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Chapter 13: Problem 3

Consider two ionic solids, both composed of singly charged ions, that have different lattice energies. (a) Will the solids have the same solubility in water? (b) If not, which solid will be more soluble in water, the one with the larger lattice energy or the one with the smaller lattice energy? Assume that solute-solvent interactions are the same for both solids. [Section 13.1]

Short Answer

Expert verified
In conclusion, (a) two ionic solids with different lattice energies will not have the same solubility in water. (b) The solid with a smaller lattice energy, indicating weaker ionic bonding, will be more soluble in water than the one with a larger lattice energy, assuming equal solute-solvent interactions.

Step by step solution

01

Recap the concepts of lattice energy and solvation

Lattice energy refers to the energy required to break one mole of a solid ionic compound into its separate ions in the gaseous state. It's a measure of the strength of ionic bonds in the solid structure. Solvation is the process of surrounding solvent molecules with solute ions or molecules.
02

Understand the relationship between lattice energy and solubility

When an ionic solid dissolves in water, its ionic bonds need to be broken, which requires a certain amount of energy. The lattice energy plays a role in this process: the stronger the lattice energy (the higher the energy required to break the ionic bonds), the less likely the solid is to dissolve in water. On the other hand, if the lattice energy is low (less energy required to break the ionic bonds), the solid may be more soluble in water because less energy is needed for the dissolution process.
03

Address question (a) - Will the solids have the same solubility in water?

Since the two ionic solids have different lattice energies, this means their ionic bonds require different amounts of energy to break. Because the energy required to dissolve each solid is impacted by its lattice energy, their relative solubilities in water would not be the same.
04

Address question (b) - Determine which solid is more soluble in water

The question asks which solid will be more soluble in water, the one with the larger lattice energy or the one with the smaller lattice energy. As mentioned in Step 2, a higher lattice energy means a stronger ionic bond, making it more difficult to dissolve the solid in water. So, the solid with a smaller lattice energy, indicating weaker ionic bonding, will be more soluble in water than the one with a larger lattice energy, given the same solute-solvent interactions. In conclusion, the solid with a smaller lattice energy will be more soluble in water than the one with larger lattice energy, assuming equal solute-solvent interactions.

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Most popular questions from this chapter

(a) What is the mass percentage of iodine in a solution containing $0.035 \mathrm{~mol} \mathrm{I}_{2}\( in \)125 \mathrm{~g}\( of \)\mathrm{CCl}_{4} ?$ (b) Seawater contains \(0.0079 \mathrm{~g}\) of \(\mathrm{Sr}^{2+}\) per kilogram of water. What is the concentration of \(\mathrm{Sr}^{2+}\) in ppm?

Commercial aqueous nitric acid has a density of $1.12 \mathrm{~g} / \mathrm{mL}\( and is 3.7 M. Calculate the percent \)\mathrm{HNO}_{3}$ by mass in the solution.

Suppose you had a balloon made of some highly flexible semipermeable membrane. The balloon is filled completely with a \(0.2 \mathrm{M}\) solution of some solute and is submerged in a 0.1 \(M\) solution of the same solute: Initially, the volume of solution in the balloon is \(0.25 \mathrm{~L}\). Assuming the volume outside the semipermeable membrane is large, as the illustration shows, what would you expect for the solution volume inside the balloon once the system has come to equilibrium through osmosis? [Section 13.5]

Which of the following in each pair is likely to be more soluble in water: (a) cyclohexane \(\left(\mathrm{C}_{6} \mathrm{H}_{12}\right)\) or glucose \(\left(\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}\right)\), (b) propionic acid \(\left(\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{COOH}\right)\) or sodium propionate $\left(\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{COONa}\right),(\mathbf{c}) \mathrm{HCl}$ or ethyl chloride \(\left(\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{Cl}\right) ?\) Explain in each case.

The normal boiling point of ethanol, $\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{OH},\( is \)78.4^{\circ} \mathrm{C}\(. When \)3.26 \mathrm{~g}$ of a soluble nonelectrolyte is dissolved in \(100.0 \mathrm{~g}\) of ethanol at that temperature, the vapor pressure of the solution is \(100 \mathrm{kPa}\). What is the molar mass of the solute?
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