@article{koronaios_osteryoung_2001, title={Buffering of 1-ethyl-3-methylimidazolium chloride/aluminum chloride ionic liquids using alkali metal bromides and iodides}, volume={148}, ISSN={["0013-4651"]}, DOI={10.1149/1.1416505}, abstractNote={The buffering of 1--ethyl-3-methylimidazolium chloride-aluminum trichloride (AlCl 3 ) room-temperature ionic liquids (melts) using alkali metal bromides and iodides was studied. The bromide or iodide salts buffer the melts by reaction with the Al 2 Cl - 7 ion, but the bromide or iodide ions do not replace the chloride from the AlCl - 4 in the melts. Unlike melts buffered with alkali metal chlorides, it is easy to deposit the alkali metals, and thus it may be possible to use these buffered melts in power sources. In melts buffered with a mixture of lithium chloride and iodide, it is possible to both deposit and strip lithium metal. As seen with melts buffered with alkali metal chlorides, the buffered melts appear to he more acidic than expected from the low concentration of the acidic Al 2 Cl 7 ion.}, number={12}, journal={JOURNAL OF THE ELECTROCHEMICAL SOCIETY}, author={Koronaios, P and Osteryoung, RA}, year={2001}, month={Dec}, pages={E483–E488} }
 @article{koronaios_osteryoung_2000, title={Use of the Ag/AgCl/Cl- electrode to estimate solubility products in ambient temperature ionic liquids}, volume={147}, ISSN={["0013-4651"]}, DOI={10.1149/1.1393914}, abstractNote={The silver-silver chloride electrode has been investigated in 1-ethyl-3-methylimidazolium chloride/aluminum chloride room-temperature ionic liquids. The electrode is stable only in a narrow range of acidity around the neutral point, but in this range functions as a reversible Ag/AgCl/Cl - system. The electrodes were used to make measurements in buffered and neutral buffered melts to estimate the solubility products (and complex formation constants) of several buffering agents; the solubility products are related to the acidity of the buffered neutral melts. For melts buffered with LiCl, NaCl, and KCl, the values of solubility products obtained were in accord with previous measurements where the ratio of solubility products was determined.}, number={9}, journal={JOURNAL OF THE ELECTROCHEMICAL SOCIETY}, author={Koronaios, P and Osteryoung, RA}, year={2000}, month={Sep}, pages={3414–3419} }
 @article{koronaios_osteryoung_1999, title={CaCl2 and MgCl2 as buffering agents for room-temperature chloroaluminate ionic liquids}, volume={146}, ISSN={["1945-7111"]}, DOI={10.1149/1.1392041}, abstractNote={We have found that it is possible to buffer acidic 1-ethyl-3-methylimidazolium chloride (EMIC)/AlCl 3 melts to neutrality using CaCl 2 as a buffering agent, while MgCl 2 will partially buffer acidic melts. The buffering reaction is MCl 2 (s) + 2Al 2 Cl 7 - → M 2+ + 4AlCl 4 - where M is Ca or Mg. From studies using the Ag/AgCl electrode as a chloride-sensitive electrode and from measurements of the relative solubility products of LiCl and CaCl 2 , it appears that the residual concentration of the acidic Al 2 Cl 7 - ion in the CaCl 2 -buffered melts is significantly higher than in any of the other neutral buffered melts studied so far, making this melt more acidic. These melts show the phenomenon known as latent acidity, forming an AlCl 3 complex with the weak Lewis base acetylferrocene. When MgCl 2 is used as a buffering agent, the reaction above does not go to completion; this is explained in terms of the solubility product of MgCl 2}, number={8}, journal={JOURNAL OF THE ELECTROCHEMICAL SOCIETY}, author={Koronaios, P and Osteryoung, RA}, year={1999}, month={Aug}, pages={2995–2999} }
 @article{koronaios_king_osteryoung_1998, title={Acidity of neutral buffered 1-ethyl-3-methylimidazolium chloride AlCl3 ambient-temperature molten salts}, volume={37}, ISSN={["0020-1669"]}, DOI={10.1021/ic971345u}, abstractNote={A series of studies on the acidity of AlCl3−1-ethyl-3-methylimidazolium chloride (EMIC) melts buffered with alkali metal chlorides were carried out. The solubility of HCl, a strong Bronsted acid in these melts, was measured in melts buffered with LiCl, NaCl, and KCl. The solubility of HCl in all three melts is 450−475 mM under 1 atm of HCl, approximately the same as that in the acidic (AlCl3-rich) melts. The relative solubility products of LiCl, NaCl, and KCl were measured, and it was found that Ksp(NaCl)/Ksp(LiCl) = 72 ± 6 and Ksp(KCl)/Ksp(NaCl) = 1000 ± 400. It is likely that the differences in the acidity of HCl in the various melts are due to the differences in the solubility product of the relevant alkali metal chlorides. These ratios are consistent with the results of previous studies on the acidity of HCl in the melts. The concentrations of the strongly Lewis acidic Al2Cl7- ion in melts buffered with LiCl were measured using an aluminum electrode. The results of the potentiometric work indicate tha...}, number={8}, journal={INORGANIC CHEMISTRY}, author={Koronaios, P and King, D and Osteryoung, RA}, year={1998}, month={Apr}, pages={2028–2032} }
 @article{koronaios_cleaver_1998, title={Effect of pressure on the conductivity of calcium nitrate tetrahydrate}, volume={94}, ISSN={["0956-5000"]}, DOI={10.1039/a707928a}, abstractNote={The conductivity of liquid Ca(NO3)2·4.17H2O has been measured as a function of pressure and temperature over the range 250–1000 atm and 21.6–84°C. The data points were fitted to the empirical VTF equation. It was found that T0, the theoretical glass-transition temperature, rises with pressure, and also that the ‘constants’ A and B in the VTF equation change with pressure. It has previously been suggested that A and B might be pressure dependent, but such changes have not previously been observed. The change in A is attributed to the formation of ion pairs under pressure, while the change in B is less easy to interpret, but may also be due to ion pair formation.}, number={10}, journal={JOURNAL OF THE CHEMICAL SOCIETY-FARADAY TRANSACTIONS}, author={Koronaios, P and Cleaver, B}, year={1998}, month={May}, pages={1477–1479} }
 @article{cleaver_koronaios_1997, title={Effect of pressure on the viscosity of liquid ZnCl2}, volume={93}, ISSN={["0956-5000"]}, DOI={10.1039/a604777g}, abstractNote={The effect of pressure on the viscosity of liquid ZnCl 
 2 
 
has been measured in the range 663⩽T/K⩽719 and 
50⩽P/atm⩽1000,using a falling-weight viscometer with 
a ceramic falling weight with a diameter considerably smaller than 
that of the fall tube, allowing the measurement of absolute viscosity. 
This viscometer has an accuracy of ca. ±5%. The 
viscosity at 670–720 K was found to drop with pressure, to 
ca. 600–700 atm, and then to rise at higher pressures. 
The initial drop in viscosity is interpreted as due to a partial 
break-up of the network structure of liquid ZnCl 
 2 
, while 
the rise in viscosity at higher pressures is probably due to the 
effect of pressure in suppressing ionic mobility.}, number={8}, journal={JOURNAL OF THE CHEMICAL SOCIETY-FARADAY TRANSACTIONS}, author={Cleaver, B and Koronaios, P}, year={1997}, month={Apr}, pages={1601–1604} }