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- The accompanying data (1.00-cm cells) were obtained for the spectrophotometric titration 10.00 mL of Pd(II) with 2.44 10-4 M Nitroso R(O. W Rollins and M. M. Oldham, Anal. chem .,1971, 43, 262, DOI: 10.1021/ac60297a026). Calculate the concentration of the Pd(II) solution, given that the ligand-to-cation ratio in the colored product is 2:1Given the Information that Fe3++Y4FeYKi=1.01025Cu2++Y4CuY2Ki=6.31018 and the further information that, among the several reactants and products, only CuY2- absorbs radiationat 750 nm, describe how Cu(II) could be used as an indicator for the photometric titration of Fe(III) with H2Y2-. Reaction:+ Fe3++ H2Y2- FeY- + 2H+.A 0.1017-g sample of KBrO3 (MW = 167 g/mole) was dissolved in dilute HCl and treated with an unmeasured excess of KI. The liberated iodine required 39.75 mL of a sodium thiosulfate solution. Calculate the molar concentration of the Na2S2O3. BrO3 - + 6I + 6HCl → Br - + 3I2 + 6KCl + 3H2O I2 + Na2S2O3 → 2NaI + Na2S4O6 The type of redox titration reaction is ___. a. iodimetry b. bromination c. iodometry d. diazotination The role of KBrO3 in the titration is ___. a. reducing agent b. oxidizing agent c. source of Br2 d. source of I2 At the endpoint of titration, the equivalence of sodium thiosulfate is equal to the following, EXCEPT ___ . a. equivalence of KI b. equivalence of liberated I2 c. equivalence of KBrO3 d. none of the other choices
- A (0.002M) Cu2+ solution gave an absorbance of 0.50 at 560 nm in a 1.0 cm cell. The molar absobitivity of solution is equel:Compute for the appropriate amount (mL) of the compostions below of CTAB precitpitation solution used for DNA extraction. a. 1% w/v CTAB b. 10 mM EDTA c. 50 mM Tris-ClIn lab, suppose that we used 0.7885 grams ofCalcium carbonate (MW 100.09) dissolved in 250mL and for a 50mL aliquot it tookexactly 43.23 mL of EDTA to titrate.Our 5.000 gram unknown sample was dissolved in 250ml and a 50 ml aliquot was usedto determine the unknown concentration. If it took 33.45 mL of EDTA to get to the pointof colour change, what is the %Ca (MW 40.078) in the original sample?
- A sample is analyzed for chloride by the Volhard method. Calculate the %KCl from the following data: Wt of sample = 0.5000g; Vol of AgNO3 added = 35.00ml; M of AgNO3 = 0.1157; Vol of SCN- used for back titration = 14.71ml; M of SCN- = 0.08598; Atomic wts: Ag = 107.87, N = 14.00, Cl = 35.5, O = 16.00what is the LFSE for [Fe(CN)6]4-? splitting parameter is 32800cm-1 pairing energy is 17600 cm-1A 0.9092 g sample of wheat flour was analysed by the Kjeldahl procedure. The ammoniaformed was distilled into 50.00 mL of 0.02532 M H2SO4. A 7.46 mL back-titration of 0.04917 MNaOH was required. (Note the stoichiometry of your acid and base) Calculate thea. %N (FM=14.007) in the sample,b. %Protein in the sample (factor = 5.70)
- A 1.00 mL aliquot of stock Na2S2O3 solution (0.0675 M) was diluted to 100. 0 mL. This was used to titrate a 50.00 mL water sample for Winkler Determination of D.O. The sample required 8.55 mL of the titrant. Compute for the ppm O2 (molar mass of O2 = 32.00).A 0.9056 g sample of KBrO3 (MM=167.0) was dissolved in dilute HCl and treated with an unmeasured excess of KI. The liberated iodine required 37.21 mL of Na2S2O3. Calculate the molar concentration of sodium thiosulfate. 1 mol BrO3- = 3 mol I2 = 6 mol S2O32- 0.8744 M 2.623 M 0.8791 M 0.2915 MHow many milliliters of 1.5% alcoholic dimethylglyoxime should be used to provide a36.0% excess with 0.6984 q of steel containing 2.95 wt% Ni? Assume that the densityof the dimethylglyoxime solution is 0.790 g/mL. a. How much Ni sample is present? b. How many moles Ni is present in the sample? c. How much DMG is present?