Answer At 25 °C, only 2.45 mg of barium sulfate will dissolve in 1.00 L water (see thereaction below). What is the equilibrium constant for this reaction?• barium sulfate molar mass = 233.38 g/mol• 1000 mg = 1gBaSO4 (s) = Ba²+ (aq) + SO²¯ (aq)O4.63 x 10-6о6.00 x 10-41.10 x 10-101.05 x 10-54.63 x 10-15OO

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At 25 °C, only 2.45 mg of barium sulfate will dissolve in 1.00 L water (see the reaction below). What is the equilibrium constant for this reaction? D barium sulfate molar mass = 233.38 g/mol . 1000 mg = 1g = Ba2+ (aq) + SO4²- (aq) BaSO4(s) = O 4.63 x 10-6 6.00 x 10-4 1.10 x 10-10 O

At 25 °C, only 2.45 mg of barium sulfate will dissolve in 1.00 L water (see the reaction below). What is the equilibrium constant for this reaction? D barium sulfate molar mass = 233.38 g/mol . 1000 mg = 1g = Ba2+ (aq) + SO4²- (aq) BaSO4(s) = O 4.63 x 10-6 6.00 x 10-4 1.10 x 10-10 O

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 12.27PAE: The following data were collected for a system at equilibrium at 140°C. Calculate the equilibrium...

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Answer

At 25 °C, only 2.45 mg of barium sulfate will dissolve in 1.00 L water (see the
reaction below). What is the equilibrium constant for this reaction?
• barium sulfate molar mass = 233.38 g/mol
• 1000 mg = 1g
BaSO4 (s) = Ba²+ (aq) + SO²¯ (aq)
O
4.63 x 10-6
о
6.00 x 10-4
1.10 x 10-10
1.05 x 10-5
4.63 x 10-15
O
O

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