The $K_{sp}$ of $AgCl$ is $1.0 \times 10^{-10}$. Calculate the solubility of $AgCl$ in $0.2 \ M \ AgNO_3$.

Solubility product is

Calculate the ionic concentration of a sparingly soluble salt $BA$ in $mol \ dm^{-3}$ at $300 \ K$ when equilibrium is attained,if the solubility product of the salt is $2.7 \times 10^{-10}$ at the same temperature.

What is the $pH$ at which $Mg(OH)_2$ starts to precipitate from a solution containing $0.1 \ M \ Mg^{2+}$ ions? (Given $K_{sp}$ for $Mg(OH)_2 = 1.0 \times 10^{-11}$)

The solubility product of $AgI$ at $25\,\text{°C}$ is $1.0 \times 10^{-16}\,\text{mol}^2\,\text{L}^{-2}$. The solubility of $AgI$ in $10^{-4}\,\text{N}$ solution of $KI$ at $25\,\text{°C}$ is approximately (in $\text{mol L}^{-1}$)

Solid $Ba(NO_3)_2$ is gradually added to a $1.0 \times 10^{-4} \, M \, Na_2CO_3$ solution. At what concentration of $Ba^{2+}$ will precipitation start? (Given $K_{sp}$ for $BaCO_3 = 5.1 \times 10^{-9}$)