Assertion : The `pH` of pure water is less than `7` at `60^(@)C`.
Reason : As the temperature increases, pure water becomes slightly acidic.

Options

A. If both Assertion & Reason are True & the Reason is a correct explanation of the Assertion.
B. If both Assertion & Reason are True but Reason is not a correct explanation of the Assertiion.
C. If Assertion is True but the Reason is False.
D. If both Assertion & Reason are False

Explanation

To solve the assertion and reason question, we need to analyze both statements carefully.

### Step-by-Step Solution:

1. **Understanding the Assertion**:
- The assertion states that the pH of pure water is less than 7 at 60°C.
- At 25°C (298 K), the pH of pure water is 7. As temperature increases, the ionic product of water (Kw) also increases.

2. **Calculating Kw at Different Temperatures**:
- At 25°C (298 K), Kw = 10^(-14).
- At 60°C, Kw increases to approximately 10^(-13).

3. **Determining pH at 60°C**:
- The relationship between Kw and pH is given by the equation:
\[ pH = -\log[H^+] \]
- Since Kw = [H+][OH-] and at neutrality [H+] = [OH-], we can set [H+] = [OH-] = x.
- Therefore, at 60°C:
\[ Kw = x^2 = 10^{-13} \implies x = \sqrt{10^{-13}} = 10^{-6.5} \]
- Thus, the pH at 60°C is:
\[ pH = -\log(10^{-6.5}) = 6.5 \]
- This shows that the pH of pure water at 60°C is indeed less than 7.

4. **Understanding the Reason**:
- The reason states that as the temperature increases, pure water becomes slightly acidic.
- While it is true that the pH decreases with increasing temperature, this does not mean that water becomes acidic in the traditional sense (where pH < 7 indicates acidity).

5. **Conclusion**:
- The assertion is true: the pH of pure water is less than 7 at 60°C.
- The reason is false: while the pH decreases, pure water remains neutral (the concentrations of [H+] and [OH-] are equal).

### Final Answer:
- The assertion is true, but the reason is false.