The solubility of ${\mathrm{A}}_2{\mathrm{X}}_3$ is $\mathrm{y} \mathrm{mol} {\mathrm{dm}}^{-3}$. Its solubility product is

Equal volumes of the following ${\mathrm{Ca}}^{2+} \mathrm{and} {\mathrm{F}}^{-}$ solutions are mixed. In which of the solutions will precipitation occur ? (${\mathrm{K}}_{\mathrm{sp}}$ of ${\mathrm{CaF}}_2$ = $1.7\times {10}^{-10}$)

 $$\begin{gathered} 1. {10}^{-2} \mathrm{M} {\mathrm{Ca}}^{2+} + {10}^{-5} \mathrm{M} {\mathrm{F}}^{-} \\ 2. {10}^{-3} \mathrm{M} {\mathrm{Ca}}^{2+} + {10}^{-3} \mathrm{M} {\mathrm{F}}^{-} \\ 3. {10}^{-4} \mathrm{M} {\mathrm{Ca}}^{2+} + {10}^{-2} \mathrm{M} {\mathrm{F}}^{-} \\ 4. {10}^{-3} \mathrm{M} {\mathrm{Ca}}^{2+} + {10}^{-3} \mathrm{M} {\mathrm{F}}^{-} \end{gathered}$$

For which of the following sparingly soluble salt, the solubility $\left(\mathrm{S}\right)$ and solubility product $\left({\mathrm{K}}_{\mathrm{sp}}\right)$ are related by the expression

$\mathrm{S} = ({\mathrm{K}}_{\mathrm{sp}}/4{)}^{1/3}$ ?

In a saturated solution of the sparingly soluble strong electrolyte ${\mathrm{AgIO}}_3$ (Molecular mass= $283$), the equilibrium which sets in is

${\mathrm{AgIO}}_3 \left(\mathrm{s}\right) \iff {\mathrm{Ag}}^{+} \left(\mathrm{aq}\right) + {{\mathrm{IO}}_3}^{-} \left(\mathrm{aq}\right)$

If the solubility product constant ${\mathrm{K}}_{\mathrm{sp}}$ of ${\mathrm{AgIO}}_3$ at a given temperature is $1.0\times {10}^{-8}$, what is the mass of ${\mathrm{AgIO}}_3$ contained in $100 \mathrm{ml}$ of its saturated solution?