20 mL~ 0 .1 (N) acetic acid is mixed with 10 mL 0.1(N) solution of NaOH. The pH of the resulting solution is (p K_a . of acetic acid is .4.74 )

Correct answer: (B) 4.74. From Henderson's equation, p H =p K_a+log frac .mid C H_j C O O N a ] |C H_3 C O O H | =4.74+log 1/1=4.74

Q31 / 160 · WBJEE 2012 · Chemistry

$20 \mathrm{mL~} 0 .1$ (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
Correct answer
B
4.74
C
5.74
D
6.74

Solution

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

Hence, the correct answer is option: 'B'.

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