Transcript Slide 1

12
Chemistry, 1Ce
Solutions
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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
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12.1 Thirsty Solutions: Why You Should Not
Drink Seawater
FIGURE 12.1
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A Typical Solution
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12.2 Types of Solutions and Solubility
TABLE 12.1 Common Types of Solutions
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FIGURE 12.2
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The Tendency to Mix
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Nature’s Tendency toward Mixing: Entropy
FIGURE 12.3
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Spontaneous Mixing of Two Ideal Gases
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Entropy
a measure of energy randomization or energy dispersal
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The Effect of Intermolecular Forces
FIGURE 12.4
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Intermolecular Forces Involved in Solutions
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TABLE 12.2 Relative Interactions and Solution Formation
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TABLE 12.3 Common Laboratory Solvents
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FIGURE 12.5
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Forces in a Solution
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EXAMPLE 12.1
Solubility
Vitamins are often categorized as either fat soluble or water soluble. Watersoluble 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 fatsoluble vitamin can be detrimental to health. Examine the structure of each
vitamin and classify it as either fat soluble or water soluble.
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EXAMPLE 12.1
continued
Solution
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12.4 Solution Equilibrium and Factors
Affecting Solubility
FIGURE 12.9
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Dissolution of NaCl
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FIGURE 12.10 Precipitation from a Supersaturated Solution
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The Temperature Dependence of the Solubility
of Solids
FIGURE 12.11 Solubility and Temperature
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Factors Affecting the Solubility of Gases in Water
Cold
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Warm
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FIGURE 12.12 Soda Fizz
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TABLE 12.4 Henry’s Law
Constants for Several Gases
in Water at 25°C
Henry’s Law
Sgas = kHPgas
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12.5 Expressing Solution Concentration
TABLE 12.5 Solution Concentration Terms
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Molarity
Molarity (M) =
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amount of solute (mol)
volume solution (L)
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FIGURE 12.13 Preparing a Solution of Known Concentration
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Molality
Molality (m) =
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amount of solute (mol)
mass of solvent (kg)
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Parts by Mass and Parts by Volume
percent by mass =
mass solute
mass solution
parts per million = ppm =
parts per billion = ppb =
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x 100%
mass solute
x 106
mass solution
mass solute
mass solution
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x 109
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Mole Fraction and Mole Percent
χ=
=
amount of solute (moles)
total amount of solute and solvent (moles)
nsolute
nsolute + nsolvent
mole % =
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nsolute
nsolute + nsolvent
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x 100%
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12.6 Colligative Properties: Vapor Pressure
Lowering, Freezing Point Depression,
Boiling Point Elevation, and Osmotic
Pressure
FIGURE 12.14 Dissolution of an Electrolyte
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Vapour Pressure Lowering
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Psolution = χsolvent P°solvent
Define vapour pressure lowering
ΔP = P°solvent - Psolution
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Psolution = χsolvent P°solvent
ΔP = P°solvent - Psolution
ΔP = P°solvent - χsolvent P°solvent
χsolvent = 1 – χsolute
ΔP = P°solvent – (1 - χsolute)P°solvent
ΔP = χsoluteP°solvent
the lowering of the vapor pressure is
directly proportional to the mole fraction of the solute.
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Vapor Pressures of Solutions Containing a
Volatile (Nonelectrolyte) Solute
PA = χA P°A
PB = χB P°B
Ptot = PA + PB
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FIGURE 12.15 Behaviour of Nonideal Solutions
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Freezing Point Depression and Boiling Point
Elevation
ΔTb=mKb
ΔTf=mKf
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ΔT =mKf
TABLE 12.7 Freezing Point Depression and Boiling Point Elevation Constants for Several Liquid Solvents
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Osmotic Pressure
FIGURE 12.16 An Osmosis Cell
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Π =MRT
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End of Chapter 12
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