http://www.ck12.org Chapter 16. Solutions
16.1 Solubility
Lesson Objectives
- Define the term solubility and describe factors affecting the solubility of a particular solution.
- Predict whether a substance will dissolve or dissociate in water. Describe what it means for a solution to be
saturated, supersaturated, or unsaturated. - Define and give examples of both miscible and immiscible mixtures.
- Explain the statement "like dissolves like" at the molecular level, and give specific examples of this concept.
- Describe how pressure and temperature affect the solubility of a liquid or solid in solution.
- Describe how pressure and temperature affect the solubility of gases in solutions, and use Henry’s Law to
predict the solubility of a gas in a solution given the necessary variables.
Lesson Vocabulary
- solubility: The degree to which a solute dissolves in a solvent.
- saturated: The point at which no more solute is able to dissolve.
- unsaturated: A solution in which more solute could be dissolved, solute concentration is less than predicted
by solubility properties. - supersaturated: When the amount of solute dissolved exceeds the solubility. Occurs when a solution is
saturated and the temperature slowly drops. - miscible: Molecules mix well with one another, and form a homogeneous mixture.
- immiscible: Molecules don’t mix well together, and form a heterogeneous mixture exhibiting a noticeable
bilayer. - van’t Hoff factor: Describes the number of moles of particles that dissociate from solid.
- Henry’s law: Mathematically describes the relationship between the vapor pressure of the solution and the
solute concentration.
Check Your Understanding
- What type of intermolecular forces will exist between molecules of the following substances?
a. H 2 O
b. CO 2
c. CH 4
d. N 2
e. CO
f. NH 3