User:Douglas M. Fox/Notebook/AU CHEM-571 F2011 Lab Support/2014/10/21: Difference between revisions
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== | ==Tasklist== | ||
* | * Continue Equilibria Studies | ||
* Prepare iodide ion selective electrodes | |||
**Prepare 10 mL 3 M NaCl | |||
***Carefully remove yellow plastic covering on Ag/AgCl electrode (as instructed) | |||
***Place electrode in 15 mL falcon tube with enough NaCl solution to match volume in electrode | |||
***cover and store upright until needed | |||
**Prepare 50 mL 4 M KNO3 | |||
***Add KNO3 to outer double junction cell, filling narrow tube + ~ 0.5 inches further | |||
***Place electrode in small vial with enough KNO3 solution to cover the vycor tip | |||
**Prepare 50 mL 0.01 M KI + 0.1 M KNO3 | |||
***Cut a short piece (~ 3 in) of silver wire | |||
***Place in KI/KNO3 solution | |||
***Electrolyze the solution using the power supply | |||
***The standard reduction potential for Ag/AgI is -0.15 V | |||
***Oxidation occurs at the anode, which is connected to the red lead | |||
***Electrolyze at low power (low current) until the wire appears coated | |||
**Test your electrodes with a range of KI solutions | |||
***The Ag/AgCl electrode slides inside of the KNO3 bridge solution (this is a double junction electrode) | |||
***The Ag/AgI wire can be connected directly to a multimeter using alligator clips | |||
***You will continue to connect your Ag wire to the red lead on the multimeter | |||
Revision as of 08:30, 21 October 2014
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Tasklist
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