Chemistry Asked on January 2, 2022
Reference electrodes such as the saturated calomel electrode and silver chloride electrode have a constant potential because the $ce{Cl-}$ concentration (or, to be more precise, the activity) is constant.
The semi-reaction for those electrodes are:
$$ce{Hg2Cl2 + 2e- <=> 2Hg + 2Cl-}$$
$$ce{AgCl + e- <=> Ag + Cl-}$$
Now, since chloride ions are produced (or consumed, when the electrode is an anode) from the half-reactions, how is it possible that their concentration remains constant?
Is the quantity of chloride produced or consumed is negligible compared to that coming from the $ce{KCl}$ dissociation?
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