Open Access

Inorganic speciation of dissolved elements in seawater: the influence of pH on concentration ratios

Geochemical Transactions20023:11

DOI: 10.1186/1467-4866-3-11

Received: 24 October 2001

Accepted: 07 January 2002

Published: 22 January 2002

Abstract

Assessments of inorganic elemental speciation in seawater span the past four decades. Experimentation, compilation and critical review of equilibrium data over the past forty years have, in particular, considerably improved our understanding of cation hydrolysis and the complexation of cations by carbonate ions in solution. Through experimental investigations and critical evaluation it is now known that more than forty elements have seawater speciation schemes that are strongly influenced by pH. In the present work, the speciation of the elements in seawater is summarized in a manner that highlights the significance of pH variations. For elements that have pH-dependent species concentration ratios, this work summarizes equilibrium data (S = 35, t = 25°C) that can be used to assess regions of dominance and relative species concentrations. Concentration ratios of complex species are expressed in the form log[A]/[B] = pH - C where brackets denote species concentrations in solution, A and B are species important at higher (A) and lower (B) solution pH, and C is a constant dependent on salinity, temperature and pressure. In the case of equilibria involving complex oxy-anions (MO x (OH) y ) or hydroxy complexes (M(OH) n ), C is written as pK n = -log K n or pK n * = -log K n * respectively, where K n and K n * are equilibrium constants. For equilibria involving carbonate complexation, the constant C is written as pQ = -log(K2 l K n [HCO3-]) where K2 l is the HCO3 - dissociation constant, K n is a cation complexation constant and [HCO3-] is approximated as 1.9 × 10-3 molar. Equilibrium data expressed in this manner clearly show dominant species transitions, ranges of dominance, and relative concentrations at any pH.

Introduction

Solution speciation exerts important controls on chemical behavior. Speciation is known to influence solubility, membrane transport and bioavailability, adsorptive phenomena and oceanic residence times, volatility, oxidation/reduction behavior, and even physical properties of solutions such as sound attenuation. In recognition of such influences, substantial efforts have been made to characterize the chemical speciation of elements in seawater. While assessments of organic speciation have dominantly been obtained using modern voltammetric procedures and, as such, have a relatively short history, assessments of inorganic speciation typically involve a wide variety of analytical procedures that have been employed over many decades.

Assessments of the inorganic speciation of seawater began with attempts [1] to determine dominant chemical forms in seawater based on available thermodynamic data. Early compilations of Principal Species [2] dominantly involved (a) simple hydrated cations and anions (e.g. Na+, Ca2+, Cl-, F-), (b) ion pairs with sulfate (e.g. MgSO40 and CaSO40), (c) fully hydrolyzed elements (e.g. H m PO4 m-3, H m AsO4m-3, MoO42-and WO42-) and (d) chloride complexes (e.g. AuCl2-, HgCl42-). While it was noted [1, 2] that hydroxide complexes were important for all ions with oxidation numbers greater than two, hydroxide complexes were notably absent in Principal Species tabulations until the following decade.

The thermodynamic data compilations of Sillén and Martell [3, 4] catalyzed rapid advances in equilibrium models of seawater speciation. These works were followed by additional compilations [57] that were critically important to modern sea-water speciation assessments. In view of these developments, and additional extensive experimental analyses appropriate to seawater, Principal Species assessments ten to fifteen years after the pioneering work of Sillén demonstrated a much improved awareness of the importance of hydrolysis in elemental speciation. [810]

An additional major speciation assessment [11] provided a greatly improved, comprehensive view of inorganic complexation in seawater. Based on the analogous characteristics of metal complexation by carbonate and oxalate, Turner et al. [11] concluded that rare earth element complexation in seawater is dominated by carbonate. Subsequently, as the result of approximately twenty years of progress in seawater speciation, the Principal Species assessment of Bruland [12] listed seventeen elements with carbonate-dominated Principal Species.

Speciation calculations

Based on currently available data, Principal Species for a substantial portion of the periodic table (through atomic number 103) are thought to be controlled or influenced by pH. The main objective of the present work is a review of Principal Inorganic Species for the elements in seawater. The principal focus of this work is an assessment of the influence of pH on inorganic speciation.

The Principal Species assessment in this work differs from previous presentation formats in its objective of providing a simple quantitative means of assessing Principal Species variations with changes in pH. Stepwise equilibrium constants provide a simple means of assessing species concentration ratios as a function of pH. In the case of equilibria involving simple protonation of complex anions, MO x (OH) y n-, stepwise equilibrium constants are expressed in the form

where An- = MO x (OH) y n-. Consequently,

and

log [H m Am-n]/[Hm+1Am+1-n] = -pKn-m+pH       (2)

where pH = -log [H+] and pKn-m= -log Kn-m. In the case of simple stepwise hydrolysis equilibria,

M(OH)n-1 +H2OM(OH) n + H+,

stepwise hydrolysis constants are written as

whereupon,

and

In the case of equilibria involving carbonate, due to the near constancy of HCO3- concentrations in seawater, equilibria can be conveniently written in the following form

M(CO3)n-1+HCO3-M(CO3) n + H+

and

where

Using the dissociation constant of HCO3- in seawater (K2 l ), and K n values appropriate to various carbonate complexation equilibria in seawater, the relative concentrations of M(CO3) n and M(CO3)n-1 can be written as

log[M(CO3) n ]/[M(CO3)n-1] = -pQ n +pH       (6)

where log Q = log(K n K2 l [HCO3-]) = -pQ n and [HCO3-] is assumed to be well approximated as 1.9 × 10-3 M (i.e. log[HCO3-] = -2.72).

Based on equilibrium data compilations including Smith and Martell, [5, 6] Martell and Smith, [7] Baes and Mesmer, [13] Turner et al., [11] Byrne et al., [14] and Liu and Byrne, [15] Table 1 provides a compilation of pK n , pK n * and pQ n data, and equilibrium speciation schemes appropriate to seawater (S = 35) at 25°C. The first two columns of Table 1 provide each element's atomic number and identity. The third column provides either (a) each element's dominant forms and speciation, or (b) the chemical species whose relative concentrations are to be evaluated using the data in column 4. As an example of the use of Table 1, the entry for Be indicates that the concentrations of Be2+ and BeOH+ are equal in seawater (25°C) at pH 5.69 and the concentrations of Be(OH)+ and Be(OH)20 are equal at pH 8.25. Hence, at pH 8.0 BeOH+ is the dominant species and the ratios [Be2+]/[BeOH+] and [Be(OH)20]/[BeOH+] are calculated as 10-2.31 and 10-0.25. The pK* and pQ entries for CuII indicate that
Table 1

A compilation of pK n , pK n *, pQ n data and equilibrium speciation schemes appropriate to seawater (S 35) at 25°C. Equilibrium constants are expressed on the free hydrogen ion concentration scale.

Atomic number

Element

Principal species

Equilibrium data

1

H

H+ (68%), HSO4 - (29%), HF0 (3%)

 

2

He

He

 

3

Li

Li+ (98%), LiSO4 - (2%)

 

4

Be

Be2+/BeOH+/Be(OH)2 0

pK1* = 5.69; pK2* = 8.25

5

B

B(OH)3 0/B(OH)4 -

pK* = 8.74

6

C

CO2/HCO3 -/CO3 2-

pK1 = 6.00; pK2 = 9.09

7

N

NO3 -, NO2 -, N2; NH4 +/NH3

pK = 9.35

8

O

O2

 

9

F

F- (50%), MgF+ (50%)

 

10

Ne

Ne

 

11

Na

Na+ 98%, NaSO4 - (2%)

 

12

Mg

Mg2+ (90%), MgSO4 0 (10%)

 

13

Al

A1(OH)2 +/A1(OH)3 0/A1(OH)4 -

pK3* = 5.7; pK4* = 7.7

14

Si

Si(OH)4/SiO(OH)3 -

pK = 9.32

15

P

H2PO4 -/HPO4 2-/PO4 3-

pK2 = 6.10; pK3 = 8.93

16

S

SO4 2- (33%), NaSO4 - (35%), MgSO4 0 (20%)

 
  

HSO4 -/SO4 2-

pK 1

17

Cl

Cl- (100%)

 

18

Ar

Ar

 

19

K

K+ (99%)

 

20

Ca

Ca2+(89%), CaSO4 0(11%)

 

21

Sc

Sc(OH)2 +/Sc(OH)3 0/Sc(OH)4 -

pK3* = 6.4; pK4* = 9.6

22

Ti

Ti(OH)3 +/Ti(OH)4 0

pK* = 2.5

23

V

VO2(OH)2 - /VO3(OH)2-/VO4 3-

pK2 = 7.4; pK3 ≤ 13

24

Cr

Cr(OH)2 +, Cr(OH)3 0, Cr(OH)4 -

pK3* = 8.3; pK4* = 9.1

25

Mn

Mn2+ (72%), MnCl+ (21%)

 

26

Fe

Fe(OH)2 +/Fe(OH)3 0, Fe(OH)4 -

pK3* = 6.60; pK4* = 8.5

27

Co

Co2+ (65%), CoCl+ (14%)

 

28

Ni

Ni2+ (53%), NiCl+ (9%)

 

29

Cu

Cu2+/CuOH+, Cu2+/CuCO3 0

pK1* = 8.11; pQ1 = 6.93

30

Zn

Zn2+ (64%), ZnCl+ (16%)

 

31

Ga

Ga(OH)2 +/Ga(OH)30/Ga(OH)4-

pK3* = 4.4; pK4* = 6.0

32

Ge

Ge(OH)4 0/GeO(OH)3 -/GeO2(OH)2 2-

pK1 = 8.98; pK2 = 11.8

33

As

H2AsO4 -/HAsO4 2-/AsO4 3-

pK2 = 6.15; pK3 = 9.84

  

As(OH)3/As(OH)4 -

pk* = 9.03

34

Se

SeO4 2- (100%)

 
  

H2SeO3/HSeO3 -/SeO3 2-

pK1 = 2.3; pK2 ≤ 7.8

35

Br

Br- (100%)

 

36

Kr

Kr

 

37

Rb

Rb+ (99%), RbSO4 - (1%)

 

38

Sr

Sr2+ (86%), SrSO4 0 (14%)

 

39

Y

Y3+/YCO3 +/Y(CO3)2 -

pQ1 = 6.63; pQ2 = 7.89

40

Zr

Zr(OH)3 +/Zr(OH)4 0/Zr(OH)5 -

pK4* = 4.6; pK5* = 5.99

41

Nb

Nb(OH)4 +/Nb(OH)5 0/Nb(OH)6 -

pK5* -0.6; pK6* = 7.4

42

Mo

HMoO4 -/MoO4 2-

pK 3.5

43

Tc

TcO4 - (100%)

 

44

Ru

Ru(OH) n 4-n

pK n (?)

45

Rh

RhCl a (OH) b 3-(a+b)

pK n (?)

46

Pd

PdCl4 2-/PdCl3OH2-

pK* = 8.7

47

Ag

AgCl3 2- (66%), AgCl2 - (26%)

 

48

Cd

CdCl+ (36%), CdCl2 0 (45%), CdCl3 - (16%)

 

49

In

In(OH)2 +/In(OH)3 0/In(OH)4 -

pK3* = 4.58; pK4* = 9.37

50

Sn

Sn(OH)3 +/Sn(OH)4 0

pK* 1.2

51

Sb

Sb(OH)5 0/Sb(OH)6 -

pK* = 2.5

52

Te

Te(OH)6 0/TeO(OH)5 -/TeO2(OH)4 2-

pK1 = 7.35; pK2 10.2

  

Te(OH)4 0/TeO(OH)3 -/TeO2(OH)2 2-

pK1 3.5; pK2 = 8.85

53

I

IO3 - (89%); I- (100%)

 

54

Xe

Xe

 

55

Cs

Cs+ (99%)

 

56

Ba

Ba2+ (86%), BaSO4 (14%)

 

57

La

La3+/LaCO3 +/La(CO3)2 -

pQ1 = 7.38; pQ2 = 8.47

58

Ce

Ce3+/CeCO3 +/Cd(CO3)2 -

pQ1 = 7.05; pQ2 = 8.34

59

Pr

Pr3+/PrCO3 +/Pr(CO3)2 -

pQ1 = 6.88; pQ2 = 8.20

60

Nd

Nd3+/NdCO3 +/Nd(CO3)2 -

pQ1 = 6.83; pQ2 = 8.15

61

Pm

Pm3+/PmCO3 +/Pm(CO3)2 -

--

62

Sm

Sm3+/SmCO3 +/Sm(CO3)2 -

pQ1 = 6.65; pQ2 = 7.97

63

Eu

Eu3+/EuCO3 +/Eu(CO3)2 -

pQ1 = 6.63; pQ2 = 7.89

64

Gd

Gd3+/GdCO3 +/Gd(CO3)2 -

pQ1 = 6.72; pQ2 = 7.95

65

Tb

Tb3+/TbCO3 +/Tb(CO3)2 -

pQ1 = 6.65; pQ2 = 7.72

66

Dy

Dy3+/DyCO3 +/Dy(CO3)2 -

pQ1 = 6.55; pQ2 = 7.69

67

Ho

Ho3+/HoCO3 +/Ho(CO3)2 -

pQ1 = 6.56; pQ2 = 7.59

68

Er

Er3+/ErCO3 +/Er(CO3)2 -

pQ1 = 6.50; pQ2 = 7.53

69

Tm

Tm3+/TmCO3 +/Tm(CO3)2 -

pQ1 = 6.43; pQ2 = 7.45

70

Yb

Yb3+/YbCO3 +Yb(CO3)2 -

pQ1 = 6.30; pQ2 = 7.55

71

Lu

Lu3+/LuCO3 +/Lu(CO3)2 -

pQ1 = 6.36; pQ2 = 7.42

72

Hf

Hf(OH)3 +/Hf(OH)4 0/Hf(OH)5 -

pK4* = 4.7; pK5* = 6.19

73

Ta

Ta(OH)4 +/Ta(OH)5 0/Ta(OH)6 -

pK5* -1; pK6* = 9.6

74

W

HWO4 -/WO4 2-

pK ≤ 3.5

75

Re

ReO4 - (100%)

 

76

Os

OsO4 0 (?)

 

77

Ir

IrCl a (OH) b 3-(a+b)

pK(?)

78

Pt

PtCl4 2-/PtCl3OH2-

pK* 8.7

79

Au

AuCl2 -

 
  

AuCl3(OH)-/AuCl2(OH)2 -/AuCl(OH)3 -

pK22* = 6.4; pK13* = 7.4(?)

80

Hg

HgCl4 2- (88%), HgCl3 - (12%)

 

81

Tl

Tl+ (61%), T1C10 37%

 
  

T1C14 -/T1(OH)3 0

pK 7.1 (?)

82

Pb

PbCl n 2-n/PbCO3 0

pQ = 7.85

83

Bi

Bi(OH)2 +/Bi(OH)3 0/Bi(OH)4 -

pK3* = 4.86; pK4* 12.7

log([CuOH+]/[Cu2+])= -8.11+pH

and

log([CuCO30]/[Cu2+]) = -6.93 + pH

As such, it is immediately seen that Cu2+ is a minor species relative to CuCO30 in seawater(e.g. [CuCO30]/[Cu2+] 18.6 at pH 8.2) and that the CuCO30/CuOH+ concentration ratio is approximately 15 (log 15 1.18 = 8.11 - 6.93), independent of pH.

Discussion

Table 1 indicates that the elements in group 1 (H, Li, Na, K, Cs, Rb) exist prominently as free hydrated cations. About 1% or less of each metal is ion paired with sulfate ([MSO4-]/[M+] ~0.01). Hydrogen ions are an exception to this generalization. The HSO4-/H+ concentration ratio in seawater is approximately 0.3.

Group 2 elements (Be, Mg, Ca, Sr, Be) are more strongly ion paired with SO42- than most of the group 1 ions. Mg2+ is approximately 10% ion paired with SO42- and the extent of SO42- ion pairing increases somewhat for the heavier members of the group. Be2+ is the only member of group 2 with an ionic radius sufficiently small to induce extensive hydrolysis. The pK* values listed for Be in Table 1 indicate that BeOH+ is the dominant form of beryllium except at high pH. With a normal seawater pH range between approximately 7.4 and 8.35 (on the free hydrogen ion concentration scale) the Be(OH)+/Be2+concentration ratio is never smaller than fifty.

The pK* and pQ compilations in Table 1 demonstrate that all group 3 elements (Sc, Y and La through Lu) are strongly complexed in seawater. Sc is the only group 3 metal that is strongly hydrolyzed. At pH 8.0 (i.e., 1.6 pH units above the Sc pK3* and 1.6 units below pK4*) the dominant form of ScIII is Sc(OH)30 and the Sc(OH)30/Sc(OH)2+ and Sc(OH)30/Sc(OH)4-concentration ratios are both equal to approximately 40. Yttrium and the rare earth elements (Y and La-Lu) are dominantly complexed by carbonate. The pQ n values for these elements shown in Table 1, calculated using the results of Liu and Byrne, [15] indicate that MCO3+ is generally the dominant form for the lighter elements while M(CO3)2- is dominant for the heavier elements. LaCO3+ is the dominant form of La even at the highest pH of seawater (pH 8.35, pQ2 = 8.47) and Lu(CO3)2- is the dominant form of Lu if pH > pQ2 = 7.42.

Group 4 elements (Ti, Zr, Hf) are all strongly hydrolyzed. Ti(OH)40 is the dominant form of Ti over a wide range of pH (pH > 2.5). The speciation characteristics of Zr and Hf are very similar. Zr(OH)5- is the dominant form of ZrIV above pH5.99 and Hf(OH)5- is the dominant form of HfIV above pH 6.19. Thus, for both ZrIV and HfIV the uncharged species, M(OH)40 is a significant but minor species. At the lowest pH of seawater the Zr(OH)40/Zr(OH)5- and Hf(OH)40/Hf(OH)5-concentration ratios are approximately 0.04 and 0.06 respectively.

Group 5 elements (V, Nb, Ta) are strongly hydrolyzed. With the smallest ionic radius of these three elements, VV is very strongly hydrolyzed. VO3(OH)2- is the dominant form of VV above pH 7.4. Since the pK3 value for VO3(OH)2-/VO43- is nearly two units higher than that for HPO42-/PO43- at zero ionic strength, only VO2(OH)2- and VO3(OH)2- appear to be relatively abundant within the normal pH range of seawater. Nb(OH)6- is the dominant form of NbV above pH 7.4, and since the Nb(OH)4+/Nb(OH)50 concentration ratio in seawater is smaller than 10-8 only Nb(OH)50 and Nb(OH)6- are significant species in seawater. Ta(OH)50 is the dominant form of TaV in seawater. The Ta(OH)6-/Ta(OH)50 concentration ratio is only on the order of 0.06 at the highest pH of seawater and, as is the case for Nb, cationic species are unimportant (Ta(OH)4+/Ta(OH)50 < 10-8). Thus, dominant forms for the group 5 elements are VO3(OH)2-, Nb(OH)6- and Ta(OH)50.

Group 6 elements (Cr, Mo, W) are all strongly hydrolyzed. Mo and W exist solely in the VI state, while Cr is found in seawater with oxidation numbers VI and III. Mo and W have dominant species transitions near pH 3.5 (pK2 = 3.5), while the HCrO4-/CrCO42- transition for CrVI occurs near pH 5.7. As such, in the VI state, all three elements dominantly exist as MO42- and ion pairs with Mg2+, Ca2+, etc. CrIII is strongly hydrolyzed and, with a pK3* value near 8.3, Cr(OH)2+ is more abundant than Cr(OH)30 except at high pH.

Group 7 elements (Mn, Tc, Re) have dissimilar group chemistries due to differences in favored oxidation numbers. TcVII and ReVII exist in solution solely as TcO4- and ReO4-and should be exceptionally unreactive. Mn has two favored oxidation states with highly dissimilar characteristics. MnII exists in seawater dominantly as free hydrated ions (Mn2+) and ion pairs with Cl-. In the IV oxidation state Mn, as MnO2(s), is highly insoluble. Thus, oxidation state transformations strongly influence Mn behavior in seawater.

Elements in group 8 (Fe, Ru, Os) have diverse and generally poorly understood seawater chemistries. Fe exists in seawater dominantly as FeIII and, to a lesser extent, as FeII. Iron in the II oxidation number has a solution chemistry very similar to those of other MII ions in period 4. MnII, FeII, CoII, NiII, and ZnII are all weakly ion paired with Cl~and are present in seawater dominantly as free hydrated ions. As FeIII, iron is strongly hydrolyzed. Table 1 indicates that the dominant form of FeIII throughout the normal pH range of seawater is Fe(OH)30. This conclusion is somewhat controversial because (a) iron biogeochemistry is important and intensively investigated, and (b) only one somewhat problematic analytical procedure (solubility analysis) has been extensively used to investigate the Fe(OH)2+/Fe(OH)30 and Fe(OH)30/Fe(OH)4- transitions. The characteristics of Ru and Os speciation in seawater are very poorly understood. It is probable that both elements are very strongly hydrolyzed. Based on available data, Principal Species for Ru and Os are tentatively assigned as Ru(OH) n 4-nand OsO4 0.

Elements in group 9 (Co, Rh, Ir) have generally complex chemistries and are, perhaps, only slightly better understood than the group 8 elements. The dominant oxidation number for Co in seawater is II. CoII exists predominantly as Co2+ and ion pairs with Cl-. RhIII is strongly complexed by chloride and is also strongly hydrolyzed. Investigations in 0.5 M NaCl (Miller and Byrne, in progress) indicate that RhIII forms a complex array of mixed ligand complexes (RhCl a (OH) b 3-(a+b)). These investigations are challenging due to slow ligand exchange kinetics. IrIII forms strong chloride complexes and, as in the case of RhIII, has slow ligand exchange rates. In analogy with RhIII the Principal Species of IrIII are tentatively assigned as IrCl a (OH) b 3-(a+b)) Both Rh and Ir occur in the IV oxidation state but the solution chemistries of RhIV and IrIV are very poorly understood.

Group 10 elements (Ni, Pd, Pt) principally occur with oxidation number II. Ni in seawater dominantly exists as free hydrated Ni2+. The chemistries of PdII and PtII are similar and contrast sharply with the speciation of NiII. Pd and Pt exist dominantly as PdCl42- and PtCl42- in seawater [16] but are, nonetheless, significantly hydrolyzed as PdCl3OH2- and PtCl3OH2- at high pH. The potential importance of PtIVspecies in seawater is poorly understood.

The solution chemistries of group 11 elements (Cu, Ag, Au) in oxidation state I are similar. CuI, AgI and AuI are strongly complexed with Cl- and hydrolysis is insignificant. While Ag solely exists as AgI, Cu occurs dominantly as CuII in oxygenated seawater and oxidation number III may be important for Au. CuII chemistry is dominated by carbonate complexation, while AuIII speciation in seawater appears (tentatively) to be dominated by mixed-ligand chlorohydroxy complexes.

The speciation of group 12 metals (Zn, Cd, Hg), all in the II oxidation state, involves a progression from very weak to very strong complexation. ZnII occurs in seawater principally as Zn2+ and ZnCl+, CdII is moderately complexed (CdCl+, CdCl20 and CdCl3-) and HgII is complexed very strongly as HgCl42- and HgCl3-.

Group 13 elements (B, Al, Ga, In, Tl) in oxidation state III are very strongly hydrolyzed. The Principal Species of these elements are B(OH)30, A1(OH)4-, Ga(OH)4-, In(OH)30 and, tentatively, T1(OH)30. The speciation of each of these elements is significantly pH dependent. For B, Al, Ga and In, each metal is partitioned between uncharged and anionic forms. In contrast, TlIII appears to be partitioned between T1(OH)30 and either T1C14- or mixed chlorohydroxy species. Tl is unique among the group 13 metals in having a significant, and perhaps dominant, I oxidation state. In this form TlI occurs principally as the free hydrated Tl+ ion.

Group 14 elements (C, Si, Ge, Sn, Pb) have diverse speciation characteristics. C is partitioned dominantly between CO32- and HCO3-, while for both Si and Ge, uncharged forms are dominant (Si(OH)40 and Ge(OH)40) with lesser concentrations (≤ 15%) of SiO(OH)3- and GeO(OH)3-. The sparse data available for assessment of SnIV speciation indicate that Sn(OH)40 is dominant over a wide range of pH. The speciation of Pb is apparently unique among seawater constituents in that PbII is partitioned between chloride complexes and carbonate complexes. [17] The latter are dominant above pH 7.85.

Group 15 elements (N, P, As, Sb, Bi) in oxidation states V and III are strongly hydrolyzed in seawater, and oxidation number V is favored relative to III for all group 15 elements except Bi. Bi is present in seawater dominantly as Bi(OH)30. NVand NIII exist solely as unprotonated NO3- and NO2-. The NH4+/NH30 ratio in seawater is significantly pH dependent and is always larger than ~10. The dominant forms of PV and AsV in seawater are HPO42- and HAsO42-. While H2PO4-/HPO42- and H2AsO4-/HAsO42- ratios are similar in seawater, the PO43-/HPO42- ratio is substantially larger than that for AsO43-/HAsO42-. SbV in seawater is present dominantly as Sb(OH)6-. The speciation of SbIII is similar to that of BiIII in that Sb(OH)30 is dominant over a wide range of pH. The As(OH)30/As(OH)4- ratio in seawater is pH dependent and generally larger than six.

Group 16 elements include O, S, Se, Te and Po. O2- and OH- are found in association with elements in every group of the periodic table except 1, 2 and 18. Dissolved O2 is very important in seawater because of its strong influence on the oxidation/reduction behavior of solutions. The dominant form of OH- in seawater is MgOH+. S exists in oxygenated seawater as SO42- and ion pairs with group 1 and group 2 elements, and is not significantly protonated except at very low pH. Se exists in seawater as both SeVI and SeIV. In the higher oxidation state Se exists as SeO42- with protonation characteristics very similar to SO42- (pK ~1). As SeIV, selenium is partitioned between HSeO3- and SeO32- with the former dominant at low pH and the latter dominant at high seawater pH. Te also exists in seawater in the VI and IV oxidation states. In the case of TeVI, since pK 7.35 for the Te(OH)60/TeO(OH)5- transition, TeO(OH)5- is the predominant species. For TeIV, pK 8.85 for the TeO(OH)3-/TeO2(OH)22- partition and TeO(OH)3- is thereby predominant. Little is known about Po equilibria in solution.

The group 17 elements (F, Cl, Br, I and At) exist with -I and V oxidation numbers and the -I state is predominant for the lighter elements. F- occurs in seawater as an approximately equimolar mixture of F- and MgF+. Cl and Br occur dominantly as unassociated Cl- and Br-. The predominant oxidation number of I is V. IV occurs as IO3- and is, to a small extent, ion paired with Mg2+. I- is found in seawater at substantially lower concentrations than IO3-. Little is known about the solution chemistry of highly radioactive At.

Overview of speciation in seawater

The results shown in Table 1 indicate that only a relatively small number of elements have major species that do not involve hydrolyzed forms or carbonate complexation. Such elements typically have oxidation numbers I, II and -I and are found in groups 1, 2, 11, 12 and 17, and in period 4 (groups 7–10). Only eight to nine elements have speciation schemes that strongly involve chloride complexation. Such elements are found in groups 9 (RhIII and IrIII), 10 (PdII and PtII), 11 (CuI, AgI, AuI), 12 (CdII, HgII) and 14 (Pb11). However, of these elements both Rh and Ir are importantly influenced by hydrolysis, Pd11 and Pt11 are significantly influenced by hydrolysis, and Pb11 is strongly influenced by carbonate complexation. Of the very large number of hydrolyzed elemental forms in seawater, approximately 17 have speciation schemes that are strongly pH dependent. These elements include Be11, ScIII (groups 2 and 3), VV, NbV and TaV (group 5), CrIII (group 6), FeIII and RuIII (group 8), RhIII and IrIII (group 9), BIII, AlIII, In111, TlIII (group 13), CIV, SiIV and GeIV (group 14), PV and AsV (group 15), SeIV and TeIV (group 16). As such, no elements with oxidation numbers 1, 2 and 6 (other than Be11) have hydrolyzed forms whose relative concentrations are strongly pH dependent within the normal pH range of seawater. Approximately 17 elements with atomic numbers less than 92 (Cu, Pb, Y, and the lanthanides) have speciation schemes that strongly involve or are dominated by carbonate complexation. With the inclusion of UVI and the 9 actinides with oxidation number III (Am-Lr), it is seen that carbonate complexation is important for a large portion of the periodic table. Altogether, including elements strongly complexed by carbonate and seventeen or more elements with pH dependent, hydrolyzed major species, it is seen that the seawater speciation of more than forty elements is strongly influenced by pH.

Elements having exceptionally poorly understood speciation schemes in seawater include Ru and Os (group 8), Rh and Ir (group 9), Pt (group 10) and Au (group 11). Speciation of the latter four elements may be dominated by a complex array of chlorohydroxy complexes and, perhaps, a variety of types of halides. It should also be anticipated that, for metals forming strong covalently bonded species, complexation by ligands containing reduced sulfur may dramatically change future Principal Species assessments. This concern is particularly relevant to Rh, Ir, Pd, Pt, Au, Hg, and T1.

Appreciation of the role of carbonate in seawater complexation has grown steadily over the past forty years. Experimental difficulties have impeded the progress of investigations involving the complexation of strongly hydrolyzed metals by carbonate ions. Using new technologies, however, future improvements in carbonate complexation assessments are probable and the perceived role of carbonate in trace element complexation may significantly expand.

In view of the importance of pH dependent speciation schemes for a wide variety of elements in seawater, it is important to note that substantial uncertainties remain in the equilibrium characterizations presented in Table 1. In many cases, estimated speciation schemes must be based on data obtained using a single analytical technique. It is, furthermore, particularly problematic when speciation characterizations of strongly hydrolyzed metals at high pH are based solely on solubility analyses. Among other complicating factors, the experimental solutions used in solubility analyses generally have much higher metal concentrations than are observed in the open ocean. Consequently, solubility analyses are conducive to the formation of a more complex set of hydrolyzed species (e.g., polymers and colloids) than are generally found in the oceans. Deconvolution of the data generated in such analyses can be challenging.

Declarations

Acknowledgements

Thanks are given to Drs. Johan Schijf and Xuewu Liu for assistance in the preparation of this manuscript. The author also gratefully acknowledges the constructive criticism of two anonymous reviewers.

Authors’ Affiliations

(1)
College of Marine Science, University of South Florida

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© The Royal Society of Chemistry and the Division of Geochemistry of the American Chemical Society 2002