Sodium carbonate

Sodium carbonate (also known as washing soda, soda ash and soda crystals), is the inorganic compound with the formula Na2CO3 and its various hydrates. All forms are white, water-soluble salts that yield moderately alkaline solutions in water. Historically it was extracted from the ashes of plants growing in sodium-rich soils. Because the ashes of these sodium-rich plants were noticeably different from ashes of wood (once used to produce potash), sodium carbonate became known as "soda ash". It is produced in large quantities from sodium chloride and limestone by the Solvay process.

Production

Sodium carbonate is produced by the Solvay process in industrial settings but can also be produced in a laboratory. The process involves the reaction of sodium chloride, ammonia and carbon dioxide in water, followed by a second reaction with calcium carbonate. The resulting product is then crystallized to produce sodium carbonate.

Uses

Sodium carbonate is used in a variety of applications, including the production of glass, paper, rayon, soaps, and detergents. It's also used in the food industry as a food additive and in the home as a water softener.

Health effects

Exposure to sodium carbonate can cause irritation to the eyes, skin, and respiratory tract. It can cause severe burns and eye damage in high concentrations. Ingestion can lead to gastrointestinal irritation and systemic effects.

See also

• Sodium bicarbonate
• Sodium chloride
• Solvay process

References

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  Sodium carbonate structure

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  Sodium carbonate monohydrate