Question

How do you prove that alcohols are weaker acids than water?

Answer 1

Hint: Water is a preferable corrosive over liquor on account of the electron-giving nature of the alkyl bunch joined to the oxygen which destabilizes the hydroxide (in the instance of liquor, Alkoxide) ion and makes it harder for the oxygen to give the proton.

Complete answer:
I'll clarify why this issue from two points of view - the connection among oxygen and hydrogen in the - OH gathering and the solidness of the form base. When contrasting the corrosive strength of alcohols and water, you should take a gander at how "energetic" the acidic proton is to hop off. A liquor's causticity comes from the significant distinction in electronegativity between the oxygen and the hydrogen in the joined - OH gathering.
Oxygen, being the more electronegative of the two particles in the practical gathering, will draw in the bond electrons towards itself; this thusly will make the proton simpler to pull off. Be that as it may, on account of liquor, the alkyl gathering will "push" electrons towards the oxygen; this will expand the electron thickness on the oxygen molecule and lessen the draw the particle has on the two holding electrons it imparts to the acidic proton.
As an immediate outcome, the hydrogen will be somewhat harder to pull off, since its bond with oxygen is currently somewhat more grounded. Thus, the acidic proton is less "anxious" to bounce off more vulnerable corrosive. Presently for the form bases. The distinction unsteadiness is because of a similar positive inductive impact of the alkyl gathering

Note: The way to showing why alcohols are more vulnerable acids than water is to consider the way that an alkyl bunch is really an EDG - electron-giving gathering (you'll once in a while consider this to be ERG - electron delivering gathering).