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Nils Walter: Chem 260
Non-ideal solutionsStrong deviations from ideality are shown by dissimilar substances Raoult’s law
obeyed for a close-to-pure
solvent
William Henry(1775-1836)
observedHenry’s law (fora dilute solute):
pB = xBKB (e.g., gas solubility)
Nils Walter: Chem 260
Ideal and real solutions: ActivitiesFrom both Raoult’s (solvent) and
Henry’s laws (solute) follows:O
][ln)(ln)()(
solvCRTlxRTll
solv
solvsolvsolv
+=+=
µµµ
O
]ln[JRTJJ += µµ O⇒⇒⇒⇒
standard chemical potential @ 1 M
The chemical potential is a measure of the ability of J to bring about physical or
chemical change
BUT:
JJJ aRT ln+= µµ O
⇓⇓⇓⇓to
preserve equation for real
solutions:
Effective concentration = activity aJ = γγγγJ[J]
Nils Walter: Chem 260
Consequences of chemical potential changes in mixtures: Colligative properties
Boiling point elevation:∆∆∆∆TB = KBbB
Freezing point depression:∆∆∆∆Tf = KfbB
cryoscopic constantmolalitySolute is insoluble
in solid solvent:
Chemical Potential
lowered by solute
ebullioscopic constant
Solute is not volatile:
Chemical Potential
lowered by solute
Nils Walter: Chem 260
Phase diagrams of binary mixturesPhase rule: F = C - P + 2
for binary mixtures = 2p,T
p = constant:Temperature-composition diagram
for binary mixture of volatile liquids
in equilibrium
Nils Walter: Chem 260
Finally, as promised: Whisky distillery
Fractional distillation:High-boiling azeotrope,
e.g., nitric acid/water
Non-ideal mixtures
Low-boiling azeotrope, e.g., ethanol/water