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Chapter 13: Problem 5

Explain why the solution process invariably leads to an increase in disorder.

Short Answer

Expert verified
The solution process invariably leads to an increase in disorder because it involves breaking down the structured arrangement of solute and solvent molecules and mixing them together, creating more molecular randomness or disorder. This aligns with the concept of entropy, which states that systems tend towards greater disorder.

Step by step solution

01

Understanding Entropy

Entropy is a physical quantity that is often associated with the amount of disorder in a system or the degree of randomness. In general, natural systems tend to move towards a state of greater entropy or disorder.
02

Recognizing the Stages of Solution Process

There are three stages in the solution process: breaking apart the solute molecules (endothermic), breaking apart the solvent molecules (endothermic), and the combining of solute and solvent molecules (exothermic).
03

Breaking Apart the Solute and Solvent

During the first two stages, the solute and solvent separate into individual particles. The order present in the original structured arrangement of solute and solvent molecules is lost, leading to increased molecular randomness or disorder.
04

Combining Solute and Solvent

After breaking apart, the individual particles of the solute and the solvent mix together. This mixing further increases the disorder, as the solute particles become randomly distributed among the solvent particles.
05

Conclusion

Overall, the solution process involves breaking ordered structures (solute and solvent) and creating a new configuration with more randomness or disorder. Hence, an increase in entropy is inevitable during the solution process.

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Most popular questions from this chapter

Basing your answer on intermolecular force considerations, explain what "like dissolves like" means.

Acetic acid is a polar molecule and can form hydrogen bonds with water molecules. Therefore, it has a high solubility in water. Yet acetic acid is also soluble in benzene \(\left(\mathrm{C}_{6} \mathrm{H}_{6}\right),\) a nonpolar solvent that lacks the ability to form hydrogen bonds. A solution of \(3.8 \mathrm{~g}\) of \(\mathrm{CH}_{3} \mathrm{COOH}\) in \(80 \mathrm{~g} \mathrm{C}_{6} \mathrm{H}_{6}\) has a freezing point of \(3.5^{\circ} \mathrm{C}\). Calculate the molar mass of the solute and explain your result.

Arrange these solutions in order of decreasing freezing point: (a) \(0.10 \mathrm{~m} \mathrm{Na}_{3} \mathrm{PO}_{4},\) (b) \(0.35 \mathrm{~m} \mathrm{NaCl}\) (c) \(0.20 \mathrm{~m} \mathrm{MgCl}_{2},\) (d) \(0.15 \mathrm{~m} \mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6},\) (e) \(0.15 \mathrm{~m}\) \(\mathrm{CH}_{3} \mathrm{COOH}\)

Calculate the molalities of these aqueous solutions: (a) \(1.22 M\) sugar \(\left(\mathrm{C}_{12} \mathrm{H}_{22} \mathrm{O}_{11}\right)\) solution (density of solution \(=1.12 \mathrm{~g} / \mathrm{mL}\) ), (b) \(0.87 \mathrm{M} \mathrm{NaOH}\) solution (density of solution \(=1.04 \mathrm{~g} / \mathrm{mL}),(\mathrm{c})\) \(5.24 \mathrm{M} \mathrm{NaHCO}_{3}\) solution (density of solution \(=\) \(1.19 \mathrm{~g} / \mathrm{mL})\)

Define the van't Hoff factor. What information does this quantity provide?
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