bonate (CO 32 - ). Measured Ca^2 +and CO 32 - ocean surface concentrations are 0.01
and 0.000 29 mol l-^1 respectively and thus the ion activity product (IAP) (see Box
4.12) can be calculated:eqn. 6.5
This value is much greater than the solubility product (see Box 4.12) of calcite
(CaCO 3 ), which is 3.3¥ 10 -^9 mol^21 -^2 at 25°C and 1 atmosphere pressure, a suit-
able choice for tropical surface seawater. The degree of saturation (see Box 4.12)
is:eqn. 6.6An Wvalue of 1 indicates saturation, values greater than 1 indicate supersatura-
tion, and values less than 1 indicate undersaturation. Using the values for calcite
above we get:eqn. 6.7a value that implies surface seawater in the tropics is highly supersaturated with
respect to calcite. This approach neglects the effects of ion pairing (Box 6.4).W=
¥
¥
=
15 10
33 10
45 4
7
9.
.
.
DegreeIAP
spof saturation==W
KIAP Ca CO Ca COmol l=¥ =◊¥◊
=¥ ¥ ¥
=¥
+-+ ---aa c c^2322327220 01 0 26 0 00029 0 2
15 10
gg
....
.The Oceans 197(a) (b)
- 5
- 4.5
- 4
- 3.5
- 3
- 2.5
- 2
- 1.5
- 1
- 0.5
0pHLog [concentration (mol kg–1
)] H+ OH–Surface seawater pH0 2 4 6 8 10 12 14CO 2 HCO 3 – CO 3 2–SedimentCoralsCaCO 3CO2(g)CaCO 3PhytoplanktonOH– + HCO 3
Ca2+2– –+CO 3 + H 2 OH 2 OSample
seawater
@ 25°C
S = 35CO2(aq) + H 2 OHH 2 CO 3 + + HCO 3Fig. 6.8(a) Schematic diagram to illustrate the buffering effect of CaCO 3 particles (suspended in the water
column) and bottom sediments on surface seawater HCO 3 - concentrations (after Baird 1995, with permission
from W.H. Freeman and Company.). (b) A sample of the seawater in (a) will have a pH very close to 8 because
of the relative proportions of CO 2 , HCO 3 - and CO 32 - , which in seawater is dominated by the HCO 3 - species.
Increased CO 2 concentrations in the atmosphere from anthropogenic sources could induce greater dissolution
of CaCO 3 sediments including coral reefs.