ABSTRACT
Experimental determinations of the conducting properties of electrolyte solutions are important essentially in two respects. Firstly, it is possible to study quantitatively the effects of interionic forces, degrees of dissociation and the extent of ion pairing. Secondly, conductance values may be used to determine quantities such as solubilities of sparingly soluble salts, ionic products of self-ionizing solvents, dissociation constants of weak acids and to form the basis for conductimetric titration methods. Differing degrees of solvation in different solvents cause effective ionic radii as well as viscosity to vary with solvent; in consequence, gross departures from the 'rule' may be observed. The conditions under which the ions deriving from strong electrolytes may associate into ion pairs have already been considered. Since such associations reduce the effective number of conducting species, occurrence of such phenomena may be expected to reduce the conductivity below values which would be obtained were all the ions to be unassociated.
