Week 14/Tu: Lecture Units 33 & 34
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1 Week 14/Tu: Lecture Units 33 & 34 Exam 3 Unit 33: Colligative Properties -- Vapor pressure of solutions -- Freezing, boiling of solutions -- Osmotic pressure Unit 34: Introduction to Equilibria -- Rate of reaction, Kinetics -- Reaction pathway -- Forward / Reverse Rxns. Unit 35: Equilibrium Constants Issues: Exam 3 results Homework Set 10 due on 08:00AM
2 Week 14/Tu: Exam Results Number of Students Number of Students CEM 141 Fall 2o12 Exam Score Number of Students CEM 141 Fall 2o12 Exam Score CEM 141 Fall 2o12 Exam Score Exam 1 Exam 2 Exam 3 Count Mean Median Mode SD Range Minimum Maximum Grade Point Estimator
3 Week 14/Tu: Final Exam Info The final exam is a common final and has been scheduled for Thursday, December 13th 7:45-9:45AM The exam will have < 40 questions, cumulative, for a total of 250 pts. There will be an alternate final exam for anyone who has EITHER: 1) another final scheduled at the same time as our final OR 2) three or more finals on Thursday (i.e., two others plus our final) The alternate exam will be given the day before (Wed. at 10am) A sign-up sheet for the alternate will be available next week.
4 Week 14/Th: Vapor Pressure of a Solution -1- Recall every liquid has a vapor pressure that depends on T. A solution will also have a vapor pressure. Constant T Pressure P o (B) 0 1 Χ Black However, the vapor pressure of solution will be lower according to the amount of other material.
5 Week 14/Th: Vapor Pressure of a Solution -1- Recall every liquid has a vapor pressure that depends on T. A solution of two liquids will have partial pressures. Constant T P o (R) Pressure P o (B) 0 1 Χ Red Χ Black
6 Week 14/Th: Vapor Pressure of a Solution -1- Recall every liquid has a vapor pressure that depends on T. A solution of two liquids will have partial pressures. Constant T P o (R) P total Pressure P o (B) 0 1 Χ Black Recall that the mole fractions add-up: Χ Black + X Red = 1 X red = 1 - Χ Black
7 Week 14/Th: Vapor Pressure of a Solution -2- Recall every liquid has a vapor pressure that depends on T. A solution with a non-volatile will also have a vapor pressure. P=1 Part of the phase diagram, Constant X (mole fraction) T NB Since the vapor pressure of a solution is lower than that of the pure liquid, it will require a higher temperature to reach a vapor pressure of one atm (or boil).
8 Week 14/Th: Phase Diagram for Solution Similar to the boiling point elevation, the freezing point of the solution will be depressed relative to the pure liquid. Note that all of the components in solution affect FP, BP. ΔT ( i is called the van t Hoff factor) FP = K FP * m total * i K FP water = K/molal NaCl i = 2 KNO 3 2 Mg(NO 3 ) 2 3 Ca 3 (PO 4 ) 2 5 HCl 2 CH 3 CO 2 H 1 Solution (cartoon)
9 Week 14/Tu: Practical Problem on the Horizon Select Brand Ice Melter is NaCl Pellets of Fire are CaCl 2 Table sugar is C 12 H 22 O 11 Solute Solubility* Molar Mass Molarity particles ΔT (g/ml) (g/mol) (mol/l) i approx.** NaCl K CaCl K Sugar K * In cold water ** using M, need density to get m
10 Week 14/Tu: Example Problem in Notes When 1.0 mole of magnesium acetate was dissolved in water, the boiling point increased by 6.0 o to o C. How much water was used to make this solution? K BP (water) = K/molal ΔT = K BP * m * i 6.0 K = 0.50 K/molal * molality * 3 & molal = moles/kg of water 6.0 K = 0.50K/molal * 1.0 moles / kg of water * 3 that s: Mg(CH 3 CO 2 ) 2 Molar Mass not needed, but what is i? kg of water = 1.0 mole * (0.50 K/molal * 3) / 6.0K = 0.25
11 Week 14/Tu: Demo Supersaturated NaCH 3 CO 2
12 Week 14/Tu: Basis of Osmotic Pressure One beaker with an aqueous solution, water mole fraction, X H2O vapor pressure P = X H2O P o Another beaker with pure water vapor pressure, P o P o P = x H2O P o Put both under a bell jar, what happens?
13 Week 14/Tu: Natural Osmosis Plants and trees in particular rely on osmotic pressure to move water from the roots to the leaves. Trees create a sugar solution which is more concentrated than the ground water. Sugars (solute) Sap (solution) Water (solvent)
14 Week 14/Tu: Osmotic Pressure Osmotic pressure is the result of a drive to form dilute solutions (generally an entropy-increasing process). There are many examples of osmotic pressure in everyday life, for example isotonic saline solution with 9.0 g/l NaCl and a density of kg/l is the basis for intravenous fluids. Molarity =(9.0 g/l) / g/mol NaCl = 0.15 moles NaCl / L Mass of solution = Mass NaCl + water For review g = show 9.0 that g + M Mass = m for water this solution g = Mass water molality = 0.15 mole NaCl / kg = 0.15 molal
15 Week 14/Tu: Reverse Osmosis To reverse osmosis one has to apply a pressure on the solution side that is bigger than that from osmosis. Pure water will flow out of the membrane (if it can hold up).
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