1. LecturePLUS Timberlake1 Acids and Bases

2. LecturePLUS Timberlake2 Arrhenius Acids and Bases Acids produce H + in aqueous solutions water HCl H + (aq) + Cl - (aq) Bases produce OH - in aqueous solutions water NaOH Na + (aq) + OH - (aq)

3. LecturePLUS Timberlake3 Acids þ Produce H + (as H 3 O + ) ions in water þ Produce a negative ion (-) too þ Taste sour þ Corrode metals þ React with bases to form salts and water

4. LecturePLUS Timberlake4 Bases Produce OH - ions in water Taste bitter, chalky Are electrolytes Feel soapy, slippery React with acids to form salts and water

5. LecturePLUS Timberlake5 Learning Check AB1 Describe the solution in each of the following as: 1) acid 2) base or 3)neutral. A. ___soda B. ___soap C. ___coffee D. ___ wine E. ___ water F. ___ grapefruit

6. LecturePLUS Timberlake6 Solution AB1 Describe each solution as: 1) acid 2) base or 3) neutral. A. _1_ soda B. _2_ soap C. _1_ coffee D. _1_ wine E. _3_ water F. _1_ grapefruit

7. LecturePLUS Timberlake7 Learning Check AB2 Identify each as characteristic of an A) acid or B) base ____ 1. Sour taste ____ 2. Produces OH - in aqueous solutions ____ 3. Chalky taste ____ 4. Is an electrolyte ____ 5. Produces H + in aqueous solutions

8. LecturePLUS Timberlake8 Solution AB2 Identify each as a characteristic of an A) acid or B) base _A_ 1. Sour taste _B_ 2. Produces OH - in aqueous solutions _B_ 3. Chalky taste A, B 4. Is an electrolyte _A_ 5. Produces H + in aqueous solutions

9. LecturePLUS Timberlake9 Some Common Acids HCl hydrochloric acid HNO 3 nitric acid H 3 PO 4 phosphor ic acid H 2 SO 4 sulfur ic acid CH 3 COOH acet ic acid

10. LecturePLUS Timberlake10 Learning Check AB3 Give the names of the following A. HBr (aq)1. bromic acid 2. bromous acid 3. hydrobromic acid B. H 2 CO 3 1. carbonic acid 2. hydrocarbonic acid 3. carbonous acid

11. LecturePLUS Timberlake11 Solution AB3 A. HBr3. hydrobromic acid The name of a nonoxy acid begins with the prefix hydro- and ends with -ic acid. In a nonoxy acid, the negative anion end in -ide. B. H 2 CO 3 1. carbonic acid The name of an oxyacid is named with the stem of the anion (carbonate) changed to -ic acid

12. LecturePLUS Timberlake12 Some Common Bases NaOHsodium hydroxide KOH potassium hydroxide Ba(OH) 2 ________________________ Mg(OH) 2 ________________________ Al(OH) 3 aluminum hydroxide

13. LecturePLUS Timberlake13 Learning Check AB4 Match the formulas with the names: A. ___ HNO 2 1) hydrochloric acid B. ___Ca(OH) 2 2) sulfuric acid C. ___H 2 SO 4 3) sodium hydroxide D. ___HCl4) nitrous acid E. ___NaOH5) calcium hydroxide

14. LecturePLUS Timberlake14 Solution AB4 Match the formulas with the names: A. _4__ HNO 2 1) hydrochloric acid B. _5__Ca(OH) 2 2) sulfuric acid C. _2__H 2 SO 4 3) sodium hydroxide D. _1__HCl4) nitrous acid E. _3__NaOH5) calcium hydroxide

15. LecturePLUS Timberlake15 Learning Check AB5 Acid, Base Name or Salt CaCl 2 _______________________ KOH_______________________ Ba(OH) 2 ______ _________________ HBr_______________________ H 2 SO 4 ________________________

16. LecturePLUS Timberlake16 Solution AB5 Acid, Base Name or Salt CaCl 2 saltcalcium chloride KOHbasepotassiuim hydroxide Ba(OH) 2 basebarium hydroxide HBracidhydrobromic acid H 2 SO 4 acidsulfuric acid

17. LecturePLUS Timberlake17 Bronsted-Lowry Acids Acids are hydrogen ion (H +) donors Bases are hydrogen ion (H + ) acceptors HCl + H 2 O H 3 O + + Cl - donor acceptor + - +

18. LecturePLUS Timberlake18 Chapter 9 Acids and Bases Acid-Base Neutralization Buffers Acid-Base Titration

19. LecturePLUS Timberlake19 Neutralization Reactions When acid and bases with equal amounts of hydrogen ion H + and hydroxide ions OH - are mixed, the resulting solution is neutral. NaOH (aq) + HCl(aq) NaCl + H 2 O base acid salt water Ca(OH) 2 + 2 HCl CaCl 2 + 2H 2 O base acid salt water

20. LecturePLUS Timberlake20 Neutralization H 3 O + and OH - combine to produce water H 3 O + + OH - 2 H 2 O from acid from base neutral Net ionic equation: H + + OH - H 2 O

21. LecturePLUS Timberlake21 Ionic Equations for Neutralization Write strong acids, bases, and salt as ions H + + Cl - + Na + + OH - Na + + Cl - + H 2 O Cross out matched ions H + + Cl - + Na + + OH - Na + + Cl - + H 2 O Write a net ionic reaction H + + OH - H 2 O

22. LecturePLUS Timberlake22 Balancing Neutralization Equations Write the equation for the neutralization between magnesium hydroxide and nitric acid. 1. Write the formulas of the acid and base Mg(OH) 2 + HNO 3 2. Balance to give equal OH - and H + Mg(OH) 2 + 2 HNO 3

23. LecturePLUS Timberlake23 3. Write the products: Mg(OH) 2 + 2HNO 3 Mg(NO 3 ) 2 + H 2 O saltwater (metal and nonmetal ) 4. Balance products Mg(OH) 2 + 2 HNO 3 Mg(NO 3 ) 2 + 2 H 2 O

24. LecturePLUS Timberlake24 Learning Check N2 Select the correct group of coefficients for the following neutralization equations A. __ HCl + __ Al(OH) 3 __AlCl 3 + __ H 2 O 1) 1, 3, 3, 12) 3, 1, 1, 1 3) 3, 1, 1 3 B.__ Ba(OH) 2 + __H 3 PO 4 __Ba 3 (PO 4 ) 2 + __ H 2 O 1) 3, 2, 2, 22) 3, 3, 1, 6 3) 2, 3, 1, 6

25. LecturePLUS Timberlake25 Solution N2 A. 3HCl + 1Al(OH) 3 1AlCl 3 + 3H 2 O B. 3Ba(OH) 2 + 2H 3 PO 4 1Ba 3 (PO 4 ) 2 + 6H 2 O

26. LecturePLUS Timberlake26 Learning Check N3 Write a balanced equation and calculate the mL of 2.00 M H 2 SO 4 required to neutralize 50.0 mL of 1.00 M KOH? ___H 2 SO 4 + ___KOH ___K 2 SO 4 + H 2 O 1)12.5 mL 2) 50.0 mL3) 200. mL

27. LecturePLUS Timberlake27 Solution N3 How many mL of 2.00 M H 2 SO 4 are required to neutralize 50.0 mL of 1.00 M KOH? H 2 SO 4 + 2KOH K 2 SO 4 + 2H 2 O 0.0500 L x 1.00 mole KOH x 1 mole H 2 SO 4 x 1 L 2 mole KOH 1 L x 1000 mL = 12.5 mL 2 mole KOH 1 L

28. LecturePLUS Timberlake28 Learning Check N4 A 25 mL sample of phosphoric acid is neutralized by 40. mL of 1.5 M NaOH. What is the molarity of the phosphoric acid solution? 3NaOH + H 3 PO 4 Na 3 PO 4 + 3H 2 O 1) 0.45 M2) 0.80 M3) 7.2 M

29. LecturePLUS Timberlake29 Solution S4 0.040 L x 1.5 mole NaOH x 1 mole H 3 PO 4 1 L 3 mole NaOH x 1 = 0.80 mol/L = 0.80 M 0.025 L

30. LecturePLUS Timberlake30 Acids and Bases Ionization of Water The pH Scale

31. LecturePLUS Timberlake31 Ionization of Water Occasionally, in water, a H + is transferred between H 2 O molecules........ H : O : + : O : H H : O : H + + : O : H -........ H H H water molecules hydronium hydroxide ion (+) ion (-)

32. LecturePLUS Timberlake32 Pure Water is Neutral Pure water contains small, but equal amounts of ions: H 3 O + and OH - H 2 O + H 2 O H 3 O + + OH - hydronium hydroxide ion ion 1 x 10 -7 M H3O+H3O+ OH -

33. LecturePLUS Timberlake33 Ion Product of Water K w [ ] = Molar concentration K w = [ H 3 O + ] [ OH - ] = [ 1 x 10 -7 ][ 1 x 10 -7 ] = 1 x 10 -14

34. LecturePLUS Timberlake34 Acids Increase H + HCl (g) + H 2 O (l) H 3 O + (aq) + Cl - (aq) More [H 3 O + ] than water > 1 x 10 -7 M As H 3 O + increases, OH - decreases [H 3 O + ] > [OH - ] H3O+H3O+ OH -

35. LecturePLUS Timberlake35 Bases Increase the hydroxide ions (OH - ) H 2 O NaOH (s) Na + (aq) + OH - (aq) More [OH - ] than water, [OH - ] > 1 x 10 -7 M When OH - increases, H 3 O + decreases [OH ] > [H 3 O + ] H3O+H3O+ OH -

36. LecturePLUS Timberlake36 Using K w The [OH - ] of a solution is 1.0 x 10 - 3 M. What is the [H 3 O + ]? K w = [H 3 O + ] [OH - ]= 1.0 x 10 -14 [H 3 O + ] =1.0 x 10 -14 [OH - ] [H 3 O + ] = 1.0 x 10 -14 = 1.0 x 10 -11 M 1.0 x 10 - 3

37. LecturePLUS Timberlake37 Learning Check pH1 The [H 3 O + ] of lemon juice is 1.0 x 10 -3 M. What is the [OH - ] of the solution? 1) 1.0 x 10 3 M 2) 1.0 x 10 -11 M 3) 1.0 x 10 11 M

38. LecturePLUS Timberlake38 Solution pH1 The [H 3 O + ] of lemon juice is 1.0 x 10 - 3 M. What is the [OH - ]? [OH - ] = 1.0 x 10 -14 = 1.0 x 10 -11 M 1.0 x 10 - 3

39. LecturePLUS Timberlake39 Using the Calculator 1.0 x 10 -14 4.0 x 10 -5 Enter 1.0 EE +/- 14 4.0 EE +/- 5 = 2.5 x 10 -10

40. LecturePLUS Timberlake40 Learning Check pH2 The [OH-] of a solution is 5 x 10 -5 M. What is the [H 3 O + ] of the solution? 1) 2 x 10 - 5 M 2) 1 x 10 10 M 3) 2 x 10 -10 M

41. LecturePLUS Timberlake41 Solution pH2 The [OH - ] of a water solution is 5 x 10 -5 M. What is the [H 3 O + ] in the solution? [ H 3 O + ] = 1.0 x 10 -14 5 x 10 - 5 On some calculators: 1.0 EE +/- 14 5 EE +/- 5 = 2 x 10 -10 M

42. LecturePLUS Timberlake42 Learning Check pH3 A.The [OH - ] when [H 3 O + ] of 1 x 10 - 4 M 1) 1 x 10 -6 M 2) 1 x 10 -8 M 3) 1 x 10 -10 M B.The [H 3 O + ] when [OH - ] of 5 x 10 -9 M 1) 1 x 10 - 6 M 2) 2 x 10 - 6 M 3) 2 x 10 -7 M

43. LecturePLUS Timberlake43 Solution pH3 K w = [H 3 O + ][OH - ] = 1.0 x 10 14 A. (3) [OH - ] = 1.0 x 10 -14 = 1.0 x 10 -10 1.0 x 10 - 4 B. (2) [H 3 O + ] = 1.0 x 10 -14 = 2 x 10 - 6 5 x 10 - 9

44. LecturePLUS Timberlake44 pH Indicates the acidity [H 3 O + ] of the solution pH = - log [H 3 O + ] From the French pouvoir hydrogene (hydrogen power or power of hydrogen)

45. LecturePLUS Timberlake45 In the expression for [H 3 O + ] 1 x 10 -exponent the exponent = pH [H 3 O + ] = 1 x 10 -pH M pH

46. LecturePLUS Timberlake46 pH Range 0 1 2 3 4 5 6 7 8 9 10 11 12 13 14 Neutral [H + ] > [OH - ] [H + ] = [OH - ] [OH - ] > [H + ] Acidic Basic

47. LecturePLUS Timberlake47 Some [H 3 O + ] and pH [H 3 O + ] pH 1 x 10 -5 M 5 1 x 10 -9 M 9 1 x 10 -11 M 11

48. LecturePLUS Timberlake48 pH of Some Common Acids gastric juice1.0 lemon juice2.3 vinegar2.8 orange juice3.5 coffee5.0 milk6.6

49. LecturePLUS Timberlake49 pH of Some Common Bases blood 7.4 tears 7.4 seawater 8.4 milk of magnesia10.6 household ammonia11.0

50. LecturePLUS Timberlake50 Learning Check pH4 A. The [H 3 O + ] of tomato juice is 1 x 10 -4 M. What is the pH of the solution? 1) - 42)43)8 B. The [OH - ] of an ammonia solution is 1 x 10 -3 M. What is the pH of the solution? 1) 32)113)-11

51. LecturePLUS Timberlake51 Solution pH4 A. pH = - log [ 1 x 10 -4 ] = -(- 4) = 4 B. [H 3 O + ] = 1 x 10 -11 pH = - log [ 1 x 10 - 11 ] = -(- 11) = 11

52. LecturePLUS Timberlake52 Learning Check pH5 The pH of a soap is 10. What is the [H 3 O + ] of the soap solution? 1) 1 x 10 - 4 M 2) 1 x 10 10 M 3) 1 x 10 - 10 M

53. LecturePLUS Timberlake53 Solution pH5 The pH of a soap is 10. What is the [H 3 O + ] of the soap solution? [H 3 O + ] = 1 x 10 -pH M = 1 x 10 -10 M

54. LecturePLUS Timberlake54 pH on the Calculator [H 3 O + ] is 4.5 x 10 -6 M pH = 4.5 x EXP(or EE) 6+/- LOG +/- = 5.35

55. LecturePLUS Timberlake55 Learning Check pH6 A soap solution has a [H 3 O + ] = 2 x 10 -8 M. What is the pH of the solution? 1)8 2) 7.7 3)6

56. LecturePLUS Timberlake56 Solution pH6 A soap solution has a [H 3 O + ] = 2.0 x 10 -8 M. What is the pH of the solution? B) 2.0 EE 8 +/- LOG +/- = 7.7

57. LecturePLUS Timberlake57 Learning Check pH7 Identify each solution as 1. acidic 2. basic3. neutral A. _____ HCl with a pH = 1.5 B. _____ Pancreatic fluid [H + ] = 1 x 10 -8 M C. _____ Sprite soft drink pH = 3.0 D. _____ pH = 7.0 E. _____ [OH - ] = 3 x 10 -10 M F. _____ [H + ] = 5 x 10 -12

58. LecturePLUS Timberlake58 Solution pH7 Identify each solution as 1. acidic 2. basic3. neutral A. _1__ HCl with a pH = 1.5 B. _2__ Pancreatic fluid [H + ] = 1 x 10 -8 M C. _1__ Sprite soft drink pH = 3.0 D. _3__ pH = 7.0 E. _1__ [OH - ] = 3 x 10 -10 M F. _2__ [H + ] = 5 x 10 -12

59. LecturePLUS Timberlake59 Acid Rain Unpolluted rain has a pH of 5.6 Rain with a pH below 5.6 is acid rain CO 2 in the air forms carbonic acid CO 2 + H 2 O H 2 CO 3 Adds to H + of rain H 2 CO 3 H + (aq) + HCO 3 -(aq) Formation of acid rain: 1. Emission of sulfur and nitrogen oxides from the burning of fuels expecially coal with high S content, power stations, oil refineries, vehicles as well as bacterial decomposition, and lighting hitting N 2 SO 2 26 million tons in 1980 NO and NO 2 22 million tons in 1980 Mt. St Helens (1980) 400,000 tons SO 2 2. Reactions in the atmosphere form SO 3 2SO 2 + O 2 2 SO 3 3. Reactions with atmosphere water form acids SO 3 + H 2 O H 2 SO 4 sulfuric acid NO + H 2 O HNO 2 nitrous acid HNO 2 + H 2 O HNO 3 nitric acid 4. Effects of Acid Rain Decline in fish populations in rivers and lasts due to toxic effect of Al leached from soil by acid rain Extensive fish kills in spring from runoff due to accumulation of large amounts of acid on the snow Dissolves minerals Mg, Ca, and K from the soil and waxy coatings that protect leaves from bacteria Corrodes metals, textiles, paper and leather

60. LecturePLUS Timberlake60 Sources of Acid Rain Power stations Oil refineries Coal with high S content Car and truck emissions Bacterial decomposition, and lighting hitting N 2

61. LecturePLUS Timberlake61 SO 2 26 million tons in 1980 NO and NO 2 22 million tons in 1980 Mt. St Helens (1980) 400,000 tons SO 2 Reactions with oxygen in air form SO 3 2SO 2 + O 2 2 SO 3 Reactions with water in air form acids SO 3 + H 2 O H 2 SO 4 sulfuric acid NO + H 2 O HNO 2 nitrous acid HNO 2 + H 2 O HNO 3 nitric acid

62. LecturePLUS Timberlake62 Effects of Acid Rain Leaches Al from soil, which kills fish Fish kills in spring from runoff due to accumulation of large amounts of acid in snow Dissolves waxy coatings that protect leaves from bacteria Corrodes metals, textiles, paper and leather

63. LecturePLUS Timberlake63 Chapter 9 Acids and Bases Strengths of Acids and Bases Making Dilutions

64. LecturePLUS Timberlake64 Strengths of Acids and Bases Strong acids completely ionize (100%) in aqueous solutions HCl + H 2 O H 3 O + + Cl - (100 % ions ) Strong bases completely (100%) dissociate into ions in aqueous solutions. NaOH Na + (aq) + OH - (aq) (100 % ions)

65. LecturePLUS Timberlake65 NH 3, A Bronsted-Lowry Base When NH 3 reacts with water, most of the reactants remain dissolved as molecules, but a few NH 3 reacts with water to form NH 4 + and hydroxide ion. NH 3 + H 2 O NH 4 + (aq) + OH - (aq) acceptor donor+

66. LecturePLUS Timberlake66 Strong and Weak Acids and Bases Strong acids HCl, HNO 3, H 2 SO 4 Most other acids are weak. Strong bases NaOH, KOH, and Ca(OH) 2 Most other bases are weak.

67. LecturePLUS Timberlake67 Learning Check SW1 Identify each of the following as a 1) strong acid or base 2) weak acid 3) weak base A. ___ HCl (aq) B. ___ NH 3 (aq) C. ___ NaOH (aq) D. ___ H 2 CO 3 (aq)

68. LecturePLUS Timberlake68 Solution SW1 Identify each of the following as a 1) strong acid or base 2) weak acid 3) weak base A. _1__ HCl (aq) B. _3__ NH 3 (aq) C. _1__ NaOH (aq) D. _2__ H 2 CO 3 (aq)

69. LecturePLUS Timberlake69 Antacids Used to neutralize stomach acid (HCl) Many contain one or more weak bases Alka-Seltzer: NaHCO 3, citric acid, and aspirin Di-gel: CaCO 3 and Mg(OH) 2 Gelusil: Al(OH) 3 and Mg(OH) 2 Maalox: Al(OH) 3 and Mg(OH) 2 Mylanta: Al(OH) 3 and Mg(OH) 2

70. LecturePLUS Timberlake70 More Antacids Milk of Magnesia: Mg(OH) 2 Rolaids: AlNa(OH) 2 CO 3 aluminum sodium dihydroxy carbonate Tums: CaCO 3 Tempo: CaCO 3, Al(OH) 3, Mg(OH) 2

71. LecturePLUS Timberlake71 Dilutions Add water Volume increases. New concentration is less than initial

72. LecturePLUS Timberlake72 Concentration of A Diluted Solution A 25 mL sample of a 6.0 M KOH is diluted by adding 75 mL of water. Calculate the new concentration of the KOH solution. Moles KOH = 0.025 L x 6.0 moles = 0.15 moles 1 L New volume = 25 mL + 75 mL = 100. mL = 0.100 L New molarity = 0.15 moles = 1.5 M 0.100 L

73. LecturePLUS Timberlake73 Learning Check SW 2 A 125 mL sample of a 3.0 M HCl is diluted by adding 250 mL of water. The new concentration of the HCl solution is 1) 8.0 M 2) 1.5 M 3) 1.0 M

74. LecturePLUS Timberlake74 Solution SW 2 3) 1.0 M moles HCl = 0.250 L x 3.0 moles = 0.75 mole 1 L new M = 0.75 mole1.0 M HCl 0.750 L (new volume)

75. LecturePLUS Timberlake75 Learning Check SW 3 A 50.0 mL sample of 15% sucrose solution is diluted by adding 200. mL of water. The new concentration of the sucrose solution is 1) 3.0 % 2) 7.5 % 3) 10. %

76. LecturePLUS Timberlake76 Learning Check SW 3 A 50.0 mL sample of 15% sucrose solution is diluted by adding 200. mL of water. The new concentration of the sucrose solution is 1) 3.0 % g sucrose = 50.0 mL x 15 g sucrose = 7.5 g 100 mL new % = 7.5 g sucrose = 3.0 % sucrose 250 mL (new volume)