Molar Mass Of Barium Hydroxide

Barium hydroxide
Identifiers


CAS Number	17194-00-2 ^Y 22326-55-two (monohydrate)^Y 12230-71-6 (octahydrate)^Y
3D model (JSmol)	Interactive paradigm
ChEBI	CHEBI:32592 ^Y
ChemSpider	26408 ^Y
ECHA InfoCard	100.037.470
EC Number	241-234-v
Gmelin Reference	846955
PubChem CID	28387
RTECS number	CQ9200000
UNII	1OHB71MYBK ^Y P27GID97XM (monohydrate)^Y L5Q5V03TBN (octahydrate)^Y
CompTox Dashboard (EPA)	DTXSID10892155
InChI InChI=1S/Ba.2H2O/h;21H2/q+ii;;/p-2^Y Key: RQPZNWPYLFFXCP-UHFFFAOYSA-L^Y InChI=i/Ba.2H2O/h;21H2/q+2;;/p-2 Key: RQPZNWPYLFFXCP-NUQVWONBAR
SMILES [Ba+2].[OH-].[OH-]
Properties
Chemical formula	Ba(OH)₂
Molar mass	171.34 g/mol (anhydrous) 189.355 g/mol (monohydrate) 315.46 one thousand/mol (octahydrate)
Appearance	white solid
Density	3.743 g/cm³ (monohydrate) two.18 thou/cm^three (octahydrate, 16 °C)
Melting signal	78 °C (172 °F; 351 K) (octahydrate) 300 °C (monohydrate) 407 °C (anhydrous)
Boiling point	780 °C (1,440 °F; ane,050 Thou)
Solubility in water	mass of BaO (not Ba(OH)₂): one.67 1000/100 mL (0 °C) 3.89 g/100 mL (20 °C) four.68 g/100 mL (25 °C) v.59 g/100 mL (30 °C) 8.22 g/100 mL (40 °C) 11.7 g/100 mL (l °C) 20.94 g/100 mL (60 °C) 101.four k/100 mL (100 °C)^{[ citation needed ]}
Solubility in other solvents	depression
Basicity (pK _b)	0.xv (first OH^–), 0.64 (2d OH^–)^[1]
Magnetic susceptibility (χ)	−53.2·10⁻⁶ cm³/mol
Refractive index (n _D)	1.l (octahydrate)
Construction
Crystal structure	octahedral
Thermochemistry^[2]
Std enthalpy of formation (Δ_f H ^⦵ ₂₉₈)	−944.7 kJ·mol⁻¹
Enthalpy of fusion (Δ_f H ^⦵ _fus)	16 kJ·mol⁻¹
Hazards
GHS labelling:
Pictograms
Signal word	Danger
Hazard statements	H302, H314, H332, H412
NFPA 704 (fire diamond)	3 0 0
Wink signal	Non-flammable
Related compounds
Other anions	Barium oxide Barium peroxide
Other cations	Calcium hydroxide Strontium hydroxide
Supplementary data page
Barium hydroxide (data folio)
Except where otherwise noted, information are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). Nverify (what is^{Y N} ?) Infobox references

Chemic compound

Barium hydroxide is a chemical compound with the chemic formula Ba(OH)₂. The monohydrate (10 = one), known equally baryta or baryta-h2o, is i of the chief compounds of barium. This white granular monohydrate is the usual commercial course.

Training and structure [edit]

Barium hydroxide tin be prepared past dissolving barium oxide (BaO) in water:

BaO + H₂O → Ba(OH)_ii

Information technology crystallises equally the octahydrate, which converts to the monohydrate upon heating in air. At 100 °C in a vacuum, the monohydrate volition yield BaO and water.^[3] The monohydrate adopts a layered structure (run into picture above). The Ba²⁺ centers adopt a square anti-prismatic geometry. Each Ba²⁺ centre is jump past ii water ligands and half-dozen hydroxide ligands, which are respectively doubly and triply bridging to neighboring Ba^two+ centre sites.^[4] In the octahydrate, the individual Ba²⁺ centers are once more eight coordinate but do not share ligands.^[5]

Coordination sphere about an individual barium ion in Ba(OH)₂.H₂O.

Uses [edit]

Industrially, barium hydroxide is used as the forerunner to other barium compounds. The monohydrate is used to dehydrate and remove sulfate from diverse products.^[6] This application exploits the very low solubility of barium sulfate. This industrial application is also applied to laboratory uses.

Laboratory uses [edit]

Barium hydroxide is used in analytical chemical science for the titration of weak acids, particularly organic acids. Its articulate aqueous solution is guaranteed to be complimentary of carbonate, unlike those of sodium hydroxide and potassium hydroxide, equally barium carbonate is insoluble in water. This allows the use of indicators such as phenolphthalein or thymolphthalein (with alkaline colour changes) without the risk of titration errors due to the presence of carbonate ions, which are much less basic.^[7]

Barium hydroxide is occasionally used in organic synthesis every bit a strong base of operations, for example for the hydrolysis of esters^[8] and nitriles,^[9] ^[10] ^[xi] and every bit a base in aldol condensations.

There are several uses for barium hydroxide such as to hydrolyse one of the 2 equivalent ester groups in dimethyl hendecanedioate.^[12]

Barium hydroxide has too been used, too, in the decarboxylation of amino acids liberating barium carbonate in the process.^[13]

It is also used in the preparation of cyclopentanone,^[14] diacetone alcohol^[15] and D-gulonic γ-lactone.^[16]

Reactions [edit]

Barium hydroxide decomposes to barium oxide when heated to 800 °C. Reaction with carbon dioxide gives barium carbonate. Its aqueous solution, being highly alkaline metal, undergoes neutralization reactions with acids due to it being a stiff base of operations. It is peculiarly useful on reactions that require the titrations of weak organic acids. Thus, information technology forms barium sulfate and barium phosphate with sulfuric and phosphoric acids, respectively. Reaction with hydrogen sulfide produces barium sulfide. Precipitation of many insoluble, or less soluble barium salts, may result from double replacement reaction when a barium hydroxide aqueous solution is mixed with many solutions of other metal salts.^[17]

Reactions of barium hydroxide with ammonium salts are strongly endothermic. The reaction of barium hydroxide octahydrate with ammonium chloride^[18] ^[19] or^[xx] ammonium thiocyanate^[20] ^[21] is often used equally a classroom chemistry sit-in, producing temperatures common cold enough to freeze h2o and enough water to dissolve the resulting mixture.

Condom [edit]

Barium hydroxide presents the same hazards such every bit skin irritation and burns as well as eye damage, just equally the other strong bases and as other water-soluble barium compounds: it is corrosive and toxic.^{[ citation needed ]}

References [edit]

^ "Sortierte Liste: pKb-Werte, nach Ordnungszahl sortiert. - Das Periodensystem online" (in German).
^ Lide, David R., ed. (2009). CRC Handbook of Chemistry and Physics (90th ed.). Boca Raton, Florida: CRC Press. ISBN978-one-4200-9084-0.
^ (1960). Gmelins Handbuch der anorganischen Chemie (8. Aufl.), Weinheim: Verlag Chemie, p. 289.
^ Kuske, P.; Engelen, B.; Henning, J.; Lutz, H.D.; Fuess, H.; Gregson, D. "Neutron diffraction study of Sr(OH)_ii(H₂O) and beta-Ba(OH)₂*(H_iiO)" Zeitschrift für Kristallographie (1979-2010) 1988, vol. 183, p319-p325.
^ Manohar, H.; Ramaseshan, S. "The crystal structure of barium hydroxide octahydrate Ba (OH)₂(H₂O)₈" Zeitschrift für Kristallographie, Kristallgeometrie, Kristallphysik, Kristallchemie 1964. vol. 119, p357-p374
^ Robert Kresse, Ulrich Baudis, Paul Jäger, H. Hermann Riechers, Heinz Wagner, Jochen Winkler, Hans Uwe Wolf, "Barium and Barium Compounds" in Ullmann's Encyclopedia of Industrial Chemistry, 2007 Wiley-VCH, Weinheim. doi:x.1002/14356007.a03_325.pub2
^ Mendham, J.; Denney, R. C.; Barnes, J. D.; Thomas, M. J. K. (2000), Vogel's Quantitative Chemical Analysis (6th ed.), New York: Prentice Hall, ISBN0-582-22628-7
^ Meyer, 1000.; Bloch, H. S. (1945). "Naphthoresorcinol". Org. Synth. 25: 73; Coll. Vol. three: 637.
^ Dark-brown, Thou. B. (1946). "Methylsuccinic acid". Org. Synth. 26: 54; Coll. Vol. 3: 615.
^ Ford, Jared H. (1947). "β-Alanine". Org. Synth. 27: ane; Coll. Vol. 3: 34.
^ Anslow, W. K.; King, H.; Orten, J. Thou.; Hill, R. M. (1925). "Glycine". Org. Synth. 4: 31; Coll. Vol. 1: 298.
^ Durham, L. J.; McLeod, D. J.; Cason, J. (1958). "Methyl hydrogen hendecanedioate". Org. Synth. 38:55; Coll. Vol. 4:635.
^ Chaudhari, Yard. R.; Kulkarni, Y. A.; Gokhale, Southward. B. (6 October 2008). Biochemistry and Clinical Pathology. ISBN9788185790169.
^ Thorpe, J. F.; Kon, K. A. R. (1925). "Cyclopentanone". Org. Synth. five: 37; Coll. Vol. i: 192.
^ Conant, J. B.; Tuttle, Niel. (1921). "Diacetone booze". Org. Synth. ane: 45; Coll. Vol. 1: 199.
^ Karabinos, J. V. (1956). "γ-lactone". Org. Synth. 36: 38; Coll. Vol. 4: 506.
^ Pradyot Patnaik. Handbook of Inorganic Chemicals. McGraw-Hill, 2002, ISBN 0-07-049439-8
^ "Endothermic Reactions of Hydrated Barium Hydroxide and Ammonium Chloride". UC San Diego. Retrieved 2 April 2014.
^ Endothermic Solid-Solid Reactions
^ ^a ^b Camp, Eric. "Endothermic Reaction". Univertist of Washington. Retrieved 2 April 2014.
^ "Endothermic solid-solid reactions" (PDF). Classic Chemical science Demonstrations. The Purple Society of Chemical science. Archived from the original (PDF) on 7 Apr 2014. Retrieved 2 April 2014.