Question:
A solid solute is dissolved in water. The mole fraction of solute is 0.02. What is the molality of the solution?
A solid solute is dissolved in water. The mole fraction of solute is 0.02. What is the molality of the solution?
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To convert mole fraction to molality, assume 1 mole of total solution components and use the solvent's molar mass.
Updated On: Jun 10, 2026
- 2.133 m
- 2.5 m
- 1.5 m
- 1.133 m
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The Correct Option is D
Solution and Explanation
Step 1: Concept
Molality ($m$) = (moles of solute / mass of solvent in kg). Mole fraction of solute ($x_A$) = $n_A / (n_A + n_B) = 0.02$.
Step 2: Analysis
Let $n_A = 0.02$ moles, then $n_B = 0.98$ moles. Mass of solvent (water) = $0.98 \text{ moles} \times 18 \text{ g/mol} = 17.64 \text{ g} = 0.01764 \text{ kg}$. $m = 0.02 / 0.01764 \approx 1.133 \text{ m}$.
Step 3: Conclusion
The molality is 1.133 m.
Final Answer: (D)
Molality ($m$) = (moles of solute / mass of solvent in kg). Mole fraction of solute ($x_A$) = $n_A / (n_A + n_B) = 0.02$.
Step 2: Analysis
Let $n_A = 0.02$ moles, then $n_B = 0.98$ moles. Mass of solvent (water) = $0.98 \text{ moles} \times 18 \text{ g/mol} = 17.64 \text{ g} = 0.01764 \text{ kg}$. $m = 0.02 / 0.01764 \approx 1.133 \text{ m}$.
Step 3: Conclusion
The molality is 1.133 m.
Final Answer: (D)
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