Energy/Enthalpy of solution

Energy/Enthalpy of solution

This refers to the enthalpy change for the formation of an infinitely dilute solution of 1 mole of salt.

NaCl(s) +aq→ Na⁺(aq) + Cl^– (aq)                                       ∆H_m^Ө(298K) = +4 kJmol^-1

 Factors affecting the magnitude of enthalpy of solution

 Enthalpy of solution = lattice energy (+ve) + sum of hydration energy of ions (-ve)

When the lattice energy exceeds the sum of hydration energies of the ions, the enthalpy of solution is positive (endothermic) and the salt is insoluble.

When the lattice energy is less than the sum of hydration energies of the ions, the enthalpy of solution is negative (exothermic) and the salt is soluble.

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