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Solution Chemistry

Solution Chemistry. Recall that a Solution:. Is a homogeneous mixture that forms when one substance disperses uniformly throughout another. Recall that a Solution:. may be any phase: Solid  solids evenly spread throughout Liquid  liquid solvent with gas, solid, or liquid dissolved in it

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Solution Chemistry

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  1. Solution Chemistry

  2. Recall that a Solution: • Is a homogeneous mixture that forms when one substance disperses uniformly throughout another.

  3. Recall that a Solution: • may be any phase: Solid solids evenly spread throughout Liquid liquid solvent with gas, solid, or liquid dissolved in it Gas gases or vapors dissolved in one another

  4. Recall that a Solution: • Does not settle on standing and will pass directly through a filter

  5. Physical vs. Chemical Solutions • Physical solutions are the result of physical changes, and therefore can be separated physically. • Chemical solutions are the result of chemical reactions, and therefore cannot be separated by physical separation.

  6. Solution Composition • Solute: Substance being dissolved, may be solid, liquid, or gas • Solvent: The dissolving medium, will be present in greater quantity. If the solvent is water  aqueous If the solvent is alcohol  tincture

  7. Practice • For each of the following solutions, determine the solute and the solvent. • 20.0g of H2O & 35.0g of alcohol • 15.5g of alcohol & 2.5g of I2 • 0.002g of O2 & 200.5g of H2O

  8. Solvation or Hydration NaCl(s) + H2O Na+(aq) + Cl-(aq)

  9. Energy Involved with Solvation

  10. Ionic Compounds in Water • Ionic compounds dissociate in water so that each ion separates from the solid structure and disperses throughout the solution.

  11. Electrolytes • A substance whose aqueous solution contains ions, and therefore can conduct electricity

  12. Molecules in Water • Molecules can dissolve in water if there are complementary intermolecular forces; however, the molecules remain intact rather than dissociating into ions.

  13. Nonelectrolytes • A substance that does not form ions in a solution.

  14. Solubility • The amount of substance that can be dissolved in a given quantity of solvent at a specific temperature

  15. Solution Equilibrium • Solute + Solvent dissolve Solution • Solute + Solvent crystallize Solution Solute + Solvent  Solution

  16. Saturation • Which one is saturated? • Regardless of saturation, all solutions will be clear and homogeneous!

  17. Saturation • Saturated Solutions: Have the maximum amount of solute dissolved in them. No more solute can dissolve. Will be at equilibrium with undissolved solute. • Unsaturated Solutions: Have less than the maximum amount of solute dissolve in them. • Supersaturated Solutions: Have more than the maximum amount of solute dissolved in them This is not normally possible. If a crystal is added to a supersaturated solution, precipitation of all the extra solute will occur.

  18. Saturation

  19. Creating Supersaturated Solutions

  20. Factors Affecting Solubility Solute-Solvent Interactions Soluble Insoluble Insoluble Soluble Insoluble Soluble

  21. Alcohol Solubility Alcohol: hydroxyl group on a carbon chain Alcohol solubility *The greater the number of OH groups, the more water soluble. *The longer the carbon chain, the more organic-solvent soluble.

  22. Gas Solubility • Kr (84 amu), N2(28 amu), CO (28 amu), O2 (32 amu), Ar (40 amu) From slide 139, Unit 5 PPT: • When the molecules of two substances have comparable molecular weights and shapes, dispersion forces will be approximately equal. In this case, the more polar molecules will have the greater attractive forces. • When the molecules of two substances differ widely in molecular weights, dispersion forces tend to be decisive in determining which substance has the stronger intermolecular attractions. In this case, The larger the molecule, the greater the attractive forces. • N2, CO, O2, Ar, Kr

  23. Factors Affecting Solubility Pressure

  24. Temperature

  25. Solubility Curve

  26. Solubility Rules

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