Table of contents

1. Intro to General Chemistry3h 48m
2. Atoms & Elements4h 16m
3. Chemical Reactions4h 10m
4. BONUS: Lab Techniques and Procedures1h 38m
5. BONUS: Mathematical Operations and Functions48m
6. Chemical Quantities & Aqueous Reactions3h 53m
7. Gases3h 49m
8. Thermochemistry2h 37m
9. Quantum Mechanics2h 58m
10. Periodic Properties of the Elements3h 9m
11. Bonding & Molecular Structure3h 29m
12. Molecular Shapes & Valence Bond Theory1h 57m
13. Liquids, Solids & Intermolecular Forces2h 23m
14. Solutions3h 1m
15. Chemical Kinetics2h 53m
16. Chemical Equilibrium2h 29m
17. Acid and Base Equilibrium5h 1m
18. Aqueous Equilibrium4h 47m
19. Chemical Thermodynamics1h 50m
20. Electrochemistry2h 42m
21. Nuclear Chemistry2h 36m
22. Organic Chemistry5h 7m
23. Chemistry of the Nonmetals2h 39m
24. Transition Metals and Coordination Compounds3h 16m

6. Chemical Quantities & Aqueous Reactions

Solubility Rules

General Chemistry

6. Chemical Quantities & Aqueous Reactions

Solubility Rules

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Multiple Choice

A compound has a melting point of 545 degrees Celsius and dissolves well in water. Which of the following best explains why it is soluble in water?

It is a nonpolar compound, and water dissolves nonpolar substances easily.

Its high melting point means it is a covalent compound that forms hydrogen bonds with water.

It contains ions that interact favorably with water molecules, making it an ionic compound that follows solubility rules.

Its large molecular size allows it to be more soluble in water.

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Verified step by step guidance

Step 1: Understand the nature of water as a solvent. Water is a polar molecule and tends to dissolve substances that are either ionic or polar due to the principle 'like dissolves like.'

Step 2: Analyze the melting point information. A high melting point (such as 545°C) often indicates strong forces holding the compound together, which is characteristic of ionic compounds rather than covalent molecular compounds.

Step 3: Consider the solubility behavior. Since the compound dissolves well in water, it suggests that the compound interacts favorably with water molecules, which is typical for ionic compounds where ions are stabilized by hydration.

Step 4: Evaluate the options given. Nonpolar compounds generally do not dissolve well in water, and large molecular size does not necessarily increase solubility in water. Covalent compounds with hydrogen bonding can be soluble but usually have lower melting points.

Step 5: Conclude that the best explanation is that the compound contains ions that interact favorably with water molecules, making it an ionic compound that follows solubility rules.