1. Solutions and Colligative
Properties

2. What is a solution?
A solution is a homogeneous mixture
of two or more substances
 A solution is made up of 2 parts: the
solute and the solvent
 A solute is the substance being
dissolved
 A solvent is the substance the solute
is being dissolved in (it is often a
liquid)


3. What does dissolve mean?
To dissolve means to break apart.
When salt dissolves in water, it is
being broken up into smaller parts.
 Those smaller parts are called atoms,
and in the case of salt, they are
beaking up into their individual ions.


4. Let’s take a closer look at the
subatomic level

The balls in the picture represent the
atoms involved in building a molecule
(like salt). When they are placed in the
solvent, they break into individual
atoms (or balls).

5. Real life examples exercise

Brainstorm some real life examples of
solutions with your neighbors and be
prepared to share them with the class.

6. Solubility Rules
Not all substances are soluable. Some
create an insoluble compound called a
precipitate. We need to be able to
predicte if a compound will dissolve or
form a precipitate.
 Today we will use the solubility rules
handout but you will need to begin
memorizing the solubility rules for
homework as you will not be given
them on the test.


7. Determine if the following
compounds are soluble
Ammonium Chloride
 Lead Chloride
 Silver Iodide
 Sodium Sulfide
 Rhubidium Nitride


8. How do we describe how much
solute is in the solution?

In order for us to determine how much of
a solute is dissolved in a solution we use
units of concentration.

Molarity (most useful and most used by
chemists) describes the amount of solute
dissolved per total liters of solution.

Molality is the amount of solute per liters
of solvent.