IntroductionIn any science requiring calculations, particularly in Chemistry, the collection of measurements of various physical and chemical properties must be rigorously accurate and precise as it is at this crucial stage that either create or curb the quality and value of science. No matter how well one might perform the experiment, without thinking about how to properly collect the data, the information collected would not be reliable enough to draw a conclusion about it. The main objective of this experiment is to thoroughly explain the reaction system which can be done through scientific observation because it is through this fundamental step that the facts necessary to clarify the reacting system are obtained. It was Antoine Lavoisier, a French chemist, who formulated one of the two laws observed in the experiment, the Law of Conservation of Mass, which stated that, in a chemical reaction, the total amount of matter of the reaction compounds remains constant. This law has been expressed in a more general form as follows: The total amount of matter in a closed system remains constant. The other law observed in the experiment is the Law of Conservation of Energy which states that energy can be neither created nor destroyed, only transformed from one form to another. Methodology Samples were taken from the three main bottles that contained the three solutions needed in the experiment. 10 ml of solution A was placed on a 50 ml Erlenmeyer flask. This solution had a consistency and appearance as transparent as water. 3 ml of solution B was placed in a 10 ml Erlenmeyer flask. This solution had a blue tint. 3 ml of solution C was also placed on another 10 ml Erlenmeyer flask. Like solution A, this latter solution had the same consistency and appearance as clear water. Cork stoppers were placed on the rim of all the flasks. After ensuring that the external parts were dry, the entire system was weighed at once and the measurement data was recorded. Solution B was then poured into the 50 mL flask, as the blue liquid slowly flowed down, a toothpaste-like precipitate appeared at the bottom of the flask. The two solutions mixed only when stirring began; before shaking the flask, the two solutions did not mix easily together. By carefully swirling the flask, the toothpaste-like precipitate began to mix with the clear liquid..