Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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Parts 4A and 4B please
Transcribed Image Text:**Solubility of Salts at Different Temperatures**
**4. Are the following salts more soluble at high temperatures or low temperatures? Why?**
**a.** \( \text{Ca(OH)}_2(s) \rightleftharpoons \text{Ca}^{2+}(aq) + 2\text{OH}^-(aq) \)
- \( \Delta H^\circ < 0 \)
**Explanation:**
When the enthalpy change (\( \Delta H^\circ \)) is less than zero, the dissolution process is exothermic. Exothermic processes release heat, making the salts more soluble at lower temperatures.
**b.** \( \text{AgCl}(s) \rightleftharpoons \text{Ag}^+(aq) + \text{Cl}^-(aq) \)
- \( \Delta H^\circ > 0 \)
**Explanation:**
When the enthalpy change (\( \Delta H^\circ \)) is greater than zero, the dissolution process is endothermic. Endothermic processes absorb heat, making the salts more soluble at higher temperatures.
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