What would be the pH of a solution obtained by mixing 5 g of acetic acid and 7.5 g of sodium acetate and making the volume equal to 500 mL ? (\(\mathrm{K_a} = 1.75 \times 10^{-5}\), \(\mathrm{pK_a} = 4.76\))
Show Hint
- \(\mathrm{pH} = 4.70\)
- \(\mathrm{pH} \lt 4.70\)
- pH of solution will be equal to pH of acetic acid
- \(4.76 \lt \mathrm{pH} \lt 5.0\)
The Correct Option is D
Solution and Explanation
Moles of \(\mathrm{CH_3COONa}\) = 7.5/82 = 0.0915 mol (M = 82)
Buffer: \(\mathrm{pH} = \mathrm{pK_a} + \log\frac{[\text{salt}]}{[\text{acid}]}\) (volume cancels)
\(\mathrm{pH} = 4.76 + \log\frac{0.0915}{0.0833} = 4.76 + \log 1.098 = 4.76 + 0.04 \approx 4.80\)
This lies between 4.76 and 5.0.
Answer: (4) \(4.76 \lt \mathrm{pH} \lt 5.0\)
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