Write the conjugated acids for the following Bronsted bases: NH₂, NH₃, and HCOO⁻.

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Points to Remember:

  • Brønsted-Lowry acid-base theory defines an acid as a proton (H⁺) donor and a base as a proton acceptor.
  • The conjugate acid of a base is formed by adding a proton (H⁺) to the base.

Introduction:

The Brønsted-Lowry theory provides a comprehensive framework for understanding acid-base reactions. A Brønsted-Lowry base accepts a proton (H⁺) from an acid. When a base accepts a proton, it forms its conjugate acid. This conjugate acid is simply the base with an additional proton. This question requires identifying the conjugate acids for three given Brønsted bases: NH₂, NH₃, and HCOO⁻. This will be achieved by systematically adding a proton to each base.

Body:

1. Conjugate Acid of NH₂⁻:

The base NH₂⁻ (amide ion) accepts a proton (H⁺) to form its conjugate acid. The reaction is:

NH₂⁻ + H⁺ → NH₃

Therefore, the conjugate acid of NH₂⁻ is NH₃ (ammonia).

2. Conjugate Acid of NH₃:

Ammonia (NH₃) acts as a base in the presence of a stronger acid. When it accepts a proton, it forms its conjugate acid:

NH₃ + H⁺ → NH₄⁺

Therefore, the conjugate acid of NH₃ is NH₄⁺ (ammonium ion).

3. Conjugate Acid of HCOO⁻:

The formate ion (HCOO⁻) is a weak base. Upon accepting a proton, it forms its conjugate acid:

HCOO⁻ + H⁺ → HCOOH

Therefore, the conjugate acid of HCOO⁻ is HCOOH (formic acid).

Conclusion:

In summary, the conjugate acids for the given Brønsted bases are: NH₃ for NH₂⁻, NH₄⁺ for NH₃, and HCOOH for HCOO⁻. Understanding conjugate acid-base pairs is crucial in predicting the outcome of acid-base reactions and in comprehending the behavior of various chemical species in solution. This knowledge is fundamental to many areas of chemistry, including analytical chemistry, biochemistry, and environmental science. Further exploration of acid-base equilibria and the concept of pKa values would provide a more complete understanding of the strength and reactivity of these acids and bases. This foundational knowledge contributes to a more holistic understanding of chemical processes.

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