Ammonium oxalate

Structural formula
General
Surname	Ammonium oxalate
other names	Diammonium oxalate; Oxalic acid diammonium salt; Ethanedioic acid diammonium salt;
Molecular formula	(NH 4 ) 2 C 2 O 4
Brief description	colorless and odorless, crystalline powder
External identifiers / databases
EC number	214-202-3
ECHA InfoCard	100.012.912
PubChem	14213
Wikidata	Q419626
properties
Molar mass	124.1 g mol −1
Physical state	firmly
density	1.48 g cm −3
Melting point	Decomposition: about 70 ° C
solubility	soluble in water: 45 g l −1 (20 ° C)
safety instructions
GHS labeling of hazardous substances Caution
H and P phrases	H: 302 + 312
	P: 302 + 352
Thermodynamic properties
ΔH f 0	−1123.0 kJ / mol
	As far as possible and customary, SI units are used. Unless otherwise noted, the data given apply to standard conditions .

Ammonium oxalate , formula (NH ₄ ) ₂ C ₂ O ₄ , is a crystalline chemical compound from the group of oxalates , i.e. the salts of oxalic acid .

Extraction and presentation

Ammonium oxalate can be prepared by neutralization of oxalic acid with ammonia solution are prepared.

{\ displaystyle \ mathrm {(COOH) _ {2} +2 \ NH_ {3} \ longrightarrow (NH_ {4}) _ {2} C_ {2} O_ {4}}}

properties

Ammonium oxalate forms rhombic crystals , is colorless and soluble in water. When heated, the compound decomposes into ammonia, water, carbon dioxide and carbon monoxide.

{\ displaystyle \ mathrm {(COONH_ {4}) _ {2} \ rightarrow 2 \, NH_ {3} + H_ {2} O + CO + CO_ {2}}}

use

Ammonium oxalate is used as a detecting agent for calcium - ion used, sparingly soluble calcium oxalate is formed, which as a white precipitate fails. Barium oxalate can be obtained by reacting with barium chloride .

{\ displaystyle \ mathrm {BaCl_ {2} + (NH_ {4}) _ {2} C_ {2} O_ {4} \ longrightarrow BaC_ {2} O_ {4} \ downarrow + \ 2 \ NH_ {4} Cl }}

Occurrence

Ammonium oxalate occurs naturally as the very rare mineral oxammite . It forms in guano deposits as a product of excretions from seabirds or bats.

Web links

Freepatentsonline: Ammonium oxalate process

Individual evidence

↑ ^a ^b ^c ^d ^e ^f Entry on diammonium oxalate in the GESTIS substance database of the IFA , accessed on February 1, 2016(JavaScript required) .
↑ David R. Lide (Ed.): CRC Handbook of Chemistry and Physics . 90th edition. (Internet version: 2010), CRC Press / Taylor and Francis, Boca Raton, FL, Standard Thermodynamic Properties of Chemical Substances, pp. 5-23.
↑ David R. Lide (Ed.): CRC Handbook of Chemistry and Physics . 90th edition. (Internet version: 2010), CRC Press / Taylor and Francis, Boca Raton, FL, Properties of the Elements and Inorganic Compounds, pp. 4-47.
↑ Entry on ammonium oxalate. In: Römpp Online . Georg Thieme Verlag, accessed on July 31, 2019.
^ Wilhelm Hurka: Chemical internship for physicians . Springer-Verlag, 2013, ISBN 978-3-662-02242-9 , pp. 32 ( limited preview in Google Book search).

[GESTIS-1] ↑ ^a ^b ^c ^d ^e ^f Entry on diammonium oxalate in the GESTIS substance database of the IFA , accessed on February 1, 2016(JavaScript required) .

[CRC90_5_23-2] David R. Lide (Ed.): CRC Handbook of Chemistry and Physics . 90th edition. (Internet version: 2010), CRC Press / Taylor and Francis, Boca Raton, FL, Standard Thermodynamic Properties of Chemical Substances, pp. 5-23.

[CRC90_4_47-3] David R. Lide (Ed.): CRC Handbook of Chemistry and Physics . 90th edition. (Internet version: 2010), CRC Press / Taylor and Francis, Boca Raton, FL, Properties of the Elements and Inorganic Compounds, pp. 4-47.

[Roempp-4] Entry on ammonium oxalate. In: Römpp Online . Georg Thieme Verlag, accessed on July 31, 2019.

[Wilhelm_Hurka-5] Wilhelm Hurka: Chemical internship for physicians . Springer-Verlag, 2013, ISBN 978-3-662-02242-9 , pp. 32 ( limited preview in Google Book search).