[huskywolf]

Hi in the following  electrochemical reaction Ag⁺ + 2NH₃   Ag(NH₃)₂⁺

The voltaic cell reaction was done twice . and the potentials measured were (a)E_cell= 0.07V and (b)E_cell= 0.10V .

I need to calculate the concentration of [Ag⁺] at equilibrium in each reaction using the Nernst equation (and the E_cell)I cannot figure out how to arrange the equation to get this.

Other information I have is E^o =0.55 V and T= 292 K

PLEASE help.. I have spent hours trying to solve this.please

[Borek]

What is the electrode reaction? How does the reaction quotient look like?

[huskywolf]

What is the electrode reaction? How does the reaction quotient look like?

Hi the initial concentrations were [AgNO₃] 0.01M for solution (a)
and [NH₃] 0.8M for solution (a)

The concentration  of [AgNO₃] 0.01M for solution (b)and [NH₃] 0.4M for solution (b)

Please help calculate the concenrations at Equilibrium

[Borek]

Answer my questions.

[huskywolf]

Answer my questions.

Sorry, I think Q= (Red/Ox)   Q=(0.01)/(0. 8 ) ? = 0.0125 for solution (a)?
Thanks

[Borek]

Geez, is it really that hard to read what I posted? Don't make me ask the same questions again and again - at some point I will simply refuse to help any longer.

What is the electrode reaction?

[huskywolf]

Geez, is it really that hard to read what I posted? Don't make me ask the same questions again and again - at some point I will simply refuse to help any longer.

What is the electrode reaction?

I am sorry my mind is confused over this problem:
   Ag|Ag⁺ NO₃^-||Ag⁺ Cl ^-|Ag

[huskywolf]

Hi I got 2.6 x 10^-4M for [Ag⁺] for solution (a) does this look correct please?

[huskywolf]

thats a great help thanks alot.