Table of contents

1. Matter and Measurements4h 31m
2. Atoms and the Periodic Table5h 23m
3. Ionic Compounds2h 18m
4. Molecular Compounds2h 18m
5. Classification & Balancing of Chemical Reactions3h 17m
6. Chemical Reactions & Quantities2h 27m
7. Energy, Rate and Equilibrium3h 46m
8. Gases, Liquids and Solids3h 25m
9. Solutions4h 10m
10. Acids and Bases3h 29m
11. Nuclear Chemistry56m
BONUS: Lab Techniques and Procedures1h 38m
BONUS: Mathematical Operations and Functions47m
12. Introduction to Organic Chemistry1h 34m
13. Alkenes, Alkynes, and Aromatic Compounds2h 12m
14. Compounds with Oxygen or Sulfur1h 6m
15. Aldehydes and Ketones1h 1m
16. Carboxylic Acids and Their Derivatives1h 11m
17. Amines39m
18. Amino Acids and Proteins1h 51m
19. Enzymes1h 37m
20. Carbohydrates1h 41m
21. The Generation of Biochemical Energy2h 8m
22. Carbohydrate Metabolism2h 22m
23. Lipids2h 26m
24. Lipid Metabolism1h 45m
25. Protein and Amino Acid Metabolism1h 37m
26. Nucleic Acids and Protein Synthesis2h 54m

9. Solutions

Electrolytes (Simplified)

GOB Chemistry

9. Solutions

Electrolytes (Simplified)

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2:29 minutes

Problem 13b

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 equation. In this case, the solute is NH₃ (ammonia).

Examine the reaction provided: NH₃(g) + H₂O(l) ⇌ NH₄⁺(aq) + OH⁻(aq). Notice the double arrow (⇌), which indicates that the reaction is reversible and does not go to completion.

Understand the behavior of NH₃ in water. Ammonia reacts with water to form NH₄⁺ (ammonium ion) and OH⁻ (hydroxide ion), but only a small fraction of NH₃ molecules ionize. This partial ionization is characteristic of a weak electrolyte.

Recall the definition of a weak electrolyte: A weak electrolyte partially ionizes in solution, producing a small number of ions while most of the solute remains in its molecular form.

Classify NH₃ as a weak electrolyte based on its partial ionization in water and the reversible nature of the reaction.

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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 this classification 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 lower concentration of ions. This distinction affects the conductivity of the solution and is essential for classifying solutes in chemical equations.

Ammonia in Water

When ammonia (NH₃) is dissolved in water, it acts as a weak base, partially reacting with water to form ammonium ions (NH₄⁺) and hydroxide ions (OH⁻). This equilibrium reaction indicates that ammonia is a weak electrolyte, as it does not fully dissociate into ions. Recognizing this behavior is key to classifying ammonia in the context of electrolyte strength.

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Classify the solute represented in each of the following equations as a strong, weak, or nonelectrolyte:

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