Which of the following are correct?

Options

A. `As^(5+)` salts are better oxidising agents
B. `Tl^(3+)` salts are better oxidising agents
C. `Ga^(o+)` salts are better oxidising agents
D. `Pb^(4+)` salts are better oxidising agents

Explanation

To determine which of the given salts are better oxidizing agents, we need to analyze the oxidation states and their stability when they gain electrons. Here’s a step-by-step solution:

### Step 1: Analyze each salt
We have four salts to analyze:
1. **As^5+**
2. **Ti^3+**
3. **Ga^+**
4. **Pb^4+**

### Step 2: Evaluate As^5+
- When As^5+ gains 2 electrons, it becomes As^3+.
- As^3+ is less stable compared to As^5+.
- Therefore, As^5+ is **not** a better oxidizing agent.

### Step 3: Evaluate Ti^3+
- When Ti^3+ gains 2 electrons, it becomes Ti^+.
- Ti^+ is more stable than Ti^3+.
- Therefore, Ti^3+ is a better oxidizing agent.

### Step 4: Evaluate Ga^+
- When Ga^+ gains 2 electrons, it becomes Ga^−.
- Ga^− is less stable than Ga^+.
- Therefore, Ga^+ is **not** a better oxidizing agent.

### Step 5: Evaluate Pb^4+
- When Pb^4+ gains 2 electrons, it becomes Pb^2+.
- Pb^2+ is more stable than Pb^4+.
- Therefore, Pb^4+ is a better oxidizing agent.

### Conclusion
From the analysis:
- **As^5+**: Not a better oxidizing agent (Incorrect)
- **Ti^3+**: Better oxidizing agent (Correct)
- **Ga^+**: Not a better oxidizing agent (Incorrect)
- **Pb^4+**: Better oxidizing agent (Correct)

Thus, the correct answers are **Ti^3+** and **Pb^4+**.

### Final Answer
The correct options are **B (Ti^3+)** and **D (Pb^4+)**.

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