Colligative Properties Name: _____________________________________ Page 1 of 2 Colligative Properties Lab – Freezing Point Depression & Boiling Point Elevation Introduction The physical properties of solutions that depend on the number of dissolved solute particles and not their specific type are known as colligative properties. These include freezing point depression, osmotic pressure, and boiling point elevation. In this lab, freezing point depression and boiling point elevation will be investigated. Purpose: What is the point of completing this lab? _______________________________________________ ________________________________________________________________________________________ Materials/Apparatus: List what you see on the virtual lab bench. Procedure: 1. Go to simulation lab below. 2. Scroll to the bottom of the page to the section Solutions – click on the Freezing-Point Depression experiment 3. Molar Mass Determination by Freezing Point Depression Experiment #1, choose the following options: cold bath (click on the switch), and 100g of distilled H2O, click start. Record your data in the table. Experiment #2, choose cold water bath, 100g H2O, and 2.0g of sucrose (C12H22O11), click start. Record your data. Experiment #3, choose cold water bath, 100 g benzene. Click start. Record your data. Experiment #4, choose cold water bath, 100 g benzene, and 4.0g of CaCl2, click start. Record your data. Experiment #5, choose cold water bath, add 100 g ethyl ether. Click start. Record data Experiment #6, choose cold water bath, ,add 100 g ethyl ether and 2.0 g of NaCl. Record your data. Experiment 1 – pure H2O Freezing point 2- 100 gH2O & 2.0 g C12H22O11 3- 100 g benzene 4- 100 g benzene& 4.0 g CaCl2 5- 100g ethyl ether 6- 100 g ethyl ether & 2.0 g NaCl Lab data 1. Make a data table showing the FP of the pure solvent, the FP of the solution. The Kf of each solvent and ΔT of each solution. 2. Determine Molar Mass of the solute in each solution. Figure that out! You will need to include a data table stating FP of pure solvent, FP of solution. Kf of each solvent. ΔT for each solution. Colligative Properties Name: _____________________________________ Page 2 of 2 Conclusion Questions 1. Why is a molality concentration scale used in the context of colligative properties and not the more common concentration scale, molarity? 2. Assume that you have a solution of an unknown solute in cyclohexane. If the solution has a freezing point depression of 9.50 0C, what is the molality of this solution? (The freezing point depression constant for cyclohexane (Kf) is 20.4 0C/m). 3. Cyclohexanol, C6H11OH, is sometimes used as the solvent in molecular weight determination by freezing point depression. If 0.253 g of benzoic acid, C6H5COOH, dissolved in 12.45 g of cyclohexanol, lowered the freezing point of pure cyclohexanol by 6.55 0C, what is the molal freezing point constant (Kf) of this solvent? 4. What is supercooling? How can it be minimized? 5. Distinguish between non-volatile and volatile substances. Give two examples of each. 6. Write a conclusion paragraph about how this lab re-enforces the concepts of colligative properties and any improvements/problems with the lab.