ch. 5. activity coefficents of dissolved species 5-1. introduction 5-1. introduction what is...
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Ch. 5. ACTIVITY COEFFICENTS OF DISSOLVED SPECIES
5-1. Introduction What is activity of a dissolved species?
Effective concentration Equivalent to the concentration acting in effect
Why do we need activity (or have activity)? Interactions among the dissolved matter Interference among the dissolved matter causes partial influences on the solution properties
Where can we observe the activity effect? Boiling point increase, freezing point decrease Conductivity Others
5-2. Activity Coefficient & Ionic Strength
Activity coefficient: A function of the ionic strength of the solution ai = gimi
Ionic strength: A measure of the ionic characteris-tics of the solution Lewis & Randall (1921) I = ½ S zi
2mi
Examples Mono-monovalent salts: KCl I=mKCl
Mono-divalent salts: K2SO4 I=3mK2SO4
Di-divalent salts: CaSO4 I = 4mCaSO4
Approximate estimation of I from TDS Eqn (4.4) to (4.6) on p.124
Approximate estimation of I from SpC Eqn (4.7) to (4.9) on p.124
Otherwise? Should be calculated from the chemical composition
5-3. Mean Ion-Activity Coefficients
The coefficients measured for a solutions which is due to the net effect of both cations and anions g± =[gn+ gn-]1/n , n = (n+ + n-)
Fig. 4.1 on p.125 McInnes convention (McInnes 1919)
g±KCl = gK = gCl
Obtain gK and gCl from g±KCl
Then other g using the above relation
Example 4.1 on p.127
5-4. Theoretical Calculation of the Activity Coefficients
Debye-Hückel limiting law (DHLL) When I <0.001: eqn (4.30) on p.129
Extended Debye-Hückel equation (EDHE) When I<0.1: eqn (4.28) on p.128 A=1.824928*106ro
1/2(eT)-3/2, 0.5092 (at 25C) B=50.3(eT)-1/2, 0.3283 (at 25C) Table 4.1 for effective ionic radii on p.130 Fig. 4.3 on p.132
Other equations for higher I Davies et al.; eqn (4.31) on p.132 Trusdell & Jones (1974) Bronsted-Guggenheim-Scatchard specific ion interaction theory (SIT)
equaton: eqn (4.32) p.133 Fig. 4.4. p.135. Pitzer model; eqn (4.49) p.138
5-5. Limitation of Debye-Huckel Theory
All interactions are not purely ionic Ions are not point charges Ion size varies with I Ions do interact w/ other ions and even with the
same species
5-6. Activity Coefficients of Molecular Species
In most cases, approximately g=1 Generally follow Setchenow eqn (Lewis & Ran-
dall, 1961) Log gi = KiI, where Ki = 0.02 ~ 0.23 Table 4.5 on p.144.