# Synergistic Effect of KI on Corrosion Inhibition of Mild Steel by Polynuclear Schiff Base in Sulphuric Acid

Authors: K. S. Shaju; K. Joby Thomas; Vinod P. Raphael; Aby Paul
Journal: ISRN Corrosion
 (2012)

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## Abstract

Synergistic effect of KI on the corrosion inhibition efficiency of polynuclear Schiff base, anthracene-9(10H)-one-3-aminopropanoic acid (A9O3AP), on mild steel (MS) in 0.5 M sulphuric acid solution has been investigated using weight loss measurements, electrochemical impedance spectroscopy (EIS), and potentiodynamic polarization studies. The results show that inhibition efficiencies on MS increase with increase in concentration of the inhibitor and enhancement in inhibition efficiency was observed on addition of potassium iodide due to synergism. The adsorptions, of inhibitor and inhibitor + KI on the surfaces of the corroding metal obey Freundlich and Langmuir isotherms, respectively. Polarization studies revealed that A9O3AP acts as a mixed type inhibitor. Thermodynamic parameters (Kads; ΔGads0) were calculated using the adsorption isotherms. A probable synergismtic mechanism is proposed.


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## Body

## 1. Introduction

The use of certain organic compounds as inhibitors is the most practical method to prevent corrosion of the mild steel (MS) in acidic media [1, 2]. Compounds with π-bonds generally exhibit good inhibitive properties due to interaction of π-orbital with the metal surface [3]. Schiff bases are organic molecules possessing azomethine linkage and many of them act as effective potential corrosion inhibitors [4–7]. The addition of halide ions to sulphuric acid solutions containing organic inhibitors has been found to stabilize the adsorption of organic cations, leading to improved inhibition efficiency. The synergistic effect of the halides have been observed to increase in the order Cl-< Br-< I-. Due to large size and ease of polarizability, iodide (I-) shows the highest synergistic effect [8–11].The present investigation was undertaken to examine the corrosion inhibition behavior and synergism mechanism [12, 13] with I- of a novel polynuclear Schiff base (A9O3AP) derived from anthracene-9 (10H)-one and 3-aminopropanoic acid in 0.5 M H2SO4 solution on MS at 303 K.


## 2. Experimental

### 2.1. Inhibitor

Polynuclear Schiff base (A9O3AP) was obtained by the condensation of equimolar mixture of anthracene-9(10H)-one and 3-aminopropanoic acid in ethanol. The reaction mixture was refluxed for 5 hours, cooled by keeping overnight to obtain yellow coloured compound, filtered, washed, and dried. Figure1 shows the molecular structure of polynuclear Schiff base A9O3AP. Anal.calcd for C17H15NO2: C, 76.88; H, 5.65; N, 5.28%. Found. C, 75.96; H, 6.13; N, 4.95%; m.p. = 240°C; IR (KBr): νC=N=1559 cm−1, νCOOH=3067 cm−1. 1Hnmr: δCOOH 12.19, 13Cnmr: δCOOH=169.93,δC=N=150.8 ppm.Figure 1
Molecular structure of A9O3AP.


### 2.2. Solutions

The aggressive solution of 0.5 M H2SO4 was prepared by the dilution of A.R grade 98% of H2SO4 (Merck) with deionized water. Inhibitor solutions were prepared in the range, 0.2 mM–1 mM concentrations.


### 2.3. Weight Loss Measurements

Mild steel specimens of dimension1.5×2×0.1 cm (composition: C, 0.5%; Mn, 0.07%; P,0.02%; S, 0.015%; Si, 0.02%, and rest Fe) were cut and abraded with various grades of silicon carbide papers (200, 400, 600, 800, 1000, 1200, and 2000). The exact area and thickness of each coupon were measured and washed with soap water. Specimens were then degreased again with acetone and finally dried. After weighing, specimens were immersed in 50 mL acid solutions (naturally aerated) at 30°C in the absence and presence of the inhibitor (A9O3AP) and I- using hooks and fishing lines. Weight loss of metal specimens was noted after 24 h. The corrosion rate (ν) and the percentage of inhibition efficiency (ηw%) were calculated by the following equations [14–16]:
(1)ν=WSt,ηw%=ν0-νν0×100,
where W is the weight loss (g) of coupon, S is the total area (cm2) of specimens, t is the time of treatment (24 hrs), ν0 and ν are the corrosion rates of uninhibited and inhibited specimens, respectively.


### 2.4. Electrochemical Impedance Spectroscopy (EIS)

The EIS measurements were performed in a three electrode assembly. Saturated calomel electrode (SCE) was used as the reference electrode. Platinum electrode having 1 cm2 area was taken as counter electrode. Metal specimens with an exposed area of 1 cm2 were used as the working electrode. The EIS experiments were carried out on an Ivium compactstat-e electrochemical system. 0.5 M H2SO4 (no deaeration, no stirring) was taken as the electrolyte and the working area of the metal specimens were exposed to the electrolyte for 1 h prior to the measurement. EIS measurements were performed at constant potential (OCP) in the frequency range from 1 KHz to 100 mHz with amplitude of 10 mV as excitation signal. The percentage of inhibitions from impedance measurements were calculated using charge transfer resistance values by the following expression [17]:
(2)ηEIS%=Rct-Rct′Rct×100,
where Rct and Rct′ are the charge transfer resistances of working electrode with and without inhibitor, respectively.


### 2.5. Potentiodynamic Polarization

Electrochemical polarization studies of MS specimens in 0.5 M H2SO4 with and without inhibitor and KI were performed by recording anodic and cathodic potentiodynamic polarization curves. Polarization plots were obtained in the electrode potential range from −100 to +100 mV Vs equilibrium potential at a scan rate of 1 mV/sec. Tafel polarization analyses were done by extrapolating anodic and cathodic curves to obtain corrosion current densities (Icorr). The percentage of inhibition efficiency (ηpol%) was evaluated from the measured Icorr values using the following relation [18]:
(3)ηpol%=Icorr-Icorr′Icorr×100,
where Icorr and Icorr′ are the corrosion current densities of the exposed area of the working electrode in the absence and presence of inhibitor.


## 2.1. Inhibitor

Polynuclear Schiff base (A9O3AP) was obtained by the condensation of equimolar mixture of anthracene-9(10H)-one and 3-aminopropanoic acid in ethanol. The reaction mixture was refluxed for 5 hours, cooled by keeping overnight to obtain yellow coloured compound, filtered, washed, and dried. Figure1 shows the molecular structure of polynuclear Schiff base A9O3AP. Anal.calcd for C17H15NO2: C, 76.88; H, 5.65; N, 5.28%. Found. C, 75.96; H, 6.13; N, 4.95%; m.p. = 240°C; IR (KBr): νC=N=1559 cm−1, νCOOH=3067 cm−1. 1Hnmr: δCOOH 12.19, 13Cnmr: δCOOH=169.93,δC=N=150.8 ppm.Figure 1
Molecular structure of A9O3AP.


## 2.2. Solutions

The aggressive solution of 0.5 M H2SO4 was prepared by the dilution of A.R grade 98% of H2SO4 (Merck) with deionized water. Inhibitor solutions were prepared in the range, 0.2 mM–1 mM concentrations.


## 2.3. Weight Loss Measurements

Mild steel specimens of dimension1.5×2×0.1 cm (composition: C, 0.5%; Mn, 0.07%; P,0.02%; S, 0.015%; Si, 0.02%, and rest Fe) were cut and abraded with various grades of silicon carbide papers (200, 400, 600, 800, 1000, 1200, and 2000). The exact area and thickness of each coupon were measured and washed with soap water. Specimens were then degreased again with acetone and finally dried. After weighing, specimens were immersed in 50 mL acid solutions (naturally aerated) at 30°C in the absence and presence of the inhibitor (A9O3AP) and I- using hooks and fishing lines. Weight loss of metal specimens was noted after 24 h. The corrosion rate (ν) and the percentage of inhibition efficiency (ηw%) were calculated by the following equations [14–16]:
(1)ν=WSt,ηw%=ν0-νν0×100,
where W is the weight loss (g) of coupon, S is the total area (cm2) of specimens, t is the time of treatment (24 hrs), ν0 and ν are the corrosion rates of uninhibited and inhibited specimens, respectively.


## 2.4. Electrochemical Impedance Spectroscopy (EIS)

The EIS measurements were performed in a three electrode assembly. Saturated calomel electrode (SCE) was used as the reference electrode. Platinum electrode having 1 cm2 area was taken as counter electrode. Metal specimens with an exposed area of 1 cm2 were used as the working electrode. The EIS experiments were carried out on an Ivium compactstat-e electrochemical system. 0.5 M H2SO4 (no deaeration, no stirring) was taken as the electrolyte and the working area of the metal specimens were exposed to the electrolyte for 1 h prior to the measurement. EIS measurements were performed at constant potential (OCP) in the frequency range from 1 KHz to 100 mHz with amplitude of 10 mV as excitation signal. The percentage of inhibitions from impedance measurements were calculated using charge transfer resistance values by the following expression [17]:
(2)ηEIS%=Rct-Rct′Rct×100,
where Rct and Rct′ are the charge transfer resistances of working electrode with and without inhibitor, respectively.


## 2.5. Potentiodynamic Polarization

Electrochemical polarization studies of MS specimens in 0.5 M H2SO4 with and without inhibitor and KI were performed by recording anodic and cathodic potentiodynamic polarization curves. Polarization plots were obtained in the electrode potential range from −100 to +100 mV Vs equilibrium potential at a scan rate of 1 mV/sec. Tafel polarization analyses were done by extrapolating anodic and cathodic curves to obtain corrosion current densities (Icorr). The percentage of inhibition efficiency (ηpol%) was evaluated from the measured Icorr values using the following relation [18]:
(3)ηpol%=Icorr-Icorr′Icorr×100,
where Icorr and Icorr′ are the corrosion current densities of the exposed area of the working electrode in the absence and presence of inhibitor.


## 3. Results and Discussion

### 3.1. Weight Loss Measurements

Weight loss of MS specimens in 0.5 M H2SO4 at 30°C was determined at 24 h in the presence of various concentrations of inhibitor (A9O3AP) and inhibitor + KI. The corrosion rates, inhibition efficiencies, and surface coverage (θ) in the presence of inhibitor and inhibitor + 0.2 mM KI for MS specimens for the period of 24 h are shown in the Table 1.Table 1
Calculated values of inhibition efficiency (ηW%) for MS corrosion in 0.5 M H2SO4 for different systems at 30°C from weight loss measurements.
Systems/concentrations
Corrosion rate(mm/y)
Inhibition efficiency(ηW %)
θ
Blank
24.01
—
—
Blank + 0.2 mM KI
19.40
19.16
0.19
0.2 mM A9O3AP
18.06
24.77
0.25
0.4 mM A9O3AP
17.19
28.38
0.28
0.6 mM A9O3AP
15.96
33.54
0.34
0.8 mM A9O3AP
14.58
39.25
0.39
1.0 mM A9O3AP
13.50
43.75
0.44
0.2 mM A9O3AP + 0.2 mM KI
10.88
54.67
0.55
0.4 mM A9O3AP + 0.2 mM KI
10.22
57.41
0.57
0.6 mM A9O3AP + 0.2 mM KI
9.08
62.16
0.62
0.8 mM A9O3AP + 0.2 mM KI
6.84
71.49
0.71
1.0 mM A9O3AP + 0.2 mM KI
5.58
76.75
0.77From Table1, it is clear that the corrosion rate markedly decreased with inhibitor concentration from 0 to 0.2 mM. Beyond this concentration, corrosion rate showed a gradual decrease. This response is due to the fact that the surface coverage (θ) of the inhibitor molecules on the metal through adsorption increases with increase in concentration. The inhibitor + KI system showed similar trend. From Table 1 it is also evident that the inhibition efficiency increased with increase in concentration. At the inhibitor concentration of 1.0 mM, the maximum ηW% was 43.75, which shows that individual inhibitor cannot protect much effectively the corrosion of MS in H2SO4. Table 1 also shows the values of ηW% for a constant KI concentration (0.2 mM) and changing inhibitor concentration in 0.5 M H2SO4 solution. Compared with the inhibition efficiency values of inhibitor (without KI), it was found that the combination of inhibitor and 0.2 mM KI has better inhibition efficiency for all studied inhibitor concentrations.


### 3.2. Comparison of Inhibition Efficiency of Schiff Base with Its Parent Amine

To compare the inhibition efficiencies of Schiff base and parent amine (3-aminopropanoic acid), weight loss measurements of MS specimens were performed in 0.5 M H2SO4 at 30°C. The percentage of corrosion inhibition efficiencies obtained for Schiff base and parent amine on MS are represented in the Figure 2. The inhibition efficiency of the Schiff base A9O3AP was markedly higher than that of 3-aminopropanoic acid for the studied concentrations. This investigation clearly establishes the role of azomethine linkage (C = N) present in the Schiff base which actively participate in the corrosion inhibition mechanism.Figure 2
Comparison of inhibition efficiency of Schiff base and parent amine in 0.5 M H2SO4 at 24 h.


### 3.3. Adsorption Isotherm and Free Energy of Adsorption

The mechanism of adsorption and the surface behavior of organic molecules can be easily viewed through adsorption isotherms. Different models of adsorption isotherms considered are Langmiur, Temkin, Frumkin, and Freundlich isotherms. For the evaluation of thermodynamic parameters it is necessary to determine the best fit isotherm with the aid of correlation coefficient (R2). Among the isotherms mentioned above, the best description of the adsorption behavior of A9O3AP and A9O3AP + KI on MS specimens in 0.5 M H2SO4 was Freundlich and Langmiur adsorption isotherms, respectively. These models are expressed as [19]Freundlich adsorption isotherm:(4)θ=KadsC,Langmiur adsorption isotherm:(5)Cθ=1Kads+C,where C is the concentration of the inhibitor, θ is the fractional surface coverage and Kads is the adsorption equilibrium constant. Figures 3 and 4 represent the adsorption plots of A9O3AP and A9O3AP + KI obtained by the weight loss measurements of MS steel specimens in 0.5 M H2SO4 at 30°C for 24 h, respectively.Figure 3
Freundlich adsorption isotherm for adsorption of A9O3AP on MS surface in 0.5 M H2SO4 at 30°C for 24 h.Figure 4
Langmuir adsorption isotherm for adsorption of A9O3AP + KI on MS surface in 0.5 M H2SO4 at 30°C for 24 h.The adsorption equilibrium constantKads is related to the standard free energy of adsorption ΔGads0, by
(6)ΔGads0=-RTln(55.5Kads),
where 55.5 is the molar concentration of water, R is the universal gas constant, and T is the temperature in Kelvin [20]. Table 2 explores thermodynamic parameters obtained from weight loss measurements of MS in 0.5 M H2SO4 at 30∘C for 24 h. ΔGads0 for A9O3AP and A9O3AP + KI on MS showed negative values indicating the spontaneity of the process. The value of ΔGads0 upto −20 kJ mol−1 is an indication of the electrostatic interaction of the charged molecule and the charged surface of the metal (physisorption) while ΔGads0 is more negative than −40 kJ implies that inhibitor molecules are adsorbed strongly on the metal surface through coordinate type bond (chemisorption) [21, 22]. In the present investigation, A9O3AP and A9O3AP + KI molecules showed ΔGads0 −23.9 and −27.1, respectively, for MS specimens suggesting that the adsorption of inhibitor involves both electrostatic and chemical interactions.Table 2
Thermodynamic parameters obtained from weight loss studies.
MS in
Isotherm
K
ads
Δ
G
ads
0 (kJ/mol)
A9O3AP
Freundlich
244
−23.9
A9O3AP + KI
Langmiur
871
−27.1


### 3.4. Synergistic Effect

The addition of KI drastically increases theηW% values; for instance, ηW% of individual 0.2 mM is 19.16%. From Table 1 it is clear that ηW% for KI in combination with inhibitor is higher than the summation of ηW% for single KI and single inhibitor, which is synergistic in nature. Aramaki and Hackerman [23] calculated the synergism parameter Sθ using the following equation:
(7)Sθ=1-θ1+21-θ1+2′,
where θ1+2=(θ1+θ2)-(θ1θ2); θ1 = surface coverage by anion; θ2 = surface coverage by cation; θ1+2′=  measured surface coverage by both anion and cation. Sθ approaches unity when there are no interactions between the inhibitor compounds, while Sθ > 1 points to a synergistic effect; in the case of Sθ<1, the antagonistic interaction prevails. The values of the synergism parameter for the various concentrations of A9O3AP studied from the gravimetric analysis are presented in Table 3.Table 3
Synergism parameter (Sθ) for different concentrations of inhibitor in combination with 0.2 mM KI.
Concentration
Synergism parameter,Sθ
0.2 mM
1.34
0.4 mM
1.36
0.6 mM
1.42
0.8 mM
1.73
1.0 mM
1.96All values shown in this table are greater than unity. This is an indication that the enhanced inhibition efficiency resulting from the addition of iodide ions to A9O3AP is synergistic in nature [24].


### 3.5. EIS Measurements

The corrosion response of MS in 0.5 M H2SO4 in the presence of various concentrations of inhibitor and inhibitor + KI systems has been investigated using Electrochemical Impedance Spectroscopy at 30∘C. Figures 5 and 6 represent the Nyquist plots of MS specimens in 0.5 M H2SO4 in the presence of various concentrations of inhibitor and inhibitor + KI, respectively. It is evident from the plots that the impedance response of metal specimens has marked difference in the presence and absence of the KI with inhibitor A9O3AP.Figure 5
Nyquist plots for MS specimens in  0.5 M H2SO4.Figure 6
Nyquist plots (synergistic effect) for MS specimens in 0.5 M H2SO4.Impedance behaviour can be well explained by pure electric models that could verify and enable to calculate numerical values corresponding to the physical and chemical properties of electrochemical system under examination [25]. The simple equivalent circuit that fit to many electrochemical systems composed of a double layer capacitance, Rs and Rct [26, 27]. To reduce the effects due to surface irregularities of metal, constant phase element (CPE) is introduced into the circuit instead of a pure double layer capacitance which gives more accurate fit as shown in the Figure 7 [28].Figure 7
Equivalent circuit fitting for EIS measurements.The impedance of CPE can be expressed as(8)ZCPE=1Y0(jω)n,
where Y0 is the magnitude of CPE, n is the exponent (phase shift), ω is the angular frequency, and j is the imaginary unit. CPE may be resistance, capacitance, and inductance depending upon the values of n [29]. In all experiments the observed value of n ranges between 0.75 and 1.0, suggesting the capacitive response of CPE. The EIS parameters such as Rct, Rs, and CPE and the calculated values of percentage of inhibition (ηEIS%) of MS specimens are listed in Tables 4(a) and 4(b) respectively.Table 4
Electrochemical Impedance parameters of MS specimens in 0.5 M H2SO4 at 30°C in the absence and presence of inhibitor (a) and inhibitor + 0.2 mM KI (b).
(a)
C (mM)
R
ct (Ω·cm2)
C
dl (μF cm−2)
η
EIS
%
0
8.9
135
—
0.2
10.9
103
18.35
0.4
17.7
95.1
49.72
0.6
21.1
94
57.82
0.8
28.8
87
69.10
1.0
38.6
75.8
76.94
(b)
C (mM)
R
ct (Ω·cm2)
C
dl (μF cm−2)
η
EIS
%
0
8.9
135
—
0.2 + KI
91
99.9
90.22
0.4 + KI
102
93.7
91.27
0.6 + KI
151
91.3
94.11
0.8 + KI
198
79.7
95.51
1.0 + KI
251
65.1
96.45From Tables4(a) and 4(b) it is clear that Rct values are increased with increasing inhibitor concentration. The capacitance values Cdl decreases with inhibitor concentration and this decrease in Cdl is enhanced upon addition of I− ions to the corrosive environment (inspect data listed in Tables 4(a) and 4(b)). These results suggest that the A9O3AP molecules function by adsorption at the metal/solution interface [30] and this adsorption is reinforced by I− ions. This decrease in Cdl may be explained on the basis that the double layer between the charged metal surface and the solution is considered as an electrical capacitor. The ηEIS% data reveal that the corrosion inhibition capacity of A9O3AP is markedly enhanced by the addition of KI.


### 3.6. Potentiodynamic Polarization Studies

Potentiodynamic polarization curves for A9O3AP in 0.5 M H2SO4 at 30°C for MS specimens in the presence of various concentrations of inhibitor and inhibitor + KI are shown in Figures 8 and 9, respectively. Polarization parameters like corrosion current densities (Icorr), corrosion potential (Ecorr), cathodic Tafel slope (bc), anodic Tafel slope (ba), and inhibition efficiency (ηpol%) for MS specimens are listed in Tables 5, and 6 respectively. The data show that, addition of the Schiff base to acid media affected both the cathodic and anodic parts of the curves. Addition of I- ions to A9O3AP-H2SO4 systems results in marked decrease in the corrosion current density (Icorr). In other words, both anodic and cathodic reactions are drastically inhibited. Generally if the shift of Ecorr is >85 with respect to Ecorr of uninhibited solution, the inhibitor can be viewed as either cathodic or anodic type [22, 31, 32]. In the present study the maximum shift of Ecorr is 19 mV, suggesting that A9O3AP acts as a mixed type inhibitor for MS specimens in 0.5 M H2SO4. From the values it is clear that the inhibition efficiency of A9O3AP alone is increased in presence of KI. These results also confirm the existence of strong synergism between A9O3AP and KI in the corrosion inhibition of MS in these solutions.Table 5
Potentiodynamic polarization parameters of MS specimens in 0.5 M H2SO4at 30°C in the absence and presence of A9O3AP.
Tafel data
C (mM)
E
corr (mV/SCE)
I
corr (mA/cm2)
b
a (mV/dec)
−bc (mV/dec)
η
pol
%
Blank
−467
1.1700
82
124
—
0.2
−457
1.0220
95
114
12.65
0.4
−475
0.8240
78
116
29.57
0.6
−450
0.7010
68
117
40.09
0.8
−458
0.4511
63
103
61.44
1.0
−470
0.1730
57
097
85.21Table 6
Polarization parameters of MS specimens in 0.5 M H2SO4 at 30°C in the absence and presence of A9O3AP + 0.2 mM KI.
Tafel data
C (mM)
E
corr (mV/SCE)
I
corr (mA/cm2)
b
a (mV/dec)
−bc (mV/dec)
η
pol
%
Blank
−467
1.1700
82
124
—
0.2 + KI
−469
0.1730
57
97
85.21
0.4 + KI
−465
0.0980
63
102
91.62
0.6 + KI
−470
0.0802
88
103
93.15
0.8 + KI
−453
0.0401
30
99
96.57
1.0 + KI
−451
0.0399
40
130
96.59Figure 8
Tafel plots of MS specimens in 0.5 M H2SO4at 30°C, with and without inhibitor.Figure 9
Tafel plots of MS specimens in 0.5 M  H2SO4 at 30°C, with and without inhibitor + KI.


## 3.1. Weight Loss Measurements

Weight loss of MS specimens in 0.5 M H2SO4 at 30°C was determined at 24 h in the presence of various concentrations of inhibitor (A9O3AP) and inhibitor + KI. The corrosion rates, inhibition efficiencies, and surface coverage (θ) in the presence of inhibitor and inhibitor + 0.2 mM KI for MS specimens for the period of 24 h are shown in the Table 1.Table 1
Calculated values of inhibition efficiency (ηW%) for MS corrosion in 0.5 M H2SO4 for different systems at 30°C from weight loss measurements.
Systems/concentrations
Corrosion rate(mm/y)
Inhibition efficiency(ηW %)
θ
Blank
24.01
—
—
Blank + 0.2 mM KI
19.40
19.16
0.19
0.2 mM A9O3AP
18.06
24.77
0.25
0.4 mM A9O3AP
17.19
28.38
0.28
0.6 mM A9O3AP
15.96
33.54
0.34
0.8 mM A9O3AP
14.58
39.25
0.39
1.0 mM A9O3AP
13.50
43.75
0.44
0.2 mM A9O3AP + 0.2 mM KI
10.88
54.67
0.55
0.4 mM A9O3AP + 0.2 mM KI
10.22
57.41
0.57
0.6 mM A9O3AP + 0.2 mM KI
9.08
62.16
0.62
0.8 mM A9O3AP + 0.2 mM KI
6.84
71.49
0.71
1.0 mM A9O3AP + 0.2 mM KI
5.58
76.75
0.77From Table1, it is clear that the corrosion rate markedly decreased with inhibitor concentration from 0 to 0.2 mM. Beyond this concentration, corrosion rate showed a gradual decrease. This response is due to the fact that the surface coverage (θ) of the inhibitor molecules on the metal through adsorption increases with increase in concentration. The inhibitor + KI system showed similar trend. From Table 1 it is also evident that the inhibition efficiency increased with increase in concentration. At the inhibitor concentration of 1.0 mM, the maximum ηW% was 43.75, which shows that individual inhibitor cannot protect much effectively the corrosion of MS in H2SO4. Table 1 also shows the values of ηW% for a constant KI concentration (0.2 mM) and changing inhibitor concentration in 0.5 M H2SO4 solution. Compared with the inhibition efficiency values of inhibitor (without KI), it was found that the combination of inhibitor and 0.2 mM KI has better inhibition efficiency for all studied inhibitor concentrations.


## 3.2. Comparison of Inhibition Efficiency of Schiff Base with Its Parent Amine

To compare the inhibition efficiencies of Schiff base and parent amine (3-aminopropanoic acid), weight loss measurements of MS specimens were performed in 0.5 M H2SO4 at 30°C. The percentage of corrosion inhibition efficiencies obtained for Schiff base and parent amine on MS are represented in the Figure 2. The inhibition efficiency of the Schiff base A9O3AP was markedly higher than that of 3-aminopropanoic acid for the studied concentrations. This investigation clearly establishes the role of azomethine linkage (C = N) present in the Schiff base which actively participate in the corrosion inhibition mechanism.Figure 2
Comparison of inhibition efficiency of Schiff base and parent amine in 0.5 M H2SO4 at 24 h.


## 3.3. Adsorption Isotherm and Free Energy of Adsorption

The mechanism of adsorption and the surface behavior of organic molecules can be easily viewed through adsorption isotherms. Different models of adsorption isotherms considered are Langmiur, Temkin, Frumkin, and Freundlich isotherms. For the evaluation of thermodynamic parameters it is necessary to determine the best fit isotherm with the aid of correlation coefficient (R2). Among the isotherms mentioned above, the best description of the adsorption behavior of A9O3AP and A9O3AP + KI on MS specimens in 0.5 M H2SO4 was Freundlich and Langmiur adsorption isotherms, respectively. These models are expressed as [19]Freundlich adsorption isotherm:(4)θ=KadsC,Langmiur adsorption isotherm:(5)Cθ=1Kads+C,where C is the concentration of the inhibitor, θ is the fractional surface coverage and Kads is the adsorption equilibrium constant. Figures 3 and 4 represent the adsorption plots of A9O3AP and A9O3AP + KI obtained by the weight loss measurements of MS steel specimens in 0.5 M H2SO4 at 30°C for 24 h, respectively.Figure 3
Freundlich adsorption isotherm for adsorption of A9O3AP on MS surface in 0.5 M H2SO4 at 30°C for 24 h.Figure 4
Langmuir adsorption isotherm for adsorption of A9O3AP + KI on MS surface in 0.5 M H2SO4 at 30°C for 24 h.The adsorption equilibrium constantKads is related to the standard free energy of adsorption ΔGads0, by
(6)ΔGads0=-RTln(55.5Kads),
where 55.5 is the molar concentration of water, R is the universal gas constant, and T is the temperature in Kelvin [20]. Table 2 explores thermodynamic parameters obtained from weight loss measurements of MS in 0.5 M H2SO4 at 30∘C for 24 h. ΔGads0 for A9O3AP and A9O3AP + KI on MS showed negative values indicating the spontaneity of the process. The value of ΔGads0 upto −20 kJ mol−1 is an indication of the electrostatic interaction of the charged molecule and the charged surface of the metal (physisorption) while ΔGads0 is more negative than −40 kJ implies that inhibitor molecules are adsorbed strongly on the metal surface through coordinate type bond (chemisorption) [21, 22]. In the present investigation, A9O3AP and A9O3AP + KI molecules showed ΔGads0 −23.9 and −27.1, respectively, for MS specimens suggesting that the adsorption of inhibitor involves both electrostatic and chemical interactions.Table 2
Thermodynamic parameters obtained from weight loss studies.
MS in
Isotherm
K
ads
Δ
G
ads
0 (kJ/mol)
A9O3AP
Freundlich
244
−23.9
A9O3AP + KI
Langmiur
871
−27.1


## 3.4. Synergistic Effect

The addition of KI drastically increases theηW% values; for instance, ηW% of individual 0.2 mM is 19.16%. From Table 1 it is clear that ηW% for KI in combination with inhibitor is higher than the summation of ηW% for single KI and single inhibitor, which is synergistic in nature. Aramaki and Hackerman [23] calculated the synergism parameter Sθ using the following equation:
(7)Sθ=1-θ1+21-θ1+2′,
where θ1+2=(θ1+θ2)-(θ1θ2); θ1 = surface coverage by anion; θ2 = surface coverage by cation; θ1+2′=  measured surface coverage by both anion and cation. Sθ approaches unity when there are no interactions between the inhibitor compounds, while Sθ > 1 points to a synergistic effect; in the case of Sθ<1, the antagonistic interaction prevails. The values of the synergism parameter for the various concentrations of A9O3AP studied from the gravimetric analysis are presented in Table 3.Table 3
Synergism parameter (Sθ) for different concentrations of inhibitor in combination with 0.2 mM KI.
Concentration
Synergism parameter,Sθ
0.2 mM
1.34
0.4 mM
1.36
0.6 mM
1.42
0.8 mM
1.73
1.0 mM
1.96All values shown in this table are greater than unity. This is an indication that the enhanced inhibition efficiency resulting from the addition of iodide ions to A9O3AP is synergistic in nature [24].


## 3.5. EIS Measurements

The corrosion response of MS in 0.5 M H2SO4 in the presence of various concentrations of inhibitor and inhibitor + KI systems has been investigated using Electrochemical Impedance Spectroscopy at 30∘C. Figures 5 and 6 represent the Nyquist plots of MS specimens in 0.5 M H2SO4 in the presence of various concentrations of inhibitor and inhibitor + KI, respectively. It is evident from the plots that the impedance response of metal specimens has marked difference in the presence and absence of the KI with inhibitor A9O3AP.Figure 5
Nyquist plots for MS specimens in  0.5 M H2SO4.Figure 6
Nyquist plots (synergistic effect) for MS specimens in 0.5 M H2SO4.Impedance behaviour can be well explained by pure electric models that could verify and enable to calculate numerical values corresponding to the physical and chemical properties of electrochemical system under examination [25]. The simple equivalent circuit that fit to many electrochemical systems composed of a double layer capacitance, Rs and Rct [26, 27]. To reduce the effects due to surface irregularities of metal, constant phase element (CPE) is introduced into the circuit instead of a pure double layer capacitance which gives more accurate fit as shown in the Figure 7 [28].Figure 7
Equivalent circuit fitting for EIS measurements.The impedance of CPE can be expressed as(8)ZCPE=1Y0(jω)n,
where Y0 is the magnitude of CPE, n is the exponent (phase shift), ω is the angular frequency, and j is the imaginary unit. CPE may be resistance, capacitance, and inductance depending upon the values of n [29]. In all experiments the observed value of n ranges between 0.75 and 1.0, suggesting the capacitive response of CPE. The EIS parameters such as Rct, Rs, and CPE and the calculated values of percentage of inhibition (ηEIS%) of MS specimens are listed in Tables 4(a) and 4(b) respectively.Table 4
Electrochemical Impedance parameters of MS specimens in 0.5 M H2SO4 at 30°C in the absence and presence of inhibitor (a) and inhibitor + 0.2 mM KI (b).
(a)
C (mM)
R
ct (Ω·cm2)
C
dl (μF cm−2)
η
EIS
%
0
8.9
135
—
0.2
10.9
103
18.35
0.4
17.7
95.1
49.72
0.6
21.1
94
57.82
0.8
28.8
87
69.10
1.0
38.6
75.8
76.94
(b)
C (mM)
R
ct (Ω·cm2)
C
dl (μF cm−2)
η
EIS
%
0
8.9
135
—
0.2 + KI
91
99.9
90.22
0.4 + KI
102
93.7
91.27
0.6 + KI
151
91.3
94.11
0.8 + KI
198
79.7
95.51
1.0 + KI
251
65.1
96.45From Tables4(a) and 4(b) it is clear that Rct values are increased with increasing inhibitor concentration. The capacitance values Cdl decreases with inhibitor concentration and this decrease in Cdl is enhanced upon addition of I− ions to the corrosive environment (inspect data listed in Tables 4(a) and 4(b)). These results suggest that the A9O3AP molecules function by adsorption at the metal/solution interface [30] and this adsorption is reinforced by I− ions. This decrease in Cdl may be explained on the basis that the double layer between the charged metal surface and the solution is considered as an electrical capacitor. The ηEIS% data reveal that the corrosion inhibition capacity of A9O3AP is markedly enhanced by the addition of KI.


## 3.6. Potentiodynamic Polarization Studies

Potentiodynamic polarization curves for A9O3AP in 0.5 M H2SO4 at 30°C for MS specimens in the presence of various concentrations of inhibitor and inhibitor + KI are shown in Figures 8 and 9, respectively. Polarization parameters like corrosion current densities (Icorr), corrosion potential (Ecorr), cathodic Tafel slope (bc), anodic Tafel slope (ba), and inhibition efficiency (ηpol%) for MS specimens are listed in Tables 5, and 6 respectively. The data show that, addition of the Schiff base to acid media affected both the cathodic and anodic parts of the curves. Addition of I- ions to A9O3AP-H2SO4 systems results in marked decrease in the corrosion current density (Icorr). In other words, both anodic and cathodic reactions are drastically inhibited. Generally if the shift of Ecorr is >85 with respect to Ecorr of uninhibited solution, the inhibitor can be viewed as either cathodic or anodic type [22, 31, 32]. In the present study the maximum shift of Ecorr is 19 mV, suggesting that A9O3AP acts as a mixed type inhibitor for MS specimens in 0.5 M H2SO4. From the values it is clear that the inhibition efficiency of A9O3AP alone is increased in presence of KI. These results also confirm the existence of strong synergism between A9O3AP and KI in the corrosion inhibition of MS in these solutions.Table 5
Potentiodynamic polarization parameters of MS specimens in 0.5 M H2SO4at 30°C in the absence and presence of A9O3AP.
Tafel data
C (mM)
E
corr (mV/SCE)
I
corr (mA/cm2)
b
a (mV/dec)
−bc (mV/dec)
η
pol
%
Blank
−467
1.1700
82
124
—
0.2
−457
1.0220
95
114
12.65
0.4
−475
0.8240
78
116
29.57
0.6
−450
0.7010
68
117
40.09
0.8
−458
0.4511
63
103
61.44
1.0
−470
0.1730
57
097
85.21Table 6
Polarization parameters of MS specimens in 0.5 M H2SO4 at 30°C in the absence and presence of A9O3AP + 0.2 mM KI.
Tafel data
C (mM)
E
corr (mV/SCE)
I
corr (mA/cm2)
b
a (mV/dec)
−bc (mV/dec)
η
pol
%
Blank
−467
1.1700
82
124
—
0.2 + KI
−469
0.1730
57
97
85.21
0.4 + KI
−465
0.0980
63
102
91.62
0.6 + KI
−470
0.0802
88
103
93.15
0.8 + KI
−453
0.0401
30
99
96.57
1.0 + KI
−451
0.0399
40
130
96.59Figure 8
Tafel plots of MS specimens in 0.5 M H2SO4at 30°C, with and without inhibitor.Figure 9
Tafel plots of MS specimens in 0.5 M  H2SO4 at 30°C, with and without inhibitor + KI.


## 4. Mechanism and Explanation for Synergism

The synergistic inhibition brought about by the combination of A9O3AP and iodide ions for the corrosion of MS in 0.5 M H2SO4 can be explained on the basis that halide ions have a greater tendency to be adsorbed on the surface in attraction with organic cations. The protonated Schiff base (A9O3AP+) is then adsorbed by coulombic attraction at the steel surface, where iodide ions are already adsorbed by chemisorptions (Figure 10). Greater surface coverage from the stabilization of adsorbed iodide ions by means of electrostatic interaction with A9O3AP+ facilitates corrosion inhibition synergism. I- alone polarizes both the anodic and cathodic reaction of iron over a wide potential range. It is apparent then that the effects of I- are not due to electrostatic effects alone, but some covalent bonding to the metal must be involved. The large size and ease of polarizability of I- facilitate electron pair bonding. The halide ions are first adsorbed on the metal surface and the inhibitor is then drawn in to the double layer by the adsorbed halide ion, such that the ion pair formation occurs directly on the metal surface:
(9)As→Aads,Bs+Aads→(BA)ads,
where Bs and As represent inhibitor and halide, ion respectively, in the bulk solution, while Aads and (BA)ads refers halide ion and ion-pair, respectively, in the adsorbed state.Figure 10
The schematic illustration of modes of adsorption on mild steel in 0.5 M H2SO4.


## 5. Conclusions

(1)
A9O3AP acts as moderate inhibitor for MS in 0.5 M sulphuric acid medium.
(2)
Inhibition efficiency increases with increase in concentration of inhibitor.
(3)
The addition of iodide ions to A9O3AP enhanced the inhibition efficiency due to synergistic effect.
(4)
The adsorption of A9O3AP alone and in combination with iodide ions obeys Freundlich and Langmiur adsorption isotherms, respectively.
(5)
The thermodynamic parameters calculated from the adsorption isotherms showed that both physisorption and chemisorption are involved in the inhibition process.



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*Source: 425878-2012-12-05.xml*