Both HCO{3}− and HS− are amphoteric. Write an equation to show how each substance can act as an acid and another equation to show how each can act as a base.

Question

Both HCO{3}−  and HS− are amphoteric. Write an equation to show how each substance can act as an acid and another equation to show how each can act as a base.

Ronnie Schechter · Accepted Answer

HCO3−(ag)+HS(ag)⇌CO32−(ag)+H2S(aq) Let HCO{3}− be a Br∅ nsted-Lowry acid and let HS− be a Br∅ nsted-Lowry base. The conjugate base of the acid is then determined by removing an H atom and a unit of positive charge. The conjugate acid of the base is then determined by adding an H atom anda unit of positive charge. HCO3−(ag)+HS−(ag)⇌H2CO3(ag)+S−2(aq) Let HCO{3}− be a ​​​​​​​Br∅ nsted-Lowry base and let HS− be a Br∅ nsted-Lowry acid. The conjugate acid of the base is then determined by adding an H atom anda unit of positive charge. The conjugate base of the acid is then determined by removing an H atom and a unit of positive charge.

soanooooo40 · Accepted Answer

Explanation: According to Bronsted and Lowry an acid is a proton donor and base is a proton acceptor. Therefore, the equation for the reaction will be as follows. HCO3−+HS−=H2CO3+S2t Here, HCO{3}− acts as a base as it is accepting a proton and HS− acts as an acid because it is donating a proton.

Both HCO^{-}_{3} and HS^{-} are amphoteric. Write an equation

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