Zinc in Water

Zinc in Water
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Zinc in Water

Zinc in Water is present only in trace amounts in most surface and ground waters .

Zinc occurs abundantly in rocks and ores. It is readily refined into a stable pure metal and it is used extensively for galvanizing and alloys and other industrial manufacture.

Many of the zinc salts are highly soluble in water. Hence, it is to be expected that zinc might occur in effluents from industrial waters. On the other hand, some zinc salts are insoluble in water and consequently some zinc will precipitate and be removed readily in most natural waters.

In zinc mining areas, zinc has been found in natural waters in concentrations as high as 50 mg/L. In effluents from metal plating works and ammunitions plants lead may occur in significant concentrations.

Zinc is an essential and beneficial element in human nutrition. The normal human intake of zinc is estimated at 10 to 15 mg per day. Also, small amounts of zinc are needed for nutrition for most crops. A deficiency of zinc causes poor growth.

Zinc has no adverse physiological effects upon man except at very high concentrations.

Zinc exhibits its greatest toxicity towards fish and aquatic organisms. In soft water, concentrations of zinc ranging from 0.1 to 1.0 mg/L have been reported to be lethal.

The presence of copper appears to have a synergistic effect on the toxicity of zinc. Zinc precipitated from solution in alkaline water showed little toxic action. Almost all of the toxicity attributed to the zinc remaining in solution.

However, calcium is antagonistic towards such toxicity. The lethal limit for zinc in water containing 1 mg/L of calcium is only 0.3 mg/L, but in water with 50 mg/L of calcium, as much as 2 mg/L is not toxic. This antagonistic effect of hardness toward zinc toxicity was confirmed by several investigators.

The toxicity of zinc salts to stickle backs in soft water is reduced by the addition of calcium chloride. Even more so than the addition of calcium carbonate. Hence, the calcium ion rather than the carbonate ion appears to be the antagonistic factor.

The toxicity of zinc salts is increased at lower concentrations of dissolved oxygen in about the same proportion as for lead, copper, and phenols. In other words, the lethal concentration at 60% saturation of dissolved oxygen is only about 0.85 that at 100% saturation.

Zinc is thought to exert its toxic action by forming insoluble compounds with the mucus that covers the gills and respiratory organs of aquatic organisms. The damage may be to the gill epithelium or possibly it may act as an internal poison.

The sensitivity of fish to zinc varies with species, age and condition of the fish as well as with the physical and chemical characteristics of the water. Some acclimatization to the presence of zinc is possible. Survivors from batches of fish subjected to dissolved zinc have been less susceptible to additional toxic concentrations than fish not previously exposed.

The zinc cyanide complex, unlike nickel cyanide, disassociates in very dilute solutions. Zinc has been found to be even more toxic than comparable solutions of cyanide without zinc, apparently because of synergism.

Finally, zinc has been shown to have a toxic effect toward protozoa and bacteria, but not nearly as pronounced as copper.

End of Zinc in Water

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