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The problem asks to calculate the pH of a buffer system containing 1.5 M \( \text{HClO} \) and 1.7 M \( \text{NaClO} \), using the dissociation constant (\( K_a \)) of the acid \( \text{HClO} \).

This is a typical buffer problem, and the pH of a buffer solution can be calculated using the **Henderson-Hasselbalch equation**:

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

Where:
- \( [\text{Base}] \) is the concentration of \( \text{ClO}^- \) from \( \text{NaClO} \),
- \( [\text{Acid}] \) is the concentration of \( \text{HClO} \),
- \( \text{p}K_a = -\log(K_a) \).

From the problem, we know:
- \( [\text{HClO}] = 1.5 \, \text{M} \),
- \( [\text{NaClO}] = 1.7 \, \text{M} \).

We still need the \( K_a \) value for hypochlorous acid \( (\text{HClO}) \) at 25°C. The typical value for \( K_a \) of \( \text{HClO} \) is around \( 2.9 \times 10^{-8} \). Now, let's proceed with the calculation.

1. **Calculate pKa**:
   \[
   \text{p}K_a = -\log(2.9 \times 10^{-8}) \approx 7.54
   \]

2. **Apply the Henderson-Hasselbalch equation**:
   \[
   \text{pH} = 7.54 + \log \left( \frac{1.7}{1.5} \right)
   \]
   \[
   \text{pH} = 7.54 + \log(1.133) \approx 7.54 + 0.054 = 7.59
   \]

Therefore, the pH of the buffer system is approximately **7.59**.

Would you like further details on this solution or any clarifications?

### Related Questions:
1. How does the Henderson-Hasselbalch equation apply to buffer systems?
2. What factors influence the pH of a buffer solution?
3. Why is it important to use significant figures when calculating pH?
4. How does temperature affect the \( K_a \) value of acids like \( \text{HClO} \)?
5. Can you calculate the pH if only \( \text{HClO} \) or \( \text{NaClO} \) was present?

### Tip:
Always check the units and make sure concentrations are in molarity (M) when applying the Henderson-Hasselbalch equation.

Calculate the pH of a buffer system containing 1.5 M HClO and 1.7 M NaClO. Be sure your answer has the correct number of significant figures.

Learn how to calculate the pH of a buffer system containing 1.5 M HClO and 1.7 M NaClO. This problem involves the Henderson-Hasselbalch equation and covers key chemistry concepts like acid-base equilibrium. Suitable for high school and college-level chemistry students.

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