| Identification | More | [Name]
Barium hydroxide | [CAS]
17194-00-2 | [Synonyms]
BARIUM HYDRATE
BARIUM HYDROXIDE
Ba(OH)2
Barium hydroxide (Ba(OH)2)
Barium hydroxide, alpha
bariumdihydroxide
bariumhydroxide(ba(oh)2)
Bariumhydroxide,anhydrous
baryta hydrate
BARIUM HYDROXIDE-8-HYDRATE TECHNICAL
BARIUM HYDROXIDE, TECH., CA. 95%
BARIUM HYDROXIDE STANDARD SOLUTION
BARIUM HYDROXIDE-8-HYDRATE R. G., REAG.ISO, REAG. PH. EU
BARIUM HYDROXIDE 0,05 MOL/L VOLUME-TRIC SOLUTION
BARIUM HYDROXIDE, ANHYDROUS, 94-98%
BariumHydroxideOctohydrate
BARIUM HYDROXIDE STANDARD SOLUTION 0,05 MOL/L
BARIUM HYDROXIDE, HIGH PURITY
BARIUMHYDROXIDEA10618
Bariumhydroxide,anhydrous,min.95% | [EINECS(EC#)]
241-234-5 | [Molecular Formula]
BaH2O2 | [MDL Number]
MFCD00003443 | [Molecular Weight]
171.34 | [MOL File]
17194-00-2.mol |
| Chemical Properties | Back Directory | [Appearance]
white crystalline powder | [Melting point ]
>300 °C(lit.)
| [Boiling point ]
decomposes at 1032 (calculated) [KNA91] | [density ]
2.2 g/mL at 25 °C(lit.)
| [form ]
Solid | [color ]
Clear | [Odor]
no odor | [PH]
11.27(1 mM solution);12.22(10 mM solution);13.08(100 mM solution) | [Stability:]
Stable. Incompatible with acids, carbon dioxide, moisture. | [Water Solubility ]
Soluble in water. | [Sensitive ]
Air Sensitive & Hygroscopic | [Merck ]
14,977 | [Exposure limits]
ACGIH: TWA 0.5 mg/m3
NIOSH: IDLH 50 mg/m3; TWA 0.5 mg/m3 | [InChIKey]
RQPZNWPYLFFXCP-UHFFFAOYSA-L | [CAS DataBase Reference]
17194-00-2(CAS DataBase Reference) | [NIST Chemistry Reference]
Barium dihydroxide(17194-00-2) | [EPA Substance Registry System]
17194-00-2(EPA Substance) |
| Hazard Information | Back Directory | [Chemical Properties]
Barium hydroxide,Ba(OH)2·8H20, is a white crystalline powder, colorless solid composed of monoclinic crystals. It has a melting point of 78°C and is soluble in water and insoluble in acetone. It is used in the fusion of silicates and fat saponification.
| [Uses]
Carbon dioxide absorbant. | [Physical properties]
Monohydrate, Ba(OH)2?H2O is a white powder; density 3.743 g/cm3; slightly soluble in water; soluble in dilute mineral acids. Octahydrate, Ba(OH)2?8H2O is a colorless monoclinic crystal; density 2.18 g/cm3 at 16°C; refractive index 1.50; melts at 78°C; vapor pressure 227 torr; loses seven molecules of water of crystallization when its solution is boiled in the absence of atmospheric CO2 forming solid monohydrate; further heating produces anhydrous Ba(OH)2 melting at 407°C; readily dissolves in water (3.76 g/100 g at 20°C and 11.7 g/100 g at 50°C); aqueous solution highly alkaline; also soluble in methanol; slightly soluble in ethanol; insoluble in acetone. | [Preparation]
Barium hydroxide is made by dissolving barium oxide in hot water. The octahydrate, Ba(OH)2?8H2O, crystallizes upon cooling. It also is prepared by precipitation with caustic soda from an aqueous solution of barium sulfide:
BaS + 2NaOH → Ba(OH)2 + Na2S. | [Hazard]
An acute poison; toxic symptoms are similar to other soluble salts of barium (see Barium). | [Flammability and Explosibility]
Notclassified | [Safety Profile]
A poison by ingestion andintraperitoneal routes. Incompatible with chlorinated rubber. |
| Safety Data | Back Directory | [Hazard Codes ]
C,Xi | [Risk Statements ]
R36/37/38:Irritating to eyes, respiratory system and skin .
R34:Causes burns.
R20/22:Harmful by inhalation and if swallowed . | [Safety Statements ]
S26:In case of contact with eyes, rinse immediately with plenty of water and seek medical advice .
S36/37/39:Wear suitable protective clothing, gloves and eye/face protection .
S45:In case of accident or if you feel unwell, seek medical advice immediately (show label where possible) .
S36/37:Wear suitable protective clothing and gloves . | [RIDADR ]
UN 3262 8/PG 2
| [WGK Germany ]
1
| [RTECS ]
CQ9200000
| [TSCA ]
Yes | [HazardClass ]
8 | [PackingGroup ]
III | [Hazardous Substances Data]
17194-00-2(Hazardous Substances Data) | [Toxicity]
LD50 ipr-mus: 255 mg/kg GTPZAB 28(6),45,84 |
| Questions And Answer | Back Directory | [Description]
Barium hydroxide is a kind of barium base. It has many kinds of
applications. It can be used as the precursor for the preparation of
other barium compounds. Its monohydrate form can be used to
dehydrate and remove sulfate in many products. In laboratory, it can
be used in analytic chemistry for the titration assay of organic
acid. In organic synthesis, it is a strong base used for the
hydrolysis of esters and nitriles. It is also a useful catalyst of
organic synthesis. Other applications also include acting as an
interlayer between zinc oxide and a luminescent conjugated polymer
for light-emitting diodes, extracting pure arabinoxylans from
water-insoluble cell wall material of wheat flour, removing sulfate
and metals from the water and acting as a selective precipitating
agent for hemicelluloses. | [Chemical Properties]
barium hydroxide is a white or colorless, poisonous powder or crystalline substance, Ba(OH)2, used for example, in the saponification of fats and the fusing of silicates. Barium hydroxide forms a strong caustic base in aqueous solution. It has many uses, e.g., as a test for sulfides; in pesticides; in the manufacture of alkali and glass.
barium hydroxide, anhydrous. the commercially available preparation usually contains 92-95% of the monohydrate and is poisonous. barium hydroxide, monohydrate (barium monohydrate). a white, poisonous, slightly water-soluble, powder, Ba(OH)2.H2O; it is soluble in dilute acids. barium hydroxide, octahydrate is a poisonous white powder, Ba(OH)2.8H2O, that is soluble in water, ethanol, and ether; it absorbs CO2 from the atmosphere. It is used chiefly in organic preparations and analytical chemistry. barium hydroxide,pentahydrate. toxic white fakes, Ba(OH)2.5H2O; uses are the same as those of the octahydrate.
| [Uses]
Barium hydroxide, especially the monohydrate, is used to produce organic barium compounds such as additives for oil and stabilizers for plastics. In addition, barium hydroxide is used for. dehydration and deacidification, especially for removing sulfuric acid from fats, oils, waxes, and glycerol. In some applications, e.g., removal of sulfate from water and as starting material for other barium compounds, barium hydroxide to some ex1ent replaces barium carbonate. The earlier use of the hydroxide in some countries forextracting the residual sucrose from molasses is no longer of much significance. The re- cent patent literature describes a procedure in which barium hydroxide is reacted with hydrogen peroxide to produce barium peroxide monohydrate. | [Production Methods]
The anhydrous hydroxide has only a secondary industrial importance; the monohydrate and octahydrate are used in industry on a far larger scale.
Barium hydroxide octahydrate is produced by hydration of barium oxide. The barium oxide is suspended in recycled mother lye and heated for several hoursto destroy peroxides. The insolubles, e.g., BaC03 , are separated, and the hydroxide is precipitated by crystallization at low temperatures in stainless steel vessels. The crystals are removed from the mother lye by centrifugation.
Another industrial method is based on the oxidation of a barium sulfide solution. Air is passed into the stirred solution containing barium hydroxide and barium hydrosulfide, the hydrolysis products of barium sulfide, until the hydrosulfide is oxidized to form polysulfide. Then the barium hydroxide octahydrate is crystallized atlow temperatures and separated with a centrifuge. The Polysulfide mother lye is partly recycled, the rest usually processed for other barium compounds.
The monohydrate is generally produced on a commercial scale by dehydration of the octahydrate in heated vacuum driers. A monohydrate of especially high reactivity is obtained with drum driers. This highly reactive monohydrate is particularly suitable for the production of oil additives. | [References]
[1]Wu, Mingmei, et al. "Hydrothermal Synthesis of Tetragonal Barium Titanate from Barium Hydroxide and Titanium Dioxide under Moderate Conditions." Journal of the American Ceramic Society 82.11 (2010):3254-3256.
[2]Meier, Hans, et al. "Barium Hydroxide as a Selective Precipitating Agent for Hemicelluloses." Acta Chemica Scandinavica 12.1(1958):144-146.
[3]Gruppen, H., R. J. Hamer, and A. G. J. Voragen. "Barium hydroxide as a tool to extract pure arabinoxylans from water- insoluble cell wall material of wheat flour." Journal of Cereal Science 13.3(1991):275-290.
[4]Li, Ping Lu, D. Kabra, and R. H. Friend. "Barium Hydroxide as an Interlayer Between Zinc Oxide and a Luminescent Conjugated Polymer for Light-Emitting Diodes." Advanced Functional Materials 22.19(2012):4165–4171.
[5]Bologo, V., J. P. Maree, and F. Carlsson. "Application of magnesium hydroxide and barium hydroxide for the removal of metals and sulphate from mine water." Water Sa 38.1(2012):23-28.
[6]Sinisterra, J. V., A. Fuentes, and J. M. Marinas. "Barium hydroxide as catalyst in organic reactions. 17. Interfacial solid- liquid Wittig-Horner reaction under sonochemical conditions." J.org.chem (1987).
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