**Concentration cell **→ anode and cathode are the** same **→

**Modified Nernst equation**:

$\overline{){{\mathbf{E}}}_{{\mathbf{cell}}}{\mathbf{=}}{\mathbf{E}}{{\mathbf{\xb0}}}_{{\mathbf{cell}}}{\mathbf{-}}\mathbf{\left(}\frac{\mathbf{0}\mathbf{.}\mathbf{0592}}{\mathbf{n}}\mathbf{\right)}{\mathbf{log}}\frac{\left[\mathrm{anode}\right]}{\left[\mathrm{cathode}\right]}}$

**anode**→ lower concentration**cathode**→ higher concentration

Consider the concentration cell shown below. Calculate the cell potential at 25°C when the concentration of Ag^{+} in the compartment on the right is the following.

c. 0.10 M

For each case, also identify the cathode, the anode, and the direction in which electrons flow.

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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.