Given below are two statements:
Statement I : The limiting molar conductivity of $KCl$ (strong electrolyte) is higher compared to that of $CH_{3} COOH$ (weak electrolyte).
Statement II : Molar conductivity decreases with decrease in concentration of electrolyte.

Question

In the light of the above statements, choose the most appropriate answer from the options given below:

TestHub · Accepted Answer

lon K + Cl - CH 3 COO - H + λ ∘ / S cm 2 mol - 1 73 . 5 76 . 3 40 . 9 349 . 6 λ ∘ M CH 3 COOH = λ ∘ M H + + λ ∘ M CH 3 COO − = 349.6 + 40.9 = 390.5 Scm 2 mol − 1 λ ∘ M ( KCl ) = λ ∘ M K + + λ ∘ M Cl − = 73.5 + 76.3 = 149.8 Scm 2 mol − 1 So, statement-I is false. For an electrolyte the dilution increases (or) decrease in concentration, the number of ions increases due to increase of degree of dissociation. So, the molar conductance increases. Hence, Statement-II is false.

lon	$K^{+}$	${Cl}^{-}$	${CH}_{3} {COO}^{-}$	$H^{+}$
$λ^{\circ} / (S {cm}^{2} {mol}^{- 1})$	$73.5$	$76.3$	$40.9$	$349.6$

Chemistry - Electrochemistry Question with Solution | TestHub

Options:

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