THE CHEMISTRY OF PROTONS IN AMBIENT-TEMPERATURE IONIC LIQUIDS - SOLUBILITY AND ELECTROCHEMICAL PROFILES OF HCL IN HCL-IMCL-ALCL3 IONIC LIQUIDS AS A FUNCTION OF PRESSURE (295 K)
Jle. Campbell et Ke. Johnson, THE CHEMISTRY OF PROTONS IN AMBIENT-TEMPERATURE IONIC LIQUIDS - SOLUBILITY AND ELECTROCHEMICAL PROFILES OF HCL IN HCL-IMCL-ALCL3 IONIC LIQUIDS AS A FUNCTION OF PRESSURE (295 K), Journal of the American Chemical Society, 117(29), 1995, pp. 7791-7800
The liquidus region of the HCl:ImCl:AlCl3 ionic liquid system has been
determined through manometric measurement of HCl solubility as a func
tion of pressure for 0 < P-HCl < 1 atm at 295 +/- 1 K. Analysis of the
pressure-composition isotherms thus obtained, in conjunction with spe
ctroscopic data, reveals that dissolution of HCl in these systems is a
ssociated with reactions of the general form HCl(g) + X(-)(1) reversib
le arrow HCIX(-)(1), where X(-) drop Cl-, HCl2-, H2Cl3- AlCl4-, or Al2
Cl7-. In the binary HCl:ImCl system, the HCl-derived proton exists as
HCl2- H2Cl3-, and H3Cl4-; the equilibrium constants for the reaction a
bove are 715 +/- 76, 3.28 +/- 0.05, and 0.74 +/- 0.02 atm(-1) for X(-)
drop Cl-, HCl2-, and H2Cl3- respectively. In Lewis acidic HCl:ImCl:Al
Cl3 melts (X(AlCl3), > X(ImCl)), HCl is complexed as the species AlCl4
. HCl- and Al2Cl7 . HCl-. The corresponding equilibrium constants wer
e determined as 0.135 +/- 0.001 and 0.109 +/- 0.001 atm(-1) for X(-) =
AlCl4- and Al2Cl7-, respectively. In Lewis basic HCl:ImCl: AlCl3 syst
ems, all species with the exception of Al2Cl7 . HCl- contribute, thoug
h the equilibrium constants associated with the reaction above are les
s well-defined, being dependent on the specific composition of the mel
t. Liquid phase equilibria such as reported earlier from this laborato
ry are obtained by combining two or more of the dissolution equilibria
above such that molecular HCl does not appear in the result. Electroc
hemical profiles of HCl dissolved in HCl:ImCl:AlCl3 ionic liquids are
reported as a function of HCl pressure for 0 < P-HCl < 1 atm at 295 +/
- 1 K. In Lewis basic systems, the electroactivity of HCl2-, H2Cl3-, a
nd AlCl4 . HCl- is observed, while in Lewis acidic systems, two electr
oactive protic species are present: AlCl4 . HCl- and Al2Cl7 . HCl-. Th
e reduction potential of Al2Cl7 . HCl is ca. 0.7 to 1.0 V more positiv
e than that of other protic species, confirming that the proton of Al2
Cl7 . HCl- is exceptionally labile. Based on this observation, we conc
lude that Al2Cl7 . HCl- is the entity responsible for Bronsted superac
idity observed in the Lewis acidic melts. It is demonstrated that the
reproducibility of voltammograins requires strict control of the HCl p
ressure.