Ionic solvation in water + co-solvent mixtures

Halawani, Kamal H.; Wells, Cecil F.

doi:10.1016/0040-6031(89)87135-7

Cited by 24 publications

(4 citation statements)

References 58 publications

Supporting

Mentioning

Contrasting

Order By: Relevance

“…A cyclic isomer is more stable than a chain one. According to the suggestions of Wells and co-workers, [Bmim]BF 4 may break the equilibrium concerning the cyclic structures and chain structures of sucrose through complexation of [Bmim] + and sucrose. This is supported via UV−visible spectra shown in Figure , where the maximum absorption band undergoes blue-shift and disappears in UV region when concentration of sucrose decreases.…”

Section: Resultsmentioning

confidence: 99%

Temperature Dependence of Phase Behavior for Ternary Systems Composed of Ionic Liquid + Sucrose + Water

Zhang

Wang

et al. 2008

J. Phys. Chem. B

View full text Add to dashboard Cite

In this work, temperature dependence of phase behaviors for the [Bmim]BF 4 + sucrose + water system was investigated. It was found that interaction of [Bmim]BF 4 with sucrose is exothermic, and lowering temperature is favorable for phase separation. In addition, a "[Bmim] (+)-induced structural changes" model was developed and used to interpret the temperature effect, whereby the salting-out effect was thought to be an entropy driving process through analysis of the structural interaction and the electrostatic interaction.

show abstract

Section: Resultsmentioning

confidence: 99%

Temperature Dependence of Phase Behavior for Ternary Systems Composed of Ionic Liquid + Sucrose + Water

Zhang

Wang

et al. 2008

J. Phys. Chem. B

View full text Add to dashboard Cite

show abstract

“…H + (aq) interacts more strongly with the CO group in a chain glucose molecule than with other oxygen atoms (−OH, −O−). It is possible, as suggested by Wells and co-workers, that a H + ion and a glucose molecule form a stable glucose−H + (aq) ion. If this is true, equilibria I will be broken.…”

Section: Discussionmentioning

confidence: 95%

“…Using the spectrophotometric solvent-sorting method, Wells and co-workers 18 obtained free energies of transfer of H + , ∆ t G°-…”

Section: Interaction Parameters Between Ions and Glucosementioning

confidence: 99%

Thermodynamics of the Interacton of HCl withd-Glucose in Water at 278.15−318.15 K

et al. 1997

View full text Add to dashboard Cite

Electromotive forces of cells without liquid-junction Pt, H 2 (g, p°)|HCl(m E )|AgCl-Ag and Pt, H 2 (g, p°)|HCl-(m E ),G(m N )|AgCl-Ag, have been measured at 10 K intervals from 278.15 to 318.15 K, where G refers to D-glucose, m E ) 0.005-0.1 mol kg -1 , and m N ) 0.1-0.3 mol kg -1 . The thermodynamic parameters of interaction, f EN (g EN , h EN , s EN c p,EN ), of G with HCl in water have been evaluated. It appears that g EN > 0, h EN > 0, Ts EN > 0, and c p,EN < 0 at all five temperatures (except for Ts EN at 318.15 K), and the values of g EN vary slightly with temperature, whereas the values of h EN and Ts EN decrease rapidly from positive to negative with increasing temperature. By use of the values of ∆ t G°(H + ) reported by Wells and co-workers, the values of g H + -G and g Cl --G have been obtained at 298.15 K. A comparison of the interaction parameters for the HCl-G pair with those for the MCl (alkali chlorides)-G pair shows that the g EN , h EN , and s EN for the HCl-G pair are obviously higher than those for the MCl-G pair. These were interpreted in terms of the suggestion "H + -induced structural changes". Furthermore, it has been shown that the group additivity parameters obtained from the HCl-alcohol-water systems is not applicable to the HCl-G-water system.

show abstract

“…Clearly once one site is protonated, this deactivates the electron availability at the other sites. 27 The early observations using 5% v/v co-solvents at 25 C, produced the following values 6 for K c (dm 3 mol À1 ): diethyl ether (0.50), dioxane (0.73). Comparison with methanol (0.09) 20 and ethanol (0.27) 6 indicates a higher basicity for ethereal -CH 2 -O-CH 2 -over -OH.…”

Section: Comparison With Dg O T (H + ) For Mixtures Of Water With Oth...mentioning

confidence: 99%

Gibbs energies of transfer of the proton from water into mixtures of water with chain multiple ethers: Equilibria involving changes of solvation of the proton

Goldie

Luck

Wells

2003

Phys. Chem. Chem. Phys.

Self Cite

View full text Add to dashboard Cite

Ionic solvation in water + co-solvent mixtures

Cited by 24 publications

References 58 publications

Temperature Dependence of Phase Behavior for Ternary Systems Composed of Ionic Liquid + Sucrose + Water

Temperature Dependence of Phase Behavior for Ternary Systems Composed of Ionic Liquid + Sucrose + Water

Thermodynamics of the Interacton of HCl withd-Glucose in Water at 278.15−318.15 K

Gibbs energies of transfer of the proton from water into mixtures of water with chain multiple ethers: Equilibria involving changes of solvation of the proton

Contact Info

Product

Resources

About