At $298 \, K$,the solubility of $PbCl_2$ is $2 \times 10^{-2} \, mol/L$,then $K_{sp} = ?$

What would be the concentration of $H_2SO_4$ necessary to precipitate $BaSO_4$ from a solution of $0.01 \ M \ Ba^{2+}$ ions $(K_{sp} = 1.0 \times 10^{-9})$?

At $20 \, ^\circ C$,the concentration of $Ag^+$ ions in a saturated solution of $Ag_2CrO_4$ is $1.5 \times 10^{-4} \, M$. The solubility product $(K_{sp})$ of $Ag_2CrO_4$ at $20 \, ^\circ C$ is:

If the solubility products of $AgBrO_3$ and $Ag_2SO_4$ are $5.5 \times 10^{-5}$ and $2 \times 10^{-5}$ respectively,what is the relationship between their solubilities?

When equal volumes of the following solutions are mixed,precipitation of $AgCl$ $(K_{sp} = 1.8 \times 10^{-10})$ will occur only with:

Solid $Ba(NO_3)_2$ is gradually dissolved in $1 \times 10^{-4} \ M \ Na_2CO_3$ solution. At what concentration of $Ba^{+2}$ will the precipitation of $BaCO_3$ start? (Given: $K_{sp}$ of $BaCO_3 = 5.1 \times 10^{-9}$)