1) A mixture of 5.1 x 10-3 moles of HSO4 (hydrogen sulfate) is dissolved in 25 mL of water. At equilibrium the vessel contains SO4² (sulfate) and H3O+ (hydronium). What is the pH at equilibrium? HSO4 (aq) + H2O(l) = SO4²¯(aq) + H3O+(aq) Ka = 1.2 x 10-2
1) A mixture of 5.1 x 10-3 moles of HSO4 (hydrogen sulfate) is dissolved in 25 mL of water. At equilibrium the vessel contains SO4² (sulfate) and H3O+ (hydronium). What is the pH at equilibrium? HSO4 (aq) + H2O(l) = SO4²¯(aq) + H3O+(aq) Ka = 1.2 x 10-2
Chemistry
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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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Give the explanation formula which using for the calculation.
Transcribed Image Text:1) A mixture of 5.1 x 10-3 moles of HSO4 (hydrogen sulfate) is dissolved in 25 mL of water. At
equilibrium the vessel contains SO4² (sulfate) and H3O+ (hydronium). What is the pH at equilibrium?
HSO4 (aq) + H2O(l) = SO4²¯(aq) + H3O+(aq)
Ka = 1.2 x 10-2
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