution. Make this dilution and titrate again to be certain that the solution is of the proper strength. 39<3 PHYSIOLOGICAL CHEMISTRY. acetone and diacetic acid in terms of acetone. It is, however, much simpler and less time consuming. The method includes the transformation of the diacetic acid into acetone and carbon dioxide by means of heat and the subsequent removal of the acetone thus formed as well as the preformed acetone by means of an air current as first suggested by Folin (see p. 400). The procedure is as fol- lows : Introduce into a wide-mouthed bottle 200 c.c. of water, an accurately measured excess of j-q iodine solution1 and an excess of 40 per cent potassium hydroxide. Prepare an aerometer cylinder containing alkaline hypoiodite solution to absorb any acetone which may be present in the air of the laboratory and between the cylinder and bottle suspend a test-tube about two inches in diameter. This large test-tube should contain 20 c.c. of the urine under examina- tion, 10 drops of a ten per cent solution of phosphoric acid, 10 grams of sodium chloride, and a little petroleum, and should be raised sufficiently high to facilitate the easy application of heat to its bottom portion. The connections on the side of the tube should be provided with bulb tubes containing cotton. When the appa- ratus is arranged as described, it should be connected with a Chap- man pump and an air current passed through for twenty-five min- utes. During this period the contents of the test-tube are heated just to the boiling-point and after an interval of five minutes again heated in the same manner. By this means the diacetic acid is con- verted into acetone and at the end of the twenty-five minute period this acetone, as well as the preformed acetone, will have been re- 1 Proceed as follows in order to obtain a rough idea regarding the amount of ~ iodine solution to be used : Introduce into a test-tube 10 c.c. of the urine under examination and 1 c.c. of a solution of ferric chloride made by dissolving 100 grams of ferric chloride in 100 c.c. of distilled water. After permitting the mixture to stand for two minutes, compare the color with that of an equal volume of the ferric chloride solution in a test-tube of similar diameter. If the two solutions be of approximately the same color intensity, 20 c.c. of the urine under examination will yield sufficient acetone to require nearly 10 c.c. of -^j iodine solution. In case the mixture is darker in color than is the ferric chloride solution, the former should be diluted with distilled water until it is of approximately the same intensity as the ferric chloride solution. From this data the amount of -^ iodine solution required may be roughly estimated by means of the following table : Urine c.c. Ferric Chloride. Water. ^ Iodine Required c.c. IO IO IO IO I I I I IO 20 30 IO 20 35 5o urine: quantitative analysis. moved from the urine to the absorption bottle and there retained as iodoform. The contents of the absorption bottle should now be acidified with concentrated hydrochloric acid,] and titrated with ,N,, sodium thio- sulphate and starch as in the Messinger Hupperl method below). 2. Messinger-Huppert Method.2 — Place [00 c.c. of urine in a distillation flask and add j c.c. of 50 per cenl acetic acid. ' !onned the flask with a condenser, properly arrange a receiver, attach a terminal series of bulbs containing water and distil over aboul nine tenths of the urine mixture. Remove the receiver, attach another and subject the residual portion of the mixture to a second distil- lation. Test this fluid for acetone and if the presence of acetone is indicated add about ioo c.c. of water to the residue and again distil. Treat the united acetone distillates with i c.c. of dilute I i _' per cent) sulphuric acid and redistil, collecting this second distillate in a glass-stoppered flask. During distillation, however, the glass stopper is replaced by a cork with a double perforation, the glass tube from one perforation passing to the condenser, while the bulbs containing water, before mentioned, are attached by means of the tube in the other perforation. Allow the distillation process to pro- ceed until practically all of the fluid has passed over, then remove the receiving flask and insert the glass stopper. Now treat the dis- tillate carefully with 10 c.c. of a y$ solution of iodine and add sodium hydroxide solution, drop by drop, until the blue color is dis- sipated and the iodoform precipitates. Stopper the flask and shake it for about one minute, acidify the solution with concentrated hydrochloric acid, and note the production of a brown color if an excess of iodine is present. In case there is no such excess, the solution should be treated with tNq iodine solution until an excess is obtained. Retitrate this excess of iodine with ,N,, sodium thio- sulphate solution until a light yellow color is observed. At this point a few cubic centimeters of starch paste should he added and the mixture again titrated until no blue color is visible. This is the end-reaction. Calculation. — Subtract the number of cubic centimeters of ,N„ thiosulphate solution used from the volume of ,x,, iodine solution employed. Since i c.c. of the iodine solution is equivalent to 1 An excess of iodine is indicated by the development of a brown color 'This method serves to determine both acetone and diacetic acid in terms of acetone. 400 -PHYSIOLOGICAL CHEMISTRY. 0.967 milligram of acetone, and since 1 c.c. of the thiosulphate solution is equivalent to 1 c.c. of the iodine solution, if we multiply the remainder from the above subtraction by 0.967 we will obtain the number of milligrams of acetone in the 100 c.c. of urine examined. Calculate the quantity of acetone in the twenty- four hour urine specimen. XV. Acetone. 1. Folin's Method. — The same type of apparatus is used in this method as that described in Folin's method for the determination of ammonia (see p. 380). The procedure is as follows: Introduce 20—25 c.c. of the urine under examination into the aerometer cylinder and add 10 drops of 10 per cent phosphoric acid,1 8-10 grams of sodium chloride,2 and a little petroleum. Introduce into an absorp- tion flask,3 such as is used in the ammonia determination (see p. 380), 150 c.c. of water, 10 c.c. of a 40 per cent solution of potassium hydroxide, and an excess of a T\ iodine solution. Connect the flask with the aerometer cylinder, attach a Chapman pump and permit an air current, slightly less rapid than that used for the determination of ammonia, to be drawn through the solution for 20-25 minutes. All of the acetone will, at this point, have been converted into iodo- form in the absorption flask. Add 10 c.c. of concentrated hydro- chloric acid (a volume equivalent to that of the strong alkali orig- inally added), to the contents of the latter and titrate the excess of iodine by means of ^ sodium thiosulphate solution and starch, as in the Messinger-Huppert method (see' p. 399). Folin has further made suggestions regarding the simultaneous determination of acetone and ammonia by the use of the same air current.4 This is an important consideration for the clinician inas- much as urines which contain acetone and diacetic acid are gener- ally those from which the ammonia data are also desired. The pro- cedure for the combination method is as follows : Arrange the ammonia apparatus as usual (see p. 380), and to the aerometer of the ammonia apparatus attach the acetone apparatus set up as de- scribed above. Regulate the air current with special reference to 1 Oxalic acid (0.2-0.3 gram) may be substituted if desired. 2 Acetone is insoluble in a saturated solution of sodium chloride. 3 Folin's improved absorption tube (see Fig. 123, p. 381) should be used in this connection inasmuch as the original type embracing the use of a rubber stopper is unsatisfactory because of the solvent action of alkaline hypoiodite on rubber. 4 These determinations may even be made on the same sample of urine if the sample is too small for the double determination. urine: quantitative analysis. 401 the determination of acetone and at the cud of -'<) 25 minutes dis- connect the acetone apparatus and complete the determination of the acetone as just described. The air current is not interrupted and after having run one and one dial f hours the ammi >nia apparatus is detached and the ammonia determination completed as described on page 380. If data regarding- diacetic acid are desired, the result obtained by Folin's method may be subtracted from the result obtained by the Messinger-Huppert method (see p. 399), inasmuch as the latter method determines both acetone and diacetic acid. Under all con- ditions the determination of acetone should he as expedition- as possible. This is essential, not only because of the fact that any diacetic acid present in the urine will become transformed into acetone but also because of the rapid spontaneous decomposition of the alkaline hypoiodite solution used in the determination of the acetone. It has been claimed that alkaline hypoiodite solutions are almost completely converted into iodate solutions in one-half hour. Folin states, however, that the transformation is not so rapid as this, but he nevertheless emphasizes the necessity of rapidity of manipulation. At the same time it should be remembered that the air current must not be as rapid as for ammonia, inasmuch as the alkaline hypoiodite solution will not absorb all the acetone under those conditions. XVI. Diacetic Acid. 1. Folin-Hart Method. — Arrange the apparatus as described under the Folin-Hart method for the determination of acetone and diacetic acid (see p. 397). Start the air current in the usual way and permit it to run 25 minutes without the application of heat to the urine under examination. Under these conditions the preformed acetone present in the solution is all removed (see p. 398). Immediately attach a freshly prepared absorption bottle or introduce fresh alkaline hypoiodite solution into the original bottle. Apply heat to the large test-tube as already described (see p. 398 >. in order to convert the diacetic acid into acetone, permit the air current to continue for the usual 2^ minute period, and determine the diacetic acid value in terms of acetone by the usual titration procedure (seep. 399). 2. Folin-Messinger-Huppert Method. — Determine the com- bined acetone and diacetic acid, in terms >>( acetone, by the Mes- singer-Huppert method (see p. 390^ and subsequently determine the 27 402 PHYSIOLOGICAL CHEMISTRY. acetone by Folin's method (see p. 400). Subtract the value deter- mined by the second method from that obtained in the first method to secure data regarding the diacetic acid content of the urine, in terms of acetone. XVII. /?-Oxybutyric Acid. 1. Shaffer's Method. — Introduce 25-250 c.c. of urine1 into a 500 c.c. volumetric flask and add an excess of basic lead acetate and 10 c.c. of concentrated ammonium hydroxide. Dilute the mixture to the 500 c.c. mark, shake the flask thoroughly and filter. Transfer 200 c.c. of the filtrate to an 800 c.c. Kjeldahl distilling flask, add 300-400 c.c. of water, 15 c.c. of concentrated sulphuric acid and a little talcum and distil the mixture until 200 to 250 c.c. of distillate has been collected (A).2 To this distillate (A), which contains acetone (both preformed and that produced from diacetic acid), and volatile fatty acids is added 5 c.c. of 10 per cent potassium hydroxide and the distillate redistilled in order to remove the vola- tile fatty acids.3 This second distillate (A2) is then titrated with standard iodine and thiosulphate (see p. 399). The urine-sulphuric acid residue from which distillate A was obtained, is again distilled, 400-600 c.c. of a 0.1-0.5 per cent potassium bichromate solution being added, by means of the dropping tube, during the process of distillation.4 In adding the bichromate, care should be taken not to add it faster than the distillate collects except in cases where the boiling fluid assumes a pure green color, thus indicating that the bichromate is being used up more rapidly. After about 500 c.c. of distillate (B) has collected 20 c.c. of a 3 per cent solution of hydrogen peroxide and a few cubic centimeters of potassium 1 The amount used depends upon the expected yield of /3-oxybutyric acid. In the case of urines which give a strong ferric chloride reaction for diacetic acid, or when 5-10 grams or more of /3-oxybutyric acid is expected, it is unnecessary to use more than 25-50 c.c. of urine. However, in case only a trace of /3-oxybutyric acid is expected, the volume should be much larger as indicated. Under all conditions, the amount specified is sufficient for duplicate determina- tions. It is desirable to use such a volume of urine as -contains the proper amount of /3-oxybutyric acid to yield 25-50 milligrams of acetone. 2 This distilling flask should be provided with a dropping tube, by means of which water may be introduced in order to prevent the contents of the flask from becoming less than 400 c.c. in volume. Care should be taken to use a good condenser in the distillation, but it is not necessary to cool the distillate with ice. 3 Formic acid is one of the most troublesome. 4 Generally the addition Of 0.5 gram of potassium bichromate is sufficient. In case the urine contains a high concentration of sugar or when a large volume of urine is used, it may be necessary to use 2-3 grams of the bichromate. urine: quantitative analysi 403 hydroxide solution are added and the mixture (B) subjected to redistillation. Distil off about 300 c.c. and titrate this distillate (B2) as usual with iodine and thiosulphate (see p. 39 Calculation. — The author advises the use of solutions of thio- sulphate and iodine which are a trifle stronger than ,s,,, 1. .-., [03 Each cubic centimeter of an iodine solution of this strength is equivalent to one milligram of acetone or to 1704 milligram of j8-oxybutyric acid. The thiosulphate solution 1- accepted as the standard and should he restandardi/.ed. Erom time to time, by a ~ solution of potassium hi-iodate. 2. Black's Method. — Render 50 c.c. of the urine under examina- tion, faintly alkaline with sodium carbonate and evaporate to one- third the original volume. Concentrate to about 10 c.c. on a water- bath, cool the residue, acidify it with a few drops of concentrated hydrochloric acid1 and add plaster of Paris to form a thick paste. Permit the mixture to stand until it begins to " set," then break it up with a stout glass rod having a blunt end and reduce the material to the consistency of a fairly dry coarse meal.- Transfer the meal to a Soxhlet apparatus and extract with ether for two hours. At the end of this period evaporate the ether-extract either spontaneously or in an air current. Dissolve the residue in water, add a little bone black, if necessary, filter until a clear solution is obtained and make up the filtrate to a known volume (25 c.c. or less) with water. The /?-oxybutyric acid should then he determined by means of the polariscope. 3. Darmstadter's Method. — This method is based on the fact that crotonic acid is formed from /?-oxybutvric acid under the influence of concentrated mineral acids. The method is as follows: Render 100 c.c. of urine slightly alkaline with sodium carbonate and evaporate nearly to dryness on a water-hath. Dissolve the resi- due in 150-200 c.c. of 50-55 per cent sulphuric acid, transfer the acid solution to a one liter distillation flask and connect it with a condenser. Through the cork of the flask introduce the stem of a dropping funnel containing water. Heat the flask gently until foaming ceases, then use a full flame and distil over about 300 35" c.c. of fluid, keeping the volume <>f liquid in the distillation flask constant by the addition of water from the dropping funnel as the distillate collects. Ordinarily it will take about 2 2] 2 hours to col- 1 The residue should give a distinct red color with litmus paper. "Before this is accomplished it may, in some cases, be accessary to add a little more plaster (if Paris. 404 PHYSIOLOGICAL CHEMISTRY. lect this amount of distillate. Extract the distillate three times1 with ether in a separatory funnel, evaporate the ether and heat the residue at 1600 C. for a few minutes to remove volatile fatty acids. Dissolve the residue in 50 c.c. of water, filter and titrate this aqueous solution of crotonic acid with f-Q sodium hydroxide solution, using phenolphthalein as indicator. Calculation. — One c.c. of y\ sodium hydroxide solution equals 0.0086 gram of crotonic acid, 1 part of crotonic acid equals 1.21 part of /?-oxybutyric acid, and 1 c.c. of j-q sodium hydroxide solu- tion equals 0.0 1 041 gram of /?-oxybutyric acid. To compute the quantity of /?-oxybutyric acid, in grams, multiply the number of cubic centimeters of jq sodium hydroxide solution used by 0.01041. 4. Bergell's Method. — Render 100-300 c.c. of sugar-free2 urine slightly alkaline with sodium carbonate, evaporate the alkaline urine to a syrup on a water-bath, cool the syrup, rub it up with syrupy phosphoric acid (being careful to keep the mixture cool), 20-30 grams of finely pulverized, anhydrous cupric sulphate and 20-25 grams of fine sand. Mix the mass thoroughly, place it in a paper extraction thimble3 and extract the dry mixture with ether in a Soxhlet apparatus (Fig. 125, page 410). Evaporate the ether, dis- solve the residue in about 25 c.c. of water, decolorize the fluid with animal charcoal, , if necessary, and determine the content of /?-oxy- butyric acid by a polarization test. 5. Boekelman and Bouma's Method. — Place 25 c.c. of urine in a flask, add 25 c.c. of 12 per cent sodium hydroxide and 25 c.c. of benzoyl chloride, stopper the flask and shake it vigorously for three minutes under cold water. Remove the clear fluid by means of a pipette, filter it and subject it to a polarization test. Through the action of the benzoyl chloride all the lsevo-rotatory substances ex- cept /?-oxybutyric acid will have been' removed and the laevo-rotation now exhibited by the urine will be due entirely to that acid. XVIII. Acidity. Folin's Method. — The total acidity of urine may be determined as follows : Place 25 c.c. of urine in a 200 c.c. Erlenmeyer flask and add 15-20 grams of finely pulverized potassium oxalate and 1-2 drops of a 1 per cent phenolphthalein solution to the fluid. 1 Shaffer has recently called attention to the fact that it is extremely difficult to extract all of the crotonic acid if but three extractions are made. 2 If sugar is present it must be removed by fermentation. 3 The Schleicher and Schiill fat-free extraction thimble is very satisfactory. urine: quantitative analysis. Shake the mixture vigorously for i 2 minutes and titrate if im- mediately with nr sodium hydroxide until a faint bul unmistakable pink remains permanent on further shaking. Take the lunette reading- and calculate the acidity of the urine under examination. Calculation. — If y represents the number of cubic centimetei Yij sodium hydroxide used and y' represents the volume of urine excreted in twenty- four hours, the total acidity of the twenty-four hour urine specimen may be calculated by means of the following nroportion : 25:3- ::y'\x (acidity of 24-hour urine expressed in cubic centimeters of is sodium hydroxide). Each cubic centimeter of f^ sodium hydroxide contains 0.004 gram of sodium hydroxide and this is equivalent to 0.0063 grani "' oxalic acid. Therefore, in order to express the total acidity of the twenty-four hour urine specimen in equivalent grams of sodium hydroxide, multiply the value of x, as just determined, by 0.004, or multiply the value of x by 0.0063 if it is desired to express the total acidity in grams of oxalic acid. XIX. Purine Bases. 1. Kriiger and Schmidt's Method. — This method serves for the determination of both uric acid and the purine bases. The principle involved is the precipitation of both the uric acid and the purine bases in combination with copper oxide and the subsequent decom- position of this precipitate by means of sodium sulphide. The uric acid is then precipitated by means of hydrochloric acid and the purine bases are separated from the filtrate in the form of their copper or silver compounds. The nitrogen content of the precipi- tates of uric acid and purine bases is then determined by means of the Kjeldahl method (see p. 381) and the corresponding values for uric acid and purine bases calculated. The method is a- follows: To 400 c.c. of albumin-free urine1 in a liter flask,2 add 24 grams of sodium acetate, 40 c.c. of a solution of sodium bisulphite8 and heat the mixture to boiling. Add 40-80 c.c.4 of a 10 per cent solu- *If albumin is present, the urine should be heated to boiling, acidified with acetic acid and filtered. -The total volume of urine for the twenty-four hours should Ik- sufficiently diluted with water to make the total volume of the solution 1600-2000 c.c. 3 A solution containing 50 grams of Kahlbaum's commercial sodium bisulphite in 100 c.c. of water. * The exact amount depending upon the contenl "t" the purine bases 406 PHYSIOLOGICAL CHEMISTRY. tion of cupric sulphate and maintain the temperature of the mix- ture at the boiling-point for at least three minutes. Filter off the flocculent precipitate, wash it with hot water until the wash water is colorless, and return the washed precipitate to the flask by punc- turing the tip of the filter paper and washing the precipitate through by means of hot water. Add water until the volume in the flask is approximately 200 c.c., heat the mixture to boiling and decom- pose the precipitate of copper oxide by the addition of 30 c.c. of sodium sulphide solution.1 After decomposition is complete, the mixture should be acidified with acetic acid and heated to boiling until the separating sulphur collects in a mass. Filter the hot fluid by means of a filter-pump, wash with hot water, add 10 c.c. of 10 per cent hydrochloric acid and evaporate the filtrate in a porcelain dish until the total volume has been reduced to about ten cubic centi- meters. Permit this residue to stand about two hours to allow for the separation of the uric acid, leaving the purine bases in solu- tion. Filter off the precipitate of uric acid, using a small filter paper, and wash the uric acid, with water made acid with sulphuric acid, until the total volume of the original filtrate and the wash water aggregates 75 c.c. Determine the nitrogen content of the pre- cipitate by means of the Kjeldahl method (see p. 381), and calcu- late the uric acid equivalent.2 Render the filtrate from the uric acid crystals alkaline with sodium hydroxide, add acetic acid until faintly acid and heat to 700 C. Now add one cubic centimeter of a 10 per cent solution of acetic acid and 10 c.c. of a suspension of manganese dioxide3 to oxidize the traces of uric acid which remain in the solution. Agitate the mixture for one minute, add 10 c.c. of the sodium bisul- phite solution4 and 5 c.c. of a 10 per cent solution of cupric sulphate and heat the mixture to boiling for three minutes. Filter off the 1 This is made by saturating a one per cent solution* of sodium hydroxide with hydrogen sulphide gas and adding an equal volume of one per cent sodium hydroxide. Ordinarily the addition of 30 c.c. of this solution is sufficient, but the presence of an excess of sulphide should be proven by adding a drop of lead acetate to a drop of the solution. Under these conditions a dark brown color will show the presence of an excess of sodium sulphide. 2 This may be done by multiplying the nitrogen value by three and adding three and one-half milligrams to the product as a correction for the uric acid remaining in solution in the 75 c.c. 3 Made by heating a 0.5 per cent solution of potassium permanganate with a little alcohol until it is decolorized. * To dissolve the excess of manganese dioxide. urine: quantitative analysi precipitate wash it with hot water and determine its nitrogen con tent by means of the Kjeldah! method I see p. 381 >. [nasmuch as the composition and proportion of the purine bases presenl in urine is variable, no factor can be applied. The result as regards these bases must therefore be expressed in terms of nitrogen. 2. Salkowski's Method. — Place 400 600 c.c. of protein urine in a beaker, [ntroduce into another beaker 30 50 1 ,c. of an ammoniacal silver solution1 with 30 50 c.c. of magnesia mixture,2 add some ammonium hydroxide and if necessary some ammonium chloride to clear the solution. Nov add this solution to the urine, stirring continually with a glass rod. and allow the mixture to stand for one-half hour. Collect the precipitate on a filter paper, wash it with dilute ammonium hydroxide and finally wash it back into the original beaker. Suspend the precipitate in 600 800 C.C. of water, add a few drops of hydrochloric acid and decompose it by means of hydrogen sulphide. Now heat the solution to boiling, bi- ter while hot and evaporate the filtrate to dryness on a water-bath. Extract the residue with 20-30 c.c. of hot 3 per cent sulphuric acid and allow the extract to stand twenty- four hours. Filter off the uric acid, wash it. make the filtrate ammoniacal and precipitate the purine bases again with silver nitrate. Collect this precipitate on a small-sized chlorine-free filter paper, wash, dry .and incinerate it in the usual manner. Xow dissolve the ash in nitric acid and titrate with ammonium thiocyanate according to the Volhard- Arnold method (see p. 396). Calculate the content of purine bases in the urine examined, bearing in mind that in an equal mixture of the silver salts of the purine bases, such as we have here, one part of silver corresponds to 0.277 gram of nitrogen or to 0.738] gram of the bases. XX. Allantoin. Paduschka-Underhill-Kleiner Method. — To 50-100 c.c. of urine in a beaker add basic lead acetate until no more precipitate forms. Filter and pass hydrogen sulphide gas through an aliquol portion of the filtrate to remove the excess of lead.3 Filter again, drive off the hydrogen sulphide by heat and treat an aliquot por- 1 Prepared by dissolving 26 gram- of silver nitrate in aboul 500 C.C. of water, adding enough ammonium hydroxide to redissolve the precipitate which forms upon the first addition of the ammonia and making the balance of the mixture up to 1 liter with water. "Directions for preparation may be found on page 295. 'In the original method of Paduschka sodium sulphate is used for tins purpose. 408 PHYSIOLOGICAL CHEMISTRY. tion of the filtrate with a 10 per cent solution of silver nitrate until precipitation is complete.1 Filter off this precipitate, wash it with water and determine its nitrogen content by means of the Kjeldahl method (see p. 381). This is the "purine nitrogen." Render an aliquot portion of the filtrate faintly alkaline,2 with a one per cent solution of ammonium hydroxide and add 50—100 c.c. of a 10 per cent solution of silver nitrate. If allantoin be present a white, floc- culent precipitate will form and gradually sink to the bottom of the solution. Filter, wash the precipitate free from ammonium hydrox- ide by means of a one per cent solution of sodium sulphate and determine its nitrogen content by the Kjeldahl method (see p. 381). XXI. Oxalic Acid. Salkowski-Autenrieth and Barth Method. — Place the twenty- four hour urine specimen in a precipitating jar, add an excess of calcium chloride, render the urine strongly ammoniacal, stir it well and allow it to stand 18-20 hours. Filter off the precipitate, wash it with a small amount of water and dissolve it in about 30 c.c. of a hot 15 per cent solution of hydrochloric acid. By means of a separatory funnel extract the solution with 150 c.c. of ether which contains 3 per cent of alcohol, repeating the extraction four or five times with fresh portions of ether. Unite the ethereal extracts, allow them to stand for an hour in a flask and then filter through a dry filter paper. Add 5 c.c. of water to the filtrate, to prevent the formation of diethyl oxalate when the solution is heated, and distil off the ether. If necessary, decolorize the liquid with animal charcoal and filter. Concentrate the filtrate to 3-5 c.c, add a little calcium chloride solution, make it ammoniacal and after a few min- utes render it slightly acid with acetic acid. Allow the acidified solution to stand several hours, collect the precipitate of calcium oxalate on a washed filter paper,3 wash, incinerate strongly (to CaO) and weigh in the usual manner. Calculation. — Since 56 parts of CaO are equivalent to 90 parts of oxalic acid, the quantity of oxalic acid in the volume of urine taken may be determined by multiplying the weight of CaO by the factor 1. 607 1. XXII. Total Solids. 1. Drying Method. — Place 5 c.c. of urine in a weighed shallow dish, acidify very slightly with acetic acid (1-3 drops) and dry it 1 Ordinarily from 20-30 c.c. is required. 2 Using litmus as the indicator. 3 Schleicher and Schull, No. 589, is satisfactory. urine: quantitative analysis. 409 in vacuo in the presence of sulphuric acid, to constant weight. Calculate the percentage of solids in the mine sample and the total solids for the twenty-four hour period. Practically all the methods the technique of which includes • poration at an increased temperature, either under atmospheric conditions or in vacuo are attended with error. 2. Calculation by Long's Coefficient. — The quantity of solid material contained in the urine excreted for any twenty-four hour period may be approximately computed by multiplying the second and third decimal figures of the specific gravity by 2.6. This gives us the number of grams of solid matter in one liter of urine Fr< >m this value the total solids for the twenty-four hour period may easily be determined. Calculation. — If the volume of urine for the twenty- four hours was 1 120 c.c. and the specific gravity I.018, the calculation would be as follows : (a) 18 X 2.6 = 46.8 grams of solid matter in 1 liter of urine. (0\ ij — iS =52.4 grams of solid matter in 1120 c.c. of 1000 urine. Long's coefficient was determined for urine whose specific grav- ity was taken at 25 ° C. and is probably more accurate, for con- ditions obtaining in America, than the older coefficient of Haeser, 2-33- CHAPTER XXIII, Fig. 125. QUANTITATIVE ANALYSIS OF MILK, GASTRIC JUICE AND BLOOD. (a) Quantitative Analysis of Milk. 1. Specific Gravity. — This may be determined conveniently by means of a Soxhlet, Veith or Ouevenne lactometer. A lactometer reading- of 320 denotes a specific gravity of 1.032. The determin- ation should be made at about 6o° F. and the lactometer reading corrected by adding or subtracting o.i° for every degree F. above or below that temperature. 2. Fat. — (a) Adams' Paper Coil Method.— Introduce about 5 c.c. of milk into a small beaker, quickly ascer- tain the weight to centigrams, stand a fat-free coil1 in the beaker and incline the vessel and rotate the coil in order to hasten the absorption of the milk. Immediately upon the complete absorp- tion of the milk remove the coil and again quickly ascertain the weight of the beaker. The difference in the weights of the beaker at the two weighings represents the quantity of milk absorbed by the coil. Dry the coil carefully at a temperature below ioo° C. and extract it with ether for 3-5 hours in a Soxhlet apparatus (Fig. 125, p. 410), using a safety water-bath, heat the flask containing the fat to constant weight at a tem- perature below ioo° C. Calculation. — Divide the weight of fat, in grams, by the weight of milk, in grams. The quotient is the percentage of fat contained in the milk examined. 1 Very satisfactory coils are manufactured by Schleicher and Schiill. 410 Soxhlet Apparatus. QUANTITATIVE ANALYSIS "I MILK. 4!I fK Fes i Lactosi OP1 . (b) Approximate Determination by l:eser's LactOSCOpe. Milk is opaque mainly because of the suspended fal globules and there- fore by means of the estimation oi this opacitj we may obtain data as to the approximate content of Fat. Feser's lacto- scope (Fig. 126, p. 41 1 ) may be used for this purpose. Proceed as follows: By means of the graduated pip- ette accompanying the instrument introduce 4 c.e. of milk into the lactoscope. Add water gradually, shaking after each addition, and note the point ai which the black lines upon the inner white glass cylin- der are distinctly visible. Observe the point on the graduated scale of the lactoscope which is level with the surface of the diluted milk. This reading repre- sents the percentage of fal present in the undiluted milk. Pure milk should contain at least 3 per cent of fat. 3. Total Solids.1 — Introduce 2-5 grams of milk into a weighed flat-bottomed platinum dish- and quickly ascertain the weight to milligrams. Expel the major portion of the water by heating the open dish on a water-bath and continue the heating in an air-bath or water oven at qj^-ioo0 C. until the weight is constant. (If platinum dishes are employed this residue may be used in the determination of ash according to the method described below.) Calculation. — Divide the weight of the residue, in grams, by the weight of milk used, in grams. The quotient is the percental solids contained in the milk examined. 4. Ash. — Heat the dry solids from 2-$ grams of milk, obtained according to the method just given, over a very low flame8 until a white or light gray ash is obtained. Cool the dish in a desiccator and weigh. (This ash may be used in testing for preservative- ac- cording to directions on page 226.) 1 The percentage of total solids may be calculated from the specific gravity and percentage of fat by means of the following formula winch has been pro by Richmond : S = 0.25 L + 1.2 F + o. 14 S = total solids. L = lactometer reading. F = fat content. 'Lead foil dishes, costing only aboul one dollar per gross, make a very satisfactory substitute for the platinum dishes. 3 Great care should be used in this ignition, the dish ai no time being heated above a faint redness, as chlorides may volatilize. 412 PHYSIOLOGICAL CHEMISTRY. 5. Proteins. — Introduce a known weight of milk (5-10 grams) into a 500 c.c. Kjeldahl digestion flask and add 20 c.c. of con- centrated sulphuric acid and about 0.2 gram of cupric sulphate. Expel the major portion of the water by heating over a low flame and finally use a full flame and allow the mixture to boil 1-2 hours. Complete the determination according to the directions given under Kjeldahl Method, page 381. Calculation — Multiply the total nitrogen content by the factor 6.371 to obtain the protein content of the milk examined. 6. Caseinogen. — Mix about 20 grams of milk with 40 c.c. of a saturated solution of magnesium sulphate and add the salt in sub- stance until no more will dissolve. The precipitate consists of caseinogen admixed with a little fat and lacto-globulin. Filter off the precipitate, wash it thoroughly with a saturated solution of magnesium sulphate,2 transfer the filter paper and precipitate to a Kjeldahl digestion flask and determine the nitrogen content ac- cording to the directions given in the previous experiment. Calculation. — Multiply the total nitrogen by the factor 6.37 to obtain the casein content. 7. Lactalbumin. — To the filtrate and washings from the deter- mination of caseinogen, as just explained, add Almen's reagent3 until no more precipitate forms. Filter off the precipitate and determine the nitrogen content according to the directions given under Proteins, above. Calculation. — Multiply the total nitrogen by the factor 6.37 to ob- tain the lactalbumin content. 8. Lactose. — To about 350 c.c. of water in a beaker add 20 grams of milk, mix thoroughly, acidify the fluid with about 2 c.c. of 10 per cent acetic acid and stir the acidified mixture continuously until a flocculent precipitate forms. At this point the reaction should be distinctly acid to litmus. Heat the solution to boiling for one-half hour, filter, rinse the beaker thoroughly and wash the precipitated proteins and the adherent fat with .hot water. Com- bine the filtrate and wash water and concentrate the mixture to about * 1 The usual factor employed for the calculation of protein from the nitrogen content is 6.25 and is based on the assumption that proteins contain on the average 16 per cent of nitrogen. This special factor of 6.37 is used here to calculate the protein content from the total nitrogen, since the principal protein constituents of milk, i. e., caseinogen and lactalbumin, contain 15.7 per cent of nitrogen. 2 Preserve the filtrate and washings for the determination of lactalbumin. 3 Almen's reagent may be prepared by dissolving 5 grams of tannin in 240 c.c. of 50 per cent alcohol and adding 10 c.c. of 25 per cent acetic acid. QUANTITATIVE ANALYSIS OF MILK. 413 150 c.c. Cool the solution and dilute it to 200 c.c. in a volumetric flask. Titrate this sugar solution according to directions - under Fehling's Method, page 367. Calculation. Make 1 1 u- calculation according to din given under Fehling's Method, p. 307, bearing in mind that to < Fehling's solution is completely reduced by O.06/6 gram of lactose. (b) Quantitative Analysis of Gastric Juice. Topfer's Method. This method is much less elaborate than many others but is suffi- ciently accurate for ordinary clinical purposes. The method em- braces the volumetric determination of (1) total acidity, | 2 1 com- bined acidity, and (3) free acidity, and the subsequent calculation of (4) acidity due to organic acids and acid salts, from the data thus obtained. Strain the gastric contents and introduce 10 c.c. of the strained material into each of three small beakers or porcelain dishes.1 Label the vessels A, B and C, respectively, and proceed with the analysis according to the directions given below. 1. Total Acidity.2 — Add 3 drops of a 1 per cent alcoholic solu- tion of phenolphthalein3 to the contents of vessel A and titrate with yg- sodium hydroxide solution until a dark pink color is produced which cannot be deepened by further addition of a drop of -fj sodium hydroxide. Take the burette reading and calculate the total acidity. Calculation. — The total acidity may be expressed in the following ways : 1. The number of cubic centimeters of yu sodium hydroxide solu- tion necessary to neutralize 100 c.c. of gastric juice. 2. The weight (in grams) of sodium hydroxide necessary to neutralize 100 c.c. of gastric juice. 3. The weight (in grams) of hydrochloric acid which the total acidity of 100 c.c. of gastric juice represents, i. c, percentage of hy- drochloric acid. The forms of expression most frequently employed are 1 and 3, preference being given to the former. 'If sufficient gastric juice is not available it may be diluted with water or a smaller amount, e. g., 5 c.c, taken for each determination. " This includes free and combined acid and acid salts. 3 One gram of phenolphthalein dissolved in ioo c.c. of 05 per cent alcohol. 4 14 PHYSIOLOGICAL CHEMISTRY. In making the calculation note the number of cubic centimeters of yq sodium hydroxide required to neutralize 10 c.c. of the gastric juice and multiply it by 10 to obtain the number of cubic centimeters necessary to neutralize 100 c.c. of the fluid. If it is desired to ex- press the acidity of ioo c.c. of gastric juice in terms of hydro- chloric acid, by weight, multiply the value just obtained by 0.00365.1 2. Combined Acidity.2 — Add 3 drops of sodium alizarin sul- phonate solution3 to the contents of vessel B and titrate with •^ sodium hydroxide solution until a violet color is produced. In this titration the red color, which appears after the tinge of yellow due to the addition of the indicator has disappeared, must be en- tirely replaced by a distinct violet color. Take the burette reading and calculate the combined acidity. Calculation. — Since the indicator used reacts to all acidities except combined "acidity in order to determine the number of cubic centi- meters of -yq sodium hydroxide necessary to neutralize the combined acidity of 10 c.c. of the gastric juice, we must subtract the burette reading just obtained from the burette reading obtained in the de- termination of the total acidity. The data for 100 c.c. of g"astric juice may be calculated according to the directions given under Total Acidity, page 413. 3. Free Acidity.4 — Add 4 drops of di-methyl-amino-azobenzene (Topfer's reagent) solution5 to the contents of the vessel C and titrate with -3^ sodium hydroxide solution until the initial red color is replaced by lemon yellow.® Take the burette reading and calcu- late the free acidity. Calculation. — The indicator used reacts only to free acid, hence the number of cubic centimeters of -^ sodium hydroxide used indi- cates the volume necessary to neutralize the free acidity of 10 c.c. of gastric juice. To determine the data for 100 c.c. of gastric juice proceed according to the directions given under Total Acidity, page 413. 4. Acidity due to Organic Acids and Acid Salts. — This value may be conveniently calculated by subtracting the number of cubic *One c.c. of ** hydrochloric acid contains 0.00365 gram of hydrochloric acid. 2 Hydrochloric acid combined with protein material. 3 One gram of sodium alizarin sulphonate dissolved in 100 c.c. of water. 4 Hydrochloric acid not combined with protein material. 5 One-half gram dissolved in 100 c.c. of 95 per cent alcohol. 6 If the lemon yellow color appears as soon as the indicator is added it denotes the absence of free acid. QUANTITATIVE ANALYSIS OF GASTRK M Ml. 415 centimeters of ,N() sodium hydroxide used in neutralizing the contents of vessel C from the number of cubic centimeters of ,s,, sodium hydroxide solution used in neutralizing the contents of vessel B. The remainder indicates the number of cubic centimeters of }s„ sodium hydroxide solution necessary to neutralize the acidity due to organic acids and acid salts present in [0 c.c. of gastric juice. The data for 100 c.c. of gastric juice may be calculated according to directions given under Total Acidity, page 413. (c) Quantitative Analysis of Blood. For the methods involved in the quantitative examination of blood see Chapter XII. APPENDIX. Almen's Reagent.1 — Dissolve 5 grams of tannin in 240 c.c. of 50 per cent alcohol and add 10 c.c. of 25 per cent acetic acid. Ammoniacal Silver Solution.2 — Dissolve 26 grams of silver nitrate in about 500 c.c. of water, add enough ammonium hydroxide to redissolve the precipitate which forms upon the first addition of the ammonium hydroxide and make the volume of the mixture up to 1 liter with water. Arnold-Lipliawsky Reagent.3 — This reagent consists of two definite solutions which are ordinarily preserved separately and mixed just before using. The two solutions are prepared as follows : (a) One per cent aqueous solution of potassium nitrite. (b) One gram of p-amino-acetophenon dissolved in 100 c.c. of distilled water and enough hydrochloric acid (about 2 c.c.) added drop by drop, to cause the solution, which is at first yellow, to become entirely colorless. An excess of acid must be avoided. Barfoed's Solution.4 — Dissolve 4.5 grams of neutral, crystal- lized cupric acetate in 100 c.c. of water and add 0.12 c.c. of 50 per cent acetic acid. Baryta Mixture.5 — A mixture consisting of one volume of a saturated solution of barium nitrate and two volumes of a saturated solution of barium hydroxide. Benedict's Solutions.6 — First Modification. — Benedict's modi- fied Fehling solution consists of two definite solutions — a cupric sulphate solution and an alkaline tartrate solution, which may be prepared as follows : Cupric sulphate solution = 34.65 grams of cupric sulphate dis- solved in water and made up to 500 c.c. Alkaline tartrate solution = 100 grams of anhydrous sodium car- 1 Ott's precipitation test, p. 321. Determination of lactalbumin, p. 412. 2 Salkowski's method, page 407. 3 Arnold-Lipliawsky reaction, page 331. 4 Barfoed's test, pages 31 and 313. 6 Isolation of urea from urine, page 269. 6 Benedict's modifications of Fehling' s test, pages 28 and 309, and Benedict's Method, page 368. 416 APPENDIX. ; i — bonate and 173 grams of Rochelle salt dissolved in water and made up to 500 c.c. These solutions should be preserved separately in rubber-stop- pered bottles and mixed in equal volumes when needed for use. This is done to prevent deterioration. Second Modification. — Very recently Benedicl has further modi- fied his solution and has succeeded in obtaining one which does not deteriorate upon long- standing. It has the following composition: Cupric sulphate 17.3 grams. Sodium citrate i~.VO grams. Sodium carbonate 100.0 Distilled water to make 1 liter. With the aid of heat dissolve the sodium citrate and carbonate in about 600 c.c. of water. Pour (through a folded filter paper if necessary) into a glass graduate and make up to 850 c.c. 1 dissolve the cupric sulphate in about 100 c.c. of water and make up to [50 c.c. Pour the carbonate-citrate solution into a large beakei casserole and add the cupric sulphate solution slowly, with constant stirring. The mixed solution is ready for use and does not dete- riorate upon long standing. Benedict's solution as used in the quantitative determination ol sugar consists of three separate solutions, the two mentioned under First Modification and in addition a potassium ferro-thioeyaiiale solution. This third solution contains 15 grams of potassium fer- rocyanide, 62.5 grams of potassium thiocyanate and 50 gram- . and water. Iodine Solution/' — Prepare a 2 per cent solution of potassium iodide and add sufficient iodine to color it a deep yellow. Jolles' Reagent.4 — This reagent has the following composition: Succinic acid 40 grams. Mercuric chloride 20 grains. Sodium chloride 20 grams. Distilled water 1000 gram-. Kraut's Reagent.-"' — Dissolve 2j2 grams of potassium iodide in water and add 80 grams of bismuth subnftrate dissolved in 200 grams of nitric acid (sp. gr. 1.1S). Permit the potassium nitrate to crystallize out, then filter it off and make the filtrate up to 1 liter with water. Lugol's Solution.0 — Dissolve 4 gram- of iodine and 6 gram- ol potassium iodide in 100 c.c. of distilled water. Magnesia Mixture.7 — Dissolve 175 grams of magnesium sul- phate and 350 grams of ammonium chloride in 14m) c.c. of distilled 1 Hopkins-Cole reaction, page 91. J Methods for determination of urea, page 374. '■' Iodine test, page 44. 'Jolles' reaction, pages 98 and 316. 'Rosenheim's bismuth test for choline, page 252. "Gunning's iodoform test, page 328, and Bardach's reaction pagi 'Sodium hydroxide and potassium nitrate fusion method for detennii of total phosphorus, page 390. 420 PHYSIOLOGICAL CHEMISTRY. water. Add 700 grams of concentrated ammonium hydroxide, mix thoroughly and preserve the mixture in a glass-stoppered bottle. Millon's Reagent.1 — Digest 1 part (by weight) of mercury with 2 parts (by weight) of nitric acid (sp. gr. 1.42) and dilute the re- sulting solution with 2 volumes of water. Molisch's Reagent.2 — A 15 per cent alcoholic solution of a-naphthol. Molybdic Solution.3 — Molybdic solution is prepared as follows, the parts being by weight: Molybdic acid 1 part. Ammonium hydroxide (sp. gr. 0.96) 4 parts. Nitric acid (sp. gr. 1.2) 15 parts. Moreigne's Reagent.4 — Combine 20 grams of sodium tungstate, 10 grams of phosphoric acid (sp. gr. 1.13) and 100 c.c. of water. Boil the mixture for twenty minutes, add water to make the vol- ume of the solution equivalent to the original volume and acidify with hydrochloric acid. ■ Morner's Reagent.5 — Thoroughly mix 1 volume of formalin, 45 volumes of distilled water and 55 volumes of concentrated sulphuric acid. Nakayama's- Reagent.6 — Prepared, by combining 99 c.c. of al- cohol and 1 c.c. of fuming hydrochloric acid containing 4 grams of ferric chloride per liter. Neutral Olive Oil.7 — Shake ordinary olive oil with a 10 per cent solution of sodium carbonate, extract the mixture with ether and remove the ether by evaporation. The residue is neutral olive oil. Nylander's Reagent.8 — Digest 2 grams of bismuth subnitrate and 4 grams of Rochelle salt in 100 c.c. of a 10 per cent solution of potassium hydroxide. The reagent should then be cooled and filtered. 1 Millon's reaction, page 90. 2 Molisch's reaction, page 23. 3 Sodium hydroxide and potassium nitrate fusion method for determination of total phosphorus, page 390. 4 Moreigne's reaction, page 275. 5 Morner's test, page 84. s Nakayama's reaction, pages 155 and 324. ' Emulsification of fats, page 136. 6 Nylander's test, pages 30 and 312. \ri'i:.\Dix. Obermayer's Reagent.1 Add _• .\ grams of ferric chloride to a liter of hydrochloric acid (sp. gr. [.19). Oxalated Plasma. 2 — Allov* arterial blood to run into an equal volume of 0.2 per rent ammonium oxalate solution, Para-dimethylaminobenzaldehyde Solution.1 This solution 1- made by dissolving 5 grains of para-dimcthvlaminobenzaldehyde in 100 c.c. of 10 per cent sulphuric acid. Para-phenelenediamine Hydrochloride Solution.' I wo grams dissolved in too c.c. of water. Phenolphthalein/' -Dissolve 1 gram of phenolphthalein in [00 c.c. of 95 per cent alcohol. Phenylhydrazine Mixture.1'' — This mixture is prepared by com- bining 1 part of phenylhydrazine-hydrochloride and 2 parts of sod- ium acetate by zveight. These are thoroughly mixed in a mortar. Phenylhydrazine-Acetate Solution.7 — This solution is prepared by mixing' 1 volume of glacial acetic acid. 1 volume <>t water and 2 volumes of phenylhydrazine (the base). Purdy's Solution.8 — Purdy's solution has the following com- position : Cupric sulphate 4-75-' grams. Potassium hydroxide 235 gram-. Ammonia (U. S. P., sp. gr. 0.9) 350.0 c.c. Glycerol 38.O c.c. Distilled water, to make total volume 1 liter. Roberts' Reagent.0 — Mix I volume of concentrated nitric acid and 5 volumes of a saturated solution of magnesium sulphate. Rosenheim's Iodo-Potassium Iodide Solution.10 —Dissolve 2 grams of iodine and 6 grams of potassium iodide in 100 c.c. ol .water. Salted Plasma.11 — Allow arterial blood to run into an equal vol- I Obermayer's test, page 281. -Experiments on blood plasma, page 201. 3 Herter's para-dimethylaminobenzaldehyde reaction, page 17° 'Detection of hydrogen peroxide, page 226. "Topfer's method, page 413. c Phenylhydrazine reaction, pages 24 and 306. 7 Phenylhydrazine reaction, pages 24 and 306. s Purdy's method, page .170. "Roberts' ring test, pages 97 and 315. "Rosenheim's periodide test, page 252. II Experiments on Mood plasma, page 201. 422 PHYSIOLOGICAL CHEMISTRY. ume of a saturated solution of sodium sulphate or a 10 per cent solution of sodium chloride. Keep the mixture in the cold room for about 24 hours. Schiff's Reagent.1 — This reagent consists of a mixture of three volumes of concentrated sulphuric acid and one volume of 10 per cent ferric chloride. Schweitzer's Reagent.2 — Add potassium hydroxide to a solution of cupric sulphate which contains some ammonium chloride. Fil- ter off the precipitate of cupric hydroxide, wash it and bring 3 grams of the moist cupric hydroxide into solution in a liter of 20 per cent ammonium hydroxide. Seliwanoff's Reagent.3 — Dissolve 0.05 gram of resorcin in 100 c.c. of dilute (1:2) hydrochloric acid. Sherrington's Solution.4 — This solution possesses the follow- ing formula : Methylene-blue 0.1 gram. Sodium chloride 1.2 gram. Neutral potassium oxalate 1.2 gram. Distilled water 300.0 grams. Sodium Acetate Solution.5 — Dissolve 100 grams of sodium acetate in 800 c.c. of distilled wtaer, add 100 c.c. of 30 per cent acetic acid to the solution and make the volume of the mixture up to 1 liter with distilled water. Sodium Alizarin Sulphonate.0 — Dissolve 1 gram of sodium aliz- arin sulphonate in 100 c.c. of water. Sodium Sulphide Solution.7 — Saturate a one per cent solution of sodium hydroxide with hydrogen sulphide gas and add an equal volume of one per cent sodium hydroxide. Solera's Test Paper.s — Saturate a good quality of filter paper with 0.5 per cent starch paste to which has been added sufficient iodic acid to make a 1 per cent solution of iodic acid and allow the paper to dry in the air. Cut it in strips of suitable size and pre- serve for use. 1 Schiff's reaction, pages 159 and 252. 2 Schweitzer's solubility test, page 50. 3 Seliwanoff's reaction, pages 35 and 339. 4 " Blood counting," page 212. 5 Uranium acetate method, page 389. 6T6pfer's method, page 413. 7 Kriiger and Schmidt's method, pages 374 and 406. s Solera's reaction, page 57. APPENDIX. Spiegler's Reagent.1 -This reagent lias the following comp tion : Tartaric acid Mercuric chloride rams. Glycerol 100 g Distilled water to Standard Ammonium Thiocyanate Solution.-' This solu- tion is made of such a strength that i c.c. of it is equal to i c< the standard argentic nitrate solution mentioned below. To pre pare the solution dissolve 12.9 grams of ammonium thiocyanate, NH4SCN. in a little less than a liter of water. In a small lla^k place 20 c.c. of the standard argentic nitrate solution, 5 c.c. of a cold saturated solution of ferric alum and 4 c.c. of nitric acid (sp. gr. 1.2), add water to make the total volume [00 c.c. and thor- oughly mix the contents of the flask. Mow run in the ammonium thiocyanate solution from a burette until a permanent bi tinge is produced. This is the end-reaction and indicates that the last trace of argentic nitrate has been precipitated. Take the burette reading and calculate the amount of water necessary t<> use in dilut- ing the ammonium thiocyanate in order that 10 c.c. of this solu- tion may be exactly equal to 10 c.c. of the argentic nitrate solution. Make the dilution and titrate again to be certain that the solution is of the proper strength. Standard Argentic Nitrate Solution.3 — Dissolve 29.06 grams of argentic nitrate in 1 liter of distilled water. Each cubic centimeter of this solution is equivalent to 0.01 gram of sodium chloride or to 0.006 gram of chlorine. Standard Uranium Acetate Solution.4 — Dissolve 35.461 grams of uranium acetate in I liter of water. One c.c. of such a solution should be equivalent to 0.005 gram of P2< >5, phosphoric anhydride. This solution may be standardized as follows: To 50 c.c. oi a standard solution of disodium hydrogen phosphate, of Mich a strength that the 50 c.c. contains o. t gram of P2< >5, add 5 C.C. of the sodium acetate solution mentioned on p. 422 and titrate with the uranium solution to the correct end-reaction as indicated in the 'Spiegler's ring test, pages 98 and 316. "Volhard-Arnold method, page 396, and Clark's modification of Dehn's method, page 394. 8 Volhard-Arnold method, page 396. Mohr's method, page 39S1 •in,i Clark's modification of Dehn's method, page 394. 'Uranium acetate method, page 389- 424 PHYSIOLOGICAL CHEMISTRY. method proper on p. 389. Inasmuch as 1 c.c. of the uranium solu- tion should precipitate 0.005 gram °f P2O5, exactly 20 c.c. of the uranium solution should be required to precipitate the 50 c.c. of the standard phosphate solution. If the two solutions do not bear this relation to each other they must be brought into the proper relation by diluting the uranium solution with distilled water or by increas- ing its strength. Starch Iodide Solution.1 — Mix 0.1 gram of starch powder with cold water in a mortar and pour the suspended starch granules into 75-100 c.c. of boiling water, stirring continuously. Cool the starch paste, add 20-25 grams of potassium iodide and dilute the mixture to 250 c.c. This solution deteriorates upon standing, and therefore must be freshly prepared as needed. Starch Paste.2 — Grind 2 grams of starch powder in a mortar with a small amount of water. Bring 200 c.c. of water to the boil- ing-point and add the starch mixture from the mortar with con- tinuous stirring. Bring again to the boiling-point and allow it to cool. This makes an approximate 1 per cent starch paste which is a very satisfactory strength for general use. Stokes' Reagent.3 — A solution containing 2 per cent ferrous sulphate and 3 per cent tartaric acid. When needed for use a small amount should be placed in a test-tube and ammonium hydroxide added until the precipitate which forms on the first addition of the hydroxide has entirely dissolved. This produces ammonium fer- rotartrate which is a reducing agent. Suspension of Manganese Dioxide.4 — Made by heating a 0.5 per cent solution of potassium permanganate with a little alcohol until it is decolorized. Tanret's Reagent.5 — Dissolve 1.35 grams of mercuric chloride in 25 c.c. of water, add to this solution 3.32 grams of potassium iodide dissolved in 25 c.c. of water, then make the total solution up to 60 c.c. with distilled water and add 20 c.c. of glacial acetic acid to the mixture. Tincture of Iodine.6 — Dissolve 70 grams of iodine and 50 grams of potassium iodide in 1 liter of 95 per cent alcohol. Toison's Solution.7 — This solution has the following formula : 1 Fehling's method, page 367. 2 Experiments on starch, page 44. 3 Haemoglobin, page 203. Hsemochromogen, page 202. * Kriiger and Schmidt's method, pages 374 and 406. 5 Tanret's test, pages 98 and 317. 6 Smith's test, pages 155 and 325. ' " Blood counting," page 212. APPENDIX. Methyl violet 0.025 gram. Sodium chloride • <, gram. Sodium sulphate ams. Glycerol 30.0 g 1 Distilled water 1O0.0 gi Topfer's Reagent.1 I )issolve 0.5 gram of di-methylamino- azobenzene in too c.c. of 95 per cent alcohol. Tropaeolin OO.2 — Dissolve 0.05 gram of tropaeolin < )< ) in [00 c.c. of 50 per cent alcohol. Uffelmann's Reagent.'1 — Add a 5 per cent solution of ferric chloride to a"i per cent solntion of carbolic acid until an amethyst- blue color is obtained. 1 Topfer's method, page 413. 2 Test for free acid, page 124. 3 Uffelman's reaction, page 129. NDEX. Acacia solution, formation of emulsion by, 133 Acetone, 305, 327 formula for, 327 Gunning's iodoform test for, 328 Legal's test for, 329 Lieben's test for, 329 quantitative determination of, 400 Reynolds-Gunning test for, 329 Taylor's test for, 329 Acholic stool, 173 Achroo-dextrins, 44, 55. 58 a-achroo-dextrin, 55 /3-achroo-dextrin, 55 7-achroo-dextrin, 55 Acid, acetic, 265, 291 alloxyproteic, 264, 285, 342 amino-acetic, 67 amino-ethyl-sulphonic, 151, 240 a-amino-/3-hydroxy-propionic, 69 a-amino-/3-imidazol-propionic. 74 a-amino-iso-butyl-acetic, 76 a-amino-methyl-ethyl-propionic, 77 a-ainino-normal glutaric, 79 a-amino-propionic, 68 amino-succinic, 78 a-amino-iso-valerianic, 75 (see Valine) aspartic, 63 benzoic, 161, 264, 289 butyric, 119, 225, 265, 290 caproic. 218 carbamic, 184 cholic, 151 chondroitin-sulphuric, 232, 264, 285 citric, 218 combined hydrochloric. 59 cyanuric, 267 a-e-di-amino-caproic, 77 a-amino-/3-thiolactic, disulphide of, 72 diaminotrihydroxydodecanoic, 63, 81 diazo-benzene-sulphonic, 342 ethereal sulphuric, 162, 264, 279 fatty, 131, 132, 138 formic, 265, 291 free hydrochloric, 119, 123 glutamic, 63 glycocholie, 151 glycuronic, 37 glycerophosphoric, 248, 249, 265, 291 glyoxylic, 91 guanidine-a-ami no- valerianic. 75 hippuric, 160, 161, 264, 281, 383 homogentisic, 28, 264, 2S8 indole-amino-propionic. 73 indoxyl-sulphuric, 162, 279 inosinic, 236, 241 kvnurenic, 264, 288 Acid, lactic. [19, 1 29, 236 lauric, 218 mucic, •.'.. !•.. .137 myristic, 218 nucleic, 107 osraic, 251, 281 oxalic. 264, 284 oxaluric, 264, 290 oxymandelic, 264, 288 oxyproteic, 204, jX- palmitic, para-cresol-sulphuric. 264, 279 para-oxyphenyl-acetic, 162, 168, 264, 287 para-oxyphenyl-a-amino-propionic, 70 para-oxyphenyl-propionie. 7.., 162, 168, 264, 287 paralactic, 237, 265, 291 phenaceturic, 265. 291, 383 phenol-sulphuric, 264, 279 phenyl-a-amino-propionic, 69 phosphocarnic, 236. 241. 265, 292 phosphoric, 299 pyrocatechin-sulphuric. 264, 279 a-pyrrolidine-carboxylic, 80 sarcolactic, 237 skatole acetic, 73 skatole-carbonic, 167 skatoxyl-sulphuric. 264. 279 sulphanilic, 342 tannic, 46, 49 taurocholic, 151 uric, 28, 236, 264 uroferric. 264, 285. 342 uroleucic. 264, 288 volatile fatty, 162, 165. 265, 290 Acid albuminate. See Acid metaprotein. Acid infraprotein. See Acid metaprotein. Acid metaprotein. no coagulation of, 110. 111 experiments on. 1 1 <■ precipitation of, 1 1 1 preparatii m of, no solubility of. 1 10 sulphur content of. 1 10 Acidity of gastric juice, quantitativi termination of. 413 urine, cause of, 256, .;■>" quantitative determination of, 404 Acidosis, cause of, 332 \cid li.emat in. 206 \ercc- Rosenheim formaldehyde reaction. Acrolein, formation of, from olive oil. 135 from yjy. Activation. 5, [42 427 428 INDEX. Activation by calcium salts, 142 Adams' paper coil method for determina- tion of fat in milk, 410 Adamkiewicz reaction, 91 Adenine, 241, 265 Adipocere, 134 Adler's benzidine reaction for blood, 192, 196, 323 Agglutination, 196 Alanine 63, 68 Albumin, egg, 101 powdered, preparation of, 101 tests on, 101 serum, 86, 89, 182, 305, 313 Albumin in urine, 305, 314 acetic acid and potassium fer- rocyanide test for, 317 coagulation or boiling test for, 316 Heller's ring test for, 314 Jolles' reaction for, 316 Roberts' ring test for, 315 sodium chloride and acetic acid test for, 317 Spiegler's ring test for, 316 Tanret's test for, 317 tests for, 314 Albumins, 86, 88, 89 Albuminates. See Metaproteins. Albuminates, formation of, by metallic salts, 95, 97 Albuminoids, 86 Albumoids, 106 Albumoscope, 97, 315 Albumoses (see Proteoses, p. 113) Alcohol-soluble proteins. See Prolamins Aldehyde, 21, 26 Aldehyde group, 39 Aldehyde test for alcohol, 43 v. Aldor's method of detecting proteose in urine, 320 Aldose, 21 Alkali albuminate. See Alkali meta- protein. Alkali-haematin, 206 Alkali metaprotein, no, in experiments on, in precipitation of, 111 preparation of, in sulphur content of, no Allantoin, 264, 285 crystalline form of, 286 experiments on, 286 formula for, 285 preparation of, from uric acid, 286 quantitative determination of, 407 separation of, from urine, 286 Allen's modification of Fehling's test, 311 Almen's reagent, preparation of, 321 Alloxyproteic acid, 264, 285, 342 Aloin-turpentine test for " occult blood," 175, 178 Amandin, 86 Amide nitrogen, 62 Amidulin. See Soluble starch, 8, 54 Amino acids, 63, 162 Amino group, 88, 92 a-amino-/3-hydroxypropionic acid, 69 a-amino-j8-imidazol-propionic acid, 74 a-amino-iso-butyl-acetic acid, 76 ct-amino-normal-glutaric acid, 79 Amino-succinic acid, 78 a-amino-iso-valerianic acid, 75 Ammonia, 67, 105 Ammonia in urine, 257, 265, 295 quantitative determination of, 380 Ammoniacal silver solution, preparation of, 407 Ammoniacal-zinc chloride test for uro- bilin, 293 Ammonium magnesium phosphate ("Triple phosphate "), 247 301 in urinary sediments, 344 Ammonium urate, 271, 347, 372 crystalline form of, Plate VI, opposite p. 348 Amphopeptone, 113 Amylase, pancreatic, 141 digestion of dry starch by, 143, 148 inulin by, 148 experiments on, 8, 147 influence of bile upon action of, 148 metallic salts, upon action of, 147 most favorable temperature for ac- tion of, 147 salivary, 54, 119 activity of, in stomach, 55, 119 experiments on, 8 inhibition of activity of, 55 nature of action of, 54 products of action of, 55 vegetable, 9 Amylases, 3 experiments on, 8 Amyloid, 49 Amylolytic enzymes. See Amylases quantitative determination of ac- tivity of, 16 Animal parasites in feces, 175, 177 in urinary sediments, 351, 361 Anti-albumid, 122 Anti-enzymes, 7 experiments on, 15 Anti-pepsin, 8, 1 5 Antipeptone, 113 Anti-rennin, 7 Anti-trypsin, 8, 15 Appendix, 416 Arabinose, 21, 37 orcin test on, 38 phenylhydrazine test on, 38 Tollens' reaction on, 37 Arginine, 63, 75, 141 Arnold-Lipliawsky reaction for diacetic acid, 331 reagent, preparation of, 331 Aromatic oxyacids, 264, 287 Ascaris, 15, 16 Asparagine, 79 Aspartic acid, 63, 78, 80, 141 [NDEX. 429 Aspartic acid, crystalline form of, 78 formula for, 78 Ash of milk, quantitative determination of, 41 1 Assimilation limit, 23 Atkinson and Kendall's lia-niin teat, 197 Autolytic enzymes, 3 Bardach's reaction, 94 Barfoed's reagent, preparation of, 12, 31, 313 Barfoed's test for monosaccharides, 31, 313 Baryta mixture, preparation of, 269 Bayberry tallow, saponification of, 136 source of, 136 Bayberry wax. See Bayberry tallow, 136 Beckmann-Heidenhain apparatus, 260 " Bence Jones' protein," detection of, 320 Benedict's method for quantitative de- termination of sugar, 368 Benedict's modifications of Fehling's test, 27, 28 solutions, preparation of, 27, 28 solution, for use in quantitative de- termination of sugar, preparation of, 368 Benedict and Gephart's method for the quantitative determination of urea, 379 Benzidine reaction, Adler's, for blood, 192, 196, 323 Benzoic acid, 161, 269, 289 crystalline form of, 289 experiments upon, 289 formula for, 289 solubility of, 289 sublimation of, 290 Berthelot-Atwater bomb calorimeter, 388 Bergell's method for determination of /3-oxybutyric acid, 404 Bile, 150, 305, 324 constituents of. 151 daily secretion of, 151 freezing-point of. 151 influence on digestion, gastric, 128 pancreatic. 146, 148 inorganic constituents of, 151, 154 nucleoprotein of, 154 reaction of, 150, 154 secretion of, 150 specific gravity of, 151 Bile acids, 151 Guerin's reaction for, 156 Hay's test for, 157 Mylius's test for. 156 Xeukomm's test for, 156 Pettenkofer's test for. 156 tests for, 156 v. Udransky's test for. 156 Bile acids in feces, detection of, 179 Bile acids in urine. 325 Hay's test for. 326 Mylius's test for, 326 Neukomm's test for, 326 Pettenkofer's test for. 325 tests for, 325 Bile a. ids in urine, v. Udran l-.r. Bile pigments, 1 < rmelin'fl '• I foi Harm I luppcrt's 1. a. ip. n for, 1 55 Smith's test for, 155 tesl for. 154, '55 Bile pigments in urini Gmi llainiii.-n :.,r. 325 I [uppert* Xakayama's reaction lor. 3-'4 Rosenbach's tesl for Salkowski's tesl for Salkowski-Schippcr's i tion for, 325 Smith's test for, 324 tests for, 324 Bile salts. 6, 151 crystallization of, [52, i?r Biliary, calculi, 154 analysis of, 158 Bilicyanin, 152, 154 Bilifuscin, 152 Bilihumin, 152 Biliprasin, 152 Bilirubin, 152, 153 crystalline form of, 153 in urinary sediments, 350 Biliverdin, 152, 154 " Biological " blood test, 193 Bismuth test for choline, 253 Biuret, 92, 267 formation of, from urea. 92, 269 Biuret potassium cupric hydroxid. See Cupri-potassium biuret, 92 test, 92 Posner's modification of, 93 Black's method for determination of /3-oxybutyric acid, 403 reaction for /3-oxybutyric acid. 332 reagent, preparation of, 333 Blood, i8j. 321 agglutination of. [96 Bordet test for, 193 clinical examination of. 207 coagulation of, 191 constituents of, 182, 184 defibrinated. 192 detection of. 192, 20. erythrocytes of. 1 s 4 experiments oil, 193 form elements of. 1 82 guaiac test for, 178, 192, 196 h.cmin test for. [92, 197 oxyhemoglobin of, 185 "occult," in feces. 175. 178 in urine. 305, .;.' 1 leuci 190 medico-legal tests for. 102 microscopical examination 01 202 430 INDEX. Blood, nucleoprotein of, 182 pigment of, 185 plaques, 182, 191 plasma, 184 preparation of hsematin from, 199 preparation of laky, 195 quantitative analysis of, 415 reaction of, 182, 193 serum, 184, 200 specific gravity of, 182, 193 spectroscopic examination of, 203 test for iron in, 195 total amount of, 182 v. Zeynek and Nencki's hsemin test for, 199 Blood casts in urine, 351, 358 Blood corpuscles, 182, 184 " counting," 212 Blood dust, 182, 191 Blood in urine, 305, 321 Adler's benzidine reaction for, 323 guaiac test for, 322 Teichmann's hsemin test for, 322 Heller's test for, 321 Heller-Teichmann reaction for, 322 Schalfijew's haemin test for, 322 Schumm's modification of guaiac test for, 323 spectroscopic examination of, 323 tests for, 321 v. Zeynek and Nencki's hasmin test for, 322 Blood plasma, 182, 201 constituents of, 182 crystallization of oxyhemoglobin of, 189, 201 effect of calcium on oxalated, 201 experiments on, 201 preparation of fibrinogen from, 201 oxalated, 201 salted, 201 Blood serum, 184, 200 coagulation temperature of, 200 constituents of, 184 experiments on, 200 precipitation of proteins of, 200 separation of albumin and globulin of, 201 sodium chloride in, 201 sugar in, 201 Blood stains, examination of, 202 Boas' reagent, as indicator, 124 , preparation of, 124 Boekelman and Bouma's method for de- termination of /3-oxybutyric acid, 404 Boettger's test for sugar, 30 Bomb calorimeter, Berthelot-Atwater, 388 Bone, constituents of, 233 ossein of, preparation of, 233 Bone ash, scheme for analysis of, 234 Borchardt's reaction for lsevulose, 35, 338 Bordet test, detection of human blood by, 193 Boric acid and borates in milk, detection of, 22(1 Buccal glands, 53 Buffy coat, formation of, 184 Bunge's mass action theory, 119 Butyric acid, 119, 225 Butyrin, 132 Bynin, 86, 105 Cadaverin, 77 Calcium and magnesium in urine, 265, 303 carbonate in urinary sediments, 344 345 casein, 121 oxalate, 344 in urinary sediments, 344 phosphate in urinary sediments, 344 in milk, 224 sulphate in urinary sediments, 344 346 Calculi, biliary, 154, 158 urinary, 362 calcium carbonate in, 363 oxalate in, 363 cholesterol in, 365 cystine in, 363 fibrin in, 363 indigo in, 365 phosphates in, 363 uric acid and urates in, 363 urostealiths in, 363 xanthine in, 363 Calliphora, larvae of, formation of fat from protein by, 134 Cane sugar (see sucrose, p. 41) Caproic acid, 218 Carbamic acid, 184 Carbohydrates, 21 classification of, 21 composition of, 21, 22 review of, 50 scheme for detection of, 51 variation in solubility of, 22 Carbonates in urine, 265, 303 Carbon moiety of protein molecule, 134 Carbon monoxide, haemoglobin, 205 tannin test for, 205 Carboxyl group, 88 Carnine, 236 Carnitine, 236 formula for, 240 Carnomuscarine, 236 Carnosine, 236, 240 Cartilage, 232 constituents of, 232 experiments on, 232 Hopkins-Cole reaction on, 232 loosely combined sulphur in, 232 Millon's reaction on, 232 preparation of gelatin from, 232 solubility of, 232 xanthoproteic test on, 232 Casein, 219 INDEX. Casein, soluble, 2 i 9 calcium, 121 quantitative determination of, 412 Caseinogen, 87, 88, 107, 180, 21m action of rennin upon, ui. 2ig biuret test on, 224 Millon's test on, 224 precipitation of, 223 preparation of, 223 solubility of, 224 test for loosely combined sulphur in, 224 test for phosphorus in, 224 Casts, 351, 354 blood, 351, 356, 358 epithelial, 351, 358 fatty, 351, 358 granular, 351, 356 hyaline, 351, 355 pus, 351, 359 waxy, 351, 358 Casts in urinary sediments, 351, 354 Cat gut, 127 Catalase, 14 experiments on, 14 Catalysis, 2 Cellulose, 22, 49 action of Schweitzer's reagent on, 49 hydrolysis of, 49 iodine test on, 49 solubility of, 49 Cellulose group, 22 Cerebrin, 248, 250 experiments on, 252 hydrolysis of, 252 microscopical examination of, 252 preparation of, 252 solubility of, 252 Cerebro-spinal fluid, choline in, 249 Charcot-Leyden crystals, 175 form of, 174 Chlorides in urine, 265, 298 detection of, 299 quantitative determination of, 394 Cholecyanin, 154 Choleprasin, 152 Cholera-red reaction for indole, 169 Cholesterol, 154, 158 crystalline form of, 159 formula for, 250 iodine-sulphuric acid test for, 158, 251 isolation of, from biliary calculi, 158 Liebermann-Burchard test for, 158, 251 occurrence of, in urinary sediments, 344. 349 preparation of. from nervous tissue, 25 1 Salkowski's test for. 150. 252 Schiff's reaction for, 159, 252 tests for, 158, 251 Choletelin, 152 Choline, 248. 252 1 holine, formula i"i for, 252 ( Ihondrigt 1 ( Ihondroalbumoid < bondromucoid Chondroitin, 232 Chondroitin Blllphuril „•, 264, 285 1 hondrosii Chromoproteins, 85, see Haemoglobin* < ipollina's test, 25, .0.7 Clark's modification of Dehn'a method for determination of chlorides, Cleavage products of protein (see De- composition products), 61 Clupeine, 87, 88 Coagulated proteins, 88, 1 1 1 biuret test on, 1 1 2 formation of, 1 1 1 I [opl ins-Cole reaction on, 1 12 Millon's reaction on, '1 12 solubility of, 112 xanthoproteic reaction on. 1:2 Coagulation of proteins, 99, 111 changes in composition during, 100, 112 fractional, 100, 112 Coagulation temperature of proteins. 100, 1 12 apparatus used in determining, 100 method employed in determin- ing, 100 Co-enzyme, 5 Collagen, 86, 106, 232, 248 experiments on, 229 percentage of, in ligament. 231 in tendon, 228 production of gelatin from, 229 solubility of. 229 transformation of, 228 Colostrum, 221 microscopical appearance of. 219 Combined hydrochloric acid. 119 tests for, 1 23- 1 25 Compound test for lactose in urine. 337 Congealing-point of fat, 139 Congo red, as indicator, 124 preparation of, 124 Conjugated proteins, 87, 89, 106 classes of, 87, 89, 106 experiments on. 195, 196 20 1. 203, 223 nomenclature of, 87 occurrence of, 106 Conjugate glycuronati fermentation reduction u - 334 Tollens' reaction on, 334 ( 'onnective tissui Cowie's guaiac test, 178 Creatine, 184, -." crystalline form of, formula for, quantitative determination separation of, from meat extr.: Creatinine, 28, 236, 432 INDEX. Creatinine, coefficient, definition of. 276 crystalline form of, 277 daily excretion of, 276 experiments on, 277 formula for, 240, 275 Jaffe's reaction for, 278 quantitative determination of, 392 Salkowski's test for, 278 separation of, from urine, 277 Weyl's test for, 278 Creatinine-zinc chloride, formation of, 276, 278 Cresol, para, 162 tests for, 170 Cryoscopy, 259 Cul-de-sac, 118 Cupri-potassium biuret, formation of, 92 formula for, 93 Cyanuric acid, 267 formula for, 267 Cylindroids in urinary sediments, 359 Cystine, 63, 72, 141 crystalline form of, 73 detection of, 349 formula for, 72 in urinary sediments, 348 Cytoglobulin, 87, 89 Cytosine, 107 Wheeler-Johnson reaction for, 107 Dakin's methods for quantitative deter- mination of hippuric acid, 383 Dare's hsemoglobinometer, 210 description of, 210 determination of haemoglobin by, 210 Darmstadter's method for determination of (3-oxybutyric acid, 403 Deamidizing enzyme, 3 Decomposition products of proteins, 61 crystalline forms of, 68-81 experiments on, 82 isolation of, 82 Degradation products of protein (see De- composition products, 61 Dehn's method, Clark's modification of, 394 Dehn's reaction for hippuric acid, 283 Delusive feeding experiments, 118 Derived proteins, 87, 108 Detection of preservatives in milk, 225 boric acid and borates, 226 formaldehyde, 225 hydrogen peroxide, 226 salicylic acid and salicylates, 226 Deuteroproteose, 88, 89 Dextrin, 22, 48 achroo-, 44, 55 a-achroo-, 55 /3-achroo-, 55 7-achroo, 55 erythro-, 44, 48, 55 action of tannic acid on, 49 diffusibility of, 49 Fehling's test on, 48 hydrolysis of, 48 Dextrin, iodine test on, 48 solubility of, 48 Dextrosazone, crystalline form of, Plate III, opposite p. 24 Dextrose, 21, 23, 305 Allen's modification of Fehling's test for, 311 Barfoed's test on, 31, 313 Boettger's test on, 30, 311 Cipollina's test on, 25, 307 Benedict's modifications of Fehling's test, 28, 29, 309, 310 diffusibility of, 25 experiments on, 23 Fehling's test on, 27, 308 fermentation of, 313 iodine test on, 25 Molisch's reaction on, 23 Moore's test on, 26 Nylander's test on, 30, 312 phenylhydrazine test on, 306 quantitative determination of, 367 reduction tests on, 26, 307 solubility of, 23 Trommer's test on, 27, 308 Dextrosazone, crystalline form of, Plate III, opposite p. 24 Diacetic acid, 305, 331 Arnold-Lipliawsky test for, 331 formula for, 330 Gerhardt's test for, 330 quantitative determination of, 401 ' Diamino acid nitrogen, 62 Diaminotrihydroxydodecanoic acid, 81 a-e-di-amino-caproic acid, 77 Diastase (see Vegetable amylase) Diazo-benzene-sulphonic acid, 342 reagent, preparation of, 342 Diazo reaction (Ehrlich's), 342 Differentiation between pepsin and pep- singen, 126 Digestion, gastric, 118 pancreatic, 140 salivary, 53 Di-methyl-amino-azobenzene (see Top- fer's reagent), 123 Dipeptides, 64, 66, 88, 89 Disaccharides, 38 classification of, 21 Dissociation products of protein (see De- composition products, 67) Doremus-Hinds ureometer, 378 Drying method for determination of total solids in urine, 408 Duodenum, epithelial cells of, 140 Earthy phosphates in urine, 299, 302 quantitative determination of, 390 Edestan, 18, 87, 109 experiments on, 109 Edestin, 86, 103 coagulation of, 103 crystalline forms of, 104 microscopical examination of, 103 [NDEX. Edestin, Millon's test on, 103 preparation of, 103 solubility of, 103 tests on crystallized, [03 filtrate of, 104 Ehrlich's diazo-benzene-sulpbonic acid reagent, preparation of, 342 Ehrlich's diazo reaction. Ehrlich's mechanical eye-piece, use of, 216 Einhorn's saccharometer, 31 Elastin, 86, 88, 106, 231 experiments on, 231 preparation of, 231 solubility of, 231 Electrical conductivity of urine, 261 Embryos, glycogen in, 237 Enterokinase, 5, 141 Enzymes, 1 activation of, 5 adsorption of, 4 classification of, 3 definition of, 1 experiments on, 8 preparation of, 4 properties of, 4 Epiguanine, 265, 294 Episarkine, 265, 294 Epithelial cells in urinary sediments, 351, 352 casts in urinary sediments, 351, 358 Epithelial tissue, 227 experiments on, 227 Erepsin, 13 experiments on, 13 Erythrocytes, 182, 184 counting the, 212 diameter of. 184 form of, 184 influence of osmotic pressure on, 195 in urinary sediments, 351, 360 number of, per cubic mm., 185 of different species, 184 stroma of, 182, 185 variation in number of, 185 Erythro-dextrin, 44, 55, 58 Esbach's albuminometer, 367 method for determination of albumin, 366 reagent, preparation of, 366 Ester, definition of, 131 hydrochloric acid, of haematin, 199 sulphuric acid, of haematin, 199 Ethereal sulphates, 296, 297 quantitative determination of, 386 Ethereal sulphuric acid. 162, 264, 279 Ethyl butyrate test for pancreatic lipase, 149 Euglobulin, 182, 183 Excelsin, 103 crystalline form of, 105 Extractives of muscular tissue, 236 nitrogenous, 236 non-nitrogenous, 236 29 Fatigue Bubstam ea "i mu FatS, 1 ;i absorption of, 133 apparatus \>>r determination --i melting point ol boiling point of, 133 chemical composition of, 131 congealing point "t crystallization of, 133, digestion of, 133 emulsification of, experiments on, 135 formation <>f from protein formation <>i a< rolein from, hydrolysis of, in milk, 218, jj., in urine. 305, ,\m melting point of, 1 ■; nomenclature of, 133 occurrence of, 131 permanent emulsions of, 133 quantitative determination of, in milk. 1 1 M rancid. 133 reaction of. 135 saponification of, 132, 136. 138 solubility of. 133. 135 transitory emulsions of, 133 Fat-splitting enzymes 1 see Lipas* - Fatty acid, 131, 132, 138 Fatty casts in urinary sediments, 351, 358 Fatty degeneration, 134 Feces, 172 blood in, 175 daily excretion of, 172 detection of albumin and globulin in. 180 bile acids in. 17') bilirubin in. 179 caseinogen in, 180 cholesterol in. 177 hydrobilirubin in. 1 7t\ importance of, 174 Fecal bacteria. 1 75 Folding's method for determination of dextrose, Benedict's modification of. solution, preparation ol test. J 7. 308 Allen's modification of, 31 1 Benedict's modificat ii Ferments, classification •■!'. 1 Fermentation test. 31, 313 434 INDEX. Fermentation method for determination of dextrose, 371 Fermentation-reduction test for con- jugate glycuronates, 334 Ferric chloride test for thiocyanate in saliva, 57 Fibrin, 183, 191, 202, 305 in urinary sediments, 351, 361 separation of, from blood, 191, 202 solubility of, 202 Fibrin ferment, 184, 191 Fibrinogen, 182, 191 Fibroin, silk, 66 Fischer apparatus, 67 photograph of, 71 Fleischl's hsemometer, 207, 208 description of, 207 determination of haemoglobin by, 207 Fleischl-Miescher hsemometer, 209 Fluorides in urine, 265, 298, 394 Fly-maggots, experiments on, 134 Folin-Hart method for determination of combined acetone and diacetic acid, 397 for determination of diacetic acid, 401 Folin-Messinger-Huppert method for de- termination of diacetic acid, 401 Folin's method for determination of acetone, 400 acidity of urine, 404 ammonia, 380 creatinine, 392 ethereal sulphates, 386 inorganic sulphates, 385 total sulphates, 384 urea, 377 Folin-Shaffer method for determination of uric acid, 372 Foreign substances in urinary sediment, 35i, 361 Formation of methylphenyllsevulosazone, 35 Form elements of blood, 184 Formic acid, 265, 291 Fractional coagulation of proteins, 112 Free hydrochloric acid, 123 tests for, 123-125 Freezing-point of bile, 151 blood, 182 milk, 218 pancreatic juice, 141 urine, 260 Fuchsin-frog experiment, 242 Fuld and Levison's method for peptic ac- tivity, 1 8 Fundus glands, 118 Furfurol solution, preparation of, 156 Fusion mixture, preparation of, 102 Galactase, 221 Galactose, 21, 36, 305, 337 experiments on, 36 Gallic acid test for formaldehyde, 225 Gastric digestion, 118 conditions essential for, 120, 125 general experiments on, 125 influence of bile on, 128 influence of different tempera- tures on, 126 most favorable acidity for, 126 power of different acids in, 127 products of, 120 Gastric fistula, 118 Gastric juice, 1 18-122 acidity of, 119 artificial, preparation of, 122 composition of, 119 enzymes of, 119 origin of hydrochloric acid of, 119 quantitative analysis of, 413 quantity of, 118 reaction of, 119 specific gravity of, 119 lactic acid in, test for, 129 Gastric lipase, 119, 121 Gastric protease, 1 Gastric rennin, 119, 121, 128 action of, upon caseinogen, 121 219 experiments on, 128, 130 influence of, upon milk, 223 in gastric juice, absence of, 121 nature of action of, 121 occurrence of, 121 Gelatin, 91, 228, 230 coagulation of, 230 experiments on, 230 formation of, 229 Hopkins-Cole reaction on, 230 Millon's reaction on, 230 precipitation of, by alcohol, 230 alkaloidal reagents, 230 metallic salts, 230 precipitation of, by mineral acids, 230 preparation of, from cartilage, 232 from collagen, 229 salting-out of, 230 solubility of, 230 Gerhardt's test for diacetic acid, 330 Gerhardt's test for urobilin, 293 Gliadin, 86, 105 Globin, 86, 88 Globulins, 86, 99, 102 experiments on, 103 preparation of, 103 serum, 86, 182, 305, 318 in urine, 305, 318 tests for, 318 vegetable, 86 Glucoproteins (see Glycoproteins, p. 89) Glucose (see Dextrose, p. 21) Glutamic acid, 63, 79, 141 formula for, 79 Glutelins, 86, 104 Glutenin, 86, 104 Glycerol, 132, 138 borax fusion test on, 139 [NDEX. 435 Glycerol, experiments on, 138 formula for, 135 Glycerol extract of pig's stomach, prepar- ation of, 122 Glycerophosphoric acid, 248, 249,265,291 Glycocholic acid, 151 Glycocholic acid group. 151 Glycocoll, 63, 67, t 5 f formula for, 67, 151 preparation of, 160 Glycocoll ester hydrochloride, crystalline form of, 68 Glycogen, 22, 47, 236, 237 experiments on, 244 hydrolysis of, 244 in embryos, 237 influence of saliva on, 244 iodine test on, 244 preparation of, 244 Glycoproteins, 87, 106, 228 experiments on, 229 hydrolysis of, 229 Glycosuria, alimentary, 23 Glycuronates, conjugate, 28, 305, 309, 334 Glycuronic acid, 37 Glycyl-glycine, formation of, 66 Glyoxylic acid, 91 formula for, 91 Gmelin's test for bile pigments, 154, 324 Rosenbach's modification of, 155, 324 _ Granular casts in urinary sediments, 351, 356 Granulose. 43 Green stools, cause of, 173 Gross' method for quantitative deter- mination of tryptic activity, 19 Guaiac solution, preparation of, 418 Guaiac test on blood, 178, 192. 196 on feces, 178 milk, 222 in urine, 322 Guaiac test, Schumm's modification of, 196 Guaiac test on pus, 354 Guanidine-a-amino-valerianic acid, 75 Guanidine-residue, 62 Guanine, 236, 241 Gums and vegetable mucilage group of carbohydrates, 22 Gunning's iodoform test for acetone, 328 Giinzberg's reagent, as indicator, 123 preparation of, 123 Giirber's reaction for indican, 281 Hsematin, 108 acid-, 206 alkali-, 206 preparation of, 199 reduced alkali-, 206 Hsematodir, 153. 173 crystalline form of, 153. 173 in urinary sediments. 344. 350 Hematuria, 321 Hsmatoporphyrin, 10. 190. 207. 305. 31a in urine. 305, 336 I l.i'iinn crystals, form of, ioX "'7 Haemochromogen, 108, 18s I fa 1 \ .miii 8; 1 '■' "' ee Blood dust. 1 1- globin 8; 89 106, 107 ■ 11 bon monoxide, 1 91 di composition of, 185 diffusion of, met, ton, nxy. 185, igo, - quantitative determination ol reduced, 203 Haemoglobins, 87, 107 I la 1 1 1 ■ ' l' 1 . . 1 1 i 1 1 1 1 r i a , 32 t Hammerschlag's method for determina- tion of specific gravity of blood, 194 Hammarsten's reaction, i$S, 325 reagent, preparation of, 155, 325 Hay's test for bile acids, 157, Heintz method for determination of uric acid, 373 Hclicoprotein. 87 • Heller's test for blood in urine. 321 Heller-Teichmann reaction for blond in urine, 322 Heller's ring test for protein, 07. 314 Hemi-cellulose, 22 Htrter's naphthaquinone reaction for indole, 168 Herter's para-dime thy lam inobenzaldehyde reaction, 170 Heteroproteose, 89 Heteroxanthine, 265, 2^4 Hexone bases, 77 Hexoses, 21, 22 Hippuric acid, 160. 161, 264. 281. 383 crystalline form of, 282 Dakin's methods for quantita- tive determination of. 383 Dehn's reaction for. experiments on, 160, formula for, 161 in urinary sediments, 54. j melting point 1 if Roaf's method for crystallization of, 283 separation of, from urin< solubility of, I I ippuric acid, sublimation of, synthesis of, 1 60 Histidine, 63, 74. '4' hydrochloride, crystalline form Knoop's color reaction 1 1 rlistones, 86, 88 I [offmann's reaction for tyn • Homogentisic acid. 28 formula for, 1 [opkins Cole reaction, . St.. 105 Horismascope - -1 1 Vlbun - Hormone, definition of, 436 INDEX. Hopkins' thiophene reaction for lactic acid, 129 Hvifner's urea apparatus, 377 Human fat, composition of, 133 Huppert's reaction for bile pigments, 155, 324 Hiirthle's experiment, 247 Hyaline casts in urinary sediments, 351, 355 Hydrobilirubin, detection of, in feces, 179 extraction of, 179 Hydrochloric acid of the gastric juice, 119 origin of, theories as to, 119 Hydrochloric acid test for formaldehyde (Leach), 225 Hydrogen peroxide in urine, 265, 304 detection of, in milk, 226 Hydrolysis of cellulose, 49 cerebrin, 252 dextrin, 48 glycogen, 244 inulin, 47 proteins, 64 starch, 46 sucrose, 41 Hyperacidity, 119 Hypoacidity, 119 Hypobromite solution, preparation of, 375 Hypoxanthine, 236, 245, 265, 294 formula for, 241 Hypoxanthine silver nitrate, crystalline form of, 245 Ichthulin, 87 Ignotine, 236 formula for, 241 Imide bonds, 66 Indican, 162, 279, 312 formula for, 163, 280 Giirber's reaction for, 281 Jaffe's test for, 280 Lavelle's reaction for, 281 Obermayer's test for, 281 origin of, 162, 279 Rossi's reaction for, 281 Indigo-blue, 163, 2.80 formula for, 163, 280 Indigo in urinary sediments, 344, 351 Indole, 162 formula for, 162 origin of, 162 test for, 168 Indole-amino-propionic acid, 73 Indoxyl, 162, 279, 280 formula for, 162, 280 Indoxyl, origin of, 163, 279 potassium sulphate (see Indican, pp. 162-163, 279) Indoxyl-sulphuric acid, 162, 279 formula for, 162, 280 Infraproteins (see Metaproteins, 87) Inorganic physiological constituents of urine, 295 Inosinic acid, 236 formula for, 241 Inosite, 21, 305, 339 formula for, 339 in urine, 305, 339 Intestinal juice, 143 enzymes of, 143 preparation of, 143 Inulase, 47 Inulin, 22, 46 action of amylolytic enzymes on, 47 58. Fehling's test on, 47 hydrolysis of, 47 iodine test on, 47 reducing power of, 46 solubility of, 46, 47 sources of, 46 Inversion, 41, 43 Invertases, experiments on, 11, 144 Invertin (see Sucrase, p. 41) Inverting enzymes, 3 Invert sugar, 41, 144 Iodide of dextrin, 48 of starch, 44 Iodine test, 25, 44, 47, 48 Iodine-sulphuric acid test for cholesterol, 158, 251 Iodoform test for alcohol, 42 Iodothymol compound, 329 Iron in blood, 189, 195 detection of, 195 in bone ash, 234 detection of, 234 Iron in protein, 62 Iron in urine, 265, 303 detection of, 304 Isoleucine, 77 Isomaltose, 21, 40, 55 Jaffe's reaction for creatinine, 278 Jaffe's test for indican, 280 v. Jaksch-Pollak reaction for melanin, 341 Jejunum, epithelial cells of, 140 Jolles' reaction for protein, 98, 316 reagent, preparation of, 98, 316 Juice, gastric, 1 18-122 pancreatic, 140-143 intestinal, 143 Kastle's peroxidase reaction, 222 Kephalin, 248, 250 Kephyr, 40 Keratin, 86, 227 experiments on, 227 solubility of, 227 sources of, 227 sulphur content of, 227 Ketone, 21, 26 Ketose, 21 Kjeldahl method for determination of nitrogen, 381 Knoop's color reaction for histidine, 74 Knop-Hiifner hypobromite method for determination of urea, 374, 376 Konto's reaction for indole, 169, 181 Koppe's electrolytic dissociation theory, 119 [NDEX. Koumyss, 40 Kraut's reagent, preparation of, 253 Kriiger and Schmidt's method for the quantitative de termination of purine bases, |"=, "i uric acid, .?".? Kiilz's test for /3-oxybutyric acid, ,$.u Kynurenic acid, 264, 288 formula for, 288 isolation of, from urine, 289 quantitative determination of, 280 Lactalbumin, 86, 218, 221 quantitative determination of, 1 1 - Lactase, 12, 141, 143 experiments on, 12 Lactic acid, 40, 129, 236 ferric chloride test for, 129 Hopkins' thiophene reaction for, 129 in muscular tissue, 236, 237 in stomach contents, 129, 130 tests for, 129 Uffelmann's test for, 129 Lacto-globulin, 218, 221 Lactometer, determination of specific gravity of milk by, 410 Lactosazone, crystalline form of, Plate III, opposite p. 24 Lactoscope, Feser's, 41 1 Lactose, 21, 40 experiments on, 41 fermentation of, 40 in urine, 305, 336 quantitative determination of, 412 Lactosin in milk, 221 Larvo-a-proline, 80 Lsevulosazone, crystalline form of, Plate III, opposite p. 24 Lsevulose, 21. 35 Borchardt's reaction for, 35 in urine, 305, 338 methyl-phenylhydrazine test for, 35 Seliwanoff's reaction for, 35 Laiose in urine, 305, 340 Laked blood, 182, 193 Laky blood, 195 Laurie acid, 218 Laurin, 132 Lavelle's reaction for indican, 281 Leach's hydrochloric acid test for form aldehyde, 225 Lecithans, 87 Lecithin, 151, 248, 250 acrolein test on, 251 decomposition of, 249 experiments on, 249 formula for, 249 microscopical examination of, 250 osmic acid test on. 250 preparation of, 250 test for phosphorus in, 25J Lecithoproteins, 87. ro8 Legal's reaction for indole, 169 L L egal's ievt for ... . torn ell. 111. , '. : . ; , 76, 141 tallint form >.i impun . pun 1 intents on, x.\ formula for, 76 in urinary sedii micros* opi< ..1 • ■ nation of eparation of fi solubility of, x.j sublimation of, 84 eucocytes, 1 82, 1 o.> counting the, 215 number of, per 1 • 1 J . i « mm., si/.- of, 1 go variation in number of, 190 eucocytosis, [90 eucosin, 96 eucyl alanyl eucyl leucine, formation of, 66 ichenin, 22, 48 ieben's tesl for acetom ieberkuhn's jelly > see Vlkali meta- proti m. p. mm iehermann Burchard test for choles- terol, 158, 251 iebermann's reaction, 93 ipase, gastric, ui ipase, pancreatic. 10, 132 experiments on, i" ethyl-butyrate tesl for, 149 litmus-milk tesl for, 1 (8 1 pases, 3, 10 experiments on, 10 ipoids of nervous tissue. J4X. 250 ipolytic enzymes (see Lipases, !• Litmus milk " test for panereatic lipase, .48 ilgol's solution, preparation .>t. 04 ysine, 63, ~7- '41 ysine picrate, crystalline form of, 78 Magnesia mixture, preparation ol Magnesium in urine. 265, 303 phosphate in urinary sediments 350 Maltase, 13 39, 55. '44 experiments on. 13 Maltosazone, crystalline form "t. Plate 111. opposite p. 24 Malti.se. _'i. 30 experiments on, p. structure of, 30 Marshall's una apparatus, 373 Melanin in urine. 305, urinary -exaluric at id, 36 1. 290 < Ixamide, ( Oxidases, .-.• 1 Oxyacids, [62, 1 '•;, 171 tests for, 171 ,; oxj but) rir acid, Black's method foi determina- tion of, 1 " ', I'.i.m k's r< action for, 332 formula for, ,i.]2 Kiilz's test for, .133 origin of, 332 polariscopic examination I quantitative determination of, 402 Shaffer's method for determina- tion of, 402 Oxyhemoglobin, 62 Reichert's method for crystallization of. 201 crystalline forms of, 186-189 Oxymandelic acid, 264, 288 Oxyproline, 81 Oxyproteic acid. 264, 285. 342 Paduschka-Underhill-Kleiner method for quantitative determination of allantoin. 407 Palmitic acid. 132, 143 crystalline form of, 137 experiments on, 138 formula for, 132, 143 preparation of, 137 Palmitin, 132 Pancreatic amylase, 141, 142. 14; digestion of dry starch by, 143, 148 inulin by, 14X experiments on, 147 influence of bile upon action of, 148 metallic -alts upon 1 1 of. 147 most favorable temperature for action of, 1 IT Pancreatic digestion, 140 general experiments on. 145 products of, 141, 1 »5 Pancreatic insufficiency, Schmidt's nuclei test for, 1 S 1 Pancreatic juice. [40 143 artificial, preparation of, I4J daily excretion of, M' enzymes of, 141 freezing point of, > 41 mechanism of secretion «i. 14° reaction of, 140 solid content of, 1 41 Specific e,r.i\ ity of, 14' Pancreatic lipase. 13a, 14 >• 143 ( xperiments on 440 INDEX. Pancreatic lipase, ethyl-butyrate test for, 149 litmus-milk test for, 148 Pancreatic protease (see Trypsin, p. 1) Pancreatic rennin, 141, 143 experiments on, 149 Papain, 10 Para-cresol-sulphuric acid, 264, 279 Paradimethylamino benzaldehyde solu- tion, preparation of, 170 Paralactic acid, 237, 265, 291 Paramyosinogen, 235 Paranucleoprotagon, 248, 250 Paraoxyphenylacetic acid, 162, 168, 264, 287 Paraoxyphenyl-a-amino-propionic acid, Paraoxyphenylpropionic acid, 162, 168, 264, 287 Paraphenelenediamine hydrochloride, 226 Parasites, 175, 351. 361 Paraxanthine, 265, 294 Parietal cells, 119 Parotid glands, characteristics of saliva secreted by, 53 Pathological constituents of urine, 305 Pathological urine, 254, 305 constituents of, 305 experiments on, 305-342 Pektoscope, 260 Pentapeptides, 88 Pentoses, 21, 37 experiments on, 37 in urine, 305, 335 tests for, 33s Pepsin (see Gastric Protease), 2, 9, 120 action of, influence of bile upon, 128 influence of different acids upon, 85 metallic salts upon, 127 temperature upon, 126 conditions essential for action of, 120 differentiation of, from pepsinogen, 126 formation of, 120 digestive properties of, 120 most favorable acidity for action of, 120 proteolytic action of. 120 Pepsin-hydrochloric acid, 125-127 Pepsinogen, 5, 120, 122 differentiation of, from pepsin, 126 formation of, 120 extract of, preparation of, 122 Peptic activity, Fuld and Levison's method for determination of, 18 Mett's method for the deter- mination of, 17 Peptic proteolysis, 120 products of, 120 relation of, to tryptic proteolysis, 121 Peptides, 64, 66, 88, 114, 115 Peptone, 63, 88, 89 ampho, 88, 89 Peptone, anti, 88, 89 differentiation of, from proteoses, 114 experiments on, 115 in urine, 305, 319 tests for, 319 separation of, from proteoses, 114 Periodide test for choline, 252 Peroxidases, 221 Pettenkoper's test for bile acids, 156, 325 Mylius's modification of, 156, 326 Neukomm's modifica- tion of, 156, 326 Phenaceturic acid, 265, 291 Phenol, 162 tests for, 170 Phenolphthalein as indicator, 124 preparation of, 124 Phenol-sulphuric acid, 264. 279 Phenyl-a-amino propionic acid, 69 Phenylalanine, 63, 69 Phenyldextrosazone, 24 crystalline form of, Plate III, op- posite p. 24 Phenylhydrazine. 24, 25 acetate solution, preparation of, 24 mixture, preparation of, 24 reaction, 24 Cipollina's modification of, 25 Phenyllactasazone, crystalline form of, Plate ill, opposite p. 24 Phenylmaltosazone crystalline form of, Plate III, opposite p. 24 Phenylpotassium sulphate, 279 Phosphates in urine, 265, 299 detection of, 301 experiments on, 301 quantitative determination of, 389 Phosphatides, 87, 151 Phosphocarnic acid, 236, 241, 265, 292 Phosphoproteins, 87, 88, 107 Phosphorized compounds in urine, 265, 291 Physiological constituents of urine. 264 Pigments of urine, 254, 265, 292 Pine wood test for indole, 169 Piria's test for tyrosine, 83 Polariscope, use of, 32 in detection of conjugate glycur- onates, 334 in determination of dextrose, 32 /3-oxybutyric acid, 333 Polypeptides, 64, 66 Polysaccharides, 22, 43 classification of, 22 properties of, 43 Posner's modification of biuret test, 93 Potassium in urine, 265, 302 Potassium indoxyl-sulphate (see Indican, pp. 162, 280) formula for, 163, 280 origin of, 162, 179 tests for, 280 Primary protein derivatives, 87 Primary proteoses, 114 [NDEX. 44 ' Products of protein hydrolysis, 63, <>; Prolamins, 105 classification of, 87, 88 Proline, 63, 80, 105, 141 crystalline form of laevo-o-, 80 crystalline form of copper salt of, Bi Prosecretin, 140 Protagon, 248, 249 preparation of, 250 Protamines, classification of, 86 Proteans, 87, 108 Protease, gastric, 9 experiments on, 9 pancreatic, 9 experiments on, 9 vegetable, 10 Proteases, 9 experiments on, 9 Proteins, 61 acetic acid and potassium ferro- cyanide test for, 99 Acree-Rosenheirn test on, 93 action of alkaloidal reagents on, 97 action of metallic salts on, 97 mineral acids, alkalies and or- ganic acids on, 96 Adamkiewicz reaction on, 91 Bardach's reaction on, 94 biuret test on, 91 chart for use in review of, 117 chemical composition of, 61 classification of, 85, 86, 88 coagulation or boiling test for, 99 color reactions of, 90 conjugated, 87, 89, 106 decomposition of, 62 by hydrolysis, 63 by oxidation, 6^ products of, 63 experiments on, 82 separation of, 82 study of, 63, 82 derived, 87 formation of fat from, 134 formulas of, 62 Heller's ring test on, 97 importance of, to life, 61 Hopkins-Cole reaction on, 91 in urine, 305, 313 test for, 314 Liebermann's reaction on, 93 Millon's reaction on, 90 molecular weights of, 62 Posner's reaction on, 93 precipitation of, by alcohol, 100 alkaloidal reagents, 97 metallic salts, 97 mineral acids, 96 precipitation reactions of. 95 quantitative determination of, in milk, 412 review of. 11 5 Robert's ring test on, 97 salting-out experiments on, 99 scheme for separation of, 116 simple, 86, 89 Proteins, Bynthi xanthoproteii rea< tion on, 91 Protein . 1 oagulated, 1 1 1 biuret 11.' foi mation of, 1 1 1 I lopkint < ole rea< tion on, 1 1 2 Millon's reai tion on, 1 1 2 solubility of, in, iu xanthoproti in on, 112 I '1 otein coagulated • Proteins 1 onjugated, 87, classes of, 87, 106 experiment on, 1 95, 196 201, 203, -'-".! nomenclature of, 87 0) 1 urrence of, 106 Protein cystine, 73 Protein derivatives, primarj I secondary, 63, 1 1 3 Proteins of milk, 218, 220, 221 quantitative determination of, 412 Proteolytic enzj Proteolysis, peptic, t20 tryptic, ij 1 Proteose, 63, 88, 89, 113 v. Aldor's method for detection of, 320 biuret tCst on, i 15 gulation test on, 1 1 5 deutero, 88, 89. 1 1 3 differentiation of, from peptone, 114 experiments on. 1 1 5 hetero, 89, 113 in urine, 305, 313, 319 test for, 319 potassium ferrocyanide and acetic test on. l 1 s powder, preparation of, 1 14 precipitation of. by nitric acid, 115 by picric acid. 1 1 5 by potassio mercuric iodide, 115 by trichloracetic acid, 1 15 primary. 1 14 proto, 88, 89. 1 1 3 Schulte's method for detection of, 319 secondary. 1 14 separation of, from peptones, 114 Protoproteose. 88, 89 Proteoses and peptones, 88, 89, 113 separation of, 114 tests on, 114 Proteose-peptone. 114 Proteose-peptone, coagulation test on, 114 experiments on, 1 1 4 Millon's reaction on, 1 1 { precipitation of, by nitric acid. 114 by picric acid. 1 14 Prothrombin. 191, 192 Pseudo globulin, 182, 183, Ptomaines and leucomaines in urine 294 Ptyalin (see Salivarj amj Purdy's method t'..r determination if dea trose 442 INDEX. Purdy's solution, preparation of, 370 Purine bases, 107, 405 in urine, quantitative determination of, 405 Pus casts in urinary sediments, 351, 359 Pus cells in urinary sediments, 351, 353 Putrefaction, indican as an index of, 162, 279 Putrefaction mixture, preparation of a, 164 Putrefaction products, 162 experiments on, 164 most important, 162 tests for, 168 Pyloric glands, 118 Pyrocatechin-sulphuric acid, 264, 279 cc-pyrrolidine-carboxylic acid (see Prolin, p. 80) Qualitative analysis of the products of salivary digestion, 60 stomach contents, 129 Quantitative analysis of blood, 415 of gastric juice, 413 of milk, 410 of urine, 366 Quantitative determination of ammonia in urine, 380 amylolytic activity, 16 acetone in urine, 400 acetone and diacetic acid in urine, 397 acidity of urine, 404 allantom in urine, 407 ash of milk, 411 caseinogen of milk, 412 chlorides in urine, 394 creatine in urine, 393 creatinine, 392 dextrose in urine, 367 diacetic acid in urine, 401 fat in milk, 410 hippuric acid in urine, 383 indican in urine, 393 lactalbumin in milk, 412 lactose in milk, 412 nitrogen in urine, 381 oxalic acid in urine, 408 /3-oxybutyric acid in urine, 402 peptic activity, 17 phosphorus in urine, 389 protein in milk, 412 protein in urine, 366 purine bases in urine, 405 sulphur in urine, 384 total solids in milk, 411 total solids in urine, 408 tryptic activity, 19 urea in urine, 374 uric acid in urine, 372 Quevenne lactometer, determination of specific gravity of milk by, 410 Raffmose, 22, 43 Rancid fat, 133 Reaction of the urine, 256, 300 Reduced alkali-haematin, 206 Reduced haemoglobin, 203 Reductases, 221 Reichert's method for crystallization of oxyhemoglobin, 201 Remont's method for detection of sali- cylic acid and salicylates, 226 Rennin, gastric, 121 action of, upon caseinogen, 121 experiments on, 128, 130 influence of, upon milk, 121, 128 in gastric juice, absence of, 121 nature of action of, 121 occurrence of, 121 Rennin, pancreatic, 141, 143 experiments on, 149 Reticulin, 106 Reversibility of enzyme action, 6, 55 Reynolds-Gunning test for acetone, 329 Rhamnose, 21, 38 Ricin, 10, 196 Ring test for urobilin, 294 Roaf's method for crystallizing hippuric acid, 283 Robin's reaction for urorosein, 341 Robert's ring test for protein, 97, 315 reagent, preparation of, 97, 315 Rosenheim's bismuth test for choline, 253 Rosenheim's periodide test for choline, 252 Rossi's reaction for indican, 281 Rubner's test for lactose in urine, 337 Saccharide group, 22 Saccharose (see Sucrose) Sahli's desmoid reaction, 127 Saliva, 53 alkalinity of, 54 amount of, 54 bacteria in, 55 biuret test on, 56 calcium in, 54 chlorides in, 57 constituents of, 54 digestion of dry starch by, 58 digestion of inulin by, 58 digestion of starch paste by, 55, 58 enzymes contained in, 54, 55 excretion of potassium iodide in, 60 inorganic matter in, tests for, 57 Millon's reaction on, 56 mucin from, preparation of, 56 nitrites in, test for, 57 phosphates in, test for, 57 potassium thiocyanate in, 54 reaction of, 54, 56 secretion of, 53 specific gravity of, 54, 56 sulphates in, test for, 57 thiocyanates in, 54 tests for, 57 Salivary amylase, 1, 54, 119 activity of, in stomach, 55, 119 inhibition of activity of, 55 nature of action of, 54 products of action of, 55 [NDEX. Salivary digestion, 53 influence of acids and alkalis on, 55. 59 dilution on, 59 metallic salts on, so temperature on, 58 nature of action of acids and alkalis on, 59 qualitative analysis of products of, 60 Salivary digestion in stomach, 55, 119 Salivary glands, 53 Salivary stimuli, 53 Salkowski-Autenrieth-Barth method for determination of oxalic acid in urine, 408 Salkowski's method for determination of purine bases, 407 Salkowski-Schippers reaction for bile pigments, 155. 325 Salkowski's test for cholesterol, 158, 252 for creatinine, 278 Salmine, 87, 88 Salted plasma, preparation of, 201 Salting-out experiments on proteins, 95, 99 Sarcolactic acid, 237 Scallops, preparation of glycogen from, 244 . Schalfijew's method for preparation of hsemin, 199 Scheme for analysis of biliary calculi, 158 bone ash, 234 stomach contents, 130 urinary calculi, 364 separation of carbohydrates, 51 of proteins, 116 Scherer's coagulation method for deter- mination of albumin in urine, 366 Schiff's reaction for cholesterol, 159, 252 for uric acid, 275 Schiff's reagent, preparation of, 159, 252 Schmidt's nuclei test for pancreatic in- sufficiency, 181 Schmidt's test for hydrobilirubin, 179 Schulte's method for detection of pro- teose in urine, 319 Schumm's modification of the guaiac test, 196 Schiitz's law, statement of, 7, 18 Schweitzer's reagent, action of, on cel- lulose, 50 preparation of, 50 Scleroproteins, 85 (see Albuminoids) Scombrine. 87 Scombrone, 86, 88 Secondary protein derivatives, 88 Secondary proteoses, 114 Secretin, 140 Seliwanoff's reaction, 35, 339 reagent, preparation of, 35, 339 Separation ot feces, importance of. in nutrition and metabolism experiments, 174 Serine, 63. 69 crystalline form of, 69 Serine, formula for, Serum albumin, 81 in .11111. . Serum globulin, in 111 111. . |OS, 318 test t'.r, 318 Shaffer's method for determination of ii oxybutj rii a. id, Sherman's compressed 1 -hod fur determination ulphur in ur in. Sherrington's solution, preparation - ' •' Silicates in urine, 265, .',., 1 SI al..l. !, [62, 1 70 for, 1 ;.. Skatole-carbonic acid, 167 test for, 171 Smith's test for bile pigments, 155, 325 Soap, salting-out of, 137 Soaponilii atioii, 132 of lard, 138 Sodium and potassium in urine. J65, 302 Sodium alizarin sulphonate as indii 125 preparation of, 125 Sodium chloride, crystalline form. 200 Sodium chloride in urine, 265, 298, 394 Sodium hydroxide and potassium nitrate fusion method for determination of total sulphur and phosphorus in urine, 3&7. 390 Sodium hypobromite solution, prepara tion of, 375 Sodium sulphide solution, preparation of, 406 Solera's reaction for detection of thio- cyanate in saliva, 57 test paper, preparation of, 57 Soluble starch, 8, 54 Soxhlet apparatus for extraction of fat. 41 o Soxhlet lactometer, determination of specific gravity of milk by, 410 Specificity of enzyme action, 6 Spectroscope, use of, in detection of blood, 323 Spermatozoa in urinary sediments, 351, 360 microscopical appearance of human. 360 Spiegler's rim; tesl for protein, 98, 316 reagent, preparation of, 98, 3'6 Sprigg's method for determination of peptic activity, 17 Standard ammonium thiocyanate solu- tion, preparation ol ntic nitrate solution, prepara tion of, ;w> uranium lution, prepara tion of, 389 Starch. 22, 4.? action of alcohol on iodide ol action of alkali on iodide ol heat on iodide of, I" 444 INDEX. Starch, dry, digestion of, by pancreatic amylase, 143, 148 dry, digestion of, by salivary amy- lase, 58 experiments on, 44 iodine test for, 44 microscopical characteristics of, 43 microscopical examination of, 44 potato, preparation of, 44 soluble, 54 solubility of, 44 various forms of, 45 Starch group, 22 Starch paste, action of tannic acid on, 46 diffusibility of, 46 digestion of, by pancreatic amy- lase, 142, 147 by salivary amylase, 54, 58 Fehling's test on, 46 hydrolysis of, 46 iodic acid paper, 58 preparation of, 44 Steapsin (see Pancreatic lipase, 132) Stearic acid, 249 Stearin, 133 Stellar phosphate, 224, 345 Stercobilin, 173 Stokes' reagent, action of, 203, 206 preparation of, 203 Stomach, motor and functional activities of, 128 Stomach contents, lactic acid in tests for, 129 qualitative analysis of, 129 Stone-cystine, 73 Sturine, 87 Sublingual glands, characteristics of saliva secreted by, 53 Submaxillary glands, characteristics of saliva secreted by, 53 Substrate, 2, 6 Sucrase, 11, 144 experiments on, 11 vegetable, 1 1 Sucrose, 21, 41 experiments on, 42 inversion of, 41 production of alcohol from, 42 structure of, 42 Sulphanilic acid, 342 Sulphates in saliva, test for, 57 Sulphates in urine, 265, 296 experiments on, 297 ethereal, 279, 296 quantitative determination of, 386 inorganic, 296 quantitative determination of, 385 _ . total, quantitative determination of, 384 Sulphocyanides (see Thiocyanates, 54) Sulphur in protein, 102 loosely combined, test for, 102 in urine, quantitative determination of, 384 Sulphur in acid, 102 lead blackening, 102 mercaptan, 102 neutral, 296 oxidized, 102 unoxidized, 102 Suspension of manganese dioxide, 406 Tallow bayberry, saponification of, 136 Tallquist's haemoglobin scale, determina- tion of haemoglobin by, 212 Tannic acid, influence of, on dextrin, 49 on starch, 46 Tannin test for carbon monoxide haemo- globin, 205 Tanret's reagent, preparation of, 98, 317 Tanret's test, 98 Tartar, formation of, 54 Taurine, 151, 240 derivatives, 264 formula for, 151, 240 preparation of, 159 Taurocholic acid, 151 group, 151 Taylor's test for acetone, 329 Teichmann's crystals, form of (see Haemin crystals, p. 198) Tendomucoid, 87, 106, 228 biuret test on, 229 chemical composition of, 106 hydrolysis of, 229 loosely combined sulphur in, test for, 229 preparation of, 228 solubility of, 229 Tetrapeptides, 88, 89 Thiocyanates in saliva, significance of, 54 ferric chloride test for, 57 Solera's reaction for, 57 Thiocyanates in urine, 264, 285 Thiophene, 129 Thoma-Zeiss haemocytometer, 212 Thrombin, 191, 192 Thymus histone, 86 Thymol, formula for, 262 interference of, in Lieben's acetone test, 329 interference in Heller's ring test, 315 use of, as preservative, 262 Tincture of iodine, preparation of, 424 Tissue, adipose, experiments on, 131, 234 connective, 2.2"] white fibrous, 227 composition of, 228 experiments on, 228 yellow elastic, 230 composition of, 230 experiments on, 231 epithelial, 227 experiments on, 227 muscular, 235 experiments on, 241 nervous, 248 experiments on, 250 osseous, 233 INDEX. Tissue, osseous, experiment on, 233 Tissue debris in urinary sediments, 351, 361 . Toison's solution, preparation of, 21 1 Tollen's reaction 011 conjugate glycuro nates, 33 1 galactose, 36 arabinose, 37 Topfer's method for quantitative analysis hi gastric juice, 41 3 Topfer's reagent, as indicator, i_>3 preparation of, 123 Total solids, of milk, quantitative deter initiation of, 41 1 of urine, quantitative determina tion of, 408 Total sulphur of urine, quantitative de- termination of, 386-389 phosphorus of urine, quantitative determination of, 390 Tri-butyrin, 218 Trimethyl-oxyethyl-ammonium hydroxide (see Choline, 248) Tri-olein, 133, 218 Tri-palmitin, 132, 143, 218 Tri-stearin, 133, 218 Trichloracetic acid, precipitation of pro- tein by, 97 Trioses. 22 Tripeptides, 88, 89 Triple phosphate, 247, 301, 344 crystalline form of, 301 formation of, 301 Trisaccharides, 2.2, 43 Trommer's test, z"j Tropaeolin 00, as indicator. 124 preparation of, 124 Trypsin (see also Pancreatic protease, 1 1 ■» action of, upon proteins, 64 experiments on, 145 influence of alkalis and mineral acids upon, 141 nature of, 141 pure, preparation of, 141 Trypsinogen, 5, 141 activation of. 142 Tryptic digestion, 140 influence of bile on, 146 metallic salts on, 146 most favorable reaction for, 145 temperature for, 146 products of, 14'. T45 Tryptic proteolysis, 121, 141 Tryptophane, 63, 73, 141, 145 bromine water test for, 145 formula for. 73 group in the protein molecule. 91 Hopkins-Cole reaction for. 91 occurrence of, as a decomposition product of protein, 63, 73 occurrence of. as an end-product of pancreatic digestion, 141. 1 451 "Twinning" of oxyhemoglobin crystals, 190 Tyrosine, 63. 70, 90, 141 1 1 imenti on, x.\ formula 1 l [offmann'i rea< tion 1 in urinary sedii mil roscopii d • ■• amination oi Morner'i t> si 1 ■ ■I 1 uri iip • Piria'a test tor, 83 sails of, 71 separation of, from solubility ol sublimation of, x.i Tyrosine sulphui ii \ . I Idranskj 's test for bile a< id rficlni.mn's reagent, preparation ol reaction for lactic acid, 1 .•■; Unknown substances in urine, Unorganized ferments, 1 Uranium acetate method for detei tion of total phosphates in urine, 389 Uracil, 107 Wheeler-Johnson reaction for, I 'rate, ammonium, crystalline form of, Plate VI, opposite p. 348 sodium, crystalline form of, 348 Urates in urinary sediments, 344. Urea, 264, 265 crystalline form of, 266 decomposition of, by sodium hyp" bromite, 268, 271 excretion of, 266 experiments on. 269 formation of, 267 formula for, 265 furfurol test for, 271 isolation of, from the urine. 269 melting-point of, 269 quantitative determination of, 374 Urea nitrate, 270 crystalline form of, 268 formula for, 268 oxalate, 270 crystalline form of, 270 formula for, 268 Urethral filaments in urinary sediments. 35*1 360 Uric acid. 28, 236, 241, 264, 271 stalline form of pun endogenous ■ Molls, 27a experiments on, formula for. 271 in leukaemia, 273 in urinary sedimi I crystalline torm of Plate V, opposite ; "on of, from the urir Moreigne's n action for, murexide test t'..r. origin of, quantitative determinati 3T- Folin Schaffer mi for, 446 INDEX. Uric acid, quantitative determination of, Heintz method for, 373 Kriiger and Schmidt's method for, 373 reducing power of, 28 Schiff's reaction for, 275 Uricolytic enzymes, 3, 14 experiments on, 14 Urinary calculi, 362 calcium carbonate in, 363 oxalate in, 363 cholesterol in, 365 compound, 362 cystine in, 363 fibrin in, 363 indigo in, 365 phosphates in, 363 scheme for chemical analysis of, 364 simple, 362 uric acid and urates in, 363 urostealiths in, 363 xanthine in, 363 Urinary concrements (see Urinary calculi, p. 362) Urinary concretion (see Urinary calculi, p. 362) Urination, frequency of, 256 Urinary sediments, 343 ammonium magnesium phos- phate in, 344 animal parasites in, 351, 361 calcium carbonate in, 345 oxalate in, 344 phosphate in, 345 sulphate in, 346 casts in, 351, 354 cholesterol in, 349 collection of, 343 cylindroids in, 359 cystine in, 348 epithelial cells in, 351, 352 erythrocytes in, 351, 360 fibrin in, 351, 361 foreign substances in, 351, 361 hffimatoidin and bilirubin in, 344,350 _ hippuric acid in, 349 indigo in, 344, 351 leucine and tyrosine in, 344, 349 magnesium phosphate in, 344, 35o_ melanin in, 344, 351 micro-organisms in, 351, 361 organized, 343 pus cells in, 351, 353 spermatozoa in, 351, 360 tissue debris in, 351, 361 unorganized, 343, 351 urates in, 344, 347 urethral filaments in, 351, 360 uric acid in, 346 xanthine in, 344, 350 Urine, 254-409 acetone in, 327 acidity of, 256, 300 Urine, acid fermentation of, 258 albumin in, 305, 314 alkaline fermentation of, 256 alantoin in, 264, 285 ammonia in, 257, 265, 295 aromatic oxyacids in, 264, 287 benzoic acid in, 264, 289 bile in, 324, 325 blood in, 305, 321 calcium in, 303 carbonates in, 265, 303 chlorides in, 265, 298 collection of, 262 conjugate glycuronates in, 305, 334 color of, 254 creatinine in, 264, 275 dextrose in, 305 diacetic acid in, 305, 331 electrical conductivity of, 261 enzymes in, 265, 290 ethereal sulphuric acid in, 264, 279 fat in, 305, 335 fluorides, in, 265, 298, 394 freezing-point of, 260 galactose in, 305, 337 general characteristics of, 254 globulin in, 305, 318 Haser's coefficient for solids in, 259, 409 hsematoporphyrin in, 305, 336 hippuric acid in, 282, 349 hydrogen peroxide in, 265, 304 inorganic physiological constituents of, 295 inosite in, 305, 339 iron in, 265, 303 lactose in, 305, 336 lsevulose in, 305, 338 laiose in, 305, 340 leucomaines in, 265, 294 Long's coefficient for solids in, 259, 409 magnesium in, 265, 303 melanin in, 305, 340 neutral sulphur compounds in, 285 nitrates in, 265, 304 nucleoprotein in, 264, 290, 305, 320 odor of, 256 organic physiological constituents of, 264 oxalic acid in, 264, 284 oxaluric acid in, 264, 290 /3-oxybutyric acid in, 332, 402 pathological constituents of, 305 paralactic acid in, 237, 265, 291 pentoses in, 305, 335 peptone in, 305, 319 phenaceturic acid in, 265, 291 phosphates in, 265, 299 phosphorized compounds in, 265, 291 physiological constituents of, 264 pigments of, 254, 265, 292 potassium in, 265, 302 proteins in, 305, 313 proteoses in, 305, 313, 319 ptomaines in, 265, 294 [NDEX. Urine, purine bases in, jos quantitative analysis (if, 366 reaction of, 256, 300 silicates in, 265, 304 sodium in, 265, 302 solids of, 259, 408 specific gravity of, 258 sulphates in, 265, 296 transparency of, 255 unknown substances in, 305, 342 urea in, 264 uric acid in, 264, 271 urorosein in, 305, 341 volatile fatty acids in, 265, 290 volume of, 254 Urobilin, 254, 265, 292 tests for, 293 Urochrome, 254, 292 Uroerythrin, 10, 254, 292, 312 Uroferric acid, 264, 285, 342 Uroleucic acid, 264, 288 Urorosein, 305, 341 tests for, 341 Valine, 75 Vegetable amylase, 9 lipase, 10 protease, 9 sucrase, 11 Vegetable globulins, 86 Vegetable gums, 22 Veith lactometer, determination of specific gravity of milk by, 410 Viscosity test, 57 Vitellin, 87, 88 Volatile fatty acids, 162, 165, 265, 290 Volhard-Arnold method for determina- tion of chlorides, 396 Volume of the urine, 254 Wax myrtle, 136 Waxy casts in urinarv sediments, 351, 358 WYImt's guaiai blood in ■■ 17H Weinland, formatioi for en atinine, 278 Wheeler [ohnson reaction for uracil and to itn . 1 ■■; White fibrous 1 onne< live ti Wirsin r urobilin Wohlgemuth's method for quantil determination <•( amylolytic activity, \(> Xanthine, 241 crystalline form of, 239 formula for. 241 in urinary sediment - isolation of, from m. at • Weidel's reaction for. 247 Xanthine bases (see Purine bases, pp. 107, 40s) Xanthine siher nitrate, 246 crystalline form of. 247 Xanthoproteic reaction, 91 Xylose, 21, 38 orcin reaction on, 38 phenylhydrazine reaction on, 38 Tollens' reaction on. 37 Yellow elastic connective tissue composition of, 230 experiments on, 231 Zappert slide, 216 Zein, 105 Zeller's test for melanin, 341 v. Zeynek and Nencki's hxmin test. 199. 322 Zikel pektoscope, 260 Zymase, preparation of, 2 Zymo-exciter, 5 Zymogen, 5, 120 H31 siological chemistry