Calculate the pH of a buffer solution prepare | vedclass

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(A) $1$. Calculate the millimoles of reactants: $n(CH_3COOH) = 100 \ mL 	imes 0.1 \ M = 10 \ mmol$ $n(NaOH) = 30 \ mL 	imes 0.1 \ M = 3 \ mmol$ $2$.

Vedclass · Accepted Answer

$4.38$

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(A) $1$. Calculate the millimoles of reactants: $n(CH_3COOH) = 100 \ mL 	imes 0.1 \ M = 10 \ mmol$ $n(NaOH) = 30 \ mL 	imes 0.1 \ M = 3 \ mmol$ $2$. Reaction: $CH_3COOH + NaOH ightarrow CH_3COONa + H_2O$ After reaction: $n(CH_3COOH)_{remaining} = 10 - 3 = 7 \ mmol$ $n(CH_3COONa)_{formed} = 3 \ mmol$ $3$. Use Henderson-Hasselbalch equation: $pH = pK_a + \log(\frac{[Salt]}{[Acid]}) = 4.76 + \log(\frac{3}{7})$ $pH = 4.76 + \log(0.428) = 4.76 - 0.368 = 4.392 \approx 4.39$

Calculate the $pH$ of a buffer solution prepared by mixing $30 \ mL$ of $0.1 \ M$ $NaOH$ and $100 \ mL$ of $0.1 \ M$ $CH_3COOH$. (Given: $pK_a$ of $CH_3COOH = 4.76$)

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