Briefly discuss interpretations of your observations and results. Discuss how your observations illustrated LeChatelier's principle. Discuss how reactant concentrations change as equilibrium reactions shift to the left or the right. Likewise, discuss how product concentrations change as equilibrium reactions shift to the left and the right. Explain using your observations in Part V if you would prepare a calcium oxalate precipitate in acidic or basic solution.

Le Chatelier's principle can be applied in explaining the results

Explanation:

According to Le Chatelier's principle, when a constraint such as a change in concentration in this case is imposed on a chemical system in equilibrium, the system will adjust itself in such a way as to annul the constraint imposed.

Hence, when the color of the solution was more like that of the control, the reaction would shift towards the left. Similarly, when the color was more like it was towards the reactant, the reaction would shift towards the right.

If we were to prepare calcium oxalate, we should prepare it in a base solution. This is because when the base was added to calcium oxalate, it did not form any precipitate but when an acid was added to the calcium oxalate, it formed a precipitate.

r just means there's a number of carbon in teh chain. for example rcooh means that after x number of carbon, the chain ends with cooh.

explanation: