**The Nernst Equation****:**

**$\overline{){{\mathbf{E}}}_{{\mathbf{cell}}}{\mathbf{=}}{\mathbf{E}}{{\mathbf{\xb0}}}_{{\mathbf{cell}}}{\mathbf{-}}\mathbf{\left(}\frac{\mathbf{0}\mathbf{.}\mathbf{05916}\mathbf{}\mathbf{V}}{\mathbf{n}}\mathbf{\right)}{\mathbf{logQ}}}$**

E_{cell} = cell potential under non-standard conditions

E°_{cell} = standard cell potential

n = number of e^{-} transferred

Q= reaction quotient = [products]/[reactants]

You have a concentration cell in which the cathode has a silver electrode with 0.10 M Ag^{+}. The anode also has a silver electrode with Ag ^{+}(aq), 0.050 M S _{2}O_{3} ^{2-}, and 1.0 X 10 ^{-3} M Ag(S_{2}O_{3})_{2} ^{3-}. You read the voltage to be 0.76 V.

a. Calculate the concentration of Ag ^{+} at the anode.

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Based on our data, we think this problem is relevant for Professor Hammerich's class at UIC.

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Our data indicates that this problem or a close variation was asked in Chemistry: An Atoms First Approach - Zumdahl Atoms 1st 2nd Edition. You can also practice Chemistry: An Atoms First Approach - Zumdahl Atoms 1st 2nd Edition practice problems.