I am trying to find the Ksp of silver thiocyanate: AgSCN(s) --> Ag+ (aq)SCN-(aq)
but I need to first prove that the lower [Ag+] = 1.27-12 M, but don't know how to find it.
The data I am given: Volume of 10-4 M Ag+ solution used: 10.00ml
Volume of 1.0 M KSCN added: 50.00ml
Measured cell potential when an Ag(s) electrode was placed into the above mixture, and then joined to the Ag+(0.1M)/Ag(s) half cell: 0.645V
Results: Calculated lower [Ag+] from cell potential: 1.27-12 M
I am suppose to use this equation for the concentration cell:
where n is the number of electrons.
So really my question is how I would go about finding the higher concentration of Ag+ and then use that to determine that lower [Ag+] = 1.27-12M