Given Ka=1.00×10−5,C=0.100 mol for a weak electrolyte, degree of dissociation ∝=CKa=0.1001×10−5=10−2=1% Related Theory In any acid-base reaction, the equilibrium will favour the reaction that moves the proton to the stronger base. This equilibrium constant is referred to as the ion-product constant for water, Kw. In pure water, some molecules act as bases and some as acids.
A weak acid, HA and a K_a of 1.00 × 10^-5. If 0.100 ~mol of this acid is dissolved in one litre of water, the percentage of acid dissociated at…
NEET UG 2007 — Chemistry Physical Chemistry
2007mcqmedium
A weak acid, HA and a Ka of 1.00×10−5. If 0.100 mol of this acid is dissolved in one litre of water, the percentage of acid dissociated at equilibrium is closer to:
Official previous-year question
Held on 30 Apr 2007 · Verified 9 Jul 2026.
Options
- A
1.00%
- B
99.9%
- C
0.100%
- D
99.0%
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