Iodometry

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iodometry

[‚ī·ə′däm·ə·trē]
(analytical chemistry)
An application of iodine chemistry to oxidation-reduction titrations for the quantitative analysis in certain chemical compounds, in which iodine is used as a reductant and the iodine freed in the associated reaction is titrated, usually in neutral or slightly acid mediums with a standard solution of a reductant such as sodium thiosulfate or sodium arsenite; examples of chemicals analyzed are copper(III), gold(VI), arsenic(V), antimony(V), chlorine, and bromine.
McGraw-Hill Dictionary of Scientific & Technical Terms, 6E, Copyright © 2003 by The McGraw-Hill Companies, Inc.
The following article is from The Great Soviet Encyclopedia (1979). It might be outdated or ideologically biased.

Iodometry

 

a method used in the titrimetric analysis of substances exhibiting oxidizing or reducing properties based on the reversible reaction I2 + 2e ⇆ 2I. The I2/2I system, with a normal potential equal to +0.5345 V (25°C), is used for the determination of reducing agents with a potential lower than +0.5345 V (for example, stannous salts, hydrogen sulfide) and oxidizing agents with a potential greater than +0.5345 V (for example, peroxides, chromic and permanganic acids, cupric salts, and ferric salts). Solutions of iodine and sodium thiosulfate are used as standard solutions during titration, and starch serves as the indicator.

REFERENCE

Kreshkov, A. P. Osnovy analiticheskoi khimii, 3rd ed., part 2. Moscow, 1971.
The Great Soviet Encyclopedia, 3rd Edition (1970-1979). © 2010 The Gale Group, Inc. All rights reserved.
References in periodicals archive ?
The progress of the reactions was monitored by periodically examining aliquots of the reaction mixture for unconsumed NCSA iodometrically using starch as the indicator.
Solutions of perborate were prepared freshly and standardized iodometrically. Kinetics of the oxidation in aqueous sulphuric acid at constant temperature was studied iodometrically under pseudo-first order conditions with a very large excess of 5-oxoacids.
The solutions used were standardized iodometrically. Demineralized distilled water was used for preparing the solution of hypo and others.
In preparation of the required concentration a dilution factor was employed and its concentration was checked iodometrically. A solution of Mn[Cl.sub.2] (Uchem limited) was prepared by dissolving the sample in known strength of very dilute hydrochloric acid (0.001 M).