Synthesis, Characterization and Computational Studies on the Corrosion Inhibitive Potentials of (E)-3-(2-P-Tolyldiazenyl)-1-Ni

Synthesis, characterization and computational studies on the corrosion inhibitive potentials of (e)-3-(2-p-tolyldiazenyl)-1-nitrosonaphthalen-2-ol

Solayide Justinah AMOKO^1,3, Olawale Folorunso AKINYELE^2*, Oluwatoba Emmanuel OYENEYIN¹, Dare Samson OLAYANJU², Christopher Olu ABOLUWOYE¹

¹Department of Chemical Sciences, Adekunle Ajasin University, Akungba-Akoko, Ondo State, Nigeria

²Department of Chemistry, Obafemi Awolowo University, Ile-Ife, Nigeria

³Department of Chemistry, Adeyemi College of Education, Ondo, Ondo State, Nigeria

Emails: ¹temiamoko@gmail.com, ²ofakinyele@oauife.edu.ng, ³emmanueltoba@gmail.com, ⁴oladare78@yahoo.com and ⁵oluaboluwoye@yahoo.com.

*Corresponding Author Phone: +2348023410301

Abstract

A novel (E)-3-(2-P-Tolyldiazenyl)-1-nitrosonaphthalen-2-ol (NAD) has been synthesized and characterized via Fourier Transform Infrared (FTIR), UV/Vis, ¹H-NMR and ¹³C-NMR spectroscopic techniques. Weight loss analysis showed that this molecule possesses excellent corrosion inhibitive potentials. Variations of inhibition efficiency with concentration and temperature were observed and the results obtained show that inhibition efficiency increases with increase in concentration while it reduces with an increase in temperature. The efficiency of this molecule was validated with theoretical models using the density functional theory (DFT) method with the hybrid functional, Becke Three Lee Yang Parr (B3LYP) correlation with 6-31G* basis set. It was observed that the molecule has very good corrosion inhibitive potentials.

Keywords

Density Functional Theory (DFT); Polarization; Activation parameters; Azo-dye; Thermodynamic parameter; Adsorption; Inhibition efficiency

Introduction

One of the most practical ways to prevent corrosion of metals and alloys in acidic media, a scourge peculiar to the oil and gas industries, is to use corrosion inhibitors, which are mainly organic compounds containing heteroatoms like sulphur, nitrogen, oxygen and phosphorus with lone pair of electrons and as a result facilitate adsorption on metal surfaces [1-4]. These inhibitors are added with the aim of reducing metal loss when in contact with acid media. Azo dyes possess π-electrons systems and heteroatoms in the moieties, this enhances adsorption on mild steel through the formation of covalent bonds [5,6]. They are adsorbed on the metal surface by forming protective layers that prevent attacks by acid media used in pickling, descaling and oil well acidizing. Methods such as the gravimetric; which gives information about the average rate of corrosion and inhibition efficiency [6-8], potentiodynamic polarization [8,9], electrochemical impedance spectroscopy [10], Fourier transform infra-red (FTIR) spectroscopy [6] and scanning electron microscope (SEM) [6,8] have been used for corrosion inhibition studies. Recently, quantum chemical calculations have been employed in investigating and predicting the corrosion inhibition potentials of molecules [4,6,10,11]. This is because they can be used to explain physical parameters like reactivities and electronic behaviours. Since it is important to describe the electronic behaviours, the density functional theory (DFT) is usually used in predicting and understanding chemical processes like corrosion inhibition processes either as a method to validate experimental findings or solely to explain inhibitive potentials of organic molecules [10-18]. Azo dyes have been extensively investigated and reported as corrosion inhibitors [8,9,12]. This may be due to the ability of complex formation between metal-ions and the azo nitrogen binding at the electrode surface [8], steric effects and electron density of donor atoms [13]. This work presents the validation of the findings from weight loss and potentiodynamic polarization experiments.

Preparation of Mild Steel

Commercially available mild steel was bought and mechanically machined into dimension 3 cm × 3 cm × 0.05 cm with hole at the centre for easy hooking. Each were polished with evenly gritted emery paper; washed with distilled water and degreased with acetone by dipping them in acetone for five minutes and dried over CaCl₂ in desiccators overnight [19].

Synthesis of NAD

NAD was synthesized using the method reported in literature (Scheme 1) [20]. A suspension of P-Toluidine (2.8 g, 40 mmol) in hydrochloric acid (36 ml) and water (16 ml) was heated to around 70^oC until complete dissolution. The clear solution poured into ice was diazotized below 5^oC with sodium nitrite (2.8 g, 40 mmol) dissolved in water (10 ml). The resulting cold diazonium solution was then added slowly with continuous vigorous stirring over the course of 45 mins at 0^oC to a solution of 1-nitrosol-2-naphatol (6.92 g, 40 mmol) in water (75 ml) containing sodium hydroxide (1.6 g) and sodium carbonate (14.8 g). The product was collected by filtration and washed with water then later recrystallized from ethanol three times.

Scheme 1. Synthetic route of NAD

The synthesized brownish-yellow molecule has a chemical formula of C₁₇H₁₆N₃O₂, molecular weight of 294.334, melting point 110-112 ^oC and 98% yield. The spectra are shown in Figures 1, 2, 3 and 4.

FTIR (KBr, cm^-1): 3443 (O-H), 3066 (aromatic C-H), 1620 (aromatic C=C), 1406 (N=N_str), 1070 (C-O)

UV/Vis λ_max (nm): 262 (π-π*), 399 (Inter-molecular charge transfer, IMCT) and 415 (n-π*)

¹H-NMR (DMSO-d₆) δ: 8.89 (s, 1H, H_g), 7.75 (d, 2H, H_e), 7.62 (d, 2H, H_d), 7.55 (m, 3H, H_c), 6.42 (d, 2H, H_b), 2.50 (s, 3H, H_a)

¹³C-NMR (DMSO-d₆) δ: 145 (s), 130 (d), 129 (m), 127 (s)

Figure 1. Infrared spectrum of NAD

Figure 2. The UV spectrum of NAD

Figure 3. ¹HNMR spectrum of NAD

Figure 4. ¹³CNMR spectrum of NAD

Preparation of solution

0.5 M HCl was prepared using hydrochloric acid of standard grade and distilled water which serve as the corrodent. The inhibitor (NAD) was added to this test solution in a dosage of 10 – 50 ppm. Steel coupons for the gravimetric experiment were introduced into beakers containing this tested solution and the tests were performed in thermostated water bath at each test temperature (25, 35, 45, 55 and 65^oC) for 6 hrs.

Weight loss experiment

The pre-treated Mild steel coupons weighed with the aid of analytical balance (0.0001 sensitivity) were immersed in 100 ml 0.5 M HCl test solution loaded with different concentrations of the inhibitor (10 – 50 ppm) in an open beaker for 6 hours at varying temperature (298 – 338K at 10K interval) using thermostated water bath. Samples were withdrawn from the test solution after 6 hrs, brushed with brittle brush, washed with distilled water, rinsed in acetone and dried in oven for 15 mins at 40^oC before reweighing [19]. Each of this experiment was performed in triplicate for accurate results and the mean of the final weight was used in the calculation. From the weight loss results, the corrosion rate, C_R, degree of surface coverage, θ and the percentage inhibition efficiency, IE % were determined using Equations 1, 2 and 3 respectively.

where W_oand W₁ are the weight loss (g) of mild steel in the absence and presence of the inhibitor respectively. A is the area of the mild steel (cm²), t is the immersion time (hrs). C_Rⁱ and C_R^o are the corrosion rates (g cm^-2hr^-1) in the presence and absence of the inhibitor respectively.

The adsorption of an inhibitor on metal surface is in form of a substitution reaction, with the inhibitor substituting the water molecules adsorbed on the metal surface and in order to describe this reaction, adsorption isotherms are usually employed. The Langmuir adsorption isotherm (Equation 4) was employed in this study to explain the adsorption of NAD on the mild steel [22, 23].

where C is the concentration of inhibitor, K_ads the equilibrium adsorption constant and θ the extent of surface coverage.

To further explain the adsorption process, thermodynamic parameters were calculated. A relation (equation 5) was used to calculate the standard Gibb’s free energies of adsorption (∆G^o_ads) from the various values of adsorptive equilibrium constant at specific temperature (K_ads) [25].

where R is universal gas constant, ∆G_ads is the free energy of adsorption and 55.5 is the molar concentration of water in the solution known as the isocratic contribution. A plot of ∆G^o_ads against temperature using Equation 6 gave the enthalpy, ∆H^o and entropy ∆S^o of adsorption as intercept and slope respectively [26].

The adsorption behavior of NAD was further explained using the kinetic model. The apparent activation energies, E_a, for the corrosion process and the pre-exponential factors, A, were determined using the plot of lnC_R against 1/T (Figure 9) as given by the Arrhenius equation 7 [28]. Values obtained are given in Table 2.

Using the transition state Equation 8, values of enthalpy, ΔH* and entropy, ΔS* of activation were calculated using the slope and intercepts of the plots of ln(C_R/T) against 1/T (Figure 6.0) and these are given in Table 3.

where h is the Planks’ constant, N the Avogadro’s number, T the absolute temperature and R the universal gas constant.

Potentio-dynamic polarization experiments

Electrochemical experiments were conducted in a three-electrode cell using corrosion Lab and Versa stat 4 software under standard condition. A platinum sheet was used as the counter electrode (CE), saturated calomel electrode (SCE) as the reference electrode, while the mild steel machined into rectangular specimens with an exposed area of 1 cm² as the working electrode (WE). All potentials were measured against the SCE (0.2412 V with respect to the normal hydrogen electrode). Measurements were carried out in naturally aerated and unstirred solutions at 298 K using a thermostated water bath. The open current potential (OCP) was established by immersing the working electrode in the test solution for 10 mins while the potentiodynamic polarization studies were carried out by sweeping the applied potential from -250 mV to +250 mV at OCP with a scan rate of 1mVs^-1 while the current, I, is recorded.

Equation 9 helped to give the inhibition efficiency calculated from the values of corrosion current density extrapolated from the tafel curves [29].

where, and I_corr are the corrosion densities in the absence and presence of the inhibitor respectively.

Computational studies

Quantum chemical calculations were performed on the most stable conformer of NAD after a conformation search has been carried out using the molecular mechanic force field (MMFF) method. The geometry of the molecule was optimized using the DFT with B3LYP correlation and a high basis set, 6-31G* using computational chemistry software. The energies of the frontier molecular orbitals, FMOs (HOMO and LUMO) were obtained, it affords us to understand the sites that are prone to nucleophilic and electrophilic attack and also used to determine the energy band gap, E_g (E_LUMO - E_HOMO) [11,12,14]. Other properties like the global reactivity descriptors like the chemical hardness (η), softness (δ), electronegativity (χ) and global electrophilicity index (ω) were calculated from the FMOs. The dipole moment (μ) and the fraction of electron transferred (ΔN) were also calculated, all in gas phase.

The chemical hardness, a direct consequence of the energy band gap was calculated using Equation 10 Its value is 1.56 eV [11,12,14];

Other global reactivity descriptors calculated are the electronegativity in Equation 12 [11,12,14]. NAD has 4.53 eV as its electronegativity, a value lower than that of iron as expected.

where; I = -E_HOMOand A = -E_LUMO and the global electrophilicity index in Equation 13

A good inhibitor is characterized by donation of electrons from its HOMO orbitals to the metal’s d orbitals and also through the acceptance of electrons from the metal’s d orbitals to its orbitals.

Fraction of electron transferred was calculated using Equation 14 [11,12].

where χ_Fe and χ_Inhare the electronegativities of iron (representing bulk metal) and the inhibitor molecule respectively. η_Fe and η_Inh are the absolute hardness of iron and the inhibitor molecule respectively. χ_Fe has a theoretical value of 7 eV while that of η_Fe is 0 eV [11,14].

Results and discussion

Gravimetric analysis

The results obtained showed that at different concentrations of NAD (0.00005, 0.0001, 0.00015 and 0.0002) mol/L, the % inhibition efficiency increases as the concentration of the inhibitor increases at a fixed temperature but reduces as the temperature is increased i.e the corrosion rate reduces with an increase in concentration at a fixed temperature and increases with an increase in temperature (Figures 5 and 6). This is in line with what researchers observed in their work [4,6,16].

Figure 5. Variation of inhibition efficiency with concentration of NAD

Figure 6. Variation of inhibition efficiency of NAD with temperature

Adsorption considerations

The plot of C/θ against C at different temperatures (298 – 338 K) gave the parameters listed in Table 1 while Figure 7 showed these plots. Both linear correlation coefficients (R²) and slope values are closer to 1, suggesting that the adsorption obeys Langmuir adsorption isotherm. The little deviation from unity observed in the slope may be traced to the repulsion force in the adsorption layer [24].

Figure 7. Langmuir adsorption isotherm plots for NAD adsorption

The decrease in the adsorptive equilibrium constant (K_ads) values with temperature gave an indication that at relatively lower temperatures, strong adsorption of NAD molecules onto the mild steel surface occurred. On the other hand, already adsorbed molecules of NAD got desorbed from the mild steel surface as experimental temperature increases [23].

From the plot (Figure 8), -41.861 kJ mol^-1 and -0.0136 kJ mol^-1K^-1 were obtained for ∆H^o_adsand ∆S^o_ads, respectively (Table 1).

Figure 8. Determination of the Enthalpy, ∆H^o_ads and Entropy, ∆S^o_ads, of Adsorption of NAD on the Mild Steel Surface in 0.5 M HCl

Table 1. Values from Langmuir adsorption isotherm and thermodynamics study

Compd	Temp. (K)	R²	Slope	1/K (mol/l)	K (l/mol)	∆G (kJ/mol)	∆S (kJ/mol K)	∆H (kJ/mol)
NAD	298	0.996671	1.049629	0.000013	76923.08	-37.8249	-0.01357	-41.861
	308	0.998672	1.00578	0.000023	43478.26	-37.6332
	318	0.993204	1.329249	0.000037	27027.03	-37.5982
	328	0.998897	1.339742	0.000061	16393.44	-37.4171
	338	0.993498	1.099285	0.000097	10309.28	-37.2544

∆G^o_ads were obtained as negative owing to spontaneity of adsorption. In general, value of ∆G^o_ads around -20 kJmol^-1 indicates physical adsorption and value of ∆G^o_ads of -40 kJ/mol and above is an indication of chemisorption [27]. ∆G^o_ads obtained in this study were around -37 kJ/mol which gave a hint of complex adsorption mechanism. The negative value of ∆S^o_adsshowed the decrease in the degree of translational freedom of the molecules as it is being adsorbed on the mild steel surface. Negative value of ∆H^o_adsobtained indicated the exothermic nature of the adsorption process [26]. To differentiate physisorption from chemisorptions in an exothermic adsorption process, ∆H^o_adsaround -40 kJmol^-1 is an indication of physisorption while, ∆H^o_ads tending to -100 kJmol^-1indicates chemical adsorption of the inhibitor molecules. -41.801 kJ/mol obtained for ∆H^o_ads can be assigned to physical adsorption of NAD molecules on the mild steel surface.

Kinetic studies and activation parameters

The results of the kinetic studies and activation parameters are given in Figure 9 and Table 2.

Figure 9. Apparent activation energy determination for the corrosion process in 0.5 M HCl in the absence and presence of NAD

Values of apparent activation energies increase in the presence of NAD than that of pure acidic medium [28]. Higher energies are required for the corrosion reaction as the concentration of NAD increases in the inhibited solution. The higher values of E_a also indicate the physical adsorption that occurred in the first stage [29,28]. The pre-exponential factor, A, in the Arrhenius equation is related to the number of active centers [28]. The larger values of A in the presence of NAD compared to that of the uninhibited solution (Table 3) implied that most of the active sites are blocked by the adsorption of the inhibitor [28].

Table 2. Activation energy, E_a and pre-exponential factor A for the corrosion process in 0.5 M HCl

Compd	Concentration (ppm)	Slope	E_a (J/mol)	lnA	A
NAD	BLANK	-2255.8	18754.72	2.3831	10.83845
	0.0000344	-5404.8	44935.51	11.673	117359.8
	0.0000687	-5571.8	46323.95	11.968	157629.1
	0.0001031	-5769.2	47965.13	12.423	248450.8
	0.0001375	-6359.8	52875.38	14.09	1315859
	0.0001718	-6740.5	56040.52	15.137	3749001

Analysis of data in Table 3 revealed an increase in ΔH* and ΔS* values in the presence of NAD an indication of the increase in energy barrier of corrosion process in the presence of NAD [28] which agreed with the values of activation energy, E_a, presented in Table 4. Positive values of enthalpies of activation ΔH* in the absence and presence of NAD suggested an endothermic nature of the mild steel dissolution [30–33]. Negative values obtained for ΔS* in the absence and presence of NAD suggested the formation of the activated complex in the rate determining step to be associative rather than been dissociative and hence, there was decrease in disorderliness as the reaction moves from the reactants to the activated complex [33,34].

Figure 10. Transition state determination of enthalpy and entropy of activation in 0.5 M HCl in the absence and presence of NAD

Table 3. Values for the corrosion activation parameters of mild steel in 0.5 M HCl in the absence and presence of different concentration of NAD

Compd	Conc. (m)	Slope	Intercept	Enthalpy (J/mol)	Entropy (Jmol^-1k^-1)
NAD	BLANK	-1939	-4.3770	16120.85	-233.93
	0.0000344	-5088	0.9124	42301.63	-189.954
	0.0000687	-5255	5.2077	43690.07	-154.243
	0.0001031	-5452	5.6628	45327.93	-150.459
	0.0001375	-6043	7.3302	50241.50	-136.597
	0.0001718	-6423	8.3769	53400.82	-127.894

Potentiodynamic polarization

The polarization curves of the mild steel in 0.5 M HCl solution in the absence and presence of different concentrations of NAD are given by Figure 11. Other parameters such as the corrosion potential (E_corr), corrosion current density (I_corr), anodic Tafel slope (β_a), cathodic Tafel slope (β_c) and percentage inhibition efficiency (% IE) are summarized in Table 4.

Generally, organic inhibitors can be classified as cathodic, anodic or mixed-type inhibitor depending on whether there is decrease in the corrosion current densities at the cathodic or anodic or both sides, respectively, of the Tafel curve on addition of the inhibitor [36, 35]. It was observed from Figure 11 that both the cathodic and the anodic corrosion current densities decreased considerably most especially in the presence of 30 ppm NAD indicating that NAD is a mixed type inhibitor.

Figure 11. Potentiodynamic polarisation curve for mild steel in 0.5 M HCl solution in the absence and presence of NAD

Table 4. Polarization parameters and inhibition efficiencies for mild steel in 0.5 M HCl solution in the absence and presence of different concentrations of NAD at 298 K

Compd	Conc (g)	- β_c(mV)	β_a(mVdec-1)	C_R mpy	-E_corr(mV)	I_corr (mA)	% IE
NAD	Blank	111.71	292.71	461.40	451.4	1.009000	-
	0.015	248.49	55.83	76.15	703.2	0.166000	83.55
	0.030	148.03	148.03	0.0059	248.1	0.000012	99.99
	0.045	269.854	221.63	397.36	703.1	0.869803	13.80
	0.060	146.87	146.87	0.4835	594.3	0.001058	99.90
	0.075	270.91	270.91	2.253	618.4	0.004931	99.51

This suggested that NAD has retarding effect on both cathodic and anodic half reactions. Analysis of data in Table 3.2 equally revealed changes in the values of β_a and β_cin the presence of NAD indicating the influence of the inhibitor on the anodic and cathodic reactions [37]. The displacement of E_corr to the more negative values in the presence of NAD suggested the retarding effect of the inhibitor on both sides of the tafel curve. Hence, the corrosion reaction of the mild steel is inhibited. An increase in the inhibition efficiency of NAD in the inhibited solution as compared to the uninhibited solution was also observed suggesting the adsorption of NAD on most of the active sites causing considerable decrease in the corrosion current of the mild steel.

Quantum chemical calculations

The energy band gap is 3.12 eV; this is indicative that there is an inherent electron donating ability and that there is an interaction between the inhibitor and the metal surface with high HOMO energy of -6.09 eV, indicative that the inhibitor has excellent donating ability and a low LUMO energy of -2.97 eV, indicative that the inhibitor can accept electrons from metal’s d orbitals.

Softness is the inverse of hardness and it determines the ability of a molecule to react. Soft molecules are more reactive than hard ones because of the ease with which they could offer electrons to an acceptor [15, 16]. It is calculated according to Equation 11 [11,12,14] and of a value of 0.64 eV^-1. The hard and soft acids and bases principle (HSAB) explains that soft acids tend to react with soft bases and hard acids with hard bases. A bulk metal, whose chemical hardness is assumed to be zero very soft, a soft acid, therefore, they tend to react with soft bases (in this case, the inhibitor). This means that the inhibitor must have a high softness value, this enhances high adsorption and hence high corrosion inhibition efficiency [15,16].

As the inhibitor is brought in contact with the bulk metal, electrons flow from the lower χ_Inh to the higher χ_Fe. ΔN represents the inhibition effect resulting from electron donations and inhibition efficiency can be seen as effective if ΔN < 3.6 [15,17]. ΔN for NAD is 0.79, an indication that it has the ability to donate electrons. This has been earlier confirmed by the low hardness and high softness values.

Also, the dipole moment is an important parameter to ascertain if electrons are distributed in the molecular structure and if there is a strong dipole-dipole interaction between NAD and the metal surface. NAD has a dipole moment of 4.49 Debye, an indication that the inhibition absorption is enhanced through electronic force [18]. The quantum chemical parameters are shown in Table 5 while the HOMO and LUMO orbital diagram are displayed in Figures 11b and c.

Table 5. Quantum chemical parameters for NAD

Properties	E_HOMO(eV)	E_LUMO(eV)	E_g(eV)	η (eV)	δ(eV^-1)	χ(eV)	ω(eV)	μ(D)	ΔN
NAD	-6.09	-2.97	3.12	1.56	0.64	4.53	6.58	4.49	0.79

Figure 12. a. Optimized structure, b. Highest Occupied Molecular Orbital (HOMO) and c. the Lowest Unoccupied Molecular Orbital (LUMO) of NAD

Conclusions

The study synthesised and characterised (E)-3-(2-P-Tolyldiazenyl)-1-Nitrosonaphthalen-2-ol with its inhibitory performance evaluated using gravimetric and electrochemical methods. It also described NAD as a good inhibitor for mild steel in acidic environment with Inhibition efficiency increasing with increase in concentration and decreasing with increase in temperature. Electrochemical measurement using potentiodynamic polarization revealing a mixed-type organic inhibitor. Considerable inhibitory efficiencies were obtained in the presence of NAD indicating good agreement with that by weight loss. The adsorption of NAD on mild steel obeys Langmuir adsorption isotherm and is an exothermal and entropy decreasing process while the adsorption mechanism follows physical adsorption. The values of activation parameters (E_a, ∆H* and ∆S*) increased in the presence of NAD. Hence, conclusion could be made that the adsorbed NAD molecules blocked the active sites of lower energy and inhibited the mild steel dissolution. The quantum chemical study showed that NAD possess a strong electron donating and accepting properties which enhanced its strong adsorption on the metal surface.

Acknowledgement

We are grateful to Tertiary Education Trust Fund (TET Fund) Nigeria for supporting this work.

References

1. Abiola O. K., Otaigbe J. O. E., The effects of Phyllanthusamarus extract on corrosion and kinetics of corrosion processes of aluminium in alkaline solution, Corrosion Science, 2009, 51, p. 2790-2793.

2. Abiola O. K., Otaigbe J. O. E., Adsorption behavior of 1-phenyl-3-methylpyrazol-5-one on mild steel from HCl solution, Int. J. Electrochem. Sci., 2008, 3, p. 191-198.

3. Obot I. O., Obi-Egbedi N. O., Inhibitive properties, thermodynamic and quantum chemical studies of alloxazine on mild steel corrosion in H₂SO₄, Corrosion Science, 2011, 53, p. 263-275.

4. Arukalam I. O., Madufor I. C., Ogbobe O., Oguzie E., Experimental and Theoretical Studies of Hydroxyethyl Cellulose as Inhibitor for Acid Corrosion Inhibition of Mild Steel and Aluminium, The Open Corrosion Journal, 2014, 6, p. 1-10.

5. Solmaz R., Investigation of corrosion inhibition mechanism and stability of Vitamin B1 on mild steel in 0.5 M HCl solution, Corrosion Science, 2014, 81, p. 75-84.

6. Ameh P. O., Koha P. U., Eddy N. O., Experimental and Quantum Chemical Studies on the Corrosion Inhibition Potential of Phthalic Acid for Mild Steel in 0.1 M H₂SO₄, Chemical Science Journal, 2015, 6, 3, p. 1-8.

7. Oguzie E. E., Enenebeaku C. K., Akalezi C. O., Okoro S. C., Ayuk A. A., Adsorption and corrosion-inhibiting effects of Dacryodis edulis extract on low-carbon-steel corrosion in acidic media, J. Colloid interface Sci., 2010, 349, p. 283-292.

8. Naguib A. M., Mahross M. H., Khalil H. F. Y., Mahran B. N. A., Yehia M. M., El-Sabbah M. M. B., Azo Dye Compounds as Corrosion Inhibitors for Dissolution of Mild Steel in Hydrochloric Acid Solution, Portugaliae Electrochimica Acta, 2013, 31(2), p. 119-139.

9. Mabrouk E. M., Eid S., Attia M. M., Corrosion inhibition of carbon steel in acidic medium using azo chromotropic acid dye compound, Journal of Basic and Environmental Sciences, 2017, 4, p. 351-355.

10. Oyeneyin O. E., Structural and Solvent Dependence of the Electronic Properties and Corrosion Inhibitive Potentials of 1,3,4-thidiazole and Its Substituted Derivatives - A Theoretical Investigation, Physical Science International Journal, 2017, 16(2), p. 1-8.

11. Kara Y. S., Seda G.S., Esme A., Theoretical Study on the Relationship between the Molecular Structure and Corrosion Inhibition Efficiency of Long Alkyl Side Chain Acetamide and Isoxazolidine Derivatives, Protection of Metals and Physical Chemistry of Surfaces, 2012, 48(6), p. 710-721.

12. Fouda A. S., El-Azaly A. H., Awad R. S., Ahmed A. M., New Benzonitrile Azo Dyes as Corrosion Inhibitors for Carbon Steel in Hydrochloric Acid Solutions, International Journal of Electrochemical Science, 2014, 9, p. 1117-1131.

13. Elmsellem H., Aouniti A., Khoutoul M., Chetouani A., Hammouti B., Banchat N., Touzani R., Elazzouzi M., Theoretical approach to the corrosion inhibition efficiency of some pyrimidine derivatives using DFT method of mild steel in HCl solution, Journal of Chemical and Pharmaceutical Research, 2014, 6(4), p. 1216-1224.

14. Hasanov, R., Bilge, S., Bilgiç, S., Gece, G. and Kılıç, Z. Experimental and theoretical calculations on corrosion inhibition of steel in 1 M H₂SO₄ by crown type polyethers. Corrosion Science, 2010, 52(3), p. 984-990.

15. Li X., Xie X., Deng S., Du G., Inhibition effect of two mercaptopyrimidine derivatives on cold rolled steel in HCl solution, Corrosion Science, 2015, 92, p. 136-147.

16. Mwadham M. K., Lutendo C. M., Eno E. E. Theoretical Studies on Phenazine and Related Compounds as Corrosion Inhibitors for Mild Steel in Sulphuric Acid Medium, Int. J. Electrochem. Sci., 2012, 7, p. 7179-7205.

17. Lukovits I., Kalman E., Zucchi F., Corrosion Inhibitors: Correlation between the electronic structures and efficiency, Corrosion Science, 2001, 57, 1, p. 3-8.

18. Zhang F., Tang Y., Cao Z., Jing W., Wu Z., Chen Y., Performance and theoretical study on corrosion inhibition of 2-(4-pyridyl)-benzimidazole for mild steel in hydrochloric acid, Corrosion Science, 2012, 61, p. 1-9.

19. Geethamani P., Kasthuri P. K., Adsorption and corrosion inhibition of mild steel in acidic media by expired pharmaceutical drug, Cogent Chemistry, 2015, 1(1), 1091558.

20. Botros R., U.S. Patent No. 4,051,119. Washington, DC: U.S. Patent and Trademark Office, 1977.

21. Ahmadi R. A., Amani S., Synthesis, spectroscopy, thermal analysis, magnetic properties and biological activity studies of Cu (II) and Co (II) complexes with Schiff base dye ligands, Molecules, 2012, 17(6), p. 6434-6448.

22. Li X. H., Deng S. D., Fu H., Inhibition by Jasminum nudiflorumLindl leaves extract of the corrosion of cold rolled steel in hydrochloric acid solution, J. Appl. Electrochem. 2010, 40, p. 1641-1649.

23. Deng S., Li X., Inhibition by Jasmium nudiflorum Lindl. Leaves extract of the corrosion of aluminium in HCl solution, Corrosion Science, 2012, 64. p. 253-262.

24. Mu G. N., Li X. H., Qu Q., Zhou J., Molybdate and tungstate as corrosion inhibitors for cold rolling steel in hydrochloric acid solution, Corrosion Science, 2006. 48, p. 445-459.

25. Stoyanova A. E., Sokolova E. I., Raicheva S. N., The inhibition of mild steel corrosion in 1 M HCl in the presence of linear and cyclic thiocarbamides-Effect of concentration and temperature of the corrosion medium on their protective action, Corrosion Science, 1997, 39, p. 1595-1604.

26. Fiori-Bimbi M. V., Alvarez P. E., Vaca, H., Gervasi, C. A., Corrosion inhibition of mild steel in HCL solution by pectin, Corrosion Science, 2015, 92, p. 192-199.

27. El-Lateef, H. M. A., Experimental and computational investigation on the corrosion inhibition characteristics of mild steel by some novel synthesized imines in hydrochloric acid solutions, Corrosion Science, 2015, 92, p. 104-117.

28. Tu S., Jiang X., Zhou L., Wang H., Jiang X., Synthesis of N-alkyl-4-(4-hydroxybut-2-ynyl) pyridinium bromides and their corrosion inhibition activities on X70 steel in 5M HCl, Corrosion Science, 2012, 65, p. 13-25.

29. Chen W., Luo H. Q., Li N. B., Inhibition effects of 2, 5-dimercapto-1, 3, 4-thiadiazole on the corrosion of mild steel in sulphuric acid solution, Corrosion Science, 2011, 53(10), p. 3356-3365.

30. Obot I. B., Obi-Egbedi N. O., Fluconazole as an inhibitor for aluminium corrosion in 0.1 M HCl, Colloids and Surfaces a: Physicochemical and Engineering Aspects, 2008, 330(2), p. 207-212.

31. Szauer T., Brandt A., Adsorption of oleates of various amines on iron in acidic solution, Electrochimica Acta, 1981, 26(9), p. 1253-1256.

32. Dahmani M., Et-Touhami A., Al-Deyab S. S., Hammouti B., Bouyanzer A., Corrosion inhibition of C38 steel in 1M HCl: A comparative Study of Black Pepper Extract and its isolated piperine, International Journal of Electrochemical Science, 2010, 5, p. 1060-1069.

33. Peme T., Olasunkanmi L. O., Bahadur I., Adekunle A. S., Kabanda M. M., Ebenso E. E., Adsorption and corrosion inhibition studies of some selected dyes as corrosion inhibitors for mild steel in acidic medium: gravimetric, electrochemical, quantum chemical studies and synergistic effect with iodide ions, Molecules, 2015, 20(9), p. 16004-16029.

34. Saliyan R., Adhikari A. V., Inhibition of corrosion of mild steel in acid media by N'-benzylidene-3-(quinolin-4-ylthio) propanohydrazide, Bulletin of Materials Science, 2008, 31(4), p. 699-711.

35. Chen Z. Y., Li L. J., Zhang G. A., Qiuand Y. B., Guo X. P., Inhibition effect of propargylalcohol on the stress corrosion cracking of super 13Cr steel in a completion fluid, Corros. Sci., 2013, 69, p. 205-210.

36. Hu J. Y., Zeng D. Z., Zhang Z., Shi T. H., G.L. Song G. L., Guo X. P., 2-Hydroxy-4-methoxy-acetophenone as an environment-friendly corrosion inhibitor for AZ91D magnesium alloy, Corros. Sci., 2013, 74, p. 35-43.

37. Al-Amiery A. A., Kadhum A. A. H., Kadihum A., Mohamad A. B., How C. K., Junaedi S., Inhibition of Mild Steel Corrosion in Sulfuric Acid Solution by New Schiff Base, Materials, 2014, 7, p. 787-804.