Question

$500$ ml $1M{H}_{2}S{O}_4$ solution is mixed with $400$ ml of $2.5MHCl$ solution. Density of final solution is $1.2$ g/ ml. Concentration of $\left[H^{+}\right]$ in the final solution is :

• A. 2.22 M
• B. 2.67 M
• C. 3.11 M
• D. 3.45 M

Answer 1

Answer: (A)

2.22 M

Total volume of the solution $=500ml+400ml=900ml=0.9L$.

The number of moles of hydrogen ions present in $500$ ml of $1$ M $H_{2}S{O}_4$ solution is $2\times 1\times \frac{500}{1000}=1mole$.

The number of moles of hydrogen ions present in $400$ ml of $2.5$ M HCl solution is $2.5\times \frac{400}{1000}=1mole$.

Thus, total number of moles of hydrogen ions present in the final solution is $1+1=2moles$.

Hence, $\left[H^{+}\right]=\frac{2}{0.9}=2.22M$.

Therefore, option $\left(A\right)$ is correct.