1. Analyst A bought a powder that contains sulfate ions, reported as 25.00% sulfur trioxide (MW 80.07 g/mol). In a 5.00-g sample dissolved in 100 mL water, how much BaSO4 (MW 233.39 g/mol) will precipitate if 50.0 mL of 0.200 M BaCl2 was used?a. 0.429 gb. 2.33 gc. 0.800 gd. 3.64 g 2. If the dried crucible weighs 1.4834 g and the dried crucible + BaSO4 (MW 233.39 g/mol) precipitate weighs 1.6858 g, what is the percent sulfite (MW 80.07 g/mol) if the starting sample weighs 500.0 mg?a. 13.89%b. 20.5%c. 29.1%d. 59.7%3. What is the minimum mass of BaCl2 (MW = 208.23 g/mol) required to be dissolved in 100.0 mL of H2O if all of this will be mixed with 200.0 mL of 0.100 M Na2SO4 (MW = 142.04 g/mol) to ensure complete precipitation?a. 3.83 gb. 2.84 gc. 4.16 gd. 2.08 g

SO3 + BaCl2 + H2O gives BaSO4 + 2 HCl So, 1 mol of sulphur trioxide will react with 1 mol…

Answered: 1. Analyst A bought a powder that…

Chemistry by OpenStax (2015-05-04)

1st Edition

ISBN:9781938168390

Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Chapter15: Equilibria Of Other Reaction Classes

Section: Chapter Questions

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1. Analyst A bought a powder that contains sulfate ions, reported as 25.00% sulfur trioxide (MW 80.07 g/mol). In a 5.00-g sample dissolved in 100 mL water, how much BaSO₄ (MW 233.39 g/mol) will precipitate if 50.0 mL of 0.200 M BaCl₂ was used?

a. 0.429 g

b. 2.33 g

c. 0.800 g

d. 3.64 g

2. If the dried crucible weighs 1.4834 g and the dried crucible + BaSO₄ (MW 233.39 g/mol) precipitate weighs 1.6858 g, what is the percent sulfite (MW 80.07 g/mol) if the starting sample weighs 500.0 mg?

a. 13.89%

b. 20.5%

c. 29.1%

d. 59.7%

3. What is the minimum mass of BaCl₂ (MW = 208.23 g/mol) required to be dissolved in 100.0 mL of H₂O if all of this will be mixed with 200.0 mL of 0.100 M Na₂SO₄ (MW = 142.04 g/mol) to ensure complete precipitation?

a. 3.83 g

b. 2.84 g

c. 4.16 g

d. 2.08 g

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