\(Conjugate\ acid \ of\ NH_2^–:\)
\(Conjugate\ acid \ of\ NH_2^–:\)
\(NH_4OH\)
\(NH4^+\)
\(NH^{2-}\)
\(NH_3\)
The Correct Option is D
Solution and Explanation
To determine the conjugate acid of a given base, we need to understand the concept of conjugate acid-base pairs. A conjugate acid is formed when a base gains a proton (H+).
In this question, we need to find the conjugate acid of \(NH_2^-\), which is the amide ion. The amide ion, \(NH_2^-\), will gain a proton to form its conjugate acid.
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The amide ion (\(NH_2^-\)) is a base. According to the Bronsted-Lowry theory, a base can accept a proton.
Reaction: NH_2^- + H^+ \rightarrow NH_3
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When the amide ion (\(NH_2^-\)) gains a proton (\(H^+\)), it becomes ammonia (\(NH_3\)).
Thus, the conjugate acid of \(NH_2^-\) is \(NH_3\).
Now let's justify why the other options are incorrect:
- NH_4OH: This is ammonium hydroxide, not relevant in the context of conjugate acid for \(NH_2^-\).
- NH_4^+: This is the conjugate acid of \(NH_3\), not \(NH_2^-\).
- NH^{2-}: This is not relevant here as it is not a common species involved in such proton transfer events.
Therefore, the correct answer is NH_3.
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