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Buffer Intensities and Equilibrium pH of Minerals and Soils: I. The Contribution of Minerals and Aqueous Carbonate to pH Buffering
Author(s) -
Breemen N.,
Wielemaker W. G.
Publication year - 1974
Publication title -
soil science society of america journal
Language(s) - English
Resource type - Journals
SCImago Journal Rank - 0.836
H-Index - 168
eISSN - 1435-0661
pISSN - 0361-5995
DOI - 10.2136/sssaj1974.03615995003800010022x
Subject(s) - gibbsite , kaolinite , carbonate minerals , chemistry , albite , nontronite , silicate minerals , oxide minerals , siderite , inorganic chemistry , alkalinity , anorthite , silicate , aqueous solution , calcite , carbonate , allophane , mineral , clay minerals , mineralogy , geology , quartz , chemical reaction , paleontology , biochemistry , organic chemistry
Thermodynamic equilibrium considerations are used to calculate pH buffer intensities for a number of aqueous systems involving 16 common soil and rock minerals (viz. gibbsite, kaolinite, allophane, hematite, limonitic iron oxide, quartz, amorphous silica, calcite, siderite, hydrated magnetite + amorphous Fe(OH) 3 , microcline, albite, anorthite, Mg‐montmorillonite, two illites, and Mg‐chlorite), gaseous CO 2 and 26 dissolved species. The calculation of buffer intensities is outlined for simple oxides and carbonates (analytical evaluation) and for silicate minerals during congruent and incongruent dissolution (graphical differentiation). Silicate minerals, carbonates and gibbsite provide strong buffering upon addition of strong acid under slightly alkaline to slightly acid conditions. Carbon dioxide at constant partial pressure is far more effective than any of the minerals considered in counteracting the effect of an increase in alkalinity.