ALBERT R. MANN 
 LIBRARY 
 
 New York State Colleges 
 
 OF 
 
 Agriculture and Home Economics 
 
 AT 
 
 Cornell University 
 
Cornell University Library 
 QD 85.W5 
 Tables for qualitative Shemte^^^^^^^ 
 
The original of tiiis book is in 
 tine Cornell University Library. 
 
 There are no known copyright restrictions in 
 the United States on the use of the text. 
 
 http://www.archive.org/details/cu31924003684895 
 
TABLES 
 
 FOR ' 
 
 QUALITATIVE 
 
 CHEMICAL ANALYSIS 
 
 WITH AN 
 
 INTRODUCTORY CHAPTER 
 
 ' 02Sr THE 
 
 COURSE OF ANALYSIS. 
 
 BY 
 
 Professor HEIMICH WILL, 
 
 OF GIESSEN, GEKMANT. 
 
 THIRD AMERICAN, FROM THE ELEVENTH GERMAN EDITION. 
 
 EDITED BY 
 
 CHARLES F. HIMES, Ph.D., 
 
 PROFESSOR OF NATURAL BOIEHOE, DICKISSOH COLLEGE, CARLISLE, PA. 
 
 PHILADELPHIA: 
 HENRY CAREY BAIRD & CO., 
 
 INDUSTRIAL PUBLISHERS, BOOKSELLERS, AND IMPORTERS, 
 
 810 "WALNUT STREET. 
 
 1881. 
 
Copyright by 
 
 HENRY CARET BAIRD & CO. 
 
 1881. 
 
 COLLINS, PRINT EB. 
 
EDITOR'S PREFACE. 
 
 The growing opinion in favor of increased attention to the 
 study of Natural Science, as a branch of liberal education, on 
 account of its disciplinary value, as well as the practical character 
 of the knowledge acquired, led to a modification of the curriculum 
 of study required for the degree of Bachelor of Arts in this in- 
 stitution, in so far as to allow of the election of more extensive 
 and practical study of Natural Science in lieu of the Latin and 
 Greek of the Junior and Senior years. The expectation is not in 
 this way to turn out Bachelors of Arts as chemists, etc., but 
 simply to make this branch of a liberal education as thorough as 
 the times seem to demand, and to afford a foundation, if desired, 
 for subsequent scientific pursuits. 
 
 In adapting a course of chemical analysis to this purpose the 
 accompanying tables seemed peculiarly suited. Whilst compact, 
 they are sufHcientl^' explicit, and the summary view of the gene- 
 ral course of qualitative analysis, and of the classification of com- 
 pounds according to the properties relied upon for their detection, 
 afibrds a thread, as it were, around which ciiemical facts may 
 crystallize as they accumulate. 
 
 For details of properties, etc., in addition to instruction in the 
 laboratory, the student is constantly referred to some one of the 
 manuals of analytical chemistry placed in the laboratoiy for this 
 purpose. 
 
 Whilst these tables seem thus well adapted to a course of college 
 studies, their general popularity, as well as scientific character, is 
 indicated bj' their extensive adoption in the German universities, 
 and their indorsement by many of the most eminent chemists in 
 this country, and their introduction, iij part at least, into many 
 laboratory handbooks. 
 
 The second American edition, prepared from the ninth German 
 edition, contains, besides the marks of careful revision, two new 
 tables by the author embodying Bunsen's valuable flame reactions. 
 
4 editor's pkefacb. 
 
 and whilst nothing in the original has been omitted or changed, 
 new matter has been freely added by the editor, generally placed 
 in [ J. Thus other methods for the separation of the alkaline 
 earths are given, and an additional table (XIY), which may re- 
 place parts of Tables VI and VIII with the advantage of greater 
 simplicity and directness. The note in regard to the detection 
 of titanic acid is inserted on account of its frequent occurrence 
 in iron ores. The chapter on the "Course of Analysis," from 
 the original, is added with the hope that it may relieve any incon- 
 venience in directing the use of the tables. 
 
 In adopting a new nomenclature for a book of this character, 
 compactness, completeness, and general intelligibility have been 
 mainly considered. 
 
 Acknowledgment is made to many practical instructors for 
 suggestions, especially to Professor P. A. Genth, of the Univer- 
 sity of Pennsylvania. 
 
 CHAKLES F. HIMES. 
 
 Dickinson College, Carlisle, Pa., 1874. 
 
 \ 
 The third American edition, from the eleventh Grei-man edition, 
 contains, besides a few changes and additions by the author, some 
 verbal changes that may render it more readily intelligible, and 
 such modifications of nomenclature as may cause it to confoi'm 
 more fully to what seems most general usage in text-books and 
 books of reference. 
 
 C. F. H. 
 
 Dickinson College, 1881. 
 
CONTENTS. 
 
 Course of Qualitative Chemical Analysis, page ' 
 
 Table 
 
 I. 
 
 Preliminary Examination. — Behavior of solid inorganic sub- 
 stances at a high temperature, alone and with reducing agents. 
 
 Preliminary Examination. — Flame reactions. 
 
 Preliminary Examination. — Flame reactions (Incrustations). 
 
 Preliminary Examination. — Behavior of metallic- oxides with 
 phosphorus salt and borax. 
 
 Fluxing. — Conversion of insoluble compounds into soluble. 
 
 Detection of Metallic Oxides. — General statement of their be- 
 havior with hydrochloric acid, 'hydrogen sulphide, ammonic 
 sulphide, ammonia, and ammonic carbonate. 
 
 Detection of Metallic Oxides. — Treatment of the precipitate ob- 
 tained by hydrogen sulphide. 
 
 Detection of Metallic Oxides. — Treatment of the precipitate ob- 
 tained by ammonic sulphide. 
 
 and X. Detection of Metallic Oxides. — IX. Treatment of the 
 precipitate obtained by ammonic carbonate, (carbonates of the 
 alkaline earths.) X. Treatment of the fluid which is not pre- 
 cipitated by hydrogen sulphide, ammonic sulphide, or ammonic 
 carbonate (magnesia and the alkalies). 
 
 Detection of Acids or Halogens. Preliminary Examination. — 
 Behavior of the more important acids, upon heating their salts 
 with concentrated sulphuric acid. 
 
 Detection of Acids. — Behavior of the more important acids with 
 the precipitants, hydrochloric or nitric acid, baric chloride, 
 calcic chloride, and magnesic sulphate. 
 
 Detection of Acids. — Behavior of the more important acids with 
 ferric chloride, argentic nitrate, and indigo solution. 
 
 [Table XIV. Detection of Metallic Oxides. — Additional method for the treat- 
 ment of the filtrate from the precipitate by HjS, that may replace 
 portions of Tables VI and VIII.] C. F. H. 
 
 Table 
 
 II. 
 
 Table 
 
 III. 
 
 Table 
 
 IV, 
 
 Table 
 
 V. 
 
 Table 
 
 VI. 
 
 Table 
 
 VII. 
 
 Table VIII. 
 
 Table 
 
 IX. 
 
 Table XI. 
 
 Table XII. 
 
 Table XIII. 
 
COURSE OF QUALITATIVE CHEMICAL ANALYSIS. 
 
 I. Preliminary Examination and Solution of Solids. — In the 
 qualitative examination of a solid, its general nature must first of 
 all be ascertained. This is accomplished by an examination in 
 the dry way, which always necessarily precedes the qualitative 
 analysis proper, in the wet way, and which includes with the care- 
 ful observation of its physical characteristics (form, color, lustre, 
 hardness, specific gravity, etc.) that of its deportment at high 
 ternperatures, either alone, with access of air, in the flame, or in 
 the presence of other compounds, which may effect its decompo- 
 sition or solution. The preliminary examination is conducted 
 according to Tables I to IV, and serves not only to determine 
 the general chemical nature of the body, and the quality of the 
 metals and metallic oxides, but may also indicate the quality of 
 some metalloids. Table XI serves exclusively for tiie prelimi- 
 nary examination for acids, and especially for volatile acids, or 
 such as afford volatile products of decomposition with concentrated 
 sulphuric acid. 
 
 These tabular statements require no elucidation for their appli- 
 cation, as they explain themselves, and continued practical em- 
 ployment of them will impart the necessary degree of certainty 
 to conclusions obtained by means of them. After the determina- 
 tion of the class of compounds, to which the substance under 
 examination belongs, hy the preliminary examination in the dry 
 way, the conversion of. it into the liquid form, alone suitable for 
 analysis in the humid way, must be considered. In many cases 
 this operation must be preceded bj' the preparation of the sub- 
 stance, bj' giving it the form best adapted to solution. If its 
 nature permits, it must be finely pulverized, and sometimes also 
 elutriated. This is especially indispensable with minerals, espe- 
 cially with silicates, as well as with all other compounds that are 
 difficultly soluble, insoluble, or decomposable with difficulty. 
 
8 COURSE OF QUALITATIVE CHEMICAL ANALYSIS. ' 
 
 It must then first be ascertained whether the substance is wholly 
 or partially soluble, or totally insoluble iii water. If partially 
 soluble, the filtrate from the undissolved portion will leave a 
 clearly perceptible residue, when evaporated on clean platinum 
 foil or in a capsule, whilst if totally insoluble no such residue 
 will be left. The reaction of the aqueous solution, whether it be 
 neutral, acid, or alkaline, must also be determined by test-paper. 
 If the substance dissolves only partially in water, the constituents 
 of the dissolved and undissolved portions must be ascertained 
 separately. If it is insoluble in water, the effect of dilute and 
 concentrated hydrochloric acid must be tried, whilst note is taken 
 of any evolution of gas in the operation; carbonates develop 
 COj with effervescence; superoxides or c/iromates, chlorine gas; 
 cyanides, prussic acid; many sulphides, H^S ; sulphites and hypo- 
 sulphites, SO^, the latter with the separation of sulphur; some 
 reguline metals (Zn, Fe, Sn, etc.) develop hydrogen gas with HCl, 
 or, in presence of arsenic, arsenetted hj'drogen ; in presence of 
 antimony, antimonetted hydrogen. J|' solution in -HCl is only 
 partial, as a rule a separation of one or more constituents is 
 effected by it, and the insoluble residue must be separated from 
 the liquid, and dissolved by further treatment (Table Y). A sub- 
 stance (or the residue) insoluble in HCl, must be treated with 
 nitric acid or aqua regia. Many sulphides yield, with nitric acid, 
 sulphur, which by sufficiently prolonged action collects as yellow 
 globules, or disappears entirely, when newly formed sulphuric 
 acid is always detected, unless the metallic oxide produced forms 
 a compound with it insoluble in the acid. 'Yhns plumbic sulphide 
 (galena) affords plumbic sulphate with nitric, acid; sulphides of 
 tin and antimony are converted into vjhite oxides ; whilst mercuric 
 sulphide is entirely unaffected by nitric acid, but dissolves very 
 readily in aqua regia. 
 
 The reguline metals are almost all soluble in nitric acid, and 
 such a metal unaffected by HNO3 must contain Au, Pt, Ir, or the 
 rarer metals in platinum ores. Oold a.i\d platinum are soluble in 
 aqua regia; palladium, also in HNO3; tin and antimo7iy are 
 converted by HN 0, into white oxides (insoluble in excess of the 
 acid), and are readily dissolved in aqua regia (or in HCl with 
 KClOj), if excess of HNO, is avoided. 
 
 A substance insoluble in and undecomposable by any of the 
 acids mentioned, even by prolonged digestion at a moderate tem- 
 perature, will be found in Table Y, and must be rendered soluble 
 (by fluxing), according to that table, after its general chemical 
 
COURSE OF QUALITATIVE CHEMICAL ANALYSIS. \) 
 
 nature has been ascertained by a preliminary examination in tlie 
 dry way (according to Tables I to IV). 
 
 II. Qualitative Examination of the Substances in Solution. — 
 In a qualitative examination of a liquid (not a solution prepared 
 by tlio investigator), it is necessary first to ascertain — 
 
 1. Whether volatile or non-volatile ingredients are present, by 
 evaporating a portion of the liquid on platinum foil, or in a cap- 
 sule. If a fixed residuum remain it must be subjected to the pro- 
 cesses for the preliminary examination of solids, except of course 
 such as relate only to solution. 
 
 2. Whether its reaction with test-paper is neutral, acid, or 
 alkaline. 
 
 These tests should never be omitted, since, with care, the pre- 
 sence or absence of whole groups of substances can be inferred 
 fr6m the results. Thus it is plain that no fixed substance need 
 be sought for in a solution which leaves no residuum upon care- 
 ful evaporation (that is, not produced by violent ebullition). A 
 neutral liquid as a rule can only contain salts of the alkalies or 
 alkaline earths, since the salts of nearlj' all other metallic oxides 
 have an acid reaction. The presence of free alkali (especially in 
 the absence of non-volatile organic compounds) excludes all 
 oxides insoluble in alkaline liquids, and if the alkaline reaction is 
 due to an alkaline carbonate no alkaline earth can be present. 
 (Among the exceptions to this rule are Fe.^0,,, CuO, etc., in pre- 
 sence of non-volatile organic matter, as well as oxides, cyanides, 
 sulphides, etc., soluble inpotassic cyanide and alkaline sulphides.) 
 The presence of certain metals also indicates the absence of cer- 
 tain acids, and vice versa; thus Ag need not be sougiit for in a 
 reguline metal completely soluble in HCl, nor Au, Sn, or Sb, etc., 
 in one soluble in HNO.,. 
 
 A portion of the solution of a solid, produced in any way, is 
 employed for the detection of the metals, and another portion for 
 the detection of the acid. 
 
 A. Detection of the Metals. 
 
 Table VI sets forth in a compact form the reactions of thfe 
 metals with general reagents, and therefore serves as the chief 
 guide to their detection. Whilst the course prescribed by it is 
 easilj' understood with a little reflection, it is, however, absolutely 
 necessary that the following rules be kept in view in the qualita- 
 tive examination of complex compounds. 
 
 1. The Precipitation by each of the General Beagents employed 
 
10 CO0ESE OF QDALITA.TIVE CHEMICAL ANALYSIS. 
 
 must he complete. The precipitant is therefore added gradually 
 as long as a precipitate is produced by it, or with H^S, until the 
 liquid smells strongly of it even after shaking. The separation 
 of the insoluble compound formed is promoted, in almost all 
 cases, by gently warming the liquid. Some metallic oxides 
 (As.p., M0O3, oxides of Pt, Ir, and Rh) are but slowly precipi- 
 tated by H^S, often only after warming the liquid, supersaturated 
 with it, from twelve to twenty-four hours. (As^O^ much more 
 rapidly, however, if heated to 60'^-'70° C.) 
 
 2. The precipitates which characterize the several groups must 
 be completely freed from the members of the remaining groups, 
 still in solution, by washing with water. This is accomplished, 
 according to circumstances, either upon a filter, or also in a test- 
 tube by allowing the precipitate to subside and pouring off the 
 clear liquid, and repeating the operation a number of times with 
 fresh water. By carefully evaporating on platinum foil a portion 
 of the filtrate from the precipitate of any group, not too small, the 
 presence of members of the remaining groups may at once be 
 ascertained. When easily oxidizable sulphides insoluble in dilute 
 acids are present, some H^S solution is added to the wash water, 
 or in case of ferric and manganic suli)hides a few drops of am- 
 monic sulphide, to prevent oxidation when the washing is pro- 
 longed. 
 
 By inattention to the two preceding conditions (complete pre- 
 cipitation and thorough washing)^ it is evident the members of 
 the various groups may remain partiallj' mixed with each other, 
 and reactions may be obtained in the subsequent analytical opera- 
 tions which are not noticed in these tables, and which are in- 
 explicable to the inexperienced. 
 
 3. The mineral acid employed for acidulaiion of the liquid (if 
 it is not already sufficiently acid) is either HC'l, or HNO.^, either 
 dilute or concentrated, but not in such a quantity as to prevent 
 the formation of insoluble sulphides. The first is usually pre- 
 ferred, when the possible precipitation of AgCl, Hg^Cl.,, PbCl^, 
 etc., as indicated in Table VI, must be considered. 
 
 4. If, in following the systematic course of qualitative analysis, 
 the presence of one or more members of the different groups is 
 recognized and proved by the reagents suggested in the tables, 
 the analyst (especially the beginner) must make a series of con- 
 firmatory experiments with the original substance, or its separate 
 constituents, which may control the results already obtained. 
 Such experiments should never be omitted by the beginner, since 
 
COURSE OF QUALITATIVE- CHEMICAL ANALYSIS. 11 
 
 it is the principal aim of analytical exercises not only to become 
 acquainted with the simple course of analysis, but to become 
 familiar with the deportment of a body in all its relations. Only 
 by following this important rule will the less experienced be pro- 
 tected from errors and deceptions. For these continually arise 
 from ignorance of the deportment of bodies, or the non-observance 
 of the conditions upon which the result of an experiment — the 
 appearance of the phenomenon which we regard as the proof of 
 the presence of a substance — rests. 
 
 The metals are further distinguished and separated according 
 to Tables VII to X. [Or the course may be much simplified 
 without sacrifice of accuracj', by proceeding according to Table 
 XIV with the filtrate from the H^S precipitate of Table VI, in- 
 stead of treating it according to the method of that table.] C. F. H. 
 
 B. Detection of Acids or Representatives of them. 
 
 The qualitative analj'sis of acids is quite as simple as that of 
 metals. In almost all cases the preliminarj^ examination accord- 
 ing to Tables I and XI, in connection with the quality of the 
 metals previously detected, indicates in what class of acids, 
 specially, tests are to be made. The knowledge of the deportment 
 of a salt toward solvents, and the reaction of its aqrieous solution 
 with test-paper, are especially important for this inference. By 
 igniting the substance alone, as well as by heating it with con- 
 centrated sulphuric acid (according to Table XI), the presence 
 of organic as well as volatile inorganic acids is ascertained. If 
 there is reason to suspect the presence of several acids, or their 
 salts, the circumstances must be, considered, in the preliminary 
 testing, which may possibly occasion deception, since changes 
 may occur, or phenomena present themselves upon ignition or 
 ti'eatment with sulphuric acid different from those afforded by the 
 several acids alone. Thus salts of organic acids, when mixed with 
 nitrates or chlorates, decompose upon ignition without blackening, 
 but generally with deflagration, and if suflScient organic matter 
 is present no nitrate can then be detected after ignition, but only 
 a carbonate, if the base is an alkali or alkaline earth. A mixture 
 of a nitrate with a chloride develops, on treatment with concen- 
 trated sulpljiuric acid, neither pure hydrochloric nor nitric acid, 
 but chlorine and red nitrous vapors; in a mixture Of a sulphite 
 with a nitrate (chromate, chlorate, etc.) the sulphurous is con- 
 verted into sulphuric acid ; and sulphur is separated from most 
 sulphides. 
 
12 COURSE OF QUALITATIVE CHEMICAL ANALYSIS. 
 
 That the presence of volatile organic acids in an uncombiiiecl 
 condition may not lie overlooked, the acid solution is neutralized 
 with sodic carbonate, evaporated and ignited, when organic acids 
 will decompose with blackening, whilst they might otherwise be 
 volatilized undecomposed. 
 
 For the detection of the more important acids in the wet way, 
 in substances in solution, the course in Tables XII and XIII is 
 followed. The use of general reagents for acids in most cases is 
 only intended to determine the presence or absence of the mem- 
 ibers of a whole group of acids. The examination for the separate 
 acids of these groups requires in addition the employment of the 
 special tests of the tables. 
 
 If the examination for acids must take place in neutral liquids, 
 acid solutions are neutralized with ammonia, alkaline ones with 
 HNO„ or also with HCl if AgNOg is not to be used as a precipi- 
 tant. If the compound was not originally soluble in water, but 
 was soluble in acids without visible decomposition, and the base 
 is an alkaline earth or an earth, then the acid solution (as in case 
 of phosphates or oxalates of the alkaline earthy) cannot be tested 
 in a neutral condition by CaCl,, since, on neutralization with am- 
 monia, the whole salt would be precipitated. In ^such cases (to 
 which besides attention is directed in the precipitate of metallic 
 oxides by HCNHJS), the test for the acids is made in acetic acid 
 solutions, (with CaCl^ for oxalic acid, and Fe.^Clg for phosphoric 
 acid), or the base is first removed in the proper way, (alkaline 
 earths by H,SO„ heavy metals by H,S or H(NHJS). From the 
 salts of oi'ganic acids, insoluble in water, the acids are removed 
 by boiling with sodic carbonate, and the neutralized filtrate is 
 tested with HCl. If a liquid, which contains H.^S, or a soluble 
 sulphide, is to be tested for such acids as are precipitated from 
 acid solutions by AgNO, but not by ferric salts (HCl,HBr,HI), the 
 sulphur, is removed by addition of ferric sulphate, and the filtrate 
 acidified with HNO3 is tested for these acids. Compounds in- 
 soluble in water and acids are decomposed according to Tables V 
 and XII to be tested for acids. 
 
TABLE I. 
 
 Pkeliminaky Examination. 
 
 Behavior of Inorganic Solid Sul 
 
 Substances of rare occurrence aJ- 
 
 1 . Easily volatilized when heated 
 upon charcoal {or upon platinum 
 foil, or in a dry test-tube) : — 
 
 2. Fusible without volatilizing, 
 and without changing color ; — 
 
 3. Deflagrate when heated upon 
 charcoals — 
 
 4. Infusible, or difficultly fusible, 
 without changing color : — 
 
 Compounds of ammonia aiid mercury, and some of a 
 the air; all organic compounds are decomposed when hea 
 
 Most of the salts of the alkalies and some of those o|!i 
 brown. Some silicates, »s Zeolites. — Borates and alum sm 
 antimony, Wad, ihalhum, cadmium, tellurium, bismuth, sine, in,'j 
 former metals at the same time give incrustations. (See a 
 
 Nitrates, chlorates, perohlorates, iodates, brom!| 
 
 The earths and their salts; the alkaline earths and j, 
 after ignition. Silica, and many of its compounds.— Of tlj| 
 and rhodium are infusible before the blowpipe. \ 
 
 5. Assume a darker color when 
 heated: — ' 
 
 Many metallic oxides and their salts, as: zinc oxiji 
 and antimonic acid, yellow; plumbic oxide, bismutij 
 
 6. Color the flame of a Bunsen 
 gas-lamp, or the point of the blue 
 flarke of the blowpipe {upon plati- 
 num wire, or in case of metallic 
 compounds upon charcoal) : — 
 
 Violet. 
 
 « 
 
 Fotassfti 
 Eahidia, 
 
 Yellow.* 
 
 r * \ 
 
 Soda, 
 
 or a mixture of salts 
 
 of the alkalies. 
 
 * The colored flames may be distiaguished with 
 most certainty by prismatic analysis. 
 
 Crimson. ;! 
 
 Lithia, ;' 
 Btrontia.*< 
 
 the:aS 
 t Especi»li 
 
 Blue Glass. 
 
 7. Cfive, when moistened with a 
 solution of cobalt, and strongly 
 heated upon charcoal: — 
 
 BoiateSi 
 Silioates, 
 
 ''"'lot 
 
 the 
 Alkalies. 
 
 Blce or Bluish- Violet Infusible I;\ 
 
 , « ti- 
 
 Alumlna. and many of its compounds, i: 
 
 Phosphates of the Earths, 
 
 Silicio Acid and some Silicates of the El' a 
 
 Garlic Odor. 
 
 Hepar.* 
 
 Metallic Gufii 
 
 8. Give, when ignited with sodic 
 carbonate [or sodic carbonate and 
 potassic cyanide), in the reducing 
 flame, upon charcoal: — 
 
 Most of the Com- AH Componnds of Snlphnr Bright malleable 8,^5 
 pounds of Aisenio, (seleninm, teUnrinm) r 
 without exception. 
 
 * The mass when moistened blackens silver, 
 and with acids, develops sulphuretted (sele- 
 niuretted or tellurettedj hydrogen. 
 
 Tin, white. 1 
 Silver, whitej. 
 Copper, 'ed. i 
 Gold, yellow.) 
 
 Odorous Gases. 
 
 9. Give, when heated in a glass 
 tube open at both er^ds, and held 
 obliquely : — 
 
 Metallic Sulphides,— of burning sulphur. 
 
 " Seleaides, — of decaying radishes. 
 
 " Arsenides,— of garlic. 
 Some ammoniacal compounds,- of ammonia. 
 Metallic fluorides (upon addition of phos- 
 phorus salt). 
 
 Metallic Coatihi 
 
 Some Arsenides, ; 
 
 Some comuounds of Me'rt 
 
 (especially with 's 
 
 carbonate). 
 
 10. In contact with zinc and 
 hydrochloric {or sulphuric) acid 
 color the fluid: — 
 
 Violet or Lilac. Blue, then Copper red. Blue th 
 
 Titanic Acid.' 
 
 Tnngstic Acid. 
 * The coloration with zinc and HCl takes pla( 
 
)stances in the Preliminary Tests. 
 
 ■e placed in [ ] in the Tables. 
 
 rsenic [and thallium], sulphur and its acids, ■water, etc. Carbon burns upon ignition in 
 .ted, most of them with the separation of carboa (blackeniDg). 
 
 ' the alkaline earths. After iotense ignition in the reducing flame, they color turmeric paper 
 ell up ; oommon salt and other salts, also many minerals, decrepitate. — Of the reguline metals, 
 dium, and tin fuse easily before the blowpipe ; silver, copper, and giold, with more difficulty ; the 
 elow, 8, and Table III.) 
 
 ates, etc. 
 
 :i 
 
 their salts. When heated they glow with white light. The earths show no alkaline reaction 
 le reguline metals, iron, nickel, cobalt, molybdenum, tungsten, platinum, iridium, palladium, 
 
 de, yellow (glows with yellowish-green light) ; stannic oxide, titanic acid, niobic acid, 
 tious oxide, chromates, mercuric oxide, etc., brown. 
 
 Orange. Yellowish-Gbben. Green. Blue. 
 
 I Lime.** Baryta,** Onpriq oxide,t Arsenic, 
 
 '* Molybdio Acid, Phosphoric Acid,tt Antimony, 
 
 ' Boraoio Acid, tt Lead, 
 
 I ' Tellurons Acid, Seleninm, 
 
 billy after moistenmg with hydrocljloric acid, or Compounds of Thallium. ' Ouprio ohlorideit 
 
 lUdition of argentic cliloride, transitory. Indinm. 
 
 idly after the addition of some argentic chloride. tt I" '^"^ ^^I's ^f'®"^ moistening with sutphurio acid. 
 
 IHass. Green Mass. Flesh-red Mass. Brown or Brick-red Mass. Gray Mass. 
 
 Zincio oxide, (yellowish- Mac^nesia, Baryta, Glncina, 
 
 Titanic Aoid, ' green. Tantalio Acid, Lime, 
 
 iliarths. Stannic oxide, BluiBh-greea. Strontia. 
 
 Antim mio Aoid, ) Muddy- 
 j Niobic Acid, ' green. 
 
 luiiNS WITHOUT Incrustation. MetallicGrains with Incrustation. Incrustation without 
 
 J ^ , , " , Metal. 
 
 Iiinmigles. Gray infusible powder. Metal brittle. Metal malleahle. , ^ , 
 
 J. . , , -^ , Antimony, Lead, Zinc, white, not volatile 
 
 ( Magnetic. Non-magnetic, j ^hjte, volatile. I. yellow. In the outer flame. 
 
 Bij Iron, Molybdenum, Bismuth, Thallium, Cadmium, reddish-brown. 
 
 i Nickel, ^ngsten, j, brownish-yellow. Tarnishes, I. yellow. Tellurium, white. 
 
 jr. Cobalt. Platinum, Indium, 
 
 Iridium, I. white. 
 
 illSO. 
 
 White Coating. Fused Sublimate. Drops of Water. 
 
 "' ' Met llio arsenides, crystalline. \ Higher Metallic snlpbides, brownish-yellow. AH hydrates, 
 (Wiry " antimonides, ( f„aii,ie Metallic selenides ahd selenium, dark red. (More distinct in a 
 
 lliiodlc " tellurides, ' ' (Also sulphide of arsenic.) bulb tube.) 
 
 i Plumbic sulphide, 
 
 I Some salts of ammonia, 
 
 \ Blue, then Green and Blue, then Muddt 
 
 , ^m Green and Violet. Dark Brown. or Brown. Ubebn. 
 
 '' j i ^ » ^ , * ^ , ^ ^ 
 
 "Tv^dioAoid. Molybdio Aoid. Tantalio and Kiobio Acids.* Chromic Aoid, 
 1 M more readily after fusion of the insoluble substance with acid potassium sulphate. 
 
' TABLE II. 
 
 Pkeliminakt Examination. 
 
 11. Flame Reactions wittfJ 
 
 
 a. 
 
 1.. 
 
 ft 
 
 c 
 
 
 ^' B 
 
 
 
 °^ &- 
 
 
 D 
 
 a.. 
 
 
 / 
 
 \^«■ 
 
 \. 
 
 J 
 
 '■ l 
 
 r 
 
 1 
 
 ci/, ti, a, a„ the dark nucleus, 
 a/,, e, a/, &, tlie flame mantle, u, &, 
 a, the luminous point not in the 
 normal flame,- but formed, when 
 needed, hy partially turning the 
 collar. 
 
 Most of the tests described 
 in Table I can be made more 
 easily than with the blowpipe, 
 by means of the non-luminous 
 flame of a Bunsen gas-lamp, 
 provided with a movable collar 
 (by turning which the access of 
 air may be regulated), and a 
 conical chimney d, d, d, d. The 
 flame should have the form 
 shown in the annexed figure. 
 The portions which serve for 
 conducting the difi^erent reac- 
 tions are distinguished as fol- 
 lows: 1. Tl'hebaseoftheflaineat 
 
 A, having the lowest tempera- 
 ture ; 2. The zone of fusion at 
 
 B, having the highest tempera- 
 ture ; 3. The lower oxidizing 
 flame at G; 4. The upper oxi- 
 dizing flame at E, the tip of the 
 non-luminous flame (serves 
 for cases of roasting and oxi- 
 dation that do not require ex- 
 cessively high temperature). 
 
 6. The lower reducing flame ai i 
 following, and serving for reduf 
 of fused salts ; 6. The upper, ret^] 
 point formed on diminishing tl 
 closing the draught holes, by 
 specimen may be snpportediiin 
 no thiclcer than a hor.?ehair, o) 
 fastened in a small glass tube, 
 Substances may be tested witl! 
 gard to : — 
 
 1 . Emissive power for lighl, b 
 of the zone of fusion. The ei(| 
 low, medium, or high, accordM 
 specimen falls below, equals, oil 
 wire introduced at the same tiiij ' 
 
 2. Fusibility, which is expreiU 
 with the following six grades, c I 
 ance of a thin platinum wire in 
 as below red heat, incipient red hi ,i 
 white heat, intense white heat. 
 
 3. Volatility, by determining 
 a weighed bead (0.01 grm.) in 
 paring it with the time require!; 
 of sodio chloride, the volat" 
 
 tility^l 
 
 4. Flame coloration, by placj 
 
 \< 
 
 [* See Bunsen's Flame Reactions, for fuller explanation and more complete list of special reactions, translat 
 ■f Forty of these may be made by drawing out an ordinary sized test-tuba and cutting it with, a diamond into le ^ 
 
the Bunsen Gas-lamp.* 
 
 t Z>, less energetic than the 
 Btion on charcoal, cr in beads 
 lucing flame at C, the luminous 
 le supply of air, by partially 
 turning the collar. The test 
 the flame on a platinum wire, 
 *|r on a small fibre of asbestos, 
 and held by a suitable holder. 
 1 very small specimens in re- 
 
 i ly holding in the hottest part 
 nissive power is estimated as 
 ing as the luminosity of the 
 r exceeds that of the platinum 
 
 k le. 
 ised on a scale of temperature 
 listinguishable by the appear- 
 cfi^'erent portions of the flame, 
 \at, red heat, incipient white heat. 
 
 the time required to volatilize 
 
 the zone of fusion, and com- 
 
 d to volatilize an equal weight 
 
 of which is taken as unity. 
 
 lit ng the test specimen in the 
 
 upper reducing flame. The coloration appears in the upper 
 oxidizing flame. Mixtures of substances are first tested in 
 the base of the flame to obtain in the flame mantle (for an in- 
 stant), the coloration produced by the more volatile, unmixed 
 with that of the less volatile. 
 
 5. Reduction and .oxidation in beads of fused salts. See 
 Table IV. 
 
 6. Reduction by charcoal dr a metal. This is accomplished, 
 in testing for mercury, arsenic, phosphorus, sulphur, selenium, 
 and tellurium, by heating the thoroughly dried test-specimen 
 in a thin glass tubef 3 cm. long, 2 to 3 mm. wide, to the 
 point of fusion of the glass, with a mixture of sodic carbonate 
 and carbon (soot from turpentine), or with a piece of magne- 
 sium wire, or of sodium. Reduction of other metallic com- 
 pounds is efl^ected, by first preparing a small charcoal rod, by 
 coating a small wooden rod (as an ordinary match) three- 
 quarters of its length with fused crystallized sodic carbonate, 
 and charring it carefully in the flame, and then placing the 
 test-specimen, about the size of a mustard seed, mixed with a , 
 drop of fused sodic carbonate,' upon the point of it, heating it 
 to fusion in the lower oxidizing flame, and then passing it 
 into the hotter portion of the lower reducing flame opposite. 
 The products of reduction may then be further examined. 
 
 ed by the editor of these Tables. 
 
 ngths double the size of the tubes, and dividing these over the lamp and rounding the closed ends 
 
 h 
 
 F. H. 
 
TABLE III. 
 
 Pbeliminaky Examination. 
 
 III. Flame Reactions. 
 
 The incrustations, if collected on porcelain or glass, afford with further tests decidedly charac|erij 
 ot the substance on an asbestos fibre in the upper reducing flame (not too large, and perfectly if' 
 filled with water, immediately above it, on which any volatile metals present will be deposited, as m 
 these with a drop of dilute nitric acid (containing 20 per cent, anhydride), on a glass rod, they arm 
 
 Instantly dissolved. Slowly and wUli difficulty f « 
 
 , A - ^ --^-^ — — \ 
 
 Lead, cadmium, zinc, indium. Bismuth, mercury, i th^ 
 
 2. Oxide Incrustations, formed by holding the porcelain capsule, in the preceding experi; 
 (a) by touching it with drops of stannous chloride, and then with caustic soda ; (A) by touching wi 
 tlon, formed by placing the oxide incrustation on the capsule [when cold], over a wide-mouthen 
 It may be tested by the moist breiith (solubility), and by ammonia blown upon it.f 4. Sulphit ll 
 gently warming the capsule; characterized by its insolubility in water,^ color, and deportmeht^iti \ 
 
 Volatile Elements Separable I 
 
 
 
 
 
 .,.„„„„„ „„^ — 
 
 i 
 
 Tellurium, 
 
 Metallic Incrustation 
 and Coating. 
 
 Oxide Inorastation 
 and Coating. 
 
 Oxide Incrnsta- 
 tion with BnCk. 
 
 Oxide Incrusta- 
 tion with" SnOk 
 and NaHO, 
 
 Oxi^eii 
 witU/Agll 
 
 Black; with brown 
 coating. 
 
 White. 
 
 Black. 
 
 Black. 
 
 White, 
 Idwii 
 
 Selenium, 
 
 Cherry-red; with 
 brick-red coating. 
 
 White. 
 
 Brick-red. 
 
 Black. 
 
 V 
 
 Antimony, 
 
 Black; with brown 
 coating. 
 
 White. 
 
 White. 
 
 White. 
 
 Black ; 
 
 in N 
 
 Arsenic, 
 
 Black; with brown 
 coating. 
 
 White. 
 
 White. 
 
 White. 
 
 Lemon 
 bra\i 
 solul 
 
 Bismuth, 
 
 Black; with soot- 
 brown coating. 
 
 Yellowish-white. 
 
 White. 
 
 Black. 
 
 1 
 
 Mercury, 
 
 Gray, incoherent 
 coating. 
 
 
 
 
 
 Thallium, 
 
 Black; with brown 
 coating. 
 
 White. 
 
 White. 
 
 White. 
 
 1 
 
 % 
 
 Lead, 
 
 Black; with brown 
 coating. 
 
 Light ochre-yel- 
 low. 
 
 White. 
 
 White. 
 
 Cadmium, 
 
 Black ; with brown 
 qoating. 
 
 Brownish-black; 
 with white coating. 
 
 White. 
 
 White. 
 
 Coatinil 
 blue| 
 
 Zinc, 
 
 Black; with brown 
 coating. 
 
 White. 
 
 White. 
 
 White. 
 
 1 
 
 Indium, 
 
 Black ; with brown 
 coating. 
 
 Yellowish-white. 
 
 White. 
 
 White. 
 
 \ 
 
 r* Witli a small quantity of the substance the lamp should he suitably turnetd 
 
 t By blowing through ammonia water in a small wash bottle, with exit tubel 
 
 L j By an apparatus similar to that for ammonia. See t- § Generally inaolij 
 
IS. (Incrustations.) 
 
 Btenstic reactions. 1. Metallic incrustations, obtained by heating a very small particle 
 Free from smoke), and at the same time holding a glazed porcelain capsule, 0.1 metre in diameter, 
 a dark incrustation, surrounded by a thinner coating [often of a diflferent tint]. On touching 
 
 r packed, 
 h'tUium. 
 
 Or unaffected. 
 
 Tellurium, selenium, arsenic, antimony. 
 
 iniient, at some distance from the test-specimen, in the upper oxidizing flame.* It may be tested : 
 ittt drops of argentic nitrate solution, and blowing ammonia upon it f 3. Iodide incrusta- 
 id vessel containing fuming HI (deliquesced phosphoric triiodide), and aflerward gently warming it. 
 iile Incrustation, obtained from the last by blowing ammonic sulphide upon it,J and then 
 lith ammonic sulphide (blown or dropped on it). 
 
 liy Eeduction as Incrustations. 
 
 
 , 
 
 
 fchorustition 
 ijNOsaudlIHa 
 
 Iodide Incrnstatioa and 
 Coating. 
 
 Iodide Incrnstation 
 with NHs (blown 
 upon it). 
 
 Sulphide Incrnsta- 
 tion and Coating. 
 
 Sulphide Inornata- 
 tion with HdlflJS. 
 
 H tinged yel- 
 liih. 
 
 Brown ; breathed upon dis- 
 appears for a time. 
 
 Disappears perma- 
 nently. 
 
 Black to blackish- 
 brown. 
 
 Disappears for a 
 time. 
 
 ffhite. 
 
 Brown ; breathed upon does 
 not wholly disappear. 
 
 Does not disap- 
 pear. 
 
 Yellow to orange. 
 
 Orange, then dis- 
 appears for a time. 
 
 t; Insoluble 
 SHa. 
 
 Orange ; breathed upon dis- 
 appears for a time. 
 
 Disappears perma- 
 nently. 
 
 Orange. 
 
 Disappears for a, 
 time. 
 
 ■ yellow or 
 ■mish-red ; 
 lUeinNHa. 
 
 Orange-yellow ; breathed 
 upon disappears for a 
 time. 
 
 Disappears perma- 
 nently. 
 
 Lemon-yellow. 
 
 Disappears for a 
 time. 
 
 Ifhite. 
 
 Bluish-brown; with light 
 redc6ating; breathed upon 
 disappears for a' time. 
 
 Rose- red to orange 
 yellow; chestnut- 
 brown when dry. 
 
 Umber-brown ; 
 with coflFee- 
 brown coating. 
 
 Does not disap- 
 pear. 
 
 
 Carmine and lemon-yellow ; 
 breathed upon does not 
 disappear. 
 
 Disappears for a 
 time. 
 
 Black. 
 
 Does not disap- 
 pear. 
 
 1/hite. 
 
 Lemon-yellow ; breathed 
 upon does not disappear. 
 
 Does not disap- 
 pear. 
 
 Black; with blu- 
 ish gray coating. 
 
 Does not disap- 
 pear. ^ 
 
 IVhite. 
 
 Orange-yellow to lemon- 
 yellow; breathed upon 
 does not disappear. 
 
 Disappears for a 
 time. 
 
 Through brown- 
 ish-red to black. 
 
 Does not disap- 
 pear. 
 
 ; becomes 
 ^black. 
 
 White. 
 
 White. 
 
 Lemon-yellow. 
 
 Does not disap- 
 pear. 
 
 fhite. 
 
 White. 
 
 White. 
 
 White. 
 
 Does not disap- 
 pear. 
 
 ?hite. 
 
 Yellowish-white. 
 
 Yellowish-white. 
 
 White. 
 
 Does not disap- 
 pear. 
 
 i down so that the coating may not be spread over too mucli surface. -i 
 
 just below the cork. It may also be treated with drops o£ ammonia. G, F. H. 
 
 ible in the breath, but possessing different degrees of solubility in drops of water. J 
 
TABLE IV. 
 
 Preliminary Examination. 
 
 TV. Behavior of Metallic Oxides before the Blowpipe i^ 
 
 and : 
 
 The bead (formed on a loop of platinum wire, or, in experiments with the reducing flame, 
 luminous gas-flame, the bead, fused on a platinum wire as thick as a horsehair, is introduceopj 
 The colors of the beads frequently differ, according to their temperature, and to the quantity ot t 
 saturated, s. s. strongly saturated.) 
 
 CoLOB or THE Beads. 
 
 With Phosphorus Salt. 
 
 In the Oxidizing Flame. 
 
 In the Reduein 
 
 Colorless : — 
 
 Silica gives skeleton of silica. Alu- 
 mina, stannic oxide. — h. c. all alkaline 
 earths, and earths (s. s. not clear). Tan- 
 talic, niobic, titanic, iungstic acids, zindc, 
 cadmic, plumbic, bismuthous, antimoni- 
 ous oxides (f. s.); 8. s. yellowish. 
 
 Silica gives skeleto 
 mina. All alkaliml 
 (s.s. not clear), eerie, d 
 and stannic oxides. 
 
 Yellow: — 
 (to broyn). 
 
 h. ff. B.) Ferric oxide, eerie oxide — h. 
 Vanadic acid, uranic oxide, argentic 
 oxide. — c. Nickelous oxide. 
 
 h. Ferric oxide (yeli 
 acid. 
 
 Red:— 
 
 h. (s. s.) Ferric oxide, eerie oxide, h. 
 Nickelous oxide, chromic oxide. 
 
 h. Ferric oxide, c .H 
 acid, containing iron ( 
 
 Violet : — 
 (amethyst). 
 
 h. c. Manganic oxide, didymic oxide. 
 
 c. Titanic acid, niab 
 
 Blite : — 
 
 h. e. Cobaltous oxide, c. Cupric oxide: 
 
 h. c. Cobaltous oxide 
 niobic add (s. s.). 
 
 Geeen : — * 
 
 h. Cupric oxide, molybdic acid. c. 
 Chromic oxide, uranic oxide, h. Ferric 
 oxide containing cobalt or copper. 
 
 c. Chromic oxide, v, 
 die add, molybdic ad 
 
 Geat: — 
 (cloudy). 
 
 
 c. Argentic, zindc, 
 bismuthous, and antiv 
 lurous add, nickelous 
 
 * Reduction geaerallj takes place more easily with phosphorus salt. In case of ferric oxide, titani 
 
 test specimett 
 
th Sodic Ammonic Hydric Phosphate (Phosphorus Salt), 
 >orax, 
 
 Iso upon charcoal) is graduUy saturated with the finely-powdered substance. In using the non- 
 meana of a holder into the lower reducing, or into the lower oxidizing flame. (Compare Table II.) 
 e dissolved oxide. (The following abbreviations are — h. hot, c. cold, h. o. hot and cold, f. s. feebly 
 
 
 With Borax. 
 
 Flame* 
 
 In the Oxidizing Flame. 
 
 In the Reducing Flame. 
 
 of silica. Alu- 
 arlha and earths 
 iymie, manganic, 
 
 h.c. Silica, alumina, stannic oxide, h.c. 
 (s. s. not clear); all alkaline earths and 
 earths,argentic oxide, ianialic, niobic, and 
 tellurous acids.— t s. Titanic, tungstic, 
 and molybdic acids, zincic, cadmic, plum- 
 bic, biamuthous, and antimonious oxides. 
 
 h. c. Silica, alumina, stannic oxide — 
 h. c. (as. not clear); all alkaline earths 
 knd eartha, lanthanic oxide, eerie oxide, 
 iantalic acid.—h. e. Manganic oxide, 
 didymic oxide, h. Cupric oxide. 
 
 w to red}, titanic 
 
 h. Ferric oxide, uranic oxide (f. s.). h. 
 Vanadic acid. h. Plumbic, biamuthous, 
 and antimonious oxides (s. s. ). 
 
 h. Tungatic acid. (h. Titanic, vanadic, 
 and molybdic acids yellow to'brown.) 
 
 arefc and iungatic 
 lood-red). 
 
 h. Oeric and ferric oxidea. c. Nickel- 
 oua oxide (reddish-brown). 
 
 c. Cupric oxide (opaque s. s.). 
 
 J acid (s. s.). 
 
 h. c. Manganic and didymic oxidea. 
 Nickeloua oxide containing cobalt. 
 
 
 c. Tungstic add, 
 
 h. c. Cobaltous oxide, c. Cupric oxide. 
 
 h. c. Cobaltous oxide. 
 
 inic oxide, vana- 
 
 c. Chromic oxide, vanadic acid. h. 
 Cupric oxide, ferric oxide, containing 
 cobalt or copper. 
 
 h. c. Ferric, uranic, and chromic oxidea. 
 a. Vanadic acid. 
 
 ',admic, plumbic, 
 nious oxides, tel- 
 xide. 
 
 
 As with phosphorus salt. 
 Also niobic add (s. s ). 
 
 and tungstic acids, the reduction is hastened 1}y the addition of a very small quantity of tinio the 
 pon charcoal). 
 
TABLE V. 
 
 Fluxing Insoluble Compounds. 
 
 V. Conversion of Insolubl( 
 
 If a finely pulverized compound, after successive treatment with water, dilute and concenti 
 or attacked by the acids in such a way aS to afford decisive conclusions as to the nature of thi 
 constituents may be determined in tlie humid way. The mode of fluxing in many cases depen( 
 with great care. If no decisive indication for the treatment gt the insoluble compound aceordi 
 of mixed sodic and potassic carbonates, and the fused mass should be treated with water, si 
 for any substances containing arsenic or any easily reducible metal (antimony, tin, lead, bismutn 
 
 a. Sulphates. 
 
 (Barie, strontic, and plumbic 
 Sulphates. ) 
 
 b. Silicic Acid and Silicates. 
 
 0. Flu 
 
 {Fluor^ 
 
 With sodic carbonate upon char- 
 coal they give Hepar. 
 
 Baric and strontic sulphates are de- 
 composed by fusing with 4 parts of 
 alkaline carbonate. After treatment 
 with water and washing, the solution 
 contains the acid, the residue the base 
 (now soluble in hydrochloric acid). 
 Plumbic sulphate gives a metallic 
 globule with sodic carbonate, is 
 blackened by ammonic sulphide, 
 and dissolves in ammonic tartrate 
 with excess of ammonia. Qypsum 
 is somewhat soluble in water. 
 
 Give with phosphorus salt skeleton 
 of silica. 
 
 The solution of the decomposable 
 silicates is efl'ected by hydrochloric 
 acid ; of the undecomposable by fu- 
 'sion with 3 — 4 parts of alkaline car- 
 bonate (or baric hydrate), treatment 
 with hydrochloric acid, and separa- 
 tion of the silicic acid by evaporation 
 with free hydrochloric acid. Or by 
 means of hydrofluoric acid. 
 
 The substance must always be very 
 finely powdered. 
 
 With concentra 
 they give hydrofluo 
 etches glass; in ] 
 acid, silicic fluori 
 precipitate with ^ 
 
 The solution is 
 with 4 parts of a 
 (completely by a 
 and boiling with i 
 tion contains the 
 residue the base, 
 hydrochloric acid. 
 
 f, Stannic Oxide, Anti- 
 monic Acid. 
 
 g. Titanic, Tugstic, Tan- 
 talic, Niohic Acids. 
 
 h. Chlorides' ( 
 
 ride, Bromid 
 
 phides {^oh 
 
 etc.) ^ 
 
 With sodic carbonate upon char- 
 coal tbey give malleable or brittle 
 metallic grains, and are colored by 
 ammonic sulphide. . 
 
 By fusion with 3^1 parts alkaline 
 carbonate they become soluble in 
 acids. They are also soluble in ex- 
 cess of yellow ammonic sulphide. 
 
 Moistened with hydrochloric acid 
 in contact with zinc, in a, platinum 
 capsule, they are reduced to metals ; 
 with the production of a black stain 
 upon the platinum when antimony 
 is present. 
 
 With phosphorus salt they give a 
 blu£, violet, or (those containing iron) 
 blood-red bead, and with zinc and 
 hydrochloric acid a coloration, espe- 
 cially after fusion with acid potas- 
 sium sulphate. (Compare Table I, 
 10.) 
 
 The solution is eff'ected by fusing 
 with 6 parts of hydrio potassic or 
 hydric sodic sulphate, (or also of 
 carbonate.) [See note to Table 
 XIV.] 
 
 Argenticchloride, 
 give with sodic c 
 granule. The dect 
 effected by means 
 sulphuric acid, o 
 lime or alkaline ca 
 being separated^ 
 gives a metallio 
 nitric acid, pluinb 
 a.) Molybdic su 
 phosphorus salt, 
 beads, and is ch« 
 into molybdic ac 
 with zinc and hyi 
 
le Compounds into Soluble. 
 
 nirated hydrochloric acid, Mtric acid, and aqua regia, remains undissolved, or is not,dooomposed 
 Ike insoluble compound, then the latter must be rendered soluble by fluxing, in order that its 
 (ods upon the result of the preliminary examination ; the latter should therefore be conducted 
 tding to this table be given, then it is always to be fused in form of fine powder .with four parts 
 land the washed residue with hydrochloric acid. Platinum crucibles should never be employed 
 *, etc.). 
 
 liorides. 
 
 ifar, etc.) 
 
 luted sulphuric acid 
 i/ioric dcidgas, which 
 in presence of silicic 
 iiiide, which gives a 
 llifater. 
 
 IB effected by fusing 
 olilkaline carbonate 
 ijidditioQ of silica) 
 ilwater. The Bolu- 
 k acid, the washed 
 m, (now soluble in 
 i.) 
 
 d. Alumina or Aluminates. 
 
 When ignited with solution of co- 
 balt they give a blue, infusible mass. 
 
 The solution is effected by fusing 
 with 3 to 4 parts of hydricpotassic, 
 or hydrio sodic sulphate (or also of 
 carbonate), and treating with water, 
 or hydrochloric acid. [See note, 
 Table XIV.] 
 
 Chromic Oxide. 
 
 ( Chromic Iron. ) 
 
 Gives with phosphorus salt and 
 borax green beads in the outer and 
 inner flame. 
 
 The solution is effected by fusing 
 with hydric potassic sulphate, or 
 with a mixture of potassic nitrate (or 
 chlorate), and alkaline carbonate. 
 Chromic iron ore, very finely pow- 
 dered, requires successive treatment 
 by both methods ; the mass result- 
 ing from the last fusion with alka- 
 line carbonate (and the oxidizing 
 agent) contains the chromium as an 
 alkaline chromate, soluble in'water. 
 [See also note. Table XIV.] 
 
 \l^[Ar gentle Ghlo- 
 4, Iodide). Sul- 
 ^jbdic Sulphide, 
 
 ^bromide, and iodide 
 iiarbonate a silver 
 iiomposition may be 
 an of zinc and dilute 
 ■IT by igniting with 
 gsrbonate, the metal 
 di Plumbic sulphide 
 iljranule, and with 
 ale sulphate. (See 
 iphide gives, with 
 il, yellowish -green 
 inged by roasting 
 Kid, becoming blue 
 (Jroohloric acid. 
 
 i, Reguline metals. {Osm- 
 
 iridium, or residue from 
 platinum ores.) 
 
 The insoluble mass has metallic 
 lustre or is blalck, pulverulent, and 
 not changeable by ignition. 
 
 The solution is effected by igniting 
 the powder, mixed with common 
 salt, in chlorine gas, or by fusing 
 with a mixture Of potaasio hydrate 
 and potassic chlorate. 
 
 k. Carbon. 
 
 The insoluble mass is black (as 
 diamond, also colorless), and dis- 
 appears when strongly ignited in an 
 open platinum crucible, or before 
 the blowpipe. 
 
 It deflagrates when fused with 
 potassic nitrate with the formation 
 of potassic carbonate, and when 
 ignited with cupric oxide (in case 
 of graphite in a stream of oxygen), 
 gives carbonic acid. 
 
TABLE VI. 
 
 Detection of Metallic Oxides. 
 
 VI. Deportment of Solutions of Metallic Oxides with Hf 
 
 (Ammonia), and Ammonic C 
 
 (For different treatment of the filtrate fromt 
 
 Hydrochloric Acid. 
 
 Hydrogen Sulphide. 
 
 Oxides which are. pre 
 cipitated from a neutral 
 or acid solution by hy 
 drochloric acid, as 
 chlorides.* 
 
 Plumbic oxide, 
 
 white, crystalline, solu- 
 ble in much water, pre- 
 cipitable by sulphuric 
 acid. 
 
 Argentic oxide 
 white, curdy ; soluble in 
 ammonia, whence it is 
 precipitable by nitric 
 acid. 
 
 Mercnrous oxide- 
 white, pulverulent ; is 
 blackened by ammonia. 
 
 [Thallious oxide], 
 
 white, curdy ; more com 
 pletely precipitated b^ 
 potassic iodide. 
 
 Uxides which are 
 partially reduced 
 in an acid solution 
 whilst sulphur is 
 precipitated.* 
 
 Oxides which are precipitated by hydrogen 
 sulphide from their solutions, acidulated bj 
 hydrochloric or nitric acid, as 
 sulphides. 
 
 Ferric oxide, 
 
 the fluid is decolor 
 ized, and contains 
 ferrous oxide. 
 
 Manganic 
 oxide. 
 
 Permanganic 
 acid, the fluid be- 
 comes joolorless, 
 and contains man- 
 ganous oxide. 
 
 Chromic acid, 
 
 the fluid becomes 
 green, and con 
 tains chromic 
 oxide. 
 
 Autimonious 
 
 * In an alkaline solution 
 hydrochloric acid (and also 
 nitric acid^ may cause a pre- 
 cipitate when any of the 
 following are present :— ^ 
 
 Silicic acid, 
 
 Soraeic acid, 
 
 Antimon^c acid, 
 
 Tungstic acid, 
 
 Molyhdic acid, 
 also oxides soluble in alka- 
 lies {plumMc oxide, alu- 
 mina, soluble in excess of 
 nitric acid) as well as metal- 
 lic cyanides and ferrocya- 
 niden, and all fnetallic sul- 
 phides soluble In ammonic 
 sulphide. A precipitate of 
 sulphur may also be forified 
 in soluble polysnlphides 
 and hyposulphites (thiosul 
 phates). 
 
 * A precipitation of 
 sulphur may also oc- 
 cur by the presence 
 of free chlorine, bro- 
 mine, iodine, sulphur: 
 ous, nitrous, hypo- 
 chlorous, chloric, 
 broniic, or iodic acid, 
 etc., or generally by 
 the presence of any of 
 the easily reducible 
 higher " oxides which 
 are not precipitated 
 as sulphides from 
 acid solutions. 
 
 Soluble in 
 Ammonic Sulphide. 
 
 1 i 
 
 oxide, I M 
 
 Antimonic \ g 
 
 acid, -' 
 
 ArseniouB ] i 
 
 acid, 
 Arsenic acid, 
 Stannous oxide, 
 
 brown. 
 Stannic oxide, 
 
 yellow. 
 Auric oxide, 
 Flatinic . _^ 
 
 oxide, I § 
 
 M 
 
 Iridic oxide, 
 
 [Oxides of Molybde 
 num],* brown. 
 
 [Selenious acid], red- 
 dish-yellow. 
 
 [Tellnrium acids], 
 black. 
 
 * The oxides of tungs- 
 ten and of vanadium are 
 precipitated as sulph- 
 ides only when their 
 solution mixed with 
 d.mmonic sulphide is de- 
 composed by an acid. 
 The solution of SnS in 
 ammonic sulphide is 
 precipitated by acids, 
 yellow, as SuSq. 
 
 Insoluble in 
 Ammonic Sulphide. 
 
 Mercurous 
 
 oxide, 
 mercuric 
 
 oxide,* 
 Argentic 
 
 oxide, 
 Plumbic 
 
 oxide,** 
 Cupric oxide, - 
 Cadmic oxide, 
 
 yellow. 
 Bismuthous oxide, 
 
 brown. • 
 
 [Oxides of 
 palladium], 
 [Oxides of 
 osmium], 
 [Oxides of 
 rhodium], 
 [Buthenic 
 oxide],*** 
 
 
 icl(t 
 
 oxi 
 CobSl 
 
 ox;i 
 Ferio 
 
 oxi 
 Feni 
 
 4 
 
 Tlraji 
 oxi 
 
 Tlraii 
 oxi 
 
 Uaiig 
 
 Zincii 
 [In^: 
 
 y61 
 [IhAl 
 
 oiiii 
 
 * Mercuric oxide is pre- 
 cipitated white or yel- 
 lowish by a little hydro- 
 gen sulphide ; by an 
 excess, black. 
 
 ** Plumbic oxide is 
 only completely precipi- 
 tated by hydrogen sul- 
 phide out of dilute, .and 
 not too acid solutions. 
 
 * * * The platinum- 
 metals are precipitated 
 with difficulty by TI^S. 
 
 BWro 
 
 awEc 
 sulpli 
 
 b3#.ai 
 
drochloric Acid, Hydrogen Sulphide, Amnionic Sulphide 
 arbonate, used successively. 
 
 he HjS precipitate see Table XIV. C. F. H ) 
 
 Ammonic Sulphide and Ammonia. 
 
 'des which are precipitated from neutral solutions (in the pre- 
 of ammonic chloride) by ammonic sulphide. 
 le solution should be supersaturated with ammonia before 
 Idition of the ammonic sulphide.) 
 
 Oxides, which are neither pre- 
 cipitated by hydrogen sulphide 
 nor by ammonic sulphide, are 
 by ammonic carbonate, in the 
 presence of ammonic chloride, 
 
 s Sulphides.* 
 
 3I0US 
 
 de, 
 
 Itous 
 
 de, 
 
 >us 
 
 Ab, 
 
 Ic 
 
 ide, 
 
 .ous 
 
 ide, 
 
 ic. |J.S 
 
 ■de, J ^ 
 
 ^anous oJiide, 
 
 ih-red. 
 
 c oxide, white. 
 
 oxidel,** 
 
 Ipwiah. 
 
 llious oxide],** 
 
 ok. 
 
 !-•« 
 
 incic sulphide Is in- 
 le in acetic acid, 
 .tous and' nickelous 
 tide are witli difli- 
 
 solubie in dilute 
 ichlorfc acid, and in 
 : acidj nickelous 
 ide is sliglitly solu- 
 a yellow ammonic 
 lide (containing am- 
 i)witlial>rown color 
 halliumand Indium 
 3t noticed further in 
 
 Tables, (traces of 
 only occur, and they 
 iBily detected by the 
 roscope.)' 
 
 As Oxides : 
 ,0 precipitlble by 
 ammonia. 
 
 a. Soluble in Potassa. 
 
 Alumina,* )^„,„,^^3, 
 [Glucina], ' 
 Chromic oxide, 
 
 green. 
 [Tantalio acid].** 
 [Mobic acid]. 
 
 b. Insoluble in 
 Potassa. 
 
 [Cerous 
 
 oxide], 
 [Iianthanic 
 
 oxide], 
 [Sidymic 
 
 oxide], 
 [Yttria], 
 [Zirconia], 
 [Thoria], 
 [Titanic acid], 
 
 As Salts:* 
 also precipitable by 
 
 ammonia. 
 
 a. In presence of 
 Phosphoric Acid. 
 
 Magnesia, crystal- 
 line. 
 
 b. In the presence of 
 Phosphoric or Oxa 
 lie Acid. 
 
 lime, J 
 Strontia, > white. 
 Baryta, J 
 
 Ammonic Carbonate. 
 
 precipitated:* 
 
 white. 
 
 Baryta, 
 
 Strontia, 
 
 Lime, 
 
 as carbon- 
 ates. 
 
 as phosphates or 
 oxalates. 
 
 * In presence of phos- 
 phoricacid, also'aluminic 
 phosphate. 
 
 ** Soluble after being 
 fused with potassic hy- 
 drate. 
 
 * The phosphates of 
 the alkaline earths are 
 insoluble in potassa, and 
 soluble in acetic acid , 
 the calcic oxalate is also 
 insoluble in acetic acid. 
 Aluminic phosphate ia 
 soluble In potassa. 
 
 * The precipi- 
 tation is only 
 complete in the 
 presence of am- 
 monia and upon 
 heating the so. 
 lution to boil- 
 ing. 
 
 not 
 precipitated : 
 
 a. Preoipitable 
 by Hydricdi- 
 sodio Phos- 
 phate (and 
 Ammonia). 
 
 Magnesia, 
 (crystalline,) 
 
 b. Not preoipi- 
 table by Sodic 
 Phosphate. 
 
 Potassa. 
 Soda. 
 
 [Lithia].* 
 [Ceesia]. 
 [Bubidia]. 
 Ammonia. 
 
 * Lithia is only 
 precipitated from 
 concentrated so- 
 lutions upon 
 heating by hy- 
 4ric-disodic 
 phosphate. 
 
TABLE VII. 
 Detection of Metallic Oxides. 
 
 VII. Treatment of the Precipitate formed by 
 
 A portion of the washed precipitate is digested with ammoDic sulphide (with potassio sul 
 to the liquid. (If the solution be partial, the remainiDg portion of the precipitate is subjected 
 dilute sulphuric acid be not white, milky (of sulphur alone), hut floceulent, and more or less a 
 according to A. — The precipitate insoluble in amnionic siilphide is examined according to B. 
 
 A. The Portion soluble 
 
 The yellow or orange-red precipitate (containing arsenious, stannic, or antimonious snlph 
 with concentrated solution of ammonic carbonate, and the sol 
 
 (a.) Solution contains : 
 
 Arsenious (a little stannic) sulphide. 
 Add some HjS solution, supersaturate with hydrochloric 
 acid, and warm ; dissolve the separated sulphide in fuming 
 nitric acid, or in hydrochloric acid and (a little) potassic 
 chlorate. When arsenic is present, a precipitate is formed in 
 the solution (after it has been supersaturE^ted with .ammonia, 
 and filtered from any separated stannic oxide), by a mixture of 
 magnesic sulphate, ammonic chloride, and ammonia. Traces 
 of arsenic are detected by converting into AsHg in Marsh's 
 apparatus, (arsenic spots disappear in sodic hypochlorite.) 
 
 Antimonic 
 
 Dissolve the sulphide in hv 
 and test the solution for:— 
 
 1. Antimony, by bringing 
 zinc on platinum foil (antim( 
 tion of SblJj (antimony spbti 
 blackened by ammonio-nitir! 
 acid cautiously evaporated) 
 
 2. Tin, by warming thei Si 
 black metallic powder, wash 
 chloric acid, and adding me 
 gray precipitate indicates' tii 
 
 * By treatment of the sulphides with cODceotrated hydrochloric acid with aid of heat, arsenious suJ 
 antimony and tin (according to {&)). The separation is more complete by digesting the solution of the Rul 
 arsenic alone will remain in solution, as an arsenite. 
 
 B, The Portion insoluble 
 
 The well-washed precipitate is treated by aid of heat, with concentrated nitric acid (fi 
 (before precipitation by hydrogen sulphide) was acidulated with hydrochloric acid, then 1 
 mercurous oxide (though it might from mercuric oxide), and but little plumbic sulphide. Osi 
 
 Residue may consist of; 
 
 Sulphur. 
 Yellow or gray, floc- 
 eulent, or balled up, 
 often inclosing metal- 
 lic sulphides. 
 
 Mercuric sulphide. 
 
 Black, floceulent. — 
 The solution in aqua 
 regia, somewhat eva 
 porated, is precipi- 
 tated by stannous 
 chloride. 
 
 Pluvibic sulphate. 
 
 White, pulverulent, 
 soluble in ammonic 
 tartrate with excess 
 of ammonia. 
 
 1' sulphide of mercury is found, the original fluid is tested for 
 mercuric and mercurous oxide. Hydrochloric acid is added to the fluid. 
 
 Precipitate. 
 Mercurous chloride. 
 Becomes black with ammonia 
 or potassa. 
 
 Filtrate. 
 
 Mercuric chloride. 
 
 Excess of stannous chloride pre- 
 
 cipitatesmetallic mercury; recog 
 
 nized by rubbing on clean copper. 
 
 Solution may c 
 
 Precipitate 
 Plumbic sul- 
 phate. 
 
 
 Preetpitat 
 
 Soluble in 
 
 Argentittcl 
 
 amnionic tar- 
 
 ride. ' 
 
 trate with ex- 
 
 Soluble 
 
 cess of ammo- 
 
 ammonia, i 
 
 nia, arid preci- 
 
 reprecipita 
 
 pitable by 
 
 by nitrioiai 
 
 potassic chro- 
 
 
 mate from the 
 
 
 solution. 
 
 
 For the recognition of i 
 solution, until the color v 
 tated sulphides are heate 
 
Hydrogen Sulphide in warmed acid solution. 
 
 phide if copper be present), filtered, if there be a residuum, and dilute sulpliurio acid added 
 the same treatment; if it be complete, this ia not necessary.) If the precipitate formed by 
 lored, it (or the original precipitate, if it is entirely soluble in ammonic sulphide) is treated 
 
 / 
 
 in Ammonic Sulphide. 
 
 de, or a mixture of them) is genlly warmed 
 ition filtered.* 
 
 Residue contains : 
 
 IS sulphide, alannic sulphide. 
 
 irochlorio acid and (a little) potassic chlorate, 
 
 several drops in contact with a fragment of 
 ny produces a deep black stain) ; or by forma- 
 do not dissolve in sodic hypochlorite, and are 
 te of silver, after oxidation by dilute nitric 
 
 ilution with zinc, dissolving the precipitated 
 3d off of the undissolved zinc, in warm hydro- 
 curie chloride to the solution. (A white or 
 
 The brown or brownish black precipitate 
 may contain : 
 
 Oupric sulphide (traces), 
 Platinic sulphide, 
 Iridic sulphide, 
 Auric sulphide, 
 Tellurous sulphide, 
 Molybdic sulphide, 
 Tungsiic sulphide, 
 Vanadic sulphide. 
 
 To be detected, 
 if their pre- 
 sence is sus- 
 pected, by the 
 methods of the 
 preliminary 
 examination. 
 
 phide remaius undissolved (to be further tested accordiap to (a)), whilst the solution may be tested for 
 phides in potassic sulphide with excess of sulphurous acid, finally expelling the latter by boiling ; the 
 
 in Ammanic Sulphide. 
 
 ee from chlorine). It is either fully dissolved, or there is a residue. If the original fluid 
 he precipitate can contain no argentic sulphide, and no sulphide of mercury arising from 
 lium, rhodium, and ruthenium need only be considered in the investigation of platinum ore 
 
 ontain ; Plumbic, argentic, bismuthous, cupric, cadmic [and palladious] oxides. 
 Dilute sulphuric acid is added to it. 
 
 Hydrochloric acid is added to the filtrate. 
 
 The filtrate is supersaturated with ammonia 
 
 Precipitate. 
 Bismuthous oxide. 
 Us solution in a 
 little hydrochloric 
 acid acquires a 
 whitish turbidity 
 with water, a black 
 with stannous oxide 
 in potassa. 
 
 The filtrate may contain : 
 
 Cupric oxide. 
 The blue ammoniacal 
 -olution is (after acid- 
 ulation) precipitated 
 reddish-brown by po- 
 tassic ferrocyanide. 
 
 Cadmic oxide. 
 The coloj'less am- 
 moniacal solution is 
 precipitated yellow by 
 hydrogen sulphide. 
 
 [Palladious oxide.] 
 The original (brown) 
 fluid is precipitated 
 black by potassic 
 iodide. 
 
 admic oxide inpresenee of cupric oxide, potassic cyanide is added to the blue ammoniacal 
 misbes ; when only cadmium will be precipitated by hydrogen sulphide. Or the precipi- 
 1 to boiling with dilute sulphuric acid, in which case only the cadmium is dissolved. 
 
TABLE VIII. 
 
 Detection of Metallic Oxides. 
 
 VIII. Treatment of the Precipitate formed by Ammor 
 
 [For a different treatment co 
 
 If nickel is present the filtrate, from the amnionic sulphide precipitate, is brown, -i 
 the resulting solution is heated with (not too much) nitric acid or potassic chlornte, in 
 ferric salt. If, upon dissolving the nmmonio sulphide precipitate in hydrochloric aci 
 dissolved in aqua regia, and the solution added to the hydrochloric acid solution. (If o 
 table. It serves also for determining, when iron is present, whether it is in the form i 
 
 The Solution is strongly supersaturated with Caustic Potassa, I 
 
 The Fluid or Filtrate may contain :*- 
 
 Chromic oxide, zincic oxide, alumina, aluminic phosphate,. 
 
 [gluoina]. 
 Boll the (green) potassa [or soda] solution for some time. 
 
 Precipitate : 
 
 Chromic oxide. 
 
 (Also glucina and zincic 
 
 oxide.) 
 Test by the blowpipe. 
 
 Filtrate may contain : — 
 
 Zincic oxide, 
 
 Alumina, 
 
 Aluminic phosphate,* 
 
 [Glucina]. 
 
 Separate the filtrate into two portions and add : — 
 
 To one part. 
 Hydrogen sulphide. 
 
 Precipitate : 
 Zincic sulphide. 
 
 To the other (after super- 
 saturating with hydrochloric 
 acid), 
 
 Ammonic carbonate. 
 
 Precipitate : 
 
 Alumina, aluminic phosphate, 
 
 [glucina]. 
 
 (Test by the blowpipe. 
 
 Glucina is soluble in ammonic 
 
 carbonate. ) 
 
 * Chromic and zincic oxjde cannot both be present in the alkaline 
 solution at the same time, as in that case, they form the compoand 
 ZnOCrgOg insoluble in potassa. Chromic and ferric oxides are suc- 
 cessively precipitated according to their relative quantities. Out of 
 a solution which contains magnesia in connection with alumina or 
 chromic oxide, a part of the magnesia is always precipitated by 
 ammonia or amnionic sulphide with those oxides as a gelatinous 
 compound insoluble in potassa. They are separated by boiling 
 with KH4CI, or by dissolving repeatedly in HCl and precipitating 
 by NH4HO in presence of much NH4CI ; the separation of chromic 
 oxide, the presence of which in the residue insolubje in potassa is 
 easily recognized by the blowpipe (by the green color of the bead), 
 from magnesia, zincic and ferjic oxide, and alumina is more per- 
 fectly effected by fusion with potassic carbonate and nitrate or by 
 beating the precipitate with sodic hypochlorite. For the detection 
 of a small quantity of alumina in connection with ferric oxide, the 
 precipitate by ammonic sulphide is boiled with potassa, the filtrate 
 supersaturated with HCI, and the clear liquid neutralized by am- 
 monic carbonate. The detection of phosphoric acid in connection 
 with alumina is effected by ammonic molybdate. 
 
 Cobaltous, nickelou 
 
 calcic oxalate; calcic 
 
 magnesia and zincic 
 
 Dissolve the 
 
 Filtrate m 
 
 Cobaltous, nickelous, and i 
 ma 
 
 Precipitate the fluid, sligh 
 with hydrogen si 
 
 Precipitate : 
 
 Cobaltous sulphide. 
 
 Nickelous sulphide. 
 
 (Zincic sulphide). 
 
 Test for cobalt by the bio 
 
 pipe, or by potassic nitril 
 
 for nickel by mixingtheliqu 
 
 heated with excess of potas 
 
 cyanide, with sodic carboni 
 
 iind hypochlorite.-f- 
 
 * The separation of zincic 
 potassa is not complete, on w 
 latter, some zincic oxide alwaj 
 and is found as zincic sulphide 
 zincic oxide, as well as from r 
 oxide, is more complete, and dt 
 tain, by boiling_ the aliglWi 
 acetate ; all the iron being pr( 
 A solution containing mangani 
 monia, deposits, when expos 
 manganese may easily pass in 
 
 t If nickel be present, a floe 
 after some time in the cold, 
 which must be tested by the 
 tates, from the slightly acii 
 nitrite. 
 
ide, or Ammonia, in presence of Ammonic Chloride. 
 
 B XIV, and notes. C. F. H.] 
 
 hed, the precipitate is treated upon the filter with warm, dilute hydrochloric acid, and 
 jy the hydrogen sulphide, and to convert any ferrous salt that may be present into a 
 idue remain. (CoS or NiS), it is first to be tested before the blowpipe for cobalt, then 
 to be sought for, the original fluid may also be employed for testing according to this 
 irric oxide.) 
 
 Sodaj] and gently heated and filtered, if a Precipitate remain. 
 
 The Precipitate may contain : 
 
 , ferric, and uranic oxides; baric, strontic, calcic, and magnesic phosphates; 
 rare earths insoluble in potassa.] (Also alumina and chromic oxide with 
 xide with ferric oxide.*) 
 litate in a little hydrochloric acid, add ammonic chloride and ammonia. 
 
 ides, (zinclc oxide, 
 
 with acetic acid, 
 
 I of heal. 
 
 Filtrate : 
 ;anou3 oxide, 
 lagnesia). 
 te to dryness, and 
 idue by fusing with 
 innate and nitre 
 lum foil. A bluish 
 I indicates manga 
 test the original 
 with plumbic per- 
 aitric acid. 
 
 c oxide by means of 
 the presence of the 
 ,he ammouiacal fluid, 
 1 otftirric oxide from 
 elous, and cobaltous 
 quantities more cer- 
 after adding sodic 
 isent as ferric oxide. 
 QIC chloride, and am- 
 rauic oxide, so that 
 precipitate, 
 jli precipitate forms, 
 on gently_ warming, 
 ,a-sic nitrite precipi- 
 )w potassio-cobaltic 
 
 Precipitate may contain : — 
 
 Ferric and uranic oxides ; baric, strontic, calcic, and magnesic 
 phosphates; calcic oxalate ; calcic fluoride; (all rare earths ;) 
 (also alumina, chromic and manganic oxides). 
 
 Digest the precipitate with concentrated solution of ammonic 
 carbonate. ■)- 
 
 Residue may contain : — 
 
 Ferric oxide; baric, strontic, calcic, and 
 magnesic phosphates'; calcic oxalate, (and 
 fluoride.) 
 
 Dissolve in a little hydrochloric acid, and 
 test the solution in separate portions for : 
 
 a. Ferric oxide (with potassic ferrocya-, 
 uide). 
 
 b. Baryta and strontia (with solution of 
 calcic sulphate). 
 
 c. Lime (with potassic [or ammonic] oxa 
 late and sodic acetate). 
 
 d. Magnesia (add sodic acetate, then ferric 
 chloride until reddish color is produced, 
 heat to boiling, precipitate the filtrate 
 with ammonic carbonate, and test with 
 sodic phosphate. 
 
 e. Phosphoric acid (add, whilst cold, sodic 
 acetate, then a drop of ferric chloride ; 
 or with ammonic molybdate). 
 
 /. Oxalic acid (calcic oxalate is precipi- 
 tated white by sodic acetate ; the preci- 
 pitate is insoluble in acetic acid, and is 
 changed by ignition into calcic carbo- 
 nate).* 
 
 g. Fluorine (with the original substance). 
 
 * Also ferric phosphate is, when cold, precipi- 
 tated from the hydrochloric acid solution (made 
 as neutral as possible) by sodic acetate. (Yel- 
 lowish, floctiulent or gelatinous.) 
 
 Solution may con- 
 tain : — 
 Uranic oxide,* 
 Cerous oxide, 
 Lanthanic oxide, 
 Didymic oxide, 
 Yttria, 
 Thoria, 
 Zirconia, 
 
 * When uranic oxide is 
 present, the solution, af- 
 ter supersaturation with 
 hydrochloric acid, gives 
 a brown precipitate with 
 potassic ferrocyanide. 
 
 ** They almost all form 
 with potassic sulphate 
 difficultly soluble double 
 salts. 
 
 t Digestion with am- 
 monic carbonate is only 
 employed when there is 
 reason to examine for 
 rare oxides. 
 
TABLES IX. AND X. 
 Detection of Metallic Oxides. 
 
 IX. Precipitate by Amnionic Carbonate in p^ 
 
 Baric, Strontic, Calcic Oc 
 
 The washed precipitate is dissolved upon the filter in a little hydrochloric acid [or in 
 
 three portions. If only one base is to be sought the original solution can also be employed 
 
 I. Portion, 
 
 II. Portion. 
 
 III. Portion. 
 
 Add 
 caldc sulphate. 
 
 Precipitate with excess 
 of dilute sulphuric acid,* 
 supersaturate the filtrate 
 with ammonia, and add 
 potassic [or ammonic] 
 oxalate. 
 
 Precipitate insoluble in 
 acetic acid. 
 
 a. When baryta is present. — Eva-' 
 porate to dryness, digest the residue 
 with alcohol, and ignite the .^Z^ra^e. i 
 
 Crimson flame : — 
 
 Immediate precipitation : 
 
 Strontia. \ 
 
 b. When barytfl is absent.— &tTont\a, 
 is then also recognized with certainty 
 by the entire absence of turbidity, even * 
 after a long time, upon the addition 
 of strontio sulphate to the hydro- 1 
 chloric acid solution, whilst calcic!! 
 sulphate produces in it a precipitate i 
 in a short time. •% 
 
 Baryta. 
 
 Turbidity after some 
 time: 
 
 Lime. 
 
 Strontia. 
 
 Fluid remains clear : 
 
 * In the absence of baryta 
 and stroutia precipitation by 
 sulphuric acid ia unneces- 
 sary. 
 
 * Or add not too little dilate solution o: 
 Add to the liquid dilute sulphuric acid, flit 
 and add ammonic oxalate. Precipitate (ii 
 
 Lime. 
 
 X. Fluid which is Precipitated neither by Hydrogen 
 
 It may contain : — Magnesia, Potassa, Soda, Lithia, ^ 
 Evaporate a portion (not too small) of the fluid-upon platinum foil; if after ignition no r( 
 
 Test for Ammonia. 
 
 Test for Magnesia. 
 
 II 
 
 Warm the origing,l substance, or its 
 solution, (not the fluid X.,) with calcic 
 hydrate. 
 
 The presence of 
 
 Ammonia 
 
 is recognized by the odor, as well as 
 by the white cloud which arises when 
 a glass rod moistened with hydro- 
 chloric acid is brought near. 
 
 Slight traces may be detected by 
 condensing the vapor, developed bj 
 calcic hydrate, in a test-tribe, and 
 adding to it an alkaline soltition of 
 mercuric iodide in potassic iodide; 
 ammonia producing a brownish-red 
 precipitate. 
 
 1 > 
 
 Add sodie phosphate (and free 
 ammonia if not already .present) to 
 a portion of the fluid X. (or to the 
 original solution if it contain no 
 oxides of the heavy metals or allta- 
 line earths). 
 
 The presence of magnesia is 
 manifested by a crystalline preci- 
 pitate, which forms slowly when 
 only traces of magnesia are pre- 
 sent. (If the separation of the 
 alkaline earths by ammonia and 
 ammonic carbonate did not take 
 place at a boiling heat, sodic phos- 
 phate will always give a small, 
 flocculent precipitate of a phos- 
 phate of an alkaline earth.) 
 
 a. When magri 
 ignite gently (to| 
 overflowing with: 
 a crimson of lithii^ 
 residue for potai 
 solution ; for litm 
 or by a mixture t 
 flame. 
 
 b. When magnt 
 and warm with w 
 Remove the exce 
 acid), and evapor 
 by the spectrosco 
 
 * Potassa [rubidl 
 upon their colored f 
 envelope of a (pure 
 flat glass bottle witl 
 the flame will entim 
 or lithia. If the fla 
 [rubidia and csesia] 
 
 [Traces of sodiun 
 from organic acids f 
 of PtCli, and gentl 
 needles, best distiui 
 
Snce of Amnionic Chloride and Free Ammonia. 
 
 ^ate, or a mixture of them. 
 
 etio acid if the Second Method below is to be used], and the solution divided into 
 ir this purpose. 
 
 [Second Method, c. f. h.] 
 
 Hssolve the precipitate by ammonie carbonate 
 dilute acetic acid, and add to the solution 
 •Ural polaasic chromate. 
 
 Precipitate (yellow). Baryta. 
 Supersaturate the filtrate with ammonia, and 
 U ammonie carbonate, wash the precipitate 
 Irontia and lime), dissolve in a little acetic 
 d, and to a portion of the solution add, not 
 I little, calcic sulphate.* 
 
 Turbidity after some time. Strontia. 
 Precipitate the strontia from another portion 
 dilute sulphuric acid, filter, supersaturate the 
 rate (or acetic acid solution, if stronti.a be 
 !ent_) with ammonia, and add ammonie oxalate. 
 Precipitate (insoluble in acetic acid), Iiime. 
 
 Eemarks. 
 
 If no metallic oxide preeipitable by hydrogen 
 sulphide or ammonie sulphide be present, the 
 original solution may also be used for these 
 tests (except that of Portion 111. a), the presence 
 of magnesia or of the alkalies not interfering 
 with the result. 
 
 Baryta is also recognized with certainty in 
 presence of strontia and lime, by a solution of 
 ctrontic sulphate, which causes a white precipi- 
 tate with it, appearing only after some time 
 with traces of baryta. Separation of baryta 
 from strontia is effected by hydrofluosilicio 
 acid, with addition of alcohol, in which baric 
 silicofluoride is quite insoluble. The alkaline 
 earths may also be detected by the spectroscope. 
 
 lotassic sulphate fl part by weight to 200 by measure of water). TurMdity after some time, Strontia. 
 . supersaturate the iiitrate (or liquid if uo turbidity was produced by potassio sulphate) with ammonia, 
 iluble in acetic acid). Lime. 
 
 lulphide, Ammonie Sulphide, nor Ammonie Carbonate. 
 
 ubidia, Ocesia, Ammonia, or a mixture of these bases. 
 
 due remains, neither magnesia nor the alkies need be considered, but ammonia should be. 
 
 Test for Potassa, Soda, Lithia, Rubidia, and Csesia. 
 
 I is absent. Evaporate fluid X. (to which no sodic phosphate has been added) to dryness, 
 move the ammonie salts), test the residue before the blowpipe upon platinum wire, or by 
 iohol and igniting. A violet flame indicates presence of jt)otesjft„[rubidia and ciBsiaj alone, 
 I yellow of soda, or a mixture of soda with potassa or lithia.* lti"'ti^le latter case, test the 
 [rubidia and csesia], by tartaric acid, or platinic chloride and alcohol in not too dilute 
 by boiling with sodic carbonate and phosphate, whereby a salt forms, soluble with difficulty ; 
 Einhydrous ether and alcohol, in which lithic chloride dissolves, recogn^able by the crimson 
 
 I is present. Evaporate to dryness, ignite the residue gently, to remove ammonie salts, 
 ir. Add to the solution baryta-water, or milk of lime to alkaline reaction, boil, and filter, 
 of baryta or lime by ammonia and ammonio carbonate (or of baryta by dilute sulphuric 
 I the filtrate to dryness. If there is a residue, proceed witli it as in a. Or test for alkalies 
 
 ;£esia], soda, and lithia can also be distinguished by the effeqt of transmission through colored media 
 les. If the substance to be tested (best as a sulphate) is held in theioop or^j^latinum wire in the outer 
 e) gas or alcohol flame, if sodn be present the whole upper part of the flame will be colored yellow. If a 
 arallel sides containing a solution of indigo is now brougl^hetween the eye aad the flame, the color of 
 disappear, in case only soda be present; a simple changf, however, to violet or red indicates potassa, 
 I is then observed through deeply colored cobalt glass, thj violet color remains by presence of potassa 
 -g last two as well as the alkalies in general are detected wim most certainty by means of the spectroscope 
 re most readily detected, and distinguished from potassium, when both are in f^rm of chlojides (frei 
 other bases), by placing a drop of the concentrated aqueWs solutipn on a slip of glass, adding " ^-"■ 
 t^aporatiug, when potassic platinic chloride will crystalilz^ in octahedra, and the sodic s^ in 
 ahable by a magnifier.] ' .£ 4 
 
 potassa 
 poscope. I I 
 es (free^ 
 ^ a dro^H 
 . orang^H 
 
 =3 
 
TABLE 
 Detection ob Acids. Prelim 
 
 Examination. 
 
 • XL BeHavior of 
 
 )f mefflore important Acids, or.of t1 
 : ." ' • " CcAentratedJ 
 
 A quantity of the dry compound, ab<j,ut as much as will lie upon th* poin' °f *i Tu S 
 upon it, and th* he&ted, bvft not to the boilitg point of sufhuric acid.: With »'''''''"" ,?^ 
 of a vapor or gas may be'observed, fi-om the properties of which, iti molt c^ses,-tne na^e^ 
 
 / 
 
 Non- Volatile Acidg. 
 
 iVb gas or nui^ is evolved * 
 Theicompound doWnot blacken by 
 ignition. 
 
 Silicic Acid, recognizafeleijby 
 means of phosphorus salt before the 
 blowpipe. 
 
 Boracic Ao^l after addition of 
 sulphuric acidf it Colors the alcohol 
 fliuhe greefi. 
 
 ' Phosphoric AGid,.precipitftble 
 in neutral solution by magnesic sul 
 phate, a^hionic chloride, and. am 
 monia; in acid solution .by ferric 
 chloride and sodic acetate. 
 
 Arsenic Acid, like the preced- 
 iijg, but the compound gives with 
 ^odic carbonate upon charcoal ar 
 sefiical odor. j [^^^ 
 
 Sulphuric Acid, thelSompaund 
 •gives hepar wh«n l^ated with sodic 
 carbonate upon charcoal. 
 
 Selenic Acid, like th« preoecl 
 ing. The 'baryta salt is decomposed 
 by boiling with concentrated hydro 
 chloric acid. , 
 
 Tungstic Acid, recognizable by 
 
 the blowpipe; becomes blue with 
 
 zinc and hydrochloric ^cid, 
 
 , Molybdic Acid, recognizable 
 
 d by the bloWpipe; becomes first blue* 
 
 i^then browD with' zinc and hydro- 
 
 "chloric acid, I 
 
 Titanic Acii 
 
 the' blowpjpe; bej 
 zinc and hydrocj 
 
 Iodic Acid, 
 
 of iodine||m-m oi 
 )hate.^rhe ci 
 larcoa! 
 
 recognizable by 
 ^iolet with 
 
 Acids'Watile, or R 
 
 ' A colored gas is'evolved. 
 
 The compeund.Boes qot 'blacken by 
 
 ign^ioD. 
 
 Biro 
 
 ceding; 
 
 ; me 
 
 Hydriodic ^oid„ the violet va- 
 por folors stanch blue. 
 
 Hydrobijomic Acid, the brown 
 vagor colors starch a fiery yellow. 
 
 44:id. * Like the pre 
 e salt 'deflagrates upon 
 chai-coal. * « ■ 
 
 Chloric Acid, the greeni^-yel 
 low gas readily explodes ; the dom 
 pound deflagratfes upon'chaa'coal. 
 
 Hy.pochlorous Acid, yellow- 
 sh-green ^Jjlorine gas, like the pre- 
 ceding discoloring solutiqn of indigo 
 
 Nitron^|&.cid, r\ 
 
 
 imes ; even 
 Citric acid. 
 
 with dilut&snlphurit 
 
 Nitric .Acid, nearly colorless 
 acid fumes, which ireredxt chlorine 
 be present; SeM^r red if ferrous 
 sulphate or organic substances be 
 added. 
 
 The compound B 
 by igrj' 
 
 / 
 
 Carbonic A^ 
 
 ders lime-w^6i^tu] 
 
 Cyanic Acid,$ 
 
 renders lime-water 
 
 Sulphurous A< 
 
 by its odor ; •colors 
 sic chromate green 
 
 Hydrp^ulpb'^ 
 
 drogen sulphide, •)<{ 
 
 odor ; colors leadf 
 
 • 
 ' Hydroehlorio 
 
 piously, and .pre8(j 
 
 of silver on a gjas! 
 
 precipitate dissofl; 
 
 Nitric. Acid,' 
 
 fumes, which becui 
 tion -of ferrous sjj 
 filings. I 
 
 Hydrc^oric 
 
 fuinn)^_ corrosive i 
 face coated with-j 
 rendered dim in th 
 the gas. Fluorl' 
 glass tube with 3 
 addition to^HP.'ti 
 gas, which gives' 
 silica on a glass n 
 water. , Siliooflubi 
 larly,; they also* 
 ride in^ platinnm 
 phuric acid. - S 
 
 ft 
 
 Tffl^O] 
 
 b^he above methods ^ hydraMd is found, the dry compound contains the co* 
 ith a nitrate develops. cU^age and fed vapors; al^^with a chromate brownis! 
 Jdes with, concentrated snlpnWic acid n-equeutly devCT^siPlphuroUs acid. 
 
 nding haloge 
 famea. 9J 
 
 sj^ed 
 
le Halogens, upon MatiJ^ their. Oompotfnds .with' 
 ' Iphuric AcM. - " ' 
 
 T 
 
 .'e, is placed id a test- tnb'b .and 
 is, or those which suffer decj 
 \ the acid or of the halogen 
 
 .aDdiL-4 titnes i^s volume of cqgqentrated sulphuric acid poured, 
 
 fipoation by sulphuric acid atu'W^h temperature, the evolution 
 ay be inferred.* . 1? ^ • ' ' 
 
 icomposable with Evolution'of Volatile Ffodiicts, . • 
 
 The vapors or gq^es fvolveS'et-e colorless. 
 
 ■m 
 
 ^\ 
 
 aes not blacken - 
 Ition. 
 
 W 
 
 odorless, ren- 
 
 sxcites tears, jind 
 *turbid; ' 
 
 :iti, recognizfjj^ie 
 di^olved pota'S. 
 
 ■ " i * 
 
 10 Acidi C^^y- 
 
 eco^^ible by its 
 pappl^w.n. ' 
 
 A6ij3, fumes co- 
 )itates a solution 
 
 rod oardy; this 
 ;a ip ammonia. 
 
 nearly eolofltss 
 be red upon addi- 
 phate or copper 
 
 Acidj^opionsly 
 as. .A gl&sssur- 
 ax a^d traced js 
 J traced places by 
 les develop in a 
 jlblyiric' acid, id' 
 so'eiticic fluoride 
 a precipitate of 
 i moiTOned" with 
 ides behave simi- 
 folve silicic fluo- 
 oible with aul-,, 
 
 ^ The coi^podnd is'decomposed by i gdjji'o n. 
 
 Mostly without separation' of carboB. • With sgpalSion of oarbop. 
 
 Oxalic Acid, develops carbonic 
 a^id and carb.ouic oxide ; ttfe Jime 
 salt is iasoluble in acetic acid. 
 
 Formic Acid, evolves osly com- 
 bustible ckrbonic oxide gas. * 
 
 : Vllydtfecyanic Acid,Alike the 
 
 '"l^fegedingj. but evolves with *dilu^, 
 
 " " "oric acid hj|drt)Cjanic acid. 
 
 ^e;rocyamo AciQ, like 
 
 * :J*he soluble compdund 
 
 d Blu^by^rrjc salts. 
 
 Hydrofeiricyanic Acid, like 
 the preceftg; the soluble compDund 
 is precipitated blue by /erroas saltsT 
 
 Cbronuf; Acid, evolves oxygen, 
 ai|^ the fluid becom^-4>rown» or 
 g^Sn, Givgs a gre 
 phospfc 
 
 lead with 
 
 Hypos' 
 Trithio; 
 Tetrat! 
 'Peutathio^ 
 
 8 'of which only th% hypo- 
 
 ■asulpharic)l8 of frequent 
 
 volve^ith sulphuric acid, 
 
 id, J^th'Bei^aratiou of sul- 
 
 iGH'of 'the alk'alies give 
 
 in a glass tub'e. 
 
 4 ■ "■ 
 
 a.' Acids rmt volatij^per se. 
 
 ',AU. compounds (jf thas^oids are de- 
 composed ^y cOKentrat'd sulphuric acid, 
 blackening. th^Tety, and developing CO., 
 CO, ain.d SOj. 
 
 Tartaric Acid, theanid potasaic 
 suit \B .soluble with difficulty ; the 
 lime s^It is soluble' in caustic po- 
 
 tassit. 
 
 Race'mic Acid; tift lime salt 
 is rnsolrfble.in atjimonic chloride, g 
 
 Gi^ric Acid<; give^lprecipitate 
 with excess of lime^lKer only on 
 'boiling. /. • . 
 
 . Malic Acidr is n^t preci^tat^ 
 by lime-water,' either cold or warm. 
 
 Lactic Acid, dissolves readily 
 lin ether. .The lime salt is easily, 
 the zipc difficultly> soluble in water. 
 
 Tannic Acid, gives a white, 
 visoqua (Precipitate with' gelatine, a 
 blue-black with ferric saUs. 
 
 Gallic Acid, not precipifeble by 
 gelatine ; lerric salts njoduoe a 
 blatfk precipitate. 
 
 IJric Acid, gives a»red color 
 with • ammonia, after ataporation 
 with nitric acid. v 
 
 ; b. Acids volatite perse. 
 
 I 
 
 Asi 
 jouilc 
 
 The compoiThdidoes not blacken, or but 
 slightly, with s.ulphuric acid.' 
 
 Acetic Acid, gives, with sul- 
 phuric acid and alcohol, ace,tio ether. 
 Their neutral 
 salts are 'preci- 
 pitated a light 
 brown b^erri(| 
 chloride.™ i 
 
 Benzdic -Acid, 
 Succinic- *" 
 
 combined With a' metals In a mixture of salts other reac^ns often take place ; thus a metallic chloride 
 ohlo'i^hroin^ acid, etc. The chlorides of mercury %re hdrdlxdecpmposed by sulphuric acid. Metallic 
 
 ■ a, ' ':'''lw, v _ .' ^ _;: : [ , 
 
TABLE XII. 
 
 Detection of Acids. 
 
 Xll. Behavior of the more impo- 
 
 A. Detection of acids in soluble compounds.— The aqueous solution is neutral, acid, or alka 
 one as neutral as possible, it is often necessary to remove the heavy metallic oxides or the ea 
 well as phosphoric or oxalic acid combined vfith alkaline earths. The quality of the base oti 
 generally an acid cannot be present in a neutral or acid solution which already contains the ss 
 by baryta, can be present in a soluble baryta compound; no chlorine in a silver com pound, sol 
 that in any compound such acids as have been added (for solution or neutralization) "ff <* n( 
 halogen), the nitrate is used ; e. g., in compounds of silver, of lead, or of mercurous oxide, bi 
 
 Precipitated by Hydro- 
 chloric or Nitric Acid : 
 
 From their soluble compounds, gene- 
 rally showing alkaline reactions. 
 
 Silicic Acid, gelatinous ; in di- 
 lute solution only after evaporating 
 the acid fluid ; also precipitable by 
 amnionic cnrhonate or chloride. 
 
 Boracic Acid, crystalline, only 
 from cuuceutrated solutions. Colors 
 the alcohol flume green upon addi- 
 tion of sulphuric acid. 
 
 Antimonic Acid, white, soluble 
 in tartaric acid. 
 
 Tungstic Acid, white ; by boil- 
 ing, yellow; with zinc and hydro- 
 chloric acid, blue. 
 
 Molybdic Acid, white, soluble 
 in excess, with zinc and hydrochlo- 
 ric acid blue, finally brown. 
 
 Sulphur, yellowish or white ; 
 with the evolution ofSOj from hypo- 
 sulphites, [thiosulphates] and H^S 
 from metallic polysulphides. 
 
 lodiile, out of a solution of an 
 iodide and an iodate or nitrite. 
 
 Also several oxides and sulphides 
 soluble in potassa, and cyanides or 
 chlorides soluble in potassic cyanide. 
 If the alkaline fluid be saturated 
 with hydrogen sulphide, all the acids 
 of the metals which form sulphides 
 insoluble in acids, are precipitated, 
 after acidulation, as sulphides. 
 
 Of the organic acids, benzoic, uric, 
 and tartaric acid (the latter as acid 
 potassa salt) may be precipitated by 
 acids from alkaline solution. 
 
 Precipitated by Baric 
 Chloride 
 
 (or Baric Nitrate) : 
 
 From the solution previously acidulated 
 with hydrochloric or nitric acid. 
 
 Sulphuric Acid, white, pulveru- 
 lent; quite insoluble in water and ip 
 acids. (In the presence of too much 
 and concentrated free acid, baric 
 chloride or baric nitrate is precipi- 
 tated; soluble in much water.) The 
 original compound gives hepar with 
 sodic carbonate upon charcoal. 
 
 Selenic Acid, like the preced 
 ing. The precipitate, when boiled 
 with concentrated hydrochlpr|c acid, 
 evolves, chlorine, and ^^murous 
 acid, then ''precipitate^^^^K the 
 solution red selenium. ^^^Higinal 
 compound gives upon fflHRoal be- 
 fore the blowpipe the characteristic 
 selenium odor. 
 
 Hydrofluosilicic Acid, like the 
 preceding, not out of very dilute so- 
 lution. The original compound gives 
 upon heating silicic fluoride and a 
 metallic fluoride, with plkalies a 
 silicate and a fluoride. 
 
 Only from m 
 The precipitate i 
 
 Phosphoric 
 
 freshly precipital 
 acid without eflei 
 
 Arsenic Acii 
 
 also easily solubl 
 ride. The soluti 
 acid is precipitab 
 phide with the ai 
 
 Boracic Aci( 
 
 luble in ammX)uii: 
 cipitated.Ksom dil 
 meric paptr dipj 
 hydrocHbric acid 
 dryinjp' 
 
 Carbonic A( 
 
 in acids with elt'e 
 
 Sulphurous 
 
 from coucehtrati 
 zinc and hydroci 
 hydrogen sulphif 
 
 Tartaric Aci 
 
 ammouiu chlorij] 
 tassa ; the potai 
 precipitate becot 
 ing. 
 
 Citric Acidv 
 
 boiling the fluid t 
 lime-water or an 
 
 Hydroferroj 
 
 forms slowly, si 
 in acetic acid. ' 
 
Iirtant Acids towards Precipitants. 
 
 '^ne, to be determined by test paper. If the acid is to be sought in an ammoniaoal solution, or 
 '"»ths that may be present (according to Table VI.), by which means metallic acids are fouLd, as 
 *ifen excludes the presence of one or more acids, thus rendering search for them unnecessary; 
 1»»ne metallic oxide that must serve as precipitant for this acid ; e. g., no sulphuric acid, detected 
 'Wble in acids, etc. (For exceptions in alkaline solutions, see Table XII. below.) It is evident 
 '% be sought ; in all compounds where the reagent can act as precipitant through its acid (or 
 "'(kric nitrate is used (instead of baric chloride). (See continuation, Table XIII.) 
 
 Irecipitated by Calcic Chloride ! 
 
 itutral solution. 
 iki soluble in acetic 
 lid. 
 
 taiiioicl, white, when 
 MiJd soluble in acetic 
 iilivesceace. 
 
 icW, like phosphoric; 
 f«i* in ammonic chlo- 
 liw in hydrochloric 
 ii|ie by hydrogen sul- 
 \H of heat. 
 
 ijJi, white, easily so- 
 uiohloride; not pre- 
 tahte solution. Tur- 
 jlf^dnn a solution in 
 liiidbetMunes brown on 
 
 litlid, white, soluble 
 niiivescence. 
 
 ginaLCid, white, only 
 (did solutions; with 
 Ijiijorio acid, evolves 
 
 j{jj, white, soluble in 
 {lbs and caustic po- 
 ii(ia solution of the 
 ,l(«es turbid by boil- 
 
 jjjivhite, but only by 
 ijilipersaturated with 
 ,,»iouia. 
 
 jg0aia.c Acid, 
 i|,*ble with difficulty 
 
 From neutral and from acetic solution. 
 
 Precipitate is insoluble in acetic 
 
 acid. 
 
 Oxalic Acid, white; insoluble 
 in ammonic chloride ; the precipi- 
 tate also forms with calcic sulphate 
 solution ; the original compound 
 evolves with concentrated sulphuric 
 acid CO and CO^ without blackening. 
 
 Racemic Acid, white, insoluble 
 in ammonic chloride. Also formed 
 with solution of calcic sulphate. 
 
 Hydrofluoric Acid, gelatin- 
 ous ; the precipitate evolves, with 
 concentrated sulphuric acid, hydro- 
 fiuoric acid, which etches glass. 
 
 Sulphuric Acid, white ; not 
 From ^J||^ solutions; completely 
 upon a^^on of alcohol. 
 
 from Uj||e 
 upon a^Rc 
 
 Precipitated by Magnesic 
 Sulphate 
 
 (or Magnesic Chloride) : . 
 
 In the presence of ammoriic chloride 
 and free ammonia. 
 
 Phosphoric Acid, white, crys- 
 tnlliue; slowly if the solution be 
 very dilute, soluble'in all acids. 
 
 Arsenic Acid, like the. preced- 
 ing. The acid solution of the preci- 
 pitate is precipitated by hydrogen 
 sulphide by the aid of heat. 
 
 Tartaric Acid, white. Tie 
 precipitate forms slowly and only in 
 concentrated solution ; it blackens 
 on ignition. 
 
 Separation of Oxalic, Tartaric, Citric, and Malic Acid. 
 
 Calcic chloride and lime water are added to alkaline reaction. 
 
 ~V 
 
 Fluid contains aS salt of lime: — 
 Citric Acid. Malic Acid. 
 
 Heat to boiling. 
 
 Filtrate : 
 
 Calcic Citrate. 
 
 Soluble in cupric 
 
 chloride. 
 
 Calcic Malate. 
 
 Precipitahle, 
 after evaporation, 
 by alcohol (and 
 then to be further 
 tesled). 
 
 Precipitate soDtaina as salt of lime : 
 Oxalic Acid. Tartaric Acid. 
 
 Treated with cold, not too dilute 
 
 potassa solution. 
 
 Residue. Filtrate. 
 
 Calcic Oxalate. 
 
 Insoluble in 
 acetic acid and in 
 cupric chloride ; 
 soluble in hydro 
 chloric acid. 
 
 Calcic Tartrate. 
 By boiling the 
 pot.assa solution 
 is precipitated 
 gelatinous. 
 
■ TABLE XIII. 
 Detection of Acids. 
 
 XIII. Behavior of the more important Aci( 
 
 B. Detection of acids in compounds which are insoluble in water and in acids. — From the ^ 
 must have been ascertained. — Inorganic compounds (which, ignited alone, afford no carbon) s 
 aqueous extract (neutralized by hydrochloric, nitric, or acetic acid) is examined according 
 decomposed by digestion with ammonic sulpjiide, the sulphates of the alkaline earths by hoi 
 sulphides afford sulphuric acid by treatment with nitric acid, aqua regia, or hydrochloric acid 
 with alkaline carbonate ; and the ferrTc salts of volatile organic acids, also by ammonia; the 
 and XIII. 
 
 Acids recognizable by Ferric Chloride. 
 
 A precipitate is formed. 
 
 a. In the presence of free hydrochloric 
 
 acid. 
 
 Hydroferrocyanic Acid, 
 
 blue ; the precipitate i-s decomposed 
 by potassa into ferric oxide and 
 potassic ferrocyanide. 
 
 b. In neutral solutions, or those con- 
 
 taining only free acetic acid. 
 
 (If free hydrochloric acid be present, 
 add sodic acetate.) 
 
 Phosphoric Acid, yellowish- 
 white ; iiiooluble in acetic acid, solu- 
 ble in hydrochloric acid and in ferric 
 acetate and in ferric chloride. 
 
 Arsenic Acid, like the preced- 
 ing; the original compound gives 
 with sodic carbonate an alliaceous 
 odor. 
 
 Tarmic Acid, dark blue. The 
 original compound is precipitated 
 by gelatine. 
 
 0. Only in neutral solution. 
 
 Boracic Acid, yellowish. Tur- 
 meric paper dipped in the hydro 
 chloric acid solution becomes, after 
 drying, brown, and then upon moist- 
 ening with a drop of potassa solu- 
 tion black. 
 
 Benzoic Acid, light brown. 
 The original couceutrated solution 
 is precipitated crystalline by hydro- 
 chloric acid. 
 
 Succinic Acid, like the pre- 
 ceding. Tne concentrated solution 
 of the ammonia salt (obtained by 
 digestion of the ferric salt with am- 
 monia) is precipitated by baric chlo- 
 ride in the presence of alcohol and 
 free ammonia. 
 
 A color is produced. 
 
 a. In the presence of free hydrochloric 
 add. 
 
 Hydroferricyanic Acid, 
 
 brownish. Ferrous salts produce a 
 blue precipitate, 
 
 Hydrosulphocyanio Acid, 
 
 [Sulphocyanic] intense blood-red, 
 not removed by much hydrochloric 
 acid, but is by mercuric chloride. 
 
 b. Only in neutral solution. 
 
 (The color vani.shes oq addition of hydro- 
 chloric acid.) 
 
 Acetic Acid, reddish-brown ; 
 the original salt warmed with alco- 
 hol and sulphuric acid gives the 
 odor of acetic ether. 
 
 Formic Acid, like thejpreced- 
 ing. The original compound reduces 
 argentic or mercuric oxide with 
 evolution of carbonic acid. 
 
 Sulphurous Acid, like the pre- 
 ceding; on boiling, the color van- 
 ishes without precipitation. The 
 original compound, upon the addi- 
 tion of hydrochloric acid, gives the 
 odor of sulphurous acid. 
 
 Meconic Acid, blood-red, un- 
 changeable by auric chloride. 
 
 Gallic Acid, black. The origi- 
 nal solution is not precipitated by 
 gelatine. 
 
 Acid-s 
 
 /: 
 
 Only from net 
 
 The precipitate ii 
 nitrm 
 
 Phosphoric 
 
 yellow; also pee 
 monic chloride,!^ 
 nesic sulphate. 
 
 Arsenic Aci 
 
 the original com] 
 table by H^S. 
 
 Arsenious Ac 
 
 wise like the pre© 
 
 Chromic Acii 
 
 nal yellow or rede 
 green by SOj. 
 
 Oxalic Acid^ 
 
 acetic acid. The 
 wise insoluble in i 
 
 Boracic Acid 
 
 acetic acid ; grje 
 after the addition 
 
 Sulphurous ,A 
 
 ening on boiling. 
 
 Hyposulp]3i|r 
 
 sulphuric Acid] ? 
 pidly ; soluble in e 
 sulphite. 
 
 * All these preciji 
 ammonia. The saltt 
 and •metaphosphatef 
 nitrate white ; the I 
 addition of acetic aci 
 albumen. In concei 
 tates are also prec 
 nitrate. 
 
is towards Precipitants and Indigo Solution. 
 
 feliminary examination, the general nature of the compound and the acids possibly present, 
 re finely pulverized, and fused with fourfold weight of pure sodic-potassio carbonate, and the 
 |to Tables XII. and XIII. Insoluble compounds of the heavy metallic oxides may also be 
 ling with a concentrated solution of sodic carbonate ; the filtrate contains the acid. Metallic 
 iind potassic chlorate. The salts of organic acids insoluble in water are decomposed by boiling 
 (filtrate contains the acids combined with the alkali, and is examined according to Tables XII. 
 
 Precipitable by Argentic Nitrate. 
 
 utral solution. 
 
 e soluble in dilute 
 lacid.* 
 
 iAcid, (tribasic) 
 
 pipitable by am- 
 
 bmonia, and mag- 
 
 i 
 
 Id, brownish-red ; 
 
 Bound is precipi- 
 
 itid, yellow; other- 
 I lading. 
 
 a, red : the origi 
 [itompouud becomes 
 
 ((white, insoluble in 
 I lime salt is like- 
 liBcetio acid. 
 
 Jl, white, soluble in 
 ;|en alcohol flame 
 iof sulphuric acid. 
 oicid, white, black- 
 i 
 
 |tous Acid, [Thio- 
 jlifhite, darkens ra- 
 litxcess of the hypo- 
 
 Likewise from acid solution. 
 
 jitates are soluble ia 
 ;,s of pyrophosphates 
 
 Jntrated solution ace^ 
 |Hpitated by argentic 
 
 Acids decolorizing Indigo 
 Solution. 
 
 The precipitate is insoluble in dilute 
 nitric acid. 
 
 Hydrochloric Acid, white, so- 
 luble in ammouia and iu sodic hypo- 
 sulphite. 
 
 Hydrobromic Acid, like the 
 pieceUinii. Toe origiual compound 
 colors carbon bisulphide reddish- 
 yellow after the addition of some 
 chlorine wnter. 
 
 Hydriodic Acid, yellowish, 
 insolut)lu in ammonia (with removal 
 of color). The origimil compound ren- 
 ders starcli blue, with nitrous acid. 
 
 Iodic Acid, white, soluble in 
 ammonia, precipitable therefrom by 
 SO2 as Agl. The original compound 
 gives (if a metallic iodide be pre- 
 sent), with acetic acid and starch, 
 blue iodide of starch. 
 
 Hydrocyanic Acid, white, so- 
 luble in ammonia and in sodic hypo- 
 sulphite. The original fluid gives, 
 with a mixture of ferrous and ferric 
 salts, potassa, and hydrochloric acid, 
 Prussian blue. 
 
 Hydroferrocyanic Acid, 
 white, insoluble lu ammonia. The 
 original compound gives iramedi- 
 aMyamih ferric salts, Prussfan blue. 
 
 I^Broferricyanic Acid, red- 
 dimj^rowQ. Ferrous salts give a 
 dark blue precipitate. 
 
 Hydrosulphocyanic Acid, 
 [Sulphocyanic Acid] white; diffi- 
 cultly soluble in ammonia; the ori- 
 ginal solution becomes, with ferric 
 chloride, blood-red. 
 
 Hydrogen Sulphide, black, 
 insoluble lu ammonia; plumbic 
 and cupric salts also give black 
 precipitates. Alkaline sulphides 
 give, with sodic nitroprusside, a 
 purple color. 
 
 a. Alone, without addition of an acid. 
 
 Free Chlorine nnd Bromine; 
 Hypochloric, Chlorous, and 
 Hypochlorous Acid, as well as 
 Hypochlorites ; and free Nitric 
 Acid not too dilute. 
 
 Also alkaline Metallic Sulph- 
 ides and Caustic Alkalies. 
 
 b. On the addition of an acid [hydro- 
 chloric or sulphuric) and heating. 
 Chlorates ; they leave by igni- 
 tion metallic chlorides. 
 
 Nitrates; dark color with fer- 
 rous sulphate and sulphuric acid; 
 the nitrates of the heavy metals and 
 earths when heated alone, those of 
 the alkalies and alkaline earths 
 when heated with dry cupric sul- 
 phate give red fumes. 
 
 lodates ; the dry compound gives 
 with sulphuric acid and ferrous sul- 
 phate violet vapor of iodine. 
 
 Bromates ; give with sulphuric 
 acid brown vapor of bromine. 
 
 0. By boiling or warming with con- 
 •ctntrated hydrochloric acid evolve 
 (bleaching) chlorine: — 
 All the preceding compounds, further : — 
 
 Chromates and Vanadates, 
 Seleniates, 
 Tellurates, 
 
 Superoxides, and the Acids 
 of Manganese. 
 
TABLE XIV. fSBCONDl 
 
 Detection of Metallic Oxides. *- ' 
 
 For the treatment of the Filtrate from the H2S precipitate 
 
 The substances precipitated, according to Table VI. by ammonio sulphide ''■"^ ^"^'f°^ff 
 examination according to Table VIII., may be as readily and completely ^^P'i'''*., Vg gltratettri 
 presence of ammonio chloride, successively/, instead of together, as follows: "°^\ , Amw 
 for an instant (to convert ferrous into ferric salts), and add Ammonio Chlonde m 
 
 Precipitate may contain 
 
 Ferric, chromic, uranic oxides; alumina, glucina; baric, strontic, calcic phosphates and 
 oxalates; magnesic phosphate; aluminic, chromic, iron, and manganous phosphates; (man- 
 ganous oxide, traces ; calcic fluoride ; borates of alkaline earths, in part ;) [cerous, lan- 
 thanic, didymic oxides; yttria, thoria, zirconia, titanic acid.]']" ' 
 
 Digest with concentrated solution of amnionic carbonate. 1^ 
 
 Solution contains 
 Uranic oxide, 
 [Cerous oxide,] 
 [Lanthanic oxide,] 
 [Didymic oxide,] 
 [Yttria,] 
 [Thoria,] 
 [Zirconia,] 
 [Glucina,] 
 
 * See remarks, Table 
 VIII., on these substances. 
 
 Dissolve the Residue , 
 in {boiling) hydrochloric acid, and boil until all COj has been 
 expelled, and add when cold NaHO (or KHO). 
 
 Boil the filtrate for some time 
 
 Precipitate, 
 
 Chromic oxide 
 
 [Glucina]. 
 
 Chromic phosphate. 
 
 Test with blowpipe. 
 
 Filtrate, 
 Acidulate with HCl, 
 and add ammonio car- 
 bonate: — 
 
 Precipitate, 
 
 Alumina, aluminic 
 
 phosphate. 
 
 Filtrate, 
 
 [Glucina] present only 
 
 if the digestion with 
 
 ammonio carbonate has 
 
 been omitted. 
 
 Test with blowpipe 
 
 Preoipitate may 
 contain ferric oxide,) 
 ferric phosphate ;>' 
 baric, strontic, cal- 
 cic, magnesic phos- 
 phates, etc. 
 
 Dissolve in a little 
 HCl, and test in se- 
 parate portions as di- 
 rected in. Table VIII 
 
 ■f- Whilst chromic oxide and phosphate, in a pure state, precipitated in the cold 1 _ 
 unless present in very great excess, will pass into solution, ilT ferric oxide be present, and, 
 will precipitate on boiling, or remain in solution with Al^Oj, depends on the concentratio' 
 enough with ammonic carbonate, the glucina will be found in the solution, and not in thep 
 The following treatment of the ammonia precipitate includes also the detection of titat 
 Dissolve the ammonia precipitate in as little sulphuric acid as possible (or fuse theiori 
 largely with water (about 1000 c. o. for 0.2 gramme TiO^ in nearly neutral solution), saf 
 acid ; filtrate, FeO, CrjOj, H3PO4, and small quantities of alkaline earths, phosphates, eto.1;(j 
 oxides if they are present in sufiScient quantity; and the earths will be found in the ammoi 
 drying the precipitate, fuse it with NajCO, and NaNOj, and treat with water. The resii- 
 alkalies. Add NH^Cl: Precipitate AljO^; and part or all of the HjPOj (to be detected by % 
 BaCrO^; filtrate BaHPO^ (if phosphates were present) precipitable by ammonia. Absent 
 of the fused mass, provided the fusion has been prolonged enough. 
 
 ^ 
 
'tETHOD.J ' 
 
 bf Table VI. instead of the method of that Table, (c. f. n.) 
 
 ••in presence of ammonic chloride, and which are subsequently separated into two groups, in 
 "tiups in the precipitation of the HjS filtrate, by employing ammonia and ammonic sulphide, in 
 "tm HjS precipitate, until all the UjS is expelled, then add a few drops of nitric acid, and boil 
 'ionic Hydrate (ammonia). 
 
 To the filtrate add 
 ammonic sulphide and warm until the supernatant liquid is clear, (if of a dark brown color 
 the presence of nickel is indicated.) 
 
 In . Frecipilate, 
 
 'I'Cobaltous sulphide, 3 , , , Manganous sulphide, flesh-colored. 
 
 Nickelous sulphide, 5 ' Zincio sulphide, white. 
 
 Treat with cold, dilute, hydrochloric acid: — 
 
 ^ Boil the soliiiion (Mn, Zn) 
 
 to expel HjS, and add NaHO to excess : 
 
 Frecipilate, 
 
 14 Manganese (traces of 
 
 ■ i^Ii and Co). Test with 
 
 jlowpipe, and as di- 
 
 ■ected in Table VIII. 
 
 il 
 
 1! 
 
 Filtrate, 
 
 Zinc. Add HjS ; 
 white precipitate. 
 
 Test with the blow- 
 pipe. 
 
 Residue (Ni, Co). 
 Wash, dissolve in aqua 
 regia, evaporate al- 
 most to dryness, boil 
 with KCy, and add, 
 when cold, slight ex- 
 cess of sulphuric acid. 
 Non-crystalline preci- 
 pitate. 
 
 Nickel. 
 Test with the blow- 
 pipe, or potassic ni- 
 trite, etc. See Table 
 VIII. 
 
 Filtrate. 
 Treat as directed for 
 filtrate from ammonic 
 sulphide precipitate in 
 Table VI., by precipi- 
 tating Ba, Sr, Ca by 
 ammonic carbonate, 
 and examining the fil- 
 trate for magnesia and 
 the alkalies. "~ 
 
 III alkalies redissolve easily and completely, and reprecipitate on boiling, not a trace of Cr^Oj, 
 jiits separation from FBjO, in this way is impossible. Whether glucina in solution in KHO 
 of the liquid as well as a moderate alkalinity. (If the precipitate has been treated long 
 iifecipitate of the sesquioxides.) 
 Aa acid, a matter of importance in many cases. 
 
 Ijginal finely pulverized substance with' KHSO4, ""'' extract the mass with cold water), dilute 
 jirate the liquid with HjS gas, and boil thoroughly for about an hour. Precipitate, Titanic 
 jf alkaline earths were originally present, the HjPO^ will remain completely with the sesqui- 
 Ijia filtrate.) Oxidize the filtrate from TiOj with HNO3; precipitate it by ammonia, and after 
 Lie will contain FejO,; the solution alumina, chromic and phosphoric acids, combined with 
 jkimonio raolybdate). Acidulate the filtrate with dilute acetic acid, and add BaCl : Precipitate 
 lof TiOj would simplify the process. If AljOj is present, it wilPaiZ be found in the solution