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Actual analysis for the detection of the acid constituent.

To the solution add excess of HNO3.

To the solution add slight excess of NaCO3 and warm.

To a fresh portion of the original solution, after careful neutralization with NH1HO, add Fe, Cl3.

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S

or U.

If the plan described in the introductory

remarks has been followed, the absence of a precipitate here might arise from the previous separation of the acid by the addition of dilute HNO3.

dicates the HNO, and

a gelatinous presence of AgNO3.

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A preci

To the so

A precipitate indicates the

pitate in-lution add

presence of

Cfy

A coloured solution indicates the presence of Csy

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BOO2

A precipitate indi

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Sio,

T

cates the presence of Cl, Br,

or Qt.

See Table for

GROUP III.

GROUP II.

TABLE FOR GROUP I.

The precipitate may be BaF, Ba,Si,F, BаŌ, BаT, Baбi, BаPO, BaBoO2, or BaSiO2.

To the solution add dilute HCl, and then divide the liquid into two parts.

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TABLE FOR GROUP II.

The precipitate may be AgCl, AgBr, AgI, AgCy, AgCsy, Ag2 Cfy, or Ag, Cfdy. Add NH ̧HO, and warm.

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The solution may contain AgCl, AgBr, (traces of AgI,) AgCy, Ag, Cfdy.

Add slight excess of dilute HNO,; collect the precipitate, wash, dry, and ignite it in a porcelain crucible: the Cy compounds are thus almost entirely reduced to the metallic state. Boil the residue in dilute HNO3.

A residue may be AgCl or AgBr. Wash; add a fragment of zinc and a drop of dilute H2SO; allow to stand a quarter of an hour, filter to the filtrate (neutralized and then concentrated) apply the starch-test. An orange colour indicates Br;

the absence of colour

indicates

Cl

(to be confirmed as usual).

The solution may contain

AgNO3. Add HCl. A precipitate indicates the previous existence of Cy or Cfdy.

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These reds may be distinguished by adding HgCl; when the colour of

Fe Csy, is discharged, and that of FeA, remains.

CHAPTER III.

ANALYSIS OF MIXED SALTS.

In the recognition of the various basic and acid-radicals which may be present in a mixture of salts, the plans described in the following Tables are to be adopted, with, however, such modifications as the preliminary examinations may suggest. To the methods of preliminary examination already given (see pp. 391, 404) recourse must again be had; indeed, the indications which they afford are often of extreme value in the analysis of complicated mixtures. The methods for preparing the solution of the substance to be analysed will be the same as those already described. (See pp. 392, 408.).

A few words may here be introduced concerning those combinations and mixtures of basic radicals with one another, known as alloys and amalgams. When once in solution, the manner of recognizing their constituents is identical with that adopted in the case of salts; but nitric acid, moderately concentrated, which is usually employed as the solvent for alloys, leaves many metals unacted upon and undissolved (e. g. platinum, gold, &c.), which require further treatment with hydrochloric or nitrohydrochloric acid. Nitric acid, moreover, partly separates tin and antimony in the form of insoluble compounds, which must then be treated according to the plan described on p. 394.

Throughout the Tables of the present and preceding chapter, the more common radicals are indicated by a conspicuous type. For the detection, &c. of the acid-radicals contained in a mixture of salts, the Tables already given may be employed (see pp. 413, 414); from these Tables, the rarer organic radicals, the reactions of which have been detailed in Chapter VII., are for the most part omitted, since they seldom occur together in the course of analysis, and generally require the employment of very special methods of separation. For these methods, reference must be made either to Chapter VII. or to a comprehensive treatise on Organic Chemistry.

The preliminary examination of the mixture of salts having been accomplished, and its results recorded, the student will then proceed to the actual analysis.

GENERAL TABLE FOR THE

If HCl has been used for the solution of the substance, and no precipitate be assumed to be absent; but if the substance has been dissolved in water addition as long as any precipitate is produced: when the precipitate ceases, ride of Bi or Sb, or any HSiO2, which may have been thrown down. Agitate

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The filtrate is first freed from HNO, by one or two separate Pt and the mass of the rarer allied metals, given in Table for Group II. If extremely acid, it suspected to contain As in the form of arsenic comof the latter is expelled*, when a rapid stream of H2 S pitation of Pb, As, and Mo, it is well to warm the filtime, with H, S. A blue colour on the first passage of precipitate may be only S, due to the oxidizing action ever, a mass of S might easily mask a small but imporsuffered to pass unexamined. Collect and wash the

The precipitate may contain

H2S and

Pb2 S Sn, S2

H, U

Hg2S

Sb2 S2

may be here precipit

Bi, S,

Sb2 S,

Cu S

As S

ated, since they are but

slightly soluble in

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water or acids.

Examine according to

Sn2 S

Examine according to Table
for GROUP II.

Table for GROUP I.

If the filtrate is of a previously formed, or evaporated to dryness at moistened with water and separation of HSiO2 as sent, the residue should not be interfered with. a current of air: the only dered insoluble in acids; bonaceous mass is left, well to burn the insoluble

TABLE FOR THE ANALYSIS OF GROUP I.

The precipitates produced by the addition of HCl, and remaining undissolved in excess of that reagent, may contain

PbCl, AgCl, and Hg, Cl; the anhydride W203; and the acids HSbO3, H4 Sb2 07, HBOO2, HBz, H, S, and H2 U.

Boil the precipitate with several fresh portions of water, and wash it, when on the filter, with hot water.

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AgCl and Hg, Cl; W203; HSbO3, H4 Sb. 07, and H2Ū.
Warm with solution of KHO, filter and wash.

The solution

may contain
KWO2
KSbO3
Ką H2 Sb2 O7

and

K2 U.

the presence of The W may be

Pb.

The acids will be found in the analysis for acid-radical.

detected by the blowpipe reactions; the Sb by the H3 Sb series of experiments.

The residue may contain AgCl and (Hg),O.
Warm with solution of NH, HO.

The solution will

contain
AgCl.

If a reprecipitation
occurs on addition of
HNO,, it indicates
Ag.

The residue will consist of
(Hg2)2O,

the presence of which may
be proved by heating the
dried substance with
Na, CO, in a bulb-tube,
and obtaining the metallic
globules of
Hg.

EXAMINATION FOR BASIC RADICALS.

either immediate or on cooling has been the result, the first group may or in HNO, or H, SO4, add a few drops of concentrated HCl, and repeat the add yet a few drops more of the concentrated acid, to redissolve any oxychlountil the solution is clear, and then filter.

evaporations on a water-bath with HCl; it is then treated with NH, Cl, to and subsequently with HCO to precipitate Au, according to the details should then be partially neutralized with Na, CO,, still keeping it acid; and if pounds, it must be saturated with SO, gas: it is then warmed until all excess gas is passed through it for at least half an hour. To ensure the perfect precitrate from the first HS precipitate, and to saturate it a second, and even a third HS should lead the student to look for Mo. A white or very pale yellow of unexpelled HNO3, of HCrO2, or of ferric salts upon the H, S. Since, howtant quantity of Sb, S., or As, S, or other bodies, no such precipitate must be precipitate completely.

fine blue colour, special search for Ru should be made in the Pt precipitate Mo may be looked for again in the following group. The filtrate should be now 100° C. with HNO3; this process should be repeated, and the residue finally just again evaporated to perfect dryness: absolute desiccation ensures the complete Si, O.; it would otherwise be mistaken for Al, H, O.... If organic matter is prebe more highly heated, in order that the detection of Al, Cr, Fe, Mn, &c. may It is well to burn organic bodies off entirely, by igniting the residue strongly in danger is, that by exposing sesquioxides to so high a temperature they are rena compromise is therefore frequently effected by heating until merely a carwhich is boiled repeatedly with HCI, and the solution filtered. It would be residue white, to ascertain whether Si, O, is present.

To the HCl solution add some quantity of NH, Cl; then almost neutralize with NH, HO; place in a flask, and add (NH), S until no more precipitate is produced: warm gently, allow to rest for some time in the corked flask, and filter, washing with water slightly impregnated with (NH1), S.

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If the filtrate is brown, the presence of Ni may be inferred. First acidify with HA; warm, filter, and add the new precipitate to the one previously produced. The filtrate should be evaporated to expel excess of (NH), S, and any precipitate of S resulting from its decomposition ascertained to be only S by its entire volatility. Solution of (NH1), CO, is then added until the precipitation ceases; the liquid warmed (not boiled, lest the precipitate should redissolve in the NHCl) and filtered.

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* Certain sulphates, as those of Ba, Sr, and Ca, may be precipitated here, the SO, being eonverted into H2 SO. If insoluble in acids, such precipitate must be examined by fusion.

† Mo is not perfectly precipitated unless H2S is passed into its alkaline solution, which is afterwards acidified.

T 5

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