Calculate the masses of sulfuric acid and barium hydroxide that should be used to extract

Calculate the masses of sulfuric acid and barium hydroxide that should be used to extract barium sulfate in an amount of 0.1 mol.

Sulfuric acid and barium hydroxide react to form water and the barium sulfate salt, which precipitates. The reaction equation can be written as:

H2SO4 + Ba (OH) 2 = BaSO4 + 2 H2O

According to the reaction equation, we see that the amount of sulfuric acid, barium hydroxide and barium sulfate are equal. This means that for the formation of 0.1 mol of barium sulfate, 0.1 mol of sulfuric acid and barium hydroxide were required.

Now, knowing the amount of a substance, you can calculate the masses of substances. The general formula will look like:

m = M * n, where

m is the mass;

M is molar mass;

n is the amount of substance.

M (H2SO4) = 96 g / mol, M (Ba (OH) 2) = 171 g / mol.

m (H2SO4) = 96 * 0.1 = 9.6 g.

m (Ba (OH) 2) = 171 * 0.1 = 17.1 g.

Answer: the mass of the true acid is 9.6 g, the mass of barium hydroxide is 17.1 g.