Sulfur containing compound weighing 4.8670 grams was digested and purified to form H,SO¸. A 25.00-mL of 0.0090 M NaOH was added to the collected H SO , and the excess base was then back titrated with 13. 45 mL of 0.0100 M HCI. Calculate the sulfur content in the sample parts per million. This problem involves back titration. Write the two chemical equations involved in the analysis. Identify the analyte, “bridging" reagent and titrant. Solve for the mole of the analyte using the titration values and the stoich relationships. One mole of H,so, is equal to one mole of sulfur in the sample. Solve for the mass of S then ppm S.

Sulfur containing compound weighing 4.8670 grams was digested and purified to form H,SO¸. A 25.00-mL of 0.0090 M NaOH was added to the collected H SO , and the excess base was then back titrated with 13. 45 mL of 0.0100 M HCI. Calculate the sulfur content in the sample parts per million. This problem involves back titration. Write the two chemical equations involved in the analysis. Identify the analyte, “bridging" reagent and titrant. Solve for the mole of the analyte using the titration values and the stoich relationships. One mole of H,so, is equal to one mole of sulfur in the sample. Solve for the mass of S then ppm S.

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter31: Introduction To Analytical Separations

Section: Chapter Questions

Problem 31.17QAP

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A bottle of concentrated hydroiodic acid is 57% HI by weight and has a density of 1.70 g/mL. A solution of this strong and corrosive acid is made by adding exactly 10.0 mL to some water and diluting to 250.0 mL. If the information on the label is correct, what volume of 0.988 M NaOH is needed to neutralize the HI solution? Suggest an indicator for the titration.
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Sulfur containing compound weighing 4.8670 grams was digested and purified to form H,SO4. A 25.00-mL of 0.0090 M NaOH was added to the collected H,SO4, and the excess base was then back titrated with 13.45 mL of 0.0100 M HCl. Calculate the sulfur content in the sample in parts per million. This problem involves back titration. Write the two chemical equations involved in the analysis. Identify the analyte, “bridging" reagent and titrant. Solve for the mole of the analyte using the titration values and the stoich relationships. One mole of H2SO4 is equal to one mole of sulfur in the sample. Solve for the mass of S then the ppm S.
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