Study Guide
Solutions
Practice Problems
- 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. (I usually don't
cover this.)
- 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.
(Related to normality.)
- 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.