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Lattice Enthalpy, Hydration Enthalpy And Enthalpy Of Solution MCQ - Practice Questions with Answers

Edited By admin | Updated on Sep 25, 2023 25:23 PM | #NEET

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Lattice Enthalpy, Hydration Enthalpy And Enthalpy Of Solution is considered one of the most asked concept.
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MEDIUM

HCl was passed through a solution of $CaCl_{2}, MgCl_{2},NaCl$ . Which of the following compound(s) crystallize (s)?

$NaCl,$ $MgCl_{2}andCaCl_{2}$

Both $MgCl_{2}andCaCl_{2}$

Only $NaCl$

Only $MgCl_{2}$

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Concepts Covered - 1

Lattice Enthalpy, Hydration Enthalpy And Enthalpy Of Solution

Lattice Enthalpy

The lattice enthalpy of an ionic compound is the enthalpy change which occurs when one mole of an ionic compound is formed from its ions in gaseous state.

$\mathrm{Na^+(g) + Cl^-(g) \longrightarrow NaCl(s), \Delta H=-788\ kJmole^{-1}}$

Heat of Hydration

The enthalpy change during hydration of one mole of any gaseous ion is called heat of hydration.

$\mathrm{Na^+(g) \longrightarrow Na^+(aq), \Delta H= \Delta H_{hyd_{Na^+}}}$

$\mathrm{Cl^-(g) \longrightarrow Cl^-(aq), \Delta H= \Delta H_{hyd_{Cl^-}}}$

Heat of Solution

It is change in enthalpy when one mole of a solid solute is dissolved in excess of solvent.

$\mathrm{NaCl(s) \longrightarrow Na^+(aq) + Cl^-(aq), \Delta H= \Delta H_{sol_{NaCl}}}$

Solubility of an Ionic Compound in water

When an ionic compound dissolves in a solvent, the ions leave their ordered positions on the crystal lattice. These are now more free in solution. But solvation of these ions (hydration in case solvent is water) also occurs at the same time. The enthalpy of solution of any ionic solid, in water is, therefore, determined by the selective values of the lattice enthalpy and enthalpy of hydration of ions. This will be more clear with the help of the diagram given below:

Thus, the enthalpy of solution, enthalpy of hydration and the lattice energy can be related as

$\mathrm{\Delta_{\text {sol }} H^{0}=\Delta_{\text {lattice }} H^{0}+\Delta_{\text {hyd }} H^{0}}$

For most of the ionic compounds, $\mathrm{\Delta_{\text {sol }} H^{0}}$ is positive and the dissociation process is endothermic. Therefore the solubility of most salts in water increases with rise of temperature. If the lattice enthalpy is very high, the dissolution of the compound may not take place at all.