Coatings 2013, 3(3), 140-152; doi:10.3390/coatings3030140

Article
Electrochemical Synthesis of Nitro-Chitosan and Its Performance in Chromium Removal
Prashant K. Jha 1,*, Gary P. Halada 1 and Scott M. McLennan 2
1
Department of Materials Science and Engineering, Stony Brook University, 314, Old Engineering Building, Stony Brook, NY 11794, USA; E-Mail: ghalada@ms.cc.stonybrook.edu
2
Department of Geosciences, Stony Brook University, 255 Earth and Space Sciences Building, Stony Brook University, Stony Brook, NY 11794, USA; E-Mail: smclennan@notes.cc.sunysb.edu
*
Author to whom correspondence should be addressed; E-Mail: pjha@ic.sunysb.edu; Tel.: +1-631-365-9344; Fax: +19735567955.
Received: 20 January 2013; in revised form: 10 July 2013 / Accepted: 12 July 2013 /
Published: 19 July 2013

Abstract

: A synthesized polymeric form of chitosan, electrochemically precipitated and photochemically modified, has been found to have significant value in removal of toxic chromate oxyanions from solution. Fourier Transform Infra-Red (FTIR), Raman and X-ray photoelectron spectroscopy (XPS) indicated that a significant percentage of the amine functional groups were oxidized to nitro groups as a result of reactions with hydroxyl ions formed in the electrochemical process with additional oxidation occurring as a result of exposure to ultra-violet light. The adsorption capacity of the modified chitosan for chromate was investigated in a batch system by taking into account effects of initial concentration, pH of the solution and contact time. Nitro-chitosan showed greater adsorption capacity towards Cr (VI) than other forms of chitosan, with a maximum adsorption of 173 mg/g. It was found that pH 3 is the optimum for adsorption, a Langmuir model is the best fit for the adsorption isotherm, and the kinetics of reaction followed a pseudo second order function. Overall, our results indicate that electrochemical modification of chitosan is an effective method to enhance the reactivity of chitosan towards metals.
Keywords:
chitosan; nitro-chitosan; electrochemical

1. Introduction

Toxic metal contamination of soil and groundwater is a major environmental threat. Contamination from toxic heavy metals is present in as many as 63% of 1200 sites on the National Priority List of the U.S. Environmental Protection Agency (EPA) for treatment of contaminated groundwater. At 11% of these sites chromium was found to be present making it one of the main toxic metal contaminants [1]. Chromium is used in industrial processes such as metal plating, leather tanning and pigment production resulting in release to groundwater [2]. In aerated aqueous solutions chromium is stable only as Cr(III) and Cr(VI) [3]. Although Cr(III) is essential for living beings in small amounts for its role in carbohydrate metabolism[4], it is toxic at higher concentrations. Also, in alkaline environments Cr(III) can oxidize to Cr(VI), which is toxic even at low concentrations, as it induces coetaneous allergies and is carcinogenic over long exposures [4,5].Various methods developed for removal of toxic metals from groundwater include: isolation and containment, mechanical separation, pyrometallurgical separation, chemical treatment, permeable treatment walls, electrokinetics, biochemical processes, phytoremediation and soil flushing [1]. Chemical remediation using naturally occurring biodegradable biomass has generated a great deal of interest due to its low cost and high efficiency [6]. Some of the sorbents based on biomass are bark, seaweed, leaf mould and chitosan; detailed information on these and a comparison of their chemistry and performance can be found in work of S.E. Bailey et al. [7]. Chitosan is among the chief biomass-based remediation agents.

Chitosan is a linear, high molecular weight, crystalline polysaccharide consisting of β-(1→4) linked N-acetyl-D-glucosamine [8]. It is produced by alkaline N-deacetylation of chitin, the second most abundant natural polymer after cellulose [9]. Changing the acetamide group to amine increases the reactivity rendering chitosan a better chelation and adsorption agent than chitin [10]. The adsorption capacity of chitosan has been further enhanced using physical modifications including conditioning as gel beads and microcrystalline chitosan as well as chemical modifications such as cross-linking and insertion of new functional groups [11]. Chemical modification of chitosan utilizes the presence of primary amine and primary hydroxyl as well as secondary hydroxyl groups in the chitosan molecule, which makes it very amenable to further functionalization and modification. Chemical modifications of chitosan have been thoroughly reviewed by Mourya and Inamdar [12].

In the present work we report a novel electrochemical process followed by photochemical treatment for chitosan modification. The process results in formation of nitro groups through oxidization of a fraction of the amine groups of chitosan. The new biopolymer formed was characterized using spectroscopic techniques, and metal binding capacity was explored using chromium as chromate in aqueous solution. The adsorption capacity of the nitro-chitosan was compared with other forms of modified chitosan as reported in the literature.

2. Results and Discussion

2.1. Electrodeposition

Chitosan dissolves in acidic aqueous solution by addition of a proton to the NH2 group to form NH3+. The process is reversible and on increasing pH higher than 6.3, protonated chitosan deprotonates and precipitates. As reported previously by this group [13] as well as in work by Fernendes et al. [14], a localized zone of high pH is created near a cathode held at sufficiently negative potential in water, a method utilized in this process to electrochemically deprotonate protonated chitosan and form deposits on the steel substrate. Stainless steel is chosen as an electrode as it is inexpensive, easy to use, and does not corrode at cathodic potentials. The presence of an ultrathin passive layer on the steel enhances initial chitosan film formation and sorption, as was shown in our previous work.

During cathodic polarization, reduction of H+ ions results in formation of H2 gas, as indicated by hydrogen bubble formation on the steel substrate. This removal of H+ ions from solution creates a zone of high pH near the substrate where chitosan is deposited. The film thus formed is shown in the scanning electron microscopy (SEM) micrograph in Figure 1. The figure shows Chitosan was deposited in a multilayer structure. The first layer of chitosan is formed on the surface of hydrogen bubbles formed on the electrode (indicated in Figure 1 as the brightest area due to the most penetration of electrons from the substrate below) with diameter around 100 μm (Figure 1). With the continuation of electrolysis and further accumulation of hydrogen, the bubbles collapse into each other to form larger bubbles of hydrogen 300–400 μm in diameter, leaving the precipitated chitosan structure behind. An additional layer of chitosan is precipitated on top of the new bubbles formed (the areas with intermediate darkness in Figure 1). The process continues forming still larger bubbles with diameter 300 μm to 1 mm forming the top layer of the precipitated chitosan film. The darkest areas (dark due to the blocking of electrons emitted from the substrate below by chitosan) in the figure are those with the maximum amount of chitosan which could have formed by transport of material along the bubble surface (hence making the top of the bubble progressively thinner until it breaks; the resulting fractures in this layer are clearly visible in the picture).

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Figure 1. Scanning electron microscopy of electrochemically deposited chitosan on stainless steel at −3.0 V vs. Ag/AgCl reference electrode.

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Figure 1. Scanning electron microscopy of electrochemically deposited chitosan on stainless steel at −3.0 V vs. Ag/AgCl reference electrode.
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2.2. Characterization

The result of FTIR spectroscopy of the deposited material is summarized in Table 1. The peaks at 1663 cm−1, 1203 cm−1 and 970 cm−1 indicate oxidation of some of the nitrogen in chitosan as a result of the electrochemical process. Raman spectra of the air-dried chitosan film as well as electrochemically modified chitosan are shown in Figure 2. The peak at 2920 cm−1 from the air-dried sample most likely results from a combination of asymmetric C–H vibration from CH2OH and C–O stretching vibration from the hydroxyl group. The broad peak at 1634 cm−1 is expected to result from a combination of amine N–H deformation and aromatic C=C stretching vibrations. The peak at 1465 cm−1 is expected to be from the C–H scissor vibration while the peak at 1384 cm−1 is expected to be from the CH2 wagging. Peaks at 1325 cm−1 and 1188 cm−1 can be attributed to C–N stretching from the amine group. The peak at 1256 cm−1 can be attributed to OH deformation vibration of the CH2OH group. The peaks at 1188 cm−1 and 820 cm−1 are expected to be from symmetrical and asymmetrical C–O–C stretching in cyclic ether while the peaks at 935 cm−1 and 468 cm−1 are expected from C–O–C bonds between monomer units. The peaks at 628 cm−1 and 560 cm−1 can be attributed to ring vibrations. Raman spectrum of electrochemically deposited material showed various new peaks: a peak at 3345 cm−1 from the N–H stretching vibration in C=N–H groups while the peak at 1860 cm−1 is expected to be from the C=O stretching vibration. The peak at 1589 cm−1 can be attributed to N–H bending in the amine and the peak at 1525 cm−1 is consistent with the asymmetric NO2 stretching vibration. The peak at 901 cm−1 is consistent with the C–N stretching vibration in nitro groups, and the new peak at 491 cm−1 is expected to be from the NO2 rocking vibration. Vibrational spectroscopy also indicates oxidation of a fraction of amine to imine and nitro groups as well as oxidation of some of the hydroxyl groups to aromatic ketone.

To confirm oxidation, XPS of the underside of a removed film layer (as described previously) was carried out. The resulting XPS spectrum of electrodeposited chitosan is shown in Figure 3. Two peaks are present for N1s; with charge correction, they correspond to binding energies of 398.6 eV (NH2) and a large, broad peak at 407 eV. The peak at 407 eV confirms the oxidation of nitrogen in chitosan, falling in the range of nitrate in cellulose nitrate (408.1 eV) and C–NO2 nitro compounds (406.3 eV) [15].

Table 1. Peak positions and assignments for the Fourier Transform Infrared spectrum of ECM-chitosan.

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Table 1. Peak positions and assignments for the Fourier Transform Infrared spectrum of ECM-chitosan.
Peak (cm−1)Assignment
1663combination of amide I C=O stretching, asymmetric NO2 stretching and OH deformation vibrations
1585NH bending frequency
1442C–C stretching vibration
1380combination of CH3 deformation and CO stretching frequencies
1203combination of NH deformation and symmetric NO2 stretching vibrations
1154, 1020symmetric and asymmetric stretching vibrations of C–O–C respectively
970amine oxide
805O–H deformation
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Figure 2. Raman spectra of electrochemically modified chitosan (ECM) chitosan and dried chitosan solution at pH 2.

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Figure 2. Raman spectra of electrochemically modified chitosan (ECM) chitosan and dried chitosan solution at pH 2.
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Figure 3. .X-ray photoelectron spectroscopy (XPS) of electrodeposited chitosan. Peak 1: primarily amine (–NH2), Peak 2: similar to nitrate, possible nitronyl (N=O).

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Figure 3. .X-ray photoelectron spectroscopy (XPS) of electrodeposited chitosan. Peak 1: primarily amine (–NH2), Peak 2: similar to nitrate, possible nitronyl (N=O).
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Hence, vibrational and X-ray spectroscopy provide clear evidence of oxidation of at least a portion of the amine groups in chitosan to nitro groups and some hydroxyl groups to aromatic ketone. The estimated structure of this novel molecule is shown in Figure 4. The oxidation can be due to reaction of amine and hydroxyl groups with OH ions formed by electrolysis of entrapped water molecules in the hydrogel structure as shown in Equations below.

–NH2 + OH → =NH + H2O + e
=NH + 5OH → =NO2 + 3H2O + 5e
–OH + OH → =O + H2O + e

Exposure of hydrogel to ultraviolet light was found to increase the intensity of the oxidized nitrogen peak in X-ray photoelectron spectroscopic spectrum (not shown) indicating oxidation of a higher fraction of amine. Enhanced oxidation of nitrogen by hydroxyl ion in the presence of UV light has also been observed by other researchers [16].

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Figure 4. Structures of chitosan and nitro-chitosan synthesized by electrochemical deposition and photochemical oxidation.

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Figure 4. Structures of chitosan and nitro-chitosan synthesized by electrochemical deposition and photochemical oxidation.
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2.3. Equilibrium Adsorption Isotherms

The amount of metal adsorbed per unit mass of electrochemically modified (ECM)-chitosan, Qe, was calculated using formula:

Qe = (CiCe)V/M
Where Ci is the initial concentration and Ce is the equilibrium concentration in mg/L and M is the dry mass of adsorbent in mg and V is the volume in liters. The results of batch equilibrium adsorption are shown in Figure 5. The amount of chromium adsorbed by unit mass of ECM-chitosan increases with initial concentration of chromium till a plateau is achieved at 300 ppm, the result was similar to observations involving other forms of modified chitosan.using poly(2-acrylamido-2-methypropane sulfonic acid) and poly 3-methyl thiophene [17,18]. The adsorption capacity was found to be 174.4 mg Cr(VI)/g of ECM-chitosan which is higher than values observed for modifications of chitosan by Verma et al. [19] and the references cited therein.

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Figure 5. Isotherm for adsorption of Cr(VI) onto ECM-chitosan.

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Figure 5. Isotherm for adsorption of Cr(VI) onto ECM-chitosan.
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Equilibrium adsorption isotherms were used to investigate interactive behavior between the solution and adsorbent. A widely used Langmuir model which is representative of monolayer adsorption occurring on an energetically uniform surface without interactive molecules [20], was found to fit the process successfully (Figure 6). The Langmuir model (Equation 5) and its linear transformation (Equation 6) are given below.

Qe = QmbCe/(1 + bCe)
1/Qe = 1/Qm + 1/bQmCe
Where Qe is equilibrium adsorption capacity (mg/g), Ce is the solution concentration at equilibrium (mg/L), Qm is the Langmuir constant representing maximum adsorption capacity (mg/g) and b is the Langmuir constant related to energy of adsorption (L/mg). The calculated value of Qm was 500 mg/g which is well above the experimentally observed value. The calculated value of b was 0.001 L/mg, with a correlation coefficient (R2) of 0.9909. A dimensionless separation factor (RL) was used to determine the efficiency of adsorption obtained by equation RL = 1/(1 + bC0) where C0 is the initial concentration. The positive value calculated for b ensures an RL value between 0 and 1 indicating the process of adsorption is feasible.

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Figure 6. Langmuir plot for adsorption of Cr(VI) onto ECM-chitosan.

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Figure 6. Langmuir plot for adsorption of Cr(VI) onto ECM-chitosan.
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2.4. Effect of pH on Adsorption of Chromate

The pH of the adsorption medium influences the physicochemical interactions between dissolved ions and adsorptive sites on the adsorbent [21]. The effect of pH on adsorption of Cr(VI) by electrochemically modified chitosan in the pH range of 1 to 8 is shown is Figure 7. The maximum adsorption of Cr(VI) was observed for pH 3 followed by a plateau region between pH 4 and 7, while the adsorption capacity of ECM-chitosan was found to collapse on reaching pH 8. Chromate exists as HCrO4 at acidic pH, at intermediate pH (pH value 5–7) chromate exists as HCrO4 as well as CrO42−, while at pH values higher than 7, chromium exists as CrO42− [22].

The adsorption behavior at intermediate pH values can be due to several single or combined effects. Adsorption most likely occurs due to formation of a pendant structure with nitro and oxidized hydroxyl groups. At low pH the surface of the ECM-chitosan, just like pure chitosan, would be surrounded by oxidanium ions which would increase the attractive force between chromium(VI) and binding sites [23]. In very acidic solution (pH value less than 3) the presence of excess oxidanium ion can lead to independent complexation with chromate thus rendering the attraction from ECM chitosan ineffective while formation of CrO42− as well as reduction in oxidanium ion can be the reason for declining adsorption with increasing pH. Adsorption may also occur due to electrostatic attraction between any remaining positively charged amino groups and negatively charged chromate/dichromate ions in solution [24].

2.5. Sorption Kinetics

Chromium removal by ECM-chitosan as a function of contact time is shown in Figure 7. The reaction was rapid initially with 50% metal uptake complete within the first 5 min after which it proceeded slowly and equilibrium was achieved in 3 h. To further investigate the adsorption, mechanism and rate controlling step kinetic models were used. Pseudo first order, pseudo second order as well as inter particle diffusion models were used for analysis. The pseudo second order reaction (Equation 7) was found to fit the experimental data successfully (Figure 8).

t/qt = 1/kqe2 + t/qe
The value of k was found to be 2.038 g/mg h with a linear correlation coefficient of 0.9987 indicating that the rate controlling step in chromium adsorption is chemisorption involving valence forces through the sharing or exchange of electrons between chromium and ECM-chitosan [25] in the concentration range tested.

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Figure 7. Effect of pH (red) and contact time (blue) on chromium adsorption onto ECM-chitosan.

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Figure 7. Effect of pH (red) and contact time (blue) on chromium adsorption onto ECM-chitosan.
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Figure 8. Curve fitting by pseudo second order reaction model on adsorption.

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Figure 8. Curve fitting by pseudo second order reaction model on adsorption.
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3. Experimental Section

3.1. Electrodeposition of Chitosan

The chitosan solution was made by mixing 1.5 g low molecular weight chitosan (Sigma Aldrich, Milwaukee, WI, USA, 75%–85% deacetylated) to 120 mL DI water under constant stirring. HCl (1 M) was then added drop wise until all the chitosan was dissolved, which occurred as the solution reached pH 2. For electrochemical deposition of chitosan, polished type 304 stainless steel (metal composition approx. 19% Cr, 9% Ni, balance Fe) was chosen as the working electrode. This process has been detailed by the authors in a previous publication [13]. Pt wire served as the counter electrode. A Gamry Reference 600 potentiostat was used to perform electrochemistry and Gamry Instrument Framework software was used for control and monitoring of voltage and current. Controlled potential coulometry at a voltage of −3.0 V (versus Ag/AgCl reference electrode) was applied for 5 min. The resulting hydrogel was rinsed in DI water to remove any chitosan solution entrapped in the resulting hydrogel. The gel was then exposed to UV light (20 W at 6 cm) for 10 min, following which it was then peeled from the electrode and left to dry further for 48 h. A thin film may remain behind on the electrode surface, bound to the passive layer, as detailed in our previous work [13]. The film removed from the electrode was dried and then crushed mechanically to form powder for spectroscopic analysis and absorption experiments.

3.2. FTIR

Fourier Transform Infrared Spectroscopy (FTIR) spectra were obtained using a Nicolet 760 infrared spectrometer modified to collect data in both mid- and far infrared regions. Samples were ground to a fine powder. Spectra were collected using an MCT-A detector with data resolution set to 2 cm−1 and summed over 256 scans to improve the signal-to-noise ratio. A Gemini sampling accessory (Spectra-Tech, Madison, WI, USA) collected diffuse reflectance data from powder samples. The analysis chamber was purged continuously with doubly dried air to prevent the absorption of water vapor, and a globar-type IR source was used.

3.3. Raman Spectroscopy

A Nicolet Almega dispersive Raman spectrometer (Thermo Scientific, Madison, WI, USA) with a 785 nm laser source was used for analysis. Powdered samples were placed on quartz slides and Raman microspectroscopy in reflectance mode was used for data acquisition. Data was collected in the 3600–400 cm−1 range. An average of 10 scans with 5 s accumulation time for each exposure was collected and data was processed using OMNIC [26]. For comparison, chitosan solution at pH 3 was dried (without any applied potential) on stainless steel and similarly analyzed.

3.4. XPS

To detect speciation of nitrogen, X-ray photoelectron spectroscopic (XPS) studies were carried out. Sample preparation consisted of peeling off the deposited film from the stainless steel substrate after immersion in liquid nitrogen for one minute. The film was removed using a stainless steel razor and mounted on the XPS sample holder using indium foil. XPS measurements were performed using a custom-designed spectrometer that utilized a VG Scientific (Newburyport, MA, USA) CLAM2 hemispherical analyzer with lensing, controlled by a VGX900I data acquisition system. An Mg Kα1,2 ( = 1253.6 eV) X-ray source operating at 20 kV and 10 mA with a 20 eV pass energy was used at a pressure of 1.33 × 10−7 Pa. Measurements were taken at a 90° take-off angle with respect to the surface and charge correction was done by referencing to the C 1s line of adventitious carbon (284.6 eV).

3.5. Absorption Experiments

Stock solution (1000 ppm) of Cr(VI) was prepared by using K2Cr2O7 obtained from Sigma Aldrich, in deionized water (>18 MΩ/cm) The stock solution was then diluted to give standard solutions of appropriate concentrations. Batch adsorption experiments were conducted in 250 mL conical flasks and equilibrated using a magnetic stirrer. This is similar to the method used in references [3,27] where 0.02 g of modified chitosan was added to 50 mL of standard solution and equilibrated for 30 min. Supernatant solution was then filtered and analyzed. For equilibrium time determination, 0.5 g of modified chitosan was mixed in 1 L of 26 ppm Cr(VI) solution under constant stirring. Samples of two milliliters of solution were removed at predetermined times, filtered and analyzed. To determine the effect of pH on adsorption, the pH of the 26 ppm Cr solution was controlled by introducing a small amount of 1 M HCl and 1 M NaOH solutions as required, while the remaining parameters were kept the same as for the batch experiments. Chromium concentrations were measured using DCP-AES.

3.6. DCP-AES

Elemental analyses were carried out with an Applied Research Laboratories Spectraspan (Valencia, CA, USA) VB Direct Current Argon Plasma Atomic Emission Spectrometer (DCP-AES,). This system uses a Czerny-Turner spectrometer with an Echelle grating and 30° prism for order separation. At 400 nm reciprocal linear dispersion is 0.122 nm/mm and for a 25 μm entrance slit spectral band pass is 0.0030 nm. Analyses were performed in single element mode, using standard settings and a solution flow rate of 0.5 mL/min. Emission lines used for analyses were Cr 425–435 nm.

Standards used for calibration for Cr analyses were prepared from commercially available single element 1000 ppm emission spectroscopy stock solution standards prepared in 1%–2% nitric acid. Net counts were calibrated using a “two-point” calibration system involving a blank and a high standard that was prepared to be slightly more concentrated than the highest concentration sample, thus bracketing the concentration range of the samples. Three to four additional standards, spanning the full concentration range of the samples, were also prepared and run as “unknowns” to confirm linear calibration curves and to monitor reproducibility. Samples were run in duplicate.

4. Conclusions

Electrochemical deposition of chitosan is an effective method to form chitosan hydrogel coating on conducting surfaces. The coating formed by electrochemical deposition becomes chemically modified with some of the amine groups changing to nitro groups. The modification is further enhanced by exposing the hydrogel to ultra-violet light. Modified chitosan containing nitro groups can have tremendous applications in various fields from remediation to drug delivery because of its higher affinity towards negatively charged metallic ions than chitosan.

Acknowledgments

This work was partially supported by a Stony Brook University/Brookhaven National Laboratory SEED grant.

Conflict of Interest

The authors declare no conflict of interest.

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