1. The Fe2+ content of iron tablets was determined by titration with a freshly standardised solution of potassium manganate(VII), KMN04. The equation for the titration reaction is 5Fe2+ + Mn04-+ 8H+ 5FE3+ + Mn2+ + 4H20 Maximum 5 iron tablets each is 0.065g of iron and 0.02 moldm potassium manganate (VII)(KMNO4) and 1 moldm aqueous sulfuric acid Describe how exactly 250 cm3 of Fe2+ solution was prepared from five iron tablets, each of mass 0.325 g in order to give a sensible titre. your calculations must be given

1. The Fe2+ content of iron tablets was determined by titration with a freshly standardised solution of potassium manganate(VII), KMN04. The equation for the titration reaction is 5Fe2+ + Mn04-+ 8H+ 5FE3+ + Mn2+ + 4H20 Maximum 5 iron tablets each is 0.065g of iron and 0.02 moldm potassium manganate (VII)(KMNO4) and 1 moldm aqueous sulfuric acid Describe how exactly 250 cm3 of Fe2+ solution was prepared from five iron tablets, each of mass 0.325 g in order to give a sensible titre. your calculations must be given

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter13: Titrations In Analytical Chemistry

Section: Chapter Questions

Problem 13.13QAP

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0.1724g of a mineral containing MnO₂ was dissolved and then treated with excess iodide according to the following unbalanced reaction: MnO2(s) + H+ → Mn²+ + I2 + H₂O The I₂ released was titrated with a solution of Na₂S2O3 0.07320 mol/L, requiring 14.65 mL to reach the point end of degree a) Determine the percentage of MnO₂ in the ore. b) When iodine solutions are used as titrants these are prepared by dissolving 1₂ in concentrated KI. Explain the reason for the need for KI in the preparation of these solutions?
The solubility of borax, which is made up of sodium tetraborate (Na2B4O5(OH)4 8H2O), was analyzed. The dissolution of borax is: Na2B4O5(OH)4 • 8H2O(s) ⇌ 2 Na+(aq) + B4O5(OH)42–(aq) + 8 H2O(l) A 50 mL saturated solution was prepared. After filtration of solution, 5 mL aliquot was transferred to a flask and titrated using 0.432 M HCl. The endpoint was found to be 4.73 mL of the titrant. Tetraborate anion (B4O5(OH)42-) is a weak base which reacts with HCl like the following reaction: B4O5(OH)42–(aq) + 2 H+(aq) + 3 H2O(l) ⇌ 4 H3BO3(aq) What is Ksp expression for the dissolution? What is the tetraborate ions concentration in the filtrate? What is the molar solubility and Ksp of borax if the titration was done at room temperature (298 K)?
The concentration of CO in the air can be determined by passing a known volume of air through a tube containing I2O5, resulting in the formation of CO2 and I2. I2 is removed from the tube by distillation and collected in a solution containing excess KI, producing I3-. I3- is titrated with a standard solution of Na2S2O3. A 4.79 L air sample was sampled as described here, requiring 7.17 ml of 0.00329 M Na2S2O3 to reach the endpoint in a typical analysis. If the density of the air is 1.23×10^-3 g/ml, what is the amount of CO in the air in ppm? (CO: 28 g/ml)
1,5419 g of magnetite (Fe3O4) ore; in concentrated HCL to form a mixture of Fe + 2 and Fe+3it's unraveling. By adding HNO3 to it, all Fe+2 s are upgraded to Fe+3. And the addition of FE+3 s NH3,with Fe (OH)3, precipitating into. The sediment is weighed as 0.8525 g in the form of Fe2O3 after the necessary operations. Calculate the percentage of Fe3O4 in the sample.
Gravimetric analysis of Fe3O4 (MW = 232 g/mole) may be undertaken with the following reactions: Fe3O4 → Fe2O3 → Fe (OH)3. Weight of sample containing 8.00% Fe3O4 that must be taken to obtain a precipitate of Fe(OH)3 (MW = 107 g/mole) that weighs 150 mg is . a. 0.108 g b. 0.325 g c. 1.355 g d. 4.065 g Amount of Fe2O3 (MW = 160 g/mole) from which 150 mg of Fe(OH)3 (MW = 107 g/mole) may be obtained is . a. 0.112 g b. 0.224 g c. 0.448 g d. none of the other choices
The mercury in a 0.8142-g sample was precipitated with an excess of paraperiodic acid, H5IO6: 5 Hg 2+ + 2 H5IO6 ---> Hg5(IO6)2 (s) + 10 H + The precipitate (MW = 1448.8 g/mol) was filtered, washed free of precipitating agent, dried, and weighed, and 0.4114 g was recovered. Calculate the a) % Hg (200.6 g/mol) b) % Hg2Cl2 (472.1 g/mol)
An ore containing Fe3O4 was analyzed by dissolving a 1.5419-g sample in concentrated HCl. HNO3 was then added to oxidize any Fe2+ to Fe3+. The Fe3+ was precipitated as Fe(OH)3 by adding NH3. The precipitate was collected by filtration and was finally heated yielding 0.8525 g of Fe2O3. Report the concentration of Fe3O4 in the sample as %(w/w). (Note: the final answer is said to be 53.4%)
An analyst weighed 0.25045 g of the Buffalo River Sediment reference material.(RM # 8704) to determine Pb levels. The material was digested in an acid medium toBring it to a solution which was made up to the 30.2450 mL mark with distilled water. If thePb concentration in the control certificate of analysis is (150 ± 17) mg / kg, and theanalyst recovered 95%, what was the concentration of Pb in the solution?
Prepare 50ml of approximately 1000ppm Mn stock solution from MnCl2*4H2)
In a lab, you diluted a sample of bleach to 1/10 concentration in a 250 vol. flask. Then quantitatively transferred into into a beaker and titrated it with a standard sodium thiosulfate solution with a molarity of 0.1215M. You repeated this 3 times. The data below is the amount of sodium thiosulfate that was titrated in the 3 runs. Calculate the molarity in each run of the diluted bleach and the concentration of undiluted bleach sample.
A 0.2500-g of dry CaCO3 was completely dissolved into a solution of 5-mL conc. HCl and 50-mL distilled water in an erlemeyer flask. The resulting solution was boiled for 5 minutes to expel CO2 from the reaction, and then it was cooled to room temperature and the solution was transferred in a 500-mL volumetric flask filled to volume by rinsing the erlenmeyer flask and combining all the washings to fill the mark. A 5.0-mL aliquot of the CaCl2 solution was taken from the orignal solution and was transferred into an erlenmeyer flask with 10-mL NH3 buffer, 20-mL distilled water, and 5 gtts of EBT. The solution consumed 4.96 mL of an EDTA solution. MW: CaCO3 = 100.1 Compute for the N EDTA solution. 0.0053 N 0.0531 N 0.5313 N None of the choices
In one trial determination of the concentration of NaOCl in the diluted bleach sample, 10.00 mL of the diluted bleach solution required 23.32 mL of 0.0195 M Na2S2O3 titrant to reach the endpoint. What is the molar concentration of NaOCl in the diluted bleach solution?