Textbook Question
The following compounds can all react as acids.
b. Rank the conjugate bases in the order you would predict, from most stable to least stable.
3. Acids and Bases
Acids and Bases
3:06 minutesProblem 42e
Textbook Question
Predict the products of the following acid–base reactions.
(e) H2O + NH3 ⇌
Verified step by step guidance1
Identify the acid and base in the reaction. In this case, water (H2O) can act as an acid, donating a proton (H⁺), and ammonia (NH3) can act as a base, accepting a proton.
Write the chemical equation for the proton transfer. Water donates a proton to ammonia, forming hydroxide ion (OH⁻) and ammonium ion (NH4⁺).
Use MathML to represent the chemical equation:
Consider the equilibrium of the reaction. The double arrow (⇌) indicates that the reaction can proceed in both directions, meaning the products can revert to reactants.
Understand the concept of conjugate acid-base pairs. In this reaction, NH3 and NH4⁺ are a conjugate acid-base pair, and H2O and OH⁻ are another conjugate acid-base pair.
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Video duration:
3mKey Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Acid-Base Reaction
An acid-base reaction involves the transfer of a proton (H+) from an acid to a base. In the given reaction, water (H2O) acts as an acid, donating a proton to ammonia (NH3), which acts as a base. Understanding the roles of acids and bases is crucial for predicting the products of such reactions.
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02:49
The Lewis definition of acids and bases.
Bronsted-Lowry Acid and Base
The Bronsted-Lowry theory defines acids as proton donors and bases as proton acceptors. In the reaction H2O + NH3, H2O donates a proton to NH3, forming OH- and NH4+. This concept helps in identifying the conjugate acid-base pairs and predicting the products formed in the reaction.
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00:54The Bronsted-Lowry definition of acids and bases.
Conjugate Acid-Base Pair
A conjugate acid-base pair consists of two species that differ by a proton. In the reaction, H2O and OH- form a conjugate acid-base pair, while NH3 and NH4+ form another. Recognizing these pairs is essential for understanding the equilibrium and direction of acid-base reactions.
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2:56Base Pairing Concept 1
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