Question

The conductivity of 0.01 M salt solution is 1.061 × 10\(^{-4}\) S cm\(^{-1}\). What is molar conductivity of the solution?

• A. \( 1.061 \times 10^{-4} \, \Omega^{-1} \, \text{cm}^2 \text{mol}^{-1} \)
• B. \( 1.061 \, \Omega^{-1} \, \text{cm}^2 \text{mol}^{-1} \)
• C. \( 106.1 \, \Omega^{-1} \, \text{cm}^2 \text{mol}^{-1} \)
• D. \( 10.61 \, \Omega^{-1} \, \text{cm}^2 \text{mol}^{-1} \)

Hint:

Molar conductivity is calculated by dividing the conductivity of the solution by its concentration.

Answer 1

The Correct Option is B

Step 1: Understanding molar conductivity.
Molar conductivity (\(\Lambda_m\)) is the conductivity of a solution per mole of solute. It is calculated using the formula: \[ \Lambda_m = \frac{\kappa}{C} \] Where \(\kappa\) is the conductivity of the solution and \(C\) is the concentration of the solution.
Step 2: Calculation.
Given \(\kappa = 1.061 \times 10^{-4} \, \Omega^{-1} \, \text{cm}^{-1} \text{mol}^{-1}\) and \(C = 0.01 \, \text{mol/L}\), we can calculate the molar conductivity: \[ \Lambda_m = \frac{1.061 \times 10^{-4}}{0.01} = 1.061 \, \Omega^{-1} \, \text{cm}^2 \text{mol}^{-1} \] Step 3: Conclusion.
The correct answer is (B) \( 1.061 \, \Omega^{-1} \, \text{cm}^2 \text{mol}^{-1} \).