Chemical elements
  Vanadium
    Isotopes
    Energy
    Preparation
    Applications
    Physical Properties
    Chemical Properties
      Hypovanadous Oxide
      Vanadous Oxide
      Hypovanadic Oxide
      Vanadic Oxide
      Hypovanadous Fluoride
      Vanadous Fluoride
      Vanadium Tetrafluoride
      Vanadium Pentafluoride
      Vanadyl Difluoride
      Vanadium Oxytrifluoride
      Vanadium Dioxyfluoride
      Hypovanadous Chloride
      Vanadous Chloride
      Hypovanadic Chloride
      Divanadyl Chloride
      Vanadium Oxymonochloride
      Vanadyl Dichloride
      Vanadium Oxytrichloride
      Vanadium Oxydichloride
      Vanadous Bromide
      Hypovanadic Bromide
      Vanadium Oxymonobromide
      Vanadyl Dibromide
      Vanadium Oxytribromide
      Hydrated Vanadium Tri-iodide
      Vanadium Suboxide
      Hypovanadous Oxide
      Vanadous Oxide
      Hypovanadic Oxide
      Hypovanadates
      Intermediate Vanadium Oxides
      Vanado-vanadates
      Vanadium Pentoxide
      Orthovanadates
      Sodium Stannovanadates
      Vanadates
      Pyrovanadates
      Metavanadates
      Polyvanadates
      Double Vanadates
      Heteropoly-Acids with Vanadium
      Vanado-phosphates
      Molybdo-vanadophosphates
      Vanado-arsenates
      Molybdo-vanadoarsenates
      Tungsto-vanadoarsenates
      Molybdo-vanadates
      Tungsto-vanadates
      Uranyl-vanadates
      Molybdo-vanadosilicates
      Tungsto-vanadosilicates
      Vanado-selenites
      Vanado-tellurites
      Vanado-iodates
      Vanado-periodates
      Oxalo-vanadates
      Pervanadic Acid
      Pyropervanadates
      Orthopervanadates
      Vanadium Monosulphide
      Vanadium Trisulphide
      Vanadium Pentasulphide
      Vanadium Oxysulphides
      Hypovanadous Sulphate
      Vanadous Sulphate
      Vanadyl Sulphites
      Vanadyl Sulphates
      Vanadic Sulphates
      Vanadyl Dithionate
      Ammonium Orthothiovanadate
      Ammonium Pyroxyhexathiovanadate
      Sodium Orthoxytrithiovanadate
      Sodium Orthoxymonothiovanadate
      Vanadium Selenides
      Vanadyl Selenite
      Vanadyl Selenates
      Vanadium Subnitride
      Vanadium Mononitride
      Vanadium Dinitride
      Alkali Vanadyl Nitrites
      Vanadium Nitrates
      Vanadyl Hypophosphite
      Vanadyl Phosphates
      Vanadous Pyrophosphate
      Vanadyl Arsenates
      Vanadium Carbide
      Vanadyl Cyanide
      Potassium Vanadocyanide
      Potassium Vanadicyanide
      Vanadium Ferrocyanides
      Ammonium Vanadyl Thiocyanate
      Vanadium Subsilicide
      Vanadium Disilicide
      Vanadium Boride
    Detection, Estimation
    PDB 1b8j-2i4e
    PDB 2jhr-6rsa

Vanadous Sulphate, V2(SO4)3






Vanadous Sulphate or vanadium sesquisulphate, V2(SO4)3, is readily obtained in solution by reducing a solution of vanadium pentoxide in sulphuric acid either by means of magnesium or electrolytically. The solid has been obtained by slowly heating to 180° C. in an atmosphere of carbon dioxide a solution of green acid vanadous sulphate, V2(SO4)3.H2SO4.12H2O (see next page), in water which has been slightly acidified with sulphuric acid. Ammonium vanadous sulphate, (NH4)V(SO4)2, can also be used. Vanadous sulphate forms a micro-crystalline, yellow powder, which is insoluble in water; it decomposes on being heated in air with formation of vanadium pentoxide. By the action of concentrated sulphuric acid on vanadic acetate several green or yellowish- green hydrates of vanadous sulphate have recently been prepared: V2(SO4)3.3H2O; V2(SO4)3.xH2O; V2(SO4)3.9H2O; V2(SO4)3.10-11H2O; of these the tri- and tetra-hydrates appear to correspond in general behaviour to the green tri- and tetra-hydrates of chromium sulphate.


Acid Vanadous Sulphates and double vanadous sulphates

Electrolytic reduction of solutions of vanadyl sulphate, VOSO4, has given two green, crystalline, acid vanadous sulphates, according to the amount of sulphuric acid also added:

HV(SO4)2.4H2O or V2(SO4)3.H2SO4.8H2O.
HV(SO4)2.6H2O or V2(SO4)3.H2SO4.12H2O.

By electrolysing a solution of ammonium metavanadate in sulphuric acid instead of vanadyl sulphate, the ammonium salts of these acid sulphates are obtained, viz. NH4V(SO4)2.4H2O and NH4V(SO4)2.6H2O. The latter is referred to again below. These acids (and their salts) differ from one another in their general properties, for instance in the acidity of their solutions, in the electrical conductivity of their solutions, and in the ease with which they undergo oxidation. From a study of their analogy with the corresponding compounds of chromium, the constitution [V(SO4)(H2O)4]SO4H has been ascribed to the tetrahydrate acid, and the constitution [V(SO4)2(H2O)2]H.4H2O to the hexahydrate acid. By the action of sulphuric acid in varying quantity on solutions of vanadic acetate in glacial acetic acid, compounds having the compositions HV(SO4)2.5H2O and HV(SO4)2.8H2O have been prepared; dehydration of these gives rise to HV(SO4)2.2H2O and HV(SO4)2. The ammonium salt of the pentahydrate acid, NH4V(SO4)2.5H2O or [V(H2O)4](SO4)(SO4NH4)-H2O, has also been isolated.

When the reduction of the vanadyl sulphate is allowed to proceed in the presence of the sulphates of the alkali metals or of thallium, two series of double salts are obtained, the composition of which again varies with the amount of sulphuric acid present and with the other conditions.

Series I

Series I. has the general formula RV(SO4)2.12H2O or R2SO4. V2(SO4)3.24H2O, which corresponds to the composition of the alums formed by the metals of Group III. and other groups. The vanadium alums are very similar in their behaviour to ferric, chromium and aluminium alums. They crystallise in regular, pentagonal hemihedra, varying in colour, with increase in atomic weight of the alkali metal, from the violet of the ammonium alum to the ruby-red of the caesium alum. The following table includes those alums which have hitherto been prepared:

Vanadium Alums

9° C.
FormulaSolubility in 2 litres of Water at 25° C. (gram- mols.).Temperature at which Crystals Melt in their Water of Crystallisation.ColourDensity
V2(SO4)3.(NH4)2SO4.24H2O1.21020° C.Violet1.687
V2(SO4)3.Na2SO4.24H2O. . .45° C. . .. . .
V2(SO4)3.K2SO4.24H2O3.480Greenish-violet1.782
V2(SO4)3.Rb2SO4.24H2O0.17764° C.Bluish-violet1.915
V2(SO4)3.Cs2SO4.24H2O0.02082° C.Ruby-red2.033
V2(SO4)3.Tl2SO4.24H2O0.57348° C.Reddish-violet2.342


Bultemann observed that vanadium ammonium alum separates out in blue crystals from a solution containing sulphuric acid, but from solutions containing a weak acid, or from neutral solutions, red crystals are obtained. (The chromium alums can also be prepared in differently coloured modifications.) The analytical data, melting-point, electrical conductivity, rate of efflorescence, and general behaviour of both kinds of crystals are identical, so that it is difficult to ascribe different constitutions to them. Meyer and Markowitz have shown that both forms separate out when the molecular proportion of sulphuric acid in the solution is less than that theoretically required, and attribute the red colour to the presence of traces of vanadous oxide, V2O3, or its hydroxide, V(OH)3. Vanadium rubidium and vanadium caesium alums behave in the same way. A vanadium guanidine alum has also been prepared.

The general constitutional formula for the vanadium alums is [V(H4O2)6](SO4)(SO4R), which differs from the formula for other double vanadium sulphates in that the sulphato groups are not attached to the nuclear vanadium atom.

Series II

Series II. - This appears to comprise the salts of the acid HV(SO4)2.6H2O mentioned above, since they can be obtained by boiling this acid with the respective alkali sulphates. Only two members of the class have been examined:

(NH4)2SO4.V2(SO4)3.12H2O or (NH4)V(SO4)2.6H2O.

(Rb)2SO4.V2(SO4)3.12H2O or RbV(SO4)2.6H2O. By heating the alkali vanadyl sulphates, compounds have been obtained which can be looked upon either as the dehydrated forms of members of this series, or as salts of the acid sulphate, HV(SO4)2, mentioned above:

(NH4)V(SO4)2 or (NH4)2SO4.V2(SO4)3.
NaV(SO4)2 or Na2SO42.2(SO4)3.
KV(SO4)2 or K2SO4.V2(SO4)3.

These have the general formula [V(SO4)2]R.

It is of some interest to note that iron and aluminium also give rise to double sulphates in which the number of molecules of water is less than in the alums.
© Copyright 2008-2012 by atomistry.com