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

Previous problemNext problem

Struggling with General Chemistry?

Join thousands of students who trust us to help them ace their exams!Watch the first video

Multiple Choice

Which compound will be more soluble in the solvent CH3OCH3 (diethyl ether), and why: HCl(g) or NaCl(s)?

NaCl(s), because it forms hydrogen bonds with diethyl ether.

NaCl(s), because ionic compounds are always more soluble in organic solvents.

HCl(g), because it is a polar molecule and can interact with the polar ether solvent.

Both HCl(g) and NaCl(s) are equally soluble in CH3OCH3.

Previous problemNext problem

Verified step by step guidance

Step 1: Identify the nature of the solvent CH3OCH3 (diethyl ether). Diethyl ether is a polar aprotic solvent, meaning it has a dipole moment but does not have hydrogen atoms bonded to highly electronegative atoms (like O-H or N-H) to form hydrogen bonds as a donor.

Step 2: Analyze the solutes: HCl(g) is a polar covalent molecule with a dipole moment, while NaCl(s) is an ionic compound composed of Na+ and Cl- ions.

Step 3: Consider the solubility principle 'like dissolves like,' which means polar solvents tend to dissolve polar molecules, and ionic compounds generally dissolve better in polar protic solvents (like water) that can stabilize ions through ion-dipole interactions and hydrogen bonding.

Step 4: Evaluate interactions: HCl, being polar, can interact with the dipole of diethyl ether through dipole-dipole interactions, enhancing its solubility. NaCl, being ionic, requires strong ion-dipole interactions and often hydrogen bonding from the solvent to dissolve well, which diethyl ether cannot provide effectively.

Step 5: Conclude that HCl will be more soluble in diethyl ether because it is a polar molecule compatible with the polar solvent, whereas NaCl's ionic nature makes it poorly soluble in diethyl ether due to lack of strong ion-dipole or hydrogen bonding interactions.