synthesis, characterization and application of ...°刷修改版 pp233-244.pdf · the present...
TRANSCRIPT
U. Rafique et al. / Journal of Water Sustainability 4 (2012) 233-244 1
* Corresponding to: [email protected]
Synthesis, Characterization and Application of Nanomaterials for
the Removal of Emerging Pollutants from Industrial Waste Water,
Kinetics and Equilibrium Model
Uzaira Rafique1*, Anum Imtiaz
1, Abida K. Khan
2
1Department of Environmental Sciences, Fatima Jinnah Women University, The Mall Rawalpindi, 46000 Pakistan. 2Institute of Information Technology, Abbottabad Campus, KPK
ABSTRACT
Nanotechnology is an emerging science offering promising models of decontamination. The present experimental
design is to synthesize novel nanoparticles of Iron and Nickel oxides to be used as catalysts for in situ removal of
different pollutants discharged from various industries. Particle size of synthesized iron and nickel oxides
nanoparticles was characteristic of ~28-36 nm and ~48-56, respectively done with help of SEM and XRD analysis.
Furthermore, the linkage of metal-oxygen linkage and red shift is confirmed through FTIR and UV-Visible
spectroscopic technique, respectively. Physico-chemical characterization of industrial effluents showed remarkably
higher concentration of nitrates and sulphates. Nitrates and sulphates were abundantly concentrated in leather
industry effluents, designating it most polluted chemical processing industry. These results directed application of
nanoparticles as adsorbents for selected removal of Nitrates and sulphates from wastewater in batch experiments.
Concentration of the pollutants like sulphates and nitrates was reduced to 18 and 54 times, respectively, lower than
the background concentration on application of Ni oxide nanoparticles. Kinetics model revealed pseudo second
order whereas Langmuir and Freundlich equilibrium gave comparable fitness to adsorption data with regression
coefficient of 0.999. The study concludes that nanotechnology provides potential and economically viable solution
for removal of wastewater pollutants through synthesis of metal nano adsorbents.
Keywords: Nanotechnology; synthesis; wastewater treatment; emerging pollutants; adsorption; isotherms and
kinetics
1. INTRODUCTION
Nanotechnology is an emerging science with
wide applications in the remediation of envi-
ronmental pollutants. In recent years, a great
deal of attention has been focused on the syn-
thesis and application of nanostructure mate-
rials as adsorbents or catalysts to remove tox-
ic and harmful substances from water and air.
Resurgence to synthesize and manipulate
nanoparticles finds use in improving air, soil
and water quality in the environment. Reac-
tive nanoparticles have a significant amount
of surfaces and thus attract much interest to be
applied as adsorbents in comparison to ma-
cromolecules. Various nanoparticles have
been applied in removing radionuclides, ad-
sorption of organic dyes, remediation of con-
taminated soils, and magnetic sensing. Metal
oxides play a significant role in many fields of
nanotechnology including nanocatalysis, sens-
ing, supermagnetic properties, nanoenergy
Journal of Water Sustainability, Volume 2, Issue 4, December 2012, 233–244
© University of Technology Sydney & Xi’an University of Architecture and Technology
Presented at the International Conference on the Challenges in Environmental Science and Engineering
(CESE-2012), Melbourne, Australia, 9–13 September 2012.
234 U. Rafique et al. / Journal of Water Sustainability 4 (2012) 233-244
storage and conversion, fuel cells, and elec-
troceramics (Bao et al., 2001; Gao et al., 2001;
Braos-Garcı´a et al., 2003; Liang et al., 2004;
Seto et al., 2005; Tian et al., 2005; Jeon et al,
2005, 2006). The compounds and nanomate-
rials of iron and nickel having low dimensions
have always been the subject of study due to
their diverse applications in the fields of elec-
tronics, catalysis, magnetics etc. (Chen et al,
2009; Dominguez- Crespo, 2009; Libor and
Zhang, 2009; Qiao et al., 2009; Masoud and
Fatemeh, 2009; Kassaee et al; 2011; Somaye
et al., 2011).
Synthesis is an important aspect of nano-
technology. An entirely new set of physical
properties and applications of nanomaterials
depends on the choice of selection procedure.
Remarkable achievements in innovative syn-
thetic routes and growth mechanisms have
been made to obtain desired size crystal, mor-
phology, microstructure and chemical compo-
sition. The sizes of nanoparticles are usually
confined to less than 100 nm and such small
sizes confer unique properties that are fre-
quently different from the properties of bulk
materials (Kannan and Sundaram, 2001;
Zhuang and Wang, 2001), making them ideal
for certain applications.
During synthesis of the nanoparticles con-
trol on nucleation and growth and agglomera-
tion stages are the important stages which
need to be controlled appropriately which is
only possible by co-precipitation method. Co-
precipitation method has been adopted to syn-
thesize the metal oxide nanoparticles as it
promise to provide not only smaller size par-
ticles as compare to solvothermal or hydro-
thermal method but also stable particles as
well. Surfactant assisted method leaves the
traces of surfactants on the surface of NPs
causes unavailability of surface to the adsor-
bents due to which the efficiency is reduced
(Bangash and Alam, 2004).
Various preparation techniques, such as
sol-gel pyrolysis method (Sun et al., 2000),
hydrothermal technique (Jing et al., 2006) and
mechanical alloying (Ponder et al., 2000) has
been used to prepare ferrite nanoparticles, but
co-precipitation method is considered to be an
economical way of producing fine particles
(Hu et al., 2004; Ko et al., 2007) .
The present study has two-fold significance.
It offers simple synthesis method for metal
and metal oxide particles and its application
for the removal of pollutants like sulphates
and nitrates from industrial wastewater. Struc-
tural properties of synthesized metal oxides
are also investigated to understand the me-
chanism. Different kinds of adsorbents have
been developed for the treatment of waste wa-
ter (Kannan and Sundaram, 2001). Metal
oxide particles enjoy a unique position having
a significant amount of surfaces, thus, attracts
much interest as potential adsorbents because
of exclusive properties and potential applica-
tion (Sun et al., 2000).
1.1 Objectives
Synthesis of nanoparticles by different me-
thods.
Application of nanoparticles for removal
of emerging pollutants from industrial ef-
fluent or waste water.
Can nanoparticles be used for the selective
removal of pollutants like sulphates and ni-
trates.
Specificity of the nanoparticle with respect
to specific pollutants.
2. MATERIALS AND METHODS
Nanoparticles were synthesized by using two
different methods in order to check which me-
thod gives best yield and particle size of the
adsorbents.
2.1 Synthesis of metal particles
(Solvothermal direct method)
The Ni-bipyridine (sample 1) and Fe-
bipyridine (sample 2) complexes were pre-
U. Rafique et al. / Journal of Water Sustainability 4 (2012) 233-244 235
pared separately by a direct reaction between
nickel chloride and iron chloride with 4,4-
bipyridine following solvothermal method.
Nickel chloride (0.1 mol) and 4,4-bipyridine
(0.1 mol) were dissolved in 2-propanol (100
ml) separately. Then 4, 4- bipyridine solution
was added drop wise to the metal salt solution.
All chemicals were mixed with vigorous stir-
ring, using a magnetic stir bar and refluxed at
80 0C for 10 hours and then cooled to room
temperature. When the reaction was complete,
greenish precipitates were collected and
washed with dry ether of analytical grade sev-
eral times to remove impurity. The final prod-
uct was dried under vacuum at 60 0C over-
night.Sample (b) was also synthesized in the
same way with white precipitates. The
grinded samples were then placed in argon
fitted carbolite furnace for sintering. The
samples were calcined under inert atmosphere,
and then final product was dried.
2.2 Synthesis of metal oxide particles
(Co-precipitation method)
Particles of Iron and Nickel were synthesized
using co-precipitation method (Patricia et al.,
1999; Chakrabarty et al., 2009). The proce-
dure layout is as follows:
Acidic solution of 4.0mL of FeCl3 and 1.0
mL of FeCl2 (1:2 molar ratio, respectively)
was thoroughly stirred for 10-15min followed
by addition of 1.0M NaOH solution till the
appearance of black precipitate. Strong mag-
net was used to settle the particles at the base
of beaker and supernatant was discarded. Par-
ticles were kept in desiccators. Percentage
yield was calculated to be 80%.
Nickel oxide particles were synthesized by
drop wise addition of aqueous solution of
NaHCO3 (1.5 gm in 10 mL water) to the con-
tinuously stirring aqueous solution of NiCl2
(2.3 gm in 10 mL distilled water). The preci-
pitates obtained were centrifuged, washed re-
peatedly with distilled water and dried in oven
at 100°C. Percentage yield of synthesized Ni
particles is calculated to be 63%.
2.3 Characterization of adsorbents
The synthesized metal oxides particles were
characterized with the help of FTIR (FTIR
8400, Shimadzu), UV-Visible (UV-1601
Shimadzu) spectrophotometer, SEM (JSM-
6490A JEOL) and XRD (Model, Theta-Theta).
2.4 Batch adsorption
Time-dependent batch experiment was con-
ducted for the study of adsorption of sulphates
and nitrates and other compound using the
synthesized materials. The following general
procedure was used for a batch experiment.
The synthetic solution of sulphate and ni-
trate with known concentration (10 mg/L, 20
mg/L) was prepared at neutral pH. A known
volume (10 mL) each was pipette into the se-
ries of cultural vial to which 1mg of the syn-
thesized materials as adsorbent was added.
Upon completion of the given contact time (in
minutes) between adsorbent and adsorbate,
the solution was filtered. The filtrate was de-
termined with the help of UV spectrophoto-
meter for metal nitrate and sulphate concen-
tration. The standard Turbid-metric (4500-
SO4) and Ultraviolet spectrophotometric
screening (4500-NO3) methods are used for
the sulphates and nitrates analysis (APHA,
2005). Each batch experiment was repeated
with varying pH and induced concentration of
metal salt solution.
2.5 Kinetics studies
In order to study the kinetics of the adsorption
process, first order, pseudo first order, pseudo
second order and intra particle diffusion equa-
tions were applied. The conformity between
experimental data and the model predicted
values is expressed by the correlation coeffi-
236 U. Rafique et al. / Journal of Water Sustainability 4 (2012) 233-244
cient (R2, values close or equal to 1). A rela-
tively high R2 value indicates that the model
successfully describes the adsorption kinetics
(Fadali et al., 2005).
2.6 Adsorption isotherms
Adsorption equilibrium models of Langmuir
(Langmuir, 1918) and Freundlich (Kalavathy
et al., 2005) were applied to determine the
relationship of sulphate and nitrate adsorption
with different induced concentration. The best
fitting isotherm was evaluated by linear re-
gression, and the parameters (Lalhruaitluanga
et al., 2010) obtained from the intercept and
slope of the linear plots of these models.
3. RESULTS AND DISCUSSION
3.1 Characterization of adsorbents
The synthesized metal oxide particles were
run on FTIR (FTIR 8400, Shimadzu) and UV-
Visible (UV-1601 Shimadzu) spectrophoto-
meter for characterization. FTIR spectrum of
Fe3O4 is represents two absorption bands at
around 592 and 630 cm-1
which is due to the
presence of Fe-O bond of Fe3O4 (Figure 1).
Peaks at 2962 cm-1
attributed to different C-H
band vibrations, peaks appeared at 1261.49
cm-1
is due to C-O stretching showing the ab-
sorption of atmospheric water and CO2. FTIR
of NiO shows the band in 700 to 800 cm-1
range assigned to Ni-O stretching vibrations
mode the broadness of band indicates that
NiO powders are nanoparticles (Korosec et al.,
2003) as shown in the Figure 1.
The broad absorption band centered at 3440
cm−1
is attributable to the band O–H stret-
ching vibrations and the weak band near 1635
cm−1
is assigned to H–O–H bending vibra-
tions mode. The jagged absorption bands in
the region of 1000–1500 cm−1
are assigned to
the O-C=O symmetric and asymmetric stret-
ching vibrations and the C–O stretching vi-
bration, but the intensity of the band has wea-
kened, which indicated that the ultrafine pow-
ers tend to strong physically absorption to
H2O and CO2 (Qiao et al., 2009). FTIR spec-
trum of composite showed both the Fe-O and
Ni-O bands.
Figure 1 FTIR spectrum of Iron oxide Particles
U. Rafique et al. / Journal of Water Sustainability 4 (2012) 233-244 237
UV-VIS indicates blue shift in the bands
which may be due to the presence of small
sized nanoparticles, moreover according to
Mie theory that absorbance increases in nano-
particles (Somaye et al, 2011). Metal clusters
also show cluster size effects in optical spec-
tra (Pinchuk et al, 2008).
A Scanning Electron Microscope (SEM)
image of catalysts was characterized using
Hitachi SEM SU-1500. The surface morphol-
ogy and geometry of the metal nanoparticles
studied by SEM and the result are presented
here for Ni and Fe particles (Figure 2) The
SEM image depicts the uniformity of the
Nickel NPs with size range 150- 250 nm. The
SEM image of Fe iron particle at low resolu-
tion reveals the dispersion of Fe-particle with
relatively less uniformity and low size range
150-200nm as well.
The typical SEM images of iron oxide and
nickel oxide particles (Figure 3) show the non
spherical shape. From the image it is seen that
a large number of particles are present and if
we consider single one then calculated aver-
age size is to be nearly equal 36 and 48nm for
iron and nickel respectively.
However the SEM results (Figure 3a and
3b) showed the particles synthesized by
adopting co-precipitation method show quite
smaller size less than 100 nm (20-39.6 nm for
Fe and 32-56.57 nm for Ni) as compared the
metal particles synthesized by solvothermal
method (Figure 2). Co-precipitation method is
typical used and most preferred method for
the synthesis of spherical smaller size NPs
with high degree of uniformity.
The details XRD patterns of the NiO nano-
particles are shown in Figure 4. All the reflec-
tion peaks with relative intensities of different
planes, indexed in the figure, specify the pres-
ence of NiO. The well crystalline nature of
the prepared sample is easily being observed
with the sharpness and the intensity of the
peaks.
The XRD results (Figure 5) of the iron
oxide nanoparticles indicated all the samples
were in face centered cubic phase and in spin-
al structure according to the standard JCPDF
file (card no-25-1402).
(a) (b)
Figure 2 SEM image of (a) Ni Particles and (b) Fe Particles
238 U. Rafique et al. / Journal of Water Sustainability 4 (2012) 233-244
(a) (b)
Figure 3 SEM image of (a) Iron oxide particles and (b) Nickel oxide particles
Figure 4 X-ray diffraction pattern of Nickel oxide Particles
U. Rafique et al. / Journal of Water Sustainability 4 (2012) 233-244 239
20 30 40 50 60 70
0
20
40
60
80
100
120
Inte
nsi
ty (
a.u
)
2 Theta (Degree)
(311)
(220)
(111)
(400)
(422)
(511)
(440)
Figure 5 X-ray diffraction pattern of Iron oxide Particles
3.2 Batch adsorption
The present study is designed to devise a de-
contamination model for the removal of ni-
trates and sulfates using synthesized materials.
For this purpose synthetic batch experiments
were designed separately for each material at
optimum operating conditions described
elsewhere (Imtiaz and Rafique, 2011). Series
of Batch experiments were conducted. The
variables used were (a) adsorbate concentra-
tion of 10 mg/L and 20 mg/L; (b) adsorbent
mass of 1 mg; (c) pH 7 (neutral). However,
the optimum concentration of the adsorbate
was found to be 10 mg/L from adsorption ex-
periments showing optimum removal of sul-
phates and nitrates.
All the plots throughout the manuscript are
constructed on the data at optimum operating
parameters of the experiment. It is concluded
from the experiments that lower concentration
of 10 mg/L of the adsorbate, 1mg of the ad-
sorbent dosage and the neutral pH are the op-
timum conditions for this study (Figure 6
showed the optimum concentration of adsor-
bate).
The results graphically presented in Figure
7 depict the efficiency of particles of nickel
and Iron oxides for the removal of aqueous
pollutants. Nitrates are removed to an opti-
mum percentage of 58% and 67% on iron
oxide and nickel oxide particles, respectively.
The results are comparable to reported in lite-
rature (Li et al., 2008; Kasaee et al., 2011).
The sulfates removal was also attempted
which shows a relatively lower percentage of
removal efficiency. It is interesting to note
that efficiency of both particles in removing
sulfates is comparable in contrast to response
for nitrates. However, on cumulative basis, it
can be deduced from the results that nickel
oxide particles are better candidate for the
removal of both inorganic pollutants.
3.3 Kinetic studies
Different kinetic models including first or-
der, pseudo first order, and pseudo second
order and intra particle diffusion equations
were applied to determine the mechanism in-
volved in adsorption process.
240 U. Rafique et al. / Journal of Water Sustainability 4 (2012) 233-244
(a) (b)
Figure 6 Removal (in %) of (a) Nitrates and (b) Sulfates by Fe and Ni Metal oxide particles at
optimum concentration (10 mg/L) of adsorbate
(a) (b)
Figure 7 Removal (in %) of (a) Nitrates and (b) Sulfates by different Metal Particles
The sorption kinetics may be described by
a simple first order equation (Khan et al,
2007).
0ClogtCtlog + 2.303
k =
1
The sorption kinetics may also be described
by a pseudo first order equation (Ozacar,
2003). The integral form of the model is
tk
qqq ee303.2
loglog 1
The adsorption kinetics may also be de-
scribed by a pseudo second-order equation
(Ho et al, 2001) the differential equation of
this model is as follows:
tqqkq eet
111
22
The intra-particle diffusion model is ex-
pressed as (Ayres et al., 1994)
taloglogklogR id
U. Rafique et al. / Journal of Water Sustainability 4 (2012) 233-244 241
3.4 Adsorption isotherm model
Adsorption models of Langmuir and Freun-
dlich were applied to determine the relation-
ship of nitrates and sulfates adsorption with
different induced concentration. The best-
fitting isotherm was evaluated by linear re-
gression, and the parameters obtained from
the intercept and slope of the linear plots of
these models.
Estimation of maximum adsorption capaci-
ty corresponding to complete monolayer cov-
erage on the nanomaterials was calculated us-
ing the Langmuir isotherm model since the
saturated monolayer isotherm can be ex-
plained by the non-linear equation of Lang-
muir Equation:
max
e
maxe
e
q
C
Lq
1
q
C+
K=
Freundlich isotherm is capable of describ-
ing the adsorption of organic and inorganic
compounds on a wide variety of adsorbents
(Kalavathy et al., 2005). The Freundlich eq-
uation is expressed as:
Clogn
1Klogqlog eFe +=
The adsorption Isotherms and Kinetics is
applied on the present study using Nickel and
Iron particles as adsorbents for the removal of
nitrates and sulphates. The data is
summarized in Table 1. The higher R2 values
reveals that isotherms of Freundlich and
Langmuir are in best agreement (R2
= 0.999
for Nitrates and R2 > 0.96 for Sulphates). The
fitness of both Isotherms is also reported by
(Hosik et al., 2009) for the adsorption of As
(V) onto maghemite nanoparticles. Kinetic
studies also stated that it follows the Pseudo
second order which is supported by (Ho and
Chiang, 2001; Wu et al., 2001; Hossain et al.,
2005).
Table 1 Calculation of Parameters of Nitrates and Sulfates using Fe and Ni Particles
Adsorption
Isotherms
Metal
Particles Nitrates Sulfates
Langmuir NN
KL qm R2 KL qm R
2
0.2315 -0.2715 0.9995 2.3807 -15.046 0.9999
FN 0.3433 -0.7184 0.9994 4.3786 -30.831 0.9666
Freundlich
KF n R2 KF n R
2
NN 1.0963 -0.5212 0.9999 3.8038 -3.8786 1
1.2921 -0.8479 0.9999 5.2062 -5.4411 0.9916
Kinetic Models
1st Order NN
Co K1 R2 Co K1 R
2
0.5559 -0.0044 0.8888 0.9033 -0.0004 0.8602
FN 0.6897 -0.0083 0.7092 0.953 -0.004 0.8962
Pseudo 1st Order NN
K1 qe cal. R2 K1 qe cal. R
2
-2E-07 4.8267 0.8957 -1E-07 4.3222 0.8597
FN -7E-07 4.7626 0.7102 -2E-06x 4.3404 0.8913
Pseudo 2nd
Order NN
K2 qe cal. R2 K2 qe cal. R
2
0.0095 0.1483 0.9998 0.0514 0.4733 0.9999
FN 0.0192 0.1705 0.9993 0.909 0.4081 0.9647
Intra-particle
Diffusion NN
α Kid R2 α Kid R
2
0.0084 1.8149 0.6281 0.0096 1.3075 0.663
FN 0.0305 1.7308 0.7103 0.1392 1.1257 0.6823
242 U. Rafique et al. / Journal of Water Sustainability 4 (2012) 233-244
CONCLUSIONS
The following conclusions are drawn from the
present study:
The synthesis procedure adopted offer sim-
ple, economical and efficient method for
the preparation of Fe and Ni oxide particles
of reduced size, percentage yield being 80
and 65, respectively.
Co-precipitation method is better than sol-
vothermal method for the synthesis of the
spherical smaller size particle with high de-
gree of uniformity.
Nitrates and Sulfates are efficiently re-
moved by Nickel oxide and iron oxide nano
particles at optimum operating conditions
of pH 7, induced concentration 10 mg/L
and adsorbent mass of 1mg.
Nickel oxide NPs are proved to be better
candidate than Fe-oxide NPs.
FUTURE PROSPECTS
Formation of thin membrane of the nickel
oxide NPs which can be used in filters to
capture inorganic pollutants like nitrates
and sulphates from water.
Ni-oxide nanoparticles can be used in small
sachets or in form of pellets to remove the
toxic pollutants efficiently at low level from
water.
Recyclable/regeneratabe thin films on neu-
tral or active support can be formed for fil-
ters
Ni-oxide nanoparticles can be dispersed ho-
mogeneously on the nano-support to get better
efficiency.
REFERENCES
APHA (2005). Standard methods for the ex-
amination of water and wastewater. 21st
edition. American Public Health Associa-
tion, Washington, DC.
Ayres, D.M., Davis, A.P. and Gietka, P.M.
(1994). Removing heavy metals from
wastewater. Engineering Research Centre
Report, 1- 21.
Bangash, F.K. and Alam, S. (2004). Extent of
Pollutants in the Effluents of Hayatabad
Industrial Estate Peshawar. Journal of
Chemical Society of Pakistan, 26(3), 271-
278.
Bao, J.C., Tie, C.Y., Xu, Z., Zhou, Q.F., Shen,
D. and Ma, Q. (2001). Template Synthesis
of an Array of Nickel Nanotubules and Its
Magnetic Behavior. Advanced Materials,
13(21), 1631–1633.
Braos-Garcı´a, P., Maireles-Torres, P.,
Rodr’ıguez-Castello n, E. and Jime nez-
Lo pez, A.J. (2003). Gas-phase hydroge-
nation of acetonitrile on zirconium-doped
mesoporous silica-supported nickel cata-
lysts. Journal of Molecular Catalysis A:
Chemical, 193, 185–196.
Chakrabarty, S. and Chatterjee, K. (2009).
Synthesis and Characterization of Nano-
Dimensional Nickelous Oxide (NiO) Sem-
iconductor. Journal of Physical Science, 13,
245-250.
Dominguez-Crespo, M.A., Ramı´rezMene-
sesa, E., Montiel-Palmab, V., Torres Huer-
taa, A.M. and Dorantes Rosalesc, H.
(2009). Synthesis and electrochemical cha-
racterization of stabilized nickel nanopar-
ticles. International journal of hydrogen
energy, 34, 1664–1676.
Fadali, O.A., Ebrahiem, E.E., Magdy, Y.H.,
Daifullah, A.A.M. and Nassar, M.M.
(2005). Removal of Chromium from Tan-
nery Effluents by Adsorption. Journal of
Environmental Science and Health, Part A:
Toxic/Hazardous Substances and Envi-
ronmental Engineering, 39(2), 465-472.
Gao, J.Z., Guan, F., Zhao, Y.C., Yang, W.,
Ma, Y.J., Lu, X.Q., Hou, J.G. and Kang,
J.W. (2001). Preparation of Ultrafine
Nickel Powder and its Catalytic Dehydro-
U. Rafique et al. / Journal of Water Sustainability 4 (2012) 233-244 243
genation Activity. Materials Chemistry
and Physics, 71, 215-219.
Ho, Y.S. and Chiang, C.C. (2001). Sorption
Studies of Acid Dye by Mixed Sorbents.
Adsorption, 7, 139-147.
Hosik, P., Nosang, V.M., Haeryong, J. and
Heechul, C. (2009). As(V) remediation us-
ing electrochemically synthesized maghe-
mite nanoparticles. Journal of Nanopar-
ticles Research, 11, 1981–1989.
Hossain, M.A., Kumita, M., Michigami, Y.,
and Mori, S. (2005). Kinetics of Cr(VI)
Adsorption on Used Black Tea Leaves.
Journal of Chemical Engineering Japan,
38(6), 402-406.
Hu, J. Lo, I.M. and Chen, G. (2004). Removal
of Cr (VI) by magnetite nanoparticles. Wa-
ter Science Technology, 50 (12), 139–146.
Imtiaz, A. and Rafique, U. (2011). Synthesis
of Metal Oxides and its Application as Ad-
sorbent for the Treatment of Wastewater
Effluents. International Journal of Chemi-
cal and Environmental Engineering, 2(6),
399-405.
Jeon, Y.T., Lee, G.H., Park, J., Kim, B. and
Chang, Y. (2005). Magnetic Properties of
Monodisperse NiHx Nanoparticles and
Comparison to those of Monodisperse Ni
Nanoparticles. The Journal of Physical
Chemistry B, 109, 12257–12260.
Jeon, Y.T., Moon, J.Y., Lee, G.H., Park, J.
and Chang, Y. (2006). Comparison of the
magnetic properties of metastable hex-
agonal close-packed Ni nanoparticles with
those of the stable face-centered cubic Ni
nanoparticles. The Journal of Physical
Chemistry B, 110, 1187–1191.
Jing, H. Guohua, C. and Irene, M. (2006). Se-
lective Removal of Heavy Metals from In-
dustrial Wastewater Using Maghemite Na-
noparticle: Performance and Mechanisms.
Journal of Environmental Engineering,
132 (7), 7 pages.
Kalavathy, M.H., Karthikeyan, T., Rajgopal S.
and Miranda, L.R. (2005). Kinetic and iso-
therm studies of Cu (II) adsorption onto
H3PO4-activated rubber wood sawdust.
Journal of Colloid Interface Science, 292
(2), 354–362.
Kannan, N. and Sundaram, M. (2001). Kinet-
ics and mechanism of removal of methy-
lene blue by adsorption on various car-
bons-A comparative study. Dyes and Pig-
ments, 51, 25–40.
Kassaee, M.Z., Motamedi, E., Mikhak, E. and
Rahnemaie, R. (2011). Nitrate removal
from water using iron nanoparticles pro-
duced by arc discharge vs. reduction.
Chemical Engineering Journal, 166(2),
490-495.
Khan, N.A. and Mohamad, H. (2007). Inves-
tigation on the Removal of Chromium (VI)
from Waste-water by Sugarcane Bagasse.
Water and Wastewater Asia, 37-41.
Ko, C.H., Park, J.G., Park, J.C., Song, H.,
Han, S.S. and Kim J.N. (2007). Surface
status and size influences of nickel nano-
particles on sulfur compound adsorption.
Applied Surface Science, 253 (13), 5864-
5867.
Korosec, C., Bukovec, R., Pihlar, P. and Sur-
ca, B. (2003). Preparation and structural
investigations of electrochromic nanosized
NiOx films made via the sol-gel route. Sol-
id State Ionics, 165, 191-200.
Lalhruaitluanga, H., Jayaram, K., Prasad,
M.N.V. and Kumar, K.K. (2010). Lead (II)
adsorption from aqueous solutions by raw
and activated charcoals of Melocanna bac-
cifera Roxburgh (bamboo)-A comparative
study. Journal of Hazardous Materials,
175 (1-3), 311-318.
Langmuir, I. (1918). The Adsorption of Gases
on Plane Surfaces of Glass, Mica and Pla-
tinum. Journal of American Chemical So-
ciety, 40, 1361-1403.
Li, T., Sun, L., Guo, A., Wang, S., Yi, A., Xiu,
Z. and Jin, Z. (2008). Reduction of Nitrate
in Groundwater with Modified Iron Nano-
particles. The 2nd International Confe-
244 U. Rafique et al. / Journal of Water Sustainability 4 (2012) 233-244
rence on Bioinformatics and Biomedical
Engineering, 16-18 May 2008, Shanghai.
Liang, Z.H., Zhu, Y.J. and Hu, X.L. (2004).
β-nickel hydroxide nanosheets and their
thermal decomposition to nickel oxide na-
nosheets. Journal of Physical Chemistry B,
108(11), 3488–3491.
Libor, Z. and Zhang, Q. (2009). The synthesis
of nickel nanoparticles with controlled
morphology and SiO2/Ni core-shell struc-
tures. Materials Chemistry and Physics,
114, 902–907.
Masoud, S.N. and Fatemeh, D. (2009). Syn-
thesis of copper and copper(I) oxide nano-
particles by thermal decomposition of a
new precursor. Materials Letters, 63 (3-4),
441–443.
Özacar, M. (2003). Equilibrium and Kinetic
Modeling of Adsorption of Phosphorus on
Calcined Alunite. Adsorption, 9(2), 125-
132.
Patricia, B., Nicholas, B.A., Katie, J.B., Dean,
J.C., Arthur, B.E. and George, C.L. (1999).
Preparation and Properties of an Aqueous
Ferro fluid. Journal of Chemical Education,
76(7), 943.
Pinchuk A.O. and Schatz G.C. (2008). Nano-
particle optical properties: Far- and near-
field electrodynamic coupling in a chain of
silver spherical nanoparticles. Materials
Science and Engineering B, 149, 251–258.
Ponder, S.M., Darab, J.G. and Mallouk, T.E.
(2000). Remediation of Cr(VI) and Pb(II)
aqueous solutions using supported, nanos-
cale zero-valent iron. Environmental
Science and Technology, 34(12), 2564–
2569.
Qiao, H., Wei, Z., Yang, H., Zhu, L. and Yan,
X. (2009). Preparation and Characteriza-
tion of NiO Nanoparticles by Anodic Arc
Plasma Method. Journal of Nanomaterial,
Volume 2009, Article ID 795928, 5 pages.
Seto, T., Akinaga, H., Takano, F., Koga, K.,
Orii, T. and Hirasawa, M. (2005). Magnet-
ic properties of monodispersed Ni/NiO
core-shell nanoparticles. Journal of Physi-
cal Chemistry B, 109(28), 13403–13405.
Somaye, B., Hossein, A., Hossein, Z. and
Morteza, S. (2011). Size Measurement of
Metal and Semiconductor Nanoparticles
via UV-Vis Absorption Spectra. Digest
Journal of Nanomaterials and Biostruc-
tures, 6(2), 709-716.
Sun, S., Murray, C.B., Weller, D., Folks, L.
and Moser, A. (2000). Monodisperse FePt
nanoparticles and ferromagnetic FePt na-
nocrystal superlattices. Science, 287(5460),
1989–1992.
Tian, F., Zhu, J., Wei, D. and Shen, Y.T.
(2005). Magnetic field assisting DC elec-
trodeposition: general methods for high-
performance Ni nanowire array fabrication.
Journal of Physical Chemistry B, 109(31),
14852–14854.
Wu, F.C., Tseng, R.L. and Juang, R.S. (2001).
Kinetics of Color Removal by Adsorption
from Water Using Activated Clay. Envi-
ronmental Technology, 22(6), 721-729.
Yong, C., Liew, K.Y. and Li, J. (2009). Size
controlled synthesis of Co nanoparticles by
combination of organic solvent and surfac-
tant. Applied Surface Science, 255, 4039–
4044.
Yu, Y., Zhuang, Y.Y. and Wang, Z.H. (2001).
Adsorption of water-soluble dye onto func-
tionalized resin. Journal of Colloid and In-
terface Science, 242(2), 288–293.
Zhang, Y.X., Fu, W.J. and An, X.Q. (2008).
Preparation of nickel nanoparticles in
emulsion. Transactions of Nonferrous
Metals Society of China, 18(1), 212–216.