What is the pH of a solution containing 50 m | vedclass

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(D) The solution is an acidic buffer consisting of a weak acid $(CH_3COOH)$ and its salt with a strong base $(CH_3COONa)$.Using the Henderson-Hasselba

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$5$

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(D) The solution is an acidic buffer consisting of a weak acid $(CH_3COOH)$ and its salt with a strong base $(CH_3COONa)$.Using the Henderson-Hasselbalch equation:$pH = pK_{a} + \log_{10} \frac{[Salt]}{[Acid]}$Given:$pK_{a} = 4.50$$[Salt] = 0.1 \ M$$[Acid] = 0.01 \ M$Substituting the values:$pH = 4.50 + \log_{10} \frac{0.1}{0.01}$$pH = 4.50 + \log_{10} (10)$Since $\log_{10} (10) = 1$,$pH = 4.50 + 1 = 5.50$

What is the $pH$ of a solution containing $50 \ mL$ each of $0.1 \ M$ sodium acetate and $0.01 \ M$ acetic acid (in $.5$)? $(pK_{a} \ CH_3COOH = 4.50)$

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