Hydrogen peroxide can act as either an oxidizing agent or a reducing agent. (a) When H₂O₂ is treated with aqueous KI, I₂ forms. In which role is H₂O₂ acting? What oxygen-containing product is formed?

When H₂O₂ serves as an oxidizing agent, the oxygen of hydrogen peroxide (that is present in -1 oxidation state) is reduced to H₂O (-2 oxidation state).

H₂O₂ + 2H+ + 2e → 2H₂O

When H₂O₂ (-1 oxidation state)serves as a reducing agent, the oxygen of H₂O₂ is oxidized to O₂ ( 0 oxidation state) and bubbles are noticed. As a reducing agent:

2 KMnO₄ + 5 H₂O₂ + 3 H₂SO₄ --> K₂SO₄ + 5O₂ + 2MnSO₄ + 8H₂O

or

2 MnO₄- + 5 H₂O₂ + 6H⁺ → 5O₂ + 2Mn₂- + 8H₂O

What is Hydrogen Peroxide?

Hydrogen peroxide is the simplest kind of peroxide available
It is a colourless liquid and is used in aqueous solution for safety reasons
Concentrated hydrogen peroxide is a very reactive oxygen species and is used as a propellant in rocketry
It is often referred to as water with one more oxygen atom.
It is acidic in nature and it's PH is nearly about 4.5(which is acidic).
It acts as a bleaching agent and is also used as a disinfectant.

Laboratory Methods of Preparation:

When barium peroxide is acidified and the excess water is removed by the process of evaporation, we thus obtain hydrogen peroxide. The following reaction will show the formation of Hydrogen Peroxide:

Equation:

BaO₂.8H₂O(s) + H₂SO₄(aq) → BaSO₄(s) + H₂O₂(aq) + 8H₂O(l)

Now,

When H₂O₂ is treated with aqueous KI it forms:

H₂O₂ and KI undergo a redox reaction, with hydrogen peroxide acting as an oxidizing agent and KI as a reducing agent. In this process, iodine gas is released which oxidised KI.

Equation :

H₂O₂+ 2KI + 2H⁺ → I₂+ 2H₂O + 2K⁺

Thus form the above conclusion we can say that, H₂O₂ acting as an oxidizing agent.

Oxygen containing product formed is H₂O.

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