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Understanding Solutions: Types, Properties, and Key Theories

This comprehensive overview explores the essential concepts of solutions, including homogeneous and heterogeneous mixtures, the differences between dissolving and melting, and key theories such as "like dissolves like." Learn about various types of solutions, suspensions, colloids, and emulsions, alongside factors influencing solution formation. We also cover concentration units such as molarity and molality, alongside colligative properties like boiling point elevation and freezing point depression. Gain insights into vapor pressure lowering and osmotic pressure's significance in solution chemistry.

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Understanding Solutions: Types, Properties, and Key Theories

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  1. Solutions – Web Site Presentations • Homogeneous vs. heterogeneous • Dissolving vs. melting

  2. Theory of Solutions • 9 solute-solvent combinations • Solutions, suspensions, colloids, emulsions

  3. Theory of Solutions • Dilute, concentrated, unsaturated, saturated, and supersaturated • 4 factors affecting solution formation

  4. Theory of Solutions • Separating solutions into their components • Like dissolves like

  5. Theory of Solutions • Relationship of equilibrium and solubility • Gases are less soluble in liquids at higher temperatures • Why do precipitates form?

  6. Concentration units • Calculating Molarity (M=moles solute/liter solution) • Molality (m=moles solute/kg solvent) Added info! • Mole fraction (XA=mol A/mol total ) • Dilutions (M1V1=M2V2)

  7. Colligative Properties • Properties that depend upon the number of solute particles present but NOT their type • Vapor Pressure Lowering • Boiling Point Elevation • Freezing Point Depression • Osmotic Pressure • Note: 1 mole of sugar dissolved in 1 kg of water will produce 1m sugar solution, but 1 mole of NaCl dissolved in 1kg of water will produce 2 moles of dissolved particles! This is why 1 mole of CaCl2 will lower the freezing point of water more than 1 mole of NaCl

  8. Colligative Properties • Explain Boiling Point Elevation • ∆Tb=iKbm     • Explain Freezing Point Depression • ∆Tf=iKfm 

  9. Osmotic Pressure / Vapor Pressure Lowering • External pressure which must be applied to stop osmosis • The greater the # particles in solution, the greater the osmotic pressure • π=iMRT     where i is the number of dissolved particles, M is molarity, R is the gas constant, and T is the Kelvin Temperature • Vapor pressure is less when solute particles are present because they interfere with the evaporating process • Psoln=XaPa + …..   Where “a” refers to a liquid because you can only have vapor pressure over a liquid

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