Chemistry Reference
In-Depth Information
Ion Concentrations and Corresponding Values on the
pH and pOH Scales
[H
3
O
+
]
Value on pH Scale
[OH
-
]
Value on pOH Scale
1 × 10
-1
M
1
1 × 10
-14
M
14
1 × 10
-2
M
2
1 × 10
-13
M
13
1 × 10
-3
M
3
1 × 10
-12
M
12
1 × 10
-4
M
4
1 × 10
-11
M
11
1 × 10
-5
M
5
1 × 10
-10
M
10
1 × 10
-6
M
6
1 × 10
-9
M
9
1 × 10
-7
M
7
1 × 10
-8
M
8
1 × 10
-8
M
8
1 × 10
-7
M
7
1 × 10
-9
M
9
1 × 10
-6
M
6
1 × 10
-10
M
10
1 × 10
-5
M
5
1 × 10
-11
M
11
1 × 10
-4
M
4
1 × 10
-12
M
12
1 × 10
-3
M
3
1 × 10
-13
M
13
1 × 10
-2
M
2
1 × 10
-14
M
14
1 × 10
-1
M
1
Of course, this only works when the coefficient in the concentration of
ions is 1. If you have any other coefficient, as in [H
3
O
+
] = 4.3 × 10
-5
M, we
must use the pH formula, as shown here:
pH = -log[H
3
O
+
] = -log(4.3 × 10
-5
) = 4.4
One of the most interesting things about acids and bases is that they
can react with each other in such a way as to render each other harmless. A
neutralization reaction occurs when aqueous solutions of an acid and a base
react with each other to produce a salt (ionic compound) and water. The
general format for neutralization reaction is this:
acid + base
salt + water
