1. Solutions
Chapter 15

2. Chemcatalyst:___.___
Think back to marking period one and define in your own words the difference between a homogeneous and a heterogeneous mixture?

3. Mixtures Uniform throughout 1 continual phase
HOMOGENEOUS
HETEROGENEOUS
Uniform throughout
1 continual phase
Example: solutions like salt water
Not uniform throughout
Multiple phases
Example: Oil and water

4. Other Heterogeneous Mixtures:
Suspension
Colloids
Particles are much larger
Do not stay suspend indefinitely
Particles begin to separate out
Multiple phases
Example: Clay in water or sand in water
Particles are medium-sized
Spread out and dispersed
Cloudy or milky appearance
Examples: Whipped cream, glue, milk, or mayo

5. Did you know?
Colloidal solutions, like fog, disperse or separate light!
It is called the Tyndall effect!
When light passes through it, the particles reflect or scatter the light in all different directions!

6. Mini Lab on types

7. Properties of Solutions
Chapter 16

8. Chemcatalyst: __.__
Predict and explain whether sugar will dissolve faster in iced tea or hot tea.
Follow up: Which would dissolve faster cubed sugar or granular sugar?

9. Solutions, eh? Solutions are homogeneous mixtures!
Meaning same throughout 
They can be solids, liquids, or gases!

10. How do I make this said solution…?
A solution has a solute and solvent
SOLUTE
SOLVENT
The dissolved particles in a solution is known as a solvent
The solute will become dispersed throughout the solvent
Can be solids, liquids, or gases
The dissolving medium is the solvent
The solvent dissolves the solute
Can be solids, liquids, or gases

11. Why do you stir sugar into your tea?

12. Agitation Stirring or shaking speeds up the solution process
More of the solute will be brought into contact with solvent
Only affects the time it takes to dissolve, not the amount of solute dissolving
Insoluble will always be insoluble

13. Back to the C.C Hot or cold tea dissolves sugar faster?

14. Temperature
High temperature, more kinetic energy molecules move faster
The rapid motion is an increase in collisions between the solvent and the solute

15. Back to the C.C. follow up Sugar cube or granular sugar dissolves faster?

16. Particle Size of Solute
The smaller the particles, the greater surface area to collide with the solvent
The more surface area, more collisions and the faster rate of dissolving

17. Chemcatalyst __.___ What does it mean if something is soluble?
Give an example

18. Solubility
The amount of solute that dissolves in a given quantity of solvent at a given temperature and pressure
This amount creates a saturated solution
Solubility is expressed in g/100 g H2O

19. Think about this… Kool aid man, “Ohh yeaa” ©
What if I put the entire container in?
What does it look/taste like if I do not put all of it in?

20. Supersaturated vs Unsaturated
A solution that contains more solute that is able to dissolve
Only so much will dissolve, the rest will be solid on the bottom
Ex: Adding too much of the Kool Aid powder, rock candy
A solution that contains less solute than the saturated solution
Ex: Not adding enough Kool Aid Powder

21. Did you know?
Miscible means soluble or the ability to dissolve in one another
Example: Water and Ethanol
Immiscible means they are insoluble
Example: Oil and water

22. Mini Lab Solution and solubility mini lab Play at end of lab

23. Factors affecting solubility
Temperature
Pressure
In general, the solubility of a solid increases as the solvent is heated
In general, the solubility of a gas increases as the solvent is cooled
Little effect on the solubility of solids and liquids
If the pressure above the liquid increases, the solubility of the gas increases

24. Henry’s Law
At a given temperature, the solubility of a gas in a liquid is proportional to the pressure above the liquid.
If the pressure increases, the solubility increases
Example: Carbonated soda (CO2)

25. Chemcatalyst: __.___ What would you need to change?
A saturated solution to an unsaturated solution
A saturated solution to a supersaturated solution
An unsaturated solution to a saturated solution

26. What is concentration?
The measure of the amount of solute that is dissolved in a given solvent
Depending on the amount it can be classified as dilute or concentrated

27. Concentrated solution
Concentration
Dilute solution
Concentrated solution
A small amount of solute dissolved
Large amounts of solute dissolved
*** Only qualitative, not QUANTITATIVE

28. If that’s qualitative, then how do we measure concentration?

29. Molarity (M)
Molarity is the number of moles dissolved in 1 liter of solution
Referred to a molar concentration or solution
Units are moles/liter or represented as M (molar)
Molarity = Moles of the solute
Liters of the solution
** Volume must be in liters

30. Let’s calculate the molarity together!
What is the molarity of a solution that contains 0.70 mol of NaCl in 250. mL?
250. 𝑚𝐿 1 𝑥 1 𝐿 1000𝑚𝐿 =0.250 𝐿
Molarity= 𝑚𝑜𝑙𝑒𝑠 𝐿 =2.8 𝑀

31. Try this one on your own:
IV fluid has 0.15 moles of saline solution in it, what would the molarity be for 200. mL?
200. 𝑚𝐿 1 𝑥 1 𝐿 1000𝑚𝐿 =0.200 𝐿
Molarity= 𝑚𝑜𝑙𝑒𝑠 𝐿 =.75 𝑀

32. How do you make a solution?
Mini Lab

33. Reach question!
A solution has a volume of 2.0 L and contains 36.0 grams of glucose. If the molar mass of glucose is 180 g/mol, what is the molarity of the solution?
0.10M

34. Chemcatalyst: __.__
What would the molarity be a solution that has moles of solute and a given volume of 400. mL?
Show work with units, try your best with SF 

35. Dilution 1 is initial conditions( concentrated solution)
To create a dilution, the number of moles of solution will be reduced
A dilution is created from a concentrated solution
We use this equation:
M1V1 =M2V2
1 is initial conditions( concentrated solution)
2 is final conditions (dilute “new” conditions)

36. Let’s do this together! M1V1 =M2V2 (2.00 M) V1= (0.400 M) (100.0 mL)
How many mL of 2.00 M MgSO4 solution must be diluted to prepare a mL of M MgSO4 ?
M1= 2.00 M
V1= ? mL
M2= M
V2= mL
M1V1 =M2V2
(2.00 M) V1= (0.400 M) (100.0 mL)
V1= 20.0 mL

37. Try this one on your own! M1V1 =M2V2 (4.00 M) V1= (0.760 M) (250.0 mL)
How many mL of a solution of 4.00 M KI are needed to prepare mL of M KI
M1= 4.00 M
V1= ? mL
M2= M
V2= mL
M1V1 =M2V2
(4.00 M) V1= (0.760 M) (250.0 mL)
V1= 47.5 mL

38. Chemcatalyst: __.__
How many moles of ammonium nitrate are in 355 mL of a M solution
0.151 mol
How many mL of a 1.0 M solution to prepare 250. mL of a 0.20 M solution?
50. mL