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? \((\log 3=0.47)\)
- A 2
- B 1.53
- C 3.53
- D 3
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…
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