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Topic: Equilibrium concentrations  (Read 1868 times)

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Offline hnd2009

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Equilibrium concentrations
« on: May 04, 2011, 11:09:28 AM »
A solution is made by mixing 500.0 mL of 4.0 M NH3 and 500.0 mL of 0.40 M AgNO3.  Ag+ reacts with NH3 to form AgNH3+ and Ag(NH3)2+ according to the equilibrium reactions:

Ag+  +  NH3  ↔ AgNH3+                                K1 =  2.1 x 103
AgNH3+  +  NH3  ↔ Ag(NH3)2+   K2  =  8.2 x 103

Assuming no change in volume on mixing calculate the concentrations of all species in solution: [Ag+], [NO3-], [NH3], [AgNH3+] and [Ag(NH3)2+].


This all I've gotten so far:

Ag+ + 2NH3 --> Ag(NH3)2+
0.4M x 0.5L = 0.2moles Ag+
4M x 0.5L = 2moles NH3
Ag+ = limiting reactant
Concentration = 0.2M

I just don't know what to do from here
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Offline rabolisk

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Re: Equilibrium concentrations
« Reply #1 on: May 04, 2011, 11:34:10 AM »
If you could disregard the second reaction and only consider the first, could you do it?

Ag+ + NH3 ::equil:: AgNH3+   K1 = 2.1 x 103

Can you find the equilibrium [Ag+], [NO3-], [AgNH3+]?
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