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The solubility product of \( \mathrm{Zn}(\mathrm{OH})_{2} \) is \( 10^{-14} \) at \( 25^{\circ} \mathrm{C} \).
\( \mathrm{P} \) What would be the concentration \( \mathrm{Zn}^{+2} \) ion in 0.1

W \( \mathrm{M}-\mathrm{NH}_{4} \mathrm{OH} \) solution which is \( 50 \% \) ionized?
(1) \( 2 \times 10^{-13} \)
(2) \( 4 \times 10^{-12} \)
(3) \( 4 \times 10^{-8} \)
(4) \( 2 \times 10^{-11} \)
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