The solubility of sparingly soluble salt $AB_2$ is $1.0 \times 10^{-4} \ mol \ dm^{-3}$. What is its solubility product?

The solubility product of $AgCl$ at $25 \, ^\circ C$ is $5 \times 10^{-13}$. Its solubility is = .......

$25.0 \ mL$ of $0.050 \ M \ Ba(NO_3)_2$ is mixed with $25.0 \ mL$ of $0.020 \ M \ NaF$. The $K_{sp}$ of $BaF_2$ is $0.5 \times 10^{-6}$ at $298 \ K$. The ratio of $[Ba^{2+}][F^{-}]^2$ to $K_{sp}$ is $.......$. (Nearest integer)

The values of $K_{sp}$ of two sparingly soluble salts $Ni(OH)_2$ and $AgCN$ are $2.0 \times 10^{-15}$ and $6 \times 10^{-17}$ respectively. Which salt is more soluble? Explain.

The molar solubility $(mol \ L^{-1})$ of a sparingly soluble salt $MX_4$ is $s$. The corresponding solubility product is $K_{sp}$. $s$ is given in terms of $K_{sp}$ by the relation:

In which of the following solvents will $AgBr$ have the highest solubility?