Difference between revisions of "Caesium hydroxide"
| Line 9: | Line 9: | ||
Caesium hydroxide is a very reactive alkali. It reacts with glass: | Caesium hydroxide is a very reactive alkali. It reacts with glass: | ||
| − | + | :2 CsOH + CaSiO<sub>3</sub> → Cs<sub>2</sub>SiO<sub>3</sub> + Ca(OH)<sub>2</sub> | |
| − | + | :2 CsOH + SiO<sub>2</sub> → Cs<sub>2</sub>SiO<sub>3</sub> + H<sub>2</sub>O | |
The resulting salt is caesium silicate, or caesium waterglass, which is water-soluble and similar in properties to [[Sodium silicate|common waterglass]]. Because of this, it is best to keep this compound in polyethylene bottles. | The resulting salt is caesium silicate, or caesium waterglass, which is water-soluble and similar in properties to [[Sodium silicate|common waterglass]]. Because of this, it is best to keep this compound in polyethylene bottles. | ||
| Line 17: | Line 17: | ||
Caesium hydroxide readily reacts with carbon dioxide in the air: | Caesium hydroxide readily reacts with carbon dioxide in the air: | ||
| − | + | :2 CsOH + CO<sub>2</sub> → Cs<sub>2</sub>CO<sub>3</sub> + H<sub>2</sub>O | |
| − | CsOH + CO<sub>2</sub> → CsHCO<sub>3</sub> | + | :CsOH + CO<sub>2</sub> → CsHCO<sub>3</sub> |
It is known to react with excess nitric acid forming unusual acidic adducts: | It is known to react with excess nitric acid forming unusual acidic adducts: | ||
| − | CsOH + 2HNO<sub>3</sub> → CsHN<sub>2</sub>O<sub>6</sub> + H<sub>2</sub>O | + | :CsOH + 2HNO<sub>3</sub> → CsHN<sub>2</sub>O<sub>6</sub> + H<sub>2</sub>O |
== Availability and synthesis == | == Availability and synthesis == | ||
| Line 47: | Line 47: | ||
Disposing of caesium compounds is not recommended because of their rarity and price. But if you absolutely want to, you should neutralize the base with any non-toxic acid. | Disposing of caesium compounds is not recommended because of their rarity and price. But if you absolutely want to, you should neutralize the base with any non-toxic acid. | ||
| + | ==References== | ||
| + | <references/> | ||
| + | ===Relevant Sciencemadness threads=== | ||
| + | *[http://www.sciencemadness.org/talk/viewthread.php?tid=29172 Cesium Hydroxide Monohydrate from 50% solution?] | ||
| + | |||
| + | [[Category:Chemical compounds]] | ||
| + | [[Category:Inorganic compounds]] | ||
| + | [[Category:Caesium compounds]] | ||
[[Category:Bases]] | [[Category:Bases]] | ||
[[Category:Alkalis]] | [[Category:Alkalis]] | ||
Revision as of 14:29, 28 August 2015
Caesium hydroxide is a crystalline solid with the formula CsOH. It is notable for being the strongest normal, aqueous base; all bases stronger than it are superbases that react with water.
Contents
Properties
Physical
Caesium hydroxide is a crystalline, hygroscopic white solid resembling potassium hydroxide.
Chemical
Caesium hydroxide is a very reactive alkali. It reacts with glass:
- 2 CsOH + CaSiO3 → Cs2SiO3 + Ca(OH)2
- 2 CsOH + SiO2 → Cs2SiO3 + H2O
The resulting salt is caesium silicate, or caesium waterglass, which is water-soluble and similar in properties to common waterglass. Because of this, it is best to keep this compound in polyethylene bottles.
Caesium hydroxide readily reacts with carbon dioxide in the air:
- 2 CsOH + CO2 → Cs2CO3 + H2O
- CsOH + CO2 → CsHCO3
It is known to react with excess nitric acid forming unusual acidic adducts:
- CsOH + 2HNO3 → CsHN2O6 + H2O
Availability and synthesis
Caesium hydroxide can be purchased from various reagent suppliers. It can also be synthesized from elemental caesium, which is sold to element collectors. There are two methods of doing this.
Kewl method: breaking the ampoule with caesium under water, remotely, from a safe distance. The reaction results in an explosion. Make sure that the vessel in which you perform the reaction is strong enough to contain it.
Safe method: treating caesium metal with small amounts of water vapor. This requires a glovebox with an inert atmosphere. Beware of hydrogen buildup in the glovebox and make sure no oxygen is present in it!
Handling
Safety
Caesium hydroxide is a very corrosive substance. It is, however, not toxic.
Storage
Store this compound in closed polyethylene bottles with no access to air.
Disposal
Disposing of caesium compounds is not recommended because of their rarity and price. But if you absolutely want to, you should neutralize the base with any non-toxic acid.
