Polarographic Characteristics of Metallic Cations in Acetate Media

DeSesa, M. A.; Hume, David N.; Glamm, Arthur C.; DeFord, D. D.

doi:10.1021/ac60078a043

Cited by 29 publications

(3 citation statements)

References 3 publications

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“…Electron changes were calculated by accepted procedures described in the literature (4, 7) and the results are given in Table I. The 3-electron change for antimony is believed to be from Sb+3 to the amalgam, which agrees with the work of Desesa (8) and Lingane (9). The electron change for indium shows the reaction to be In+3 to In0.…”

Section: Resultssupporting

confidence: 64%

Simultaneous polarographic determination of indium and antimony

Frank¹,

Meloan²

1967

Anal. Chem.

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Polarographic investigationson indium and antimony singly have been very extensive. However, no procedure exists for the determination of these elements simultaneously, and combinations of the individual procedure were found not to work. Because In and Sb occur together in several types of semiconductors, a definite need for an analysis scheme exists.It is generally recognized that antimony can undergo two different reactions: Sb+i to Sb+S, with a half-wave potential at about zero vs. SCE (j); and Sb+3 to Sb°with a half-wave

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Section: Resultssupporting

confidence: 64%

Simultaneous polarographic determination of indium and antimony

Frank¹,

Meloan²

1967

Anal. Chem.

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“…With most of the metal driers the reaction at the dropping mercury electrode is thought to be associated with the reduction of the metal complex to the metallic state (2).…”

Section: Discussionmentioning

confidence: 99%

Polarographic Determination of Metal Driers in a Nonaqueous Solution

Kuta¹

1960

Anal. Chem.

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ure 1 is a polarogram of a solution containing 3.76 X 10~4M arsenic as arsenite ions, whereas curve B is a polarogram of the same solution but without arsenic. The increase in current of the solution containing the arsenite ions occurred earlier along the voltage axis than the solution containing no arsenite. This difference may indicate that the arsenite ions wrere reduced in this medium but that the polarographic wave was not formed because of the early reduction of the sodium ions present in the supporting electrolyte. This theory agrees with the work of Bayerle (2), who reported polarographic activity for arsenite ions in a sodium hydroxide solution.In the case of the lithium chloridelithium hydroxide electrolyte the lithium ions were not reduced until a potential of -2.1 volts had been reached as shown by curve C. This additional range permits full development of the arsenite wave.Logarithmic analysis of the polarographic curve indicated that it was irreversible. The same analysis indi-VOLTS (-]

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“…The molybdosilicic acid complex present in an acetic acid-sodium acetate buffer of pH 3.5 produced a single, double, and triple wave with increasing concentration and gave half-wave potentials in the neighborhood of -0.2, -0.5, and -0.55 volt vs. saturated calomel electrode. These studies were not directty applicable to analytical determinations because the polarograms were made on solutions prepared by dissolving the solid heteropoly acid directly in the supporting electrolyte, whereas in an analytical procedure the heteropoly acid would be formed in solution using excess molybdate which is reducible in an acetate buffer (8). The study by Strickland (20), comparing the polarographic behavior of the a and 0 forms of molybdosilicic acid in 0.1V potassium sulfate at a pH of approxi-mately 3.5, was encouraging.…”

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confidence: 99%