Correct relation b/w dissociation constant's of a di-basic acid:

Options

A. `Ka_(1) = Ka_(2)`
B. `Ka_(1) gt Ka_(2)`
C. `Ka_(1) lt Ka_(2)`
D. `Ka_(1) = (1)/(Ka_(2))`

Answer

To determine the correct relationship between the dissociation constants (Ka1 and Ka2) of a dibasic acid, we can follow these steps:

### Step-by-Step Solution:

1. **Understanding Dissociation Constants**:
- The dissociation constant (Ka) is a measure of the strength of an acid in solution. It indicates how easily an acid donates protons (H⁺ ions) to the solution.

2. **Identifying the Acid**:
- A dibasic acid can donate two protons. A common example is sulfuric acid (H₂SO₄), which can dissociate in two steps:
- First dissociation: H₂SO₄ ⇌ H⁺ + HSO₄⁻ (Ka1)
- Second dissociation: HSO₄⁻ ⇌ H⁺ + SO₄²⁻ (Ka2)

3. **Comparing the First and Second Dissociation**:
- In the first dissociation (Ka1), we are removing a proton from a neutral molecule (H₂SO₄), which is relatively easy.
- In the second dissociation (Ka2), we are removing a proton from a negatively charged ion (HSO₄⁻). The presence of the negative charge creates repulsion, making it more difficult to remove the proton.

4. **Analyzing Acidic Strength**:
- Since Ka is directly proportional to the acidic strength of the acid, we can conclude that:
- The first dissociation (Ka1) is stronger than the second dissociation (Ka2) because it is easier to remove a proton from a neutral molecule than from a negatively charged ion.

5. **Conclusion**:
- Therefore, we can conclude that Ka1 > Ka2.

### Final Answer:
The correct relationship between the dissociation constants of a dibasic acid is: **Ka1 > Ka2**.