Reaction Lab

This lab’s end result was to correctly identify each unknown solution using prior knowledge of chemical properties and the results of the first experiment conducted. Unknown solution D was the only colored solution, being blue while the others were clear. This made it easy to then match D up to Copper Sulfate because of its color. As unknown A and B were added together, lots of gaseous bubbles formed and revealed the fact that that reaction was the reaction between Hydrochloric Acid and Sodium Carbonate because it was the only reaction that produced a gas release. Unknown A and C produced the only yellow, brown precipitate just as the reaction between Sodium Carbonate and Silver Nitrate had previously. This led to the conclusion that A is Sodium

The solubility rules pertaining to the substances used during this lab are as follows: All nitrates, sulfates (except those containing Ba, Ca, Sr, Pb, and Hg₂), compounds containing alkali metals (Na), and chlorides (except those containing Ag, Pb, and Hg₂) are soluble. All compounds containing CO₃, the compound AgCl and some sulfates such as Ag₂SO₄ are insoluble. Given this, the reaction between Silver Nitrate and Hydrochloric produced aqueous nitric acid and a solid precipitate of Silver Chloride because of AgCl insolubility and all nitrates solubility. Silver Nitrate and Copper Sulfate produced aqueous Copper (II) Nitrate and a solid precipitate of Silver Sulfate because of all nitrates solubility and the exception that Ag₂SO₄ is insoluble. Silver Nitrate and Sodium Carbonate reaction resulted in the formation of a solid Silver Carbonate precipitate and aqueous Sodium Nitrate because of all nitrates solubility and carbonates insolubility. The reaction between Hydrochloric Acid and Sodium Carbonate led to the formation of gaseous Carbon Dioxide, aqueous water, and aqueous solution of Sodium Chloride as a result of all compounds containing alkali metals solubility. Lastly, Copper Sulfate and Sodium Carbonate reaction produced an aqueous sodium sulfate solution and a solid precipitate of Copper (II) Sulfite because of all alkali metals and sulfates ability to be soluble and the rule that any compound containing CO₃ is insoluble. In the end, the hypothesis that if we react mystery chemicals with one another, we will be able to identify the reactants and products, create balanced equations, and observe properties because of our prior knowledge learned throughout the course of the unit and using the known chemical reaction was accepted by the data