1. Chapter 12: Solutions

2. Goals:
Read Ch (pg )
Title the notes “Ch 12 Solutions” (in notes section)
Copy table 1 pg 402 *summarize/abbreviate as possible
Table 2 pg 404
Table 3 pg 404
Read and take notes/ create vocab list
Materials, Procedures and Hypothesis for final science fair project: Due Friday
Pg 5 and 6 of packet
Get PhET activity to start (Friday activity, due next Monday)

3. Section 1- Types of Mixtures
Solutions are homogeneous mixtures of two or more substances in a single phase.
Soluble describes a substance as capable of being dissolved.
Solvent is the dissolving medium in a solution.
Solute is the substance that is dissolved in a solution.

4. Types of Solutions
Solutions can be in any of the three common physical states.
solid- a mixture of metals called an alloy
liquid- salt water, sugar water, Kool-Aid…
gas- the atmosphere

5. Suspensions & Colloids
A suspension has large particles that settle out of a solvent. ex. muddy water
A colloid has intermediate size particles. Also called an emulsion or a foam.

6. Solutes: electrolytes vs. nonelectrolytes
An electrolyte is a substance that dissolves in water to give a solution that conducts electricity.
A nonelectrolyte is a substance that dissolves in water to give a solution that does NOT conduct electricity.
Do section review questions #1, #2, & #6 on page 406.

7. Ch 12.2- The Solution Process
Factors that affect the rate of solution (how quickly a substance dissolves):
Any process that increases the number of contacts between the solvent and the solute will increase the solution rate.
increasing the surface area of the solute
agitating (shaking or stirring) the solution
heating the solvent

8. Graphs All Graphs Need: Title Labeled axis Units as needed Key:
Dependant variable
(units)
independent variable (units)
All Graphs Need:
Title
Labeled axis
Units as needed
Key:

9. Warm up: Compare and contrast molarity and molality.
If given or asked for grams, how do you relate grams to moles?

10. Ex C: Suppose you want to dissolve 205g of Na2CO3 in enough water to make 5.00L of solution. What is the molarity?
Molar mass= 106.0g/mol
205/106 =

11. Solubility Vocab
Solubility is a measurement of how much solute will dissolve in a specific amount of solvent at a specific temperature to make a saturated solution.
“Likes dissolve likes”- polar solvents dissolve polar solutes & nonpolar solvents dissolve nonpolar solutes.
Hydration: the solution process with water as the solvent.
Hydrates: ionic compounds that have formed crystals that have incorporated water molecules in their structure.
Immiscible liquids are not soluble in one another. eg. oil & water
Miscible liquids dissolve freely in one another in any proportion. eg. water & alcohol

12. Solutions
Solution equilibrium: the physical state in which the opposing processes of dissolution and crystallization occur at equal rates.
Dissolution: dissolve
Crystallization: form solid

13. Factors that affect the rate of solution: (how quickly a substance dissolves)
Any process that increases the number of contacts between the solvent and the solute will increase the solution rate.
Increase solution rate by:
increasing the surface area of the solute
agitating (shaking or stirring) the solution
heating the solvent

14. temp. and pressure affects on solubility:
Increasing the pressure increases the solubility of gases in a liquid.
has no effect on the solubility of a solid in a liquid
For gas in liquid, increasing temp decreases the solubility.
For solid in liquid, increasing temperature often increases the solubility

15. Henry’s Law: the solubility of a gas in a liquid is directly proportional to the partial pressure of the gas on the surface of the liquid.
Effervescence is the rapid escape of a gas from a liquid in which the gas is dissolved.
A solvated solute particle is surrounded
by solvent molecules.

16. saturated solution: contains the maximum amount of dissolved solute.
unsaturated solution: contains less than the maximum amount of dissolved solute.
A supersaturated solution: contains more dissolved solute than a saturated solution.

17. Solubility curve
Solubility is a measurement of how much solute will dissolve in a specific amount of solvent at a specific temperature to make a saturated solution.

18. Will the solubility increase, decrease, remain the same?
Soda is opened and heated (the gas)?
Solid sodium chloride is dissolved is water as it is heated.
Carbon dioxide is dissolved in water as it is cooled.
Potassium chloride is added to a saturated solution.
The surface pressure of salt water is increased.
Surface pressure of dissolved oxygen is increased.
Decrease
Increase
Same
increase

19. Enthalpy of solution: amount of heat absorbed by a solution when a specific amount of solute dissolves in a solvent.

20. Classwork Solutions Matching
Put in classwork section, number your page and write out the vocab word for answers
2. When done, work on solutions PHeT simulation (see handout section of website)
3. Then work on study guide

21. Classwork Solutions Matching
Put in classwork section, number your page and write out the vocab word for answers
Ch 12.3 Practice C and E
Answer questions:
Pg 421 Practice #1-3
Pg 424 Practice #1-2
Solutions on pg 920

22. Solutions
Soluble
Solvent
Solute
Nonelectrolyte
miscible
Colloid
Suspension
Supersaturated
Saturated
unsaturated
Electrolyte
Solubility
immiscible B.
Solute
Immiscible
Colloid
Solution, miscible
Saturated
Electrolyte
Solvent
suspension

23. 12.3 Concentrations of Solutions
The concentration measure of the amount of solute dissolved in a given amount of solvent or solution.
Molarity (M) is the number of moles of solute in one liter of solution.
M = #mol L
Do practice problems #1, #2, & #3 on page 421.

24. Warm up:
What is a solution?
A solute?
A solvent?

25. 12.3 Concentrations of Solutions
Molarity (M) is the number of moles of solute in one liter of solution.
M = mol L
Ex A: pg 420
What is the molarity of a 3.50L solution that contains 90.0g of NaCl
Molar mass = 58.44g/mol
90.0g x (1mol/58.44g) = 1.54 mol
1.54 mol = .440 M NaCl
3.50 L
Do practice problems #1, #2, & #3 on page 421.

26. How many moles of HCl in 0.8L of a 0.5M solution?
Ex B:
How many moles of HCl in 0.8L of a 0.5M solution?
M = mol .5M = mol
L L
.8L(.5mol/L) = .4mol HCl

27. Molality (m) is the concentration of a solution expressed in moles of solute per kilogram of solvent.
m = mol kg
Ex D: pg 423
A solution dissolved .0500mol C12H22O11 in 125g of water, what is the molal concentration?
125g (1kg/1000g) = .125kg
.0500 mol = .400 m C12H22O kg
Do practice problems #1 & #2 on page 424.

28. Read Ch12.1-12.2 (pg 400-412.) and take notes in note section of notebook.
Title the notes “Ch 12 Solutions”
Copy table 1 pg 401
Table 2 pg 404
Table 3 pg 404
Create a vocab list

29. Graphs All Graphs Need: Title Labeled axis Units as needed Key:
Dependant variable
(units)
independent variable (units)
All Graphs Need:
Title
Labeled axis
Units as needed
Key:

30. What are the independent and dependent variables
What are the independent and dependent variables? What is the saturation point of the blue chemical? What unit is used to measure saturation?

32. Solubility curve
Solubility is a measurement of how much solute will dissolve in a specific amount of solvent at a specific temperature to make a saturated solution.

34. Solution Concentrations
Percent composition by mass (%) is a concentration that expresses the percent of solute in a solution.
% = #g solute x 100
# g solution
Do section review problems #1, #2, & #3 on page 424.

35. matching
homogeneous mixtures of two or more substances in a single phase.
describes a substance as capable of being dissolved.
the dissolving medium in a solution.
the substance that is dissolved in a solution.
Doe not conduct electricity
Liquids that dissolve freely in one another
intermediate size particles, also called an emulsion or a foam
large particles that settle out of a solvent.
Contains more dissolved solute than saturated solution under same conditions
Solution containing maximum amount of dissolved solute
Contains less solute than possible under the existing conditions
Conducts electricity
Amount of substance to form a saturated solution under specific conditions
Liquids that are not soluble in each other
Solutions
Soluble
Solvent
Solute
Nonelectrolyte
miscible
Colloid
Suspension
Supersaturated
Saturated
unsaturated
Electrolyte
Solubility
immiscible
Soluble
Solvent
Solute
Solutions
Solubility
Electrolyte
Nonelectrolyte
Immiscible
Miscible
Suspention
Saturated
Unsaturated
Supersaturated
Colloid

36. Chapter 12 Test Review multiple choice
define & identify suspensions & solutions
define an alloy
define & identify electrolytes & nonelectrolytes
factors that affect the rate of dissolution
definitions of unsaturated, saturated & supersaturated solutions
general rules for predicting whether a solute is soluble in a solvent
definition of solubility
effects of temperature & pressure on the solubility of gases and solids in liquids
definitions of molarity (M) and molality (m)
solving molarity & molality problems
FORMULAS: M = #mol/L m = #mol/kg