# Corrosion Behavior of Carbon Steel in Synthetically Produced Oil Field Seawater

Authors: Subir Paul; Anjan Pattanayak; Sujit K. Guchhait
Journal: International Journal of Metals
 (2014)

---

## Abstract

The life of offshore steel structure in the oil production units is decided by the huge corrosive degradation due toSO
4
2
-, S2−, and Cl−, which normally present in the oil field seawater. Variation in  pH and temperature further adds to the rate of degradation on  steel. Corrosion behavior of mild steel is  investigated through polarization, EIS, XRD, and optical and SEM microscopy. The effect of all 3 species is huge  material degradation with FeSx and FeCl3 and their complex as corrosion products. EIS data match the model  of Randle circuit with Warburg resistance.  Addition of more corrosion species decreases impedance and increases capacitance values of the Randle circuit at the interface. The attack is found to be at the grain boundary  as well as grain body with  very prominent sulphide corrosion crack.


---

## Body

## 1. Introduction

The severe corrosion of the submersed structures in the oil field at the production site and crude oil transportation is unpredictable and is a major component of the total corrosion loss in oil and gas industries. The corrosion species in the aqueous oil field seawater areCO
3
2
-, S2−, Cl−, SO
4
2
-, and O (Table 1) [1] which are also influenced by the variation of pH and temperature. CO
3
2
- and S2− are formed from CO2 and H2S of the oil in the aqueous environment. And Cl−, SO
4
2
-, and O are present in the seawater. Besides these parameters, there are fluid dynamics of sea water and suspended solids and sands, influencing the erosion corrosion of the marine structures. Crude oil and natural gas can carry various high-impurity products which are inherently corrosive. In the case of oil and gas wells and pipelines, such highly corrosive media are carbon dioxide (CO2), hydrogen sulfide (H2S), and free water [2].Table 1
Ions present in typical oil field seawater.
Species typically found in oil field brines
Element
Concentration mg/L
CO2
Dissolved carbon dioxide
Barium
Ba2+
31
H2CO3
Carbonic acid
Boron
B
6
HC
O
3
-
Bicarbonate ion
Calcium
Ca2+
284
C
O
3
2
-
Carbonate ion
Iron
Fe3+
55.85
H+
Hydrogen ion
Magnesium
Mg2+
24.31
OH−
Hydroxide ion
Phosphorous
P3−
1
Fe2+
Iron ion
Potassium
K
50
Cl−
Chloride ion
Sodium
Na
4770
Na+
Sodium ion
Strontium
Sr2+
83
K+
Potassium
Chloride
Cl−
7480
Ca2+
Calcium ion
Bromide
Br−
20
Mg2+
Magnesium ion
Sulphate
S
O
4
2
-
21
Ba2+
Barium ion
Nitrate
N
O
3
-
0.50
Sr2+
Strontium ion
Hydroxyl
OH−
0
CH3COOH (HAc)
Acetic acid
Carbonate
C
O
3
2
-
0
CH3COO− (Ac−)
Acetate ion
Bicarbonate
HC
O
3
-
500
HS
O
4
-
Bisulphate ion
Dissolved CO2
CO2
92.4
S
O
4
2
-
Sulphate ion
Specific gravity
1.014
pH
6.58
Resistivity
0.4405 Ohm
Total dissolved solids 1
3.453 mgThe effect of any individual parameter on corrosion rate has been studied extensively [3–6]. But the conjoint effect of the above mentioned parameters and interfering effects and interactions are complex and are not very well understood. The salts and sulfide compounds dissolved in crude oil can provoke the formation of a corrosive aqueous solution whose chemical composition involves the presence of both hydrochloric acid (HCI) and hydrogen sulfide (H2S) [3, 4]. Corrosion mitigation in the oil field industry has traditionally been performed by combining methods for measuring the corrosion rates such as corrosion coupons and regular pipeline inspections with prevention strategies [6]. But that required years to get empirical results and could not be applied to other geographical locations of different sea water chemistry. All the factors make the corrosion mechanisms in the oil fields very complex with high degree of interaction among the species. Several previous studies have been performed related to the corrosion process of iron and steel in H2S solutions [4, 7–13]. These works studied the influence of H2S on the corrosion phenomena at ambient temperature. In H2S-containing solutions, the corrosion process of metal may be accompanied by the formation of a sulfide film on the metal surface and leads to more complicated corrosion behavior. Previous researches [14–16] have shown that H2S had a remarkable acceleration effect on both the anodic iron dissolution and the cathodic evolution in most cases but H2S may exhibit an inhibitive effect on the corrosion of iron or steel weld. Recently, the influence of H2S concentration on the corrosion behavior of carbon steel at 90°C has been investigated [15]. Physical modeling of ships and offshore structures in ocean water by Melchers et al. [17–19] and Shehadeh and Hassan [20] adds to better understanding of the present investigation. However, little research has been done on the corrosion behavior of carbon steel in the presence of both H2S and NaCl at ambient and elevated temperature.Corrosion mechanisms in oil field systems are complex and are showing high degrees of interaction between corrosion species, products, and oil field metallurgies. The interactions of sulfate and chloride are of interest in this work, since presence of sulfate ions, in oilfield produced water, strongly influence corrosion mechanisms. While there are many research works on the effects of CO2 and H2S on corrosion of carbon steel, those of conjoint effects of S2−, Cl−, and SO
4
2
- are much less. The present investigation aims to study the conjoint effects of S2−, Cl−, and SO
4
2
- along with variation of pH and temperature on carbon steel. The corrosive species included are sulfate, chloride, hydrogen sulfide, temperature, and pH. Sulphate and chloride were added as Na2SO4 and NaCl. Hydrogen sulfide was introduced to the corrosion cell with the following reaction:
(1)
Na
2
S
+
H
2
SO
4
=
H
2
S
+
Fe
SO
4The effect on corrosion of these species was examined through polarization experimentation using a three-electrode glass corrosion cell and potentiostat. Electrochemical AC impedance spectroscopy studies were also carried out for better understanding of electrochemical effects of corrosive species on electrical phenomenon occurring at metal-solution interface. The corroded and uncorroded substrates were characterized by XRD. The morphology of the corroded surface was investigated by optical microscopy and SEM.


## 2. Experimental Methods

### 2.1. Polarization Studies

Electrochemical measurements were conducted using Gamry Potentiostat instrument coupled with Echem analyst software, controlled by a personal computer, in a conventional three-electrode cell systems. The working electrode was carbon steel, the counter electrode was graphite, and a saturated calomel electrode (SCE) acted as the reference electrode. Experiments were performed in different concentrations of Cl−, SO
4
2
-, and S2− solutions, at preselected pH and temperature, to determine the corrosion potential E
corr and corrosion current i
corr. The potential was scanned between −1.5 V and 1 V at a scan rate of 1 mV/s.


### 2.2. Electrochemical Impedance Spectroscopy (EIS)

The experimental arrangement was the same as that of polarization studies. The electrochemical cell was connected to an impedance analyzer (EIS300 controlled by Echem analyst software) for electrochemical impedance spectroscopy. The electrochemical impedance spectra were obtained at frequencies between 300 kHz and 0.01 Hz. The amplitude of the sinusoidal wave was 10 mV. The following results and information are obtained from the EIS experiments: Polarization resistance (R
p), electrolyte resistance (R
u), double layer capacitance (C
dl), capacitive load or constant phase element, CPE
(
Y
), and α which is defined from the capacitive impedance equation Z
=
1
/
C
(
j
w
)
-
α.Capacitors in EIS experiments often do not behave ideally. Instead, they act like a constant phase element (CPE). The exponentα
=
1 for pure capacitance. For a constant phase element, the exponent α is less than one. The “double layer capacitor” on real cells often behaves like a CPE instead of like a pure capacitor.


### 2.3. X-Ray Diffraction (XRD) Analysis

The X-ray diffraction technique is used to define the crystalline structure and the crystalline phases. This test was done using a Rigaku Ultima III X-Ray Diffractometer for recording the diffraction traces of the samples with monochromatized Cu Kα radiation, at room temperature; the scan region (2θ) ranged from 10° to 100° at a scan rate of 5° min−1.


### 2.4. Scanning Electron Microscope (SEM) Morphology

The electron micrographs were studied by SEM with accelerating voltage 30 kV, magnification up to 300,000x, and resolution of 3.5 nm. The images of the corroded samples were photographed at low and high magnification.


## 2.1. Polarization Studies

Electrochemical measurements were conducted using Gamry Potentiostat instrument coupled with Echem analyst software, controlled by a personal computer, in a conventional three-electrode cell systems. The working electrode was carbon steel, the counter electrode was graphite, and a saturated calomel electrode (SCE) acted as the reference electrode. Experiments were performed in different concentrations of Cl−, SO
4
2
-, and S2− solutions, at preselected pH and temperature, to determine the corrosion potential E
corr and corrosion current i
corr. The potential was scanned between −1.5 V and 1 V at a scan rate of 1 mV/s.


## 2.2. Electrochemical Impedance Spectroscopy (EIS)

The experimental arrangement was the same as that of polarization studies. The electrochemical cell was connected to an impedance analyzer (EIS300 controlled by Echem analyst software) for electrochemical impedance spectroscopy. The electrochemical impedance spectra were obtained at frequencies between 300 kHz and 0.01 Hz. The amplitude of the sinusoidal wave was 10 mV. The following results and information are obtained from the EIS experiments: Polarization resistance (R
p), electrolyte resistance (R
u), double layer capacitance (C
dl), capacitive load or constant phase element, CPE
(
Y
), and α which is defined from the capacitive impedance equation Z
=
1
/
C
(
j
w
)
-
α.Capacitors in EIS experiments often do not behave ideally. Instead, they act like a constant phase element (CPE). The exponentα
=
1 for pure capacitance. For a constant phase element, the exponent α is less than one. The “double layer capacitor” on real cells often behaves like a CPE instead of like a pure capacitor.


## 2.3. X-Ray Diffraction (XRD) Analysis

The X-ray diffraction technique is used to define the crystalline structure and the crystalline phases. This test was done using a Rigaku Ultima III X-Ray Diffractometer for recording the diffraction traces of the samples with monochromatized Cu Kα radiation, at room temperature; the scan region (2θ) ranged from 10° to 100° at a scan rate of 5° min−1.


## 2.4. Scanning Electron Microscope (SEM) Morphology

The electron micrographs were studied by SEM with accelerating voltage 30 kV, magnification up to 300,000x, and resolution of 3.5 nm. The images of the corroded samples were photographed at low and high magnification.


## 3. Results and Discussions

The effects ofCl
-, SO
4
2
-, S
2
-, pH, and temperature on degradation behavior of carbon steel were studied by potentiostatic polarization to determine corrosion current and corrosion potential. The various electrical properties at the metal-solution interface were determined by electrochemical impedance spectroscopy (EIS). The presence of different elements on corroded surface was detected by XRD. The morphology of the degraded surfaces was characterized by optical microscopy and SEM. Before going into the experimental findings of the effects of different interfering ions, it is worthwhile to discuss the basic electrochemical reactions of aqueous corrosion of steel in the presence of those ions.The main electrochemical anodic and cathodic reactions for the corrosion of carbon steel in aqueous oil fields environments in presences of the ions are as follows.Half Cell Reactions (E versus SCE).Consider
(2)
Fe
=
Fe
2
+
+
2
e
E
0
=
-
.
681
(3)
O
2
+
2
H
2
O
+
4
e
-
⟶
4
O
H
-
E
0
=
0.579
(4)
H
+
e
=
1
2
H
2
E
0
=
-
0.241
In presence ofSO
4
2
-, present reactions are
(5)
SO
4
2
-
+
2
e
+
H
2
O
=
2
SO
3
2
-
+
OH
E
0
=
-
1.177
(6)
2
SO
3
2
-
+
4
e
+
3
H
2
O
=
3
S
2
O
3
2
-
+
6
OH
-
E
0
=
-
0.99
(7)
2
SO
3
2
-
+
4
e
+
3
H
2
O
=
S
+
6
OH
-
(8)
S
+
2
e
-
=
S
2
-
E
0
=
-
0.688
In presence of Na2S or H2S (Na2S was added in state of H2S to understand the effect of s2−),
(9)
H
2
S
=
H
+
+
H
S
-
(10)
H
S
-
=
H
+
+
S
-
E
0
=
-
0.688
In the presence of Cl−, that is (NaCl/HCl),
(11)
Fe
2
+
+
2
Cl
-
=
Fe
Cl
2
(12)
Fe
Cl
2
+
2
H
2
O
=
Fe
OH
2
+
2
H
+
+
2
Cl
-
(13)
Fe
Cl
2
+
Cl
-
=
Fe
Cl
3
+
e
(14)
Fe
+
2
H
+
=
Fe
2
+The above equations would help in better understanding of the effects of the corrosion species found in the experimental results.


### 3.1. Polarization Studies

#### 3.1.1. Effect ofSO
4
2
-

Figure1 shows the potential dynamic polarization curve with increasing SO
4
2
- concentration at pH 6. The pH of sea water normally varies from 7.5 to 8.2. but in the oil fields due to the presence of few acidic substances, namely, carbonic acid, H2S, and other organic acids, pH may shift from near neutral towards the acidic side between 6 and 4. It is seen here that the corrosion rate increases with increase in concentration of SO
4
2
-. It is seen from (5)–(8) that the cathodic reduction of SO
4
2
- ions produces thiosulfate and sulphide ions, both of which are aggressive corrosion species and hence degrade the steel surface in sea water in the acidic pH range below the neutral medium. The corrosion product in this case should be iron sulphide or thiosulfate.Figure 1
Potentiodynamic polarization curves of low carbon steel in different concentration of Na2SO4 solution at pH 6 and temperature 25°C.


#### 3.1.2. Effect ofSO
4
2
- + S2−

Addition of S2− to the solution containing SO
4
2
- further enhances the corrosion rate as can be seen from Figure 2. And the pH has a strong effect on it. It can be seen from (11) and (12) above that the conjoint effect of SO
4
2
- and S
- is the production of increasing amount of S
-, as well as corrosive sulphur compound.Figure 2
Effect of S2− on potentiodynamic polarization curves of carbon steel in 0.25 M Na2SO4 solution at pH 6 and temperature 25°C.


#### 3.1.3.  Effect ofSO
4
2
- + Cl−

Corrosion rate also increases with addition of Cl− to the solution containing SO
4
2
- (Figure 3). The rate increases with increase in Cl− concentration. It is seen from (11)–(14) above that the Cl− ions attack Fe/Fe2+ with the formation of corrosion products FeCl2 and FeCl3. FeCl2 is unstable and may hydrolyse or further react with Cl− ions to form Fe(OH)2 or FeCl3, respectively.Figure 3
Effect of Cl− on potentiodynamic polarization curves of carbon steel in 0.25 M Na2SO4 solution at pH 8 and temperature 25°C.


#### 3.1.4. Effect ofSO
4
2
- + S2− + Cl−

The conjugate of all 3 ions which are normally present in the oil field sea water is the degradation of carbon steel structure at the highest level. It is seen from Figure4 that i
corr values have shifted to the right and E
corr towards the active potential with increasing the concentration of both S2− and Cl−.Figure 4
Effect of Cl− + S2− on potentiodynamic polarization curves of carbon steel in 0.25 M Na2SO4 solution at pH 8 and temperature 25°C.


#### 3.1.5. Effect of pH

There is not any much significant effect of polarization curves with change in pH except at pH 11 under alkaline condition (Figure5), when the corrosion rate is very low. The steel is in the passive region at this pH. The pH of the oil field water is in the range of 4–6 when the corrosion rate is high.Figure 5
Potentiodynamic polarization curves of carbon steel in an aqueous solution of 0.25 M Na2SO4 and 0.3 M Na2S at temperature 25°C, at different pH.


#### 3.1.6. Effect of Temperature

Temperature aggravates the material degradation (Figure6) by increasing diffusion and mass transfer coefficient of the aggressive ions corroding the metallic surface. Temperature also increases the I
L, the limiting current density of the concentration polarization, and hence shifts the polarization curves to the right.Figure 6
Potentiodynamic polarization curves of low carbon steel in 0.25 M Na2SO4 solution at (pH = 8) at different temperature.


### 3.2. Electrochemical Impedance Spectroscopy (EIS)

The phenomenon at the interface of the solid metal and aqueous electrolyte is a complex process consisting of a line of positively and negatively charged ions, capacitance due to double layer, corroded product or film formation on surfaces, polarization resistance (R
p), pore resistance (R
po), and various types of impedance due to diffusion of ions, movement of charge in or away from metal surface, and adsorption of cation and anion. The whole phenomenon can be represented by an equivalent AC electrical circuit. The phenomenon can be interpreted from the Bode plots, which are depicted and discussed in the following section for various corrosive species.Figure7 displays the Bode plots of carbon steel in solutions of SO
4
2
-, SO
4
2
- + S2−, and SO
4
2
- + S2− + Cl−. It is to be noticed that, in all the solutions, EIS data match the model of Randle circuit with a Warburg resistance, W
d (given in the inset of each figure), that prevails at the metal-solution interface. It is seen that the impedance decreases with addition of different aggressive ions compared to those with base solution of only SO
4
2
-. This decrease in impedance leads to more current flow across the interface and hence increase in corrosion rate. There is a phase angle shift with frequency. The minimum phase angle reaches much less than 90 degrees, indicating the capacitance in the circuit is not a pure capacitance but constant phase element, CPE
(
Y
), and is given by the capacitive impedance equation Z
=
1
/
C
(
j
w
)
-
α, where α is fraction varying from 0 to 1; the value less than one indicates that it does not behave ideally as pure capacitance. At high frequency, the value of impedance Z
mod
⁡ is roughly equal to R
S, while at low frequency the value is (R
S
+
R
P). Both can be determined from the blots. Table 1 depicted the computed values of the EIS parameters. It is seen that polarization resistance decreases with addition of more types of ions which support the polarization results of corrosion rates increase as found in Figures 2, 3, and 4. The increase in corrosion rate is supported by the EIS data, increase in Y
0 which behaves like capacitance, and decrease in polarization resistance (Table 2). The values of α indicate that the capacitance behaves like constant phase element rather than pure capacitance. The Warburg resistance W
d which signifies resistance to the flow of ions from the solution to corroded metal surface also decreases with addition of more types of ions. All the facts confirm the enhanced corrosion rates of carbon steel in the oil field sea water with presence of SO
4
2
- + S2− + Cl−.Table 2
Computed EIS parameters.
Sample
Corrosive ions
R
s
(ohm)
R
p (ohm)
Y
0
μF
α
W
d (ohm)
Carbon steel
S
O
4
2
-
9.443
8500.0
75.0
0.720
10.430
Carbon steel
S
O
4
2
- + S2−
8.268
3700
572.2
0.769
4.187
Carbon steel
S
O
4
2
- + S2− + Cl−
13.31
95
905.6
0.602
2.432Bode plots of carbon steel inSO
4
2
-, SO
4
2
- + S2−, and SO
4
2
- + S2− + Cl− solution at pH 8 and temperature 25°C.
(a)
(b)
(c)


### 3.3. X-Ray Diffraction

The presence of corrosion products of FeS, FeCl2, and FeCl3 is clearly indicated by the XRD peak intensities in Figure 8. This supports the corrosion enhancement by SO
4
2
-, S2−, and Cl− ions as found in polarization and EIS studies.X-ray diffraction showing peaks of different corroded phases.
(a)
(b)
(c)
(d)


### 3.4. Optical and SEM Microscopy Images

The microstructures by optical microscopy clearly show (Figure9) the corroded structure of steel with products of corrosion over it. The form of corrosion seems to be uniform, not localized. SEM images (Figure 10) distinctly reveal how the degree of degradation increases with presence of ions in the solutions from SO
4
2
- to SO
4
2
- + S2− to SO
4
2
- + S2− + Cl−. It is interesting to observe from the morphology of SEM image at higher magnification (Figure 11) that the corrosion has taken place at grain boundary as well as grain body but the attack at grain boundary is very prominent with sulphide (S) corrosion crack. The corrosion products of sulphide compounds as well as element sulphur are clearly revealed. The structure of SEM images shows almost catastrophic failure with the presence of minor and major cracks when the seawater is enriched with the presence of all three corrosive ions, SO
4
2
-, S2−, and Cl−. The morphology of SEM image analysis along with XRD is in complete agreement with the corrosion data of the polarization experiments and EIS.Figure 9
Optical microscopy images of corroded steel. (a) Na2SO4, (b) Na2SO4 + Na2S, and (c) Na2SO4 + Na2S + NaCl.Figure 10
SEM images of corroded steel (a) before corrosion, (b) in Na2SO4, (c) in Na2SO4 + Na2S, and (d) in Na2SO4 + Na2S + NaCl.Figure 11
SEM images of corroded steel (a) in Na2SO4, (b) in Na2SO4 + Na2S, and (c) in Na2SO4 + Na2S + NaCl.From (5)–(8), it is seen that SO
4
2
- is cathodically reduced to give rise to S2−. It is observed from the polarization curve (Figure 1) that the increase of SO
4
2
- concentration depolarizes the cathodic curves much more compared to anodic ones, shifting E
corr towards the negative potential. The release of S2− from the reaction produces corrosion products: iron sulfides (Fe
S
x) on carbon steel surface. They are nonstoichiometric iron sulfide films mainly composed of mackinawite and pyrrhotite Berner [21–26]. The black color of mackinawite phase is also seen as corrosion products in optical microstructures (Figures 9(a) and 9(b)).The deterioration of metal due to contact with S2− (H2S) and moisture is sour corrosion. The forms of sour corrosion are uniform (Figure 9(b)), pitting, and stepwise cracking (Figures 10(c) and 11(b)).The general equation of sour corrosion can be expressed as follows [21]:
(15)
S
2
-
+
2
H
+
=
H
2
S
(
aq
)
E
=
0
.
097
V
versus
SCEHydrogen sulphide dissociates to produce proton and bisulphide as described [22] by the following equations:
(16)
H
2
S
(
aq
)
=
H
+
+
H
S
-
K
=
9.1
×
10
-
8
H
S
-
=
H
+
+
S
2
-
K
=
9.1
×
10
-
12This reaction scheme shows that the presence of hydrogen sulfide can contribute to the concentration of sulfide at the surface by dissociation rather than charge exchange with the surface. The sulfide concentration at the surface is, therefore, dependent on the concentration of aqueous hydrogen sulfide in the electrolyte as well as the reduction processes of sulfate.H2S exhibits the different role in anodic process of carbon steel depending on the pH value in the solutions. The local supersaturation of Fe
S
x could be formed on the carbon steel surface via the following reaction, with the nucleation and growth of one or more of the iron sulfide, mackinawite:
(17)
H
2
S
+
Fe
+
H
2
O
⟶
FeS
x
+
2
H
+
H
2
OThe black corrosion products (FeS
x) formed on the steel surface in the H2S-containing solutions could be observed (Figure 9(b)). The addition of chloride to the corrosion system did not exhibit any localized corrosion; rather it drastically increased the i
corr values and shifted E
corr towards the negative potential (Figures 3 and 4), depolarizing the anodic reactions. The increase in i
corr with Cl addition seems to have modified the anodic substrate area (Figures 9(c) and 10(d)) and has enhanced the exchange current density for the iron oxidation process.


## 3.1. Polarization Studies

### 3.1.1. Effect ofSO
4
2
-

Figure1 shows the potential dynamic polarization curve with increasing SO
4
2
- concentration at pH 6. The pH of sea water normally varies from 7.5 to 8.2. but in the oil fields due to the presence of few acidic substances, namely, carbonic acid, H2S, and other organic acids, pH may shift from near neutral towards the acidic side between 6 and 4. It is seen here that the corrosion rate increases with increase in concentration of SO
4
2
-. It is seen from (5)–(8) that the cathodic reduction of SO
4
2
- ions produces thiosulfate and sulphide ions, both of which are aggressive corrosion species and hence degrade the steel surface in sea water in the acidic pH range below the neutral medium. The corrosion product in this case should be iron sulphide or thiosulfate.Figure 1
Potentiodynamic polarization curves of low carbon steel in different concentration of Na2SO4 solution at pH 6 and temperature 25°C.


### 3.1.2. Effect ofSO
4
2
- + S2−

Addition of S2− to the solution containing SO
4
2
- further enhances the corrosion rate as can be seen from Figure 2. And the pH has a strong effect on it. It can be seen from (11) and (12) above that the conjoint effect of SO
4
2
- and S
- is the production of increasing amount of S
-, as well as corrosive sulphur compound.Figure 2
Effect of S2− on potentiodynamic polarization curves of carbon steel in 0.25 M Na2SO4 solution at pH 6 and temperature 25°C.


### 3.1.3.  Effect ofSO
4
2
- + Cl−

Corrosion rate also increases with addition of Cl− to the solution containing SO
4
2
- (Figure 3). The rate increases with increase in Cl− concentration. It is seen from (11)–(14) above that the Cl− ions attack Fe/Fe2+ with the formation of corrosion products FeCl2 and FeCl3. FeCl2 is unstable and may hydrolyse or further react with Cl− ions to form Fe(OH)2 or FeCl3, respectively.Figure 3
Effect of Cl− on potentiodynamic polarization curves of carbon steel in 0.25 M Na2SO4 solution at pH 8 and temperature 25°C.


### 3.1.4. Effect ofSO
4
2
- + S2− + Cl−

The conjugate of all 3 ions which are normally present in the oil field sea water is the degradation of carbon steel structure at the highest level. It is seen from Figure4 that i
corr values have shifted to the right and E
corr towards the active potential with increasing the concentration of both S2− and Cl−.Figure 4
Effect of Cl− + S2− on potentiodynamic polarization curves of carbon steel in 0.25 M Na2SO4 solution at pH 8 and temperature 25°C.


### 3.1.5. Effect of pH

There is not any much significant effect of polarization curves with change in pH except at pH 11 under alkaline condition (Figure5), when the corrosion rate is very low. The steel is in the passive region at this pH. The pH of the oil field water is in the range of 4–6 when the corrosion rate is high.Figure 5
Potentiodynamic polarization curves of carbon steel in an aqueous solution of 0.25 M Na2SO4 and 0.3 M Na2S at temperature 25°C, at different pH.


### 3.1.6. Effect of Temperature

Temperature aggravates the material degradation (Figure6) by increasing diffusion and mass transfer coefficient of the aggressive ions corroding the metallic surface. Temperature also increases the I
L, the limiting current density of the concentration polarization, and hence shifts the polarization curves to the right.Figure 6
Potentiodynamic polarization curves of low carbon steel in 0.25 M Na2SO4 solution at (pH = 8) at different temperature.


## 3.1.1. Effect ofSO
4
2
-

Figure1 shows the potential dynamic polarization curve with increasing SO
4
2
- concentration at pH 6. The pH of sea water normally varies from 7.5 to 8.2. but in the oil fields due to the presence of few acidic substances, namely, carbonic acid, H2S, and other organic acids, pH may shift from near neutral towards the acidic side between 6 and 4. It is seen here that the corrosion rate increases with increase in concentration of SO
4
2
-. It is seen from (5)–(8) that the cathodic reduction of SO
4
2
- ions produces thiosulfate and sulphide ions, both of which are aggressive corrosion species and hence degrade the steel surface in sea water in the acidic pH range below the neutral medium. The corrosion product in this case should be iron sulphide or thiosulfate.Figure 1
Potentiodynamic polarization curves of low carbon steel in different concentration of Na2SO4 solution at pH 6 and temperature 25°C.


## 3.1.2. Effect ofSO
4
2
- + S2−

Addition of S2− to the solution containing SO
4
2
- further enhances the corrosion rate as can be seen from Figure 2. And the pH has a strong effect on it. It can be seen from (11) and (12) above that the conjoint effect of SO
4
2
- and S
- is the production of increasing amount of S
-, as well as corrosive sulphur compound.Figure 2
Effect of S2− on potentiodynamic polarization curves of carbon steel in 0.25 M Na2SO4 solution at pH 6 and temperature 25°C.


## 3.1.3.  Effect ofSO
4
2
- + Cl−

Corrosion rate also increases with addition of Cl− to the solution containing SO
4
2
- (Figure 3). The rate increases with increase in Cl− concentration. It is seen from (11)–(14) above that the Cl− ions attack Fe/Fe2+ with the formation of corrosion products FeCl2 and FeCl3. FeCl2 is unstable and may hydrolyse or further react with Cl− ions to form Fe(OH)2 or FeCl3, respectively.Figure 3
Effect of Cl− on potentiodynamic polarization curves of carbon steel in 0.25 M Na2SO4 solution at pH 8 and temperature 25°C.


## 3.1.4. Effect ofSO
4
2
- + S2− + Cl−

The conjugate of all 3 ions which are normally present in the oil field sea water is the degradation of carbon steel structure at the highest level. It is seen from Figure4 that i
corr values have shifted to the right and E
corr towards the active potential with increasing the concentration of both S2− and Cl−.Figure 4
Effect of Cl− + S2− on potentiodynamic polarization curves of carbon steel in 0.25 M Na2SO4 solution at pH 8 and temperature 25°C.


## 3.1.5. Effect of pH

There is not any much significant effect of polarization curves with change in pH except at pH 11 under alkaline condition (Figure5), when the corrosion rate is very low. The steel is in the passive region at this pH. The pH of the oil field water is in the range of 4–6 when the corrosion rate is high.Figure 5
Potentiodynamic polarization curves of carbon steel in an aqueous solution of 0.25 M Na2SO4 and 0.3 M Na2S at temperature 25°C, at different pH.


## 3.1.6. Effect of Temperature

Temperature aggravates the material degradation (Figure6) by increasing diffusion and mass transfer coefficient of the aggressive ions corroding the metallic surface. Temperature also increases the I
L, the limiting current density of the concentration polarization, and hence shifts the polarization curves to the right.Figure 6
Potentiodynamic polarization curves of low carbon steel in 0.25 M Na2SO4 solution at (pH = 8) at different temperature.


## 3.2. Electrochemical Impedance Spectroscopy (EIS)

The phenomenon at the interface of the solid metal and aqueous electrolyte is a complex process consisting of a line of positively and negatively charged ions, capacitance due to double layer, corroded product or film formation on surfaces, polarization resistance (R
p), pore resistance (R
po), and various types of impedance due to diffusion of ions, movement of charge in or away from metal surface, and adsorption of cation and anion. The whole phenomenon can be represented by an equivalent AC electrical circuit. The phenomenon can be interpreted from the Bode plots, which are depicted and discussed in the following section for various corrosive species.Figure7 displays the Bode plots of carbon steel in solutions of SO
4
2
-, SO
4
2
- + S2−, and SO
4
2
- + S2− + Cl−. It is to be noticed that, in all the solutions, EIS data match the model of Randle circuit with a Warburg resistance, W
d (given in the inset of each figure), that prevails at the metal-solution interface. It is seen that the impedance decreases with addition of different aggressive ions compared to those with base solution of only SO
4
2
-. This decrease in impedance leads to more current flow across the interface and hence increase in corrosion rate. There is a phase angle shift with frequency. The minimum phase angle reaches much less than 90 degrees, indicating the capacitance in the circuit is not a pure capacitance but constant phase element, CPE
(
Y
), and is given by the capacitive impedance equation Z
=
1
/
C
(
j
w
)
-
α, where α is fraction varying from 0 to 1; the value less than one indicates that it does not behave ideally as pure capacitance. At high frequency, the value of impedance Z
mod
⁡ is roughly equal to R
S, while at low frequency the value is (R
S
+
R
P). Both can be determined from the blots. Table 1 depicted the computed values of the EIS parameters. It is seen that polarization resistance decreases with addition of more types of ions which support the polarization results of corrosion rates increase as found in Figures 2, 3, and 4. The increase in corrosion rate is supported by the EIS data, increase in Y
0 which behaves like capacitance, and decrease in polarization resistance (Table 2). The values of α indicate that the capacitance behaves like constant phase element rather than pure capacitance. The Warburg resistance W
d which signifies resistance to the flow of ions from the solution to corroded metal surface also decreases with addition of more types of ions. All the facts confirm the enhanced corrosion rates of carbon steel in the oil field sea water with presence of SO
4
2
- + S2− + Cl−.Table 2
Computed EIS parameters.
Sample
Corrosive ions
R
s
(ohm)
R
p (ohm)
Y
0
μF
α
W
d (ohm)
Carbon steel
S
O
4
2
-
9.443
8500.0
75.0
0.720
10.430
Carbon steel
S
O
4
2
- + S2−
8.268
3700
572.2
0.769
4.187
Carbon steel
S
O
4
2
- + S2− + Cl−
13.31
95
905.6
0.602
2.432Bode plots of carbon steel inSO
4
2
-, SO
4
2
- + S2−, and SO
4
2
- + S2− + Cl− solution at pH 8 and temperature 25°C.
(a)
(b)
(c)


## 3.3. X-Ray Diffraction

The presence of corrosion products of FeS, FeCl2, and FeCl3 is clearly indicated by the XRD peak intensities in Figure 8. This supports the corrosion enhancement by SO
4
2
-, S2−, and Cl− ions as found in polarization and EIS studies.X-ray diffraction showing peaks of different corroded phases.
(a)
(b)
(c)
(d)


## 3.4. Optical and SEM Microscopy Images

The microstructures by optical microscopy clearly show (Figure9) the corroded structure of steel with products of corrosion over it. The form of corrosion seems to be uniform, not localized. SEM images (Figure 10) distinctly reveal how the degree of degradation increases with presence of ions in the solutions from SO
4
2
- to SO
4
2
- + S2− to SO
4
2
- + S2− + Cl−. It is interesting to observe from the morphology of SEM image at higher magnification (Figure 11) that the corrosion has taken place at grain boundary as well as grain body but the attack at grain boundary is very prominent with sulphide (S) corrosion crack. The corrosion products of sulphide compounds as well as element sulphur are clearly revealed. The structure of SEM images shows almost catastrophic failure with the presence of minor and major cracks when the seawater is enriched with the presence of all three corrosive ions, SO
4
2
-, S2−, and Cl−. The morphology of SEM image analysis along with XRD is in complete agreement with the corrosion data of the polarization experiments and EIS.Figure 9
Optical microscopy images of corroded steel. (a) Na2SO4, (b) Na2SO4 + Na2S, and (c) Na2SO4 + Na2S + NaCl.Figure 10
SEM images of corroded steel (a) before corrosion, (b) in Na2SO4, (c) in Na2SO4 + Na2S, and (d) in Na2SO4 + Na2S + NaCl.Figure 11
SEM images of corroded steel (a) in Na2SO4, (b) in Na2SO4 + Na2S, and (c) in Na2SO4 + Na2S + NaCl.From (5)–(8), it is seen that SO
4
2
- is cathodically reduced to give rise to S2−. It is observed from the polarization curve (Figure 1) that the increase of SO
4
2
- concentration depolarizes the cathodic curves much more compared to anodic ones, shifting E
corr towards the negative potential. The release of S2− from the reaction produces corrosion products: iron sulfides (Fe
S
x) on carbon steel surface. They are nonstoichiometric iron sulfide films mainly composed of mackinawite and pyrrhotite Berner [21–26]. The black color of mackinawite phase is also seen as corrosion products in optical microstructures (Figures 9(a) and 9(b)).The deterioration of metal due to contact with S2− (H2S) and moisture is sour corrosion. The forms of sour corrosion are uniform (Figure 9(b)), pitting, and stepwise cracking (Figures 10(c) and 11(b)).The general equation of sour corrosion can be expressed as follows [21]:
(15)
S
2
-
+
2
H
+
=
H
2
S
(
aq
)
E
=
0
.
097
V
versus
SCEHydrogen sulphide dissociates to produce proton and bisulphide as described [22] by the following equations:
(16)
H
2
S
(
aq
)
=
H
+
+
H
S
-
K
=
9.1
×
10
-
8
H
S
-
=
H
+
+
S
2
-
K
=
9.1
×
10
-
12This reaction scheme shows that the presence of hydrogen sulfide can contribute to the concentration of sulfide at the surface by dissociation rather than charge exchange with the surface. The sulfide concentration at the surface is, therefore, dependent on the concentration of aqueous hydrogen sulfide in the electrolyte as well as the reduction processes of sulfate.H2S exhibits the different role in anodic process of carbon steel depending on the pH value in the solutions. The local supersaturation of Fe
S
x could be formed on the carbon steel surface via the following reaction, with the nucleation and growth of one or more of the iron sulfide, mackinawite:
(17)
H
2
S
+
Fe
+
H
2
O
⟶
FeS
x
+
2
H
+
H
2
OThe black corrosion products (FeS
x) formed on the steel surface in the H2S-containing solutions could be observed (Figure 9(b)). The addition of chloride to the corrosion system did not exhibit any localized corrosion; rather it drastically increased the i
corr values and shifted E
corr towards the negative potential (Figures 3 and 4), depolarizing the anodic reactions. The increase in i
corr with Cl addition seems to have modified the anodic substrate area (Figures 9(c) and 10(d)) and has enhanced the exchange current density for the iron oxidation process.


## 4. Conclusion

All three corrosive ionsSO
4
2
-, S2−, and Cl− have a strong effect on increasing the corrosion rate of carbon steel.Cathodic reduction ofSO
4
2
- generates elemental S or S2− ions, in addition to S2− from H2S in oil. The species cause major corrosion with formation of FeS
x as corrosion products. The attack is found at grain boundary with sulphide cracking as well as some grain body degradation. The effect of addition of Cl− is the increase of i
corr values by hundreds of times possibly due to enhancement of exchange current density of the anodic reactions.



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*Source: 628505-2014-12-17.xml*