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Exp 12A: A Molar Mass from Freezing-Point Depression

Exp 12A: A Molar Mass from Freezing-Point Depression. Purpose Determine the freezing-point depression in a solution when a solute is added to a pure solvent Use the freezing-point depression of the solution to determine the molar mass of the solute

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Exp 12A: A Molar Mass from Freezing-Point Depression

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  1. Exp 12A: A Molar Mass from Freezing-Point Depression Purpose • Determine the freezing-point depression in a solution when a solute is added to a pure solvent • Use the freezing-point depression of the solution to determine the molar mass of the solute • Detemine the molecular formula of the solute based on the given empirical formula and the calculated molar mass • See also: Silberberg, Chapter 13, pp. 515-520, and Sample problems 13.7 and 13.8

  2. Exp 12A: A Molar Mass from Freezing-Point Depression • The melting point is the temperature at which a solid changes to a liquid • The freezing point is the temperature at which a liquid changes to a solid • The freezing point of pure water is 0°C • The melting point can be depressed by adding a solute such as a salt. • Use of ordinary salt (sodium chloride, NaCl) on icy roads in the winter helps to melt the ice from the roads by lowering the melting point of the ice. • Making ice-cream by using a water-salt mixture to lower the freezing point of the solution • A solution (solvent + solute) typically has a measurably lower melting point than the pure solvent

  3. Exp 12A: A Molar Mass from Freezing-Point Depression • The freezing point depression ΔTf is a colligative property of the solution • properties that depend on the concentration of solute molecules or ions, but not upon the identity of the solute • they include freezing point depression, boiling point elevation, vapor pressure lowering, and osmotic pressure • Example • ethylene glycol (C2H6O2) in automobile cooling systems • ethylene glycol (antifreeze) protects against freezing by lowering the freezing point and permits a higher operating temperature by raising the boiling point

  4. Coolant Pure Water 50/50C2H6O2/H2O 70/30C2H6O2/H2O Freezing Point 0°C/32°F -37°C/-35°F -55°C/-67°F Boiling Point 100°C/212°F 106°C/223°F 113°C/235°F Exp 12A: A Molar Mass from Freezing-Point Depression

  5. Solvent Formula Melting Point (°C) Boiling Point (°C) Kf(°C/m) Kb(°C/m) Water H2O 0.000 100.000 1.858 0.521 Acetic acid HC2H3O2 16.60 118.5 3.59 3.08 Benzene C6H6 5.455 80.2 5.065 2.61 Camphor C10H16O 179.5 ... 40 ... Carbon disulfide CS2 ... 46.3 ... 2.40 Cyclohexane C6H12 6.55 80.74 20.5 2.79 Ethanol C2H5OH ... 78.3 ... 1.07 Freezing Point Depression and Boiling Point Elevation of Some Solvents

  6. Exp 12A: A Molar Mass from Freezing-Point Depression • For dilute solutions freezing-point depression is found to be proportional to the molal concentration cm of the solution: • ΔTf = Kf cm where Kf is called the freezing-point-depression constant • Kf (cyclohexane) = 20.5oC/m • Molality (m) equals the number of moles of a given substance per kilogram of solvent (mol/kg) • it does not change with the temperature, as it deals with the mass of solvent rather than the volume of solution  molality of a solution is always constant irrespective of the physical conditions like temperature and pressure

  7. Exp 12A: A Molar Mass from Freezing-Point Depression - Experimental Part A: Measuring the freezing point of cyclohexane • Pipet exactly 20.0 ml cyclohexane in a large test tube. Close immediately • Calculate mass of cyclohexane • d = 0.779 g/ml • 20.0 ml = 20.0 ml x 0.779 g/ml = 15.58 g = 15.6 g • Record volume and calculated mass on your worksheet

  8. Exp 12A: A Molar Mass from Freezing-Point Depression - Experimental Part A: Measuring the freezing point of cyclohexane • Place the test tube with cylcohexane in a beaker with crushed ice and water • Stir gently, but constantly • When the temperature gets close to the freezing point of cyclohexane (melting point = 6.6oC), take temperature readings every 15 sec. This will take 10-15 min • Record the temperature change to the nearest 0.1oC. Stop the experiment once all cyclohexane is frozen and the temperature decreases further. • Allow cyclohexane to melt completely. • Repeat the freezing point determination • Plot the data, determine the freezing point in each case, and calculate the mean freezing point

  9. Exp 12A: A Molar Mass from Freezing-Point Depression - Experimental Part B: Measuring the freezing point of solutions • Weigh 0.24 - 0.25 g of the solute on weighing paper (sample 1). Determine the mass exactly (record in 4 decimals) • Weigh 0.10 - 0.11 g of solute on a 2nd piece of weighing paper (sample 2). Weigh in 4 decimals • Transfer sample 1 to the solvent in freezing point depression apparatus • Stir until the solute is completely dissolved. All of the solute must be dissolved • Stir gently but constantly and cool the solution as before • Determine the temperature as described under (A) until the entire solution is frozen • Remove the apparatus and allow the frozen solution to melt completely. • Graph your data! • How do your data look?

  10. Exp 12A: A Molar Mass from Freezing-Point Depression - Experimental Part B: Measuring the freezing point of solutions • Add sample 2 to the solution containing sample 1 and repeat the freezing process • Plot data for both experiments • Calculate the change in freezing point, DTf • Calculate the molal mass of the solute from each DTf. Mind the significant figures • Obtain the mean molar mass • Share data with the rest of the class • Calculate the molecular formula of the solute from the grand average and the empirical formula (C3H2Cl)

  11. Exp 12A: A Molar Mass from Freezing-Point Depression - Calculations Prelab Problem #3 • a 0.2436-g sample of an unknown substance was dissolved in 20.0 mL cyclohexane. • The density of cyclohxane = 0.779 g/mL. • The freezing point depression was 2.5oC. • Kf= 20.5oC/m • Calculate the molar mass of the unknown substance.

  12. Exp 12A: A Molar Mass from Freezing-Point Depression - Calculations Prelab Problem #3 Solution • ΔTf = Kf cm = 2.5oC • cm=ΔTf / Kf = 2.5oC / 20.5oC/m = 0.12 m = 0.12 mol solute/kg solvent • Convert molality to mols of solute • cm= 0.12 m = 0.12 mol/kg = = (0.12 mol solute/kg solvent)x (20.0 mL solvent x 0.779 g/mL) x (1 kg solvent/1000 g solvent) = 1.9 x 10-3 mol solute • molar mass = 0.2436 g solute/1.9 x 10-3 mol solute = 1.3 x 102 g/mol

  13. Exp 12A: A Molar Mass from Freezing-Point Depression - Calculations Freezing Point of Cyclohexane • Volume of cyclohexane _____ mL • Mass of cylohexane _____ mL x 0.779 g/mL = ____ g = ____ kg • Mean freezing point ____ o C Sample 1 (adding 1st amount of solute) • Freezing point ____ o C • Change DTf. ____ o C • Molal concentration cm = DTf./Kf = ____ m (mol/kg) • Molar concentration Mm = DTf./Kf (mol/kg) x volume (mL) x density (g/mL) x 1 kg/103 g = _____ mol • Molar mass = ___ g solute / ___ mol = g/mol

  14. Exp 12A: A Molar Mass from Freezing-Point Depression - Calculations Sample 2 (adding 2st amount of solute) • Freezing point ____ o C • Change DTf. ____ o C • Molal concentration cm = DTf./Kf = ____ m (mol/kg) • Molar concentration Mm = DTf./Kf (mol/kg) x volume (mL) x density (g/mL) x 1 kg/103 g = _____ mol • Molar mass = ___ g solute / ___ mol = ____ g/mol

  15. Exp 12A: A Molar Mass from Freezing-Point Depression - Calculations Determining molecular formula • Empirical formula for the solute: C3H2Cl • Formula weight = (3 x 12.01) + (2 x 1.008) + 35.45 = 73.50 g/mol • Molar mass = _____ g/mol • Formula units = (_____ g/mol)/73.50 g/mol = ___ (needs to be (close to) a whole number) • Molecular formula = (C3H2Cl) x (whole number)

  16. This Thursday • Exp. 12A: Postlab • Exp. 13: Rate of an Iodine Clock Reaction • Prelab preparations and • Prelab assignment

  17. Phase Diagram of Solvent and Solution

  18. Exp 12A: A Molar Mass from Freezing- Point Depression Molarity • molarity (M) equals the number of moles of a given substance per liter of solution (mol/L) • measurement of the absolute number of particles in a solution, irrespective of their weight and volume Molality • molality (m) equals the number of moles of a given substance per kilogram of solvent (mol/kg) • it does not change with the temperature, as it deals with the mass of solvent rather than the volume of solution  molality of a solution is always constant irrespective of the physical conditions like temperature and pressure

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