CHE 442G
Spring 2007
Course Outline: Section III

Chpt. 9	(Ideal) Solutions
	Measures of composition
	Ideal solutions (mi = i* + RT ln Xi) Raoult's Law: Pi = Xi Pi*; DHmix = DVmix = 0
	Ideally dilute solutions (mb = b° + RT ln Xb or mb = m,b° + RT ln mb) Henry's Law (Pb = Xb Kb or Pb = mb Km,b)
	Standard states

Chpt. 10	Nonideal Solutions
	Activities (mi = i° + RT ln ai = i° + RT ln gi Xi)
	Convention I (based on ideal solutions, Raoult's law) Convention II (based on ideally dilute solutions, Henry's law)
	Positive, negative deviations from Raoult's law (including molecular interpretation)
	Gibbs-Duhem equation
	Debye-Hueckel approach (including calculation of ionic strength)
	Davis equation for activity coefficients

Chpt. 11	Reaction Equilibrium in Nonideal Systems
	Standard states; use of activity coefficients
	Equilibria involving weak acids and weak bases
	Equilibria involving sparingly soluble electrolytes
	Reaction quotient (Q)

Chpt 12	Multicomponent Phase Equilibria
	Colligative properties (vapor-pressure lowering, boiling-point elevation, freezing-point depression, osmotic pressure)
	Two-component phase diagrams solution formation; regions of immiscibility; compound formation eutectic temperatures; peritectic temperatures
	Calculations of vapor pressures and vapor composition in equilbrium with a two-component liquid

Chpt. 14	Electrochemical Systems
	Electrical potentials
	Cell notation; types of electrodes; liquid junctions (and salt bridges)
	Ered° values and combinations thereof (to give cell potentials; to give Ered° values for a different half cells)
	E = -n F E ; Nernst equation [ E = E° - (RT / nF) ln Q ]
	Applications (determination of equilibrium constants and solubility products; DGf° values for ions, activity coefficients, and pH values)