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Other Fertility Issues: Nutrients,
CEC, Acidity and Alkalinity
The potential available nutrients in a soil,
whether natural or added in
manures or fertilizer, are only in part utilized by plants
T.L. Lyon and E.O. Fippin, 1909
Other
Nutrients
Although farmers
understandably emphasize nitrogen and phosphorus because of the large
quantities used and the potential for environmental problems additional
nutrient and soil chemical issues remain important. In most cases, the
overuse of these other fertilizers and amendments doesn't cause problems
for the environment, but inappropriate use may waste money and reduce
yields. There are also animal health considerations. For example, excess
potassium in feeds for dry cows (between lactations) results in metabolic
problems, and low magnesium availability to dairy or beef cows in early
lactation can cause grass tetany. As with most other issues we have
discussed, focusing on the management practices that build up and maintain
soil organic matter will help eliminate many problems or, at least,
make them easier to manage.
Potassium
is one of the N-P-K "big three" primary nutrients needed in
large amounts and frequently not present in sufficient quantities for
plants. Potassium availability to plants is sometimes decreased when
liming a soil to increase the pH by one or two units. The extra calcium,
as well as the "pull" on potassium exerted by the new cation
exchange sites (see discussion of CEC), contribute to lower potassium
availability. Problems with low potassium levels are usually dealt with
easily by applying muriate of potash (potassium chloride), potassium
sulfate, or Sul-Po-Mag or K-Mag (potassium and magnesium sulfate). Manures
also usually contain large quantities of potassium.
Magnesium
deficiency is easily corrected if the soil is acidic by using a high-magnesium
(dolomitic) limestone to raise soil pH (see discussion of soil acidity
below). Otherwise, Sul-Po-Mag is one of the best choices for correcting
such a deficiency.
Calcium
deficiencies are usually associated with low pH soils and soils with
low CECs. The best remedy is usually to lime and build up the soil's
organic matter. However, some important crops, such as peanuts, potatoes
and apples, commonly need added calcium. Calcium additions also may
be needed to help alleviate soil structure and nutrition problems of
sodic soils (see below). In general, if the soil
does not have too much sodium, is properly limed and has a reasonable
amount of organic matter, there will be no advantage to adding a calcium
source, such as gypsum. However, soils with very low aggregate stability
may sometimes benefit from the extra salt concentration associated with
surface gypsum applications. This is not a calcium nutrition effect,
but a stabilizing effect of the dissolving gypsum salt. Higher soil
organic matter and surface residues should do as well as gypsum to alleviate
this problem.
Sulfur deficiencies
are common on soils with low organic matter. Some soil testing labs
around the country offer a sulfur soil test. (Those of you who grow
garlic should know that a good supply of sulfur is important for the
full development of garlic's pungent flavor so garlic growers want to
make sure there's plenty available to the crop.) Much of the sulfur
in soils occurs as organic matter, so building up and maintaining good
amounts of organic matter should result in sufficient sulfur nutrition
for plants. Although reports of crop response to added sulfur in the
Northeast are rare, it is thought that deficiencies of this element
may become more common now that there is less sulfur air pollution originating
in the Midwest. Some fertilizers used for other purposes, such as Sul-Po-Mag
and ammonium sulfate, contain sulfur. Calcium sulfate (gypsum) also
can be applied to remedy low soil sulfur. The amounts used on sulfur-deficient
soils are typically 20 to 25 lbs. sulfur/acre.
Zinc deficiencies
occur with certain crops on soils low in organic matter and in sandy
soils or those with a pH near neutral. Zinc problems are sometimes noted
on silage corn when manure hasn't been applied for a while. It also
can be deficient following topsoil removal from parts of fields as land
is leveled for furrow irrigation. Sometimes, crops outgrow the problem
as the soil warms up and organic sources become more available to plants.
Zinc sulfate (about 35 percent zinc) applied to soils is one of the
materials used to correct zinc deficiencies. If the deficiency is due
to high pH, or if an orchard crop is zinc-deficient, a foliar application
is commonly used. If a soil test before planting an orchard reveals
low zinc levels, zinc sulfate should be soil-applied.
Boron
deficiencies show up in alfalfa when growing on eroded knolls where
topsoil and organic matter have been lost. Root crops seem to need higher
soil boron levels than many other crops. Cole crops, apples, celery
and spinach are also sensitive to low boron levels. The most common
fertilizer used to correct a boron deficiency is sodium tetraborate
(about 15 percent boron). Borax (about 11 percent boron), a compound
containing sodium borate, also can be used to correct boron deficiencies.
On sandy soils low in organic matter, boron may be needed on a routine
basis.
Manganese
deficiency, usually associated with soybeans and cereals on high
pH soils and vegetables grown on muck soils, is corrected with the use
of manganese sulfate (about 27 percent manganese). About 10 lbs. of
water-soluble manganese per acre should satisfy plant needs for a number
of years. Up to 25 lbs. per acre of manganese is recommended, if the
fertilizer is broadcast on a very deficient soil. Natural, as well as
synthetic, chelates (at about 5 to 10 percent manganese) usually are
applied as a foliar spray.
Iron
deficiency occurs when blueberries are grown on moderate to high pH
soils. Iron deficiency also sometimes occurs on soybeans, wheat, sorghum,
and peanuts growing on high pH soils. Iron (ferrous) sulfate or chelated
iron are used to correct iron deficiency. Both manganese and iron deficiencies
are frequently corrected by using foliar application of inorganic salts.
Cation
Exchange Capacity Management
The CEC in soils
is due to well humified ("very dead") organic matter and clay
minerals. The total CEC in a soil is the sum of the CEC due to organic
matter and CEC due to the clays. In fine-textured soils with medium
to high CEC-type clays, much of the CEC may be due to clays. On the
other hand, in sandy loams with little clay, or in some of the soils
of the southeastern U.S. containing clays with low CEC, organic matter
may account for the overwhelming fraction of the total CEC.
There are two
practical ways to increase the ability of soils to hold nutrient cations,
such as potas-sium, calcium, magnesium, and ammonium:
- Add organic matter
by many of the methods discussed earlier in Part Two.
- If the soil is too
acidic, use lime (see below) to raise its pH to the high end of
the range needed for the crops you grow.
One of the benefits
of liming acid soils is to increase soil CEC! Here's why: As the pH
increases, so does the CEC of organic matter. As hydrogen (H+) on humus
is neutralized by liming, the site where it was attached now has a negative
charge and can hold onto Ca++, Mg++, K+, etc.
Estimating Organic Matter's Contribution
to a Soil's CEC
The CEC of a soil is usually
expressed in terms of the number of milliequivalents (me)
of negative charge per 100 grams of soil. (The actual number
of charges represented by one me is about 6 followed by
20 zeros.) A useful rule of thumb for estimating the CEC
due to organic matter is as follows: for every pH unit above
pH 4.5, there is 1 me of CEC in 100 gm of soil for every
percent organic matter. (Don't forget that there will also
be CEC due to clays.)
Example 1: pH = 5.0
and 3% SOM → (5.0 4.5) x 3 = 1.5 me/100g
Example 2: pH = 6.0 and 3% SOM → (6.0 4.5) x 3
= 4.5 me/100g
Example 3: pH = 7.0 and 3% SOM → (7.0 4.5) x 3
= 7.5 me/100g
Example 4: pH = 7.0 and 4% SOM → (7.0 4.5) x 4
= 10.0 me/100g
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Many soil testing
labs also will run CEC, if asked. However, there are a number of possible
ways to do the test. Some labs determine what the CEC would be if the
soil's pH was 7 or higher. They do this by adding the acidity that would
be neutralized if the soil was limed to the current soil CEC. This is
the CEC the soil would have at the higher pH, but is not the
soil's current CEC. For this reason, some labs total the major cations
actually held on the CEC (Ca++ + K+ + Mg++)
and call it effective CEC. It is more useful to know the effective CEC
the actual current CEC of the soil than CEC determined at a higher pH.
Soil
Acidity
Background
Plants have evolved under specific environments, which in turn influence
their needs as agricultural crops. For example, alfalfa originated in
a semiarid region where soil pH was high; alfalfa requires a pH in the
range of 6.5 to 6.8 or higher (see figure 18.1 for common soil pH levels).
On the other hand, blueberries, which evolved under acidic conditions,
require a low pH to provide needed iron (iron is more soluble at low
pH). Other crops, such as peanuts, watermelons, and sweet potatoes,
do best in moderately acid soils in the range of pH 5 to 6. Most other
agricultural plants do best in the range of pH 6 to 7.5.
Several problems
may cause poor growth of acid-sensitive plants in low pH soils. The
following are three common ones:
- aluminum and manganese
are more soluble and can be toxic to plants;
- lack of calcium, magnesium,
potassium, phosphorus or molybdenum (especially needed for nitrogen
fixation by legumes); and
- a slowed decomposition
of soil organic matter and decreased mineralization of nitrogen.
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Figure 18.1 Soil pH and acid/base status.
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The problems caused by soil acidity are usually less severe, and the
optimum pH is lower, if the soil is well supplied with organic matter.
Organic matter helps to make aluminum less toxic and, of course, humus
increases the soil's CEC. Soil pH will not change as rapidly in soils
that are high in organic matter. Soil acidification is a natural process
that is accelerated by acids produced in soil by most nitrogen fertilizers.
Soil organic matter slows down acidification and buffers the soil's
pH because it holds the acid hydrogen tightly. Therefore, more acid
is needed to decrease the pH by a given amount when a lot of organic
matter is present. Of course, the reverse is also true more lime is
needed to raise the pH of high-organic matter soils by a given amount
(see "Soil Acidity" box below).
Limestone application
helps create a more hospitable soil for acid-sensitive plants in many
ways, such as:
- neutralizing acids;
- adding calcium in large
quantities (because limestone is calcium carbonate, CaCO3);
- adding magnesium in
large quantities if dolomitic limestone is used (containing carbonates
of both calcium and magnesium);
- making molybdenum and
phosphorus more available;
- helping to maintain
added phosphorus in an available form;
- enhancing bacterial
activity; and
- making aluminum and
manganese less soluble.
Almost all the
acid in acidic soils is held in reserve on the solids, with an extremely
small amount active in the soil water. If all that we needed to neutralize
was the acid in the soil water, a few handfuls of lime per acre would
be enough to do the job, even in a very acid soil. However, tons of
lime per acre are needed to raise the pH. The explanation for this is
that almost all of the acid that must be neutralized in soils is reserve
acidity associated with either organic matter or aluminum.
Soil Acidity
Background
- pH 7 is neutral.
- Soil with pH levels above 7 are alkaline,
those less than 7 are acidic.
- The lower the pH, the more acidic is the
soil.
- Soils in humid regions tend to be acidic,
those in semi-arid and arid regions tend to be around
neutral or are alkaline.
- Acidification is a natural process.
- Most commercial nitrogen fertilizers are
acid forming, but many manures are not.
- Crops have different pH needs pro-bably
related to nutrient availability or sus-ceptibility to
aluminum toxicity at low pH.
- Organic acids on humus and aluminum on
the CEC account for most of the acid in soils.
Management
- Use limestone to raise soil pH (if magnesium
is also low, use a high magnesium or dolomitic lime).
- Mix lime thoroughly into the plow layer.
- Spread lime well in advance of sensitive
crops, if at all possible.
- If the lime requirement is high some labs
say greater than 2 tons and others say greater than 4
tons consider splitting the application over two years.
- Reducing soil pH (making soil more acid)
for acid-loving crops is done best with elemental sulfur
(S).
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pH
Management
Increasing the pH of acidic soils is usually accomplished
by adding ground or crushed limestone. Three pieces of information
are used to determine the amount of lime that's needed:
- What is the soil pH?
Knowing this and the needs of the crops you are growing tell whether
lime is needed and what target pH you are shooting for. If the soil
pH is much lower than the pH needs of the crop, you need to use
lime. But the pH value doesn't tell you how much lime is needed.
- What is the lime requirement
needed to change the pH to the desired level? There are a number
of different tests used by soil testing laboratories that estimate
soil lime requirements. Most give the results in terms of tons/acre
of agricultural grade limestone to reach the desired pH.
- Is the limestone you
use very different from the one assumed in the soil test report?
The fineness and the amount of carbonate present govern the effectiveness
of limestone how much it will raise the soil's pH. If the lime you
will be using has an effective calcium carbonate equivalent that's
very different from the one used as the base in the report, the
amount applied may need to be adjusted upward (if the lime is very
coarse or has a high level of impurities) or downward (if the lime
is very fine and is high in magnesium and contains few impurities).
Testing labs usually use the information you provide
about your cropping intentions and integrate the three issues
(see left column) when recommending limestone application rates.
There are laws governing the quality of limestone sold in each
state. Soil testing labs give recommendations assuming the use
of ground limestone that meets the minimum state standard. |
Soils with more clay and more organic matter need more lime to change
their pH (see figure 18.2). Although organic matter
buffers the soil against pH decreases, it also buffers against pH increases
when you are trying to raise the pH with limestone. Most states recommend
a soil pH around 6.8 only for the most sensitive crops, such as alfalfa,
and about pH 6.2 to 6.5 for many of the clovers. As pointed out above,
most of the commonly grown crops do well in the range of pH 6.0 to 7.5.
There are other
liming materials in addition to limestone. One of the commonly used
ones in some parts of the U.S. is wood ash. Ash from a modern air-tight
wood burning stove may have a fairly high calcium carbonate content
(80 percent or higher). However, ash that is mainly black indicating
incompletely burned wood may have as little as 40 percent effective
calcium carbonate equivalent. Lime-sludge from wastewater treatment
plants and fly ash sources may be available in some locations. Normally,
minor sources like the ones mentioned above are not locally available
in sufficient quantities to put much of a dent in the lime needs of
a region. Because they might carry unwanted contaminants to the farm,
be sure that liming materials are thoroughly evaluated for metals and
field-tested before you use any new byproduct liming sources.
"Overliming" Injury
Sometimes there are problems when soils are
limed, especially if a very acidic soil has been quickly raised
to high pH levels. Decreased crop growth because of "overliming"
injury is usually associated with lowered availability of
phosphorus, potassium, or boron, although zinc and copper
deficiencies can be produced by liming acidic sandy soils.
If there has been a long history of use of triazine herbicides,
such as atrazine, liming may release these chemicals and kill
sensitive crops.
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Figure 18.2 Examples of approximate lime needs
to reach pH 6.8. Modified from Peech, 1961. |
Need to Lower the Soil's pH?
When growing plants that require low pH, you
may want to add acidity to the soil. This is probably only
economically possible for blueberries and is most easily done
with elemental sulfur (S), which is converted into an acid
by soil microorganisms over a few months. For the examples
in figure 18.2, the amounts of S needed to drop the pH by
one unit would be approximately 3/4 ton per acre for the
silty clay loams, ½ ton per acre for the loams and silt
loams, 600 lbs. per acre for the sandy loams, and 300 lbs.
per acre for the sands. Sulfur should be applied the year
before planting blueberries.
Alum (aluminum sulfate) may also be used to acidify soils.
About six times more alum than elemental sulfur is needed
to achieve the same pH change.
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Arid Region Problems: Sodic (alkali)
and Saline Soils
Special soil
problems are found in arid and semi-arid regions, including soils that
are high in salts, called saline soils, and those that have excessive
sodium (Na+), called sodic soils. Sometimes these go together and the
result is a saline-sodic soil. Saline soils usually have good soil tilth,
but plants can't get the water they need because the high salt levels
inhibit water-uptake. Sodic soils tend to have very poor physical structure
because the high sodium levels cause clays to disperse, leading to the
breaking apart of aggregates. As aggregates break down, these soils
become difficult to work with and very unpleasant for plants. Wet sodic
soils with an adequate amount of clay end up looking and behaving like
chocolate pudding.
Saline soil.
Electrical conductivity of a soil extract is greater than
4 ds/m, enough to harm sensitive crops.
Sodic soil. Sodium occupies more than
15 percent of the CEC. (Soil structure can significantly deteriorate
in some soils at even lower levels of sodium.) |
Saline and sodic soils are commonly found in the semi-arid and arid
regions in the western U.S., with pockets of saline soils found near
the coastline. Sometimes, the extra moisture accumulated during a fallow
year in semi-arid regions causes field-seeps, which lead to the development
of saline and sodic patches.
Before embarking
on a program to improve saline or sodic soil, it is important to find
out what is causing the problem. Do you have a high water table that
contains salty water? Is there a saline or alkali "seep" in
a portion of the field? Is it a generalized problem over the entire
field without a high water table? If a high water table is causing salts
to migrate upward to the root zone, installation of tile drainage may
be necessary. Water surfacing in saline and alkali seeps usually can
be reduced by changing from an alternate year fallow to a more intense
annual cropping regime.
There are a
number of ways to deal with saline soils that don't have shallow salty
groundwater. One is to keep the soil continually moist. For example,
by using drip irrigation with low salt water plus a surface mulch, the
salt content will not get as high as it would if allowed to concentrate
when the soil dries. Another is to grow crops or varieties of crops
that are more tolerant of soil salinity. Saline-tolerant plants include
barley, bermuda grass, oak, rosemary, and willow. However, the only
way to get rid of the salt is to add sufficient water to wash it below
the root zone. The amount of water needed to do this is related to the
salt content of the irrigation water, expressed as electrical conductivity
(ECw) and the salt content desired in the drainage water (ECdw). The
amount of water needed can be calculated using the following equation:
Water needed
= (amount of water needed to saturate soil) x (ECw/ECdw)
Salts are Present in All Soils
Salts of calcium, magnesium, potassium and other
cations along with the common negatively charged anions chloride,
nitrate, sulfate, and phosphate are found in all soils. However,
in soils in subhumid and humid climates with from an inch
or two to well over 7 inches of water percolating beneath
the root zone every year salts don't usually accumulate to
the levels where they can be harmful to plants. Even when
high rates of fertilizers are used, salts usually only become
a problem when you place large amounts in direct contact with
seeds or growing plants. Salt problems frequently occur in
greenhouse potting mixes because growers regularly irrigate
their greenhouse plants with water containing fertilizers
and may not add enough water to leach the accumulating salts
out of the pot.
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The amount of
extra irrigation water needed to leach salts is also related to the
sensitivity of the plants that you're growing. For example, sensitive
crops like onions and strawberries may have twice the leaching requirement
as moderately sensitive broccoli or tomatoes. Drip irrigation uses relatively
low amounts of water, so lack of leaching may cause salt build-up even
for moderately saline irrigation sources. This means that the leaching
may need to occur during the growing season, but care is needed to prevent
leaching of nitrate below the root zone.
For sodic soils,
a calcium source is added usually gypsum (calcium sulfate). The calcium
replaces sodium held by the cation-exchange capacity. The soil is then
irrigated so that the sodium can be leached deep in the soil. Because
the calcium in gypsum easily replaces the sodium on the CEC, the amount
of gypsum needed can be estimated as follows for every milliequilivent
of sodium that needs to be replaced to 1 foot, about 2 tons of agricultural
grade gypsum is needed per acre. Adding gypsum to non-sodic soils doesn't
help physical properties if the soil is properly limed, except for those
soils containing easily dispersible clay that are also low in organic
matter.
Sources
Hanson, B.R., S.R. Grattan, and A. Fulton. 1993. Agricultural
Salinity and Drainage. Publication 3375, Div. of Agriculture
and Natural Resources, University of California, Oakland, CA.
Magdoff, F.R. and R.J. Bartlett. 1985. Soil pH buffering
revisited. Soil Science Society of America Journal 49:145148.
Peech, M. 1961. Lime Requirement vs. Soil pH Curves
for Soils of New York State. Mimeographed. Cornell University
Agronomy Department, Ithaca, NY.
Pettygrove, G.S., S.R. Grattan, T.K. Hartz, L.E. Jackson,
T.R. Lockhart, K.F. Schulbach, and R. Smith. 1998. Production
Guide: Nitrogen and Water Management for Coastal Cool-Season Vegetables.
Publication 21581, Division of Agriculture and Natural Resources,
University of California, Oakland, CA.
Rehm, G. 1994. Soil Cation Ratios for Crop Production.
North Central Regional Extension Publication 533. University of
Minnesota Extension Service, St. Paul, MN.
Tisdale, S.L., W.I. Nelson, J.D. Beaton, and J.L.
Havlin. 1993. Soil Fertility and Fertilizers. Macmillan Publishing
Co., New York, NY.
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