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

[30] Nernst, Theoretical Chemistry, p. 103.

[31] Van 't Hoff, Lectures on Physical Chemistry, Part II, p. 37.

[32] J. Phys. Chem., 10, 141 (1906).

[33] This term must not be confounded with the term osmotic pressure, which has been defined on p. [10].

[34] See Chapter VII on the law of physical or heterogeneous equilibrium, where the relations are discussed in detail.

[35] Z. phys. Chem., 5, 175 (1890).

[36] Ibid., 3, 119 (1889).

[37] Phil. Mag., 38, 206 (1894).

[38] Cf. van 't Hoff's Lectures on Physical Chemistry, Vol. II, 40 (1899).

[39] The molecules may have different masses in the different conditions, and the principle of the mean kinetic energy would always apply to them as they are, in the condition under observation, and not as they are in some other condition; any change in mass, in solution, for instance, would show itself in the osmotic pressure measurements (see p. [18]), just as it is shown in the measurements of gases, when the gas molecules show a change in composition, as is the case with hydrogen fluoride (H₂F₂ ⇄ 2 HF), nitrogen tetroxide (N₂O₄ ⇄ 2 NO₂), phosphorus pentachloride (PCl₅ ⇄ PCl₃ + Cl₂) and other compounds.