Geschichte der analytischen chemie in ungarn

Szabadváry, F.

doi:10.1016/0039-9140(63)80049-1

Cited by 4 publications

(3 citation statements)

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“…Unusually, Georgii applied a reversed titration, by freezing the solutions and removing the ice. 34 For the description of the methodological and historical background, see Szabadvary (1966) and, in particular, Freund (1904).…”

Section: Titrimetrymentioning

confidence: 99%

Acidity: Modes of characterization and quantification

Ruthenberg

Chang

2017

Studies in History and Philosophy of Science Part A

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This paper provides an account of early historical developments in the characterization and quantification of acidity, which may be considered preliminary steps leading to the measurement of acidity. In this "pre-history" of acidity measurement, emphasis is laid on the relative independence of the rich empirical knowledge about acids from theories of acidity. Many attempts were made to compare and assess the strengths of various acids, based on concrete laboratory operations. However, at least until the arrival of the pH measure, the quantification attempts failed to produce anything qualifying as a measurement scale of a recognizable type. It is doubtful whether even pH qualifies as a true measure of acidity, when the full meaning of acidity is taken into account.

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Section: Titrimetrymentioning

confidence: 99%

Acidity: Modes of characterization and quantification

Ruthenberg

Chang

2017

Studies in History and Philosophy of Science Part A

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“…In the first half of the 19 th century "galvanic electricity", or in modern term the electric charge, was regarded as a sensitive reagent by analytical chemists, e.g., by Buchner [4], and was used in qualitative analysis (cf. [5,6]). Subsequently, electrolysis was utilized for analytical separations.…”

Section: Introductionmentioning

confidence: 96%

History of Electroanalytical Methods

Lubert

Kalcher

2010

Electroanalysis

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There are many historical reviews on electrochemistry as well as on analytical chemistry, where-as hardly any survey of the history of electroanalytical methods exists. This contribution is an approach to provide a short overview on the development of the electroanalytical methods, electrodes and electrochemical sensors. Electrogravimetry belongs to the oldest quantitative procedures introduced 1864 by Wolcott Gibbs. Roots are even older and are represented by "voltameters". Closely related to electrogravimetry is coulometry, which is also based on Faradays laws; early applications comprise determinations of atomic masses and of thin metal layers. Conductivity measurements are also a rather old analytical method, applied (with direct current) in the 18 th century already. The effective procedure was developed in the 1860s after the use of alternating current by Friedrich Kohlrausch. The Nernst equation (1889) was the base for direct potentiometry, e.g., determination of sparingly soluble electrolytes. Max Cremer is the inventor of the glass electrode (1906), which is the first electrochemical sensor. Potentiometric indication of titrations by Robert Behrend (1883) was the first instrumental indication in volumetric analysis. The invention of polarography by Jaroslav Heyrovský (1922) is the starting point of the electroanalysis with the dropping mercury electrode. The polarograph, developed in cooperation with Masuro Shikata, was the first automated analytical device. As a follow-up various methods (e.g., pulse and alternating current methods) as well as voltammetry including stripping analysis have gained importance. Further development of electroanalysis is characterized by new electrodes and electrode materials, e.g., stationary mercury electrodes, carbon-paste electrodes, chemically modified electrodes, and increased application of electrochemical sensors.

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“…The principles of titrimetric methods have been developed at the beginning of the 18th century, and interesting historical annotations are given in the literature [7][8][9][10][11]. Already in the middle of the 18th century, indicator papers soaked with litmus have been used for a precise indication of the completion of the reaction between potash and an acid.…”

Section: Introductionmentioning

confidence: 99%

Colour maps of acid–base titrations with colour indicators: how to choose the appropriate indicator and how to estimate the systematic titration errors

2016

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To recognise the end point of acid-base titrations, colour indicators are still frequently used. Colour indicators can cause systematic errors, and the theoretical evaluation of these errors is given in many textbooks. Random errors caused by the transition range of an indicator can also be estimated with the help of pH-logc i diagrams. However, very often, undergraduate students have problems to correctly interpret the colours of the different species of an indicator (its acidic and alkaline forms) and colour changes during titration. Frequent questions are of the type: ''Is it still blue, or is it already red?'' The aim of the present text is to show how carefully a suitable colour indicator has to be chosen, and what colour changes happen at the inflection point of a titration. Typical acid-base titrations like the alkalimetry of hydrochloric acid, sulphuric acid, oxalic acid, and the acidimetry of borax at two concentration levels using eleven common colour indicators are compared with potentiometric end point determination. Photographs were taken of solutions containing the indicators during the course of titration, i.e., at different pH values. These photographs were used to prepare a colour map for each indicator. Such colour maps are very helpful to find the most suitable indicator for a certain reaction, and also to estimate the maximum accuracy.

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Geschichte der analytischen chemie in ungarn

Cited by 4 publications

References 1 publication

Acidity: Modes of characterization and quantification

Acidity: Modes of characterization and quantification

History of Electroanalytical Methods

Colour maps of acid–base titrations with colour indicators: how to choose the appropriate indicator and how to estimate the systematic titration errors

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