Aqueous solution of `BaBr_(2)` , gives yellow ppt with

Options

A. `K_(2)CrO_(4)`
B. `AgNO_(3)`
C. both
D. none

Answer

To solve the question, we need to analyze the reactions of barium bromide (BaBr₂) with the given reagents: potassium chromate (K₂CrO₄) and silver nitrate (AgNO₃).

### Step-by-Step Solution:

1. **Identify the Reactants**: We have barium bromide (BaBr₂) and two possible reagents: potassium chromate (K₂CrO₄) and silver nitrate (AgNO₃).

2. **Reaction with Potassium Chromate (K₂CrO₄)**:
- When BaBr₂ reacts with K₂CrO₄, the reaction can be written as:
\[ \text{BaBr}_2 (aq) + \text{K}_2\text{CrO}_4 (aq) \rightarrow \text{BaCrO}_4 (s) + 2\text{KBr} (aq) \]
- In this reaction, barium chromate (BaCrO₄) is formed, which is a yellow precipitate.

3. **Reaction with Silver Nitrate (AgNO₃)**:
- When BaBr₂ reacts with AgNO₃, the reaction can be written as:
\[ \text{BaBr}_2 (aq) + 2\text{AgNO}_3 (aq) \rightarrow \text{Ba(NO}_3)_2 (aq) + 2\text{AgBr} (s) \]
- In this case, silver bromide (AgBr) is formed, which is also a yellow precipitate.

4. **Conclusion**:
- Since BaBr₂ gives a yellow precipitate with both K₂CrO₄ (BaCrO₄) and AgNO₃ (AgBr), the answer to the question is that BaBr₂ gives a yellow precipitate with both reagents.

5. **Final Answer**: The correct option is **both (C)**.