Study of the self-association of amoxicillin, thiamine and the hetero-association with biologically active compound chlorgenic acid

Ataklti Abraha; Alemu Kebede; Abebe Belay

doi:10.5897/AJPP2016.4542

African Journal of
Pharmacy and Pharmacology

Abbreviation: Afr. J. Pharm. Pharmacol.
Language: English
ISSN: 1996-0816
DOI: 10.5897/AJPP
Start Year: 2007
Published Articles: 2207

Full Length Research Paper

Study of the self-association of amoxicillin, thiamine and the hetero-association with biologically active compound chlorgenic acid

Ataklti Abraha

Ataklti Abraha
Department of Physics, School of Natural and Computational Sciences, Samara University, P. O. Box 132, Samara, Ethiopia.
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Alemu Kebede

Alemu Kebede
Department of Physics, School of Natural Sciences, Adama Science and Technology University, P. O. Box 1888, Adama, Ethiopia.
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Abebe Belay

Abebe Belay
Department of Physics, School of Natural Sciences, Adama Science and Technology University, P. O. Box 1888, Adama, Ethiopia.
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Article Number - 25EE1EE58542
Vol.10(18), pp. 393-402 , May 2016
https://doi.org/10.5897/AJPP2016.4542

Received: 30 January 2015
Accepted: 25 February 2016
Published: 15 May 2016

Abstract

The self-association of amoxicillin (AMX) and its hetero-association with biologically active compound, chlorogenic acid (CGA) were investigated at room temperature (295°K). The dimerization constant of amoxicillin and thiamine (THIA) analyzed using the dimer model at the wavelength of 278 and 256 nm were found to be and , respectively. The hetero-association constant of amoxicillin and chlorogenic acid analyzed using Benesi-Hildebrand approach were . Thermodynamic parameters such as Gibbs free energy, enthalpy and entropy of dimerization reactions for the self-association and hetero-association of the compounds were also investigated using Vant’s Hoff equation at the temperature ranges (295 to 305°K). The change of enthalpy calculated for amoxicillin, thiamine and the complexes of amoxicillin-chlorogenic acid are 34.73±2.17, 54.1±4.585, and 6.988±0.493 at the temperature of 305°K, respectively. The values of change in enthalpy and entropy indicate that the hydrophobic interaction play the major role in the interaction between the molecules.