Soil Acidity and Liming
- Introduction
- Aqueous systems (like the soil) exhibit the property of being acid or basic depending on the relative amounts of H + and OH- ions present.
- Soils in areas with high rainfall are usually acid. Basic cations are leached more readily than Al. The presence of exchangeable Al +3 results in acid soils.
3 = acid peat soils
4,5,6 = pH range common for humid regions mineral soils
7,8,9 = common pH range for arid regions soils
10 and 11 = alkali mineral
- Aqueous systems (like the soil) exhibit the property of being acid or basic depending on the relative amounts of H + and OH- ions present.
- Measuring Acidity
pH measures active acidity or the H+ concentration of the soil solution.
pH = log 1/[H+] where H+ is the concentration in moles per liter[H+]
(moles/liter)pH .001 3 .0001 4 .00001 5 .000001 6 .0000001 7
A 10-fold change in H+ concentration results in a one unit change in pH. - Active and Potential Acidity
- an acid ionizes into hydrogen ions and the accompanying anion.
HA (Potential Acidity) = H+ + A- (Active Acidity)
Total Acidity = Active + Potential Acidity - In soils, active acidity is H+ in soil solution. Potential acidity is exchangeable Al+3.
Most of a soils acidity is potential.
Al+3 + 3H2O ==> Al(OH)3 + 3H+
Both active and potential acidity must be measured to estimate the amount of lime needed.
- an acid ionizes into hydrogen ions and the accompanying anion.
- Causes of Soil Acidity
- Parent Material - Rocks from which soil was formed may have been basic or acidic
- Rainfall - The higher the average annual rainfall the more leaching. Basic cations are removed more readily than H+ and Al+3.
- Native vegetation - Soils under forest are more acid than those developed under grassland.
Decomposition of O.M. forms acid
CO2 forms H2CO3 - Fertilizer containing NH4+
Conversion of NH4+ => NO3- produces H+ ions - Hydrolysis of Al
Al + H2O ===> AlOH3 + H+
Al can come from clay structures
- Reasons to Add Lime
- to neutralize toxic elements
- Al+3
- Reduces root growth by inhibiting cell
- Reduces Ca uptake
- Fixes soil Phosphorus
- Reduces root growth by inhibiting cell
- Mn 2+ -- toxicity is a problem on red, clayey acid soils
- At pH 4 or less, H+ can damage root membranes
- Al+3
- Increases molybdenum availability. Mo is the only micronutrient that is more available at higher pH's.
- To Supply Ca and Mg - ( two of the secondary nutrients).
- Increases microorganism activity for N fixation and nitrification
- Increases efficiency of P fertilization. P is fixed and not available to plants at low pH's.
- Improves soil physical properties. (structure)
- to neutralize toxic elements
- Determining lime requirements of a soil
- Concept of buffer capacity
- buffering - a resistance to change in pH. Removal of H+ ions from the soil solution results in their replacement by H+ ions (Al+3) from the exchange complex.
- The higher CEC of a soil the greater will be its buffer capacity because more reserve (potential) amount must be neutralized to change the pH. The percent OM must be taken into account as well as the pH when estimating the amount of lime needed to raise the pH.
Clay soils have a high buffer capacity.
Organic soils have a high buffer capacity.
Sandy soils have a low buffer capacity.
Example of the effect of CEC on lime requirements and buffer capacity![effect of CEC on lim]()
We want to change from pH 5 to 6. We look at the curve and see that this is a change from 25 to 75% base saturation or a 50% change.
How many meq of H+ must be neutralized if the CEC of the soil is 2?
- buffering - a resistance to change in pH. Removal of H+ ions from the soil solution results in their replacement by H+ ions (Al+3) from the exchange complex.
- Soil testing labs use an indirect method of measuring exchangeable acidity. N.C. method
add 10 cm3 soil + 10 ml water + 10 ml buffer at pH 6.6
measure the pH
It has been determined that each .1 decrease in pH of the solution equals 0.4 meq ac/100 cm3 of soil
rapid - large numbers of soil samples can be processed.![soil sample]()
- Concept of buffer capacity
- How lime neutralizes acidity.
H+ H+ + CaCO3 ==> Ca2+ + H2O + CO2
in solution
CaCO3 + H2O ==> Ca2+ + HCO3- +OH -
This can react with H+ ==> HOH (water) or to precipitate Al as Al(OH)3
Lime reduces the concentration of H+ ions and increases the concentration of OH - ions, and adds non acid forming cations. the material must contain an anion that combines with and neutralizes H+ ions and Al ions.
CO3 ............. does
SO4..............doesn't
oxides .......................CaO
hydroxides.................CaOH
carbonates.................CaCO3
silicates .....................SiO3- - Factors influencing the quality of liming materials
- purity - any impurities in the lime will reduce its ability to neutralize acidity. ( sand, rocks, clay, etc. )
- fineness - large particles react more slowly and less completely than fine particles.
Particle Size Efficiency Rate (%) larger than 4 mesh 0 4-8 mesh 10 8-20 mesh 20 20-60 mesh 60 60-80 mesh 80 100 mesh 100 In NC for calcitic 25% through 100 mesh 90% through 20 mesh dolomitic 35% through 100 mesh - neutralizing value - the ability to neutralize acids. expressed in terms of calcium carbonate equivalent. Calcium carbonate is the standard by which other materials are measured ( 100%) Molecular weight of CaCO3 is 100 MgCO3 is 84 1 molecule of each will neutralize the same amount of acid but on a weight basis it only takes 84g of MgCO3 to do the job of 100g of CaCO3. Neutralizing value (CCE) calcium carbonate equivalent of the pure forms of some commonly used liming materials
Neutralizing Value CaO 179 Ca(OH)2 136 CaMg(CO3)2 109 CaCO3 100 CaSiO3 86
- purity - any impurities in the lime will reduce its ability to neutralize acidity. ( sand, rocks, clay, etc. )
- Liming materials - To be considered a liming material an anion must produce OH - ions to react with H+ and Al3+ ions. Oxides, hydroxides, carbonates, and silicates
- Calcium oxide (CaO) Common names - burned lime, quicklime, unslaked lime
CaCO3 ===> CaO + CO2
Advantage is immediate reaction with the soil.
Disadvantage - caustic, difficult to handle and apply
Caking may occur. Through mixing is necessary - Calcium hydroxide (Ca(OH)2)
common names -- slaked, hydrated, builders lime
CaO + H20 ===> Ca(OH)2
Advantage - quick reaction with the soil
Disadvantage - difficult and unpleasant to handle - Calcitic limestone (CaCO3)
Dolomitic limestone (CaMg(CO3)2)
Mined from deposits. Quality depends on amount of impurities such as clay. Good handling properties. Reaction time several months. - Marl (CaCO3)
Unconsolidated deposits of CaCO3. Usually contaminated with clay. Low in Mg. - Slags (CaSiO3)
byproduct of furnaces used for making iron, steel and elemental P. - Placement of lime - Thorough mixing of lime throughout the zone of root growth is ideal.
- Particles of lime do not move in the soil.
- Application - Spread half of lime and plow down. Spread other half and disk. On established sods, lime must be topdressed. Reaction is slower and less complete. * Add smaller amounts more often.
- Factors determining the selection of a liming program.
- Lime requirements of crop to be grown. Plants differ in pH requirements.
acid - blueberries, cranberies, azaleas and camellias
neutral alkaline - Sweet clover, alfalfa, sugar beets.
Field crops in N.C. 5.8 - 6.2 is best.
Turf - 6.5 except centipede 5.5 - Texture and O.M. content affects amount of lime required to change pH and frequency of application. Overliming coarse textured soils is a possibility.
- Time and frequency of liming - use soil test. Depends on texture and organic matter content. Nitrogen fertilization and crop removal. Take soil samples at least every 3-5 years.
- Liming material to be used.
Purity, fineness, calcium carbonate equivalent
Fluid Lime- good distribution pattern, no dust
- finely divided - reacts quickly with soil
- 500-1000 pounds per acre applied at one time. Reg. annual applications.
- 2 to 4 times more expensive
- good distribution pattern, no dust
- Lime requirements of crop to be grown. Plants differ in pH requirements.
- Calcium oxide (CaO) Common names - burned lime, quicklime, unslaked lime
- Acidulating the soil
- arid western regions of the country
- overlimed soils
- further acidification of soils for growth of plants such as potatoes, azaleas, rhododendrons or camellias.
elemental sulfur, sulfuric acid, aluminum sulfate, iron sulfate and ammonium sulfate.- Elemental sulfur - pound for pound is most effective. Converted to sulfuric acid in warm moist soils by bacteria.
- Sulfuric acid H2SO4
- Aluminum sulfate - commonly used by Horticulturists for acidulating soil for azaleas, camellias, rhododendrons, etc.
- Iron sulfate ( FeSO4) - reacts similar to aluminum sulfate.