Consider the following list of reagent
`"Acidified" K_(2)Cr_(2)O_(7), "alkaline" KMnO_(4), CuSO_(4), H_(2)O_(2), Cl_(2) ,O_(3),FeCl_(3),HNO_(3) and Na_(2)S_(2)O_(3)`
The total number of reagents that can oxidise aqueous iodide iodine is

Explanation

To determine the total number of reagents from the provided list that can oxidize aqueous iodide ions (I⁻) to iodine (I₂), we will analyze each reagent one by one.

### Step-by-Step Solution:

1. **Identify the Reagents:**
The reagents listed are:
- Acidified K₂Cr₂O₇
- Alkaline KMnO₄
- CuSO₄
- H₂O₂
- Cl₂
- O₃
- FeCl₃
- HNO₃
- Na₂S₂O₃

2. **Analyze Each Reagent:**

- **Acidified K₂Cr₂O₇:**
- Reaction: K₂Cr₂O₇ + 7H₂SO₄ + 6KI → 2Cr₂(SO₄)₃ + 3I₂ + 7H₂O
- Oxidation occurs (I⁻ to I₂). **Can oxidize.**

- **Alkaline KMnO₄:**
- Reaction: 2KMnO₄ + 6KI + 4H₂O → 2KIO₃ + 2MnO₂ + 6KOH
- Oxidation occurs (I⁻ to I₂). **Can oxidize.**

- **CuSO₄:**
- Reaction: CuSO₄ + 2KI → Cu₂I₂ + I₂ + 2K₂SO₄
- Oxidation occurs (I⁻ to I₂). **Can oxidize.**

- **H₂O₂:**
- Reaction: 2KI + H₂O₂ → 2KOH + I₂
- Oxidation occurs (I⁻ to I₂). **Can oxidize.**

- **Cl₂:**
- Reaction: 2KI + Cl₂ → 2KCl + I₂
- Oxidation occurs (I⁻ to I₂). **Can oxidize.**

- **O₃:**
- Reaction: 2KI + O₃ + H₂O → 2KOH + I₂ + O₂
- Oxidation occurs (I⁻ to I₂). **Can oxidize.**

- **FeCl₃:**
- Reaction: 2FeCl₃ + 2KI → 2FeCl₂ + I₂ + 2KCl
- Oxidation occurs (I⁻ to I₂). **Can oxidize.**

- **HNO₃:**
- Reaction: 8HNO₃ + 6KI → 6KNO₃ + 2NO + 4H₂O + 3I₂
- Oxidation occurs (I⁻ to I₂). **Can oxidize.**

- **Na₂S₂O₃:**
- Reaction: Na₂S₂O₃ + KI → No reaction
- No oxidation occurs. **Cannot oxidize.**

3. **Count the Oxidizing Reagents:**
From the analysis, the reagents that can oxidize aqueous iodide ions are:
- Acidified K₂Cr₂O₇
- Alkaline KMnO₄
- CuSO₄
- H₂O₂
- Cl₂
- O₃
- FeCl₃
- HNO₃

Total: 8 reagents can oxidize aqueous iodide ions.

### Final Answer:
The total number of reagents that can oxidize aqueous iodide ions is **8**.

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