1 / 28

Trace Metal Biogeochemistry (Marine Bioinorganic Chemistry) 12.755 Lecture 2

Trace Metal Biogeochemistry (Marine Bioinorganic Chemistry) 12.755 Lecture 2. Last week: Four types of trace metal profiles Geochemical properties that cause these profiles shapes: solubility, inorganic speciation, organic speciation, and redox. Began Speciation lecture with

talasi
Télécharger la présentation

Trace Metal Biogeochemistry (Marine Bioinorganic Chemistry) 12.755 Lecture 2

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. Trace Metal Biogeochemistry(Marine Bioinorganic Chemistry) 12.755 Lecture 2 Last week: Four types of trace metal profiles Geochemical properties that cause these profiles shapes: solubility, inorganic speciation, organic speciation, and redox. Began Speciation lecture with Definitions of ligands, chelates Stability constants, solubility products, Hard vs soft ions, Irving Williams series, Non-ideal effects/Debye Huckel/Davies corrections, Hydration energies of different transition metals Today: Metal Speciation continued The Conditional Stability constant Setting up equations for inorganic species Setting up equations for organic species Literature: speciation of metals in seawater overview Introduction to Minqel+ (if time) Brief Discussion of readings

  2. Why are we talking about complexation chemistry? • How do metals influence the biota (and carbon cycling) of seawater? • To answer the question we have to understand: - Natural organic-metal complexes: FeL, CoL, NiL, CuL, ZnL, CdL • What are the geochemical roles of these ligands? 1. Controls on “bioavailability” - high affinity uptake systems - ecological warfare between species 2. Protection from scavenging processes 3. Increases in solubility • How do you study something at picomolar quantities which we don’t know much about?

  3. Chelators are everywhere

  4. FROM LAST WEEK: Background Aquatic Chemistry of Trace Elements:A marine water column context Solubility Products: Example for Fe(OH)3(s) Ksp= [Fe][OH]3= 1042.7 Stability constants for metal complexes (where L is ligand, M is Metal): K = [ML]/[M][L] Ligands can include inorganic chemical species: In oxic systems: OH-, CO32-,SO42-, Cl-, PO43-, In anoxic systems add: HS-,, S2- Ligands can also include organic chemical species: EDTA, DTPA, NTA, Citrate, Tris, siderophores, cobalophores, DFB, TETA, and the famous unknown ligand(s) “L”

  5. FROM LAST WEEK: Definitions • Ligand – an atom, ion, or molecule that donates/shares electrons with one or more central atoms or ions. • Chelate – (from Greek chelos = crab, with two binding claws) two or more donor atoms from a single ligand to the central metal atom

  6. Conditional stability constants: specific to “conditions” Thermodynamic constant based on activities Activity corrected, Now based on concentrations L- can interact with other ions: Na+ K+ Ca2+ Mg2+ But we may not know anything about their equilbrium constants L- will have acid base chemistry In seawater where there are many salts: Kcond = Kapp If acid-base chemistry dominates: Kcond = Keff

  7. We’ve already talked about the effects of saltsAcid base chemistry also matters for complexation chemistry in seawater: We just usually don’t know enough to correctly parameterize it experimental Protonation constants of EDTA matter Co2+ + 2HDMG  CoHDMG2 Co2+ + EDTA4-CoEDTA2- modeling

  8. Which brings us to:How do we measure metal speciation? • Use ligand exchange reactions: Natural Ligands: CoL Co2+ + L2- Our “Probe” Ligand Co2+ + 2HDMG  CoHDMG2 Net reaction: CoL + 2HDMG  CoHDMG2 + L2- Core Idea: There are reactions compounds we can measure extremely sensitively in seawater using electrochemistry They are Electroactive like CoHDMG2 There are many electroactive ligands (synthetic): Fe: 1N,2N; TAC, Cu: Bzac Zn: APDC

  9. Ligand Exchange M + L1  ML1 M + L2  ML2 ML1 + L2  ML2 +L1

  10. Ligand Exchange M + L1  ML1 M + L2  ML2 ML1 + L2  ML2 +L1 There are kinetic considerations to this: If in seawater and either L1 or L2 has a high affinity for Ca or Mg, it will clog up the exchange reactions Disjunctive Adjunctive ML  M + L M* + ML  M*LM M* + L  M*L M*LM  M*L + M If M = Ca and M* = a trace metal the concentration gradient is many orders of magnitude!

  11. Trace Metal Speciation Calculations: • Inorganic speciation Terminology: • M’ or METAL-“PRIME” = summation of inorganic species • Organic speciation • L for unknown organic ligand (variants L1 and L2), metal-specific (?) • EDTA as a “model” ligand Ethylene diaminetetraacetic acid

  12. The calculation of equilibrium between multiple chemical speciesStart with a simple system 3 species: M2+, MA, MB2 M + A  MA K =[MA] / [M][A] MA = K[M][A] M + 2B  MB2 K = [MB2] / [M][B]2 MB2 = K[M][B]2 Total M = M2++ MA + MB Total M = M2+(1 + K[A] + K[B]2) M2+/Total M = 1 / (1 + K[A] + K[B]2) MA/Total M = K[A] / (1 + K[A] + K[B]2)

  13. Species dependent on pH: [CoOH-] / [Co2+][OH-] = 104.3 [H+][OH-] = 10-14 At pH 8.0: [OH-] = 10-14 / 10-8 = 10-6 [CoOH-] = 104.3[Co2+]10-6 = 10-1.7 [Co2+] Also carbonate species, H2CO3, HCO3-, CO32- are pH dependent and can be ligands. Acidity constants: Ka1=6.3, Ka2=10.3 [CO32-] = [CO32-]Total / ( 1 + 1010.3[H+]+1016.6[H+]2) We typically do not assume redox equilibrium in chemical speciation reactions – instead we investigate/calculate only one redox state (Fe III)

  14. FROM LAST WEEK: From Morel and Hering, 1993

  15. FROM LAST WEEK: Background Aquatic Chemistry of Trace Elements:A marine water column context However, there can be Non-Ideal effects: • The effects of other solutes on the free energy of ion(s) of interest • Solubility product and stability constants need to be corrected, or better, determined to/at the appropriate ionic strength. • The activity of the metal is: {Mn+} = [Mn+]gMn+ • The activity coefficient, gMn+, can be estimated by the Debye-Huckel correction or the Davies expression (modified Debye-Huckel) • Thermodynamic databases (Martell and Smith) will provide the ionic strength experimental conditions for each constant (e.g. 0.1M)

  16. Calculations of organic speciation in seawater

  17. From Bruland 1988

  18. Note of caution: • Tables in Morel and Hering and Stumm and Morgan are made for teaching • They have been back corrected to zero ionic strength from constants • If your application really matters, go to the literature or NIST databases for each constant • You can use the textbooks as guidelines of species to look for though

  19. History of Metal Speciation in Seawater(Brief and Incomplete) • Cu - Sunda 1983, Coale and Bruland 1988, Moffett et al., 1990 • Zn - Bruland, 1988 • Cd - Bruland, 1988 • Fe – Gledhill and van den Berg 1994 • Rue and Bruland 1995, Wu and Luther 1995, van den Berg 1995 • Co – Saito and Moffett 2001, Ellwood and van den Berg 2001 • Ni and Cr – Achterburg and van den Berg, 1997 • Hg – Lamborg et al., 2004

  20. Morel, Allen, Saito, Treatise on Geochemisrty 2003

More Related