unit 1.7 simple equilibria and acid based reaction

Cards (14)

  • reversible
    reaction in which the conversion of reactants to products and conversion of products to reactants occurs simultaneously
  • dynamic equilibrium
    occurs in a closed system when the rate of the forward reaction is equal to the rate of the reverse reaction and all concentration remain the same
  • le chateliers principle
    states that when a system in dynamic equilibrium is subjected to change, the position of equilibrium will shift to minimise change
  • 3 factors affecting position of equilibrium
    1. concentration
    2. temperature
    3. pressure (only in reactions involving gases)
  • temperature
    • increaes in temperature will always favour endothermic as temp will decrease as heat is absorbed
    • decrease temp will always favour exothermic as temp will increase as heat is released
  • equilibria constant
    Kc=[C][D][A][B]\frac{\left[C\right]\left[D\right]}{\left[A\right]\left[B\right]}
    CD= products
    AB= reactants
  • Kc= 1
    dynamic equilibrium
  • pH
    measure of how much hydrogen is in a solution
    small changes are actually a big difference
  • pH= log10\log_{10}[H+(aq)]\left[H^+(aq)\right]
    [H+(aq)]\left[H^+(aq)\right]=10pH10^{-pH}
  • strong acid
    any acid thats not a carboxylic acid
  • proton
    hydrogen ion
  • monoprotic
    acid with only one hydrogen
  • strong acids completely dissociate
    concentration of hydrogen will be the same as the original acid concentration
  • acid dissociation constant
    Ka, equilibria constant for acids