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Sodium oxalate
Names
Preferred IUPAC name
Other names
Oxalic acid, disodium salt
Identifiers
CAS Number
3D model (JSmol )
ChEBI
ChEMBL
ChemSpider
ECHA InfoCard 100.000.501
EC Number
PubChem CID
RTECS number
UNII
CompTox Dashboard (EPA )
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
Chemical formula
Na 2 C 2 O 4
Molar mass
−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]
Solubility in water
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
Crystal structure
monoclinic
Thermochemistry
Std enthalpy of (Δf H ⦵ 298 )
−1318 kJ/mol
Hazards
GHS labelling[3]
Pictograms
Signal word
Warning
Hazard statements
H302 , H312
Precautionary statements
P280 , P301+P312 , P302+P352
NFPA 704
Lethal dose or concentration (LD, LC):
LD 50 median dose )
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).
Infobox references
Chemical compound
Sodium oxalate , or disodium oxalate , is a chemical compound with the chemical formula Na 2 C 2 O 4 sodium salt of oxalic acid . It contains sodium cations Na + oxalate anions C 2 O 2− 4 °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 mineral form of sodium oxalate is natroxalate . It is only very rarely found and restricted to extremely sodic conditions of ultra-alkaline pegmatites .[4]
Preparation [ edit ]
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 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 NaHC2 O 4 , 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 [ edit ]
Sodium oxalate starts to decompose above 290 °C into sodium carbonate and carbon monoxide :[2]
Na 2 C 2 O 4 2 CO 3
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 Na 2 C 2 O 4 2 O 5 x V 2 O 5 x CO 2
with x
Sodium oxalate is used to standardize potassium permanganate solutions. It is desirable that the temperature of the titration mixture be greater than 60 °C to ensure that all the permanganate added reacts quickly. The kinetics of the reaction are complex, and the manganese (II ) ions (Mn 2+ 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 Na2 C 2 O 4 4 2 SO 4 K 2 SO 4 Na 2 SO 4 MnSO4 + 10 CO2 2 O
Biological activity [ edit ]
Like 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/kilogram of body weight (per MSDS ).
Sodium oxalate, like citrates , can also be used to remove calcium ions (Ca 2+ 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 .
References [ edit ]
^ a b c d Yoshimori T1, Asano Y, Toriumi Y, Shiota T. (1978) "Investigation on the drying and decomposition of sodium oxalate". Talanta , volume 25, issue 10, pages 603-605. doi :10.1016/0039-9140(78 )80158-1
^ GHS: GESTIS 570199
^ "Natroxolate" (PDF) . RRUFF . Mineral Data Publishing. Retrieved 7 January 2019 .
^ D. Ballivet-Tkatchenko, J. Galy, -M. Savariault (1994): "Thermal decomposition of sodium oxalate in the presence of V2O5: Mechanistic approach of sodium oxibronzes formation". Thermochimica Acta doi :10.1016/0040-6031(94 )80061-8
^ Mcbride, R. S. (1912). "The standardization of potassium permanganate solution by sodium oxalate" . J. Am. Chem. Soc. 34 4 ): 393–416. doi :10.1021/ja02205a009 .
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R e t r i e v e d f r o m " https://en.wikipedia.org/w/index.php?title=Sodium_oxalate&oldid=1199038071 " C a t e g o r i e s : ● O x a l a t e s ● S o d i u m c o m p o u n d s H i d d e n c a t e g o r i e s : ● A r t i c l e s w i t h o u t I n C h I s o u r c e ● A r t i c l e s w i t h o u t K E G G s o u r c e ● A r t i c l e s w i t h c h a n g e d E B I i d e n t i f i e r ● A r t i c l e s w i t h c h a n g e d C h e m S p i d e r i d e n t i f i e r ● E C H A I n f o C a r d I D f r o m W i k i d a t a ● A r t i c l e s w i t h c h a n g e d I n C h I i d e n t i f i e r ● C h e m b o x h a v i n g G H S d a t a ● A l l a r t i c l e s l a c k i n g r e l i a b l e r e f e r e n c e s ● A r t i c l e s l a c k i n g r e l i a b l e r e f e r e n c e s f r o m M a y 2 0 2 0 ● A r t i c l e s c o n t a i n i n g u n v e r i f i e d c h e m i c a l i n f o b o x e s ● A r t i c l e s w i t h s h o r t d e s c r i p t i o n ● S h o r t d e s c r i p t i o n m a t c h e s W i k i d a t a ● A l l a r t i c l e s w i t h u n s o u r c e d s t a t e m e n t s ● A r t i c l e s w i t h u n s o u r c e d s t a t e m e n t s f r o m A p r i l 2 0 1 7
● T h i s p a g e w a s l a s t e d i t e d o n 2 5 J a n u a r y 2 0 2 4 , a t 1 8 : 5 6 ( U T C ) . ● T e x t i s a v a i l a b l e u n d e r t h e C r e a t i v e C o m m o n s A t t r i b u t i o n - S h a r e A l i k e L i c e n s e 4 . 0 ;
a d d i t i o n a l t e r m s m a y a p p l y . B y u s i n g t h i s s i t e , y o u a g r e e t o t h e T e r m s o f U s e a n d P r i v a c y P o l i c y . W i k i p e d i a ® i s a r e g i s t e r e d t r a d e m a r k o f t h e W i k i m e d i a F o u n d a t i o n , I n c . , a n o n - p r o f i t o r g a n i z a t i o n . ● P r i v a c y p o l i c y ● A b o u t W i k i p e d i a ● D i s c l a i m e r s ● C o n t a c t W i k i p e d i a ● C o d e o f C o n d u c t ● D e v e l o p e r s ● S t a t i s t i c s ● C o o k i e s t a t e m e n t ● M o b i l e v i e w
