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Chapter 11: Problem 23

When pure methanol is mixed with water, the resulting solution feels warm. Would you expect this solution to be ideal? Explain.

Short Answer

Expert verified
The methanol-water solution is not ideal because it feels warm when mixed, indicating that heat is evolved during the mixing process. This exothermic behavior implies that the solute-solvent interactions between methanol and water are stronger than the pure solute-solute and solvent-solvent interactions, resulting in a non-ideal solution.

Step by step solution

01

Understanding Ideal Solutions

An ideal solution is a solution in which the interactions between the solute and solvent particles are essentially the same as those in the pure solvents. In other words, the solute-solvent interactions are equal to the solute-solute and solvent-solvent interactions. This means that there is no change in enthalpy as a result of mixing the solute and solvent, hence, no heat is evolved or absorbed during the process.
02

Exothermic and Endothermic Solutions

In a non-ideal solution, the solute-solvent interactions are different from the interactions present before mixing. This difference in interactions results in a change in enthalpy. Depending on whether the solute-solvent interactions are stronger or weaker than the solute-solute and solvent-solvent interactions, the solution can be exothermic (heat evolves) or endothermic (heat is absorbed).
03

Methanol-Water Solution

In the given exercise, when methanol is mixed with water, the resulting solution feels warm, which indicates that heat is evolved during mixing. This means that the solute-solvent interactions, in this case between methanol and water, are stronger than the pure solute-solute and solvent-solvent interactions. Therefore, mixing methanol and water results in an exothermic process.
04

Conclusion

Based on the observation that the methanol-water solution feels warm, we can conclude that the solution is not ideal, as energy is released in the form of heat due to the difference in solute-solvent interactions compared to the pure solute and solvent. The solution is exothermic and non-ideal.

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Most popular questions from this chapter

A solution is prepared by mixing 0.0300 mole of \(\mathrm{CH}_{2} \mathrm{Cl}_{2}\) and 0.0500 mole of \(\mathrm{CH}_{2} \mathrm{Br}_{2}\) at \(25^{\circ} \mathrm{C}\) . Assuming the solution is ideal, calculate the composition of the vapor (in terms of mole fractions at \(25^{\circ} \mathrm{C}\) . At \(25^{\circ} \mathrm{C}\) , the vapor pressures of pure \(\mathrm{CH}_{2} \mathrm{Cl}_{2}\) and pure \(\mathrm{CH}_{2} \mathrm{Br}_{2}\) are 133 and 11.4 torr, respectively.

From the following: Pure water solution of \(\mathrm{C}_{12} \mathrm{H}_{22} \mathrm{O}_{11}(m=0.01)\) in water solution of \(\mathrm{NaCl}(m=0.01)\) in water solution of \(\mathrm{CaCl}_{2}(m=0.01)\) in water Choose the one with the a. highest freezing point. b. lowest freezing point. c. highest boiling point. d. lowest boiling point. e. highest osmotic pressure.

An aqueous antifreeze solution is 40.0\(\%\) ethylene glycol \(\left(\mathrm{C}_{2} \mathrm{H}_{6} \mathrm{O}_{2}\right)\) by mass. The density of the solution is 1.05 \(\mathrm{g} / \mathrm{cm}^{3}\) . Calculate the molality, molarity, and mole fraction of the ethylene glycol.

The term proof is defined as twice the percent by volume of pure ethanol in solution. Thus, a solution that is 95\(\%\) (by volume) ethanol is 190 proof. What is the molarity of ethanol in a 92 proof ethanol-water solution? Assume the density of ethanol, \(\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}\) , is 0.79 \(\mathrm{g} / \mathrm{cm}^{3}\) and the density of water is 1.0 \(\mathrm{g} / \mathrm{cm}^{3}\) .

An aqueous solution is 1.00\(\% \mathrm{NaCl}\) by mass and has a density of 1.071 \(\mathrm{g} / \mathrm{cm}^{3}\) at \(25^{\circ} \mathrm{C}\) . The observed osmotic pressure of this solution is 7.83 atm at \(25^{\circ} \mathrm{C}\) . a. What fraction of the moles of NaCl in this solution exist as ion pairs? b. Calculate the freezing point that would be observed for this solution.
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