Solutions
Definitions

Solution: homogeneous mixture of 2 or
more substances in a single physical state


Solute: the substance dissolved in the solution
Solvent: the substance the solute is dissolved in
General Properties of
Solutions

1. solute particles in solutions are very small

2. solute particles are evenly distributed
throughout the solution

3. particles in a solution will not separate
under normal conditions
Types of Solutions

Aqueous solutions: solutions with water as
the solvent.


Electrolyte solutions: aqueous solutions of
ionic compounds. Ionic compounds dissociate
allowing for the solution to conduct an
electrical charge
Nonelectrolyte solutions: aqueous solutions
of molecular compounds. The solute does not
dissociate.
Solution Formation


When ionic compounds dissolve in water,
they dissociate
NaCl --> Na+ + ClEach component has an attraction to a
certain part of the water molecules
Solubility Rules

Used to predict the solubility of ionic
compounds.


Not all ionic compounds are soluble in water.
Some only dissolve partially and some not at all.
Solubility Rules
PRECIPITATION REACTIONS
Precipitation Reactions


Generally reactants are soluble ionic
compounds dissolved in water.
When mixed, one of the possible cations
joins with one of the anions to produce a
compound that is insoluble.

The insoluble compound falls out of solution as a
precipitate.

A solution of silver nitrate is reacted with a
solution of potassium chloride. Write the
complete balanced chemical equation with
notations for state of matter.

Write the equation for the reaction of lead (II)
nitrate with ammonium sulfide.
Net Ionic Equations



Removes unused ions (spectator ions) from
an equation.
Simpler form of a reaction
Examples: write net ionic equations for
previous slide examples.
SOLUTION CONCENTRATION
Molarity (M)

Most common expression of solution
concentration
M=
Mols of solute
Liters of Solution

What is the molarity of a solution formed by
mixing 38 grams of potassium hydroxide in
enough water to make 250 mL of solution?

If I have a 2.5 M sulfuric acid solution, how
many liters of solution will be needed to
obtain 70 grams of sulfuric acid? How many
milliliters?
SOLUTION STOICHIOMETRY

37 mL of a 0.45 M silver nitrate solution are
reacted with 3 grams of copper. What mass
of silver will be produced from the reaction?

18 mL of 1.39M sodium iodide is combined
with 83 mL of 0.25 M lead (II) nitrate.

Will a reaction occur?

If a reaction occurs, what mass of precipitate should
be produced?

What volume of 0.750 M Pb(NO3)2, in
milliliters, is required to react completely with
1 L of 2.25 M NaCl?
Changing the Concentration of
a Solution (Diluting)
M1V1 = M2V2

What volume of 18 M sulfuric acid is needed
to create 6 Liters of 3.25 M sulfuric acid?

Describe how you would prepare 400 mL of a
3.75 M solution of nitric acid if given a supply
of 14.3 M nitric acid.

Describe how to prepare 500 mL of a 0.8 M
solution of sodium hydroxide when provided
with solid sodium hydroxide and distilled
water.
Saturation



Saturated: solution contains all possible
solute under current conditions
Unsaturated: more solute can be dissolved
Supersaturated: solution contains solute
past the saturation point for the current
conditions