The solubility of a sparingly soluble salt $AB_2$ is $1 \times 10^{-6} \text{ mol/dm}^3$. Calculate its solubility product.

The solubility of $Ca_3(PO_4)_2$ in water is $y \text{ moles/litre}$. Its solubility product is

How many grams of $CaC_2O_4$ will dissolve in distilled water to make one litre of saturated solution (in $g$)? (Solubility product of $CaC_2O_4$ is $2.5 \times 10^{-9} \ mol^2 \ L^{-2}$ and its molecular weight is $128$)

The sulphide ion concentration $[S^{2-}]$ in a saturated $H_2S$ solution is $1 \times 10^{-22} \ M$. Which of the following sulphides should be quantitatively precipitated by $H_2S$ in the presence of dilute $HCl$?

Product	Sulphide Solubility $(K_{sp})$
$I$	$1.74 \times 10^{-16}$
$II$	$1.2 \times 10^{-22}$
$III$	$8.2 \times 10^{-46}$
$IV$	$5.0 \times 10^{-34}$

The solubility product of $AgCl$ is $10^{-10} \, M^2$. The minimum volume (in $m^3$) of water required to dissolve $14.35 \, mg$ of $AgCl$ is approximately

If the solubility of salts $M_2X$,$QY_2$,and $PZ_3$ is the same $(S < 1)$,what is the relationship between their solubility products $(K_{sp})$?