Journal Title
Title of Journal: J Solution Chem
|
Abbravation: Journal of Solution Chemistry
|
|
|
|
|
|
|
|
Authors: Yihua Li Wenge Yang Tuan Zhang Chaoyuan Wang Kai Wang Yonghong Hu
Publish Date: 2013/11/12
Volume: 42, Issue: 12, Pages: 2342-2353
Abstract
Solubility data were measured for omeprazole sulfide in ethanol 95 mass ethanol ethyl acetate isopropanol methanol acetone nbutanol and npropanol in the temperature range from 28035 to 31965 K by employing the gravimetric method The solubilities increase with temperature and they are in good agreement with the calculated solubility of the modified Apelblat equation and the λh equation The experimental solubility and correlation equation in this work can be used as essential data and model in the purification process of omeprazole sulfide The thermodynamic properties of the solution process including the Gibbs energy enthalpy and entropy were calculated using the van’t Hoff equationOmeprazole sulfide is synthesized using 2mercapto5methoxybenzene imidazole and 2chloromethyl4methoxy35lutidine 8 or 4methoxy35dimethyl2pyridinemethyl bromide 9 as substrate It should be purified by dissolution crystallization and separation Crystallization processes are the critical steps that determine the quality of the product 10 of omeprazole sulfide to provide sufficient purity for the next reaction So it is very important to know the solubility of omeprazole sulfide as a function of temperature and solvent composition in selected solvents required for the preparation and purification of the products 11 Moreover no literature study has reported the correlation between the solubility and temperature or the solvent composition The most basic information for solving the solvent selection problem is the basic physical properties and solubility data 12 Therefore we measured and correlated the solubility data of omeprazole sulfide in different solvents ethanol 95 mass ethanol ethyl acetate isopropanol methanol acetone nbutanol and npropanol over the temperature range 28035–31965 K under atmospheric pressure by the gravimetric method 13 14 Thus systematic and necessary information on the crystallization of omeprazole sulfide was obtained For predicting the solubility of a solute in different solvents several methods have been presented 11 15 This study used the modified Apelblat equation and the Buchowski–Ksiazaczak λh equation to correlate and predict the solubility of omeprazole sulfide in different solventsA white crystalline powder of omeprazole sulfide was supplied by Shanghai Lingfeng Chemical Reagent Co China The mass fraction was higher than 0995 measured by high performance liquid chromatography HPLC type DIONEX P680 DIONEX Technologies The melting temperature was 39215 K determined by differential scanning calorimeter Netzsch DSC 204 The ethanol ethyl acetate isopropanol methanol acetone nbutanol and npropanol used for experiment were all analytical purity grade with mass fraction purity higher than 0995 except for 95 ethanol They were supplied by Shanghai Shenbo Chemical Co Ltd and used without further purificationThe solubility of omeprazole sulfide was determined by a gravimetric method The balance used in these experiments was an analytical balance with an uncertainty of ±00001 g Sartorius BS210S 8 mL of solvent and a rotor were put into a 10 mL glass test tube with stopper and then excess omeprazole sulfide was added into the glass test tube 16 The test tubes were partly immersed in a constanttemperature bath The temperature was controlled by a jacketed vessel with water circulated through the outer jacket from a super thermostatic watercirculator bath type DC2006 Ningbo XinYi Biotechnology Co Ltd Meanwhile the inner chamber of the vessel needs a mercuryinglass thermometer with an uncertainty of ±005 K calibrated by using a standard thermometer for measuring the solution equilibrium temperature Continuous stirring was adopted for fully mixing the suspension with a magnetic stirrer at each temperature 17
Keywords:
.
|
Other Papers In This Journal:
- Ab Initio Molecular Dynamics Simulation of Infrared Absorption Spectra of H 3 O + and H 5 O 2 + in Nonaqueous Solutions of Trifluoromethanesulfonic Acid Hydrates
- Modified Screen-Printed Electrode for Potentiometric Determination of Copper(II) in Water Samples
- Inclusion Complexes of Cyclodextrins with Galangin: a Thermodynamic and Reactivity Study
- Determination of Activation Energy for the Diffusion of Fe 3+ Ions in Agar Gel Medium Containing Various Transition Metal Sulfates
- NMR Study of the Exchange Kinetics of 30-Crown-10 Complexes with Sr 2+ and Ba 2+ Cations and Crystal Structure of the 30-Crown-10 Complex with Barium Perchlorate
- A Study of the Excess Properties of Aliphatic Chlorinated Compounds with Benzylalcohol at Various Temperatures
- Liquid–Liquid Equilibria of the Methanol + Toluene + Methylcyclohexane Ternary System at 278.15, 283.15, 288.15, 293.15, 298.15 and 303.15 K
- Complexation of Am(III) and Nd(III) by 1,10-Phenanthroline-2,9-Dicarboxylic Acid
- Diffusion Coefficients for the Ternary System Water + Chloroform + Acetic Acid at 25 °C
- Binding Mechanism of Bioactive Cetirizine Hydrochloride to Sudlow’s Site I of Serum Albumins
- Electroluminescent Properties of LECs Based on Ionic Transition Metal Complexes Using Tetrazole-Based Ancillary Ligand
- High-Pressure Densities and Derived Volumetric Properties (Excess, Apparent and Partial Molar Volumes) of Binary Mixtures of Methanol + [BMIM][PF 6 ]
- Solvent Effects on the Protonation Constants of Some α -Amino Acid Esters in 1,4-Dioxane–Water Mixtures
- Lanthanide Complexes with Allyl Acetoacetate in Mixed Water–Organic Media: Formation, Stability and Bonding
- A Study on Host–Guest Complexation of 5-Amino-2-Mercaptobenzimidazole with β -Cyclodextrin
- The Mixing Enthalpy Interaction Coefficients of N , N ′-Hexamethylenebisacetamide with l -Alanine and l -Serine in Aqueous Glucose Solutions at 298.15 K
- Effect of Temperature on Salt–Salt Aqueous Biphasic Systems: Manifestations of Upper Critical Solution Temperature
- Studies on Intermolecular Interactions in Liquid Mixtures of Alkoxyalkanols and Branched Alcohols by Volumetric and Acoustic Measurements at Different Temperatures
- Li + Transport Mechanism in Oligo(Ethylene Oxide)s Compared to Carbonates
- Thermodynamics of concentrated electrolyte mixtures. I. Activity coefficients in aqueous NaCl−CaCl 2 at 25°C
- Study of the Association Behavior Between Bromophenol Blue and Octylphenol Polyoxyethylene Ether (10) in Aqueous Solution and the Solubilization of Bromophenol Blue by Micelles
- Kinetics and Mechanism of the Reactions Between Triphenylphosphine, Dialkyl Acetylenedicarboxilates and a NH-Acid, Pyrazole, by UV Spectrophotometry
- Isopiestic Determination of the Osmotic and Activity Coefficients of Li 2 SO 4 (aq) at T =298.15 and 323.15 K, and Representation with an Extended Ion-Interaction (Pitzer) Model
- Volumetric and Transport Properties of Ternary Mixtures Containing 1-Butanol or 1-Pentanol, Triethylamine and Cyclohexane at 303.15 K: Experimental Data, Correlation and Prediction by the ERAS Model
- First Hydrolysis Constant of Lutetium (III) by Solvent Extraction
- Volumetric Properties of the Nucleoside Thymidine in Aqueous Solution at T = 298.15 K and p = (10 to 100) MPa
- Spinodal Composition of the System Water + Chloroform + Acetic Acid at 25 °C
- Complexation Studies of Pyridyl Sulfonamide Ligands for Sensing Zinc and Copper Ions
- A Thermodynamic Study on the Binding of Cobalt(II) and Iron(III) Ions with Bovine Carbonic Anhydrase II at Different Temperatures
- Chemical Equilibria Modeling of Calcium Phosphate Precipitation and Transformation in Simulated Physiological Solutions
- Isopiestic Determination of the Osmotic and Activity Coefficients of the { y Na 2 HPO 4 + (1 − y )K 2 HPO 4 }(aq) System at T = 298.15 K
- Ionic Strength Effect on the Stability of the V(V) + IDA Complex
- Viscosities for Ionic Liquid Binary Mixtures with a Common Ion
- Kinetics and Mechanism for Hydrolysis of α -Amino Acid Esters in Mixed Ligand Complexes with Zn(II)–Nitrilo-tris(methyl phosphonic Acid)
- The Oxidation of Iron(II) with Oxygen in NaCl Brines
|