`H_5IO_6` is a

Options

A. Strong reducing agent
B. Strong base
C. Strong oxidizing agent
D. Weak base

Explanation

To determine the nature of the compound \( H_5IO_6 \), we need to analyze its oxidation state and properties. Here’s a step-by-step solution:

### Step 1: Determine the oxidation state of iodine in \( H_5IO_6 \)

1. **Assign oxidation states**:
- Hydrogen (H) has an oxidation state of +1.
- Oxygen (O) has an oxidation state of -2.

2. **Set up the equation**:
- The compound has 5 hydrogen atoms and 6 oxygen atoms.
- Let the oxidation state of iodine (I) be \( x \).
- The overall charge of the compound is neutral (0).

The equation can be set up as follows:
\[ 5(+1) + x + 6(-2) = 0 \]

### Step 2: Solve the equation

1. **Calculate the contributions**:
- Contribution from hydrogen: \( 5 \times +1 = +5 \)
- Contribution from oxygen: \( 6 \times -2 = -12 \)

2. **Substitute into the equation**:
\[ 5 + x - 12 = 0 \]

3. **Rearrange to find \( x \)**:
\[ x - 7 = 0 \implies x = +7 \]

### Step 3: Analyze the oxidation state

1. **Identify the oxidation state of iodine**:
- The oxidation state of iodine in \( H_5IO_6 \) is +7.

2. **Determine the implications of this oxidation state**:
- Iodine in the +7 oxidation state is its highest oxidation state.
- Compounds with iodine in this state are typically strong oxidizing agents because they can easily gain electrons and be reduced to a lower oxidation state.

### Conclusion

Based on the analysis, \( H_5IO_6 \) is identified as a strong oxidizing agent due to the presence of iodine in its highest oxidation state (+7).