The solubility of $AgCl$ in $0.2 \ M \ NaCl$ solution ($K_{sp}$ for $AgCl = 1.20 \times 10^{-10}$) is:

$A$ precipitate of calcium oxalate $(CaC_2O_4)$ will not dissolve in which of the following?

The $K_{sp}$ of $Mg(OH)_2$ is $1.0 \times 10^{-12}$. At which $pH$ does $0.01 \ M$ $Mg^{2+}$ solution begin to precipitate? Calculate the solubility of $Mg(OH)_2$ in pure water.

The solubility of a sparingly soluble salt $A_3B_2$ (Molar mass $= M \ g/mol$) in water is $x \ g/L$. The ratio of the solubility product of the salt to the molar concentration of $B^{-3}$ ion is:

The solubility of $AgCl$ at $20 \, ^oC$ is $1.435 \times 10^{-3} \, g/L$. The solubility product $(K_{sp})$ of $AgCl$ is:

The solubility of salt $BA_2$ is $4 \times 10^{-4} \ mol \ dm^{-3}$. What is the solubility product of the salt?