The solubility product $(K_{sp})$ of $AgCl$ at $100 \, ^\circ C$ is $1.44 \times 10^{-4}$. The solubility of $AgCl$ in boiling water is $.......$

The $pH$ of a saturated solution of $Ba(OH)_2$ is $12$. What is the value of the solubility product $(K_{sp})$ of $Ba(OH)_2$?

Concentration of $H_2SO_4$ and $Na_2SO_4$ in a solution is $1 \ M$ and $1.8 \times 10^{-2} \ M$,respectively. Molar solubility of $PbSO_4$ in the same solution is $X \times 10^{-Y} \ M$ (expressed in scientific notation). The value of $Y$ is. . . .
[Given: Solubility product of $PbSO_4$ $(K_{sp})=1.6 \times 10^{-8}$. For $H_2SO_4$,$K_{a1}$ is very large and $K_{a2}=1.2 \times 10^{-2}$]

The conductivity of a saturated solution of $BaSO_4$ is $3.06 \times 10^{-6} \ \Omega^{-1} \ cm^{-1}$ and its equivalent conductance is $1.53 \ \Omega^{-1} \ cm^2 \ eq^{-1}$. Then the $K_{sp}$ for $BaSO_4$ will be:

Assertion : Addition of silver ions to a mixture of aqueous sodium chloride and sodium bromide solution will first precipitate $AgBr$ rather than $AgCl$.
Reason : $K_{sp}$ of $AgCl < K_{sp}$ of $AgBr$.

At $25^{\circ} C$,the solubility product of $MCl$ is $1 \times 10^{-10}$. What is its molar solubility in $0.1 \ M \ NaCl$ solution at the same temperature?