Given the equation representing a reaction at equilibrium: h2s(aq) ch3nh2(aq) hs(aq) ch3nh3 (aq) according to one acid-base theory, the forward reaction is classified as an acid-base reaction because

loses proton and accepts proton

Explanation: According to the Bronsted-Lowry conjugate acid-base theory, an acid is defined as a substance which looses donates protons and thus forming conjugate base and a base is defined as a substance which accepts protons and thus forming conjugate acid.

For the given chemical equation:

Here, is loosing a proton, thus it is considered as an acid and after losing a proton, it forms which is a conjugate base.

And, is gaining a proton, thus it is considered as a base and after gaining a proton, it forms which is a conjugate acid.

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am i too late?

explanation: