Enthalpy change of solution is the enthalpy change that takes place when one mole of a compound dissolves completely in water under standard conditions. When a solid dissolves, two processes take place:
- breakdown of the ionic lattice into gaseous ions
This involves breaking down the crystal lattice and separating the ions. This requires energy, and is therefore ΔH-ve. The energy involved has the same magnitude as lattice enthalpy but the sign is opposite.
The positively charged ions will be slightly attracted to the negative oxygen atoms in water. The negatively charged ions will be slightly attracted to the slightly positive hydrogen ions. Standard enthalpy change of hydration releases energy. It is always exothermic. It is the enthalpy change that takes place when one mole of isolated gaseous ions dissolves completely in water, forming one mole of aqueous ions under standard conditions.
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