Acids and Bases Flashcards
1
Q
Arrhenius definition
A
- acid produces H+ in an aqueous solution
- base produces OH- in an aqueous solution
2
Q
Bronsted-Lowry definition
A
- acid donates protons
- base accepts protons
3
Q
Lewis definition
A
- acid is an electron-pair acceptor
- base is an electron-pair donor
4
Q
pH
A
- hydrogen ion concentration
- pH = -log [H+] = log (1/[H+])
5
Q
pOH
A
- hydroxide ion concentration
- pOH = -log [OH-] = log (1/[OH-])
6
Q
Kw
A
- water dissociation constant
- Kw = [H+] [OH-] = 10^ -14
- pH + pOH = 14
- Ka x Kb
7
Q
Ka
A
- acid dissociation constant
- Ka = ([H+][A-])/[HA]
8
Q
Kb
A
- base dissociation constant
- Kb = ([B+][OH-])/[BOH]
9
Q
buffer solution
A
- mixture of a weak acid and its salt (which consists of its conjugate base and a cation) or a mixture of a weak base and its salt (which consists of its conjugate acid and an anion
- resist changes in pH when small amounts of acid or base are added
10
Q
amphoteric
A
can act as an acid or a base
11
Q
titration
A
the addition of a solution of known concentration and volume to another solution to determine its unknown concentration
12
Q
equivalence point
A
MV = MV
