At 300 K, the molar conductivities of the aqueous solutions of three salts at two different concentrations are given below:
The conductivity of a saturated aqueous solution of AgCl is S cm⁻¹ at 300 K. If the solubility of AgCl in water at 300 K is mol L⁻¹, then is
(Assume that AgCl dissolved in water ionizes completely and that the molar conductivity of saturated AgCl solution is equal to its limiting molar conductivity.)
| Salt | Concentration (M) | Molar conductivity (S cm² mol⁻¹) |
|---|---|---|
| NaNO₃ | 0.01 | 111 |
| 0.04 | 101 | |
| NaCl | 0.01 | 117 |
| 0.04 | 107 | |
| AgNO₃ | 0.01 | 125 |
| 0.04 | 116 |
The conductivity of a saturated aqueous solution of AgCl is S cm⁻¹ at 300 K. If the solubility of AgCl in water at 300 K is mol L⁻¹, then is
(Assume that AgCl dissolved in water ionizes completely and that the molar conductivity of saturated AgCl solution is equal to its limiting molar conductivity.)
- (A)3
- (B)4
- (C)5✓ Correct
- (D)6
Answer: (C)
Solution
Using Kohlrausch's law, we first find the limiting molar conductivities from the given data.
For each salt, using :
For NaNO₃: From the two concentrations, solving gives S cm² mol⁻¹
For NaCl: Similarly, S cm² mol⁻¹
For AgNO₃: S cm² mol⁻¹
Using Kohlrausch's law:
For the saturated solution:
Therefore,
For each salt, using :
For NaNO₃: From the two concentrations, solving gives S cm² mol⁻¹
For NaCl: Similarly, S cm² mol⁻¹
For AgNO₃: S cm² mol⁻¹
Using Kohlrausch's law:
For the saturated solution:
Therefore,
JEE Advanced · 2026 · 17 May 2026 · Paper 2 · Single correct option