# Freezing Point Depression: Why Don t Oceans Freeze? Teacher Version

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1 Freezing Point Depression: Why Don t Oceans Freeze? Teacher Version Freezing point depression describes the process where the temperature at which a liquid freezes is lowered by adding another compound. It depends only on the number of dissolved particles in solution. This is known as a colligative property. For example, water freezes at 0 C, but when a solute such as salt or sugar is added to a solvent (water), the freezing point decreases. In order to see the freezing point depression of saltwater and how it changes with varying amounts of solute concentration, you will use 5 cups with water and varying amounts of salt and measure each individual temperature. Then, using the volume of the water and the volume of the solute, you will find the concentration of the solution. In the second part of the lab, you will use two freezer bags to observe how readily water freezes when surrounded by saltwater. California Science Content Standards: 3. Conservation of Matter and Stoichiometry: The conservation of atoms in chemical reactions leads to the principles of conservation of matter and the ability to calculate the mass of products and reactants. 6. Solutions: Solutions are homogeneous mixtures of two or more substances. 6a. Students know the definitions of solute and solvent. 6c. Students know temperature, pressure, and surface area affect the dissolving process. 6d. Students know how to calculate the concentration of a solute in terms of grams per liter, molarity, parts per million, and percent composition. **6e. Students know the relationship between the molality of a solute in a solution and the solution's depressed freezing point or elevated boiling point. 7. Chemical Thermodynamics: Energy is exchanged or transformed in all chemical reactions and physical changes of matter. 7a. Students know how to describe temperature and heat flow in terms of the motion of molecules (or atoms). Key Concepts: A solution is a mixture composed of two or more substances. In a solution, the solute dissolves into another substance, referred to as the solvent. A solution s colligative properties refer to the number of dissolved particles contained in the solution and are not dependent on the identity of the solutes. A solution s concentration refers to the amount of solute mixed in with the solvent (e.g.10% saline solution). When water freezes, energy is released in the form of heat. This is why ice has a lower temperature than water. When ice melts, energy is absorbed, increasing the temperature. Materials (Part 1): 5 foam cups Water Ice Salt and sugar Thermometer 100mL graduated cylinder Measuring cup 1 tablespoon and teaspoon Access to the Periodic Table of Elements Stirring rod Strainer Graph paper (if available)

2 Materials (Part 2): 1 gallon freezer bag 1 quart freezer bag 1 cup Crushed ice Salt Gloves or towel Part 1 Measuring Freezing Points 1. Separate the table on the last page of the lab for use during the lab. 2. Set up 5 cups in a line in front of you. 3. Label the cups - 0mL of Salt, 10mL of Salt, 20mL of Salt, 30mL of Salt, and Sugar. 4. Fill the measuring cup to about 100mL of crushed ice. Slowly pour water into the cup until the ice/water mixture reaches 100mL. (If your measuring cup does not measure in ml, 100mL is a little less than half a cup.) Fill the first 4 salt cups with 100mL of ice/water. 5. Measure out each respective amount of salt, using tablespoons and teaspoons. Note: 1 teaspoon=5ml and 1 tablespoon=15ml. 6. Stir the amount of salt into each cup until the salt dissolves. Note: If the saltwater is not continually stirred, the salt will pile up at the bottom. Stir slowly to ensure salt dissolves. Also, for 30mL of solute, add the solute in portions. (Example: 10mL first and then 20mL later). Why does the 10mL of salt dissolve more readily than the 30mL of salt? How does the temperature of the solution affect the solubility of the solution? Both 10mL of salt and 30mL of salt when in solution with ice and water are saturated solutions, yet 10mL of salt dissolves more readily with ice water because it is a lesser amount that needs to dissolved. If the water were at a higher temperature, the salt would dissolve with much more ease; this is because at a higher temperature, the bonds of the salt break more easily. What other factors can you think of that might affect the solubility of the solution? The amount of stirring as well as pressure and surface area contribute to the solubility of the solution. 7. After you have stopped stirring, wait for the temperature to reach equilibrium. This temperature is the freezing point of the solution. Record the temperatures in Column B. How did the temperature change by increasing the amount of salt in the water? Answers vary based on student data, but the freezing point should decrease with the addition of more salt.

3 8. Using a strainer, strain the ice out of each cup. Measure the volume of the remaining liquid (salt water) using the graduated cylinder. Record the results in Column C. 9. Now, in the final foam cup, add 30mL of sugar solute into 100mL of cold water. Record the temperature below: Temperature: Student Answer How does the temperature obtained by sugar water compare to the temperature obtained when 30mL of salt were added to the same amount of water? The salt solute depresses the freezing point more than the sugar solute. Concept Questions Find the concentration of each solution. The concentration is the amount of solute mixed with an amount of solvent. What is the solute and solvent in our solutions? Salt is the solute and water is the solvent First find the mass of the salt in grams. To find the mass of the salt, follow the example below: Volume of Solute (ml) Density of Salt (g/ml) = Mass of Salt (g) The volume of salt can be found in Column A of the table and the density of salt is 2.2 g/ml so use the following equation to calculate the mass of salt for each cup. Column A Value x 2.2 g/ml = Mass of Salt (g) Record your answer in Column D. Next use the equation below to find the concentrations of each of the solutions. Mass of solute (g) Concentration of Salt Water = Volume of solvent (ml) Column C Value (g) Column D Value (ml) = Concentration (g/ml) Record your answers in Column E above.

4 Plot a Concentration vs. Freezing Temperature graph. Describe the relationship. Concentration is Column E in your table and Freezing Temperature is Column B. As the concentration increases the freezing temperature decreases. Freezing Temperature Column B Concentration Column E Do you notice any patterns in the freezing temperature as the concentration increases? As the molality increases the temperature decreases. What freezing temperature would you predict if 40 ml of salt was placed in the water? Based on the above graph the students should predict a temperature ~5 C colder then the temperature of the solution with 30mL of salt. Instructions for Part 2 1. Add crushed ice into the gallon freezer bag until the bag is ¼ full. Take the temperature. Record below: Temperature: Student Answer should be near 0 C 2. Add one cup of salt and ½ cup of water into the gallon freezer bag. 3. Squeeze out as much air as possible and close the gallon bag. 4. Mix until the ice has completely melted. The bag will get very cold so put on gloves or hold the bag in a towel to protect your hands. Rub your hands against the ice in order to melt the ice faster. Take the temperature. Record below. Temperature: Student Answer

5 How did the addition of salt change the freezing temperature? Is this similar to the first part of the lab? This part of the lab is similar in that the addition of salt depresses the freezing point. If the temperature is below 0 C, the freezing point of water, why is the saltwater not frozen? The salt water is not frozen because by adding a salt to water, the freezing point decreases, lowering to more than 0 C. 5. Open the quart-size freezer bag and pour 1 ounce (2 tablespoons) of water into it. 6. Close the quart-size bag and put it inside the gallon freezer bag. 7. Let it sit for one minute. 8. Remove the quart size bag. Describe your observations below: Various student observations will be given, however water in quart-sized bag should be frozen Concept Questions Is it possible to make the salt water colder and colder forever just by adding more salt? Why or why not? This is not possible. The freezing point of saturated salt water (i.e. there's no way to dissolve any more salt in it no matter how hard you tried), is degrees Celsius, which would also be the coldest temperature for a salt water solution. Why is the ocean able to maintain temperatures lower than 0 C without turning into ice? Small lakes and rivers often freeze due to harsh winter temperatures, but oceans never completely freeze due to their large quantity of salt. References: 1. Freezing Point Depression Lab: 2. Freezing Water in a Bag:

6 Results Table for Part 1 Column A Column B Column C Column D Column E Solute Freezing Temperature (Cº) Strained Water (ml) Mass of Salt (g) Concentration (g/ml) 0 ml salt 0 ºC 10 ml salt decreasing ~60-90mL g ~ g/ml 20 ml salt decreasing ~60-90mL 43.3 g ~ g/ml 30 ml salt decreasing ~60-90mL g ~ g/ml 30 ml sugar ~0- -5 ºC The values in the table are approximate. Students answers could vary greatly depending on experimental conditions. The temperatures will be decreasing values with the increased amounts of salt.

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