In the following net ionic equation, identify each reactant as either a Bronsted-Lowry acid or a Bronsted-Lowry base. HF-(aq) + H2O(l) rightarrow F-(aq) + H3O(aq)
B-L B-L
The formula of the reactant that acts as a proton donor is.
The formula of the reactant that acts as a proton acceptor is.

Bronsted lowry base = Proton acceptor = H2O

Bronsted lowry acid = Proton donor = HF-

Explanation:

The equation is given as;

HF-(aq) + H2O(l) --> F-(aq) + H3O(aq)

A bronsted lowry base is any specie that can accept hydrogen ion (proton) from another molecule.

Basically a bronsted lowry base is  a proton acceptor while a bronsted lowry acid is a proton donor.

In the reaction above, upon comparing both the reactants and products;

Bronsted lowry base = Proton acceptor = H2O

Bronsted lowry acid = Proton donor = HF-

it would only be the stuff in module eight so you need to study all the lessons in that you also could check the flvs

hope this : )