8.5 - Acid - base titrations
8.5.1: Draw and explain a graph showing pH against volume of titrant for titrations involving strong acids and bases.
|General Type||Example||Typical Titration Curve||Features of Curve|
|Strong acid & Strong Base||HCl added to NaOH||Curve begins at high pH typical of strong base and ends at low pH typical of strong acid. There is a large rapid change in pH near the equivalence point (pH =7).|
|Strong base & strong acid||NaOH added to HCl||Curve begins at low pH typical of strong acid, and ends at high pH typical of strong base. There is a large rapid change in pH near the equivalence point (pH=7).|
|Weak acid & Strong base||NaOH added to acetic acid (ethanoic acid - CH3COOH)||Curve begins at a higher acidic pH and ends at high basic pH. The pH change at the equivalence point (pH > 7)is not so great.|
|Strong acid & Weak base||Ammonia (NH3) added to HCl||Curve begins at low pH and ends at a less high basic pH. The pH change at the equivalence point (pH < 7) is similar to that for Strong base & Weak acid.|
|Weak acid & Weak base||Ammonia (NH3) added to ethanoic acid (CH3COOH)||Curve begins at higher acidic pH and ends at low basic pH. There is not a great pH change at the equivalence point (pH ~ 7) making this a very difficult titration to perform.|
Try it yourself
The following applet (Courtesy of the RSC) allows you to plot a titration curve using the acids and bases of your choice. You can then select a suitable indicator for the titration.
The Y-axis shows the pH of the mixture during the titration and the X-axis shows the amount of base added.
The equivalence point shows the pH at the point when all the acid has been neutralised by the base added. Notice that this is not necessarily at pH=7, it depends on the acids and bases used. For further explanation see section 18.4 "salt hydrolysis"
To run the program a second time you must refresh the page