In what volume should iron fumarate (M=169.85g/mol) with a mass of 152.1mg be dissolved and what volume of the analyzed solution should be taken for titration so that the volume of titrant used during the titration does not exceed 3ml. What titrant would be suitable for rapid titration if it is known that standardization of this titrant does not need to be done and the concentration of the titrant is 0.01667M?1) what is the name of this type of titration?2) sketch the relevant titration curve.3) how can you be sure of the accuracy and correctness of the obtained results?

In what volume should iron fumarate (M=169.85g/mol) with a mass of 152.1mg be dissolved and what volume of the analyzed solution should be taken for titration so that the volume of titrant used during the titration does not exceed 3ml. What titrant would be suitable for rapid titration if it is known that standardization of this titrant does not need to be done and the concentration of the titrant is 0.01667M?1) what is the name of this type of titration?2) sketch the relevant titration curve.3) how can you be sure of the accuracy and correctness of the obtained results?

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter11: Solutions

Section: Chapter Questions

Problem 72AP

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Molarity of Na2S2O3 (stock solution). 0.100 M Volume of diluted bleach titrated (taken from the volumetric flask). 10ml Initial Burette Reading. 14.80 Final Burette Reading 25.60 Volume of Na2S2O3 used in the titration (mL). 10.80 Moles of Na2S2O3 used in the titration. 1.71 Moles of S2O3–2 used. 1.66 Moles of I2 initially present in titration mixture 0.83 Moles of NaOCl in the diluted bleach titrated. 0.415 Volume of bleach titrated. 1ml Mass of NaOCl in commercial bleach titrated. ?
You want to determine Fe in a solution via manganometric titration. To determine the exact concentration of the KMnO4 solution, you titrate a sodium oxalate solution in a strongly acidic environment. Thereby oxalate will be oxidized to CO2 by KMnO. For this purpose you dissolve exactly 185.4 mg sodium oxalate (M = 134.0 g/mol) and titrate with KMnO4 solution. Your consumption equals 22.8 ml. Subsequently you use the permanganate solution to titrate 25 ml of a sample containing Fe² (M = 55.8 g/mol) whereby Fe2+ will be oxidized to Fe by MnO in a strongly acidic environment. For this titration you need 3.9 ml of the KMnO, solution. Please give all relevant reaction equations (with correct stoichiometry). Calculate the exact concentration of the permanganate solution. How much Fe (in g) was in 250 ml of your sample solution? If you do this titration in a solution containing HCI, you have to add the Reinhard/Zimmermann solution. What are the ingredients, why do you need to add it and what…
1. A 0.3516 g sample of commercial phosphate detergent was ignited at a heat to destroy the organic matter. The residue was taken up in hot HCI which converted P to H3PO4. The phosphate was precipitated as MGNH4PO4.6H2O by addition of Mg+ followed by aqueous NH3. After being filtered and washed, the precipitate was converted to Mg2P2O7 by ignition at 1000 OC. This residue weighed 0.2161 g. Calculate the percent P (30.974) in the sample? Ans 17.11%
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