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Chemistry: Equilibrium

  1. Apr 5, 2005 #1
    Hello there. I'm having trouble understanding equilibrium. Especially understanding if the reactions go foward or reverse when there is a change in tempertature, concentration, pressure/volume etc. For example:

    In a solution of copper (II) chloride, the following equilibrium exists.

    [tex] CuCl_4^{2-}_{(aq)} + 4H_2O_{(l)} \rightleftharpoons Cu(H_2O)_4^{2+}_{(aq)} + 4Cl^{-}_{(aq)} [/tex]

    For the following stresses put on the equilirbrium, predict the shift in the equilibrium.

    1) Hydrochloric acid is added
    2) Silver nitrate is added.


    1) Would this be a reverse reaction since the acid dissociates into [tex] HCl_{(aq)} \rightarrow H^{+}_{(aq)} + Cl^{-}_{(aq)} [/tex]? So the concentration of Cl will be increased and it will shift to the left?

    2)I think it's a reverse reaction but I'm not sure. Why would it be a reverse reaction (or foward if I'm wrong)? Thanks for the help.
     
  2. jcsd
  3. Apr 5, 2005 #2
    Yes exactly,

    Silver nitrate is soluble in water, but silver chloride isn't. So adding silver nitrate is like taking away chloride ions from solution...
     
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