Chemistry, 1Ce Copyright © 2014 Pearson Canada Inc.slide 12-1 12 Solutions

Chemistry, 1Ce Copyright © 2014 Pearson Canada Inc. slide 12-1

12 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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FIGURE

12.1 Thirsty Solutions: Why You Should Not Drink Seawater

12.1 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 The Tendency to Mix

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FIGURE

Nature’s Tendency toward Mixing: Entropy

12.3 Spontaneous Mixing of Two Ideal GasesFIGURE

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Entropy

a measure of energy randomization or energy dispersal

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FIGURE

The Effect of Intermolecular Forces

12.4 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 Forces in a Solution

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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.

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EXAMPLE 12.1 continued

Solution

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FIGURE

12.4 Solution Equilibrium and Factors Affecting Solubility

12.9 Dissolution of NaCl

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FIGURE 12.10 Precipitation from a Supersaturated Solution

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FIGURE

The Temperature Dependence of the Solubility of Solids

12.11 Solubility and Temperature

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Factors Affecting the Solubility of Gases in Water

Warm Cold

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FIGURE 12.12 Soda Fizz

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Sgas = kHPgas

Henry’s Law

TABLE 12.4 Henry’s Law Constants for Several Gases in Water at 25°C

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12.5 Expressing Solution Concentration

TABLE 12.5 Solution Concentration Terms

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Molarity

Molarity (M) =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) =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 solutionx 100%

parts per million = ppm =mass solute

mass solutionx 106

parts per billion = ppb =mass solute

mass solutionx 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 % = x 100% nsolute

nsolute + nsolvent

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FIGURE

12.6 Colligative Properties: Vapor Pressure Lowering, Freezing Point Depression, Boiling Point Elevation, and Osmotic Pressure

12.14 Dissolution of an Electrolyte

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Vapour Pressure Lowering

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Psolution = χsolvent P°solvent

ΔP = P°solvent - Psolution

Define vapour pressure lowering

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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.

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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

ΔTf=mKf

ΔTb=mKb

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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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FIGURE

Osmotic Pressure

12.16 An Osmosis Cell Π =MRT

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End of Chapter 12