We've already known that Fe+ + e Fe+, E-0.77v (1) Fe(OH)2 Fe+ + 2OH,...

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We've already known that Fe³+ + e Fe²+, Eº-0.77v (1) → Fe(OH)2 → Fe²+ + 2OH, Ksp1-6.0×10-¹5 (2) -> Fe(OH)3 Fe³+ + 3OH, Ksp2=2.0X10-38 (3) Please calculate the pEº for Fe(OH)3 + e Fe(OH)2(s) + OH- → We've already known that Fe³+ + e Fe²+, Eº-0.77v (1) → Fe(OH)2 → Fe²+ + 2OH, Ksp1-6.0×10-¹5 (2) -> Fe(OH)3 Fe³+ + 3OH, Ksp2=2.0X10-38 (3) Please calculate the pEº for Fe(OH)3 + e Fe(OH)2(s) + OH- →

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Solution To calculate the pE for the given redox reaction we need to write the balanced halfreactions and their respective standard reduction potentials E Then we can calculate the overall standard cell potential Ecell and use the Nernst equation to find the cell potential Ecell at the given conditions Finally we can use the relation pE logEcell to find the pE The oxidation halfreaction ... View the full answer