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Acids and Bases

Acids and Bases. …and Airman 1 st class HCl flew back over the front lines, confident that he had neutralized the enemy’s strongest base. NaOH into HCl. NaOH into HC 2 H 3 O 2. NaOH into NH 4 Cl. Arrhenius acids and bases. Substances that ionize in water to form H + ions are acids .

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Acids and Bases

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  1. Acids and Bases …and Airman 1st class HCl flew back over the front lines, confident that he had neutralized the enemy’s strongest base.

  2. NaOH into HCl

  3. NaOH into HC2H3O2

  4. NaOH into NH4Cl

  5. Arrhenius acids and bases • Substances that ionize in water to form H+ ions are acids. • Substances that ionize in water to form OH-ions are bases.

  6. Arrhenius acids and bases • Substances that ionize in water to form H+ ions are acids. • Substances that ionize in water to form OH-ions are bases. • Remember strong and weak electrolytes?

  7. Arrhenius acids and bases • Substances that ionize in water to form H+ ions are acids. • Substances that ionize in water to form OH-ions are bases. • Remember strong and weak electrolytes?Strong acids and bases ionize completelyWeak acids and bases ionize partially.

  8. Acids Bases Examples?

  9. Acids Bases Properties of Acids and Bases

  10. Acids Are electrolyte solutions Make ions in solution Affect indicators Have low pH Taste sour Neutralize bases Can cause serious burns Corrode reactive metals Have more H+ than OH- (in solution) Bases Are electrolyte solutions Make ions in solution Affect indicators Have high pH Taste bitter Neutralize acids Can cause serious burns Corrode aluminum only Have more OH- than H+ (in solution) Properties of Acids and Bases

  11. Acids Are electrolyte solutions Make ions in solution Affect indicators Have low pH Taste sour Neutralize bases Can cause serious burns Corrode reactive metals Have more H+ than OH- (in solution) Bases Are electrolyte solutions Make ions in solution Affect indicators Have high pH Taste bitter Neutralize acids Can cause serious burns Corrode aluminum only Have more OH- than H+ (in solution) Properties of Both

  12. BrØnsted-Lowry Definition • Substances that donate a proton (H+ ion) in a reaction are acids. • Substances that accept a proton (H+ ion) are bases.

  13. Lewis Definition • Substances that accept an electron pair in a reaction are acids. • Substances that donate an electron pair are bases.

  14. Conjugates • After an acid has donated a proton, the rest of the species is the conjugate base. HAA- + H+ • After a base has accepted a proton, the resulting species is the conjugate acid. B- + H+ HB

  15. What is the conjugate base of… • HCl • CH3COOH • H2SO4 • HSO4- • H2O • NH4+ • NH3

  16. What is the conjugate base of… ACID(loses H+ to form its)Conjugate base • HCl • CH3COOH • H2SO4 • HSO4- • H2O • NH4+ • NH3

  17. What is the conjugate base of… ACID(loses H+ to form its)Conjugate base • HCl ( H+ and)Cl- • CH3COOH • H2SO4 • HSO4- • H2O • NH4+ • NH3

  18. What is the conjugate base of… ACID(loses H+ to form its)Conjugate base • HCl ( H+ and)Cl- • CH3COOH( H+ and)CH3COO- • H2SO4( H+ and)HSO4- • HSO4-( H+ and)SO4-2 • H2O ( H+ and)OH- • NH4+ ( H+ and)NH3 • NH3( H+ and)NH2-

  19. What is the conjugate acid of… • NO3- • C2O4-2 • HPO4-2 • HSO4- • H2O • F-

  20. What is the conjugate acid of… Base(gains H+ to form its)Conjugate acid • NO3- • C2O4-2 • HPO4-2 • HSO4- • H2O • F-

  21. What is the conjugate acid of… Base(gains H+ to form its)Conjugate acid • NO3-(+H+  ) HNO3 • C2O4-2 • HPO4-2 • HSO4- • H2O • F-

  22. What is the conjugate acid of… Base(gains H+ to form its)Conjugate acid • NO3-(+H+  ) HNO3 • C2O4-2(+H+  ) HC2O4- • HPO4-2(+H+  ) H2PO4- • HSO4-(+H+  ) H2SO4 • H2O (+H+  ) H3O+ • F-(+H+  ) HF

  23. Nomenclature • If the anion name then the acid name • ends in…. is…

  24. Fill in the blanks • HCl is _____________acid • HClO4 is _____________acid • HClO3 is _____________acid • HClO2 is _____________acid • HClOis _____________acid

  25. Fill in the blanks Hydrogen chloride Hydrogen perchlorate • HCl is _____________acid • HClO4 is _____________acid • HClO3 is _____________acid • HClO2 is _____________acid • HClOis _____________acid Hydrogen chlorate Hydrogen chlorite Hydrogen hypochlorite

  26. Nomenclature • If the anion name then the acid name • ends in…. is… • --ide Hydro___ic acid • (hypo--) --ite Hypo___ous acid • --ite ___ous acid • --ate ___ic acid • (per--) –ate Per ___ic acid

  27. Fill in the blanks • HNO3 is _____________acid • HIO4 is _____________acid • H2CO3 is _____________acid • H3PO3 is _____________acid • HBrOis _____________acid

  28. Fill in the blanks • _____________is hydrocyanic acid • _____________is perbromic acid • _____________is phosphoric acid • _____________is sulfurous acid • _____________is hypoiodous acid

  29. Show the conjugate acid/base pairs in the following reactions. • C2O4-2 + H3O+ HC2O4- + H2O • CH3COOH + NH2-  NH3 + CH3COO-

  30. Show the conjugate acid/base pairs in the following reactions. Acid • C2O4-2 + H3O+ HC2O4- + H2O • CH3COOH + NH2-  NH3 + CH3COO- ConjugateBase Conjugate Acid Base

  31. Show the conjugate acid/base pairs in the following reactions. Acid • C2O4-2 + H3O+ HC2O4- + H2O • CH3COOH + NH2-  NH3 + CH3COO- ConjugateBase Conjugate Acid Base Conjugate Acid Base Acid ConjugateBase

  32. Water dissociates! H2O  H+ + OH- This makes an equilibrium for water where: Kw=[H+][OH-]=1 x 10-14 (at 25oC)

  33. Water dissociates! H2O  H+ + OH- This makes an equilibrium for water where: Kw=[H+][OH-]=1 x 10-14 (at 25oC) (endothermic or exothermic?) (Does Kw increase or decrease at higher T?)

  34. Water dissociates! H2O  H+ + OH- This makes an equilibrium for water where: Kw=[H+][OH-]=1 x 10-14 (at 25oC) (endothermicor exothermic?) (Does Kwincreaseor decrease at higherT?)

  35. [H+] is inversely related to [OH-] • When [H+] increases, [OH-] decreases in a water solution, and vice versa.

  36. [H+] is inversely related to [OH-] • When [H+] decreases, [OH-] increases in a water solution, and vice versa. (Why?)

  37. pH • The basic (and acidic) definitions are: pH= -log [H+] [H+]= 10-pH pOH= -log [OH-] [OH-]=10 -pOH Kw=[H+][OH-]=1 x 10 -14 (at 25oC) pH + pOH = 14 (at 25oC)

  38. pH practice • If pH is 3.38…. • What is the pOH?

  39. pH practice • If pH is 3.38…. • What is the pOH? 14-pH= 10.62

  40. pH practice • If pH is 3.38…. • What is the pOH? 14-pH= 10.62 • What is [H+]?

  41. pH practice • If pH is 3.38…. • What is the pOH? 14-pH= 10.62 • What is [H+]? 10-3.38= 4.17 x 10-4M

  42. pH practice • If pH is 3.38…. • What is the pOH? 14-pH= 10.62 • What is [H+]? 10-3.38= 4.17 x 10-4M • What is [OH-]?

  43. pH practice • If pH is 3.38…. • What is the pOH? 14-pH= 10.62 • What is [H+]? 10-3.38= 4.17 x 10-4M • What is [OH-]? 10-10.62=2.40x10-11M and Kw/4.17x10-4M=2.40x10-11 M!

  44. pH practice • If [OH-]= 4.8 x 10-6 M…

  45. pH practice • If [OH-]= 4.8 x 10-6 M… • What is pOH?

  46. pH practice • If [OH-]= 4.8 x 10-6 M… • What is pOH? -log (4.8 x 10-6 )= 5.32

  47. pH practice • If [OH-]= 4.8 x 10-6 M… • What is pOH? -log (4.8 x 10-6 )= 5.32 • What is pH?

  48. pH practice • If [OH-]= 4.8 x 10-6 M… • What is pOH? -log (4.8 x 10-6 )= 5.32 • What is pH? 14-5.32= 8.68

  49. pH practice • If [OH-]= 4.8 x 10-6 M… • What is pOH? -log (4.8 x 10-6 )= 5.32 • What is pH? 14-5.32= 8.68 • What is [H+]?

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