Jonathan Versino
Peter Lansky
Unit 2 Equilibrium and Ksp
AxBy (s)  xAy+ (aq) + yBx- (aq)
-Equilibrium constant = K = [Ay+]x[Bx-]y / [AB]
-Solubility product constant = Ksp = [Ay+]x [Bx-]y
Le Chatelier’s principal – “a change in any of the factors that determine the
equilibrium conditions of a system will cause the system to change in such a manner as
to reduce or counteract the effect of the change.”
Reaction Quotient = Q = [products] / [reactants]
Q is used for a chemical reaction that is doesn’t have to be at equilibrium.
If Q < Ksp then reactants will be converted to products.
If Q = Ksp the system is at equilibrium.
If Q > Ksp some products will be converted to reactants
Common ion effect – When excess ions are added to the equilibrium it will lower the
salt solubility.
-10
If, Ksp = [Ag+][Cl-] = 2.5x10
Then, (x)(x) = 2.5x10-10
Then, x = [Ag+] = [Cl-] = 1.6x10-5
So,if 0.10 mol of NaCl is added to 1 L of the AgCl solution
Then, [Ag+] [0.1M] = 2.5x10-10
And [Ag+] = 2.5x1-9
Solubility rules
-Almost all salts of Na+, K+, andNH4+
-All salts of Cl-, Br-, and I-  except Halides of Ag+, Hg22+, and Pb2+
-Compounds containing F-  except Fluorides of Mg2+, Ca2+, Sr2+, Ba2+, Pb2+
-Salts of NO3-, ClO3-, ClO4-, CH3CO2-Salts of SO42Colligative Properties
-The properties of a solution that are dependant only on the number of solute
particles per solvent molecule
-Molality = moles of solute/kilogram of solvent
Freezing Point Depression
-Freezing point of a solution is lowered with the addition of a solute, usually quite
small
∆Tf =Kfm
∆Tf = freezing point depression; m=molality, Kf=molal freezing point
constant
Boiling Point Elevation
-Adding a solute to a solution increases the temperature at which it boils
∆Tb =Kbm
Metallic and Ionic Solids Structure
-Simple Cubic
• 1 net atom per unit cell
• Cell edge = 2r
-Body Centered Cubic
• 2 atom per unit cell
• Cell diagonal = 4r = (√3)(Length of Edge)
-Face Centered Cubic
• 4 net atoms per unit cell
• Cell diagonal = (√2)(length of edge)