At $T(K)$,$K_{sp}$ of two ionic salts $MX_2$ and $MX$ is $5 \times 10^{-13}$ and $1.6 \times 10^{-11}$ respectively. The ratio of molar solubility of $MX_2$ and $MX$ is

The $K_{sp}$ values of $Ag_2CrO_4, AgCl, AgBr,$ and $AgI$ are $1.1 \times 10^{-12}, 1.8 \times 10^{-10}, 5.0 \times 10^{-13},$ and $8.3 \times 10^{-17}$ respectively. If $AgNO_3$ solution is added to a solution containing equal moles of $NaCl, NaBr, NaI,$ and $Na_2CrO_4$,which will precipitate last?

Which of the following is most soluble in water?

$K_{sp}$ for $CaSO_4$ is $9 \times 10^{-6}$. The minimum volume of water needed to dissolve $1 \ g$ of $CaSO_4$ at $298 \ K$ temperature is ...... (in $L$)

Evaporation of $1 \ L$ of a saturated solution of $CaCO_3$ leaves a residue of $7.0 \ g$. What is the solubility product $(K_{sp})$ for $CaCO_3$?

In an aqueous solution containing $AgCl_{(s)}$,$AgBr_{(s)}$,and $AgI_{(s)}$,find the ratio $[Cl^{-}] : [Br^{-}] : [I^{-}]$ at equilibrium if $K_{sp}(AgCl) = 10^{-10}$,$K_{sp}(AgBr) = 10^{-13}$,and $K_{sp}(AgI) = 10^{-16}$.