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Chapter 12: Problem 8

Suppose we want to dissolve a gaseous solute in water. Would you expect \(\Delta E_{\text {solute separation }}\) to be larger for the gaseous solute or for a solid ionic solute? Explain.

Short Answer

Expert verified
We would expect ΔE (solute separation) to be larger for a solid ionic solute than for a gaseous solute. This is because the particles in a gaseous solute are held together by weak intermolecular forces (van der Waals forces), while solid ionic solutes are held together by strong electrostatic forces (ionic bonds). Dissolving a solid ionic solute requires breaking these strong bonds, leading to a higher energy change compared to the relatively small energy change needed for separating the weakly bound particles in a gaseous solute.

Step by step solution

01

Understand the concept of solute separation

Before moving on to the comparisons, we need to understand solute separation. Solute separation happens when a solute dissolves in a solvent, breaking the intermolecular forces holding its particles together. During this process, energy is either absorbed or released.
02

Gaseous solute

For a gaseous solute, the intermolecular forces between the particles are weak (van der Waals forces or dispersion forces). When a gas dissolves in a solvent like water, it forms weak interactions with the water molecules, which are primarily the London dispersion forces. As a result, the energy change (ΔE) required for solute separation will generally be small for gaseous solutes.
03

Solid ionic solute

In the case of a solid ionic solute, the particles are held together by strong electrostatic forces (ionic bonds). When an ionic solid is dissolved in water, the water molecules will need to break these strong bonds to separate the ions. This process requires a significant amount of energy to be absorbed for solute separation, making the change in energy (ΔE) larger.
04

Comparing the energy change

When comparing the gaseous solute and the solid ionic solute, we must consider the intermolecular forces holding their particles together. As previously mentioned, gaseous solutes have weak intermolecular forces (van der Waals forces), whereas solid ionic solutes have strong electrostatic forces (ionic bonds). In the dissolving process, a gaseous solute will require less energy to separate its particles due to weak forces. On the other hand, a significant amount of energy is needed to break the strong bonds in a solid ionic solute, leading to a higher energy change. Consequently, we would expect ΔE (solute separation) to be larger for a solid ionic solute compared to a gaseous solute.

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