[192] The solution of these salts is due to the action of hydrogen ions on their anions; see Chap. VIII.
[193] Goodwin, ‹Z. phys. Chem.›, «21», 1 (1896).
[194] See Kohlrausch and Holborn, ‹loc. cit.›, p. 194. Their values for K (last column) must be divided by 100 to express the constants in terms of the same units as those used in the above table.
[195] J. H. Long, ‹J. Am. Chem. Soc.›, «18», 693 (1896). Ley, ‹Z. phys. Chem.›, «30», 322 (1899); Bruner, ‹ibid.›, «32», 133 (1900); Walker, ‹J. Chem. Soc.›, (London), «67», 585 (1895).
[196] Instances are found in the laboratory experiments, Parts III and IV.
[197] The ionization of salts of other types, ‹e.g.› MeX_{ 2}, Me_{ 2}Y, etc., likewise fails to conform to the law of chemical equilibrium.
[198] See below (pp. 112–4), also, further, confirmatory evidence, derived from the application of the same law to the influence upon the degree of ionization of weak acids and weak bases, exerted by the presence of their own salts.
[199] See below, in regard to evidence that the disturbing factors, predominant with strong electrolytes, are exhibited in much slighter, but perceptible measure in the case of the weak electrolytes.
[200] See also the interpretation of the law of chemical equilibrium from the viewpoint of the kinetic theory, Nernst, ‹Theoretical Chemistry›, p. 428.
[201] For a more detailed discussion of these views, see Lehfeldt's ‹Electrochemistry› (1904), pp. 78, 79.
[202] Various empirical laws, expressing the behavior of strong electrolytes, have been suggested: see Nernst, ‹Theoretical Chemistry›, p. 498, as to Rudolphi's and van 't Hoff's rules; see also A. A. Noyes, ‹Report of the Congress of Arts and Science›, «IV», p. 316 (1904).
[203] Wegscheider, ‹Z. phys. Chem.›, «70» (I), 603 (1909).
[204] It is possible that this effect is only another form of expressing the very relation discussed in the preceding paragraph.
[205] Arrhenius, ‹Z. Elektrochem.›, «6», 10 (1899); ‹Z. phys. Chem.›, «31», 197 (1899).
[206] Salts have constants averaging about 7, and running from 5 to 28; the constant for ice is about 3. Landolt, Börstein, Meyerhoffer, ‹Tabellen›, p. 766 (1905).
[207] We have: Ice, 3, water (at 0°), 80; glacial acetic acid, 2.8, acetic acid (liquid), 10; cane sugar, 4, cane sugar in aqueous solution (40%), 67.5, (6.5%), 45.3. ‹Ibid.›