1. Lecture 112/9/07

2. 1. Mix 0.2 L of 0.3 M Ca(NO 3 ) 2 and 0.2 L of 0.06 M NaF. Does a precipitate form? K sp (CaF 2 ) = 3.9 x 10 -11 2. Write the balanced equation for formation and the equilibrium expression for the complex: [Cd(NH 3 ) 4 ] 2+ Quiz 4

3. Bronsted-Lowry Acids Proton donor (H + or H 3 O + ) Acidic vs. non-acidic protons Bronsted-Lowry Bases Proton acceptor

4. Acids Strong HCl HBr HI HClO 3 HClO 4 HNO 3 H 2 SO 4 Weak All other acids R-COOH HCl → H + + Cl - Concentration of H + if you add 0.5 M HCl? HF ⇄ H + + F - Concentration of H + if you add 0.5 M HF?

5. Bases Strong LiOH NaOH KOH RbOH CsOH Ba(OH) 2 Sr(OH) 2 O 2- H - N 3- Weak Conjugate bases NH 3 R-NH 2

6. Oxide (O 2- : CaO, Na 2 O) O 2- (aq) + H 2 O → 2 OH - (aq) Hydride (H - : NaH) H - (aq) + H 2 O → H 2 (aq) + OH - (aq) Nitride (N 3- : Na 3 N) N 3- (aq) + 3H 2 O → NH 3 (aq) + 3OH - (aq)

7. Amphoteric (Amphiprotic)

8. pH What is it? How do you measure it?

9. pH of some common substances pH Bleach12.5 Baking soda8.4 Egg White7.7 Milk6.8 Unpolluted rain5.6 Coffee4.9 Soda2.9 Stomach acid1.2

10. Autoionization of Water What is it? What is the definition of: Neutral solutions? Acidic solutions? Basic solutions?

11. T (°C)KwKw 100.29 x 10 -14 150.45 x 10 -14 200.68 x 10 -14 251.01 x 10 -14 301.47 x 10 -14 505.48 x 10 -14

12. pH vs. pOH

13. Degree of ionization