Open Question
Which molecule would you expect to be more soluble in water: CCl4 or CH2Cl2?
Ch.13 - Solutions
Chapter 13, Problem 35
When ammonium chloride (NH4Cl) is dissolved in water, the solution becomes colder: a. Is the dissolution of ammonium chloride endothermic or exothermic? b. What can you conclude about the relative magnitudes of the lattice energy of ammonium chloride and its heat of hydration? c. Sketch a qualitative energy diagram similar to Figure 13.7 for the dissolution of NH4Cl. d. Why does the solution form? What drives the process?
Verified step by step guidance1
Identify the type of reaction: Since the solution becomes colder, the dissolution process absorbs heat from the surroundings, indicating that it is endothermic.
Compare lattice energy and heat of hydration: In an endothermic dissolution, the lattice energy (energy required to break the ionic bonds in the solid) is greater than the heat of hydration (energy released when ions interact with water).
Sketch an energy diagram: Draw an energy diagram with the initial energy of solid NH4Cl higher than the final energy of the dissolved ions, showing an upward arrow to represent the absorption of energy.
Explain solution formation: The solution forms because the increase in entropy (disorder) from dissolving the solid compensates for the energy absorbed, making the process favorable.
Identify the driving force: The process is driven by the increase in entropy, which is a key factor in the spontaneity of the dissolution despite being endothermic.
Related Practice
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For each compound, would you expect greater solubility in water or in hexane? Indicate the kinds of intermolecular forces that occur between the solute and the solvent in which the molecule is most soluble. a. glucose
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Textbook Question
For each compound, would you expect greater solubility in water or in hexane? Indicate the kinds of intermolecular forces that would occur between the solute and the solvent in which the molecule is most soluble. d. ethylene glycol
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Textbook Question
When lithium iodide (LiI) is dissolved in water, the solution becomes hotter. a. Is the dissolution of lithium iodide endothermic or exothermic?
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Textbook Question
When lithium iodide (LiI) is dissolved in water, the solution becomes hotter. b. What can you conclude about the relative magnitudes of the lattice energy of lithium iodide and its heat of hydration?
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Textbook Question
When lithium iodide (LiI) is dissolved in water, the solution becomes hotter. c. Sketch a qualitative energy diagram similar to Figure 13.7 for the dissolution of LiI.
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