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

What concentration of the lead ion, Pb2+, must be exceeded to precipitate PbCl2 from a solution that is 1.00×10⁻² M in the chloride ion, Cl⁻? The Ksp for lead(II) chloride is 1.17×10⁻⁵.

1.00×10⁻² M

1.00×10⁻⁴ M

1.17×10⁻³ M

1.17×10⁻⁵ M

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Verified step by step guidance

Understand the concept of solubility product constant (Ksp). The Ksp is the equilibrium constant for the dissolution of a sparingly soluble ionic compound. For PbCl2, the dissolution can be represented as: PbCl2(s) ⇌ Pb²⁺(aq) + 2Cl⁻(aq).

Write the expression for the solubility product constant (Ksp) for PbCl2. The Ksp expression is:

K_{sp} = [Pb²⁺][Cl⁻]²

. Here, [Pb²⁺] is the concentration of lead ions and [Cl⁻] is the concentration of chloride ions.

Substitute the given concentration of chloride ions into the Ksp expression. You are given [Cl⁻] = 1.00×10⁻² M. Substitute this value into the Ksp expression:

K_{sp} = [Pb²⁺](1.00×10⁻²)²

Rearrange the Ksp expression to solve for the concentration of lead ions, [Pb²⁺]. This gives:

[Pb²⁺] = \frac{K_{sp}}{{1.00}^{-2}}

Substitute the value of Ksp (1.17×10⁻⁵) into the rearranged expression to find the concentration of lead ions required to exceed the solubility product and precipitate PbCl2. Calculate: