Which of the following bases would favorably deprotonate a hydroxyl group?
(e)

Verified step by step guidance

1. Identify the pKa of the hydroxyl group. Hydroxyl groups typically have a pKa around 16-18.
2. Consider the concept of acid-base reactions, where a base will deprotonate an acid if the base is stronger than the conjugate base of the acid. This means the base should have a higher pKa than the hydroxyl group.
3. Examine the list of bases provided in the problem. Compare the pKa values of these bases to the pKa of the hydroxyl group.
4. Select the base with a pKa higher than that of the hydroxyl group, as it will be more likely to deprotonate the hydroxyl group.
5. Remember that steric hindrance and solvent effects can also influence the ability of a base to deprotonate a hydroxyl group, but the primary factor is the relative pKa values.

Key Concepts

Acid-Base Chemistry

Acid-base chemistry involves the transfer of protons between molecules. A base is a substance that can accept protons, while an acid can donate them. Understanding the strength of acids and bases is crucial, as stronger bases are more likely to deprotonate acids, such as hydroxyl groups, by accepting their protons.

pKa and Basicity

The pKa value is a measure of the acidity of a substance, indicating how easily it can donate a proton. A lower pKa means a stronger acid. Basicity refers to a base's ability to accept protons. To deprotonate a hydroxyl group, the base must have a higher basicity than the hydroxyl's acidity, which is reflected in its pKa.

Hydroxyl Group Characteristics

A hydroxyl group consists of an oxygen atom bonded to a hydrogen atom (-OH). It is a polar group, making it capable of forming hydrogen bonds. The acidity of the hydroxyl group is relatively weak, so a base must be sufficiently strong to deprotonate it, meaning it must have a higher affinity for protons than the hydroxyl group itself.