Near surface pH measurements in aqueous CO2 corrosion
Introduction
The formation and development of corrosion product films on a metal surface is essential to corrosion science. A “protective film” can cause a significant reduction in the corrosion rate by blocking the underlying steel from further dissolution. However, local defects or damage in the corrosion product film/scale covered surface can lead to severe localised corrosion by exposing the underlying metal to the aggressive corrosion environment [1]. Over the years, intensive research [[2], [3], [4], [5], [6]] has been carried out offering insight into the various complex processes occurring in CO2 corrosion. These studies show that CO2 corrosion product films can be affected by many factors such as temperature, pressure, flow rate and pH value. Among these parameters, it has been shown both experimentally and computationally that pH has a strong influence on the corrosion rate [3,[7], [8], [9]]. The most important effect of pH is indirect and relates to how pH changes conditions for formation of iron carbonate (FeCO3) scales and can have a profound effect on how effectively the film is able to limit corrosion kinetics on the underlying steel.
The formation of FeCO3 on a metal surface in a CO2 environment takes place when the concentrations of iron ions (Fe2+) and carbonate ions (CO32−) exceed the solubility product (Ksp) of FeCO3 in a solution [10]:
The nature, morphology and protection offered by the FeCO3 precipitation process is dependent on the environmental conditions which influence the formation of CO2 corrosion product films primarily by changing FeCO3 supersaturation (SS) [11]. The supersaturation level which is deemed to be the driving force behind the precipitation process [7,8] is defined as:Where [Fe2+] and [CO32−] (in mol/m3) are the concentrations of ferrous and carbonate ions, respectively. Ksp (in mol2/m6) is the solubility product of FeCO3, which is a function of ionic strength and temperature [12].
Solution pH affects the supersaturation of FeCO3 due to its impact on the carbonate ion concentration. At high solution pH, high concentrations of CO32− result in fewer Fe2+ ions being required to exceed the solubility product of FeCO3 and generate significant levels of precipitation [2]. Through consideration of the equilibrium and dissociation chemical reactions that take place in a CO2 corrosive environment, referenced in Nordsveen et al. [13], the CO32− concentration and concentration of other ions in the system as a function of pH is determined and is shown in Fig. 1. The values are calculated for a temperature of 80 °C and atmospheric total pressure.
Fig. 1 shows that the concentration of CO32− increases by over an order of magnitude with increasing pH meaning much less Fe2+ ions are needed to reach the critical SS required for substantial crystal nucleation and growth. The supersaturation of FeCO3, for a constant Fe2+ ion concentration (0.001 M), is calculated for varying solution pH and is included in Fig. 1. This calculation is used to clearly indicate the indirect impact of pH on the SS of FeCO3. Furthermore, the figure is annotated to indicate the CO32− ion concentration and SS value at both pH 6 and pH 6.6.
Experimental evidence of the influence of pH on FeCO3 supersaturation and hence the protectiveness of the developed film is clearly shown in a study by Sun et al. [14]. The work demonstrated that under conditions of pH 6 at 80 °C in a 0.54 bar CO2 saturated 1 wt% NaCl brine with an addition of 50 ppm Fe2+, a low bulk SSFeCO3 was obtained resulting in the formation of a porous, detached and poorly protective FeCO3 film forming on the carbon steel surface. Higher pH values of 6.6, under the same operating conditions, resulted in a higher bulk SSFeCO3, faster precipitation kinetics and formation of a more protective FeCO3 film. The obtained corrosion rate results for varying bulk SSFeCO3 is shown in Fig. 2. Other similar studies have also demonstrated that protective FeCO3 formation is accelerated/enhanced at higher solution pH [7,8,15,16].
One main limitation within most experimental studies in literature is that the characteristics of FeCO3 precipitation is studied as a function of bulk solution properties. It is well understood amongst researchers [[17], [18], [19]] that the local surface chemistry conditions can be very different than those in the bulk solution due to electrochemical surface processes that result in metal dissolution (corrosion) and deposition. This has been further illustrated with the aid of mathematical modelling based on thermodynamic, kinetic and transport theories providing a numerical quantification of surface conditions [13,20,21]. However, difficulties with probe design and development limit the accurate measurement of properties at the near surface region of a corroding surface.
For varying research topics, direct [22,23] and indirect measurement [24,25] methods have been designed to measure the surface pH. The most recent and relevant study was carried out by Han et al. [17] where a mesh capped probe was designed for direct pH measurements on an actively corroding surface. The probe design consists of a flat sensor pH probe with a tip which is adhered to a mild steel mesh allowing the surface pH to be monitored during the corrosion of the mesh. The design was initially suggested by Romankiw [22] for electrolysis systems. The study monitored the surface pH for varying temperature (25 °C and 80 °C) and solution pH (pH = 4, 5, 6 and 6.6) in a CO2 corrosion environment. Higher surface pH deviation from the bulk was observed at higher temperatures as well as at lower bulk pH conditions. The observed results provided an experimental observation that coincides with the theoretical predictions. However, certain aspects that are believed to be essential to corrosion science was not considered within the research article. The study was limited to a series of short tests and did not take into account the formation of FeCO3 that may take place on the steel mesh under the conditions of high temperature and pH studied. The duration of the experiments conducted were noted to be 10 h. Previous research [8] has shown that the formation of FeCO3 may be expected for some of the conditions studied by Han et al. [17] however it may have not been sufficiently “protective” within the short duration of exposure to disrupt the stable measurements obtained and cause a change in surface pH. In order to study the effect of a protective film on the surface pH, the study artificially deposited inert sand (100–500 μm in size) and glass beads (50–80 μm in size) on the mild steel mesh surface to simulate a deposit layer of varying porosity. Both were deposited in the form of a layer of 5 mm in thickness on the mild steel mesh resulting in diffusion affected corrosion reactions. The meshed pH electrode measured the surface pH under the artificially deposited layer (under-deposit pH). The results showed high values of surface pH and was observed to be higher for the less porous glass bead deposit (30% porosity) compared with the more porous sand particle deposit layer (40% porosity). Within the research study by Han et al. [17], the unique experimental method provided an effective and extensive analysis of the measurement of surface pH under an array of conditions. However, it may be argued that the lack of a link with the corrosion rate limits the realistic implications of the study.
The focus of this work is to design and employ a flexible surface pH probe based on that by Han et al. [17] and Romankiw [22]. The probe shall be used to study the surface pH of a metal mesh under conditions of high pH and temperature over a period of 12 days. The research aims to further understand the development of the surface pH as a function of the protectiveness of the corrosion product scale. The study is carried out in conjunction with electrochemical measurements and surface characterisation techniques to provide a link between pH, the mild steel corrosion rate and the protective properties of the corrosion product layer.
Section snippets
Sample preparation
API 5L X65 carbon steel specimens were used in this study for electrochemical measurements, mass loss measurements and surface analysis. The steel was introduced in each test in the form of a cylindrical rod (surface area = 6.4 cm2) to function as a working electrode and rectangular coupons (surface area = 4.0 cm2) to be extracted for ex-situ surface analysis and mass measurements. Prior to each experiment, the specimens were polished sequentially with 320 and 600 grit silicon carbide (SiC)
Literature comparison of surface pH measurements
Initial experiments were conducted to compare with results reported by Han et al. [17] to establish confidence in the experimental procedure used. The experiments were similarly conducted over a period of 10 h at conditions of 80 °C, pCO2 0.54 bar, 1 wt% NaCl and bulk pH of 4, 6, 6.6. Fig. 6 shows the results obtained in the form of a bar graph annotated with a dotted line to clearly indicate the bulk pH. Exp_IFP is used to represent the results obtained within this study and Exp_Han represents
Conclusion
In the following research, the effect of surface pH on the formation of a protective corrosion layer in mild steel CO2 corrosion conditions has been studied. A mesh-based surface pH probe was mounted to attempt the direct measurement of surface pH for tests conducted at 80 °C and two varying conditions of pH of 6 and 6.6. The following conclusions can be drawn from the results and discussion of this work:
- •
A more protective corrosion film is observed to have developed at pH 6.6 in comparison with
Acknowledgements
The authors would kindly like to thank Alexandre Bonneau for his active participation in the implementation of the experimental setup and the contribution of the IFPEN analysis department in surface characterisation, specifically Florent Moreau and Nathalie Crozet.
References (29)
Key issues related to modelling of internal corrosion of oil and gas pipelines - a review
Corrosion Sci.
(2007)- et al.
In situ SR-XRD study of FeCO3 precipitation kinetics onto carbon steel in CO2-containing environments: the influence of brine pH
Electrochim. Acta
(2017) - et al.
The early stages of FeCO3 scale formation kinetics in CO2 corrosion
Mater. Chem. Phys.
(2018) - et al.
The growth mechanism of CO2 corrosion product films
Corrosion Sci.
(2011) - et al.
The effect of temperature and ionic strength on iron carbonate (FeCO3) solubility limit
Corrosion Sci.
(2009) - et al.
Effect of interfacial pH on the reduction of oxygen on copper in neutral NaClO4 solution
J. Electroanal. Chem.
(1995) - et al.
Roles of passivation and galvanic effects in localized CO2 corrosion of mild steel
NACE Corrosion
(2008) - et al.
Carbon dioxide corrosion in oil and gas production—a compendium
Corrosion
(2003) Mechanism of protective film formation during CO2 corrosion of carbon steel
NACE Corrosion
(1998)- et al.
Algorithm of the protectiveness of corrosion layers 1-protectiveness mechanisms and CO2 corrosion prediction
NACE Corrosion
(2010)
Carbonic acid corrosion of steel
Corrosion
Effect of pH on CO2 corrosion of mild steel at elevated temperatures
NACE Corrosion
Internal corrosion of carbon steel pipelines for dense-phase CO2 transport in carbon capture and storage (CCS) – a review
Int. Mater. Rev.
A mechanistic model for carbon dioxide corrosion of mild steel in the presence of protective iron carbonate films - Part 1: theory and verification
Corrosion
Cited by (29)
Effect of alloying (Cr, Mo, and V) on corrosion behaviors of API-grade steel in CO<inf>2</inf>-saturated aqueous solutions with different pH
2024, Journal of Industrial and Engineering ChemistryThe role of Cr content on the corrosion resistance of carbon steel and low-Cr steels in the CO<inf>2</inf>-saturated brine
2023, Petroleum ScienceCitation Excerpt :The calculated Pourbaix diagram agreed with the XRD results in Fig. 5, where FeCO3 was identified as the main corrosion products for X65 steel. The pH value at steel surface has a significant effect on the formation kinetics of the corrosion products (De Motte et al., 2018). In our research, the pH values of the solution close to the steel surface were monitored to analyse the surface pH variations roughly.
Galvanic effects induced by siderite and cementite surface layers on carbon steel in aqueous CO<inf>2</inf> environments
2022, Corrosion ScienceCitation Excerpt :Alternative mechanisms have been proposed, whereby galvanic interaction is initiated as a result of local differences in occluded electrolyte chemistry (e.g. pH, Fe2+ concentration) underneath FeCO3 crystals and uncovered regions of the steel surface, in a manner similar to under deposit corrosion [6]. Higher local surface pH (compared to bulk solution pH) has also been suggested to initiate pseudo-passivation effects, whereby the carbon steel’s open circuit potential (OCP) can increase dramatically during the FeCO3 layer growth process, often observed with the simultaneous formation of other surface layers, such as magnetite [24–26]. This increase in OCP has also been suggested as a cause of galvanic corrosion, with the surface layers formed acting as the net cathode [27].