Question

The biological oxidation of Fe2+ in mine drainage waters can result in red discoloration in steams from subsequent Fe3+ precipitation

(a) Name the type of organism responsible for this process

(b) Is this reaction spontaneous? Show calculations to justify your answer

(c) Write a balanced overall equation for biological of Fe2+, assuming fs(max) and the presence of ammonia

(d) How many grams of oxygen are required per gram of Fe2+ oxidized?

plz let me know the detailed procedure especially (c)

Answer 1

Acid mine drainage impacts stream and river ecosystems through acidity, ferric ion (Fe³⁺) precipitation, oxygen depletion, and release of heavy metals associated with coal and metal mining, such as aluminum (Al³⁺), zinc (Zn²⁺), and manganese (Mn²⁺).

When mineral deposits that contain sulfides are mined, they have the potential to produce acid mine drainage. This includes the mining of coal, copper, gold, silver, zinc, lead, and uranium. The mineral pyrite, more commonly known as "fool's gold," is iron disulfide (FeS₂). Pyrite is one of the most important sulfides found in the waste rock of mines. When exposed to water and oxygen, it can react to form sulfuric acid (H₂SO₄). The following oxidation and reduction reactions express the breakdown of pyrite that leads to acid mine drainage.

1. 2FeS₂ + 7O₂ + 2H₂O -> 2FeSO₄ + 2H₂SO₄

2. 2Fe²⁺ + 1/2 O₂ + 2H⁺ -> 2Fe³⁺ + H₂O

3. Fe³⁺ + 3H₂O -> Fe(OH)₃ + 3H⁺

4. FeS₂(s) + 15/4 O₂ + 7/2 H₂O <--> 4H⁺ + 2SO₄^- +Fe(OH)₃ (s)

Production of acid mine drainage can occur long after mines have been abandoned if piles of waste rock are in contact with air and water. The red color often seen in streams receiving acid mine drainage is actually a stain on the rocks called "Yellow-Boy," or ferrous hydroxide (Fe(OH)₃) formed during Reaction 3 above.

Equation 4 shows that by introducing hydrogen ions, acid mine drainage affects the acidity of a stream. Acidity is commonly measured by pH values, which are easy to collect and compare. pH, however, is not always a good indicator of acid mine drainage because it only indicates the concentration of hydrogen ions. When evaluating the extent of acid mine drainage, it is important to know the amount of hydrogen ions remaining in solution after the natural buffering of the stream is completed. For example, pH measurements may not detect heavy acid mine drainage in a stream because of high alkalinity due to dissolved carbonates. Assessing the excess of hydrogen ions over basic ions,"total acidity," is a better measurement of acid mine drainage.

Acid mine drainage depletes the buffering ability of water by neutralizing carbonate and bicarbonate ions to form carbonic acid (H₂CO₃).

H⁺ + CO₃^2- <--> HCO^3-

H⁺ + HCO^3- <--> H₂CO₃

Once exposed to acid mine drainage, the affected carbonate buffering system is not able to control changes in pH as well. The buffering system is completely destroyed below a pH of 4.2, where all carbonate and bicarbonate ions are converted to carbonic acid. The carbonic acid readily breaks down into water and carbon dioxide.

H₂CO₃ --> H₂O + CO₂

Table comparing waters receiving acid mine drainage, acid rain, and peat drainage.

Bright orange-colored water and stained rocks are usually tell-tale signs of acid mine drainage. The orange color is caused by ferric hydroxide ( Fe(OH)₃ ) precipitating out of the water. The precipitate forms as the acid mine drainage becomes neutralized. At low pH values, the metal ions remain soluble. When the pH rises, the iron oxidizes and precipitates out. Depending on the conditions, the orange-colored precipitates may form inside the mine or several miles downstream. The precipitates can be harmful to aquatic life. The clumps reduce the amount of light that can penetrate the water, affecting photosynthesis and visibility for animal life. Futhermore, when the precipitate settles, it blankets the stream bed, smothering the bottom-dwellers and their food resources.

Treatment of mine effluent
Today's active deep mines in the upper reaches of Wheeling Creek follow state and federal regulations for discharging effluent from a mine. Acid mine drainage must be treated to increase pH and remove heavy metals before being discharged into a receiving stream. Treatment commonly consists of adding strong bases, such as caustic soda (NaOH, sodium hydroxide), soda ash (Na₂CO₃, sodium carbonate), or lime (CaO, calcium oxide, or Ca(OH)₂, calcium dihydroxide). Photo: Courtesy of Dr. Ben Stout

Note the color change in the treatment pond pictured to the right. The water is red where mine effluent enters the pond. The red color indicates that iron hydroxide is precipitating out of the water column. Mechanical aeration speeds the process by making oxygen more available in Reactions 1 and 3 above. The iron precipitate eventually settles to the bottom of the pond, indicated by the area where the red water turns green. The green color is a result of the presence of sulfate (SO₄^2-), sodium (Na⁺), and calcium (Ca²⁺) ions remaining from acid neutralization reactions. Photo: Courtesy of Dr. Ben Stout

The bases used in the treatment of acid mine drainage work by neutralizing the acidity of the mine effluent. Because they are strong bases, they ionize and dissolve in water. The resulting hydroxide (OH^-) and carbonate (CO₃^2-) ions combine with hydrogen (H+) ions, taking them out of solution. The resulting products are water (H⁺ + OH^- <-> H₂O) and carbonic acid (H₂CO₃). The carbonic acid is relatively harmless because it is a weak acid and can be dissociated as water and carbon dioxide, as described in the bicarbonate buffering system under alkalinity.

Water hardness and conductivity are useful indicators of upstream mining activity. Water hardness may be higher in watersheds with active or abandoned mines. Ferrous iron (Fe²⁺) from acid generating reactions and calcium (Ca²⁺) from acid-neutralizing reactions may contribute to higher than average levels of water hardness. Leftover ions from acid-generating and acid-neutralizing reactions can effectively increase the salt concentration, or salinity, of the water. The greater the salt concentration, the greater the conductivity of the water, which makes conductivity a very useful indicator of upstream mining activity.