3.2.2. Linear Polarization Measurement
Figure 8 shows linear polarization resistance (LPR) plots for the as-received and solutionized samples. From the LPR curves, it can be observed that all the solutionized samples possessed higher corrosion resistance than the as-received cold-rolled UN08029 alloy, as evident from the steepness of the slope of the potential vs. current curves. The corrosion resistance is directly proportional to the slope of the LPR curve. It is often used to estimate the corrosion current density (
Icorr) according to the Stern Geary relationship as in Equation (1) [
18,
19]. Accordingly, the polarization resistance (R
p) was obtained from the slope of the LPR curves, while the
Icorr and corrosion rate (
CR) were then obtained from Equations (1) and (2), respectively [
18,
19].
where R
p is the polarization resistance obtained from the LPR slope, and βc and βa are the cathodic and anodic Tafel constants taken as ±0.12, respectively.
where
is the density, and
EW is the equivalent weight of the UN08029 alloy.
The parameters R
p and I
corr for the samples obtained from the LPR measurement are shown in
Table 3 and
Table 4 showing the effects of solutionizing duration and temperatures, respectively. All the solutionized samples demonstrated a higher slope, thus larger R
p and consequently lower I
corr than the as-received UN08029 alloy (A29). As seen from
Table 3, as the solutionizing duration increases from 30 to 120 min, the R
p increases. This necessitates a corresponding reduction in the current density and corrosion rate with an increase in the solutionizing duration. The R
p of the untreated alloy sample was increased by about 67, 68, and 76% after solutionizing for a duration of 30, 60, and 120 min, respectively, as estimated from the resistive efficiency (ε
lpr) according to the LPR measurement. Though there is an appreciable increase in the Rp compared with the untreated sample A29, the increment among the solutionized samples is not that significant, especially for the duration between 30 and 60 min, as the grain size distribution is fairly similar (see
Figure 3). The increasing corrosion resistance behavior can be associated with the microstructure of the samples after solutionizing for the different duration, as shown in
Figure 3 and
Figure 4. An increase in the grain size with solutionizing duration reduces the grain boundary defects and thus improves the corrosion resistance. Though there are precipitated carbide and sigma phases, as observed in
Figure 4(a
1,a
2), this does not seem to affect the corrosion behavior of this alloy. This may be attributed to the substantial availability of Cr, Mo, and Ni in the matrix (as seen in
Table 2), which are instrumental in the corrosion resistance property, so the matrix was not detrimentally depleted of these elements for the formation of the secondary phases.
The LPR parameters for the sample solutionized at different temperatures are shown in
Table 4, and the I
corr is lower for the solutionized samples, with sample AT12 exhibiting the lowest values. In addition, it is seen that the R
p of the untreated alloy sample (A29) was increased by about 72, 74, 76 and 42% after solutionizing at temperatures of 1000, 1100, 1200, and 1300 °C, respectively, as enumerated from the ε
lpr. The obtained resistive efficiency of 72% for sample AT10 increases slightly until 1200
oC and then drops to about 42% at 1300 °C (sample AT13). Similarly, the increased corrosion resistance with increasing solutionizing temperature can be linked to grain size growth, as evident from
Figure 5. However, the reduction in the corrosion behavior at a temperature of 1300 °C may be attributed to the increased growth and coalesces of secondary phases in the matrix as well as wider grain boundaries of carbides and sigma phases, as shown in
Figure 6. The increased secondary phases are associated with the lower number of twin boundaries than that of sample AT12. Since twin boundaries are highly resistant to carbide precipitation during treatments [
16], it is expected that a sample with a lower number of twin boundary samples will exhibit a percentage of carbide precipitates.
3.2.3. Cyclic Potentiodynamic Polarization Measurement
The CPDP measurement also revealed important corrosion characteristics of the as-received and solutionized samples. The Tafel extrapolation method was employed to obtain the corrosion potential (E
corr) and corrosion current density (I
corr) from which the corrosion rate (CR) was calculated. The CPDP plots for the solutionized samples are shown in
Figure 9, and they exhibited both active and passive behavior at various polarizing potentials. The parameters E
corr, I
corr, and CR quantify the general corrosion behavior of the samples, while the pitting potential (E
pit), passivation current density (I
p), and the repassivation or protection potential (E
p) are essential parameters for quantifying the localized pitting corrosion behavior of the samples [
12,
20]. The E
pit is defined as the potential at which the surface passive film breakdown occurs, as indicated by the rapid increase in the current in the active-passive region [
12,
20,
21]. For a better insight into the film breakdown, the Ip was determined as the corresponding current density at which the surface film breakdown occurs. While the E
p is defined as the potential in the reverse scan direction when repassivation occurs or the hysteresis loop (approximated to E
pit – E
p) is completed (i.e., when the reverse scan intercepts the forward scan) [
20].
Figure 9a is the CPDP plot for the samples solutionized for different time durations, and the samples exhibited similar behavior. However, all the solutionized samples were shifted to lower current density while the E
corr of the samples T30 and T120 became nobler than the as-received sample. Subsequently, the solutionized samples showed higher potential at any given current density almost throughout the passive region. Though the E
pit for the untreated sample A29 is slightly higher than for the solutionized samples, a closer look into the hysteresis loop shows that the loop size is in the decreasing order of T30 < T120 < T60 < A29. The lower the hysteresis loop, the faster the repassivation and the lesser the damage due to pitting corrosion on the sample.
Table 5 shows the quantitative CPDP parameters for the solutionized samples for a different duration. It is evident from the table that the I
corr and, consequently, CR decreases, necessitating an increase in resistance efficiency (ε
cp) with solutionizing duration and consonant with the LPR findings. The E
pit, I
p, and E
p values which quantify the pitting corrosion behavior, show that the as-received sample A29 exhibited the highest E
pit and lowest I
p. However, it has the lowest E
p values. This indicates that though the pitting potential is the highest and occurs at a lower current density, repassivation is somewhat delayed, which means more pitting corrosion damage to the sample. Based on the repassivation capability, samples T30 and T120 possessed improved repassivation tendencies which resulted in lesser pitting damage, especially considering that their I
p values are just barely higher than that of the as-received sample.
Similarly, the CPDP plots for the samples solutionized at different temperatures are shown in
Figure 9b, and the E
corr of the solutionized samples shifted to the noble positive potentials with correspondingly lower I
corr. This behavior shows that all the samples solutionized at different temperatures exhibited improved resistance against general corrosion in comparison with the as-received sample A29. Furthermore, for the pitting behavior, the as-received sample offered the highest E
pit and lowest I
p, just as observed with the samples solutionized for a different duration. However, the hysteresis loop of sample A29 is the largest due to its E
p value being the least. Interestingly, the hysteresis loop for the solutionized samples is almost overlapping, and the E
p is only slightly different. The E
corr, I
corr, and ε
cp parameters, alongside the pitting corrosion parameters for these samples, are given in
Table 6. The ε
cp parameter can be seen to be within a close range between 84 and 87% with the solutionizing temperature and then sharply drops to 55% for the sample solutionized at 1300 °C (sample AT13). The samples can be ranked according to increasing E
pit, thus, A29 > AT12 > AT13 > AT10 > AT11, while the hysteresis loop can be ranked in the increasing order thus: A29 > AT12 > AT13 > AT10 > AT11. It should be noted that the sample with a high E
pit and a low hysteresis loop will demonstrate superior pitting resistance. Thus, it can be proposed that sample AT12 showed an optimum combination of both E
pit and a relatively low hysteresis loop, therefore will suffer less from pitting corrosion damage.
3.2.4. Electrochemical Impedance Spectroscopy Measurements
Electrochemical impedance spectroscopy (EIS) is probably among the most sophisticated non-destructive steady-state electrochemistry techniques used for corrosion evaluation as it can provide information relating to the reaction parameters, corrosion rates, oxide formation, and their characteristics, surface integrity, and porosity as well as other interfacial properties [
22,
23]. Thus, the investigation of the corrosion behavior of the as-received and heat-treated alloys using EIS was also conducted.
Figure 10 and
Figure 11 are the Bode and Nyquist EIS plots showing the effect of solutionizing duration and temperature on the electrochemical behavior of the alloy, respectively. It can be observed from the Bode plots (which consist of modulus impedance (|Z|) and phase angle (θ) plots) that the log |Z| vs. log f (frequency) relationship does not conform to −1. The phase angle maxima (θ
max) is much below −90 degrees, indicating a deviation from ideal capacitive behavior. It is known that the |Z| measured from the low-frequency portion of the modulus impedance plot is related inversely to the corrosion rate; thus, a larger absolute impedance assures superior charge transfer resistance at the surface/electrolyte interface [
24,
25,
26,
27].
In
Figure 10a, the |Z| can be observed to increase with increasing solutionizing duration. At the same time, the θ
max also tends to increase fairly above −80 degrees in comparison with the as-received alloy, which is just about −70 degrees. The higher the θ
max, the higher the capacitive behavior of the alloy, which indicates improved resistance to charge leakage or transfer to the corrosive medium. Similarly, the peak of the θ
max for the solutionized samples is also observed to shift to a lower frequency than that of the as-received alloy. This may be associated with surface film formation resulting from corrosion. The accompanying broadening of the phase angle plot with solutionizing duration indicates a two-time constant phenomenon [
22].
Figure 10b shows the Nyquist plot, which supports the increment with solutionizing duration evident from the increasing diameter of the incomplete semi-circle capacitive arc. The higher the diameter of the semi-circle, the higher the total resistance to corrosion which indicates the protective performance of the alloys in the medium under consideration [
26,
27].
Similarly, the samples solutionized at different temperatures demonstrated an increasing |Z|, a higher θ
max, and a broader phase angle plot with temperature until 1200 °C (sample AT12), and these parameters then decrease at the solutionizing temperature of 1300 °C (sample AT13) as shown in
Figure 11a. This is also seen in the Nyquist plot in
Figure 11b from the increasing diameter of the incomplete semi-circle capacitive arc with temperature until 1200 °C after which the capacitive arc reduces. It is interesting to note that the θ
max of sample AT13 does not drop. Rather the broadening of the phase angle only reduces. This illustrates the mechanism and reason for the observed reduction in the protectiveness of this sample, and this can be associated with the oxide film instability and not being compact or dense enough in comparison to the other solutionized samples.
The EIS data were fitted with an equivalent circuit (EC) to enumerate the various parameters useful in further understanding the electrochemical behavior of the solutionized samples. An observation of the EIS plots shows that the samples exhibited a two-time constant phenomenon as seen from the two inflection points and/or wideness of the phase angle plots of the Bode diagram. This will be more evident if allowed for more time or at a lower frequency. Thus, the EC consisted of a constant phase element accounting for the non-ideal capacitive behavior of the electrical double-layer (CPE
dl). The CPE
dl is connected in parallel with the surface resistance to charge transfer (R
ct). Both CPE
dl and R
ct are further connected serially to the resistance of the oxide films (Rf) and a constant phase element (CPE
f), which accounts for the capacitive properties of the oxide film. The solution resistance (Rs) is connected in series with the R
f and CPE
f elements. The EC used in this study is shown in the insert of
Figure 10c as well described as Model C in [
28], and it is from the most famous EC used for fitting EIS data of stainless steels [
29,
30,
31]. The chi-square or the goodness of fit (χ
2) is usually utilized to access the agreement between the experimental and simulated data, and the lower the χ
2, the better the agreement and the more reliable the obtained parameters from the fitting. In general, a χ
2 value of 10−3 and lower is accredited to a better quality of the EIS fitting [
32]. In this study, the goodness of fit (χ
2) values were found to be about 10
−4, which signifies an appropriate equivalent circuit choice. The constant phase element (CPE), which has been widely used to model surfaces with oxide films and the numerical relationship is well documented [
28,
33,
34], was employed to account for the deviation from ideal capacitive behavior caused by the heterogeneous nature of the inherent surface oxide film formed on stainless steel when exposed aqueous environment [
19]. The electrical impedance of a CPE can be calculated according to Equation (3) [
19,
28].
where
Q is a frequency-dependent real constant (Ω
−1 s
α),
n is the quantity that represents the deviation from ideal capacitive behavior, ω is the angular frequency (
). When
n approaches unity, an ideal capacitive behavior is observed, and
Q is equivalent to the film capacitance. The EIS parameters obtained from the fitting are presented in
Table 4 and
Table 5 for the effect of solutionizing duration and temperature, respectively.
The parameters showing the effect of solutionizing duration (in
Table 7) illustrate that both R
ct and Rf increased for the solutionized samples compared with the untreated A29 alloy. Quantitatively, the R
ct and R
f for the sample T30 (solutionized for 30 min) were increased by 68 and 47%, respectively. In contrast, for sample T60, they were increased by 88 and 59%, respectively, and by 126 and 66%, respectively, for sample T120. It is observed from this analysis that the higher resistance of the solutionized samples results from both the charge transfer resistance and the resistance of the surface oxide film and that the oxide film resistance also increases with solutionizing duration. The total impedance (R
T), which is the sum of the R
ct and R
f, was used to estimate the protective performance (ε
eis), which shows the increasing protectiveness of 46 to 60% with increasing solutionizing duration from 30 to 120 min. Similarly, for the effect of solutionizing temperature on the electrochemical behavior of UN08029 alloy (as shown in
Table 8), the R
ct increases with increasing the solutionizing temperature until 1200 °C, which then drops. However, the R
f values remain almost unchanged with increasing solutionizing temperature. Thus, the R
T shows 45, 52, 60, and 26% improvement in the corrosion protection performance for sample solutionized at temperatures of 1000, 1100, 1200, and 1300 °C, respectively. These EIS results obtained substantiated the LPR and CPDP measurements.
3.2.5. Corroded Surface Characterization
The SEM and EDS analyses of the corroded surfaces are presented in
Figure 12 and
Figure 13, respectively. Several pits at the microscale can be observed on the exposed surface of the as-received sample A29 (
Figure 12(a,a
1)). These pits range between 1–3 µm in diameter and vary in depth but are mostly shallow. In comparison, on the corroded surfaces of the solutionized samples at different duration shown in
Figure 12b–d, lesser or no pitting was observed at the same scale. However, for sample T30, a preferential grain boundary etching effect (GB attack) and subsequent deposition on the grain boundary were observed. The EDS analysis of the deposits on the grain boundary, as shown in Spectrum 10 of
Figure 13a, shows that the deposits are corrosion products consisting mostly of oxides and carbides of the Fe, Ni, and Cr. Similar deposits are observed within the grains at the initial stage; hence, they can only be well observed at much higher magnification. Spectrum 8 of
Figure 13a also shows the composition of typical deposits within the grains compared with the matrix composition shown in spectrum 11. The GB attack or etching effect was also observed in samples T60 and T120. However, the severity reduces with duration showing that these samples exhibited better resistance in comparison. Furthermore, no apparent pitting was observed on the corroded surface of sample T120 (
Figure 12d).
Similarly,
Figure 12e–g shows the representative corroded surfaces for the samples solutionized at different temperatures, and it is observed that the density of the micro pitting increases for samples AT10 and AT11 in comparison with that of sample A29. Though the density of pits was higher in these samples, the pits were much shallow and spread mostly on the surface. Both GB attack, micro pits as well as corrosion deposits can be observed on the surface of sample AT13. The sample actively corroded uniformly with the presence of micro pitting, which causes the deterioration of its corrosion resistance.
Figure 13b shows the EDS analysis of the deposits (Spectrum 4), which are similar in composition to those observed in the grain boundaries, only that the carbon content is higher while Fe, Ni, and Cr are lower. This indicates that the sample actively corrodes uniformly. The content of the Fe, Ni, and Cr in the grain boundaries is associated with increased reactivity due to the availability of dangling or unbonded atoms. Contrastingly, sample AT12 exhibited the least surface damage, as evident from
Figure 12d.