Question

hlorine (Cl₂) is used to purify driving water. Too much chlorine is harmful to humans. The excess chlorine is often removed by treating with sulfur dioxide (SO₂). Using the unbalanced chemical equation determine the mass of SO₂ needed to remove 442 g of excess Cl₂.

Cl₂ + SO₂ + H₂O ----> Cl^– + SO₄^2– + H⁺

If the volume of the solution is 69.3 L what is the final concentration of H⁺ after reacting all 442 g of Cl₂?

Answer 1

Ans.

The unbalanced chemical reaction is

To solve for the mass of SO₂ needed, first write the balanced chemical equation.

1 mol of SO₂ is required to react with 1 mol of Cl₂

Molar mass of Cl₂ = 70.906g/mol

Molar mass of SO₂ = 64.066g/mol

Therefore, 70.906g of Cl₂ will react with 64.066g of SO₂

1g of Cl₂ will react with mass of SO₂ given by

Therefore, 442g of Cl₂ will react with SO₂ given by

of SO₂

Therefore, the mass of SO₂ needed to remove 442g of excess Cl₂ = 399.362g

From the balanced equation, 1 mol of Cl₂ produces 4 mol of H⁺

No. of mol of excess Cl₂ is

Therefore, no. of mol of H⁺ is

Volume of the solution = 69.3L

Concentration of H⁺ is

or

Therefore, the concentration of H⁺ after reacting all 442g of Cl₂ = 0.360M