Solutions
Subtopics include: (1) Describing
Solutions, (2) Concentrations, (2) Solubility
& (3) the Effects of Solutes on Solutions.
Solutions
Describing Solutions
 Define: solution, solute, solvent, suspensions,
colloidal dispersions, distillation, filtration &
chromatography.
 Explore types of solutions.
 Identify homogenous mixtures that are not
solutions.
Concentrations
 Express the concentrations of solutions in terms
of percent by mass, percent by volume, parts
per million and molarity.
 Use Table T to calculate problems relating to
concentrations.
 Describe the preparation of a solution given the
molarity.
 Identify the process of separating solutions:
distillation, filtration & chromatography.
Solubility
 Define: miscible, saturated, unsaturated,
solubility, supersaturation.
 Describe factors that effect solubility.
 Use “solubility rules” to predict the solubility of an
ionic compound in water.
 Interpret and construct solubility curves.
 Use solubility curves to distinguish among
saturated, supersaturated, and unsaturated
solutions.
 Apply the “like dissolves like” rule to real-world
situations.
Effects of Solutes on Solution
 Define: boiling point, freezing point and
electrolytes.
 Explore the effect of solutes on the boiling point
and freezing point of solutions.
 Solve problems involving freezing point
depressions and boiling point elevation
(colligative properties).
 How can we describe the behavior of
electrolytes in a solution?
Describing Solutions
 Define: solution, solute, solvent, suspensions, colloidal dispersions, distillation filtration &
chromatography.
 Explore types of solutions.
 Identify homogenous mixtures that are not solutions.
 Identify the process of separating solutions: distillation, filtration & chromatography.

Molecular Set: 3 water molecules, 2 hydrogen florides, 2 Iodines
Essential Questions:
1. What is a solution?
Aim:
How can we
describe
solutions?
2. What are some types
of solutions?
Key Words:
3. How do we separate
solutions? Explain.
solution, solute,
solvent, suspensions,
colloidal dispersions,
distillation, filtration,
chromatography.
Name Some Solutions!
Q: What are some solutions you
have encountered today?
Which One is a Solution?
Salt Water
Oil Water
A) The Salt Water
B) The Oil Water
C) Both
D) Neither
Deduction
Q: Based on the previous example,
how can we describe a solution?
Notes
I. Describing Solutions
A. Definitions
1. Solution - homogenous
mixture of a solute
dissolved in a solvent.
Solutes, Solvents & Solutions
Solute
Solution
Solvent
Notes
2. Solute –
3. Solvent –
4. Solution –
What Makes Solutions
Homogenous?
Water and rubbing alcohol have different densities
so why don’t they separate themselves into layers
based on their densities as shown in the picture?
Why do they form solutions instead?
What makes their atoms arrange
together homogenously?
---
Notes
B. “Like Dissolves Like”
1. In a solution, all particles attract each
other with intermolecular forces of
similar strength.
i. Polar substances dissolve other polar
substances and ionic substances.
ii. Nonpolar substances dissolve other
nonpolar substances.
Solutions Exist Between
Particles in Different
States (Gas, Liquid, Solid)!
Can you think of any
examples.
Notes
C. States of Matter & Solutions
1. The solute and solvent may be in different
phases as long as the particles are evenly
distributed amongst each other.
i. Ex: Solid NaCl dissolved in liquid water.
ii. Ex: Gaseous CO2 is dissolved in liquid soda.
2. All mixtures of gases are solutions.
Solutions Among Various
Phases of Matter
Example
Phase of Solute
Phase of Solvent
Metallic Alloy
Solid
Solid
Table salt-water
Solid
Liquid
Ethyl alcohol-water
Liquid
Liquid
CO2-water (Soda)
Gas
Liquid
Air
Gas
Gas
How Do We Determine
Which Substance is a
Solute & Which is the
Solvent?
Notes
D. Identification of Solutes vs. Solvents
1. If the solute and solvent are in different
phases, then solute assumes the
solvent’s phase.
2. If the solute and solvent are in the same
phase, then the solvent is the one that
there is more of.
Our Chemistry class has
run out of salt and we
want to make a new batch
from collected sea water.
How do I separate the salt
from the water?
E. Separating Solutions
1. Evaporation
Separates dissolved SOLUTE from
SOLUTION
Ex. Separating salt from water
2. Simple distillation
Separates SOLVENT from SOLUTION
Ex. Obtaining pure water from sea water
3. Fractional distillation
Separates one liquid from a mixture of
different liquids using differences in
boiling points.
Ex. Obtaining alcohol from wine or
oxygen/nitrogen from air.
Video Clip
Distillation
http://www.youtube.com/watch?v=mP4Hguig6U&playnext=1&list=PL73CDD6FFC04D04A4&feat
ure=results_main
Cont’d
4. Chromatography
Separates mixtures
into their constituents
by preferential
absorption by a solid.
Ex. Separating ink
dyes using paper
Filtration
Filtration
Separates large particles from
mixtures but it does not
separate solutions
Why is that?
Learning Check
1) The solvent is the part of the solution that
A. gets dissolved
B. does the dissolving
C. changes phase
3) What is a solution?
4) What are some types of solutions?
5) How do we separate solutions? Explain.
Notes
Describing & Separating Solutions
I. Describing Solutions
A. Definitions
1.
2.
3.
4.
Solution - homogenous mixture of a solute dissolved in a solvent.
Solute – substance dissolved.
Solvent – substance that does the dissolving.
Solution – A homogenous mixture composed on tiny particles.
B. “Like Dissolves Like”
1. In a solution, all particles attract each other with intermolecular forces of similar
strength.
i.
ii.
Polar molecules dissolve other polar molecules and ionic compounds.
Nonpolar molecules dissolve nonpolar molecules.
2. In gasses there are essentially no intermolecular forces, therefore all mixtures of
gasses are solutions.
C. States of Matter & Solutions
1. The solute and solvent may be in different phases as long as the particles are
evenly distributed amongst each other.
i.
ii.
Ex: Solid NaCl dissolved in liquid water.
Ex: Gaseous CO2 is dissolved in liquid soda.
D. Identification of Solutes vs. Solvents
1. If the solute and solvent are in different phases, then solute assumes the
solvent’s phase.
2. If the solute and solvent are in the same phase, then the solvent is the one that
there is more of.
E. Suspensions – suspensions are formed by the
physical homogenous mixture of large particles.
(Solutions are made by the chemical mixture of smaller
particles).
1. Suspensions will settle in time (solutions will not).
2. A light bean passing through a suspension mixture will be visible (in a
solution, it will not).
3. Ex. Sand + Water
F. Colloidal Dispersion – formed when particles
larger than those in solution but smaller than those
in suspensions are dispersed in a medium
1. The terms dispersed substance vs dispersed medium are used for
colloidal dispersion instead of solute and solvent.
2. A colloidal dispersion will not settle.
3. Tyndall effect: a light beam passing through will be clearly visible.
G. Separating Solutions
1. Evaporation – separates dissolved SOLUTE from
SOLUTION.
i. Ex. Separating salt from water
2. Simple distillation – separates solvent from solution
i. Ex. Obtaining pure water from sea water
3. Fractional distillation – separates one liquid from a
mixture of different liquids that have different
boiling points.
i. Ex. Obtaining ALCOHOL from wine or
oxygen/nitrogen from air.