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Both carboxylic acids and alcohols contain an —OH group, one is acidic in water and the other is not because - resonance delocalization of charge stabilizes the conjugate base anion relative to the reactant acid
Explanation of Why —OH group, one is acidic in water and the other is not :
We want the water to serve as a base in this scenario. Therefore, we will consider the acidity qualities to determine which one can establish the most stable base when we want the water to behave as a base. We will therefore act as though there is water everywhere and believe that water is serving as a base if we are in a solution of water. As a result, it will accept those hydrogen atoms if it is acting as a base. Therefore, we want it to be able to release our hydrogen bombs and release them into the sea using our compounds.
Therefore, if substances were to lose hydrogen, they would resemble this and essentially create the conjugate bases of both of our acids. So, if we deep throat nated both of our chemicals, this is what we would get. One of them will create a stable base that will be content in the solution where it contributed its hydrogen to water, and it is content to do so because it creates such a stable base. And that is our carb oxalate ion, which is our carb oxalic acid's conjugate acid. You might therefore assume that we have all of our lone pairs in this resonant configuration.
Those can go ahead and push down well these push up over here and we'll get a similar structure just the opposite way where we have this and we just move our carbon Neil. So that resonant structure is what's going to stabilize that conjugate base and because that conjugate bases so stable, this um carb oxalic acid almost wants to give up its hydrogen to water, even though water is not super, it's not super good at taking that hydrogen.
Those can go ahead and press down, while these can push up over here, and we'll have a similar structure if we just move our carbon Neil in the opposite direction. Because the conjugate base is so stable as a result of the resonance structure, the carbohydrate oxalic acid nearly begs to give up its hydrogen to water even though water is not particularly adept at absorbing that hydrogen. It is not a particularly solid base, nor is it particularly strong. However, because this conjugate base is so persistent, the oxalic acid really wants to give up its hydrogen, making it a very potent acid.
The oxygen must simply maintain its charge on its own because this ion cannot be stabilized in any way. Nothing, not even a resonant structure, can stabilize it. As a result, this is a really robust base even though it isn't particularly stable. However, it will still take a hydrogen quite easily. It will thus be able to take that hydrogen back and reconstruct our alcohol because it can absorb that hydrogen quite simply and water is not really dedicated to being a strong base. And so our alcohol will want to accept this challenge just as much as it will want to reject it.
A super good acid would want to give up this hydrogen and it's not a super strong acid because it doesn't have a stable base to turn into, so it can't give up that hydrogen very readily because it won't form a super stable structure that can hold in our water because our water isn't super committed to being either an acid or a base.
In this situation, a strong acid, such as the silica in our automobile, or a strong base will need to interact with it in order for it to operate as either an acid or a base. However, in this instance, the alcohol is not acidic in the water because our water is a base and only interacts with carboxalic acid as a water.
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