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  • 2005-2009  (1)
  • 1995-1999  (7)
  • 1
    Book
    Book
    In honor of Dana R. Kesten (2005)
    Amsterdam [u.a.] : Elsevier
    Details Availability
    Type of Medium: Book
    Pages: V, 139 S. , Ill., graph. Darst., Kt.
    Series Statement: Marine Chemistry 97.2005,1/2
    Language: English
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  • 2
    Electronic Resource
    Electronic Resource
    Comprehensive Investigation of Yttrium and Rare Earth Element Complexation by Carbonate Ions Using ICP–Mass Spectrometry (1998)
    Springer
    Journal of solution chemistry 27 (1998), S. 803-815 
    Details
    ISSN: 1572-8927
    Keywords: Rare earth ; complexation ; carbonate ; ICP–MS
    Source: Springer Online Journal Archives 1860-2000
    Topics: Chemistry and Pharmacology
    Notes: Abstract Carbonate stability constants for yttrium and all rare earth elements have been determined at 25°C and 0.70 molal ionic strength by solvent exchange and inductively coupled plasma–mass spectrometry (ICP–MS). Measured stability constants for the formation of $${\text{MCO}}_3^ +$$ and $${\text{M}}\left( {{\text{CO}}_{\text{3}} } \right)_2^--$$ from M3+ are in good agreement with previous direct measurements, which involved the use of radio-chemical techniques and trivalent ions of Y, Ce, Eu, Gd, Tb, and Yb. Direct ICP–MS measurements of $${\text{MCO}}_3^ +$$ and $${\text{M}}\left( {{\text{CO}}_{\text{3}} } \right)_2^--$$ formation constants are also in general agreement with modeled stability constants for the metals La, Pr, Nd, Sm, Dy, Ho, Er, Tm, and Lu, based on linear-free energy relationship (LFER). The experimental procedures developed in this work can be used for assessing the complexation behavior of other geochemically important ligands such as phosphate, sulfate, and fluoride.
    Type of Medium: Electronic Resource
    URL: http://dx.doi.org/10.1023/A:1022677119835
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  • 3
    Electronic Resource
    Electronic Resource
    Comparative Coprecipitation of Phosphate and Arsenate with Yttrium and the Rare Earths: The Influence of Solution Complexation (1997)
    Springer
    Journal of solution chemistry 26 (1997), S. 1187-1198 
    Details
    ISSN: 1572-8927
    Keywords: Coprecipitation ; rare earths ; lanthanides ; yttrium ; phosphate ; arsenate
    Source: Springer Online Journal Archives 1860-2000
    Topics: Chemistry and Pharmacology
    Notes: Abstract Coprecipitation of yttrium (Y) and rare earth elements (REEs) with phosphate and arsenate removes these elements from solution in variable proportions. During both phosphate and arsenate Coprecipitation, middle REEs (Sm and Eu) are progressively depleted in solution relative to heavier and lighter elements. Solution complexation by oxalate (Ox 2-) influences Y and REE removal patterns by strongly enhancing the retention of Y and the heaviest REEs in solution. The extent of this enhancement is well described by a quantitative account of the comparative solution complexation of Y and REEs as M(Ox)+ and M(Ox) $$_{\text{2}}^ - $$ . The comparative behavior of phosphate and arsenate coprecipitation exhibits both similarities and differences. During arsenate coprecipitation the light REEs are retained in solution, relative to the heavy REEs, to a greater extent than is the case for phosphate coprecipitation. Notable irregularities are observed in the comparative coprecipitation behavior of nearest-neighbor elements (e.g., Eu–Gd–Tb and Tm–Yb–Lu). Such irregularities are very similar for phosphate and arsenate coprecipitation in the absence and in the presence of solution complexation.
    Type of Medium: Electronic Resource
    URL: http://dx.doi.org/10.1023/A:1022933224074
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  • 4
    Electronic Resource
    Electronic Resource
    The hydrolysis and fluoride complexation behavior of Fe(III) at 25°C and 0.68 molal ionic strength (1996)
    Springer
    Journal of solution chemistry 25 (1996), S. 773-785 
    Details
    ISSN: 1572-8927
    Keywords: Iron(III) ; ferric ; hydrolysis ; fluoride ; complexation
    Source: Springer Online Journal Archives 1860-2000
    Topics: Chemistry and Pharmacology
    Notes: Abstract Fe(III) hydrolysis and fluoride complexation behavior was examined in 0.68 molal sodium perchlorate at 25°C. Our assessment of the complexation of Fe(III) by fluoride ions produced the following results: logFβ1 = 5.155, logFβ2 = 9.107, logFβ3 = 11.96, logFβ4 = 13.75, where logFβn = 5.155=[FeF n (3-n)+ ][Fe3+]−1[F−]−n. The stepwise fluoride complexation constants,FK n+1, obtained in our work (where logF K n+1 =logFβn) indicate that K n+1/K n =0.072±0.01. Formation constants for equilibria, Fe3++nH2O⇌Fe(OH) n (3−n)+ +nH+, expressed in the form β n * [Fe(OH) n (3-n)+ ][H+]n ,[Fe 3+]-1, were estimated as β 1 * = −2.754, and β 2 * ≤ −7. Our study indicates that the results of previous hydrolysis investigations include very large overestimates of Fe(OH) 2 + formation constants.
    Type of Medium: Electronic Resource
    URL: http://dx.doi.org/10.1007/BF00973784
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  • 5
    Electronic Resource
    Electronic Resource
    Ionic Strength Dependence of Rare Earth – NTA Stability Constants at 25°C (1997)
    Springer
    Aquatic geochemistry 3 (1997), S. 99-115 
    Details
    ISSN: 1573-1421
    Keywords: rare earth elements ; copper ; complexation ; ionic strength effects ; nitrilotriacetic acid ; lanthanide ; yttrium
    Source: Springer Online Journal Archives 1860-2000
    Topics: Chemistry and Pharmacology , Geosciences
    Notes: Abstract Observations of competitive complexation of NTA by Cu2+ and rare earth element (REE) ions are used to determine REE-NTA stability constants at ionic strengths between 0.1 and 5.0 molar. Although REE stability constants change markedly with ionic strength, differences in the ionic strength dependence of REE-NTA stability constants across the rare earth element series are small. The ionic strength dependence of logβ1 for Y and REEs with NTA at 25 °C can be described as: logβ1(M) = logβ1(M)0 - 9.198 I1/2/(1+B I1/2)+C I + D I3/2, where β1(M) = [MNTA°][M3+]-1[NTA3-]-1, I is ionic strength, B = 1.732, C = 0.1596, D = 0.0816, and logβ1(M)° is the metal-NTA stability constant at zero ionic strength.
    Type of Medium: Electronic Resource
    URL: http://dx.doi.org/10.1023/A:1009643409154
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  • 6
    Electronic Resource
    Electronic Resource
    The solubility control of rare earth elements in natural terrestrial waters and the significance of PO 4 3− and CO 3 2− in limiting dissolved rare earth concentrations: A review of recent information (1995)
    Springer
    Aquatic geochemistry 1 (1995), S. 157-173 
    Details
    ISSN: 1573-1421
    Keywords: rare earth elements ; lakes ; groundwaters ; activity products ; solubility products ; solubility controls ; complexation
    Source: Springer Online Journal Archives 1860-2000
    Topics: Chemistry and Pharmacology , Geosciences
    Notes: Abstract Rare earth element (REE) concentrations in alkaline lakes, circumneutral pH groundwaters, and an acidic freshwater lake were determined along with the free carbonate, free phosphate, and free sulfate ion concentrations. These parameters were used to evaluate the saturation state of these waters with respect to REE phosphate and carbonate precipitates. Our activity product estimates indicate that the alkaline lake waters and groundwaters are approximately saturated with respect to the REE phosphate precipitates but are significantly undersaturated with respect to REE carbonate and sulfate precipitates. On the other hand, the acidic lake waters are undersaturated with respect to REE sulfate, carbonate, and phosphate precipitates. Although carbonate complexes tend to dominate the speciation of the REEs in neutral and alkaline waters, our results indicate that REE phosphate precipitates are also important in controlling REE behavior. More specifically, elevated carbonate ion concentrations in neutral to alkaline natural waters tend to enhance dissolved REE concentrations through the formation of stable REE-carbonate complexes whereas phosphate ions tend to lead to the removal of the REEs from solution in these waters by the formation of REE-phosphate salts. Removal of REEs by precipitation as phosphate phases in the acid lake (pH=3.6) is inconsequential, however, due to extremely low [PO 4 3− ] F concentrations (i.e., ∼ 10−23 mol/kg).
    Type of Medium: Electronic Resource
    URL: http://dx.doi.org/10.1007/BF00702889
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  • 7
    Electronic Resource
    Electronic Resource
    Interaction of B $$(OH)_3^0 $$ and $$HCO_3^ - $$ in Seawater: Formation of B $$(OH)_2 CO_3^ - $$ (1997)
    Springer
    Aquatic geochemistry 3 (1997), S. 345-356 
    Details
    ISSN: 1573-1421
    Keywords: boron ; boric acid ; carbonate ; CO2 system ; complexation ; spectrophotometric pH
    Source: Springer Online Journal Archives 1860-2000
    Topics: Chemistry and Pharmacology , Geosciences
    Notes: Abstract Boron is known to interact with a wide variety of protonated ligands(HL) creating complexes of the form B(OH)2L-.Investigation of the interaction of boric acid and bicarbonate in aqueoussolution can be interpreted in terms of the equilibrium $$B(OH)_3^0 + HCO_3^ - \rightleftharpoons B(OH)_2 CO_3^ - + H_2 O$$ The formation constant for this reaction at 25 °C and 0.7 molkg-1 ionic strength is $$K_{BC} = \left[ {B(OH)_2 CO_3^ - } \right]\left[ {B(OH)_3^0 } \right]^{ - 1} \left[ {HCO_3^ - } \right]^{ - 1} = 2.6 \pm 1.7$$ where brackets represent the total concentration of each indicatedspecies. This formation constant indicates that theB(OH)2 $$CO_3^ - $$ concentration inseawater at 25 °C is on the order of 2 μmol kg-1. Dueto the presence of B(OH)2 $$CO_3^ - $$ , theboric acid dissociation constant ( $$K\prime _B $$ ) in natural seawaterdiffers from $$K\prime _B $$ determined in the absence of bicarbonate byapproximately 0.5%. Similarly, the dissociation constants of carbonicacid and bicarbonate in natural seawater differ from dissociation constantsdetermined in the absence of boric acid by about 0.1%. Thesedifferences, although small, are systematic and exert observable influenceson equilibrium predictions relating CO2 fugacity, pH, totalcarbon and alkalinity in seawater.
    Type of Medium: Electronic Resource
    URL: http://dx.doi.org/10.1023/A:1009633804274
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  • 8
    Electronic Resource
    Electronic Resource
    A Coupled Riverine-Marine Fractionation Model for Dissolved Rare Earths and Yttrium (1998)
    Springer
    Aquatic geochemistry 4 (1998), S. 103-121 
    Details
    ISSN: 1573-1421
    Keywords: Rare earth ; Rare earth ; fractionation ; model ; riverine ; oceanic ; estuarine
    Source: Springer Online Journal Archives 1860-2000
    Topics: Chemistry and Pharmacology , Geosciences
    Notes: Abstract Fractionation of yttrium (Y) and the rare earth elements (REEs) begins in riverine systems and continues in estuaries and the ocean. Models of yttrium and rare earth (YREE) distributions in seawater must therefore consider the fractionation of these elements in both marine and riverine systems. In this work we develop a coupled riverine/marine fractionation model for dissolved rare earths and yttrium, and apply this model to calculations of marine YREE fractionation for a simple two-box (riverine/marine) geochemical system. Shale-normalized YREE concentrations in seawater can be expressed in terms of fractionation factors (λ ij ) appropriate to riverine environments ( $$\lambda _{ij}^{river}$$ ) and seawater ( $$\lambda _{ij}^{ocean}$$ ): $$\log \frac{{\left( {M_i } \right)_T^{ocean} }}{{\left( Y \right)_T^{ocean} }} = log\;\lambda _{ij}^{ocean} + ((\lambda _{ij}^{river} )^{ - 1} - 1)\;log\frac{{[Y]_T^{river} }}{{[Y^0 ]_T^{river} }}$$ where $$\left( {M_i } \right)_T^{ocean}$$ and $$\left( Y \right)_T^{ocean}$$ are input-normalized total metal concentrations in seawater and $$[Y]_T^{river} /[Y^0 ]_T^{river}$$ is the ratio of total dissolved Y in riverwater before $$([Y^0 ]_T^{river} )$$ and after $$([Y]_T^{river} )$$ commencement of riverine metal scavenging processes. The fractionation factors (λ ij ) are calculated relative to the reference element, yttrium, and reflect a balance between solution and surface complexation of the rare earths and yttrium.
    Type of Medium: Electronic Resource
    URL: http://dx.doi.org/10.1023/A:1009651919911
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