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

The solubility product of $PbS$ is $3.4 \times 10^{-28}$. If $[Pb^{2+}] = 1 \times 10^{-2} \ mol/L$,what concentration of $[S^{2-}]$ is required to precipitate $PbS$?

The solubility product of $AgCl$ is $1.5625 \times 10^{-10}$ at $25\ ^oC$. Its solubility in grams per litre will be

Which of the following would increase the solubility of $Pb(OH)_2$?

Derive the solubility product $(K_{sp})$ expression for the following sparingly soluble salts:
$(i)$ Two ions having $MX$ formula
$(ii)$ Three ions having $MX_{2}$ or $M_{2}X$ types
$(iii)$ Four ions having $AX_{3}$ or $A_{3}X$ type salts
$(iv)$ Five ions $A_{2}X_{3}$ or $A_{3}X_{2}$ type salts.

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: