Question:
The conjugate acid of \( \text{NH}_2^- \) is:
The conjugate acid of \( \text{NH}_2^- \) is:
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To easily find the conjugate partner:
- For a conjugate acid: Add one $\text{H}^+$ to the formula.
- For a conjugate base: Remove one $\text{H}^+$ from the formula.
For example, the conjugate acid of $\text{NH}_2^-$ is $\text{NH}_3$, and the conjugate acid of $\text{NH}_3$ is $\text{NH}_4^+$.
- For a conjugate acid: Add one $\text{H}^+$ to the formula.
- For a conjugate base: Remove one $\text{H}^+$ from the formula.
For example, the conjugate acid of $\text{NH}_2^-$ is $\text{NH}_3$, and the conjugate acid of $\text{NH}_3$ is $\text{NH}_4^+$.
Updated On: May 21, 2026
- $\text{NH}_3$
- $\text{NH}_2\text{OH}$
- $\text{NH}_4^+$
- $\text{N}_2\text{H}_4$
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The Correct Option is A
Solution and Explanation
Step 1: Understanding the Question:
The question asks to identify the conjugate acid of the amide ion ($\text{NH}_2^-$) according to the Brønsted-Lowry acid-base concept.
Step 2: Key Formula or Approach:
According to the Brønsted-Lowry theory:
\[ \text{Conjugate Acid} = \text{Base} + \text{H}^+ \] A conjugate acid is formed when a base accepts a proton ($\text{H}^+$).
Step 3: Detailed Explanation:
• The Brønsted-Lowry model defines an acid as any chemical species that can donate a proton ($\text{H}^+$), and a base as any chemical species that can accept a proton.
• When a base accepts a proton, it transforms into its conjugate acid. The conjugate acid has one additional hydrogen atom and a charge that is one unit more positive than the starting base.
• Conversely, when an acid loses a proton, it transitions into its conjugate base, which has one less hydrogen atom and a charge that is one unit more negative.
• Here, we are starting with the amide ion, which is represented by the formula $\text{NH}_2^-$. Since we want to find its conjugate acid, we treat $\text{NH}_2^-$ as a Brønsted-Lowry base.
• To form the conjugate acid of $\text{NH}_2^-$, we add a proton ($\text{H}^+$) to the species:
\[ \text{NH}_2^- + \text{H}^+ \rightleftharpoons \text{NH}_3 \]
• In this protonation process, the chemical composition changes by adding one hydrogen atom (increasing the number of hydrogen atoms from two to three).
• The electrical charge also changes. The initial charge on the amide ion is $-1$, and adding a proton with a $+1$ charge results in a neutral species: $(-1) + (+1) = 0$.
• The resulting neutral molecule is ammonia, $\text{NH}_3$. Therefore, $\text{NH}_3$ is the conjugate acid of the $\text{NH}_2^-$ ion.
Step 4: Final Answer:
The conjugate acid of $\text{NH}_2^-$ is $\text{NH}_3$.
The question asks to identify the conjugate acid of the amide ion ($\text{NH}_2^-$) according to the Brønsted-Lowry acid-base concept.
Step 2: Key Formula or Approach:
According to the Brønsted-Lowry theory:
\[ \text{Conjugate Acid} = \text{Base} + \text{H}^+ \] A conjugate acid is formed when a base accepts a proton ($\text{H}^+$).
Step 3: Detailed Explanation:
• The Brønsted-Lowry model defines an acid as any chemical species that can donate a proton ($\text{H}^+$), and a base as any chemical species that can accept a proton.
• When a base accepts a proton, it transforms into its conjugate acid. The conjugate acid has one additional hydrogen atom and a charge that is one unit more positive than the starting base.
• Conversely, when an acid loses a proton, it transitions into its conjugate base, which has one less hydrogen atom and a charge that is one unit more negative.
• Here, we are starting with the amide ion, which is represented by the formula $\text{NH}_2^-$. Since we want to find its conjugate acid, we treat $\text{NH}_2^-$ as a Brønsted-Lowry base.
• To form the conjugate acid of $\text{NH}_2^-$, we add a proton ($\text{H}^+$) to the species:
\[ \text{NH}_2^- + \text{H}^+ \rightleftharpoons \text{NH}_3 \]
• In this protonation process, the chemical composition changes by adding one hydrogen atom (increasing the number of hydrogen atoms from two to three).
• The electrical charge also changes. The initial charge on the amide ion is $-1$, and adding a proton with a $+1$ charge results in a neutral species: $(-1) + (+1) = 0$.
• The resulting neutral molecule is ammonia, $\text{NH}_3$. Therefore, $\text{NH}_3$ is the conjugate acid of the $\text{NH}_2^-$ ion.
Step 4: Final Answer:
The conjugate acid of $\text{NH}_2^-$ is $\text{NH}_3$.
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