Question

Two sparingly soluble salts $AX$ and $B{X}_2$ have their solubility product constants equal. Which of the following is incorrect ?

• A. Solubility of $AX$ is less than solubility of $B{X}_2$
• B. If $S_1$ and $S_2$ are molar solubility of $AX$ and $B{X}_2$ then $S_1=2{\left(S_2\right)}^{2/3}$
• C. If $X$ is a conjugate base of a weak acid, addition of $HN{O}_3$ will increase solubility of both $AX$ and $B{X}_2$
• D. Increasing the temperature, increases the solubility of both $AX$ and $B{X}_2$

Answer 1

Answer: (B)

$Ks{p}_1=s^2$
$Ks{p}_2=4s^{{}^{\prime }3}$
$s^2=4s^{{}^{\prime }3}$