Chapter 12. Solutions and Their Behavior. Supersaturated contains more than the saturation limit (very unstable)

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1 Chapter 12 Solutions and Their Behavior Unsaturated holds less than maximum capacity at a given T Supersaturated contains more than the saturation limit (very unstable) Saturated maximum amount of solute dissolved at a given T

2 Concentration Units Molarity (M) = moles of solute liter of solvent Temperature dependent Molality (m) = moles of solute kilogram of solvent Temperature independent Mole fraction (χ A ) = moles of solute A total moles

3 Colligative Properties of Nonelectrolyte Solutions Colligative properties are properties that depend only on the number of solute particles in solution and not on the nature of the solute particles. e.g. Vapor-Pressure Lowering Raoult s Law Adding an inert, nonvolatile solute to a solvent lowers the equilibrium vapor pressure of the solvent. The partial pressure of the solvent depends on its mole fraction (χ)

4 Raoult s Law P = Problem A solution is prepared by dissolving 393 g of sucrose (C O 11 ) in 624 g of water. What is the vapor pressure of this solution at 3 o C? (The vapor pressure of water is 31.8 mmg at 3 o C.)

5 Solutions with Two Volatile Solutes Ideal Solution P A = X A P A P B = X B P B P T = P A + P B P T = X A P A +X B P B P T is greater than predicted by Raoults s law P T is less than predicted by Raoults s law Force A-B Force < & A-A Force B-B Force A-B Force > & A-A Force B-B

6 Fig. 12.9(TE Art) Thermometer Copyright The McGraw-ill Companies, Inc. Permission required for reproduction or display. Condenser Adapter Fractionating column Water Water Distilling flask eater Receiving flask Boiling-Point Elevation T b = T b T b T b is the boiling point of the pure solvent T b is the boiling point of the solution T b > T b T b > T b = K b m m is the molality of the solution K b is the molal boiling-point elevation constant ( C/m)

7 Freezing-Point Depression T f = T f T f T f T f > T f T f is the freezing point of the pure solvent is the freezing point of the solution T f > T f = K f m m is the molality of the solution K f is the molal freezing-point depression constant ( C/m)

8 Using Colligative Properties to Determine Molar Mass Can be accomplished using freezing point depression or boiling point elevation

9 Colligative Properties of Electrolyte Solutions Colligative properties depend on the number of particles, so if an ionic compound is dissolved, it s dissociation increases the total number of particles delivered to solution. This increases T f and T b. T f = T b = i = van t off factor, a scaling factor that approximately equals the number of particles produced after dissociation of the ionic compound. e.g. NaCl MgCl 2

10 Chapter problem 12.77(a). What are the boiling and freezing points for a solution containing 21.2 g of NaCl in 135 ml of water? K f = 1.86 o C/m and K b =.52 o C/m A Molecular View of the Solution Process Liquids Dissolving in Liquids Two liquids that mix completely together are said to be MISCIBLE - otherwise they are IMMISCIBLE. CuSO 4 (aq) Nonpolar octane (C 8 18 ) Nonpolar CCl 4

11 Mixing of Polar Liquids δ - δ + C 3 C 2 -O- δ - O δ - C 3 C 2 -O- δ - C 3 C 2 -O- δ + δ - O δ + δ - O Polar molecules can break up groups of other polar molecules through dipoledipole interactions, resulting in a thorough mixing Mixing of Polar and Nonpolar Liquids δ - -C -C -C- O δ - O δ - O -C -C -C- The weak London forces present in the C 3 C 2 C 3 molecules are not strong enough to break the hydrogen bonds, so the two liquids are immiscible.

12 Mixing Nonpolar Liquids Cl Cl C Cl -C -C -C -C -C -C - Cl London forces are the only interactions, but the strength of these forces between CCl 4 molecules is comparable to those between C 6 14 molecules, so the two liquids are miscible with each other. General Observation: Solids Dissolving in Liquids Like Dissolves Like Again The solvent molecules must be able to overcome the attractive forces holding the solute molecules/atoms/ions together

13 Temperature and Solubility Solid solubility and temperature most solids exhibit increased solubility with temperature, but exceptions do exist solubility increases with increasing temperature solubility decreases with increasing temperature Fractional crystallization is the separation of a mixture of substances into pure components on the basis of their differing solubilities. Suppose you have 9 g KNO 3 contaminated with 1 g NaCl. Fractional crystallization: 1. Dissolve sample in 1 ml of water at 6 C 2. Cool solution to C 3. All NaCl will stay in solution (s = 34.2g/1g) g of PURE KNO 3 will precipitate (s = 12 g/1g). 9 g 12 g = 78 g

14 Temperature and Solubility Gas solubility and temperature solubility usually decreases with increasing temperature Why? Pressure and Solubility of Gases The solubility of a gas in a liquid is proportional to the pressure of the gas over the solution (enry s law). c = kp c is the concentration (M) of the dissolved gas P is the pressure of the gas over the solution k is a constant (mol/l atm) that depends only on temperature low P low c high P high c

15 Chemistry In Action: The Killer Lake 8/21/86 CO 2 Cloud Released 17 Casualties Trigger? earthquake landslide strong Winds Lake Nyos, West Africa

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