# What volume of ammonia, measured under normal conditions

**What volume of ammonia, measured under normal conditions, is required to completely neutralize a 20 ml solution with a mass fraction of sulfuric acid of 3% and a density of 1.02 g / ml**

1.Let’s find the mass of the sulfuric acid solution.

m = V p.

m = 20 ml × 1.02 g / ml = 20.4 g.

2.Let’s find the mass of sulfuric acid in the solution.

W = m (substance): m (solution) × 100%,

hence m (substance) = (m (solution) × w): 100%.

m (substance) = (20.4 g × 3%): 100% = 0.612 g.

Let’s find the amount of sulfuric acid substance H2SO4.

n = m: M.

M (H2SO4) = 98 g / mol.

n = 0.612 g: 98 g / mol = 0.00624 mol.

3. Let’s compose the reaction equation. Let’s find the quantitative ratios of substances.

2NH3 + H2SO4 = (NH4) 2SO4

For 1 mol of H2SO4, there are 2 mol of NH3.

The substances are in quantitative ratios of 1: 2. The amount of the NH3 substance will be 2 times more than the amount of the H2SO4 substance.

n (NH3) = 2 n (H2SO4) = 2 × 0.00624 = 0.0125 mol.

4. Find the volume of NH3.

V = Vn n, where Vn is the molar volume of gas, equal to 22.4 l / mol, and n is the amount of substance.

V = 0.0125 mol × 22.4 L / mol = 0.28 L.

Answer: 0.28 l.