According to the Debye-Hückel-Onsager equation for strong electrolytes, the variation of molar conductivity () with concentration () is . For a weak electrolyte like aqueous acetic acid, how does the

Question

According to the Debye-Hückel-Onsager equation for strong electrolytes, the variation of molar conductivity ($\Lambda_m$) with concentration ($C$) is $\Lambda_m = \Lambda_m^\circ - b\sqrt{C}$. For a weak electrolyte like aqueous acetic acid, how does the $\Lambda_m$ vs $\sqrt{C}$ curve behave as concentration approaches zero?

Prashant Kotian · Accepted Answer

Correct answer: D. For weak electrolytes, the degree of dissociation () increases significantly at extremely low concentrations. This causes a steep, non-linear increase in molar conductivity. As , the curve becomes asymptotic (parallel) to the y-axis, meaning the limiting molar conductivity () cannot be found by direct graphical extrapolation, requiring Kohlrausch's law instead.

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