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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 2:1Determine the percentage of iron in a sample of limonite from the following data:weight of sample = 0.5000g volume of KMNO4 added 50.0mL ; 1.00mL Kmno4 = 0.0005507 g fevolume of FeSO4 used for back titration 8.00mL ; 1.00mL FeSO4= 0.008950 g FeOMW: Fe= 55.85 FeO= 71.84When I was a boy, I watched Uncle Wilbur measure the iron content of runoff from his banana ranch. He acidified a 25.0-mL sample with HNO3 and treated it with excess KSCN to form a red complex. (KSCN itself is colorless.) He then diluted the solution to 100.0 mL and put it in a variablepathlength cell. For comparison, he treated a 10.0-mL reference sample of 6.80X 1024 M Fe31 with HNO3 and KSCN and diluted it to 50.0 mL. The reference was placed in a cell with a 1.00-cm pathlength. Runoff had the same absorbance as the reference when the pathlength of the runoff cell was 2.48 cm. What was the concentration of iron in Uncle Wilbur’s runoff ?
- A 0.9352g sample of ore containing Fe³+, Al³+ and Sr²+ was dissolved and made up to 500.00 mL. The analysis of metals was performed using complexation volumetry. Initially, an aliquot of 50.00 mL had its pH adjusted to 1.0 and titrated with a standard 0.03145 mol/L EDTA solution, requiring 6.95 mL to reach the end point. Subsequently, another 25.00 mL aliquot was buffered at pH=5 and titrated with the same EDTA solution, requiring 6.24 mL to reach the end point. Finally, a third aliquot of 25.00 mL was titrated at pH=11, requiring 11.10 mL of the same EDTA solution to complete the titration. Given the molar masses: Fe=55.845 g/mol; Al-26.982 g/mol and Sr-87.620 g/mol. a) Determine the percentage of each of the metals in the sample. b) Explain why the change in pH allows the determination of the three ions in this sample.A foot powder sample containing Zn was dissolved on 50.00 mL water and was titrated to the end point color with 22.57 mL of 0.01639 M EDTA at pH=4. (α= 3.61x109, KKzny2 = 3.2 x 1016). The pZn in the sample is:A volume of 50.00 ml of 0.01800 mol L-1 EDTA solution was added to a solution containing 0.02550 g of Ni. The unreacted excess of EDTA was then titrated with V mL 0.01500 mol L-1 ZnSO4 solution. Calculate the value of V. Data: Ni = 58.69 EDTA = 292.24
- Ex(1): In the analysis for chloride. The sample weighed (0.8732 gm) and the AgCl (p.p.t) from the sample weighed (1.0292 gm). Calculate the precent of chloride in the sample. At. wt. of Cl= 35.5, Ag = %3D 101.88.An EDTA solution was allowed to react with Pb²⁺ to produce 0.25 M PbY²⁻, 2.67×10⁻⁸ M Pb²⁺ and an excess of 0.10 M at equilibrium (K = 1.1×10⁸). What will be the α₄ value under these conditions?H2S(aq) is analyzed by titration with coulometrically generated I2 in Reactions 17-3a and 17-3b. To 50.00 mL of unknown H2S sample were added 4 g of KI. Electrolysis required 812 s at 52.6 mA. Find the concentration of H2S (mg/mL)in the sample.
- A sample of iron ore weighing 800 mg was treated with HNO3 , boiled to dryness and redissolved in dilute HCl. After filtration and removal of undissolved silica, the liquid was passed through a Walden reductor. The collected sample was titrated with 0.0210 M KMnO4 , requiring 12.0 mL to reach the end point. Calc %Fe (55.845) in the ore.The thickness of the chromium plate on an auto fender is determined by dissolving a 30.0-cm2 section in acid and oxidizing Cr3+ to Cr2O7 2-with peroxydisulfate. After removing excess peroxydisulfate by boiling, 500.0 mg of Fe(NH4 )2 (SO4 )2•6H2O is added, reducing the Cr2O7 2- to Cr3+ . The excess Fe2+ is back titrated, requiring 18.29 mL of 0.00389 M K2Cr2O7 to reach the end point. Determine the average thickness of the chromium plate given that the density of Cr is 7.20 g/cm3 . Note: thickness = volume /area50.00 ml of 0.1000 M Fe(CN)64- solution is titrated with 0.05000 M Tl3+ solution potentiometrically using S.C.E. and Pt electrodes. Calculate the values of the potential when 10.0, 50.0 and 60.0 ml of titrant have been added.