# In Situ Evaluation of Fludarabine-DNA Interaction Using a DNA-Electrochemical Biosensor

Authors: H. Eda Satana; Ana Maria Oliveira-Brett
Journal: International Journal of Electrochemistry
 (2011)

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## Abstract

Fludarabine, 9-β-D-arabinosyl-2-fluoroadenine, the nucleoside analog, represents a highly effective treatment for hairy cell leukemia. The electrochemical behaviour of fludarabine is an irreversible diffusion controlled oxidation mechanism and was investigated at a glassy carbon electrode in different supporting electrolytes using cyclic, differential pulse, and square wave voltammetry. The diffusion coefficient of fludarabine was calculated to be DFLU=1.71×10−6 cm2 s-1 in pH 7.0 0.1 M phosphate buffer. The oxidation mechanism of fludarabine occurs with the transfer of one proton and one electron and the formation of a hydroxylated species. The interaction of fludarabine with DNA was investigated, by differential pulse voltammetry, in incubated solutions and using dsDNA- and polyhomonucleotides-, poly[G] and poly[A], electrochemical biosensors. The results showed that fludarabine interacts with DNA causing changes in the DNA structure.


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## Body

## 1. Introduction

Nucleotides are essential components of the signal transduction system and energy providers such as adenosine tri phosphate (ATP). Nucleoside analogs are antimetabolites used in cellular and molecular biology research, as well as in the treatment of some diseases as antiviral or anticancer drugs. These analogs are metabolized to pharmacologically active derivatives in cells and compete with natural products.The nucleoside analog fludarabine (FLU, 9-β-D-arabinosyl-2-fluoroadenine), Scheme 1, represents a highly effective treatment for hairy cell leukemia, chronic lymphocytic leukaemia, and other several hematopoietic malignancies [1]. The introduction of a fluorine atom in the nucleoside group has improved the pharmacological properties of the molecule with minor stereochemistry changes. Unlike the former nucleoside analogs, FLU is resistant to deamination by adenosine deaminase. After entering the cells by means of specific nucleoside transporters, FLU is activated to its phosphorylated derivative by intracellular kinase. Its active metabolite competes with deoxy-ATP for incorporation into the growing nucleic acid chain causing disruption of nucleic acid synthesis. In the same way, this metabolite interrupts the elongation of the RNA primer strand [2].Scheme 1
Chemical structure of fludarabine.To improve treatment results in patients, individualization of FLU dosing is important. This individualization must be depended on correlations between dosing and plasma concentration of drug and its derivatives. Furthermore, the determination of cellular concentrations of FLU could provide valuable information for understanding the mechanisms of DNA damage and cell death. Therefore, some methods based on high performance liquid chromatographic and voltammetric techniques were developed for the determination of FLU especially in biological samples. FLU and its triphosphate derivative were determined by liquid chromatography with UV detection [3–7] and with tandem mass spectrometry [8] in human cells, urine, plasma, and pharmaceuticals, and the electrochemical behaviour of FLU was also investigated using pyrolytic graphite electrode [9].Most studies were related with the pharmacological character and effects of FLU on biological molecules, carried out in cell lines, and several studies indicated that FLU is an agent that causes disruption or breakages in the genetic material. Deoxyribonucleic acid (DNA) is the genetic material and has important biological roles including transcription of the genetic information, signalling, and metabolic regulation. Formation of DNA strand breaks causes chromosome aberrations and accumulation of these mutations and other DNA damages increase carcinogenic or teratogenic risks. Finally, these events may result in a malignant transformation or cell death. Due to their important biological and genetic roles, nucleic acids have been intensively studied and a number of different techniques have been developed to elucidate various aspects of DNA and RNA structures and properties. Electrochemical methods including DNA-electrochemical biosensors comprise an important group of these techniques. Compared with optical devices, electrochemical sensors have some advantages such as their high sensitivity, simplicity, low cost, and fast response time [10–13].A DNA-electrochemical biosensor consists of an electrode with DNA immobilized on the surface. Interaction of a damaging agent with DNA causes changing of electrochemical properties of the DNA recognition layer. This effect is turned to measurable electrical signals and DNA damage and interaction caused by hazardous compounds, such as metals or pharmaceutical drugs, can be determined.In this study, the electrochemical oxidation of FLU and the mechanism of FLU-dsDNA and polyhomonucleotides, poly[G] and poly[A], interaction were carried out using cyclic, square wave and differential pulse voltammetry at a glassy carbon electrode. The results will contribute to the clarification of the mechanism by which FLU can cause directin vivo DNA damage.


## 2. Experimental

### 2.1. Materials and Reagents

Fludarabine, double stranded (dsDNA), polyadenylic acid (Poly[A]), and polyguanylic acid (Poly[G]) were obtained from Sigma and used without further purification. A stock solution of 1 mM FLU was prepared in deionized water and stored at 5°C.Solutions of different concentrations of FLU were prepared by dilution of the appropriate quantity in supporting electrolyte. Stock solutions of 186μg mL−1 dsDNA, 477 μg mL−1 Poly[G], and 587 μg mL−1 Poly[A] were prepared in deionized water and diluted to the desired concentrations in pH 4.5 0.1 M acetate buffer.All supporting electrolyte solutions (Table1) were prepared using analytical grade reagents and purified water from a Millipore Milli-Q system (conductivity ≤ 0.1 μS cm−1).Table 1
Supporting electrolyte buffer solutions.
pHComposition2.1HCl + KCl3.4HAcO + NaAcO4.3HAcO + NaAcO4.5HAcO + NaAcO5.4HAcO + NaAcO6.1NaH2PO4 + Na2HPO47.0NaH2PO4 + Na2HPO48.0NaH2PO4 + Na2HPO49.2NH3 + NH4Cl10.5NH3 + NH4Cl12.0NaOH + KCl


### 2.2. Apparatus

Voltammetric experiments were carried out using aμ Autolab running with GPES 4.9 software, Eco-Chemie, Utrecht, The Netherlands. Measurements were carried out using a three-electrode system in a 0.5 mL one-compartment electrochemical cell (Cypress System Inc., USA). Glassy carbon electrode (GCE, d=1.5 mm) was the working electrode, Pt wire the counter electrode, and Ag/AgCl (3 M KCl) the reference electrode.The pH measurements were carried out with a Crison micropH 2001 pH-meter with an Ingold combined glass electrode. All experiments were done at room temperature (25±1°C) and, microvolumes were measured using EP-10 and EP-100 Plus Motorized Microliter Pippettes (Rainin Instrument Co. Inc., Woburn, USA).The experimental conditions for differential pulse (DP) voltammetry were: pulse amplitude 50 mV, pulse width 70 ms, and scan rate 5 mV s−1. For square wave (SW) voltammetry, a frequency of 50 Hz and a potential increment of 2 mV, corresponding to an effective scan rate of 100 mV s−1 were used.The GCE was polished using diamond spray (particle size 3μm) (Kemet, UK) before each electrochemical experiment. After polishing, it was rinsed thoroughly with Milli-Q water. Following this mechanical treatment, the GCE was placed in buffer supporting electrolyte and voltammograms were recorded until a steady-state baseline voltammogram was obtained. This procedure ensured very reproducible experimental results.


### 2.3. Acquisition and Presentation of Voltammetric Data

All the voltammograms presented were background-subtracted and baseline-corrected using the moving average application with a step window of 5 mV included in GPES version 4.9 software. This mathematical treatment improves the visualization and identification of peaks over the baseline without introducing any artifact, although the peak intensity is, in some cases, reduced (<10%) relative to that of the untreated curve. Nevertheless, this mathematical treatment of the original voltammograms was used in the presentation of all experimental voltammograms for a better and clearer identification of the peaks. The values for peak current presented in all plots were determined from the original untreated voltammograms after subtraction of the baseline.


### 2.4. Incubation Procedure and DNA-Electrochemical Biosensor Preparation

In order to perform the incubation procedure in pH 4.5 0.1 M acetate buffer, 100μg mL−1 dsDNA were mixed with 2 μM FLU and 100 μg mL−1 Poly[G] or Poly[A] were mixed with 5 μM FLU, and then incubated during different periods at room temperature. Control solutions of FLU, dsDNA, Poly[G], and Poly[A] in pH 4.5 0.1 M acetate buffer were also prepared and stored during the same periods in similar conditions as the FLU-dsDNA, FLU-Poly[G], and FLU-Poly[A] incubated solutions.The thin layer dsDNA-modified electrode was prepared with three drops of 5μL each containing 50 μg mL−1 dsDNA. After setting each drop on the electrode surface, the biosensor was allowed to dry under the constant flux of N2. The dsDNA-electrochemical biosensor was incubated in 50 μM FLU solution during different times. Then, in order to remove unbound FLU molecules from the surface, the electrode was carefully rinsed with deionized water and transferred to supporting electrolyte. After each measurement, the dsDNA film was removed from the electrode surface and a new biosensor was prepared for each experiment.Poly[G]- and Poly[A]-electrochemical biosensors were prepared placing three drops of 5μL each containing 25 μg mL−1 of each polyhomonucleotide on the electrode surface.


## 2.1. Materials and Reagents

Fludarabine, double stranded (dsDNA), polyadenylic acid (Poly[A]), and polyguanylic acid (Poly[G]) were obtained from Sigma and used without further purification. A stock solution of 1 mM FLU was prepared in deionized water and stored at 5°C.Solutions of different concentrations of FLU were prepared by dilution of the appropriate quantity in supporting electrolyte. Stock solutions of 186μg mL−1 dsDNA, 477 μg mL−1 Poly[G], and 587 μg mL−1 Poly[A] were prepared in deionized water and diluted to the desired concentrations in pH 4.5 0.1 M acetate buffer.All supporting electrolyte solutions (Table1) were prepared using analytical grade reagents and purified water from a Millipore Milli-Q system (conductivity ≤ 0.1 μS cm−1).Table 1
Supporting electrolyte buffer solutions.
pHComposition2.1HCl + KCl3.4HAcO + NaAcO4.3HAcO + NaAcO4.5HAcO + NaAcO5.4HAcO + NaAcO6.1NaH2PO4 + Na2HPO47.0NaH2PO4 + Na2HPO48.0NaH2PO4 + Na2HPO49.2NH3 + NH4Cl10.5NH3 + NH4Cl12.0NaOH + KCl


## 2.2. Apparatus

Voltammetric experiments were carried out using aμ Autolab running with GPES 4.9 software, Eco-Chemie, Utrecht, The Netherlands. Measurements were carried out using a three-electrode system in a 0.5 mL one-compartment electrochemical cell (Cypress System Inc., USA). Glassy carbon electrode (GCE, d=1.5 mm) was the working electrode, Pt wire the counter electrode, and Ag/AgCl (3 M KCl) the reference electrode.The pH measurements were carried out with a Crison micropH 2001 pH-meter with an Ingold combined glass electrode. All experiments were done at room temperature (25±1°C) and, microvolumes were measured using EP-10 and EP-100 Plus Motorized Microliter Pippettes (Rainin Instrument Co. Inc., Woburn, USA).The experimental conditions for differential pulse (DP) voltammetry were: pulse amplitude 50 mV, pulse width 70 ms, and scan rate 5 mV s−1. For square wave (SW) voltammetry, a frequency of 50 Hz and a potential increment of 2 mV, corresponding to an effective scan rate of 100 mV s−1 were used.The GCE was polished using diamond spray (particle size 3μm) (Kemet, UK) before each electrochemical experiment. After polishing, it was rinsed thoroughly with Milli-Q water. Following this mechanical treatment, the GCE was placed in buffer supporting electrolyte and voltammograms were recorded until a steady-state baseline voltammogram was obtained. This procedure ensured very reproducible experimental results.


## 2.3. Acquisition and Presentation of Voltammetric Data

All the voltammograms presented were background-subtracted and baseline-corrected using the moving average application with a step window of 5 mV included in GPES version 4.9 software. This mathematical treatment improves the visualization and identification of peaks over the baseline without introducing any artifact, although the peak intensity is, in some cases, reduced (<10%) relative to that of the untreated curve. Nevertheless, this mathematical treatment of the original voltammograms was used in the presentation of all experimental voltammograms for a better and clearer identification of the peaks. The values for peak current presented in all plots were determined from the original untreated voltammograms after subtraction of the baseline.


## 2.4. Incubation Procedure and DNA-Electrochemical Biosensor Preparation

In order to perform the incubation procedure in pH 4.5 0.1 M acetate buffer, 100μg mL−1 dsDNA were mixed with 2 μM FLU and 100 μg mL−1 Poly[G] or Poly[A] were mixed with 5 μM FLU, and then incubated during different periods at room temperature. Control solutions of FLU, dsDNA, Poly[G], and Poly[A] in pH 4.5 0.1 M acetate buffer were also prepared and stored during the same periods in similar conditions as the FLU-dsDNA, FLU-Poly[G], and FLU-Poly[A] incubated solutions.The thin layer dsDNA-modified electrode was prepared with three drops of 5μL each containing 50 μg mL−1 dsDNA. After setting each drop on the electrode surface, the biosensor was allowed to dry under the constant flux of N2. The dsDNA-electrochemical biosensor was incubated in 50 μM FLU solution during different times. Then, in order to remove unbound FLU molecules from the surface, the electrode was carefully rinsed with deionized water and transferred to supporting electrolyte. After each measurement, the dsDNA film was removed from the electrode surface and a new biosensor was prepared for each experiment.Poly[G]- and Poly[A]-electrochemical biosensors were prepared placing three drops of 5μL each containing 25 μg mL−1 of each polyhomonucleotide on the electrode surface.


## 3. Results and Discussion

The electrochemical behaviour of FLU was investigated using the glassy carbon electrode (GCE) and cyclic (CV), differential pulse (DP), and square wave (SW) voltammetry.Systematic studies to explain the mechanism of interaction of FLU with dsDNA, Poly[A], and Poly[G] were carried out, with the multilayer modified electrodes or in incubated solutions, using the GCE and DP voltammetry. DP voltammetry, due of its high sensitivity, enabled the detection of minor changes on the DNA double helical structure and DNA oxidative damage.


### 3.1. Electro-Oxidation of Fludarabine

#### 3.1.1. Cyclic Voltammetry

The CV of 100μM FLU at a GCE, in pH 6.1 0.1 M phosphate buffer, showed one anodic peak 1a, at Epa1=+1.36 V, Figure 1. Reversing the potential no reduction peak was observed, indicating that the oxidation process was irreversible, and peak 1a current decreased with increasing number of scans due to FLU and/or its oxidation product adsorption on the GCE surface.Figure 1
Cyclic voltammograms of 100μM FLU in pH 6.1 0.1 M phosphate buffer solution, N2 saturated; “solid line” first scan, “dotted line” second scan, and ν=100 mV s−1.The effect of pH on the electrochemical oxidation behaviour of FLU was investigated in aqueous buffered solutions in the range 2 < pH < 12. CVs showed that in strong acidic buffer solutions, pH ≤ 2, no FLU oxidation peak was observed. For pH > 2, the CVs showed irreversible peak 1a. The oxidation process was pH-dependent, and the peak potentials of FLU shifted, with increasing pH.The effect of the scan rate in a 100μM FLU solution, in N2 saturated pH 6.1 0.1 M phosphate buffer, between 5 and 500 mV s−1 was also investigated. Increasing the scan rate, the peak 1a potential was slightly shifted to more positive potentials, and |Epa-Ep/2a|=~33 mV. Since for a diffusion-controlled irreversible system |Epa-Ep/2a|=47.7/(αan’)  where αa is the charge transfer coefficient and n’ the number of electrons in the rate-determining step [14], it was calculated the value of αan’=1.8.Increasing the scan rate the peak 1a current increased linearly with square root of ν, indicating a diffusion controlled behaviour of FLU. The peak current for a diffusion-controlled irreversible system is given by Ipa(A)=-2.99×105n(αan′)1/2A[O]∞DO1/2ν1/2 where n is the number of the electrons transferred during the oxidation of FLU (n=1 as shown Section 3.1.2), A is the electrode area in cm2, DO is the diffusion coefficient in cm2 s−1, [O]∞ is the concentration in mol cm−3, and ν is in V s−1 [14]. The GCE electroactive area of A=0.00691 cm2 was determined as described elsewhere [15]. By plotting Ipc versus ν1/2, the value of DO was obtained from the slope −3.04×10-7 A (V s−1)−1/2. The diffusion coefficient of FLU was calculated to be DFLU=1.71×10-6 cm2s−1.


#### 3.1.2. Differential Pulse Voltammetry

DP voltammetry was used to investigate the effect of pH on the electrochemical oxidation of 100μM FLU, and peak 1a, in aqueous supporting electrolytes over a pH range from 2.0 to 12.0, Figure 2(a). As already found by CV, in strong acidic buffer solution, no FLU oxidation peak was observed.(a) 3D plots of baseline corrected DP voltammograms in 100μM FLU (b) Plot of peak 1a: (□) Epa and  (●) Ipa versus pH. Dotted line corresponds to 59 mV per pH unit.
(a)(b)The peak 1a potential shifted linearly with pH towards more negative values and peak current increased up to pH 6.1 and afterwards decreased with increasing pH, Figure 2(b). The relationship was linear following the equation Epa(mV)=1.48-0.06 pH, Figure 2(b). The slope of the line, −59 mV per pH unit, shows that the mechanism of oxidation involves the same number of electrons and protons. The number of electrons transferred, n, was determined by the peak width at half height, W1/2~75 mV and is close to the theoretical value of 90 mV, corresponding to an electrochemical reaction involving the transfer of one electron.According to these results, the oxidation of FLU occurs with a transfer of one electron and one proton to produce a finally hydroxylated product. Since FLU is an adenine analogue, the irreversible oxidation mechanism is similar to adenine.Successive scans in the same solution, without cleaning the electrode, showed the decrease of peak 1a current and the occurrence of oxidation peak 2a, at Ep=+0.33 V, corresponding to the oxidation of FLU oxidation product.The effect of pH on the electrochemical oxidation behaviour of peak 2a showed that with increasing pH, peak 2a shifted to less positive potentials, and a linear relationship, with the slope of the Epa versus pH of −59 mV per pH unit, was found corresponding to the transfer of the same number of electron and proton in aqueous buffer solution.


#### 3.1.3. Square Wave Voltammetry

The electrochemical behaviour of FLU was also investigated using SW voltammetry due to the its advantages such as fast analysis time, lower blocking of electrode surface by the species, and less consumption of analyte. This method enables to detect during only one scan whether the electron transfer reaction is reversible or not. Due to the sampling of current values in both positive and negative going pulses, peaks belonging to the oxidation and reduction of the species at the electrode surface can be obtained simultaneously.SW voltammetric experiments were carried out in the same pH range as CV and DP voltammetry. The oxidation peak 1a was observed in all buffer solutions, and its irreversibility was confirmed by plotting the forward and backward components of the total current obtained in solutions of 100 μM FLU in pH 6.1 0.1 M phosphate buffer, Figure 3(a). The results obtained on the second and subsequent scans in the same solution without cleaning electrode showed the second oxidation peak 2a, at Epa=+0.33 V, related to the oxidation of FLU oxidation product, Figure 3(b). Since reduction and oxidation currents were equal, the reversibility of the second peak was confirmed.SW voltammograms of 100μM FLU in pH 6.1 0.1 M phosphate buffer: (a) first scan, (b) second scan, f=50 Hz, ΔEs=2 mV, 1pulse amplitude 100 mV, It—total, If—forward and Ib—backward, and νeffective=100 mV s−1.
(a)(b)


#### 3.1.4. Analytical Determination of Fludarabine

DP voltammetry was used for the electroanalytical determination of FLU due to its advantages such as good discrimination, low detection limit, and short analysis time. According to Figure2, the best pH was pH 6.1 0.1 M phosphate buffer and linearity range was achieved between 0.99 and 14.8 μM FLU, Table 2. Above this range, due to the adsorption of FLU or its oxidation product on the GCE surface, a loss of linearity was observed. In order to ensure a clean electrode surface and to avoid the adsorption of FLU and/or its oxidation product, the GCE surface was always cleaned between each measurement. The detection limit (LOD) and quantification limit (LOQ) were calculated according to the 3 s/m and 10 s/m, [16, 17], where s is the standard deviation of the peak current, m is slope of calibration curve, and LOD=0.28 μM and LOQ=0.94 μM were found, Table 2.Table 2
Regression and validation data of calibration line of fludarabine.
PotentialLinearity range (μM)SlopeInterceptCorrelation coefficientLOD (μM)LOQ (μM)Repeatability of peak current (RSD%)Repeatability of peak potential (RSD%)1.281.6–14.81.56×10-81.29×10-80.99930.280.941.550.09


### 3.2. DNA-Fludarabine Interaction

FLU was synthesized as an adenosine nucleoside analogue and used in the treatment of leukemia. After intravenous infusion, FLU is transported to cell by means of transporters, inhibits DNA synthesis, and causes DNA disruption or breakages. Therefore, the investigation and clarification of the interaction mechanism between FLU and DNA is very important.The mechanism of interaction of FLU with dsDNA, Poly[A] and Poly[G], in incubated solutions or with the multilayer GCE modified as described in the Experimental (Section2.4), was investigated.


#### 3.2.1. DNA-Fludarabine Interaction in Incubated Solutions

In order to investigate the interaction between FLU and dsDNA, Figure4, presents the DP voltammograms obtained, in pH 4.5 0.1 M acetate buffer, for FLU, one oxidation peak 1a, at Epa=+1.35 V, and for dsDNA, two well-defined and separated peaks corresponding to the oxidation of desoxyguanosine (dGuo), at Epa=+0.98 V, and desoxyadenosine (dAdo), at Epa=+1.25 V, Figure 4.Figure 4
DP voltammograms baseline corrected in pH 4.5 0.1 M acetate buffer of: (solid line) 100μg mL−1 dsDNA and incubated solutions during (dashed line) 0 h, (dotted line) 1 h, and (dash-dotted line) 3 h of 100 μg mL−1 DNA with 2 μM FLU. Pulse amplitude-50 mV, pulse width-70 ms, and ν=5 mV s−1.The interaction between FLU and dsDNA was studied in incubated solutions of 2μM FLU and 100 μg mL−1 dsDNA, in pH 4.5 0.1 M acetate buffer, and DP voltammograms recorded for different incubation times. Control solutions of 2 μM FLU and 100 μg mL−1 dsDNA, in pH 4.5 0.1 M acetate buffer, were also prepared, and DP voltammograms recorded for the same incubation times. The GCE surface was cleaned between each measurement to avoid the blocking of the GCE surface by adsorption of the FLU and dsDNA.The DP voltammograms obtained immediately after addition of FLU to dsDNA solution, showed three peaks corresponding to the oxidation of dsDNA purinic bases, dGuo, atEpa=+0.98 V, dAdo, at Epa=+1.25 V, and FLU, at Epa=+1.35 V, Figure 4. Increasing the incubation time, the peak current of dGuo and dAdo decreased, indicating that dsDNA structure was modified due to the interaction FLU-dsDNA by condensation and/or aggregation, which makes more difficult the access of the dsDNA bases to the electrode surface hindering their oxidation. However, no dsDNA oxidative damage caused by FLU occurred, as no peaks corresponding to the oxidation of 8-oxoGua or 2,8-oxoAde, the oxidation products of dsDNA purinic bases, were observed in the DP voltammograms, Figure 4.To clarify the interaction of FLU and dsDNA, experiments were also carried out in incubated solutions of 5μM FLU and 100 μg mL−1 purinic base solutions, poly[G] or poly[A], in pH 4.5 0.1 M acetate buffer, Figure 5. DP voltammograms showed similar results as with dsDNA, confirming the decrease of the oxidation peaks of dGuo and dAdo and no oxidative damage, as no peaks corresponding to the oxidation products of guanine, 8-oxoGua, and adenine, 2,8-oxoAde, occurred.DP voltammograms baseline corrected in pH 4.5 0.1 M acetate buffer of 100μg mL−1: (a) Poly[G] and (b) Poly[A] (solid line) before and after incubation with 5 μM FLU during (dashed line) 0 h, (dotted line) 1 h, and (dash-dotted line) 3 h. Pulse amplitude-50 mV, pulse width-70 ms, and ν=5 mV s−1.
(a)(b)


#### 3.2.2.  In Situ DNA-Fludarabine Interaction

Multilayer dsDNA-, Poly[G]-, and Poly[A]-electrochemical biosensors were prepared and used to investigate thein situ DNA-fludarabine interaction. The electrochemical biosensor surface was covered by a multilayer to make sure that the undesired adsorption of FLU on GCE could not occur. The dsDNA-, Poly[G]-, and Poly[A]-electrochemical biosensors enable the identification of the in situ interaction with time, besides the advantage of low cost, fast response time, simple design, and high detection limit.The dsDNA-electrochemical biosensor was prepared, Section2.4, incubated in 50 μM FLU solution for different times, 5, 10, and 15 min, and transferred to supporting electrolyte buffer solution. In order to remove unbounded FLU, the dsDNA-electrochemical biosensor was carefully washed with deionized water before being transferred to pH 4.5 0.1 M acetate buffer where the DP voltammograms were recorded, Figure 6. In this way, the observed peaks in the DP voltammograms can only be caused by the interaction between dsDNA and FLU. As expected, dGuo and dAdo, and a very small FLU oxidation peaks were also obtained, Figure 6. After each measurement, the dsDNA film was removed from the electrode surface and the experiments were always performed with a newly prepared biosensor. The results showed that dGuo and dAdo oxidation peaks decreased with increasing incubation time in the FLU solution. This is caused by modifications in the dsDNA morphological structure and strand breaks, due to the interaction with FLU. No oxidation peaks for 8-oxoGua and 2,8-oxoA, the dsDNA purinic bases oxidation products, were observed, so there was no DNA oxidative damage.Figure 6
DP voltammograms baseline corrected in pH 4.5 0.1 M acetate buffer with dsDNA-electrochemical biosensors (solid line) before and after incubation during (dashed line) 5 min, (dotted line) 10 min, and (dash dotted line) 15 min in a solution of 50μM FLU. Pulse amplitude-50 mV, pulse width-70 ms, and scan rate ν=5 mV s−1.Polynucleotides biosensors, Poly[G]- and Poly[A]-electrochemical biosensors, were prepared,Section 2.4, and incubated in 50 μM FLU in pH 4.5 0.1 M acetate buffer for different times, in order to shine more information on the interaction between dsDNA and FLU, Figure 7.DP voltammograms baseline corrected in pH 4.5 0.1 M acetate buffer with (a) Poly[G]- and (b) Poly[A]-electrochemical biosensors (solid line) before and after incubation during (dashed line) 5 min, (dotted line) 10 min, and (dash-dotted line) 15 min in a solution of 50μM FLU. Pulse amplitude-50 mV, pulse width-70 ms and scan rate ν=5 mV s−1.
(a)(b)Poly[G]-electrochemical biosensor, after being transferred to pH 4.5 0.1 M acetate buffer, showed two peaks one for FLU and the other for poly[G], corresponding the oxidation of dGuo, atEpa=+0.98 V, which decreased with increasing incubation time, and no oxidation peak for 8-oxoGua was observed, Figure 7(a).Poly[A]-electrochemical biosensor, after being transferred to pH 4.5 0.1 M acetate buffer, showed two peaks one for FLU and the other for poly[A], corresponding the oxidation of dAdo, atEpa=+1.25 V, which decreased with increasing incubation time, and no oxidation peak for 2,8-oxoA was observed, Figure 7(b).These experiments using polyhomopurinenucleotide single-stranded sequences, poly[G]- and poly[A]-electrochemical biosensors, confirm the results obtained using the dsDNA-electrochemical biosensor.


## 3.1. Electro-Oxidation of Fludarabine

### 3.1.1. Cyclic Voltammetry

The CV of 100μM FLU at a GCE, in pH 6.1 0.1 M phosphate buffer, showed one anodic peak 1a, at Epa1=+1.36 V, Figure 1. Reversing the potential no reduction peak was observed, indicating that the oxidation process was irreversible, and peak 1a current decreased with increasing number of scans due to FLU and/or its oxidation product adsorption on the GCE surface.Figure 1
Cyclic voltammograms of 100μM FLU in pH 6.1 0.1 M phosphate buffer solution, N2 saturated; “solid line” first scan, “dotted line” second scan, and ν=100 mV s−1.The effect of pH on the electrochemical oxidation behaviour of FLU was investigated in aqueous buffered solutions in the range 2 < pH < 12. CVs showed that in strong acidic buffer solutions, pH ≤ 2, no FLU oxidation peak was observed. For pH > 2, the CVs showed irreversible peak 1a. The oxidation process was pH-dependent, and the peak potentials of FLU shifted, with increasing pH.The effect of the scan rate in a 100μM FLU solution, in N2 saturated pH 6.1 0.1 M phosphate buffer, between 5 and 500 mV s−1 was also investigated. Increasing the scan rate, the peak 1a potential was slightly shifted to more positive potentials, and |Epa-Ep/2a|=~33 mV. Since for a diffusion-controlled irreversible system |Epa-Ep/2a|=47.7/(αan’)  where αa is the charge transfer coefficient and n’ the number of electrons in the rate-determining step [14], it was calculated the value of αan’=1.8.Increasing the scan rate the peak 1a current increased linearly with square root of ν, indicating a diffusion controlled behaviour of FLU. The peak current for a diffusion-controlled irreversible system is given by Ipa(A)=-2.99×105n(αan′)1/2A[O]∞DO1/2ν1/2 where n is the number of the electrons transferred during the oxidation of FLU (n=1 as shown Section 3.1.2), A is the electrode area in cm2, DO is the diffusion coefficient in cm2 s−1, [O]∞ is the concentration in mol cm−3, and ν is in V s−1 [14]. The GCE electroactive area of A=0.00691 cm2 was determined as described elsewhere [15]. By plotting Ipc versus ν1/2, the value of DO was obtained from the slope −3.04×10-7 A (V s−1)−1/2. The diffusion coefficient of FLU was calculated to be DFLU=1.71×10-6 cm2s−1.


### 3.1.2. Differential Pulse Voltammetry

DP voltammetry was used to investigate the effect of pH on the electrochemical oxidation of 100μM FLU, and peak 1a, in aqueous supporting electrolytes over a pH range from 2.0 to 12.0, Figure 2(a). As already found by CV, in strong acidic buffer solution, no FLU oxidation peak was observed.(a) 3D plots of baseline corrected DP voltammograms in 100μM FLU (b) Plot of peak 1a: (□) Epa and  (●) Ipa versus pH. Dotted line corresponds to 59 mV per pH unit.
(a)(b)The peak 1a potential shifted linearly with pH towards more negative values and peak current increased up to pH 6.1 and afterwards decreased with increasing pH, Figure 2(b). The relationship was linear following the equation Epa(mV)=1.48-0.06 pH, Figure 2(b). The slope of the line, −59 mV per pH unit, shows that the mechanism of oxidation involves the same number of electrons and protons. The number of electrons transferred, n, was determined by the peak width at half height, W1/2~75 mV and is close to the theoretical value of 90 mV, corresponding to an electrochemical reaction involving the transfer of one electron.According to these results, the oxidation of FLU occurs with a transfer of one electron and one proton to produce a finally hydroxylated product. Since FLU is an adenine analogue, the irreversible oxidation mechanism is similar to adenine.Successive scans in the same solution, without cleaning the electrode, showed the decrease of peak 1a current and the occurrence of oxidation peak 2a, at Ep=+0.33 V, corresponding to the oxidation of FLU oxidation product.The effect of pH on the electrochemical oxidation behaviour of peak 2a showed that with increasing pH, peak 2a shifted to less positive potentials, and a linear relationship, with the slope of the Epa versus pH of −59 mV per pH unit, was found corresponding to the transfer of the same number of electron and proton in aqueous buffer solution.


### 3.1.3. Square Wave Voltammetry

The electrochemical behaviour of FLU was also investigated using SW voltammetry due to the its advantages such as fast analysis time, lower blocking of electrode surface by the species, and less consumption of analyte. This method enables to detect during only one scan whether the electron transfer reaction is reversible or not. Due to the sampling of current values in both positive and negative going pulses, peaks belonging to the oxidation and reduction of the species at the electrode surface can be obtained simultaneously.SW voltammetric experiments were carried out in the same pH range as CV and DP voltammetry. The oxidation peak 1a was observed in all buffer solutions, and its irreversibility was confirmed by plotting the forward and backward components of the total current obtained in solutions of 100 μM FLU in pH 6.1 0.1 M phosphate buffer, Figure 3(a). The results obtained on the second and subsequent scans in the same solution without cleaning electrode showed the second oxidation peak 2a, at Epa=+0.33 V, related to the oxidation of FLU oxidation product, Figure 3(b). Since reduction and oxidation currents were equal, the reversibility of the second peak was confirmed.SW voltammograms of 100μM FLU in pH 6.1 0.1 M phosphate buffer: (a) first scan, (b) second scan, f=50 Hz, ΔEs=2 mV, 1pulse amplitude 100 mV, It—total, If—forward and Ib—backward, and νeffective=100 mV s−1.
(a)(b)


### 3.1.4. Analytical Determination of Fludarabine

DP voltammetry was used for the electroanalytical determination of FLU due to its advantages such as good discrimination, low detection limit, and short analysis time. According to Figure2, the best pH was pH 6.1 0.1 M phosphate buffer and linearity range was achieved between 0.99 and 14.8 μM FLU, Table 2. Above this range, due to the adsorption of FLU or its oxidation product on the GCE surface, a loss of linearity was observed. In order to ensure a clean electrode surface and to avoid the adsorption of FLU and/or its oxidation product, the GCE surface was always cleaned between each measurement. The detection limit (LOD) and quantification limit (LOQ) were calculated according to the 3 s/m and 10 s/m, [16, 17], where s is the standard deviation of the peak current, m is slope of calibration curve, and LOD=0.28 μM and LOQ=0.94 μM were found, Table 2.Table 2
Regression and validation data of calibration line of fludarabine.
PotentialLinearity range (μM)SlopeInterceptCorrelation coefficientLOD (μM)LOQ (μM)Repeatability of peak current (RSD%)Repeatability of peak potential (RSD%)1.281.6–14.81.56×10-81.29×10-80.99930.280.941.550.09


## 3.1.1. Cyclic Voltammetry

The CV of 100μM FLU at a GCE, in pH 6.1 0.1 M phosphate buffer, showed one anodic peak 1a, at Epa1=+1.36 V, Figure 1. Reversing the potential no reduction peak was observed, indicating that the oxidation process was irreversible, and peak 1a current decreased with increasing number of scans due to FLU and/or its oxidation product adsorption on the GCE surface.Figure 1
Cyclic voltammograms of 100μM FLU in pH 6.1 0.1 M phosphate buffer solution, N2 saturated; “solid line” first scan, “dotted line” second scan, and ν=100 mV s−1.The effect of pH on the electrochemical oxidation behaviour of FLU was investigated in aqueous buffered solutions in the range 2 < pH < 12. CVs showed that in strong acidic buffer solutions, pH ≤ 2, no FLU oxidation peak was observed. For pH > 2, the CVs showed irreversible peak 1a. The oxidation process was pH-dependent, and the peak potentials of FLU shifted, with increasing pH.The effect of the scan rate in a 100μM FLU solution, in N2 saturated pH 6.1 0.1 M phosphate buffer, between 5 and 500 mV s−1 was also investigated. Increasing the scan rate, the peak 1a potential was slightly shifted to more positive potentials, and |Epa-Ep/2a|=~33 mV. Since for a diffusion-controlled irreversible system |Epa-Ep/2a|=47.7/(αan’)  where αa is the charge transfer coefficient and n’ the number of electrons in the rate-determining step [14], it was calculated the value of αan’=1.8.Increasing the scan rate the peak 1a current increased linearly with square root of ν, indicating a diffusion controlled behaviour of FLU. The peak current for a diffusion-controlled irreversible system is given by Ipa(A)=-2.99×105n(αan′)1/2A[O]∞DO1/2ν1/2 where n is the number of the electrons transferred during the oxidation of FLU (n=1 as shown Section 3.1.2), A is the electrode area in cm2, DO is the diffusion coefficient in cm2 s−1, [O]∞ is the concentration in mol cm−3, and ν is in V s−1 [14]. The GCE electroactive area of A=0.00691 cm2 was determined as described elsewhere [15]. By plotting Ipc versus ν1/2, the value of DO was obtained from the slope −3.04×10-7 A (V s−1)−1/2. The diffusion coefficient of FLU was calculated to be DFLU=1.71×10-6 cm2s−1.


## 3.1.2. Differential Pulse Voltammetry

DP voltammetry was used to investigate the effect of pH on the electrochemical oxidation of 100μM FLU, and peak 1a, in aqueous supporting electrolytes over a pH range from 2.0 to 12.0, Figure 2(a). As already found by CV, in strong acidic buffer solution, no FLU oxidation peak was observed.(a) 3D plots of baseline corrected DP voltammograms in 100μM FLU (b) Plot of peak 1a: (□) Epa and  (●) Ipa versus pH. Dotted line corresponds to 59 mV per pH unit.
(a)(b)The peak 1a potential shifted linearly with pH towards more negative values and peak current increased up to pH 6.1 and afterwards decreased with increasing pH, Figure 2(b). The relationship was linear following the equation Epa(mV)=1.48-0.06 pH, Figure 2(b). The slope of the line, −59 mV per pH unit, shows that the mechanism of oxidation involves the same number of electrons and protons. The number of electrons transferred, n, was determined by the peak width at half height, W1/2~75 mV and is close to the theoretical value of 90 mV, corresponding to an electrochemical reaction involving the transfer of one electron.According to these results, the oxidation of FLU occurs with a transfer of one electron and one proton to produce a finally hydroxylated product. Since FLU is an adenine analogue, the irreversible oxidation mechanism is similar to adenine.Successive scans in the same solution, without cleaning the electrode, showed the decrease of peak 1a current and the occurrence of oxidation peak 2a, at Ep=+0.33 V, corresponding to the oxidation of FLU oxidation product.The effect of pH on the electrochemical oxidation behaviour of peak 2a showed that with increasing pH, peak 2a shifted to less positive potentials, and a linear relationship, with the slope of the Epa versus pH of −59 mV per pH unit, was found corresponding to the transfer of the same number of electron and proton in aqueous buffer solution.


## 3.1.3. Square Wave Voltammetry

The electrochemical behaviour of FLU was also investigated using SW voltammetry due to the its advantages such as fast analysis time, lower blocking of electrode surface by the species, and less consumption of analyte. This method enables to detect during only one scan whether the electron transfer reaction is reversible or not. Due to the sampling of current values in both positive and negative going pulses, peaks belonging to the oxidation and reduction of the species at the electrode surface can be obtained simultaneously.SW voltammetric experiments were carried out in the same pH range as CV and DP voltammetry. The oxidation peak 1a was observed in all buffer solutions, and its irreversibility was confirmed by plotting the forward and backward components of the total current obtained in solutions of 100 μM FLU in pH 6.1 0.1 M phosphate buffer, Figure 3(a). The results obtained on the second and subsequent scans in the same solution without cleaning electrode showed the second oxidation peak 2a, at Epa=+0.33 V, related to the oxidation of FLU oxidation product, Figure 3(b). Since reduction and oxidation currents were equal, the reversibility of the second peak was confirmed.SW voltammograms of 100μM FLU in pH 6.1 0.1 M phosphate buffer: (a) first scan, (b) second scan, f=50 Hz, ΔEs=2 mV, 1pulse amplitude 100 mV, It—total, If—forward and Ib—backward, and νeffective=100 mV s−1.
(a)(b)


## 3.1.4. Analytical Determination of Fludarabine

DP voltammetry was used for the electroanalytical determination of FLU due to its advantages such as good discrimination, low detection limit, and short analysis time. According to Figure2, the best pH was pH 6.1 0.1 M phosphate buffer and linearity range was achieved between 0.99 and 14.8 μM FLU, Table 2. Above this range, due to the adsorption of FLU or its oxidation product on the GCE surface, a loss of linearity was observed. In order to ensure a clean electrode surface and to avoid the adsorption of FLU and/or its oxidation product, the GCE surface was always cleaned between each measurement. The detection limit (LOD) and quantification limit (LOQ) were calculated according to the 3 s/m and 10 s/m, [16, 17], where s is the standard deviation of the peak current, m is slope of calibration curve, and LOD=0.28 μM and LOQ=0.94 μM were found, Table 2.Table 2
Regression and validation data of calibration line of fludarabine.
PotentialLinearity range (μM)SlopeInterceptCorrelation coefficientLOD (μM)LOQ (μM)Repeatability of peak current (RSD%)Repeatability of peak potential (RSD%)1.281.6–14.81.56×10-81.29×10-80.99930.280.941.550.09


## 3.2. DNA-Fludarabine Interaction

FLU was synthesized as an adenosine nucleoside analogue and used in the treatment of leukemia. After intravenous infusion, FLU is transported to cell by means of transporters, inhibits DNA synthesis, and causes DNA disruption or breakages. Therefore, the investigation and clarification of the interaction mechanism between FLU and DNA is very important.The mechanism of interaction of FLU with dsDNA, Poly[A] and Poly[G], in incubated solutions or with the multilayer GCE modified as described in the Experimental (Section2.4), was investigated.


### 3.2.1. DNA-Fludarabine Interaction in Incubated Solutions

In order to investigate the interaction between FLU and dsDNA, Figure4, presents the DP voltammograms obtained, in pH 4.5 0.1 M acetate buffer, for FLU, one oxidation peak 1a, at Epa=+1.35 V, and for dsDNA, two well-defined and separated peaks corresponding to the oxidation of desoxyguanosine (dGuo), at Epa=+0.98 V, and desoxyadenosine (dAdo), at Epa=+1.25 V, Figure 4.Figure 4
DP voltammograms baseline corrected in pH 4.5 0.1 M acetate buffer of: (solid line) 100μg mL−1 dsDNA and incubated solutions during (dashed line) 0 h, (dotted line) 1 h, and (dash-dotted line) 3 h of 100 μg mL−1 DNA with 2 μM FLU. Pulse amplitude-50 mV, pulse width-70 ms, and ν=5 mV s−1.The interaction between FLU and dsDNA was studied in incubated solutions of 2μM FLU and 100 μg mL−1 dsDNA, in pH 4.5 0.1 M acetate buffer, and DP voltammograms recorded for different incubation times. Control solutions of 2 μM FLU and 100 μg mL−1 dsDNA, in pH 4.5 0.1 M acetate buffer, were also prepared, and DP voltammograms recorded for the same incubation times. The GCE surface was cleaned between each measurement to avoid the blocking of the GCE surface by adsorption of the FLU and dsDNA.The DP voltammograms obtained immediately after addition of FLU to dsDNA solution, showed three peaks corresponding to the oxidation of dsDNA purinic bases, dGuo, atEpa=+0.98 V, dAdo, at Epa=+1.25 V, and FLU, at Epa=+1.35 V, Figure 4. Increasing the incubation time, the peak current of dGuo and dAdo decreased, indicating that dsDNA structure was modified due to the interaction FLU-dsDNA by condensation and/or aggregation, which makes more difficult the access of the dsDNA bases to the electrode surface hindering their oxidation. However, no dsDNA oxidative damage caused by FLU occurred, as no peaks corresponding to the oxidation of 8-oxoGua or 2,8-oxoAde, the oxidation products of dsDNA purinic bases, were observed in the DP voltammograms, Figure 4.To clarify the interaction of FLU and dsDNA, experiments were also carried out in incubated solutions of 5μM FLU and 100 μg mL−1 purinic base solutions, poly[G] or poly[A], in pH 4.5 0.1 M acetate buffer, Figure 5. DP voltammograms showed similar results as with dsDNA, confirming the decrease of the oxidation peaks of dGuo and dAdo and no oxidative damage, as no peaks corresponding to the oxidation products of guanine, 8-oxoGua, and adenine, 2,8-oxoAde, occurred.DP voltammograms baseline corrected in pH 4.5 0.1 M acetate buffer of 100μg mL−1: (a) Poly[G] and (b) Poly[A] (solid line) before and after incubation with 5 μM FLU during (dashed line) 0 h, (dotted line) 1 h, and (dash-dotted line) 3 h. Pulse amplitude-50 mV, pulse width-70 ms, and ν=5 mV s−1.
(a)(b)


### 3.2.2.  In Situ DNA-Fludarabine Interaction

Multilayer dsDNA-, Poly[G]-, and Poly[A]-electrochemical biosensors were prepared and used to investigate thein situ DNA-fludarabine interaction. The electrochemical biosensor surface was covered by a multilayer to make sure that the undesired adsorption of FLU on GCE could not occur. The dsDNA-, Poly[G]-, and Poly[A]-electrochemical biosensors enable the identification of the in situ interaction with time, besides the advantage of low cost, fast response time, simple design, and high detection limit.The dsDNA-electrochemical biosensor was prepared, Section2.4, incubated in 50 μM FLU solution for different times, 5, 10, and 15 min, and transferred to supporting electrolyte buffer solution. In order to remove unbounded FLU, the dsDNA-electrochemical biosensor was carefully washed with deionized water before being transferred to pH 4.5 0.1 M acetate buffer where the DP voltammograms were recorded, Figure 6. In this way, the observed peaks in the DP voltammograms can only be caused by the interaction between dsDNA and FLU. As expected, dGuo and dAdo, and a very small FLU oxidation peaks were also obtained, Figure 6. After each measurement, the dsDNA film was removed from the electrode surface and the experiments were always performed with a newly prepared biosensor. The results showed that dGuo and dAdo oxidation peaks decreased with increasing incubation time in the FLU solution. This is caused by modifications in the dsDNA morphological structure and strand breaks, due to the interaction with FLU. No oxidation peaks for 8-oxoGua and 2,8-oxoA, the dsDNA purinic bases oxidation products, were observed, so there was no DNA oxidative damage.Figure 6
DP voltammograms baseline corrected in pH 4.5 0.1 M acetate buffer with dsDNA-electrochemical biosensors (solid line) before and after incubation during (dashed line) 5 min, (dotted line) 10 min, and (dash dotted line) 15 min in a solution of 50μM FLU. Pulse amplitude-50 mV, pulse width-70 ms, and scan rate ν=5 mV s−1.Polynucleotides biosensors, Poly[G]- and Poly[A]-electrochemical biosensors, were prepared,Section 2.4, and incubated in 50 μM FLU in pH 4.5 0.1 M acetate buffer for different times, in order to shine more information on the interaction between dsDNA and FLU, Figure 7.DP voltammograms baseline corrected in pH 4.5 0.1 M acetate buffer with (a) Poly[G]- and (b) Poly[A]-electrochemical biosensors (solid line) before and after incubation during (dashed line) 5 min, (dotted line) 10 min, and (dash-dotted line) 15 min in a solution of 50μM FLU. Pulse amplitude-50 mV, pulse width-70 ms and scan rate ν=5 mV s−1.
(a)(b)Poly[G]-electrochemical biosensor, after being transferred to pH 4.5 0.1 M acetate buffer, showed two peaks one for FLU and the other for poly[G], corresponding the oxidation of dGuo, atEpa=+0.98 V, which decreased with increasing incubation time, and no oxidation peak for 8-oxoGua was observed, Figure 7(a).Poly[A]-electrochemical biosensor, after being transferred to pH 4.5 0.1 M acetate buffer, showed two peaks one for FLU and the other for poly[A], corresponding the oxidation of dAdo, atEpa=+1.25 V, which decreased with increasing incubation time, and no oxidation peak for 2,8-oxoA was observed, Figure 7(b).These experiments using polyhomopurinenucleotide single-stranded sequences, poly[G]- and poly[A]-electrochemical biosensors, confirm the results obtained using the dsDNA-electrochemical biosensor.


## 3.2.1. DNA-Fludarabine Interaction in Incubated Solutions

In order to investigate the interaction between FLU and dsDNA, Figure4, presents the DP voltammograms obtained, in pH 4.5 0.1 M acetate buffer, for FLU, one oxidation peak 1a, at Epa=+1.35 V, and for dsDNA, two well-defined and separated peaks corresponding to the oxidation of desoxyguanosine (dGuo), at Epa=+0.98 V, and desoxyadenosine (dAdo), at Epa=+1.25 V, Figure 4.Figure 4
DP voltammograms baseline corrected in pH 4.5 0.1 M acetate buffer of: (solid line) 100μg mL−1 dsDNA and incubated solutions during (dashed line) 0 h, (dotted line) 1 h, and (dash-dotted line) 3 h of 100 μg mL−1 DNA with 2 μM FLU. Pulse amplitude-50 mV, pulse width-70 ms, and ν=5 mV s−1.The interaction between FLU and dsDNA was studied in incubated solutions of 2μM FLU and 100 μg mL−1 dsDNA, in pH 4.5 0.1 M acetate buffer, and DP voltammograms recorded for different incubation times. Control solutions of 2 μM FLU and 100 μg mL−1 dsDNA, in pH 4.5 0.1 M acetate buffer, were also prepared, and DP voltammograms recorded for the same incubation times. The GCE surface was cleaned between each measurement to avoid the blocking of the GCE surface by adsorption of the FLU and dsDNA.The DP voltammograms obtained immediately after addition of FLU to dsDNA solution, showed three peaks corresponding to the oxidation of dsDNA purinic bases, dGuo, atEpa=+0.98 V, dAdo, at Epa=+1.25 V, and FLU, at Epa=+1.35 V, Figure 4. Increasing the incubation time, the peak current of dGuo and dAdo decreased, indicating that dsDNA structure was modified due to the interaction FLU-dsDNA by condensation and/or aggregation, which makes more difficult the access of the dsDNA bases to the electrode surface hindering their oxidation. However, no dsDNA oxidative damage caused by FLU occurred, as no peaks corresponding to the oxidation of 8-oxoGua or 2,8-oxoAde, the oxidation products of dsDNA purinic bases, were observed in the DP voltammograms, Figure 4.To clarify the interaction of FLU and dsDNA, experiments were also carried out in incubated solutions of 5μM FLU and 100 μg mL−1 purinic base solutions, poly[G] or poly[A], in pH 4.5 0.1 M acetate buffer, Figure 5. DP voltammograms showed similar results as with dsDNA, confirming the decrease of the oxidation peaks of dGuo and dAdo and no oxidative damage, as no peaks corresponding to the oxidation products of guanine, 8-oxoGua, and adenine, 2,8-oxoAde, occurred.DP voltammograms baseline corrected in pH 4.5 0.1 M acetate buffer of 100μg mL−1: (a) Poly[G] and (b) Poly[A] (solid line) before and after incubation with 5 μM FLU during (dashed line) 0 h, (dotted line) 1 h, and (dash-dotted line) 3 h. Pulse amplitude-50 mV, pulse width-70 ms, and ν=5 mV s−1.
(a)(b)


## 3.2.2.  In Situ DNA-Fludarabine Interaction

Multilayer dsDNA-, Poly[G]-, and Poly[A]-electrochemical biosensors were prepared and used to investigate thein situ DNA-fludarabine interaction. The electrochemical biosensor surface was covered by a multilayer to make sure that the undesired adsorption of FLU on GCE could not occur. The dsDNA-, Poly[G]-, and Poly[A]-electrochemical biosensors enable the identification of the in situ interaction with time, besides the advantage of low cost, fast response time, simple design, and high detection limit.The dsDNA-electrochemical biosensor was prepared, Section2.4, incubated in 50 μM FLU solution for different times, 5, 10, and 15 min, and transferred to supporting electrolyte buffer solution. In order to remove unbounded FLU, the dsDNA-electrochemical biosensor was carefully washed with deionized water before being transferred to pH 4.5 0.1 M acetate buffer where the DP voltammograms were recorded, Figure 6. In this way, the observed peaks in the DP voltammograms can only be caused by the interaction between dsDNA and FLU. As expected, dGuo and dAdo, and a very small FLU oxidation peaks were also obtained, Figure 6. After each measurement, the dsDNA film was removed from the electrode surface and the experiments were always performed with a newly prepared biosensor. The results showed that dGuo and dAdo oxidation peaks decreased with increasing incubation time in the FLU solution. This is caused by modifications in the dsDNA morphological structure and strand breaks, due to the interaction with FLU. No oxidation peaks for 8-oxoGua and 2,8-oxoA, the dsDNA purinic bases oxidation products, were observed, so there was no DNA oxidative damage.Figure 6
DP voltammograms baseline corrected in pH 4.5 0.1 M acetate buffer with dsDNA-electrochemical biosensors (solid line) before and after incubation during (dashed line) 5 min, (dotted line) 10 min, and (dash dotted line) 15 min in a solution of 50μM FLU. Pulse amplitude-50 mV, pulse width-70 ms, and scan rate ν=5 mV s−1.Polynucleotides biosensors, Poly[G]- and Poly[A]-electrochemical biosensors, were prepared,Section 2.4, and incubated in 50 μM FLU in pH 4.5 0.1 M acetate buffer for different times, in order to shine more information on the interaction between dsDNA and FLU, Figure 7.DP voltammograms baseline corrected in pH 4.5 0.1 M acetate buffer with (a) Poly[G]- and (b) Poly[A]-electrochemical biosensors (solid line) before and after incubation during (dashed line) 5 min, (dotted line) 10 min, and (dash-dotted line) 15 min in a solution of 50μM FLU. Pulse amplitude-50 mV, pulse width-70 ms and scan rate ν=5 mV s−1.
(a)(b)Poly[G]-electrochemical biosensor, after being transferred to pH 4.5 0.1 M acetate buffer, showed two peaks one for FLU and the other for poly[G], corresponding the oxidation of dGuo, atEpa=+0.98 V, which decreased with increasing incubation time, and no oxidation peak for 8-oxoGua was observed, Figure 7(a).Poly[A]-electrochemical biosensor, after being transferred to pH 4.5 0.1 M acetate buffer, showed two peaks one for FLU and the other for poly[A], corresponding the oxidation of dAdo, atEpa=+1.25 V, which decreased with increasing incubation time, and no oxidation peak for 2,8-oxoA was observed, Figure 7(b).These experiments using polyhomopurinenucleotide single-stranded sequences, poly[G]- and poly[A]-electrochemical biosensors, confirm the results obtained using the dsDNA-electrochemical biosensor.


## 4. Conclusion

The electrochemical behaviour of fludarabine was investigated on the GCE in different aqueous buffer solutions using CV, DP, and SW voltammetry. The oxidation mechanism of fludarabine is irreversible, pH dependent and occurs with one electrode and one proton transfer. The diffusion coefficientDFLU=1.71×10-6 cm2 s−1·10−6 cm2 s−1 was determined. In the electroanalytical determination of FLU, the values of LOD=0.28 μM and LOQ=0.94 μM were found.The mechanism of interaction of FLU with dsDNA, poly[A] and poly[G], in incubated solutions or with multilayer GC modified electrodes, clearly showed, using the concentrations chosen, that fludarabine-DNA interaction caused morphological changes and strand breaks in the dsDNA structure in a time-dependent manner, but no DNA oxidative damage.



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*Source: 340239-2011-04-14.xml*