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

Both $$\displaystyle{H}{C}{O}^{{-}}_{\left\lbrace{3}\right\rbrace}$$ and $$\displaystyle{H}{S}^{{-}}$$ 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.

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Ronnie Schechter

$$HCO_3^{-}(ag) + HS(ag) \rightleftharpoons CO_3^{2-}(ag) + H_2S(aq)$$
Let $$\displaystyle{H}{C}{O}^{{-}}_{\left\lbrace{3}\right\rbrace}$$ be a $$Br\emptyset$$ nsted-Lowry acid and let $$HS^{-}$$ be a $$Br\emptyset$$ 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.
$$HCO_3^{-}(ag) + HS^{-}(ag) \rightleftharpoons H_2CO_3(ag) + S^{-2}(aq)$$
Let $$\displaystyle{H}{C}{O}^{{-}}_{\left\lbrace{3}\right\rbrace}$$ be a ​​​​​​​$$Br\emptyset$$ nsted-Lowry base and let $$HS^{-}$$
be a $$Br\emptyset$$ 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.

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soanooooo40

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.
$$HCO^{-}_{3}+ HS^{-}= H_{2}CO_{3} +S^{2} t$$
Here, $$\displaystyle{H}{C}{O}^{{-}}_{\left\lbrace{3}\right\rbrace}$$ acts as a base as it is accepting a proton and $$\displaystyle{H}{S}^{{-}}$$ acts as an acid because it is donating a proton.