Open Access

The usability of ark clam shell (Anadara granosa) as calcium precursor to produce hydroxyapatite nanoparticle via wet chemical precipitate method in various sintering temperature

  • Mohammad Zulhasif Ahmad Khiri1, 2,
  • Khamirul Amin Matori1, 2Email author,
  • Norhazlin Zainuddin3,
  • Che Azurahanim Che Abdullah2,
  • Zarifah Nadakkavil Alassan2,
  • Nur Fadilah Baharuddin1, 2 and
  • Mohd Hafiz Mohd Zaid2
SpringerPlus20165:1206

https://doi.org/10.1186/s40064-016-2824-y

Received: 6 April 2016

Accepted: 13 July 2016

Published: 29 July 2016

Abstract

This paper reported the uses of ark clam shell calcium precursor in order to form hydroxyapatite (HA) via the wet chemical precipitation method. The main objective of this research is to acquire better understanding regarding the effect of sintering temperature in the fabrication of HA. Throughout experiment, the ratio of Ca:P were constantly controlled, between 1.67 and 2.00. The formation of HA at these ratio was confirmed by means of energy-dispersive X-ray spectroscopy analysis. In addition, the effect of sintering temperature on the formation of HA was observed using X-ray diffraction analysis, while the structural and morphology was determined by means of field emission scanning electron microscopy. The formation of HA nanoparticle was recorded (~35–69 nm) in the form of as-synthesize HA powder. The bonding compound appeared in the formation of HA was carried out using Fourier transform infrared spectroscopy such as biomaterials that are expected to find potential applications in orthopedic and biomedical industries .

Keywords

HydroxyapatiteArk clam shellWet chemical precipitateSinteringStructural

Background

Recently, hydroxyapatite (HA) was widely used in the field of orthopedic and biomedical application (Rujitanapanich et al. 2014; Singh and Purohit 2011; Dědourková et al. 2012; Hoque et al. 2014). The structure of HA which is similar to the structure of bone become the main criteria in the creation and innovation of future synthetic bone. HA has been synthesis using various methods, and the most practical technique is known as wet chemical precipitation. HA with the molecular formula of Ca10(PO4)6(OH)2 is one of the essential mineral consist from the calcium phosphate salt group (Rajkumar et al. 2011). It is the most stable calcium phosphate salt among the other salt such as tricalcium phosphate (TCP) and tetracalcium phosphate (TTCP) at the range pH value in between 4 and 12 and at normal temperatures (Koutsopoulos 2002; Sadat-Shojai et al. 2013; Abidi and Murtaza 2014). The composition of HA will be formed when the stoichiometric of Ca/P ratio approximately in the range of 1.67 (Rujitanapanich et al. 2014; Abidi and Murtaza 2014). HA is usually found in the vertebrate group, especially in the hard tissue of bone and teeth enamel. The similarity properties of the chemical composition and the crystal structure of HA with the natural human bone give an alternative biomedical application uses in the human body such as bone implant for bone tissue substitution and drug delivery system (Santhosh and Prabu 2013). Besides, HA can be directly ingrowths in the host bone as artificial bones in human body and it was widespread used in orthopedic application due to its special abilities in bioactivity and biocompatibility (Zhang 2007).

HA is not only biocompatible, nontoxic, esteoconductive, non-inflammatory, but also bioactive (Fathi et al. 2008). The biocompatibility refer to the properties of material which is show biologically compatible with living system without gives any respond in local or systemic environment while bioactivity can be describe in any interaction or effect of material on living system. These properties are very important for synthetic bone which acts as bone grafting in successfully of osteoconductivity. This compound was commonly used as coating on metal implant to enhance their osteointegration (ability of biomaterial that can guide the reparative growth of natural bone) which promote the bone ingrowths between the host bone and artificial bone (Moore et al. 2001).

Sadat-Shojai et al. (2013) has been review the HA as a material used for the medical applications. From the evaluation, they state that HA can be synthesize using several methods such as wet method, dry method, high temperature process method, biogenic sources method and combination procedure method. Each method may produced different structure and morphology of HA due to its different starting “Methods”. According to their study, focusing on the wet method, it consist of several sub-group methods, which is known as conventional wet chemical precipitation, hydrolysis method, sol–gel method, hydrothermal method, emulsion method and sonochemical method. The wet chemical precipitate method was selected in this research due to promise the HA product in nano size with regular morphology. According to the statistic, the conventional wet chemical precipitation method is usually used in synthesize HA due to the economical advantages and versatile route (Angelescu et al. 2011). Moreover, it is also one of the easy ways to prepared HA powder under atmospheric condition (Wang et al. 2010). However, it needs extra attention to control the Ca:P ratio as well as the crystallinity (Mustafa 2005). The physical and chemical properties of HA produce in this method is depend on the techniques used and calcium precursor sources. Thus, the different technique and calcium source can affect the thermal stability of the as synthesized HA produce (Kamalanathan et al. 2014).

Recently, the uses of wastes material in order to synthesize HA was received encourage response from many researcher across the world. This idea gives an innovation to produce a new valuable product from the wastes material. Besides that, these wastes material also can be recycled, then change it into more valuable things and keep environment safely In previous report, HA was synthesize by using wastes material such as sea shell (Santhosh and Prabu 2013), eggshell (Dávila et al. 2007), animal bones (Sobczak et al. 2009), shell of garden snail (Singh 2012), and fruit waste extract (Wu et al. 2013). These materials consist of high source of calcium that can be act as calcium precursor which is suitable to produce HA. Therefore, this study has focused on the synthesis of HA by using the ark clam shell (ACS) as wastes material to be used in synthesis HA via wet chemical precipitate method. Some researcher found that the content of calcium carbonate (CaCO3) in ACS is approximately between 98 and 99 % (Kamba et al. 2013; Mohamed et al. 2012). ACS which is rich in calcium content was seen pursuant act as an initial material in synthesize HA. Mustafa et al. (2015), synthesize HA from ACS by sol–gel precipitate method give a positive result in getting high purity of HA. Furthermore, Rujitanapanich et al. was successfully to synthesize HA from abalone shell which is same group of clam shell via the same method at various pH value from 8 to 10 (Rujitanapanich et al. 2014). They found that, the crystallinity of the HA from abalone shell is good compare to the HA from commercial CaO. From that, they observed the crystallize size of HA was in nano size about 89.5 nm. The previous researcher prove that the HA nanocrystalline can be prepared from waste material at room temperature by simple wet precipitate. In Table 1, the summarizes of recent studies in synthesis HA from waste material with various method and properties.
Table 1

Recent studies of synthesis HA powder from waste and various method in period of 2010–2015

References

Raw material

Method

pH value

Powder properties

Venkatesan and Kim (2010)

Tuna bone

Drying

Pure HA in nano-sized range

Wu et al. (2011)

Oyster shell

Ball mailing and heat treatment

HA and β-TCP composition in the sample

Singh and Purohit (2011)

Garden Snail

Wet chemical precipitate

10

Pure HA in micron-sized range

Santhosh and Prabu (2013)

Sea shell

Wet chemical precipitate

10

Pure HA in nano-sized range

Rujitanapanich et al. (2014)

Oyster shell

Wet chemical precipitate

8–10

Improve crystallinity of HA at pH value of 10.

Kamalanathan et al. (2014)

Eggshell

Wet chemical precipitate

10.5 and above

Pure HA at low temperature and present of α-TCP and TTCP at high temperature

Wu et al. (2015)

Eggshell

Wet chemical precipitate

HA/β-TCP biphase at low temperature and pure HA at high temperature

Chen et al. (2015)

Abalone shell

Solid-state conversion

10

Mix of HA, calcite and aragonite composition in the sample. HA nanorod is obtained

Yelmilda et al. (2015)

Cockle shell

Hydrothermal

10–11

Pure HA in nano-sized range and no toxic effect

Shavandi et al. (2015)

Mussel shell

Rapid microwave irradiation

13

Pure HA in nano-sized range

This study

Ark clam shell

Wet chemical precipitate

8

Pure HA as-synthesized and nano-sized range. HA/β-TCP biphase composition was present at high temperature

In this research, HA powder was synthesized via wet chemical precipitate method using ACS with control pH value at 8. The purpose of this research is to investigate the effect of HA on physical, chemical properties, morphology and behaviour of biphasic HA/β-TCP at various sintering temperature.

Methods

ACS were thoroughly washed and cleaned to isolate the contaminate. Then, ACS was dried and transfer into the electrical furnace at a rate of 10 °C/min and holding at 900 °C for 4 h for the calcination process. The ACS consists of calcium carbonate (CaCO3) was transform to amorphous calcium oxide (CaO) by releasing carbon dioxide (CO2) during calcination process. The sample obtained was characterized by means of XRD to confirm the presence of CaO. Following Eq. (1) show the chemical reactions occur during calcinations process.
$${\text{CaCO}}_{3} \to {\text{CaO}} + {\text{CO}}_{2}$$
(1)
After that, the ACS has been through milling process with the milling balls in the jar at 100 rpm for 24 h to obtain a fine powder with a size of 45 μm. The obtained powder was used to prepare 1.0 M of calcium hydroxide solution (CaOH)2 by adding pre-determined amount of distilled water in the Eq. (2). The solution was stirred about 2 h to get the uniform mixing of (CaOH)2.
$${\text{CaO}} + {\text{H}}_{2} {\text{O}} \to {\text{Ca}}\left( {\text{OH}} \right)_{2}$$
(2)
In order to produce the HA powder, 0.6 M of phosphoric acid (H3PO4) was added to Ca(OH)2 at rate 15–20 drop/min by using titration technique with continuous stirring using a magnetic stirrer at room temperature. The estimated molar ratio of Ca:P was adjusted in the range between 1.67 and 2.00. The pH value of the solution was controlled and maintained around pH 8 by adding ammonium hydroxide solution (NH4OH) until the reaction was complete. The solution was continuously stirring and aging about 2 h. The gelatinous white precipitate was appeared when the solution was stop stirred. Subsequently, the solution was filtered and washed with distilled water several times before dried in the electrical furnace at 200 °C for 24 h to remove the water completely. The reaction of mixing of both solutions was showed below in Eq. (3) and the HA powder was produced.
$$10{\text{Ca}}\left( {\text{OH}} \right)_{2} + 6{\text{H}}_{3} {\text{PO}}_{4} {\text{Ca}}_{10} \to \left( {{\text{PO}}_{4} } \right)_{6} \left( {\text{OH}} \right)_{2} + 18{\text{H}}_{2} {\text{O}}$$
(3)
Then, HA powder was forms into pellet shape by using hydraulic press pellet machine with dimension of 13 mm in diameter and about 2 mm thick with 2.5 tons of applied load. Polyvinyl alcohol (PVA) were used as binder to avoid the pellet from crack and broken. The HA pellet were subjected to sintering in the furnace at temperatures of 200–1200 °C with an interval of 200 °C for 4 h and cooled in the furnace itself at room temperature. After the sintering process, the samples were characterized by XRD analysis using Philips X-ray diffractometer with Cu Kα radiation (λ = 1.5406 Å). The result was analyzed by using PANalytical X’Pert Pro PW3050/60 diffractometer at the diffraction angle (2θ) in scanning range from 20° to 60°. The densities of the samples were determined by using Archimedes method with water as the immersion liquid in this process. The molecular bonds structure of HA were observed by using FTIR(Perkim Elmer Spectrum 100 series) and FESEM (FEI NOVA NanoSEM 230) was used to study the morphology and microstructure of HA while EDX was carried out to analysis the elements present in HA.

Result and discussion

Characterization of ark clam shell to prepare hydroxyapatite

Physically, the ACS is tougher compared with calcined ACS and the appearance of calcined ACS produced was brittle and have yellowish white in colour. In detail, the XRD pattern of ACS in Fig. 1 shows the presence of pure CaCO3 phase while after treated the ACS at 900 °C calcination temperature, the pure CaO was observed by comparing with JCPDS files No. 005-0586 and 037-1497, respectively. The highest intensity peaks of CaCO3 were observed in the structure of ACS at 2θ = 29.5° while the highest peak of CaO was showed at a 2θ = 37.4° by calcined at 900 °C. In previous report, the decomposition of CaCO3 into the CaO and CO2 was occurs at the minimum temperature of 954 °C (Rujitanapanich et al. 2014). From XRD result, it can be observed that CaCO3 was completely converted to the CaO by calcination of CO2 at 900 °C for 4 h and eliminating other organic matter (Raya et al. 2015; Wang et al. 2007). The single phase of CaO also indicates that the complete transformation of CaCO3 to CaO has been occur. These results supported with previous reports, which suggest that the calcinations temperature of CaCO3 to CaO were at the range of 850–1000 °C due to the highest crystallinity and the formation of a single phase of CaO (Kamalanathan et al. 2014; Singh 2012). Singh (2012), mention that CaO is easily to be converted to Ca(OH) by absorbing moisture or water from surrounding atmosphere for the CaO prepared from shell of garden snail. Due to this reason, the precaution steps were taken by stored all the sample in desiccators to avoid vapor attack and taken out only during measurement of their properties. Besides that, the sample was preheated at 900 °C before use to remove the water in the sample.
Fig. 1

X-ray diffraction of the a ark clam shell and b calcined clam shell at 900 °C for 4 h

Figure 2 shows the FTIR of ACS and calcined ACS at 900 °C in the frequency of 280–4000 cm−1. The ACS in Fig. 2a was further confirm contain of CaCO3 phase with significant characteristic peak at ~855 (v2), ~1454 (v3), and ~708 (v4) which indicate to the carbonate group in the sample. Besides that, the small infrared absorption spectra were shown at ~1786, ~2520, and ~2874 cm−1 attributed to the combination modes of different CO3 2− band (Kamalanathan et al. 2014; Gunasekaran et al. 2006). The spectra at ~3743 cm−1 are related to the stretching vibration of the hydroxyl group and C–O stretching mode was observed at ~1082 cm−1 as CO2 adsorbed on the surface of CaO (Kamalanathan et al. 2014). All detail of these modes and references is shown in Table 2.
Fig. 2

FTIR spectrum of ark clam shell and calcined ark clam shell at 900 °C for 4 h

Table 2

FTIR vibration modes of Clam shell powder and references

Assignments

Vibrational frequencies (cm−1)

FTIR result

Gunasekaran et al. (2006)

Islam et al. (2013)

Hoque et al. (2013)

v 4—Symmetric CO3 2− deformation

708

712

706

705

v 2—Asymmetric CO3 2− deformation

855

874

857

853

Symmetric stretching vibration of CO3 2−

1082

1082

1080

v 3—Asymmetric CO3 2− deformation

1454

1425

1455

1421

v 1 + v 4—CO3 2− deformation

1786

1798

1794

2v 2 + v 4—CO3 2− deformation

2520

2514

H2O stretching mode

3743

3378

The FTIR of ACS calcined at 900 °C is shown in Fig. 2b. The calcined ACS knows as CaO show the three small frequency band that corresponding to the structure of CaO. The frequency band at ~1454 cm−1 show the CO3 2− band become small compare to the spectra of ACS due to decomposition of CO2. The peak at ~3480 and ~3742 cm−1 is related to –OH bond group present in CaO. These result is supported from the previous report which stated that at ~3640 cm−1 is related to the O–H group (Galvan-Ruiz et al. 2007). The presence of moisture allow the CaO easily absorbed it and form of Ca(OH). As the result, the CaO sample cannot keep expose to environment in long time to avoid the CaO with moisture to become Ca(OH)2 (Loy et al. 2016). Due to this reaction, the result may affects the characteristic of CaO. The different pattern of FTIR spectra of both CaCO3 and CaO shown in Fig. 2 and the detail of frequency band of both was shown in Tables 2 and 3 respectively.
Table 3

FTIR vibration modes of calcined ark clam shell powder and references

Assignments

Vibrational frequencies (cm−1)

FTIR result

Singh and Purohit (2011)

Rujitanapanich et al. (2014)

Chen et al. (2015)

v C–O

1456

1422

1416

874, 1418, 1462

v O–H

3480

3431

v O–H

3742

3642

3567

Characterization of hydroxyapatite (HA)

HA powder was analyzed by comparing with standard HA JCPDS file No. 001-084-1998 in range between 20° and 60°. The XRD pattern of HA sintered at 200–1000 °C (Fig. 3) was showed the single phase of HA only, without any secondary phase of HA decomposition. The secondary phases were consisting of another compound such as CaO, tricalcium phosphate (TCP) and tetracalcium phosphate (TTCP) (Singh 2012; Wu et al. 2013; Salma et al. 2010). Other researcher found the appearance of secondary phase due to the insufficient usage of either the calcium or phosphorous precursors (Kamalanathan et al. 2014). As precaution, the calculation of Ca:P ratio must in the range of 1.69–2.00 to obtained a single phase of HA in beginning synthesis process. From the result, the highest intensity peak detected at 2θ angle of 31.80° while the standard HA JCPDS is at 31.79° corresponding plane at (1 2 1). This highest peak indicates the HA was formed in the sample as resembled well with standard HA JCPDS file No. 001-084-1998. The peaks of intensity become more high and sharp as temperature increases from 200 to 1000 °C. These stability and purity of HA powder is very close to standard HA that used by the previous report (Venkatesan and Kim 2010). Unlike sintered HA powder at 1100 °C, HA was transform into new phase know as TCP as well as sintered at 1200 °C. The β-TCP phase was started become the dominant against HA in this stage. It is proving by comparing with standard β-TCP JCPDS file No. 000-009-0169 and presence of highest peak of β-TCP was detected at 2θ angle of 31.04°. In addition, the intensity of peaks of sintered HA was slightly decreases from at 1000 to 1200 °C.
Fig. 3

XRD patterns of sintered HA at different temperature for 4 h: a 200 °C, b 600 °C, c 800 °C, d 1000 °C, e 1100 °C and f 1200 °C

Figure 4 shows the FTIR spectra of HA in the frequency between 280 and 4000 cm−1. The IR spectrum of HA consists of four absorption bands and it show the identical pattern and changes slightly during the temperature rise from 200 to 1200 °C for 4 h for each sample. The band was corresponding to the presence of PO4 3−, CO3 2−, and OH in the sample. The frequency of ~565 cm−1 was detected corresponding to PO4 3− symmetric bending mode (v 4) while at ~1024 cm−1 was corresponding to PO4 3− asymmetric stretching mode (v 3). Both PO4 3− mode (v 3) and PO 4 −3 mode (v 4) corresponding to the vibrational groups to the structure of HA. In addition, the band positioned at ~1454 cm−1 is indicating to the CO3 2− group (v 3). Structure of OH vibrational mode was observed only at low temperature at 3744 cm−1 and totally not visible at 1100 °C. Table 4 shows the references of HA FTIR vibration modes sintered at various temperature.
Fig. 4

FTIR spectrum of sintered HA between 200 and 1200 °C for 4 h: a 200 °C, b 600 °C, c 800 °C, d 1000 °C, e 1100 °C, and f 1200 °C

Table 4

FTIR vibration modes of HA sintered at 200 °C and references

Assignments

Vibrational frequencies (cm−1)

FTIR result

Salma et al. (2010)

Singh and Purohit (2011)

Kamalanathan et al. (2014)

PO4 3− bending v 4

565

560, 599

567

568

PO4 3− stretching v 3

1024

1046

1046

1038

CO3 2− group v 3

1454

1424, 1424

1422

1421

OH structure

3744

1637, 3100–3700

3431

3425

Crystallite size and density of hydroxyapatite (HA)

The sintering temperature of HA was affect the physical of the sample. Generally, as the sintering temperature increases, the size of HA pallet and porosity will decreases due to the grains shifting to more dense packing. Table 4 showed the crystallite size, linear linkage and density at various sintering temperature of HA. From the result, it can be described that as temperature increases, the crystallite size of HA become increases (Abidi and Murtaza 2014). From the previous reports, the researchers have proved the high temperature of HA sintered show the improvement in the high peak of crystallinity (Abidi and Murtaza 2014; Bouyer et al. 2000). It is reported that samples with good crystallinity show little or no activity in the bioresorption activity, which is important for formation of chemical bonding with hard tissue area (Sanosh et al. 2009; Aoki 1994). Thus, the amorphous HA were obtained at lower temperature are expected to be more metabolically active rather than high temperature of HA which show the fully developed crystalline HA structure which otherwise insolubility in physiological environment (Sanosh et al. 2009; Kim et al. 2000).

As can be seen in the Table 5, it is expected the linear shrinkage increases as the sintering temperature increases from 200 to 1200 °C. The increasing in shrinkage of the sample was due to the eliminating of porosity or pore in the sample as sintering temperature increases (Mustafa 2005; Kamalanathan et al. 2014; Champion 2013; Ramesh et al. 2008). Besides that, the density of HA increases with increasing the sintering temperature from 2.76 to 3.12 g/cm3 at 200 to 1000 °C respectively can be confirm due to the porosity decreases and grains of HA shift to obtain more dense packing particle (Kamalanathan et al. 2014). However, at high temperature of 1000–1200 °C represent the decrement of density value from 3.12 to 2.86 g/cm3. The decreasing density value from 1000 to 1200 °C may due to partially decomposition of HA phases to TCP phases (Mustafa 2005; Kamalanathan et al. 2014; Hung et al. 2012; Mobasherpour et al. 2007; Raynaud et al. 2002).
Table 5

The crystallite size and linear shrinkage of the HA sample at various sintering temperature

Temperature (°C)

Crystallite size [D (nm)]

Linear shrinkage (%)

Density (g/cm3)

200

26.58

0

2.76

600

29.54

3.08

2.81

800

37.98

6.15

2.96

1000

53.18

11.53

3.12

1100

66.32

14.84

2.93

1200

66.34

16.69

2.86

Microstructure of hydroxyapatite (HA) FESEM and EDX

Figure 5 show the FESEM images of the sintered HA from 200 to 1200 °C under Ca:P ratio below of 2.00 and pH value of 8. Its can clearly observed the stage of evolution microstructure of sintered HA samples. The particle size is found to be increases parallel as increasing the sintering temperature of the samples. At temperature 200–800 °C, the irregular shape of particles was observed. Besides that, the microstructure of HA are mostly agglomerated in this stage. This strong agglomerated was occurring because of the presence of water molecule that could not remove from the sample by freeze drying process (Yoruc and Koca 2009). The presence of HA nanoparticle size was observed at 200 °C in between ~35 and ~69 nm in Fig. 5a. The further sintering temperature in Fig. 5b, c was show the increases of the HA particle size at 600 and 800 °C was recorded between ~0.13–0.24 and ~0.33–0.79 μm respectively. As sintering temperature increases from 1000 to 1200 °C, the morphology of HA become increases in grain size. At 1000 °C, morphology of HA start become granular in shape and irregular grain of HA was observed. Further sintering temperature at 1100 °C, the single phase of HA decomposed to a new phase as HA/β-TCP phase. The necking among particles becomes more prominent in this temperature due to high temperature sintering. The dense grain become significant at 1200 °C and it clearly observed the shape exhibited denser packing grain and the porosity is decreases due to pore removing occurs during densification. The increases of sintering temperature help the sample to improve the homogeneity and grain growth resulting in an increase in mean grain size (Mustafa 2005). In the Fig. 5d–f show the HA particle size was obviously increased parallel to the sintering temperature (1000, 1100 and 1200 °C) is between ~0.34–0.79, ~1.96–4.68, and ~1.87–6.40 μm respectively.
Fig. 5

FESEM micrograph of HA: a 200 °C, b 600 °C, c 800 °C, and d 1000 °C under 50 k magnification and e 1100 °C and f 1200 °C under 5 k magnification

EDX analysis are used for determine the element or chemical composition of the HA which is different in sintering temperature. Figure 6 represent the EDX spectra of the entire sample sintered at various temperatures from 200 to 1200 °C. From the result, the presence of element such as Ca, P, C, and O are observed and the Ca:P ratio are calculated in Table 6 to compare with the theoretical ratio which is 1.67. The element composition in the HA sample with different sintering temperature was summarized in Table 6. From the result, the Ca:P ratio of HA decreases as the sintering temperature increases. Although that, at temperature of 1000 °C, the Ca:P ratio immediately increases and it decreases back at temperature of 1100 °C. The pattern continues to decreases until the temperature at 1200 °C which is calculated the value of Ca:P ratio is 1.66. From overall result of EDX spectra, the calculated Ca:P ratio of HA decreases from 1.95 to 1.66 as HA undergo sintering process for 4 h with each sintering temperature. In detail, as the sample of HA were sinter at high temperature, there was a possibility for the HA decompose to biphasic in form of HA/TPC (Mustafa 2005; Kamalanathan et al. 2014; Hung et al. 2012; Mobasherpour et al. 2007; Raynaud et al. 2002). The presence of oxygen in EDX spectra shows the decreases in the element weight percentage from 200 to 1100 °C. However, at temperature of 1100 °C, the oxygen was started to rise in the element weight percentage of due to the present of possibility of CaO or β-TCP as another phase in the sample. From the previous research, they found the existence of CaO phase in the HA when the Ca:P ratio was high than 1.67 (Abidi and Murtaza 2014; Best et al. 2008).
Fig. 6

EDX spectra of HA at different sintering temperatures: a 200 °C, b 600 °C, c 800 °C, d 1000 °C, e 1100 °C, and f 1200 °C

Table 6

The element composition present in the HA sample with different sintering temperature

Sintering temperature (°C)

Weight of element composition (wt%)

Ca:P ratio

Ca

P

C

O

200

25.64

13.12

17.48

43.76

1.95

600

31.61

16.61

7.05

44.74

1.90

800

27.83

15.27

8.20

48.70

1.82

1000

34.45

17.35

7.27

40.92

1.98

1100

37.06

18.76

3.78

40.40

1.97

1200

30.96

18.63

3.41

47.00

1.66

Conclusion

The usability of ACS as a CaO source to produced hydroxyapatite via wet chemical precipitated method was characterize by XRD, FTIR, FESEM and EDX results. The using waste materials can cut off the cost of synthesis material since the quality and purities of the product almost same as commercial HA. In this studies, the formation of as-synthesize HA nanoparticle (~35–69 nm) through using waste precursor resources was successful done. The characterization of HA depend on various parameter such that Ca:P ratio, pH value and the temperature of initial solution. From this research, the some of the HA phase is start decompose to β-TCP phase at temperature of 1100 °C with fix pH value at 8 and the Ca:P ratio value above 1.67 but was control below 2. The microstructure and morphology of HA show the relationship of temperature. As the sintering temperature increases, HA particle was forming a dense particle and resulted in increasing density of HA. It was confirmed that the density decreases due reduced in porosity in the sample by increase the sintering temperature.

Declarations

Authors’ contributions

MZAK prepared all the sample and had done analyzed with XRD, FTIR, FESEM and EDX, prepared and drafted manuscript from the analysis result. KAM carried out the material science studies and take participated in the project. NZ and CACA carried out the chemistry and biological physic studies and participated in suggesting design and material used in this project. ZNA and NFB were provided an addition idea and helped to design in the manuscript. KAM, CACA, ZNA and MHMZ were helped in suggesting and improve the manuscript. All authors read and approved the final manuscript.

Acknowledgements

The authors gratefully acknowledge the financial support from the Malaysian Ministry of Higher Education (MOHE) and Universiti Putra Malaysia (UPM) through the Exploratory Research Grant Scheme (5527189) and Inisiatif Putra Berkumpulan (9412601) research grant.

Competing interests

All authors declare that they have no competing interests.

Open AccessThis article is distributed under the terms of the Creative Commons Attribution 4.0 International License (http://creativecommons.org/licenses/by/4.0/), which permits unrestricted use, distribution, and reproduction in any medium, provided you give appropriate credit to the original author(s) and the source, provide a link to the Creative Commons license, and indicate if changes were made.

Authors’ Affiliations

(1)
Material Synthesis and Characterization Laboratory, Institute of Advanced Technology, Universiti Putra Malaysia (UPM)
(2)
Department of Physics, Faculty of Science, Universiti Putra Malaysia (UPM)
(3)
Department of Chemistry, Faculty of Science, Universiti Putra Malaysia (UPM)

References

  1. Abidi SS, Murtaza Q (2014) Synthesis and characterization of nano-hydroxyapatite powder using wet chemical precipitation reaction. J Mater Sci Technol 30(4):307–310View ArticleGoogle Scholar
  2. Angelescu N, Ungureanu DN, Anghelina FV (2011) Synthesis and characterization of hydroxyapatite obtained in different experimental conditions. Sci Bull Valahia Univ Mater Mech 6(9):15–18Google Scholar
  3. Aoki H (1994) Medical applications of hydroxyapatite. Ishiyaku EuroAmerica Incorporated, TokyoGoogle Scholar
  4. Best SM, Porter AE, Thian ES, Huang J (2008) Bioceramics: past, present and for the future. J Eur Ceram Soc 28(7):1319–1327View ArticleGoogle Scholar
  5. Bouyer E, Gitzhofer F, Boulos MI (2000) Morphological study of hydroxyapatite nanocrystal suspension. J Mater Sci Mater Med 11(8):523–531View ArticleGoogle Scholar
  6. Champion E (2013) Sintering of calcium phosphate bioceramics. Acta Biomater 9(4):5855–5875View ArticleGoogle Scholar
  7. Chen J, Wen Z, Zhong S, Wang Z, Wu J, Zhang Q (2015) Synthesis of hydroxyapatite nanorods from abalone shells via hydrothermal solid-state conversion. Mater Des 87:445–449Google Scholar
  8. Dávila JA, Cuevas JL, Gutiérrez GV, Angeles JR, Nonell JM (2007) Chemical synthesis of bone-like carbonate hydroxyapatite from hen eggshells and its characterization. Boletín de la Sociedad Española de Cerámica y Vidrio 46(5):225–231View ArticleGoogle Scholar
  9. Dědourková T, Zelenka J, Zelenková M, Beneš L, Svoboda L (2012) Synthesis of sphere-like nanoparticles of hydroxyapatite. Proc Eng 42:1816–1821View ArticleGoogle Scholar
  10. Fathi MH, Hanifi A, Mortazavi V (2008) Preparation and bioactivity evaluation of bone-like hydroxyapatite nanopowder. J Mater Process Technol 202(1):536–542View ArticleGoogle Scholar
  11. Galvan-Ruiz M, Baños L, Rodriguez-Garcia ME (2007) Lime characterization as a food additive. Sens Instrum Food Qual 1(4):169–175View ArticleGoogle Scholar
  12. Gunasekaran S, Anbalagan G, Pandi S (2006) Raman and infrared spectra of carbonates of calcite structure. J Raman Spectrosc 37(9):892–899View ArticleGoogle Scholar
  13. Hoque ME, Shehryar M, Nurul Islam KM (2013) Processing and characterization of cockle shell calcium carbonate (CaCO3) bioceramic for potential application in bone tissue engineering. J Mater Sci Eng 2(4):132Google Scholar
  14. Hoque ME, Sakinah N, Chuan YL, Ansari MNM (2014) Synthesis and characterization of hydroxyapatite bioceramic. Int J Sci Eng Technol 3(5):458–462Google Scholar
  15. Hung I, Shih WJ, Hon MH, Wang MC (2012) The properties of sintered calcium phosphate with [Ca]/[P] = 1.50. Int J Mol Sci 13(10):13569–13586View ArticleGoogle Scholar
  16. Islam KN, Ali ME, Bakar MZ, Loqman MY, Islam A, Islam MS, Rahman MM, Ullah M (2013) A novel catalytic method for the synthesis of spherical aragonite nanoparticles from cockle shells. Powder Technol 246:434–440View ArticleGoogle Scholar
  17. Kamalanathan P, Ramesh S, Bang LT, Niakan A, Tan CY, Purbolaksono J, Chandran H, Teng WD (2014) Synthesis and sintering of hydroxyapatite derived from eggshells as a calcium precursor. Ceram Int 40(10):16349–16359View ArticleGoogle Scholar
  18. Kamba AS, Ismail M, Ibrahim TAT, Zakaria ZAB (2013) Synthesis and characterisation of calcium carbonate aragonite nanocrystals from cockle shell powder (Anadara granosa). J Nanomater 5Google Scholar
  19. Kim HM, Kim Y, Park SJ, Rey C, Lee H, Glimcher MJ, Ko JS (2000) Thin film of low-crystalline calcium phosphate apatite formed at low temperature. Biomater 21(11):1129–1134View ArticleGoogle Scholar
  20. Koutsopoulos S (2002) Synthesis and characterization of hydroxyapatite crystals: a review study on the analytical methods. J Biomed Mater Res 62(4):600–612View ArticleGoogle Scholar
  21. Loy CW, Matori KA, Lim WF, Schmid S, Zainuddin N, Wahab ZA, Zaid MHM (2016) Effects of calcination on the crystallography and non-biogenic aragonite formation of ark clam shell under ambient condition. Adv Mater Sci Eng. doi:10.1155/2016/2914368 Google Scholar
  22. Mobasherpour I, Heshajin MS, Kazemzadeh A, Zakeri M (2007) Synthesis of nanocrystalline hydroxyapatite by using precipitation method. J Alloys Compd 430(1):330–333View ArticleGoogle Scholar
  23. Mohamed M, Yusup S, Maitra S (2012) Decomposition study of calcium carbonate in cockle shell. J Eng Sci Technol 7(1):1–10Google Scholar
  24. Moore WR, Graves SE, Bain GI (2001) Synthetic bone graft substitutes. ANZ J Surg 71(6):354–361View ArticleGoogle Scholar
  25. Mustafa NY (2005) Characterization, thermal stability and sintering of hydroxyapatite powders prepared by different routes. Mater Chem Phys 94(2):333–341View ArticleGoogle Scholar
  26. Mustaffa R, Yusof M, Reusmaazran M, Abdullah Y (2015) A novelty of synthetic hydroxyapatite from cockle shell and characterization. Adv Mater Res 1087:429–433View ArticleGoogle Scholar
  27. Rajkumar M, Sundaram NM, Rajendran V (2011) Preparation of size controlled, stoichiometric and bioresorbable hydroxyapatite nanorod by varying initial pH, Ca/P ratio and sintering temperature. Digest J Nanomater Biostruct 6:169–179Google Scholar
  28. Ramesh S, Tan CY, Bhaduri SB, Teng WD, Sopyan I (2008) Densification behaviour of nanocrystalline hydroxyapatite bioceramics. J Mater Process Technol 206(1):221–230View ArticleGoogle Scholar
  29. Raya I, Mayasari E, Yahya A, Syahrul M, Latunra AI (2015) Synthesis and characterizations of calcium hydroxyapatite derived from crabs shells (Portunus pelagicus) and its potency in safeguard against to dental demineralizations. Int J Biomater. doi:10.1155/2015/469176 Google Scholar
  30. Raynaud S, Champion E, Bernache-Assollant D, Thomas P (2002) Calcium phosphate apatites with variable Ca/P atomic ratio I. Synthesis, characterisation and thermal stability of powders. Biomater 23(4):1065–1072View ArticleGoogle Scholar
  31. Rujitanapanich S, Kumpapan P, Wanjanoi P (2014) Synthesis of hydroxyapatite from oyster shell via precipitation. Energy Proc 56:112–117View ArticleGoogle Scholar
  32. Sadat-Shojai M, Khorasani MT, Dinpanah-Khoshdargi E, Jamshidi A (2013) Synthesis methods for nanosized hydroxyapatite with diverse structures. Acta Biomater 9(8):7591–7621View ArticleGoogle Scholar
  33. Salma K, Berzina-Cimdina L, Borodajenko N (2010) Calcium phosphate bioceramics prepared from wet chemically precipitated powders. Process Appl Ceram 4(1):45–51View ArticleGoogle Scholar
  34. Sanosh KP, Chu MC, Balakrishnan A, Kim TN, Cho SJ (2009) Preparation and characterization of nano-hydroxyapatite powder using sol-gel technique. Bull Mater Sci 32(5):465–470View ArticleGoogle Scholar
  35. Santhosh S, Prabu SB (2013) Thermal stability of nano hydroxyapatite synthesized from sea shells through wet chemical synthesis. Mater Lett 97:121–124View ArticleGoogle Scholar
  36. Shavandi A, Bekhit AEDA, Ali A, Sun Z (2015) Synthesis of nano-hydroxyapatite (nHA) from waste mussel shells using a rapid microwave method. Mater Chem Phys 149:607–616View ArticleGoogle Scholar
  37. Singh A (2012) Hydroxyapatite, a biomaterial: its chemical synthesis, characterization and study of biocompatibility prepared from shell of garden snail, Helix aspersa. Bull Mater Sci 35(6):1031–1038View ArticleGoogle Scholar
  38. Singh A, Purohit KM (2011) Chemical synthesis, characterization and bioactivity evaluation of hydroxyapatite prepared from garden snail (helix aspersa). J Biotechnol Biomater 1:105View ArticleGoogle Scholar
  39. Sobczak AG, Kowalski Z, Wzorek Z (2009) Preparation of hydroxyapatite from animal bones. Acta Bioeng Biomech 11(4):31–36Google Scholar
  40. Venkatesan J, Kim SK (2010) Effect of temperature on isolation and characterization of hydroxyapatite from tuna (Thunnus obesus) bone. Mater. 3(10):4761–4772View ArticleGoogle Scholar
  41. Wang Y, Lin S, Suzuki Y (2007) Study of limestone calcination with CO2 capture: decomposition behavior in a CO2 atmosphere. Energy Fuels 21(6):3317–3321View ArticleGoogle Scholar
  42. Wang P, Li C, Gong H, Jiang X, Wang H, Li K (2010) Effects of synthesis conditions on the morphology of hydroxyapatite nanoparticles produced by wet chemical process. Powder Technol 203(2):315–321View ArticleGoogle Scholar
  43. Wu SC, Hsu HC, Wu YN, Ho WF (2011) Hydroxyapatite synthesized from oyster shell powders by ball milling and heat treatment. Mater Charact 62(12):1180–1187View ArticleGoogle Scholar
  44. Wu SC, Tsou HK, Hsu HC, Hsu SK, Liou SP, Ho WF (2013) A hydrothermal synthesis of eggshell and fruit waste extract to produce nanosized hydroxyapatite. Ceram Int 39(7):8183–8188View ArticleGoogle Scholar
  45. Wu SC, Hsu HC, Hsu SK, Chang YC, Ho WF (2015) Effects of heat treatment on the synthesis of hydroxyapatite from eggshell powders. Ceram Int 41(9):10718–10724View ArticleGoogle Scholar
  46. Yoruc AB, Koca Y (2009) Double step stirring: a novel method for precipitation of nano-sized hydroxyapatite powder. Digest J Nanomater Biostruct 4:73–81Google Scholar
  47. Zhang X (2007) Preparation and characterization of calcium phosphate ceramics and composites as bone substitutes. ProQuest, San DiegoGoogle Scholar

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