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  • 2020-2023  (1)
  • 2000-2004  (275)
  • 1995-1999  (47)
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  • 1
    Electronic Resource
    Electronic Resource
    Binding of Cu(II) to the Surface and Exudates of the Alga Dunaliella tertiolecta in Seawater (1995)
    s.l. : American Chemical Society
    Environmental science & technology 29 (1995), S. 289-301 
    Details
    ISSN: 1520-5851
    Source: ACS Legacy Archives
    Topics: Chemistry and Pharmacology , Energy, Environment Protection, Nuclear Power Engineering
    Type of Medium: Electronic Resource
    URL: http://dx.doi.org/10.1021/es00002a001
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  • 2
    Electronic Resource
    Electronic Resource
    Rates and Mechanism of Fe(II) Oxidation at Nanomolar Total Iron Concentrations (1995)
    s.l. : American Chemical Society
    Environmental science & technology 29 (1995), S. 818-824 
    Details
    ISSN: 1520-5851
    Source: ACS Legacy Archives
    Topics: Chemistry and Pharmacology , Energy, Environment Protection, Nuclear Power Engineering
    Type of Medium: Electronic Resource
    URL: http://dx.doi.org/10.1021/es00003a033
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  • 3
    Electronic Resource
    Electronic Resource
    The Activity Coefficients of HCl in HCl–Na2SO4 Solutions from 0 to 50°C and Ionic Strengths Up to 6 Molal (1997)
    Springer
    Journal of solution chemistry 26 (1997), S. 31-45 
    Details
    ISSN: 1572-8927
    Keywords: Activity coefficient ; electromotive force ; Pitzer ; HCl ; Na2SO4 ; NaHSO4
    Source: Springer Online Journal Archives 1860-2000
    Topics: Chemistry and Pharmacology
    Notes: Abstract The electromotive force of HCl–Na2SO4 solutions has been determined from 5 to 50°C and ionic strengths from 0.5 to 6m with a Harned type cell $${\text{Pt; H}}_{\text{2}} ({\text{g, 1 atm}})|{\text{HCl(}}m_1 {\text{) + Na}}_{\text{2}} {\text{SO}}_{\text{4}} {\text{(}}m_2 {\text{)}}|{\text{AgCl, Ag}}$$ The results have been used to determine the activity coefficient of HCl in the mixtures. The activity coefficients have been analyzed with the Pitzer equations to account for the ionic interactions. The measurements were used to determine interaction coefficients (β0, β1) for NaHSO4 solutions from 5 to 50°C. The model represents the mean activity coefficients of HCl in the mixtures to ±0.005 over the entire temperature and concentration range of the measurements. The results have been combined with literature data to provide parameters that are valid from 0 to 250°C for NaHSO4 solutions.
    Type of Medium: Electronic Resource
    URL: http://dx.doi.org/10.1023/A:1024433011426
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  • 4
    Electronic Resource
    Electronic Resource
    The Speciation of (CH3)2Sn2+ in Electrolyte Solution Containing the Major Components of Natural Waters (1999)
    Springer
    Aquatic geochemistry 5 (1999), S. 381-398 
    Details
    ISSN: 1573-1421
    Keywords: dependence on medium of hydrolysis constants ; ΔH° for the hydrolysis of (CH3)2Sn2+ ; hydrolysis of (CH3)2Sn2+ ; Pitzer interaction parameters ; speciation of (CH3)2Sn2+ in natural waters
    Source: Springer Online Journal Archives 1860-2000
    Topics: Chemistry and Pharmacology , Geosciences
    Notes: Abstract Hydrolysis constants of dimethyltin(IV) cation, in different salt solutions (CaCl2: 0.15 ≤ I ≤ 0.90; MgCl2: 0.30 ≤ I ≤ 0.60; NaCl-–NaClO4, NaCl-–NaNO3 mixtures: I = 3; NaCl-–Na2SO4 mixtures: I = 1 mol dm-3) were determined by potentiometric ([H+]-glass electrode) measurements. These data, together with previous data (De Stefano et al., 1996b) were interpreted in terms of DHT (Debye–Hückel type) and Pitzer equations. The mixed electrolyte solution results also allowed us to obtain Θ and Ψ parameters for the Pitzer equation. Calorimetric measurements were made at different ionic strengths in order to find the temperature dependence of hydrolysis constants and of the relative interaction parameters. The body of results allows us to determine the speciation of natural waters in a wide range of ionic strengths and temperatures.
    Type of Medium: Electronic Resource
    URL: http://dx.doi.org/10.1023/A:1009613712280
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  • 5
    Electronic Resource
    Electronic Resource
    Modeling Heat Capacities of High Valence-Type Electrolyte Solutions with Pitzer's Equations (1999)
    Springer
    Journal of solution chemistry 28 (1999), S. 849-864 
    Details
    ISSN: 1572-8927
    Keywords: Apparent molar heat capacities ; partial molar heat capacities ; Pitzer's equations ; lanthanide elements ; transition metals ; alkali metal sulfates ; magnesium sulfate
    Source: Springer Online Journal Archives 1860-2000
    Topics: Chemistry and Pharmacology
    Notes: Abstract Apparent molar heat capacities C p,φ for 71 rare earth chlorides, nitrates, and perchlorates, alkaline earth and transition metal chlorides, nitrates, and perchlorates, and alkali metal carbonates and sulfates have been fitted to the Pitzer equation for heat capacities. The apparent molar heat capacities at infinite dilution $$C_{{\text{p,}}\Phi }^{\text{o}} $$ (equal to the standard partial molar heat capacity, $$\overline C _{{\text{p,2}}}^{\text{o}} $$ ) were used to evaluate a set of “best” ionic heat capacities, from which improved values of $$C_{{\text{p,}}\Phi }^{\text{o}} $$ for the electrolytes were calculated. These were then used in the Pitzer equation to reevaluate the higher Pitzer coefficients. The Pitzer coefficients so evaluated can express, in most cases, the behavior of C p,φ within experimental error from infinite dilution to the upper limit of the data. Ionic heat capacities have been correlated with the absolute entropies of the ions by statistically assigning the ionic heat capacities to obtain the best linear fit.
    Type of Medium: Electronic Resource
    URL: http://dx.doi.org/10.1023/A:1021732214671
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  • 6
    Electronic Resource
    Electronic Resource
    Hydrolysis of (CH3)3Sn+ in Various Salt Media (1999)
    Springer
    Journal of solution chemistry 28 (1999), S. 959-972 
    Details
    ISSN: 1572-8927
    Keywords: Hydrolysis of trimethyltin(IV) ; hydrolysis constants ; enthalpy of hydrolysis ; dependence on ionic strength ; Pitzer interaction parameters ; speciation of trimethyltin(IV)
    Source: Springer Online Journal Archives 1860-2000
    Topics: Chemistry and Pharmacology
    Notes: Abstract The hydrolysis of trimethyltin(IV) has been studied by potentiometry (H+ -glass electrode) and calorimetry in various salt media (NaNO3, NaCl, KCl, Na2SO4, and NaNO3—NaCl mixtures). The effect of ionic strength on the hydrolysis constants is accounted for by a simple Debye–Hückel type equation and by Pitzer equations. The results allow us to obtain ΔH for hydrolysis and the temperature dependence of the Pitzer parameters. The resulting coefficients can be used to examine the speciation of (CH3)3Sn+ in multicomponent electrolyte solutions, such as natural waters, over a wide range of temperature and ionic strength.
    Type of Medium: Electronic Resource
    URL: http://dx.doi.org/10.1023/A:1021744517397
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  • 7
    Electronic Resource
    Electronic Resource
    Thermodynamics of the System HCl + SmCl3 + H2O from 5 to 55°C. Application of Harned's Rule and the Pitzer Formalism (2000)
    Springer
    Journal of solution chemistry 29 (2000), S. 1211-1227 
    Details
    ISSN: 1572-8927
    Keywords: samarium chloride: activity coefficients ; Nernst equation ; Harned's rule ; emf ; Pitzer equations
    Source: Springer Online Journal Archives 1860-2000
    Topics: Chemistry and Pharmacology
    Notes: Abstract A comprehensive array of electrochemical cell measurements for the system HCl +SmCl3 + H2O was made from 5 to 55°C using a cell without liquid junction ofthe type:Pt; H2(g, 1 atm)|HCl (m A) + SmCl3 (m B)|AgCl, Ag (A)The present study, unlike previous studies of trivalent ions, are not complicatedby hydrolysis reactions. Measurements of the emf were performed for solutionsat constant total ionic strengths of 0.025, 0.05, 0.1, 0.25, 0.5, 1.0, 1.5, 2.0, 2.5,and 3.0 mol-kg−1. The mean activity coefficients of HCl (γHCl) in the mixtureswere calculated using the Nernst equation. All the experimental emf measurements(about 850) were first treated in terms of the simpler Harned's rule. Harnedinteraction coefficients (αAB and βAB) were calculated. The linear form of Harned'srule is valid for most ionic strengths, but quadratic terms are needed at I = 1.5and 3 mol-kg−1. The Pitzer model was used to evaluate the activity coefficientsusing literature values, β(0), β(1), and C φ, for HCl from 0 to 50°C and 25°C forSmCl3. The effect of temperature on the parameters for SmCl3 has been estimatedusing enthalpy and heat-capacity data. The mixing parameter ΘH,Sm wasdetermined at 25°C. The addition of the ΨH,Sm,Cl coefficient did not improve the fitsignificantly and no temperature dependence was found to be significant. Thevalue of ΘH,Sm = 0.2 ± 0.01 represented the values of γHCl with a standarddeviation of σ = 0.009 over the entire range of temperatures and ionic strength.The use of higher-order electrostatic effects (EΘH,Sm, EΘH,Sm) was included as itgave a better fit of the activity coefficients of HCl.
    Type of Medium: Electronic Resource
    URL: http://dx.doi.org/10.1023/A:1026484112080
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  • 8
    Electronic Resource
    Electronic Resource
    Activity Coefficients of HCl + GdCl3 + H2O System from 5 to 55°C. Application of Pitzer Formalism (2000)
    Springer
    Journal of solution chemistry 29 (2000), S. 619-631 
    Details
    ISSN: 1572-8927
    Keywords: Hydrochloric acid ; gadolinium chloride ; emf ; Harned's rule ; Pitzer equations ; activity coefficients ; mixtures of electrolytes
    Source: Springer Online Journal Archives 1860-2000
    Topics: Chemistry and Pharmacology
    Notes: Abstract The emf of the cell $${\text{Pt, H}}_{\text{2}} ({\text{g, 1 atm}})|{\text{HCI(}}m_{\text{A}} {\text{),GdCl}}_{\text{3}} (m_B )|{\text{AgCl, Ag}}$$ without a liquid junction was used to investigate the HCl + GdCl3 + H2O mixedelectrolyte system. The emf of the cell was measured for HCl + GdCl3 + H2Osolutions at ionic strengths of 0.025, 0.05, 0.1, 0.5, 1.0, 1.5, and 2.0 mol-kg−1and at eleven temperatures ranging from 5 to 55°C at 5°C intervals. The meanactivity coefficients for HCl in the mixtures were determined using the Nernstequation. About 793 experimental emf data points were treated by the Harnedequations. Results show that hydrochloric acid follows Harned's rule at all ionicstrengths, but the quadratic term is needed for I = 1.5 mol-kg−1. Theion-interaction treatment of Pitzer was used to evaluate the results. The binary andternary mixing parameters at 25°C were found to be ΘH,Gd = 0.07 ± 0.03 andΨH,Gd,Cl = 0.14 ± 0.03. These values were determined using literature values ofβ(0), β(1), and C ψ for GdCl3 at 25°C and estimates of the effect of temperaturefrom 5 to 55°C using enthalpy and heat capacity data.
    Type of Medium: Electronic Resource
    URL: http://dx.doi.org/10.1023/A:1005129407455
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  • 9
    Electronic Resource
    Electronic Resource
    The Apparent Molal Volume and Compressibility of Seawater Fit to the Pitzer Equations (2000)
    Springer
    Journal of solution chemistry 29 (2000), S. 719-742 
    Details
    ISSN: 1572-8927
    Keywords: Apparent molal volumes ; apparent molar compressibilities ; sea water ; Pitzer equations ; sea salts
    Source: Springer Online Journal Archives 1860-2000
    Topics: Chemistry and Pharmacology
    Notes: Abstract The density and compressibility of seawater salt solutions for ionic strengths 0to 0.8 m, temperatures 0–40°C, and applied pressure 0 to 1000 barare fitted tothe Pitzer equations. The apparent molal volumes and compressibilities (Xφ) arefitted to equations of the form $$X_\phi = \mathop {X^0 }\limits^ + A_X I/(1.2m)\ln (1 + 1.2I^{0.5} ) + 2 RT m(\beta ^{(0)X} + \beta ^{(1)X} g(y) + m C^X )$$ where I is the ionic strength, m is the molality of seasalt, A X is the Debye—Hückelslope for the volume (X = V) or compressibility(X = κ) and g(y) = (2/y 2)[1 − (1 + y)exp(x)] where y = 2I 0.5. The Pitzer parameters β(0)X,β(1)X, and C Xare fitted to functions of temperature and pressure in the form $$Y^{\text{x}} = \Sigma _{\text{i}} \Sigma _{\text{j}} a_{{\text{ij}}} (T - T_{\text{R}} )^{\text{i}} P^{\text{j}} $$ where a ij are adjustable parameters, Y X is the Pitzer parameter, T is the temperaturein K, T R = 298.15 K, and P is the applied pressure in bars (P = 0 at 1 atm or1.013 bar). The standard deviations of the seawater fits are 8.3×10−6 cm3-g−1for the specific volumes, 0.0007×10−6 bar−1 for the compressibilities, and0.63×10−6 K−1 for the thermal expansibilities. At 25°C, the measured densitiesof seawater are compared to the calculated values using Pitzer coefficients forthe major sea salts. The results agree with the measured values to within 45×10−6g-cm−3.
    Type of Medium: Electronic Resource
    URL: http://dx.doi.org/10.1023/A:1005164911283
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  • 10
    Electronic Resource
    Electronic Resource
    The Equation of State of Lakes (2000)
    Springer
    Aquatic geochemistry 6 (2000), S. 1-17 
    Details
    ISSN: 1573-1421
    Keywords: lakes ; density ; compressibility ; expansibility ; conductivity ; stability ; pvt properties
    Source: Springer Online Journal Archives 1860-2000
    Topics: Chemistry and Pharmacology , Geosciences
    Notes: Abstract In recent years, a number of workers have studied the stability of deep lakes such as Lake Tanganyika, Lake Baikal and Lake Malawi. In this paper, the methods that can be used to determine the effect that the components of lakes have on the equation of state are examined. The PVT properties of Lakes have been determined by using apparent molal volume data for the major ionic components of the lake. The estimated PVT properties (densities, expansibility and compressibilities) of the lakes are found to be in good agreement with the PVT properties (P) of seawater diluted to the same salinity. This is similar to earlier work that showed that the PVT properties of rivers and estuarine waters could also be estimated from the properties of seawater. The measured densities of Lake Tanganyika were found to be in good agreement (± 2 × 10-6 g cm-3) with the values estimated from partial molal properties and the values of seawater at the same total salinity (ST = 0.568‰). The increase in the densities of Lake Tanganyika waters increased due to changes in the composition of the waters. The measured increase in the measured density (45 × 10-6 g cm-3) is in good agreement (46 × 10-6 g cm-3) with the values calculated for the increase in Na+, HCO3 -, Mg2+, Ca2+ and Si(OH)4. Methods are described that can be used to determine the conductivity salinity of lakes using the equations developed for seawater. By combining these relationships with apparent molal volume data, one can relate the PVT properties of the lake to those of seawater.
    Type of Medium: Electronic Resource
    URL: http://dx.doi.org/10.1023/A:1009626325650
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