1. Principles of Reactivity: Other Aspects of Aqueous Equilibria
Chapter 18 || v
Principles of Reactivity: Other Aspects of Aqueous Equilibria

2. Common Ion Effect
•The limiting of the ionization of an acid or base by the presence of a significant concentration of its conjugate
The extent to which the acid can ionize is affected, affecting pH

3. Buffer solutions
•Buffer solutions cause resistance to change in pH when a strong acid or base is added.
•Prepared from a conjugate acid-base pair
•pH= pK a+ log([conjugate base]/[acid])
•Requirements:
•the acid and base must not react with one another
•Acids capable of reacting with OH- ions
•base that can consume added H3O+ ions
Dank memes | v

4. Acid base titrations
The equivalence point is the midpoint of the vertical segment of the pH vs volume of titrant curve.
pH at the equivalence point in a strong acid/strong base is 7
More memes→
<--- Actual science stuff

5. Solubility of salts
Precipitation reactions have a product which is a water-insoluble compound
Equilibrium constant reflects the solubility of a compound referred to as its solubility product constant Ksp
The solubility of a salt is the amount present in some volume of saturated solution. The Ksp is an equilibrium constant
(SALT)

6. Precipitation Reactions
The Q (reaction quotient) and K (equilibrium constant) may or may not be at equilibrium
-If Q=Ksp the solution is saturated
-If Q<Ksp the solution is not saturated
-If Q>Ksp the solution is over(super) saturated
(precipitation→)

7. Solubility and complex ions
Metal ions exist in aqueous solutions as complex ions
Equilibrium constant for formation of complex ions is called formation constant, Kform
Knet=KspKform

8. Henderson Hasselbalch
pH=pKa+log(base/acid)
Determines the pH range of a buffered solution
Uses the acid dissipation constant by: Ka=[H+][A-]/[HA]
Rearranged as: [H+]=Ka[HA]/[A-]
Then take the -log of the expression and rearrange in order to make each figure positive

9. Assignment:
Page : 7, 8, 25, 29, 33, 53