Given below are two statements :Statement I : | vedclass

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(D) Statement $I$: The limiting molar conductivity $(\Lambda_{m}^{\infty})$ is the sum of the ionic conductivities of the constituent ions. For $CH_{3

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Both Statement $I$ and Statement $II$ are false.

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(D) Statement $I$: The limiting molar conductivity $(\Lambda_{m}^{\infty})$ is the sum of the ionic conductivities of the constituent ions. For $CH_{3}COOH$,$\Lambda_{m}^{\infty} = \lambda^{\infty}(H^{+}) + \lambda^{\infty}(CH_{3}COO^{-}) \approx 349.8 + 40.9 = 390.7 \, S \, cm^{2} \, mol^{-1}$. For $KCl$,$\Lambda_{m}^{\infty} = \lambda^{\infty}(K^{+}) + \lambda^{\infty}(Cl^{-}) \approx 73.5 + 76.3 = 149.8 \, S \, cm^{2} \, mol^{-1}$. Since $390.7 > 149.8$,Statement $I$ is false.Statement $II$: Molar conductivity $(\Lambda_{m})$ is defined as $\Lambda_{m} = \frac{\kappa}{c}$. As concentration $(c)$ decreases,the dilution increases. For both strong and weak electrolytes,the decrease in concentration leads to an increase in molar conductivity because the interionic attractions decrease (for strong electrolytes) or the degree of dissociation increases (for weak electrolytes). Thus,Statement $II$ is false.

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