Determination of Carbonate Alkalinity in Natural Waters

Thomas, Jerome F.; Lynch, J J

doi:10.1002/j.1551-8833.1960.tb00473.x

Cited by 34 publications

(13 citation statements)

References 10 publications

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“…The alkalinity of water (Alk) was determined by the two-point titration method (to pH 4.5 and 4.2) [4,5] and calculated from the equation Alk = (2 V 4.5 -V 4.2 ) N / V , where V 4.5 and V 4.2 are the volumes of a strong acid consumed for the titration of a sample to pH 4.5 and 4.2, respectively; V is the sample volume; and N is the normality of the acid solution. The amount of organic acid anions was calculated from the ion balance of water,…”

Section: Methodsmentioning

confidence: 99%

Contribution of Organic Acid Anions to the Alkalinity of Natural Humic Water

Лозовик

2005

J Anal Chem

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The alkalinity of water is widely used for the monitoring of natural water. The concentration of hydrogen carbonates [1,2] is often calculated from this alkalinity index. However, this is incorrect because other salts of weak acids can contribute to the alkalinity of water. It would be more reliable to express the alkalinity of water in mg L -1 , thus indicating which equivalent amount of hydrogen carbonates corresponds to the given alkalinity, or, as is customary done in Ireland, in units of mg CaCO 3 L -1 [3]. The concentration of the other anions of weak acids is calculated from an ion balance of water; however, as the concentration of hydrogen carbonate differs from the true value, the concentration of the former ions will also be unreliable. Consequently, the classification of waters with respect to the predominant ions will not correspond with reality. This is of particular importance for natural humic water enriched in organic matter of allochthonous origin.The aim of this work was to determine the contribution of organic acid anions to the alkalinity of water and, based on this contribution, to refine procedures for calculating the concentration of hydrogen carbonate in natural humic water. EXPERIMENTALThe alkalinity of water (Alk) was determined by the two-point titration method (to pH 4.5 and 4.2) [4, 5] and calculated from the equation Alk = (2 V 4.5 -V 4.2 ) N / V , where V 4.5 and V 4.2 are the volumes of a strong acid consumed for the titration of a sample to pH 4.5 and 4.2, respectively; V is the sample volume; and N is the normality of the acid solution. The amount of organic acid anions was calculated from the ion balance of water,HCO 3 -A org -HCO 3 -where Σ cat is the sum of cations and Σ sa is the sum of strong acid anions. The ë ‡ 2+ and Mg 2+ ions were determined by atomic absorption spectrometry [6], Na + and K + were determined by flame photometry [7], and was determined by the indophenol method [8]. Sulfates and chlorides were determined by ion chromatography [9]. Nitrates were determined by reduction to nitrites on a Cu-Cd reductor [10], and pH was determined by potentiometry. All chemical analyses were performed in the Laboratory of Hydrochemistry and Hydrology of the Institute of Water Problems of the North of the Karelian Scientific Center of the Russian Academy of Sciences; this laboratory was accredited by the Gosstandart of Russia. The reliability of the chemical analyses of water was tested by internal and external controls. The latter was performed within the framework of an ICP-Waters international project [11]. RESULTS AND DISCUSSIONIn the general case, the alkalinity of water is due to the presence of anions of weak acids (carbonic acid, organic acids, phosphoric acid, silicic acid, sulfurous acid, etc.) [12]. Silicates in natural water are fully hydrolyzed and occur as silicic acid in the studied pH regions; therefore, silicates do not contribute to the alkalinity.Phosphates occur in microgram amounts. The occurrence of sulfites is unlikely if oxygen is present in water. Ther...

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Section: Methodsmentioning

confidence: 99%

Contribution of Organic Acid Anions to the Alkalinity of Natural Humic Water

Лозовик

2005

J Anal Chem

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“…The highest value of alkalinity ( Fig. 9) was found to be 270 mg/L in Station 7 during the dry season and the lowest value was 78 mg/L in Station 6 during the rainy season due to municipal waste disposal and oil pollution (Thomas and Lynch 1960). This similar observation was made by Mahmood et al (1992) and Paul (1981) who reported that oil pollution in the Karnaphuli River was responsible for increasing the total alkalinity of this river and its tributaries.…”

Section: Seasonal Variation Of Water Parametersmentioning

confidence: 93%

Environmental assessment of water and soil contamination in Rajakhali Canal of Karnaphuli River (Bangladesh) impacted by anthropogenic influences: a preliminary case study

et al. 2015

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Soil and water quality determines the health of an aquatic ecosystem. Rajakhali Canal, a tributary of Karnaphuli River estuary, flowing through Chittagong City (the commercial capital of Bangladesh) receives a huge amount of domestic and industrial wastes and sewages. Monitoring the environmental status of Karnaphuli River and its tributaries is very important for their ecological and economical services provided to city areas. This study evaluated some environmental characteristics of water and soil in the Rajakhali Canal as it affected the environment, and ultimately the life and human beings of Chittagong City. The mean concentrations of physicochemical parameters were pH (8.5), DO (0.1 mg/L), TA (47.6 mg/L), TDS (631.8 mg/L), TSS (280 mg/L), SO 4 -S (2.3 mg/L), NH 3 (1.1 mg/L), NO 3 -N (0.2 mg/L) and PO 4 -P (0.1 mg/L) in the dry season. During the rainy season, the mean concentrations of physico-chemical parameters were pH (7.01), DO (0.55 mg/L), TA (65.9 mg/L), TDS (653.6 mg/L), TSS (300.3 mg/L), SO 4 -S (1 mg/L), NH 3 -(0.6 mg/L), (NO 3 -N (0.3 mg/L) and PO 4 -P (0.5 mg/L) in water.In case of soil, the mean concentration of physicochemical parameters in dry and rainy seasons was represented respectively as follows: pH (6.8), OM (4.5 %), sand (71.7 %), silt (3.1 %), clay (25.2 %), organic nitrogen (45.4 ppm) and phosphorus (9.6 ppm); and pH (6.7), OM (4.5 %), sand (74.4 %), silt (2.4 %), clay (23.2 %), organic nitrogen (35.3 ppm) and phosphorus (7.6 ppm). The result revealed that water and soil quality of this canal became deteriorated and that the total environment of the water body became polluted due to the anthropogenic activities such as industrial, domestic and irrigation effluents. Statistical analyses also supported that water and soil parameters were strongly correlated (1-tailed 0.05 level and 0.01 level significant) with each other at all stations during all seasons. The result of this study will be useful for management and planning for water quality monitoring in this estuary. To protect this vital estuarine region, the government agencies, private agencies and scientists should work with proper attention.

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“…A Gran titration is often used to linearize the titration curve using pH endpoints of 4.2 and 3.9, especially in waters of low alkalinity (American Public Health Association, 2005;Thomas and Lynch, 1960).…”

Section: Ph-alkalinity Titrationsmentioning

confidence: 99%

“…Temperature and pH were measured in-situ at the same location where the CO 2 water samples were collected. Alkalinity was measured using a two-endpoint method (pH 4.2 and 3.9) and calculated using a Gran function (Thomas and Lynch, 1960). A digital titrator (Hach Company, Loveland, CO) was used to titrate samples using 1.6 N sulfuric acid.…”

Section: Field and Laboratory Analysismentioning

confidence: 99%

Determination of free CO2 in emergent groundwaters using a commercial beverage carbonation meter

Vesper

Edenborn

2012

Journal of Hydrology

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Keywords:Dissolved carbon dioxide (CO 2 ) Groundwater Alkalinity Carbonate Springs Mine water s u m m a r y Dissolved CO 2 in groundwater is frequently supersaturated relative to its equilibrium with atmospheric partial pressure and will degas when it is conveyed to the surface. Estimates of dissolved CO 2 concentrations can vary widely between different hydrochemical facies because they have different sources of error (e.g., rapid degassing, low alkalinity, non-carbonate alkalinity). We sampled 60 natural spring and mine waters using a beverage industry carbonation meter, which measures dissolved CO 2 based on temperature and pressure changes as the sample volume is expanded. Using a modified field protocol, the meter was found to be highly accurate in the range 0.2-35 mM CO 2 . The meter provided rapid, accurate and precise measurements of dissolved CO 2 in natural waters for a range of hydrochemical facies. Dissolved CO 2 concentrations measured in the field with the carbonation meter were similar to CO 2 determined using the pH-alkalinity approach, but provided immediate results and avoided errors from alkalinity and pH determination. The portability and ease of use of the carbonation meter in the field made it well-suited to sampling in difficult terrain. The carbonation meter has proven useful in the study of aquatic systems where CO 2 degassing drives geochemical changes that result in surficial mineral precipitation and deposition, such as tufa, travertine and mine drainage deposits.

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Determination of Carbonate Alkalinity in Natural Waters

Cited by 34 publications

References 10 publications

Contribution of Organic Acid Anions to the Alkalinity of Natural Humic Water

Contribution of Organic Acid Anions to the Alkalinity of Natural Humic Water

Environmental assessment of water and soil contamination in Rajakhali Canal of Karnaphuli River (Bangladesh) impacted by anthropogenic influences: a preliminary case study

Determination of free CO2 in emergent groundwaters using a commercial beverage carbonation meter

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