Which of the following is the strongest oxidising agent ?

Options

A. HOCl
B. `HClO_(2)`
C. `HClO_(3)`
D. `HClO_(4)`

Explanation

To determine the strongest oxidizing agent from the given options, we can follow these steps:

### Step 1: Understand the Concept of Oxidizing Agents
An oxidizing agent is a substance that facilitates the oxidation of another substance while being reduced itself. This means that it gains electrons and its oxidation state decreases.

### Step 2: Identify the Compounds
Let's assume the options provided are:
1. HOCl
2. HClO2
3. HClO3
4. HClO4

### Step 3: Calculate the Oxidation States
We will calculate the oxidation state of chlorine (Cl) in each compound to determine which one has the highest potential to be reduced (thus acting as the strongest oxidizing agent).

1. **For HOCl:**
- H = +1
- O = -2
- Let the oxidation state of Cl be X.
- The equation becomes: +1 + X - 2 = 0
- Solving gives: X = +1

2. **For HClO2:**
- H = +1
- O = -2 (two O atoms contribute -4)
- Let the oxidation state of Cl be Y.
- The equation becomes: +1 + Y - 4 = 0
- Solving gives: Y = +3

3. **For HClO3:**
- H = +1
- O = -2 (three O atoms contribute -6)
- Let the oxidation state of Cl be Z.
- The equation becomes: +1 + Z - 6 = 0
- Solving gives: Z = +5

4. **For HClO4:**
- H = +1
- O = -2 (four O atoms contribute -8)
- Let the oxidation state of Cl be W.
- The equation becomes: +1 + W - 8 = 0
- Solving gives: W = +7

### Step 4: Compare the Oxidation States
Now we have the oxidation states of Cl in each compound:
- HOCl: +1
- HClO2: +3
- HClO3: +5
- HClO4: +7

### Step 5: Determine the Strongest Oxidizing Agent
The strongest oxidizing agent will be the one with the lowest oxidation state of chlorine because it has a higher tendency to gain electrons (be reduced).

From our calculations:
- HOCl has Cl in the +1 oxidation state, which is the lowest among the given options.

### Conclusion
Thus, **HOCl** is the strongest oxidizing agent among the options provided.

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