A: Amino acids are amphoteric in nature.R: Am | vedclass

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(A) Amino acids contain both an acidic carboxyl group $(-COOH)$ and a basic amino group $(-NH_2)$ in the same molecule.Due to the presence of both aci

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$A$ and $R$ are true and $R$ is the correct explanation of $A$.

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(A) Amino acids contain both an acidic carboxyl group $(-COOH)$ and a basic amino group $(-NH_2)$ in the same molecule.Due to the presence of both acidic and basic groups,they can react with both acids and bases,making them amphoteric.In an aqueous solution,the carboxyl group can lose a proton to form a carboxylate ion $(-COO^-)$ and the amino group can accept a proton to form an ammonium ion $(-NH_3^+)$,resulting in a zwitterion.Because they exist as charged ions (zwitterions) in solution,they behave as electrolytes and can migrate in an electric field.Therefore,both statements are true,and the fact that they act as electrolytes is a direct consequence of their amphoteric nature (zwitterion formation).

Column-$I$ (Type of Amino Acid)	Column-$II$ (Example)
$(A)$ Polar and uncharged $R$ group	$(i)$ Methionine
$(B)$ Non-polar $R$ group	$(ii)$ Glutamic acid
$(C)$ Polar and negatively charged $R$ group	$(iii)$ Lysine
$(D)$ Polar and positively charged $R$ group	$(iv)$ Cysteine

$A$: Amino acids are amphoteric in nature.
$R$: Amino acids act as electrolytes in solution.

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$A$: Amino acids are amphoteric in nature.$R$: Amino acids act as electrolytes in solution.