Question

$500\text{mL}$ of a $\frac{N}{5}{H}_{2}S{O}_4$ and $200\text{ml}$ of $\frac{N}{10}NaOH$ are mixed. What will be the normality of $H^{+}$ ions in the solution?

• A. $0.114\text{N}$
• B. $0.328\text{N}$
• C. $0.256\text{N}$
• D. $0.780\text{N}$

Answer 1

The correct option is A $0.114\text{N}$

$\Rightarrow$Number of milliequivalents = Normality $\times$ volume in mL
$\Rightarrow$Number of milliequivalents of $H_{2}S{O}_4$ $=\frac{1}{5}\times 500=100milliequivalents$
$\Rightarrow$Number of milliequivalents of $NaOH$
$=\frac{1}{10}\times 200=20$ milliequivalents
$\Rightarrow$After mixing of the acid and the base, milliequivalents of $H^{+}ions$$=100-20=80$ milliequivalents
$\Rightarrow$Normality of $H^{+}$ ions:
$\frac{\text{milliequivalents}}{\text{total volume of the solution in mL}}=\frac{80}{700}=0.114\text{N}$