$K_{sp}$ for $Cr(OH)_3$ is $2.7 \times 10^{-31}$. What is its solubility in moles / litre?

Let the solubility of an aqueous solution of $Mg(OH)_2$ be $x$,then its $K_{sp}$ is:

In qualitative analysis,the metals of group $I$ can be separated from other ions by precipitating them as chloride salts. $A$ solution initially contains $Ag^{+}$ and $Pb^{2+}$ at a concentration of $0.10 \, M$. Aqueous $HCl$ is added to this solution until the $Cl^{-}$ concentration is $0.10 \, M$. What will the concentrations of $Ag^{+}$ and $Pb^{2+}$ be at equilibrium? ($K_{sp}$ for $AgCl = 1.8 \times 10^{-10}$,$K_{sp}$ for $PbCl_2 = 1.7 \times 10^{-5}$)

What is the $pH$ of a saturated solution of $Cu(OH)_2$? $(K_{sp} = 4.0 \times 10^{-6})$

Calculate solubility $(mol \ dm^{-3})$ of a sparingly soluble electrolyte $AB$ at $298 \ K$ if its solubility product is $1.6 \times 10^{-5}$?

The solubility product of a sparingly soluble salt is defined as the product of the ionic concentrations in a: