1. Advanced Chemistry Mrs. Klingaman
Ch. 12: Solutions
Advanced Chemistry
Mrs. Klingaman

2. 1. Define Soluble-
Capable of being dissolved
2. Define Solution-
A homogeneous mixture of two or more substances uniformly dispersed through a single phase

3. 3. Define Solvent-
The dissolving medium in the solution
4. Define Solute-
The substance being dissolved in the solution

4. 5.
The solute is designated as the component of a solution that is of ________ quantity.
lesser

5. rubbing alcohol (l) in H2O (l)6.
Solutions may exist as ______, ________, or _______.
gases
liquids
solids
Solute State
Solvent State
Example
Gas
O2 (g) in N2 (g)
Liquid
CO2 (g) in H2O (l)
rubbing alcohol (l) in H2O (l)
Solid
Hg (l) in Ag (s) & Sn (s)
– dental amalgam
Sugar (s) in H2O (l)
Cu (s) in Ni (s)

6. Sterling Silver (Ag & Cu) Desirable Properties: - more strength
7. Give an example of an alloy and list the properties of that alloy that make it more desirable than the individual pure metal from which it is composed
Brass (Zn & Cu)
Sterling Silver (Ag & Cu)
Desirable Properties:
- more strength
- greater resistance to corrosion

7. 8. Define Suspension-
Particles in a solvent that are so large that they settle out of the solution unless the mixture is constantly stirred or agitated
Ex: jar of muddy water

8. 9. Define Colloid -
Particles that are of intermediate size between those in solutions and suspensions
a) an emulsion is a liquid in a liquid example of a colloid (milk)
b) clouds and fog are examples of colloids called liquid aerosols in which a liquid is dispersed in a gas
c) Foam is a type of colloid in which a gas is dispersed throughout a liquid
d) A sol is a type of colloid in which a solid is dispersed throughout a liquid (ex: paint)

9. 10. Define Tyndall effect -
Light is scattered by colloidal particles in a transparent medium
The Tyndall effect can be used to distinguish a solution from a colloid
(colloids will scatter light making a beam visible)

10. 11. Define Brownian Motion-
Under a microscope, the tiny particles in a colloid are in motion due to collisions of rapidly moving particles suspended in a fluid

11. 12. Figure 1.7 – Properties of solutions, suspensions, and colloids
homogeneous
heterogeneous
particle size:
0.01 – 1 nm
1 – 1000 nm
over 1000 nm
Do NOT separate upon standing
Particles settle out after standing
Can’t be separated by filtration
CAN be separated by filtration
Do NOT scatter light
Scatter light
(Tyndall effect)
May scatter light but are not transparent

12. Types of Mixtures Activity
(a) Solution, (b) Suspension, or (c) Colloid
____ - particles in a solvent that are of intermediate size; solution scatters light; does not separate & cannot be filtered
____ - homogeneous mixture of 2+ substances in a single phase; solution does not scatter light; does not does not separate & cannot be filtered
____- particles in a solvent are so large that they settle out upon standing; solution may scatter light; solution can be separated by filtration c a b

13. 4. Define Nonelectrolyte
13. Define Electrolyte
A substance that dissolves in water to give a solution which conducts electricity (NaCl, soluble ionic compounds, acids, bases)
4. Define Nonelectrolyte
A substance that dissolves in water to give a solution that does not conduct an electric current (sugar, soluble covalent compounds)

14. Factors that Affect Solubility - Solids Packet pg. 5
“Like-dissolves-Like”–
polar solvents dissolve polar (and ionic) solutes and nonpolar solvents dissolve nonpolar solutes

15. Factors that Affect Solubility - Solids Packet pg. 5
2) Surface Area of Solute – increasing the surface area of solute exposed to the solvent increases solubility (crushing up a solid; sugar cube vs. granulated sugar)

16. Factors that Affect Solubility - Solids Packet pg. 5
3) Stirring/Agitation– movement of the solute has the same effect as increasing the surface area exposed to the solvent = increased collisions = increased solubility

17. Factors that Affect Solubility - Solids Packet pg. 5
4) Temperature – Increased temperature increases the solubility of a solid (or liquid) because the KE is increased = molecules moving faster = more collisions between solute & solvent

18. Factors that Affect Solubility - Gases Packet pg. 5
Pressure–
Increased pressure on a gas increases its solubility in a liquid (forces gas particles closer to liquid solvent so that they can collide

19. Factors that Affect Solubility - Gases Packet pg. 5
2) Temperature– LOWER temperatures increase gas solubility  this slows down the gas particles so they can interact/collide with the liquid solvent

20. Factors that Affect Solubility - Gases Packet pg. 5
3) Molecular Size– The larger the gas molecule (larger molar mass) the greater the solubility of the gas in a liquid solvent (due to greater forces of attraction between solute/solvent)

21. The Process of Solvation (aka: dissociation for ionic solutes) Packet pg. 6
Solvation– A physical process in which the molecules (or ions) making up a solid, soluble SOLUTE are separated and surrounded by solvent molecules.

22. The Process of Solvation (aka: dissociation for ionic solutes) Packet pg. 6
Step 1 – The solid solute must be SOLUBLE in the solvent. If the solute is ionic, it is made of cations & anions and is only soluble in polar solvents

23. The Process of Solvation (aka: dissociation for ionic solutes) Packet pg. 6
Step 2 – The water molecules (solvent) orient themselves around the cations and anions of the solute. The H in water is attracted to the anions, while the O in water is attracted to the cations.

24. The Process of Solvation (aka: dissociation for ionic solutes) Packet pg. 6
Step 3 – Each ion is surrounded by water molecules (solvent) until the entire solid is separated (aka: dissociated) into its individual ions. This means the solute is completely dissolved.

25. Types of Solutions Saturated
A solution that contains the maximum amount of dissolved solute

26. Types of Solutions Unsaturated
A solution that contains less than a saturated solution under existing conditions

27. Types of Solutions Supersaturated
Supersaturated
A solution that contains more dissolved solute than a saturated solution contains under the same conditions

28. Solubility Curves – pg. 6
Solubility
The amount of that substance required to form a saturated solution with a specific amount of solvent at a specified temperature

29. Packet pg. 13 Colligative Properties
There are 4 colligative properties!

30. 1) Vapor Pressure Lowering

31. Boiling Point Elevation

32. Freezing Point Depression

33. Osmotic Pressure (π) https://www.youtube.com/watch?v=eQsAzXr0UCU

34. Osmosis
(aka: dilute solution)

35. Osmosis in Blood Cells