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Chapter 12: Problem 121

What do we mean when we say that solute particles diffuse through a solution?

Short Answer

Expert verified
When we say that solute particles diffuse through a solution, we mean that the solute particles move from areas of higher concentration to areas of lower concentration in the solvent, resulting in an even distribution and uniform concentration throughout the solution. This process happens due to random molecular motion and is influenced by factors such as temperature, concentration gradient, molecular size, and solvent properties.

Step by step solution

01

Understand Diffusion

Diffusion is the process where particles move from an area of higher concentration to an area of lower concentration, eventually reaching an equilibrium. In simpler terms, diffusion occurs when particles spread out evenly within a given space or medium.
02

Define Solute Particles

Solute particles are the substances that are dissolved in a solvent to make a solution. For example, sugar or salt dissolved in water forms a solution.
03

Explain the Process of Diffusion in a Solution

When solute particles are introduced into a solvent, they start moving randomly. Due to this random molecular motion, solute particles spread out in the solvent and eventually are evenly distributed throughout the solution. This process occurs due to the molecular attractions and collisions between the solute and solvent particles. The solute particles will continue to move and spread until their concentration is uniform across the entire solution.
04

Factors Affecting Diffusion of Solute Particles

Several factors affect the rate of diffusion of solute particles in a solution. These factors include: 1. Temperature: Higher temperature increases the kinetic energy of particles, which results in faster diffusion rates. 2. Concentration gradient: The higher the difference in concentration between two areas in a solution, the faster the rate of diffusion. 3. Molecular size: Smaller solute particles move faster, resulting in quicker diffusion rates compared to larger solute particles. 4. Solvent properties: The properties of the solvent, such as viscosity, can also affect the rate of diffusion. In conclusion, when we say that solute particles diffuse through a solution, we mean the solute particles move from an area of higher concentration to an area of lower concentration in the solvent, eventually spreading out evenly and achieving a uniform concentration throughout the solution.

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Key Concepts

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

Solute Particles
Solute particles are the tiny substances that are dissolved within another substance known as the solvent to create a solution. In the context of our daily life, when we stir sugar into coffee, sugar acts as the solute particles, and coffee is the solvent. These particles can be atoms, ions, or molecules, depending on the substance being dissolved. Their behavior in diffusion is fascinating as they move from an area where they are in high concentration, like right after you drop a sugar cube into a cup, towards lower concentration areas, which leads to a sweetened coffee throughout. This process contributes greatly to the homogeneity of mixtures in chemistry and various biological processes.
Concentration Gradient
Imagine you're at the top of a hill; naturally, you'll find your way down to the bottom due to gravity. Similarly, solute particles move along the concentration gradient, a path from an area of high solute concentration to an area of lower solute concentration. This movement is spontaneous and requires no external energy. Think of it as perfume dispersing in a room. The 'hill' in this scenario is defined by the concentration differences – the steeper the gradient, the faster the diffusion. This is akin to objects rolling down steeper hills faster. This gradient is the driving force behind the diffusion process, and it's an essential concept in understanding how substances spread through solutions.
Kinetic Energy
Kinetic energy refers to the energy that particles possess due to their motion. It's the microscopic hustle of atoms and molecules moving in random directions that can lead to large-scale observation of diffusion. In a warmer solution, particles wiggle, jiggle, and zoom around faster, which increases the rate at which they spread out. Kinetic energy is an invisible player in the symphony of diffusion, explaining why a cup of hot tea diffuses its aroma faster than a cool one. It's an intriguing phenomenon, demonstrating the swift dance of particles is one of the central pillars of how diffusion works. Higher kinetic energy implies more vigorous particle motion, hence a quicker diffusion.
Solvent Properties
The type of solvent and its characteristics have a considerable impact on how solute particles will diffuse. If the solvent is more viscous, meaning it's thicker like syrup, the solute particles will have a harder time moving through it, resulting in slower diffusion. Water, being a 'thin' solvent with low viscosity, allows solute particles like salt or sugar to move freely and quickly. Other properties like temperature and the solvent's molecular structure can alter the interaction with solute particles. For instance, some solvents might interact more strongly with certain solute particles, hindering or facilitating the diffusion process. It's much like swimming through different bodies of water; each requires a unique effort to move through them.

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Most popular questions from this chapter

When water boils, its temperature does not increase even though it is being heated. If the heat energy isn't being used to increase the temperature of the water, what is it being used for?

An aqueous solution is \(25.0\) mass \% \(\mathrm{NaCl}\). The density of the solution is \(1.05 \mathrm{~g} / \mathrm{mL}\). What is the molarity of the solution?

The freezing point of a solution prepared by dissolving \(0.200\) mole of \(\mathrm{HF}(g)\) in \(2.00 \mathrm{~kg}\) of water is \(-0.19{ }^{\circ} \mathrm{C}\). Is HF primarily intact in solution, existing as \(\mathrm{HF}(a q)\), or has it dissociated to \(\mathrm{H}^{+}(a q)\) and \(\mathrm{F}^{-}(a q)\) ions? Does this mean \(\mathrm{HF}\) is a weak or a strong acid?

Use the dueling-arrows model to explain what heating does to a liquid that eventually causes the liquid to boil.

There is a bottle of \(0.500 \mathrm{M}\) sucrose stock solution in the laboratory. Give precise instructions to your assistant on how to use the stock solution to prepare \(250.0 \mathrm{~mL}\) of a \(0.348 \mathrm{M}\) sucrose solution.
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