The pH is the negative logarithm of the hydrogen ion concentration

**pH CALCULATION**

The pH is the negative
logarithm of the hydrogen ion concentration

**pH
= –log _{10} [H^{+}]**

**Example: **Calculate the pH of 0.01
M HNO_{3}?

[H^{+}] = 0.01

pH = –log_{10}
[H^{+}]

pH = –log_{10}
[0.01]

pH = –log_{10}
[1 × 10^{−}^{2}]

pH = –(log_{10}1
– 2 log_{10}10)

pH = 0 + 2 × log_{10}10

pH = 0 + 2 × 1 = 2

pH = 2

**pOH: **The pOH of an aqueous
solution is** **realted to the pH.

The pOH is the negative
logarithm of the hydroxyl ion concentration

**pOH
= –log _{10}[OH^{–}]**

The hydroxyl ion
concentration of a solution is 1 × 10^{−}^{9}M. What is the pOH of the solution?

pOH = –log_{10}
[OH^{–}]

pOH = –log_{10}
[1 × 10^{−}^{9}]

pOH = –(log_{10}
1.0 + log_{10} 10^{−}^{9})

pOH = –(0–9 log_{10}10)

pOH = –(0 – 9)

pOH = 9

The pH and pOH of a
water solution at 25^{o}C are related by the following equation.

**pH
+ pOH = 14**

If either the pH or the
pOH of a solution is known, the other value can be calculated.

**Example: **A solution has a pOH of
11.76.

What is the pH of this
solution?

pH = 14 – pOH

pH = 14 – 11.76 = 2.24

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10th Science : Chapter 10 : Types of Chemical Reactions : pH Calculation |

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