The lattice energy of NaCl is -786 kJ / mol, and the enthalpy of hydration of 1 mole of gaseous

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The lattice energy of NaCl is -786 kJ / mol, and the...

The lattice energy of $\mathrm{NaCl}$ is $-786 \mathrm{kJ} / \mathrm{mol}$, and the enthalpy of hydration of 1 mole of gaseous $\mathrm{Na}^{+}$ and 1 mole of gaseous $\mathrm{Cl}^{-}$ ions is $-783 \mathrm{kJ} / \mathrm{mol} .$ Calculate the enthalpy of solution per mole of solid NaCl.

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Key Concepts

Hydration Enthalpy

Hydration enthalpy is the energy released when gaseous ions are solvated by water molecules upon dissolution. This exothermic process occurs as water molecules surround and stabilize the ions, and its magnitude depends on factors such as ion charge and size. It plays a crucial role in determining the overall energy change during the dissolution of ionic compounds in water.

Lattice Energy

Lattice energy refers to the amount of energy released when gaseous ions combine to form an ionic solid, or equivalently, the energy required to convert the solid into its constituent gaseous ions. It is a key parameter that reflects the strength of the ionic bonds in a crystalline lattice and helps explain the stability and structure of ionic compounds.

Enthalpy of Solution

The enthalpy of solution is the overall heat change that occurs when a solute dissolves in a solvent, and it is determined by combining the energy needed to break the ionic lattice (endothermic) with the energy released during the hydration of the ions (exothermic). Understanding this combined effect is essential in predicting whether a dissolution process will be exothermic or endothermic, which in turn impacts solubility and reaction conditions.

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