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TRANSCRIPT
Corrosion Protection Mechanism of 2-Mercaptibenzothiazole and its
Potential Synergistic Effect with Cerium Ions for treatment of AA
2024-T3
A. C. Balaskas*, M. Curioni and G. E. Thompson
Corrosion and Protection Centre, School of Materials, The University of Manchester,
Manchester, M13 9PL, United Kingdom
Abstract
The corrosion protection mechanism of 2-mercaptobenzothiazole (2-MBT)
and its potential synergistic effect with cerium chloride (CeCl3) for sustainability of
the aerospace alloy AA 2024-T3 was investigated. The corrosion inhibitors 2-MBT
and CeCl3 and their potential synergistic properties were assessed with image-assisted
electrochemical noise, the split-cell technique, potentiodynamic polarization,
electrochemical impedance spectroscopy (EIS) and scanning electron microscopy
(SEM) observations. It is suggested that 2-MBT inhibits the dealloying of S-phase
particles and prevents the formation of Cu-rich particles on the surface of AA 2024-
T3. 2-MBT protects the second phase particles from corrosion and offers
sustainability in 3.5% NaCl solution by formation of a protective layer on the surface
of AA 2024-T3. Additionally, 2-MBT is adsorbed on the surface of AA 2024-T3
during anodic dissolution of aluminium. A synergistic effect between 2-MBT and the
Ce3+ based corrosion inhibitor was not found. It is suggested that 2-MBT protects the
intermetallic particles from corrosion from the early immersion time and blocks the
precipitation of cerium hydroxides over the second phase particles. 2-MBT revealed
better corrosion protection properties compared with CeCl3 and 2-MBT + CeCl3 in the
tested time scale.
*Corresponding Author: [email protected]
Keywords: AA 2024-T3, electrochemical noise, EIS, corrosion, corrosion inhibitors
1
1. Introduction
Chromate containing treatments are widely used for corrosion protection of
aluminium alloys (AA). In the latest years, significant effort has been focused on new
environmentally-friendly treatments for the replacement of hexavalent chromium,
since it is toxic and causes environmental issues [1].
The AA 2024-T3 aerospace alloy contains Cu-rich intermetallic particles such
as the S-phase (Al2CuMg) and the θ-phase (Al2Cu) particles and is susceptible to
pitting corrosion induced by the galvanic connection between Cu-rich particles and
the aluminium matrix which is less noble than the intermetallic particles. Pitting
corrosion sites can initiate from the dealloyed S-phase [2–6] and Al-Cu-Fe-Mn
particles [2,7] and the aluminium matrix close to the Cu-rich remnants from the
dealloyed S-phase particles [2–6]. The S-phase particles before the selective
dealloying of the Mg and Al elements are anodic with respect to the aluminium
matrix. The Cu-sponge remnants after selective dealloying of the Mg and Al elements
are cathodic with respect to the aluminium matrix [2–6]. The trenches in proximity of
the dealloyed S-phase particles are formed from the alkaline pH values induced from
the oxygen reduction reaction (equation 1) dissolving the aluminium oxide layer
(equation 2) [5]. The electrons from the aluminium oxidation are consumed by the
oxygen reduction reaction and hydroxyl anions are produced. The electrons can also
be consumed by the reduction of water producing hydrogen gas and hydroxyl ions
(equation 3). The products of the cathodic reactions, the hydroxyl ions, lead to further
increase of the pH to more alkaline values [5,6].
O2 + 2H2O + 4e– → 4OH– eq. 1
Al → Al3+ + 3e– eq. 2
2H2O + 2e– → 2OH– + H2 eq. 3
Al3+ + 3H2O → Al(OH)3 + 3H+ eq. 4
2H+ + 2e– → H2 eq. 5
Further on the corrosion process, the oxidation of aluminium reduces locally the pH
(equation 4). Consequently, the stability of the aluminium oxide layer is decreased
[2,5,6] and a pit starts to form. As the pit grows the corrosive environment expose
2
new surface of aluminium. Inside the pit, the pH is more acidic at the bottom of the
pit and dissolves further the aluminium matrix and prevents the repassivation of
aluminium [5,6]. During the progress of the pit, new Cu-rich particles are revealed
which are cathodic with respect to the aluminium matrix. As the aluminium further
dissolves more H+ is produced decreasing the pH. The reduction of the H+ inside the
pit might produce hydrogen evolution (equation 5) [5,6].
Corrosion inhibition of Ce3+ for aluminium alloys was first introduced by
Hinton [8]. The concentration of 100 ppm CeCl3 in the corrosive environment of 0.1
M NaCl solution decreased significantly the corrosion rate of the aluminium alloy. A
layer of hydroxide precipitates is formed over the intermetallic particles decreasing
the rate of cathodic reactions [9,10]. The formation of the layer of precipitates takes
place in alkaline environment over the dealloyed S-phase particles [10,11]. The
corrosion inhibition of Ce(NO3)3 for AA 2024-T3 was studied with image-assisted
electrochemical noise and potentiodynamic polarization. The results indicated that
Ce(NO3)3 is an effective corrosion inhibitor in concentration of mM in 3.5% NaCl
solution. Potentiodynamic polarization indicated decreased cathodic current density
for AA 2024-T3 electrodes immersed in Ce(NO3)3 in the concentration of mM
compared with specimens immersed without inhibitor [11,12]. Ce based conversion
coatings on aluminium alloys and their effect on protection of intermetallic particles
have been reported in the literature [13].
The inhibitor 2-MBT has been studied for corrosion protection of aluminium
alloys [14–16]. Potentiodynamic polarization tests indicated that 2-MBT in 0.05 M
NaCl [16] and 3.5% NaCl [14] solution decreases both anodic and cathodic reaction
rates compared with the AA 2024-T3 electrodes immersed without inhibitor.
Electrochemical impedance spectroscopy (EIS) measurements revealed the increase
of the low frequency impedance values with the addition of 2-MBT in the corrosive
environment. The results of fittings on the spectra indicated a decrease in double layer
capacitance suggesting the presence of the formation of a protective film on the top of
AA 2024-T3 [14]. The effect of 2-MBT on copper electrodes has been reported in the
literature [17–19]. Raman spectroscopy [19] and cycle voltammetry measurements
revealed the formation of a film between the ionized form of 2-MBT and copper ions.
This film prevents the corrosion of the electrodes [18,19]. The formation of the
protective film of the ionized form of 2-MBT and copper oxides during dissolution of
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copper takes place in an environment with various pH values [17]. The film is water
insoluble and it is a barrier to corrosive species [17].
The synergistic effect of inhibitors has been evaluated for corrosion protection
of AA 2024-T3 in the literature [11,16,20–23]. The effect of Ce(NO3)3 with 2-MBT
for protection of AA 2024-T3 in 50 mM NaCl was evaluated with electrochemical
methods [16]. It was reported that better corrosion protection was offered with
combination of inhibitors compared with the individual inhibitors. 2-MBT has been
encapsulated into nanocontainers and used in coated specimens for corrosion
protection of aluminium and other alloys [24–27]. Double shell structured CeO2
nanocontainers [25], crystalline CeO2 nanocontainers and CeMo [24] nanocontainers
loaded with 2-MBT were added in coated AA 2024-T3 specimens for corrosion
protection. Additionally, EIS rtests revealed that treated with 2-MBT anodized AA
2024-T3 revealed improved corrosion protection properties compared with anodized
AA 2024-T3 electrodes [28]. X-ray photoelectron spectroscopy studies indicated the
formation of insoluble film of 2-MBT with copper oxides on the surface of copper
electrodes. This layer inhibited the corrosion of copper [17].
In this study, the corrosion protection mechanism of the inhibitor 2-MBT and
potential synergistic properties with CeCl3 was studied for sustainability of AA 2024-
T3. It was found that 2-MBT offers very good corrosion protection properties to AA
2024-T3 by inhibition of dealloying of S-phase particles and protection of the Cu-rich
intermetallic particles from corrosion. No synergistic effect between 2-MBT and
CeCl3 was found. It is suggested that the inhibition of dealloying of S-phase particles
and corrosion protection of Cu-rich second phase particles by 2-MBT prevents the
precipitation of cerium hydroxides. The precipitation of the cerium hydroxide layer
over dealloyed intermetallics and the necessary local alkaline environment was
revealed in the literature [10]. In order to reveal the corrosion mechanism of 2-MBT
and to investigate possible synergistic effect of 2-MBT with CeCl3 advanced and
traditional electrochemical techniques were used. Furthermore, SEM micrographs and
energy dispersive X-ray spectroscopy (EDX) measurements indicated the morphology
of AA 2024-T3 immersed in 3.5% NaCl solution with the presence the inhibitors and
the composition of second phase particles. With electrochemical noise no external
perturbation is applied to the electrodes and coupled with the images from the surface
provide real-life estimation of the inhibitors corrosion protection [29].
Potentiodynamic polarization revealed the effect of inhibitors on the anodic and the
4
cathodic reaction rates. The split-cell technique indicated the effect of the inhibitors
on the reactions rate in the scale of seconds after the addition of the inhibitor in the
corrosive environment. EIS tests revealed the corrosion protection mechanism of
inhibitors and the phenomena on the surface of AA 2024-T3 in the presence of
inhibitors.
2. Experimental details
2.1. Materials and Reagents
The AA 2024-T3 specimens have nominal composition in wt.% of Si <0.5, Fe
<0.5, Cu 3.8-4.9, Mn 0.3-0.9, Mg 1.2-1.8, Cr <0.1, Zn <0.25, Ti <0.15 and Al matrix.
2-MBT, CeCl3, sodium hydroxide (NaOH) pellets and nitric acid were of analytical
reagent grade and purchased from Sigma-Aldrich, St. Louis, USA.
2.2. Specimen preparation and corrosion evaluation
The AA 2024-T3 specimens were pretreated by etching and desmutting. The
procedure includes immersion in 10% w/v NaOH for 30 seconds at 60oC with stirring,
then rinsing with distilled water and immersion in 30 vol.% HNO3 for 30 seconds at
ambient temperature. Finally, the specimens were rinsed with deionized water.
Beeswax was used for masking the edges of the electrodes with exposed area of 2.25
cm2.
For the image assisted electrochemical noise experiments, the method
described in detail elsewhere was used [29]. Briefly, in this method two AA 2024-T3
electrodes were coupled with a 10 kohm resistor. A NI-USB6009 (National
Instrument) analogue to digital converter was used to measure the potential of each
electrode with respect to a saturated calomel electrode (SCE). The Labview
programming language was used to develop a software to record the noise potential
and to calculate the noise current. The noise resistance values were calculated
according to the following procedure described in [14,29]. In the first step, a segment
of 1024 points was extracted on the initial data sets of potential and current. Then, the
square root of the variance of the potential divided by the variance of the current was
calculated on the first point of the segment (equation 6 [29]) until the end of the
5
segment. A new segment was extracted with a step of 250 points and the calculations
were continued until the end of the dataset. The final Rn(t) diagrams were smoothed.
Rn(t )=√ σ2[V (t ) ]σ2[ I ( t )]
eq. 6 [29]
Maplin USB microscopes were used to record the images from the surface of
the AA 2024-T3 electrodes immersed in 3.5% NaCl solution in the presence of
inhibitors.
A SI 1287 Solartron Electrochemical interface was used for potentiodynamic
polarization and the split-cell tests. The AA 2024-T3 electrode was the working
electrode, a platinum electrode was the counter electrode and a saturated calomel
electrode (SCE) was the reference electrode in a three-electrode cell. The corrosive
environment was 1 litre of naturally aerated 3.5 wt.% NaCl with the addition of the
corrosion inhibitors. The potential was scanned from the open circuit potential (OCP)
to -1 V vs SCE in the case of the cathodic polarization and form -0.005 V vs SCE to -
0.5 V vs SCE in the case for the anodic polarization with the scan rate of 0.10 mV/s.
Two AA 2024-T3 electrodes connected with a zero resistance ammeter (ZRA)
and a SCE were used for the split-cell technique. The electrodes were immersed in
naturally aerated 3.5% NaCl solution in two different compartments connected with a
porous glass frit. After initiation of nitrogen gas in one compartment and oxygen gas
in the other compartment, the AA 2024-T3 electrode in the first compartment became
a net anode and the electrode in the compartment filled with air became a net cathode.
The time of addition of the inhibitors in the compartments is indicated with arrows
(Figure 8).
The EIS measurements carried out with a SI 1287 Solartron Electrochemical
interface connected with a SI 1250 impedance/frequency response analyser (Figure 9a
and 9b) and an Autolab PGSTAT302N – Metrohm potentiostat equipped with FRA
module impedance/frequency response analyser (Figure 11a and 11b). The EIS
spectra acquired with a three-electrode cell configuration at the open circuit potential
(Figure 9a and 9b) and at -0.610 V vs SCE (Figure 11a and 11b). The electrochemical
cell consisted of the working electrode, a saturated calomel electrode (SCE) and a
platinum foil with area of 2 cm2 was the counter electrode. The frequency range was
6
between 10 kHz and 5 mHz (Figure 9a and 9b) and between 100 kHz and 10 mHz
(Figure 11a and 11b), with rms voltage at 10 mV. All EIS spectra were fitted with the
Z-view software.
2.3. SEM
In the first step, the surface of the AA 2024-T3 specimens was smoothed by
grinding and polishing. The mirror polished surface was achieved with polishing with
1 micron diamond paste. Afterwards, the specimens were immersed in the tested
environment. After the immersion, the specimens were rinsed and dried. The
specimens for the cross-section observations were prepared with the method of
ultramicrotomy. A glass knife was used for the first cuts of the specimen. The final
polishing was achieved with dry cuts with daemon knife. The surface and the cross
section of the specimens were investigated with ZEISS Ultra 55 field-emission gun
scanning electron microscope. The microscope was operated in the acceleration
voltage of 1 kV and the working distance was below 3 mm at 0 degrees angle of tilt.
3. Results
3.1 Image assisted electrochemical noise
The corrosion protection performance of 2-MBT and CeCl3 and their potential
synergistic effect for corrosion protection of AA 2024-T3 has been evaluated with
image assisted electrochemical noise. Figure 1 shows the time evolution of the noise
resistance of AA 2024-T3 electrodes in 3.5% NaCl in the presence of a) 2-MBT in
saturated conditions, b) 0.075 mM CeCl3 and c) 2-MBT + 0.075 mM CeCl3 until 40
hours of testing. Electrodes immersed with 2-MBT, CeCl3 and 2-MBT + CeCl3 reveal
similar corrosion protection properties. AA 2024-T3 electrodes immersed with 2-
MBT had noise resistance values of 110 kohm cm2 after 1 hour and close to 105 kohm
cm2 after 10 hours of immersion. AA 2024-T4 specimens without inhibitor had noise
resistance values of 8 kohm cm2 after 1 hour and 13 kohm cm2 after 10 hours of
immersion. The values of the noise resistance with CeCl3 were 23 kohm cm2 after 1
hour and increased to 100 kohm cm2 after 10 hours of immersion. Specimens
immersed with 2-MBT + CeCl3 revealed slightly decreased noise resistance values
7
compared with specimens with 2-MBT, 80 kohm cm2 after 1 hour and 100 kohm cm2
after 10 hours.
The optical images recorded during the electrochemical noise experiments are
shown in Figure 2. The images from the first hour until the 40 th hour of immersion
show the changes in the morphology of the surface during immersion in the
corresponding environment. AA 2024-T3 specimens reveal initiation of darkening in
the first hour and more intense darkening and pitting with increasing immersion time.
The electrodes immersed with 2-MBT reveal hydrogen bubbles in the first hours of
immersion indicating increased cathodic activity. The surface of AA 2024-T3 reveals
no darkening and pitting. With addition of 0.075 mM CeCl3 in the NaCl solution
initiation of pitting is observed on the surface of the electrodes after 40 hours of
immersion. The addition of 2-MBT + CeCl3 in 3.5% NaCl solution reveals increasing
number of hydrogen bubbles with time of immersion (Figure 2). However, no
darkening and pitting is observed until 40 hours of immersion.
Figure 3 shows the time evolution of noise current for AA 2024-T3 electrodes
immersed in 3.5% NaCl solution without inhibitor and immersed with 0.075 mM
CeCl3, with 2-MBT and 2-MBT + CeCl3. The diagrams indicate the large fluctuations
of current for AA 2024-T3 electrodes immersed without inhibitor compared with the
significantly decreased current fluctuations for electrodes immersed in the presence of
inhibitors. More specifically, large fluctuations of the noise current are observed for
AA 2024-T3 without inhibitor in the rage of 0.2 μA in the first hour and increased to
0.75 μA after 24 hours. The noise current for the electrodes immersed with addition of
all inhibitors reveal significantly decrease values compared with the specimens
immersed without inhibitor. In the case of addition of CeCl3 in the corrosive
environment, in the first hour of immersion the noise current of AA 2024-T3 reveal
increased values compared with the addition of 2-MBT and 2-MBT + CeCl3. AA
2024-T3 with CeCl3 has noise current values of 0.1 μA after 1 hour and values of 0.02
μA after 24 hours. The electrodes immersed with 2-MBT reveal noise current values
in the range of 0.01 μA in the first hour of immersion and the range of 0.005 μA after
24 hours. The specimens immersed with 2-MBT + CeCl3 have similar behaviour as in
the case of addition of 2-MBT. The noise current values are in the range of 0.02 μA in
the first hour of immersion and the range of 0.005 μA after 24 hours.
3.2 Effect of the inhibitors on the second phase particles
8
SEM observations indicate the morphology of the second phase particles after
immersion of AA 2024-T3 in 3.5% NaCl solution for the specimens immersed
without inhibitor and for the specimens immersed in the presence of 2-MBT. Figure 4
shows backscattered images from the cross section of AA 2024-T3 immersed in 3.5%
NaCl solution without inhibitor. Figure 4a shows trenching in proximity of second
phase particles and Figure 4b shows a cavity possibly after removal of second phase
particles. The backscattered image reveals the presence of copper inclusions and the
dissolved aluminium matrix near by the intermetallics. Figure 5 shows backscattered
images from the surface (Figure 5a and 5b) and the cross section (Figure 5c) of AA
2024-T3 immersed in 3.5% NaCl solution with 2-MBT. An Al-Cu-Fe-Mn and a S-
phase particle are indicated in Figure 5a. A cluster of intermetallic particles is
presented in Figure 5b. The S-phase, the Al-Cu-Fe-Mn and the θ-phase particles are
revealed uncorroded and the S-phase particles are not dealloyed from Al and Mg after
24 hours of immersion. Furthermore, no cavities and trenches around the second
phase particles are revealed on the surface of AA 2024-T3. The EDX spectra taken at
the indicated areas on Figure 5a and 5b reveal the elemental weight percentages. The
Al-Cu-Fe-Mn particle is indicated with the symbols Xi (C: 23.6, Al: 33.7, Mn: 3.0,
Fe: 11.2, Cu: 28.5) and Xvi (C: 6.2, Al: 50.0, Si: 1.35, Mn: 7.5, Fe: 12.3, Cu: 23.1).
The S-phase particle (Al2CuMg) is indicated with the symbol Xii (C: 21.2, Mg: 12.6,
Al: 32.5, Cu: 33.7). The θ-phase particles (Al2Cu) are indicated with the symbols Xiii,
Xiv and Xv. Xiii (C: 4.6, Mg: 1.3, Al: 87.5, Mn: 0.4, Cu: 4.7), Xiv (C: 8.0, Mg: 1.2,
Al: 84.6, Mn: 0.5, Cu: 4.3), Xv (C: 7.2, Mg: 1.2, Al: 85.1, Mn: 0.4, Cu: 4.7).
3.3 Effect of inhibitors on anodic and cathodic reaction rates
Figure 6 shows the polarization curves for the AA 2024-T3 immersed in 3.5%
NaCl without inhibitor after 1 hour (a) and 24 hours (b), AA 2024-T3 with addition of
2-MBT after 1 hour (c), 24 (d) and 72 hours (e) of immersion. The corrosion process
of AA 2024-T3 electrodes immersed without inhibitor is under cathodic control. The
cathodic part of the curves after 1 and 24 hours the current has little dependence on
potential. On the anodic part of the scan, after 1 hour of immersion the pitting
potential is very close to the OCP. After 24 hours, the OCP drops at –0.69 V vs. SCE
while the pitting potential remains at –0.59 V vs. SCE, very close to the pitting
potential after 1 hour of immersion. As the corrosion process proceeds the rate of the
anodic reactions increases and subsequently the OCP drops to more negative values.
9
For AA 2024-T3 electrodes immersed after 1 hour in the presence of 2-MBT the
pitting potential increases for about 30 mV to the value of –0.57 V vs. SCE compared
with the specimen without inhibitor. Additionally, the rates of anodic and cathodic
reactions are decreased. After 24 and 72 hours the pitting potential drops to values
close to the pitting potential of the control experiment. The anodic reactions rates and
the OCP reveal a small decrease while the rates of cathodic reactions are stable with
increased immersion.
In Figure 7 the cathodic polarization curves of AA 2024-T3 in 3.5% NaCl
solution a) without inhibitor with b) 1.5 mM CeCl3, c) 2-MBT and d) 2-MBT + 1.5
mM CeCl3 after 24 hours are shown. AA 2024-T3 electrodes immersed with 1.5 mM
CeCl3 show decreased cathodic current density values and decrease OCP compared
with specimens immersed without inhibitor revealing very good cathodic inhibition
properties. Additionally, AA 2024-T3 electrodes immersed in the presence of 1.5 mM
CeCl3 reveal decreased cathodic current density. Additionally, AA 2024-T3 electrodes
immersed with addition of 2-MBT and with addition of 2-MBT + CeCl3 reveal less
decreased cathodic current density compared with AA 2024-T3 immersed with 1.5
mM CeCl3. Furthermore, the OCP of AA 2024-T3 with immersion with 1.5 mM
CeCl3 is decreased compared with immersion with 2-MBT and with 2-MBT + CeCl3.
This behaviour indicates that CeCl3 decreased the cathodic reaction rates of AA 2024-
T3 in 3.5% NaCl more successfully than 2-MBT and 2-MBT + CeCl3.
The split-cell experiments are presented in Figure 8. The increase of the
current (after 16 minutes) is the result of initiation of nitrogen gas in one compartment
and oxygen gas in the other compartment. The AA 2024-T3 electrode in the
compartment filled with nitrogen gas becomes a net anode and the electrode in the
compartment with oxygen gas becomes a net cathode. Consequently, the rate of
anodic reactions increases and the current density increases as well [12,14]. After 35
minutes the inhibitors were added in the individual compartments. The time of
addition of the inhibitor is indicated with arrows. With addition of CeCl3 inhibitor a
gradual decrease of the cathodic current is observed. The addition of 1.5 mM CeCl3
results in the stronger decrease of the current compared with addition of 2-MBT. The
decrease of the current was 0.5 μA/cm2 after 40 minutes (time after the addition of
inhibitor). While, the addition of 2-MBT revealed a minor decrease of 0.09 μA/cm2.
3.4 Electrochemical impedance spectroscopy
10
The corrosion protection properties of 2-MBT and 2-MBT with CeCl3 on AA
2024-T3 electrodes was evaluated with EIS measurements. Figure 9a shows the Bode
plots and Figure 9b shows the Nyquist plots for AA 2024-T3 electrodes in 3.5% NaCl
solution in the presence of 2-MBT (saturated) and in 2-MBT (saturated) + 0.075 mM
CeCl3 compared with AA 2024-T3 electrodes immersed without inhibitors.
Similar EIS spectra were revealed for AA 2024-T3 electrodes immersed in 2-
MBT and in 2-MBT + CeCl3. The low frequency impedance for electrodes immersed
in 2-MBT showed values close to 9 x 10-4 Ω cm2, while specimens immersed in 2-
MBT + CeCl3 revealed a small decrease in low frequency impedance with values
close to 7-8 x 10-4 Ω cm2. AA 2024-T3 electrodes immersed in both inhibiting
solutions have low frequency impedance values close to one order of magnitude
higher than AA 2024-T3 immersed without inhibitor. The linear part of the
impedance spectra from the high to medium frequency range is the capacitive
behaviour of the electrode due to the protective properties of the aluminium oxide
layer. The specimens immersed in both inhibiting solutions revealed increased
capacitive behaviour until lower frequency values and more broad and increased
phase angle values compared with the specimens immersed without inhibitor.
The electrical circuit presented in Figure 10 was used to extract quantitative
parameters from the EIS spectra. The Rsol accounts for the solution resistance,
connected in series is the capacitor associated with the capacitive behaviour of the
aluminium oxide layer (Coxide). The corrosion product resistance (Rcorr products) is
connected in parallel with the Coxide. Connected in series with Rcorr products is the constant
phase element (CPEdl) associated with capacitive behaviour of the double layer
capacitance. Connected in parallel with CPEdl is the polarization resistance (Rpol)
connected in series with a short Warburg element related with the diffusion prosses on
the surface of AA 2024-T3 electrodes [14]. The Warburg element parameters are the
Warburg resistance (WS-R), the length of the diffusion layer (WS-T) and the Warburg
exponent (WS-P) [30,31].
Potentiostatic EIS measurements at -0.610 V vs SCE for AA 2024-T3
electrodes immersed with 2-MBT and with 2-MBT + 0.075 mM CeCl3 after 24 hours
of immersion in 3.5% NaCl are shown in Figure 11a and 11b. EIS tests performed at
potential above OCP and below the pitting potential for AA 2024-T3 electrodes
characterization immersed with inhibitors under anodic dissolution. Similar work with
EIS spectra obtained at potential above pitting potential and in the passive region (-1.0
11
V vs Hg/Hg2SO4) for pure aluminium electrodes immersed in 10-3/10-5 M hydrofluoric
acid were reported in [32]. EIS spectra at -0.610 V vs SCE reveal the behaviour of
AA 2024-T3 immersed with and without inhibitors during anodic dissolution with
rate of 6 x 10-6 A/cm2. The results reveal a capacitive part from high to medium
frequency range and an inductive loop at low frequency range for AA 2024-T3
immersed with 2-MBT and with 2-MBT + 0.075 mM CeCl3. While, AA 2024-T3
immersed without inhibitor showed an incline trend of the resistive part at the low
frequency range related with diffusion phenomena [32]. It is suggested that the
inductive behaviour of AA 2024-T3 electrodes immersed with inhibitors is related
with adsorption phenomena at the electrode surface [33]. Similar results have been
reported for corrosion of carbon steel in the presence of inhibitors [34]. It was
suggested that the inductive loops could be attributed to adsorption phenomena of
monoethylene glycol during dissolution of iron [34]. Inductive behaviour and the
determination of Rp have been reported for iron in the presence of acidic media [35–
37]. The inductive loop in the low frequency range has been observed for carbon steel
electrodes immersed in the presence of acids and has been caused by the relaxation
phenomena of the absorbed species [35].
The potentiostatic EIS spectra at -0.610 V vs SCE of AA 2024-T3 electrodes
immersed with and without inhibitors were fitted with the electrical circuit presented
in Figure 12 to extract quantitative parameters during the corrosion process. The
electrical circuit in Figure 12 is similar with the circuit in Figure 10. The elements
Lanod and Ranod were added in parallel with Rct (charge transfer resistance) and Ws. Lanod
is associated with the variation of the active anodic sites on AA 2024-T3 and Ranod
represents the resistance related with adsorption phenomena of 2-MBT at the potential
of -0.610 V vs SCE [30]. A constant phase element (CPEoxide) (Figure 12) was used
instead of a capacitor (Figure 10) to associate the behaviour of the aluminium oxide
layer in this condition. The EIS spectra for AA 2024-T3 electrodes immersed without
inhibitor at -0.610 V vs SCE revealed on inductive behaviour and was fitted without
the parameters Lanod and Ranod.
4. Discussion
4.1 The corrosion inhibition mechanism of 2-MBT for AA 2024-T3.
12
The corrosion process of AA 2024-T3 initiates from the selective dealloy of S
phase particles which are initially anodic to Al matrix. The resulting Cu-rich particles
are cathodic with respect to the matrix and the cathodic activity increases locally.
Trenches in proximity of second phase particles are formed (Figure 4a) and some of
the intemetallics may be removed from the surface (Figure 4b). The oxidation of
aluminium (anodic activity) increases with increase of the cathodic activity. This
behaviour is evident from the potentiodynamic polarization of AA 2020-T3 after 1
and 24 hours. The small dependence of the cathodic current on the applied potential
and the increased anodic current density with decrease of the OCP after 24 hours are
observed (Figure 6).
With addition of 2-MBT in 3.5% NaCl solution the anodic reactions rate of
AA 2024-T3 decreases and the pitting potential increases from the first hour of
immersion (Figure 6). It is revealed immediate inhibition of anodic reactions
indicating inhibition of the initial dealloying of the S-phase particles. For specimens
immersed with 2-MBT, dealloying of S-phase particles and trenches did not appear
after 24 hours as revealed from SEM observations (Figure 5a). The S-phase particle is
indicated with the symbol Xii in Figure 5a. Additionally, θ-phase particles in Figure
5b (indicated with the symbols Xiii, Xiv and Xv) and the Al-Cu-Fe-Mn intermetallics
revealed uncorroded. Corroded θ-phase particles have been reported in the literature
for clusters of intermetallic particles which consist of θ-phase and S-phase particles
[38]. Al-Cu-Fe-Mn particles are noble with respect to the aluminium matrix and
trenches may be observed after long term tests as a result from cathodic reactions over
these particles [39]. After 72 hours of immersion the anodic reactions rate is
maintained decreased indicating very good long-term corrosion protection properties
for 2-MBT inhibitor. Additionally, the noise resistance values were close to 9 times
higher compared to the specimens immersed without inhibitor (Figure 1). The split-
cell tests suggest that 2-MBT is a poor cathodic inhibitor in the very early immersion
time before the completion of the first hour (Figure 8). The hydrogen bubbles
observed in the early immersion time also suggest cathodic activity on the surface of
the AA 2024-T3 electrodes (Figure 2) [40–42]. The decreased cathodic current
density after 1 until the 72 hours is due to the prevention of formation of Cu-rich
particles. In the literature the formation of a protective film with the ionized form of
2-MBT and Cu oxides preventing the dissolution of Cu electrodes has been reported
[17].
13
EIS measurements at OCP for AA 2024-T3 electrodes immersed with 2-MBT
in 3.5 % NaCl indicated increased corrosion protection properties for AA 2024-T3.
The low-frequency impedance is increased for close to one order of magnitude
compared with AA 2024-T3 immersed without inhibitors. Additionally, AA 2024-T3
immersed with 2-MBT reveal increased capacitive behaviour and more broad and
increased phase angle values compared with electrodes immersed without inhibitor. It
is suggested that with addition of 2-MBT in 3.5% NaCl solution a protective film is
formed on the surface of AA 2024-T3 [14]. The formation of a film between the
ionized form of 2-MBT and copper Cu which prevents the corrosion of Cu electrodes
has been reported in the literature [18,19]. Fittings revealed significantly decreased
aluminium oxide layer capacitance (1.17 μF cm-2) and double layer capacitance values
(19 μF cm-2) for AA 2024-T3 immersed with 2-MBT compared with electrodes
immersed without inhibitor (Coxide: 55.4 μF cm-2, Cdl: 150 μF cm-2) (Table 1). The
value of Coxide and Cdl remained stable after 48 and 72 hours of immersion indicating
that the thickness of the aluminium oxide layer did not change significantly with
increasing exposure time. The low capacitance values for both aluminium oxide layer
and double layer were maintained low until 72 hours indicating that the protective
inhibitor film formed on the surface of AA 2024-T3 remained stable until 72 hours.
Consequently, the polarization resistance for the electrodes immersed with 2-MBT
ranged between values from 50 to 60 kΩ cm2, while electrodes immersed without
inhibitor had polarization resistance value of 0.9 kΩ cm2. Additionally, the Warburg
resistance was increased for electrodes immersed with 2-MBT (30 - 50 kΩ cm2)
compared with specimens immersed without inhibitor (20 kΩ cm2).
EIS tests acquired at -0.610 V vs SCE indicated inductive behaviour at low
frequency for specimens immersed with 2-MBT. On the contrary, electrodes
immersed without inhibitor did not reveal inductive parts on the spectra (Table 2). For
carbon steel electrodes immersed in the presence of inhibitors, the inductive
behaviour was related with adsorption phenomena of the inhibitor on the metallic
surface [34]. Lanod can be related with the extension of the anodic dissolution area of
aluminium and Ranod with the resistance associated with the adsorption phenomena of
2-MBT on the surface of AA 2024-T3 during dissolution of aluminium. Specimens
immersed with 2-MBT reveal increased Rct (20 kΩcm2) and Ws-R values (27 kΩcm2)
compared with specimens immersed without inhibitor (Rct: 0.7 kΩcm2, Ws-R: 1
kΩcm2). Moreover, the Coxide (30 μF cm-2) and Cdl (0.9 μF cm-2) values for specimens
14
immersed with 2-MBT are significantly decreased compared with specimens
immersed without inhibitor (Coxide: 150 μF cm-2, Cdl: 250 μF cm-2). This behaviour
indicates very good corrosion protection properties for 2-MBT by formation of a
protective layer on AA 2024-T3 and the adsorption of 2-MBT during anodic
dissolution of aluminium.
4.2 Investigation of potential synergistic effect between 2-MBT and CeCl3.
AA 2024-T3 electrodes immersed with 2-MBT + CeCl3 reveal decreased
values of noise resistance and low frequency impedance values compared with
electrodes immersed with 2-MBT. Additionally, the immediate effect of 2-MBT on
the corrosion protection of Cu-rich intermetallic particles and on the inhibition of
dealloying of S-phase particles and the gradual effect of CeCl3 on the protection of the
S-phase particles (precipitation of Ce hydroxides on the S-phase particles after initial
dealloy from Mg) indicates no synergistic effect of 2-MBT and CeCl3 on protection of
AA 2024-T3 in the tested timescale.
It is suggested that the immediate effect of 2-MBT on inhibition of dealloying
of S-phase particles and corrosion protection of Cu-rich intermetallics prevents the
deposition of Ce hydroxides over these particles. Cathodic potentiodymanic
polarization revealed decreased current densities and OCP values for AA 2024-T3
electrodes immersed with CeCl3 compared with electrodes immersed with 2-MBT and
with 2-MBT + CeCl3 and specimens without inhibitor. Additionally, similar cathodic
current densities are observed for specimens immersed in 2-MBT and in 2-MBT +
CeCl3 revealing that CeCl3 did not further decrease the cathodic current density when
2-MBT is present in the corrosive environment. In Figure 2, specimens immersed
with 2-MBT + CeCl3 revealed increased generation of hydrogen bubbles with
increasing immersion time. It is suggested that the cathodic activity is not inhibited
for specimens immersed with 2-MBT + CeCl3 indicating that CeCl3 with 2-MBT did
not effectively inhibit cathodic reactions.
Complementary, image assisted electrochemical noise (Figures 1-3) indicate
that CeCl3 in concentration of mM in 3.5% NaCl is an effective corrosion inhibitor of
AA 2024-T3. However, Ce3+ ions well known corrosion inhibitors in the literature are
protective after initiation of corrosion [10]. The cerium hydroxides precipitate at
alkaline pH on the dealloyed S-phase particles and Cu-rich intermetallics resulting in
15
the increase of the corrosion resistance of AA 2024-T3 [10]. The anodic dissolution of
the aluminium and the consumption of electrons by the cathodic reactions over the
Cu-rich particles provide the alkaline environment revealing that the corrosion
process has initiated [10].
The gradual effect of CeCl3 on inhibition of cathodic reactions in the very
early immersion time is indicated by the split-cell technique (Figure 8) with the
gradual decrease of the current with addition of the inhibitor in the corrosive
environment. Additionally, in the early immersion time addition of CeCl3 revealed
increased noise current values (0.1 μA after 1 hour) and were decreased (0.02 μA)
after 24 hours. After 24 hours of immersion cathodic potentiodynamic polarization of
AA 2024-T3 with 1.5mM CeCl3 revealed the lowest cathodic current density with
decreased OCP compared with addition of 2-MBT and 2-MBT + CeCl3 (Figure 7).
The decreased cathodic current density and the high noise resistance values reveal
very good corrosion protection properties. It is known that the corrosion process of
AA 2024-T3 is under cathodic control [5,6,43]. However, pitting is evident after 40
hours of immersion on the surface of AA 2024-T3 (Figure 2).
EIS measurements for AA 2024-T3 electrodes immersed with 2-MBT + CeCl3
revealed small decrease in low frequency impedance compared with specimens
immersed with 2-MBT. EIS measurements for AA 2024-T3 electrodes immersed with
2-MBT + CeCl3 revealed decreased polarization resistance values (30 – 44 kΩ cm2)
compared with specimens immersed with 2-MBT (50 – 60 kΩ cm2). Additionally,
specimens immersed with 2-MBT showed slightly decreased Coxide (6 – 0.5 μF cm2)
and Cdl (6 – 15 μF cm2) values compared with specimens immersed with 2-MBT +
CeCl3 (Coxide: 6 – 10 μF cm2, Cdl: 10 – 20 μF cm2) (Table 1). This behaviour indicates
the better corrosion protection of 2-MBT compared with 2-MBT + CeCl3 and the
presence of CeCl3 with 2-MBT did not inhibit the formation of the protective layer on
AA 2024-T3 from 2-MBT.
EIS tests performed at -0.610 V vs SCE for electrodes immersed with 2-MBT
+ CeCl3 revealed inductive behaviour at low frequency range similar with specimens
immersed with 2-MBT. Electrodes immersed with 2-MBT and with 2-MBT + CeCl3
showed similar Rct (20 and 30 kΩ cm2), Ws-R (25 kΩ cm2) and Coxide (25 μF cm2)
values. However, Cdl values for specimens in 2-MBT (0.9 μF cm2) were decreased
compared with specimens in 2-MBT + CeCl3 (10 μF cm2) indicating the formation of
a thinner protective inhibitor layer on AA 2024-T3 surface (Table 2). Additionally,
16
Lanod values for AA 2024-T3 electrodes immersed with 2-MBT (100 kΩ s cm2) are
significantly increased compared with specimens immersed with 2-MBT + CeCl3
(750 kΩ s cm2). Ranod values for electrodes immersed with 2-MBT (5 kΩ cm2)
revealed small decrease compared with specimens immersed with 2-MBT + CeCl3 (10
kΩ cm2). This behaviour indicates that the addition of CeCl3 with 2-MBT reveals
decrease of the adsorption of 2-MBT on the surface of AA 2024-T3 and increased of
the dissolution area of aluminium compared with the specimens immersed with 2-
MBT.
Consequently, 2-MBT inhibits the anodic reactions from the early immersion
time indicating inhibition of the initial dealloying of the S-phase particles. SEM
observations revealed that the S-phase particles are not dealloyed from Al and Mg
after 24 hours of immersion. EIS measurements indicated the formation of a
protective layer on AA 2024-T3. Additionally, EIS tests indicate the adsorption of 2-
MBT on AA 2024-T3 during anodic dissolution of aluminium. Possible synergistic
effect of 2-MBT with cerium ions for protection of AA 2024-T3 was investigated
with addition of 2-MBT + CeCl3 in the corrosive environment. The results from
electrochemical noise, the split-cell technique and potentiodynamic polarization
indicated that the immediate effect of 2-MBT on the protection of second phase
particles blocks the precipitation of cerium hydroxides over the Cu-rich particles. The
addition of 2-MBT + CeCl3 in 3.5% NaCl resulted in domination of 2-MBT on the
surface of AA 2024-T3 protecting the second phase particles from corrosion. The
corrosion protection of Cu-rich particles did not provide the necessary alkaline
environment over the intermetallics for the precipitation of cerium hydroxide
protection layer. Therefore, addition of CeCl3 with 2-MBT in the corrosive
environment resulted in similar noise resistance values as in the case of addition of the
individual inhibitor 2-MBT revealing no synergistic effect between the inhibitors 2-
MBT and CeCl3. The addition of the individual inhibitor CeCl3 in the corrosive
environment revealed a gradual effect on the corrosion protection of AA 2024-T3 as
indicated from electrochemical noise and the split-cell tests. The noise resistance
values revealed increased to 100 kohm cm2 after 10 hours of immersion (23 kohm cm2
after 1 hour) and the split-cell revealed gradual decrease of the cathodic reaction rates.
The precipitation of the cerium hydroxide layer over the second phase particles is
formed in alkaline environment over the dealloyed S-phase particles [10,11].
17
5. Conclusions
The corrosion protection mechanism of 2-MBT and potential synergistic effect
with CeCl3 for sustainability of AA 2024-T3 was evaluated with traditional and
advanced electrochemical methods. It was found that 2-MBT inhibits the anodic
reaction of dealloying of S-phase particles from Al and Mg from the early immersion
time. The formation of Al-Cu particles from the dealloyed S-phase particles is
prevented and consequently the cathodic reactions are decreased. The Cu-rich and the
Al-Cu-Fe-Mn intermetallic particles are also protected from corrosion. Additionally,
EIS tests revealed the corrosion protection of AA 2024-T3 by formation of a
protective layer and the adsorption of 2-MBT on electrode surface during anodic
dissolution of aluminium. No synergistic properties found between 2-MBT and the
Ce3+ based inhibitor CeCl3. It is suggested that the protection of second phase particles
from dealloying prevents the precipitation of Ce hydroxides. However, the formation
of the 2-MBT protective layer on AA 2024-T3 and the adsorption of 2-MBT during
anodic dissolution is not prevented by Ce3+ ions. SEM observations reveal the
protection of the second phase particles when the AA 2024-T3 electrodes are
immersed with 2-MBT compared with the control test.
Acknowledgements: The authors acknowledge EPSRC for the support of the
LATEST2 Programme Grant
18
Figure 1. Time evolution of noise resistance of AA 2024-T3 immersed in 3.5%
NaCl solution without inhibitor, in the presence of a) 2-MBT (saturated), b)
0.075 mM CeCl3 and c) 2-MBT (saturated) + 0.075 mM CeCl3.
19
Figure 2. Optical images obtained during the EN measurements for AA 2024-T3
immersed in 3.5% NaCl solution without inhibitor, in the presence of 2-MBT
(saturated), 0.075 mM CeCl3 and 2-MBT (saturated) + 0.075 mM CeCl3.
20
Figure 3. Time evolution of a) noise current of AA 2024-T3 immersed in 3.5%
NaCl solution without inhibitor and in the presence of in the presence of 0.075
mM CeCl3, 2-MBT (saturated), and 2-MBT (saturated) + 0.075 mM CeCl3 and b)
magnification of diagram (a).
21
Figure 4. Backscattered electron images from the cross-section of AA 2024-T3
specimen immersed in 3.5% NaCl solution for 6 hours showing a) trenching in
proximity of second phase particles and b) a cavity on the surface.
22
23
Figure 5. Backscattered electron images from a,b) the surface after 24
hours and c) the cross-section after 6 hours of immersion of AA 2024-T3 in 3.5%
NaCl solution with 2-MBT. The marks on Figure 5a and 5b indicate the locations
where the EDX spectra were taken.
Figure 6. Potentiodynamic polarization of AA 2024-T3 electrodes in 3.5% NaCl
solution without inhibitor after a) 1 hour, b) 24 hours, with 2-MBT (saturated)
after c) 1 hour, d) 24 hours and e) 72 hours.
24
Figure 7. Cathodic potentiodynamic polarization of AA 2024-T3 electrodes in
3.5% NaCl solution a) without inhibitor, with b) 1.5 mM CeCl3, c) 2-MBT
(saturated) and d) 2-MBT (saturated) + 1.5 mM CeCl3 after 24 hours of
immersion.
25
Figure 8. Time evolution of the current density from the split-cell tests for AA
2024-T3 electrodes with addition of the individual inhibitor. a) without inhibitor,
with b) 1.5 mM CeCl3 and c) 2-MBT (saturated) in the cathodic side and 2-MBT
(saturated) in the anodic side (d). The arrows indicate the time of addition of the
inhibitor in the compartment.
26
Figure 9. a) Bode and b) Nyquist plots for AA 2024-T3 electrodes without
inhibitor, with 2-MBT (saturated) and 2-MBT (saturated) + 0.075mM CeCl3.
The inset graph in Figure b is the magnification of AA 2024-T3 without
inhibitor. The symbols present the EIS spectra and the lines present the
calculated spectra from the values reported in Table 1.
27
Figure 10. Schematic representation of AA 2024-T3 electrode and the electrical
circuit model used for fittings. All the fitted values are reported in Table 1.
28
Figure 11. a) Bode and b) Nyquist plots for AA 2024-T3 electrodes at -0.610 V vs
SCE without inhibitor, with 2-MBT (saturated) and 2-MBT (saturated) +
0.075mM CeCl3. The inset graph in Figure b is the magnification of AA 2024-T3
without inhibitor. The symbols present the EIS spectra and the lines present the
calculated spectra from the values reported in Table 2.
29
Figure 12. Schematic representation of AA 2024-T3 electrode at -0.610 V vs SCE
and the electrical circuit model used for fittings. All the fitted values are reported
in Table 2.
Table 1. The fitted parameters obtained from the circuit presented in Figure 10
for AA 2024-T3 electrodes without inhibitor, with 2-MBT (saturated) and 2-
MBT (saturated) + 0.075mM CeCl3.
AA 2024-T3 with 2-MBT (saturated)
Time 1 h 24 h 48 h 72 h
error error error error
Rsol Ω cm2 4.96 ±0.055 4.89 ±0.881 4.23 ±0.333 3.21 ±1.51
Coxide μF cm-2 6.18 ±0.064 1.17 ±2.16 3.72 ±1.92 1.02 ±1.48
Rcorr pr Ω cm2 111 ±14.8 0.59 ±1.39 2.44 ±1.6 2.3 ±0.95
Cdl μF cm-2 6.33 ±0.157 14.3 ±1.97 12.47 ±1.69 14.98 ±1.38
ndl 0.831 ±0.005 0.921 ±0.018 0.901 ±0.024 0.927 ±0.01
Rpol Ω cm2 61471 ±1515 60002 ±1646 60737 ±1560 50041 ±586.58
30
Ws-R Ω cm2 31385 ±3363 48314 ±5268 30731 ±3949 29818 ±1585
Ws-T sec-1 46.8 ±8.34 69.5 ±11.7 52.7 ±7.7 56.8 ±4.37
Ws-P 0.46 ±0.036 0.524 ±0.031 0.587 ±0.041 0.526 ±0.017
X2 1.42×10-3 2.37×10-3 3.82×10-3 4.19×10-4
AA 2024-T3 with 2-MBT (saturated) + 0.075mM CeCl3
Time 1 h 24 h 48 h 72 h
error error error error
Rsol Ω cm2 4.37 ±0.049 4.56 ±0.065 5.09 ±0.093 4.37 ±0.096
Coxide μF cm-2 6.76 ±0.066 8.29 ±0.079 9.44 ±0.12 8.8 ±0.624
Rcorr pr Ω cm2 91.6 ±9.66 172 ±9.15 308 ±33.4 23.9 ±37.7
Cdl μF cm-2 13.5 ±0.273 19.1 ±0.426 26 ±0.813 23 ±0.617
ndl 0.78 ±0.005 0.843 ±0.006 0.752 ±0.01 0.697 ±0.021
Rpol Ω cm2 31145 ±662 37968 ±1063 49915 ±2688 44278 ±3875
Ws-R Ω cm2 36772 ±1471 54755 ±3045 53163 ±5774 82294 ±9067
Ws-T sec-1 38.5 ±2.27 52.5 ±3.65 52.2 ±5.93 83.5 ±16.4
Ws-P 0.525 ±0.014 0.593 ±0.017 0.617 ±0.033 0.479 ±0.029
X2 1.07×10-3 2.47×10-3 4.9×10-3 1.74×10-3
AA 2024-T3 no inhibitor
Time 24 h
error
Rsol Ω cm2 3.826 ±0.078
Coxide μF cm-2 55.4 ±8.53
Rcorr pr Ω cm2 2.53 ±0.720
Cdl μF cm-2 150.5 ±10.8
ndl 0.892 ±0.01
Rpol Ω cm2 913 ±27.98
Ws-R Ω cm2 19352 ±2075
Ws-T sec-1 255.7 ±48.2
Ws-P 0.682 ±0.013
X2 5.23×10-3
31
Table 2. The fitted parameters obtained from the circuit presented in Figure 12
to fit the EIS spectra at potential -0.610 V vs SCE for AA 2024-T3 electrodes
without inhibitor, with 2-MBT (saturated) and 2-MBT (saturated) + 0.075mM
CeCl3.
AA 2024-T3
-0.610 V vs SCEAA 2024-T3 with 2-
MBT (sat)
-0.610 V vs SCE
AA 2024-T3 with 2-MBT
(sat) + 0.075mM CeCl3
-0.610 V vs SCE
Time 24 h 24 h 24 h
error error error
Rsol Ω cm2 4.21 ±0.034 3.53 ±0.124 5.1 ±0.069
Coxide μF cm-2 146 ±196 27.2 ±6.65 25.6 ±4.05
noxide 0.926 ±0.129 0.898 ±0.017 0.91 ±0.017
Rcorr pr Ω cm2 2.5 ±1.6 59.7 ±268.07 221 ±73.1
Cdl μF cm-2 252 ±207 0.86 ±5.46 9.55 ±3.94
ndl 0.881 ±0.058 0.991 ±0.55 0.941 ±0.047
Rct Ω cm2 650 ±18.9 19848 ±1176 31856 ±616
Ws-R Ω cm2 1084 ±45.7 26919 ±14751 24598 ±12103
Ws-T sec-1 22.4 ±1.52 22.3 ±3.2 77.6 ±3.11
Ws-P 0.525 ±0.014 0.811 ±0.034 0.967 ±0.019
Ranod Ω cm2 - - 5283 ±591 12761 ±4326
Lanod Ω s cm2 - - 105240 ±13172 658410 ±88596
X2 1.47×10-3 26.8×10-3 5.13×10-3
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