The K_{sp} values of Al(OH)_3 and Zn(OH)_2 ar | vedclass

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(A) The precipitation of a sparingly soluble salt occurs when the ionic product exceeds its solubility product constant $(K_{sp})$.Since $K_{sp}(Al(OH

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$Al(OH)_3$

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(A) The precipitation of a sparingly soluble salt occurs when the ionic product exceeds its solubility product constant $(K_{sp})$.Since $K_{sp}(Al(OH)_3) = 8.5 	imes 10^{-23}$ and $K_{sp}(Zn(OH)_2) = 1.8 	imes 10^{-14}$,the $K_{sp}$ value of $Al(OH)_3$ is significantly lower than that of $Zn(OH)_2$.$A$ substance with a lower $K_{sp}$ value requires a lower concentration of precipitating ions to reach the saturation point.Therefore,$Al(OH)_3$ will precipitate earlier than $Zn(OH)_2$ upon the addition of $NH_4OH$.

The $K_{sp}$ values of $Al(OH)_3$ and $Zn(OH)_2$ are $8.5 \times 10^{-23}$ and $1.8 \times 10^{-14}$ respectively. If $NH_4OH$ is added to a solution containing $Al^{3+}$ and $Zn^{2+}$ ions,which will precipitate earlier?

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