Sodium oxalate: Difference between revisions

Latest revision as of 11:41, 15 February 2025

Sodium oxalate[edit]

Sodium oxalate is a chemical compound with the formula Na₂C₂O₄. It is the sodium salt of oxalic acid, and it appears as a white, crystalline, odorless solid. Sodium oxalate is used in various applications, including as a reducing agent in chemical reactions and in the preparation of other oxalates.

Chemical properties[edit]

Sodium oxalate is a sodium salt of oxalic acid, and it is a dicarboxylate salt. It is soluble in water, and its aqueous solution is slightly basic due to the hydrolysis of the oxalate ion. The compound can act as a reducing agent, and it is often used in titrations as a primary standard for potassium permanganate solutions.

Uses[edit]

Sodium oxalate is used in various industrial and laboratory applications. It serves as a reducing agent in chemical processes and is used in the preparation of other oxalate compounds. In analytical chemistry, sodium oxalate is used as a standard in redox titrations, particularly with potassium permanganate.

Safety[edit]

Sodium oxalate is considered to be toxic if ingested, as it can cause hypocalcemia by binding to calcium ions in the body, forming insoluble calcium oxalate. This can lead to kidney stones and other health issues. Proper handling and storage are necessary to prevent accidental ingestion or exposure.

Related compounds[edit]

Related pages[edit]

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-'''Sodium oxalate''', also known as disodium oxalate, is an organic compound with the formula Na2C2O4. It is a white, crystalline, odorless solid that forms a monohydrate, Na2C2O4·H2O. Sodium oxalate is a salt of [[oxalic acid]], a dicarboxylic acid that occurs naturally in many plants and vegetables. It is used in various industrial processes, including the manufacture of certain dyes and bleaching agents, as well as in laboratories for the standardization of [[potassium permanganate]] solutions.
+{{DISPLAYTITLE:Sodium oxalate}}
-==Properties==
+== Sodium oxalate ==
-Sodium oxalate is soluble in water, with its solubility decreasing with the increase in temperature. It is practically insoluble in ethanol. When heated, it decomposes to form [[sodium carbonate]], carbon monoxide, and carbon dioxide. This compound acts as a reducing agent in chemical reactions and can form coordination compounds with transition metals.
+[[File:Sodium-oxalate-2D.png|thumb|right|Structural formula of sodium oxalate]]
+'''Sodium oxalate''' is a chemical compound with the formula Na<sub>2</sub>C<sub>2</sub>O<sub>4</sub>. It is the sodium salt of [[oxalic acid]], and it appears as a white, crystalline, odorless solid. Sodium oxalate is used in various applications, including as a reducing agent in chemical reactions and in the preparation of other oxalates.
-==Production==
+== Chemical properties ==
-Sodium oxalate can be produced by neutralizing oxalic acid with [[sodium hydroxide]] (NaOH) in a controlled environment. The reaction yields sodium oxalate and water. Industrially, it can also be generated as a byproduct in the processing of [[titanium dioxide]].
+Sodium oxalate is a [[sodium]] salt of [[oxalic acid]], and it is a [[dicarboxylate]] salt. It is soluble in water, and its aqueous solution is slightly basic due to the hydrolysis of the oxalate ion. The compound can act as a reducing agent, and it is often used in [[titration]]s as a primary standard for [[potassium permanganate]] solutions.
-==Uses==
+== Uses ==
-In the laboratory, sodium oxalate is primarily used as a primary standard for standardizing potassium permanganate solutions, a common titrant in [[redox titration]]s. Its precise known concentration and stability make it suitable for this purpose. Additionally, it finds application in the preparation of metal oxalates for electroplating and in the textile industry as a mordant.
+Sodium oxalate is used in various industrial and laboratory applications. It serves as a reducing agent in chemical processes and is used in the preparation of other oxalate compounds. In analytical chemistry, sodium oxalate is used as a standard in [[redox titration]]s, particularly with potassium permanganate.
-==Health and Safety==
+== Safety ==
-Sodium oxalate is toxic if ingested, inhaled, or upon contact with skin. It can cause irritation to the skin, eyes, and respiratory system. Ingestion of sodium oxalate can lead to serious health issues, including renal failure, due to the formation of insoluble calcium oxalate crystals that can damage the kidneys. Safety measures include wearing protective clothing, gloves, and eye protection when handling the substance. In case of exposure, immediate medical attention is necessary.
+Sodium oxalate is considered to be toxic if ingested, as it can cause [[hypocalcemia]] by binding to calcium ions in the body, forming insoluble calcium oxalate. This can lead to [[kidney stones]] and other health issues. Proper handling and storage are necessary to prevent accidental ingestion or exposure.
-==Environmental Impact==
+== Related compounds ==
-The environmental impact of sodium oxalate is primarily associated with its potential to form insoluble oxalate salts with heavy metals, which can persist in the environment. Proper disposal methods should be employed to minimize its environmental footprint.
+* [[Oxalic acid]]
+* [[Calcium oxalate]]
+* [[Potassium oxalate]]
-[[Category:Chemical compounds]]
+== Related pages ==
+* [[Oxalate]]
+* [[Sodium carbonate]]
+* [[Sodium bicarbonate]]
+[[Category:Oxalates]]
 [[Category:Sodium compounds]]
-[[Category:Organic salts]]
-{{Chem-stub}}