**Concentration cell →*** same electrodes, different concentrations*

**E****°**_{cell }= 0 →*same electrodes*

Recall that a **cell notation** is written from** anode (oxidation) to cathode (reduction)**:

lose electrons → oxidation → anode

gain electrons → reduction → cathode

Anode cathode

Zn(s)|Zn^{2+}(aq,0.100 M)|| Zn^{2+} (**aq, ? M**)|Zn(s)

**Oxidation: Zn**_{(s)}**→****Zn**+^{2+}_{(aq)}**2e**^{-}**Reduction: Zn**+^{2+}_{(aq)}**2e**^{- }**→****Zn**_{(s)}**n = 2e**^{-}

**Modified Nernst Equation:**

$\overline{){{\mathbf{E}}}_{{\mathbf{cell}}}{\mathbf{=}}{\mathbf{-}}\mathbf{\left(}\frac{\mathbf{0}\mathbf{.}\mathbf{0592}\mathbf{}\mathbf{V}}{\mathbf{n}}\mathbf{\right)}{\mathbf{log}}\frac{{\left[{\mathrm{Zn}}^{2+}\right]}_{\mathrm{anode}}}{{\left[{\mathrm{Zn}}^{2+}\right]}_{\mathrm{cathode}}}}$

The voltage generated by the zinc concentration cell described by.

Zn(s)|Zn^{2+}(aq,0.100 M)|| Zn^{2+} (aq,? M)|Zn(s)

is 13.0 mV at 25 °C. Calculate the concentration of the Zn^{2+}(aq) ion at the cathode.

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