Which of the following can not function as a buffer solution under any condition ?

Options

A. NaCl and NaOH
B. NaOH and `NH_(4)OH`
C. `CH_(3)COONa ` and HCl
D. Borax and boric acid

Answer

To determine which of the given options cannot function as a buffer solution under any condition, we need to understand the characteristics of buffer solutions.

### Step-by-Step Solution:

1. **Definition of Buffer Solutions**:
- A buffer solution is one that resists changes in pH when small amounts of acid or base are added.
- There are two types of buffer solutions:
- **Acidic Buffer**: Composed of a weak acid and its conjugate base (often a salt).
- **Basic Buffer**: Composed of a weak base and its conjugate acid (often a salt).

2. **Identifying the Components**:
- For a solution to act as a buffer, it must contain a weak acid and its conjugate base or a weak base and its conjugate acid.
- Strong acids and strong bases do not form buffers because they completely dissociate in solution.

3. **Analyzing the Given Options**:
- **Option 1**: A strong base (e.g., NaOH) and a salt derived from a strong acid (e.g., NaCl). This combination does not provide a weak acid or weak base, hence cannot function as a buffer.
- **Option 2**: A strong base and a weak base. This combination does not meet the criteria for a buffer since it lacks a conjugate acid.
- **Option 3**: A weak acid (e.g., acetic acid) and its salt (e.g., sodium acetate). This can function as an acidic buffer.
- **Option 4**: Borax (a salt) and boric acid (a weak acid). This can function as a basic buffer.

4. **Conclusion**:
- The options that cannot function as buffer solutions are those that involve strong acids or strong bases without their corresponding weak counterparts. Specifically, options 1 and 2 do not meet the criteria for buffer solutions.

### Final Answer:
Options 1 and 2 cannot function as buffer solutions under any condition.