Sodium oxalate

Source: Wikipedia, the free encyclopedia.
Sodium oxalate
Disodium oxalate
Names
Preferred IUPAC name
Disodium oxalate
Other names
Oxalic acid, disodium salt
Sodium ethanedioate
Identifiers
3D model (
JSmol
)
ChEBI
ChEMBL
ChemSpider
ECHA InfoCard
 100.000.501 Edit this at Wikidata
EC Number
  • 200-550-3
RTECS number
  • K11750000
UNII
  • InChI=1S/C2H2O4.2Na/c3-1(4)2(5)6;;/h(H,3,4)(H,5,6);;/q;2*+1/p-2 ☒N
    Key: ZNCPFRVNHGOPAG-UHFFFAOYSA-L ☒N
  • C(=O)(C(=O)[O-])[O-].[Na+].[Na+]
Properties
Na2C2O4
Molar mass 133.998 g·mol−1
Appearance White crystalline solid
Odor Odorless
Density 2.34 g/cm3
Melting point 260 °C (500 °F; 533 K) decomposes above 290 °C[2]
  • 2.69 g/(100 mL) (0 °C)
  • 3.7 g/(100 mL) (20 °C)
  • 6.25 g/(100 mL) (100 °C)
Solubility Soluble in formic acid, insoluble in ethanol, diethyl ether
Structure
monoclinic
Thermochemistry
Std enthalpy of
formation
(ΔfH⦵298)
 −1318 kJ/mol
Hazards
GHS labelling:[3]
GHS07: Exclamation mark
Warning
H302, H312
P280, P301+P312, P302+P352
NFPA 704 (fire diamond)
NFPA 704 four-colored diamondHealth 1: Exposure would cause irritation but only minor residual injury. E.g. turpentineFlammability 0: Will not burn. E.g. waterInstability 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g. liquid nitrogenSpecial hazards (white): no code
1
0
0
Lethal dose or concentration (LD, LC):
11160 mg/kg (oral, rat)[1]
Safety data sheet (SDS) Oxford MSDS [unreliable source]
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
☒N verify (what is checkY☒N ?)

Sodium oxalate, or disodium oxalate, is a

°C.[2]

Sodium oxalate can act as a reducing agent, and it may be used as a primary standard for standardizing potassium permanganate (KMnO4) solutions.

The

alkaline pegmatites.[4]

Preparation

Sodium oxalate can be prepared through the neutralization of oxalic acid with sodium hydroxide (NaOH) in a 1:2 acid-to-base molar ratio. Evaporation yields the anhydrous oxalate[5] that can be thoroughly dried by heating to between 200 and 250 °C.[2]

Half-neutralization can be accomplished with NaOH in a 1:1 ratio which produces NaHC2O4, monobasic sodium oxalate or sodium hydrogenoxalate.

Alternatively, it can be produced by decomposing sodium formate by heating it at a temperature exceeding 360 °C.[citation needed]

Reactions

Sodium oxalate starts to decompose above 290 °C into sodium carbonate and carbon monoxide:[2]

Na2C2O4 → Na2CO3 + CO

When heated at between 200 and 525°C with

vanadium pentoxide in a 1:2 molar ratio, the above reaction is suppressed, yielding instead a sodium vanadium oxibronze with release of carbon dioxide[6]

x Na2C2O4 + 2 V2O5 → 2 NaxV2O5 + 2x CO2

with x increasing up to 1 as the temperature increases.

Sodium oxalate is used to standardize

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:[7]

5 Na2C2O4 + 2 KMnO4 + 8 H2SO4 → K2SO4 + 5 Na2SO4 + 2 MnSO4 + 10 CO2 + 8 H2O

Biological activity

Like several other

MSDS
).

Sodium oxalate, like

kidneys
.

References

  1. ^ a b "ChemIDplus - 62-76-0 - ZNCPFRVNHGOPAG-UHFFFAOYSA-L - Disodium oxalate - Similar structures search, synonyms, formulas, resource links, and other chemical information". chem.nlm.nih.gov. NIH. Retrieved 7 January 2019.
  2. ^
    doi:10.1016/0039-9140(78)80158-1
  3. ^ GHS: GESTIS 570199
  4. ^ "Natroxolate" (PDF). RRUFF. Mineral Data Publishing. Retrieved 7 January 2019.
  5. doi:10.2475/ajs.s5-26.151.16
  6. doi:10.1016/0040-6031(94)80061-8
  7. doi:10.1021/ja02205a009
    .
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