Aqueous solution of sodium acetate is

Options

A. Alkaline
B. Neutral
C. Weakly acidic
D. Strongly acidic

Answer

To determine the nature of an aqueous solution of sodium acetate, let's break down the problem step by step.

### Step 1: Identify the Chemical Composition
Sodium acetate is represented by the formula CH₃COONa. It consists of the acetate ion (CH₃COO⁻) and the sodium ion (Na⁺).

**Hint:** Remember that sodium acetate is a salt formed from a weak acid (acetic acid) and a strong base (sodium hydroxide).

### Step 2: Dissociation in Water
When sodium acetate is dissolved in water, it dissociates into its constituent ions:
\[ \text{CH}_3\text{COONa} \rightarrow \text{CH}_3\text{COO}^- + \text{Na}^+ \]

**Hint:** Consider how salts dissociate in water and what ions are produced.

### Step 3: Analyze the Ions
- The acetate ion (CH₃COO⁻) can react with water:
\[ \text{CH}_3\text{COO}^- + \text{H}_2\text{O} \rightleftharpoons \text{CH}_3\text{COOH} + \text{OH}^- \]
This reaction shows that the acetate ion can accept a proton (H⁺) from water, producing acetic acid (CH₃COOH) and hydroxide ions (OH⁻).

**Hint:** Look for the behavior of the acetate ion in water and how it affects the pH.

### Step 4: Determine the pH of the Solution
The production of hydroxide ions (OH⁻) indicates that the solution will become basic (alkaline). Since the acetate ion is derived from a weak acid (acetic acid) and reacts to produce OH⁻, the overall solution will be alkaline.

**Hint:** Remember that the presence of OH⁻ ions in solution indicates a basic environment.

### Step 5: Conclusion
Based on the above analysis, we conclude that an aqueous solution of sodium acetate is alkaline in nature.

**Final Answer:** The correct option is **alkaline**.