Complete this brønsted-lowry reaction, placing each product by its appropriate label. hco3-+f-

Brønsted-Lowry reaction

HCO₃⁻ + F⁻ ⇔ CO₃⁻² + HF

Acids and bases according to Bronsted-Lowry

If the acid gives (H⁺), then the remaining acid is a conjugate base because it receives protons. Conversely, if a base receives (H +), then the base formed has the ability to release protons and is called the conjugate acid from the original base.

Can be formulated:

Acid ⇒ H⁺ + conjugate base

Bases + H⁺⇒ conjugate acids

So that in the Bronsted-Lowry acid-base reaction the acid turns into a conjugate base while the base turns into a conjugate acid. Then there will be two conjugate acid-base pairs. There is a difference of one proton (H⁺) from the conjugate acid-base pair

In this concept, it can also be explained that strong acids are substances that easily release protons, and strong bases are substances that have a strong tendency to attract electrons

Example

NH₃ (aq) + H₂O (l) ⇔NH₄⁺ (aq) + OH⁻ (aq)

The acid-base conjugate pair is:

H₂O as an acid gives a proton to NH₃ so that it becomes NH₄ so that the remaining OH- as its conjugate base

While NH₃ as a base and NH₄ as a conjugate acid

In reaction:

HCO₃⁻ + F⁻ ⇔ CO₃⁻² + HF

HCO₃⁻ is acid because it donates its proton and its conjugate base is CO₃⁻²

 F⁻ as a base because it accepts protons becomes its conjugate acid, HF

The acid-base conjugate pair is:

the Bronsted-Lowry definition of an acid

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the Bronsted-Lowry definition of a base

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the acids and the bases in the chemical equation according to Bronsted-Lowry Theory

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Keywords: Bronsted-Lowry Theory, acid, base, proton, donor, acceptor, acid-base conjugate

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