Question

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

Answer 1

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The complete Brønsted-Lowry reaction is the following:

HCO₃⁻ +   F⁻    ⇄       CO₃⁻²   +     HF

Acid      Base      Conj. Base        Conj. Acid

The Brønsted-Lowry theory establishes that acids are substances capable of donating protons (H⁺) and bases are substances capable of accepting them. HCO₃⁻ is the Acid in the Reaction, as it donates its protons, and F⁻ is the base. In Acid-Base reactions, Acids transform into their conjugate base, and Bases transform into their conjugate acids, so HCO₃⁻ transforms into CO₃⁻² and F⁻ transforms into HF.

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Answer 2

Brønsted-Lowry reaction

HCO₃⁻ + F⁻ ⇔ CO₃⁻² + HF

Further explanation

Acids and bases according to Bronsted-Lowry

• Acid = donor (donor) proton (H⁺ ion)
• Base = proton (receiver) acceptor (H⁺ ion)

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:

• NH₃ and NH₄
• H₂O and OH⁻

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:

• HCO₃⁻ and CO₃⁻²
•  F⁻ and HF

Learn more

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