Difference between revisions of "Caesium hydroxide"
| Line 105: | Line 105: | ||
| OtherFunction = | | OtherFunction = | ||
| OtherFunction_label = | | OtherFunction_label = | ||
| − | | OtherCompounds = [[Sodium hydroxide]]<br>[[Potassium hydroxide]]<br>[[Rubidium hydroxide]] | + | | OtherCompounds = [[Lithium hydroxide]]<br>[[Sodium hydroxide]]<br>[[Potassium hydroxide]]<br>[[Rubidium hydroxide]] |
}} | }} | ||
}} | }} | ||
Revision as of 16:08, 28 April 2018
| Names | |
|---|---|
| IUPAC name
Caesium hydroxide
| |
| Other names
Caesium hydrate
Cesium hydroxide | |
| Properties | |
| CsOH | |
| Molar mass | 149.912 g/mol |
| Appearance | White hygroscopic solid |
| Odor | Odorless |
| Density | 3.675 g/cm3 |
| Melting point | 272 °C (522 °F; 545 K) |
| Boiling point | Decomposes |
| 300 g/100 ml (30 °C) | |
| Solubility | Reacts with acids Soluble in ethanol |
| Vapor pressure | ~0 mmHg |
| Thermochemistry | |
| Std molar
entropy (S |
104.2 J·K-1·mol-1 |
| Std enthalpy of
formation (ΔfH |
-416.2 kJ/mol |
| Hazards | |
| Safety data sheet | Sigma-Aldrich (monohydrate) |
| Flash point | Non-flammable |
| Lethal dose or concentration (LD, LC): | |
| LD50 (Median dose)
|
570 mg/kg (oral, rat) |
| Related compounds | |
| Related compounds
|
Lithium hydroxide Sodium hydroxide Potassium hydroxide Rubidium hydroxide |
| Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |
| Infobox references | |
Caesium hydroxide or cesium 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!
Another safer way is to carefully let the cesium metal oxidize in open air, in a corrosion resistant container. After the metal has completely oxidized, slowly add water vapor, as the reaction is highly exothermic and dry the resulting wet hydroxide.
Handling
Safety
Caesium hydroxide is a very corrosive substance. Caesium ions however, are 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.
