C - Lublin
C - Lublin
C - Lublin
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Q V (pH)/N t = α(pH) =<br />
n<br />
∑<br />
i=<br />
1<br />
n<br />
αi(K i , pH s ) N i /N t = ∑ αi(K i , pH s ) f(K i ), (4)<br />
where N t is the total amount of surface groups and f(K i )=N i /N t is a fraction of i-th<br />
groups. Using condensation approximation (Nederlof et al. 1993) the f(K i ) values<br />
are:<br />
f(K i ) = 1/N t ∆ Q V (pH)/∆K i ; K i = [H + s ], (5)<br />
and in logarithmic scale:<br />
f(pK i ) = 1/N t ∆ Q V (pH)/∆pK i ; pK i = pH s . (6)<br />
The distribution function of surface dissociation constants, i.e. f(K i ) vs. K i dependence,<br />
can be calculated knowing both surface protons activity (pH s ) and N t<br />
values. Soil components, as well as plant root surfaces may have different shapes<br />
and different charges thus may vary in surface potential values. For pH s (and K i )<br />
calculations, basing on the diffuse double layer theory, a single potential value<br />
spread uniformly over all surfaces of the same shape is a common assumption,<br />
which seems not to be valid in the case of soils and plants. Also, there still exist<br />
much controversies on the application of the DDL theory to surface chemistry (Mc<br />
Bride, 1997). Therefore, the surface proton activity is replaced by the solution activity<br />
and N t is taken as N max = maximal value of (N susp -N sol ) measured within the<br />
experimental window and, instead of the intrinsic, the distribution functions of<br />
apparent surface dissociation constants, K app , are determined:<br />
f (pK app,i ) = 1/N max ∆Q V (pH)/∆pK app ; pK app = pH. (7)<br />
The average value of pK app , pK app,av , is calculated as:<br />
n<br />
pK app,av = ∑ pKi,app f i (pK app ), (8)<br />
i=1<br />
which is direct measure of the average energy of the proton binding.<br />
Having the variable charge vs. pH dependence one can find the relation of actual<br />
surface charge, Q A , vs. pH. To do this the Q V (pH) curves are shifted against y-<br />
axis to meet the actual charge value at any pH e.g. a cation exchange capacity of<br />
the studied solid, estimated at the same ionic strength, at which the titration is performed.<br />
One should select a higher pH value to diminish eventual occurrence of<br />
positive surface charge that is not determined during the CEC measurements.<br />
i=1<br />
68