Solubility product $(K_{sp})$ of the salts $MX\,,\, MX_2\,,\, M_3X$ at temperature $'T'$ are $4 \times 10^{-8}\,,\, 3.2 \times 10^{-14}$ and $2.7 \times 10^{-15}$ respectively. Solubilities of the salt at temperature $'T'$ are in the order

At $25\,^oC,$ the solubility product of $Mg(OH)_2$ is $1.0 \times 10^{-11}.$ At which $pH,$ will $Mg^{2+}$ ions start precipitating in the form of $Mg(OH)_2$ from a solution of $0.001 \,M \,Mg^{2+}$ ions?

Solid $Ba(NO_3)_2$ is gradually dissolved in a $1.0 \times 10^{-3} \,M \,Na_2CO_3$ solution. At what concentration of $Ba^{2+}$ will be precipitate begin to form ($K_{sp}$ for $BaCO_3 = 5.1 \times 10^{-9}$)

The solubility product of $AgI$ at $25\,^oC$ is $1.0 \times {10^{ – 16}}\,mo{l^2}\,{L^{ – 2}}$. The solubility if $AgI$ in ${10^{ – 4}}\,N$ solution of $KI$ at $25\,^oC$ is approximately (in $mol$ ${l^{ – 1}})$

$K_{sp}$ for $AgBr$ at $25\,^oC$ is $4.9 × 10^{-13}$. How much $AgBr$ will dissolved in $20\  litres$ of its saturated solution if molecular weight of $AgBr =$  $188$