Year 11 Lesson May 1-17, 2019

1. REVISION GENERAL
CHEMISTRY
UNIT 1
YEAR 11 GENERAL CHEMISTRY
MAY 1, 2019

2. Terms in General Chemistry
matter
particles
atoms
molecules
ions
properties of matter
elements
compounds
mixtures
homogenous
heterogenous
states of matter
gas
liquid
solid
physical properties
chemical properties
physical changes
chemical changes
decantation
filtration
crystallisation
evaporation
distillation
chromatography

3. SOLUTIONS
YEAR 11 GENERAL CHEMISTRY
MAY 6, 2019

4. By the end of this section, you will be able to:
Define a solution, solute and solvent (in chemistry context)
Name six different types of solutions and provide examples
each
Define saturated solution and unsaturated solution
differentiate saturated solution from unsaturated solution

5. Definition of terms
Mixtures – substances formed by combining or mixing
two or more different substances in such a way that no
chemical reaction occurs.
Examples:
• Ink, Water and Alcohol
• Sand and gravel
• Oil and water

6. Homogenous mixture – a mixture in which the
composition is uniform throughout.
Examples:
• Ink, Water and Alcohol
• Salt in water

8. Solutions – a homogenous mixture of two or more
substances.
Examples:
• Ink, Water and Alcohol
• Salt in water
• Coffee in water

9. Types of Solutions
1. LIQUID in a LIQUID  Liquid Solution
Examples:

10. 2. SOLID in a LIQUID  Liquid Solution
Examples:

11. 3. GAS in a LIQUID  Liquid Solution
Examples:

12. 4. SOLID in a SOLID  Solid Solution
Examples:

13. 5. GAS in a GAS  Gas Solution
Examples:

14. 6. LIQUID in a SOLID  Solid Solution
Examples: Liquid Hg in Ag and Sn (dental amalgam- used to
fill dental cavities)

15. Components of Solution
Salt Water Salt Solution
+ 
Solute + Solvent 
Solution
Dissolved in Produces

16. Definition of terms
Solute – is a substance to be dissolve to produce a solution
(can be solid liquid gas)
Solvent – a substance that does the dissolving (can be solid,
liquid, gas)
Dissolution- process of dissolving a solute in a solvent
- is the process in which these molecules interact
and attract each other to form a solution.

17. Definition of terms
Solubility – ability of the a substance to dissolve
- maximum amount of solute that can dissolved in
an amount of solvent.

18. Saturated solution – a solution that contains maximum
amount of solute in a given amount of solvent
Example: Solubility of NaCl in H2O at 25oC = 360 g / L
A solution containing 360 g NaCl in a litre of water is called
Saturated solution

19. unsaturated solution – a solution that contains less
amount of solute in a given amount of solvent
Example: Solubility of NaCl in H2O at 25oC = 360 g / L
A solution containing 100 g NaCl in a litre of water is called
unsaturated solution

20. supersaturated solution – a solution that contains ?
amount of solute in a given amount of solvent
Example: Solubility of NaCl in H2O at 25oC = 360 g / L
A solution containing ? g NaCl in a Liter of water is called
Saturated solution

21. VIDEO LINKS
HTTPS://WWW.YOUTUBE.COM/WATCH?V=VTMFQUNLLMY

22. By the end of this section, you will be able to:
 Define a solution, solute and solvent (in chemistry context)
---------------------------------------------------------------------------------------------------
---------------------------------------------------------------------------------------------------
---------------------------------------------------------------------------------------------------
---------------------------------------------------------------------------------------------------
---------------------------------------------------------------------------------------------------
---------------------------------------------------------------------------------------------------
 Name six different types of solutions and provide examples each
---------------------------------------------------------------------------------------------------
---------------------------------------------------------------------------------------------------
---------------------------------------------------------------------------------------------------
---------------------------------------------------------------------------------------------------
---------------------------------------------------------------------------------------------------
---------------------------------------------------------------------------------------------------
---------------------------------------------------------------------------------------------------
 Define saturated solution and unsaturated solution
---------------------------------------------------------------------------------------------------
---------------------------------------------------------------------------------------------------
---------------------------------------------------------------------------------------------------
---------------------------------------------------------------------------------------------------

23. Melting Dissolving
Put these statements into the correct part in the Venn diagram
1. Requires two substances
2. Forms a new substance
3. Mass is conserved (stays the same)
4. Forms a liquid
5. Involves a reaction
6. Involves a solid breaking down
7. Requires temperature increase
8. NaCl(aq)
9. Involves change of state
Melting and Dissolving Distinction

24. LABORATORY TECHNIQUES
IN PREPARING LIQUID
SOLUTIONS
YEAR 11 GENERAL CHEMISTRY
MAY 13, 2019

25. Safety in the Laboratory
 Behavior (mature and responsible manner)
 Wearing Personal Protection Equipment
(PPE)

26. Measuring Volumes
Graduated
cylinder
Beaker Volumetric flask

27. “Read Volume at Lower Meniscus”

28. Transferring liquids
1. Use stirring rod to guide the
liquid.
2. Use funnel to let the liquid
flow to the container.

29. Dilution techniques
2. Make sure you dilute
up to the lower meniscus
1. Use wash bottle to dilute

30. Using top balance
1. Place the weighing boat
on the top of the
balance.
1. Press TARE before
weighing your sample.

31. Storage and Labelling
Name of Solution:
Date Prepared:
Prepared by:
Example
5 % NaCl solution
May 13, 2019
By: Year 11 …

32. 0oC 10oC 20oC 30oC 60oC
35.65 35.72 35.89 36.09 37.04
Solubility of NaCl in grams in 100 ml of water

33. 0oC 10oC 20oC 30oC 60oC
7 8.1 9.6 11.1 16
Solubility of NaHCO3 in grams in 100 ml of water

34. Factors affecting Solubility
1. Temperature
For solid in a liquid
- The increase of temperature increases
solubility
- Kinetic energy of solvent molecules increases,
thus increasing the chance to break the solute
molecule

35. For gas in a liquid
- The increase of temperature decreases solubility
- Kinetic energy of gas molecules increases, thus
increasing the chance to break away from solvent

36. 2. Pressure
For gas in a liquid
- The increase of pressure increases solubility
- Solute and solvent molecules are constraint in
small space, thus higher possibility of contact,
increasing solubility.

37. 3. Nature of the Substance
“Like dissolves like”

38. 4. Surface Area
Affects the RATE of dissolution
but does not increases solubility
More solute molecules get in contact
with solvent molecules, thus
increases the speed of dissolution

39. 5. Stirring
Affects the RATE of dissolution
but does not increases solubility
Stirring allows solute and solvent
molecules to continually be in contact

40. Analysis
Nitrox is an “enriched air” used for scuba diver’s
O2 tank. It has about 40% O2 and about 60% N2.
a. As divers swim deeper, what happens to the
solubility of N2 in their blood?
b. If the diver abruptly ascend to the surface,
what happens to the N2 solubility?

41. Analysis
What happens to the Dissolved Oxygen in the river
if a high temperature waste water will be dumped?

42. Parts Per Million (ppm)
• https://ed.ted.com/lessons/how-to-visualize-one-part-per-million-
kim-preshoff-the-ted-ed-community#watch

43. Calculation concentrations in ppm
Examples:
1. A 15 grams (g) soil sample was found to contain
0.098 milligram (mg) of Calcium (Ca). What is the
concentration of Calcium in the soil, expressed in
ppm?

44. 2. A 50 grams rock sample was analyzed in a mining
laboratory. The result shows that the sample
contains 0.20 milligrams of Gold (Au). Calculate the
concentration of Gold in ppm.