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EFFECTS OF CHANGES IN CARBONATE CHEMISTRY
ON NUTRIENT AND METAL SPECIATION
Hein De Baar Loes GerringaHein De Baar, Loes Gerringaand Charles-Edouard Thuroczy
Biological Elements in SeawaterC N
Al Si PGe
Ca Mn Fe Co Ni Cu ZnAg Cd
Ba La
L C Nd S E Gd Tb D H E T Yb LLa Ce Nd SmEu Gd Tb Dy Ho Er Tm Yb Lu
Element in biochemical function (soft tissue)Element in biochemical function (soft tissue)
Element in skeletal part (hard shell, frustule)
Apparent coupling with ocean biological cycle
Metals Abundance & Biological Evolution
Zn1260
Cu522
Ni49300
Co2250
Fe900000
Mn9550
Cd ?Ag
12605224930022509000009550
PbH
Cd ?1.61
Ag0.49
Pb315
Hg0.34
Biological Evolution used abundant metals: essentialL b d t t l bi f ti t i
numbers of atoms versus 1 million Si atoms
Low abundant metals no bio-functions: toxic
De Baar & La Roche (2003)Case studies for Fe, Cu, Zn, Cd
Contents
• Small changes in CO2 chemistry are significant– effects on underwater sound– effects on biology
• Small changes in nutrient chemistry– Silicate
• sidestep: AluminiumPh h t– Phosphate
• Speciation of trace metals Zn, Cu, CdS i ti f i F• Speciation of iron Fe
• Future work• Summary
What is SpeciationWhat is Speciation
Different physical chemical states of a• Different physical-chemical states of a chemical element in seawater
t l di l d ll id l ti l– truly dissolved, colloids, larger particles– oxidation state, Fe(II) versus Fe(III)– weak acid (H2CO3) or weak base (NH4OH)– inorganic complexation (e.g. NaHCO3
0)– organic complexation (e.g. Fe(III)Lorganic)
DIC and Alkalinity at the Zero Meridian
50 0S station Steven van Heuven, unpubl. data, 2008
Zero Meridian Station 10700 16 13’ S 01026 1’ W500 16.13’ S, 01026.71’ W
2100.0 2200.0 2300.0 2400.00
7.8 7.9 8.0 8.1020.0 30.0
0
500
0
500
1000
0
500
1000 CO21000
1500
2000
Dept
h (m
)
1000
1500
2000
Dept
h (m
) pH 1500
2000Dept
h (m
)
2000
2500
DICAlk
2000
2500
3000
2500
3000
3000
3500
3000
35003500
deep waters already are natural laboratory for low pH
Steven van Heuven, unpubl. data, 2008
Today and future scenario at 49 m depthStation 107 (50 0S 01 0W)Station 107 (50 0S, 01 0W)
year DIC ALK pCO2 pHy p p
2008 2144 2287 360 8.07
Future:
2100 ? 2249 2287 800 7.76
2300 ? 2325 2287 1500 7.5DIC and ALK above units micromol per kg seawater
these were converted to micromol per Liter for Mineql+ Version 4.6 (2007) simulations
CO2 System Speciation ith M j I i S twith Major Ions in Seawater
CO2 System Speciation at pCO2=360 ppm and pH=8.07
CO3(2-)
CaHCO3+
H2CO3 (aq)
HCO3HCO3-
MgHCO3+
NaHCO3 (aq)NaHCO3 (aq)
CaCO3 (aq)
MgCO3 (aq)Mineql+ g ( q)
NaCO3-
MineqlVersion 4.6(2007)
Unanticipated Consequences of Ocean Acidification: A Noisier Ocean at Lower pH
Keith Hester, Edward Peltzer, William Kirkwood and Peter BrewerGeophysical Research Letters (2008)
Decrease in ocean sound absorption for frequencies lower than 10 kHz Decrease in ocean sound absorption for frequencies lower than 10 kHz.
This effect is due to known pH-dependent chemical relaxations in theB(OH) /B(OH) - and HCO -/CO 2- systems B(OH)3/B(OH)4 and HCO3 /CO3 systems.
The pH change of 0.3 units anticipated by mid-century, results in adecrease of sound absorption by almost 40% decrease of sound absorption by almost 40%.
Simplified scheme is a coupled exchange reaction with ion-pairing:
In fact the species CaCO3(aq) and CaHCO3+ as well as MgCO3(aq) and MgHCO3
+ are involved
Also Presentation by D. Browning at Wednesday morning
Will marine mammals adapt ?
U d t d i l d Underwater sound is already increasing due to human activity (ships, sonar, etc.)
The additional decrease of sound absorption is an extra concern59 oSouth, February 2008
Simplified CO2 System in SeawaterCO2 System in Seawater
at pCO2=360 ppm and pH=8.07
CO2
HCO3-HCO3
CO32-
CO2 System Speciation at pCO2=360 ppm and pH=8.07
CO3(2-)
CaHCO3+
H2CO3 (aq)
HCO3-HCO3
MgHCO3+
NaHCO3 (aq)
CaCO3 (aq)
MgCO3 (aq)
NaCO3-
Future changes CO2 system:changes of minor players can make a difference
2500
2000
2500
1500
= [1
0-6
M]
CO2(aqueous)
1000
[Mic
rom
ol] = CO32-
HCO3-
500
01 2 38.07 7.76 7.5 pH
360 800 1500 pCO2
M j l HCO i it t blMajor player HCO3- remains quite stable
Minor players CO2 and CO32- change more
this is our concern for photosynthesis and calcification, respectively
Equilibrium Thermodynamics in Mineql+4.6(2007)
The thermodynamic equilibrium simulation only mimics The thermodynamic equilibrium simulation only mimics the existing or predicted situation
The rate or kinetics of any chemical reaction is notassessed
Conversion between chemical species:H2O + CO2 = HCO3
- + H+H2O + CO2 = HCO3 + HThis is a slow reaction
Therefore chemical speciation is importantTherefore chemical speciation is important(acceleration by enzyme Carbonic Anhydrase)
When the rates of conversion reactions are fast, then chemical speciation in seawater may be less important
15Si(OH)4 [10-6M]
Silicate Speciation
10
or P
erce
nt
Si(OH)4 [10 6M]H3SiO4- [10-6M]H3SiO4- [%]
0
5
[10-
6 M
]
pH 8.07 7.76 7.5
Si(OH) [10 6 M] 12 0 12 1 12 2
%%%
1 2 3
pH
8.07 7.76 7.50
At tenfold expanded scale:
Si(OH)4 [10-6 M] 12.0 12.1 12.2
H3SiO4- [10-6 M] 0.151 0.074 0.041
1
1.5
Perc
ent
Total Si [10-6 M] 12.2 12.2 12.2
Percent H3SiO4- 1.2 % 0.6 % 0.3 %
%
0.5
0-6
M]
or P
Si(OH)4 [10-6M]H3SiO4- [10-6M]
%
%
01 2 3
pH
[1 H3SiO4- [%]
8.07 7.76 7.50
Silicate speciation: does it matter ??(who cares ?)( )
Milligan et al (2004)Si uptake and dissolution by diatomsconditions pH = 8.5 and pH = 7.8Si uptake rate not affected by pHSi dissolution rate is 6-7 fold higher at low pHat low pH more Si efflux from cell: lower Si/C ratioeffect on Si stable isotope fractionation yet to be assessed
Del Amo & Brzezinski (1999)4 diatoms at pH 8.0 and pH 9.2Si(OH)4 is by far the preferred Si species for diatom uptakeone diatom P. tricornutum behaves different from other 3 diatoms
Recommendation:assess conceivable effect on fractionation of stable isotopes of Si
With gratitude to Damien Cardinal for responding to my questions
use more realistic pH value ranges in diatom studies
Biological Elements in SeawaterC N
Al Si PGe
Ca Mn Fe Co Ni Cu ZnAg Cd
Ba La
L C Nd S E Gd Tb D H E T Yb LLa Ce Nd SmEu Gd Tb Dy Ho Er Tm Yb Lu
Element in biochemical function (soft tissue)Element in biochemical function (soft tissue)
Element in skeletal part (hard shell, frustule)
Apparent coupling with ocean biological cycle
Titanium ultraclean sampling systemwith Kevlar hydrowirefor trace elements in seawater(De Baar et al., 2008, Marine Chemistry)
Ultra Clean Sub-sampling inside clean containers de c ea co a e
Al in high latitude Arctic Ocean Steady increase of dissolved Al with increasing depth
Looks like silicate
Rob Middag, unpublished data, Arctic Geotraces, Polarstern 2007
Aluminium Speciation 70
65 69
Aluminium: major shiftsp
at pH = 8.07 and pCO2 = 360 ppm
50
60
44
53
65
Al(OH)2+Al(OH)3 (aq)Al(OH)4- 30
40
Perc
enta
ge [%
]
Al(OH)2+Al(OH)3 (aq)Al(OH)4-27( )
10
20
P
3
15
8
16
01 2 3
pH
3
8.07 7.76 7.5
pH = 8.07 pH = 7.76 pH = 7.5
Al(OH)2+
Al(OH)3 (aq)
Al(OH)4-
Major shifts Al speciation: does it matter ?
Thalassiosira nordenskjioldiiAl Si 1 3 1000
Gehlen et al (2002); Al incorporation in growing diatoms
Al : Si = 1.3 : 1000Al : Si = 3.8 : 1000
uptake ratio varies with Al/Si ratio in t diseawater medium
Dissolution of opal diatom frustules decreases significantly with higher Al:Si decreases significantly with higher Al:Si ratio of the biogenic opal (Van Bennekom)
Speciation changes of Al in seawater likely affect the uptake ratio Al:Si by diatoms
The 6-7 fold higher opal dissolution at l H (Milli t l 2004) ll b lower pH (Milligan etal 2004) may well be due to shifts in Al speciation affecting the Al:Si ratio of opal hence the dissolution
Phosphate speciationPhosphate Speciation with Major IonsPhosphate Speciation with Major Ions
at pH = 8.07
MgHPO4 (aq)
NaHPO4-
H2PO4-
Phosphate Speciation at pH = 8.07Simplified in 3 Categories
HPO4-2
CaPO4-
H2PO4-
HPO42-
PO43-PO43
Phosphate speciation with ocean acidification100
pH 8.07 7.76 7.5
H2PO4- 2 2 % 4 4 % 7 8 %
60
80
tage
[%]
H2PO4-HPO42- H2PO4 2.2 % 4.4 % 7.8 %
HPO42- 96.2 % 94.8 % 91.7 %20
40
Perc
ent HPO42
PO43-
At tenfold expanded scale:
PO43- 1.6 % 0.8 % 0.4 %
01 2 3
pH8.07 7.76 7.5
• major shifts of two minor species• (just like the CO2 system)8
10
%]
• does it matter ?• probably not ?
onl 1 stable isotope 31P2
4
6
Perc
enta
ge [% H2PO4-
HPO42-PO43-
• only 1 stable isotope 31P• who cares ?
01 2 3
pH8.07 7.76 7.5
Acidification effect on third major nutrient NitrogenNitrogen
• Nitrate is strong ion• Nitrate is strong ion– only one species NO3
- and this will not be affected
• Ammonia is weak ion– speciation obviously will be affected
Zinc, Copper and Cadmium
Zn1260
Cu522
Ni49300
Co2250
Fe900000
Mn9550
Cd Ag
12605224930022509000009550
PbH
Cd 1.61
Ag0.49
Pb315
Hg0.34
numbers of atoms versus 1 million Si atoms
Zinc Inorganic SpeciationZn is key element in enzyme Carbonic Anhydrasey y y
Zinc Inorganic Speciation at pH = 8.07 Total Zn = 0.4 nM
Zn(2+)
ZnHCO3+ Zn Inorganic Speciation
ZnCO3 (aq)
Zn(SO4)2-2
ZnSO4 (aq) 70
80
90
100
%]
Zn(2+)
ZnHCO3+
30
40
50
60
Perc
enta
ge [%
ZnCO3 (aq)
Zn(SO4)2-2
0
10
20
1 2 3
ZnSO4 (aq)
decrease of ZnCO3(aq) species
pH
Zn Inorganic Speciation
15Zn(2+)
10
ge [%
] ZnHCO3+
ZnCO3 (aq)10
5Perc
enta
g ( q)
Zn(SO4)2-26
5P
ZnSO4 (aq)3
01 2 3
pH
8.07 7.76 7.5
pH
ZnCO3(aq) would decrease from 10 % to 6% to 3 % with ocean acidification
Zinc Speciation with Natural Organic LigandZinc Organic SpeciationT t l Z 0 4 M Zinc Organic Speciation
100 ZnLZn(2+)
96.6 97.297Total Zn = 0.4 nM
Total Ligand = 2.2 nMK(ZnL) = 10.8
[%]
( )
le
This Ligand also binds Cd and Cu at same time
Sum (Zn+Cd+Cu)=1.2 nM
10
Perc
enta
ge
Lo
g s
cal
Assumption:L binding strength does not
h ith H
18 07 7 76 7 5
1.6 1.6 1.6change with pH
Zinc-binding Ligand after Ellwood 2004; Lohan et al., 2005;
Very strong organic complexation stabilizes everything
1 2 3
pH
8.07 7.76 7.5Bruland 1989
Very strong organic complexation stabilizes everythingNo impact of ocean acidification on Zn speciationNo tipping point manuscript to Nature/Science
Copper (Cu) Inorganic SpeciationCu Inorganic Speciation
at pH = 8.07 at pCO2 =360 ppm
Cu(2+)70
80
90
Cu(2+)Cu(2+)
CuOH+
Cu(OH)2 (aq)
CuCl+40
50
60
erce
ntag
e [%
]
Cu(2+)CuOH+Cu(OH)2 (aq)CuCl+CuCO3 (aq)
CuCl+
CuCO3 (aq)
Cu(CO3)2-210
20
30
Pe Cu(CO3)2-2
Cu Inorganic Speciation mostly carbonatesand also OH species
Very promising for major changes ??
01 2 3
pH8.07 7.76 7.5
Very promising for major changes ?? pH 8.07 7.76 7.5
Free Cu(2+) 6 % 11 % 17 %
CuCO3 (aq) 81 % 80 % 72 %
Cu(CO3)22- 7 % 4 % 2 %
Copper speciation with natural organic ligandTotal Cu = 0.6 nM
Total Ligand = 2.2 nMK(CuL) = 13.8
80
100
This Ligand also binds Cd and Cu at same time
Sum (Zn+Cd+Cu)=1 2 nM
60
80
tage
[%]
CuLSum (Zn+Cd+Cu)=1.2 nM
Assumption:L binding strength does not 20
40
Perc
ent CuL
change with pH
Cu binding Ligand after Gerringa et al 1995;
01 2 3
H8.07 7.76 7.5
Gerringa et al., 1995; Laglera & Van Den Berg, 2003; Moffett, 2007
Full 100% organic complexation at every pH value
pH
Full 100% organic complexation at every pH valueNo impact of ocean acidification on Cu speciationNo tipping point manuscript to Nature/Science
80
Cadmium Speciation without and with Organic Ligand
60
80
[%]
Free Cd(2+)
Cd Inorganic Speciation
40
5064% 64% 64%
40
erce
ntag
e [ ( )
CdCl+CdCl3-CdCl2 (aq)CdL20
30
40
cent
age
[%]
Free Cd(2+)CdCl+CdCl3-
0
20
1 2 3
P CdL
0
10
20
Per CdCl2 (aq)
8.07 7.76 7.5
pH1 2 3
pH
8.07 7.76 7.5
3 % free Cd2+ ionFor the rest only Chlorine species
Total Cd = 0.2 nMTotal Ligand = 2.2 nMFor the rest only Chlorine species
No pH dependence at all
64 % Cd-L organic complex
K(CdL) = 10.8 after Ellwood, 2004
This Ligand also binds Zn and Cu at same timeSum (Zn+Cd+Cu)=1.2 nM
64 % Cd L organic complex1 % free Cd2+ ion
For the rest only Chlorine speciesNo pH dependence at all
Gold is for the mistressSilver for the maid
Copper for the craftsmanCopper for the craftsmancunning at his trade.
“Good” said De BaaronGood said De Baaronsitting in this hall:
“But iron – cold iron –is master of them all ”is master of them all.
free after Rudyard Kipling (1910)
Surface Ocean: Iron Speciation crucial for biological uptake by phytoplankton in the euphotic zone
photoreduction
solidsFe2O3
colloids
[FeCO ]0
Fe2O3Fe(OH)3FeOOH
[Fe ] [Fe ]? ?
[Fe(OH) ][Fe(OH) ]2+
+23+2+
[FeCO ]3
[FeOH ]+
[Fe(II)L]?
sidero-
[ ( ) ]
cell
[Fe(III)L]? ?
siderophoresphotoreduction
[Fe(III)L]organic complexes
Gerringa et al, 2000
Deep Ocean: Competition between Stabilization by Organic Complexation versus Removal via Colloids controls Residence Time of Fe in the Oceans
upper ocean
eanstabilization removal
eep
oce
dissolvedstable fine colloids
Fe-particles
000m
dedissolved[Fe3+]dissolved
[Fe3+]-organiccomplex
colloidsFe-
particles
particles
> 0.2 micron
40
complex
sedimentation
seafloor
Case 1: inorganic speciation, no light (dark ocean)
photoreduction
solid
colloids
[FeCO ]0
FeOOHgoethite
[Fe ] [Fe ]? ?
[Fe(OH) ][Fe(OH) ]2+
+23+2+
[FeCO ]3
[FeOH ]+
[Fe(II)L]?
sidero-
[ ( ) ]
cell
[Fe(III)L]? ?
siderophoresphotoreduction
[Fe(III)L]organic complexes
Gerringa et al, 2000
Case 1: inorganic speciation, no light (dark ocean)
Surface sample at 49 m depth:< 0.2 micron
[Fe] = 0.096 nM = 96 pM 1.E-10 Fe'[Fe] 0.096 nM 96 pMAssume no Ligand
7.E-11
8.E-11
9.E-11 GOETHITE88 pM82 pM
72 pM
4.E-11
5.E-11
6.E-11
Con
cent
ratio
nDissolved Inorganic Iron
Fe(OH)2+
1.E-11
2.E-11
3.E-11
8 pM
24 pM
14 pM
Fe(OH)2+
Fe(OH)3 (aq)
Fe(OH)4-
0.E+001 2 3
pH
90 % of the dissolved Fe would precipitate
8.07 7.76 7.5
( )
S f ll i i iSum of all inorganic species:Fe’ = Fe(OH)2
+ + Fe(OH)3 + Fe(OH)4-
Case 2: include organic ligand, delete solid FeOOH, no light (dark ocean)
photoreduction
solid
colloids
[FeCO ]0
FeOOHgoethite
[Fe ] [Fe ]? ?
[Fe(OH) ][Fe(OH) ]2+
+23+2+
[FeCO ]3
[FeOH ]+
[Fe(II)L]?
sidero-
[ ( ) ]
cell
[Fe(III)L]? ?
siderophoresphotoreduction
[Fe(III)L]organic complexes
Gerringa et al, 2000
Case 2: include organic ligand, delete solid FeOOH, no light (dark ocean)
Surface sample at 49 m depth:< 0 2 micron
100
Prediction of speciation model:
< 0.2 micron[Fe] = 0.096 nM = 96 pMLigand = 0.668 nM = 668 pM
80
96pM
96pM
96pM
40
60
FeL
[pM
]
FeL
20
01 2 3
pH
8.07 7.76 7.5
All the dissolved Fe is bound by the ligand, thus stable in seawater
Case 2: Measure the organic complexation in real samplecomplexation in real sample
• deep water sample (2500m depth)– measurement onboard: Fe=0.95 nM, L=1.64 nMmeasurement onboard: Fe 0.95 nM, L 1.64 nM
• adjusted to 3 different pH values 7.75, 8.05, 8.25 in laboratory• measure ligand concentration L and its stability constant K
pH L [nM] error (L) logK error logKOnboard 1.638 0.110 22.42 0.18
8.057.75 1.686 0.067 22.52 0.118 05 1 734 0 081 22 82 0 158.05 1.734 0.081 22.82 0.158.25 1.694 0.065 22.84 0.10
Ligand concentration L does not change significantlyLigand concentration L does not change significantlyStability constant logK does not change significantlyThis supports modeling assumption that K is independent of pH
Case 3: include organic ligand, dissolve FeOOH as much as possible, no light (dark ocean)
photoreduction
solid
colloids
[FeCO ]0
FeOOHgoethite
[Fe ] [Fe ]? ?
[Fe(OH) ][Fe(OH) ]2+
+23+2+
[FeCO ]3
[FeOH ]+
[Fe(II)L]?
sidero-
[ ( ) ]
cell
[Fe(III)L]? ?
siderophoresphotoreduction
[Fe(III)L]organic complexes
Gerringa et al, 2000
Case 3: include organic ligand, dissolve FeOOH as much as possible, no light (dark ocean)
700
800Total Dissolved Fe = Fe’ + FeLSurface sample:
Ligand = 0.668 nM =
698674
522 712688
500
600
Dis
s Fe
[pM
]Fe'
FeL
668 pM
Original Fe = 96 pM514
300
400
FeL
or T
otal
D FeL
TotalDissolved Fe
100
200
Fe' o
r Dissolved Fe
8 14 24Original Fe = 96 pM
01 2 3
pH8.07 7.76 7.5
8 14 24
The Excess Ligand of Todays Ocean Can Accomodate more dissolved FeBy Ocean Acidification the dissolved Fe in Seawater can increase even more
Dissolution of solid phase Fe and Mn is much Dissolution of solid phase Fe and Mn is much more a function of low oxygen conditions than of pHthan of pH
Strong Fe and Mn maxima exist in subsurface i i f E t i l E t oxygen minimum zones of Equatorial East
Pacific, Northwest Indian Ocean (L di t l 1987 S t l 1989)(Landing et al. 1987, Saager et al. 1989)
... however this meeting happens to be about pH not oxygen
How about photoreduction to Fe(II) in open ocean ?How about the fine colloids in open ocean ?
photoreduction
solidsFe2O3
colloids
[FeCO ]0
Fe2O3Fe(OH)3FeOOH
[Fe ] [Fe ]? ?
[Fe(OH) ][Fe(OH) ]2+
+23+2+
[FeCO ]3
[FeOH ]+
[Fe(II)L]?
sidero-
[ ( ) ]
cell
[Fe(III)L]? ?
siderophoresphotoreduction
[Fe(III)L]organic complexes
Gerringa et al, 2000
Photochemistry in upper euphotic zoneof the open oceanof the open ocean
Photoreduction of Fe(III) to Fe(II)only in upper euphotic zoneonly in upper euphotic zonebeyond chemical thermodynamics predictionrapid re-oxidation but slower in cold polar waters
ll ti f th d i t F (III)L i di i tsmall portion of the dominant Fe(III)L species dissociatesinto free Fe(II) and free L
the free Fe(II) likely is more available for uptake by algae
Photochemical breakdown of organic ligand Lyes but only of small labile portion of total L poolyes but only of small labile portion of total L poolligand L is very stable and uniform throughout world ocean
this supports the notion of long term chemical stability li d b i f d i f t f bi tnew ligand being formed in surface waters from biota
surface waters tend to have large excess of ligand versus Fe
Future work in open ocean waters
• response of Fe colloids size class to acidification• response of Fe-colloids size class to acidification– adjust 0.2 micron filtered seawater to different pH values– wait some timewait some time– ultrafiltration and then measure Fe and L in size fractions– physical-chemical modeling ?
• Acidification effects on other metals– Mn manganese– lanthanides series (dominated by CO3
2- species)• but who cares about the lanthanides ?
Summary• shifts in Silicate speciation may affect fractionation of Si stable
isotopesf ff• major shifts in Aluminium speciation may affect its uptake in
diatom frustules, hence dissolution of biogenic Silicon• major shifts of two minor species of Phosphate any effects onmajor shifts of two minor species of Phosphate, any effects on
biota unknown• Zn, Cu and Cd are strongly stabilized by organic complexation• excess organic ligand in modern ocean may accomodate more
dissolved Fe than is currently present• if so then in the future more acidic ocean somewhat more Fe• if so, then in the future more acidic ocean somewhat more Fe
may dissolve• caveats:
– in fact the open ocean ligand does not carry as much Fe as it could