Take the results from your titration experiment and calculate the moles (mol) of standard it took to react with the unknown. Begin by taking the volume of standard you added and converting this to the number of moles of the standard molecule. You should know the concentration of the standard and the volume you added to the unknown. These two pieces can be combined by multiplying the volume added (in liters) and the concentration (in moles per liter). Now you have the moles of standard it took to neutralize the unknown solution.

Relate the moles of standard solution to the moles of unknown solution. Because this is a neutralization reaction, assume that the standard solution is the base (OH- ions). You calculated the moles of base it took to neutralize the unknown acid (H+). Use the calculated number of moles of base and relate it, through the chemical reaction equation, to the number of moles of acid in the unknown. If your reaction is 1 mol of base for every 1 mol of acid (as most usually are), then you know that the number of moles of standard is the same as the number of moles of the unknown. If the number is not 1 to 1, then multiply by the correct factor (this is reaction specific). You now have the number of moles of acid (H+) in the unknown solution.

Convert the number of moles of H+ to the concentration of H+ by taking the number of moles of H+ and dividing by the volume (in liters) of unknown that you originally had. This gives you the concentration of H+ in the unknown solution.

Take the concentration of H+ (in moles per liter) and plug it into the following pH formula: pH=-log(H+). Determine the negative log of the H+ concentration using your calculator. You will arrive at the pH value of the unknown solution. If your solution is acidic, you will have a pH less than seven; if neutral, a pH equal to seven; and if basic, a pH greater than seven.