The Effects of pH Values on Functional Mechanisms of Nitrite Anions for Q235 Carbon Steels in 0.01 mol L^-1 NaNO₂-HCl Solutions

Abstract

For Q235 carbon steels in 0.01 mol L^-1 NaNO₂-HCl solutions with different pH values, the effects of pH values on the functional mechanisms of nitrite anions (NO₂^-) were studied. In the pH 1 and pH 2 solutions, the Q235 steels showed the electrochemical behavior of activation, and uniform corrosion (UC) was the main corrosion type on the Q235 surface. The presence of NO₂^- did not affect the electrochemical behavior and the corrosion type but only accelerated the anodic reaction of Fe oxidation. In the pH 3 and pH 4 solutions, the Q235 steels presented the electrochemical behavior of activation-passivation transition, and intergranular corrosion (IGC) occurred on the Q235 surface. The cathodic reaction of NO₂^- reduction resulted in the transition of electrochemical behavior from activation to passivation and the change of corrosion type from UC to IGC. In the pH 5 and pH 6 solutions, the Q235 steels exhibited the electrochemical behavior of self passivation-pitting, and pitting corrosion (PC) was present on the Q235 surface. The strong oxidability of NO₂^- played a critical role in the formation of γ-Fe₂O₃ passive film on the Q235 surface under the combined action of Fe²⁺ and NO₂^-.

Keywords:
Q235 carbon steel; pH value; NO₂^-; corrosion; passivation; polarization

Introduction

Carbon steels are used in the different fields of production and living widely,^1-3 but it is unavoidable that the application and development of carbon steels are limited by the disadvantage of corrosion and failure.^4-6 For carbon steels, the addition of inhibitors into service environments is one of main methods to decrease the corrosion rate,⁷ and nitrite anions (NO₂^-) are kind of effective inhibitors to restrain the corrosion process.⁸

At present, the studies on the inhibitive effect and mechanism of NO₂^- for carbon steels are mainly focused on alkaline and neutral media, particularly on the corrosion environments of reinforced concrete^9-11 and chloride.^12-14 It is generally accepted that in alkaline and neutral media, the presence of NO₂^- promotes the surface passivation of carbon steels, which is attributed to the mechanism of NO₂^- for repairing the defects in the air-formed oxide film and making the oxide film to grow and re-arrange towards a regular passive film.^8,11,13 However, in acidic media, the related studies involving NO₂^- are relatively few, and the present studies are summarized as follows. In carbon dioxide (CO₂) corrosion environments, Zhou et al.^15-18studied the influence of NO₂^- on the corrosion / passivation behavior of Q235 carbon steel in CO₂ saturated solution (pH 3.7) in detail.The Q235 steel presented the electrochemical behavior of activation in CO₂ saturated solution without NO₂^-;¹⁵ after the addition of NO₂^-, the electrochemical behavior transferred from activation to anodic passivation, and the critical NO₂^- concentration for the stable passivation was approximately 0.05 mol L^-1;¹⁶ intergranular corrosion (IGC) was observed on the surface of Q235 carbon steel when the Q235 steel was polarized into activation-passivation potential region with a low potential scanning rate;¹⁷ the occurrence of IGC was very closely associated with the electrochemical behavior of activation-passivation transition, which was resulted from the synergetic mechanisms of CO₂ and NO₂^-.¹⁸ In other acidic media, Zuo et al.¹⁹ studied the combined influences of NO₂^- and thioureido imidazoline (TAI) on the passivation behavior and the pitting corrosion (PC) of X70 carbon steels in acidic NaCl solution (pH 5.5) and reported that the mechanisms of NO₂^- and TAI were both interactive and superimposed, and the addition of NO₂^- was beneficial to restrain the initiation and propagation of PC. Nevertheless, the detailed mechanism of NO₂^- was not discussed further. Garces et al.²⁰ studied the influence of NO₂^- on the propagation of PC for the corrugated steel bar in simulated pit solution (pH 1.46-6.38). The authors reported that the addition of NO₂^- showed a limited inhibition for the pit propagation, but the excessive addition even increased the uniform corrosion (UN) rate. However, due to the complicated component of simulated pit solution, the mechanism of NO₂^- was not completely clear.

From the above statements, although the studies about the mechanism of NO₂^- for the corrosion and passivation of carbon steels in acidic media are present, the pH values of acidic media are relatively single and not systematic. Therefore, it is necessary to carry out the detailed discussion for the mechanism of NO₂^- in the entire acidic pH range. At the same time, in our previous study,⁸ it was reported that the critical NO₂^- concentration of stable passivation for the Q235 steel in pure nitrite solution was 0.01 mol L^-1. Based on this result, in this work, diluted hydrochloric acid is introduced into 0.01 mol L^-1 NaNO₂ solution to adjust pH value, and 0.01 mol L^-1 NaNO₂-HCl solutions with different pH values are obtained. Further, the effects of pH values on the functional mechanisms of NO₂^- for Q235 carbon steels in the above solutions are studied by electrochemical measurements and microstructure observations, and the related mechanisms of electrochemical behavior and localized corrosion are also discussed.

Experimental

The tested material was Q235 carbon steel with the following chemical composition (wt.%): C, 0.160; Mn, 0.530; Si, 0.300; S, 0.045; P, 0.015, and Fe, 98.950. Samples were manually abraded up to 1000 grit with SiC abrasive papers, rinsed with de-ionized water and degreased in alcohol.

The tested electrolyte was 0.01 mol L^-1 NaNO₂-HCl solutions with different pH values which were adjusted to acidic range from pH 1 to 6 with the introduction of diluted hydrochloric acid into 0.01 mol L^-1 NaNO₂ solution.

The electrochemical measurements of polarization curve, electrochemical impedance spectroscopy (EIS) and Mott-Schottky plot were carried out using a CS350 electrochemical workstation (China). A typical three electrode system was applied for all the electrochemical measurements. The system was composed of a saturated calomel electrode (SCE) as reference electrode, a platinum sheet as counter electrode and a Q235 sample as working electrode. Before each electrochemical test, the working electrode was immersed in the corresponding tested electrolyte for a certain period of time until the open circuit potential (OCP) was stable. In the polarization curve test, the potential scanning rate was 0.1 mV s^-1, and the potential scanning range was from -0.3 V_OCP to the potential value corresponding to the objective electrochemical characteristic. In the EIS test, a perturbation potential of 10 mV amplitude was applied in the frequency range from 10⁵ to 10^-2 Hz. In the Mott-Schottky plot test, the potential scanning rate was 5.0 mV s^-1, and the potential scanning range was from -0.2 to 1.2 V_SCE. All of the electrochemical measurements were carried out at 25 ºC, which was controlled with an electro-thermostatic water bath.

The surface morphologies were observed by a SU1510 scanning electron microscope (SEM) instrument (Japan), and the surface composition was detected by a Kevex SuperDry energy dispersion X-ray spectroscopy (EDS) instrument attached on the SEM system.

Results and Discussion

Electrochemical behavior and corrosion type

Figure 1 shows the polarization curves and the EIS of Q235 samples in 0.01 mol L^-1 NaNO₂-HCl solutions with different pH values. From Figure 1a, the effects of pH values on the electrochemical behaviors are very significant: the Q235 samples presented the electrochemical behaviors of activation, activation-passivation transition and self passivation-pitting in the solutions with pH 1 and 2, pH 3 and 4, and pH 5 and 6, respectively. It may suggest the different mechanisms of NO₂^- for Q235 carbon steels in acidic pH range. At the same time, under the different electrochemical behaviors, the effects of pH values on the electrochemical parameters, including corrosion potential (E_corr), corrosion current density (i_corr), activation-passivation transition potential (E_trans), passive current density (i_pass) and pitting potential (E_pit), are also prominent.

Figure 1
Polarization curves and EIS of Q235 samples in 0.01 mol L^-1 NaNO₂-HCl solutions with different pH values: (a) polarization curves and (b) EIS.

Table 1 lists the effects of pH values on the electrochemical behavior and the electrochemical parameter value. From Table 1, with the increase of pH value, the E_corr value moves to the positive direction and the i_corr value decreases obviously, indicating the decreased rate of UC with the increased pH value.²¹ Similar results are also confirmed by the EIS data, which will be discussed later. Besides, in the solutions from pH 3 to 6, under the electrochemical behaviors of activation-passivation transition and self passivation-pitting, the negative direction of E_trans and the decrease of i_pass are present with the increase of pH value, suggesting that the passivation occurred in the solution with high pH value is easier than that in the solution with low pH value.

Table 1
Effects of pH values on electrochemical behavior and electrochemical parameter value

pH value	Electrochemical behavior	Ecorr / VSCE	icorr / (A cm-2)	Etrans / VSCE	ipass / (A cm-2)	Epit / VSCE
1	activation	-0.61	4.55 × 10-3	-	-	-
2	activation	-0.53	1.69 × 10-3	-	-	-
3	activation-passivation	-0.47	3.23 × 10-4	0.04	2.91 × 10-5	-
4	activation-passivation	-0.39	7.81 × 10-5	-0.11	4.92 × 10-6	-
5	self passivation-pitting	-0.25	3.25 × 10-6	-	3.25 × 10-6	0.62
6	self passivation-pitting	-0.11	1.75 × 10-6	-	1.75 × 10-6	0.76

• E_corr: corrosion potential; i_corr: corrosion current density; E_trans: activation-passivation transition potential; i_pass: passive current density; E_pit: pitting potential.

From Figure 1b, all of Nyquist plots for the EIS are composed of only depressed capacitive loop at the tested frequency range, which was independent on the pH values. It was reported that the characteristic of capacitive loop reflected the corrosion resistance of surface protection film on metals and alloys.¹⁶ Figure 1b illustrates that the radius of capacitive loop enlarges with the increase of pH value, indicating that the corrosion resistance of surface protection film formed in the high pH solution is greater than that formed in the low pH solution, which is in agreement with the results of E_corr and i_corr. Further, in order to confirm the above discussion, the equivalent electrical circuit (EEC) fitting is also performed. According to the Nyquist plots shown in Figure 1b and the previous study,⁸ the EEC model shown in Figure 2 is applied to fit the EIS, in which R_S represents the solution resistance, and R_f and CPE_f represent the resistance and the capacitance of surface protection film, respectively.

Figure 2
Equivalent electrical circuit model.

Table 2 lists the calculated values of R_f from the EEC fitting. From Table 2, the R_f value increases with the increased pH value, confirming the faster rate of UC in the low pH solution than in the high pH solution.

Table 2
Calculated values of surface protection film resistance from EEC fitting

pH value	Rf / (Ω cm2)
1	1750.85
2	1954.58
3	2091.90
4	2162.67
5	2326.45
6	2415.71

• R_f: resistance of surface protection film.

Figure 3 shows the surface SEM morphologies of Q235 samples in 0.01 mol L^-1 NaNO₂-HCl solutions with different pH values when the values of anodic current density in the polarization curve tests reach 0.1 A cm^-2. From Figures 3a and 3b, except some parallel scratches attributed to the mechanical action of abrasive paper, no localized corrosion feature is observed on the sample surface, which is consistent with the results shown in Figure 1a that the Q235 steels showed the electrochemical behavior of activation in the pH 1 and 2 solutions. Further, the scratches shown in Figure 3b is more obvious and abundant than those shown in Figure 3a, which is due to the dissolution rate of Q235 carbon steel is quicker in the pH 1 solution than in the pH 2 solution, confirmed by the values of anodic current density shown on the polarization curves in Figure 1a.

Figure 3
Surface SEM morphologies of Q235 samples in 0.01 mol L^-1 NaNO₂-HCl solutions with different pH values when values of anodic current density in polarization curve tests reach 0.1 A cm^-2: pH (a) 1, (b) 2, (c) 3, (d) 4, (e) 5 and (f) 6.

From Figures 3c and 3d, obvious corrosion dissolution along grain boundaries is observed on the sample surface, indicating the occurrence of IGC for the Q235 steels in the pH 3 and 4 solutions. Similar results were also reported in our previous study: for Q235 carbon steel in NaNO₂-CO₂ solution with 0.01 mol L^-1 NO₂^- and pH 3.7, the occurrence of IGC was observed on the Q235 surface when the Q235 steel was polarized into activation-passivation potential region.¹⁷ From Figure 1a, the electrochemical behavior of activation-passivation transition is also present when the Q235 steels were polarized in the pH 3 and 4 solutions. Therefore, by referring to the previous study,¹⁷ the mechanisms of NO₂^- for the electrochemical behavior of activation-passivation transition and the occurrence of IGC can be clarified, which will be discussed later.

From Figures 3e and 3f, for the Q235 steels in the pH 5 and 6 solutions, the presence of corrosion pits is observed on the sample surface obviously, indicating the occurrence of PC. It is in agreement with the results shown in Figure 1a that the electrochemical behavior of self passivation-pitting is present on the polarization curves in the pH 5 and 6 solutions. Further, EDS analysis revealed that the elements of Mn, S and Cl were present within each pit. It is generally accepted that for carbon steels in chloride solutions, the initiation and propagation of PC is very closely related to the adsorption of Cl^- at MnS inclusions.^22-24 Besides Cl^-, NO₂^- is responsible for the formation of passive film on the surface of carbon steels,²⁵ which also plays a critical role in the occurrence of PC.

From the results shown in Figures 1 and 3, for Q235 carbon steels in 0.01 mol L^-1 NaNO₂-HCl solutions, the effects of pH values on the electrochemical behavior and the corrosion type are very prominent, which are list in Table 3. The above results also suggest the different mechanisms of NO₂^- for carbon steels in the entire acidic pH range. The effects of pH values on the functional mechanisms of NO₂^- for the Q235 steels will be discussed as follows.

Table 3
Effects of pH values on electrochemical behavior and corrosion type for Q235 carbon steels in 0.01 mol L^-1 NaNO₂-HCl solutions

pH value	Electrochemical behavior	Corrosion type
1 and 2	activation	uniform corrosion (UC)
3 and 4	activation-passivation transition	intergranular corrosion (IGC)
5 and 6	self passivation-pitting	pitting corrosion (PC)

NO₂^- mechanism in 0.01 mol L^-1 NaNO₂-HCl solutions with pH 1 and 2

In order to understand the mechanisms of NO₂^- in 0.01 mol L^-1 NaNO₂-HCl solutions with pH 1 and 2, two Q235 samples were polarized in the pH 1 NaNO₂-HCl solution and the pH 1 pure HCl solution, respectively.

Figure 4 shows the polarization curves of Q235 samples in the pH 1 NaNO₂-HCl solution and the pH 1 pure HCl solution. Both samples showed the same electrochemical behavior of activation in the corresponding tested solutions. However, it is noteworthy that at the same applied potential, the value of anodic current density for the Q235 sample in the pH 1 NaNO₂-HCl solution is greater than that in the pH 1 pure HCl solution, suggesting the mechanism of NO₂^- to accelerate the electrode process.

Figure 4
Polarization curves of Q235 samples in pH 1 NaNO₂-HCl solution and in pH 1 pure HCl solution.

For carbon steels in acidic media, the main anodic and cathodic reactions are as follows:

(1) $\mathrm{Fe}\to {\mathrm{Fe}}^{2+}+2e$

(2) $2H^{+}+2e\to H_2$

It was reported that the cathodic process was accelerated when NO₂^- was present in acidic media, which was due to the following cathodic reaction:²⁶

(3) ${\mathrm{NO}}_2^{-}+2H^{+}+e\to \mathrm{NO}+H_{2}O$

Because the equilibrium potential of NO₂^- reduction (equation 3) is more positive than that of H⁺ reduction (equation 2),²⁶ the cathodic process is accelerated derived from the addition of NO₂^-, further resulting in that the anodic reaction of Fe oxidation (equation 1) moves to the right direction. Therefore, the higher value of anodic current density for the Q235 steel is observed in the pH 1 NaNO₂-HCl solution than in the pH 1 pure HCl solution, as shown in Figure 4.

In 0.01 mol L^-1 NaNO₂-HCl solutions with pH 1 and 2, besides H⁺ and NO₂^-, the presence of Cl^- is not neglected, which may greatly affect the electrochemical behaviors of Q235 carbon steels.²⁷ In order to clarify the effect of Cl^-, the application of diluted nitric acid was performed to adjust the pH values of 0.01 mol L^-1 NaNO₂-HNO₃ solutions.

Figure 5 shows the polarization curves of Q235 samples in 0.01 mol L^-1 NaNO₂-HCl solutions and in 0.01 mol L^-1 NaNO₂-HNO₃ solutions with pH 1 and 2. From Figure 5, the Q235 samples showed the electrochemical behavior of activation-passivation-transpassivation when the solution acidity was adjusted with diluted nitric acid. The change of electrochemical behavior from the activation in the pH 1 and 2 NaNO₂-HCl solutions to the activation-passivation-transpassivation in the pH 1 and 2 NaNO₂-HNO₃ solutions confirms that the presence of Cl^- also plays a critical role in the electrochemical behavior and the corrosion type for the Q235 steels in 0.01 mol L^-1 NaNO₂-HCl solutions with pH 1 and 2.

Figure 5
Polarization curves of Q235 samples in 0.01 mol L^-1 NaNO₂-HCl solutions and in 0.01 mol L^-1 NaNO₂-HNO₃ solutions with pH 1 and 2.

Further, from Figure 5, besides on the polarization curves in the pH 1 and 2 NaNO₂-HNO₃ solutions, the electrochemical behavior of activation-passivation transition occurring at the potential value of 0 V_SCE is also observed on the polarization curve in the pH 2 NaNO₂-HCl solution. However, it is worth noting that the activation-passivation transition region is not complete, and the anodic current density increases suddenly once again after the applied potential exceeds 0 V_SCE. Therefore, it can be inferred that in the pH 1 and 2 NaNO₂-HCl solutions, in the potential range from E_corr to 0 V_SCE, the presence of H⁺ may dominate the anodic process of Q235 carbon steel; after the potential value of 0 V_SCE, the presence of Cl^- does it. Nevertheless, the detailed combined effects of H⁺ and Cl^- need to be studied further.

From the above results, for Q235 carbon steels in 0.01 mol L^-1 NaNO₂-HCl solutions with pH 1 and 2, the presence of NO₂^- do not affect the electrochemical behavior and the corrosion type but only accelerate the anodic reaction of Fe oxidation.

NO₂^- mechanism in 0.01 mol L^-1 NaNO₂-HCl solutions with pH 3 and pH 4

As shown in Figure 4, the Q235 steel showed the electrochemical behavior of activation in the pH 1 pure HCl solution, and the same electrochemical behaviors are also observed in pure HCl solutions from pH 2 to 6. In contrast, from Figure 1a, the Q235 steels presented the electrochemical behavior of activation-passivation transition in the pH 3 and 4 NaNO₂-HCl solutions. The significant change of electrochemical behavior is attributed to the presence of NO₂^-.

For Q235 carbon steels in 0.01 mol L^-1 NaNO₂-HCl solutions with pH 3 and 4, the electrochemical behavior of activation-passivation transition and the occurrence of IGC are present, which is similar to our previous study on the corrosion behavior of Q235 carbon steel in 0.01 mol L^-1 NaNO₂-CO₂ solution with pH 3.7.¹⁷ In order to confirm the similar mechanism of NO₂^-, or not, in the pH 3.7 NaNO₂-CO₂ solution and in the pH 3 and 4 NaNO₂-HCl solutions, the polarization curve test for the Q235 steel in the pH 3.7 NaNO₂-HCl solution is carried out, as shown in Figure 6.

Figure 6
Polarization curves of Q235 samples in 0.01 mol L^-1 NaNO₂-HCl solutions with pH 3, 3.7 and 4.

From Figure 6, besides the sudden increase of anodic current density in the stable passivation region due to the presence of Cl^-,²⁸ the polarization curve for the Q235 steel in the pH 3.7 NaNO₂-HCl solution exhibits the highly similar rule to that in the pH 3.7 NaNO₂-CO₂ solution.¹⁷ Further, the same electrochemical behavior is also observed on the polarization curves of Q235 carbon steels in the pH 3, 3.7 and 4 NaNO₂-HCl solutions. The above results indicate the similar mechanism of NO₂^- for Q235 carbon steels in NaNO₂-CO₂ solution and in NaNO₂-HCl solutions, which is discussed as follows.

Besides the cathodic reaction of NO₂^- reduction (equation 3), it was reported that the following cathodic reaction was present in acidic media:²⁹

(4) ${\mathrm{NO}}_2^{-}+e\to \mathrm{NO}+O^{2-}$

Further, it was reported that in the pH 3.7 NaNO₂-CO₂ solution, the equilibrium potential of equation 4 (0.715 V_SCE) was more positive than that of equation 3 (0.429 V_SCE) and that of equation 1 (-0.684 V_SCE), resulting in the following reaction spontaneously:¹⁷

(5) ${\mathrm{Fe}}^{2+}+{\mathrm{NO}}_2^{-}\to {\mathrm{Fe}}^{3+}+\mathrm{NO}+O^{2-}$

Therefore, for the Q235 steels in the pH 3, 3.7 and 4 NaNO₂-HCl solutions, the presence of equation 5 is responsible for the electrochemical behavior of activation-passivation transition, as shown in Figure 6. At the same time, due to the enrichment of Fe in grain interiors and the segregation of Si and Mn in grain boundaries, the occurrence of IGC is observed on the Q235 surface when the electrochemical behavior of activation-passivation transition is present,¹⁷ as shown in Figures 3c and 3d. In order to further confirm the same mechanism of NO₂^- in the pH 3.7 NaNO₂-CO₂ solution and in the pH 3 and 4 NaNO₂-HCl solutions, the application of SEM is performed to observe the Q235 samples polarized to different potentials in the pH 3.7 NaNO₂-HCl solution, and the detailed potentials are marked on the polarization curve, as shown in Figure 6.

From Figure 7a, when the Q235 sample was polarized to potential 1 (0 V_SCE), the occurrence of IGC is observed on the Q235 surface but with a moderate degree: only parts of grain boundaries are damaged and the attacked grain boundaries are discontinuous. Further, from Figures 7b and 7c, all of grain boundaries are damaged and the dissolved grain boundaries form a complete network when the Q235 samples were polarized to potential 2 (0.1 V_SCE) and potential 3 (0.2 V_SCE), and the IGC degree for the Q235 sample polarized to potential 3 is more serious than that polarized to potential 2. The IGC process of Q235 carbon steel in the pH 3.7 NaNO₂-HCl solution is consistent with that in the pH 3.7 NaNO₂-CO₂ solution, confirming the same mechanism of NO₂^-.

Figure 7
Surface SEM morphologies of Q235 samples polarized to different potentials in 0.01 mol L^-1 NaNO₂-HCl solution with pH 3.7: (a) potential 1 (0 V_SCE), (b) potential 2 (0.1 V_SCE) and (c) potential 3 (0.2 V_SCE).

However, it needs to clarify that in our previous study, it was reported that the occurrence of IGC was attributed to the combined effects of CO₂ and NO₂^-, and NO₂^- promoted the passivation on the surface of crystal grains but CO₂ induced the dissolution at the vicinity of grain boundaries.¹⁷ In this work, according to the results shown in Figures 6 and 7, it is H⁺, rather than CO₂, to cause the dissolution of grain boundaries.

From the above results, for Q235 carbon steels in 0.01 mol L^-1 NaNO₂-HCl solutions with pH 3 and 4, the cathodic reaction of NO₂^- reduction results in the transition of electrochemical behavior from activation to passivation and the change of corrosion type from UC to IGC.

NO₂^- mechanism in 0.01 mol L^-1 NaNO₂-HCl solutions with pH 5 and pH 6

For Q235 carbon steels in 0.01 mol L^-1 NaNO₂-HCl solutions with pH 5 and 6, the electrochemical behavior of self passivation-pitting and the occurrence of PC are present, as shown in Figures 1a, 3e and 3f. By contrast, the Q235 steels presented the electrochemical behavior of activation in pure HCl solutions with pH 5 and 6. The above results suggest the mechanism of NO₂^- during the process of PC.

It was reported that for the occurrence of PC on the surface of carbon steels, the formation of passive film on the steel surface and the presence of aggressive anions in the service environment were two essential factors.¹² In this work, for the Q235 steels in the pH 5 and 6 NaNO₂-HCl solutions, the above two factors are present.

In alkaline and neutral media containing NO₂^-, carbon steels usually shows the electrochemical behavior of self passivation⁸ and the γ-Fe₂O₃ passive film is formed on the steel surface,⁹ which is attributed to the following reaction:¹⁴

(6) $2{\mathrm{Fe}}^{2+}+2{\mathrm{OH}}^{-}+2{\mathrm{NO}}_2^{-}\to 2\mathrm{NO}+\gamma -{\mathrm{Fe}}_2{O}_3+H_{2}O$

From Figure 1a, the electrochemical behavior of self passivation is also observed on the polarization curves for the Q235 steels in pH 5 and pH 6 solutions before the applied potential is up to E_pit, indicating the occurrence of equation 6 on the Q235 surface. At the same time, the other factor of PC, aggressive Cl^-, is also present, which is introduced during the process of adjusting pH value with diluted hydrochloric acid. Therefore, the combined actions of passive film and aggressive Cl^- result in the electrochemical behavior of self passivation-pitting and the occurrence of PC, the mechanism of NO₂^- is attributed to its contribution for the formation of γ-Fe₂O₃ passive film on the Q235 surface.

However, as shown in Figure 1a and Table 1, the value of E_pit for the Q235 steel in the pH 5 solution is more negative than that in the pH 6 solution, which is due to the different concentrations of OH^- and Cl^- in the pH 5 and 6 solutions. Because of different amount of diluted hydrochloric acid to adjust pH value, the concentrations of OH^- and Cl^- in the pH 5 solution are lower and higher than those in the pH 6 solution, respectively.

On the one hand, the higher OH^- concentration in the pH 6 solution than in the pH 5 solution results in the different extent of equation 6 in the two solutions. It is inferred that the corrosion resistance of passive film formed in the pH 6 solution is better than that formed in the pH 5 solution, which can be confirmed by the film resistance and the film defect. From Table 2, the R_f value for the Q235 steel in the pH 6 solution is higher than that in the pH 5 solution, indicating that the corrosion resistance of passive film formed in the pH 6 solution is greater than that formed in the pH 5 solution.³⁰ Besides film resistance, the electrochemical test of Mott-Schottky plot is also performed to characterize the film defect.

Figure 8 shows the Mott-Schottky plots of Q235 samples in 0.01 mol L^-1 NaNO₂-HCl solutions with pH 5 and 6. From Figure 8, the slopes of straight line parts on the both Mott-Schottky plots show positive values, indicating that the passive film on the surface of Q235 carbon steels is an n-type semiconductor.³¹ For n-type semiconductors, the following equation can be applied to interpret Mott-Schottky plot:

Figure 8
Mott-Schottky plots of Q235 samples in 0.01 mol L^-1 NaNO₂-HCl solutions with pH 5 and 6.

(7) $\frac{1}{C_{\mathrm{sp}}^2}=\frac{2\left(E_{\mathrm{apply}}-U_{\mathrm{fb}}-\frac{\mathrm{kT}}{e}\right)}{{\epsilon \epsilon }_0{\mathrm{eN}}_{\mathit{D}}}$

In equation 7, C_sp represents the space electron layer capacitance, E_apply represents the applied potential, U_fb represents the flat band potential, k is the Boltzmann constant, T is the absolute temperature, e is the electron charge, e is the dielectric constant of passive film, e₀ is the permittivity of free space, and N_D represents the donor density.

It was reported that the defect of passive film was closely associated with the value of N_D, which was inversely proportional to the slope of straight line part on the Mott-Schottky plot.³² From Figure 8, the slope of straight line part for the Q235 steel in the pH 6 solution is greater than that in the pH 5 solution, indicating the defect of passive film formed in the pH 6 solution is less than that formed in the pH 5 solution. The above results of film resistance and film defect confirm that the corrosion resistance of passive film formed in the pH 6 solution is larger than that formed in the pH 5 solution.

On the other hand, the Cl^- concentrations in the pH 5 and 6 solutions before and after the polarization curve tests were measured, as shown in Figure 9. Both before and after the polarization curve tests, the Cl^- concentration in the pH 5 solution is higher than that in the pH 6 solution, which is also responsible for the more negative of E_pit for the Q235 steel in the pH 5 solution than in the pH 6 solution.

Figure 9
Concentrations of CL⁻ in 0.01 mol L^-1 NaNO₂-HCl solutions with pH 5 and 6 before and after polarization curve tests.

Conclusions

In this work, the effects of pH values on the mechanisms of NO₂^- for Q235 carbon steels in 0.01 mol L^-1 NaNO₂-HCl solutions with different pH values were studied, and the related mechanisms of electrochemical behavior and localized corrosion were also discussed. In the pH 1 and 2, pH 3 and 4, and pH 5 and 6 NaNO₂-HCl solutions, the Q235 steels showed the electrochemical behaviors of activation, activation-passivation transition and self passivation-pitting, respectively corresponding to the occurrence of UC, IGC and PC. The effects of pH values on the mechanisms of NO₂^- were very significant. The presence of NO₂^- did not affect the electrochemical behavior and the corrosion type but only accelerated the anodic reaction of Fe oxidation in the pH 1 and 2 solutions. In the pH 3 and 4 solutions, the transition of electrochemical behavior from activation to passivation and the change of corrosion type from UC to IGC were attributed to the cathodic reaction of NO₂^- reduction. In the pH 5 and 6 solutions, the strong oxidability of NO₂^- played a critical role in the formation of γ-Fe₂O₃ passive film under the combined action of Fe²⁺ and NO₂^-.

Acknowledgments

This work is supported by the National Natural Science Foundation of China (contract 51601133).

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Publication Dates

• Publication in this collection
  12 Aug 2019
• Date of issue
  Aug 2019

History

• Received
  30 Dec 2018
• Accepted
  24 Apr 2019