# Interaction of Calf Thymus DNA with the Ni(II) Complex of Sodium 1,4-Dihydroxy-9,10-Anthraquinone-2-Sulphonate: A Novel Method of Analysis Using Cyclic Voltammetry

Authors: Partha Sarathi Guin; Piyal Das; Saurabh Das; Parikshit Chandra Mandal
Journal: International Journal of Electrochemistry
 (2012)

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## Abstract

Hydroxy-9,10-anthraquinones are cheaper alternatives to anthracycline drugs. They closely resemble anthracycline drugs both from a structural and functional viewpoint. Electrochemical behavior of the Ni(II) complex (Na2[Ni(NaLH)2Cl2]·2H2O) of sodium 1,4-dihydroxy-9,10-anthraquinone-2-sulphonate (NaLH2), analogue of the core unit of anthracycline anticancer drugs, was studied at physiological pH using cyclic voltammetry. The Ni(II) complex of sodium 1,4-dihydroxy-9,10-anthraquinone-2-sulphonate undergoes diffusion-controlled one-electron reduction that enables performing an electrochemical study on the interaction of the complex with calf thymus DNA. The complex was titrated with increasing concentrations of DNA, and the reduction peak for the unbound complex helped in evaluating binding parameters. Analysis of binding data using nonlinear curve fit in a cyclic voltammetry experiment is the first such attempt. The paper evaluates site size of interaction that also serves as a means to determine stoichiometry of complex formation, between a metal ion and ligand from a DNA interaction study, probably a first of its kind.


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## Body

## 1. Introduction

Anthracycline drugs, the most widely used anticancer agents [1, 2], get limited in their use due to high cost and cardiotoxic properties [3, 4]. Although the exact mechanism by which anthracyclines exert their anticancer activity is still uncertain [5], dominant amongst various mechanisms appear to involve impairment of topoisomerase-IIα activity [6, 7], that is consistent with observed DNA intercalation and nuclear localization of the drug [8–10]. Biochemical studies show that the drugs inhibit both DNA-directed DNA synthesis [11] and DNA-directed RNA synthesis [12], presumably by their ability to interact with the DNA template primer [13, 14]. Owing to aforesaid reasons, research on the interaction of anthracyclines and their analogues with DNA is being actively pursued [1–14].Chemotherapeutic efficiency as well as cardiotoxicity of anthracycline drugs are associated with electron transfer processes, which show a very good correlation with the redox behavior of the molecules [15–18]. Owing to one-electron reduction, the quinone moiety in these drugs is converted to semiquinone playing a major role in determining chemotherapeutic efficiency and toxicity in cellular systems [19, 20]. Analogues of anthracyclines, the hydroxy-9,10-anthraquinones and their complexes, were reported to be suitable radiosensitizers [21–23], a phenomenon, also linked to electron transfer processes.In order to develop cheap but efficient substitutes of anthracycline drugs, different analogues are being tried clinically [2, 24–28], and efforts are on going to modify the quinone moiety. One route to such modification has been through complex formation using metal ions that reduce formation of superoxide, generating less cardiotoxic yet active anthracyclines [29, 30]. Several metal complexes of anthracyclines were tried for treating various forms of human cancer [29, 30]. Studies on the decrease in the formation of superoxide was done by forming metal complexes of 1,2-dihydroxy-9,10-anthraquinone, an analogue of anthracycline drugs [21, 31]. There is, however, a lack of research on the electrochemical behavior of metal-anthracycline complexes to understand whether the biochemical properties of these metal complexes are improved in comparison to the parent drug molecule. Through a recent investigation [32] on a Cu(II)-complex of sodium 1,4-dihydroxy-9,10-anthraquinone-2-sulphonate (NaLH2), we showed that the electrochemical behavior of NaLH2  is significantly modified in the metal complex. Our recent results [33–35] in aqueous and nonaqueous solvent and a very recent review on the electrochemistry of quinone systems [35] suggest that NaLH2and other hydroxy-9,10-anthraquinones exhibit electrochemical behavior similar to anthracycline drugs.In recent studies [32, 34–37], we were successful in showing that 1,4-dihydroxy-9,10-anthraquinone, 1,2,4-trihydroxy-9,10-anthraquinone, NaLH2 and its Cu(II) complex interact with calf thymus DNA (CT DNA), and that the binding parameters evaluated [32] were close to those reported for the anthracycline drugs [38]. Encouraged by these findings, we decided to extend the study to an Ni(II)-NaLH2 complex because of a difference in electronic constitution with Cu(II). Using a metal ion whose chemistry differs from Cu(II) enabled us to understand the role played by metal ions during the process of interaction of the complexes of hydroxy-9,10-anthraquinones to CT DNA. Further, this study was carried out to see whether metal complex formation could increase the intrinsic binding constant value of sodium 1,4-dihydroxy-9,10-anthraquinone-2-sulphonate (NaLH2) to calf thymus DNA. Ni(II) being a biologically friendly metal ion [39, 40] was another reason for our choice.The cytotoxicity of hydroxy-9,10-anthraquinones and anthracyclines increase with an increase in their single-electron reduction midpoint potential [41, 42]. A close parallel was found in the reactivity of hydroxy-9,10-anthraquinones and anthracyclines with single-electron transferring flavoenzymes ferredoxin: NADP+ reductase and NADPH: cytochrome P-450 reductase, and their cytotoxicity [42]. Thus it is important to evaluate the electrochemical parameters for this class of molecules to correlate their cytotoxicity with electrochemical behavior. In previous studies from our group we observed that metal complex formation reduces the toxicity of hydroxy-9,10-anthraquinones [21, 31] which means that our present Ni(II) complex would be less toxic than NaLH2.Ni(II) forms 1 : 2 metal complex with NaLH2. The effective stability constant of the complex was found to be 2.46×1013 [43]. The complex [Ni(NaLH)2Cl2] · 2H2O [43] was characterized by quantitative analysis of the metal ion, elemental analysis, IR, mass spectra, TGA, and magnetic studies. The proposed structure of the complex has been shown in Scheme 1. To find out the crystal structure of the Ni(II) complex several methods to grow a single crystal were carried out extensively using different solvent compositions and techniques. The method used in the reported crystal structure of terbium(III) complex of sodium 1,4-dihydroxy-9,10-anthraquinone-2-sulphonate [44] was also followed. However, all attempts failed to obtain a single crystal for the said species. This is in accordance with the nature of anthracyclines and anthraquinones as there are not many reports of their forming single crystals with metal ions [32, 44]. The planarity of the anthraquinone moiety may be responsible for this, why such compounds do not easily form crystals that can be collected and mounted on a X-ray diffractometer for systematic analysis. Therefore, a crystal structure of our Ni(II) complex with sodium 1,4-dihydroxy-9,10-anthraquinone-2-sulphonate was not achieved. This being a disadvantage as far as characterization of the complex is concerned we were cautious in the other experiments we performed to determine the structure of the complex such as elemental analysis, IR spectroscopy and mass spectra. These were performed several times from different crops of prepared material and the results obtained were reproducible. In this study, interaction with CT DNA was monitored by cyclic voltammetry (CV) and the binding parameters evaluated using non-linear curve fit analysis, for the first time by monitoring the cathodic peak current of the compound.Scheme 1
Proposed structure of Na2[Ni(NaLH)2Cl2] · 2H2O.


## 2. Experimental

### 2.1. Reagents and Chemicals

Sodium 1,4-dihydroxy-9,10-anthraquinone-2-sulphonate was prepared by sulphonation of 1,4-dihydroxy-9,10-anthraquinone (Sigma-Aldrich) and was characterized by our methods [32, 34]. The Ni(II) complex, Na2[Ni(NaLH)2Cl2] · 2H2O was prepared and characterized as described earlier [43]. The quinone moiety being sensitive to light solutions were prepared just before the experiment and kept in dark. Sodium chloride (AR grade) obtained from Merck, Germany, was used as supporting electrolyte in aqueous media. Since in physiological solution the ionic strength is mainly maintained by NaCl, therefore, in our studies we used NaCl inspite of other electrolytes. Analytical grade Hepes buffer (N-2-Hydroxyethylpiperazine-N-2-ethane-Sulphonic acid [45]), (0.02 mol dm−3); (Specrochem Pvt. Ltd., India) was used to maintain pH. Calf thymus DNA (CT DNA) was purchased from Sisco Research Laboratories Pvt. Ltd., India, and after dissolution in buffer purity was checked from the absorbance ratio A260/A280. For all the solutions the absorption ratio was in the range 1.8<A260/A280<1.9. Therefore, no further deproteinization of the DNA was required. Concentration of DNA in terms of nucleotide was determined taking ε260=6600 mol−1 dm3 cm−1 per base for calf thymus DNA. In all the experiments, DNA concentration was expressed in terms of base. All solutions were prepared in triple distilled water.


### 2.2. Apparatus

Cyclic voltammetry experiments were carried out using conventional three-electrode system at 25°C. The temperature was maintained using a circulating water bath. A glassy carbon electrode of surface area 0.1256 cm2 served as the working electrode, a platinum wire acted as the counter electrode while Ag/AgCl, satd. KCl was the reference electrode. Experiments were done using EG & G Potentiostat Model 263A (Princeton Applied Research, USA). All experimental solutions were degassed for 30 min with high-purity argon gas, before an electrochemical experiment. Microprocessor pH/ION Meter (pMX 3000) (WTW, Weilheim, Germany) was used for checking pH-values of solutions. The absorbance of DNA solution was measured using a UNICAM spectrophotometer, model UV 500 (UNICAM Ltd., Cambridge). A pair of 10×10 mm path length quartz cuvette was used for absorption experiments. Fluorescence spectroscopic measurements were carried out using a fluorimeter, model HITACHI S-7000 (HITACHI, Japan).


### 2.3. Preparation of Experimental Solutions

The uncertainty in weighing of the solid Na2[Ni(NaLH)2Cl2] · 2H2O was less than 0.3% indicating that the error in weighing is negligible or within acceptable limits. In the DNA interaction study, the concentration of Na2[Ni(NaLH)2Cl2] · 2H2O was 23.81 μM, that is, 23.81×10-6 mol dm−3. The solution was prepared by an exact dilution of a stock aqueous solution (2×10-4 mol dm−3) with an aqueous solution containing 0.500 mol dm−3 NaCl and 10×10-3 mol dm−3 Hepes buffer (pH 7.4) using a calibrated micropipette (Pipetman-M23866E, Gilson, France). To check concentrations of Na2[Ni(NaLH)2Cl2] · 2H2O in the experimental solutions, a calibration experiment (Lambert Beer’s Law) was done by measuring absorbance of different solutions of Na2[Ni(NaLH)2Cl2] · 2H2O of known strength at 465 nm, using which the concentration of Na2[Ni(NaLH)2Cl2] · 2H2O could be checked during the experiments. A 6.00×10-3 mol dm−3 aqueous solution of CT DNA (stock solution) was prepared and this was added quantitatively using a calibrated micropipette in each titration.


### 2.4. Methods

The electrochemical behavior of the Ni(II)-NaLH2 complex was studied in aqueous solution using cyclic voltammetry. Cyclic voltammetry was also carried out to study the interaction of the compound with calf thymus DNA. The non linear curve fit analysis usually applied in the spectrophotometric and fluorimetric studies was used first time in cyclic voltammetry studies to determine the binding parameters. The intercalation of Ni(II)-NaLH2 complex into DNA base pairs was established by competitive binding study using ethidium bromide in fluorescence spectroscopy.


## 2.1. Reagents and Chemicals

Sodium 1,4-dihydroxy-9,10-anthraquinone-2-sulphonate was prepared by sulphonation of 1,4-dihydroxy-9,10-anthraquinone (Sigma-Aldrich) and was characterized by our methods [32, 34]. The Ni(II) complex, Na2[Ni(NaLH)2Cl2] · 2H2O was prepared and characterized as described earlier [43]. The quinone moiety being sensitive to light solutions were prepared just before the experiment and kept in dark. Sodium chloride (AR grade) obtained from Merck, Germany, was used as supporting electrolyte in aqueous media. Since in physiological solution the ionic strength is mainly maintained by NaCl, therefore, in our studies we used NaCl inspite of other electrolytes. Analytical grade Hepes buffer (N-2-Hydroxyethylpiperazine-N-2-ethane-Sulphonic acid [45]), (0.02 mol dm−3); (Specrochem Pvt. Ltd., India) was used to maintain pH. Calf thymus DNA (CT DNA) was purchased from Sisco Research Laboratories Pvt. Ltd., India, and after dissolution in buffer purity was checked from the absorbance ratio A260/A280. For all the solutions the absorption ratio was in the range 1.8<A260/A280<1.9. Therefore, no further deproteinization of the DNA was required. Concentration of DNA in terms of nucleotide was determined taking ε260=6600 mol−1 dm3 cm−1 per base for calf thymus DNA. In all the experiments, DNA concentration was expressed in terms of base. All solutions were prepared in triple distilled water.


## 2.2. Apparatus

Cyclic voltammetry experiments were carried out using conventional three-electrode system at 25°C. The temperature was maintained using a circulating water bath. A glassy carbon electrode of surface area 0.1256 cm2 served as the working electrode, a platinum wire acted as the counter electrode while Ag/AgCl, satd. KCl was the reference electrode. Experiments were done using EG & G Potentiostat Model 263A (Princeton Applied Research, USA). All experimental solutions were degassed for 30 min with high-purity argon gas, before an electrochemical experiment. Microprocessor pH/ION Meter (pMX 3000) (WTW, Weilheim, Germany) was used for checking pH-values of solutions. The absorbance of DNA solution was measured using a UNICAM spectrophotometer, model UV 500 (UNICAM Ltd., Cambridge). A pair of 10×10 mm path length quartz cuvette was used for absorption experiments. Fluorescence spectroscopic measurements were carried out using a fluorimeter, model HITACHI S-7000 (HITACHI, Japan).


## 2.3. Preparation of Experimental Solutions

The uncertainty in weighing of the solid Na2[Ni(NaLH)2Cl2] · 2H2O was less than 0.3% indicating that the error in weighing is negligible or within acceptable limits. In the DNA interaction study, the concentration of Na2[Ni(NaLH)2Cl2] · 2H2O was 23.81 μM, that is, 23.81×10-6 mol dm−3. The solution was prepared by an exact dilution of a stock aqueous solution (2×10-4 mol dm−3) with an aqueous solution containing 0.500 mol dm−3 NaCl and 10×10-3 mol dm−3 Hepes buffer (pH 7.4) using a calibrated micropipette (Pipetman-M23866E, Gilson, France). To check concentrations of Na2[Ni(NaLH)2Cl2] · 2H2O in the experimental solutions, a calibration experiment (Lambert Beer’s Law) was done by measuring absorbance of different solutions of Na2[Ni(NaLH)2Cl2] · 2H2O of known strength at 465 nm, using which the concentration of Na2[Ni(NaLH)2Cl2] · 2H2O could be checked during the experiments. A 6.00×10-3 mol dm−3 aqueous solution of CT DNA (stock solution) was prepared and this was added quantitatively using a calibrated micropipette in each titration.


## 2.4. Methods

The electrochemical behavior of the Ni(II)-NaLH2 complex was studied in aqueous solution using cyclic voltammetry. Cyclic voltammetry was also carried out to study the interaction of the compound with calf thymus DNA. The non linear curve fit analysis usually applied in the spectrophotometric and fluorimetric studies was used first time in cyclic voltammetry studies to determine the binding parameters. The intercalation of Ni(II)-NaLH2 complex into DNA base pairs was established by competitive binding study using ethidium bromide in fluorescence spectroscopy.


## 3. Results and Discussion

### 3.1. Electrochemical Reduction of Na2[Ni(NaLH)2Cl2] · 2H2O in Aqueous Solution

In Hepes buffer [45], pH 7.4 containing 0.500 mol dm−3 NaCl, Na2[Ni(NaLH)2Cl2] · 2H2O (23.81×10-6 mol dm−3) undergoes one-electron reversible reduction generating a cathodic peak at −(515±5) mV (versus Ag/AgCl, satd. KCl) with the corresponding anodic peak at −(462  ±  5) mV (versus Ag/AgCl, satd. KCl); (Figure 1). The formal reduction potential (E1/2) was −(489 ± 5) mV (versus Ag/AgCl, satd. KCl). Previous study showed that the formal reduction potential for the one-electron reduction of sodium 1,4-dihdroxy-9,10-anthraquinone-2-sulphonate is −270 mV (versus NHE) [46], that is, −469 mV (versus Ag/AgCl, satd. KCl) which is nearer to the formal reduction potential of the complex Na2[Ni(NaLH)2Cl2] · 2H2O −(489 ± 5) mV (versus Ag/AgCl, satd. KCl) obtained in this study. The slight deviation in the value of the formal reduction potential of the Ni(II) complex is due to a different environment for the quinone in the metal complex. This indicates that in the present study the electron does not reduce Ni(II) in the complex to Ni(I); rather it reduces the free quinone site in the complex. Under the similar experimental conditions the cyclic voltammetry of 23.81×10-6 mol dm−3 NiCl2 (same concentration as that in the complex) did not exhibit any reduction or oxidation peak in the same potential range clearly indicating that Ni(II) present in the complex was not responsible for the peak. Thus it is evident from this study that the reduction and oxidation peaks of Na2[Ni(NaLH)2Cl2] · 2H2O are solely due to the quinone and not due to the Ni(II) present in the complex.Figure 1
Cyclic voltammogram of23.806×10-6 mol dm−3 Na2[Ni(NaLH)2Cl2] · 2H2O in Hepes buffer at pH 7.4 containing 0.500 mol dm−3 NaCl. Electrode: glassy carbon of surface area 0.1256 cm2; scan rate = 0.200 V/s, 25°C. Inset: typical plot of cathodic peak current versus square root of scan rate for the one-electron reduction of Na2[Ni(NaLH)2Cl2] · 2H2O in Hepes buffer at pH 7.4.In aqueous media, except for the cathodic peak at −(515 ± 5) mV (versus Ag/AgCl, satd. KCl) no other cathodic peak was observed at more negative potential. It was found that the ratio of the anodic to cathodic peak current(Ipa/Ipc) is less than unity in lower scan rate while at higher scan rate it is almost unity, indicating that in aqueous solution reduction of the compound at lower scan rates is quasireversible at physiological pH. The cathodic peak current (Ipc) for the reduction has a linear relationship with square root of scan rate that passes through the origin (inset of Figure 1) following equation-(1) [47] indicating that the reduction is diffusion controlled and that there is no adsorption on to the electrode surface. Therefore, it could be concluded that the reduction peak current (Ipc) has a linear relationship with concentration;(1)Ipc=0.4463(F3RT)1/2n3/2A0D01/2C0v1/2,
where, Ipc,n,A0,D0,C0,andvrefer to the cathodic peak current (A), number of electrons involved in the reduction, area of the electrode (cm2), diffusion coefficient (cm2s−1), concentration (mol cm−3), and scan rate (Vs−1), respectively. In our experiments temperature was maintained at 25°C (298 K) and therefore one gets the value of 0.4463(F3/RT)1/2 as 2.687×105 A s (mol V1/2)−1. Using (1) the diffusion coefficient of Na2[Ni(NaLH)2Cl2] · 2H2O was evaluated to be (1.15 ± 0.10) ×10-5 cm2s−1.Our recent studies [33, 34] showed that sodium 1,4-dihydroxy-9,10-anthraquinone-2-sulphonate undergoes diffusion-controlled two-electron reduction in aqueous media at any pH. The present study showed upon complex formation with metal ions, the electrochemical behavior of sodium 1,4-dihydroxy-9,10-anthraquinone-2-sulphonate changes significantly indicating an improvement in biochemical behavior. This could lead to a lesser generation of semiquinone, responsible for cardiotoxicity in anthracycline drugs [19, 20].


### 3.2. Interaction of Na2[Ni(NaLH)2Cl2] · 2H2O with CT DNA

Interaction of Na2[Ni(NaLH)2Cl2] · 2H2O with CT DNA was studied using cyclic voltammetry in aqueous buffer at physiological pH (7.4) containing 0.500 mol dm−3 NaCl.Since in aqueous solution the Ni(II) complex has negative charge on it and DNA being a negatively charged polymer there should be a repulsion in between the two. A high concentration of NaCl was used to suppress the negative charge on the Ni(II) complex and negative charge on DNA. Under the experimental conditions, the compound shows a cathodic peak at −(515 ± 5) mV (versus Ag/AgCl, satd. KCl); (curve-1, Figure2). Separate solutions were made containing a constant concentration (23.81×10−6 mol dm−3) of Na2[Ni(NaLH)2Cl2] · 2H2O and different concentrations of CT DNA. Cyclic voltammetry of each solution was carried out and the change in cathodic peak current at −515 mV (versus Ag/AgCl, satd. KCl) was used to construct binding isotherms. The cyclic voltammogram of the compound in the absence and presence of different amounts of CT DNA are shown in Figure 2. Under the same experimental conditions cyclic voltammetry experiments with pure DNA (curve 8 of Figure 2) show that there is no cathodic or anodic peak, clearly indicating that pure DNA is electrochemically inactive in the potential range 0.0 to −0.65 V on a glassy carbon electrode. Therefore, the cathodic peak current is exclusively due to the Ni(II) complex which gradually decreased with a positive shift (8 mV) with increasing amounts of CT DNA. The change in cathodic peak current (Ipc) at −515 mV (versus Ag/AgCl, satd. KCl) of Na2[Ni(NaLH)2Cl2] · 2H2O in presence of different CT DNA concentration is shown in Figure 3. At the high concentration of NaCl used (0.500 mol dm−3) charge on phosphate groups of DNA and the sulphonate oxygen of NaLH2 in the Ni(II) complex are suppressed [48]. As a result, electrostatic interaction between the Ni(II) complex and DNA would be almost negligible, suggesting intercalation as the main and dominating mode of interaction [48]. In an earlier pioneering study on metal complex-DNA interaction Bard et al. [49] reported a positive shift in peak potential for intercalators in the process of binding via hydrophobic interactions (intercalation) and said electrostatic interactions (groove binding) lead to a negative shift of peak potential. In our case upon increasing DNA concentration the cathodic peak decreased in current with a positive shift of about 8 mV. Comparing our results with those of Bard et al. [49] we could conclude that the Ni(II) complex intercalates into DNA base pairs (Scheme 2).Scheme 2
Proposed scheme for the intercalation of Na2[Ni(NaLH)2Cl2] · 2H2O into DNA base pairs.Figure 2
Cyclic voltammogram of23.806×10-6 mol dm−3 Na2[Ni(NaLH)2Cl2] · 2H2O in absence (1) and presence of different CT DNA concentrations (mol dm−3): 98.3×10-6 (2), 194.78×10-6 (3), 336.13×10-6 (4),  518.65×10-6(5), 694.67×10-6 (6), 906.07×10-6 (7); cyclic voltammogram of 289.44×10-6 mol dm−3  CT DNA (8); pH = 7.4, [NaCl] = 0.500 mol dm−3, scan rate 0.200 V/s, 25°C.Figure 3
Plot of cathodic peak current(Ip) of 23.806×10-6 mol dm−3 Na2[Ni(NaLH)2Cl2] · 2H2O in presence of different total CT DNA concentrations, CD (mol dm−3) = 0, 49.38×10-6; 98.30×10-6; 146.78×10-6; 194.78×10-6; 242.33×10-6; 336.13×10-6; 428.25×10-6; 518.65×10-6; 607.45×10-6; 694.67×10-6; 780.35×10-6; 906.07×10-6; 1028.58×10-6; 1147.57×10-6; 1264.35×10-6. [NaCl] = 0.500 mol dm−3, pH = 7.4, 25°C.Mode of binding was further established by carrying out competitive binding study using an established DNA intercalator ethidium bromide (EB) [50] and monitoring change in fluorescence under similar conditions of pH, ionic strength, and temperature. A solution of EB shows a strong absorption band with λmax at 470 nm which upon interaction with DNA shifts to 510 nm. When the DNA-EB adduct was excited at 510 nm fluorescence emission maxima was observed at 590 nm. A mixture containing 200×10-6 mol dm−3 CT DNA with saturating EB (4000×10-6 mol dm−3) was incubated for one hour and fluorescence was recorded (Figure 4(a)). To this mixture the complex Na2[Ni(NaLH)2Cl2] · 2H2O was added and fluorescence of the resultant mixture was taken at different time intervals ranging from incubation time t=0 (i.e., taken immediately after adding Ni(II) complex) to t=30 min (Figure 4(a)). It is evident from the figure that addition of the Ni(II) complex causes a decrease in fluorescence intensity on increasing incubation time.  As EB is an intercalator and since fluorescence occurs due to intercalation, a decrease in fluorescence upon addition of Na2[Ni(NaLH)2Cl2] · 2H2O clearly indicates that the complex intercalates between the strands of DNA for it replaces EB leading to loss in  fluorescence. Though EB is  amuch stronger  intercalator to DNA (having very high binding constant) in comparison to the Ni(II) complex but there is some competition between EB and Na2[Ni(NaLH)2Cl2] · 2H2O for binding to DNA that could be explained considering the equilibrium for binding of EB with ct DNA and that of Na2[Ni(NaLH)2Cl2] · 2H2O with ct DNA. Thus there is a replacement of EB from the already formed EB-DNA adduct by the Ni(II) complex according to the principle of chemical equilibrium.(a) Fluorescence spectra of (1)200×10-6 mol dm−3 DNA with saturating EB (4000×10-6 mol dm−3) incubated for 1 hour; (2) 200×10-6 mol dm−3 DNA with saturating EB (4000×10-6 mol dm−3) incubated for 1 hour followed by addition of 3×10-6 mol dm−3 Na2[Ni(NaLH)2Cl2] · 2H2O; (3) 200×10-6mol dm−3 DNA with saturating EB incubated for 1 hour followed by addition of 3×10-6mol dm−3 Na2[Ni(NaLH)2Cl2] · 2H2O with incubation time 30 mins. pH = 7.4, [NaCl] = 0.500 mol dm−3, 25°C. (b) Typical double reciprocal plot for Na2[Ni(NaLH)2Cl2] · 2H2O – CT DNA interaction; [Na2[Ni(NaLH)2Cl2] · 2H2O] =23.81×10-6 mol dm−3, pH = 7.4, [NaCl] = 0.500 mol dm−3, 25°C.
(a)(b)It needs to be mentioned that the decrease in the cathodic peak current upon addition of increasing amount of DNA is due to interaction of the Ni(II)-complex with DNA and not due to any blockage of the electrode surface by an adsorbed layer of DNA. To verify this we carried out cyclic voltammetry experiment of potassium ferricyanide in absence and presence of different amount of ct DNA under similar experimental conditions. It was observed that although concentration of ct DNA was increased, the cathodic peak current of potassium ferricyanide did not decrease, indicating that there was no adsorption of DNA onto the glassy carbon electrode surface. In a previous study involving metal complex-DNA interaction Bard et al. [49] established that a decrease in current in CV experiments was due to diffusion of the metal complex bound to the large, slowly diffusing DNA molecule. Enhanced viscosity of DNA solutions apparently has only a small effect on diffusion, and there is no significant obstruction of the glassy carbon surface via adsorption of DNA even at very high concentration of DNA (~5×10-3 mol dm−3) [49]. In our study, since we used ~1.3×10-3 mol dm−3 DNA concentration as maximum reasons obvious there is very little chance [49] of adsorption of DNA on to the glassy carbon electrode surface. In another DNA interaction study, Radi et al. [51] carried out a similar ferricyanide experiment to establish that the cyclic voltammetric behavior of their studied compound was not affected by the addition of a very large excess of DNA and decrease in peak current of the compound was due to interaction of the compound with DNA.Results of the DNA titration using cyclic voltammetry were analyzed by the method of nonlinear fitting. To do so, the following compound-DNA equilibrium was considered [32, 34–37, 52–55]:
(2)L+D⇌LDKd=⌊L⌋[D][LD]={[L0]-[LD]}{[D0]-[LD]}LD,
where L represents Na2[Ni(NaLH)2Cl2] · 2H2O, D represents CT DNA and LD, represents the DNA · Na2[Ni(NaLH)2Cl2] · 2H2O adduct. The dissociation constant (Kd)=1/K;Kbeing the apparent binding constant of the compound to DNA. [L0]= initial concentration of Na2[Ni(NaLH)2Cl2] · 2H2O = [Na2[Ni(NaLH)2Cl2] · 2H2O]0=23.81×10-6  mol dm−3 (which was kept constant during the titration experiment). [D0] = [DNA] = concentration of DNA added to an aliquot. If C0 be the initial concentration of Na2[Ni(NaLH)2Cl2] · 2H2O, that is, C0=[L0]=[Na2[Ni(NaLH)2Cl2] · 2H2O]0 and CD=[D0]=[DNA] = the concentration of DNA added to an aliquot then: (3)Kd={C0-⌊LD⌋}{CD-⌊LD⌋}[LD].As discussed earlier, reduction of the compound in aqueous buffer is purely diffusion controlled and that there is no adsorption on to the electrode surface. As there is no interference from the DNA bound form the cathodic peak current(Ipc) is therefore linearly proportional to the concentration of Na2[Ni(NaLH)2Cl2] · 2H2O (1) [40]. Using this linear relationship between cathodic peak current and concentration of the compound and applying the same analogy that one applies for absorption and fluorescence methods [32, 34–37, 52–55] the following parameters can be defined.ΔI=(Ipc0-Ipc)= change in cathodic peak current (Ipc) of Na2[Ni(NaLH)2Cl2] · 2H2O at −515 mV (versus Ag/AgCl, satd. KCl) upon each addition of CT DNA for each point of the titration curve. Ipc0 and Ipc are cathodic peak current of Na2[Ni(NaLH)2Cl2] · 2H2O at −515 mV (versus Ag/AgCl, satd. KCl)  in the absence and presence of different amounts of CT DNA respectively. ΔImax is the same parameter when the compound is totally bound to CT DNA. Therefore, (ΔI/ΔImax) denotes the fraction of Na2[Ni(NaLH)2Cl2] · 2H2O bound to DNA and one gets, (ΔI/ΔImax)C0=[LD]=[DNA · Na2[Ni(NaLH)2Cl2] · 2H2O]. At any point of the titration the cathodic peak current is due to the contribution of both the free and the bound forms. ΔI corresponds to (mcfi-m′cbi) where cbi refers to the concentration of the bound form of Na2[Ni(NaLH)2Cl2] · 2H2O, cfi being its corresponding concentration in absence of DNA. m is a constant equal to 0.4463 (F³/RT)1/2n3/2A0D01/2C0v1/2 for the free form of Na2[Ni(NaLH)2Cl2] · 2H2O, while m′ is the same constant for the bound form of Na2[Ni(NaLH)2Cl2] · 2H2O that is, DNA · Na2[Ni(NaLH)2Cl2] · 2H2O. Putting the value of [LD] in (3) one gets,(4)Kd=[C0-(ΔI/ΔImax⁡)C0][CD-(ΔI/ΔImax⁡)C0](ΔI/ΔImax⁡)C0,(5)C0(ΔIΔImax⁡)2-(C0+CD+Kd)(ΔIΔImax⁡)+CD=0,Determination ofKd using (5) requires the value of ΔImax which was determined by double reciprocal plot (Figure 4(b)) using (6) [32, 34–37, 52–55]:(6)1ΔI=1ΔImax⁡+KdΔImax⁡(CD-C0).This double reciprocal plot (Figure4(b)) was also used to determine the apparent dissociation constant (Kd). The apparent dissociation constant (Kd) was determined using nonlinear curve fit analysis using (5). All experimental points in binding isotherms were fitted by least square analysis. The basic assumption of this study is that the concentration of Na2[Ni(NaLH)2Cl2]2H2O was 23.81×10-6mol dm−3 (which was kept constant all along the titration) and CT DNA concentration was kept 53-fold greater than that of the compound.Binding stoichiometry or the binding site size was determined from the point of intersection of two straight lines obtained from the least square fit plot of normalized increase ofΔI/ΔImax against the ratio of concentration of CT DNA (in base) and the compound [52]. The two straight lines were drawn considering points before and after saturation, respectively [52]. The point of intersection of the two straight lines indicate a ratio of the moles of DNA (in bases) to the mole of the Ni(II) complex at the point in which the saturatation is just reached, that is, the number of DNA bases bound per molecule of  Na2[Ni(NaLH)2Cl2] · 2H2O. Figure 5 shows the binding isotherm of Na2[Ni(NaLH)2Cl2] · 2H2O and CT DNA. The apparent binding constant (K=1/Kd) was calculated using (5) as described above and obtained as (2.03 ± 0.10) ×103 mol−1 dm3. The apparent binding constant obtained from double reciprocal plot ((6), Figure 4(b)) is (2.01 ± 0.16) ×103 mol−1 dm3. It indicates that there is an excellent agreement between the apparent binding constant values obtained from two different mathematical methods. Inset of Figure 5 shows the plot of normalized increase of ΔI/ΔImax  as a function of mole-ratio of DNA to Na2[Ni(NaLH)2Cl2] · 2H2O. The point of intersection of the two straight lines drawn using points before and after saturation gives the stoichiometry or the binding site-size (n). For Na2[Ni(NaLH)2Cl2] · 2H2O the “n” value of binding to CT DNA is (29.02 ± 1.70) bases per molecule of Na2[Ni(NaLH)2Cl2] · 2H2O, that is, (14.51 ± 0.85) base pairs per molecule of Na2[Ni(NaLH)2Cl2] · 2H2O. Knowing n, the intrinsic binding constant K′, that is, (K×n) was obtained as (5.89 ± 0.10) ×104 mol−1 dm3. The intrinsic binding constant (K′) and binding site size (n) were also studied using absorption and fluorescence methods. The obtained values of K′ and n were 6.09×104 mol−1 dm3and 30 bases per molecule of Na2[Ni(NaLH)2Cl2] · 2H2O using absorption spectroscopy and 5.92×104 mol−1 dm3 and 32 bases per molecule of Na2[Ni(NaLH)2Cl2] · 2H2O using fluorescence spectroscopy, respectively [56]. Thus nonlinear curve fit analysis using cyclic voltammetry applied for first time to monitor  binding of compounds to DNA generates values that are in excellent agreement with those obtained earlier from spectroscopic methods. It should be mentioned here that sodium 1,4-dihydroxy-9,10-anthraquinone-2-sulphonate (NaLH2) intercalates into DNA base pairs with intrinsic binding constant and binding site size values of 3.44×104 mol−1 dm3 and 16 bases per molecule of NaLH2 respectively [34]. Since the Ni(II) ion occupies very little space binding of two NaLH2 units to Ni(II) makes the size of the complex almost double that of the ligand thus further corroborating an observation that the complex binds to (29.02 ± 1.70) bases with regard to the evaluated binding site of NaLH2 with CT DNA [30]. The binding site size data therefore justifies the ratio of binding of NaLH2 to Ni(II) in the complex (2 : 1) and therefore such studies can also help in determining  stoichiometry of the complex when both the ligand and its metal complex bind to DNA under almost identical experimental conditions. The intrinsic binding constant of the Ni(II) complex obtained from this experiment is ~1.7 times greater than that found for the interaction of sodium 1,4-dihydroxy-9,10-anthraquinone-2-sulphonate with CT DNA [34] and is also higher than that observed for the interaction of the Cu(II) complex of NaLH2 with CT DNA [32]. Introduction of a metal ion to the ligand by means of metal complex formation brings about better targeting of DNA [29, 32], and this study is actually able to show this. The interaction of Cu(II) and Ni(II) complexes were carried out using UV-Vis, fluorescence, and cyclic voltammetry repeatedly, and in all such studies we observed that the results were reproducible and the intrinsic binding constant for the Cu(II) complex-DNA interaction has a higher value in comparison to that of the Ni(II) complex. In strong NaCl media (0.500 mol dm−3) since the negative charge on Cu(II) and Ni(II) complexes and phosphate group of DNA were suppressed, therefore the effect of negative charge on the binding affinity of these metal complexes to DNA was insignificant. The extra electron present in Cu(II) (3d9) in comparison to Ni(II) (3d8) probably makes the Cu(II) complex-DNA adduct slightly weaker in binding CT DNA than the Ni(II) complex.Figure 5
Typical binding isotherm of Na2[Ni(NaLH)2Cl2] · 2H2O and CT DNA and corresponding nonlinear fit using cyclic voltammetry method; [Na2[Ni(NaLH)2Cl2] · 2H2O] = 23.81×10-6 mol dm−3, pH = 7.4, [NaCl] = 0.500 mol dm−3, 25°C; Inset: typical plot of normalized increase of cathodic peak current as a function of mole-ratio of CT DNA to Na2[Ni(NaLH)2Cl2] · 2H2O.


## 3.1. Electrochemical Reduction of Na2[Ni(NaLH)2Cl2] · 2H2O in Aqueous Solution

In Hepes buffer [45], pH 7.4 containing 0.500 mol dm−3 NaCl, Na2[Ni(NaLH)2Cl2] · 2H2O (23.81×10-6 mol dm−3) undergoes one-electron reversible reduction generating a cathodic peak at −(515±5) mV (versus Ag/AgCl, satd. KCl) with the corresponding anodic peak at −(462  ±  5) mV (versus Ag/AgCl, satd. KCl); (Figure 1). The formal reduction potential (E1/2) was −(489 ± 5) mV (versus Ag/AgCl, satd. KCl). Previous study showed that the formal reduction potential for the one-electron reduction of sodium 1,4-dihdroxy-9,10-anthraquinone-2-sulphonate is −270 mV (versus NHE) [46], that is, −469 mV (versus Ag/AgCl, satd. KCl) which is nearer to the formal reduction potential of the complex Na2[Ni(NaLH)2Cl2] · 2H2O −(489 ± 5) mV (versus Ag/AgCl, satd. KCl) obtained in this study. The slight deviation in the value of the formal reduction potential of the Ni(II) complex is due to a different environment for the quinone in the metal complex. This indicates that in the present study the electron does not reduce Ni(II) in the complex to Ni(I); rather it reduces the free quinone site in the complex. Under the similar experimental conditions the cyclic voltammetry of 23.81×10-6 mol dm−3 NiCl2 (same concentration as that in the complex) did not exhibit any reduction or oxidation peak in the same potential range clearly indicating that Ni(II) present in the complex was not responsible for the peak. Thus it is evident from this study that the reduction and oxidation peaks of Na2[Ni(NaLH)2Cl2] · 2H2O are solely due to the quinone and not due to the Ni(II) present in the complex.Figure 1
Cyclic voltammogram of23.806×10-6 mol dm−3 Na2[Ni(NaLH)2Cl2] · 2H2O in Hepes buffer at pH 7.4 containing 0.500 mol dm−3 NaCl. Electrode: glassy carbon of surface area 0.1256 cm2; scan rate = 0.200 V/s, 25°C. Inset: typical plot of cathodic peak current versus square root of scan rate for the one-electron reduction of Na2[Ni(NaLH)2Cl2] · 2H2O in Hepes buffer at pH 7.4.In aqueous media, except for the cathodic peak at −(515 ± 5) mV (versus Ag/AgCl, satd. KCl) no other cathodic peak was observed at more negative potential. It was found that the ratio of the anodic to cathodic peak current(Ipa/Ipc) is less than unity in lower scan rate while at higher scan rate it is almost unity, indicating that in aqueous solution reduction of the compound at lower scan rates is quasireversible at physiological pH. The cathodic peak current (Ipc) for the reduction has a linear relationship with square root of scan rate that passes through the origin (inset of Figure 1) following equation-(1) [47] indicating that the reduction is diffusion controlled and that there is no adsorption on to the electrode surface. Therefore, it could be concluded that the reduction peak current (Ipc) has a linear relationship with concentration;(1)Ipc=0.4463(F3RT)1/2n3/2A0D01/2C0v1/2,
where, Ipc,n,A0,D0,C0,andvrefer to the cathodic peak current (A), number of electrons involved in the reduction, area of the electrode (cm2), diffusion coefficient (cm2s−1), concentration (mol cm−3), and scan rate (Vs−1), respectively. In our experiments temperature was maintained at 25°C (298 K) and therefore one gets the value of 0.4463(F3/RT)1/2 as 2.687×105 A s (mol V1/2)−1. Using (1) the diffusion coefficient of Na2[Ni(NaLH)2Cl2] · 2H2O was evaluated to be (1.15 ± 0.10) ×10-5 cm2s−1.Our recent studies [33, 34] showed that sodium 1,4-dihydroxy-9,10-anthraquinone-2-sulphonate undergoes diffusion-controlled two-electron reduction in aqueous media at any pH. The present study showed upon complex formation with metal ions, the electrochemical behavior of sodium 1,4-dihydroxy-9,10-anthraquinone-2-sulphonate changes significantly indicating an improvement in biochemical behavior. This could lead to a lesser generation of semiquinone, responsible for cardiotoxicity in anthracycline drugs [19, 20].


## 3.2. Interaction of Na2[Ni(NaLH)2Cl2] · 2H2O with CT DNA

Interaction of Na2[Ni(NaLH)2Cl2] · 2H2O with CT DNA was studied using cyclic voltammetry in aqueous buffer at physiological pH (7.4) containing 0.500 mol dm−3 NaCl.Since in aqueous solution the Ni(II) complex has negative charge on it and DNA being a negatively charged polymer there should be a repulsion in between the two. A high concentration of NaCl was used to suppress the negative charge on the Ni(II) complex and negative charge on DNA. Under the experimental conditions, the compound shows a cathodic peak at −(515 ± 5) mV (versus Ag/AgCl, satd. KCl); (curve-1, Figure2). Separate solutions were made containing a constant concentration (23.81×10−6 mol dm−3) of Na2[Ni(NaLH)2Cl2] · 2H2O and different concentrations of CT DNA. Cyclic voltammetry of each solution was carried out and the change in cathodic peak current at −515 mV (versus Ag/AgCl, satd. KCl) was used to construct binding isotherms. The cyclic voltammogram of the compound in the absence and presence of different amounts of CT DNA are shown in Figure 2. Under the same experimental conditions cyclic voltammetry experiments with pure DNA (curve 8 of Figure 2) show that there is no cathodic or anodic peak, clearly indicating that pure DNA is electrochemically inactive in the potential range 0.0 to −0.65 V on a glassy carbon electrode. Therefore, the cathodic peak current is exclusively due to the Ni(II) complex which gradually decreased with a positive shift (8 mV) with increasing amounts of CT DNA. The change in cathodic peak current (Ipc) at −515 mV (versus Ag/AgCl, satd. KCl) of Na2[Ni(NaLH)2Cl2] · 2H2O in presence of different CT DNA concentration is shown in Figure 3. At the high concentration of NaCl used (0.500 mol dm−3) charge on phosphate groups of DNA and the sulphonate oxygen of NaLH2 in the Ni(II) complex are suppressed [48]. As a result, electrostatic interaction between the Ni(II) complex and DNA would be almost negligible, suggesting intercalation as the main and dominating mode of interaction [48]. In an earlier pioneering study on metal complex-DNA interaction Bard et al. [49] reported a positive shift in peak potential for intercalators in the process of binding via hydrophobic interactions (intercalation) and said electrostatic interactions (groove binding) lead to a negative shift of peak potential. In our case upon increasing DNA concentration the cathodic peak decreased in current with a positive shift of about 8 mV. Comparing our results with those of Bard et al. [49] we could conclude that the Ni(II) complex intercalates into DNA base pairs (Scheme 2).Scheme 2
Proposed scheme for the intercalation of Na2[Ni(NaLH)2Cl2] · 2H2O into DNA base pairs.Figure 2
Cyclic voltammogram of23.806×10-6 mol dm−3 Na2[Ni(NaLH)2Cl2] · 2H2O in absence (1) and presence of different CT DNA concentrations (mol dm−3): 98.3×10-6 (2), 194.78×10-6 (3), 336.13×10-6 (4),  518.65×10-6(5), 694.67×10-6 (6), 906.07×10-6 (7); cyclic voltammogram of 289.44×10-6 mol dm−3  CT DNA (8); pH = 7.4, [NaCl] = 0.500 mol dm−3, scan rate 0.200 V/s, 25°C.Figure 3
Plot of cathodic peak current(Ip) of 23.806×10-6 mol dm−3 Na2[Ni(NaLH)2Cl2] · 2H2O in presence of different total CT DNA concentrations, CD (mol dm−3) = 0, 49.38×10-6; 98.30×10-6; 146.78×10-6; 194.78×10-6; 242.33×10-6; 336.13×10-6; 428.25×10-6; 518.65×10-6; 607.45×10-6; 694.67×10-6; 780.35×10-6; 906.07×10-6; 1028.58×10-6; 1147.57×10-6; 1264.35×10-6. [NaCl] = 0.500 mol dm−3, pH = 7.4, 25°C.Mode of binding was further established by carrying out competitive binding study using an established DNA intercalator ethidium bromide (EB) [50] and monitoring change in fluorescence under similar conditions of pH, ionic strength, and temperature. A solution of EB shows a strong absorption band with λmax at 470 nm which upon interaction with DNA shifts to 510 nm. When the DNA-EB adduct was excited at 510 nm fluorescence emission maxima was observed at 590 nm. A mixture containing 200×10-6 mol dm−3 CT DNA with saturating EB (4000×10-6 mol dm−3) was incubated for one hour and fluorescence was recorded (Figure 4(a)). To this mixture the complex Na2[Ni(NaLH)2Cl2] · 2H2O was added and fluorescence of the resultant mixture was taken at different time intervals ranging from incubation time t=0 (i.e., taken immediately after adding Ni(II) complex) to t=30 min (Figure 4(a)). It is evident from the figure that addition of the Ni(II) complex causes a decrease in fluorescence intensity on increasing incubation time.  As EB is an intercalator and since fluorescence occurs due to intercalation, a decrease in fluorescence upon addition of Na2[Ni(NaLH)2Cl2] · 2H2O clearly indicates that the complex intercalates between the strands of DNA for it replaces EB leading to loss in  fluorescence. Though EB is  amuch stronger  intercalator to DNA (having very high binding constant) in comparison to the Ni(II) complex but there is some competition between EB and Na2[Ni(NaLH)2Cl2] · 2H2O for binding to DNA that could be explained considering the equilibrium for binding of EB with ct DNA and that of Na2[Ni(NaLH)2Cl2] · 2H2O with ct DNA. Thus there is a replacement of EB from the already formed EB-DNA adduct by the Ni(II) complex according to the principle of chemical equilibrium.(a) Fluorescence spectra of (1)200×10-6 mol dm−3 DNA with saturating EB (4000×10-6 mol dm−3) incubated for 1 hour; (2) 200×10-6 mol dm−3 DNA with saturating EB (4000×10-6 mol dm−3) incubated for 1 hour followed by addition of 3×10-6 mol dm−3 Na2[Ni(NaLH)2Cl2] · 2H2O; (3) 200×10-6mol dm−3 DNA with saturating EB incubated for 1 hour followed by addition of 3×10-6mol dm−3 Na2[Ni(NaLH)2Cl2] · 2H2O with incubation time 30 mins. pH = 7.4, [NaCl] = 0.500 mol dm−3, 25°C. (b) Typical double reciprocal plot for Na2[Ni(NaLH)2Cl2] · 2H2O – CT DNA interaction; [Na2[Ni(NaLH)2Cl2] · 2H2O] =23.81×10-6 mol dm−3, pH = 7.4, [NaCl] = 0.500 mol dm−3, 25°C.
(a)(b)It needs to be mentioned that the decrease in the cathodic peak current upon addition of increasing amount of DNA is due to interaction of the Ni(II)-complex with DNA and not due to any blockage of the electrode surface by an adsorbed layer of DNA. To verify this we carried out cyclic voltammetry experiment of potassium ferricyanide in absence and presence of different amount of ct DNA under similar experimental conditions. It was observed that although concentration of ct DNA was increased, the cathodic peak current of potassium ferricyanide did not decrease, indicating that there was no adsorption of DNA onto the glassy carbon electrode surface. In a previous study involving metal complex-DNA interaction Bard et al. [49] established that a decrease in current in CV experiments was due to diffusion of the metal complex bound to the large, slowly diffusing DNA molecule. Enhanced viscosity of DNA solutions apparently has only a small effect on diffusion, and there is no significant obstruction of the glassy carbon surface via adsorption of DNA even at very high concentration of DNA (~5×10-3 mol dm−3) [49]. In our study, since we used ~1.3×10-3 mol dm−3 DNA concentration as maximum reasons obvious there is very little chance [49] of adsorption of DNA on to the glassy carbon electrode surface. In another DNA interaction study, Radi et al. [51] carried out a similar ferricyanide experiment to establish that the cyclic voltammetric behavior of their studied compound was not affected by the addition of a very large excess of DNA and decrease in peak current of the compound was due to interaction of the compound with DNA.Results of the DNA titration using cyclic voltammetry were analyzed by the method of nonlinear fitting. To do so, the following compound-DNA equilibrium was considered [32, 34–37, 52–55]:
(2)L+D⇌LDKd=⌊L⌋[D][LD]={[L0]-[LD]}{[D0]-[LD]}LD,
where L represents Na2[Ni(NaLH)2Cl2] · 2H2O, D represents CT DNA and LD, represents the DNA · Na2[Ni(NaLH)2Cl2] · 2H2O adduct. The dissociation constant (Kd)=1/K;Kbeing the apparent binding constant of the compound to DNA. [L0]= initial concentration of Na2[Ni(NaLH)2Cl2] · 2H2O = [Na2[Ni(NaLH)2Cl2] · 2H2O]0=23.81×10-6  mol dm−3 (which was kept constant during the titration experiment). [D0] = [DNA] = concentration of DNA added to an aliquot. If C0 be the initial concentration of Na2[Ni(NaLH)2Cl2] · 2H2O, that is, C0=[L0]=[Na2[Ni(NaLH)2Cl2] · 2H2O]0 and CD=[D0]=[DNA] = the concentration of DNA added to an aliquot then: (3)Kd={C0-⌊LD⌋}{CD-⌊LD⌋}[LD].As discussed earlier, reduction of the compound in aqueous buffer is purely diffusion controlled and that there is no adsorption on to the electrode surface. As there is no interference from the DNA bound form the cathodic peak current(Ipc) is therefore linearly proportional to the concentration of Na2[Ni(NaLH)2Cl2] · 2H2O (1) [40]. Using this linear relationship between cathodic peak current and concentration of the compound and applying the same analogy that one applies for absorption and fluorescence methods [32, 34–37, 52–55] the following parameters can be defined.ΔI=(Ipc0-Ipc)= change in cathodic peak current (Ipc) of Na2[Ni(NaLH)2Cl2] · 2H2O at −515 mV (versus Ag/AgCl, satd. KCl) upon each addition of CT DNA for each point of the titration curve. Ipc0 and Ipc are cathodic peak current of Na2[Ni(NaLH)2Cl2] · 2H2O at −515 mV (versus Ag/AgCl, satd. KCl)  in the absence and presence of different amounts of CT DNA respectively. ΔImax is the same parameter when the compound is totally bound to CT DNA. Therefore, (ΔI/ΔImax) denotes the fraction of Na2[Ni(NaLH)2Cl2] · 2H2O bound to DNA and one gets, (ΔI/ΔImax)C0=[LD]=[DNA · Na2[Ni(NaLH)2Cl2] · 2H2O]. At any point of the titration the cathodic peak current is due to the contribution of both the free and the bound forms. ΔI corresponds to (mcfi-m′cbi) where cbi refers to the concentration of the bound form of Na2[Ni(NaLH)2Cl2] · 2H2O, cfi being its corresponding concentration in absence of DNA. m is a constant equal to 0.4463 (F³/RT)1/2n3/2A0D01/2C0v1/2 for the free form of Na2[Ni(NaLH)2Cl2] · 2H2O, while m′ is the same constant for the bound form of Na2[Ni(NaLH)2Cl2] · 2H2O that is, DNA · Na2[Ni(NaLH)2Cl2] · 2H2O. Putting the value of [LD] in (3) one gets,(4)Kd=[C0-(ΔI/ΔImax⁡)C0][CD-(ΔI/ΔImax⁡)C0](ΔI/ΔImax⁡)C0,(5)C0(ΔIΔImax⁡)2-(C0+CD+Kd)(ΔIΔImax⁡)+CD=0,Determination ofKd using (5) requires the value of ΔImax which was determined by double reciprocal plot (Figure 4(b)) using (6) [32, 34–37, 52–55]:(6)1ΔI=1ΔImax⁡+KdΔImax⁡(CD-C0).This double reciprocal plot (Figure4(b)) was also used to determine the apparent dissociation constant (Kd). The apparent dissociation constant (Kd) was determined using nonlinear curve fit analysis using (5). All experimental points in binding isotherms were fitted by least square analysis. The basic assumption of this study is that the concentration of Na2[Ni(NaLH)2Cl2]2H2O was 23.81×10-6mol dm−3 (which was kept constant all along the titration) and CT DNA concentration was kept 53-fold greater than that of the compound.Binding stoichiometry or the binding site size was determined from the point of intersection of two straight lines obtained from the least square fit plot of normalized increase ofΔI/ΔImax against the ratio of concentration of CT DNA (in base) and the compound [52]. The two straight lines were drawn considering points before and after saturation, respectively [52]. The point of intersection of the two straight lines indicate a ratio of the moles of DNA (in bases) to the mole of the Ni(II) complex at the point in which the saturatation is just reached, that is, the number of DNA bases bound per molecule of  Na2[Ni(NaLH)2Cl2] · 2H2O. Figure 5 shows the binding isotherm of Na2[Ni(NaLH)2Cl2] · 2H2O and CT DNA. The apparent binding constant (K=1/Kd) was calculated using (5) as described above and obtained as (2.03 ± 0.10) ×103 mol−1 dm3. The apparent binding constant obtained from double reciprocal plot ((6), Figure 4(b)) is (2.01 ± 0.16) ×103 mol−1 dm3. It indicates that there is an excellent agreement between the apparent binding constant values obtained from two different mathematical methods. Inset of Figure 5 shows the plot of normalized increase of ΔI/ΔImax  as a function of mole-ratio of DNA to Na2[Ni(NaLH)2Cl2] · 2H2O. The point of intersection of the two straight lines drawn using points before and after saturation gives the stoichiometry or the binding site-size (n). For Na2[Ni(NaLH)2Cl2] · 2H2O the “n” value of binding to CT DNA is (29.02 ± 1.70) bases per molecule of Na2[Ni(NaLH)2Cl2] · 2H2O, that is, (14.51 ± 0.85) base pairs per molecule of Na2[Ni(NaLH)2Cl2] · 2H2O. Knowing n, the intrinsic binding constant K′, that is, (K×n) was obtained as (5.89 ± 0.10) ×104 mol−1 dm3. The intrinsic binding constant (K′) and binding site size (n) were also studied using absorption and fluorescence methods. The obtained values of K′ and n were 6.09×104 mol−1 dm3and 30 bases per molecule of Na2[Ni(NaLH)2Cl2] · 2H2O using absorption spectroscopy and 5.92×104 mol−1 dm3 and 32 bases per molecule of Na2[Ni(NaLH)2Cl2] · 2H2O using fluorescence spectroscopy, respectively [56]. Thus nonlinear curve fit analysis using cyclic voltammetry applied for first time to monitor  binding of compounds to DNA generates values that are in excellent agreement with those obtained earlier from spectroscopic methods. It should be mentioned here that sodium 1,4-dihydroxy-9,10-anthraquinone-2-sulphonate (NaLH2) intercalates into DNA base pairs with intrinsic binding constant and binding site size values of 3.44×104 mol−1 dm3 and 16 bases per molecule of NaLH2 respectively [34]. Since the Ni(II) ion occupies very little space binding of two NaLH2 units to Ni(II) makes the size of the complex almost double that of the ligand thus further corroborating an observation that the complex binds to (29.02 ± 1.70) bases with regard to the evaluated binding site of NaLH2 with CT DNA [30]. The binding site size data therefore justifies the ratio of binding of NaLH2 to Ni(II) in the complex (2 : 1) and therefore such studies can also help in determining  stoichiometry of the complex when both the ligand and its metal complex bind to DNA under almost identical experimental conditions. The intrinsic binding constant of the Ni(II) complex obtained from this experiment is ~1.7 times greater than that found for the interaction of sodium 1,4-dihydroxy-9,10-anthraquinone-2-sulphonate with CT DNA [34] and is also higher than that observed for the interaction of the Cu(II) complex of NaLH2 with CT DNA [32]. Introduction of a metal ion to the ligand by means of metal complex formation brings about better targeting of DNA [29, 32], and this study is actually able to show this. The interaction of Cu(II) and Ni(II) complexes were carried out using UV-Vis, fluorescence, and cyclic voltammetry repeatedly, and in all such studies we observed that the results were reproducible and the intrinsic binding constant for the Cu(II) complex-DNA interaction has a higher value in comparison to that of the Ni(II) complex. In strong NaCl media (0.500 mol dm−3) since the negative charge on Cu(II) and Ni(II) complexes and phosphate group of DNA were suppressed, therefore the effect of negative charge on the binding affinity of these metal complexes to DNA was insignificant. The extra electron present in Cu(II) (3d9) in comparison to Ni(II) (3d8) probably makes the Cu(II) complex-DNA adduct slightly weaker in binding CT DNA than the Ni(II) complex.Figure 5
Typical binding isotherm of Na2[Ni(NaLH)2Cl2] · 2H2O and CT DNA and corresponding nonlinear fit using cyclic voltammetry method; [Na2[Ni(NaLH)2Cl2] · 2H2O] = 23.81×10-6 mol dm−3, pH = 7.4, [NaCl] = 0.500 mol dm−3, 25°C; Inset: typical plot of normalized increase of cathodic peak current as a function of mole-ratio of CT DNA to Na2[Ni(NaLH)2Cl2] · 2H2O.


## 4. Conclusion

In aqueous buffer at physiological pH the Ni(II) complex of sodium 1,4-dihydroxy-9,10-anthraquinone-2-sulphonate (NaLH2), that is, Na2[Ni(NaLH)2Cl2] · 2H2O undergoes diffusion-controlled one-electron reduction. The redox behavior of sodium 1,4-dihydroxy-9,10-anthraquinone-2-sulphonate is modified significantly in the Ni(II) complex-indicating an improvement in biochemical behavior. The Ni(II) complex intercalates calf thymus DNA which was established by competitive binding study with ethidium bromide. Interaction with CT DNA was  monitored by cyclic voltammetry (CV) and binding parameters was determined for the first time using nonlinear curve fit analysis by monitoring the cathodic peak current of the compound. The intrinsic binding constant (K′) and the bind site size for interaction were found to be (5.89 ± 0.10) ×104 mol−1 dm3 and (29.02 ± 1.70) bases per molecule of Na2[Ni(NaLH)2Cl2] · 2H2O, respectively. The bind site size for the interaction of Ni(II) complex with CT DNA is double to the same for the ligand NaLH2 under similar experimental condition. The intrinsic binding constant for Na2[Ni(NaLH)2Cl2] · 2H2O – CT DNA interaction obtained from this experiment is ~1.7-times greater than that found for the interaction of sodium 1,4-dihydroxy-9,10-anthraquinone-2-sulphonate (NaLH2) with CT DNA indicating an improvement in biochemical action of NaLH2 in the form of the metal complex.



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*Source: 183745-2011-07-25.xml*