what is the conjugate acid of nh3
What is the conjugate acid of NH₃?
Answer: To understand the concept of conjugate acids and bases, we can refer to the Brønsted-Lowry theory of acids and bases. According to this theory, an acid is a species that donates a proton (H⁺ ion), while a base is a species that accepts a proton.
NH₃ (ammonia) is a common example of a Brønsted-Lowry base. When NH₃ accepts a proton (H⁺), it forms its conjugate acid. The protonation of NH₃ can be represented by the following chemical equation:
\text{NH}_{3} + \text{H}^{+} \rightarrow \text{NH}_{4}^{+}
Here, the ammonia molecule (NH₃) accepts a proton from an acid, resulting in the formation of NH₄⁺ (ammonium ion). Therefore, NH₄⁺ is the conjugate acid of NH₃.
Explanation:
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Base (NH₃): A base is defined as a species that has a tendency to accept a proton. NH₃ is a base because it can accept a proton (H⁺) from an acid.
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Conjugate Acid (NH₄⁺): The species that results from the addition of a proton to the base is called the conjugate acid. When NH₃ gains an H⁺ ion, it forms NH₄⁺, which is its conjugate acid.
General Concept of Conjugate Acid-Base Pairs:
- Base: NH₃
- Accepts proton (H⁺) to become
- Conjugate Acid: NH₄⁺
Strategic Importance:
Understanding conjugate acids and bases helps in predicting the outcome of acid-base reactions and is fundamental to many areas of chemistry, including acid-base equilibrium, buffer solutions, and chemical reactivity.
Example Reaction:
\text{NH}_{3} + \text{HCl} \rightarrow \text{NH}_{4}Cl
In this reaction, NH₃ acts as a base and accepts a proton from hydrochloric acid (HCl), forming the ammonium ion (NH₄⁺) and chloride ion (Cl⁻).
Thus, the conjugate acid of NH₃ is \boxed{\text{NH}_{4}^{+}} (ammonium ion). This is a critical concept in both general and organic chemistry, affecting reaction mechanisms and the behavior of substances in solution.