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. 2021 Jan 29;6(6):4300–4312. doi: 10.1021/acsomega.0c05476

Corrosion Inhibition of Carbon Steel in Hydrochloric Acid Solution Using Ethoxylated Nonionic Surfactants Based on Schiff Base: Electrochemical and Computational Investigations

Ahmed G Bedir †,‡, Mohamed Abd El-raouf †,‡,*, Samah Abdel-Mawgoud §, Nabel A Negm †,‡, N M El Basiony †,‡,*
PMCID: PMC7893636  PMID: 33623841

Abstract

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Two ethoxylated nonionic surfactants (L400 and L600) based on Schiff base are prepared from polyoxyethylene, glyoxalic acid, and phenylenediamine. They are evaluated electrochemically as carbon steel corrosion inhibitors in 1 M HCl by electrochemical impedance spectroscopy (EIS) and Tafel techniques and complemented with microscopic analysis methods. The obtained Tafel data indicate the mixed-type behavior of the inhibitor used. The inhibition efficiency touches the peak at 1 × 10–4 M, exhibiting 92 and 94% for L400 and L600, respectively. The presence of the tested inhibitors decreases corrosion current density (icorr) and double-layer capacitance (Cdl) due to the formation of a protective adsorption layer in place of the already adsorbed water and aggressive Cl– ions. Both L400 and L600 adsorption modes follow Langmuir adsorption isotherm. The density functional theory (DFT) calculated indices (ΔEgap and EHOMO) indicate the superiority of L600 over the L400 counterpart as a reactive compound. Adsorption of L600 and L400 over the Fe(1 1 0) in simulated acidic medium is investigated by Monte Carlo (MC) simulation to verify their inhibition performance and are matched with adsorption free energy ΔGads calculated values. Both experimental and theoretical data are in agreement.

1. Introduction

Carbon steel is frequently used in innumerable engineering and manufacturing applications, including design and construction, as it has some excellent mechanical–chemical properties. However, one of the major dilemmas of using carbon steel is its susceptibility to corrosion.1−3 Corrosion of carbon steel is an unavoidable but controllable process. Inhibitors are considered one of the essential additives tools to protect carbon steel corrosion. The acid pickling process is a common industrial cleaning process in petrochemical production and oil-well practices to remove mineral oxides and mineral scale depositions. Still, this process must be controllable due to the highly destructive corrosion effect of mineral acid used (HCl).4 Eco-friendly organic inhibitor applications have emerged to meet the environmental demands. Therefore, inorganic inhibitors (such as chromates, molybdates, phosphates, and nitrates) are extensively used in the corrosion protection of metal/alloys (e.g., X65 carbon steel), which are replaced despite their high efficiency.5−8 Organic surfactants, besides their eco-friendly and biodegradable features, also have corrosion inhibition feature. They have high electron density centers (N, P, and π electrons), which allows their adsorption over the metallic surface and shields the metal surface from the corrosive media.9−11 We can find that recent trends of publications of environmental and eco-friendly corrosion inhibitors, according to the Sci-Finder database, are estimated to be 50% of the total publications of the corrosion inhibitors. Therefore, many researchers have focused on using environmental and eco-friendly inhibitors. Also, many researchers have focused on using nonionic inhibitors; for example, Al-Abdali et al. studied nonionic surfactants containing six-membered rings as oxazine;12 Fouda et al. studied HENPEM surfethoxymer;13 Shaban et al. studied nonionic dithiol surfactants (SH600);14 Al-Sabagh et al. studied nonionic surfactants based on amino acid (S1);15 and Abdallah et al. studied 4-(3,6,9,12-tetraoxatetracosyloxy) phenol,16 which achieved an inhibition efficiency in the range from 31 up to 91%. The recently studied compounds achieved a good antimicrobial activity as evaluated elsewhere; also, the compounds are enriched with high electron density centers, which results in their high-potential applications as eco-friendly corrosion inhibitors with high efficiency, which reached 94%. In this work, we focused on the previously synthesized nonionic surfactants (L400 and L600) as acid corrosion inhibitors for X65 carbon steel, which acts as a surface-active agent with good surface activity as well as a multifunctional compound. The chemical composition of the prepared molecules is mainly formed from poly(ethylene glycol) (PEG) and oleic acid, which have an eco-friendly behavior.17 These characteristics give them the potentiality to act as novel corrosion inhibitors. The study included electrochemical tests such as electrochemical impedance spectroscopy (EIS) and potentiodynamic polarization (Tafel), complemented with surface morphology study (scanning electron microscopy (SEM) and energy-dispersive X-ray analysis (EDX)). The computational studies via density functional theory (DFT) and Monte Carlo simulations (MC) on the (1 1 0) Fe crystal were performed to confirm and support the experimental data.18−20

2. Experimental Section

2.1. Corrosion Test

2.1.1. Solution

Diluted 1 M HCl from 37% HCl is the tested aggressive media. The tested inhibitors’ concentrations are in the range 1 × 10–6 to 1 × 10–4 M and are freshly prepared using bidistilled water.21

2.1.2. Metal Alloy X65 Steel

Elemental analysis of X65 used as a working electrode in wt % was 0.103 C; 0.210 Si; 0.024 P; 1.05 Mn; 0.012 Ni; 0.032 Co; and Fe balance.

2.2. Electrochemical Measurements

Auto-lab (PGSTAT128N) potentiostat/galvanostat with NOVA 2.1.4 software was used to perform the electrochemical corrosion tests at room temperature. The three-electrode system in a jacketed glass cell consisted of X65, Ag/AgCl (3 M KCl), and Pt as the working, reference, and auxiliary electrodes, respectively. The working electrode was mounted with the epoxy resin where the surface area exposed to the tested aggressive media was 0.283 cm2. The exposed area was polished with different grades of SiC papers until 2500 to obtain a mirror image surface before each run. The electrochemical tests were conducted after 30 min of immersion in a tested solution.22 The EIS measurements were conducted within the frequency range of 100 kHz to 0.1 Hz under potentiostatic conditions at an open-circuit potential (OCP) and an amplitude of 10 mV. The potentiodynamic polarization responses were sought without and with the addition of various concentrations of corrosion inhibitors (1 × 10–6, 5 × 10–6, 1 × 10–5, 5 × 10–5, and 1 × 10–4 M) for the tested (L400 and L600) compounds in 1 M HCl solution at 25 °C, while adopting a scan rate of 1 mV/s. Potentiodynamic sweeps were ±1 V vs OCP.23 The inhibition efficiency (IE) and the surface coverage degree (θ) for EIS and Tafel data were calculated using eqs 1–424

2.2. 1
2.2. 2
2.2. 3
2.2. 4

where Rct(o) and Rct(i) are the charge-transfer resistances of C-steel in the absence and presence of inhibitors, respectively. icorr(o) and icorr(i) are the corrosion current densities of the steel specimen (A·cm–2) in the absence and presence of different concentrations of the tested compounds (L400 and L600), respectively. Each electrochemical test was duplicated twice and the mean value was taken.

2.3. Surface Analysis Study

The aggressive action of HCl on the X65 surface was imaged in the absence and presence of 1 × 10–4 M of L600 after 3 h of treatment using SEM and EDX with the help of QUANTA FEG-250 at CMRDI.25

2.4. Quantum Calculation Method

Recently, theoretical calculations are necessary to simulate the experimental data. Quantum chemical calculations were done using Material Studio (MS 6.0; Accelrys) software in a vacuum and solvated phases. To study the chemical reactivity of L400 and L600 compounds, we apply the DMOL3 module based on the gradient-corrected functional (GGA) method with Becke One Parameter (BOP) and double numerical polarized (DNP) basis set group functional was done. The tested method gives the following quantum parameters of energy gap (ΔE), fraction of electron transfer (ΔN), dipole moment (μ), absolute electronegativity (χ), ionization energy (I), hardness (η), and softness (σ) for the prepared compounds L400 and L600 in both gas and solvated phases. The adsorption energy of the tested compound on Fe is induced from the MC simulation with the aid of the adsorption locator module in the same software. The MC simulation has been done in gas and solution simulated phases of the tested acidic (HCl) medium.26,27

3. Results and Discussion

3.1. Tafel

The electrochemical kinetic parameters of the corrosion and corrosion inhibition of the X65 carbon steel have been obtained from the Tafel polarization data in the absence and presence of different concentrations of the prepared nonionic surfactant compounds, which have different in an in situ number of ethylene oxide units (L400 and L600) are exported from Figure 1a1,a2.

Figure 1.

Figure 1

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(a1) Polarization curves of the X65 steel in 1 M HCl in the absence and presence of different concentrations of the L400 inhibitor. (a2) Polarization curves of the X65 steel in 1 M HCl in the absence and presence of different concentrations of the L600 inhibitor. (b) Relation between C.R., Rp, and inhibitor concentrations.

Figure 1a represents the relation between the carbon steel corrosion potential (EmV) vs the Ag/AgCl reference electrode and log Icorr (corrosion current density) in 1 M HCl in the absence and presence of different concentrations of L400 and L600. From Figure 1a, it can be seen that the addition of L400 and L600 shifts the anodic/cathodic polarization curves toward the noble direction, indicating a decrease in the corrosion rate of the tested alloy.28 Not to mention, with the addition of the prepared nonionic surfactant molecules, the corrosion potential changed within ±85 mV towards the blank one, and this indicates that these tested inhibitors act as mixed-type inhibitors.29

The electrochemical parameters obtained from Figure 1a, such as icorr, Ecorr, βa, and βc, are tabulated in Table 1. In addition to that, the surface coverage (θ) and the inhibition efficiency percentage (IE (%)) are calculated according to eqs 2 and 3 and tabulated in Table 1.

Table 1. Potentiodynamic Polarization Measurements of the X65 Steel in 1 M HCl in the Absence and Presence of Various Concentrations of the L400 and L600 Nonionic Surfactants at 25 °C.

  conc (M) –Ecorrvs Ag/AgCl (3 M KCl) (mV) icorr(μA/cm2) –βc(mV/dec) βa(mV/dec) Rp(Ω·cm2) CR (Mpy) θ IE (%)
blank   451 618 147.22 121.9 46.85 283.23    
L400 1 × 10–6 434 186 95.84 52.366 79.05 85.24 0.6993 69.93
  5 × 10–6 482 158 159.15 88.01 155.74 72.41 0.7436 74.36
  1 × 10–5 430 89.8 175.67 106.98 321.50 41.15 0.8547 85.47
  5 × 10–5 433 76.4 172.78 118.36 399.22 35.01 0.8763 87.63
  1 × 10–4 423 48 157.27 104.85 569.09 21.99 0.9223 92.23
L600 1 × 10–6 462 174 143.7 70.505 118.03 79.74 0.7181 71.81
  5 × 10–6 463 119 182.73 111.84 253.15 54.53 0.8079 80.79
  1 × 10–5 414 67.3 156.86 114.29 426.58 30.84 0.8911 89.11
  5 × 10–5 397 56.7 142.64 125.16 510.53 25.98 0.9082 90.82
  1 × 0–4 352 36 87.119 130.52 630.17 16.48 0.9418 94.18
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The close inspection of Table 1 declares that the addition of inhibitors has a huge effect on the corrosion current density and corrosion rate even in low concentrations. icorr is dramatically decreased compared to the blank. This refers to the adsorption ability of the prepared inhibitors due to the presence of high-electron-density centers (O, N, and π electrons). Corrosion rate (mpy) can be calculated using the corrosion current density according to eq 5

3.1. 5

where eq. wt., d, and icorr are the current equivalent weight, the iron density, and the corrosion current density, respectively.30 Furthermore, the corrosion current density and CR decrease with both concentrations of inhibitor and the number of ethylene oxide units (L400 < L600), as shown in Figure 1b. Furthermore, the polarization resistance calculated using the Stern–Geary equation (eq 6) and tabulated in Table 1

3.1. 6

where βa and βc are the slopes of the anodic and cathodic Tafel, respectively. The polarization resistance value is inversely proportional to the corrosion current density. The Rp increases from 79 to 569 Ω·cm2 with the increasing concentration from 1 × 10–6 to 1 × 10–4 M of the added inhibitor L400. Also, it increases from 569 to 630 Ω·cm2 as the number of ethylene oxide units increase for L600 at the same concentration (1 × 10–4 M). The potentiodynamic polarization values agree with Rct values obtained from EIS, which will be discussed later.31,32 The adsorption of the inhibitor molecule over the X65 surface increases the surface coverage and, in turn, decreases the dissolution rate of X65. The order of the inhibition efficiency of the prepared compounds is (L400 < L600).

3.2. EIS

The nondestructive electrochemical impedance spectroscopy (EIS) test method is used to evaluate the performance of the tested corrosion inhibitor compounds for the X65 steel in 1 M HCl at room temperature. Nyquist and Bode plots for X65 in 1 M HCl in the absence and the presence of different concentrations of the prepared nonionic surfactants differ in an in situ number of ethylene oxide units represented the EIS performance of the X65 steel corrosion in acidic media are shown in Figures 2 and 3. The Nyquist curves show the depressed semicircles under the real axis with one time constant, as shown in bode plots; this indicates that the charge transfer process controls the X65 corrosion process.33 The depressed shape of the Nyquist plot is due to the frequency depression phenomenon that returned into the inhomogeneity of the electrode surface.34 The overall shape of the EIS diagrams (Nyquist and Bode) of X65 in 1 M HCl before and after the inhibitor addition are not changed; this suggested that the X65 dissolution reaction mechanism controlled by the charge transfer process is neither changed or nor affected by inhibitor addition.35

Figure 2.

Figure 2

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EIS Nyquist plot of the X65 steel in 1 M HCl with various concentrations of L400 and L600 at 25 °C.

Figure 3.

Figure 3

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EIS bode for the X65 steel in 1 M HCl in the presence of different concentrations of L400 and L600 at 25 °C.

The addition of the tested compounds leads to an increase in the diameter of the Nyquist plot (as seen in Figure 2), shift in the /Z/ at the lower-frequency region to a higher value, and shift in the phase-angle value toward −90 °C at an intermediate frequency region (as presented in the bode plots; Figure 3). This is related to the inhibitor adsorption over the X65 surface.36,37 The EIS experimental data can be fitted using a simple Randles equivalent circuit that is composed of Rs, electrolyte (solution) resistance, Rct, Fe ion transfer resistance, and constant phase element (CPE) parameter Y0 in place of Cdl (double-layer capacitance) to obtain more fitted simulated data. Figure 4 shows the blank and high concentration (1 × 10–4 M) from both compounds as representative concentrations fitted with the proposed equivalent circuit in situ.

Figure 4.

Figure 4

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Nyquist plot of X65 steel in absence and presence 1 × 10–4 M of L400 and L600 using the proposed in situ equivalent circuit.

The EIS parameters obtained are tabulated in Table 2. The addition of nonionic surfactants with different ethylene oxide units even in low doses has a great effect on the Rct value, as shown in Table 2.

Table 2. Electrochemical Parameters of the Impedance of the X65 Steel in 1 M HCl in the Absence and Presence of Various Concentrations of the L400 and L600 Nonionic Surfactants at 25 °C.

          CPE
    
  conc. (M) Rs (Ω·cm2) Rct (Ω·cm2) CPE (μF) Cdl(F) N θ IE (%)
blank 0.00 2.0121 42.6 2.115 × 10–4 0.587 0.7861    
L400 1 × 10–6 1.2371 102.76 1.9202 × 10–4 0.675 0.7898 0.58544 58.54
  5 × 10–6 1.6935 136.16 1.5658 × 10–4 0.634 0.8098 0.6871 68.71
  1 × 10–5 1.5089 284.35 1.0297 × 10–4 0.555 0.8511 0.8501 85.01
  5 × 10–5 1.326 331.17 8.1964 × 10–5 0.373 0.8210 0.8713 87.13
  1 × 10–4 0.73274 532.4 6.2021 × 10–5 0.312 0.8325 0.9199 91.99
L600 1 × 10–6 1.9861 119.62 1.7422 × 10–4 0.633 0.7928 0.6438 64.38
  5 × 10–6 1.8153 265.12 1.4336 × 10–4 0.619 0.8107 0.8393 83.93
  1 × 10–5 1.5884 362.68 8.9572 × 10–5 0.484 0.8481 0.8825 88.25
  5 × 10–5 1.1883 446.85 5.5337 × 10–5 0.265 0.8345 0.9046 90.46
  1 × 10–4 1.2608 579.27 4.5035 × 10–5 0.237 0.8510 0.9264 92.64
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Increasing both the concentration and ethylene oxide unit increases the X65 surface coverage, which, in turn, leads to an increase in the charge-transfer resistance.38 Also, the addition of inhibitor leads to the decrease in the double-layer capacitance Cdl values recorded in Table 2, as the protective layer formed (over X65 surface) by the tested compounds have lower dielectric constant values compared with the replaced adsorbed water and aggressive chloride ion counterparts.39Figure 5 represents the relationship between the inhibitor dose of both the used inhibitors differ in in situ number of ethylene oxide units and Rct and Cdl. It can be said that the corrosion inhibition order is related to the molecular weight of the tested compound (L400 < L600), and this is matched with the previously discussed potentiodynamic polarization data.

Figure 5.

Figure 5

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Relation between Rct, CPE, and inhibitor concentrations of different ethylene oxide units.

3.3. Adsorption Isotherm

Competitive adsorption process occurring at the electrode/electrolyte interface between the inhibitor molecules and the water or/and Cl– ion is controlled by the quasi-substitution process according to eq 7

3.3. 7

where EOsol and EOads are the ethylene oxide molecules in the aqueous solution and adsorbed on the metallic surface, respectively. The protective shielded layer covering the electrode surface (θ) is related to the adsorption phenomenon. Different adsorption isotherm models such as Temkin, Frumkin, Flory–Huggins, and Langmuir are used to fit the Tafel and the EIS data via the relation between the inhibitor concentration (Cinh) and the surface coverage (θ). Based on the high correlation coefficient (R2), the more fitted adsorption model was found Langmuir adsorption isotherm (as shown in Figure 6) that describes the inhibitor adsorption process faultlessly according to40,41

3.3. 8

where θ is the surface coverage, Kads is the adsorption constant, and C is the inhibitor concentration. The inhibitor adsorption free energy (ΔGads) was calculated with the help of (Kads) value according to eq 9

3.3. 9

where the molar concentration value of water was 55.5 M and R is the gas constant under standard conditions.

Figure 6.

Figure 6

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Langmuir isotherm adsorption model of L400 and L600 on the X65 steel surface in 1 M HCl at 25 °C from the EIS and Tafel measurements.

The values of ΔGads and Kads are recorded in Table 3. The higher value of Kads indicates the adsorption strength of the inhibitor, and the negative sign of ΔGads points to the spontaneity of the adsorption process. The higher ΔGads values recorded in Table 3 indicate that the chemical adsorption behavior of the prepared compound, which occurs via the transfer of electrons from high electron centers to the vacant 3d orbital of Fe, forming a covalent bond. The negative value of the adsorption free energy charge increases with the increasing molecular weight of the tested compounds (from −43.22 to −45.16 for L400 and L600), and this is matched with the potentiodynamic and the EIS data.42,43

Table 3. Langmuir Isotherm Parameters for the Adsorption of the Synthesized Inhibitors on the X65 Steel Surface in 1 M HCl at 25 °C from the EIS and Tafel Measurements.

    method
inhibitor parameter Tafel EIS
L400 R2 0.9994 0.9994
slope 1.08 1.08
K (L·mg–1) × 105 8.60 6.79
–ΔG (kJ·mol–1) 43.81 43.22
L600 R2 0.9997 0.9999
slope 1.05 1.07
K (L·mg–1) × 105 12.01 14.80
–ΔG (kJ·mol–1) 44.64 45.16
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3.4. SEM and EDX Analysis

Surface analysis studies (SEM and EDX) for the X65 steel slides immersed for 3 h in a pure solution of 1 M HCl and the other treated with optimum concentration (1 × 10–4 M) of the best tested nonionic surfactant compound (L600) have been represented in Figures 7 and 8, respectively. SEM analysis technique gives the two-dimensional (2D) visual information about the performance of the insight inhibitor toward the metal corrosion. From Figure 7, it can be observed that the higher damage X65 surface fulfilled with corrosion product while, with Figure 8, after adding the optimum concentration of L600, the X65 surface becomes more smooth and free somewhat from corrosion product this inferred the inhibition action of L600 via blocking the active centers of the metal surface.44 EDX gives the chemical composition of the outer layer surface of X65 in the absence and presence of 1 × 10–4 M of L600 in 1 M HCl. The peak intensity of Fe higher in the absence of an inhibitor while a decrease in the presence of inhibitor confirms the shielding X65 surface with protecting inhibitor and decrease with corrosion product. The (−N−) atom peak appearance in the presence of inhibitor indicates the formation of the protective adsorbed layer. These observations are in agreement with the previously published data.45−47

Figure 7.

Figure 7

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SEM surface analysis micrograph of the X65 steel immersed in 1 M HCl at 25 °C for 3 h and the EDX analysis for the X65 steel blank quantification of the elements present.

Figure 8.

Figure 8

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SEM surface analysis micrograph of the X65 steel after the addition of 1 × 10–4 M L600 at 25 °C for 3 h and the EDX analysis for the X65 steel and quantification of elements present.

3.5. Quantum Chemical Calculation

The adsorption ability of the prepared nonionic surfactants L400 and L600 over the X65 steel surface can be discussed from a quantum chemical calculation point of view via frontier molecular orbital theory (FMOT) and Monte Carlo simulation with the aid of Material Studio software (MS 6.0, Accelrys).48 The adsorption of the tested inhibitors could be based on the donor–acceptor interaction phenomena. In that case, the electrons are transferred from the high-electron-density centers (O, N, and π electrons, i.e., regions of highly electronic distributions) of the organic compounds to the vacant 3d orbital of the metal (iron). The quantum chemical parameters obtained from the optimization of L400 and L600 in the gas and solvent phases (shown in Figure 9a,b) are depicted in Table 4 and discussed as follows. The energy of the highest occupied molecular orbital (EHOMO) represents the electron-donating ability of the tested compounds. The lower value of ELUMO indicates the ability of the molecules to accept the electrons from the back donation of Fe and thus increase the binding energy between the metal and the inhibitor.

Figure 9.

Figure 9

Figure 9

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(a) Optimized structures, highest occupied molecular orbitals (HOMO), lowest unoccupied molecular orbitals (LUMO), and molecular electrostatic potential maps of the synthesized L400. (b) Optimized structures, highest occupied molecular orbitals (HOMO), lowest unoccupied molecular orbitals (LUMO), and molecular electrostatic potential maps of the synthesized L600.

Table 4. Quantum Chemical Parameters of the Investigated Inhibitors.

inhibitor   EHOMO ELUMO ΔE (eV) A I χ (eV) η (eV) ΔN (eV) μ (D)
L400 gas –4.2812 –1.998 2.2827 1.998 4.2812 3.1399 1.141 1.1413 4.9768
solvent –4.6104 –2.361 2.2492 2.361 4.6104 3.4858 1.124 1.5623 9.7372
L600 gas –4.2648 –2.340 1.9242 2.340 4.2648 3.3027 0.962 1.9213 4.3482
solvent –4.5482 –2.321 2.2271 2.321 4.5482 3.4346 1.113 1.6008 8.9902
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The higher EHOMO and the lower ELUMO, the higher the adsorption/binding ability of the tested inhibitor with the metal surface.20,49−53EHOMO increases with increasing the ethylene oxide units, as presented in Table 4. This is in good agreement with the experimental data, suggesting that L600 is better than L400.54 The chemical reactivity is controlled by the energy gap ΔEgap values. From the reactivity point of view, the higher inhibition performance molecule is the higher reactive ones toward the substrate surface, and the most stable ones is the lower ΔEgap. Therefore, L600 forms a more stable complex with the Fe substrate rather than L400. The dipole moment (μ) results from nonuniform charge distribution over the atoms in the molecule. Decreasing in the dipole moment values support inhibitor molecule accumulation over the Fe surface and thus increase the adsorption ability of L600 over that of L400 as well as matched with the experimental data.55,56 The absolute electronegativity (χ), hardness (η), softness (σ), and fraction of electron transfer (ΔN) collectively represent the active parameters that are calculated from eqs 10 to 13

3.5. 10
3.5. 11
3.5. 12
3.5. 13

where I is the ionization energy (I = −EHOMO) and A is the electron affinity (A = −ELUMO).

According to the concept of the hard–soft acid–base, the soft molecule has lower values of ΔEgap and higher basicity and vice versa compared with the hard ones.57 Therefore, the soft molecule has adsorption ability due to the ease of electron transfer compared to the hard one and the better corrosion inhibitor. According to Lukovit’s study, the inhibition performance as a function of electron transfer increases when the number of electrons transferred (ΔN) is less than 3.6.27

The higher the fraction of electron transfer (ΔN), the better is the corrosion inhibitor. ΔN increases as the number of ethylene oxide units increase, as reported in Table 4, and this confirms the highest electroadsorption ability of L600 compared to L400 as previously declared by the experimental data. Ionization energy represents the chemical reactivity of atoms and molecules. Therefore, as the ionization energy increases, the reactivity increases and, in turn, the inhibition efficiency decreases (L400 < L600).58 These support the obtained electrochemical data (Tafel and EIS).

3.6. Monte Carlo Simulations

The MC simulations for both L400 and L600 in the gas phase and solution simulated the acidic medium with 500 H2O/5 Cl–/5 H3O+ were introduced to simulate the real corrosive medium has been executed using adsorption locator module via the following system:

  • (A)

    Fe (1 1 0) crystal, the metal, is considered in the recent study, as the most stable surface was used in the simulation process.

  • (B)

    Cleavage plane (35 × 35) supercell.

  • (C)

    30 Å vacuum slab to remove the periodic boundary effect.

MC simulation gives us a good image of the orientation and interaction between the prepared compounds over the Fe surface, as shown in Figure 10a,b. Both L400 and L600 are oriented horizontally and parallel to the Fe crystal (1 1 0) surface to maximize the contact and increase the surface coverage, which achieves higher adsorption energy and reflects a higher inhibition efficiency.

Figure 10.

Figure 10

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(a) Top (left) and side (right) views of the most stable low-energy configurations for the adsorption of L400 on the Fe (1 1 0) in a vacuum and a simulated solution (500 H2O/5 Cl–/5 H3O+) phases obtained using the Monte Carlo simulations. (b) Top (left) and side (right) views of the most stable low-energy configuration for the adsorption of L600 on the Fe (1 1 0) in a vacuum and a simulated solution (500 H2O/5 Cl–/5 H3O+) phases obtained using the Monte Carlo simulations.

From Table 5, it is obvious that Eads for L600 on the Fe (1 1 0) in the presence of H2O and HCl is greater than that for L400 due to a higher number of electron-donating (ethylene oxide) units and achieves a higher inhibition efficiency. The higher adsorption energy of the molecules indicates the ability of the tested compound to replace the corrosive ions and H2O molecules to form a protective shield layer against the corrosive medium.27,39

Table 5. Output Energies Calculated by Monte Carlo Simulations for the Prepared Compounds in Gas and Solution Phases on the Fe (1 1 0).

compound total energy (kJ/mol) adsorption energy (kJ/mol) rigid adsorption energy (kJ/mol) deformation energy (kJ/mol) (dEads/dNi) (kJ/mol) H2O:dEad/dNi H3O+:dEad/dNi Cl–:dEad/dNi
L400 gas –670.09 –741.91 –594.728 –147.182 –741.91      
L400 + 5 HCl + 500 H2O –6.57 × 103 –1.65 × 104 –6.68 × 103 –9.78 × 103 –555.947 –19.85 –116.81 –76.022
L600 gas –763.809 –798.002 –662.044 –135.958 –798.002      
L600 + 5 HCl + 500 H2O –6.69 × 103 –1.66 × 104 –6.78 × 103 –9.77 × 103 –643.178 –20.08 –185.35 –122.98
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4. Mechanism of Corrosion Inhibition on X65 Steel

The inhibition inertia of organic molecules originated from the formation of a protective layer that is absorbed on the iron surface. Both the electrochemical and microscopic measurements confirmed that the corrosion of the X65 steel was meaningfully reduced in the presence of inhibitors (L400 and L600). Additionally, the adsorption isotherm studies prove that the adsorption of the inhibitors over the iron surface is highly fitted to the Langmuir adsorption model. Besides, the adsorption behavior of the formed protective film is primarily achieved by (1) the electrostatic interaction via the protonated heteroatoms and (2) various bonds between the inhibitor molecules and the X65 steel surface. More precisely, the interaction between the inhibitors (L400 and L600) and the X65 steel surface is shown in Figure 11. There are two predominant adsorption methods between the inhibitor molecule and the X65 surface: first, the interaction between the π-electrons of the benzene ring and the unoccupied d-orbital of the Fe atoms; second, the donor–acceptor interactions between the vacant d-orbital of the iron (X65 steel) surface atoms and the lone electron pairs in the heteroatoms (N and O). These active electrons are disposed to be shared with the d-orbitals of the Fe atom.

Figure 11.

Figure 11

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Simulated corrosion and corrosion inhibition reaction mechanism of X65 in 1 M HCl in the absence and presence of the tested nonionic surfactants.

5. Conclusions

  • (1)

    The synthesized ethoxylated nonionic surfactants have high corrosion inhibition performance in the X65 steel in 1 M HCl due to the presence of the highly effective electronic adsorption centers (O, N, and π-bond) that block the active centers of iron metal.

  • (2)

    The EIS and Tafel electrochemical techniques showed that the inhibition efficiency increases with increasing both the concentration and the ethoxylation degree; therefore, the IE (%) for L600 is higher than that of L400 over the whole concentrations used.

  • (3)

    The potentiodynamic polarization (PDP) data suggest the mixed-type behavior of the tested inhibitors as the change in Ecorr was within ±85 mV around Eocp of the blank.

  • (4)

    MC simulation clarifies that the adsorption energy of the inhibitor molecule over the X65 steel was more than those of the water molecule and chloride ions and agrees with the decrease in Cdl as a result of the adsorption of inhibitor over the X65 surface in place of water and aggressive ions.

Acknowledgments

Support of this work by the Egyptian Petroleum Research Institute is gratefully acknowledged.

The authors declare no competing financial interest.

Due to a production error, the version of this paper that was published ASAP January 29, 2021, contained a corrupt version of Figure 11. The error was fixed, and the corrected version was posted February 1, 2021.

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