Benner
فلاح شريف الخفاجي ( أستاذ )
كلية الصيدلة - صيدلة عام ( رئيس القسم )
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Stability of Anticancer Drug 5-Fluorouracil in Aqueous Solution: An Assessment of Kinetic Behavior
تحميل
بحث النوع:
علوم التخصص العام:
Razzaq Abd Al-Zahra Ibrahim اسم الناشر:
Falah Shareef Abed Suhail, Hussein Kadhem Al-Hakeim اسماء المساعدين:
Nano Biomed. Eng., 2018, Vol. 10, Iss. 3 الجهة الناشرة:
Nano Biomedicine and Engineering. Copyright © 2009-2019 OAHOST, Publication and Conference Management by Scientists and for Scientists. © Shanghai Jiao Tong University Press  
2018 سنة النشر:

الخلاصة

Spectroscopic measurements of pharmaceutical compound 5-fluorouracil (5-FU) drug was achieved in solvents with different polarity. The drug gave clear absorption peak at 259, 269, 270 and 266 nm in hexane, dimethyl sulfoxide (DMSO), N, N-dimethylformamide (DMF) and ethanol, as well as phosphate buffer respectively, which was consistent with the standard values in literatures. The results of extension coefficient (ε) and wave length (λmax) showed reduction in polar medium as compared to non-polar medium. The calibration curve of 5-FU drug was achieved by using serials solutions dissolved in phosphate buffer (pH = 7.4 and T = 37 °C) within the range of 1×10– 6 ~ 1×10– 4 M. The stability of 5-FU drug was studied in phosphate buffer at pH = 5, 6, 7, 7.4 and 8 with 1×10– 5 M and T = 37 °C, according to the equation of first-order reaction. The hydrolysis of 5-FU disappeared at alkaline solution, but had noticeable hydrolysis in acidic solutions with the rate constant 25, 14 and 20 at pH of 5, 6 and 7 respectively. The calculation of molar extension coefficient and half-life (t1/2) showed same sequence of 5-FU hydrolysis. Then, rearrangement of obtained results offered complicated reversible equilibrium state by the combination between thermodynamic and kinetic behaviors of 5-FU hydrolysis; with Keq = 8.46, 6.11 and 142.8 at pH of 5, 6 and 7 respectively. The acidic hydrolysis of 5-FU occurred spontaneously within free energy (ΔG) did not exceed 10 kJ/mol, which meant the electro motive forces of interactions were weak, notable to release energy such as Van der Waals forces or hydrogen bonding.