Solubility and Complex Ion Equilibria
General Chemistry • 9 topics in this chapter.
This Solubility and Complex Ion Equilibria chapter in General Chemistry focuses on how sparingly soluble salts dissolve and how ions interact in solution, with interactive calculators and explanations for Ksp (solubility product), molar solubility, and predicting precipitation. It also introduces complex ion formation (Kf) and how ligands like NH3, CN−, or OH− can increase solubility by shifting equilibrium, connecting directly to qualitative analysis and real lab chemistry.
On this page you can calculate molar solubility from Ksp (and Ksp from solubility), evaluate the ion product Q vs Ksp to decide whether a precipitate forms, and solve common-ion effect problems that reduce solubility. Tools can also help you work multi-step equilibria where complex formation competes with precipitation, guiding you through equilibrium expressions, ICE-table setups, and unit consistency step by step.
The difficulty level ranges from beginner-friendly Ksp solubility practice to advanced precipitation and complex-ion equilibrium problems, making it ideal for AP/IB Chemistry and introductory university chemistry while still accessible to strong high school students. Teachers can use it to demonstrate solubility logic clearly, self-learners can build confidence with structured practice, and advanced users can quickly verify Q vs K decisions, selective precipitation setups, and complex-ion calculations for labs and exam preparation.
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1. Solubility Product Constant Ksp
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2. Relationship Between Solubility and Ksp
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3. Common Ion Effect in Solubility Equilibra
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4. Criteria for Precipitation and Its Completeness
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5. Fractional Precipitation
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6. Solubility and pH
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7. Equilibria Involving Complex Ions
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8. Solubility of Solute When Complex Ions Form
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9. Equilibria Involving Hydrogen Sulfide
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