1. Unit 13: Solutions & Chemical Equilibrium
Section 1: Properties of Solutions
Solution Formation
Rate of Dissolving
Solubility

2. Can it be physically separated?
Matter Flowchart
MATTER
yes no
Can it be physically separated?
MIXTURE
PURE SUBSTANCE
Is the composition uniform? no
yes
Can it be chemically decomposed? no
yes
Homogeneous Mixture
(solution)
Heterogeneous Mixture
Compound
Element
Colloids
Suspensions

3. A. Solution Formation Solution - homogeneous mixture
Solute - substance being dissolved
Solvent –
dissolving medium (dissolver)

4. A. Solution Formation Types of Solutions: Solute Solvent Example Gas
Air (O2 & CO2 in Nitrogen)
Liquid
Water in Air
Soda
Vinegar (acetic acid in water)
Solid
Salt in water
Stainless Steel (Cr & Ni in Iron)

5. A. Solution Formation
Solvation The process of surrounding solute particles with solvent particles to form a solution Ionic compounds and polar covalent compounds undergo solvation in water (dissolve)

6. A. Solution Formation
Water molecules surround the positive and negative ions, pulling them out of the crystal.

7. A. Solution Formation Solvation Process of Sucrose, C12H22O11
Water molecules H-bond with the O-H groups in sucrose, breaking the IMAF’s, and pulling the sucrose molecules apart

8. B. Rate of Dissolving
Solids dissolve better...
more stirring

9. B. Rate of Dissolving Solids dissolve better... more stirring
more surface area
(small particle size)

10. B. Rate of Dissolving Solids dissolve better... stirring
more surface area
(small particle size)
high temp.

11. B. Rate of Dissolving Gases dissolve better... no stirring
high pressure
low temp.

12. Solubility in 100 g of Water at 20oC
C. Solubility
Solubility
maximum grams of solute that will dissolve in an
amount of solvent
at a given temp.
varies with temp.
Solubility in 100 g of Water at 20oC
Compound
Solubility (g)
Table Salt
(NaCl)
36.0
Baking Soda (NaHCO3)
9.6
Table Sugar
(C12H22O11)
203.9

13. C. Solubility Solubility Curve
1. What is the solubility of KCl at 70C?
50 g/100 g H2O
2. If you have 35 g of NaCl dissolved in 100 g of water at 70C, how many more grams can be dissolved?
5 g

14. Solubility Graph WS

15. less solute than max dissolved more than max solute dissolved
C. Solubility
UNSATURATED
less solute than max dissolved
SATURATED
max solute dissolved
SUPERSATURATED
more than max solute dissolved
concentration

16. less solute than max dissolved more than max solute dissolved
C. Solubility
UNSATURATED
less solute than max dissolved
SATURATED
max solute dissolved
SUPERSATURATED
more than max solute dissolved
Add a seed crystal
concentration

17. less solute than max dissolved more than max solute dissolved
C. Solubility
UNSATURATED
less solute than max dissolved
SATURATED
max solute dissolved
SUPERSATURATED
more than max solute dissolved
concentration

18. less solute than max dissolved more than max solute dissolved
C. Solubility
UNSATURATED
less solute than max dissolved
SATURATED
max solute dissolved
SUPERSATURATED
more than max solute dissolved
Extra solute crystallizes
concentration

19. D. 3 Factors Affecting Solubility
Temp.
Pressure
high T:
solids more soluble
low T:
gases more soluble
high P:
gases more soluble

20. D. 3 Factors Affecting Solubility
Solvent Polarity:
“Like Dissolves Like” H H H C C C H C C C
C6H14 H H H
H2O
CCl4

21. D. 3 Factors Affecting Solubility
Polar –Polar
Polar –Nonpolar

22. Quick Quiz.
1) For a given substance, which of the following will NOT influence
how fast it dissolves?
A) temperature
B) amount of agitation
C) molar mass
D) size of the crystals

23. Quick Quiz. 3) The solubility of a gas in a solvent is affected by?
A) both temperature and pressure.
B) only pressure
C) only temperature
D) your face

24. Quick Quiz. 4) Polar water molecules will NOT dissolve…
A) polar alcohol molecules
B) most ionic compounds
C) nonpolar fat molecules
D) partially ionized acetic acid molecules