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, we can follow these steps:

### Step 1: Identify the components of sodium acetate
Sodium acetate (CH₃COONa) is a salt formed from the reaction of acetic acid (CH₃COOH), a weak acid, and sodium hydroxide (NaOH), a strong base.

### Step 2: Understand the nature of the ions in solution
When sodium acetate is dissolved in water, it dissociates into sodium ions (Na⁺) and acetate ions (CH₃COO⁻).
- Na⁺ is a spectator ion and does not affect the pH of the solution.
- CH₃COO⁻, being the conjugate base of the weak acid acetic acid, can accept protons (H⁺) from water, leading to an increase in hydroxide ions (OH⁻) in the solution.

### Step 3: Analyze the effect on pH
The acetate ion (CH₃COO⁻) will react with water in a hydrolysis reaction:
\[ \text{CH}_3\text{COO}^- + \text{H}_2\text{O} \rightleftharpoons \text{CH}_3\text{COOH} + \text{OH}^- \]

This reaction produces hydroxide ions (OH⁻), which increases the pH of the solution.

### Step 4: Determine the pH of the solution
Since the solution contains a weak acid's conjugate base (acetate ion), the pH can be calculated using the formula for the pH of a salt derived from a weak acid and a strong base:
\[ \text{pH} = 7 + \frac{1}{2} \text{pK}_a + \frac{1}{2} \log C \]
Where:
- \( \text{pK}_a \) is the negative logarithm of the acid dissociation constant of acetic acid.
- \( C \) is the concentration of the sodium acetate solution.

This formula indicates that the pH will be greater than 7.

### Step 5: Conclusion
Since the pH of the solution is greater than 7, we conclude that an aqueous solution of sodium acetate is basic (alkaline).

### Final Answer
An aqueous solution of sodium acetate is basic (alkaline).

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