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JFraserBest ResponseYou've already chosen the best response.1
start by drawing some lewis structures
 7 months ago

abb0tBest ResponseYou've already chosen the best response.5
Yes! A good way to explain this would be to draw resonance structures for both! The delocalization of the negative across a structures means more stability. The greater area over which the delocalization is possible, the greater the stabilization. Thus, this is what makes it a stronger acid.
 7 months ago

goformit100Best ResponseYou've already chosen the best response.0
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 7 months ago

VincentLyon.FrBest ResponseYou've already chosen the best response.2
When you want to compare the strengths of acids, study the relative stability of their conjugate bases.
 7 months ago

Vikas_gargBest ResponseYou've already chosen the best response.0
Firstly to check the acidic strenght of any acid or to compare any acid draw its structure and conjugate base in the above question when you draw the conjugate base of carboxylic acid it is stabilise by 2 resonating structures where as in conjugate base of phenol i.e phenoxide ion has 5 or 6 resonating structures but in carboxylic acid the resonating structure has 2 equilating resonance structures ( i.e dispersal of charge on same atom in resonating structure ) this type of resonance is more stable than normal resonance so i.e why carboxylic acid is more acidic than phenol
 7 months ago
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