MU 16/P13/Q10
Sulfur dioxide is used as a preservative in wine making.
The following equations describe the reactions that occur when sulfur dioxide dissolves in water.
H2O + SO2 (reversible sign)--- HSO3- + (H+)
HSO3- + (H+) (reversible sign)--- SO3(2-) + 2H+
Which statement about these two reactions is correct?
A HSO3 - acts as a base.
B S03(2-)acts as an acid
C SO2, acts as an oxidising agent.
D SO3(2-) acts as a reducing agent.
Answers
Answered by
0
Explanation: OPTION D
as SO3(-2) GAVE ITS H+ TO H+ TO FORM 2H+ THEREFORE H+ IS GETTING REDUCED
Answered by
7
The true statement about these two reactions is (A) HSO₃⁻ acts as a base.
- There is no change in the oxidation state of any species at any stage, so C and D options are ruled out.
- B cannot be correct as SO₃²⁻ doesn't contain H+, so it cannot act as an acid.
- So we are left only with the option (A)
- The first reaction is:
H₂O + SO₂ ⇄ HSO₃⁻ + H⁺
- As it is a reversible reaction, so it can also be considered in the backward direction as following:
HSO₃⁻ + H⁺ ⇄ H₂O + SO₂
- Here, HSO₃⁻ is acting as a base. So it is the correct option.
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