Yttrium water

III) nitrate 4-water (III) oxide (III) sulfate 8-water Yttrium chloride fluoride... 

Bismuth Trisulfate. Bismuth(III) sulfate [7787-68-0], Bi2(S0 3, is a colorless, very hygroscopic compound that decomposes above 405°C to yield bismuthyl salts and Bi202. The compound hydrolyzes slowly in cold water and rapidly in hot water to the yellow bismuthyl sulfate [12010-64-9], (Bi0)2S04. The normal sulfate is isomorphous with the sulfates of yttrium, lanthanum, and praseodymium. 

For elimination of intramolecular energy losses, we have synthesized ligands with high hydrophobisity - perfluoro-P-diketones R -CO-CH -CO-R, (R = CgF j or CgF R = phenyl or a-thienyl), that without second ligand eliminate completely water molecules from the inner coordination sphere. These ligands we have used in analysis at determination of Sm, Eu, Nd, Yb microamounts in high-purity lanthanide and yttrium oxides. 

Silver-colored, ductile metal that is attacked slowly by air and water. The element exhibits interesting magnetic properties. Found in television tubes. Laser material such as YAG (yttrium-aluminum garnet) doped with holmium (as well as chromium and thulium) can be applied in medicine, especially in sensitive eye operations. 

Sc(OTf)3 is stable in water, and effectively activates carbonyl and related compounds as a Lewis acid in water. This is remarkable, because most Lewis acids react immediately with water rather than the substrates, and are decomposed or deactivated. It has already been found that lanthanide trifiates Ln(OTf)3 (Ln = La, Ce, Pr, Nd, Sm, Eu, Gd, Tb, Dy, Ho, Er, Tm, Yb, Lu) and yttrium trifiate Y(OTf)3 are stable in water, and can act as Lewis-acid catalysts in aqueous media.46-48 They are used catalytically in many reactions and can often be recovered and reused, because they are stable under the usual water-quenching conditions. 

The reactions of the yttrium-carbon cluster ions were very ion dependent with dehydrogenation of water and loss of carbon groups common modes of reaction. 

The results in the three preceding subsections conform fairly well to a consistent pattern. However, there are gaps and inconsistencies that require further thermochemical, and in some cases chemical, study. The series of solution enthalpies for the lanthanide trichlorides is satisfactory, but disagreements over the value for the enthalpy of solution of yttrium trichloride in water need resolving, and a modern value for scandium trichloride (at 25°C) would be welcome. The complete absence of enthalpies of solution of tribromides of the lanthanide elements and yttrium is regrettable, as is the lack of a value for scandium triiodide. 

The lanthanide fluorides Eire all sparingly soluble in water, as are the fluorides of yttrium and scEmdiiun. Thus, solubility information is generally presented in the form of the solubility product Ksp. 

The triiodides are slightly more soluble in water than the tribromides [Table XXI (269-276)] the published value for samarium triiodide looks suspiciously high. The addition of hydrogen iodide produces a large decrease in the solubility of yttrium triiodide, from 66.98 wt % in water to 4.90 wt % in 63.45 wt % HI (in both cases at 0°C) (269). Other lanthanide triiodides behave similarly (272-274). 

Solubilities of LaCl3-7H20 and of NdCl3-6H20 in acetone/water mixtures have been reported, and compared with those for chlorides of barium and of the alkali metals (323). For these trichlorides, the solubility increases as acetone is added to water up to about 15% acetone, then decreases (LaCl3 and NdCl3 are effectively insoluble in acetone itself). There is also some information, presented only in graphical form, on solubilities of praseodymium trichloride in water-rich methanol, ethanol, and ether mixtures (314), and one fact on yttrium trichloride in a water/ether mixture (264). 

Yttrium dissolves in weak acids and also dissolves in strong alkalis such as potassium hydroxide. It will also decompose in water. 

The measurement of stability constants of complexes of yttrium, lanthanide, and actinide ions with oxalate, citrate, edta, and 1,2-diaminocyclohexanetetra-acetate ligands has revealed that there is a slight increase in the stability of complexes of the /-electron elements, relative to the others. A series of citric acid (H cit) complexes of the lanthanides have been investigated by ion-exchange methods and the species [Ln(H2cit)]", [Ln(H2cit)2] , [Ln-(Hcit)], and [Ln(Hcit))2] were detected. Simple and mixed complexes of dl- and jeso-tartaric acid have been obtained with La " and Nd ions, and the stability constants of lactate, pyruvate, and x-alaninate complexes of Eu and Am " in water have been determined. 

Insoluble silica residues are removed by filtration. The solution now contains beryllium, iron, yttrium, and the rare earths. The solution is treated with oxalic acid to precipitate yttrium and the rare earths. The precipitate is calcined at 800°C to form rare earth oxides. The oxide mixture is dissolved in an acid from which yttrium and the rare earths are separated by the ion-exchange as above. Caustic fusion may be carried out instead of acid digestion to open the ore. Under this condition sihca converts to sodium sihcate and is leached with water. The insoluble residue containing rare earths and yttrium is dissolved in an acid. The acid solution is fed to an ion exchange system for separating thuhum from other rare earths. 

---