The experiment was aimed at determining the effects of temperature on solubility of salt (Potassium Nitrate) in sodium chloride solution. Its solubility was determined with respect to concentration per volume for a range of temperatures. The objectives were achieved by dissolving a known mass of the solute in sodium chloride under a water bath. Once all the crystals were dissolved, the temperature after the solute was dissolve was recorded since it is considered that this is the point at which a reaction is at point of equilibrium (Krumhansl 19). To have the necessary values, molarities were calculated at each point where all pellets had dissolved. Since the temperature recordings were positive, it was clear that the reaction was exothermic. Having known the solutionâ€™s volume and the quantity of KNO3 that was added, it was possible to calculate molarity at every point of equilibrium. [K+][NO3-] was the constant for dissociation, a point where the molarity of potassium nitrate is at equilibrium since the solventâ€™s stoichiometry is in the ration of 1:1. To determine the relationship that exists between temperature and rate of dissociation, a graph of potassium nitrate against 1/T was plotted, and the two variables demonstrated a linear relationship. An increase in temperature positively correlated with an increase in the quantity of KNO3Â that dissolved in the sodium chloride solution, and vice versa. When the quantity of KNO3Â that was fully dissociated was 9.111 grams, 1/T was 0.00329. In the second trial, 12.221 grams dissolved at 0.0019, which is a much higher volume than the previous trial. A similar trend is evidenced in the third and fourth test tubes, and correlates to findings from a number of studies (Krumhansl 23).
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