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Lecture5_S08

# Lecture5_S08 - Lecture 5 Final Colligative property is...

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Lecture 5 Final Colligativeproperty is osmotic pressure: Osmosis describes the net movement of pure solvent into solutions (with higher concentrations of impurities (solutes)) in order to maximize entropy and mixing. time Flow stops when solution can no longer fight gravity and atmospheric pressure Quantified by: π = i M RT Osmotic pressure (in atm) Temperature (K) Gas constant ( = 0.0821 L*atm/(K*mol)) Molarity(mol/L) van’tHoff constant For ideal solution of 3.4 g NaClin 1000 mLH 2 O @ 20 o C, calculate osmotic pressure. Example π = i M RT= i (mol NaCl) RT i = 2 for NaCl= Na + + Cl - T = 20oC = 293 K V soln = 1 L V soln (L) Mol NaCl= 3.4 g NaCl/58.44( g/mol) = 0.05818 mol π = 2(0.05818 mol)(0.0821 L*atm/K*mol)(293 K)/1L π = 2.8 atm

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Finding Molecular Weight using freezing point depression/boiling point elevation (Usually given mass solute, amount solvent, and freezing/boiling point) Δ T f = i K f m For molecular compounds i = 1, so Δ T f = K f m Keeping in mind units for molality(mol solute/kg solvent): Δ T f = K f m = K f * (mol solute/kg solvent)
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Lecture5_S08 - Lecture 5 Final Colligative property is...

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