The solubility of $AgCl$ is $1.43 \times 10^{-3} \ g/L$. If the molar mass of $AgCl$ is $143 \ g/mol$,then the solubility product $(K_{sp})$ is:

Match the following metal sulfides with their respective solubility product $(K_{sp})$ values:

Metal sulfide	Solubility product
$A$. $PbS$	$I$. $4.0 \times 10^{-53}$
$B$. $HgS$	$II$. $8.0 \times 10^{-28}$
$C$. $MnS$	$III$. $1.6 \times 10^{-24}$
$D$. $ZnS$	$IV$. $2.5 \times 10^{-13}$

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 solubility of sparingly soluble salts $MX$, $MX_2$ and $MX_3$ is $1 \times 10^{-3} \text{ mol/L}$. Hence, their respective solubility products are

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 $Mg(OH)_2 = 58 \ g \ mol^{-1}$)

When equal volumes of the following solutions are mixed,precipitation of $AgCl$ will occur in - ($K_{sp}$ of $AgCl = 1.8 \times 10^{-10}$)