Bicarbonate

Bicarbonate alkalinity HCO₃^–  is present if the phenolphthalein alkalinity is less than half of the total alkalinity. In other words, it is a very common mineral ion in water that is naturally found in surface water, groundwater, and mineral waters. It plays an important role in regulating the pH of water. Increased HCO₃^– in water can lead to alkalinity of water and the formation of carbonate deposits in pipes.

Sources of bicarbonate in water

1- Natural sources:

 -Rainwater: Carbon dioxide in the air reacts with rainwater to form carbonic acid. Carbonic acid then breaks down into hydrogen ions and HCO₃^–.

-Carbonated rocks: Carbonated rocks such as limestone and dolomite dissolve in contact with water to form bicarbonate.

-Volcanic activity: Volcanic activity releases sulfur dioxide and carbon dioxide gases, which form hydrogen sulfide and bicarbonate in water.

2- Artificial sources:

-Chemical industries: In the chemical industry, sodium bicarbonate (NaHCO₃) is used in the production of various materials.

-Water purification: In water purification, NaHCO₃ is used to adjust pH and soften water.

-Agriculture: NaHCO₃ is used as a pesticide and fungicide in agriculture.

Storage period

The sample can be stored for up to 14 days unless stored at 4°C.

How to calculate

It is calculated in mg/L CaCO₃.