Formation of a solution from two components can be considered as: (i) Pure solvent $\rightarrow$ separated solvent molecules $\Delta \mathrm{H}_1$ (ii) Pure solute $\rightarrow$ separated solute molecules, $\Delta \mathrm{H}_2$ (iii) Separated solvent and solute molecules $\rightarrow$ solution,…

Question

Formation of a solution from two components can be considered as: (i) Pure solvent $\rightarrow$ separated solvent molecules $\Delta \mathrm{H}_1$ (ii) Pure solute $\rightarrow$ separated solute molecules, $\Delta \mathrm{H}_2$ (iii) Separated solvent and solute molecules $\rightarrow$ solution, $\Delta \mathrm{H}_3$ Solution so formed will be ideal of:

Aicharya · Accepted Answer

So the enthalpy of solution can either be endothermic, exothermic or neither $(\Delta$ Hsolution $=0)$, depending on how much heat is required or release in each step. If $\Delta$ Hsolution $=$ 0 , then the solution is called an ideal solution and if
$\Delta$ Hsolution $ > 0$ or $\Delta$ Hsolution $< 0$, then these solutions are called non-ideal solutions.
Related Theory
The enthalpy of solution depends on the strengths of intermolecular forces of the solute and solvent. If the solution is ideal, and $\Delta \mathrm{H}$ solution $=0$, then
$\begin{aligned}
& \Delta H_{\text {solution }}=\Delta H_1+\Delta H_2+\Delta H_3=0 \\
& \Delta H_1+\Delta H_2=-\Delta H_3
\end{aligned}$

Formation of a solution from two components can be considered as: (i) Pure solvent $\rightarrow$ separated…

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