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Aqueous Solutions and Solution Stoichiometry Experiment 2 *1Cindy Nguyen CHEM 117-509Tyler Nardecchia Summary:The purpose of the experiment was to determine the behavior of weak electrolytes, strongelectrolytes and nonelectrolytes by measuring conductivity in solutions and then to determine theequivalence point and concentration of barium hydroxide. The experiment consisted of two parts,part A was to determine if conductivity was related to a solution being strong or weak and part B focused on finding the equivalence point between the mixture of an acid and base. In part A therewere 11 different solutions given (some with the same solution but with different molarities) these solutions were: 0.1 M, 0.2 M, 0.3 M of NaCl, 0.1 M, 0.2 M, 0.3 M of CH3OOH, 0.1 M of CaCl2, 0.1 M of HCl, 0.1 M CH3OH, distilled water and tap water. With these 11 solutions a conductivity probe was connected to LoggerPro and used to measure the conductivity of each of solution in unites of microsiemens. After the conductivity of the solutions were found, it is discovered that NaCl, HCl, and CaCl2were strong electrolytes, CH3OH, CH3OOH, and tap waterwere weak electrolytes and distilled water was founded to be a nonelectrolyte. In part B 50 mL of an unknown concentration of Ba(OH)2 was poured into a graduated cylinder then into a 150 mL beaker. Then a stir bar was added to the solution along with 2-3 drops of phenolphthalein indicator. The beaker was then placed on top of a hot plate with a conductivity probe extended down into the solution along with a buret arranged above the beaker filled with 50 mL of a 0.08 M concentration of H2SO4. The beaker of Ba(OH)2was then titrated by the solution of H2SO4. At