Introduction to Soil Chemistry
Introduction to Soil Chemistry
Introduction to Soil Chemistry
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pH<br />
9.5<br />
9<br />
8.5<br />
8<br />
7.5<br />
7<br />
6.5<br />
6<br />
5.5<br />
ph titration of soil 117<br />
Titration of <strong>Soil</strong> with NaOH<br />
5<br />
0 20 40<br />
Titrant Volume<br />
60<br />
Figure 6.5. Titration of 50g of soil suspended in 50mL of distilled water with 0.1M NaOH using<br />
a pH meter. Titrant was added slowly and continuously with stirring.<br />
titration endpoint is seen here as there is in Figure 6.1. However, it is possible<br />
<strong>to</strong> determine the amount of base needed <strong>to</strong> bring this soil <strong>to</strong> pH 6.5, which is<br />
a typical pH desired for crop production.<br />
This also explains why the pH of any extracting solution is important.<br />
Depending on the pH of the extracting solution, the component(s) of interest<br />
may be in the form of an ion or a polar or neutral molecule.This, in turn, determines<br />
whether it will be solvated by the solvent chosen as the extractant. If a<br />
certain pH is needed for an extraction process, then titration of a soil can be<br />
carried out in order <strong>to</strong> determine how much base or acid would be needed for<br />
the process. This would be useful in cases where removal of a contaminant<br />
from a spill site or a field is required.<br />
Caution: Lowering or raising a soil’s pH <strong>to</strong> effect remediation, especially<br />
on a large scale, is not feasible for four reasons: (1) changing<br />
the pH of soil <strong>to</strong> any great extent requires large amounts of acid or<br />
base because soil is highly buffered, (2) soil is destroyed at both very<br />
high and very low pH levels, (3) a large amount of material that<br />
cannot be readily returned <strong>to</strong> the environment is produced, and (4)<br />
the material is no longer soil!