The pH of 0.1 , M acetic acid solution is clo | vedclass

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(A) Given,dissociation constant,$K_{a} = 1.8 	imes 10^{-5}$ and concentration $c = 0.1 \, M$. For the dissociation of acetic acid: $CH_{3}COOH ight

Vedclass · Accepted Answer

$2.87$

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(A) Given,dissociation constant,$K_{a} = 1.8 	imes 10^{-5}$ and concentration $c = 0.1 \, M$. For the dissociation of acetic acid: $CH_{3}COOH ightleftharpoons CH_{3}COO^{-} + H^{+}$. Since acetic acid is a weak acid,the concentration of $H^{+}$ ions is given by $[H^{+}] = \sqrt{K_{a} 	imes c}$. $[H^{+}] = \sqrt{1.8 	imes 10^{-5} 	imes 0.1} = \sqrt{1.8 	imes 10^{-6}} = 1.34 	imes 10^{-3} \, M$. $pH = -\log[H^{+}] = -\log(1.34 	imes 10^{-3}) = 3 - \log(1.34) \approx 3 - 0.127 = 2.873$. Thus,the $pH$ is closest to $2.87$.

The $pH$ of $0.1 \, M$ acetic acid solution is closest to $.....$ [Dissociation constant of the acid,$K_{a} = 1.8 \times 10^{-5}$]

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