1. CHAPTER 06: CHEMICAL EQUILIBRIUM Harris: Quantitative Chemical Analysis, Eight Edition

2. CaCO 3 (s) ＋ CO 2 (aq) ＋ H 2 O(l) = Ca 2 ＋ (aq) ＋ 2HCO 3 － (aq) HCO3 － (aq) ＋ H ＋ (aq) s --- > CO 2 (g) ＋ H 2 O(l)

3. aA + bB = cC + dD in its standard state HA = H ＋ ＋ A － K 1 ＝ [H ＋ ][A － ] / [HA] 만약 반응의 방향을 바꾸면 새 K 값은 처음 K 값의 역수가 된다. H ＋ ＋ A － = HA K 1 ′ ＝ [HA] / [H ＋ ][A － ] ＝ 1/K 1 HA = H ＋ ＋ A － K 1 H ＋ ＋ C = CH ＋ K 2 ---------------------------------- HA ＋ C = A － ＋ CH ＋ K 3 K 3 ＝ K 1 K 2 ＝ [H ＋ ][A － ] / [HA] ·[CH ＋ ] / [H ＋ ][C] ＝ [A － ] ·[CH ＋ ] / [HA] [C]

6. Le Chˆatelier’s principle: Reaction quotient: Because Q > K, the reaction must go to the left

7. When the temperature changes: The term including e ᅀ S/R is independent of T. The term e - ᅀ H/RT increases with increasing temperature if ᅀ H o is positive, and decreases if it is negative. K of the endothermic reaction increases if T is raised. K of the exothermic reaction decreases if T is raised.

8. 6-3 Solubility product Ion pair

9. Disproportionation: an element in an intermediate oxidation state gives products.

10. Common ion effect A salt will be less soluble if one of its constituent ions is already present in the solution.

11. Separation by Precipitation Co-precipitation: foreign ions adsorbed on the precipitate. Q < Ksp for PbI 2, Pb ions will not precipitate.

12. Lewis Acid and Bases 6-4 Complex Formation

13. Effect of Complex Ion Formation on Solubility

15. 6-5 Protic Acids and Bases - Hydronium ion: H 3 O + Brønsted － Lowry Acids and Bases: Acid: proton donor, Base: proton acceptor Salt: Any ionic solid When [I - ] = 1.0 M, [Pb] total = 3.2 x 10 -4 M

16. Conjugate Acids and Bases

17. - Structure of Hydronium ion

18. The Nature of H + and OH -

23. Autoprotolysis - Protic solvents have a reactive H +

24. 6-6 pH

26. Is There Such a Thing as Pure Water? 6-7 Strength of Acids and Bases Strong Acids and Bases

27. Weak Acids and Bases K a : Acid dissociation constant K b : Base hydrolysis constant

28. Common Classes of Weak Acids and Bases

33. Polyprotic Acids and Bases

37. K al ( 또는 K 1 ) 은 가장 많은 양성자를 가진 산성 화학종에 대한 것이고, K bl 은 가장 적은 양성자를 가진 염기성 화학종에 대한 것이다.

38. Relationship between K a and K b

39. Carbonic Acid

46. 6-8 Solving Equilibrium Problems