Bronsted-Lowry (B-L) Acid/Base Table

Categories

Acid, HA

Base, A-

KaHA (pKa)

KbA- = Kw/KaHA (pKb)

 

HClO4

ClO4-

¥

~0

Strong Acids

HI

I-

¥

~0

Ka > 1

HBr

Br-

¥

~0

 

HCl

Cl-

¥

~0

 

H2SO4

HSO4-

¥

~0

 

HNO3

NO3-

22 (-1.3)

4.5 * 10-16 (15.3)

 

H3O+

H2O

1 (0)

1.0 * 10-14 (14)

 

HSO4-

SO42-

1.2 * 10-2 (1.9)

8.3 * 10-13 (12.1)

 

HClO2

ClO2-

1.2 * 10-2 (1.9)

8.3 * 10-13 (12.1)

 

H3PO4

H2PO4-

5.9 * 10-3 (2.2)

1.7 * 10-12 (11.8)

 

HF

F-

6.5 * 10-4 (3.2)

1.5 * 10-11 (10.8)

 

HNO2

NO2-

5.1 * 10-4 (3.3)

2.0 * 10-11 (10.7)

 

HCOOH

HCOO-

1.8 * 10-4 (3.7)

5.6 * 10-11 (10.3)

Weak Acids

CH3COOH

CH3COO-

1.8 * 10-5 (4.7)

5.6 * 10-10 (9.3)

Ka < 1

Al(H2O)63+

Al(H2O)5(OH)2+

1.4 * 10-5 (4.9)

7.1 * 10-10 (9.1)

 

NH3OH+

NH2OH

9 * 10-7 (6.0)

1.1 * 10-8 (8.0)

 

H2CO3

HCO3-

4.2 * 10-7 (6.4)

2.4 * 10-8 (7.6)

 

H2S

HS-

1.1 * 10-7 (7.0)

9.0 * 10-8 (7.0)

 

H2PO4-

HPO42-

6.3 * 10-8 (7.2)

1.6 * 10-7 (6.8)

 

HOCl

OCl-

3.5 * 10-8 (7.5)

2.9 * 10-7 (6.5)

 

NH4+

NH3

5.6 * 10-10 (9.3)

1.8 * 10-5 (4.7)

 

HCN

CN-

4.9 * 10-10 (9.3)

2.0 * 10-5 (4.7)

 

HCO3-

CO32-

4.7 * 10-11 (10.3)

2.1 * 10-4 (3.7)

 

CH3NH3+

CH3NH3

2.3 * 10-11 (10.6)

4.3 * 10-4 (3.4)

 

HPO42-

PO43-

4.8 * 10-13 (12.3)

2.1 * 10-2 (1.7)

 

H2O

OH-

1.0 * 10-14 (14)

1 (0)

 

NH3

NH2-

10-35 (35)

1021 (-21)

Very weak acids

H2

H-

2 * 10-38 (37.7)

5 * 1023 (-23.7)

Ka < 10-14

CH4

CH3-

?

 

 

OH-

O2-

?

 

Strong acids react completely with water.
Conjugate bases of strong acids are spectator ions
Strong bases react completely with water
An acid reacts completely with any base below it in the table
A base reacts completely with any acid above it in the table.
Very weak acids (and bases) do not react at all with H2O.
Ka(HA) * Kb(A-) = Kw = 10-14