First slide

Common ion effect

Question

Let the solubilities of AgCl in pure water be 0.01 M ${CaCl}_{2},$ 0.01 M NaCl and 0.05 M ${AgNO}_{3}$ be $s_{1}, s_{2}, s_{3} and s_{4}$ respectively. What is the correct order of these quantities ? Neglect any complexation.

Moderate

A

$s_{1} > s_{2} > s_{3} > s_{4}$
B

$s_{1} > s_{2} = s_{3} > s_{4}$
C

$s_{1} > s_{3} > s_{2} > s_{4}$
D

$s_{4} > s_{2} > s_{3} > s_{1}$

Solution

Let $K_{sp}$ of AgCl = x
(a) solubility of AgCl in pure water = $s_{1} = \sqrt{x}$
(b) solubility oif AgCl in 0.01 M ${CaCl}_{2} s_{2} = \frac{x}{0.02}$
(c) solubility of AgCl in 0.01 M NaCl = $s_{3} = \frac{x}{0.01}$
(d) solubility of AgCl in 0.05 M ${AgNO}_{3} = s_{4} = \frac{x}{0.05}$
So $s_{1} > s_{3} > s_{2} > s_{4}$
Alternatively
more the concentration of common ion concentration lesser is the solubility.

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