Analytical Electrochemistry : Potentiometry
{"Image DocumentName": "Analytical Electrochemistry : Potentiometry", "Image ImageDescription": "Introduction. Goals and Objectives. Potentiometry Timeline. Potentiometric Theory. Instrumentation. pH Electrodes. Experiments. Common Troubleshooting Tips. References. Introduction. This module provides an introduction to the measurement technique of potentiometry. It is intended to be a primary learning tool for a student in a Quantitative Analysis or Analytical Chemistry course and as a review resource for a student in Instrumental Analysis. It could also serve as a beginning resource for new practitioners. If you have ever used a pH meter, then you have already performed potentiometry, an electrochemical method in which the potential of an electrochemical cell is measured while little to no current is passed through the sample. In a potentiometric measurement, an indicator electrode responds to changes in the activity, or effective concentration of the analyte. A potential, or voltage, that develops at the interface between the electrode and the analyte solution is measured relative to a reference electrode. This potential will be proportional to the amount of analyte in the sample. An illustration of one type of indicator electrode, the hydrogen ion or pH electrode, is shown in the upper right-hand corner of this page. Click here to continue reading the introduction. Erin M. Gross1, Richard S. Kelly2, and Donald M. Cannon, Jr.3. 1Department of Chemistry, Creighton University, Omaha, NE. 2Department of Chemistry, East Stroudsburg University, East Stroudsburg, PA. 3Department of Chemistry, University of Iowa, Iowa City, IA. This work is licensed under a. Creative Commons Attribution-Noncommercial-Share Alike 2.5 License. 1.", "Image XResolution": "37", "Image YResolution": "37", "Image ResolutionUnit": "Pixels/Centimeter", "Image Software": "SlidePlayer", "Image YCbCrPositioning": "Centered"}