Introduction to Soil Chemistry
Introduction to Soil Chemistry
Introduction to Soil Chemistry
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82 soil basics iv<br />
ionized will be determined by the pK a of the acid or phenol or in the case of<br />
amines, their pK b. The solubility of organic molecules that contain ionizable<br />
groups is greatly increased once they become ionized.<br />
Once ionized, the acid molecule carries a negative charge and can thus<br />
attract cations and participate in the cation exchange capacity of soil. The contribution<br />
of this source of negative charge will depend on the pH of the soil<br />
solution and will change as the pH changes. This is thus a variable or pH<br />
dependent cation exchange capacity (CEC).<br />
Because of the variability of this component of soil, the CEC determined<br />
at two different pHs should expectedly result in different CEC values; this can<br />
also happen if two different labora<strong>to</strong>ries determine the CEC. For this reason<br />
it is essential that CEC always be measured in the same way, taking care <strong>to</strong><br />
define the pH of the solutions used in its determination.<br />
4.9. SOIL pH<br />
In any aqueous solution the pH is a measure of the hydrogen ion or pro<strong>to</strong>n<br />
activity. However, in many if not most cases, pH is treated as the concentration<br />
of pro<strong>to</strong>ns in solution rather that their activity. The soil solution is no different<br />
except that the measurement is much more complex. The complexity<br />
arises from two sources:<br />
1. An electrical potential develops at all interfaces. In soil, there are interfaces<br />
between solids and solution, solution and suspension, suspension<br />
and the electrode surface, and the reference electrode and all these<br />
interfaces.<br />
2. The concept of activity is extremely important in soil. Pro<strong>to</strong>ns or hydronium<br />
ions attracted <strong>to</strong> exchange sites or other components in the system<br />
will not be measured as part of the solution composition.<br />
For these reasons, a standard method of measuring soil pH is chosen and all<br />
phenomena related <strong>to</strong> pH or involving pH is related <strong>to</strong> this “standardized” pH<br />
measurement. The most common method is <strong>to</strong> use a 1:1 ratio of soil <strong>to</strong> water,<br />
typically 10mL of distilled water and 10g of soil. In this method, the soil and<br />
water are mixed and allowed <strong>to</strong> stand for 10min and the pH determined using<br />
a pH meter.<br />
This method does not measure exchangeable pro<strong>to</strong>ns attached <strong>to</strong> cation<br />
exchange sites; therefore, it is also common <strong>to</strong> use a salt solution (either KCl<br />
or CaCl2) instead of distilled water in determining soil pH. The K + or Ca 2+ in<br />
the solution exchanges with exchangeable hydronium, thus bringing it in<strong>to</strong><br />
solution where it can be measured. These procedures therefore usually give a<br />
pH that is less, more acidic, than that obtained using distilled water. The justification<br />
for this approach is that it is thought <strong>to</strong> more closely relate <strong>to</strong> the<br />
pH experienced by plant roots.