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Special Section Papers

Resistance Improvement of Aluminum Surface to Corrosion Through Reactions With Fluoride Ions

[+] Author and Article Information
Magal Saphier

Chemistry Department,
Nuclear Research Centre Negev,
P.O. Box 9001,
Beer-Sheva 84190, Israel
e-mail: magal_saphier@yahoo.com

Oron Zamir

Department of Nuclear Engineering,
Ben-Gurion University of the Negev,
Beer-Sheva 8410501, Israel;
Chemistry Department,
Nuclear Research Centre Negev,
P.O. Box 9001,
Beer-Sheva 84190, Israel
e-mail: oron_z1@walla.co.il

Polina Berzansky

Chemistry Department,
Ben-Gurion University of the Negev,
Beer-Sheva 8410501, Israel
e-mail: lilith479@gmail.com

Oshra Saphier

Department of Chemical Engineering,
Sami Shamoon College of Engineering,
Beer-Sheva 84100, Israel
e-mail: oshras@sce.ac.il

Dan Meyerstein

Chemical Sciences Department,
Ariel University,
Ariel 407000, Israel
e-mail: danmeyer@bgu.ac.il

Manuscript received June 12, 2016; final manuscript received March 28, 2017; published online May 25, 2017. Assoc. Editor: Ilan Yaar.

ASME J of Nuclear Rad Sci 3(3), 030914 (May 25, 2017) (3 pages) Paper No: NERS-16-1059; doi: 10.1115/1.4036432 History: Received June 12, 2016; Revised March 28, 2017

The reaction of fluoride ions with alumina was found to strongly depend on the concentration of fluoride ions in the aqueous solution. At low concentrations ([fluoride ions] < 0.1 mol/l in the case of potassium fluoride), the aqueous concentration of aluminum ions is relatively high as measured by using inductively coupled plasma optical emission spectroscopy (ICP-OES), and the aluminum oxide dissolves as a fluoride complex. At high concentrations of fluoride ([fluoride ions] > 0.5 mol/l in the case of potassium fluoride), a new structure is formed on the alumina surface involving fluoride, aluminum, potassium, and oxygen (in the case of potassium fluoride). The structure was characterized by using X-ray powder diffraction (XRD), scanning electron microscope (SEM), and energy-dispersive X-ray spectroscopy (EDS). The resulting structure improved the passivation of alumina, the solubility of aluminum ions decreasing compared to the untreated alumina. Aluminum surfaces that were fluoride-treated showed a better resistance to dissolution in both acidic and basic media.

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References

Figures

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Fig. 1

Concentration of aluminum ions as a function of fluoride concentration in aqueous solution at pH 6.0, 1 g alumina in 30 ml potassium fluoride solution for 24 h

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Fig. 2

EDS spectrum of fluoride-treated alumina

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Fig. 3

SEM micrograph of (a) untreated alumina and (b) fluoride-treated alumina

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Fig. 4

Aqueous concentration of aluminum ions at different pH values for fluoride-treated and untreated reference: (a) at pH 4, 6, 9 and (b) at pH 2, 12

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Fig. 5

Comparison of aqueous concentrations of aluminum ions at different pH values, comparison of different salts for fluoride-treated and untreated reference

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Fig. 6

Picture of aluminum stripes: (a) “fluoride-treated” and (b) untreated reference

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