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Solutions

Solutions. IB Chemistry: Chapter 1 Section 1.5. 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 ).

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Solutions

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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.)

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