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Chapter 12: Problem 61

Consider an ionic solid dissolving in a liquid. Suppose the energy released as solute-solvent interactions take place is substantially less than the energy required to break up the lattice and to make room in the solvent. Would the solid be very soluble in this liquid? Explain your answer fully.

Short Answer

Expert verified
In conclusion, the ionic solid would not be very soluble in the given liquid due to a positive enthalpy of solution (∆H_sol) arising from the substantially lower solvation energy (∆H_solvation) compared to the lattice energy (∆H_lattice). This indicates an endothermic and energetically unfavourable dissolution process.

Step by step solution

01

Understand the energy changes during dissolution of ionic solids

Ionic solids dissolve in a liquid through the breaking of ionic lattice to form separated ions, which then form a solution through solute-solvent interactions. Energy changes in two main ways during this process: 1. Lattice energy is required to break the ionic lattice into separated ions. 2. Solvation energy is the energy released as a result of solute-solvent interactions.
02

Define the relationship between solvation energy, lattice energy, and the enthalpy of solution

The enthalpy of solution (∆H_sol) represents the overall energy change during the dissolution process. It's the sum of the lattice energy (∆H_lattice) and the solvation energy (∆H_solvation): ∆H_sol = ∆H_lattice + ∆H_solvation If ∆H_sol is negative (exothermic), it implies that the dissolution process is energetically favourable, leading to a more soluble ionic solid. If ∆H_sol is positive (endothermic), it implies that the dissolution process is energetically unfavourable, leading to a less soluble ionic solid.
03

Analyze the given information about energy changes

The information provided states that the solvation energy (∆H_solvation) is substantially less than the lattice energy (∆H_lattice). In other words: ∆H_solvation << ∆H_lattice This implies that the energy released by solute-solvent interactions is not sufficient to overcome the energy required to break the ionic lattice.
04

Determine the solubility of the ionic solid

Recall the relationship between the enthalpy of solution, lattice energy, and solvation energy: ∆H_sol = ∆H_lattice + ∆H_solvation Given that ∆H_solvation is substantially less than ∆H_lattice, it follows that the enthalpy of solution (∆H_sol) will be positive, indicating an endothermic process. Since the dissolution process is energetically unfavourable, the ionic solid will not be very soluble in the given liquid.
05

Conclude the explanation

In conclusion, an ionic solid with a substantially lower solvation energy compared to its lattice energy would have a positive enthalpy of solution (∆H_sol), making the dissolution process endothermic and energetically unfavourable. Therefore, the solid would not be very soluble in the given liquid.

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