Unit 9 Reaction Lab

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In this experiment, 9 reaction systems were studied to observe how pH, temperature, and concentration of reactants can shift the equilibrium of a system. To accomplish this purpose, nine reactions were performed under different constrains to observe chemical and physical changes. These shifts can be explained through the Le Chatelier’s principle as the system reacts to counteract any stress added. By studying these shifts through color changes, gases formation, dissolution and formation of solids, a greater understanding of the system is developed.

In Reaction 1, Potassium Chromate initially is seen as yellow. When NaOH was added, the solution did not change color. This mean reaction quotient (Q) equals to K (equilibrium constant). Moreover, …show more content…
Water shifts the equilibrium to the right, which resulted in a cloudy solution. Adding HCl to the solution lead to bubbling, which probably the indication of formation of of carbonic acid. Eventually, this carbonic acid will ionize back into calcium and carbonate ions, which shift the equilibrium back to the right. This resulted in the cloudy solution again. Adding HCl again will shift the reaction to the left, making the cloudy disappear. However, when that acid ionize, the solution will stabilize at the right side by turning cloudy …show more content…
However, there were several systemic errors throughout the experiment that prevented accurate observations. In particular in reaction 3, the stock solution for cobalt (II) chloride was contaminated. Initially, this solution should appear blue, but the contamination made it pink. Therefore, adding a few drops of HCl did not change the color of solution. However, adding a bunch of HCl did change the solution to a blue color. This suggests that the stock solution begin with a lot of products. Adding more HCl would of restore the equilibrium on the left. If the reaction had went well, adding HCl would change the solution from blue to pink. Further, HCl would make the solution blue again because the Le Chatelier principles explains the reaction will go toward the reactants when there are too much products. In this case, the addition of chlorine ions contributed to increased amount of products. Since this error was never fixed, that observations that cooling the solution formed a purple color and heating it will form a dark blue color is not accurate in describing this system. The system that was experimented was reverse due to contamination because the initial stock solution contained instead of . Another systemic error that contribute to wrong observation was due to people not capping the stock solution bottles. This can have negative effects by distributing the equilibrium in the system by exposing the solution
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