# Problem: The enthalpy of solution for NaOH is -44.46 kJ/mol. What can you conclude about the relative magnitudes of the absolute values of ΔHsolute and ΔHhydration, where ΔHsolute is the heat associated with separating the solute particles and ΔHhydration is the heat associated with dissolving the solute particles in water?

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###### FREE Expert Solution

Lattice energy represents the energy released when 1 mole of an ionic crystal is formed from its gaseous ions. Can be associated with the energy required to separate the ions:

The heat of hydration of an ion is the amount of heat released when one mole of that ion dissolves in water.

The heat of solution, enthalpy change related to the dissolution of a substance in a solvent. It will be composed of the process - bonds being broken and bonds being formed.

The equation below relates the lattice energy, heat of solution, and heat of hydration: ###### Problem Details

The enthalpy of solution for NaOH is -44.46 kJ/mol. What can you conclude about the relative magnitudes of the absolute values of ΔHsolute and ΔHhydration, where ΔHsolute is the heat associated with separating the solute particles and ΔHhydration is the heat associated with dissolving the solute particles in water?