Xi Chena,
Hongyan Liua,
Xiang Suna,
Botao Zanb and
Meisheng Liang*a
aCollege of Environmental Science and Engineering, Taiyuan University of Technology, Taiyuan, China. E-mail: liangmeisheng@tyut.edu.cn
bUniversity of Washington, Seattle, 98105, WA, USA
First published on 2nd December 2021
In order to transport reclaimed water safely through stainless steel (SS) heat-supply pipeline networks during their idle period, one must understand the degree to which chlorine in reclaimed water is corrosive to SS. In this study, electrochemical methods were used to evaluate the corrosion resistances of two types of SS materials, AISI 304 and AISI 316, in simulated reclaimed water at chloride concentrations of 25 to 400 mg L−1, which are similar to those present in practice. The differences in corrosion resistance between the two types of SS material were investigated using electrochemical impedance spectroscopy (EIS) and potentiodynamic polarization tests (Tafel curves). The passivation layers on the two types of SS exhibited obvious similarities under several experimental conditions. However, EIS, polarization resistance, effective capacitance, Tafel curve, and Scanning Electron Microscope (SEM) data showed that AISI 316 has better corrosion resistance than AISI 304. The corrosion behaviours could be described as a series of reactions between Fe, Cr, and H2O that generate several precipitated products such as Fe2O3, Cr2O3, FeOOH, and CrOOH.
The electrochemical technique is a reliable and accurate method of studying the corrosion process. The technique utilises the principle of electrochemical corrosion to simulate the real electrochemical reaction on the metal surface, and then uses a computer to obtain corresponding parameters so that one can analyse the corrosion process and benefit from the advantages of high sensitivity, simple operation, and easy access. Of the several electrochemical techniques available, potentiodynamic polarization tests and electrochemical impedance spectroscopy (EIS) are common, non-disruptive tools for investigating the states of the passivating films formed on metal surfaces.
Over the past few years, numerous studies have considered the characteristics and mechanisms of corrosion of iron and steel components.20–22 Well-known studies have focused on corrosion products and scale within water supply system pipelines23,24 because of reports that corrosion scale inside pipelines is related to interactions between the pipeline material and water that contains dissolved corrosive substances.25–27 In addition, the type of pipeline corrosion must be considered. Corrosion is typically classified as either uniform or localised.28 Localised corrosion (including pitting corrosion, crevice corrosion, intergranular corrosion, and stress corrosion cracking) can affect the SS pipeline service life greatly.29,30 However, few studies have focused on the corrosion of pipelines in heat supply networks. And there was an idea that what would happen if heating pipes were used to transport reclaimed water during its idle period. Some unpredictable phenomena may occur during transport due to the complex components of reclaimed water. Then the causes and processes of the corrosion on the heating pipes must be studied due to the practical consideration. Cl− is significant factor in pipeline corrosion, but studies have focused mainly on the effects of seawater on steel-reinforced concrete and of desalinated seawater on water pipe systems. These studies are all aimed at high concentrations of Cl−, which have limited reference significance to corrosion driven by low-concentration Cl− in a reclaimed water pipeline system.
Based on this, we studied the corrosion behaviours of AISI 304 and AISI 316 in a simulated reclaimed water solution that contained Cl−. Chloride ion was provided via addition of sodium chloride (NaCl) at various concentrations. Based on the results of electrochemical tests and the influence of Cl− on SS passivation behaviours, we can provide a theoretical basis for the industrial application of SS heat-supply pipeline systems to the transport of Cl− containing reclaimed water during their idle period. Such information has practical application value.
Material | C | Mn | Si | P | S | Cr | Ni | Cu | Mo | N | Fe |
---|---|---|---|---|---|---|---|---|---|---|---|
AISI 304 | 0.042 | 1.06 | 0.47 | 0.033 | 0.004 | 18.02 | 8.02 | — | — | — | Balance |
AISI 316 | 0.017 | 1.310 | 0.562 | 0.029 | 0.002 | 16.60 | 10.01 | — | 2.01 | 0.014 | Balance |
Items | Value |
---|---|
Cl− (mg L−1) | 226.7 |
SO42− (mg L−1) | 300 |
HCO3− (mg L−1) | 320 |
Alkalinity (mg L−1) | 254 |
Hardness (mg L−1) | 670 |
Ca2+ (mg L−1) | 158.54 |
Mg2+ (mg L−1) | 59.63 |
pH | 7.24 |
DO (mg L−1) | 8.02 |
NH3–N (mg L−1) | 3.03 |
Total phosphorus (mg L−1) | 0.232 |
All electrochemical tests were performed using a conventional three-electrode configuration, with the processed AISI 304 and AISI 316 samples acting as working electrodes, an Ag/AgCl electrode as a reference electrode with the standard potential of 0.198 V (25 °C), and a graphite rod as the counter electrode. The test cell of the three-electrode configuration is shown schematically in Fig. 1. During the experiments, a CHI760E (Shanghai Chenhua Instruments) electrochemical workstation was used to perform the electrochemical tests. The morphologies of the two types of SS were observed using a scanning electron microscope (SEM, LYRA3, TESCAN) produced by TESCAN. Details of the electrochemical tests are shown in S1.†
In Fig. 2a and d, it can be seen clearly that the maximum phase angle is smaller than 90°. The phase angles (ϕ) are maintained at zero degrees under high-frequency conditions due to resistive behaviour, rather than a relaxation process. The phenomenon appears to present a capacitive-like behaviours, where the phase angle maximum is in the position of the medial frequencies. At the lowest values, the phase angle gradually approaches zero. This suggests that |Z| shown in Fig. 2c and f could be recognized as the characteristic resistance. The raw experimental results indicate that this system seems to be defined by a single resistance process.
A type of EIS spectrum, the Nyquist plot is drawn with the real part of Z (Zre) on the horizontal axis and the imaginary part of Z (Zim) on the vertical axis. The interfacial layer between the working electrode and the electrolyte is regarded as a type of circuit element. The imaginary part of the impedance is shown as a circular arc in the first quadrant of the impedance spectrum, and is known as the capacitive arc. In Fig. 2b and e, for the two samples, the radians of the curves present the similar trends in solutions with different chloride concentrations. The radius of the capacitive arc can reflect the status of charge transfer and can indirectly imply the corrosion resistance of the working electrode. Comparison of the Nyquist plots in Fig. 2b and e indicates that both SS materials produce imperfect semicircles without straight lines in the low-frequency range. The phenomenon could be explained as the incomplete diffusion of chloride.31 When the chloride concentration is increased, there is a remarkable increase in the diameter of the capacitive arc. This can be understood as a change in corrosion behaviour in the presence of chloride.32 The charge-transfer resistance also increases accordingly, resulting in the emergence of more stable passivation films with stronger corrosion resistance on both SS materials. Also, it can be seen clearly that the arc diameter of AISI 316 is larger than that of AISI 304. This indicates that AISI 316 has better corrosion resistance.
Fig. 2c and f show that the slope of the |Z|-frequency decreases as the chloride concentration increases. This suggests deviation from the ideal capacitor. This may be attributed to the irregular distribution of the applied potential, which results in the variations of time constants (related to the charge–discharge time of a capacitance).33 This may be caused by electrode surface irregularities, surface roughness, fractal surfaces, etc.
EIS analysis indicates that the electrode surface experiences periodic charging and discharging of the electric double layer. The former is called the non-Faraday process and the latter is called the Faraday process. The impedance of the electrode is equivalent to that of a circuit composed of the non-Faraday impedance (ZNF) and the Faraday impedance (ZF) in parallel. Of course, there is also a resistance between the reference electrode and the solution. This is shown in front of the parallel circuit and referred to as the solution resistance. Based on the analysis above, the impedance was fitted using the equivalent electrical circuit depicted in Fig. 3. Traditionally, a capacitor is used to measure the ZNF. When disturbed by a polarization potential or polarization current, the non-faradaic process from the double layer on the electrode surface is the same as the disturbance signal produced during charging and discharging. Thus, a constant-phase element (CPE) unit was used to account for the frequency dispersion observed via the disturbance signals. If diffusion and adsorption are ignored, ZF can be replaced by a polarization resistance (RP). The passivating film RP experienced by the current flow is related to the time constant (τ) presented at medium and low frequencies. Otherwise, the solution or electrolyte resistance between the reference and working electrodes is represented by RS.
Typically, a CPE is used to represent the non-ideal capacitance of the electrode when seeking to simulate a real capacitor. Its impedance is defined by the following equation:
(1) |
(2) |
[Cl−] (mg L−1) | RS (Ω cm2) | Error (%) | RP (MΩ cm2) | Error (%) | Y0 (μS cm−2 sn) | Error (%) | n | Error (%) | χ2 |
---|---|---|---|---|---|---|---|---|---|
AISI 304 | |||||||||
25 | 490 | 1.20 | 0.608 | 0.74 | 69.51 | 0.68 | 0.78 | 0.79 | 4.9 × 10−3 |
50 | 359 | 0.40 | 0.596 | 0.31 | 76.64 | 0.48 | 0.80 | 0.23 | 2.4 × 10−3 |
100 | 325 | 0.84 | 0.413 | 0.66 | 87.46 | 0.52 | 0.81 | 0.62 | 2.4 × 10−3 |
200 | 114 | 0.86 | 0.245 | 1.24 | 133.16 | 1.73 | 0.80 | 0.63 | 2.1 × 10−3 |
400 | 89 | 1.05 | 0.131 | 1.15 | 149.25 | 0.64 | 0.79 | 0.59 | 2.8 × 10−3 |
AISI 316 | |||||||||
25 | 442 | 1.20 | 0.765 | 0.39 | 54.62 | 1.96 | 0.78 | 1.08 | 8.1 × 10−3 |
50 | 336 | 1.06 | 0.672 | 1.09 | 77.47 | 1.70 | 0.79 | 0.95 | 7.0 × 10−3 |
100 | 217 | 0.74 | 0.396 | 0.47 | 86.05 | 1.36 | 0.82 | 0.63 | 3.1 × 10−3 |
200 | 137 | 0.84 | 0.327 | 0.34 | 88.51 | 1.25 | 0.79 | 0.52 | 1.9 × 10−3 |
400 | 115 | 1.02 | 0.172 | 1.29 | 107.81 | 1.69 | 0.78 | 0.66 | 2.6 × 10−3 |
We combine the EIS results in Table 3 with Fig. 2b and e to show that the phase angle peak shifts to lower frequency values. In addition, the capacitive region shrinks substantially when RS increases. One can conclude that the phase angle (ϕ) is calculated using arctan (Zim/Zre), where Zim and Zre are the imaginary and real parts of the impedance, respectively, and are represented using complex numbers. It can be seen from formula (2) that RP is contained exclusively in the impedance function. Thus, RP played an important role in the total impedance, and depended on the chloride concentrations.34
According to eqn (1), there is an obvious relationship between the CPE and the index n. When n equals zero, the CPE is equivalent to a pure capacitor. And the values of the capacitor could be determined by Y0. Then when n deviates from zero, the capacitance decreases accordingly. Hsu and Mansfeld35 proposed the concept of an effective capacitance (Ceff), which is calculated using eqn (3). It shows how the capacitance changes based on the chloride concentration.
Ceff = Y0(ωC)α−1 | (3) |
(4) |
The α in eqn (4) can be obtained using the following relations:36
Ecorr = A − BlogαCl− | (5) |
B = A − 2.303RT/αF | (6) |
Next, Ceff was calculated according to eqn (3). Comparison of the resulting values to Y0 in Fig. 5 indicates that there is a marked difference between the two parameters.
The Ceff of AISI 304 and AISI 316 from Fig. 4 are plotted separately and shown in Fig. S1.† The Ceff values of both SS samples exhibit similar trends when the chloride concentration changes. Their behaviours can be described using linear fits. In addition, Fig. S1† indicates that the Ceff of AISI 304 ranges from 200 to 330 μm cm−2, while that of AISI 316 ranges from 170 to 230 μm cm−2. Obviously, the Ceff of AISI 316 is consistently lower than that of AISI 304.
Fig. 4 Admittance (Y0) and calculated effective capacitance (Ceff) of AISI 304 and AISI 316 at different chloride concentration. |
Treating the capacitive system as a parallel plate capacitor allows the passivating film thickness (δ) to be estimated from Ceff using the following equation:
δ = ε0ε/Ceff | (7) |
Fig. 5 Calculated passive film thickness (δ) of AISI 304 and AISI 316 at different chloride concentration. |
As previously described, RP represents the electrical resistance of the passivating film. Fig. 6 shows the RP values of the two SS materials in simulated solutions with various chloride concentrations. RP decreases as the chloride concentration increases. Linear fitting indicates that the SS RP values and chloride concentration have a clear negative linear relationship. It is also noted that the corrosion resistances of these two SS materials decrease at the same rate with respect to the Cl ion concentration, although the resistance of AISI 316 is always higher than that of AISI 304. This phenomenon is consistent with previous studies regarding passivating film thicknesses. The results above demonstrate that the presence of chloride not only affects the corrosion resistance of SS but also affects the protective performance of the passivating film in its non-polarised state.
It also can be seen from Fig. 7(a) and (b) that all of the self-corrosion potentials of AISI 304 and AISI 316 move in the negative direction as the chloride concentration increases. Generally, the more negative the self-corrosion potential, the worse the corrosion resistance. There is an obvious negative movement of the self-corrosion potential at a chloride concentration of 400 mg L−1 in Fig. 7(a). This indicates that chloride enrichment can cause serious damage to the AISI 304 surface. For AISI 316, the change in the self-corrosion potential with the chloride concentration is smaller. That implies a stronger corrosion resistance due to the reduced chloride accumulation on the passive film. So, the passivating film was still effective to protect the metal materials.40
The relationships between Ecorr, Icorr, and the chloride concentration are reflected in Fig. 8, where the Ecorr values for the AISI 304 and AISI 316 electrodes are calculated using the cathodic and anodic Tafel slopes from the polarization curve. The corrosion current density (Icorr) is obtained based on the corrosion currents from the potentiodynamic polarization test. The relevant data from Fig. 8 are shown in Table S1.† It can be observed that the Ecorr values of the two SS materials decrease with the chloride concentration, while Icorr moves to the opposite side with the increase of Cl−. In other words, the Ecorr and Icorr values of the two SS materials have negative and positive linear relationships with the chloride concentration, respectively.
Previous studies indicate41 that RP is often inversely proportional to the current density a given Ecorr. The corrosion current density (Icorr) is related directly to the corrosion rate. Thus, the determination of Icorr can provide valuable information about the corrosion resistance in a specific environment. In Fig. 6 and 8, there is a clear negative linear relationship between RP and the chloride concentration but a positive relationship between Icorr and the chloride concentration. This is completely consistent with previous studies.42 Icorr also has substantial influence on the SS passivating film. The increased corrosion current density in the presence of chloride thins the passivating film, leading to further corrosion.
Comparison of the linear fit data from AISI 304 and AISI 316 in Fig. 8 allows one to determine whether Ecorr or Icorr depend on the chloride concentration. One can also determine that the R2 (linear correlation coefficients) of the AISI 304 are always higher than that of AISI 316. Based on this, it can be concluded that the polarization behaviour of AISI 304 is more closely linked to Cl− concentrations, and the passive film is likely to change in chloride. The results indicate that the stability of the AISI 304 passivating film is worse than that of the AISI 316 film. This indicates that AISI 304 is more susceptible to influence from chloride.
In the EDS analysis of AISI 316 shown in Fig. 9(c) and (d), the variation of Fe and O is similar to that of AISI 304, where the contents decreased when the sample was corroded. However, the chlorine contents are close (about 0.17 wt%) regardless of whether the AISI 316 is corroded or not. This is different with AISI 304, where the Cl content had a marked increase from 0.12 wt% to 27.36 wt% when the sample was corroded. The EDS analysis indicates that corrosion can occur as a reaction between Cl− and several components such as Fe, Cr, and O ions. Some reaction products tend to exist in free state, while others apt to aggregate around the corrosion areas. In addition, AISI 304 is more likely to be corroded due to Cl− enrichment on its surface.
Fe = Fe2+ + 2e− | (8) |
Cr = Cr3+ + 3e− | (9) |
In a chloride-rich solution, the increased Fe2+ and Cr3+ in the etch pits can cause continuous migration of chloride to maintain a relatively neutral solution.45 The solution becomes acidic and its oxidation state changes such that some Fe2+ can be oxidised to Fe3+. Then, metal chloride is generated due to the combination of Fe2+ and Fe3+ with chloride ion.46 Next, these metal chlorides are hydrolysed into metal hydroxides and hydrogen ions by water. This series of reactions accelerates corrosion development and can be explained using the following chemical formulas:
Cl− + H2O = HClO + H+ + 2e− | (10) |
Fe2+ + 2Cl− = FeCl2 | (11) |
Cr3+ + 3Cl− = CrCl3 | (12) |
2FeCl2 + 2HClO = 2FeCl3 + H2O | (13) |
FeCl2 + 2H2O = Fe(OH)2 + 2H+ + 2Cl | (14) |
FeCl3 + 3H2O = Fe(OH)3 + 3H+ + 3Cl− | (15) |
CrCl3 + 3H2O = Cr(OH)3 + 3H+ + 3Cl− | (16) |
Some of the Fe(OH)2 produced via eqn (14) can dehydrate and become FeO as follows:
Fe(OH)2 = FeO↓ + H2O | (17) |
The Fe(OH)3 produced via eqn (15) and Cr(OH)3 produced via eqn (16) can be converted into FeOOH and CrOOH via dehydration. Then, FeOOH and CrOOH continue to dehydrate and generate Fe2O3 and Cr2O3. Fe2O3, Cr2O3, FeOOH, and CrOOH precipitate as corrosion scale and become the main components of the corrosion products. The related chemical reactions can be depicted as follows:
Fe(OH)3 = FeOOH↓ + H2O | (18) |
2FeOOH = Fe2O3↓ + H2O | (19) |
Cr(OH)3 = CrOOH↓ + H2O | (20) |
2CrOOH = Cr2O3↓ + H2O | (21) |
In summary, the occurring of corrosion is mainly processed as the formation of corrosion pits on the passive film. The reaction results in a continuous accumulation of corrosion products due to the invading of chlorine. Electrochemical reactions between the iron and chromium phases generated play crucial roles in the corrosion process, where the absence of oxygen suppresses AISI 316 corrosion. The results indicate that AISI 316 pipelines can provide a reliable means of delivering reclaimed water. The electrochemical analysis indicates that the bottom of the pit can be seen as the anode and the passivating film on the SS surface can be seen as the cathode. Electrons are transferred directly from the anode to the cathode on the SS substrate when a chloride-containing solution is used as the electrolyte. Finally, corrosion products with a wavy appearance formed under the action of water pressure.
Footnote |
† Electronic supplementary information (ESI) available. See DOI: 10.1039/d1ra06695a |
This journal is © The Royal Society of Chemistry 2021 |