measuring the freezing point depression of a known amount in an aqueous solution. Freezing point depression is a colligative property of solutions. There are three other properties‚ which are boiling point elevation‚ vapor pressure depression‚ and osmotic pressure. Colligative properties of a solution depend on the amount of solute and solvent molecules and not the specific properties of the molecules. The temperature at which the solvent starts to freeze will be specified as the freezing point of the solution
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Freezing Point Depression Purpose: The purpose of this lab is to demonstrate freezing point depression by dissolving salt into two liquids and monitoring temperature. Materials: test tube‚ Thermometer‚ 10 mL graduated cylinder‚ 2 micropipettes‚ Styrofoam cups‚ 4 pieces plastic wrap‚ 70% ethyl rubbing alcohol‚ 91% isopropyl rubbing alcohol‚ ice‚ distilled water‚ rock salt Procedure: Using the graduated cylinder‚ measure 2 mL of alcohol and pour it into the test tube. Add 10 mL of
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Ben Quinones AP Chem Mr. Perry 25 January 2013 Molar Mass by Freezing Point Depression Conclusion: My Lab unsuccessfully found the molar mass of the unknown given to us in the lab. We were tasked with finding the molar mass of an unknown compound using the colligative property of Freezing Point Depression. The way we did this was first finding the temperature at which ice crystals form for just regular BHT. Luckily thanks to our TA we were given temperature probes so we could pinpoint exact
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Molar Mass by Freezing Point Depression November 28‚ 2012 NAME Lab partner- Purpose: To determine the molar mass of an unknown substance by measuring the freezing point depression of a solution of an unknown substance and BHT. Equipment: Test tube‚ 18*150 millimeters Wire stirrer Weighing dish Timer‚ seconds Chemicals: 2‚ 6-Di-tert-butyl-4-methylphenol‚ BHT‚ 16 grams Cetyl alcohol‚ CH3(CH2)14CH2OH‚ 1 gram Unknown substance
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be the freezing point depression as an example of a colligative property. Every liquid has a freezing point: the temperature at which a liquid undergoes a phase change from liquid to solid. When solutes are added to a liquid‚ forming a solution‚ the solute molecules disrupt the formation of crystals of the solvent. That disruption in the freezing process results in a depression of the freezing point for the solution relative to the pure solvent. The amount of the freezing point depression can be
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properties are: freezing point of depression‚ boiling point elevation‚ vapor pressure lowering‚ and osmotic pressure.1 Colligative properties are present in everyday life‚ such as adding salt to a boiling pot of water. By adding salt to the water‚ the boiling point of elevation is raised and the boiling salt water will have a higher temperature compared to the temperature of boiling pure water.2 The colligative property that will be used in this experiment is the freezing point of depression‚ which can
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the quality of NaCl as a deicer. These experiments included testing the freezing point depression of NaCl in solution at two different concentrations‚ testing for the H of an aqueous NaCl solution‚ and combining NaCl with MgCl2 in an aqueous solution to test for freezing point depression. Through these various experiments we found NaCl to be the best deicer for our region due to its proficient freezing point depression and its cost efficiency. Introduction As scientists we were given the
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Colligative Properties The Physical Properties of Solutions Colligative Properties • There are 3 colligative or physical properties of solutions that you should know. They are Vapor pressure Boiling point elevation Freezing point depression Osmotic pressure is one you don’t need to worry about. 1. 2. 3. 4. Molality • Molality measures the moles of solute dissolved in the mass (kg) of solvent. • Molality normally expresses concentrations of colloids. • m = moles solute kg solvent
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ΔT1 = Kfm where Kf is a constant that depends on the specific solvent and m is the molality of the molecules or ions solute. Table 1 gives data for several common solvents. Table 1. Molal Freezing Point and Boiling Point Constants | Solvent | Formula | Freezing Point (°C) | Kf(°C/molal) | Boiling Point (°C) | Kb(°C/molal) | Water | H2O | 0.0 | 1.86 | 100.0 | 0.51 | Acetic acid | CH3COOH | 17.0 | 3.90 | 118.1 | 3.07 | Benzene | C6H6 | 5.5 | 4.90 | 80.2 | 2.53 | Chloroform | CHCl3 | –63
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of solutions that depend upon the ratio of the number of solute particles to the number of solvent molecules in a solution. Colligative properties include: 1. Relative lowering of vapor pressure 2. Elevation of boiling point 3. Depression of freezing point 4. Osmotic pressure Vapor Pressure The vapor pressure of a liquid is the pressure of a vapor in equilibrium with the liquid phase. The
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