Chemical elements
    Physical Properties
    Chemical Properties
      Barium Hydride
      Barium Subfluoride
      Barium Fluoride
      Acid Barium Fluoride
      Barium Subchloride
      Barium Chloride
      Barium Bromide
      Barium Perbromides
      Barium Iodide
      Barium Periodides
      Barium Mixed Halides
      Barium Mixed Perhalides
      Barium Oxychloride
      Barium Hypochlorite
      Barium Chlorite
      Barium Chlorate
      Barium Perchlorate
      Barium Oxybromide
      Barium Hypobromite
      Barium Bromate
      Barium Perbromate
      Barium Oxyiodide
      Barium Iodate
      Barium Periodate
      Barium Manganites
      Barium Manganate
      Barium Permanganate
      Barium Suboxide
      Barium Oxide
      Barium Hydroxide
      Barium Peroxide
      Barium Peroxyhydrate
      Barium Tetroxide
      Barium Sulphide
      Barium Hydrosulphide
      Barium Polysulphides
      Barium Hydroxyhydrosulphide
      Barium Oxysulphides
      Barium Sulphite
      Barium Thiosulphate
      Barium Dithionate
      Barium Trithionate
      Barium Tetrathionate
      Barium Pentathionate
      Barium Sulphate
      Acid Barium Sulphates
      Barium Pyrosulphate
      Barium Persulphate
      Barium Selenide
      Barium Selenite
      Barium Selenate
      Acid Barium Selenate
      Barium Telluride
      Barium Tellurite
      Barium Tellurate
      Barium Chromite
      Barium Chromate
      Barium Dichromate
      Barium Potassium Trichromate
      Barium Chlorochromate
      Barium Perchromate
      Barium Molybdate
      Barium Permolybdate
      Barium Tungstate
      Barium Uranate
      Barium Diuranate
      Barium Peruranate
      Barium Nitride
      Barium Azide
      Barium Hexammoniate
      Barium Ammonium
      Barium Amide
      Barium Amidosulphonate
      Barium Imide
      Barium Imidosulphonate
      Barium Hyponitrite
      Barium Nitroxysulphite
      Barium Nitrososulphate
      Barium Nitrohydroxylaminate
      Barium Nitrite
      Barium Nitrate
      Barium Phosphide
      Barium Dihydrohypophosphite
      Barium Hydrophosphite
      Barium Hypophosphate
      Barium Orthophosphates
      Barium Pyrophosphate
      Barium Metaphosphate
      Basic Barium Phosphates
      Barium Thiophosphites
      Barium Thiophosphates
      Barium Selenophosphates
      Barium Azophosphates
      Barium Phosphimates
      Barium Arsenide
      Barium Orthoarsenite
      Barium Pyroarsenite
      Barium Orthoarsenates
      Barium Pyroarsenate
      Barium Thioarsenites
      Barium Thioarsenates
      Barium Sodium Selenoxyarsenate
      Barium Metantimonate
      Barium Thioantimonites
      Barium Chloroantimonite
      Barium Orthothioantimonate
      Barium Hypovanadate
      Barium Vanadates
      Barium Metapervanadate
      Barium Niobate
      Barium Tantalate
      Barium Pertantalate
      Barium Carbide
      Barium Carbonyl
      Barium Formate
      Barium Acetate
      Barium Oxalate
      Barium Carbonate
      Barium Thiocarbonate
      Barium Percarbonate
      Barium Cyanide
      Barium Cyanamide
      Barium Cyanate
      Barium Cyanurate
      Barium Thiocyanate
      Barium Selenocyanate
      Barium Silicide
      Barium Silicates
      Barium Fluosilicate
      Barium Stannate
      Barium Orthoplumbate
      Barium Titanate
      Barium Peroxide Pertitanate
      Barium Pertitanate
      Barium Fluoroxytitanate
      Barium Zirconate
      Barium Boride
      Barium Borates
      Barium Fluorborate
      Barium Perborate
      Barium Aluminates
      Barium Ferrite
      Barium Ferrate
      Barium Gobaltite
      Barium Dinickelite
      Barium Platinate
    Detection of Barrium
    PDB 1djh-3iqp
    PDB 3iqr-4e7y

Barium Silicates

Barium silicate occurs in nature under the form of various silico-aluminates, such as harmotome, brewsterite, and barytafelspar.

A barium orthosilicate, Ba2SiO4, melting at 1750° C., has been mentioned, but it is probably not stable in contact with water.

Barium metasilicate, BaSiO3, may be formed by fusing a mixture of barium chloride and carbonate with silica. It may be obtained as the hydrate, BaSiO3.H2O, by precipitation of a soluble barium salt with an alkali silicate. A hexahydrate has also been described, prepared by the action of barium hydroxide solution on sodium silicate or colloidal silica. The heat of reaction of dissolved barium hydroxide with colloidal silica is 8 Cal. It is probably decomposed by water, but the decomposition is prevented by the presence of barium hydroxide in solution. Barium silicate is formed on the walls of glass vessels containing barium hydroxide solution.

The anhydrous metasilicate forms small crystals showing a weak double refraction. The density is 4.435 and melting-point 1604° C. The heat of formation from barium oxide and silica is 26.3 Cal.

The metasilicate is not isomorphous with calcium or strontium metasilicates. With α-calcium metasilicate it forms a double compound, 2CaO.BaO.3SiO2.

By treatment of hydrated silicic acid, or powdered quartz, with barium hydroxide solution, or by boiling barium metasilicate with water for some time, a number of hydrated acid silicates may be obtained. Crystals of barium disilicate, BaSi2O5, have been observed to separate in optical glass in the form of hexagonal plates.

A compound, 2BaO.3SiO2, which forms a complete series of solid solutions with the disilicates is also known.

The use of barium silicate as a constituent of glass has already been mentioned. Its employment was first suggested by Dobereiner in 1829, and its effect upon the properties of the glass is much the same as that of lead. It gives a higher refractive index and greater brilliancy than lime alone, and it has the additional advantage over lead of being unaffected by the products of combustion in the furnace.

With barium aluminate a cement may be formed of composition 2(SiO2.2BaO).Al2O3.2BaO. It sets hard with water, but, after some time, it splits, becomes soft, and deposits crystals of barium hydroxide.

© Copyright 2008-2012 by