There are two reasons why I have these here:
The textbook used is by Silberberg; Chemistry: The Molecular Nature of Matter and Change. (Mosby, 1996)
Lecture Notes: Tuesday 13th October, 1998.
COMPLEX ION EQUILIBRIA
Formation constant = Stability constant
Complex formation greatly increases the solubility of a metal salt, because it reduces [Mn+(aq)], the concentration of "free" metal ions in solution.
1. Calculate [Ag+] when 0.0005M AgNO3
is treated with 0.011M KCN.
Kf Ag(CN)2- = 5.56 * 10-18
2. Calculate [Ag+] when 0.010M AgNO3 is
treated with 0.80M NH3 solution.
Kf Ag(NH3)2+ = 107
Lecture Notes: Monday, 19th October, 1998.
Complex formation increases the solubility of sparingly soluble salts.
3. Calculate the solubility of AgBr in a) pure water and
b) 0.4M NH3 solution.
Ksp AgBr = 5.0 * 10-13
Kf Ag(NH3)2+ = 1.6 * 107
Oxidation and Reduction Reactions
Oxidising Agent (Oxidant):
reagent which causes another species to be oxidised; is reduced in doing so.
Reducing Agent (Reductant):
reagent which reduces another species; is oxidised in the process.
Redox Reaction involve changes in oxidation state.
OXIDATION STATE (NUMBERS)
Oxidation Numbers (ON) are a formalism, used to assist in assigning and balancing redox equations. (They do not really exist).
ON = charge on atoms if the compound was purely ionic (ie the electrons in covalent bonds go to the more electronegative atom.)
Rules for Assigning Oxidation Numbers are on page 155 of Silberberg (I refuse to type these stupid things out. Everyone knows them anyway.)