• we need to consider solubility of substances
  • heterogeneous mixture
    • consists of two or more phases e.g oil and water, sand and water
  • homogenous mixture
    • solution (heterogeneous mixture is NOT a solution)
  • decanting
  • filtration
    • depends on size of particles
    • funnel will utilise gravity to filter out the mixture.
    • residue: material left on the filter paper (in our case sand)
      • the residue left will most likely not be pure
      • there will be water on the sand
        • distilled water will take out sodium chloride in the residue.
  • evaporation
    • using evaporating basin (made of porcelain and has a particular shape), to evaporate the

solubility

solute, solvent and solution

  • solute: substance that is dissolved
  • residue: substance that is left that cannot be dissolved
  • precipitate: substances that are formed in a reaction when two solutions form together.
  • solvent is the thing solute is dissolved with.
  • solution is the homogeneous mixture of solute dissolved in solvent.
    • process of forming solutions involves breaking the bonds and attractions
    • this requires energy which is an endothermic process

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  • ion-dipole attraction
    • attraction between an ion and a dipole dipole attracted molecule.
  • attractions forming between the solvent and solute
    • so the bond is an exothermic process
  • whether the solution forms depends on if the process requires too much energy to be favourable.
  • dissolving can be endothermic or exothermic

why substances dissolve

  • polarity of solvent matters.
  • highly polar solvent dissolves only substances that has some sort of charge.
  • if its an ionic compound dissolved in water, ion-dipole attraction will occur.
  • water is more polar than ethanol
    • ethanol cannot dissolve sodium chloride, as forces of attraction that is formed between ions and ethanol molecules is not strong enough to overcome ionic bonds between ions in sodium chloride.
  • non-polar solvents
    • cyclohexane
    • benzene
    • these non-polar solvents can only dissolve non-polar substances
  • water is the universal solvent
    • water is great at dissolving polar molecules substances and many ionic substances.
    • water can form a great range of intermolecular forces to stabilise solution:
      • dipole
      • hydrogen bonds
      • ion-dipole bonds