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TS EAMCET · Chemistry · Ionic Equilibrium

What is the \(\mathrm{pH}\) of acetic acid at equilibrium, given that acetic acid concentration is \(0.1 \mathrm{M}\) and it is \(30 \%\) dissociated at equilibrium? \((\log 3=0.47)\)

  1. A 2
  2. B 1.53
  3. C 3.53
  4. D 3
Verified Solution

Answer & Solution

Correct Answer

(B) 1.53

Step-by-step Solution

Detailed explanation

The required relation is \[ \mathrm{CH}_3 \mathrm{COOH} \rightleftharpoons \mathrm{CH}_3 \mathrm{COO}^{-}+\mathrm{H}^{+} \] \(\because\) Dissociation occurs \(=30 \%\), means 100 moles of \(\mathrm{CH}_3 \mathrm{COOH}\), gives \(=30\) moles of \(\mathrm{H}^{+}\)-ions. Thus, 0.1…