Hydroxyapatite (HA) is an important synthetic biomaterial owing to its similarity to naturally occurring biological apatite found in the organs of living organisms. It is the major constituent of inorganic component of human hard tissues, bone, teeth and tendon, which is responsible for the stability, hardness and function of these organs. Majority of calcium phosphates are remarkably biocompatible and bioactive. This property is increasingly important in medicine and dentistry [1] . However, it is soft in its nature which limits its application to non-load bearing parts and segments only. It cannot sustain large constant and impact loads and undergoes deformation which causes them to lose their shape. For example, in a study by Ashok and co-workers [1] , it is shown that hydroxyapatite only stays intact and maintains their integrity under normal operating conditions. As the loading is increased and becomes critical, fine hydroxyapatite crystals starts disintegrating and finally deteriorate resulting in de shaping of internal and external structure of organ or wound. This may be illustrated by another example, in which synthetic hydroxyapatite crystals were compacted and sintered to make pellets which are subjected to indentation hardness [2] . Again, they do not exhibit consistency in their behaviour with the application of load like metals or alloys. Under the effect of indenter, they tend to show complete structural disintegration and no visible or remarkable indent shape is observed. This property, however, is a strong function of applied load and sintering conditions and its effect varies from case to case. Doping is a technique which is attributed to countering this effect and contributes towards increase of hardness of synthetic hydroxyapatite [3] [4] [5] [6] . Classically, HA powders and coatings can be synthesised using several methods including sol-gel processing [7] , wet chemistry and co-precipitation [8] , emulsion techniques, microwave synthesis [9] , batch hydrothermal processes [1] [2] [10] [11] [12] [13] , mechano-chemical methods, sono-chemical methods and chemical vapour deposition. The disadvantages of these methods include: Imprecise control over reaction conditions, expensive starting materials or large amounts of toxic organic solvents, expensive tooling, and/or prolonged reaction time. Furthermore, the aforementioned synthesis approaches give little or no control over HA particle characteristics (i.e. particle size, its distribution, agglomeration surface area, morphology and shape) [2] . These drawbacks could be overcome by adopting to certain modifications in hydrothermal process which is one of the oldest techniques used to develop different forms of crystalline material(s) [13] . In biomaterials development, it has gained recent attention due to its ability to produce nanosize crystals, time and energy efficiency, low temperatures and hence low processing cost [12] . Disadvantages include high initial cost and inability to go to high temperatures to achieve high productivity by speeding up of the process due to inner liner (TEFLON) limitation. Recently, hydroxyapatite [1] [2] [10] [11] and titania [14] [15] [16] [17] [18] powders are produced by hydrolysis [15] [17] or hydrothermal techniques [15] [16] [18] employing homogeneous and heterogeneous type reactions using different precursors and/or starting materials (e.g. isopropoxide with [16] or without [14] [17] acetic acid). In titania, two distinct phases occur namely Rutile and Anatase. Rutile is always used as a source of light scattering but anatase is used as photo catalyst and photo-electron transfer medium [17] . Results showed that hydrothermal processing saves a lot of time and energy and is environment friendly to produce very fine size pure (phase pure) and mixed hydroxyapatite and titania (mixture of anatase and rutile) powders. In present study, above mentioned bottlenecks are removed, and inherent advantages are utilised by employing a novel batch hydrothermal reactor which gives higher yield, higher throughput and versatility in control of reaction conditions by manipulation of temperature and pressure not attempted previously. This results in improved and enhanced product quality. Carefully selected calcium and ammonium precursors of salts and hydroxides are used as starting material for the synthesis of hydroxyapatite under strong basic conditions followed by hydrothermal treatment at 130˚C for 6 hrs and organic oxide of titanium along with acid―base reflux is used as starting material for the synthesis of titania under strong basic conditions. The phase, structure, composition and morphology are studied by x-ray diffraction (XRD), Fourier transform infrared spectroscopy (FTIR), and differential scanning calorimetry (DSC)―thermos-gravimetric analysis (TGA) analysis techniques.

Hydroxyapatite nano powder (phase pure), phase pure titania and homogeneously and heterogeneously titania mixed (doped) hydroxyapatite are synthesized by hydrothermal route. Calcium Nitrate (Ca(NO₃)₂∙4H₂O), ≥99.0%, Fluka Chemie, Switzerland), di-ammonium hydrogen phosphate ((NH₄)₂HPO₄) Assay 99% - 102%, Sigma Aldrich Inc. USA) and ammonium hydroxide (NH₄OH, 5.0 N, Sigma Aldrich Inc, USA) were used as starting material. Also, titanium dioxide micro powder is synthesized by hydrothermal route. titanium propoxide (Ti(OC₃H₇)₄), 98%, Fluka Chemie, Switzerland), ammonium hydroxide (NH₄OH, 5.0 N, Sigma Aldrich Inc, USA) and nitric acid (HNO₃, 65% Merck, Germany) were used as starting materials. Same chemicals are also used for homogeneous reactions. Calculated amount of calcium nitrate (Table 1) is first

dissolved in water and di-ammonium hydrogen phosphate is added in it drop wise (40 drops/min) (~1.4 ml/sec) using 250 ml dropping funnel. Immediate precipitation starts. pH of solution is maintained at ~11 and not allowed to go below 10 by continuous time dependent addition of NH₄OH (hydroxyapatite formation).

For homogeneous precipitation, calculated amount of titanium isopropoxide (TPO) (Ti(OC₃H₇)₄) (Table 1) is first mixed with calcium nitrate under the action of rigorous stirring and di-ammonium hydrogen phosphate is added in it drop wise (40 drops/min) (~1.4 ml/sec) using 250 ml dropping funnel. Immediate precipitation starts. pH of solution is maintained at ~11 and not allowed to go below 10 by continuous time dependent addition of NH₄OH. For heterogeneous precipitation, first phase pure titania is synthesized. This is done by addition of NH₄OH solution to (Ti(OC₃H₇)₄) in an ice bath to form titanic acid (Ti(OH)₄) and then dissolved with HNO3 to form titanyl nitrate (TiO(NO₃)₂). HNO₃ was added until the pH of final solution becomes 1. This is washed with excess water to separate out titania which is then dried. Final titania crystals are scraped out from filter paper. Calculated amount of these titania (TiO₂) crystals (Table 1) is mixed with calcium nitrate with constant stirring by using inert TEFLON stirrer. di-ammonium hydrogen phosphate is added in it drop wise (40 drops/min) (~1.4 ml/sec) using 250 ml dropping funnel. Immediate precipitation starts. pH of solution is maintained at ~11 and not allowed to go below 10 by continuous time dependent addition of NH₄OH. All three above mixtures are poured into hydrothermal vessel one after the other and treated at 130˚C for 6 hrs. Final solutions are filtered and dried in an Oven (Diahan Scientific Co., Korea) at 80˚C for 24 hrs to form final products. Hydrothermal vessel used for conducting reactions is shown schematically in below figure (Figure 1(A) and Figure 1(B)) to illustrate its manufacture and construction. The significance of this device is that it was first of its kind in Pakistan used for production of hydroxyapatite and other reactive oxides at large scale. Vessel has the capacity to produce 1 Kg hydroxyapatite in one batch. Process has higher efficiency, is environment friendly and easy to control. Very fine crystals are produced which can be further tailored to the meet requirement of application.

Flow chats describing synthesis and processing of all three materials are shown in Figures 2(A)-(C) below. They describe in detail the step by step production of hydroxyapatite, homogeneously precipitated hydroxyapatite and titania (co precipitated) and heterogeneously precipitated hydroxyapatite and titania (seeded growth).

The phases were studied by an X-ray diffractometer (BRUKER D8-Advanced, USA at Department of Chemistry, Quaid-e-Azam University, Islamabad, Pakistan) (step size 0.02, scan Rate 2o/s, voltage 40 KV, radiation Cu Kα). (Figure 3(A) & (Figure 3(B)). Infrared spectroscopic analysis of nanopowder was done using Nicolet 6700 FT-IR Thermo Fisher, USA Instrument at IRCBM, COMSATS Institute of information technology, Lahore, Pakistan (Resolution 8 cm⁻¹, Scan

time 256, Region 500 - 4000 cm⁻¹) (Figure 4(A) & (Figure 4(B)). DSC and TGA analysis was done using SDT (DSC-TGA Q 600 TA, USA Instrument at IRCBM, COMSATS Institute of information technology, Lahore, Pakistan (heating rate 10˚C/min, heating temperature 1200˚C) (Figures 5(A)-(h)).

1) X-Ray Diffraction (XRD)

XRD pattern of hydroxyapatite (phase pure), Titania (phase pure), Hydroxyapatite and titania (homogeneous precipitation) and Hydroxyapatite, titania (heterogeneous precipitation) as precipitated and heat treated 1000˚C, 1 hr are shown in Figure 3(A) & Figure 3(B) respectively. They are identified as HAp (Figure 3(A) & Figure 3(B)-(a)) [19] [20] . All peaks correspond to hexagonal crystal system of HAp [21] . Meanwhile, the high purity of HA phase was confirmed by XRD patterns. However, it is shown that the diffraction peaks of HAp in pattern ((B) (a)) are much stronger than pattern ((A) (a)) indicating that the crystallinity of the HAp nanoparticles heat treated after processing is much higher than “as precipitated” also XRD patterns of the powders treated for 6 hrs show peaks attributed only to HAp, indicating the absence of monetite (CaHPO₄) [10] .

Figure 3(A) & Figure 3(B)-(b) shows the XRD pattern of TiO₂ nanopowder

synthesized by hydrothermal route treated at 130˚C for 6 hrs and dried at 80˚C for 24 hrs (Figure 3(A)-(b)), treated at 130˚C for 6 hrs, dried at 80˚C for 24 hr and heat treated 1000˚C for 1 hr (Figure 3(B)-(b)). At 130˚C for 6 hrs and dried at 80˚C for 24 hrs multiphase of anatase and rutile structure of TiO₂ nanopowder were obtained [22] . Pattern exhibited strong diffraction peaks at 26˚, 27˚, 36˚, 49˚ and 54˚ indicating TiO₂ in the anatase and rutile phase [23] while at 130˚C for 6 hrs, dried 80˚C for 24 hrs and heat treated 1000˚C for 1 hr pattern exhibited strong diffraction peaks at 27˚, 36˚ and 54˚ indicating TiO₂ in the form of rutile phase [23] . The temperature and holding time of hydrothermal process was lower than the previously reported values [24] . The noise in the pattern is due to large step size and less step time, the wideness is due to nanosized [25] . From Figure 3(A) & Figure 3(B)-(b), it was shown that the diffraction pattern peak intensity of the TiO₂ increases with increasing particles size. These results suggested that the nano-TiO₂ powder is composed of irregular polycrystals. Amorphous structure revealed a broad pattern with low intensity; however, the effect of the amorphous materials on the broadening of the XRD patterns of nanosized TiO₂ is negligible [23] .

Figure 3(A) & Figure 3(B)-(c) shows the XRD pattern of TiO₂ and hydroxyapatite nanopowder co precipitated (homogeneous precipitation) by hydrothermal route while keeping the operating parameter same as for standalone hydroxyapatite and titania processing. At 130˚C for 6 hrs and dried at 80˚C for 24 hrs pattern is typical of hydroxyapatite [19] [20] , however it is not that distinct as Figure 3(A)-(a) above and this deviation from distinct pattern is attributed to the presence of small amount of titania (anatase) though there is no sharp evidence/peak of it at given experimental conditions which is confirmed later on (Figure 3(B)-(c)). Same powder treated thermally at 1000˚C for 1 hour shows sharp peaks of titania (rutile) along with hydroxyapatite indicating successful doping (Figure 3(B)-(c)). Pattern exhibited strong diffraction peaks at 34˚ and 48˚ indicating TiO₂ in the form of rutile phase [26] . Further analysis of pattern exhibits absence of TCP indicating formation of phase pure hydroxyapatite [27] .

Figure 3(A) & Figure 3(B)-(d) shows the XRD pattern of TiO₂ and hydroxyapatite nanopowder (seeded growth (heterogeneous precipitation)) synthesized by hydrothermal route while keeping the operating parameter same as for standalone hydroxyapatite and titania processing. At 130˚C for 6 hrs and dried at 80˚C for 24 hrs pattern is typical of hydroxyapatite [19] [20] . Titania, though present in the composition, does not shows up in the pattern, is due to the fact percentage of titania is too low as well as powder is in as precipitated condition. Pattern also differs from standard phase pure hydroxyapatite pattern [19] [20] (i.e. shows peak broadening and intensity change) due to aforementioned reasons. Same powder treated thermally at 1000˚C for 1 hour shows sharp peaks of titania (rutile) along with hydroxyapatite indicating successful doping (seeded growth of hydroxyapatite on already existing titania (precursor) nanoparticles) (Figure 3(B)-(d)). Pattern exhibited strong diffraction peaks at 34˚ and 48˚ indicating TiO₂ in the form of rutile phase [26] .

From thermodynamics and kinetics stand point [9] , undercooling is suppressed while kinetics is promoted during hydroxyapatite synthesis and processing, Undercooling is suppressed by continuous time dependent supply of heat from reaction itself (autogenous reaction), and from external heating elements. This combination of heating does not allow solution to go to a subzero temperature or at a temperature below crystallization temperature. Thus, no undercooling occurs at all. This also promotes proper crystallisation as it gives ample time to solution to allow second phase to precipitate out from it due to difference in solubility/immiscibility. On the other hand, kinetics is promoted as again there is enough time available for solute to come out of solution along with existence of a thermal gradient. These both factors contribute towards triggering of nucleation and growth events and their promotion. Proper crystallisation occurs which is a distinct and significant feature of this process for hydroxyapatite synthesis. This may be explained more elaborately by the help of a cooling curve.

2) Fourier Transform Infrared (FTIR) Spectroscopy

FTIR Spectra of hydroxyapatite (phase pure), Titania (phase pure), Hydroxyapatite and titania (co precipitated (homogeneous precipitation)) and Hydroxyapatite, titania (seeded growth (heterogeneous precipitation)) as precipitated and heat treated at 1000˚C, 1 hr are shown in Figure 4(A) & Figure 4(B) respectively.

i) Hydroxyapatite

The wave numbers for characteristic peaks in both spectra are a function of heat treating temperature and changes with degree of heat treatment given which helped in removal of unwanted constituents and/or formation of new phases [28] .

・ Bands at 3572, 631, and 342 cm⁻¹ are assigned to stretching mode (νs), librational mode (νL), and translational mode (νT), respectively, of the hydroxyl group, OH [8] [29] . The peak at 342, which is followed by another weak at 355 cm⁻¹ (known as shoulder peak), is assigned to the hydroxyl group oscillating vertically to the crystallographic c-axis approaching and going away from the neighbouring plane defined by the three calcium ions, Ca²⁺ [30] .

・ Bands at 1087, 1072 - 1032, 962, 601, 571, and 474 cm⁻¹ are assigned to vibrations of the phosphate group, PO₄. The first peak at 1087 cm⁻¹ emanates from a triply degenerated asymmetric stretching mode vibration, ν₃ [8] [31] . The other two components of this triply degenerated vibration (ν₃) of the P−O bond of the phosphate group appear at 1046 and 1032 cm⁻¹. The peak at 962 cm⁻¹ is assigned to a nondegenerated symmetric stretching mode (ν₁) of the P−O bond of the phosphate group, PO₄ [30] . The peaks at 601, 575, and 561 cm⁻¹ are assigned to a triply degenerated bending mode (ν₄) of the O−P−O bond [30] . The weak peaks at 472 and the shoulder at 462 cm⁻¹ are components of the doubly degenerated bending mode, (ν₂) of the phosphate group, PO₄ [30] [32] .

・ The peak at 2000 cm⁻¹ is assigned to a 2 ν₃ harmonic overtone or to a combination mode ν₁ + ν₃ [16] .

・ The peak at 361 cm cm⁻¹ is a combination mode from the difference ν₁ - ν₄ [30] .

・ The peaks at 2070 and 1154 cm⁻¹ have been interpreted as combination bands or harmonic overtones [33] .

This information is summarized in Table 2. The changes in the heat-treated sample was verified from the absence of peaks, which might be due to the removal of volatile constituents and/or transformation of low temperature phase(s) to high temperature phase(s) [34] [35] [36] .

ii) Titania

Characteristic peaks for N-H stretch appear at 3382.27 cm⁻¹ (S-A) & 3393.37 cm⁻¹ (S-B) [35] . A peak at 3498.77 (S-A) & at 3149.92 (S-B) occurs due to O-H stretch. Peak at wave number of 2911.70 (S-A) & 2908.58 (S-B) is due to C-H

w: weak, m: medium, s: strong, sh: shoulder, shp: sharp.

stretch. Peak at wave number of 2364.50 (S-A) & 2361.67 (S-B) is due to C (triple bond) N stretch in nitriles. Peak at wave number of 2109.48 (S-A) & 2117.26 (S-B) is due to C (triple bond) C stretch in alkynes. Peaks at wave number of 1685.42 & 1716.96 (S-A) & 1696.79 & 1716.66 (S-B) is due to C=O stretch in carbonyl (general) groups. Large domb (peak) on the left of spectra (Figure 4(A)) is may be due Unreacted species in reactants which are causing abnormalities [34] and adsorbed OH groups on the surface of titania [35] [36] which is not removed upon drying of materials at such low temperatures. This however, is removed at higher temperature heat treatment.

iii) Hydroxyapatite, titania (co precipitated (homogeneous precipitation))

The wave numbers for characteristic peaks in both spectra are a function of heat treatment temperature in this case also and changes with degree of heat treatment given, removing of unwanted constituents and/or formation of new phases [28] .

・ Bands at 3572, 631, and 342 cm⁻¹ are assigned to stretching mode (νs), librational mode (νL), and translational mode (νT), respectively, of the hydroxyl group, OH [8] [29] . The peak at 342, which is followed by another weak at 355 cm⁻¹ (shoulder), is assigned to the hydroxyl group oscillating vertically to the crystallographic c-axis approaching and going away from the neighbouring plane defined by the three calcium ions, Ca²⁺ [30] .

・ Bands at 1087, 1072 - 1032, 962, 601, 571, and 474 cm⁻¹ are assigned to vibrations of the phosphate group, PO₄. The first peak at 1087 cm⁻¹ emanates from a triply degenerated asymmetric stretching mode vibration, ν₃ [8] [31] . The other two components of this triply degenerated vibration, ν₃, of the P−O bond of the phosphate group appear at 1046 and 1032 cm⁻¹. The peak at 962 cm⁻¹ is assigned to a nondegenerated symmetric stretching mode, ν₁, of the P−O bond of the phosphate group, PO₄ [30] . The peaks at 601, 575, and 561 cm⁻¹ are assigned to a triply degenerated bending mode, ν₄, of the O−P−O bond [30] . The weak peaks at 472 and the shoulder at 462 cm⁻¹ are components of the doubly degenerated bending mode, ν₂, of the phosphate group, PO₄ [30] [32] .

・ The peak at 2000 cm⁻¹ is assigned to a 2 ν₃ harmonic overtone or to a combination mode, ν₁ + ν₃ [30] .

・ The peak at 361 cm⁻¹ is a combination mode from the difference ν₁ - ν₄ [30] .

・ The peaks at 2070 and 1154 cm⁻¹ have been interpreted as combination bands or harmonic overtones [33] .

iv) Hydroxyapatite, titania (seeded growth (heterogeneous precipitation))

The wave numbers for characteristic peaks in both spectra also depend on heat treatment temperature and alters with extent of heat treatment given which helped in removal of unwanted constituents and/or formation of new phases as occur in earlier formulations [28] .

・ Bands at 3572, 631, and 342 cm⁻¹ are assigned to stretching mode (νs), librational mode (νL), and translational mode (νT), respectively, of the hydroxyl group, OH [8] [29] . The peak at 342, which is followed by another weak at 355 cm⁻¹ (shoulder), is assigned to the hydroxyl group oscillating vertically to the crystallographic c-axis approaching and going away from the neighbouring plane defined by the three calcium ions, Ca²⁺ [30] .

・ Bands at 1087, 1072 - 1032, 962, 601, 571, and 474 cm⁻¹ are assigned to vibrations of the phosphate group, PO₄. The first peak at 1087 cm⁻¹ emanates from a triply degenerated asymmetric stretching mode vibration, ν₃ [8] [31] . The other two components of this triply degenerated vibration, ν₃, of the P−O bond of the phosphate group appear at 1046 and 1032 cm⁻¹. The peak at 962 cm⁻¹ is assigned to a nondegenerated symmetric stretching mode, ν₁, of the P−O bond of the phosphate group, PO4 [30] . The peaks at 601, 575, and 561 cm⁻¹ are assigned to a triply degenerated bending mode, ν₄, of the O−P−O bond [30] . The weak peaks at 472 and the shoulder at 462 cm⁻¹ are components of the doubly degenerated bending mode, ν₂, of the phosphate group, PO₄ [30] [32] .

・ The peak at 2000 cm⁻¹ is assigned to a 2 ν₃ harmonic overtone or to a combination mode, ν₁ + ν₃ [30] .

・ The peak at 361 cm⁻¹ is a combination mode from the difference ν₁ - ν₄ [30] .

・ The peaks at 2070 and 1154 cm⁻¹ have been interpreted as combination bands or harmonic overtones [33] .

c) Differential scanning calorimetry and thermo-gravimetric analysis (DSC-TGA)

i) Hydroxyapatite (phase pure)

The thermogram of the synthesized material shows three distinct stages of decomposition (Figure 5(A)). The first stage that occurs between 35˚C and 120˚C is due to loss of adsorbed water. The major weight loss that occurs between 150˚C and 260˚C is assigned to the decomposition of agarose and ammonium. The dehydration of Ca(OH)₂ into CaO also contributes to a part of this weight loss and the total weight loss in this second stage is 9.55%. The third weight loss that occurs between 260˚C and 380˚C is due to the decomposition of nitrate. This temperature range for nitrate decomposition was also reported previously [7] . DSC analysis (heating) (Figure 4(B)) shows a large broad peak demonstrated by HA powder, which is labelled from around 1200˚C to 1340˚C (extrapolated). It suggests the dehydration of HA over a wide temperature range and phase transformation of HA to oxyhydroxyapatite (OHAP, Ca₁₀(PO₄)₆(OH)_2-xO_x) [41] [42] . In order to further reveal the thermal behaviour of the samples at elevated temperatures. DSC cooling curves was also studied, which are demonstrated in Figure 5(B). It is found that, for pure HA, only one visible peak appears, which is around 1440˚C (not shown), and it may refer to the reversed full phase transformation from unstable a-TCP to α-TCP [42] . The a-TCP may come from the transformation of α-TCP at elevated temperatures [42] . Owing to lack of water in the pure nitrogen atmosphere, no peaks referring to reversible transformation from TCP or TTCP to oxyapatite or HA are present, which was revealed by other researchers using air circumstance [41] .

ii) Titania

TGA of the samples was carried out in the range ambient −1200˚C at heating rate of 10˚C minute in a nitrogen atmosphere [25] (Figure 5(C)). Prior to each run, the empty sample pan was completely tared to get accurate balance. The final weight loss is about 26.34%. Below 100˚C, the weight loss is attributed to the loss of adsorbed water on the surface of the powder. The second rage of weight lost ranges from 100˚C - 550˚C, is attributed to the decomposition of volatile organic solvents [14] [43] . The DSC curve (Figure 5(D)) showed a sharp endothermic peak around 100˚C, which was followed by a broad exothermic peak. The broad peak changed to a plateau shape around 520˚C, and continued until around 800˚C [44] , indicating no considerable change in titania over a temperature range.

iii) Hydroxyapatite, titania (co precipitated (homogeneous precipitation))

The thermogram of the synthesized material is more similar to that for titania, deviating from standard titania curve (Figure 5(C)), indicating the presence of hydroxyapatite as well (Figure 5(E)). It shows that below 100˚C, the weight loss is attributed to the loss of adsorbed water on the surface of the powder. The second rage of weight lost ranges from 100˚C - 550˚C, is attributed to the decomposition of volatile organic solvents [29] [30] . The final weight loss is about 23.81%. The DSC curve (Figure 5(F)) also deviates from standard curve for titania

(Figure 5(D)), indicating the presence of co precipitates of HA and titania as a result of homogeneous precipitation. Pattern showed a very sharp endothermic peak around 100˚C (characteristic of co precipitation), which was followed by a broad exothermic peak (including a small endothermic bump). The broad peak changed to a plateau shape around 520˚C, and continued until around 800˚C [41] .

iv) Hydroxyapatite, titania (seeded growth (heterogeneous precipitation))

Like phase pure HA (Figure 5(A)), the thermogram of the synthesized material shows three distinct stages of decomposition (Figure 5(G)). The first stage that occurs between 35˚C and 120˚C is due to loss of adsorbed water. The major weight loss that occurs between 150˚C and 260˚C is assigned to the decomposition of agarose and ammonium. The dehydration of Ca(OH)₂ into CaO also contributes to a part of this weight loss and the total weight loss in this second stage is 9.55%. The third weight loss that occurs between 260 and 380 ◦C is due to the decomposition of nitrate. The pattern has very high similarity to standard HA pattern because the amount of dopant (titania) is very small and is in “as precipitated” state. This is also confirmed by XRD pattern of same material and reinforces the hypothesis. DSC analysis (heating) (Figure 5(H)) shows a large broad peak demonstrated by HA powder, which is labelled from around 1200˚C to 1340˚C (not shown). It suggests the dehydration of HA over a wide temperature range and phase transformation of HA to oxyhydroxyapatite (OHAP, Ca₁₀(PO₄)₆(OH)_2-xO_x) as discussed previously for phase pure HA [41] [42] . DSC cooling curves also showed similar pattern as is observed in Figure 5(B) for phase pure HA. Like phase pure HA, only one visible peak is observed, which is around 1440˚C (not shown), and as discussed previously, it may refer to the reversed full phase transformation from unstable α ¯ -TCP to α-TCP [42] . which in turn may have originated from transformation of α-TCP at elevated temperatures [42] . Owing to lack of water in the pure nitrogen atmosphere, no peaks referring to reversible transformation from TCP or TTCP to hydroxyapatite or HA are present as was observed previously (Figure 5(B)) [41] . Similarity, Figure 5(B) and Figure 5(H) are attributed to same facts and are confirmed by subsequent XRD patterns.

a) Very fine powders of hydroxyapatite (phase pure), titania (mixture of anatase and rutile), HA, titania (co precipitated (homogeneous reaction)), HA, titania (seeded growth of HA onto titania (heterogeneous reaction)) are formed from novel batch hydrothermal process.

b) XRD patterns along with DSC-TGA scans show successful coprecipitation as well as doping of HA and titania, indicating successful completion of reaction under given condition providing a novel, low temperature quick route to fabricate HA and doped HA materials.

c) Homogeneous precipitation is observed to be a good method for production of doped materials with good process completion, efficiency and phase development.

d) DSC-TGA analysis showed product retained enough properties (in terms of non-transformed phases) to be used for further advanced applications (photocatalysis, drug delivery, and bio marking)

Author would like to thank Aqif A Chaudhry for his helpful guidance, encouragement, support and scientific discussion throughout the work. Author, also like to thank Dr. Adeel Afzal for help in conducting XRD, Ms Sehrish Mukhtar for conducting FTIR and Ms Inum Arshad for conducting TGA Analysis.

Rafique, M.M.A. (2018) Hydrothermal Processing of Phase Pure and Doped Hydroxyapatite and its Characterization. Journal of Encapsulation and Adsorption Sciences, 8, 18-37. https://doi.org/10.4236/jeas.2018.81002