2agno3(aq) + nas(aq) + 40200 how many milliliters of 0.225 m nh, solution will exactly react with 30.0 ml of a 0.190 m h2so4 solution? 2nh3(aq) + h2so4(aq) → (nh4)2so4(aq) - 2+1

Approximately 50.67 mL of a 0.225 M NH₃ solution will react with 30.0 mL of a 0.190 M H₂SO₄ solution.

Explanation:

Considering the balanced equation below, we have that 2 mol of NH₃ reacts with  1 mol of H₂SO₄:

2NH₃(aq) + H₂SO₄(aq) → (NH₄)₂SO₄(aq)

Therefore, we need to know the amount of H₂SO₄ present in the 30.0 mL given. We can use the following equation to calculate it:

C is the concentration, n the number of moles of the solute and V is the volume.

H₂SO₄ :  ∴ n = 5.7 x 10⁻³ mol

The amount of NH₃ needed to react will be twice the amount of H₂SO₄, therefore:

NH₃: ∴ V = 50.67 mL

b.false that your answer