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A solution of 1.50 g of solute dissolved in 25.0 mLof H2O
Chapter 14, Problem 93P(choose chapter or problem)
Problem 93P
A solution of 1.50 g of solute dissolved in 25.0 mLof H2O at 25°C has a boiling point of 100.45°C. (a) What is the molar mass of the solute if it is a nonvolatile nonelectrolyte and the solution behaves ideally (d of H2O at 25°C = 0.997 g/mL)? (b) Conductivity measurements show the solute to be ionic of general formula AB2 or A2B. What is the molar mass if the solution behaves ideally? (c) Analysis indicates an empirical formula of CaN2O6. Explain the difference between the actual formula mass and that calculated from the boiling point elevation, (d) Find the van't Hoff factor (i) for this solution.
Questions & Answers
QUESTION:
Problem 93P
A solution of 1.50 g of solute dissolved in 25.0 mLof H2O at 25°C has a boiling point of 100.45°C. (a) What is the molar mass of the solute if it is a nonvolatile nonelectrolyte and the solution behaves ideally (d of H2O at 25°C = 0.997 g/mL)? (b) Conductivity measurements show the solute to be ionic of general formula AB2 or A2B. What is the molar mass if the solution behaves ideally? (c) Analysis indicates an empirical formula of CaN2O6. Explain the difference between the actual formula mass and that calculated from the boiling point elevation, (d) Find the van't Hoff factor (i) for this solution.
ANSWER:
Solution 93P:
Step 1: (a)
Here, we are going to determine the molar mass of the solute if it is a nonvolatile nonelectrolyte and the solution behaves ideally.
Given that,
Mass of the solute = 1.50 g
Volume of the solvent (H2O) = 25.0 mL
Density of the solvent = 0.997 g/mL
Therefore, the mass of the solvent = 25.0 mL
= 24.925 g
= 0.0249 kg
We know that,
The boiling point elevation is given by:
where m is the solution molality, Kb is the molal boiling point elevation constant,
Given that,
= 100.45°C.
= 0 oC
=0.512 oC/m
Thus,
=
= 0.8789 mol/kg
Thus,
Molality (m) = Mass of the solute/mass of the solvent (kg)
=0.02188 mol
Therefore, the molar mass of the solute =
= = 68.56 g/mol