Rubidium hydroxide (+1)
3D model (JSmol)
CompTox Dashboard (EPA)
|Molar mass||102.475 g/mol|
|Appearance||grayish-white solid, |
|Density||1.74 g/mL at 25 °C|
|Melting point||301 °C (574 °F; 574 K)|
|Boiling point||1,390 °C (2,530 °F; 1,660 K)|
|100 g/100 mL (15 °C)|
|Solubility||soluble in ethanol|
|Basicity (pKb)||-1.4 (dissociation of OH–)|
Std enthalpy of
|NFPA 704 (fire diamond)|
|Rubidium oxide (+1)|
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
Rubidium hydroxide does not appear in nature. However it can be obtained by synthesis from rubidium oxide. In addition, rubidium hydroxide is commercially available in form of an aqueous solution from a few suppliers.
Rubidium hydroxide is highly corrosive, therefore suitable protective clothing, gloves and eye-face protection are required when handling this material.
- Rb2O (s) + H2O (l) → 2 RbOH (aq)
Rubidium hydroxide is rarely used in industrial processes because potassium hydroxide and sodium hydroxide can perform nearly all the industrial functions of rubidium hydroxide in a less violent and hence safer way.
Rubidium hydroxide is used in scientific research. It is often used sparingly to prevent waste of the expensive element rubidium. For example, it is used to give fireworks a violet color in place of pure rubidium.
Despite the fact that rubidium hydroxide is rarely used in normal industrial processes, it is notable that the synthesis of nearly all rubidium compounds involves rubidium hydroxide as an intermediate. Natural rubidium oxide is added to water, and the resulting reaction forms soluble rubidium hydroxide as a product.
Rubidium hydroxide is a corrosive compound that causes immediate burns to the skin on contact. Ultimate care must be carried out when handling this chemical.
In the laboratory, protective clothing, gloves, and eye-face protection made from alkali-resistant materials are to be worn to prevent injury caused by accidental leakage of rubidium hydroxide onto human skin.
Dilution of this strong alkali must be done by adding the chemical slowly into the beaker of water.
In addition, chemical experiments on this compound must be performed with caution to prevent the great amount of heat released in an exothermic reaction from causing the solution to boil-over or damage the vessel.