The volume of water required to dissolve $0.1 \ g$ $PbCl_2$ to get a saturated solution (in $mL$) is (Given $K_{sp}(PbCl_2) = 3.2 \times 10^{-8}$; Atomic mass of $Pb = 207 \ u$, $Cl = 35.5 \ u$)

In a saturated solution of the sparingly soluble strong electrolyte $AgIO_3$ (molecular mass $= 283$),the equilibrium which sets in is $AgIO_{3(s)} \rightleftharpoons Ag^+_{(aq)} + IO^-_{3(aq)}$. If the solubility product constant $K_{sp}$ of $AgIO_3$ at a given temperature is $1.0 \times 10^{-8}$,what is the mass of $AgIO_3$ contained in $100 \ mL$ of its saturated solution?

If the $K_{sp}$ of $AgCl$ is $10^{-10}$,what is the volume of the solution required to prepare a saturated solution of $1.43 \ g$ of $AgCl$? $[M.W. = 143]$

The solubility of $AgBr_{(s)}$,having solubility product $5 \times 10^{-10}$ in $0.2 \ M$ $NaBr$ solution,equals

The solubility product for salt $AB_2$ is $4 \times 10^{-12}$. Calculate its solubility.

The low solubility of $BaSO_4$ in water can be attributed to