1. Chapter 15 Acids and Bases

2. Some Properties of Acids þ Produce H + (_______) ions in water (the ________ ion is a hydrogen ion attached to a water molecule) þ Taste ______ þ ______metals þ _____________ þ React with bases to form a ____ and ____ þ pH is less than______ þ Turns ______ litmus paper to ___ “___________”

3. Some Properties of Bases  Produce _____ ions in water  Taste ______, ______  Are ________  Feel _______, _______  React with acids to form _____and _____  pH greater than ____  Turns ____ litmus paper to _____ “_________”

4. Acid Nomenclature Review No Oxygen  w/Oxygen An easy way to remember which goes with which… “In the cafeteria, you ATE something ICky”

5. ___________ is a substance that produces ______in water __________ is a substance that produces _____in water 4.3 Acid/Base definitions Definition 1: _________

6. Acid/Base Definitions Definition #2: __________Definition #2: __________ Acids – ________ donor Bases – _______ acceptor A “proton” is really just a ______ atom that has lost it’s electron!

7. A Brønsted-Lowry ______ is a _____ donor A Brønsted-Lowry _______ is a _____acceptor bas

8. ACID-BASE THEORIES The Brønsted definition means _____ is a BASE in water — and _________an ACID

9. Conjugate Pairs

10. Learning Check! Label the acid, base, conjugate acid, and conjugate base in each reaction: HCl + OH -  Cl - + H 2 O H 2 O + H 2 SO 4  HSO 4 - + H 3 O +

11. Acids & Base Definitions Lewis acid - a substance that ______an_____________ Lewis base - a substance that _______an___________. Definition #3 – ______

12. Formation of ___________is also an excellent example. Lewis Acids & Bases _____________of the new O-H bond originates on the Lewis_________._____________of the new O-H bond originates on the Lewis_________.

13. Lewis Acid/Base Reaction

14. The pH scale is a way of expressing the strength of acids and bases. Under 7 = _______ 7 = _______ Over 7 = _______

15. Calculating the pH Equation: ____________ (Remember that the [ ] mean________) Example: If [H + ] = 1 X 10 -10 pH = - log 1 X 10 -10 pH = - (- 10) pH = 10 Example: If [H + ] = 1.8 X 10 -5 pH = - log 1.8 X 10 -5 pH = - (- 4.74) pH = 4.74

16. Try These! Find the pH of these: 1)A 0.15 M solution of Hydrochloric acid 2) A 3.00 X 10 -7 M solution of Nitric acid

17. pH calculations – Solving for H+ If the pH of Coke is 3.12, [H + ] = ???

18. More About Water H 2 O can function as both an _____and a______. In pure water there can be________________ Equilibrium constant for water = K w K w = [H 3 O + ] [OH - ] = _________at 25 o C

19. More About Water K w = [H 3 O + ] [OH - ] = _________at 25 o C In a neutral solution [_____________ and so_______________________ Autoionization

20. pOH Since acids and bases are opposites, ______and _______are opposites!Since acids and bases are opposites, ______and _______are opposites! _______looks at the perspective of a base_______looks at the perspective of a base________ Since ____and _______are on opposite ends, Since ____and _______are on opposite ends,_____________

21. pH [H + ] [OH - ] pOH

22. [H 3 O + ], [OH - ] and pH What is the pH of the 0.0010 M NaOH solution?

23. What is the pH of a 2 x 10 -3 M HNO 3 solution? Start End What is the pH of a 1.8 x 10 -2 M Ba(OH) 2 solution? Start End 0 15.4

24. HNO 3, HCl, HBr, HI, H 2 SO 4 and HClO 4 are the __________acids. Strong and Weak Acids/Bases The strength of an acid (or base) is determined by the amount of_________________.

25. Generally divide acids and bases into STRONG or WEAK ones.Generally divide acids and bases into STRONG or WEAK ones. STRONG ACID: HNO 3 (aq) + H 2 O (l)  H 3 O + (aq) + NO 3 - (aq) HNO 3 is about 100% dissociated in water. Strong and Weak Acids/Bases

26. _________are much less than ________ionized in water._________are much less than ________ionized in water. Strong and Weak Acids/Bases

27. ________: _______dissociated in water.________: _______dissociated in water. NaOH (aq)  Na + (aq) + OH - (aq) NaOH (aq)  Na + (aq) + OH - (aq) Other common strong bases include KOH and Ca(OH) 2. CaO (lime) + H 2 O --> Ca(OH) 2 (slaked lime) Ca(OH) 2 (slaked lime) CaO Strong and Weak Acids/Bases Strong bases are the __________ ____________________are strong, but only soluble in water to 0.01 M

28. Weak ________: less than _______ionized in waterWeak ________: less than _______ionized in water One of the best known_____________. NH 3 (aq) + H 2 O (l) ↔ NH 4 + (aq) + OH - (aq) Strong and Weak Acids/Bases

29. Weak Bases

30. Equilibria Involving Weak Acids and Bases

31. Ionization Constants for Acids/Bases Acids ConjugateBases Increase strength

32. Equilibrium Constants for Weak Acids

33. Equilibria Involving A Weak Acid You have 1.00 M HOAc. Calc. the equilibrium concs. of HOAc, H 3 O +, OAc -, and the pH.

34. Equilibria Involving A Weak Acid

35. You have 1.00 M HOAc. Calc. the equilibrium concs. of HOAc, H 3 O +, OAc -, and the pH.

36. Equilibria Involving A Weak Acid

37. Calculate the pH of a 0.0010 M solution of formic acid, HCO 2 H. HCO 2 H + H 2 O ↔ HCO 2 - + H 3 O + HCO 2 H + H 2 O ↔ HCO 2 - + H 3 O + K a = 1.8 x 10 -4

38. Equilibrium Constants for Weak Bases

39. Relation of K a, K b, [H 3 O + ] and pH

40. Equilibria Involving A Weak Base You have 0.010 M NH 3. Calc. the pH. NH 3 + H 2 O ↔ NH 4 + + OH - NH 3 + H 2 O ↔ NH 4 + + OH - K b = 1.8 x 10 -5

41. Equilibria Involving A Weak Base You have 0.010 M NH 3. Calc. the pH. NH 3 + H 2 O  NH 4 + + OH - NH 3 + H 2 O  NH 4 + + OH - K b = 1.8 x 10 -5

42. Equilibria Involving A Weak Base You have 0.010 M NH 3. Calc. the pH. NH 3 + H 2 O  NH 4 + + OH - NH 3 + H 2 O  NH 4 + + OH - K b = 1.8 x 10 -5

43. Types of Acid/Base Reactions: Summary

44. F - (aq) + H 2 O (l) OH - (aq) + HF (aq) Weak Bases are _________ electrolytes NO 2 - (aq) + H 2 O (l) OH - (aq) + HNO 2 (aq) Conjugate acid-base pairs: The conjugate base of a strong acid has no measurable strength. strongest acid _______ the strongest acid that can exist in aqueous solution. strongest baseThe ______is the strongest base that can exist in aqueous solution. 15.4

46. Strong AcidWeak Acid 15.4

47. percent ionization = x 100% For a monoprotic acid HA Percent ionization = [H + ] [HA] 0 x 100% [HA] 0 = initial concentration 15.5

48. 15.7 Ionization Constants of Conjugate Acid-Base Pairs KaKa KbKb KwKw

49. Molecular Structure and Acid Strength H X H + + X - 15.9

50. Molecular Structure and Acid Strength Z O HZ O-O- + H + -- ++ 15.9

51. Molecular Structure and Acid Strength ________ having different central atoms (Z) that are from the same group and that have the same oxidation number. Acid strength increases with increasing electronegativity of Z H O Cl O O H O Br O O Cl is more _____________than Br HClO 3 > HBrO 3 15.9

52. Molecular Structure and Acid Strength 2. ___________having the same central atom (Z) but different numbers of attached groups. Acid strength __________as the oxidation number of Z increases. HClO 4 > HClO 3 > HClO 2 > HClO 15.9

53. Acid-Base Properties of Salts Neutral Solutions: Salts containing an alkali metal or alkaline earth metal ion (except Be 2+ ) and the conjugate base of a strong acid (e.g. Cl -, Br -, and NO 3 - ). NaCl (s) Na + (aq) + Cl - (aq) H2OH2O Basic Solutions: Salts derived from a strong base and a weak acid. NaCH 3 COO (s) Na + (aq) + CH 3 COO - (aq) H2OH2O CH 3 COO - (aq) + H 2 O (l) CH 3 COOH (aq) + OH - (aq) 15.10

54. Acid-Base Properties of Salts Acid Solutions: Salts derived from a strong acid and a weak base. NH 4 Cl (s) NH 4 + (aq) + Cl - (aq) H2OH2O NH 4 + (aq) NH 3 (aq) + H + (aq) Salts with small, highly charged metal cations (e.g. Al 3+, Cr 3+, and Be 2+ ) and the conjugate base of a strong acid. Al(H 2 O) 6 (aq) Al(OH)(H 2 O) 5 (aq) + H + (aq) 3+2+ 15.10

55. Acid-Base Properties of Salts Solutions in which both the cation and the anion hydrolyze: K b for the anion > K a for the cation, solution will be basic K b for the anion < K a for the cation, solution will be acidic K b for the anion  K a for the cation, solution will be neutral 15.10