Acid sulfate soils are naturally
occurring soils, sediments or organic substrates (e.g. peat) that are formed
under waterlogged conditions.
These soils contain iron sulfide
minerals (predominantly as the mineral pyrite) or their oxidation products. In
an undisturbed state below the water table, acid sulfate soils are benign.
However, if the soils are drained,
excavated or exposed to air by a lowering of the water table, the sulfides
react with oxygen to form sulfuric acid.
Release of this sulfuric acid from
the soil can in turn release iron, aluminium, and other heavy metals
(particularly arsenic) within the soil.
Once mobilized in this way, the acid
and metals can create a variety of adverse impacts : killing vegetation, seeping
into and acidifying groundwater and surface water bodies, killing fish and
other aquatic organisms, and degrading concrete and steel structures to the
point of failure.
Chemical reaction
When drained, pyrite- (FeS2) containing soils (also called cat-clays) may become extremely acidic (pH
< 4) due to the oxidation of pyrite into sulfuric acid (H2SO4)..
2FeS2 + 9O2 +
4H2O 8H+ + 4SO42- + 2Fe(OH)3
Fe(OH)3, iron(III)
hydroxide (orange), precipitates as a solid, insoluble mineral by which the
alkalinity component is immobilized, while the acidity remains active in the
sulfuric acid.
The process of acidification is
accompanied by the formation of high amounts of aluminium (Al3+,
released from clay minerals under influence of the acidity), which are harmful
to vegetation.
Other products of the chemical
reaction are:
1. Hydrogen sulfide (H2S),
a smelly gas
2. Sulfur (S), a yellow solid
3. Iron(II) sulfide (FeS), a
black/gray/blue solid
4. Hematite (Fe2O3),
a red solid
5. Goethite (FeO.OH), a brown mineral
6. Schwertmannite, a brown mineral
7. Iron sulfate compounds (e.g.
jarosite)
8. H-Clay (hydrogen clay, with a
large fraction of adsorbed H+ ions, a stable mineral, but poor in
nutrients)