Ian W. Wyman and Donal H. Macartney*
Department of Chemistry, Queen's University, 90 Bader Lane, Kingston, Ontario K7L 3N6, Canada. E-mail: donal@chem.queensu.ca; Fax: +1 613 533 6669; Tel: +1 613 533 2617
First published on 6th November 2009
The cucurbit[7]uril (CB[7]) host molecule forms very stable host–guest complexes with the local anaesthetics procaine (KCB[7] = (3.5 ± 0.7) × 104 dm3 mol−1), tetracaine (KCB[7] = (1.5 ± 0.4) × 104 dm3 mol−1), procainamide (KCB[7] = (7.8 ± 1.6) × 104 dm3 mol−1), dibucaine (KCB[7] = (1.8 ± 0.4) × 105 dm3 mol−1) and prilocaine (KCB[7] = (2.6 ± 0.6) × 104 dm3 mol−1) in aqueous solution (pD = 4.75). The stability constants are 2–3 orders of magnitude greater than the values reported for binding by the comparably sized β-cyclodextrin host molecule. The inclusion by CB[7] raises the first pKa values of the anaesthetics by 0.5–1.9 pK units, as the protonated forms are bound more strongly in acidic solution. The complexation-induced chemical shift changes in the guest proton resonances provide an indication of the site(s) of binding and the effects of protonation on the location of the binding sites.
The slow, controlled delivery of anaesthetics by employing liposomes,4 lipid–protein–sugar microparticles,5 biodegradable polymers,6 catanionic gels,7 bentonite clays8 and macrocyclic host molecules9 have been investigated. Among the various host molecules which have been studied, the most attention has been paid to the cyclodextrins.9 There have been numerous investigations of the β-cyclodextrin (β-CD) inclusion complexes of procaine (novocaine) by a myriad of spectroscopic and other techniques. The strength of the binding depends on the state of protonation of the guest, with cyclodextrins preferring neutral or anionic guests over cationic species. With the anaesthetic procaine, the cationic form binds to β-CD with a stability constant of about 300 dm3 mol−1, while the neutral form has a stability constant of 1500 dm3 mol−1.9h Extremely weak binding (K = ∼1.4 dm3 mol−1) with the dicationic form in acidic solution is observed with β-CD,9h as inclusion results in an increase in the acidity of the guest and formation of the host–guest complex with the monocationic form of procaine.
We have recently shown that the cationic histamine H2-receptor antagonist drug ranitidine binds five orders of magnitude stronger with the cucurbit[7]uril host molecule compared with β-cyclodextrin in neutral solution.10 The cucurbit[n]urils (CB[n], where n = 5–8, 10) are a family of macrocyclic host molecules,11 comprised of n glycoluril units bridged by n pairs of methylene groups (Scheme 1), whose host–guest behaviour towards cationic and neutral organic and organometallic guests have been of increasing interest recently. The cucurbiturils contain a hydrophobic interior cavity, with polar carbonyl groups surrounding the two restrictive portals. In particular, the cucurbit[7]uril (CB[7]) host12 has received considerable recent attention because of its solubility in aqueous solution, a capacity to include aromatic13 and metallocene molecules,14 and for its molecular recognition of molecules and processes of biological interest.15
Scheme 1 Cucurbit[7]uril. |
One of the most interesting effects of the complexation of guests by cucurbit[7]uril in aqueous solution is the increase in the pKa of acidic protons on nitrogen, oxygen and carbon centers, as the host forms more stable host–guest complexes with the protonated forms of the guest, with ion–dipole interactions between the protonated site and the polar carbonyl groups on the CB[7] portals.16 Recently, examples of significant increases in the pKa values of guests such as the fungicide thiabenzole,16g and the 5,6-dimethylbenzimidazole base in vitamin B12 and coenzyme B1216h have been reported. We have observed that CB[7] inclusion can facilitate a switching in the fluorescence behaviour of protonated 2-aminoanthracene as a result of increases in their ground-state and excited-state pKa values upon hydrogen bonding between the ammonium group and the portal carbonyl oxygens.16a
In the same manner as the cyclodextrins, cucurbit[7]uril has been investigated as a potential drug carrier, with anti-tumor platinum(II) complexes for example.17 With a number of neutral and cationic organic and organometallic guest molecules, including the aforementioned ranitidine, cucurbit[7]uril forms host–guest complexes which have stability constants several orders of magnitude greater than for the corresponding inclusion complexes with β-cyclodextrin. While the cavity dimensions of the two hosts are similar, the somewhat restrictive portals on CB[7], coupled with the potential for stronger dipole–dipole, ion–dipole and hydrogen-bonding interactions between the guest and the polar carbonyl groups, lead to higher stability constants. Examples of stability constant comparisons include a KCB[7]/Kβ-CD ratio of 7 × 108 for the (trimethylammonio)methylferrocene cation.13d,14b Even small neutral molecules such as acetone and other ketones, dimethylsulfoxide and dimethylformamide exhibit binding enhancements of two orders of magnitude with CB[7] over β-CD.18
In this paper, we report the properties of the host–guest complexes formed in aqueous solution between cucurbit[7]uril and five local anaesthetics: the esters procaine and tetracaine, and the amides procainamide, dibucaine and prilocaine (Scheme 2). The formation of host–guest complexes has been observed by UV-visible absorbance and emission spectroscopy, 1H NMR spectroscopy, and electrospray mass spectrometry.19 The stability constants and complexation-induced pKa shifts of the guests have been determined, and compared with the values observed with the β-cyclodextrin host.
Scheme 2 Local anaesthetic guest molecules (structures at pH 7). The upper numbers represent the CB[7] complexation-induced chemical shift changes (Δδlim) in the proton resonances in D2O (pD = 5), and the lower values in italics are for the shifts observed in D2O containing 0.10 mol dm−3 DCl. For prilocaine, significant overlap in the aromatic region prevented determinations of individual Δδlim values and an average value is given. |
Guest | KCB[7]/dm3 mol−1 (pD 4.75) | KCB[7]/dm3 mol−1 (pD 1.0) | Kβ-CD/dm3 mol−1 | pKa | pKaCB[7] |
---|---|---|---|---|---|
a Ref. 9a.b Ref. 3b.c For diprotonated form, ref. 9h.d Ref. 3c.e Ref. 9b. | |||||
Procaine | (3.5 ± 0.7) × 104 | (4.4 ± 1.6) × 105 | 3.3 × 102a | 2.28b | 3.50 ± 0.05 |
1.4c | |||||
Tetracaine | (1.5 ± 0.4) × 104 | (1.1 ± 0.3) × 106 | 1.1 × 103a | 2.24b | 4.15 ± 0.05 |
Procainamide | (7.8 ± 1.6) × 104 | (5.5 ± 1.1) × 104 | 2.83b | 3.38 ± 0.05 | |
Dibucaine | (1.8 ± 0.4) × 105 | (1.1 ± 0.2) × 107 | 6.6 × 102a | 1.77d | 3.55 ± 0.05 |
Prilocaine | (2.6 ± 0.6) × 104 | (2.1 ± 0.4) × 104 | 9.6 × 101e |
We have recently shown that tetraalkylammonium ions (NR4+, R = Me, Et, nPr or nBu) form very stable inclusion complexes with CB[7] in aqueous solution, with the hydrophobic cations residing partially or fully within the cavity of the host,20 rather than outside at the portals, as observed for alkali and transition metal cations, and primary ammonium groups on RNH3+ or NH3RNH32+.11,13 The upfield chemical shift changes in the triethylammonium groups on the monocationic forms of the procaine, procainamide and dibucaine guests (Fig. 1) indicate that the entire group may be encapsulated in the CB[7] cavity, leaving the aromatic portion outside of the cavity near the portal. This may be contrasted with the behaviour of procaine with β-cyclodextrin, in which the neutral or monocationic forms of the guest are postulated to bind with the aromatic amine and ester groups within the cavity, leaving the triethylamine group outside.9h The two resonances for the non-equivalent diastereotopic CH2 protons of the terminal ethyl groups on the prochiral protonated nitrogen further separate upon CB[7] inclusion of these guests, as these protons also likely experience non-equivalent local environments within the cavity. We have previously observed this phenomenon with methylene protons in the case of the CB[7] inclusions of more rigid guests, such as substituted adamantanes.13e
Fig. 1 1H NMR spectra of dibucaine (1.02 mmol dm−3) with CB[7] in (right) D2O: (a) 0.0 equiv., (b) 0.21 equiv., (c) 0.44 equiv., (d) 0.68 equiv. and (e) 1.37 equiv. of CB[7], and (left) D2O containing 0.10 mol dm−3 DCl: (a) 0.0 equiv., (b) 0.31 equiv., (c) 0.78 equiv., and (d) 1.24 equiv. of CB[7]. |
The tetracaine guest displays interesting behaviour with respect to the site of binding (Scheme 2). It might be expected in neutral solution, with protonation of the tertiary amine group in the free guest, that binding might occur at this site. The 1H NMR spectra of the 1:1 complex, however, clearly reveals large upfield shifts in the protons of the butyl group, with smaller shifts in the aromatic protons, suggesting that CB[7] prefers to bind to the larger, hydrophobic butylanilinium end of the molecule. While the protonated triethylammonium site is encapsulated by CB[7] on procaine, procainamide and dibucaine, binding to the protonated trimethylammonium group on tetracaine would be expected to be much weaker, by analogy to the weaker binding of NMe4+ compared with NEt4+.20 This is much more thermodynamically plausible than the possibility that the binding to the secondary aromatic amine end causes it to become preferentially protonated over the tertiary amine, despite the fact that the pKa value for the secondary aromatic amine is much lower (2.24) than the tertiary amine group (8.48).3b The prilocaine appears to bind exclusively to the phenyl ring and its methyl substituent (Scheme 2), with only a small upfield shift in the resonance for the protons on the middle carbon of the propyl group. The lack of binding to the propylammonium group is again unusual, especially in terms of the binding to the butylamine group in the case of the tetracaine guest.
The effects of CB[7] complexation on the proton resonances of the guests in acidic media (0.10 mol dm−3 DCl in D2O) reveal different binding sites on some of the anaesthetic molecules than observed in neutral solution. With procaine, tetracaine and procainamide, the aromatic amine center becomes protonated and the CB[7] complexation of the aromatic ring induces significant upfield shifts in these protons (Scheme 2). With procaine and to a lesser extent with procainamide, the protons of the triethylammonium group also shift upfield somewhat, indicating that the CB[7] is spending some time on this portion of the molecule, or a second CB[7] is weakly bound (see below). With tetracaine, the upfield shifts of the aromatic protons are larger, with the butyl proton resonances now shifted significantly downfield.
The dibucaine guest appears to shift its binding site from the triethylammonium group in neutral solution to the butyloxy group in acidic solution upon protonation of the imine nitrogen (Fig. 1 and Scheme 2). Inclusion of the butyloxy group, with significant upfield shifts in the butyl proton resonances, places the protonated nitrogen on the aromatic ring (with a downfield shift in aromatic proton H4) closer to the portal of CB[7] than would binding over the triethylammonium group. The CB[7] otherwise displays no affinity for the aromatic end of the molecule in either neutral or acidic solution.
The host–guest stability constants for the 1:1 complexes formed between CB[7] and the local anaesthetics at 25 °C and pD 4.75 or pD 1.0 are listed in Table 1. At pD 4.75, the values are in the range of (1.5–18) × 104 dm3 mol−1. At pD 1.0, generally higher stability constants are observed, in the range of (2.2–1100) × 104 dm3 mol−1. For the two ester anaesthetics procaine and tetracaine, as well as for dibucaine, there is a significant increase in the binding constant on going to acidic solution, while for the amide anaesthetics procaineamide and prilocaine, the binding constants exhibit small decreases. The host–guest stability constants for the complexes between the anaesthetics and β-cyclodextrin are also listed in Table 1. The values for β-CD are in the range of 102–103 lower than the corresponding values measured for CB[7] at pD 4.75. While both host molecules have similar cavity sizes, the more polar portals (rimmed with ureido carbonyl groups) of CB[7], compared with β-CD (rimmed with hydroxyl groups), likely account for the tighter binding with the cationic guests. This is probably due to a combination of stronger non-covalent interactions (dipole–dipole, ion–dipole and hydrogen bonding). Recently, the binding constant between an amide anaesthetic agent, bupivacaine, and CB[6] has been reported to be 3 × 103 dm3 mol−1 in aqueous solution.21 The corresponding values for α-CD and β-CD are 102 ± 10 and 63 ± 5 dm3 mol−1, respectively.22
With β-CD, the binding constant decreases for the diprotonated form of procaine (1.4 dm3 mol−1), while it increases for the neutral forms of procaine (from 3.0 × 102 to 1.5 × 103 dm3 mol−1)9h and tetracaine (from 1.36 × 103 to 6.60 × 103 dm3 mol−1).9j With α-CD, only the neutral form of procaine binds, with a stability constant of 120 dm3 mol−1 at pH 10.4.9i The complexation of tetracaine has also been investigated with the hydroxypropyl-β-cyclodextrin9d and p-sulfonated calix[6]arene hosts,9j and stability constants of 1.31 × 103 and 3.89 × 103 dm3 mol−1, respectively, were determined for the monocationic guest species. The stability constant for prilocaine with the smaller α-CD host molecules has been reported to be < 5 dm3 mol−1, compared with the value of 96 dm3 mol−1 for β-CD.
For some of the local anaesthetics, there is evidence from the 1H NMR and UV spectroscopic titrations of much weaker 2:1 host–guest binding with CB[7] at higher concentrations of the host. Plots of UV absorbance against [CB[7]]/[guest] for procaine, for example, suggest a very strong 1:1 complex is formed initially, followed by a much weaker inclusion by a second CB[7]. With amine groups at each end of the molecule, a second CB[7] could bind at the opposite end to that of the 1:1 complex, although the electrostatic repulsions between the polar carbonyl groups on each host would be expected to reduce the stability constant of the second CB[7] substantially.
Fig. 2 UV titration of tetracaine (50 μmol dm−3) with CB[7] in water. Inset: dependence of the absorbance at 322 nm on the concentration of CB[7]. |
Fig. 3 Emission spectra of procaine (50 μmol dm−3) in the presence of increasing amounts of CB[7] (7 mmol dm−3 additions) in water. Inset: dependence of F/F0 at 354 nm as a function of [CB[7]], with a solid curve fit to F∞/F0 of 2.5 and KCB[7] = 1.0 × 105 dm3 mol−1. |
The pKa1 values for the CB[7]-included anaesthetic guests were determined by UV pH titrations at 25.0 °C (Fig. 4), and were found to increase between 0.5 and 1.9 pK units compared to the literature values for the free guests in aqueous solution. The raising of the pKa values, due to stabilization of the dication in the CB[7] host, has been observed previously for a number of N- and C-centered organic acids, and is attributed to the greater stabilization of the diprotonated forms of the guests through cation–dipole interactions with the polar carbonyl groups on the host portals.
Fig. 4 UV pH titrations of CB[7] host–guest complexes of (□) procaine (288 nm), (■) tetracaine (312 nm), (○) dibucaine (318 nm) and (●) procainamide (378 nm) at 25 °C. |
Footnote |
† Electronic supplementary information (ESI) available: UV, 1H NMR and ESI-MS spectral data, and titration curves. See DOI: 10.1039/b915694a |
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