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Complete these Brønsted-Lowry reactions:
HSO4- + H+ <-->
HSO4- +OH- <-->
1 answer
Can't you just add them?
HSO4- + H+ ==> H2SO4
HSO4- + OH- ==> H2O + SO4^2-
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H2SO4(aq) + H2O(l) ⟶ H3O+(aq) + HSO4–(aq) (Stage I)
Identify the Brønsted-Lowry acid and base in the reaction.
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Identify the products formed in this Brønsted-Lowry reaction.
HSO4^−+HBrO↽−−⇀acid+base
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Calculate the pH of the following aqueous solution:
1.00 mol/L sulfuric acid, H2SO4(aq) H2SO4 ==> H^+ + HSO4^- 100% HSO4^- ==>
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Calculate the pH of the following aqueous solutions:
1.00 mol/L sulfuric acid H+ = 1.00 M for the first ionization THe second one
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