Table of contents

1. The Chemical World9m
- The Scientific Method
  9m
2. Measurement and Problem Solving2h 19m
3. Matter and Energy2h 15m
4. Atoms and Elements2h 33m
5. Molecules and Compounds1h 50m
6. Chemical Composition1h 23m
7. Chemical Reactions1h 43m
8. Quantities in Chemical Reactions1h 8m
9. Electrons in Atoms and the Periodic Table2h 32m
10. Chemical Bonding2h 10m
11 Gases2h 7m
12. Liquids, Solids, and Intermolecular Forces1h 11m
13. Solutions3h 1m
14. Acids and Bases2h 14m
15. Chemical Equilibrium1h 27m
16. Oxidation and Reduction1h 33m
17. Radioactivity and Nuclear Chemistry53m

7. Chemical Reactions

Electrolytes (Simplified)

Introduction to Chemistry

7. Chemical Reactions

Electrolytes (Simplified)

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Problem 13

Textbook Question

Classify the solute represented in each of the following equations as a strong, weak, or nonelectrolyte:b. NH₃(g) + H₂O(l) ⇌ NH₄⁺(aq) + OH⁻(aq)

Verified step by step guidance

Identify the solute in the given chemical equation. In this case, the solute is ammonia, NH₃.

Understand the nature of the solute. Ammonia (NH₃) is a molecular compound that can react with water to form ammonium ions (NH₄⁺) and hydroxide ions (OH⁻).

Recognize the type of reaction. The double arrow (⇌) indicates that this is an equilibrium reaction, meaning it does not go to completion and both reactants and products are present in solution.

Determine the classification of the solute. Since NH₃ partially ionizes in water and establishes an equilibrium, it is classified as a weak electrolyte.

Conclude that NH₃ is a weak electrolyte because it only partially dissociates in water, producing a small concentration of ions.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Electrolytes

Electrolytes are substances that dissociate into ions when dissolved in water, allowing the solution to conduct electricity. They are classified into strong electrolytes, which completely dissociate into ions, weak electrolytes, which partially dissociate, and nonelectrolytes, which do not dissociate at all. Understanding the behavior of electrolytes is crucial for analyzing chemical reactions in aqueous solutions.

Strong vs. Weak Electrolytes

Strong electrolytes, such as sodium chloride, fully ionize in solution, resulting in a high concentration of ions. In contrast, weak electrolytes, like ammonia (NH₃), only partially ionize, leading to a mixture of un-ionized molecules and ions in solution. This distinction is important for predicting the conductivity and reactivity of solutions in chemical processes.

Ammonia as a Weak Electrolyte

Ammonia (NH₃) is classified as a weak electrolyte because it does not fully dissociate in water. Instead, it establishes an equilibrium with water, forming ammonium ions (NH₄⁺) and hydroxide ions (OH⁻). This partial ionization is characteristic of weak electrolytes, which influences the pH and conductivity of the solution.