1. Chemistry
Solutions Unit

2. A solution is a homogenous mixture
What is a solution?
A solution is a homogenous mixture

3. What is a homogenous mixture?
You cannot identify what the mixture is made up of.
It looks the same throughout

4. What are the two main parts of a solution?
1. The Solute- the dissolved substance (usually in a smaller amount)
Ex. Sugar, salt
2. The Solvent- the dissolver (usually in a larger amount)
Ex. Water

5. What is the Universal solvent?
Water

6. How are solutions formed?
Through a process called Solvation also known as dissolving.

7. What affects the rate of solvation (dissolving)?
Heating
Stirring
Surface Area

8. How does heating affect dissolving?
At higher temperature, the molecules of the solvent move around faster and contact the solute more often. Speeds up dissolving.

9. How does stirring affect dissolving?
Stirring moves fresh solvent into contact with the solute.

10. How does surface area affect dissolving?
Smaller pieces increase the amount of surface area of the solute.
Ex. Think of how fast a breath mint dissolves when you chew it

11. What is Solubility?
The maximum amount of substance that will be dissolved at a specific temperature Units are: g of solute 100 g of H2O

12. What are the types of solutions?
Unsaturated
Saturated
Supersaturated

13. What is an unsaturated solution?
A solution where more solutes can be added and will completely dissolve. Ex. Adding more sugar to tea and it still dissolves

14. What is an Saturated solution?
A solution that contains the maximum amount of solutes dissolved Ex. You hit the point where if you add any more sugar to the tea it will not dissolve

15. What is a Supersaturated solution?
A solution that contains more solutes than it can hold. Ex. You put to much sugar in the tea now it will not dissolve and the sugar settles to the bottom.

16. How do you know that a solution is Supersaturated?
The solutes will settle to the bottom of the container and will eventually begin to crystallize.

17. How do we know what type of solution?
We use Solubility Curves!

18. Get out solubility chart and color each line on the chart with a different color, tape in notebook when done 

19. How do you read solubility chart?
If it falls on the line its saturated
If it falls BELOW the line its unsaturated
If it falls ABOVE the line its supersaturated

20. If the line is decreasing is that a solid or gas?
If the line is decreasing it is a gas
In other words as temperature increase the solubility of a gas decrease
Two on the chart
NH3
Ce2(SO4)3

21. If the line is increasing is it a solid or gas?
It’s a solid!
So everything else on the chart
As the temperature increase so does the solublity for a solid

22. What is the solubility of KCl at 10C?

23. What is the solubility of NH3 at 600C?

24. What is the solubility of NH4Cl at 750C?

25. What mass of KClO3 will dissolve in 50g of water at 200C?

26. To make a solution at 20oC you have 77g of NH4Cl
To make a solution at 20oC you have 77g of NH4Cl. How many grams of water would?

27. You require 350g of solution at 40oC
You require 350g of solution at 40oC. How many grams of NaNO3 would be necessary to make that solution?

28. At 90C, 10g of Ce2(SO4)3 is dissolved in 100g of water
At 90C, 10g of Ce2(SO4)3 is dissolved in 100g of water. Is this solution saturated, unsaturated or supersaturated?

29. This the measure of how much solute is dissolved in a solvent.
What is concentration?
This the measure of how much solute is dissolved in a solvent.

30. How do you calculate concentration for solutions?
We use Molarity! Represented by a big M

31. What is the formula?

32. example
0.5 moles of NaCl is dissolved to make 0.05 liters. Calculate the molarity.

33. Example 2
How many moles of Na2CO3 are there in 10.0 L of 2.0M solution?

34. What mass of NaOH is needed to make 1.5L of 1.0M solution?

35. What is the molarity of a solution containing 42 grams of solute in 950.mL of solution? The molar mass of solute is 50.g/mol.

36. What mass of CaCO3 is needed to make 2.5L of 2.0M solution

37. What is a metal solution called?
An alloy This solution contains two or more metals mixed.

38. What is a water solution that conducts electricity called?
An electrolyte

39. What are heterogenous mixtures called?
Suspensions
Particles settle
They can be easily separated by filtration

40. Examples
Sand and water

41. What are colloids?
Uniform mixtures (homogenous mixtures) that do not settle but instead are dispersed throughout the solvent They CAN scatter light!

42. Examples of colloids
Milk Lotion Fog

43. What is Tyndall effect?
This is the scattering of light of colloidal particles. Solutions CANNOT scatter light.

44. What is the Tyndall effect used for?
It is used to distinguish between solutions and colloids

45. What is it called when a substance dissolves?
Soluble
Ex. Salt is soluble in water

46. What is it called when a substance does not dissolve?
Insoluble Ex. Chalk in insoluble in water

47. What is it called when something dissolves in water?
An aqueous solution Abbreviated (aq)

48. What is it called when a solid forms in a solution?
A precipitate

49. How do some solutes dissolve in a solvent and others do not?
It depends on the polarity of both the solute and the solvent.

50. The “Like dissolves like” rule
How does this work?
The “Like dissolves like” rule

51. What is the like dissolve like rule?
A polar substance will dissolve another polar substance
A non-polar substance will dissolve another non-polar substance

52. What happens if you mix a polar and a non-polar substance?
They DO NOT MIX!!!!

53. Use the Solubility Chart to tell if a substance will dissolve in water!

54. How do you know if a reaction will happen?
A solid (precipitate) product MUST be produced for a reaction to occur. Ex. (aq) + (aq)  (aq) + (s) A reaction occurs!!!

55. Example
CuSO4 + Na2CO3  Na2SO4(___) + CoCO3(___)

56. What is produced when two (aq) products are formed?
Ex. (aq) + (aq)  (aq) + (aq) A mixture forms!!

57. Example
CuSO AgNO3  Ag2SO4 (___)+ Cu(NO3)2 (___)