1. The Material World Properties of Matter and Solutions

2. Properties of Matter

3. Matter Matter is anything that has a mass and volume.
Has a certain weight and takes up space.
Matter exists in one of three states or phases:
Solid
Liquid
Gas
Matter has a number of properties, both characteristic and non-characteristic.

4. Non-characteristic Properties
Any property that is NOT unique to a specific type of matter.
These properties help to determine an unknown substance, but cannot precisely identify it.
Mass
Volume
Temperature
Acidity / Alkalinity
Colour
Etc.

5. Characteristic Physical Properties
Any property that is unique to a specific type of matter. That is, we can precisely identify an unknown substance using these properties.
Melting point: H₂O is the only matter that melts at 0°C
Boiling point: H₂O is the only matter that boils at 100°C
Density: mass per unit of volume.
Solubility: Maximum amount of solute dissolved in a solvent.
Note: Melting point and boiling point were covered in Cycle One. Density and solubility are new this year – more info on the next slides.

6. Density Why do some objects float and others don’t? Density!
Definition: Mass per unit of volume.
Unit: g/cm³ or kg/m³ if the object is especially large.
Instruments: balance, (for mass), graduated cylinder, (for volume), calculator, (to divide mass by volume).
How to calculate: Find the mass. Divide by the volume. m/V

7. Solubility
Some substances are soluble in others. This means that they will dissolve.
Definition: The maximum amount of solute that can be dissolved in a solvent.
Unit: g/L often, but there are others as well. %m/V, %V/V, %m/m

8. Solutions

9. Review from Cycle One
Mixtures are any type of matter that contains at least two substances. This means there are two types of particles that can be separated by a physical process. Air, milk and granite are examples of mixtures.
Pure substances are any type of matter made up of one substance, that is, one type of particle. They can only be separated by a chemical process. Water and salt are examples.

10. Atoms and Molecules
Matter
Pure Substances
Mixtures / Solutions
Compounds
Elements
Heterogeneous
Homogenous
Colloids
Solutions

11. …
A heterogeneous mixture is made up of two substances that are distinguishable to the naked eye. Granite, a $2 coin and vegetable soup are examples.
A homogeneous mixture is made up of two substances, but the they are uniformly mixed and therefore the particles are indistinguishable to the naked eye. Milk and mayonnaise are examples. There are two types of homogeneous mixtures:
Colloids
Solutions

12. Colloids
Colloids are homogeneous mixtures in which, when observed with a magnifying glass or a microscope, the various particles are evident.
When milk or mayonnaise are observed under a microscope, their fat particles are easily distinguished from their water particles.
When blood is observed, the various blood cells, platelets and plasma are seen.

13. Homogenized
Milk

14. Solutions
A solution is a homogeneous mixture whose parts are not distinguishable, even with a microscope or magnifying glass. Generally, solutions are transparent.
Apple juice is made of sugars and other substances which are dissolved in water. A ten-karat gold ring is made of silver and copper, dissolved in gold.
The substance that is dissolved in the solute – sugars and silver and copper in the examples. There is usually less of a solute.
The substance that dissolves the solute is the solvent – water and gold in the previous examples. There is usually more of a solvent.

15. … We have already looked at many solutions found in the human body.
Solute
Solvent
Urine
Urea, salts
Water
Sweat
Salts
Tears
Lymph
Oxygen, carbon dioxide, salts

16. Phases of solution substances (Solute + Solvent  Solution)
Gas + Gas  gas solution
Oxygen, carbon dioxide, water vapour, argon, etc.
Nitrogen
Air
Gas + Liquid  liquid solution
Carbon dioxide
Water
Carbonated water
Liquid + Liquid  liquid solution
Alcohol, aromatic substances
Wine
Solid + Liquid  Liquid solution
Salt
Salt water
Solid + Solid  Solid solution
Carbon
Iron
Steel
The phase of matter of the SOLVENT will determine the phase of matter of the solution itself.

17. Properties of Solutions
Solutions have many properties, both characteristic and non-characteristic, (see earlier in this package).
Solutions have a few other properties that only apply to solutions. This is how solutions are distinguished from each other.
Concentration
Dilution
Solubility

18. Concentration
The concentration of a solution is the quantity of dissolved solute in a given quantity of solution.
Concentration is determined by calculating:
C = m / V
Where C is Concentration in g/L, m is mass of the solute in g, and V is volume of the solution in L.

19. …
A solution is said to be concentrated when it contains a large amount of solute.
This would be like adding an extra spoonful of Kool-Aid than the recipe calls for. You drink would be darker and more sugary.
So, in order to increase the concentration of a solution, simply add more solute.

20. Dilution
Dilution is a lab technique that involves decreasing the concentration of a solution by adding more solvent.
Adding more of the solvent will dilute your solution.
Examples: Adding water to frozen juice concentrate to make juice.

21. Most concentrated
Less concentrated
Least concentrated

22. Solute varies, solvent costant
Least concentrated
Less concentrated
Most concentrated

23. Solubility
There is a limit to the amount of solute that can be added to a solvent. The maximum amount refers to solubility.
Unsaturated
If the solution contains less than the maximum amount of solute.
Saturated
If the solution contains the maximum amount of solute.
Supersaturated
If the solution contains more than the maximum amount of solute.

24. Solubility depends on many factors:
Nature of the solvent
Temperature
Nature of the Solvent:
Some solutes do not dissolve well or at all in certain solvents, so it is important to know the solvent.
Salt dissolves easily in water, but not in oil – hydrophilic.
Substances that dissolve easily in oils are called lipophilic.

25. Gases, however, become less soluble when temperature increases.
The solubility of many substances, particularly solids, increases as temperature increases.
This is why it is easier to make juice with warm water than cold.
Gases, however, become less soluble when temperature increases.
This is why fish populations are affected during summer heat waves – less oxygen in lakes.
A warm can of soft drink releases more carbon dioxide when opened than a cold one.