Solvent extraction studies of ion association. Some europium complexes

Manning, P. G.; Monk, C. B.

doi:10.1039/tf9625800938

Cited by 30 publications

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“…Stability constant expressed in terms of free ion concentrations. (b) Manning and Monk (1962), solvent extraction. Data corrected for YREE acetate complexation.…”

Section: Introductionmentioning

confidence: 99%

Determination of SO4β1 for yttrium and the rare earth elements at I = 0.66 m and t = 25°C—implications for YREE solution speciation in sulfate-rich waters

Schijf

Byrne

2004

Geochimica et Cosmochimica Acta

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“…Stability constant expressed in terms of free ion concentrations. (b) Manning and Monk (1962), solvent extraction. Data corrected for YREE acetate complexation.…”

Section: Introductionmentioning

confidence: 99%

Determination of SO4β1 for yttrium and the rare earth elements at I = 0.66 m and t = 25°C—implications for YREE solution speciation in sulfate-rich waters

Schijf

Byrne

2004

Geochimica et Cosmochimica Acta

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“…42 In this paper (Part I), both techniques have been applied for studying the complexation of Eu(III) as an analog of trivalent actinides by small organic ligands (AA, GA, and A4HPA) as model molecules for HS. The first two systems have been extensively studied by various techniques, the Eu-GA system by ion exchange, 43,44 electrochemistry, [45][46][47][48] or time-resolved laser-induced fluorescence spectrometry, 49 and the Eu-AA system by spectrophotometry, 50 ion exchange, 43,51 or electrochemistry, 48,52,53 which will allow comparisons. In the next publication, the methodology and results introduced in this paper will be applied to the study of the interactions between Eu(III) and humic substances by the same techniques (Part II).…”

Section: Introductionmentioning

confidence: 99%

On the Use of Spectroscopic Techniques for Interaction Studies, Part I: Complexation between Europium and Small Organic Ligands

et al. 2005

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In the framework of environmental studies, it is important to understand the interaction of humic substances with cations (heavy metals, radionuclides) and to determine their complexation constants in order to evaluate their potential impact on their fate. For this purpose, two techniques have been used: electrospray ionization mass spectrometry, a newly used technique in speciation studies, and time-resolved laser-induced fluorescence spectrometry, a well-known technique for such studies. As a first step, for simplification purposes and to compare both techniques, simple molecules having functional groups present in humic substances have been selected, such as acetic, glycolic, and 4-hydroxyphenylacetic acids. Both techniques have been used to obtain stoichiometries and complexation constants between these simple molecules and europium (III).

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“…The experimental techniques have been described in detail in earlier publicatiol~s (7). The organic phase was 0.035 i M thenoytrilluoroacetone in toluene.…”

Section: E S P E R I M E K T I \ Lmentioning

confidence: 99%

Europium Oxalate Ion Association in Water

Manning¹

1966

Can. J. Chem.

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IASSINGd [ilres Brcln( 11, Depnrttr~ent of ilFi'iltes atld Tecl~r~zcc~l Sl~wcys, Ottawa, C(~nada Received March 4, 1066 .-iRSTRACT The partitioning of radiotracer 1"1151fC~~ between aqueous sodium osalate (3a.L) solutions and toluene solutio!ls of thenoyltritluoroaceto~le (HTTz1) has been studied as a function of the oxalate concentrat~on. The pl-I of the aqLleoLrs phase was controlled by Incans of sodiunl acetate -acetic acid ~nixtures and the ionic strength (I) by NaCl or NaCIO.,. The magnit~~des of the stepwise stability constant ratios are disc~~sscd. INTRODUCTIONRare earth -oxalate complexing in solution has been studied extensively by Croutha~llel and Martin (1) and by Seliine (2). The absolute magnitudes of the stability constants of the complexes cannot be compared directly because of the vastly dilierent ionic strengths used in these worlis. However, the ratios of the stepwise stability coilstants are clearly a t variance (Table I). The stepwise stability constallt is defined a s where L is the ligand. Bjerrunl (3) has sho\\.n that for siinple conlplexes where S is a statistical factor and T is a llleasure of the work done in bringing a charged ligand from infinity to its equilibrium position in the 1:2 complex against the repulsive force exerted by already bound ligands. For singly charged ligands that bind to rare earth or transition metal ions it has been shown that T = 1.6 (4, 5). If the cation has Navailable sites and if, for example, the ligand is monodentate,The factor of 2 arises because the probability of a ligand's leaving the 1:2 complex is twice that of a ligand's leaving the 1 : l . The R factor, termed the rest effect, covers those contributions to P that are neitller statistical nor electrostatic. R w-ill be an inlportant entity in stepwise reactions where, for example, the cation coordinatioll number changed.Steric hindrance and metal-ligand covalency are other obvious contributors to R. The nlagnitudes of the ratios of the stepwise stability constants are discussed later in this paper. The solvent extraction -radiotracer technique has proved useful in the study of rare earth ion association reactions in solution (6). The method is particularly applicable in the

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Solvent extraction studies of ion association. Some europium complexes

Cited by 30 publications

References 0 publications

Determination of SO4β1 for yttrium and the rare earth elements at I = 0.66 m and t = 25°C—implications for YREE solution speciation in sulfate-rich waters

Determination of SO4β1 for yttrium and the rare earth elements at I = 0.66 m and t = 25°C—implications for YREE solution speciation in sulfate-rich waters

On the Use of Spectroscopic Techniques for Interaction Studies, Part I: Complexation between Europium and Small Organic Ligands

Europium Oxalate Ion Association in Water

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