`2Al + 6HCl to 2Al^(3+) + 6Cl^- + 3H_2`
`2Al + 2NaOH + 6H_2 O to 2Na(OH)_4] + 3H_2`
These reactions suggest that aluminium is

Options

A. acidic in nature
B. Basic in nature
C. Amphoteric in nature
D. Neutral in nature

Answer

To determine the nature of aluminum based on the given reactions, we will analyze each reaction step by step.

### Step 1: Analyze the first reaction
The first reaction is:
\[ 2Al + 6HCl \rightarrow 2Al^{3+} + 6Cl^- + 3H_2 \]

- In this reaction, aluminum (Al) reacts with hydrochloric acid (HCl).
- HCl is a strong acid, and when it reacts with aluminum, it produces aluminum ions (\(Al^{3+}\)), chloride ions (\(Cl^-\)), and hydrogen gas (\(H_2\)).
- Here, aluminum is donating electrons to the acid, which indicates that aluminum is acting as a base.

### Step 2: Analyze the second reaction
The second reaction is:
\[ 2Al + 2NaOH + 6H_2O \rightarrow 2Na[Al(OH)_4] + 3H_2 \]

- In this reaction, aluminum reacts with sodium hydroxide (NaOH) and water.
- Sodium hydroxide is a strong base, and when it reacts with aluminum, it forms sodium tetrahydroxoaluminate (\(Na[Al(OH)_4]\)) and hydrogen gas (\(H_2\)).
- Here, aluminum is accepting hydroxide ions from the base, indicating that aluminum is acting as an acid.

### Step 3: Conclusion
From the analysis of both reactions:
- In the first reaction with HCl, aluminum acts as a base.
- In the second reaction with NaOH, aluminum acts as an acid.

Since aluminum can act both as an acid and as a base, it is classified as **amphoteric** in nature.

### Final Answer
Therefore, the reactions suggest that aluminum is **amphoteric in nature**.

---