How many ml of 96% sulfuric acid p = 1.84 g / ml is required to prepare 300 ml of a 0.5 M solution?

Let’s find the required amount of the substance for the preparation of this solution.

To do this, multiply the volume of the solution and its molar concentration.

In order to prepare such a solution, it is necessary to weigh and dissolve 0.3 x 0.5 = 0.15 mol of acid in water.

Let’s find the required mass of acid.

To do this, we multiply the molar weight of the acid by the chemical amount of the substance.

M H2SO4 = 2 + 32 + 16 x 4 = 98 grams / mol;

m H2SO4 = 98 x 0.15 = 14.7 grams;

Let’s calculate the volume of the acid.

V H2SO4 = 14.7 / 1.84 / 0.96 = 8.322 ml.