Paper Menu >>
Journal Menu >>
Journal of Minerals & Materials Characterization & Engineering, Vol. 8, No. 8, pp 591-609, 2009
jmmce.org Printed in the USA. All rights reserved
Surface and Physicochemical Characterization of Phosphates
Vivianite, Fe2(PO4)3 and Hydroxyapatite, Ca5(PO4)3OH
D. Luna-Zaragoza1, E. T. Romero-Guzmán1* and L. R. Reyes-Gutiérrez2,3
1 Departamento de Química, Gerencia de Ciencias Básicas. Instituto Nacional de
Investigaciones Nucleares. Carretera México-Toluca km 36.5. C.P. 52045. A.P. 18–1027. México.
2 Centro de Investigaciones en Ciencias de la Tierra. Universidad Autónoma del Estado de
Hidalgo. Carretera Pachuca–Tulancingo Km. 4.5, Col. Carboneras. Pachuca de Soto. C.P.
42184, Hidalgo, México..
3 División de Geociencias Aplicadas. Instituto Potosino de Investigación Científica y
Tecnológica (IPICYT). Camino a la Presa San José 2055. Col. Lomas 4 sección. C.P. 78216.
San Luis Potosí S.L.P.
* Corresponding author: email@example.com
Hydroxyapatite is a calcium phosphate in the apatite group. It has numerous applications due to
its particular properties including the sorption of metallic ions. This makes it useful for the
treatment of contaminated groundwater and for soil decontamination. The least expensive
source of hydroxyapatite for synthesis is bovine bone, since this is a waste material. Vivianite is
an iron phosphate which has received little study. Like hydroxyapatite, it has particular
properties. This paper describes the method of obtaining these phosphates; calcium phosphate
from bovine bone, and iron phosphate by synthesis. Also described are the methods of purifying
the materials and characterization of these two phosphates by X-ray diffraction, infrared
analysis, thermogravimetric and differential scanning calorimetric analysis, scanning electron
microscopy, and surface area by the BET method. Physicochemical characteristics of
hydroxyapatite obtained from bovine bone are described, and preliminary results are presented
of an investigation into whether hydroxyapatite and iron phosphate are suitable as a permeable
reactive barrier for the treatment of metallic and radionuclide contaminants.
Key words: Phosphates, surface, site density, mass titration
592 D. Luna-Zaragoza, E. T. Romero-Guzmán and L. R. Reyes-Gutiérrez Vol.8, No.8
Among potential materials under investigation in the safety of underground radioactive waste
repositories, phosphate compounds are expected to play an important role because they could be
used for engineered barriers [1,2]. The management of radioactive wastes has become a major
concern, particularly in regard to the release of radioactive materials into the environment.
Migration of uranium in water-rock systems is largely controlled by uranium solution–mineral
equilibrium and sorption reactions . A large quantity of sorption data for various radionuclides
on minerals have been compiled . Zirconium, thorium and aluminium phosphates have been
studied in great detail [5–7], however little attention has been paid to the surface and sorption
properties of other metal phosphates such as those of calcium and iron II. Calcium and iron
phosphates could be considered a promising materials for this use due to their physicochemical
and surface propertiees.
One of the main characteristics of calcium phosphate compounds is their great stability and their
capacity to retain a large variety of elements, due to their particular structure which allows
substitution at different points and diffusion phenomena, in addition to the complexation reaction
with functional groups on the surface of the compound and the formation of insoluble
compounds via dissolution processes .
One of the most popular phosphates is the hydroxylapatite (HAp), with chemical formula
Ca10(PO4)6(OH)2. The common crystal phase is hexagonal , but the monoclinic phase can also
be present . HAp has many applications, such as in bone surgery, due to its biocompatibility
properties in the body ; in chromatography, to separate and purify proteins ; in solid state
ionics ; catalysis ; drug delivery systems ; fuel cells ; and chemical gas sensors
. HAp can be synthesized in the laboratory by a variety of methods including the sol-gel
process , hydrothermal synthesis , microwave synthesis , ultrasonic spray pyrolysis
; wet precipitation ; emulsion system synthesis , and sonochemical synthesis .
HAp has been found in bone and teeth. It has several impurities, mainly carbonates (5–6% of dry
weight) . Between 60 and 70% of the total weight of bone is HAp. Bovine bone is a waste
product because the bone is not used for human consumption. This material could be used as a
source of HAp.
The composition of vivianite (iron phosphate II) is Fe3(PO4)2•8H2O. It has great chemical and
thermal stability and is used in the manufacture of metallic foils, in the manufacture of knives, in
the steel and glass industry, and in the manufacture of fertilizer . The aim of this
investigation was to evaluate the chemical and surface properties of these calcium and iron
phosphates as the first stage in an investigation of their use as reactive materials to sorb metal
ions from aqueous solutions.
Vol.8, No.8 Surface and Physicochemical Characterization of Phosphates Vivianite 593
2. MATERIALS AND METHODS
2.1. Preparation of Phosphates
2.1.1. Calcium phosphate (bovine hydroxyapatite)
A bovine femur obtained from a slaughterhouse was cleaned, cut, milled, and washed with
deionized water and hydrogen peroxide in water. Fat was removed from the bone particles,
which were then were annealed at 960°C for 24 hours. An experiment was carried out in order to
determine the initial pH in deionized water, based on previous results on carbonate content in
hydroxyapatite from a vertebrate bone source . The annealed bone particles were then
centrifuged 3 minutes with deionized water and the pH of the original deionized water and the
residue from the washed bone measured. The annealed hydroxyapatite was washed with 2,000
mL of deionized water until the pH of the remaining solution was similar to the pH of the
deionized water. Lastly, the remaining material was washed with phosphoric acid at 2.3 pH. In
order to eliminate all acidic residues, the sample was washed several times with de-ionized
water. The apatite obtained was freeze-dried and meshed at 36.
2.1.2. Iron (II) phosphate
The iron (II) phosphate was prepared by the reaction:
423 SOHSONHPOFeFeSOHPONH ++→+ .
A 7.5 X 10-3M dibasic diammonium phosphate was dissolved in deionized water, and a 1.1 X 10-
2M iron sulphate aqueous solution was added while shaking slowly. A precipitate was obtained
immediately, but the full reaction time was two hours. The precipitate was then filtered in a
vacuum and washed several times with de-ionized water to eliminate remaining insoluble
material. The filtered material was then freeze-dried for 24 hours at an initial temperature of
-35°C. The main drying was carried out in a vacuum of 0.22 mBars and the final drying in a
vacuum of 0.024 mBars. After freeze-drying, the material was meshed at 36.
2.2. Physicochemical Characterization of Phosphates
2.2.1. Scanning electron microscopy (SEM)
The morphology of the iron (II) and calcium (bovine bone) phosphates was analyzed in a Phillips
XL-30 scanning electron microscope at 25kV. The samples were mounted on an aluminium
holder with carbon conductive tape, and covered with a gold layer approximately 200 Å thick
using a Denton Vacuum model Desk II sputter coater. Images were made using a backscattered
594 D. Luna-Zaragoza, E. T. Romero-Guzmán and L. R. Reyes-Gutiérrez Vol.8, No.8
electron detector. The elemental chemical composition of the samples was determined by energy
dispersion spectroscopy (EDS) with an EDAX-4 spectrometer.
2.2.2. X-ray powder diffraction (XRD)
An analysis by X-ray diffraction was performed for all samples. Samples were placed in a lucite
holder on the goniometer of a Siemens D-5000 diffractometer with a copper anode X-ray tube
(λ=1.543 Å). Kα radiation was selected with a diffracted beam monochromator at 25 KV with a
step size of 0.02° for 50 minutes to create X-ray patterns with sufficiently high intensities to
produce lines to identify the material at a 2θ angle (4°–70°). Compounds were identified by
comparing with Joint Committee on Powder Diffraction Standards (JCPDS) cards in the
2.2.3. Fourier transform infrared spectroscopy (FTIR)
Infrared analysis was also performed for the phosphate material using a Nicolette 550 IR
spectrophotometer with the KBr disc method. The samples were scanned from 4000 cm-1 to 400
cm-1. Tests including FTIR were done along with the adsorption measurements to explore the
role of hydrogen and OH- bonding in the adsorption mechanism.
2.2.4. Thermogravimetric analysis (TGA)
A small amount of the sample material was placed directly into platinum crucibles and the
analysis was carried out under N2 flow at a heating rate of 10°C min-1 at a temperature range
from room temperature to 800°C using a TGA-TDA 51 TA Instruments thermogravimetric
2.3 Surface Characterizat i o n of Iron and Calcium Phosphates
2.3.1. Specific surface areas
Specific surface areas (As, m2g-1) were determined for both phosphate compounds by the N2
Brunauer-Emmett-Teller (BET) nitrogen adsorption method in a Micromeritrics Gemini 2360
surface area analyzer. The samples were dried and degassed, and analyzed using a multipoint N2
adsorption/desorption method at room temperature.
2.3.2. Hydration kinetics
The time taken for the surface to be hydrated was determined by means of acid/base
potentiometric titrations. The potentiometric titration tests were carried out with 10 gL-1 aqueous
suspensions of solid in 0.5 M KNO3 medium, keeping ionic strength constant, since it is
Vol.8, No.8 Surface and Physicochemical Characterization of Phosphates Vivianite 595
recognized that K+ and NO3- ions do not usually sorb specifically . Distilled water and
nitrogen-controlled atmosphere were used in order to avoid the presence of carbonates. In situ
pH values were measured with a combined ORION® glass electrode. The precision of the
measured pH values was estimated to be ± 0.2 units. The sample was shaken continuously to
prevent settling. For the hydration step, the suspensions were shaken for 0, 1, 2, 3, 4, 5, 6, 7, 24,
48 and 72 hour contact times at room temperature. A kinetic study showed that 24 hours is
sufficient to reach hydration equilibrium. After hydration, the pH of the initial suspension was
adjusted to a value lower than the pHpzc (pH close to 2) using a 0.5 M HNO3 solution. The
solution was shaken for 5 min. until pH value was constant. The solid was titrated by adding
incremental volumes of a 0.1 M KOH solution.
2.3.3. Point of zero charge (PZC) determination by mass titration
Mass titration experiments were performed with 0.01, 0.05, 0.10, 0.2, 0.5, 1.0, 1.5 and 2 g of
calcium and iron (II) phosphates in polypropylene tubes with 10 mL of 0.5 M KNO3 (Fermont™)
solution. In these solutions, the solid in suspension acts a pH buffer . The resulting
suspensions were shaken for 24 hours to allow complete hydration of the solid surface before
being centrifuged at 3500 rpm for 15 minutes. The pH values of the supernatant were then
measured untill they reached a constant value (pHpzc). The pH at which the solid surface attains a
zero net charge is known as the point of zero charge or pHpzc.
2.3.4. Active site density
Surface site density (Ns) can be determined directly from the potentiometric titration curve of the
suspension (20 gL-1) . This was adjusted to an initial pH value close to 2 using a 0.5 M HNO3
solution. The solution was shaken for 5 minutes until the pH value was constant and then titrated
by adding incremental volumes of a 0.1 M KOH solution. If we plot the mole number of OH-
ions added to the suspension versus the mole number of these aqueous ions, it can be related to
the pH measurement. The final part of the resulting curve is linear. In this range, the reaction no
longer occurs and the total quantity of hydroxide ions introduced is entirely in solution. The solid
surface has reacted completely and the amphoteric sites are no longer protonated. The titration
curve obtained for the background salt alone (without phosphates) shows a linear part as well.
After extrapolation of this linear part to a zero OH- concentration for both suspensions and
background salt, we can determine OH- uptake by the solid phase by subtracting these two
values. Thus knowing the specific surface area and the quantity of powdered solid in the
suspension, we can calculate surface site density using the formula
596 D. Luna-Zaragoza, E. T. Romero-Guzmán and L. R. Reyes-Gutiérrez Vol.8, No.8
where n1 and n2 are the number of moles of OH consumed by the solid, NA is the Avogrado
Number, As is the specific area, Cs is the solid concentration and VT corresponds to the total
volume of titration solution.
3. RESULTS AND DISCUSSION
3.1. Physicochemical Characterization
3.1.1. Scanning electron microscopy
The morphology and the chemical composition of the calcium phosphate annealed at 960°C were
determined by means of SEM, considering the physical characteristics of particles in the
materials. The treatment at high temperature produces changes in the surface of particles in the
bone. These materials consist of agglomerates of rigid crystal. In addition, a significant increase
in the number of pores is observed. This is to be expected, since once the bone is annealed, this
material is between 30 and 40% organic matter, which is transformed into gases (mainly CO2)
and obviously where before there was organic matter, now there are holes as can be seen in
Figure 1. These pores seem to be connected by solid walls to form separated continuous
networks with a surface texture varying from rough to smooth. Some particles show pores
between particles (200X). Similar results were reported by Mostafa, 2005 . When
approaching 4000X (Figure 1b), the surfaces of the bone that are not seen to be porous at low
amplification show smaller pores, although these particles do not show agglomerates. The
common chemical elements of the calcium phosphate (phosphorus, calcium and oxygen) can
also be observed by EDS.
Iron (II) phosphate shows crystals with radial growth and crystalline aggregates. The size of the
crystals varies from 5 to 10 µm. The EDS chemical analysis showed that the main elements of
the sample were P, O and Fe, Figure 2.
3.1.2. X-ray diffracti on
Identification of the mineralogical components of the annealed bone was carried out by X-ray
diffraction. The main mineral found in the sample is hydroxyapatite, Ca3(PO4)5OH (JCPDS card
9-0432), according to the Joint Committee on Powder Diffraction Standard (JCPDS) , Figure
3. Each JCPDS card has the crystallographic information of the chemical composition and a
table of interplanar distances of 2θ angles against intensity. The bovine samples annealed at
960°C show highly crystalline structure and all the interplanar distances reported for this
mineral, which agrees with the hexagonal structure of the reference data. The diffractograms of
the annealed sample indicate that there were no changes in crystallinity, nor in the structural of
calcium phosphate, which indicates that the compound is still calcium phosphate. X-ray
Vol.8, No.8 Surface and Physicochemical Characterization of Phosphates Vivianite 597
diffraction analysis was carried out on the iron (II) phosphate. The diffraction standard of
vivianite was found. The diffractogram showed that the material is also highly crystalline,
consistent with JCPDS card 30-622 , Figure 3.
Figure 1. Scanning Electron Microscope (SEM) micrograph of HAp at 1000X, 4000X and
20,000X, and the respective Energy Dispersion Spectroscopy (EDS) spectrum showing a high
abundance of the principal components of calcium phosphate.
598 D. Luna-Zaragoza, E. T. Romero-Guzmán and L. R. Reyes-Gutiérrez Vol.8, No.8
Figure 2. Scanning Electron Microscope (SEM) micrograph of iron (II) phosphate at 1000X and
2500X, and the respective Energy Dispersion Spectroscopy (EDS) spectrum showing a high
abundance of the principal components of iron (II) phosphate.
Vol.8, No.8 Surface and Physicochemical Characterization of Phosphates Vivianite 599
10 20 30 40 50 60 70
Intensity, a. u.
C alcium phosphate
Iron (I I) p h os p ha te
Figure 3. X-ray diffraction (XRD) patterns that show the intensity of diffracted X-rays from
various planes as a function of 2θ value for calcium phosphate particles and iron (II) phosphate.
3.1.3. Infrared spectroscopy
Infrared spectroscopy was used to give chemical information on the compounds. The IR
spectrum for hydroxyapatite showed the characteristic bands for calcium phosphate in the
interval from 4000 cm-1 to 400 cm-1, Figure 4. The OH- bands appear at 3572 cm-1 (stretching)
and 634 cm-1 (vibration). The phosphate bands are the largest, at 1094 cm-1 and 1045 cm-1. These
appear specifically in the range of 1000 cm-1 to 1150 cm-1 (asymmetric stretching or ν3). A
defined band also appears at 962 cm-1 (symmetrical stretching or v1); from 560 cm-1 to 610 cm-1
(bending or v4) and 479 cm-1, showing v2 mode. The presence of carbonate groups is shown by
bands between 1459 cm-1 and 1413 cm-1 (asymmetric stretching or v3). These indicate the
presence of type B carbonate groups, in this case of carbonate groups replacing the phosphate
group. Type A carbonate groups could not be seen (doublet in 1451 cm-1 and 1540 cm-1), and
probably disappeared during annealing. Based on band vibration intensity, it is predicted that
concentration is low. The well-defined shape of the vibration bands at 634 cm-1, 603 cm-1 and
569 cm-1 indicates that the material is crystalline.
600 D. Luna-Zaragoza, E. T. Romero-Guzmán and L. R. Reyes-Gutiérrez Vol.8, No.8
The infrared analysis of the iron (II) phosphate clearly showed the main functional groups. The
strongest bands are the phosphates, which appear at 1050 cm-1, 979 cm-1 and 579 cm-1, Figure 4.
The OH- group produces a broad, intense band, which appeared in the spectrum. This is due to
the water groups joined to iron (II) phosphate, which appear at 3660 cm-1 (this compound is
octal-hydrated). The band that appears at 2360 cm-1 corresponds to CO2 contained in air.
4000 3500 3000 2500 2000 1500 1000500
Iron (II) phosphate
Figure 4. FTIR spectra of Iron (II) phosphate and hydroxyapatite.
3.1.4. Thermogravimetric analysis
The thermogravimetric analysis of the annealed bovine bone shows a loss of mass at
approximately 700°C, although this loss is very small (less than 2%). This is due to the fact that
at this temperature the carbonates are transformed to carbon dioxide. The small size of this loss
means that this phosphate is stable, Figure 5. This behavior was reported too by Pramanik et al.,
2007 . The thermogram for iron (II) phosphate shows that past 50°C, the compound begins
to lose weight constantly, but up to 800°C the compound not lose more weight, is stable.
Vol.8, No.8 Surface and Physicochemical Characterization of Phosphates Vivianite 601
Comparing the iron and calcium phosphate, the calcium phosphate is more stable, but even at
800°C the iron (II) phosphate is still the same compound except with several water molecules
fewer, Figure 5.
Figure 5. TGA curves of iron (II) phosphate and hydroxyapatite.
3.2. Surface Characterization
3.2.1. Surface area
During determination of surface area, the adsorption isotherm of nitrogen was also obtained for
hydroxyapatite. According to IUPAC pore size classification, there are six kinds of adsorption
isotherms. Type II isotherm in the classification of Brunauer, Deming and Teller is associated
with macroporous solids (more than 50 nm) or non-porous materials. This indicates that at
relatively low pressures, an adsorbed molecular monolayer is formed in the surface of the
material, while at relatively high pressures, multi-layer adsorption takes place. The isotherm
adsorption that is close to annealed bovine bone is very similar to type II, Figure 6. The surface
area of calcium phosphate was 3.31 m2g-1 and the pore volume was 0.0065 cm3g-1.
20120220 320 420520 620 720
602 D. Luna-Zaragoza, E. T. Romero-Guzmán and L. R. Reyes-Gutiérrez Vol.8, No.8
The specific area for the iron (II) phosphate by the BET method was 10.5 m2g-1. As can be seen
in the Figure 6, the two compounds presents a very similar behaviour but the iron (II) phosphate
sorbs more rapidly than the calcium phosphate. This is consistent with the surface area of both
compounds to sorb chemical species in solution, both are IUPAC type II.
Figure 6. Sorption isotherm of hydroxyapatite and iron (II) phosphate.
3.2.2. Hydration kinetics
The time required for the hydroxyapatite from bovine bone to reach equilibrium in solution was
determined. Several titrations were carried out at different times. Equilibrium is reached once the
curve at time t is the same for several curves, giving the final value for time. The results obtained
from the hydratation kinetics for calcium phosphate was shown in Figure 7.
00.2 0.4 0.6 0.81
Adsorbed volume, cm3/g STP
Relative pressure, P/Po
Iron (II) phosphate
Vol.8, No.8 Surface and Physicochemical Characterization of Phosphates Vivianite 603
Figure 7. Potentiometric titrations data of HAp suspensions (10 gL-1) in 0.5 M KNO3.
The curves at different times for calcium phosphate shows that this compound is hydrated at 4 h,
as the union of the majority of the curves is observed at this time. For iron (II) phosphate, it can
be seen that the union of the curves in the upper point occurs at 5 hours. For this reason it can be
considered that at this time, the hydration of the compound is completed. It therefore takes at
least 4-5 hours to hydrate both compounds, Figure 8.
0 h0.5 h1 h2 h3 h4 h
5 h6 h7 h24 h48 h72 h
604 D. Luna-Zaragoza, E. T. Romero-Guzmán and L. R. Reyes-Gutiérrez Vol.8, No.8
Figure 8. Potentiometric titrations data of iron (II) phosphate suspensions (10 gL-1) in 0.5 M
3.2.3. Point of zero charge
The point of zero charge (PZC) was determined in order to find the pH at which the solution has
been prepared to removed the heavy metal waste. The PZC for the calcium phosphate was 10.9
pH, as seen in Figure 9. In contrast, the PZC for iron (II) phosphate, at 3.3 pH, was acidic.
0h 1h 2h 3h 4h 5h 6h 24h 48h 72h
Iron (II) phosphate
Vol.8, No.8 Surface and Physicochemical Characterization of Phosphates Vivianite 605
Figure 9. Mass titration data of iron (II) phosphate and hydroxyapatite.
3.2.4. Surface sites
In order to find the surface sites of calcium phosphate, 0.5 M KNO3 was used. The results of
active surface sites were determined for the equation
The number of OH- left by the material (nOH-) is the difference between the values of the
ordinates at origin, and this was equal to 0.00125 sitesnm-2. The surface area (SA) of calcium
phosphate is 3.31 m2g-1. The concentration (c) of calcium phosphate in solution was 16.67 gL-1,
with a surface area of 3.31 m2g-1, nOH- are 4.5 sites nm-2 for the calcium phosphate surface,
We ight, g
606 D. Luna-Zaragoza, E. T. Romero-Guzmán and L. R. Reyes-Gutiérrez Vol.8, No.8
0.0008 0. 001
OH- fr ees/m ol
ha te + 0.5 M KN O
0.5 M KNO
Figure 10. Comparation of curves of titration solution of 0.5M KNO3 and 0.5M KNO3 +
The main objective of this work was the surface and physicochemical characterization of
calcium phosphate obtained from bovine bone and iron (II) phosphate. The chemical elemental
compositions determined by EDS were Ca, P and O for the hydryapatite and Fe, P and O for the
iron (II) phosphate. The minerals identified by XRD were hydroxylapatite and vivianite for the
iron (II) phosphate. The calcium phosphate is more stable than iron (II) phosphate. On the other
hand, the surface properties obtained suggests that iron (II) phosphate has the best surface
characteristics, specific area (10.5 m2g-1), sorbed volume, hydration time (5 hr) and wide range
of pH to evaluate the heavy metal sorption with this phosphate. The next step will be to evaluate
the sorption process for both compounds in metals and radionuclides.
One of the main characteristics of phosphates compounds is their great stability and their
capacity to retain a large variety of elements, due to their particular structure which allows
substitution at different points and diffusion phenomena, in addition to the complexation reaction
with functional groups in the surface of the compound and the formation of insoluble compounds
via dissolution processes.
Vol.8, No.8 Surface and Physicochemical Characterization of Phosphates Vivianite 607
We thank Rastro de Toluca for technical support, ININ Project CONACYT 36348. To Leticia
Carapia Morales and Jorge Pérez Del Prado from the Instituto Nacional de Investigaciones
Nucleares for their technical help. Finally to, Liliana Romero Guzmán for all her help.
 Ferguson, J. E., 1990, The Heavy Elements, In: Chemistry, Environmental Impact and Health
Effects, Oxford, Pergamon Press., 211–212.
 Hasan, M. A., Moore, R.C., Holt, K. C., and Hasan, A. A., 2003, “Overview on backfill
materials and permeable reactive barriers for nuclear waste disposal facilities.” Sandia National
Laboratories. New México, USA, pp. 1–27.
 Romero, G. E. T., 2000, “Migración de uranio en la zona no saturada.” Ph.D. Thesis, Toluca
México, Universidad Autónoma del Estado de México.
 Romero, G. E. T., Ordoñez, R. En., Esteller, A. M. V., Rojas, H. A., Reyes, G. L. R. and
Ordoñez, R. Ed., 2006, “Contamination of corn growing areas due to intensive fertilization in the
high plane of Mexico.” Water Air and Soil Pollution, Vol. 175, pp. 77–98.
 Drot, R., Lindecker, C., Fourest, B. and Simoni, E., 1998, “Surface characterization of
zirconium and thorium phosphate compounds.” New J. Chem., pp. 1105–1109.
 Romero, G. E. T., Esteller, A. M. V. and Ordoñez, R. E., 2002, “Uranium and phosphate
behaviour in the vadose zone of a fertilised corn field.” Journal of Radioanalytical and Nuclear
Chemistry, Vol. 254, No. 3, pp. 509–517.
 Wang, D., Qian, L., Zhang, M., Xu, J., and Wu, W., 2008, “Sorption of Eu(III) and Am(III)
on thorium phosphate diphosphate.” Journal of Nuclear and Radiochemistry, Vol. 30, No. 3,
 Perrone, J., Fourest, B., and Giffaut, E., 2002, “Surface characterization of synthetic and
mineral carbonate fluoroapatites.” J. Colloidal and Interface Science, Vol. 249, pp. 441–452.
 Badillo, A. V. and Ly, J., 2001, “Retención de especies aniónicas homólogas de dos
productos de fisión en una hidroxiapatita.” México Nuclear, Vol. 2, No. 3, pp. 83–92.
 Narasaraju, T. S. B., and Phebe, D. E., 1996, “Review, some physicochemical aspects of
hydroxyapatite.” Journal of Materials Sciences, Vol. 31, pp. 1–21.
 Coughlin, M. J., Grines, J. J. and Kennedy, M. P., 2006, “Coralline Hydroxyapatite bone
graft substitute in hind foot.” Foot Ankle Int., Vol. 27, No. 1, pp. 19–22.
 Morales, J. G., Burgues, J. J., Boix, T., Fraile, J., and Clemente, R. R. (2001). Precipitation
of stoichiometric hydroxyapatite by continuous method. Cryst. Res. Technol., 36(1), 15–26.
 Aizawa, M., Howell, F. S., Itatani, K., Yokogawa, Y., Nishizawa, K., Toriyama, M., and
Kameyama, T., 2000, “Fabrication of porous ceramic with well-controlled open porous by
sintering of fibrous hydroxyapatite.” J. Ceram. Soc. Jpn., Vol. 108, pp. 249–253.
608 D. Luna-Zaragoza, E. T. Romero-Guzmán and L. R. Reyes-Gutiérrez Vol.8, No.8
[14 ] Tanaka, H., Chikazawa, M., Kandori, K., and Ishikawa, T., 2000, “Influence of thermal
treatment on the structure of calcium hydroxyapatite.” Phys. Chem. Chem. Phys., Vol. 2, pp.
 Panda, R. N., Ming-Fa, H., Chung, R. J., and Chin, T. S., 2001, “X-ray diffractometry and
X-ray photoelectron spectroscopy investigations on nanocrystalline hydroxyapatite synthesized
by hydroxide gel technique.” Jpn. J. Appl. Phys., Vol. 40, pp. 5030–5035.
 Gross, K. A., Berndt, C. C., Stephens, P., and Innebier, R., 1998, “Oxiapatite in
hydroxyapatite coating.” J. Mater. Sci., Vol. 33, pp. 3985–3991.
 Verges, M. A., González, C. F, Martínez, G. M., Solier, J. D., Cachadina, I., and Matijevic,
E., 2000, “A new route for the synthesis of calcium deficient hydroxyapatites with low Ca/P
ratio: Both spectroscopic and electric.” J. Mater. Res., Vol. 15, pp. 2526–2533.
 Andersson, J., Areva, S., Bernd, S., and Lindén, M., 2005, “Sol-gel synthesis of
multifunctional hierachically porous silica/apatite composition.” Biomaterials, Vol. 26, No. 34,
 Wang, Y., Zhang, S., Wei, K., Zhao, N., Chen, J., and Wang, X., 2006, “Hydrothermal
synthesis of hydroxyapatite nanopowders using cationic surfactant as a template.” Material
Letters, Vol. 60, No. 12, pp. 1484–1487.
 Liu, J., Li, K., Wang, H., Zhu, M., and Yam, H., 2004, “Rapid formation of hydroxyapatite
nanostructures by microwave irradiation.” Chemical Physiscs Letters, Vol. 396, No. 4–6, pp.
 Aizawa, M., Hanazawa, T., Itatani, K., Howell, F. S., and Kishioka, A., 1999,
“Characterization of hydroxyapatite powders prepared by ultrasonic spray-pyrolysis technique.”
J. Mater. Sci., Vol. 34, pp. 2865–2873.
 Silva, C. C., Rocha, H. H., Freire, F. N. A., Santos, M. R. P., Saboia, K. A., Góes, J. C., and
Sombra, A. S. B., 2005, “Hydroxyapatite screen-printed thick films: optical and electrical
properties.” Material, Chemistry and Physics, Vol. 92, No. 1, pp. 260–268.
 Chen, C. W., Riman, R. E., Kener, S. T., and Kelly, B., 2004, “Mechanochemical-
hydrothermal synthesis of hydroxypapatite from noionic surfactant emulsions precursors.” J.
Crystal Growth., Vol. 270, No. 3–4, pp. 615–623.
 Kim, W., and Saito, F., 2001, “Sonochemical synthesis of hydroxylapatite from H3PO4
solution with Ca(OH) 2.” Ultrasonic Sonochemistry, Vol. 8, pp. 65–88.
 Danilchenko, S. N., Pokrovskiy, V. A., Bogatyrov, V. M., Sukhodub, L. F., and Sulkio-
Cleff, B., 2005, “Carbonate location in bone tissue mineral by X-ray diffraction and temperature-
programmed desorption mass spectrometry.” Cryst. Res. Technol., Vol. 40, No. 7, 692–697.
 Fontanetto, H. B., 1993, Efecto del método de aplicación del fertilizante fosfórico en maíz a
dos niveles de disponibilidad hídrica. Tesis Magister Scientiae. Facultad de Ciencias Agrarias,
Universidad Nacional de Mar del Plata, Argentina, 61.
 Dzombak, D. A., and Morel, F.M.M., 1990, “Surface Complexation Modeling, In: Hydrous
Ferric Oxide”, (J. Wiley & Sons Eds), New York.
Vol.8, No.8 Surface and Physicochemical Characterization of Phosphates Vivianite 609
 Noh, J. S., and Schwarz, J.A., 1990, “Estimation of surface ionization constant for
amphoteric solids.” Journal of Colloid and Interface Science, Vol. 139, pp. 139–148.
 Mostafa, N. Y., 2005, “Characterization, thermal stability and sintering of hydroxyapatite
powders prepared by different routes.” Materials Chemistr y and Physics, Vol. 94, pp. 333–341.
 Bayliss, P., 1986, Mineral Powder Diffraction File Date Book: Swarthmore, PA, Joint
Committee on Powder Diffraction Standards (JCPDS).
 Pramanik, S., Kumar, A. A., Rai, K.N., and Garg, A., 2007, “Development of high strength
hydroxyapatite by solid-state-sintering process.” Ceramics International, Vol. 33, pp. 419–426.