Acetic acid dissociated to $1.20 \%$ in its $0.01 \mathrm{M}$ solution. What is the value of its…

Acetic acid dissociated to $1.20 \%$ in its $0.01 \mathrm{M}$ solution. What is the value of its dissociation constant?
  1. $2.20 \times 10^{-2}$
  2. $1.60 \times 10^{-4}$
  3. $1.44 \times 10^{-6}$
  4. $2.40 \times 10^{-4}$

Solution

Percent dissociation $=1.20 \%$ Degree of dissociation $(\alpha)=0.012$ For a weak monobasic acid, $\mathrm{K}_{\mathrm{a}}=\alpha^2 \mathrm{c}=(0.012)^2 \times 0.01=1.44 \times 10^{-6}$

Asked in: MHT CET 2023 (10 May Shift 1)

Practice more Solutions questions on Aicharya