Albendazole Solubilization in Aqueous Solutions of Nicotinamide: Thermodynamics and Solute Solvent Interactions

Tripathy, S. Swarupa; Kar, Pravin Kumar

doi:10.13005/ojc/290335

Cited by 7 publications

(10 citation statements)

References 13 publications

(15 reference statements)

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“…transfer of drug from pure water to aqueous solution of solubilizers (Mixed solvents). [23,24] The value of Gibbs free energy for cosolvent and solid colvents was observed in range of -2490.16 to -6820.39 kJ mol −1 , respectively. Saturated solutions of drug were studied for pH dependent solubility at room temperature.…”

Section: Resultsmentioning

confidence: 99%

“…For various aqueous formulation blends of mixed solvents (AF1 to AF8) the value of ΔG 0 tr are extremely negatives and the value are observe to decrease as increase in solubilizers concentration, demonstrating spontaneous nature of drug solubilization. [23,24] The structures of drugs and hydrotropes with different centers of different electro negativity might responsible for the intermolecular hydrogen bonding and electrostatic attraction. Hydrogen bonding between the amide group of urea and various negative centers of drug molecule seems to impart aqueous solubility to aceclofenac.…”

Section: Resultsmentioning

confidence: 99%

“…The solubilizing power and the Gibbs free energy of transfer (ΔG 0 tr) of drug from pure water to the mixed solvent systems emphasize the solubilization effectiveness and thermodynamics involved during the solubility enhancement respectively. [23,24] Application of the mixed solvency has been employed in the present research work to develop the injection formulations of the model poorly water-soluble drug, aceclofenac. It may reduce the individual concentration of solubilizers and so reduce their toxicity associated with them.…”

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Untitled

Solanki

2017

AJP

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Context: Water solubility is an important molecular property for successful drug development as it is a key factor governing drug access to biological membranes. The solubilization of poorly water soluble drug by facilitated mixed solvency is presented. Aim: The aim was to develop the injection formulations of the model poorly water-soluble drug. Settings and Design: Trial and error based experimental study. Materials and Methods: Mixed solvency approach was used to solubilize the hydrophobic drug. Mixed solvent system prepared using water-soluble hydrotropes (such as sodium citrate and urea) and water-miscible cosolvents, such as polyethylene glycol (PEG) 200, PEG 300, PEG 400, PEG 600, glycerin, propylene glycol, and ethanol. Drug was characterized using ultraviolet, Fourier Transform infrared (FT-IR), and Raman spectroscopy. Solubilizing power (Φ) and the Gibbs free energy of transfer (ΔG 0 tr) were determined. Various properties of solution such as pH, viscosity, specific gravity, and refractive index were also studied. Results: Desired solubility of drug achieved in a mixed solvent blend AF5, which was more than 200 fold as compared to the solubility in distilled water 0.152 mg/ml. Drug content was found to be more than 98%. FT-IR and Raman spectroscopy results may support intermolecular hydrogen bonding between drug and mixed solvent system. Developed formulation was physically and chemically stable. Conclusion: This technique proved a synergistic enhancement in solubility of a poorly water soluble drug due to mixed solvent effect and produces a stable formulation. Mixed solvency concept may reduce the individual concentration of solubilizers and so reduce their toxicity associated with them.

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Section: Resultsmentioning

confidence: 99%

Section: Resultsmentioning

confidence: 99%

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confidence: 99%

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Untitled

Solanki

2017

AJP

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“…This improvement was likely due to several mechanisms including addition of solvent to disperse quercetin molecularly and formation of eutectic that reduced particle size 6 . Moreover, the chemical interaction that likely occurred between quercetin and nicotinamide increased the solubility due to properties of nicotinamide which is highly hydrotropic causing an increase in solubility of quercetin 19 . The solubility improvement result was corresponded to DTA result, which a decrease in the melting point of the binary system formed.…”

Section: Resultsmentioning

confidence: 99%

Identification and Characterization of Solid Binary System of Quercetin-Nicotinamide

Zaini¹,

Azhari²,

Fitriani³

2016

Orient. J. Chem

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Preparation of binary system quercetin-nicotinamide and the solubility evaluation have been conducted in this study. Binary system was prepared by solvent evaporation technique and physical mixture was used as comparison. The aim of this study is to analyze the type of interaction and to investigate the solubility of quercetin-nicotinamide produced. Identification of binary system interaction were done using Powder X-ray diffraction (PXRD), Differential Thermal Analysis (DTA), Infrared spectroscopy (IR), Scanning Electron Microscopy (SEM), and solubility test. Determination of quercetin was done in ethanol:water (1:1) by High Performance Liquid Chromatography (HPLC) using acetonitrile:phosphate acid 0,1% (55:45) as mobile phases. Diffractogram powder X-ray showed a decrease in the peak intensity, but did not show a new crystalline phase. DTA thermal analysis showed a decrease in the melting point of the binary system compared to quercetin, which likely eutectic mixture was formed. SEM results indicated the changes in the morphology of the crystal compared to pure components. FT IR analysis showed a shift wavenumber of the spectrum quercetin and nicotinamide. Interaction between these compound showed that the conglomerated form (simple eutectic) between two crystalline phases. The solubility of binary system quercetin-nicotinamide increased compared to intact quercetin. Solubility of quercetin, physical mixture and binary system quercetin nicotinamide were 0.294±0.005 mg/mL, 0.338±0.004 mg/mL, and 0.419±0.001 mg/mL, respectively. In conclusion, the solubility increased after the formation of binary system quercetinnicotinamide.

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“…Thermo physical investigations can provide information regarding the involved thermodynamic and the solute-solvent interaction(r). Conductometric analyses of the surfactant solutions have been widely utilized to study the thermodynamics of the systems (6,7,8,9) [references]. Hence we intend to determine the CMC by conductometric technique so to revalidate the value from literature and to elucidate the involved energetics and thermodynamics with further explanation of the solute solvent interactions.…”

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confidence: 99%