Bronsted-Lowry Acid/Base Theory

Front

What is the Bronsted-Lowry Acid/Base Theory?

Back

The Bronsted-Lowry Acid/Base Theory defines acids as proton (H+) donors and bases as proton (H+) acceptors.

Front

Identify a Bronsted-Lowry acid in the reaction: H₂O + HCl → H₃O⁺ + Cl^-.

Back

Hydrogen chloride (HCl) is the Bronsted-Lowry acid as it donates a proton to water.

Front

What is a conjugate base?

Back

A conjugate base is the species that remains after an acid donates a proton.

Front

Identify the conjugate base in the reaction: HCO₃^- + HCl → H₂CO₃ + Cl^-.

Back

The conjugate base is Cl^-.

Front

Identify the Bronsted-Lowry acid in the reaction: HSO₄^- + H₂O → H₃O⁺ + SO₄^2-.

Back

HSO₄^- is the Bronsted-Lowry acid as it donates a proton.

Front

What is a Bronsted-Lowry base?

Back

A Bronsted-Lowry base is a substance that accepts a proton (H+).

Front

Identify the Bronsted-Lowry base in the reaction: HCl + NH₃ → Cl^- + NH₄⁺.

Back

NH₃ is the Bronsted-Lowry base as it accepts a proton from HCl.

Front

What does it mean for a substance to donate H+?

Back

To donate H+ means that the substance acts as a Bronsted-Lowry acid, releasing a proton to another substance.

Front

What is the relationship between acids and their conjugate bases?

Back

When an acid donates a proton, it forms its conjugate base, which can accept a proton in a reverse reaction.

Front

What is the relationship between bases and their conjugate acids?

Back

When a base accepts a proton, it forms its conjugate acid, which can donate a proton in a reverse reaction.