The solubility of $PbCl_2$ is equal to .......

Which of the following has the maximum solubility? (Given $K_{sp}$ values)

The required amount of $KBr$ (molar mass $= 119 \ g/mol$) in grams to start the precipitation of $AgBr$ in $500 \ mL$ solution of $0.05 \ M \ AgNO_3$ will be :- ($K_{SP}$ of $AgBr = 5 \times 10^{-13}$)

Which of the following provides the best explanation for the solubility of $MnS$ in dilute $HCl$?

$0.08 \ g$ of $CaF_2$ is dissolved in $2.90 \ L$ of water to form a saturated solution at $298 \ K$. Calculate the solubility product constant $(K_{sp})$ of $CaF_2$. (Molar mass of $CaF_2 = 78.08 \ g/mol$)

Find the concentration of the ion which is first precipitated at the point when the third ion starts precipitating,if $AgNO_3$ is added gradually to a solution that contains $0.1 \ M \ Cl^{-}$,$0.1 \ M \ Br^{-}$,and $0.1 \ M \ I^{-}$.
Given that:

Salt	$K_{sp}$
$AgCl$	$2 \times 10^{-10}$
$AgBr$	$5 \times 10^{-13}$
$AgI$	$9 \times 10^{-17}$