Choose the wrong statement(s).

Options

A. If the eqb. constant changes, the state of eqb. has to change.
B. If the state of eqb. changes, the eqb. constant has to change.
C. The acid with a lower `pK_(a)` value has higher acid strength than the acid with a higher value of `PK_(a)`.
D. Two acids of the same pH are always of equal acid strength

Answer

To solve the question of identifying the wrong statements, we will analyze each statement one by one.

### Step-by-Step Solution:

1. **Statement 1: If the equilibrium constant changes, the state of equilibrium has to change.**
- This statement is **incorrect**. The equilibrium constant (K) only changes with temperature. If the temperature remains constant, the equilibrium constant does not change, even if other conditions (like concentration or pressure) change. Thus, this statement is wrong.

2. **Statement 2: If the state of equilibrium changes, then the case value will change.**
- This statement is also **incorrect**. The equilibrium constant (K) only changes with temperature. Changes in concentration or pressure do not affect the value of K, so this statement is wrong.

3. **Statement 3: The lower pKa value has higher acid strength.**
- This statement is **correct**. A lower pKa value indicates a stronger acid because it means the acid dissociates more completely in solution, leading to a higher concentration of hydrogen ions (H+). Therefore, this statement is true.

4. **Statement 4: Two acids of the same pH are always of equal acid strength.**
- This statement is **incorrect**. Two acids can have the same pH but different strengths. The pH is influenced by the concentration of hydrogen ions, which can be the same for different acids, but their ability to donate protons (strength) can vary. Thus, this statement is wrong.

### Conclusion:
The wrong statements are:
- Statement 1
- Statement 2
- Statement 4

### Final Answer:
The wrong statements are: **1, 2, and 4.**

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