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Chapter 13: Problem 1

Briefly describe the solution process at the molecular level. Use the dissolution of a solid in a liquid as an example.

Short Answer

Expert verified
Dissolution of a solid in a liquid at the molecular level involves the interactions between the solid's and liquid's molecules resulting in the breakdown of the solid into smaller fragments. These fragments then diffuse or spread out within the liquid due to the process of entropy, resulting in a uniform distribution of particles.

Step by step solution

01

Understanding the concepts

The solution process at the molecular level involves concepts from physical chemistry like intermolecular interactions and diffusion. Solids dissolve in liquids under the right conditions; this process is not merely mechanical, but it involves movement and interaction on a molecular scale.
02

Explanation of Intermolecular Interactions

The first part of the process involves the interactions between molecules. When a solid is placed in a liquid, the molecules of the solid interact with the molecules of the liquid. If the intermolecular forces of attraction are strong enough, the liquid molecules will penetrate the solid and cause it to split into smaller components. This could be explained by a principle called 'like dissolves like'. For example, polar solvents like water break down ionic or other polar substances.
03

Explanation of the Diffusion Process

Once the solid has been divided into smaller fragments or particles, these particles will start to spread or diffuse through the liquid. The particles will continue to move and spread out until they are evenly distributed throughout the liquid. This distribution process is a result of a property called entropy which is a measure of randomness or disorder. The system will always tend towards higher entropy, meaning it will always favor a more dispersed, random arrangement of particles.

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Most popular questions from this chapter

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.

How does each of the following affect the solubility of an ionic compound: (a) lattice energy, (b) solvent (polar versus nonpolar), (c) enthalpies of hydration of cation and anion?

Define boiling-point elevation and freezing-point depression. Write the equations relating boilingpoint elevation and freezing-point depression to the concentration of the solution. Define all the terms, and give their units.

The solubility of \(\mathrm{KNO}_{3}\) is \(155 \mathrm{~g}\) per \(100 \mathrm{~g}\) of water at \(75^{\circ} \mathrm{C}\) and \(38.0 \mathrm{~g}\) at \(25^{\circ} \mathrm{C}\). What mass (in grams) of \(\mathrm{KNO}_{3}\) will crystallize out of solution if exactly \(100 \mathrm{~g}\) of its saturated solution at \(75^{\circ} \mathrm{C}\) are cooled to \(25^{\circ} \mathrm{C} ?\)

Give two exceptions to Henry's law.
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