1Bond strength is
inversly related to acid strength
2Two main factors that affect bond strenagth in a binary acid
1. size of anion 2. the electronegativity of the envionment around the H atom
3Anion size
the smaller aniona allow for better orbital overlap with the 1s orbitals of hydrigen atoms & stronger bonds
4electonegativity w/ the context of bond strength
if the bond to a hydrgen atom is higly polar, the more ionizable it is
5Acid strentgh increases when
more oxygens are added to oxyacids
6electronegtativity increases as you move
right on th peroidic table
7Lewis base
electron pair donot
8lewis acid
electron pair acceptor
9bronstead acids react with bronstead bases to produce
sallt and water
10lewis acid react with lewis base to create
a single compound resulting from a synthesis reaction
11Common Ion effect
When a compound containing a conjgate base of an acid is added to a reaction at equilibrium resulting in a shift to restore equilibirum
12buffer
a solution containing a weak acid its conjugate base that resistes pH change
14henderson hasselbalch
pH= pKA +Log(A/HA)
15When {A} > {HA}
ratio of A/HA>1 pH> pKa
16when [HA] >[A]
ratio A/HA <1 Ph< pKA
18effectiveness of a buffer is affected by
buffer capcity and effectve pH range
19Buffer Capcity
ability of buffer to resist a change inpH when a acid or base is added. dependent on reactant concentrations.
20effective pH range
W/ in 1 pH unit og the pKa of the Buffer’s conjugate acid