Iron was analyzed by dissolving 1.1324 g sample inconcentrated HCL. The solution was diluted in H20, Fe(II) wasprecipitated as Fe,03.H20 by adding NH3. After filteration,washing the residue ignited to give 0.5394 g of pure Fe203(159.69 g/mol). Calculate %Fe (55.847g/mol) in the sample.O 33.32 %O 69.12 %O 45.21 %O 54.21 %23.21 %

Given: Mass of iron sample = 1.1324 g Mass of Fe2O3 produced = 0.5394 g

Iron was analyzed by dissolving 1.1324 g sample in concentrated HCL. The solution was diluted in H20, Fe(lII) was precipitated as Fe2O3.H2O by adding NH3. After filteration, washing the residue ignited to give 0.5394 g of pure Fe203 (159.69 g/mol). Calculate %Fe (55.847g/mol) in the sample. O 33.32 % 69.12 % 45.21 % 54.21 % 23.21 %

Iron was analyzed by dissolving 1.1324 g sample in concentrated HCL. The solution was diluted in H20, Fe(lII) was precipitated as Fe2O3.H2O by adding NH3. After filteration, washing the residue ignited to give 0.5394 g of pure Fe203 (159.69 g/mol). Calculate %Fe (55.847g/mol) in the sample. O 33.32 % 69.12 % 45.21 % 54.21 % 23.21 %

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

A solution of sodium hydroxide is standardized against potassium hydrogen phthalate (molecular mass = 204.224 g mol-1). From the following data, calculate the molarity of the NaOH solution. The mass of the KHP is 0.7840 g. Before the titration the buret reading was 0.8400 mL and afterwards it was 39.20 mL. A 85.12 mL sample of a solution of sulfuric acid, H2SO4, is neutralized by 59.82 mL of the NaOH solution from the problem above. Calculate the molarity of the sulfuric acid solution.
A pure organic compound has the formula C4H8SOx. A sample of a compound wasdecomposed; the sulfur was converted to sulfate and titrated in a modified version of theadsorption indicator procedure. From the following data, determine the correct formula forthe compound.Given: weight of sample = 12.64 mgBa(ClO4)2 needed for titration = 10.60 mL of 0.0100 M Ba(ClO4)2
A sample contains MgCl2 (95.211 g/mol) and KCl (74.551 g/mol). A 6.6933-g sample was dissolved in enough H2O to make 250.0-mL solution. A 50.00-mL aliquot was treated with AgNO3 to precipitate the chlorides and after proper collection and drying gave a precipitate weighing 1.9620-g. Another 50.00-mL aliquot was tested for its Mg2+ content by precipitating it with NH4+ and PO43- giving an Mg2P2O7 (222.551 g/mol) precipitate weighing 0.5186 g with FW AgCl 143.32 g/mol. What is percent KCl in the sample?
2. A 0.4912-g sample of a petroleum product was burned in a tube furnace, and the SO2 produced was collected in H2O2. SO2(g) + H2O2 → H2SO4 A 25.00-mL portion of 0.00873 M NaOH was introduced into the solution of H2SO4, following which the excess base was back-titrated with 15.17 mL of 0.01102 M HCl. Calculate the sulfur concentration in parts per million.
A 1.00 gram sample of anhydrous cerium sulfate was dissolved in water. Barium nitrate solution was then added until no further precipitation occurred. The precipitate was filtered from the solution then dried and was found to weigh 1.41 g. Determine the formula of the cerium sulfate. Encom calt is hydrated
A sample weighing 10.91 g containing an unknown amount of H3PO4 was diluted with water and titrated with a standardized concentration of 0.7255 M NaOH. The endpoint was reached after 27.03 mL of the titrant was added. What is the % H3PO4 (97.994 g/mole) in the sample? H3PO4 + 2 NaOH --> Na2HPO4 + 2H2O ROUND OFF FINAL ANSWER TO FOUR (4) SIG FIGS
A sample consisting of Na2CO3 (105.96), NaOH (39.99) and inert matter weighs 1.179 g. It is titrated with 0.300 N HCI with phenolphthalein as the indicator, and the solution becomes colorless after the addition of 48.16 ml. Methyl orange is then added and 24.08 ml more of the acid are needed for the color change. What is the percentage of NaOH and N22CO3? *
A sample consisting of Na2CO3, NaHCO3 and inert matter weighs 1.179 grams. It is titrated with 0.1 N HCl with phenolphthalein as the indicator, and the solution became colorless after the addition of 24.00 mL. Another duplicate sample was titrated with HCl using methyl orange as indicator. It required 50.25 mL of the acid for the color change from yellow to red. What are the percentage of Na2CO3 and NaHCO3 in the sample? Note [EXAMPLE IN THE IMAGE]
Use the data below to detemine the % by mass of Fe to TWO decimal places, if a 0.02 M KMNO4 solution was used for the titration. (MM Fe = 56 g/mol) mass of iron compound (g) 0.691 initial buret reading (mL) 0.77 final buret reading (mL) 16.71
A solid sample containing some Fe2+ion had a total mass of .9791 g. It required 18.2 ml of 0.02304 M KMnO4 to titrate the Fe2+ in the dissolved sample to a pink endpoint. How many moles of Fe2+ were in the the sample? How many grams of irion were present in the sample and what was the mass percent iron in the sample?
A serum sample of 3mL is analyzed for nitrogen by modified Kjeldahl. The sample is digested, distilled, and 14mL of standard of HCl is needed to titrate the ammonium borate. The HCl was standardized using 0.30g (NH4)2SO4. 30mL acid was required in titrating for standardization. What is the concentration of nitrogen in the serum (weight/volume)?