Dip the conductometer's electrode into the known solution. The electrode measures the conductivity of the solution. The conductometer measures the strength and concentration of ions. Write down the electric current, noted as I. Keep an accurate measurement of the known solution you are titrating, because you will need this to calculate the unknown solution.
Add the unknown solution to your beaker. Dip the conductometer’s electrode into the unknown solution to identify the solution strength. Write down the electric current and leave the electrode in the solution.
Test the solution with a pH meter to determine whether it is an acid or base. If the pH meter reads below 7, it is an acid. If it reads above 7, it is a base. Choose a solution that is the opposite, either acid or base, of the solution you are measuring. Choose a solution with a known chemical make-up. For instance, if your unknown solution is an acid, use a base solution. The positive hydrogen acid ions will bond with the hydroxide solution in the base to create water, a pH neutral solution. These ions are attracted to each other, because opposite ion charges attract and hydrogen must bond with either oxygen, nitrogen or fluorine to stabilize.
Leave the pH meter in the unknown solution. Add the known solution slowly and watch closely for the solution to change colors. As soon as the color changes, you have reached a point of equivalence or the endpoint. The pH meter will go to neutral when the solutions are ready.
Identify the volume of the known solution you used to reach the equivalence point or the endpoint, or the point when the solution changes color and the pH meter reads that the solution is neutral.
Identify the electrical resistance, noted as R, on the conductometer. To get the voltage, multiple the electrical resistance by the electric current, or V = IR.
Identify the molecular weight. The molecular weight is the atomic mass of the known substance. Go to the periodic table and locate the atom weight of each atom present in your known solution. Add these weights together to identify the molecular weight. For instance, for solution C2H5OH, the carbon weighs 12.01 g/mole, hydrogen is 1.008 g/mole and oxygen weighs 16 g/mole. You have two carbons, so you multiply 12.01 by 2, giving you 24.02. You have six hydrogen atoms, so you multiply 1.008 by 6, or 6.048. You have one oxygen. Now, you add the three numbers together to get your molecular weight. The molecular weight of the example is 24.02 plus 6.048 plus 16, or 46.068.
Calculate the molarity, or how many moles of the known solution were dissolved. The molarity is calculated by dividing the number of solution moles by the number of liters of the solution. To get the molarity, divide the molecular weight you calculated in Step 7 by the volume of the solution you calculated in Step 5.
To calculate the solution strength, or redox, multiply the molarity you calculated in Step 8 by the molecular weight you calculated in Step 7.