To perform an acid base titration, you will need litmus paper, an acid or base of unknown concentration, an opposite solution of known concentration, a beaker, a burette and an indicator. By using the litmus paper, you can determine whether the unknown solution is acidic or basic. If it is acidic, the opposite solution needs to be basic. If it is basic, the opposite solution must be acidic.
To choose the correct indicator, estimate the pH based on the litmus test, then compare it to the pH ranges of the different indicators. For example, if the litmus test suggested the pH of the unknown solution was around 9, you would use phenolphthalein, because its pH range is 8.2 to 10.0. However, if the litmus test suggest the pH to be between 5 and 6, you would use methyl red.
Pour the unknown solution into the beaker and record the volume. Add a few drops of indicator solution to the unknown solution in the beaker. Place the burette above the beaker and add the known solution to the burette and record its volume.
Slowly introduce the known solution into the unknown solution by turning the burette knob to allow drops to fall into the beaker. It is easy to add too much too quickly and miss the titration point, so only add a drop at a time. If you are not quite sure if you have reached the equilibrium point, record the amount left in the burette and add another drop. If the color changes dramatically, you have added too much, so use the original measurement. For example, if you are using phenolphthalein, which turns from colorless to pink when the acid is neutralized, and you aren't quite sure if the solution has a tint of pink yet, add another drop. If the solution turns bright pink, you known you have gone too far.
Calculate the amount of known solution you used by subtracting the amount remaining in the burette from the amount you originally started with. For example, if you started with 40ml in the burette and now there are only 20, you used 20ml of the solution. Multiply this number by the molecular concentration of the known solution. For example, if the concentration was 0.5 M, multiply 0.5 times 20 and you get 10. Then divide that number by the volume of the unknown solution. If there were originally 30ml of the unknown solution in the beaker, you would divide 10 by 30 and get 0.33 M as the concentration of the unknown solution.