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The following chart shows the solubility of various ionic compounds in water at 1 atm pressure and room temperature (approx. 25 °C, 298.15 K). "Soluble" means the ionic compound doesn't precipitate, while "slightly soluble" and "insoluble" mean that a solid will precipitate; "slightly soluble" compounds like calcium sulfate may require heat to precipitate.
The tables below provides information on the variation of solubility of different substances (mostly inorganic compounds) in water with temperature, at one atmosphere pressure. Units of solubility are given in grams of substance per 100 millilitres of water (g/100 ml), unless shown otherwise. The substances are listed in alphabetical order.
The Pourbaix diagram for vanadium in water, which shows the redox potentials between various vanadium species in different oxidation states [39] Vanadium(V) forms various peroxo complexes, most notably in the active site of the vanadium-containing bromoperoxidase enzymes. The species VO(O 2)(H 2 O) 4 + is stable in acidic solutions.
Vanadium pentoxide is a commercially important catalyst for the production of sulfuric acid, a reaction that exploits the ability of vanadium oxides to undergo redox reactions. [2] The vanadium redox battery utilizes all four oxidation states: one electrode uses the +5/+4 couple and the other uses the +3/+2 couple. Conversion of these oxidation ...
Vanadium(V) oxide (vanadia) is the inorganic compound with the formula V 2 O 5. ... it is slightly water soluble, giving a pale yellow, acidic solution.
VCl 3 dissolves in water to give the aquo complexes. From these solutions, the hexahydrate [VCl 2 (H 2 O) 4]Cl. 2H 2 O crystallizes. In other words, two of the water molecules are not bound to the vanadium, whose structure resembles the corresponding Fe(III) derivative. Removal of the two bound chloride ligands gives the green hexaaquo complex ...
Like other charge-neutral acetylacetonate complexes, it is not soluble in water. ... The complex is generally prepared from vanadium(IV), e.g. vanadyl sulfate: [1]
Some hydroxides of non-metallic elements are soluble in water; they are not included in the following table. Examples cited by Baes and Mesmer (p. 413) include hydroxides of Gallium(III), Indium(III), Thallium(III), Arsenic(III), Antimony(III) and Bismuth(III). Most hydroxides of transition metals are classified as being "insoluble" in water.