The pH of a solution at 25,^oC containing 0.1 | vedclass

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(B) The solution is a buffer solution consisting of a weak acid $(CH_3COOH)$ and its salt with a strong base $(CH_3COONa)$.We use the Henderson-Hassel

Vedclass · Accepted Answer

$5.09$

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(B) The solution is a buffer solution consisting of a weak acid $(CH_3COOH)$ and its salt with a strong base $(CH_3COONa)$.We use the Henderson-Hasselbalch equation: $pH = pK_a + \log \frac{[salt]}{[acid]}$.Given: $pK_a = 4.57$,$[salt] = 0.10\,M$,$[acid] = 0.03\,M$.Substituting the values: $pH = 4.57 + \log \frac{0.10}{0.03} = 4.57 + \log(3.33)$.Since $\log(3.33) \approx 0.52$,we get $pH = 4.57 + 0.52 = 5.09$.

The $pH$ of a solution at $25\,^oC$ containing $0.10\,M$ sodium acetate and $0.03\,M$ acetic acid is ($pK_a$ for $CH_3COOH = 4.57$)

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