2. 100.0-mL sample of spring water was treated to convert any iron present to Fe2+. Addition of 25.00 mL of 0.002107 M K2Cr207 resulted in the reaction 6FE2+ + Cr20,2- + 14H* ® 6FE3+ + 2Cr3+ + 7H2O The excess K2CR207 was back-titrated with 7.47 mL of a 0.00979 M Fe2* solution. Calculate iron concentration (molarity) in the sample.
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- 2) A 100.0-mL sample of spring water was treated to convert any iron present to Fe2*. Addition of 25.00 mb. of 0.008 M K2Cr207 resulted in the reaction 6F22+ + Cr2O72- + 14H*2 6FE3+ + 2Cr3+ + 14H2O The excess K2C12O7 was back-titrated with 8.53 ml of 0.00949 M Fe2* şolution. Calculate the molar concentration of iron in the sample.A 100.0-mL sample of spring water was treated to convert any iron present to Fe2+.Titration with 35.00-mLof 0.002345 M K2Cr2O7 resulted in the reaction6Fe2+ + Cr2O72- + 14H+ 6Fe3+ 1 2Cr3+ + 7H2OThe excess K2Cr2O7 was back-titrated with 8.32 mL of 0.00897 M Fe2+ solution.Calculate the concentration of iron in the sample in parts per million.The amount of Fe (55.85g/mole)in a 16.9776-g sample of an ore was determined by a redox titration with K2Cr2O7. The sample was dissolved in HCI and the iron brought into the +2 oxidation state using a Jones reductor. Titration to the diphenylamine sulfonic acid end point required 43.7238 mL of 0.1351 M K2Cr2O7. Report the iron content of the ore as %w/w Fe2O3 (159.69g/mole) (Answers should be written in 2 decimals place and do not include the UNIT)
- Chromel is an alloy composed of nickel, iron, and chromium. A 0.6392-g sample was dissolved and diluted to 250.0 mL. When a 50.00-mL aliquot of 0.05173 M EDTA was mixed with an equal volume of the diluted sample, all three ions were chelated, and a 5.15-mL back-titration with 0.06139 M copper(II) was required. The chromium in a second 50.0-mL aliquot was masked through the addition of hexamethylenetetramine; titration of the Fe and Ni required 34.27 mL of 0.05173 M EDTA. Iron and chromium were masked with pyrophosphate in a third 50.0-mL aliquot, and the nickel was titrated with 24.31 mL of the EDTA solution. Calculate the percentages of nickel, chromium, and iron in the alloy. Percentage of nickel = % Percentage of iron = Percentage of chromium = % 10A 110.0-mL sample of spring water was treated to convert any iron present to Fet. Addition of 25.00-mL of 0.002525 M K2C1207 resulted in the reaction 6Fe?+ + Cr2 O7²- + 14H+ → 6Fe+ + 2Cr³+ + 7H2O The excess K2C12 07 was back-titrated with 8.05 mL of 0.00951 M Fe-t solution. Calculate the concentration of iron in the sample in parts per million. Concentration of iron ppm3. A 100.0 mL sample of ground water was treated to convert the iron present to Fe2+. Addition of 25.00 mL of 0.002412 M K2Cr2O7 resulted in the reaction below. 6Fe2+ + Cr2O72 - + 14H+ → 6Fe3+ + 2Cr3+ + 7H2O The excess K2Cr2O7 was back-titrated with 8.12 mL of 0.00859 M Fe2+ solution. What is the concentration of Fe in the sample in parts per million?
- A Chemist collected a 0.4891-g sample of an ore for Fe determination by a redox titration with K2Cr2O7.The ore was carefully crushed prior to weighing and dissolved in HCl and using a Jones reductor the ironin the sample was brought into the +2 oxidation state. After titration with diphenylamine sulfonic acid,itrequired 36.92 mL of 0.02153 M K2Cr2O7 to reach the end point. Show your solution why 77.86% is the iron content of the ore as %w/w Fe2O3.A Chemist collected a 0.4891-g sample of an ore for Fe determination by a redox titration with K2Cr2O7.The ore was carefully crushed prior to weighing and dissolved in HCl and using a Jones reductor the ironin the sample was brought into the +2 oxidation state. After titration with diphenylamine sulfonic acid,itrequired 36.92 mL of 0.02153 M K2Cr2O7 to reach the end point. Calculate the iron content of the ore as%w/w Fe2O3To analyze the amount of iron (Fe; Mw = 55.85 g/mol) contained in an ore sample, the sample was digested with acid and diluted to 50 mL with water. This solution was then treated with 25.00 mL of 0.2922 M EDTA. The excess EDTA was back titrated with 6.47 mL of 0.0843 M Zn2+ to reach the equivalence point. How many grams of Fe contained in the ore sample?
- 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.Chromel is an alloy composed of nickel, iron and chromium. A 0.6553-g sample was dissolved and diluted to 250.0 mL. When a 50.00-mL aliquot of 0.05173 M EDTA was mixed with an equal volume of the diluted sample, all three ions were chelated, and a 5.34-mL back titration with 0.06139 M copper (II) was required.The chromium in a second 50.0-mL aliquot was masked through the addition of hexamethylenetetramine; titration of the Fe and Ni required 36.98 mL of 0.05173M EDTA. Iron and chromium were masked with pyrophosphate in a third 50.00-mL aliquot, and the nickel was titrated with 24.53 mL of the EDTA solution. Calculate the percentage of Cr in the alloy. Express your answer in 2 decimal places.A pure oxide of iron weighing 1.000 g is fused with K2S2O7 and the fused material dissolved in acid. The Fe3+ is reduced with SnCl2, HgCl2 is added, and the Fe2+ titrated with 0.1667 M K2Cr2O7 solution, requiring 12.96 mL. What was the formula of the original oxide?