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

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? Email 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.

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]

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) 0 b) 1 c) 2 d) 3 e) 4

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

Selective Precipitation

(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

Clicker Question Determine the pH of an aqueous solution that is initially 1.00M HC2H3O2 (Ka = 1.8 x 10–5) and 0.0100M HCl. a) 1.85 b) 1.94 c) 2.00 d) 2.07 e) 2.37

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