Chapter 12: Solutions
Goals:
1. Read Ch12.1-12.2 (pg 400-414.)
– Title the notes “Ch 12 Solutions” (in notes section)
– Copy table 1 pg 402 *summarize/abbreviate as possible
– Table 2 pg 404
– Table 3 pg 404
– Read and take notes/ create vocab list
2. Materials, Procedures and Hypothesis for
final science fair project: Due Friday
– Pg 5 and 6 of packet
3. Get PhET activity to start (Friday activity,
due next Monday)
Section 1- Types of Mixtures
• Solutions are
homogeneous mixtures
of two or more
substances in a single
phase.
– Soluble describes a substance
as capable of being dissolved.
– Solvent is the dissolving
medium in a solution.
– Solute is the substance that is
dissolved in a solution.
Types of Solutions
• Solutions can be in
any of the three
common physical
states.
 solid- a mixture of
metals called an alloy
 liquid- salt water,
sugar water, KoolAid…
 gas- the atmosphere
Suspensions & Colloids
• A suspension has
large particles that
settle out of a solvent.
ex. muddy water
• A colloid has
intermediate size
particles. Also called
an emulsion or a
foam.
Solutes:
electrolytes vs. nonelectrolytes
• An electrolyte is a
substance that dissolves
in water to give a solution
that conducts electricity.
• A nonelectrolyte is a
substance that dissolves
in water to give a solution
that does NOT conduct
electricity.
Ch 12.2- The Solution Process
• Factors that affect the rate of solution (how
quickly a substance dissolves):
– Any process that increases the number of
contacts between the solvent and the solute
will increase the solution rate.
• increasing the surface area of the solute
• agitating (shaking or stirring) the solution
• heating the solvent
Graphs
Title
Dependant
variable
(units)
All Graphs Need:
Title
Labeled axis
Units as needed
independent
variable (units)
Key:
Warm up:
1. Compare and contrast molarity and
molality.
2. If given or asked for grams, how do you
relate grams to moles?
Ex C:
Suppose you want to dissolve 205g
of Na2CO3 in enough water to make
5.00L of solution.
What is the molarity?
• Molar mass= 106.0g/mol
• 205/106 =
Solubility Vocab
• Solubility is a measurement of how much solute will dissolve
in a specific amount of solvent at a specific temperature to
make a saturated solution.
• “Likes dissolve likes”- polar solvents dissolve polar solutes &
nonpolar solvents dissolve nonpolar solutes.
• Hydration: the solution process with water as the solvent.
• Hydrates: ionic compounds that have formed crystals that
have incorporated water molecules in their structure.
• Immiscible liquids are not soluble in one another. eg. oil &
water
• Miscible liquids dissolve freely in one another in any
proportion. eg. water & alcohol
Solutions
• Solution equilibrium: the physical state
in which the opposing processes of
dissolution and crystallization occur at
equal rates.
– Dissolution: dissolve
– Crystallization: form solid
Factors that affect the rate of solution:
(how quickly a substance dissolves)
– Any process that increases the number of contacts
between the solvent and the solute will increase the
solution rate.
– Increase solution rate by:
• increasing the surface area of the solute
• agitating (shaking or stirring) the solution
• heating the solvent
temp. and pressure affects on solubility:
• Increasing the pressure increases the
solubility of gases in a liquid.
– has no effect on the solubility of a solid in a liquid
• For solid in liquid, increasing
temperature often increases
the solubility
• For gas in liquid, increasing
temp decreases the
solubility.
• Henry’s Law: the solubility of a gas in a liquid is directly
proportional to the partial pressure of the gas on the
surface of the liquid.
• Effervescence is the rapid escape of a gas from a liquid
in which the gas is dissolved.
• A solvated solute particle is surrounded
by solvent molecules.
• saturated solution: contains the maximum
amount of dissolved solute.
• unsaturated solution: contains less than
the maximum amount of dissolved solute.
• A supersaturated solution: contains more
dissolved solute than a saturated solution.
Solubility curve
Solubility is a measurement of how much solute will dissolve in a
specific amount of solvent at a specific temperature to make a
saturated solution.
Will the solubility increase,
decrease, remain the same?
1. Soda is opened and heated (the gas)?
2. Solid sodium chloride is dissolved is
water as it is heated.
3. Carbon dioxide is dissolved in water as it
is cooled.
1. Decrease
2. Increase
4. Potassium chloride is added to a
3. Increase
saturated solution.
4. Same
5. Same
5. The surface pressure of salt water is 6. increase
increased.
6. Surface pressure of dissolved oxygen is
increased.
• Enthalpy of solution: amount of heat
absorbed by a solution when a specific
amount of solute dissolves in a solvent.
Classwork
1. Solutions Matching
• Put in classwork section, number your
page and write out the vocab word for
answers
2. When done, work on solutions PHeT
simulation (see handout section of
website)
3. Then work on study guide
Classwork
Solutions Matching
• Put in classwork section, number your
page and write out the vocab word for
answers
Ch 12.3 Practice C and E
• Answer questions:
– Pg 421 Practice #1-3
– Pg 424 Practice #1-2
• Solutions on pg 920
1. Solutions
2. Soluble
3. Solvent
4. Solute
5. Nonelectrolyte
6. miscible
7. Colloid
8. Suspension
9. Supersaturated
10.Saturated
11.unsaturated
12.Electrolyte
13.Solubility
14. immiscible
B.
1. Solute
2. Immiscible
3. Colloid
4. Solution, miscible
5. Saturated
6. Electrolyte
7. Solvent
8. suspension
12.3
Concentrations of Solutions
• The concentration measure of the amount of
solute dissolved in a given amount of solvent or
solution.
• Molarity (M) is the number of moles of solute in
one liter of solution.
M = #mol
L
• Do practice problems #1, #2, & #3 on page 421.
Warm up:
1. What is a solution?
2. A solute?
3. A solvent?
12.3
Concentrations of Solutions
• Molarity (M) is the number of moles of solute in
one liter of solution.
M = mol
L
Ex A: pg 420
What is the molarity of a 3.50L solution that contains 90.0g
of NaCl
Molar mass = 58.44g/mol
90.0g x (1mol/58.44g) = 1.54 mol
1.54 mol
3.50 L
= .440 M NaCl
Ex B:
How many moles of HCl in 0.8L of a 0.5M
solution?
M = mol
L
.5M = mol
.8L
.8L(.5mol/L) = .4mol HCl
• Molality (m) is the concentration of a
solution expressed in moles of solute per
kilogram of solvent.
m = mol
kg
Ex D: pg 423
A solution dissolved .0500mol C12H22O11 in 125g
of water, what is the molal concentration?
125g (1kg/1000g) = .125kg
.0500 mol
.125kg
= .400 m C12H22O11
•Read Ch12.1-12.2 (pg 400-412.) and take
notes in note section of notebook.
– Title the notes “Ch 12 Solutions”
– Copy table 1 pg 401
– Table 2 pg 404
– Table 3 pg 404
– Create a vocab list
Graphs
Title
Dependant
variable
(units)
All Graphs Need:
Title
Labeled axis
Units as needed
independent
variable (units)
Key:
What are the independent and dependent variables?
What is the saturation point of the blue chemical?
What unit is used to measure saturation?
Concentration vs Amount of
Solute
red chemical
2
conc (M)
1.8
blue chemical
1.6
1.4
1.2
1
0.8
0.4
0.6
0.8
amount of solute (moles)
1
Solubility curve
Solubility is a measurement of how much solute will dissolve in a
specific amount of solvent at a specific temperature to make a
saturated solution.
Solution Concentrations
• Percent composition by mass (%) is a
concentration that expresses the percent
of solute in a solution.
% = #g solute x 100
# g solution
matching
1.
2.
3.
4.
5.
6.
7.
8.
9.
10.
11.
12.
13.
14.
homogeneous mixtures of two or more substances
in a single phase.
describes a substance as capable of being
dissolved.
the dissolving medium in a solution.
the substance that is dissolved in a solution.
Doe not conduct electricity
Liquids that dissolve freely in one another
intermediate size particles, also called an emulsion
or a foam
large particles that settle out of a solvent.
Contains more dissolved solute than saturated
solution under same conditions
Solution containing maximum amount of dissolved
solute
Contains less solute than possible under the
existing conditions
Conducts electricity
Amount of substance to form a saturated solution
under specific conditions
Liquids that are not soluble in each other
a.
b.
c.
d.
e.
f.
g.
h.
i.
j.
k.
l.
m.
n.
Soluble
Solvent
Solute
Solutions
Solubility
Electrolyte
Nonelectrolyte
Immiscible
Miscible
Suspention
Saturated
Unsaturated
Supersaturated
Colloid
1
2
3
4
5
6
7
8
9
1
1
1
1
1
Chapter 12 Test Review
• multiple choice
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–
–
–
–
–
–
–
–
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define & identify suspensions & solutions
define an alloy
define & identify electrolytes & nonelectrolytes
factors that affect the rate of dissolution
definitions of unsaturated, saturated & supersaturated solutions
general rules for predicting whether a solute is soluble in a
solvent
definition of solubility
effects of temperature & pressure on the solubility of gases and
solids in liquids
definitions of molarity (M) and molality (m)
solving molarity & molality problems
FORMULAS:
M = #mol/L
m = #mol/kg