Journal of Renewable Materials

DOI: 10.32604/jrm.2021.015518

ARTICLE

Performance Evaluation of a Novel and Effective Water-Soluble Aldehydes as Corrosion Inhibitor for Carbon Steel in Aggressive Hydrochloric Medium

Yun Wang1, Tiantian Wang2, Bei Wang1, Wei Chang3, Jiangli Cao1, Lihua Hu3, Minxu Lu1 and Lei Zhang1,*

1University of Science and Technology Beijing, Beijing, 100083, China
2Wenzhou Hongfeng Electrical Alloy Co., Ltd., Wenzhou, 325603, China
3CNOOC Research Institute, Beijing, 100028, China
*Corresponding Author: Lei Zhang. Email: zhanglei@ustb.edu.cn
Received: 24 December 2020; Accepted: 11 March 2021

1  Introduction

The corrosion of carbon steel, a common material used in petroleum and biomedicine industries, has become increasingly prominent [1–8]. In industrial production, sulfuric acid and hydrochloric acid are the most widely used pickling agents [9]. Due to the strong corrosivity of acid, acid can remove rust and dirt, but also have a strong corrosive effect on the metal part of the substrate, and serious corrosion of the equipment will bring huge economic losses and harm. In order to solve the problem of metal material loss caused by pickling every year in China, corrosion scientists have developed a variety of solutions, such as surface coating, bond coating, corrosion inhibitor, etc. [10]. Numerous physical, chemical and mechanical methods, the addition of corrosion inhibitor is most effective and economical approach to prevent corrosion in the corrosive media [11–13]. Some effective inhibitors have been developed such as imidazoline and pyran derivatives [14,15]. However, most of the derivatives are toxic, and it can cause dizziness, insomnia, or even liver damage to human. In view of the shortcomings of traditional corrosion inhibitors, it is necessary to develop green and environmental-friendly corrosion inhibitors, especially for the food, biological and pharmaceutical industries.

Plant-type corrosion inhibitor is used in industrial production to inhibit the corrosion of metal materials in corrosive environment, which is a new type of natural green corrosion inhibitor. To date, some green inhibitors have been derived from natural products or synthesized [16–18]. Ma et al. prepared a supramolecular complex (CDCA) based on β-cyclodextrin (β-CyD) and trans-cinnamaldehyde (MHB) through organic solvent extraction. The inhibition efficiency for mild steel in HCl solution could reach 93.8% in the presence of 12 mM CDCA, and both the cathodic and anodic process could be depressed in the presence of CDCA, which was categorized as the mix-type inhibitior [19]. Su et al. investigated the corrosion inhibitive performance of a new schiff base N, N'-dicinnamylidene-o-phenylenediamine as acid inhibitor by the condensation of ophenylenediamine and cinnamaldehyde. The results showed that DCPD could effectively inhibit the corrosion to carbon steel in 10% HCl solution [20]. El-Etre [21] find vanillin can achieve 99% surface coverage on aluminum surface by the adsorption through the active contained in its structure [21]. 3-Methoxy-4-hydroxybenzaldehyde can also be used as the inhibitors in food system, e.g., the oxidation of dihydrorhodamine 123 to fluorescent rhodamine 123 was inhibited by vanillin [22]. Furthermore, (E)-3-phenylprop-2-enal can also be used as a good inhibition against steel corrosion by formation of a continuously thickening polymer film [23]. Gupta et al. manifested that L-lysine and aromatic aldehydes, as green corrosion inhibitors for mild steel, exhibited a maximum inhibition efficiency of 95.6% at 400 mg·L−1 concentration, and adsorption of the SBs (Schiff’s bases) on mild steel surface obeys the Langmuir adsorption isotherms [24]. These corrosion inhibitors are derived or synthesized from natural products. They are able to become excellent corrosion inhibitors, while reducing the potentially negative impact to nature and human being. In addition to furfural, 3-Methoxy-4-hydroxybenzaldehyde (MHB) and (E)-3-phenylprop-2-enal (PE) also have the characteristics of high efficiency and environmental-friendliness. PE is recognized as a safe and non-toxic substance by the U.S. Food and Drug Administration. It is commonly used as food and spice additives. MHB, as the principal raw material for aroma modification, is widely used in food, soap, tobacco, drugs and other light industries. Technically, the function of corrosion inhibition is mainly achieved through the formation a polymeric film on the surface. PE and MHB contain many functional groups, such as aromatic groups, carbonyl groups, hydroxyl groups, and methoxy groups, which can easily form a film through adsorption. Therefore, it is hypothesized that PE and MHB can be used as inhibitors due to abundant adsorption groups.

In this paper, we developed a novel corrosion inhibitor β-HA by catalyst-free green method, and its structure was characterized by Fourier transform infrared (FT-IR) and 1H NMR spectra. The corrosion resistance of β-HA was studied by scanning electron microcopy (SEM), weight-loss method and electrochemical methods to verify the effectiveness for protection and reveal the mechanisms of corrosion prevention. Quantum chemical calculation and molecular dynamics simulation were utilized to study the electronic properties and the interaction between inhibitor molecule and metal surface.

2  Materials and Methods

2.1 Preparation of Electrode and Solution

N80 steel was used for the corrosion test. Its chemical composition is shown in Tab. 1. All specimens (1 × 1 cm2) were polished using 360∼1200 grit sandpapers and then cleaned with deionized water and ethanol, respectively. Hydrochloric acid (36.5%, Beijing Chemical Plant), acetone analytical reagent(≥99.5%, Tianjin Bohua Chemical Reagent Co., Ltd., China), absolute ethyl alcohol (≥99.7%, Lizhi Chemical Engineering), 3-Methoxy-4-hydroxybenzaldehyde (MHB) (99%, Sigma-Aldrich), (E)-3-phenylprop-2-enal (PE) (93%, Sigma-Aldrich) were purchased, all of the reagents were analytical grades. The test corrosion solution is 15% HCl solution, which is made of 36.5% concentrated HCl (AR grade) diluted with distilled water.

2.2 Preparation of 3-methoxy-4-hydroxybenzaldehyde (MHB) and (e)-3-phenylprop-2-enal (PE)

In order to analyze the corrosion inhibition performance of MHB and PE for N80 steel corrosion in 15% HCl solution, the concentrations of inhibitor MHB and PE were prepared as 0, 2, 4, 6 and 8 mmol·L−1.

2.3 Preparation of β-hA

The preparation of β-HA is shown in Fig. 1. When preparing the β-HA corrosion inhibitor, 2 mmol of MHB powder was first weighed and dissolved in 50 ml deionized water, followed by 4 mmol PE (4 ml, 1 mol·L−1) solution and 5 ml dilute NaOH with stirring. Finally, the solution was transferred to a Teflon-lined stainless-steel autoclave and then heated at 120°C for 4 h. After cooling to room temperature, the reaction solution was centrifuged for 15 min [25].

Figure 1: Synthesis procedure of inhibitor β-HA

2.4 Preparation of β-hA Solution

To compare the performance of corrosion inhibitor β-HA, the solution with the same concentration as MHB and PE was prepared.

2.5 Structure Characterization

Structure of β-HA was characterized using Thermo Fisher Scientific Nicolet 6700 FTIR and 1H NMR spectra was recorded in CDCl3 by a Bruker digital FT-NMR spectrometer (Bruker BioSpin GmbH).

2.6 Weight Loss Experiments

All samples were exposed to 15% HCl solution in the absence and presence of β-HA for 12 h at 303 K and different immersion time. Prior to each test, the samples were weighed three times using a digital weighing balance of precision ± 0.01 mg. After the experiment, the samples were taken out and washed thoroughly in running water and distilled water, rinsed in acetone, and finally dried in a stream of warm air. The dried specimens were reweighed to calculate the corrosion rate (υ), which was calculated by following Eq. (1) [26]:

υ=K×ΔWA×t×ρ (1)

where K is the constant (8.76 × 104), ΔW is the mass loss (g), A is the surface area of the specimen (cm2), t is the immersion time (h) and ρ is the density of the steel sample (g/cm3).

2.7 Electrochemical Measurements

A conventional three-electrode system (working electrode: N80 steel with area of 0.85 cm2, counter electrode: Pt, reference electrode: a saturated calomel electrode) was used in all electrochemical measurements by CS350 electrochemical workstation. The sweeping rate during polarization measurements was 0.5 mV/s, and the potential was changed from −0.5 to +0.5 V (vs. SCE). Electrochemical impedance spectroscopy (EIS) was performed at the open-circuit potential in the frequency range from 0.01 to 100 kHz with an excitation signal of 10 mV. The electrode potential was allowed to stabilize for 30 min before starting the measurements. Each experiment was repeated three times to ensure repeatability. The experimental schematic diagram of electrochemical device is shown in Fig. 2.

Figure 2: Schematic diagram of the electrochemical device

2.8 Surface Characterization

The corrosion morphology of specimen was observed by scanning electron microscope (SEM, S4800, Japan) and the electron gun acceleration voltage was 10 kV. X-ray photoelectron spectroscopy (XPS) was obtained using a Shimadzu-Kratos AXIS Ultra DLD with Al Kα as excitation source, and the binding energy was calibrated by ± 0.1 eV C1 s peaking at 284.6 eV [27]. The three-dimensional morphology of steel surface was observed using Olympus.

2.9 Computational Details

All quantum chemical calculations were performed at the BLYP-D3BJ/def2-SVP level using Density Functional Theory (DFT) using the GGA functional and the DNP basis set by using Materials Studio8.0 package with Density Functional Theory (DFT) [28,29]. This basis set can guarantee the precise geometric and electronic properties for organic molecules. Initial structural optimization of the three inhibitors was carried out with DFT-D correction at the convergence thresholds of energy change of 1.0 × 10−5 Ha, the maximum force of 0.002 Ha/Å and maximum displacement of 5.0 × 10−3 Å. In addition, the global orbital cutoff and the self-consistent field tolerance are 4.6 Å and 1.0 × 10−6 Ha, respectively. Theoretical parameters such as the energy of the highest occupied orbital (EHOMO), energy of lowest unoccupied molecular orbitals (ELUMO), chemical potential (χ), energy gap (ΔE), global hardness (η), global chemical softness (σ), global electrophilicity index (ω) and Nucleophilicity (ɛ) were calculated as follows:

ΔE=ELUMO−EHOMO (2)

χ=−EHOMO+ELUMO2 (3)

η=−EHOMO−ELUMO2 (4)

σ=−2EHOMO+ELUMO (5)

ω=μ22η=χ22η (6)

ε=1ω (7)

For molecular dynamics (MD) simulation, Fe (110) was selected due to it has the good stability among all the crystal planes of iron. The dimension of constructed simulation cells for Fe (110) with 5-layer atom was as 24.82 × 24.82 × 48.80 Å3. A medium slab containing 85 H2O molecules, 20 H3O+, 10 Cl−and 1 inhibitor molecule was built using Amorphous cell module. When the layer was built by means of Layer builder module, a large vacuum space of 20 Å was placed in the Z direction perpendicular to the Fe(110) surface and the corrosion medium layer in order to limit the interaction between inhibitor molecules and the side of Fe substrate. The geometry-optimized structures of MHB, PE and β-HA molecule were obtained using Forcite module with the force field COMPASS, which is successful in the previous study of polymer-metal interaction [30]. The built layer is minimized by using smart minimizer. Later, 500 ps with the time step 0.1 fs of MD simulation for the minimum simulation unit at 303 K was carried out to make the simulation unit reach an equilibrium state, followed by simulating in NVE ensemble for 1000 ps. The interaction between van der Waals (vdW) and electrostatic non-bonding was calculated by atomic cut-off method and electronic Wald method, respectively [31]. The operating temperature was monitored by the Andersen thermostat [32]. During calculating, all Fe atoms and molecules in the medium layer were frozen.

ΔEbinding is used to quantitatively evaluate the bonding strength of organic molecules on metals, and calculated as following:

Ebinding=Etotal−Emolecule+Esurface (8)

where, Ebinding is the binding energy, Emolecule is the potential energy of inhibitor molecule; Esurface is the potential energy of Fe (110) surface in absence of inhibitor; Etotal is the total potential energy of the simulated layer.

3  Results and Discussion

3.1 Characterization of β-hA

FTIR, 1H NMR and 13C NMR spectra characterized the chemical structures of β-HA is shown in Fig. 3. For FTIR spectrum (Fig. 3a), some functional groups were presented in β-HA, including C-O-C stretching vibration (1021 cm−1), -C-O stretching vibration (1114.0 cm−1), -OH stretching vibration (1402.2 cm−1), -C=C stretching vibration (1315.9 cm−1) in benzene ring structure, -C=O stretching vibration (1632.1 cm−1), -C-H stretching vibration (2853.3 cm−1) and -O-H stretching vibration (3339.1 cm−1) [33]. Based on FTIR spectra results, the formation of carboxyl -COOH indicated that MHB and PE has a certain aldehyde-aldehyde condensation reaction.

Figure 3: FTIR (a), 1H NMR (b) and 13C NMR (c) spectra of β-HA

It can be seen from Fig. 3b that the absorption peak of CDCl3 is at 7.46 ppm. In addition, δHppm = 2.39 (-OH), δHppm = 2.61 (-CH2), δHppm = 3.99 (-CH3), δHppm = 7.44 (benzene ring), and δHppm = 8.66 (phenol hydroxyl) [34]. 13C NMR (Fig. 3c) showed that the compound exists 16 carbon signals, among which δCppm 168.99, 177.8 was presumed to be carboxyl carbon signal, δCppm 145.56, 146.08, 128.58, 127.36 and 126.61 were conjugated double bond carbon signal, δCppm 56.36 was phenoxymethyl carbon signal, δCppm 35.05 and 29.26 were methylene carbon signal. Combined with the data of 1H NMR and 13C NMR spectra, it is speculated that the compound has the carboxyl group.

3.2 Weight Loss Measurement

The corrosion rates of N80 steel exposed to 15% HCl solution in the absence and presence of inhibitor for 12 h at 303 K and immersion time were obtained by weight loss in Fig. 4. The inhibition efficiencies (η %) can be calculated by using the Eq. (9):

η=νcorr0−νcorr′νcorr0×100 (9)

where, ν0corr and ν′corr are rate of corrosion with and without inhibitor.

Figure 4: Corrosion rate for N80 steel in 15% HCl solution from weight loss measurements at 303 K (a) β-HA concentration (b) immersion time

After being soaked into the solution with corrosion inhibitors MHB, PE and β-HA for 12 h, the corrosion rates of N80 steel decreased (Fig. 4a).

In addition, the decrement gradually decreased with the increase of inhibitor concentration. The presence of 8 mmol·L−1 inhibitor in the acid solution was sufficient to reduce the corrosion rate of the N80 steel from 21.56 mm/a to 3.03 mm/a, 2.85 mm/a, 1.8 mm/a, respectively. The maximum inhibition efficiency for MHB, PE and β-HA were 85.95, 86.78 and 91.65% at 8 mmol·L−1 concentration (Tab. 2), respectively. For immersion time (Fig. 4b), the corrosion rate of steel in 15% HCl solution showed an upward trend overall with the increase of immersion time, while an opposite trend was observed at 8 mmol·L−1 inhibitor MHB, PE and β-HA, respectively. Furthermore, the inhibition effect of β-HA inhibitor was verified.

3.3 Open Circuit Potential

Fig. 5 shows the OCP curves of N80 steel immersed in 15% HCl solution at 303 K. It can be seen from Fig. 5 that after immersing for 1800 s, the OCP floating range is within 10 mV, and the system reaches a stable state. In addition, it is noticed that the initial value of OCP with inhibitor is higher than that without inhibitor, which may be related to the adsorption of inhibitor molecules on the surface of N80 steel [35].

Figure 5: OCP curves of N80 steel in various test solutions: (a) MHB; (b) PE; (c) β-HA

3.4 Potentiodynamic Polarization Measurements

Potentiodynamic polarization curves for MHB, PE and β-HA are showed in Fig. 6. The electrochemical parameters were attained by using Extrapolation method from the polarization curves containing corrosion current density (icorr), corrosion potential (Ecorr), anodic and cathodic Tafel slopes (βa, βc), and inhibition efficiency (η). Moreover, the value of inhibition efficiency(η) were estimated by Eq. (10):

η=icorr0−icorricorr0×100 (10)

where i0corr and icorr represent the corrosion current density in the absence and presence of inhibitors, respectively.

Figure 6: Polarization curves of N80 steel in various test solutions: (a) MHB; (b) PE; (c) β-HA

As indicated in Figs. 6a–6c, the values of Ecorr in the presence of the inhibitor MHB, PE and β-HA shift less than 85 mV, respectively, the three inhibitors belong to mixed-type inhibitor [36]. The polarization curve after the addition of the corrosion inhibitor moves to the left, which indicates that the corrosion current density has decreased with the inhibitor. The reduced slope of the anode and cathode displays that the inhibitors have the ability to block the anodic and cathodic reactions simultaneously. Tab. 3 shows that the values of βa and βc for the 15% HCl solution are extremely larger than other groups, which indicates that adsorption films were formed on the N80 surface after inhibitors were added.

The values βa and βc did not change much with different types of inhibitors, which means that the anodic and cathodic reactions were similar among all. The corrosion current density on the N80 electrode in 15% HCl solution in the absence of inhibitor was 6.42 × 10−4 A·cm−2. As the inhibitor concentration increases, corrosion current density icorr decreases and inhibition efficiency increases, which is related to the adsorption of inhibitors molecules on the N80 steel surface. The interaction between corrosion inhibitors and Fe atoms on the surface of carbon steel, and the rate of corrosion on the surface of N80 decreased. By comparing the corrosion current density of MHB, PE and β-HA, the lowest value was observed at 0.38 × 10−4 A·cm−2 for 8 mmol·L−1 β-HA. This indicates that the corrosion inhibition of β-HA is better than individual inhibitor.

3.5 Electrochemical Impedance Spectroscopy Measurements

Fig. 7 shows Nyquist and Bode plots of the N80 steel in 15% HCl solution in the absence and presence of various concentrations of inhibitors. It can be seen from Fig. 7, the Nyquist curves of the three inhibitors show only one time constant corresponding to one capacitor circuit, indicating that the dynamics of the electrochemical system is controlled by the charge transfer process. In addition, the shape of Nyquist plots is almost similar in absence and presence of inhibitor, which suggests that the addition of corrosion inhibitor has no effect on the corrosion mechanism of N80 steel. The radius of capacitive reactance arc in Nyquist plots is below the real axis due to the roughness and uniformity of N80 steel electrode surface [37]. The radius of capacitive arc increases with the increase of inhibitor concentration in the 15% HCl solution, suggesting that inhibition efficiency increases with inhibitor concentration. Compared with capacitive arcs when MHB or PE is added alone (Fig. 7d, Fig. 7g), the radius of capacitive arc of the β-HA inhibitor is obviously larger than that of MHB or PE alone. This indicates that the corrosion inhibition performance of β-HA is better than that of MHB and PE alone [38–40].

Figure 7: EIS images of N80 steel in various test solutions

Based on Bode plots, the |Z|0.01Hz can be used to evaluate the corrosion rate of electrode [41]. It can be seen from Fig. 7b that the |Z|0.01Hz is about 10 Ω·cm−2 when N80 steel was immersed into 15% HCl solution for 12 h. As the concentration of inhibitor MHB, PE and β-HA increased respectively, the |Z|0.01Hz presented an increase trend. When the concentration of β-HA is 8 mmol·L−1, the |Z|0.01Hz increase to 104 Ω·cm−2.

In order to better understand the corrosion reaction process, the equivalent circuit model (Fig. 7) are used to fit EIS data, the fitting parameter was presented in Tab. 4. Among them, Rs is the solution resistance, Rct is the charge transfer resistance, CPE was the constant phase angle element, representing the capacitive property of electric double layer. The value of Cdl can be calculated by Eq. (11) [42], the corrosion inhibition efficiency(η) and surface coverage (θ) could be obtained according to the Eqs. (12) and (13), respectively [43]:

Cdl=(Y0Rct1−n)1n (11)

η=Rct−Rct0Rct×100 (12)

θ=Rct−Rct0Rct (13)

where, the Rct0 is the charge transfer resistance without inhibitor, Rct is the charge transfer resistance with inhibitor obtained by electrochemical impedance spectroscopy data.

As shown in Tab. 4, the change of Rs is not obvious in different corrosion environments. However, the film resistance Rf and Rct values show an increasing trend after adding inhibitors MHB, PE, or β-HA, indicating the inhibitor molecules are adsorbed on the sample surface to form a protective film. By comparison, arc radius of capacitive resistance and film coverage are the largest when the concentration of β-HA is 8 mmol·L−1, respectively (Tab. 4). These results also illustrate that β-HA is better than individual inhibitor for corrosion prediction. Moreover, the change trend of Cdl was opposite to that of Rct value with the increase of inhibitor concentration.

The corrosion inhibition efficiency (η) can be obtained by Eq. (14). In the case of MHB and PE added alone, the η value can be up to 83.82% and 87.88% when the adding concentration is 8 mmol·L−1. However, the η values in the case of β-HA were greatly enhanced as the injection concentration increased. When the concentration of β-HA is 8 mmol·L−1, the η values reached up to 91.46%. Therefore, the corrosion inhibition effect of β-HA was stronger than that of MHB and PE added alone, suggesting that the corrosion rate of N80 steel in 15% HCl solution is further reduced and the corrosion inhibition performance is increased. Also, it is important to note that the weight loss results are in conformity with the weight loss results.

3.6 Adsorption Isotherm

The experimental data were fitted with adsorption models, and the Langmuir model Eq. (14) has the best fit. The Gibbs free energy (ΔGads) for the adsorbent is obtained from electrochemical impedance spectroscopy results, as shown in Eq. (15) [44].

cinhθ=cinh+1Kads (14)

ΔGads=−RTln(55.5Kads) (15)

where the Kads is the equilibrium constant of the adsorption, Cinh is the inhibitor concentration and θ is the film coverage. R is the mole constant of gas with unit of J·mol−1·K−1 and T is the temperature with unit of Kelvin, and the concentration of water molecules is 55.5 mol·L−1.

The linear C/θ∼ C curves fitting by the Langmuir model are shown in Fig. 8, and the value of Kads are 208.3, 555.5 and 1666.7 with a high correlation coefficient of 0.9927, 0.9865 and 0.9932, respectively. Therefore, the adsorption behavior of MHB, PE and β-HA obey the Langmuir adsorption isotherm. The ΔGads can reflect the adsorption type of corrosion inhibitor on N80 steel surface, and it is related to Kads. ΔGads is −20 kJ·mol−1 or more negative, the corrosion inhibitor molecules are adsorbed on the metal surface by electrostatic interaction, which is physical adsorption; while ΔGads is −40 kJ·mol−1 or more negative, it belongs to chemical adsorption because of the covalent bond formed by electron transfer or sharing. Using Eq. (16), the ΔGads were −23.57, −26.04 and −28.81 kJ·mol−1 under the standard atmospheric pressure, respectively, which indicates that the adsorption of MHB, PE and β-HA on N80 steel surface could be the mixed adsorption process that involves both physical and chemical adsorption. By comparing outcomes of experiments, the adsorption force of β-HA is stronger than MHB and PE, and adsorption cannot be easily reversed. The adsorption is exothermic because ΔGads is smaller than zero [45].

Figure 8: C/θ∼ C plots of N80 steel after 12 h immersion in corrosion solution with different inhibitors at 303 K

In order to further understand the adsorption of corrosion inhibitor at the metal/solution interface, the adsorption entropy of activation (ΔS*) and enthalpy of activation (ΔH*) were introduced. Based on the transition state equation, ΔS* and ΔH* are be obtained [15].

νcorr=RTNHexp(ΔS∗R)exp(−ΔH∗RT) (16)

The plots of log (νcorr /T) vs. 1/T yield a straight line, as shown in Fig. 9, the values of ΔH* and ΔS* can be determined according to the slope and intercept of linear fitting. The obtained values are listed in Tab. 5. It can be clearly seen from Tab. 5 that the value of ΔH* is positive, which indicates that the adsorption of corrosion inhibitor on the metal interface is endothermic process, that is to say, the interaction between inhibitor molecules and Fe atoms on metal surface is more favorable at high temperature, and the adsorption of corrosion inhibitor molecules on the surface of N80 steel is easier. Due to the negative ΔS* value, the adsorption process is entropy increasing. The results suggest that the adsorption of corrosion inhibitor molecules is greater than desorption in the rate determining step. The increase of adsorption substances leads to the increase of solution confusion, and the active substances adsorb on the surface of N80 steel instead of water molecules to form an adsorption layer to inhibit the corrosion of N80 steel.

Figure 9: The relationship between log (νcorr/T) and (1/T) for N80 steel in 15% HCl solution with MHB PE and β-HA

3.7 Adsorption Rate

The surface coverage of N80 steel sample in HCl solution with 8 mmol·L−1 concentration of MHB, PE and β-HA at 303 K is given in Fig. 10.

Figure 10: The relationship between θ and time on the N80 steel surface after 6 h immersion in 15% HCl solution with 8 mmol·L−1 MHB, PE and β-HA, respectively

The whole adsorption process is divided into two stages: the first stage is a rapid adsorption process from 0∼120 min for β-HA, and the second stage is a rearrangement stage from 120–360 min, while the rapid adsorption process of MHB and PE is from 0 to 270 min, suggesting that that the film forming speed of inhibitor molecule β-HA is relatively fast. The behavior is similar with other self-assembled films [46,47]. In the first stage, the benzene ring and the organic functional aldehyde groups in the inhibitor molecule play a major role. Among them, the aldehyde group rapidly attach to metal surface via chemical bonding. In the meantime, the benzene ring has a hydrophobic structure and generates a hydrophobic film. In the second stage, large π bond of benzene ring is combined with the empty orbital of Fe atoms to form more stable bonds, resulting in a stronger adsorption and denser film [48].

3.8 Scanning Electron Microscopy

SEM analysis was performed to obtain deeper understanding about the corrosion morphology of N80 steel immersed in 15% HCl solution in absence and presence of inhibitor at 303 K. Fig. 11a shows the morphology of N80 steel after immersing in 15% HCl solution without inhibitor for 12 h, N80 steel surface was severely damaged with cracks and pits. Figs. 11b and 11c show the morphology after being soaked into the solution with 8 mmol·L−1 β-HA corrosion inhibitors. Compared with Fig. 11a, there were no obvious corrosion marks and serious corrosion pits on the metal surface. However, some small cracks still existed under a high magnification, indicating that the area covered by the corrosion inhibitor was incomplete. After adding inhibitor β-HA into the 15% hydrochloric acid solution, a layer of white coating appears on the surface of the sample, as shown in Fig. 11d. It was noted that the white coatings are unevenly distributed in an overlapping pattern and cracks are greatly decreased in this case. This indicates that the β-HA corrosion inhibitor can effectively slow down the corrosion by increasing the surface film coverage.

Figure 11: Corrosion morphology and element distribution of N80 steel in various solutions (a) 15%HCl solution-12 h (b) 15%HCl+8 mmol·L−1 MHB solution-12 h (c) 15%HCl+8 mmol·L−1 PE solution-12 h (d) 15%HCl+8 mmol·L−1 β-HA-12 h; and (e) C; (f) O distribution

3.9 3D Morphology

The 3D morphology of N80 samples were immersed in 15%HCl for 12 h at 303 K without and with inhibitors are shown in Fig. 12.

Figure 12: 3D corrosion morphology and roughness of N80 steel in various solutions (a) 15%HCl solution-12 h (b) 15%HCl+8 mmol·L−1 MHB solution-12 h (c) 15%HCl+8 mmol·L−1 PE solution-12 h (d) 15%HCl+8 mmol·L−1 β-HA-12 h

As shown in Fig. 12a, the surface of N80 samples in the 15% HCl solution without corrosion inhibitor was irregular and occurred severe corrosion, then the average roughness value reached up to 30.48 μm. After being soaked into the solution with 8 mmol·L−1 MHB, 8 mmol·L−1 PE and 8 mmol·L−1 β-HA inhibitors, the surface of the N80 samples became more and more smoother, which suggests that the corrosion process of N80 steel was hindered in the corrosive medium. According to Figs. 12b–12d, the average roughness values of N80 steel are 2.11 μm, 1.53 μm and 0.32 μm, respectively. The results show that the density of β-HA inhibition film is better than that of MHB and PE.

3.10 X-Ray Photoelectron Spectroscopy

The XPS results are shown in Fig. 13. The elements on the N80 surface are consistent with the composition given in Tab. 1.

Figure 13: (a) XPS results of the N80 steel with inhibitors in 15% HCl solution; (b) The binding energies along sputtering time of N80 steel in 15%HCl with 8 mmol·L−1 β-HA

After the corrosion test, the content of chlorine becomes an indicator for the effect of corrosion inhibitors. As shown in Tab. 6, the content of chlorine on the metal surface was 9.51% for the blank hydrochloric acid solution without addition of any inhibitor. The content was greatly reduced when there is β-HA in the solution, and the lowest one was observed in the condition of 8 mmol·L−1 β-HA. This implies that β-HA inhibitor is the best among other concentrations. Fig. 13b is the binding energies along with increased sputtering time during the XPS measurements. It suggests that the coating on the surface of N80 steel has been basically stabilized.

In order to account for the composition of the film more clearly, the peaks of C1 s, O1 s, Fe2p and Cl2p were fitted. In Fig. 14a, there are two peaks in C1 s, located in 284.60 eV and 288.20 eV. The binding energy at 284.60 eV corresponds to the C-H bond in the β-HA inhibitor. The binding energy at 288.20 eV is due to the C-O bond or -CHO bond. The binding energy at 529.68 eV and 531.0 eV comes from the O1 s. The energy at 529.68 eV is the dissolved oxygen, and the one at 531.0 eV indicates the C-O bond or -CHO bond. There are three principal peaks and some oscillating peaks appearing in the single peak of Fe element. Referring to XPS literature of the compounds with different valence of Fe elements [49–51], the binding energies at 710.9 eV and 724.4 eV in Fig. 14c correspond to the Fe2p3 and Fe2p1 in Fe2O3. The peak at 718.0 eV is related to the Fe2p1 in elemental iron. In Fig. 14d, Cl2p shows two main peaks at 198.15 eV and 199.71 eV. The peak at 198.15 eV represents the chloride ion in the etching solution, and the binding energy at 199.71 eV represents the C-Cl bond. Because of the low content of chlorine, the C-Cl peak intensity is lower. Therefore, it may be indicated that the film mainly consists of corrosion products such as iron oxide or ferrous hydroxide (film) and adsorbed organic functional groups. In the group without corrosion inhibitor, the C-Cl peak was the strongest due to the high chlorine content, and the corrosion products were mainly iron chloride/oxide. In the groups that only single corrosion inhibitor was added, the organic functional group detected is weaker and the C-Cl peak intensity is stronger than the β-HA inhibitor. The corrosion products were mainly iron chloride/oxide and a small amount of adsorption functional groups.

Figure 14: The (a) C1 s peak, (b) O1 s peak, (c) Fe2p peak, (d) Cl2p peak on N80 steel with 8 mmol·L−1 β-HA

3.11 Quantum Calculations

Based on the frontier molecular orbital theory, the adsorption centers of three kinds of organic corrosion inhibitors combined with carbon steel matrix through Lewis acid-base interaction were further revealed. The global minimum energy structure of the three inhibitors and the distribution of the highest occupied molecular orbital (HOMO) and the lowest unoccupied molecular orbital (LUMO) are shown in Fig. 15. The calculated parameters are listed in Tab. 7.

Figure 15: Optimized structure, HOMO and LUMO orbital distribution of MHB, PE and β-HA inhibitor molecules

The HOMO orbital can provide electrons to the vacancy metal orbital and interact with the metal atoms at the active site on the substrate surface, while the active site in the LUMO region of the inhibitor molecule can receive electrons from the filling orbital of the Fe atoms on the substrate surface [52]. For MHB and PE based on the distribution of HOMO and LUMO (Fig. 15), it can be seen that the HOMO orbit is concentrated on the O atoms and C atoms, while the LUMO orbital covers on the aldehyde group and its adjacent C atoms. For β-HA, the active centers of the HOMO orbital and the LUMO orbital were mainly located on O atoms, C atoms on benzene ring, and -COOH. The results indicate that β-HA molecules can contribute delocalized π electrons from benzene ring to the low energy vacancy orbit of Fe atoms on the surface, thus promoting the adsorption of inhibitor molecules.

According to the results in Tab. 7, the EHOMO of β-HA is higher than that of MHB and PE, which indicates that β-HA is easier to provide electrons to the unoccupied metal d orbit. Moreover, the ELUMO of β-HA is lower than that of MHB and PE, illustrating that the ability to accept electron of β-HA is stronger than that of MHB and PE. Compared with MHB and PE, the energy gap ΔE between HOMO and LUMO orbitals for β-HA is lowest, indicating inhibitor β-HA has better adsorption capacity on Fe (110) surface. Meanwhile, the O heteroatom play an important role as the active center of the interaction between inhibitor and steel surface. The adsorption trends of three inhibitors were studied by using the Hard and Soft Acids and Bases (HSAB) theory [53]. As a soft acid, Fe atom is easier to coordinate with soft base. Based on the DFT calculation results, the interaction ability of β-HA molecule with metal surface is better than that of MHB and PE, which is in good agreement with the experimental data.

3.12 Molecular Dynamic (MD) Simulation

Fig. 16 shows the free volume distribution of 1000ps for three inhibitors, and the blue part is the free volume in the model space. Based on the simulation results, it can be seen that the free volume fraction (FFV) of β-HA inhibitor film is the lowest among the three kinds of inhibitor films, which indicates that the porosity of the β-HA film is the lowest. Meanwhile, the diffusion ability of corrosion medium molecules through the film to the substrate is the weakest after adding inhibitor β-HA into corrosion medium.

Figure 16: The distribution of free volume in simulated inhibitor layers

In order to better understand the adsorption of MHB, PE and β-HA on metal surface, the adsorption configurations of three inhibitors on the Fe (110) surface are shown in Fig. 17.

As shown in Fig. 17, all three inhibitor molecules are adsorbed on the Fe (110) surface in parallel. The parallel adsorption of the three inhibitors on the iron surface may be due to the homogeneous distribution of HOMO and LUMO orbital density. The inhibitor molecules cannot only form a coordination bond with the empty d-orbital on the iron surface by providing lone pair electrons, but also form an anti-bond by accepting electrons from the d-orbital with π bond on the Fe surface.

Figure 17: Adsorption configurations of MHB, PE and β-HA inhibitor molecules on Fe (110) surface in HCl solution, (a, d) MHB, (b and e) PE and (c and f) β-HA

By calculating the interaction energy (Ebinding) between the molecules and the Fe (110) surface, the adsorption level of inhibitor molecules with Fe matrix layer in simulated solvent was quantitatively studied. The binding energy of the three inhibitor molecules interacting with the Fe layer are shown in Tab. 8. The order of the interaction energies of the three inhibitor molecules with Fe (110) is β-HA (−553.16 kJ mol−1) < PE (−329.94 kJ mol−1) < MHB (−312.69 kJ mol−1), respectively. It can be seen that the Einteraction value of β-HA is significantly lower than that of MHB and PE, in other words, the adsorption energy of β-HA is higher than that of MHB and PE. The higher adsorption energy suggests that the interaction between inhibitor molecules and the metal surface is relatively stable, and the inhibitor can show good inhibition performance.

In order to verify the experimental results more accurately, the bond length of the interaction between the three inhibitors and the Fe (110) surface was calculated. Generally, if the bond length is less than 3.5 Å, there is a strong chemical bond between the heteroatom and the Fe atoms. On the contrary, the interaction force is van der Waals force [54]. According to the shortest bond distance between the O atom of three inhibitors and the surface of Fe (110) in Tab. 6, the results show that the three inhibitors are adsorbed by chemical bond on the surface of Fe (110). The order of the bond lowest distance is β-HA (1.45 nm) < PE (1.96 nm) < MHB (2.08 nm). The adsorption of β-HA on Fe (110) surface is more stable, which can effectively block the migration of electrons at the interface of metal solution and the diffusion of chloride ions to metal surface. This suggests that the new β-HA has a good interface binding property and enhances the interaction between the inhibitor molecule and Fe surface.

3.13 Inhibition Mechanism

The corrosion of N80 steel in HCl solution belongs to electrochemical corrosion:

Fe−2e−→Fe2+ (17)

H++2e−→H2↑ (18)

It can be seen that the higher concentration of H+ in hydrochloric acid medium accelerates the corrosion cathodic reaction of N80 steel, and further aggravates the dissolution of matrix. The surface of N80 samples in the 15% HCl solution without corrosion inhibitor was irregular and occurred severe corrosion.

The corrosion inhibition of MHB, PE and β-HA is devoted to the O atoms with lone pair electrons in inhibitor molecules, which may interact with Fe atom by the coordination bond, neatly arranging on the N80 steel corrosion surface. According to the results of ΔGads, the mixed adsorption process that involves both physical and chemical adsorption on the surface of N80 steel occurs. The ionization of acid radical ions in β-HA molecules and the electrostatic repulsion between molecular chains promote the spread of β-HA groups and form a film on the surface of N80 steel, which has a good inhibition effect on the corrosion of N80 steel in HCl medium. When the metal is in contact with acidic medium, the inhibitor can form a single molecule adsorption film on the metal surface, and the inhibition effect can be achieved by changing the redox potential of hydrogen ion. However, the inhibition efficiency of MHB and PE is lower, which is related to the physical adsorption of the film formed on the surface of N80 steel.

4  Conclusion

The MHB, PE and β-HA were chosen to be as corrosion inhibitor for N80 steel corrosion in 15%HCl solution, and the corrosion inhibition performance was evaluated by using weight loss, electrochemical measurements, scanning electron microscope (SEM), quantum chemical calculation and molecular dynamics simulation (MDS).

(1)   By compare the corrosion inhibition performance of three different organic, the synthesized β-HA inhibitor can provide better protection for N80 steel in hydrochloric acid solution. Corrosion inhibition efficiency has a trend of increase along the concentration. The adsorption of inhibitor molecules obeys Langmuir adsorption isotherm with the ΔGads at −28.81 kJ·mol−1. In addition, the whole adsorption process can be divided into two stages: the first is that inhibitor molecules rapidly adsorbed on the N80 steel surface, and this is followed by large π bond of benzene ring to combine with the empty orbital of Fe atoms to form more stable bonds. The formed film can successfully hinder chlorine contact with metal.

(2)   Based on quantum chemical calculation and molecular dynamics simulation results, inhibitor β-HA has better adsorption capacity on Fe (110) surface and the Fe-O bong length of β-HA is lower than that of MHB and PE. Accordingly, the current work finds that inhibitor β-HA can greatly reduce the corrosion rate of N80 steel in hydrochloric acid medium. Since both MHB and PE are environmentally friendly chemicals, this finding is expected to possess a wider application in corrosion protection.

Acknowledgement: The authors thank the postgraduate students their kind help. The authors also sincerely thank the anonymous reviewers for their constructive suggestions.

Funding Statement: This work was supported by the National Science and Technology Major Project of China (Grant No. 2016ZX05028–004) and the Fundamental Research Funds for the Central Universities (Grant No. FRF-IC-18–007).

Conflicts of Interest: The authors declare that they have no conflicts of interest to report regarding the present study.

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