1. Phenols are more acidic than alcohols because:
   1. Easier hydrogen release: Lone pair electrons on oxygen in phenols are delocalized through resonance, stabilizing the phenoxide ion.
   2. Phenoxide ion stability: The negative charge in the phenoxide ion is delocalized, enhancing stability.

Alcohols do not exhibit such resonance stabilization.

Reactions highlighting acidity

1. Reaction with alkaline solutions: Phenols react with NaOH to form sodium phenoxide, while alcohols do not.

   $C_6H_5OH + NaOH \rightarrow C_6H_5ONa + H_2O$

2. Reaction with sodium carbonate: Phenols release $CO_2$, while alcohols do not.

3. Reaction with carboxylic acids: Alcohols form esters, but phenols do not react in this manner.

1. Replacement of hydrogen in the –OH group:

   • React with alkali metals to form alkoxides and release hydrogen gas.

     $ROH + Na \rightarrow RONa + H_2$

2. Replacement of the –OH group:

   • Halogenation: Alcohols react with halogenating agents to form alkyl halides.

     $C_2H_5OH + PCl_5 \rightarrow C_2H_5Cl + POCl_3 + HCl$

3. Oxidation:

   1. Primary alcohols: Form aldehydes with mild oxidizing agents and carboxylic acids with strong oxidizing agents.
   2. Secondary alcohols: Oxidize to ketones.
   3. Tertiary alcohols: Resistant to oxidation due to the absence of a hydrogen atom on the carbon bonded to –OH.

Lucas test

1. Primary alcohols: No turbidity.
2. Secondary alcohols: Turbidity within 5 minutes.
3. Tertiary alcohols: Immediate turbidity.

Phenol tests

1. Turns blue litmus paper red.
2. Forms violet color with $FeCl_3$.
3. Reacts with bromine water to form white precipitate.

Similarities

1. Evolve hydrogen gas with alkaline metals.
2. Form ethers with haloalkanes.
3. React with hydrogen halides.

Differences