Difference between revisions of "Rubidium nitrite"
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| MeltingPtC = 450 | | MeltingPtC = 450 | ||
| MeltingPt_ref = | | MeltingPt_ref = | ||
| − | | MeltingPt_notes = | + | | MeltingPt_notes = also given as 422 °C<ref>Izvestiya Vysshikh Uchebnykh Zavedenii, Khimiya i Khimicheskaya Tekhnologiya, Vol. 12, Issue 1, p. 3-5, 1969 (from abstract)</ref> |
| Odor = Odorless | | Odor = Odorless | ||
| pKa = | | pKa = | ||
| pKb = | | pKb = | ||
| − | | Solubility = | + | | Solubility = Very high, sat. solution perhaps 89% w/w or 8.2 kg per kg water at 25 °C<ref>Jacob G. Reynolds, Chemical Physics Letters, Vol. 749, |
| + | 2020, 137439, https://doi.org/10.1016/j.cplett.2020.137439</ref> | ||
| SolubleOther = | | SolubleOther = | ||
| Solvent = | | Solvent = | ||
| Line 117: | Line 118: | ||
===Physical=== | ===Physical=== | ||
| − | Rubidium nitrite is a colorless solid, soluble in water. | + | Rubidium nitrite is a colorless to pale yellow deliquescent solid, very soluble in water. Is is sparingly soluble in hot [[ethanol]] and insoluble in [[acetone]].<ref>Walter Craven Ball and Harold Helling Abram, J. Chem. Soc., Trans., 1913, 103, 2130-2134, https://doi.org/10.1039/CT9130302130</ref> |
==Availability== | ==Availability== | ||
| Line 123: | Line 124: | ||
==Preparation== | ==Preparation== | ||
| − | Rubidium nitrite can be prepared by adding a solution of [[rubidium carbonate]] to a solution of [[barium nitrite]]. The resulting [[Barium carbonate|BaCO<sub>3</sub>]] is filtered off and the rubidium nitrite is recrystallized from solution. | + | Rubidium nitrite can be prepared by adding a solution of [[rubidium carbonate]] to a solution of [[barium nitrite]]. The resulting [[Barium carbonate|BaCO<sub>3</sub>]] is filtered off and the rubidium nitrite is recrystallized from solution. Alternative methods involve the use of [[rubidium sulfate]] and barium nitrite (precipitating [[barium sulfate]]), or alternatively rubidium chloride and [[silver nitrite]] (precipitating [[silver chloride]]), but due to the low solubility of silver nitrite the latter method is not recommended. The rubidium nitrite may be recovered from solution by shaking with absolute ethanol. It can be dried at 170 °C.<ref>Walter Craven Ball and Harold Helling Abram, J. Chem. Soc., Trans., 1913, 103, 2130-2134, https://doi.org/10.1039/CT9130302130</ref> |
| − | Rubidium nitrate will decompose above 300-310 °C to yield | + | An alternative way is the reaction of [[rubidium hydroxide]] with an excess of [[ethyl nitrite]] in ethanol for two days at room temperature, followed by evaporation/distillation of the volatile components and recrystallisation. (It should be noted that ethyl nitrite has a boiling point of just 17 °C!)<ref>Petru, Frantisek; Pokorny, Josef, Chemicke Listy pro Vedu a Prumysl, Vol. 51, p. 964-5, 1957 (from abstract)</ref> |
| + | |||
| + | Rubidium nitrate will decompose above 300-310 °C to yield rubidium nitrite and oxygen. | ||
==Projects== | ==Projects== | ||
| Line 135: | Line 138: | ||
===Storage=== | ===Storage=== | ||
| − | In closed bottles | + | In closed bottles. |
===Disposal=== | ===Disposal=== | ||
Revision as of 10:37, 8 November 2021
| Names | |
|---|---|
| IUPAC name
Rubidium nitrite
| |
| Preferred IUPAC name
Rubidium nitrite | |
| Other names
Rubidium mononitrite
| |
| Properties | |
| RbNO2 | |
| Molar mass | 131.473 g/mol |
| Appearance | Colorless crystalline solid |
| Odor | Odorless |
| Melting point | 450 °C (842 °F; 723 K) also given as 422 °C[3] |
| Boiling point | Decomposes[1] |
| Very high, sat. solution perhaps 89% w/w or 8.2 kg per kg water at 25 °C[2] | |
| Vapor pressure | ~0 mmHg |
| Thermochemistry | |
| Std molar
entropy (S |
172 J·mol-1·K-1 |
| Std enthalpy of
formation (ΔfH |
-367.4 kJ/mol |
| Hazards | |
| Safety data sheet | None |
| Flash point | Non-flammable |
| Related compounds | |
| Related compounds
|
Lithium nitrite Sodium nitrite Potassium nitrite Caesium nitrite |
| Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |
| Infobox references | |
Rubidium nitrite is an inorganic chemical compound with the formula RbNO2.
Contents
Properties
Chemical
Rubidium nitrite is an oxidizer, albeit a weaker one compared to rubidium nitrate, and mixtures with flammable materials will burn if ignited with an open flame.
In a flame test, RbNO2 gives a mauve/light purple color.
Physical
Rubidium nitrite is a colorless to pale yellow deliquescent solid, very soluble in water. Is is sparingly soluble in hot ethanol and insoluble in acetone.[4]
Availability
Rubidium nitrite is hard to find, and when it's available, it's quite expensive.
Preparation
Rubidium nitrite can be prepared by adding a solution of rubidium carbonate to a solution of barium nitrite. The resulting BaCO3 is filtered off and the rubidium nitrite is recrystallized from solution. Alternative methods involve the use of rubidium sulfate and barium nitrite (precipitating barium sulfate), or alternatively rubidium chloride and silver nitrite (precipitating silver chloride), but due to the low solubility of silver nitrite the latter method is not recommended. The rubidium nitrite may be recovered from solution by shaking with absolute ethanol. It can be dried at 170 °C.[5]
An alternative way is the reaction of rubidium hydroxide with an excess of ethyl nitrite in ethanol for two days at room temperature, followed by evaporation/distillation of the volatile components and recrystallisation. (It should be noted that ethyl nitrite has a boiling point of just 17 °C!)[6]
Rubidium nitrate will decompose above 300-310 °C to yield rubidium nitrite and oxygen.
Projects
- Compound collecting
Handling
Safety
Rubidium nitrite, like all nitrites may be harmful if ingested.
Storage
In closed bottles.
Disposal
Best to try and recycle it, as rubidium is expensive.
References
- ↑ Stern K.H. High temperature properties and thermal decomposition of inorganic salts with oxyanions. - CRC Press, 2001. - pp. 164
- ↑ Jacob G. Reynolds, Chemical Physics Letters, Vol. 749, 2020, 137439, https://doi.org/10.1016/j.cplett.2020.137439
- ↑ Izvestiya Vysshikh Uchebnykh Zavedenii, Khimiya i Khimicheskaya Tekhnologiya, Vol. 12, Issue 1, p. 3-5, 1969 (from abstract)
- ↑ Walter Craven Ball and Harold Helling Abram, J. Chem. Soc., Trans., 1913, 103, 2130-2134, https://doi.org/10.1039/CT9130302130
- ↑ Walter Craven Ball and Harold Helling Abram, J. Chem. Soc., Trans., 1913, 103, 2130-2134, https://doi.org/10.1039/CT9130302130
- ↑ Petru, Frantisek; Pokorny, Josef, Chemicke Listy pro Vedu a Prumysl, Vol. 51, p. 964-5, 1957 (from abstract)
Relevant Sciencemadness threads
None as of yet - why not start some research on this compound?
