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Advances in Chemistry

Volume 2014 (2014), Article ID 808456, 10 pages

http://dx.doi.org/10.1155/2014/808456
Research Article

Baphia nitida Leaves Extract as a Green Corrosion Inhibitor for the Corrosion of Mild Steel in Acidic Media

1Department of Chemistry, Faculty of Science, Imo State University, PMB 2000, Owerri, Nigeria

2Department of Chemistry, Federal University of Technology Owerri, PMB 1526, Owerri, Nigeria

3Department of Pure and Industrial Chemistry, University of Port Harcourt, PMB 5323, Port Harcourt, Nigeria

Received 21 April 2014; Accepted 10 July 2014; Published 4 August 2014

Academic Editor: Ana Mornar

Copyright © 2014 V. O. Njoku 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.

Abstract

The inhibiting effect of Baphia nitida (BN) leaves extract on the corrosion of mild steel in 1 M H2SO4 and 2 M HCl was studied at different temperatures using gasometric and weight loss techniques. The results showed that the leaves extract is a good inhibitor for mild steel corrosion in both acid media and better performances were obtained in 2 M HCl solutions. Inhibition efficiency was found to increase with increasing inhibitor concentration and decreasing temperature. The addition of halides to the extract enhanced the inhibition efficiency due to synergistic effect which improved adsorption of cationic species present in the extract and was in the order KCl < KBr < KI suggesting possible role of radii of the halide ions. Thermodynamic parameters determined showed that the adsorption of BN on the metal surface is an exothermic and spontaneous process and that the adsorption was via a physisorption mechanism.

1. Introduction

One of the most practical methods of preventing electrochemical corrosion is to isolate the metal surface from corrosive agents [1]. Of the many methods available, the use of corrosion inhibitors is usually the most appropriate method to achieve this objective [29]. These inhibitors could be in the form of organic, inorganic, precipitating, passivating, or volatile species. Generally, corrosion inhibitors may be divided into three broad classes, namely, oxidizing, precipitating, and adsorption inhibitors [10]. Adsorption inhibitors are usually organic substances containing heteroatoms with high electron density such as nitrogen, sulfur, and oxygen [11, 12] and the presence of unsaturated bonds or aromatic rings in the molecular structure of the inhibitor favors adsorption on corroding metal surface [13]. The adsorption is influenced by the nature and the surface charge of the metal, the type of corrosion media, and the molecular structure of the inhibitor [4]. Some corrosion inhibitors used in different media and for different metals and alloys decrease considerably the oxidation states of the corroding metals. In acid corrosion, inhibitor adsorption may lead to structural changes in the double layer, which could reduce the rates of either the anodic metal dissolution and the cathodic hydrogen ion reduction or both.

It is known that some corrosion inhibitors and their derivatives are toxic and pollute the environment [14]. There is therefore the need to explore new nontoxic, environmental friendly, ecologically acceptable and inexpensive corrosion inhibitor substitutes. Among the alternative corrosion inhibitors, natural products of plant origin have been shown to be quite efficient as corrosion inhibitors [1519].

In this work, the inhibitory properties of leaf extracts of Baphia nitida on mild steel corrosion in 1 M H2SO4 and 2 M HCl have been studied using gasometric and weight loss techniques. The plant popularly called camwood and also known as African sandalwood belongs to the family of Leguminosae and its wood is commonly used to make a red dye. Phytochemical analysis of the leaves detected tannins, flavonoids, and saponin glycosides [20]. The actions of the leaf extract as inhibitor in both acid media over a range of inhibitor concentration and solution temperature, as well as synergistic effects of halides, have been studied.

2. Experimental

2.1. Materials Preparation
2.1.1. Metal Specimen

Mild steel strips of compositions 0.05% C, 0.6% Mn, 0.36% P, and 0.03% Si remainder iron and dimensions 3 cm × 1.5 cm × 0.14 cm were used for gasometric and weight loss studies. The specimens were washed with distilled water, degreased by soaking in absolute ethanol, dried in acetone, and stored in moisture-free desiccators prior to use.

2.1.2. Reagents

Analytical grade reagents were utilized to prepare 1 M H2SO4 and 2 M HCl using distilled water.

2.1.3. Plant Extracts

The Baphia nitida leaves used were obtained locally and were dried to a constant weight in an oven at a temperature of 110°C, and then ground to fine powder. The Baphia nitida (BN) extract was prepared by adding 10 g of the powder into 250 mL of 1 M H2SO4 in a round bottom flask. The same was repeated for 2 M HCl. The resulting solutions were heated under reflux for 2 h and left to cool overnight, and then filtration was carried out using filter paper. From the respective stock solutions, inhibitor test solutions were prepared in the concentration range 5–100 mg/L.

2.2. Methods
2.2.1. Gasometric Experiments

The gasometric setup is essentially an apparatus that measures the volume of gas evolved from a reaction system as described by Onuchukwu [21]. The reaction vessel was connected to a burette via a delivery tube, which was in turn connected to a reservoir of paraffin oil. Fifty milliliters of the test solutions were introduced, respectively, into the reaction vessel for blank determinations and the initial volumes of air in the burette, taken against that of the paraffin oil, were recorded. Thereafter, two mild steel coupons were introduced into the reaction vessel and the flask quickly closed. The volume of hydrogen gas evolved by the corrosion reaction was monitored by the drop in the volume of the paraffin oil level in the gasometric gauge. The progress of the corrosion reaction was monitored by careful volumetric measurement of the evolved hydrogen gas at fixed time intervals. The temperature of the experiment was controlled at 30 ± 1 and 60 ± 1°C. The experiments were performed separately employing 20 and 100 mg/L inhibitor concentrations in 1 M H2SO4 and 2 M HCl. The effects of halide ions on the inhibitive action of the BN extract were studied by adding KCl, KBr, and KI separately to 1 M H2SO4 and 2 M HCl with and without 100 mg/L BN extract solutions to yield 0.5 mM concentrations of the halides in each case.

2.2.2. Weight Loss Experiments

The prepared and weighed mild steel coupons were immersed in beakers containing 200 mL of the test solutions with and without the addition of BN extract of concentrations ranging from 5 to 100 mg/L inhibitor concentrations in 1 M H2SO4 and 2 M HCl at 30, 40, 50, and 60°C. The metal strips were suspended in the beakers using glass rods and hooks. After 3 h, the specimens were removed from the solutions, washed appropriately, dried, and reweighed. The weight loss was taken to be the difference between the weight of the coupons after the 3 h period of immersion in the solutions and the initial weight of the coupons. Gravimetric experiments were performed in triplicate and the results showed good reproducibility. The average values were taken and used in subsequent calculations.

3. Results and Discussion

3.1. Gasometric Measurements
3.1.1. Effect of Immersion Time on Corrosion Rate

The spontaneous dissolution of mild steel in acidic media is accompanied by the cathodic reduction of hydrogen ions as shown in (1) The corrosion of iron and steel in acidic solutions is controlled by the hydrogen evolution reaction [22]. Thus, the corrosion rates of the test coupons in absence and presence of inhibitor were assessed using hydrogen evolution measurements. Previous workers have demonstrated the effectiveness of the gas-volumetric technique in monitoring any modifications in the double layer resulting from the action of an adsorbed inhibitor in a metal/corrodent system [2325]. Results obtained by this technique are corroborated by other well established methods including weight loss and thermometry, potentiostatic polarization, and impedance spectroscopy [24, 2628].

Gasometric measurements of mild steel subjected to the effect of acidic media in the absence and presence of BN extract were made at various time intervals. Figures 1(a) and 1(b) present plots of evolved hydrogen gas as a function of time for mild steel corrosion in 1 M H2SO4, in absence and presence of 20 and 100 mg/L BN extract concentrations at 30 and 60°C, respectively. Similar plots are shown in Figures 2(a) and 2(b) for 2 M HCl at 30 and 60°C. The plots in Figures 1 and 2 show a remarkable decrease in hydrogen evolution with the introduction of the inhibitor indicating that BN extract inhibits corrosion of mild steel in acidic environments. The rates of hydrogen evolution were observed to decrease with increasing inhibitor concentration, suggesting that the inhibiting effectiveness of the BN extract depends on the inhibitor concentration. This dependence was almost linear throughout the time interval studied in the absence and presence of BN extract indicating that the inhibitor acts rapidly and does not lose its inhibitory properties with time. However, the kinetic parameters indicate satisfactory inhibitor efficiencies even at low concentration of BN extract.

fig1
Figure 1: Hydrogen evolution during mild steel corrosion in 1 M H2SO4 in absence and presence of Baphia nitida extract at (a) 30°C and (b) 60°C.
fig2
Figure 2: Hydrogen evolution during mild steel corrosion in 2 M HCl in absence and presence of BN extract at (a) 30°C and (b) 60°C.

In all the cases, the dissolution of steel was characterized by a linear increase in the evolution of hydrogen with time. The reaction rate was characterized by differentiating the volume of hydrogen evolved with time and was obtained from the slope of the linear portions of Figures 1(a) and 1(b). Table 1 shows the values of corrosion rates obtained for the different test solutions. The results show that corrosion rate reduced in the presence of the inhibitor and was found to decrease with increasing BN extract concentration in both corrodents. Also, mild steel was observed to exhibit higher corrosion susceptibility in 2 M HCl than in 1 M H2SO4.

tab1
Table 1: Corrosion rates of mild steel in 1 M H2SO4 and 2 M HCl in absence and presence of BN extract obtained from gasometric method.
3.1.2. Inhibition Efficiency

For the gasometric experiments, the degree of surface coverage ( ) and the inhibition efficiency (IE, %) of BN extract on mild steel in acidic media was evaluated from (2). Consider where and are the corrosion rates in the absence and presence, respectively, of a given concentration of BN extract. Table 2 shows values of the degree of surface coverage ( ) and the inhibition efficiency (IE, %) obtained for different concentrations of BN extract in both corrodents using the gasometric technique. The result shows that the extract retarded acid corrosion of the mild steel and surface coverage and hence inhibition efficiencies increased with increasing inhibitor concentration at both temperatures.

tab2
Table 2: Degree of surface coverage and inhibition efficiencies of different concentrations of BN extract during mild steel corrosion in 1 M H2SO4 and 2 M HCl obtained from gasometric method.

Phytochemical analysis of leaves of BN detected tannins, flavonoids, and saponin glycosides and these are known to possess corrosion inhibitory properties [20]. The inhibitive effect could be attributed to the net adsorption of the organic matter on the steel/acid solution interface thereby reducing the surface area available for corrosion reaction and the degree of protection increases with increasing inhibitor concentration. It can be clearly noticed that the inhibition efficiency of BN extract was higher in 2 M HCl than in 1 M H2SO4 over the concentration range studied, suggesting that the nature of the acid anion influences metal-inhibitor interactions. In the presence of strong acids, some inhibitor species become protonated. The surface charge on iron in acidic solution is positive at the corrosion potential and specific adsorption of chloride ions of HCl renders the metal surface more negative and susceptible to adsorption of protonated inhibitor species compared to H2SO4 [29, 30]. Thus, the adsorption of the protonated inhibitor species on the metal surface will be enhanced in HCl, leading to higher inhibition efficiencies.

3.2. Weight Loss Measurements

The inhibition efficiency (IE, %) for the weight loss measurements was calculated using (3) as follows: where (mg) is the weight loss of steel in uninhibited solutions and (mg) the weight loss of steel in inhibited solutions. IE (%) and for mild steel exposed to 1 M H2SO4 and 2 M HCl at various temperatures as a function of BN concentration are shown in Tables 3 and 4. It is observed that at all temperatures inhibition efficiency increased on increasing BN concentration. This observation is in support of results obtained with the gasometric experiments.

tab3
Table 3: Corrosion parameters obtained from weight loss of mild steel in 1 M H2SO4 containing various concentrations of BN extract at different temperatures.
tab4
Table 4: Corrosion parameters obtained from weight loss of mild steel in 2 M HCl containing various concentrations of BN extract at different temperatures.

The effect of temperature on the corrosion behavior of mild steel in the absence and presence of BN extract was investigated by performing weight loss experiments at 30, 40, 50, and 60°C. The results as shown in Tables 3 and 4 demonstrate that the weight loss increased and the inhibition efficiency decreased with increase in temperature. The decrease in inhibition efficiency with increasing temperature suggests weak adsorption interaction between the metal and the extract organic matter. Such behavior corresponds to physical adsorption, such that at higher temperatures, there is a possible shift of the adsorption-desorption equilibrium towards desorption of adsorbed inhibitor [31]. The increase in solution agitation resulting from higher rates of H2 gas evolution as well as the agitation of the interface and roughening of the metal surface as a result of enhanced corrosion all contribute to the reduced stability of the adsorbed inhibitor at higher temperature [15, 32].

3.3. Adsorption Isotherm Behaviour

Experimental and theoretical studies have shown that the protective action of organic substances during metal corrosion is based on the adsorption ability of their molecules, where the resulting adsorption film isolates the metal surface from the corrosive medium [416]. Therefore, Langmuir adsorption isotherm expression (4), which relates the surface coverage defined by IE/100 and the inhibitor concentration ( ), could be applied to determine adsorption equilibrium constant, , at the different temperatures. Consider The plots of versus for 1 M H2SO4 and 2 M HCl are shown in Figures 3(a) and 3(b), respectively, and the values of subsequently calculated from the intercept are shown in Table 5. The adjusted correlation coefficient ( ) values which were all above 0.990 shows a good fit of the experimental data and suggests that the adsorption of BN extract on metal surface followed the Langmuir adsorption isotherm. The results show that the adsorption equilibrium constant ( ) decreased with increasing temperature, indicating better adsorption of BN extract onto the steel surface at lower temperatures. However, at higher temperatures, the equilibrium tends towards desorption.

tab5
Table 5: Thermodynamic parameters for the adsorption of BN extract in 1 M H2SO4 and 2 M HCl on the mild steel at different temperatures.
fig3
Figure 3: Langmuir adsorption plots for mild steel corrosion with BN extract as inhibitor at different temperatures in (a) 1 M H2SO4 and (b) in 2 M HCl.
3.4. Thermodynamic Parameters

The thermodynamic parameters, the standard free energy of adsorption ( ), the standard heat of adsorption ( ), and the standard entropy of adsorption ( ) give an insight into the mechanism of the corrosion inhibition process. From the van’t Hoff equation (5), was determined by a linear regression between and [33]. Consider The values of were evaluated from (6) [34] The values were then obtained from the basic thermodynamic equation The thermodynamic parameters obtained are listed in Table 5. The negative values of show that the adsorption of BN on the metal surface is an exothermic process, supporting the previous observation that IE decreases with increase in temperature. Exothermic process signifies either physisorption or chemisorption while endothermic process is indicative solely of chemisorptions [35]. For an exothermic process, the absolute value of of the process is used to distinguish physisorption from chemisorptions. If is lower than 41.86 kJ/mol, physisorption is involved, while if approaches 100 kJ/mol, it is a chemisorption process [36]. The absolute value of in the present study is lower than 41.86 kJ/mol, confirming the physisorption mechanism proposed involving electrostatic interactions between charged BN molecules and charged metal. The negative values of indicate the stability of the adsorbed layer on the steel surface and that the adsorption of BN molecules onto the steel surface is spontaneous. The negative values of show that the adsorption process is accompanied by a decrease in entropy. The explanation is that the adsorption of BN molecules onto the steel surface reduces the level of chaos on the steel surface leading to a decrease in entropy.

3.5. Apparent Activation Energy ( )

It has been reported that for the acid corrosion of mild steel, the natural logarithm of the corrosion rate is a linear function of . Therefore, the apparent activation energy of the corrosion inhibition process could be obtained by the application of the Arrhenius-type equation (8) [1]. Consider where (mg/cm2 h) is the corrosion rate, (J/mol) is the apparent activation energy, (8.314 J/mol K) is the universal gas constant, is the absolute temperature, and (mg/cm2 h) is the pre-exponential factor. The corrosion rate, , was obtained from the relation where (mg/cm2) is the weight loss per area and is the immersion (corrosion) time (3 h). From the slope and intercept of the linear regression of versus (Figure not shown), the values of and for mild steel corrosion in different concentrations of BN in both 1 M H2SO4 and 2 M HCl were calculated, respectively, as shown in Table 6. The results show that the value of increased with the addition of BN extract. Increase in with increasing concentration of inhibitor indicates physisorption mechanism [21]. Similar results have been reported in some previous studies [9, 37].

tab6
Table 6: Calculated values of apparent activation energy ( ) and preexponential factor ( ) for mild steel corrosion in 1 M H2SO4 and 2 M HCl with BN extract as inhibitor.

Analysis of the temperature dependence of inhibition efficiency as well as comparison of corrosion activation energies in absence and presence of inhibitor gives some insight into the possible mechanism of inhibitor adsorption. A decrease in inhibition efficiency with rise in temperature, with analogous increase in corrosion activation energy in the presence of inhibitor compared to its absence, is frequently interpreted as being suggestive of formation of an adsorption film of physical (electrostatic) nature. The reverse effect, corresponding to an increase in inhibition efficiency with rise in temperature and lower activation energy in the presence of inhibitor, suggests a chemisorption mechanism [22]. The results for both acid media show higher activation energy values in the presence of the extract compared to the blank acids, suggesting physical adsorption [3032, 38].

3.6. Synergism Considerations

The influence of halide ions on the inhibitive action of BN extract was assessed. Table 7 illustrates the effects of 0.5 mM KCl, KBr, and KI without or with 100 mg/L BN extract on the corrosion of mild steel in 1 M H2SO4 and 2 M HCl. The inhibition efficiency of BN extract was significantly improved in the presence of halide ions in both acid media and at both temperatures studied. This suggests that adsorption of protonated species in the BN extract is enhanced through ion pair interactions, with the halide ions forming an intermediate bridge between the positively charged metal surface and the inhibitor [22, 39]. From the inhibition efficiencies, corrosion inhibition efficiencies of the halide alone as well as in combination with BN extract increased in the order KCl < KBr < KI. This is in accordance with the findings of other researchers [15, 3942]. This observation could be explained on the basis of the halide ion radii, which increases in the order Cl (0.09 nm) < Br (0.114 nm) < I (0.135 nm), with the highest ionic radius being more predisposed to adsorption.

tab7
Table 7: Effect of halide ions on the mild steel corrosion in 1 M H2SO4 and 2 M HCl in the absence and presence of BN extract.

The data in Table 7 also shows that inhibition efficiencies in the presence of halides were better improved in 1 M H2SO4 than in 2 M HCl which implies that more halide ions are adsorbed on the metal surface in 1 M H2SO4. This could be attributed to comparatively more positive charge on the steel surface in 1 M H2SO4 [43].

At 60°C, all the halides in combination with BN extract exhibited reduced inhibition efficiencies, indicating that the synergistic effect of BN extract and halide ions is diminished at higher temperatures. The decrease in inhibition efficiency of the BN extract and halide complex with rise in temperature as shown in Table 7 still supports the physisorption mechanism for BN extract on the mild steel surface which is in line with the observation in the absence of halides.

The synergism parameters, , were calculated using the relationship (10) given by Aramaki and Hackermann [44]: where ; is the inhibition efficiency of the halide; is the inhibition efficiency of BN extract; is the inhibition efficiency of BN extract in combination with halide. The calculated values are presented in Table 8 for the different halides at 30 and 60°C. From Table 8, it could be seen that all values of are greater than unity, clearly showing that the corrosion inhibition brought about by the complex of BN extract and halide is due mainly to synergistic effect [41, 45].

tab8
Table 8: Synergism parameter ( ) for the various halides at 30 and 60°C.

4. Conclusion

B. nitida leaf extract inhibited mild steel corrosion in 1 M H2SO4 and 2 M HCl at the temperatures studied. Inhibition efficiency increased with increase in BN extract concentration and synergistically increased in the presence of halide ions. Temperature studies revealed a decrease in inhibition efficiency with rise in temperature and corrosion activation energies being higher in the presence of the plant extract. Comparative analyses of the results from both acid solutions suggest that protonated species in the extract play a predominant role in inhibitive behavior observed, with the predominant effect being the physical adsorption of protonated species.

Conflict of Interests

The authors declare that there is no conflict of interests regarding the publication of this paper.

References

  1. E. S. Ferreira, C. Giacomelli, F. C. Giacomelli, and A. Spinelli, “Evaluation of the inhibitor effect of L-ascorbic acid on the corrosion of mild steel,” Materials Chemistry and Physics, vol. 83, no. 1, pp. 129–134, 2004. View at Publisher · View at Google Scholar · View at Scopus
  2. D. A. Jones, Principles and Prevention of Corrosion, Prentice Hall, Upper Saddle River, NJ, USA, 2nd edition, 1996.
  3. M. G. Fontana, Corrosion Engineering, McGraw-Hill, Singapore, 3rd edition, 1986.
  4. A. Popova, M. Christov, and T. Deligeorgiev, “Influence of the molecular structure on the inhibitor properties of benzimidazole derivatives on mild steel corrosion in 1M hydrochloric acid,” Corrosion, vol. 59, no. 9, pp. 756–764, 2003. View at Scopus
  5. E. E. Oguzie, C. K. Enenebeaku, C. O. Akalezi, S. C. Okoro, A. A. Ayuk, and E. N. Ejike, “Adsorption and corrosion-inhibiting effect of Dacryodis edulis extract on low-carbon-steel corrosion in acidic media,” Journal of Colloid and Interface Science, vol. 349, no. 1, pp. 283–292, 2010. View at Publisher · View at Google Scholar · View at Scopus
  6. A. R. Hosein Zadeh, I. Danaee, and M. H. Maddahy, “Thermodynamic and adsorption behaviour of medicinal nitramine as a corrosion inhibitor for AISI steel alloy in HCl solution,” Journal of Materials Science and Technology, vol. 29, no. 9, pp. 884–892, 2013. View at Publisher · View at Google Scholar · View at Scopus
  7. I. Lukovists, E. Kalman, and F. Zuchi, “Corrosion inhibitors-correlation between electronic structure and efficiency,” Corrosion, vol. 57, no. 1, pp. 3–8, 2001. View at Publisher · View at Google Scholar
  8. P. Mohan and G. P. Kalaignan, “1, 4-Bis (2-nitrobenzylidene) thiosemicarbazide as effective corrosion inhibitor for mild steel,” Journal of Materials Science & Technology, vol. 29, no. 11, pp. 1096–1100, 2013. View at Publisher · View at Google Scholar
  9. E. E. Oguzie, V. O. Njoku, C. K. Enenebeaku, C. O. Akalezi, and C. Obi, “Effect of hexamethylpararosaniline chloride (crystal violet) on mild steel corrosion in acidic media,” Corrosion Science, vol. 50, no. 12, pp. 3480–3486, 2008. View at Publisher · View at Google Scholar · View at Scopus
  10. E. E. Oguzie, “Inhibition of acid corrosion of mild steel by Telfaria occidentalis,” Pigment and Resin Technology, vol. 34, no. 6, pp. 321–326, 2005. View at Publisher · View at Google Scholar · View at Scopus
  11. N. O. Eddy, P. A. Ekwumemgbo, and P. A. P. Mamza, “Ethanol extract of Terminalia catappa as a green inhibitor for the corrosion of mild steel in H2SO4,” Green Chemistry Letters and Reviews, vol. 2, no. 4, pp. 223–231, 2009. View at Publisher · View at Google Scholar · View at Scopus
  12. E. S. H. El Ashry, A. El Nemr, S. A. Esawy, and S. Ragab, “Corrosion inhibitors. Part II: quantum chemical studies on the corrosion inhibitions of steel in acidic medium by some triazole, oxadiazole and thiadiazole derivatives,” Electrochimica Acta, vol. 51, no. 19, pp. 3957–3968, 2006. View at Publisher · View at Google Scholar · View at Scopus
  13. M. Lebrini, F. Bentiss, H. Vezin, and M. Lagrenée, “The inhibition of mild steel corrosion in acidic solutions by 2,5-bis(4-pyridyl)-1,3,4-thiadiazole: structure-activity correlation,” Corrosion Science, vol. 48, no. 5, pp. 1279–1291, 2006. View at Publisher · View at Google Scholar · View at Scopus
  14. S. E. Manahan, Environmental Chemistry, CRC Press, Boca Raton, Fla, USA, 1999.
  15. E. E. Oguzie, “Studies on the inhibitive effect of Occimum viridis extract on the acid corrosion of mild steel,” Materials Chemistry and Physics, vol. 99, no. 2-3, pp. 441–446, 2006.
  16. O. K. Abiola, J. O. E. Otaigbe, and O. J. Kio, “Gossipium hirsutum L. extracts as green corrosion inhibitor for aluminum in NaOH solution,” Corrosion Science, vol. 51, no. 8, pp. 1879–1881, 2009. View at Publisher · View at Google Scholar · View at Scopus
  17. A. K. Satapathy, G. Gunasekaran, S. C. Sahoo, K. Amit, and P. V. Rodrigues, “Corrosion inhibition by Justicia gendarussa plant extract in hydrochloric acid solution,” Corrosion Science, vol. 51, no. 12, pp. 2848–2856, 2009. View at Publisher · View at Google Scholar · View at Scopus
  18. S. K. Sharma, A. Mudhoo, G. Jain, and J. Sharma, “Corrosion inhibition and adsorption properties of Azadirachta indica mature leaves extract as green inhibitor for mild steel in HNO3,” Green Chemistry Letters and Reviews, vol. 3, p. 7, 2010.
  19. E. I. Ating, S. A. Umoren, I. I. Udousoro, E. E. Ebenso, and A. P. Udoh, “Leaves extract of ananas sativum as green corrosion inhibitor for aluminium in hydrochloric acid solutions,” Green Chemistry Letters and Reviews, vol. 3, no. 2, pp. 61–68, 2010. View at Publisher · View at Google Scholar · View at Scopus
  20. N. D. Onwukaeme, “Anti-inflammatory activities of flavonoids of Baphia nitida Lodd. (Leguminosae) on mice and rats,” Journal of Ethnopharmacology, vol. 46, no. 2, pp. 121–124, 1995. View at Publisher · View at Google Scholar · View at Scopus
  21. A. I. Onuchukwu, “Corrosion inhibition of aluminum in alkaline medium. I: influence of hard bases,” Materials Chemistry and Physics, vol. 20, no. 4-5, pp. 323–332, 1988. View at Publisher · View at Google Scholar
  22. A. Popova, E. Sokolova, S. Raicheva, and M. Christov, “AC and DC study of the temperature effect on mild steel corrosion in acid media in the presence of benzimidazole derivatives,” Corrosion Science, vol. 45, no. 1, pp. 33–58, 2003. View at Publisher · View at Google Scholar · View at Scopus
  23. B. Muller, “Corrosion inhibition of aluminium and zinc pigments by saccharides,” Corrosion Science, vol. 44, pp. 1583–1591, 2002. View at Publisher · View at Google Scholar
  24. A. Aytac, U. Ozmen, and M. Kabasakaloglu, “Investigation of some Schiff bases as acidic corrosion of alloy AA3102,” Materials Chemistry and Physics, vol. 89, no. 1, pp. 176–181, 2005. View at Publisher · View at Google Scholar
  25. E. E. Ebenso and E. E. Oguzie, “Corrosion inhibition of mild steel in acidic media by some organic dyes,” Materials Letters, vol. 59, no. 17, pp. 2163–2165, 2005. View at Publisher · View at Google Scholar · View at Scopus
  26. M. N. Moussa, A. S. Fouda, A. I. Taha, and A. Elnenaa, “Some Thiosemicarbazide derivatives as corrosion inhibitors for aluminium in sodium hydroxide solution,” Bulletin of the Korean Chemical Society, vol. 9, no. 4, pp. 191–195, 1988.
  27. A. Y. El-Etre, “Inhibition of aluminum corrosion using Opuntia extract,” Corrosion Science, vol. 45, no. 11, pp. 2485–2495, 2003. View at Publisher · View at Google Scholar · View at Scopus
  28. M. Abdallah, “Antibacterial drugs as corrosion inhibitors for corrosion of aluminium in hydrochloric solution,” Corrosion Science, vol. 46, no. 8, pp. 1981–1996, 1981.
  29. E. E. Oguzie, Y. Li, and F. H. Wang, “Effect of surface nanocrystallization on corrosion and corrosion inhibition of low carbon steel: synergistic effect of methionine and iodide ion,” Electrochimica Acta, vol. 52, no. 24, pp. 6988–6996, 2007. View at Publisher · View at Google Scholar · View at Scopus
  30. M. S. S. Morad, A. E. A. Hermas, and M. S. Abdel Aal, “Effect of amino acids containing sulfur on the corrosion of mild steel in phosphoric acid solutions polluted with Cl, F and Fe3+ ions–behaviour near and at the corrosion potential,” Journal of Chemical Technology and Biotechnology, vol. 77, pp. 486–494, 2002. View at Publisher · View at Google Scholar
  31. K. Orubite-Okorosaye and N. C. Oforka, “Corrosion inhibition of zinc on HCl using Nypa fruticans Wurmb extract and 1,5 diphenyl carbazone,” Journal of Applied Sciences & Environmental Management, vol. 8, pp. 56–61, 2004.
  32. S. Martinez and M. Matikos-Hukovic, “A nonlinear kinetic model introduced for the corrosion inhibitive properties of some organic inhibitors,” Journal of Applied Electrochemistry, vol. 33, pp. 1137–1142, 2003.
  33. T. Zhao and G. Mu, “The adsorption and corrosion inhibition of anion surfactants on aluminium surface in hydrochloric acid,” Corrosion Science, vol. 41, no. 10, pp. 1937–1944, 1999. View at Publisher · View at Google Scholar
  34. M. Bouklah, B. Hammouti, M. Lagrenée, and F. Bentiss, “Thermodynamic properties of 2,5-bis(4-methoxyphenyl)-1,3,4-oxadiazole as a corrosion inhibitor for mild steel in normal sulfuric acid medium,” Corrosion Science, vol. 48, no. 9, pp. 2831–2842, 2006. View at Publisher · View at Google Scholar
  35. W. Durnie, R. de Marco, A. Jefferson, and B. Kinsella, “Development of a structure-activity relationship for oil field corrosion inhibitors,” Journal of the Electrochemical Society, vol. 146, no. 5, pp. 1751–1756, 1999. View at Publisher · View at Google Scholar · View at Scopus
  36. S. Martinez and I. Stern, “Thermodynamic characterization of metal dissolution and inhibitor adsorption processes in the low carbon steel/mimosa tannin/sulfuric acid system,” Applied Surface Science, vol. 199, no. 1–4, pp. 83–89, 2002. View at Publisher · View at Google Scholar
  37. G. Mu and X. Li, “Inhibition of cold rolled steel corrosion by Tween-20 in sulfuric acid: Weight loss, electrochemical and AFM approaches,” Journal of Colloid and Interface Science, vol. 289, pp. 184–192, 2005. View at Publisher · View at Google Scholar
  38. O. Olivares, N. V. Likhanova, B. Gómez et al., “Electrochemical and XPS studies of decylamides of α-amino acids adsorption on carbon steel in acidic environment,” Applied Surface Science, vol. 252, no. 8, pp. 2894–2909, 2006. View at Publisher · View at Google Scholar · View at Scopus
  39. A. I. Onuchukwu and S. P. Trasatti, “Hydrogen permeation into aluminium AA1060 as a result of corrosion in an alkaline medium. Influence of anions in solution and of temperature,” Corrosion Science, vol. 36, no. 11, pp. 1815–1817, 1994. View at Publisher · View at Google Scholar · View at Scopus
  40. E. E. Oguzie, G. N. Onuoha, and A. I. Onuchukwu, “Inhibitory mechanism of mild steel corrosion in 2 M sulphuric acid solution by methylene blue dye,” Materials Chemistry and Physics, vol. 89, no. 2-3, pp. 305–311, 2005. View at Publisher · View at Google Scholar · View at Scopus
  41. G. K. Gomma, “Corrosion of low-carbon steel in sulphuric acid solution in presence of pyrazole—halides mixture,” Materials Chemistry and Physics, vol. 55, no. 3, pp. 241–246, 1998. View at Publisher · View at Google Scholar
  42. E. E. Ebenso, “Synergistic effect of halide ions on the corrosion inhibition of aluminium in H2SO4 using 2-acetylphenothiazine,” Materials Chemistry and Physics, vol. 79, no. 1, pp. 58–70, 2003. View at Publisher · View at Google Scholar
  43. E. E. Oguzie, “Evaluation of the inhibitive effect of some plant extracts on the acid corrosion of mild steel,” Corrosion Science, vol. 50, no. 11, pp. 2993–2998, 2008. View at Publisher · View at Google Scholar · View at Scopus
  44. K. Aramaki and N. Hackermann, “Inhibition mechanism of medium-sized polymethyleneimine,” Journal of the Electrochemical Society, vol. 116, no. 5, pp. 568–574, 1969. View at Publisher · View at Google Scholar
  45. L. Tang, X. Li, G. Mu et al., “The synergistic inhibition between hexadecyl trimethyl ammonium bromide (HTAB) and NaBr for the corrosion of cold rolled steel in 0.5 M sulfuric acid,” Journal of Materials Science, vol. 41, pp. 3063–3069, 2006. View at Publisher · View at Google Scholar