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Ch.14-16 Electrochemistry Redox Reaction - the basics ox1 + red2 <=> red1 + ox2 Oxidizing Reducing Agent Agent Redox reactions: involve transfer of electrons from one species to another. Oxidizing agent (oxidant): takes electrons Reducing agent (reductant): gives electrons Redox Reaction - the basics Reduced Oxidized ox1 + red2 <=> red1 + ox2 Oxidizing Reducing Agent Agent Redox reactions: involve transfer of electrons from one species to another. Oxidizing agent (oxidant): takes electrons Reducing agent (reductant): gives electrons Fe3+ +V2+→Fe2++V3+ Balance Redox Reactions (Half Reactions) 1. Write down the (two half) reactions. 2. Balance the (half) reactions (Mass and Charge): a. Start with elements other than H and O. b. Balance O by adding water. c. balance H by adding H+. d. Balancing charge by adding electrons. (3. Multiply each half reaction to make the number of electrons equal. 4. Add the reactions and simplify.) Example: Balance the two half reactions and redox reaction equation of the titration of an acidic solution of Na2C2O4 (sodium oxalate, colorless) with KMnO4 (deep purple). MnO4-(aq) + C2O42-(aq) → Mn2+ (aq) + CO2(g) 16H+(aq) + 2MnO4-(aq) + 5C2O42-(aq) → 2Mn2+(aq) + 8H2O(l) + 10CO2(g) Example: Balance Sn2+ + Fe3+ <=> Sn4+ + Fe2+ Fe2+ + MnO4- <=> Fe3+ + Mn2+ Important Redox Titrants and the Reactions Oxidizing Reagents (Oxidants) (1) Potassium Permanganate MnO − +8H+ +5e− →Mn2+ +4H O 42 MnO − + 4H + + 3e− → MnO (s) + 2H O 422 MnO− +e− →MnO2− 44 1PDF Image | Electrochemistry Chapter 14 to 16
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