Textbook Question
Based on the one species that is identified for you, label the remaining molecules as acid, base, conjugate acid, or conjugate base.
(a)
3. Acids and Bases
Acids and Bases
3:54 minutesProblem 9d
Textbook Question
What is the conjugate base of each of the following acids? [The most acidic proton is indicated.]
(d) 
Verified step by step guidance1
Identify the acidic proton in the molecule. In this case, the blue arrow points to the hydrogen atom attached to the oxygen in the hydroxyl (-OH) group.
Recall that the conjugate base is formed by removing the most acidic proton from the molecule. This involves deprotonation of the hydroxyl group.
Write the chemical equation for the deprotonation process: \( \text{R-OH} \rightarrow \text{R-O}^- + \text{H}^+ \), where \( \text{R} \) represents the cyclohexyl group.
Recognize that the conjugate base of the acid is the cyclohexoxide ion (\( \text{R-O}^- \)), which is the cyclohexyl group bonded to an oxygen atom carrying a negative charge.
Ensure that the negative charge on the oxygen is properly represented, as it results from the loss of the proton during deprotonation.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Acid-Base Chemistry
Acid-base chemistry involves the transfer of protons (H+) between species. An acid is defined as a proton donor, while a base is a proton acceptor. Understanding this concept is crucial for identifying conjugate acid-base pairs, where the conjugate base is formed when an acid donates a proton.
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The Lewis definition of acids and bases.
Conjugate Base
The conjugate base of an acid is what remains after the acid has donated a proton. For example, when phenol (C6H5OH) donates its acidic proton from the hydroxyl group, it forms the phenoxide ion (C6H5O-), which is its conjugate base. Recognizing the structure of the conjugate base is essential for predicting its reactivity and properties.
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Resonance Stabilization
Resonance stabilization refers to the delocalization of electrons across multiple atoms in a molecule, which can enhance stability. In the case of phenoxide ion, the negative charge on the oxygen can be delocalized into the aromatic ring, making the conjugate base more stable than if the charge were localized. This concept is important for understanding the acidity of phenols compared to other alcohols.
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