A solution in part C initially contains (4.2100x10^-4) molar SCN¯ and (3.1700x10^-3) molar Fe3+. This solution was then measured using the colorimeter, and an absorbance of (5.01x10^-1) was recorded.The constant determined in part A of the experiment was found to be (3.4800x10^3). Using the data provided above, determine the equilibrium concentration of Fe3+ , [Fe3+ ]e in this solution. Note: Your answer is assumed to be reduced to the highest power possible. Your Answer: x10 Answer units
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- Mixing the chelating reagent B with Ni(II) forms the highly colored NiB22+, whose solutions obey Beer’s lawat 395 nm overa wide range. Provided the analytical concentration of the chelating reagent exceeds that of Ni(II) by a factor of 5 (or more), the cation exists, within the limits of observation, entirely in the form of the complex. Use the accompanying data to evaluate the formation constant Kf for the process Ni2++2BNiB22+A standard solution was put through appropriate dilutions to give the concentrations of iron shown in the table that follows. The iron(II)-1,10-phenanthroline complex was then formed in 25.0-mL aliquots of these solutions, following which each was diluted to 50.0 mL. The following absorbances (1.00-cm cells) were recorded at 510 nm: Calculate the concentration, in ppm, of a sample with an abosrbance of 0.829. Fe(II) concentration (ppm) A510 4.00 0.160 10.0 0.390 16.0 0.630 24.0 0.950 32.0 1.260 40.0 1.580A second calibration standard solution of an iron(III) salicylate complex was prepared in two steps. First, 10.0 mL of a 0.100 M stock solution was added to 90.0 mL of solvent to make 100.0 mL of the first calibration standard solution and, secondly, 80 mL of that first calibration solution plus 20.0 mL of solvent were mixed to make the second calibration standard. What is the concentration of the second calibration standard solution?
- A second calibration standard solution of an iron(III) salicylate complex was prepared in two steps. First, 12.9 mL of a 0.481 M stock solution was diluted with solvent to make 100.0 mL of the first calibration standard solution and, secondly, 86.6 mL of that first calibration solution was diluted to 100 mL to make the second calibration standard. What is the molar concentration of the second calibration standard solution? Report your answer to 3 significant figures.A reaction was carried out with Fe3+ and SCN- to produce FeSCN2+. Two best-fit lines for Absorbance vs [FeSCN-] were obtained. The first line produced: y = 200x + 0.005, r2=0.951 and the second line produced: y= 10,000x + 0.005, r2 = 0.993. Determine the best-fit line of two, and then use the line equation to determine the equilibrium concentration of FeSCN2+ if the absorbance = 0.863.A metal complex with a Molecular mass of 820 g mol−1 was dissolved and the solution made up to 25 mL in a volumetric flask. 1 mL was withdrawn, placed in a 100 mL volumetric flask and diluted to the mark. The absorbance (at 457 nm) of this solution (in a 1 cm cuvette) was 0.245. The extinction coefficient for this compound at 457 nm (ε530) = 11715 M-1cm-1.(a) calculate the concentration of the compound in the cuvette.(b) calculate the concentration of the compound in the 25mL volumetric flask(c) determine the mass of compound used to make the 25mL solution
- 3. An antacid tablet, weighing 1.25 g, was dissolved in a 1.0 L volumetric flask to allow for determination of calcium carbonate and magnesium carbonate contents. After preparing the solution, an aliquot of 10.0 ml was transferred to an Erlenmeyer flask containing a buffer solution with pH = 10. This aliquot was then titrated with EDTA 0.0040 mol/L and the average volume spent was 15.01 mL. To measure calcium after precipitation. After the magnesium was fractionated, a second 10.00 mL aliquot of the stock solution was transferred to an Erlenmeyer flask, and the pH of the present solution was adjusted to a value of approximately 13. In EDTA titration, the volume consumed for observation ofthe end point was equal to 13.03 mL. Based on this information,a) Outline the two steps involved, representing the related reactions./5b) Calculate the concentrations of CaCO3 and MgCO3 present in the initialsolution./6c) Calculate the masses of CaCO3 and MgCO3 present in the pellet./6d) Calculate the…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.An antacid tablet, weighing 1.25 g, was dissolved in a 1.0 L volumetric flask to allow for determination of calcium carbonate and magnesium carbonate contents. After preparing the solution, an aliquot of 10.0 ml was transferred to an Erlenmeyer flask containing a buffer solution with pH = 10. This aliquot was then titrated with EDTA 0.0040 mol/L and the average volume spent was 15.01 mL. To measure calcium after precipitation After the magnesium was fractionated, a second 10.00 mL aliquot of the stock solution was transferred to an Erlenmeyer flask. and the pH of the present solution was adjusted to a value of approximately 13. In EDTA titration, the volume consumed for observation of the end point was equal to 13.03 mL. Based on this information, (a) Outline the two steps involved, representing the related reactions. (b) Calculate the concentrations of CaCO3 and MgCO3 present in the initial solution. (c) Calculate the masses of CaCO3 and MgCO3 present in the pellet. (d) Calculate the…
- . An antacid tablet, weighing 1.25 g, was dissolved in a 1.0 L volumetric flask to allow for determination of calcium carbonate and magnesium carbonate contents. After preparing the solution, an aliquot of 10.0 ml was transferred to an Erlenmeyer flask containing a buffer solution with pH = 10. This aliquot was then titrated with EDTA 0.0040 mol/L and the average volume spent was 15.01 mL. To measure calcium after precipitation. After the magnesium was fractionated, a second 10.00 mL aliquot of the stock solution was transferred to an Erlenmeyer flask, and the pH of the present solution was adjusted to a value of approximately 13. In EDTA titration, the volume consumed for observation of the end point was equal to 13.03 mL. Based on this information, a) Outline the two steps involved, representing the related reactions./5 b) Calculate the concentrations of CaCO3 and MgCO3 present in the initial solution./6 c) Calculate the masses of CaCO3 and MgCO3 present in the pellet./6 d) Calculate…Ammonium iron(II) sulfate crystals have the following formula: (NH4)2SO4.FeSO4.nH2O . In an experiment to determine n 8.492g of the salt were dissolved and made up to 250cm^-3 of solution with distilled water and sulphuric acid. A 25.0cm^-3 portion of the solution was titrated against 0.0150 mol dm^-3 KMnO4. A volume of 22.5cm^-3 was required. Find the value of nThe concentration of iron in a solution can be determined using UV?Vis spectrophotometry by reacting the iron with 1.10-phenanthroline to produce a colored complex. The following data were obtained for a series of standard solutions of iron/1,10-phenanthroline complex measured in a 1.00 cm cell. Concentration (M) Absorption 0.50x10-4 0.109 1.0x10-4 0.218 2.0x10-4 0.436 3.0x10-4 0.656 4.0x10-4 0.872 a.Prepare a Beer’s law plot using the above data b.Calculate the concentration of an iron 1, 10-phenanthroline complex solution that has an absorbance of 0.317 c.Calculate the molar absorptivity of the iron/1, 10-phenanthroline complex