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The $\mathrm{pH}$ of $0.1 \mathrm{M}$ acetic acid solution is closest to [Dissociation constant of acid $\mathrm{K}_{\mathrm{a}}=1.8 \times 10^{-5}$ ]
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The correct answer is:
$2.87$
$\left[\mathrm{H}^{+}\right]=\sqrt{\mathrm{K}_{\mathrm{a}} \cdot \mathrm{c}}=\sqrt{1.8 \times 10^{-5} \times 0.1}=\sqrt{1.8} \times 10^{-3}$
$\mathrm{pH}=3-\log (1.34)=2.87$
$\mathrm{pH}=3-\log (1.34)=2.87$
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