CONJUGATE ACID-BASE PAIRS
Name________________________
Date__________________Per.____
In the exercise, Bronsted-Lowry Acids and Bases. it was shown that after an acid has given
up its proton, It is capable of getting back that proton and acting as a base.
Conjugate base is what is left after an acid gives up a proton.
The stronger the acid, the weaker the conjugate base.
The weaker the acid, the stronger the conjugate base.
Fill in the blanks in the table below.
CONJUGATE PAIRS
1.
2.
3.
Acid
Conjugate Base
H2SO4
HSO4-
(Sulfuric Acid)
HsSO4 ↔ H+ + HSO4Arrow (goes either way)
H3PO4
HF
FAdd H+
NO3-
4.
5.
H2PO4-
6.
H2O
SO4-2
7.
8.
HPO4+
9.
HN4-
10.
Gives away 1 H+
Equation
H2O
HF ↔ H+ + F-
(F with –1 remains)
Name _____________________
Date _____________Per ______
BRONSTED - LOWRY
ACIDS AND BASES
According to Bronsted-Lowry theory, an acid is a proton (H+) donor, and a base is a proton
acceptor.
H+
Example:
HCI + OH- → Cl- + H2O
Acid give away H+
The HCI acts as an acid, the OH as a base
H2O (acid)
This reaction is reversible in that the H2O
Cl- (base)
can give back the proton to the Cl
Label the Bronsted-Lowry acids and bases in the following reactions and show the direction of
proton transfer.
H+
H-
H2O gave H(Acid)
+
Cl picks up H (Base)
[now conjugate Acid]
Example: H2O + Cl- ↔ OH- + HCl
Acid
Base
C. Base C. Acid
1. H20 + H20
Acid
↔
Base
H3O+
C. Acid
+ OHC. Base
2.
H2S04 + OH-
↔ HSO4 - + H2O+
3.
HSO4 - + H2O
↔ SO4-2 + H3O+
4.
OH- + H3O+
↔
H2O + H20
5.
NH3 + H2O
↔
NH4+ + OH-
0
