Which of the following statement is not correct?

Options

A. `CI^(-)` is a Lewis acid
B. The `p^(H)` of `10^(-8)` M HCI solution is less than 7
C. The ionic product of water at `25^(@)` C is `10^(14) M^(2)`
D. Bronsted -Lowry theory could not explain the acidic nature of `AICl^(3)`

Answer

To determine which of the following statements is not correct, we will analyze each statement one by one.

### Step 1: Analyze the first statement
**Statement 1:** Cl⁻ is a Lewis acid.

- **Explanation:** A Lewis acid is defined as a species that can accept a pair of electrons to form a covalent bond. Cl⁻ (chloride ion) has an extra electron, making it negatively charged, and it can donate a pair of electrons. Therefore, Cl⁻ acts as a Lewis base, not a Lewis acid.

### Step 2: Analyze the second statement
**Statement 2:** The pH of 10⁻⁸ M HCl solution is less than 7.

- **Explanation:** A 10⁻⁸ M HCl solution is very dilute. The concentration of H⁺ ions from water itself is 10⁻⁷ M. In this case, the total concentration of H⁺ ions is 10⁻⁸ M (from HCl) + 10⁻⁷ M (from water) = 1.1 x 10⁻⁷ M. The pH is calculated as -log(1.1 x 10⁻⁷), which is approximately 6.96, thus it is indeed less than 7.

### Step 3: Analyze the third statement
**Statement 3:** The ion product of water at 25 degrees Celsius is 10⁻¹⁴ M².

- **Explanation:** The ion product of water (Kw) at 25 degrees Celsius is indeed 1.0 x 10⁻¹⁴ M². This statement is correct.

### Step 4: Analyze the fourth statement
**Statement 4:** Bronsted-Lowry theory could not explain the acidic nature of AlCl₃.

- **Explanation:** AlCl₃ can act as a Lewis acid and can accept a pair of electrons, but it does not donate protons (H⁺ ions), which is a requirement for a substance to be classified as an acid under the Bronsted-Lowry theory. Therefore, this statement is correct.

### Conclusion
After analyzing all the statements, the incorrect statement is:
- **Cl⁻ is a Lewis acid.**

### Final Answer
The statement that is not correct is: **Cl⁻ is a Lewis acid.**

---