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Acids

definition - increases the concentration of H+ ions when dissolved in water 

  • the H+ ion generally forms H3O+ w/ water
  • Bronsted-Lowry definition - donates proton to another substance
    • even applies to substances not dissolved in water
    • weak H-X bond, stable base, positively polarized H >> stronger acid
  • Lewis definition - electron-pair acceptor
  • pH = -log [H+]
  • strong acid - complete dissociates, [H+] = [acid]
    • HCl, HBr, HI, HNO3, HClO3, HClO4, H2SO4
  • weak acid - partially dissociates
    • Ka = [H+][conjugate base] / [acid]
    • [H+] = [conjugate base] when Ka is very small
  • polyprotic acids - have more than 1 ionizable H atom
    • easier to remove 1st proton than second
    • Ka becomes smaller
  • binary acids - contains hydrogen and 1 other element
    • bond strength determines acid strength
    • element increases in size >> bond strength decreases >> acid strength increases
    • element electronegativity increases >> polarity increases >> acid strength increases
  • oxyacids - OH and oxygen bonded to a central atom
    • element electronegativity increases, # of oxygen increases >> acid strength increases
  • carboxylic acids - contains a carboxyl group, largest cateogry of organic acids
    • # of electronegative atoms increase >> acid strength increases

Find the pH of a 0.001 M solution of acetic acid  

  • Ka = 1.8 x 10-5
  • Ka = [H+] [acetate] / [acetic acid] = x2 / 0.001
  • x = [(1.8 x 10-5) (0.001)]1/2 = 1.3 x 10-4 = [H+]
  • pH = -log [H+] = 3.87

Find the pH of 0.1 M solution of HCl  

  • strong acid, completely dissociates
  • pH = -log [HCl] = 1
Subject: 
Chemistry
Subject X2: 
Chemistry

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