János P.
Mészáros
ab,
Jelena M.
Poljarević
ac,
István
Szatmári
d,
Oszkár
Csuvik
d,
Ferenc
Fülöp
d,
Norbert
Szoboszlai
e,
Gabriella
Spengler
bf and
Éva A.
Enyedy
*ab
aDepartment of Inorganic and Analytical Chemistry, Interdisciplinary Excellence Centre, University of Szeged, Dóm tér 7, H-6720 Szeged, Hungary. E-mail: enyedy@chem.u-szeged.hu
bMTA-SZTE Lendület Functional Metal Complexes Research Group, University of Szeged, Dóm tér 7, H-6720 Szeged, Hungary
cFaculty of Chemistry, University of Belgrade, Studentski trg. 12-16, 11000 Belgrade, Serbia
dInstitute of Pharmaceutical Chemistry and Stereochemistry Research Group of Hungarian Academy of Sciences, University of Szeged, Eötvös u. 6, H-6720 Szeged, Hungary
eLaboratory for Environmental Chemistry and Bioanalytics, Institute of Chemistry, Eötvös Lóránd University, Pázmány Péter stny. 1/A, H-1117 Budapest, Hungary
fDepartment of Medical Microbiology and Immunobiology, University of Szeged, Dóm tér 10, H-6720 Szeged, Hungary
First published on 14th May 2020
Herein the design and synthesis of a new 8-hydroxyquinoline derivative, (S)-5-chloro-7-((proline-1-yl)methyl)8-hydroxyquinoline (HQCl-Pro), with good water solubility and multidrug resistance reversal activity are reported. In this work the proton dissociation processes of HQCl-Pro and its complex formation with [Rh(η5-C5Me5)(H2O)3]2+, [Ru(η6-p-cymene)(H2O)3]2+ and [Ru(η6-toluene)(H2O)3]2+ were investigated by the combined use of pH-potentiometry, UV-visible spectrometry and 1H NMR spectroscopy. Our results revealed the prominent solution stability of the complexes in all cases. The lipophilicity of the complexes increased with the chloride ion concentration, and the complexes showed moderate logD values (−0.8 to +0.4) at pH 7.4 at all tested Cl− concentrations. The formation of mixed hydroxido complexes from the aqua complexes was characterized by relatively high pKa values (8.45–9.62 in chloride-free medium). Complexation processes are much slower with the Ru(η6-arene) triaqua cations than with [Rh(η5-C5Me5)(H2O)3]2+. Both the pKa values and H2O/Cl− exchange constants of the Ru-complexes are lower by 0.5–1.0 orders of magnitude than those of the Rh analogue. Arene loss (p-cymene and toluene) and oxidation were found in the case of Ru-complexes when an excess of HQCl-Pro and aromatic (N,N) bidentate ligands was added. The cytotoxicity and antiproliferative effect of HQCl-Pro and its complexes were assayed in vitro. In contrast to the structurally familiar 8-hydroxyquinoline, HQCl-Pro and its Rh(η5-C5Me5) complex were somewhat more effective against drug resistant Colo 320 adenocarcinoma human cells compared to the drug sensitive Colo 205 cells. The Ru- and Rh-complexes showed a similar metal uptake level after 4 h, while a longer incubation time resulted in higher cellular Rh concentration.
Compounds with the 8-hydroxyquinoline moiety were also reported to exhibit anti-inflammatory, antiviral and antiparasitic effects and numerous HQ derivatives with various substituents have been developed and tested as anticancer agents in the last few decades.3–5 Among them halogenated compounds were often found to be more efficient.5,6
Not only 8-hydroxyquinolines but their particular metal complexes show anticancer activity as well. The most prominent example is the orally active tris(8-hydroxy-quinolato)gallium(III) (KP46), which is now under clinical trials and was successfully tested in phase I on renal cancer.7,8
Other examples are the complexes of platinum group organometallic cations bearing an aromatic ligand in a half-sandwich configuration (usually p-cymene (p-cym) or 1,2,3,4,5-pentamethyl-cyclopentadienyl (C5Me5) ligand). The complexes of these cations usually have various physico-chemical properties: the low oxidation state of the metal center (e.g. Ru2+) was stabilized and the lipophilicity was increased by the arene ligand; their kinetic lability can be associated with the strong π-donor/acceptor ability of the arene ligand as well.9,10 Moreover, the fine-tuning of the 3D structure and electronic properties can be easily achieved by functionalization of the arene or the remaining facial ligands. The interaction with the chloride content of the medium can change charge and lipophilicity. Nevertheless, new reaction pathways with biomolecules can be reached, which differ from the ligand–biomolecule interactions: e.g. catalysis of GSH oxidation.9 There are two main types of active complexes: in the first class, a monodentate ligand binds strongly to the metal centre and the leaving group(s) is/are present on two other coordination sites. Widely known examples are the RAPTA complexes where a strong P-donor, 1,3,5-triaza-7-phosphaadamantane (PTA), is the monodentate ligand.11 In the other class, the strongly coordinated bidentate ligand occupies two sites, and a leaving group is bound in a monodentate way. The dissociation of the latter can be fine-tuned well with the change of donor atoms. For example, the target biomolecule is switched from DNA to protein, depending on the nature of the bidentate ligand: (N,N) or (O,O).12 This field contains a plethora of studied complexes, and an early example is the group of RAED complexes which are in vivo active compounds showing activity on cisplatin-resistant cell lines.13 Though structure–activity relationships have been reported for these complexes, there is still no organoruthenium containing drug in clinical use.14,15
Half-sandwich organometallic complexes of the (N,O) donor 8-hydroxyquinolines are also often investigated. The organo-ruthenium complexes formed with clioquinol and other halogenated 8-hydroxyquinoline derivatives were studied thoroughly by Turel et al., and the inhibition of cathepsin B16 and the anticancer,17 antileukaemic18 and antibacterial effects19 were reported for these compounds. Nitroxoline (8-hydroxy-5-nitroquinoline) derivatives showed the anti-metastatic effect, which was improved by coordination to a half-sandwich Ru(p-cym) cation.20 An earlier study demonstrated the anticancer and antibacterial activities of the half-sandwich Rh and Ir complexes of HQ as well.21 These complexes are characterized by fairly low IC50 values (∼10 μM or less), which are promising results; however, they suffer from poor water solubility.6 The limited water solubility is a major problem encountered with drug formulation since it makes the administration difficult and might restrain the attainment of the desired concentration in the blood circulatory system. Movassaghi et al. introduced a more polar aromatic ligand (N-acetyl-L-phenylalanine ethyl ester) instead of p-cymene, and with this modification the solubility could be improved, while the cytotoxicity remained at the low-micromolar level.22
The hydrophilic nature of the complexes can be increased via the improved water solubility of the coordinating HQ derivative by the introduction of polar functional groups. However, the use of 8-hydroxyquinoline-5-sulfonate with excellent water-solubility caused the loss of the anticancer activity reported in our previous study.23 Therefore, the lipophilic nature of the HQ ligand should be optimized very carefully, and finding the optimal balance between lipophilicity and water-solubility is a very important endeavour in the development of novel anticancer compounds. Therefore, in this work we aimed to design an HQ–proline hybrid with elevated water solubility containing the CH2–N subunit at position 7 for the expected MDR-selectivity. It is also interesting how the coordination to metal ions has an effect on the cytotoxicity and MDR selectivity. When the MDR selective ligand 7-(1-piperidinylmethyl)-8-hydroxyquinoline (NSC57969) was combined with organometallic half-sandwich rhodium and ruthenium cations, the MDR selectivity remained only in the case of the Rh(η5-C5Me5) complex, while the coordination to Ru(η6-p-cym) resulted in the loss of this property.23 Herein the synthesis and solution chemical characterization of a new, water-soluble derivative of HQ, (S)-5-chloro-7-((proline-1-yl)methyl)8-hydroxyquinoline (HQCl-Pro, Scheme 1), is reported. Its complex formation with half-sandwich cations [Rh(η5-C5Me5)(H2O)3]2+, [Ru(η6-p-cym)(H2O)3]2+ and [Ru(η6-toluene)(H2O)3]2+ (abbreviated as [Ru(η6-tol)(H2O)3]2+) is also characterized in solution. In addition, the measurement of the lipophilicity of the compounds depending on the actual chloride ion concentration was performed: in the different biofluids the concentration of this coordinating ion may change charge and may have serious effects. The cytotoxicity of HQCl-Pro was monitored in sensitive and in multidrug resistant cancer cells and the effect of complexation with the selected organometallic triaqua cations on the biological activity was assayed as well.
The half-sandwich organometallic complexes with Rh(η5-C5Me5), Ru(η6-p-cym) and Ru(η6-tol) were prepared by mixing the ligand with a half-equivalent amount of the dimeric precursors [M(arene)Cl2]2 in methanol solution for 1 h at room temperature, then the solution was concentrated and precipitation was completed with the addition of diethyl ether. The formed complex was filtered out, washed with n-hexane and dried. Complexes were collected in good yields (84–90%). HQCl-Pro and its complexes were characterized by 1H and 13C NMR spectroscopy (attached proton test (APT)) and electrospray ionization mass spectrometry (ESI-MS). Mass spectra and NMR spectra are shown in the ESI (Fig. S1–S12†). The NMR spectra showed a double set of peaks in CD3OD, which can be explained by diastereomer formation (as was found in ref. 22 for complexes with chiral arene) or the appearance of a rigid structure (as it appears also in water for deprotonation vide infra). The differences of the two sets are shown in Fig. S13† peak-by-peak, projected on the proposed structures of complexes. The biggest differences are found in positions 14, 6 and 9, which can be connected with the diastereomer formation: in the complex, next to the chiral carbon atom, the Ru centre and the N of the protonated amino group become chiral, and these positions (6,9,14) are close to these atoms.
Additionally, the increased solubility and stability of the ligand and complexes were checked in phosphate buffer at pH = 7.4. All compounds were water-soluble; 10 mM concentration exceeds the limits of solubility of HQ, HQCl and their complexes. The compounds were stable for 1 week (not shown), except for the ligand itself, which showed a new set of peaks in the aliphatic region in a ∼20% ratio (see Fig. S14†) after 6 days.
The knowledge of the pKa value of a bioactive compound is needed not only for speciation studies, but it is also a key parameter affecting the pharmacokinetic properties, since with the pKa values the actual protonation state and charge of the molecule at a given pH can be calculated. In HQCl-Pro the incorporation of the L-prolinylmethyl substituent results in two additional dissociable protons besides the quinolinium-NH+ (NqH+) and the hydroxyl group (Scheme 2) of the HQ scaffold. N-methyl-L-proline (N-Me-Pro) is structurally similar to this substituent and it has two pKa values for the carboxylic acid and amino functions (Table 1).26
Method | pKa (COOH) | pKa (NqH+) | pKa (OH) | pKa (NProH+) | |
---|---|---|---|---|---|
a I = 0.20 M (KCl), taken from ref. 27. b Calculated with Marvin (ref. 28). c Estimated from the data obtained by UV-Vis titrations, pH = 2.0–11.5 (I = 0.20 M (KNO3)). d I = 0.10 M (KCl), taken from ref. 26. | |||||
HQ | pH-potentiometry | — | 4.99a | 9.51a | — |
HQCl | Predicted | 4.01b | 8.37b | — | |
UV-Vis | 3.8c | 7.6c | |||
N-Me-Pro | pH-potentiometry | 1.75d | — | — | 10.36d |
HQCl-Pro | pH-potentiometry | — | 2.36 ± 0.02 | 7.76 ± 0.01 | >11.5 |
UV-Vis | — | — | 7.63 ± 0.01 | — | |
1H NMR | ≪2 | 2.22 ± 0.02 | 7.62 ± 0.01 | — |
In order to characterize the proton dissociation processes of HQCl-Pro pH-potentiometric, UV-visible (UV-Vis) and 1H NMR titrations were performed. Although this compound has four dissociable protons, only two deprotonation processes could be determined adequately (with acceptable standard deviation) in the studied pH range by pH-potentiometry. The assignment of the deprotonation processes to the functional groups was done by the interpretation of the 1H NMR and UV-Vis spectral changes (Fig. 1, S15† and Table 1). Notably, HL denotes the neutral (zwitterionic) form of the ligand.
The most acidic pKa (≪2) of HQCl-Pro belongs to the carboxylic group of the prolinyl substituent, which caused shifts of the peaks only in the aliphatic region of the 1H NMR spectra (not shown). The deprotonation of the quinolinium NqH+ (up to pH 4) and OH (pH 5.5–9.5) groups was ascertained as high-field shifts of all the CH proton peaks (Fig. 1). The pKa values of these groups are much lower than those of HQ (see in Table 1) as a consequence of the presence of the two electron-withdrawing substituents (chlorine and the protonated CH2–NProH+ moiety). The structurally more related HQCl suffers from very poor solubility in aqueous medium and we could not determine its pKa values accurately enough in pure water by UV-Vis titrations even at rather low concentrations (5–10 μM) (see the estimated values in Table 1). Both the experimentally obtained and the predicted values for HQCl represent significantly lower values compared to those of HQ due to the electron withdrawing effect of the chlorine substituent as it is expected. Based on the pKa values it can be observed that the prolinyl amino group deprotonates at a much higher pH than the amino group in N-Me-Pro.
This can be the result of an intramolecular H-bond between the deprotonated hydroxylate and the NProH+ moiety (Scheme 2). A similar hydrogen bond was found in the crystal structures between the hydroxylate group and a protonated morpholine or piperidinyl nitrogen in HQ derived Mannich bases, and these substituents also had a similar effect on the pKa values.29
According to the 1H NMR spectra, only the singlet C6H peak seems to be sensitive to this deprotonation and a high-field shift was observed at pH > 10. The UV-Vis spectra, recorded at various pH values (Fig. 2), revealed three deprotonation processes. However, only one pKa value could be computed accurately by the deconvolution of the spectra (Table 1) as in the other two cases the whole deprotonation processes could not be seen.
On increasing the pH, the first two deprotonation processes detected in the UV-Vis spectra belong to the NqH+ and the hydroxyl groups, since changes in their protonation state have a considerable effect on the electron density of the aromatic rings. Thus, their deprotonation results in significant spectral changes, especially in the case of the hydroxyl moiety, namely the emerging strong bands in the range 330–430 nm originate from the more extended conjugated π-electron system in the deprotonated form. Surprisingly, the deprotonation of the prolinyl amino group also affects the spectra; it is accompanied by a minor bathochromic shift (see changes at pH > 10 in Fig. 2). Proton dissociation constants determined on the basis of the UV-Vis spectrophotometric and pH-potentiometric data are in good agreement with those obtained by the 1H NMR spectroscopic studies (Fig. S16† and Table 1).
On the basis of the obtained pKa values, species distribution was calculated at pH 7.4 and 63.5% of the ligand is present in its neutral form (HL+/−) that has notably a zwitterionic structure. In 36.5% the hydroxyl group is deprotonated (L−) resulting in the excellent water solubility of the compound at physiological pH (vide infra lipophilicity characterization).
The 1H NMR spectrum recorded for the [Rh(η5-C5Me5)(H2O)3]2+–HQCl-Pro system at pH 2 revealed peaks belonging only to a metal complex, and neither a free organometallic triaqua ion nor an unbound ligand was detected (not shown). It suggests the formation of significantly highly stable complexes. Even though the ligand has carboxylate and amino functions that might coordinate to another metal center, there is no sign of the formation of any dinuclear species based on the recorded 1H NMR spectra, and only the mono complex [Rh(η5-C5Me5)(L)(H2O)]+ is formed (where L is the coordinated form of HQCl-Pro). The Ru(η6-arene) complexes of HQCl-Pro behaved similarly. Fig. 4 shows the suggested structures for complexes [M(arene)(L)(H2O)]+ in water.
Fig. 4 The schematic representation of the mono complexes [M(arene)(L)(H2O)]+ formed with HQCl Pro and the various organometallic cations. |
However, the formation of the hydrogen bond is not indicated in Fig. 4, which may occur between the coordinated hydroxylate group and the protonated prolinyl nitrogen (O−⋯H+N) as it was determined for the Zn(II) complexes of various 8-hydroxyquinolines.30 A sign of this hydrogen bond may appear in methanol: the doubling found in the 13C NMR spectra may belong to the isomers formed after this hydrogen bond (Fig. S13†); the biggest differences are seen in the positions, which are close to this suggested hydrogen bond.
In order to determine the stability constants of the [M(arene)(L)] complexes, the UV-Vis spectra of acidic samples were recorded (pH = 0.8–2.8) to force the complex dissociation. The spectra obtained for the [Rh(η5-C5Me5)(H2O)3]2+–HQCl-Pro system were practically identical in the entire monitored pH range, however they are significantly different from the spectra of the unbound organometallic ion and ligand (Fig. 5a). It indicates that the complex formation is already complete at pH = 0.8, which hindered the calculation of the stability constant, and similarly no constants could be determined for the Ru(η6-arene) species (Fig. 5b). However, this approach was successfully used previously for the Rh(η5-C5Me5) and Ru(η6-p-cym) 8-hydroxyquinolinato complexes.23 In this work a logK [M(arene)(L)] = 16.45 ± 0.02 was obtained for the complex [Ru(η6-tol)(8-hydroxyquinolinato)(H2O)]+ based on the pH-dependent UV-Vis spectra (pH = 1.2–2.8, Fig. S18†) for comparison. Notably, this constant is slightly smaller than that of [Ru(η6-p-cym)(8-hydroxyquinolinato)(H2O)]+.23
Fig. 5 UV-Vis absorption spectra (solid lines) of the (a) Rh(η5-C5Me5)–HQCl-Pro system at pH = 0.8–2.0 and of the (b) Ru(η6-p-cym)–HQCl–Pro system at pH = 0.8–2.8. The dotted curve shows the absorption spectrum of the free organometallic cation (A), the dashed curve (B) shows the spectrum of the free HQCl-Pro ligand and the long dashed curve (A + B) shows their additive spectrum. {c([Rh(η5-C5Me5)(H2O)3]2+) = c(HQCl-Pro, in Fig. 4a) = 60 μM; c([Ru(η6-p-cym)(H2O)3]2+) = c(HQCl-Pro, in Fig. 4b) = 115 μM; I = 0.20 M (KNO3); T = 25.0 °C; = 1 cm}. |
Therefore, displacement reactions were performed to determine the stability constants of these highly stable complexes. First, ethylenediamine (en) was chosen as a competitor ligand. It has no absorbance in the 200–800 nm wavelength range, which makes it an attractive choice for these studies. However, mixed-ligand complex formation was detected according to the 1H NMR spectra (Fig. S19†) hindering the constant determination. The peaks belonging to the methyl hydrogens in the C5Me5 moiety reflect the various chemical environments of the organometallic fragment. E.g. at an excess of 23 equivalents of ethylenediamine not only the peaks of binary complexes [Rh(η5-C5Me5)(en)(H2O)]2+ and [Rh(η5-C5Me5)(L)(H2O)]+ appear (L: coordinated form of HQCl-Pro), but two unexpected peaks were also observed, signed with ♠ and ♣ in Fig. S19.† Addition of chloride ions decreased the ratio of these peaks (38% → 6%), which indicates that the Cl− and ethylenediamine compete for the third coordination site. Only ternary complex formation occurred in the case of the [Ru(η6-p-cym)(L)(H2O)]+ complex even at a huge excess (70 equivalents) of ethylenediamine, and at this high c(en)/c(HQCl-Pro) ratio ca. 50% of Ru(η6-p-cym) is found in the mixed-ligand complex.
In the next step, 2-picolylamine (pin) was selected and found to be an appropriate competitor in the case of the rhodium complex. Since pin has an intense ligand band in the UV region, only the use of 1H NMR spectroscopy was helpful to determine the speciation. Therefore, 1H NMR spectra were recorded for the [Rh(η5-C5Me5)(H2O)3]2+–HQCl-Pro–pin ternary system at various complex-to-pin ratios (Fig. 6a). The spectra revealed that while the amount of free HQCl-Pro and [Rh(η5-C5Me5)(pin)(H2O)]2+ is increasing with the 2-pin excess, the amount of the [Rh(η5-C5Me5)(L)(H2O)]+ complex is decreasing. Based on the integrals of the peaks, fractions of the different compounds were calculated (Fig. 6b) and the stability constant was determined (Table 2) using the stability constant of [Rh(η5-C5Me5)(pin)(H2O)]2+ taken from our previous work.31
Ru(η6-p-cym) | Ru(η6-tol) | Rh(η5-C5Me5) | |
---|---|---|---|
a For the [Rh(η5-C5Me5)(L)(H2O)]2+ + pin ⇌ [Rh(η5-C5Me5)(pin)(H2O)]2+ + L equilibrium determined at various c(pin) concentrations by 1H NMR spectroscopy. b Determined by UV-Vis spectroscopy at pH 2.0–11.5. c pH = 5.50 (phosphate buffer). For the [M(arene)(L)(H2O)]+ + Cl− ⇌ [M(arene)(L)Cl] + H2O equilibrium determined at various total chloride ion concentrations by UV-Vis spectrophotometry. | |||
logK [M(arene)(L)] | — | — | 13.41 ± 0.02a |
pKa [M(arene)(L)]b | 8.62 ± 0.04 | 8.45 ± 0.03 | 9.62 ± 0.04 |
logK′ (H2O/Cl−)c | 1.21 ± 0.01 | 1.09 ± 0.01 | 1.57 ± 0.01 |
However, in the case of [Ru(η6-arene)(H2O)3]2+ complexes the original yellow colour of the samples changed to pink and the peaks of the coordinated HQCl-Pro, p-cymene and toluene disappeared in the 1H NMR spectra at an excess of the competitor 2-picolylamine ligand, which can be explained by arene loss and the probable oxidation of the Ru centre (Fig. S20†). Thus, determination of the stability constants failed in these cases.
This side reaction aroused our interest as other competitor ligands (including e.g. ligands from biofluids) may also cause arene loss and may affect bioactivity. Therefore, ligand displacement reactions were studied by UV-Vis spectroscopy. First the effect of HQCl-Pro itself was studied using different conditions. The addition of two equivalents of ligand to the complex [Ru(η6-p-cym)(L)(H2O)]+ resulted in a too slow reaction at pH 2 to detect any changes during 1 h (while O2 passed through the solution). On the other hand, considerable changes of the spectra can be seen at physiological pH in Fig. 7a. The shape of the spectrum changes markedly, and a strong band developed at 420 nm, which is most probably related to the loss of the arene ligand and binding of the second and third HQCl-Pro. The rising broad band at higher wavelengths (λ > 500 nm) directly indicates the presence of the Ru(III) compound as it was found for [Ru(III)(8-hydroxyquinolate)3].32 Thus the change at 640 nm provides information about the rate of the Ru(III) complex formation (see Fig. 7b). In the literature the loss of arene (benzene, p-cymene) and the formation of [Ru(III)(L)3] were also found in the case of 8-hydroxyquinoline.23,32 As competitor ligands, deferiprone (1,2-dimethyl-3-hydroxy-pyridin-4(1H)-one) as an (O,O) model and 1,10-phenanthroline (phen) as a representative of (N,N) bidentate ligands were chosen. Addition of deferiprone to the complex [Ru(η6-p-cym)(L)(H2O)]+ did not result in spectral changes, while the reaction with phen was undoubtedly fast, and there was a significant difference between the initial solution (see the additive spectrum) and the spectrum recorded after 7 s for the mixed reactants (Fig. S21†). The yellow solution turned red and a strong band developed with λmax = 502 nm. After the first reaction step seemed to be completed in ∼90 s, another process started at ∼150 s and the main band shifted to 440 nm. The sign of a tiny amount of Ru(III) was also observed at higher wavelengths (A(690 nm) ∼ 0.05). When this experiment was repeated under argon, similar spectral changes were observed; however, the formation of Ru(III) could be successfully avoided. To explain the two main processes, the experiment was repeated with only 1 equiv. of phen under aerobic conditions (Fig. S22a†). The first step accompanied by the development of a band with 502 nm maximum was similar and was completed within 7 min (Fig. S22b†). Although the second process was different, most probably oxidation took place as the development of the strong band at 694 nm indicates (Fig. S22c†). Based on these findings the first step is most probably the loss of p-cymene and the formation of the mixed-ligand complex [Ru(II)(phen)(L)(H2O)2]+ (λmax = 502 nm, shown in gray rhombuses in Fig. S21b, S22b and c†). This is followed by the slow coordination of the second phen forming [Ru(II)(phen)2(L)]+ when 2 equiv. of phen were provided, while the slow oxidation occurs without the second phen ligand forming [Ru(III)(phen)(L)(H2O)2]2+ (shown in orange squares in Fig. S21b, S22b and c†).
Reactions of [Ru(η6-p-cym)(L)(H2O)]+ with various biomolecules were tested as well. Addition of histidine (His), human serum albumin (HSA) and RPMI 1640 medium components resulted in similar spectral changes (Fig. S23a, c and e†). We concluded that no Ru(III) was present in the systems, and most probably a mixed-ligand complex ([Ru(η6-p-cym)(L)(His)]+) is formed in the presence of histidine and the RPMI 1640 medium components (vide infra for NMR spectra). Albumin is also able to bind the complex most probably through its side chains in a monodentate fashion due to the coordination of a histidine nitrogen, or cysteine thiolate or methionine thioether.33,34 The reaction with HSA was somewhat slower under the same experimental setup (Fig. S23b, d and f†).
Based on these findings the following can be concluded: (i) the excess of rigid (O,O) donor bidentate ligands cannot cause the loss of p-cymene; (ii) the excess of the rigid 8-hydroxyquinolate-type (N,O−) and rigid (N,N) donor bidentate ligands can cause liberation of the arene ligand followed by oxidation to Ru(III) at physiological pH in the presence of O2; (iii) the flexible (N,N) donor ethylenediamine and biologically available molecules (like histidine, amino acids of RPMI 1640 or human serum albumin) can readily react with the complex [Ru(η6-p-cym)(L)(H2O)]+ forming mixed-ligand complexes. A previously described class of half-sandwich complexes containing azopyridine ligands also showed arene-loss (even at 1:1 metal-to-ligand ratio), which was explained with the π-acceptor properties of the bidentate ligand35 as the stronger π-acceptor bidentate ligands can compete with the arene.
From these sigmoid curves pKa [M(arene)(L)] values were determined (Table 2), which are much lower for the Ru containing complexes than for the Rh-complex. Notably, following the deprotonation the forming hydroxido complex exhibits more peaks than the aqua complex. Most probably the deprotonation leads to the loss of the twofold symmetry of the p-cymene ligand and peaks are doubled. Due to the rigid structure the rotation of the p-cymene ligand is blocked most likely. Earlier, computational studies revealed that the rotation has a very low energy barrier in the ruthenium–arene complexes bearing 1,2-ethylenediamine (RAED), e.g. benzene completes a full rotation in 2 ps.37 In that case, a steric interaction between HQCl-Pro, OH− and p-cymene can increase this rotational barrier.
Using the pKa [M(arene)(L)] values the ratio of the hydroxido form of the complexes was calculated at physiological pH revealing the formation of [M(arene)(L)(OH)] in 6% for Ru(η6-p-cym), 8% for Ru(η6-tol) and less than 1% for the Rh(η5-C5Me5)-complex in the absence of chloride ions. pKa of this type of complexes increases with the chloride ion concentration,24,38 thus these percentages are merely maximum values. When the organometallic fragments are compared with each other, the same trend of the pKa values was observed for complexes of (N,O) ligands such as 2-picolinates, HQ-5-sulfonate (HQS), HQ and 7-(1-piperidinylmethyl)-HQ (PHQ)23,38–40 as Fig. 9 shows.
Fig. 9 Comparison of pKa[M(arene)(L)] constants for the half-sandwich Ru- and Rh-complexes of (N,O) bidentate ligands (I = 0.20 M KNO3). HL = pic (2-picolinic acid),38–40,a HQ (8-hydroxyquinoline),23,b HQS (8-hydroxyquinoline-5-sulfonate),23 PHQ (7-(1piperidinylmethyl)-8-hydroxyquinoline)23 and HQCl-Pro. aI = 0.20 M KCl; bpKa([Ru(η6-tol)(8-hydroxyquinolinato)(H2O)]+) = 8.94(2) determined by UV-Vis spectrophotometric titration in this work, see Fig. S26.† |
Based on the logK and pKa [M(arene)(L)] constants (Table 2) concentration distribution curves were calculated for the Rh(η5-C5Me5) complex of HQCl-Pro (Fig. 10a). A very small amount (<3%) of free organometallic ions appears at pH 2, while the formation of the [Rh(η5-C5Me5)(L)(H2O)]+ complex is predominant at pH 7.4. The stability constants determined for the complexes of HQ derivatives cannot be compared directly due to the different basicity of ligands. For comparison, pM* (the negative logarithm of the unbound metal ion) values were calculated and plotted against the pH (Fig. 10b). (pM* is calculated by taking into consideration the hydrolyzed forms: pM* = −log([M(arene)] + 2×[(M(arene))2(OH)2] + 2×[(M(arene))2(OH)3]). The higher pM* value indicates higher stability of the complex. In these calculations, stability constants of the half-sandwich rhodium complexes with HQ, 8-hydroxyquinoline-5-sulfonate and 7-(1-piperidinyl-methyl)-8-hydroxyquinoline were used.23 Although the HQCl-Pro complex has the highest stability among the others up to pH ∼3.5, at physiological pH the other complexes have somewhat higher stability.
Fig. 10 (a) Calculated concentration distribution curves of the [Rh(η5-C5Me5)(H2O)3]2+–HQCl-Pro system based on the stability constants from Table 2. (b) Calculated pM* curves of the Rh(η5-C5Me5)–HQ (-·-),23 8-hydroxyquinoline-5-sulfonate (–),23 7-(1-piperidinylmethyl)-8-hydroxyquinoline (-··-)23 and HQCl-Pro systems (solid line), pM* = −log([M(arene)] + 2 × [(M(arene))2(OH)2] + 2 × [(M(arene))2(OH)3]). {c([Rh(η5-C5Me5)(H2O)3]2+) = c(HQCl-Pro) = 50 μM; T = 25.0 °C; I = 0.20 M (KNO3)}. |
Adding chloride ions to the solutions of the complexes causes changes in their 1H NMR and UV-Vis spectra. This is the result of a third equilibrium process, shown in Scheme S1,† which is the exchange of the coordinated water molecule to a chloride ion. Half-sandwich organorhodium and ruthenium complexes have a relatively high chloride ion affinity, and the chlorinated forms of the HQCl-Pro complexes are charge neutral. The chloride content of the medium has an effect on not only the charge, but also on the pKa [M(arene)(L)]24,38 and on the lipophilicity.39,41 This affinity is well described by the logK′ (H2O/Cl−) constant, which is determined from the UV-Vis spectra of the complexes by varying the total concentrations of chloride ions (Fig. S27–S30† and Table 2).
The logK′ (H2O/Cl−) constants show that the Rh(η5-C5Me5) complex has the highest, while [Ru(η6-tol)(L)(H2O)]+ has the lowest value (Table 2). The constants for [Ru(η6-arene)(L)(H2O)]+ complexes have tiny differences, and a similar trend was found previously in the case of 8-hydroxyquinoline, and Fig. S31† shows this tendency.23 The concentration of the chloride ion is around 100 mM in blood 24 mM in the cytoplasm and 4 mM in the nucleus,42 and the actual concentration affects the ratio of the chloride and aqua complexes (Fig. 11). The lower the c(Cl−), the higher fraction of the aqua complex. According to the proposed activation mechanism by aquation42 the complexes are in their neutral (zwitterionic) chlorinated form in the blood serum at 100 mM chloride concentration. The neutral chlorinated form may penetrate more easily through the cell membranes and might be trapped in the cytosol due to the lower chloride concentration and formation of charged aqua forms. While 79% of the rhodium complex is in the neutral form when the c(Cl−) is 100 mM, it drops to 47% and 13% at 24 mM and 4 mM chloride ion concentrations, respectively (Fig. 11). The Ru(η6-arene) complexes show somewhat weaker chloride ion affinity.
Fig. 11 The calculated ratio of aquated ([M(arene)(L)(H2O)]+) (white) and chlorinated ([M(arene)(L)Cl]) (gray) forms of the HQCl-Pro complexes at different chloride concentrations of modelling biofluids, based on the constants in Table 2. {c([M(arene)(H2O)3]2+) = c(HQCl-Pro) = 100 μM; c(Cl−) = 4, 24 and 100 mM; T = 25.0 °C}. |
The actual chemical form of the studied organometallic complexes strongly depends on the chloride ion affinity and concentration, as was described previously. Fig. 11 clarifies the ratios of the neutral chlorinated and the positively charged aquated forms at pH 7.4. Based on the data in Fig. 12 it can be concluded that the most lipophilic complex is [Ru(η6-p-cym)(L)(H2O/Cl)]+/0 at 100 mM of Cl−, and the most hydrophilic is [Ru(η6-tol)(L)(H2O/Cl)]+/0 at 4–24 mM of Cl−. Here the trend of lipophilicity is different from the trend of the logK′ (H2O/Cl−) values: Ru(η6-tol) < Rh(η5-C5Me5) < Ru(η6-p-cym). Although the rhodium complex has the highest chloride ion affinity, other factors also affect the lipophilicity such as the higher charge of the Rh-center (+3) (vs. the +2 charge of Ru) and the negative charge of the C5Me5 ligand (vs. neutral toluene/p-cymene).
Inhibiting the proliferation and causing cell death may occur at the same time when the drug is administered to the cells. Using a lower number of cells per well (6 × 103) and a longer incubation time (72 h) the MTT assay provides more information about the activity of the complexes to inhibit cell proliferation rather than growth inhibition. On the other hand, in the case of a higher number of cells per well (6 × 104) and a shorter exposure time (24 h) it is possible to monitor preferably the cytotoxic effect. IC50 values collected for HQCl-Pro in the absence and in the presence of [Rh(η5-C5Me5)(H2O)3]2+, [Ru(η6-p-cym)(H2O)3]2+ and [Ru(η6-tol)(H2O)3]2+ and for the precursor dimers [M(η5/6-arene)(μ-Cl)Cl]2 are shown in Table 3. Doxorubicin and cisplatin were used as positive controls.
Antiproliferative effect | Cytotoxic effect | |||
---|---|---|---|---|
Colo 205 | Colo 320 | Colo 205 | Colo 320 | |
a 1 × 104 cells were used for cisplatin. | ||||
HQCl-Pro | 23.4 ± 3.3 | 8.5 ± 1.7 | 42.5 ± 7.4 | 17.4 ± 2.5 |
[Ru(η6-tol)(L)(H2O)]+ | 25.3 ± 3.1 | 85.0± 7.5 | 72.6 ± 4.8 | 60.9 ± 8.2 |
[Ru(η6-p-cym)(L)(H2O)]+ | 68.3 ± 10.7 | >100 | >100 | >100 |
[Rh(η5-C5Me5)(L)(H2O)]+ | 25.8 ± 4.8 | 9.7 ± 1.1 | 81.5 ± 3.3 | 24.1 ± 3.7 |
[Ru(η6-p-cym)(μ-Cl)Cl]2 | >100 | >100 | >100 | >100 |
[Ru(η6-tol)(μ-Cl)Cl]2 | >100 | >100 | >100 | >100 |
[Rh(η5-C5Me5)(μ-Cl)Cl]2 | >100 | >100 | >100 | >100 |
Doxorubicin | 3.28 ± 0.22 | 3.12 ± 0.27 | 1.56 ± 0.03 | 6.45 ± 0.19 |
Cisplatin | 10.1 ± 0.3 | 4.78 ± 0.11 | 83.9 ± 3.5a | 18.1 ± 0.3a |
The organometallic precursors have no toxic effect on cancer cell lines (IC50 > 100 μM). HQCl-Pro and its Rh(η5-C5Me5) complex exhibited similar and relatively low IC50 values, while in the presence of Ru(η6-tol) and especially Ru(η6-p-cym) much higher values were obtained. Additionally, HQCl-Pro and its Rh(η5-C5Me5) complex showed higher anticancer activity in Colo 320 than in Colo 205. In contrast the toluene and p-cymene complexes have similar cytotoxicity in both cell lines and the antiproliferative effect is weaker in the Colo 320 cells. These data do not correlate with the lipophilicity of the complexes, suggesting that other factors seem to be more dominant in the bioactivity. Notably, the complexes have similar or weaker cytotoxicity compared to cisplatin.
For the Mg(II) and Ca(II) complexes of the structurally closer HQCl stability constants were determined in a 60% (v/v) dioxane/water mixture,44 and based on these stability constants the bound fraction of the ligand can be ∼60%.
Therefore, peak shifting of the ligand HQCl-Pro can be explained by the fast exchange between the free ligand and the Mg(II)/Ca(II) complexes. However, the competition of Ca2+ and Mg2+ with half-sandwich cations does not occur because the stability of the latter complexes is much higher. Peaks of different amino acid components are shown in the medium (Fig. 13). The singlets of histidine at δ = 7.0 and 7.7 ppm suffer from the most important change, as they disappeared/shifted after reacting with the complex [Ru(η6-p-cym)(L)(H2O)]+. This interaction is most probably the formation of a mixed-ligand species, and can also affect the final biological activity. In all, instead of the ligand displacement only the ternary complex formation with histidine is the most probable interaction, and there is no sign of ligand release (no free HQCl-Pro or in the form of the Mg(II) complex). It can be concluded that the reduced biological activity is most likely not connected to a dissociation process of the original complexes (at least not in the medium).
The preparation of solutions and the determination of the concentration of stock solutions were performed as in our former works,23,24 see the ESI†/pH-potentiometry part for more information.
The buffered samples were prepared in 20 mM phosphate buffer or in a modified phosphate buffered saline (PBS′) at pH 7.40. PBS′ contains 12 mM Na2HPO4, 3 mM KH2PO4, 1.5 mM KCl and 100.5 mM NaCl; and the concentration of the K+, Na+ and Cl− ions corresponds to that of the human blood serum.
1H and 13C NMR spectroscopic studies were carried out on a Bruker Avance III HD Ascend 500 Plus instrument. All 1H NMR spectra were recorded with the WATERGATE water suppression pulse scheme using the DSS internal standard, while 13C NMR spectra were recorded with the attached proton test method, which shows CH and CH3 in positive mode, and C and CH2 in negative mode. Samples were made in a 10% (v/v) D2O/H2O mixture to yield a concentration of 300 μM and was titrated at 25 °C, at I = 0.20 M (KNO3) in the absence or presence of [Rh(η5-C5Me5)(H2O)3]2+, [Ru(η6-p-cym)(H2O)3]2+ and [Ru(η6-tol)(H2O)3]2+ at 1:1 metal-to-ligand ratio. Stability constants for the complexes were calculated using the computer program PSEQUAD.47 For characterization, 10 mM CD3OD solutions were used.
Distribution coefficients at physiological pH (D7.4) of the complexes and the ligand were determined by the traditional shake-flask method in n-octanol/buffered aqueous solution at pH 7.40 at various chloride concentrations using UV-Vis detection as described in our former works.23,39
ESI-MS measurements were performed using a Waters Q-TOF Premier (Micromass MS Technologies, Manchester, UK) mass spectrometer equipped with an electrospray ion source. Samples contained 200 μM ligand or complex dissolved in water, and pH was adjusted to ∼7 with a small amount of HCl or KOH.
Samples were analyzed by TXRF spectrometry; a TXRF 8030C spectrometer (Atomika Instruments GmbH, Oberschleissheim, Germany), equipped with a 3 kW fine focus X-ray tube containing a Mo/W alloy anode, a W/C multi-layer monochromator, adjusted to obtain an excitation energy of 33 keV selected out from the Bremsstrahlung was used. A Si(Li) detector with an active area of 80 mm2 was in operation with a resolution of 150 eV at 5.9 keV. 10 μL of 100 mg L−1 Ga was added to the samples prior to the TXRF analysis as the internal standard for the quantification procedure. Rh and Ru were not detected in blank samples. Due to the imprecision of cell counting, the Rh results were normalized to the Zn or S content of the samples.
Formation of mixed hydroxido [M(arene)(L)(OH)] complexes is less than 10% at physiological pH in the absence of chloride ions, and it is assumed to be an even lower fraction in the presence of this coordinating co-ligand. Substitution of the coordinated water molecule in the complex [M(arene)(L)(H2O)]+ by chloride ions results in neutral complexes, which have much higher lipophilicity than the aqua form and the ligand itself. The Rh(η5-C5Me5) complex has stronger chloride ion affinity than the Ru(η6-arene) containing ones, and the Ru(η6-tol) complex was found to be the most hydrophilic among the studied compounds.
The in vitro cytotoxic and antiproliferative activity of HQCl-Pro and its half-sandwich organometallic complexes were studied in Colo 205 drug sensitive and Colo 320 multidrug resistant cancer cell lines by the MTT assay in addition to cellular metal uptake studies. HQCl-Pro and its [Rh(η5-C5Me5)(L)(H2O)]+ complex showed relatively strong anticancer activity and moderate MDR selectivity, while complexation with ruthenium–arene species results in a lower or similar activity in the Colo 320 cell lines compared to that obtained in Colo 205 cells. Based on the 1H NMR spectra recorded for the Ru(η6-p-cym) complex of HQCl-Pro in the cell medium RPMI 1640 it was concluded that only mixed-ligand complex formation occurred with histidine, and the bidentate ligand is not dissociated from the complex. While a similar metal uptake level was found for both the Rh(η5-C5Me5) and Ru(η6-p-cymene) complexes using a 4 h incubation period, the longer incubation led to a higher intracellular Rh content which might contribute to the lower IC50 values of the Rh(η5-C5Me5) complex.
Footnote |
† Electronic supplementary information (ESI) available: Characterization, additional UV-Vis spectra of kinetic measurements and titrations, and pH-dependent 1H NMR spectra of compounds. See DOI: 10.1039/D0DT01256D |
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