What volume of H2SO4 solution with mass fraction (ω) equal to 96%, density (ρ1) of which is 1.84 g / cm3

What volume of H2SO4 solution with mass fraction (ω) equal to 96%, density (ρ1) of which is 1.84 g / cm3, is required to prepare 2 liters of H2SO4 solution with ω = 40%, density (ρ2) 1.31 g / cm3?

Let’s calculate the masses of the components of the solution.

To do this, it is necessary to multiply their mass fraction by the weight of the solution.

Let’s calculate the weight of pure sulfuric acid.

M of pure acid = 2000 x 0.4 x 1.31 = 1048 grams;

In order to find the volume of a sulfuric acid solution with such an acid weight, it is necessary to divide such an acid weight by its concentration and density.

The volume of the sulfuric acid solution will be:

V sulfuric acid solution = 1048 / 0.96 / 1.84 = 593.3 ml;

The weight of water in the solution will be:

M water = 2000 x 0.6 x 1.31 = 1572 grams;

Let’s check:

M solution = M acid + M water (solvent) = 1048 + 1572 = 2620 = 2000 x 1.31 grams;