Concentrated aqueous sulphuric acid is 98% $H_{2}S{O}_4$ by mass and has a density of 1.80gm/L. Volume of acid required to make one litre of 0.1M $H_{2}S{O}_4$ solution is:

The correct option is B 5.55 ml

Solution:- (C) $5.55mL$

Given:-

Concentrated aqueous sulphuric acid is $98\%H_{2}S{O}_4$ by mass

Density $=1.80gm/L$

Number of moles in $H_{2}S{O}_4$ of concentration $0.1M$ and volume $1L$-

$n=M\times V$

$\Rightarrow =0.1\times 1=0.1\text{mol}$

Molecular mass of $H_{2}S{O}_4=98g$

Therefore,

Mass of $0.1$ mole $H_{2}S{O}_4=0.1\times 98=9.8g$

As we know that,

$\text{density}=\frac{\text{mass}}{\text{volume}}$

$\Rightarrow \text{Volume}=\frac{9.8}{1.80}=5.44mL$

Given that the solution is $98\%$ pure.

Therefore,

Volume required $=\frac{5.44}{98}\times 100=5.55mL$

Hence the volume of acid required to make $1$ litre of $0.1M{H}_{2}S{O}_4$ solution is $5.55ml$.