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Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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**Question 8.17:** What is the **acid form** of \( \text{NH}_3 \)? **Answer:** \( \text{NH}_4^+ \) **Explanation:** The **acid form** of a conjugate pair contains *one more* \( \text{H}^+ \) than the **base form**. The **acid form** is obtained by **adding** an \( \text{H}^+ \) to the **base form**. - Note that when an \( \text{H}^+ \) is **added** to a species, its charge **increases** by one charge unit. \( \text{NH}_3 \) has a **zero charge**, however when an \( \text{H}^+ \) is added, it is converted to \( \text{NH}_4^+ \); the charge increases by one charge unit.
Transcribed Image Text:**Question 8.17:** What is the **acid form** of \( \text{NH}_3 \)? **Answer:** \( \text{NH}_4^+ \) **Explanation:** The **acid form** of a conjugate pair contains *one more* \( \text{H}^+ \) than the **base form**. The **acid form** is obtained by **adding** an \( \text{H}^+ \) to the **base form**. - Note that when an \( \text{H}^+ \) is **added** to a species, its charge **increases** by one charge unit. \( \text{NH}_3 \) has a **zero charge**, however when an \( \text{H}^+ \) is added, it is converted to \( \text{NH}_4^+ \); the charge increases by one charge unit.
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Step 1

We have to write the acid form of the NH3.

Introduction: We know that an acid is a proton (H+) donor and a base is a proton (H+) acceptor.

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