At $298 \ K$,the solubility of $PbCl_2$ is $2 \times 10^{-2} \ mol/L$. Calculate the $K_{sp}$.

How many grams of $CaC_2O_4$ will dissolve in distilled water to make $1 \, L$ of a saturated solution (in $, g$)? The solubility product $(K_{sp})$ of $CaC_2O_4$ is $2.5 \times 10^{-9} \, mol^2 \, L^{-2}$ and its molar mass is $128 \, g \, mol^{-1}$.

What is the molarity of $F^{-}$ in a saturated solution of $InF_3$? $(K_{sp} = 7.9 \times 10^{-10})$

The solubility product of $Ni(OH)_2$ at $298 \ K$ is $2 \times 10^{-15} \ mol^3 \ dm^{-9}$. The $pH$ value of its aqueous and saturated solution is

What is the maximum concentration of equimolar solutions of ferrous sulphate and sodium sulphide so that when mixed in equal volumes,there is no precipitation of iron sulphide? (For iron sulphide,$K_{sp} = 6.3 \times 10^{-18}$).

The correct order of solubility of the given salts in water at $298 K$ is:

Salt	$K_{sp}$ at $298 K$
$AgBr$	$5.0 \times 10^{-13}$
$Zn(OH)_2$	$1.0 \times 10^{-15}$
$Hg_2Cl_2$	$1.3 \times 10^{-18}$