Interaction of B(OH)sup0/supsub3/sub and HCOsup-/supsub3/sub in Seawater: Formation of B(OH)sub2/subCOsup-/supsub3/sub

Sean McElligott; Robert H. Byrne

doi:10.1023/A:1009633804274

Interaction of B(OH)sup0/supsub3/sub and HCOsup-/supsub3/sub in Seawater: Formation of B(OH)sub2/subCOsup-/supsub3/sub

Sean McElligott, Robert H. Byrne

College of Marine Science

Research output: Contribution to journal › Article › peer-review

Abstract

Boron is known to interact with a wide variety of protonated ligands(HL) creating complexes of the form B(OH) 2 L - .Investigation of the interaction of boric acid and bicarbonate in aqueoussolution can be interpreted in terms of the equilibrium B(OH)30+HCO3−&rlhar;B(OH)2CO3−+H2O">B(OH)03+HCO−3&rlhar;B(OH)2CO−3+H2OB(OH)30+HCO3−&rlhar;B(OH)2CO3−+H2O The formation constant for this reaction at 25 °C and 0.7 molkg -1 ionic strength is KBC=[B(OH)2CO3−][B(OH)30]−1[HCO3−]−1=2.6±1.7">KBC=[B(OH)2CO−3][B(OH)03]−1[HCO−3]−1=2.6±1.7KBC=[B(OH)2CO3−][B(OH)30]−1[HCO3−]−1=2.6±1.7 where brackets represent the total concentration of each indicatedspecies. This formation constant indicates that theB(OH) 2 CO3−">CO−3CO3− concentration inseawater at 25 °C is on the order of 2 μmol kg -1 . Dueto the presence of B(OH) 2 CO3−">CO−3CO3− , theboric acid dissociation constant (K′B">K′BK′B ) in natural seawaterdiffers from K′B">K′BK′B determined in the absence of bicarbonate byapproximately 0.5%. Similarly, the dissociation constants of carbonicacid and bicarbonate in natural seawater differ from dissociation constantsdetermined in the absence of boric acid by about 0.1%. Thesedifferences, although small, are systematic and exert observable influenceson equilibrium predictions relating CO 2 fugacity, pH, totalcarbon and alkalinity in seawater.

Original language	American English
Journal	Aquatic Geochemistry
Volume	3
DOIs	https://doi.org/10.1023/A:1009633804274
State	Published - Jan 1 1997

Keywords

boron
boric acid
carbonate
CO2 system
complexation
spectrophotometric pH

Disciplines

Life Sciences

Access to Document

10.1023/A:1009633804274License: CC BY

https://doi.org/10.1023/A:1009633804274

Cite this

@article{6c8344ffd02a49258ba30cbb22c52653,

title = "Interaction of B(OH)sup0/supsub3/sub and HCOsup-/supsub3/sub in Seawater: Formation of B(OH)sub2/subCOsup-/supsub3/sub",

abstract = " Boron is known to interact with a wide variety of protonated ligands(HL) creating complexes of the form B(OH) 2 L - .Investigation of the interaction of boric acid and bicarbonate in aqueoussolution can be interpreted in terms of the equilibrium B(OH)30+HCO3−&rlhar;B(OH)2CO3−+H2O{"}>B(OH)03+HCO−3&rlhar;B(OH)2CO−3+H2OB(OH)30+HCO3−&rlhar;B(OH)2CO3−+H2O The formation constant for this reaction at 25 °C and 0.7 molkg -1 ionic strength is KBC=[B(OH)2CO3−][B(OH)30]−1[HCO3−]−1=2.6±1.7{"}>KBC=[B(OH)2CO−3][B(OH)03]−1[HCO−3]−1=2.6±1.7KBC=[B(OH)2CO3−][B(OH)30]−1[HCO3−]−1=2.6±1.7 where brackets represent the total concentration of each indicatedspecies. This formation constant indicates that theB(OH) 2 CO3−{"}>CO−3CO3− concentration inseawater at 25 °C is on the order of 2 μmol kg -1 . Dueto the presence of B(OH) 2 CO3−{"}>CO−3CO3− , theboric acid dissociation constant (K′B{"}>K′BK′B ) in natural seawaterdiffers from K′B{"}>K′BK′B determined in the absence of bicarbonate byapproximately 0.5%. Similarly, the dissociation constants of carbonicacid and bicarbonate in natural seawater differ from dissociation constantsdetermined in the absence of boric acid by about 0.1%. Thesedifferences, although small, are systematic and exert observable influenceson equilibrium predictions relating CO 2 fugacity, pH, totalcarbon and alkalinity in seawater.",

keywords = "boron, boric acid, carbonate, CO2 system, complexation, spectrophotometric pH",

author = "Sean McElligott and Byrne, {Robert H.}",

year = "1997",

month = jan,

day = "1",

doi = "10.1023/A:1009633804274",

language = "American English",

volume = "3",

journal = "Aquatic Geochemistry",

}

TY - JOUR

T1 - Interaction of B(OH)sup0/supsub3/sub and HCOsup-/supsub3/sub in Seawater: Formation of B(OH)sub2/subCOsup-/supsub3/sub

AU - McElligott, Sean

AU - Byrne, Robert H.

PY - 1997/1/1

Y1 - 1997/1/1

N2 - Boron is known to interact with a wide variety of protonated ligands(HL) creating complexes of the form B(OH) 2 L - .Investigation of the interaction of boric acid and bicarbonate in aqueoussolution can be interpreted in terms of the equilibrium B(OH)30+HCO3−&rlhar;B(OH)2CO3−+H2O">B(OH)03+HCO−3&rlhar;B(OH)2CO−3+H2OB(OH)30+HCO3−&rlhar;B(OH)2CO3−+H2O The formation constant for this reaction at 25 °C and 0.7 molkg -1 ionic strength is KBC=[B(OH)2CO3−][B(OH)30]−1[HCO3−]−1=2.6±1.7">KBC=[B(OH)2CO−3][B(OH)03]−1[HCO−3]−1=2.6±1.7KBC=[B(OH)2CO3−][B(OH)30]−1[HCO3−]−1=2.6±1.7 where brackets represent the total concentration of each indicatedspecies. This formation constant indicates that theB(OH) 2 CO3−">CO−3CO3− concentration inseawater at 25 °C is on the order of 2 μmol kg -1 . Dueto the presence of B(OH) 2 CO3−">CO−3CO3− , theboric acid dissociation constant (K′B">K′BK′B ) in natural seawaterdiffers from K′B">K′BK′B determined in the absence of bicarbonate byapproximately 0.5%. Similarly, the dissociation constants of carbonicacid and bicarbonate in natural seawater differ from dissociation constantsdetermined in the absence of boric acid by about 0.1%. Thesedifferences, although small, are systematic and exert observable influenceson equilibrium predictions relating CO 2 fugacity, pH, totalcarbon and alkalinity in seawater.

AB - Boron is known to interact with a wide variety of protonated ligands(HL) creating complexes of the form B(OH) 2 L - .Investigation of the interaction of boric acid and bicarbonate in aqueoussolution can be interpreted in terms of the equilibrium B(OH)30+HCO3−&rlhar;B(OH)2CO3−+H2O">B(OH)03+HCO−3&rlhar;B(OH)2CO−3+H2OB(OH)30+HCO3−&rlhar;B(OH)2CO3−+H2O The formation constant for this reaction at 25 °C and 0.7 molkg -1 ionic strength is KBC=[B(OH)2CO3−][B(OH)30]−1[HCO3−]−1=2.6±1.7">KBC=[B(OH)2CO−3][B(OH)03]−1[HCO−3]−1=2.6±1.7KBC=[B(OH)2CO3−][B(OH)30]−1[HCO3−]−1=2.6±1.7 where brackets represent the total concentration of each indicatedspecies. This formation constant indicates that theB(OH) 2 CO3−">CO−3CO3− concentration inseawater at 25 °C is on the order of 2 μmol kg -1 . Dueto the presence of B(OH) 2 CO3−">CO−3CO3− , theboric acid dissociation constant (K′B">K′BK′B ) in natural seawaterdiffers from K′B">K′BK′B determined in the absence of bicarbonate byapproximately 0.5%. Similarly, the dissociation constants of carbonicacid and bicarbonate in natural seawater differ from dissociation constantsdetermined in the absence of boric acid by about 0.1%. Thesedifferences, although small, are systematic and exert observable influenceson equilibrium predictions relating CO 2 fugacity, pH, totalcarbon and alkalinity in seawater.

KW - boron

KW - boric acid

KW - carbonate

KW - CO2 system

KW - complexation

KW - spectrophotometric pH

UR - https://digitalcommons.usf.edu/msc_facpub/1620

UR - https://doi.org/10.1023/A:1009633804274

U2 - 10.1023/A:1009633804274

DO - 10.1023/A:1009633804274

M3 - Article

VL - 3

JO - Aquatic Geochemistry

JF - Aquatic Geochemistry

ER -

Interaction of B(OH)sup0/supsub3/sub and HCOsup-/supsub3/sub in Seawater: Formation of B(OH)sub2/subCOsup-/supsub3/sub

Abstract

Keywords

Disciplines

Access to Document

Other files and links

Cite this