The ammonium oxalate It is a salt of ammonium and oxalic acid that combine in a 2: 1 ratio. It is produced from a neutralization reaction in water of oxalic acid, HtwoCtwoOR4, with ammonium carbonate or ammonium hydroxide. In the first case, CO is producedtwo secondarily.
Its molecular formula is CtwoH8NtwoOR4, but this is commonly written as (NH4)twoCtwoOR4. It is produced biologically in vertebrate animals, starting from the metabolism of glyoxylic acid or ascorbic acid.
Ammonium oxalate may be present in some types of kidney stones, although the greater proportion of oxalate kidney stones, it is found in combination with calcium, forming calcium oxalate..
It cannot be metabolized in the human body, but it can be absorbed from the intestine and excreted in the feces. It can also be eliminated from the human body through urine..
In nature, it is found in the mineral oxammite, which is considered a very scarce and rare mineral. In addition, it is present in guano: a product of the decomposition of the feces of seabirds, bats and seals in a very arid environment. Guano, due to its richness in nitrogen, has been used as a fertilizer and fungicide for plants.
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The upper image shows the structures of the ions that make up ammonium oxalate. Although it is not appreciated, the NH4+ consists of a tetrahedron, while the CtwoOR4two- has a flat structure due to sp hybridizationtwo of all its carbon atoms.
Its chemical formula, (NH4)twoCtwoOR4, indicates that there must be two NH4+ interacting electrostatically with a CtwoOR4two-; that is, two tetrahedra around a plane.
In addition to ionic bonding, ions are capable of forming multiple hydrogen bonds; NH4+ donates them, and the CtwoOR4two- accepts them (through its four oxygens).
As there is a high possibility that a molecule also forms hydrogen bonds with one of the ions, it intercalates giving rise to (NH4)twoCtwoOR4∙ HtwoOR.
Crystals are made up of millions of ions and unit cells, in which the 2NH ratio is fulfilled.4/1 CtwoOR4 just named.
This being the case, in a crystal of (NH4)twoCtwoOR4∙ HtwoOr an orthorhombic crystal arrangement is formed, where hydrogen bonds play a crucial role in its physical properties..
Observing its crystalline structure from a frontal plane, NH4+ form a phase, while the CtwoOR4two- and HtwoOr they form another phase; rows of tetrahedra separated by planes and angular molecules (water).
Solid white.
CtwoH8NtwoOR4
124.096 g / mol.
70ºC (158ºF), as it appears on Wikipedia. However, Chemspider and Softschools indicate a melting point between 131 and 135 ºC.
Meanwhile, Pubchem indicates that the decomposition of the compound occurs at 70 ºC, making it unlikely that a melting point higher than this temperature can be found..
Indeterminate by compound decomposition.
5.1 g / 100 mL of water at 20 ºC. Ammonium oxalate slowly dissolves in water and often sinks in.
Slightly soluble in alcohols and insoluble in ammonia.
1.5 g / cm3 at 65.3ºF.
0 mmHg at 20 ºC.
Between 6 and 7 in a 4% solution at 25 ° C.
When exposed to high temperatures, it decomposes, emitting a toxic and corrosive smoke that includes ammonium and nitrogen oxides..
-It is used in the manufacture of explosives
-Serves as electrolytic destaining of iron
-Allows to polish the surface of metals.
Recently, pectins have been extracted with ammonium oxalate, for the manufacture of food gelling agents.
It is used in combination with potassium oxalate to form Wintrobe's reagent, which is used as an anticoagulant..
The reagent is a mixture of 1.2 g of ammonium oxalate with 0.8 g of potassium oxalate and 0.5 mL of formaldehyde, making up to 100 mL with water..
-The ammonium salt increases the volume of erythrocytes, while the potassium salt decreases it. Therefore, their effect on erythrocytes is compensated, guaranteeing their morphological integrity. This system exerts its anticoagulant action by sequestering the calcium ion.
-Ammonium oxalate is used as an analytical reagent and reducing agent, being used in the quantification of the plasma concentration of calcium and lead. In addition, ammonium oxalate is used as a dispersing agent in the study of platelet surface interactions..
-It also integrates a pH buffer system.
-Direct contact with the skin and eyes can cause irritation and burns. Likewise, prolonged or repetitive skin contact with the compound can cause signs such as: rashes, dryness and redness..
-Inhalation can irritate the nose, throat and lungs. Repeated exposure could cause bronchitis with cough, phlegm, and shortness of breath..
-High exposure to this salt can cause headache, dizziness, nausea, vomiting, seizures, coma, and even death..
-Ingestion or excessive inhalation causes systemic poisoning. Possible symptoms include pain in the throat, esophagus, and stomach. The mucosal membranes turn white, there are severe diarrhea, weak pulse, cardiovascular and neuromuscular collapse. In addition, it can affect kidney function and calcium balance..
-Calcium is involved in numerous processes that occur in living beings, among them: it mediates muscle contraction, both in smooth and striated muscles; intervenes at synapses in neuromuscular transmission; it is essential in various stages of the coagulation cascade; regulates ionic permeability and conductance in membranes, etc..
Therefore, by sequestering the ammonium oxalate to the calcium ion, the performance of the essential functions for life is compromised..
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