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(A) The isoelectric point $(pI)$ is the $pH$ at which the amino acid exists as a zwitterion,i.e.,$H_3N^{+}-CH(R)-COO^{-}$.At $pH$ values lower than th

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$H_3N^{+}-CH(R)-COOH$

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(A) The isoelectric point $(pI)$ is the $pH$ at which the amino acid exists as a zwitterion,i.e.,$H_3N^{+}-CH(R)-COO^{-}$.At $pH$ values lower than the $pI$,the concentration of $H^{+}$ ions is high.This leads to the protonation of the carboxylate group $(COO^{-})$,converting it into a carboxylic acid group $(COOH)$.Since the given $pH$ $(1.0)$ is significantly lower than the $pI$ $(6.0)$,the amino acid will exist predominantly in its cationic form,$H_3N^{+}-CH(R)-COOH$.

Assume that a particular amino acid has an isoelectric point of $6.0$. In a solution of $pH$ $1.0$,which of the following species will predominate?

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