1. Slide 1 of 52  Ch.16. Acids and Bases (the fundamentals)

2. Slide 2 of 52 Contents 16-1The Arrhenius Theory: A Brief Review 16-2Brønsted-Lowry Theory of Acids and Bases 16-3The Self-Ionization of Water and the pH Scale 16-4Strong Acids and Strong Bases 16-5Weak Acids and Weak Bases 16-6Polyprotic Acids 16-7Ions as Acids and Bases 16-8Molecular Structure Acid-Base Behavior

3. Slide 3 of 52 16-1 The Arrhenius Theory: A Brief Review HCl(g) → H + (aq) + Cl - (aq) NaOH(s) → Na + (aq) + OH - (aq) H2OH2O H2OH2O Na + (aq) + OH - (aq) + H + (aq) + Cl - (aq) → H 2 O(l) + Na + (aq) + Cl - (aq) H + (aq) + OH - (aq) → H 2 O(l) Arrhenius theory did not handle non OH - bases such as ammonia very well.

4. Slide 4 of 52 16-2 Brønsted-Lowry Theory of Acids and Bases  An acid is a proton donor.  A base is a proton acceptor. NH 3 + H 2 O NH 4 + + OH - NH 4 + + OH - NH 3 + H 2 O baseacid baseacid conjugate acid conjugate base ??

5. Slide 5 of 52 The Solvated Proton

6. Slide 6 of 52 Base Ionization Constant NH 3 + H 2 O NH 4 + + OH - Kc=Kc= [NH 3 ][H 2 O] [NH 4 + ][OH - ] K b = K c [H 2 O] = [NH 3 ] [NH 4 + ][OH - ] = 1.8  10 -5 baseacid conjugate acid conjugate base

7. Slide 7 of 52 Acid Ionization Constant CH 3 CO 2 H + H 2 O CH 3 CO 2 - + H 3 O + Kc=Kc= [CH 3 CO 2 H][H 2 O] [CH 3 CO 2 - ][H 3 O + ] K a = K c [H 2 O] = = 1.8  10 -5 [CH 3 CO 2 H] [CH 3 CO 2 - ][H 3 O + ] baseacid conjugate acid conjugate base

8. Slide 8 of 52

9. Slide 9 of 52 A Weak Base

10. Slide 10 of 52 A Weak Acid

11. Slide 11 of 52 A Strong Acid

12. Slide 12 of 52  Worked Examples Follow:

13. Slide 13 of 52

14. Slide 14 of 52

15. Slide 15 of 52  CRS Questions Follow:

16. Slide 16 of 52 -- ++ In the reaction depicted below, which species are acids?

17. Slide 17 of 52 -- ++ In the reaction depicted below, which species are acids?