My conclusion based on this experiment is that the barium chloride hydrate was dehydrated and then re-hydrated with distilled water. That solution was added to a solution of silver nitrate and then heated. A chemical reaction occurred that caused a precipitate to form in the solution and settle at the bottom. This precipitate was most likely silver from the silver nitrate. This solution was then filtered to get the precipitate by itself. The masses were obtained along the way and then used to calculate the moles of silver chloride, the chloride, and the barium. This was then used with the masses to calculate the Empirical formula for the hydrated salt. This formula was BaCl2 (H2O).
Error could have occurred at this experiment at many different places. Error