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Understanding Solutions in Chemistry: Components, Concentration, and Types

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nibaw
16 diapositives · 361 Views · Jul 21, 2014

This section explores the fundamentals of solutions in chemistry, detailing the two main components: solute and solvent. A solute is the lesser abundant substance dissolved in a solvent, which is the more abundant dissolving component. Solutions can be classified based on concentration levels, with terms like saturated and supersaturated describing how much solute the solvent can hold. Additionally, types of mixtures—solutions, suspensions, and colloids—are discussed alongside the Tyndall effect and the concept of hydrates, which are ionic compounds with water in their structure.

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  1. Solutions IB Chemistry: Chapter 1 Section 1.5

  2. What parts make up a solution? • Solution is a mixture of two components. • 1. Solute: less abundant component, the substance being dissolved • 2. Solvent: more abundant component, the dissolver • Solutions in water are called aqueous (aq).

  3. Concentration • As more and more solute gets dissolved, the solution becomes more concentrated. • When the solvent can no longer dissolve any more solute, it is saturated. (If less solute is dissolved, unsaturated.) • Solution can dissolve more solute than usual under particular circumstances – supersaturated.

  4. Molarity • Molarity is a term we use to describe concentration. • M = mol/dm3, Molarity = moles (n) of solute dissolved in 1 dm3 of solution. • What is the molarity of 2.98g of NaCO3 in 500cm3 of solution?

  5. Dilutions • Sometimes, we need a diluted solution for a particular procedure. • In order to dilute, you add water to a more concentrated solution. • The equation we use to determine how much concentrated solution we need is: • M1V1=M2V2

  6. Types of Mixtures • Classified by: • Size of the particles • Whether they exhibit the Tyndall effect

  7. Types of Mixtures • Solution: • Particles are evenly distributed and do not separate on standing • No Tyndall Effect • Example: food coloring and water mixture

  8. Solution Example Notice how you cannot see a distinction between solute and solvent. It is the same throughout the solution.

  9. Types of Mixtures • Suspensions: • Particles are not evenly distributed. Particles are suspended but will eventually settle into layers • Exhibits Tyndall Effect • Examples: Dirt and water mixture

  10. Suspensions The larger particles in a suspension settle out over time. Particles are only physically combined.

  11. Types of Mixtures • Colloids: • Particles are not evenly distributed. Particles are suspended but will eventually settle into layers • Exhibits Tyndall Effect • Examples: Dirt and water mixture

  12. Colloids Looks like a solution to the naked eye. Particles are suspended. The particle size is the “in betweener”, larger than a solutions’ particles but smaller than a suspensions’ particles.

  13. What is this “Tyndall effect”? • Light scattering by particles. • Found in colloids and suspensions, but not solutions.

  14. Tyndall Effect

  15. Hydrates • Hydrates are ionic compounds that have water molecules absorbed into the crystal lattice. • Hydrates are still solid, just have certain amounts of water attached to the ions. • An example of a hydrate is Copper (II) Sulfate pentahydrate: • CuSO4 ● 5H2O

  16. Hydrates • An example of a hydrate is: • CuSO4 5H2O • This means that for every 1 unit of copper sulfate, there are 5 units of water. • Or, for every 1 mole of copper sulfate there are 5 moles of water. • Solve for the molar mass. (The dot does not mean multiply, just add the mass of water to mass of copper sulfate.)