Oxalic acid (CAS: 6153-56-6)

 

Item	Index
Appearance	Heavy white powder
Purity %≥	99.5
Sulfate (SO4) %≤	0.002
Residue on ignition  (as sulfate) %≤	0.02
Chloride (Cl) %≤	0.002
Total nitrogen (N) %≤	0.002
Water insoluble %≤	0.005
Heavy metals (as Pb) %≤	0.0004
Calcium (Ca) %≤	0.003
Iron (Fe) %≤	0.0005
Clarity test / No. ≤	3

 

Oxalic acid is an organic compound with the formula H2C2O4. It is a colorless crystalline solid that

dissolves in water to give colorless solutions. It is classified as a dicarboxylic acid. In terms of acid strength,

it is much stronger than acetic acid. Oxalic acid is a reducing agent  and its conjugate base, known as oxalate 

(C2O42−), is a chelating agent for metal cations. Typically, oxalic acid occurs as the dihydratewith the formula

H2C2O4·2H2O. Oral consumption of oxalic acid in excess or prolonged skin contact can be dangerous.

Preparation

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.[4] 

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.

Historically oxalic acid was obtained exclusively by using caustics, such as sodium or potassium hydroxide, on sawdust.

Laboratory methods

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.

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

Of historical interest, Wöhler prepared oxalic acid by hydrolysis of cyanogen in 1824. This experiment may

represent the first synthesis of anatural product.

Structure

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. Because the anhydrous

material is both acidic and hydrophilic (water seeking), it is used inesterifications.

Reactions

Oxalic acid is a relatively strong acid, despite being a carboxylic acid:

C2O4H2 → C2O4H− + H+; pKa = 1.27C2O4H− → C2O42− + H+; pKa = 4.27

Oxalic acid undergoes many of the reactions characteristic of other carboxylic acids. It forms esters such as 

dimethyl oxalate (m.p. 52.5 to 53.5 °C (126.5 to 128.3 °F)). It forms an acid chloride called oxalyl chloride.

Oxalate, the conjugate base of oxalic acid, is an excellent ligand for metal ions, e.g. the drug oxaliplatin.

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

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:

[O2CC(O)CH2CO2]2− + H2O → C2O42− + CH3CO2−

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

Occurrence in foods and plants

Calcium oxalate is the most common component of kidney stones. Early investigators isolated oxalic acid from 

wood-sorrel (Oxalis). Members of thespinach family are high in oxalates, as is sorrel. Rhubarb leaves contain

about 0.5% oxalic acid and jack-in-the-pulpit (Arisaema triphyllum) contains calcium oxalate crystals. Bacteria

produce oxalates from oxidation of carbohydrates.

Plants of the fenestraria genus produce optical fibers made from crystalline oxalic acid to transmit light to

subterranean photosynthetic sites.

Other

Oxidized bitumen or bitumen exposed to gamma rays also contains oxalic acid among its degradation products.

Oxalic acid may increase the leaching of radionuclides conditioned in bitumen for radioactive waste disposal.

[citation needed]

Biochemistry

The conjugate base of oxalic acid (oxalate) is a competitive inhibitor of the lactate dehydrogenase(LDH) enzyme.

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 throughglycolysis. As cancer cells preferentially use anaerobic metabolism

(see Warburg effect) inhibition of LDH has been shown to inhibit tumor formation and growth,thus is an interesting

potential course of cancer treatment.

Applications

About 25% of produced oxalic acid is used as a mordant in dyeing processes. It is used in bleaches, especially

for pulpwood. It is also used in baking powder.

Cleaning

Oxalic acid’s main applications include cleaning or bleaching, especially for the removal of rust (iron complexing agent),

e.g. Bar Keepers Friend is an example of a household cleaner containing oxalic acid. Its utility in rust removal agents

is due to its forming a stable, water soluble salt with ferric iron, ferrioxalate ion.

Extractive metallurgy

Oxalic acid is an important reagent in lanthanide chemistry. Hydrated lanthanide oxalates form readily in strongly acidic

solutions in a densely crystalline, easily filtered form, largely free of contamination by nonlanthanide elements. Thermal

decomposition of these oxalate gives the oxides, which is the most commonly marketed form of these elements.

Niche uses

Vaporized oxalic acid, or a 3.2% solution of oxalic acid in sugar syrup, is used by some beekeepers as a 

miticide against the parasitic varroa mite.

Oxalic acid is rubbed onto completed marble sculptures to seal the surface and introduce a shine. Oxalic acid

is also used to clean iron and manganese deposits from quartz crystals.

Toxicity and safety

Oxalic acid has toxic effects through contact and if ingested; manufacturers provide details in Material Safety

Data Sheets (MSDS). It is not identified as mutagenic or carcinogenic; there is a possible risk of congenital

malformation in the fetus; may be harmful if inhaled, and is extremely destructive to tissue of mucous membranes

 and upper respiratory tract; harmful if swallowed; harmful to and destructive of tissue and causes burns if absorbed

through the skin or is in contact with the eyes. Symptoms and effects include a burning sensation, cough, wheezing, 

laryngitis, shortness of breath, spasm, inflammation and edema of the larynx, inflammation and edema of the bronchi, 

pneumonitis, pulmonary edema.

In humans, ingested oxalic acid has an oral LDLo (lowest published lethal dose) of 600 mg/kg. It has been reported that

the lethal oral dose is 15 to 30 grams.

The toxicity of oxalic acid is due to kidney failure caused by precipitation of solid calcium oxalate, the main

component of kidney stones. Oxalic acid can also cause joint pain due to the formation of similar precipitates

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