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Solutions

Solutions. Mixtures. Combination of 2 or > substances Substances retain distinct identities Heterogeneous Components seen separately Homogeneous Composition same throughout mixture. Got Milk?. Definitions. Soluble: Capable of being dissolved

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Solutions

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  1. Solutions

  2. Mixtures Combination of 2 or > substances Substances retain distinct identities Heterogeneous Components seen separately Homogeneous Composition same throughout mixture
  3. Got Milk?
  4. Definitions Soluble: Capable of being dissolved Solution: Homogeneous mixture of two or more substances in a single phase. Solvent: Dissolving medium in a solution Usually present in a larger amount Solute: Substance dissolved in a solution Usually present in a smaller amount.
  5. Solute-Solvent Examples
  6. Suspensions Particles in a solvent are so large that they settle out unless constantly agitated. Muddy Water 
  7. Colloids Particles are intermediate in size Colloidal dispersions Tyndall Effect Brownian Motion
  8. Tyndall Effect
  9. Colloid Examples
  10. Colloid Examples Cont’d
  11. Classifying Solutes Electrolyte: Dissolves in H2O and conducts electricity NaCl, HCl Nonelectrolyte: Dissolves in H2O and gives solution that doesn’t conduct electricity Sugar
  12. Electrolytes/Nonelectrolytes
  13. Mixture vs. Colloid
  14. Filtrate
  15. Factors Affecting Rates of Dissolution Surface area of solute Molecules or ions attracted by solvent Occurs at surface of solute Crushing crystals Agitation of solution Concentration of solute highest at surface of solute Stirring disperses solute particles and brings fresh solvent particles in contact with solute
  16. Factors Cont’d Heating a Solvent Increase Temp : Increases KE of solvent molecules More collisions occur Higher energy collisions
  17. Solubility Solution Equilibrium Dissolution rate = Crystallization rate Saturated Solution Maximum amount of dissolved solute Unsaturated Solution Less than maximum amount of dissolved solute Supersaturated Solution More than maximum amount of dissolved solute

  18. Saturated Solution

  19. Supersaturated Solution
  20. Solubility Values Solubility: Maximum amount of solute that will dissolve in a given quantity of solvent at a specific temperature. g of solute / 100 g solvent g of solute / 100 mL solvent
  21. Solute-SolventInteractions Like dissolves Like Type of bonding Polarity or non-polarity of molecule IMF between solute and solvent
  22. Like Dissolves Like
  23. Polar Hydration: A solution process with water as the solvent. Ions are hydrated Hydrates: Crystalline compounds incorporate water molecules. CuSO4·5H2O
  24. Interactions Cont’d Nonpolar Solvents Nonpolar solutes Don’t dissolve ionic solutes Immiscible: Liquid Solutes/Solvents not soluble in each other. Miscible: Liquid Solutes/Solvents that are soluble in each other.
  25. Pressure Liquids Little effect on solids within a liquid Gases ↑ Pressure ↑Solubility within a liquid.
  26. Henry’s Law The solubility of a gas in a liquid is directly proportional to the partial pressure of that gas on the surface of the liquid. C = kP Gas/Liq solutions at constant Temperature Effervescence: Rapid escape of Gas
  27. Gas-Liquid Solubility and Temperature
  28. Solid-Liquid Solubilityand Temperature
  29. Heats of Solution Solvated: Solute particle is surrounded by solvent molecules. Heat of Solution: Amount of heat energy absorbed or released when a specific amount of solute dissolves in a solvent. Endothermic + (absorbs heat) Exothermic - (releases heat)
  30. Concentration of a Solution A measure of the amount of solute in a given amount of solvent or solution. Molarity = M M = (# moles of solute) / ( 1 L of solution) Molality = m m = (# moles of solute) / ( 1 kg of solvent)
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