Open Access

Thiosemicarbazide derivative-functionalized carbon nanotube for simultaneous determination of isoprenaline and piroxicam

  • Mohammad Mazloum‐Ardakani1Email author,
  • Hamideh Mohammadian-Sarcheshmeh1,
  • Alireza Khoshroo1 and
  • Mohammad Abdollahi-Alibeik1
Journal of Analytical Science and Technology20178:6

DOI: 10.1186/s40543-017-0115-z

Received: 30 September 2016

Accepted: 9 March 2017

Published: 12 April 2017

Abstract

Background

Piroxicam (PX) is a nonsteroidal anti-inflammatory drug of the oxicam category that has been known worth as a chemopreventative, anti-tumor agent, for acute and chronic musculoskeletal. To the best of our knowledge, no paper has been published until now reporting the simultaneous electrocatalytic detection of isoprenaline and PX by using any type of modified electrodes.

Methods

The glassy carbon electrode modified with multiwalled carbon nanotubes chemically modified with (z)-1-(3,4-dihydroxybenzylidene)-2-methylthiosemicarbazide (DBT–CNT/GCE). The electrocatalytic behavior of analytes was examined using cyclic voltammetry (CV), chronoamperometry, and differential pulse voltammetry (DPV) on the modified electrode.

Results

In order to determine kinetic parameters such as the anodic transfer coefficient (α = 0.47) and the electron transfer rate constant between the nanocomposite and glassy carbon electrode (ks/s = 0.51), cyclic voltammetry was applied. The results represented a linear relationship versus isoprenaline concentrations in the wide range of 0.5–1500.0 μM and a detection limit of 0.35 μM. Furthermore, DPV was applied successfully for the simultaneous determination of isoprenaline and piroxicam.

Conclusions

This proposed sensor has been successfully applied to determine the IP and PX in blood serum human, which demonstrates that it has excellent potential application for detection of different concentrations of IP and PX.

Keywords

Isoprenaline Piroxicam Functionalized carbon nanotube Thiosemicarbazide

Background

Carbon nanotubes have gotten a great deal of attention in all around the world due to their prominent mechanical, structural, and electronic properties. The newly developed chemical methods for chemical functionalization of carbon nanotubes, specially modification techniques, permit variation of the electronic properties of the tubes, as well as chemical surface properties. These functionalized carbon nanotubes have provided an extensive range of new applications such as nanostructured electronic devices, chemical sensors, and electrochemical sensors (Balasubramanian and Burghard 2005; Mazloum-Ardakani et al. 2014; Mazloum-Ardakani et al. 2013). In addition, functionalized carbon nanotubes were used in the construction of polymeric carbon nanocomposites, the combination with biological species, and the probing of nanotube molecule interactions (Sun et al. 2002).

It is important to know that carbon nanotubes (CNTs) usually are agglomerates of several hundred micrometers in size (Wang et al. 2003). These entanglements cause nanotubes to disperse in polymer matrix difficultly. Therefore, it is essential that alter the chemical nature of the nanotube surface. Solution processing has been performed in the construction of the well-dispersed carbon nanotube composites. Nevertheless, it is difficult to attain homogeneous dispersion of nanotubes in polymer matrix, owing to the fact that carbon nanotubes are bundled and insoluble. Chemical functionalization of the CNT surface raises interfacial interaction between CNTs and the polymer matrix, increases adhesion of them in different polymers and organic solvents, decreases agglomeration, and improves dispersion (Andrews and Weisenberger 2004). The enhanced interactions between CNTs and the polymer matrix improve the load transfer from the polymer to the nanotubes. Acid treatment of the nanotube is an important technique to chemical functionalization. It produces functional groups on sidewalls or open ends of nanotubes, removes catalytic impurities, and simplifies dispersion of CNTs in various solutions or melts. Also, the amine treatment and heat treatment are usually used for chemical functionalization of carbon nanotubes (Lee et al. 2007).

Researchers have used another type of classification for functionalization methods. These are various covalent and noncovalent functionalization methods for chemical modification and solubilization of single-walled (SWNT) and multiwalled (MWNT) carbon nanotubes (Bahr and Tour 2001; Chen et al. 2001a; Georgakilas et al. 2002; Holzinger et al. 2001; Huang et al. 2003; Jin et al. 2000; Lin et al. 2002; Riggs et al. 2000; Sun et al. 2001; Tasis et al. 2006). Covalent functionalization approaches are coupling reactions that target oxidized defect sites on the carbon nanotube surface and additional reactions that perform for graphite surfaces conventionally. Covalent functionalization approaches can disorder the expanded п-networks on the carbon nanotube surfaces and decrease both their electrical and mechanical properties. To solve these problems, noncovalent approaches were introduced. In comparison with covalent functionalization, noncovalent functionalization is an easier method and has the benefit of preserving nanotube s sp2 structure, therefore preserving the electronic properties (Fernando et al. 2004; Tournus et al. 2005). Noncovalent approaches use different types of functionalization agents involving polymers, poly nuclear aromatic compounds, surfactants, and biomolecules for the noncovalent dispersion of carbon nanotubes (Reddy et al. 2009). Among these approaches, modifying the nanotube surface using aromatic moieties is very significant (Chen et al. 2001b).

In this work, thiosemicarbazide derivative-functionalized multiwalled carbon nanotubes were used for modification of a glassy carbon electrode in order to determine isoprenaline (IP) and piroxicam (PX). Piroxicam or [4-hydroxy-2-methyl-N-(2-pyridyl)-H-1,2-benzothiazine-3-carboxamide-1,1-di-oxide] is a nonsteroidal anti-inflammatory drug (NSAID) of the oxicam category that has been known worth as a chemopreventative, anti-tumor agent, for acute and chronic musculoskeletal and joint disorders such as ankylosing spondylitis, rheumatoid arthritis, and osteoarthritis (Kate et al. 2013).

Isoprenaline or isoproterenol (4-[1-hydroxy-2-[(1-methylethyl)amino]ethyl]-1,2-benzenediol) is a significant neurotransmitter applied to cure the neural disorders such as Parkinson’s disease (Stryer 1990). IP is a catecholamine drug that is extremely utilized in the cure of allergic emergencies, bronchial asthma, status asthmatic, cardiac arrest, and ventricular bradycardia (Mandell and Petri 1996).

Here, electrochemical analysis was performed by a glassy carbon electrode with added multiwalled carbon nanotubes chemically modified with (z)-1-(3,4-dihydroxybenzylidene)-2-methylthiosemicarbazide (DBT–CNT/GCE). Thiosemicarbazide derivative compound was selected as a modifier because this compound is insoluble in aqueous solution (Benvidi et al. 2011; Mazloum-Ardakani et al. 2010; Mazloum-Ardakani et al. 2009). Furthermore, this compound shows a redox behavior which can reduce overpotential oxidation of analytes and electrocatalytic effect (Jin and Lin 2004; Murray 1984; Zhu et al. 2007).

In comparison to bare electrodes, modified electrodes improve the motion of electrons between the analyte and electrodes, which causes a substantial reduction in activation potential (Beitollahi et al. 2008). In addition, these electrodes are less affected by surface fouling and oxide formation (Santana et al. 2009). In fact, electrode modification improves sensitivity, reproducibility, electron transfer reaction, stability, and high overpotential for the electron transfer process. To the best of our knowledge, no paper has been published until now reporting the simultaneous electrocatalytic detection of IP and PX by using any type of modified electrodes. The modified electrode (DBT–CNT/GCE) was used to investigate electrocatalytic behavior of isoprenaline in phosphate buffer solution (pH = 7.0) using cyclic voltammetry, chronoamperometry, and differential pulse voltammetry (DPV). Moreover, it was used to detect different concentrations of IP and PX in solution simultaneously. The calibration curve was plotted to obtain the linear concentration range and detection limit. To examine the applicability of the proposed electrode for real sample analysis, the recovery of IP, PX was determined. The results showed that the suggested electrode has been successfully employed for the evaluation of the above compounds in real samples.

Methods

Apparatus and chemicals

The electrochemical measurements were performed with a potentiostat/galvanostat (SAMA 500, electro analyzer system, I.R. Iran) at the ambient temperature. In all experiments were applied a three-electrode assembly including a saturated calomel as the reference electrode, a platinum wire as the counter electrode, and DBT–CNT/GCE as the working electrode. All potentials were quoted vs. reference electrode. A Metrohm 691 pH/ion meter was used to pH measurements. The solutions were freshly prepared with doubly distilled water. Buffer solution was prepared from orthophosphoric acid and its salts in the pH = 7.0. Multiwalled carbon nanotubes (MWCNT) is obtained from PlasmaChem GmbH company. The IP, PX, and other reagents were of analytical grade (Merck). Also, DBT and functionalized carbon nanotubes were synthesized in our laboratory.

Synthesis of (z)-1-(3,4-dihydroxybenzylidene)-2-methylthiosemicarbazide

In 10-mL round bottom flask, 3,4-dihydroxybenzaldehyde (1 mmol), thiosemicarbazide (1 mmol), and methanol (5 mL) were taken and refluxed at 65 °C for 4 h. The precipitated product was filtered and washed with methanol. Further, purification was performed with recrystallization of the solid product in ethanol. NMR data: 1H NMR (250 MHz, DMSO-d 6): δ (ppm) = 9.63(OH, 1H), 9.07(OH, 1H), 8.08(CH = N, 1H, S), 7.81(NH, 1H), 7.20(NH2, 2H, S), 7.09-6.78(Ar, 3H). FTIR data: FTIR (KBr disk), 3446, 3329, 3178, 1620, 1592, 1538, 1508, 1365, 1279, 979, 867, and 841 cm−1. Scheme 1 shows chemical structure of thiosemicarbazide derivative.
Scheme 1

Chemical structure of thiosemicarbazide derivative

Oxidation of CNTs

We performed acid treatment method to oxidation of CNTs. The MWCNTs were immersed in a 65% solution of 3:1 mixture of 98% H2SO4 and 68% HNO3, and the suspension was heated at 100 °C for 30 min. Then, they were washed several times with deionized water on a filter paper with the pore size of 1 mm and were dried in a vacuum oven at 90 °C for 1 day. In this process, MWCNTs were oxidized and purified by omitting impurities.

Preparation of the electrode

For the preparation of DBT–CNT composite solution, 10 mg of DBT and 10 mg of CNTs were added into the 7.5 mL of dimethyl formamide (DMF). This mixture was dispersed for 30 min, stirred for 48 h at room temperature, and centrifuged for 10 min at 500 rpms, respectively. This sample was first washed off with DMF to ensure removal of unadsorption DBT from CNT surface and then dried at 50 °C under vacuum for 14 h to obtain the DBT–CNT composites. One milligram of obtained composite was added into 0.5 mL ethanol, dispersed for 30 min. In order to prepare DBT–CNT/GC-modified electrode, we dropped 4 μL of dispersed DBT–CNT solution composite on the surface of GC electrode and dried it at the ambient laboratory temperature.

Results and discussion

Characterization of DBT–CNT

Scanning electron microscopy was used to detect possible morphological changes on CNTs after the acid treatment. SEM images of CNTs before and after oxidation are shown in Fig. 1. The raw  CNT before oxidation being strongly entangled, it is practically impossible to align them (Fig. 1a). As the oxidation proceeds, the CNTs are gradually freed from the entanglements favoring their alignment. The stronger oxidation reagent, for example, acids, will induce more carboxyl groups than hydroxyl groups on the CNTs.
Fig. 1

SEM images of MWCNTs before oxidation (a) and after oxidation (b)

Electrochemical properties of DBT–CNT/GCE

The electrochemical behavior of the DBT–CNT/GC modified electrode was investigated by cyclic voltammetry at different scan rates in a buffered solution (pH = 7.0). The pH effect on the modified electrode signal was examined by CV using 0.1 M phosphate buffer solutions at different pH values. We selected pH 7 for the study because pH = 7 showed maximum electrocatalyst behavior. Also, pH = 7 is the pH of biological environment. A potential-pH diagram showed a straight line with a slope, nearly 60 mV/pH. Such behavior suggests a two-electron, two-proton process. Insolubility of DBT in an aqueous media is its advantage as electrode modifier. It ensures lack of leaching DBT from the CNT surface.

In Fig. 2, the CVs were obtained for the DBT–CNT/GCE in the absence of IP. The cyclic voltammograms in Fig. 2a indicated that the electrode process was quasi-reversible, because ΔE p was higher than (59/n) mV the same as a reversible system. In Fig. 2b, both the anodic and cathodic peak currents (I p) increased linearly with the scan rate. In addition, they were linearly dependent on ʋ in the range of 10 to 1800 mVs−1, indicating that redox process is controlled in a diffusion-independent manner for a surface-confined redox process.
Fig. 2

a CVs of DBT–CNT/GCE in phosphate buffer (pH 7.0, 0.1 M) at scan rates of 10 (1), 20 (2), 40 (3), 60 (4), 100 (5), 130 (6), 200 (7), 250 (8), 400 (9), 600 (10), 700 (11), 900 (12), 1200 (13), 1600 (14), and 1800 (15) mVs−1. b Variations in I p with scan rate. c Variations in E p with logarithm of scan rate. d Magnification of the same plots for high scan rates

For the purpose of estimating electron transfer rate constant (ks) and the transfer coefficient (α) of DBT, we used CV voltamograms in condition that the variations of anodic and cathodic peak potentials with logarithm of scan rate were studied by Laviron procedure (Laviron 1979). Figure 2c shows the variations of peak potentials (E p) as a function of the logarithm of the potential scan rate. At high scan rates (above 100 mVs−1), these plots become linear. The slopes of these linear segments in Fig. 2d can be applied to estimate the kinetic parameters. The slope of the linear segments is equal to −2.303RT/αn α F for the cathodic peak and 2.303RT/(1−α)n α F for anodic peak (n α is the number of electron in rate determining step). The values of anodic and cathodic transfer coefficients were obtained as α a = 0.47 and α c = 0.53. Furthermore, Eq. (1) was used to obtain ks between DBT and CNT/GCE:
$$ \log\ {\mathrm{k}}_{\mathrm{s}} = \alpha \log\ \left(1-\alpha \right) + \left(1-\alpha \right)\ \log \upalpha\ \hbox{--}\ \log\ \left(\mathrm{RT}/ nF\nu \right)\hbox{--}\ \upalpha\ \left(1-\alpha \right)\ {n}_{\upalpha} F{\Delta \mathrm{E}}_{\mathrm{p}}/2.3\mathrm{R}\mathrm{T} $$
(1)

In Eq. (1), ʋ is the sweep rate and n is the number of electrons involved in the overall redox reaction of the modifier (DBT), and all other symbols have their ordinary meanings. The amount of k s was obtained to be 0.512 s−1.

An approximate estimate of the surface coverage of the electrode (Г/mol cm−2) was obtained by the method used by Sharp et al (Sharp et al. 1979). According to this method, the peak current is related to the surface concentration of electroactive species by the following Eq. (2):
$$ {I}_{\mathrm{p}} = {n}^2{F}^2 A\varGamma \upsilon /4\mathrm{R}\mathrm{T} $$
(2)

Where I p represents the current peak, A is the surface of electrode (cm2), and Г is the surface coverage (mol/cm2), and there is no relationship between Г (mol/cm2) and geometric surface area. The other symbols have their usual meanings. Г = 1.30 × 10−6 mol/cm2 for n = 2 was calculated from the slope of the anodic peak current versus scan rate (Fig. 2b).

Electrocatalytic oxidation of IP at DBT–CNT/GCE

The cyclic voltammetric responses from the electrochemical oxidation of 2 mM IP at the DBT–CNT/GCE are shown in Fig. 3. The comparison of CV at GCE (Fig. 3 (curve c)) and DBT–CNT/GCE (Fig. 3 (curve d)) exhibited an increase of the anodic peak current at DBT–CNT/GCE, which indicated that the presence of DBT–CNT on the GCE could improve the peak currents. Also, the results showed that the peak potential of IP oxidation at the bare GCE (Fig. 3 (curve c)) and DBT–CNT/GCE (Fig. 3 (curve d)) was about 190 and 138 mV, respectively. These curves (curves c and d of Fig. 3) indicated the peak potential of IP oxidation at the surface of modified electrode shifts up to 52 mV toward negative values in comparison to that at the bare electrode. It is worth mentioning that the measurement of CV for both bare and modified electrodes in the presence of IP shows an increase of anodic current remarkably, whereas current is lower in the absence of IP. From these results, it was concluded that the best electrocatalytic effect for IP oxidation was observed at the DBT–CNT/GCE.
Fig. 3

CVs of a bare electrode and b DBT–CNT/GCE in 0.1 M phosphate buffer solution (pH = 7.0) at scan rate of 10 mVs−1. Also, CVs of c bare electrode and d DBT–CNT/GCE in presence of 2000 μM IP and 0.1 M phosphate buffer solution (pH = 7.0) at scan rate of 20 mVs−1

Figure 4a shows effect of scan rate on the electrocatalytic oxidation of IP at the DBT–CNT/GCE by cyclic voltammetry, the oxidation peak potential moved with increasing scan rates to a more positive potential, confirming the kinetic limitation of the electrochemical reaction. We can expect very clear cathodic peak at higher scan rate (Bard and Faulkner 2001). A linear plot of peak current (I p) vs the square root of the scan rate (υ 1/2) was depicted (Fig. 4b). It expresses that the process is diffusion controlled. So, a plot of the scan rate-normalized current (I p/υ 1/2) against scan rate (Fig. 4c) indicates that the characteristic shape typical of an EC′ process. Figure 4d exhibits the Tafel plot, drawn by using the data extracted from the increasing segment of the current–voltage curve at a scan rate of 10 mVs−1. Charge transfer coefficient α = 0.42 was estimated from slope of the Tafel plot. The redox reaction scheme of DBT has been shown in Scheme 2.
Fig. 4

a Cyclic voltammograms of DBT–CNT/GCE in a 0.1 M phosphate buffer (pH = 7.0) containing 1000 μM IP at different scan rates, CVs AF corresponding to 10, 15, 20, 25, 30, and 40 mVs−1 scan rates. b Variation of the electrocatalytic currents versus the square root of the scan rate. c Variation of the scan rate-normalized current (I p/υ 1/2) with scan rate. d Tafel plot derived from the rising part of the voltammogram recorded at a scan rate of 10 mVs−1

Scheme 2

Electrocatalytic reaction mechanism for IP oxidation at the DBT–CNT/GCE surface

Chronoamperometric measurements

In the chronoamperometric studies, we calculated the diffusion coefficient of IP at the DBT–CNT/GCE based on the Cottrell equation (Bard and Faulkner 2001). Chronoamperograms of IP at DBT–CNT/GCE were showed at different concentrations of IP (Fig. 5). At first, plots of I against t −1/2 were depicted with the best fits for different concentrations of IP (Fig. 5 (A)). Then, the slopes of the obtained straight lines were plotted versus IP concentrations (Fig. 5 (B)). Finally, from the resulting slope and Cottrell equation, the value of the diffusion coefficient was estimated (D = 1.56 × 10−5 cm2s−1).
Fig. 5

Chronoamperograms obtained at DBT–CNT/GCE in 0.1 M phosphate buffer solution (pH = 7.0) for various concentration of IP at a potential step of 240 mV. The numbers 16 correspond to 100.0, 400.0, 600.0, 800.0, 1000.0, and 1400.0 μM of IP. Inset (A): plots of I vs. t −1/2/s−1/2 obtained from chronoamprograms 16. Inset (B): plot of the slope of the straight lines vs the IP concentration

Calibration curve and limit of detection for IP

In view of high sensitivity, differential pulse voltammetry (DPV) was used to acquire the calibration curve and detection limit of IP at the DBT–CNT/GCE (Fig. 6). The plot of peak current vs IP concentration included two linear segments with different slopes and different concentration ranges of 0.5–100.0 μM and 100.0–1500.0 μM, respectively (inset of Fig. 6). The slope in high concentrations of IP (range of 100.0–1500.0 μM) is lower. It reduces, probably due to two reasons. The first reason is kinetic limitations (Mazloum-Ardakani and Khoshroo 2013; Taleat et al. 2008; Zare et al. 2006). The second is the presence of lower empty sites in surface of electrode in range of 100.0–1500.0 μM in comparison with lower range.
Fig. 6

DPVs of DBT–CNT/GCE in 0.1 M buffer solution (pH = 7.0) containing different concentrations of IP (inner to outer corresponds to 50.0, 100.0, 200.0, 300.0, 400.0, 500.0, 600.0, 700.0, 800.0, 1000.0, 1200.0, and 1300.0 μM). Inset: calibration plot of IP

The detection limit (3σ) was computed from the first linear segment of the calibration plot as 0.35 μM.

Simultaneous determination of isoprenaline and piroxicam

In this study, DPV was applied to detect IP and PX (piroxicam) simultaneously. The results represented two well-separated anodic peaks for the oxidation of IP and PX at potentials of 100 and 400 mV at the surface of the DBT–CNT/GCE (Fig. 7a). The sensitivity of the modified electrode to the oxidation of IP was obtained (0.0044 μA μM−1). Moreover, the sensitivity of IP in the presence of PX was obtained (0.0067 μA μM−1). The sensitivities of the modified electrode for IP in the presence and absence of PX were the same approximately; this suggested that the oxidation processes of IP and PX at modified electrode were independent. Consequently, independent measurements of the two analytes are reasonable without any interference. If slopes were different, PX would affect the IP signal.
Fig. 7

(a) DPVs of DBT–CNT/GCE in buffer solution (pH = 7.0) containing different concentrations of IP and PX: from inner to outer corresponds to mixed solutions of 100.0 + 104.1, 300.0 + 312.3, 400.0 + 416.9, 500.0+ 500.3, 700.0 + 700.4, 800.0 + 800.5, 900.0 + 900.6, 1000.0 + 999.7, 1200.0 + 1199.5, and 1300.0 + 1299.8, (b) Calibration plot of IP and (c) Calibration plot of PX

Interference study

The influence of different species on the determination of 1 mM IP was investigated. When the relative error was less than ±5%, no interference was realized in the presence of 1 mM of K+, Na+, NH4 +, Cl, F, Br, glucose, fructose, uric acid, and caffeine. In addition, no interference was realized in the presence of 0.5 mM of l-alanine, ascorbic acid, and l-cysteine.

Determination of IP and PX in human blood serum samples

The explained method was examined by direct analysis of IP and PX in blood serum samples as real samples. For preparation of real sample, 1 mL blood serum is diluted in 20 mL buffer solution and placed in the electrochemical cell. Known amount of IP and PX were spiked in real samples. Each solution was analyzed by DPV. Based on the currents of DPVs and using the calibration plots, the concentration and recovery of IP and PX are calculated. The results are shown in Table 1. The obtained results and recoveries exhibited that the DBT–CNT/GCE showed great catalytic activity for serum samples which contained diverse biological and mineral compounds.
Table 1

Recovery for different amounts of IP and PX spiked to the blood serum

Sample

Added (μM)

Found (μM)

Recovery (%)

IP

300.0

286.8

95.6

400.0

412.8

103.2

600.0

585.36

97.56

PX

200.0

201.4

100.7

400.0

404.4

101.1

600.0

593.94

98.99

The repeatability and stability of DBT–CNT/GC electrode

The repeatability of electrode surface was investigated by use of cyclic voltammetry for several separately prepared DBT–CNT/GCEs. The obtained RSD demonstrated that surface repeatability was acceptable with the amount of RSD = 4.0%. Also, reproducibility study was examined. For this purpose, we investigated cyclic voltammograms of modified electrode in different days. The results showed RSD = 4.8%. Besides, the stability of the DBT–CNT/GCEs was studied by recording CVs of IP after having cycled the potential 25 times at a scan rate of 10 mVs−1. The peak potentials were invariant, and the currents decreased by less than 2.13%.

To examine the antifouling property, it was recorded two cyclic voltammograms in solution of buffer (pH = 7.0) and IP at a scan rate of 10 mVs−1. The first was recorded as soon as putting the modified electrode in solution, and the second was recorded after passing 1 h from staying electrode in the solution. The results showed that peak potentials remained unchanged, and the currents reduced by less than 4.1%.

Conclusions

Chemically functionalized carbon nanotubes have presented a significant role in the investigation and progression of nanotube-based materials and systems. Improvement of dispersion and solubility of the carbon nanotubes associated with the functionalization and chemical modification exhibit great opportunities in the fabrication and the employment of carbon nanotubes for various nanostructures. In this paper, a simple preparation technique has been explained for fabrication of functionalized nanotube-based electrode to detect different concentrations of IP and PX simultaneously. The electrochemical behavior of the modified electrode was examined by CV, and it was realized that the utilization of potential cycling ensures great electrochemical reproducibility and mechanical stability of the deposited electrocatalyst. The oxidation of IP is catalyzed in a buffered aqueous solution (pH = 7.0) at DBT–CNT/GCE. It was proved with shifted peak potential of IP to a less positive potential rather than bare GCE. This proposed sensor has been successfully applied to determine the IP and PX in blood serum human, which demonstrates that it has excellent potential application for detection of different concentrations of IP and PX.

Abbreviations

CNTs: 

Carbon nanotubes

CV: 

Cyclic voltammetry

DBT: 

(z)-1-(3,4-dihydroxybenzylidene)-2-methylthiosemicarbazide

DMF: 

Dimethylformamide

DPV: 

Differential pulse voltammetry

FTIR: 

Fourier transform infrared spectroscopy

GCE: 

Glassy carbon electrode

IP: 

Isoprenaline

MWNT: 

Multiwalled carbon nanotubes

NMR: 

Nuclear magnetic resonance spectroscopy

NSAID: 

Nonsteroidal anti-inflammatory drug

PX: 

Piroxicam

rpm: 

Revolutions per minute

RSD: 

Relative standard deviation

SEM: 

Scanning electron microscope

SWNT: 

Single-walled carbon nanotubes

Declarations

Acknowledgements

The authors wish to thank the Yazd University Research Council, IUT Research Council and Excellence in Sensors for financial support of this research.

Authors’contributions

MMA and AK designed the experiment and drafted the manuscript. Experimental part and calculations were carried out by HMS. Synthesis of DBT and obtaining information of NMR and FTR were performed by MAA. The corresponding author is MMA. All the authors have read and approved the final manuscript.

Competing interests

The authors declare that they have no competing interests.

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Authors’ Affiliations

(1)
Department of Chemistry, Faculty of Science, Yazd University

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