Stabilité des carboxylates de terres, III. Maléates, méthylsuccinates et malates

Roulet, Raymond; Feuz, J.; Duc, T. Vu

doi:10.1002/hlca.19700530736

Cited by 17 publications

(4 citation statements)

References 6 publications

Supporting

Mentioning

Contrasting

Order By: Relevance

“…Binuclear complexes with various stoichiometry to a considerable amounts are not detected by us. Calculated stability constants of L-malate complexes are satisfactorily agreed with data [3,5,6,8,[9][10][11][12][13]. In works [10][11] calculated stability constants of monomalate complexes were probably overestimated because of the neglect of protonated complexes.…”

Section: +supporting

confidence: 67%

“…In works [10][11] calculated stability constants of monomalate complexes were probably overestimated because of the neglect of protonated complexes. And it is possible to explain the understated stability constants of dimalate complexes [3,5,6,8,9,12,13] by use both of the uncoordinated scheme of equilibrium and the neglect of protonated complexes and hydroxocomplexes. ion.…”

Section: +mentioning

confidence: 99%

“…The complex formation of the Nd 3+ ion and the Sm 3+ ion with the malic acid was studied by potentiometric methods [3][4][5][6][7][8][9][10][11] and spectroscopy method [12].…”

Section: Introductionmentioning

confidence: 99%

See 2 more Smart Citations

The Difference of the Complex Formation of the Samarium (3+) Ion with the L-malic Acid as Compared to the Neodymium (3+) Ion

Buz’ko

Sukhno

Gavriluyk

et al. 2017

Eurasian Chem. Tech. J.

View full text Add to dashboard Cite

The complex formation of the neodymium Nd 3+ ion and the samarium Sm 3+ ion with L-malic acid (H 3 Mal) in the aqueous solutions was studied by pH-metric titration in pH region 2.80 to 10.00 and constant ionic strength 0.1 M KCl at 25°C. The ratios of the concentrations of the rare-earth elements (Ln) and the L-malic acid were 1:0.5, 1:1 and 1:2. The number of experimental points of each curve of pH-metric titration was 160-190 at 5-6 independent titrations. Inasmuch as the literature data give mainly the dissociation constants for the racemic DL-malic acid, acid-base equilibria of L-malic acid at ionic strength of 0.1 M KCl were also previously studied in pH 3.1-11.0 range. The number of experimental points for the each titration curve of L-malic acid was 70-100 at 8 independent titrations. The dissociation constants of Lmalic acid were calculated.The compositions and the stability constants of the rare-earth element complexes with L-malic acid were calculated by SuperQuad program for complex equilibria. It was shown, that in addition to 1:1 and 1:2 complexes with differently deprotonated L-malic acid, the hydroxocomplexes and protonated complexes of the rare-earth elements are also formed. The difference of the complex formation of the Sm 3+ ion with Lmalic acid as compared to the Nd 3+ ion was discussed.

show abstract

Section: +supporting

confidence: 67%

Section: +mentioning

confidence: 99%

See 1 more Smart Citation

The Difference of the Complex Formation of the Samarium (3+) Ion with the L-malic Acid as Compared to the Neodymium (3+) Ion

Buz’ko

Sukhno

Gavriluyk

et al. 2017

Eurasian Chem. Tech. J.

View full text Add to dashboard Cite

show abstract

“…We feel that the different results obtained in the two buffer systems is a reflection of the difference in metal ion binding capacities of the two buffers. Hepes has a very low affinity for metal ions (Good et al, 1966) whereas a dicarboxylic acid such as maleate would be expected to have a higher affinity for the metal ions (A) for the Nd3" complex is 4610, Roulet et al (1970)). In maleate buffer there is less free metal ion present and hence the effective metal ion concentration is much lower than in Hepes buffer.…”

Section: Resultsmentioning

confidence: 99%