The $K_{sp}$ value of $AgCl$ at $25^{\circ}C$ is $1.8 \times 10^{-10}$. If $10^{-5} \ mol$ of $Ag^{+}$ is added to the solution,the new $K_{sp}$ value will be:

The $K_{sp}$ of $M(OH)_2$ is $3.2 \times 10^{-11}$. The $pH$ of its saturated solution in water is:

For which sparingly soluble salt is the relationship between $K_{sp}$ and $S$ (solubility) given by $S = (K_{sp} / 4)^{1/3}$?

The molar solubility of $Cd(OH)_2$ is $1.84 \times 10^{-5} \ M$ in water. The expected solubility of $Cd(OH)_2$ in a buffer solution of $pH = 12$ is

$1 \ dm^{3}$ solution containing $10^{-5} \ mol$ each of $Cl^{-}$ ions and $CrO_{4}^{2-}$ ions is treated with $10^{-4} \ mol$ of silver nitrate. Which one of the following observations is made?
$[K_{sp} \ Ag_{2}CrO_{4} = 4 \times 10^{-12}]$
$[K_{sp} \ AgCl = 1 \times 10^{-10}]$

$0.08 \ g$ 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 $CaF_2 = 78.08 \ g/mol$)