1. Drill #12 5/13, 14/2014  Write the balanced neutralization equations for the following reactions: 1. carbonic acid & calcium hydroxide 2. potassium hydroxide and carbonic acid 3. barium hydroxide and hydrochloric acid

2. Drill #12 5/13, 14/2014  Write the balanced neutralization equations for the following reactions: 1. H 2 CO 3 +CA(OH) 2 ===> CaCO 3 +2H 2 O 2. 2 KOH + H 2 CO 3 ===> K 2 CO 3 + 2H 2 O 3. Ba(OH) 2 + 2HCl ===> BaCl 2 + 2H 2 O

3. Objectives  SWBAT describe the concept of chemical equilibrium and explain how and when it is achieved.  SWBAT write an equilibrium expression.  SWBAT describe the progress of a chemical reaction by using the equilibrium constant.  SWBAT explain how physical changes such as concentration, pressure, and temperature can affect a chemical reaction at equilibrium.

4. Agenda  Equilibrium notes  Equilibrium lab  Review Worksheets

5. CHEMICAL EQUILIBRIUM

6.  Up to this point we have mostly been considering reactions “to completion”, where all the reactants change into product. reversible  However, most reactions are reversible = occurs in both the forward and the reverse directions.

7.  N 2 (g) + 3H 2 (g)  2NH 3 (g) forward  N 2 (g) + 3H 2 (g)  2NH 3 (g) reverse N 2 (g) + 3H 2 (g) 2NH 3 (g) or N 2 (g) + 3H 2 (g) ↔ 2NH 3 (g)   Combined in one equation using double arrows

8. Chemical Equilibrium  A state in which the forward and reverse reactions balance each other and when the forward reaction proceeds at the same rate as the reverse reaction.  Concentrations of reactants and products are constant at equilibrium. (Constant ≠ equal)

9. Rate vs. Time

10. Equilibrium Lab  Work in pairs  Read directions first then follow directions carefully  Answer questions 1-4 for homework

11. Equilibrium constant  Kequilibrium constant  K is called the equilibrium constant. It is a ratio of the concentrations of products to the concentration of reactants.

12. Equilibrium Constant Expression aA + bB ↔ cC + dD K eq = [C] c [D] d [A] a [B] b A & B = molar [ ] of reactants C & D = molar [ ] of products Exponents a, b, c, and d = coefficients in the balanced equation.

13. Equilibrium Constant K eq > 1  If K eq > 1: products are favored at equilibrium  If K eq < 1  If K eq < 1: reactants are favored at equilibrium

14. Important!  Only substances that are gases and aqueous get factored into the equilibrium expression  Pure liquids and solids do not appear in the expression.

15. Example #1  Write the equilibrium expression for the following reaction: 2 CO (g) + O 2 (g) ↔ 2 CO 2 (g)

16. Answer  K eq = [CO 2 ] 2 / ([CO] 2 [O 2 ])

17. Example #2  Write the equilibrium expression for the following reaction: CO (g) + 3 H 2 (g) ↔ CH 4 (g) + H 2 O (g)

18. Answer  K eq = [CH 4 ][H 2 O] / ([CO][H 2 ] 3 )

19. Assignment  Complete Equilibrium Constant WS – #1-5

20. Drill #13 5/15, 19/2014  What is the pH of a 2.23 x 10 -6 M solution of HI?  What is the pH and pOH of a 2.34 x 10 - 5 M NaOH solution?

21. Drill #13 5/15, 19/2014  What is the pH of a 2.23 x 10 -6 M solution of HI? Ans: pH = 5.65  What is the pH and pOH of a 2.34 x 10 -5 M NaOH solution? Ans: pOH = 4.63, pH = 9.38

22. Agenda  Acids and Bases Test  Le Chatelier Principle Homework  Le Chatelier’s Worksheet (given to you last class)

23. Homework Due:  Bean Lab  Equilibrium Constant WS

24. Important! Changes to Test 7. In the titration of a solution of Sr(OH) 2 with HCl, the mole ratio of base to acid a.) is 1:1 c.) is 2:1 b.) is 1:2 d.) cannot be determined 10. An Arrhenius acid is a(an) a.) a substance that reacts with a salt. b.) substance that donates a H+ ion when combined with a base. c.) substance that releases H+ ions in an aqueous solution. d.) substance that releases OH- ions in a aqueous solution.

25. LE CHÂTELIER’S PRINCIPLE

26. Question  Can we change the equilibrium position thereby increasing the amount of products in a reaction? adding stress  Yes – by adding stress to a system in equilibrium.

27. Le Châtelier’s Principle stress is applied relieves the stress.  If a stress is applied to a system at equilibrium, the system shifts in the direction that relieves the stress.  Stress is anything that upsets equilibrium – changes in concentration, pressure, or temperature.

28. Concentration  Measure of molarity (moles/L)  If you ↑ concentration of a reactant, equilibrium will shift toward the products.  If you ↓ concentration of a reactant, equilibrium will shift toward the reactants.

29. CO(g) + 3H 2 (g) ↔ CH 4 (g) + H 2 O(g) CO(g) H 2 O(g)

30. Changes in Concentration A + B C + D Increasing the concentration of “A” will shift the reaction to the right –we need to get rid of excess “A” Decreasing the concentration of “C” will shift the reaction to the right –there is a deficit, so more “C” needs to be made

31. Temperature Increasing the temperature shifts the reaction away from the side that contains the “heat” Decreasing the temperature shifts the reaction toward the side that contains the “heat”

32. Temperature Think of heat as a reactant or a product. CO(g) + 3H 2 (g) ↔ CH 4 (g) + H 2 O(g) + heat Is this Exothermic or Endothermic?

33. heat CO(g) + 3H 2 (g) ↔ CH 4 (g) + H 2 O(g) + heat

34. Sample Reaction heat + NH 4 Cl (s) NH 3 (g) + HCl (g) endothermicIn the above endothermic reaction, increasing the temperature will drive the reaction to the right (in other words, forward)

35. Pressure PV=nRTIdeal Gas Law: PV=nRT If ↑P then ↑n, which means more number of atoms. If ↑P, then the equilibrium will shift toward the side with fewer moles of gas.

36. CO(g) + 3H 2 (g) ↔ CH 4 (g) + H 2 O(g) 4 moles of gas 2 moles of gas Note: If moles of gaseous reactant = moles of gaseous product, then no shift in equilibrium will occur from a change in pressure

37. Le Châtelier’s Principle If a stress is applied to a system at equilibrium, the system shifts in the direction that relieves the stress. – Concentration – Pressure – Temperature Note: Only temperature affects K. The larger the value of K, the more product at equilibrium.

38. Assignment Le Châtelier’s Principle Worksheet

39. Wrap up K eq > 1  If K eq > 1: are favored at equilibrium  If K eq < 1  If K eq < 1: are favored at equilibrium

40. Drill #14May 19 & 20, 2014  What are the 3 types of stress that can affect the equilibrium of a system?  Which states of matter get factored into an equilibrium expression?

41. Agenda  Go over Equilibrium Worksheet  Notes on Equilibrium Problems  Complete the following worksheets:  16-3 Review and Reinforcement  2 – Equilibrium Worksheets handed out to you by sub

42. Announcement!!  Wear closed-toed shoes next class. We will be in the lab!

43. DIFFERENT TYPES OF EQUILIBRIUM

44. Concentration Equilibrium K c (or K eq )  nA + mB ↔ xC + yD  K c = [C] x [D] y [A] n [B] m

45.  Remember…equilibrium is where the rates of forward and reverse reactions are the same. It means that the concentrations do not change, NOT that they are identical.

46.  Because equilibrium expressions have to do with concentration (in molarity) we do not include items that are not in solution so NO LIQUID or SOLID states! They are in excess so can be ignored.

47. Acid Equilibrium  Acid + H 2 O ↔ H 3 O + + Acid Ion or HA + H 2 O ↔ H 3 O + + A - K a = [H 3 O + ][A - ] [HA][H 2 O] [HA] Because water is a solvent and its conc. greatly exceeds the acid, we can assume that the conc. of water does not change.

48. Base Equilibrium  Base + H 2 O ↔ OH - + Base Ion or B + H 2 O ↔ OH - + HB + K b = [OH - ][HB + ] [B][H 2 O] [B]

49. PropertyStrong AcidWeak Acid K a valueK a is largeK a is small Position of equilibrium Far to the right (a lot of dissociation) Far to the left (little dissociation) [H+] compared to original [HA] [H+]≈[HA] o [H+]<<[HA] o Strength of conjugate base A- is much weaker A- is much stronger

50. Graphic Representation of the Behavior of Acids of Different Strengths in Aqueous Solution

51. Solubility Equilibrium  Salt (s) ↔ Cation (aq) + Anion (aq)  Solids are not included in equilibrium equations! So… K sp = [Cation][Anion]

52. Solubility Equilibrium Example  CaF 2 (s) ↔ Ca +2 (aq) + 2F - (aq)  Solids are not included in equilibrium equations! So…  K sp = [Ca +2 ][F - ] 2

53.  Write the equilibrium expression for the reaction: H 2 (g) + I 2 (s)  2HI (g) K eq = [HI] 2 [H 2 ]

54.  How would the following shift the equilibrium in the equation (forward, reverse or no change): H + (aq) + Cl - (aq) ↔ HCl (aq) + 10.3 kJ a) Increasing temperature b) Decreasing pressure c) Adding NaCl d) Adding NaOH