Arrange the following in increasing order of solubility product $(K_{sp})$: $Ca(OH)_2, AgBr, PbS, HgS$

The molar solubility of a sparingly soluble salt $MX_4$ is $s \ mol \ L^{-1}$. If the solubility product is $K_{sp}$,then $s$ in terms of $K_{sp}$ is:

Assign $A$,$B$,$C$,$D$ from the given type of reaction.
$Pb(AcO)_2 + H_2S \longrightarrow PbS \downarrow + 2AcOH$

The solubility product of $AgBr$ is $4.9 \times 10^{-13}$ at a certain temperature. Calculate the solubility.

The solubility of $AgCl$ in its solution is $1.25 \times 10^{-5} \ mol \ dm^{-3}$. What is the solubility product of $AgCl$?

The solubility of $CdSO_{4}$ in water is $8.0 \times 10^{-4} \ mol \ L^{-1}$. Its solubility in $0.01 \ M \ H_{2}SO_{4}$ solution is $..... \ \times 10^{-6} \ mol \ L^{-1}$.
(Round off to the Nearest integer) (Assume that solubility is much less than $0.01 \ M$)