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

Which of the following compounds would you expect to have poor solubility in water?

AgCl

NaNO3

NH4Br

K2SO4

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Verified step by step guidance

Step 1: Understand the concept of solubility in water, which is largely influenced by the ionic nature of the compound and the strength of the ionic bonds. Water is a polar solvent, so ionic compounds that dissociate easily into ions tend to be soluble.

Step 2: Recall the solubility rules for common ionic compounds in water. For example, most nitrates (NO\_3\^-), ammonium (NH\_4\^+), and alkali metal salts (like K\^+) are generally soluble in water.

Step 3: Analyze each compound based on these rules: NaNO\_3 contains the nitrate ion, which is highly soluble; NH\_4Br contains ammonium and bromide ions, both of which form soluble salts; K\_2SO\_4 contains potassium and sulfate ions, and potassium salts are usually soluble.

Step 4: Consider AgCl, which contains silver (Ag\^+) and chloride (Cl\^-). According to solubility rules, most silver salts are poorly soluble in water, especially silver chloride, which is known to be sparingly soluble.

Step 5: Conclude that AgCl is expected to have poor solubility in water compared to the other compounds listed, based on the solubility rules and the nature of the ions involved.