The solubility of salt $AX_2$ is $6 \times 10^{-12} \text{ mol dm}^{-3}$. What is the solubility product $(K_{sp})$ of the salt?

If the solubility product of $Zr_3(PO_4)_4$ is denoted by $K_{SP}$ and its molar solubility is denoted by $S$,then which of the following relations between $S$ and $K_{SP}$ is correct?

What is the minimum volume of water required to dissolve $1 \, g$ of calcium sulphate at $298 \, K$? (For calcium sulphate,$K_{sp}$ is $9.1 \times 10^{-6}$).

For a sparingly soluble strong electrolyte $AgIO_3$ (molar mass = $283 \, g/mol$),the equilibrium in a saturated solution is given by $AgIO_3(s) \rightleftharpoons Ag^+(aq) + IO_3^-(aq)$. If the solubility product constant $K_{sp}$ of $AgIO_3$ at a given temperature is $1.0 \times 10^{-8}$,how many grams of $AgIO_3$ are contained in $100 \, mL$ of its saturated solution?

Given that the solubility product constants $(K_{sp})$ follow the order $K_{sp}(Mg(OH)_2) > K_{sp}(Zn(OH)_2) > K_{sp}(Fe(OH)_3)$,what is the order of precipitation of these hydroxides?

The solubility products of $NiS$,$ZnS$,$CdS$,and $HgS$ are $4.7 \times 10^{-5}$,$1.6 \times 10^{-24}$,$8 \times 10^{-27}$,and $4 \times 10^{-53}$ respectively. An aqueous solution contains $Ni^{2+}$,$Zn^{2+}$,$Cd^{2+}$,and $Hg^{2+}$ of equal concentration. $H_2S$ gas was passed into this solution very slowly. The first and the last ions that precipitate as sulphides are respectively.