Textbook Question
Identify the Lewis acid and the Lewis base in each of the following reactions.
(c)
3. Acids and Bases
Acids and Bases
1:19 minutesProblem 11c
Textbook Question
Identify the acid from which the following conjugate bases were formed. [The most basic atom is indicated.]
(c) 
Verified step by step guidance1
Step 1: Understand the concept of conjugate bases. A conjugate base is formed when an acid donates a proton (H⁺). To identify the acid, you need to add a proton back to the conjugate base.
Step 2: Examine the structure of the conjugate base provided in the problem. Identify the most basic atom, as this is the site where the proton was removed.
Step 3: Add a proton (H⁺) to the most basic atom in the conjugate base. This will reverse the deprotonation process and reconstruct the original acid.
Step 4: Write the chemical formula or structure of the acid formed after adding the proton. Ensure the valency and bonding are correct.
Step 5: Verify the acid by considering its chemical properties and ensuring it matches the expected acid that corresponds to the given conjugate base.
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Video duration:
1mKey Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Acid-Base Theory
Acid-base theory explains the behavior of acids and bases in chemical reactions. According to the Brønsted-Lowry theory, an acid is a proton donor, while a base is a proton acceptor. Understanding this concept is crucial for identifying conjugate acids and bases, as the conjugate base is formed when an acid donates a proton.
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The Lewis definition of acids and bases.
Conjugate Acid-Base Pairs
Conjugate acid-base pairs consist of two species that differ by the presence or absence of a proton. When an acid donates a proton, it becomes its conjugate base, and the base that accepts the proton becomes its conjugate acid. Recognizing these pairs helps in determining the original acid from which a conjugate base is derived.
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Basicity and Electronegativity
Basicity refers to the ability of a species to accept protons, which is influenced by the electronegativity of the atoms involved. The most basic atom in a conjugate base is typically the one that can stabilize the negative charge most effectively. Understanding the relationship between basicity and electronegativity is essential for identifying the original acid based on the properties of its conjugate base.
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