Which of the following is the strongest acid?

Options

A. `CIO_(3)(OH)`
B. `CIO_(2)(OH)`
C. `SO(OH)_(2)`
D. `SO_(2)(OH)_(2)`

Explanation

To determine which of the given acids is the strongest, we can analyze the oxidation states of the central atoms in each acid. The general principle is that as the oxidation state of the central atom increases, the acidic strength also increases.

### Step-by-step Solution:

1. **Identify the Acids**: The acids we need to analyze are:
- HClO4 (Perchloric acid)
- HClO3 (Chloric acid)
- H2SO3 (Sulfurous acid)
- H2SO4 (Sulfuric acid)

2. **Calculate Oxidation State for HClO4**:
- Let the oxidation state of Cl be \( x \).
- The equation is: \( 1 + x + 4(-2) = 0 \)
- Simplifying: \( 1 + x - 8 = 0 \) → \( x = +7 \)
- Thus, the oxidation state of Cl in HClO4 is +7.

3. **Calculate Oxidation State for HClO3**:
- Let the oxidation state of Cl be \( x \).
- The equation is: \( 1 + x + 3(-2) = 0 \)
- Simplifying: \( 1 + x - 6 = 0 \) → \( x = +5 \)
- Thus, the oxidation state of Cl in HClO3 is +5.

4. **Calculate Oxidation State for H2SO3**:
- Let the oxidation state of S be \( x \).
- The equation is: \( 2 + x + 3(-2) = 0 \)
- Simplifying: \( 2 + x - 6 = 0 \) → \( x = +4 \)
- Thus, the oxidation state of S in H2SO3 is +4.

5. **Calculate Oxidation State for H2SO4**:
- Let the oxidation state of S be \( x \).
- The equation is: \( 2 + x + 4(-2) = 0 \)
- Simplifying: \( 2 + x - 8 = 0 \) → \( x = +6 \)
- Thus, the oxidation state of S in H2SO4 is +6.

6. **Compare Oxidation States**:
- HClO4: +7
- HClO3: +5
- H2SO3: +4
- H2SO4: +6

7. **Conclusion**: The highest oxidation state is +7 in HClO4, indicating that HClO4 is the strongest acid among the given options.

### Final Answer:
The strongest acid is **HClO4** (option A).