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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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Most popular questions from this chapter

A nonvolatile organic compound \(Z\) was used to make up two solutions. Solution A contains \(5.00 \mathrm{~g}\) of \(Z\) dissolved in \(100 \mathrm{~g}\) of water, and solution \(\mathrm{B}\) contains \(2.31 \mathrm{~g}\) of \(\mathrm{Z}\) dissolved in \(100 \mathrm{~g}\) of benzene. Solution A has a vapor pressure of \(754.5 \mathrm{mmHg}\) at the normal boiling point of water, and solution \(\mathrm{B}\) has the same vapor pressure at the normal boiling point of benzene. Calculate the molar mass of \(Z\) in solutions \(\mathrm{A}\) and \(\mathrm{B}\) and account for the difference.

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