The Question is from neet-chemistry , and it was created by the author Mr. S M HUSSAIN

Question

A mixture of $H_2O_2$ and $KI$ liberates iodine. In this reaction, $H_2O_2$ acts as:

Mr. S M HUSSAIN · Accepted Answer

## CORE INFORMATION
✓ **Answer**: A
## CONCEPT FRAMEWORK
 **Primary Concept**: Redox reactions and identification of oxidizing and reducing agents
 **Related Topics**: Hydrogen peroxide reactions, iodine liberation
 **Prerequisites**: Understanding of oxidation states, oxidation and reduction processes
## SOLUTION PATHWAY
**Given Information**:
  The reaction between $H_2O_2$ and $KI$ produces iodine ($I_2$).
  We need to determine the role of $H_2O_2$ in this reaction.
**Method & Steps**:
 1. Write the balanced chemical equation for the reaction between $H_2O_2$ and $KI$.
  The reaction is:
  $H_2O_2 + 2KI + 2H^+ ightarrow I_2 + 2H_2O + 2K^+$
 2. Analyze the oxidation states of the elements involved.
  In $H_2O_2$, the oxidation state of oxygen is -1.  In $I_2$, the oxidation state of iodine is 0. In $KI$, the oxidation state of iodine is -1.
 3. Determine whether $H_2O_2$ is oxidized or reduced.
  The oxidation state of oxygen in $H_2O_2$ decreases from -1 to -2 in $H_2O$. This is a reduction.
  The oxidation state of iodine in $KI$ increases from -1 to 0 in $I_2$. This is an oxidation.
  Since $H_2O_2$ causes the oxidation of $I^-$, $H_2O_2$ acts as an oxidizing agent.
 4.  Confirm the role of $H_2O_2$.
  $H_2O_2$ is reduced, meaning it gains electrons.  A substance that gains electrons is an oxidizing agent (it oxidizes another substance).
  Result: $H_2O_2$ acts as an oxidizing agent.
  Verification: The balanced equation shows $H_2O_2$ is reduced while $KI$ is oxidized, confirming its role as an oxidizing agent.
 ## OPTION ANALYSIS
A ✓:  $H_2O_2$ is reduced in the reaction, meaning it accepts electrons from iodide ions ($I^-$), thus oxidizing them to iodine ($I_2$).  This is the definition of an oxidizing agent.
B :x: $H_2O_2$ is not a reducing agent in this reaction because it gains electrons itself.
C :x: $H_2O_2$ is a reactant, not a catalyst. A catalyst is not consumed in the reaction.
D :x: While $H_2O_2$ can be acidic, its primary role in this specific reaction is as an oxidizing agent.
 ## LEARNING AIDS
 **Common Mistakes**:
  1.Confusing oxidizing and reducing agents: Remember OIL RIG (Oxidation Is Loss, Reduction Is Gain) of electrons.  An oxidizing agent gains electrons and is reduced; a reducing agent loses electrons and is oxidized.
  2.Ignoring the balanced chemical equation: The balanced equation provides crucial information about changes in oxidation states and thus the role of each reactant.
 **Quick Tips**:
  1.Always determine the oxidation states of elements before deciding on whether a substance acts as an oxidizing or reducing agent.
  2.Remember that an oxidizing agent is reduced and a reducing agent is oxidized.

Mr. S M HUSSAIN · Answer

The correct Option is "An oxidizing agent"

Mr. S M HUSSAIN · Answer

A reducing agent

Mr. S M HUSSAIN · Answer

A catalyst

Mr. S M HUSSAIN · Answer

An acid

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