CHEMICAL STABILITY OF ALKALINE BOTTLED WATER BASED ON LANGELIER SATURATION INDEX AND CALCIUM CARBONATE PRECIPITATION
Main Article Content
Abstract
Alkaline bottled drinking water is characterized by high pH and relatively high alkalinity, which may influence its chemical stability during storage. One commonly observed phenomenon is the formation of white precipitates that can reduce the perceived quality of the product. This study aimed to evaluate the chemical stability of alkaline bottled drinking water based on physicochemical parameter analysis, characterization of the formed precipitates, and calculation of the Langelier Saturation Index (LSI) as an initial indicator of calcium carbonate precipitation tendency. The study was conducted on ten alkaline bottled water samples from a single producer by measuring pH, temperature, total dissolved solids (TDS), alkalinity, and Ca²⁺ and Mg²⁺ ion concentrations. The white precipitates formed during storage were qualitatively analyzed and confirmed through reaction tests with hydrochloric acid. The results showed that all samples had pH values of 8.35-8.50, alkalinity of 146-154 mg/L as CaCO₃, and a dominance of Ca²⁺ ions over Mg²⁺ ions. All samples exhibited positive LSI values, indicating supersaturation with respect to calcium carbonate. These findings indicate that LSI is a relevant initial indicator for evaluating the chemical stability of alkaline bottled drinking water during storage.
Downloads
Article Details
This work is licensed under a Creative Commons Attribution 4.0 International License.
References
W. F. Langelier, “The analytical control of anti-corrosion water treatment,” Journal of the American Water Works Association, vol. 28, no. 10, pp. 1500–1521, 1936.
[2] World Health Organization, Guidelines for Drinking-water Quality. [Online]. Available: https://www.who.int/publications/i/item/9789241549950. [Accessed: Dec. 28, 2025].
[3] V. L. Snoeyink and D. Jenkins, Water Chemistry, 1st ed. New York, NY, USA: John Wiley & Sons, 1980.
[4] W. Stumm and J. J. Morgan, Aquatic Chemistry, 3rd ed. New York, NY, USA: John Wiley & Sons, 1996.
[5] Y. Tang, Y. Yang, and Z. Liu, “Calcium carbonate scaling mechanisms in alkaline water systems,” Water Research, vol. 188, p. 116519, 2021.
[6] L. N. Plummer and E. Busenberg, “The solubilities of calcite, aragonite, and vaterite in CO₂–H₂O solutions,” Geochimica et Cosmochimica Acta, vol. 46, no. 6, pp. 1011–1040, 1982.
[7] American Water Works Association, Water Quality and Treatment, 6th ed. Denver, CO, USA: American Water Works Association, 2011.
[8] A. I. Vogel, Vogel’s Textbook of Quantitative Chemical Analysis, 5th ed. Harlow, UK: Longman Scientific & Technical, 1989.
[9] J. W. Morse, R. S. Arvidson, and A. Lüttge, “Calcium carbonate formation and dissolution,” Chemical Reviews, vol. 107, no. 2, pp. 342–381, 2007.
[10] D. C. Harris, Quantitative Chemical Analysis, 9th ed. New York, NY, USA: W. H. Freeman and Company, 2015.
[11] J. A. Cotruvo, “Drinking water quality and contaminants of emerging concern,” in Drinking Water Quality and Contaminants Guide. Boca Raton, FL, USA: CRC Press, 2019, vol. 1, pp. 1–28.