The molar solubility of $PbI_2$ in $0.2 \ M \ Pb(NO_3)_2$ solution in terms of solubility product of $PbI_2$ is

At $25 \, ^\circ C$,the solubility product $(K_{sp})$ of $Mg(OH)_2$ is $1.0 \times 10^{-11}$. What is the minimum $pH$ required to precipitate $Mg(OH)_2$ from a $0.001 \, M \, Mg^{2+}$ solution?

For the following Assertion and Reason,the correct option is
Assertion $(A) :$ When $Cu^{2+}$ and sulphide ions are mixed,they react together extremely quickly to give a solid.
Reason $(R) :$ The equilibrium constant of $Cu^{2+}_{(aq)} + S^{2-}_{(aq)} \rightleftharpoons CuS_{(s)}$ is high because the solubility product is low.

Calculate the equilibrium concentration of $Pb^{2+}$ ions in a solution of $PbS$ containing $1 \times 10^{-11} \ mol \ dm^{-3}$ of sulphide ions. (Given $K_{sp}$ for $PbS = 8.0 \times 10^{-28}$)

The solubility product of silver bromide $(AgBr)$ is $5.0 \times 10^{-13}$. How much potassium bromide $(KBr)$ (molar mass $120 \, g \, mol^{-1}$) should be added to $1 \, L$ of $0.05 \, M$ silver nitrate $(AgNO_3)$ solution to initiate the precipitation of $AgBr$?

Solubility of a salt $M_2X_3$ is $y \ mol \ dm^{-3}$. The solubility product of the salt will be