In the next place, account must be taken, in analytical work, of the fact that ‹colloids carry down› with them the ‹precipitating ion› by which they are coagulated, a fact which may lead to the ‹loss of ions› which, it is intended, should be kept in solution. To a certain extent, this loss may also be avoided by insuring the presence of electrolytes (acids, ammonium salts) in sufficient concentration to cause the coagulation without the aid of the ions which, it is intended, should not be precipitated. In view of the much weaker precipitating power of univalent ions (of hydrochloric acid, ammonium nitrate and chloride), as compared with that of polyvalent ions, which may be present, the acid and ammonium salts must not be used in too small concentrations. In quantitative analysis, when conditions permit it, ammonium or sodium sulphate is frequently substituted for the ammonium salts of the univalent monobasic acids. The washing of the precipitated colloid with such salt solutions gradually removes[289] the ions which are precipitated with the colloid and forms a further safeguard against their loss. But this source of loss is avoided only with great difficulty and is seldom absolutely removed. Finally, the presence of ‹protective colloids›, especially of the [p138] gelatine and albumen type, may interfere so decidedly with the common precipitation tests for ions, that ‹their destruction is imperative›, before these tests can be applied with any degree of confidence. Thus, the mixing of solutions (0.1 molar) of silver nitrate and hydrochloric acid, each containing one per cent of gelatine, fails to produce the ordinary, characteristic precipitate[290] of silver chloride, ‹the reaction which is used to determine the presence of the silver-ion in systematic analysis›. The mixture is opalescent and, in reflected light, looks opaque-white; on somewhat prolonged standing a white ‹milk› is produced, but no precipitate. When the mixture is boiled, the same deep white milk is formed, but no coagulated precipitate, the mixture running unchanged through a filter. Hydrogen sulphide converts the mixture into a similar suspension of the black sulphide. FOOTNOTES: [227] The ratio is affected somewhat by the fineness of division of liquids and solids as a result of surface tension phenomena, as explained below. [228] An aqueous solution of iodine and potassium iodide shaken with chloroform gives similar results, and the difference in color between the two layers is an advantage for a lecture experiment. But the iodine is partially combined with the iodide, according to KI + I_{2} ⇄ KI_{3}, or I^{−} + I_{2} ⇄ I_{3}^{−}, and the theoretical relations are not so simple as for bromine in aqueous and chloroform solutions.