The oxidation state of chromium in the final product formed by the reaction between Kl and acidified potassium dichromate solution is `:`

Options

A. `+3`
B. `+2`
C. `+6`
D. `+4`

Explanation

To determine the oxidation state of chromium in the final product formed by the reaction between potassium iodide (KI) and acidified potassium dichromate (K2Cr2O7), we can follow these steps:

### Step 1: Identify the Reactants
The reactants in this reaction are potassium iodide (KI) and acidified potassium dichromate (K2Cr2O7).

### Step 2: Determine the Oxidation States of Reactants
In potassium iodide (KI), potassium (K) has an oxidation state of +1 and iodine (I) has an oxidation state of -1. In potassium dichromate (K2Cr2O7), potassium (K) has an oxidation state of +1, oxygen (O) has an oxidation state of -2, and we need to find the oxidation state of chromium (Cr).

### Step 3: Calculate the Oxidation State of Chromium in K2Cr2O7
Using the formula for the oxidation state:
\[ \text{Oxidation state of Cr} + 2(+1) + 7(-2) = 0 \]
Let the oxidation state of Cr be \( x \):
\[ x + 2 - 14 = 0 \implies x - 12 = 0 \implies x = +6 \]
Thus, the oxidation state of chromium in K2Cr2O7 is +6.

### Step 4: Identify the Reaction
In the presence of an acid (H+), potassium dichromate acts as an oxidizing agent and oxidizes the iodide ions (I-) from KI. The iodide ions (I-) are oxidized to iodine (I2), while the chromium is reduced.

### Step 5: Write the Balanced Reaction
The balanced reaction can be represented as:
\[ Cr_2O_7^{2-} + 14H^+ + 6I^- \rightarrow 2Cr^{3+} + 7H_2O + 3I_2 \]
In this reaction, the Cr2O7^2- ion is reduced to Cr^3+.

### Step 6: Determine the Oxidation State of Chromium in the Product
From the balanced reaction, we see that chromium (Cr) is reduced to Cr^3+. Therefore, the oxidation state of chromium in the final product is +3.

### Final Answer
The oxidation state of chromium in the final product formed by the reaction between KI and acidified potassium dichromate solution is **+3**.

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