Definition & Determination of pH (Oxford AQA International A Level Chemistry)
Revision Note
Written by: Alexandra Brennan
Reviewed by: Stewart Hird
pH Scale Calculations
The pH scale is a numerical scale that shows how acidic or alkaline a solution is
The values on the pH scale go from 0-14 (extremely acidic substances have values of below 1)
All acids have pH values below 7
All alkalis have pH values above 7
The pH scale is a measure of the concentration of hydrogen ions in a solution
The lower the pH, the higher the concentration of hydrogen ions and the more acidic the solution is
The higher the pH, the lower the concentration of hydrogen ions and the more alkaline the solution is
The pH scale
Calculating pH
The pH is defined as:
pH = -log[H+]
where [H+] is the concentration of hydrogen ions in mol dm–3
Similarly, the concentration of H+ of a solution can be calculated if the pH is known by rearranging the above equation to:
[H+] = 10-pH
The pH scale is a logarithmic scale with base 10
This means that each value is 10 times the value below it
For example, pH 5 is 10 times more acidic than pH 6
pH values are usually given to 2 decimal places
The relationship between concentration is easily seen on the following table:
[H+] | Scientific notation | pH |
---|---|---|
1.0 | 100 | 0 |
0.1 | 10-1 | 1 |
0.01 | 10-2 | 2 |
0.001 | 10-3 | 3 |
0.0001 | 10-4 | 4 |
Worked Example
Find the pH when the hydrogen concentration is 1.60 x 10-4 mol dm-3
Find the hydrogen concentration when the pH is 3.10
Answers:
The pH of the solution is:
pH = -log[H+]
pH = -log 1.6 x 10-4
pH = 3.80
The hydrogen concentration can be calculated by rearranging the equation for pH
pH = -log[H+]
[H+] = 10-pH
[H+] = 10-3.10
[H+] = 7.94 x 10-4 mol dm-3
Calculating the pH of strong acids
Strong acids are completely ionised in solution
HA (aq) → H+ (aq) + A- (aq)
Therefore, the concentration of hydrogen ions, H+, is equal to the concentration of acid, HA
The number of hydrogen ions formed from the ionisation of water is very small relative to the [H+] due to ionisation of the strong acid and can therefore be neglected
The total [H+] is therefore the same as the [HA]
Worked Example
What is the pH of 0.01 mol dm-3 hydrochloric acid?
Answer:
[HCl] = [H+] = 0.01 mol dm-3
pH = - log[H+]
pH = - log[0.01]
pH = 2.00
Examiner Tips and Tricks
pH values should always be to two decimal places.
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