Explain amphoteric nature of water.
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One of the two water molecules acts as an Bronsted-Lowry acid and donates a proton to the other water molecule, which subsequently acts as a Bronsted-Lowry base.
Water can act as an acid or as a base in various chemical reactions, the most common two examples involving the ammonia and hydrochloric acid reactions.
NH3(aq)+H2O(l)⇌NH+4(aq)+OH−(aq)
Here water acts as a Bronsted-Lowry acid because it donates a proton to ammonia.
HCl(g)+H2O((l))⇌H3O+(aq)+Cl−(aq)
This time water acts a Bronsted-Lowry base because it accepts a proton from hydrochloric acid.
To be exact, in reactions that involve the transfer of protons, the term is actually amphiprotic.
Water can act as an acid or as a base in various chemical reactions, the most common two examples involving the ammonia and hydrochloric acid reactions.
NH3(aq)+H2O(l)⇌NH+4(aq)+OH−(aq)
Here water acts as a Bronsted-Lowry acid because it donates a proton to ammonia.
HCl(g)+H2O((l))⇌H3O+(aq)+Cl−(aq)
This time water acts a Bronsted-Lowry base because it accepts a proton from hydrochloric acid.
To be exact, in reactions that involve the transfer of protons, the term is actually amphiprotic.
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