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. 6.6
An 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. 6.7
a 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
.
.
.
Degree
IAP
sp
of saturation==W
K
IAP Ca CO Ca CO
mol l
=¥ =◊¥◊
=¥ ¥ ¥
=¥
+-+ -
--
aa c c^232232
722
0 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
0
pH
Log [concentration (mol kg
–1
)] H+ OH–
Surface seawater pH
0 2 4 6 8 10 12 14
CO 2 HCO 3 – CO 3 2–
Sediment
Corals
CaCO 3
CO2(g)
CaCO 3
Phytoplankton
OH– + HCO 3
Ca2+
2– –
+
CO 3 + H 2 O
H 2 O
Sample
seawater
@ 25°C
S = 35
CO2(aq) + H 2 OHH 2 CO 3 + + HCO 3
Fig. 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.