Solubility of Ce2(SO4)3.
Correct answer: B. Decreases with temperature
- A. Increases with temperature
- B. Decreases with temperature
- C. Shows exceptional behavior
- D. Remains constant
Explanation
The solubility of most salts increases with temperature due to increased kinetic energy and greater interaction between solute and solvent molecules. However, Ce2(SO4)3 is an exception to this rule; its solubility decreases as temperature rises. This is due to complex interactions between the ions and water molecules that dominate at higher temperatures, leading to reduced solubility. Option B is correct because it accurately describes this unique behavior. Option A is incorrect because it follows the general trend, not the exception. Option C is incorrect because although the solubility behavior is exceptional, the option does not specify the temperature dependence. Option D is incorrect because the solubility of Ce2(SO4)3 does not remain constant with temperature changes.
This question appeared on the UHS MDCAT 2010 paper, which you can sit online with every answer explained.
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About Solubility Product
The solubility product constant, Ksp, represents the equilibrium concentrations of ions from a sparingly soluble salt, each raised to its stoichiometric power. Problems involve writing Ksp expressions, calculating molar solubility, applying the common-ion effect and predicting precipitation from the ionic product.
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