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 Give the study set the name: Chapter 18
Solutions
 Create the study set with the following vocab
terms: saturated solution, solubility, unsaturated
solution, miscible, immiscible, concentration,
dilute solution, concentrated solution, molarity,
colligative properties, boiling point elevation,
freezing-point depression, molality, mole fraction
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Chapter 18 - Solutions
18.1 Properties of Solutions

Solution Formation
 Solvent
 This
is the liquid that is doing the dissolving
 Solute
 This
is what is being dissolved
 Form a homogenous mixture
Solubility

When a solute is dissolved, an
equilibrium is established:
 Equilibrium
is a condition in which both
reactants and products are present in
concentrations which have no further
tendency to change with time
EXAMPLE:
HC2H2O3 ↔ C2H3O2- + H+
Solubility
 When
an equilibrium is established, the
solution is said to be saturated
 If
a solution is not at equilibrium, then it is
said to be unsaturated (solution has the
ability to hold more)
Saturated vs. Unsaturated Solutions
Solubility
 Two
liquids that dissolve in each other are
said to be miscible
 Immiscible
other
liquids are insoluble in each
Immiscible vs. Miscible Solutions
Factors Affecting Solubility
Solubility increases with the increase in
temperature (Easier to dissolve
something when the temperature is
increased)
 Solubility increases with an increase in
surface area (ex. CRUSHING)

 Few
exceptions that occur in the reverse
Thursday, April 10th, 2014

PDN: What is the differences between
miscible and immiscible? Saturated and
unsaturated?

Daily Log:
 Molarity
Notes
 Molarity Calculations
18.2 Concentrations of Solutions

Molarity is the concentration of moles
per liters
 Molarity
(M) = moles of solute / liters of
solution
 Dilute solution contains a low concentration
of solute
 Concentrated solution contains a high
concentration of solute
Practice Problems:

Calculate the molarity of a solution
which contains 0.40 mol of C6H12O6
dissolved in 1.6 L of a solution.

What is the molarity of a solution
containing 325 g of NaCl dissolved in
750. mL of solution?(1000 ml = 1L)
Monday, April 14th, 2014
PDN: Determine the volume of a 1.7M
solution containing 3.3 grams of NaCl.
 Daily Log:

 Science
Scheduling
 Dilution Notes/Practice Problems
Making Dilutions

Formula for
making a dilution
 C1 X
V1 = C2 X V2
 “Stock
solution”
is the same as
the original
solution.
Example

A stock solution of HCl has a
concentration of 12M. How much of the
stock solution would be required to
make 325 mL of a 6M solution?
Monday, April 21st, 2014

Daily Log:
 Molality
Notes
 Practice Problems
 Chapter 18 Test on
Friday
Molality
Molality is another way to represent the
concentration of a solution.
 It is represented by a lower case m.
 Molality = moles of solute/kg of solvent


Example: A 4.9m solution of NaCl is
dissolved in 1000 grams of water. How
many grams of NaCl is this?
Tuesday, April 22nd, 2014

PDN: Determine the molality of a NaCl
solution in which 17.3 moles of solute
are dissolved in 1400 grams.

Daily Log:
 Practice
Problems
 Test on Friday!
18.3 Colligative Properties of
Solutions

Properties that depend on the number
of particles dissolved in a given mass of
solvent
 Boiling
Point Elevation
 Freezing Point Depression
Boiling-Point Elevation
∆Tb
= Kb x m x i
m is the molaity
i is the number of ions in
solution
Kb is the molal boiling point
elevation constant
It is dependent on the
solvent
Freezing Point Depression
∆Tf
= Kf x m x i
m is the molaity
i is the number of ions in
solution
Kf is the molal freezing point
constant
It is also dependent on
the solvent
Example:

Determine the boiling point and freezing
point of a solution in which 600 grams of
MgCl2 is dissolved in 2400 grams of
water. (Kb = 0.512 and Kf = 1.86)