Materials Sciences and Applicatio ns, 2011, 2, 546-554
doi:10.4236/msa.2011.26073 Published Online June 2011 (http://www.SciRP.org/journal/msa)
Copyright © 2011 SciRes. MSA
Corrosion Behavior of Cu60Zr30Ti10 Metallic Glass
in the Cl Containing Solution
Wei-Ke An1, An-hui Cai1,2, Xiang Xi o ng2, Yong Liu2, Yun Luo1, Tie-lin Li1, Xiao-Song Li1
1College of Mechanical Engineering, Hunan Institute of Science and Technology, Yueyang, China; 2State Key Laboratory of Powder
Metallurgy, Central South University, Changsha, China.
Email: anweike12@163.com
Received December 24th, 2010; revised March 10th, 2011; accepted April 6th, 2011.
ABSTRACT
Cu60Zr30Ti10 (at%) ribbon was prepared by melt spinning. Its glassy structure was confirmed by X-ray diffraction
(XRD). Its corrosion behavior in HCl and NaCl solutions was investigated by electrochemical polarization measure-
ment. The surfaces before and after corrosion were observed with scanning electron microscope (SEM) and analysis
was performed using electron dispersive spectroscopy (EDS). The results show that the decrease of current density is
due to the formation of a mixture of simple oxides or complex oxidic compounds. In both cases, the corrosion potential
decreases with increasing chloride concentration. The passive film forms easier in HCl than in NaCl. In addition, the
higher is the chloride concentration, the easier is the passivation.
Keywords: Metallic Glass, Corrosion Behavior, Chloride Media
1. Introduction
Metallic glasses have acquired significant attention from
the scientific and technological viewpoints. They usually
show high strength, a large elastic strain limit, and ex-
cellent wear and corrosion resistances, along with other
remarkable engineering properties [1]. A number of me-
tallic glasses have been used in practical applications.
For example, Pd-Cu-Ni-P metallic glasses were used as
die materials while Zr-based metallic glasses were used
for sporting equipments. In addition, the metallic glasses
have also been proposed for some biomedical applica-
tions [2,3]. For example, it can be used for making bone
fracture fixation and hip arthroplasty components where
a low modulus comparable to bone is critical to avoid
stress shielding. Furthermore, the superior strength
would permit a smaller, less intrusive device that would
be capable of withstanding the large forces generated
within the skeletal system of the human body [2]. How-
ever, the applications of the metallic g lasses require high
chemical stability in various environments in order to
ensure its lifetime. Without high corrosion resistance in
the service environments, their favorable mechanical
properties cannot be fully exploited. Up to now, a num-
ber of corrosion studies have already been reported for
metallic glasses in different corrosive media [4-11]. In
order to expand the fields of applications of the metallic
glasses, the development of new metallic glasses with
better mechanical properties and higher corrosion resis-
tance for lower cost is desirable. Compared with Zr- and
Pd-based metallic glasses, Cu-based metallic glasses ex-
hibit even higher mechanical properties and lower cost
[12,13]. The Cu-Zr-Ti ternary system is a typical glass
forming system first explored by Inoue’s group [14]. The
maximum size for glass formation in this system can be
up to 5 mm [13]. However, it is found that the corrosion
resistance of Cu-based metallic glasses is low in acidic
solutions, especially when chloride ions are present [15].
In order to apply this type of metallic glasses as engi-
neering materials, the corrosion resistance and the effect
of additiona l elements on Cu-based metallic g lasses, such
as Cu-Zr [10,11], Cu-Zr-Ti-Nb [16], Cu-Hf-Ti-(Mo, Ta
and Nb) [17], Cu-Zr-Ti-Ni-(Nb, Cr, Mo and W) [18-20],
Cu-Zr-Ti-(Mo, Ta and Nb) [15], and Cu-Zr-Al-Y [21]
have been carried out. Many researches have shown that
they are strongly susceptible to chloride-induced pitting
corrosion. For example, Zender, et al. [22] investigated
the corrosion performances of Cu46Zr42Al7Y5 and Zr58.5
Cu15.6Ni12.8Al10.3Nb2.8 bulk metallic glasses in 0.001 - 0.1
M HCl aqueous solutions. They found that in both cases
the corrosion potential changed to more positive poten-
tials and the corrosion current increased with increasing
chloride concentration. However, the pitting potential
Corrosion Behavior of CuZr Ti Metallic Glass in the Cl Containing Solution547
6030 10
decreased and the usable passive region became smaller
with increasing chloride concentration. Recently, Gostin,
et al. [5] have investigated the corrosion behavior of
(Fe44.3Cr5Co5Mo12.8Mn11.2C15.8B5.9)98.5Y1.5 bulk metallic
glass in 0.01 - 0.6 M NaCl aqueous solutions. They
found that the corrosion potential was larger in 0.01 M
NaCl aqueous solution than in 0.1 and 0.6 M NaCl
aqueous solutio ns. Thus, it is of interest to investigate the
influence of the Cl concentration on the corrosion prop-
erty of metallic glasses. In present work, the corrosion
behavior of Cu60Zr30Ti10 metallic glass is investigated in
HCl and NaCl aqueous solutions with different Cl con-
centration.
2. Experimental
Cu60Zr30Ti10 (at%) ternary alloy ingots were prepared
from the mixture of pure metals by arc melting in an ar-
gon atmosphere. Ribbon samples with a thickness of 50
μm and a width of 1.3 mm were prepared by melt spin-
ning at the wheel speed of 30 ms–1. The glassy structure
was confirmed by X-ray diffraction (XRD) using Cu Kα
radiation.
Corrosion behavior of the glassy alloys was investi-
gated by electrochemical polarization measurement.
Prior to electrochemical measurements, the specimens
were degreased in acetone, washed in distilled water and
dried in air. Electrolytes were NaCl and HCl aqueous
solutions whose concentrations were 0.005, 0.01, 0.5,
and 1 M, respectively, which were prepared from reagent
grade chemicals and deionized water. Electrochemical
measurements were conducted using a three-electrode
cell with a platinum foil as a counter electrode. The ref-
erence electrode was a standard saturated calomel elec-
trode (SCE). All potentials given in this article are re-
ferred to the SCE electrode. Potentiodynamic polariza-
tion curves were measured with an IM6ex instrument at a
potential sweep rate of 0.05 mV·s–1. The cell was open to
air at room temperature and measurement started after
the immersion of the samples for 20 min so that the
open-circuit potentials of the samples became almost
stable. The working electrode was exposed only to an
area of 0.04 - 0.08 cm2 while the rest of the specimen
was embedded in a thermoplastic resin to provide elec-
trical isolation. The surfaces of before and after corrosion
were observed with an SIRION scanning electron mi-
croscope (SEM) and analysis was performed using elec-
tron dispersive spectroscopy (EDS).
3. Results
The glassy structure of Cu60Zr30Ti10 alloy was con-
firmed by XRD, the resu lt of which is shown in Figure
1. The diffraction pattern exhibits the characteristic
broad peak for a glassy structure without any distinct
Figure 1. X-ray diffraction pattern for Cu60Zr30Ti10 glassy
alloy.
crystalline peaks within the sensitivity limit of XRD
measurement, indicating the amorphous state of the
melt-spun Cu60Zr30Ti10 ribbon.
The corrosion behavior of the Cu60Zr30Ti10 glassy alloy
was examined by potentiodynamic polarization meas-
urement. To ensure reproducibility, at least three meas-
urements were run for each specimen. Figure 2 shows
the anodic and cathodic polarization curves in NaCl and
HCl aqueous solutions open to air at room temperature,
respectively. As shown in Figures 2(a) and (b), the an-
odic current density increases rapidly without the pres-
ence of any passive region when the Cl concentration is
less than 0.5 M. This indicates that the glassy alloy un-
dertakes strong active dissolution upon anodic polariza-
tion and accordingly has a poor corrosion resistance in
less than 0.5 M Cl solutions. However, the passive pro-
cedure starts out in more than 0.5 M Cl solutions. The
passive potentials are 0.57 V vs SCE in 0.5 M HCl, 0.52
V vs SCE in 1 M HCl, 0.66 V vs SCE in 0.5 M NaCl,
and 0.52 V vs SCE in 1 M NaCl, respectively. In addi-
tion, the large passive current density up to 0.01 Am–2
indicates the pseudopassive behavior. Comparing with
Figure 2(a) and Figure 2(b), the passive potentials in 1
M HCl and 1 M NaCl are hardly the same, indicating the
same passive ability of this glassy alloy in two solutions.
However, the passive potential is larger in 0.5 M Cl so-
lution than in 1 M Cl solution, indicating that the pas-
sive procedure easily sets out under higher Cl concen-
tration. In addition, the passive potential is larger in 0.5
M NaCl than in 0.5 M HCl, indicating that the passive
procedure happens easier in 0.5 M HCl than in 0.5 M
NaCl.
On the other hand, the values of the corrosion current
density icorr were determined by graphical extrapolation
from the polarization curves. The intersection point of
Copyright © 2011 SciRes. MSA
Corrosion Behavior of CuZr Ti Metallic Glass in the Cl Containing Solution
548 6030 10
the vertical line corresponding to the corrosion potential
Ecorr, with the tangents on the anodic and cathodic
branches was determined. The Ecorr and icorr values in all
solutions are listed in Table 1. The relationship between
the Cl concentration and Ecorr is plotted in Figure 3. It is
clearly observed that the corrosion potential decreases
with increasing Cl concentration in both HCl and NaCl.
It indicates that the stability of the metallic glass de-
creases with increasing Cl concentration at thermody-
namic point of view. The relationship between the Cl
concentration and icorr is plotted in Figure 4. The corro-
sion current density in HCl solution slightly increases
when the Cl concentration is less than 0.1 M, and then
decreases with increasing Cl concentration. It indicates
that the general corrosion decreases when the HCl con-
centration exceeds 0.1 M. The corrosion current density
sharply decreases with increasing NaCl concentration,
and then maintains a low value when the NaCl concen-
tration exceeds 0.1 M.
In addition, the corrosion rate was calculated by Fara-
day’s law [23]:
7
3.16 10
Corrosion rate(cmy)corr
iM
zF

 , (1)
where icorr is the corrosion cu rrent density (A·cm–2), M is
the molar mass of the metal (g·mol–1), z is number of
electrons transferred per metal atom, F is the Faraday’s
constant, and ρ is the density of the metal (g·cm–3). The
corrosion rate values in all solutions are listed in Table 1 .
The relationship between the corrosion rate and the Cl
concentration is plotted in Figure 5. As shown in Figure
5, the corrosion rate increases when the HCl concentra-
tion is less than 0.1 M, and then decreases with increas-
ing Cl concentration. It indicates that the corrosion re-
sistance increases when the HCl concentration exceeds
0.1 M. However, the corrosion rate decreases with in-
creasing NaCl concentration, and then maintains a low
value when the NaCl concentration exceeds 0.1 M.
Furthermore, SEM was employed to investigate the
morphologies of the samples after polarization tests. Fig-
ure 6 and Figure 7 show the SEM micrographs of the
surfaces corroded in HCl and NaCl solutions, respec-
tively. As shown in Figures 6(a)-(c), the pits can be
clearly observed on the surfaces in less than 0.5 M HCl
solutions, indicating the occurrence of the pitting in less
than 0.5 M HCl solutions. However, the pits disappear
and the cracked passive film due to the heavy attack of
corrosion can be observed in 1 M HCl, as shown in Fig-
ure 6(d). As shown in Figure 6(a) and Figure 6(b), the
number and depth of the pits increase with increasing
chloride concentration, indicating the decrease of the
corrosion resistance. However, the number of the pits
obviously decreases and the passive film can be observed
Table 1. The corrosion potential Ecorr, corrosion current
density icorr, and corrosion rate of Cu60Zr30Ti10 glassy alloy.
Type of
solution Concentration
M Ecorr
mV vs SCE icorr
Am-2 Corrosion rate
cm/y
0.005 12.79 2.19 0.34
0.01 2.30 2.39 0.37
0.5 –59.94 1.04 0.16
HCl
1 –76.91 0.48 0.08
0.005 23.45 2.70 0.42
0.01 3.89 0.33 0.05
0.5 –63.07 0.83 0.13
NaCl
1 –78.12 0.17 0.03
Current density i, A·cm
–2
(a)
Current density i, A·cm
–2
(b)
Figure 2. The polarization curves in aqueous solutions con-
taining different Cl concentration open to air at room
temperature. (a) For HCl; (b) For NaCl.
Copyright © 2011 SciRes. MSA
Corrosion Behavior of CuZr Ti Metallic Glass in the Cl Containing Solution549
6030 10
Figure 3. The relationships between the Cl concentration
and corrosion potential Ecorr.
Corrosion current density, A·cm
–2
Figure 4. The relationships between the Cl concentration
and corrosion current density icorr.
Corrosion rate, cm·y
–1
Figure 5. The relationships between the Cl concentration
and the corrosion rate.
(shown in Figures 6(c) and (d)), indicating the increase
of the corrosion resistance. As shown in Figure 7, the
pits and corrosion products distribute on the surfaces
corroded in all NaCl solutions. The size of the pits de-
creases with increasing chloride concentration, indicating
the increase of the corrosion resistance. However, the
number of the pits in 0.5 M NaCl increases, which would
be a reason for the decrease of the corrosion resistance.
In addition, in order to clearly observe the passive film,
the enlarged SEM microstructures in 0.5 and 1 M NaCl
solutions are shown in Figure 8. One can clearly observe
from Figure 8 that the local passive film appears. These
SEM results are in coherent with the potentiodynamic
polarization measurements.
4. Discussion
As shown in Figure 6 and Figure 7, the pits display on
all corroded surfaces except for in 1 M HCl, indicating
that the Cu60Zr30Ti10 metallic glass is susceptible to pit-
ting corrosion in chloride media. However, the pitting
corrosion doesn’t appear in the potentiodynamic polari-
zation curves, as shown in Figure 2. The reasons would
be as follows. Ideally, metallic glasses are regarded as
being physically and chemically homogeneous, free from
secondary phases or inclusions which should diminish or
prevent the occurrence of galvanic or localized corrosion
[24]. However, in practice the presence of defects in cast
samples cannot be completely avoided, at least in com-
mercial production [25]. Not surprisingly, several studies
show that some metallic glasses have high pitting sus-
ceptibility and pits are initiated at the interface between
such defects and the surrounding matrix [5, 10, and 26].
The surface morphology of the melt-spun glassy ribbon
is illustrated in Figure 9. There ar e three types of r egions,
including the relatively flat region, the troughs, and the
pores. It would be a reason for the pitting corro sion. The
other reason would be the selective dissolution of Ti and
Zr, and/or simultaneous dissolution of Cu, Ti and Zr
[10,27-29].
As shown in Figure 2, there is a sharply increase of
current density in polarization curve when the chloride
concentration exceeds 0.5 M. It is generally thought of
the formation of a CuCl film on the surface in chloride
media [10, 30 and 31]. In order to further investigate the
composition of the passive film, the EDS analysis was
performed on the passive films in 1 M HCl and 1 M
NaCl. The results are shown in Table 2. It is clearly from
Table 2 that the compositions for the passive film consist
of O, Zr, Ti, and Cu, respectively. It indicates that the
passive film is composed of a mixture of simple oxides
or complex oxidic compounds .of all alloying elements.
Earlier corrosion studies of Zr69.5Cu12Ni11Al7.5 showed
that the formation of an amorphous ZrO2 layer [32]. Cu
Copyright © 2011 SciRes. MSA
Corrosion Behavior of Cu60Zr30Ti10 Metallic Glass in the Cl Containing Solution
Copyright © 2011 SciRes. MSA
550
is known to form a protective passive layer of CuO in
chloride solution [33]. Corrosion investigations of
Cu50Zr40Al5Nb5 in 0.5 M NaCl [34] indicated the deple-
tion of Cu in surface film and increases Zr and Nb, lead-
ing to the formation of a Zr (Nb)-rich protective surface
film. In addition, it is clearly from Figure 2 that the pas-
sive potential decreases with increasing chloride concen-
tration. This would be due to the fact that the pure ele-
ment displays a lower passive potential in higher chloride
concentration. For example, the pure zirconium shows a
stable passive state up to +0.15V in 1.0 mol/L HCl and
+0.25V in 0.1 mol/L HCl, resp ectively [10,35]. Thu s, the
higher is the chlorid e concentration, the easier is the pas-
sivation.
Comparing with Figure 6(d) and Figure 7(d), the pit
does not appear on the surface corroded in 1 M HCl,
while appear on the surface corroded in 1 M NaCl. It
would be related with the different distribution of the
alloying elements on the surface in HCl and NaCl solu-
tions because the corrosion of metallic glass is strongly
influenced by the alloying elements [22]. Asami, et al. [15]
investigated the concentration of the alloying elements of
(a) (b)
(c) (d)
Figure 6. SEM micrographs of the corroded surfaces in different HCl concentrations, (a) 0.005 M; (b) 0.01 M; (c) 0.5 M; (d) 1
M, respectively.
Corrosion Behavior of CuZr Ti Metallic Glass in the Cl Containing Solution551
6030 10
(a) (b)
(c) (d)
Figure 7. SEM micrographs of the corroded surfaces in different NaCl concentrations, (a) 0.005 M; (b) 0.01 M; (c) 0.5 M; (d)
1 M, respectively.
Cu60Zr30Ti10 metallic glass on the surface immersed in 1
N HCl and 3% NaCl, respectively. They found that the
cationic fraction of the surface film after immersion in
3% NaCl was almost the same as the alloy composition,
but in the surface film formed in 1 N HCl solution, its
cationic fraction of Cu was more than the alloy composi-
tion. In addition, one can observe from Table 2 that the
content of Cu and Zr + Ti is more in 1 M HCl than in 1
M NaCl. Thus, one can presume that the passive film
forms easier and faster in HCl than in NaCl, resulting in
the formation of the passive film to prevent the occur-
rence of the pitting corrosion in 1 M HCl. On the other
hand, it is well-known that Cu is nobler than Zr and Ti,
i.e. the standard equilibrium electrode potentials for the
Zr/Zr4+, Cu/Cu2+ and Ti/Ti2+ couples are –1.529 VSHE,
+0.337 VSHE and –1.628 VSH E , respectively. This large
electrochemical potential difference between Cu and Zr
(Ti) can provide a sufficient potential window for a se-
lective dissolution of Zr (Ti) in Cu-Zr-Ti metallic glass.
In addition, the stability of the oxide of the alloying ele-
ment is different from each other. For example, Zr- and
Ti-oxides are more stable chemically and denser struc-
Copyright © 2011 SciRes. MSA
Corrosion Behavior of CuZr Ti Metallic Glass in the Cl Containing Solution
552 6030 10
(a) (b)
Figure 8. The enlarged SEM micrographs related to the passive films in 0.5 M NaCl (a) and 1 M NaCl (b), respectively.
Figure 9. SEM surface morphology of the ribbon before
corrosion.
turally than Cu-oxides [20 ]. These results would result in
the different corrosion behavior in HCl and NaCl.
5. Conclusions
The influence of the concentration of HCl and NaCl so-
lutions on corrosion properties of Cu60Zr30Ti10 glassy
alloy was investigated. The results are as follows.
The corrosion potential decreases with increasing
chloride concentration in HCl and NaCl. It indicates that
the stability of the metallic glass decreases with increas-
ing chloride concentration at thermodynamic point of
Table 2. Content of alloying elements in passive film in 1 M
HCl and 1 M NaCl, respectively.
O (at%) Zr (at%) Ti (at%) Cu (at%)
1 M HCl 33.63 21.48 3.97 40.91
1 M NaCl45.32 13.70 7.36 33.62
view.
The corrosion current density and corrosion rate in
HCl solution slightly increase, and then decrease when
the chloride concentration exceeds 0.1 M. However, the
corrosion current density and corrosion rate sharply de-
crease with increasing NaCl concentration, and then
maintain a low value when the NaCl concentration ex-
ceeds 0.1 M.
The passive film can form when the chloride concen-
tration exceeds 0.5 M in HCl and NaCl solutions. The
passive potentials are 0.57 V vs SCE in 0.5 M HCl, 0.52
V vs SCE in 1 M HCl, 0.66 V vs SCE in 0.5 M NaCl,
and 0.52 V vs SCE in 1 M NaCl, respectively. This indi-
cates that the higher is the chloride concentration, the
easier is the passivation. The passive film is composed of
a mixture of simple oxides or complex oxidic compounds
of all alloying elements.
The passive film forms easier in HCl than in NaCl,
which is due to the different distribution of the alloying
elements on the surface in HCl and NaCl solutions.
6. Acknowledgements
This work was financially supported by the National
Natural Science Foundation (Grant No. 50874045),
Copyright © 2011 SciRes. MSA
Corrosion Behavior of CuZr Ti Metallic Glass in the Cl Containing Solution553
6030 10
Postdoctoral Science Foundation of China (Grant Nos.
20080431021 and 200902472), Postdoctoral Science
Foundation of Hunan Province (Grant No. 2008RS4021),
and Scientific Research Fund of the Hunan Provincial
Education Department (Grant No. 10A044).
REFERENCES
[1] W. H. Wang, C. Dong and C. H. Shek, “Bulk Metallic
Glasses,” Materials Science and Engineering: Reports,
Vol. 44, No. 2-3, 2004, pp. 45-89.
doi:10.1016/j.mser.2004.03.001
[2] M. L. Morrison, R. A. Buchanan, R. V. Leon, C. T. Liu,
B. A. Green, P. K. Liaw and J. A. Horton, “The Electro-
chemical Evaluation of a Zr-Based Bulk Metallic Glass in
a Phosphate-Buffered Saline Electrolyte,” Journal of
Biomedical Materials Research A, Vol. 74A, No. 3, 2005,
pp. 430-438. doi:10.1002/jbm.a.30361
[3] S. Hiromoto, A. P. Tsai, M. Sumita and T. Hanawa, “Ef-
fect of Chloride Ion on the Anodic Polarization Behavior
of the Zr65Al7.5Ni10Cu17.5 Amorphous Alloy in Phosphate
Buffered Solution,” Corrosion Science, Vol. 42, No. 9,
2000, pp. 1651-1660.
[4] A. P. Wang, X. C. Chang, W. L. Hou and J. Q. Wang,
“Corrosion Behavior of Ni-Based Amorphous Alloys and
Their Crystalline Counterparts,” Corrosion Science, Vol.
49, No. 6, 2007, pp. 2628-2635.
doi:10.1016/j.corsci.2006.12.017
[5] P. F. Gostin, A. Gebert and L. Schultz, “Comparison of
the Corrosion of Bulk Amorphous Steel with Conven-
tional Steel,” Corrosion Science, Vol. 52, No. 1, 2010, pp.
273-281. doi:10.1016/j.corsci.2009.09.016
[6] Z. M. Zhang, J. Zhang, X. C. Chang, W. L. Hou and J. Q.
Wang, “Structure Inhibited Pit Initiation in a Ni-Nb Me-
tallic Glass,” Corrosion Science, Vol. 52, No. 4, 2010, pp.
1342-1350.
[7] R. V. S. Rao, U. Wolff, S. Baunack, J. Eckert and A.
Gebert, “Corrosion Behaviour of the Amorphous Mg65Y10
Cu15Ag10 Alloy,” Corrosion Science, Vol. 45, No. 4,
2003, pp. 817-832.
doi:10.1016/S0010-938X(02)00131-2
[8] S. J. Pang, T. Zhang, K. Asami and A. Inoue, “Bulk
Glassy Fe-Cr-Mo-C-B Alloys with High Corrosion Re-
sistance,” Corrosion Science, Vol. 44, No. 8, 2002, pp.
1847-1856. doi:10.1016/S0010-938X(02)00002-1
[9] A. Gebert, P. F. Gostin and L. Schultz, “Effect of surface
Finishing of a Zr-Based Bulk Metallic Glass on Its Cor-
rosion Behaviour,” Corrosion Science, Vol. 52, No. 5,
2010, pp. 1711-1720. doi:10.1016/j.corsci.2010.01.027
[10] H. B. Lu, Y. Li and F. H. Wang, “Dealloying Behaviour
of Cu–20Zr Alloy in Hydrochloric Acid Solution,” Cor-
rosion Science, Vol. 48, No. 8, 2006, pp. 2106-2119.
doi:10.1016/j.corsci.2005.08.009
[11] H. B. Lu, L. C. Zhang, A. Gebert and L. Schultz, “Pitting
Corrosion of Cu-Zr Metallic Glasses in Hydrochloric
Acid Solutions,” Journal of Alloys Compounds, Vol. 462,
No. 1-2, 2008, pp. 60-67.
doi:10.1016/j.jallcom.2007.08.023
[12] A. Inoue, “Stabilization of Metallic Supercooled Liquid
and Bulk Amorphous Alloys,” Acta Materialia, Vol. 48,
No. 1, 2000, pp. 279-306.
doi:10.1016/S1359-6454(99)00300-6
[13] A. Inoue, W. Zhang, T. Zhang and K. Kurosaka, “High-
Strength Cu-Based Bulk Glassy Alloys in Cu-Zr-Ti and
Cu-Hf-Ti Ternary Systems,” Acta Materialia, Vol. 49, No.
14, 2001, pp. 2645-2652.
doi:10.1016/S1359-6454(01)00181-1
[14] A. Inoue, W. Zhang, T. Zhang and K. Kurosaka, “Ther-
mal and Mechanical Properties of Cu-Based Cu-Zr-Ti
Bulk Glassy Alloys,” Materials Transactions JIM, Vol.
42, No. 6, 2001, pp. 1149-1151.
doi:10.2320/matertrans.42.1149
[15] K. Asami, C. Qin, T. Zhang and A. Inoue, “Effect of Ad-
ditional Elements on the Corrosion Behavior of a
Cu-Zr-Ti Bulk Metallic Glass,” Materials Science and
Engineering: A, Vol. 375-377, No. 7, 2004, pp. 235-239.
doi:10.1016/j.msea.2003.10.034
[16] C. Qin, K. Asami, T. Zhang, W. Zhang and A. Inoue,
“Corrosion Behavior of Cu-Zr-Ti-Nb Bulk Glassy Al-
loys,” Materials Transactions JIM, Vol. 44, No. 4, 2003,
pp. 749-753. doi:10.2320/matertrans.44.749
[17] F. R. Niessen, “Cohesion in Metals,” Elsevier Science,
Amsterdam, 1988.
[18] T. Yamamoto, C. Qin, T. Zhang, K. Asami and A. Inoue,
“Formation, Thermal Stability, Mechanical Properties and
Corrosion Resistance of Cu-Zr-Ti-Ni-Nb Bulk Glassy
Alloys,” Materials Transactions JIM, Vol. 44, No. 6,
2003, pp. 1147-1152. doi:10.2320/matertrans.44.1147
[19] B. Liu and L. Liu, “Improvement of Corrosion Resistance
of Cu-Based Bulk Metallic Glasses by the Microalloying
of Mo,” Intermetallics, Vol. 15, No. 5-6, 2007, pp. 679-
682. doi:10.1016/j.intermet.2006.10.039
[20] B. Liu and L. Liu, “The Effect of Microalloying on Ther-
mal Stability and Corrosion Resistance of Cu-Based Bulk
Metallic Glasses,” Materials Science and Engineering: A,
Vol. 415, No.1-2, 2006, pp. 286-290.
doi:10.1016/j.msea.2005.09.099
[21] M. K. Tam, S. J. Pang and C. H. Shek, “Corrosion Be-
havior and Glass-Forming Ability of Cu-Zr-Al-Nb Al-
loys,” Journal of Non-Crystalline Solids, Vol. 353, No.
32-40, 2007, pp. 3596-3599.
[22] D. Zander, B. Heisterkamp and I. Gallino, “Corrosion
Resistance of Cu-Zr-Al-Y and Zr-Cu-Ni-Al-Nb Bulk
Metallic Glasses,” Journal of Alloys and Compound, Vol.
434-435, No. 5, 2007, pp. 234-236.
doi:10.1016/j.jallcom.2006.08.112
[23] D. A. Jonse, “Principles and Prevention of Corrosion,”
Printice-Hall, New Jersey, 1996.
[24] K. Hashimoto, “Chemical Properties,” In: F. E. Luborsky
Ed., Amorphous Metallic Alloys, Butterworth, London,
1983, p. 53.
[25] Y. H. Liu, G. Wang, R. J. Wang, D. Q. Zhao, M. X. Pan
and W. H. Wang, “Super Pla stic Bulk Metallic Glasses at
Copyright © 2011 SciRes. MSA
Corrosion Behavior of Cu60Zr30Ti10 Metallic Glass in the Cl Containing Solution
Copyright © 2011 SciRes. MSA
554
Room Temperature,” Science, Vol. 315, No. 3, 2007, pp.
1385-1388. doi:10.1126/science.1136726
[26] A. Gebert, U. Kuehn, S. Baunack, N. Mattern and L.
Schultz, “Pitting Corrosion of Zirconium-Based Bulk
Glass-Matrix Composites,” Materials Science and Engi-
neering: A, Vol. 415, No. 1, 2006, pp. 242-249.
doi:10.1016/j.msea.2005.09.062
[27] G. Kear, B. D. Barker and F. C. Walsh, “Electrochemical
Corrosion of Unalloyed Copper in Chloride Media—A
Critical Review,” Corrosion Science, Vol. 46, No. 1,
2004, pp. 109-135. doi:10.1016/S0010-938X(02)00257-3
[28] M. Chmielová, J. Seidlerová and Z. Weiss, “X-Ray Dif-
fraction Phase Analysis of Crystalline Copper Corrosion
Products after Treatment in Different Chloride Solu-
tions,” Corrosion Science, Vol. 45, No. 5, 2003, pp.
883-889. doi:10.1016/S0010-938X(02)00176-2
[29] A. V. Vvedenskii and S. N. Grushevskaya, “Kinetic Pe-
culiarities of Anodic Dissolution of Copper and Its Gold
Alloys Accompanied by the Formation of Insoluble Cu (I)
Products,” Corrosion Science, Vol. 45, No. 10, 2003, pp.
2391-2413. doi:10.1016/S0010-938X(03)00064-7
[30] R. S. Copper and J. H. Bartlett, “Convection and Film
Instability Copper Anodes in Hydrochloric Acid,” Jour-
nal of the Electrochemical Society, Vol. 105, No. 3, 1958,
pp. 109-116. doi:10.1149/1.2428773
[31] L. Stephenson and J. H. Bartlett, “Anodic Behavior of
Copper in HCl,” Journal of the Electrochemical Society,
Vol. 101, No. 11, 1954, pp. 571-581.
doi:10.1149/1.2781156
[32] D. Zander and U. KÖster, “Corrosion of Amorphous and
Nanocrystalline Zr-Based Alloys,” Materials Science and
Engineering: A, Vol. 375-377, No. 7, 2004, pp. 53-59.
doi:10.1016/j.msea.2003.10.230
[33] E. Kunze, “Koeeosion and Korrosionsschutz,” Wiley-
VCH, Weinheim, 2001.
[34] C. Qin, W. Zhang, H. Kimura, K. Asami and A. Inoue,
“New Cu-Zr-Al-Nb Bulk Glassy Alloys with High Cor-
rosion Resistance,” Materials Transactions JIM, Vol. 45,
No. 6, 2004, pp. 1958-1961.
doi:10.2320/matertrans.45.1958
[35] H. Bala and S. Szymura, “Acid Corrosion of Amorphous
and Crystalline Cu-Zr Alloys,” Applied Surface Science,
Vol. 35, No. 1, 1988, pp. 41-51.
doi:10.1016/0169-4332(88)90036-0