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 \(\left.4.74\right)\)
- A 3.74
- B 4.74
- C 5.74
- D 6.74
Answer & Solution
Correct Answer
(B) 4.74
Step-by-step Solution
Detailed explanation
From Henderson's equation, \[ \begin{aligned} p H &=p K_{a}+\log \frac{\left.\mid C H_{j} C O O N a\right]}{\left|C H_{3} C O O H\right|} \\ &=4.74+\log \frac{1}{1}=4.74 \end{aligned} \]
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