Question

The equation for the solubility product constant of $A{g}_{2}Cr{O}_4$ is:

• A. $K_{sp}=\left[A{g}^{2+}\right]\cdot \left[Cr{O}^{2-}\right]$
• B. $K_{sp}=[A{g}^{+}{]}^2\cdot [C{r}^{6+}]\cdot [{O_4}^{8-}]$
• C. $K_{sp}=\left[A{g}^{+}\right]\cdot \left[C{r}^{6+}\right]\cdot \left[{O_4}^{8-}\right]$
• D. $K_{sp}=[A{g}^{+}{]}^2\cdot [{Cr{O}_4}^{2-}]$

Answer 1

The correct option is D $K_{sp}=[A{g}^{+}{]}^2\cdot [{Cr{O}_4}^{2-}]$

$A{g}_{2}Cr{O}_4$ dissociates as-

$A{g}_{2}Cr{O}_4$ $=$ $2A{g}^{+}$ $+$ $Cr{O}_4^{2-}$.

The stoichiometric co-efficient of $A{g}^{+}$ is $2$ and its charge is $+1$. The stoichiometric co-efficient of $Cr{O}_4^{-2}$ is $1$ and its charge is $-2$.

Solubility product, $K_{sp}$ is defined as the product of the concentrations of the constituent ions present in salt, with their powers raised to their respective stoichiometric coefficients.

Hence, the $K_{sp}$ $=$ $[A{g}^{+}{]}^2$$[Cr{O}_4^{-2}{]}^1$

Therefore, option $D$ is the correct answer.