Other
Scientific paper
Aug 1965
adsabs.harvard.edu/cgi-bin/nph-data_query?bibcode=1965gecoa..29..947b&link_type=abstract
Geochimica et Cosmochimica Acta, vol. 29, Issue 8, pp.947-965
Other
4
Scientific paper
Measurements of pH of sea water samples equilibrated with known partial pressures of CO 2 and with calcite and aragonite have enabled the determination of molal activity coefficient for bicarbonate, carbonate, and calcium ions in two sea water samples at 25°C and 1 atm total pressure. Results are: For standard artificial sea water (chlorinity = 19.0 , titration alkalinity = 2.36 × 10 -3 molal): HCO 3 - = 0.550 ± 0.007 CO 3 2- = 0.021 ± 0..004 Ca 2+ = 0.203 ± 0.010 For natural sea water from Woods Hole, Massachusetts (chlorinity = 17.0 , titration alkalinity = 2.09 × 10 -3 molal): HCO 3 - = 0.561 ± 0.006 CO 3 2- = 0.024 ± 0..004 Ca 2+ = 0.223 ± 0.020 These values indicate the essential validity of the chemical model of Garrels and Thompson (1962). The normal range in temperature and salinity of the open ocean, away from immediate sources of fresh water, is sufficiently small so that the values cited above can be used, as a first approximation, to represent the whole ocean. Only relatively minor corrections for the effect of depth (pressure) on the activity coefficients need be made for depths less than 5000 m. Values of the activity coefficients when combined with measurements of pH, m CO 3 2+ and carbonate alkalinity can be used to calculate the ion activity product, IAP = a Ca 2+ + · a CO 3 2- , for sea water. Comparison of IAP with the thermodynamic solubility product, K s , of calcite and aragonite indicates that low latitude surface sea water is supersaturated with respect to both phases. Similar calculations for sea water at depth, based on an assumed "average" ocean model, indicate that a large proportion of sub-surface sea water is undersaturated with respect to calcite and, therefore, all other forms of CaCO 3 .
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