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(B) For an ideal solution,the enthalpy of mixing is zero,i.e.,$\Delta H_{mix} = 0$. The total enthalpy change of the solution is given by $\Delta H_{s

Vedclass · Accepted Answer

$\Delta H_{soln} = \Delta H_1 + \Delta H_2 + \Delta H_3$

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(B) For an ideal solution,the enthalpy of mixing is zero,i.e.,$\Delta H_{mix} = 0$. The total enthalpy change of the solution is given by $\Delta H_{soln} = \Delta H_1 + \Delta H_2 + \Delta H_3$. Since $\Delta H_{soln} = 0$ for an ideal solution,we have $\Delta H_1 + \Delta H_2 + \Delta H_3 = 0$. However,based on the standard thermodynamic cycle for solution formation,the enthalpy of solution is $\Delta H_{soln} = \Delta H_1 + \Delta H_2 + \Delta H_3$. If we define $\Delta H_3$ as the enthalpy of interaction between solute and solvent,then for an ideal solution,$\Delta H_1 + \Delta H_2 + \Delta H_3 = 0$.

The formation of a binary solution is considered as follows:
$(1)$ Pure solvent enthalpy $\Delta H_1$ (separated)
$(2)$ Pure solute enthalpy $\Delta H_2$ (separated)
$(3)$ Pure solvent + Pure solute $\to$ Solution $\to$ Enthalpy $\Delta H_3$
If $......$ then the resulting solution is ideal.

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The formation of a binary solution is considered as follows: $(1)$ Pure solvent enthalpy $\Delta H_1$ (separated) $(2)$ Pure solute enthalpy $\Delta H_2$ (separated) $(3)$ Pure solvent + Pure solute $\to$ Solution $\to$ Enthalpy $\Delta H_3$ If $......$ then the resulting solution is ideal.