`PbO_(2)` is:

Options

A. acidic
B. basic
C. reducing agent
D. oxidising agent

Answer

To determine the properties of `PbO2` (lead(IV) oxide), we will analyze its acidic, basic, and oxidizing/reducing characteristics step by step.

### Step 1: Determine if `PbO2` is Acidic
An oxide is considered acidic if it reacts with a base to produce salt and water.

**Reaction:**
When `PbO2` reacts with sodium hydroxide (NaOH), it forms sodium plumbate (Na2PbO3) and water.

**Balanced Reaction:**
\[ \text{PbO}_2 + 2 \text{NaOH} \rightarrow \text{Na}_2\text{PbO}_3 + 2 \text{H}_2\text{O} \]

**Conclusion:**
Since `PbO2` reacts with a base to form a salt and water, it is acidic in nature.

### Step 2: Determine if `PbO2` is Basic
An oxide is considered basic if it reacts with an acid to produce salt and water.

**Reaction:**
When `PbO2` reacts with hydrochloric acid (HCl), it forms lead(IV) chloride (PbCl4) and water.

**Balanced Reaction:**
\[ \text{PbO}_2 + 4 \text{HCl} \rightarrow \text{PbCl}_4 + 2 \text{H}_2\text{O} \]

**Conclusion:**
Since `PbO2` reacts with an acid to form a salt and water, it is also basic in nature.

### Step 3: Determine if `PbO2` is an Oxidizing or Reducing Agent
To determine if `PbO2` acts as an oxidizing or reducing agent, we need to analyze the oxidation states.

In `PbO2`, the oxidation state of lead (Pb) is +4 (because oxygen is -2, and there are two oxygen atoms).

**Conclusion:**
Since lead in `PbO2` has a higher oxidation state compared to its more stable +2 oxidation state, `PbO2` can act as an oxidizing agent. It can gain electrons and thus is reduced.

### Final Conclusion
- `PbO2` is **acidic** (reacts with bases).
- `PbO2` is **basic** (reacts with acids).
- `PbO2` is an **oxidizing agent** (can gain electrons).