Silver nitrate has a lattice energy of -820 kJ/mol and a heat of solution of 22.6 kJ/mol. Calculate the heat of hydration for silver nitrate.

Verified step by step guidance

1. Identify the given values: Lattice energy (U) = -820 kJ/mol and Heat of solution (\( \Delta H_{sol} \)) = 22.6 kJ/mol.
2. Recall the relationship between lattice energy, heat of solution, and heat of hydration: \( \Delta H_{sol} = \Delta H_{hydration} - U \).
3. Rearrange the equation to solve for the heat of hydration (\( \Delta H_{hydration} \)): \( \Delta H_{hydration} = \Delta H_{sol} + U \).
4. Substitute the given values into the equation: \( \Delta H_{hydration} = 22.6 \text{ kJ/mol} + (-820 \text{ kJ/mol}) \).
5. Perform the arithmetic operation to find the heat of hydration.

Key Concepts

Lattice Energy

Lattice energy is the amount of energy released when gaseous ions combine to form an ionic solid. It is a measure of the strength of the forces between the ions in an ionic compound. A more negative lattice energy indicates a more stable ionic compound, as it reflects stronger ionic bonds.

Heat of Solution

The heat of solution is the amount of energy absorbed or released when a solute dissolves in a solvent. In the case of silver nitrate, a positive heat of solution indicates that energy is absorbed when it dissolves, which can affect the overall energy balance during the dissolution process.

Heat of Hydration

The heat of hydration is the energy change that occurs when ions are surrounded by water molecules during the dissolution process. It is typically exothermic, meaning it releases energy, and is crucial for understanding how solutes interact with solvents, influencing solubility and solution stability.