`[Al(OH)_3(H_2O)_3](s)` more simply written as `Al(OH)_(3)(s)` is :

Options

A. acidic
B. basic
C. neutral
D. amphoteric

Explanation

To determine the nature of aluminum hydroxide, represented as \( Al(OH)_3 \), we can follow these steps:

### Step 1: Identify the Compound
We start with the compound \( Al(OH)_3 \). This is aluminum hydroxide, which is a common compound in chemistry.

### Step 2: Determine the Nature of the Hydroxide
Next, we need to classify the nature of aluminum hydroxide. Hydroxides can be classified as either basic, acidic, or amphoteric.

### Step 3: Test with Acids
To see if aluminum hydroxide is amphoteric, we can test its reaction with an acid. For example, when aluminum hydroxide reacts with hydrochloric acid (\( HCl \)), it forms aluminum chloride (\( AlCl_3 \)) and water (\( H_2O \)):
\[ Al(OH)_3 + 3HCl \rightarrow AlCl_3 + 3H_2O \]

### Step 4: Test with Bases
Next, we test its reaction with a base. When aluminum hydroxide reacts with sodium hydroxide (\( NaOH \)), it forms sodium aluminate (\( NaAlO_2 \)) and water:
\[ Al(OH)_3 + NaOH \rightarrow NaAlO_2 + 2H_2O \]

### Step 5: Conclusion
Since aluminum hydroxide reacts with both acids and bases, we conclude that it is amphoteric. Therefore, the nature of \( Al(OH)_3 \) is that it is an amphoteric hydroxide.

### Final Answer
The correct classification of \( Al(OH)_3 \) is that it is an **amphoteric hydroxide**.

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