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Solutions

This comprehensive overview of the solution process details how solute dissolves in solvent, examining intermolecular attractions and energy changes involved. It explores the differences between physical and chemical changes during dissolution, emphasizing key concepts like "like dissolves like" and factors affecting solubility such as temperature and pressure. The piece also covers the steps of solvation, hydration of ionic solids, and the principles of Henry’s Law, providing insights into the behavior of gases and solids in solutions.

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Solutions

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Presentation Transcript

  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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