Of the given anions, the strongest base is

Options

A. `ClO^(-)`
B. `ClO_(2)^(-)`
C. `ClO_(3)^(-)`
D. `ClO_(4)^(-)`

Explanation

To determine the strongest base among the given anions, we need to analyze the conjugate acids of each anion and their respective oxidation states. Here’s a step-by-step solution:

### Step 1: Understand the Concept of Bases
Bases are substances that can accept protons (H⁺ ions). According to the Brønsted-Lowry theory, a stronger base corresponds to a weaker conjugate acid.

### Step 2: Identify the Given Anions
The anions provided are:
1. ClO⁻ (Hypochlorite)
2. ClO₂⁻ (Chlorite)
3. ClO₃⁻ (Chlorate)
4. ClO₄⁻ (Perchlorate)

### Step 3: Determine the Conjugate Acids
For each anion, we can find the conjugate acid by adding a proton (H⁺):
1. ClO⁻ → HClO (Hypochlorous acid)
2. ClO₂⁻ → HClO₂ (Chlorous acid)
3. ClO₃⁻ → HClO₃ (Chloric acid)
4. ClO₄⁻ → HClO₄ (Perchloric acid)

### Step 4: Calculate the Oxidation State of Chlorine in Each Conjugate Acid
To determine the strength of the conjugate acids, we calculate the oxidation state of chlorine in each:
1. **HClO**:
- 1 (H) + x (Cl) + 1(-2)(O) = 0
- 1 + x - 2 = 0 → x = +1
2. **HClO₂**:
- 1 (H) + x (Cl) + 2(-2)(O) = 0
- 1 + x - 4 = 0 → x = +3
3. **HClO₃**:
- 1 (H) + x (Cl) + 3(-2)(O) = 0
- 1 + x - 6 = 0 → x = +5
4. **HClO₄**:
- 1 (H) + x (Cl) + 4(-2)(O) = 0
- 1 + x - 8 = 0 → x = +7

### Step 5: Analyze the Acidity Based on Oxidation States
The higher the oxidation state of chlorine, the stronger the acid:
- HClO₄ (Cl +7) > HClO₃ (Cl +5) > HClO₂ (Cl +3) > HClO (Cl +1)

### Step 6: Determine the Strength of the Bases
Since stronger acids have weaker conjugate bases, we can conclude:
- ClO⁻ (from HClO) is the strongest base.
- ClO₂⁻ (from HClO₂) is weaker than ClO⁻.
- ClO₃⁻ (from HClO₃) is weaker than ClO₂⁻.
- ClO₄⁻ (from HClO₄) is the weakest base.

### Conclusion
Thus, the strongest base among the given anions is **ClO⁻**.