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1. Part 1 - Geta Lab Appointmentand Install Software:
Findthe email fromyourinstructorwiththe URL (link) tosignupat the scheduler.
Setup your schedulingsystemaccountandschedule yourlabappointment.
NOTE: You cannotmake an appointmentuntil twoweekspriortothe start date of thislabassignment.
You can get yourusername andpasswordfromyouremail toschedule withinthistimeframe.
Install the Citrix software: – go to http://receiver.citrix.com andclick
download>accept > run > install (FIRSTTIME USING NANSLO).
You onlyhave to dothisONCE. Do NOT openit afterinstalling.Itwill workautomaticallywhenyougo
to yourlab. (more infoat
http://www.wiche.edu/info/nanslo/creative_science/Installing_Citrix_Receiver_Program.pdf)
SchedulingAdditional Lab Appointments:
Get yourscheduleraccountusername andpasswordfromyouremail.
Go to the URL (link) giventoyouby your instructorandsetup your appointment.
(more infoat http://www.wiche.edu/nanslo/creative-science-solutions/students-scheduling-labs)
ChangingYour ScheduledLab Appointment:
Get yourscheduleraccountusername andpasswordfromyouremail.Goto http://scheduler.nanslo.org
and selectthe “Iam a student”button. Login to go to the studentdashboardandmodifyyour
appointmenttime. (more infoathttp://www.wiche.edu/nanslo/creative-science-solutions/students-
scheduling-labs)
Part 2 – Before Lab Day:
Read your labexperimentbackgroundandprocedure below,pages1-8.
Submit yourcompletedPre-LabQuestions(page5-6) peryourfaculty’sinstructions.
Watch the TitrationApparatus Control Panel VideoTutorial
http://www.wiche.edu/nanslo/lab-tutorials#titration
Part 3 – Lab Day
Log in to your labsession –2 options:
1)Retrieve youremail fromthe schedulerwithyourappointmentinfoor
2) Log in to the studentdashboardandjoinyoursessionby goingtohttp://scheduler.nanslo.org
NOTE: You cannotlog into yoursessionbefore the date andstarttime of yourappointment.Use
InternetExplorerorFirefox.
Clickon the yellowbutton on the bottomof the screenandfollow the instructions totalkto yourlab
partnersand the labtech

2. 1 | P a g e L a s t U p d a t e d M a y 2 6 , 2 0 1 5
Remote Lab Activity
SUBJECT SEMESTER: ____________
TITLE OF LAB: Colligative Properties – Freezing
Point Depression
Lab format: This lab is a remote lab activity.
Relationship to theory (if appropriate): In this lab you will explore the effects of dissolved
materials on the freezing point of the solvent. Students should have been introduced to the
concepts of ionic and molecular compounds and poly-atomic ions.
Instructions for Instructors: This protocol is written under an open source CC BY license. You
may use the procedure as is or modify as necessary for your class. Be sure to let your students
know if they should complete optional exercises in this lab procedure as lab technicians will not
know if you want your students to complete optional exercises.
Instructions for Students: Read the complete laboratory procedure before coming to lab.
Under the experimental sections, complete all pre-lab materials before logging on to the
remote lab. Complete data collection sections during your online period, and answer questions
in analysis sections after your online period. Your instructor will let you know if you are
required to complete any optional exercises in this lab.
Remote Resources: Primary – Titration Apparatus; Secondary – Temperature Probe
CONTENTS FOR THIS NANSLO LAB ACTIVITY:
Learning Objectives ....................................................................................................... 2
Background Information ............................................................................................... 2-4
Estimating Error ............................................................................................................ 4-5
Pre-lab Questions .......................................................................................................... 5-6
Equipment ..................................................................................................................... 6
Preparing for this NANSLO Lab Activity ......................................................................... 6
Experimental Procedure ............................................................................................... 7
Exercise 1: Measuring Freezing Points of Various Solutions ....................................... 7
Post-Lab Analysis .......................................................................................................... 7
Creative Commons Licensing ........................................................................................ 8
U.S. Department of Labor Information ......................................................................... 8

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LEARNING OBJECTIVES:
After completing this laboratory experiment, you should be able to do the following things:
1. Explain the difference between molecular and ionic substances when they dissolve in a
solvent.
2. Use the mathematical expression for freezing point depression to calculate
concentration of solute, change in freezing point, etc.
3. Describe various applications for freezing point depression.
4. Determine the value of the van’t Hoff factor for various molecules.
5. Explain the meaning of the van’t Hoff factor.
BACKGROUND INFORMATION:
The Colligative Properties are a collection of macroscopic phenomena that are related to
dissolved solutes in liquid solvents.
Solvent: A liquid in which materials are dissolved.
Solute: Something that is dissolved into a solvent.
They are: freezing point depression, boiling point elevation, vapor pressure lowering and
osmotic pressure. These are all properties of bulk liquids that are affected by having dissolved
solutes, and they are not dependent on the identity of the solute, but only of the solvent itself.
In other words, the Colligative Properties of water are affected in the same way, no matter
what you dissolve in the water.
All you need to know, in order to calculate the magnitude of the change in boiling point,
freezing point, etc., is the identity of the solvent, and the total concentration of the dissolved
material. By “total concentration”, we mean the concentration of all the particles that form
when the solute dissolves.
For example, the molecules of the solute stay intact when a molecular solute such as isopropyl
alcohol (also called “rubbing alcohol”) dissolves in water. So, if we dissolved 1.25 moles of
isopropyl alcohol in water, there are 1.25 moles of isopropyl alcohol molecules dispersed into
the water molecules. However, if we dissolve an ionic solute, such as copper sulfate (sold in
hardware stores as “root killer”), each formula unit of the ionic substance breaks into positive
and negative ions when it dissolves.
In the case of copper sulfate (CuSO4), each formula unit breaks up into a copper ion (Cu2+) and a
sulfate ion (SO4
2-). So if we dissolved 1.25 moles of copper sulfate in water, there would be

4. 3 | P a g e L a s t U p d a t e d M a y 2 6 , 2 0 1 5
1.25 moles of Cu2+ and 1.25 moles of SO4
2- dispersed into the water molecules, or a total of 2.50
moles of ions.
Make sure you have memorized the complex ions, like sulfate, phosphate,
carbonate, etc. so you can recognize them when you see them in an ionic
compound.
In the case of ionic compounds, then, the “total concentration” is the concentration of the ionic
substance multiplied by the number of ions that it breaks up into when it dissolves. Usually, the
number of ions that a substance breaks up into is referred to in this context as the “van’t Hoff
Factor” and is given the symbol i. This factor is named for Jacobus van’t Hoff, the first chemist
ever awarded the Nobel Prize, which was given for his work on osmotic pressure in 1901
(Nobelprize.org). For a molecular substance, like isopropyl alcohol, the value of i is 1. For an
ionic substance, i is equal to the number of ions in each formula unit. For example, the van’t
Hoff factor for copper sulfate would be 2.*
* It is beyond the scope of this lab activity, but the van’t Hoff factor for some ionic
substances is actually not an integer and is less than the theoretical maximum of the
number of ions in the formula unit. This is because in some solutions, the ionic
substance is not 100% dissociated. However, for this activity, the ionic substances used
will be assumed to be 100% dissociated.
In this activity, we will be investigating the colligative property of freezing point depression.
The relationship between the freezing point and the amount of dissolved solute is expressed
mathematically as:
∆𝑇𝑓 = 𝑖 ∙ 𝑚 ∙ 𝐾𝑓
In the above equation, ∆𝑇𝑓 is the change in the freezing point, i is the van’t Hoff factor, m is the
concentration of the solute in molality and Kf is the freezing point constant. For water, the
value of Kf is 1.86 °C/m. Remember that molality is defined as:
𝑚𝑜𝑙𝑒𝑠 𝑜𝑓 𝑠𝑜𝑙𝑢𝑡𝑒
𝑘𝑔 𝑜𝑓 𝑠𝑜𝑙𝑣𝑒𝑛𝑡
Notice that in the denominator, it is only the mass of the solvent, not of the entire solution.
Why does the freezing point of the solution change just because something is dissolved in the
solvent? And why does the freezing point always decrease? To understand this, we have to
think about it at a molecular level. When a solvent freezes, the molecules of that solvent must
form a particular structure. Think of molecules in a pure liquid phase. The molecules are
constantly moving around each other. Even though they are attracted to each other by
intermolecular forces, they aren’t in any fixed positions relative to each other.

5. 4 | P a g e L a s t U p d a t e d M a y 2 6 , 2 0 1 5
However, when the substance becomes cold enough, the molecular motion slows down
enough that the intermolecular forces become significant, and they eventually begin to “stick”
together. When the solvent molecules begin to connect with each other, they arrange
according to the strongest intermolecular attractions between them and form a particular
crystalline arrangement as they become a solid.
Of course, a certain amount of energy is required to be removed from the solvent in order to
induce this process. Well, if there is something dissolved in the solvent, it interferes with this
process. When anything dissolves in a solvent, the solvent molecules form a three-dimensional
cage around each of the dissolved particles, whether they are molecules or ions. This makes it
much more difficult for the solvent molecules to get into a close arrangement with each other,
and more energy must be removed from the systemin order to induce the change from liquid
to solid. This means that the solution must be made colder than the pure solvent in order to
form solid crystals.
But it also means that when things are dissolved into the solvent, the motions of the solvent
molecules are decreased, because they are “stuck to” the dissolved particles. When the solvent
molecules aren’t moving around as much that means the temperature of the system is
decreased, because “temperature” is related to how fast the molecules are moving around.
The faster the molecular motion, the higher the temperature, and vice versa.
There are several practical applications of freezing point depression (Advanced Instruments
website). One obvious application that most people are familiar with is the prevention of ice
formation in the winter. Salts such as sodium chloride or magnesium chloride are put onto
roads and sidewalks, and ice is prevented from forming because the freezing point of the
salt/water solution is lower than the freezing point of pure water. A related application that
you may have experienced is the use of salt and ice to create a lower temperature for making
ice cream. Putting salt onto the ice surrounding the ice cream maker creates a lower
temperature than ice alone, and the more salt you add, the colder it gets!
ESTIMATING ERROR:
You can always estimate the error in any measurement by taking several measurements of it
and calculating the standard deviation of the set of results. In other words, if you measure
something several times, you are likely to end up with a set of results that are not all exactly the
same number. The standard error of that set of numbers is an estimate of how much error
there is in your results, and it is equal to the standard deviation divided by the square root of
the number of samples in the data set. Here’s an example. Let’s say we measured something
five times, and the result was:

6. 5 | P a g e L a s t U p d a t e d M a y 2 6 , 2 0 1 5
Trial #1 Measurement
1 0.324
2 0.332
3 0.325
4 0.328
5 0.322
We would report that the value was: average +/- standard error, which in this case is: 0.326
+/- 0.002. This means that the uncertainty in your result (0.326) starts in the third decimal
place, because that’s the first digit in your standard error. Since the uncertainty starts in the
thousandths place, we have to limit the average value to the thousandths place as well. When
reporting uncertainty in this way, you always report only one digit in the standard error.
The standard deviation can be calculated manually (you’ve probably done this in a math
course), or you can use a spreadsheet program like Excel. If you have fewer than 100 samples
to work with, use the “stdev.s” function, which is more accurate for small samples.
Sources:
Official Web Site of the Nobel Prize,
http://www.nobelprize.org/nobel_prizes/chemistry/laureates/1901/ (accessed Oct 3, 2014)
Advanced Instruments, Freezing Point Osmometry Practical Applications,
http://www.aicompanies.com/index.cfm/AiUniversity/TheoryandBenefitsofFreezingOsmometr
y/Freezing_Point_Osmometry_Practical_Applications (accessed Oct 3, 2014)
PRE-LAB QUESTIONS:
1. What are the values of the van’t Hoff factor for the following substances? (Hint: It
helps to write the chemical formula for each substance.)
a. Sucrose ___________
b. Magnesium chloride __________
c. Iron (III) carbonate __________
d. Calciumphosphate __________
e. Sodium chloride ___________
2. Can the van’t Hoff factor ever be zero? Explain.
3. Calculate the freezing point change from 20.56 grams of magnesium chloride are
dissolved in 300.0 grams of water.
a. What is the freezing point of this solution?

7. 6 | P a g e L a s t U p d a t e d M a y 2 6 , 2 0 1 5
4. Calculate the concentration in molality of calcium phosphate in a solution containing
250.0 grams of pure water when the freezing point is -8.5o C.
5. Complete this sentence: When solid sodium chloride is poured into a glass of water
containing ice cubes, the temperature of the water will __________________________.
6. Explain the reasoning behind your answer to question 5.
EQUIPMENT:
 Paper
 Pencil/pen
 Computer with Internet access (for the remote laboratory and for data analysis)
 A spreadsheet program such as Excel
PREPARING FOR THIS NANSLO LAB ACTIVITY:
Readand understandthe informationbelowbefore youproceedwiththe lab!
Scheduling an Appointment Using the NANSLO Scheduling System
Your instructor has reserved a block of time through the NANSLO Scheduling System for you to
complete this activity. For more information on how to set up a time to access this NANSLO lab
activity, see
www.wiche.edu/nanslo/scheduling-software.
Students Accessing a NANSLO Lab Activity for the First Time
For those accessing a NANSLO laboratory for the first time, you may need to install software on
your computer to access the NANSLO lab activity. Use this link for detailed instructions on
steps to complete prior to accessing your assigned NANSLO lab activity –
www.wiche.edu/nanslo/lab-tutorials.
Video Tutorial for RWSL: A short video demonstrating how to use the Remote Web-based
Science Lab (RWSL) control panel for the titration apparatus can be viewed at
http://www.wiche.edu/nanslo/lab-tutorials#titration.
NOTE: Disregard the conference number in this video tutorial.
AS SOON AS YOU CONNECT TO THE RWSL CONTROL PANEL: Click on the yellow button at the
bottom of the screen (you may need to scroll down to see it). Follow the directions on the pop
up window to join the voice conference and talk to your group and the Lab Technician.

8. 7 | P a g e L a s t U p d a t e d M a y 2 6 , 2 0 1 5
EXPERIMENTAL PROCEDURE:
Read and understand these instructions BEFORE starting the actual lab procedure and collecting
data. Feel free to “play around” a little bit and explore the capabilities of the equipment before
you start the actual procedure.
Once you have logged onto the remote lab, you will perform the following laboratory
procedures:
EXERCISE 1: Measuring Freezing Points of Various Solutions
1. Measure the temperature of the ice-water solution.
2. Add 100 mL of sucrose solution to the first cup of ice and measure the temperature.
3. Repeat step 2 for the second cup of ice and measure the temperature.
4. Add 100.0 mL of sodium chloride to the third cup of ice and measure the temperature.
5. Repeat step 4 for the second cup of ice and measure the temperature.
6. Return the temperature probe to the first cup (just ice water). As the Lab Technician to
dump some sodium chloride into the ice water. As the Lab Technician for the mass of
water and the mass of sodium chloride. Measure the temperature.
POST-LAB ANALYSIS
(Show all necessary calculations. Can be done offline if you run out of time)
1. If you had added more or less glucose and sodium chloride solutions in steps 2 – 5 of the
Experimental Procedure, would it have made a difference in the freezing points? Why
or why not?
2. When you measure the temperature of water with some ice in it, and if you measure
the temperature very close to where the ice cubes are, is that measuring the “freezing
point”? Why or why not?
3. Calculate the concentration in motality of the sucrose solution and estimate the error in
your result: ___________________molal +/- _________________
4. Calcuate the concentration in molality of the sodium chloride solution and
estimate the error in our result: ____________molal +/- _______________
5. What happened in step 6 of the exercise? Did it match your hypothesis from the pre-
lab? Explain.
6. Calculate how much sodium chloride actually dissolved in step 6 of the exercise.

9. 8 | P a g e L a s t U p d a t e d M a y 2 6 , 2 0 1 5
For more information about NANSLO, visit www.wiche.edu/nanslo.
All material produced subject to:
Creative Commons Attribution 3.0 United States License 3
This product was funded by a grant awarded by the U.S.
Department of Labor’s Employment and Training Administration.
The product was created by the grantee and does not necessarily
reflect the official position of the U.S. Department of Labor. The
Department of Labor makes no guarantees, warranties, or
assurances of any kind, express or implied, with respect to such
information, including any information on linked sites and
including, but not limited to, accuracy of the information or its
completeness, timeliness, usefulness, adequacy, continued
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