Question

A mixture of 0.1 M $HCl$ and 0.2 M $H_{2}S{O}_4$ is titrated with 0.1 M $NaOH$. How much volume of $NaOH$ is required for complete neutralization, if the initial volume of the acidic solution (V) is 10 mL?

• A. 10 mL
• B. 20 mL
• C. 30 mL
• D. 40 mL

Answer 1

The correct option is C 30 mL

n-factor$\left(n_f\right)$ for $HCl,H_{2}S{O}_{4}andNaOH$ are 1, 2 and 1 respectively.

So, for neutralization,
number of equivalents of acids = number of equivalents of base
$(M_1\times V)+(2\times M_2\times V)=M_3\times V^{{}^{\prime }}$; where $M_1$, $M_2$ and $M_3$ are concentrations of $HCl,H_{2}S{O}_{4}andNaOH$ respectively.

$\therefore$ volume of base required = $\frac{0.1\times 10+2\times 0.1\times 10}{0.1}=30mL$