Schedule for Second Summer Session
| Date |
Day |
Topics |
| 7/13 | Mon | Discussed class syllabus. |
| 7/14 | Tue | Chapter 16 sections 10 and 11. Heating curves. |
| 7/15 | Wed | Equilibrium is a dynamic process. Can be described
2 ways: (1) Kinetically. The rates of the 2 opposing processes (forward rxn and reverse rxn)
are equal at equilibrium. (2> Thermodynamically. ΔG = 0. Free energy of the system
is at a minimum. Vapor pressure is a manifestation of an equilibrium process between evaporation
and condensation. Discussed the Claussius-Clapeyron Equation which compares 2 vapor pressures at
2 different temperatures. Also discussed phase diagrams and how to interpret them.
|
| 7/16 | Thu | Chapter 17 - dissolution of solids into solution.
Thermodynamics of dissolution. How the crystal lattice energy and the enthalpy of
hydration combine to give the enthalpy of solution. Introduced Colligative properties. |
| 7/17 | Fri | Went over more on solubility. Likes dissolve likes. Solubility of
gases in water. Temperature dependence of solubility. Henry's Law.
Colligative properties. van Hoff factor - we will only consider complete ionization of salts.
Quick Exam overview - its 20 questions. |
| 7/20 | Mon | EXAM 1 |
| 7/21 | Tue | Chapter 6 - chemical equilibrium. The mass action expression. |
| 7/22 | Wed | Closer look at Q vs K relationships. Le Chatlier's Principle -
system at equil will respond to stress so as to relieve the stress. "Stress" is moving Q away
from K by changing conc or press. You can move K away from Q by changing the T. Showed how to
set up ICE Tables for solving equilibrium questions. Showed that you can write equilibrium
constants with concentration terms (Kc) or with pressures (Kp).
|
| 7/23 | Thu | The relationship of Kp and Kc. Temperature dependence of K.
Finish chapter 6 and intro Chapter 7 - Acid/Base equilibria. |
| 7/24 | Fri | Chapter 7 solving pH problems (Type 1) |
| 7/27 | Mon | Chapter 7 - finish - Exam 2 recap of material |
| 7/28 | Tue | EXAM 2 |
| 7/29 | Wed | Chapter 8. Defined what a buffer is. These are Type 2 problems in
my way of thinking (and on my helpsheets). Also defined fraction of species and how the pH of
a solution affects the RATIO of the conjugates. Showed the solution to the ICE tables for a
buffer problem (type2). Took -log and got the Henderson-Hasselbalch equation for buffers. |
| 7/30 | Thu | Showed how to calculate points on a pH curve or a titration curve.
How do you know when to stop a titration? When the indicator changes color (aka: the end point).
Indicators are just special weak acids (or bases) themselves that happen to have different colors
for the two conjugates. All indicators transition from one visual color to the other through about
2 pH units which are centered on the pKa value. PICK an indicator that changes color at the pH
where you want to stop (this should be the equivalence point). |
| 7/31 | Fri | Finished up titrations and indicators. Introduced Solubility
equilibria. Now we use Ksp for our equil constant. You can calculate the molar solubility (x)
from Ksp. The formula varies with the type of ratio salt you have. 1:1, 1:2, 1:3, 2:3 salts each
have their own "formula" to solve to get x. Solubilities come in many different units - we need
MOLAR solubility to go into the solubility product equation. "ppm" is parts-per-million which
you need to switch to mg/L for aqueous solutions - then switch to mol/L for the solving for Ksp
part. |
| 8/3 | Mon | More Chapter 8 on solubility equilibria. Showed that you can
still calculate Q and compare to K, then predict the direction of the shift in equilibria. Remember
that a LEFT shift in this section corresponds to a precipitation reaction. Showed the concept and
the way a fractional precipitation works (called selective precipitation in your book). Showed how
to predict the order of precipitation. Showed how you can dissolve hydroxide salts by adding acid.
Introduced complex ions.
|
| 8/4 | Tue | Finishing Chapter 8 - more details on complex ion formation and
dissociation. Plus some more dissolving precipitates. Will discuss exam also.
|
| 8/5 | Wed | EXAM 3 |
| 8/6 | Thu | Chapter 11. "Reviewed" redox reactions. Defined reduction and
oxidation. LEO says GER. 1/2 rxns are written and tabulated as reductions - the TABLE you get is
called a Standard Potential table. The potentials are given in volts and volts is really just a
measure of the tendency of a reaction to want to go forward. Big + potentials want to really go
forward (large -ΔG value). Negative potentials (-E) are NON-spontaneous as written.
The overall potential for a redox reaction is just the reduction potential plus the oxidation
potential. So this is just the difference between two numbers off the standard potential table.
Which one do you substract from which? Leave the reduction alone (straight off the table), "flip"
the reaction that is to be the oxidation. That "flip" puts the electrons on the RIGHT side of
the equation (which will cancel out with the ones on the left in the other rxn) AND changes the
sign of the potential. That new "flipped" potential is an oxidation potential.
|
| 8/7 | Fri | More on cell notation. Non-standard conditions - the Nernst
Equation. Electrolysis calculations using the faraday constant: I(t)/n(F) = mol of stuff. |
| 8/10 | Mon | Recap of electrochem up to now. Showed my "cartoony"
looking Electrochemistry help sheet. Talked about batteries, types, examples. Told you to know the
reactions for a lead-storage battery. Introduced chemical reaction rates, how we write a
reaction rate and what the units are. |
| 8/11 | Tue | How to write the rate law. How to use the Method of Initial Rates
to find the rate law. This is basically solving a table full of concentration and rate data. Then
did an integration of a rate law and got the integrated rate law equations for 1st, 2nd, and
zero order reactions. Defined 1/2 life and how to calculate it. |
| 8/12 | Wed | Temp dependence of rate. Reaction mechanisms. |
| 8/13 | Thu | EXAM 4 |
| 8/14 | Fri | COOL Chemistry DEMOS!! Come one - come all.
Course Overview - Final Exam discussion |