In alcohols, the more electron-withdrawing the substituent, the more acidic the alcohol. Methyl groups decrease acidity by donating electrons to the oxygen atom.
Step 1: Understanding acidity in alcohols.
The acidity of alcohols is influenced by the electron-donating or electron-withdrawing effects of substituents attached to the carbon atom bonded to the hydroxyl group. The more electron-withdrawing the group, the more acidic the alcohol.
Step 2: Analyzing the options. (A) (CH\(_3\))\(_3\)C-OH: This alcohol is a tertiary alcohol, where the hydroxyl group is attached to a carbon surrounded by three methyl groups. Methyl groups are electron-donating, making the alcohol less acidic. (B) (CH\(_3\))\(_2\)CH-OH: This is a secondary alcohol with electron-donating effects from two methyl groups. It is less acidic than CH\(_3\)OH. (C) CH\(_3\)OH: This is a primary alcohol with no additional electron-donating groups. It is more acidic than tertiary or secondary alcohols. (D) CH\(_3\)-CH\(_2\)-OH: This is also a primary alcohol, but the ethyl group is slightly more electron-donating than the methyl group in CH\(_3\)OH, making it slightly less acidic.
Step 3: Conclusion.
The most acidic alcohol is (C) CH\(_3\)OH, as it is a primary alcohol without electron-donating substituents.
