Rubidium fluoride

Other name: Rubidium monofluoride

CAS no. : 13446-74-7

EINECS no. : 236-603-2

Molecular formula: FRb

Molecular weight: 104.4662

Melting point (℃) : 775.

The boiling point (℃) : 1410.

Relative density (water =1) : 3.56.

The saturation vapor pressure (kPa) : 0.13 (920 ℃).

Solubility: soluble in water, insoluble in ethanol, ether, liquid ammonia, soluble in hydrofluoric acid.

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Purity: 99.9%

Impurity content
Li : ≤ 0.001%
Na: ≤ 0.005%
K: ≤ 0.05%
Cs: ≤ 0.05%
Ca: ≤ 0.01%
Mg: ≤ 0.005%
Fe:   ≤ 0.001%
Al:   ≤ 0.001%

Octahedral coordination crystal. Colorless cubic powder crystal, soluble in water, dilute hydrofluoric acid, insoluble in ethanol and ether. Rubidium hydroxide and hydrofluoric acid can be mixed to prepare rubidium carbonate. Can be used as reagent, toothpaste, etc..

The storage method:
Storage precautions: store in a cool and ventilated warehouse. Package sealed. Should be stored separately from acid, edible chemicals, avoid by all means mixed storage. The storage area shall be provided with appropriate materials to contain leakage.


Related information:

The synthetic methods:
Rubidium fluoride can be synthesized in several ways.
Rubidium hydroxide mixed with hydrofluoric acid:
RbOH plus HF goes to RbF plus H2O
Neutralize rubidium carbonate with hydrofluoric acid:
Rb2CO3 plus 2HF goes to 2RbF plus H2O plus CO2
Rubidium carbonate was reacted with a concentrated solution of hydrofluoric acid in a platinum dish. Heat to red heat, so that the residue melt into a completely transparent melt, cool the white flake. Can also be melted into bars, stored in the dryer, because it is extremely hygroscopic, so often need to repeat melting. Rubidium chloride solution can be softened by adding silver fluoride to rubidium fluoride and silver chloride. Excess silver salts are removed by passing H2S. After filtration, the filtrate was evaporated in the platinum dish until RbF crystals were obtained.
Another method is to use rubidium metal to react directly with fluorine gas, but rubidium metal is very expensive, so it is the least commonly used method. In addition, rubidium reacts violently with halogen and burns:
2Rb plus F2 goes to 2RbF

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