chemistry, 1ce copyright © 2014 pearson canada inc.slide 12-1 12 solutions

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

12 Solutions


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


FIGURE

12.1 Thirsty Solutions: Why You Should Not Drink Seawater

12.1 A Typical Solution


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


FIGURE

Nature’s Tendency toward Mixing: Entropy

12.3 Spontaneous Mixing of Two Ideal GasesFIGURE

Chemistry, 1Ce Copyright © 2014 Pearson Canada Inc.


Entropy

a measure of energy randomization or energy dispersal


FIGURE

The Effect of Intermolecular Forces

12.4 Intermolecular Forces Involved in Solutions


TABLE 12.2 Relative Interactions and Solution Formation


TABLE 12.3 Common Laboratory Solvents


FIGURE 12.5 Forces in a Solution


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.


EXAMPLE 12.1 continued

Solution


FIGURE

12.4 Solution Equilibrium and Factors Affecting Solubility

12.9 Dissolution of NaCl


FIGURE 12.10 Precipitation from a Supersaturated Solution


FIGURE

The Temperature Dependence of the Solubility of Solids

12.11 Solubility and Temperature


Factors Affecting the Solubility of Gases in Water

Warm Cold


FIGURE 12.12 Soda Fizz


Sgas = kHPgas

Henry’s Law

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


12.5 Expressing Solution Concentration

TABLE 12.5 Solution Concentration Terms


Molarity

Molarity (M) =amount of solute (mol)

volume solution (L)


FIGURE 12.13 Preparing a Solution of Known Concentration


Molality

Molality (m) =amount of solute (mol)

mass of solvent (kg)


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


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


FIGURE

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

12.14 Dissolution of an Electrolyte


Vapour Pressure Lowering


Psolution = χsolvent P°solvent

ΔP = P°solvent - Psolution

Define vapour pressure lowering


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.


Vapor Pressures of Solutions Containing a Volatile (Nonelectrolyte) Solute

PA = χA P°A

PB = χB P°B

Ptot = PA + PB


FIGURE 12.15 Behaviour of Nonideal Solutions


Freezing Point Depression and Boiling Point Elevation

ΔTf=mKf

ΔTb=mKb


ΔT =mKf

TABLE 12.7 Freezing Point Depression and Boiling Point Elevation Constants for Several Liquid Solvents


FIGURE

Osmotic Pressure

12.16 An Osmosis Cell Π =MRT


End of Chapter 12

chemistry, 1ce copyright © 2014 pearson canada inc.slide 12-1 12 solutions

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temperature slide

supersaturated solution

continued solution slide

typical solution slide

water warmcold slide

osmotic pressure slide