Discussion
Why does the molar conductivity of acetic acid rise steeply on dilution?
Answer: A
Acetic acid is weak, so dilution shifts its equilibrium towards the ions and the number of charge carriers per mole of acid rises sharply, far outweighing the small interionic effects. The limiting value cannot be reached by extrapolation from measurable concentrations, which is precisely why Kohlrausch's law is needed to assemble it from sodium acetate, hydrochloric acid and sodium chloride. Individual ion mobilities change only slightly, water contributes negligibly, and the cell constant is fixed by geometry.
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