Concentrated aqueous sulphuric acid is  98% H2SO4 by mass and has  densityof 1.80gm/L.

what is the volume of acid required to make 1 litre of 0.1 M H2SO4 solution? 

Concentrated aqueous sulphuric acid is 98% H₂SO₄ by mass

Density = 1.80gm/L

Number of moles in H₂SO₄ of Concentration 0.1 M and volume 1 l =
n = C × v

= 0.1 × 1

= 0.1

Calculate the mass required to get 0.1 mol H₂SO₄
n = unknown mass/Molar mass

= unknown mass/98 gmol^-1

0.1 × 98 gmol-1 = 9.8 g
?

We need 9.8 gram H₂SO₄

Convert this mass in volume using density = mass/volume

1.80 gml-1 = 9.8g /volume
volume = 9.8 g/1.8g ml-1

= 5.44 ml.

5.44 ml will require if solution is 100 % pure, But given it is 98%

So the volume required = 100 x 5.44/98

= 5.55 ml

Ans: The volume of acid required to make 1 litre of 0.1 M H₂SO₄ solution is 5.55 ml.