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Mastering Solution Chemistry and Solubility
Unlock the secrets of solution chemistry and solubility. Discover how solutes dissolve in solvents, understand chemical reactions, and apply these concepts to real-world scenarios. Perfect for beginners and advanced learners alike.

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Now Playing:Intro to solution chemistry and solubility – Example 0a
Intros
  1. Solution Chemistry: Introduction
  2. Solution Chemistry: Introduction
    Key definitions in solution chemistry.
  3. Solution Chemistry: Introduction
    Why are solutions important in chemistry?
Examples
  1. Recall the key definitions of solution chemistry.
    1. Label the diagram below with the terms solvent, solute, and solution.
      chem11-8-1 Ex1a solution, solvent, solute

    2. Label the diagrams below with the terms soluble and insoluble.
      chem11-8-1 Ex1b soluble, insoluble

Introduction to solution chemistry and solubility
Jump to:NotesConceptFAQsPrerequisites
Notes
In this lesson, we will learn:
  • What a solution is and the definitions around it.
  • Why most chemical reactions are done in solutions and why they are useful.
  • The definitions of solubility and factors that affect it.

Notes:
  • Solutions are important in chemistry because most chemical reactions and processes are done with the reactants dissolved in solutions. There are good reasons for this that will be revealed throughout this chapter.

  • A solution is a single-phase homogenous (evenly spread) mixture of two components called the solvent and the solute:
    • The solvent is the chemical in larger amount – its greater number of molecules surround the dispersed, outnumbered solute. Chemists say that a solvent dissolves a solute.
    • The solute is the chemical in smaller amount – its smaller quantity means individual molecules of solute are dispersed throughout the solvent molecules and surrounded by them. Chemists say a solute is dissolved by a solvent.

  • The diagram below illustrates the definitions above. Remember a few key points below:
    • The solvent is also made of molecules, only in much greater numbers than the solute, easily in 1:1000 ratio of solute to solvent, and normally larger than this!
    • Solute particles are far too small to be visible when dissolved. Diagrams showing them visible are just for illustration!
    solution, solvent, solute


  • In a solution, the solute (e.g. chemical A) molecules are so outnumbered by the solvent (chemical B) molecules, that we can think of each individual chemical A molecule as fully exposed to the chemical B molecules and anything else that might be dissolved in chemical B as well – all particles are colliding with energy into one another.
    • This is extremely useful for chemicals that are solids at room temperature! By dissolving them, we can get them to 'behave' like liquids without melting them, which might have needed very high temperatures. Then, reactions can be done with them.

  • The solution 'state' allows atoms and molecules to collide with each other freely at mild conditions as if they were liquids. This is extremely useful in chemistry! Think about chemical A and chemical B reacting in the following situations:
    • Chemicals A and B are both solids: Particles in solids are very close together and tightly packed. Very few particles of A and B will be making contact with each other at any one time and so the reaction is extremely slow.
    • Chemicals A and B are both gases: Gas particles are very high in energy and will spread through space very quickly. The reactants will not collide with each other much and will escape the reaction vessel unless it is air tight.
    • Chemicals A and B are both liquids: This is an advantage, but the two chemicals might not be able to mix together – they may be immiscible. If they are then the chemicals form two separate layers where A and B particles are generally not colliding with each other.

  • Solubility is the amount of a substance that can dissolve in a specific amount of another substance at a specific temperature. Whether a chemical can dissolve in another chemical and make a solution is largely to do with intermolecular forces acting between the molecules. A well-known phrase to explain solubility is "like dissolves like."
    • This means a chemical that is polar – one that has hydrogen bonding – will dissolve other polar molecules and other polar molecules will dissolve it.
    In the same way, less polar chemicals – those displaying just van der Waals intermolecular forces – will dissolve other non-polar chemicals and vice versa.
    There are a number of factors that affect solubility and when you report solubility they must all be mentioned!
    • The solute used, and the quantity of solute
    • The solvent used, and the quantity of solvent
    • The temperature the solution is made at.
    A typical solubility measurement might read "250g / 1L H2O, 25°C" – this means that for every liter of water solvent, 250g of the solute will dissolve at 25°C. Changing any of those factors will change solubility of your solution.

  • As stated above, like dissolves like:
    • If a compound doesn't dissolve in a solvent we say it is insoluble. For example, when a non-polar compound and a polar compound are mixed together, they will not dissolve the other because of the different intermolecular forces between their molecules.
    • If a compound does dissolve in a solvent we say it is soluble in the solvent. For example, if two polar or two non-polar compounds were mixed together, their similar intermolecular forces would enable a solution to form.

  • A solution is made in a way that the amount of solvent is much greater than the solute it is dissolving – if there is too much solute added or not enough solvent it becomes a saturated solution. Saturation, then, is when a solution has dissolved the maximum amount of solute possible.
    • An unsaturated solution is a solution that is able to dissolve more solute – it is not saturated.
    • A saturated solution is a solution that cannot dissolve any more solute if it was added – like a sponge saturated with water, it is saturated with solute! If your solution is saturated, you need to add more solvent before you can add any more solute.
  • When chemicals are dissolved they often show different properties to their undissolved state. This is particularly true of ionic compounds which can conduct electricity only in solution!
Concept

Introduction to Solution Chemistry

Welcome to the fascinating world of solution chemistry! Solutions play a crucial role in chemical reactions and are fundamental to understanding many processes in chemistry. In this article, we'll explore the basics of solution chemistry, including key concepts like solutes and solvents. Solutions are mixtures where one substance (the solute) is dissolved in another (the solvent). This process is essential in various chemical reactions, from simple everyday occurrences to complex industrial processes. To help you grasp these concepts, we've included an introductory video that explains the fundamental principles of solution chemistry. Whether you're a beginner or looking to refresh your knowledge, this overview will provide a solid foundation for understanding how solutions work in chemical reactions. Join us as we dive into the world of solution chemistry and discover its importance in the broader field of chemistry!

FAQs

  1. What is a solution in simple words?

    A solution is a homogeneous mixture where one substance (the solute) is dissolved in another substance (the solvent). For example, when sugar dissolves in water, it forms a solution. The sugar is the solute, and water is the solvent.

  2. What is a solution example?

    Common examples of solutions include salt water, coffee, and air. In salt water, salt (solute) is dissolved in water (solvent). Coffee is a solution of various compounds extracted from coffee beans dissolved in water. Air is a solution of different gases like nitrogen, oxygen, and carbon dioxide.

  3. What best describes a solution in chemistry?

    In chemistry, a solution is best described as a homogeneous mixture at the molecular level, where the solute is uniformly distributed throughout the solvent. It forms a single phase and its composition can be varied within certain limits.

  4. What is solution and mixture?

    A solution is a type of mixture, but not all mixtures are solutions. A mixture is a combination of two or more substances that are not chemically bonded. A solution is a specific type of mixture where one substance (solute) is completely dissolved in another (solvent), forming a homogeneous mixture.

  5. How does temperature affect solubility?

    Temperature generally affects solubility in two ways: For most solid solutes, increasing temperature increases solubility. This is why sugar dissolves more easily in hot tea. For gases, however, increasing temperature typically decreases solubility. This is why carbonated drinks lose their fizz faster when warm.

Prerequisites

Before delving into the fascinating world of solution chemistry and solubility, it's crucial to have a solid foundation in certain prerequisite topics. One of the most important areas to understand is the Introduction to kinetics. This fundamental concept plays a significant role in comprehending the behavior of substances in solutions and their solubility characteristics.

Understanding reaction kinetics in solutions is essential when studying solution chemistry and solubility. The rate at which chemical reactions occur in solutions directly impacts the dissolution process and the formation of precipitates. By grasping the principles of kinetics, students can better predict and explain the behavior of various substances when they are introduced into solvents.

The Introduction to kinetics provides valuable insights into factors that influence reaction rates, such as concentration, temperature, and the presence of catalysts. These factors are equally important in solution chemistry, as they affect the speed at which solutes dissolve and the maximum amount of substance that can be dissolved in a given solvent.

Moreover, kinetics concepts help explain the dynamic equilibrium that exists in saturated solutions. Understanding how forward and reverse reactions reach a balance is crucial for grasping the principles of solubility equilibrium and the factors that can shift this equilibrium. This knowledge is particularly useful when dealing with topics like solubility product constants and precipitation reactions.

The study of reaction kinetics also introduces students to important mathematical models and equations that are applicable to solution chemistry. These tools are invaluable for quantifying and predicting solubility behavior, making calculations related to concentration changes over time, and analyzing the effects of various factors on dissolution rates.

Furthermore, the Introduction to kinetics lays the groundwork for understanding more advanced topics in solution chemistry, such as the kinetics of complex ion formation and the rates of precipitation reactions. These concepts are crucial for students pursuing further studies in analytical chemistry, environmental science, and chemical engineering.

By mastering the principles of kinetics, students will be better equipped to tackle the challenges presented in solution chemistry and solubility. They will have the tools to analyze and predict the behavior of substances in various solvents, understand the factors that influence solubility, and apply this knowledge to real-world scenarios in both academic and industrial settings.

In conclusion, a strong grasp of reaction kinetics is indispensable for anyone looking to excel in the study of solution chemistry and solubility. It provides the necessary framework for understanding the dynamic processes that occur in solutions and sets the stage for exploring more complex phenomena in this fascinating field of chemistry.