Heats of solution of 1∶1 electrolytes in 1-propanol,and derived enthalpies of transfer from water

Heats of solution of 13 11 electrolytes in 1-propanol have been determined calorimetrically at various electrolyte concentrations, and extrapolated to zero concentration to give H _s ^o values for these electrolytes. Together with literature data on three additional 11 electrolytes, these measurements yield a self-consistent set of single-ion enthalpies of transfer from water to 1-propanol. Values are tabulated for 10 univalent cations and five univalent anions. It is shown that the H _t ^o (Ph ₄ As⁺)=H _t ^o (Ph ₄ B^–) assumption yields chemically reasonable single-ion values. Using this assumption, it may be deduced that all the univalent ions studied have about the same enthalpy in 1-propanol as in methanol.     

Ionic enthalpies of transfer from water to water-sulfolane mixtures

NaCl, NaBr, NaI, NaClO₄, KCl, KClO₄, NaBPh₄, and Ph₄PBr solution enthalpies were measured in water-sulfolane mixtures at 30°C. Ionic enthalpies of transfer from water to mixed solvents were calculated on the basis of the assumption H _s ^o (BPh ₄ ^– )=H _s ^o (Ph₄P⁺). The variation of the ionic enthalpies of transfer with solvent composition is discussed in terms of ion-solvent interactions and of the effects caused by sulfolane on the structure of water.     

Standard molar enthalpies of solvation of aliphatic esters in 1,2-dichloroethane andn-hexane

The molar enthalpies of solution at infinite dilution of methyl-, ethyl-, n-butyl-and n-pentylacetate, and ethylpropionate, ethylbutanoate and ethylhexanoate were obtained by means of calorimetric determinations in 1,2-dichloroethane and n-hexane. From these values and the standard molar enthalpy of vaporization, the standard molar enthalpy of solvation of these esters in both solvents were calculated. These calculated values are shown to correlate with the number of methylene groups in the esters.     

Solvation of bivalent transition metal cations. I. Heats of transfer of the metal perchlorates between water,acetonitrile, and dimethylsulfoxide

Heats of solution of Mn(ClO₄)₂·6AN, Fe(ClO₄)₂·6AN, Co(ClO₄)₂·6AN, as well as Ni(ClO₄)₂·6AN, Cu(ClO₄)₂·4AN, and Zn(ClO₄)₂·6AN (AN=acetonitrile) have been determined in water, acetonitrile, and dimethylsulfoxide (DMSO). Coupled with the heats of solution of AN in the respective solvents they give the heats of transfer of the metal perchlorates. Heats of transfer of the cations as well as their heats of solvation are calculated using literature data for the heat of transfer of the perchlorate anion and the heats of hydration of the cations, respectively. The results are discussed in terms of the different contributions to the overall heat effects.     

Thermodynamics of transfer of hydrochloric acid from water to aqueous glucose at 25°C

Enthalpies of transfer of HCl from water to aqueous glucose were determined calorimetrically at 25°C at several mixed solvent compositions ranging up to glucose mole fraction X₃=0.0624 (40 wt. %). These were combined with free energies of transfer calculated from emf measurements to yield entropies of transfer, and all properties are compared with those observed for HCl and NaCl transfer to other aqueous nonelectrolyte mixed solvents.     

Thermodynamics of transfer of sodium chloride from water to aqueous sucrose at 25°C

Enthalpies of transfer of sodium chloride over the mixed-solvent range from pure water to mole fraction sucroseX ₃=0.05 (50 wt. %) were determined calorimetrically at 25°C. These were combined with free energies of transfer at constant molality (per 100 g of mixed solvent) calculated from isopiestic activity coefficients to yield negative entropies of transfer. The positive free energy is approximately a linear function ofX ₃, and the negative enthalpies show that the free energies and activity coefficients of NaCl increase with temperature. The enthalpy behavior of NaCl in aqueous hydrogen peroxide and the urea is very similar to that in the present study, indicating the possibility of rough colligative effect for such systems.     

Reaction of 1-alkynylsilanes with triallylborane—competition between 1,1- and 1,2-allylboration

The reaction of triallylborane (All₃B, 1) with various 1-alkynylsilanes of the type Me₃Si–CCR¹ [R¹=H (2a), Me (2b), Ph (2c), CC–SiMe₃ (2d), SiMe₃ (2e)], Ph₃Si–CCPh (3) MeCC–SiMe₂SiMe₂–CCMe (4) and Me₂Si(Cl)–CCPh (5) was studied. Triallylborane 1 turned out to be much more reactive than other triorganoboranes R₃B (e.g. R=Et, Ph). In the cases of 2 and 5, the products are organometallic-substituted alkenes 6 and 11, respectively, with the boryl and silyl group in cis-positions as the result of selective 1,1-allylboration (via cleavage of the Si–C bond) or mixtures of such and other alkenes 7 or 8 because of competition between 1,1- and 1,2-allylboration (the composition of these mixtures depends on the polarity of the solvent). In the case of 4, the 1,2-dihydro-1,2-disilaborepine derivative 12 is formed selectively (twofold 1,1-allylboration). The alkyne 3 did not react with 1. The products were characterised by ¹H-, ¹¹B-, ¹³C- and ²⁹Si-NMR spectroscopy.     

Formation and Ring Contraction of Benzo[f][1,2]Thiazepine-1,1-Dioxides from and to Benzo[e][1,2]Thiazine-1,1-Dioxides

Alkoxide-promoted ring expansion of the novel ethyl 2-(6,7-dimethoxy-3-oxo-3,4-dihydrobenzo[e][1,2]thiazine-1,1-dioxide-2-yl)acetate 3a and analogous 4,4-diethyl derivative 3b and cyclization of methyl 2-[2-(phenylaminocarbonylmethyl sulfamoyl)-4,5-dimethoxyphenyl] acetate 9 to the corresponding new 3-carboxylates and 3-carboxanilide of 7,8-dimethoxy-4-hydroxy-2,5-dihydrobenzo[f][1,2]thiazepine-1,1-dioxide (5a,b and 10 respectively) is described. Compound 5a was deacylated upon treatment with sodium hydroxide followed by hydrochloric acid to give 7,8-dimethoxy-2,3-dihydrobenzo[f][1,2]thiazepine-1,1-dioxide-4 (5H)-one 8 and its N-ethyl derivative transferred to 6,7-dimethoxy-2-ethyl-3-oxo-3,4-dihydrobenzo[e][1,2]thiazine-1,1-dioxide 7 by the reaction with ethyl methyl ketone in the presence of pyrrolidine.     

Solvation of bivalent transition metalcations. II. Heats of transfer of metal perchlorates between water and several amides

Heats of solution of acetonitrile, solvated or hydrated perchlorates, Mn(ClO₄)₂·6AN, Co(ClO₄)₂·6AN, Ni(ClO₄)₂·6AN, Cu(ClO₄)₂·4AN, Cu(ClO₄)₂·6H₂O, Zn(ClO₄)₂·6AN, and Zn(ClO₄)₂·6H₂O have been determined in NMF, DMF, DMA, and water. Complete or almost complete exchange of AN and water molecules in amides is inferred from the visible spectra determinations. The heats of transfer of perchlorate anion from water to DMA and NMF have been obtained from separately determined heats of solution of NaBPh₄, AsPH₄Cl·H₂O, NaClO₄, NaCl, and SiPh₄ in the respective solvents. The heats of transfer of cations from water to amides have been determined from the above data and the heats of solvation of cations using literature data for the heats of hydration.     

Evaluation of Gibbs free energy for the transfer of a highly hydrophilic ion from an acidic aqueous solution to an organic solution based on ion pair extraction

A method to determine the standard Gibbs free energy for the transfer, ΔG°_tr, of a highly hydrophilic metal ion from an aqueous solution, W, in the presence of high concentration of H⁺ to an organic solution, O, was proposed based on the theoretical consideration of the distribution process of ions between W and O. The usefulness of the proposed method was verified experimentally by comparing ΔG°_tr of Mg²⁺ determined by the method with that obtained by voltammetry for the ion transfer at the W|O interface. The O examined were nitrobenzene (NB) and 1,2-dichloroethane (DCE). By applying the proposed method, ΔG°_tr of NpO₂⁺, UO₂²⁺, NpO₂²⁺ and PuO₂²⁺ from an acidic W to NB were determined.     

Partial molar enthalpies of solution as indicators of interactions in mixtures of 2-butoxyethanol and 2-butanol with water

Calorimetric measurements have been made of differential enthalpies of solution of both components in the binary system 2-butoxyethanol-water and of 2-butanol in the system 2-butanol-water as a function of composition at three different temperatures. The heat capacity changes for dissolution were calculated from the temperature variation of the solution enthalpies. Drastic changes of the solution properties are seen with increasing solute concentration in water-rich solutions. In the 2-butoxyethanol-water system, which could be studied over the whole composition range, four different regions can be identified. At extreme dilution in water, the solute is fully hydrated with a primary hydration layer of monolayer thickness involved in long-range secondary hydration. In dilute solutions the primary hydration layer is unchanged but the secondary hydration diminishes with increasing solute concentration. In semi-dilute solution the primary hydration layer breaks down and the particular hydrophobic characteristics of hydrocarbon groups in aqueous solution disappear. At higher solute content the mixtures show no hydrophobic character but the behavior of regular mixtures of polar solutes.     

Synthesis and study of new 2-aryl-1-(4-nitrophenyl)-1,1a-dihydroazireno[1,2-a]quinoxaline derivatives

New derivatives of photochromic 2-aryl-1-(4-nitrophenyl)-1,1a-dihydroazireno[1,2-a]quinoxalines were synthesized by condensation of 4-methyl-and 4,5-dimethyl-1,2-phenylenediamine with 1,3-diaryl-2,3-dibromopropan-1-ones. The reactions of 4-methyl-1,2-phenylenediamine produce mixtures of regioisomers. The chemical properties of the reaction products were studied. The structure of one of the latter was established by X-ray diffraction. Published in Russian in Izvestiya Akademii Nauk. Seriya Khimicheskaya, No. 2, pp. 350–356, February, 2006.     

Enthalpies of transfer of amino acids and sodium chloride from water to aqueous fructose at 25°C

Enthalpies of transfer H ₂ of three amino acids glycine, L-alanine, and L-phenylalanine, and of NaCl, from water to aqueous fructose at low fructose mole fraction were determined at 25°C. Comparison with H ₂ for glycine in the presence and absence of KCl shows that the effect of additional ion-dipole interactions is apparent only in more concentrated fructose solutions. Limiting slopes indicate that glycine resembles NaCl more than it does the other two amino acids. The effect on H ₂ of the polarity of the zwitterion is offset and dominated by the growing non-polar side chain. Values of H ₂ for glycine, L-phenylalanine, and NaCl from water to aqueous urea are compared with the results of the present study. A rough colligative effect similiar to that observed for NaCl in a variety of polar mixed aqueous solvents may also be possible for glycine, since the change of the enthalpies of transfer with mole fraction for glycine are the same for transfer to both aqueous urea and fructose.     

First observation of Chapman rearrangement of a pseudosaccharyl ether in the solid state: the thermal isomerization of 3-(methoxy)-1,2-benzisothiazole 1,1-dioxide revisited

3-(Methoxy)-1,2-benzisothiazole 1,1-dioxide, a pseudosaccharyl ether, was long ago known to undergo a thermal Chapman-like [1,3′]-isomerization to the corresponding N-methyl pseudosaccharin at temperatures above its melting point (ca. 184 °C) [Hettler H., Tetrahedron Lett.1968, 15, 1793]. In the present study, it is shown that this rearrangement can also take place in the solid state, at temperatures as low as 150 °C. This was the first observation of a Chapman-like [1,3′]-isomerization in pseudosaccharyl ethers in the solid state. The study has been carried out by a multidisciplinary approach using temperature dependent infrared spectroscopy, differential scanning calorimetry (DSC), and polarized light thermomicroscopy, complemented by theoretical methods.     

Reaction of 1,1-disubstituted hydrazines with bromine in the presence of aryl- and heteroarylnitroso compounds in acid media: A general method for the synthesis of 1-aryl(heteroaryl)-3,3-disubstituted triazene 1-oxides

We have worked out a method for the synthesis of 1,3,3-trisubstituted triazene 1-oxides based upon reaction of 1,1-disubstituted hydrazines with bromine in the presence of aryl- and heteroarylnitroso compounds in acid media. Obtained are a broad range of triazene 1-oxides, among which hitherto unknown compounds of the series of pyrazole and 3,3-dialkyltriazene 1-oxides that contain functional groups at the alkyl part of the molecule. We propose a reaction scheme which includes in situ formation of diazenium cations and reaction of them with nitroso compounds that are present in the system. By means of PMR,¹³C, and¹⁴N NMR spectroscopy, and mass spectroscopy, it has been shown that in all the prepared compounds the oxidated nitrogen atom is at the N¹ position of the triazene N-oxide group.N. D. Zelinskii Institute of Organic Chemistry, Russian Academy of Sciences, 117913 Moscow. Translated from Izvestiya Akademii Nauk, Seriya Khimicheskaya, No. 8, pp. 1804–1820, August, 1992.     

Excess enthalpies of solution of some primary and secondary alcohols in sodium dodecylsulfate micellar solutions

The exces enthalpies of solution of some primary and secondary alcohols in aqueous sodium dodecylsulfate micellar solutions were measured and the results were explained by considering the distribution of alcohols between aqueous and micellar phases. The distribution constant and the enthalpy of transfer (and the standard free energy and entropy of transfer) were obtained. The thermodynamic parameters for the transfer of secondary alcohols from the aqueous to the sodium dodecylsulfate (NaDS) micellar phase differ slightly from those of the corresponding primary alcohols. For both series of alcohols the additivity rule holds for free energies of transfer whereas enthalpies and entropies display convex curves. The present data are compared to those for the transfer of the same solutes from the aqueous to the dodecyldimethylamine oxide (DDAO) and dodecyltrimethylammonium bromide (DTAB) micellar phases. The role of the hydrophilic interactions between the OH group and the micelles' head groups is formulated. The thermodynamics of the branched methyl group were determined. Furthermore, the thermodynamics of solvation of primary alcohols in water, in NaDS micelles, and in octane have been calculated using reference states based on the assumption that the empty space around alcohols in the initial and final states is the same. It is shown that the solvation of alcohols in NaDS micellar phase is enthalpy driven and that the thermodynamic properties of solvation vs. the length of the alcohol tail is the same for water and NaDS micelles whereas it is different for octane. A possible explanation for this difference is that the alkyl chain of alcohols folds in octane.     

Excess enthalpies of solution of primary and secondary alcohols in dodecyldimethylamine oxide micellar solutions

The excess enthalpies of solution with respect to water of some primary and secondary alcohols in dodecyldimethylamine oxide (DDAO) micellar solutions were measured by mixing aqueous solutions of alcohols with surfactant solutions. Standard free energies, enthalpies and entropies were obtained from the distribution of alcohols between aqueous and micellar phases. It is shown that thermodynamics of transfer of secondary alcohols from aqueous to the DDAO micellar phase differ slightly from those of their corresponding primary alcohols, that the additivity rule holds for free energies of transfer and that enthalpy and entropy display convex curves. The present data are compared with those from the aqueous to the dodecyltrimethylammonium bromide (DTAB) micellar phases and to the literature data for transfer from water to octane. The role of the hydrophilic interactions between OH group and the micellar head groups and of the hydrophobic interactions between the methylene group and its apolar environment is evidenced.     

Gibbs functions for transfer of divalent metal cations from water to water + methanol mixtures using potentiometry, polarography and solubility measurements

Gibbs functions for transfer from water to methanol and to a full range of water + methanol mixtures were obtained for Cu²⁺, Cd²⁺, Pb²⁺, Hg²⁺, Zn²⁺, Mg²⁺, Ca²⁺, Sr²⁺ and Ba²⁺ using potentiometric or polarographic measurements in these solvents. In addition, data were obtained from the solubility products of the alkaline-earth iodates. From values obtained by the different methods and literature data, a table of selected values is given.     

Stabilities in water and transfer activity coefficients from water to nonaqueous solvents of 15-crown-5 and 16-crown-5-metal ion complexes

Stability constants of 1 : 1 16-crown-5 (16C5)-metal ion complexes were determined in water at 25°C by conductometry and potentiometry with ion-selective electrodes. The selectivity sequences of 16C5 in water for univalent and bivalent metal ions are Ag⁺ > Na⁺ Tl⁺ > K⁺ and Sr²⁺ > Ba²⁺ Pb²⁺, respectively. The stability of a given 16C5-metal ion complex in water is much lower than might be expected on the basis of the solvation power (i.e. relative solubility of the metal ion) of water for the metal ion. The same tendency is observed for the cases of 15-crown-5 (15C5) -metal ion complexes. Transfer activity coefficients () of 15C5 and 16C5 for tetradecane (TD)/water, TD/methanol, TD/acetonitrile, and propylene carbonate/water systems were determined at 25°C. From these data, contributions of a methylene group and an ether oxygen atom to the log value of a crown ether were then obtained. The values from water to acetonitrile, propylene carbonate, and methanol of 15C5- and 16C5-univalent metal ion complexes were calculated, s, M⁺, and L being a solvent, a univalent metal ion, and a crown ether, respectively. The log value is greater than the corresponding log value. The log values are negative. This indicates that, although the M^- ions are more soluble in water than in the nonaqueous solvents, when the crown ether forms a complex with the M⁺ ion, the complex becomes more soluble in the nonaqueous solvents than in water, compared with the free crown ether. It was concluded from this finding that the unexpectedly low stability of the crown ether-M⁺ complex in water is attributed to strong hydrogen bonding between ether oxygen atoms of the free crown ether and water.