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.
It is both. H2PO4 is a bronsted acid and a bronsted base.
By definition, any compound that donates a proton is called a Bronsted-Lowry acid. NH4+ doesn't have the tendency to donate H+ ion and hence is not a Bronsted acid.
NH3 is a bronsted base. It has a lone pair.
Substances that can act both as an acid and as a base are called
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..
The conjugate base for acid NH4+ is NH3 (ammonia). When NH4+ loses a proton, it forms NH3, which can act as a weak base in a chemical reaction.
base
NH3 is a bronsted base. It has a lone pair.
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 )
Yes, the ammonium ion NH4 is a Bronsted-Lowry base.
Substances that can act both as an acid and as a base are called
The conjugate base for acid NH4+ is NH3 (ammonia). When NH4+ loses a proton, it forms NH3, which can act as a weak base in a chemical reaction.
The species that contains the greatest percent by mass of hydrogen is H3O with a plus 1 charge on the Oxygen molecule. The species that is the Bronsted-Lowery acid in the forward reaction is NH4 with a plus 1 charge.
Hpo2- +f-
Nh4+ Apex
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..
Water can act as both a BrΓΈnsted-Lowry acid and base. As an acid, it donates a proton (H+) to a base; as a base, it accepts a proton from an acid. This ability is due to its amphiprotic nature.
Bronsted Base