The solubility of $CaCO_3$ in water is $3.05 \times 10^{-4} \, mol/L$. Its solubility product will be:

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

$A$ 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: $K_{sp}(SrCO_3) = 7.0 \times 10^{-10}$, $K_{sp}(SrF_2) = 7.9 \times 10^{-10}$

What is the solubility of $PbSO_4$ in centinormal $(0.01 \ N)$ $H_2SO_4$ solution? The solubility product $(K_{sp})$ of $PbSO_4$ at a given temperature is $1 \times 10^{-8} \ (mol/L)^2$.

The concentration of a saturated solution of $Mg(OH)_2$ is $8.2 \times 10^{-4} \% \ w/V$. Calculate its solubility product. Its molecular mass is $58.3 \ g \ mol^{-1}$.

For the precipitation reaction of $Ag^{+}$ ions with $NaCl$,which of the following statements is correct?