In the lab, a student follows the following steps to determine the freezing point and molality of a deicer solution. 1. Measured the mass of calorimeter with stir bar. 2. Measured the mass of deicer. 3. Measured the volume of water and transfered it to the calorimeter. 4. Added the deicer to calorimeter and dissolved it in the water. 5. Measured the mass of the calorimeter with its contents. 6. Added ice to the calorimeter and reweigh it. 7. Placed a lid on the calorimeter, monitored the temperature of the solution, and recorded the freezing temperature. 8. Decanted the deicer solution, keeping the stir bar and remaining ice. Then measured the mass of the calorimeter with its remaining contents. Trial 1 Freezing temperature of deionized water 0.02°C Deicer used (chemical formula) CaCl2 Mass of calorimeter + stir bar 12.74 g Mass of deicer 4.27 g Volume of water 58.6 mL Mass of calorimeter, stir bar, deicer, and water 75.61 g Mass of calorimeter, stir bar, deicer, water, and added ice 126.97 g Mass of calorimeter, stir bar, and remaining ice 65.10 g Minimum temperature reached −3.76°C (a) Using the data from the table, determine the molality of the deicer solution. molality = __ m CaCl2 (b) Based on the collected data, what is the van't Hoff factor? The Kf for water is 1.86 °C/m. i = _

Chemistry

10th Edition

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

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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In the lab, a student follows the following steps to determine the freezing point and molality of a deicer solution.

1.	Measured the mass of calorimeter with stir bar.
2.	Measured the mass of deicer.
3.	Measured the volume of water and transfered it to the calorimeter.
4.	Added the deicer to calorimeter and dissolved it in the water.
5.	Measured the mass of the calorimeter with its contents.
6.	Added ice to the calorimeter and reweigh it.
7.	Placed a lid on the calorimeter, monitored the temperature of the solution, and recorded the freezing temperature.

8.	Decanted the deicer solution, keeping the stir bar and remaining ice. Then measured the mass of the calorimeter with its remaining contents.

Trial 1
Freezing temperature of deionized water	0.02°C
Deicer used (chemical formula)	CaCl₂
Mass of calorimeter + stir bar	12.74 g
Mass of deicer	4.27 g
Volume of water	58.6 mL
Mass of calorimeter, stir bar, deicer, and water	75.61 g
Mass of calorimeter, stir bar, deicer, water, and added ice	126.97 g
Mass of calorimeter, stir bar, and remaining ice	65.10 g
Minimum temperature reached	−3.76°C

(a) Using the data from the table, determine the molality of the deicer solution.

molality = ______ m CaCl₂

(b) Based on the collected data, what is the van't Hoff factor? The K_f for water is 1.86 °C/m.

i = _____

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