Statement- 1 . `Be(OH)_(2)` is soluble both in HCl and NaOH .
Statement- 2 . `Be(OH)_(2)` is amphoteric in nature .

Options

A. Statement-1 is True, Statement-2 is True, Statement-2 is a correct explanation for statement-1.
B. Statement-1 is True, Statement-2 is True, Statement-2 is not a correct explanation for statement-1.
C. Statement-1 is True, Statement-2 is False.
D. Statement-1 is False, Statement-2 is True.

Answer

To analyze the statements regarding beryllium hydroxide, we will break down the information step by step.

### Step 1: Understand the Solubility of Be(OH)₂
Beryllium hydroxide, \( \text{Be(OH)}_2 \), is known to be soluble in both hydrochloric acid (HCl) and sodium hydroxide (NaOH).

- **In HCl**: When beryllium hydroxide reacts with hydrochloric acid, it forms beryllium chloride and water:
\[ \text{Be(OH)}_2 + 2 \text{HCl} \rightarrow \text{BeCl}_2 + 2 \text{H}_2\text{O} \]
This indicates that \( \text{Be(OH)}_2 \) dissolves in HCl.

- **In NaOH**: When beryllium hydroxide reacts with sodium hydroxide, it forms sodium beryllate:
\[ \text{Be(OH)}_2 + 2 \text{NaOH} \rightarrow \text{Na}_2\text{Be(OH)}_4 \]
This indicates that \( \text{Be(OH)}_2 \) also dissolves in NaOH.

### Step 2: Determine the Nature of Be(OH)₂
Beryllium hydroxide is classified as an amphoteric hydroxide. Amphoteric substances can react with both acids and bases.

- **Amphoteric Nature**: Since \( \text{Be(OH)}_2 \) reacts with both an acid (HCl) and a base (NaOH), it confirms its amphoteric nature.

### Step 3: Evaluate the Statements
- **Statement 1**: "Be(OH)₂ is soluble both in HCl and NaOH." - This statement is **true** based on the reactions we analyzed.

- **Statement 2**: "Be(OH)₂ is amphoteric in nature." - This statement is also **true**, as it can react with both acids and bases.

### Conclusion
Both statements are correct, and statement 2 correctly explains statement 1.

### Final Answer
Both Statement 1 and Statement 2 are correct, and Statement 2 is the correct explanation for Statement 1.

---