Sulfate (SO2) is typically determined by dissolving in H₂O followed by precipitation as BaSO4 via addition of BaCl₂. Calculate the percent (w/w) Na2SO4 (FW-142.04) in an unknown sample based on the data below? What percent SO, (FW-80.06) is in the unknown sample? Constant weight of crucible: 25.6390 g Weight of vial with solid unknown sample: 13.1131 g Weight of vial minus some sample: 12.4122 g Weight of crucible + BaSO4 after 1" heating (ignition): 25.9365 g Weight of crucible + BaSO4 after 2nd heating (ignition): 25.9348 g Weight of crucible +BaSO, after 3rd heating (ignition): 25.9347 g

Sulfate (SO2) is typically determined by dissolving in H₂O followed by precipitation as BaSO4 via addition of BaCl₂. Calculate the percent (w/w) Na2SO4 (FW-142.04) in an unknown sample based on the data below? What percent SO, (FW-80.06) is in the unknown sample? Constant weight of crucible: 25.6390 g Weight of vial with solid unknown sample: 13.1131 g Weight of vial minus some sample: 12.4122 g Weight of crucible + BaSO4 after 1" heating (ignition): 25.9365 g Weight of crucible + BaSO4 after 2nd heating (ignition): 25.9348 g Weight of crucible +BaSO, after 3rd heating (ignition): 25.9347 g

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter8: Thermochemistry

Section: Chapter Questions

Problem 11QAP: When one mol of KOH is neutralized by sulfuric acid, q=56 kJ. (This is called the heat of...

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When one mol of KOH is neutralized by sulfuric acid, q=56 kJ. (This is called the heat of neutralization.) At 23.7C, 25.0 mL of 0.475 M H2SO4 is neutralized by 0.613 M KOH in a coffee-cup calorimeter. Assume that the specific heat of all solutions is 4.18J/gC, that the density of all solutions is 1.00 g/mL, and that volumes are additive. (a) How many mL of KOH is required to neutralize H2SO4? (b) What is the final temperature of the solution?
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