How Does Electrochemistry Calculate the Solubility of AgI?

AI Thread Summary
The discussion revolves around calculating the solubility of AgI using electrochemistry and the Nernst equation. The standard potential of the cell is given as +0.9509 V, and the user is attempting to find the natural log of the solubility (ln s) for AgI. There is confusion regarding the correct value for the standard reduction potential of AgI, which is noted to be -0.15 V. The user mistakenly calculates a value of -18.51, which is identified as a decimal log rather than the natural log. Clarification on the correct logarithmic calculations is needed to resolve the issue.
koomanchoo
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hey i seem to be having a lot of trouble qith this question may i get some help?
The standard potential of the cell below is + 0.9509 V at 25 oC. Calculate the solubility, normally called s, of AgI (Note: Enter the natural log of s (ln s) as your answer)

Ag|AgI(s)|AgI(aq)|Ag

i'm using nernst equation and found the standard potential for Ag+,Ag to be 0.7991V

i am using Eo as 0.7991 and E as 0.9509 and rearanging the equation to find the solubility as LnS.. the correct answer is suppose to be -18.51.. where i am going wrong? please help.
thanks

n.b standard reduction potential of AgI(s) is -.15V
 
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IIRC -18.51 is not a natural log of the AgI solubility product - it's decimal log.
 
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