1. Solve the following queries (parts a), b), & c)) dealing with volumetric analysis. Make sure you show complete procedures a) A 4.912-g sample of a petroleum product was burned in a tube furnace, and the SO₂ produced was collected in 3% H2O2. Reaction: SO2(g) + 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 the sample in parts per million b) The ethyl acetate concentration in an alcoholic solution was determined by diluting a 10.00-mL sample to 100.00 mL. A 20.00-mL portion of the diluted solution was refluxed with 40.00 mL of 0.04672 M KOH: CH3COOC₂H5 + OH¯ → CH3COOC₂H5OH After cooling, the excess OH was back-titrated with 3.41 mL of 0.05042 M H₂SO4. Calculate the amount of ethyl acetate in the original sample in grams. c) The arsenic in a 1.203-g sample of a pesticide was converted to H3ASO4 by suitable treatment. The acid was then neutralized, and 40.00 mL of 0.05871 M AgNO3 was added to precipitate the arsenic quantitatively as Ag3AsO4. The excess Ag+ in the filtrate and in the washings from the precipitate was titrated with 9.63 mL of 0.1000 M KSCN, and the reaction was: Ag+ + SCN → AgSCN (s) Find the percentage of As2O3 in the sample.
1. Solve the following queries (parts a), b), & c)) dealing with volumetric analysis. Make sure you show complete procedures a) A 4.912-g sample of a petroleum product was burned in a tube furnace, and the SO₂ produced was collected in 3% H2O2. Reaction: SO2(g) + 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 the sample in parts per million b) The ethyl acetate concentration in an alcoholic solution was determined by diluting a 10.00-mL sample to 100.00 mL. A 20.00-mL portion of the diluted solution was refluxed with 40.00 mL of 0.04672 M KOH: CH3COOC₂H5 + OH¯ → CH3COOC₂H5OH After cooling, the excess OH was back-titrated with 3.41 mL of 0.05042 M H₂SO4. Calculate the amount of ethyl acetate in the original sample in grams. c) The arsenic in a 1.203-g sample of a pesticide was converted to H3ASO4 by suitable treatment. The acid was then neutralized, and 40.00 mL of 0.05871 M AgNO3 was added to precipitate the arsenic quantitatively as Ag3AsO4. The excess Ag+ in the filtrate and in the washings from the precipitate was titrated with 9.63 mL of 0.1000 M KSCN, and the reaction was: Ag+ + SCN → AgSCN (s) Find the percentage of As2O3 in the sample.
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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show full & complete procedure. Please answer parts a), b) & c). Note they are subparts of the same question
Transcribed Image Text:1. Solve the following queries (parts a), b), & c)) dealing with volumetric analysis. Make sure you show complete
procedures
a)
A 4.912-g sample of a petroleum product was burned in a tube furnace, and the
SO2 produced was collected in 3% H2O2. Reaction:
SO2(g) + 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 the sample in parts per
million
b)
The ethyl acetate concentration in an alcoholic solution was determined by
diluting a 10.00-mL sample to 100.00 mL. A 20.00-mL portion of the diluted
solution was refluxed with 40.00 mL of 0.04672 M KOH:
CH3COOC₂H5 + OH¯ → CH3COOC₂H5OH
After cooling, the excess OH was back-titrated with 3.41 mL of 0.05042 M H₂SO4.
Calculate the amount of ethyl acetate in the original sample in grams.
c)
The arsenic in a 1.203-g sample of a pesticide was converted to H3AsO4 by
suitable treatment. The acid was then neutralized, and 40.00 mL of 0.05871 M
AgNO3 was added to precipitate the arsenic quantitatively as Ag3AsO4. The
excess Ag+ in the filtrate and in the washings from the precipitate was titrated
with 9.63 mL of 0.1000 M KSCN, and the reaction was:
Ag+ + SCN¯ → AgSCN (s)
Find the percentage of As2O3 in the sample.
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