n Exchange therms dels ermodynamic Exchange Constant ly ions adsorbed as outer-sphere complexes or in the diffuse ion arm are exchangeable change capacities can be determined either at the native pH of soil a buffered pH (effective and total exchange capacities, respectively)
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Ion Exchange Isotherms Models Thermodynamic Exchange Constant
Ion Exchange Isotherms Models Thermodynamic Exchange Constant Only ions adsorbed as outer-sphere complexes or in the diffuse ion swarm are exchangeable Exchange capacities can be determined either at the native pH of soil or - PowerPoint PPT Presentation
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Ion Exchange
Isotherms
Models
Thermodynamic Exchange Constant
Only ions adsorbed as outer-sphere complexes or in the diffuse ionswarm are exchangeable
Exchange capacities can be determined either at the native pH of soil or at a buffered pH (effective and total exchange capacities, respectively)
Exchange Isotherms
Typically developed for binary systems
Plot charge fraction adsorbed against charge fraction in solution
For the surface phase, Xi = Ziqi / Q = Ziqi / (z1q1 + z2q2)
where Z is valance (absolute value if an anion), q is surface excess and Q is exchange capacity
For the solution phase, Ei = Zi Ci / CT
where C is solution concentration of charge
Homovalent exchange
Ca2+ - Mg2+
XCa = 2qCa / Q XMg = 2qMg / Q XCa + XMg = 1
ECa = 2CCa / CT EMg = 2CMg / CT ECa + EMg = 1
If the adsorbent had no preference for either species,it make sense that the isotherm should conform to
XCa = ECa
This can be shown if start with an expression for an exchange equilibrium constant
Mg2+(ads) + Ca2+(aq) = Ca2+(ads) + Mg2+(aq)
K = XCa(Mg) / XMg(Ca)
which assumes Xi accurately models the adsorbed phase activity
For non-preference, K = 1
Let’s do some substituting in the above equilibrium expression
Example of nearlynon-preference Ca – Mgexchange on 2:1 mineral.Dominant surface was Si tetrahedral sheet with diffuse charge. Use of ClO4
- avoided solutioncomplexes.
The same result is obtained if instead of modeling activity of adsorbedspecies by X, it is modeled by mole fraction, N, on the surface where
N1 = q1 / (q1 +q2) and N2 = q2 / (q1 + q2)
This is obviously true for homovalent exchange since in this case Ni = Xi,however, for heterovalent exchange, i.e., Ca – Na, the expressions aredifferent.
Deviation from non-preference Ca – Mg exchange in mixed mineralogy system
For the exchange reaction,
2Na+(ads) + Ca2+(aq) = Ca2+(ads) + 2Na+(aq)
for which
K = NCa(Na)2 / NNa2(Ca) i.e., surface phase activities modeled as mole fractions
Derive XCa = F(ECa) in the case of non-preference exchange, i.e., K = 1
This is less straightforward but start with the substitutions
NNa = qNa / (qCa + qNa) = 2(1 - XCa) / (2 - XCa) CCa = ECaCT / 2 CNa = ENaCT = (1 – ECa)CT since ECa + ENa = 1
where CT = 2CCa + CNa
Substituting in terms of XCa and ECa and including γis
1 = [XCa (1 – ECa)2CT2 γNa
2] / {[2(1 – XCa)2 / (2 – XCa)] (ECa CT γCa)}
which rearranges to
XCa2 - 2XCa + 2 / (1 - ECa)2CT2γNa
2 / ECaγCa = 0 from which
XCa = 1 - [β / (1 + β)]1/2
where β = (1 - ECa)2CTγNa2 / 2ECaγCa and ranges from to 0
ECa = 0, XCa = 0
ECa = 1, XCa = 1
ECa = y, XCa > y
Can show this by substitutionor dXCa / dECa at ECa = 0and ECa = 1
Deviation from non-preference in heterovalent exchange occurs even with2:1 minerals dominated by Si tetrahedral surface. Non-preference isothermnot shown but would lie below (Ca – Na) or above (Na – Mg) data.
5. Given the below exchange data for solution, mNa and mMg, and adsorbed, qNa and qMg, phases, graph the exchange isotherm, examine applicability of the non-preference isotherm and compare it with a fitted isotherm.
mNa mMg qNa qMg ------ mol / kg ------ - mol / kg -0.04950 0.00117 0.53 0.28 ENa = mNa / (mNa + 2mMg) = mNa / CT
The form of conditional exchange constantused mole fraction to model surface phaseactivities. Vanselow, KV.
Exchange Models
These equilibrium expressions are referred to as selectivity coefficients.
Largely differ based on how surface phase activities are approximated.
Either as a function of equivalent fraction or mole fraction on the adsorbent,
(AZ+ads) = XA
F(Z) or (AZ+ads) = NA exp(F(NA, NB)), where B is the other
cation in the binary exchange.
The objective in modeling surface phase activities is to best describe theexchange equilibria across the full range of surface phase compositionsusing a single value, a constant. This value would, therefore, approximatethe thermodynamic exchange constant.
(AZ+ads) = XA
F(Z)
Gaines-Thomas
Model surface phase activities as equivalent fractions directly, for example,
Notice that this form is very close to the exchange isotherm data and if isothermdata were used to calculate k at each point, k = KGaines-Thomas(2 / CT) (γCa / γNa
2),for this heterovalent exange and k = KGaines-Thomas for homovalent exchange.
The form of conditional exchange constantused charge fraction to model surface phaseactivities. Gaines-Thomas, KGT.
Gapon
The exchange reaction may be written
½ Ca2+(aq) + Na+(ads) = ½ Ca2+(ads) + Na+(aq)
for which
K (XCa)1/2 = XCa (Na+) / XNa (Ca2+)1/2 = KGapon
If (AZ+ads) = XA
Z , then (Caads) = XCa2 and (Naads) = XNa
which gives
KGapon = XCa (Na+) / XNa (Ca2+)1/2
Thus, KGapon = XCa1/2 (KGaines-Thomas)1/2
(AZ+ads) = NA exp(F(NA, NB))
Vanselow
Simplest among such models with F(NA, NB) = 0, thus, surfacephase activities are modeled directly as mole fractions
2Na+(ads) + Ca2+(aq) = Ca2+(ads) + 2Na+(aq)
K = NCa(Na)2 / NNa2(Ca) = 1
where NCa = qCa / (qCa + qNa) NNa = qNa / (qCa + qNa) and
NCa + NNa = 1
This form of a conditional exchange constant (selectivity coefficient) can bemanipulated in such way as to give a thermodynamic exchange constantbased on exchange isotherm data. May furthermore calculate ΔGo, ΔHo and ΔSo for the exchange reaction. See handout.