Oxalate

Oxalate

The structure of the oxalate anion
A ball-and-stick model of oxalate
Names
Preferred IUPAC name Oxalate[1][2]
Other names oxalate ion,[1] ethanedioic acid dianion, oxalic acid dianion,[2] ethanedioate[3]
Identifiers
CAS Number	338-70-5 [4][2]
3D model (JSmol)	Interactive image
Beilstein Reference	1905970[12][13]
ChEBI	CHEBI:30623 [1][5]
ChemSpider	64235 [1]
Gmelin Reference	2207[14]
KEGG	C00209 [6]
PubChem CID	71081 [2]
show InChI InChI=1S/C2H2O4/c3-1(4)2(5)6/h(H,3,4)(H,5,6)/p-2 Key: MUBZPKHOEPUJKR-UHFFFAOYSA-L[8] [9]: InChI=1S/C2H2O4/c3-1(4)2(5)6/h(H,3,4)(H,5,6)/p-2 Key: MUBZPKHOEPUJKR-UHFFFAOYSA-L[10][11]
show SMILES C(=O)(C(=O)[O-])[O-]
Properties
Chemical formula	C 2O2− 4[18]
Molar mass	88.019 g·mol−1[15][16]
Conjugate acid	Hydrogenoxalate[17]
Structure
Point group	D2h
Related compounds
Related isoelectronic	dinitrogen tetroxide
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
Infobox references

Oxalate (IUPAC: ethanedioate) is a compound found in some foods, which when consumed exits the body through the urine. Excess consumption has been linked to gout and kidney stones. Many metal ions form insoluble precipitates with oxalate, a prominent example being calcium oxalate, the primary constituent of the most common kind of kidney stones. Several plant foods such as the root and/or leaves of spinach, rhubarb, and buckwheat are high in oxalic acid and can contribute to the formation of kidney stones in some individuals. Chemically, oxalate is a dianion with the formula C
₂O²⁻
₄, also written (COO)²⁻
₂. Either name is often used for derivatives, such as salts of oxalic acid, for example sodium oxalate Na₂C₂O₄, or dimethyl oxalate ((CH₃)₂C₂O₄). Oxalate also forms coordination compounds where it is sometimes abbreviated as ox.

Relationship to oxalic acid[]

The dissociation of protons from oxalic acid proceeds in a stepwise manner as for other polyprotic acids. Loss of a single proton results in the monovalent hydrogenoxalate anion HC
₂O⁻
₄. A salt with this anion is sometimes called an acid oxalate, monobasic oxalate, or hydrogen oxalate. The equilibrium constant (K_a) for loss of the first proton is 5.37×10⁻² (pK_a = 1.27). The loss of the second proton, which yields the oxalate ion, has an equilibrium constant of 5.25×10⁻⁵ (pK_a = 4.28). These values imply, in solutions with neutral pH, no oxalic acid and only trace amounts of hydrogen oxalate exist.^[19] The literature is often unclear on the distinction between H₂C₂O₄, HC
₂O⁻
₄, and C
₂O²⁻
₄, and the collection of species is referred to as oxalic acid.

Structure[]

X-ray crystallography of simple oxalate salts show that the oxalate anion may adopt either a planar conformation with D_2h molecular symmetry, or a conformation where the O–C–C–O dihedrals approach 90° with approximate D_2d symmetry.^[20] Specifically, the oxalate moiety adopts the planar, D_2h conformation in the solid-state structures of M₂C₂O₄ (M = Li, Na, K).^[21][22] However, in structure of Cs₂C₂O₄ the O–C–C–O dihedral angle is 81(1)°.^[23][24] Therefore, Cs₂C₂O₄ is more closely approximated by a D_2d symmetry structure because the two CO₂ planes are staggered. Two forms of Rb₂C₂O₄ have been structurally characterized by single-crystal X-ray diffraction; one contains a planar and the other a staggered oxalate.

As the preceding examples indicate that the conformation adopted by the oxalate dianion is dependent upon the size of the alkali metal to which it is bound, some have explored the barrier to rotation about the central C−C bond. The barrier to rotation about this bond was determined computationally to be roughly 2–6 kcal/mol for the free dianion, C
₂O²⁻
₄.^[25][26][27] Such results are consistent with the interpretation that the central carbon–carbon bond is best regarded as a single bond with only minimal pi interactions between the two CO⁻
₂ units.^[20] This barrier to rotation about the C−C bond (which formally corresponds to the difference in energy between the planar and staggered forms) may be attributed to electrostatic interactions as unfavorable O−O repulsion is maximized in the planar form.

Importantly, oxalate is often encountered as a bidentate, chelating ligand, such as in potassium ferrioxalate. When the oxalate chelates to a single metal center, it always adopts the planar conformation.

Occurrence in nature[]

Oxalate occurs in many plants, where it is synthesized by the incomplete oxidation of carbohydrates.

Oxalate-rich plants include fat hen ("lamb's quarters"), sorrel, and several Oxalis species. The root and/or leaves of rhubarb and buckwheat are high in oxalic acid.^[28] Other edible plants that contain significant concentrations of oxalate include, in decreasing order, star fruit (carambola), black pepper, parsley, poppy seed, amaranth, spinach, chard, beets, cocoa, chocolate, most nuts, most berries, fishtail palms, New Zealand spinach (Tetragonia tetragonioides), and beans.^{[citation needed]} Leaves of the tea plant (Camellia sinensis) contain among the greatest measured concentrations of oxalic acid relative to other plants. However, the beverage derived by infusion in hot water typically contains only low to moderate amounts of oxalic acid due to the small mass of leaves used for brewing.

Physiological effects[]

Scanning electron micrograph of the surface of a kidney stone showing tetragonal crystals of weddellite (calcium oxalate dihydrate) emerging from the amorphous central part of the stone; the horizontal length of the picture represents 0.5 mm of the figured original.

In the body, oxalic acid combines with divalent metallic cations such as calcium (Ca²⁺) and iron(II) (Fe²⁺) to form crystals of the corresponding oxalates which are then excreted in urine as minute crystals. These oxalates can form larger kidney stones that can obstruct the kidney tubules. An estimated 80% of kidney stones are formed from calcium oxalate.^[30] Those with kidney disorders, gout, rheumatoid arthritis, or certain forms of chronic vulvar pain (vulvodynia) are typically advised to avoid foods high in oxalic acid.^{[citation needed]} Methods to reduce the oxalate content in food are of current interest.^[31]

Magnesium (Mg²⁺) oxalate (K_sp = 8.5×10⁻⁵) is 177 times more soluble than calcium oxalate (K_sp = 2.7×10⁻⁹).^[32] Indeed, the ratio of their respective solubility (S) is equal to the square root of the ratio of their respective solubility products:

${\displaystyle {\frac {S_{\mathrm {Mg} }}{S_{\mathrm {Ca} }}}={\sqrt {\frac {K_{\mathrm {sp(Mg)} }}{K_{\mathrm {sp(Ca)} }}}}}$

So, calcium oxalate is more likely to precipitate out when magnesium levels are low and calcium and oxalate levels are high. Magnesium oxalate is a million times more soluble than mercury oxalate. Oxalate solubility for metals decreases in the order Mg > Ca > Cd > Zn > {Mn, Ni, Fe, Cu} > {As, Sb, Pb} > Hg.^{[dubious – discuss]}

The highly insoluble iron(II) oxalate appears to play a major role in gout, in the nucleation and growth of the otherwise extremely soluble sodium urate. This explains why gout usually appears after age 40,^[33] when ferritin levels in blood exceed 1 μg/L^{[citation needed]}. Foods high in oxalate^[34] should be avoided by people suffering from, or at risk of gout.^[35]

Cadmium catalyzes the transformation of vitamin C into oxalic acid. This can be a problem for people exposed to high levels of cadmium in their diets, in the workplace, or through smoking.

In studies with rats, calcium supplements given along with foods high in oxalic acid can cause calcium oxalate to precipitate in the gut and reduce the levels of oxalate absorbed by the body (by 97% in some cases).^[36][37]

Oxalic acid can also be produced by the metabolism of ethylene glycol ("antifreeze"), glyoxylic acid, or ascorbic acid (vitamin C).^{[38][dubious – discuss]}

Powdered oxalate is used as a pesticide in beekeeping to combat the bee mite.

Some fungi of the genus Aspergillus produce oxalic acid.^[39]

Some preliminary evidence indicates the administration of probiotics can affect oxalic acid excretion rates in a positive manner.^[40]

As a ligand[]

Oxalate, the conjugate base of oxalic acid, is an excellent ligand for metal ions. It usually binds as a bidentate ligand forming a 5-membered MC₂O₂ ring. An illustrative complex is potassium ferrioxalate, K₃[Fe(C₂O₄)₃]. The drug oxaliplatin exhibits improved water solubility relative to older platinum-based drugs, avoiding the dose-limiting side-effect of nephrotoxicity. Oxalic acid and oxalates can be oxidized by permanganate in an autocatalytic reaction. One of the main applications of oxalic acid is rust-removal, which arises because oxalate forms water-soluble derivatives with the ferric ion.

Excess[]

An excess oxalate level in the blood is termed hyperoxalemia, and high levels of oxalate in the urine is termed hyperoxaluria.

Acquired[]

Although unusual, consumption of oxalates (for example, the grazing of animals on oxalate-containing plants such as Bassia hyssopifolia, or human consumption of wood sorrel or, specifically in excessive quantities, black tea) may result in kidney disease or even death due to oxalate poisoning. The New England Journal of Medicine reported acute oxalate nephropathy "almost certainly due to excessive consumption of iced tea" in a 56-year-old man, who drank "sixteen 8-ounce glasses of iced tea daily" (roughly 3.8 liters). The authors of the paper hypothesized that acute oxalate nephropathy is an underdiagnosed cause of kidney failure and suggested thorough examination of patient dietary history in cases of unexplained kidney failure without proteinuria (an excess of protein in the urine) and with large amounts of calcium oxalate in urine sediment.^[41] Oxalobacter formigenes in the gut flora may help alleviate this.^[42]

Congenital[]

Primary hyperoxaluria is a rare, inherited condition, resulting in increased excretion of oxalate, with oxalate stones being common.

See also[]

• Dimethyl oxalate – (CH₃)₂C₂O₄
• Diphenyl oxalate – (C₆H₅)₂C₂O₄
• Potassium ferrioxalate – K₃[Fe(C₂O₄)₃], an iron complex with oxalate ligands
• Praseodymium oxalate – C
  ₆O
  ₁₂Pr
  ₂
• Raphide
• Sodium oxalate – Na₂C₂O₄
• Iron(II) oxalate - FeC₂O₄•xH₂O

References[]

Further reading[]

• Euler. "K_sp Table: Solubility product constants near 25 °C". chm.uri.edu. Retrieved 10 June 2021.
• Ibis, Fatma; Dhand, Priya; Suleymanli, Sanan; van der Heijden, Antoine E. D. M.; Kramer, Herman J. M.; Eral, Huseyin Burak (2020). "A combined experimental and modelling study on solubility of calcium oxalate monohydrate at physiologically relevant pH and temperatures". Crystals. 10 (10): 924. doi:10.3390/cryst10100924. ISSN 2073-4352.
• Ulmgren, Per; Rådeström, Rune (1999). "Solubility of calcium oxalate in the presence of magnesium ions, and solubility of magnesium oxalate in sodium chloride medium". Nordic Pulp & Paper Research Journal. 14 (4): 330–335. doi:10.3183/npprj-1999-14-04-p330-335. ISSN 2000-0669.

External links[]

• Oxalate.org - Oxalate content of 750+ foods from university and government sources