Calcium peroxide hydrate

Other Reactions. Dry hydrated lime adsorbs halogen gases, eg, CI2 and F2, to form hypochlorites and fluorides. It reacts with hydrogen peroxide to form calcium peroxide, a rather unstable compound. At sintering temperatures, quicklime combines with iron to form dicalcium ferrite. 

Kemikal Food Chemical Codex Hydrate Kemikal GL Specialty Hydrate Kemikal GL Specialty Pulverized Oxide Kemikal Hydrate Kemikal Oxide-Crushed Mississippi Pebble Lime Pebble Quicklime Peerless Rotary Quicklime Quicklime Rhenosorb C Rhenosorb C/GW Rhenosorb F Unichem CAO 215-139-4 Calcium peroxide 215-142-0 Calcium phosphide 215-145-7 Ebonex Bone Ash Hydroxyapatite 215-146-2 Cadmium oxide E-Z Cad ox 215-147-8 Cadmium sulfide 215-150-4 Cerium oxide 215-154-6 Cobalt oxide (ous)... 

One-part sealants use calcium peroxide as a curing agent since it is inert in an anhydrous environment. In this sealant, barium oxide is incorporated as a dehydrating agent which is added last, but just before the addition of the calcium peroxide paste. The barium peroxide picks up 6 molecules of water of hydration and is very effective in making the sealant package stable. 

Calcium caiix)nate, surface treated Titanium dioxide, rutile Hydrated lime Synthetic zeolite Calcium peroxide Phthalate plasticizer Ganuna aminopropyltriethoxy silane Toluol Total... 

In spite of widespread usage of these compounds, the stmctures of only the calcium, barium, and strontium compounds are reasonably weU-estabhshed. The materials are generally made by trituratiag the oxides, or hydroxides, with aqueous hydrogen peroxide and dryiag the soHd products. The commercial products are typically mixtures of the peroxides with varyiag amounts of hydroxides, oxides, carbonates, hydrates, and peroxohydrates. 

Barium is a member of the aLkaline-earth group of elements in Group 2 (IIA) of the period table. Calcium [7440-70-2], Ca, strontium [7440-24-6], Sr, and barium form a closely aUied series in which the chemical and physical properties of the elements and thek compounds vary systematically with increa sing size, the ionic and electropositive nature being greatest for barium (see Calcium AND CALCIUM ALLOYS Calcium compounds Strontium and STRONTIUM compounds). As size increases, hydration tendencies of the crystalline salts increase solubiUties of sulfates, nitrates, chlorides, etc, decrease (except duorides) solubiUties of haUdes in ethanol decrease thermal stabiUties of carbonates, nitrates, and peroxides increase and the rates of reaction of the metals with hydrogen increase. 

After formulation with a flame retardant filler such as alumina trihydrate Al203 3H20, hydrated silica or calcium carbonate, a peroxide curing agent and... 

To prepare the 8-hydrate, llg of calcium chloride 6-hydrate are dissolved in 5ml of water and treated with 50ml of fresh 3% hydrogen peroxide and then with 7ml of concentrated ammonia solution in 100ml of water. If this procedure is carried out at 55°C, or if only 30ml of water are used for the ammonia at 20°C, the four-tenths hydrate is obtained. Palmer may be consulted for more details. 

After filtration, addition of sodium sulphide to the clear solution effects the precipitation of the three metals, cobalt, nickel, and manganese, as sulphides. Digestion with the calculated quantity of ferric chloride oxidises the manganese sulphide to sulphate, which passes into solution. The residue consists of cobalt and nickel sulphides, which are washed and converted into their soluble sulphates by roasting. The sulphates are extracted with water, and converted into chlorides by addition of calcium chloride solution. Their separation is effected g.s follows The requisite fraction of the chloride solution is precipitated with milk of lime, and the insoluble hydroxides of nickel and cobalt thus obtained are oxidised to the black hydroxides by treatment with chlorine. The. washed precipitate is then introduced into the remainder of the chloride solution, and the whole is well stirred and heated, when the black hydrated oxide of nickel passes, into solution, displacing tlm Remainder of. the cobalt from the solution, into. the precipitate.. The final product is thus a suspension of hydrated peroxide.of cobalt,in p. solution of nickel chloride, from which idle cobalt precipitate is removed by filtration, washed, and ignited, to the black oxide. 

OSHA PEL TWA 2 mg(Sn)/m3 ACGIH TLV IW A 2 mg(SnVm3 SAFETY PROFILE Poison by ingestion, intraperitoneal, intravenous, and subcutaneous routes. Experimental reproductive effects. Human mutation data reported. Potentially explosive reaction with metal nitrates. Violent reactions with hydrogen peroxide, ethylene oxide, hydra2ine hydrate, nitrates, K, Na. Ignition on contact with bromine trifluoride. A vigorous reaction with calcium acetylide is initiated by flame. When heated to decomposition it emits toxic fumes of Cl. See also TIN COMPOUNDS. 

The stability of the [—0—0—] ion is evidently due to the low polarising power of these cations compared with those earlier in the group. Hydrates of the form MOg.SHgO are formed by Ca, Sr and Ba when H2O2 is added to cold saturated solutions of the hydroxides dehydration is possible without decomposition. All three anhydrous peroxides contain [—0—0—] ions in the tetragonal calcium carbide lattice. They are the only simple compounds in this group which exhibit paramagnetism. 

TIN(II) CHLORIDE (7772-99-8) SnClj A powerful reducing agent. Reacts violently with strong oxidizers, strong alkalis, bromine, bromine trifluoride (ignition), calcium carbide, chlorine, chlorine monofluoride, copper nitrate, ethylene oxide fluorine, hydrogen peroxide, nitrates, potassium, potassium dioxide, sodium, with risk of fire and explosions. Incompatible with calcium acetylide, hydrazine hydrate (forms explosive stannous dihydrazine chloride) metal nitrates. On small fires, use dry chemical powder (such as Purple-K-Powder), alcohol-resistant foam, or COj extinguishers. 

ETHYL HYDRATE (64-17-5) Forms explosive mixture with air [flash point 55°F/13°C 68°F/20°C (80%) 72°F/22°C (60%) 79°F/26 C (40%)]. Reacts, possibly violently, with strong oxidizers, bases, acetic anhydride, acetyl bromide, acetyl chloride, aliphatic amines, bromine pentafluoride, calcium oxide, cesium oxide, chloryl perchlorate, disulfuryl difluoride, ethylene glycol methyl ether, iodine heptafluoride, isocyanates, nitrosyl perchlorate, perchlorates, platinum, potassium-terr-butoxide, potassium, potassium oxide, potassium peroxide, phosphorus(III) oxide, silver nitrate, silver oxide, sulfuric acid, oleum, sodium, sodium hydrazide, sodium peroxide, sulfinyl cyanamide, tetrachlorosilane, i-triazine-2,4,6-triol, triethoxydialuminum tribromide, triethylaluminum, uranium fluoride, xenon tetrafluoride. Mixture with mercury nitrate(ll) forms explosive mercury fulminate. Forms explosive complexes with perchlorates, magnesium perchlorate (forms ethyl perchlorate), silver perchlorate. Flow or agitation of substance may generate electrostatic charges due to low conductivity. 

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