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Solution

Solution. Homogeneous mixture in a single phase. Classification of Matter. Also called solutions. Also called suspensions. Solvent. Substance you have the most of. Substance that retains its phase. Dispersing medium. Solute. Substance you have the least of. Substance that dissolves.

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Solution

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  1. Solution Homogeneous mixture in a single phase.

  2. Classification of Matter Also called solutions Also called suspensions

  3. Solvent Substance you have the most of. Substance that retains its phase. Dispersing medium.

  4. Solute Substance you have the least of. Substance that dissolves.

  5. Dilute Solution Relatively small amount of solute.

  6. Concentrated Solution Relatively large amount of solute.

  7. Aqueous Solution Water is the solvent.

  8. NaCl(aq) Solution of NaCl dissolved in water!

  9. Soluble Capable of being dissolved.

  10. Solubility Maximum amount of 1 substance that will dissolve in a given amount of another substance.

  11. Factors that influence solubility Temperature for all systems & pressure for systems involving gases.

  12. Factors that influence the rate of dissolving. Temperature Stirring or agitation Surface Area of solute Amount of solute already present

  13. What kind of change is dissolving? Physical change

  14. How does a chemist represent the dissolving of a covalently bonded substance? C6H12O6(s)  C6H12O6(aq)

  15. How does a chemist represent the dissolving of an ionically bonded substance? NaCl(s)  Na+1(aq) + Cl-1(aq)

  16. What happens to an ionic substance when it dissolves? It separates into ions.

  17. What is the equation for the dissolving of CaBr2? CaBr2(s)  Ca+2(aq) + 2Br-1(aq)

  18. Molecule-Ion Attraction Interaction between water molecules and ions in solution.

  19. What kind of molecule is H2O? Polar – the O end is a bit negative & the H’s are a bit positive.

  20. Is the orange ion positive or negative & how do you know?

  21. Is the orange ion positive or negative & how do you know?

  22. Units of Solubility? Grams of solute per 100 grams of solvent

  23. What happens to the solubility of all gases as the temperature increases? The solubility of gases  as the temperature 

  24. What happens to the solubility of most solids as the temperature increases? The solubility of most solids  as the temperature .

  25. What do you need to conduct electricity? Mobile charged particles!

  26. Electrolyte? A substance that dissolves in water to produce a solution that conducts an electric current!

  27. Nonelectrolyte? A substance that dissolves in water to produce a solution that does not conduct an electric current!

  28. Saturated solution Contains the maximum amount of dissolved solute at that temperature.

  29. Supersaturated solution Contains more than the maximum amount of dissolved solute at that temperature.

  30. Unsaturated solution Contains less than the maximum amount of dissolved solute at that temperature.

  31. Precipitation The opposite of dissolving. A solid comes out of solution.

  32. Dynamic Equilibrium Term used to describe a saturated solution. Precipitation & dissolving are ocurring at the same rates. No net change.

  33. How do you test a solution for saturation? Throw a crystal of the solute into the solution & observe what happens.

  34. What are 3 possible outcomes of the saturation test? Crystal dissolves – Soln was unsaturated. No change in crystal – Soln was saturated. Crystal gets larger – Soln was supersaturated.

  35. What are 3 regions of a solubility curve? On the trace – saturated solution. Above the trace – supersaturated solution. Below the trace – unsaturated solution.

  36. Concentration A number that describes how much solute compared to how much solution or how much solvent.

  37. Percent Part over Whole X 100%

  38. Molarity (M) Liters of solution Molarity = # moles solute

  39. No. of Grams by F.M. X formula mass No. of Moles X 22.4 L/mol X 6.02 X 1023 • by 6.02 X 1023  by 22.4 No. of Particles No. of Liters Mole Map

  40. Parts per Million (PPM) grams solution PPM = grams solute X 1000000

  41. Problem: How much KCl will dissolve in 300 grams of water at 50C? Use the graph to set up a proportion. 42 g KCl = X g KCl 100 g H2O 300 g H2O X = 126 g KCl

  42. 88 g KNO3 in 100 g H2O at 50C. 20 g KNO3 in 100 g H2O at 10C. 88 g – 20 g = 68 g KNO3 precipitates. 50 to 10 - How much KNO3 precipitates?

  43. Measuring Heat of Solution Water is the environment! If Temperature of H2O , dissolving was exothermic. If temperature of H2O , dissolving was endothermic. source

  44. Factors affecting Solubility Temperature Pressure Nature of the Solvent & Solute

  45. Nature? Ionic Polar Covalent Nonpolar Covalent “Like Dissolves Like”

  46. MolarityC X VolumeC = MolarityD X VolumeD MC X VC = MD X VD Dilution Problems

  47. Colligative Property Depends on the concentration of the solute, NOT on the nature of the solute. Does not matter if ions or neutral particles are in solution.

  48. What are 2 colligative properties? Freezing Point Depression & Boiling Point Elevation

  49. Which solution has the most dissolved particles? 1 mole of C6H12O6 in 1 Liter H2O 1 mole of NaCl in 1 Liter H2O 1 mole of CaBr2 in 1 Liter H2O

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