How do you calculate the pH of a weak acid?

Strong acids dissociate fully in solution. Examples of strong bases include HCl and H2SO4. Organic acids, such as methanoic acid or oxalic acid, as well as some inorganic acids such as hydrogen fluoride, are weak acids.

A weak acid differs to a strong acid in that it does not fully dissociate in solution (it does not release all of it's potential hydrogen ions). This means that you cannot use the usual formula (pH=-log
10[H^+]) by simply letting [H^+] equal the concentration of the acid. Instead, you must use the acid dissociation constant, Ka. Where, at equilibrium, [H^+] is the hydrogen ion concentration, [A^-] is the dissociated acid concentration, and [HA] is the concentration of the undissociated acid:
 

Ka = ([H^+][A^-])/[HA]

If we assume that when the weak acid dissociates, [H^+]=[A^-], then:
 

Ka = ([H^+]^2)/[HA]

If you know the equilibrium concentration of the acid and the Ka (which you will usually be given), you can rearrange this formula to give [H^+], which should be all you need to work out the pH.

Answered by Joe M. Chemistry tutor

11648 Views

See similar Chemistry A Level tutors

Related Chemistry A Level answers

All answers ▸

Explain why cyclohexene will react with bromine gas but benzene will not


How can you work out, using the changes in oxidation numbers, which compound out of KCl, KBr and KI has the greatest reducing power?


What is a stereoisomer?


Why is CO2 a linear molecule whereas H2O has a v-shaped geometry?


We're here to help

contact us iconContact usWhatsapp logoMessage us on Whatsapptelephone icon+44 (0) 203 773 6020
Facebook logoInstagram logoLinkedIn logo

© MyTutorWeb Ltd 2013–2025

Terms & Conditions|Privacy Policy
Cookie Preferences