Mixed-metal hydroxycarboxylic acid complexes. Formation constants of complexes of UVI with FeIII, AlIII, InIII and CuII

Manzurola, Emanual; Apelblat, Alexander; Markovits, G.; Levy, Ophir

doi:10.1039/f19898500373

Cited by 22 publications

(8 citation statements)

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“…Reagents DQ716 and DQ2 were used as synthesised. 12, 13 The Fe(III) solution (0.05 M, containing HCl 0.3 M) was prepared by dissolving a known amount of iron granules (Aldrich, nominal purity 99.999%) in HCl + HNO 3 , following a method proposed by Manzurola et al 14…”

Section: Methodsmentioning

confidence: 99%

“…5c experimentally determined with L= 0.0 mM for peak I, L= 0.28 mM for peak II and L= 2.0 for peak III. (14) In this equation the proportionality constant is known, the derivative and the [Fe] j concentration are measured at the peak and from the peak area, respectively, after a simple peaks deconvolution. Table 4 summarizes all the results.…”

Section: Characterization Of the Experimental Data With Empirical App...mentioning

confidence: 99%

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Use of electrochemical transient techniques to obtain thermodynamic and kinetic data on aqueous Fe(III)–1,6-dimethyl-4-hydroxy-3-pyridinecarboxylate and Fe(III)–4-hydroxy-2-methyl-3-pyridinecarboxylate complexes

et al. 2009

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Voltammetric experiments were used to demonstrate the possibility to rapidly obtain stability constants, E degrees values and kinetic parameters of Fe(III) complexes with 1,6-dimethyl-4-hydroxy-3-pyridinecarboxylic acid (DQ716) at pH 2.3 and 4-hydroxy-2-methyl-3-pyridinecarboxylic acid (DQ2) at pH 3. Fe(III) diffusion coefficient (D(Fe)= 5.5.10(-6) cm(2)/s), heterogeneous electron transfer kinetic constant (k degrees = 2.7.10(-4)cm/s), symmetry coefficient (alpha= 0.57) and Fe(III)/Fe(II) standard reduction potential (E degrees = 0.53 V vs. SCE) were determined beforehand and used to obtain all the other results. Digital simulation together with potentiometric data were used to define the whole reaction system in terms of thermodynamic and kinetic parameters. In particular, E degrees and the dissociation kinetic constant, k(b), of the 1:1 (E degrees = 0.22 V vs. SCE, k(b)= 0.032 s(-1)), 1:2 (E degrees = 0.098 V vs. SCE; k(b)= 0.22 s(-1)) and 1:3 (E degrees < or =-0.29 V vs. SCE, k(b)= 157.9 s(-1)) Fe(III)/DQ716 complexes, were estimated. Stability constants of the Fe(II) complexes were computed from these values. The voltammetric data were also interpreted with two independent formalisms: (1) solution of an equation system and (2) a curve fitting method based on the Koutecky-Levich equation. Both approaches allowed us to obtain the speciation of a Fe(III)/DQ716 solution at pH 2.3. Moreover, the second approach allowed the evaluation of the kinetic contributions, the stepwise stability constant of Fe(III)L(2) (7.65 +/- 0.07), and to define the mathematical formalization of the experimental result which link some key-points of the voltammetric curve (inflection points and plateaux) to D(Fe), k degrees , alpha(j) and E degrees . This approach was also successfully applied to obtain the speciation of a Fe(III)/DQ2 solution at pH 3.

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Section: Methodsmentioning

confidence: 99%

Section: Characterization Of the Experimental Data With Empirical App...mentioning

confidence: 99%

Use of electrochemical transient techniques to obtain thermodynamic and kinetic data on aqueous Fe(III)–1,6-dimethyl-4-hydroxy-3-pyridinecarboxylate and Fe(III)–4-hydroxy-2-methyl-3-pyridinecarboxylate complexes

et al. 2009

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“…This gave more confidence in the data presented in Figure 1. It is worth mentioning here that although malic acid has two titratable carboxylate groups, the alcoholic group does not release its proton unless malic acid is reacting with a strong Lewis acid (the metal ion) [7,12,[16][17][18][19][22][23][24][25][26]. The next section gives more details on this point at which multiple examples prove the chelation of the alcoholic group participation to a variety of metal ions.…”

Section: Free Metal Ions and Free Malic Acidmentioning

confidence: 99%

“…Until now, *Address correspondence to these authors at the Division of Natural and Mathematical Sciences, LeMoyne-Owen College, 807 Walker Avenue, Memphis, TN 38126, USA; Tel: 1(901) 435-1392; Fax: 1(901) 435-1424; E-mail: Yahia_hamada@loc.edu citrate or malate has been identified as the organic acid anions secreted by roots in plants to detoxify aluminum in high aluminum-containing soils [15]. Some reports have investigated reactions of malic acid with metal ions [16][17][18][19]. The main objectives of the current report are 1-To collect the potentiometric titration plots for malic acid with Al 3+ and Cr 3+ , 2-To show the type of metal complexes formed under the ambient conditions of the study, and 3-To measure the potential response of the reaction mixture in milli-volts and relate this to Nernst Equation.…”

Section: Introductionmentioning

confidence: 99%

“…The main objectives of the current report are 1-To collect the potentiometric titration plots for malic acid with Al 3+ and Cr 3+ , 2-To show the type of metal complexes formed under the ambient conditions of the study, and 3-To measure the potential response of the reaction mixture in milli-volts and relate this to Nernst Equation. These objectives will confirm if malic acid is a candidate to un-leach these metal ions from the soil and if one of the formed metal complexes plays a role in the transport of these metal ions across cell membrane [14][15][16][17][18][19]. Potentiometry is one of the most powerful tools to study metal ions in aqueous solutions at ambient conditions [16][17][18][19][20][21].…”

Section: Introductionmentioning

confidence: 99%

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Detailed Potentiometric Study of Al3+ and Cr3+ with Malic Acid in Aqueous Solutions

Hamada¹

2013

J. Memb. Separ. Tech.

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It appeared that malic acid solubilized both Al 3+ and Cr 3+ in aqueous solutions at all pH-values in 0.1 M NaNO3 at 25 o C. The detailed potentiometric measurements indicated that these free tri-valent metal ions released a net of three protons (3H + 's) into the solution. Free malic acid released a net of (2H + 's) into the solution from the two carboxylates. However, in the presence of metal ions malic acid effectively releases a net of three protons (3H + 's) into the solution; two from the two carboxylates and the third from the alcoholic group. The reaction mixture of Al 3+ :malic acid indicated the formation of a dimeric species. The proposed structure of this dimeric species is in good agreement with what has been shown in the literature. We are presenting a dimeric species that may play an important role in malate transportation across cell membrane. Formation of the Al 3+ -malic acid complexes cover the span of a total of 400 mV; from +250 mV to -150 mV. The Cr 3+ -malic acid reaction mixture indicated the formation of a dimeric species as well.

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Amphiphilic Amide Derivatives of D‐Glucaric Acid. Synthesis and Complexing Properties Toward Lanthanide(III) Ions

Aury¹,

Rubini²,

Gérardin³

et al. 2004

Eur J Org Chem

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Hydrophobic derivatives of D‐glucaric acid, HOOC−(CHOH)4−CONHR,where R is an alkyl chain having 3, 8, 10, or 12 carbon atoms, have been synthesized from D‐glucaro‐1,4‐lactone and the corresponding amines. The complexing abilities of these compounds toward trivalent lanthanide cations have been studied, using the water‐soluble propyl compound, and compared to that of gulonic acid, which corresponds to the complexing part of these molecules. The formation constants of the complexes have been determined and their structures discussed. The surfactant properties of the C8, C10 and C12 glucaramides and their extracting ability toward LnIII ions have also been evaluated. (© Wiley‐VCH Verlag GmbH & Co. KGaA, 69451 Weinheim, Germany, 2004)

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Mixed-metal hydroxycarboxylic acid complexes. Formation constants of complexes of UVI with FeIII, AlIII, InIII and CuII

Cited by 22 publications

References 3 publications

Use of electrochemical transient techniques to obtain thermodynamic and kinetic data on aqueous Fe(III)–1,6-dimethyl-4-hydroxy-3-pyridinecarboxylate and Fe(III)–4-hydroxy-2-methyl-3-pyridinecarboxylate complexes

Use of electrochemical transient techniques to obtain thermodynamic and kinetic data on aqueous Fe(III)–1,6-dimethyl-4-hydroxy-3-pyridinecarboxylate and Fe(III)–4-hydroxy-2-methyl-3-pyridinecarboxylate complexes

Detailed Potentiometric Study of Al3+ and Cr3+ with Malic Acid in Aqueous Solutions

Amphiphilic Amide Derivatives of D‐Glucaric Acid. Synthesis and Complexing Properties Toward Lanthanide(III) Ions

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