کد مقاله | کد نشریه | سال انتشار | مقاله انگلیسی | نسخه تمام متن |
---|---|---|---|---|
816357 | 906439 | 2013 | 4 صفحه PDF | دانلود رایگان |
عنوان انگلیسی مقاله ISI
Thermodynamic study of complex formation between 3,5-di iodo-hydroxy quinoline and Zn2+, Ni2+ and Co2+ cations in some binary solvents using a conductometric method
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موضوعات مرتبط
مهندسی و علوم پایه
سایر رشته های مهندسی
مهندسی (عمومی)
پیش نمایش صفحه اول مقاله
چکیده انگلیسی
The complexation reactions between 3,5-di iodo-8-hydroxy quinoline (IQN) and Zn2+, Ni2+ and Co2+ were studied in dimethylformamide (DMF)-ethanol (EtOH) binary solvent systems at different temperatures using a conductometric method. The stoichiometry of complexes was established 1:1. It was found that the stability of complexes formed between cations and this ligand increases with increases temperature. The standard enthalpies and standard entropies of complexes were obtained from the temperature dependence of stability constants. The results obtained by conductometric technique show that there is an inverse relationship between the formation constants of complexes and donor number of solvents. In all cases, the formation constants increased with increasing amounts of EtOH versus DMF in these binary systems. The standard enthalpy and standard entropies of complexes were obtained from the temperature dependence of stability constant. In all cases, ÎH° was positive and ÎS° was negative. The selectivity order for IQN complexes among various neat studied solvents varies in the order: Zn-IQN2+⺠Ni-IQN2+âºCo-IQN2+.
ناشر
Database: Elsevier - ScienceDirect (ساینس دایرکت)
Journal: Alexandria Engineering Journal - Volume 52, Issue 4, December 2013, Pages 797-800
Journal: Alexandria Engineering Journal - Volume 52, Issue 4, December 2013, Pages 797-800
نویسندگان
A. Nezhadali, Gh. Taslimi,