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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

18. Aqueous Equilibrium

Solubility Product Constant: Ksp

General Chemistry

18. Aqueous Equilibrium

Solubility Product Constant: Ksp

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Multiple Choice

Ksp = 2 × 10^(-19) for LaF3. Calculate the solubility of LaF3 in grams per liter in a solution that is 0.013 M in KF.

3.4 × 10^(-5) g/L

7.8 × 10^(-2) g/L

1.2 × 10^(-7) g/L

5.6 × 10^(-3) g/L

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Verified step by step guidance

Identify the dissolution reaction for LaF3: LaF3(s) ⇌ La³⁺(aq) + 3F⁻(aq).

Write the expression for the solubility product constant (Ksp): Ksp = [La³⁺][F⁻]³.

Since the solution is 0.013 M in KF, assume that the concentration of F⁻ from KF is 0.013 M. Let the solubility of LaF3 be 's' mol/L, then [La³⁺] = s and [F⁻] = 0.013 + 3s.

Substitute the concentrations into the Ksp expression: 2 × 10^(-19) = s(0.013 + 3s)³.

Assume 3s is negligible compared to 0.013, simplify the expression to: 2 × 10^(-19) ≈ s(0.013)³, and solve for 's'. Convert the solubility from mol/L to g/L using the molar mass of LaF3.