The solution of `Na_2CO_3` has PH

Options

A. greater than 7
B. less than 7
C. equal to 7
D. equal to zero

Answer

To determine the pH of a solution of sodium carbonate (Na₂CO₃), we can follow these steps:

### Step 1: Dissociation of Sodium Carbonate
When sodium carbonate (Na₂CO₃) is dissolved in water, it dissociates into sodium ions (Na⁺) and carbonate ions (CO₃²⁻):
\[ \text{Na}_2\text{CO}_3 \rightarrow 2\text{Na}^+ + \text{CO}_3^{2-} \]

### Step 2: Reaction of Carbonate Ions with Water
The carbonate ions (CO₃²⁻) can react with water to form bicarbonate ions (HCO₃⁻) and hydroxide ions (OH⁻):
\[ \text{CO}_3^{2-} + \text{H}_2\text{O} \rightleftharpoons \text{HCO}_3^{-} + \text{OH}^- \]

### Step 3: Basic Nature of the Solution
The production of hydroxide ions (OH⁻) indicates that the solution is basic. Since the concentration of OH⁻ ions increases, the pH of the solution will be greater than 7.

### Step 4: Conclusion
Since the solution of Na₂CO₃ produces more hydroxide ions than hydrogen ions, we conclude that the pH of the solution will be in the basic range. Therefore, the pH of the solution of Na₂CO₃ is greater than 7.

### Final Answer
The pH of the solution of Na₂CO₃ is basic (greater than 7).

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