The Electrode Potential of Evaporated Aluminum Films in Chloride Solution

Hagyard, T.; Earl, WB; Kirkpatrick, Karen; Watson, I. G.

doi:10.1149/1.2424170

Cited by 9 publications

(8 citation statements)

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“…The OCP drop at the beginning of the test could be linked to the dissolution of the protective oxide [27]. Importantly, Hagyard et al showed that the potential rose to a peak at the beginning of the immersion and that this increase was attributed to the dissolution of aluminum and to the formation of the protective oxide [28,29]. This reaction was very quick and, thus, is rarely observed, which was the case in this study because no peak was visible in Fig.…”

Section: Corrosion Susceptibility Of the 2050 Alloy During Continuous Immersion Testsmentioning

confidence: 49%

Effect of varying conditions of exposure to an aggressive medium on the corrosion behavior of the 2050 Al–Cu–Li alloy

et al. 2014

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The corrosion behavior of aluminum alloy 2050 was studied as a function of varying conditions of exposure to an aqueous NaCl solution. Two metallurgical states were considered, i.e., an as-received alloy (NHT) and aged samples (HT). After continuous immersion tests, the NHT samples were susceptible to intergranular corrosion, whereas intragranular corrosion was observed for the HT samples. For the NHT samples, cyclic corrosion tests, with alternate immersion -emersion periods, induced subgrain boundary dissolution, and for the HT samples, grain and/or subgrain boundary sensibilization was induced. Hydrogen content measurements suggested a hydrogen enrichment of the alloy under cyclic corrosion tests.

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Section: Corrosion Susceptibility Of the 2050 Alloy During Continuous Immersion Testsmentioning

confidence: 49%

Effect of varying conditions of exposure to an aggressive medium on the corrosion behavior of the 2050 Al–Cu–Li alloy

et al. 2014

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“…The initial step must be the adsorption of water onto the fresh metal surface which proceeds rapidly to completion immediately behind the stylus Fe + H20 ~ Fe.H2Oads [1] Reaction [1] is followed by one of two mechanisms as follows Fe'H2Oads ~ FeOHa~s + H + + e- [2] or Fe'H2Oads .~ Fe 'OH-ads + H + [3] Fe'OH-ads-~ FeOHads ~ e- [4] By considering the coverage of adsorbed water to be complete, and the coverage of FeOH to be small, reaction [2] gives…”

Section: Discussionmentioning

confidence: 99%

“…and OE/O log is ----118 mV, OE/O pH ----0 for ~ -----0.5. Reaction [3] forms a rapid equilibrium prior to reaction [4], with Ks = 0[H+]/(1 --0) [6] where 0 is the coverage of adsorbed OH-, and…”

Section: Discussionmentioning

confidence: 99%

“…[5] controls the bare surface reaction rate, and reaction [2] (pH independent) is rate controlling. For 7 < pH < 11.7 the scheme represented by reactions [3] and [4] controls the reaction rate, with 0 --> 0; the rate is given by Eq. [8], which is first order in pH.…”

Section: Discussionmentioning

confidence: 99%

“…Measurements of bare surface corrosion potentials on A1 made by cutting a lacquered electrode with a ruby stylus (1,2) showed that the metal adopts a very low potential on cutting; the potential then rises owing to the evolution of hydrogen followed by repassivation. Later work on evaporated A1 films (3) confirmed that this behavior is a feature of a bare A1 surface and does not arise from stress or heating effects during cutting and subsequent relaxation or cooling. Similar measurements have been made on a large number of metals by high speed drilling with a dentist's drill-bit (4).…”

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confidence: 91%

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The Electrochemical Behavior of Scratched Iron Surfaces in Aqueous Solutions

Burstein

Davies

1981

J. Electrochem. Soc.

101

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A technique involving rapid scratching of rotating disk electrodes under potential control is presented and used to examine rapid reaction steps in the anodic behavior of iron in aqueous solutions of pH 0–14. Both anodic and cathodic reaction rates are greatly accelerated during scratching; current densities of up to ∼10 A cm−2 of bare metal surface were observed. The results obey Tafel's law and demonstrate the formation of an adsorbed layer of normalFeOH by: (i) normalFe+H2O⇌normalFe·H2Onormalads , followed by (ii) normalFe·H2Onormalads→FeOHnormalads +H++e− for pH<7 , or (iii) normalFe·H2Onormalads⇌normalFe·OHnormalads−+H+ , and (iv) normalFe·OHnormalads−→FeOHnormalads+e− for pH>7 . The layer of adsorbed normalFeOH is formed at potentials negative with respect to the reversible potentials for oxide formation and exists on the surface during steady‐state anodic oxidation of Fe and during cathodic reduction of H+ from solution. The results are discussed in terms of the mechanism of steady‐state dissolution of Fe.

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