An aqueous solution of ammonium acetate is

Options

A. Faintly acidic
B. Faintly basic
C. Fairly acidic
D. Almost neutral

Explanation

To determine the nature of an aqueous solution of ammonium acetate, we can follow these steps:

### Step 1: Identify the components of ammonium acetate
Ammonium acetate (NH4C2H3O2) is composed of two ions:
- Ammonium ion (NH4⁺), which is derived from a weak base (ammonia, NH3).
- Acetate ion (C2H3O2⁻), which is derived from a weak acid (acetic acid, CH3COOH).

### Step 2: Understand the properties of the ions
- The ammonium ion (NH4⁺) can donate protons (H⁺) in solution, making it a weak acid.
- The acetate ion (C2H3O2⁻) can accept protons, making it a weak base.

### Step 3: Determine the pH of the solution
Since ammonium acetate is a salt formed from a weak acid and a weak base, we can use the formula for the pH of such a solution:
\[ \text{pH} = 7 + \frac{1}{2} \text{pK}_a - \frac{1}{2} \text{pK}_b \]

Where:
- pK_a is the negative logarithm of the acid dissociation constant (K_a) of acetic acid.
- pK_b is the negative logarithm of the base dissociation constant (K_b) of ammonia.

### Step 4: Analyze the pH calculation
Since both K_a and K_b are relatively small (indicating weak acid and weak base), the pH will be close to neutral (7). The contributions from the weak acid and weak base will balance each other out, leading to a pH that is not significantly above or below 7.

### Step 5: Conclusion
Thus, the pH of an aqueous solution of ammonium acetate is approximately neutral, which means it is neither strongly acidic nor strongly basic.

### Final Answer
The aqueous solution of ammonium acetate is **almost neutral**.

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