Match List I with List II

Choose the correct answer from the options given below:

A-III, B-II, C-I, D-IV

The correct answer is option 3. A-III, B-II, C-I, D-IV.

Let us go through each of the acids mentioned in List I and understand their corresponding chemical formulas and the reasoning behind them.

A. Chloric Acid: III. \( \text{HClO}_3 \)

Formula: \( \text{HClO}_3 \)

Chloric acid is an oxoacid of chlorine where chlorine is in the +5 oxidation state. The general formula for oxoacids of chlorine follows \( \text{HClO}_n \) where \( n \) represents the number of oxygen atoms. In chloric acid, there are three oxygen atoms attached to chlorine, hence the formula is \( \text{HClO}_3 \).

B. Chlorous Acid : II. \( \text{HClO}_2 \)

Formula: \( \text{HClO}_2 \)

Chlorous acid is another oxoacid of chlorine, but here chlorine is in the +3 oxidation state. This acid contains two oxygen atoms attached to chlorine. Therefore, the correct formula for chlorous acid is \( \text{HClO}_2 \).

C. Hypochlorous Acid : I. \( \text{HOCl} \)

Formula: \( \text{HOCl} \)

Hypochlorous acid is the simplest oxoacid of chlorine, where chlorine is in the +1 oxidation state. It has only one oxygen atom attached to the chlorine, making its formula \( \text{HOCl} \).

D. Perchloric Acid: IV. \( \text{HClO}_4 \)

Formula: \( \text{HClO}_4 \)

Perchloric acid is the strongest oxoacid of chlorine, with chlorine in the +7 oxidation state. It has four oxygen atoms attached to the chlorine atom. Thus, the formula for perchloric acid is \( \text{HClO}_4 \)

Additional Notes on Oxoacids of Chlorine:

Hypochlorous Acid (\( \text{HOCl} \)): Chlorine is in the +1 oxidation state. It's a weak acid and is often used as a disinfectant.

Chlorous Acid (\( \text{HClO}_2 \)): Chlorine is in the +3 oxidation state. It's less common and less stable than the other oxoacids.

Chloric Acid (\( \text{HClO}_3 \)): Chlorine is in the +5 oxidation state. It's a strong acid and a powerful oxidizing agent.

Perchloric Acid (\( \text{HClO}_4 \)): Chlorine is in the +7 oxidation state. It's the strongest acid among the oxoacids of chlorine and is highly reactive, especially as an oxidizing agent.