Journal of Thermal Analysis and Calorimetry

, Volume 94, Issue 2, pp 507–510 | Cite as

Studies on thermochemical properties of ionic liquids based on transition metal

  • W. Guan
  • L. Li
  • H. Wang
  • J. Tong
  • J. -Z. Yang


A brown and transparent ionic liquid (IL), [C4mim][FeCl4], was prepared by mixing anhydrous FeCl3 with 1-butyl-3-methylimidazolium chloride ([C4mim][Cl]), with molar ratio 1/1 under stirring in a glove box filled with dry argon. The molar enthalpies of solution, Δs H m, of [C4mim][FeCl4], in water with various molalities were determined by a solution-reaction isoperibol calorimeter at 298.15 K. Considering the hydrolyzation of anion [FeCl4] in dissolution process of the IL, a new method of determining the standard molar enthalpy of solution, Δs H m 0 , was put forward on the bases of Pitzer solution theory of mixed electrolytes. The values of Δs H m 0 and the sum of Pitzer parameters: \( (4\beta _{Fe,Cl}^{(0)L} + 4\beta _{C_4 mim,Cl}^{(0)L} + \Phi _{Fe,C_4 mim}^L ) \) and \( (\beta _{Fe,Cl}^{(1)L} + \beta _{C_4 mim,Cl}^{(1)L} ) \) were obtained, respectively. In terms of thermodynamic cycle and the lattice energy of IL calculated by Glasser’s lattice energy theory of ILs, the dissociation enthalpy of anion [FeCl4], ΔH dis≈5650 kJ mol−1, for the reaction: [FeCl4](g)→Fe3+(g)+4Cl(g), was estimated. It is shown that large hydration enthalpies of ions have been compensated by large the dissociation enthalpy of [FeCl4] anion, Δd H m, in dissolution process of the IL.


enthalpy of solution ionic liquid isoperibol calorimeter Pitzer’s theory 


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Copyright information

© Springer Science+Business Media, LLC. 2008

Authors and Affiliations

  • W. Guan
    • 1
  • L. Li
    • 1
  • H. Wang
    • 1
  • J. Tong
    • 1
  • J. -Z. Yang
    • 1
  1. 1.Department of Chemistry, Laboratory of Green ChemistryLiaoning UniversityShenyangP.R. China

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