Q31 / 150 · MHT CET 2023 (10 May Shift 1) · Chemistry

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

  • A
    $2.20 \times 10^{-2}$
  • B
    $1.60 \times 10^{-4}$
  • Correct answer
    C
    $1.44 \times 10^{-6}$
  • D
    $2.40 \times 10^{-4}$

Solution

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

Hence, the correct answer is option: 'C'.

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