Specific conductance of concentrated solutions of magnesium salts in water-ethanol system

Casteel, Jerry F.; Amis, Edward S.

doi:10.1021/je60052a029

Cited by 156 publications

(112 citation statements)

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“…Fig. 1 shows the specific conductivity κ and the molar conductivity Λ of KF + GC solutions as a function of c. The data of κ and Λ were fitted according to the Casteel-Amis equation [15], and to the Fuoss-Kraus model, respectively (see Appendix A) [16].…”

Section: Electric Conductivity Measurementsmentioning

confidence: 99%

“…The specific conductivity (κ) was fitted according to the Casteel-Amis model that provides an empirical equation commonly used to describe the conductivity behavior of electrolytes over wide ranges of salt concentration [15,36]. In this model the relation between κ and the concentration m (in molal units) is expressed as:…”

Section: Appendix a Casteel-amis Equation And Fuoss-kraus Formalismmentioning

confidence: 99%

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The curious effect of potassium fluoride on glycerol carbonate. How salts can influence the structuredness of organic solvents

Sarri

Tatini

Ambrosi

et al. 2018

Journal of Molecular Liquids

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Glycerol carbonate (4-hydroxymethyl-1,3-dioxolan-2-one, shortly GC) is a dense, viscous, water soluble solvent. The high dielectric constant and dipole moment make it a suitable non-aqueous green solvent for several salts in different applications. GC dissolves significant amounts of inorganic salts such as KF. The saturation of GC with KF leads to the formation of a viscous liquid at room temperature. In this paper, we report on conductivity, rheology, differential scanning calorimetry and infrared spectroscopy experiments that indicate the formation of a glassy liquid where GC molecules and KF ion pairs are intercalated in a firm and ordered bidimensional structure, stabilized by hydrogen bonding and strong ion-dipole interactions.

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Section: Electric Conductivity Measurementsmentioning

confidence: 99%

Section: Appendix a Casteel-amis Equation And Fuoss-kraus Formalismmentioning

confidence: 99%

The curious effect of potassium fluoride on glycerol carbonate. How salts can influence the structuredness of organic solvents

Sarri

Tatini

Ambrosi

et al. 2018

Journal of Molecular Liquids

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“…The most conspicuous feature emerging from these plots is the ''dome'' shape of the surfaces, as a result of peaking in both m and w. Peaking of in m is a common feature for liquid electrolytes, reflecting the process of first increasing with the number of dissociated ions as m increases and then falling as the rise in and in ion association become dominant; this has been observed for many electrolytes of lithium salts. 1,2,[5][6][7]14,15,22,[31][32][33] Peaking of in w, on the other hand, seems to be the result of the and of DEC both being much lower than those of PC and both being monotonic functions of w. As such, as w rises from zero, the change of is first dominated by the fall of of the electrolyte causing to rise and then by the fall of of the solvent which by allowing stronger ion association causes to fall. The same behavior has been observed in LiPF 6 -(PC-DEC), 1 LiBF 4 -(PC-DEC), 2 and LiPF 6 -(EC-EMC), 7 where the linear carbonates DEC and EMC have much lower and than their cyclic counterparts PC and EC, and in LiClO 4 -(PC-DME) 8 and NaClO 4 -(PC-DME), 9 where DME ͑dimethoxyethane͒ has a much lower and than PC.…”

Section: 25mentioning

confidence: 99%

Conductivity and Viscosity of PC-DEC and PC-EC Solutions of LiBOB

Ding

Jow

2005

J. Electrochem. Soc.

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Conductivity of propylene carbonate-diethyl carbonate ͑PC-DEC͒ and propylene carbonate-ethylene carbonate ͑PC-EC͒ solutions of lithium bis͑oxalato͒borate ͑LiBOB͒ was experimentally determined at temperatures from 60 to Ϫ80°C, salt molalities m from 0.04 to 1.1 mol kg Ϫ1 , and solvent compositions w from 0 to 0.7 weight fraction of DEC and EC. Viscosity of LiBOB in PC-EC was studied through measuring its glass transition temperature T g in the same ranges of m and w. T g was found to rise with m and w of EC, indicating a concurrent change in the of the solution. The of the PC-DEC solution of LiBOB peaked in both m and w thus forming a ''dome'' in its 3D presentation in the coordinates of m and w, while that of the PC-EC solution peaked only in m resulting in an ''arch''-shaped surface. As the was lowered, these surfaces fell in height and shifted in the direction of low . These observations correlated well with the changes of dielectric constant of the solvents and of the solutions with the same set of variables. The measured (T) data for the PC-DEC solution was fitted with the Vogel-Tamman-Fulcher equation for an evaluation of its vanishing mobility temperature and apparent activation energy. The results of and of the LiBOB solutions were further compared with those of LiPF 6 solutions from a previous study. This report parallels two earlier ones 1,2 in both structure and content, those dealing with conductivities and viscosities of propylene carbonate-diethyl carbonate ͑PC-DEC͒ and propylene carobonate-ethylene carbonate ͑PC-EC͒ solutions of LiPF 6 and LiBF 4 , respectively; this report dealing with lithium bis͑oxalato͒bo-rate ͑LiBOB͒.3 As such, this report, while giving full account of the new experimental results, skips over some of the detailed descriptions and explanations that can be found in previous reports. Also, although the measured properties of LiBOB are briefly compared with those of LiPF 6 in this report, a fuller comparison across all three salts and its discussion will be left to another report that is to follow.The aim of this report is mainly to provide a relatively complete picture for the change of conductivity with salt molality m and solvent weight fraction w at different temperatures ͑ symbolizes temperature in degrees centigrade and T in degrees of absolute temperature, K͒ 3 for PC-DEC and PC-EC solutions of LiBOB, denoted here as (LiBOB) m -PC 1Ϫw DEC w and (LiBOB) m -PC 1Ϫw EC w . It is felt that such a picture, together with what is already known of dielectric constant and viscosity of PC-DEC and PC-EC solvents and of and of their electrolytes of LiBF 4 and LiPF 6 , 1,2,4,5 could lead to a clear demonstration of the similarities and differences in the change of with m and w and with for the three important lithium salts in the carbonate solvents and to an elucidation of the mechanisms giving rise to these similarities and differences.As has been amply demonstrated, of an electrolyte of a particular salt is critically dependent on the of the solvent and the of the electrolyte:-rises wi...

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“…7 shows the typical concentration-dependence of the specific conductance, x[Q 1 cm" 1 ], of LiClO 4 at various temperatures in propylene carbonate 232) and propylene carbonate-dimethoxyethane mixtures 227) . Lacking a reliable theory, an empirical equation 231) was used to reproduce the conductance data. The concentration, m max , at maximum conductance, x mux , decreases with decreasing temperature, i.e.…”

Section: Concentrated Solutionsmentioning

confidence: 99%