Elementary quantitative analysis / by Alexander Classen ; translated, with additions, by Edgar F. Smith.

  • Classen, Alexander, 1843-1934.
Date:
1878
Catalogue details

Licence: Public Domain Mark

Credit: Elementary quantitative analysis / by Alexander Classen ; translated, with additions, by Edgar F. Smith. Source: Wellcome Collection.

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    If n C. C of uimnoniiiiu hydrate were used for the saturation o'i m C. C. of the acid, 1 C. C. of lh(! acid will corresi)ond to — C. C. aninioniuni hydrate. AVerci rC.C. in used for the supersaturation of the sodium carbonate solu- tion, and for the titration of the excess t C. C. of ammo- nium hydrate, which would equal—< C. C, there must n have been necessary for the neutralization of the sodium carbonate r — t C. C. acid. If the latter is expressed by f, and if a grms. sodium carbonate have been used in the experiment, 1 C. C. of the acid will correspond to ^ grms. sodium carbonate. From this the amount of anhydrous acid in 1 C. C. may be readily calculated. If, for example, in using sulphuric acid 1 C. C. of it equals a grms. sodium carbonate, the quantity of anhydrous sulphuric acid in 1 C. C. is calculated from the proportion— Na^C03 : SO3 : : a : X. The estimation of the quantity of sodium in any sample of soda is made exactly as in the standardization of tlie acid. If the soda contains sodium hydrate, sulphide or hypo- sulphite, these are decomposed by the acid in titration, and incorrectly brought into the equation as sodium carbonate.* To estimate sodium hydrate in the presence of sodium carbonate, precipitate the aqueous solution of the soda ash with an excess of barium hydrate, and determine the sodium hydrate in the filtrate, or an aliquot portion of it, with an acid of known strength. Follow the above in- structions. * If a hyposulphite is not present, the other sul]jhur com- pounds can be oxidized with potassium chlorate and the acpieous Solution of the residue titrated.