Sulfolanes as solvents for potentiometric titrations

Morman, Donald H.; Harlow, G. A.

doi:10.1021/ac50157a064

Cited by 36 publications

(14 citation statements)

References 10 publications

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“…This confirms the existence of the stable cationic homocomplexed cation (PyOHÁ Á ÁOPy) + . It is worth mentioning that similar shapes of the potentiometric titration curves have also been observed in the experiments carried out by Van der Heijde [38] and Harlow [39,40], who investigated the homoconjugation equilibria in acetonitrile, acetone, pyridine, benzene, toluene, and sulfolanes.…”

Section: Resultssupporting

confidence: 71%

Experimental and theoretical studies of solvent effects on the hydrogen bonds in homoconjugated cations of substituted 4-halo (Cl, Br) pyridine N-oxide derivatives

Gurzyński

Puszko

Makowski

et al. 2007

The Journal of Chemical Thermodynamics

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Hydrogen bond OHO-type bridges formed between six substituted 4-halo (Cl, Br) pyridine N-oxide systems and their simple cations have been investigated by using the potentiometric titration method. The formation constants of these complexes (expressed as lg K BHB þ ) have been determined in two non-aqueous aprotic solvents with different polarity, i.e., acetone (AC) and acetonitrile (AN). It has been observed that tri-and tetra-substituted pyridine N-oxides [B] and their cationic acids [BH + ] form stable homocomplexed cations [BHB + ] stabilized by OÁ Á ÁHÁ Á ÁO bridges in both solvents used. It has been found that the most stable homocomplexed system is formed by 3,5-dimethyl-4-chloropyridine N-oxide (3,5Me 2 4ClPyO). The lg K BHB þ values for this compound in acetone and acetonitrile are 3.15 and 2.82, respectively. Furthermore, by using ab initio methods at the RHF and MP2 levels utilizing the Gaussian 6-31++G ** basis set, the energies of formation of the homocomplexed cations and Gibbs free energies have been determined in vacuo. The calculated energy parameters in vacuo have been compared with the cationic homoconjugation constants determined potentiometrically in acetone and acetonitrile to establish a correlation between these magnitudes. Additionally, the results of potentiometric measurements have been used to determine the acidity constants of the conjugate acids of N-oxides.

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Section: Resultssupporting

confidence: 71%

Experimental and theoretical studies of solvent effects on the hydrogen bonds in homoconjugated cations of substituted 4-halo (Cl, Br) pyridine N-oxide derivatives

Gurzyński

Puszko

Makowski

et al. 2007

The Journal of Chemical Thermodynamics

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“…The maximum ionic conductivity achieved for each solvent is presented in Figure 2a together with the viscosity and dielectric constant for the salt‐free solvents, [12–21] while the conductivity as a function of concentration is displayed in Figure 2b.…”

Section: Resultsmentioning

confidence: 99%

“…The maximum ionic conductivity achieved for each solvent is presented in Figure 2a together with the viscosity and dielectric constant for the salt-free solvents, [12][13][14][15][16][17][18][19][20][21] while the Dielectric constant and viscosity for salt-free solvents, [12][13][14][15][16][17][18][19][20][21] compared with the maximum achieved ionic conductivity at room temperature for all the tested solvents (a). The ionic conductivity as a function of the NaPF 6 concentration in molal for all the tested solvents (b).…”

Section: Resultsmentioning

confidence: 99%

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An Attempt to Formulate Non‐Carbonate Electrolytes for Sodium‐Ion Batteries

Mogensen

Colbin

Younesi

2021

Batteries & Supercaps

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Non‐aqueous carbonate solvents have been the main choice for the development of lithium‐ion batteries, and similarly most research on sodium‐ion batteries have been performed using carbonate‐based solvents. However, the differences between sodium and lithium batteries – in term chemistry/electrochemistry properties as well as electrode materials used – open up opportunities to have a new look at solvents that have attracted little attention as electrolyte solvent. This work investigates properties of a wide range of different solvent classes in the context of sodium‐ion battery electrolytes and compares them to the performance of propylene carbonate. The thirteen solvents studied here include one or several members of glymes, carbonates, lactones, esters, pyrrolidones, sulfones, and alkyl phosphates. Out of those, five outperforming solvents of γ‐butyrolactone (GBL), γ‐valerolactone (GVL), N‐methyl‐2‐pyrrolidone (NMP), propylene carbonate (PC), and trimethyl phosphate (TMP) were further investigated using additives of ethylene sulfite (ES), vinylene carbonate (VC), fluoroethylene carbonate (FEC), prop‐1‐ene‐1,3‐sultone (PES), sulfolane (TMS), tris(trimethylsilyl) phosphite (TTSPI), and sodium bis(oxalato)borate (NaBOB). The solvents TMS and tetraethylene glycol dimethyl ether (TEGDME) were tested in 1 : 1 mixtures by volume with the co‐solvents; NMP, dimethoxyethane (DME), and TMP. All electrolytes used NaPF6 as the salt. Primary evaluation relied on electrochemical cycling of full‐cell sodium‐ion batteries consisting of Prussian white cathodes and hard‐carbon anodes. Galvanostatic cycling was performed using both two‐ and three‐electrode cells, in addition, cyclic and linear sweep voltammetry was used to further evaluate the electrolyte formulations. Moreover, the resistance was measured on the anode and cathode, using Intermittent current interruption (ICI) technique.

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“…[12][13][14][15], transport properties of electrolytes (Ref. 4 and 16), and voltammetry of inorganic compounds (Ref.…”

Section: Introductionmentioning

confidence: 99%