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A problem in ionic equilbrium

  1. Apr 28, 2016 #1
    1. The problem statement, all variables and given/known data

    please see the attached image

    1998 ,b part question



    2. Relevant equations

    none

    3. The attempt at a solution

    i thought that Agcl would give Ag+ and cl- ions whose concentration can be found from Ksp as √Ksp,this Ag+ reacts with NH3 to give Ag(NH3)2+ (reverse of the given reaction) since Kc of the reaction is given we can find concentration of Ag(NH3)2+ from it which is Kc= [Ag(NH3)2+]/[Ag+][NH3]2

    but answer obtained is not matching, is the method correct ?,please help.
     

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  2. jcsd
  3. Apr 28, 2016 #2

    Borek

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    Staff: Mentor

    It is not clear to me whether 1M ammonia is the final concentration, or added concentration (in which case some of the ammonia would be consumed).

    Your approach is OK in the first case, can be wrong in the latter.
     
  4. Apr 28, 2016 #3
    sir it is the initial concentration i suppose
     
  5. Apr 28, 2016 #4

    Borek

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    Staff: Mentor

    Then you need to take the reaction stoichiometry into account (simplest approach: an ICE table).
     
  6. Apr 28, 2016 #5
    oh i think i made a mistake concentration of ammonia in initial state is 1 M not the equilbrium concentration,sir are the rest of steps correct?
     
  7. Apr 29, 2016 #6

    Borek

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    Staff: Mentor

    As I told you:

     
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