Question

what are the advandages of potentiometric titration
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Answer 1

Answer:

This kind of titration is far more accurate and precise than manual titration, with high accuracy up to three digits in milliliters. A number of kinds of potentiometric titrations exist, providing options depending on the need for determining analytes.

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Answer 2

Explanation:

Potentiometric titrations involves the measurement of the potential of a suitable indicator electrode with respect to a reference electrode as a function of titrant volume. Potentiometric titrations provide more reliable data than data from titrations that use chemical indicators and are particularly useful with colored or turbid solutions and for detecting the presence of unsuspected species. Titration involves measuring and recording the cell potential (in units of millivolts or pH) after each addition of titrant. The titrant is added in large increments at the outset and in smaller and smaller increments as the end point is approached ( as indicated by larger changes in response per unit volume). Sufficient time must be allowed for the attainment of equilibrium after each addition of the reagent by continuous stirring. For this a magnetic stirrer with a stirring magnet bar is used.

A typical set up for potentiometric titrations is :

Potentiometric titrations can be classified as precipitation titrations, complex formation titrations, neutralization titrations and oxidation/reduction titrations.

Modern pH electrodes are usually of the "combination" type, meaning that a single cylinder contains both a glass membrane electrode and the outer-reference calomel electrode:

General Principle

A typical cell for potentiometric analysis consists of a reference electrode, an indicator electrode and a salt bridge. This cell can be represented as

A reference electrode, Eref, is a half-cell having a known potential that remains constant at constant temperature and independent of the composition of the analyte solution. The reference electrode is always treated as the left-hand electrode in potentiometric measurements. Calomel electrodes and silver/silver chloride electrodes are types of reference electrodes.

An indicator electrode has a potential that varies with variations in the concentration of an analyte. Most indicator electrodes used in potentiometry are selective in their responses. Metallic indicator electrode and membrane electrodes are types of indicator electrodes.

The third component of a potentiometric cell is a salt bridge that prevents the components of the analyte solution from mixing with those reference electrode. A potential develops across the liquid junctions at each end of the salt bridge. The junctions potential across the salt bridge, Ej, is small enough to be neglected.

The potential of the cell is given by the equation:

Ecell= Eind – Eref + Ej

Advantages:

There are a number of advantages of potentiometric titrations over the ordinary titrations involving the use of indicators. Potentiometric titration can be carried out in coloured solutions while indicators cannot be used in such cases. Also, in ordinary titrations, one must have prior information about the relative strengths of acids and bases before a proper indicator is selected. However no such information is required in the case of potentiometric titrations.