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Chapter 12: Problem 112

How does each of the following affect the solubility of an ionic compound? (a) lattice energy, (b) solvent (polar versus nonpolar), (c) enthalpies of hydration of cation and anion

Short Answer

Expert verified
(a) Higher lattice energy leads to lower solubility, and vice versa. (b) Ionic compounds are more soluble in polar solvents compared to nonpolar solvents. (c) Greater the enthalpies of hydration (more negative), greater the solubility.

Step by step solution

01

Explain the effect of lattice energy

Lattice energy is the energy required to separate one mole of an ionic compound into its ions. If the lattice energy is high, it means more energy is required to separate the ions and so the ionic compound will be less soluble in a given solvent. Conversely, if the lattice energy is low, less energy will be required to separate the ions and so the solubility of the ionic compound could be higher.
02

Elucidate the effect of the nature of the solvent

The polarity of the solvent plays an instrumental role in the solubility of an ionic compound. Polar solvents such as water are effective at dissolving ionic and other polar substances because of their ability to stabilize the ions through the process of hydration. On the other hand, non-polar solvents like oil do not have enough charge separation to stabilize the ions, which makes them poor solvents for ionic compounds.
03

Clarify the effect of enthalpies of hydration of cation and anion

Enthalpies of hydration refer to the energy changes when gaseous ions are completely surrounded by water molecules. It is a exothermic process for ionic compounds. High hydration enthalpies (negative values as it's exothermic) of cation and anion suggest more stabilizing interactions with the solvent and thus greater solubility.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Lattice Energy
Lattice energy is crucial in understanding the solubility of ionic compounds. When a compound breaks apart into ions, energy is required, and this energy is known as lattice energy. Essentially, it's the energy needed to pull apart one mole of an ionic crystal into gaseous ions.

High lattice energy means that the ions are held tightly together in the solid crystal, making it more challenging for the solvent to separate them. This results in lower solubility because more energy is needed to dissolve the compound. Conversely, low lattice energy indicates a weaker hold between the ions, requiring less energy to dissolve them, leading to higher solubility in a solvent.
  • Higher lattice energy = Lower solubility
  • Lower lattice energy = Higher solubility
Polar vs Nonpolar Solvents
The nature of the solvent significantly impacts the solubility of an ionic compound. A solvent's polarity can either facilitate or hinder the dissolving process. Polar solvents, such as water, contain molecules with distinct positive and negative regions. These regions help stabilize and disband the ionic bonds in a compound through hydration.

In contrast, nonpolar solvents, like oils, lack distinct charges and cannot interact effectively with the charged ions in an ionic compound. As a result, they tend to be ineffective at dissolving ionic substances.
  • Polar solvents (e.g., water): Good for dissolving ionic compounds
    - Stabilizes ions through charge interactions
  • Nonpolar solvents (e.g., oil): Poor for dissolving ionic compounds
    - Lacks charge distribution to stabilize ions
Enthalpy of Hydration
The enthalpy of hydration is concerned with the energy change when ions become surrounded by solvent molecules, typically water. This process is always exothermic for ionic compounds, meaning it releases energy.

When ions dissolve in a solvent, they are stabilized by interactions with the molecules of the solvent. High exothermic enthalpies of hydration indicate strong interactions and greater energy release when an ion becomes surrounded by solvent. These energetic interactions promote solubility.
  • Higher (more negative) enthalpy of hydration = Stronger interactions = Greater solubility
  • Energetic interactions help stabilize ions, facilitating dissolving

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