Molar ionic conductivities of divalent cation and anion are \(57 \mathrm{~S} \mathrm{~cm}^2…

Molar ionic conductivities of divalent cation and anion are \(57 \mathrm{~S} \mathrm{~cm}^2 \mathrm{~mol}^{-1}\) and \(73 \mathrm{~S} \mathrm{~cm}^2 \mathrm{~mol}^{-1}\) respectively. The molar conductivity of solution of an electrolyte with the above cation and anion will be :
  1. \(187 \mathrm{~S} \mathrm{~cm}^2 \mathrm{~mol}^{-1}\)
  2. \(260 \mathrm{~S} \mathrm{~cm}^2 \mathrm{~mol}^{-1}\)
  3. \(130 \mathrm{~S} \mathrm{~cm}^2 \mathrm{~mol}^{-1}\)
  4. \(65 \mathrm{~S} \mathrm{~cm}^2 \mathrm{~mol}^{-1}\)

Solution

$\begin{aligned} & \Lambda_{\mathrm{C}}^{+2}=57 \mathrm{Scm}^2 \mathrm{~mol}^{-1} \\ & \Lambda_{\mathrm{A}}^{+2}=73 \mathrm{Scm}^2 \mathrm{~mol}^{-1} \\ & \Lambda_{\text {Solution }}=\lambda_{\mathrm{C}}^{+2}+\Lambda_{\mathrm{A}}^{-2} \\ & =57+73=130\end{aligned}$

Asked in: JEE Main 2024 (05 Apr Shift 1)

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