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2. Soil acidification - Wikipedia

   en.wikipedia.org/wiki/Soil_acidification

   This compound causes rainfall pH to be around 5.0–5.5. When rainfall has a lower pH than natural levels, it can cause rapid acidification of soil. Sulfur dioxide and nitrogen oxides are precursors of stronger acids that can lead to acid rain production when they react with water in the atmosphere

3. Acidophiles in acid mine drainage - Wikipedia

   en.wikipedia.org/wiki/Acidophiles_in_acid_mine...

   Upon exposure to oxygen (O 2) and water (H 2 O), metal sulfides undergo oxidation to produce metal-rich acidic effluent. If the pH is low enough to overcome the natural buffering capacity of the surrounding rocks (‘calcium carbonate equivalent’ or ‘acid neutralising capacity’), the surrounding area may become acidic, as well as contaminated with high levels of heavy metals.

4. Acid mine drainage - Wikipedia

   en.wikipedia.org/wiki/Acid_mine_drainage

   Both AMD and ARD refer to low pH or acidic waters caused by the oxidation of sulfide minerals, though ARD is the more generic name. In cases where drainage from a mine is not acidic and has dissolved metals or metalloids , or was originally acidic, but has been neutralized along its flow path, then it is described as "neutral mine drainage ...

5. Soil pH - Wikipedia

   en.wikipedia.org/wiki/Soil_pH

   The prevailing view in the 1940s and 1950s was that P availability was maximized near neutrality (soil pH 6.5–7.5), and decreased at higher and lower pH. [ 29 ] [ 30 ] Interactions of phosphorus with pH in the moderately to slightly acidic range (pH 5.5–6.5) are, however, far more complex than is suggested by this view.

6. Environmental impact of iron ore mining - Wikipedia

   en.wikipedia.org/wiki/Environmental_impact_of...

   The high demand for iron necessitates continuous mining and processing, which generates a large amount of solid and liquid waste. Iron ore tailings are leftover materials that are released once mineral processing is complete. [10] This waste includes large amounts of iron and manganese oxides in addition to high pH values. [11]

7. Iron(II) sulfate - Wikipedia

   en.wikipedia.org/wiki/Iron(II)_sulfate

   Iron(II) sulfate is sold as ferrous sulfate, a soil amendment [23] for lowering the pH of a high alkaline soil so that plants can access the soil's nutrients. [24] In horticulture it is used for treating iron chlorosis. [25] Although not as rapid-acting as ferric EDTA, its effects are longer-lasting.

8. Manganese deficiency (plant) - Wikipedia

   en.wikipedia.org/wiki/Manganese_deficiency_(plant)

   The first is to adjust the soil pH. Two materials commonly used for lowering the soil pH are ammonium sulfate and sulfur. Ammonium sulfate will change the soil pH instantly because the ammonium produces the acidity as soon as it dissolves in the soil. Sulfur, however, requires some time for the conversion to sulfuric acid by soil

9. Acidithiobacillus thiooxidans - Wikipedia

   en.wikipedia.org/wiki/Acidithiobacillus_thiooxidans

   In addition to sulfur, A. thiooxidans can use thiosulfate or tetrathionate as sources of energy, but growth in a liquid medium on thiosulfate is slow, generally taking about 10 to 12 days under favorable conditions as opposed to only 4 to 5 days for growth on elemental sulfur, as demonstrated by the change in pH and turbidity. [2]