# The Effect ofAchyranthes aspera Extracts on Mild Steel Corrosion in Industrial Water Medium

Authors: Chikkur B. Pradeep Kumar; Kikkeri N. Mohana
Journal: ISRN Corrosion
 (2013)

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## Abstract

Achyranthes aspera (AA) extracts were studied as corrosion inhibitor for mild steel (MS) in industrial water medium using mass loss and electrochemical techniques. The results of the study revealed that AA extracts inhibit MS corrosion through adsorption process following Langmuir adsorption isotherm model. The protection efficiency increased with increase in inhibitor concentration and decreased with temperature. The electrochemical impedance spectroscopy (EIS) measurements showed that the charge transfer resistance increases with increase in the concentration of AA extracts. The polarization curves obtained indicate that AA extracts act as mixed type of inhibitor. Scanning electron microscopy (SEM) was used to analyze the surface adsorbed film.


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## Body

## 1. Introduction

The use of inhibitors is one of the most practical methods for protection against corrosion and prevention of unexpected metal dissolution. Different organic and inorganic compounds have been studied as inhibitors to protect metals from corrosive attack. The efficiency of these organic corrosion inhibitors is related to the presence of polar functional groups with S, O, and N atoms in the molecule [1–5]. Such compounds can adsorb onto the metal surface and block the active surface sites, thus reducing the corrosion rate. Nevertheless, most of these compounds are not only expensive but also toxic for living beings. So, plant extracts have attracted the attention of researchers as ecofriendly corrosion inhibitors for many decades [6–9]. Plant extracts are an incredibly rich source of natural chemical compounds that can be extracted by simple procedures with low cost and are biodegradable in nature. The actual inhibitors in the plant extracts are usually alkaloids and other organic nitrogen bases, as well as carbohydrates, proteins, and their acid hydrolysis products [10]. Alkaloids have an ability to coordinate the transition metals or their alloys via the d-orbitals of metal and empty p-orbitals of the heteroatoms in the inhibitor molecules. A number of natural compounds have been used as corrosion inhibitors for metals and their alloys in acidic, alkaline, and neutral solutions [11–15].Achyranthes aspera (AA) is one of the most important antioxidant medicinal plants, and it is an excellent source of several flavonoids, tannins, reducing sugars, alkaloids, and saponins [16]. Besides these phytoconstituents, several glycosides [17], fatty acids [18], ecdysterone [19], and triterpenoids [20] were isolated in various parts of plant. In the light of phytoconstituents reported, the present study was intended to ascertain the ability of methanolic extracts of AA to protect the mild steel in industrial water medium. Effects of inhibitor concentration, temperature, and immersion time on the corrosion rate were investigated and discussed. Gravimetric, potentiodynamic polarization, and electrochemical impedance spectroscopy (EIS) techniques were employed to study the mechanism of corrosion inhibition. Adsorption behaviour and thermodynamic parameters were obtained to establish the mechanism of adsorption. The morphology of the inhibited mild steel was analyzed using scanning electron microscopic images.


## 2. Experimental

### 2.1. Preparation of Plant Extracts

Healthy, disease free, mature leaves ofAchyranthes aspera(AA) collected from Western Ghats, Karnataka, India, were used for the preparation of methanolic extracts. Thoroughly washed mature leaves were shade dried and then powdered with the help of a blender. The powder was extracted with methanol using a Soxhelt extractor. The extracts were concentrated using rotary flash evaporator and preserved at ±5°C in airtight bottle until further use.


### 2.2. Materials

The specimens used for corrosion tests were mild steel (MS) coupons which have the following composition (wt %): 0.051 C : 0.023 Si : 0.005 P : 0.103 Al : 0.179 Mn : 0.023 S and the remainder iron. The test solution was industrial water collected from heat exchangers and reboilers of the chemical industries in and around Mysore city, India. The chemical composition of the industrial water (ppm) obtained from ionic chromatograph was 7500 Cl−; 64 Ca2+; 3440SO42-; 23 Mg2+; 140 Na+; 0.28PO43-. Prior to gravimetric and electrochemical measurements, the surface of the specimens was polished under running tap water using emery paper (SiC, grade 220–600), rinsed with distilled water, dried on a clean tissue paper, immersed in benzene for 5 s, dried and immersed in acetone for 5 s, and dried with clean tissue paper. Finally, the specimens were kept in desiccators until use. At the end of the gravimetric experiment, the specimens were carefully washed with acetone and benzene, dried, and then weighed. For polarization and electrochemical impedance studies, the MS specimen was embedded in epoxy resin to expose a geometrical surface area of 1 cm2 to the electrolyte.


### 2.3. Methods

#### 2.3.1. Gravimetric Measurements

Gravimetric experiments were carried out in a glass cell, and the solution volume was 100 cm3. The temperature of the environment was maintained by thermostatically controlled water bath (Weiber, India) with an accuracy of ±0.2°C under aerated condition. The mild steel specimens used were rectangular with a dimension of 1 cm × 1 cm × 0.1 cm. The initial weight of the specimen was recorded using an analytical balance (precision ±0.1 mg). After the corrosion test in industrial water with and without inhibitor, the specimens were carefully washed in double distilled water, dried, and then weighed. The weight loss of the specimen was determined after an immersion period of 10 to 50 h at the temperature range of 30 to 60°C. Triplicate experiments were performed in each case, and the average mass loss was reported. The corrosion rate (CR) and inhibition efficiency (% IE) are calculated using
(1)CR=ΔWSt,IE%=(CR)a-(CR)p(CR)a×100,
where ΔW is the weight loss, S is the surface area of the specimen (cm2), t is the immersion time (h), and (CR)a, (CR)p are corrosion rates in the absence and presence of the inhibitor, respectively.


#### 2.3.2. Electrochemical Measurements

Electrochemical tests were carried out with a CH-analyzer model CH1660D. The cell arrangement used was a conventional three-electrode cell with platinum counter electrode, saturated calomel electrode as reference electrode, and test material (mild steel) as working electrode. Anodic and cathodic polarization curves were recorded in the potential range from −350 to −800 mV with a scan rate of 0.4 mV s−1. The AC impedance measurements were performed in the frequency range from 10 kHz to 0.05 Hz with signal amplitude of ±10 mV.


#### 2.3.3. Morphological Investigation

The surface morphology of the mild steel samples in the absence and presence of AA extracts (1200 ppm in industrial water) at 30°C was investigated by scanning electron microscopy (SEM) technique (Model JSM-5800).


## 2.1. Preparation of Plant Extracts

Healthy, disease free, mature leaves ofAchyranthes aspera(AA) collected from Western Ghats, Karnataka, India, were used for the preparation of methanolic extracts. Thoroughly washed mature leaves were shade dried and then powdered with the help of a blender. The powder was extracted with methanol using a Soxhelt extractor. The extracts were concentrated using rotary flash evaporator and preserved at ±5°C in airtight bottle until further use.


## 2.2. Materials

The specimens used for corrosion tests were mild steel (MS) coupons which have the following composition (wt %): 0.051 C : 0.023 Si : 0.005 P : 0.103 Al : 0.179 Mn : 0.023 S and the remainder iron. The test solution was industrial water collected from heat exchangers and reboilers of the chemical industries in and around Mysore city, India. The chemical composition of the industrial water (ppm) obtained from ionic chromatograph was 7500 Cl−; 64 Ca2+; 3440SO42-; 23 Mg2+; 140 Na+; 0.28PO43-. Prior to gravimetric and electrochemical measurements, the surface of the specimens was polished under running tap water using emery paper (SiC, grade 220–600), rinsed with distilled water, dried on a clean tissue paper, immersed in benzene for 5 s, dried and immersed in acetone for 5 s, and dried with clean tissue paper. Finally, the specimens were kept in desiccators until use. At the end of the gravimetric experiment, the specimens were carefully washed with acetone and benzene, dried, and then weighed. For polarization and electrochemical impedance studies, the MS specimen was embedded in epoxy resin to expose a geometrical surface area of 1 cm2 to the electrolyte.


## 2.3. Methods

### 2.3.1. Gravimetric Measurements

Gravimetric experiments were carried out in a glass cell, and the solution volume was 100 cm3. The temperature of the environment was maintained by thermostatically controlled water bath (Weiber, India) with an accuracy of ±0.2°C under aerated condition. The mild steel specimens used were rectangular with a dimension of 1 cm × 1 cm × 0.1 cm. The initial weight of the specimen was recorded using an analytical balance (precision ±0.1 mg). After the corrosion test in industrial water with and without inhibitor, the specimens were carefully washed in double distilled water, dried, and then weighed. The weight loss of the specimen was determined after an immersion period of 10 to 50 h at the temperature range of 30 to 60°C. Triplicate experiments were performed in each case, and the average mass loss was reported. The corrosion rate (CR) and inhibition efficiency (% IE) are calculated using
(1)CR=ΔWSt,IE%=(CR)a-(CR)p(CR)a×100,
where ΔW is the weight loss, S is the surface area of the specimen (cm2), t is the immersion time (h), and (CR)a, (CR)p are corrosion rates in the absence and presence of the inhibitor, respectively.


### 2.3.2. Electrochemical Measurements

Electrochemical tests were carried out with a CH-analyzer model CH1660D. The cell arrangement used was a conventional three-electrode cell with platinum counter electrode, saturated calomel electrode as reference electrode, and test material (mild steel) as working electrode. Anodic and cathodic polarization curves were recorded in the potential range from −350 to −800 mV with a scan rate of 0.4 mV s−1. The AC impedance measurements were performed in the frequency range from 10 kHz to 0.05 Hz with signal amplitude of ±10 mV.


### 2.3.3. Morphological Investigation

The surface morphology of the mild steel samples in the absence and presence of AA extracts (1200 ppm in industrial water) at 30°C was investigated by scanning electron microscopy (SEM) technique (Model JSM-5800).


## 2.3.1. Gravimetric Measurements

Gravimetric experiments were carried out in a glass cell, and the solution volume was 100 cm3. The temperature of the environment was maintained by thermostatically controlled water bath (Weiber, India) with an accuracy of ±0.2°C under aerated condition. The mild steel specimens used were rectangular with a dimension of 1 cm × 1 cm × 0.1 cm. The initial weight of the specimen was recorded using an analytical balance (precision ±0.1 mg). After the corrosion test in industrial water with and without inhibitor, the specimens were carefully washed in double distilled water, dried, and then weighed. The weight loss of the specimen was determined after an immersion period of 10 to 50 h at the temperature range of 30 to 60°C. Triplicate experiments were performed in each case, and the average mass loss was reported. The corrosion rate (CR) and inhibition efficiency (% IE) are calculated using
(1)CR=ΔWSt,IE%=(CR)a-(CR)p(CR)a×100,
where ΔW is the weight loss, S is the surface area of the specimen (cm2), t is the immersion time (h), and (CR)a, (CR)p are corrosion rates in the absence and presence of the inhibitor, respectively.


## 2.3.2. Electrochemical Measurements

Electrochemical tests were carried out with a CH-analyzer model CH1660D. The cell arrangement used was a conventional three-electrode cell with platinum counter electrode, saturated calomel electrode as reference electrode, and test material (mild steel) as working electrode. Anodic and cathodic polarization curves were recorded in the potential range from −350 to −800 mV with a scan rate of 0.4 mV s−1. The AC impedance measurements were performed in the frequency range from 10 kHz to 0.05 Hz with signal amplitude of ±10 mV.


## 2.3.3. Morphological Investigation

The surface morphology of the mild steel samples in the absence and presence of AA extracts (1200 ppm in industrial water) at 30°C was investigated by scanning electron microscopy (SEM) technique (Model JSM-5800).


## 3. Results and Discussion

### 3.1. Mass Loss Studies

Weight loss of MS was determined in industrial water medium in the absence and presence of different concentrations of AA extracts. The inhibition efficiency of MS with and without the addition of different concentrations of AA extracts was determined after 40 h at different temperature, and the results are depicted in Table1. It has been observed that 1200 ppm of AA extracts serve as an optimum concentration that exhibit higher inhibition efficiency. The corrosion rate of MS decreased on increasing the inhibitor concentration up to 1200 ppm. This behavior could be attributed to the increase in adsorption of the inhibitor at the metal/solution interface [21] and reduces the surface area that is available for direct attack on the metal surface. Above 1200 ppm, the corrosion rate approximately remained constant. The constant rate obtained could be attributed to the competitive adsorption effect between inhibitor molecules and the metal surface which is already covered with initial layers of molecules [22]. The % IE at different concentrations of AA extracts decreases with increasing temperature from 303 K to 333 K (Figure 1). This is due to increased rate of dissolution process of MS and partial desorption of the inhibitor from the metal surface with temperature [23].Table 1
C
R and IE (%) obtained from weight loss measurements of MS in industrial water medium containing various concentrations of AA extracts at different temperatures.
C (ppm)
Temperature
30°C
40°C
50°C
60°C
C
R (mg cm−2 h−1)
IE %
C
R (mg cm−2 h−1)
IE %
C
R (mg cm−2 h−1)
IE %
C
R (mg cm−2 h−1)
IE %
0
0.1204
—
01428
—
0.2048
—
0.3326
—
200
0.0573
52.40
0.0736
48.48
0.1122
44.04
0.2001
39.84
400
0.0501
58.38
0.0656
54.08
0.1011
50.63
0.1795
46.09
600
0.0433
64.03
0.0568
60.24
0.0901
56.00
0.1601
51.87
800
0.0365
69.68
0.0499
65.07
0.0795
61.18
0.1426
57.13
1000
0.0298
75.24
0.0406
71.58
0.0668
67.38
0.1201
63.89
1200
0.0223
81.47
0.0328
77.04
0.0552
73.04
0.0995
70.08Figure 1
Variation of inhibition efficiency with temperature and inhibitor concentration in the absence and presence of different concentrations of AA extracts.The inhibitive effect of AA extracts is ascribed to the presence of several organic compounds in the extracts. AA extracts are rich in organic compounds of high molecular weight with heteroatoms andπ centers in their molecular structures. These include several flavonoids, tannins, reducing sugars, alkaloids, saponines, glycosides, fatty acids, ecdysterone, betaine, and triterpenoids. The synergistic and antagonistic effects may play an important role in the inhibition efficiency of AA extracts [24].


### 3.2. Effect of Immersion Time

In order to assess the stability of the inhibitor on MS surface, weight loss measurements were performed in industrial water medium in the absence and presence of AA extract for 10–50 h of immersion time at 303 K. From Figure2, it can be observed that the inhibition efficiency of AA extracts increased with immersion time and stabilized after 40 hr. This increase in inhibition of AA extracts with immersion time reflects strong adsorption on the mild steel surface resulting in a more protective layer.Figure 2
Effect of immersion time on IE % of AA extracts.


### 3.3. Effect of Temperature

Analysis of temperature dependence of inhibition efficiency and comparison of corrosion activation energies in the absence and presence of AA extracts give some insight into the possible mechanism of inhibitor adsorption. The weight loss measurements were carried out as a function of temperature (30 to 60°C) and concentration (200 to 1200 ppm) at 10 to 50 h immersion time.The percentage inhibition efficiencies (IE%) and corrosion rates (CR) are summarized in Table1. It was found that increase in temperature leads to an increase in the corrosion rate in the absence and presence of AA extracts in industrial water medium. The dependence of corrosion rate on temperature can be expressed by the following Arrhenius equation:
(2)CR=Aexp(-Ea*RT),
where Ea* is the apparent activation energy, T is the absolute temperature, A is the Arrhenius preexponential constant, and R is the universal gas constant. The apparent activation energy and preexponential factor for different concentrations of the inhibitor were calculated from the plots of logarithm of CR versus 1/T (Figure 3), and the results are shown in Table 2. It is clear that the activation energy increases in the presence of AA extracts and consequently corrosion rate decreases. An alternative formulation of Arrhenius equation is [25]
(3)CR=RTNhexpΔS*Rexp(-ΔH*RT),
where h is Planck’s constant, N is Avogadro’s number, R is the universal gas constant, ΔH* is the enthalpy of activation, and ΔS*is the entropy of activation. Using (3), plots of log (CR/T) versus 1/T gave straight lines with a slope of (-ΔH*/2.303R) and an intercept of [log(R/Nh)+ΔS*/2.303R] (Figure 4) from which the values of ΔH* and ΔS*are calculated and tabulated in Table 2. Inspection of Table 2 reveals that the calculated values of ΔS* for AA extracts in industrial water medium are large and negative. The entropy of activation values are less negative for inhibited solutions than that for the uninhibited solutions. This suggests that an increase in randomness occurred while moving from reactants to the activated complex [26]. The positive sign of ΔH* reflects the endothermic nature of the MS dissolution process, suggesting that the dissolution of MS is slow in the presence of inhibitor [27]. The values of ΔH* could also be obtained from the following equation:
(4)ΔH*=Ea*-RT.
The values of ΔH* obtained here are in very good agreement with those obtained from (3), confirming the endothermic process of mild steel dissolution in industrial water medium.Table 2
Activation parameters for MS in industrial water medium in the absence and presence of different concentrations of AA extracts.
C (ppm)
E
a
* (kJ mol−1)
k (mg cm−2 h−1)
Δ
H
* (kJ mol−1)
Δ
H
*
=
E
a
*
-
R
T (kJ mol−1)
Δ
S
* (J mol−1 K−1)
0
28.41
9977.06
25.77
25.89
-
178.35
200
35.34
66221.65
32.16
32.82
-
163.43
400
35.47
65162.84
32.91
32.96
-
162.03
600
36.66
93972.33
33.94
34.14
-
159.85
800
38.84
181970.1
35.40
36.33
-
156.44
1000
39.80
215774.4
36.43
37.28
-
154.72
1200
40.11
179060.6
39.23
37.59
-
147.77Figure 3
Arrhenius plots for MS in industrial water medium in the absence and presence of different concentrations of AA extracts.Figure 4
Alternative Arrhenius plots for MS in industrial water medium in the absence and presence of different concentrations of AA extracts.


### 3.4. Adsorption Isotherm

The surface coverage(θ) of corrosion inhibitor on MS is the most useful parameter for the study of the adsorption behaviour of the inhibitor. A direct relationship between inhibition efficiency and the degree of surface coverage can be assumed for different concentrations of the inhibitor. Data obtained from mass loss measurements were tested graphically for fitting various isotherms including Langmuir, Frumkin, and Temkin. However, the best fit is obtained from Langmuir isotherm (Figure 5). This isotherm assumes that the adsorbed molecules occupy only one site, and there are no interactions with other adsorbed species [28]. According to this isotherm Θ is related to inhibitor concentration as
(5)Cθ=1Kads+C,
where Kads is the equilibrium constant for adsorption, C is the concentration of the inhibitor, and θ is the surface coverage. The strong correlation (R2>0.97) suggests that the adsorption of inhibitor on the MS surface obeyed this isotherm. The Kads is related to the free energy of adsorption (ΔGads) using the following equation:
(6)Kads=155.5exp(-ΔGadsRT),
where R is the universal gas constant, T is the absolute temperature, and 55.5 is the concentration of water in solution (mol L−1). The values free energy of adsorption for AA extracts are presented in Table 3. The negative values of ΔGads means that the adsorption of AA on MS surface is a spontaneous process and furthermore shows the strong interaction of the inhibitor onto the MS surface [29].Table 3
Thermodynamic adsorption parameters for adsorption of AA extracts on MS in industrial water medium at different temperatures from Langmuir adsorption isotherm.
Temperature (K)
R
2
K
ads (L g−1)
Δ
G
ads (kJ mol−1)
Δ
H
ads (kJ mol−1)
Δ
S
ads (J mol−1 K−1)
Δ
G
ads
=
Δ
H
ads
-
T
Δ
S
ads (kJ mol−1)
303
0.983
4310.34
-
31.20
-
30.26
313
0.981
3816.79
-
31.91
−11.98a  −12.11b
63.58a  63b
-
30.90
323
0.977
3448.27
-
32.66
-
31.53
333
0.970
2762.43
-
33.06
-
32.17
aValues obtained from (7). bValues obtained from (8).Figure 5
Langmuir adsorption isotherm of AA extracts on MS in industrial water medium at different temperatures.Generally,ΔGads values of the order of −20 kJ mol−1 or higher are associated with an electrostatic interaction between charged molecules and charged metal surface (physisorption), and those of −40 kJ mol−1 or lower indicate charge sharing or a transfer from the inhibitor molecules to the metal surface to form a coordinate covalent bond (chemisorption) [30]. The values for ΔGads for AA extracts on the MS surface are in the ranges of −31.20 to −33.06; indicating that the adsorption of AA extracts on MS surface is neither typical physisorption nor typical chemisorption, but it is a complex mixed—type adsorption; that is, it involves both physisorption and chemisorption [31]. The enthalpy and entropy of adsorption (ΔHads and ΔSads) can be calculated using
(7)lnKads=ln155.5-ΔHadsRT+ΔSadsR.
From (7), the values of ΔHads and ΔSads were evaluated from the slope and intercept of the plot of lnKads versus 1/T (Figure 6). All the calculated thermodynamic parameters are listed in Table 3. It has been found that the values ΔHads are negative, suggesting that the adsorption of the inhibitor is an exothermic process [32]. Adsorption entropy is positive and large indicating that the driving force for the adsorption of adsorbate is the increase in entropy during the process of adsorption rather than the decrease in enthalpy [33].Figure 6
Plot oflnKads versus 1/T.The values ofΔHads and ΔSads can also be calculated by using following equation:
(8)ΔGads=ΔHads-TΔSads.
Using (8), the plot of ΔGads versus T gives a straight line (Figure 7) with a slope of -ΔSads and intercept of ΔHads. The values obtained are well correlated with those obtained from (7).Figure 7
Plot of Gibbs free energy versus absolute temperature.


### 3.5. Potentiodynamic Polarization Studies.

Anodic and cathodic polarization curves for MS in industrial water medium without and with different concentrations of AA extracts are shown in Figure8. It is observed that both cathodic and anodic curves show a lower current density in the presence of AA extracts than those recorded in the industrial water medium alone. The values of corrosion potential (Ecorr), corrosion current density (Icorr), anodic Tafel slope (ba) and cathodic Tafel slope (bc), and percentage inhibition efficiency (IE %) are presented in Table 4. The % IE was calculated from polarization measurements according to following equation:
(9)IE(%)=(Icorr)a-(Icorr)p(Icorr)a×100,
where (Icorr)a and (Icorr)p are the corrosion current densities (mA cm−2) in the absence and presence of the inhibitor, respectively. From Figure 8, it is evident that the addition of AA extracts shifts the corrosion potential (Ecorr) values significantly in cathodic direction. The presence of AA extracts causes a significant decrease in the corrosion rate that is predominantly shifts the cathodic curves to lower values of current densities. On the other hand, the anodic reaction is slightly affected by AA extracts. But it alters both the tafel slope values indicating that AA extracts act as a mixed type of inhibitor [34]. The % IE increases with the inhibitor concentration due to the increase in the blocked fraction of the electrode surface by adsorption. % IE of AA extracts reaches to as high as 81.23 which indicates that AA extracts are a good inhibitor for MS in industrial water medium.Table 4
E
corr, Icorr, Rct, and IE % obtained from polarization and impedance measurements for mild steel in industrial water medium containing various concentrations of AA extracts at 30°C.
C (ppm)
EIS
Polarization
R
ct (Ω cm2)
IE %
E
corr (mV)
I
corr (mA cm−2)
b
a (mA dec−1)
b
c (mA dec−1)
IE %
0
111.7
-
0.785
0.00476
6.000
1.034
200
226.7
50.72
-
0.503
0.00250
10.585
2.301
47.57
400
232.7
51.99
-
0.574
0.00270
12.216
3.715
52.29
600
290.6
61.56
-
0.706
0.00199
10.174
1.380
58.29
800
328.7
66.01
-
0.684
0.00156
9.978
1.763
67.23
1000
412.0
72.88
-
0.653
0.00128
7.320
1.481
73.14
1200
559.7
80.04
-
0.610
0.00089
8.949
2.423
81.23Figure 8
Potentiodynamic polarization curves for MS in industrial water medium containing different concentrations of compound AA extracts.


### 3.6. Electrochemical Impedance Spectroscopy (EIS)

Figure9 shows the impedance response of MS in industrial water medium without and with different concentration of the inhibitor. Nyquist impedance plots were analyzed by fitting the experimental data to a simple circuit model (Figure 10). All the obtained plots show only one capacitive loop, and the diameter of the semicircle increases with increasing the inhibitor concentration suggesting that the inhibitive film formed was strengthened by the addition of inhibitor [35]. The presence of the inhibitor increases the impedance but does not change other aspects of the behavior. These results support the results of polarization measurements that the inhibitor does not alter the electrochemical reactions responsible for corrosion. The experimental results of EIS measurements for the corrosion of MS in industrial water medium in the absence and presence of AA extracts are given in Table 4. Inspection of the Table 4 shows that AA extracts enhances the charge transfer resistance which is attributed to a decrease in local dielectric constant and/or an increase in the thickness of electrical double layer [36]. % IE obtained from this technique is also comparable with those obtained from polarization measurements.Figure 9
Nyquist plots for MS in industrial water medium containing different concentrations of AA extracts.Figure 10
Equivalent circuit diagram.


### 3.7. Scanning Electron Microscopy (SEM)

To establish whether inhibition of MS surface is due to the formation of inhibitor protective film on the metal surface, SEM images were taken. SEM photographs obtained from MS surface after immersion in industrial water medium in the absence and presence of optimum concentration of inhibitors are shown in Figures11(a)–11(c). Figure 11(a) shows the clear smooth surface morphology of MS examined. It can be seen from Figure 11(b) that the MS surface is strongly damaged in the absence of the inhibitor (blank). Figure 11(c) showed the protected MS surface after the addition of AA extracts, whereby the surface damage has diminished in comparison to the blank material. This is attributed to the formation of a good protective film on the MS surface.SEM images of MS in industrial water medium after 40 h of immersion at 30°C (a) before immersion (polished), (b) without inhibitor (blank), and (c) with 1200 ppm of AA extracts.
(a)
(b)
(c)


## 3.1. Mass Loss Studies

Weight loss of MS was determined in industrial water medium in the absence and presence of different concentrations of AA extracts. The inhibition efficiency of MS with and without the addition of different concentrations of AA extracts was determined after 40 h at different temperature, and the results are depicted in Table1. It has been observed that 1200 ppm of AA extracts serve as an optimum concentration that exhibit higher inhibition efficiency. The corrosion rate of MS decreased on increasing the inhibitor concentration up to 1200 ppm. This behavior could be attributed to the increase in adsorption of the inhibitor at the metal/solution interface [21] and reduces the surface area that is available for direct attack on the metal surface. Above 1200 ppm, the corrosion rate approximately remained constant. The constant rate obtained could be attributed to the competitive adsorption effect between inhibitor molecules and the metal surface which is already covered with initial layers of molecules [22]. The % IE at different concentrations of AA extracts decreases with increasing temperature from 303 K to 333 K (Figure 1). This is due to increased rate of dissolution process of MS and partial desorption of the inhibitor from the metal surface with temperature [23].Table 1
C
R and IE (%) obtained from weight loss measurements of MS in industrial water medium containing various concentrations of AA extracts at different temperatures.
C (ppm)
Temperature
30°C
40°C
50°C
60°C
C
R (mg cm−2 h−1)
IE %
C
R (mg cm−2 h−1)
IE %
C
R (mg cm−2 h−1)
IE %
C
R (mg cm−2 h−1)
IE %
0
0.1204
—
01428
—
0.2048
—
0.3326
—
200
0.0573
52.40
0.0736
48.48
0.1122
44.04
0.2001
39.84
400
0.0501
58.38
0.0656
54.08
0.1011
50.63
0.1795
46.09
600
0.0433
64.03
0.0568
60.24
0.0901
56.00
0.1601
51.87
800
0.0365
69.68
0.0499
65.07
0.0795
61.18
0.1426
57.13
1000
0.0298
75.24
0.0406
71.58
0.0668
67.38
0.1201
63.89
1200
0.0223
81.47
0.0328
77.04
0.0552
73.04
0.0995
70.08Figure 1
Variation of inhibition efficiency with temperature and inhibitor concentration in the absence and presence of different concentrations of AA extracts.The inhibitive effect of AA extracts is ascribed to the presence of several organic compounds in the extracts. AA extracts are rich in organic compounds of high molecular weight with heteroatoms andπ centers in their molecular structures. These include several flavonoids, tannins, reducing sugars, alkaloids, saponines, glycosides, fatty acids, ecdysterone, betaine, and triterpenoids. The synergistic and antagonistic effects may play an important role in the inhibition efficiency of AA extracts [24].


## 3.2. Effect of Immersion Time

In order to assess the stability of the inhibitor on MS surface, weight loss measurements were performed in industrial water medium in the absence and presence of AA extract for 10–50 h of immersion time at 303 K. From Figure2, it can be observed that the inhibition efficiency of AA extracts increased with immersion time and stabilized after 40 hr. This increase in inhibition of AA extracts with immersion time reflects strong adsorption on the mild steel surface resulting in a more protective layer.Figure 2
Effect of immersion time on IE % of AA extracts.


## 3.3. Effect of Temperature

Analysis of temperature dependence of inhibition efficiency and comparison of corrosion activation energies in the absence and presence of AA extracts give some insight into the possible mechanism of inhibitor adsorption. The weight loss measurements were carried out as a function of temperature (30 to 60°C) and concentration (200 to 1200 ppm) at 10 to 50 h immersion time.The percentage inhibition efficiencies (IE%) and corrosion rates (CR) are summarized in Table1. It was found that increase in temperature leads to an increase in the corrosion rate in the absence and presence of AA extracts in industrial water medium. The dependence of corrosion rate on temperature can be expressed by the following Arrhenius equation:
(2)CR=Aexp(-Ea*RT),
where Ea* is the apparent activation energy, T is the absolute temperature, A is the Arrhenius preexponential constant, and R is the universal gas constant. The apparent activation energy and preexponential factor for different concentrations of the inhibitor were calculated from the plots of logarithm of CR versus 1/T (Figure 3), and the results are shown in Table 2. It is clear that the activation energy increases in the presence of AA extracts and consequently corrosion rate decreases. An alternative formulation of Arrhenius equation is [25]
(3)CR=RTNhexpΔS*Rexp(-ΔH*RT),
where h is Planck’s constant, N is Avogadro’s number, R is the universal gas constant, ΔH* is the enthalpy of activation, and ΔS*is the entropy of activation. Using (3), plots of log (CR/T) versus 1/T gave straight lines with a slope of (-ΔH*/2.303R) and an intercept of [log(R/Nh)+ΔS*/2.303R] (Figure 4) from which the values of ΔH* and ΔS*are calculated and tabulated in Table 2. Inspection of Table 2 reveals that the calculated values of ΔS* for AA extracts in industrial water medium are large and negative. The entropy of activation values are less negative for inhibited solutions than that for the uninhibited solutions. This suggests that an increase in randomness occurred while moving from reactants to the activated complex [26]. The positive sign of ΔH* reflects the endothermic nature of the MS dissolution process, suggesting that the dissolution of MS is slow in the presence of inhibitor [27]. The values of ΔH* could also be obtained from the following equation:
(4)ΔH*=Ea*-RT.
The values of ΔH* obtained here are in very good agreement with those obtained from (3), confirming the endothermic process of mild steel dissolution in industrial water medium.Table 2
Activation parameters for MS in industrial water medium in the absence and presence of different concentrations of AA extracts.
C (ppm)
E
a
* (kJ mol−1)
k (mg cm−2 h−1)
Δ
H
* (kJ mol−1)
Δ
H
*
=
E
a
*
-
R
T (kJ mol−1)
Δ
S
* (J mol−1 K−1)
0
28.41
9977.06
25.77
25.89
-
178.35
200
35.34
66221.65
32.16
32.82
-
163.43
400
35.47
65162.84
32.91
32.96
-
162.03
600
36.66
93972.33
33.94
34.14
-
159.85
800
38.84
181970.1
35.40
36.33
-
156.44
1000
39.80
215774.4
36.43
37.28
-
154.72
1200
40.11
179060.6
39.23
37.59
-
147.77Figure 3
Arrhenius plots for MS in industrial water medium in the absence and presence of different concentrations of AA extracts.Figure 4
Alternative Arrhenius plots for MS in industrial water medium in the absence and presence of different concentrations of AA extracts.


## 3.4. Adsorption Isotherm

The surface coverage(θ) of corrosion inhibitor on MS is the most useful parameter for the study of the adsorption behaviour of the inhibitor. A direct relationship between inhibition efficiency and the degree of surface coverage can be assumed for different concentrations of the inhibitor. Data obtained from mass loss measurements were tested graphically for fitting various isotherms including Langmuir, Frumkin, and Temkin. However, the best fit is obtained from Langmuir isotherm (Figure 5). This isotherm assumes that the adsorbed molecules occupy only one site, and there are no interactions with other adsorbed species [28]. According to this isotherm Θ is related to inhibitor concentration as
(5)Cθ=1Kads+C,
where Kads is the equilibrium constant for adsorption, C is the concentration of the inhibitor, and θ is the surface coverage. The strong correlation (R2>0.97) suggests that the adsorption of inhibitor on the MS surface obeyed this isotherm. The Kads is related to the free energy of adsorption (ΔGads) using the following equation:
(6)Kads=155.5exp(-ΔGadsRT),
where R is the universal gas constant, T is the absolute temperature, and 55.5 is the concentration of water in solution (mol L−1). The values free energy of adsorption for AA extracts are presented in Table 3. The negative values of ΔGads means that the adsorption of AA on MS surface is a spontaneous process and furthermore shows the strong interaction of the inhibitor onto the MS surface [29].Table 3
Thermodynamic adsorption parameters for adsorption of AA extracts on MS in industrial water medium at different temperatures from Langmuir adsorption isotherm.
Temperature (K)
R
2
K
ads (L g−1)
Δ
G
ads (kJ mol−1)
Δ
H
ads (kJ mol−1)
Δ
S
ads (J mol−1 K−1)
Δ
G
ads
=
Δ
H
ads
-
T
Δ
S
ads (kJ mol−1)
303
0.983
4310.34
-
31.20
-
30.26
313
0.981
3816.79
-
31.91
−11.98a  −12.11b
63.58a  63b
-
30.90
323
0.977
3448.27
-
32.66
-
31.53
333
0.970
2762.43
-
33.06
-
32.17
aValues obtained from (7). bValues obtained from (8).Figure 5
Langmuir adsorption isotherm of AA extracts on MS in industrial water medium at different temperatures.Generally,ΔGads values of the order of −20 kJ mol−1 or higher are associated with an electrostatic interaction between charged molecules and charged metal surface (physisorption), and those of −40 kJ mol−1 or lower indicate charge sharing or a transfer from the inhibitor molecules to the metal surface to form a coordinate covalent bond (chemisorption) [30]. The values for ΔGads for AA extracts on the MS surface are in the ranges of −31.20 to −33.06; indicating that the adsorption of AA extracts on MS surface is neither typical physisorption nor typical chemisorption, but it is a complex mixed—type adsorption; that is, it involves both physisorption and chemisorption [31]. The enthalpy and entropy of adsorption (ΔHads and ΔSads) can be calculated using
(7)lnKads=ln155.5-ΔHadsRT+ΔSadsR.
From (7), the values of ΔHads and ΔSads were evaluated from the slope and intercept of the plot of lnKads versus 1/T (Figure 6). All the calculated thermodynamic parameters are listed in Table 3. It has been found that the values ΔHads are negative, suggesting that the adsorption of the inhibitor is an exothermic process [32]. Adsorption entropy is positive and large indicating that the driving force for the adsorption of adsorbate is the increase in entropy during the process of adsorption rather than the decrease in enthalpy [33].Figure 6
Plot oflnKads versus 1/T.The values ofΔHads and ΔSads can also be calculated by using following equation:
(8)ΔGads=ΔHads-TΔSads.
Using (8), the plot of ΔGads versus T gives a straight line (Figure 7) with a slope of -ΔSads and intercept of ΔHads. The values obtained are well correlated with those obtained from (7).Figure 7
Plot of Gibbs free energy versus absolute temperature.


## 3.5. Potentiodynamic Polarization Studies.

Anodic and cathodic polarization curves for MS in industrial water medium without and with different concentrations of AA extracts are shown in Figure8. It is observed that both cathodic and anodic curves show a lower current density in the presence of AA extracts than those recorded in the industrial water medium alone. The values of corrosion potential (Ecorr), corrosion current density (Icorr), anodic Tafel slope (ba) and cathodic Tafel slope (bc), and percentage inhibition efficiency (IE %) are presented in Table 4. The % IE was calculated from polarization measurements according to following equation:
(9)IE(%)=(Icorr)a-(Icorr)p(Icorr)a×100,
where (Icorr)a and (Icorr)p are the corrosion current densities (mA cm−2) in the absence and presence of the inhibitor, respectively. From Figure 8, it is evident that the addition of AA extracts shifts the corrosion potential (Ecorr) values significantly in cathodic direction. The presence of AA extracts causes a significant decrease in the corrosion rate that is predominantly shifts the cathodic curves to lower values of current densities. On the other hand, the anodic reaction is slightly affected by AA extracts. But it alters both the tafel slope values indicating that AA extracts act as a mixed type of inhibitor [34]. The % IE increases with the inhibitor concentration due to the increase in the blocked fraction of the electrode surface by adsorption. % IE of AA extracts reaches to as high as 81.23 which indicates that AA extracts are a good inhibitor for MS in industrial water medium.Table 4
E
corr, Icorr, Rct, and IE % obtained from polarization and impedance measurements for mild steel in industrial water medium containing various concentrations of AA extracts at 30°C.
C (ppm)
EIS
Polarization
R
ct (Ω cm2)
IE %
E
corr (mV)
I
corr (mA cm−2)
b
a (mA dec−1)
b
c (mA dec−1)
IE %
0
111.7
-
0.785
0.00476
6.000
1.034
200
226.7
50.72
-
0.503
0.00250
10.585
2.301
47.57
400
232.7
51.99
-
0.574
0.00270
12.216
3.715
52.29
600
290.6
61.56
-
0.706
0.00199
10.174
1.380
58.29
800
328.7
66.01
-
0.684
0.00156
9.978
1.763
67.23
1000
412.0
72.88
-
0.653
0.00128
7.320
1.481
73.14
1200
559.7
80.04
-
0.610
0.00089
8.949
2.423
81.23Figure 8
Potentiodynamic polarization curves for MS in industrial water medium containing different concentrations of compound AA extracts.


## 3.6. Electrochemical Impedance Spectroscopy (EIS)

Figure9 shows the impedance response of MS in industrial water medium without and with different concentration of the inhibitor. Nyquist impedance plots were analyzed by fitting the experimental data to a simple circuit model (Figure 10). All the obtained plots show only one capacitive loop, and the diameter of the semicircle increases with increasing the inhibitor concentration suggesting that the inhibitive film formed was strengthened by the addition of inhibitor [35]. The presence of the inhibitor increases the impedance but does not change other aspects of the behavior. These results support the results of polarization measurements that the inhibitor does not alter the electrochemical reactions responsible for corrosion. The experimental results of EIS measurements for the corrosion of MS in industrial water medium in the absence and presence of AA extracts are given in Table 4. Inspection of the Table 4 shows that AA extracts enhances the charge transfer resistance which is attributed to a decrease in local dielectric constant and/or an increase in the thickness of electrical double layer [36]. % IE obtained from this technique is also comparable with those obtained from polarization measurements.Figure 9
Nyquist plots for MS in industrial water medium containing different concentrations of AA extracts.Figure 10
Equivalent circuit diagram.


## 3.7. Scanning Electron Microscopy (SEM)

To establish whether inhibition of MS surface is due to the formation of inhibitor protective film on the metal surface, SEM images were taken. SEM photographs obtained from MS surface after immersion in industrial water medium in the absence and presence of optimum concentration of inhibitors are shown in Figures11(a)–11(c). Figure 11(a) shows the clear smooth surface morphology of MS examined. It can be seen from Figure 11(b) that the MS surface is strongly damaged in the absence of the inhibitor (blank). Figure 11(c) showed the protected MS surface after the addition of AA extracts, whereby the surface damage has diminished in comparison to the blank material. This is attributed to the formation of a good protective film on the MS surface.SEM images of MS in industrial water medium after 40 h of immersion at 30°C (a) before immersion (polished), (b) without inhibitor (blank), and (c) with 1200 ppm of AA extracts.
(a)
(b)
(c)


## 4. Conclusion

(1)
The inhibition efficiency of AA extracts increases with the inhibitor concentration and reaches a maximum at 1200 ppm of AA extracts.
(2)
IE % decreases with the increasing temperature in industrial water medium and remains constant at higher temperature.
(3)
The adsorption of AA extracts in industrial water medium on MS surface obeys Langmuir adsorption isotherm. The adsorption process involved is both physisorption and chemisorption.
(4)
Polarization curves indicate that AA extracts act as mixed type of inhibitor.
(5)
The adsorbed film containing the investigated compound was identified by SEM analysis.



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*Source: 261847-2013-05-28.xml*