The pH of a 0.01 , M solution of acetic acid | vedclass

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(B) The concentration of hydrogen ions $[H^{+}]$ is given by the formula $[H^{+}] = C 	imes \alpha$,where $C$ is the molar concentration and $\alpha$

Vedclass · Accepted Answer

$2.903$

Vedclass · Answer

(B) The concentration of hydrogen ions $[H^{+}]$ is given by the formula $[H^{+}] = C 	imes \alpha$,where $C$ is the molar concentration and $\alpha$ is the degree of dissociation.Given $C = 0.01 \, M$ and $\alpha = \frac{12.5}{100} = 0.125$.$[H^{+}] = 0.01 	imes 0.125 = 1.25 	imes 10^{-3} \, M$.The $pH$ is calculated as $pH = -\log[H^{+}]$.$pH = -\log(1.25 	imes 10^{-3}) = -(\log(1.25) + \log(10^{-3}))$.$pH = -(\log(1.25) - 3) = 3 - \log(1.25)$.Since $\log(1.25) \approx 0.097$,$pH = 3 - 0.097 = 2.903$.

The $pH$ of a $0.01 \, M$ solution of acetic acid having a degree of dissociation of $12.5 \%$ is:

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