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Journal of Materials
Volume 2013 (2013), Article ID 479728, 5 pages
Corrosion Inhibition of Aluminium in HCl by Amine Modified Epoxy Resin
1Institute of Petroleum Studies, University of Port Harcourt, PMB 2, Choba, Port Harcourt 500102, Rivers State, Nigeria
2Department of Chemical Sciences, Oduduwa University, Ipetumodu, Ile-Ife 220371, State of Osun, Nigeria
3Technical Department, Greenfield-Oaks Limited, London SE25 4HL, UK
4Department of Pure and Industrial Chemistry, University of Port Harcourt, PMB 5323, Port Harcourt 500102, Rivers State, Nigeria
Received 12 November 2012; Revised 3 February 2013; Accepted 3 February 2013
Academic Editor: Wolfgang Maser
Copyright © 2013 Makanjuola Oki et al. This is an open access article distributed under the Creative Commons Attribution License, which permits unrestricted use, distribution, and reproduction in any medium, provided the original work is properly cited.
N-Butyl amine has been grafted unto Dow epoxy resin. The product was evaluated as an acid inhibitor by gravimetric techniques. The reduction in corrosion of aluminium in 1 M HCl solution was 92% at and 83% at with an inhibitor concentration of 100 ppm. The corrosion rate at this concentration was and mm/yr at and . For the specimens in HCl without inhibitor at 10-hour immersion period, the corrosion rate was and mm/yr, respectively, at and . Data obtained correlate with Langmuir isotherm.
Aluminium and its alloys find extensive application in the construction of heat exchangers, radiators, and related components in water cooling/treatment facilities. It is often observed that such facilities may suffer corrosion damage from ingress of chlorides and other extraneous anions as a result of inadequate provision for corrosion mitigation such as faulty design features and nonintroduction of suitable corrosion inhibitors into the system. Pitting corrosion at crevices and under sediments is often encountered in such industrial situations.
The use of organic inhibitors is the most economical and practical method of protecting metals against aqueous corrosion [1–3]. These inhibitors contain heteroatoms such as Sulphur, Oxygen, and Nitrogen in their structures in addition to multiple bonds and may contain cyclic hydrocarbons as well [3–6]. The mechanism of inhibition of these organic compounds is thought to be by adsorption which may depend on the number of heteroatoms and the surface area of the corroding metal/alloy [7, 8].
Various investigators [8–13] have researched on polymers as corrosion inhibitors because of their large surface areas, cost effectiveness, and inherent stability. These polymers have been reported to be very efficient at low concentrations in very aggressive media although efficiencies vary widely as a result of differences in composition. Chemically modified polyurethane  gave about 95% inhibition efficiency for mild steel corroding in acidic medium. On the other hand, polyacrylamide  achieved an efficiency of about 63% for aluminium corroding freely in 0.5 M HCl solution.
In order to contribute towards the search for suitable corrosion inhibitors of polymeric origin, in the present investigation, a Dow epoxy resin was chemically modified with n-butyl amine at suitable temperatures and examined as corrosion inhibitor for aluminium in 1 M HCl solution.
99.99% aluminium with nominal impurities of 0.004 wt% Fe, 0.002 wt% Cu, and 0.003 wt% Si was made into electrodes measuring 10 mm × 10 mm × 1 mm. The epoxy resin, Resin 828, is a product of Dow Chemicals, USA, while all other chemicals employed in this investigation are laboratory grade reagents from BDH Chemicals, UK.
2.2.1. Inhibitor Formulation
The inhibitor employed in this investigation was synthesised by mixing in a 500 mL beaker, equal moles of epoxy resin which had amber colouration, and n-butyl amine in a water bath, set at a controlled temperature of 100°C. A consistent brown coloured product, Amine Modified Epoxy Resin (AMER), was obtained after 30 mins of constant stirring.
The various concentrations of inhibitor were obtained by serially diluting 1 g/litre solution of the inhibitor with the corrodents of interest, 1 M HCl solution.
2.2.2. Corrosion Measurements
The aluminium electrodes were etched in 10% NaOH solution for 3 mins, rinsed in running doubly distilled water and thereafter desmutted in 50% for 2 mins, rinsed in doubly distilled water and in acetone, dried in air for 10 minutes prior to being stored in desiccators. Triplicate experiments, at 30°C and 60°C were performed by separately immersing 10 preweighed electrodes, with exposed area of 2.3 cm2, in 200 mL of 1 M HCl contained in 250 mL beakers for times ranging from 1 hr to 10 hrs. After each period of immersion, the electrodes were washed in running distilled water for 3 mins while scrubbing the surfaces with a soft brush and later in acetone for 30 sec. After drying in a stream of cool air, the electrodes were reweighed. The mean of the weight changes were taken as the weight change for each period of immersion. Similar procedure was performed in 1 M HCl with different concentrations of AMER as inhibitor of interest.
3. Results and Discussions
3.1. Corrosion Rates
For the calculation of corrosion rates, the relationship in (1) as described by Jones  and other authors [15–17] was employed where is the corrosion rate in mm/yr, is the weight loss, is the density of Aluminium in g/cm3, and is the time of exposure.
The efficiency of the inhibitor, %Inh., was obtained from the following equation where CRO and are Corrosion rates without and in the presence of inhibitor, respectively.
, the surface coverage, is given by the relationship, , where all the symbols have their usual meanings.
The weight loss and corrosion rates of aluminium specimens in hydrochloric acid at both 30°C and 60°C are displayed in Figures 1 and 2, respectively. The rate of change in weight at 30°C increased rapidly between 1 and 2 hours with a rate that decreased with time between 2 and 10 hours of immersion in HCl. The initial rapid increase in weight loss is consistent with the rapid dissolution of the amphoteric air formed oxide skin on aluminium in acidic media which exposes freshly prepared aluminium surface to rapid dissolution of the substrate metal.
However, the decrease in rate of dissolution may be attributed to the formation of corrosion products at cathodic sites on the aluminium electrode. Such corrosion products will retard the corrosion process for a while before they are subsequently dissolved by the acidic medium to reveal further areas of the specimen and corrosion processes will proceed.
At 60°C, the weight loss is linear with time of immersion in HCl solution as all corrosion products formed are dissolved rapidly in the warm corrodent.
The gravimetric method for corrosion studies is a time tested and reliable technique. Several authors have reported good correlation between this technique and gasometric, impedance, and polarisation techniques [16–20]. The corrosion rate of aluminium in HCl at 60°C (Figure 2) increased at a rate which decreased with exposure time and was maximum at mm/yr at 10 hours. On the other hand, the corrosion rate at 30°C was at its peak, mm/yr, after 2 hours of exposure in the corrodent which corroborates the weight loss measurement described earlier. Thereafter, the corrosion rate decreased to about mm/year at 3 hours of exposure, beyond which steady increase in corrosion rate was observed and was about mm/yr at 10 hours in HCl solution.
From Figure 3, the corrosion rates decreased exponentially as the concentration of the inhibitor was increased. Thus, it can be safely inferred that the inhibitor reduced the corrosion rates of aluminium at both 30°C and 60°C.
Displayed in Figure 4 is the percent inhibition which increases with increase in the concentration of the inhibitor. Inhibitors of organic origin inhibit corrosion by adsorbing on metals in corroding systems. The increase in % inhibitor efficiency was more pronounced at concentration levels between 40 and 60 ppm probably as the surface of the corroding aluminium specimens became saturated with adsorbed inhibitor species. The efficiency of the inhibitor was better at lower temperatures and this may be attributed to desorption of inhibitor molecules from the corroding surface at high temperatures as described by El-Etre  and Abdallah . However, AMER was more effective at 30°C with an efficiency of about 92% as against 86% at 60°C, with an inhibitor concentration of 100 ppm.
Furthermore, the energy of activation, , for the corrosion reactions in the presence and absence of corrosion inhibitor obtained from the condensed Arrhenius equation (3) is 40.11 kJ/mol and 28.54 kJ/mol, respectively. The increase in in the presence of inhibitor further demonstrates that there was a hindrance placed on the electrochemical reaction path on the substrate by some adsorbed inhibitor species. With a positive value, the mechanism of inhibition is likely to be by physical adsorption [21–23] of the inhibitor species
The interpretation of adsorption isotherms has been employed by several authors [24–27] to describe the mode(s) of interaction of inhibitor molecules with corroding surfaces in various media in which, the values for surface coverage of inhibitors, , were plotted against concentration to fit Frumkin  or, versus to establish a Langmuir  type of adsorption isotherm. Displayed in Figure 5 are curves for Langmuir adsorption.
Displayed in Figure 5 are curves of Langmuir adsorption for AMER at both 60° and 30°C where it can be observed that the inhibitor obeys this adsorption isotherm. From observed data, it is obvious that the adsorption isotherm curves are neither in agreement with Temkin nor Frumkin adsorption isotherms, respectively. Thus there are no interactions among the adsorbed inhibitor molecules on the corroding surfaces .
The heat of adsorption, , can be obtained from the relationship where is the temperature of the corroding system at 30°C and the corresponding temperature at 60°C. is the surface coverage of the inhibitor at 30°C while is the surface coverage at 60°C.
The calculated approximate value of is −17.52 kJ/mol. The negative value of is consistent and agrees with the findings of other researchers [20, 21] that for physio-sorption, the heat of adsorption is generally negative and positive values indicate mechanism by chemisorption .
Amine modified epoxy resin (AMER) effectively reduced the corrosion rate of aluminium in hydrochloric acid by physically adhering to the corroding metallic surface.
The data obtained from the gravimetric studies correlate with the Langmuir adsorption isotherm which indicate that there are no interactions among the adsorbed inhibitor species. However, the reactions at the electrolyte/aluminium interface was sufficiently interrupted by the inhibitor species to lower the corrosion rates by 92% and 86% at 30° and 60°C, respectively.
The corrosion rates of aluminium in 1 M hydrochloric acid in the presence of 100 ppm of AMER at 10 hours of exposure are and mm/yr, respectively at 60° and 30°C. On the other hand, for specimens exposed in hydrochloric acid without AMER for the same period, the corrosion rates are and mm/yr at 30° and 60°C.
The mechanism of inhibition is proposed by physical adsorption of the inhibitor species on the corroding aluminium surface.
Dr. M. Oki acknowledges the National Universities Commission, Nigeria, for the award of one-year Linkages with Academics and Experts in Diaspora Scheme which was utilised at the Institute of Petroleum Studies/Department of Petroleum and Gas Engineering, University of Port Harcourt, Nigeria. S. Otikor acknowledges the Head of Department of Chemistry and Industrial Chemistry for the use of laboratory facilities while T. k. Oki is grateful to the management of Greenfield-Oaks Ltd., UK, for the use of time share facilities.
- D. A. Jones, Principles and Prevention of Corrosion, Prentice Hall, Upper Saddle River, NJ, USA, 2nd edition, 1996.
- G. Y. Elewady, I. A. El-Said, and A. S. Fouda, “Effect of anions on the corrosion inhibition of aluminum in HCI using ethyl trimethyl ammonium bromide as cationic inhibitor,” International Journal of Electrochemical Science, vol. 3, pp. 644–655, 2008.
- E. A. Noor, “The inhibition of mild steel corrosion in phosphoric acid solutions by some N-heterocyclic compounds in the salt form,” Corrosion Science, vol. 47, no. 1, pp. 33–55, 2005.
- K. Babic-Samardzija, C. Lupu, N. Hackerman, and A. R. Barron, “Inhibitive properties, adsorption and surface study of butyn-1-ol and pentyn-1-ol alcohols as corrosion inhibitors for iron in HCl,” Journal of Materials Chemistry, vol. 15, no. 19, pp. 1908–1916, 2005.
- D. Turcio-Ortega, T. Pandiyan, J. Cruz, and E. Garcia-Ochoa, “Interaction of imidazoline compounds with (n = 1-4 Atoms) as a model for corrosion inhibition: DFT and electrochemical studies,” The Journal of Physical Chemistry C, vol. 111, no. 27, pp. 9853–9866, 2007.
- E. E. Oguzie, S. G. Wang, Y. Li, and F. H. Wang, “Influence of iron microstructure on corrosion inhibitor performance in acidic media,” The Journal of Physical Chemistry C, vol. 113, no. 19, pp. 8420–8429, 2009.
- R. Solmaz, G. Kardaş, M. Çulha, B. Yazici, and M. Erbil, “Investigation of adsorption and inhibitive effect of 2-mercaptothiazoline on corrosion of mild steel in hydrochloric acid media,” Electrochimica Acta, vol. 53, no. 20, pp. 5941–5952, 2008.
- P. Manivel, S. Sathiyanarayanan, and G. Venkatachari, “Synthesis of poly(p-phenylene diamine) and its corrosion inhibition effect on iron in 1M HCl,” Journal of Applied Polymer Science, vol. 110, no. 5, pp. 2807–2814, 2008.
- S. Banerjee, A. Mishra, M. M. Singh, B. Maiti, B. Ray, and P. Maiti, “Highly efficient polyurethane ionomer corrosion inhibitor: the effect of chain structure,” RSC Advances, vol. 1, pp. 199–210, 2011.
- M. A. Amin, S. S. A. EI-Rehim, E. E. F. El-Sherbini, O. A. Hazzazi, and M. N. Abbas, “Polyacrylic acid as a corrosion inhibitor for aluminium in weakly alkaline solutions. Part I: weight loss, polarization, impedance EFM and EDX studies,” Corrosion Science, vol. 51, no. 3, pp. 658–667, 2009.
- A. Y. Musa, A. A. H. Kadhum, A. B. Mohamad, M. S. Takrif, and E. P. Chee, “Inhibition of aluminum corrosion by phthalazinone and synergistic effect of halide ion in 1.0M HCl,” Current Applied Physics, vol. 12, no. 1, pp. 323–330, 2012.
- C. Jeyaprabha, S. Sathiyanarayanan, and G. Venkatachari, “Co-adsorption effect of polyaniline and halide ions on the corrosion of iron in 0.5 M solutions,” Journal of Electroanalytical Chemistry, vol. 583, no. 2, pp. 232–240, 2005.
- V. Srivastava, S. Banerjee, and M. M. Singh, “Inhibitive effect of polyacrylamide grafted with fenugreek mucilage on corrosion of mild steel in 0.5 M at ,” Journal of Applied Polymer Science, vol. 116, no. 2, pp. 810–816, 2010.
- S. Banerjee, A. Mishra, M. M. Singh, and P. Maiti, “Effects of naniclay and polyurethanes on inhibition of mild steel corrosion,” Journal of Nanoscience and Nanotechnology, vol. 11, no. 2, pp. 966–978, 2011.
- S. A. Umoren and M. M. Solomon, “Effect of halide ions additives on the corrosion inhibition of aluminum in HCL by polyacrylamide,” The Arabian Journal of Science and Engineering, vol. 35, no. 2A, pp. 115–130, 2009.
- A. A. El-Maghraby, “Corrosion inhibition of aluminium in HCl using potassium iodate,” The Open Corrosion Journal, vol. 2, pp. 189–196, 2009.
- P. C. Okafor, U. J. Ekpe, E. E. Ebenso, E. E. Oguzie, N. S. Umo, and A. R. Etor, “Extract of Allium cepa and Allium sativum as corrosion inhibitors of mild steel in HCl solution,” Transactions of the SAEST, vol. 41, no. 2, pp. 82–87, 2006.
- A. Y. El-Etre, “Inhibition of aluminum corrosion using Opuntia extract,” Corrosion Science, vol. 45, no. 11, pp. 2485–2495, 2003.
- M. Abdallah, “Antibacterial drugs as corrosion inhibitors for corrosion of aluminium in hydrochloric solution,” Corrosion Science, vol. 46, no. 8, pp. 1981–1996, 2004.
- S. A. Umoren, I. B. Obot, E. E. Ebenso, P. C. Okafor, O. Ogbobe, and E. E. Oguzie, “Gum arabic as a potential corrosion inhibitor for aluminium in alkaline medium and its adsorption characteristics,” Anti-Corrosion Methods and Materials, vol. 53, no. 5, pp. 277–282, 2006.
- P. C. Okafor, E. E. Ebenso, and U. J. Ekpe, “Äzadirachta indica extracts as corrosion inhibitor for mild steel in acid medium,” International Journal of Electrochemical Science, vol. 5, no. 7, pp. 978–993, 2010.
- L. A. Nnanna, I. U. Anozie, A. G. I. Avoaja, C. S. Akoma, and E. P. Eti, “Comparative study of corrosion inhibition of Aluminium alloy type AA 3003 in acidic and alkaline media by Euphorbia hirta extract,” African Journal of Pure & Applied Chemistry, vol. 5, no. 8, pp. 265–271, 2011.
- I. B. Obot and N. O. Obi-Egbedi, “An interesting and efficient green corrosion inhibitor for Aluminium from extracts of Chlomolaena odorata L. in acidic solution,” Journal of Applied Electrochemistry, vol. 40, pp. 1977–1984, 2010.
- M. Oki, E. Charles, C. Alaka, and T. K. Oki, “Corrosion inhibition of mild steel in HCl by tannins from Rhizophora racemosa,” Materials Science and Applications, vol. 2, pp. 592–595, 2011.
- K. F. Khaled and N. Hackerman, “Investigation of the inhibitive effect of ortho-substituted anilines on corrosion of iron in 1 M HCl solutions,” Electrochimica Acta, vol. 48, no. 19, pp. 2715–2723, 2003.
- E. E. Oguzie, “Corrosion inhibition of aluminium in acidic and alkaline media by Sansevieria trifasciata extract,” Corrosion Science, vol. 49, no. 3, pp. 1527–1539, 2007.
- K. F. Khaled, K. Babić-Samardžija, and N. Hackerman, “Cobalt(III) complexes of macrocyclic-bidentate type as a new group of corrosion inhibitors for iron in perchloric acid,” Corrosion Science, vol. 48, no. 10, pp. 3014–3034, 2006.
- A. N. Frumkin, “Electrocapillary curve of higher aliphatic acids and the state equation of the surface layer,” Zeitschrift für Physikalische Chemie, vol. 116, pp. 466–470, 1925.
- I. Langmuir, “The adsorption of gases on plane surfaces of glass, mica and platinum,” The Journal of the American Chemical Society, vol. 40, no. 9, pp. 1361–1403, 1918.