Appendix

AppendicesAppendix 13: Standard Reduction PotentialsThe following table provides E o and E o´ values for selected reduction reactions. Values are from the followingsources: Bard, A. J.; Parsons, B.; Jordon, J., eds. Standard Potentials in Aqueous Solutions, Dekker: New York,1985; Milazzo, G.; Caroli, S.; Sharma, V. K. Tables of Standard Electrode Potentials, Wiley: London, 1978; Swift,E. H.; Butler, E. A. Quantitative Measurements and Chemical Equilibria, Freeman: New York, 1972.Solids, gases, and liquids are identified; all other species are aqueous. Reduction reactions in acidic solution arewritten using H + in place of H 3 O + . You may rewrite a reaction by replacing H + with H 3 O + and adding to theopposite side of the reaction one molecule of H 2 O per H + ; thusbecomesH 3 AsO 4 + 2H + + 2e – HAsO 2 + 2H 2 OH 3 AsO 4 + 2H 3 O + + 2e – HAsO 2 + 4H 2 OConditions for formal potentials (E o´) are listed next to the potential.Aluminum E° (V) E°’(V)Al+ 3e Al() s–1.6763+ −Al(OH) − 4+ 3e− Al() s + 4OH−–2.3103AlF − + 3e− Al() s + 6F−–2.0761107Antimony E° (V) E°’(V)Sb + 3H + + 3e− SbH3( g ) –0.510Sb2O5() s + 6H + 4e 2SbO + 3H2O()l0.605+ + −SbO + 2H + 3e Sb() s + HO() l0.2122Arsenic E° (V) E°’(V)As + 3H + + 3e− AsH3( g ) –0.225+HAsO + 2H + 2e− HAsO + 2H O() l0.5603 4 2 2+HAsO 2+ 3H + 3e − As() s + 2H 2O() l0.240Barium E° (V) E°’(V)Ba+ 2e Ba() s–2.922+ −BaO() s + 2H + + 2e− Ba() s + HO()l2.3652