Solubility Prediction of Satranidazole in Aqueous N,N-dimethylformamide Mixtures Using Extended Hildebrand Solubility Approach

The solubility of satranidazole in several water–N,N-dimethylformamide mixtures was analysed in terms of solute–solvent interactions and data were treated on the basis of extended Hildebrand solubility approach. The solubility profile of satranidazole in water–N,N-dimethylformamide mixtures shows a curve with a solubility maxima well above the ideal solubility of drug. This is attributed to solvation of the drug with the water–N,N-dimethylformamide mixture, and indicates that the solute–solvent interaction energy (W) is larger than the geometric mean (δ₁δ₂) of regular solution theory. The new approach provides an accurate prediction of solubility once the interaction energy (W) is obtained. In this case, the energy term is regressed against a polynomial in δ₁ of the binary solvent mixture. A quartic expression of W in terms of solvent solubility parameter was found for predicting the mole fraction solubility of satranidazole in the studied mixtures. The method has potential usefulness in preformulation and formulation studies during which solubility prediction is important for drug design.     

Extended hildebrand solubility approach: satranidazole in mixtures of dioxane and water

The extended Hildebrand solubility parameter approach is used to estimate the solubility of satranidazole in binary solvent systems. The solubility of satranidazole in various dioxane-water mixtures was analyzed in terms of solute-solvent interactions using a modified version of Hildebrand-Scatchard treatment for regular solutions. The solubility of satranidazole in the binary solvent, dioxane-water shows a bell-shaped profile with a solubility maximum well above the ideal solubility of the drug. This is attributed to solvation of the drug with the dioxane-water mixture, and indicates that the solute-solvent interaction energy is larger than the geometric mean (δ(1)δ(2)) of regular solution theory. The new approach provides an accurate prediction of solubility once the interaction energy is obtained. In this case, the energy term is regressed against a polynomial in δ(1) of the binary mixture. A quartic expression of W in terms of solvent solubility parameter was found for predicting the solubility of satranidazole in dioxane-water mixtures. The method has potential usefulness in preformulation and formulation studies during which solubility prediction is important for drug design.     

Excess free energy approach to the estimation of solubility in mixed solvent systems III: Ethanol-propylene glycol-water mixtures

The reduced three-suffix solubility equation derived from the Wohl excess free energy expression is used to describe the solubility of phenobarbital in propylene glycol-water, ethanol-propylene glycol, and ethanol-water-propylene glycol mixtures and the solubility of hydrocortisone in propylene glycol-water mixtures. Solvent-solvent interaction constants were obtained by fitting total vapor pressure versus composition data, obtained at 25 +/- 0.1 degrees C, to the Wohl excess free energy model for the solvents. The equation describes solubility in these systems satisfactorily except for phenobarbital in ethanol-propylene glycol, where the solubility is fairly high and assumptions involved in the derivation of the equation do not hold.     

A Study on Improvement of Solubility of Rofecoxib and its effect on Permeation of Drug from Topical Formulations

Rofecoxib, a practically insoluble cox-2 selective nonsteroidal antiinflammatory agent was subjected to improvement in solubility by preparing its binary mixtures with β cyclodextrin using various methods such as physical mixing, co-grinding, kneading with aqueous methanol and co-evaporation from methanol-water mixture. Characterization of the resulting binary mixtures by differential scanning calorimetry and X-ray diffraction studies indicated partial amorphization of the drug in its binary mixtures. In vitro dissolution studies exhibited remarkable increase in rate and extent of dissolution of the drug from its complexes with β -cyclodextrin. Pure rofecoxib as well as its co-ground binary mixture were formulated as aqueous gels for topical application. In vitro skin permeation of rofecoxib from formulation containing rofecoxib-cyclodextrin complex was significantly higher (p<0.05) at 1, 2, 12, 18 and 24 hr as compared to formulation containing pure rofecoxib. This could be attributed to better solubility of binary mixture in the aqueous gel vehicle leading to greater concentration gradient between the vehicle and skin and hence higher flux of the drug.     

The Effects of pH and Mixed Solvent Systems on the Solubility of Oxytetracycline

The solubility of oxytetracycline (OTC) in aqueous and mixed solvent systems was studied. The effects of pH and cosolvent composition on the solubility and apparent dissociation constants (pK′_a) of OTC were determined by a solubility method. The pK′_a values of OTC in each mixed solvent system were estimated and used to generate expressions for predicting drug solubility in each cosolvent as a function of pH. Cosolvent systems of PEG 400, propylene glycol, glycerin, and 2-pyrrolidone were studied in the pH range of 2.5–9. Solubility results showed increased solubility with increased cosolvent concentration, especially in 2-pyrrolidone solvent systems. These results also showed that cosolvents enhanced drug solubility through either their effects on polarity of the solvent medium or complex formation with OTC. Aqueous and mixed solvent systems at lower pH values resulted in higher OTC solubilization because the drug existed primarily in its cationic form. A mass balance equation including all ionic species of OTC allowed for estimation of the intrinsic solubilities and pK′_a values in each solvent system. pK′_a values and intrinsic solubility of the OTC zwitterion increased with increasing cosolvent content. These parameters allowed prediction of drug solubility within the pH range and cosolvent concentrations used in this study.     

The Estimation of Solubility in Binary Solvents: Application of the Reduced 3-Suffix Solubility Equation to Ethanol–Water Mixtures

The reduced 3-suffix solubility equation (R3SSE) is applied to the characterization of solubility in the ethanol–water system. The data needed are the solubility of the compound in each of the pure solvents and at one ethanol–water composition. This composition has been estimated from solubility data to be 0.56 volume fraction of ethanol. The solubility obtained at this volume fraction is used to estimate the ternary solute–solvent interaction constant, C ₂. The R3SSE, with the C ₂ thus obtained, predicts the mixed solvent solubilities of the compounds tested, as accurately as that obtained from several volume fractions. The superiority of the R3SSE over two related equations—a simple second-degree polynomial equation and a simplified form of the R3SSE which neglects contributions to solubility from the solvent mixture—is also demonstrated for a number of solutes.     

A Modification of the Extended Hildebrand Approach to Predict the Solubility of Structurally Related Drugs in Solvent Mixtures

Abstract— A modification of the extended Hildebrand equation is proposed to estimate the solubility of an organic drug in solvent mixtures. The equation accurately reproduces the solubility of four sulphonamides in dioxane-water mixtures without requiring the heat of fusion of the solute. A single equation is obtained for predicting the solubility of related drugs using the solubilities of the drugs in the pure solvents, dioxane and water, and solute-solvent interaction terms consisting of the solubility parameter, δ₂, of the solute and the solubility parameter, δ₁, and basic partial solubility parameter, δ_1b, of the solvent mixture. By this procedure a single equation was obtained to estimate the solubilities of three xanthines in dioxane-water and another equation to obtain the solubilities of four sulphonamides. The equation obtained for sulphonamides is able to predict the experimental solubilities of two parent compounds, sulphasomidine and sulphathiazole, and the solubilities of a drug of different structure, p-hydroxybenzoic acid. This suggests that the intermolecular solute-solvent interaction of sulphonamides and p-hydroxybenzoic acid are similar. The results indicate that the solubility behaviour of drugs having different structures may be modelled using a common equation provided that they show similar solute-solvent interactions.     

Predicting the Solubility of the Anti-Cancer Agent Docetaxel in Small Molecule Excipients using Computational Methods

Purpose To develop an in silico model that provides an accurate prediction of the relative solubility of the lipophilic anticancer agent docetaxel in various excipients. Materials and Methods The in silico solubility of docetaxel in the excipients was estimated by means of the solubility (δ) and Flory-Huggins interaction (χ _FH) parameters. The δ values of docetaxel and excipients were calculated using semi-empirical methods and molecular dynamics (MD) simulations. Cerius² software and COMPASS force-field were employed for the MD simulations. The χ _FH values for the binary mixtures of docetaxel and excipient were also estimated by MD simulations. Results The values obtained from the MD simulations for the solubility of docetaxel in the various excipients were in good agreement with the experimentally determined values. The simulated values for solubility of docetaxel in tributyrin, tricaproin and vitamin E were within 2 to 6% of the experimental values. MD simulations predicted docetaxel to be insoluble in β-caryophyllene and this result correlated well with experimental studies. Conclusions The MD model proved to be a reliable tool for selecting suitable excipients for the solubilization of docetaxel. Electronic supplementary material The online version of this article (doi: ) contains supplementary material, which is available to authorized users.     

Enthalpy and Entropy Contributions to the Solubility of Sulphamethoxypyridazine in Solvent Mixtures Showing Two Solubility Maxima

The solubility of sulphamethoxypyridazine was measured at several temperatures in mixtures of water: ethanol and ethanol: ethyl acetate. Sulphamethoxypyridazine was chosen as a model drug to compare the solvation effects of proton donor-proton acceptor (water and ethanol) and proton acceptor (ethyl acetate) solvents and mixtures of these solvents because this drug contains functional groups capable of Lewis acid-base interaction. A plot of the mole fraction solubility against the solubility parameter (δ₁) of these solvent mixtures showed two solubility maxima, one at δ₁ = 30·87 MPa^1/2 (20:80 v/v water: ethanol) and another at δ₁ = 20·88 MPa^1/2 (30:70 v/v ethanol: ethyl acetate) at all the temperatures under study. The enthalpies and entropies of mixing as well as the enthalpies and entropies of transfer of sulphamethoxypyridazine from ethanol to water:ethanol and ethanol:ethyl acetate mixtures were calculated to compare solvation characteristics of the solvent mixtures toward the drug. As ethanol is added to water, the entropy increases and the structure of the solvent mixture became less ordered, favouring the interaction of the drug with the solvent mixture. On the other hand, in the case of the ethanol: ethyl acetate mixture, solubility is favoured by the more negative enthalpy values. This way, the same result, i.e. a solubility maximum, is obtained by different routes. In the ethanol: water mixtures, the dissolution process is entropy-controlled while enthalpy is the driving force in the case of ethanol: ethyl acetate mixtures. The two solvent systems show enthalpy-entropy compensation. Water deviates from the linear relationship due possibly to its hydrophobic effect.     

Experimental and Computational Screening Models for Prediction of Aqueous Drug Solubility

Purpose. To devise experimental and computational models to predict aqueous drug solubility. Methods. A simple and reliable modification of the shake flask method to a small-scale format was devised, and the intrinsic solubilities of 17 structurally diverse drugs were determined. The experimental solubility data were used to investigate the accuracy of commonly used theoretical and semiexperimental models for prediction of aqueous drug solubility. Computational models for prediction of intrinsic solubility, based on lipophilicity and molecular surface areas, were developed. Results. The intrinsic solubilities ranged from 0.7 ng/mL to 6.0 mg/mL, covering a range of almost seven log₁₀ units, and the values determined with the new small-scale shake flask method agreed well with published solubility data. Solubility data computed with established theoretical models agreed poorly with the experimentally determined solubilities, but the correlations improved when experimentally determined melting points were included in the models. A new, fast computational model based on lipophilicity and partitioned molecular surface areas, which predicted intrinsic drug solubility with a good accuracy (R ²of 0.91 and RMSE_tr of 0.61) was devised. Conclusions. A small-scale shake flask method for determination of intrinsic drug solubility was developed, and a promising alternative computational model for the theoretical prediction of aqueous drug solubility was proposed.     

Cosolvency and Deviations from Log-Linear Solubilization

The solubilities of three nonpolar drugs, phenytoin, diazepam, and benzocaine, have been measured in 14 cosolvent–water binary mixtures. The observed solubilities were examined for deviations from solubilities calculated by the equation log S _m = f log S _c + (1 – f) log S _w, where S _m is the solubility of the drug in the cosolvent–water mixture, S _c is the solubility of the drug in neat cosolvent, f is the volume fraction of cosolvent, and S _w is the solubility of the drug in water. When presented graphically, the patterns of the deviations were similar for all three drugs in mixtures of amphiprotic cosolvents (glycols, polyols, and alcohols) and water as well as nonpolar, aprotic cosolvents (dioxane, triglyme, dimethyl isosorbide) and water. The deviations were positive for phenytoin and benzocaine but negative for diazepam in mixtures of dipolar, aprotic cosolvents (dimethylsulfoxide, dimethylformamide, and dimethylacetarnide) and water. The source of the deviations could not consistently be attributed to physical properties of the cosolvent–water mixtures or to alterations in the solute crystal. Similarities between the results of this study and those of previous investigations suggest that changes in the structure of the solvent play a role in the deviations from the expected solubilities.     

Formulation and characterization of eprosartan mesylate and β-cyclodextrin inclusion complex prepared by microwave technology

The goal of this work was to improve the aqueous solubility and dissolution rate of eprosartan mesylate by preparing inclusion complex of drug with β-cyclodextrin (β-CD) by microwave technique. In order to determine the solubility of eprosartan, phase solubility was determined and dissolution study was also conducted. Further, analytical techniques for instance, particle size distribution, differential scanning calorimetry, powder X-ray diffraction, scanning electron microscopy, Fourier-transform infrared spectroscopy, and nuclear magnetic resonance spectroscopy were used for the characterization of inclusion complex. In addition, the binding pattern of eprosartan with the β-CD was investigated by molecular modeling study. Phase solubility study revealed that approximately 4.48 folds improvement in the solubility of drug was noted with β-CD (10 mM). The estimated stability constant (K_c) values for eprosartan:β-CD binary mixture was found to be 280.78 M^–1. The prepared inclusion complex of drug with β-CD presented better drug release profile (62.96 ± 2.01% in 1 h) as compared to their physical mixture (41.41 ± 1.77% in 1 h) or drug per se (29.97 ± 3.13%). The inclusion complex demonstrated different features and properties from pure drug, and we inferred that this could be due to the inclusion of drug into cyclodextrin cavity that confirmed by different analytical method. Molecular modeling study demonstrated a good affinity of eprosartan to entangle to β-CD. The outcomes have shown that guest molecule has many significant interactions with the host molecule. These observations are very interesting and may be a valuable approach to improve the solubility and in turn the bioavailability of eprosartan.     

A Quantitative Model to Evaluate Solubility Relationship of Polymorphs from Their Thermal Properties

Purpose The objective of the study is to develop a model to estimate the solubility ratio of two polymorphic forms based on the calculation of the free energy difference of two forms at any temperature. This model can be used for compounds with low solubility (a few mole percent) in which infinite dilution can be approximated.Methods The model is derived using the melting temperature and heat of fusion for apparent monotropic systems, and the solid–solid transition temperature and heat of transition for apparent enantiotropic systems. A rigorous derivation also requires heat capacity (C_p) measurement of liquid and two solid forms. This model is validated by collecting thermal properties of polymorphs for several drugs using conventional or modulated differential scanning calorimetry. From these properties the solubility ratio of two polymorphs is evaluated using the model and compared with the experimental value at different temperatures.Results The predicted values using the full model agree well with the experimental ones. For the purpose of easy measurement, working equations without C_p terms are also applied. Ignoring C_p may result in an error of 10% or less, suggesting that the working equation is applicable in practice. Additional error may be generated for the apparent enantiotropic systems due to the inconsistency between the observed solid–solid transition temperature and the true thermodynamic transition temperature. This inconsistency allows the predicted solubility ratios (low melt/high melt) to be smaller. Therefore, a correction factor of 1.1 is recommended to reduce the error when the working equation is used to estimate the solubility ratio of an enantiotropic system.Conclusions The study of the free energy changes of two crystalline forms of a drug allows for the development of a model that successfully predicts the solubility ratio at any temperature from their thermal properties. This model provides a thermodynamic foundation as to how the free energy difference of two polymorphs is reflected by their equilibrium solubilities. It also provides a quick and practical way of evaluating the relative solubility of two polymorphs from single differential scanning calorimetry runs.     

Solubility in binary solvent systems. V. Monomer and dimer models for the solubility of p-tolylacetic acid in systems of non-specific interactions

Solubilities are reported for p-tolylacetic acid in binary mixtures of cyclohexane with n-hexane, n-heptane, n-octane and isooctane at 25 °C. The results are compared to the predictions of equations developed previously for solubility in systems of purely non-specific interactions, with the carboxylic acid considered as either monomeric or dimeric molecules in solution. The dimer model provided the more accurate predictions, with a maximum deviation of 5.6% between observed and predicted solubility in all systems studied.     

Solubility of drugs in aqueous solutions. Part 2: binary nonideal mixed solvent

As in a previous paper [Int. J. Pharm. 258 (2003) 193–201], the Kirkwood–Buff theory of solutions was employed to calculate the solubility of a solid in mixed solvents. Whereas in the former paper the binary solvent was assumed ideal, in the present one it was considered nonideal. A rigorous expression for the activity coefficient of a solute at infinite dilution in a mixed solvent [Int. J. Pharm. 258 (2003) 193–201] was used to obtain an equation for the solubility of a poorly soluble solid in a nonideal mixed solvent in terms of the solubilities of the solute in the individual solvents, the molar volumes of those solvents, and the activity coefficients of the components of the mixed solvent.

The Flory–Huggins and Wilson equations for the activity coefficients of the components of the mixed solvent were employed to correlate 32 experimental data sets regarding the solubility of drugs in aqueous mixed solvents. The results were compared with the models available in literature. It was found that the suggested equation can be used for an accurate and reliable correlation of the solubilities of drugs in aqueous mixed binary solvents. It provided slightly better results than the best literature models but has also the advantage of a theoretical basis.     

Effect of hydroxylpropyl-��-cyclodextrin on Solubility of Carvedilol

The present study was undertaken to examine the effect of pH and concentration of hydroxypropyl-β-cyclodextrin on the solubility of carvedilol as it shows pH-dependent solubility. The equilibrium solubility of carvedilol in a series of solutions of varying pH (from 1.2 to 11) was determined and compared with the equilibrium solubility of carvedilol in the presence of 20% hydroxypropyl-β-cyclodextrin at same pH values. It was observed that solubility of protonated form is more than neutral molecule. Hydroxypropyl-β-cyclodextrin resulted in increased solubility at all the pH. But inclusion in the cavity of hydroxypropyl-β-cyclodextrin might depend upon charge state of the molecule. So it can be concluded that solubility of carvedilol, can be increased either by the addition of hydroxypropyl-β-cyclodextrin or by adding pH lowering agents. But both these methods if are to be used together, pH should be selected carefully.     

Kinesin Spindle Protein Inhibitors with Diaryl Amine Scaffolds: Crystal Packing Analysis for Improved Aqueous Solubility

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Quantitative Solubility Relationships and the Effect of Water Uptake in Triglyceride/Monoglyceride Microemulsions

Purpose This paper aims to elucidate quantitative relationships between small molecule solubility/water-uptake in triglyceride/monoglyceride lipid formulations, the chemical structure of the solute, and the solvent composition. Methods Solubility and water uptake in tricaprylin/1-monocaprylin and tricaprylin/1-monocaprin mixtures in the “microemulsion” region at 37°C were determined with HPLC and KF coulometry, respectively. Twelve model solutes varying in hydrogen bond acidity, basicity, polarity, and molecular volume were chosen. Linear free energy relationships (LFER) (Abraham type) were implemented to obtain solvent coefficients at various monoglyceride concentrations. Results Profiles for both solubility and water uptake (at different water activities) in lipid mixtures containing different monoglycerides were superimposable, producing a single master curve when the monoglyceride concentrations were plotted on a molar scale. The LFER derived solvent coefficients showed a systematic dependence on the lipid composition consistent with the view that relative solubility is determined largely by the molar concentrations of individual functional groups such as glyceride ester moieties and hydroxyl groups. At low RH, water uptake increased linearly with monoglyceride concentration while cooperativity was evident in water uptake profiles at high RH. Conclusions This study provides a potential universal framework for predicting relative drug solubility in mixtures containing fully saturated triglycerides and monoglycerides.