Question

The solubility of $AgCl$ in water, in $0.02MCaC{l}_2$, in $0.01MNaCl$, and in $0.05MAgN{O}_3$ are $S_0,S_1,S_2$, and $S_3$ respectively. Which of the following relationships between these quantities is correct?

• A. $S_0>S_1>S_2>S_3$
• B. $S_0>S_2>S_1>S_3$
• C. $S_0>S_1=S_2>S_3$
• D. $S_0>S_2>S_3>S_1$

Answer 1

Answer: (B)

Solubility $=\frac{\text{ Solubility Product }}{\text{ Concentration of common ion }}$

$S_1=\frac{K_{sp}}{0.02}=50K_{sp}$

$S_2=\frac{K_{sp}}{0.01}=100K_{sp}$

$S_3=\frac{K_{sp}}{0.05}=20K_{sp}$

So, $S_2>S_1>S_3$ Again solubility will be greatest in water. So, $S_0>S_2>S_1>S_3$