Abstract
Titanium is well known as one of the most corrosion-resistant metals. However, it can suffer corrosion attacks in some specific aggressive conditions. To further increase its corrosion resistance, it is possible either to modify its surface, tuning either thickness, composition, morphology or structure of the oxide that spontaneously forms on the metal, or to modify its bulk composition. Part 2 of this review is dedicated to the corrosion of titanium and focuses on possible titanium treatments that can increase corrosion resistance. Both surface treatments, such as anodization or thermal or chemical oxidation, and bulk treatments, such as alloying, are considered, highlighting the advantages of each technique.
Post author correction
Article Type: REVIEW
DOI:10.5301/jabfm.5000396
Authors
Davide Prando, Andrea Brenna, Maria Vittoria Diamanti, Silvia Beretta, Fabio Bolzoni, Marco Ormellese, MariaPia PedeferriArticle History
- • Accepted on 01/11/2017
- • Available online on 21/11/2017
Disclosures
This article is available as full text PDF.
Introduction
Titanium has outstanding corrosion resistance due to a thin, amorphous, nonstoichiometric TiO2 protective layer (max. 10-nm thick (1)) that is formed spontaneously on the surface when exposed to an aerated environment. This protective layer is very stable and allows the use of titanium in severe working conditions, such as offshore; in an acid environment; in aerospace (2, 3) and automotive industries; in high-temperature applications; in the chemical and food industries (4-5-6); and in marine hydrometallurgical applications and nuclear fuel waste containment (7-8-9-10), where no other metal can be used.
Nevertheless, commercially pure titanium may suffer different forms of corrosion in very severe environments (11). Generalized corrosion is caused by small quantities of fluoride ions (more than 0.002 M that combine with titanium, forming TiF4, and destroy the passivity film. Hydrogen embrittlement happens mainly on α and α-β titanium, due to the low hydrogen solubility in α-Ti (12). Stress corrosion cracking can also happen in very specific environments, such as anhydrous methanol, nitrogen tetroxide, red-fuming nitric acid or solid cadmium (13). However, the most critical forms of corrosion of titanium are due to localized breaking of the passive layer, and this is favored by the presence of concentrated halides, such hot salty water (above 200°C) or bromide-containing species (14, 15).
To overcome this weakness, corrosion resistance–enhancing treatments can be completed, or proper alloying elements may be added; the latter is the case with inclusion of elements that promote cathodic reactions, raising the cathodic polarization curve above the critical active anodic curve at higher potentials in the passive region, such as with palladium (16). A well-know treatment is nitration, which involves introducing nitrogen in the first micrometer of the surface to promote the formation of TiN and increase corrosion resistance (17, 18). These methods, acting on the titanium composition, are effective but complicated to perform and expensive, as are other surface coating techniques, such as vacuum plasma spray coating, plasma spraying and chemical vapor deposition (19).
For this reason, treatments that act on the naturally formed passive layer are preferred. The easiest and cheapest treatment to tune the oxide layer is anodic oxidation, which involves applying an anodic polarization of several 10s of volts to the metal, promoting the growth of the natural oxide layer with thicknesses from about 40 nm, with an anodizing potential of 10 V, to about 250 nm at 100 V (20-21-22). At potentials higher than 100 V, the anodizing begins to cause the instauration of microarcs in the insulating oxide layer; in this regime, called
Due to the promising results with increasing corrosion resistance using anodizing treatments, as described in this review the effect of anodizing potential has been investigated, with values ranging from 10 to 200 V, to define a treatment procedure able to delay or prevent localized corrosion in very severe environments.
Surface treatments are greatly influenced by the condition of the initial surface, in terms of roughness and chemical composition. Prior to any anodizing treatment, the surface has to be degreased, cleaned and have any adsorbed chemicals removed; for this reason, pretreatments such as etching and mechanical polishing are required. Moreover, by controlling the conditions of these pretreatments, it is possible to obtain a similar surface roughness on all titanium samples prior to oxidation. However, to perform chemical etching on titanium, a hydrofluoric acid–containing solution has to be used, and this is reported to cause fluoride surface enrichment (24, 25). To investigate the effect of the presence of bromides on anodized titanium corrosion resistance, the same treatments, in terms of final potential, anodizing solution and anodizing current density, are performed on samples prepared with the 2 different pretreatments. The samples are then tested for corrosion resistance.
The corrosion resistance of each metal strongly depends on its surface behavior when exposed to corrosive agents: The development of a protective passive layer is required, to reach a passive state in which corrosion is still proceeding but at such a low rate as to be negligible. For this reason, barrier layer treatments are very important to increase the corrosion resistance of metals. The most common and promising treatments to increase titanium corrosion resistance are described in the next sections.
Anodizing
Anodizing is one of the easiest techniques for modifying the thickness, composition and morphology of oxides appearing on valve metals, such as aluminum and titanium. The treatment involves anodically polarizing a metal to a fixed voltage in an electrochemical cell containing a counter electrode and an electrolyte providing conduction. Common electrolytes are acids, such as H2SO4 and H3PO4, and salts, such as (NH4)2SO4, Na2SO4 and NH4BF4.
The main parameters affecting the characteristics of the resulting oxides are as follows (19, 26, 27):
Current density of anodization;
Anodizing voltage;
Duration;
Electrolyte composition, pH, concentration and temperature;
Agitation of the solution;
Chemical composition and surface finishing of the electrode.
Increasing the current density of anodization accelerates the oxidation rate and increases the amount of oxide converted from an amorphous state to anatase or even rutile crystalline structure (28), as shown in
Relationship between anodization potential and anatase peak intensity on titanium anodized in 0.5 H2SO4 at different current densities (19).
Titanium anodized up to 120 V shows the appearance of a surface color, which is due to interference between light and the oxide layer and is dependent on the oxide thickness, in the range of 10s of 100s of nanometers (29). For this reason, anodizing techniques are distinguished between
Traditional anodizing
Oxide thickness is directly related to anodizing voltage and can be estimated by analysis of the sample reflectance spectrum, following the equation (6):
where
With increasing anodizing voltage, there is an increase in film thickness, crystallinity and porosity. In
Anodic films grown on titanium anodized in sulfuric acid: refractive index, thickness, free corrosion potential and corrosion rate
Anodizing voltage (V) | λmax (nm) | Anodic film refractive index | Anodic film thickness (nm) | Corrosion potential (mV vs. SCE) | Corrosion rate (μ/year) |
---|---|---|---|---|---|
SCE = saturated calomel electrode. | |||||
5 | 259 | 1.458 | 44 | -399.7 | 391 |
10 | 319 | 1.454 | 84 | -365.1 | 2.3 |
15 | 348 | 1.451 | 59 | -339.9 | 0.96 |
20 | 366 | 1.449 | 63 | -336.9 | 2.35 |
25 | 398 | 1.446 | 68 | -355.2 | 1.01 |
30 | 452 | 1.440 | 78 | -293.1 | 4.38 |
35 | 541 | 1.427 | 94 | -287 | 5.41 |
40 | 519 | 1.430 | 90 | -338.5 | 3.51 |
45 | 545 | 1.427 | 95 | -260.3 | 2.87 |
50 | 569 | 1.423 | 99 | -251.4 | 7.78 |
55 | 643 | 1.410 | 114 | -236.9 | 3.16 |
60 | 780 | 1.379 | 141 | -247.2 | 7.3 |
65 | 802 | 1.374 | 145 | -264.9 | 12.21 |
70 | 826 | 1.376 | 150 | -261.9 | 8.67 |
75 | 912 | 1.342 | 169 | -256.2 | 4.95 |
80 | 1000 | 1.311 | 190 | -295.6 | 11.48 |
Several studies have found correlations between applied voltage and film thickness. The anodizing ratio is generally observed to be in the range of 1.5 to 3 nm/V.
The electrolyte used for anodization may vary regarding the ease of film growth, chemical composition of the oxide and oxide crystallinity. In sulfuric acid, for example, anodizing potential was reported to grow faster with a concentration of 0.5 M, within the range from 0.25 M to 2 M studied (19).
Liu et al (33) reported that oxide growth in H2SO4 compared with that in H3PO4 had a higher free corrosion potential, but further observation indicated there was oxide rupture due to oxygen bubbles formed from oxygen evolution during anodization. The oxide rupture appeared to be more severe when produced in 1 M sulfuric acid than 1 M phosphoric acid, indicating that the oxygen evolution reaction was not favored in the phosphoric acid.
Anodizing treatment can be modified to achieve better corrosion resistance; one example of this is the introduction of nitrogen into a titanium lattice prior to anodization. This nitridation can be performed by a plasma nitriding unit, which uses nitrogen plasma in vacuum (34), or through an annealing treatment in a nitrogen environment (35). Nitrogen is reported to have a beneficial effect on anodization due to the fact that TiN is overstoichiometric with a weak bond existing between Ti and N atoms. Thus, while in the conventional anodization process, anatase TiO2 hardly forms on titanium surfaces, because of the passive amorphous film that acts as a barrier to prevent further anodization, the presence of TiN helps oxide growth and crystallization. It should also be noted that titanium has a hexagonal close-packed structure, while TiN has a cubic structure, so oxygen atoms can easily migrate into the TiN crystal structure due to its low atomic packing factor (34).
Anodic spark deposition or plasma electrolytic oxidation
PEO usually forms oxides from 10ths to a 100 micrometers thick (40), with compared with traditional anodizing that produces oxides up to 300 nm. This technique is also interesting because of its ability to transfer chemical species from the electrolyte to the oxide. In fact, local melting and solidification of the oxide leads particles and ions present in the electrolyte to be incorporated into the TiO2.
For instance, by executing the treatment in Na2SiO3, it is possible to enrich the surface layer with Si and Na. At 400 V, this produces a layer with a complex structure composed of an inner portion, adjacent to the titanium, which contains mainly TiO2, and an outer portion built primarily of silicon, sodium and oxygen compounds (41). The outer layer is mostly porous and does not contribute efficiently to corrosion resistance, which is an effect provided by the inner layer. However, morphology, chemical composition and phase composition of the surface are changed, and this finds applications in other fields, such as biomedical implants. In another study (42), the formation of titanium silicides above 250 V was reported: TiSix are known as corrosion resistant compounds, and the electrolyte with the higher amount of Na2SiO3·5H2O and Na3PO4 produces the most corrosion resistant oxide.
A possible explanation for the enhanced corrosion resistance of samples anodized in silicon containing electrolytes is given by Hu et al (43). They found that the higher conductivity of Na2SiO3-containing electrolyte gives a denser microstructure compared with respect electrolytes that do not contain this additive, leading to a more protective and insulating layer.
Babaei et al (44) studied the effect of the addition of Zr-containing species to the anodizing electrolyte: Na2ZrO3 was used for this purpose. They found that ZrOx and ZrTiO4 were formed in the oxide layer during anodization. TiO2 immersed in aggressive media for a long time hydrates to form Ti(OH)4, dissolving into the solution; as ZrO2 has higher stability in aqueous solution, its incorporation into the layer increases the corrosion protection of the metallic substrate, provided by the anodic oxide. On the other hand, the addition of Na2ZrO3 usually decreases electrolyte resistivity, leading to more powerful microdischarges, which create bigger pores on the surface, with a detrimental effect on corrosion resistance.
Chlorides can also be used to tune titanium oxide properties. It is reported that PEO treatment on preanodized surfaces with low-voltage alternating current in a HCl environment causes the growth of a thick and rough oxide, which can be suitable for purposes where multiple scale roughnesses are desired (20) – e.g., in biomedical applications. In contrast, the use of Cl--containing electrolyte during PEO causes the growth of a chlorine-rich region on the oxide, with the formation of TiCl4 species. This phenomenon needs to be avoided, because it causes oxide cracking (45).
The voltage reached during PEO treatment is reported to influence not only film thickness and crystallinity, but also morphology. Galvis et al (23) performed galvanostatic PEO treatment on titanium at 50 mA/cm2 current density, reaching a voltage up to 260 V. They report a transition potential between grooved and porous structure that depended strongly on the composition of electrolyte and weakly on the current density.
The effect of anodizing duration was studied by Mizukoshi et al (46), by anodizing in 1.2 M sulfuric acid for 2, 5, 10, 30 and 60 minutes at 8 mA/cm2 of current density, reaching a maximum voltage of 210 V after 33 minutes. They report an intense dependence of surface structure and oxide crystallinity on anodizing duration, as can be seen in
Scanning electron microscopy (SEM) images of TiO2 surfaces with the progression of anodization (46).
Liu and Thompson (1) have proposed an oxide growth mechanism for anodic spark deposition in phosphoric acid (
Scanning electron microscopy (SEM) images of anodic oxide film formed on titanium after 100 V (
PEO can be carried out in direct current or alternating current; in the case of alternating current, a frequency of 50 Hz or 60 Hz is frequently used. These layers are comparatively thick and provide an excellent wear resistance, but they are porous and therefore provide an insufficient protection against corrosion.
In recent years, PEO at higher frequency has been evaluated. Mann et al (49) studied PEO up to 4 kHz on different metals. In this range, the corrosion resistance of the PEO layer can be significantly improved using bipolar pulses. The higher frequencies and bipolar pulses create layers with lower roughness than direct current layers. The increased density and the smoothness of the layers produced with higher frequencies can be explained by the fact that a shorter duration of the discharge results in smaller surface structures and lower porosity, since pulses with higher frequencies create arcs with shorter discharge time. A smoother surface created with high-frequency bipolar pulses leads at least to a better corrosion protection because of a sealing effect where cathodic pulses follow anodic ones. Up to now, only a few studies have been conducted on titanium or Ti alloy anodized with high-frequency plasma electrolytic oxidation (37, 44, 49-50-51-52-53).
Thermal oxidation
Another method to grow titanium oxides is to thermally treat titanium in an oxygen-containing atmosphere. The passive layer formed on titanium with exposure to air is some nanometers thick and composed of amorphous or poorly crystallized nonstoichiometric TiO2. This layer is highly stable and provides protection against aggressive environments but can be disrupted at very low shear stresses, even by rubbing against soft tissue (54). The structure of thermally grown titanium oxides can be either anatase or rutile, depending on treatment temperatures (55).
Such oxides show higher chemical resistance than those grown anodically, as well as those produced through chemical oxidation: In fact, the latter can be removed by an acid pickle, while the removal of thermally grown oxides often requires sandblasting or a caustic descaling bath (55).
With thermal oxidation, surface morphology changes from a thin adherent surface layer at 500°C to the formation of a small grain structure at 650°C, until there is a complete coverage with grains oriented perpendicular to the substrate, at 800°C. Corrosion resistance increases with increasing treatment temperature, with lower anodic current densities at higher temperature (
Potentiodynamic polarization curves of untreated and thermally treated Ti samples with temperatures between 500°C and 800°C (53).
Concerning treatment time, Kumar et al (57) performed thermal treatment at 650°C with a duration of from 8 to 48 hours. Their results showed the presence of oxide scales throughout the surface without any spalling, irrespective of treatment time. At 800°C longer treatment caused oxide spallation. X-ray diffraction (XRD) on oxidized samples with different durations reveals the formation of rutile, TiO and α-Ti phase, as reported in
X-ray diffraction (XRD) patterns of untreated and thermally treated Ti samples with different treatment durations (57). R = rutile phase.
The advantages of thermal oxidation compared with anodic oxidation are well reported in the literature (55, 58).
Birch and Burleigh report the effect of anodization at low voltages (up to a few volts), and of thermal treatment at different temperatures with different durations, on free corrosion potential (55). They performed potentiodynamic tests and electrochemical impedance spectroscopy (EIS) tests, measuring anodic current densities in the passive range and free corrosion potentials of all samples prepared with those treatments.
Higher-temperature oxides show progressively lower passive current density and higher corrosion potential, which implies that the films are more protective and inert. The oxide formed at 700°C for 30 minutes shows the highest free corrosion potential and the lowest current density. Both anodization and thermal oxidation provide better corrosion resistance compared with nontreated metal. The difference in corrosion behaviors of the tested oxidizing techniques is due to the crystal structure of the oxide: In
Titanium oxide structures with different surface treatments.
Chemical oxidation
Thermal oxidation is simple, but its reproducibility is poor and should be preceded by acid pickling to remove embedded surface contamination, such as iron. In addition, the temperature has to be higher than 500°C to build a film with good corrosion resistance. It is not practical to heat a large vessel at 500°C. Anodic oxidation, instead, is more consistent and can be effective as a single step if it is applied for a sufficient time to dissolve surface contamination. However, sometimes anodizing at high voltage is time consuming and laborious with potential safety problems, and applying current to a large vessel is not practical. In these cases, another technique can be used – that is, chemical oxidation (8).
Heating up titanium in a H2O2 or NaOH environment at temperatures of 60°C-90°C results in oxidation of the surface with no external contamination. Acids like H2SO4 and HCl can be added to the treatment solution to remove surface contaminants (59).
Oxide thickness increases almost linearly with treatment duration. Oxide growth with this technique is comparable to that produced with anodization or thermal oxidation.
Films obtained in solutions containing HCl are thicker. XRD analyses of the same samples show that the addition of SO4- ions promotes the formation of pure anatase, while the addition of Cl- ions favors the formation of pure rutile phase.
An evolution of this oxide growing method has involved annealing a chemically oxidized surface. Wang et al (60) studied the effect of thermally treating the sample at 350°C, 400°C, 500°C and 600°C after chemical oxidation at 80°C for 6 hours in H2O2. They found large differences in surface wettability: with average water contact angles of 29.5°, 130.5°, 115.6° and 30.6°, respectively. This effect influences corrosion resistance, as can be seen from the potentiodynamic tests reported in
Potentiodynamic test results for thermally treated chemically oxidized titanium, carried out in sea water solution (60).
Scanning electron microscopy (SEM) images of TiO2 film prepared at different temperatures, 350°C (
A different trend is reported by Krupa et al (61) for chemical oxidation carried out in a 10 M NaOH solution at 60°C for 24 hours and then heated at 500°C, 600°C and 700°C. In this case, the last sample, calcined at 700°C, showed the best corrosion resistance according to the polarization resistance of the oxide and the potentiodynamic behavior. Corrosion resistance follows the order: 700°C > 500° > 600° > untreated. The explanation proposed is related to the sodium titanate hydrogel present in the oxide. At 500°C, the sodium titanate hydrogel surface layer is dehydrated and transformed into amorphous sodium titanate. At 600°C, the hydrogel layer is partially transformed into crystalline sodium titanate and rutile, but remains amorphous. From 600°C, a densification process begins, resulting in the pores being closed. The transformation of the amorphous structure into crystalline is observed to occur above 700°C. The higher corrosion resistance achieved at 500°C compared with that measured on samples heated at 600°C may result from the better structural homogeneity of the former samples. The structure of samples heated at 600°C is partially amorphous and partially crystalline, and this morphology negatively affects corrosion resistance (61).
Ion implantation
The ion implantation technique has been exploited to enrich the surface of titanium with certain amounts of selected elements; this permits the production of surfaces that are more biocompatible (62). Thus, the majority of the studies reported in the literature available regarding this technique refer to attempts to enhance biocompatibility. Another requirement for devices in the human body is the resistance to corrosion, and ion implanted samples are usually tested for this purpose in simulated body fluid (SBF).
According to EIS analyses, implantation of calcium at a dose of 1017 Ca+/cm2 with ion energy 25 keV produces an increment in uniform corrosion resistance of titanium in an SBF environment. However, the formation of pits is reported in corrosion tests after this treatment. The mechanism of the initiation of the pits on the surface of implanted titanium has not yet been explained, though it is suggested that the alteration of chemical composition of the oxide layer results in a weakening of the oxide toward localized corrosion (63).
The same test performed on samples implanted with 1015-3 × 1017 P+/cm2 shows that for doses higher than 106, a new TiP phase appears in the oxide (64). Phosphorous implantation causes an increase in corrosion resistance performance – a conclusion derived from both potentiodynamic and EIS analyses – and the resistance to polarization of the implanted layer is 2.5 times larger than that of the untreated oxide, which is due to the amorphous structure of the TiO2 surface during the implantation. Phosphorous is known to stabilize amorphous structures (28, 65). The authors claim that the amorphous layer made up of the native titanium oxide does not contain defects, such as grain boundaries and contaminant segregation, which are characteristic of the crystalline state; this fact can be considered the reason for the increased corrosion resistance of amorphous oxides compared with crystalline oxide with the same thickness. The formation of the TiP phase, which itself has a high corrosion resistance, probably helps the increase in resistance (64).
The effect of both calcium and phosphorous ion implantation is to avoid the pitting corrosion observed in the case of implantation of Ca alone (66). The corrosion resistance of the treatments can be classified as follows: Ca + P implanted titanium > P implanted titanium > Ca implanted titanium > untreated titanium (67).
Oxygen implantation in concentrations from 1013 to 1015 ions/cm2 has been exploited by Ningshen et al (68). Unfortunately, this treatment was found to be detrimental for titanium corrosion resistance in highly aggressive environments.
Carbon implantation was found to have a much greater effect on titanium corrosion resistance.
Free corrosion potential and polarization resistance on titanium samples implanted with different amounts of C
C implanted dose | Ecorr (mV) | Rp (MΩ cm2) |
---|---|---|
Ecorr = free corrosion potential; Rp = polarization resistance. | ||
Not implanted | -95 | 2.5 |
5 × 1015 ions/cm2 | 34 | 6 |
1 × 1016 ions/cm2 | 65 | 12 |
1 × 1017 ions/cm2 | 220 | 50 |
2 × 1017 ions/cm2 | 330 | 54 |
A similar study was conducted on nitrogen implantation, with doses from 1016 to 1018 ions/cm2.
Free corrosion potential and polarization resistance on titanium samples implanted with different amounts of N
N implanted dose | Ecorr (mV) | Rp (MΩ cm2) |
---|---|---|
Ecorr = free corrosion potential; Rp = polarization resistance. | ||
Nonimplanted | -95 | 2.5 |
1 × 1016 ions/cm2 | 85 | 6.6 |
1 × 1017 ions/cm2 | 233 | 62.9 |
6 × 1017 ions/cm2 | 230 | 40.3 |
1 × 1018 ions/cm2 | 160 | 4.8 |
Grain refinement
In recent years, a variety of techniques to obtain ultrafine grain (UFG) size on metals were developed (71). A comparison between corrosion resistance of UFG titanium with that of coarse grain titanium was proposed from Balyanov et al (72). UFGs were obtained using the equal channel angular pressing (ECAP) technique, reaching an average grain size of 300 nm.
Free corrosion potential (OCP, V SCE) and mass loss rate (g/m2h) for coarse grain (CG) and ultrafine grain (UFG) titanium, measured in HCl and H2SO4 acids
Solution | ||||||
---|---|---|---|---|---|---|
1 M HCl | 3 M HCl | 5 M HCl | 1 M H2SO4 | 3 M H2SO4 | 5 M H2SO4 | |
Corr. = corrosion; OCP = open circuit potential; SCE = saturated calomel electrode. | ||||||
CG Ti OCP, V | 0.193 | -0.252 | -0.362 | 0.237 | -0.235 | -0.352 |
UFG Ti OCP, V | 0.210 | -0.242 | -0.358 | 0.256 | -0.223 | -0.345 |
OCP difference, % | 8.8 | 4.7 | 1.1 | 8.0 | 5.1 | 2.0 |
CG Ti corr. rate (g/m2h) | 0.62 | 1.37 | 1.98 | 0.76 | 1.46 | 1.87 |
UFG Ti corr. rate (g/m2h) | 0.42 | 0.90 | 1.38 | 0.58 | 0.78 | 1.09 |
Corr. rate difference, % | 32 | 34 | 30 | 24 | 47 | 43 |
Kim et al (73) carried out a similar study on UFG titanium produced using 3 different methods. The first 2 methods involved rolling with a single pass at different speed ratios of 3 and 5, and producing a thickness reduction of 61% and 77% (W3 and W5), respectively. The third method involved cold rolling to produce a thickness reduction of 63% by a single rolling pass (C3).
Corrosion current density and corrosion potential measured on untreated titanium and that treated with procedures W3, W5 and C3
Corrosion current density (μA/cm2) | Corrosion potential (V SCE) | |||
---|---|---|---|---|
1 M HCl | 1 M H2SO4 | 1 M HCl | 1 M H2SO4 | |
C3 = cold rolling to produce a thickness reduction of 63% by a single rolling pass; SCE = saturated calomel electrode; W3 = rolling with a single pass at speed ratio of 3, producing a thickness reduction of 61%; W5 = rolling with a single pass at speed ratio of 5, producing a thickness reduction of 77%. | ||||
Untreated | 186 | 257 | -0.635 | -0.677 |
W3 | 165 | 235 | -0.623 | -0.653 |
W5 | 148 | 206 | -0.612 | -0.639 |
C3 | 124 | 178 | -0.597 | -0.621 |
The treatment C3 produced the best result, with the corrosion rate decreasing by 40.6% and 48.2% in HCl and H2SO4 solutions, respectively. The corrosion rate decreased linearly with the inverse square root of grain size. This effect was due to the higher energy of the grain boundaries. Corrosion tends to take place in grain-boundary regions, and a large extent of grain boundaries in nanocrystalline materials enhances passivation kinetics, leading to rapid formation of a stable passive layer.
Alloying with palladium
Among the variety of titanium alloys, 3 of them were developed to enhance titanium corrosion resistance: titanium grade 7, grade 12 and grade 16. The best alloying elements to enhance corrosion resistance are palladium, molybdenum and nickel (12, 74). Palladium and nickel have the effect of accelerating cathodic hydrogen evolution reactions (HERs) on titanium, due to their higher exchange current density for HER, while molybdenum is used to enhance the stability of the oxide.
Among the 3 elements, palladium is the one that gives higher corrosion resistance to titanium to the point that Ti-Pd alloy has been proposed for the manufacture of high-level nuclear waste containers (75). Nakagawa et al (76) showed that alloying with palladium altered the cathodic process and resulted in lower overvoltages for HER: This may shift the working potential in the passive region of the alloy. They also found that palladium adsorbs hydrogen to form a protective layer of titanium hydride.
Brossia and Cragnolino (77) report a comparison between Ti grade 2 and 7 pitting resistance, in a 1 M solution of Cl- at 95°C. Pitting potential increases from 1.08 V vs. saturated calomel reference electrode (SCE) to 7.69 V vs. SCE, in passing from Ti grade 2 to Ti grade 7 (with 0.2% of palladium). They also pointed out the effect of palladium alloying on the cathodic polarization curve, as visible in
Cathodic polarization curves for Ti grades 2 and 7 in deaerated 5 M chloride + 0.1 M HCl at 95°C (77). SCE = saturated calomel electrode.
Conclusions
The excellent corrosion resistance of titanium in many aggressive environments can be further enhanced by tuning its surface properties and/or bulk composition. In the second part of this review concerning the corrosion of titanium, some of the most important treatments to increase corrosion resistance are described, in relation to the forms of corrosion described in Part 1. The effects of the variation of treatment parameters have been described, with particular attention to those techniques that enable the modification of natural titanium oxide in terms of thickness and morphology.
However, knowledge of even these kinds of treatment is far from being exhaustive, and further research will likely be conducted into this important topic.
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Authors
- Prando, Davide [PubMed] [Google Scholar] 1, 2
- Brenna, Andrea [PubMed] [Google Scholar] 1, 2
- Diamanti, Maria Vittoria [PubMed] [Google Scholar] 1, 2
- Beretta, Silvia [PubMed] [Google Scholar] 1, 2
- Bolzoni, Fabio [PubMed] [Google Scholar] 1, 2
- Ormellese, Marco [PubMed] [Google Scholar] 1, 2
- Pedeferri, MariaPia [PubMed] [Google Scholar] 1, 2, * Corresponding Author ([email protected])
Affiliations
-
Department of Chemistry, Materials and Chemical Engineering “G. Natta”, Politecnico di Milano, Milan - Italy -
National Interuniversity Consortium of Materials Science and Technology, Florence - Italy
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