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  • Articles: DFG German National Licenses  (100)
  • Cell & Developmental Biology  (89)
  • thermodynamics  (11)
  • 1
    Electronic Resource
    Electronic Resource
    The dissociation quotients of formic acid in sodium chloride solutions to 200°C (1993)
    Springer
    Journal of solution chemistry 22 (1993), S. 125-136 
    Details
    ISSN: 1572-8927
    Keywords: Formic acid ; methanoic acid ; dissociation constant ; thermodynamics ; potentiometry ; ionic strength
    Source: Springer Online Journal Archives 1860-2000
    Topics: Chemistry and Pharmacology
    Notes: Abstract The dissociation quotients of formic acid were measured potentiometrically from 25 to 200°C in NaCl solutions at ionic strengths of 0.1, 0.3 1.0, 3.0, and 5.0 mol-kg−1. The experiments were carried out in a concentration cell with hydrogen electrodes. The resulting molal acid dissociation quotients for formic acid, as well as a set of infinite dilution literature values and a calorimetrically-determined enthalpy of reaction, were fitted by an empirical equation involving an extended Debye Hückel term and seven adjustable parameters involving functions of temperature and ionic strength. This regressional analysis yielded the following thermodynamic quantities for 25°C: logK=−3.755±0.002, ΔHo=−0.09±0.15 kJ-mol−1, ΔSo=−72.2±0.5 J-K−1-mol−1, and ΔC p o =−147±4 J-K−1-mol−1. The isocoulombic form of the equilibrium constant is recommended for extrapolation to higher temperatures.
    Type of Medium: Electronic Resource
    URL: http://dx.doi.org/10.1007/BF00650679
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  • 2
    Electronic Resource
    Electronic Resource
    Complexation of aluminate anion by bis-tris in aqueous media at 25–50°C (1990)
    Springer
    Journal of solution chemistry 19 (1990), S. 159-173 
    Details
    ISSN: 1572-8927
    Keywords: Aluminum ; Bis-tris ; dextrose ; solubility ; Raman ; complex ; thermodynamics ; aqueous
    Source: Springer Online Journal Archives 1860-2000
    Topics: Chemistry and Pharmacology
    Notes: Abstract Gibbsite, Al(OH)3, solubility studies in aqueous NaCl solutions at pH 9 demonstrate that the aluminate anion forms a strong complex with the neutral Bis-tris molecule 2,2-Bis(hydroxymethyl)-2,2′,2″-nitrilotriethanol, at low temperatures. The logarithm of the molal concentration quotient for the reaction $$Al(OH)_4^ - + H_2 [Bis - tris] _ \leftarrow ^ \to Al(OH)_2 [Bis - tris]^ - + 2H_2 O$$ in aqueous NaCl solutions at 0.1 molal ionic strength is 2.63±0.03 at 25°C and 2.6±0.1 at 50°C. Raman spectroscopy of NaOH−NaAl(OH)4 solutions at 25°C quantitatively verifies these results and indicates that a complex with symmetrical vibrational frequencies at 498 and 574 cm−1 is stabilized in the presence of excess Bis-tris in these solutions. Gibbsite solubility and Raman spectroscopy also indicate that a similar complexation reaction between the aluminate anion and dextrose occurs, with a molal equilibrium quotient of 100.65 at 25°C, 0.1 molal ionic strength. These complexation reactions are suggested to be equivalent to the wellknown reactions involving the borate anion and polyhydroxyl sugar-like molecules. Experiments with ethylene glycol, glycerol, mannitol and sucrose indicate no significant complexing of these compounds with the aluminate anion.
    Type of Medium: Electronic Resource
    URL: http://dx.doi.org/10.1007/BF00646610
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  • 3
    Electronic Resource
    Electronic Resource
    Dissociation quotients of succinic acid in aqueous sodium chloride media to 225°C (1995)
    Springer
    Journal of solution chemistry 24 (1995), S. 65-87 
    Details
    ISSN: 1572-8927
    Keywords: Succinic acid ; butanedioic acid ; dissociation constants ; thermodynamics ; potentiometry ; ionic strength
    Source: Springer Online Journal Archives 1860-2000
    Topics: Chemistry and Pharmacology
    Notes: Abstract The first and second molal dissociation quotients of succinic acid were measured potentiometrically with a hydrogen-electrode, concentration cell. These measurements were carried out from 0 to 225°C over 25° intervals at five ionic strengths ranging from 0.1 to 5.0 molal (NaCl). The dissociation quotients from this and two other studies were combined and treated with empirical equations to yield the following thermodynamic quantities for the first acid dissociation equilibrium at 25°C: log K1a=−4.210±0.003; ΔH 1a 0 =2.9±0.2 kJ-mol−1; ΔS 1a 0 =−71±1 J-mol−1-K−1; and ΔC p1a 0 =−98±3 J-mol−1-K−1; and for the second acid dissociation equilibrium at 25°C: log K2a=−5.638±0.001; ΔH 2a 0 = −0.5±0.1 kJ-mol−1; ΔS 2a 0 =−109.7±0.4 J-mol−1-K−1; and ΔC p2a 0 = −215±8 J-mol−1-K−1.
    Type of Medium: Electronic Resource
    URL: http://dx.doi.org/10.1007/BF00973050
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  • 4
    Electronic Resource
    Electronic Resource
    Dissociation quotients for citric acid in aqueous sodium chloride media to 150°C (1997)
    Springer
    Journal of solution chemistry 26 (1997), S. 63-84 
    Details
    ISSN: 1572-8927
    Keywords: Citric acid ; dissociation constants ; thermodynamics ; potentiometry ; ionic strength
    Source: Springer Online Journal Archives 1860-2000
    Topics: Chemistry and Pharmacology
    Notes: Abstract The three molal dissociation quotients for citric acid were measured potentiometrically with a hydrogen-electrode concentration cell from 5 to 150°C in NaCl solutions at ionic strengths of 0.1, 0.3, 0.6, and 1 molal. The molal dissociation quotients and available literature data at infinite dilution were fitted by empirical equations in the all-anionic form involving an extended Debye-Hückel term and up to five adjustable parameters involving functions of temperature and ionic strength. This treatment yielded the following thermodynamic quantitites for the first dissociation equilibrium at 25°C: logK 1a=−3.127±0.002, ΔH 1a o =4.1±0.2 kJ-mol−1, ΔS 1a o =−46.3±0.7 J-K−1-mol−1, and ΔCp 1a o =−162±7 J-K−1-mol−1; for the second acid dissociation equilibrium at 25°C: logK 2a =−4.759±0.001, ΔH 2a o =2.2±0.1, ΔS 2a o =−83.8±0.4, and ΔCp 2a o =−192±15, and for the third dissociation equilibrium at 25°C: logK 3a=−6.397±0.002, ΔH 3a o =−3.6±0.2, ΔS 3a o =−134.5±0.7, and ΔCp 3a o =−231±7.
    Type of Medium: Electronic Resource
    URL: http://dx.doi.org/10.1007/BF02439444
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  • 5
    Electronic Resource
    Electronic Resource
    Dissociation quotients of malonic acid in aqueous sodium chloride media to 100°C (1992)
    Springer
    Journal of solution chemistry 21 (1992), S. 883-900 
    Details
    ISSN: 1572-8927
    Keywords: Malonic acid ; propanedioic acid ; dissociation constants ; thermodynamics ; potentiometry ; ionic strength
    Source: Springer Online Journal Archives 1860-2000
    Topics: Chemistry and Pharmacology
    Notes: Abstract The first and second molal dissociation quotients of malonic acid were measured potentiometrically in a concentration cell fitted with hydrogen electrodes. The hydrogen ion molality of malonic acid/bimalonate solutions was measured relative to a standard aqueous HCl solution from 0 to 100°C over 25° intervals at five ionic strengths ranging from 0.1 to 5.0 molal (NaCl). The molal dissociation quotients and available literature data were treated in the all anionic form by a seven-term equation. This treatment yielded the following thermodynamic quantities for the first acid dissociation equilibrium at 25°C: logK 1a =-2.852±0.003, ΔH 1a /o =0.1±0.3 kJ-mol−1, ΔS 1a o =−54.4±1.0 J-mol−1-K−1, and ΔC p,1a o =−185±20 J-mol−1-K−1. Measurements of the bimalonate/malonate system were made over the same intervals of temperature and ionic strength. A similar regression of the present and previously published equilibrium quotients using a seven-term equation yielded the following values for the second acid dissociation equilibrium at 25°C: logK2a=−5.697±0.001, ΔH 2a o =−5.13±0.11 kJ-mol−1, ΔS 2a o =−126.3±0.4 J-mol−1-K−1, and ΔC p,2a o =−250+10 J-mol−1-K−1.
    Type of Medium: Electronic Resource
    URL: http://dx.doi.org/10.1007/BF00651513
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  • 6
    Electronic Resource
    Electronic Resource
    Acid association quotients of bis-tris in aqueous sodium chloride media to 125°C (1989)
    Springer
    Journal of solution chemistry 18 (1989), S. 545-559 
    Details
    ISSN: 1572-8927
    Keywords: 2,2-Bis(hydroxymethyl)-2,2′,2″-nitrilotriethanol ; equilibrium constant ; thermodynamics ; buffer ; association ; salt effect ; temperature dependence
    Source: Springer Online Journal Archives 1860-2000
    Topics: Chemistry and Pharmacology
    Notes: Abstract The ionic strength and temperature dependencies of the molal acid association quotients of 2,2-Bis(hydroxymethyl)-2,2′,2″-nitrilotriethanol (also abbreviated as bis-tris) were determined potentiometrically in a concentration cell fitted with hydrogen electrodes. The emf was recorded for equimolal bis-tris/bis- trisHCl buffer solutions from 5 to 125°C at approximately 25°C intervals, and at nine ionic strengths from 0.05 to 5.0m (NaCl). The molal association quotients, combined with infinite dilution values from the literature, are described precisely by a seven parameter equation which yielded the following thermodynamic quantities at infinite dilution and 25°C: logK=6.481±0.003, ΔH o =−28.5±0.2 kJ-mol −1 , ΔS o =28.5±0.8 J-K −1 -mol −1 , and ΔC P o =−22±5 J-K −1 -mol −1 . The equation incorporates a simple three term expression for logK, but requires four terms to describe the rather complex ionic strength dependence despite the reaction being isocoulombic. The molal association quotients from this study and the literature were also subjected to the Pitzer ion interaction treatment.
    Type of Medium: Electronic Resource
    URL: http://dx.doi.org/10.1007/BF00664236
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  • 7
    Electronic Resource
    Electronic Resource
    Dissociation quotients of oxalic acid in aqueous sodium chloride media to 175°C (1991)
    Springer
    Journal of solution chemistry 20 (1991), S. 905-927 
    Details
    ISSN: 1572-8927
    Keywords: Oxalic acid ; ethanedioic acid ; dissociation constants ; thermodynamics ; potentiometry ; ionic strength
    Source: Springer Online Journal Archives 1860-2000
    Topics: Chemistry and Pharmacology
    Notes: Abstract The first and second molal dissociation quotients of oxalic acid were measured potentiometrically in a concentration cell fitted with hydrogen electrodes. The emf of oxalic acid-bioxalate solutions was measured relative to an HCl standard solution from 25 to 125°C over 25o intervals at nine ionic strengths ranging from 0.1 to 5.0 molal (NaCl). The molal dissociation quotients and available literature data were treated in the all anionic form by a five-term equation that yielded the following thermodynamic quantities at infinite dilution and 25°C: logK1a=−1.277±0.010, ΔH 1a o =−4.1±1.1 kJ-mol−1, ΔS 1a o =38±4 J-K−1-mol−1, and ΔC p,1a o =−168±41 J-K−1-mol−1. Similar measurements of the bioxalate-oxalate system were made at 25o intervals from 0 to 175°C at seven ionic strengths from 0.1 to 5.0m. A similar regression of the experimentally-derived and published equilibrium quotients using a seven-term equation yielded the following values at infinite dilution and 25°C: logK2a=−4.275±0.006, ΔH 2a o =−6.8±0.5 kJ-mol−1, ΔS 2a o =−105±2 J-K−1-mol−1, and ΔC p,2a o =−261±12 J-K−1-mol−1.
    Type of Medium: Electronic Resource
    URL: http://dx.doi.org/10.1007/BF01074952
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  • 8
    Electronic Resource
    Electronic Resource
    Dissociation quotient of benzoic acid in aqueous sodium chloride media to 250°C (1995)
    Springer
    Journal of solution chemistry 24 (1995), S. 385-407 
    Details
    ISSN: 1572-8927
    Keywords: Benzoic acid ; dissociation constant ; ionization constant ; potentiometry ; ionic strength ; temperature and pressure dependence ; thermodynamics
    Source: Springer Online Journal Archives 1860-2000
    Topics: Chemistry and Pharmacology
    Notes: Abstract The dissociation quotient of benzoic acid was determined potentiometrically in a concentration cell fitted with hydrogen electrodes. The hydrogen ion molality of benzoic acid/benzoate solutions was measured relative to a standard aqueous HCl solution at seven temperatures from 5 to 250°C and at seven ionic strengths ranging from 0.1 to 5.0 molal (NaCl). The molal dissociation quotients and selected literature data were fitted in the isocoulombic (all anionic) form by a six-term equation. This treatment yielded the following thermodynamic quantities for the acid dissociation equilibrium at 25°C and 1 bar: logKa=−4.206±0.006, ΔH a o =0.3±0.3 kJ-mol−1, ΔS a o =−79.6±1.0 J-mol−1-K−1, and ΔC p;a o =−207±5 J-mol−1-K−1. A five-term equation derived to describe the dependence of the dissociation constant on solvent density is accurate to 250°C and 200 MPa.
    Type of Medium: Electronic Resource
    URL: http://dx.doi.org/10.1007/BF01150876
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  • 9
    Electronic Resource
    Electronic Resource
    Dissociation Quotients for Citric Acid in Aqueous Sodium Chloride Media to 150°C (1997)
    Springer
    Journal of solution chemistry 26 (1997), S. 63-84 
    Details
    ISSN: 1572-8927
    Keywords: Citric acid ; dissociation constants ; thermodynamics ; potentiometry ; ionic strength
    Source: Springer Online Journal Archives 1860-2000
    Topics: Chemistry and Pharmacology
    Notes: Abstract The three molal dissociation quotients for citric acid were measured potentiometrically with a hydrogen-electrode concentration cell from 5 to 150°C in NaCl solutions at ionic strengths of 0.1, 0.3, 0.6, and 1 molal. The molal dissociation quotients and available literature data at infinite dilution were fitted by empirical equations in the all-anionic form involving an extended Debye-Hückel term and up to five adjustable parameters involving functions of temperature and ionic strength. This treatment yielded the following thermodynamic quantities for the first dissociation equilibrium at $$\begin{gathered} 25^ \circ {\text{C: log }}K_{1{\text{a}}} = - 3.127 \pm 0.002{\text{, }}\Delta H_{{\text{la}}}^{\text{o}} = \hfill \\ 4.1 \pm 0.{\text{2 kJ - mol}}^{{\text{ - 1}}} {\text{, }}\Delta S_{{\text{1a}}}^{\text{o}} = - 46.3 \pm 0.{\text{7 J - K}}^{{\text{ - 1}}} - {\text{mol}}^{{\text{ - 1}}} {\text{, and }}\Delta Cp_{{\text{1a}}}^{\text{o}} = - 162 \pm \hfill \\ {\text{7 J - K}}^{{\text{ - 1}}} - {\text{mol}}^{{\text{ - 1}}} ; \hfill \\ \end{gathered} $$ for the second acid dissociation equilibrium at $$\begin{gathered} 25^ \circ {\text{C: log }}K_{{\text{2a}}} = - 4.759 \pm 0.001{\text{, }}\Delta H_{{\text{2a}}}^{\text{o}} = \hfill \\ 2.2 \pm 0.1,{\text{ }}\Delta S_{{\text{2a}}}^{\text{o}} = - 83.8 \pm 0.4{\text{, and }}\Delta Cp_{{\text{2a}}}^{\text{o}} = - 192 \pm 15 \hfill \\ \end{gathered} $$ , and for the third dissociation equilibrium at $$\begin{gathered} 25^ \circ {\text{C: log }}K_{{\text{3a}}} = - 6.397 \pm 0.002{\text{, }}\Delta H_{{\text{3a}}}^{\text{o}} = \hfill \\ - 3.6 \pm 0.2,{\text{ }}\Delta S_{{\text{3a}}}^{\text{o}} = - 134.5 \pm 0.7{\text{, and }}\Delta Cp_{{\text{3a}}}^{\text{o}} = - 231 \pm 7 \hfill \\ \end{gathered} $$ .
    Type of Medium: Electronic Resource
    URL: http://dx.doi.org/10.1023/A:1024437112335
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  • 10
    Electronic Resource
    Electronic Resource
    Exactly soluble magnetoelastic lattice with a magnetic phase transition (1973)
    Springer
    Journal of statistical physics 7 (1973), S. 337-360 
    Details
    ISSN: 1572-9613
    Keywords: Magnetoelastic system ; phase transition ; renormalization of critical exponents ; Ising model ; statistical mechanics ; soluble models ; thermodynamics
    Source: Springer Online Journal Archives 1860-2000
    Topics: Physics
    Notes: Abstract We examine the soluble magnetoelastic Ising model developed by Baker and Essam and give a detailed discussion of its thermodynamic properties. Particular attention is devoted to the properties of the magnetic phase transition at zero field, which is found to be either first order or second order, depending on whether the experiment is performed at negative or positive pressure.
    Type of Medium: Electronic Resource
    URL: http://dx.doi.org/10.1007/BF01014909
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