Solute transport
1 / 73

Solute Transport - PowerPoint PPT Presentation

  • Uploaded on

Solute Transport. Ions and molecules being transported in the subsurface often travel at rates slower than water The migration is “retarded” primarily due to their interactions with mineral surfaces Surface complexation reactions. Surface Complexation Reactions.

I am the owner, or an agent authorized to act on behalf of the owner, of the copyrighted work described.
Download Presentation

PowerPoint Slideshow about ' Solute Transport' - lenora

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.While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server.

- - - - - - - - - - - - - - - - - - - - - - - - - - E N D - - - - - - - - - - - - - - - - - - - - - - - - - -
Presentation Transcript
Solute transport
Solute Transport

  • Ions and molecules being transported in the subsurface often travel at rates slower than water

  • The migration is “retarded” primarily due to their interactions with mineral surfaces

  • Surface complexationreactions

Surface complexation reactions
Surface Complexation Reactions

  • Reactions occurring at the mineral-water interface (mineral surface)

  • Important for:

    • Transport and transformation of metals and organic contaminants

    • Nutrient availability in soils

    • Formation of ore deposits

    • Acidification of watersheds

    • Global cycling of elements

Surface charge
Surface Charge

  • Solids typically have an electrically charged surface

  • There are 2 main sources of surface charge

  • (1) Chemical reactions

    • pH dependent: surfaces tend to have positive charges at low pH, negative charges at high pH

    • For most common solid phases at natural pHs, the surface charge is negative

  • (2) Lattice imperfections and substitutions in the solid

Surface charge1
Surface Charge

  • Clays: substitution or vacancy result in negative charge, which is the dominant charge

  • Al/Fe hydroxides adsorb both cations and anions depending on pH: Amphoteric

    • Low pH: positive surface charge

    • High pH: negative surface charge

  • Organic compounds can also have pH dependent charge

    • DOM can be important in transport of low solubility metals

Surface charge2
Surface Charge

  • The interfacial system (surface – water) must be electrically neutral

  • Electrical Double Layer

    • Fixed surface charge on the solid

    • Charge distributed diffusely in solution

      • Excess of counterions (opposite charge to surface) and deficiency of ions of same charge as surface

      • Counterions attracted to the surface


  • Adsorption refers to a dissolved ion or molecule binding to a charged surface

  • All ions (including H+ and OH-) are continually competing for sites

  • Reversible reactions; i.e., if conditions change, the ion can desorb

  • Kinetically fast reactions; equilibrium often assumed



Fixed Surface


Ion exchange
Ion Exchange

  • Ion exchange refers to exchange of ions between solution and solid surfaces

  • It differs from adsorption in that an ion is released from the surface as another is adsorbed

    • AX + B+ BX + A+

    • X refers to a mineral surface to which an ion has adsorbed

    • Most important for cations, anions less so, because most mineral surfaces are negatively charged

  • Primarily occurs on clay minerals of colloidal size (10-3 – 10-6 mm)

Ion exchange1
Ion Exchange

  • Ion size (radius) and charge affect how they exchange

    • Smaller ions from stronger bonds on surfaces

    • Ions with more positive charge form stronger bonds on surfaces

    • Stronger to weaker, increasing ionic radii:

      • Al3+ > Ca2+ > Mg2+ > K+ = NH4+ > Na+

  • Reversible reactions

Cation exchange capacity cec
Cation Exchange Capacity (CEC)

  • CEC is the capacity of a mineral to exchange one cation for another

    • Depends on charge imbalances in the crystal lattice

  • Amount of exchange sites per mass of solid (meq/100 g)

    • Measured in lab by uptake and release of NH4+ acetate

    • Not a precise measurement: pH dependent, organic coatings

    • Primarily applicable to clays

Ion exchange equilibrium
Ion Exchange Equilibrium

  • Mass action equation:

    • B-clay + A+ ↔ A-clay + B+

      • Where A+ and B+ are monovalentcations

      • aA-clay and aB-clay = activities of A and B on exchange sites

      • aA+ and aB+ = activities in solution

      • KAB = exchange constant

Ion exchange equilibrium1
Ion Exchange Equilibrium

  • Mass action equation can be rewritten using mole fractions in the solid phase

    • XA-clay and XB-clay = mole fractions of A and B on clay

      • XA-clay + XB-clay = 1

    • K’AB = selectivity coefficient

    • K’AB is not a constant because activity coefficients in the solid dependent on composition

Ion exchange equilibrium2
Ion Exchange Equilibrium

  • Example: Mix 10 g of a Na-saturated smectite with CEC = 100 meq/100 g with 1 liter of water containing 20 mg/L Na+ and 20 mg/L K+ as the only cations. Assume KK+-Na+ = 2.

  • What will the final Na+ and K+ concentrations be?

Ion exchange equilibrium3
Ion Exchange Equilibrium

  • Exchange between monovalent and divalent cation:

    • 2 A-clay + C2+ ↔ C-clay + 2A+

Ion exchange equilibrium4
Ion Exchange Equilibrium

  • Example: Suppose a solution in contact with a clay is at equilibrium and has a Ca2+ concentration = 35 mg/L and Na+ = 10 mg/L. Assume KCa2+-Na+ = 2.

  • What are the mole fractions (XCa2+ and XNa+) in the solid phase?

Monovalent divalent effect
Monovalent-divalent effect

  • In fresh (dilute) waters, the dominant exchangeable cation is Ca2+

  • In the ocean, the dominant exchangeable cation is Na+

Cation exchange capacity and groundwater composition
Cation Exchange Capacity and Groundwater Composition

  • Ion exchange reacts important control on groundwater chemistry

  • Typically CEC value in aquifer of 5 meq/100 g gives an exchange capacity of ~500 meq/L

    • Much larger than concentration of dissolved cations in dilute groundwater

Clay mineralogy
Clay Mineralogy

  • Clays are fine-grained, crystalline, hydrous silicates with sheet structures

    • Phyllosilicates

  • Most common type of secondary mineral

  • Have surface charge, usually negative

    • Charge attracts cations to surface where they are bound by electrostatic forces

    • Not part of crystal structure so they can easily exchange with other ions in solution

Clay structure
Clay structure

  • Clays have 2 distinct sheet structures

    • Tetrahedral: 3-sided pyramid, 4 oxygen (O2-) atoms (or OH-) surrounding a silicon atom (Si4+)

      • Al3+ can substitute for Si4+, resulting in negative charge

Clay structure1
Clay structure

  • Octahedral: two 3-sided pyramids joined at the base

    • Surface charge results from substitution or vacancy in central cation (usually Al, Mg, Fe)

Clay structures
Clay Structures

  • The tetrahedrons and octahedrons are joined to each other in sheets

  • The sheets join in 2 main patterns to create different clays: 2-layer and 3-layer

Types of clays
Types of clays

  • 2-layer phyllosilicates

    • Alternating tetrahedral and octahedral layers (T:O or 1:1)

    • Each T and O sheet are strongly bound, while T:O’s are held together by weak van der Waal’s forces

    • Kaolinte (Al2Si2O5(OH)4) and serpentite (Mg3Si2O5(OH)4) groups

    • Relatively pure clays, close to stoichiometric

    • Low substitution results in low surface charge, no interlayer adsorption sites

    • Low CEC (kaolinite: 3-5 meq/100 g)

Types of clays1
Types of clays

  • 3-layer phyllosilicates

    • Each layer consists of 2 tetrahedrons and one octahedron (T:O:T or 2:1)

    • Interlayers can be adsorption sites

    • Smectite, vermiculite, and mica groups

3 layer phyllosilicates
3-Layer Phyllosilicates

  • Smectites

    • Wide interlayer spacing, easily exchange ions/ H2O

    • High substitution/vacancy, high CEC

      • CEC: 70-150 meq/100 g

    • Shrink/swell: as moisture content increases, more water in interlayer expands; vice versa as water content decreases

      • Due to type of cation

        • Ca2+ Na+ exchange

        • 2 ions for 1, increases interlayer thickness

      • Road salt can cause expansion of smectities next to roads due to increased Na+, resulting in engineering problems

      • Solution: add lime or CaCO3 to exchange Ca2+ for Na+

3 layer phyllosilicates1
3-Layer Phyllosilicates

  • Vermiculite

    • Stronger interlayer cation bonding, slower cation exchange, higher surface charge

    • High CEC

3 layer phyllosilicates2
3-Layer Phyllosilicates

  • Illite: most common in nature, makes up most ancient shales

    • 80% mica, 20% smectite

    • Low surface charge and CEC

3 layer phyllosilicates3
3-Layer Phyllosilicates

  • Mica

    • Muscovite and biotite primary minerals with little substitution or vacancy, little surface charge

    • Similar structure to illite

Double layer theory
Double Layer Theory

  • Describes the distribution of charge near a charge surface and how charge is neutralized

    • Stern layer: closest to surface where cations bonded by weak electrostatic forces (van der Waals)

      • Cations can exchange relatively rapidly and easily

    • Gouy layer: further from surface, thickness related to ionic strength of solution

      • High I, thin Gouy layer; more ions can neutralize charge over shorter distance

      • Low I, thick Gouy layer

    • Adsorption can occur in both layers

Double layer theory1
Double Layer Theory

Net positive charge

in Gouy layer

Double layer theory2
Double Layer Theory

  • The likelihood of attachment of a charged species approaches a surface is controlled by the sum of attractive and repulsive forces

    • Attractive: van der Waals between species of opposite charge

    • Repulsive: net positive charge in Gouy layer repels incoming cations

    • Sum of these 2 is the energy barrier (or lack thereof) needed to be overcome before a species can adsorb at the surface (Stern layer)

Double layer theory3
Double Layer Theory

  • Attachment also dependent of charge density of an ion and ionic strength

    • As charge density increases, attraction increases

    • As I decreases, Gouy layer thickness increases, repulsion moves further away from surface where attraction is weaker

  • Adsorption preference

    • Fe3+ > Al3+ > Co2+ > Ca2+ = Sr2+ > Rb+ > Mg2+ > K+ > NH4+ > Na+ > Li+

Strength of adsorption
Strength of adsorption

  • Outer (Gouy) layer complexes: cation still surrounded by sphere of hydration

    • Weakly bound to surface, easily exchanged

  • Inner (Stern) layer: no sphere of hydration, strongly bound directly to solid surface

    • Not easily exchange, may be effectively irreversible


  • Reversible reactions: desorption can be caused by:

    • Decreasing ionic strength

    • Change in composition of ions in solution

      • Ions with higher charge density are more likely to adsorb

Measuring adsorption
Measuring adsorption

  • Adsorption is measured in the laboratory by mixing a solution containing an ion with a solid phase (batch experiments)

    • Mix solution of known concentration with solid

    • Agitate until equilibrium is reached

    • Measure final dissolved concentration

    • Initial – final = amount adsorbed

    • Repeat at different initial concentrations

  • Plot data, and a graph called an adsorption isotherm is prepared

    • Isotherm = experiments done at constant temperature

Depicting adsorption mathematically
Depicting Adsorption Mathematically

  • Can be represented in terms of relatively simple empirical formulas, or more sophisticated models like double layer, triple layer, or constant capacitance theories

  • Most often, the simple empirical formulas are used because we don’t have the data for more sophisticated approaches


  • Since adsorption is a chemical process, we can write chemical reactions to describe it:

    • C + S ↔ CS

      • C = ion (mg/L)

      • S = surface (g)

      • CS = adsorbed ion (mg/g)

        • Adsorbed ion measure with respect to amount of solid

Linear isotherms
Linear Isotherms

  • Ratio of adsorbed to dissolved concentration is constant

    • Kd = C* / C

      • Kd = distribution coefficient (L3/mass)

      • C* = adsorbed species (massion/masssolid)

      • C = dissolved concentration (mass /L3)

  • This approach produces Linear Isotherms

  • Once Kd determined, calculate adsorbed “concentration” for any measured dissolved concentration

Typical adsorption isotherm1
Typical Adsorption Isotherm

Linear portion

of isotherm

Linear isotherms2
Linear Isotherms

  • Assumptions:

    • Fast reaction (i.e. equilibrium quickly reached)

    • Reversible reaction

    • Isothermal

    • Monolayer adsorption

  • Use Kd’s with great care because:

    • Reactions are pH, temperature, and Eh dependent

    • Species specific, don’t account for competition

    • Ionic strength dependent

    • Surface dependent

    • Can’t be universally applied

Langmuir isotherms
Langmuir Isotherms

  • These recognize that there are a limited number of adsorption sites for charged species

    • Take into account that batch experiments at higher concentration do not result in linear increases in adsorption

    • Plots go non-linear as they approach a maximum

Langmuir isotherms2
Langmuir Isotherms

  • α = KLang = adsorption constant (L3 / mass)

  • β = maximum amount of adsorption sites (mass/mass)

    • Also Cmax*

  • α and β can be obtained by plotting C/C* vs. C

    • Slope = 1/β

    • Intercept pt = 1/αβ

    • Still specific to species, site, water chemistry

  • Surface complexation adsorption models
    Surface Complexation Adsorption Models

    • Diffuse double layer, triple layer, constant capacitance

    • Best used to describe adsorption of metals and other cationic species

    Surface complexation adsorption models1
    Surface Complexation Adsorption Models

    • Advantages:

      • Based on thermodynamics

      • Balanced reactions

      • Law of mass action

      • Adsorption function of pH and solution chemistry

    Surface complexation adsorption models2
    Surface Complexation Adsorption Models

    • Recognizes that all exchange sites are not equal (inner vs. outer)

    • Types of exchange sites:

      • Aluminosilicates: crystal damage results in permanent change, “exchange” sites

      • Surface functional groups: usually a hydroxyl (OH-) on mineral edge

        • Surface charge is pH dependent

        • Positive and negative sites can co-exist

    Surface complexation adsorption models3
    Surface Complexation Adsorption Models

    • So there are a variety of sites based on surface type, charge varies between types

      • The same surface type can have sites with different bond strength

        • Inner sphere complex: strong covalent bond, bonds directly to surface

        • Outer sphere complex: cation still surrounded by sphere of hydration; held by weaker electrostatic forces

    Surface complexation adsorption models4
    Surface Complexation Adsorption Models

    • Writing surface complexation reactions; account for free energy based on chemical and electrostatic contributions

      • ≡S-OH + M2+ ↔ ≡S-OM + H+

        • ≡S = surface

        • OH = functional group

        • M2+ = dissolved metal

      • Anion adsorption

        • ≡S-OH + A- ↔ ≡S-A + OH-

    Surface complexation adsorption models thermodynamically based
    Surface Complexation Adsorption Models: Thermodynamically Based

    • Law of mass action for reaction:

      • This reaction accounts for chemical ΔG, but not electrostatic

      • Based on activity of species in bulk solution

      • Work is necessary to move ions through charged Gouy layer

      • Close to the surface, the diffuse layer has excess of cations, therefore activity (concentration) of cations increases

    Surface complexation adsorption models5
    Surface Complexation Adsorption Models

    • The equations from these models take into account multiple site types, multiple species, changes in solution chemistry

    • These surface complexation models have been shown to realistically model adsorption in lab experiments

      • However, most lab experiments use pure mineral phases and artificial solutions.

    • Surface complexation models require measurement of numerous parameters on heterogeneous materials, so their field application may not be practical


    • Adsorption is an enormously complicated subject

    • It is usually very difficult to apply laboratory derived values to the field

      • It is very difficult to get meaningful field data on surface properties

      • Beware!

    • Changing conditions can lead to changing behavior

      • e.g., contaminated sites and plumes

    Organic compounds1
    Organic Compounds

    • Definition: molecules with a carbon skeleton

      • Usually have H and O as well

    • Importance:

      • Weathering and diagenesis

      • Redox conditions of water

      • Transport of trace metals

      • Contaminants: organic contaminants and biodegradation

    Organic compound properties
    Organic Compound Properties

    • In general, organic matter is not very soluble in water.

      • Organics are non-polar or slightly polar while water is highly polar

    • Uncharged or weakly charged

    • Can exist as dissolved, solid, or gaseous phases

    • Organic matter in water is composed of an almost infinite variety of compounds

      • With current technology, can determine the general chemical composition of organics, but don’t know specific formulas

      • The exception is anthropogenic compounds where we know exact formulas

    Organic compound properties1
    Organic Compound Properties

    • Most dissolved organic matter in groundwater are humic acids

      • Substances are formed by the microbial degradation of dead plant matter, such as lignin

      • Very resistant to further biodegradation

        • Easy stuff already degraded

        • Explains why old groundwater still has organic matter

      • Defined operationally: extracted into a strongly basic aqueous solution, then precipitated from solution when pH adjusted to 1 with HCl

        • Remaining organics in solution = fulvic acids (dominate surface water)

    Typical humic acid
    Typical Humic Acid

    Humic acid chromatography
    Humic Acid Chromatography

    Measuring organic compound in groundwater
    Measuring Organic Compound in Groundwater

    • Dissolved organic carbon (DOC) (water passed through 0.45 μm filter)

      • Arbitrary division between dissolved and suspended material

      • DOC can be converted to CO2, which is how it’s typically measured

      • Can also measure DON and DOP

    • Total organic carbon (TOC)

      • Same procedures, but not filtered

    • DOC in groundwater typically low, ≤ 2 mg/L

    • DOC visible in water at about 10 mg/L (dark color)

    • Swamps and other wetlands have some of the highest DOC values, ~60 mg/L

    Organic compound nomenclature
    Organic Compound Nomenclature

    • All organics have carbon skeletons with functional groups attached

    • Aliphatics: straight or branched chains

      • e.g., propane, methylpropane

    Propane c 3 h 8 and butane c 4 h 10
    Propane (C3H8) and Butane (C4H10)

    Organic compound nomenclature1
    Organic Compound Nomenclature

    • Aromatics: ring structure

      • e.g., benzene, naphthalene

    A very little humor
    A (Very) Little Humor

    Benzene (C6H6)

    Mercedes Benzene

    Organic compound nomenclature2
    Organic Compound Nomenclature

    • Aromatics: ring structure

      • e.g., benzene, naphthalene

      • Multi-rings = polyaromatics (PNAs or PAHs)

    Organic compound nomenclature3
    Organic Compound Nomenclature

    • Aromatics: ring structure

      • e.g., benzene, naphthalene

      • Multi-rings = polyaromatics (PNAs or PAHs)

      • Heterocyclic: ring structure with atoms other than C in skeleton

        • e.g. pyridine