Reversible and Irreversible Adsorption of Surfactants at a Hanging Mercury Drop Electrode

Sawamoto, Hiromiti

doi:10.2116/analsci.19.1381

Cited by 11 publications

(3 citation statements)

References 36 publications

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“…These electrons are provided through reactions at the electrodes. Among the chemical reaction which can occur at low potentials with platinum electrodes, we might have: Reversible adsorption of tetraalkylammonium ions has also been previously observed at hanging mercury drop electrodes, 21 gold electrodes 22 and CO-coated platinum electrodes. 23 The image charge induced in platinum by a positive tetraalkylammonium ion sticking to the surface could also participate to electron transport in the external circuit.…”

Section: B Variations Of the Seebeck Coefficient With Salt Concentrationmentioning

confidence: 91%

Huge Seebeck coefficients in nonaqueous electrolytes

Bonetti

Nakamae

Roger

et al. 2011

The Journal of Chemical Physics

217

186

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The Seebeck coefficients of the non-aqueous electrolytes tetrabutylammonium nitrate, tetraoctylphosphonium bromide and tetradodecylammonium nitrate in 1-octanol, 1-dodecanol and ethylene-glycol are measured in a temperature range from T =30 to T = 45 • C. The Seebeck coefficient is generally of the order of a few hundreds of microvolts per Kelvin for aqueous solution of inorganic ions. Here we report huge values of 7 mV/K at 0.1M concentration for tetrabutylammonium nitrate in 1-dodecanol. These striking results open the question of unexpectedly large kosmotrope or "structure making effects" of tetraalkylammonium ions on the structure of alcohols.

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Section: B Variations Of the Seebeck Coefficient With Salt Concentrationmentioning

confidence: 91%

Huge Seebeck coefficients in nonaqueous electrolytes

Bonetti

Nakamae

Roger

et al. 2011

The Journal of Chemical Physics

217

186

View full text Add to dashboard Cite

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“…8a) signifies the adsorption of the surfactant on the mercury surface. The increase in the differential capacity is connected with the desorption of molecules from the electrode, which may indicate the reversibility of the adsorption process [36,37]. The slight increase in capacity, indicating a partial desorption of EHS, is observed in the potential range from −0.46 to −0.86 V vs. SCE.…”

Section: Adsorption Of Ehs On Mercury Electrodementioning

confidence: 90%

Electrochemical Reactions of Sodium 2-Ethylhexyl Sulfate Salt

2017

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The electrochemical reactions of sodium 2-ethylhexyl sulfate (EHS) and its effect on the Zn 2+ electroreduction have been investigated at a mercury electrode using cyclic voltammetry. It has been shown that the reduction takes place in two steps. The presence of EHS in the solution containing Zn 2+ ions moves slightly the potential of zinc reduction towards more negative potentials and causes a slight increase in current density. The differential capacity-potential and differential capacity-time measurements indicate strong adsorption in a wide potential range on the electrode surface. In the potential range −0.46 to −0.86 V vs. saturated calomel electrode and at the concentration lower than the critical micelle concentration (CMC), adsorption for the longer time is hardly reversible. At the concentration higher than the CMC, the formation of hemispherical surface micelles is observed. The theoretical maximum degree of electrode coverage computed with the use of quantum-chemical calculations is equal to 3.53 × 10 14 particles cm, and it is larger than the value determined experimentally from cyclic voltammograms. In the case of electrochemical reaction, at a current of 0.3 A, during 180 min, the obtained mineralization of EHS is only 3%.

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“…It has a great tendency to adsorb onto surfaces, e.g. [15][16][17][18][19], influencing mass and energy transfer across the modified interface. With respect to ASV measurements, Triton adsorption, besides reducing the available electrode surface area, can also lead to broader peaks and shifts in peak potential, as in [20].…”

Section: Introductionmentioning

confidence: 99%