WBJEE · Chemistry · Ionic Equilibrium
In which of the following mixed aqueous solutions, \(\mathrm{pH}=\mathrm{p} K_{a}\) at equilibrium?
(1) \(100 \mathrm{mL}\) of \(0.1 \mathrm{M} \mathrm{CH}_{3} \mathrm{COOH}+100 \mathrm{mL}\) of \(0.1 \mathrm{MCH}_{3} \mathrm{COONa}\)
(2) \(100 \mathrm{mL}\) of \(0.1 \mathrm{MCH}_{3} \mathrm{COOH}+50 \mathrm{mL}\) of 0.1 \(\mathrm{M} \mathrm{NaOH}\)
(3) \(100 \mathrm{mL}\) of \(0.1 \mathrm{M} \mathrm{CH}_{3} \mathrm{COOH}+100 \mathrm{mL}\) of \(0.1 \mathrm{M} \mathrm{NaOH}\)
(4) \(100 \mathrm{mL}\) of \(0.1 \mathrm{M} \mathrm{CH}_{3} \mathrm{COOH}+100 \mathrm{mL}\) of \(0.1 \mathrm{M} \mathrm{NH}_{3}\)
- A (1) is correct
- B (2) is correct
- C (3) is correct
- D Both (1) and (2) are correct
Answer & Solution
Correct Answer
(D) Both (1) and (2) are correct
Step-by-step Solution
Detailed explanation
pH of buffer solutions is given by \[ \mathrm{pH}=\mathrm{pK}_{a}+\mathrm{log} \frac{[\mathrm{salt}]}{[\mathrm{acid}]} \] (1) \(\mathrm{CH}_{3} \mathrm{COOH}\) and \(\mathrm{CH}_{3} \mathrm{COONa}\) \(\quad \quad\) \(100 \times 0.1\) \(\quad \quad…
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