Sodium bicarbonate or sodium hydrogen carbonate (NaHCO3 ) occurs naturally as the mineral nahcolite and has a molar mass of 84.007 g/mol. It is an amphoteric compound that reacts with both acids and bases.
A simplified reaction equation is:
NaHCO3 + Ca2• + 2OH· ➔ CaCQ3.,J,+ Hp+ NaOH
Sodium bicarbonate is inexpensive; and therefore, it is an economical method for countering the effects of cementcontamination. In cases of severe contamination, it could be necessary to use citric acid to further reduce pH.
ADVANTAGES
• An effective, economic treatment for calcium removal
• Widely available
• Nonhazardous chemical
APPLICATIONS
• Primarily used to treat cement contamination because it precipitates calcium as a carbonate, as well as reacting with hydroxyl ions to reduce the pH
USAGE
Sodium bicarbonate is added at 0.000735 lb/bbl (0.0021 kg/m3) to treat 1.0 mg/L of calcium. Therefore, the approach is to determine the soluble calcium content of the water phase by standard analytical methods, calculate the total treatment required, and proceed to add the sodium bicarbonate over a complete circulation. An alternative pretreatment is 50 lb of sodium bicarbonate per 1.0 ft3 (22.7 kg per 0.028 m3 ) of cement. However, the degree to which the cement has set has to be considered.
Sodium bicarbonate is not used to treat make-up water to remove calcium because it lowers the pH. Soda ash should be used for that purpose. Avoid overtreatment because it can induce carbonate problems. Sodium bicarbonate must be stored in a dry location, away from water sources. Consult the MSDS, safety posters, and/or product label before use, and use personal protective equipment as advised.
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