The $K_{sp}$ for $BaSO_4$ at $25\ ^\circ C$ is $1.1 \times 10^{-10}$. To make the new solubility equal to $1.1 \times 10^{-8} \ M$,it is necessary to use a solution of $Na_2SO_4$ of the following concentration (in $M$):

The solubility product constants of $M(OH)_3$ and $M(OH)_2$ are $10^{-23}$ and $10^{-14}$ respectively. If both ions are present in a solution,which one will precipitate first upon the addition of $NH_4OH$?

What is the value of $K_{sp}$ for a saturated solution of $Ba(OH)_2$ having $pH = 12$?

In an aqueous solution,$SCN^-$,$Br^-$,$I^-$,and $Cl^-$ are present. Which will get precipitated first when $AgNO_3$ is added to the solution? Given that:
$K_{sp}(AgCl) = 1.2 \times 10^{-10}$,
$K_{sp}(AgI) = 1.7 \times 10^{-16}$,
$K_{sp}(AgSCN) = 7.1 \times 10^{-7}$,
$K_{sp}(AgBr) = 3.5 \times 10^{-13}$

Equal volumes of $0.02 \ M$ $CaCl_2$ and $0.00004 \ M$ $Na_2SO_4$ solutions are mixed. Will a precipitation of $CaSO_4$ occur? $(K_{sp} = 2.4 \times 10^{-5})$

$A$ precipitate of $AgCl$ is formed when equal volumes of the following are mixed. [$K_{sp}$ for $AgCl = 10^{-10}$]