The $K_{sp}$ expression for $Ca_3(PO_4)_2$ is:

The solubility product of $Hg_2Cl_2$ in water at $25 \, ^\circ C$ is $3.2 \times 10^{-17} \, mol^3 \, dm^{-9}$. The solubility of $Hg_2Cl_2$ at $25 \, ^\circ C$ is:

The $K_{sp}$ for $AgBr$ at $25 \, ^\circ C$ is $4.9 \times 10^{-13}$. How much $AgBr$ (in grams) will dissolve in $20 \, L$ of its saturated solution? (Molecular weight of $AgBr = 188$)

The concentration of a saturated solution of $Mg(OH)_2$ is $8.2 \times 10^{-4} \% \ w/V$. Calculate its solubility product. Its molecular mass is $58.3 \ g \ mol^{-1}$.

If '$s$' and '$S$' are the solubility and solubility product of a sparingly soluble binary electrolyte respectively,then which of the following relations is correct?

The solubility product of $AgCl$ is $1.5625 \times 10^{-10}$ at $25\ ^oC$. Its solubility in grams per litre will be