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 2.4 M 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

$\text{Number of moles in 12.0 L of 2.4 M solution}=12.0\times 2.4=28.8mol$
The sulfuric acid solution is 98% w/w.
The weight of sulfuric acid $=28.8\times 98\times \frac{100}{98}=2880g$.
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.