If the solubility product of $PbS$ is $3.4 \times 10^{-28}$,what is the minimum concentration of sulfide ions required to precipitate $PbS$ from a $0.001 \ M \ Pb^{2+}$ solution?

What is the molar solubility of $Ag_{2}CO_{3}$ $(K_{sp} = 4 \times 10^{-13})$ in $0.1 \ M \ Na_{2}CO_{3}$ solution?

If $[S^{2-}] = 0.6 \times 10^{-2} \ mol \ m^{-3}$ and $[Hg^{2+}] = [Mn^{2+}] = [Fe^{2+}] = [Zn^{2+}] = 1 \times 10^{-16} \ mol \ m^{-3}$,which of the following will precipitate first in an aqueous solution?

Solubility product constant $(K_{sp})$ of salts of types $MX$,$MX_2$ and $M_3X$ at temperature '$T$' are $4.0 \times 10^{-8}$,$3.2 \times 10^{-14}$ and $2.7 \times 10^{-15}$,respectively. Solubilities $(\text{mol } dm^{-3})$ of the salts at temperature '$T$' are in the order:

Express the relationship between $K_{sp}$ and solubility $(S)$ for the salt $Ca_3(PO_4)_2$.

The solubility products of three sparingly soluble salts are given below. What is the correct decreasing order of their molar solubility?

$S.No.$	$Formula$	$K_{sp}$
$1$	$PQ$	$4.0 \times 10^{-20}$
$2$	$PQ_2$	$3.2 \times 10^{-14}$
$3$	$PQ_3$	$2.7 \times 10^{-35}$