Arrange the following in the increasing order of acidity and justify the same.
$(C H_{3})_{3} C O H$ , $C H_{3} O H$ , $(C H_{3})_{2} C H O H$

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Solution

The correct increasing order of acidity is:
$(C H_{3})_{3} C - O H < (C H_{3})_{2} C H - O H < C H_{3} - O H$
For an acid to be strong its conjugate base anion has to be very stable. Only then acid will disassociate faster to give hydronium ion.
As we can see in the figure, conjugate base $(I)$ has a negatively charged $O$ atom and 3 $+ I$ groups attached to it. So, it is least stable. Again, $(I I I)$ has no $+ I$ groups, so it is most stable, and hence the most acidic.

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