Question

Label each reactant as either a Bronsted-Lowry acid or a Bronsted-Lowry base.

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

HF(aq) ["Bronsted-Lowry acid", "Bronsted-Lowry base"]

H2O(l) ["Bronsted-Lowry acid", "Bronsted-Lowry base"]

b. HCO3-(aq) + H2O(l) --> H2CO3(aq) + OH-(aq)

HCO3-(aq) ["Bronsted-Lowry base", "Bronsted-Lowry acid"]

H2O(l) ["Bronsted-Lowry acid", "Bronsted-Lowry base"]

Answer 1

a. HF (aq) ["Bronsted-Lowry acid"]

H₂O (l) ["Bronsted-Lowry base"]

b. HCO₃⁻ (aq) ["Bronsted-Lowry base"]

H₂O (l) ["Bronsted-Lowry acid"]

Step-by-step explanation:

Bronsted Lowry theory expose this:

Acid is the one that release a proton

Base is the one that accept a proton

a. HF (aq) + H₂O(l) → H₃O⁺ (aq) + F⁻ (aq)

HF is the acid, it donates the proton to water.

Water is the base, it accepts the H⁺

b. HCO₃⁻ (aq) + H₂O (l) → H₂CO₃ (aq) + OH⁻(aq)

Anion bicarbonate is the base because it accepted the H⁺ from the water, which is the acid.