CE 428 Water and Wastewater Treatment Design Lime Softening Dr. S.K. Ong Hardness in water is caused by the presence of polyvalent metallic cations such as calcium, magnesium, aluminum, iron and strontium. Most prevalent cations are calcium and magnesium. Usually expressed as mg/L as CaCO3 or meq/L In most waters Total Hardness = __________________________________ Hardness classification scale Hardness range (mg/L as CaCO3) 0 – 75 75 – 150 150 – 300 > 300 Water Description _________________ Hardness (temporary hardness) – hardness that are associated with bicarbonate and carbonate ions or alkalinity _______________ Hardness (permanent hardness) - hardness that are associated with sulfate, chloride and silicates or the difference between total hardness and carbonate hardness i.e., Noncarbonate Hardness = ____________________________________ If total hardness is equal or less than alkalinity then and Total hardness = _________________ Noncarbonate Hardness = ___________________ Example: Water Analysis Ca2+ Mg2+ Na+ = 75 mg/L = 40 mg/L = 10 mg/L HCO3CO32ClSO42- = 300 mg/L = 0 mg/L = 10 mg/L = 109 mg/L Draw a bar chart and estimate the total hardness, carbonate hardness and noncarbonate hardness in mg/L as CaCO3 Conc. (mg/L) Ca2+ Mg2+ Na+ 75 40 10 HCO3ClSO42- 300 10 109 Equivalent wt Conc (meq/l) Bar Diagram (Cations on the top row – start with Ca2+ followed by Mg2+, Na+ Anions on the bottom row – start with OH-, CO32-, HCO3-, SO42-, Cl-) Conc (mg/L as CaCO3) Total hardness = _____________ = ________________mg/L as CaCO3 Alkalinity = bicarbonate alkalinity = ______________ mg/L as CaCO3 Carbonate Hardness = alkalinity = ________________ mg/L as CaCO3 Noncarbonate Hardness = _____________ = _________ mg/L as CaCO3 Removal of Hardness (i) chemical precipitation using lime and soda ash (ii) ion exchange – exchange of ions in solution for other ions on the ion exchange resin (iii) membrane processes – separate dissolved constituents from water using pressure (reverse osmosis), electrical gradient with a membrane (electrodialysis) Chemical Precipitation - Lime Softening Process - removal of calcium and magnesium by precipitation - examples of solubility of various calcium and magnesium compounds (solids) at 25o C. CaCO3 Ca(OH)2 CaSO4 CaCl2 mg/L 18 770 1620 745,000 Mg(OH)2 MgCO3 MgSO4 mg/L 40 727,000 738,000 See Attached chart for chemical reactions With lime softening, hardness cannot be removed completely because of the solubility of calcium carbonate and magnesium hydroxide. The minimum practical limits are calcium = 30 mg/L of CaCO 3 and magnesium = 10 mg/L as CaCO3. 3 Basic Schemes to produce finished water with desired hardness: (i) ________________________ – providing enough lime to precipitate the calcium only, usually done when the Mg is < 40 mg/L as CaCO3, single stage system (ii) ___________________________ - excess lime added, can be one or two stages (iii) __________________________ Excess Lime Treatment - addition of surplus lime, normally about 35 mg/L of CaCO3 above stoichiometric requirements, will bring the pH up to 11.0 2 ________________________________________________________________________________________________________________________________ Species Conc. Reactions Comments Lime and Soda Ash Needs and Solids Produced (meq/L) _________________________________________________________________________________________________________________________________ Lime needed Soda Ash Solids Produced _______________________________________________________________________________________(meq/L)________(meq/L)_________(meq/L)_____ CO2 X1 CO2 + Ca(OH)2 => CaCO3 +H2O Ca(HCO3)2 X2 Mg(HCO3)2 X3 MgSO4 X4 CaSO4 X5 CO2 not part of hardness but consumes Ca(OH)2 X1 0 X1 (CaCO3) Ca(HCO3)2 + Ca(OH)2 => 2CaCO3 + 2 H2O X2 0 2X2 (CaCO3) Mg(HCO3)2 + Ca(OH)2 => CaCO3 + MgCO3 + H2O X3 0 X3 (CaCO3) MgCO3 + Ca(OH)2 = > Mg(OH)2 + CaCO3 X3 0 X3 (CaCO3) X3 (Mg(OH)2) MgSO4 + Ca(OH)2 => Mg(OH)2 + CaSO4 X4 0 X4 (Mg(OH)2) CaSO4 + Na2CO3 => 0 X 4 + X5 X5 (CaCO3) CaCO3 + Na2SO4 _____________________________________________________________________________________________________________________________ ___ Total Lime needed = X1 + X2 + 2X3 + X4 + excess (if any) Total Soda Ash = X4 + X5 Sludge produced = X1 + 2 X2 + 2 X3 + X5 of CaCO3 and X3 + X4 of Mg(OH)2 Lime Softening Example Determine the amount of lime (CaO) and soda ash (Na2CO3) needed to soften the following water. Assume excess lime is used. Estimate the approximate water quality after softening and recarbonation. Flow rate = 10 5 m3/day - practical limits : Ca2+ at 30 mg/L as CaCO3 Mg2+ at 10 mg/L as CaCO3 - excess lime added - 35 mg/L as CaCO3 or 0.7 meq/L - assume recarbonation converts one-half of the remaining alkalinity to bicarbonate ions. Useful information Water Analysis Components CO2 Ca2+ Mg2+ Na+ Alkalinity SO42Cl- mg/L 8.8 70 9.7 6.9 115 mg/L as CaCO3 96 10.6 Equiv. Wt. Plot Bar Graph meq/L Lime Soda ash CO2 Ca(HCO3)2 CaSO4 MgSO4 __________________________________________________________ _____________________________________ Lime required = ____________________________________ Soda ash required = _________________________________ 4 meq/L Ions Removal by Ion Exchange ● Use of naturally occurring porous materials (___________________) or synthetic resins (ion exchange resins) with functional groups which the capacity of preferentially sorbing certain ions in solutions and at the same time release replacement ions back into the water ● Ion exchange resins are used for ________________ and __________________ of water (producing pure water). ● Most resins have a structure of polymer (styrene or divinylbenzene) with functional groups : ● Cation exchange resins Strong acid cation exchange (functional groups – SO3-) Weak acid cation exchange (functional groups – COO-) Anion exchange resins Strong base anion exchange (functional groups – R N+) Weak base anion exchange (functional groups – R NH3+) where R is the polymer base Softening Regeneration: R2Ca + 2 Na + = > 2 R- Na + Ca2+ R2 Mg + 2 Na+ = > 2 R – Na + Mg2+ Certain ions (Fe2+ and Fe3+) cannot be easily removed and eventually the resin cannot be fully regenerated. Demineralization Use strong acid cation and strong base anion resin Cation x R - SO3 H + Mx+ == > (R SO3)x M + x H+ Anion z R - OH + Az - == > Rz A + z OH- Where Mx+ and Az - are cations and anions. Final water in terms of H+ and OH-. Regenerate the cation resin with strong acid (HCl or H2SO4) and anion resin with a strong base (NaOH). 5