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Question: Answered & Verified by Expert
$20 \mathrm{mL~} 0 .1$ (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 $\left.4.74\right)$
ChemistryIonic EquilibriumWBJEEWBJEE 2012
Options:
  • A 3.74
  • B 4.74
  • C 5.74
  • D 6.74
Solution:
1725 Upvotes Verified Answer
The correct answer is: 4.74


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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