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We are given a buffer made of \(0.057 \, \text{M NaF}\) (the base) and \(0.043 \, \text{M HF}\) (the acid), with a dissociation constant for hydrofluoric acid, \(K_a = 6.60 \times 10^{-4}\).

The equation for the pH of a buffer is:

\[
\text{pH} = \text{p}K_a + \log \left( \frac{\text{[base]}}{\text{[acid]}} \right)
\]

First, we need to calculate \(\text{p}K_a\):

\[
\text{p}K_a = -\log(K_a) = -\log(6.60 \times 10^{-4})
\]

Now, we substitute the concentrations of the base (NaF) and the acid (HF) into the Henderson-Hasselbalch equation.

### Step-by-step solution:

1. Calculate \(\text{p}K_a\):
   \[
   \text{p}K_a = -\log(6.60 \times 10^{-4}) = 3.181
   \]

2. Now use the Henderson-Hasselbalch equation:
   \[
   \text{pH} = 3.181 + \log \left( \frac{0.057}{0.043} \right)
   \]

3. Calculate the ratio of base to acid:
   \[
   \frac{0.057}{0.043} = 1.326
   \]

4. Take the logarithm:
   \[
   \log(1.326) = 0.123
   \]

5. Finally, calculate the pH:
   \[
   \text{pH} = 3.181 + 0.123 = 3.304
   \]

The pH of the buffer is **3.304** (rounded to three significant figures).

---

Would you like more details on any step or have any further questions? Here are 5 related questions you might consider:

1. How would the pH change if the concentration of NaF increased?
2. What is the significance of the buffer capacity in this system?
3. How does the \(K_a\) value affect the pH of the buffer?
4. What is the relationship between \([\text{base}]\) and \([\text{acid}]\) in determining buffer pH?
5. How would adding a strong acid affect the pH of this buffer solution?

**Tip:** Always ensure the concentrations of both acid and base are close to equal to achieve an effective buffer system.

Calculate the pH of a buffer that is made up of 0.057 M NaF and 0.043 M HF solutions. Ka(HF) = 6.60x10^(-4).

Learn how to calculate the pH of a buffer solution made of 0.057 M NaF and 0.043 M HF using the Henderson-Hasselbalch equation. This solution covers concepts of acid-base chemistry, logarithms, and buffer systems, suitable for high school chemistry students.

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