Overview
Oxalate, also known as ethanedioate, is the conjugate base of oxalic acid and forms salts with various metals. It occurs naturally in many plants, such as spinach and rhubarb, and is also synthesized for industrial use. Oxalates are widely utilized in chemical processes due to their ability to form stable complexes with metal ions. In industrial settings, oxalates serve as reducing agents, bleaching agents, and chelating agents. Their ability to bind calcium makes them useful in water treatment and metal cleaning applications. However, excessive oxalate intake can lead to health issues, such as kidney stones, due to its insolubility with calcium in the body.
Physical and Chemical Properties
Oxalates are typically white crystalline solids with varying solubility in water, depending on the metal ion they are paired with. For example, sodium and potassium oxalates are highly soluble, while calcium oxalate is nearly insoluble. The density of oxalate salts ranges around 1.9 g/cm³, though this can vary. Chemically, oxalates act as reducing agents and can form coordination complexes with transition metals. They decompose upon heating, releasing carbon monoxide and carbon dioxide. The stability and reactivity of oxalates make them valuable in metallurgy, photography, and chemical synthesis.
Main Applications
Oxalates are used in textile and pulp industries as bleaching agents, where they help remove stains and brighten fabrics. In metal cleaning, oxalates dissolve rust and scale from surfaces, making them essential in maintenance and restoration. They are also employed in analytical chemistry as precipitants for calcium and other metal ions. In pharmaceuticals, oxalates serve as excipients or active ingredients in certain medications. Additionally, they are used in the production of rare earth metals and as catalysts in organic synthesis. Their chelating properties are exploited in water treatment to control metal ion concentrations.
Safety and Storage
Oxalates can be hazardous if inhaled, ingested, or exposed to skin and eyes. Proper personal protective equipment (PPE), such as gloves and goggles, should be worn when handling them. Ingestion can lead to systemic toxicity, including kidney damage, due to the formation of insoluble calcium oxalate crystals. Store oxalates in a cool, dry place, away from acids and oxidizing agents to prevent decomposition or hazardous reactions. Ensure containers are tightly sealed and labeled clearly. In case of spills, neutralize with a mild base and dispose of according to local regulations.
B2B Procurement Guide
When procuring oxalates, consider the required purity and solubility for your application. Industrial-grade oxalates are suitable for cleaning and metallurgy, while pharmaceutical-grade products require higher purity standards. Verify supplier certifications and compliance with regional safety regulations. Prices vary based on purity and quantity, typically ranging from $5 to $20 per kg. Bulk purchases may offer cost savings. Request material safety data sheets (MSDS) and test reports to ensure quality. For international shipments, confirm import/export restrictions and proper packaging to prevent contamination or degradation.
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