Question

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

Answer 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.

Step-by-step 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 = (n)/(V)`

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

H₂SO₄ :
`0.190 M = (n)/(0.0 3L)` ∴ n = 5.7 x 10⁻³ mol

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

NH₃:
`0.225 = (0.0114)/(V)` ∴ V = 50.67 mL