Calculate the pH of a buffer solution contain | vedclass

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(A) For an acidic buffer solution,the Henderson-Hasselbalch equation is given by:$pH = pK_{a} + \log_{10} \frac{[	ext{Salt}]}{[	ext{Acid}]}$Given:$p

Vedclass · Accepted Answer

$4.5$

Vedclass · Answer

(A) For an acidic buffer solution,the Henderson-Hasselbalch equation is given by:$pH = pK_{a} + \log_{10} \frac{[	ext{Salt}]}{[	ext{Acid}]}$Given:$pK_{a} = 4.2$$[	ext{Salt}] = 0.054 \ M$$[	ext{Acid}] = 0.027 \ M$Substituting the values:$pH = 4.2 + \log_{10} \left( \frac{0.054}{0.027} ight)$$pH = 4.2 + \log_{10} (2)$Since $\log_{10} 2 \approx 0.3010$,$pH = 4.2 + 0.3010 = 4.5010$Thus,the $pH$ is approximately $4.5$.

Calculate the $pH$ of a buffer solution containing $0.027 \ M$ weak acid and $0.054 \ M$ of its salt with a strong base,if the $pK_{a}$ is $4.2$.

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