1. Mixtures, Solubility, and Solutions
Chapter 13
Mixtures, Solubility, and Solutions

2. 13.1-Substances and Mixtures
A substance is matter with composition that is always the same
Two major types of substances
Elements
Compounds

3. 13.1-Substances and Mixtures
Elements are substances that consist of just one type of atom
Elements are found on the periodic table
Each element has its own characteristic properties.
These include boiling/melting point, density, reactivity, flammability, etc.
An element may share one or two properties with another element, but it will not share all its properties with another element. There will be specific properties for each element.

4. 13.1-Substances and Mixtures
Compounds are substances containing atoms of two or more different elements chemically bonded together
Occurs as a result of a chemical reaction
Compounds are represented by chemical formulas
Ex. NaCl, CO2, H2O

5. 13.1-Substances and Mixtures
Properties of compounds
Compounds have a SET RATIO
Ex. H2O (water) vs H2O2 (hydrogen peroxide)
Each compound has its own physical properties and chemical properties.
The properties of a compound are different from the properties of the elements that form it.
Sodium Chlorine  Table Salt
Explosive soft metal Yellow Piousness Gas

6. 13.1-Substances and Mixtures
Are they elements or compounds?

7. 13.1-Substances and Mixtures
What is a mixture?
A Mixture is two or more substances that are physically blended but are not chemically bonded together
No chemical reaction
No compound formed
Each substance keeps its original identity
No fixed ratio—NOT always the same

8. 13.1-Substances and Mixtures
Types of Mixtures
Heterogeneous
Homogeneous

9. 13.1-Substances and Mixtures
A heterogeneous mixture is a type of mixture in which the individual substances are unevenly mixed
Two different samples of the same mixture can have different amounts of substances
Example: salad, pizza, granola bar

10. 13.1-Substances and Mixtures
Types of heterogeneous mixtures
Suspension
A suspension is a mixture in which particles are large enough to be dispersed, but they settle out over time
Can be filtered, can scatter light
Colloid
A colloid is a mixture in which the particles are medium in size and dispersed throughout but are not heavy enough to settle out
Cannot be filtered, can scatter light

11. 13.1-Substances and Mixtures
A homogeneous Mixture is a type of mixture in which the individual substance are evenly mixed
Example: Apple juice, salt water
Appears to be a single substance due to small particles
Cannot be filtered, cannot scatter light
Also known as a solution

12. 13.1-Substances and Mixtures
Solution
Colloid
Suspension
Particle size:
S, M, L
 small
 medium
 large
Filter?
 no
 yes
Scatter light?
Settle out?
 No no
Yes
Two examples
 Salt water
Kool Aide
 Mayo
milk
 Italian dressing
Snow globe

13. 13.1-Substances and Mixtures
Compounds
Made of elements, compounds or both
Made of elements
No change in original properties of components
Change in original properties of components
Separated by physical means
Separated by chemical means
Formed by using any ratio of components
Formed using a set ratio of components

14. 13.2- Properties of Solutions
Parts of a solution
The solute is the substance that is dissolved
The solvent is the substance that exists in the greatest quantity in a solution

15. 13.2- Properties of Solutions
Concentration of Solutions
The concentration is the amount of a particular solute in a given amount of solvent
Units: g/mL
Lots of solute  concentrated
Little solute dilute

16. 13.2- Properties of Solutions
The term soluble means able to dissolve. Insoluble means unable to dissolve.
Solutions can be solids, liquids, or gases.
Solubility- is the maximum amount of solute that can dissolve in a given amount of solvent at a given temperature and pressure

17. 13.2- Properties of Solutions
Solubility
Saturated solutions are solutions that contain the maximum amount of solute that the solution can hold at a given temperature and pressure
Unsaturated solutions are solutions that can still dissolve more solute at a given temperature and pressure

18. 13.2- Properties of Solutions
How does temperature affect solubility?
For liquid solvents
A higher temperature decreases the solubility of a gas
A higher temperature inceases the solubility of a solid or liquid
How does pressure affect solubility?
A higher pressure increases the solubility of a gas

19. 13.2- Properties of Solutions
What is a solubility curve?
This is a graph that shows how solubility of a substance can change with temperature
Reading the graph
X-axis – temperature
Y-axis – solubility

20. To what temperature would water have to be heated if I wanted to dissolve 70 grams of NH3?
To what temperature would water have to be heated if I wanted to dissolve 70 grams of NH4Cl?
How many grams of KClO3 can be dissolved into 100 g H2O heated to 70°C?
How many grams of KClO3 can be dissolved into 100g H2O heated to 45°C?

21. 13.2- Properties of Solutions
How fast a solute dissolves
All speed up dissolving

22. Mixture vs. compound vs. element

23. Elements, Compounds, Mixtures
Elements
Compounds
Mixtures
How many parts make it up?  1
 2 or more
 2 or more elements or compounds
Pure: more than one substance?
 pure
 Not pure
Chemically or physically combined?
 N/A
 Chemically
physically
Chemical change to make them?
 Yes no
Fixed ratio?
Yes
How separated: chemically/
physically?
Chemically