`FeCL_(3)+KI to Fe^(2+)(aq.)+KI_(3)`

Options

A. For coloured ppt./Black ppt
B. For coloured solution.
C. for clear/colourless solution
D. For white ppt.

Answer

To solve the given reaction \( \text{FeCl}_3 + \text{KI} \rightarrow \text{Fe}^{2+} (aq) + \text{KI}_3 \), we will analyze the reactants and products to determine the characteristics of the resulting solution.

### Step-by-Step Solution:

1. **Identify the Reactants**: The reactants in this reaction are iron(III) chloride (\( \text{FeCl}_3 \)) and potassium iodide (\( \text{KI} \)).

2. **Write the Balanced Equation**: The reaction can be written as:
\[ \text{FeCl}_3 + 3 \text{KI} \rightarrow \text{Fe}^{2+} + 3 \text{KCl} + \text{I}_2 \]
However, the question states the products as \( \text{Fe}^{2+} (aq) + \text{KI}_3 \). This indicates that the iodide ions are reacting with iron(III) ions, leading to the formation of \( \text{Fe}^{2+} \) and \( \text{KI}_3 \).

3. **Determine the State of Products**:
- \( \text{Fe}^{2+} \) is in aqueous form, which means it is dissolved in water.
- \( \text{KI}_3 \) is also soluble in water.

4. **Analyze the Color of the Products**:
- The \( \text{Fe}^{2+} \) ion in aqueous solution is known to impart a green color.
- Since both products are in aqueous form and do not precipitate, we conclude that the solution will be colored.

5. **Eliminate Options**:
- Since a precipitate is not formed, options indicating a precipitate (like colored or black ppt, or white precipitate) can be eliminated.
- The remaining options are either colored solution or colorless solution.

6. **Final Conclusion**: Given that \( \text{Fe}^{2+} \) is green in color, the resulting solution will be a colored solution.

### Final Answer:
The reaction \( \text{FeCl}_3 + \text{KI} \) produces a colored solution due to the presence of \( \text{Fe}^{2+} \) ions.