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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 involves solute particles being surrounded and separated by solvent molecules due to interaction forces, resulting in a uniform mixture.

Step by step solution

01

Identify the Substances Involved

First, identify the solid that is dissolving and the liquid solvent. For example, if we are dissolving salt (sodium chloride, NaCl) in water, NaCl is the solute, and water is the solvent.
02

Understand the Nature of Interactions

Recognize that molecules of the solute (NaCl) and molecules of the solvent (water) are held together by forces. The solute molecules are held together by ionic bonds, and the water molecules by hydrogen bonds. These bonds must be overcome for dissolution to occur.
03

Solute-Solvent Interaction

When NaCl is added to water, the positive and negative ions of NaCl are attracted to the polar water molecules. Water's partially negatively charged oxygen atoms attract Na+ ions, and its hydrogen atoms (partially positive) attract Cl- ions.
04

Dissolution Process

The water molecules surround the Na+ and Cl- ions, effectively pulling them away from the solid structure (crystal lattice) of NaCl. This process is called hydration and is the key molecular event in the dissolution of NaCl in water.
05

Establishment of Solution Equilibrium

As more ions are hydrated, the solid NaCl eventually disperses fully within the water, resulting in a homogeneous solution. The process reaches equilibrium when the rate of dissolution equals the rate of precipitation (if any occurs), assuming a saturated solution is formed.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Molecular Level
When we describe the solution process at the molecular level, we focus on the smallest particles involved鈥攎olecules and ions. These particles interact through forces that dictate how substances mix and dissolve.
Imagine the scenario as an intricate dance of particles. Each particle is influenced by forces that attract or repel others. For example, in our classic case of salt (sodium chloride, NaCl) dissolving in water, both substances are made up of molecules that interact vigorously.
  • The salt is composed of ions, which are positively (Na+) and negatively (Cl-) charged particles.
  • Water, the solvent, is made up of polar molecules with areas of partial positive and negative charges due to its molecular shape.
Understanding these interactions at the molecular level is key to grasping why and how substances dissolve.
Dissolution
Dissolution is the process where a solute integrates into a solvent, forming a solution. Let's break it down using the dissolution of sodium chloride (NaCl) in water.
Initially, solid NaCl is held together by strong ionic bonds, forming a crystal structure. When introduced to water, this structure begins to alter dramatically.
  • The ionic bonds between salt's particles must be overcome for the crystals to disband.
  • Simultaneously, the water molecules begin to interact with the surface ions.
Dissolution at this point means transforming the ordered solid structure into a dispersed and homogeneous state within the liquid solvent.
Solute-Solvent Interaction
The interaction between solute and solvent particles is fundamental to the dissolution process. This relationship can be visualized as a competitive attraction between different forces.
For NaCl and water, the process involves:
  • Breaking the ionic bonds in NaCl crystals.
  • Overcoming hydrogen bonds between water molecules.
  • Forming new interactions between Na+ and Cl- ions with water molecules.
Water acts as a magnet because its polar molecules have partial charges, which makes them exceptionally effective at surrounding and stabilizing ions from the solute.
Ion Hydration
Ion hydration is the heart of the dissolution process where ions become enveloped by solvent molecules.
In our NaCl example, water molecules play a crucial role. As water molecules interact with Na+ and Cl- ions, they effectively shield these ions from each other, disrupting the original ionic lattice.
  • Oxygen's partial negative charges in water molecules are attracted to Na+ ions.
  • Hydrogen's partial positive charges are attracted to Cl- ions.
This attraction forms a stable cage of water molecules around each ion, known as a hydration shell. This hydration prevents the ions from recombining into a solid, facilitating a clear and stable solution.

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Most popular questions from this chapter

Valinomycin is an antibiotic. It functions by binding \(\mathrm{K}^{+}\) ions and transporting them across the membrane into cells to offset the ionic balance. The molecule is represented here by its skeletal structure in which the end of each straight line corresponds to a carbon atom (unless a \(\mathrm{N}\) or an \(\mathrm{O}\) atom is shown at the end of the line). There are as many \(\mathrm{H}\) atoms attached to each \(\mathrm{C}\) atom as necessary to give each \(\mathrm{C}\) atom a total of four bonds. Use the "like dissolves like" guideline to explain its function. (Hint: The \(-\mathrm{CH}_{3}\) groups at the two ends of the Y shape are nonpolar.)

Explain why ethanol \(\left(\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}\right)\) is not soluble in cyclohexane \(\left(\mathrm{C}_{6} \mathrm{H}_{12}\right)\).

Before a carbonated beverage bottle is sealed, it is pressurized with a mixture of air and carbon dioxide. (a) Explain the effervescence that occurs when the cap of the bottle is removed. (b) What causes the fog to form near the mouth of the bottle right after the cap is removed?

Hydrogen peroxide with a concentration of 3.0 percent \(\left(3.0 \mathrm{~g}\right.\) of \(\mathrm{H}_{2} \mathrm{O}_{2}\) in \(100 \mathrm{~mL}\) of solution) is sold in drugstores for use as an antiseptic. For a 10.0 -mL 3.0 percent \(\mathrm{H}_{2} \mathrm{O}_{2}\) solution, calculate (a) the oxygen gas produced (in liters) at STP when the compound undergoes complete decomposition and (b) the ratio of the volume of \(\mathrm{O}_{2}\) collected to the initial volume of the \(\mathrm{H}_{2} \mathrm{O}_{2}\) solution.

Which of these two aqueous solutions has (a) the higher boiling point, (b) the higher freezing point, and (c) the lower vapor pressure: \(0.35 \mathrm{~m} \mathrm{CaCl}_{2}\) or \(0.90 \mathrm{~m}\) urea? State your reasons.
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