pH-Responsive templates modulate the dynamic enzymatic synthesis of cyclodextrins.

Product selection in the dynamic enzymatic synthesis of cyclodextrins can be controlled by changing the pH. Using cyclodextrin glucanotransferase to make labile the glycosidic linkages in cyclodextrins (CDs), we generate a dynamic combinatorial library of interconverting linear and cyclic α-1,4-glucans. Templates can be employed to favour the selective production of specific CDs and, herein, we show that by using ionisable templates, the synthesis of α-CD or ß-CD can be favoured by simply changing the pH. Using 4-nitrophenol as the template, ß-CD is the preferred product at low pH, while α-CD is the preferred product at high pH. Furthermore, a new methodology is described for the simulation of product distributions in dynamic combinatorial libraries with ionisable templates at any given pH.

Specific Buffers Affect the Stability of a Charged Cyclodextrin Complex Via Competitive Binding and Ionic Strength.

The effect of 11 buffers as well as the effect of ionic strength were investigated on the binding between the bile salt taurochenodeoxycholate and the ionic sulfobutylether-ß-cyclodextrin. The investigations showed that both ionic strength and competitive binding affected the stability constant. The stability constant for the sulfobutylether-ß-cyclodextrin complex increased from 34,400 M-1 to 114,000 M-1 as the ionic strength of the solution increased to 0.15 M. Keeping the ionic strength constant, the stability constant for the complex depended on the buffer in the solution, with citric and succinic acid reducing the stability constant. The reduction in the stability constant by buffers was related to a competitive mechanism. The results showed that, when accounting for the variation in ionic strength between the buffers, three groupings of buffers existed. All carboxylic acid buffers decreased the stability constant of the sulfobutylether-ß-cyclodextrin complex, relative to the effect observed by altering the ionic strength, whereas the other buffers only affected the stability constant in terms of the changes in ionic strength. Both buffer species and ionic strength impacted the stability of ionic cyclodextrin complexes, hence, it is important to be aware of these effects when working with, comparing and reporting stability constants.

Derivatives of usnic acid cause cytostatic effect in Caco-2 cells.

Usnic acid has anti-cancer activity, however, low solubility and toxicity limit the potential. To investigate biological activity of usnic acid derivatives, enantiopure derivatives were synthesised by reacting usnic acid with ethylenediamine, which yielded one dimer product ((+)-1), and two tetra cyclic compounds ((+)-2 and (-)-2). The products were characterised with NMR, and evaluated in vitro in human colon cancer cell line Caco-2 by cell count, phase-contrast microscopy, MTT-assay, measurement of DNA content and cell cycle distribution. All compounds tested showed cytostatic effect in Caco-2 cells, but each compound had a distinct cellular effect. Compound (+)-1 showed anti-proliferative activity by increasing the percentage of cells in S-phase with 25% compared to the control. Compounds (+)-2 and (-)-2 induced paraptosis, but only compound (+)-2 modulated cell cycle distribution by accumulating cells in G2/M-phase by 47% and reduced DNA content by 60%. All compounds express interesting cellular and potential anti-proliferative activity.

Certain carboxylic acid buffers can destabilize ß-cyclodextrin complexes by competitive interaction.

Thirteen buffers were investigated for their effect on the binding of adamantanol to ß-cyclodextrin and hydroxypropyl-ß-cyclodextrin. Stability constants for the ß-cyclodextrin complex ranged from 14,800 to 46,000 M-1, and the binding enthalpies were between -23.2 and -10.4 kJ/mole. Compared to water, the stability constant in seven carboxylic acid buffers (citric acid, maleic acid, fumaric acid, succinic acid, malonic acid, malic acid and tartaric acid) was reduced. All seven buffers exhibited a competitive mechanism. Binding constants for the interaction between ß-cyclodextrin and buffers ranged from 4 to 44 M-1, and binding enthalpies were in the range -19 to -11 kJ/mole. There was a relation between the chemical structures of the buffers and their ability to bind to cyclodextrin. All seven buffers had a carbon chain consisting of more than three carbons in the backbone. Hydroxyl groups on the carbon chain decreased the binding affinity. 1H and ROESY NMR spectroscopy supported inclusion of the citric acid into the cyclodextrin cavity, although the results for succinic and maleic acids were ambiguous. The results demonstrated that some buffers can interact with cyclodextrin complexes, and careful considerations are necessary when choosing a buffer for cyclodextrin research.

Cyclodextrin binding constants as a function of pH for compounds with multiple pKa values.

Complex formation between cyclodextrins and ionizable guest molecules depends on pH. In general, the neutral species of an ionizable guest molecule has the highest affinity for the cyclodextrin cavity, but ionized species will also be able to form complexes with cyclodextrins. This work presents a theoretical expression for the relationship between the stability constant and pH for interaction between neutral cyclodextrins and ionizable guest molecules with multiple pKa values. Input parameters for the theoretical expression are pKa values of the guest molecule and stability constants for the complex at specific pH values. The pH profile of the stability constant for a complex depends on the acid-base properties of the guest and the closeness of the pKa values, and examples of pH profiles for polyprotic acids, bases and amphoteric guests are shown. Empirical data sets from the literature were used to confirm the accuracy of the theoretical expression, and Monte Carlo simulations were used to validate that the theoretical expression yield a good fit to empirical data. Lastly, an experimental protocol was suggested, and a freely available graphical user interface was presented to facilitate easy use of the theoretical expression.

Determination of acidity constants for weak acids and bases by isothermal titration calorimetry.

The advantage of isothermal titration calorimetry (ITC) to determine the acid dissociation constant (pKa value) is the simultaneous determination of the binding constant and binding enthalpy, as well as being precise and easy to use. The pKa can be calculated from the binding constant, and the temperature dependency of the pKa can be calculated from the binding enthalpy. The use of ITC to study protonation reactions is less common compared to its more conventional use of studying macromolecules and ligands. Water will influence the equilibrium due to autoionization, meaning that both the conjugate base and acid will exist in the sample cell at the beginning of the experiment. These differences are accounted for by optimizing the theoretical model used to estimate the binding constant and binding enthalpy. Through simulations and experimental measurements, we show that ITC can be used to determine the pKa for ibuprofen, ascorbic acid, 2-morpholin-4-ylethanesulfonic acid and paracetamol. The pKa values were consistent with potentiometric or spectrophotometric determinations as well as literature values. Optimizing the theoretical model does not lead to an improved determination, so the "one set of sites" model is adequate for the determination of pKa values.

Correlation between the stability constant and pH for ß-cyclodextrin complexes.

In drug formulations, cyclodextrins are used to increase aqueous solubility and chemical stability of drugs via formation of inclusion complexes. For ionizable drug molecules, the complexation strength depends on pH. Increased ionization leads to a more soluble drug, but also results in destabilization of cyclodextrin complexes. Therefore, formulation scientists aim to find a balance between increased drug solubility and high complexation strength. In this work, a theoretical expression for the dependency between the stability constant and pH is presented, allowing the accurate prediction of the stability constant at any pH. The theoretical expression requires three out of four input parameters; the pKa of the free guest molecule, the pKa of the complex, and the stability constants for the neutral and fully ionized complex. Stability constants for ß-cyclodextrin and ibuprofen complexes were determined by isothermal titration calorimetry at seven pH values (2.5-5.5) and four temperatures (15-55 °C). All these measured stability constants complied with the theoretical expression. Ten additional data sets from the literature comprising eight different drug molecules and three different cyclodextrins confirmed the ability of the theoretical expression to account for the observed pH-dependence of stability constants.

Buffer solutions in drug formulation and processing: How pKa values depend on temperature, pressure and ionic strength.

Solution pH is an important factor during drug formulation and processing. Changes in pH present challenges. Regulation of pH is typically managed by using a buffer system, which must have a suitable pKa. The pKa of buffers depends on temperature, pressure and ionic strength. In addition, the pKa can also be affected by the polarity of the solvent, e.g., by the addition of a co-solvent. Theoretical considerations and accessible experimental data were used to understand how the pKa values of pharmaceutically relevant buffers depend on these factors. Changes in temperature also affect the buffer pKa. Carboxylic acid moieties were least affected by changes in temperature. Buffers containing amino groups were most affected by changes in temperature, and the pKa decreased as temperature was increased. It was possible to predict accurately how buffer pKa varies with temperature, based on changes in enthalpy and heat capacity for the ionization reactions. Changes in pressure had a limited effect on buffer pKa for pressures <100 MPa. At higher pressures, buffer pKa varied by up to 0.5 pH units. Altering the ionic strength or polarity of the solvent influenced buffer pKa slightly. However, it is possible to keep both the ionic strength and the polarity of the solvent constant during drug formulation and processing.