Transcription of Lecture 10 - Redox Titrations
{{id}} {{{paragraph}}}
Example: stock market
Lecture 10 - Redox Titrations
Redox Titrations -the oxidation/reduction reaction between analyte and titrant -titrants are commonly oxidizing agents, although reducing titrants can be used -the equivalence point is based upon: Aox + Bred ! Ared + Box Rx n goes to completion after each addition of titrant Potentiometric Titration: Titration reaction: Ce4+ + Fe2+ ! Ce3+ + Fe3+ (1) Reference half-reaction: 2Hg(l) + 2Cl- ! Hg2Cl2(s) + 2e- At the Pt indicator electrode (Indicator half-reaction) Fe3 + e- !Fe2+ E0 = V (2) Ce4+ + e- !Ce3+ E0 = (3) Cell reactions (in 1 M HClO4): 2Fe3+ + 2Hg(l) + 2Cl- !2Fe2+ + Hg2Cl2(s) (4) 2Ce4+ + 2Hg(l) + 2Cl- ! 2Ce3+ + Hg2Cl2(s) (5) Relationships - Cell reactions are not the same as the titration reaction - May describe the cell voltage with either (4) or (5) or both Balancing Redox Reactions Balance: -atoms -# of electrons transferred Example: Cr(s) + Ag+ !
Redox Titrations -the oxidation/reduction reaction between analyte and titrant -titrants are commonly oxidizing agents, although reducing titrants can be used -the equivalence point is based upon: A ox + B red! A red + B ox Rx’n goes to completion after each addition of titrant – Potentiometric Titration: Titration reaction: Ce4+ + Fe2 ...
Loading..
Tags:
Information
Domain:
Source:
Link to this page:
Please notify us if you found a problem with this document: