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Unformatted text preview: ions into iodine: 2. 3. 4. 5. Now that we know that iodate is reduced, the other half-reaction must be the oxidation of hydrogen: 6. If we multiply the second half-reaction by five and add this to the first half-reaction, 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...
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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