Chemical Forums
Specialty Chemistry Forums => Biochemistry and Chemical Biology Forum => Topic started by: Creflo on August 27, 2015, 06:10:38 PM
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I'm assuming the ester is incorrect, but I don't see how it's a carboxyl group as there is no H attached to the O (the Oxygen has an extra lone pair giving it a negative charge right?) I know this is simple, but any help would be appreciated. :P UPDATE: I'm assuming that since COO- is carboxylate that it is indeed a carboxyl group?
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UPDATE: ok so apparently I was right, it is a carboxyl group, I would just delete this post if I could but whatevs. Sorry I'm so dumb!
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A carboxyl group (also known as a carboxylic acid) can exist as in a protonated form R-COOH and a deprotonated form R-COO- depending on the pH of the solution. This is similar to the amino group which also undergoes acid-base chemistry, and a primary amine can either be protonated (R-NH3+) or deprotonated (R-NH2).
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I figured it out. But thank you for the reply Yggdrasil!
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I usually call the conjugate base form a carboxylate group, and the conjugate acid form a carboxylic acid group.