Iodine reacts with concentrateed `HNO_3` to yield Y along with other products. The oxidation state of iodine in Y, is _______.

Explanation

To determine the oxidation state of iodine in the compound Y formed when iodine reacts with concentrated HNO3, we can follow these steps:

### Step 1: Write the Reaction
Iodine (I2) reacts with concentrated nitric acid (HNO3) to form iodic acid (HIO3) along with other products such as nitrogen dioxide (NO2) and water (H2O). The balanced chemical reaction is:

\[ 2 I_2 + 10 HNO_3 \rightarrow 6 HIO_3 + 10 NO_2 + 4 H_2O \]

### Step 2: Identify the Compound Y
From the balanced reaction, we can see that the compound Y is HIO3 (iodic acid).

### Step 3: Assign Oxidation States
Now, we need to determine the oxidation state of iodine in HIO3.

1. **Assign oxidation states for other elements:**
- Hydrogen (H) is typically +1.
- Oxygen (O) is typically -2.

2. **Set up the equation for the oxidation state of iodine (let's denote it as Z):**
The overall charge of the molecule must equal zero since HIO3 is neutral. Therefore, we can write:

\[ (+1) + Z + 3(-2) = 0 \]

### Step 4: Solve for Z
Now, substituting the values into the equation:

\[ 1 + Z - 6 = 0 \]

\[ Z - 5 = 0 \]

\[ Z = +5 \]

### Conclusion
Thus, the oxidation state of iodine in Y (HIO3) is +5.

### Final Answer
The oxidation state of iodine in Y is **+5**.

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