Difference between revisions of "Rubidium nitrite"

From Sciencemadness Wiki
Jump to: navigation, search
Line 60: Line 60:
 
| 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 = Soluble
+
| 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 [[rubidium nitrite]] and oxygen.
+
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

Rubidium nitrite
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
172 J·mol-1·K-1
-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.

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

  1. Stern K.H. High temperature properties and thermal decomposition of inorganic salts with oxyanions. - CRC Press, 2001. - pp. 164
  2. Jacob G. Reynolds, Chemical Physics Letters, Vol. 749, 2020, 137439, https://doi.org/10.1016/j.cplett.2020.137439
  3. Izvestiya Vysshikh Uchebnykh Zavedenii, Khimiya i Khimicheskaya Tekhnologiya, Vol. 12, Issue 1, p. 3-5, 1969 (from abstract)
  4. Walter Craven Ball and Harold Helling Abram, J. Chem. Soc., Trans., 1913, 103, 2130-2134, https://doi.org/10.1039/CT9130302130
  5. Walter Craven Ball and Harold Helling Abram, J. Chem. Soc., Trans., 1913, 103, 2130-2134, https://doi.org/10.1039/CT9130302130
  6. 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?