Q. \( \mathrm{NH}_4^+ \) conjugate base.

Q: What is the conjugate base of \mathrm{NH_4^+} ?

The conjugate base is \mathrm{NH_3} (ammonia), formed by removing one \mathrm{H^+} from \mathrm{NH_4^+} .

Q: How do I find the conjugate base of an acid like \mathrm{NH_4^+} ?

Conjugate base comes from the acid losing one proton: \mathrm{NH_4^+} \rightarrow \mathrm{NH_3} . So the conjugate base is always one hydrogen less than the acid.

Q: What reaction corresponds to \mathrm{NH_4^+} and its conjugate base?

In water, \mathrm{NH_4^+} can donate a proton to give \mathrm{NH_3} . The pair is \mathrm{NH_4^+}/\mathrm{NH_3} .

Q: What is the conjugate acid of \mathrm{NH_3} ?

Adding a proton to \mathrm{NH_3} gives \mathrm{NH_4^+} . So \mathrm{NH_4^+} is the conjugate acid of \mathrm{NH_3} .

Q: Are \mathrm{NH_4^+} and \mathrm{NH_3} a conjugate acid-base pair?

Yes. \mathrm{NH_4^+} is the acid and \mathrm{NH_3} is its conjugate base, differing by one \mathrm{H^+} and having charges +1 vs 0 .

Q: What is the general rule for conjugate bases?

The conjugate base is what remains after removing \mathrm{H^+} from the acid. It has one fewer hydrogen and is \mathrm{+1} charge lower for each proton removed (net charge decreases by 1).

Answer

The conjugate base of \( \mathrm{NH_4^+} \) is found by removing one proton \( \mathrm{H^+} \).

\[
\mathrm{NH_4^+ \rightarrow NH_3 + H^+}
\]

Final result: \(\mathrm{NH_3}\)

Detailed Explanation

Goal: Find the conjugate base of the species given by \( \mathrm{NH_4^+} \).

Step 1: Understand what “conjugate base” means.

The conjugate base is what you get after a species loses a proton, \( \mathrm{H^+} \).

Step 2: Identify the proton donor.

\( \mathrm{NH_4^+} \) is an acid, meaning it can donate one \( \mathrm{H^+} \).

Step 3: Remove one proton.

\( \mathrm{NH_4^+} \) has 4 attached hydrogens. Losing one \( \mathrm{H^+} \) leaves 3 hydrogens attached to nitrogen and decreases the charge by 1.

\[
\mathrm{NH_4^+ \rightarrow NH_3 + H^+}
\]

Step 4: State the conjugate base.

The conjugate base is \( \mathrm{NH_3} \) (ammonia).

Final Answer: \( \mathrm{NH_3} \).

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General Chemistry FAQs

What is the conjugate base of \( \mathrm{NH_4^+} \)?

The conjugate base is \( \mathrm{NH_3} \) (ammonia), formed by removing one \( \mathrm{H^+} \) from \( \mathrm{NH_4^+} \).

How do I find the conjugate base of an acid like \( \mathrm{NH_4^+} \)?

Conjugate base comes from the acid losing one proton: \( \mathrm{NH_4^+} \rightarrow \mathrm{NH_3} \). So the conjugate base is always one hydrogen less than the acid.

What reaction corresponds to \( \mathrm{NH_4^+} \) and its conjugate base?

In water, \( \mathrm{NH_4^+} \) can donate a proton to give \( \mathrm{NH_3} \). The pair is \( \mathrm{NH_4^+}/\mathrm{NH_3} \).

What is the conjugate acid of \( \mathrm{NH_3} \)?

Adding a proton to \( \mathrm{NH_3} \) gives \( \mathrm{NH_4^+} \). So \( \mathrm{NH_4^+} \) is the conjugate acid of \( \mathrm{NH_3} \).

Are \( \mathrm{NH_4^+} \) and \( \mathrm{NH_3} \) a conjugate acid-base pair?

Yes. \( \mathrm{NH_4^+} \) is the acid and \( \mathrm{NH_3} \) is its conjugate base, differing by one \( \mathrm{H^+} \) and having charges \( +1 \) vs \( 0 \).

What is the general rule for conjugate bases?

The conjugate base is what remains after removing \( \mathrm{H^+} \) from the acid. It has one fewer hydrogen and is \( \mathrm{+1} \) charge lower for each proton removed (net charge decreases by 1).

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