In which of the following pairs of insoluble chlorides,one dissolves in concentrated $HCl$ and the other is not soluble?

At $25\,^oC$,$K_{sp}$ for $PbBr_2$ is equal to $8 \times 10^{-5}$. If the salt is $80\%$ dissociated,what is the solubility of $PbBr_2$ in $mol/L$?

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

The solubility product for salt $AB_2$ is $4 \times 10^{-12}$. Calculate its solubility.

Explain the equilibrium involving the dissolution of a solid in a liquid.

In qualitative analysis,the metals of group $I$ can be separated from other ions by precipitating them as chloride salts. $A$ solution initially contains $Ag^{+}$ and $Pb^{2+}$ at a concentration of $0.10 \, M$. Aqueous $HCl$ is added to this solution until the $Cl^{-}$ concentration is $0.10 \, M$. What will the concentrations of $Ag^{+}$ and $Pb^{2+}$ be at equilibrium? ($K_{sp}$ for $AgCl = 1.8 \times 10^{-10}$,$K_{sp}$ for $PbCl_2 = 1.7 \times 10^{-5}$)