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Unit 9

Unit 9. Solutions, Suspensions, + Colloids. Unit Objectives:. At the end of this unit, you will be able to: Define, describe, and compare the properties of solutions, suspensions and colloids. Describe the chemical process of dissolving.

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Unit 9

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  1. Unit 9 Solutions, Suspensions, + Colloids

  2. Unit Objectives: At the end of this unit, you will be able to: Define, describe, and compare the properties of solutions, suspensions and colloids. Describe the chemical process of dissolving. List factors that influence solubility and the rate of dissolving. Define and apply terms related to solubility, solutions and concentration of solutions.

  3. Use Solubility Curves (Table G) to determine saturation level and reagent needs for solution preparation. Predict the solubility of a solute in a given solvent based on the polarity of each. Predict changes in the solubility of solids in liquids and gases in liquids at different temps. Describe and apply six quantitative methods used to measure solution concentration. Calculate solution concentration, preparation, and solute mass basedon given concentration units.

  4. Calculate the molarity of a solution. Describe and predict the effect of a solute on the colligative properties of a solvent. Explain how the presence of an electrolyte affects solution conductivity. Use the Arrhenius Theory and the Modern Theory of Ionization to explain conductivity of a solution. Write dissosciation equations, ionic equations and net ionic equations.

  5. 1. What is a mixture? Two or more substances physically combined. Individual properties are retained.

  6. 2) 3 Categories of Matter • Elements • Compounds • Mixtures

  7. 4) 3 Categories of Mixtures • Solution – homogeneous mixture

  8. 4) 3 Categories of Mixtures • Suspension –heterogeneous mixture

  9. 4) 3 Categories of Mixtures • Colloid – heterogeneous mixture with permanently suspended particles

  10. 5) 5 Characteristics of Solutions • Will not settle out • Transparent • Can’t be filtered • Particles are molecules or ions • Homogenous

  11. 6) Solution Terminology • Solute – substance that is being dissolved • Solvent – substance that the solute is being dissolved in

  12. 6) Solution Terminology • Aqueous Solution – any solution where water is the solvent • Tincture – any solution where alcohol is the solvent

  13. 7) Ionic Solute in a Polar Solvent The permanent charges of the ionic solute are attracted to the charges of the polar solvent molecules and it dissolves.

  14. 8) Polar Solute in a Polar Solvent The charges of the polar solute are attracted to the charges of the polar solvent molecules and it dissolves.

  15. 9) Non-Polar Solute in a Polar Solvent The lack of charges on the non-polar solute results in no attraction for the charges of the polar solvent molecules and it does not dissolve.

  16. 10) N-P Solute in a N-P Solvent The lack of charges in both the n-p solute and the n-p solvent allow both to be close to each other it dissolves.

  17. 11) Polar Solute in a N-P Solvent The charges of the polar solute are not attracted to the n-p solvent due to lack of charges and it does not dissolve.

  18. 12) What does (aq) mean? Aqueous Solution – Water is the solvent

  19. 13) Why is water the universal solvent? Water will dissolve more substances than any other liquid.

  20. 15) 3 Examples of solid-solid mixtures • Soil • Concrete

  21. 16) 3 Examples of liquid-liquid mixtures • Crude oil • Gasoline • Oil & water

  22. 17) Why does gas-gas combo. Always make a mixture Both gases expand and diffuse to fill the container

  23. 18) 3 Examples of a gas-liquid mixture • Soda Pop • Seltzer Water • Club Soda

  24. 19) 3 Examples of a solid-liquid mixture • Salt Water • Mud • Hot Chocolate

  25. 20) 3 Factors that affect the rateof dissolving • Particle Size • Amount already dissolved • Stirring

  26. 21) 3 Factors that affectsolubility • Nature of solute and solvent • Temperature • Pressure

  27. 22) How does adding heat affect the solubility of a solid in a liquid? As heat is added, Solubility increases

  28. 22) WHY ? The liquid molecules spread out so more solid can fit into solution.

  29. 23) How does adding heat affect the solubility of a GAS in a liquid? As heat is added, solubility of the gas decreases.

  30. 23) WHY ? The gas particles move too fast and cannot be held in solution.

  31. 24) What effect does the addition of pressure have on the solubility of a solid in a liquid ? None

  32. 25) What effect does the addition of pressure have on the solubility of a gas in a liquid ? As pressure  gas solubility  *Direct relationship*

  33. 26) Why do bubbles escape when the cap is removed ? When cap is opened, pressure is released. As pressure , solubility of gas .

  34. 27) What does effervescence mean? The rapid escape of a gas from a solution in which it is dissolved.

  35. 28) Terminology: Solubility The amount of solute that can dissolve in a solvent at given conditions.

  36. Note in Margin Soln. = solution

  37. 29) Terminology: Dilute A soln. where the amount of solute is small compared to solvent.

  38. 29) Terminology: Concentrated A soln. where the amount of solute is large compared to solvent.

  39. 29) Terminology: Saturated A soln. that has dissolved all the solute that it can at given conditions.

  40. 29) Terminology: Unsaturated A soln. that has not dissolved all the solute that it can at given conditions.

  41. 29) Terminology: Supersaturated A soln. containing more solute than a saturated soln. at the same conditions. (Unstable)

  42. 30) What is a Solubility Curve ? A graph of the relationship between solubility and temperature. See Reference Table G

  43. 31) Refer to Reference Table GSolubility Curves

  44. 32) Under what conditions will gases have maximum solubility in a liquid? • Low temp. • High Pressure

  45. 33) Why are dilute and concentrated inadequate terms? They are too vague. i.e., how dilute ?

  46. 34) Why are saturated and unsaturated inadequate terms? Saturation level is temp. dependent.

  47. 35) 6 Quantitative Methods to Express Concentration • Percent by Mass • Percent by Volume • Molarity (M)

  48. 35) 6 Quantitative Methods to Express Concentration • Molality (m) • Mole Fraction • Parts per Million (ppm)

  49. 36) What does % by massand% by volume mean? % by mass is used for solids dissolved in liquids % by volume is used for liquids dissolved in liquids

  50. 38) Define Molarity? Moles of solute per liter of solution. (Note: not per liter of solvent).

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