Sulphate, lead mineral
Specific gravity: 6.37 to 6.39
Hardness: 2½ to 3
Colour: Colourless, white, yellow, green; colourless in transmitted light.
Solubility: Anglesite is not very soluble in water.
Common impurities: Ba, Cu
Anglesite is a common high temperature secondary mineral in the
oxidation zone of hydrothermal replacement deposits
rich in lead.
Lead will generally precipitate as primary galena from ore fluids rich in sulphur and lead. Removal of sulphur by precipitation of sulphides, however, may lead ultimately to an ore fluid from which galena cannot be precipitated, even with a high concentration of lead in solution. In these circumstances, anglesite, as well as cerussite and pyromorphite, could be precipitated as a primary mineral. (Strens (1963), MM 33.722-3).
Anglesite is commonly associated with galena, sphalerite, smithsonite, hemimorphite and iron oxides.
At Tsumeb, Namibia, anglesite has been found associated with native copper (R&M 93.6.539). Also, wulfenite and mimetite pseudomorphs after anglesite have been found here (KL p216, 206).
At Caldbeck Fells, Cumbria, England, UK, anglesite is uncommon but widespread. At Brae Fell mine it has been found associated with cerussite, pyromorphite and galena. At the Barndy Gill lead mine it is associated with wulfenite. At the Driggith mine and at Short Grain it is associated with galena. At Dry Gill it occurs with mimetite variety campylite. At Red Gill mine it is associated with linarite or caledonite, and at Silver Gill it is occasionally found altered to leadhillite (C&S).
At Whitwell quarry, Derbyshire, England, UK, anglesite occurs on an oxidised galena - baryte matrix (RES p136, 137).
At the Blanchard mine, Bingham, New Mexico, USA, anglesite pseudomorphs after galena have been found (KL p188).
In the oxidation zone, oxidation of pyrite forms ferrous (divalent) sulphate and sulphuric acid:
pyrite + oxygen + water → ferric sulphate + sulphuric acid
FeS2 + 7O + H2O → FeSO4 + H2SO4
The ferrous (divalent) sulphate readily oxidizes to ferric (trivalent) sulphate and ferric hydroxide:
ferrous sulphate + oxygen + water → ferric sulphate + ferric hydroxide
6FeSO4 + 3O + 3H2O → 2Fe2(SO4)3 + 2Fe(OH)3
Ferric sulfate is a strong oxidizing agent; it attacks galena as below.
Anglesite and cerussite do not usually occur together. Generally anglesite is stable in lower pH (more acid) environments and cerussite in higher pH (more alkaline) environments. Seawater has a pH of approximately 8.3 (somewhat alkaline) so cerussite is the stable lead supergene mineral in contact with seawater (JRS 18.9,11).
Hydrocerussite requires an alkaline environment, and it cannot co-exist with anglesite (JRS 18.11).
galena, ferric sulphate, water and oxygen to anglesite, ferrous sulphate and sulphuric acid
PbS + Fe2(SO4)3 + H2O + 3O → PbSO4 + 2FeSO4 + H2SO4
Galena is oxidised to anglesite and ferric iron is reduced to ferrous iron (AMU b3).
galena and oxygen to anglesite
In air, at outcrops of galena,
PbS + 2O2 → PbSO4
At ordinary temperatures the equilibrium is displaced far to the right, and the apparent stability of galena is a result of the slowness of the oxidation (KB).
galena may also dissolve in carbonic acid from percolating rainwater to form hydrogen sulphide, which is then oxidised to form anglesite. (KB).
galena and carbonic acid to Pb2+, hydrogen sulphide and HCO3-
PbS + 2H2CO3 → Pb2+ + H2S + 2HCO3- (KB).
hydrogen sulphide, oxygen, Pb2+ and HCO3- to anglesite and carbonic acid
H2S + 2O2 + Pb2+ + 2HCO3- → PbSO4 + 2H2CO3 (KB)
The Activity-pH diagram below was calculated for some lead minerals. Boundaries are calculated for constant activity (roughly equivalent to concentration) of (SO4)2- and constant partial pressure (also roughly equivalent to concentration) of CO2, over a range of values of pH and of Cl1- activity. In this case the concentration of CO2 is is appreciably more than the atmospheric value.
Anglesite is stable in an acid environment with a low concentration of Cl- ions. If the concentration of CO2 decreases the stability field of anglesite does not change significantly (JRS 15.20).
The lead mineral formulae are:
The Activity-pH diagram below is similar, but the concentration of CO2 is close to zero, at about 0.01% of the atmospheric value, and the (SO4)2- activity is about 0.5% of its value in the first diagram.
Cerussite does not form in these conditions, the stability field of mendipite is very large, and mereheadite and plumbonacrite can form, although they are not stable at higher levels of concentration of CO2 (JRS 15.22).
The lead mineral formulae are:
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