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Chemistry, 1Ce Copyright © 2014 Pearson Canada Inc. slide 12-1
12 Solutions
Chemistry, 1Ce Copyright © 2014 Pearson Canada Inc. slide 12-2
12 Solutions
12.1 Thirsty Solutions: Why You Shouldn’t Drink Seawater
12.2 Types of Solutions and Solubility
12.4 Solution Equilibrium and Factors Affecting Solubility
12.5 Expressing Solution Concentration
12.6 Colligative Properties: Vapour Pressure Lowering, Freezing Point Depression, Boiling Point Elevation, and Osmotic Pressure
Chemistry, 1Ce Copyright © 2014 Pearson Canada Inc. slide 12-3
FIGURE
12.1 Thirsty Solutions: Why You Should Not Drink Seawater
12.1 A Typical Solution
Chemistry, 1Ce Copyright © 2014 Pearson Canada Inc. slide 12-4
Chemistry, 1Ce Copyright © 2014 Pearson Canada Inc. slide 12-5
12.2 Types of Solutions and Solubility
TABLE 12.1 Common Types of Solutions
Copyright © 2014 Pearson Canada Inc.
Chemistry, 1Ce Copyright © 2014 Pearson Canada Inc. slide 12-6
FIGURE 12.2 The Tendency to Mix
Chemistry, 1Ce Copyright © 2014 Pearson Canada Inc. slide 12-7
FIGURE
Nature’s Tendency toward Mixing: Entropy
12.3 Spontaneous Mixing of Two Ideal GasesFIGURE
Chemistry, 1Ce Copyright © 2014 Pearson Canada Inc.
Chemistry, 1Ce Copyright © 2014 Pearson Canada Inc. slide 12-8
Entropy
a measure of energy randomization or energy dispersal
Chemistry, 1Ce Copyright © 2014 Pearson Canada Inc. slide 12-9
FIGURE
The Effect of Intermolecular Forces
12.4 Intermolecular Forces Involved in Solutions
Chemistry, 1Ce Copyright © 2014 Pearson Canada Inc. slide 12-10
TABLE 12.2 Relative Interactions and Solution Formation
Chemistry, 1Ce Copyright © 2014 Pearson Canada Inc. slide 12-11
TABLE 12.3 Common Laboratory Solvents
Chemistry, 1Ce Copyright © 2014 Pearson Canada Inc. slide 12-12
FIGURE 12.5 Forces in a Solution
Chemistry, 1Ce Copyright © 2014 Pearson Canada Inc. slide 12-13
EXAMPLE 12.1 Solubility
Vitamins are often categorized as either fat soluble or water soluble. Water-soluble vitamins dissolve in body fluids and are easily eliminated in the urine, so there is little danger of overconsumption. Fat-soluble vitamins, on the other hand, can accumulate in the body’s fatty deposits. Overconsumption of a fat-soluble vitamin can be detrimental to health. Examine the structure of each vitamin and classify it as either fat soluble or water soluble.
Chemistry, 1Ce Copyright © 2014 Pearson Canada Inc. slide 12-14
EXAMPLE 12.1 continued
Solution
Chemistry, 1Ce Copyright © 2014 Pearson Canada Inc. slide 12-15
FIGURE
12.4 Solution Equilibrium and Factors Affecting Solubility
12.9 Dissolution of NaCl
Chemistry, 1Ce Copyright © 2014 Pearson Canada Inc. slide 12-16
FIGURE 12.10 Precipitation from a Supersaturated Solution
Chemistry, 1Ce Copyright © 2014 Pearson Canada Inc. slide 12-17
FIGURE
The Temperature Dependence of the Solubility of Solids
12.11 Solubility and Temperature
Chemistry, 1Ce Copyright © 2014 Pearson Canada Inc. slide 12-18
Factors Affecting the Solubility of Gases in Water
Warm Cold
Chemistry, 1Ce Copyright © 2014 Pearson Canada Inc. slide 12-19
FIGURE 12.12 Soda Fizz
Chemistry, 1Ce Copyright © 2014 Pearson Canada Inc. slide 12-20
Sgas = kHPgas
Henry’s Law
TABLE 12.4 Henry’s Law Constants for Several Gases in Water at 25°C
Chemistry, 1Ce Copyright © 2014 Pearson Canada Inc. slide 12-21
12.5 Expressing Solution Concentration
TABLE 12.5 Solution Concentration Terms
Chemistry, 1Ce Copyright © 2014 Pearson Canada Inc. slide 12-22
Molarity
Molarity (M) =amount of solute (mol)
volume solution (L)
Chemistry, 1Ce Copyright © 2014 Pearson Canada Inc. slide 12-23
FIGURE 12.13 Preparing a Solution of Known Concentration
Chemistry, 1Ce Copyright © 2014 Pearson Canada Inc. slide 12-24
Molality
Molality (m) =amount of solute (mol)
mass of solvent (kg)
Chemistry, 1Ce Copyright © 2014 Pearson Canada Inc. slide 12-25
Parts by Mass and Parts by Volume
percent by mass =mass solute
mass solutionx 100%
parts per million = ppm =mass solute
mass solutionx 106
parts per billion = ppb =mass solute
mass solutionx 109
Chemistry, 1Ce Copyright © 2014 Pearson Canada Inc. slide 12-26
Mole Fraction and Mole Percent
χ = amount of solute (moles)
total amount of solute and solvent (moles)
= nsolute
nsolute + nsolvent
mole % = x 100% nsolute
nsolute + nsolvent
Chemistry, 1Ce Copyright © 2014 Pearson Canada Inc. slide 12-27
FIGURE
12.6 Colligative Properties: Vapor Pressure Lowering, Freezing Point Depression, Boiling Point Elevation, and Osmotic Pressure
12.14 Dissolution of an Electrolyte
Chemistry, 1Ce Copyright © 2014 Pearson Canada Inc. slide 12-28
Vapour Pressure Lowering
Chemistry, 1Ce Copyright © 2014 Pearson Canada Inc. slide 12-29
Psolution = χsolvent P°solvent
ΔP = P°solvent - Psolution
Define vapour pressure lowering
Chemistry, 1Ce Copyright © 2014 Pearson Canada Inc. slide 12-30
ΔP = P°solvent - Psolution
χsolvent = 1 – χsolute
ΔP = P°solvent - χsolvent P°solvent
ΔP = P°solvent – (1 - χsolute)P°solvent
ΔP = χsoluteP°solvent
Psolution = χsolvent P°solvent
the lowering of the vapor pressure is directly proportional to the mole fraction of the solute.
Chemistry, 1Ce Copyright © 2014 Pearson Canada Inc. slide 12-31
Vapor Pressures of Solutions Containing a Volatile (Nonelectrolyte) Solute
PA = χA P°A
PB = χB P°B
Ptot = PA + PB
Chemistry, 1Ce Copyright © 2014 Pearson Canada Inc. slide 12-32
FIGURE 12.15 Behaviour of Nonideal Solutions
Chemistry, 1Ce Copyright © 2014 Pearson Canada Inc. slide 12-33
Freezing Point Depression and Boiling Point Elevation
ΔTf=mKf
ΔTb=mKb
Chemistry, 1Ce Copyright © 2014 Pearson Canada Inc. slide 12-34
ΔT =mKf
TABLE 12.7 Freezing Point Depression and Boiling Point Elevation Constants for Several Liquid Solvents
Chemistry, 1Ce Copyright © 2014 Pearson Canada Inc. slide 12-35
FIGURE
Osmotic Pressure
12.16 An Osmosis Cell Π =MRT
Chemistry, 1Ce Copyright © 2014 Pearson Canada Inc. slide 12-36
End of Chapter 12