DRAFT: This module has unpublished changes.

The purpose of this lab is to determine how conductometry can be used to help obtain the concentration of a Ba(OH)2 solution. Titrations determine the amount or concentration of a reactant. This is accomplished by determining the equivalence point of two solutions, at which point the stoichiometric quantities of reactants are the same. In the experiment we will determine the equivalence point of two reactants using conductometry. We already know that solutions conduct electricity when ions are present, so a higher ion concentration in a solution will yield higher conductivity. If two strong electrolytes were mixed together and they react with the ions, then a precipitate or non-conducting molecule or gas is produced, which leaves the system. Thus, the ion concentration and conductivity decreases. If more of either strong electrolyte is added the ion concentration will keep decreasing and also the conductivity until the equivalence point is reached. At the equivalence point, the two electrolytes are combined in their stoichiometric ratio. In other words, all the ions are removed and the conductivity is at its minimum. If more of the second electrolyte is added after the equilibrium point the conductivity will increase again due to additional ions that are being added to the solution. In this experiment we will determine the concentration of a Ba(OH)2 solution by titrating it with H2SO4. 

DRAFT: This module has unpublished changes.