Question

The density of a solution containing by mass of sulphuric acid is 1.09 g/ml.then the molarity of sulphuric acid is?

Answer 1

Concentrated aqueous sulphuric acid is 98% H2SO4 by massDensity = 1.80gm/LNumber of moles in H2SO4 of Concentration 0.1 M and volume 1 l =n = C × v= 0.1 × 1= 0.1Calculate 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 H2SO4Convert this mass in volume using density = mass/volume1.80 gml-1 = 9.8g /volumevolume = 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 mlAns: The volume of acid required to make 1 litre of 0.1 M H2SO4