Question

When $100ml$ of $\frac{M}{10}{H}_{2}S{O}_4$ is mixed with $500ml$ of $\frac{M}{10}NaOH$ then nature of resulting solution and normality of excess of reactant left is :

• A. Acidic, $\frac{N}{5}$
• B. Basic, $\frac{N}{5}$
• C. Basic, $\frac{N}{20}$
• D. Acidic, $\frac{N}{20}$

Answer 1

The correct option is C Basic, $\frac{N}{20}$

$100ml$ of $\frac{M}{10}{H}_2{SO}_4$

$\left[H^{+}\right]=100\times \frac{M}{10}\times 2=20$ millimoles

$\left[{OH}^{-}\right]=500\times \frac{M}{10}\times 1=50$ millimoles

Hence after reaction $30$ millimoles of $\left[{OH}^{-}\right]$ remaining.

So, basic. Normality $=\frac{30\times {10}^{-3}}{600\times {10}^{-3}}=\frac{N}{20}$