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6.1.4 - Equilibrium Involving Dissolution of Solid or Gases in Liquids

Interactive Audio Lesson

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Dissolution of Solids

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Teacher
Teacher

Today, we're going to discuss the dissolution of solids in liquids and the concept of equilibrium. When a solid, like sugar, is added to water, what happens to the sugar?

Student 1
Student 1

It starts to dissolve!

Teacher
Teacher

Exactly! But, eventually, there comes a point where no more sugar can dissolve. This is known as a saturated solution. Can anyone tell me what might be happening at that point?

Student 2
Student 2

I think the rate of dissolving equals the rate of crystallization.

Teacher
Teacher

Great insight! This balance between dissolving and crystallizing means we've reached dynamic equilibrium. Remember this acronym, 'DC', for 'Dissolve and Crystallize' to help recall this concept.

Dissolution of Gases

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Teacher
Teacher

Now, let's discuss the dissolution of gases in liquids, like carbon dioxide in soda. What happens when you open a soda bottle?

Student 3
Student 3

It fizzes and some gas escapes!

Teacher
Teacher

Exactly! The gas was dissolved under pressure. According to Henry's Law, if the pressure decreases, less gas can remain dissolved. Can someone explain how this relates back to equilibrium?

Student 4
Student 4

When the pressure drops, the equilibrium shifts to release more gas, causing it to fizz out.

Teacher
Teacher

Well put! Keep in mind that for gases, higher pressure leads to increased solubility. The key phrase to remember here is 'Pressure Develops Solubility' or PDS.

Influence of Temperature and Pressure

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Teacher
Teacher

How do you think temperature affects the solubility of solids?

Student 1
Student 1

I think higher temperatures allow more solids to dissolve.

Teacher
Teacher

Exactly! Warmer water can dissolve more sugar, for instance. Remember: 'Heat Helps Solubility' – HHS. Now regarding gases, what would happen if temperatures increase?

Student 2
Student 2

The gas would dissolve less, right?

Teacher
Teacher

Precisely! Increased temperature reduces gas solubility. Good job, everyone! Let's summarize: solids generally become more soluble with heat, while gases become less soluble.

Dynamic Equilibrium Overview

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Teacher
Teacher

Today we covered the concept of equilibrium involving the dissolution of solids and gases. Can someone define dynamic equilibrium for us?

Student 3
Student 3

It's when the rates of dissolving and crystallizing are equal.

Teacher
Teacher

Absolutely correct! Dynamic equilibrium is crucial not only in chemistry but also in various biological systems. Let's remember 'Equilibrium Equals Stability' – EES.

Introduction & Overview

Read a summary of the section's main ideas. Choose from Basic, Medium, or Detailed.

Quick Overview

This section discusses the dynamic equilibrium established during the dissolution of solids and gases in liquids and the factors affecting it.

Standard

The dissolution of solids and gases in liquids reaches a state of dynamic equilibrium where the rate of dissolution equals the rate of crystallization or condensation. This section covers the nature of saturated solutions, factors influencing solubility, the role of pressure for gases, and key principles such as Henry’s law. Furthermore, it outlines the implications of these equilibria in various chemical and biological contexts.

Detailed

Equilibrium Involving Dissolution of Solid or Gases in Liquids

This section delves into the concept of equilibrium in the context of dissolution, focusing on how solids and gases interact with liquids to reach a state of equilibrium. The equilibrium involving the dissolution of solids occurs when the concentration of the solid in solution is constant, indicating that the rate at which solid dissolves equals the rate at which it crystallizes. For instance, in a saturated solution like sugar in water, if we dissolve sugar at a higher temperature and cool it down, sugar crystals will precipitate, indicating the dynamic equilibrium between dissolved and solid sugar.

For gases, the dissolution is influenced by Henry's Law, which states that the amount of gas dissolved is proportional to its partial pressure above the liquid. For example, when soda bottles are opened, carbon dioxide escapes due to decreased pressure, showcasing how pressure changes affect gas solubility. The section further discusses how the equilibrium constant can help quantify these interactions and how different conditions such as temperature and pressure can shift the equilibrium state, affecting the solubility and concentration of gases and solids.

Understanding these concepts is crucial for interpreting reactions, controlling industrial synthesis processes, and even appreciating physiological processes where equilibria play a vital role.

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Audio Book

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Solids in Liquids

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We know from our experience that we can dissolve only a limited amount of salt or sugar in a given amount of water at room temperature. If we make a thick sugar syrup solution by dissolving sugar at a higher temperature, sugar crystals separate out if we cool the syrup to the room temperature. We call it a saturated solution when no more of solute can be dissolved in it at a given temperature. The concentration of the solute in a saturated solution depends upon the temperature. In a saturated solution, a dynamic equilibrium exists between the solute molecules in the solid state and in the solution:
Sugar (solution) ⇌ Sugar (solid),
and the rate of dissolution of sugar = rate of crystallisation of sugar.

Detailed Explanation

When we try to dissolve substances like sugar in water, there is a limit to how much can dissolve at a given temperature, leading to a point where the solution becomes saturated. At this point, the solid sugar and the dissolved sugar molecules are in a state of dynamic equilibrium. This means that sugar molecules are continually dissolving into the solution and solidifying back into sugar crystals at equal rates, keeping the total amount of dissolved sugar constant. This equilibrium illustrates that the system is active and balanced, with no net change in concentration.

Examples & Analogies

Think of making lemonade. When you add sugar to the water, it starts to dissolve. If you keep adding sugar after a while, it won't dissolve anymore because the water can't hold any more sugar at that temperature, just like a sponge unable to absorb more water once it's full. If you heat the lemonade, more sugar can dissolve; however, if you cool it down again, some of that sugar will crystallize back out, demonstrating the concept of dynamic equilibrium.

Gases in Liquids

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When a soda water bottle is opened, some of the carbon dioxide gas dissolved in it fizzes out rapidly. The phenomenon arises due to difference in solubility of carbon dioxide at different pressures. There is equilibrium between the molecules in the gaseous state and the molecules dissolved in the liquid under pressure i.e.,
CO2 (gas) ⇌ CO2 (in solution).
This equilibrium is governed by Henry’s law, which states that the mass of a gas dissolved in a given mass of a solvent at any temperature is proportional to the pressure of the gas above the solvent.

Detailed Explanation

When you open a bottle of soda, the pressure inside is released, causing the carbon dioxide gas, previously dissolved in the liquid, to escape rapidly as bubbles. This process is an example of gas dissolving in a liquid reaching equilibrium. Henry's law helps explain this process, which tells us that the concentration of dissolved gas in a liquid is directly proportional to the pressure exerted by that gas in the atmosphere above the liquid. As the pressure drops when the bottle is opened, the dissolved gas molecules cannot be retained in the solution and escape as bubbles.

Examples & Analogies

This is similar to shaking a can of soda. When you shake it, the pressure builds up inside the can. When you finally open it, all that accumulated gas escapes quickly as fizz. Just like a sponge that can hold more water under pressure, the soda can hold more carbon dioxide when under pressure, but releases that gas when the pressure is released.

General Characteristics of Solubility Equilibria

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We can generalize that:
(i) For solid-liquid equilibrium, there is only one temperature (melting point) at 1 atm at which the two phases can coexist. If there is no exchange of heat with the surroundings, the mass of the two phases remains constant.
(ii) For liquid-vapour equilibrium, the vapour pressure is constant at a given temperature.
(iii) For dissolution of solids in liquids, the solubility is constant at a given temperature.
(iv) For dissolution of gases in liquids, the concentration of a gas in liquid is proportional to the pressure (concentration) of the gas over the liquid.

Detailed Explanation

These general characteristics describe the behavior of different types of solubility equilibria. For solid-liquid equilibria, a specific temperature allows the solid to exist together with its dissolved form without losing mass. In the case of liquid-vapour equilibria, the pressure exerted by the vapour remains constant for a particular liquid and temperature. When dealing with solids dissolving in liquids, the maximum amount of solute that can dissolve remains constant at a designated temperature. Conversely, for gases, their solubility in liquids varies directly with the pressure of the gas above the liquid, illustrating that changes in pressure affect how much gas can dissolve.

Examples & Analogies

For instance, if you take a pot of water and heat it to boil, you will see the water vaporize into steam. The steam represents the liquid-vapour equilibrium while the temperature of the water remains constant until it is fully boiled. Similarly, you can think of an experiment where we dissolve sugar in water; it stops dissolving when it reaches a particular saturation point, resembling a limitation in solubility reflecting these equilibria.

Definitions & Key Concepts

Learn essential terms and foundational ideas that form the basis of the topic.

Key Concepts

  • Dynamic equilibrium: Achieved when the rate of dissolution equals the rate of precipitation.

  • Saturation point: The maximum concentration of solute that can dissolve at a given temperature and pressure.

  • Henry's Law: Gas solubility increases with pressure and decreases with temperature.

  • Solubility product (Ksp): The equilibrium constant associated with the solubility of a sparingly soluble salt.

Examples & Real-Life Applications

See how the concepts apply in real-world scenarios to understand their practical implications.

Examples

  • The creation of a saturated sugar solution demonstrates the concept of dynamic equilibrium as the sugar dissolves until no more can do so.

  • Opening a soda can shows how gases escape from a liquid when pressure is released, illustrating Henry's Law.

Memory Aids

Use mnemonics, acronyms, or visual cues to help remember key information more easily.

🎵 Rhymes Time

  • If you want the gas to stay, keep the pressure high all day.

📖 Fascinating Stories

  • Imagine a party where gas balloons float until someone opens a door, letting them all escape!

🧠 Other Memory Gems

  • Remember PDS: Pressure Develops Solubility.

🎯 Super Acronyms

KSP for 'Keep Salt in the Product.'

Flash Cards

Review key concepts with flashcards.

Glossary of Terms

Review the Definitions for terms.

  • Term: Saturated Solution

    Definition:

    A solution that cannot dissolve any more solute at a given temperature.

  • Term: Dynamic Equilibrium

    Definition:

    A state where the forward and reverse processes occur at equal rates, resulting in constant concentrations.

  • Term: Henry's Law

    Definition:

    A principle stating that the amount of gas dissolved in a liquid is proportional to its partial pressure above the liquid.

  • Term: Solubility Product (Ksp)

    Definition:

    An equilibrium constant for the dissolution of a sparingly soluble salt.