Chapter 14
Solutions
- General Properties of Solutions
- Homogeneous mixture, transparent, uniformly distributed on a
molecular level, solvent and solute can be separated by
physical methods.
- Solubility
- Amount of solute (grams) that can be dissolved in 100 grams
of the solvent at a certain temperature. Take a look at the
tables and figures in the book.
- Types of solutions (think of examples of each)
- solid in liquid, solid in solid, gas in liquid, gas in solid,
liquid in liquid...
- Concentration
- The amount of solute dissolved, per amount of solvent or
per amount of total solution.
- Dilute vs concentrated solutions.
- Saturated, unsaturated, and supersaturated solutions.
- Standard solutions.
- Factors that affect solubility
- Polarity (like dissolves like)
- Temperature
- Pressure (gases only)
- Dissolving rate (kinetics)
- Particle size
- Temperature
- Concentration
- Agitation
- Equilibrium
- Rate of dissolving equals rate of precipitation.
- This is the normal state for saturated solutions, when
a portion of the solute is present as a solid.
- Concentration Units - Know how to do calculations for these
units, based on the amounts of solute, solvent, or solution.
- Percent by Mass
- Molarity
- Molality
- Dilution problems
- Know how to calculate the molarity of a solution that has been diluted with water, given the original concentration of the undiluted solution. Note, you can use M1V1 = M22V2 here, but make sure you realize that the concentration of the resultant solution is "moles of solute" per "liter of solution" (where the "moles of solute" is determined by the volume and molarity of the original solution, and the "liters of solution" is the total liters as mixed). Think about it.
- Know how to calculate the resulting concentration after two solutions of differing concentrations are mixed. See above for the concept. The difference here is that "moles of solute" is a sum, rather than just one number.
- Normality
- Number of equivalents of solute per liter of solution.
- Equivalent mass
- The mass of a substance that will react with, combine with, contain, replace, or otherwise be equivalent to one more of hydrogen atoms or hydrogen ions.
- Stoichiometry
- Be ready for stoichiometry problems involving solutions. Remember that all stoichiometry problems (including limiting reactant problems) focus around a balanced equation, which allows us to convert from moles of something to moles of something else. The unit of molariy allows us to convert from liters of solution to moles of solute.
Return to the
CHEM 151 Syllabus.
Return to the Schedule.
Go back to the study guide for
Chapter 12 or
Chapter 15.
Return to the
Chem 151 main home page.
This page hosted on the Internet by
GeoCities.
