Question

The correct order of decreasing solubility of AgCl in
(A) water
(B) 0.1 M NaCl
(C) 0.1 $BaC{l}_2$
(D) 0.1M $N{H}_3$ is

• A. D>A>B>C
• B. D>C>B>A
• C. B>A>D>C
• D. A>D>B>C

Answer 1

The correct option is A D>A>B>C

With ammonia, AgCl forms a complex $\left[Ag\right(N{H}_3{)}_2]Cl$ . Hence AgCl is more soluble in ammonia than in water.
When a common ion such as chloride ion is present, the solubility of AgCl is decreased. Greater is the concentration of chloride ion from strong electrolyte, greater will be the decreases in the solubility.
The chloride ion concentration in 0.1M NaCl solution is 0.1.
The chloride ion concentration in 0.1 M $BaC{l}_2$ solution is 0.2$\alpha$ where $\alpha$ is the degree of dissociation of $BaC{l}_2$.
Hence, the decreasing order of the solubility is $D>A>B>C$.