Hypothetical elements A, B, C, and D form the divalent ions A²+, B²+, C²+, and D2+. The follow- ing equations indicate reactions that can, or cannot, occur. Use these data to arrange the metal ion/metal couples into a short redox couple table. T23U0 BAJ-35
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- Please help me out with making flowchart with thes steps. Write the result. Procedure 1. Place 20 drops of each of the following aqueous solutions to separate centrifuge tubes: 0.1M Cr (NO3)3, 0.1M Al (NO3)3, 0.1M Co (NO3)2, 0.1M Zn (NO3)2, 0.1M Mn (OH)2, 0.1M Ni (NO3)2, 0.1 M Fe (NO3)3. Make each solution basic by adding few drops of 6M NH4OH. Confirm using a litmus paper. 2. Add 5 drops of freshly prepared 6M (NH4)2S to each centrifuge tube. Place the samples in the centrifuge machine for 3 mins. After centrifuge record results. Decant the supernatant liquid of all the samples. 3. Add one drop of NH4OH in each centrifuge tubes. Add 20 drops of distilled water in each centrifuge tubes. Then add a few drops of 6M HCl in each solution. Place the samples in the water bath for 10 mins. After water bath, centrifuge the samples for 3 mins. 4. After centrifuge, add a few drops of 6M NH4Cl in each sample. Decant the supernatant liquid in each sample. 5. To the centrifuge containing…Why is it necessary to carry out the reduction of iron and then the titration, before goin on to the next sample? Procedure Weigh four (4) 0.3 g sample of the dried unknown into four 400 or 600 mL beakers. Add 50 mL of 6 M HCI to each sample beaker and heat in the fume hood until the solutions boil for 30 seconds or until the sample dissolves Obtain approximately 20 mL of stannous chloride solution (SnCl2) from the reagent hood Add SnCl2 to the hot unknown solution drop-wise with a disposable plastic pipet until the solution changes from yellow to light green Add three drops of SnCl2 solution in excess Remove the sample from the fume hood and cool the solution to room temperature (a room temperature tap water bath is OK but no ice) After cooling, rapidly add 10 mL of the saturated HgClh solution (obtained from the reagent hood). Allow the sample solution to stand for 3 minutes – a precipitate should form To the sample solution add 60 mL of 3 M H2SO4, 15 mL of 85% H3PO4 and 100 mL…3I- + OCl- + 2H+ ----> I3- + Cl- + H2: A 25.00 ml sample of liquid bleach was diluted to 1000 ml in a graduated flask. A 25 ml portion of the diluted sample was pipetted into an Erlenmeyer flask and treated with excess KI to oxidize OCl- to Cl- and I3- was produced at the end of the reaction. The released I3 was titrated with 0.09892 M Na2S2O3 and 8.96 ml was spent to reach the turning point besides the starch indicator. What is the percent by weight/volume of NaOCl in the bleach sample? (NaOCl:74.44 g/mol)
- 2.1 Calculate the pH of 1.0 M HC2H3O2 solution, using Ka = 1.7 × 10-5 . Begin this calculation by defining the variable x. List the pH answer as “theoretical pH” on the report sheet. Have the instructor check this answer and all subsequent calculations. To test your prediction, obtain about 35 mL 1.0 M HC2H3O2 and add to a clean, dry 50 mL beaker. Measure the pH of this solution. Be sure the electrode is properly submerged and gives a stable reading. Record the pH reading in the “Observed pH” column on the report sheet. The value should be within ± 0.2 pH units of the calculated value. From the experimental pH and beginning concentrations of the solution components, calculate the remainder of the entries across the table to pKa . Save this solution for Sections 2.3 and 2.6. 2.2 Calculate the pH of 0.10 M HC2H3O2 solution. List this answer as “theoretical pH” on the report sheet. Test your prediction by placing 5 mL of 0.10 M HC2H3O2 in a test tube and testing its…Balance and add phase labels to the following reaction for the sodium test: Na++Zn2++UO2+2+HC2H3O2+H2O⟶NaZn(UO2)3(C2H3O2)9(H2O)9+H+Asking for lab help Fe3+ (aq) + SCN- (aq) = FeSCN2+ (aq) + heat pale yellow redWe have a solution at equilibrium after mixing 10 drops of 0.10M FeCl3 (aq), 10 drops 0.10M KSCN (aq), and then adding enough deionized water to bring the whole thing up to 25mL. We then added 2mL of that solution to a test tube. If I add 2.0mL of deionized water to that test tube, following Le Chateiler's Principles, how should the equilibrium be expected to change? Please give a detailed explination as to why.
- Prepare 100.00 mL of a solution with ALL the following chemicals into together; CHEMICALS PROVIDED solid FeCl3 6H2O, iron(II) chloride hexahydrate (source of FeCl3) dilute hydrochloric acid in the rack – 3.0 M solid sodium salicylate – 99.7% assay Concentrations needed in the 100mL solution FeCl3: 0.020 M HCl: 0.050 M Salicylate (mg/L): 40.25 PLEASE SHOW HOW TO CALUATE AND WORK. The only equations you will need to use are the equations for molarity and dilutions.A. What is the characteristic color of ferric ions in solution? B. Why is the titration of the oxalate in the green salt with KMnO4 performed prior to carrying out the redox titration for iron content? (Why can’t you do them the other way – iron first then oxalate?) C. In a titration using 0.02000 M KMnO4 solution, the following data were obtained: Buret readings: FINAL = 15.31 mL INITIAL = 5.02 mL How many moles of KMnO4 were used?6. Why do we need to precipitate from a hot solution? 7. Why is the precipitating agent added all at once? 8. What is the purpose of adding 6M HCI in the sample solution? 9. Why do we need to test the washings with AgNO3? 10. What is done in an ignition process? 11. What is the product after the precipitate was ignited? 12. What are the advantages of performing ignition? 13. Cite the sources of errors for this experiment and explain how to possibly circumvent these kinds of problems.
- Which zinc solution is saturated? 1x10-5 M ZnCO3 (Ksp=1.0x10-10) 4.0x10-6M Zn(OH)2 (Ksp=3.0x10-16) 1.5x10-4M ZnC2O4 (Ksp=2.7x10-8) 4.0x10-13 M ZnS (Ksp=2x10-25)What is the coefficient for H+ after balancing the following reaction in acidic medium? (Please note that element X and Y are NOT Hydrogen, Oxygen or group 1 A, 2 A or 7 A elements. Also, because this is not a calculation, your answer should be a whole number, so do NOT write answer in 3 sig. figs.) XO4¯ + H2YO3 → X2+ + HYO4¯ HOW DO I SOLVE THIS NEED THE ANSER IN 20 MINUTES TRYING TO STUDY BEFORE MY TEST AT 3 THANKSWhich species is the best reducing agent? E° (V) S2O62-(aq) + 4 H+(aq) + 2 e− ➝ 2 H2SO3(aq) +0.569 Fe3+(aq) + e− ➝ Fe2+(aq) +0.771 VO2+(aq) + 2 H+(aq) + e− ➝ VO2+(aq) + H2O(ℓ) +1.00 N2O(aq) + 2 H+(aq) + 2 e− ➝ N2(g) + H2O(ℓ) +1.77 Group of answer choices N2 VO2+ H2SO3 Fe2+ S2O62− VO2+ Fe3+