$0.01 \mathrm{M}$ acetic acid solution is $1 \%$ ionised, then $\mathrm{pH}$ of this acetic acid solution is :

$0.01 \mathrm{M}$ acetic acid solution is $1 \%$ ionised, then $\mathrm{pH}$ of this acetic acid solution is :
  1. 3
  2. 2
  3. 4
  4. 1

Solution

Ionisation of $\mathrm{CH}_3 \mathrm{COOH}$ is $1 \%$ in aqueous solution. So, $\left[\mathrm{H}^{+}\right]=\frac{1}{100} \times$ concentration of $\mathrm{CH}_3 \mathrm{COOH}$ $\begin{aligned} & =\frac{1}{100} \times 10^{-2}=10^{-4} \\ \mathrm{pH} & =-\log \left[\mathrm{H}^{+}\right]=-\log \left(1 \times 10^{-4}\right) \\ \mathrm{pH} & =4 \end{aligned}$

Asked in: MHT CET Full Test 11

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