# EXPERIMENT 15 FREEZING POINT: A COLLIGATIVE PROPERTY OF SOLUTIONS

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1 EXPERIMENT 15 FREEZING POINT: A COLLIGATIVE PROPERTY OF SOLUTIONS INTRODUCTION Scientists seldom work alone today. Instead they work in teams on projects, sharing the labor of carrying out the experiments and of interpreting the results. In this experiment, your lab group will work together to collect and analyze data to determine the freezing points of a number of liquids, both pure solvent and solutions made from the solvent and several solutes. The freezing point data you and your lab partner collect will be combined with the data for your entire lab group, and your instructor will lead a discussion of what conclusions can be drawn from the data. Following this you will measure the freezing point of a solution containing an unknown solid. Using the information gathered above, you will determine the molar mass of the unknown solid. TECHNIQUE Determination of Freezing Points Using Cooling Curves A cooling curve for a liquid shows graphically how the temperature varies with time as the liquid is cooled in a constant-temperature bath. The liquid is contained in a test tube and is stirred continuously to maintain thermal homogeneity. The rate of cooling is determined mainly by two factors. The first is the difference in temperature between the liquid and the bath. This factor causes the cooling curve to become gradually less steep (smaller negative slope) as the liquid temperature approaches that of the bath, eventually becoming zero, yielding a horizontal line at the bath temperature. The second factor is the extent to which the liquid is insulated from the bath. This factor does not control the overall shape of the cooling curve, but it does affect how long the experiment takes. If the freezing point of the liquid is above the bath temperature, the cooling curve will not proceed in a smooth curve all the way to the bath temperature. It will instead show a discontinuity, i.e., a sudden decrease in slope, at the freezing point of the liquid. This slowing of the cooling occurs because the heat of fusion of the liquid is released as the liquid freezes, at least partially compensating for the heat being lost to the bath. It is occasionally observed that freezing does not begin immediately at the freezing point, but that supercooling occurs. When freezing does begin, the heat released will raise the temperature to the level that would have been observed in the absence of supercooling. Should supercooling occur in any of your samples, it will be obvious from the sudden, small rise in temperature after the supercooling dip in the cooling curve. Cooling curves for pure liquids differ from those for solutions. The temperature remains constant as a pure liquid freezes, so a flat, horizontal region is expected in the cooling curve. If the cooling is continued until all of the liquid has frozen, the temperature will then decrease further as the solid is cooled, until it finally reaches the temperature of the bath. For a solution, on the other hand, the temperature continues to decrease as freezing occurs, although at a lower rate. This occurs because it is pure solvent that is freezing out of the solution, leaving the liquid solution more and more concentrated, continually decreasing the freezing point. If cooling is continued until all of

2 the solution has frozen, the cooling curve will become steeper again, since no more heat of fusion is being released. It is important to note that it is the temperature at which the solution begins to freeze that is desired, since it is only there that the concentration is known. An experimental cooling curve for a pure liquid is shown in FIGURE 15-1 and for a solution in FIGURE Careful examination shows that a small supercooling dip occurred in both curves. It is also apparent that the T f = 6.52C T f = 3.35C Figure Cooling curve of a pure liquid. Figure Cooling curve of a solution. region after the onset of freezing in FIGURE 15-1 isn t quite horizontal. The temperature continued to decrease slightly as the solvent froze. This could mean that the solvent wasn t 100% pure. It might, however, be due simply to a cooling rate that was too high. The temperature remains constant as a pure liquid freezes only if the solid and liquid are always essentially in equilibrium with each other. This may not be the case if the cooling is too rapid or if the stirring is not adequate. The solvent must freeze rapidly enough to produce heat (heat of fusion) at the rate at which heat is lost to the bath, and the stirring must be rapid and thorough enough to keep the temperature uniform throughout the sample. The cooling curve in FIGURE 15-1 was followed much longer than necessary after the onset of freezing, in order to illustrate how the temperature drops quickly again after all of the liquid has frozen. Note how the freezing point, T f, is determined in each case. A line is drawn to extrapolate the behavior just after freezing began back through the supercooling dip to the curve just before freezing began. The intersection of the extrapolated line with this curve is taken as the freezing point. If supercooling were not observed, the freezing point would be taken to be the point where the slope changes abruptly.

3 OBJECTIVES to determine the freezing points of several liquids to combine and discuss your data with the other students on your network to prepare a solution of an unknown solute and measure its freezing point to determine the molar mass of the unknown solute from the freezing point EQUIPMENT NEEDED beakers (150 ml and 800 ml) ring stand and clamp Styrofoam cups (2) Kimwipe tissues medium test tube glass stirring rod temperature probe smaller test tube (supplied by stockroom) CHEMICALS NEEDED Note: Concentrations of solutions are expressed in units of molality. cyclohexane, C 6 H 12 naphthalene in cyclohexane (0.040 m, m, m, m) biphenyl in cyclohexane (0.040 m, m, m, m) PROCEDURE A. Freezing Point Determination of Known Solutions and/or Pure Solvents Each pair of students will be assigned at least three test liquids from the front of the lab room. Your instructor will give you an assignment sheet. One of the liquids you will investigate will be pure solvent (cyclohexane); the others will be solutions of a solute dissolved in cyclohexane. You will determine the freezing point of each of the liquids you have been assigned. Calibration of the Temperature Probe and Setup of Workstation Display Press MAIN MENU on the workstation, press the function key for TEMPERATURE, and then the function key for TEMPERATURE V TIME. Fill your 800-mL beaker with ice. Fill a Styrofoam cup approximately threequarters full with ice and add enough distilled water to barely cover the ice. This ice/water mixture will be at 0.0 C. Press CALIBRATE and place the temperature probe in the ice water, using the temperature probe to continuously stir the ice water for at least two minutes. Follow the instructions on the display for the calibration of the temperature probe. Since data from all of the students on your network will be combined in this exercise, it is particularly important to do a good job calibrating the temperature probe. Calibration errors will lead directly to disagreement among the values obtained by various group members. When you have finished calibrating the temperature probe, remove it from the ice bath and carefully dry it. This is necessary in order to avoid contaminating one of the liquids to be studied by introducing water. Press SETUP and set the graph limits for your workstation display. Set the minimum and maximum temperatures at 0 C and 10 C, respectively, and set the maximum time at 900 seconds. Press DISPLAY to accept the graph limits and begin monitoring the temperature.

4 Cooling Curve Measurements Measuring a cooling curve experimentally would seem to be a very simple matter. However, in order to achieve results of comparable quality to those in FIGURES 15-1 and 15-2, you must pay surprisingly close attention to various details. Lack of careful technique in following the instructions below will be immediately apparent in your cooling curves. Place the Styrofoam cup you used in the temperature probe calibration inside another Styrofoam cup. Use this nested pair of cups as the constant-temperature bath for each cooling curve measurement. Before each experiment fill the cup to the top with ice and add (or pour out) just enough water to bring its level to within a centimeter or so of the top. You need to have ice all the way to the bottom of the cup. Be sure to stir the ice-water bath thoroughly before each experiment. Perform the cooling curve experiment on the pure solvent first. Attach the clamp to the ring stand and clamp a medium (18 mm 150 mm) test tube near its open end. Obtain a KimWipe, roll it into a ball, and place it in the medium test tube. Fill a smaller (15 mm x 125 mm) test tube (not in your drawer obtain from the front bench) ~1/4 full (no more!) with cyclohexane and place it inside the medium test tube. The KimWipe will hold the smaller test tube in the center of the larger one in such a way that they do not actually touch. The reason for this rather strange-sounding arrangement is that it conveniently limits the rate at which heat can be transferred from the smaller test tube to the bath around the larger one. If the cooling occurs too quickly, in addition to the resulting problems discussed above, the temperature probe may not be able to keep up and accurately show what is happening. The result would be a smearing out of the details around the onset of freezing, and that would make it difficult or impossible to determine just where freezing begins. Loosen the clamp on the ring stand and slide it down to lower the test tubes into the ice bath in the Styrofoam cups. Wiggle the cups around as you insert the tube until it rests on the bottom. Do not press down too hard, though, or you will break through the bottom of the cup. Insert the temperature probe into the liquid in the smaller test tube and begin stirring the liquid. The best stirring technique is a regular, but gentle, up-and-down motion, about twice per second, in which the probe is raised about two centimeters and then returned to the bottom of the tube. It is important that you keep stirring smoothly throughout the course of the measurements in order to maintain temperature homogeneity. While you stir, monitor the temperature on the workstation screen. When it reaches 10 C, press START/STOP to begin collecting data. Continue stirring and monitor the plot of temperature vs. time on the workstation screen. After freezing begins, as seen in the a change in slope on the plot or from the numbers themselves, continue collecting data for about a minute more, then remove the smaller test tube from the larger test tube (do not press START/STOP yet). When the liquid in the test tube has warmed up to ~10ºC, place it back in the larger test tube and allow the liquid to cool down to its freezing point. In this manner, you will have two cooling curve experiments plotted on the workstation screen. When the second experiment is complete, press START/STOP to stop collecting data. Remove the smaller test tube from the ice bath (you can leave the larger one in the ice bath), remove the probe from the test tube, and wipe it off. (If the probe becomes stuck in the frozen liquid, warm the tube with your hand until the liquid melts and you can remove the probe.) Dispose of the liquid in the non-halogenated liquid organic waste container. Print your temperature versus time plot. To do this, press FILE OPTIONS, press the function key for PRINT standard, and enter the number of copies to print, probably 2 one for you and one for your lab partner. As soon

6 2. Fill out the report sheet table summarizing the results of your freezing point measurements. Part B. Molar Mass of Unknown Solute 1. Determine the freezing point, T f, from the cooling curve of the solution containing your unknown solute. Show how you determined the freezing point, and be sure the graph is given an appropriate title. 2. Use the freezing point of your unknown solution and the equation of the best fit line drawn through the group plot data to determine the molality of your solution. Show how you obtained this value. 3. Calculate the mass of cyclohexane used in the experiment. Use the mass of cyclohexane and the solution molality determined above to calculate the molar mass of your unknown solute. Recall that molality is calculated by: moles solute molality = kg of solvent (15-1) Record this information on the REPORT SHEET. Show all calculations. DISCUSSION Write a paragraph or two briefly describing the results and conclusions of the group experiment involving the freezing points of the known solutions. Be sure to cover the following topics: 1. How is the freezing point determined from a cooling curve graph? 2. What is the effect of the concentration of solute (expressed in molality, m) on the freezing point of the solution? 3. What is the effect of the chemical identity of the solute on the slope of the concentration vs. freezing point curve? 4. Explain how the data support the assertion that freezing point depression is a colligative property.

7 EXPERIMENT 15 REPORT SHEET Name: Date: Partner: PART A. FREEZING POINTS OF KNOWN SOLUTIONS concentration solute freezing point PART B. MOLAR MASS OF UNKNOWN SOLUTE Unknown Number of Solute Mass of Solute Volume of Cyclohexane Density of Cyclohexane Mass of Cyclohexane, kg calculation:

8 Freezing Point of Solution Concentration of Solution (from freezing point curve) Moles of Solute calculation: Molar Mass of Unknown calculation:

9 Procedure considerations Lab Notes Experiment 15 Freezing Point: A Colligative Property of Solutions Part A: You should perform three freezing point experiments: one with a pure solvent, two with solutions. Your assigned liquids are listed on the last page. Measure the freezing point of the pure liquid first. You should be able to do two cooling curve trials for a liquid without having to reset the workstation screen. Do not press 'Start/Stop' until after the second time the liquid has frozen. You will be following a timetable during this experiment in order to have a group discussion of the Part A data. The timetable will be as follows: First two hours Collect freezing point data for Part A; analyze curves; enter data on computer At 2 hour mark After discussion TA leads group discussion of compiled data Complete Part B Be sure to take notes during this discussion! There will be topics discussed that will need to be included in your lab report. If you have completed Part A before the discussion you may begin Part B by preparing your unknown solution. You may perform the cooling curve trials for Part B if you are ready do so before the discussion; however, you should stop what you are doing when it is time for the group discussion. Helpful Hints: The two most important points to remember in this experiment are stir the solution or solvent continually and make sure the ice bath is sufficiently cold. The ice bath should be at least 3/4 filed with ice for each trial. Stir the ice water briefly before each trial to ensure that the temperature of the ice bath is relatively uniform. Submerge the test tube in the ice bath as far as possible.

10 Freezing Point Liquid Assignments Station # Liquid Assignment 1, 9 1) Cyclohexane 2) 0.04 m biphenyl in cyclohexane 3) 0.16 m naphthalene in cyclohexane 2, 10 1) Cyclohexane 2) 0.08 m biphenyl in cyclohexane 3) 0.12 m naphthalene in cyclohexane 3, 11 1) Cyclohexane 2) 0.12 m biphenyl in cyclohexane 3) 0.08 m naphthalene in cyclohexane 4, 12 1) Cyclohexane 2) 0.16 m biphenyl in cyclohexane 3) 0.04 m naphthalene in cyclohexane Station # Liquid Assignment 5 1) Cyclohexane 2) 0.04 m biphenyl in cyclohexane 3) 0.16 m naphthalene in cyclohexane 6 1) Cyclohexane 2) 0.08 m biphenyl in cyclohexane 3) 0.12 m naphthalene in cyclohexane 7 1) Cyclohexane 2) 0.12 m biphenyl in cyclohexane 3) 0.08 m naphthalene in cyclohexane 8 1) Cyclohexane 2) 0.16 m biphenyl in cyclohexane 3) 0.04 m naphthalene in cyclohexane

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