Answer:
Explanation:
The definition of acids and bases by Arrhenius Theory was modified and extended by Bronsted-Lowry.
Bronsted-Lowry defined acid as a molecule or ion which donates a proton while a base is a molecule or ions that accepts the proton. This definition can be extended to include acid -base titrations in non-aqueous solutions.
In this theory, the reaction of an acid with a base constitutes a transfer of a proton from the acid to the base.
From the given information:
[tex]\mathsf{HCN _{(aq)} + H_2O_{(l)} \to CN^{-}_{(aq)} + H_3O_{(aq)}}[/tex]
From above:
We will see that HCN releases an H⁺ ion, thus it is a Bronsted-Lowry acid
[tex]H_2O[/tex] accepts the H⁺ ion ,thus it is a Bronsted-Lowry base.
The formula of the reactant that acts as a proton donor is HCN
The formula of the reactant that acts as a proton acceptor is H2O
