Question

50 mL of a $\frac{N}{2}$ HCl solution, 50 mL of a $\frac{N}{5}{H}_{2}S{O}_4$ solution and 200 mL of a $\frac{N}{10}$ NaOH solution are mixed. What will be the normality of $H^{+}$ ions in the resultant solution?

• A. 0.05 N
• B. 0.25 N
• C. 0.02 N
• D. 0.50 N

Answer 1

The correct option is A 0.05 N

Milliequivalents of $H^{+}=(50\times \frac{1}{2})+(50\times \frac{1}{5})=25+10=35$
Milliequivalents of $O{H}^{-}=200\times \frac{1}{10}=20$
After mixing, milliequivalents of $H^{+}$ left = 35 – 20 = 15
$\therefore$ Normality of $H^{+}$ ion = $\frac{15}{300}$ = 0.05 N