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Mixtures

Mixtures. 3 Types based on particle size suspensions colloids solutions Relate to particle size 9 types solutions based on phase sol/liq liq/liq gas/liq sol/sol liq/sol gas/sol sol/gas liq/gas gas/gas. Terms of Solutions. solvent/solute separation of solution components

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Mixtures

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  1. Mixtures • 3 Types based on particle sizesuspensions colloids solutionsRelate to particle size • 9 types solutions based on phasesol/liq liq/liq gas/liqsol/sol liq/sol gas/sol sol/gas liq/gas gas/gas

  2. Terms of Solutions • solvent/solute • separation of solution components • filtration • chromatography • distillation • concentrated/dilute • saturatedunsaturated supersaturated know definitions

  3. Solubility • How much solute will dissolve into 100 g of solvent (usually water)

  4. Solubility Terms • soluble/insoluble • miscible/immiscible • like dissolves like • The more alike the IMF's holding 2 substances are, the more likely they will dissolve in each other • relates to imf’s • polar/nonpolar

  5. Insolubility • “Like dissolves like” • The more alike the IMFs holding 2 substances are, the more likely they will dissolve in each other • Water dipoles dissolve ionic and polar compounds • All have charged areas • Water won't dissolved nonpolar compounds

  6. Solids in Liquids • How much solute will dissolve into 100 g of solvent (usually water) • Effects of temp on solubility solids in H2O • Temp solubility • Direct relationship • Gases behave in the opposite way • Temp solubility • Inverse relationship

  7. Gases in Liquids • Henry's Law: Gas Press and Solubility • press solubility • direct relationship • Gas Temp and Solubility • Temp solubility • inverse relationship

  8. Concentration units • mass % = g solute x 100 g sol'n • molarity = M = mol solute L sol'n • molality = m = mol solute Kg solv

  9. aq solution conducts e- current1 - charged particles 2 – mobility of charges ionic compounds (SALTS)are electrolytes if they dissolve in H2O dissociate into ions NaCl(s) --> Na+(aq) + Cl-(aq) Electrolytes

  10. Nonelectrolytes • Molecular compounds • Dissolve as whole neutral molecules C6H12O6(s) --> C6H12O6(aq) • No ions formed • Acids are the exception • Molecular electrolytes • They produce ions in water solution • ionize HCl (g) --> H+(aq) + Cl-(aq)

  11. Strong vs Weak Electrolytes • Based on percent ionization • Strong electrolyte dissociate completely 1000 0 0 • HCl(g) H+(aq) + Cl-(aq)100% ionization 0 1000 1000 1000 0 0 • CH3COOH(g) H+(aq) + CH3COO-(aq) 995 5 5 Dbl arrow?

  12. Heats of solutions • 2 factors at work • 1- breaking bonds of the solute • endothermic • requires energy • 2- Forming bonds between H2O dipoles and solute • exothermic • gives off energy • Overall solution process can be endo or exo

  13. Colligative properties • depend on # solute particles in sol'n • based on molality – m • m = mol solute Kg solvent • freezing pt depression • Dtf = kf x m kf = 1.86°C/m • boiling pt elevation • Dtb = kb x m kb = 0.52°C/m • osmotic pressure

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