Textbook Question
Based on the one species that is identified for you, label the remaining molecules as acid, base, conjugate acid, or conjugate base.
(b)
3. Acids and Bases
Acids and Bases
3:43 minutesProblem 10a
Textbook Question
What is the conjugate acid of each of the following bases? [The most basic atom is indicated.]
(a) 
Verified step by step guidance1
Step 1: Identify the base in the given structure. The base is the negatively charged carbon atom (CH₂⁻) in the ethyl anion (CH₃CH₂⁻).
Step 2: Recall the concept of conjugate acids and bases. A conjugate acid is formed when a base gains a proton (H⁺).
Step 3: Add a proton (H⁺) to the most basic atom, which is the negatively charged carbon atom in this case. This will neutralize the negative charge.
Step 4: Write the resulting chemical structure after the proton is added. The ethyl anion (CH₃CH₂⁻) becomes ethane (CH₃CH₃).
Step 5: Verify the result by checking that the conjugate acid (CH₃CH₃) is neutral and consistent with the addition of a proton to the base.
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Video duration:
3mKey Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Conjugate Acid-Base Pair
A conjugate acid is formed when a base accepts a proton (H+). In acid-base chemistry, every base has a corresponding conjugate acid, which is the species that results from the base gaining a proton. Understanding this relationship is crucial for predicting the behavior of substances in chemical reactions.
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Base Pairing Concept 1
Basicity and Proton Affinity
Basicity refers to the ability of a substance to accept protons. The most basic atom in a molecule is typically the one with the highest electron density and the ability to stabilize the positive charge after accepting a proton. This concept is essential for identifying which atom in a given structure will form the conjugate acid.
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06:21Understanding the difference between basicity and nucleophilicity.
Resonance Stabilization
Resonance stabilization occurs when a molecule can be represented by multiple valid Lewis structures, allowing for the delocalization of electrons. This delocalization can significantly affect the stability of the conjugate acid formed from a base, influencing its acidity and basicity. Recognizing resonance structures helps predict the strength of acids and bases.
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03:43The radical stability trend.
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