Many nutrients required by plants exist in soil as basic cations:
A soil’s cation-exchange capacity is a measure of its ability to adsorb these basic cations as well as exchangeable hydrogen and aluminum ions. The cation-exchange capacity of soil is derived from two sources: small clay particles called micelles consisting of alternating layers of alumina and silica crystals, and organic colloids.
Replacement of 
+ by other cations of lower valence creates a net negative charge within the inner layers of the micelles. This is called the soil’s permanent charge. For example, replacement of an atom of aluminum by calcium within a section where the net charge was previously zero, as shown below, produces a net charge of –1, to which other cations can become adsorbed.
Figure 1
A pH-dependent charge develops when hydrogen dissociates from hydroxyl moieties on the outer surfaces of the clay micelles. This leaves negatively-charged oxygen atoms to which basic cations may adsorb. Likewise, a large pH-dependent charge develops when hydrogen dissociates from carboxylic acids and phenols in organic matter.
In most clays, permanent charges brought about by substitution account for anywhere from half to nearly all of the total cation-exchange capacity. Soils very high in organic matter contain primarily pH-dependent charges.
In a research study, three samples of soil were leached with a 1 N solution of neutral KCl, and the displaced A13+ and basic cations measured. The sample was then leached again with a buffered solution of BaCl2 and triethanolamine at pH 8.2, and the displaced H+ measured. Table 1 gives results for three soils tested by this method.
Table 1
Due to the buffering effect of the soil’s cation exchange capacity, just measuring the soil solution’s pH will not indicate how much base is needed to change the soil pH. In another experiment, measured amounts of acid and base were added to 10gram samples of well-mixed soil that had been collected from various locations in a field. The volumes of the samples were equalized by adding water. The results were recorded in Figure 2.
Figure 2.
How much solid NaOH is required to neutralize 700 mL of 2 N HNO3?
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Reference / correct answer:
To solve this problem, you need to remember the definition of normality, and know how acids and bases interact to neutralize each other. Normality is defined as the number of equivalents per liter of solution. Here nitric acid has one equivalent, that is, it has one proton to donate pr mole. Thus, for this compound, normality equals molarity, and we have 2 moles in one liter, or 1.4 moles in 700 milliliters. Since acids and bases react in a 1 to 1 ration of equivalents, in order to neutralize 1.4 moles of nitric acid, you must have an equal number of equivalents of the neutralizing substance present. Since sodium hydroxide also has 1 equivalent per mole, we need the same number of moles of each. Therefore, we need 1.4 moles of sodium hydroxide. Sodium hydroxide has a molar weight of 40 grams, 1.4 moles will have a mass of 56 grams. This is answer C, which is the correct choice.
