Acids and Bases


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  • Hello class! Today we will be discussing acids and bases. Also we will be looking at pH, pOH, and anything in between!
  • Arrhenius acids vs Arrhenius bases.
  • With the definitions on the board we can see what is required, in the Arrhenius theory, to be classified as an acid or base.
  • With the Arrhenius theory, an acid would contain hydrogen and ionizes to form hydrogen ions (H+).
  • With the Arrhenius theory, a base contains a hydroxide group and ionizes to form hydroxide ions (OH-).
  • What are some examples of acids and bases that will follow these rules?
  • Acids HCl, HBr, HNO3 Bases NaOH,KOH, Mg(OH)2
  • Brønsted and Lowry build on the Arrhenius theory because sometimes a base may not contain OH-.
  • In the Brønsted Lowry theory an acid is a hydrogen donor.
  • Some examples that follow this rule is NH3, H2O, H2CO.
  • In the Brønsted Lowry theory a base is a hydrogen acceptor.
  • Acid
  • H2SO4 + KOH
  • Base
  • KHSO4 + H2O
  • Conjugate Acid
  • Here is an example of a reation
  • Conjugate Base
  • pH=-log[H+] pOH=-log[OH-]
  • In order to calculate how strong the acids and bases are you will need these formulas.
  • [H+]=[acid]*(the number of H+ ions dissociated)
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