The pH of a 0.1 M solution of acetic acid wi | vedclass

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(D) The dissociation reaction of acetic acid is: $CH_3COOH \rightleftharpoons CH_3COO^{-} + H^{+}$Given concentration $c = 0.1 \ M$ and degree of diss

Vedclass · Accepted Answer

$2.88$

Vedclass · Answer

(D) The dissociation reaction of acetic acid is: $CH_3COOH ightleftharpoons CH_3COO^{-} + H^{+}$Given concentration $c = 0.1 \ M$ and degree of dissociation $\alpha = 0.0132$.The concentration of hydrogen ions is given by $[H^{+}] = c 	imes \alpha$.$[H^{+}] = 0.1 	imes 0.0132 = 0.00132 \ M$.The $pH$ is calculated as $pH = -\log[H^{+}]$.$pH = -\log(0.00132) = -\log(1.32 	imes 10^{-3}) = 3 - \log(1.32) \approx 3 - 0.12 = 2.88$.Thus,the $pH$ of the solution is $2.88$.

The $pH$ of a $0.1 \ M$ solution of acetic acid will be (degree of dissociation of acetic acid is $0.0132$).

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