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Exp # [A] [B] [C] Rate 1) 27 C 0.10 0.10 0.10 4.0

1A + 2B  1C + 1D Calculate the equilibrium concentrations of each species when 150 mL 2.5 M A is mixed with 100.0 mL 2.5 M B. K c = 2.0 x 10 -10. 1A + 2B  1C + 1D Calculate the equilibrium concentrations of each species when a solution is made with 1.0 M A & 1.0 M B. K c = 2.0 x 10 -12.

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Exp # [A] [B] [C] Rate 1) 27 C 0.10 0.10 0.10 4.0

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  1. 1A + 2B  1C + 1DCalculate the equilibrium concentrations of each species when 150 mL 2.5 M A is mixed with 100.0 mL 2.5 M B. Kc = 2.0 x 10-10

  2. 1A + 2B  1C + 1DCalculate the equilibrium concentrations of each species when a solution is made with 1.0 M A & 1.0 M B. Kc = 2.0 x 10-12

  3. Exp # [A] [B] [C] Rate 1) 27 C 0.10 0.10 0.10 4.0 2) 27 C 0.10 0.10 0.20 8.0 3) 27 C 0.10 0.20 0.20 64 4) 27 C 0.30 0.10 0.10 36 5)127 C 0.10 0.10 0.10 400.0

  4. Exp # [A] [B] [C] Rate 1) 27 C 0.10 0.10 0.10 4.0 2) 27 C 0.10 0.10 0.20 8.0 3) 27 C 0.10 0.20 0.20 64 4) 27 C 0.30 0.10 0.10 36 5)127 C 0.10 0.10 0.10 400.0 ([A4]/[A1])a = rate4/rate1 3a = 9; thus, a = 2

  5. Exp # [A] [B] [C] Rate 1) 27 C 0.10 0.10 0.10 4.0 2) 27 C 0.10 0.10 0.20 8.0 3) 27 C 0.10 0.20 0.20 64 4) 27 C 0.30 0.10 0.10 36 5)127 C 0.10 0.10 0.10 400.0 ([B3]/[B2])b = rate3/rate2 2b = 8; thus b = 3

  6. Exp # [A] [B] [C] Rate 1) 27 C 0.10 0.10 0.10 4.0 2) 27 C 0.10 0.10 0.20 8.0 3) 27 C 0.10 0.20 0.20 64 4) 27 C 0.30 0.10 0.10 36 5)127 C 0.10 0.10 0.10 400.0 ([C2]/[C1])c = rate2/rate1 2c = 2; thus c = 1

  7. Rate = k[A]2[B]3[C] k = Rate[A]2[B]3[C]

  8. __N2 +__CO2 +__O2__NO2 +__CO __NO2 __N2O4 __N2O4 + __CO __NO +__CO2 __ NO + __ CO2  __ N2O5 + __ C __N2O5 + __C __C2N2O5

  9. __N2 +__CO2 +__O2__NO2 +__CO __NO2 __N2O4 __N2O4 + __CO __NO +__CO2 4 NO + 3 CO2 2 N2O5 + 3 C __N2O5 + __C __C2N2O5

  10. __N2 +__CO2 +__O2__NO2 +__CO __NO2 __N2O4 2 N2O4 + 4 CO 4 NO +4 CO2 4 NO + 3 CO2 2 N2O5 + 3 C __N2O5 + __C __C2N2O5

  11. __N2 +__CO2 +__O2__NO2 +__CO __NO2 __N2O4 2 N2O4 + 4 CO 4 NO +4 CO2 4 NO + 3 CO2 2 N2O5 + 3 C __N2O5 + __C __C2N2O5

  12. __N2 +__CO2 +__O2__NO2 +__CO 4 NO2 2 N2O4 2 N2O4 + 4 CO 4 NO +4 CO2 4 NO + 3 CO2 2 N2O5 + 3 C __N2O5 + __C __C2N2O5

  13. __N2 +__CO2 +__O2__NO2 +__CO 4 NO2 2 N2O4 2 N2O4 + 4 CO 4 NO +4 CO2 4 NO + 3 CO2 2 N2O5 + 3 C __N2O5 + __C __C2N2O5

  14. 2 N2 + 4 CO2 + 2 O24 NO2 + 4 CO 4 NO2 2 N2O4 2 N2O4 + 4 CO 4 NO +4 CO2 4 NO + 3 CO2 2 N2O5 + 3 C __N2O5 + __C __C2N2O5

  15. 2 N2 + 4 CO2 + 2 O24 NO2 + 4 CO 4 NO2 2 N2O4 2 N2O4 + 4 CO 4 NO +4 CO2 4 NO + 3 CO2 2 N2O5 + 3 C 2 N2 + 3 CO2 + 2 O2 2 N2O5 + 3 C __N2O5 + __C __C2N2O5

  16. 2 N2 + 4 CO2 + 2 O24 NO2 + 4 CO 4 NO2 2 N2O4 2 N2O4 + 4 CO 4 NO +4 CO2 4 NO + 3 CO2 2 N2O5 + 3 C 2 N2 + 3 CO2 + 2 O2 2 N2O5 + 3 C 2 N2O5 + 4 C 2 C2N2O5

  17. 2 N2 + 4 CO2 + 2 O24 NO2 + 4 CO 4 NO2 2 N2O4 2 N2O4 + 4 CO 4 NO +4 CO2 4 NO + 3 CO2 2 N2O5 + 3 C 2 N2 + 3 CO2 + 2 O2 2 N2O5 + 3 C 2 N2O5 + 1 4 C 2 C2N2O5

  18. Acid/Base

  19. Properties of Acids • Sour taste, Change color of dyes, Conduct electricity in solution, React with many metals, React with bases to form salts

  20. Properties of Bases • Bitter taste, Feel slippery, Change color of dyes, Conduct electricity in solution, React with acids to form salts

  21. Arrhenius • Acids: release H+ or H3O+ in solution • Bases: release OH- in solution

  22. Arrhenius • Acid: HA --> H+ + A- • HCl --> H+ + Cl- • Base: MOH --> M+ + OH- • NaOH -->Na+ + OH-

  23. Bronsted-Lowry • Acid: Proton donor • Base: Proton Acceptor

  24. Bronsted-Lowry • HA + H2O --> H3O+ + A- • HI + H2O --> H3O+ + I- • Acid Base CACB • NH3 + H2O --> NH4+ + OH- • Base Acid CA CB

  25. Lewis Acid/Base • Acid: Electron Acceptor • Base: Electron Donor

  26. Lewis Acid/Base H3N: + BF3 --> H3N-BF3 Base Acid Neutral

  27. Drill: • List 3 properties each of both acids & bases

  28. Common Names • H+ Hydrogen ion • H3O+ Hydronium ion • H- Hydride ion • OH- Hydroxide ion • NH3 Ammonia • NH4+ Ammonium ion

  29. Amphoterism • Can act like an acid or a base • Can donate or accept protons

  30. Define acids & bases by each of the three methods

  31. Naming Acids • All acids are H-anion • If the anion is: • -ides  hydro___ic acids • -ates  ___ic acids • -ites  ___ous acids

  32. Naming Bases • Almost all bases are metal hydroxides • Name by normal method • Ammonia (NH3) as well as many amines are bases

  33. Drill: Name each of the following:NaOH HIBa(OH)2 H2SO4HMnO4 H3PO3

  34. Strong Acids or Bases • Strong acids or bases ionize 100 % in solution • Weak acids or bases ionize <100 % in solution

  35. Strong Acids • HClO4 Perchloric acid • H2SO4 Sulfuric acid • HNO3 Nitric acid • HCl Hydrochloric acid • HBr Hydrobromic acid • HI Hydroiodic acid

  36. Strong Bases • All column I hydroxides • Ca(OH)2 Calcium hydroxide • Sr(OH)2 Strontium hydroxide • Ba(OH)2 Barium hydroxide

  37. Binary Acids • Acids containing only 2 elements • HCl Hydrochloric acid • H2S Hydrosulfuric acid

  38. Ternary Acids • Acids containing 3 elements • H2SO4 Sulfuric acid • H2SO3 Sulfurous acid • HNO3 Nitric acid

  39. Drill: Name & give the formula for at least 4 each of strong acids & strong bases

  40. Strong Acid/Base Ionizes 100 % (1 M) HA H+ + A- 1 M – all 1 1

  41. Monoprotic Acids • Acids containing only one ionizable hydrogen • HBr Hydrobromic acid • HCN Hydrocyanic acid • HC2H3O2 Acetic acid

  42. Diprotic Acids • Acids containing 2 ionizable hydrogens • H2SO4 Sulfuric acid • H2SO3 Sulfurous acid • H2CO3 Carbonic acid

  43. Triprotic Acids • Acids containing 3 ionizable hydrogens • H3PO4 Phosphoric acid • H3PO3 Phosphorus acid • H3AsO4 Arsenic acid

  44. Polyprotic Acids • Acids containing more than one ionizable hydrogens • H2SO4 Sulfuric acid • H4SiO4 Silicic acid • H2CO2 Carbonous acid

  45. Monohydroxic Base • A base containing only one ionizable hydroxide • NaOH Sodium hydroxide • KOH Potassium hydro. • LiOH Lithium hydroxide

  46. AP CHM HW • Read: Chapter 13 • Problems: 1 - 3 • Page: 395

  47. CHM II HW • Read: Chapter 18 • Problems: 3 & 5 • Page: 787

  48. Neutralization Rxn • A reaction between an acid & a base making salt & H2O • HA(aq) + MOH(aq) •  MA(aq) + H2O(l)

  49. Neutralization Rxn • HCl(aq) + NaOH(aq) •  • NaCl(aq) + H2O(l)

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