Solution – a homogeneous mixture of two or more substances
Solvent: dissolving medium Ex: water
Solute: substance that dissolves Ex: sugar, salts

Classification of Mixtures: true solution, suspension, and colloids
1.
True solution: when a solute is dispersed throughout a solvent and form a homogeneous mixture (single phase)
Ex: sugar+water; salt + water

2. Suspension: particles of a solute are huge compared to molecules of a solvent and form a heterogeneous mixture. Ex: muddy water, orange juice (filtration)
3. Colloids: particles are suspended through out the solvent. It may appear to be homogeneous, but examination (tyndall effect) shows that they are not a true solution.

Ex: mayonnaise (emulsion), milk, butter, gelatin, whipped cream, fog. smoke, mist, paints, glue.
Tyndall Effect: distinguish true solution and colloid by passing a beam of light.
Emulsion: liquid suspended in a liquid.

SUSPENSION COLLOID SOLUTIONS
Completely Settle Out
Pass Changed
(Separated)
Separated by
Membranes
Scatter Light
Not Affect Colligative
Property
> 100 nm
Do not Settle Out
Pass Unchanged
Through Filter Paper
Separated by by Membranes
Scatter Light
Affect Colligative
Properties
100 nm – 10 nm
Do not Settle Out
Pass Unchanged
Through Filter Paper
Not separated by by Membranes
Not Scatter Light
Not Affect Colligative
Property
< 10 nm

1. Brownian Motion: Continuous motion of colloidal properties, random
2. Tyndall Effect: Light scattering by colloidal particles. “ Like dissolves Like.”
Definition:Substances with similar bonding are mutually soluble – Miscible
Examples
1. HOH with Alcohol Polar/ Polar
2. HOH with Glycerol Polar/ Polar
3. HOH with salt Polar/ Ionic
4. Oil with gasoline Covalent/ Covalent

3.
4.
1.
2.
Aqueous = HOH based
Gaseous = Gas based
Other = Liquid/Solid/ Gas
Alloys= Metals- 2 or more (melt the solidify)
SOLVENT- The dissolving medium-large mass/volume
SOLUTE - The substance be dissolved- small mass/volume

Types of Solutes:
1.
Electrolytes: conduct electric current.
Ex: salt water
2.
Nonelectrolytes: non conduct electric current. Ex: sugar water
Factors affecting the rate of dissolution:
1.
2.
3.
Increasing the surface area of the solute
Agitating a solution
Heating a solution

Solubility: the amount of solute is dissolved by a solvent at a given temperature.
Unsaturated solution: more solute can be dissolved.
Saturated solution: the maximum amount of dissolved solute in a solution
Supersaturated solution: a solution that has more dissolved solute than a saturated solution at the same conditions.

Types of Solutions:
Solute Solvent Example gas gas gas gas deep sea gas (He in O
2
) liquid soda (CO
2 in water) solid stove lighter (H2 in platinum) liquid gas water vapor in air liquid liquid antifreeze in water liquid solid Hg in Sn/Ag-dental amalgam

1
S
2
L
Solids
Alloy
(Jewelry Ag
& Au)
Salt Water
(HOH/NaCl)
3
G
Air
Naphthalene
(Moth Balls)
Liquids
Dental
Amalgam
(Silver/ Hg)
Vinegar
(Acetic
Acid/HOH)
Humidity
(Air/ HOH)
Gases
Gas Stove
Lighter
(Pd/H
2
)
Carbonate
Beer
(HOH/CO
2
)
Deep Sea
Gas
(He/O
2
)

2.
3.
1.
Solvent-Solvent Dissociation ( Solvation)
(Hydration)
Solute-Solute Dissociation
Solvent-Solute Association H +,--,0
Rate of Dissolving
1.
Heat Solvent
2.
Powder Solute
3.
4.
Stirring Solution (Agitate)
Adjust Volume of Solvent v. Solute

1
S/S
Factors
L D L
Melt
2
S/L
L D L
Melt
3
S/G
L D L
Adsorbs/
Absorbs
Pressure
Temperature
No
No
No
Limits
No
No
Surface
Area of
Solid

1
L/S
2
L/L
Factors
L D L
Powder
Agitate
L D L
3
L/G
L D L
Pressure
Henry’s Law
Temperature
Yes
T,
Solubility
Yes
Limits
No
Yes
T,
Solubility
No
Yes

1
G/S
2
G/L
3
G/G
Factors
Nature of
Solute
Gravity
Temperature
No
Pressure
Availability of Solute
No
Yes
T,
Solubility
No No
Limits
Yes
Volume of Gas
Yes
Temp. &
Volume

Henry’s Law: Solubility of a gas in a liquid is directly proportional to the partial pressure of that gas on the surface of the liquid.
Solubility:the amount of solute is dissolved by a solvent at a given temperature.

Saturation: Quantity of Solute per Volume (Mass)
Solvent
Unsaturated- holding less than max. under the conditions
Saturated- Maximum Solute per Unit of Solvent
L/S Temp. sensitive
L/G Temp. & Pressure Sensitive
Supersaturated- holding greater than Max. under specific condition.
L/S Heat, Add Solute, Cool
L/G Keep under pressure

Return to Saturation
1.
2.
3.
Addition of a seed crystal; Shock “ping”, agitate
Sudden Temp. Change Cooling
Sudden Reduction in Pressure (gases only)
DILUTE vs. COCENTRATED: Add solvent/ remove solvent

SOLUTION EQUILIBRIUM
Definition: Physical state in which opposing processes of dissolving & crystallizing occur at equal rate.
LeChatelier: Stress on a system causes a shift in the equilibrium of a system
“Stress”: 1. T
2. P
3.Agitation

AT “0”C AT 20 C AT 40 C AT 60 C AT 80 C AT 100 C
1 Sugar
C
12
H
22
O
11
179 g 204 g 238 g 287 g 362 g 487 g
2
NaCl
35.7 g 36.0 g 36.6 g 37.3 g 38.4 g 39.8 g
3
Li
2
CO
3
1.54 g 1.33 g 1.17 g
1.01 g .85 g .72 g

“+” curve
S
S
M
A
Temperature
“0” Curve
“_” Curve

Heat of a Solution: The difference between the heat contents of a solution and the H of its components.
Exothermic: Heating; H ;KOH,NaOH
Endothermic: Cooling; + H; KNO
3
, AgNO
3
Isothermic: No Change “Neutral”; zero H;
C
2
H
3
OOH(1), NaCl