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10553-31-8
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???(??):
???????;??????;??????(?????);??????(?????)(BARIUMBROMIDE);?? ????
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BARIUM BROMIDE
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BaBr2;BARIUM BROMIDE;BARIUM BROMIDE;Barium dibromide;BARIUM (II) BROMIDE;Reaxys ID: 15952940;bariumbromide(babr2);Barium bromide (BaBr2);BARIUM BROMIDE, 99.99%;BARIUM BROMIDE, 99.998%
CBNumber:
CB2204828
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BaBr2
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297.14
MOL ??:
10553-31-8.mol
MSDS ??:
SDS

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850 °C
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1835°C
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4,781 g/cm3
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Specific Gravity
4.781
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Hygroscopic
Merck
14,968
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ACGIH: TWA 0.5 mg/m3
NIOSH: IDLH 50 mg/m3; TWA 0.5 mg/m3
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CAS ??????
10553-31-8(CAS DataBase Reference)
EPA
Barium bromide (BaBr2) (10553-31-8)
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??? ?? Xn
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????? 28
????(UN No.) UN 1564 6.1/PG 2
WGK ?? 1
TSCA Yes
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???? III
HS ?? 28275900
???? ?? KE-02030
????(GHS): GHS hazard pictograms
?? ?: Warning
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P261 ??·?·??·???·??·...·????? ??? ????.
P264 ?? ??? ?? ??? ????.
P264 ?? ??? ?? ??? ????.
P270 ? ??? ??? ??? ???, ???? ???? ???.
P271 ?? ?? ??? ? ?? ???? ?????.
P301+P312 ??? ???? ??? ????(??)? ??? ????.
NFPA 704
0
2 1

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Barium bromide has the molecular formula of BaBr2. Like barium chloride, it is soluble in water but is toxic if ingested. BaBr2 crystallizes in a PbCl2 motif, as white orthorhombic crystals that are deliquescent. In aqueous solution, BaBr2 behaves as a simple salt.
Barium bromide can be crystallized from its solution as a dihydrate, BaBr2·2H2O (molecular weight: 333.19), which forms the anhydrate by heating to 120°C. It dissolves in its own water-of-hydration at 75°C before decomposing to the anhydrate.

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White Crysatalline Powder

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White orthorhombic crystal; density of anhydrous BaCl2 4.78 g/cm3, and dihydrate BaCl2 ? 2H2O 3.58 g/cm3; melts at 857°C; vaporizes at 1,835°C; readily dissolves in water (92.2 g/100 g water at 0°C).

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Barium bromide is a precursor to chemicals used in photography as well as to form other bromides.Historically, barium bromide was used to purify radium in a process of fractional crystallization devised by Marie Curie. Since radium precipitates preferentially in a solution of barium bromide, the ratio of radium to barium in the precipitate was found to be higher than the ratio in the solution.

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Barium bromide can be prepared from barium sulfide or barium carbonate by reaction with hydrobromic acid to give hydrated barium bromide:
BaS+HBr→BaBr2+H2S
BaCO3+HBr→BaBr2+CO2+H2O

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Ingestion of the salt or its aqueous solution can produce severe poisoning.

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