CHEMISTRY
Solutions Objectives
Chapter 13: Pages 394 – 423
Vocabulary:
colloid
electrolyte
heat of solution
Henry’s law
hydration
immiscible
molality
molarity
miscible
nonelectrolyte
saturated solution
soluble
solute
solution
solution equilibrium
solvated
solvent
supersaturated solution
suspension
unsaturated solution
Objectives:
After studying this chapter, students should be able to:
 13.1.1 distinguish between heterogeneous and homogeneous mixtures
 13.1.2 list three different solute-solvent combinations
 13.1.3 compare the properties of suspensions, colloids, and solutions
 13.1.4 distinguish between electrolytes and nonelectrolytes
 13.2.1 list and explain three factors that affect the rate at which a solid solute dissolves in a liquid
solvent
 13.2.2 explain solution equilibrium and distinguish among saturated, unsaturated, and
supersaturated solutions
 13.2.3 explain the meaning of “like dissolves like” in terms of polar and nonpolar substances
 13.2.4 list the three interactions that contribute to the heat of solution, and explain what causes
dissolution to be exothermic or endothermic
 13.2.5 compare the effects of temperature and pressure on solubility
 13.3.1 given the mass of solute and volume of solvent, calculate the concentration of a solution
 13.3.2 given the concentration of a solution, determine the amount of solute in a given amount of
solution
 13.3.3 given the concentration of a solution, determine the amount of solution that contains a given
amount of solute
Chapter 14: Pages 394 – 423
Vocabulary:
boiling point elevation
colligative properties
dissociation
freezing-point depression
hydronium ion
ionization
molal boiling-point constant
molal freezing-point constant
net ionic equation
Objectives:
After studying this chapter, students should be able to:
nonvolatile substance
osmosis
osmotic pressure
precipitate
semipermeable membrane
spectator ions
strong electrolyte
weak electrolyte
 14.1.1 write equations for the dissolution of soluble ionic compounds in water
 14.1.2 predict whether a precipitate will form when solutions of soluble ionic compounds are
combined, and write net ionic equations for precipitation reactions
 14.1.3 compare dissociation of ionic compounds with ionization of molecular compounds
 14.1.4 draw the structure of the hydronium ion, and explain why it is used to represent they
hydrogen ion in solution
 14.1.5 distinguish between strong electrolytes and weak electrolytes
 14.2.1 list four colligative properties, and explain why they are classified as colligative properties
 14.2.2 calculate freezing-point depression, boiling-point elevation, and solution molality of
nonelectrolytic solutions
 14.2.3 calculate the expected changes in freezing point and boiling point of an electrolytic solution
 14.2.4 discuss causes of the differences between expected and experimentally observed colligative
properties of electrolytic solutions
Schedule (subject to change):
Day 1: 13 – 1
Day 2: 13 – 2
Day 3: 13 – 3
Day 4: lab
Day 5: lab
Day 6: 14 – 1
Day 7: 14 – 2
Day 8: lab
Day 9: review
Day 10: test