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

Determine the molar solubility of Ag2CrO4 in a solution containing 0.153 M AgNO3. The Ksp for Ag2CrO4 is 2.0 × 10^-12.

7.5 × 10^-6 M

2.0 × 10^-12 M

3.9 × 10^-8 M

1.3 × 10^-10 M

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Verified step by step guidance

Start by writing the balanced dissolution equation for Ag2CrO4:

{Ag 2}_{CrO 4} (s) \to 2 Ag (aq) + CrO 4 (aq)^- 2

Express the solubility product constant (Ksp) for Ag2CrO4 in terms of the concentrations of the ions:

K_{sp} = (2 s + 0.153)^2 \cdot s

, where s is the molar solubility of Ag2CrO4.

Since the solution already contains 0.153 M AgNO3, the concentration of Ag⁺ ions from AgNO3 is 0.153 M. Therefore, the total concentration of Ag⁺ ions is

2 s + 0.153

Substitute the known Ksp value into the expression:

2.0 \times 10^{- 12} = (2 s + 0.153)^2 \cdot s

Solve the equation for s, which represents the molar solubility of Ag2CrO4 in the solution containing 0.153 M AgNO3. This involves algebraic manipulation and potentially using the quadratic formula if necessary.