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Acids and Bases

Acids and Bases. Acids and Bases. 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). Acids. Produce H + (as H 3 O + ) ions in water

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Acids and Bases

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  1. Acids and Bases Acids and Bases LecturePLUS Timberlake

  2. 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) LecturePLUS Timberlake

  3. Acids • Produce H+ (as H3O+) ions in water • Produce a negative ion (-) too • Taste sour • Corrode metals • React with bases to form salts and water LecturePLUS Timberlake

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

  5. 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 LecturePLUS Timberlake

  6. 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 LecturePLUS Timberlake

  7. 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 LecturePLUS Timberlake

  8. 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, B4. Is an electrolyte _A_ 5. Produces H+ in aqueous solutions LecturePLUS Timberlake

  9. Some Common Acids HCl hydrochloric acid HNO3 nitric acid H3PO4 phosphoric acid H2SO4 sulfuric acid CH3COOH acetic acid LecturePLUS Timberlake

  10. Learning Check AB3 Give the names of the following A. HBr (aq) 1. bromic acid 2. bromous acid 3. hydrobromic acid B. H2CO3 1. carbonic acid 2. hydrocarbonic acid 3. carbonous acid LecturePLUS Timberlake

  11. Solution AB3 A. HBr 3. 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.H2CO3 1. carbonic acid The name of an oxyacid is named with the stem of the anion (carbonate) changed to -ic acid LecturePLUS Timberlake

  12. Some Common Bases NaOH sodium hydroxide KOH potassium hydroxide Ba(OH)2 ________________________ Mg(OH)2________________________ Al(OH)3 aluminum hydroxide LecturePLUS Timberlake

  13. Learning Check AB4 Match the formulas with the names: A. ___ HNO21)hydrochloric acid B. ___ Ca(OH)2 2) sulfuric acid C. ___ H2SO4 3) sodium hydroxide D. ___ HCl 4) nitrous acid E. ___ NaOH 5) calcium hydroxide LecturePLUS Timberlake

  14. Solution AB4 Match the formulas with the names: A. _4__ HNO21)hydrochloric acid B. _5__ Ca(OH)2 2) sulfuric acid C. _2__ H2SO4 3) sodium hydroxide D. _1__ HCl 4) nitrous acid E. _3__ NaOH 5) calcium hydroxide LecturePLUS Timberlake

  15. Learning Check AB5 Acid, Base Name or Salt CaCl2 ______ _________________ KOH ______ _________________ Ba(OH)2 ______ _________________ HBr ______ _________________ H2SO4 ______ __________________ LecturePLUS Timberlake

  16. Solution AB5 Acid, Base Name or Salt CaCl2 salt calcium chloride KOH base potassiuim hydroxide Ba(OH)2 base barium hydroxide HBr acid hydrobromic acid H2SO4 acid sulfuric acid LecturePLUS Timberlake

  17. Bronsted-Lowry Acids Acids are hydrogen ion (H+) donors Bases are hydrogen ion (H+) acceptors HCl + H2O H3O+ + Cl- donor acceptor + - + + LecturePLUS Timberlake

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

  19. 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 + H2O base acid salt water Ca(OH)2 + 2 HCl CaCl2 + 2H2O base acid salt water LecturePLUS Timberlake

  20. Neutralization H3O+ and OH- combine to produce water H3O+ + OH- 2 H2O from acid from base neutral Net ionic equation: H+ + OH- H2O LecturePLUS Timberlake

  21. Ionic Equations for Neutralization Write strong acids, bases, and salt as ions H+ + Cl- + Na+ + OH- Na+ + Cl- + H2O Cross out matched ions H+ + Cl-+ Na+ + OH-Na+ + Cl- + H2O Write a net ionic reaction H+ + OH-H2O LecturePLUS Timberlake

  22. 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 + HNO3 2. Balance to give equal OH- and H+ Mg(OH)2 + 2 HNO3 LecturePLUS Timberlake

  23. 3. Write the products: Mg(OH)2 + 2HNO3 Mg(NO3)2 + H2O salt water (metal and nonmetal) 4. Balance products Mg(OH)2 + 2 HNO3 Mg(NO3)2 + 2 H2O LecturePLUS Timberlake

  24. Learning Check N2 Select the correct group of coefficients for the following neutralization equations A. __ HCl + __ Al(OH)3 __AlCl3 + __ H2O 1) 1, 3, 3, 1 2) 3, 1, 1, 1 3) 3, 1, 1 3 B.__ Ba(OH)2 + __H3PO4 __Ba3(PO4)2 + __ H2O 1) 3, 2, 2, 2 2) 3, 3, 1, 6 3) 2, 3, 1, 6 LecturePLUS Timberlake

  25. Solution N2 A. 3HCl + 1Al(OH)31AlCl3 + 3H2O B. 3Ba(OH)2 + 2H3PO41Ba3(PO4)2 + 6H2O LecturePLUS Timberlake

  26. Learning Check N3 Write a balanced equation and calculate the mL of 2.00 M H2SO4 required to neutralize 50.0 mL of 1.00 M KOH? ___H2SO4 + ___KOH ___K2SO4 + H2O 1) 12.5 mL 2) 50.0 mL 3) 200. mL LecturePLUS Timberlake

  27. Solution N3 How many mL of 2.00 M H2SO4 are required to neutralize 50.0 mL of 1.00 M KOH? H2SO4 + 2KOH K2SO4 + 2H2O 0.0500 L x 1.00 mole KOH x 1 mole H2SO4 x 1 L 2 mole KOH 1 L x 1000 mL = 12.5 mL 2 mole KOH 1 L LecturePLUS Timberlake

  28. 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 + H3PO4 Na3PO4 + 3H2O 1) 0.45 M 2) 0.80 M 3) 7.2 M LecturePLUS Timberlake

  29. Solution S4 0.040 L x 1.5 mole NaOH x 1 mole H3PO4 1 L3 mole NaOH x 1 = 0.80 mol/L = 0.80 M 0.025 L LecturePLUS Timberlake

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

  31. Ionization of Water Occasionally, in water, a H+ is transferred between H2O molecules . . . . . . . . H:O: + :O:H H:O:H + + :O:H- . . . . . . . . HH H water molecules hydronium hydroxide ion (+)ion (-) LecturePLUS Timberlake

  32. Pure Water is Neutral Pure water contains small, but equal amounts of ions: H3O+ and OH- H2O + H2O H3O+ + OH- hydronium hydroxide ion ion 1 x 10-7 M1 x 10-7 M H3O+ OH- LecturePLUS Timberlake

  33. Ion Product of Water Kw [ ] = Molar concentration Kw = [ H3O+ ] [ OH- ] = [ 1 x 10-7 ][ 1 x 10-7 ] = 1 x 10-14 LecturePLUS Timberlake

  34. Acids • Increase H+ • HCl (g) + H2O (l)H3O+(aq) + Cl-(aq) • More [H3O+] than water > 1 x 10-7M • As H3O+ increases, OH- decreases [H3O+] > [OH-] H3O+ OH- LecturePLUS Timberlake

  35. Bases • Increase the hydroxide ions (OH-) H2O • NaOH (s) Na+(aq) + OH- (aq) • More [OH-] than water, [OH-] > 1 x 10-7M • When OH- increases, H3O+ decreases [OH] > [H3O+] OH- H3O+ LecturePLUS Timberlake

  36. Using Kw The [OH- ] of a solution is 1.0 x 10- 3M. What is the [H3O+]? Kw = [H3O+ ] [OH- ] = 1.0 x 10-14 [H3O+] = 1.0 x 10-14 [OH-] [H3O+] = 1.0 x 10-14= 1.0 x 10-11 M 1.0 x 10- 3 LecturePLUS Timberlake

  37. Learning Check pH1 The [H3O+] of lemon juice is 1.0 x 10-3 M. What is the [OH-] of the solution? 1) 1.0 x 103 M 2) 1.0 x 10-11 M 3) 1.0 x 1011 M LecturePLUS Timberlake

  38. Solution pH1 The [H3O+] 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 LecturePLUS Timberlake

  39. Using the Calculator 1.0 x 10 -14 4.0 x 10-5 Enter1.0 EE +/- 14 4.0 EE+/- 5 = 2.5 x 10 -10 LecturePLUS Timberlake

  40. Learning Check pH2 The [OH-] of a solution is 5 x 10 -5 M. What is the [H3O+ ] of the solution? 1) 2 x 10- 5 M 2) 1 x 1010 M 3) 2 x 10-10 M LecturePLUS Timberlake

  41. Solution pH2 The [OH-] of a water solution is 5 x 10-5 M. What is the [H3O+] in the solution? [ H3O+] =1.0 x 10 -14 5 x 10- 5 On some calculators: 1.0 EE +/- 14 5 EE +/-5 = 2 x 10 -10 M LecturePLUS Timberlake

  42. Learning Check pH3 A.The [OH-] when [H3O+ ] 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 [H3O+] 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 LecturePLUS Timberlake

  43. Solution pH3 Kw = [H3O+ ][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) [H3O+] = 1.0 x 10 -14 = 2 x 10 - 6 5 x 10- 9 LecturePLUS Timberlake

  44. pH • Indicates the acidity [H3O+] of the solution • pH = - log [H3O+] • From the French pouvoir hydrogene (“hydrogen power” or power of hydrogen) LecturePLUS Timberlake

  45. pH In the expression for [H3O+] 1 x 10-exponent the exponent = pH [H3O+] = 1 x 10-pH M LecturePLUS Timberlake

  46. pH Range 0 1 2 3 4 5 6 7 8 910 11 12 13 14 Neutral [H+]>[OH-][H+] = [OH-][OH-]>[H+] Acidic Basic LecturePLUS Timberlake

  47. Some [H3O+] and pH [H3O+] pH 1 x 10-5 M 5 1 x 10-9 M 9 1 x 10-11M 11 LecturePLUS Timberlake

  48. pH of Some Common Acids gastric juice 1.0 lemon juice 2.3 vinegar 2.8 orange juice 3.5 coffee 5.0 milk 6.6 LecturePLUS Timberlake

  49. pH of Some Common Bases blood 7.4 tears 7.4 seawater 8.4 milk of magnesia 10.6 household ammonia 11.0 LecturePLUS Timberlake

  50. Learning Check pH4 A. The [H3O+] of tomato juice is 1 x 10-4 M. What is the pH of the solution? 1) - 4 2) 4 3) 8 B. The [OH-] of an ammonia solution is 1 x 10-3 M. What is the pH of the solution? 1) 3 2) 11 3) -11 LecturePLUS Timberlake

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