E) In anoxic conditions (e.g. Ен= -0.3 V and pH=8) trace metals form very insoluble sulfides. Would it make sense to treat water to anoxic conditions to eliminate dissolved Hg? 1. What is the balance of sulfates/sulfides species? 2. Make a Pourbaix diagram for sulfate/sulfide species. 3. What other minerals can precipitate? (Hint: use the concentration of sulfides computed in the previous step, recompile the matrix using S²- and without e¯ and check for precipitation Hg + S minerals)
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- This is an unknown solution which comprises of several ions possible for analysis. From the given information, determine which ions are present. Use + for positive, - for negative, or ? for insufficient information. An unknown solution containing the ions listed to the right was found: For Group I Cations: 1). A white precipitate was generated when 2 drops of 6M HCl solution was added to the unknown solution test tube. 2). Di water was added to the solution from part 1, and then the ppt was separated from the supernatant. The ppt was then washed with DI water few times to make sure is ppt is clean. 3). On the ppt separated from part 2 excess 6M NH3 was added and as a result all the ppt was dissolved. For Group III Cations: 4). An addition of Excess 6M NH3 led to a basic solution and a ppt. The ppt was then separated from the supernatant. 5). When Excess 6M NaOH was…Solve the following problem: Calamine, which is used to relieve skin irritations, is a mixture of zinc and iron oxides. A 1.056 g sample of dry calamine was dissolved in acid and diluted to 250.0 mL. Potassium fluoride was added to a 10.00 mL aliquot of the diluted solution to mask the iron. After adjusting the pH, the Zn2+ consumed 38.37 mL of EDTA 0.01133 M. A second aliquot of 50.00 mL was buffered and titrated with 2.30 mL of a solution of ZnY2- 0.002647 M: Fe3+ + ZnY2- → FeY- + Zn2+ Calculate the percentages of ZnO and Fe2O3 in the sample.Why is it less desirable to wash AgCl precipitate with aqueous NaNO3 than with HNO3 solution?
- While pipetting the solution at approximately 50.0 C you don't move fast enough and notice that the KHP is crystallizing inside the pipet. How would this change your Ksp value if you were to titrate this solution?For µ=0.1, the activity coefficient (gamma) of M2+ is 0.41 while gamma of X- is 0.75. Calculate how many micrograms of MX2 dissolve in 324 mL of 0.10 M NaX solution. The molar mass of MX2 is 201 g/mol, and its Ksp is 3.8 x 10-9. Note that NaX is a salt of X-, an ion that participates in the equilibrium that applies to the solubility of MX2. a. 110 µg b. 27 µg c. 9.7 µg d. 44 µg e. 1000 µgQuestion: How do you expect solubility of potassium bitartrate to vary between solutions with and without KNO3?
- 100 mL of mineral water containing Mg2+ and Ca2+ is taken and titrated with 86.65 mL of 0.06120 M EDTA. NH4F was added to the second 100 mL portion taken from the mineral water to mask the magnesium in the sample as MgF2, and when this sample was titrated with the same EDTA solution, 38.56 mL was spent. Find the concentration of CaCO3 and MgCO3 in the sample in ppm.A piece of Gold weighing 12,359 Kg is suspected of being contaminated with Iron. To perform an instrumental analysis and To confirm whether or not it contains Fe, a portion of the sample (0.954 g) is taken from the piece and dissolved with 25 mL of aqua regia. Heats up For its complete dissolution, it is cooled and made up to 100 mL. A 10 mL aliquot is taken from this solution and made up to 50 mL. From This last solution is given the appropriate treatment to visualize Fe+2, for which the 1,10-phenanthroline reagent is added. (it forms a complex that is red in color) and is taken to a visible spectrophotometer and with a 12 mm cell a absorbance of 0.45. Previously, a calibration curve of Fe+2 was obtained under the same instrumental conditions obtaining the following data: (view table) Calculate the purity of the gold piece, assuming impurities only due to Fe.Is this for Average Molarity of EDTA Standard Solution? Then, would it be always the same with average Molarity of EDTA? How about the Ca Titer (mg Ca/mL of EDTA Solution? Show step by step solution.
- Using basic conditions, MnO4- can be used as titrant for the analysis of Mn2+, with both the analyte and the titrant ending up as MnO2. In the analysis of a mineral sample for manganese, a 0.5165-g sample is dissolved, and the manganese is reduced to Mn2+. The solution is made basic and titrated with 0.03358 M KMnO4, requiring 34.88 mL to reach the endpoint. Calculate the %w/w Mn in the mineral sample. Answer: % Mn =For an insoluble metallic salt, Ksp will always be less than 1. True or False.a) When considering the overall dialysis procedure, why is it important to exchange old/used dialysis buffer (or “dialysate” solution) with a fresh dialysis buffer solution at least once throughout the process? NOTE: Your TAs will do this for your group’s samples over the next week. b) This week’s lab utilizes a dialysis buffer with the following composition: 10 mM Tris-HCl, 10 mM MgSO4, and a pH of 7.4. Let’s presume an ERROR occurred with the creation of this buffer during the pH titration and you unknowingly titrated to a final pH of 5.0. What effects, if any, could you expect to observe on your final, dialyzed sample?