Freezing point depression can be used to experimentally determine the van 't Hoff factor of a solute in solution. Given the data in the table, answer the questions below and determine the "real" van 't Hoff factor of the solute. Experimental Results Mass of solvent (water) 8.413 g Freezing point of water 0.00°C Freezing point depression constant (Kf) of water 1.86°C/m Mass of solution 9.226 g Freezing point of solution −4.73°C (a) What mass of solute was used? g (b) What is the freezing point depression ΔTf of the solution? °C (c) What is the colligative molality mc of the solution? m (d) How many moles of solute particles are present in solution? mol (e) If the solute has a molar mass of 144.02, what is the van 't Hoff factor i for the solute? (Remember that experimentally, i does not have to be an integer.)
Freezing point depression can be used to experimentally determine the van 't Hoff factor of a solute in solution. Given the data in the table, answer the questions below and determine the "real" van 't Hoff factor of the solute. Experimental Results Mass of solvent (water) 8.413 g Freezing point of water 0.00°C Freezing point depression constant (Kf) of water 1.86°C/m Mass of solution 9.226 g Freezing point of solution −4.73°C (a) What mass of solute was used? g (b) What is the freezing point depression ΔTf of the solution? °C (c) What is the colligative molality mc of the solution? m (d) How many moles of solute particles are present in solution? mol (e) If the solute has a molar mass of 144.02, what is the van 't Hoff factor i for the solute? (Remember that experimentally, i does not have to be an integer.)
Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Freezing point depression can be used to experimentally determine the van 't Hoff factor of a solute in solution. Given the data in the table, answer the questions below and determine the "real" van 't Hoff factor of the solute.
Experimental Results
| Mass of solvent (water) | 8.413 g |
| Freezing point of water | 0.00°C |
| Freezing point depression constant (Kf) of water | 1.86°C/m |
| Mass of solution | 9.226 g |
| Freezing point of solution |
−4.73°C
|
(a) What mass of solute was used?
g
(b) What is the freezing point depression ΔTf of the solution?
°C
(c) What is the colligative molality mc of the solution?
m
(d) How many moles of solute particles are present in solution?
mol
(e) If the solute has a molar mass of 144.02, what is the van 't Hoff factor i for the solute? (Remember that experimentally, i does not have to be an integer.)
g
(b) What is the freezing point depression ΔTf of the solution?
°C
(c) What is the colligative molality mc of the solution?
m
(d) How many moles of solute particles are present in solution?
mol
(e) If the solute has a molar mass of 144.02, what is the van 't Hoff factor i for the solute? (Remember that experimentally, i does not have to be an integer.)
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According to the question,
Mass of solvent (water) = 8.413 g
The Freezing point of water= is 0.00°C
The Freezing point depression constant (Kf) of water =1.86°C/m
The Mass of solution= 9.226 g
The Freezing point of solution = −4.73°C
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