A 1.9300 g impure sample of Fe(NH4)2(SO4)2 (FW = 392.14) was dissolved in 75 mL 0.75 M H2SO4 and was titrated with the standard KMnO4 in problem 1. Titration of the sample required 24.00mL while the blank containing only 75mL 0.75 M H2SO4 required 0.75 mL of the KMnO4 titrant. (Hint: subtract blank). Calculate the concentration of Fe(NH4)2(SO4)2 in %w/w in the impure sample. 5Fe²+ + MnO4 + 8H+ → 5Fe³+ + Mn²+ + 4H₂O

A 1.9300 g impure sample of Fe(NH4)2(SO4)2 (FW = 392.14) was dissolved in 75 mL 0.75 M H2SO4 and was titrated with the standard KMnO4 in problem 1. Titration of the sample required 24.00mL while the blank containing only 75mL 0.75 M H2SO4 required 0.75 mL of the KMnO4 titrant. (Hint: subtract blank). Calculate the concentration of Fe(NH4)2(SO4)2 in %w/w in the impure sample. 5Fe²+ + MnO4 + 8H+ → 5Fe³+ + Mn²+ + 4H₂O

Chemistry & Chemical Reactivity

10th Edition

ISBN:9781337399074

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter4: Stoichiometry: Quantitative Information About Chemical Reactions

Section4.9: Spectrophotometry

Problem 2.1ACP: Excess KI is added to a 100.0-mL sample of a soft drink that had been contaminated with bleach,...

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A 1.9300 g impure sample of Fe(NH4)2(SO4)2 (FW = 392.14) was dissolved in 75 mL 0.75 M H2SO4 and was titrated with the standard KMnO4 in problem 1. Titration of the sample required 24.00mL while the blank containing 75mL 0.75 M H2SO4 required 0.75 mL of the KMnO4 titrant. Calculate the concentration of Fe(NH4)2(SO4)2 in %w/w in the impure sample.
A mixture containing only KCl and NaBr is analyzed by the Mohr Method. A 0.3172-g sample is dissolved in 50 mL water and titrated to the Ag2CrO4 endpoint, requiring 36.85 mL of 0.1120 M AgNO3. A blank titration requires 0.71 mL of titrant to reach the same endpoint. Report the % (w/w) KCl and NaBr in the sample. [Answer should be 82.41 % (w /w)]
Calculate the concentration of Fe2O3 in a mineral sample after solubilization of 0.4891g and availability of Fe as Fe2+. The released Fe2+ ions were titrated with a 0.02153 mol/L K2Cr2O7 solution requiring 36.92 mL to reach the end point of the titration. Show the calculations and express the concentration in % m/m. K2Cr2O7; + 6Fe2+ + 14H+ → 2Cr+3 + 2K+ + 6Fe3+ + 7H20
The amount of iron in a meteorite is determined by a redox titration using KMnO4 as the titrant. A 2.1800 g sample is dissolved in acid and the liberated Fe3+ quantitatively reduced to Fe2+ using a Walden reductor. Titrating with 0.02500 M KMnO4 requires 22.0 mL to reach the end point. Determine the %w/w Fe2O3 in the sample of meteorite.
The amount of iron in a meteorite was determined by a redox titration using KMnO4 as the titrant. A 0.4185 -g sample was dissolved in acid and the liberated Fe3+ quantitatively reduced to Fe2+, using a reductor column. Titrating with 0.0044 M KMnO4 requires 28.76 mL to reach the end point. Determine the %w/w Fe2O3 in the sample of meteorite. (Fe = 55.845 amu, Fe2O3 = 159.69 g/mol
If the molar solubility of Tl2S at 25 oC is 5.31e-08 mol/L, what is the Ksp at this temperature?Ksp = (b) It is found that 9.14e-08 g of Sc(OH)3 dissolves per 100 mL of aqueous solution at 25 oC. Calculate the solubility-product constant for Sc(OH)3.Ksp = (c) The Ksp of Cu3(PO4)2 at 25 oC is 1.40e-37. What is the molar solubility of Cu3(PO4)2?solubility = mol/L
What is the solubility (in g/L) for PbBr2(s) in a 1.00 L solution that has 251 g Pb(NO3)2 already dissolved in it? The Ksp for PbBr2 is 5.67 × 10-6. If you need more room, use a second sheet.
25.00 mL of a solution containing KIO4 is treated with excess potassium iodide. IO4- + 8H+ + 7I- → 4I2 + 4H2O The resulting solution is titrated with 0.15 M sodium thiosulfate pentahydrate. The average titre was 21.76 mL. I2 + 2S2O32- → 2I- + S4O62- What is the concentration of the sodium thiosulfate solution as a percentage (w/v)
A mixture containing only KCl and NaBr is analyzed by the Mohr method. A 0.2125-g sample is dissolved in 25 mL of water and titrated to the Ag2CrO4 endpoint, requiring 25.63 mL of 0.1110 M AgNO3. A blank titration requires 1.15 mL of titrant to reach the same end point. Report the %w/w KCl and NaBr in the sample. KCl = 74.551 NaBr = 102.89
A mixture containing only KCl and NaBr is analyzed by the Mohr method. A 0.2125- g sample is dissolved in 25 mL of water and titrated to the Ag2CrO4 end point, requiring 25.63 mL of 0.1110 M AgNO3. A blank titration requires 1.15 mL of titrant to reach the same end point. Report the %w/w KCl and NaBr in the sample.KCl = 74.551 NaBr = 102.89
Determine the solubility of KIO4 in water. Volume of saturated KIO4 in conical flask is 25.0 ml,KI is 2g,H2SO4 (3.0M) is 20.0 ml added to KI solution , volume of 0.200 M sodium thiosulphate used for titration is 8.00 ml.and if mean ionic activity co efficient,y+- of KIO4 in the saturated solution is 0.85 ,what is Ksp. .
A 0.7352g sample of ore containing Fe3+, Al3+ and Sr2+ was dissolved and made up to 500.00 mL. The analysis of metals was performed by a chemistry using complexation volumetry. Initially, an aliquot of 50.00 mL had its pH adjusted to 1.0 and titrated with a standard solution of EDTA 0.02145 mol/L, 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. Determine the percentage of each of the metals in the sample Given the molar masses: Fe=55.845 g/mol; Al=26.982 g/mol and Sr=87.620 g/mol.