# A Dopamine Sensor Based on Pre-Concentration by Magnetic Nanoparticles

Authors: Mojtaba Bagherzadeh; Somayeh Ansari; Fariborz Riahi; Anahita Farahbakhsh
Journal: International Journal of Electrochemistry
 (2013)

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## Abstract

Herein, Fe3O4 magnetic nanoparticles (MNPs) were synthesized and characterized. Afterward, a magnetic carbon paste electrode (MCPE) was modified with MNPs via casting and drying MNPs on top of the MCPE (MCPE/MNP). Electrochemical behavior of the MCPE/MNP was studied by cyclic voltammetry in the presence of [Fe(CN)6]3−/4− as a redox probe, and surface pKa of MNPs was evaluated as 6.3±0.1. The behavior of MCPE/MNP towards dopamine (DA) and ascorbic acid (AA) has been investigated by electrochemical methods, and the obtained results showed that the MCPE/MNP has adsorption behavior towards only DA. Based on this behavior, the DA molecules were pre-concentrated on top of the MCPE/MNP and followed with stripping in DA free solution. Subsequent to experimental and instrumental optimization, a calibration curve from 5.0×10-6 to 1.0×10-3 M DA with r2=0.999, DL = 7.6×10-7 M DA, and RSD = 4.6%, was obtained in the presence of 1.0×10-3 M AA. Performance of the MCPE/MNP was successfully tested in a pharmaceutical sample.


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## Body

## 1. Introduction

Dopamine (DA) is one of the most important neurotransmitters. It plays a significant role in the functioning of central nervous, renal, and hormonal systems as well as in drug addiction and Parkinson’s disease [1, 2]. Therefore, understanding its electrochemical properties and quantifying its presence in human body fluids are the most important. Dopamine can be easily oxidized electrochemically at conventional electrodes, which have been used to detect the neurotransmitter [3–7]. Apart from the need to reach low detection limits, determination of the DA is complicated by the coexistence of many interfering compounds. Among them, ascorbic acid (AA) is of particular importance [8]. Ascorbic acid accompanies DA in biological samples: for instance, in the extracellular fluid of central nervous system, AA is present at the 100–500 μM concentration level, whereas the concentration of DA is less than 100 nM [9]. But, in the biological samples, the basic concentrations of DA and AA vary from region to region and time to time in an extremely wide range, from 1.0×10-7 to 1.0×10-3 M [10]. Therefore, improving the sensitivity and especially the selectivity of working electrodes toward the DA has been a goal of researchers in this area. To meet this challenge, a variety of modified electrodes have been proposed. These include self-assembled monolayer electrodes [5–7], polymer electrodes [11, 12], and nanomaterial film electrodes [13–15]. However, in all cases two general strategies were employed for detection of DA; (i) separation of DA and AA oxidation potentials, or (ii) selective pre-concentration of DA and following its determination [16].Materials in the nanometer range are expected to exhibit new functional properties for a wide range of applications, including: catalysis, optics, microelectronics, and chemical/biological aspects. One of the most interesting and practically promising fields is the research on magnetic nanoparticles for their attractive properties and many potential applications as sensors technology [17]. Recently, ferromagnetic materials have gained much intense research on biomedical and biotechnological applications. Superparamagnetic iron oxide nanoparticle (Fe3O4) is one of the famous magnetic materials in common use. Due to its biocompatibility, catalytic activity, and low toxicity, its applications in biotechnology and medicine have gained significant attention, and it would be promising to utilize Fe3O4 nanoparticles for the sensing application [18]. It has been reported that these kinds of particles could be functionalized with a wide range of functional groups [19–22] and favorably interacted with enzymes by some active groups such as –OH, –COOH, and –NH2 [23]. So it is of interest to examine the interaction of biologically active molecules such as DA by ferromagnetic nanoparticles. There are few reports on the electrochemical study of Fe3O4 MNPs interaction with DA [24–26]. In all reported works, Fe3O4 MNPs were employed in determination of DA via strategy (i), that is, oxidation potential separation. On the other hand, recently interest reports were published on bonding DA to the Fe3O4 MNPs via its diols [27–31]. However, this interesting behavior did not employ in dopamine determination via strategy (ii), that is, selective pre-concentration of DA.In the present work,Fe3O4 nanoparticles have been synthesized and characterized, and then its dispersing solution was casted on the magnetic CPE to form a novel modified electrode (MCPE/MNP). The experimental results showed that the modified electrodes displayed a significant promoting effect on the oxidation of [Fe(CN)6]3−/4− as a redox probe with the remarkable enhancement in the peak current. Effects of scan rate and pH were evaluated on the MCPE/MNP response to the redox probe, and surface area and charge state (surface pKa) of the MCPE/MNP were calculated from its response. Interaction of the Fe3O4 MNP with DA molecules was studied by electrochemical and spectroscopic methods, and an adsorption behavior was observed and confirmed. This adsorption behavior of DA allowed us to pre-concentrate DA on top of the MCPE/MNP surface from solution. Effective parameters such as pH, pre-concentration time, amount of Fe3O4, and instrumental parameters on adsorbed DA response were evaluated. Finally, the performance of the MCPE/MNP was successfully examined for electrochemical determination of DA in a pharmaceutical sample. Recently, Liu et al. reported the first example of the quantification of DA using Fe3O4 nanoparticles via fluorescence spectroscopy [32], but the current work is an example of electrochemical determination of DA by using Fe3O4 MNPs based on selective pre-concentration of DA, that is, strategy (ii). The obtained results will be presented and described here.


## 2. Experimental

### 2.1. Chemicals

Dopamine, ascorbic acid, and other materials were of analytical grade (Sigma or Merck) and were used as received without further purifying.Fe3O4 magnetic nanoparticles were prepared according to the literature [33]. Graphite powder (spectrum grade, average particle size 4 μm) and paraffin oil were from Merck. Phosphate buffer saline solutions (PBS) in the pH range of 2.0 to 10.0 were prepared using Smalley’s method [34]. The initial pH was ca. 2.1 for 0.1 M NaClO4+0.01 M H3PO4. The higher pH was adjusted by the addition of 0.11 M NaOH. The ionic strength of the solutions was constant over the entire range of pH. A DOPADIC ampoule (Iran Pharmaceutical Development Investment Co., I.P.D.I.C., Rasht, Iran) containing 5 mL of 200 mg mL−1 DA hydrochloride was used as DA source of pharmaceutical sample.


### 2.2. Electrode Preparation

The conventional carbon paste was prepared by mixing 70 mg graphite powder and 30μL paraffin oil. A magnetic carbon paste electrode (MCPE) consisted of a permanent cylinder magnet (5mmd.×2mml.) and was press-fit into a syringe cylindrical tube (6mmo.d.×50mml.). The magnet was connected to a copper wire for electrical connection on one end. On the other end, it was packed with carbon paste to about 2 mm depth from the liquid interface. The surface of carbon paste was smoothed on a weighing paper for the MCPE, and the surface area of 0.12 cm2 was calculated based on Randle-Sevcik equation [35]. One hundred mg of nanosized Fe3O4 particles were dispersed in 10 mL ethanol under ultrasonication for 30 min. Six μL of this dispersion solution was chosen as the modifying amount and dropped onto the surface of the MCPE, then dried in air at room temperature for forming the modified electrode (MCPE/MNP).


### 2.3. Instruments

The crystal structure of the as-preparedFe3O4 powders was studied by an X-ray diffractometer (XRD, Bruker Advanced D8 model), using Cu Kα radiation (λ=1.5406Å). The size and morphology of the as-prepared Fe3O4 particles and the chemical composition of the prepared particles were characterized using transmission electron microscope, TEM, (Philips-EM-208S) and scanning electron microscope, SEM, (Seron Technology AIS 2100 (South Korea)) equipped EDXA instruments. Magnetic properties were analyzed using a vibrating sample magnetometer (VSM, Daghigh Meghnatis Kashan Co., Kashan, Iran). The specific surface areas of MNPs were determined by the BET method. Fourier-transform infrared (FTIR) spectroscopy analysis was performed with a Nicolet Impact 400D Model spectrophotometer (Nicolet Impact, Madison, USA). Instruments UV-Vis detection was carried out on a double beam UV-Vis spectrometer (Cintra 404, GBC).All electrochemical measurements including cyclic voltammetry (CV) and square wave voltammetry (SWV) were carried out on Metrohm 797VA instrument (Herisau, Switzerlan). A three-electrode conventional cell, including the modified MCPE as working electrode, a large surface area Pt plate (99.99%) as auxiliary electrode, and a Ag/AgCl (3 M KCl) electrode as reference, was used for electrochemical measurements. All experiments were carried out at room temperature.


## 2.1. Chemicals

Dopamine, ascorbic acid, and other materials were of analytical grade (Sigma or Merck) and were used as received without further purifying.Fe3O4 magnetic nanoparticles were prepared according to the literature [33]. Graphite powder (spectrum grade, average particle size 4 μm) and paraffin oil were from Merck. Phosphate buffer saline solutions (PBS) in the pH range of 2.0 to 10.0 were prepared using Smalley’s method [34]. The initial pH was ca. 2.1 for 0.1 M NaClO4+0.01 M H3PO4. The higher pH was adjusted by the addition of 0.11 M NaOH. The ionic strength of the solutions was constant over the entire range of pH. A DOPADIC ampoule (Iran Pharmaceutical Development Investment Co., I.P.D.I.C., Rasht, Iran) containing 5 mL of 200 mg mL−1 DA hydrochloride was used as DA source of pharmaceutical sample.


## 2.2. Electrode Preparation

The conventional carbon paste was prepared by mixing 70 mg graphite powder and 30μL paraffin oil. A magnetic carbon paste electrode (MCPE) consisted of a permanent cylinder magnet (5mmd.×2mml.) and was press-fit into a syringe cylindrical tube (6mmo.d.×50mml.). The magnet was connected to a copper wire for electrical connection on one end. On the other end, it was packed with carbon paste to about 2 mm depth from the liquid interface. The surface of carbon paste was smoothed on a weighing paper for the MCPE, and the surface area of 0.12 cm2 was calculated based on Randle-Sevcik equation [35]. One hundred mg of nanosized Fe3O4 particles were dispersed in 10 mL ethanol under ultrasonication for 30 min. Six μL of this dispersion solution was chosen as the modifying amount and dropped onto the surface of the MCPE, then dried in air at room temperature for forming the modified electrode (MCPE/MNP).


## 2.3. Instruments

The crystal structure of the as-preparedFe3O4 powders was studied by an X-ray diffractometer (XRD, Bruker Advanced D8 model), using Cu Kα radiation (λ=1.5406Å). The size and morphology of the as-prepared Fe3O4 particles and the chemical composition of the prepared particles were characterized using transmission electron microscope, TEM, (Philips-EM-208S) and scanning electron microscope, SEM, (Seron Technology AIS 2100 (South Korea)) equipped EDXA instruments. Magnetic properties were analyzed using a vibrating sample magnetometer (VSM, Daghigh Meghnatis Kashan Co., Kashan, Iran). The specific surface areas of MNPs were determined by the BET method. Fourier-transform infrared (FTIR) spectroscopy analysis was performed with a Nicolet Impact 400D Model spectrophotometer (Nicolet Impact, Madison, USA). Instruments UV-Vis detection was carried out on a double beam UV-Vis spectrometer (Cintra 404, GBC).All electrochemical measurements including cyclic voltammetry (CV) and square wave voltammetry (SWV) were carried out on Metrohm 797VA instrument (Herisau, Switzerlan). A three-electrode conventional cell, including the modified MCPE as working electrode, a large surface area Pt plate (99.99%) as auxiliary electrode, and a Ag/AgCl (3 M KCl) electrode as reference, was used for electrochemical measurements. All experiments were carried out at room temperature.


## 3. Result and Discussion

### 3.1. Characterization ofFe3O4

The XRD spectrum of the as-preparedFe3O4 particles is shown in Figure 1(a). In the 2θ range of 20–70°, the peak positions at corresponding 2θ value are indexed as (2 0 0), (3 1 1), (4 0 0), (5 1 1), and (4 4 0), respectively [23]. It is demonstrated that no impurity peaks are detected and the high purity Fe3O4 spinel structure is synthesized. A particle diameter of about 12 nm was calculated according to Scherrer’s formula from the peak widths.Typical (a) XRD, (b) TEM, (c) SEM image, and hysteresis loop pattern (d) of as-prepared magnetite nanoparticles (MNPs). The scale bar in TEM and SEM image is 75 nm and 10μm, respectively.
(a)
(b)
(c)
(d)The size and morphology of as-prepared Fe3O4 particles were further examined by TEM and SEM, and magnetization was studied by VSM (Figures 1(b), 1(c), and 1(d), resp.). Figure 1(b) shows a typical TEM image of as-prepared Fe3O4 nanoparticles. As displayed, the particles exhibited spherical morphology but with small tendency to agglomeration. In general, magnetite nanoparticles that synthesized through the coprecipitation are usually agglomerate, that to achieve stable colloids and avoid agglomeration, the surface of magnetite nanoparticles precipitate can be modified by desired organic or inorganic modifiers. Consequently, a big agglomeration is predicted in the bulk Fe3O4 nanoparticles as displayed in the SEM image (Figure 1(b)). As can be seen from the SEM image, morphology of bulk Fe3O4 particles is irregular but their distribution is uniform. However, from TEM image, the average size of dispersed Fe3O4 MNPs was estimated about 9 nm. The specific surface area of Fe3O4 nanoparticles was 145 m2 g−1, which support nanosize of prepared Fe3O4 particles. The strong peaks for Fe and O were observed in the EDXA spectrum with atomic ratio of 1 : 1.3, which matches well with magnetite. The VSM magnetization of Fe3O4 nanoparticles at room temperature was recorded (Figure 1(d)). The results proved that the magnetic nanoparticles exhibited typical superparamagnetic behavior, characterized with strong magnetic susceptibility and no hysteresis, remanence, and coercivity (see Table SM1 in Supplementary Materials, containing complementary information of VSM and voltammetry, available online at http://dx.doi.org/10.1155/2013/803672). These results verified the successful synthesize of Fe3O4 magnetic nanoparticles and superparamagnetic behavior of them.


### 3.2. Electrochemical Characterization of the MCPE/MNP Electrode

Cyclic voltammetry can provide information on changes of electrode surfaces during modification processes. Figure2(a) presents the cyclic voltammograms for (A) the MCPE and (B) the MCPE/MNP electrodes in 0.1 M NaClO4 containing 0.5 mM [Fe(CN)6]3−/4− as a redox probe. An increase in faradaic current was observed for the MCPE/MNP electrode (Figure 2(a), curve (B)). The peak current of [Fe(CN)6]3−/4− at the MCPE/MNP electrode increased linearly with the square root of the scan rate over the range of 50–500 mV s−1 (Figure 2(b)); suggesting that the overall oxidation reduction of [Fe (CN)6]3−/4− at the modified electrode is controlled by the diffusion of [Fe(CN)6]3−/4− in solution. On the basis of this result, a surface area of 0.26 cm2 was calculated for the prepared MCPE/MNP electrode, using the Randle Sevcik equation [35]. By comparison of the surface area of the MCPE/MNP (0.26 cm2) with the MCPE (0.12 cm2), it is indicated that the increased faradaic current of the MCPE/MNP may be due to presence of nanometer sized Fe3O4 particles on the electrode surface (compare curves (A) and (B) in Figure 2(a)).(a) The cyclic voltammograms of (A) the MCPE and (B) the MCPE/MNP in a solution of 0.1 M NaClO4 containing 0.5 mM [Fe(CN)6]3−/4−, scan rate 100 mV s−1. (b) Linear relationship of ip and square root of scan rate (ν1/2) at the MCPE/MNP. Inset is the cyclic voltammograms of the MCPE/MNP in a solution of 0.1 M NaClO4 containing 0.5 mM [Fe(CN)6]3−/4− with different scan rates ((a)–(j): 50, 100, 150, 200, 250, 300, 350, 400, 450, and 500 mV s−1).
(a)
(b)Determination of the surface charge or surfacepKa has important significance in both theory and practice [36]. In this propose, several methods have been previously reviewed and adopted [37]. Amongst them, the electrochemical methods have been found to be the simplest and most convenient approaches for the determination of surface charge and surface pKa. Accordingly, the surface charge or surface pKa of the MCPE/MNP electrode was evaluated in a straightforward manner in this study using Faradaic current titration.We estimated the surfacepKa of the modified electrode using CV measurements, that is, faradaic current titration. The surface pKa of the MCPE/MNP electrode was estimated by recording cyclic voltammograms over a wide range of pH values (Figure 3(a)), and then monitoring ip as a function of pH. A value of 6.3±0.1 was obtained from the midpoint of the titration curve for the MCPE/MNP electrode (Figure 3(b)). This value is comparable with the pH value of 6.5 reported in the literature for the zero potential charge (ZPC) of Fe3O4 [38]. It means that in the pH region of above 6.5, the surface is negatively charged. Surface pKa is an essential quantity to estimate the charge-state of the surfaces and to explain the behavior of the modified electrodes towards charged probes or biological molecules like DA and AA.(a) The cyclic voltammograms obtained at the MCPE/MNP in 0.1 M PBS containing 0.1 M NaClO4 in the presence of 0.5 mM [Fe(CN)6]3-/4- at different pH. Outer to inner; pH 2.5, 3.0, 4.1, 4.6, 5.0, 5.5, 6.0, 6.5, 7.0, 7.5, 8.0, 8.5, 9.0, and 9.5. (b) Faradaic current titration curve for the MCPE/MNP (solid line) and its first derivative (dotted line), normalized ip is (ip(max)-ip)/ip(max).
(a)
(b)


### 3.3. Interaction of DA and AA with Fe3O4 MNP

The comparison of the cyclic voltammograms for the oxidation-reduction of AA, DA and a mixture of AA and DA at the MCPE and the MCPE/MNP electrodes showed that the presence of MNP on the MCPE electrode decreased the peak current and increased over potential for AA oxidation, increased the peak current and over potential for DA oxidation, and did not lead to peak separation in the oxidation potential of AA and DA (Supplementary Materials, FigureSM1 and Table SM2). Additionally, comparison of the SWVs for AA, DA, and a mixture of AA and DA showed no separation between their oxidation potentials. However, an interesting behavior was observed after incubation of the MCPE/MNP electrode in AA and DA. Figure 4 presents the electrochemical responses of the MCPE/MNP electrode in PBS (pH 7.0) after pre-concentration of the MCPE/MNP electrode in PBS (pH 7.0) containing 1.0×10-3 M AA (curve (B)) or 5.0×10-5 M DA (curve (C)) for 30 min. A sharp wave with a high peak current due to DA oxidation was observed at the MCPE/MNP electrode; however, the same wave was not observed for AA. This behavior is due to the adsorption of DA to Fe3O4 NPs and allows us to present a selective sensor for DA based on strategy (ii).Figure 4
The square wave voltammograms obtained on the MCPE/MNP in PBS, DA free, pH 7.0, and 0.1 M NaClO4 after 30 min pre-concentration in PBS (pH 7.0) containing (B) 1.0×10-3 M AA, (C) 5.0×10-5 M DA. Curve (A) was obtained from blank solution.Further studies were performed to verify the adsorption between DA and MNPs. The peak current for the oxidation of pre-concentrated DA on the MCPE/MNP electrode increased linearly with the scan rate over the range of 50–400 mV s−1 (Figure 5). This suggests that the overall oxidation/reduction of DA at the modified electrode is controlled by an adsorption phenomenon.Figure 5
Linear relationship ofip of DA oxidation/reduction and scan rate (ν) at the MCPE/MNP. Inset is the cyclic voltammograms of the MCPE/MNP in PBS, DA free, pH 7.0, and 0.1 M NaClO4 after 30 min pre-concentration in PBS (pH 7.0) containing 1 mM DA with different scan rates ((a)–(g): 50, 100, 150, 250, 300, 450, and 500 mV s−1).Our literature survey reviled some reports on the attachment of DA as a robust anchor to immobilize functional molecules on MNPs by sonication of the DA and MNPs during 30 min [27–31]. Thus, the adsorption of DA on MNPs without sonication was compared to the reported sonication route. Therefore, 200 mL of 0.1 M PBS (pH 7.0) containing 1.0×10-3 M DA was (a) stirred with 200 mg MNPs for 30 min to form MNP/DA (stirred) or (b) sonicated with 200 mg MNPs for 30 min to form MNP/DA (sonicated). The resulting MNP/DA was removed, washed several times, and then compared via FTIR spectroscopy (Figure 6).(a) Typical FTIR spectrum of the MNPs (A),MNP/DA(stirred) (B), and MNP/DA(sonicated) (C). MNP/DA(stirred); stirred 200 mg MNPs for 30 min in 200 mL PBS, pH=7.0, containing 1.0×10-3 M DA. MNP/DA(sonicated); sonicated 200 mg MNPs for 30 min in 200 mL PBS, pH=7.0, containing 1.0×10-3 M of DA. (b) UV-Vis spectrums of Fe3O4 MNPs (A), Fe3O4/DA (B) and DA molecule (C).
(a)
(b)Comparison of the FTIR spectrums of DA-coated particles and naked MNP (Figure6(a)) demonstrated the weak, wide absorption peaks at approximately 1090–1700 cm−1 in spectra (b) and (c) which could be attributed to vibration of the C–O bond in Fe3O4/DA. This feature was not observed in pure Fe3O4 MNPs (spectrum A). The absorption peak at 580 cm−1 was attributed to Fe–O vibration in unmodified Fe3O4 MNP and modified MNP in both route. However, the absorption peaks of MNP/DA (stirred or sonicated) were slightly wider than pure Fe3O4. It demonstrates that the vibration of the Fe–O bond was altered in DA-modified Fe3O4, and indicates that the DA bonded to the surface of Fe3O4 MNPs via a Fe–O–C bond in both route. Figure 6(b) shows the UV-Vis spectrums of Fe3O4 MNPs (A), Fe3O4/DA (B), and DA molecule (C). No absorption peaks were observed for the bare Fe3O4 (curve (A)). When DA was attached onto Fe3O4, a sharp absorption peak and another relatively broad peak were observed at 210 and 285 nm, respectively (curve (B)). Compared to the spectra of pure DA (curve (C)), the deviation of the DA absorption wavelength could be ascribed to the interaction of Fe3O4 with DA molecules. The same results also are recently reported by Li et al. [39]. The obtained results demonstrate the successful attachment of DA onto the Fe3O4 MNPs.Mechanism of selective adsorption of DA ontoFe3O4 MNPs surface can explicate by recent reports of Chen et al. [40]. They report that DA has ability to convert the coordinatively unsaturated iron surface sites back into a bulk-like lattice structure with an octahedral geometry for the oxygen-coordinated iron centers, resulting in tight binding of DA to iron oxide, in compared to AA without diol on benzene ring, which caused to selectivity of the MCPE/MNPs toward DA.


### 3.4. Optimization of the Adsorption Condition

#### 3.4.1. pH

DA (pKa=8.9) exhibits a different charge depending on its pH [1], and as shown in this work MNP (surface pKa of 6.3±0.1) also, the interaction of MNPs with DA is influenced by the pH of the solution. Therefore, studying the pH effect on their interaction was a critical step in the current work. The pH effect was investigated in a 0.1 M PBS containing 5.0×10-5 M of DA for 30 min pre-concentration time. Optimal conditions for pre-concentration and stripping steps were achieved around a pH of 7.0 (Figure 7(a)).Response of the MCPE/MNP as a function of (a) pH, (b) pre-concentration time, and (c) amount of MNPs. Pre-concentration conditions: PBS (pH 7.0) containing5.0×10-5 M DA at the open-circuit potential. Measurement conditions, SWV in PBS, DA free, pH 7.0, and 0.1 M NaClO4.
(a)
(b)
(c)


#### 3.4.2. Pre-Concentration Time

The dependence of the anodic stripping peak current on the pre-concentration time at the MCPE/MNP electrodes was also studied. The MCPE/MNP electrodes were immersed in 0.1 M PBS atpH=7.0, containing 5.0×10-5 M of DA stirred solution for different time periods. The peak current was increased as a function of pre-concentration time and the asymptotic value was reached within 20 min (Figure 7(b)).


#### 3.4.3. Amount of MNP

The MCPE/MNP electrode response to adsorbed DAs was dependent on the amount of MNPs that were casted on the MCPE. Therefore, different amounts of MNPs (differentμL of the homogenized 10 mg mL−1 MNPs suspension) were casted on the MCPE and its SWV response in PBS (pH=7.0), DA free, after pre-concentration in 0.1 M PBS at pH = 7.0, containing 5.0×10-5 M of DA for 20 min, was recorded. As evident from Figure 7(c), higher response was observed for 6 μL (60 μg) of MNPs suspension.


### 3.5. Optimization of Instrumental Parameters

The peak current of square wave voltammograms is also dependent on instrumental parameters. The instrumental parameters are interrelated and can be optimized by monitoring of the peak current as a function of studying parameter values, while other parameters are fixed. After a careful examination, the setting of pulse height (10 mV), square wave amplitude (50 mV), and square wave frequency (40 Hz) were found as optimized values for instrumental parameters.


### 3.6. Calibration and Detection Limit

The calibration curve (Figure8, inset) was obtained under optimized conditions by systematically increasing the concentration of DA from 5.0×10-6 to 1.0×10-3 M in pre-concentration solution containing 1.0×10-3 M AA (PBS, pH=7.0) and by monitoring the response of the MCPE/MNP electrode in determination solution by SWV {(ip-ipb)/μA=100.1(±1.123)/μA+18.62(±0.271)log([DA]/M), r2=0.999}. The detection limit of this electrode, calculated from the standard deviation of the background (signal equals 3δ of the background noise), is 7.6×10-7 M DA, with a relative standard deviation of 4.6% (n=5) for 5.0×10-5 M DA. The reproducibility of the MCPE/MNP electrode was evaluated by RSD, n=5, of the DA with different electrodes. The RSD of 5.0% was obtained at 5.0×10-5 M DA. These results indicated the good and acceptable reproducibility and repeatability of the MCPE/MNP electrode.Figure 8
The square wave voltammograms obtained on the MCPE/MNP in PBS, DA free, pH 7.0, and 0.1 M NaClO4 after 20 min pre-concentration in PBS (pH 7.0) containing 1.0×10-3 M AA and different concentrations of DA; bottom to top: 0.0, 5.0×10-6, 1.0×10-5, 2.0×10-5, 5.0×10-5, 1.0×10-4, 2.0×10-4, 4.0×10-4, 5.0×10-4, and 1.0×10-3 M DA. SWV conditions were as; pulse height (10 mV), square wave amplitude (50 mV), and square wave frequency (40 Hz). Inset is calibration curve {(ip-ipb)/μA=100.1(±1.123)/μA+18.62(±0.271)log([DA]/M), r2=0.999} obtained from variation of the SWV anodic peak current as a function of DA concentration. (ipb; anodic peak current of blank).The interday and intraday stability of the MCPE/MNP electrode was assessed by determination of5.0×10-5 M DA. The inter-day stability of our proposed method was detected by using a prepared MCPE/MNP electrode with three different days in a week. The RSD of inter-day stability was obtained as 4.8%. Similarly, the intra-day stability was evaluated from the response to the same prepared MCPE/MNP electrode and detected three times every day. The RSD of intra-day was obtained 5.7%, 6.1%, and 5.8%, respectively. Thus, the inter-day and intra-day stabilities of the modified electrode were acceptable.The interference of a few common interferes was investigated in the presence of1.0×10-3 M DA. Na+, Ca2+, Mg2+, glucose and sucrose in 500-fold, and AA in 10-fold of the DA concentration did not change the signal of SWV. However, based on mentioned interaction mechanism between Fe3O4 MNPs and diol on benzene ring of DA molecule, there is a possibility of the same behavior for other catechols compounds like norepinephrine, methyldopa, and epinephrine. We investigated interaction of epinephrine as one of the important interferes of DA, with MCPE/MNPs electrode, and the same adsorption behavior was observed for it, but with totally different oxidation potential (0.4 V) in comparison to DA (0.2 V). This result showed that proposed modified electrode may be suitable for catechol derivative distinguishing. However, the aim of this work was study of the selectivity of Fe3O4 MNPs toward DA and AA, and its interaction with other catechols not intended here.On the other hand, a literature survey reviled that there is a similar report on application of Fe3O4 MNP in voltammetric sensing of DA by using a gold electrode [26]. But there are distinct differences between our work and previous papers. In the previous reports, the dopamine determination was done based on the diffusion current of DA oxidation at the modified electrode, not based on pre-concentration of DA on top of the modified electrode (our method). The premier advantage of our work is high selectivity of our method to detection of dopamine against AA. Furthermore, our investigation showed if determination was done based on diffusion current, a fouling effect was observed due to oxidation products on the electrode surface (Supplementary Materials, Figure SM2.). Finally, the observed results are not only important in view of analytical chemistry but also are critical in view point of MNP modification. Because our results showed that there is a simple approach for amination of MNP via attachment of DA to MNP (Fe3O4).


### 3.7. Analytical Performance for Determination of DA in Pharmaceutical Sample

The proposed sensor was tested for determination of DA in dopamine hydrochloride injection samples. Pharmaceutical samples were prepared and adjusted to5.0×10-6 M DA, in 0.1 M PBS, pH 7.0, by dilution of DOPADIC ampoule contents (5 mL of 200 mg mL−1 DA hydrochloride injection solution). The standard additions of DA were done by addition of different concentrations of DA to this sample. After pre-concentration of the MCPE/MNP electrode in these solutions, the square wave voltammograms were recorded (displayed in Figure 9, inset). The anodic peak currents were extracted and plotted versus DA concentration. A linear relation {ip/μA=102.2(±6.543)/μA+19.39(±1.560)log([DA]/M), r2=0.997} was found from variations of ip versus DA concentrations (Figure 9). Obtained result (5.3×10-6 M DA) was in good agreement with the value of dopamine hydrochloride in diluted sample, RSD≅7.2%.Figure 9
Calibration curve{ip/μA=102.2(±6.543)/μA+19.39(±1.560)log([DA]/M), r2=0.997} obtained from variation of the SWV anodic peak current as a function of DA concentration in standard addition solutions. Inset shows square wave voltammograms obtained on the MCPE/MNP in 5.0×10-6 M DOPADIC solution prepared by standard addition method, inner to outer; 1.0×10-5, 5.0×10-5, 1.0×10-4, and 5.0×10-4 M DA. Conditions are the same as in Figure 8.


## 3.1. Characterization ofFe3O4

The XRD spectrum of the as-preparedFe3O4 particles is shown in Figure 1(a). In the 2θ range of 20–70°, the peak positions at corresponding 2θ value are indexed as (2 0 0), (3 1 1), (4 0 0), (5 1 1), and (4 4 0), respectively [23]. It is demonstrated that no impurity peaks are detected and the high purity Fe3O4 spinel structure is synthesized. A particle diameter of about 12 nm was calculated according to Scherrer’s formula from the peak widths.Typical (a) XRD, (b) TEM, (c) SEM image, and hysteresis loop pattern (d) of as-prepared magnetite nanoparticles (MNPs). The scale bar in TEM and SEM image is 75 nm and 10μm, respectively.
(a)
(b)
(c)
(d)The size and morphology of as-prepared Fe3O4 particles were further examined by TEM and SEM, and magnetization was studied by VSM (Figures 1(b), 1(c), and 1(d), resp.). Figure 1(b) shows a typical TEM image of as-prepared Fe3O4 nanoparticles. As displayed, the particles exhibited spherical morphology but with small tendency to agglomeration. In general, magnetite nanoparticles that synthesized through the coprecipitation are usually agglomerate, that to achieve stable colloids and avoid agglomeration, the surface of magnetite nanoparticles precipitate can be modified by desired organic or inorganic modifiers. Consequently, a big agglomeration is predicted in the bulk Fe3O4 nanoparticles as displayed in the SEM image (Figure 1(b)). As can be seen from the SEM image, morphology of bulk Fe3O4 particles is irregular but their distribution is uniform. However, from TEM image, the average size of dispersed Fe3O4 MNPs was estimated about 9 nm. The specific surface area of Fe3O4 nanoparticles was 145 m2 g−1, which support nanosize of prepared Fe3O4 particles. The strong peaks for Fe and O were observed in the EDXA spectrum with atomic ratio of 1 : 1.3, which matches well with magnetite. The VSM magnetization of Fe3O4 nanoparticles at room temperature was recorded (Figure 1(d)). The results proved that the magnetic nanoparticles exhibited typical superparamagnetic behavior, characterized with strong magnetic susceptibility and no hysteresis, remanence, and coercivity (see Table SM1 in Supplementary Materials, containing complementary information of VSM and voltammetry, available online at http://dx.doi.org/10.1155/2013/803672). These results verified the successful synthesize of Fe3O4 magnetic nanoparticles and superparamagnetic behavior of them.


## 3.2. Electrochemical Characterization of the MCPE/MNP Electrode

Cyclic voltammetry can provide information on changes of electrode surfaces during modification processes. Figure2(a) presents the cyclic voltammograms for (A) the MCPE and (B) the MCPE/MNP electrodes in 0.1 M NaClO4 containing 0.5 mM [Fe(CN)6]3−/4− as a redox probe. An increase in faradaic current was observed for the MCPE/MNP electrode (Figure 2(a), curve (B)). The peak current of [Fe(CN)6]3−/4− at the MCPE/MNP electrode increased linearly with the square root of the scan rate over the range of 50–500 mV s−1 (Figure 2(b)); suggesting that the overall oxidation reduction of [Fe (CN)6]3−/4− at the modified electrode is controlled by the diffusion of [Fe(CN)6]3−/4− in solution. On the basis of this result, a surface area of 0.26 cm2 was calculated for the prepared MCPE/MNP electrode, using the Randle Sevcik equation [35]. By comparison of the surface area of the MCPE/MNP (0.26 cm2) with the MCPE (0.12 cm2), it is indicated that the increased faradaic current of the MCPE/MNP may be due to presence of nanometer sized Fe3O4 particles on the electrode surface (compare curves (A) and (B) in Figure 2(a)).(a) The cyclic voltammograms of (A) the MCPE and (B) the MCPE/MNP in a solution of 0.1 M NaClO4 containing 0.5 mM [Fe(CN)6]3−/4−, scan rate 100 mV s−1. (b) Linear relationship of ip and square root of scan rate (ν1/2) at the MCPE/MNP. Inset is the cyclic voltammograms of the MCPE/MNP in a solution of 0.1 M NaClO4 containing 0.5 mM [Fe(CN)6]3−/4− with different scan rates ((a)–(j): 50, 100, 150, 200, 250, 300, 350, 400, 450, and 500 mV s−1).
(a)
(b)Determination of the surface charge or surfacepKa has important significance in both theory and practice [36]. In this propose, several methods have been previously reviewed and adopted [37]. Amongst them, the electrochemical methods have been found to be the simplest and most convenient approaches for the determination of surface charge and surface pKa. Accordingly, the surface charge or surface pKa of the MCPE/MNP electrode was evaluated in a straightforward manner in this study using Faradaic current titration.We estimated the surfacepKa of the modified electrode using CV measurements, that is, faradaic current titration. The surface pKa of the MCPE/MNP electrode was estimated by recording cyclic voltammograms over a wide range of pH values (Figure 3(a)), and then monitoring ip as a function of pH. A value of 6.3±0.1 was obtained from the midpoint of the titration curve for the MCPE/MNP electrode (Figure 3(b)). This value is comparable with the pH value of 6.5 reported in the literature for the zero potential charge (ZPC) of Fe3O4 [38]. It means that in the pH region of above 6.5, the surface is negatively charged. Surface pKa is an essential quantity to estimate the charge-state of the surfaces and to explain the behavior of the modified electrodes towards charged probes or biological molecules like DA and AA.(a) The cyclic voltammograms obtained at the MCPE/MNP in 0.1 M PBS containing 0.1 M NaClO4 in the presence of 0.5 mM [Fe(CN)6]3-/4- at different pH. Outer to inner; pH 2.5, 3.0, 4.1, 4.6, 5.0, 5.5, 6.0, 6.5, 7.0, 7.5, 8.0, 8.5, 9.0, and 9.5. (b) Faradaic current titration curve for the MCPE/MNP (solid line) and its first derivative (dotted line), normalized ip is (ip(max)-ip)/ip(max).
(a)
(b)


## 3.3. Interaction of DA and AA with Fe3O4 MNP

The comparison of the cyclic voltammograms for the oxidation-reduction of AA, DA and a mixture of AA and DA at the MCPE and the MCPE/MNP electrodes showed that the presence of MNP on the MCPE electrode decreased the peak current and increased over potential for AA oxidation, increased the peak current and over potential for DA oxidation, and did not lead to peak separation in the oxidation potential of AA and DA (Supplementary Materials, FigureSM1 and Table SM2). Additionally, comparison of the SWVs for AA, DA, and a mixture of AA and DA showed no separation between their oxidation potentials. However, an interesting behavior was observed after incubation of the MCPE/MNP electrode in AA and DA. Figure 4 presents the electrochemical responses of the MCPE/MNP electrode in PBS (pH 7.0) after pre-concentration of the MCPE/MNP electrode in PBS (pH 7.0) containing 1.0×10-3 M AA (curve (B)) or 5.0×10-5 M DA (curve (C)) for 30 min. A sharp wave with a high peak current due to DA oxidation was observed at the MCPE/MNP electrode; however, the same wave was not observed for AA. This behavior is due to the adsorption of DA to Fe3O4 NPs and allows us to present a selective sensor for DA based on strategy (ii).Figure 4
The square wave voltammograms obtained on the MCPE/MNP in PBS, DA free, pH 7.0, and 0.1 M NaClO4 after 30 min pre-concentration in PBS (pH 7.0) containing (B) 1.0×10-3 M AA, (C) 5.0×10-5 M DA. Curve (A) was obtained from blank solution.Further studies were performed to verify the adsorption between DA and MNPs. The peak current for the oxidation of pre-concentrated DA on the MCPE/MNP electrode increased linearly with the scan rate over the range of 50–400 mV s−1 (Figure 5). This suggests that the overall oxidation/reduction of DA at the modified electrode is controlled by an adsorption phenomenon.Figure 5
Linear relationship ofip of DA oxidation/reduction and scan rate (ν) at the MCPE/MNP. Inset is the cyclic voltammograms of the MCPE/MNP in PBS, DA free, pH 7.0, and 0.1 M NaClO4 after 30 min pre-concentration in PBS (pH 7.0) containing 1 mM DA with different scan rates ((a)–(g): 50, 100, 150, 250, 300, 450, and 500 mV s−1).Our literature survey reviled some reports on the attachment of DA as a robust anchor to immobilize functional molecules on MNPs by sonication of the DA and MNPs during 30 min [27–31]. Thus, the adsorption of DA on MNPs without sonication was compared to the reported sonication route. Therefore, 200 mL of 0.1 M PBS (pH 7.0) containing 1.0×10-3 M DA was (a) stirred with 200 mg MNPs for 30 min to form MNP/DA (stirred) or (b) sonicated with 200 mg MNPs for 30 min to form MNP/DA (sonicated). The resulting MNP/DA was removed, washed several times, and then compared via FTIR spectroscopy (Figure 6).(a) Typical FTIR spectrum of the MNPs (A),MNP/DA(stirred) (B), and MNP/DA(sonicated) (C). MNP/DA(stirred); stirred 200 mg MNPs for 30 min in 200 mL PBS, pH=7.0, containing 1.0×10-3 M DA. MNP/DA(sonicated); sonicated 200 mg MNPs for 30 min in 200 mL PBS, pH=7.0, containing 1.0×10-3 M of DA. (b) UV-Vis spectrums of Fe3O4 MNPs (A), Fe3O4/DA (B) and DA molecule (C).
(a)
(b)Comparison of the FTIR spectrums of DA-coated particles and naked MNP (Figure6(a)) demonstrated the weak, wide absorption peaks at approximately 1090–1700 cm−1 in spectra (b) and (c) which could be attributed to vibration of the C–O bond in Fe3O4/DA. This feature was not observed in pure Fe3O4 MNPs (spectrum A). The absorption peak at 580 cm−1 was attributed to Fe–O vibration in unmodified Fe3O4 MNP and modified MNP in both route. However, the absorption peaks of MNP/DA (stirred or sonicated) were slightly wider than pure Fe3O4. It demonstrates that the vibration of the Fe–O bond was altered in DA-modified Fe3O4, and indicates that the DA bonded to the surface of Fe3O4 MNPs via a Fe–O–C bond in both route. Figure 6(b) shows the UV-Vis spectrums of Fe3O4 MNPs (A), Fe3O4/DA (B), and DA molecule (C). No absorption peaks were observed for the bare Fe3O4 (curve (A)). When DA was attached onto Fe3O4, a sharp absorption peak and another relatively broad peak were observed at 210 and 285 nm, respectively (curve (B)). Compared to the spectra of pure DA (curve (C)), the deviation of the DA absorption wavelength could be ascribed to the interaction of Fe3O4 with DA molecules. The same results also are recently reported by Li et al. [39]. The obtained results demonstrate the successful attachment of DA onto the Fe3O4 MNPs.Mechanism of selective adsorption of DA ontoFe3O4 MNPs surface can explicate by recent reports of Chen et al. [40]. They report that DA has ability to convert the coordinatively unsaturated iron surface sites back into a bulk-like lattice structure with an octahedral geometry for the oxygen-coordinated iron centers, resulting in tight binding of DA to iron oxide, in compared to AA without diol on benzene ring, which caused to selectivity of the MCPE/MNPs toward DA.


## 3.4. Optimization of the Adsorption Condition

### 3.4.1. pH

DA (pKa=8.9) exhibits a different charge depending on its pH [1], and as shown in this work MNP (surface pKa of 6.3±0.1) also, the interaction of MNPs with DA is influenced by the pH of the solution. Therefore, studying the pH effect on their interaction was a critical step in the current work. The pH effect was investigated in a 0.1 M PBS containing 5.0×10-5 M of DA for 30 min pre-concentration time. Optimal conditions for pre-concentration and stripping steps were achieved around a pH of 7.0 (Figure 7(a)).Response of the MCPE/MNP as a function of (a) pH, (b) pre-concentration time, and (c) amount of MNPs. Pre-concentration conditions: PBS (pH 7.0) containing5.0×10-5 M DA at the open-circuit potential. Measurement conditions, SWV in PBS, DA free, pH 7.0, and 0.1 M NaClO4.
(a)
(b)
(c)


### 3.4.2. Pre-Concentration Time

The dependence of the anodic stripping peak current on the pre-concentration time at the MCPE/MNP electrodes was also studied. The MCPE/MNP electrodes were immersed in 0.1 M PBS atpH=7.0, containing 5.0×10-5 M of DA stirred solution for different time periods. The peak current was increased as a function of pre-concentration time and the asymptotic value was reached within 20 min (Figure 7(b)).


### 3.4.3. Amount of MNP

The MCPE/MNP electrode response to adsorbed DAs was dependent on the amount of MNPs that were casted on the MCPE. Therefore, different amounts of MNPs (differentμL of the homogenized 10 mg mL−1 MNPs suspension) were casted on the MCPE and its SWV response in PBS (pH=7.0), DA free, after pre-concentration in 0.1 M PBS at pH = 7.0, containing 5.0×10-5 M of DA for 20 min, was recorded. As evident from Figure 7(c), higher response was observed for 6 μL (60 μg) of MNPs suspension.


## 3.4.1. pH

DA (pKa=8.9) exhibits a different charge depending on its pH [1], and as shown in this work MNP (surface pKa of 6.3±0.1) also, the interaction of MNPs with DA is influenced by the pH of the solution. Therefore, studying the pH effect on their interaction was a critical step in the current work. The pH effect was investigated in a 0.1 M PBS containing 5.0×10-5 M of DA for 30 min pre-concentration time. Optimal conditions for pre-concentration and stripping steps were achieved around a pH of 7.0 (Figure 7(a)).Response of the MCPE/MNP as a function of (a) pH, (b) pre-concentration time, and (c) amount of MNPs. Pre-concentration conditions: PBS (pH 7.0) containing5.0×10-5 M DA at the open-circuit potential. Measurement conditions, SWV in PBS, DA free, pH 7.0, and 0.1 M NaClO4.
(a)
(b)
(c)


## 3.4.2. Pre-Concentration Time

The dependence of the anodic stripping peak current on the pre-concentration time at the MCPE/MNP electrodes was also studied. The MCPE/MNP electrodes were immersed in 0.1 M PBS atpH=7.0, containing 5.0×10-5 M of DA stirred solution for different time periods. The peak current was increased as a function of pre-concentration time and the asymptotic value was reached within 20 min (Figure 7(b)).


## 3.4.3. Amount of MNP

The MCPE/MNP electrode response to adsorbed DAs was dependent on the amount of MNPs that were casted on the MCPE. Therefore, different amounts of MNPs (differentμL of the homogenized 10 mg mL−1 MNPs suspension) were casted on the MCPE and its SWV response in PBS (pH=7.0), DA free, after pre-concentration in 0.1 M PBS at pH = 7.0, containing 5.0×10-5 M of DA for 20 min, was recorded. As evident from Figure 7(c), higher response was observed for 6 μL (60 μg) of MNPs suspension.


## 3.5. Optimization of Instrumental Parameters

The peak current of square wave voltammograms is also dependent on instrumental parameters. The instrumental parameters are interrelated and can be optimized by monitoring of the peak current as a function of studying parameter values, while other parameters are fixed. After a careful examination, the setting of pulse height (10 mV), square wave amplitude (50 mV), and square wave frequency (40 Hz) were found as optimized values for instrumental parameters.


## 3.6. Calibration and Detection Limit

The calibration curve (Figure8, inset) was obtained under optimized conditions by systematically increasing the concentration of DA from 5.0×10-6 to 1.0×10-3 M in pre-concentration solution containing 1.0×10-3 M AA (PBS, pH=7.0) and by monitoring the response of the MCPE/MNP electrode in determination solution by SWV {(ip-ipb)/μA=100.1(±1.123)/μA+18.62(±0.271)log([DA]/M), r2=0.999}. The detection limit of this electrode, calculated from the standard deviation of the background (signal equals 3δ of the background noise), is 7.6×10-7 M DA, with a relative standard deviation of 4.6% (n=5) for 5.0×10-5 M DA. The reproducibility of the MCPE/MNP electrode was evaluated by RSD, n=5, of the DA with different electrodes. The RSD of 5.0% was obtained at 5.0×10-5 M DA. These results indicated the good and acceptable reproducibility and repeatability of the MCPE/MNP electrode.Figure 8
The square wave voltammograms obtained on the MCPE/MNP in PBS, DA free, pH 7.0, and 0.1 M NaClO4 after 20 min pre-concentration in PBS (pH 7.0) containing 1.0×10-3 M AA and different concentrations of DA; bottom to top: 0.0, 5.0×10-6, 1.0×10-5, 2.0×10-5, 5.0×10-5, 1.0×10-4, 2.0×10-4, 4.0×10-4, 5.0×10-4, and 1.0×10-3 M DA. SWV conditions were as; pulse height (10 mV), square wave amplitude (50 mV), and square wave frequency (40 Hz). Inset is calibration curve {(ip-ipb)/μA=100.1(±1.123)/μA+18.62(±0.271)log([DA]/M), r2=0.999} obtained from variation of the SWV anodic peak current as a function of DA concentration. (ipb; anodic peak current of blank).The interday and intraday stability of the MCPE/MNP electrode was assessed by determination of5.0×10-5 M DA. The inter-day stability of our proposed method was detected by using a prepared MCPE/MNP electrode with three different days in a week. The RSD of inter-day stability was obtained as 4.8%. Similarly, the intra-day stability was evaluated from the response to the same prepared MCPE/MNP electrode and detected three times every day. The RSD of intra-day was obtained 5.7%, 6.1%, and 5.8%, respectively. Thus, the inter-day and intra-day stabilities of the modified electrode were acceptable.The interference of a few common interferes was investigated in the presence of1.0×10-3 M DA. Na+, Ca2+, Mg2+, glucose and sucrose in 500-fold, and AA in 10-fold of the DA concentration did not change the signal of SWV. However, based on mentioned interaction mechanism between Fe3O4 MNPs and diol on benzene ring of DA molecule, there is a possibility of the same behavior for other catechols compounds like norepinephrine, methyldopa, and epinephrine. We investigated interaction of epinephrine as one of the important interferes of DA, with MCPE/MNPs electrode, and the same adsorption behavior was observed for it, but with totally different oxidation potential (0.4 V) in comparison to DA (0.2 V). This result showed that proposed modified electrode may be suitable for catechol derivative distinguishing. However, the aim of this work was study of the selectivity of Fe3O4 MNPs toward DA and AA, and its interaction with other catechols not intended here.On the other hand, a literature survey reviled that there is a similar report on application of Fe3O4 MNP in voltammetric sensing of DA by using a gold electrode [26]. But there are distinct differences between our work and previous papers. In the previous reports, the dopamine determination was done based on the diffusion current of DA oxidation at the modified electrode, not based on pre-concentration of DA on top of the modified electrode (our method). The premier advantage of our work is high selectivity of our method to detection of dopamine against AA. Furthermore, our investigation showed if determination was done based on diffusion current, a fouling effect was observed due to oxidation products on the electrode surface (Supplementary Materials, Figure SM2.). Finally, the observed results are not only important in view of analytical chemistry but also are critical in view point of MNP modification. Because our results showed that there is a simple approach for amination of MNP via attachment of DA to MNP (Fe3O4).


## 3.7. Analytical Performance for Determination of DA in Pharmaceutical Sample

The proposed sensor was tested for determination of DA in dopamine hydrochloride injection samples. Pharmaceutical samples were prepared and adjusted to5.0×10-6 M DA, in 0.1 M PBS, pH 7.0, by dilution of DOPADIC ampoule contents (5 mL of 200 mg mL−1 DA hydrochloride injection solution). The standard additions of DA were done by addition of different concentrations of DA to this sample. After pre-concentration of the MCPE/MNP electrode in these solutions, the square wave voltammograms were recorded (displayed in Figure 9, inset). The anodic peak currents were extracted and plotted versus DA concentration. A linear relation {ip/μA=102.2(±6.543)/μA+19.39(±1.560)log([DA]/M), r2=0.997} was found from variations of ip versus DA concentrations (Figure 9). Obtained result (5.3×10-6 M DA) was in good agreement with the value of dopamine hydrochloride in diluted sample, RSD≅7.2%.Figure 9
Calibration curve{ip/μA=102.2(±6.543)/μA+19.39(±1.560)log([DA]/M), r2=0.997} obtained from variation of the SWV anodic peak current as a function of DA concentration in standard addition solutions. Inset shows square wave voltammograms obtained on the MCPE/MNP in 5.0×10-6 M DOPADIC solution prepared by standard addition method, inner to outer; 1.0×10-5, 5.0×10-5, 1.0×10-4, and 5.0×10-4 M DA. Conditions are the same as in Figure 8.


## 4. Conclusion

Here,Fe3O4 superparamagnetic iron oxide nanoparticles were successfully synthesized via coprecipitation method and characterized. Then a simple magnetic carbon paste electrode was modified with the magnetic nanoparticles, MCPE/MNP, and characterized by electrochemical methods in the presence of [Fe(CN)6]3−/4− as a redox probe. Surface pKa of the MCPE/MNP was evaluated as 6.3±0.1 by using Faradaic current titration method. Interaction of the MCPE/MNP with DA was investigated, and the results proved an adsorption behavior between Fe3O4 and DA. Based on this behavior, a calibration curve from 5.0×10-6 to 1.0×10-3 M DA with correlation coefficients of 0.999 and a detection limit of 7.6×10-7 M DA was constructed by using the MCPE/MNP. The MCPE/MNP showed good selectivity, reproducibility, and stability for the detection of trace DA, especially in the presence of AA. Another challenge is that this modified MNP (MNP/DA), with amine end functional group, could be further modified by large molecular complexing agents for sensor and clinical application or radiolabeling; this work is in progress.



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*Source: 803672-2013-09-30.xml*