• In this example, strong sodium hydroxide, NaOH (aq), is being added to weak ethanoic acid, CH3COOH (aq)

NaOH (aq) + CH3COOH (aq) →?CH3COONa (aq) + H2O (l)

• The pH on the intercept on the y axis starts at roughly 3 due to the relative strength of the ethanoic acid
• The initial rise in pH is steep as the neutralisation of the weak acid by the strong base is rapid
• Ethanoate ions (conjugate base to ethanoic acid) are formed which then creates a?buffer
  • A buffer consists of a weak acid and its conjugate base or a weak base and its conjugate acid

   

• At this point, the buffer formed will resist changes in pH so the pH rises gradually as shown in the?buffer region
• The?half equivalence point?is the stage of the titration at which exactly half the amount of weak acid has been neutralised
  • [CH3COOH (aq)] = [CH3COO-?(aq)]
  • At this point, it is important to note that the pKa?of the acid is equal to the pH
    • pKa?= pH?at?half equivalence
• The equivalence point in a weak acid - strong base titration is?above 7

Weak acid - strong base pH curve