`PbCl_(2)darr+H_(2)SO_(4)hArr PbSO_(4)darr+2HCL`

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 given reaction \( \text{PbCl}_2 + \text{H}_2\text{SO}_4 \rightleftharpoons \text{PbSO}_4 + 2\text{HCl} \), we will determine the type of reaction it represents.

### Step-by-Step Solution:

1. **Identify the Reactants and Products:**
- The reactants are lead(II) chloride (\( \text{PbCl}_2 \)) and sulfuric acid (\( \text{H}_2\text{SO}_4 \)).
- The products are lead(II) sulfate (\( \text{PbSO}_4 \)) and hydrochloric acid (\( \text{HCl} \)).

2. **Determine the State of the Compounds:**
- Both \( \text{PbCl}_2 \) and \( \text{PbSO}_4 \) are precipitates, indicated by the downward arrows in the reaction.
- \( \text{HCl} \) is typically in aqueous form in this context.

3. **Analyze the Reaction Type:**
- A precipitate formation reaction occurs when a solid forms from a solution.
- A precipitate dissolution reaction occurs when a solid dissolves in a solution.
- A precipitate exchange reaction occurs when two precipitates exchange ions to form new precipitates.
- No reaction would imply that no change occurs.

4. **Evaluate the Presence of Precipitates:**
- Since both \( \text{PbCl}_2 \) and \( \text{PbSO}_4 \) are precipitates, we have precipitates on both sides of the reaction.
- This indicates that there is an exchange of ions between the reactants, leading to the formation of new precipitates.

5. **Conclude the Type of Reaction:**
- Given that both reactants and products contain precipitates, this reaction is classified as a **precipitate exchange reaction**.

### Final Answer:
The reaction \( \text{PbCl}_2 + \text{H}_2\text{SO}_4 \rightleftharpoons \text{PbSO}_4 + 2\text{HCl} \) is a **precipitate exchange reaction**.

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