Addition of sodium acetate solution to acetic acid causes the following change–

Options

A. increases in pH
B. decrease in pH
C. no change in pH
D. change in pH that cannot be predicted

Explanation

To solve the problem regarding the addition of sodium acetate to acetic acid and its effect on the pH of the solution, we can follow these steps:

### Step 1: Understand the Components
- Sodium acetate (CH₃COONa) dissociates in solution to give acetate ions (CH₃COO⁻) and sodium ions (Na⁺).
- Acetic acid (CH₃COOH) is a weak acid that partially dissociates into acetate ions (CH₃COO⁻) and hydrogen ions (H⁺).

### Step 2: Write the Equilibrium Expression
The dissociation of acetic acid can be represented as:
\[ \text{CH}_3\text{COOH} \rightleftharpoons \text{CH}_3\text{COO}^- + \text{H}^+ \]

### Step 3: Apply Le Chatelier's Principle
When sodium acetate is added to the acetic acid solution, the concentration of acetate ions (CH₃COO⁻) increases. According to Le Chatelier's Principle, if the concentration of a product (in this case, acetate ions) increases, the equilibrium will shift to the left to counteract this change.

### Step 4: Effect on Hydrogen Ion Concentration
As the equilibrium shifts to the left, the dissociation of acetic acid is suppressed. This means that fewer hydrogen ions (H⁺) are produced in the solution, leading to a decrease in H⁺ concentration.

### Step 5: Determine the Change in pH
Since pH is inversely related to the concentration of hydrogen ions (H⁺), a decrease in H⁺ concentration results in an increase in pH. Therefore, the addition of sodium acetate to acetic acid causes the pH of the solution to increase.

### Conclusion
The addition of sodium acetate to acetic acid suppresses the dissociation of acetic acid, leading to a decrease in H⁺ concentration and an increase in pH.

---