An Ion-Selective Electrode (ISE) produces a potential that is proportional to the concentration of an analyte. Making measurements with an ISE is therefore a form of potentiometry. The most common ISE is the pH electrode, which contains a thin glass membrane that responds to the H+ concentration in a solution.
The potential difference across an ion-sensitive membrane is:
E = K - (2.303RT/nF)log(a)
where K is a constant to account for all other potentials, R is the gas constant, T is temperature, n is the number of electrons transferred, F is Faraday's constant, and a is the activity of the analyte ion. A plot of measured potential versus log(a) will therefore give a straight line.
ISEs are susceptible to several interferences. Samples and standards are therefore diluted 1:1 with total ionic strength adjuster and buffer (TISAB). The TISAB consists of 1 M NaCl to adjust the ionic strength, acetic acid/acetate buffer to control pH, and a metal complexing agent.
ISEs consist of the ion-selective membrane, an internal reference electrode, an external reference electrode, and a voltmeter. A typical meter is shown in the document on the pH meter.
Schematic of an ISE measurement
Commercial ISEs often combine the two electrodes into one unit that are then attached to a pH meter.
Picture of a commercial fluoride ISE
/chem-ed/echem/ise.htm, updated 2/12/97
Copyright © 1997 by Brian M. Tissue, all rights reserved.
Science Hypermedia Home Page