ChemicalBook > Product Catalog > Organic Chemistry > Carboxylic acids and derivatives > Carboxylic Acid Salts > Sodium oxalate
Sodium oxalate Chemical Properties
- Melting point:250-270 °C
- Density 2.34
- storage temp. Store at RT.
- solubility H2O: 0.1 M at 20 °C, clear, colorless
- form Powder
- color White
- PH7-8.5 (25℃, 2.5% in H2O)
- Water Solubility 37 g/L (20 ºC)
- Sensitive Hygroscopic
- Merck 14,8650
- BRN 3631622
- Stability:Stability Stable; hygroscopic. Incompatible with strong oxidizing agents.
- CAS DataBase Reference62-76-0(CAS DataBase Reference)
- NIST Chemistry ReferenceSodium oxalate(62-76-0)
- EPA Substance Registry SystemSodium oxalate (62-76-0)
Sodium oxalate Usage And Synthesis
- Physical PropertiesWhite crystalline powder; density 2.34 g/cm3; decomposes around 250° C; sparingly soluble in water, 3.7 g/100 mL at room temperature; moderately soluble in boiling water, about 6.25 g/100 mL; the aqueous solution is practically neutral; insoluble in alcohol
- UsesSodium oxalate is used as an analytical standard for standardization of potassium permanganate and other strong oxidizing agents. It also is used in finishing textiles, tanning leather, and blue printing.
- PreparationSodium oxalate can be made by heating sodium formate at about 250°C:
2HCOONa → Na2C2O4 + H2
It also can be prepared by reacting oxalic acid with a dilute aqueous solution of sodium hydroxide followed by evaporation and crystallization.
- DescriptionSodium oxalate, or disodium oxalate, is the sodium salt of oxalic acid with the molecular formula Na2C2O4. It is usually a white, crystalline, odorless powder, that decomposes at 250–270 °C.
Disodium oxalate can act as a reducing agent, and it may be used as a primary standard for standardizing potassium permanganate (KMnO4) solutions.
The mineral form of sodium oxalate is natroxalate. It is only very rarely found and restricted to extremely sodic conditions of ultraalkaline pegmatites.
- Chemical PropertiesWhite, crystalline powder. Soluble in water; insolu- ble in alcohol.
- Physical propertiesWhite crystalline powder; density 2.34 g/cm3; decomposes around 250° C; sparingly soluble in water, 3.7 g/100 mL at room temperature; moderately soluble in boiling water, about 6.25 g/100 mL; the aqueous solution is practically neutral; insoluble in alcohol.
- UsesSodium Oxalate is obtained in such high purity and is so stable that it is used as a titrimetric standard.
- UsesFinishing textiles, tanning and finishing leather; for standardizing potassium permanganate solution.
- DefinitionChEBI: An organic sodium salt consisting of sodium and oxalate ions in a 2:1 ratio.
- PreparationSodium oxalate can be prepared through the neutralization of oxalic acid with sodium hydroxide (NaOH) in a 1:2 acid-to-base molar ratio. Half-neutralization can be accomplished with NaOH in a 1:1 ratio which produces NaHC2O4, monobasic sodium oxalate or sodium hydrogenoxalate.
- ReactionsSodium oxalate is used to standardize potassium permanganate solutions. It is desirable that the temperature of the titration mixture is greater than 60 °C to ensure that all the permanganate added reacts quickly. The kinetics of the reaction is complex, and the manganate (II) ions formed catalyze the further reaction between permanganate and oxalic acid (formed in situ by the addition of excess sulfuric acid). The final equation is as follows:
5Na2C2O4 + 2KMnO4 + 8H2SO4 → K2SO4 + 2MnSO4 + 10CO2 + 8H2O.
- General DescriptionOdorless white solid. Sinks and mixes slowly with water.
- Reactivity ProfileDisodium oxalate gives basic aqueous solutions. Neutralizes acids in exothermic reactions. Can serve as a reducing agent in reactions that generate carbon dioxide.
- HazardToxic by ingestion.
- Health HazardInhalation or ingestion causes pain in throat, esophagus, and stomach; mucous membranes turn white; other symptoms include vomiting, severe purging, weak pulse, cardiovascular collapse, neuromuscular symptoms, and kidney damage. Contact with eyes or skin causes irritation.
- ToxicologyLike several other oxalates, sodium oxalate is toxic to humans. It can cause burning pain in the mouth, throat and stomach, bloody vomiting, headache, muscle cramps, cramps and convulsions, drop in blood pressure, heart failure, shock, coma, and possible death. Mean lethal dose by ingestion of oxalates is 10-15 grams (per MSDS).
Sodium oxalate, like citrates, can also be used to remove calcium ions (Ca2+) from blood plasma. It also prevents blood from clotting. Note that by removing calcium ions from the blood, sodium oxalate can impair brain function, and deposit calcium oxalate in the kidneys.
- Purification MethodsIt crystallises from hot water (16mL/g) by cooling to 0o. Before use as a volumetric standard, analytical grade quality sodium oxalate should be dried for 2hours at 120o and allowed to cool in a desiccator. [Beilstein 2 IV 1819.]
Sodium oxalate Preparation Products And Raw materials
- Hexafluorosilicic acid FERROUS SULFATE Iron(III) sodium oxalate OXALIC ACID Oxalic acid dihydrate AMMONIUM SODIUM OXALATE SODIUM OXALATE (REDUCTOMETRIC) FERRIC SODIUM OXALATE SODIUM OXALATE, ACS UN2811- Sodium orthovanadate Sodium bioxalate monohydrate Iron(Ⅲ) sodium oxalate Sodium oxalate Sodium glycolate SODIUM GLYOXYLATE SODIUM OXALATE-13C2, 99 ATOM % 13C,SODIUM OXALATE-13C2 Oxalic acid
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