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- What is the dominant iron species in water samples ? What environmental factors may have contributed. why is it necesseyy to to investigate Fe3+ concentration and total Fe concentration dpeedtaely ? Why do we need to do the sample to determine total Fe concentration ? And how did then determine Fe2+ concentration?An alkaline sample of sodium compounds weighing 1.196 g was dissolved in water, cooled to 15°C, treated with 2 drops of Pp indicator and titrated with 1.058 N H2SO4 requiring 6.8 ml to render the solution colorless. Upon adding 2 drops of MO and continuing the titration, 16.5 ml more of the acid were needed to complete the analysis. What is the quantitative composition of the sample? MW: NaOH = 40.0, Na2CO3 = 106.0, NaHCO3 = 84.01A 4.912-g sample of a petroleum product was burnedin a tube furnace, and the SO2produced was collectedin 3% H2O2.Reaction:SO2(g)+H2O2→H2SO4A 25.00-mL portion of 0.00873 M NaOH was introducedinto the solution of H2SO4, following whichthe excess base was back-titrated with 15.17 mL of0.01102 M HCl. Calculate the sulfur concentrationin the sample in parts per million.
- The first step in purifying the urine collected on the ISS is to treat every liter of urine with 20 mL of 1.0 M H2SO4. To simplify the calculations, lets assume that urine is water. a) What is the pH of a solution of 20. mL of 1.0 M H2SO4 added to 1.00 L water? To determine this, you can safely assume that 100% of the H2SO4 reacts to form H3O+ and HSO4- ions. Use pKa2 (1.92) to determine if any more protons are added to the solution from HSO4-.1. Write the reaction involved in Ferrox Test. a. What is the species responsible? 2. Why is phenol negative in Ferrox Test?Would you expect calcite to be appreciably soluble in a solution whose pH is maintained at 4? A solution at pH? A solution containing 0.1 m H2S? where might you find such solutions in nature?
- Given this series of equilibrium reactions. See Image(a) Which way should the reaction to “tend” at high pH? Why?(b) Which way should the reaction to “tend” at low pH? Why? (c) What Fe(III) species would be least soluble?Explain how (the dreaded chemistry) the addition of alum decreases alkalinity and tends to lower the pH of the treated water. (you may want to have a separate slide or graphic to help you explain this).(i) How does O3react with lead sulphide? Write chemical equation.(ii) What happens when SO2is passed in acidified KMnO4solution?(iii) SO2 behaves with lime water similar to CO2.
- Why alkali is added to the nitrification tank? A. to provide electron donors B. to provide alkalinity for the nitrification reaction C. to acidify the reaction solution D. to provide nutrients for the nitrifier bacteriaWhen creating Alum KAl(SO4)2.H20: 30 mL of 6.0 M sulphuric acid was added to 50 mL solution of Al foil and 1.5 M KOH. Next, the solution was gently boiled until there was a volume of 50 mL. Why is the solution boiled down to 50 mL? Why isn’t it boiled dry so that all of the alum recovered?There are two different types of reactions that NaI might undergo with concentratedsulfuric acid in Part E. Describe and write balanced equations for both possibilities. From Part E: Reactions with NaI and NaCl17. CAUTION: 18 M H2SO4 is extremely caustic. Handle it with care.18. This part will utilize the “Testing for an Acidic or Basic Gas” technique described in Appendix B.1419. Collect about 2 dropper’s worth of 18 M H2SO4 in a small tube and take it to your workstation for this part;don’t perform the following reactions in the main hood where this acid is kept.20. Place a small quantity (about the same amount of solid used for part D above) of NaI in a clean dryevaporating dish. Place the same amount of NaCl in a separate dish.23. Lift one of the watch glasses just enough to add one dropper’s worth* of 3 M H2SO4 to the salt inside andthen quickly replace it.25. Clean the dishes out and set them up as you did before with solid NaI and NaCl, and fresh pieces of litmuspaper. Add acid…