27774-13-6 Usage
Uses
The dihydrate is a mordant in dyeing and printing fabrics; used in preparing aniline black; a colorant in ceramics to form blue and green glazes; used in making colored glass; and a reducing agent.
Preparation
Vanadyl sulfate is prepared by passing sulfur dioxide through a cold solution of vanadium pentoxide in sulfuric acid, followed by crystallization:
V2O5 + H2SO4 + H2O + SO2 → 2VOSO4 + 2H2O
Chemical Properties
Vanadyl sulfate is a pale blue crystalline powder.
Odorless.
Physical properties
The dihydrate, VOSO4?2H2O is a blue black crystalline powder, soluble in water.
General Description
A blue crystalline solid. Very soluble in water. Denser than water. Contact may irritate skin, eyes, and mucous membranes. May be toxic by ingestion, inhalation and skin absorption.
Reactivity Profile
Vanadyl sulfate has weak oxidizing or reducing powers. Redox reactions can however still occur.
Health Hazard
Highly toxic, may be fatal if inhaled, swallowed or absorbed through skin. Avoid any skin contact. Effects of contact or inhalation may be delayed. Fire may produce irritating, corrosive and/or toxic gases. Runoff from fire control or dilution water may be corrosive and/or toxic and cause pollution.
Fire Hazard
Non-combustible, substance itself does not burn but may decompose upon heating to produce corrosive and/or toxic fumes. Containers may explode when heated. Runoff may pollute waterways.
Flammability and Explosibility
Nonflammable
Safety Profile
A poison and an
inhalation hazard. Poison by intravenous,
intraperitoneal, and subcutaneous routes.
Mutation data reported. When heated to
decomposition it emits toxic fumes of VOx
and SOx. See also SULFATES and
VANADIUM COMPOUNDS.
Potential Exposure
Vanadyl sulfate is used as a fixative
for textile dyes, a colorant for glass and ceramics; a reducing
agent and a catalyst.
Shipping
UN2931 Vanadyl sulfate, Hazard Class: 6.1;
Labels: 6.1-Poisonous materials.
Incompatibilities
Vanadyl sulfate has weak oxidizing or
reducing powers. Redox reactions can however still
occur. Incompatible with oxidizers (chlorates, nitrates,
peroxides, permanganates, perchlorates, chlorine, bromine,
fluorine, etc.); contact may cause fires or explosions. Keep
away from alkaline materials, strong bases, strong acids,
oxoacids, epoxides. Vanadyl sulfate may attack metals; sulfates
react with aluminum, magnesium.
Check Digit Verification of cas no
The CAS Registry Mumber 27774-13-6 includes 8 digits separated into 3 groups by hyphens. The first part of the number,starting from the left, has 5 digits, 2,7,7,7 and 4 respectively; the second part has 2 digits, 1 and 3 respectively.
Calculate Digit Verification of CAS Registry Number 27774-13:
(7*2)+(6*7)+(5*7)+(4*7)+(3*4)+(2*1)+(1*3)=136
136 % 10 = 6
So 27774-13-6 is a valid CAS Registry Number.
InChI:InChI=1/H2O4S.2H2O.V/c1-5(2,3)4;;;/h(H2,1,2,3,4);2*1H2;/q;;;+3/p-2
27774-13-6Relevant articles and documents
α-VOSO4:A 2D-ferromagnet
Lezama, L.,Villeneuve, G.,Marcos, M. D.,Pizarro, J. L.,Hagenmuller, P.
, p. 899 - 902 (1989)
A reexamination of the magnetic behavior of vanadyl sulfate α-VOSO4 shows that the main magnetic interaction occurs within the layers through |SO42-| anions. The exchange constant is found to be positive (J/k = + 1.5 K) involving ferromagnetic couplings in contrast to vanadyl phosphates which exhibit nearly the same geometry but whose exchange interactions are antiferromagnetic. An explanation is proposed, taking into account both bond angles and nature of the counterion.
Lithium electrochemical intercalation in β-VOSO4
Gaubicher,Chabre,Angenault,Lautie,Quarton
, p. 34 - 38 (2008/10/08)
A new low-temperature route for β-VOSO4 synthesis is proposed, involving reduction in sulphuric acid in the presence of sulphur. Lithium intercalation has been performed on this material, both chemically and electrochemically and the compounds have been characterized by XRD as well as IR and Raman spectroscopy. From potentio-dynamic and galvano-static electrochemical studies it is shown that intercalation occurs in two steps, firstly with a structural change at 2.84 V vs. Li metal, then in a solid solution domain. The process appears partly reversible and the system is shown to present a good cycling behavior on almost 0.6 e- per transition metal. From these results it appears that the energy of redox transition metal couples involving VO2+ structural units in octahedral coordination is between those observed in oxides and in M2(XO4)3 (X = S, P, As) compounds, respectively.
