1304-29-6 Usage
Description
Barium peroxide, is a grayish-white powder that is slightly soluble in water. Barium peroxide is a dangerous fire and explosion risk in contact with organic materials and decomposes around 1450°F (787°C). It is also toxic by ingestion, is a skin irritant, and should be kept cool and dry in storage. The four-digit UN identification number is 1449. The primary uses of barium peroxide are in bleaching, in thermal welding of aluminum, as an oxidizing agent, and in the dyeing of textiles.
Chemical Properties
Barium peroxide is a grayish-white powder.
Physical properties
BaO2 is an iron gray or white powder. It is slowly
decomposed in air, forming the hydroxide and oxygen.
It does not dissolve in water, but can slowly hydrolyze,
forming hydrogen peroxide in solution. Barium peroxide is a strong oxidizing agent and will explode if direct contact with organic matter occurs. Therefore, barium peroxide is always diluted to form a slurry before usage.
Barium peroxide is a strong oxidizing agent that is
used for bleaching. Barium peroxide contains O22-
subunits wherein the oxygen atoms bond to each other
as well as to the barium.
Uses
Different sources of media describe the Uses of 1304-29-6 differently. You can refer to the following data:
1. Bariumperoxide is used as a hydrogen peroxide source
and oxygen oxidant, as well as a bleaching agent. Its main
usage has been for making hydrogen peroxide and
oxygen, in organic syntheses, fabric printing and dyeing.
Barium peroxide is available commercially, primarily
as the oxctahydrate (which is the more stable form of
this peroxide).
2. Barium peroxide (BaO2) is a grayish-white dry powder that makes an excellent bleaching agent
that can be stored in paper packages. Its bleaching qualities are released when mixed with water.
3. Bleaching animal substances, vegetable fibers and straw; glass decolorizer; manufacture of H2O2 and oxygen; dyeing and printing textiles; with powdered aluminum in welding; in cathodes; in igniter compositions. Oxidizing agent in organic synthesis.
Production Methods
Barium peroxide, BaO2, was the first-known peroxo compound. It was used until mid-1900 in the manufacture of oxygen by the Brin process and of hydrogen peroxide by the Thenard reaction.
Definition
barium peroxide: A dense offwhitesolid, BaO2, prepared by carefullyheating barium oxide inoxygen; r.d. 4.96; m.p. 450°C. It is used as a bleaching agent. Withacids, hydrogen peroxide is formedand the reaction is used in the laboratorypreparation of hydrogen peroxide.
Preparation
Barium peroxide is best prepared by reacting barium
nitrate with sodium peroxide in a cold solution:
Ba(NO3)2＋Na2O2＋xH2O→BaO2·xH2O＋2NaNO3
The hydrated form is usually the octahydrate. If the
anhydrate is desired, the hydrated peroxide is dried
and then sintered at 350°C for 10 min or less:
4BaO2·xH2O＋ heat→2BaO＋2BaO2＋xH2O＋O2
About equal amounts of oxide and peroxide form.
The ratio is a function of the time and temperature of
heating. To separate the two forms, the heated mass is
plunged into a large volume of water where the
hydroxide is formed. The peroxide is insoluble whereas
the hydroxide is soluble, allowing the separation of the
two by filtration. The peroxide is then vacuum dried.
General Description
A grayish-white granular solid. Insoluble in water. Noncombustible, but accelerates the burning of combustible material. Mixture with finely divided combustible material may be explosive. Mixtures with combustible material may be ignited by friction or contact with moisture.
Air & Water Reactions
Decomposed by water. Insoluble in water.
Reactivity Profile
Barium peroxide is a strong oxidizing agent. Contact with water can produce a temperature and oxygen concentration high enough to ignite organic materials [Bretherick's, 5th ed., 1995, p. 94]. Reacts explosively with acetic anhydride due to the formation of acetyl peroxide [Rust, 1948, p. 337]. Ignites when mixed with powdered aluminum, powdered magnesium or calcium-silicon alloys. Wood may ignite with friction from the peroxide. Decomposes when heated to 700°C to produce barium oxide and pure oxygen [Sax, 9th ed., 1996, p. 317]. Forms highly reactive mixtures with fuel-type materials.
Hazard
Oxidizing material. Fire and explosion risk
in contact with organic materials. Keep cool and
dry. Toxic by ingestion, skin irritant.
Health Hazard
Inhalation causes irritation of mucous membranes, throat, and nose. Contact with eyes or skin causes severe burns. Ingestion causes excessive salivation, vomiting, colic, diarrhea, convulsive tremors, slow, hard pulse, and elevated blood pressure; hemorrhages may occur in the stomach, intestines, and kidneys; muscular paralysis may follow.
Fire Hazard
Behavior in Fire: Can increase intensity of fire.
Flammability and Explosibility
Notclassified
Safety Profile
A poison via
subcutaneous route. A powerful oxidtzer.
Explodes on contact with acetic anhydride.
Ignites when mixed with calcium-silicon
alloys, powdered aluminum, powdered
magnesium, water + organic compounds.
Mixtures with propane react violently when
heated. The powder ignites when heated to
265℃ with selenium. Wood ignites with
friction from the peroxide. Incompatible
with H2S, water, peroxyformic acid,
hydroxylamine solution, mixture of (Mg +
Zn + Ba(NO3)2), and organic matter. See
also BARIUM COMPOUNDS (soluble)
and PEROXIDES, INORGANIC.
Potential Exposure
Is used as a bleaching agent; in making
hydrogen peroxide, oxygen; in aluminum welding; in
textile dyeing and for bleaching fibers; animal substances.
Shipping
UN1449 Barium peroxide, Hazard Class: 5.1;
Labels: 5.1—Oxidizer, 6.1—Poisonous materials.
Incompatibilities
A strong oxidizer. Keep away from
organic and combustible materials (such as wood, paper,
oil, fuels, and other easily oxidized materials) and peroxyformic
acid, hydrogen sulfide and hydroxylamine solutions,
since violent reactions occur.
Waste Disposal
Dispose of contents and container
to an approved waste disposal plant. All federal,
state, and local environmental regulations must be
observed. Contact your local or federal environmental protection
agency for specific recommendations.
Check Digit Verification of cas no
The CAS Registry Mumber 1304-29-6 includes 7 digits separated into 3 groups by hyphens. The first part of the number,starting from the left, has 4 digits, 1,3,0 and 4 respectively; the second part has 2 digits, 2 and 9 respectively.
Calculate Digit Verification of CAS Registry Number 1304-29:
(6*1)+(5*3)+(4*0)+(3*4)+(2*2)+(1*9)=46
46 % 10 = 6
So 1304-29-6 is a valid CAS Registry Number.
InChI:InChI=1/Ba.O2/c;1-2/q+2;-2/rBaO2/c1-2-3-1
1304-29-6Relevant articles and documents
Enhancement of Tc by Sr substitution for Ba in Hg-2212 superconductor
Toulemonde,Odier
, p. 152 - 159 (2004)
The Ba substitution by Sr has been studied in two Hg-2212 series: Hg 2(Ba1-ySry)2YCu2O 8-δ and Hg2(Ba1-ySry) 2(Y0.80Ca0.20)Cu2O 8-δ. In both series a Tc enhancement of about 40 K is observed when Sr substitutes Ba from y=0 to 1.0. The y=0 compound of the first series is the non-superconducting Hg2Ba2YCu 2O8-δ prototype. In the second series, this y=0 compound is already superconducting at 21 K. Indeed the members of this series present a higher charge carrier density in their CuO2 superconducting planes than their homologues of the first series due to the doping introduced by the substitution of 20% of Y by Ca. The compounds of both series were synthesized in high pressure (3.5 GPa)-high temperature (950-1050 °C) conditions. In both cases Sr substitution was successful up to the full replacement of Ba (y=1.0). The Hg-2212 phases were characterized by XRD, SEM, EDX and a.c. susceptibility.
Jasim, Fadhil,Jameel, Ibtisam
, p. 37 - 44 (1987)
Dissanayake, Dhammike,Kharas, Karl, C. C.,Lunsford, Jack H.,Rosynek, Michael P.
, p. 652 - 663 (1993)
Struve, H.
, p. 22 - 25 (1872)
Synthesis, characterization and thermal decomposition kinetics of barium(II)bis(oxalato)barium(II)dihydrate and lead(II)bis(oxalato)lead(II)monohydrate
Deb,Baruah,Sen Sarma,Dass
, p. 129 - 139 (1999)
Barium(II)bis(oxalato)barium(II)dihydrate (BOD), Ba[Ba(C2O4)2]·2H2O and lead(II)bis(oxalato)lead(II)monohydrate (LOM), Pb[Pb(C2O4)2]·H2O have been synthesized and characterized by elemental analysis, conductance measurements, IR spectral, reflectance and X-ray powder diffraction studies. Thermal decomposition studies (TG, DTG and DTA) in air showed that at ca. 1000°C, a mixture of BaO2 and BaCO3 is generated from the compound, BOD, through the formation of BaO2 and BaC2O4 at around 514°C as intermediates. LOM gave Pb2O3 as final product at ca. 390°C. DSC study in nitrogen showed a different decomposition pattern from that in air for both compounds. Using seven mechanistic equations, the rate controlling process of the dehydration and decomposition mechanism of BOD is inferred to be one- and three-dimensional diffusion, respectively. The decomposition mechanism of LOM is a phase boundary reaction having cylindrical symmetry. Some of the decomposition products were identified by analytical, IR spectral and X-ray powder diffraction studies. A tentative reaction mechanism for the thermal decomposition of both the complexes is proposed.
Characterization studies of physicochemical modifications conceded by equimolar-mixed chromia and barium carbonate powders as a function of temperature
Al-Hajji,Hasan,Zaki
, p. 8 - 14 (2009)
Occurrence and products of solid/solid interactions in equimolar-mixed BaCO3 and Cr2O3 powders were examined isothermally (700-1000 °C) and non-isothermally (25-1200 °C) under different gas atmospheres, employing thermogra
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