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AIIMS 2002
Exam
AIIMS
Year
2002
Subject
Chemistry
Chapter
Ionic Equilibrium

AIIMS 2002 · Chemistry · Ionic Equilibrium

The pH of solution containing 0.10 M sodium acetate and 0.03 M...

The pH\mathrm{pH} of solution containing 0.10M0.10 \mathrm{M} sodium acetate and 0.03M0.03 \mathrm{M} acetic acid is (pKa\left(\mathrm{p} K_a\right. for CH3COOH=4.57)\left.\mathrm{CH}_3 \mathrm{COOH}=4.57\right)

Options

  1. A4.09
  2. B6.09
  3. C5.09
  4. D7.09

Correct answer

C. 5.09

Step-by-step solution

According to Henderson's equation, pH=pKa+log⁡[ salt ][ acid ]CH3COOH+NaOH→CH3COONa+H2O\begin{aligned} & \mathrm{pH}=\mathrm{p} K_a+\log \frac{[\text{ salt }]}{[\text{ acid }]} \\ & \mathrm{CH}_3 \mathrm{COOH}+\mathrm{NaOH} \rightarrow \mathrm{CH}_3 \mathrm{COONa}+\mathrm{H}_2 \mathrm{O}\end{aligned} Puttingthethevalues, we get : pH=4.57+log⁡0.100.03⇒pH=5.09\begin{aligned}\mathrm{pH} & =4.57+\log\frac{0.10}{0.03} \\ \Rightarrow \quad \mathrm{pH} & =5.09 \end{aligned}
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