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 H2SO4, 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.
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 H2SO4, 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.
Chemistry: Principles and Practice
3rd Edition
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter16: Reactions Between Acids And Bases
Section: Chapter Questions
Problem 16.98QE: A monoprotic organic acid that has a molar mass of 176.1 g/mol is synthesized. Unfortunately, the...
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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 HCI. 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.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F5311adf0-879f-470f-8813-fd8db48d85eb%2F32aaa2e3-2b4d-4a52-924b-a66138ae311a%2Frjee04t_processed.jpeg&w=3840&q=75)
Transcribed Image Text: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 HCI. 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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