1. Solutions, Suspensions and Colloids
Acids, Bases and Salts

2. Solutions
All solutions are made of very small particles that do not affect light beams with:
Solute – the chemical that is dispersed
Solvent – the chemical that causes dispersal
Examples: Salt water, Sugar water, vinegar, Coke, Air, Gold jewelry

3. Properties of Solutions
Solute is homogeneously dispersed
All properties are the same throughout solution
Particle size is very small
Gravity does not affected solutions over time
Solute particles can be molecular(as a sugar solution) or ionic (as a salt solution)
Ionic solutions will conduct electricity

4. Colloids
A mixture with small undissolved particles that do not easily settle out.
Particles are larger than a solution but smaller than a suspension
Particles are large enough to begin to scatter light (Tyndall Effect)
Examples: Milk, gelatin, whipped cream, mayonnaise,

5. Suspensions Much larger particles
Often totally blocks transmission of light
Gravity will remove the suspended particles in time to clear the solvent
Heterogeneous dispersal of suspended particles
Examples: Pepper, sand or dirt in water

6. Comparison of Solutions, Colloids, and Suspensions
< 1 nm
> 100 nm
solutions
colloids
suspensions
-atoms
-small molecules
-ions
-aggregates of atoms, molecules or ions
-macromolecules (proteins)
-clumps of particles,
-mineral grains such as sand

7. More Comparison… solutions colloids suspensions < 1 nm > 100 nm
transparent
(clear)
Transparent to Opaque
Translucent to
Opaque
molecular motion
Brownian motion
movement by gravity
never settle
coagulation – can settle

8. Using whole blood as an example…
< 1 nm
> 100 nm
solutions
colloids
suspensions
-dissolved in water
electrolytes (salts)
gases
glucose
-plasma proteins
albumins
globulins
fibrinogen
-cellular stuff
red blood cells
white blood cells
platelets

9. Dissolving process in water
2. Hydration of solute
Orientation of water molecules around solute
Na+
Cl-
1. Overcome attractive forces in solid

10. Pure Water Non-electrolyte - No dissociation,
no conductivity
Non-electrolyte -
No dissociation,
all molecules in solution. No Ions are present to allow electrons to pass.
H20

11. Types of solutes Strong Electrolyte - 100% dissociation,
high conductivity
Strong Electrolyte -
100% dissociation,
all ions in solution
Na+
Cl-

12. Types of solutes Weak Electrolyte - partial dissociation,
slight conductivity
Weak Electrolyte -
partial dissociation,
molecules and ions in solution
CH3COOH
CH3COO- H+

13. Types of solutes Non-electrolyte - No dissociation,
no conductivity
Non-electrolyte -
No dissociation,
all molecules in solution
sugar

14. Solubility of Solutes in Water
Most solids
(endothermic
hydration)
All gases
Solubility, g/100 mL water
Some solids
(exothermic
hydration)
Temperature

15. How do I get sugar to dissolve faster in my iced tea?
Stir, and stir, and stir
Fresh solvent contact and interaction with solute
Add sugar to warm tea then add ice
Faster rate of dissolution at higher temperature
Grind the sugar to a powder
Greater surface area, more solute-solvent interaction