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Solutions

Solutions. Part I: The Solution Process. Solution:. Solutions:. Solute: Solvent. Types of Solutions. The solution process.

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Solutions

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  1. Solutions Part I: The Solution Process

  2. Solution:

  3. Solutions: • Solute: • Solvent

  4. Types of Solutions

  5. The solution process • To dissolve a solute in a solvent, the intermolecular attractions between solute and solute must be strong enough to compete with solvent-solvent and solute-solute attractions.

  6. Solvation

  7. Hydration

  8. Dissolving an ionic solid in water • The ion-dipole attractions between the salt and the solvent must be strong enough to overcome the lattice energy

  9. “Steps” of the solution process • Step 1

  10. “Steps” of the solution process • Step 1 • Step 2

  11. “Steps” of the solution process • Step 1 • Step 2 • Step 3

  12. Endothermic vs. exothermic?

  13. Why do processes occur? • Achieve a lower energy state • Exothermic processes lead to lower enthalpy

  14. Why do processes occur? • More randomness • Greater “entropy” • Can more than compensate for increasing enthalpy

  15. Did it dissolve, or did it react? • Just because a substance “disappears” into a solvent doesn’t mean that the substance dissolved!

  16. Dissolving vs. reaction • Dissolving • Physical change • Can recover the original substance by evaporating the solvent

  17. Dissolving vs. reaction • Dissolving • Physical change • Can recover the original substance by evaporating the solvent • Chemical change • New substances form

  18. saturated unsaturated Solutions

  19. Supersaturated solutions

  20. Will this substance dissolve?

  21. “Like dissolves like” • Non-polar substances tend to dissolve in non-polar solvents

  22. “Like dissolves like” • Non-polar substances tend to dissolve in non-polar solvents • Polar substances tend to dissolve in polar solvents.

  23. “Like dissolves like” • It comes down to having similar intermolecular attractions.

  24. Gases in solution • Solubility depends on intermolecular attractions

  25. Gases in solution • Solubility depends on intermolecular attractions • London forces • As molar mass increases, dispersion forces are stronger

  26. Henry’s Law • The solubility of a gas in a liquid is directly dependent on the gas pressure

  27. Henry’s Law • The solubility of a gas in a liquid is directly dependent on the gas pressure • Pressure really doesn’t affect solubility of solids and liquids

  28. Henry’s Law • Sg = kPg

  29. Solubility and temperature • Usually, solubility of ionic solids increases with temperature

  30. Gas solubility and temperature • Solubility of gases typically decreases with increasing temperature

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