By Shyama P. Sinha (Auth.)
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Additional resources for Complexes of the Rare Earths
Citric acid. OXYGEN DONORS 49 species such as [HM(Cit) 2 ] 2 -, [H 2 M(Cit) 2 ]-, and [H3M(Cit)2]° are undoubtedly present in solution. 0 x IO9 These values show a regular increase from La to Eu. Malyarov and Sudakov (4,66) have also investigated the formation of citrate (and tartrate) complexes of La, Pr, Nd and Sm by pH potentiometric method. Complexes of the type M2(OH)3(Cit) · 6H 2 0 are formed in alkaline solution, since in alkaline solution citric acid exists mainly in ionic form C6H507~.
The Ox2- ion has been used for /OH ON I QT x OH XIV. Oxalic acid. the coprecipitation of the rare earths specially in a homogeneous medium, using dimethyl oxalate for the generation of the oxalate ions. The kinetics of the hydrolysis of dimethyl oxalate has also been investigated/4·3*0 The systems Nd-Ce, Y-Ce and Yb-Nd TABLE 6. 5 at 25°C) M3+ log/:! 9) The criteria of the insolubility of the rare-earth oxalates in acid solution is often used for rapid separation of these ions from others. (4,42) Using 91Y, 152Eu and 154Eu the formation of mixed crystals has been demonstrated.
The acids complex through —C( anion losing a proton from the carboxylic group. Let us investigate in a little detail the nature of coordination of a carboxylate anion with a metal ion, taking the simplest case of a metal acetate (CH 3 —COOM). O-M C H a - Œv O-M 36 CH3-CÌX VIII )M 07 OXYGEN DONORS 37 From the study of the vibrational spectrum of the acetate ion one would expect to get some idea of the nature of the bonding in compounds VI-IX. Unfortunately, the free ion has a low symmetry (C2y) and no marked change inthe spectrum would arise from these various structures.
Complexes of the Rare Earths by Shyama P. Sinha (Auth.)