Definition & Determination of pH (Oxford AQA International A Level Chemistry)

Revision Note

Alexandra Brennan

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

The pH scale
The pH scale shows the acidity, neutrality and alkalinity of chemicals

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

  1. Find the pH when the hydrogen concentration is 1.60 x 10-4 mol dm-3

  2. Find the hydrogen concentration when the pH is 3.10

Answers:

  1. The pH of the solution is:

    • pH = -log[H+]

    • pH = -log 1.6 x 10-4

    • pH = 3.80

  2. 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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Alexandra Brennan

Author: Alexandra Brennan

Expertise: Chemistry

Alex studied Biochemistry at Newcastle University before embarking upon a career in teaching. With nearly 10 years of teaching experience, Alex has had several roles including Chemistry/Science Teacher, Head of Science and Examiner for AQA and Edexcel. Alex’s passion for creating engaging content that enables students to succeed in exams drove her to pursue a career outside of the classroom at SME.

Stewart Hird

Author: Stewart Hird

Expertise: Chemistry Lead

Stewart has been an enthusiastic GCSE, IGCSE, A Level and IB teacher for more than 30 years in the UK as well as overseas, and has also been an examiner for IB and A Level. As a long-standing Head of Science, Stewart brings a wealth of experience to creating Topic Questions and revision materials for Save My Exams. Stewart specialises in Chemistry, but has also taught Physics and Environmental Systems and Societies.