What Makes an Acid the Strongest?

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SUMMARY

This discussion focuses on the acidity of benzylic alcohol and phenols, specifically examining the influence of electron-withdrawing groups on acidity. It is established that phenols are generally more acidic than alcohols due to their ability to stabilize the negative charge after deprotonation. The presence of an electron-withdrawing group para to the hydroxyl (OH) group enhances acidity by stabilizing the conjugate base, making it easier to remove a proton (H+).

PREREQUISITES
  • Understanding of acid-base chemistry
  • Familiarity with the concept of conjugate bases
  • Knowledge of electron-withdrawing and electron-donating groups
  • Basic principles of organic chemistry
NEXT STEPS
  • Research the effects of different electron-withdrawing groups on acidity
  • Study the concept of resonance stabilization in conjugate bases
  • Explore the acidity of various functional groups in organic compounds
  • Learn about the comparative acidity of alcohols versus phenols
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Chemistry students, organic chemists, and anyone interested in understanding the principles of acidity in organic compounds.

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So, you have a benzylic alcohol and two phenols. Are phenols more or less acidic than alcohols? One of the phenols has an electron withdrawing group para to the OH. Do electron withdrawing groups increase or decrease acidity?
 
More acidic?
 
the stronger the acid, the easier it will be to remove a proton(H+) from it.
 

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