`Cu^(2+)` ion is

Options

A. weakly acidic
B. weakly basic
C. strongly basic
D. neutral

Explanation

To determine the nature of the `Cu^(2+)` ion, we can follow these steps:

### Step 1: Understand the Definition of Acids and Bases
- Acids are substances that can donate protons (H⁺ ions).
- Bases are substances that can accept protons or donate hydroxide ions (OH⁻).

**Hint:** Remember the definitions of acids and bases as proton donors and acceptors.

### Step 2: Analyze the Charge of the `Cu^(2+)` Ion
- The `Cu^(2+)` ion has a positive charge, indicating that it can interact with water and other substances.

**Hint:** A positive charge suggests that the ion may have acidic properties.

### Step 3: Determine the Behavior of the `Cu^(2+)` Ion in Water
- When `Cu^(2+)` is dissolved in water, it can interact with water molecules. This interaction can lead to the release of protons (H⁺ ions) into the solution, making the solution acidic.

**Hint:** Consider how metal ions can affect the pH of a solution when they interact with water.

### Step 4: Classify the `Cu^(2+)` Ion
- Since `Cu^(2+)` can donate protons when dissolved in water, it behaves as an acid. However, it does not completely dissociate like a strong acid; instead, it partially dissociates, which classifies it as a weak acid.

**Hint:** Recall that weak acids only partially dissociate in solution.

### Conclusion
The `Cu^(2+)` ion is classified as a weakly acidic ion.

**Final Answer:** `Cu^(2+)` ion is weakly acidic.