1. Identifying Unknown Substances

2. Why it is important to be able to identify unknown substances:
To identify a pure substance.
To choose the best material to build an object or a machine.

3. Tungsten
Given this unknown sample of metal, how can we identify which element it is?
Physical description
Freezing point
Melting point
Density
Electrical conductivity
Reaction with other substances (Nitric Acid)
Oxidation

4. 2. Using the characteristic properties of this metal we can determine its usefulness in making a light bulb.
- A high melting point = durable at high temperatures
- Electric conductivity = a good conductor
- Is not easily oxidized = Doesn’t wear out in the presence of Oxygen.

5. Characteristic Properties: Properties that are unique to the given substance only.
Non-characteristic Properties: Properties that are common among different substances.

6. Properties of Pure Substances
Pure substances (not mixtures) can be described by describing their characteristic properties.
A Characteristic Property is one that helps us to identify a pure substance or the group to which the pure substance belongs.
They can be divided into two categories:
Characteristic physical properties
Characteristic chemical properties

7. Characteristic Physical Properties
Allow us to identify a substance without changing the nature of the substance in the process.
E.g. Finding the boiling point of water.
This changes the phase of the substance not the nature of it.
No two pure substances boil at the exact same temperature.

8. The following table contains some examples however there are more including:
Electrical conductivity Heat conductivity Hardness Malleability Magnetism

9. Physical Properties
Description
Examples
Melting Point
The temperature at which a solid becomes a liquid or a liquid becomes a solid.
Can be expressed in °c
Water: 0°c
Ethanol: -117°c
Table Salt: 801°c
Boiling Point
The temperature at which a liquid becomes a gas or a gas becomes a liquid
Water: 100°c
Ethanol: 79°c
Table Salt: 1465°c
Density
Mass per unit of volume
We often use the following formula:
Where:
P = density M = Mass V = Volume
Can be expressed in g/ml
Water: 1.0g/ml
Ethanol: 0.79g/ml
Table Salt: 19.3g/ml
Solubility
The maximum amount of solute that can be dissolved in a given volume of solvent
Can be expressed in g/L or in % (% m/V, % m/m, % V/V
Table salt in Water: 357g/L
Carbon Dioxide in water: 3.48g/L
Sugar in Water: 1792g/L

10. Density What does density mean? What does Mass mean?
What does volume mean?
Mass is a measure of the quantity of matter, which is constant all over the universe..
Volume is a measure of the amount of space that matter takes up.

11. Density Calculation p = Density m = Mass V = Volume
Calculate the density in g/mL of aluminum if a 50 mL block weighs135 g.
A student determines that a piece of an unknown material has a mass of g and a volume of 7.57 cm3.  What is the density of the material, rounded to the correct number of significant digits?

12. Why do different substances have different properties?

13. An Element
A Compound

14. Homogeneous Mixture
Heterogenous Mixture

15. Definitions
Element: A pure substance made up of only a single type of atom or molecule.
Compound: A pure substance made up of molecules containing different types of atoms.
Heterogeneous mixtures: are mixtures where we can see the different constituent that make up the mixture.
Homogeneous mixtures: are still made up of different parts, but they look the same everywhere (uniform).
Homogeneous mixtures, when liquid, are called solutions

16. Colloids
A homogeneous mixture with microscopic particles visible under a microscope.

18. Compound or Element? Homogeneous or Heterogeneous?

19. Solutions

20. Solutions
Example: A glass of water with other things dissolved inside, maybe salt.
Each of the substances in that glass of water keeps the original chemical properties.
Can it be separated?

21. Distillation
So, if you have some dissolved substances, you can boil off the water and still have those dissolved substances left over.

22. Concentration A measure of density for solutions.
Measures the amount of solute present per unit volume of solution.
The formula:
Solute = The substance that is dissolved in the solvent (minor constituent).
Solvent = The substance that the solution that is present in larger quantity. Solute is added to this substance (major constituent).
Solution = the final mixture.
C = concentration (g/L)
M = mass of solute (g)
V= volume of solution (L)

23. Examples
1. A chemist dissolves 3.50g in water to create a 300mL solution. What is the concentration of this solution?
2. Youssuf records the following measurements before mixing a salt water solution in the lab:
What is the solvent and solute in this solution?
What is the concentration of this solution?
3.5g/ 0.300L = 11.67g/L
Mass of Salt
5500 mg
Volume of Salt in the beaker
150 mL
Volume of water
0.75L
5.5g/0.90L = 6.11 g/L

24. Other Units of Concentration
Mass Percent: Example: 2.5g of salt are dissolved in 100g of water. What is the concentration of this solution?

25. Mass/Volume Percent:
2.5g salt are dissolved in 500mL of a chicken broth solution. What is the concentration of this solution?

26. Volume/Volume Percent:
50mL of acetic acid are dissolved in 1L of vinegar. What is the concentration of this solution?

27. Note for answering concentration questions
When something is dissolved in a solvent.
Ex: salt dissolved in water
You need to add the solute and solvent!!!
When you are dissolving in a solution.
Ex: acid dissolved in a vinegar solution.
You do not need to add anything before finding your concentration!!!

29. Solubility
The maximum amount of solute that can be dissolved in a given solvent.
A saturated solution is a solution that contains exactly the maximum amount of solute dissolved in it.

30. DEMO!

31. Effects of Temperature on Solubility
For most solid and liquid solutes, the solubility tends increases as temperature increases.
For gas solutes, the solubility tends to decrease as temperature increases.