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Mole fraction of the solute in a 1.00 molal aqueous solution is
- a)0.071
- b)0.0177
- c)0.058
- d)1.72
Correct answer is option 'B'. Can you explain this answer?
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Verified Answer
Mole fraction of the solute in a 1.00 molal aqueous solution isa)0.071...
1 molal aq. solution means 1 mol of solute is dissolved in 1000 g of H2O
Number of moles of H2O = 1000/18 = 55.55 mol
Number of moles of H2O = 1000/18 = 55.55 mol
Most Upvoted Answer
Mole fraction of the solute in a 1.00 molal aqueous solution isa)0.071...
Mole Fraction Calculation
To find the mole fraction of the solute in a 1.00 molal aqueous solution, we first need to understand the definitions involved.
Definitions
- Molality (m): This is defined as the number of moles of solute per kilogram of solvent.
- Mole Fraction (X): This is defined as the ratio of the moles of solute to the total moles in the solution.
Given Data
- 1.00 molal solution: This implies there is 1 mole of solute in 1 kg (1000 g) of solvent (water).
Calculating Moles of Solvent
1. Molar Mass of Water: The molar mass of water (H₂O) is approximately 18 g/mol.
2. Calculating Moles of Water:
\[
\text{Moles of water} = \frac{1000 \text{ g}}{18 \text{ g/mol}} \approx 55.56 \text{ moles}
\]
Finding Total Moles
- Moles of Solute: 1 mole (as given).
- Total Moles in Solution:
\[
\text{Total moles} = \text{Moles of solute} + \text{Moles of solvent} = 1 + 55.56 \approx 56.56 \text{ moles}
\]
Calculating Mole Fraction of Solute
- Mole Fraction of Solute (X₁):
\[
X_{\text{solute}} = \frac{\text{Moles of solute}}{\text{Total moles}} = \frac{1}{56.56} \approx 0.0177
\]
Conclusion
Thus, the mole fraction of the solute in a 1.00 molal aqueous solution is approximately 0.0177, confirming that the correct answer is option B.
To find the mole fraction of the solute in a 1.00 molal aqueous solution, we first need to understand the definitions involved.
Definitions
- Molality (m): This is defined as the number of moles of solute per kilogram of solvent.
- Mole Fraction (X): This is defined as the ratio of the moles of solute to the total moles in the solution.
Given Data
- 1.00 molal solution: This implies there is 1 mole of solute in 1 kg (1000 g) of solvent (water).
Calculating Moles of Solvent
1. Molar Mass of Water: The molar mass of water (H₂O) is approximately 18 g/mol.
2. Calculating Moles of Water:
\[
\text{Moles of water} = \frac{1000 \text{ g}}{18 \text{ g/mol}} \approx 55.56 \text{ moles}
\]
Finding Total Moles
- Moles of Solute: 1 mole (as given).
- Total Moles in Solution:
\[
\text{Total moles} = \text{Moles of solute} + \text{Moles of solvent} = 1 + 55.56 \approx 56.56 \text{ moles}
\]
Calculating Mole Fraction of Solute
- Mole Fraction of Solute (X₁):
\[
X_{\text{solute}} = \frac{\text{Moles of solute}}{\text{Total moles}} = \frac{1}{56.56} \approx 0.0177
\]
Conclusion
Thus, the mole fraction of the solute in a 1.00 molal aqueous solution is approximately 0.0177, confirming that the correct answer is option B.
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Community Answer
Mole fraction of the solute in a 1.00 molal aqueous solution isa)0.071...
X solute= 1/1+55.5>0.0177
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Mole fraction of the solute in a 1.00 molal aqueous solution isa)0.071b)0.0177c)0.058d)1.72Correct answer is option 'B'. Can you explain this answer?
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