Open access peer-reviewed chapter

Factor Affecting Geometry of TiO2 Nanotube Arrays (TNAs) in Aqueous and Organic Electrolyte

Written By

Khairul Arifah Saharudin, Srimala Sreekantan, Rabiatul Basria S. N. M. Mydin, Norfatehah Basiron and Warapong Krengvirat

Submitted: December 1st, 2017 Reviewed: January 18th, 2018 Published: February 13th, 2018

DOI: 10.5772/intechopen.74193

Chapter metrics overview

1,042 Chapter Downloads

View Full Metrics


TiO2 nanotube arrays (TNA) have attracted scientific interest due to the combination of functional material properties with controllable nanostructure. Superior properties of TNA, including vectorial pathway of e− transport, minimized e− recombination, and high specific surface area render them as the most promising candidate for environment remediation, energy conversion and biocompatibility applications. The superior properties and efficacy of the TNA in various applications influenced by structural characteristics such as pore size, length and wall thickness. Therefore in this chapter the effect of various electrochemical parameters such as applied voltage, anodization time, electrolyte composition on the formation of controlled dimension of TNA in aqueous and organic electrolytes are reviewed.


  • TiO2 nanotube arrays (TNA)
  • anodization
  • electrochemical parameters
  • aqueous electrolyte
  • organic electrolytes

1. Introduction

Within the last decade, nanoscale and nanostructured metal oxide materials have strongly influenced numerous fields in science and technology. Among the various nanostructured oxide materials, TiO2 nanotube arrays (TNA) have received special attention due to its enhanced properties, cost-effective fabrication and higher surface-to-volume ratio [1]. TNA offers unique properties and a high functionality for various applications such as photocatalysis [2, 3], solar cell [4, 5, 6], biomedical [7, 8], and sensors [9, 10]. Their performance in various applications significantly determined by geometry, shape, and morphology of nanostructures [11]. In this concern, a defined arrangement and a vertical and homogeneous alignment over the entire substrate surface, based on the self-organized anodic oxidation is pursued. Electrochemical anodization is widely used because of its controllable, reproducible results and simplicity of the process. The feasibility to tune the size and shape of nanotubular arrays to the desired dimensions and meeting the demands of specific applications by means of controlled anodic oxidation of the metal substrate have widen the application of TNA. Furthermore, it is a cost-effective method and the tubes prepared via this method have good adherent strength.


2. Factor affecting geometry and composition of TNA

The anodic growth of self-organized tubular structure is well known as the equilibrium reaction between electrochemical oxidation at the metal/electrolyte interface and chemical dissolution at the oxide/electrolyte interface [12, 13]. The structural characteristics of the nanotube arrays can be controlled through various synthesis parameters, including applied potential [14, 15, 16], anodization time [14, 17, 18], electrolyte type and chemical composition [12, 13, 19]. Therefore, this section provides a comprehensive review on the influence of aforementioned parameters on the formation of TNA.

2.1. TNA synthesis using aqueous electrolytes

Gong and co-workers [20] first obtained self-organized, highly-uniform TNA by anodizing Ti in aqueous electrolyte containing 0.5 wt% HF under applied potential of 10–20 V. The pore size increased with increasing applied potential while the nanotube length was dependent on the anodization time. Titanium undergoes electrochemical oxidation process as follow: Ti+2H2OTiO2+4H+(Reaction 1) and chemical dissolution process: TiO2+6HFTiF62+2H2O+2H+(Reaction 2) to form nantubular structure. However, the length of nanotubes was limited to a maximum of ~500 nm, due to the restriction imposed by high chemical dissolution of formed oxide by strong acidity of HF aqueous electrolyte, c.a., pH < 2 [14, 21]. The chemical dissolution of the formed oxide is determined by the F concentration and the pH value of the solution (Reaction 2). The model proposed by Macak and co-workers suggest that F and H+ are attracted toward the pore bottom during anodization (Figure 1a), followed by establishment of pH profile as in (Figure 1b). The variation in pH profile triggers different degree of dissolution rate along the tube inner surface (Figure 1c).

Figure 1.

(a) Schematic diagram to illustrate the presence of NH4+ and F that creates a local acidification, (b) pH profile within the nanotube, (c) rate of dissolution of the tube.

This work directly leads to the use of buffer solution as electrolyte to control pH and increase the length of nanotube produced. Reaction 2 permits the dissolution reaction and become the core foundation of field-assisted dissolution model. Since then, many authors have adapted the dissolution process into their research framework such that field-assisted dissolution model is gradually established for TNA anodization [22, 23, 24].

Large number of F and H+ ions in HF aqueous electrolyte dominates high chemical dissolution and thus hinders the equilibrium growth of the nanotube arrays [12]. Beranek et al. [25] found that the incorporation of low concentration of HF aqueous electrolyte with acetic acid (H2SO4) addition could reduce the chemical dissolution, and thus allows the formation of porous TiO2 with improved structural morphologies. This basis was later used to obtain TNA with well-defined tubular structure over applied potential range of 10–25 V [14]. The nanotube length and pore diameter increased linearly with increasing applied potential. In summary, the structural morphologies of anodic growth oxides can be controlled by the acidity of electrolyte [26].

Macak et al. [12] investigated the influence of the electrolyte acidity on the growth of nanotube arrays using HF, potassium fluoride (KF) and sodium fluoride (NaF) as F sources. TNA with ~280 nm long and ~40 nm pore diameter were formed in strong acidity (pH < 1) HF aqueous electrolyte after 2 h of anodization at 10 V. The increase in the pH value of electrolyte to 1.3 and 2.8 by using KF and NaF instead of HF resulted in the formation of TNA with the nanotube length of ~320 and 590 nm, respectively. TNA with a maximum length of 1.5 μm were achieved at 25 V. Moreover, the nanotube length is proportional to the anodization time, and thus resulted in the formation of nanotube arrays with length of ~800 nm, ~1.8 μm and ~2.3 μm after exposure for 20, 60 and 90 h in electrolyte with pH of 3.8. It is interesting to note that the acidity of electrolyte plays an essential role for the growth of long nanotube arrays instead of the anodization time. The increase of pH value from 3.8 to 4.5 resulted in significant increase in the nanotube length from ~800 nm to ~4.4 μm after anodization at 10 V for 20 h.

The significance of the pH value of an electrolyte on the growth of TNA was proven by Bauer et al. [27]. Self-organized TNA was successfully formed in 1 M H3PO4 containing 0.3 wt% HF over applied potential range from 1 V to 25 V. Weak acidity of H3PO4 governs the local acidification during pore growth, and thus allowed the control of nanotube geometry over wide range of applied potential [12]. In 2007, Allam and Grimes [28] demonstrated an alternative method to fabricate TNA using hydrochloride (HCl) instead of fluoride-containing electrolyte. The anodization in 3 M HCl aqueous electrolyte at 20 V for 20 min allowed the formation of TNA with the nanotube length of ~600 nm. However, high chemical dissolution of aqueous electrolytes still remains as significant restriction in achieving long nanotubes with smooth walls. This limitation of forming long TNA in aqueous electrolyte has extended the use organic electrolyte to reduce the chemical dissolution process.

2.2. TNA synthesis using organic electrolytes

An organic electrolyte is known as efficient solvent in anodic fabrication of highly-ordered self-organized porous alumina (Al2O3) at high applied potential, c.a., 100 V [29, 30]. The incorporation of organic component from the electrolyte into anodic oxide film is known to lower the relative permittivity of oxide and increase its dielectric breakdown potential [18], thereby allowing the anodic growth of oxide film under wide range of applied potential [13, 31].

2.2.1. Dimethyl sulfoxide (DMSO)

Ruan et al. [19] demonstrated the anodic growth of TNA in fluorinated dimethyl sulfoxide (DMSO) and ethanol (EtOH) mixture. Well-aligned TNA with 2.3 μm in length were formed by anodization in 1:1 DMSO and EtOH mixture containing 4 wt% HF at 20 V for 70 h. DMSO is a dipolar aprotic solvent. Unlike protic solvents, aprotic solvents do not have a hydrogen atom directly bonded to an electronegative atom, such as oxygen or nitrogen. DMSO has a very weak ability to donate protons (hydrogen bond donation) and it is more basic than water, implying that DMSO has a protophilic nature [21]. DMSO accepts the hydrogen proton from HF and thus allows the formation of long nanotubes by the reduction of the chemical dissolution. However, the donation of oxygen in organic electrolyte is more difficult than aqueous electrolyte, and thus limited the nanotube length even after long anodization time. Discrete nanotube arrays obtained in 1:1 DMSO and EtOH mixture exhibited fourfold higher photocurrent density as compared to that formed in aqueous electrolyte [20]. This reveals the potential of organic electrolyte for the formation of long TNA for superior photoelectrochemical properties. The nanotube length was later increased up to 93 μm by anodization in DMSO containing 2 wt% HF at 60 V for 70 h refer to Figure 2a-d [13, 15].

Figure 2.

(a) Cross-sectional, (b) magnified-cross sectional, (c) surface and (d) pore bottom morphologies of TNA grown in DMSO containing 2 wt% HF at 60 V for 70 h [19].

To enhance the oxidation rate in organic electrolyte, water usually serves as a source of O2− and hydroxyl ion; OH [13, 15]. Several authors reported that small amount of water addition could improve the adhesion between the nanotube and underlying oxide barrier layer. This facilitates the growth of long nanotubes [32, 33]. Large amount of water addition however decreased the viscosity of electrolyte [3, 34], leading to high chemical dissolution by the higher diffusion rate of reactant ions [35]. The minimum amount of water less than 5 wt% limits the chemical dissolution and thus allows the nanotube to grow deeply into the metal without significant loss at the pore mouth. Besides, thinner barrier layer in such condition allows greater ionic conduction and faster movement of the metal/oxide interface into the metal, thus producing long TNA [13, 32].

The significance of anodization parameters, including applied potential, F concentration, water content and anodization time on the structural characteristics of TNA were extensively investigated by Yoriya et al. [33] and the finding are presented in Figure 3a-e. Higher applied potentials provide a greater driving force for both electronic and ionic conduction and thus allow the growth of long nanotube arrays. A maximum length of TNA of 101 μm was achieved by anodic growth in DMSO containing 2 wt% HF at 60 V for 70 h.

Figure 3.

Variation of TiO2 nanotube array length as a function of (a) applied voltage for a 70 h anodization using DMSO containing 2% HF with and without a pre-anodization step to template the surface, (b) HF concentration in DMSO for 40 and 60 V 70 h anodization, (c) variation of nanotube length obtained from a 2.0% HF-DMSO containing different deionized water concentrations (40 V, 40 h), and (d) duration for a 40 V anodization in 2.0% HF-DMSO electrolytes with 0, 3, and 5% deionized water content [33].

Figure 3b reveals that 2 wt% HF concentration allowed the formation of longest nanotube at both 40 and 60 V. HF concentration higher than 2% greatly increases the chemical dissolution, and thus reduces nanotube length. Furthermore, chemical dissolution is relatively lower than electrochemical oxidation in DMSO electrolyte containing less than 2 wt% HF, resulting in the formation of short nanotubes. The addition of H2O facilitates the extraction of O2– and OH from electrolyte to form oxide, contributing to the formation of long nanotube with thick walls. However, high H2O amount (> 2 wt%) dominates chemical dissolution and thus reduces the nanotube length (Figure 3c). Figure 3d shows that nanotube length increased up to 70 h and then decreased continuously. The shorter nanotube length after 70 h is caused by slow diffusion of F, due to the accumulation of reaction products at the tube bottom, as well as significant loss at atop of nanotube by high chemical dissolution [5, 13].

2.2.2. Amide – Formamide (FA) and N-methylformamide (NMF)

Formamide (FA) and N-methylformamide (NMF) have been used as electrolyte for fabricating long nanotubes with high growth rate [15]. FA and NMF are both protophilic like DMSO, meaning that their acidity nature is weaker than water [21]. The dielectric constant of FA and NMF are 111 and 182.4, respectively, which are much higher than water; ~78.39. Higher dielectric constant of electrolyte induces more charges on the oxide layer and thus improves the extraction of Ti4+ ions, and facilitates the dissolution of HF for it to be chemically available at the oxide/electrolyte interface [13]. Paulose et al. [15] fabricated TNA of ~69 μm long in FA electrolyte containing 0.27 M NH4F at 35 V for 48 h. It is noticeable that the growth rate increased to ~24.3 nm min−1, which is relatively higher than that formed in DMSO [19] or aqueous electrolyte [36]. Shankar et al. [13] further investigated the influence of applied potential at 20–30 V, and NH4F concentration in the range of 0.11– 0.37 M. The nanotube length and pore size increase with increasing applied potential and concentration of NH4F, achieving a maximum length of ~78 μm in FA containing 0.37 M NH4F. Besides, the incorporation of high polarity electrolyte, NMF into FA also accelerates the chemical dissolution and thus results in nanotubes with larger pore size.

2.2.3. Glycerol

The diffusion of ionic species in electrolyte greatly affects the growth of TNA by local acidification at the pore bottom [12]. Macak and colleagues [34] investigated the influence of electrolyte viscosity on the formation of TNA by anodization in various types of electrolyte; 1 M ammonium sulfate [(NH4)2SO4] containing 0.5 wt% NH4F, 1:1 glycerol and H2O mixture containing 0.5 wt% NH4F, and glycerol containing 0.5 wt% NH4F. The viscosities of these electrolytes were ~0.001, ~0.004 and ~1.5 Pa.s, respectively. The anodization in (NH4)2SO4 electrolyte allowed the formation of TNA with length of ~2 μm while the anodization in glycerol electrolyte resulted in nanotube arrays with ~1.3 μm in length. However, the incorporation of large amount of water leads to the presence of ripples at the nanotube walls, resulting from high chemical dissolution in electrolyte. The nanotube length formed in glycerol-based electrolyte increases almost linearly with increasing anodization time, and achieved ~6.1 μm after anodization at 20 V for 18 h.

The viscosity of electrolyte can be also affected by anodization temperature [34, 37]. The viscosity of glycerol containing 0.5 wt% NH4F decreases from 12 Pa.s to 1.5 and 0.3 Pa.s by increasing temperature from 0°C to 20 and 40°C, respectively. Low viscosity facilitates the diffusion of reactants at the pore tip, resulting in long nanotube with large pore. As mentioned earlier, the incorporation of organic species from organic electrolyte into the oxide film during anodization allows the growth of nanotube arrays under a wide range of applied potential. Alivov et al. [31] investigated the formation behavior of TNA in a broad range of applied potential of 5–350 V and F concentration of 0.1–0.7 wt%. TNA were formed in glycerol under applied potential of 10–240 V, and the applied potential is disproportional to F concentration.

2.2.4. Ethylene glycol (EG)

The anodization in high viscosity (μv) electrolyte of about 945 cP at 25°C resulted in relatively shorter nanotube length as compared to that formed in aqueous electrolyte. Hence, the potential of low viscosity polyol solvent, such as ethylene glycol (EG, μv = 16 cP at 25°C) for the formation of TNA was investigated by [34]. TNA with ~1.6 μm in length were obtained by anodization in EG containing 0.5 wt% NH4F at 12 V for 3 h. The significant increase in the nanotube length in EG-based electrolyte could be attributed to lower diffusion resistance in electrolyte with lower viscosity [21]. The potential of EG as efficient electrolyte was later confirmed by [32]. The anodization in EG containing 0.25 wt% NH4F at 60 V allowed the rapid formation of nanotube arrays with the growth rate up to 131.4 nm min−1. The resulting nanotube arrays exhibited length of 134 μm and pore size of 25 nm after 17 h of anodization. The nanotube length was further increased to 220 μm by anodization in EG containing 0.3 wt% NH4F and 2 wt% H2O [13], implying the significant role of H2O addition on the growth of long nanotube arrays.

The influences of anodization parameters, including H2O content, NH4F concentration, applied potential and anodization time on the growth of TNA in EG-based electrolytes were systematically investigated by Prakasam et al. [35]. The increase in the H2O content and NH4F concentration stimulate electrochemical oxidation at the metal/oxide interface and chemical dissolution at the oxide/electrolyte interface, resulting in longer nanotube length up to 220 μm by anodization in EG containing 2 wt% H2O and 0.3 wt% NH4F. Further increase of water content and NH4F concentration leads to disequilibrium reaction between electrochemical oxidation and chemical dissolution and thus resulted in shorter nanotube in the range of 54–136 μm (Table 1).

Table 1.

Summary of nanotube length (in μm) obtained by varying the concentration of H2O of 1–3 wt%, and NH4F of 0.1–0.5 wt% in EG with respect to fresh and once-used solution [35].

In the presence of optimum H2O content, O2– and/or OH are injected into the body of the oxide layer, and affect the structure efficiently to impede the ionic transport at barrier layer [38]. This greatly accelerates the inward movement of the metal/oxide interface into the metal surface and thus resulting in long nanotubes with thick walls. Higher content of H2O largely increases the number of extracted oxygen and/or hydroxyl ions per unit area of the oxide layer, leading to higher chemical dissolution. The increase in the F concentration provides higher chemical dissolution at the oxide/electrolyte interface, thereby allowing higher number of ion migrate across thin barrier layer. This resulted in the formation of long nanotube with thin walls. However, high chemical dissolution in electrolyte containing high F concentration induces a significant loss from the pore mouth and thus formed short nanotubes.

The anodic growth of TNA in used electrolyte significantly increased the nanotube length. Lower electrical conductivity of used electrolyte hinders ionic migration across barrier layer, thereby reducing loss at the pore tip by high chemical dissolution. Inner and outer diameters and nanotube length were found to increase with increasing applied potential from 20 V to 60 V (Table 2). Further increase of applied potential to 65 V resulted in further increase in inner and outer diameters but decreased the nanotube length. This implies a significant loss at the pore tip by high chemical dissolution under applied potential higher than 60 V. The anodization time is also an important available. The nanotube length increased with increasing anodization time, and achieved a maximum of 360 μm at 96 h. The growth rate was found as 241.7 nm min−1 at 4 h. It decreased exponentially and reached a minimum of 62.5 nm min−1 at 96 h. Paulose and co-workers [15] later achieved the formation of ultra-long TNA with 1000 μm in length by anodization in EG containing 3.5 wt% H2O and 0.6 wt% NH4F at 60 V for 216 h.

Table 2.

Summary of nanotube inner diameter, outer diameter and length obtained by anodization in fresh-EG containing 2 and 0.3 wt% NH4F at different applied potential for 17 h [35].

2.2.5. Polyol – Diethylene glycol (DEG), triethylene glycol (TEG), polyethylene glycol (PEG)

The investigation of organic electrolyte was extended to several types of polyol solvents, for example diethylene glycol (DEG), triethylene glycol (TEG) and polyethylene glycol (PEG) in comparison to EG [39]. Large amount of oxy and hydroxyl groups in TEG and PEG allows higher self-association via intra- and intermolecular hydrogen bonds, and consequently forms anatase crystallite by bridging the oxygen atom and hydroxyl groups in TiO2. However, their high viscosity and molecular weight retard the growth of nanotubes, and thus does not satisfy the requirement of practical applications. In 2010, Sreekantan et al. [3] demonstrated extremely fast-formation of TNA with approximately ~15 μm in length by anodization in EG containing excessive-fluoride 0.5 wt% NH4F and 1 wt% H2O. The nanotubes were formed with high growth rate up to 308.3 nm min−1. However, high chemical dissolution in EG containing excessive-fluoride limits the anodization time at 1 h. Recently, the addition of alkali species appears as alternative approach to improve the balance between electrochemical oxidation and chemical dissolution. The incorporation of sodium carbonate (NaCO3) into EG allowed the rapid growth of TNA with the growth rate up to 1 μm min−1 [40]. It is noteworthy that the anodic growth of TNA in EG is only method that induces the carbon species into the nanotube through the pyrogenation of ethylene (C2H2) in EG [41], thereby enabling visible-light absorption [42] without urther processing [43, 44].


3. Conclusion

TNA is by far among the most investigated functional metal oxide. The possibility of growing porous anodic nanostructure, particularly self-organized and highly-ordered TNA through anodization has further enlarged the research interest on this TNA due to specific advantages, such as large surface area, relatively long electron diffusion length and biocompatibility. In this chapter, the formation of TNA and various parameters, which affects the tube formation and properties of TNA were discussed. The tube length, thickness, and diameter were varied according to the pH, electrolytes, anodization potential, and time. Today, TNA are used as solar cell, self-cleaning coating, orthopedic and dental implants, and also an effective drug delivery carrier for the cancer therapy.



The authors are thankful to the Ministry of Education (MOE) Malaysia for funding this work under Transdisciplinary Research Grant Scheme (TRGS) grant no. 6769002. The authors are very much grateful to Universiti Sains Malaysia (USM) for providing the necessary facilities to carry out the research work and financial support under Research University (RU) grant no. 814281.


Conflict of interest

There is no conflict of interest in this chapter.


  1. 1. Zhao J, Wang X, Li L. Electrochemical fabrication of well-ordered titania nanotubes in H3PO4/HF electrolytes. Electronics Letters. 2005;41:771-772. DOI: 10.1049/el:20051328
  2. 2. Saharudin KA, Sreekantan S, Lai CW. Fabrication and photocatalysis of nanotubular C-doped TiO2 arrays: Impact of annealing atmosphere on the degradation efficiency of methyl orange. Materials Science in Semiconductor Processing. 2014;20:1-6. DOI: 10.1016/j.mssp2013.12.019
  3. 3. Sreekantan S, Saharudin KA, Lockman Z, Tzu TW. Fast-rate formation of TiO2 nanotube arrays in an organic bath and their applications in photocatalysis. Nanotechnology. 2010;21:365603. DOI: 10.1088/0957-4484/21/36/365603
  4. 4. Park H, Kim W-R, Jeong H-T, Lee J-J, Kim H-G, Choi W-Y. Fabrication of dye-sensitized solar cells by transplanting highly ordered TiO2 nanotube arrays. Solar Energy Materials and Solar Cells. 2011;95:184-189. DOI: 10.1016/j.solmat.2010.02.017
  5. 5. Roy P, Berger S, Schmuki. TiO2 nanotubes: Synthesis and applications. Angewandte Chemie. 2011;50:2904-2939. DOI: 10.1002/anie.201001374
  6. 6. Alivov Y, Fan ZY. Dye-sensitized solar cells using TiO2 nanoparticles transformed from nanotube arrays. Journal of Materials Science. 2010;45:2902-2906. DOI: 10.1007/s10853-010-4281-2
  7. 7. Saharudin KA, Sreekantan S, Abd Aziz S, Hazan R, Lai CW, Mydin R. Surface modification and bioactivity of anodic Ti6Al4V alloy. Journal of Nanoscience and Nanotechnology. 2013;13:1696-1705. DOI: 10.1166/jnn.2013.7115
  8. 8. Lin Z, Lee G-H, Liu C-M, Lee I-S. Controls in wettability of TiOx films for biomedical applications. Surface and Coatings Technology. 2010;205:S391-S3S7. DOI: 10.1016/j.surfcoat.2010.08.052
  9. 9. Mun K-S, Alvarez SD, Choi W-Y, Sailor MJ. A stable, label-free optical interferometric biosensor based on TiO2 nanotube arrays. ACS Nano. 2010;4:2070-2076. DOI: 10.1021/nn901312f
  10. 10. Kwon Y, Kim H, Lee S, Chin I-J, Seong T-Y, Lee WI, et al. Enhanced ethanol sensing properties of TiO2 nanotube sensors. Sensors and Actuators B: Chemical. 2012;173:441-446. DOI: 10.1016/j.snb.2012.07.062
  11. 11. Peighambardoust N-S, Nasirpouri F. Manipulating morphology, pore geometry and ordering degree of TiO2 nanotube arrays by anodic oxidation. Surface and Coatings Technology. 2013;235:727-734. DOI: 10.1016/j.surfcoat.2013.08.058
  12. 12. Macak JM, Tsuchiya H, Schmuki P. High-aspect-ratio TiO2 nanotubes by anodization of titanium. Angewandte Chemie. 2005;44:2100-2102. DOI: 10.1002/anie.200462459
  13. 13. Shankar K, Mor GK, Prakasam HE, Yoriya S, Paulose M, Varghese OK, et al. Highly-ordered TiO2 nanotube arrays up to 220 μm in length: Use in water photoelectrolysis and dye-sensitized solar cells. Nanotechnology. 2007;18:065707. DOI: 10.1088/0957-4484/18/6/065707
  14. 14. Cai QY, Paulose M, Varghese OK, Grimes CA. The effect of electrolyte composition on the fabrication of self-organized titanium oxide nanotube arrays by anodic oxidation. Journal of Materials Research. 2005;20:230-236. DOI: 10.1557/JMR.2005.0020
  15. 15. Paulose M, Prakasam HE, Varghese OK, Peng L, Popat KC, Mor GK, et al. TiO2 nanotube arrays of 1000 μm length by anodization of titanium foil: Phenol red diffusion. The Journal of Physical Chemistry C. 2007;111:14992-14997. DOI: 10.1021/jp075258r
  16. 16. Lockman Z, Ismail S, Sreekantan S, Schmidt-Mende L, MacManus-Driscoll JL. The rapid growth of 3 μm long titania nanotubes by anodization of titanium in a neutral electrochemical bath. Nanotechnology. 2010;21. DOI: 10.1088/0957-4484/21/5/055601
  17. 17. Wan J, Yan X, Ding J, Wang M, Hu K. Self-organized highly ordered TiO2 nanotubes in organic aqueous system. Materials Characterization. 2009;60:1534-1540. DOI: 10.1016/j.matchar.2009.09.002
  18. 18. Antony RP, Mathews T, Dash S, Tyagi AK, Raj B. X-ray photoelectron spectroscopic studies of anodically synthesized self aligned TiO2 nanotube arrays and the effect of electrochemical parameters on tube morphology. Materials Chemistry and Physics. 2012;132:957-966. DOI: 10.1016/j.matchemphys.2011.12.041
  19. 19. Ruan C, Paulose M, Varghese OK, Mor GK, Grimes CA. Fabrication of highly ordered TiO2 nanotube arrays using an organic electrolyte. The Journal of Physical Chemistry B. 2005;109:15754-15759. DOI: 10.1021/jp052736u
  20. 20. Gong D, Grimes CA, Varghese OK, Hu WC, Singh RS, Chen Z, et al. Titanium oxide nanotube arrays prepared by anodic oxidation. Journal of Materials Research. 2001;16:3331-3334. DOI: 10.1557/JMR.2001.0457
  21. 21. Mohamed AER, Rohani S. Modified TiO2 nanotube arrays (TNTAs): Progressive strategies towards visible light responsive photoanode, a review. Energy & Environmental Science. 2011;4:1065-1086. DOI: 10.1039/C0EE00488J
  22. 22. Taveira LV, Macák JM, Tsuchiya H, Dick LFP, Schmuki P. Initiation and growth of self-organized TiO2 nanotubes Anodically formed in NH4F∕(NH4)2SO4 electrolytes. Journal of the Electrochemical Society. 2005;152:B405. DOI: 10.1149/1.2008980
  23. 23. Yasuda K, Schmuki P. Control of morphology and composition of self-organized zirconium titanate nanotubes formed in (NH4)2SO4/NH4F electrolytes. Electrochimica Acta. 2007;52:4053-4061. DOI: 10.1016/j.electacta.2006.11.023
  24. 24. Ghicov A, Schmuki P. Self-ordering electrochemistry: A review on growth and functionality of TiO2 nanotubes and other self-aligned MOx structures. Chemical Communications. 2009:2791-2808. DOI: 10.1039/B822726H
  25. 25. Beranek R, Hildebrand H, Schmuki P. Self-organized porous titanium oxide prepared in H2SO4/HF electrolytes. Electrochemical and Solid-State Letters. 2003;6:B12. DOI: 10.1149/1.1545192
  26. 26. Sreekantan S, Hazan R, Lockman Z. Photoactivity of anatase–rutile TiO2 nanotubes formed by anodization method. Thin Solid Films. 2009;518:16-21. DOI: 10.1016/j.tsf.2009.06.002
  27. 27. Bauer S, Kleber S, Schmuki P. TiO2 nanotubes: Tailoring the geometry in H3PO4/HF electrolytes. Electrochemistry Communications. 2006;8:1321-1325. DOI: 10.1016/j.elecom.2006.05.030
  28. 28. Allam NK, Grimes CA. Formation of vertically oriented TiO2 nanotube arrays using a fluoride free HCl aqueous electrolyte. The Journal of Physical Chemistry C. 2007;111:13028-13032. DOI: 10.1021/jp073924i
  29. 29. Morita M, Shibata T, Yoshimoto N, Ishikawa M. Anodic behavior of aluminum in organic solutions with different electrolytic salts for lithium ion batteries. Electrochimica Acta. 2002;47:2787-2793. DOI: 10.1016/S0013-4686(02)00164-0
  30. 30. Ono S, Saito M, Asoh H. Self-ordering of anodic porous alumina formed in organic acid electrolytes. Electrochimica Acta. 2005;51:827-833. DOI: 10.1016/j.electacta.2005.05.058
  31. 31. Alivov Y, Pandikunta M, Nikishin S, Fan ZY. The anodization voltage influence on the properties of TiO2 nanotubes grown by electrochemical oxidation. Nanotechnology. 2009;20:225602. DOI: 10.1088/0957-4484/20/22/225602
  32. 32. Paulose M, Shankar K, Yoriya S, Prakasam HE, Varghese OK, Mor GK, et al. Anodic growth of highly ordered TiO2 nanotube arrays to 134 μm in length. Journal of Physical Chemistry B. 2006;110:16179-16184. DOI: 10.1021/jp064020k
  33. 33. Yoriya S, Paulose M, Varghese OK, Mor GK, Grimes CA. Fabrication of vertically oriented TiO2 nanotube arrays using dimethyl sulfoxide electrolytes. The Journal of Physical Chemistry C. 2007;111:13770-13776. DOI: 10.1021/jp074655z
  34. 34. Macak JM, Schmuki P. Anodic growth of self-organized anodic TiO2 nanotubes in viscous electrolytes. Electrochimica Acta. 2006;52:1258-1264. DOI: 10.1016/j.electacta.2006.07.021
  35. 35. Prakasam HE, Shankar K, Paulose M, Varghese OK, Grimes CA. A new benchmark for TiO2 nanotube array growth by anodization. The Journal of Physical Chemistry C. 2007;111:7235-7241. DOI: 10.1021/jp070273h
  36. 36. Cai Q, Yang L, Yu Y. Investigations on the self-organized growth of TiO2 nanotube arrays by anodic oxidization. Thin Solid Films. 2006;515:1802-1806. DOI: 10.1016/j.tsf.2006.06.040
  37. 37. Lee K, Kim D, Schmuki P. Highly self-ordered nanochannel TiO2 structures by anodization in a hot glycerol electrolyte. Chemical Communications. 2011;47:5789-5791. DOI: 10.1039/C1CC11160D
  38. 38. Li Y-M, Young L. Non-thickness-limited growth of anodic oxide films on tantalum. Journal of the Electrochemical Society. 2001;148:B337-BB42. DOI: 10.1149/1.1386387
  39. 39. Allam NK, Grimes CA. Room temperature one-step polyol synthesis of anatase TiO2 nanotube arrays: Photoelectrochemical properties. Langmuir : The ACS Journal of Surfaces and Colloids. 2009;25:7234-7240. DOI: 10.1021/la9012747
  40. 40. Wang D, Liu L, Zhang F, Tao K, Pippel E, Domen K. Spontaneous phase and morphology transformations of anodized titania nanotubes induced by water at room temperature. Nano Letters. 2011;11:3649-3655. DOI: 10.1021/nl2015262
  41. 41. An G, Ma W, Sun Z, Liu Z, Han B, Miao S, et al. Preparation of titania/carbon nanotube composites using supercritical ethanol and their photocatalytic activity for phenol degradation under visible light irradiation. Carbon. 2007;45:1795-1801. DOI: 10.1016/j.carbon.2007.04.034
  42. 42. Mohapatra S, Misra M, Mahajan V, Raja K. A novel method for the synthesis of titania nanotubes using sonoelectrochemical method and its application for photoelectrochemical splitting of water. Journal of Catalysis. 2007;246:362-369. DOI: 10.1016/j.jcat.2006.12.020
  43. 43. Park JH, Kim S, Bard AJ. Novel carbon-doped TiO2 nanotube arrays with high aspect ratios for efficient solar water splitting. Nano Letters. 2006;6:24-28. DOI: 10.1021/nl051807y
  44. 44. Raja KS, Gandhi T, Misra M. Effect of water content of ethylene glycol as electrolyte for synthesis of ordered titania nanotubes. Electrochemistry Communications. 2007;9:1069-1076. DOI: 10.1016/j.elecom.2006.12.024

Written By

Khairul Arifah Saharudin, Srimala Sreekantan, Rabiatul Basria S. N. M. Mydin, Norfatehah Basiron and Warapong Krengvirat

Submitted: December 1st, 2017 Reviewed: January 18th, 2018 Published: February 13th, 2018