The strongest Bronsted base in the following anion is

Options

A. `CIO^(Theta)`
B. `CIO_(2)^(Theta)`
C. `CIO_(3)^(Theta)`
D. `CIO_(4)^(Theta)`

Explanation

To determine the strongest Bronsted base among the given anions (ClO⁻, ClO₂⁻, ClO₃⁻, ClO₄⁻), we can follow these steps:

### Step 1: Understand the relationship between acids and their conjugate bases
The strength of a Bronsted base is inversely related to the strength of its conjugate acid. This means that the stronger the acid, the weaker its conjugate base will be.

### Step 2: Identify the acids corresponding to the given anions
The anions provided are conjugate bases of the following acids:
- ClO⁻ is the conjugate base of HClO (hypochlorous acid)
- ClO₂⁻ is the conjugate base of HClO₂ (chlorous acid)
- ClO₃⁻ is the conjugate base of HClO₃ (chloric acid)
- ClO₄⁻ is the conjugate base of HClO₄ (perchloric acid)

### Step 3: Determine the strength of the acids
The strength of these acids can be compared based on the oxidation state of chlorine in each acid. The higher the oxidation state of chlorine, the stronger the acid. The oxidation states are as follows:
- HClO: +1
- HClO₂: +3
- HClO₃: +5
- HClO₄: +7

From this, we can conclude:
- HClO is the weakest acid (lowest oxidation state)
- HClO₄ is the strongest acid (highest oxidation state)

### Step 4: Relate the strength of the acids to their conjugate bases
Since HClO is the weakest acid, its conjugate base ClO⁻ will be the strongest base. Conversely, HClO₄, being the strongest acid, will have the weakest conjugate base ClO₄⁻.

### Step 5: Conclusion
Thus, the strongest Bronsted base among the given anions is ClO⁻.

### Final Answer:
The strongest Bronsted base in the following anion is ClO⁻.

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