![]() Store this compound in closed polyethylene bottles with no access to air.ĭisposing of caesium compounds is not recommended because of their rarity and price. Keep in mind however, that caesium may be pyrophoric and could ignite.Ĭaesium hydroxide is a very corrosive substance. After the metal has completely oxidized, slowly add water vapor, as the reaction is highly exothermic and dry the resulting wet hydroxide. Beware of hydrogen buildup in the glovebox and make sure no oxygen is present in it!Īnother safer way is to carefully let the cesium metal oxidize in open air, in a corrosion resistant container. This requires a glovebox with an inert atmosphere. Safe method: treating caesium metal with small amounts of water vapor. Make sure that the vessel in which you perform the reaction is strong enough to contain it. Kewl method: breaking the ampoule with caesium under water, remotely, from a safe distance. It can also be synthesized from elemental caesium, which is sold to element collectors. It is known to react with excess nitric acid forming unusual acidic adducts:ĬsOH + 2HNO 3 → CsHN 2O 6 + H 2O Availability and synthesisĬaesium hydroxide can be purchased from various reagent suppliers. Because of this, it is best to keep this compound in polyethylene bottles.Ĭaesium hydroxide readily reacts with carbon dioxide in the air:Ģ CsOH + CO 2 → Cs 2CO 3 + H 2O CsOH + CO 2 → CsHCO 3 ![]() The resulting salt is caesium silicate, or caesium waterglass, which is water-soluble and similar in properties to common waterglass. ![]() It reacts with glass:Ģ CsOH + CaSiO 3 → Cs 2SiO 3 + Ca(OH) 2 2 CsOH + SiO 2 → Cs 2SiO 3 + H 2O Caesium hydroxide is a crystalline, hygroscopic white solid resembling potassium hydroxide.Ĭaesium hydroxide is a very reactive alkali.
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