Question

The solubility of $AgCl$ in water, in $0.02 \,M\, CaCl _{2}$, in $0.01 \,M\, NaCl$, and in $0.05 \,M\, AgNO _{3}$ 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 $=\frac{\text { Solubility Product }}{\text { Concentration of common ion }}$

$S_{1}=\frac{K_{ sp }}{0.02}=50 K _{ sp }$

$S_{2}=\frac{K_{ sp }}{0.01}=100 K _{ sp }$

$S_{3}=\frac{K_{ sp }}{0.05}=20 K _{ sp }$

So, $S_{2}>\,S_{1}>\,S_{3}$ Again solubility will be greatest in water. So, $S_{0}>\,S_{2}>\,S_{1}>\,S_{3}$