Question

Find out the volume of $98\%$ (w/w) $H_{2}S{O}_4$ (density $=1.8$ g/ml) that must be diluted to prepare $12.0$ litres of $2.4M$ sulphuric acid solution.

• A. $1.6$ L
• B. $1.8$ L
• C. $2.3$ L
• D. $2.8$ L

Answer 1

The correct option is A $1.6$ L

Number of moles in $12.0$ L of $2.4M$ solution $=12.0\times 2.4=28.8$ moles.

The sulfuric acid solution is $98\%$ w/w.

The weight of sulfuric acid $=28.8\times 98\times \frac{100}{98}=2880g$.

$\text{Density}=\frac{\text{Mass}}{\text{Volume}}=1.8$ g/ml.

Hence, volume of the sulfuric acid solution is $\frac{\text{Mass}}{\text{density}}=\frac{2880g}{1.8g/ml}=1600ml=1.6L$.

Therefore, option A is correct.