Imperial College London
Portrait Picture

Prof Jason P. Hallett

Faculty of Engineering, Department of Chemical Engineering

Professor of Sustainable Chemical Technology
 
 
 
//

Contact

 

+44 (0)20 7594 5388j.hallett Website

 
 
//

Location

 

228bBone BuildingSouth Kensington Campus

//

Summary

 

Publications

Citation

BibTex format

@article{Hunt:2016:10.1039/C6CP02286C,
author = {Hunt, PA and Welton, T and Hallett, J and Schmauck, J and Bordes, E and Kuzmina, O},
doi = {10.1039/C6CP02286C},
journal = {Physical Chemistry Chemical Physics},
pages = {16161--16168},
title = {Solubility of Alkali Metal Halides in the Ionic Liquid [C4C1im][OTf]},
url = {http://dx.doi.org/10.1039/C6CP02286C},
volume = {18},
year = {2016}
}
Download

RIS format (EndNote, RefMan)

TY  - JOUR
AB  - The solubilities of the metal halides LiF, LiCl, LiBr, LiI, NaF, NaCl, NaBr, NaI, KF, KCl, KBr, KI, RbCl, CsCl,CsI, were measured at temperatures ranging from 298.15 to 378.15 K in the ionic liquid 1-butyl-3-methylimidazolium trifluoromethanesulfonate ([C4C1im][OTf]). Li+, Na+and K+salts with anionsmatching the ionic liquid have been also investigated to determine how well these cations dissolve in[C4C1im][OTf]. This study compares the influence of metal cation and halide anion on the solubility ofsalts within this ionic liquid. The highest solubility found was for iodide salts and the lowestsolubility, for the three fluoride salts. There is no outstanding difference in the solubility of salts withmatching anions in comparison to halide salts. The experimental data were correlated employingseveral phase equilibria models, including ideal mixtures, van’t Hoff, the λh (Buchowski) equation,the modified Apelblat equation, and the non-random two-liquid model (NRTL). It was found that thevan’t Hoff model gave the best correlation results. On the basis of the experimental data thethermodynamic dissolution parameters (ΔH, ΔS, and ΔG) were determined for the studied systemstogether with computed gas phase metathesis parameters. Dissolution depends on the energydifference between enthalpies of fusion and dissolution of the solute salt. This demonstrates thatovercoming the lattice energy of the solid matrix is the key to the solubility of inorganic salts in ionicliquids.
AU  - Hunt,PA
AU  - Welton,T
AU  - Hallett,J
AU  - Schmauck,J
AU  - Bordes,E
AU  - Kuzmina,O
DO  - 10.1039/C6CP02286C
EP  - 16168
PY  - 2016///
SN  - 1463-9084
SP  - 16161
TI  - Solubility of Alkali Metal Halides in the Ionic Liquid [C4C1im][OTf]
T2  - Physical Chemistry Chemical Physics
UR  - http://dx.doi.org/10.1039/C6CP02286C
UR  - http://hdl.handle.net/10044/1/33096
VL  - 18
ER  -
Download