KCET · Chemistry · Ionic Equilibrium
A buffer solution contains \(0.1\) mole of sodium acetate dissolved in \(1000 \mathrm{~cm}^{3}\) of \(0.1 \mathrm{M}\) acetic acid. To the above buffer solution, \(0.1\) mole of sodium acetate is further added and dissolved. The \(\mathrm{pH}\) of the resulting buffer is
- A \(\mathrm{p} K_{a}\)
- B \(\mathrm{p} K_{a}+2\)
- C \(\mathrm{p} K_{a}-\log 2\)
- D \(\mathrm{p} K_{a}+\log 2\)
Answer & Solution
Correct Answer
(D) \(\mathrm{p} K_{a}+\log 2\)
Step-by-step Solution
Detailed explanation
\(\mathrm{pH}=\mathrm{p} K_{a}+\log \frac{\text { [salt] }}{\text { [acid] }}\)
When extra \(0.1\) mole sodium acetate is added
[salt \(]=0.2 \mathrm{~mol} \mathrm{dm^{-3 }}\)
[acid] \(=0.1 \mathrm{~mol} \mathrm{dm}^{-3}\)
\(\therefore \quad \mathrm{pH}=\mathrm{p} K_{a}+\log \frac{[0.2]}{[0.1]}\)
\(\mathrm{pH}=\mathrm{p} K_{\mathrm{a}}+\log 2\)
When extra \(0.1\) mole sodium acetate is added
[salt \(]=0.2 \mathrm{~mol} \mathrm{dm^{-3 }}\)
[acid] \(=0.1 \mathrm{~mol} \mathrm{dm}^{-3}\)
\(\therefore \quad \mathrm{pH}=\mathrm{p} K_{a}+\log \frac{[0.2]}{[0.1]}\)
\(\mathrm{pH}=\mathrm{p} K_{\mathrm{a}}+\log 2\)
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