Oxalic acid

Last updated
Oxalic acid
Oxalsaure2.svg
Oxalic acid molecule ball from xtal.png
Oxalic acid molecule spacefill from xtal.png
Oxalic acid dihydrate.jpg
Oxalic acid dihydrate
Names
IUPAC name
1,2-ethanedioic acid
Preferred IUPAC name
Oxalic acid [1]
Systematic IUPAC name
Ethanedioic acid [1]
Other names
Wood bleach
(Carboxyl)carboxylic acid
Carboxylformic acid
Dicarboxylic acid
Diformic acid
Identifiers
3D model (JSmol)
3DMet
385686
ChEBI
ChEMBL
ChemSpider
DrugBank
ECHA InfoCard 100.005.123 OOjs UI icon edit-ltr-progressive.svg
EC Number
  • 205-634-3
2208
KEGG
MeSH Oxalic+acid
PubChem CID
RTECS number
  • RO2450000
UNII
UN number 3261
  • InChI=1S/C6H6O6/c3-1(4)2(5)6/h(H,3,4)(H,5,6) Yes check.svgY
    Key: MUBZPKHOEPUJKR-UHFFFAOYSA-N Yes check.svgY
  • OC(=O)C(=O)O
Properties
C2H2O4
Molar mass 90.034 g·mol−1(anhydrous)
126.065 g·mol−1 (dihydrate)
AppearanceWhite crystals
Odor Odorless
Density 1.90 g/cm3 (anhydrous, at 17 °C) [2]
1.653 g/cm3 (dihydrate)
Melting point 189 to 191 °C (372 to 376 °F; 462 to 464 K)
101.5 °C (214.7 °F; 374.6 K) dihydrate
Boiling point decomposes (see article for details)
  • In g/L:
  • 46.9 (5 °C)
  • 57.2 (10 °C)
  • 75.5 (15 °C)
  • 95.5 (20 °C)
  • 118 (25 °C)
  • 139 (30 °C)
  • 178 (35 °C)
  • 217 (40 °C)
  • 261 (45 °C)
  • 315 (50 °C)
  • 376 (55 °C)
  • 426 (60 °C)
  • 548 (65 °C)
[3]
Solubility 237 g/L (15 °C) in ethanol
14 g/L (15 °C) in diethyl ether [4]
Vapor pressure <0.001 mmHg (20 °C) [5]
Acidity (pKa)pKa1 = 1.25
pKa2 = 4.14 [6]
Conjugate base Hydrogenoxalate
−60.05·10−6 cm3/mol
Thermochemistry [7]
91.0 J/(mol·K)
Std molar
entropy (S⦵298)
109.8 J/(mol·K)
−829.9 kJ/mol
Pharmacology
QP53AG03 ( WHO )
Hazards
Occupational safety and health (OHS/OSH):
Main hazards
Corrosive
GHS labelling:
GHS-pictogram-acid.svg GHS-pictogram-exclam.svg GHS-pictogram-silhouette.svg
Danger
H302+H312, H318, H402
P264, P270, P273, P280, P301+P312+P330, P302+P352+P312, P305+P351+P338+P310, P362+P364, P501
NFPA 704 (fire diamond)
NFPA 704.svgHealth 3: Short exposure could cause serious temporary or residual injury. E.g. chlorine gasFlammability 1: Must be pre-heated before ignition can occur. Flash point over 93 °C (200 °F). E.g. canola oilInstability 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g. liquid nitrogenSpecial hazard ACID: Acid
3
1
0
ACID
Flash point 166 °C (331 °F; 439 K)
Lethal dose or concentration (LD, LC):
1000 mg/kg (dog, oral)
1400 mg/kg (rat)
7500 mg/kg (rat, oral) [8]
NIOSH (US health exposure limits):
PEL (Permissible)
TWA 1 mg/m3 [5]
REL (Recommended)
TWA 1 mg/m3 ST 2 mg/m3 [5]
IDLH (Immediate danger)
500 mg/m3 [5]
Safety data sheet (SDS) External MSDS
Related compounds
Related compounds
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
X mark.svgN  verify  (what is  Yes check.svgYX mark.svgN ?)

Oxalic acid is an organic acid with the systematic name ethanedioic acid and chemical formula HO−C(=O)−C(=O)−OH, also written as (COOH)2 or (CO2H)2 or H2C2O4. It is the simplest dicarboxylic acid. It is a white crystalline solid that forms a colorless solution in water. Its name comes from the fact that early investigators isolated oxalic acid from flowering plants of the genus Oxalis , commonly known as wood-sorrels. It occurs naturally in many foods. Excessive ingestion of oxalic acid or prolonged skin contact can be dangerous.

Contents

Oxalic acid has much greater acid strength than acetic acid. It is a reducing agent [9] and its conjugate bases hydrogen oxalate (HC2O−4) and oxalate (C2O2−4) are chelating agents for metal cations. It is used as a cleaning agent, especially for the removal of rust, because it forms a water-soluble ferric iron complex, the ferrioxalate ion. Oxalic acid typically occurs as the dihydrate with the formula H2C2O4·2H2O.

History

The preparation of salts of oxalic acid from plants had been known, at least since 1745, when the Dutch botanist and physician Herman Boerhaave isolated a salt from wood sorrel, akin to kraft process. [10] By 1773, François Pierre Savary of Fribourg, Switzerland had isolated oxalic acid from its salt in sorrel. [11]

In 1776, Swedish chemists Carl Wilhelm Scheele and Torbern Olof Bergman [12] produced oxalic acid by reacting sugar with concentrated nitric acid; Scheele called the acid that resulted socker-syra or såcker-syra (sugar acid). By 1784, Scheele had shown that "sugar acid" and oxalic acid from natural sources were identical. [13] The modern name was introduced along with many other acid names by de Morveau, Lavoisier and coauthors in 1787. [14]

In 1824, the German chemist Friedrich Wöhler obtained oxalic acid by reacting cyanogen with ammonia in aqueous solution. [15] This experiment may represent the first synthesis of a natural product. [16]

Production

Industrial

Oxalic acid is mainly manufactured by the oxidation of carbohydrates or glucose using nitric acid or air in the presence of vanadium pentoxide. A variety of precursors can be used including glycolic acid and ethylene glycol. [17] A newer method entails oxidative carbonylation of alcohols to give the diesters of oxalic acid:

4 ROH + 4 CO + O2 → 2 (CO2R)2 + 2 H2O

These diesters are subsequently hydrolyzed to oxalic acid. Approximately 120,000 tonnes are produced annually. [16]

Historically oxalic acid was obtained exclusively by using caustics, such as sodium or potassium hydroxide, on sawdust, followed by acidification of the oxalate by mineral acids, such as sulfuric acid. [18] Oxalic acid can also be formed by the heating of sodium formate in the presence of an alkaline catalyst. [19]

Laboratory

Although it can be readily purchased, oxalic acid can be prepared in the laboratory by oxidizing sucrose using nitric acid in the presence of a small amount of vanadium pentoxide as a catalyst. [20]

The hydrated solid can be dehydrated with heat or by azeotropic distillation. [21]

Structure

Anhydrous

Anhydrous oxalic acid exists as two polymorphs; in one the hydrogen-bonding results in a chain-like structure, whereas the hydrogen bonding pattern in the other form defines a sheet-like structure. [22] Because the anhydrous material is both acidic and hydrophilic (water seeking), it is used in esterifications.

Dihydrate

The dihydrate H
2C
2O
4·2H
2O has space group C52h–P21/n, with lattice parameters a = 611.9 pm , b = 360.7 pm, c = 1205.7 pm, β = 106°19′, Z = 2. [23] The main inter-atomic distances are: C−C 153 pm, C−O1 129 pm, C−O2 119 pm. [24]

Reactions

Acid–base properties

Oxalic acid's pKa values vary in the literature from 1.25 to 1.46 and from 3.81 to 4.40. [25] [26] [27] The 100th ed of the CRC, released in 2019, has values of 1.25 and 3.81. [28] Oxalic acid is relatively strong compared to other carboxylic acids:

H2C2O4 ⇌ HC2O−4 + H+          pKa1 = 1.27
HC2O−4 ⇌ C2O2−4 + H+          pKa2 = 4.27

Oxalic acid undergoes many of the reactions characteristic for other carboxylic acids. It forms esters such as dimethyl oxalate (m.p. 52.5 to 53.5 °C, 126.5 to 128.3 °F). [29] It forms an acid chloride called oxalyl chloride.

Metal-binding properties

Transition metal oxalate complexes are numerous, e.g. the drug oxaliplatin. Oxalic acid has been shown to reduce manganese dioxide MnO2 in manganese ores to allow the leaching of the metal by sulfuric acid. [30]

Oxalic acid is an important reagent in lanthanide chemistry. Hydrated lanthanide oxalates form readily in very strongly acidic solutions as a densely crystalline, easily filtered form, largely free of contamination by nonlanthanide elements:

2 Ln3+ + 3 H2C2O4 → Ln2(C2O4)3 + 6 H+

Thermal decomposition of these oxalates gives the oxides, which is the most commonly marketed form of these elements. [31]

Other

Oxalic acid and oxalates can be oxidized by permanganate in an autocatalytic reaction. [32]

Oxalic acid vapor decomposes at 125–175 °C into carbon dioxide CO
2 and formic acid HCOOH. Photolysis with 237–313 nm UV light also produces carbon monoxide CO and water. [33]

Evaporation of a solution of urea and oxalic acid in 2:1 molar ratio yields a solid crystalline compound H2C2O4·2CO(NH2)2, consisting of stacked two-dimensional networks of the neutral molecules held together by hydrogen bonds with the oxygen atoms. [34]

Occurrence

Biosynthesis

At least two pathways exist for the enzyme-mediated formation of oxalate. In one pathway, oxaloacetate, a component of the Krebs citric acid cycle, is hydrolyzed to oxalate and acetic acid by the enzyme oxaloacetase: [35]

[O2CC(O)CH2CO2]2− + H2O → C2O2−4 + CH3CO−2 + H+

It also arises from the dehydrogenation of glycolic acid, which is produced by the metabolism of ethylene glycol.

Occurrence in foods and plants

Stems of Oxalis triangularis contain oxalic acid. OxalisTriangularis.jpg
Stems of Oxalis triangularis contain oxalic acid.

Early investigators isolated oxalic acid from wood-sorrel (Oxalis). Members of the spinach family and the brassicas (cabbage, broccoli, brussels sprouts) are high in oxalates, as are sorrel and umbellifers like parsley. [36] The leaves and stems of all species of the genus Chenopodium and related genera of the family Amaranthaceae, which includes quinoa, contain high levels of oxalic acid. [37] Rhubarb leaves contain about 0.5% oxalic acid, and jack-in-the-pulpit ( Arisaema triphyllum ) contains calcium oxalate crystals. Similarly, the Virginia creeper, a common decorative vine, produces oxalic acid in its berries as well as oxalate crystals in the sap, in the form of raphides. Bacteria produce oxalates from oxidation of carbohydrates. [16]

Plants of the genus Fenestraria produce optical fibers made from crystalline oxalic acid to transmit light to subterranean photosynthetic sites. [38]

Carambola, also known as starfruit, also contains oxalic acid along with caramboxin. Citrus juice contains small amounts of oxalic acid.

The formation of naturally occurring calcium oxalate patinas on certain limestone and marble statues and monuments has been proposed to be caused by the chemical reaction of the carbonate stone with oxalic acid secreted by lichen or other microorganisms. [39] [40]

Production by fungi

Many soil fungus species secrete oxalic acid, which results in greater solubility of metal cations and increased availability of certain soil nutrients, and can lead to the formation of calcium oxalate crystals. [41] [42] Some fungi such as Aspergillus niger have been extensively studied for the industrial production of oxalic acid; [43] however, those processes are not yet economically competitive with production from oil and gas. [44] Cryphonectria parasitica may excrete oxalic acid containing solutions at the advancing edge of its chestnut cambium infection. The lower pH (<2.5) of more concentrated oxalic acid excretions may degrade cambium cell walls and have a toxic effect on chestnut cambium cells. Cambium cells that burst provide nutrients for a blight infection advance. [45] [46]

Biochemistry

The conjugate base of oxalic acid is the hydrogenoxalate anion, and its conjugate base (oxalate) is a competitive inhibitor of the lactate dehydrogenase (LDH) enzyme. [47] LDH catalyses the conversion of pyruvate to lactic acid (end product of the fermentation (anaerobic) process) oxidising the coenzyme NADH to NAD+ and H+ concurrently. Restoring NAD+ levels is essential to the continuation of anaerobic energy metabolism through glycolysis. As cancer cells preferentially use anaerobic metabolism (see Warburg effect) inhibition of LDH has been shown to inhibit tumor formation and growth, [48] thus is an interesting potential course of cancer treatment.

Oxalic acid plays a key role in the interaction between pathogenic fungi and plants. Small amounts of oxalic acid enhances plant resistance to fungi, but higher amounts cause widespread programmed cell death of the plant and help with fungi infection. Plants normally produce it in small amounts, but some pathogenic fungi such as Sclerotinia sclerotiorum cause a toxic accumulation. [49]

Oxalate, besides being biosynthesised, may also be biodegraded. Oxalobacter formigenes is an important gut bacterium that helps animals (including humans) degrade oxalate. [50]

Applications

Oxalic acid's main applications include cleaning or bleaching, especially for the removal of rust (iron complexing agent). Its utility in rust removal agents is due to its forming a stable, water-soluble salt with ferric iron, ferrioxalate ion. Oxalic acid is an ingredient in some tooth whitening products. About 25% of produced oxalic acid is used as a mordant in dyeing processes. It is also used in bleaches, especially for pulpwood, cork, straw, cane, feathers, and for rust removal and other cleaning, in baking powder, and as a third reagent in silica analysis instruments.

Niche uses

Honeybee coated with oxalate crystals Beecrystals.PNG
Honeybee coated with oxalate crystals

Oxalic acid is used by some beekeepers as a miticide against the parasitic varroa mite. [51]

Dilute solutions (0.05–0.15 M) of oxalic acid can be used to remove iron from clays such as kaolinite to produce light-colored ceramics. [52]

Oxalic acid can be used to clean minerals like many other acids. Two such examples are quartz crystals and pyrite. [53] [54] [55]

Oxalic acid is sometimes used in the aluminum anodizing process, with or without sulfuric acid. [56] Compared to sulfuric-acid anodizing, the coatings obtained are thinner and exhibit lower surface roughness.

Oxalic acid is also widely used as a wood bleach, most often in its crystalline form to be mixed with water to its proper dilution for use.[ citation needed ]

Semiconductor industry

Oxalic acid is also used in electronic and semiconductor industries. In 2006 it was reported being used in electrochemical–mechanical planarization of copper layers in the semiconductor devices fabrication process. [57]

Proposed uses

Reduction of carbon dioxide to oxalic acid by various methods, such as electrocatalysis using a copper complex, [58] is under study as a proposed chemical intermediate for carbon capture and utilization. [59]

Content in food items

[60] [ clarification needed ]

VegetableContent of oxalic acid
(%) a
Amaranth
Asparagus
Beans, snap
Beet leaves
Beetroot
Broccoli
Brussels sprouts
Cabbage
Carrot
Cassava
Cauliflower
Celery
Chicory
Chives
Collards
Coriander
Corn, sweet
Cucumber
Eggplant
Endive
Garlic
Kale
Lettuce
Okra
Onion
Parsley
Parsnip
Pea
Bell pepper
Potato
Purslane
Radish
Rhubarb leaves
Rutabaga
Spinach
Squash
Sweet potato
Swiss chard, green
Tomato
Turnip
Turnip greens
Watercress

Toxicity

Oxalic acid has an oral LDLo (lowest published lethal dose) of 600 mg/kg. [64] It has been reported that the lethal oral dose is 15 to 30 grams. [65] The toxicity of oxalic acid is due to kidney failure caused by precipitation of solid calcium oxalate. [66]

Oxalate is known to cause mitochondrial dysfunction. [67]

Ingestion of ethylene glycol results in oxalic acid as a metabolite which can also cause acute kidney failure.

Kidney stones

Most kidney stones, 76%, are composed of calcium oxalate. [68]

Notes

^a Unless otherwise cited, all measurements are based on raw vegetable weights with original moisture content.

Related Research Articles

<span class="mw-page-title-main">Rhubarb</span> Species of herbaceous perennial plant with fleshy, sour edible stalks

Rhubarb is the fleshy, edible stalks (petioles) of species and hybrids of Rheum in the family Polygonaceae, which are cooked and used for food. The plant is a herbaceous perennial that grows from short, thick rhizomes. Historically, different plants have been called "rhubarb" in English. The large, triangular leaves contain high levels of oxalic acid and anthrone glycosides, making them inedible. The small flowers are grouped in large compound leafy greenish-white to rose-red inflorescences.

<span class="mw-page-title-main">Calcium oxalate</span> Calcium salt of oxalic acid

Calcium oxalate (in archaic terminology, oxalate of lime) is a calcium salt of oxalic acid with the chemical formula CaC2O4 or Ca(COO)2. It forms hydrates CaC2O4·nH2O, where n varies from 1 to 3. Anhydrous and all hydrated forms are colorless or white. The monohydrate CaC2O4·H2O occurs naturally as the mineral whewellite, forming envelope-shaped crystals, known in plants as raphides. The two rarer hydrates are dihydrate CaC2O4·2H2O, which occurs naturally as the mineral weddellite, and trihydrate CaC2O4·3H2O, which occurs naturally as the mineral caoxite, are also recognized. Some foods have high quantities of calcium oxalates and can produce sores and numbing on ingestion and may even be fatal. Cultural groups with diets that depend highly on fruits and vegetables high in calcium oxalate, such as those in Micronesia, reduce the level of it by boiling and cooking them. They are a constituent in 76% of human kidney stones. Calcium oxalate is also found in beerstone, a scale that forms on containers used in breweries.

<span class="mw-page-title-main">Oxalate</span> Any derivative of oxalic acid; chemical compound containing oxalate moiety

Oxalate is an anion with the chemical formula C2O2−4. This dianion is colorless. It occurs naturally, including in some foods. It forms a variety of salts, for example sodium oxalate, and several esters such as dimethyl oxalate. It is a conjugate base of oxalic acid. At neutral pH in aqueous solution, oxalic acid converts completely to oxalate.

<span class="mw-page-title-main">Vanadium(V) oxide</span> Precursor to vanadium alloys and industrial catalyst

Vanadium(V) oxide (vanadia) is the inorganic compound with the formula V2O5. Commonly known as vanadium pentoxide, it is a dark yellow solid, although when freshly precipitated from aqueous solution, its colour is deep orange. Because of its high oxidation state, it is both an amphoteric oxide and an oxidizing agent. From the industrial perspective, it is the most important compound of vanadium, being the principal precursor to alloys of vanadium and is a widely used industrial catalyst.

<span class="mw-page-title-main">Tin(II) chloride</span> Chemical compound

Tin(II) chloride, also known as stannous chloride, is a white crystalline solid with the formula SnCl2. It forms a stable dihydrate, but aqueous solutions tend to undergo hydrolysis, particularly if hot. SnCl2 is widely used as a reducing agent (in acid solution), and in electrolytic baths for tin-plating. Tin(II) chloride should not be confused with the other chloride of tin; tin(IV) chloride or stannic chloride (SnCl4).

<span class="mw-page-title-main">Glyoxylic acid</span> Acetic acid bearing an aldehyde group

Glyoxylic acid or oxoacetic acid is an organic compound. Together with acetic acid, glycolic acid, and oxalic acid, glyoxylic acid is one of the C2 carboxylic acids. It is a colourless solid that occurs naturally and is useful industrially.

<span class="mw-page-title-main">Acetylenedicarboxylic acid</span> Chemical compound

Acetylenedicarboxylic acid or butynedioic acid is an organic compound with the formula H2C4O4 or HO−C(=O)−C≡C−C(=O)−OH. It is a crystalline solid that is soluble in diethyl ether.

<span class="mw-page-title-main">Hydrogenoxalate</span> Ion

Hydrogenoxalate or hydrogen oxalate(IUPAC name: 2-Hydroxy-2-oxoacetate) is an anion with chemical formula HC2O−4 or HO−C(=O)−CO−2, derived from oxalic acid by the loss of a single proton; or, alternatively, from the oxalate anion C2O2−4 by addition of a proton. The name is also used for any salt containing this anion. Especially in older literature, hydrogenoxalates may also be referred to as bioxalates, acid oxalates, or monobasic oxalates. Hydrogenoxalate is amphoteric, in that it can react both as an acid or a base.

<span class="mw-page-title-main">Potassium hydrogenoxalate</span> Chemical compound, salt of sorrel

Potassium hydrogenoxalate is a salt with formula KHC2O4 or K+·HO2C-CO2−. It is one of the most common salts of the hydrogenoxalate anion, and can be obtained by reacting potassium hydroxide with oxalic acid in 1:1 mole ratio.

<span class="mw-page-title-main">Ammonium oxalate</span> Chemical compound

Ammonium oxalate is a chemical compound with the chemical formula [NH4]2C2O4. Its formula is often written as (NH4)2C2O4 or (COONH4)2. It is an ammonium salt of oxalic acid. It consists of ammonium cations ([NH4]+) and oxalate anions (C2O2−4). The structure of ammonium oxalate is ([NH4]+)2[C2O4]2−. Ammonium oxalate sometimes comes as a monohydrate ([NH4]2C2O4·H2O). It is a colorless or white salt under standard conditions and is odorless and non-volatile. It occurs in many plants and vegetables.

<span class="mw-page-title-main">Magnesium oxalate</span> Magnesium compound

Magnesium oxalate is an organic compound comprising a magnesium cation with a 2+ charge bonded to an oxalate anion. It has the chemical formula MgC2O4. Magnesium oxalate is a white solid that comes in two forms: an anhydrous form and a dihydrate form where two water molecules are complexed with the structure. Both forms are practically insoluble in water and are insoluble in organic solutions.

Chromium(II) oxalate is an inorganic compound with the chemical formula CrC2O4.

<span class="mw-page-title-main">Sodium hydrogenoxalate</span> Partly deprotonated oxalic acid

Sodium hydrogenoxalate or sodium hydrogen oxalate is a chemical compound with the chemical formula NaHC2O4. It is an ionic compound. It is a sodium salt of oxalic acid H2C2O4. It is an acidic salt, because it consists of sodium cations Na+ and hydrogen oxalate anions HC2O−4 or HO−C(=O)−CO−2, in which only one acidic hydrogen atom in oxalic acid is replaced by sodium atom. The hydrogen oxalate anion can be described as the result of removing one hydrogen ion H+ from oxalic acid, or adding one to the oxalate anion C2O2−4.

<span class="mw-page-title-main">Caesium oxalate</span> Chemical compound

Caesium oxalate, or dicesium oxalate, or cesium oxalate is a chemical compound with the chemical formula Cs2C2O4. It is a caesium salt of oxalic acid. It consists of caesium cations Cs+ and oxalate anions C2O2−4.

The nickel organic acid salts are organic acid salts of nickel. In many of these the ionised organic acid acts as a ligand.

Praseodymium(III) oxalate is an inorganic compound, a salt of praseodymium metal and oxalic acid, with the chemical formula C6O12Pr2. The compound forms light green crystals that are insoluble in water. It also forms crystalline hydrates.

<span class="mw-page-title-main">Yttrium oxalate</span> Chemical compound

Yttrium oxalate is an inorganic compound, a salt of yttrium and oxalic acid with the chemical formula Y2(C2O4)3. The compound does not dissolve in water and forms crystalline hydrates—colorless crystals.

Manganese oxalate is a chemical compound, a salt of manganese and oxalic acid with the chemical formula MnC
2O
4. The compound creates light pink crystals, does not dissolve in water, and forms crystalline hydrates. It occurs naturally as the mineral Lindbergite.

<span class="mw-page-title-main">Tin(II) oxalate</span> Chemical compound

Tin(II) oxalate is an inorganic compound, a salt of tin and oxalic acid with the chemical formula SnC
2O
4. The compound looks like colorless crystals, does not dissolve in water, and forms crystalline hydrates.

<span class="mw-page-title-main">Rubidium oxalate</span> Chemical compound

Rubidium oxalate is a chemical compound with the chemical formula Rb2C2O4. It is a rubidium salt of oxalic acid. It consists of rubidium cations Rb+ and oxalate anions C2O2−4. Rubidium oxalate forms a monohydrate Rb2C2O4·H2O.

References

  1. 1 2 "Front Matter". Nomenclature of Organic Chemistry : IUPAC Recommendations and Preferred Names 2013 (Blue Book). Cambridge: The Royal Society of Chemistry. 2014. pp. P001–P004. doi:10.1039/9781849733069-FP001. ISBN   978-0-85404-182-4.
  2. ↑ Record in the GESTIS Substance Database of the Institute for Occupational Safety and Health
  3. ↑ Apelblat, Alexander; Manzurola, Emanuel (1987). "Solubility of oxalic, malonic, succinic, adipic, maleic, malic, citric, and tartaric acids in water from 278.15 to 338.15 K". The Journal of Chemical Thermodynamics. 19 (3): 317–320. doi:10.1016/0021-9614(87)90139-X.
  4. ↑ Radiant Agro Chem. "Oxalic Acid MSDS". Archived from the original on 2011-07-15. Retrieved 2012-02-02.
  5. 1 2 3 4 NIOSH Pocket Guide to Chemical Hazards. "#0474". National Institute for Occupational Safety and Health (NIOSH).
  6. ↑ Bjerrum, Jannik; Sillén, Lars Gunnar; Schwarzenbach, Gerold Karl; Anderegg, Giorgio (1958). Stability constants of metal-ion complexes, with solubility products of inorganic substances. London: Chemical Society.
  7. ↑ CRC handbook of chemistry and physics : a ready-reference book of chemical and physical data. William M. Haynes, David R. Lide, Thomas J. Bruno (2016-2017, 97th ed.). Boca Raton, Florida. 2016. ISBN   978-1-4987-5428-6. OCLC   930681942.{{cite book}}: CS1 maint: location missing publisher (link) CS1 maint: others (link)
  8. ↑ "Oxalic acid". Immediately Dangerous to Life or Health Concentrations (IDLH). National Institute for Occupational Safety and Health (NIOSH).
  9. ↑ Ullmann's Encyclopedia of Industrial Chemistry. Wiley. 2005. pp. 17624/28029. doi:10.1002/14356007. ISBN   9783527306732.
  10. ↑ See:
    • Herman Boerhaave, Elementa Chemiae (Basil, Switzerland: Johann Rudolph Im-hoff, 1745), volume 2, pp. 35-38. (in Latin) From p. 35: "Processus VII. Sal nativum plantarum paratus de succo illarum recens presso. Hic Acetosae." (Procedure 7. A natural salt of plants prepared from their freshly pressed juice. This [salt obtained] from sorrel.)
    • Henry Enfield Roscoe and Carl Schorlemmer, ed.s, A Treatise on Chemistry (New York, New York: D. Appleton and Co., 1890), volume 3, part 2, p. 105.
    • See also Wikipedia's articles "Oxalis acetosella" and "Potassium hydrogen oxalate".
  11. ↑ See:
    • François Pierre Savary, Dissertatio Inauguralis De Sale Essentiali Acetosellæ [Inaugural dissertation on the essential salt of wood sorrel] (Jean François Le Roux, 1773). (in Latin) Savary noticed that when he distilled sorrel salt (potassium hydrogen oxalate), crystals would sublimate onto the receiver. From p. 17: "Unum adhuc circa liquorem acidum, quem sal acetosellae tam sincerissimum a nobis paratum quam venale destillatione fundit phoenomenon erit notandum, nimirum quod aliquid ejus sub forma sicca crystallina lateribus excipuli accrescat, ..." (One more [thing] will be noted regarding the acid liquid, which furnished for us sorrel salt as pure as commercial distillations, [it] produces a phenomenon, that evidently something in dry, crystalline form grows on the sides of the receiver, ...) These were crystals of oxalic acid.
    • Leopold Gmelin with Henry Watts, trans., Hand-book of Chemistry (London, England: Cavendish Society, 1855), volume 9, p. 111.
  12. ↑ See:
    • Torbern Bergman with Johan Afzelius (1776) Dissertatio chemica de acido sacchari [Chemical dissertation on sugar acid] (Uppsala, Sweden: Edman, 1776).
    • Torbern Bergman, Opuscula Physica et Chemica, (Leipzig (Lipsia), (Germany): I.G. Müller, 1776), volume 1, "VIII. De acido Sacchari," pp. 238–263.
  13. ↑ Carl Wilhelm Scheele (1784) "Om Rhabarber-jordens bestånds-delar, samt sått at tilreda Acetosell-syran" (On rhubarb-earth's constituents, as well as ways of preparing sorrel-acid), Kungliga Vetenskapsakademiens Nya Handlingar [New Proceedings of the Royal Academy of Science], 2nd series, 5 : 183-187. (in Swedish) From p. 187: "Således finnes just samma syra som vi genom konst af socker med tilhjelp af salpeter-syra tilreda, redan förut af naturen tilredd uti o̊rten Acetosella." (Thus it is concluded [that] the very same acid as we prepare artificially by means of sugar with the help of nitric acid, [was] previously prepared naturally in the herb acetosella [i.e., sorrel].)
  14. ↑ "OXALIQUE : Définition de OXALIQUE". www.cnrtl.fr. Retrieved 2024-09-27.
  15. ↑ See:
    • F. Wöhler (1824) "Om några föreningar af Cyan" (On some compounds of cyanide), Kungliga Vetenskapsakademiens Handlingar [Proceedings of the Royal Academy of Science], pp. 328–333. (in Swedish)
    • Reprinted in German as: F. Wöhler (1825) "Ueber Cyan-Verbindungen" (On cyanide compounds), Annalen der Physik und Chemie, 2nd series, 3 : 177-182.
  16. 1 2 3 Riemenschneider, Wilhelm; Tanifuji, Minoru (2000). "Oxalic Acid". Ullmann's Encyclopedia of Industrial Chemistry. doi:10.1002/14356007.a18_247. ISBN   3527306730.
  17. ↑ Eiichi, Yonemitsu; Tomiya, Isshiki; Tsuyoshi, Suzuki and Yukio, Yashima "Process for the production of oxalic acid", U.S. patent 3,678,107 , priority date March 15, 1969
  18. ↑ Von Wagner, Rudolf (1897). Manual of chemical technology. New York: D. Appleton & Co. p. 499.
  19. ↑ "Oxalic acid | Formula, Uses, & Facts | Britannica". 29 August 2024.
  20. ↑ Practical Organic Chemistry by Julius B. Cohen, 1930 ed. preparation #42
  21. ↑ Clarke H. T.;. Davis, A. W. (1941). "Oxalic acid (anhydrous)". Organic Syntheses : 421{{cite journal}}: CS1 maint: multiple names: authors list (link); Collected Volumes, vol. 1.
  22. ↑ Wells, A.F. (1984) Structural Inorganic Chemistry, Oxford: Clarendon Press. ISBN   0-19-855370-6.
  23. ↑ Sabine, T. M.; Cox, G. W.; Craven, B. M. (1969). "A neutron diffraction study of α-oxalic acid dihydrate". Acta Crystallographica Section B. 25 (12): 2437–2441. doi:10.1107/S0567740869005905.
  24. ↑ Ahmed, F. R.; Cruickshank, D. W. J. (1953). "A refinement of the crystal structure analyses of oxalic acid dihydrate". Acta Crystallographica. 6 (5): 385–392. doi: 10.1107/S0365110X53001083 .
  25. ↑ Bjerrum, J., et al. (1958) Stability Constants, Chemical Society, London.
  26. ↑ Haynes, W. M. (ed.). (2014). CRC Handbook of Chemistry and Physics, 95th ed., Boca Raton; London; New York: CRC Press.
  27. ↑ Clayton, G. D. and Clayton, F. E. (eds.). Patty's Industrial Hygiene and Toxicology, Volume 2A, 2B, 2C: Toxicology, 3rd ed., New York: John Wiley Sons, 1981–1982, p. 4936.
  28. ↑ Rumble, J. (ed.). (2019). CRC Handbook of Chemistry and Physics, 100th ed., CRC Press.
  29. ↑ Bowden, E. (1943). "Methyl oxalate". Organic Syntheses : 414; Collected Volumes, vol. 2.
  30. ↑ Sahoo, R. N.; Naik, P. K.; Das, S. C. (December 2001). "Leaching of manganese from low-grade manganese ore using oxalic acid as reductant in sulphuric acid solution". Hydrometallurgy. 62 (3): 157–163. Bibcode:2001HydMe..62..157S. doi:10.1016/S0304-386X(01)00196-7 . Retrieved 4 December 2021.
  31. ↑ DezhiQi (2018). "Extraction of Rare Earths From RE Concentrates". Hydrometallurgy of Rare Earths Separation and Extraction. pp. 1–185. doi:10.1016/B978-0-12-813920-2.00001-5. ISBN   9780128139202.
  32. ↑ Kovacs K. A.; Grof P.; Burai L.; Riedel M. (2004). "Revising the mechanism of the permanganate/oxalate reaction". Journal of Physical Chemistry A . 108 (50): 11026–11031. Bibcode:2004JPCA..10811026K. doi:10.1021/jp047061u.
  33. ↑ Higgins, James; Zhou, Xuefeng; Liu, Ruifeng; Huang, Thomas T.-S. (1997). "Theoretical Study of Thermal Decomposition Mechanism of Oxalic Acid". The Journal of Physical Chemistry A. 101 (14): 2702–2708. Bibcode:1997JPCA..101.2702H. doi:10.1021/jp9638191.
  34. ↑ Harkema, S.; Bats, J. W.; Weyenberg, A. M.; Feil, D. (1972). "The crystal structure of urea oxalic acid (2:1)". Acta Crystallographica Section B. 28 (5): 1646–1648. doi:10.1107/S0567740872004789.
  35. ↑ Dutton, M. V.; Evans, C. S. (1996). "Oxalate production by fungi: Its role in pathogenicity and ecology in the soil environment". Canadian Journal of Microbiology. 42 (9): 881–895. doi:10.1139/m96-114..
  36. ↑ Rombauer, Rombauer Becker, and Becker (1931/1997). Joy of Cooking, p.415. ISBN   0-684-81870-1.
  37. ↑ Siener, Roswitha; Honow, Ruth; Seidler, Ana; Voss, Susanne; Hesse, Albrecht (2006). "Oxalate contents of species of the Polygonaceae, Amaranthaceae, and Chenopodiaceae families". Food Chemistry. 98 (2): 220–224. doi:10.1016/j.foodchem.2005.05.059.
  38. ↑ Attenborough, David. "Surviving." The Private Life of Plants: A Natural History of Plant Behaviour. Princeton, NJ: Princeton UP, 1995. 265+. "OpenLibrary.org: The Private Life of Plants" Print.
  39. ↑ Sabbioni, Cristina; Zappia, Giuseppe (2016). "Oxalate patinas on ancient monuments: The biological hypothesis". Aerobiologia. 7: 31–37. doi:10.1007/BF02450015. S2CID   85017563.
  40. ↑ Frank-Kamemetskaya, Olga; Rusakov, Alexey; Barinova, Ekaterina; Zelenskaya, Marina; Vlasov, Dmitrij (2012). "The Formation of Oxalate Patina on the Surface of Carbonate Rocks Under the Influence of Microorganisms". Proceedings of the 10th International Congress for Applied Mineralogy (ICAM). pp. 213–220. doi:10.1007/978-3-642-27682-8_27. ISBN   978-3-642-27681-1.
  41. ↑ Dutton, Martin V.; Evans, Christine S. (1 September 1996). "Oxalate production by fungi: its role in pathogenicity and ecology in the soil environment". Canadian Journal of Microbiology. 42 (9): 881–895. doi:10.1139/m96-114.
  42. ↑ Gadd, Geoffrey M. (1 January 1999). "Fungal Production of Citric and Oxalic Acid: Importance in Metal Speciation, Physiology and Biogeochemical Processes". Advances in Microbial Physiology. 41. Academic Press: 47–92. doi:10.1016/S0065-2911(08)60165-4. ISBN   9780120277414. PMID   10500844.
  43. ↑ Strasser, Hermann; Burgstaller, Wolfgang; Schinner, Franz (June 1994). "High-yield production of oxalic acid for metal leaching processes by Aspergillus niger". FEMS Microbiology Letters. 119 (3): 365–370. doi: 10.1111/j.1574-6968.1994.tb06914.x . PMID   8050718. S2CID   39060069.
  44. ↑ Jan S. Tkacz, Lene Lange (2012): Advances in Fungal Biotechnology for Industry, Agriculture, and Medicine. 445 pages. ISBN   9781441988591
  45. ↑ Rigling, Daniel; Prospero, Simone (31 January 2017). "Cryphonectria parasitica, the causal agent of chestnut blight: invasion history, population biology and disease control". Molecular Plant Pathology. 19 (1): 7–20. doi: 10.1111/mpp.12542 . PMC   6638123 . PMID   28142223.
  46. ↑ Havir, Evelyn; Anagnostakis, Sandra (November 1983). "Oxalate production by virulent but not by hypovirulent strains of Endothia parasitica". Physiological Plant Pathology. 23 (3): 369–376. doi:10.1016/0048-4059(83)90021-8.
  47. ↑ Novoa, William; Alfred Winer; Andrew Glaid; George Schwert (1958). "Lactic Dehydrogenase V. inhibition by Oxamate and Oxalate". Journal of Biological Chemistry. 234 (5): 1143–8. doi: 10.1016/S0021-9258(18)98146-9 . PMID   13654335.
  48. ↑ Le, Anne; Charles Cooper; Arvin Gouw; Ramani Dinavahi; Anirban Maitra; Lorraine Deck; Robert Royer; David Vander Jagt; Gregg Semenza; Chi Dang (14 December 2009). "Inhibition of lactate dehydrogenase A induces oxidative stress and inhibits tumor progression". Proceedings of the National Academy of Sciences. 107 (5): 2037–2042. doi: 10.1073/pnas.0914433107 . PMC   2836706 . PMID   20133848.
  49. ↑ Lehner, A; Meimoun, P; Errakhi, R; Madiona, K; Barakate, M; Bouteau, F (September 2008). "Toxic and signalling effects of oxalic acid: Oxalic acid-Natural born killer or natural born protector?". Plant Signaling & Behavior. 3 (9): 746–8. doi:10.4161/psb.3.9.6634. PMC   2634576 . PMID   19704845.
  50. ↑ Daniel SL, Moradi L, Paiste H, Wood KD, Assimos DG, Holmes RP, et al. (August 2021). Julia Pettinari M (ed.). "Forty Years of Oxalobacter formigenes, a Gutsy Oxalate-Degrading Specialist". Applied and Environmental Microbiology. 87 (18): e0054421. Bibcode:2021ApEnM..87E.544D. doi:10.1128/AEM.00544-21. PMC   8388816 . PMID   34190610.
  51. ↑ Yu-Lun Lisa Fu (2008). Exploring New Methods for Varroa Mite Control. Michigan State University.
  52. ↑ Lee, Sung Oh; Tran, Tam; Jung, Byoung Hi; Kim, Seong Jun; Kim, Myong Jun (2007). "Dissolution of iron oxide using oxalic acid". Hydrometallurgy. 87 (3–4): 91–99. Bibcode:2007HydMe..87...91L. doi:10.1016/j.hydromet.2007.02.005.
  53. ↑ Jackson, Faith. "Quartz Crystal Cleaning". Archived 2013-10-29 at the Wayback Machine . bluemooncrystals.com.
  54. ↑ "Rock Currier – Cleaning Quartz". mindat.org
  55. ↑ Georgia Mineral Society. "Cleaning Pyrites". Archived 2023-06-05 at the Wayback Machine . www.gamineral.org.
  56. ↑ Keshavarz, Alireza; Parang, Zohreh; Nasseri, Ahmad (2013). "The effect of sulfuric acid, oxalic acid, and their combination on the size and regularity of the porous alumina by anodization". Journal of Nanostructure in Chemistry. 3. doi: 10.1186/2193-8865-3-34 . S2CID   97273964.
  57. ↑ Lowalekar, Viral Pradeep (2006). "Oxalic Acid Based Chemical Systems for Electrochemical Mechanical Planarization of Copper". UA Campus Repository. University of Arizona. Bibcode:2006PhDT........96L.
  58. ↑ Bouwman, Elisabeth; Angamuthu, Raja; Byers, Philip; Lutz, Martin; Spek, Anthony L. (July 15, 2010). "Electrocatalytic CO2 Conversion to Oxalate by a Copper Complex". Science. 327 (5393): 313–315. Bibcode:2010Sci...327..313A. CiteSeerX   10.1.1.1009.2076 . doi:10.1126/science.1177981. PMID   20075248. S2CID   24938351.
  59. ↑ Schuler, Eric; Demetriou, Marilena; Shiju, N. Raveendran; Gruter, Gert-Jan M. (2021-09-20). "Towards Sustainable Oxalic Acid from CO2 and Biomass". ChemSusChem. 14 (18): 3636–3664. doi:10.1002/cssc.202101272. ISSN   1864-5631. PMC   8519076 . PMID   34324259.
  60. ↑ All data not specifically annotated is from Agriculture Handbook No. 8-11, Vegetables and Vegetable Products, 1984. ("Nutrient Data : Oxalic Acid Content of Selected Vegetables". ars.usda.gov)
  61. 1 2 3 Chai, Weiwen; Liebman, Michael (2005). "Effect of Different Cooking Methods on Vegetable Oxalate Content". Journal of Agricultural and Food Chemistry. 53 (8): 3027–30. doi:10.1021/jf048128d. PMID   15826055.
  62. ↑ Pucher, GW; Wakeman, AJ; Vickery, HB (1938). "The organic acids of rhubarb (Rheum hybridium). III. The behavior of the organic acids during culture of excised leaves". Journal of Biological Chemistry. 126 (1): 43. doi: 10.1016/S0021-9258(18)73892-1 .
  63. ↑ Durham, Sharon. "Making Spinach with Low Oxalate Levels". AgResearch Magazine. No. January 2017. United States Department of Agriculture. Retrieved 26 June 2017. The scientists analyzed oxalate concentrations in 310 spinach varieties—300 USDA germplasm accessions and 10 commercial cultivars. "These spinach varieties and cultivars displayed oxalate concentrations from 647.2 to 1286.9 mg/100 g on a fresh weight basis," says Mou.
  64. ↑ "Oxalic Acid Material Safety Data Sheet" (PDF). Radiant Indus Chem. Archived from the original (PDF) on 2014-05-20. Retrieved 2014-05-20.
  65. ↑ "CDC – Immediately Dangerous to Life or Health Concentrations (IDLH): Oxalic acid – NIOSH Publications and Products". cdc.gov
  66. ↑ EMEA Committee for veterinary medicinal products, oxalic acid summary report, December 2003
  67. ↑ Patel, Mikita; Yarlagadda, Vidhush; Adedoyin, Oreoluwa; Saini, Vikram; Assimos, Dean G.; Holmes, Ross P.; Mitchell, Tanecia (May 2018). "Oxalate induces mitochondrial dysfunction and disrupts redox homeostasis in a human monocyte derived cell line". Redox Biology. 15: 207–215. doi:10.1016/j.redox.2017.12.003. PMC   5975227 . PMID   29272854.
  68. ↑ Singh, Prince; Enders, Felicity T.; Vaughan, Lisa E.; Bergstralh, Eric J.; Knoedler, John J.; Krambeck, Amy E.; Lieske, John C.; Rule, Andrew D. (October 2015). "Stone Composition Among First-Time Symptomatic Kidney Stone Formers in the Community". Mayo Clinic Proceedings. 90 (10): 1356–1365. doi:10.1016/j.mayocp.2015.07.016. PMC   4593754 . PMID   26349951.
This page is based on this Wikipedia article
Text is available under the CC BY-SA 4.0 license; additional terms may apply.
Images, videos and audio are available under their respective licenses.