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

Question

Given below are two statements:
Statement I : The limiting molar conductivity of

KCl

(strong electrolyte) is higher compared to that of

\mathrm{CH}_{3} \mathrm{COOH}

(weak electrolyte).
Statement II : Molar conductivity decreases with decrease in concentration of electrolyte.

Quantrex Academy · Accepted Answer

Correct answer: D. Both Statement I and Statement II are false

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	${K}^{+}$	${Cl}^{-}$	${CH}_{3}{COO}^{-}$	${H}^{+}$
${\lambda}^{∘} / \left(S{cm}^{2}{mol}^{- 1}\right)$	$73 . 5$	$76 . 3$	$40 . 9$	$349 . 6$

Given below are two statements: Statement I : The limiting molar...

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