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====Neutralization with calcium carbonate====
====Neutralization with calcium carbonate====
Often, [[limestone]] rocks or appropriate [[calcareous]] [[Stratum|strata]] able to neutralize acid effluents are lacking, or insufficiently accessible (too short residence time for acidic waters flowing too fast), at sites affected by acidic rock drainage. Crushed limestone can be dumped on site to provide a neutralizing effect. Where limestone has been used, such as at [[Cwm Rheidol]] in mid [[Wales]], the positive impact has been much less than anticipated because of the formation of a poorly soluble [[calcium sulfate]] layer onto the surface of limestone chips, binding the material and preventing further neutralization.{{Citation needed|date=July 2024}}<!-- What was exactly the granulometry of the so-called "limestone chips"? Was it limestone gravel, limestone sand, or limestone dust? An improperly sorted and too small granulometry of the material could easily explain the problems of clogging encountered at Cwm Rheidol (Wales) and one must be prudent before to draw too general conclusions here and to reject limestone, the less expensive material used for neutralisation of sulfuric acid in AMD -->
Often, [[limestone]] rocks or appropriate [[calcareous]] [[Stratum|strata]] able to neutralize acid effluents are lacking, or insufficiently accessible (too short residence time for acidic waters flowing too fast), at sites affected by acidic rock drainage. Crushed limestone can be dumped on site to provide a neutralizing effect. Where limestone has been used, such as at [[Cwm Rheidol]] in mid [[Wales]], the positive impact has been much less than anticipated because of the formation of a poorly soluble [[calcium sulfate]] layer onto the surface of limestone chips, binding the material and preventing further neutralization.
Indeed, [[calcium carbonate]] grains suffer from the formation of a coating of [[gypsum]] ({{Chem2|CaSO4*2H2O}}) surrounded by a thin impermeable and protective membrane of less soluble Fe-Al hydroxysulfate. This [[Passivation (chemistry)|passivating]] coating, sometimes referred to as an ''armor'' (shield, encrustation, rim, rind…), prevents [[calcite]] [[Dissolution (chemistry)|dissolution]] and the further release of [[bicarbonate]] in solution.<ref name="Hammarstrom2003" /><!-- What was exactly the granulometry of the so-called "limestone chips"? Was it limestone gravel, limestone sand, or limestone dust? An improperly sorted and too small granulometry of the material could easily explain the problems of clogging encountered at Cwm Rheidol (Wales) and one must be prudent before to draw too general conclusions here and to reject limestone, the less expensive material used for neutralisation of sulfuric acid in AMD -->


====Neutralization with lime====
====Neutralization with lime====

Revision as of 23:32, 22 July 2024

Rio Tinto in Spain presents an acid drainage of both natural and artificial origin (mining)
Rocks stained by ferrous precipitate from acid mine drainage on Shamokin Creek in Northumberland County, Pennsylvania

Acid mine drainage, acid and metalliferous drainage (AMD), or acid rock drainage (ARD) is the outflow of acidic water from metal mines and coal mines.[citation needed]

Acid rock drainage occurs naturally within some environments as part of the rock weathering process but is exacerbated by large-scale earth disturbances characteristic of mining and other large construction activities, usually within rocks containing an abundance of sulfide minerals. Areas where the earth has been disturbed (e.g. construction sites or highway construction) may create acid rock drainage. In many localities, the liquid that drains from coal stocks, coal handling facilities, coal washeries, and coal waste tips can be highly acidic, and in such cases it is treated as acid rock drainage. This liquid often contains highly toxic metals, such as copper or iron. These, combined with reduced pH, have a detrimental impact on the streams' aquatic environments.[citation needed]

The same type of chemical reactions and processes may occur through the disturbance of acid sulfate soils formed under coastal or estuarine conditions after the last major sea level rise, and constitutes a similar environmental hazard.[citation needed]

Nomenclature

Historically, the acidic discharges from active or abandoned mines were called acid mine drainage, or AMD. The term acid rock drainage, or ARD, was introduced in the 1980s and 1990s to indicate that acidic drainage can originate from sources other than mines.[1] For example, a paper presented in 1991 at a major international conference on this subject was titled: "The Prediction of Acid Rock Drainage – Lessons from the Database".[2] 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",[3] "mining-influenced water"[4] or otherwise. None of these other names have gained general acceptance.

Occurrence

In this case, the pyrite has dissolved away yielding a cube shape and residual gold. This break down is the main driver of acid mine drainage.

Sub-surface mining often progresses below the water table, so water must be constantly pumped out of the mine in order to prevent flooding. When a mine is abandoned, the pumping ceases, and water floods the mine. This introduction of water is the initial step in most acid rock drainage situations. Tailings piles or ponds, mine waste rock dumps,[3] and coal spoils are also an important source of acid mine drainage.

After being exposed to air and water, oxidation of metal sulfides (often pyrite, which is iron-sulfide) within the surrounding rock and overburden generates acidity. Colonies of bacteria and archaea greatly accelerate the decomposition of metal ions, although the reactions also occur in an abiotic environment. These microbes, called extremophiles for their ability to survive in harsh conditions, occur naturally in the rock, but limited water and oxygen supplies usually keep their numbers low. Extremophiles known as acidophiles especially favor the low pH levels of abandoned mines. In particular, Acidithiobacillus ferrooxidans is a key contributor to pyrite oxidation.[5]

Metal mines may generate highly acidic discharges where the ore is a sulfide mineral or is associated with pyrite. In these cases the predominant metal ion may not be iron but rather zinc, copper, or nickel. The most commonly mined ore of copper, chalcopyrite, is itself a copper-iron-sulfide and occurs with a range of other sulfides. Thus, copper mines are often major culprits of acid mine drainage.

At some mines, acidic drainage is detected within 2–5 years after mining begins, whereas at other mines, it is not detected for several decades.[citation needed] In addition, acidic drainage may be generated for decades or centuries after it is first detected. For this reason, acid mine drainage is considered a serious long-term environmental problem associated with mining.[citation needed]

Chemistry

Further information: Acidophiles in acid mine drainage

The chemistry of oxidation of pyrites, the production of ferrous ions and subsequently ferric ions, is very complex, and this complexity has considerably inhibited the design of effective treatment options.[6]

Although a host of chemical processes contribute to acid mine drainage, pyrite oxidation is by far the greatest contributor. A general equation for this process is:[7]

2 FeS2(s) + 7 O2(g) + 2 H2O(l) → 2 Fe2+(aq) + 4 SO2−4(aq) + 4 H+(aq)

The oxidation of the sulfide to sulfate solubilizes the ferrous iron (iron(II)), which is subsequently oxidized to ferric iron (iron(III)):

4 Fe2+(aq) + O2(g) + 4 H+(aq) → 4 Fe3+(aq) + 2 H2O(l)

Either of these reactions can occur spontaneously or can be catalyzed by microorganisms that derive energy from the oxidation reaction. The ferric cations produced can also oxidize additional pyrite and reduce into ferrous ions:[8]

FeS2(s) + 14 Fe3+(aq) + 8 H2O(l) → 15 Fe2+(aq) + 2 SO2−4(aq) + 16 H+(aq)

The net effect of these reactions is to release H+, which lowers the pH and maintains the solubility of the ferric ion.

Effects

Effects on pH

Yellow boy in a stream receiving acid drainage from surface coal mining

Water temperatures as high as 47 °C (117 °F)[9] have been measured underground at the Iron Mountain Mine, and the pH can be as low as −3.6.[10]

Organisms which cause acid mine drainage can thrive in waters with pH very close to zero. Negative pH[11] occurs when water evaporates from already acidic pools thereby increasing the concentration of hydrogen ions.

About half of the coal mine discharges in Pennsylvania have pH under 5.[12] However, a portion of mine drainage in both the bituminous and anthracite regions of Pennsylvania is alkaline, because limestone in the overburden neutralizes acid before the drainage emanates. [citation needed]

Yellow boy

When the pH of acid mine drainage is raised past 3, either through contact with fresh water or neutralizing minerals, previously soluble iron(III) ions precipitate as iron(III) hydroxide, a yellow-orange solid colloquially known as yellow boy.[13] Other types of iron precipitates are possible, including iron oxides and oxyhydroxides, and sulfates such as jarosite. All these precipitates can discolor water and smother plant and animal life on the streambed, disrupting stream ecosystems (a specific offense under the Fisheries Act in Canada). The process also produces additional hydrogen ions, which can further decrease pH. In some cases, the concentrations of iron hydroxides in yellow boy are so high, the precipitate can be recovered for commercial use in pigments.[14]

Trace metal and semi-metal contamination

Many acid rock discharges also contain elevated levels of potentially toxic metals, especially nickel and copper with lower levels of a range of trace and semi-metal ions such as lead, arsenic, aluminium, and manganese. The elevated levels of heavy metals can only be dissolved in waters that have a low pH, as is found in the acidic waters produced by pyrite oxidation. In the coal belt around the south Wales valleys in the UK highly acidic nickel-rich discharges from coal stocking sites have proved to be particularly troublesome.[citation needed]

Effects on aquatic wildlife

Acid mine drainage also affects the wildlife living within the affected body of water. Aquatic macroinvertebrates living in streams or parts of streams affected by acid mine drainage show fewer individuals, less diversity, and lower biomass. Many species of fish also cannot tolerate the pollution.[15] Among the macroinvertebrates, certain species can be found at only certain levels of pollution, while other species can be found over a wide range.[16]

Identification and prediction

In a mining setting it is leading practice to carry out a geochemical assessment of mine materials during the early stages of a project to determine the potential for AMD. The geochemical assessment aims to map the distribution and variability of key geochemical parameters, acid generating and element leaching characteristics.[17]

The assessment may include:[17]

  1. Sampling;
  2. Static geochemical testwork (e.g. acid-base accounting, sulfur speciation);
  3. Kinetic geochemical testwork - Conducting oxygen consumption tests, such as the OxCon, to quantify acidity generation rates[18]
  4. Modelling of oxidation, pollutant generation and release; and
  5. Modelling of material composition.

Treatment

Oversight

In the United Kingdom, many discharges from abandoned mines are exempt from regulatory control. In such cases the Environment Agency and Natural Resources Wales working with partners such as the Coal Authority have provided some innovative solutions, including constructed wetland solutions such as on the River Pelenna in the valley of the River Afan near Port Talbot and the constructed wetland next to the River Neath at Ynysarwed.

Although abandoned underground mines produce most of the acid mine drainage, some recently mined and reclaimed surface mines have produced ARD and have degraded local ground-water and surface-water resources. Acidic water produced at active mines must be neutralized to achieve pH 6–9 before discharge from a mine site to a stream is permitted.

In Canada, work to reduce the effects of acid mine drainage is concentrated under the Mine Environment Neutral Drainage (MEND) program. Total liability from acid rock drainage is estimated to be between CA$2 billion and CA$5 billion.[19] Over a period of eight years, MEND claims to have reduced ARD liability by up to CA$400 million, from an investment of CA$17.5 million.[20]

Methods

Neutralization with calcium carbonate

Often, limestone rocks or appropriate calcareous strata able to neutralize acid effluents are lacking, or insufficiently accessible (too short residence time for acidic waters flowing too fast), at sites affected by acidic rock drainage. Crushed limestone can be dumped on site to provide a neutralizing effect. Where limestone has been used, such as at Cwm Rheidol in mid Wales, the positive impact has been much less than anticipated because of the formation of a poorly soluble calcium sulfate layer onto the surface of limestone chips, binding the material and preventing further neutralization.

Indeed, calcium carbonate grains suffer from the formation of a coating of gypsum (CaSO4·2H2O) surrounded by a thin impermeable and protective membrane of less soluble Fe-Al hydroxysulfate. This passivating coating, sometimes referred to as an armor (shield, encrustation, rim, rind…), prevents calcite dissolution and the further release of bicarbonate in solution.[21]

Neutralization with lime

Depending on the volume and flowrate of acid effluents to be neutralised, a commonly used commercial process for treating acid mine drainage is lime (CaO) precipitation in a high-density sludge (HDS) process. In this application, a slurry of lime is dispersed into a tank containing acid mine drainage and recycled sludge to increase water pH to about 9. At this pH, most toxic metals become insoluble and precipitate, aided by the presence of recycled sludge. Optionally, air can be injected in the tank to oxidize iron(II) and manganese(II) and assist in their precipitation. The resulting slurry is directed to a sludge-settling vessel, such as a clarifier. In that vessel, clean water will overflow for release, whereas settled metal precipitates (sludge) are recycled to the acid mine drainage treatment tank, with a sludge-wasting side stream. A number of variations of this process exist, as dictated by the chemistry of ARD, its volume, and other factors.[22] Generally, the products of the HDS process also contain gypsum (CaSO4) and unreacted lime, which enhance both its settleability and resistance to re-acidification and metal mobilization. A general equation for this process is:

H2SO4 + CaO → CaSO4 + H2O

Less complex variants of this process, such as simple lime neutralization, may involve no more than a lime silo, a mixing tank and a settling pond. These systems are far less costly to build, but are also less efficient (longer reaction times are required, and they produce a discharge with higher trace metal concentrations, if present). They would be suitable for relatively small flows or less complex acid mine drainage.[23]

Neutralization with calcium silicate

A calcium silicate feedstock, made from processed steel slag, can also be used to neutralize active acidity in AMD systems by removing free hydrogen ions from the bulk solution, thereby increasing pH. As the silicate anion captures H+ ions (raising the pH), it forms monosilicic acid (H4SiO4), a neutral solute. Monosilicic acid remains in the bulk solution and play many roles in correcting the adverse effects of acidic conditions. In the bulk solution, the silicate anion is very effective in neutralizing H+ cations in the soil solution.[24] While its mode-of-action is quite different from limestone, the ability of calcium silicate to neutralize acid solutions is equivalent to limestone as evidenced by its CCE value[clarification needed] of 90–100% and its relative neutralizing value of 98%[clarification needed].[25]

In the presence of heavy metals, calcium silicate reacts in a different way than limestone. As limestone raises the pH of the bulk solution, when heavy metals are present, precipitation of the poorly soluble metal hydroxides is accelerated and the tendency for an impermeable metal hydroxide coating, termed armoring, to form on limestone grains surface increases significantly. Limestone grains become coated by a rind of gypsum encapsulated itself in a thin external film of Fe-Al hydroxysulfate. Armoring slows the CaCO3 dissolution and prevents the limestone grains from releasing additional alkalinity in solution.[21] In the calcium silicate aggregates, as silicic acid species are adsorbed onto the metal hydroxide surface, the development of silica layers (mono- and bi-layers) lead to the formation of colloidal complexes with neutral or negative surface charges. These negatively charged colloids are electrostatically repelled by each other (as well as with the negatively charged calcium silicate granules). The sequestered metal colloids are stabilized and remain in a stable dispersed state – effectively interrupting metal precipitation and reducing vulnerability of the material to armoring (formation of an impervious crust around material grains preventing their dissolution and decreasing their reactivity).[24]

Removal of toxic metals by ion exchange

Cation exchange processes have previously been investigated as a potential treatment for acid mine drainage. The principle is that an ion exchange resin can remove potentially toxic metals (cationic resins), or chlorides, sulfates and uranyl sulfate complexes (anionic resins) from mine water.[26] Once the contaminants are adsorbed, the exchange sites on resins must be regenerated, which typically requires acidic and basic reagents and generates a brine that contains the pollutants in a concentrated form. A South African company that won the 2013 IChemE award for water management and supply (treating AMD) have developed a patented ion-exchange process that treats mine effluents (and AMD) economically.

Constructed wetlands

Constructed wetlands systems have been proposed during the 1980s to treat acid mine drainage generated by the abandoned coal mines in Eastern Appalachia.[27] Generally, the wetlands receive near-neutral water, after it has been neutralized by (typically) a limestone-based treatment process.[28] Metal precipitation occurs from their oxidation at near-neutral pH, complexation with organic matter, precipitation as carbonates or sulfides. The latter results from sediment-borne anaerobic bacteria capable of reverting sulfate ions into sulfide ions. These sulfide ions can then bind with heavy metal ions, precipitating heavy metals out of solution and effectively reversing the entire process.[citation needed]

The attractiveness of a constructed wetlands solution lies in its relative low cost. They are limited by the metal loads they can deal with (either from high flows or metal concentrations), though current practitioners have succeeded in developing constructed wetlands that treat high volumes (see description of Campbell Mine constructed wetland) and/or highly acidic water (with adequate pre-treatment). Typically, the effluent from constructed wetland receiving near-neutral water will be well-buffered at 6.5–7.0 and can readily be discharged. Some of metal precipitates retained in sediments are unstable when exposed to oxygen (e.g., copper sulfide or elemental selenium), and it is very important that the wetland sediments remain largely or permanently submerged.

An example of an effective constructed wetland is on the Afon Pelena in the River Afan valley above Port Talbot where highly ferruginous discharges from the Whitworth mine have been successfully treated.

Precipitation of metal sulfides

Most base metals in acidic solution precipitate in contact with free sulfide, e.g. from H2S or NaHS. Solid-liquid separation after reaction would produce a base metal-free effluent that can be discharged or further treated to reduce sulfate, and a metal sulfide concentrate with possible economic value.

As an alternative, several researchers have investigated the precipitation of metals using biogenic sulfide. In this process, Sulfate-reducing bacteria oxidize organic matter using sulfate, instead of oxygen. Their metabolic products include bicarbonate, which can neutralize water acidity, and hydrogen sulfide, which forms highly insoluble precipitates with many toxic metals. Although promising, this process has been slow in being adopted for a variety of technical reasons.[29]

Technologies

Many technologies exist for the treatment of AMD.[30]

Metagenomic study

With the advance of large-scale sequencing strategies, genomes of microorganisms in the acid mine drainage community are directly sequenced from the environment. The nearly full genomic constructs allows new understanding of the community and able to reconstruct their metabolic pathways.[31] Our knowledge of acidophiles in acid mine drainage remains rudimentary: we know of many more species associated with ARD than we can establish roles and functions.[32]

Microbes and drug discovery

Scientists have recently begun to explore acid mine drainage and mine reclamation sites for unique soil bacteria capable of producing new pharmaceutical leads. Soil microbes have long been a source for effective drugs[33] and new research, such as that conducted at the Center for Pharmaceutical Research and Innovation, suggests these extreme environments to be an untapped source for new discovery.[34][35]

List of selected acid mine drainage sites worldwide

This list includes both mines producing acid mine drainage and river systems significantly affected by such drainage. It is by no means complete, as worldwide, several thousands of such sites exist.

Africa

Europe

North America

Oceania

See also

References

  1. ^ Dowding, B. & Mills, C,: Natural acid rock drainage and its impact upon background metal concentrations Archived 15 September 2014 at the Wayback Machine, InfoMine.com. Accessed 23 September 2013.
  2. ^ Ferguson, K.D. and Morin, K.A. The Prediction of Acid Rock Drainage - Lessons from the Database. Proceedings: Second International Conference on the Abatement of Acidic Drainage. Sept 16 to 18, 1991, Montreal, Quebec.
  3. ^ a b Global Acid Rock Drainage Guide (GARD Guide) INAP: The International Network for Acid Prevention. Accessed 23 September 2013.
  4. ^ Gusek, J.J., Wildeman, T.R. and Conroy, K.W. 2006. Conceptual methods for recovering metal resources from passive treatment systems. Proceedings of the 7th International Conference on Acid Rock Drainage (ICARD), March 26–30, 2006, St. Louis MO.
  5. ^ Mielke, R.E.; Pace, D.L.; Porter, T.; Southam, G. (2003). "A critical stage in the formation of acid mine drainage: Colonization of pyrite by Acidithiobacillus ferrooxidans under pH-neutral conditions". Geobiology. 1 (1): 81–90. Bibcode:2003Gbio....1...81M. doi:10.1046/j.1472-4669.2003.00005.x. S2CID 129323041.
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  25. ^ Calcium Silicon-Based Mineral CSA. Harsco Minerals.
  26. ^ M. Botha, L. Bester, E. Hardwick "Removal of Uranium from Mine Water Using Ion Exchange at Driefontein Mine"
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  31. ^ Tyson GW, et al. (4 March 2004). "Community structure and metabolism through reconstruction of microbial genomes from the environment". Nature. 428 (6978): 37–43. Bibcode:2004Natur.428...37T. doi:10.1038/nature02340. PMID 14961025. S2CID 4420754.
  32. ^ Villegas-Plazas M, et al. (1 December 2019). "A composite taxonomical and functional framework of microbiomes under acid mine drainage bioremediation systems". Journal of Environmental Management. 251 (109581): 109581. doi:10.1016/j.jenvman.2019.109581. PMID 31563048. S2CID 203592485.
  33. ^ Dias, D.A.; Urban, S.; Roessner, U. (2012). "A Historical Overview of Natural Products in Drug Discovery". Metabolites. 2 (4): 303–336. doi:10.3390/metabo2020303. PMC 3901206. PMID 24957513.
  34. ^ Wang, X.; Elshahawi, S.I.; Shaaban, K.A.; Fang, L.; Ponomareva, L.V.; Zhang, Y.; Copley, G.C.; Hower, J.C.; Zhan, C.-G.; Kharel, M.K.; Thorson, J.S. (2014). "Ruthmycin, a new tetracyclic polyketide from Streptomyces sp. RM-4-15". Org. Lett. 16 (2): 456–459. doi:10.1021/ol4033418. PMC 3964319. PMID 24341358.
  35. ^ Wang, X.; Shaaban, K.A.; Elshahawi, S.I.; Ponomareva, L.V.; Sunkara, M.; Copley, G.C.; Hower, J.C.; Morris, A.J.; Kharel, M.K.; Thorson, J.S. (2014). "Mullinamides A and B, new cyclopeptides produced by the Ruth Mullins coal mine fire isolate Streptomyces sp. RM-27-46". J. Antibiot. 67 (8): 571–575. doi:10.1038/ja.2014.37. PMC 4146655. PMID 24713874.
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  38. ^ David Falchek (26 December 2012). "Old Forge borehole drains mines for 50 years". The Scranton Times Tribune. Retrieved 18 March 2013.
  39. ^ DMITRE Minerals >...> Former Mines > Brukunga mine site Archived 2 April 2011 at the Wayback Machine Accessed 6 December 2011.
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  42. ^ Farmers 'disgusted' as proposal at abandoned central Queensland gold mine canned ABC News, 16 March 2018. Retrieved 24 March 2018.
  43. ^ Marychurch, Judith; Natalie Stoianoff (4–7 July 2006). "Blurring the Lines of Environmental Responsibility: How Corporate and Public Governance was Circumvented in the Ok Tedi Mining Limited Disaster" (PDF). Australasian Law Teachers Association – Refereed Conference Papers. Victoria University, Melbourne, Victoria, Australia. Archived from the original (PDF) on 7 October 2011. Retrieved 6 December 2011.
  44. ^ [4] Archived 27 September 2007 at the Wayback Machine Accessed 6 December 2011.
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