molar ionic conductivities of a divalent cation and anion are \(57 \, \text{S cm}^2 \text{mol}^{-1}\) and \(73 \, \text{S cm}^2 \text{mol}^{-1}\), respectively. The molar conductivity of the solution of an electrolyte with the above cation and anion will be:
- \(65 \, \text{S cm}^2 \text{mol}^{-1}\)
- \(130 \, \text{S cm}^2 \text{mol}^{-1}\)
- \(187 \, \text{S cm}^2 \text{mol}^{-1}\)
- \(260 \, \text{S cm}^2 \text{mol}^{-1}\)
The Correct Option is B
Solution and Explanation
The molar conductivity of a solution (ΛSolution) is given by the sum of molar ionic conductivities:
Λ+2C = 57 S cm2 mol-1
Λ+2A = 73 S cm2 mol-1
ΛSolution = λ+ + λ-
ΛSolution = 57 + 73 = 130 S cm2 mol-1
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