Sodium Carbonate

  • Sodium carbonate (\(\ce{NaCO3}\)) is also called as ‘soda ash’, or ‘washing soda’. 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”.

  • Industrial production of sodium carbonate is from sodium chloride and limestone by the “Solvay process”.

  • In terms of its largest applications, sodium carbonate is used in the manufacture of glass, paper, rayon, soaps, and detergents. Sodium carbonate is a food additive used as an acidity regulator, anticaking agent, raising agent, and stabilizer.

  • Sodium carbonate is also used as a relatively strong base in various fields. As a common alkali, it is preferred in many chemical processes because it is cheaper than \(\ce{NaOH}\) and far safer to handle. Its mildness especially recommends its use in domestic applications.

  • Sodium bicarbonate (\(\ce{NaHCO3}\)) or baking soda, also a component in fire extinguishers, is often generated from sodium carbonate. Although \(\ce{NaHCO3}\) is itself an intermediate product of the Solvay process, the heating needed to remove the ammonia that contaminates it decomposes some \(\ce{NaHCO3}\), making it more economical to react finished \(\ce{Na2CO3}\) with \(\ce{CO2}\):

    \[\ce{Na2CO3} + \ce{CO2} + \ce{H2O} \rightarrow \ce{2NaHCO3}\]