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バリウム 化学構造式
バリウム;金属バリウム;バリウム(片状);バリウム.片状;バリウム 塊状 (99.7%);バリウム pieces, 2.5cm (1in) & down, 99.2% (metals basis), Sr |<0.8%;バリウム rod (99+%, Sr-<1.6%);バリウム rod, 22mm (0.9in) dia, 99+% (metals basis), Sr |<0.8%;バリウム crystalline dendritic solid, 99.9% (metals basis);バリウム pieces, dendritic (99.9%)
bario;BARIUM;barium(0);BARIUM, ROD;Barium, 99+%;BARIUM METAL;Barium powder;Barium element;BARIUM STANDARD;bario (spanish)
MOL File:

バリウム 物理性質

融点 :
725 °C(lit.)
沸点 :
1640 °C(lit.)
比重(密度) :
3.6 g/mL at 25 °C(lit.)
貯蔵温度 :
water-free area
外見 :
電気抵抗率 (resistivity):
50.0 μΩ-cm, 20°C
水溶解度 :
soluble with H2 evolution in cold H2O and hot H2O; slightly soluble alcohol; insoluble benzene [CRC10]
Sensitive :
air sensitive, moisture sensitive
Merck :
TLV-TWA 0.5 mg/m3 (for soluble compounds) (ACGIH and MSHA); IDLH (for soluble compounds) 250 mg/m3 (NIOSH). .
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 データベース:
7440-39-3(CAS DataBase Reference)
  • リスクと安全性に関する声明
  • 危険有害性情報のコード(GHS)
主な危険性  C,Xi,F
Rフレーズ  25-26-34-36/37/38-14/15-11
Sフレーズ  23-26-36-36/37/39-45-43-36/37-16
RIDADR  UN 3264 8/PG 3
WGK Germany  3
RTECS 番号 CQ8370000
HSコード  2805 19 10
国連危険物分類  8
容器等級  III
消防法 危-3-AM-2-II
安衛法 57,57-2
注意喚起語 Danger
コード 危険有害性情報 危険有害性クラス 区分 注意喚起語 シンボル P コード
H228 可燃性固体 可燃性固体 1
P210, P240,P241, P280, P370+P378
H261 水に触れると可燃性/引火性ガスを発生 水反応可燃性化学品 2
P231+P232, P280, P370+P378,P402+P404, P501
P210 熱/火花/裸火/高温のもののような着火源から遠ざ けること。-禁煙。
P223 激しい反応と火災の発生の危険があるため、水と接 触させないこと。
P231+P232 湿気を遮断し、不活性ガス下で取り扱うこと。
P240 容器を接地すること/アースをとること。
P280 保護手袋/保護衣/保護眼鏡/保護面を着用するこ と。
P335+P334 固着していない粒子を皮膚から払いのけ、冷たい水に浸 すこと/湿った包帯で覆うこと。
P370+P378 火災の場合:消火に...を使用すること。
P402+P404 乾燥した場所または密閉容器に保管するこ と。

バリウム 価格 もっと(26)

メーカー 製品番号 製品説明 CAS番号 包装 価格 更新時間 購入
富士フイルム和光純薬株式会社(wako) W01ALF000653
Barium pieces, 2.5cm (1in) & down, 99.2% (metals basis), Sr |<0.8%
7440-39-3 5g ¥9800 2018-12-26 購入
富士フイルム和光純薬株式会社(wako) W01ALF000653
Barium pieces, 2.5cm (1in) & down, 99.2% (metals basis), Sr |<0.8%
7440-39-3 50g ¥56300 2018-12-26 購入
関東化学株式会社(KANTO) 04005-32 バリウム
Barium, in paraffin liquid
7440-39-3 25g ¥14500 2018-12-13 購入
Sigma-Aldrich Japan 403334 バリウム pieces, 1?cm, 99% trace metals basis
Barium pieces, 1?cm, 99% trace metals basis
7440-39-3 10g ¥11000 2018-12-25 購入
Sigma-Aldrich Japan 237094 バリウム rod, diam. ~2?cm, ≥99% trace metals basis
Barium rod, diam. ~2?cm, ≥99% trace metals basis
7440-39-3 25g ¥11200 2018-12-25 購入

バリウム 化学特性,用途語,生産方法


  1. バリウムは最も重いアルカリ土類金属で性質はカルシウムやストロンチウムに似る(反応性はそれよりも強い)
  2. 空気中では常温でも表面が酸化される(高温では酸化バリウムと窒化バリウムを生ずる)。水と激しく反応し水素を発生して溶ける


  1. 管球光学ガラス(テレビブラウン管、パソコンモニター)
  2. コンデンサ、フェライト
  3. 塗料、顔料用増量材(インク、塗料、顔料)
  4. 印刷インキ(配合剤)
  5. ゴム充填材(食料用白色ゴム)
  6. 摩擦材(自動車用ブレーキパッド)


Barium 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.


Barium 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.


Barium 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.


yellow-white, slightly lustrous solid


Barium is the fifth element in group 2 (IIA) of the alkali earth metals and has most of theproperties and characteristics of the other alkali earth metals in this group. For example, theyall are called alkaline earths because, when first discovered, they exhibited both characteristicsof alkaline (basic) substances and characteristics of the earth from which they came. Ancienthumans did not know they were metals because their metallic forms do not exist in nature.Barium is a silvery metal that is somewhat malleable and machineable (can be worked on alathe, stretched and pounded). Its melting point is 725°C, its boiling point is about 1640°C,and its density is 3.51 g/cm3. (The accurate figures for its properties are difficult to determinebecause of barium’s extreme activity—the pure metal will ignite when exposed to air, water,ammonia, oxygen, and the halogens.


There are currently 35 known isotopes of barium, ranging from Ba-120 to Ba-148. Seven of these isotopes are stable. The percentages of each as found in natureare as follows: Ba-130 = 0.106%, Ba-132 = 0.101%, Ba-134 = 2.147%, Ba-135 =6.592%, Ba-136 = 7.854%, Ba-137 = 11.23%, and Ba-138 = 71.7%.


The name barium is derived from the Latin word barys, which means “heavy.


Barium is the 17th most abundant element in the Earth’s crust, making up about 0.05%of the crust. It is found in the minerals witherite, which is barium carbonate (BaCO3), andbarite, known as barium sulfate (BaSO4). Pure barium metal does not exist on Earth—only ascompounds or in minerals and ores. Barium ores are found in Missouri, Arkansas, Georgia,Kentucky, Nevada, California, Canada, and Mexico.It is produced by the reduction of barium oxide (BaO), using aluminum or silicon ina high-temperature vacuum. It is also commercially produced by the electrolysis of moltenbarium chloride (BaCl2) at about 950oC, wherein the barium metal is collected at the cathodeand chlorine gas is emitted at the anode.


When barium burns in air, it produces barium oxide (2Ba + O2 → 2BaO). When metallicbarium burns in water, it forms barium hydroxide [Ba + 2H2O → Ba(OH)2 + H2↑]. Severalbarium compounds burn with a bright green flame, which make them useful for fireworks.Barium is more reactive with water than are calcium and strontium. This is a result of thevalence electrons’ being further from the positive nucleus. Therefore, barium is more electronegative than the alkali earth metals with smaller nuclei.In powdered form, it will burst into a bright green flame at room temperature.


Baryta 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.


Alloys 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.


Pure barium metal has few commercial uses because of it reactivity with air and water.Nevertheless, this property makes it useful as a “getter” or scavenger to remove the last tracesof gas from vacuum tubes. Barium metal is used to form alloys with other metals. One alloy isused to make sparkplugs that easily emit electrons when heated, thus improving the efficiencyof internal combustion engines.Its compounds have many practical uses. For example, when the mineral barite is groundup into a fine powder, it can be used as a filler and brightener for writing and computer paper.It is also used (along with zinc sulfide) as a pigment, called lithopone, for white paint. Bariumcompounds are also used in the manufacture of plastics, rubber, resins, ceramics, rocket fuel,fireworks, insecticides, and fungicides and to refine vegetable oils.A major medical use is a solution of barium sulfide (with flavoring) that is ingested bypatients undergoing stomach and intestinal X-ray and CT scan examinations. Barium sulfideis opaque to X-rays, and thus it blocks the transmission of the rays. The organs appear in contrast against a background, which highlights any problems with the digestive system.


The element barium (Ba) has the atomic number 56 and is classified as a heavy metal. Barium metal is highly reactive and therefore no elemental barium exists in nature. Natural sources of barium are the water-insoluble minerals barite (barium sulfate) and whiterite (barium carbonate). In order to obtain pure barium compounds, the mineral barite is reacted with carbon, and barium sulfide is formed.


Barium is used in electronic tubes and asa carrier for radium. Many barium saltsare used for various purposes, such as inpaints, ceramics, lubricating oils, and analyticalwork.


Alkaline-earth element of atomic number 56, group IIA of periodic table; aw 137.34; valence 2; 7 stable isotopes.


A dense, low-melting reactive metal; the fifth member of group 2 (formerly IIA) of the periodic table and a typical alkaline-earth element. The electronic configuration is that of xenon with two additional outer 6s electrons. Barium is of low abundance; it is found as witherite (BaCO3) and barytes (BaSO4). The metal is obtained by the electrolysis of the fused chloride using a cooled cathode which is slowly withdrawn from the melt. Because of its low melting point barium is readily purified by vacuum distillation. Barium metal is used as a ‘getter’, i.e., a compound added to a system to seek out the last traces of oxygen; and as an alloy constituent for certain bearing metals.
Barium has a low ionization potential and a large radius. It is therefore strongly electropositive and its properties, and those of its compounds, are very similar to those of the other alkaline-earth elements calcium and strontium.


barium: Symbol Ba. A silvery-whitereactive element belonging to group2 (formerly IIA) of the periodic table;a.n. 56; r.a.m. 137.34; r.d. 3.51; m.p.725°C; b.p. 1640°C. It occurs as theminerals barytes (BaSO4) andwitherite (BaCO3). Extraction is byhigh-temperature reduction of bariumoxide with aluminium or siliconin a vacuum, or by electrolysis offused barium chloride. The metal isused as a getter in vacuum systems.It oxidizes readily in air and reactswith ethanol and water. Soluble bariumcompounds are extremely poisonous.It was first identified in 1774 byKarl Scheele, and was extracted byHumphry Davy in 1808.


Barium 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.


Finely 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].


Alloys containing a substantial amount of barium react violently with acids [Lab. Gov. Chemist 1965].


Flammable (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.


Barium metal, in powder form, is flammable at room temperature. It must be stored in anoxygen-free atmosphere or in petroleum.
Many of barium’s compounds are toxic, especially barium chloride, which affects the functioningof the heart, causing ventricular fibrillation, an erratic heartbeat that can lead to death.Several of barium’s compounds are explosive as well as toxic if ingested or inhaled. Care shouldbe used when working with barium and other alkali metals in the laboratory or in industry.


Inhalation of barium dusts can cause irritationof the nose and upper respiratory tract.All soluble salts of barium are acute poisons.Barium ion is toxic to muscle. Ingestioncan cause severe hypokalemia. The toxicityof barium salts depends on their solubility.Ingestion of about 1 g of barium chlorideor 4 g of barium carbonate can be lethal tohumans.


Fire 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.


The 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.


Flammable/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.


Barium (symbol Ba) is a metallic element thatoccurs in combination in the minerals witheriteand barite, which are widely distributed. Themetal is silvery white in color and can beobtained by electrolysis from the chloride, butit oxidizes so easily that it is difficult to obtainin the metallic state. Its melting point is 850°C,and its specific gravity 3.78. The most extensiveuse of barium is in the form of its compounds.The salts that are soluble, such as sulfide andchloride, are toxic. An insoluble, nontoxic bariumsulfate salt is used in radiography. Bariumcompounds are used as pigments, in chemicalmanufacturing, and in deoxidizing alloys of tin, copper, lead, and zinc. Barium is introducedinto lead-bearing metals by electrolysis toharden the lead.Barium is also a key ingredient in ceramicsuperconductors.


Water 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.


Metallic 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.


Move 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.


UN1400 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.


Barium 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.


Barium 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.


Barium in solution (see spill handling) may be precipitated with soda ash and the sludge may be landfilled.

バリウム 上流と下流の製品情報



バリウム 生産企業

Global( 103)Suppliers
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  • 7440-39-3
  • 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, rods, ca. 2 cm diam., 99+%
  • Barium, dendritic pieces in mineral oil
  • Barium, rods, ca. 2 cm diam. in mineral oil
  • Barium,99+%,rods, ca. 2 cm diam. in mineral oil
  • Barium,99.9%,dendritic pieces in mineral oil
  • Barium, plasma standard solution, Specpure, Ba 10g/ml
  • Barium pieces (99.7%, Sr-<1.0%)
  • Barium, Reference Standard Solution, 1000ppm ± 1%
  • Barium rod, 22mm (0.9 in.) dia. x 450mm (17.7 in.)
  • Barium, plasma standard solution, Ba 10μg/mL
  • Barium, Oil based standard solution, Ba 5000μg/g
  • Barium Oil based standard solution, Ba 1000μg/g
  • Barium, AAS standard solution, Ba 1000μg/mL
  • Barium plasma standard solution, Ba 10000μg/mL
  • Barium, 99+%
  • バリウム
  • 金属バリウム
  • バリウム(片状)
  • バリウム.片状
  • バリウム 塊状 (99.7%)
  • バリウム pieces, 2.5cm (1in) & down, 99.2% (metals basis), Sr |<0.8%
  • バリウム rod (99+%, Sr-<1.6%)
  • バリウム rod, 22mm (0.9in) dia, 99+% (metals basis), Sr |<0.8%
  • バリウム crystalline dendritic solid, 99.9% (metals basis)
  • バリウム pieces, dendritic (99.9%)
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