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Chemistry Lecture Exam 2 Results and New Homework Set

Check your exam results and get ready for the new homework set covering Cloud Chemistry, Precipitation Chemistry, and more topics. Focus on understanding cloud reactions, pollutants' incorporation, and cloud droplet formation. Practice problems provided for better grasp.

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Chemistry Lecture Exam 2 Results and New Homework Set

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  1. Chem. 250 – 11/18 Lecture

  2. Exam 2 Results Average = 73 New Homework Set (Text Ch. 4: 25; Ch. 7: 3, 5, 6, 8, 10, 24, 25, 26, 35, 44 + Furlough Questions) Announcements I

  3. Announcements - II • Topic Covering • Cloud Chemistry • Precipitation Chemistry • Hydrologic Cycle • Water Properties • Water Composition • Some of the above topics may be covered in the next lecture

  4. Announcements - III Rough Drafts due today (one copy to me + keep track of who receives other copies) Next Wednesday – Furlough Day - I will give a couple of additional homework problems for you to do as practice toward understanding of concepts (not collected or graded)

  5. Furlough Problems: • A cloud is nucleated on an aerosol containing 8.0 μg m-3 NH4HSO4 with 75% efficiency and reaches a LWC of 0.5 g m-3. The SO2 mixing ratio is present at 2.0 ppb. If P = 0.8 atm and T = 15ºC, calculate the pH of the cloud water. Calculate the pH independently for aerosol only acidity and SO2 only acidity and use only the source which adds the most acidity. Then determine the following: [H2SO3 (aq)], [HSO3-], [SO42-] • Derive the equation on slide 34.

  6. Cloud Chemistry • Rationale for Studying - Cloud reactions can be important (e.g. formation of H2SO4) - Precipitation composition depends on cloud composition - Provide introduction to aqueous chemistry

  7. Cloud Chemistry- Incorporation of Pollutants

  8. Cloud Chemistry- Incorporation of Pollutants • Main mechanisms - Nucleation of cloud droplets on aerosol particles - Scavenging of gases - Reactions within the droplet

  9. Cloud ChemistryNucleation of Cloud Droplets (some review?) • Cloud droplets can not form in the absence of aerosol particles unless RH ~ 300%. • Cloud droplets nucleate on aerosol particles at RH of ~100.1 to ~101%. • Cloud droplets should nucleate when RH = 100% except that the vapor pressure over a curved surface is less than that over a flat surface (due to water surface tension) • Smaller particles (d < 50 nm) have more curved surfaces and are harder to nucleate

  10. Cloud Chemistry- Nucleation of Cloud Droplets • Nucleation more readily occurs with: - Larger particles - Particles with more water soluble compounds (due to growth according to Raoult’s law) - Compounds that reduce surface tension - Smaller aerosol number concentrations (less competition for water so higher RH values)

  11. Cloud Chemistry- Nucleation of Cloud Droplets • The concentration of constituents incorporated from nucleation depends on the efficiency of nucleation and on the liquid water content (or LWC). • LWC = g liquid H2O/m3 of air • The higher the LWC, the lower the concentration (dilution effect) • Cloud nucleation leads to heterogeneous cloud droplet composition – Ignored here for calculations

  12. Cloud ChemistryNucleation Example Problems • Why is a RH over 100% required for cloud droplet nucleation? • Why is nucleation efficiency higher in less polluted regions? • An ammonium bisulfate aerosol that has a concentration of 5.0 μg m-3 is nucleated with 50% efficiency (by mass) in a cloud that has a LWC of 0.40 g m-3. What is the molar concentration? What is the cloud pH?

  13. Cloud Chemistry- Scavenging of Gases • Also Important for covering water chemistry (e.g. uptake of CO2 by oceans) • For “unreactive” gases, the transfer of gases to cloud droplets depends on: the Henry’s law constant (always) • In special cases, transfer can depend on LWC (if high), or can be limited by diffusion • Henry’s Law: where KH = constant (at given T) and X = molecule of interest

  14. Cloud Chemistry- Scavenging of Gases: “unreactive” gases • When LWC and KH are relatively low, we can assume that PX is constant Then [X] = KH∙PX • When KH is high (>1000 M/atm), conservation of mass must be considered (PX decreases as molecules are transferred from gas to liquid) • We will only consider 2 cases (low KH case and 100% gas to water case) • Example Problem (low KH case): What is the concentration of CH3OH in cloud water if the gas phase mixing ratio is 10 ppbv and a LWC of 0.2 g/m3? The Henry’s law constant is 290 M/atm (at given temp.). Assume an atmospheric pressure of 0.9 atm and 20°C.

  15. Cloud Chemistry- Scavenging of Gases “unreactive” gases • For compounds with high Henry’s law constants, a significant fraction of compound will dissolve in solution • fA = 10-6KHRT(LWC) where fA = aqueous fraction (not used in assigned problems) • When fA ~ 1, can use same method as for cloud nucleation From Seinfeld and Pandis (1998)

  16. Cloud Chemistry- Scavenging of Gases: “reactive” gases • Many of the gases considered are acidic and react further • Example: Dissolution of SO2 gas Reaction: Equation: SO2(g) + H2O(l) ↔ H2SO3(aq) KH = [H2SO3]/PSO2 H2SO3(aq) ↔ H+ + HSO3- Ka1 = [H+][HSO3-]/[H2SO3(aq)] HSO3- ↔ H+ + SO32- Ka2 = [H+][SO32-]/[HSO3-] Note: concentration of dissolved SO2 = [S(IV)] = [H2SO3] + [HSO3-] + [SO32-] = [H2SO3](1 + Ka1/[H+] + Ka1Ka2/[H+]2) “Effective” Henry’s law constant = KH* = KH(1 + Ka1/[H+] + Ka1Ka2/[H+]2) = function of pH

  17. Cloud Chemistry- Scavenging of Gases: “reactive” gases • For SO2 problems in homework, assume: • Little SO2 is depleted from gas phase (usually valid) (This means PSO2 and [H2SO3] are constant) • pH is just determined from SO2 (usually not valid) • The third reaction can be ignored (dissociation of HSO3- doesn’t affect pH) • Dissolution of HNO3 • Because both KH and Ka are large, we can not assume little HNO3 is depleted from gas phase • Better assumption is 100% transfer to aqueous phase

  18. Cloud Chemistry- Scavenging of Gases: “reactive” gases • Example problem: Determine the pH and aqueous NO3- concentration (in M) if air containing 1 ppbv enters a cloud with a pressure of 0.90 atm, a T = 293K, and a LWC of 0.50 g/m3. Assume 100% scavenging.

  19. Cloud Chemistry- Combining two scavenging methodsexample including ammonium bisulfate, sulfur dioxide and carbon dioxide Equilibrium pH where sum of anion charge = sum of cation charge Calculation method is fairly complex (uses systematic method)

  20. Cloud Chemistry- Reactions in Clouds • Cloud reactions are important for water soluble species because of higher concentrations in clouds • Only sulfur chemistry covered here

  21. Cloud Chemistry- Reactions in Clouds • Reaction of S(IV) and H2O2 - HSO3- + H2O2→ HSO4- + H2O (acid catalyzed) - Rate = k[HSO3-][H+][H2O2] - Rate = k’[H2O2]PSO2 - Effectively pH independent (despite what text says)

  22. Cloud Chemistry- Reactions in Clouds • Reaction of S(IV) and Ozone - Two main reactions: HSO3- + O3→ HSO4- + O2 moderately fast SO32- + O3→ SO42- + O2 fast reaction is faster at high pH because more S(IV) is present in reactive forms

  23. Cloud Chemistry- Reactions in Clouds

  24. Precipitation Chemistry • Precipitation Formation • Cloud droplets are collected by collisions with rain droplets or snow crystals and transfer their contents • Snow crystals also can form mainly through diffusion from water vapor and are very clean • Below Cloud Scavenging • Incorporation of gases or particles

  25. Cloud/Precipitation ChemistrySome Questions • Which reactant for sulfur dioxide oxidation is likely to be most important if a cloud is nucleated on a soil dust aerosol? on an acidic sulfate aerosol? • Two snow events occur down-wind of a pollution source. In one case, the snow is mostly crystals formed from diffusional growth. In the other the snow grew by removing cloud droplets. How will the snow composition be different?

  26. Water ChemistryHydrological Systems • Most of water on Earth is in the ocean • Much of the freshwater is inaccessible for use • Groundwater is becoming an increasingly important resource from Girard

  27. Water ChemistryHydrological Systems • The hydrologic cycle is the cycle by which water is distributed around the Earth • Evaporation removes most of the non-volatile constituents of water • For this reason, atmospheric source of many compounds are not large (although they are important atmospheric sinks) • As with clouds, regions of heavier precipitation tend to have greater “dilution” of pollutants • Water flowing through sediments can add or remove constituents from Girard

  28. Water ChemistryHydrological Systems Data From Chem. 31 N Sacramento Valley Groundwater?? sediments River Water?? granite Tap Water West East Transect

  29. Water ChemistryProperties of Water • See Text for boiling point/melting point and heat capacity properties • Temperature – Density Relationship: density maximum occurs at 4°C and ice density is much lower than water density • Note: if density increases with depth, water is stable. from Girard Kotz et al., “Chemistry and Chemical Reactivity” (6th Ed.)

  30. Water ChemistryProperties of Water • In the oceans, production of dense water that can sink occurs when warm water evaporates producing cool water with high salinity • This only occurs in two areas (near Iceland and near Antarctica) • The volume of deep water formed equals the volume of upwelling water

  31. Water ChemistryWater Composition • Salt Water - main ions are sodium (1.06%) and chloride (1.9%) with lower amounts of magnesium and sulfate - main compound affecting pH is HCO3- ion (a weak base) • Fresh Water - main ions are HCO3-, Mg2+, Ca2+, Na+, and Cl- - main source of major ions is dissolution of carbonates e.g. CaCO3(s) + CO2(g) + H2O(l) ↔ Ca2+ + 2HCO3-

  32. Water ChemistryWater Composition • Dissolved solids • Mass of material left after evaporating water • Expressed in ppm • Surrogate measure is electrical conductivity

  33. Water ChemistryChemical Reactions • Acid-Base Equilibria Dissociation of water (always important) H2O ↔ H+ + OH- Carbon dioxide reactions: 1) Acid-Base Reactions CO2 (g) ↔ CO2 (aq) KH = 0.0338 M/atm CO2 (aq) + H2O ↔ H+ + HCO3- Ka1 = 4.45 x 10-7 HCO3- ↔ H+ + CO32- Ka2 = 4.7 x 10-11

  34. Water ChemistryChemical Reactions • Acid-Base Properties – continued Note: If water is in contact with atmosphere, PCO2 = fixed value, so [CO2] = independent of pH Other equations useful for solving water chemistry equations: Mass balance: T = [CO2] + [HCO3-] + [CO32-] where T = total carbonate concentration Charge balance equation: Σ(zi*[cation]i) = Σ(zj*[anion]j) zi = charge of ion i

  35. Water ChemistryChemical Reactions • Form of carbonate as a function of pH The fraction of carbonate species α present in a single form (e.g. HCO3-) can be calculated as follows: The right part to the equation can be derived from equilibrium equations When pH < pKa1, CO2 is the dominant species, when pKa1 < pH < pKa2, HCO3- is the dominant species, and when pH > pKa2, CO32- is the dominant species

  36. Water ChemistryChemical Reactions 80% of US surface water

  37. Water ChemistryChemical Reactions • Second source of carbonate: dissolution or weathering of carbonate rock/soil CaCO3(s) ↔ Ca2+ + CO32- Ksp = 4.6 x 10-9 This reactions normally must be considered with other reactions (because in most waters, the pH is such that [HCO3-] >> [CO32-]) Problems normally can be solved using 1) the systematic method or 2) simplifying assumptions

  38. Water ChemistryChemical Reactions Example of simplifying assumption: Solubility of CaCO3 in pure water (no CO2 present) Water with carbonate soils is usually in regime where α(HCO3-) > α(CO2) > α(CO32-), so a more representative reaction would result in HCO3- By combining CaCO3(s) ↔ Ca2+ + CO32- with H+ + CO32- ↔ HCO3- and H2O ↔ H+ + OH- The following is obtained: CaCO3(s) + H2O↔ Ca2+ + HCO3- + OH- where: K = KspKw/Ka2 = 9.7 x 10-13 = [Ca2+ ][HCO3-][OH-] Assumption that [Ca2+] = [HCO3-] = [OH-] leads to [Ca2+] = solubility = 9.9 x 10-5 M pH = 10.00 Vs. solubility = 6.8 x 10-5 M and pH = 7.00 considering solubility reaction only

  39. Water ChemistryChemical Reactions Simplifying assumption when both CaCO3 and CO2 are present Combine simplified equation for CaCO3 solubility with first 2 CO2 reactions: CaCO3(s) + H2O ↔ Ca2+ + HCO3- + OH- and CO2 (g) + H2O ↔ H+ + HCO3- (and H+ + OH-↔ H2O) Net reaction: CaCO3(s) + CO2 (g) + H2O ↔ Ca2+ + 2HCO3- Notes: 1) increased CO2 leads to increased solubility 2) 2[Ca2+] = [HCO3-] expected

  40. Water ChemistryChemical Reactions From Harris, Quantitative Chemical Analysis, 6th Ed., 2003 Additional CO2 sources Low Carbonate Soils

  41. Water ChemistryChemical Reactions Buffering capacity and alkalinity Through their reactions carbonate soils buffer water from the addition of acids. Alkalinity is a measure of the buffering capacity of water. Alkalinity = mmol of acid that can be added to a 1 L water sample before the pH → 4.5. Alkalinity = [OH-] + 2[CO32-] + [HCO3-] (approximate) Alkalinity = [OH-] + 2[CO32-] + [HCO3-] – [H+] (better, but still approximate equation)

  42. Water ChemistrySome Problems • What are first and second largest reservoirs of water on Earth? • What two ions are the most prevalent in sea-water? • What three ions are the most prevalent in fresh water? • How do the three major ions in fresh water generally get into fresh water? • How do the concentrations of major ions in rain water compare with fresh water?

  43. Water ChemistrySome Problems - II • At 5°C, the water hydrolysis equilibrium constant is 2.0 x 10-15. What is the pH of pure water (no CO2, no other sources of trace species)? • Determine the solubility of CaCO3 in water in equilibrium with 380 ppm CO2. What is the pH of the water? What is its alkalinity? • Coral is largely CaCO3. As PCO2 goes up, what will happen to the solubility of coral in the ocean? What should happen to the pH of the ocean? What will happen to [Ca2+]?

  44. Water ChemistryOne last problem • A water sample has a measured alkalinity of 0.4 mM and a pH of 6.7. Determine the concentration of [OH-], [HCO3-], [CO32-], and [CO2].

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