Effect of Chloride lorn Coeceetratioe on the Anodic Dissolution Behavior of Nickel

Zamin, M.; Ives, M. B.

doi:10.5006/0010-9312-29.8.319

Cited by 28 publications

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“…An electrical lead wire was attached at the center of one side with Pb-Sn solder. Specimen preparation and the cell assembly were identical to that described elsewhere (16)(17)(18). Specimens were mechanically polished to 1 ~m diamond, followed by electropolishing (19) in 60% H2SO4 for 1 rain at 0.5 A/cm 2 and then 2 min at 1.0 A/cm2.…”

Section: Methodsmentioning

confidence: 99%

The Anodic Oxidation of Nickel in 1N H 2 SO 4 Solution

Zamin

Ives

1979

J. Electrochem. Soc.

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The anodic oxidation of nickel in 1N H2SO4 solution has been studied employing potentiostatic and galvanostatic techniques. It has been found that although a large amount of charge is consumed during anodic oxidation, only about 5% of this charge is involved in film growth. The thickness of the passive film on nickel in 1N H2SO4 is between 6–16Å for anodic oxidation times of 15–60 min. The experimental results have been used to develop a kinetic equation describing the film growth on nickel. It is shown that the logarithm of the film growth current density is inversely proportional to the charge stored in the film. The resistivity of the film suggests that the film is pure and almost stoichiometric normalNiO . It is suggested that the Flade potential of nickel in 1N H2SO4 corresponds to that potential, more noble than the passivation potential, at which the surface of the nickel is covered with a pore‐free film of normalNiO and passivation is complete.

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Section: Methodsmentioning

confidence: 99%

The Anodic Oxidation of Nickel in 1N H 2 SO 4 Solution

Zamin

Ives

1979

J. Electrochem. Soc.

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“…For these reasons the anodic dissolution and the active to passive transition of nickel in aggressive solutions containing anions, like Br-, F-, and I- (9)(10)(11), and particularly C1-ions (11)(12)(13)(14)(15)(16)(17)(18)(19)(20), have been extensively investigated. The basic conclusion of most authors is that the electrodissolution mechanism, as with other related metals such as Fe and Co (1), involves a hydroxo-metal intermediate adsorbed at the electrode surface (4).…”

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confidence: 99%

Influence of Chloride Concentration on the Active Dissolution and Passivation of Nickel Electrodes in Acid Sulfate Solutions

Real¹,

Barbosa

Vilche

et al. 1990

J. Electrochem. Soc.

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The influence of C1-ion concentration on the active dissolution and passivation of polycrystalline nickel rotating disk electrodes in sulfuric acid-potassium sulfate solutions at pH 2.6 and 25~ was studied. The voltammetric data suggest that the passive layer results from a complex reaction involving the electrodissolution of the base metal, the formation of the anodic layer and its partial chemical dissolution. The influence of C1-ions under different hydrodynamic conditions is discussed taking into account the competitive adsorption involving C1-ions and species containing oxygen at the initial stages of the reaction yielding soluble products, and the appearance of Ni(OH)2 as a new phase. Solution stirring favors the electrodissolution reaction by increasing the transport rate of C1-and H § ions to the electrode surface, and simultaneously decreasing the thickness of the Ni(OH)2 layer.

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“…Passive film formation of nickel under atmosphere pressure can be recognized to range from Ni304 to Ni203 from the Pourbaix diagram [1]. Many detailed studies have been conducted recently to investigate the effect of chloride ions on the passivity of nickel [2][3][4][5]. The presence of halogen ions, particularly chloride, breaks down the passive film and causes pitting corrosion.…”

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Effect of chloride ions on the corrosion behaviour of nickel

Hsu

1987

J Mater Sci Lett

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Protection against corrosion in most metals is afforded by the presence of a passive film. Passive film formation of nickel under atmosphere pressure can be recognized to range from Ni304 to Ni203 from the Pourbaix diagram [1]. Many detailed studies have been conducted recently to investigate the effect of chloride ions on the passivity of nickel [2][3][4][5]. The presence of halogen ions, particularly chloride, breaks down the passive film and causes pitting corrosion. Moon and Nobe [6] reported that corrosion rates of nickel increased with a reaction order of chloride ion of 0.4. Chevalet and Zutic [7] also summarized and proposed a reaction mechanism of nickel in chloride ion solutions.The main purpose of this work was to study the corrosion behaviour of nickel in the presence and absence of chloride ions at various pH values under atmospheric pressure at 25 and 56 ° C, respectively.Nickel specimens were prepared for polarization measurements from 99.99% nickel sheet. The specimens were polished with 600 grit silicon carbide paper, cleaned in acetone and dried. The test electrode assembly consisted of a teflon sleeve which covered all metal surfaces except the polished surface. The area of specimen surface contact with the cell solution was 1.07 cm 2. Electrochemical measurements were obtained using a typical three-electrode system. The electrode consisted of a stationary flat nickel electrode, a pair of counter electrodes and a saturated calomel reference electrode. A Nichia model G1001E potentiostat was used for the electrochemical measurements.The potential between the working electrode and the reference electrode was measured through a Luggin capillary which was placed as close as possible to the nickel electrode. Electrochemical corrosion experiments were initiated in one litre of desired pH solution prepared from reagents H2SO4, NaOH, NaC1 and deionized water, and then was operated under atmospheric pressure. Calibration was conducted in accordance with and .Evans diagrams for nickel specimens in solutions of various pH values under atmospheric pressure at 25 and 56 ° C, respectively, are shown in Figs 1 and 2. The log current (i) against potential plots in (3 g l-~ NaC1) chloride solutions are also shown in Figs 3 and 4. Each profile was begun approximately at the cathodic overpotential (t/,) value of -0.4V and scanned in an anodic direction to an anodic overpotential (r/a) of approximately 4-0.4V, or more, at a rate of 0.2 mV sec 1. As the scan rises from low to high potential, the current decreases to a zero value at the corrosion potential, Ecorr. Values of the polarization resistance (Rp) and corrosion current density (i~o~) from linear polarization are included in Table I

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Effect of Chloride lorn Coeceetratioe on the Anodic Dissolution Behavior of Nickel

Cited by 28 publications

References 0 publications

The Anodic Oxidation of Nickel in 1N H 2 SO 4 Solution

The Anodic Oxidation of Nickel in 1N H 2 SO 4 Solution

Influence of Chloride Concentration on the Active Dissolution and Passivation of Nickel Electrodes in Acid Sulfate Solutions

Effect of chloride ions on the corrosion behaviour of nickel

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