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WBJEE · Chemistry · Ionic Equilibrium

\(20 \mathrm{mL~} 0 .1\) (N) acetic acid is mixed with \(10 \mathrm{mL}\) \(0.1(\mathrm{N})\) solution of NaOH. The pH of the resulting solution is \(\left(p K_{a}\right.\) of acetic acid is \(\left.4.74\right)\)

  1. A 3.74
  2. B 4.74
  3. C 5.74
  4. D 6.74
Verified Solution

Answer & Solution

Correct Answer

(B) 4.74

Step-by-step Solution

Detailed explanation

From Henderson's equation, \[ \begin{aligned} p H &=p K_{a}+\log \frac{\left.\mid C H_{j} C O O N a\right]}{\left|C H_{3} C O O H\right|} \\ &=4.74+\log \frac{1}{1}=4.74 \end{aligned} \]