Calculate dissociation constant of $0.001 \mathrm{M}$ weak monoacidic base undergoing $2 \%$ dissociation.

Calculate dissociation constant of $0.001 \mathrm{M}$ weak monoacidic base undergoing $2 \%$ dissociation.
  1. $4 \times 10^{-7}$
  2. $2 \times 10^{-6}$
  3. $2 \times 10^{-7}$
  4. $1 \times 10^{-7}$

Solution

$\begin{aligned} & \alpha=\frac{\text { Percent dissociation }}{100}=\frac{2}{100}=0.02 \\ & K_a=\alpha^2 c=(0.02)^2 \times 0.001=4 \times 10^{-7}\end{aligned}$

Asked in: MHT CET 2023 (14 May Shift 1)

Practice more Ionic Equilibria questions on Aicharya