Sodium+Carbonate

Also known as washing soda or soda ash.
==Sodium carbonate is domestically well known for its everyday use as a water softener. It can be extracted from the ashes of many plants. It is synthetically produced in large quantities from salt and limestone in a process known as the Solvay process. It most commonly occurs as a crystalline heptahydrate which readily forms a white powder.== Sodium carbonate can react with calcium hydroxide producing sodium hydroxide and calcium carbonate. Sodium carbonate can react with carbon dioxide and water producing calcium bicarbonate. There are two categories of reaction between sodium carbonate and hydrochloric acid: Less hydrochloric acid: Na2CO3+ HCl ==== NaCl + NaHCO3 More hydrochloric acid: Na2CO3+ 2HCl ==== 2NaCl + H2O + CO2 In chemical lab sodium carbonate is prepared by treating sodium hydroxide and carbon dioxide. 2NaOH + CO2==== Na2CO3+ H2O

Uses:
Sodium Carbonate is a strong base and is used in pool to cancel the acidic effect of Chlorine and to raise the PH

The manufacture of glass is one of the most important uses of sodium carbonate. When combined with silica and calcium carbonate and heated to high temperatures, then cooled rapidly, glass is produced. This type of glass is known as soda lime glass.

It is used in toothpastes, where it acts as a foaming agent and an abrasive, and to temporarily increase mouth pH. It is a common additive in municipal pools used to neutralize the acidic effects of chlorine and raise pH. In cooking it is sometimes used in place of sodium hydroxide for lyeing, especially with German pretzels. These dishes are treated with a solution of alkaline substance in order to change the pH of the surface of the food and improve browning.