Question

The solubility of $MX$, $M{X}_2$ and $M{X}_3$ is ${10}^{-4}$ mole per litre. Hence their solubility products are respectively:

• A. ${10}^{-6}$, $4\times {10}^{-9}$, $27\times {10}^{-12}$
• B. ${10}^{-8}$, $4\times {10}^{-12}$, $27\times {10}^{-16}$
• C. ${10}^{-9}$, $8\times {10}^{-8}$, $32\times {10}^{-12}$
• D. None of these

Answer 1

The correct option is B ${10}^{-8}$, $4\times {10}^{-12}$, $27\times {10}^{-16}$

$K_{sp}$ for $MX$, $M{X}_2$ and $M{X}_3$ is $s^2$, $4s^3$ and $27s^4$ respectively,
$s^2$=${10}^{-8}$
$4s^3$=$4\times {10}^{-12}$
$27s^4$=$27\times {10}^{-16}$