# A Revisit to the Corrosion Inhibition of Aluminum in Aqueous Alkaline Solutions by Water-Soluble Alginates and Pectates as Anionic Polyelectrolyte Inhibitors

Authors: Refat Hassan; Ishaq Zaafarany; Adil Gobouri; Hideo Takagi
Journal: International Journal of Corrosion
 (2013)

---

## Abstract

The corrosion behavior of aluminum (Al) in alkaline media in presence of some natural polymer inhibitors has been reinvestigated. The inhibition action of the tested inhibitors was found to obey both Langmuir and Freundlich isotherms models. The inhibition efficiency was found to increase with increasing the inhibitors concentration and decrease with increasing the temperature, suggesting physical adsorption mechanism. Factors such as the concentration and geometrical structure of the inhibitor, concentration of the corrosive medium, and temperature affecting the corrosion rates were examined. The kinetic parameters were evaluated, and a suitable corrosion mechanism consistent with the kinetic results obtained is suggested and discussed.


---

## Body

## 1. Introduction

Aluminum and its alloys are known as attractive materials which have a wide application in engineering technology owing to their low cost, light weights, and high thermal and electrical conductivities [1]. They also showed high resistivity toward a wide variety of corrosion environments [2]. This behavior may be attributed to the formation of a protective, tightly adhered invisible oxide film on the metal surface.The remarkable potential applications of aluminum in industrial technology particularly in aluminum-air industry encouraged many investigators to study the influence of various inhibitors on Al dissolution in both acidic [1–14] and alkaline [15–20] media since the kinetics of dissolution is reduced by the presence of a thick oxide-hydroxide film at the anode surface. Most of workers have directed their research towards concentrated alkaline media, which permit optimum performance of the air cathode and a low level of aluminum polarization during normal operation [20].Unfortunately, most of the inhibitors available in the markets are not only expensive but also toxic to living beings. Again, the safety of environmental issues of corrosion inhibitors which may be arise in industry has always been a global concern. Therefore, the cheap, nontoxic, ecological, and friendly corrosion inhibitors are of more importance. Consequently, many alternative ecofriendly corrosion inhibitors have been developed [17].Recently, the influence of alginate and pectate anionic polyelectrolyte as natural polymers inhibitors on the behavior of dissolution of Al metal in alkaline solutions has been reported elsewhere [21]. Unfortunately, the adsorption isotherm models have not been tested to the experimental results. Hence, the information on the corrosion mechanism still remains incomplete.In view of the above arguments and our interest in physicochemical properties of macromolecules in particularly biodegradable and nontoxic polysaccharides [22–38], the present work seems to merit a further reinvestigation with the aims at shedding more highlights on the corrosion behavior in terms of fitting the kinetic data to the adsorption isotherm models. Furthermore, this study aims to throw some light on the role of the functional groups and geometrical configuration of the inhibitors used in the adsorption process as well as the influence of the nature of the medium on the corrosion mechanism.


## 2. Experimental

### 2.1. Materials

All materials used were of analytical grade. Doubly distilled conductivity water was used in all preparations. The temperature was controlled within ±0.1°C.Sodium alginate (ALG) and sodium pectate (PEC) were purchased from Fluka and were used without further purification. The degree of substitution was found to be 4.3 mmol g−1 (0.91 mol mol−1) and 4.1 mmol g−1 (0.82 mol mol−1) for alginates and pectates, respectively.Aluminum metal used was of 99.98% purity (Ventron Crop, Osaka, Japan).


### 2.2. Preparation of Inhibitor Sols

Sols of alginate and pectate polysaccharides were prepared as described earlier [21, 22]. This process was performed by stepwise addition of the powder reagent to bidistilled water whilst rapidly and vigorously stirring the solutions to avoid the formation of lumps, which swell with difficulty. Then, the prepared alginate or pectate sols were left at room temperature (25°C) for about 24 h in order to become air-bubbles-free being before used.


### 2.3. Measurement Techniques

Although the weight-loss technique is the most employed method to acquire the corrosion rate data for metal coupons at natural environmental corrosion tests, it makes the corrosion rate obtained a long-term average; that is, it needs a long-time immersion. Therefore, gasometric method is usually preferred for assessing the inhibitive performance in case of short-time immersion of the corrosive metals in acidic or alkaline solutions as in the cited work. The technique was the same as described elsewhere [18]. The course of reaction was followed by measuring the evolved hydrogen gas, as a function of time.Some kinetic measurements were performed using the classical weight-loss method [1, 13, 39, 40] in order to check the reproducibility of the gasometric data obtained. Fortunately, the results obtained for the corrosion rates in both techniques were found to be correlated with each other within experimental errors (±5%). This fact may indicate the reproducibility of the results obtained by the gasometric method.All experiments were repeated using different concentrations of NaOH and inhibitors at various temperatures. The cited results were at least an average of four experimental runs. The corrosion medium was not stirred during the test. The experimental data obtained were found to well agree with that reported earlier (within experimental errors ±5%) [21].


## 2.1. Materials

All materials used were of analytical grade. Doubly distilled conductivity water was used in all preparations. The temperature was controlled within ±0.1°C.Sodium alginate (ALG) and sodium pectate (PEC) were purchased from Fluka and were used without further purification. The degree of substitution was found to be 4.3 mmol g−1 (0.91 mol mol−1) and 4.1 mmol g−1 (0.82 mol mol−1) for alginates and pectates, respectively.Aluminum metal used was of 99.98% purity (Ventron Crop, Osaka, Japan).


## 2.2. Preparation of Inhibitor Sols

Sols of alginate and pectate polysaccharides were prepared as described earlier [21, 22]. This process was performed by stepwise addition of the powder reagent to bidistilled water whilst rapidly and vigorously stirring the solutions to avoid the formation of lumps, which swell with difficulty. Then, the prepared alginate or pectate sols were left at room temperature (25°C) for about 24 h in order to become air-bubbles-free being before used.


## 2.3. Measurement Techniques

Although the weight-loss technique is the most employed method to acquire the corrosion rate data for metal coupons at natural environmental corrosion tests, it makes the corrosion rate obtained a long-term average; that is, it needs a long-time immersion. Therefore, gasometric method is usually preferred for assessing the inhibitive performance in case of short-time immersion of the corrosive metals in acidic or alkaline solutions as in the cited work. The technique was the same as described elsewhere [18]. The course of reaction was followed by measuring the evolved hydrogen gas, as a function of time.Some kinetic measurements were performed using the classical weight-loss method [1, 13, 39, 40] in order to check the reproducibility of the gasometric data obtained. Fortunately, the results obtained for the corrosion rates in both techniques were found to be correlated with each other within experimental errors (±5%). This fact may indicate the reproducibility of the results obtained by the gasometric method.All experiments were repeated using different concentrations of NaOH and inhibitors at various temperatures. The cited results were at least an average of four experimental runs. The corrosion medium was not stirred during the test. The experimental data obtained were found to well agree with that reported earlier (within experimental errors ±5%) [21].


## 3. Results and Discussions

### 3.1. Hydrogen Evolution and Weight-Loss Measurements

The volume of the evolved H2 gas (or the loss in Al weight) as a function of time may be taken as the rate of dissolution of aluminum in sodium hydroxide and can be expressed, respectively, by
(1)Rc=VH2L·t,(2)Rc=ΔWL·t,
where Rc is the corrosion rate, L is the surface area of Al metal sheet (cm2), t is the immersion period (min), VH2 is volume of evolved hydrogen gas (mL), and ΔW is the weight-loss (mg) of Al metal dissolved into the corrosive medium. Typical plots of the gasometric and weight-loss data are shown in Figures 1 and 2, respectively. These plots revealed that the volume of H2 evolved or the loss in weight is varied linearly with the immersion times. The rate of corrosion (Rc) can be obtained from the slopes of the linear portions of such plots which corresponds to the rate constants of dissolution of Al in alkaline media obtained from either evolved hydrogen or the weight-loss methods. These values were calculated by the least-squares method and are summarized in Table 1.Table 1
The corrosion rates (Rc) for corrosion of Al in alkaline media in absence and presence of inhibitors. [OH−] = 4.0 and I = 4.0 mol dm−3 at  30°C.
[Inhibitor]mol dm−3
0.0
0.01
0.02
0.03
0.04
Alginate
0.52 (0.48)*
0.33
0.28
0.22
0.16
Pectates
0.52 (0.48)*
0.25
0.20
0.15
0.11
*Calculated from the weight-loss method.Figure 1
A typical plot of the evolvedVH2 versus time for corrosion of Al in alkaline media in absence of inhibitors at 30°C. [OH−] = 4.0 mol dm−3.Figure 2
A typical plot of the weight-loss versus time for corrosion of Al in alkaline media in absence of inhibitors at 30°C. [OH−] = 4.0 mol dm−3.


### 3.2. Inhibition Efficiency (% I.E.)

The inhibition efficiencies of the added inhibitors were calculated using the following relationship:(3)%I.E.=Rc°-Rc’Rc°×100,
where Rc° and Rc’ are the corrosion rates of Al metal in absence and presence of such natural polymeric inhibitors, respectively. The results are summarized in Table 2. The values of inhibition efficiency (% I.E.) listed in Table 2 were found to follow the same trend, which increases with increasing the inhibitors concentration and decreases with rising the temperature.Table 2
Percentage of inhibitor efficiency (% I.E.) for corrosion of Al in alkaline media in presence of inhibitors.[OH−] = 4.0 and I = 4.0 mol dm−3 at 30°C.
[Inhibitor] mol dm−3
0.01
0.02
0.03
0.04
Alginate
36.54
46.15
57.69
69.23
Pectates
51.92
61.54
71.15
78.85


### 3.3. Dependence of Corrosion Rates on [OH−]

In order to examine the corrosion rates as a function of alkali concentration, some experimental runs were performed at various initial concentrations of the alkali and constants of all other reagents. Plots ofVH2 gas versus time (evolved active H2) were found to be linear in which the rate constants increased with increasing the [OH−] as shown in Figure 3. This result means that the corrosion rate is a function of the alkali concentration.Figure 3
Plots of evolvedVH2 versus time for corrosion of Al in alkaline media in absence of inhibitors at 30°C. [OH−]: (A)=2.0; (B)=3.0; (C)=4.0 mol dm−3.


### 3.4. Dependence of Corrosion Rates on Inhibitor Concentrations

The relative rapidity and effectiveness of the hydrogen evolution method as well as its suitability for monitoring any in situ interruption of the inhibitors with regard to the gas evolution in metal/coordinate systems have been discussed elsewhere [4, 40].The reduction in hydrogen evolution rate for dissolution of Al metal in NaOH was found to be dependent upon the concentration of the inhibitors which decreased with increasing the inhibitors concentration (ALG and PEC) as shown in Table1 and Figures 4 and 5. On the other hand, the rate of hydrogen evolution was increased with rising the temperature in either the presence or absence of inhibitors added.Figure 4
Influence of alginates as inhibitor of corrosion of Al in alkaline media. [OH−] = 4.0 and I=4.0 mol dm−3 at 35°C. A: absence of inhibitor; B: 0.03 mol dm−3 inhibitor; C: 0.06 mol dm−3 inhibitor.Figure 5
Influence of pectates as inhibitor of corrosion of Al in alkaline media. [OH−] = 4.0 and I=4.0 mol dm−3 at 35°C. A: absence of inhibitor; B: 0.03 mol dm−3 inhibitor; C: 0.06 mol dm−3 inhibitor.In view of the above aspects and the experimental observations, a tentative corrosion mechanism based on the electrochemical processes for dissolution of Al in NaOH may be suggested. This mechanism can be illustrated by anodic (4)–(7) and cathodic (8) reactions, respectively. For the anode process,
(4)Al+OH-=Al(OH)ads+e-,(5)Al(OH)ads+OH-=Al(OH)2ads+e-,(6)Al(OH)2ads+OH-=Al(OH)3ads+e-,(7)Al(OH)3ads+OH-=Al(OH)-4ads,
and, for the cathode process,
(8)H2O+e-=H+OH-.
The overall electrochemical process is
(9)2Al+2OH-+6H2O=2Al(OH)4-+3H2.The dissolution of Al metal in the anodic reaction is accompanied by the cathodic reaction which consumes the electrons released in the anodic process in order to form hydrogen atoms which react by combining with other adsorbed hydrogen atoms to give bubbles ofH2 gas molecules at the metal surface
(10)H+H2O+e-=H2+OH-.The lesserH2 gas liberated from Al metal surface in the presence of ALG or PEC inhibitors compared to the blank solution indicates that the cited inhibitors are actually effective inhibitors for the corrosion of Al metal in alkaline media.Of course a little amount of the formed hydrogen atoms will remain without adsorption, but it does not affect the corrosion processes. So, the rate of combination and adsorption of hydrogen atoms is the same for all inhibitor levels. This fact may be confirmed by the observed identical results obtained from the gasometric and weight-loss techniques (Table1).


### 3.5. Corrosion Activation Parameters

Arrhenius suggested the famous equation that correlates the temperature variation with rate constants (Rc) [41]
(11)lnRc=lnA-Eapp≠RT.
Here, A is the frequency factor, Eapp≠ is the apparent activation energy, R is the gas constant, and T is the absolute temperature. Equation (11) predicts that plotting of lnRc versus 1/T should be linear as was experimentally observed. The slope of the line gives -Eapp≠/RT, whereas the intercept of the lines extrapolated to (-1/T=0) gives lnA.On the other hand, the changes in enthalpies (ΔH≠) and entropies (ΔS≠) of activation for the activated complexes formation in the transition states can be obtained from the transition state theory [42]
(12)-lnRhNTRc=ΔH≠RT-ΔS≠R,
where h is Planck’s constant and N is Avogadro’s number.According to (12), plots of -ln(Rh/NT)Rc versus 1/T gave good straight lines with intercepts on y axis, from whose slopes and intercepts the activation parameters ΔH≠ and ΔS≠ can be evaluated, respectively. These values were calculated using the least-squares method and are summarized in Table 3.Table 3
Activation parameters for corrosion of Al in alkaline media in absence and presence of some added inhibitors. [OH−] = 4.0 and I = 4.0 mol dm−3.
Inhibitor
[Inhibitor] mol dm−3
Parameter
Δ
H
≠ kJ mol−1
Δ
S
≠ J mol−1 K−1
Δ
G
≠ kJ mol−1
E
a
≠ kJ mol−1
A   mol−1 s−1
Alginate
0.0
58.85
+61.97
77.31
61.15
1.11
×
10
11
0.01
66.61
−30.64
75.74
69.03
4.14
×
10
11
0.03
63.60
−44.10
76.74
66.17
8.71
×
10
11
Pectates
0.0
58.85
+26.71
77.31
61.15
1.11
×
10
11
0.01
64.94
−38.45
76.40
67.51
1.72
×
10
11
0.03
61.48
−54.23
77.64
64.05
2.57
×
10
10The values of theEapp≠ for non-inhibited  solutions are higher than those of inhibited ones, indicating the inhibitive action of influence of both ALG and PEC inhibitors on the corrosion processes, by increasing the energy barriers for the corrosion processes emphasizing the electrostatic character of the inhibitors adsorption on Al surface.Again, the decrease ofEapp≠ value with increasing the inhibitor concentration (Table 3) may be attributed to the shift of the net corrosion reaction from that on the uncovered surface to one involving the adsorbed sites [43]. In fact one has to take into account the effect of the frequency factor (A). It was found that the tendency of variation in the frequency factor seemed to be quite similar to that in the appreciated activation energy. A similar phenomenon has been observed elsewhere [43, 44].


### 3.6. Adsorption Isotherms

Adsorption isotherms provide basic information on the nature of interaction between the inhibitor and the Al metal through applying some adsorption isotherm models. Two main types of interaction can describe the adsorption of inhibitors on the metal surface; they are physisorption and chemisorption, depending on the chemical structure of the inhibitor, the type of the corrosive medium, and the charge and nature of corrosive metal.In aqueous solutions, the metal surface is always covered with adsorbed water molecules. Therefore, the adsorption of inhibitor molecules from an aqueous solution is a quasisubstituted process [45], and the inhibitors that have the ability to be adsorbed strongly on the metal surface will hinder the dissolution reaction of the immersed metal into the corrosive medium. The mechanism of corrosion inhibition can be explained in terms of the adsorption behavior based on the calculated surface coverage degrees.Generally, several adsorption isotherms such as Langmuir, Freundlich, Temkin, Frukmin, and El-Wady et al. isotherm models were postulated for graphical fitting of these calculated surface coverage values [46, 47]. Here, the degree of surface coverage (θ) for different inhibitor concentrations was calculated from the gas evolution data using the relationship
(13)θ=1-Rc°Rc’.The correlation coefficient(R2) can be used to determine the best fit isotherm. By far, the best fit model for the present experimental data was fitted with applying Langmuir adsorption isotherm
(14)Cθ=1Kads+C,
where θ is the surface coverage, C is the inhibitor concentration, and Kads is the equilibrium constant of adsorption.The value ofKads is related to the standard free-energy of adsorption ΔGads° by the following equation [48]:
(15)lnKads=-lnCH2O-ΔGads°RT
or
(16)ΔGads°=-RT(55.5Kads),
where CH2O is the molar concentration of water expressed in mol dm−3 (the same as that of inhibitor concentration).As shown in Figure6, plotting of C/θ against [C] was fairly linear for all inhibitors concentrations and different temperatures. The slopes were found to be approximately unity in all cases as suggested by Langmuir adsorption isotherm (R2>0.99). Also, it was surprising when the results obtained were also found to verify the thermodynamic model of Freundlich isotherm as is shown in Figure 7(17)logθ=logKads+nlogC.Figure 6
A plot of Langmuir isotherm for corrosion of Al in alkaline media at 35°C.Figure 7
A plot of Freundlich isotherm for corrosion of Al in alkaline media at 35°C.The kinetic parameters for adsorption were calculated by the least-squares method and are summarized in Tables4, 5, and 6. The values of Kads were found to increase with increasing the temperature indicating that the adsorption processes are endothermic in nature. This trend may also indicate that the inhibitor molecules are physically adsorbed on Al metal surface. Again, the negative values observed of ΔGads° (Tables 4 and 6) are consistent with the spontaneity for the adsorption processes and stability of the adsorbed layer on Al metal surface; that is, it may confirm the existence of a physical adsorption mechanism. In view of the correlation coefficients (R2), Langmuir isotherm model is the more favorable one to fit the experimental data of the present investigation.Table 4
Some kinetic parameters from Langmuir isotherm model for corrosion of Al in alkaline media. [OH−] = 4.0 and I = 4.0 mol dm−3.
Inhibitor
Temp. (°C)
Δ
G
ads
° (kJ mol−1)
Slope (n)
K
ads (dm3 mol−1)
R
2
Alginate
30
−19.66
1.004
50.38
>0.99
35
−20.74
1.032
67.80
>0.99
45
−21.83
1.094
90.91
>0.99
Pectates
30
−21.31
1.042
98.04
>0.99
35
−22.03
1.006
112.99
>0.99
45
−23.10
0.984
129.03
>0.99Table 5
Thermodynamic parameters ofΔHads° and ΔSads° for corrosion of Al  in alkaline media in the absence and presence of ALG and PEC inhibitors. [OH−] = 4.0 and I = 4.0 mol dm−3.
Inhibitor
Parameters
Δ
H
ads
° (kJ mol−1)
Δ
S
ads
° (J mol−1 K−1)
R
2
Alginate
45.05
217.15
>0.99
Pectates
20.98
141.91
>0.99Table 6
Some kinetic parameters from Freundlich isotherm model for corrosion of Al in alkaline media. [OH−] = 4.0 and I = 4.0 mol dm−3.
Inhibitor
Temp. (°C)
Δ
G
ads
° kJ mol−1
Slope (n)
K
ads dm3 mol−1
R
2
Alginate
30
−7.38
0.45
0.36
~0.99
35
−7.87
0.38
0.41
~0.99
45
−8.57
0.30
0.51
~0.98
Pectates
30
−8.15
0.31
0.48
~0.99
35
−8.45
0.27
0.52
~0.99
45
−8.79
0.25
0.53
~0.98Generally, the adsorption can be described by two main types, namely, chemisorptions [49] and physisorption [50], respectively. Physisorption involves electrostatic interaction between ionic charges or dipoles on the adsorbed species and the electric charge at the metal/solution surface, while chemisorption involves charge sharing or charge transfer process from the inhibitor molecules to the metal surface in order to form a sort of covalent or coordinate bonds.It has been accepted that the values ofΔGads° up to ~−20 kJ mol−1 are corresponding to the physisorption in which the inhibition action is due to the electrostatic interaction between the charged molecules and the charged metal. On the other hand, the values which lie around −40 kJ mol−1 or smaller are corresponding to chemisorption process and are attributed to the charge sharing or transfer processes from the inhibitor molecules to the metal surface in order to form a sort of covalent or coordinate bonds [51, 52]. Therefore, the thermodynamic parameters obtained can be considered as a useful tool for clarifying the adsorption behavior of the inhibitor used [53].


## 3.1. Hydrogen Evolution and Weight-Loss Measurements

The volume of the evolved H2 gas (or the loss in Al weight) as a function of time may be taken as the rate of dissolution of aluminum in sodium hydroxide and can be expressed, respectively, by
(1)Rc=VH2L·t,(2)Rc=ΔWL·t,
where Rc is the corrosion rate, L is the surface area of Al metal sheet (cm2), t is the immersion period (min), VH2 is volume of evolved hydrogen gas (mL), and ΔW is the weight-loss (mg) of Al metal dissolved into the corrosive medium. Typical plots of the gasometric and weight-loss data are shown in Figures 1 and 2, respectively. These plots revealed that the volume of H2 evolved or the loss in weight is varied linearly with the immersion times. The rate of corrosion (Rc) can be obtained from the slopes of the linear portions of such plots which corresponds to the rate constants of dissolution of Al in alkaline media obtained from either evolved hydrogen or the weight-loss methods. These values were calculated by the least-squares method and are summarized in Table 1.Table 1
The corrosion rates (Rc) for corrosion of Al in alkaline media in absence and presence of inhibitors. [OH−] = 4.0 and I = 4.0 mol dm−3 at  30°C.
[Inhibitor]mol dm−3
0.0
0.01
0.02
0.03
0.04
Alginate
0.52 (0.48)*
0.33
0.28
0.22
0.16
Pectates
0.52 (0.48)*
0.25
0.20
0.15
0.11
*Calculated from the weight-loss method.Figure 1
A typical plot of the evolvedVH2 versus time for corrosion of Al in alkaline media in absence of inhibitors at 30°C. [OH−] = 4.0 mol dm−3.Figure 2
A typical plot of the weight-loss versus time for corrosion of Al in alkaline media in absence of inhibitors at 30°C. [OH−] = 4.0 mol dm−3.


## 3.2. Inhibition Efficiency (% I.E.)

The inhibition efficiencies of the added inhibitors were calculated using the following relationship:(3)%I.E.=Rc°-Rc’Rc°×100,
where Rc° and Rc’ are the corrosion rates of Al metal in absence and presence of such natural polymeric inhibitors, respectively. The results are summarized in Table 2. The values of inhibition efficiency (% I.E.) listed in Table 2 were found to follow the same trend, which increases with increasing the inhibitors concentration and decreases with rising the temperature.Table 2
Percentage of inhibitor efficiency (% I.E.) for corrosion of Al in alkaline media in presence of inhibitors.[OH−] = 4.0 and I = 4.0 mol dm−3 at 30°C.
[Inhibitor] mol dm−3
0.01
0.02
0.03
0.04
Alginate
36.54
46.15
57.69
69.23
Pectates
51.92
61.54
71.15
78.85


## 3.3. Dependence of Corrosion Rates on [OH−]

In order to examine the corrosion rates as a function of alkali concentration, some experimental runs were performed at various initial concentrations of the alkali and constants of all other reagents. Plots ofVH2 gas versus time (evolved active H2) were found to be linear in which the rate constants increased with increasing the [OH−] as shown in Figure 3. This result means that the corrosion rate is a function of the alkali concentration.Figure 3
Plots of evolvedVH2 versus time for corrosion of Al in alkaline media in absence of inhibitors at 30°C. [OH−]: (A)=2.0; (B)=3.0; (C)=4.0 mol dm−3.


## 3.4. Dependence of Corrosion Rates on Inhibitor Concentrations

The relative rapidity and effectiveness of the hydrogen evolution method as well as its suitability for monitoring any in situ interruption of the inhibitors with regard to the gas evolution in metal/coordinate systems have been discussed elsewhere [4, 40].The reduction in hydrogen evolution rate for dissolution of Al metal in NaOH was found to be dependent upon the concentration of the inhibitors which decreased with increasing the inhibitors concentration (ALG and PEC) as shown in Table1 and Figures 4 and 5. On the other hand, the rate of hydrogen evolution was increased with rising the temperature in either the presence or absence of inhibitors added.Figure 4
Influence of alginates as inhibitor of corrosion of Al in alkaline media. [OH−] = 4.0 and I=4.0 mol dm−3 at 35°C. A: absence of inhibitor; B: 0.03 mol dm−3 inhibitor; C: 0.06 mol dm−3 inhibitor.Figure 5
Influence of pectates as inhibitor of corrosion of Al in alkaline media. [OH−] = 4.0 and I=4.0 mol dm−3 at 35°C. A: absence of inhibitor; B: 0.03 mol dm−3 inhibitor; C: 0.06 mol dm−3 inhibitor.In view of the above aspects and the experimental observations, a tentative corrosion mechanism based on the electrochemical processes for dissolution of Al in NaOH may be suggested. This mechanism can be illustrated by anodic (4)–(7) and cathodic (8) reactions, respectively. For the anode process,
(4)Al+OH-=Al(OH)ads+e-,(5)Al(OH)ads+OH-=Al(OH)2ads+e-,(6)Al(OH)2ads+OH-=Al(OH)3ads+e-,(7)Al(OH)3ads+OH-=Al(OH)-4ads,
and, for the cathode process,
(8)H2O+e-=H+OH-.
The overall electrochemical process is
(9)2Al+2OH-+6H2O=2Al(OH)4-+3H2.The dissolution of Al metal in the anodic reaction is accompanied by the cathodic reaction which consumes the electrons released in the anodic process in order to form hydrogen atoms which react by combining with other adsorbed hydrogen atoms to give bubbles ofH2 gas molecules at the metal surface
(10)H+H2O+e-=H2+OH-.The lesserH2 gas liberated from Al metal surface in the presence of ALG or PEC inhibitors compared to the blank solution indicates that the cited inhibitors are actually effective inhibitors for the corrosion of Al metal in alkaline media.Of course a little amount of the formed hydrogen atoms will remain without adsorption, but it does not affect the corrosion processes. So, the rate of combination and adsorption of hydrogen atoms is the same for all inhibitor levels. This fact may be confirmed by the observed identical results obtained from the gasometric and weight-loss techniques (Table1).


## 3.5. Corrosion Activation Parameters

Arrhenius suggested the famous equation that correlates the temperature variation with rate constants (Rc) [41]
(11)lnRc=lnA-Eapp≠RT.
Here, A is the frequency factor, Eapp≠ is the apparent activation energy, R is the gas constant, and T is the absolute temperature. Equation (11) predicts that plotting of lnRc versus 1/T should be linear as was experimentally observed. The slope of the line gives -Eapp≠/RT, whereas the intercept of the lines extrapolated to (-1/T=0) gives lnA.On the other hand, the changes in enthalpies (ΔH≠) and entropies (ΔS≠) of activation for the activated complexes formation in the transition states can be obtained from the transition state theory [42]
(12)-lnRhNTRc=ΔH≠RT-ΔS≠R,
where h is Planck’s constant and N is Avogadro’s number.According to (12), plots of -ln(Rh/NT)Rc versus 1/T gave good straight lines with intercepts on y axis, from whose slopes and intercepts the activation parameters ΔH≠ and ΔS≠ can be evaluated, respectively. These values were calculated using the least-squares method and are summarized in Table 3.Table 3
Activation parameters for corrosion of Al in alkaline media in absence and presence of some added inhibitors. [OH−] = 4.0 and I = 4.0 mol dm−3.
Inhibitor
[Inhibitor] mol dm−3
Parameter
Δ
H
≠ kJ mol−1
Δ
S
≠ J mol−1 K−1
Δ
G
≠ kJ mol−1
E
a
≠ kJ mol−1
A   mol−1 s−1
Alginate
0.0
58.85
+61.97
77.31
61.15
1.11
×
10
11
0.01
66.61
−30.64
75.74
69.03
4.14
×
10
11
0.03
63.60
−44.10
76.74
66.17
8.71
×
10
11
Pectates
0.0
58.85
+26.71
77.31
61.15
1.11
×
10
11
0.01
64.94
−38.45
76.40
67.51
1.72
×
10
11
0.03
61.48
−54.23
77.64
64.05
2.57
×
10
10The values of theEapp≠ for non-inhibited  solutions are higher than those of inhibited ones, indicating the inhibitive action of influence of both ALG and PEC inhibitors on the corrosion processes, by increasing the energy barriers for the corrosion processes emphasizing the electrostatic character of the inhibitors adsorption on Al surface.Again, the decrease ofEapp≠ value with increasing the inhibitor concentration (Table 3) may be attributed to the shift of the net corrosion reaction from that on the uncovered surface to one involving the adsorbed sites [43]. In fact one has to take into account the effect of the frequency factor (A). It was found that the tendency of variation in the frequency factor seemed to be quite similar to that in the appreciated activation energy. A similar phenomenon has been observed elsewhere [43, 44].


## 3.6. Adsorption Isotherms

Adsorption isotherms provide basic information on the nature of interaction between the inhibitor and the Al metal through applying some adsorption isotherm models. Two main types of interaction can describe the adsorption of inhibitors on the metal surface; they are physisorption and chemisorption, depending on the chemical structure of the inhibitor, the type of the corrosive medium, and the charge and nature of corrosive metal.In aqueous solutions, the metal surface is always covered with adsorbed water molecules. Therefore, the adsorption of inhibitor molecules from an aqueous solution is a quasisubstituted process [45], and the inhibitors that have the ability to be adsorbed strongly on the metal surface will hinder the dissolution reaction of the immersed metal into the corrosive medium. The mechanism of corrosion inhibition can be explained in terms of the adsorption behavior based on the calculated surface coverage degrees.Generally, several adsorption isotherms such as Langmuir, Freundlich, Temkin, Frukmin, and El-Wady et al. isotherm models were postulated for graphical fitting of these calculated surface coverage values [46, 47]. Here, the degree of surface coverage (θ) for different inhibitor concentrations was calculated from the gas evolution data using the relationship
(13)θ=1-Rc°Rc’.The correlation coefficient(R2) can be used to determine the best fit isotherm. By far, the best fit model for the present experimental data was fitted with applying Langmuir adsorption isotherm
(14)Cθ=1Kads+C,
where θ is the surface coverage, C is the inhibitor concentration, and Kads is the equilibrium constant of adsorption.The value ofKads is related to the standard free-energy of adsorption ΔGads° by the following equation [48]:
(15)lnKads=-lnCH2O-ΔGads°RT
or
(16)ΔGads°=-RT(55.5Kads),
where CH2O is the molar concentration of water expressed in mol dm−3 (the same as that of inhibitor concentration).As shown in Figure6, plotting of C/θ against [C] was fairly linear for all inhibitors concentrations and different temperatures. The slopes were found to be approximately unity in all cases as suggested by Langmuir adsorption isotherm (R2>0.99). Also, it was surprising when the results obtained were also found to verify the thermodynamic model of Freundlich isotherm as is shown in Figure 7(17)logθ=logKads+nlogC.Figure 6
A plot of Langmuir isotherm for corrosion of Al in alkaline media at 35°C.Figure 7
A plot of Freundlich isotherm for corrosion of Al in alkaline media at 35°C.The kinetic parameters for adsorption were calculated by the least-squares method and are summarized in Tables4, 5, and 6. The values of Kads were found to increase with increasing the temperature indicating that the adsorption processes are endothermic in nature. This trend may also indicate that the inhibitor molecules are physically adsorbed on Al metal surface. Again, the negative values observed of ΔGads° (Tables 4 and 6) are consistent with the spontaneity for the adsorption processes and stability of the adsorbed layer on Al metal surface; that is, it may confirm the existence of a physical adsorption mechanism. In view of the correlation coefficients (R2), Langmuir isotherm model is the more favorable one to fit the experimental data of the present investigation.Table 4
Some kinetic parameters from Langmuir isotherm model for corrosion of Al in alkaline media. [OH−] = 4.0 and I = 4.0 mol dm−3.
Inhibitor
Temp. (°C)
Δ
G
ads
° (kJ mol−1)
Slope (n)
K
ads (dm3 mol−1)
R
2
Alginate
30
−19.66
1.004
50.38
>0.99
35
−20.74
1.032
67.80
>0.99
45
−21.83
1.094
90.91
>0.99
Pectates
30
−21.31
1.042
98.04
>0.99
35
−22.03
1.006
112.99
>0.99
45
−23.10
0.984
129.03
>0.99Table 5
Thermodynamic parameters ofΔHads° and ΔSads° for corrosion of Al  in alkaline media in the absence and presence of ALG and PEC inhibitors. [OH−] = 4.0 and I = 4.0 mol dm−3.
Inhibitor
Parameters
Δ
H
ads
° (kJ mol−1)
Δ
S
ads
° (J mol−1 K−1)
R
2
Alginate
45.05
217.15
>0.99
Pectates
20.98
141.91
>0.99Table 6
Some kinetic parameters from Freundlich isotherm model for corrosion of Al in alkaline media. [OH−] = 4.0 and I = 4.0 mol dm−3.
Inhibitor
Temp. (°C)
Δ
G
ads
° kJ mol−1
Slope (n)
K
ads dm3 mol−1
R
2
Alginate
30
−7.38
0.45
0.36
~0.99
35
−7.87
0.38
0.41
~0.99
45
−8.57
0.30
0.51
~0.98
Pectates
30
−8.15
0.31
0.48
~0.99
35
−8.45
0.27
0.52
~0.99
45
−8.79
0.25
0.53
~0.98Generally, the adsorption can be described by two main types, namely, chemisorptions [49] and physisorption [50], respectively. Physisorption involves electrostatic interaction between ionic charges or dipoles on the adsorbed species and the electric charge at the metal/solution surface, while chemisorption involves charge sharing or charge transfer process from the inhibitor molecules to the metal surface in order to form a sort of covalent or coordinate bonds.It has been accepted that the values ofΔGads° up to ~−20 kJ mol−1 are corresponding to the physisorption in which the inhibition action is due to the electrostatic interaction between the charged molecules and the charged metal. On the other hand, the values which lie around −40 kJ mol−1 or smaller are corresponding to chemisorption process and are attributed to the charge sharing or transfer processes from the inhibitor molecules to the metal surface in order to form a sort of covalent or coordinate bonds [51, 52]. Therefore, the thermodynamic parameters obtained can be considered as a useful tool for clarifying the adsorption behavior of the inhibitor used [53].



---

*Source: 508596-2013-11-17.xml*