Q.31 Acetic acid dissociates 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}
C. 1.44 \times 10^{-6}
D. 2.40 \times 10^{-4}
Answer: C. 1.44 \times 10^{-6}
Explanation:-
Percent dissociation = 1.20 %
Degree of dissociation ( \alpha) = 0.012
For a weak monobasic acid,
Ka = \alpha^{2}c = (0.012)2 x 0.01 = 1.44 x 10-6