Gifts of Phosphate Fertilizers and Curses of Idyllic Life Styles
Phosphorus, the eleventh most abundant element in Earth’s crust, exists in three allotropic forms: white, red, and black. The white form of phosphorus is a highly active, waxy solid that catches fire spontaneously when exposed to air. In contrast, red phosphorus is a reddish powder that is relatively inert. It does not catch fire unless exposed to an open flame. Phosphorus always occurs in the form of a phosphate, a compound consisting of phosphorus, oxygen, and at least one more element. By far the most abundant source of phosphorus on Earth is a family of minerals known as the apatites which contain phosphorus, oxygen, calcium, and a halogen. The state of Florida in US is the world’s largest producer of phosphorus and is responsible for about a third of the entire element produced in the world. Phosphorus also occurs in all living organisms, most abundantly in bones, teeth, horn, and similar materials. It is found in all cells, however, in the form of compounds essential to the survival of all life. Like carbon and nitrogen, phosphorus is cycled through the environment. But since it has no common gaseous compounds, the phosphorus cycle occurs entirely within the solid and liquid portions of Earth’s crust.
About 95 percent of all the phosphorus used in industry goes to the production of phosphorus compounds. By far the most important of these is phosphoric acid, which accounts for about 83 percent of all phosphorus use in industry. A minor use is in the manufacture of safety matches. Phosphoric acid (H3PO4) typically ranks about number seven among the chemicals most widely produced in the United States. It is converted to a variety of forms, all of which are then used in the manufacture of synthetic fertilizer, accounting for about 85 percent of all the acid produced. Other applications of phosphoric acid include the production of soaps and detergents, water treatment, the cleaning and rust proofing of metals, the manufacture of gasoline additives, and the production of animal feeds.
The extraction of phosphate fertilizers from the island of Nauru is an illustrative case history regarding involvement or role of human element in our study of industrial chemistry or any branch of science. The Republic of Nauru, located in the Pacific Ocean, has an area of 21 km2, yet it is one of the world’s major suppliers of calcium phosphate which provides this small nation a gross national income of about 200 million USD per person per annum. This income provides an opulent life style with all the conveniences of modern living to native Naurans. In addition, they hire servants and maids from Asia and other island countries for work in and around their houses.
However, the down side of this idyllic life style is that there is little incentive for the owners and employers to work or study. Obesity, heart disease and alcohol abuse have suddenly taken them in the clutches. Moreover the long term effects on the environment have also been catastrophic as extraction of the phosphate rock is like large-scale dentistry. The ore is scooped up from between enormous tooth like stalks of coral limestone, some of which are 25m high. These barren pinnacles of lime stone will be all that is left of 80% of the island when the deposits are exhausted. Furthermore, silt run off from the mixing operation has damaged the offshore coral reefs that once provided abundant fishing resources.
At one time, large amounts of phosphoric acid were converted to a compound known as sodium tripolyphosphate (STPP that, in turn, was used in the manufacture of synthetic detergents. When STPP is released to the environment, however, it serves as a primary nutrient for algae in bodies of water such as ponds and lakes. As phosphates are a major source of pollution in lakes and streams, and high phosphate levels support over-production of algae and water weeds. However, many of us have misconceptions regarding the source of polluting phosphates, and many homeowners unknowingly contribute to the problem. Lawn and Garden fertilizers often are implicated as the major source of phosphate pollution. However, research clearly demonstrates that with proper application, fertilizer does not pollute. When phosphates are applied to soils, they quickly bind to soil particles, much like a magnet picks up paper clips. Soil-bound phosphates contribute to pollution only when soil erosion occurs. Research studies have found little or no difference in the phosphate content of storm runoff from lawn fertilizers with and without phosphate. The growth of huge algal blooms in the 1970s and 1980s as a result of phosphate discharges eventually led to bans on the use of this compound in detergents. As a consequence, the compound is no longer commercially important.
Problems arise, however, when fertilizer is over-spread or spilled onto hard surfaces like streets, driveways and sidewalks. Here, the phosphate washes with rain through the storm drains into lakes and rivers. Likewise, grass clippings and leaves that fall on hard surfaces release their phosphorous into water sources. Research studies indicate that 80 percent of the phosphorous from urban settings comes from lawn clippings and leaves that end up in street gutters. While a few grass clippings mowed into the street look rather innocent, collectively they have a major impact on our water quality. Using a mulching lawn mower to keep lawn clippings on your lawn is especially useful. Another important source of phosphate pollution comes from soil erosion caused by water or wind. When soil moves, it takes the soil-bound phosphates with it. Construction sites and sparsely vegetated ground also cause erosion.
About the Author
Dr.Badruddin Khan teaches Chemistry in the University of Kashmir, Srinagar, India.
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