When $150 \ mL$ of $0.0008 \ M$ ammonium sulfate solution is mixed with $50 \ mL$ of $0.04 \ M$ calcium nitrate solution,given $K_{sp} = 2.4 \times 10^{-5}$ for $CaSO_4$,what is the ionic product of $CaSO_4$?

For a sparingly soluble salt $AB_2$,the equilibrium concentrations of $A^{2+}$ ions and $B^{-}$ ions are $1.2 \times 10^{-4} \ M$ and $0.24 \times 10^{-3} \ M$,respectively. The solubility product of $AB_2$ is :

The concentration of $500 \ mL$ $NaOH$ solution is $0.02 \ M$. How many grams of $FeSO_4$ must be added to this solution to initiate the precipitation of $Fe(OH)_2$? The $K_{sp}$ of $Fe(OH)_2$ is $1.5 \times 10^{-15}$. The molecular mass of $FeSO_4$ is $152 \ g \ mol^{-1}$.

Which substance precipitates when $HCl$ is added to a solution of $SnS$ in yellow ammonium sulfide?

$A$ solution is saturated with $SrCO_3$ and $SrF_2$. The $[CO_3^{2-}]$ is found to be $1.2 \times 10^{-3} \ M$. The concentration of $F^{-}$ in the solution would be:
Given: $K_{sp}(SrCO_3) = 7.0 \times 10^{-10}$,$K_{sp}(SrF_2) = 7.9 \times 10^{-10}$

The concentration of a saturated solution of $Mg(OH)_2$ is $8.2 \times 10^{-4} \ g \ L^{-1}$ at $298 \ K$. Calculate its solubility product $(K_{sp})$. (Molar mass of $Mg(OH)_2 = 58 \ g \ mol^{-1}$)