Adsorption, Thermodynamic and Quantum Chemical Studies of 1-hexyl-3-methylimidazolium Based Ionic Liquids as Corrosion Inhibitors for Mild Steel in HCl

Abstract

The inhibition of mild steel corrosion in 1 M HCl solution by some ionic liquids (ILs) namely, 1-hexyl-3-methylimidazolium trifluoromethanesulfonate [HMIM][TfO], 1-hexyl-3-methylimidazolium tetrafluoroborate [HMIM][BF₄], 1-hexyl-3-methylimidazolium hexafluorophosphate [HMIM][PF₆], and 1-hexyl-3-methylimidazolium iodide [HMIM][I] was investigated using electrochemical measurements, spectroscopic analyses and quantum chemical calculations. All the ILs showed appreciably high inhibition efficiency. At 303 K, the results of electrochemical measurements indicated that the studied ILs are mixed-type inhibitors. The adsorption studies showed that all the four ILs adsorb spontaneously on steel surface with [HMIM][TfO], [HMIM][BF₄] and [HMIM][I] obeying Langmuir adsorption isotherm, while [HMIM][PF₆] conformed better with Temkin adsorption isotherm. Spectroscopic analyses suggested the formation of Fe/ILs complexes. Some quantum chemical parameters were calculated to corroborate experimental results.

1. Introduction

Mild steel is extensively used in industries for various applications including construction of tanks, gas cylinders, pipelines, heat exchangers among others due to its excellent mechanical strength and relatively low cost. Many industrial processes involve the use of acid solutions and other chemical substances that constitute aggressive media for steel corrosion [1,2,3,4,5]. As a result, researches on corrosion inhibition of mild steel are of considerable interest due to the importance of steel in industrial and/or structural applications.

Various organic compounds containing nitrogen, oxygen, phosphorus and/or sulfur heteroatoms, and/or π-electron systems have been reported as inhibitors of metal corrosion in different aggressive media [1,2,3,4,5,6,7,8,9,10,11]. These groups of atoms or bonds facilitate electronic interactions between organic corrosion inhibitors and metal surface thereby aid adsorption of the inhibitors onto metal surface [9]. Researches in the field of corrosion inhibitors in the recent years have been directed towards the design and quest for “green” corrosion inhibitors due to the new generation of environmental regulations requirements for the replacement of toxic chemicals with the so-called “green chemicals” [12,13,14,15,16]. The quest for eco-friendly compounds as corrosion inhibitors has shifted research focus to exploring potential application of ILs as corrosion inhibitors in the past few years [17,18,19,20,21,22,23].

Ionic liquids (ILs) are materials that compose of entirely ions, and large organic cations and organic/inorganic anions and demonstrate melting points below 100 °C [24,25]. They possess various distinct properties such as high thermal and chemical stability, low vapour pressure, large electrochemical window, tuneable/designer nature, and excellent solvent properties for a range of polar and nonpolar compounds [25]. The low vapour pressure characteristic makes ILs to be easy to regenerate and reuse without appreciable loss into the environment [25,26,27]. This makes them to be classified as benign compounds to the environment. Imidazolium-based ILs have been reported to possess efficient inhibition properties against corrosion of metals and alloys in acidic environments [22,28,29,30,31]. Despite their good anti-corrosion potential, corrosion inhibition properties of some imidazolium-based ILs have not yet been explored.

The objective of the present work is to investigate the inhibition properties of four 1-hexyl-3-methylimidazolium (HMIM) based ionic liquids (ILs) namely, 1-hexyl-3-methylimidazolium trifluoromethanesulfonate [HMIM][TfO], 1-hexyl-3-methylimidazolium tetrafluoroburate [HMIM][BF₄], 1-hexyl-3-methylimidazolium iodide [HMIM][I] and 1-hexyl-3-methylimidazolium hexafluorophosphate [HMIM][PF₆] for mild steel corrosion in 1 M HCl. To the best of our knowledge, the ILs used in this work have not been considered for exactly the same study in the past. The studied ILs have the same cations, [HMIM] but different anions. Therefore, the effect of different anions on the corrosion inhibition activities of the four ILs will be investigated.

2. Results and Discussion

2.1. Electrochemical Measurements

2.1.1. Potentiodynamic Polarization (PDP)

Potentiodynamic polarization curves for mild steel in 1 M HCl without and with different concentrations (100–500 ppm) of the studied ionic liquid inhibitors are presented in Figure 1. The values of corrosion potential (E_corr) and kinetic parameters such as corrosion current density (i_corr), anodic and cathodic Tafel slopes (β_a and β_c) and polarization resistance (R_P) obtained from the polarization curves are presented in Table 1. The results as presented in Figure 1 show that in the presence of the inhibitors, the curves are shifted to the lower current regions. This observation confirms the corrosion inhibition property of the ILs. There is a slight difference in the values of E_corr between the inhibitor containing systems and the blank system. However, it is important to state that the E_corr values for the inhibitor containing systems shift essentially towards the cathodic region relative to that of the blank as shown in Figure 1. The maximum shift in E_corr value relative to the E_corr of the blank is 71 mV. Since an inhibitor can only be regarded as anodic or cathodic type when the displacement in E_corr is greater than 85 mV [32,33], the studied ILs behave as mixed-type inhibitors. That is, they inhibit both the anodic dissolution and cathodic hydrogen evolution reaction. The slight change in the values of β_a and β_c upon addition of the inhibitors when compared with the blank suggests that the ILs get adsorbed onto the metal surface without affecting the mechanism of the mild steel corrosion in the acid [34]. The higher values of β_c compared to the values of β_a suggests predominant cathodic reactions and hence, the inhibitors will have more effect on the cathodic reaction sites [34]. It can be observed that the current density (i_corr) decreases as the concentration of inhibitors increases, which confirms the corrosion inhibition activity of the studied ILs. The inhibition efficiency increases with increase in concentration of the inhibitors with a maximum value of 81.16% obtained for [HMIM][TfO] as shown in Table 1. The plots of %IE obtained from the potentiodynamic polarization study versus concentration of inhibitors are shown in Figure 2.

The %IE at 500 ppm follows the order [HMIM][TfO] > [HMIM][I] > [HMIM][BF₄] > [HMIM][PF₆]. It is clear from the results in Table 1 and Figure 2 that the trend of inhibition strength of the studied ILs is not easy to generalize for the range of concentrations of the ILs considered in this work. For instance, [HMIM][I] exhibits the highest inhibition activity at 100 ppm (58.25%), while [HMIM][BF₄] shows the highest inhibition potential at 200 ppm (71.32%). This dissension in the trend of inhibition efficiency with change in concentration of ILs is not impossible and can be attributed to self-aggregation of the ILs at their critical aggregation concentrations (cac). Similar trend has been reported for ionic liquids with imidazolium and pyridinium cations but without possible reasons [31]. Our suggestion is in line with the fact that ILs and surfactants are known to undergo self-aggregation and micellization at some characteristic concentrations [35,36,37,38,39,40,41,42]. Association into aggregates by ILs as well as micelle formation by surfactants are affected by a number of factors, which include alkyl chain, nature of counterions and interactions with water [35,36,37]. Since the studied ILs have different anions, they are expected to have different critical aggregate concentration (cac) values, which could have effect on their inhibition ability. Surface active compounds such as ILs and surfactants have been reported to exhibit higher corrosion inhibition potential in their aggregated or micelle forms [38,39]. There are some reports on the relationship between corrosion inhibition efficiency and surface activities [39,40,41,42]. Though, these reports are common for surfactant inhibitors with special attention on effect of alkyl chain length, the possibility of such relationship for ILs inhibitors having with common cations but different anions, such as the case in the present work cannot be ruled out. It is evident that further studies need to be carried out on the ability of the studied ILs to undergo association into aggregates in aqueous acidic medium for better understanding of the variation in their %IE at various concentrations. The higher %IE obtained for [HMIM][TfO] (at 500 ppm) compared with other ILs considered in this study can be attributed to the presence of more than one heteroatoms with high electronegativity (S, O) in its anions which enhances its adsorption on the surface of the mild steel thus improving its inhibition efficiency [43].

Figure 1. Potentiodynamic polarization curves for mild steel in 1 M HCl without and with different concentrations of [HMIM][BF₄], [HMIM][TfO], [HMIM][PF₆] and [HMIM][I].

Figure 1. Potentiodynamic polarization curves for mild steel in 1 M HCl without and with different concentrations of [HMIM][BF₄], [HMIM][TfO], [HMIM][PF₆] and [HMIM][I].

Figure 2. Inhibition efficiency from the potentiodynamic polarization technique versus concentration of inhibitors.

Figure 2. Inhibition efficiency from the potentiodynamic polarization technique versus concentration of inhibitors.

Table 1. Kinetic parameters obtained from potentiodynamic polarization study of mild steel in 1 M HCl without and with different concentrations of [HMIM][BF₄], [HMIM][TfO], [HMIM][PF₆] and [HMIM][I].

Concentration (ppm)	−Ecorr (mV)	icorr (mA/cm2)	Rp (Ohm/cm2)	βa (mV/dec)	βc (mV/dec)	%IEPDP
Blank	480	9.45	1.04	123	184	-
[HMIM][BF4]
100	537	3.89	4.88	198	220	58.84
200	498	2.91	2.13	101	141	69.21
300	512	2.52	2.17	100	126	73.33
400	516	2.14	5.79	160	178	77.35
500	512	2.06	2.37	79	142	78.20
[HMIM][TfO]
100	527	5.85	2.13	162	178	38.10
200	532	4.13	2.07	129	153	56.30
300	538	3.60	3.62	161	186	61.90
400	551	2.82	6.20	195	206	70.16
500	497	1.78	4.94	114	178	81.16
[HMIM][PF6]
100	505	7.36	1.57	159	168	22.12
200	484	4.39	1.84	114	164	53.54
300	478	3.75	1.42	89	138	60.32
400	502	3.34	1.74	81	165	64.76
500	475	2.50	4.26	124	198	73.54
[HMIM][I]
100	507	3.86	3.02	133	202	59.15
200	477	3.28	3.88	145	117	65.29
300	498	2.62	5.56	173	193	72.38
400	502	2.55	3.82	118	190	73.02
500	497	1.94	3.90	120	146	79.47

Table 1. Kinetic parameters obtained from potentiodynamic polarization study of mild steel in 1 M HCl without and with different concentrations of [HMIM][BF₄], [HMIM][TfO], [HMIM][PF₆] and [HMIM][I].

Concentration (ppm)	−Ecorr (mV)	icorr (mA/cm2)	Rp (Ohm/cm2)	βa (mV/dec)	βc (mV/dec)	%IEPDP
Blank	480	9.45	1.04	123	184	-
[HMIM][BF4]
100	537	3.89	4.88	198	220	58.84
200	498	2.91	2.13	101	141	69.21
300	512	2.52	2.17	100	126	73.33
400	516	2.14	5.79	160	178	77.35
500	512	2.06	2.37	79	142	78.20
[HMIM][TfO]
100	527	5.85	2.13	162	178	38.10
200	532	4.13	2.07	129	153	56.30
300	538	3.60	3.62	161	186	61.90
400	551	2.82	6.20	195	206	70.16
500	497	1.78	4.94	114	178	81.16
[HMIM][PF6]
100	505	7.36	1.57	159	168	22.12
200	484	4.39	1.84	114	164	53.54
300	478	3.75	1.42	89	138	60.32
400	502	3.34	1.74	81	165	64.76
500	475	2.50	4.26	124	198	73.54
[HMIM][I]
100	507	3.86	3.02	133	202	59.15
200	477	3.28	3.88	145	117	65.29
300	498	2.62	5.56	173	193	72.38
400	502	2.55	3.82	118	190	73.02
500	497	1.94	3.90	120	146	79.47

2.1.2. Electrochemical Impedance Spectroscopy (EIS)

The impedance method provides information about the kinetics of the electrode processes as well as the surface properties of the investigated systems. The shape of the impedance gives information about the mechanism of corrosion inhibition [44]. EIS measurements were carried out to study the corrosion of mild steel in 1 M HCl in the absence and presence of different concentrations of [HMIM][BF₄], [HMIM][TfO], [HMIM][PF₆] and [HMIM][I] ILs. The Nyquist and Bode plots were obtained and are presented in Figure 3 and Figure 4 respectively. Each spectrum in the Nyquist plots is characterized by a single full semicircle. It can be observed that the diameter of semicircle for the inhibitor containing systems have large capacitive loop with low frequency dispersion (inductive arc). Normally the anodic adsorbed intermediates that control the anodic reactions are the main factors behind the inductive arc [45,46]. The increasing diameter of capacitive loop obtained with increasing concentration of the ILs showed the inhibition of mild steel corrosion by the ILs. The curve fitting and simulation of the Nyquist and Bode plots was carried out by using the R(RQ) equivalent model circuit of the form in Figure 5. The kinetic parameters obtained from the fitting are presented in Table 2. The depression in Nyquist semicircles is a feature for solid electrodes and often referred to as frequency dispersion and attributed to the roughness and inhomogeneity of the solid electrode [47]. In this behaviour of solid electrodes, the parallel network charge transfer resistance-double layer capacitance is established where an inhibitor is present. For the description of a frequency-independent phase shift between an applied alternating current (ac) potential and its current response, a constant phase element (CPE) is used. The values of C_dl (double-layer capacitance) were calculated using the equation below:

$$C_{\text{dl}}={(Y_0{R}_{\text{ct}}^{\text{1-n}})}^{1/\text{n}}$$

(1)

where Y₀ is the CPE (constant phase capacitance) constant, R_ct the resistance of charge transfer and n is a CPE exponent which can be used as a gauge of the heterogeneity or roughness of the surface [33].

Figure 3. Nyquist plots for mild steel in 1 M HCl without and with different concentrations of [HMIM][BF₄], [HMIM][TfO], [HMIM][PF₆] and [HMIM][I].

Figure 3. Nyquist plots for mild steel in 1 M HCl without and with different concentrations of [HMIM][BF₄], [HMIM][TfO], [HMIM][PF₆] and [HMIM][I].

Figure 4. Bode plots (a) Phase angle vs. log f and (b) log Z vs. log f for mild steel in 1 M HCl without and with different concentrations of [HMIM][BF₄], [HMIM][TfO], [HMIM][PF₆] and [HMIM][I].

Figure 4. Bode plots (a) Phase angle vs. log f and (b) log Z vs. log f for mild steel in 1 M HCl without and with different concentrations of [HMIM][BF₄], [HMIM][TfO], [HMIM][PF₆] and [HMIM][I].

Figure 5. The equivalent model circuit of the impedance spectra.

Figure 5. The equivalent model circuit of the impedance spectra.

Table 2. Kinetic parameters obtained from the electrochemical impedance spectroscopy study on mild steel in 1 M HCl without and with different concentrations of [HMIM][BF₄], [HMIM][TfO], [HMIM][PF₆] and [HMIM][I].

Concentration. (ppm)		RS (Ω cm2)		Cdl (µF·cm−2)	Rct (Ω cm2)			%IEEIS
Blank		1.25		42.10	63.30			-
[HMIM][BF4]
100		1.80		19.12	146.30			56.70
200		1.74		10.24	220.70			71.32
300		2.19		9.92	254.40			75.32
400		2.50		8.19	280.00			77.39
500		2.07		7.01	294.90			78.54
[HMIM][TfO]
100		1.53		39.20	105.50			40.00
200		1.96		30.43	147.40			57.06
300		2.01		22.52	176.10			64.05
400		1.90		20.10	203.30			68.86
500		1.91		10.60	314.6			79.88
[HMIM][PF6]
100		2.39		30.02	79.60			20.48
200		1.62		25.23	127.70			50.43
300		3.20		16.93	162.70			61.09
400		2.49		15.78	192.70			67.15
500		2.10		14.29	222.50			71.55
[HMIM][I]
100		1.71		14.73	151.60			58.25
200		1.71		11.90	173.10			63.43
300		1.87		8.35	216.50			70.76
400		2.75		11.91	278.90			77.30
500		7.95		5.21	313.50			79.81

Table 2. Kinetic parameters obtained from the electrochemical impedance spectroscopy study on mild steel in 1 M HCl without and with different concentrations of [HMIM][BF₄], [HMIM][TfO], [HMIM][PF₆] and [HMIM][I].

Concentration. (ppm)		RS (Ω cm2)		Cdl (µF·cm−2)	Rct (Ω cm2)			%IEEIS
Blank		1.25		42.10	63.30			-
[HMIM][BF4]
100		1.80		19.12	146.30			56.70
200		1.74		10.24	220.70			71.32
300		2.19		9.92	254.40			75.32
400		2.50		8.19	280.00			77.39
500		2.07		7.01	294.90			78.54
[HMIM][TfO]
100		1.53		39.20	105.50			40.00
200		1.96		30.43	147.40			57.06
300		2.01		22.52	176.10			64.05
400		1.90		20.10	203.30			68.86
500		1.91		10.60	314.6			79.88
[HMIM][PF6]
100		2.39		30.02	79.60			20.48
200		1.62		25.23	127.70			50.43
300		3.20		16.93	162.70			61.09
400		2.49		15.78	192.70			67.15
500		2.10		14.29	222.50			71.55
[HMIM][I]
100		1.71		14.73	151.60			58.25
200		1.71		11.90	173.10			63.43
300		1.87		8.35	216.50			70.76
400		2.75		11.91	278.90			77.30
500		7.95		5.21	313.50			79.81

The results in Table 2 show that the R_ct values in the presence of inhibitors are generally higher than that of the blank system. This can be attributed to the adsorption of ionic liquid inhibitors to mild steel surface thereby minimizing direct or continuous exposure of the mild steel to the corrosive medium. There is also an increase in R_ct values with increasing concentration of the inhibitors. This can be attributed to increase in number of molecules of ILs that bind to the mild steel surface. On the other hand, the C_dl values decreased accordingly except at 500 ppm concentration of [HMIM][BF₄] and [HMIM][I] where a small increase in the C_dl value was noticed. The decrease in C_dl values at the metal/solution interface with increasing inhibitor concentration can result from the decrease in local dielectric constant which indicates that the inhibitors were adsorbed on the surface at both anodic and cathodic sites [48]. Decrease in C_dl values could also mean an increase in the thickness of a protective layer at mild steel electrode surface, therefore enhancing the corrosion resistance of the steel. The thickness of the protective layer (d) is related to C_dl according to the equation:

$$C_{\text{dl}}=\frac{\epsilon {\epsilon }_0}{d}$$

(2)

where, ε is the dielectric constant of the protective layer and ε₀ is the permittivity of free space.

It was also observed that the %IE increases as the concentration of the ILs increases reaching a maximum value of 79.88% for [HMIM][TfO] at 500 ppm. The plot of %IE values obtained from the electrochemical impedance spectroscopy study versus concentration of inhibitors is shown in Figure 6. The variation of %IE with concentration shown in Figure 6 is similar to the one presented in Figure 2 for the potentiodynamic polarization experiments. The discussion of the trend of %IE for the studied ILs presented under Section 2.1.1 therefore applies.

Figure 6. Inhibition Efficiency versus Concentration from the EIS method.

Figure 6. Inhibition Efficiency versus Concentration from the EIS method.

2.2. Adsorption Isotherms

Adsorption isotherms are used to describe the nature of metal/inhibitor interactions. The results obtained from both the polarization and impedance studies were fitted into different adsorption isotherms. Adsorption of [HMIM][BF₄], [HMIM][TfO], and [HMIM][I] were found to obey the Langmuir adsorption equation of the form:

$$\frac{C}{\theta }=C+\frac{1}{K_{ads}}$$

(3)

where C is the concentration of the inhibitors, θ the degree of surface coverage, K_ads is the equilibrium constant of the adsorption/desorption process. However, the adsorption of [HMIM][PF₆] on mild steel surface followed the Temkin adsorption isotherm equation of the form:

–2aθ = ln K + ln C

(4)

where θ is surface coverage, K_ads equilibrium constant of adsorption/desorption process, “a” is molecular interaction parameter, and C is the concentration of the inhibitor. The respective adsorption isotherms are shown in Figure 7. The estimated K_ads and change in Gibbs free energy of adsorption (∆G°_ads) for the four ILs are presented in Table 3. The change in Gibbs free energies (∆G°_ads) is related to the K_ads according to the equation:

$$\mathrm{\Delta }{G^o}_{ads}=-RT\ln (55.5K_{ads})$$

(5)

where ∆G°_ads is the change in Gibbs free energy, R is gas constant, T is absolute temperature, K_ads is the adsorption equilibrium constant and the constant value (55.5) is the molar concentration of water in solution. High values of K_ads and negative values of ∆G°_ads obtained for the studied inhibitors as shown in Table 3 imply effective adsorption and spontaneous adsorption of the ILs to mild steel surface. The value of Temkin parameter “a” indicates the repulsive nature of the inhibitor on the metal surface. The negative values obtained for [HMIM][PF₆] in this study suggest possibility of repulsion in the adsorption layer [49]. The magnitude of ∆G°_ads determines the nature of adsorption process whether it is physisorption or chemisorption. Values around −20 kJ·moL⁻¹ and less are associated with physical adsorption mechanism or physisorption, while values around −40 kJ·moL⁻¹ and more are associated with chemical adsorption mechanism or chemisorption [50]. The results in Table 3 show that the magnitudes of ∆G°_ads for the four inhibitors are greater than 20 but less than 40. This suggests that the adsorption process of the studied inhibitors features both physisorption and chemisorption [17,51,52].

Table 3. Adsorption parameters derived from the Langmuir and Temkin adsorption isotherm plots for the inhibitors.

Inhibitor		Kads (103 × moL−1)		Molecular Interaction Parameter (ppm)	$-\mathrm{\Delta }{G}_{\mathrm{ads}}^o$ (kJ·moL−1)
Potentiodynamic Polarization
[HMIM][BF4]		4.65			−31.41
[HMIM][TfO]		1.76			−28.96
[HMIM][I]		7.37			32.56
[HMIM][PF6]		4.55		−1.65	31.35
Impedance
[HMIM][BF4]		4.03			−31.04
[HMIM][TfO]		1.73			−28.92
[HMIM][I]		3.45			−30.65
[HMIM][PF6]		6.06		−1.58	−32.07

Table 3. Adsorption parameters derived from the Langmuir and Temkin adsorption isotherm plots for the inhibitors.

Inhibitor		Kads (103 × moL−1)		Molecular Interaction Parameter (ppm)	$-\mathrm{\Delta }{G}_{\mathrm{ads}}^o$ (kJ·moL−1)
Potentiodynamic Polarization
[HMIM][BF4]		4.65			−31.41
[HMIM][TfO]		1.76			−28.96
[HMIM][I]		7.37			32.56
[HMIM][PF6]		4.55		−1.65	31.35
Impedance
[HMIM][BF4]		4.03			−31.04
[HMIM][TfO]		1.73			−28.92
[HMIM][I]		3.45			−30.65
[HMIM][PF6]		6.06		−1.58	−32.07

Figure 7. Langmuir adsorption isotherms of [HMIM][BF₄], [HMIM][TfO], [HMIM][I] and Temkin adsorption isotherm of [HMIM][PF₆] obtained from (a) polarization and (b) impedance experimental data.

Figure 7. Langmuir adsorption isotherms of [HMIM][BF₄], [HMIM][TfO], [HMIM][I] and Temkin adsorption isotherm of [HMIM][PF₆] obtained from (a) polarization and (b) impedance experimental data.

2.3. Spectroscopic Analysis

2.3.1. Fourier Transform Infrared Spectroscopy (FTIR)

Fourier transform infrared (FTIR) spectroscopy was used to investigate possible chemical interactions between the ILs and mild steel. The FTIR spectra of the pure ILs and the resulting solution after 24 h of mild steel immersion in 1 M HCl with 500 ppm ILs were studied and presented in Figure 8. Though reports on vibrational spectra of 1-hexyl-3-methylimidazolium ILs are still scanty compared to the 1-butyl analogues, various vibrational bands characteristic of the imidazole ring in imidazolium-based ILs have been reported in literature [53,54,55,56,57,58]. These include the bands at 3000–3250 cm⁻¹ for the C-H stretching of imidazole ring, those at 750–755 cm⁻¹ for out-of-plane bending of imidazole ring, bands at 1500–1620 cm⁻¹ for stretching of the imidazole ring and those at 1020–1050 cm⁻¹ for ring elongation along the N-C stretch [53,54,55,56,57,58]. Berg et al. (2005) reported the vibrational spectra of 1-hexyl-3-methylimidazolium chloride and 1-hexyl-3-methylimidazolium hexafluorophosphate and their binary mixture in which it was observed that anions have little or no significant effect on the positions of the vibrational bands of the imidazole ring [58]. Some of the observed spectral bands for the pure ILs in the present work and assignments of the bands are listed in Table 4. The C-H stretch of imidazole ring was observed at 3163 cm⁻¹ for pure [HMIM][BF₄] and 3140 cm⁻¹ for pure [HMIM][I]. This band might have been affected by the strong cation-anion interactions in pure [HMIM][TfO] leading to its absence in the spectrum. The bands for methylene (–CH₂) stretching were observed at 2939 cm⁻¹ and 2866 cm⁻¹ in [HMIM][BF₄], 2946 cm⁻¹ and 2866 cm⁻¹ in [HMIM][TfO] and 2931 cm⁻¹ and 2860 cm⁻¹ in [HMIM][I]. These bands were also reported to appear between 2862–2937 cm⁻¹ in [HMIM][Cl] and [HMIM][PF₆] according to the work by Berg et al. [58]. Bands for the deformations of the two –CH₃ appeared at 1573 cm⁻¹ and 1465 cm⁻¹ (in both pure [HMIM][BF₄] and [HMIM][TfO]), while the same bands appeared respectively at 1567 cm⁻¹ and 1459 cm⁻¹ in pure [HMIM][I]. These bands were also observed between 1442–1570 cm⁻¹ in the work of Berg et al. [58] on pure [HMIM][Cl], [HMIM][PF₆] and their binary mixture. In the absence of FTIR spectrum for the pure [HMIM][PF₆] in the present work, the FTIR features of [HMIM][PF₆] after mild steel immersion were compared with the vibrational spectrum of pure [HMIM][PF₆] reported by Berg and his co-workers (Table 4) [58]. As shown in Figure 8, all the prominent bands in the pure ILs have disappeared upon mild steel immersion. This is due to the adsorption of the ILs on mild steel surface.

Figure 8. FTIR spectra of pure, 500 ppm solution and 500 ppm with mild steel immersed of the ILs [HMIM][BF₄], [HMIM][TfO], [HMIM][I] and [HMIM][PF₆].

Figure 8. FTIR spectra of pure, 500 ppm solution and 500 ppm with mild steel immersed of the ILs [HMIM][BF₄], [HMIM][TfO], [HMIM][I] and [HMIM][PF₆].

Table 4. Assignment of major vibrational bands in the FTIR spectra of the pure ILs.

[HMIM][BF4]	[HMIM][TfO]	[HMIM][I]	[HMIM][PF6] a	Assignments b
628	-	628	623	ring def (C2-H oopl bend) + N-C6 N-C7 iph str + C7H2 rock + C7-C8-C9 bend
657	642	645	658	N-C6 str + ring def (N1 and H on C2 oopl ooph departure) + C8H2 wag + N-C7-C8 bend + ring def (bend around line NN) + C8H2 rock + N-C7-C8 bend
758	765	751	762	ring C-H oopl iph bend (umbrella)
851	866	823	817, 852	C7H2 rock and chain def
1053	1032	-	1026	ring elongation (C3) + N-C6 str
1085	-	-	1079	chain ooph C-C str
1170	1170	1170	1169	chain ooph C-C str
-	1256	-	1257	chain def, CH2 twi
1343	-	-	1339	chain (CH2 twi)
1386	-	1386	1389	ring breathing + C7H2 twi
1465	1465	1460	1460	C7H2 + C8H2 + C9H2 + C10H2 def
1573	1573	1573	1570	C12H3 def & C6H3 def
2866	2866	2860	2866	methylene CH2 str
2939	2946	2931	2927, 2937	methylene CH2 str
-	-	3069	3115	C-H str. (ring, position 2)
3163	-	3140	3180	C-H str. (ring, position 4,5)

^a data from Ref. [58]. ^b abbreviations used for different vibrational modes: bend = angle bending (scissoring), breathing = all ring bonds iph, def = more complicated deformation of skeleton, iph = in phase (symmetric), oopl = out of ring plane, ooph = opposite motion, out of phase (asymmetric), ring = imidazole core, rock = rocking, str = bond stretching, twi = twisting of CH₂ group or chain, wag = wagging.

Table 4. Assignment of major vibrational bands in the FTIR spectra of the pure ILs.

[HMIM][BF4]	[HMIM][TfO]	[HMIM][I]	[HMIM][PF6] a	Assignments b
628	-	628	623	ring def (C2-H oopl bend) + N-C6 N-C7 iph str + C7H2 rock + C7-C8-C9 bend
657	642	645	658	N-C6 str + ring def (N1 and H on C2 oopl ooph departure) + C8H2 wag + N-C7-C8 bend + ring def (bend around line NN) + C8H2 rock + N-C7-C8 bend
758	765	751	762	ring C-H oopl iph bend (umbrella)
851	866	823	817, 852	C7H2 rock and chain def
1053	1032	-	1026	ring elongation (C3) + N-C6 str
1085	-	-	1079	chain ooph C-C str
1170	1170	1170	1169	chain ooph C-C str
-	1256	-	1257	chain def, CH2 twi
1343	-	-	1339	chain (CH2 twi)
1386	-	1386	1389	ring breathing + C7H2 twi
1465	1465	1460	1460	C7H2 + C8H2 + C9H2 + C10H2 def
1573	1573	1573	1570	C12H3 def & C6H3 def
2866	2866	2860	2866	methylene CH2 str
2939	2946	2931	2927, 2937	methylene CH2 str
-	-	3069	3115	C-H str. (ring, position 2)
3163	-	3140	3180	C-H str. (ring, position 4,5)

^a data from Ref. [58]. ^b abbreviations used for different vibrational modes: bend = angle bending (scissoring), breathing = all ring bonds iph, def = more complicated deformation of skeleton, iph = in phase (symmetric), oopl = out of ring plane, ooph = opposite motion, out of phase (asymmetric), ring = imidazole core, rock = rocking, str = bond stretching, twi = twisting of CH₂ group or chain, wag = wagging.

2.3.2. Ultraviolet-visible (UV-vis) Spectroscopy

UV-vis spectroscopy was used to provide evidence of interactions between mild steel and ILs. The UV-vis absorption spectra of the pure ILs, the 500 ppm solution of ILs and the resulting solution after 24 h of mild steel immersion were recorded and presented in Figure 9. The absorption spectra of the pure ILs show a single shoulder-like absorption peak at 226 nm, 225 nm and 218 nm for [HMIM][BF₄], [HMIM][TfO] and [HMIM][I] respectively corresponding to n-π* and/or π-π* transitions. The UV-vis spectrum of [HMIM][I] also shows additional peak at 245 nm. The absorption spectrum of the pure [HMIM][PF₆] was not reported in this work because it was characterized with a lot of noise, which may be due to impurities or high concentration of the pure [HMIM][PF₆]. The 500 ppm solutions of the ILs in 1 M HCl show absorption characteristics similar to the pure ILs but with generally lower absorbance and slight blue shift in the maximum absorption wavelength to 222 nm, 220 nm and 242 nm for [HMIM][BF₄], [HMIM][TfO] and [HMIM][I] respectively. The absorption spectrum of 500 ppm solution of [HMIM][PF₆] also shows a shoulder-like peak at 220 nm. Upon mild steel immersion, there is a significant change in the UV-vis absorption spectra of the studied ILs as they undergo further blue shift and now appear at 211 nm, 210 nm, 210 nm and 222 nm for [HMIM][BF₄], [HMIM][TfO], [HMIM][PF₆] and [HMIM][I] respectively. This blue shift in the wavelength of maximum absorbance is attributed to the formation of Fe/IL complex. Apart from [HMIM][I], the other three ILs show new absorption peak at 248 nm. This new peak can be attributed to transition between π-bonding orbital of the Fe/IL complex and the π* (antibonding) orbital of the anion. The absence of this new peak in [HMIM][I] can be due to lack of appropriate π*-orbital in the iodide ion.

Figure 9. UV/Vis spectra of the pure [HMIM][BF₄], [HMIM][TfO], [HMIM][I] and [HMIM][PF₆], and their 500 ppm solution without and with mild steel immersed.

Figure 9. UV/Vis spectra of the pure [HMIM][BF₄], [HMIM][TfO], [HMIM][I] and [HMIM][PF₆], and their 500 ppm solution without and with mild steel immersed.

2.3.3. Quantum Chemical Calculations

Geometry optimizations and quantum chemical calculations were carried out on the studied ILs using the B3LYP/6-31G+(d,p) model. The optimized structures of the ILs are shown in Figure 10. The frontier molecular orbital surfaces provide information about the occupied molecular orbital (HOMO) of the inhibitor that may be responsible for forward donation of a pair of electrons to the vacant d-orbital of the metal and the unoccupied molecular orbital (LUMO) of the inhibitor that may be liable to accept a pair of electrons from an electron-rich metal surface during back-bonding. The HOMO and LUMO graphics of the optimized structures are shown in Figure 11. It can be observed from Figure 11 that the HOMO of [HMIM][I] and [HMIM][TfO] are essentially localized on the corresponding anions; I⁻ and TfO⁻ respectively. This may be due to high polarizability of I⁻ ion and high electron density of TfO⁻. The HOMO of [HMIM][BF₄] and [HMIM][PF₆] on the other hand are significantly localized on the imidazolium ring and extended along the hexyl side chain as well as to some of the fluorine atoms in the anions. The LUMO surfaces of the four ILs are mainly distributed on the imidazolium ring. This may be due to the presence of highly electronegative nitrogen atoms in the imidazolium ring, which can make the ring to be relatively electron-deficient, and the fact that it is a cationic moiety. The numerical values obtained for some of the quantum chemical parameters are listed in Table 5. The results in Table 5 show that [HMIM][I] has the highest value of E_HOMO, while [HMIM][PF₆] is characterized with the lowest value of E_LUMO among the four ILs. It can be inferred from the E_HOMO results that [HMIM][I] and [HMIM][TfO] have higher electron donating ability than [HMIM][BF₄] and [HMIM][PF₆]. [HMIM][I] and [HMIM][TfO] also have lower energy gap (∆E) than [HMIM][BF₄] and [HMIM][PF₆]. This connotes higher reactivity with mild steel, which is in agreement with their higher percentage inhibition efficiency as observed from polarization experiment. The values of hardness (η) and softness (σ) also favour better reactivity of [HMIM][I] and [HMIM][TfO] over [HMIM][BF₄] and [HMIM][PF₆] and hence, better corrosion inhibition ability. Dipole moment does not appear to be a good descriptor of the corrosion inhibition potency of the studied ILs because the values of the dipole moments obtained for the inhibitors are relatively close.

Mulliken population analysis provides information about the amount of charges centred on each atom in a molecule. An atom with large amount of negative charge is expected to be prone to an attack by an electron-deficient species. The estimated Mulliken atomic charges for the studied ILs are displayed alongside the optimized structures in Figure 12. It can be observed from Figure 12 that the I-ion in [HMIM][I], the sulphur and oxygen atoms in [HMIM][TfO], the fluorine atoms in [HMIM][BF₄] and [HMIM][PF₆] all show relatively high negative values of Mulliken atomic charges. This suggests that the metallic atom with a charge-deficient centre will readily be attracted to the appropriate atom in the anionic moiety of the studied ILs.

Table 5. Quantum chemical parameters of the studied ILs.

ILs	Quantum Chemical Parameters
	Dipole Moment (Debye)	EHOMO (eV)	ELUMO (eV)	∆E (eV)	Hardness (η)	Softness (σ)
[HMIM][I]	13.36	−4.53	−1.36	3.17	1.58	0.63
[HMIM][TfO]	12.80	−6.67	−1.49	5.18	2.59	0.39
[HMIM][BF4]	12.58	−8.24	−1.37	6.87	3.44	0.29
[HMIM][PF6]	14.26	−8.42	−1.54	6.88	3.44	0.29

Table 5. Quantum chemical parameters of the studied ILs.

ILs	Quantum Chemical Parameters
	Dipole Moment (Debye)	EHOMO (eV)	ELUMO (eV)	∆E (eV)	Hardness (η)	Softness (σ)
[HMIM][I]	13.36	−4.53	−1.36	3.17	1.58	0.63
[HMIM][TfO]	12.80	−6.67	−1.49	5.18	2.59	0.39
[HMIM][BF4]	12.58	−8.24	−1.37	6.87	3.44	0.29
[HMIM][PF6]	14.26	−8.42	−1.54	6.88	3.44	0.29

Figure 10. Gas phase optimized structures of [HMIM][BF₄], [HMIM][TfO], [HMIM][I] and [HMIM][PF₆] at B3LYP/6-31+G(d,p) level of theory.

Figure 10. Gas phase optimized structures of [HMIM][BF₄], [HMIM][TfO], [HMIM][I] and [HMIM][PF₆] at B3LYP/6-31+G(d,p) level of theory.

Figure 11. Graphical surfaces of the HOMO (left) and LUMO (right) of the gas phase optimized structures of [HMIM][BF₄], [HMIM][TfO], [HMIM][I] and [HMIM][PF₆] at B3LYP/6-31G+(d,p) level of theory.

Figure 11. Graphical surfaces of the HOMO (left) and LUMO (right) of the gas phase optimized structures of [HMIM][BF₄], [HMIM][TfO], [HMIM][I] and [HMIM][PF₆] at B3LYP/6-31G+(d,p) level of theory.

Figure 12. Mulliken atomic charges with optimized structures of [HMIM][BF₄], [HMIM][TfO], [HMIM][I] and [HMIM][PF₆] obtained at B3LYP/6-31+G(d,p) level of theory.

Figure 12. Mulliken atomic charges with optimized structures of [HMIM][BF₄], [HMIM][TfO], [HMIM][I] and [HMIM][PF₆] obtained at B3LYP/6-31+G(d,p) level of theory.

Fukui indices were also calculated for the studied ILs as a measure of local reactivity. The preferred site for nucleophilic attack is the atom/region in the molecule with the highest value of f ⁺ while the most probable site for electrophilic attack is the atom/region in the molecule with the highest value of f ⁻. The Fukui functions are utilised in the study of corrosion inhibitors to characterize local electron-donating and electron-accepting ability of the inhibitor. Hence, the preferred sites at which the inhibitor is most likely to interact with either an electron-rich or electron-deficient metal surface can be predicted. The results obtained for the f ⁺ and f ⁻ are shown in Figure 13. Due to convergence problem, effective core potential was put on the iodide ion in [HMIM][I] using the LanL2DZ basis and 6-31G(d) for other atoms. 6-31+G(d,p) basis set was used for other ILs. The regions of a molecule where the Fukui function is large are chemically softer than the regions where the Fukui function is small [59]. Fukui function provide information about the atoms in a molecule that have a tendency to either donate (nucleophilic character) or accept (electrophilic character) an electron or pair of electrons [60]. The local selectivity of a corrosion inhibitor is best analysed by means of condensed Fukui function. For all the studied ILs, the preferred sites for nucleophilic attack are the N and some of the C atoms, especially C-2 of the imidazolium ring. This is because the imidazolium ring is positively charged and can readily receive charges when attacked by a nucleophilic reagent. The preferred sites for electrophilic attack are essentially on the anions of each IL. As shown in Figure 13, the preferred site for electrophilic attack is the iodide ion for [HMIM][I], the oxygen atoms of the sulfonate for [HMIM][TfO], some of the fluorine atoms of the fluoroborate for [HMIM][BF₄] and fluorine atoms of the fluorophosphate for [HMIM][PF₆]. This is due to high electron density of these atoms, which make it possible for them to donate charge when attacked by an electrophilic reagent.

Figure 13. Fukui indices, f ⁺ (Left) and f ⁻ (Right) of [HMIM][I] ^a,b, [HMIM][TfO] ^c, [HMIM][BF₄] ^b and [HMIM][PF₆] ^c at B3LYP/6-31+G(d,p). ^a B3LYP/6-31G(d)//LanL2DZ basis set; ^b Isosurface value = 0.04; ^c Isosurface value = 0.3.

Figure 13. Fukui indices, f ⁺ (Left) and f ⁻ (Right) of [HMIM][I] ^a,b, [HMIM][TfO] ^c, [HMIM][BF₄] ^b and [HMIM][PF₆] ^c at B3LYP/6-31+G(d,p). ^a B3LYP/6-31G(d)//LanL2DZ basis set; ^b Isosurface value = 0.04; ^c Isosurface value = 0.3.

3. Experimental Section

3.1. Materials

The mild steel sheet used for this work was of the composition 0.02% Phosphorus (P), 0.37% Manganese (Mn), 0.03% Sulphur (S), 0.01% Molybdenum (Mo), 0.039% Nickel (Ni), 0.21% Carbon (C) and the remaining part being iron (Fe). For all electrochemical measurements, mild steel sheet was cut into 1 cm × 1 cm sizes and embedded in a Teflon holder with epoxy resin thereby exposing a surface area of 1 cm². Mild steel surface was mechanically abraded and treated to a finely ground surface by polishing it with SiC papers of 600–1200 grit sizes. The polished surface was washed with water, degreased with ethanol, rinsed with water again and finally dried with a clean towel paper. Mild steel specimens were used for appropriate studies immediately after surface preparation.

3.2. Inhibitors

The ILs used in this study were purchased from Sigma-Aldrich Chemicals. The molecular structures of the ILs 1-Hexyl-3-methylimidazolium trifluoromethanesulfonate [HMIM][TfO], 1-Hexyl-3-methylimidazolium tetrafluoroburate [HMIM][BF₄], 1-Hexyl-3-methylimidazolium iodide [HMIM][I] and 1-Hexyl-3-methylimidazolium hexafluorophosphate [HMIM][PF₆] are shown in Figure 14.

Figure 14. Molecular Structures of 1-Hexyl-3-methylimidazolium hexaflurophosphate ([HMIM][PF₆]), Hexyl-3-methylimidazolium trifluoromethanesulfonate ([HMIM][TFO]), 1-Hexyl-3-methylimidazolium iodide ([HMIM][I]) and 1-Hexyl-3-methylimidazolium tetrafluoroborate ([HMIM][BF₄]).

Figure 14. Molecular Structures of 1-Hexyl-3-methylimidazolium hexaflurophosphate ([HMIM][PF₆]), Hexyl-3-methylimidazolium trifluoromethanesulfonate ([HMIM][TFO]), 1-Hexyl-3-methylimidazolium iodide ([HMIM][I]) and 1-Hexyl-3-methylimidazolium tetrafluoroborate ([HMIM][BF₄]).

3.3. Solutions

The aggressive solution of 1 M HCl was prepared by diluting the analytical grade 32% HCl from MERCK CHEMICALS with distilled water. The inhibitor concentrations: 100, 200, 300, 400 and 500 ppm were prepared.

3.4. Electrochemical Measurements

The electrochemical measurements were performed under unstirred conditions at room temperature (30 °C) using the Autolab (PGSTAT 302N) electrochemical work station from Metrohm driven by the general purpose electrochemical system (GPES) software by Eco Chemie. A stabilization time of 30 min was allowed before the electrochemical measurements were performed and this time was deemed to be sufficient to attain a stable open circuit potential (OCP). A three-electrode cell composed of a platinum counter electrode (CE), a silver-silver chloride electrode in 3 M KCl (Ag/AgCl, 3 M KCl) as a reference electrode (RE) and a mild steel specimen of 1 cm² surface area as a working electrode (WE) was used for all electrochemical measurements. A potential range of −800 to −200 V with scan rate 1 mV·s⁻¹ was utilized to generate the potentiodynamic polarization curves. The Tafel slope analysis tool of the GPES software was used to obtain relevant kinetic parameters such as corrosion current density (i_corr), anodic and cathodic Tafel slopes (β_a and β_c) and polarization resistance (R_P). The inhibition efficiency was evaluated from the measured i_corr value using the relationship

$$\%I{E}_{PDP}=100\left(\frac{i_{corr}^o-i_{corr}^i}{i_{corr}^o}\right)$$

(6)

where $i_{corr}^o$ and $i_{corr}^i$ are values of corrosion current density in the absence and presence of inhibitors respectively.

The EIS measurements were carried out at the frequency range of 100,000.0 Hz to 1.0 Hz at an amplitude of 5 mV peak-to-peak using AC signal at the OCP. Parameters such as the solution resistance (R_s), the resistance of charge transfer (R_ct) and the capacity of double layer (C_dl) were obtained from the EIS study by fitting the experimental data to the R_s(R_ctQ) equivalent model circuit using the fit and simulation tool of the GPES software. The inhibition efficiency was calculated using the equation:

$$\%I{E}_{EIS}=100\left(1-\frac{R_{ct}^o}{R_{ct}}\right)$$

(7)

where $R_{ct}^o$ is the charge transfer resistance in the absence of the inhibitor and $R_{ct}$ is the charge transfer resistance in the presence of the inhibitors.

All potentials were measured with reference to that of Ag/AgCl in 3 M KCl.

3.5. Fourier Transform Infrared (FTIR) and Ultraviolet-Visible (UV-Vis) Spectroscopy Experiments

The FTIR and UV-vis experiments were carried out on the pure ILs and also on the resulting solutions from the aggressive media containing 500 ppm of the studied ILs after 24 h of mild steel immersion. Fourier transform infrared spectrophotometer (Cary 600 series FTIR spectrometer by Agilent Technology) and the UV-visible spectrophotometer (Cary 300 series UV-vis spectrometer by Agilent Technology) were used for the FTIR and UV-vis studies respectively. Mild steel samples immersed in the aggressive solutions were prepared as explained in Section 3.1 above. The FTIR spectroscopic measurements were recorded between 500–4000 cm⁻¹ wavenumbers, while the UV-vis absorption profiles were recorded between 200–400 nm wavelengths in the double-beam UV-vis equipment using the 1 cm quartz cell.

3.6. Quantum Chemical Calculations

All geometry optimizations and quantum chemical calculations were performed using the density functional theory (DFT) method. The Becke’s three parameter hybrid functional together with the Lee-Yang-Parr correlation functional (B3LYP) [61] and 6-31+G(d,p) basis set were used for the calculations, except when mentioned otherwise. The frontier molecular orbital parameters, i.e., the highest occupied molecular orbital energy (E_HOMO) and the lowest unoccupied molecular orbital energy (E_LUMO) are often used to corroborate observed inhibition potency of corrosion inhibitors. The energy gap (∆E, ∆E = E_LUMO – E_HOMO) and other chemical reactivity indices including electron affinity (A) and ionization potential (I) are related to the frontier molecular orbital energy parameters according to the Koopman’s approximation [62] and also used to explain the observed inhibition potency.

Global hardness (η) and softness (σ) are molecular properties that also have direct relationship with the molecular reactivity [63]. Soft molecules are more reactive than hard molecules if electron transfer or rearrangement is necessary for the reaction. Hard molecules resist changes in their electron density distribution [64].

$$\eta \cong -\frac{1}{2}(E_{HOMO}-E_{LUMO})$$

(8)

$$\sigma =\frac{1}{\eta }\cong -\frac{2}{(E_{HOMO}-E_{LUMO})}$$

(9)

The Fukui function, f(r), is the differential change in electron density due to an infinitesimal change in the number of electrons [65]. The nucleophilic and electrophilic Fukui functions are often used to describe local reactivity condensed on an atom in a molecule. Atom condensed Fukui indices can also be calculated using the finite difference approximation [60]:

$$f^{+}={\rho }_{(N+1)}-{\rho }_N$$

(10)

$$f^{-}={\rho }_N-{\rho }_{(N-1)}$$

(11)

All geometry optimizations were carried out in vacuo using the Gaussian 09 W D (V.01) [66] software. Molecular modelling and initial geometries were generated using the Gaussview 5.0 software. Fukui functions were visualized using Multiwfn software [67,68].

4. Conclusions

The following conclusions can be drawn from the results obtained from this study:

• The electrochemical measurements were performed and the inhibition efficiency of the ILs studied was found to be increasing as the inhibitor concentration increased (from 100 ppm to 500 ppm).
• The %IE at 500 ppm follows the order [HMIM][TfO] > [HMIM][I] > [HMIM][BF₄] > [HMIM][PF₆] though the trend of inhibition strength of the studied ILs is not easy to generalize for the range of concentrations of the ILs considered in this work due to the fact that ILs and surfactants are known to undergo self-aggregation and micellization at some characteristic concentrations. Association into aggregates by ILs as well as micelle formation by surfactants are affected by a number of factors, which include alkyl chain, nature of counterions and interactions with water. Since the studied ILs have different anions, they are expected to have different critical aggregate concentration (cac) values, which could have effect on their inhibition ability.
• Mixed-type inhibition mechanism has been proposed for the studied ILs based on the results obtained from the electrochemical studies.
• Three of the ILs, 1-Hexyl-3-methylimidazolium iodide [HMIM][I], 1-Hexyl-3-methylimidazolium tetrafluoroburate [HMIM][BF₄] and 1-Hexyl-3-methylimidazolium trifluoromethanesulfonate [HMIM][TfO] obeyed the Langmuir adsorption isotherm while 1-Hexyl-3-methylimidazolium hexafluorophosphate [HMIM][PF₆] obeyed the Temkin adsorption isotherm.
• Adsorption parameters such as K_ads and ∆G°_ads were obtained from the calculations. Results showed that the adsorption process was spontaneous since ∆G°_ads value was negative. The range of values of ∆G°_ads suggest that the adsorption mechanism of the studied ILs features both physisorption and chemisorption.
• Fourier transform infrared (FTIR) and ultraviolet-visible (UV-vis) spectroscopy studies have been used to support the results obtained from the electrochemical technique.
• Trends in the quantum chemical parameters support the order of inhibition efficiency values obtained from the experimental data.