Presentation on theme: "Class evaluations Class evaluations. Soil Chemistry."— Presentation transcript:
Class evaluations Class evaluations
Ion Exchange Ions adsorbed to soil surfaces can be exchanged with ions in soil solution. Ions adsorbed to soil surfaces can be exchanged with ions in soil solution. Cations and anions Cations and anions
Ion exchange Organic colloids and inorganic micelles (clays) are sites of ion exchange Organic colloids and inorganic micelles (clays) are sites of ion exchange Where do ions in soil come from? Where do ions in soil come from? Release from organic matter Release from organic matter Rain Rain Weathering of parent material Weathering of parent material
Ion exchange Exchangeable cations (on soil surfaces) cannot be removed by leaching. Exchangeable cations (on soil surfaces) cannot be removed by leaching. Soluble cations (in solution) Soluble cations (in solution) can be removed by leaching.
When soil is dried… When soil is dried… …exchangeable cations hold to adsorption sites on soil surfaces. …soluble cations (and anions) precipitate or crystallize as salts. …soluble cations (and anions) precipitate or crystallize as salts.
Examples of soluble cations precipitating
Ion exchange Exchangeable ions on soil surface trading places with ions in solution.
On soil surfaces, there are: Exchangeable and Nonexchangeable Ions : Exchangeable: weakly held, in contact with soil solution, ready for quick replacement. “outer sphere complex” Nonexchangeable: “inner sphere complex” adsorbed by strong bonds or held in inaccessible places (e.g., the K + between layers of illite) not part of ion exchange !
Cation exchange capacity (CEC) Sum total of exchangeable cations that a soil can adsorb. ( prevents nutrients from leaching away from roots)
CEC Expressed in: milliequivalents per 100 g (meq/100g)
Base saturation % of exchange sites occupied by basic cations Basic cations are cations other than H + and Al +3 Base saturation Base saturation + H+ ion saturation should equal 100% should equal 100%
For midwest US soils Notice neutral pH (7.0) requires a base sat of 80%. (neutral pH is not 50% because most base cations have a + charge of 2)
equilibrium Strive for equivalent proportions of solution and exchangeable ions. Upset equilibrium by: removal by plants leachingfertilizationweathering Initiate ion exchange
Ion exchange example: Add H + ions to soil : soil Ca+ + H+H+ H+ solution exchangeablesolution + H+ Ca+ exchangeablesolution
Rules of ion exchange Process is Reversible Process is Reversible Charge by charge basis Charge by charge basis Ratio Law: Ratio Law: ratio of exchangeable cations will be same as ratio of solution cations ratio of exchangeable cations will be same as ratio of solution cations
Add K fertilizer… Ca +2 K+K+ + K+ + 1 Ca : 2 K Same ratio
Energy of adsorption Strong Weak Al +3 > Ca +2 > Mg +2 > [K + = NH 4 + ] > Na + > H + (based on charge and hydrated radius)
Soil pH importance Determines solubility of nutrients Determines solubility of nutrients Before plants can get nutrients, they must be dissolved in soil solution Before plants can get nutrients, they must be dissolved in soil solution Microbial activity also depends on pH Microbial activity also depends on pH
pH negative log of the hydrogen ion concentration (also a measure of OH - concentration) If H + concentration > OH - : acidic If OH - > H + : basic Soil pH is pH of solution, NOT exchange complex
In soil, both H + and Al +3 ions produce acidity Al +3 produces H + ions when it reacts with water. ( when pH below 6: Al +3 is the cause of acidity )
Causes of soil basicity 1. Hydrolysis of basic cations 2. Hydrolysis of carbonates
1. Hydrolysis of basic cations: (especially Ca +2, Mg +2, K +, NH 4 +, Na + ) ( also called exchangeable bases ) Extent to which exchangeable bases will hydrolyze depends on ability to compete with H+ ions for exchange sites. Na + H2OH2O H + + OH -
K + and Na + are weakly held compared to Ca +2 and Mg +2. Recall energy of adsorption Recall energy of adsorption So, K + and Na + are hydrolyzed easily and yield higher pHs.
2. Hydrolysis of carbonates (especially CaCO 3, MgCO 3, Na 2 CO 3 ) As long as there are carbonates in the soil, carbonate hydrolysis controls pH. As long as there are carbonates in the soil, carbonate hydrolysis controls pH. Calcareous soils remain alkaline because H+ ions combine with OH - to form H 2 O. Calcareous soils remain alkaline because H+ ions combine with OH - to form H 2 O. For those soils to become acid, all carbonates must be leached. For those soils to become acid, all carbonates must be leached. Basic cations replaced by Al +3 and H + Basic cations replaced by Al +3 and H + CaCO 3 + H 2 O Ca +2 + HCO OH - Na 2 CO 3 + H 2 O Na + HCO OH - (higher pH because Na more soluble)
Causes of soil acidity 1. Accumulation of soluble acids 2. Exchangeable acids (Al +3, H + )
1.Accumulation of soluble acids at faster rate than they can be neutralized or removed a. Carbonic acid (respiration and atmospheric CO 2 ) b. Mineralization of organic matter (produces organic, nitric, sulfuric acids) Precipitation increases both a and b
2. Exchangeable acids Exch. H + or Al +3 dissociate Al +3 ties up OH - from water, releases an equivalent amount of H+ ions. Al +3 ties up OH - from water, releases an equivalent amount of H+ ions. Al +3 + H 2 OAlOH +2 + H+
CEC and pH Only 2:1 silicate clays do not have pH-dependent CECs. Others are pH-dependent: 1:1 kaolinite: low pH: low CEC high pH: high CEC Oxidic clays