Question

$100$ ml of $0.1M$ $H_{2}S{O}_4$ was added to $100$ ml of $0.1M$ $NaOH$, and the mixture was diluted exactly to one litre. Normality of hydrogen ions in the final solution is:

• A. $0.003N$
• B. $0.03N$
• C. $0.01N$
• D. $0.001N$

Answer 1

Answer: (C)

$0.01N$

Total number of moles of hydrogen ions $=0.1\times 0.1\times 2=0.02$

Total number of moles of hydroxide ions $=0.1\times 0.1=0.01$
$0.01$ moles of hydrogen ions will react with $0.01$ moles of hydroxide ions and $0.01$ moles of hydrogen ions will remain.
$0.01$ moles of hydrogen ions are present in $1$ L of solution. Since the valency factor of hydrogen ions is $1$, normality will be equal to molarity.

Hence, the normality of the solution is $0.01$ N.