If the solubility of $MX_2$ in water is $0.0002 \ mol/L$,then its $K_{sp}$ is:

Solid $Ba(NO_3)_2$ is gradually dissolved in a $1.0 \times 10^{-4} \ M \ Na_2CO_3$ solution. At which concentration of $Ba^{2+}$,precipitate of $BaCO_3$ begins to form? ($K_{sp}$ for $BaCO_3 = 5.1 \times 10^{-9}$)

Which of the following compounds will not dissolve in a hot mixture of $NaOH$ and $H_2O$?

Which from the following equations represents the relation between solubility ($S$ in $mol \ L^{-1}$) and solubility product $(K_{sp})$ for a salt $B_3A_2$?

The $K_{sp}$ of $Mg(OH)_2$ is $1.2 \times 10^{-11}$. Calculate its solubility in pure water.

The solubility of $CaCO_3$ is $7 \times 10^{-5} \ mol \ dm^{-3}$ at $25^{\circ} C$. What is its solubility product at same temperature?