Difference between revisions of "Ammonium oxalate"

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| MolarMass = 124.10 g/mol
 
| MolarMass = 124.10 g/mol
 
| MeltingPt =  
 
| MeltingPt =  
| MeltingPtC = 133
+
| MeltingPtC = 120-133
 
| MeltingPt_ref =  
 
| MeltingPt_ref =  
 
| MeltingPt_notes = (decomposition observed at 70 °C)
 
| MeltingPt_notes = (decomposition observed at 70 °C)
Line 65: Line 65:
 
| pKa =  
 
| pKa =  
 
| pKb =  
 
| pKb =  
| Solubility = 4.5 g/100 ml (at 20 ºC)<ref>[http://pubs.acs.org/doi/abs/10.1021/ja01314a049 Hill; Distler; Journal of the American Chemical Society; vol. 57; (1935); p. 2203]</ref>
+
| Solubility = 2.36 g/100 ml (0 °C)<br>3.21 g/100 ml (10 °C)<br>4.45 g/100 ml (20 °C)<br>5.21 g/100 ml (25 °C)<br>6.08 g/100 ml (30 °C)<br>8.18 g/100 ml (40 °C)<br>10.8 g/100 ml (50 °C)<br>14.0 g/100 ml (60 °C)<br>22.4 g/100 ml (80 °C)<br>34.6 g/100 ml (100 °C)<ref>[http://pubs.acs.org/doi/abs/10.1021/ja01314a049 Hill; Distler; Journal of the American Chemical Society; vol. 57; (1935); p. 2203]</ref><ref>Rabinovich V.A., Khavin Z.Ya. Brief chemical reference book. - L.: Chemistry, 1977 (Рабинович В.А., Хавин З.Я. Краткий химический справочник. - Л.: Химия, 1977)</ref>
| SolubleOther = Insoluble in [[benzene]], [[carbon tetrachloride]]
+
| SolubleOther = Slightly soluble in [[ethanol]]<br>Insoluble in [[benzene]], [[carbon tetrachloride]]
 
| Solvent =  
 
| Solvent =  
| VaporPressure =  
+
| VaporPressure = ~0 mmHg
 
   }}
 
   }}
 
| Section3 = {{Chembox Structure
 
| Section3 = {{Chembox Structure
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| DeltaGf =  
 
| DeltaGf =  
 
| DeltaHc =  
 
| DeltaHc =  
| DeltaHf =  
+
| DeltaHf = -1,424 kJ/mol
 
| Entropy =  
 
| Entropy =  
 
| HeatCapacity = 227.36 J·mol<sup>-1</sup>·K<sup>-1</sup> (at 10 °C)<ref>Crenshaw, J. L.; Ritter, I.; Zeitschrift fuer Physikalische Chemie, Abteilung B: Chemie der Elementarprozesse, Aufbau der Materie; vol. 16;
 
| HeatCapacity = 227.36 J·mol<sup>-1</sup>·K<sup>-1</sup> (at 10 °C)<ref>Crenshaw, J. L.; Ritter, I.; Zeitschrift fuer Physikalische Chemie, Abteilung B: Chemie der Elementarprozesse, Aufbau der Materie; vol. 16;
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   }}
 
   }}
 
| Section6 = {{Chembox Hazards
 
| Section6 = {{Chembox Hazards
| AutoignitionPt =  
+
| AutoignitionPt = Non-flammable
| ExploLimits =  
+
| ExploLimits = Non-flammable
| ExternalMSDS = [http://www.dogee.org/lab/chemicals/2171.pdf DoGee]
+
| ExternalMSDS = [https://jmp.sh/yJ2vNIOv Sigma-Aldrich]
| FlashPt =  
+
| FlashPt = Non-flammable
| LD50 =  
+
| LD50 = 375 mg/kg (rat, oral)
 
| LC50 =  
 
| LC50 =  
 
| MainHazards = Harmful
 
| MainHazards = Harmful

Latest revision as of 23:52, 13 January 2024

Ammonium oxalate
Ammonium oxalate crystals sample.jpg
Crystals of ammonium oxalate
Names
IUPAC name
Diammonium ethanedioate
Properties
C2H8N2O4
Molar mass 124.10 g/mol
Appearance White crystalline solid
Odor Odorless
Density 1.5 g/cm3 (at 20 °C)
Melting point 120–133 °C (248–271 °F; 393–406 K) (decomposition observed at 70 °C)
Boiling point Decomposes
2.36 g/100 ml (0 °C)
3.21 g/100 ml (10 °C)
4.45 g/100 ml (20 °C)
5.21 g/100 ml (25 °C)
6.08 g/100 ml (30 °C)
8.18 g/100 ml (40 °C)
10.8 g/100 ml (50 °C)
14.0 g/100 ml (60 °C)
22.4 g/100 ml (80 °C)
34.6 g/100 ml (100 °C)[1][2]
Solubility Slightly soluble in ethanol
Insoluble in benzene, carbon tetrachloride
Vapor pressure ~0 mmHg
Thermochemistry
-1,424 kJ/mol
Hazards
Safety data sheet Sigma-Aldrich
Flash point Non-flammable
Lethal dose or concentration (LD, LC):
375 mg/kg (rat, oral)
Related compounds
Related compounds
Oxalic acid
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
Infobox references

Ammonium oxalate, also known as diammonium ethanedioate is a chemical compound, with the chemical formula (NH4)2C2O4. It can sometimes be encountered in nature, in guano.

Properties

Chemical

Ammonium oxalate will decompose when heated, to yield oxamide:

(NH4)2C2O4 → (CONH2)2 + 2 H2O

Further heating will give off carbon monoxide, dioxide, water and cyanide.

Physical

Ammonium oxalate is a white crystalline solid, soluble in water. It is generally encountered as a monohydrate. Ammonium oxalate has a density of 1.5 g/cm3 at 20 °C.[4]

Availability

Ammonium oxalate is sold by many chemical suppliers. Can also be bought online.

Preparation

Ammonium oxalate can be obtained by reacting ammonium carbonate, bicarbonate or aqueous ammonia with oxalic acid.

Another route involves the hydrolysis of cyanogen, in a neutral or slightly acidic aqueous environment.

Heating a mixture of anhydrous oxalic acid and urea between 150 - 160°C will yield ammonium oxalate, as well as oxamide and carbon dioxide.[5]

Projects

  • Make oxamide

Handling

Safety

Ammonium oxalate is harmful if ingested.

Storage

In closed bottles, away from acidic vapors.

Disposal

Ammonium oxalate can be destroyed by reacting it with a base, followed by pyrolysis.

References

  1. Hill; Distler; Journal of the American Chemical Society; vol. 57; (1935); p. 2203
  2. Rabinovich V.A., Khavin Z.Ya. Brief chemical reference book. - L.: Chemistry, 1977 (Рабинович В.А., Хавин З.Я. Краткий химический справочник. - Л.: Химия, 1977)
  3. Crenshaw, J. L.; Ritter, I.; Zeitschrift fuer Physikalische Chemie, Abteilung B: Chemie der Elementarprozesse, Aufbau der Materie; vol. 16; (1932); p. 147
  4. Alyaev; Belousov; Bukin; Efimova; Kuz'micheva; Rapoport; Roudenko; Chaban; Russian Journal of Inorganic Chemistry; vol. 47; nb. 3; (2002); p. 398 - 406
  5. Das-Gupta, J. M.; Journal of the Indian Chemical Society; vol. 10; (1933); p. 117 - 123

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