Assertion`:-` In a solution having `0.1M` each of `Br^(_)` , `SO_(4)^(2-)` &
`Cl^(-)`, on adding `Ag^(+)` ion slowly. Salt having highest value of `K_(sp)`
will precipitate first.
Reason`:-` Precipitate occurs when `Q_(sp)=K_(sp)``

Options

A. If both Assertion & Reason are True & the Reason is a correct explanation of the Assertion.
B. If both Assertion & Reason are True but Reason is not a correct explanation of the Assertiion.
C. If Assertion is True but the Reason is False.
D. If both Assertion & Reason are False

Explanation

To solve the question, we need to analyze the assertion and reason provided, and determine their validity based on the principles of solubility product (Ksp) and precipitation.

### Step-by-Step Solution:

1. **Understanding the Assertion**:
The assertion states that in a solution with 0.1 M concentrations of \( Br^- \), \( SO_4^{2-} \), and \( Cl^- \), the salt with the highest Ksp will precipitate first when \( Ag^+ \) ions are added.

- **Analysis**: This is incorrect because the salt with the **lowest** Ksp will precipitate first. The reason is that a lower Ksp indicates that the salt is less soluble, meaning it will reach its saturation point (and thus precipitate) at a lower concentration of ions compared to salts with higher Ksp values.

2. **Understanding the Reason**:
The reason states that precipitation occurs when \( Q_{sp} = K_{sp} \).

- **Analysis**: This statement is also false. Precipitation occurs when the ionic product \( Q_{sp} \) exceeds the Ksp, i.e., \( Q_{sp} > K_{sp} \). When \( Q_{sp} = K_{sp} \), the solution is saturated, and no precipitation occurs until \( Q_{sp} exceeds \( K_{sp} \).

3. **Conclusion**:
Both the assertion and the reason are false. Therefore, the correct answer to the question is that both the assertion and the reason are false.

### Final Answer:
Both the assertion and the reason are false.

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