NH3 is a bronsted base. It has a lone pair.
The Bronsted-Lowry definition of an acid is a species which can give up an H+ ion, and HSO4- can deprotonate to give SO42- and H+. This is where the second hydrogen ion from sulfuric acid comes from.
NH3 is the conjugate base of NH4+
it can either be an acid or a base depending on its participation in the reaction. if it accepts H+ then it is a base and if it donates H+ then it is an acid..
Substances that can act both as an acid and as a base are called
NH3 is a bronsted base. It has a lone pair.
The Bronsted-Lowry definition of an acid is a species which can give up an H+ ion, and HSO4- can deprotonate to give SO42- and H+. This is where the second hydrogen ion from sulfuric acid comes from.
Yes, the ammonium ion NH4 is a Bronsted-Lowry base.
NH4+ is NH3's conjugate acid. NH3 accepts H+ to become a Bronsted-Lowry base.
Because a bronsted-lowry acid donates proton such as ( H+ ) and water can donate H+ such as ( H2O + NH3 ---> NH4+ + OH- ) here water donated H+ to ammonia to produce NH4 ( which is an acid )
NH3 is the conjugate base of NH4+
it can either be an acid or a base depending on its participation in the reaction. if it accepts H+ then it is a base and if it donates H+ then it is an acid..
Substances that can act both as an acid and as a base are called
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well NH3 is a base that reacts with H2O to get NH4 + OH- NH3+ H2O-->NH4+ + OH- A conjugate base is the species formed when a Bronsted- Lowry base accepts a proton. NH4+ is the conjugate acid of NH3
Yes, it can accept an H+ to form NH4+
Ammonia (NH3) --> can become NH2- or NH4+ Water (H2O) --> can become OH- or H3O+