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

18. Aqueous Equilibrium

Solubility Product Constant: Ksp

General Chemistry

18. Aqueous Equilibrium

Solubility Product Constant: Ksp

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Multiple Choice

The Ksp of CuI(s) is 1.1 × 10^-12. Calculate the value of E° for the half-reaction CuI(s) + e^- → Cu(s) + I^-(aq).

0.17 V

0.54 V

0.29 V

0.42 V

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Verified step by step guidance

Understand that the problem involves calculating the standard electrode potential (E°) for the given half-reaction using the solubility product constant (Ksp) of CuI(s).

Recognize that the relationship between the solubility product (Ksp) and the standard electrode potential (E°) can be determined using the Nernst equation and the Gibbs free energy equation. The Nernst equation relates the concentration of ions to the electrode potential.

Use the formula for the Gibbs free energy change: ΔG° = -RT ln(Ksp), where R is the universal gas constant (8.314 J/mol·K), T is the temperature in Kelvin (usually 298 K for standard conditions), and Ksp is the solubility product constant.

Relate the Gibbs free energy change to the standard electrode potential using the equation: ΔG° = -nFE°, where n is the number of moles of electrons transferred in the half-reaction (n = 1 for this reaction), F is Faraday's constant (96485 C/mol), and E° is the standard electrode potential.

Solve for E° using the rearranged equation: E° = (RT ln(Ksp)) / (nF). Substitute the known values (R, T, Ksp, n, and F) into the equation to find the value of E°.