The molar solubility of a sparingly soluble salt $MX_4$ is $s \ mol \ L^{-1}$. If the solubility product is $K_{sp}$,then $s$ in terms of $K_{sp}$ is:

Which of the following would increase the solubility of $Pb(OH)_2$?

Which is the correct representation of the solubility product constant of $Ag_2CrO_4$?

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

Let the solubility of an aqueous solution of $Mg(OH)_2$ be $x$,then its $K_{sp}$ is:

The solubility product of a salt having the general formula $MX_2$ in water is $4 \times 10^{-12}$. What is the concentration of $M^{2+}$ ions in the saturated aqueous solution of the salt?