GY1004 Principles of Physical Geography B Lecture 2 Chemical Weathering DEPARTMENT OF GEOGRAPHY.
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Transcript of GY1004 Principles of Physical Geography B Lecture 2 Chemical Weathering DEPARTMENT OF GEOGRAPHY.
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GY1004 Principles of Physical Geography B
Lecture 2Chemical Weathering
DEPARTMENT OF GEOGRAPHY
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Chemical weathering
Chemical weathering, therefore, reflects the tendency for new minerals to be formed which are stable under conditions prevailing at the Earth’s surface.
The formation of granite
Open cast Kaolinite mine, Devon.
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Approaches to studying chemical weathering
Thermodynamic approach
Considers the ultimate stable forms by analysing the energy changes involved in chemical reactions
Kinetic approach
Considers the factors that control the rate of chemical reactions
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Chemical weathering processes 1
Solution – the process by which ions are detached by water molecules and then carried away from the weathering zone
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Chemical weathering processes 2
Hydration – the absorption of water into the mineral structure
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Chemical weathering processes 3
Oxidation and reduction – the process by which minerals gain and lose electrons
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Chemical weathering processes 4
Hydrolysis – the replacement of metal cations in a mineral structure by hydrogen ions (H+) and the combining of these released cations with hydroxyl ions (OH-)
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Chemical weathering processes 5
Organic processes e.g. chelation – the release and mobilisation of metal cations (e.g. Fe3+ and Al3+)
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Chemical weathering processes 6
Cation exchange – the substitution of one cation for another of a different element in a mineral structure.
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Chemical weathering processes 1
Solution – the process by which ions are detached by water molecules and then carried away from the weathering zone
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Why is water a good solvent?
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Mineral solubility
Halite Calcite
Rock salt Limestone
NaCl CaCO3
Quartz
SiO2
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Equilibrium solubility
The extent to which a mineral will dissolve in water (ppm; mg l-1)
Determined by the types of chemical bonds
Ionically bonded minerals are more susceptible to solution than covalently bonded minerals
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Equilibrium solubility and ionic potential
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Equilibrium solubility and pH
Self ionisation of water
H20 + H+ H3O+
pH = -log10 (H3O+)
H20 H+ + (OH)-
Concentration of H3O
+ in 1 litre pure water at 25oC is 0.0000001 (10-7) mole
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pH
pH = -log10 (H3O+)
pH = -log10 10-7
Thus for pure water at 298K (25oC)
pH = -(-7) = 7
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Acids and bases
Substances which increase the concentration of H+ cause the pH to fall and are called acidsAcids are, therefore, proton (H+) donors
Self ionisation of water
H20 H+ + (OH)-
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Acids and bases
Substances which decrease the concentration of H+ cause the pH to rise and are called basesBases are, therefore, proton (H+) acceptors
Self ionisation of water
H20 H+ + (OH)-
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0 1 2 3 4 5 6 7 8 9 10 11 12 13 14 antacid
tabletsbeer
coffee
The pH scale
acid alkaline
bleach
neutral
lemon juice
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0 1 2 3 4 5 6 7 8 9 10 11 12 13 14 rivers
and lakes
rain water
The pH scale
acid alkaline
oceanic water
neutral
peat water
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Equilibrium solubility and pH
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Carbonation
The dissolution and disassociation of carbon dioxide and water in a reversible reaction to produce
bicarbonate ions
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Carbonation
Carbon dioxide + water carbonic acid
H2CO3- H+ +
HC03-
bicarbonate ion
CO2+ H2O H2CO3-
carbonic acid
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Carbonation and the weathering of calcareous
rocks
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Chemical weathering processes 2
Hydration – the absorption of water into the mineral structure
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Chemical weathering processes 3
Oxidation and reduction – the process by which minerals gain and lose electrons
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Oxidation and reduction
Oxidation – the loss of electrons
Oxygen dissolved in water is the most common oxidising agent
Reduction – the gaining of electrons
Iron is the most commonly oxidised material
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The oxidation of iron
4Fe2+ +3O2 2Fe2O3
iron + oxygen iron oxide
Bivalent (Fe2+)
Ferrous iron oxide
FeO
Trivalent (Fe3+)
Ferric iron oxide
Fe2O3
oxidation
reduction
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Bivalent (Fe2+)
Ferrous iron oxide
FeO (Reduced form)
Trivalent (Fe3+)
Ferric iron oxide
Fe2O3 (Oxidised form)
Gley soil Laterite
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Redox potential (Eh)
Eh is measured in millivolts (mV)
Positive Eh = oxidising environment
Negative Eh = reducing environment
Eh varies with pH
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Chemical weathering processes 4
Hydrolysis – the replacement of metal cations in a mineral structure by hydrogen ions (H+) and the combining of these released cations with hydroxyl ions (OH-)
In situ weathered granite
Core stones
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The weathering of feldspar by hydrolysis
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Chemical weathering processes 5
Organic processes e.g. chelation – the release and mobilisation of metal cations (e.g. Fe3+ and Al3+)
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Chemical weathering processes 5
Desert varnish (10-30 m thick)
clay minerals
oxides/hydroxides of iron and manganese
detritus
Libyan Desert
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Chemical weathering processes 6
Cation exchange – the substitution of one cation for another of a different element in a mineral structure.
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The chemical weathering of silicate minerals
The formation of silicate minerals in
cooling magmaSilicate minerals are the constituent minerals of nearly all rocks
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The chemical weathering of silicate minerals
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Summary
Chemical weathering is the chemical process of mineral and rock decay;
The relative stability of silicate minerals is roughly the reverse order of crystallisation of a granitic melt;
Carbonate rocks are prone to solution.
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Summary
The extent to which a mineral will dissolve is termed its equilibrium solubility;
Calcium is the most soluble mineral followed by sodium and potassium. These are all more soluble than silica, aluminium and iron;
Other important chemical weathering processes include hydrolysis, hydration, oxidation and reduction.
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Summary
Overall, chemical weathering arises from the chemical instability of silicate minerals and the solubility of carbonate minerals at or near the earth’s surface.