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TS EAMCET · Chemistry · Ionic Equilibrium

If the ionic product of \(\mathrm{Ni}(\mathrm{OH})_2\) is \(1.9 \times 10^{-15}\), the molar solubility of \(\mathrm{Ni}(\mathrm{OH})_2\) in \(1.0 \mathrm{M} \mathrm{NaOH}\) is

  1. A \(1.9 \times 10^{-18} \mathrm{M}\)
  2. B \(1.9 \times 10^{-13} \mathrm{M}\)
  3. C \(1.9 \times 10^{-15} \mathrm{M}\)
  4. D \(1.9 \times 10^{-14} \mathrm{M}\)
Verified Solution

Answer & Solution

Correct Answer

(C) \(1.9 \times 10^{-15} \mathrm{M}\)

Step-by-step Solution

Detailed explanation

\begin{aligned} & \mathrm{NaOH} \rightleftharpoons \underset{\mathrm{CM}}{\mathrm{Na}^{+}}+\underset{\mathrm{CM}}{\mathrm{OH}^{-}} \\ & \mathrm{Ni}(\mathrm{OH})_2 \rightleftharpoons \mathrm{Ni}_x^{2+}+\underset{x}{2 \mathrm{OH}^{-}} \\ & \therefore \quad…