Enthalpies of solution of some alkali halides in <i>N</i>‐methylformamide at 25°

Weeda, L.; Somsen, G.

doi:10.1002/recl.19660850208

Cited by 12 publications

(3 citation statements)

References 26 publications

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“…In Figure , we plot m s versus anions of the crystallographic radius, r – (the cation is always the same, Na + ). For the three mixtures studied, the solubility decreases with the weight percent of cosolvent, and the order is NaF < NaCl < NaBr < NaI. ,− …”

Section: Resultsmentioning

confidence: 95%

“…The electrolytes studied are practically dissociated in these media, , and the charges of its ions are 1. In Figure , we plot m s versus anions of the crystallographic radius, r – (the cation is always the same, Na + ).…”

Section: Resultsmentioning

confidence: 99%

“…The immense majority of experimental studies on the solubility of salts have been carried out in water, , pure organic solvents, or aqueous–organic mixtures with cosolvents that have a dielectric constant lower than that of water (ε-decreasing system). Among the systems of this kind, the most studied are those containing alcohols − ,− ,− and ketones, esters and ethers, among other chemical compounds. ,,,,− Data on systems with cosolvents with dielectric constants greater than the dielectric constant of pure water (ε-increasing system) are somewhat more scarce and usually include some amides as the cosolvent. − Aqueous mixtures containing amides (in particular, cyclic amides) constitute an essential tool in the understanding of the behavior of complex molecules of biological interest. , Extensive work has been published on water–amide systems to discover the mode in which water exercises kinetic and thermodynamic control of the chemical activities of polypeptides. The unusually high density of hydrogen bonds in water (strongly self-associated) and the character of the acceptor–donor (−CO–NH–peptide bond) make these water–amide systems very interesting from a structural point of view.…”

Section: Introductionmentioning

confidence: 99%

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Solubility of Sodium Halides in Aqueous Mixtures with ε-Increasing Cosolvents: Formamide, N-Methylformamide, and N-Methylacetamide at 298.15 K

Hernández-Luis

Rodríguez-Raposo

Galleguillos

et al. 2016

Ind. Eng. Chem. Res.

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The solubility data for sodium halides (NaF, NaCl, NaBr, and NaI) have been determined at 298.15 K in the ε-increasing mixtures of water–formamide, water–N-methylformamide, and water–N-methylacetamide. In all cases, the solubility of the electrolytes was decreased significantly in the presence of a cosolvent. The solubility of an electrolyte in a given solvent depends on both the nature of the solvent (mainly the polarity, dielectric constant, solvation, or preferential solvation if the solvent is a mixture of solvents, etc.) and the properties of the electrolyte (principally the size, the charge, and the possible association of its ions). If the molality of saturation is not sufficiently small, the ion–ion and ion–solvent interactions must be considered. Although it was not the objective of this work, the solubility values were qualitatively correlated with several properties of the solvent and solute. Finally, a simple justification, which was both qualitative and quantitative, was carried out.

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Section: Resultsmentioning

confidence: 95%

Section: Resultsmentioning

confidence: 99%

Section: Introductionmentioning

confidence: 99%

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Solubility of Sodium Halides in Aqueous Mixtures with ε-Increasing Cosolvents: Formamide, N-Methylformamide, and N-Methylacetamide at 298.15 K

Hernández-Luis

Rodríguez-Raposo

Galleguillos

et al. 2016

Ind. Eng. Chem. Res.

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Enthalpies of solvation of alkali metal and halide ions in N‐methylformamide and N‐methylacetamide at 25°

Weeda

Somsen

1967

Recl. Trav. Chim. Pays‐Bas

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Measurements of the enthalpies of solution of LiI, NaI, KF, KC1, KBr, KI, RbI and CsI in N-methylacetamide at 35" with an adiabatic calorimeter are reported.A calculation of the ionic enthalpies of solvation of the alkali metal and halide ions in N-methylformamide and N-methylacetamide is given. From the ditference in ionic enthalpy of solvation of the fluoride and the potassium ions in water, formamide, N-mc:thylformamide and N-methylacetaniide, respectively, the quadrupole moments of these solvent molecules have been calculated. IntroductionIn previous papers measurements of the enthalpies of solution of alkali halides in formarnide and N-methylformamide 2 (NMF) have been reported. In order to get a broader experimental basis for the solvation of simple ions in non-aqueous solvents the enthalpies of solution in N-methylacetamide (NMA) should be interesting. The solubility of most salts in NMA is good, only the rate of dissolution is lower than in formamide and NMF.

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Enthalpies of solution of some alkali halides in N,N‐dimethylformamide at 25°C: (Short communication)

Weeda

Somsen

1967

Recl. Trav. Chim. Pays‐Bas

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In connection with our investigations about the enthalpies of solvation of univalent ions in non-aqueous solvents we previously reported enthalpies of solution of alkali halides in formamide 1, N-methylformamide (NMF) and N-methylacetamide (NMA) 3. In this short communication we give a brief account of the measurements of the enthalpies of solution of LiCI, LiBr, LiI, NaI, KI, RbI and CsI in N,N-dimethylformamide (DMF).The adiabatic calorimeter and the experimental technique were described previously. DMF was taken from stock (Merck, Darmstadt; Uvasole fur die Spektroskopie). The small amount of water still present was removed by drying over KOH and distilling twice under reduced pressure. An upper limit for the water content of 0.02% was observed (Karl Fischer titration).In order to obtain the standard molar enthalpy of solution, AHosol, (at infinite dilution) the enthalpy of dilution, AHmdil, from molality m (the concentration of the solution reached on dissolving the salt) to m = 0 must be known. Measurements 4 9 5 of the conductivity of alkali halides in D M F indicate that there is no association of the ions at the low concentrations used (< 10-2 molal). Consequently it is allowable to use the Debye-Huckel theory for calculating AHmdil-values. The result of this calculation was :A H m d i l = -6350 m'" (1 -2.04 m'k) J . mole-', using the physical constants reported in the literature 6-9, G. Somsen and J. Coops, Rec. Trav. Chim. 84, 985 (1965). L. Weeda and G. Somsen, ibid. 85, 159 (1966).

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Enthalpies of solution of some alkali halides in N‐methylformamide at 25°

Cited by 12 publications

References 26 publications

Solubility of Sodium Halides in Aqueous Mixtures with ε-Increasing Cosolvents: Formamide, N-Methylformamide, and N-Methylacetamide at 298.15 K

Solubility of Sodium Halides in Aqueous Mixtures with ε-Increasing Cosolvents: Formamide, N-Methylformamide, and N-Methylacetamide at 298.15 K

Enthalpies of solvation of alkali metal and halide ions in N‐methylformamide and N‐methylacetamide at 25°

Enthalpies of solution of some alkali halides in N,N‐dimethylformamide at 25°C: (Short communication)

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