1. The thiourea in a 1.455 g sample of an organic material was extracted into a dilute H2SO, solution and titrated with 37.31 mL of 0.009372 M Hg²* via the reaction below. 4(NH2)2CS + Hg2 - [(NH2)2CS]«Hg² What is the percentage of (NH2)2CS in the sample?
1. The thiourea in a 1.455 g sample of an organic material was extracted into a dilute H2SO, solution and titrated with 37.31 mL of 0.009372 M Hg²* via the reaction below. 4(NH2)2CS + Hg2 - [(NH2)2CS]«Hg² What is the percentage of (NH2)2CS in the sample?
Chemistry by OpenStax (2015-05-04)
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Chapter15: Equilibria Of Other Reaction Classes
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Problem 10E: The Handbook of Chemistry and Physics (http://openstaxcollege.org/l/16Handbook) gives solubilities...
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![Instruction: Show your solutions. Observe significant figures.
1. The thiourea in a 1.455 g sample of an organic material was extracted into a dilute H2SO,
solution and titrated with 37.31 mL of 0.009372 M Hg²* via the reaction below.
4(NH2)2CS + Hg² [(NH2)>CS]«Hg²•
What is the percentage of (NH2)2CS 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@) + 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 HCI. Calculate the sulfur
concentration in parts per million.
3. 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+ + Cr2O,2+ 14H* → 6FE3+ + 2Cr³+ + 7H;O
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?
4. A 10.00 mL portion of an HCI solution required 11.01 mL of 0.09883 M NAOH to reach an end
point with phenolphthalein.
HCI + NaOH –→ NaCI + H2O
Calculate the molar concentration of HCI.
5. Describe the preparation of 2.50 L of 0.500 M HCIO4, starting with a 9.00 M solution of the
reagent.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F72826c95-4899-4d14-8ca5-5005055e6f9d%2F97aeedbb-689f-494d-96c6-e86a3553f23f%2Fbl1frtdn_processed.jpeg&w=3840&q=75)
Transcribed Image Text:Instruction: Show your solutions. Observe significant figures.
1. The thiourea in a 1.455 g sample of an organic material was extracted into a dilute H2SO,
solution and titrated with 37.31 mL of 0.009372 M Hg²* via the reaction below.
4(NH2)2CS + Hg² [(NH2)>CS]«Hg²•
What is the percentage of (NH2)2CS 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@) + 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 HCI. Calculate the sulfur
concentration in parts per million.
3. 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+ + Cr2O,2+ 14H* → 6FE3+ + 2Cr³+ + 7H;O
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?
4. A 10.00 mL portion of an HCI solution required 11.01 mL of 0.09883 M NAOH to reach an end
point with phenolphthalein.
HCI + NaOH –→ NaCI + H2O
Calculate the molar concentration of HCI.
5. Describe the preparation of 2.50 L of 0.500 M HCIO4, starting with a 9.00 M solution of the
reagent.
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