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.


Hsolution=bond breaking-bond forming


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

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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?

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What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Lattice Energy Application concept. You can view video lessons to learn Lattice Energy Application. Or if you need more Lattice Energy Application practice, you can also practice Lattice Energy Application practice problems.

What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Snow's class at SHU.