Open access peer-reviewed chapter

Electrochemical, Thermodynamic, Surface, and Spectroscopic Study in Inhibition of Iron Corrosion with Turmeric Root Extract (TRE)

By Khuloud Almzarzie, Ayman Almassri, Ahmad Falah and Hassan Kellawi

Submitted: November 12th 2019Reviewed: April 24th 2020Published: December 16th 2020

DOI: 10.5772/intechopen.92648

Downloaded: 86

Abstract

Turmeric root extract was tested as corrosion inhibitor for iron in 0.5 M HCl, using potentiodynamic polarization and electrochemical impedance spectroscopy, scanning electron microscope, and energy dispersive X-ray analysis. The inhibition efficiency increases as the time of immersion rises but decreases with temperature rise. The Nyquist plots showed that the charge transfer resistance increases and the double-layer capacitance decreases as the time of immersion increases. Tafel results show that both corrosion current and corrosion speed are reduced with time of immersion. All impedance spectra of EIS tests exhibit one capacitive loop, which indicates that the corrosion reaction is controlled by charge transfer process. Inhibition efficiency increases with the concentration of the inhibitor reaching its maximum value, 88.90%, at 8 g/100 mL. Thermodynamic parameters, Ea, ∆H*, and ∆S*, were estimated, and the mechanism of corrosion and inhibition was discussed. The adsorption of turmeric root extract followed Langmuir adsorption isotherm.

Keywords

  • iron corrosion
  • electrochemical impedance spectroscopy (EIS)
  • turmeric toot extract (TRE)
  • double-layer capacitance (Cdl)
  • scanning electron microscopy (SEM)
  • inhibition efficiency IE (%)

1. Introduction

Inhibition of corrosion of iron is important for theoretical and practical aspects [1]. Iron and its alloys are of great importance in the industry, prompting vast research on corrosion resistance and its conducts [2]. Acids are wildly used in industries [3], such as industrial acid cleaning, acid descaling, and acid picking, and used to remove mill scale from metallic surfaces. Natural compounds containing sulfur, oxygen, and nitrogen atoms are effective as corrosion inhibitors in acid media; inhibitors are used to reduce the rate of dissolution of metals [4]. Natural plant inhibitors that contain organic compounds are widely used to inhibit minerals in an acidic medium [5] and are called environmentally friendly nontoxic inhibitors [6]. The adsorption of these compounds is influenced by the electronic structure of their content of active compounds, electrons density, aromatic rings, and functional groups possessing free electrons such as, R–OH –CHO, –N=N, etc. [7]. The adsorption of organic inhibitors at the metal/solution interface takes place through the replacement of water molecules by organic inhibitor molecules [8]. The efficiency of these compounds depends mainly on their abilities to be adsorbed on the metal surface with their polar groups moving as the reactive centers. The purpose of this research is to use a nontoxic environment friendly inhibitor formed from turmeric root extract to reduce iron corrosion and study its effect using electrochemical impedance and Tafel polarization methods. Turmeric root extract contains active substances represented by turmeric derivatives with a high percentage (90%), which are phenolic compounds of antioxidant. The most important are curcumin, demethoxycurcumin, and bisdemethoxycurcumin, which have the following chemical formulas (Figures 1 and 2) [9]:

Figure 1.

Chemical formulas for turmeric derivative compounds [9].

Figure 2.

Sinusoidal signal applied and the sinusoidal current signal produced by a specific phase difference.

Recent reference studies indicate the use of turmeric root extract in 2012 to inhibit copper metal. The inhibit corrosion was 98% with EIS technology and Tafel polarization [10]. In 2014, the effect of turmeric on steel was studied with Tafel polarization in a petroleum medium. The inhibit corrosion was 92% [11]. In 2017, the effect of turmeric on solid carbon in a saline medium (3.5% NaCl) was studied with Tafel technology; the inhibit corrosion was 91% [12].

This phenomenon has not been adequately studied in Syria; therefore, this research is an important step in studying the phenomenon of corrosion and understanding the mechanism of its occurrence and the conditions affecting it with the latest technologies Electrochemical impedance spectrometry and Mott-Schottky plot are used as a basis for future research in order to implement solutions on the ground.

1.1 Definition of electrochemical impedance spectrometry (EIS)

Electrochemical impedance spectrometry is also called alternating current (AC) and impedance spectroscopy (EI). It is a useful tool and the newest method in many studies, especially the study of corrosion of minerals. Impedance is defined as the measurement of the impedance of alternating current passage in each part of the electrical circuit, and it has units of ohm. Electromagnetic impedance spectroscopy measures the sinusoidal changes of the current and potential signals as a function of the frequency at the value of a current, a field of current, a value of a potential, or a field of potential. Frequency changes give rise to a different phase difference between the current and potential signals for each circuit element [1].

Impedance is measured by applying a sinusoidal signal or current and then measuring the resulting response to the corresponding variable in a given frequency range. The following equations show the signal of latency and current response at a specific frequency [3], which are found via Eq. (1):

Et=E0sinωtE1

where Et is the latency at time t, E0 is the applied signal amplitude, ω is the angular frequency (radians/second) equal to 2лf, and f (frequency) is the number of integrated vibrations per second (Hz/s).

The resulting current response is measured at the same frequency value with a phase difference between the current and potential signals and a difference in signal amplitude, which are found via Eq. (2):

It=I0sinωt+φE2

where φ is the phase difference in radians and I0 is the signal response amplitude.

The relationship of impedance is given according to Ohm’s law:

Z=Et/It=E0sinωt/I0sinωt+φE3
=Z0sinωt/sinωt+φE4

where Z0 = E0/I0.

The value of the phase difference at the value of a specific frequency is given by

tanφ=Zimg/ZrealE5

where Zimg is the imaginary impedance and Zreal is the true impedance.

1.2 Features and applications

The electromagnetic impedance spectroscopy is distinguished as its results are accurate, as each point of the EIS curve contains information about the electrical process taking place, compared to conventional electrical methods that depend on measuring current changes, electrical charges, or the potential of the electrodes as a function of time, which depends on a certain value of its spectrum, such as a cyclic voltage, which includes current changes in hundreds of points for the potential to obtain a specific value for the peak oxidation and return at the corresponding current and potential value [3].

Among the applications of electromagnetic impedance spectroscopy, in addition to studying corrosion processes, electroplating processes, and semiconductors, it studies surface processes that include oxidation and reduction processes on the electrode surface, adsorption processes, electrical adsorption, and diffusion, as well as the kinetics of reactions in solutions, mass transfer, and resistance to solution, cells, and their electrical properties and batteries, determining the effect of each circuit element on impedance [1, 6]. It is also distinguished by not destroying the studied sample after testing [13].

2. Materials and methods

2.1 Preparation of plant extract

Turmeric root extract was prepared by washing and drying the turmeric root and grinding it then dissolving 1 g of powder in 100 mL methanol 50% and removing the solvent by placing the solution in a vacuum evaporator, at 60°C. Distilled water is used in the preparation process [14].

2.2 Preparation of metal specimen

The iron specimens have a composition (wt%) of 0.200% C, 0.500% Si, 1.600% Mn, 0.035% S, 0.035% P, 0.040% Nb, 0.012% N, 0.020% Al, and remaining Fe. This sample was analyzed in the Atomic Energy Commission and abraded with a series of emery papers 400, 1200, 1500, and 1800 grades. The samples were then washed thoroughly with distilled water and dried in air.

2.3 Test solution

A solution of 0.5 M concentrated acid was prepared using distilled water and 37% hydrochloric acid.

2.4 Electrochemical measurements

Electrochemical measurements were carried out using a potentiostat IVIUM-STAT.XR (Holland). A three-electrode cell system containing working electrode (iron coupon) of a 1 cm2 exposed area, saturated (Ag/AgCl) electrode as a reference electrode, and then a platinum wire as auxiliary electrode was used. The electrochemical impedance spectroscopy measurements were carried out using the mentioned electrochemical system. Polarization curves were recorded at a sweep rate of 50 mV s−1. Electrochemical impedance spectroscopy measurements were carried out at open-circuit potential over a frequency range of 1 MHz to 1 Hz. The sinusoidal perturbation has an amplitude of 0.01 mV.

2.5 Scanning electron microscopy (SEM) and energy dispersive X-rays (EDX)

The inhibitor film formation of the extracts surface was studied using SEM and EDX techniques.

3. Results and discussion

3.1 Mechanism of inhibition process

Turmeric root extract (TRE) used here as a corrosion inhibitor can serve as a scale inhibitor as well. This plant is characterized by the existence of a percentage of phenolic compounds (categories of curcumin) of a percentage up to 90%. It is a natural, nontoxic, environmentally friendly material. Active compounds in turmeric root extract are attributed to curcumin, demethoxycurcumin, and bisdemethoxycurcumin and to the multiple lone pair of electrons, multiple bonds, and/or conjugated л-type bond system [15]. Adsorption of these active molecules forms thin inhibitor films on the metal surface, which isolate the metal surface from the corrosive environment [16]. The oxygen atoms, the aromatic rings, and the bilateral bond of the aromatic rings boost the electronic pair freedom on the surface of the electrode. These compounds adsorb their free electrons on the surface of the electrode, and the iron is oxidized to form positively charged iron, thus forming a double electrical layer, and difference in voltage arises, as schematically presented in Figure 3. The inhibitor enhances the free electrons, which reduces iron corrosion and enhances inhibition.

Figure 3.

Schematic presentation of the electric double-layer formation [Chem draw].

3.2 Electrochemical impedance spectroscopy measurements

In the corrosion behavior of iron in 0.5 M HCl solution, in the absence and presence of TRE, it is investigated by the EIS, at 298 K after 1 hour of immersion in the acid solution. The double-layer capacitance (Cdl) and the frequency at which the imaginary component of the impedance is maximum (−Zmax) are found via Eq. (6):

Cdl=1/wmaxRctwherewmax=2πfmaxE6

The inhibition efficiency %IERct that resulted from the charge transfer resistance (Rct) is calculated by

%IERct=RctR0ct/Rct100E7

where R0ct and Rct are the charge transfer resistance (Rct) in the absence and presence of different concentrations of inhibitor, respectively [17].

Nyquist’s and Bode’s graphs of the results of the EIS of iron in 0.5 M HCl, in the absence and presence of different concentrations of TRE, were presented in Figures 4 and 5, respectively. The big capacitive loop refers to the adsorption of the inhibitor molecules (active compounds) presented in Figure 2 on the iron samples [18]. Rs represents the resistance of the corrosive solution, and Rct represents the effective resistance of the transport groups of the damper and the adsorption of their electrons onto the metal surface. Cdl is the amplitude of the formed double layer between the surface of the metal and solution.

Figure 4.

Nyquist plots of iron in 0.5 M HCl containing varying concentrations of TRE after 1 hour of immersion in acid solution.

Figure 5.

Bode plots of iron in 0.5 M HCl containing varying concentrations of TRE after 1 hour of immersion in acid solution.

Table 1 indicates that the Rct values of the inhibited substrates increased with the concentration of inhibitors and Cdl values decreased because of the increased prevalence of active compounds from the inhibitor and the adsorption of their electrons on the iron surface, which confirms that TRE extract is an effective inhibitor of corrosion of iron in the medium of water chlorine acid [19]. The values of n between 0.7 and 0.98 indicate that the constant phase element Q operates as a capacitance in the equivalent electrical circuit, which indicates a complex. The adsorbent inhibitor is a capacitive capacitor in the electrical circuit equivalent to its positive bus, the surface of the solution, and the negative capacitor, the electrode surface [20]. Resistance values of the solution are small Rs due to the corrosion concentration and temperature of the corrosive medium at different immersion times. Equivalent circuit model used to fit impedance spectra data is presented in Figure 6.

InhibitorConcentration (g/100 mL)Rct (ohm)fmax (Hz)Cdl (F/cm2)ɑIERct%
Blank0.020.31604.90*10−50.73
Turmeric root extract2.027.71603.59*10−50.9826.71
4.050.81003.13*10−50.7060.04
6.073.11601.36*10−50.7072.23
8.01171608.51*10−60.7082.65

Table 1.

Impedance parameters of corrosion of iron in 0.5 M HCl at 298 K in the absence and presence of different concentrations of TRE.

Figure 6.

Equivalent circuit model used to fit impedance spectra data.

3.3 Potentiodynamic polarization measurements

3.3.1 Influence of concentration

Polarization measurements were done in order to know about the kinetics of the cathodic and anodic reactions. The anodic and cathodic current potential curves are extrapolated up to their intersection at a point where corrosion current density (Icorr) and corrosion potential (Ecorr) are acquired [21]. Table 2 shows the electrochemical parameters (Icorr, Ecorr, βa, βc, and CR) obtained from Tafel plots for the iron electrode in 0.5 M HCl solution without and with various concentrations of TRE. The Icorr values were used to calculate the inhibition efficiency, IE (%), in Table 2, using Eq. (8):

InhibitorConcentration (g/100 mL)Ecorr- (mV/SCE)Icorr (A*10−4/cm2)βa (mV/dec)βc (mV/dec)CR (mm/year)IE%
Blank0.00.67726.130.3520.1838.56
Turmeric root extract2.00.396810.80.1550.3233.5458.67
4.00.4744.70.1460.2331.5582.01
6.00.4533.80.1390.1791.2585.46
8.00.4173.40.1310.2251.1186.99

Table 2.

Electrochemical parameters of iron in 0.5 M HCl solution at different concentrations without and with TRE.

IE=IIcorr/I100E8

where Icorr and I are the corrosion current densities with the presence and absence of inhibitor, respectively. The CR values in Table 2 used the following equation [22]:

CR=3.27103icorrEw/dE9

where icorr is the corrosion current density in micro A/cm2, Ew is the equivalent weight of the corroding metal in grams, and d is the density of the corroding metal in g/cm3.

Under the experimental conditions performed, the cathodic section of the plot represents the hydrogen evolution reaction, while the anodic section represents the iron dissolution reaction. They are determined by the extrapolation of Tafel lines to the respective corrosion potentials.

The results in Table 3 indicates that the inhibitor reduces the corrosion current value and inhibition; IE (%) increases with the concentration of the inhibitor reaching 88. 90%, at 8 g/100 mL. This result suggests that good inhibition act for TRE [23].

T(K)C (g/100 mL)Ecorr- (mv/SCE)Icorr (μA/cm2)βa (mV/dec)βc (mV/dec)CR mm/yearIE%
283Blank0.67726.130.3520.1838.56
20.396810.80.1550.3233.5458.67
40.4685.90.1480.1771.93377.42
60.4533.80.1390.1791.2585.46
80.4422.90.1430.1880.97988.90
293Blank0.66131.10.3160.17410.19
20.3798.350.1420.3282.7373.15
40.4586.60.1380.2052.16778.78
60.4584.80.1640.2061.58184.57
80.44140.1310.1931.31887.14
303Blank0.67733.80.3310.16811.07
20.45213.50.1670.2494.460.06
40.42690.1320.2632.9773.37
60.47470.1520.1932.2979.29
80.4985.70.140.161.8783.14
313Blank0.71436.20.3780.11911.84
20.47714.60.1880.2374.78859.67
40.419110.1350.283.63169.61
60.3797.90.1330.3392.678.18
80.4685.90.1480.1771.93383.70

Table 3.

Polarization parameters of iron in 0.5 M HCl at different temperatures with various concentrations of TRE.

3.3.2 Influence of temperature

Polarization curves for the iron in 0.5 M HCl solution are shown in Figures 7 and 8 in two different conditions, with constant concentrations of TRE and in the presence of different concentrations of TRE in the temperature range 283–313 K. The surface overage (Θ) was calculated using

Figure 7.

Polarization curves of iron in 0.5 M HCl at different temperatures.

Figure 8.

Polarization curves of iron in 0.5 M HCl at different temperatures in the presence of 8 g/100 mL of TRE.

Θ=IE%/100E10

The inhibition efficiency IE (%) is given by Eq. (8).

The results of the Table 2 refer that temperature increase leads to Icorr increase, while the addition of TRE resulted in the decrease of the Icorr values across the temperature range. The results also indicate that the inhibition efficiencies increased with the concentration of inhibitor but decreased proportionally with temperature. Such behavior can be rationalized that the inhibitor acts by adsorption onto the metal surface [24].

Ea, ∆S*, and ∆H*, for both corrosion inhibition and corrosion of iron in 0.5 M HCl in the presence and absence of TRE at different concentrations between 283 and 313 K, were calculated from an Arrhenius-type plot (Eqs. (11) and (12)) [25]:

LogIcorr=Ea/2.303RTE11

where Icorr is the corrosion current density (taken from averaged polarization), Ea is the activation of ion energy, and R is the universal gas constant.

I=RTNhexpΔSRexpΔHRTE12

where h is Plank’s constant, N is Avogadro’s number, ∆H*a is the enthalpy of activation, and ∆S*a is the entropy of activation.

The plots of Log (Icorr) vs. 1/T and Log (Icorr/T) vs. 1/T gave straight lines with the slope of -Ea/R and -∆H* /R, respectively. The intercepts were A and [Ln (R/Nh) + (∆S*/R)] for the Arrhenius and transition state equations, respectively (Figures 9 and 10). The calculated values of the activation energy Ea, the entropy of activation ∆S*, and the enthalpy of activation ∆H* are presented in Table 4.

Figure 9.

Arrhenius plots of log (Icorr) versus 1/T at various concentrations of TRE.

Figure 10.

Variation of log (Icorr/T) versus 1/T at various concentrations of TRE.

InhibitorC (g/100 mL)Ea (kJ/mol)∆H* (kJ/mol)∆S* (J/mol)
0.5 M HCl7.695.22−275.37
Turmeric root extract (TRE)2.010.027.55−275.83
4.015.9913.52258.93
6.018.9916.52−251.65
8.018.4315.96−255.51

Table 4.

Values of activation parameters ∆S* and ∆H* for iron 0.5MHCl in the presence and absence of various inhibition concentrations.

The activation energy values with TRE film are greater than the absence as shown in Table 4. This result is consistent with previous results, since adsorption of active compounds on the metal surface impeded the corrosion reaction as if an additional energy barrier had arisen to dampen the corrosion reaction. The positive signal for a change in the enthalpy of the corrosion reaction indicates that the pyrolysis process is endothermic. The decreasing entropy of the reaction at the formation of the complex indicates that the adsorbent inhibitor complex has a coherent structure [26, 27, 28].

The study of adsorption behavior of active compounds on the iron surface shows the following data:

3.3.3 Adsorption isotherm

Study the effect of turmeric root extract concentration on the inhibition efficacy by acting C\θ in terms of C. Gibbs standard free energy (ΔGads) is calculated as a single molecule of water, which replaces a molecule. One of the inhibitor molecules has a ratio of 1/55.5, from relationships (13) and (14), according to the isotope of the immersion in adsorption. Langmuir adsorption isotherm is represented by Eq. (13) [29]:

LogK=log1\55.5ΔG0ads\RTE13

Rearrangement gives Eq. (14):

C\θ=1/Kads+CE14

where θ is the degree of surface cover with the inhibitor, K ads is the adsorption equilibrium constant, and C is the concentration of inhibitor used in the corrosive medium (Figure 11).

Figure 11.

Plots of Langmuir adsorption isotherm of TRE on iron surface at different temperatures.

The value of ∆Ga is less than −20 kJ mol−1 which is an indication that physical adsorption is dominant [30] (Table 5).

T (K)1/K∆Gads (kJ mol−1)∆Sa (J mol−1)R2∆Ha (kJ mol−1)
2830.16−13.816948.750.9986−20
2930.04−17.795460.670.9910
3030.13−15.292650.400.9999
3130.15−15.430649.240.9961

Table 5.

Calculated parameters of Langmuir adsorption isotherm.

3.4 SEM–EDX analysis

Surface morphology of iron was studied by scanning electron microscopy after 1 h immersion in HCl with and without addition of the inhibitor. Figure 12a represents the micrograph obtained by polished steel before exposing to the corrosive medium, while Figure 12b showed strongly damaged steel surface due to the corrosion effect after immersion in HCl solution. SEM images of steel surface after 1 hour immersion in HCl with 1 g/100 mL TRE are shown in Figure 12c. It can be seen from Figure 12a that the iron sample before immersion seems smooth and shows some abrading scratches on the surface. Inspection of Figure 12b reveals that the iron surface after immersion in uninhibited HCl shows an aggressive attack of the corroding medium on the iron surface. In contrast, in the presence of 1 g/100 mL TRE (Figure 12c), the iron surface was corroded only negligibly. In addition, there was an adsorbed film on the iron surface that was not observed in Figure 12b. These results confirmed enhancement of surface coverage of steel surface that led to the decrease in contact between the iron and the aggressive medium. Thus, a good adsorptive protection layer that was formed by the inhibitor can efficiently inhibit corrosion of steel.

Figure 12.

SEM of polished iron (a) before immersion (b) after 1 hour of immersion in HCl 1 g/100 mL of TRE and (c) treated iron in the presence of 1 g/100 mL extract.

The following table shows the percentages of the studied elements in the presence and absence of TRE.

Increasing the percentage of carbon on the surface of the iron treated with the inhibitor compared to the surface of the polished iron is presented in Table 6 and Figure 13, due to the spread of the effective groups in the inhibitor and the adsorption of its electrons on the surface of the iron. Oxygen content is reduced at the surface of the iron treated with an inhibitor, compared to the surface of iron exposed to the corrosive medium, due to its interaction with iron to form a complex inhibitor film. Chlorine content is reduced in the presence of the extract compared to the iron surface exposed to corrosive medium due to the reaction of chlorine with iron forming chloride dissolved iron.

ElementCOCl
Without inhibitor0.20
After adding HCl0.2029.861.76
With inhibitor26.847.140.1

Table 6.

The percentages of the studied elements in the presence of TRE.

Figure 13.

EDX of (a) polished iron, (b) after 1 hour of immersion in HCl, and (c) treated iron in the presence of 1 g/100 mL extract.

4. Conclusion

The inhibition efficiency (%IE) of TRE increases with the increase of extract concentration. EIS results showed that the double-layer capacitance (Cdl) decreases and charge transfer resistance (Rct) increases with the time of immersion in the extract. The inhibitor showed maximum inhibition efficiency (%IE), 88.9% at 8 g/100 mL concentration. The inhibition efficiency (%IE) of TRE decreased with temperature, which leads to a decrease in activation energy (Ea) of the corrosion process.

The activation energy value of Ea = −20 kJ mol−1 indicates that the adsorption process is spontaneous and the is physical adsorption. Langmuir adsorption isotherm and SEM studies showed that TRE inhibitions occur through adsorption mechanism. The results of SEM and EDX have been shown to form a protective film on the iron surface.

Acknowledgment

I thank everyone who helped in the face of this work, from laboratory professors to the Atomic Energy Commission.

© 2020 The Author(s). Licensee IntechOpen. This chapter is distributed under the terms of the Creative Commons Attribution 3.0 License, which permits unrestricted use, distribution, and reproduction in any medium, provided the original work is properly cited.

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Khuloud Almzarzie, Ayman Almassri, Ahmad Falah and Hassan Kellawi (December 16th 2020). Electrochemical, Thermodynamic, Surface, and Spectroscopic Study in Inhibition of Iron Corrosion with Turmeric Root Extract (TRE), Electrochemical Impedance Spectroscopy, Marwa El-Azazy, Mart Min and Paul Annus, IntechOpen, DOI: 10.5772/intechopen.92648. Available from:

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