Conductometric Studies of Thermodynamics of 1, 10-Didecyl-1, 10-diaza-18-crown-6 Complexes with Li+, Na+, K+, Cs+, NH4+, Mg2+, and Ca2+ Ions in Acetonitrile, Methanol, and Ethanol Solutions. (21st November 2012)

• Record Type: Journal Article
• Authors: Taghdiri, Mehdi; Payehghadr, Mahmood; Behjatmanesh-Ardakani, Reza; Movahhedi, Sirous; Nourifard, Farzaneh
• Other Names: Avila-Pérez Pedro Academic Editor.
• Is Part Of: Journal of chemistry. Volume 2013(2013)
• Publication Date: 2012-11-21
• Subjects: Chemistry -- Periodicals; 540.5
• DOI: 10.1155/2013/318015
• Languages: English
• ISSNs: 2090-9063

Abstract

Abstract : The complexation reactions between 1, 10-didecyl-1, 10-diaza-18-crown-6 (DD18C6) and Li +, Na +, K +, Cs + NH 4 +, Mg 2+, and Ca 2+ ions were studied conductometrically in acetonitrile, methanol, and ethanol at various temperatures. The formation constants of the resulting 1 : 1 complexes were calculated from the computer fitting of the molar conductance-mole ratio data at different temperatures. In the solvents studied, the stability of the resulting complexes varied in the order acetonitrile ≫ methanol > ethanol. The enthalpy and entropy changes of the complexation reactions were evaluated from the temperature dependence of formation constants. The TΔ S ° versus Δ H ° plot of thermodynamic data obtained shows a linear correlation indicating the existence of enthalpy-entropy compensation in the complexation reactions. The ab initio studies calculated at B3LYP/6-31G level of theory indicate that the binding energy of complexes decreases with increasing cation size in the gas phase. The experimental data obtained in the solvents show different trends so that the stability constant of Li + and Mg 2+ complexes is lower than other alkali and alkaline earth ions, respectively due to the solvation of these small ions in solution.