bronsted lowry / arrhenius?

Question

In this expression what is acting as the Bronsted-Lowry acid and the Bronsted-Lowry base? What is acting as the Arrhenius acid and the Arrhenius base?

HCO3- + H2O <--> H3O+ + CO3^2-

Answer 1

bronsted lowry acids are those that can donate H+
bronsted lowry bases are those that can accept H+
Arrhenius acids are those that can donate H+
Arrhenius bases are those that can donate -OH

in this given equation:
the bronsted acid and arrhenius was HCO3-
the bronsted base was H2O
since no -OH was donated then either the Arrhenius base was H2O or there's no Arrhenius base in the rxn, however, that's not possible thus H2O is still the Arrhenius base

Answer 2

1. Bronsted-Lowry acid - donates protons (hydrogen ion)
HCO3- , proton is donated to water
(CO3^2- is the conjugate base referring to the reverse direction)

2. Bronsted-Lowry base - accepts protons
H2O - accepts protons to form H3O
(H3O is the conjugate acid - in the reverse direction)

3. Arrhenius acid - dissolved in water increases conc of protons - in this case it is HCO3 - (because although we see that the reaction product in the forward direction is H3O - in actuality, the solvation of the H+ is much more complicated)

4. Arrhenius base - dissolved in water increases the concentration of OH-
in the reaction, there is no Arrhenius base