Notes

• The apparatus includes a 25 mL buret and a 125 mL flask. After selection of the parameters, the buret is filled with titrant to a random level just below the zero mark, and the flask is loaded with a 25 mL aliquot.
• To begin, select the acid and base. Hovering over an empty ^* box will cause an arrow to show and clicking it will drop down a few preset acids or bases. You can choose one or type the name of an acid of your choice ^†. If you enter an acid or base of your own, you will need to supply its K_a or K_b value. You can use exponential format
  e.g. 1.8e-5. For a strong acid or base, you should just type the the word "large" ^‡. If you use one of the sample acids or bases, the K_a or K_b will be filled in for you.

  ^* Note that the complete list will only drop down if the box is empty. Starting to type in the box will drop down a subset of acids or bases containing the string you have typed so far.
  ^† Note that what you type is not used for anything.
  ^‡ Entering a K_a or K_b value greater than about 0.01 may not give a clean graph.)

• You will need enter the acid and base concentrations, to select an indicator, and say whether the acid or the base is in the buret. Then click "Add solutions...".
• Left-click and hold down the mouse button on the burette stopcock to open it. Release the mouse button to close it. (The titration will stop automatically at the 25 mL mark if it is not stopped earlier.)
• Any parameter or parameters can be changed after the first have been chosen. Click "Add solutions..." again to begin a new titration.
  
• Check "Show the equivalence point" to see and compare the equivalence point to the end point.
• Check "Show the data points" to record a data point each time the stopcock is closed.
• Use the scroll bar to adjust the dropping rate.
• Click in the graph area to clear it. (Changing any of the parameters will clear it anyway.)

Note: The full the quadratic solution is used to calculate the pH and generate the curves: the "usual approximation" is not applied. However, the contribution to [H⁺] from the auto-ionization of water is ignored. For very dilute solutions and/or very weak acids or bases, this leads to a discontinuity in the curve near the equivalence point which would not be seen in a real experimental plot.