Why HCl not used to make the mdeium acidic in oxidation reactions of `KMnO_(4)` in acidic medium ?

Options

A. Both HCl and `KMnO_(4)` act as oxidising agents
B. `KMnO_(4)` oxidises HCl into `Cl_(2)` which is also an oxidising agent
C. `KMnO_(4)` is a weaker oxidising agents than HCl
D. `KMnO_(4)` acts as a reducing agent in the presence of HCl

Explanation

To answer the question of why HCl is not used to make the medium acidic in oxidation reactions of KMnO4 in acidic medium, we can follow these steps:

### Step-by-Step Solution:

1. **Understanding KMnO4**:
- KMnO4, or potassium permanganate, is a strong oxidizing agent. In oxidation reactions, it acts to oxidize other substances while itself being reduced.

2. **Role of HCl in Reactions**:
- Hydrochloric acid (HCl) is a strong acid that can provide protons (H⁺ ions) to make a solution acidic. However, it also contains chloride ions (Cl⁻).

3. **Reaction Between KMnO4 and HCl**:
- When KMnO4 is added to an acidic medium created by HCl, a reaction occurs where KMnO4 oxidizes the chloride ions (Cl⁻) present in HCl. This oxidation results in the formation of chlorine gas (Cl2).

4. **Oxidation of Chloride Ions**:
- The oxidation of Cl⁻ to Cl2 indicates that HCl is being oxidized in the presence of KMnO4. This means that instead of solely using KMnO4 as the oxidizing agent, HCl is also participating in the reaction.

5. **Consequences of Using HCl**:
- Since Cl2 is also an oxidizing agent, it can interfere with the intended oxidation reactions that KMnO4 is supposed to carry out. This dual role complicates the reaction mechanism and can lead to unintended results.

6. **Conclusion**:
- Therefore, HCl is not used to make the medium acidic in oxidation reactions of KMnO4 because it gets oxidized by KMnO4, producing Cl2, which can act as an additional oxidizing agent, thereby complicating the reaction.

### Final Answer:
HCl is not used to make the medium acidic in oxidation reactions of KMnO4 because KMnO4 oxidizes HCl to form Cl2, which is also an oxidizing agent, thus interfering with the intended oxidation process.

---