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Acids and Bases

Acids and Bases. 1. 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). 2. 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 1

  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) 2

  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 3

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

  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 5

  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 6

  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 7

  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 8

  9. Some Common Acids HClhydrochloric acid HNO3nitric acid H3PO4phosphoric acid H2SO4sulfuric acid CH3COOH acetic acid 9

  10. Learning Check AB3 Give the names of the following A. HBr (aq)1. bromic acid 2. bromous acid 3. hydrobromic acid B. H2CO31. carbonic acid 2. hydrocarbonic acid 3. carbonous acid 10

  11. 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.H2CO31. carbonic acid The name of an oxyacid is named with the stem of the anion (carbonate) changed to -ic acid 11

  12. Some Common Bases NaOHsodium hydroxide KOHpotassium hydroxide Ba(OH)2________________________ Mg(OH)2________________________ Al(OH)3aluminum hydroxide 12

  13. Learning Check AB4 Match the formulas with the names: A. ___ HNO21)hydrochloric acid B. ___Ca(OH)22) sulfuric acid C. ___H2SO43) sodium hydroxide D. ___HCl4) nitrous acid E. ___NaOH5) calcium hydroxide 13

  14. Solution AB4 Match the formulas with the names: A. _4__HNO21)hydrochloric acid B. _5__Ca(OH)22) sulfuric acid C. _2__H2SO43) sodium hydroxide D. _1__HCl4) nitrous acid E. _3__NaOH5) calcium hydroxide 14

  15. Learning Check AB5Learning Check AB5 Acid, Base Name or Salt CaCl2 _______________________ KOH_______________________ Ba(OH)2 ______ _________________ HBr_______________________ H2SO4________________________ 15

  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 16

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

  18. pH • Indicates the acidity [H3O+] of the solution • pH = - log [H3O+] • From the French pouvoir hydrogene (“hydrogen power” or power of hydrogen) 18

  19. pH In the expression for [H3O+] 1 x 10-exponent the exponent = pH [H3O+] = 1 x 10-pH M 19

  20. Basic Acidic pH Range 0 1 2 3 4 5 6 7 8 910 11 12 13 14 Neutral [H+]>[OH-][H+] = [OH-][OH-]>[H+] 20

  21. Some [H3O+] and pH [H3O+]pH 1 x 10-5 M5 1 x 10-9 M9 1 x 10-11M11 21

  22. pH of Some Common Acids gastric juice1.0 lemon juice2.3 vinegar2.8 orange juice3.5 coffee5.0 milk6.6 22

  23. pH of Some Common Bases blood 7.4 tears 7.4 seawater 8.4 milk of magnesia10.6 household ammonia11.0 23

  24. Learning Check pH4 A. The [H3O+] 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 24

  25. Solution pH4 A. pH = - log [ 1 x 10-4] = -(- 4) = 4 B. [H3O+] = 1 x 10-11 pH = - log [ 1 x 10- 11] = -(- 11) = 11 25

  26. Solution pH5 The pH of a soap is 10. What is the [H3O+] of the soap solution? [H3O+] = 1 x 10-pH M = 1 x 10-10 M 26

  27. Acid Rain • Unpolluted rain has a pH of 5.6 • Rain with a pH below 5.6 is “acid rain“ • CO2 in the air forms carbonic acid CO2 + H2O H2CO3 • Adds to H+ of rain H2CO3H+ (aq) + HCO3-(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 N2 SO226 million tons in 1980 NO and NO222 million tons in 1980 Mt. St Helens (1980) 400,000 tons SO2 2. Reactions in the atmosphere form SO3 2SO2 + O2⎯→ 2 SO3 3. Reactions with atmosphere water form acids SO3 + H2O ⎯→ H2SO4 sulfuric acid NO + H2O ⎯→ HNO2 nitrous acid HNO2 + H2O ⎯→ HNO3 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 27

  28. Acid Rain continued...Sources of Acid Rain • Power stations • Oil refineries • Coal with high S content • Car and truck emissions • Bacterial decomposition, and lighting hitting N2 28

  29. SO226 million tons in 1980 NO and NO222 million tons in 1980 Mt. St Helens (1980) 400,000 tons SO2 • Reactions with oxygen in air form SO3 2SO2 + O22 SO3 • Reactions with water in air form acids SO3 + H2O H2SO4 sulfuric acid NO + H2O HNO2 nitrous acid HNO2 + H2O HNO3 nitric acid 29

  30. 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 30

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