Nernst Equation
Ecell=E�cell- (RT/nF) (lnQ)
Gibbs Free Energy (in relation to EMF)
?G=-nFEcell
Standard Electromotive Force
EMF=E�reduction-E�oxidation
Standard Conditions
25� C, 1 atm Pressure, 1 M concentrations, most stable form of each compound
Faraday's Constant
1 F=96487 J/V
Henderson-Hasselbach Equation
pH=pKa + log [conj. Base]/[weak acid]
Relation Between base and acid dissociation constants
Ka * Kb = Kw= 1E-14
Base dissociation Constant
Kb= [B?]*[OH?]/[BOH]
Acid dissociation constant
Ka=[H3O?]*[A?]/[HA]
Water dissociation constant
Kw=[H?]*[OH?]=1E-14; pH + pOH=14
pH
pH=-log([H?])=log(1/[H?])
Boyle's Law
P?V?=P?V?
Charles' Law
V?/T?=V?/T?
Avagadro's Principle
n?/V?=n?/V?
Ideal Gas Law
PV=nRT
Ideal Gas Constant
0.0821 L
atm/mol
k or 8.314 J/mol*K
Dalton's Law of Partial Pressures
P(total)=Pa+Pb+Pc+...
Pa=Xa*P(total)
Root Mean Square Speed
uRMS=?(3RT/MM), MM=molec mass
Graham's Law of Diffusion/Effusion
r1/r2=?(MM2/MM1)
Freezing Point Depression
?Tf=Kf*m; m=molality (moles/kg), Kf=freezing constant for solvent
Boiling point elevation
?Tb=Kb*m; m=molality (moles/kg), Kb= boiling constant for solven
Osmotic Pressure
?=MRT; M=molarity (moles/L)
Raoult's Law
?P=Xb
P�a; Pa=Xa
a*P�a, where P�a is the vapor pressure of pure a, Xa is the mole fraction of a.
Dilution
M?V?=M?V?
Heat absorbed or released
q=mc?T; where m is mass and c is specific heat
Enthalpy change
?Hreaction=Hproducts-Hreactants; where positive, endothermic rxn, negative, exothermic
Entropy change
?S=Sfinal-Sinitial; where positive, disorder increases, negative, order increases
Gibbs Free Energy
?G=?H-T?S, must be negative to be spontaneous