Synergistic Combination Effect of Green Organic Derivatives on the Corrosion Inhibition of Mild Steel in Simulated Seawater

Introduction

The corrosion process results in deterioration of the surface properties and metallic substrate of carbon steels. Corrosion initiates at flaws on the oxide film formed on the steel. The flaws are the products of discontinuities in the film, presence of impurities, inclusions and mechanical damage. In corrosive environments oxidation reactions occurs at the flaws resulting in the release of electron radicals, ferrous ions and eventual breakdown of the steel. The free electrons participate in the reduction reactions occurring at the metal/electrolyte interface where dissolved oxygen are present especially in aerated conditions, resulting in the formation of hydroxyl ions. Reaction between the hydroxyl and ferrous ions results in ferrous hydroxide, which transforms to hydrated oxide known as rust. The porosity of the hydrated oxide allows the continuity of the corrosion process leading to insidious degeneration and general surface deterioration of the steel¹. The corrosion process is influenced by a number of factors such as types of corrosive species, presence of alloying elements, strength of the protective oxide film, temperature, amount of oxygen present, velocity of flow of the corrosive environment, extent of impurities etc.² Despite the weak resistance of carbon steel to corrosion, it has extensive industrial application across most industries representing about 85% of the annual steel production worldwide due to their low cost, ready availability and good mechanical strength. Carbon steel corrosion is detrimental most especially in the presence of chlorides. Chlorides are majorly involved in corrosion reactions and kinetics of the corrosion process. Marine environments have abundance of chloride anions hence the serious debilitating effect of corrosion encountered metal alloys in such environments. The corrosion exists in different forms such as pitting, galvanic, cavitation and general corrosion. According to NACE the estimated cost of marine corrosion worldwide is about $80 billion yearly.³ Corrosion prevention by chemical compounds known as inhibitors has been proven to be one of the most feasible, reliable and cost effective methods.⁴ Most corrosion inhibitors are organic derivatives consisting of heteroatoms and multiple bonds enabling strong intermolecular attraction and adsorption in the presence of corrosive anions.^5,6 Research on the use of corrosion inhibitors is geared toward the application of cost effective environmentally sustainable organic derivatives. Previous individual research on the corrosion inhibition effect of leucine and vanillin compounds have been done in acid solution with above average results.^7-12 The purpose of this study is to assess the adsorption and corrosion inhibition performance of leucine and vanillin admixture on mild steel in 3.5% NaCl solution.

Experimental Methods

Mild steel (MS) obtained the open market and analysed  at the Materials Characterization Laboratory, Department of Mechanical Engineering, Covenant University, Ota, Ogun State, Nigeria gave nominal (wt. %) composition shown in Table 1. The mild steel is of cylindrical configuration with a diameter of 1.2 cm². The steel was machined, sectioned and smoothened with silicon grinding papers (80, 320, 600, 800 and 1000 grits), after with cleansed washing with deionized H₂O and methyl-ketone. Leucine sourced from Sigma Aldrich, USA is a white powdered substance (molecular formular C₆H₁₃NO₂ and molecular weight 131.17 g/mol). Its molecular structure is shown in Fig. 1(a). Vanillin is a phenolic aldehyde (molecular formular C₈H₈O₃ and molecular weight 152.15 g/mol). Its molecular structure is shown in Fig. 1(b). The admixed compound (LEV) was prepared in molar concentrations of 1.76 x 10², 3.53 x 10², 5.29 x 10², 7.06 x 10², 8.82 x 10², 1.06 x 10¹ per 200 mL of 3.5% NaCl solution. Potentiodynamic polarization analysis was performed at 35^°C with a triple electrode system (platinum counter electrode, Ag/AgCl reference electrode and resin mounted MS with exposed surface area of 1.13 cm³) in 200 mL of the electrolyte within a transparent cell connected to Digi-Ivy 2311 potentiostat and interface with a computer. Graphs were produced at a scan rate of 0.0015 V/s between potentials of -1.25 V and +1.5 V. Morphological representations of corroded and LEV inhibited MS morphology were studied after electrochemical analysis with Omax trinocular. Open circuit potential measurement (OCP) was done at 0.05 V/s step potential for 3000s to obtain information on thermodynamic stability and electrochemical equilibrium of 1070AL/SiC without applied potentials.

Table 1: Composition (wt. %) of Mild steel

Element Symbol	C	Si	Mn	P	S	Cu	Ni	Al	Fe
% Composition	0.401	0.169	0.440	0.005	0.012	0.080	0.008	0.025	98.86

 

Figure 1: Molecular structure of (a) Leucine and (b) Vanillin Click here to View figure

 

Result and Discussion

Potentiodynamic Polarization

The potentiodynamic polarization plots indicating the anodic-cathodic behavior of MS in LEV /3.5%NaCl solution is shown in Fig. 2. Table 2 depicts the results of inhibition efficiency (Υ), corrosion rate (C_R), corrosion current (C_I), corrosion current density (C_ID), corrosion potential (C_P), polarization resistance (R_P), anodic Tafel slope (B_a) and cathodic Tafel slope (B_c) from the polarization test. MS at 0% and 0.5% LEV severely deteriorated in the presence of Cl^– ions attaining corrosion rate values of 2 mm/y and 1.99 mm/y. The corrosion reaction process takes place when MS loses electrons, releasing ferrous cations into the solution which transforms into ferric cations. The cathodic reaction in aerated condition occurs through oxygen reduction by gaining electron radicals. The corrosion reaction process causes the formation rust oxides on MS surface; however the porosity of the oxide formed allows Cl^– ions to penetrate easily through the oxide layer. This allows the corrosion reaction mechanism responsible for anodic degradation to continue causing deeper attack on the steel substrate and releasing more Fe⁺ ions into the electrolyte. LEV at 0.5% was unable to inhibit the corrosion of MS due to insufficient protonated molecules to oppose the deterioration effect of Cl^– ions. As a result the change in corrosion rate and corrosion current density is marginal, though. The anodic tafel slope value decreased from 16.140 mm/y to 13.630 mm/y as a result of decrease in anodic current density resulting from metal dissolution reactions on the steel surface. The C_ID values decreased with increment in LEV concentration and hence the inhibitor protection value (Table 2) due to the adsorption reaction on MS surface. At 1% – 2% LEV, the corrosion rate has decreased to values between 0.96 mm/y and 0.75 mm/y corresponding to inhibition efficiencies of 51.84%, 55.45% and 62.73% respectively due to the availability of sufficient LEV molecules to inhibition the electrochemical action of chlorides. It shows the inhibition performance of LEV is concentration dependent. While changes in the cathodic Tafel slope a marginal a significant decrease in anodic Tafel slope was observed beyond 0.5% LEV due to decrease in anodic reactions on the steel, however changes in anodic Tafel slope vales from 1% LEV to 2% LEV are quite negligible.

Observation of the polarization plot shows the cathodic branches of the plot with respect to LEV concentration are quite similar indicating the cathodic reaction mechanism involving oxygen reduction and production of hydroxyl ions is under activation control. The anodic branch of the polarization plot at 0% LEV and 0.5% LEV were linear due to oxidation reaction on MS surface causing the release of Fe²⁺ ions into the electrolyte as earlier mention, however beyond 0.5% LEV short passivation behavior was observed to inhibiting action of LEV compound. It shows the inhibition mechanism is through surface coverage whereby the reactive sites of the steel surface are enveloped by LEV molecules whereby suppressing the oxidation reactions. At 2.5% LEV and 2% LEV, the inhibition efficiency has attained values of 80.85% and 89% respectively signifying effective inhibition of MS corrosion. The maximum change in corrosion potential of MS between 0% LEV and 1% LEV in the reduction reaction direction is 81 mV thus it is a mixed type inhibitor.¹³

Figure 2: MS corrosion polarization plots from 3.5% NaCl/0% – 2.5% LEV. Click here to View figure

 

Table 2: Results of potentiodynamic polarization test of MS corrosion in 3.5% NaCl/0% – 2.5% LEV.

Sample	LEV Conc. (%)	LEV Conc. (M)	MS CR (mm/y)	LEV γ, (%)	CI (A)	CID (A/cm2)	CP (V)	Rp (Ω)	Bc (V/dec)	Ba (V/dec)
A	0	0	2.00	0	1.95E-04	1.73E-04	-0.593	116.00	-4.167	16.140
B	0.5	1.76E-02	1.99	0.73	1.93E-04	1.71E-04	-0.604	108.00	-6.002	13.630
C	1	3.53E-02	0.96	51.84	9.38E-05	8.30E-05	-0.674	273.80	-6.573	5.744
D	1.5	5.29E-02	0.89	55.45	8.68E-05	7.68E-05	-0.659	296.00	-7.401	7.001
E	2	7.06E-02	0.75	62.73	7.26E-05	6.42E-05	-0.634	353.90	-6.639	6.681
F	2.5	8.82E-02	0.38	80.85	3.73E-05	3.30E-05	-0.586	688.90	-4.579	6.306
G	3	1.06E-01	0.22	89.00	2.14E-05	1.90E-05	-0.651	759.70	-6.560	6.010

 

Mechanism of LEV Inhibition

LEV consisting of leucine and vanillin are compounds consisting of organic molecules which adsorbs on the metallic surface during corrosion inhibition reactions, as a result hinders metal oxidation through blockage of the cathodic and/or anodic half-cell reactions. These compounds form precipitates with metal cations on the ionized metal surface.¹⁴ Observation of the inhibition reaction mechanism in the presence of LEV shows passivation resulting from film formation (surface coverage) of protonated LEV molecules occurred on MS surface as evident on the anodic branch of the polarization plots. This is further confirmed from the increase  in surface coverage with increase in LEV concentration which shows amount of LEV molecules present significantly influence the corrosion of MS.¹⁵ Most organic compounds are electrons and when in the vicinity of electron acceptor metallic atoms donor–acceptor interchange occurs among the heteroatoms of LEV and the empty‘d’ orbitals of MS. This process does occur through chemisorption reaction mechanisms and or through electrostatic interaction between the molecular species.

Open Circuit Potential Measurement

The thermodynamic stability of MS in 3.5% NaCl/0%, 0.5% and 3% LEV is shown in the variation of OCP versus exposure time (Fig. 3.). MS at 3.5% NaCl/0% LEV generally depicts the most electronegative results due to redox electrochemical processes on the steel surface. At 26.45 s its OCP value is most electronegative (-0.680 V) due to active corrosion of the steel. The OCP progress sharply at short time interval to -0.503 V at 200 s due to short instantaneous passivation of the steel resulting from the formation of surface oxide, however the oxide formed are porous in nature, as a result the OCP immediately decreased to -0.551 V at 500 s before remaining marginally stable till 750.01 s (-0.554 V. Beyond this point the OCP values of MS at 3.5% NaCl/0% LEV continue to decrease till 3200 s. The presence of LEV at 0.5% concentration caused an instantaneous increase in OCP due to marginal passivation of MS 250 s at -0.559 V, beyond which the OCP value remained thermodynamically stable and at higher OCP values than MS at 0% LEV. At 3% LEV the OCP value of MS starting at -0.605 V (0 s) increased to -0.460 V at 300 s due to the corrosion inhibiting action of LEV. A progressive but stable marginal decrease later occurred till the end of the OCP test. It must be noted that MS at 3% is significantly more anodic than its counterparts due to interdiction of the oxidation-reduction reactions. The relatively positive values of MS at this concentration shows surface coverage by LEV molecules protected the steel.

Figure 3: Variation of MS OCP values versus exposure time in 3.5% NaCl/LEV compound Click here to View figure

Adsorption Isotherm Studies

Adsorption of inhibitor molecules onto metallic surfaces results from the electrostatic between them. Adsorption isotherms are graphical plots showing the amount of inhibitor molecules on metallic surfaces with respect to its concentration at fixed temperature. Langmuir, Frumkin and Freundlich isotherm models produced significantly high correlation coefficients amongst other isotherms evaluated to further understand the nature of LEV adsorption and corrosion inhibition of MS¹⁶. Langmuir isotherm states that in the presence of one adsorbate, metallic surfaces has fixed amount of adsorption sites with equal value of Gibbs free energy irrespective of the configuration of molecular arrangement and the effect of lateral synergy among the adsorbed inhibitor is negligible. Fig. 4 shows the graphical illustration of

at correlation coefficient of 0.8024 with respect to Langmuir equation below.

θ is the sum of LEV a assimilated per unit gram on MS surface at constant temperature. C_LEV is LEV concentration and K_LEV is the equilibrium constant of adsorption. Frumkin isotherm states that surface coverage values is subject to the electrode potential resulting from changes in the energy of the double-layer capacitor due to the substitution of H₂O molecules by organic molecules of organic compounds with having a lower dielectric constant. The metallic surfaces are non-homogeneous and the result of lateral synergy is important with respect to the equation below:

α is the lateral synergism parameter determined from the gradient of the graphical illustration of the Frumkin isotherm. K is the adsorption-desorption constant. Graph of

Against θ in Fig. 5(a) 0.9813 correlation coefficient. The Freundlich adsorption isotherm gives the experimental relationship between the amount of adsorbed inhibitor molecules by the unit mass of metal and concentration at a constant temperature according to the equation below. The Freundlich isotherm graph for LEV adhesion and assimilation in Fig. 5(b) gave 0.7570 correlation coefficient value. The equations below align with the Freundlich isotherm;

θ = KCⁿ                                                                                   (3)

log θ = n log C + log K_ads                                                     (4)

n is a constant subject to the properties of the inhibitor molecules involved in the adsorption reaction. K_ads is the adsorption–desorption equilibrium constant showing the adsorption strength.

Figure 4: Click here to View figure

 

Figure 5a: Click here to View figure

 

Thermodynamics of inhibitor adsorption

Gibbs free energy data values determined from equation 5 below are depicted in Table 3.

ΔG_ads = – 2.303RT log [55.5K_LTC]                                                 (5)

5.5 is the molar concentration of H₂O, R is the ideal gas constant, T is the thermodynamic temperature and K_LEV is the equilibrium constant of LEV adsorption on MS. The negative values of ΔG^o_ads results show the unconstrained nature and cohesion of adsorption. The highest ΔG^o_ads value obtained is -20.70 KJmol^-1 while the lowest significant ΔG^o_ads value obtained is -18.42 KJmol^-1. The ΔG^o_ads values shows the mechanism of adsorption is through physical attraction which shows that surface coverage of the inhibiting compound hinders the movement of the corrosive anions.^13,17

Table 3: Gibbs free energy (ΔG^o_ads), surface coverage (θ) and equilibrium constant of adsorption (K_ads) data for LEV adsorption on MS

Sample	LEV Concentration (M)	Surface Coverage (θ)	Equilibrium Constant of adsorption (K)	Gibbs Free Energy, ∆G (Kjmol-1)
A	0	0	0	0
B	1.76E-02	0.007	0.42	-7.79
C	3.53E-02	0.518	30.49	-18.42
D	5.29E-02	0.555	23.53	-17.78
E	7.06E-02	0.627	23.84	-17.81
F	8.82E-02	0.809	47.87	-19.54
G	1.06E-01	0.890	76.33	-20.70

 

Morphological studies

Morphological representations of MS before corrosion and after corrosion in 3.5% NaCl/0%, 0.5% and 3% LEV solution from optical microscopy (mag. x40 and x100) are shown from Fig. 6(a) to 7(b). The morphology of MS in Fig. 6(b) significantly contrast the morphology in Fig 6(a) due to the debilitating action of Cl^– ions as earlier discussed in the section under polarization studies. Numerous conjoined and enlarged corrosion pits in addition to general surface deterioration are clearly visible with iron oxides as corrosion product. Addition of LEV at 0.5% concentration [Fig. 7(a)] did not offer any significant protection. General corrosion seems to have been inhibited however the corrosion pits on the surface appears larger. The MS morphology at 3% LEV [Fig. 7(b)] shows a remarkable improvement in comparison the earlier observed surfaces due to the inhibitive action of LEV, though mild deterioration is visible, it is superficial in nature as the integrity of the surface properties of MS is still intact. The superficial deterioration is probably due to initial attack by the Cl^– ions before adsorption of the protonated inhibitor molecules which prevents further attack on the steel. However taking cue from adsorption isotherm studies it is also probable that lateral attraction between the inhibitor molecules results in an envelope covering (protective film) over the entire steel surface whereby the bulk of Cl^– ions cannot diffuse through.

Figure 6: Optical images of MS at mag. x 40 and x 100 (a) MS morphology before corrosion, (b) MS morphology after corrosion in 3.5% NaCl Click here to View figure

 

Figure 7: Optical images of MS at mag. x40 and x100 (a) MS morphology after corrosion in 3.5% NaCl/0.5% LEV, (b) MS morphology after corrosion in 3.5% NaCl/3% LEV Click here to View figure

 

Conclusion

The combined admixture of leucine and vanillin effectively inhibited the corrosion of mild steel in 3.5% NaCl solution with maximum inhibition efficiency above 85%. The inhibition mechanism was through surface coverage whereby inhibitor molecules formed a protective film over the steel surface. This caused a large anodic shift in corrosion potential from opencircuit potential analysis however, thermodynamic calculations show physisorption interaction between the protonated inhibitor molecules and the ionized steel surface occurred. Severe morphological deterioration of the steel with inhibitor compound significantly contrasts the morphology of the inhibited steel.

Acknowledgement

The author acknowledges Covenant University Ota, Ogun State, Nigeria for the sponsorship and provision of research facilities for this project.

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