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Mixtures

Heterogeneous mixtures Components in different phases Homogeneous mixtures All components in same phase. Mixtures. Homogeneous mixture Most commonly a solid dissolved in a liquid Gaseous solutions air Solid solutions Alloys. Solutions. Dissolving process.

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Mixtures

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  1. Heterogeneous mixtures Components in different phases Homogeneous mixtures All components in same phase Mixtures

  2. Homogeneous mixture Most commonly a solid dissolved in a liquid Gaseous solutions air Solid solutions Alloys Solutions

  3. Dissolving process • Solute – the component that gets dissolved; the compound in the smaller amount • Solvent – the component that does the dissolving; the compound in the larger amount

  4. Dissociation – the process in which a solid dissolves in a liquid • Depends on polarity • Solvent usually water • Polar water molecules are attracted to other polar molecules and to ions • Non-polar molecules are attracted to other nonpolarmolecules

  5. Caroline Loves Ya’ll  • Hydration – water molecules surround the other molecules until the attraction between the water and the ion is stronger than the crystal

  6. Dissociation • Individual molecules or ions are pulled away from each other • Solvation – the surrounding of the solute particles • Once dissociation occurs the ions of the compound act independently

  7. Miscibility • Whether or not two liquids will form a solution • Miscible liquids are mutually soluble • Like dissolves like

  8. Factors that affect solubility • Temperature • Solids generally more soluble in liquids at higher temperature • Gases more soluble in liquids at lower temperatures

  9. Pressure • Henry’s law – at a given temperature, the solubility of a gas in a liquid is directly proportional to the pressure of the gas above the liquid • Nature of the solvent/solute • Polarity • Molecular size/structure

  10. Factors that affect rate of solution • Temperature • Agitation • Particle Size • Surface area • Concentration • Saturated • Unsaturated • Supersaturated

  11. Solubility Curves • Used to predict the conditions under which substances will form solutions

  12. At 0.0°C, which is more soluble, NaCl or KBr? • True or false, temperature has a significant effect on the solubility of NaCl. • Which of these dissolutions would have the highest value for heat of solution • What would be the approximate value of the heat of solution for NaCl?

  13. At what temperature will 140g of NaClO3 dissolve in 100g of water?

  14. Physical Properties Review • Properties that can be measured without changing the substance • Intrinsic properties • Properties that do not change when the amount of substance changes • Density, boiling point, freezing point • Extrinsic properties • Properties that change with a change in the amount of substance • Volume shape size

  15. Dissociation of solute particles • Ionic solute particles dissociate in solution and act independently • Covalent bonds are not usually broken in solution • So covalently bonded molecules will almost always be treated as one particle

  16. Concentration • Saturated • Contains the normal amount of solute • Unsaturated • Contains less than the normal amount of the solute • Supersaturated • Contains more solute than normal

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