`PbO_(2)↓+HNO_(3)("Conc.") to Pb(NO_(3))_(2)+H_(2)O+[O]`

Options

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

Answer

To solve the reaction \( \text{PbO}_2 + \text{HNO}_3 \text{(Conc.)} \rightarrow \text{Pb(NO}_3)_2 + \text{H}_2\text{O} + [\text{O}] \), we will break it down step by step.

### Step 1: Identify the Reactants and Products
- **Reactants**: Lead(IV) oxide (\( \text{PbO}_2 \)) and concentrated nitric acid (\( \text{HNO}_3 \)).
- **Products**: Lead(II) nitrate (\( \text{Pb(NO}_3)_2 \)), water (\( \text{H}_2\text{O} \)), and oxygen (\([O]\)).

### Step 2: Analyze the Reaction Type
This reaction involves the conversion of a solid precipitate (\( \text{PbO}_2 \)) into soluble lead(II) nitrate, along with the release of water and oxygen.

### Step 3: Determine the Nature of the Reaction
Since \( \text{PbO}_2 \) is a precipitate that dissolves in concentrated nitric acid to form a soluble product (\( \text{Pb(NO}_3)_2 \)), this reaction can be classified as a **precipitate dissolution reaction**.

### Step 4: Write the Balanced Equation
The balanced equation for the reaction is:
\[ \text{PbO}_2 + 4 \text{HNO}_3 \rightarrow \text{Pb(NO}_3)_2 + 2 \text{H}_2\text{O} + [O] \]
Here, we ensure that the number of atoms for each element is balanced on both sides of the equation.

### Step 5: Conclusion
The correct classification of the reaction is **precipitate dissolution reaction** since the lead oxide precipitate is dissolved in nitric acid to form lead nitrate.