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Standard 6: Solutions chapter 16

Standard 6: Solutions chapter 16. Chemistry Ms. Siddall. Aqueous solution Solvent Solute Solvation Electrolyte Solubility Solution. 8. Saturated solution 9. Unsaturated solution 10. Miscible 11. Immiscible 12. Concentration 13. Dilute solution 14. Concentrated solution

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Standard 6: Solutions chapter 16

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  1. Standard 6: Solutionschapter 16 Chemistry Ms. Siddall

  2. Aqueous solution Solvent Solute Solvation Electrolyte Solubility Solution 8. Saturated solution 9. Unsaturated solution 10. Miscible 11. Immiscible 12. Concentration 13. Dilute solution 14. Concentrated solution 15. Molarity vocabulary

  3. Standard 6a: solution definitions • Solution: a homogeneous mixture of 2 or more substances in the same physical state. • Properties: • Particles are small • Particles are evenly mixed • Particles will not separate • Examples: • air (nitrogen & oxygen) • Gatorade (water, sugar, etc) • NaCl(aq) (salt & water)

  4. Summary 1 • Is muddy water a solution? Why/why not?

  5. Solute: substance that is dissolved e.x. sugar • Solvent: does the dissolving e.x. water • Concentration: The amount of solute in a given amount of solvent e.x. [HCl] • (aq) = aqueous= A solution where water is the solvent

  6. Summary 2 Consider lemonade. • What is the solvent? • What are the solutes?

  7. Standard 6b: Dissolving Process • Solvent: H2O molecules with dipole • Solute: Ionic crystal lattice + + -

  8. Polar H2O molecules surround positive and negative ions and break apart crystal lattice Water molecules move away (diffusion) so the process is repeated Show animation

  9. Summary 3 Explain how water dissolves ionic compounds

  10. It takes energy to break bonds Energy needed to overcome lattice energy NaCl(s) Energy released during dissolving energy NaCl(aq) Dissolving

  11. Summary 4 Does the energy diagram for dissolving NaCl represent an endothermic or exothermic process? Explain your answer.

  12. Saturated solution: A solvent can not dissolve any more solute • A saturated solution is at equilibrium. Particles are dissolving and precipitating at the same rate • NaCl(s) Na+(aq) + Cl-(aq)

  13. Summary 5 Does the dissolving process stop at equilibrium? Explain why/why not.

  14. Standard 6c:Factors that affect the dissolving process • Some factors affect solubility (how much solute is dissolved) • Some factors affect rate (how fast solute is dissolved) • Some factors affect rateandsolubility

  15. Standard 6c:Factors that affect the dissolving process Factors affecting how much solute is dissolved 1. Type of solvent / solute • Polar solvents dissolve polar & ionic solutes • Non-polar solvents dissolve non-polar & covalent solutes e.x oil and water do not mix

  16. Summary 6 Is oil a polar compound or a non polar compound? How do you know?

  17. 2. Temperature • For solids: Temperature  solubility  Temperature increases kinetic energy of solvent particles therefore more solute can be dissolved • For gases: Temperature  solubility  Temperature increases the kinetic energy of solute particles therefore more particles escape from solution

  18. Summary 7 Why does the solubility of gas in solution decrease with increasing temperature?

  19. 3. Pressure (Gasses Only!) • Increasing pressure forces more gas into solution • Pressure  solubility  • Pressure  solubility  low pressure High pressure Gas air solution

  20. Summary 8 Does the concentration of carbon dioxide in your soda increase or decrease when you open the bottle? Why?

  21. Factors that affect the rate of solubility (how quickly something dissolves) 1. Temperature: • T rate • T rate • Increasing temperature increases kinetic energy = increased motion = increased diffusion

  22. 2. Surface Area (particle size): • S.A.  (particle size ) rate  • S.A.  (particle size ) rate  • Increasing surface area increases opportunity for interaction between solute and solvent

  23. 3. Stirring: • stirring  rate  • stirring rate  • Stirring increases particle motion so more particles can be dissolved at the surface of the solid

  24. Summary 9 • Name one factor that affects only solubility • Name one factor that affects only rate • Name one factor that affects rate and solubility

  25. Standard 6d: calculations • Molarity (mol/L) Molarity = Moles solute Liters solution • Grams per Liter (g/L) = Grams solute Liters solution • Percent Composition (%) grams solute x 100% grams solution • Parts Per Million (ppm) grams solute x 106 grams solution

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