1. Section 14.1 Types of Mixtures
Compare the properties of suspensions, colloids, and solutions.
Identify types of colloids and types of solutions.
Describe the electrostatic forces in colloids.
Mixtures can be either heterogeneous or homogeneous.
Section 14-1

2. Heterogeneous Mixtures
A heterogeneous mixture is a mixture that does not have a uniform composition and in which the individual substances remain distinct.
Suspensions
mixtures containing particles that settle out if left undisturbed.
Section 14-1

3. Heterogeneous Mixtures (cont.)
Colloids
heterogeneous mixtures of intermediate sized particles and do not settle out.
remained mixed due to an emulsifier
categorized according to the phases of their particles.
Section 14-1

4. Heterogeneous Mixtures (cont.)
Section 14-1

5. Heterogeneous Mixtures (cont.)
Brownian Motion
jerky, random movements of particles in a liquid colloid, from the results of particle collisions.
Tyndall effect
dispersed colloid particles scatter light.
Section 14-1

6. Most solutions are liquids, but gaseous and solid solutions exist.
Homogeneous Mixtures
Solutions are homogeneous mixtures that contain two or more substances called the solute and solvent.
Most solutions are liquids, but gaseous and solid solutions exist.
Section 14-1

7. Homogeneous Mixtures (cont.)
Section 14-1

8. Homogeneous Mixtures (cont.)
Soluble
a substance that dissolves in a solvent is
Miscible
two liquids that are soluble in each other
Insoluble
a substance that does not dissolve in a solvent
Immiscible
Two liquids that can be mixed but separate shortly after are
Section 14-1

9. Expressing Concentration
The concentration of a solution is a measure of how much solute is dissolved in a specific amount of solvent or solution
concentrated
dilute
Section 14-2

10. Expressing Concentration
Molarity
the number of moles of solute dissolved per liter of solution.
Section 14-2

11. Section 14.2 Solution Concentration
Describe concentration using different units.
Determine the concentrations of solutions.
Calculate the molarity of a solution.
Concentration can be expressed in terms of percent or in terms of moles.
Section 14-2

12. Stock solution Concentrated solutions of standard molarities
HCl stock solution is 12 M
Dilution equation: M1V1 = M2V2
M1V1 represents the molarity and volume of the stock solution
M2V2 represents the molarity and volume of the dilute solution

13. Expressing Concentration (cont.)
Molality
the ratio of moles of solute dissolved in 1 kg of solvent.
Section 14-2

14. Expressing Concentration (cont.)
Mole fraction
is the ratio of the number of moles of solute in solution to the total number of moles of solute and solvent.
Section 14-2

15. Expressing Concentration (cont.)
Section 14-2

16. Percent by mass Percent by volume
Ratio of solutes mass to the solution’s mass
Percent by volume
Ratio of the volume of the solute to the volume of the solution

17. Quantitative descriptions of concentrations
Express concentrations as a ratio of measured amounts of solute and solvent
% by mass
% by volume
Molarity
Molality
Mole Fraction

18. GO TO KAHOOT.IT

19. Section 14.1 Types of Mixtures
Key Concepts
The individual substances in a heterogeneous mixture remain distinct.
Two types of heterogeneous mixtures are suspensions and colloids.
Brownian motion is the erratic movement of colloid particles.
Colloids exhibit the Tyndall effect.
A solution can exist as a gas, a liquid, or a solid, depending on the solvent.
Solutes in a solution can be gases, liquids, or solids.
Study Guide 1

20. Section 14.2 Solution Concentration
Key Concepts
Concentrations can be measured qualitatively and quantitatively.
Molarity is the number of moles of solute dissolved per liter of solution.
Molality is the ratio of the number of moles of solute dissolved in 1 kg of solvent.
Study Guide 2

21. Section 14.2 Solution Concentration (cont.)
Key Concepts
The number of moles of solute does not change during a dilution.
M1V1 = M2V2
Study Guide 2