(IPPM) in Vegetables - Vegetableipmasia.org
(IPPM) in Vegetables - Vegetableipmasia.org
(IPPM) in Vegetables - Vegetableipmasia.org
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Resource Manual on <strong>IPPM</strong> <strong>in</strong> Rice<br />
World Education Philipp<strong>in</strong>es, Inc.<br />
To further expla<strong>in</strong> the idea of soil pH, a more general analogy can be used. Imag<strong>in</strong>e the<br />
soil as a huge pantry or a place for stor<strong>in</strong>g food <strong>in</strong> the house. The pantry must be a goodenough<br />
cab<strong>in</strong>et, cool enough to ma<strong>in</strong>ta<strong>in</strong> the freshness of the food kept <strong>in</strong> it. Similarly,<br />
the soil has to have the good qualities for it to be an appropriate storage place for<br />
nutrients. In the case of sandy soil or a soil under high ra<strong>in</strong>fall conditions, the nutrients<br />
are often leached or dissolved. Thus, the pantry turns out to be a poor place for stor<strong>in</strong>g<br />
food. In this case, putt<strong>in</strong>g OM back <strong>in</strong>to the soil is just like stock<strong>in</strong>g the pantry with<br />
food. An ideal soil with a good mixture of sand, silt, clay and <strong>org</strong>anic matter, therefore,<br />
is like a large pantry that allows storage for many k<strong>in</strong>ds of food. If the soil pH is too low<br />
or too high, storage of nutrients will be difficult and the pantry will be empty. Thus, to<br />
<strong>in</strong>crease soil nutrients, pH level must be ma<strong>in</strong>ta<strong>in</strong>ed at a desirable balance.<br />
Improv<strong>in</strong>g Acid Soils<br />
Lime is the most common material used to neutralize acid soils. Lime <strong>in</strong> pure form is<br />
calcium carbonate (CaCO 3 ). What is important <strong>in</strong> lime is not the calcium (Ca++),<br />
although calcium is a required nutrient for plant growth. Rather, it is the carbonate<br />
(CO 3 ) that helps balance the pH level of acid soils. It does this by comb<strong>in</strong><strong>in</strong>g with the<br />
hydrogen ion (H+). Each carbonate molecule comb<strong>in</strong>es with two hydrogen ions, and <strong>in</strong><br />
this way the lime cleans up the excess H+ and raises the soil pH toward neutral.<br />
The formal description of the reaction goes as follows:<br />
2 CaCO 3 + 3H+ 2Ca++ + HCO 3 - + H 2 CO 3<br />
For every two molecules of CaCO 3 , 3 ions of hydrogen (3H+) are taken up (lower<strong>in</strong>g the<br />
pH), produc<strong>in</strong>g 2Ca++ (which are now available for storage <strong>in</strong> the soil, or uptake by the<br />
plant), and one molecule each of bicarbonate (H 2 CO 3 ) and HCO 3 -.<br />
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