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 1Freezing temperature of deionized water0.02°CDeicer used (chemical formula)CaCl2Mass of calorimeter + stir bar12.74 gMass of deicer9.57 gVolume of water58.6 mLMass of calorimeter, stir bar, deicer, and water80.91 gMass of calorimeter, stir bar, deicer, water, and added ice126.97 gMass of calorimeter, stir bar, and remaining ice65.10 gMinimum temperature reached−9.32°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 =

Given mass of CaCl2 = 9.57 g Volume of water = 58.6 mL = 58.6 g Convert grams to kg using…

Answered: (a) Using the data from the table,…

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

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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	9.57 g
Volume of water	58.6 mL
Mass of calorimeter, stir bar, deicer, and water	80.91 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	−9.32 ° 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 =

Expert Solution

Step 1

Given

mass of CaCl₂ = 9.57 g
Volume of water = 58.6 mL = 58.6 g

Convert grams to kg using conversion factor : 1 kg = 1000 g

mass of water (solvent) = 0.0586 kg

Required data -

molar mass of CaCl₂ = 110.98 g/mol

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