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  • 1
    Electronic Resource
    Electronic Resource
    Conductivity and ion pairing of hydrogen chloride inN-methylpropionamide at 25°C (1976)
    Springer
    Journal of solution chemistry 5 (1976), S. 765-771 
    Details
    ISSN: 1572-8927
    Keywords: Association constant ; conductivity ; hydrogen chloride ; ion association ; ionic conductivity ; N-methylpropionamide ; nonaqueous solvent
    Source: Springer Online Journal Archives 1860-2000
    Topics: Chemistry and Pharmacology
    Notes: Abstract The electrical conductivity of solutions of HCl inN-methylpropionamide (NMP) has been measured at 25°C for concentrations of HCl ranging from 0.0012 to 0.07 mole-liter−1. The results, combined with other data recently reported, were analyzed by means of the conductivity equation of Pitts. Some evidence for association was found in spite of the very large relative permittivity of the solvent medium (ε=176 at 25°C). The limiting molar conductivity for HCl is 10.949 S-cm2-mole−1. The limiting ionic conductivities in NMP are estimated to be 5.548 S-cm2-mole−1 for chloride ion and 5.401 S-cm2-mole−1 for hydrogen ion.
    Type of Medium: Electronic Resource
    URL: http://dx.doi.org/10.1007/BF00651486
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  • 2
    Electronic Resource
    Electronic Resource
    Excess Gibbs energy of mixing of the systems H2O-LiCl-Na2SO4 and H2O-CsCl-Na2SO4 at 25°C (1972)
    Springer
    Journal of solution chemistry 1 (1972), S. 71-75 
    Details
    ISSN: 1572-8927
    Keywords: Cesium chloride ; excess energy of mixing ; lithium chloride ; mixed solutions ; sodium sulfate
    Source: Springer Online Journal Archives 1860-2000
    Topics: Chemistry and Pharmacology
    Notes: Abstract The osmotic coefficients of aqueous solutions of lithium chloride+sodium sulfate and cesium chloride+sodium sulfate at 25°C have been measured. Interaction coefficients have been calculated and also the excess Gibbs energy of mixing. A correlation is found between the binary interaction coefficients and the Pauling cation radius of the alkali halide component.
    Type of Medium: Electronic Resource
    URL: http://dx.doi.org/10.1007/BF00648417
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  • 3
    Electronic Resource
    Electronic Resource
    Introduction to the Prue memorial issue (1974)
    Springer
    Journal of solution chemistry 3 (1974), S. 548-552 
    Details
    ISSN: 1572-8927
    Source: Springer Online Journal Archives 1860-2000
    Topics: Chemistry and Pharmacology
    Type of Medium: Electronic Resource
    URL: http://dx.doi.org/10.1007/BF00650399
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  • 4
    Electronic Resource
    Electronic Resource
    Osmotic coefficients and activity coefficients of lodic acid at high concentrations (1974)
    Springer
    Journal of solution chemistry 3 (1974), S. 593-602 
    Details
    ISSN: 1572-8927
    Keywords: Activity coefficients ; iodic acid ; ionic equilibria ; isopiestic measurements ; osmotic coefficients
    Source: Springer Online Journal Archives 1860-2000
    Topics: Chemistry and Pharmacology
    Notes: Abstract Isopiestic vapor pressure measurements have been used to determine the osmotic coefficients of aqueous solutions of iodic acid at molalities from 0.1 to 17 mole-kg−1 at 25°C. The isopiestic standards were solutions of sodium chloride and solutions of sulfuric acid. Because of the corrosive nature of iodic acid, platinum cups were used. Stoichiometric activity cofficients of iodic acid were derived by a Gibbs-Duhem integration. The activity coefficients for solutions of molality greater than 0.5 mole-kg−1 cannot be accounted for in terms of the two equilibria, namely, the acidic dissociation of iodic acid and formation of the ion H(IO3) 2 − , shown by Pethybridge and Prue to explain adequately the behavior in dilute solutions. The activity coefficient is unexpectedly small in concentrated solutions, suggesting the formation of neutral aggregates of iodic acid. The presence of dimers and tetramers, or alternatively trimers and tetramers, can explain the observed results up to a molality of 7 mole-kg−1.
    Type of Medium: Electronic Resource
    URL: http://dx.doi.org/10.1007/BF00650403
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  • 5
    Electronic Resource
    Electronic Resource
    Thermodynamics of aqueous mixtures of sodium chloride, potassium chloride, sodium sulfate, and potassium sulfate at 25°C (1972)
    Springer
    Journal of solution chemistry 1 (1972), S. 167-172 
    Details
    ISSN: 1572-8927
    Keywords: Excess free energy of mixing ; mixed salt solutions ; osmotic coefficients ; KCl ; K2SO4 ; NaCl ; Na2SO4
    Source: Springer Online Journal Archives 1860-2000
    Topics: Chemistry and Pharmacology
    Notes: Abstract Aqueous solutions of sodium chloride, potassium chloride, sodium sulfate, and potassium sulfate can be mixed in six ways to give ternary mixtures. Two of these have already been studied and results are now presented for the remaining four systems: H2O−NaCl−K2SO4, H2O−Na2SO4−K2SO4, H2O−KCl−Na2SO4, and H2O−KCl−K2SO4.
    Type of Medium: Electronic Resource
    URL: http://dx.doi.org/10.1007/BF01028452
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  • 6
    Electronic Resource
    Electronic Resource
    Dissociation constant of acetic acid in N-methylpropionamide from 5 to 55°C and related thermodynamic quantities (1972)
    Springer
    Journal of solution chemistry 1 (1972), S. 507-516 
    Details
    ISSN: 1572-8927
    Keywords: Acetic acid ; dissociation constant ; N methylpropionamide ; nonaqueous solvents ; solute-solvent interactions ; weak acids
    Source: Springer Online Journal Archives 1860-2000
    Topics: Chemistry and Pharmacology
    Notes: Abstract The dissociation constant of acetic acid in N-methylpropionamide (NMP) has been determined at 11 temperatures from 5 to 55°C by measurement of the electromotive force of cells without liquid junction containing hydrogen gas electrodes and silver-silver chloride electrodes. The pK at 25°C was found to be 7.995 (molal scale) as compared with 4.756 in water; thus, acetic acid is much weaker in NMP than in water despite the higher dielectric constant of the nonaqueous solvent (176 as compared with 78.3 at 25°C). The standard changes of enthalpy and entropy for the dissociation of acetic acid were calculated from the temperature coefficient of pK, and thermodynamic functions for the transfer dissociation process were obtained. The weakness of acetic acid in NMP is discussed in terms of electrostatic effects and solute-solvent interactions.
    Type of Medium: Electronic Resource
    URL: http://dx.doi.org/10.1007/BF00651727
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  • 7
    Electronic Resource
    Electronic Resource
    Dissociation constant of protonated tris(hydroxymethyl)aminomethane in N-methylpropionamide and related thermodynamic quantities from 10 to 55°C (1973)
    Springer
    Journal of solution chemistry 2 (1973), S. 405-415 
    Details
    ISSN: 1572-8927
    Keywords: Acidic dissociation ; dissociation constant ; emf measurements ; ionization processes ; N-methylpropionamide ; solvation ; tris-(hydroxymethyl)aminomethane
    Source: Springer Online Journal Archives 1860-2000
    Topics: Chemistry and Pharmacology
    Notes: Abstract The dissociation constant of protonated tris(hydroxymethyl)aminomethane (tris·H+) in the solvent N-methylpropionamide (NMP) has been determined at intervals of 5°C from 10 to 55°C by measurement of the emf of cells without liquid junction using hydrogen and silver-silver chloride electrodes. At 25°C, pK a was found to be 8.831, as compared with 8.075 in water. The standard changes in Gibbs energy, enthalpy, and entropy for the dissociation process have been evaluated from the dissociation constant and its change with temperature. By comparison with similar data for the dissociation of tris·H+ in water, thermodynamic functions for the transfer from water to NMP have been derived. The dissociation process is isoelectric, and the solvent dielectric constant is high (ε=176 at 25°C). Consequently, electrostatic charging effects are expected to be minimal, and the change in dissociation constant depends primarily on solute-solvent interactions. The results, combined with transfer energies for HCl, tris, and tris·HCl from emf and solubility measurements, demonstrate that the decreased acidic strength of tri·H+ in NMP is attributable in large part to the fact that NMP is less effective than water in stabilizing tris and its salts.
    Type of Medium: Electronic Resource
    URL: http://dx.doi.org/10.1007/BF00713253
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  • 8
    Electronic Resource
    Electronic Resource
    Solvation equilibria in very concentrated electrolyte solutions (1973)
    Springer
    Journal of solution chemistry 2 (1973), S. 173-191 
    Details
    ISSN: 1572-8927
    Keywords: Calcium bromide ; calcium chloride ; hydration of ions ; hydrochloric acid ; lithium bromide ; lithium chloride ; osmotic coefficient ; perchloric acid ; potassium hydroxide ; sodium chloride ; sodium hydroxide ; solvation of ions
    Source: Springer Online Journal Archives 1860-2000
    Topics: Chemistry and Pharmacology
    Notes: Abstract A stepwise hydration-equilibrium model for aqueous electrolytes is developed and shown to give a good quantitative account of osmotic coefficients of strong, highly soluble electrolytes up to concentrations of 20–30 m. The main parameters needed are two equilibrium constants describing the stepwise hydration and the number of hydration sites. Choice of ion-size parameter has only a minor effect.
    Type of Medium: Electronic Resource
    URL: http://dx.doi.org/10.1007/BF00651972
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  • 9
    Electronic Resource
    Electronic Resource
    Free energy relationships in aqueous amino acid and peptide solutions containing sodium chloride (1974)
    Springer
    Journal of solution chemistry 3 (1974), S. 493-501 
    Details
    ISSN: 1572-8927
    Keywords: Amino acids ; peptides ; diglycine ; triglycine ; isopiestic method ; ion-dipole interactions ; NaCl
    Source: Springer Online Journal Archives 1860-2000
    Topics: Chemistry and Pharmacology
    Notes: Abstract Three systems of the type amino acid or peptide-sodium chloride-water have been investigated over wide solute molality ranges using the isopiestic vapor pressure method. The amino acid employed was L-α-alanine, while the peptides were diglycine and triglycine. Equations were obtained for the activity coefficients of these compounds in the salt solutions in terms of the molalities of the solutes. The trace activity coefficients of the peptides were negative at low salt molality and became positive as the salt molality was increased. The limiting interaction parameters were calculated for the systems using the Kirkwood ion-dipole expression and empirical quantities derived from previous work to obtain the salt effect on the nonpolar and amide portion of the molecule. Good agreement was obtained between the calculated values and the experimental results in the case of diglycine, but they diverged in the case of triglycine. The calculated value for L-α-alanine is in poorer agreement with the experimental value than for the other amino acids studied previously.
    Type of Medium: Electronic Resource
    URL: http://dx.doi.org/10.1007/BF00648134
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  • 10
    Electronic Resource
    Electronic Resource
    Activity coefficient of hydrochloric acid in aqueous solutions of sodium chloride (1977)
    Springer
    Journal of solution chemistry 6 (1977), S. 385-392 
    Details
    ISSN: 1572-8927
    Keywords: Activity coefficient ; electrolytes ; mixed ; Harned coefficients ; hydrochloric acid ; mixed electrolyte solutions ; sodium chloride
    Source: Springer Online Journal Archives 1860-2000
    Topics: Chemistry and Pharmacology
    Notes: Abstract Electromotive-force measurements of the cell $$Pt;H_2 \left( {g,1{\text{ }}atm} \right)|HCl\left( {{\text{m}}_A } \right),NaCl\left( {{\text{m}}_B } \right)|AgCl;Ag$$ have been made at temperatures between 5 and 45°C at values ofm A+m B of 0.1, 0.3809, 0.6729, and 0.8720 mole-kg−1. The activity coefficients of HCl in HCl/NaCl mixtures and the Harned coefficients α12 have been obtained. The change of α12 with total molality is consistent with the existence of binary interactions between H+ and Na+ ions. The linear variation of the relative partial molal heat content with the fraction of NaCl in the mixture suggests that an analog of the Harned rule exists for this thermodynamic quantity.
    Type of Medium: Electronic Resource
    URL: http://dx.doi.org/10.1007/BF00645511
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