Statement I: The limiting molar conductivity of KCl (strong electrolyte) is higher compared to that of (weak electrolyte). Statement II: Molar conductivity increases 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 ${CH}_{3} COOH$ (weak electrolyte).

Statement II: Molar conductivity increases with decrease in concentration of electrolyte.

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

Smart Achievers · Accepted Answer

(2)

$Ion$	$H^{+}$	$K^{+}$	${Cl}^{-}$	${CH}_{3} {COO}^{-}$
$Λ_{m}^{\infty} (S {cm}^{2} {mol}^{- 1})$	$349.8$	$73.5$	$76.3$	$40.9$

So, $Λ_{m}^{\infty} ({CH}_{3} COOH) = Λ_{m}^{\infty} (H^{+}) + Λ_{m}^{\infty} ({CH}_{3} {COO}^{-}) = 349.8 + 40.9 = 390.7 S {cm}^{2} {mol}^{- 1}$

$Λ_{m}^{\infty} (KCl) = Λ_{m}^{\infty} (K^{+}) + Λ_{m}^{\infty} ({Cl}^{-}) = 73.5 + 76.3 = 149.8 S {cm}^{2} / mole$

$So statement-I is wrong or false.$

As the concentration decreases, the dilution increases, which increases the degree of dissociation, thus increasing the number of ions, which increases the molar conductance.

Solution

1 Statement I is true but Statement II is false.

2 Statement I is false but Statement II is true.

3 Both Statement I and Statement II are true.

4 Both Statement I and Statement II are false.

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