`(NH_(4))_(2)SO_(4)+Ba(OH)_(2) to BaSO_(4)darr+2NH_(3)uarr`

Options

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

Answer

To determine the nature of the products formed in the reaction between ammonium sulfate \((NH_4)_2SO_4\) and barium hydroxide \(Ba(OH)_2\), we can analyze the reaction step by step.

### Step 1: Write the balanced chemical equation
The reaction is given as:
\[ (NH_4)_2SO_4 + Ba(OH)_2 \rightarrow BaSO_4 + 2NH_3 \]

### Step 2: Identify the products
From the equation, we can see that the products formed are:
- Barium sulfate \((BaSO_4)\)
- Ammonia gas \((NH_3)\)

### Step 3: Analyze the nature of the products
1. **Barium sulfate \((BaSO_4)\)**:
- It is known that barium sulfate is insoluble in water and forms a precipitate.
- The color of barium sulfate is white.

2. **Ammonia \((NH_3)\)**:
- Ammonia is a gas, and in this reaction, it is released as a product.

### Step 4: Determine the overall nature of the reaction
- Since barium sulfate is a white precipitate and ammonia is released as a gas, we can conclude that the reaction produces a solid precipitate and a gaseous product.

### Conclusion
Based on the analysis, the reaction will form a **white precipitate** of barium sulfate and ammonia gas. Therefore, the answer is that the reaction produces a **white precipitate**.

### Final Answer
The reaction will form a **white precipitate**.

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