Among the following, the correct order of acidity is:

Options

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

Explanation

To determine the correct order of acidity among the given oxoacids, we need to analyze the structure and oxidation states of the central atom (chlorine in this case) in each oxoacid. The acidity of oxoacids generally increases with the oxidation state of the central atom and the number of oxygen atoms bonded to it.

### Step-by-Step Solution:

1. **Identify the Oxoacids**:
We are considering the following oxoacids of chlorine:
- HClO4 (Perchloric acid)
- HClO3 (Chloric acid)
- HClO2 (Chlorous acid)
- HClO (Hypochlorous acid)

2. **Determine the Oxidation States**:
- For HClO4:
- Chlorine (Cl) has an oxidation state of +7.
- For HClO3:
- Chlorine (Cl) has an oxidation state of +5.
- For HClO2:
- Chlorine (Cl) has an oxidation state of +3.
- For HClO:
- Chlorine (Cl) has an oxidation state of +1.

3. **Analyze the Structure**:
- HClO4 has three double bonds with oxygen and one hydroxyl group (OH), allowing for significant resonance stabilization and a strong tendency to release H+.
- HClO3 has two double bonds with oxygen and one hydroxyl group, which also allows for resonance but to a lesser extent than HClO4.
- HClO2 has one double bond with oxygen and one hydroxyl group, which means less resonance stabilization compared to HClO3.
- HClO has no double bonds with oxygen, making it the least acidic as it lacks the ability to stabilize the release of H+.

4. **Establish the Order of Acidity**:
The acidity increases with the oxidation state and the number of oxygen atoms. Therefore, the order of acidity is:
- HClO4 > HClO3 > HClO2 > HClO

### Final Answer:
The correct order of acidity is: **HClO4 > HClO3 > HClO2 > HClO**.