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Research Letters in Physical Chemistry
Volume 2009 (2009), Article ID 574359, 4 pages
http://dx.doi.org/10.1155/2009/574359
Research Letter

Electrochemical Behavior of Titanium and Its Alloys as Dental Implants in Normal Saline

Department of Metallurgical and Materials Engineering, Colorado School of Mines, Golden, CO 80401, USA

Received 21 January 2009; Accepted 19 February 2009

Academic Editor: Claudio Fontanesi

Copyright © 2009 Rahul Bhola et al. This is an open access article distributed under the Creative Commons Attribution License, which permits unrestricted use, distribution, and reproduction in any medium, provided the original work is properly cited.

Abstract

The electrochemical behavior of pure titanium and titanium alloys in a simulated body fluid (normal saline solution) has been tested, and the results have been reported. The significance of the results for dental use has been discussed. The tests also serve as a screening test for the best alloy system for more comprehensive long-term investigations.

1. Introduction

Commercially pure titanium and titanium alloys are known for their use in dental practice owing to their good corrosion resistance, biocompatibility, and biofunctionality in the human body [1].

Titanium is a thermodynamically reactive metal as suggested by its relatively negative reversible potential in the electrochemical series [2]. It gets readily oxidized during exposure to air and electrolytes to form oxides, hydrated complexes, and aqueous cationic species. The oxides and hydrated complexes act as barrier layers between the titanium surface and the surrounding environment and suppress the subsequent oxidation of titanium across the metal/barrier layer/solution interface. Even if the barrier layer gets disrupted, it can get reformed very easily, leading to spontaneous repassivation. A review of literature reveals that extensive work has been done on the use of titanium alloys as prostheses when the alloy comes in contact with saliva [35]. Whereas when titanium alloys are used as implants, the alloy remains in contact with saliva only during the transition period of healing of the bony socket and gingiva (gum) but when it is capped with the crown, it is in contact with only bone cells for the rest of its life. The aim of this study is to keep in focus the use of titanium alloy as an implant inside the bone tissue and hence normal saline solution was used to simulate the extracellular interstitial environment. The decrease in pH can occur inside the bone tissue owing to surgical trauma, infection [6, 7] as well as the healing process of the bony socket. Ti3+ ions, if produced, can hydrolyze to further acidify the area [8]. Acidification can also be observed if crevice corrosion occurs in the clefts between the implant and the crown [5]. According to Black [9], the potential of a metallic biomaterial can range from 1 to 1.2 V versus SCE in the human body. It is, thus, significant to study the electrochemical behavior of titanium in this potential range.

Electrochemical corrosion behavior of commercially pure titanium (grades Ti1 & Ti2) and its alloys, Ti64, TiOs, Ti15Mo, and TMZF in normal saline solution was analyzed at the body temperature of 37C.

2. Experimental

2.1. Materials Preparation

Titanium alloy grades Ti1, Ti2, Ti64, TiOs, Ti15Mo, and TMZF of compositions Ti1 (0.1%C, 0.2%Fe, 0.015%H, 0.03%N, 0.18%O, and 99.47% Ti), Ti2 (0.1%C, 0.3%Fe, 0.015%H, 0.03%N, 0.25%O, and 99.30%Ti), Ti64 (0.1%C, 0.2%Fe, 0.015%H, 0.03%N, 0.2%O, 6%Al, 4%V, and 89.45%Ti), TiOs (0.05%C, 0.05%Fe, 0.015%H, 0.02%N, 0.15%O, 35.5% Nb, 5.7%Ta, 7.3%Zr, and 51.21%Ti), Ti15Mo (0.05%C, 0.1%Fe, 0.015%H, 0.01%N, 0.15%O, 15%Mo, and 84.67%Ti), and TMZF (0.02%C, 2%Fe, 0.02%H, 0.01%N, 0.18%O, 6%Zr, 12%Mo, and 79.77%Ti) were used for the present investigation. Available cuboidal and cylindrical rods were cut to expose cross-section areas of 0.855cm2 for Ti1, 1.0cm2 for Ti2, 1.5525cm2 for Ti64, 1.3270cm2 for TiOs, 0.4869cm2 for Ti15Mo, and 2.7606cm2 for TMZF as working electrodes. Normal saline solution (5.26gL1 sodium chloride, 2.22gL1 anhy. sodium acetate, 5.02gL1 sodium gluconate, 0.37gL1 potassium chloride, and 0.3gL1 magnesium chloride hexahydrate) having pH 6.6 was used to carry out the electrochemical testing of alloys.

2.2. Measurements

A Princeton Applied Research Potentiostat 273A was used for the electrochemical measurements. A three-electrode cell assembly consisting of titanium alloy as the working electrode, platinum wire as the counter electrode, and a saturated calomel electrode as the reference electrode was used. 450 mL of normal saline solution was used for the immersion and electrochemical testing of the alloys.

Open Circuit Potential (OCP)
Open circuit potential values of the alloys were measured just after immersion, followed by a duration of 2, 6, and 24 hours up to seven days.

Tafel
After the end of the seven days, Tafel curves of various alloys were obtained by polarizing each electrode from 250mV versus OCP to 2 V with an ASTM scan rate of 1 mV/s [10].

Cyclic Polarization
Cyclic polarization measurements were extended after Tafel measurements by choosing a vertex potential of 2 V, at which the scan was reversed, and the final potential was 250mV versus OCP.

3. Results and Discussion

It can be seen from Figure 1 and Table 1 that the OCP values for all alloys have shown an overall increase for the time duration of seven days, despite showing a small decrease in a few intervals.

tab1
Table 1: Open circuit potential values of alloys with change in time at 37C.
574359.fig.001
Figure 1: Open circuit potential values of alloys as a function of time at 37C.

The OCP shift in the noble direction for the alloys suggests the formation of a passive film that acts as a barrier for metal dissolution and reduces the corrosion rate. The shift can also suggest that the composition of corrosive medium might be changing in the implant cavity but since large volume of solution is used in testing, that can be neglected. The potential increase shows that the alloys become thermodynamically more stable with time. According to Blackwood et al. [11], the shift in OCP to positive values lowers the corrosion rate by reducing the driving force of the cathodic reaction and increasing the thickness of the passive oxide film. The initial decrease observed in the OCP values for Ti1, TiOs, and TMZF suggests the initial dissolution of the air-formed oxide film till the formation of a new oxide in solution [12].

The pH values of all alloys in normal saline solution of pH 6.6 were less than 8 till seven days of immersion. Figure 2 shows the pH-potential Pourbaix diagram for titanium-water system at 37C [13], with potential also shown with respect to SCE on another 𝑦-axis. The corresponding region of pH (6.6–8) and potential to which the present system is studied is similar to that of TiO2 in the Pourbaix diagram indicating the fact that under steady-state conditions, the alloys form a stable oxide layer of TiO2.

574359.fig.002
Figure 2: Pourbaix diagram for titanium at 37C.

Figure 3 shows the potentiodynamic curves for the alloys at 37C. The corresponding corrosion parameters are given in Table 2, and passivation parameters are given in Table 3.

tab2
Table 2: Corrosion parameters for the forward and reverse scans for the alloys at 37C after seven days.
tab3
Table 3: Passivation parameters for the alloys at 37C after seven days.
574359.fig.003
Figure 3: Potentiodynamic curves for the alloys at 37C.

The corrosion rate was calculated using the expression [14] Corrosionratemm=year0.00327×E.W.×𝐼corr𝜌,(1) where E.W.  =  equivalent weight, 𝐼corr  =  current density in 𝜇A/cm2, and 𝜌  =  density in g/cm3.

The corrosion rates observed are in the order Ti15Mo > Ti2 > TMZF > Ti1 > Ti64 > TiOs. The corrosion rates observed are very low and belong to the outstanding corrosion resistance category of less than 0.02 mm/year as classified by Fontana [15]. Studies have further revealed that to prevent tissue damage and irritation, the corrosion rate of a metallic implant should be less than 2.5×104mm/year [16]. The difference between the passivation potential and 𝐸corr can provide an indication of the ease of passivation of the alloys. The lower the difference is, the easier the passivation will be. The difference follows the order TMZF > Ti15Mo > Ti1 > Ti2 > TiOs > Ti64.

Cyclic polarization method is a highly useful method for determining the susceptibility of a metal or alloy to pitting [17]. From Figures 4(a)4(f), it can be seen that at the vertex potential of 2 V when the scan reverses its direction, the reverse scan starts left of the forward scan curve, that is, towards the low current density region. This type of the cyclic polarization curve is known to resist localized corrosion [18]. It is also observed that the reverse scan curves meet the forward scan curve along the passive range. The reverse scan curves show lower current densities as can be seen in Table 2 except for Ti1 and Ti2. The potentials for the reverse scan curves are more positive than those for the forward scan. These results show that a stable oxide film is formed during the forward scan.

fig4
Figure 4: Cyclic polarization curves for alloys (a)–(f) at 37C.

4. Conclusions

(1)In normal saline solution, all alloys exhibit a high corrosion resistance, and the corrosion rates observed fall in the acceptable range for biocompatibility of metallic implants.(2)All alloys show considerable ennoblement and form a stable oxide film of TiO2 as indicated by their corresponding pH and potential position in the Pourbaix diagram.(3)From the cyclic polarization curves obtained, it can be concluded that the alloys resist localized corrosion.

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