Stuck with a problem in electrochemistry

AI Thread Summary
The discussion revolves around calculating the cell potential (Ecell) for a galvanic cell with silver electrodes in saturated solutions of AgBr and Ag2CrO4. Participants clarify the process of determining the concentration of Ag+ ions from the given solubility product constants (Ksp) and how to apply the Nernst equation. There is confusion about the correct substitution in the logarithm and whether to use a standard electrode potential (E0) of zero. It is noted that E0 cancels out in the calculation, but the standard value for the Ag(s)/Ag+ system should be used for accuracy. The original poster expresses progress in understanding the problem after receiving guidance.
johncena
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Homework Statement


A galvanic cell consisting of two silver electrodes,one in a saturated solution of AgBr and the other in a saturated solution of Ag2CrO4 is prepared.Calculate the value of Ecell at 298K Given Ksp(AgBr) = 5x10-13 M2 and
Ksp(Ag2CrO4)=2.4x10-12M3


Homework Equations


to find conc from Ksp
and
Nernst equation
77fd93e90bedd188d9d0c0b65cfa49a5.png


The Attempt at a Solution



I got the conc of Ag+ in both the solutions ... but i don't know how to substitute them...(means ...i don't know which comes in the numerator of the logarithm)
and Is the value of E0 to be taken as 0? How ?

pls help...

thanks in advance:smile:
 
Physics news on Phys.org
Report the potential as positive. E0 cancels out, but technically you should use value for the Ag(s)/Ag+ system.
 
thank you sir...

i am getting it now...:smile:
 

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