Introduction For this experiment, we are going to determine the effect of temperature on solubility, to be done in a chemical by dissolving a solute in a definite amount of solution which is saturated. Specifically, the goal of this experiment is to prepare a saturated solution of Na2C2O4 in water at different temperatures, determine the effect of temperature in solubility, and to apply Le Chatelier's Principle. We can do all this by simply titrating a certain amount of standard KMnO4, and measuring how much KMnO4 was needed to help Na2C2O4 reach chemical equilibrium at certain temperatures. In doing this, we will have fulfilled all the goals of our experiment, as well as being able to determine the Solubility of Na2C2O3 at both 20 and …show more content…

Additionally, the higher the temperature of the solution, the more standard KMnO4 was needed in order to balance out the sodium oxalate. Regarding ∆H and K, it is apparent that they are proportional to each other, the higher the rate law, the more change in heat there is, which effectively means that the more amount of a substance is used, the greater the amount of reactant dissolved in order to reach chemical equilibrium and/or minimize the amount of change, trying to return back to equilibrium. This in turn gives a greater amount of heat discharged as well, with regards to the amount of temperature.
Conclusion
In conclusion, Le Chatelier's Principle has indeed been proven to be a valid principle regarding chemistry because of the fact that through my experimentation, I have consistently noticed that the greater the amount of reactants and products I had, as well as the higher the temperature, the greater the amount of work and heat was generated (obvious because of a large rate law), which means that there is a greater struggle to reach chemical equilibrium the more substance there is. The heat given off was also proportional to these reactions.
Questions

1. When I compared my