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 is expected to be the least soluble in H2O?

NaNO3

AgCl

K2SO4

NH4Br

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Verified step by step guidance

Step 1: Understand that solubility in water depends on the compound's ability to dissociate into ions and the strength of the ionic bonds in the solid. Generally, most alkali metal salts (like NaNO3 and K2SO4) and ammonium salts (like NH4Br) are highly soluble in water.

Step 2: Recall the solubility rules for ionic compounds in water. For example, nitrates (NO3-) and alkali metal salts (Na+, K+) are usually soluble, as are most ammonium (NH4+) salts.

Step 3: Identify that silver chloride (AgCl) is a well-known example of a sparingly soluble salt due to the strong ionic lattice and low tendency to dissociate in water.

Step 4: Compare the compounds given: NaNO3, K2SO4, and NH4Br are all generally soluble, while AgCl is known to have low solubility in water.

Step 5: Conclude that AgCl is expected to be the least soluble compound in water among the options provided.