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Acids and Bases: Strong and Weak, pH

  • Arrhenius acids give H+ ; Arrhenius bases give OH-

  • Bronsted-Lowry acids are H+ donors; B-L bases are H+ acceptors

  • Lewis bases are electron pair donors, like NH3 ; Lewis acids are electron pair acceptors like BF3

  • Common strong acids: HCl, HNO3 (monoprotic); H2SO4 (diprotic)

  • Common strong bases: NaOH, KOH, Ca(OH)2

  • Weak acid: acetic, CH3COOH

  • Weak base: NH3

  • Water is both weak acid and weak base; Kw = 1.0 x 10-14

  • Equilibria of weak acids and bases: Ka and Kb

  • pH = -log10[H+] ; pH = 7.0, neutral; pH < 7, acidic; pH >7, basic

Acids and Bases: Strong and Weak, pH

Lecture Slides are screen-captured images of important points in the lecture. Students can download and print out these lecture slide images to do practice problems as well as take notes while watching the lecture.

  • Intro 0:00
  • Acids 0:36
    • React with Some Metals
    • Litmus Test (Red)
  • Bases 4:33
    • Litmus Test (Blue)
    • Acids and Base Neutralize
  • Classification: Arrhenius and Bronsted-Lowry 8:52
    • Arrhenius Classification
    • Example: HCl (Hydronium) and NaOH (Hydroxide)
    • Bronsted-Lowry Classification
    • Example: HCl
    • Conjugate Acid, Conjugate Base
  • Lewis Acids and Bases 16:23
    • Lewis Base: Electron Pair Donor
    • Lewis Acid: Electron Pair Acceptor
    • Example: Lewis Acid Base Reaction
  • Common Strong Acids 22:02
  • Common Strong Bases 24:39
  • Common Weak Acids 26:24
  • Common Weak Bases 31:14
  • Water as an Acid and Base: Kw 34:01
    • K of Water
  • Ionization Constants for Weak Acids 38:11
    • Examples: Constants
  • Ionization Constants for Weak Bases 40:30
    • Examples: Constants
  • pH and the pH Scale 43:12
    • Sorenson pH
    • Neutral Water
    • Acid and Base pH
    • pH Scale (Acid and Alkaline)
  • Additional Example 1