DRAFT: This module has unpublished changes.

In conclusion, the purpose of this experiment was to determine how conductometry can be used to obtain the concentration of a Ba(OH)2 solution. We accomplished this by titrating a Ba(OH)2 solution with H2SO4, in order to obtain the equivalence point and calculate the concentration of Ba(OH)2 using stoichiometric ratios. In the first trial we determined that the concentration fo Ba(OH)2 was 0.264M and in the second trial it turned out to be 0.208M. The average of these two concentrations is around 0.236M so the concentration of the Ba(OH)2 solution was roughly 0.2M. 

 

Like any experiment there were sources of error that have to be discussed. One of these sources was perhaps spilling some of the Ba(OH)2 solution when water was being added to the jar. Another error may have occurred due to residue left on the jar from previous use that was not cleaned well. Finally we must also consider that the H2SO4 solution was mixed with other substances, which may have thrown off the equivalence point depending on the concentration of the extra ions from the other substances that were present. 

DRAFT: This module has unpublished changes.