See image — GOC and Organic Chemistry Basics Chemistry Question

💡 Solution & Explanation

# Determining the Most Acidic Hydrogen ## Analysis of Each Option: **(A) Diketone (1,3-dicarbonyl compound):** - $\alpha$-hydrogens between two carbonyl groups are acidic due to resonance stabilization of the conjugate base - However, these hydrogens are on $sp^3$ carbon **(B) Cyclic ketone:** - $\alpha$-hydrogens to a single carbonyl - Standard ketone acidity; less acidic than option C **(C) $(CH_3CO)_3CH$ - Tricarbonyl compound:** - This is a **triketone** with the central H attached to a carbon bearing **three acetyl groups** - The H is on a carbon directly bonded to three electron-withdrawing carbonyl groups - The conjugate base is stabilized by **three resonance structures** simultaneously: $$\text{R}_3\overset{+}{C}-H \rightleftharpoons \text{R}_3C^- + H^+$$ - Multiple electron-withdrawing groups dramatically increase acidity **(D) $(CH_3)_3COH$ - Tertiary butanol:** - Simple alcohol with only one OH - Alcohols are much weaker acids than carbonyl-activated hydrogens - No resonance stabilization of conjugate base ## Why (C) is Correct: The hydrogen in option (C) is bonded to a carbon flanked by **three carbonyl groups**, making it extraordinarily acidic. The conjugate base is stabilized by three resonance structures through the electron-withdrawing effect of three carbonyls simultaneously, far exceeding the stabilization in any other option. **Answer: (C)**