`Pb(AcO)_(2)+H_(2)S to PbS darr+2AcOH`

Options

A. For precipitate formation formation reaction
B. For precipitate dissolution reaction
C. For precipitate exchange reaction
D. For no reaction

Answer

To analyze the reaction \( \text{Pb(AcO)}_2 + \text{H}_2\text{S} \rightarrow \text{PbS} \downarrow + 2\text{AcOH} \), we will break it down step by step.

### Step 1: Identify the Reactants and Products
The reactants in this reaction are:
- Lead(II) acetate, \( \text{Pb(AcO)}_2 \)
- Hydrogen sulfide, \( \text{H}_2\text{S} \)

The products formed are:
- Lead(II) sulfide, \( \text{PbS} \) (which is a precipitate)
- Acetic acid, \( \text{AcOH} \) (or \( \text{CH}_3\text{COOH} \))

### Step 2: Determine the Type of Reaction
This reaction involves the formation of a solid product (precipitate) from two aqueous solutions. Specifically, lead(II) sulfide \( \text{PbS} \) is formed as a precipitate, which indicates that a reaction has occurred.

### Step 3: Analyze the Formation of Precipitate
In this reaction, when lead(II) acetate reacts with hydrogen sulfide, lead(II) sulfide precipitates out of the solution. The downward arrow \( \downarrow \) next to \( \text{PbS} \) signifies that it is a solid precipitate.

### Step 4: Conclusion
Since a solid precipitate is formed from the reaction of two soluble reactants, we classify this reaction as a **precipitate formation reaction**.

### Final Answer
The reaction \( \text{Pb(AcO)}_2 + \text{H}_2\text{S} \rightarrow \text{PbS} \downarrow + 2\text{AcOH} \) is a **precipitate formation reaction**.

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