2.  Usually consider solids (salts)  Dissolving in water – “like dissolves like” ◦ Forming aqueous solutions.  Remember pure liquids and solids are not part of K expressions  Solubility product constant = K sp ◦ equilibrium constant for solubility ◦ chart of K sp ’s page 761 MgF 2 (s) ⇄ Mg 2+ (aq) + 2F - (aq) K sp = [Mg 2+ ][F - ] 2

3.  May still need to do ICE calculations if do not know concentrations of species in reaction or if don’t know solubility of each ion.  Will be do Q to K comparisons to determine if a solid will form in from solution. ◦ Look at reaction equation ◦ May need a net ionic equation ◦ Consider solubility rules ◦ Q = ion product (just like Q from ch13)  If Q > K, precipitation occurs (shifts right)  If Q < K, no precipitation occurs (shifts left)

4.  Compare Ksp values to determine solubility or rank solubility.  Larger Ksp value = more soluble ◦ Breaks up fully into ions and wants to stay  Smaller Ksp value = less soluble  Solubility can be affected by pH ◦ Need to consider if conjugate acid or base  Or by addition of extra stuff (Le Chatelier’s Principle)

5.  Complex ion – a charged species consisting of a metal ion surrounded by ligands (a molecule or ion having a lone pair of electrons that can be donated) ◦ # ligands attached is called coordination # ◦ Occurs in a stepwise method – ligands are added 1 at a time  Equilibrium constant called formation constants or stability constants = K f ◦ K 1, K 2, etc – one for each step ◦ May need to determine one first, then use to find the others.

6.  To get overall complex ion formation equation, need to add all steps together.  If reactions are added, the K expressions are multiplied ◦ Kf = K 1 * K 2