We already calculated the molality using the formula:

\[
m = \frac{\Delta T_f}{K_f} = \frac{0.32 \, \text{K}}{1.86 \, \text{K/m}} \approx 0.172 \, \text{mol/kg}
\]

Thus, the molality of the solutes in the solution is approximately \(0.172 \, \text{mol/kg}\). If you need a more detailed explanation or have additional questions, please let me know! 

Here are some related questions you might find useful:

1. What is the difference between molality and molarity, and when is each used?
2. How does freezing-point depression relate to colligative properties?
3. How would the calculation change if the solute were an electrolyte that dissociates in solution?
4. What is the significance of the freezing-point depression constant (\(K_f\))?
5. How can you determine the molar mass of a solute using freezing-point depression?

**Tip:** Always double-check units when performing calculations involving colligative properties to ensure consistency and accuracy.

Learn how to calculate the molality of a solution with a detailed step-by-step solution. This problem covers colligative properties, freezing-point depression, and the formula \( m = \frac{\Delta T_f}{K_f} \). The molality of the solutes in the solution is approximately 0.172 mol/kg. Explore related questions on molality, freezing-point depression, and more.

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