Final answer:
True, the heat of solution of a solid salt is indeed related to its lattice energy (the energy required to break the ionic lattice) and the heat of hydration (the energy released when ions are surrounded by water molecules). This is because dissolving an ionic compound involves breaking its lattice, requiring energy, and then hydrating the ions, releasing energy.
Step-by-step explanation:
The statement that the heat of solution of a solid salt is related to its lattice energy and its heat of hydration is true. When a solid ionic compound dissolves in water, the process can be viewed in two main steps:
- The breakup of the ionic lattice of the solid, which requires an endothermic input of energy, equivalent to the lattice energy.
- The hydration of ions, where water molecules surround and stabilize the ions, releasing energy known as the heat of hydration.
Therefore, the net energy change for the solution process, which is the heat of solution, depends on these two large and opposite energy contributions. A substance with high lattice energy typically requires more energy to break apart the lattice, which could make the compound less soluble unless the heat of hydration is sufficiently exothermic to compensate for it.