This preview shows pages 1–3. Sign up to view the full content.
This preview has intentionally blurred sections. Sign up to view the full version.
View Full Document
Unformatted text preview: ions into iodine: 2. 3. 4. 5. Now that we know that iodate is reduced, the other halfreaction must be the oxidation of hydrogen: 6. If we multiply the second halfreaction by five and add this to the first halfreaction, we get or, after simplification, 2. We need the activities of all the reactants and products. The activity of iodine is . We started out with 0.04mol/L of iodate ions but each iodine formed requires the reaction of two iodate ions so . The initial pH is 4 so we started out with . Again, we need two hydrogen ions per iodine so at the time of measurement, . The activity of hydrogen gas is 1. Therefore, by rearrangement of the Nernst equation, Referring back to the balancing process, we see that . Therefore Marc Roussel Wed Dec 11 12:34:02 MST 1996...
View
Full
Document
This note was uploaded on 03/03/2012 for the course CHEM 2000 taught by Professor Roussel during the Fall '06 term at Lethbridge College.
 Fall '06
 Roussel
 Electrochemistry

Click to edit the document details