Interaction of Iron ( III )-5 , 10 , 15 , 20-Tetrakis ( 4-Sulfonatophenyl ) Porphyrin with Chloroquine , Quinine and Quinidine

Iron(III)-5,10,15,20-tetrakis(4-sulfonatophenyl) porphyrin (FeTPPS) is used as non-physiological metalloporphyrin model for the natural iron (III)-protoporphyrin IX (FePPIX) resulting from hemoglobin degradation to investigate ligand binding reactions in aqueous solution. Studies were conducted on the interaction of FeTPPS with Chloroquine, Quinine, and Quinidine, which are historically the most common quinoline-based drugs used to treat malaria, an infectious disease afflicting several hundred millions every year worldwide, mainly in tropical regions. Using UV-Visible spectrophotometry, the binding reaction was studied at pH 7.40 in purely aqueous solution, and in aqueous solution containing NaNO3 at concentration of 0.1 M. Fitted titration curves obtained were in agreement with experimental data according to a formation scheme of 1:1 complex (1 FeTPPS μ-oxo-dimer: 1 Antimalarial). Values of apparent binding constant (K) obtained were between 4.3 × 103 M−1 to 7.59 × 104 M−1, demonstrating that FeTPPS and the antimalarials formed stable complexes. The stability of the complex decreased when NaNO3 was added to the solution. This ionic strength dependence was ascribed to electrostatic effects. Quinine and Chloroquine interacted with FeTPPS stronger than Quinidine did. Chloroquine showed the strongest affinity to FeTPPS. These findings revealed the influence of steric and stereochemical factors. Molecular electrostatic potentials (MEP) calculated with Hartree-Fock theory argue in favor of π-π and electrostatic interactions between reaction partners as driving forces for the complex formation. In the case of FeTPPS: ChloroHow to cite this paper: Bibelayi, D.D., Kilunga, P.I., Lundemba, A.S., Bokolo, M.K., Mpiana, P.T., Tsalu, P.V., Pradon, J., Groom, C.C., Kadima, C.W., Van Meervelt, L. and Yav, Z.G. (2017) Interaction of Iron(III)-5, 10,15,20-Tetrakis(4-Sulfonatophenyl) Porphyrin with Chloroquine, Quinine and Quinidine. Crystal Structure Theory and Applications, 6, 25-38. https://doi.org/10.4236/csta.2017.63003 Received: June 1, 2017 Accepted: August 8, 2017 Published: August 11, 2017 Copyright © 2017 by authors and Scientific Research Publishing Inc. This work is licensed under the Creative Commons Attribution International License (CC BY 4.0). http://creativecommons.org/licenses/by/4.0/

quine interaction, it is suggested that an intramolecular hydrogen bond is formed between phenyl
FePPIX has been suggested as drug target of quinoline-based antimalarials [4] [9] [10] [11] [12] [13].FePPIX is the oxidized form of heme released by the malarial parasite during the blood stage.The parasite digests hemoglobin in infected erythrocytes to recuperate the amino acids it needs.Detoxification of free heme into the acidic digestive vacuole is achieved by the formation of a polymer well known as hemozoin (β-hematin) or malarial pigment [4] [14].The interaction of quinoline antimalarial with FePPIX plays the important role of bringing  back the porphyrin into solution in order to block FePPIX unities, and to prevent the formation of hemozoin.The binding of FePPIX and its derivate Iron(III)-deuteroporphyrin IX (FeDPIX) to quinoline-based antimalarials Chloroquine, Quinine and Quinidine (Figure 2) have been demonstrated in vitro using mixtures of water with ethylene glycol, propylene glycol and DMSO [4] [11] [12] [15] [16] [17] [18].It has been shown that the interaction depends on steric, stereochemical and electrostatic effects.Quinine is a carbinol-4 quinoline, originally derived from the bark of the cinchona tree.Quinidine is a stereoisomer of Quinine.Chloroquine is a 4-aminoquinoline long used in the malaria prevention and treatment, as it was cheap and widely available, before the most dangerous malarial parasite Plasmodium falciparum started to develop resistance to it.
It has been suggested that the most important driving forces for the formation of the complex are π-π and hydrophobic interactions between the porphyrin ring and quinoline ring.The coordination of the iron center of Ferri-porphyrin by the alcohol/alkoxy functionality and an intramolecular hydrogen bond formed between the protonated quaternary quinuclidine nitrogen atom of a drug molecule and the negatively charged propionate side chain of the Ferri-porphyrin have been also mentioned as additional forces stabilizing the complex [12] [15] [19] [20].Growing resistance of the Plasmodium to the quinoline antimalarials spurred the development of a new antimalarial pharmacological approach based on designing new molecules [21] [22].A new antimalarial chemotherapy has been reported based on choline analogues with novel mechanisms of action [7] [23].The authors reported that these drugs are "dual molecules", structurally unrelated to existing antimalarial agents, acting through two mechanisms: they interact with the plasmodial phospholipid metabolism and also with the malarial FePPIX polymer.However, quantitative studies of the interaction of the iron (III) porphyrin FePPIX in pure aqueous solution, the physiological medium, are hampered by the tendency of FePPIX to form aggregates considerably larger than dimers.In weakly acid and neutral solutions of FePPIX, a stable state cannot be achieved probably due to colloidal precipitation leading to artefacts in quantitative investigations [4] [7] [11] [15] [20] [24].FeTPPS is sufficiently soluble in aqueous solution in a wide pH range due to four very strong acid groups (SO 3 H) compared to two weak acid groups (-CH 2 CH 2 CO 2 H) of FePPIX.Dimerization of FeTPPS into μ-oxo-Dimer (O-FeTPPS 2 ) can also be well controlled un-der experimental conditions in aqueous solution [3] [25] [26].In this study, we report the results of the interaction of the iron porphyrin FeTPPS with Chloroquine, Quinine and Quinidine in pure aqueous solution and in aqueous solution containing NaNO 3 .The main goal is to explore the use of FeTPPS as ferric porpohryin model for the natural FePPIX for binding reactions in aqueous solution, the biological medium.FeTPPS has been considered as a non-physiological metalloporphyrin model for FePPIX.Gibbs E. et al. [27] investigated the interaction of Hemopoxin with FeTPPS used as model for FePPIX, which is the presumed target of the serum protein in blood stream.The authors demonstrated that hemopoxin is capable of binding with either Monomers or μ-oxo-Dimers of FeTPPS.Complexes of FeTPPS with Nitric Oxide and Per-O-methylated-Cyclodextrin have also been used as primary models for FePPIX in ferrihemoproteins [5] [6].

Chemicals
FeTPPS acid chloride, Chloroquine diphosphate and Quinidine, and Quinine were purchased from Frontier Scientific, Fluka (PA) and Merck (PA), respectively.Tris(hydroxymethyl) aminomethane (TRIS) was from Sigma Aldrich (PA).Stock solutions of FeTPPS and antimalarials were prepared in Mil-liQ-water (MQ-water) and buffered with TRIS.All static measurements were carried out in solutions containing 0.01 M buffer.The pH values were measured with a glass electrode, which was soaked and kept in aqueous solution of KCl (3 M) and was calibrated with aqueous standard buffers.A series of titration solutions at pH 7.40 were prepared as previously described [4] [28] in which the concentrations of FeTPPS μ-oxo dimer (D), TRIS and NaNO 3 were held constant, at 5 × 10 −6 M, 0.01 M and 0 or 0.1 M, respectively, while the concentrations of the antimalarial ligand (L) were varied from 0 to 1.5 M.

UV-Visible Spectrophotometric Study
Experimental titration curves were carried out with a Perkin Elmer Lambda 40 UV-Visible spectrophotometer.Fitted curves were performed using a nonlinear least-squares regression based on the scheme describing the formation of a 1:1 complex (Scheme 1) according to the equation (Scheme 2) previously reported by Yav Gushimana et al. [3].

Computational Study
In addition to the experimental studies, a computational study was performed to Model of Binding reaction of μ-oxo-FeTPPS Dimer (D) with antimalarial ligand as ligand (A).K is the binding constant related to activities of reaction partners.Thus, K is depending on ionic strength.For diluted solutions, K is an apparent binding constant related to concentrations: ( ) Nonlinear least-squares regression equation for the formation of 1:1 complex assuming that 0 A ε ≅ at wavelength of titration [3], and consequently calculate molecular electrostatic potentials (MEP) based on the Hartree-Fock theory at basis sets 6 -31 G(d) and 3 -21 G implemented in GAUSSIAN09 [29].
The value of 0.1 a.u. was used for the isopotential.

CSD Analysis
The Cambridge Structural Database (CSD) Version 5.38 [November 2016] with a total of 843,799 structural entries was also used to explore the ability of phenyl 3 SO − and protonated nitrogen to form hydrogen bond.We used the CSD system program ConQuest program for substructure searches and the location of non-bonded interactions [30] with the following secondary search criteria: atomic coordinates present in the entry and error-free after CSD evaluation; no disorder in the crystal structure; no polymeric (catena) bonding; no powder studies; crystallographic R-factor ≤ 0.10; only organic structures (according to standard CSD definitions).The CSD System program Mercury [31] [32] was used for 3D structure visualizations.

UV-Visible Spectrophotometry
The Figure 3 depicts the absorption of FeTPPS and the antimalarial-based drugs between 600 nm to 350 nm.As it is shown, given that the results were the same for the three antimalarial-based drugs, only Chloroquine is plotted.We can see that (Figure 3) no absorption of quinoline-based antimalarials was observed in the visible region as illustrated with Chloroquine, whereas the spectrum of FeTPPS has a marked peak in the Soret Band around 413 nm and a small peak around 565nm (Figure 3).These peaks correspond very well to those at 415 nm and 565 nm, respectively, previously reported for μ-oxo-Dimer of FeTPPPS [25].And the variation of Extinction of FeTPPS at 410 nm in pure aqueous solution at pH 7.40 versus concentration is plotted in Figure 4.
It can be seen that the absorption increases linearly obeying Beer's Law.This behavior demonstrates that only one species predominates in solution under the experimental conditions.Fitting of the molar absorption coefficient by the least-squares regression provides a value of (1.59 ± 0.02) × 10 5 M −1 •cm −1 , which is in good agreement with the value of 1.15 × 10 5 M −1 •cm −1 previously reported for the absorption of FeTPPS μ-oxo-Dimer [25].Figure 5 shows titration of FeTPPS with Quinidine, which illustrates typical spectral changes in the Soret band of FeTPPS when the ferriporphyrin was titrated with antimalarial drug.as the quinoline containing antimalarials with the strongest affinity to FePPIX [28].They also argued that the affinity of the antimalarials depends on ionic strength and stereochemical factors.Figure 6 illustrates the experimental titration curves of FeTPPS with antimalarial drugs.The shape of titration curves reveals that the absorbance of the μ-oxo-Dimer decreases steeply and becomes relatively steady with the increase of the ligands as expected [4] [15] [28] [33] [34].The complexation parameters were determined by plotting the titration curves of FeTPPS with antimalarial drugs according to the nonlinear least-squares regression equation (Scheme 2).Results (Figure 6) are in good agreement with curves fitted according to the formation    4) and those reported by Everly et al. for FeTPPS μ-oxo-Dimer [25].The values of the apparent binding constant (K) calculated from fitted curves are listed in Table 1.
The values of the apparent binding constant (Table 1) reveal that FeTPPS forms stable complexes with Chloroquine, Quinine and Quinidine in aqueous solution as well as FePPIX and its derivative FeDPPIX do in mixtures of water with organic solvents like glycol and DMSO.Values K of (0.33 ± 0.06) × 10 5 M −1 and (0.11 ± 0.03) × 10 5 M −1 have been obtained for the complex formation of FePPIX with Chloroquine and Quinine, respectively, in 50% water-propylene glycol mixture at pH 7.40 [28] [34].Kai F. et al. [13] reported constants of dissociation for the complex formed between Chloroquine and FePPIX μ-oxo-dimer at pH 6.5 and pH 9 of 3.9 × 10 −6 M −1 and 4.1 × 10 −6 M −1 , respectively, which correspond to 2.6 × 10 5 M −1 and 2.4 × 10 5 M −1 in terms of binding constant.FeTPPS has the strongest affinity to Chloroquine in comparison to Quinine and Quinidine under the same experimental conditions.The affinity of FeTPPS to Quinine and Chloroquine decreases in aqueous solution when NaNO 3 is added.These findings are similar to those for the binding of FePPIX and its derivate FeDPIX to quinoline antimalarials [15] [28] [33] [34].It can be assumed that similar forces are involved in the interaction of FePPIX, FeDPIX and FeTPPS with the quinoline-based antimalarials considering that these ferriporphyrins have similar molecular structures.The main forces driving the complexation, as suggested, are π-π stacking between the quinoline ring and the porphyrin ring, hydrophobic interactions, and electrostatic interactions [4] [19] [20] [28] [33] [34] [35].De Villiers et al. [20] demonstrated that additional forces providing further stability of complexes between ferriporphyrins and carbinol-4 quinoline drugs are the possible coordination of the iron (III) by the alcohol/alkoxy functionality and a hydrogen bond formed between the protonated quinuclidine nitrogen atom and the propionate side chain.The strong affinity of Chloroquine to ferriporphyrins suggests that the complex is stabilized by the flexible aliphatic side-chain of Chloroquine, which is less crowded than the stiff quinuclidine group of Quinine and Quinidine [4] [20] [28].The decrease of the FeTPPS affin-ity to Quinine and Chloroquine by addition of NaNO 3 illustrates the dependence of the complex stability on ionic strength.The influence of ionic strength on the complex stability was also found by investigations in polar mixtures of water with ethylene-or propylene glycol [15] [28] [34].However, no effects of ionic strength, which is characteristic of electrostatic interactions, have been observed in mixtures of water and DMSO probably due the weak polarity of the medium [18].One could attribute the decrease of affinity to the influence of the ionic strength on the formation of FeTPPS μ-oxo-Dimer.However, no major spectral change of FeTPPS absorption is observed in aqueous solution containing NaNO 3 compared to the absorption in solution without NaNO 3 (Figure 3 and Figure 5).Moreover, the values of the molar absorption coefficient fitted from titration are consistent with the value of the molar absorption coefficient of the FeTPPS μ-oxo-Dimer reported by Everly et al. [25].In aqueous solution at pH value of 7.40, the acid phenylsulfonic group of FeTPPS is dissociated in anionic form and H + as the value of the dissociation constant pKa is 4.8 [25].Investigations on the acid dissociation of protonated nitrogen atoms of quinoline antimalarials in aqueous solution provided two apparent constants, pKa 1 and pKa 2 , [36] [37].The authors found, respectively, pKa 1 and pKa 2 values of 8.08 and 10.16 for Chloroquine, 3.67 and 7.95 for Quinine and 3.50 and 7.81 for Quinidine.According to these pKa1 and pKa 2 values, two nitrogen atoms of Chloroquine are protonated and only, one nitrogen atom (pKa 2 ) of Quinine and Quinidine is protonated according to values of pKa 2 at pH 7.40.Thus, the observation that the addition of NaNO 3 at high concentration in solution decreases the electrostatic interactions can be ascribed to shielding effects of Na + and 3 NO − counter- ions on interacting charged groups in FeTPPS and antimalarial molecules [15] [28] [33].In comparison to FePPIX and FeDPIX, two additional negative groups are provided to FeTPPS by phenylsulfonate side chains.However, no enhancement of electrostatic interactions and, consequently, no increased affinity of FeTPPS to antilamarial drugs is observed as expected.Contrary, K values of FeTPPS complexes are lower than those of FePPIX and FeDPIX complexes.This behavior demonstrates the main role played by steric effects on complex stability.

Molecular Electrostatic Potentials
The calculation of molecular electrostatic potential surfaces revealed that there are regions of negative charges and positive charges in the ferriporphyrins and the antimalarial molecule as expected.Marked negative charges (in red) are around the carboxylic groups of propionate side chains of FePPIX and sulfonic groups of sulfonate side chains of FeTPPS, but also around oxygen and nitrogen atoms of antimalarials (Figure 7).These charged sites are probably responsible for electrostatic interactions between FeTPPS and antimalarial drugs enhanced in aqueous solution.However, Figure 3 also shows that the steric mesophenylsulfonic groups of FeTPPS are symmetrically disposed, all orthogonal to the porphyrin plane.Thus, electrostat-  ic interactions as well as the π-π stacking between the quinoline ring of antimalarials and the porphyrin ring of FeTPPS can be hampered by steric effects.

CSD Analysis
The complete CSD (all entries, with no secondary filters applied) contained 17,755 CSD searches provided many crystal structures forming relatively strong-3 SO − … H-N + hydrogen bonds with median values of normalized lengths be- tween 1.65 to 2.72 Å.This suggests that an additional hydrogen bond between the protonated quinuclidine nitrogen atom of Chloroquine and the negatively charged sulfonate side chain of FeTPPS molecule is also possible, which increases the complex stability.

Conclusion
The binding of FeTPPS to Chloroquine, Quinine and Quinidine in aqueous solution was investigated using UV-Visible spectrophotometry in conjunction with quantum mechanical calculations and (Cambridge Structural Database) CSD analysis.The results of the study show that FeTPPS can be used as ferric porphyrin model for the natural FePPIX for binding reactions in aqueous solution, the physiological medium.Indeed, spectrophotometric titration curves are well described by 1:1 binding scheme of FeTPPS dimer with the quinoline containing antimarials chloroquine, Quinine and quinidine.K values obtained support the formation of stable complexes.They also revealed that the stability of the complex depends not only on structural factors such as steric and stereoisomeric factors, but also on ionic strength.Thus, the complexation of FeTPPS with Chloroquine, Quinine, and Quinidine seems to be very similar to the complexation of FePPIX.In the light of this finding and results of ab initio calculations, it can be assumed that the main driving forces for the complexation of FeTPPS with quinoline-based antimalarials are also π -π interactions more or less enhanced by structural factors and electrostatic effects.This work will be extended to the formation of complexes in acidic pH range aqueous solution as the biological activity of the drugs in vivo occurs in the acidic digestive vacuole of the malaria parasite.
ε and d represent the apparent binding constant, the concentration, the extinction, the molar absorption coefficient and the optical path, respectively; C˚ is the initial total concentration and o

Figure 3 .
Figure 3. Absorption of FeTPPS and chloroquine between 350 to 600 nm at pH 7.40 25˚C and NaNO3 0.1 M.

Figure 5
Figure 5 reveals typical spectral changes induced by the addition of the antimalarial ligand in the aqueous solution of FeTPPS.The peaks of FeTPPS around 413 nm and 565 nm were still observed, but somewhat shifted and markedly damped with the increasing of ligand concentration.As illustrated in Figure 3, with the wavelength range (350 nm -600 nm), only FeTPPS absorbs.Thus, any change of the peaks of FeTPPS by adding an amount of antimalarial-based drugs is the result of interaction.The variation in extinction is caused by the interaction of the FeTPPS μ-oxo-Dimer with the antimalarial.Indeed, Also, there are two isosbestic points around 370 nm and 430 nm, respectively, suggesting the

Figure 5 .
Figure 5. Spectral changes in the Soret Band when FeTPPS is titrated with increasing concentration of Quinidine in pure aqueous solution at pH 7.40 without NaNO3.

Table 1 .
Apparent binding constants (K) obtained from spectrophotometric titration in pure aqueous solution at pH 7.40, 25˚C in pure aqueous solution and in solution containing NaNO3.