If the concentration of $[Ag^{+}]$ in a solution is $1 \times 10^{-6} \ M$,what is the concentration of $[Br^{-}]$? Given that the $K_{sp}$ for $AgBr$ is $4.0 \times 10^{-13}$.

For a metal hydroxide with an oxidation state of $+3$,the solubility is $1 \times 10^{-5} \ mol/L$. What is its solubility product $(K_{sp})$?

Which of the following compounds is sparingly soluble in ammonia?

The solubility product of $PbI_{2}$ is $8.0 \times 10^{-9}$. The solubility of lead iodide in $0.1 \ M$ solution of lead nitrate is $x \times 10^{-6} \ mol/L$. The value of $x$ is ....... .(Rounded off to the nearest integer)
$[$Given: $\sqrt{2}=1.41]$

At $T(K)$ in a saturated solution of $MgCO_3$ and $Ag_2CO_3$, if the concentration of $Mg^{2+}$ ion is $3.2 \times 10^{-5} \ M$, then the concentration of $Ag^{+}$ ion in the solution will be [Given: $K_{sp}(MgCO_3) = 1.6 \times 10^{-6}$ and $K_{sp}(Ag_2CO_3) = 8.0 \times 10^{-12}$ at $T(K)$]

The solubility of $CaF_2$ in a solution of $0.1 \ M \ Ca(NO_3)_2$ is.