pH Curves (AQA A Level Chemistry): Revision Note

pH Curves

• During a titration, a pH meter can be used and a pH curve plotted

• A pH curve is a graph showing how the pH of a solution changes as the acid (or base) is added

• The result is a characteristically shaped graph, which can yield useful information about how the particular acid and alkali react together, with stoichiometric information

• All pH curves show an S-shape curve, and the midpoint of the inflection is called the equivalence or stoichiometric point

• From the curves, you can

  • Determine the pH of the acid by looking at where the curve starts on the y-axis

  • Find the pH at the equivalence point

  • Find the volume of the base at the equivalence point

  • Obtain the range of pH at the vertical section of the curve

Four types of acid-base titrations

• There are four combinations of acids and alkalis that you should know about:

  • strong acid + strong base

  • weak acid + strong base

  • strong acid + weak base

  • weak acid + weak base

• Without titles for the graph, you can easily recognise which combination is shown by looking at the starting and ending pH and deducing whether the acid and alkali are strong or weak

• Sometimes you may see pH titration curves that show pH plotted against the volume of acid added

• This produces the mirror image graph from which you can get all the same information

Related topics

• Titrations

• Acid dissociation constant

• Buffers

• pH & H+

Choosing an Indicator

• An acid-base indicator is a weak acid that dissociates to give an anion of a different colour

• Consider a weak acid HIn:

HIn (aq)  + H₂O (l)  ⇌ H₃O⁺ (aq) + In^- (aq)

colour 1                                          colour 2

• HIn and its conjugate base In^- are different colours

• The colour of the solution depends on the relative concentrations of the two species

• If the solution is acidic, the above equilibrium will be shifted to the left, and more HIn will be present

  • Colour 1 will thus dominate

• If the solution is alkaline, the above equilibrium will shift to the right, and more In^- will be present

  • Colour 2 will thus dominate

• The colour of the indicator thus depends on the pH of the solution

• The colour will not change suddenly at a certain pH, but will change gradually over a pH range

• The colour of the indicator depends on the ratio of [HIn] to [In^-]

• The pH at which these transitions will occur depends on the K_a of the indicator

$K_{\mathit{a}}=\frac{\left[{\mathrm{H}}^{+}\right]\left[{\mathrm{In}}^{-}\right]}{\left[\mathrm{HIn}\right]}$

• The endpoint of the reaction is where there is a balance between [HIn] and [In^-]. At this point, these two concentrations are equal

$K_a=\frac{\left[{\mathrm{H}}^{+}\right]\bcancel{\left[{\mathrm{In}}^{-}\right]}}{\bcancel{\left[\mathrm{HIn}\right]}}=\left[{\mathrm{H}}^{+}\right]$

• Taking negative logs of both sides:

$pKa=pH$

• This means the pK_a of an indicator is the same as the pH of its endpoint

 Common Indicators and their colours table

Choosing a suitable indicator

• Around the equivalence point of a titration, the pH changes very rapidly

• Indicators change colour over a narrow pH range, approximately centred around the pK_a of the indicator

• An indicator will be appropriate for a titration if the pH range of the indicator falls within the rapid pH change for that titration

• The indicator's pH range must fall entirely within the steep/vertical part of the titration curve

Strong acid-strong base

• In strong acid - strong base titrations, the pH changes from 4 to 10 at the end-point, so a suitable indicator must change colour within this range

  • Methyl red and phenolphthalein are suitable indicators for these titrations

  • Methyl orange is not ideal, but it shows a significant enough colour change at the end point, so it is widely used

Weak acid-strong base

• In weak acid - strong base titrations, the pH changes from 7 to 10 at the end-point, so a suitable indicator must change colour within this range

  • Phenolphthalein is the only suitable indicator for weak acid - strong base titrations that is widely available

Strong acid-weak base

• In strong acid - weak base titrations, the pH changes from 4 to 7 at the end-point, so a suitable indicator must change colour within this range

  • Methyl red is the most suitable indicator for these titrations

  • However, methyl orange is often used since it shows a significant enough colour change at the end-point and is more widely available than methyl red

Weak acid-weak base

• In weak acid -weak alkali titrations, there is no sudden pH change at the end-point, and thus there are no suitable indicators for these titrations

• The end-points of these titrations cannot be easily determined

• The pH change is too gradual at the equivalence point, so no indicator will give a distinct colour change