CHEM10006 Lecture Notes - Lecture 31: Covalent Bond, Lone Pair, Nernst Equation

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The ne(cid:396)(cid:374)st e(cid:395)uatio(cid:374) allows us to calculate the pote(cid:374)tial at i(cid:374)te(cid:396)(cid:373)ediate ph"s. Standard reduction potentials depend on ph, and are based on unit concentrations. As ph = - log[h+], ecell = eo - 0. 0591 ph, which will graph to a straight line. Plot of e vs ph for the reduction of o2 and h2o. The stability field of water is the range of values of potential and ph for which water is thermodynamically stable towards both oxidation and reduction. Species with a potential more positive than the top line will release o2 from water. Species with a potential more negative than the bottom line will release h2 from water. Lines mark places where two species exist in equilibrium. Pure redox reactions are horizontal lines - these reactions are not ph-dependent. Pure acid-base reactions are vertical lines - these do not depend on potential. Reactions that are both acid-base and redox have a slope of -0. 0592 v/ph.

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