enhanced chitosan beads-supported fe0-nanoparticles for removal of heavy metals from electroplating...
TRANSCRIPT
ww.sciencedirect.com
wat e r r e s e a r c h x x x ( 2 0 1 3 ) 1e1 0
Available online at w
journal homepage: www.elsevier .com/locate/watres
Enhanced chitosan beads-supportedFe0-nanoparticles for removal of heavy metals fromelectroplating wastewater in permeable reactivebarriers
Tingyi Liu a, Xi Yang a, Zhong-Liang Wang a,b,*, Xiaoxing Yan b
a Tianjin Key Laboratory of Water Resources and Environment, Tianjin Normal University, Tianjin 300387, PR Chinab College of Urban and Environment Science, Tianjin Normal University, Tianjin 300387, PR China
a r t i c l e i n f o
Article history:
Received 20 December 2012
Received in revised form
21 August 2013
Accepted 1 September 2013
Available online xxx
Keywords:
Nanoscale zero-valent iron (NZVI)
Permeable reactive barriers (PRBs)
Ethylene glycol diglycidyl
ether (EGDE)
Heavy metals
Electroplating wastewater
* Corresponding author. Tianjin Key LaboratChina. Tel./fax: þ86 22 23766256.
E-mail addresses: [email protected]
Please cite this article in press as: Liu, Tmetals from electroplating wastewaterj.watres.2013.09.006
0043-1354/$ e see front matter ª 2013 Elsevhttp://dx.doi.org/10.1016/j.watres.2013.09.006
a b s t r a c t
The removal of heavy metals from electroplating wastewater is a matter of paramount
importance due to their high toxicity causing major environmental pollution problems.
Nanoscale zero-valent iron (NZVI) became more effective to remove heavy metals from
electroplating wastewater when enhanced chitosan (CS) beads were introduced as a sup-
port material in permeable reactive barriers (PRBs). The removal rate of Cr (VI) decreased
with an increase of pH and initial Cr (VI) concentration. However, the removal rates of Cu
(II), Cd (II) and Pb (II) increased with an increase of pH while decreased with an increase of
their initial concentrations. The initial concentrations of heavy metals showed an effect on
their removal sequence. Scanning electron microscope images showed that CS-NZVI beads
enhanced by ethylene glycol diglycidyl ether (EGDE) had a loose and porous surface with a
nucleus-shell structure. The pore size of the nucleus ranged from 19.2 to 138.6 mm with an
average aperture size of around 58.6 mm. The shell showed a tube structure and electro-
plating wastewaters may reach NZVI through these tubes. X-ray photoelectron spectro-
scope (XPS) demonstrated that the reduction of Cr (VI) to Cr (III) was complete in less than
2 h. Cu (II) and Pb (II) were removed via predominant reduction and auxiliary adsorption.
However, main adsorption and auxiliary reduction worked for the removal of Cd (II). The
removal rate of total Cr, Cu (II), Cd (II) and Pb (II) from actual electroplating wastewater was
89.4%, 98.9%, 94.9% and 99.4%, respectively. The findings revealed that EGDE-CS-NZVI-
beads PRBs had the capacity to remediate actual electroplating wastewater and may
become an effective and promising technology for in situ remediation of heavy metals.
ª 2013 Elsevier Ltd. All rights reserved.
1. Introduction persistent, bioaccumulative and harmful substances (US EPA,
Electroplating wastewater contains many kinds of heavy
metals, such as Cr, Pb, Cu, Cd, and etc., which are considered
ory of Water Resources
kleg.cn, [email protected]
., et al., Enhanced chitoin permeable reactive
ier Ltd. All rights reserved
1998; Algarra et al., 2005). Due to the serious threat to human
health and ecological systems, these contaminants must be
and Environment, Tianjin Normal University, Tianjin 300387, PR
, [email protected] (Z.-L. Wang).
san beads-supported Fe0-nanoparticles for removal of heavybarriers, Water Research (2013), http://dx.doi.org/10.1016/
.
wat e r r e s e a r c h x x x ( 2 0 1 3 ) 1e1 02
removed from wastewaters before discharge to the environ-
ment (Panayotova et al., 2007).
Various remediation technologies have been developed for
the removal of the metals from wastewaters (Fu and Wang,
2011). One of the most promising and effective remediation
technologies is the use of permeable reactive barriers (PRBs)
filled with reactive material(s) for the treatment of contami-
nated groundwater (Thiruvenkatachari et al., 2008). Owing to
low production costs and high efficiency for removal of a wide
range of contaminants, zero-valent iron (ZVI) is usually used
as a reactivematerial in engineered PRBs in the form ofmicro-
scale powders and/or macro scale filings/granules (Choi et al.,
2007; Farrell et al., 2000; Scott et al., 2011).
Because of its extremely small particle size, large surface
area, and high reactivity, nanoscale zero-valent iron (NZVI) has
been introduced into wastewaters treatment to remove heavy
metals with a much higher efficiency than normal iron pow-
ders (Cao and Zhang, 2006; Geng et al., 2009; Kanel et al., 2006).
NZVI was applied to remediate wastewaters with a higher
removal efficiency in PRBs. However, few studies used NZVI as
the reactivemedia in PRBs.Oneof the reasonsmaybe thatNZVI
particles are not easily contained in PRBs due to their extremely
small particle size (Joo et al., 2004; Thiruvenkatachari et al.,
2008). To overcome these problems, it may be advisable to
support NZVI particles on macro-scale and stable composite
beads without reducing their reactivity. More recently, NZVI
has been supported by chitosan (CS) beads to prepare com-
posite beads with a mean diameter of 3.1 mm (Liu et al., 2010,
2012).Most studies have focused onNZVI synthesis (Zhan et al.,
2009), modification (Johnson et al., 2009), and the transport and
fate of NZVI in porous media (Phenrat et al., 2009), thus infor-
mation has been lacking on using CS-NZVI composite beads
with a good mechanical strength in PRBs.
NZVI has shown high efficiency to remove only one or two
kinds of heavy metals in wastewater (Kanel et al., 2006; Liu
et al., 2009; Manning et al., 2007; Ponder et al., 2000). Howev-
er, the interactions between metal ions affected the removal
efficiency when several heavy metals co-existed in the
wastewaters (McKenzie, 1980; Shama et al., 2010).
The goal of the research is to prepare a new and stable
system, chitosan/Fe0-nanoparticles beads, as the reactive
materials in permeable reactive barriers, for the remediation
of electroplating wastewater, containing four heavy metals
(Cr, Cu, Cd and Pb). Themain objectives were to: (1) synthesize
and characterize the new and stable CS-NZVI beads; (2) eval-
uate the removal efficiency of the co-existing heavy metals by
enhanced chitosan/Fe0-nanoparticles beads PRBs under
different experimental conditions and (3) investigate the
elemental composition and their valence variation during
remediation process to reasonably conclude the removal
mechanism of co-existing heavy metals in the chitosan/Fe0-
nanoparticles beads PRBs.
2. Materials and methods
2.1. Materials and chemicals
Cellulose powder (20 mm) and chitosan flakes (75% deacety-
lated) were purchased from Sigma Co. NZVI particles with a
Please cite this article in press as: Liu, T., et al., Enhanced chitometals from electroplating wastewater in permeable reactivej.watres.2013.09.006
mean diameter of 45.2 nm were purchased from Nanjing
Emperor Nano Material Co., Ltd. Ethylene glycol diglycidyl
ether (EGDE), K2Cr2O7, CuCl2, CdCl2 and PbCl2 were provided
by First Chemical Reagent Manufactory (Tianjin, China). All
other chemicals were of analytical grade purity.
2.2. Preparation of EGDE-CS-NZVI beads
CS-NZVI beads were prepared according to the procedures
described in detail elsewhere (Li and Bai, 2005; Liu et al., 2010).
Briefly, chitosan flake (2.0 g) was dissolved in 100mL 1.0% (v/v)
acetic acid solution at 60 �C and 220 revolutions per min (rpm)
for 5 h. Then, a 1.0 g amount of cellulose powerwas added into
the chitosan solution and the mixing was continued for
another 5 h at 30 �C and 220 rpm. As the chitosan-cellulose
solution was cooled down to 20 �C, a 1.0 g amount of NZVI
was gently added into the solution. Then, the mixture was
promptly dropped into a 2 mol/L NaOH solution to form
chitosan-cellulose-NZVI beads. The beads were allowed to
stand in the deoxygenated NaOH solution for 24 h for hard-
ening and then washed with deionized water. The CS-NZVI
beads were stored in deionized water for further use.
The beads in stock were put into a beaker with 100 mL
deionizedwater, adjusting pH to 12 by adding 0.1mol/L NaOH.
Then, a 0.8 g of EGDE solution was introduced into the beaker.
After continuous agitation at 60 �C for 4 h in a thermostatic
water bath, the mixture was cooled down to room tempera-
ture, and the EGDE-CS-NZVI beads were washed extensively
with deionized water to remove any residual cellulose and
EGDE. These beads were stored in deionized water for further
use. The beads prepared in this way had an average of
3.0 � 0.04 mm and the water content of the studied material
was 89.5% in wet. The whole process was carried out in a ni-
trogen atmosphere.
2.3. PRBs experimental set-up and procedure
A laboratory-scale PRBs system was designed using a plex-
iglass columnwith 50 cm length and 15mm internal diameter.
The columnwas filledwith the prepared EGDE-CS-NZVI beads
as the reactive media and the length of the filler was about
35.6 cm. A 3 cmheight of quartz sand (about 0.5mmdiameter)
was used to fix the fillers on the top and the bottom, respec-
tively. Electroplating wastewater was continuously pumped
into the reactive material column with a downflow mode by
peristaltic pump at a flow rate of 60 mL/h. Every 10 min, 1 mL
sample was withdrawn using disposable syringes and filtered
through a 0.42 mm micro-hole filter. Only one column was
constructed due to logistical constraints, meaning that a total
of PRBs experimental runs were conducted on the column.
Each treatment was replicated three times, with the column
completely emptied and repacked between each experiment.
After removing themedia, the columnwas soaked in 0.1mol/L
HCl for 24 h and then washed with deionized water 3 times.
2.4. Effects of different experimental conditions on theremoval efficiency of heavy metals
The pH of the solutions was one of themost important factors
in removing heavy metals. The pH was adjusted to 2.88, 4.09,
san beads-supported Fe0-nanoparticles for removal of heavybarriers, Water Research (2013), http://dx.doi.org/10.1016/
wat e r r e s e a r c h x x x ( 2 0 1 3 ) 1e1 0 3
5.12, 6.06, 7.02, 8.06 and 9.20 by adding 0.1 mol/L HCl and
NaOH, respectively.
In addition, the concentration of heavy metals was also
varied at four concentrations. The highest concentration of Cr
(VI), Cu (II), Cd (II) and Pb (II) was 100, 100, 75 and 50 mg/L,
respectively. These concentrations are extremely high
compared with the maximum concentrations allowed in
groundwater by the National Quality Standard for Ground-
water in China (GB/T 14848-93) (GAQSIQ, 1993), which permit
0.1mg/L for Cr (VI), 1.5mg/L for Cu (II), 0.01mg/L for Cd (II) and
0.1 mg/L for Pb (II). However, the main goal of the test was to
evaluate the performance of EGDE-CS-NZVI beads PRBs under
extreme contaminated conditions.
2.5. Removal capacity of heavy metals by EGDE-CS-NZVI beads PRBs
Removal capacity of heavy metals was conducted and the
concentration of Cr (VI), Cu (II), Cd (II) and Pb (II) in simulated
electroplating wastewater was 20, 20, 15 and 10 mg/L,
respectively. The wastewater was continuously pumped into
the reactive material column with a downflow mode for 10 h.
Samples were withdrawn using disposable syringes at certain
time intervals.
The Thomas model is used to predict the column break-
through capacities. The expression of the Thomas model for
an adsorption column is as follows (Fu and Viraraghavan,
2003; Vijayaraghavan et al., 2005):
Cout
Cin¼ 1
1þ exp�kTHQ
�qeqX� CinVout
�� (1)
where Cout and Cin represent the concentration of the effluent
and influent, respectively. kTH is the Thomas rate constant
(mL/min mg), qeq is the maximum solid-phase concentration
of the solute (mg/g), Vout is the effluent volume (mL), X is the
mass of adsorbent (g), and Q is the flow rate (mL/min).
The linearized form of the Thomasmodel is as equation (2)
(Kavak and Ozturk, 2004):
ln
�Cin
Cout� 1
�¼ kTHqeqX
Q� kCinVout
Q(2)
The kinetic coefficient kTH and the adsorption capacity of
the bed qeq can be determined from a plot of ln[(Cin/Cout) �1]
against t at a given condition.
2.6. EGDE-CS-NZVI beads characterization andanalytical methods
The concentration of each heavy metal was measured using
inductively coupled air-acetylene flame atomic emission
spectrometry (AAF-AES) (WFX-130, BJR Co.). The EGDE-CS-
NZVI beads were dried by a vacuum freeze drier (BYK FD-
1A-50, China) at �52 �C for 5 h. Morphological analysis of the
beads was then performed using a scanning electron micro-
scope (SEM) with energy-dispersive X-ray (EDS) detection
(SEM/EDS, FEI Nova NanoSEM 230). The X-ray photoelectron
spectroscope (XPS, PHI 5000 Versa Probe) analysis was
employed to investigate the elemental composition of the
EGDE-CS-NZVI beads before and after heavymetals reduction.
Please cite this article in press as: Liu, T., et al., Enhanced chitometals from electroplating wastewater in permeable reactivej.watres.2013.09.006
The typical wide scan XPS spectra for final products were also
investigated.
2.7. Application of EGDE-CS-NZVI beads PRBs to removeheavy metals from electroplating wastewater
To explore the feasibility of the removal of heavy metal ions
from wastewater, EGDE-CS-NZVI beads PRBs was used to
remediate actual electroplating wastewater collected from an
electroplate factory’s sewage outfall (Tianjin, China). The
wastewater was not treated by any means before being
introduced into the EGDE-CS-NZVI-beads PRBs.
3. Results and discussion
3.1. Mechanical property of EGDE-CS-NZVI beads
Mechanical strength of EGDE-CS-NZVI beads was determined
following a previously reported method (Guo et al., 2004). The
deformation ratio is only 2% when the stirring speed reached
800 rpm. In comparisonwith other studies (Guo et al., 2004; Liu
et al., 2012), the conclusion can be reasonably generalized that
crumpling ratios are significantly reduced after cross-linking
reaction, which indicates that the mechanical strength of
EGDE-CS-NZVI beads is enhanced. Thus, it is likely that the
new and stable EGDE-CS-NZVI beads will be suitable as the
reactive materials in PRBs.
3.2. Removal capacity of heavy metals by EGDE-CS-NZVI beads PRBs
The results of the removal capacity of heavymetals are shown
in Fig. 1. Within the reaction time of 6 h, the heavy metals Cr
(VI), Cu (II), Cd (II) and Pb (II) can be efficiently removed and all
of the removal rates are higher than 96%. Then, the removal
rates generally decreasedwith increasing reaction time, as the
redox reaction between heavy metals and NZVI was a chem-
ically controlled and irreversible process (Shi et al., 2011). It
also can be seen that there is a steep decrease in the removal
rate of Cr (VI) after 6 h (Fig. 1). The pH gradually increased
during the reaction process (Table 1), resulting in a decrease in
Cr (VI) removal rate (Boddu et al., 2003). Similar phenomena
have been observed in other NZVI systems (Liu et al., 2010).
However, a significant decrease in the removal rate of Cu (II),
Cd (II) and Pb (II) was not observed after 6 h because of the
removal rate of Cu (II), Cd (II) and Pb (II) increasing with an
increase of pH (Lai and Chen, 2001).
As the column saturation/uptake capacity was not
observed in this study, a Thomas model is used to predict the
column breakthrough capacities (at Ce/C0 ¼ 1), described in
detail in other studies (Reynolds and Richards, 1996). Ac-
cording to Thomas model, the removal capacity at the
breakthrough point is 44.8, 67.2, 82.6 and 55.8 mg/g for Cr, Cu,
Cd and Pb, respectively. The removal capacities obtained in
our study are much higher than the results using commercial
iron filings or NZVI particles (Genc-Fuhrman et al., 2008;
Ponder et al., 2000). It is mainly attributed to the fact that
the EGDE-CS-NZVI beads may form the surface films in the
PRBs, which in turn causes higher diffusion and adsorption
san beads-supported Fe0-nanoparticles for removal of heavybarriers, Water Research (2013), http://dx.doi.org/10.1016/
0 2 4 6 8 100.0
0.2
0.4
0.6
0.8
1.0 Cr Cu Cd Pb
Cou
t/Cin
Time (h)
Fig. 1 e Removal capacity of heavy metals by EGDE-CS-
NZVI beads PRBs. Initial concentration: 20 mg/L Cr (VI),
20 mg/L Cu (II), 15 mg/L Cd (II), and 10 mg/L Pb (II); the
concentration of NZVI in CS-NZVI: 10.0 g/L; pH: 6.4;
temperature: 20 �C. Cout and Cin represented the
concentration of the effluent and influent, respectively.
Error bars represent the standard deviation of the
measurements.
4 6 8 100.00
0.05
0.10
Cou
t/Cin
Cr Cu Cd Pb
wat e r r e s e a r c h x x x ( 2 0 1 3 ) 1e1 04
than batch experiments (Lai and Chen, 2001). The biofilm has
an influence on the transport of stabilized NZVI (Lerner et al.,
2012). Due to microbial degradation, ZVI integrated
sequencing batch reactor (SBR) resulted in the increased
organic removal efficiency compared to the control (Lee et al.,
2010). NZVI stimulatedmethanogenic activity while inhibiting
biological dechlorination in a mixed culture containing Deha-
lococcoides spp (Kirschling et al., 2010; Xiu et al., 2010).
The results indicated that EGDE-CS-NZVI beads PRB were
effective to remove various heavy metals and a potential
promising candidate for applications to in situ environmental
remediation.
3.3. Effect of pH
A change of pH can influence the reaction rate of iron oxida-
tion and corrosion (Alowitz and Scherer, 2002) and heavy
metals can be removed through oxidation or/and complexa-
tion with the oxide and hydroxides of iron (Melitas et al., 2001;
Shokes and Moller, 1999). The dominant forms of heavy
metals in aqueous solution were also affected by pH (Mohan
and Pittman, 2006). Thus pH of electroplating wastewater
played an important role in removing of heavy metals.
The effect of pH on heavy metals removal was conducted
and the result is shown in Fig. 2. It is obvious that the removal
Table 1e The change of the solution pH during the courseof adsorption. Initial concentration of Cr (VI): 20 mg/L, Cu(II): 20 mg/L, Cd (II): 15 mg/L, and Pb (II): 10 mg/L; NZVI:10.0 g/L; pH: 2.88; temperature: 20 �C.
Time (min) 0 10 20 30 40 50 60
pH 2.88 3.84 4.92 5.12 5.58 6.18 6.62
Please cite this article in press as: Liu, T., et al., Enhanced chitometals from electroplating wastewater in permeable reactivej.watres.2013.09.006
rates of all heavy metals are higher than 91.8% (Fig. 2), which
suggests that EGDE-CS-NZVI beads as a reactivemedia in PRBs
is highly efficient to remove heavy metals from aqueous so-
lutions. It is further noted that with an increase of pH, removal
rate of Cr (VI) decreased but the removal rates of Cu (II), Cd (II)
and Pb (II) increased. HCrO4- predominates at pH between 1.0
and 6.0, and CrO42� pH above about 6.0 (Mohan and Pittman,
2006). At lower pH the beads were positively charged due to
the protonation of amino groups, while Cr (VI) existed mostly
as an anion leading to the electrostatic attraction between Cr
(VI) and the beads (Boddu et al., 2003). Furthermore, the lower
pH could prevent the formation of Fe(III)eCr(III) precipitate.
Thus Cr (VI) removal rate decreasedwith an increase in pH. On
the other hand, with increased hydroxyl groups, the number
of negatively charged sites was improved, leading to the
enhanced attraction force between heavy metals (Cu (II), Cd
(II) and Pb (II)) and these beads surface. Therefore, the removal
amount of Cu (II), Cd (II) and Pb (II) was increased. The trend is
consistent with the reported results by other researchers who
investigated the adsorption of heavy metals on the iron-
coated sand, CS-NZVI beads and a composite chitosan bio-
sorbent (Boddu et al., 2003; Lai and Chen, 2001; Liu et al., 2010).
The change of the solution pH during the reaction was also
recorded and the result is shown in Table 1 (Initial concen-
tration of Cr (VI): 20 mg/L, Cu (II): 20 mg/L, Cd (II): 15 mg/L, and
Pb (II): 10 mg/L; NZVI: 1.0 g/L; pH: 2.88; temperature: 20 �C). Itcan be seen fromTable 1 that the solution pH is increasedwith
increasing reaction time. The oxidation of iron and dissolution
of Fe(III)eCr(III) precipitate consumed Hþ in the solution,
which led to the increase of pH (Alowitz and Scherer, 2002).
However, the removal of Cu (II), Cd (II) and Pb (II) also
consumedhydroxyl groups. As a result, the final pH value near
neutrality was 6.62. This is consistent with the results as
observed in Fig. 2.
pH value
Fig. 2 e Effect of pH value on the removal of heavy metals
by EGDE-CS-NZVI beads PRBs. Initial concentration: 20 mg/
L Cr (VI), 20 mg/L Cu (II), 15 mg/L Cd (II), and 10 mg/L Pb (II);
the concentration of NZVI in CS-NZVI: 10.0 g/L; pH: 6.4;
temperature: 20 �C. Cout and Cin represented the
concentration of the effluent and influent, respectively.
Error bars represent the standard deviation of the
measurements.
san beads-supported Fe0-nanoparticles for removal of heavybarriers, Water Research (2013), http://dx.doi.org/10.1016/
wat e r r e s e a r c h x x x ( 2 0 1 3 ) 1e1 0 5
3.4. Effect of initial concentrations of heavy metals
Heavy metals pollution incidents have occurred repeatedly in
recent years (Arao et al., 2010). The concentrations of heavy
metals in the incidents were extremely high compared with
the maximum concentrations allowed in groundwater. Then,
studying on the effect of initial concentrations of heavy
metals on the removal efficiency is very important to the ap-
plications of EGDE-CS-NZVI beads PRBs. Thus, the effect of
initial concentrations of heavy metals was estimated and the
result is shown in Fig. 3. It can be observed that the removal
rate of Cr (VI), Cu (II), Cd (II), and Pb (II) decreases with an in-
crease of the initial Cr (VI) concentration. With a fixed adsor-
bent dose, the total available adsorption sites are limited thus
leading to a decrease in removal rate of adsorbate corre-
sponding to an increased initial adsorbate concentration
(Hiemstra and Van-Riemsdijk, 1999).
At the lower concentration (less than 40 mg/L), heavy
metals are removed in the order Cd (II) > Cu (II) > Pb (II) > Cr
(VI) (Inset of Fig. 3 (a) and (b)). As the concentration increases,
the removal order is changed into Pb (II) > Cu (II) > Cd (II) > Cr
(VI) (Fig. 3 (c) and (d)). Iron has greater affinity with Pb (II) than
Cu (II) in the process of adsorption/oxidation (Lai and Chen,
2001). The similar phenomenon had been reported where
heavy metals were adsorbed in the order Pb (II) > Cu (II) > Zn
(II) > Cd (II) by hematite (Schwertman and Taylor, 1989). Using
0 1 2 30.0
0.2
0.4
0.6
0.8
1.0
Cou
t/Cin
Time (h)
(a)
0.0 0.5 1.0 1.5 2.0 2.5 3.00.0
0.2
0.4
0.6
0.8
1.0 (c)
Cou
t/Cin
Time (h)
Cr (Cin=60mg/L) Cu (Cin=60mg/L) Cd (Cin=45mg/L) Pb (Cin=30mg/L)
Fig. 3 e Effect of concentrations of heavy metals on the remova
concentration of Cr (VI): 20 mg/L, Cu (II): 20 mg/L, Cd (II): 15 mg
experimental time from 0.5 to 3 h), (b) initial concentration of C
20 mg/L (Inset: expanded chart of (b) at the experimental time fr
(II): 60 mg/L, Cd (II): 45 mg/L, and Pb (II): 30 mg/L, and (d) initial
75 mg/L, and Pb (II): 50 mg/L. Cout and Cin represented the concen
represent the standard deviation of the measurements.
Please cite this article in press as: Liu, T., et al., Enhanced chitometals from electroplating wastewater in permeable reactivej.watres.2013.09.006
Eichhornia crassipes, heavy metals were removed in the
order: Pb (II) > Zn (II) > Cd (II) > Cu (II) (Shama et al., 2010). The
solution pH is increased as the reaction proceeds, leading to a
decrease in Cr (VI) removal (Table 1). However, previous re-
searchers also found that the order was Cu (II) > Pb (II) > Zn
(II) > Cd (II) using goethite (McKenzie, 1980).
3.5. SEM characterization
Themorphology of EGDE-CS-NZVI beads is presented in Fig. 4.
It can be seen from Fig. 4(a) that the surface of these spherical
beads is loose and porous. The particular structure is favor-
able for mass transfer and energy flow between wastewaters
and the EGDE-CS-NZVI beads. There is a nucleus-shell struc-
ture inside of these beads in Fig. 4(b). The pore size of the
nucleus ranges from 19.2 to 138.6 mmwith an average aperture
size of around 58.6 mm. According to the previous results
(Wan-Ngah and Fatinathan, 2008), the nucleus of the beads is
macroporous and the pore sizes in EGDE-CS-NZVI beads are
heterogeneous. Other studies pointed out that the uniform
reaction between NaOH and acetic acid throughout the beads
led to the unique structure inside of the beads (Liu et al., 2010,
2012). The shell shows a tube structure linking the wastewater
with NZVI in the beads (Fig. 4(c)) and wastewaters can be
introduced into the beads through these tubes. It can be found
in Fig. 4(d) that NZVI particles are uniformly distributed in the
0 1 2 30.0
0.2
0.4
0.6
0.8
1.0
Cou
t/Cin
Time (h)
(b)
(d)
0.0 0.5 1.0 1.5 2.0 2.5 3.00.0
0.2
0.4
0.6
0.8
1.0
Cou
t/Cin
Time (h)
Cr(Cin=100mg/L) Cu(Cin=100mg/L) Cd(Cin=75mg/L) Pb(Cin=50mg/L)
l of heavy metals by EGDE-CS-NZVI beads PRBs: (a) initial
/L, and Pb (II): 10 mg/L (Inset: expanded chart of (a) at the
r (VI): 40 mg/L, Cu (II): 40 mg/L, Cd (II): 30 mg/L, and Pb (II):
om 0.5 to 3 h), (c) initial concentration of Cr (VI): 60 mg/L, Cu
concentration of Cr (VI): 100 mg/L, Cu (II): 100 mg/L, Cd (II):
tration of the effluent and influent, respectively. Error bars
san beads-supported Fe0-nanoparticles for removal of heavybarriers, Water Research (2013), http://dx.doi.org/10.1016/
Fig. 4 e Themorphology of EGDE-CS-NZVI beads was analyzed: (a) SEM image of the surface of EGDE-CS-NZVI beads, (b) SEM
image of the cross-section of EGDE-CS-NZVI beads, (c) higher magnification of SEM image of the edge of the cross-section, (d)
the distribution of NZVI particles in the EGDE-CS-NZVI beads.
25000
(b)
wat e r r e s e a r c h x x x ( 2 0 1 3 ) 1e1 06
EGDE-CS-NZVI beads. It indicates that NZVI supported in
EGDE-CS beads can prevent the particles from aggregation.
Similar phenomena are also found in other NZVI systems,
such as kaolinite-supported NZVI, ECH-CS-NZVI beads (Liu
et al., 2012; Uzum et al., 2009).
0
5000
10000
15000
20000
1400 1200 1000 800 600 400 200 0
C/S
Binding Energy (eV)
(a)
Cu
CCr
CdPb
Fe
O
Fig. 5 e Typical wide scan XPS spectra for the EGDE-CS-
NZVI beads before and after heavy metals reduction: (a)
before heavy metals reduction and (b) after heavy metals
reduction. Initial concentration: 60 mg/L Cr (VI), 60 mg/L Cu
(II), 45 mg/L Cd (II), and 30 mg/L Pb (II); the concentration of
NZVI in CS-NZVI: 10.0 g/L; pH: 6.4; temperature: 20 �C.
3.6. XPS characterization
The results of XPS characterization were shown in Fig. 5 and
Fig. 6. It is clear that new peaks at the binding energy (BE) of
944 eV, 580 eV, 406 eV and 139 eV appeared after heavymetals
reduction. The presence of the bands were assigned to the
photoelectron peak of Cu, Cr, Cd and Pb, respectively, which
indicated the uptake of Cu, Cr, Cd and Pb on the surface of
EGDE-CS-NZVI beads.
Detailed XPS surveys on the region of Fe2p3/2, Cr2p3/2,
Cu2p3/2, Cd3d5/2 and Pb4f7/2 are presented in Fig. 6. Photo-
electron peaks at 711.8 and 725.0 eV (Fig. 6 (a)) correspond to
the binding energies of 2p3/2 of oxidized iron [Fe (III)]. The peak
at 706.5 eV assigned to Fe0 (Chatterjee et al., 2009) was not
observed in this study. It indicates that extensive oxidation of
iron occurs on the surface of NZVI and little Fe0 remains. The
photoelectron peak for Cr2p3/2 centers at 577.2 and 587.6 eV
(Fig. 6(b)) which have binding energies and line structures
similar to those of Cr (III) (Wan-Ngah et al., 2008). The XPS
Please cite this article in press as: Liu, T., et al., Enhanced chitosan beads-supported Fe0-nanoparticles for removal of heavymetals from electroplating wastewater in permeable reactive barriers, Water Research (2013), http://dx.doi.org/10.1016/j.watres.2013.09.006
1900
2000
2100
2200
2300
2400
2500
2600
727 723 719 715 711 707 703
C/S
Binding Energy (eV)
Fe2p3/2
Fe(III)
(a)Fe(III)
1350
1400
1450
1500
1550
1600
1650
1700
589 585 581 577 573 569
C/S
Binding Energy (eV)
Cr2p3/2
Cr(III)
(b)
Cr(III)
2600
2800
3000
3200
3400
957 953 949 945 941 937 933 929
C/S
Binding Energy (eV)
Cu2p3/2
Cu(II)
(c) Cu(0)
700
750
800
850
900
950
1000
419 415 411 407 403 399C
/S
Binding Energy (eV)
Cd3d5/2
Cd(0)
(d)
Cd(II)
450
470
490
510
530
550
570
590
150 146 142 138 134 130 126
C/S
Binding Energy (eV)
Pb4f7/2(e)
Pb(II)
Pb(0)
Fig. 6 e High-resolution XPS survey of (a) Fe2p3/2, (b) Cr2p3/2, (c) Cu2p3/2, (d) Cd3d5/2 and (e) Pb4f7/2 of EGDE-CS-NZVI-beads
PRBs after reacting with electroplating wastewater for 2 h. Initial concentration of Cr (VI): 100 mg/L, Cu (II): 100 mg/L, Cd (II):
75 mg/L, and Pb (II): 50 mg/L; the concentration of NZVI in CS-NZVI: 10.0 g/L; pH: 6.4; temperature: 20 �C.
wat e r r e s e a r c h x x x ( 2 0 1 3 ) 1e1 0 7
results implied that the reduction of Cr (VI) to Cr (III) was
complete in less than 2 h.
The new peaks at a BE of 932.4 eV and 952.2 eV can be
attributed to the spin-orbit doublet of the Cu2p core level
transition (Mekki et al., 1997), which are assigned to Cu (0) and
Cu (II) (Fig. 6 (c)), respectively (Li and Bai, 2005). The main peak
was known as characteristics of Cu (0) (Fig. 6 (c)). Hence, it was
reasonably proposed that Cu (II) was removed predominantly
by reduction and the formation of Fe(III)eCu(II) co-
precipitated in this study. According to the previous study,
at pH > 6, Cu (II) species presenting in the solution were
mainly Cu(OH)þ and Cu(OH)2 (Nuhoglu and Oguz, 2003). At
pH < 5.7, Cu (II) removal by NZVI conformed to a chemically
reductive model, whilst at higher pH (>5.7) removal mecha-
nism of Cu (II) was neither by a reductive or adsorptive model
(Scott et al., 2011). Lai and Chen (2001) reported that Cu was
Please cite this article in press as: Liu, T., et al., Enhanced chitometals from electroplating wastewater in permeable reactivej.watres.2013.09.006
chemisorbed onto iron-coated sand. However, it is also re-
ported that the Cu adsorption on the iron-containing adsor-
bents was attributed to the formation of strong bonds
between Cu (II) and the iron (hydr)oxides (Qian et al., 2009).
Similarly, the Cd3d5/2 survey (Fig. 6(d)) presents a photo-
electron peak centering at 404.8 and 411.6 eV, which come
from Cd (II) and Cd (0), respectively (Li and Zhang, 2007). It is
also observed that the peak at 404.8 eV is stronger than that at
411.6 eV, which means that Cd (II) are mainly adsorbed on the
EGDE-CS-NZVI beads surface and a small portion of Cd (II) is
reduced to Cd (0). Fe(III)eCr(III) hydroxide can be used as an
efficient adsorbent material for Cd(II) removal from waste-
waters (Namasivayam and Ranganathan, 1995). In fact, the
presence of both cationic and anionic species, such as CrO42�,
CuClþ, CdClþ and PbðNO3Þþ, caused Cd (II) removal via pre-
cipitation of their minerals/salts (Genc-Fuhrman et al., 2008).
san beads-supported Fe0-nanoparticles for removal of heavybarriers, Water Research (2013), http://dx.doi.org/10.1016/
0
0.02
0.04
0.06
0.08
0.1
0.12
Cou
t/Cin
Cr Cu Cd Pb
Fig. 7 e Application of EGDE-CS-NZVI beads PRBs to
remove heavy metals from actual electroplating
wastewater. The concentration of NZVI in CS-NZVI: 10.0 g/
L; pH: 4.56; temperature: 20 �C. Cout and Cin represented the
concentration of the effluent and influent, respectively.
Error bars represent the standard deviation of the
measurements.
wat e r r e s e a r c h x x x ( 2 0 1 3 ) 1e1 08
In the study, both sorption and reduction are in effect for the
removal of Cd (II). Shokes and Moller (1999) proposed that
cadmium was rapidly reduced and plated onto the iron sur-
face, which is consist with the result reported by other re-
searchers (Wilkin and McNeil, 2003). However, some
researchers reported that Cd (II) was adsorbed on NZVI sur-
face by electrostatic interaction and specific surface bonding
(Li and Zhang, 2007).
As shown in Fig. 6(e), the Pb4f7/2 has two peaks at 136.0 eV
and 138.4 eV, which can be contributed to Pb (0) and Pb (II)
(Ponder et al., 2000), respectively. That is, both metillic Pb (0)
and Pb (II) are present on the surface of EGDE-CS-NZVI beads.
Themain peak is known as characteristic of Pb (0). Hence, it is
reasonably proposed that both adsorption and predominant
reduction are in effect for the removal of Pb (II), conforming
the observation of previous studies (Lai and Chen, 2001;
Ponder et al., 2000).
3.7. Application of EGDE-CS-NZVI beads PRBs for heavymetals removal from actual electroplating wastewater
Before the remediation of actual electroplating wastewater,
the pH, dissolved oxygen (DO) and chemical oxygen demands
(COD) were 4.56, 4.37 mg/L and 1500 mg/L, respectively. The
concentrations of total Cr, Cu (II), Cd (II) and Pb (II) in actual
electroplating wastewater were 62.6, 55.8, 32.4 and 22.8 mg/L,
respectively (Table 2). After treatment by EGDE-CS-NZVI-
beads PRBs for 4 h, the pH, DO and COD was 7.56, 1.37 mg/L
and 32.4 mg/L, respectively. The pH of actual electroplating
wastewater increased, which is consistent with the result of
Table 1. The obviously reduction of COD means that the
degradable organic matter can be also removed by EGDE-CS-
NZVI-beads PRBs, which was confirmed by other researchers
using NZVI (Giasuddin et al., 2007; Zhang et al., 2011). The
removal rate of total Cr, Cu (II), Cd (II) and Pb (II) is 89.4%,
98.9%, 94.9% and 99.4%, respectively (Fig. 7), which is consis-
tent with the results shown in Fig. 3. The result revealed that
EGDE-CS-NZVI-beads PRBs had the capacity to remediate
actual electroplating wastewater and could become an effec-
tive and promising technology for remediation of heavy
metals.
However, microbial degradation may play an important
role in the in situ remediation of heavy metals. Some re-
searchers reported that a chlorophenol-degrading microor-
ganism entrapped in carrageenan-chitosan gels showed a
higher bioactivity than free microorganism (Wang and Qian,
1999). Chitosan hydrogel beads could serve as a carrier to
delivermacromolecules to the colon (Zhang et al., 2002). In situ
remediation combining ZVI and biodegradation has been
proposed for the treatment of mixed organic plumes (e.g.,
chlorinated solvents and petroleum hydrocarbons) (Ma and
Zhang, 2008). More attention should be paid to the effect of
Table 2e The concentration of each heavymetal in actualelectroplating wastewater.
Wastewater Total Cr Cu(II) Cd(II) Pb(II)
Concentration (mg/L) 62.6 55.8 32.4 22.8
Please cite this article in press as: Liu, T., et al., Enhanced chitometals from electroplating wastewater in permeable reactivej.watres.2013.09.006
microbial degradation on the removal of heavy metals by
EGDE-CS-NZVI beads in future study.
4. Conclusions
In this study, NZVI particles is more effective to remove heavy
metals from electroplating wastewater when enhanced chi-
tosan beads were introduced as a support material in PRBs.
Based on the results, the major finding are summarized as
follows:
1) Due to enhanced mechanical strength, the new and stable
EGDE-CS-NZVI beads are suitable as the reactive materials
in PRBs.
2) With an increase of pH, removal rate of Cr (VI) decreased
but the removal rates of Cu (II), Cd (II) and Pb (II) increased.
The solution pH increased as the reaction proceeded.
3) The removal rate of Cr (VI), Cu (II), Cd (II), and Pb (II)
decreased with an increase of the initial Cr (VI) concentra-
tion. At low concentrations (less than 40 mg/L), heavy
metals were removed in the order: Cd (II) > Cu (II) > Pb
(II) > Cr (VI). As the concentration increased, the removal
order was changed into Pb (II) > Cu (II) > Cd (II) > Cr (VI).
4) SEM images showed that with a loose and porous surface,
EGDE-CS-NZVI beads showed a nucleus-shell structure.
The pore size of the nucleus ranged from 19.2 to 138.6 mm
with an average aperture size of around 58.6 mm. The shell
showed a tube structure linking the outside environment
with NZVI particles and wastewater could be introduced
into the beads through these tubes.
5) The XPS results suggested that extensive oxidation of iron
happened on the surface of NZVI and little Fe0 was left. The
reduction of Cr (VI) to Cr (III) was complete in less than 2 h.
Cu (II) and Pb (II) were removed by predominant reduction
and the formation of Fe(III)-heavy metals co-precipitate.
However, Cd (II) was mainly adsorbed on the EGDE-CS-
san beads-supported Fe0-nanoparticles for removal of heavybarriers, Water Research (2013), http://dx.doi.org/10.1016/
wat e r r e s e a r c h x x x ( 2 0 1 3 ) 1e1 0 9
NZVI beads surface and a small portion of Cd (II) was
reduced to Cd (0).
The result revealed that EGDE-CS-NZVI-beads PRBs had the
capacity to remediate actual electroplating wastewater and
could become an effective and promising technology for in situ
remediation of heavy metals.
Acknowledgments
The authors thank Zhigang Zhang, Qian Wang and Fei He for
their support with analyses. This work was financially sup-
ported by National Science & Technology Pillar Program
(2012BAC07B02), National Natural Science Foundation of
China (21307090), the University Science & Technology
Development Project of Tianjin (20110528), Program for New
Century Excellent Talents in University (NCET-10-0954), the
Natural Science Foundation of Tianjin (10SYSYJC27400),
Foundation of Tianjin Normal University (5RL109, 52XQ1104)
and Opening Fund of Tianjin Key Laboratory of Water Re-
sources and Environment (YF11700102).
r e f e r e n c e s
Algarra, M., Jimenez, M.V., Rodriguez-Castellon, E., Jimenez-Lopez, A., Jimenez-Jimenez, J., 2005. Heavy metals removalfrom electroplating wastewater by aminopropyl-Si MCM-41.Chemosphere 59 (6), 779e786.
Alowitz, M.J., Scherer, M.M., 2002. Kinetics of nitrate, nitrite, andCr (VI) reduction by iron metal. Environ. Sci. Technol. 36 (3),299e306.
Arao, T., Ishikawa, S., Murakami, M., Abe, K., Maejima, Y.,Makino, T., 2010. Heavy metal contamination of agriculturalsoil and countermeasures in Japan. Paddy Water Environ. 8,247e257.
Boddu, V.M., Abburi, K., Talbott, J.L., Smith, E.D., 2003. Removal ofhexavalent chromium from wastewater using a newcomposite chitosan biosorbent. Environ. Sci. Technol. 37 (19),4449e4456.
Cao, J.S., Zhang, W.X., 2006. Stabilization of chromium oreprocessing residue (COPR) with nanoscale iron particles. J.Hazard. Mater. 132 (2e3), 213e219.
Chatterjee, S., Lee, D.S., Lee, M.W., Woo, S.H., 2009. Nitrateremoval from aqueous solutions by cross-linked chitosanbeads conditioned with sodium bisulfate. J. Hazard. Mater. 166(1), 508e513.
Choi, J.H., Kim, Y.H., Choi, S.J., 2007. Reductive dechlorination andbiodegradation of 2,4,6-trichlorophenol using sequentialpermeable reactive barriers: laboratory studies. Chemosphere67 (8), 1551e1557.
EPA (US Environmental Protection Agency), 1998. Office of SolidWaste Draft PBT Chemical List. EPA/530/D-98/001A. Office ofSolid Waste and Emergency Response, Technology InnovationOffice, Washington, DC.
Farrell, J., Kason, M., Melitas, N., Li, T., 2000. Investigation of thelong term performance of zero-valent iron for reductivedechlorination of trichloroethylene. Environ. Sci. Technol. 34(3), 514e521.
Fu, F., Wang, Q., 2011. Removal of heavy metal ions fromwastewaters: a review. J. Environ. Manage. 92 (3), 407e418.
Fu, Y., Viraraghavan, T., 2003. Column studies for biosorption ofdyes from aqueous solutions on immobilised Aspergillus nigerfungal biomass. Water SA 29 (4), 465e472.
Please cite this article in press as: Liu, T., et al., Enhanced chitometals from electroplating wastewater in permeable reactivej.watres.2013.09.006
General Administration of Quality Supervision, Inspection andQuarantine of the People’s Republic of China (GAQSIQ), 1993.National Quality Standard for Groundwater in China (GB/T14848-93), pp. 2e3.
Genc-Fuhrman, H., Wu, P., Zhou, Y.S., Ledin, A., 2008. Removal ofAs, Cd, Cr, Cu, Ni and Zn from polluted water using an ironbased sorbent. Desalination 226, 357e370.
Geng, B., Jin, Z.H., Li, T.L., Qi, X.H., 2009. Kinetics of hexavalentchromium removal from water by chitosan-Fe0 nanoparticles.Chemosphere 75 (6), 825e830.
Giasuddin, A.B.M., Kanel, S.R., Choi, H., 2007. Adsorption of humicacid onto nanoscale zerovalent iron and its effect on arsenicremoval. Environ. Sci. Technol. 41 (6), 2022e2027.
Guo, T.Y., Xia, Y.Q., Hao, G.J., Song, M.D., Zhang, B.H., 2004.Adsorptive separation of hemoglobin by molecularlyimprinted chitosan beads. Biomaterials 25 (27), 5905e5912.
Hiemstra, T., Van-Riemsdijk, W.H., 1999. Surface structural ionadsorption modeling of competitive binding of oxyanions bymetal (hydr)oxides. J. Colloid. Interface Sci. 210 (1), 182e193.
Johnson, R.L., O’Brien, R.J., Nurmi, J.T., Tratnyek, P.G., 2009.Natural organic matter enhanced mobility of nano zero-valentiron. Environ. Sci. Technol. 43 (14), 5455e5460.
Joo, S.H., Feitz, A.J., Waite, T.D., 2004. Oxidative degradation of thecarbothioate herbicide, molinate, using nanoscale zero-valentiron. Environ. Sci. Technol. 38 (7), 2242e2247.
Kanel, S.R., Greneche, J.M., Choi, H., 2006. Arsenic(V) removal fromgroundwater using nanoscale zero-valent iron as a colloidalreactivebarriermaterial. Environ.Sci.Technol. 40 (6), 2045e2050.
Kavak, D., Ozturk, N., 2004. Adsorption of boron from aqueoussolution by sepirolite: II. column studies. II. illuslrararasi. Bor.Sempozyumu 23e25, 495e500.
Kirschling, T.L., Gregory, K.B., Minkley, E.G., Lowry, G.V.,Tilton, R.D., 2010. Impact of nanoscale zero-valent iron ongeochemistry and microbial populations in trichloroethylenecontaminated aquifer materials. Environ. Sci. Technol. 44 (9),3474e3480.
Lai, C.H., Chen, C.Y., 2001. Removal of metal ions and humic acidfrom water by iron-coated filter media. Chemosphere 44 (5),1177e1184.
Lee, J.W., Cha, D.K., Oh, Y.K., Ko, K.B., Jin, S.H., 2010. Wastewaterscreening method for evaluating applicability of zero-valentiron to industrial wastewater. J. Hazard. Mater. 180 (1e3),354e360.
Lerner, R.N., Lu, Q., Zeng, H., Liu, Y., 2012. The effects of biofilmon the transport of stabilized zerovalent iron nanoparticles insaturated porous media. Water Res. 46 (4), 975e985.
Li, N., Bai, R.B., 2005. Copper adsorption on chitosan-cellulosehydrogel beads: behaviors and mechanisms. Sep. Purif.Technol. 42 (3), 237e247.
Li, X.Q., Zhang, W.X., 2007. Sequestration of metals cations withzerovalent iron nanoparticles e a study with high resolutionX-ray photoelectron spectroscopy (HR-XPS). J. Phys. Chem. C111 (19), 6939e6946.
Liu, Q.Y., Bei, Y.L., Zhou, F., 2009. Removal of lead (II) fromaqueous solution with amino-functionalized nanoscale zero-valent iron. Cent. Eur. Chem. 7 (1), 79e82.
Liu, T., Zhao, L., Sun, D.S., Tan, X., 2010. Entrapment of nanoscalezero-valent iron in chitosan beads for hexavalent chromiumremoval from wastewater. J. Hazard. Mater. 184 (1e3),724e730.
Liu, T., Wang, Z.L., Zhao, L., Yang, X., 2012. Enhanced chitosan/Fe0-nanoparticles beads for hexavalent chromium removalfrom wastewater. Chem. Eng. J. 189-190, 196e202.
Ma, L.M., Zhang, W.X., 2008. Enhanced biological treatment ofindustrial wastewater with bimetallic zero-valent iron.Environ. Sci. Technol. 42 (15), 5384e5389.
Manning, B.A., Kiser, J.R., Kwon, H., Kanel, S.R., 2007.Spectroscopic investigation of Cr (III) and Cr (VI)-treatednanoscale zero-valent iron. Environ. Sci. Technol. 41, 586e592.
san beads-supported Fe0-nanoparticles for removal of heavybarriers, Water Research (2013), http://dx.doi.org/10.1016/
wat e r r e s e a r c h x x x ( 2 0 1 3 ) 1e1 010
McKenzie, R.M., 1980. The adsorption of lead and other heavymetals on oxides of manganese and iron. J. Soil Res. 18, 61e73.
Mekki, A., Holland, D., McConville, C.F., 1997. X-ray photoelectronspectroscopy study of copper sodium silicate glass surfaces.J. Non-Cryst. Solid 215, 271e282.
Melitas, N., Chuffe-Moscoso, O., Farrell, J., 2001. Kinetics ofsoluble chromium removal from contaminated water byzerovalent iron media: corrosion inhibition and passive oxideeffects. Environ. Sci. Technol. 35 (19), 3948e3953.
Mohan, D., Pittman, C.U., 2006. Activated carbons and low costadsorbents for remediation of tri- and hexavalent chromiumfrom water. J. Hazard. Mater. 137, 762e811.
Namasivayam, C., Panganathan, K., 1995. Removal of Cd (II) fromwastewater by adsorption on “waste” Fe(III)/Cr(III) hydroxide.Water Res. 29 (7), 1737e1744.
Nuhoglu, Y., Oguz, E., 2003. Removal of copper (II) from aqueoussolutions by biosorption on the cone biomass of Thujaorientalis. Process. Biochem. 38 (11), 1627e1631.
Panayotova, T., Dimova-Todorova, M., Dobrevsky, I., 2007.Purification and reuse of heavy metals containingwastewaters from electroplating plants. Desalination 206,135e140.
Phenrat, T., Kim, H.J., Fagerlund, F., Illangasekare, T., Tilton, R.D.,Lowry, G.V., 2009. Particle size distribution, concentration, andmagnetic attraction affect transport of polymer-modified Fe0
nanoparticles in sand columns. Environ. Sci. Technol. 43 (13),5079e5085.
Ponder, S.M., Darab, J.C., Mallouk, T.E., 2000. Remediation of Cr(VI) and Pb (II) aqueous solutions using supported, nanoscalezero-valent iron. Environ. Sci. Technol. 34 (12), 2564e2569.
Qian, Q., Mochidzuki, K., Fujii, T., Sakoda, A., 2009. Removal ofcopper from aqueous solution using iron-containingadsorbents derived from methane fermentation sludge. J.Hazard. Mater. 172 (2e3), 1137e1144.
Reynolds, T.M., Richards, P.S., 1996. Unit Operations andProcesses in Environmental Engineering. PSW Publishing Co.,Boston, p. 364.
Schwertman, U., Taylor, R.M., 1989. Iron oxides. In: Dixon, J.B.,Weed, S.B. (Eds.), Minerals in Soil Environments, second ed.,pp. 379e428 Soil Sci. Soc. Am. J., Medison, Wisconsin, USA.
Scott, T.B., Popescu, I.C., Crane, R.A., Noubactep, C., 2011. Nano-scale metallic iron for the treatment of solutions containingmultiple inorganic contaminants. J. Hazard. Mater. 186 (1),280e287.
Shama, S.A., Moustafa, M.E., Gad, M.A., 2010. Removal of heavymetals Fe3þ, Cu2þ, Zn2þ, Pb2þ, Cr3þ and Cd2þ from aqueoussolutions by using eichhornia crassipes. PortugaliaeElectrochim. Acta 28 (2), 125e133.
Please cite this article in press as: Liu, T., et al., Enhanced chitometals from electroplating wastewater in permeable reactivej.watres.2013.09.006
Shi, L.N., Zhang, X., Chen, Z.L., 2011. Removal of chromium (VI)from wastewater using bentonite-supported nanoscale zero-valent iron. Water Res. 45 (2), 886e892.
Shokes, T.E., Moller, G., 1999. Removal of dissolved heavy metalsfrom acid rock drainage using iron metal. Environ. Sci.Technol. 33 (2), 282e287.
Thiruvenkatachari, R., Vigneswaran, S., Naidu, R., 2008.Permeable reactive barrier for groundwater remediation. J.Ind. Eng. Chem. 14 (2), 145e156.
Uzum, C., Shahwan, T., Erolu, A.E., Hallam, K.R., Scott, T.B.,Lieberwirth, I., 2009. Synthesis and characterization ofkaolinite-supported zero-valent iron nanoparticles and theirapplication for the removal of aqueous Cu2þ and Co2þ ions.Appl. Clay Sci. 43 (2), 172e181.
Vijayaraghavan, K., Jegan, J., Palanivelu, K., Velan, M., 2005. Batchand column removal of copper from aqueous solution using abrown marine alga Turbinaria ornate. Chem. Eng. J. 106 (2),177e184.
Wang, J., Qian, Y., 1999. Microbial degradation of 4-chlorophenolby microorganisms entrapped in carrageenan-chitosan gels.Chemosphere 38 (13), 3109e3117.
Wan-Ngah, W.S., Fatinathan, S., 2008. Adsorption of Cu (II) ionsin aqueous solution using chitosan beads, chitosan-GLAbeads and chitosan-alginate beads. Chem. Eng. J. 143 (1e3),62e72.
Wan-Ngah, W.S., Hanafiah, M.A.K.M., Yong, S.S., 2008.Adsorption of humic acid from aqueous solutions oncrosslinked chitosan-epichlorohydrin beads: kinetics andisotherm studies. Colloid Surf. B 65 (1), 18e24.
Wilkin, R.T., McNeil, M.S., 2003. Laboratory evaluation of zero-valent iron to treat water impacted by acid mine drainage.Chemosphere 53 (7), 715e725.
Xiu, Z.M., Jin, Z.H., Li, T.L., Mahendra, S., Lowry, G.V.,Alvarez, P.J.J., 2010. Effects of nanoscale zero-valent ironparticles on a mixed culture dechlorinating trichloroethylene.Bioresour. Technol. 101 (4), 1141e1146.
Zhan, J., Sunkara, B., Le, L., John, V.T., He, J., McPherson, G.L.,Piringer, G., Lu, Y., 2009. Multifunctional colloidal particles forin situ remediation of chlorinated hydrocarbons. Environ. Sci.Technol. 43 (22), 8616e8621.
Zhang, H., Alsarra, I.A., Neau, S.H., 2002. An in vitro evaluation ofa chitosan-containing multiparticulate system formacromolecule delivery to the colon. Int. J. Pharm. 239,197e205.
Zhang, M., He, F., Zhao, D., Hao, X., 2011. Degradation of soil-sorbed trichloroethylene by stabilized zero valent ironnanoparticles: effects of sorption, surfactants, and naturalorganic matter. Water Res. 45 (7), 2401e2414.
san beads-supported Fe0-nanoparticles for removal of heavybarriers, Water Research (2013), http://dx.doi.org/10.1016/