The pH of a solution containing 0.10 M sodiu | vedclass

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Question

(C) The given solution is a buffer solution consisting of a weak acid (acetic acid) and its conjugate base (sodium acetate). The $pH$ of such a buffer

Vedclass · Accepted Answer

$5.09$

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(C) The given solution is a buffer solution consisting of a weak acid (acetic acid) and its conjugate base (sodium acetate). The $pH$ of such a buffer can be calculated using the Henderson-Hasselbalch equation: $pH = pK_a + \log \left( \frac{[	ext{salt}]}{[	ext{acid}]} ight)$ Given: $pK_a = 4.57$ $[	ext{salt}] = [	ext{CH}_3	ext{COONa}] = 0.10 \ M$ $[	ext{acid}] = [	ext{CH}_3	ext{COOH}] = 0.03 \ M$ Substituting the values: $pH = 4.57 + \log \left( \frac{0.10}{0.03} ight)$ $pH = 4.57 + \log(3.333)$ $pH = 4.57 + 0.5228$ $pH = 5.0928 \approx 5.09$

The $pH$ of a solution containing $0.10 \ M$ sodium acetate and $0.03 \ M$ acetic acid $(pK_a = 4.57)$ at $298 \ K$ will be ...........

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