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Glycine exists as the zwitter ion, N^(+)...

Glycine exists as the zwitter ion, `N^(+)H_(3), CH_(2),COO^(-)`. Its conjugate base is

A

`NH_(2),CH_(2) COOH `

B

`NH_(2),CH_(2) COO^(-)`

C

`NH_(3)CH_(2)COOH`

D

`NH_(3)CH_(2)COOH`

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To determine the conjugate base of the zwitter ion form of glycine, we can follow these steps: ### Step 1: Understand the Structure of Glycine Glycine is the simplest amino acid with the formula NH2CH2COOH. In its zwitter ion form, it has both a positive and a negative charge, represented as \( \text{NH}_3^+ \text{CH}_2 \text{COO}^- \). ### Step 2: Identify the Zwitter Ion The zwitter ion of glycine is formed when the carboxylic acid group (\(-COOH\)) donates a proton (\(H^+\)) to the amino group (\(-NH_2\)), resulting in the structure: \[ \text{NH}_3^+ \text{CH}_2 \text{COO}^- \] ### Step 3: Define the Conjugate Base The conjugate base of an acid is formed when the acid loses a proton (\(H^+\)). In this case, the zwitter ion acts as an acid when it donates a proton from the ammonium group. ### Step 4: Remove the Proton from the Zwitter Ion When the zwitter ion loses a proton from the ammonium group (\(NH_3^+\)), it transforms into: \[ \text{NH}_2 \text{CH}_2 \text{COO}^- \] ### Step 5: Write the Conjugate Base The conjugate base of the zwitter ion is: \[ \text{NH}_2 \text{CH}_2 \text{COO}^- \] ### Conclusion Thus, the conjugate base of the zwitter ion form of glycine is \( \text{NH}_2 \text{CH}_2 \text{COO}^- \).
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