How can the ocean be colder than 0 degrees C, the temperature at which water freezes? As it turns out, the concentration of the particles (in this case, the ions from the salt) in ocean water lowers the temperature at which the saltwater will freeze. Students will learn how ocean water freezes at a lower temperature than freshwater by conducting an experiment to determine the temperature of a freezer. This experiment can be performed in the classroom or at home by students in honors and AP level chemistry or can be easily modified to use in any physical science class.
Students will learn:
- To make saltwater (NaCl) solutions of varying concentrations, including how to calculate the molality of the solution.
- To determine the freezing point depression of the saltwater solutions.
- To estimate the temperature of a freezer by observing the behavior of various concentrations of saltwater.
The concept of the freezing point depression of saltwater is a perfect application of colligative properties and can be used as an opportunity to introduce students to the extremely cold environment of arctic and antarctic ocean waters. According to NOAA, arctic ocean water freezes at -1.9 degrees C (http://oceanservice.noaa.gov/facts/oceanfreeze.html) due to the salt dissolved in it. More concentrated saltwater bodies of water (such as the Great Salt Lake in Utah) would require even colder temperatures to freeze.
If you are teaching an advanced chemistry class, prior to this experiment, the background chemistry concepts (see attached) should be covered for your students to perform the calculations for determining the freezing point depression of saltwater solution.
If you are teaching an earlier level science class, refer to the Freezing Temperatures for the Various Saltwater Solutions chart (see attached background chemistry information) to determine the freezing point of each of the successively more dilute saltwater solutions obtained in the procedure. Your students can skip Procedural steps 7 & 8.
- Using masking tape, label the four household glasses "A", "B", "C", and "D". Save these for step 3.
- Dissolve one tablespoon (20 g) of table salt in exactly ¼ cup (59 mL = 0.059 kg) of tap water in each of the glasses labeled A, B, C, and D. Stir very well.
- Set glass A aside. Glass A now contains 20 g NaCl and 0.059 kg of water.
- Dilute the solution in glass B with an additional 0.104 cups of water (1 tablespoon and 2 teaspoons). Stir well. Glass B now contains 20 g NaCl and 0.084 kg of water.
- Dilute the solution in glass C with an additional 0.25 cups of water (1/4 cup). Stir well. Glass C now contains 20 g NaCl and 0.118 kg of water.
- Dilute the solution in glass D with an additional 0.75 cups of water (3/4 cup). Stir well. Glass D now contains 20 g NaCl and 0.236 kg of water.
- Calculate the molality, m, of each of the saltwater solutions in glasses A, B, C, and D using the formula: molality, m = # of moles NaCl / # of kg water
- Calculate the freezing point depression of the saltwater solutions in glasses A, B, C, and D using the formula: deltaT = - (Kf) (m) (i) = (1.86)(m)(2). This is also the freezing point of the saltwater solution in degrees C. If you wish to see this freezing point in °F, convert using the formula: °F = (1.8 degrees C) + 32.
- With masking tape, label five of the cube slots of the ice cube tray (or the 5 small bathroom cups) as follows "A", "B", "C", "D", and "Control".
- Pour equal amounts of the solutions from each of the labeled glasses into the appropriate ice cube slot (or small cup). Do not fill these above 2/3 full. Into the "Control" ice cube slot (or small cup), add tap water.
- Place the ice cube tray (or small cups) into the freezer in an area that can be easily observed. Be careful not to mix or spill the solutions.
- Every 30 minutes for 3 hours, observe the freezing process. Use a fork (or toothpick) to determine the state of each solution. Rinse the fork between testing each sample. Do not cross-contaminate the solutions with the fork. Record the state of each solution at every observation time.
Students could research the freezing temperatures of saltwater bodies near them or of how some animals and insects use this freezing point depression to keep their blood from freezing in very cold temperatures.
The teacher can use the student lab report to assess student understanding.
This is an original lesson by Mark Paricio, mparicio [at] cherrycreekschools.org, adapted from his original take-home-experiment: "How Cold is my Freezer?"
Standards9-12 Content Standard A: Science As Inquiry: Content Standard B: Physical Science: a. Abilities necessary to do scientific inquiry a. Structure of atoms b. Structure and properties of matter c. Chemical reactions
Colorado Science Standards: 2. Matter has definite structure that determines characteristic physical and chemical properties Students can: b. Gather, analyze and interpret data on chemical and physical properties of elements such as density, melting point, boiling point, and conductivity (DOK 1-2).
|Download Complete Lesson (PDF - 256 KB)256.25 KB||256.25 KB|
|Download Background Chemistry Concepts (Word - 13 KB)13.78 KB||13.78 KB|
|Download Worksheet and Questions (Word -14 KB)14.46 KB||14.46 KB|
This program is supported by the National Science Foundation. Any opinions, findings, and conclusions or recommendations expressed by this program are those of the PIs and coordinating team, and do not necessarily reflect the views of the National Science Foundation.