Question:
The conjugate acid of $NH_2^-$ is:
The conjugate acid of $NH_2^-$ is:
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To remember the difference:
• Conjugate Acid: Base + $H^+$ (Add an H, increase charge by 1).
• Conjugate Base: Acid - $H^+$ (Remove an H, decrease charge by 1).
• Conjugate Acid: Base + $H^+$ (Add an H, increase charge by 1).
• Conjugate Base: Acid - $H^+$ (Remove an H, decrease charge by 1).
Updated On: May 20, 2026
- $NH_3$
- $NH_2OH$
- $NH_4^+$
- $N_2H_4$
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The Correct Option is A
Solution and Explanation
Concept:
According to the Brønsted-Lowry theory, an acid is a proton ($H^+$) donor and a base is a proton acceptor. A conjugate acid is formed when a base accepts a proton.
Step 1: Understand the relationship.
To find the conjugate acid of a given species, you must add one proton ($H^+$) to it. The formula relationship is: \[ \text{Base} + H^+ \rightarrow \text{Conjugate Acid} \]
Step 2: Apply the rule to $NH_2^-$.
Starting with the amide ion ($NH_2^-$):
• Add one Hydrogen atom ($H$).
• Increase the net charge by $+1$ (from $-1$ to $0$). \[ NH_2^- + H^+ \rightarrow NH_3 \]
Step 3: Conclusion.
Ammonia ($NH_3$) is the conjugate acid of the amide ion ($NH_2^-$).
Step 1: Understand the relationship.
To find the conjugate acid of a given species, you must add one proton ($H^+$) to it. The formula relationship is: \[ \text{Base} + H^+ \rightarrow \text{Conjugate Acid} \]
Step 2: Apply the rule to $NH_2^-$.
Starting with the amide ion ($NH_2^-$):
• Add one Hydrogen atom ($H$).
• Increase the net charge by $+1$ (from $-1$ to $0$). \[ NH_2^- + H^+ \rightarrow NH_3 \]
Step 3: Conclusion.
Ammonia ($NH_3$) is the conjugate acid of the amide ion ($NH_2^-$).
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