The Solubility of Ferrous Hydroxide and Its Effect Upon Corrosion

Whitman, W. G.; Russell, R. P.; Davis, G. H. B.

doi:10.1021/ja01678a009

Cited by 17 publications

(9 citation statements)

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“…The corrosion process is illustrated in Figure 1, where the dimensions are given. At pH 9.2, ferric ion concentration is >10 -22 mol/L, estimated from the solubility product of Fe(OH) 3 . 8 In this model, ferric ion is neglected because of its extremely low concentration.…”

Section: Corrosion-february 2002mentioning

confidence: 99%

“…Experimental work has shown that the corrosion products, ferrous ions and hydroxide ions, combine to form a precipitate on an iron surface that is porous and nonprotective. [1][2][3] This precipitate results in a solution pH of 9.2, calculated according to the solubility product of ferrous hydroxide (Fe[OH] 2 ). Oxygen, which is the major oxidizer for iron corrosion, is partially reacted when diffusing through the boundary layer because it is consumed by oxidizing ferrous ions to ferric ions.…”

Section: Introductionmentioning

confidence: 99%

“…Oxygen, which is the major oxidizer for iron corrosion, is partially reacted when diffusing through the boundary layer because it is consumed by oxidizing ferrous ions to ferric ions. Ferric hydroxide (Fe[OH] 3 ) is often present as a porous precipitate in the solution and does not provide appreciable resistance to the transport of oxygen and other solution species. Although formation of a passive film is possible without chloride ions, it is active iron corrosion that is the subject of this work.…”

Section: Introductionmentioning

confidence: 99%

“…Although Fe(OH) 2 precipitate may saturate the boundary layer near the iron surface, the solution layer usually appears brown. This color is caused by Fe(OH) 3 formed from ferrous ion oxidation. [1][2][3] Since oxygen is partially depleted in the boundary layer, the oxygen concentration at the solutioniron interface is decreased, which results in a decreased iron corrosion rate.…”

Section: Introductionmentioning

confidence: 99%

“…This color is caused by Fe(OH) 3 formed from ferrous ion oxidation. [1][2][3] Since oxygen is partially depleted in the boundary layer, the oxygen concentration at the solutioniron interface is decreased, which results in a decreased iron corrosion rate. The quantitative significance of this decrease in corrosion rate has not been reported in the literature, although a great deal of work has been devoted to iron oxide film characterization.…”

Section: Introductionmentioning

confidence: 99%

See 4 more Smart Citations

Effect of Ferrous Ion Oxidation on Corrosion of Active Iron under an Aerated Solution Layer

Song¹,

Kirk²,

Graydon³

et al. 2002

CORROSION

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A new model was developed to study the effect of ferrous ion oxidation on the corrosion of active iron. When ferrous hydroxide precipitate is present at the iron surface as the result of corrosion, the solution boundary layer near the iron surface is saturated with ferrous hydroxide and the pH and ferrous ion concentration are fixed within the layer. The ferrous hydroxide precipitate and that of ferric hydroxide are often porous and do not provide resistance to the transport of solution species. Since this work deals with active iron corrosion, a passive film at the iron surface is not considered. The results show that ferrous ion oxidation decreases corrosion because it decreases oxygen concentration in the boundary layer. The corrosion rate can be decreased by up to 13.9%. This value is independent of boundary layer thickness, temperature, and saturation factor of ferrous hydroxide. The results indicate that ferrous ion oxidation does have an effect on the rate of iron corrosion and that neglecting ferrous ion oxidation when determining iron corrosion results in an overestimate of the corrosion rate.

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Section: Corrosion-february 2002mentioning

confidence: 99%

Section: Introductionmentioning

confidence: 99%

Section: Introductionmentioning

confidence: 99%