Question

Calculate the volume of $0.2\text{N}NaOH$ required for neutralising the solution obtained by mixing $20\text{mL}$ of $0.1\text{N}{H}_{2}S{O}_4$ and $20\text{mL}$ of $0.1\text{N}HCl$.

• A. $10\text{mL}$
• B. $20\text{mL}$
• C. $30\text{mL}$
• D. $40\text{mL}$

Answer 1

The correct option is B $20\text{mL}$

In any acid base titration, the number of equivalents of the acids and the bases are equal.
$\text{Milliequivalent of the acids}=\text{volume in mL}\times \text{normality}$
$=20\times 0.1\text{N}{H}_{2}S{O}_4+20\times 0.1\text{N}HCl=4$

$\text{Volume of NaOH}=\frac{\text{milliequivalents}}{\text{normality}}=\frac{4}{0.2}=20\text{mL}$