• Any parts of the AP Chemistry Lab Review that you did not complete in class should be finished as homework.  The information for each station is included as an attachment. (note that #6 is actually on the last page)
• Also go over the following released laboratory-based AP questions and answers.  We will have a quiz based on those topics on Monday (10-15 points):
    2007 form B #5, 2008 #2, 2008 form B #5, 2010 form B #5, 2011 #2, 2013 #2, 2011 form B #5.

• Complete the attached homework assignment which relates to the practice AP equilibrium problems you did in class.
• Finish the assignment from class on Tuesday 2007 through 2011.
• Today (Thursday) is an early day for extra credit.  Please be here by 7:05 am and bring your three multiple choice practice tests.

1. Six reactions (oxidation of a metal by a metal ion) should have taken place in lab today spontaneously.  The opposites of those six are non-spontaneous and should not have occurred.  Compare your results against the table of reduction potentials, and for each reaction, write a complete balanced net ionic equation and calculate the voltage that would be expected if these were carried out in galvanic cells.  Note that the aluminum-copper one was done in our class notes.  Also make a table of activity series for these four metals with the most active metal (more likely to be oxidized) at the top and the least active at the bottom.
2. Download and complete the attached file using your understanding of electrochemistry from class on Thursday.
   

• task 5 - Using the Ka you found for potassium acetate and your notes from class, carryout the necessary calculations to determine the pH of a buffer solution containing 0.400 M acetic acid and 0.250 M acetate ion.
• task 6 - Carryout the necessary calculations to determine the pH of a 250.0 mL sample of the buffer solution described above after 20.0 mL of 2.50 M NaOH has been titrated into it.  Was the buffer effective?
• task 7 - Carryout the necessary calculations to show that the buffer cannot handle 40.0 mL of the 2.50 M NaOH.  This is similar to a weak acid strong base titration that has gone to the equivalence point.  The pH is determined by the hydrolysis of the acetate ion.  Refer to your notes on weak acid-strong base titration to the equivalence point.

• task 1 - write the equation for the formation of that salt from the reaction of the appropriate acid and base. Identify each acid and base as strong or weak.
• task 2 - write the equation for the dissolving of the salt in water.
• task 3 - research on line and find either the Ka (for the weak acid) or Kb (for the weak base) that made that salt.
• task 3 1/2 - write the salt hydrolysis equation for each of the four salts.
• task 4 - write both equations that would represent the buffer system for that weak acid (or weak base) and its salt anion (or cation).

• Calculate the hydroxide ion concentration using a stoichiometry chart and new total volume.
• Calculate the pOH.
• Use pH + pOH = 14 to solve for the pH.

• Determine the order with respect to each of the reactants.  Show evidence of work in at least one example for each of the three reactants.
• Determine the activation energy for the reaction.  Show sample calculations to get the data for the log (or ln) rate vs. 1/T graph, and show calculations to determine the activation energy.  If you do not have enough data, here is additional data you can use:

• Write a balanced equation for the decomposition of Nitrogen dioxide gas to nitrogen monoxide gas and oxygen gas.

• Calculate the instantaneous rate of reaction for each of the following (for those that were absent, draw a line tangent to the curve at that point in time and determine the slope.  The rate is the slope.  See me before the homework is due if you need assistance)

AP Chemistry – Reaction Kinetics

Analyzing Experimental Rate of Decomposition Data

                                2 NO₂ (g)  →  2 NO (g)  +  O₂ (g)

                            2 N₂O₅ (g)   →  4 NO₂ (g)  +  O₂ (g)

                            C₂H₅OH (g)  →  CH₃CHO (g)   +   H₂ (g)

1. Finish the Advanced Study assignment.
2. Complete the analysis of your group lab data as you did in the ASA.  The atmospheric pressure in the room was 766.1 Torr.  The Experiment handout is included as an attachment here.  The goal is to finish with a graph of natural log of vapor pressure vs. 1/Kelvin temperature.  The relationship is linear with a negative slope.  Calculate the enthalpy of vaporization which is equal to the negative of the slope times R (8.31 J/mole K)

• Write the chemical formula and structural formula for each. 
• Predict the bond angles around each carbon atom for each structure.
• Determine the type of intermolecular force of attraction each exhibits. Justify your answer.
• Write the numerical value of the molar enthalpy of vaporization for each.  Use your understanding of chemical bonding and intermolecular forces of attraction to explain the differences in molar enthalpy of vaporization between the three compounds.
• Based on the enthalpies of vaporization and your understanding of intermolecular forces of attraction, rate the three in order of increasing normal boiling point temperature.  Justify your answer.
• Based on the enthalpies of vaporization and your understanding of intermolecular forces of attraction, rate the three in order of increasing vapor pressure.  Justify your answer.