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Class evaluations

Class evaluations. Soil Chemistry. Ion Exchange. Ions adsorbed to soil surfaces can be exchanged with ions in soil solution. Cations and anions. Ion exchange. Organic colloids and inorganic micelles (clays) are sites of ion exchange Where do ions in soil come from?

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Class evaluations

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  1. Class evaluations

  2. Soil Chemistry

  3. Ion Exchange • Ions adsorbed to soil surfaces can be exchanged with ions in soil solution. • Cations and anions

  4. Ion exchange • Organic colloids and inorganic micelles (clays) are sites of ion exchange • Where do ions in soil come from? • Release from organic matter • Rain • Weathering of parent material

  5. Ion exchange • Exchangeable cations (on soil surfaces) cannot be removed by leaching. • Soluble cations (in solution) can be removed by leaching.

  6. When soil is dried… …exchangeable cations hold to adsorption sites on soil surfaces. …soluble cations (and anions) precipitate or crystallize as salts.

  7. Examples of soluble cations precipitating

  8. Ion exchange Exchangeable ions on soil surface trading places with ions in solution.

  9. 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 !

  10. Cation exchange capacity (CEC) Sum total of exchangeable cations that a soil can adsorb. ( prevents nutrients from leaching away from roots)

  11. CEC Expressed in: milliequivalents per 100 g (meq/100g)

  12. Base saturation % of exchange sites occupied by basic cations Basic cations are cationsother than H+ and Al+3 Base saturation + H+ ion saturation should equal 100%

  13. 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)

  14. equilibrium Strive for equivalent proportions of solution and exchangeable ions. Upset equilibrium by: removal by plants leaching fertilization weathering Initiate ion exchange

  15. Ion exchange example:Add H+ ions to soil : H+ H+ Ca+ Ca+ Ca+ Ca+ H+ Ca+ Ca+ soil H+ Ca+ + + H+ Ca+ Ca+ H+ H+ Ca+ H+ Ca+ Ca+ Ca+ Ca+ solution Ca+ Ca+ exchangeable solution exchangeable solution

  16. Rules of ion exchange • Process is Reversible • Charge by charge basis • Ratio Law: • ratio of exchangeable cations will be same as ratio of solution cations

  17. Add K fertilizer… K+ Ca+2 Ca+2 K+ Ca+2 + K+ + K+ K+ Ca+2 K+ K+ K+ 1 Ca : 2 K 1 Ca : 2 K Same ratio

  18. Energy of adsorption Strong --------------------------------------Weak Al+3 > Ca+2 > Mg+2 > [K+ = NH4+ ] > Na+ > H+ (based on charge and hydrated radius)

  19. Soil pH importance • Determines solubility of nutrients • Before plants can get nutrients, they must be dissolved in soil solution • Microbial activity also depends on pH

  20. 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

  21. “Slightly acid” 6.0 – 6.6 “Moderately acid” 5.0 – 6.0 “Strongly acid” < 5.0 “Slightly basic” 7.4 – 8.0 “Moderately basic” 8.0 – 9.0 “Strongly basic” > 9.0 General soil pH conditions:

  22. 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)

  23. Causes of soil basicity • Hydrolysis of basic cations • Hydrolysis of carbonates

  24. 1. Hydrolysis of basic cations:(especially Ca+2, Mg+2, K+, NH4+, Na+) (also called exchangeable bases) Extent to which exchangeable bases will hydrolyze depends on ability to compete with H+ ions for exchange sites. Na Na Na Na + + OH- H2O Na H Na + Na Na Na Na

  25. K+ and Na+ are weakly held compared to Ca+2 and Mg+2. • Recall energy of adsorption So, K+ and Na+ are hydrolyzed easily and yield higher pHs .

  26. 2. Hydrolysis of carbonates(especially CaCO3, MgCO3, Na2CO3) • 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 H2O. • For those soils to become acid, all carbonates must be leached. • Basic cations replaced by Al+3 and H+ Ca+2 + HCO3- + OH- CaCO3 + H2O Na2CO3 + H2O Na + HCO3- + OH- (higher pH because Na more soluble)

  27. Causes of soil acidity • Accumulation of soluble acids • Exchangeable acids (Al+3, H+)

  28. Accumulation of soluble acidsat faster rate than they can be neutralized or removed • Carbonic acid (respiration and atmospheric CO2) b. Mineralization of organic matter (produces organic, nitric, sulfuric acids) Precipitation increases both a and b

  29. 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 + H2O AlOH+2 + H+

  30. 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

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