Katrina EppsLab Partner: Jennifer CarterTim LittleCHE113-011February 17, 2014Freezing Point of Sugar and SaltIntroductionThe purpose of this lab was to determine the molality of sugar and substance saline by calculating the freezing point depression (freezing point depression is the effect of the lowering of the freezing point of a substance due to a greater amount of solute added to the solvent as the solute decreases the amount of pressure of vapor) when the sugar or salt substance is added as a solute to a solvent with known properties. The results of the experiment confirmed our hypothesis that the freezing point would decrease more in sugar than in salt solvent. “The following mathematical expression relating freezing point depression and molality has been developed: ΔTf=iKfm T is the temperature change from the original freezing point, is the van't Hoff factor, Kf is the freezing point depression constant of the solvent em is the molality of the solution. Molality is defined as the moles of solute per gram of solvent. Remember that we use molality instead of molarity because the mass of the solvent will not change with temperature.”(Lab Manual, 60)Procedure1. Wear glasses when entering the laboratory2. Get with lab partner3. Arrange the test tube rack with 6 test tubes placed in the rack4. Requires small and large graduated cylinder. These will be used to measure distilled water.5. A 200ml beaker and a 25ml beaker are required6. Lab Partner 1 should load the sugar into the spacecraft and weigh it (4x). Lab Partner 2 created Measurenet.7. Calibrate the temperature probe before starting tests.8. While lab partner 1 is still working with the sugar, lab partner 2 has to take the salt in the boat and weigh it (record it in the notebook) and also has to take some disti......in the center of the paper ..... .11 and 2.47613) was much lower than the temperature of the saline solution (38). Conclusion This lab was performed to provide another way to determine the molality and concentration of a sugar and salt solution. The method of providing this information was through the use of colligative properties and, more specifically, freezing point depression. When a solute is added to a solvent, the point at which the solution freezes is lower than the freezing point of the pure solvent alone. This temperature change is equal to the freezing point depression constant multiplied by the van't Hoff factor of the solute and the molality of the solution. Since molality is equal to moles of solute divided by solvent, moles of solute can be obtained experimentally by finding the temperature change and knowing the freezing point depression constant, the van't Hoff factor, and the solvent used.