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隆, 垣内

doi:10.5796/electrochemistry.81.932

Cited by 3 publications

(3 citation statements)

References 6 publications

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“…In the first place, an electrochemical cell is not a thermodynamic device [13]. The cell is realized by splitting a redox reaction between the two redox couples, Ox 1 /Rd 1 and Ox 2 /Rd 2 ,…”

Section: Secret Of the Nernst Equationmentioning

confidence: 99%

“…The main difficulty in measuring pH of these samples is ascribed to the nonnegligible liquid junction potential or its unstable variation with time. The use of a moderately hydrophobic ionic liquid 13 for a salt bridge brings about several advantages [18,19] 14 over KCl-based salt bridge. The most notable feature is that the liquid junction potential between the ionic liquid salt bridge and an aqueous solution is maintained constant even when the ionic strength of a sample solution is very low.…”

Section: Kcl-salt Bridge and Ionic Liquid Salt Bridgementioning

confidence: 99%

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Obscurity in Electroanalytical Chemistry

Kakiuchi

2015

Review of Polarography

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The criticism to the concept and use of single ion activity raised by de Levie (2010) has been examined. The lack of falsifiability in the concept of single ion activity, which he claims, led him to categorize the single ion activity as one of non-falsifiables, typified by the emperor's new clothes (2012). However, his criticism is overeager, because the single ion activity can be estimated with a reasonable certainty, whose degree varies with a nonthermodynamic assumption employed, though. Electrochemistry is intrinsically nonthermodynamic, although in many of electrochemistry textbooks its cell voltage is correlated with the Gibbs energy of a redox reaction that would proceed in a homogeneous solution between the two redox couples, which are employed in the electrochemical cell. Ironically, such oversimplified understanding or picture of the nature of electrochemical cells partly justifies the criticism raised by de Levie. The obscurity associated with nonthermodynamic nature of electrochemical cells translates to the obscure interpretation of the Nernst equation in the form, E = E 0 + (RT/F)ln(a Ox /a Rd), which has long been applied to a working electrode in electroanalytical chemistry. By focusing on this obscurity, it is possible not only to make our understanding of electroanalytical chemistry clearer but to design an electrochemical cell for less obscure, more reliable estimation of single ion activities.

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Section: Secret Of the Nernst Equationmentioning

confidence: 99%

Section: Kcl-salt Bridge and Ionic Liquid Salt Bridgementioning

confidence: 99%

Obscurity in Electroanalytical Chemistry

Kakiuchi

2015

Review of Polarography

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“…Electrode potential is the most salient and puzzling concept in electrochemistry. [1][2][3][4][5][6][7][8][9][10] Although electric potentials in physics certainly underlie the concept of the electrode potential, the thermodynamic connection of the electrode potential to Gibbs energy represents the direction and scale of a redox reaction. A basic understanding of the electrode potential is necessary for constructing an appropriate electrochemical system and extending it to different applications.…”

Section: Introductionmentioning

confidence: 99%

Electrode Potentials Part 1: Fundamentals and Aqueous Systems

et al. 2022

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Electrochemistry deals with the interrelationship between electrical and chemical energy. Various potentials appear in electrochemistry and pertain to one another in practical cells. Understanding the electrode potential is an important step in acquiring basic knowledge of electrochemistry and extending it to specific applications. This comprehensive paper outlines the fundamentals and related subjects of electrode potentials, including electrochemical cells and liquid junction potentials. Aqueous solution systems are ideal for connecting the theoretical background of electrode potentials to practical electrochemical measurements. Accordingly, the basic electrode chemistry in aqueous systems is described in this paper, as well as several advanced concepts introduced in recent studies.

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Obscurity in Electroanalytical Chemistry

Kakiuchi¹

2014

Rev. Polarogr.

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Cited by 3 publications

References 6 publications

Obscurity in Electroanalytical Chemistry

Obscurity in Electroanalytical Chemistry

Electrode Potentials Part 1: Fundamentals and Aqueous Systems

Obscurity in Electroanalytical Chemistry

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