The Elements of Qualitative Chemical Analysis, vol. 1, parts 1 and 2. / With Special Consideration of the Application of the Laws of Equilibrium and of the Modern Theories of Solution.

by Julius Stieglitz

[366] The symbols in heavy type indicate the chief components of the final system. Vide Smith's General Chemistry for Colleges and Inorganic Chemistry, for the form of equations used.

[367] Emich, Ber. d. chem. Ges. 40, 1482 (1901).

[368] Arrhenius, Z. phys. Chem., 5, 16 (1890); Shields, ibid., 12, 167 (1893).

[369] See below for the corresponding equation, developed by Walker for a salt of a weak base and a strong acid.

[370] Potassium sulphate, K₂SO₄, reacts faintly alkaline in aqueous solution, the secondary ionization of sulphuric acid (table, p. [104]) being somewhat weaker than the ionization of potassium hydroxide. We have: K₂SO₄ + HOH ⇄ KHSO₄ + KOH or SO₄²⁻ + HOH ⇄ HSO₄⁻ + HO⁻.

[371] Walker, Z. phys. Chem., 4, 319, (1889); Arrhenius, loc. cit.; Bredig, ibid., 13, 321 (1894).

[372] Arrhenius, loc. cit.

[373] See p. [183].

[374] Arrhenius developed the relation for aniline acetate, loc. cit.

[375] Putting x = [Acid] = [Base], we have [Salt] = (0.1 − x), and (0.1 − x)² / x² = (7E−10)² / 1.2E−14. Then (0.1 − x) / x = 0.0064 and x = .09935, which is 99.35% of the total salt used. The degree of ionization, α, of the salt, in the extremely dilute solution, is taken to be 100%.