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Question

The weak acid, HA has a Ka of 1.00×105. If 0.1 mol of this acid is dissolved in one litre of water, the percentage of acid dissociated at equilibrium is closet to:
  1. 1%
  2. 99.9%
  3. 0.1%
  4. 99%

A
99.9%
B
1%
C
0.1%
D
99%
Solution
Verified by Toppr

0.1 mole of acid is dissolved in 1 litre of water means [HA]=0.1M
Let 'α' be degree of dissocition
HAH++A
0.1
0.1(1α) 0.1α 0.1α
Ka=[H+][A][HA]=0.12α20.1(1α)
Let α<<1 so 1α=1
Ka=0.1α2=105
α=102
% of acid dissociated=1%

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