1. Schedule Today (3/11): Finish Chapter 8
Should have read all of Chapter 8
Wednesday (3/13): Review for Exam 2
Thursday (3/14): Exam 2
New OWL opens at 9 pm!
Friday (3/15): Go over Exam 2
Monday (3/25): Begin Chapter 17
Read at least through Section 17.3

2. Exam II Thursday, March 14, 7:00-9:00 pm; rooms are on the website.
Conflict: (3/14) 4:30-6:30pm in 329 Davenport; sign up in 1026 CA
Conflict with conflict? me right away.
Review sessions:
Monday (3/11): 1024 Chem Annex (8-10 pm)
Tuesday (3/12): 140 Burrill (4-6 pm)
Practice Exam is posted.

3. Solubility Question
You found that the solubility of Ag2CrO4(s) in pure water is equal to 1.3 x 10–4M (Ksp = 9.0 x 10–12). Compare this solubility to the solubility of Ag2CrO4(s) in: I. 0.10M AgNO3(aq) II. 0.10M NaNO3(aq) III. 0.10M NaCl(aq) [for AgCl, Ksp = 1.6 x 10–10]

4. Clicker Question a) 0 b) 1 c) 2 d) 3 e) 4
How many of the following ionic compounds are more soluble in a strong acid solution than in water?
I. PbF2
II. PbCl2
III. PbBr2
IV. PbI2
a) b) c) d) e) 4

5. Complex Ion Question
How does the solubility of AgCl(s) in 15.0M NH3(aq) compare to its solubility in pure water?

6. Selective Precipitation

7. (Ka for HCN = 6.2 x 10–10, Ka for HF = 7.2 x 10–4)
Clicker Question
Calculate the pH of an aqueous solution of 0.20M HCN and 0.10M HF at 25°C.
(Ka for HCN = 6.2 x 10–10, Ka for HF = 7.2 x 10–4)
a) 1.57
b) 2.07
c) 2.09
d) 3.52
e) 4.95

8. Clicker Question
Determine the pH of an aqueous solution that is initially 1.00M HC2H3O2 (Ka = 1.8 x 10–5) and M HCl. a) 1.85 b) 1.94 c) 2.00 d) 2.07 e) 2.37

9. Problem Solving: Acids-Bases
What are the major species?
What are the reactions in solution?
Which reaction dominates?