Hco3- => h2co3
The Bronsted-Lowry definition describes acids as being proton (H+) donators and bases as being proton acceptors. So the answer would be C, because the carbonate anion is accepting a proton (H+ cation) to become the HCO3-
The anion of Lowery-Bronsted acid acts as the conjugate base in this case, for example the conjugate base of HCl is Cl anion.
the Bronsted-Lowry theory classifies a substance as an acid if it acts as a proton(H+) donor, and as a base if it acts as a proton acceptor.
base
no, arhenious base is also a bronsted lowry base
The Bronsted-Lowry definition describes acids as being proton (H+) donators and bases as being proton acceptors. So the answer would be C, because the carbonate anion is accepting a proton (H+ cation) to become the HCO3-
The anion of Lowery-Bronsted acid acts as the conjugate base in this case, for example the conjugate base of HCl is Cl anion.
Bronsted Base
the Bronsted-Lowry theory classifies a substance as an acid if it acts as a proton(H+) donor, and as a base if it acts as a proton acceptor.
It is a Bronsted base.
base
Dissolving formic acid in water the formiate ion formed is the conjugate base of the acid.
no, arhenious base is also a bronsted lowry base
A Bronsted-Lowry base is a proton acceptor.
A Bronsted-Lowery base accepts H+ ions
a bronsted base can accept at least one H+ ion once dissolved, for instance SO42- is a bronsted base because it can accept 2 H+ ions to become H2SO42- (which is then considered a bronsted acid)
A Bronsted-Lowery base accepts H+ ions