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# Basic Principle of Potentiometry Potentiometry is an important electroanalytical method used for the qualitative and quantitative determination of ions and other chemical species in a solution. The basic principle of potentiometry is the measurement of the potential difference, or electromotive force (EMF), between two electrodes immersed in a solution, under conditions where essentially no current flows through the electrochemical cell. The measured potential is related to the activity or concentration of the ion being determined. Thus, potentiometry provides a convenient method for determining the concentration of a particular ionic species by measuring electrical potential rather than measuring the amount of current. A potentiometric cell generally consists of two electrodes: an indicator electrode and a reference electrode. The indicator electrode responds selectively to the activity of the ion of interest, whereas the reference electrode has a stable and known potential that remains practically constant during the measurement. Common reference electrodes include the saturated calomel electrode and the silver/silver chloride electrode. Indicator electrodes may be metallic electrodes, such as platinum or silver electrodes, or ion-selective electrodes such as the glass electrode used for pH measurement. When the two electrodes are connected to a high-resistance voltmeter or __________ _______ _____ ________ ___ _________ _________ ____ _________ ________ ______.
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