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Solubility

Solubility. Today’s class:. Solubility Saturation. Separation of mixtures. unsaturated solution. saturated solution. remaining undissolved solute. precipitate. Practice solubility / saturated solution. Solubility :.

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Solubility

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  1. Solubility

  2. Today’s class: Solubility Saturation Separation of mixtures

  3. unsaturated solution saturated solution remaining undissolved solute precipitate

  4. Practice solubility / saturated solution Solubility: Maximum concentration of a solute that can be attained in given solvent. Maximum amount of solute that can be dissolved in a given amount of solvent. Saturated Solution: Contains maximum amount of solute that can be dissolved. Unsaturated Solution: More solute can be dissolved in the solution. Supersaturated Solution: An extra amount of solute was dissolved; solution “wants” to precipitate some solute

  5. 2.65 g of a solute is dissolved in 70.0 mL of water to produce a saturated solution at 20 oC. Calculate the solubility in units of g/100 mL; g/L. msolute = 1.) in g/100ml = % m/v 100 mL vsolution m = 2.65 g 2.65 g = 100 mL 70 ml v = 70 ml g/100ml = ? 2.65 g = 100 mL 70 ml 3.79 g = The solubility is 3.79 g /100 mL

  6. 2.65 g of a solute is dissolved in 70.0 mL of water to produce a saturated solution at 20 oC. Calculate the solubility in units of g/100 mL; g/L. msolute = c 2.) in g/L vsolution m = 2.65 g 2.65 g = c v = 70 mL = 37.9 g/L 0.07 L = 0.07 L c = ? g/L The solubility is 37.9 g /L

  7. Example 2 4.5 g is the maximum amount of a solute that can be dissolved in 200 mL of water at 20 oC. Calculate the solubility in units of g/100 mL; g/L.

  8. Effect of temperature on solubility • How to make a supersaturated solution For most salts: The warmer the water the more salt dissolves 1.) make a saturated solution at high temperature 2.) let hot, saturated solution cool  supersaturated 3.) eventually excess solute will PRECIPATE (form new crystals)

  9. solubility (g/100 ml of water) For most solids solubility increases with temperature Temperature °C

  10. Solubility of gases and temperature Air bubbles forming, before the water starts to boil The warmer the water the less Oxygen / CO2 can be dissolved

  11. Solubility of most gasesdecreases with temperature  When oceans warm up, less CO2 can be dissolved – CO2 is released

  12. Solubility and solvent ? salt • salt is soluble in water • salt is not soluble in oil Solubility of a substance depends on the nature of the solvent

  13. Substances that are soluble in water are called hydrophilic • Substances that are soluble in oil are called lipophilic • Soap has a hydrophilic and a lipophilic part and can help oily substances dissolve in water.

  14. Solubility Saturation Separation of mixtures

  15. Separating mixtures Most substances are not found in their pure form in nature but need to be isolated from a mixture.

  16. Separating solid and liquid- a difference in state of matter • Filtration

  17. A difference in density I Example: Pouring water off rice / pasta (without using a strainer). • Decantation oil water

  18. A difference in density II Example: Centrifugation of blood samples • Centrifugation Accelerates and improves sorting by density  dense material collects at the bottom

  19. A difference in speed of travel • Chromatography • Mixture is separated into its components using paper and a solvent. • The different components of the mixture are transported by the solvent along the paper, but with different speeds.

  20. Isolating a solute - evaporation The liquid solvent is evaporated, leaving behind the solid solvent Example: Harvesting of sea salt form the ocean.

  21. A difference in boiling point Example: Distilling wine to make brandy. • Distillation

  22. Notes on separating mixtures

  23. Homework • Solubility: work book p. 8 # 4, 5 p. 10 # 9 • Separating mixtures p. 12

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