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• 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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