[317] Mulder. See Sutton's Volumetric Analysis, p. 304 (1904).
[318] Vide Chapters XII and XIII.
[319] A table of exact solubilities is given at the end of the Lab. Manual, q.v.
[320] In the most exact quantitative work, as demanded in the determinations of atomic weights, every known loss must, as far as possible, be measured and taken into account. Beautiful instances of such work are found in T. W. Richards' classic determinations of atomic weights. See, for instance, Richards, Carnegie Institution Publications, No. 125 (1910), Determinations of the Atomic Weights of Silver, Lithium and Chlorine (Stud.).
[321] Z. Elektrochem., 11, 797 (1905).
[322] Ibid., 11, 936 (1905), and 12, 725 (1906).
[323] Z. phys. Chem., 55, 707 (1906), and 61, 638 (1907).
[324] If n is the number of moles of solute dissolved in N moles of solute, the concentration of the solute may be expressed as n / (n + N), which is called its "mole fraction." This form of expressing concentrations is in many particulars preferable to the mole / liter form. For very dilute solutions (n is very small compared with N) the two forms become practically identical, but they are not so for more concentrated solutions, and the mole-fraction expression is then easier to treat rigorously.
[325] See Walden, loc cit., for more extended data.