Print version Updated: 23 January 2016 Lecture #1 Introduction: Course Administration and Chemistry Review (Stumm & Morgan, Chapt. 1) (pp.1-4) (Benjamin, 1.1 & 1.4) David Reckhow CEE 680 #1 1 Course Administration Course Syllabus Textbook: Benjamin, Water Chemistry, Waveland Press, 2010 must read, not all topics may be covered Detailed Course Outline Homework policy most graded; Projects MINEQL, review of literature Web site David Reckhow CEE 680 #1 2 Other References 1. Pankow, Aquatic Chemistry Concepts. Lewis Publ., Chelsea, MI, 1991 2. Stumm & Morgan, Aquatic Chemistry. 3rd Ed., John Wiley & Sons., 1995 Extra copy on shelf in 3rd floor Elab II office UM Science GB855 .S78 1996 3. Jensen, A problem Solving Approach to Aquatic Chemistry, Wiley, 2003. UM Science GB855 .J46 2003 4. Sawyer, McCarty & Parkin, Chemistry for Environmental Engineering, McGraw Hill, 2003. Extra copy of 3rd edition on shelf in 3rd floor Elab II office 5. Snoeyink & Jenkins, Water Chemistry, John Wiley & Sons., 1980. David Reckhow UM Science QD169.W3 S66 CEE 680 #1 3 General Questions for Aquatic Chemists What is the chemical composition of natural waters? Will it change with time, location? What happens to chemical species when they enter new aquatic or non-aquatic environments? How does transport affect the chemistry? What types of reactions occur in treatment systems? What do we need to do to make it work better? David Reckhow CEE 680 #1 4 Examples from Water Treatment How can we use chemistry to stop corrosion and dissolution of lead? What with the pH, alkalinity and hardness be after mixing two different types of water e.g., groundwater and surface water How do we get the best performance from chemical precipitation processes e.g., coagulation, softening What can we do to optimize oxidation treatments e.g., removal of Mn, trace organic constituents David Reckhow CEE 680 #1 5 Example 1: Lead and Water Lead is a neural toxin Especially serious in children EPA: Pb & Cur Rule Published in 1991 The treatment technique for the rule requires systems to monitor drinking water at customer taps. If lead concentrations exceed an action level of 15 ppb or copper concentrations exceed an action level of 1.3 ppm in more than 10% of customer taps sampled (i.e., 90%ile), the system must undertake a number of additional actions to control corrosion. David Reckhow CEE 680 #1 6 Flint Michigan Crisis Timeline April 2014: the city stopped getting its water from Detroit as a cost-saving measure and began instead drawing water from the Flint River. High blood lead levels noted in children Water led levels were above standard Oct 16, 2015: Flint switches back to Detroit Water Sources VPI website: http://flintwaterstudy.org/ 12/22/2015 Rachel Maddow video: David Reckhow CEE 680 #1 7 Flint Water Quality - Edwards Parameter Before 4/2014 After 4/2014 units pH 7.38 7.61 Hardness 101 183 mg-CaCO3/L Alkalinity 78 77 mg-CaCO3/L Chloride 11.4 92 mg/L Sulfate 25.2 41 mg/L CSMR 0.45 1.6 Inhibitor 0.35 None Larson Ratio 0.5 2.3 mg-P/L WQ data From MOR and 2014 WQR CSMR = chloride to sulfate mass ratio Larson Ratio = ([Cl-] + 2[SO4-2])/[HCO3-] David Reckhow CEE 680 #1 8 Edwards slide David Reckhow CEE 680 #1 9 Daily Hampshire Gazette: 22 Jan 2013 das David Reckhow CEE 680 #1 10 Daily Hampshire Gazette: 22 Jan 2013 Environmental Justice issue David Reckhow CEE 680 #1 11 Example 2: differing water quality Many, perhaps most, drinking water utilities have multiple sources Often those sources have contrasting water quality Especially common for regional supplies, like Tampa Bay David Reckhow CEE 680 #1 12 Groundwater and surface water Tampa Bay area and regional supply Groundwater River water Ocean water: desal David Reckhow CEE 680 #1 13 Pinellas County Water Standard WQ Analyte List (103 total) 1,1-Dichloro-2propanone Bromochloroacetonitrile Total Haloacetic Acids (HAA5) sec-Butylbenzene Chloropicrin Trichloroacetic acid Dichlorodifluoromethane Styrene Decafluorobiphenyl Alkalinity as CaCO3 1,1-Dichloroethylene 4-Isopropyltoluene Ethylbenzene tert-Butylbenzene Dibromoacetonitrile Total Hardness 1,1-Dichloropropene Benzene Fluorobenzene Tetrachloroethylene Dichloroacetonitrile Total Dissolved Solids cis-1,3Dichloropropene Dibromochloro2,2-Dichloropropane methane Calcium 1,1,1-Trichloroethane 1,4-Dichlorobenzene n-Propylbenzene Iron 1,1,2,2Tetrachloroethane ortho-Xylene Magnesium 1,1,2-Trichloroethane 2-Chlorotoluene Dibromomethane Arsenic 1,1-Dichloroethane Copper Lead Bromide Chloride Nitrate as N Nitrite as N 1,2,3Trichlorobenzene 1,2,4Trichlorobenzene 1,2,4Trimethylbenzene 4-Chlorotoluene Bromobenzene Bromochloromethane Isopropylbenzene Bromodichloromethane 1,2-Dichlorobenzene Bromoform Orthophosphate as P 1,2-Dichloroethane Hexachlorobutadiene Toluene meta/para-Xylene Methyl bromide Carbon tetrachloride Methyl chloride Total Trihalomethanes trans-1,2Dichloroethylene trans-1,3Dichloropropylene Total Haloacetonitriles Ammonia as N Trichloroacetonitrile Free Ammonia as N Chloral hydrate Total Organic Carbon Decafluorobiphenyl UV 254 1,2,3Trichloropropane Trichlorofluorometha 2-Bromopropionic ne Acid Heterotrophic Plate Count Total Coliforms Trichloroethene Orthophosphate as PO4, calculated 1,2-Dichloropropane Chlorobenzene Methylene chloride Sulfate 1,3,5Trimethylbenzene Methyl tert-butyl ether Vinyl chloride Bromoacetic acid Phosphorus, Total (as P) 1,3-Dichlorobenzene Chloroform Naphthalene Xylene (total) Chloroacetic acid n-Butylbenzene CEE 680 #1 1,1,1-Trichloro-2propanone Dibromoacetic acid Chloroethane 1,1,1,2cis-1,2David Reckhow 1,3-Dichloropropane Dichloroethylene Tetrachloroethane Dichloroacetic acid E. coli 14 Keller 2 Groundwater source: Eldridge Wilde Wellfield 40 MGD WQ Challenge 1-1.5 ppm H2S, VOCs Water Treatment Air Stripping with CO2 Chlorination Ammoniation Polyphosphate Air treatment Water scrubbing with caustic & chlorine David Reckhow CEE 680 #1 15 Majors – mostly inorganics Keller Plant 2 Sample Station: Aug 9, 2010 Parameter Calcium Value Units Parameter 77.7 mg/L Sulfate 0.018 mg/L Phosphorus, Total (as P) 5.08 mg/L Arsenic 0.0002 Copper Lead Value Units 4 mg/L 0.23 mg/L Alkalinity as CaCO3 209 mg/L mg/L Total Hardness 215 mg/L 0.0013 mg/L Total Dissolved Solids 316 mg/L 0.0001 mg/L Ammonia as N 0.84 mg/L Bromide 0.05 mg/L Free Ammonia as N 0.16 mg/L Chloride 22 mg/L Total Organic Carbon 3.7 mg/L 0.04 mg/L UV 254 0.117 cm - 1 Nitrite as N 0.02 mg/L Heterotrophic Plate Count 3 CFU/ml Orthophosphate as P 0.12 mg/L E. coli 1 MPN/100ml Orthophosphate as PO4 0.37 mg/L Total Coliforms 1 MPN/100ml Iron Magnesium Nitrate as N David Reckhow CEE 680 #1 16 Trace Organics above MDL Keller Plant 2 Sample Station: Aug 9, 2010 Parameter Bromodichloromethane Value Units Parameter Value Units 8.3 ug/L Dibromoacetonitrile 0.77 ug/L 45 ug/L Dichloroacetonitrile 10.7 ug/L 0.9 ug/L Total Haloacetonitriles 13.3 ug/L Total Trihalomethanes 54.2 ug/L Trichloroacetonitrile 0.12 ug/L 1,1,1-Trichloro-2-propanone 3.47 ug/L Chloral hydrate 5.45 ug/L 1,1-Dichloro-2-propanone 1.36 ug/L Dichloroacetic acid 12.6 ug/L Bromochloroacetonitrile 1.73 ug/L Total Haloacetic Acids (HAA5) 31.8 ug/L Chloropicrin 0.21 ug/L Trichloroacetic acid 19 ug/L Chloroform Dibromochloromethane David Reckhow CEE 680 #1 17 Pinellas Questions What does the detailed analysis tell you? Does it make sense? Expressions of concentration? Principle of electroneutrality? TDS, TH, Alk, TOC, UV – what do these mean David Reckhow CEE 680 #1 18 Pinellas calculations 1 Calcium Iron Magnesium Arsenic Copper Lead Bromide Chloride Nitrate as N Nitrite as N Orthophosphate as P Orthophosphate as PO4, calculated Sulfate Phosphorus, Total (as P) Alkalinity as CaCO3 Total Hardness Total Dissolved Solids Ammonia as N Free Ammonia as N Total Organic Carbon UV 254 Heterotrophic Plate Count E. coli Total Coliforms conc (mg/L) 77.70 0.02 5.08 0.00 0.00 0.00 0.05 22.00 0.04 0.02 0.12 77.7 mg/L 0.018 mg/L 5.08 mg/L 0.0002 mg/L 0.0013 mg/L 0.0001 mg/L 0.05 mg/L 22 mg/L 0.04 mg/L 0.02 mg/L 0.12 mg/L 0.37 mg/L 4 mg/L 0.23 mg/L 209 mg/L 215 mg/L 316 mg/L 0.84 mg/L 0.16 mg/L 3.7 mg/L 0.117 cm - 1 0.37 4.00 0.23 209.00 215.00 316.00 0.84 0.16 3.70 GFW mM charge/M meq/L pos neg 40.078 1.9387 2 3.87744 3.87744 55.845 0.0003 3 0.00097 0.00097 24.305 0.2090 2 0.41802 0.41802 74.922 0.0000 -1 0.00000 0.00000 63.546 0.0000 2 0.00004 0.00004 207.2 0.0000 2 0.00000 0.00000 79.904 0.0006 -1 -0.00063 -0.00063 35.453 0.6205 -1 -0.62054 -0.62054 14.007 0.0029 -1 -0.00286 -0.00286 14.007 0.0014 -1 -0.00143 -0.00143 30.974 0.0039 -3 -0.01162 -0.01162 94.97 96.061 30.974 50.037 100.074 0.0039 0.0416 0.0074 4.1769 2.1484 14.007 14.007 12.011 0.0600 . 0.0114 0.3081 -3 -2 -0.01169 -0.08328 0.00000 -4.17691 4.29682 . -1 2 -0.08328 -4.17691 . 1 0.01142 0.00000 0.01142 0.00000 3 CFU/ml 1 MPN/100ml 1 MPN/100ml Total = 854.33 add 323.33 exclude TDS, TH sum diff % David Reckhow . CEE 680 #1 4.30789 -4.89726 -0.58937 12.0% 19 Pinellas calcs 2 mass of E. coli 0.5 um 2 um cylinder volume = density = 0.3927 um3 = 3.927E-10 mm3 = 3.93E-13 g = 1 in 3.93E-10 mg 100 mL mass concentra tion = 3.93E-09 mg/L = HPC example conc = 3 in mass concentra tion = David Reckhow 3.927E-13 cm3 1 g/cm3 mass/cell = E.coli example conc = diameter long 3.93E-06 ug/L = 3.93E-03 ng/L 1.18E-03 ug/L = 1.18E+00 ng/L 1 mL 1.18E-06 mg/L = CEE 680 #1 20 Pinellas Discussion Missing Na, K 13.5 mg/L Na would close the balance David Reckhow CEE 680 #1 21 Relation with Environmental Engineering Math Environmental Engineering Biology Physics Chemistry David Reckhow CEE 680 #1 22 Relation with other Chemistry Disciplines Physical Chemistry Analytical Chemistry Inorganic Organic Chemistry Chemistry Chemistry 680 Thermodynamics 684 Kinetics A cornerstone of the good grad programs in our field David Reckhow CEE 680 #1 23 Review Units Mass based Molarity Molality Normality Mole fraction Atmospheres David Reckhow CEE 680 #1 Chemical Stoichiometry mass balance balancing equations Thermodynamics law of mass action types of equilibria 24 SI Unit prefixes Factor Prefix Symbol 10-1 deci d 10-2 centi c 10-3 milli m 10-6 micro µ 10-9 nano n 10-12 pico p 10-15 femto f 10-18 atto a David Reckhow CEE 680 #1 Factor 101 102 103 106 109 1012 1015 1018 Prefix deka hecto kilo mega giga tera peta exa Symbol da d k M G T P E 25 Mass Based Concentration Units Solid samples 17.5mg Pb 17.5 x10 −3 g Pb 17.5 g Pb = = 6 3 g soil 10 1kg soil 1x10 g soil = 17.5 ppm m Pb in soil 1mg / kg = 1 ppmm 1µg / kg = 1 ppbm David Reckhow CEE 680 #1 26 Liquid samples Density of Water at 5ºC 0.35mg Fe 1L water x 3 1L water 10 g water 0.35mg Fe 0.35 x10 −3 g Fe 0.35 g Fe = 3 = = 6 3 10 g water 10 g water 10 g water = 0.35 ppm m Fe in water David Reckhow CEE 680 #1 27 Mass/Volume Units Mass/Mass Units Typical Applications g/L (grams/liter) mg/L (milligrams/liter) 10-3g/L µg/L (micrograms/liter) 10-6g/L ng/L (nanograms/liter) 10-9g/L pg/L (picograms/liter) 10-12g/L (parts per thousand) ppm (parts per million) ppb (parts per billion) Stock solutions Conventional pollutants (DO, nitrate, chloride) Trihalomethanes, Phenols. ppt (parts per trillion) PCBs, Dioxins David Reckhow CEE 680 #1 Pheromones 28 Gas samples (compressible) 0.056mg Ozone 1m 3 air Could be converted to a ppmm basis But this would change as we compress the air sample Could also be converted to a ppmv basis Independent of degree of compression But now we need to convert mass of ozone to volume of ozone David Reckhow CEE 680 #1 29 Ideal Gas Law By definition: mass ( g ) n= GFW An ideal gas Will occupy a certain fixed volume as determined by: PV = nRT RT mass ( g ) RT V =n = P GFW P regardless of the nature of the gas Where: David Reckhow P=pressure =22.4 L V=volume at 1 atm, 273.15ºK n=number of moles T=temp R=universal gas constant=0.08205 L-atm/mole-ºK GFW=gram formula weight CEE 680 #1 30 Convert mass to moles Now we know that ozone’s formula is O3 Which means it contains 3 oxygen atoms Therefore the GFW = 3x atomic weight of oxygen in grams or 48 g/mole 0.056mg Ozone 3 1m air David Reckhow n=mass(g)/GFW n=0.056x10-3g/(48g/mole) n=0.00117x10-3 moles CEE 680 #1 0.00117 x10 −3 moles Ozone 1m 3 air 31 Now determine ppmv volumeozone ppmv = volumeair 0.00117 x10 −3 moles x 22.4 L / mole = 1m 3 air 0.026 x10 −3 L Ozone = 1x103 L air = 0.026 ppm v O 3 in air = 26 ppb v O 3 in air David Reckhow CEE 680 #1 32 Mole & volume fractions Based on the ideal gas law: RT Vi = ni P RT Vtotal = ntotal P The volume fraction (ratio of a component gas volume to the total volume) is the same as the mole fraction of that component Vi ni = Therefore: V n total total Defined as: Volume fraction Defined as: mole fraction And since the fraction of the total is one-millionth of the number of ppm: David Reckhow CEE 680 #1 Vi ni 10 ppmv ≡ = Vtotal ntotal −6 33 PV = nRT n P = RT V Partial pressures Based on the ideal gas law: And defining the partial pressure (Pi) as the pressure a component gas (i) would exert if all of the other component gases were removed. We can write: ni Pi = RT Vtotal Which leads to: Pi ni = Ptotal ntotal ni = Ptotal 10 −6 ppmv ntotal And: David Reckhow Pi = Ptotal CEE 680 #1 and Ptotal ntotal RT = Vtotal 34 Earth’s Atmosphere David Reckhow CEE 680 #1 Divide by 100 and you get the partial pressure for a total pressure of 1 atm. 35 To next lecture David Reckhow CEE 680 #1 36