The solubility product of $AgCl$ at $25 \, ^\circ C$ is $5 \times 10^{-13}$. Its solubility is = .......

Solubility products $(K_{sp})$ of the salts of types $MX, MX_2$ and $M_3X$ at temperature $T$ are $4.0 \times 10^{-8}, 3.2 \times 10^{-14}$ and $2.7 \times 10^{-15}$ respectively. Solubilities (in $mol \text{ dm}^{-3}$) of the salts at temperature $T$ are in the order:

The solubility product $({K_{sp}})$ of $BaCO_3$ is $1.5 \times 10^{-9}$. At what concentration of $Ba^{2+}$ ions will precipitation begin when solid $Ba(NO_3)_2$ is added to a $10^{-4} \ M$ solution of $Na_2CO_3$?

The solubility product of $AgBr$ is $4.9 \times 10^{-13}$ at a certain temperature. Calculate the solubility.

Which one of the following is most soluble?

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 $PbCl_2 = 1.7 \times 10^{-5}$)