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The aim of this booklet is to explore titration from a historical, theoretical and practical point of view, dealing first with preset end-point titration then with inflection-point titration. We look at common applications and give useful advice on how to choose between techniques and get the best results.
Titration, also known as titrimetry, is a common laboratory method of quantitative chemical analysis that is used to determine the unknown concentration of an identified analyze. Since volume measurements play a key role in titration, it is also known as volumetric analysis.
Titration. A procedure in which one substance (titrant) is carefully added to another (analyte) until complete reaction has occurred. The quantity of titrant required for complete reaction tells how much analyte is present.
In titrimetry we add a reagent, called the titrant, to a solution containing another reagent, called the titrand, and allow them to react. In acid–base titrations, an acidic or basic titrant reacts with a titrand that is a base or an acid Complexometric titrations: metal–ligand complexation
titrant is an oxidizing or reducing agent; and precipitation titrations, in which the titrand and titrant form a precipitate. Despite the difference in chemistry, all titrations share several com-
Thus, an acid-base indicator is itself an acid or base which exhibits a visual change on neutralization by the basic or acidic titrant at or near the equivalence point. Similar terms apply to complexometry (metallochromic indicator), oxidation-reduction, and precipitation titrimetry.
1.1 Introduction to Titration. A titration is a quantitative, volumetric procedure used in analytical chemistry to determine the concentration of an analyte (the species being measured) in solution. The concentration of the analyte is determined by slowly adding a titrant (reagent) to the solution.
