Solutions
Chapter 12 Modern Chemistry
Sections 1-3
Types of Mixtures
The Solution Process
Concentrations of Solution
1
Section 12.2
The Solution Process
Chapter 12 Section 2 The Solution
Process p. 407-417
2
Vocabulary
Solubility
Factors affecting
rate of dissolution
Saturated
Unsaturated
Supersaturated
Solubility equilibrium
Solubility values
Dissociation
Hydration
Insoluble
Immiscible
Miscible
Henry’s Law
Effervescence
Chapter 12 Section 1 Types of
Mixtures p. 401-406
3
UNSATURATED
SOLUBILITY
EQUILIBRIUM
SATURATED
SUPERSATURATED
SOLUBILITY
SOLUBILITY
VALUES
FACTORS AFFECTING RATE OF DISSOLUTION
LIQUID SOLUTE
GAS SOLUTE
EFFERVESCENCE
Concept Map 12.2
Chapter 12 Section 1 Types of
Mixtures p. 401-406
PRESSURE
HENRY’S
LAW
INSOLUBLE
LIKES
DISSOLVE
LIKES
IMMISCIBLE
SOLUBLE
MISCIBLE
TEMPERATURE
HYDRATION
DISSOCIATION
IONIC SOLUTE
4
Factors Affecting the Rate of Dissolution
How would you make a solute dissolve faster?
• Stir.
Agitate the solution
• Break it up.
Increase the surface area
of the solute
• Heat it.
Heat the solvent
Chapter 12 Section 2 The Solution
Process p. 407-417
5
Factors Affecting Dissolution Rate
Chapter 12 Section 2 The Solution
Process p. 407-417
6
Solubility
• Solubility of a substance is
the amount of that substance in grams
required to form a saturated solutions with a
specific amount of solvent 100 g H2O
at a specific temperature 20° C
• Look at the chart on page 410
• Dependant on
the nature of the solvent and the solute
and the temperature of the solute
• The maximum amount that can be dissolved is
not dependantChapter
on 12the
rate it dissolves
Section 2 The Solution
7
Process p. 407-417
Solubility & Temperature
p. 410
Chapter 12 Section 2 The Solution
Process p. 407-417
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Solubility and Temperature
p. 414*
Chapter 12 Section 2 The Solution
Process p. 407-417
9
Solubility of Solids in Liquids
Chapter 12 Section 2 The Solution
Process p. 407-417
10
Solubility
• There is a limit to the amount of solute that
can be dissolved. Why?
• Solubility Equilibrium – the physical state in
which the opposing processes of dissolution
and crystallization of a solute occur at equal
rates.
• In other words… the same amount of solute is
dissolving and “undissolving” at the same
time.
Chapter 12 Section 2 The Solution
Process p. 407-417
11
Solubility & Solution Equilibrium
Chapter 12 Section 2 The Solution
Process p. 407-417
12
Solubility Equilibrium
Insert Holt Disc 2
Chapter 12 Section 2 The Solution
Process p. 407-417
13
Saturated & Unsaturated Solns
• Saturated – A solution that contains the
maximum amount of dissolved solute.
• You can tell that it is saturated because no
more solute will dissolve and fall to the bottom
of the container.
• Unsaturated – A solution that contains less
solute than a saturated solution under the
existing conditions.
Chapter 12 Section 2 The Solution
Process p. 407-417
14
Mass of Solute Added vs Mass of Solute Dissolved
p. 409
Chapter 12 Section 2 The Solution
Process p. 407-417
15
Supersaturated Solutions
• A solution that contains more dissolved solute
than a saturated solution contains under the
same conditions.
• HOW?
Saturate a solution.
Heat the solution so that more solute can be
added.
When the solution is cooled undisturbed it will
be saturated.
Chapter 12 Section 2 The Solution
Process p. 407-417
16
LESS than 35.9g NaCl
in 100g H2O at 20°C
Unsaturated
EXACTLY 35.9g NaCl
in 100g H2O at 20°C
Saturated
MORE than 35.9g NaCl
in 100g H2O at 20°C
Supersaturated
Chapter 12 Section 2 The Solution
Process p. 407-417
17
NaC2H3O2 Tower
Insert Holt Disc 2
Chapter 12 Section 2 The Solution
Process p. 407-417
18
Solubility of Compounds
notes
Chapter 12 Section 2 The Solution
Process p. 407-417
19
Solubility of Compounds
notes
Chapter 12 Section 2 The Solution
Process p. 407-417
20
Molecule Polarity REVIEW!!
• What is the molecule polarity of H2O? CCl4?
• How do we determine this?
Insert Holt Disc 2
Chapter 12 Section 2 The Solution
Process p. 407-417
21
Ionic Solute-Solvent Interaction
• Ionic solids that dissolve are soluble.
• Ionic solids will dissolve in polar solvents but
not nonpolar solvents
• Water molecules break the crystal lattice into
separate ions. This is dissociation.
• Then the water molecules surround the ions.
This is hydration.
• Ionic solids that do not dissolve are insoluble.
Chapter 12 Section 2 The Solution
Process p. 407-417
22
Ionic Solute-Solvent Interaction
p. 411
Chapter 12 Section 2 The Solution
Process p. 407-417
23
Dissociation Animations
Insert Holt Disc 2
Insert Glencoe Disk 2
Chapter 12 Section 2 The Solution
Process p. 407-417
24
Hydrated Na+
Insert Holt Disc 2
Chapter 12 Section 2 The Solution
Process p. 407-417
25
Liquid Solute-Solvent Interaction
• Miscible – Liquids that dissolve freely in one
another in any proportion.
• Immiscible – Liquids that are not soluble in
each other.
• “Likes dissolve likes”
Polar solutes dissolve in polar solvents.
Nonpolar solutes dissolve in nonpolar
solvents.
• Alcohols are slightly polar.
Chapter 12 Section 2 The Solution
Process p. 407-417
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Miscible and Immiscible
Chapter 12 Section 2 The Solution
Process p. 407-417
27
Immiscible & Miscible
p. 412
Chapter 12 Section 2 The Solution
Process p. 407-417
28
How Soap Works
Iodine Solubility
Insert Holt Disc 2
Chapter 12 Section 2 The Solution
Process p. 407-417
29
Gas Solute-Solvent Interactions
• Effect of pressure on gas solubility
• Pressure changes have little effect on liquid or
solid solutes.
• Gases dissolved in a liquid are in an
equilibrium
• This means that some of the gas molecules
are going into the solvent and some are going
out of the solvent at equal rates.
Chapter 12 Section 2 The Solution
Process p. 407-417
30
Solubility of a Gas in a Liquid
Chapter 12 Section 2 The Solution
Process p. 407-417
31
Gas Solute-Solvent Interactions
• Henry’s Law
– The solubility
of a gas in a
liquid is
directly
proportional to
the partial
pressure of
that gas on
the surface of
the liquid.
Chapter 12 Section 2 The Solution
Process p. 407-417
32
Gas Solute-Solvent Interactions
After being underwater for a long
time, a diver will have more gases
dissolved in the blood. The diver must
pause during the ascent to allow the
dissolved gas to come out of solution
(the blood) slowly and to be exhaled.
If the ascent is too fast the gas can
come out of solution while flowing
through blood vessels and block
essential blood vessels, causing
extreme pain, paralysis, or even
Chapter 12 Section 2 The Solution
death.
Process p. 407-417
33
Efervescence
Chapter 12 Section 2 The Solution
Process p. 407-417
34
Keep the fizz in your soda!
Chapter 12 Section 2 The Solution
Process p. 407-417
35
Mentos and Coke?
Eepy Bird
http://www.eepybird.com/videos.html
Steve Spangler Science
http://www.stevespanglerscience.com/experimen
t/00000109
Mythbuster
http://www.youtube.com/watch?v=kMXPOqovSB
s&feature=related
Chapter 12 Section 2 The Solution
Process p. 407-417
36
Gas Solute-Solvent Interactions
• Effect of temperature on gas solubility
• Increasing temperature decreases the
solubility of a gas
• An increased temperature increases the kinetic
energy so that gas molecules can escape from
the solvent
Chapter 12 Section 2 The Solution
Process p. 407-417
37
Enthalpy of Solution
• The net amount of energy absorbed as heat
by the solution when a specific amount of
solute dissolves in a solvent.
• If heat is given off when the solute dissolves,
it is exothermic and the enthalpy is negative.
• If heat is taken in when the solute dissolves, it
is endothermic and the enthalpy is positive.
• Look at the table of enthalpies on page 416.
Chapter 12 Section 2 The Solution
Process p. 407-417
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Enthalpies of Solutions
p. 416
Chapter 12 Section 2 The Solution
Process p. 407-417
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Handheld Heater
Insert Holt Disc 2
Chapter 12 Section 2 The Solution
Process p. 407-417
40
Enthalpies of Solutions
p. 415
Chapter 12 Section 2 The Solution
Process p. 407-417
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Ch 12 Sec 2 Homework
Section Review Page 416 # 1-7
Chapter 12 Section 2 The Solution
Process p. 407-417
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