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Barium

Barium Suppliers list
Company Name: Mainchem Co., Ltd.
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Products Intro: Product Name:Barium
CAS:7440-39-3
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Products Intro: Product Name:Barium rod (99+%, Sr-<1.6%)
CAS:7440-39-3
Purity:(99+%, Sr-<1.6%) Package:100g;500g
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Products Intro: Product Name:BariuM
CAS:7440-39-3
Purity:99% HPLC Package:1Mg ; 5Mg;10Mg ;100Mg;250Mg ;500Mg ;1g;2.5g ;5g ;10g
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Products Intro: Product Name:BariuM rod, 22MM (0.9in) dia x 450MM (17.7in), 99+% (Metals basis), Sr |<0.8%
CAS:7440-39-3
Package:1pc Remarks:041302
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Products Intro: Product Name:BariuM
CAS:7440-39-3
Purity:99.9% Package:100g,25g
Barium Basic information
Defination Occurrence Uses
Product Name:Barium
Synonyms:Barium, Oil based standard solution, Specpure(R), Ba 1000μg/g;Barium, plasma standard solution, Specpure(R), Ba 10,000μg/ml;Barium, plasma standard solution, Specpure(R), Ba 1000μg/ml;Barium, AAS standard solution, Specpure(R), Ba 1000μg/ml;Barium, Oil based standard solution, Specpure(R), Ba 5000μg/g;Barium rod, 22mm (0.9in) dia x 450mm (17.7in), 99+% (metals basis), Sr ≤0.8%;Barium compounds, soluble (as Ba);BARIUM, 99.90%, DENDRITIC PIECES IN MINERAL OIL
CAS:7440-39-3
MF:Ba
MW:137.33
EINECS:231-149-1
Product Categories:Alkali MetalsMetal and Ceramic Science;Barium;Metals;Reduction;Synthetic Reagents;AA Standard SolutionsAlphabetic;AAS;B;BA - BHSpectroscopy;ChlorideSpectroscopy;Matrix Selection;Reference/Calibration Standards;Single Solution;Standard Solutions;Inorganics;metal or element
Mol File:7440-39-3.mol
Barium Structure
Barium Chemical Properties
Melting point 725 °C(lit.)
Boiling point 1640 °C(lit.)
density 3.6 g/mL at 25 °C(lit.)
storage temp. water-free area
form rod
color Silver-gray
resistivity50.0 μΩ-cm, 20°C
Water Solubility soluble with H2 evolution in cold H2O and hot H2O; slightly soluble alcohol; insoluble benzene [CRC10]
Sensitive air sensitive, moisture sensitive
Merck 13,967
Stability:Stability Reacts vigorously or violently with acids, water, tetrachloromethane, small halogenated hydrocarbons. Should be stored under an inert material such as petroleum ether to exclude air. Flammable.
CAS DataBase Reference7440-39-3(CAS DataBase Reference)
Safety Information
Hazard Codes C,Xi,F
Risk Statements 25-26-34-36/37/38-14/15-11
Safety Statements 23-26-36-36/37/39-45-43-36/37-16
RIDADR UN 3264 8/PG 3
WGK Germany 3
RTECS CQ8370000
TSCA Yes
HS Code 2805 19 10
HazardClass 8
PackingGroup III
MSDS Information
ProviderLanguage
SigmaAldrich English
ACROS English
ALFA English
Barium Usage And Synthesis
DefinationSymbol Ba; atomic number 56; atomic weight 137.327; a Group IIA (Group 2) alkaline earth element; electronic configuration [Xe]s2; valence state +2; ionic radius of Ba2+ in crystal (corresponding to coordination number 8) 1.42 Å; first ionization potential 10.00eV; stable isotopes and their percent abundances: Ba–138 (71.70), Ba–137 (11.23), Ba–136 (7.85), Ba–135 (6.59), Ba–134 (2.42); minor isotopes: Ba–130 (0.106) and Ba–132 (0.101); also twenty-two radioisotopes are known.
OccurrenceBarium was discovered in 1808 by Sir Humphrey Davy. Its abundance in the earth’s crust is about 0.0425% (425 mg/kg). The element also is found in sea water at trace concentration, 13 μg/L. It occurs in the minerals barite or heavy spar (as sulfate) and witherite (as carbonate).
UsesThe most important use of barium is as a scavenger in electronic tubes. The metal, often in powder form or as an alloy with aluminum, is employed to remove the last traces of gases from vacuum and television picture tubes. Alloys of barium have numerous applications. It is incorporated to lead alloy grids of acid batteries for better performance; and added to molten steel and metals in deoxidizing alloys to lower the oxygen content. Thin films of barium are used as lubricant suitable at high temperatures on the rotors of anodes in vacuum X-ray tubes and on alloys used for spark plugs. A few radioactive isotopes of this element find applications in nuclear reactions and spectrometry.
DescriptionBarium is a silvery-white metal. It exists in nature only in ores containing mixtures of elements. The important combinations are the peroxide, chloride, sulphate, carbonate, nitrate, and chlorate. The pure metal oxidises readily and reacts with water emitting hydrogen. It combines with other chemicals such as sulphur or carbon and oxygen to form barium compounds. Barium compounds are used by the oil and gas industries to make drilling muds. Barium attacks most metals with the formation of alloys; iron is the most resistant to alloy formation. Barium forms alloys and intermetallic compounds with lead, potassium, platinum, magnesium, silicon, zinc, aluminium, and mercury. Barium compounds exhibit close relationships with the compounds of calcium and strontium, which are also alkaline earth metals. Twenty-five barium isotopes have been identified, 138Ba being the most abundant, and the others are unstable isotopes with half-lives ranging from 12.8 days for 140Ba to 12 s for 143Ba. Two of these isotopes, 131Ba and 139Ba, are used in research as radioactive tracers. The general population is exposed to barium through air, drinking water, and food.
Chemical Propertiesyellow-white, slightly lustrous solid
Chemical PropertiesBarium is a silvery-white metal. It exists in nature only in ores containing mixtures of ele- ments. The important combinations are peroxide, chloride, sulfate, carbonate, nitrate, and chlorate. The pure metal oxidizes readily and reacts with water, emitting hydrogen. It com- bines with other chemicals such as sulfur or carbon and oxygen to form barium compounds. Barium compounds are used by the oil and gas industries to make drilling muds. Barium attacks most metals with the formation of alloys; iron is the most resistant to alloy formation. Barium forms alloys and intermetallic compounds with lead, potassium, platinum, mag- nesium, silicon, zinc, aluminum, and mercury. Barium compounds exhibit close relation- ships with the compounds of calcium and strontium, which are also alkaline earth metals. Doctors sometimes use barium sulfate to perform medical tests and to take x-rays of the gastrointestinal tract. Twenty-i ve barium isotopes have been identii ed. 138Ba is the most abundant; the others are unstable isotopes with half-lives ranging from 12.8 days for 140Ba to 12 sec for 143Ba. Two of these isotopes, 131Ba and 139Ba, are used in research as radioactive tracers. The general population is exposed to barium through air, drinking water, and food.
Chemical PropertiesBarium is a flammable, silver white or yellowish metal in various forms including powder. Barium may ignite spontaneously in air in the presence of moisture, evolving hydrogen.
HistoryBaryta was distinguished from lime by Scheele in 1774; Barium was discovered by Sir Humphrey Davy in 1808. It is found only in combination with other elements, chiefly in barite or heavy spar (sulfate) and witherite (carbonate) and is prepared by electrolysis of the chloride. Large deposits of barite are found in China, Germany, India, Morocco, and in the U.S. Barium is a metallic element, soft, and when pure is silvery white like lead; it belongs to the alkaline earth group, resembling calcium chemically. The metal oxidizes very easily and should be kept under petroleum or other suitable oxygen-free liquids to exclude air. It is decomposed by water or alcohol. The metal is used as a “getter” in vacuum tubes. The most important compounds are the peroxide (BaO2), chloride, sulfate, carbonate, nitrate, and chlorate. Lithopone, a pigment containing barium sulfate and zinc sulfide, has good covering power, and does not darken in the presence of sulfides. The sulfate, as permanent white or blanc fixe, is also used in paint, in X-ray diagnostic work, and in glassmaking. Barite is extensively used as a weighting agent in oilwell drilling fluids, and also in making rubber. The carbonate has been used as a rat poison, while the nitrate and chlorate give green colors in pyrotechny. The impure sulfide phosphoresces after exposure to the light. The compounds and the metal are not expensive. Barium metal (99.2 + % pure) costs about $3/g. All barium compounds that are water or acid soluble are poisonous. Naturally occurring barium is a mixture of seven stable isotopes. Thirty-six other radioactive isotopes and isomers are known to exist.
UsesAlloys with Al or Mg as "getters" to remove residual gases from vacuum systems and electronic tubes. Deoxidizer for steel and other metals. Carrier for radium. The b- and g-radiation emitted by 140Ba + 140La makes a large contribution to the activity of the fission products of uranium rods during the first few weeks after their withdrawal from the reactor. The emissions from 133Ba and 137mBa as standards in g-spectrometry: Haissinsky, Adloff, Radiochemical Survey of the Elements (Elsevier, 1965) pp 12-14.
DefinitionAlkaline-earth element of atomic number 56, group IIA of periodic table; aw 137.34; valence 2; 7 stable isotopes.
General DescriptionBarium alloy, pyrophoric is mixture of barium and other metals or nonmetallic elements to improve the specific usefulness of barium. Barium alloys are a solid and can ignite spontaneously in contact with air. Barium is toxic and products given off in fire could be very toxic.
Air & Water ReactionsFinely divided metal powder is pyrophoric, ignites spontaneously in air [Bretherick 1979 p. 170-171]. Alloys containing a substantial proportion of barium rapidly decomposed water. The heat of the reaction is sufficient that the evolved hydrogen may ignite [Lab. Govt. Chemist 1965].
Reactivity ProfileAlloys containing a substantial amount of barium react violently with acids [Lab. Gov. Chemist 1965].
HazardFlammable (pyrophoric) at room tem- perature in powder form; store under inert gas, petroleum, or other oxygen-free liquid. When heated to approximately 200C in hydrogen, barium reacts violently, forming BaH2. Eye, skin, and gas- trointestinal irritant, and muscular stimulant. Ques- tionable carcinogen.
Health HazardThe health effects of barium compounds depend on how well the compound dissolves in water or in the stomach contents. Barium compounds that do not dissolve well, such as barium sulfate, are considered not harmful. Barium carbonate dust and barium oxide dust have been reported to be a bronchial irritant. While barium carbonate is a dermal irritant, barium oxide is a nasal irritant. Occupational workers exposed to barium dust, usually in the form of barium sulfate or carbonate, often develop a benign pneumoco- niosis also called “baritosis.” The effect of baritosis has been shown to be reversible and has not caused any kind of severe pulmonary adverse effect. Barium compounds that do not dissolve in water are considered safe. However, the health effects of the different barium compounds depend on the degree of their water solubility. The compounds that dissolve well in water are known to cause harmful health effects when ingested in high levels. Symptoms of poisoning include stomach irritation, brain swelling, muscle weak- ness, liver and kidney damage, adverse effects to the heart, increased blood pressure, changes in heart rhythm, effects on the spleen, difi culties in breathing, and swelling of the brain. Exposures to high concentrations of barium through food and drinking water cause gastrointestinal disturbances. Barium causes vomiting, abdominal cramps, diar- rhea, difi culties in breathing, increased or decreased blood pressure, numbness around the face, and muscle weakness, changes in heart rhythm or paralysis, and possibly death. Animals exposed to barium over long periods showed kidney damage, decreased body weight, and fatal injury. Ingestion of large amounts of barium chloride (2 and 4 g) causes fatal injury, because barium ions paralyze the heart. Acute poisoning with barium causes nausea and diarrhea, cardiac problems, and muscular spasms, as well as cardiac arrest. Thus, barium, at concentrations normally found in our environment, does not pose any signii cant risk for the general population. However, for specii c subpopulations and under conditions of high barium exposure, the potential for adverse health effects should be taken into account.
Health HazardFire will produce irritating, corrosive and/or toxic gases. Inhalation of decomposition products may cause severe injury or death. Contact with substance may cause severe burns to skin and eyes. Runoff from fire control may cause pollution.
Fire HazardFlammable/combustible material. May ignite on contact with moist air or moisture. May burn rapidly with flare-burning effect. Some react vigorously or explosively on contact with water. Some may decompose explosively when heated or involved in a fire. May re-ignite after fire is extinguished. Runoff may create fire or explosion hazard. Containers may explode when heated.
Safety ProfileWater and stomach acids solubilize barium salts and can cause poisoning. Symptoms are vomiting, colic, diarrhea, slow irregular pulse, transient hypertension, and convulsive tremors and muscular paralysis. Death may occur in a few hours to a few days. Half-life of barium in bone has been estimated at 50 days. Dust is dangerous and explosive when exposed to heat, flame, or chemical reaction. Violent or explosive reaction with water, CCh, fluorotrichloromethane, trichloroethylene, and C2Cl4. Incompatible with acids, C2CLF3, C2H2FCl3, C2HCl3 and water, 1,1,2- trichlorotrifluoroethane, and fluorotrichloroethane. The powder may ignite or explode in air or other oxidizing gases. See also BARIUM COMPOUNDS.
Potential ExposureMetallic barium is used for removal of residual gas in vacuum tubes and in alloys with nickel, lead, calcium, magnesium, sodium, and lithium. Barium compounds are used in the manufacture of lithopone (a white pigment in paints), chlorine, sodium hydroxide, valves, and green flares; in synthetic rubber vulcanization; X-ray diagnostic work, glassmaking, papermaking, beet-sugar purification; animal and vegetable oil refining. They are used in the brick and tile, pyrotechnics, and electronics industries. They are found in lubricants, pesticides, glazes, textile dyes and finishes; pharmaceuticals; in cements which will be exposed to saltwater; and barium is used as a rodenticide, a flux for magnesium alloys, a stabilizer and mold lubricant in the rubber and plastics industries, an extender in paints; a loader for paper, soap, rubber, and linoleum; and as a fire extinguisher for uranium or plutonium fires.
First aidMove victim to fresh air. Call 911 or emergency medical service. Give artificial respiration if victim is not breathing. Do not use mouth-to-mouth method if victim ingested or inhaled the substance; give artificial respiration With the aid of a pocket mask equipped with a one-way valve or other proper respiratory Medical device. Administer oxygen if breathing is difficult. Remove and isolate contaminated clothing and shoes. In case of contact with substance, immediately flush skin or eyes with running water for at least 20 minutes. For minor skin contact, avoid spreading material on unaffected skin. Keep victim warm and quiet. Effects of exposure (inhalation, ingestion or skin contact) to substance may be delayed. Ensure that medical personnel are aware of the material(s) involved and take precautions to protect themselves. Medical observation is recommended for 24 to 48 hours after breathing overexposure, as pulmonary edema may be delayed. As first aid for pulmonary edema, a doctor or authorized paramedic may consider administering a drug or other inhalation therapy.
ShippingUN1400 Barium, Hazard Class: 4.3; Labels: 4.3—Dangerous when wet material. UN1854 Barium alloys, pyrophoric, Hazard Class: 4.2; Labels: 4.2—Spontaneously combustible material. UN1564 Barium compound, n.o.s., Hazard Class: 6.1; Labels: 6.1—Poisonous materials.
Purification MethodsBarium is cleaned by washing with diethyl ether to remove adhering paraffin, then filed in an argon-filled glove box, washed first with ethanol containing 2% conc HCl, then with dry ethanol. It is dried in a vacuum and stored under argon [Addison et al. J Chem Soc 3868 1962]. It has also been purified by double distillation under 10mm of argon pressure.
IncompatibilitiesBarium powder may spontaneously ignite on contact with air. It is a strong reducing agent and Barium 337 reacts violently with oxidizers and acids. Reacts with water, forming combustible hydrogen gas and barium hydroxide. Reacts violently with halogenated hydrocarbon solvents, causing a fire and explosion hazard.
Waste DisposalBarium in solution (see spill handling) may be precipitated with soda ash and the sludge may be landfilled.
Barium Preparation Products And Raw materials
Raw materialsBarium nitrate-->BARIUM OXIDE
Tag:Barium(7440-39-3) Related Product Information
BARIUM DIETHOXIDE,BARIUM ETHOXIDE 1-CARBOXY-4-HYDROXY-ALPHA-OXO-2,5-CYCLOHEXADIENE-1-PROPANOIC ACID BARIUM SALT BARIUM DITHIONATE BARIUM DIMETHOXIDE BARIUM FERRICYANIDE BARIUM EOSINATE BARIUM DI-N-BUTOXIDE Barium diacetate Barium carbonate BARIUM DI-I-BUTOXIDE BARIUM DI-SEC-BUTOXIDE 1-(4-CHLORO-O-SULFO-5-TOLYLAZO)-2-NAPHTHOL BARIUM SALT BARIUM FLUOROPHOSPHATE BARIUM GLYCOLATE BARIUM FLUORIDE Barium hydroxide BARIUM CYANOPLATINITE BARIUM GLUCONATE