Carbon Dioxide: Waste, Nutrient

In low-alkalinity waters, application of liming materials helps increase pH

Summary: 

Carbon dioxide is both a nutrient and a waste product in aquaculture. Some pond managers feel that application of organic matter to provide additional carbon dioxide can reduce pH and control blue-green algae. The overall effect of elevated carbon dioxide concentration in water is to reduce respiratory efficiency and the tolerance of aquatic animals to low dissolved-oxygen concentrations.

Carbon dioxide is both a nutrient and a waste product in aquaculture. Phytoplankton require carbon dioxide for photosynthesis. All organisms release carbon dioxide as a respiratory waste, and high concentrations of this metabolite can be harmful to aquatic animals. The concentration of carbon dioxide also is a major factor in controlling the pH of water.

Atmospheric Carbon Dioxide

The atmosphere is a vast reservoir of carbon dioxide. The average carbon dioxide concentration in the atmosphere is 380 ppm – up from 315 ppm in the 1950s and 280 ppm before the industrial revolution. Readers have no doubt heard concerns about the increasing atmospheric carbon dioxide concentration contributing to global warming

Carbon dioxide is acidic, for it reacts with water to form carbonic acid. This acid dissociates into hydrogen ion and bicarbonate ion

Rainfall becomes saturated with carbon dioxide while falling through the air. At the present atmospheric carbon dioxide concentration, the pH of rainfall normally should be around 5.6. Although rainfall is naturally acidic, there are regions where pollution of the atmosphere with sulfur dioxide and other wastes from combustion of fuels results in rainfall with much lower pH values that sometimes drop below 4.

Behavior in Aquaculture Systems

The carbon dioxide concentration at saturation in pure water is quite low (Table 1). Nevertheless, the small amount of carbon dioxide in rain enhances the dissolution of limestone and calcium silicate in soil and other geological formations to yield bicarbonate and calcium ion – sources of alkalinity and hardness, respectively.

In a system prepared by placing calcitic limestone in distilled water and allowing it to equilibrate with the atmosphere, the total alkalinity would be about 58 mg/l, but in natural waters and aquaculture ponds, total alkalinity concentration can be greater. In areas with calcareous soils, alkalinity in aquaculture ponds can exceed 150 mg/l, and in arid regions, even higher values can occur. Seawater typically contains 142 mg/l alkalinity.

The concentration of plant-available inorganic carbon is much greater in a system where carbon dioxide is in equilibrium with calcium carbonate and dissolved bicarbonate than in pure water where the equilibrium is between atmospheric carbon dioxide and dissolved carbon dioxide only. When plants remove carbon dioxide from the water in natural systems and aquaculture ponds, more carbon dioxide is made available from the bicarbonate. To illustrate, at 25° C and pH 7, water with 50 mg/l total alkalinity would contain about 15 mg/l of available carbon. Pure water in equilibrium with air at 25° C would have less than 1 mg/l available carbon

Table 1. Solubility of carbon dioxide (mg/l) in pure water at different temperatures and salinities from moist air.

Application of liming materials to low-alkalinity waters to increase pH also increases the alkalinity and availability of inorganic carbon for plants. The dissolution of liming material and associated increase in alkalinity can be greatly enhanced by applying liming materials and organic matter to ponds simultaneously. Bacteria decompose the organic matter to increase the amount of carbon dioxide available to react with the liming material.

Relevance of Phytoplankton

During daytime, phytoplankton normally remove carbon dioxide from water faster than it is released by respiration, causing a decline in carbon dioxide concentration and increase in pH (Figure 1). In waters below 50 mg/l alkalinity, pH can rise to 9.5 or more in response to rapid photosynthesis. The pH rise usually is not as great in waters of 50-200 mg/l alkalinity because buffering by the alkalinity lessens the pH change. Waters of high alkalinity concentration often have a permanently high pH. 

Phytoplankton use carbon dioxide as long as it is present, but when pH reaches 8.3, it is depleted. Most algal species can obtain carbon from bicarbonate when pH is above 8.3. The removal of carbon from bicar bonate by plants results in the release of carbonate ions into the water. Carbonate is alkaline and causes a further increase in pH. However, calcium reacts with carbonate to form calcium carbonate and limit the increase in pH.

Since blue-green algae are efficient at using low levels of carbon dioxide and obtaining carbon from bicarbonate, their abundance often increases in nutrient-rich waters.

Blue-green algae are more efficient than other types of algae in using low concentrations of carbon dioxide and obtaining carbon from bicarbonate. Thus, the abundance of blue-green algae often increases in nutrient-rich waters, where pH tends to increase over time because of the removal of inorganic carbon for photosynthesis.

Studies have revealed that bluegreen algae often are replaced by other more desirable phytoplankton species when carbon dioxide is bubbled into the water column. Thus, some pond managers feel that application of organic matter to provide additional carbon dioxide can be beneficial in reducing pH and controlling blue-green algae.

Carbon Dioxide Concentrations

Carbon dioxide concentrations in aquaculture ponds typically are 5-10 mg/l in early morning, but can exceed 20 mg/l in ponds with large inputs of feed. Carbon dioxide concentrations usually are highest when dissolvedoxygen concentrations are lowest.

Carbon dioxide is not particularly toxic to fish and other aquatic animals, but fish generally avoid carbon dioxide concentrations above 5- 10 mg/l. Concentrations of carbon dioxide above 20 mg/l are suspected to stress aquatic animals if exposure exceeds a few hours. Carbon dioxide at more than 60 mg/l can have a narcotic effect, and higher concentrations can cause death.

High concentrations of carbon dioxide in water interfere with carbon dioxide excretion through the gills of fish. This causes elevated concentrations of carbon dioxide in the blood plasma, which decreases blood pH. This condition lessens the ability of hemoglobin to bind oxygen and reduces oxygen uptake by blood at the gills, even when dissolved oxygen concentration is high.

High concentrations of carbon dioxide in water interfere with carbon dioxide excretion through the gills of fish.

The overall effect of elevated carbon dioxide concentration in water is to reduce respiratory efficiency and the tolerance of aquatic animals to low dissolved-oxygen concentrations. Thus, high carbon dioxide concentrations are particularly undesirable when dissolved-oxygen concentration is low – less than about 25% of saturation

Mechanical aeration of pond water adds dissolved oxygen and removes carbon dioxide. Thus, the combination of low dissolved oxygen and elevated carbon dioxide concentration that can occur in early morning is especially troublesome where mechanical aeration cannot be applied.

Well Water

Water that infiltrates downward through the soil becomes depleted of dissolved oxygen and supersaturated with carbon dioxide while passing through the root zone. Groundwater often has high carbon dioxide and low dissolved-oxygen concentrations. Where wells are used to supply ponds, this usually has no effect on culture species.

Hatchery waters should be aerated to add dissolved oxygen and remove carbon dioxide. It usually requires more aeration to saturate water with dissolved oxygen than to reduce carbon dioxide concentration to saturation. A high concentration of carbon dioxide in well water introduced into ponds usually does not have negative impacts on aquatic organisms.

CO2 Removal

Carbon dioxide can be removed from water by treatment with lime, calcium oxide or calcium hydroxide. Thus, lime can be applied to ponds during crises with low dissolved oxygen to remove carbon dioxide and allow fish to use the existing dissolved oxygen more efficiently.

Based on chemical relationships, the removal of 1 mg/l carbon dioxide requires about 0.84 mg/l calcium hydroxide or 0.64 mg/l calcium oxide. However, lime does not dissolve quickly to react completely with carbon dioxide, and the theoretical rates mentioned above should be doubled