Thank you Chris Pham for acquiring this information:
The final is going to be given as a mock AP exam. You will have two parts: Part A, Multiple Choice (50 minutes) and Part B, short answer (50 minutes). (I might be a little lenient on the time.) Part A was a little bit difficult for me because I do not know everything that you have covered up until this point, but there will be 42 questions ranging from stoichiometry to equilibrium. There are a few questions on electrochemistry, but I tried to keep it simple. Part B consists of three short answer questions. One is an acid-base equilibriaproblem, one is a buffer problem, and one is a thermochemistry problem. (the thermochemistry problem requires the use of Gibbs free energy and calculating Keq. This should help, I hope! Let me know if you have any questions. Good luck studying for your other finals!
Saturday, January 24, 2009
Wednesday, January 21, 2009
Lab report format
Wednesday, January 14, 2009
Monday, January 12, 2009
Homework Janurary 12
Homework today is the two example problems in the chapter 17 notes packet under Addition of Strong Acids or Bases to Buffers.
For those who have misplaced said notes here are the problems:
1. Consider a buffer prepared by placing 0.60 moles of HF (Ka = 7.2 x 10-4) and 0.48 moles of NaF in a 1.00 L solution.
a) Calculate the pH of the buffer
b) Calculate the pH after addition of 0.08 moles of HCl
c) Calculate the pH after the addition of a total of 0.16 moles of HCl
d) Calculate the pH after the addition of 0.10 moles of NaOH
2. Consider a buffer containing 0.78 moles of HC2H3O2 (Ka = 1.8 x 10-5) and 0.67 moles of NaC2H3O2 in 1.00 L of solution.
a) Calculate the pH of the buffer
b) Calculate the pH after addition of 0.10 moles of HNO3
c) Calculate the pH after the addition of a total of 0.20 moles of HNO3
d) Calculate the pH after the addition of 0.10 moles of NaOH
For those who have misplaced said notes here are the problems:
1. Consider a buffer prepared by placing 0.60 moles of HF (Ka = 7.2 x 10-4) and 0.48 moles of NaF in a 1.00 L solution.
a) Calculate the pH of the buffer
b) Calculate the pH after addition of 0.08 moles of HCl
c) Calculate the pH after the addition of a total of 0.16 moles of HCl
d) Calculate the pH after the addition of 0.10 moles of NaOH
2. Consider a buffer containing 0.78 moles of HC2H3O2 (Ka = 1.8 x 10-5) and 0.67 moles of NaC2H3O2 in 1.00 L of solution.
a) Calculate the pH of the buffer
b) Calculate the pH after addition of 0.10 moles of HNO3
c) Calculate the pH after the addition of a total of 0.20 moles of HNO3
d) Calculate the pH after the addition of 0.10 moles of NaOH
Saturday, January 10, 2009
Wednesday, January 7, 2009
Textbook Assignment
This is due on Friday.
End of Chapter 17: [14, 16, 18, 20, 22, 24, 30]
Remember the lab is due tomorrow, Thursday!
End of Chapter 17: [14, 16, 18, 20, 22, 24, 30]
Remember the lab is due tomorrow, Thursday!
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